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TRANSCRIPT
Developing kinetic mechanisms for larger hydrocarbon fuels
1
Larger Fuel Chemistry
Boundary between ldquosmallrdquo and ldquolargerdquo fuel molecules is somewhat arbitrary however
C5 fuels have much more low T kinetics than C4
C6 fuels have much more low T kinetics than C5
C6 and larger molecules have lots of low T reaction pathways ldquocool flamesrdquo and lower ON values than smaller fuels
2
TF Lu CK Law lsquoToward accommodating realistic fuel chemistry in large‐scale computationsrsquoProgress in Energy and Combustion Science 35 (2009) 192ndash215
Methyl decanoate is a biomass fuel surrogate Detailed kinetic mechanism consists of 3036 species and 8555 reactions
Automatic Generation of kinetic mechanisms easily produces
Large Kinetic Models
Mechanism Size
3
Mechanism Size
Mechanism size grows with molecule size
4
Dominance of H2O2 Reactions
For nearly all hydrocarbon oxidation no matterhow large or small the fuel molecule at hightemperatures the reactions of H2O2 have thegreatest sensitivity controlling the overall rate ofreaction This is true in flames detonations shocktubes and many other practical combustors
5
Combustion Chemistry Complexity
6
Low temperature High temperature
+ O2 Oxidation
Pyrolysis
Pyrolysis
+ O2 Oxidation
Courtesy of Prof Tiziano Faravelli Politecnico di Milano
7
R + O2 harr RȮ2 Low TRȮ2 QOOH (~500 850 K)
QOOH + O2 harr Ȯ2QOOH Ȯ2QOOH RȮ + ȮH + ȮH
conversion
Reactor Temperature
Zhandong Wang Proc Natl Acad Sci 114(50) (2017) 13102ndash13107Zhandong Wang et al Combust Flame 187 (2018) 199ndash216
Evidence of further additions to O2 have been reported
Three distinct temperature regimes
8
Negative Temperature Coefficient Regime
Intermediate T (850 1100 K)RȮ2 rarr olefin + HȮ2 (NTC)
QOOH rarr cyclic ether + ȮH (NTC)
Three distinct temperature regimes
conversion
Reactor Temperature
9
Flame images taken by a CH-filtered digital stillcamera (a) Normal flame (U = 40 cms) (b) FREI (U= 20 cms) and (c) weak flames (U = 30 cms) Computed profiles of major species at U = 20 cms
Vertical dotted lines indicate the locations of HRR peaks
Akira Yamamoto Hiroshi Oshibe Hisashi Nakamura Takuya Tezuka Susumu Hasegawa Kaoru Maruta
Proceedings of the Combustion Institute vol 33 pp 3259‐3266 (2011)
Three distinct temperature regimes nC7H16
0
300
600
900
1200
1500
000 020 040 060 080 100
Tem
pera
ture
-K
Time - seconds
n-heptane RON = 0
heat release rateTemperature
Slide courtesy of Dr Charles Westbrook10
Three distinct temperature regimes nC7H16
11ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
Intermediate TḢ + O2 (+M) = HȮ2 (+M)RH + HȮ2 = R+ H2O2
H2O2 (+M) = ȮH + ȮH (+M)R + O2harr RȮ2
RȮ2 rarr olefin + HȮ2
High TFuel = R + Rprime
R = olefin + ĊH3 or ḢḢ + O2 = Ouml + ȮH
ĊH3 + O2 = CH2O + ȮH
22
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
12
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Ḣ + O2 (+M) = HȮ2 (+M)RH + HȮ2 = R+ H2O2
H2O2 (+M) = ȮH + ȮH (+M)R + O2harr RȮ2
RȮ2 rarr olefin + HȮ2
Three distinct temperature regimes
13
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
14ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Importance of concerted HȮ2 elimination reaction
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
15
Intermediate temperature chemistrymdash Concerted eliminations are not well known ndash quantum chemistry
mdash Quelch et al1 first proposed Ċ2H5 + O2 = C2H4 + HȮ2 cyclic TS via concerted elimination
mdash Miyoshi23 variational TST and RRKMmaster equation (Ċ2iĊ3n‐s‐t‐Ċ4 + O2)
mdash Villano et al45 calculated 23 different straight and branched alkyl‐peroxyl radicals
mdash Goldsmith et al6 for the propyl + O2 system
Need for further studies of these reactions due to their high importance
1GE Quelch MM Gallo M Shen Y Xie HF Schaefer III D Moncrieff J Am Chem Soc 116 (1994) 4953ndash49622A Miyoshi J Phys Chem A 115 (2011) 3301ndash33253A Miyoshi A Int J Chem Kinet 44 (2012) 59ndash744SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 115 (2011) 13425ndash134425SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 116 (2012) 5068ndash50896CF Goldsmith WH Green SJ Klippenstein J Phys Chem A 2012 116 3325ndash3346
16
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
17
Few direct measurements of H‐atom abstraction by HȮ2 ndash lack of suitable precursors mdash CH2O + HȮ2 Jemi‐Alade et al1 using flash photolysismdash Walker et al23 made indirect relative rate measurementsmdash Scott and Walker4 review of alkanes aromatics and related compounds in 2002
Recent developments in quantitative measurements of HȮ2 radicals mdash Fluorescence assay by Gas Expansion by Blocquet et al5 (2013)mdash Dual‐modulation Faraday Spectroscopy67 (2014 2015)mdash Cavity ring‐down spectroscopy8 (2014)
These measurements are very useful in assessing mechanism performance1AA Jemi‐Alade PD Lightfoot R Lesclaux Chem Phys Lett 195 (1992) 25ndash302RR Baldwin RW Walker Proc Combust Inst 17 (1979) 525ndash5333RW Walker C Morley in Comprehensive Chem Kinetics (M J Pilling Ed) Elsevier Amsterdam 351 (1997)4M Scott RW Walker Combust Flame 129 (2002) 365ndash3775M Blocquet C Schoemaecker D Amedro O Herbinet F Battin‐Leclerc C Fittschen Proc Natl Acad Sci U S A 110 (2013) 20014ndash200176B Brumfield WT Sun Y Wang Y Ju G Wysocki Opt Lett 39 (2014) 1783ndash17867N Kurimoto B Brumfield X Yang T Wada P Dieacutevart G Wysocki Y Ju Proc Combust Inst 35(1) (2015) 457ndash4648M Djehiche NL Le Tan CD Jain G Dayma P Dagaut C Chauveau L Pillier A Tomas J Am Chem Soc 136 (2014) 16689ndash16694
93
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
18
CH3OH oxidation 855 O2 p = 40 atm and T = 885 K
Sensitivity to ignition delay timeU Burke WK Metcalfe SM Burke KA Heufer P Dagaut HJ Curran Combust Flame 165 (2016) 125ndash13694
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
19
CH3OH + HȮ2 = ĊH2OH + H2O2
05 10 15 20104
105
106
107
108
109
1010
1011
1012
rate
con
stan
t (k)
cm
3 mol
-1 s
-1
1000 K T
Altarawneh (2011) Olm et al (2017) Alecu and Truhlar (2011) Klippenstein (2011)
104
105
106
107
108
109
1010
1011
1012
2000 1500 1000 500T K
20
Klippenstein et al1 reported high sensitivity to CH3OH + HȮ2 also calculated k Altarawneh et al2 and Alecu and Truhlar3
Olm et al4 via computer optimization using direct and indirect measurements Alecu and Truhlar attributed differences with Klippenstein et al calculations to
differences in treatment of anharmonicity
Possible chemically activated reactions involving HȮ2 radicals
1SJ Klippenstein LB Harding MJ Davis AS Tomlin RT Skodje Proc Combust Inst 33 (2011) 351ndash3572M Altarawneh AH Al‐Muhtaseb BZ Dlugogorski EM Kennedy JC Mackie J Comp Chem 32 (2011) 1725ndash17333IM Alecu DG Truhlar J Phys Chem A 115 (2011) 14599ndash146114C Olm T Varga Eacute Valkoacute HJ Curran T Turaacutenyi Combust Flame 186 (2017) 45ndash64
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
21
Carstensen and Dean12 for CH4 C2H6 C3H8 C4H10 + HȮ2
Aguilera‐Iparraguirre et al3 CH4 C2H6 C3H8 nC4H10 iC4H10 + HȮ2
mdashAgree well with the determinations of Walker et al
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash1573J Aguilera‐Iparraguirre HJ Curran W Klopper JM Simmie J Phys Chem A 112 (2008) 7047ndash7054
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
22ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
RH + CH3Ȯ2 = R + CH3O2H can also be important
HJ Curran P Gaffuri WJ Pitz CK WestbrookCombustion and Flame 129253ndash280 (2002)
iC8H18 oxidationφ = 10 in air p = 40 atm
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
23
RH + CH3Ȯ2 = R + CH3O2HĊH3 + O2 = CH3Ȯ2
RH + CH3Ȯ2 = R + CH3O2HCH3O2H = CH3Ȯ + ȮH
Carstensen and Dean1 for CH4C2H6 + ḢCH3Ȯ2C2H5Ȯ2
CarstensenDeanDeutschmann2 for CH4 C2H6 C3H8 C4H10 + HȮ2 CH3Ȯ2 C2H5Ȯ2 C3H7Ȯ2 C3H7Ȯ2 HC(O)Ȯ2 CH3C(O)Ȯ2
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash157
24ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
25
Rate rules for large molecular weight molecules
bull High temperature mechanismReaction class 1 Unimolecular fuel decompositionReaction class 2 H atom abstractions from fuelReaction class 3 Alkyl radical decompositionReaction class 4 Alkyl radical + O2 = olefin + HȮ2
Reaction class 5 Alkyl radical isomerizationReaction class 6 H atom abstraction from olefinsReaction class 7 Addition of radical species to olefinsReaction class 8 Alkenyl radical decompositionReaction class 9 Olefin decomposition
26Slide Courtesy of Dr William Pitz
Reaction rate rules for higher MW species
27Slide Courtesy of Dr William Pitz
Reaction classes for low temperature reactionsLow temperature mechanismReaction class 10 Alkyl radical addition to O2 (R + O2)Reaction class 11 R + RrsquoO2 = RȮ + RrsquoȮReaction class 12 Alkylperoxy radical isomerizationReaction class 13 RȮ2 + HȮ2 = ROOH + O2Reaction class 14 RȮ2 + H2O2 = ROOH + HȮ2Reaction class 15 RȮ2 + CH3Ȯ2 = RȮ + CH3Ȯ +O2Reaction class 16 RȮ2 + RrsquoȮ2 = RȮ + RrsquoȮ + O2Reaction class 17 ROOH = RȮ + ȮHReaction class 18 RȮ DecompositionReaction class 19 QOOH = Cyclic Ether + ȮHReaction class 20 QOOH = Olefin + HȮ2Reaction class 21 QOOH = Olefin + Aldehyde or Carbonyl + ȮHReaction class 22 Addition of QOOH to molecular oxygen O2Reaction class 23 Ȯ2QOOH isomerization to carbonylhydroperoxide + ȮHReaction class 24 Carbonylhydroperoxide decompositionReaction class 25 Reactions of cyclic ethers with ȮH and HȮ2
28
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Larger Fuel Chemistry
Boundary between ldquosmallrdquo and ldquolargerdquo fuel molecules is somewhat arbitrary however
C5 fuels have much more low T kinetics than C4
C6 fuels have much more low T kinetics than C5
C6 and larger molecules have lots of low T reaction pathways ldquocool flamesrdquo and lower ON values than smaller fuels
2
TF Lu CK Law lsquoToward accommodating realistic fuel chemistry in large‐scale computationsrsquoProgress in Energy and Combustion Science 35 (2009) 192ndash215
Methyl decanoate is a biomass fuel surrogate Detailed kinetic mechanism consists of 3036 species and 8555 reactions
Automatic Generation of kinetic mechanisms easily produces
Large Kinetic Models
Mechanism Size
3
Mechanism Size
Mechanism size grows with molecule size
4
Dominance of H2O2 Reactions
For nearly all hydrocarbon oxidation no matterhow large or small the fuel molecule at hightemperatures the reactions of H2O2 have thegreatest sensitivity controlling the overall rate ofreaction This is true in flames detonations shocktubes and many other practical combustors
5
Combustion Chemistry Complexity
6
Low temperature High temperature
+ O2 Oxidation
Pyrolysis
Pyrolysis
+ O2 Oxidation
Courtesy of Prof Tiziano Faravelli Politecnico di Milano
7
R + O2 harr RȮ2 Low TRȮ2 QOOH (~500 850 K)
QOOH + O2 harr Ȯ2QOOH Ȯ2QOOH RȮ + ȮH + ȮH
conversion
Reactor Temperature
Zhandong Wang Proc Natl Acad Sci 114(50) (2017) 13102ndash13107Zhandong Wang et al Combust Flame 187 (2018) 199ndash216
Evidence of further additions to O2 have been reported
Three distinct temperature regimes
8
Negative Temperature Coefficient Regime
Intermediate T (850 1100 K)RȮ2 rarr olefin + HȮ2 (NTC)
QOOH rarr cyclic ether + ȮH (NTC)
Three distinct temperature regimes
conversion
Reactor Temperature
9
Flame images taken by a CH-filtered digital stillcamera (a) Normal flame (U = 40 cms) (b) FREI (U= 20 cms) and (c) weak flames (U = 30 cms) Computed profiles of major species at U = 20 cms
Vertical dotted lines indicate the locations of HRR peaks
Akira Yamamoto Hiroshi Oshibe Hisashi Nakamura Takuya Tezuka Susumu Hasegawa Kaoru Maruta
Proceedings of the Combustion Institute vol 33 pp 3259‐3266 (2011)
Three distinct temperature regimes nC7H16
0
300
600
900
1200
1500
000 020 040 060 080 100
Tem
pera
ture
-K
Time - seconds
n-heptane RON = 0
heat release rateTemperature
Slide courtesy of Dr Charles Westbrook10
Three distinct temperature regimes nC7H16
11ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
Intermediate TḢ + O2 (+M) = HȮ2 (+M)RH + HȮ2 = R+ H2O2
H2O2 (+M) = ȮH + ȮH (+M)R + O2harr RȮ2
RȮ2 rarr olefin + HȮ2
High TFuel = R + Rprime
R = olefin + ĊH3 or ḢḢ + O2 = Ouml + ȮH
ĊH3 + O2 = CH2O + ȮH
22
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
12
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Ḣ + O2 (+M) = HȮ2 (+M)RH + HȮ2 = R+ H2O2
H2O2 (+M) = ȮH + ȮH (+M)R + O2harr RȮ2
RȮ2 rarr olefin + HȮ2
Three distinct temperature regimes
13
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
14ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Importance of concerted HȮ2 elimination reaction
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
15
Intermediate temperature chemistrymdash Concerted eliminations are not well known ndash quantum chemistry
mdash Quelch et al1 first proposed Ċ2H5 + O2 = C2H4 + HȮ2 cyclic TS via concerted elimination
mdash Miyoshi23 variational TST and RRKMmaster equation (Ċ2iĊ3n‐s‐t‐Ċ4 + O2)
mdash Villano et al45 calculated 23 different straight and branched alkyl‐peroxyl radicals
mdash Goldsmith et al6 for the propyl + O2 system
Need for further studies of these reactions due to their high importance
1GE Quelch MM Gallo M Shen Y Xie HF Schaefer III D Moncrieff J Am Chem Soc 116 (1994) 4953ndash49622A Miyoshi J Phys Chem A 115 (2011) 3301ndash33253A Miyoshi A Int J Chem Kinet 44 (2012) 59ndash744SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 115 (2011) 13425ndash134425SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 116 (2012) 5068ndash50896CF Goldsmith WH Green SJ Klippenstein J Phys Chem A 2012 116 3325ndash3346
16
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
17
Few direct measurements of H‐atom abstraction by HȮ2 ndash lack of suitable precursors mdash CH2O + HȮ2 Jemi‐Alade et al1 using flash photolysismdash Walker et al23 made indirect relative rate measurementsmdash Scott and Walker4 review of alkanes aromatics and related compounds in 2002
Recent developments in quantitative measurements of HȮ2 radicals mdash Fluorescence assay by Gas Expansion by Blocquet et al5 (2013)mdash Dual‐modulation Faraday Spectroscopy67 (2014 2015)mdash Cavity ring‐down spectroscopy8 (2014)
These measurements are very useful in assessing mechanism performance1AA Jemi‐Alade PD Lightfoot R Lesclaux Chem Phys Lett 195 (1992) 25ndash302RR Baldwin RW Walker Proc Combust Inst 17 (1979) 525ndash5333RW Walker C Morley in Comprehensive Chem Kinetics (M J Pilling Ed) Elsevier Amsterdam 351 (1997)4M Scott RW Walker Combust Flame 129 (2002) 365ndash3775M Blocquet C Schoemaecker D Amedro O Herbinet F Battin‐Leclerc C Fittschen Proc Natl Acad Sci U S A 110 (2013) 20014ndash200176B Brumfield WT Sun Y Wang Y Ju G Wysocki Opt Lett 39 (2014) 1783ndash17867N Kurimoto B Brumfield X Yang T Wada P Dieacutevart G Wysocki Y Ju Proc Combust Inst 35(1) (2015) 457ndash4648M Djehiche NL Le Tan CD Jain G Dayma P Dagaut C Chauveau L Pillier A Tomas J Am Chem Soc 136 (2014) 16689ndash16694
93
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
18
CH3OH oxidation 855 O2 p = 40 atm and T = 885 K
Sensitivity to ignition delay timeU Burke WK Metcalfe SM Burke KA Heufer P Dagaut HJ Curran Combust Flame 165 (2016) 125ndash13694
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
19
CH3OH + HȮ2 = ĊH2OH + H2O2
05 10 15 20104
105
106
107
108
109
1010
1011
1012
rate
con
stan
t (k)
cm
3 mol
-1 s
-1
1000 K T
Altarawneh (2011) Olm et al (2017) Alecu and Truhlar (2011) Klippenstein (2011)
104
105
106
107
108
109
1010
1011
1012
2000 1500 1000 500T K
20
Klippenstein et al1 reported high sensitivity to CH3OH + HȮ2 also calculated k Altarawneh et al2 and Alecu and Truhlar3
Olm et al4 via computer optimization using direct and indirect measurements Alecu and Truhlar attributed differences with Klippenstein et al calculations to
differences in treatment of anharmonicity
Possible chemically activated reactions involving HȮ2 radicals
1SJ Klippenstein LB Harding MJ Davis AS Tomlin RT Skodje Proc Combust Inst 33 (2011) 351ndash3572M Altarawneh AH Al‐Muhtaseb BZ Dlugogorski EM Kennedy JC Mackie J Comp Chem 32 (2011) 1725ndash17333IM Alecu DG Truhlar J Phys Chem A 115 (2011) 14599ndash146114C Olm T Varga Eacute Valkoacute HJ Curran T Turaacutenyi Combust Flame 186 (2017) 45ndash64
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
21
Carstensen and Dean12 for CH4 C2H6 C3H8 C4H10 + HȮ2
Aguilera‐Iparraguirre et al3 CH4 C2H6 C3H8 nC4H10 iC4H10 + HȮ2
mdashAgree well with the determinations of Walker et al
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash1573J Aguilera‐Iparraguirre HJ Curran W Klopper JM Simmie J Phys Chem A 112 (2008) 7047ndash7054
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
22ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
RH + CH3Ȯ2 = R + CH3O2H can also be important
HJ Curran P Gaffuri WJ Pitz CK WestbrookCombustion and Flame 129253ndash280 (2002)
iC8H18 oxidationφ = 10 in air p = 40 atm
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
23
RH + CH3Ȯ2 = R + CH3O2HĊH3 + O2 = CH3Ȯ2
RH + CH3Ȯ2 = R + CH3O2HCH3O2H = CH3Ȯ + ȮH
Carstensen and Dean1 for CH4C2H6 + ḢCH3Ȯ2C2H5Ȯ2
CarstensenDeanDeutschmann2 for CH4 C2H6 C3H8 C4H10 + HȮ2 CH3Ȯ2 C2H5Ȯ2 C3H7Ȯ2 C3H7Ȯ2 HC(O)Ȯ2 CH3C(O)Ȯ2
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash157
24ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
25
Rate rules for large molecular weight molecules
bull High temperature mechanismReaction class 1 Unimolecular fuel decompositionReaction class 2 H atom abstractions from fuelReaction class 3 Alkyl radical decompositionReaction class 4 Alkyl radical + O2 = olefin + HȮ2
Reaction class 5 Alkyl radical isomerizationReaction class 6 H atom abstraction from olefinsReaction class 7 Addition of radical species to olefinsReaction class 8 Alkenyl radical decompositionReaction class 9 Olefin decomposition
26Slide Courtesy of Dr William Pitz
Reaction rate rules for higher MW species
27Slide Courtesy of Dr William Pitz
Reaction classes for low temperature reactionsLow temperature mechanismReaction class 10 Alkyl radical addition to O2 (R + O2)Reaction class 11 R + RrsquoO2 = RȮ + RrsquoȮReaction class 12 Alkylperoxy radical isomerizationReaction class 13 RȮ2 + HȮ2 = ROOH + O2Reaction class 14 RȮ2 + H2O2 = ROOH + HȮ2Reaction class 15 RȮ2 + CH3Ȯ2 = RȮ + CH3Ȯ +O2Reaction class 16 RȮ2 + RrsquoȮ2 = RȮ + RrsquoȮ + O2Reaction class 17 ROOH = RȮ + ȮHReaction class 18 RȮ DecompositionReaction class 19 QOOH = Cyclic Ether + ȮHReaction class 20 QOOH = Olefin + HȮ2Reaction class 21 QOOH = Olefin + Aldehyde or Carbonyl + ȮHReaction class 22 Addition of QOOH to molecular oxygen O2Reaction class 23 Ȯ2QOOH isomerization to carbonylhydroperoxide + ȮHReaction class 24 Carbonylhydroperoxide decompositionReaction class 25 Reactions of cyclic ethers with ȮH and HȮ2
28
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
TF Lu CK Law lsquoToward accommodating realistic fuel chemistry in large‐scale computationsrsquoProgress in Energy and Combustion Science 35 (2009) 192ndash215
Methyl decanoate is a biomass fuel surrogate Detailed kinetic mechanism consists of 3036 species and 8555 reactions
Automatic Generation of kinetic mechanisms easily produces
Large Kinetic Models
Mechanism Size
3
Mechanism Size
Mechanism size grows with molecule size
4
Dominance of H2O2 Reactions
For nearly all hydrocarbon oxidation no matterhow large or small the fuel molecule at hightemperatures the reactions of H2O2 have thegreatest sensitivity controlling the overall rate ofreaction This is true in flames detonations shocktubes and many other practical combustors
5
Combustion Chemistry Complexity
6
Low temperature High temperature
+ O2 Oxidation
Pyrolysis
Pyrolysis
+ O2 Oxidation
Courtesy of Prof Tiziano Faravelli Politecnico di Milano
7
R + O2 harr RȮ2 Low TRȮ2 QOOH (~500 850 K)
QOOH + O2 harr Ȯ2QOOH Ȯ2QOOH RȮ + ȮH + ȮH
conversion
Reactor Temperature
Zhandong Wang Proc Natl Acad Sci 114(50) (2017) 13102ndash13107Zhandong Wang et al Combust Flame 187 (2018) 199ndash216
Evidence of further additions to O2 have been reported
Three distinct temperature regimes
8
Negative Temperature Coefficient Regime
Intermediate T (850 1100 K)RȮ2 rarr olefin + HȮ2 (NTC)
QOOH rarr cyclic ether + ȮH (NTC)
Three distinct temperature regimes
conversion
Reactor Temperature
9
Flame images taken by a CH-filtered digital stillcamera (a) Normal flame (U = 40 cms) (b) FREI (U= 20 cms) and (c) weak flames (U = 30 cms) Computed profiles of major species at U = 20 cms
Vertical dotted lines indicate the locations of HRR peaks
Akira Yamamoto Hiroshi Oshibe Hisashi Nakamura Takuya Tezuka Susumu Hasegawa Kaoru Maruta
Proceedings of the Combustion Institute vol 33 pp 3259‐3266 (2011)
Three distinct temperature regimes nC7H16
0
300
600
900
1200
1500
000 020 040 060 080 100
Tem
pera
ture
-K
Time - seconds
n-heptane RON = 0
heat release rateTemperature
Slide courtesy of Dr Charles Westbrook10
Three distinct temperature regimes nC7H16
11ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
Intermediate TḢ + O2 (+M) = HȮ2 (+M)RH + HȮ2 = R+ H2O2
H2O2 (+M) = ȮH + ȮH (+M)R + O2harr RȮ2
RȮ2 rarr olefin + HȮ2
High TFuel = R + Rprime
R = olefin + ĊH3 or ḢḢ + O2 = Ouml + ȮH
ĊH3 + O2 = CH2O + ȮH
22
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
12
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Ḣ + O2 (+M) = HȮ2 (+M)RH + HȮ2 = R+ H2O2
H2O2 (+M) = ȮH + ȮH (+M)R + O2harr RȮ2
RȮ2 rarr olefin + HȮ2
Three distinct temperature regimes
13
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
14ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Importance of concerted HȮ2 elimination reaction
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
15
Intermediate temperature chemistrymdash Concerted eliminations are not well known ndash quantum chemistry
mdash Quelch et al1 first proposed Ċ2H5 + O2 = C2H4 + HȮ2 cyclic TS via concerted elimination
mdash Miyoshi23 variational TST and RRKMmaster equation (Ċ2iĊ3n‐s‐t‐Ċ4 + O2)
mdash Villano et al45 calculated 23 different straight and branched alkyl‐peroxyl radicals
mdash Goldsmith et al6 for the propyl + O2 system
Need for further studies of these reactions due to their high importance
1GE Quelch MM Gallo M Shen Y Xie HF Schaefer III D Moncrieff J Am Chem Soc 116 (1994) 4953ndash49622A Miyoshi J Phys Chem A 115 (2011) 3301ndash33253A Miyoshi A Int J Chem Kinet 44 (2012) 59ndash744SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 115 (2011) 13425ndash134425SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 116 (2012) 5068ndash50896CF Goldsmith WH Green SJ Klippenstein J Phys Chem A 2012 116 3325ndash3346
16
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
17
Few direct measurements of H‐atom abstraction by HȮ2 ndash lack of suitable precursors mdash CH2O + HȮ2 Jemi‐Alade et al1 using flash photolysismdash Walker et al23 made indirect relative rate measurementsmdash Scott and Walker4 review of alkanes aromatics and related compounds in 2002
Recent developments in quantitative measurements of HȮ2 radicals mdash Fluorescence assay by Gas Expansion by Blocquet et al5 (2013)mdash Dual‐modulation Faraday Spectroscopy67 (2014 2015)mdash Cavity ring‐down spectroscopy8 (2014)
These measurements are very useful in assessing mechanism performance1AA Jemi‐Alade PD Lightfoot R Lesclaux Chem Phys Lett 195 (1992) 25ndash302RR Baldwin RW Walker Proc Combust Inst 17 (1979) 525ndash5333RW Walker C Morley in Comprehensive Chem Kinetics (M J Pilling Ed) Elsevier Amsterdam 351 (1997)4M Scott RW Walker Combust Flame 129 (2002) 365ndash3775M Blocquet C Schoemaecker D Amedro O Herbinet F Battin‐Leclerc C Fittschen Proc Natl Acad Sci U S A 110 (2013) 20014ndash200176B Brumfield WT Sun Y Wang Y Ju G Wysocki Opt Lett 39 (2014) 1783ndash17867N Kurimoto B Brumfield X Yang T Wada P Dieacutevart G Wysocki Y Ju Proc Combust Inst 35(1) (2015) 457ndash4648M Djehiche NL Le Tan CD Jain G Dayma P Dagaut C Chauveau L Pillier A Tomas J Am Chem Soc 136 (2014) 16689ndash16694
93
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
18
CH3OH oxidation 855 O2 p = 40 atm and T = 885 K
Sensitivity to ignition delay timeU Burke WK Metcalfe SM Burke KA Heufer P Dagaut HJ Curran Combust Flame 165 (2016) 125ndash13694
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
19
CH3OH + HȮ2 = ĊH2OH + H2O2
05 10 15 20104
105
106
107
108
109
1010
1011
1012
rate
con
stan
t (k)
cm
3 mol
-1 s
-1
1000 K T
Altarawneh (2011) Olm et al (2017) Alecu and Truhlar (2011) Klippenstein (2011)
104
105
106
107
108
109
1010
1011
1012
2000 1500 1000 500T K
20
Klippenstein et al1 reported high sensitivity to CH3OH + HȮ2 also calculated k Altarawneh et al2 and Alecu and Truhlar3
Olm et al4 via computer optimization using direct and indirect measurements Alecu and Truhlar attributed differences with Klippenstein et al calculations to
differences in treatment of anharmonicity
Possible chemically activated reactions involving HȮ2 radicals
1SJ Klippenstein LB Harding MJ Davis AS Tomlin RT Skodje Proc Combust Inst 33 (2011) 351ndash3572M Altarawneh AH Al‐Muhtaseb BZ Dlugogorski EM Kennedy JC Mackie J Comp Chem 32 (2011) 1725ndash17333IM Alecu DG Truhlar J Phys Chem A 115 (2011) 14599ndash146114C Olm T Varga Eacute Valkoacute HJ Curran T Turaacutenyi Combust Flame 186 (2017) 45ndash64
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
21
Carstensen and Dean12 for CH4 C2H6 C3H8 C4H10 + HȮ2
Aguilera‐Iparraguirre et al3 CH4 C2H6 C3H8 nC4H10 iC4H10 + HȮ2
mdashAgree well with the determinations of Walker et al
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash1573J Aguilera‐Iparraguirre HJ Curran W Klopper JM Simmie J Phys Chem A 112 (2008) 7047ndash7054
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
22ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
RH + CH3Ȯ2 = R + CH3O2H can also be important
HJ Curran P Gaffuri WJ Pitz CK WestbrookCombustion and Flame 129253ndash280 (2002)
iC8H18 oxidationφ = 10 in air p = 40 atm
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
23
RH + CH3Ȯ2 = R + CH3O2HĊH3 + O2 = CH3Ȯ2
RH + CH3Ȯ2 = R + CH3O2HCH3O2H = CH3Ȯ + ȮH
Carstensen and Dean1 for CH4C2H6 + ḢCH3Ȯ2C2H5Ȯ2
CarstensenDeanDeutschmann2 for CH4 C2H6 C3H8 C4H10 + HȮ2 CH3Ȯ2 C2H5Ȯ2 C3H7Ȯ2 C3H7Ȯ2 HC(O)Ȯ2 CH3C(O)Ȯ2
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash157
24ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
25
Rate rules for large molecular weight molecules
bull High temperature mechanismReaction class 1 Unimolecular fuel decompositionReaction class 2 H atom abstractions from fuelReaction class 3 Alkyl radical decompositionReaction class 4 Alkyl radical + O2 = olefin + HȮ2
Reaction class 5 Alkyl radical isomerizationReaction class 6 H atom abstraction from olefinsReaction class 7 Addition of radical species to olefinsReaction class 8 Alkenyl radical decompositionReaction class 9 Olefin decomposition
26Slide Courtesy of Dr William Pitz
Reaction rate rules for higher MW species
27Slide Courtesy of Dr William Pitz
Reaction classes for low temperature reactionsLow temperature mechanismReaction class 10 Alkyl radical addition to O2 (R + O2)Reaction class 11 R + RrsquoO2 = RȮ + RrsquoȮReaction class 12 Alkylperoxy radical isomerizationReaction class 13 RȮ2 + HȮ2 = ROOH + O2Reaction class 14 RȮ2 + H2O2 = ROOH + HȮ2Reaction class 15 RȮ2 + CH3Ȯ2 = RȮ + CH3Ȯ +O2Reaction class 16 RȮ2 + RrsquoȮ2 = RȮ + RrsquoȮ + O2Reaction class 17 ROOH = RȮ + ȮHReaction class 18 RȮ DecompositionReaction class 19 QOOH = Cyclic Ether + ȮHReaction class 20 QOOH = Olefin + HȮ2Reaction class 21 QOOH = Olefin + Aldehyde or Carbonyl + ȮHReaction class 22 Addition of QOOH to molecular oxygen O2Reaction class 23 Ȯ2QOOH isomerization to carbonylhydroperoxide + ȮHReaction class 24 Carbonylhydroperoxide decompositionReaction class 25 Reactions of cyclic ethers with ȮH and HȮ2
28
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Mechanism Size
Mechanism size grows with molecule size
4
Dominance of H2O2 Reactions
For nearly all hydrocarbon oxidation no matterhow large or small the fuel molecule at hightemperatures the reactions of H2O2 have thegreatest sensitivity controlling the overall rate ofreaction This is true in flames detonations shocktubes and many other practical combustors
5
Combustion Chemistry Complexity
6
Low temperature High temperature
+ O2 Oxidation
Pyrolysis
Pyrolysis
+ O2 Oxidation
Courtesy of Prof Tiziano Faravelli Politecnico di Milano
7
R + O2 harr RȮ2 Low TRȮ2 QOOH (~500 850 K)
QOOH + O2 harr Ȯ2QOOH Ȯ2QOOH RȮ + ȮH + ȮH
conversion
Reactor Temperature
Zhandong Wang Proc Natl Acad Sci 114(50) (2017) 13102ndash13107Zhandong Wang et al Combust Flame 187 (2018) 199ndash216
Evidence of further additions to O2 have been reported
Three distinct temperature regimes
8
Negative Temperature Coefficient Regime
Intermediate T (850 1100 K)RȮ2 rarr olefin + HȮ2 (NTC)
QOOH rarr cyclic ether + ȮH (NTC)
Three distinct temperature regimes
conversion
Reactor Temperature
9
Flame images taken by a CH-filtered digital stillcamera (a) Normal flame (U = 40 cms) (b) FREI (U= 20 cms) and (c) weak flames (U = 30 cms) Computed profiles of major species at U = 20 cms
Vertical dotted lines indicate the locations of HRR peaks
Akira Yamamoto Hiroshi Oshibe Hisashi Nakamura Takuya Tezuka Susumu Hasegawa Kaoru Maruta
Proceedings of the Combustion Institute vol 33 pp 3259‐3266 (2011)
Three distinct temperature regimes nC7H16
0
300
600
900
1200
1500
000 020 040 060 080 100
Tem
pera
ture
-K
Time - seconds
n-heptane RON = 0
heat release rateTemperature
Slide courtesy of Dr Charles Westbrook10
Three distinct temperature regimes nC7H16
11ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
Intermediate TḢ + O2 (+M) = HȮ2 (+M)RH + HȮ2 = R+ H2O2
H2O2 (+M) = ȮH + ȮH (+M)R + O2harr RȮ2
RȮ2 rarr olefin + HȮ2
High TFuel = R + Rprime
R = olefin + ĊH3 or ḢḢ + O2 = Ouml + ȮH
ĊH3 + O2 = CH2O + ȮH
22
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
12
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Ḣ + O2 (+M) = HȮ2 (+M)RH + HȮ2 = R+ H2O2
H2O2 (+M) = ȮH + ȮH (+M)R + O2harr RȮ2
RȮ2 rarr olefin + HȮ2
Three distinct temperature regimes
13
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
14ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Importance of concerted HȮ2 elimination reaction
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
15
Intermediate temperature chemistrymdash Concerted eliminations are not well known ndash quantum chemistry
mdash Quelch et al1 first proposed Ċ2H5 + O2 = C2H4 + HȮ2 cyclic TS via concerted elimination
mdash Miyoshi23 variational TST and RRKMmaster equation (Ċ2iĊ3n‐s‐t‐Ċ4 + O2)
mdash Villano et al45 calculated 23 different straight and branched alkyl‐peroxyl radicals
mdash Goldsmith et al6 for the propyl + O2 system
Need for further studies of these reactions due to their high importance
1GE Quelch MM Gallo M Shen Y Xie HF Schaefer III D Moncrieff J Am Chem Soc 116 (1994) 4953ndash49622A Miyoshi J Phys Chem A 115 (2011) 3301ndash33253A Miyoshi A Int J Chem Kinet 44 (2012) 59ndash744SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 115 (2011) 13425ndash134425SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 116 (2012) 5068ndash50896CF Goldsmith WH Green SJ Klippenstein J Phys Chem A 2012 116 3325ndash3346
16
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
17
Few direct measurements of H‐atom abstraction by HȮ2 ndash lack of suitable precursors mdash CH2O + HȮ2 Jemi‐Alade et al1 using flash photolysismdash Walker et al23 made indirect relative rate measurementsmdash Scott and Walker4 review of alkanes aromatics and related compounds in 2002
Recent developments in quantitative measurements of HȮ2 radicals mdash Fluorescence assay by Gas Expansion by Blocquet et al5 (2013)mdash Dual‐modulation Faraday Spectroscopy67 (2014 2015)mdash Cavity ring‐down spectroscopy8 (2014)
These measurements are very useful in assessing mechanism performance1AA Jemi‐Alade PD Lightfoot R Lesclaux Chem Phys Lett 195 (1992) 25ndash302RR Baldwin RW Walker Proc Combust Inst 17 (1979) 525ndash5333RW Walker C Morley in Comprehensive Chem Kinetics (M J Pilling Ed) Elsevier Amsterdam 351 (1997)4M Scott RW Walker Combust Flame 129 (2002) 365ndash3775M Blocquet C Schoemaecker D Amedro O Herbinet F Battin‐Leclerc C Fittschen Proc Natl Acad Sci U S A 110 (2013) 20014ndash200176B Brumfield WT Sun Y Wang Y Ju G Wysocki Opt Lett 39 (2014) 1783ndash17867N Kurimoto B Brumfield X Yang T Wada P Dieacutevart G Wysocki Y Ju Proc Combust Inst 35(1) (2015) 457ndash4648M Djehiche NL Le Tan CD Jain G Dayma P Dagaut C Chauveau L Pillier A Tomas J Am Chem Soc 136 (2014) 16689ndash16694
93
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
18
CH3OH oxidation 855 O2 p = 40 atm and T = 885 K
Sensitivity to ignition delay timeU Burke WK Metcalfe SM Burke KA Heufer P Dagaut HJ Curran Combust Flame 165 (2016) 125ndash13694
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
19
CH3OH + HȮ2 = ĊH2OH + H2O2
05 10 15 20104
105
106
107
108
109
1010
1011
1012
rate
con
stan
t (k)
cm
3 mol
-1 s
-1
1000 K T
Altarawneh (2011) Olm et al (2017) Alecu and Truhlar (2011) Klippenstein (2011)
104
105
106
107
108
109
1010
1011
1012
2000 1500 1000 500T K
20
Klippenstein et al1 reported high sensitivity to CH3OH + HȮ2 also calculated k Altarawneh et al2 and Alecu and Truhlar3
Olm et al4 via computer optimization using direct and indirect measurements Alecu and Truhlar attributed differences with Klippenstein et al calculations to
differences in treatment of anharmonicity
Possible chemically activated reactions involving HȮ2 radicals
1SJ Klippenstein LB Harding MJ Davis AS Tomlin RT Skodje Proc Combust Inst 33 (2011) 351ndash3572M Altarawneh AH Al‐Muhtaseb BZ Dlugogorski EM Kennedy JC Mackie J Comp Chem 32 (2011) 1725ndash17333IM Alecu DG Truhlar J Phys Chem A 115 (2011) 14599ndash146114C Olm T Varga Eacute Valkoacute HJ Curran T Turaacutenyi Combust Flame 186 (2017) 45ndash64
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
21
Carstensen and Dean12 for CH4 C2H6 C3H8 C4H10 + HȮ2
Aguilera‐Iparraguirre et al3 CH4 C2H6 C3H8 nC4H10 iC4H10 + HȮ2
mdashAgree well with the determinations of Walker et al
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash1573J Aguilera‐Iparraguirre HJ Curran W Klopper JM Simmie J Phys Chem A 112 (2008) 7047ndash7054
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
22ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
RH + CH3Ȯ2 = R + CH3O2H can also be important
HJ Curran P Gaffuri WJ Pitz CK WestbrookCombustion and Flame 129253ndash280 (2002)
iC8H18 oxidationφ = 10 in air p = 40 atm
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
23
RH + CH3Ȯ2 = R + CH3O2HĊH3 + O2 = CH3Ȯ2
RH + CH3Ȯ2 = R + CH3O2HCH3O2H = CH3Ȯ + ȮH
Carstensen and Dean1 for CH4C2H6 + ḢCH3Ȯ2C2H5Ȯ2
CarstensenDeanDeutschmann2 for CH4 C2H6 C3H8 C4H10 + HȮ2 CH3Ȯ2 C2H5Ȯ2 C3H7Ȯ2 C3H7Ȯ2 HC(O)Ȯ2 CH3C(O)Ȯ2
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash157
24ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
25
Rate rules for large molecular weight molecules
bull High temperature mechanismReaction class 1 Unimolecular fuel decompositionReaction class 2 H atom abstractions from fuelReaction class 3 Alkyl radical decompositionReaction class 4 Alkyl radical + O2 = olefin + HȮ2
Reaction class 5 Alkyl radical isomerizationReaction class 6 H atom abstraction from olefinsReaction class 7 Addition of radical species to olefinsReaction class 8 Alkenyl radical decompositionReaction class 9 Olefin decomposition
26Slide Courtesy of Dr William Pitz
Reaction rate rules for higher MW species
27Slide Courtesy of Dr William Pitz
Reaction classes for low temperature reactionsLow temperature mechanismReaction class 10 Alkyl radical addition to O2 (R + O2)Reaction class 11 R + RrsquoO2 = RȮ + RrsquoȮReaction class 12 Alkylperoxy radical isomerizationReaction class 13 RȮ2 + HȮ2 = ROOH + O2Reaction class 14 RȮ2 + H2O2 = ROOH + HȮ2Reaction class 15 RȮ2 + CH3Ȯ2 = RȮ + CH3Ȯ +O2Reaction class 16 RȮ2 + RrsquoȮ2 = RȮ + RrsquoȮ + O2Reaction class 17 ROOH = RȮ + ȮHReaction class 18 RȮ DecompositionReaction class 19 QOOH = Cyclic Ether + ȮHReaction class 20 QOOH = Olefin + HȮ2Reaction class 21 QOOH = Olefin + Aldehyde or Carbonyl + ȮHReaction class 22 Addition of QOOH to molecular oxygen O2Reaction class 23 Ȯ2QOOH isomerization to carbonylhydroperoxide + ȮHReaction class 24 Carbonylhydroperoxide decompositionReaction class 25 Reactions of cyclic ethers with ȮH and HȮ2
28
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Dominance of H2O2 Reactions
For nearly all hydrocarbon oxidation no matterhow large or small the fuel molecule at hightemperatures the reactions of H2O2 have thegreatest sensitivity controlling the overall rate ofreaction This is true in flames detonations shocktubes and many other practical combustors
5
Combustion Chemistry Complexity
6
Low temperature High temperature
+ O2 Oxidation
Pyrolysis
Pyrolysis
+ O2 Oxidation
Courtesy of Prof Tiziano Faravelli Politecnico di Milano
7
R + O2 harr RȮ2 Low TRȮ2 QOOH (~500 850 K)
QOOH + O2 harr Ȯ2QOOH Ȯ2QOOH RȮ + ȮH + ȮH
conversion
Reactor Temperature
Zhandong Wang Proc Natl Acad Sci 114(50) (2017) 13102ndash13107Zhandong Wang et al Combust Flame 187 (2018) 199ndash216
Evidence of further additions to O2 have been reported
Three distinct temperature regimes
8
Negative Temperature Coefficient Regime
Intermediate T (850 1100 K)RȮ2 rarr olefin + HȮ2 (NTC)
QOOH rarr cyclic ether + ȮH (NTC)
Three distinct temperature regimes
conversion
Reactor Temperature
9
Flame images taken by a CH-filtered digital stillcamera (a) Normal flame (U = 40 cms) (b) FREI (U= 20 cms) and (c) weak flames (U = 30 cms) Computed profiles of major species at U = 20 cms
Vertical dotted lines indicate the locations of HRR peaks
Akira Yamamoto Hiroshi Oshibe Hisashi Nakamura Takuya Tezuka Susumu Hasegawa Kaoru Maruta
Proceedings of the Combustion Institute vol 33 pp 3259‐3266 (2011)
Three distinct temperature regimes nC7H16
0
300
600
900
1200
1500
000 020 040 060 080 100
Tem
pera
ture
-K
Time - seconds
n-heptane RON = 0
heat release rateTemperature
Slide courtesy of Dr Charles Westbrook10
Three distinct temperature regimes nC7H16
11ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
Intermediate TḢ + O2 (+M) = HȮ2 (+M)RH + HȮ2 = R+ H2O2
H2O2 (+M) = ȮH + ȮH (+M)R + O2harr RȮ2
RȮ2 rarr olefin + HȮ2
High TFuel = R + Rprime
R = olefin + ĊH3 or ḢḢ + O2 = Ouml + ȮH
ĊH3 + O2 = CH2O + ȮH
22
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
12
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Ḣ + O2 (+M) = HȮ2 (+M)RH + HȮ2 = R+ H2O2
H2O2 (+M) = ȮH + ȮH (+M)R + O2harr RȮ2
RȮ2 rarr olefin + HȮ2
Three distinct temperature regimes
13
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
14ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Importance of concerted HȮ2 elimination reaction
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
15
Intermediate temperature chemistrymdash Concerted eliminations are not well known ndash quantum chemistry
mdash Quelch et al1 first proposed Ċ2H5 + O2 = C2H4 + HȮ2 cyclic TS via concerted elimination
mdash Miyoshi23 variational TST and RRKMmaster equation (Ċ2iĊ3n‐s‐t‐Ċ4 + O2)
mdash Villano et al45 calculated 23 different straight and branched alkyl‐peroxyl radicals
mdash Goldsmith et al6 for the propyl + O2 system
Need for further studies of these reactions due to their high importance
1GE Quelch MM Gallo M Shen Y Xie HF Schaefer III D Moncrieff J Am Chem Soc 116 (1994) 4953ndash49622A Miyoshi J Phys Chem A 115 (2011) 3301ndash33253A Miyoshi A Int J Chem Kinet 44 (2012) 59ndash744SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 115 (2011) 13425ndash134425SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 116 (2012) 5068ndash50896CF Goldsmith WH Green SJ Klippenstein J Phys Chem A 2012 116 3325ndash3346
16
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
17
Few direct measurements of H‐atom abstraction by HȮ2 ndash lack of suitable precursors mdash CH2O + HȮ2 Jemi‐Alade et al1 using flash photolysismdash Walker et al23 made indirect relative rate measurementsmdash Scott and Walker4 review of alkanes aromatics and related compounds in 2002
Recent developments in quantitative measurements of HȮ2 radicals mdash Fluorescence assay by Gas Expansion by Blocquet et al5 (2013)mdash Dual‐modulation Faraday Spectroscopy67 (2014 2015)mdash Cavity ring‐down spectroscopy8 (2014)
These measurements are very useful in assessing mechanism performance1AA Jemi‐Alade PD Lightfoot R Lesclaux Chem Phys Lett 195 (1992) 25ndash302RR Baldwin RW Walker Proc Combust Inst 17 (1979) 525ndash5333RW Walker C Morley in Comprehensive Chem Kinetics (M J Pilling Ed) Elsevier Amsterdam 351 (1997)4M Scott RW Walker Combust Flame 129 (2002) 365ndash3775M Blocquet C Schoemaecker D Amedro O Herbinet F Battin‐Leclerc C Fittschen Proc Natl Acad Sci U S A 110 (2013) 20014ndash200176B Brumfield WT Sun Y Wang Y Ju G Wysocki Opt Lett 39 (2014) 1783ndash17867N Kurimoto B Brumfield X Yang T Wada P Dieacutevart G Wysocki Y Ju Proc Combust Inst 35(1) (2015) 457ndash4648M Djehiche NL Le Tan CD Jain G Dayma P Dagaut C Chauveau L Pillier A Tomas J Am Chem Soc 136 (2014) 16689ndash16694
93
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
18
CH3OH oxidation 855 O2 p = 40 atm and T = 885 K
Sensitivity to ignition delay timeU Burke WK Metcalfe SM Burke KA Heufer P Dagaut HJ Curran Combust Flame 165 (2016) 125ndash13694
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
19
CH3OH + HȮ2 = ĊH2OH + H2O2
05 10 15 20104
105
106
107
108
109
1010
1011
1012
rate
con
stan
t (k)
cm
3 mol
-1 s
-1
1000 K T
Altarawneh (2011) Olm et al (2017) Alecu and Truhlar (2011) Klippenstein (2011)
104
105
106
107
108
109
1010
1011
1012
2000 1500 1000 500T K
20
Klippenstein et al1 reported high sensitivity to CH3OH + HȮ2 also calculated k Altarawneh et al2 and Alecu and Truhlar3
Olm et al4 via computer optimization using direct and indirect measurements Alecu and Truhlar attributed differences with Klippenstein et al calculations to
differences in treatment of anharmonicity
Possible chemically activated reactions involving HȮ2 radicals
1SJ Klippenstein LB Harding MJ Davis AS Tomlin RT Skodje Proc Combust Inst 33 (2011) 351ndash3572M Altarawneh AH Al‐Muhtaseb BZ Dlugogorski EM Kennedy JC Mackie J Comp Chem 32 (2011) 1725ndash17333IM Alecu DG Truhlar J Phys Chem A 115 (2011) 14599ndash146114C Olm T Varga Eacute Valkoacute HJ Curran T Turaacutenyi Combust Flame 186 (2017) 45ndash64
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
21
Carstensen and Dean12 for CH4 C2H6 C3H8 C4H10 + HȮ2
Aguilera‐Iparraguirre et al3 CH4 C2H6 C3H8 nC4H10 iC4H10 + HȮ2
mdashAgree well with the determinations of Walker et al
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash1573J Aguilera‐Iparraguirre HJ Curran W Klopper JM Simmie J Phys Chem A 112 (2008) 7047ndash7054
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
22ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
RH + CH3Ȯ2 = R + CH3O2H can also be important
HJ Curran P Gaffuri WJ Pitz CK WestbrookCombustion and Flame 129253ndash280 (2002)
iC8H18 oxidationφ = 10 in air p = 40 atm
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
23
RH + CH3Ȯ2 = R + CH3O2HĊH3 + O2 = CH3Ȯ2
RH + CH3Ȯ2 = R + CH3O2HCH3O2H = CH3Ȯ + ȮH
Carstensen and Dean1 for CH4C2H6 + ḢCH3Ȯ2C2H5Ȯ2
CarstensenDeanDeutschmann2 for CH4 C2H6 C3H8 C4H10 + HȮ2 CH3Ȯ2 C2H5Ȯ2 C3H7Ȯ2 C3H7Ȯ2 HC(O)Ȯ2 CH3C(O)Ȯ2
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash157
24ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
25
Rate rules for large molecular weight molecules
bull High temperature mechanismReaction class 1 Unimolecular fuel decompositionReaction class 2 H atom abstractions from fuelReaction class 3 Alkyl radical decompositionReaction class 4 Alkyl radical + O2 = olefin + HȮ2
Reaction class 5 Alkyl radical isomerizationReaction class 6 H atom abstraction from olefinsReaction class 7 Addition of radical species to olefinsReaction class 8 Alkenyl radical decompositionReaction class 9 Olefin decomposition
26Slide Courtesy of Dr William Pitz
Reaction rate rules for higher MW species
27Slide Courtesy of Dr William Pitz
Reaction classes for low temperature reactionsLow temperature mechanismReaction class 10 Alkyl radical addition to O2 (R + O2)Reaction class 11 R + RrsquoO2 = RȮ + RrsquoȮReaction class 12 Alkylperoxy radical isomerizationReaction class 13 RȮ2 + HȮ2 = ROOH + O2Reaction class 14 RȮ2 + H2O2 = ROOH + HȮ2Reaction class 15 RȮ2 + CH3Ȯ2 = RȮ + CH3Ȯ +O2Reaction class 16 RȮ2 + RrsquoȮ2 = RȮ + RrsquoȮ + O2Reaction class 17 ROOH = RȮ + ȮHReaction class 18 RȮ DecompositionReaction class 19 QOOH = Cyclic Ether + ȮHReaction class 20 QOOH = Olefin + HȮ2Reaction class 21 QOOH = Olefin + Aldehyde or Carbonyl + ȮHReaction class 22 Addition of QOOH to molecular oxygen O2Reaction class 23 Ȯ2QOOH isomerization to carbonylhydroperoxide + ȮHReaction class 24 Carbonylhydroperoxide decompositionReaction class 25 Reactions of cyclic ethers with ȮH and HȮ2
28
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Combustion Chemistry Complexity
6
Low temperature High temperature
+ O2 Oxidation
Pyrolysis
Pyrolysis
+ O2 Oxidation
Courtesy of Prof Tiziano Faravelli Politecnico di Milano
7
R + O2 harr RȮ2 Low TRȮ2 QOOH (~500 850 K)
QOOH + O2 harr Ȯ2QOOH Ȯ2QOOH RȮ + ȮH + ȮH
conversion
Reactor Temperature
Zhandong Wang Proc Natl Acad Sci 114(50) (2017) 13102ndash13107Zhandong Wang et al Combust Flame 187 (2018) 199ndash216
Evidence of further additions to O2 have been reported
Three distinct temperature regimes
8
Negative Temperature Coefficient Regime
Intermediate T (850 1100 K)RȮ2 rarr olefin + HȮ2 (NTC)
QOOH rarr cyclic ether + ȮH (NTC)
Three distinct temperature regimes
conversion
Reactor Temperature
9
Flame images taken by a CH-filtered digital stillcamera (a) Normal flame (U = 40 cms) (b) FREI (U= 20 cms) and (c) weak flames (U = 30 cms) Computed profiles of major species at U = 20 cms
Vertical dotted lines indicate the locations of HRR peaks
Akira Yamamoto Hiroshi Oshibe Hisashi Nakamura Takuya Tezuka Susumu Hasegawa Kaoru Maruta
Proceedings of the Combustion Institute vol 33 pp 3259‐3266 (2011)
Three distinct temperature regimes nC7H16
0
300
600
900
1200
1500
000 020 040 060 080 100
Tem
pera
ture
-K
Time - seconds
n-heptane RON = 0
heat release rateTemperature
Slide courtesy of Dr Charles Westbrook10
Three distinct temperature regimes nC7H16
11ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
Intermediate TḢ + O2 (+M) = HȮ2 (+M)RH + HȮ2 = R+ H2O2
H2O2 (+M) = ȮH + ȮH (+M)R + O2harr RȮ2
RȮ2 rarr olefin + HȮ2
High TFuel = R + Rprime
R = olefin + ĊH3 or ḢḢ + O2 = Ouml + ȮH
ĊH3 + O2 = CH2O + ȮH
22
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
12
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Ḣ + O2 (+M) = HȮ2 (+M)RH + HȮ2 = R+ H2O2
H2O2 (+M) = ȮH + ȮH (+M)R + O2harr RȮ2
RȮ2 rarr olefin + HȮ2
Three distinct temperature regimes
13
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
14ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Importance of concerted HȮ2 elimination reaction
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
15
Intermediate temperature chemistrymdash Concerted eliminations are not well known ndash quantum chemistry
mdash Quelch et al1 first proposed Ċ2H5 + O2 = C2H4 + HȮ2 cyclic TS via concerted elimination
mdash Miyoshi23 variational TST and RRKMmaster equation (Ċ2iĊ3n‐s‐t‐Ċ4 + O2)
mdash Villano et al45 calculated 23 different straight and branched alkyl‐peroxyl radicals
mdash Goldsmith et al6 for the propyl + O2 system
Need for further studies of these reactions due to their high importance
1GE Quelch MM Gallo M Shen Y Xie HF Schaefer III D Moncrieff J Am Chem Soc 116 (1994) 4953ndash49622A Miyoshi J Phys Chem A 115 (2011) 3301ndash33253A Miyoshi A Int J Chem Kinet 44 (2012) 59ndash744SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 115 (2011) 13425ndash134425SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 116 (2012) 5068ndash50896CF Goldsmith WH Green SJ Klippenstein J Phys Chem A 2012 116 3325ndash3346
16
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
17
Few direct measurements of H‐atom abstraction by HȮ2 ndash lack of suitable precursors mdash CH2O + HȮ2 Jemi‐Alade et al1 using flash photolysismdash Walker et al23 made indirect relative rate measurementsmdash Scott and Walker4 review of alkanes aromatics and related compounds in 2002
Recent developments in quantitative measurements of HȮ2 radicals mdash Fluorescence assay by Gas Expansion by Blocquet et al5 (2013)mdash Dual‐modulation Faraday Spectroscopy67 (2014 2015)mdash Cavity ring‐down spectroscopy8 (2014)
These measurements are very useful in assessing mechanism performance1AA Jemi‐Alade PD Lightfoot R Lesclaux Chem Phys Lett 195 (1992) 25ndash302RR Baldwin RW Walker Proc Combust Inst 17 (1979) 525ndash5333RW Walker C Morley in Comprehensive Chem Kinetics (M J Pilling Ed) Elsevier Amsterdam 351 (1997)4M Scott RW Walker Combust Flame 129 (2002) 365ndash3775M Blocquet C Schoemaecker D Amedro O Herbinet F Battin‐Leclerc C Fittschen Proc Natl Acad Sci U S A 110 (2013) 20014ndash200176B Brumfield WT Sun Y Wang Y Ju G Wysocki Opt Lett 39 (2014) 1783ndash17867N Kurimoto B Brumfield X Yang T Wada P Dieacutevart G Wysocki Y Ju Proc Combust Inst 35(1) (2015) 457ndash4648M Djehiche NL Le Tan CD Jain G Dayma P Dagaut C Chauveau L Pillier A Tomas J Am Chem Soc 136 (2014) 16689ndash16694
93
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
18
CH3OH oxidation 855 O2 p = 40 atm and T = 885 K
Sensitivity to ignition delay timeU Burke WK Metcalfe SM Burke KA Heufer P Dagaut HJ Curran Combust Flame 165 (2016) 125ndash13694
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
19
CH3OH + HȮ2 = ĊH2OH + H2O2
05 10 15 20104
105
106
107
108
109
1010
1011
1012
rate
con
stan
t (k)
cm
3 mol
-1 s
-1
1000 K T
Altarawneh (2011) Olm et al (2017) Alecu and Truhlar (2011) Klippenstein (2011)
104
105
106
107
108
109
1010
1011
1012
2000 1500 1000 500T K
20
Klippenstein et al1 reported high sensitivity to CH3OH + HȮ2 also calculated k Altarawneh et al2 and Alecu and Truhlar3
Olm et al4 via computer optimization using direct and indirect measurements Alecu and Truhlar attributed differences with Klippenstein et al calculations to
differences in treatment of anharmonicity
Possible chemically activated reactions involving HȮ2 radicals
1SJ Klippenstein LB Harding MJ Davis AS Tomlin RT Skodje Proc Combust Inst 33 (2011) 351ndash3572M Altarawneh AH Al‐Muhtaseb BZ Dlugogorski EM Kennedy JC Mackie J Comp Chem 32 (2011) 1725ndash17333IM Alecu DG Truhlar J Phys Chem A 115 (2011) 14599ndash146114C Olm T Varga Eacute Valkoacute HJ Curran T Turaacutenyi Combust Flame 186 (2017) 45ndash64
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
21
Carstensen and Dean12 for CH4 C2H6 C3H8 C4H10 + HȮ2
Aguilera‐Iparraguirre et al3 CH4 C2H6 C3H8 nC4H10 iC4H10 + HȮ2
mdashAgree well with the determinations of Walker et al
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash1573J Aguilera‐Iparraguirre HJ Curran W Klopper JM Simmie J Phys Chem A 112 (2008) 7047ndash7054
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
22ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
RH + CH3Ȯ2 = R + CH3O2H can also be important
HJ Curran P Gaffuri WJ Pitz CK WestbrookCombustion and Flame 129253ndash280 (2002)
iC8H18 oxidationφ = 10 in air p = 40 atm
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
23
RH + CH3Ȯ2 = R + CH3O2HĊH3 + O2 = CH3Ȯ2
RH + CH3Ȯ2 = R + CH3O2HCH3O2H = CH3Ȯ + ȮH
Carstensen and Dean1 for CH4C2H6 + ḢCH3Ȯ2C2H5Ȯ2
CarstensenDeanDeutschmann2 for CH4 C2H6 C3H8 C4H10 + HȮ2 CH3Ȯ2 C2H5Ȯ2 C3H7Ȯ2 C3H7Ȯ2 HC(O)Ȯ2 CH3C(O)Ȯ2
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash157
24ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
25
Rate rules for large molecular weight molecules
bull High temperature mechanismReaction class 1 Unimolecular fuel decompositionReaction class 2 H atom abstractions from fuelReaction class 3 Alkyl radical decompositionReaction class 4 Alkyl radical + O2 = olefin + HȮ2
Reaction class 5 Alkyl radical isomerizationReaction class 6 H atom abstraction from olefinsReaction class 7 Addition of radical species to olefinsReaction class 8 Alkenyl radical decompositionReaction class 9 Olefin decomposition
26Slide Courtesy of Dr William Pitz
Reaction rate rules for higher MW species
27Slide Courtesy of Dr William Pitz
Reaction classes for low temperature reactionsLow temperature mechanismReaction class 10 Alkyl radical addition to O2 (R + O2)Reaction class 11 R + RrsquoO2 = RȮ + RrsquoȮReaction class 12 Alkylperoxy radical isomerizationReaction class 13 RȮ2 + HȮ2 = ROOH + O2Reaction class 14 RȮ2 + H2O2 = ROOH + HȮ2Reaction class 15 RȮ2 + CH3Ȯ2 = RȮ + CH3Ȯ +O2Reaction class 16 RȮ2 + RrsquoȮ2 = RȮ + RrsquoȮ + O2Reaction class 17 ROOH = RȮ + ȮHReaction class 18 RȮ DecompositionReaction class 19 QOOH = Cyclic Ether + ȮHReaction class 20 QOOH = Olefin + HȮ2Reaction class 21 QOOH = Olefin + Aldehyde or Carbonyl + ȮHReaction class 22 Addition of QOOH to molecular oxygen O2Reaction class 23 Ȯ2QOOH isomerization to carbonylhydroperoxide + ȮHReaction class 24 Carbonylhydroperoxide decompositionReaction class 25 Reactions of cyclic ethers with ȮH and HȮ2
28
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
7
R + O2 harr RȮ2 Low TRȮ2 QOOH (~500 850 K)
QOOH + O2 harr Ȯ2QOOH Ȯ2QOOH RȮ + ȮH + ȮH
conversion
Reactor Temperature
Zhandong Wang Proc Natl Acad Sci 114(50) (2017) 13102ndash13107Zhandong Wang et al Combust Flame 187 (2018) 199ndash216
Evidence of further additions to O2 have been reported
Three distinct temperature regimes
8
Negative Temperature Coefficient Regime
Intermediate T (850 1100 K)RȮ2 rarr olefin + HȮ2 (NTC)
QOOH rarr cyclic ether + ȮH (NTC)
Three distinct temperature regimes
conversion
Reactor Temperature
9
Flame images taken by a CH-filtered digital stillcamera (a) Normal flame (U = 40 cms) (b) FREI (U= 20 cms) and (c) weak flames (U = 30 cms) Computed profiles of major species at U = 20 cms
Vertical dotted lines indicate the locations of HRR peaks
Akira Yamamoto Hiroshi Oshibe Hisashi Nakamura Takuya Tezuka Susumu Hasegawa Kaoru Maruta
Proceedings of the Combustion Institute vol 33 pp 3259‐3266 (2011)
Three distinct temperature regimes nC7H16
0
300
600
900
1200
1500
000 020 040 060 080 100
Tem
pera
ture
-K
Time - seconds
n-heptane RON = 0
heat release rateTemperature
Slide courtesy of Dr Charles Westbrook10
Three distinct temperature regimes nC7H16
11ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
Intermediate TḢ + O2 (+M) = HȮ2 (+M)RH + HȮ2 = R+ H2O2
H2O2 (+M) = ȮH + ȮH (+M)R + O2harr RȮ2
RȮ2 rarr olefin + HȮ2
High TFuel = R + Rprime
R = olefin + ĊH3 or ḢḢ + O2 = Ouml + ȮH
ĊH3 + O2 = CH2O + ȮH
22
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
12
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Ḣ + O2 (+M) = HȮ2 (+M)RH + HȮ2 = R+ H2O2
H2O2 (+M) = ȮH + ȮH (+M)R + O2harr RȮ2
RȮ2 rarr olefin + HȮ2
Three distinct temperature regimes
13
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
14ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Importance of concerted HȮ2 elimination reaction
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
15
Intermediate temperature chemistrymdash Concerted eliminations are not well known ndash quantum chemistry
mdash Quelch et al1 first proposed Ċ2H5 + O2 = C2H4 + HȮ2 cyclic TS via concerted elimination
mdash Miyoshi23 variational TST and RRKMmaster equation (Ċ2iĊ3n‐s‐t‐Ċ4 + O2)
mdash Villano et al45 calculated 23 different straight and branched alkyl‐peroxyl radicals
mdash Goldsmith et al6 for the propyl + O2 system
Need for further studies of these reactions due to their high importance
1GE Quelch MM Gallo M Shen Y Xie HF Schaefer III D Moncrieff J Am Chem Soc 116 (1994) 4953ndash49622A Miyoshi J Phys Chem A 115 (2011) 3301ndash33253A Miyoshi A Int J Chem Kinet 44 (2012) 59ndash744SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 115 (2011) 13425ndash134425SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 116 (2012) 5068ndash50896CF Goldsmith WH Green SJ Klippenstein J Phys Chem A 2012 116 3325ndash3346
16
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
17
Few direct measurements of H‐atom abstraction by HȮ2 ndash lack of suitable precursors mdash CH2O + HȮ2 Jemi‐Alade et al1 using flash photolysismdash Walker et al23 made indirect relative rate measurementsmdash Scott and Walker4 review of alkanes aromatics and related compounds in 2002
Recent developments in quantitative measurements of HȮ2 radicals mdash Fluorescence assay by Gas Expansion by Blocquet et al5 (2013)mdash Dual‐modulation Faraday Spectroscopy67 (2014 2015)mdash Cavity ring‐down spectroscopy8 (2014)
These measurements are very useful in assessing mechanism performance1AA Jemi‐Alade PD Lightfoot R Lesclaux Chem Phys Lett 195 (1992) 25ndash302RR Baldwin RW Walker Proc Combust Inst 17 (1979) 525ndash5333RW Walker C Morley in Comprehensive Chem Kinetics (M J Pilling Ed) Elsevier Amsterdam 351 (1997)4M Scott RW Walker Combust Flame 129 (2002) 365ndash3775M Blocquet C Schoemaecker D Amedro O Herbinet F Battin‐Leclerc C Fittschen Proc Natl Acad Sci U S A 110 (2013) 20014ndash200176B Brumfield WT Sun Y Wang Y Ju G Wysocki Opt Lett 39 (2014) 1783ndash17867N Kurimoto B Brumfield X Yang T Wada P Dieacutevart G Wysocki Y Ju Proc Combust Inst 35(1) (2015) 457ndash4648M Djehiche NL Le Tan CD Jain G Dayma P Dagaut C Chauveau L Pillier A Tomas J Am Chem Soc 136 (2014) 16689ndash16694
93
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
18
CH3OH oxidation 855 O2 p = 40 atm and T = 885 K
Sensitivity to ignition delay timeU Burke WK Metcalfe SM Burke KA Heufer P Dagaut HJ Curran Combust Flame 165 (2016) 125ndash13694
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
19
CH3OH + HȮ2 = ĊH2OH + H2O2
05 10 15 20104
105
106
107
108
109
1010
1011
1012
rate
con
stan
t (k)
cm
3 mol
-1 s
-1
1000 K T
Altarawneh (2011) Olm et al (2017) Alecu and Truhlar (2011) Klippenstein (2011)
104
105
106
107
108
109
1010
1011
1012
2000 1500 1000 500T K
20
Klippenstein et al1 reported high sensitivity to CH3OH + HȮ2 also calculated k Altarawneh et al2 and Alecu and Truhlar3
Olm et al4 via computer optimization using direct and indirect measurements Alecu and Truhlar attributed differences with Klippenstein et al calculations to
differences in treatment of anharmonicity
Possible chemically activated reactions involving HȮ2 radicals
1SJ Klippenstein LB Harding MJ Davis AS Tomlin RT Skodje Proc Combust Inst 33 (2011) 351ndash3572M Altarawneh AH Al‐Muhtaseb BZ Dlugogorski EM Kennedy JC Mackie J Comp Chem 32 (2011) 1725ndash17333IM Alecu DG Truhlar J Phys Chem A 115 (2011) 14599ndash146114C Olm T Varga Eacute Valkoacute HJ Curran T Turaacutenyi Combust Flame 186 (2017) 45ndash64
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
21
Carstensen and Dean12 for CH4 C2H6 C3H8 C4H10 + HȮ2
Aguilera‐Iparraguirre et al3 CH4 C2H6 C3H8 nC4H10 iC4H10 + HȮ2
mdashAgree well with the determinations of Walker et al
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash1573J Aguilera‐Iparraguirre HJ Curran W Klopper JM Simmie J Phys Chem A 112 (2008) 7047ndash7054
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
22ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
RH + CH3Ȯ2 = R + CH3O2H can also be important
HJ Curran P Gaffuri WJ Pitz CK WestbrookCombustion and Flame 129253ndash280 (2002)
iC8H18 oxidationφ = 10 in air p = 40 atm
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
23
RH + CH3Ȯ2 = R + CH3O2HĊH3 + O2 = CH3Ȯ2
RH + CH3Ȯ2 = R + CH3O2HCH3O2H = CH3Ȯ + ȮH
Carstensen and Dean1 for CH4C2H6 + ḢCH3Ȯ2C2H5Ȯ2
CarstensenDeanDeutschmann2 for CH4 C2H6 C3H8 C4H10 + HȮ2 CH3Ȯ2 C2H5Ȯ2 C3H7Ȯ2 C3H7Ȯ2 HC(O)Ȯ2 CH3C(O)Ȯ2
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash157
24ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
25
Rate rules for large molecular weight molecules
bull High temperature mechanismReaction class 1 Unimolecular fuel decompositionReaction class 2 H atom abstractions from fuelReaction class 3 Alkyl radical decompositionReaction class 4 Alkyl radical + O2 = olefin + HȮ2
Reaction class 5 Alkyl radical isomerizationReaction class 6 H atom abstraction from olefinsReaction class 7 Addition of radical species to olefinsReaction class 8 Alkenyl radical decompositionReaction class 9 Olefin decomposition
26Slide Courtesy of Dr William Pitz
Reaction rate rules for higher MW species
27Slide Courtesy of Dr William Pitz
Reaction classes for low temperature reactionsLow temperature mechanismReaction class 10 Alkyl radical addition to O2 (R + O2)Reaction class 11 R + RrsquoO2 = RȮ + RrsquoȮReaction class 12 Alkylperoxy radical isomerizationReaction class 13 RȮ2 + HȮ2 = ROOH + O2Reaction class 14 RȮ2 + H2O2 = ROOH + HȮ2Reaction class 15 RȮ2 + CH3Ȯ2 = RȮ + CH3Ȯ +O2Reaction class 16 RȮ2 + RrsquoȮ2 = RȮ + RrsquoȮ + O2Reaction class 17 ROOH = RȮ + ȮHReaction class 18 RȮ DecompositionReaction class 19 QOOH = Cyclic Ether + ȮHReaction class 20 QOOH = Olefin + HȮ2Reaction class 21 QOOH = Olefin + Aldehyde or Carbonyl + ȮHReaction class 22 Addition of QOOH to molecular oxygen O2Reaction class 23 Ȯ2QOOH isomerization to carbonylhydroperoxide + ȮHReaction class 24 Carbonylhydroperoxide decompositionReaction class 25 Reactions of cyclic ethers with ȮH and HȮ2
28
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
8
Negative Temperature Coefficient Regime
Intermediate T (850 1100 K)RȮ2 rarr olefin + HȮ2 (NTC)
QOOH rarr cyclic ether + ȮH (NTC)
Three distinct temperature regimes
conversion
Reactor Temperature
9
Flame images taken by a CH-filtered digital stillcamera (a) Normal flame (U = 40 cms) (b) FREI (U= 20 cms) and (c) weak flames (U = 30 cms) Computed profiles of major species at U = 20 cms
Vertical dotted lines indicate the locations of HRR peaks
Akira Yamamoto Hiroshi Oshibe Hisashi Nakamura Takuya Tezuka Susumu Hasegawa Kaoru Maruta
Proceedings of the Combustion Institute vol 33 pp 3259‐3266 (2011)
Three distinct temperature regimes nC7H16
0
300
600
900
1200
1500
000 020 040 060 080 100
Tem
pera
ture
-K
Time - seconds
n-heptane RON = 0
heat release rateTemperature
Slide courtesy of Dr Charles Westbrook10
Three distinct temperature regimes nC7H16
11ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
Intermediate TḢ + O2 (+M) = HȮ2 (+M)RH + HȮ2 = R+ H2O2
H2O2 (+M) = ȮH + ȮH (+M)R + O2harr RȮ2
RȮ2 rarr olefin + HȮ2
High TFuel = R + Rprime
R = olefin + ĊH3 or ḢḢ + O2 = Ouml + ȮH
ĊH3 + O2 = CH2O + ȮH
22
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
12
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Ḣ + O2 (+M) = HȮ2 (+M)RH + HȮ2 = R+ H2O2
H2O2 (+M) = ȮH + ȮH (+M)R + O2harr RȮ2
RȮ2 rarr olefin + HȮ2
Three distinct temperature regimes
13
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
14ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Importance of concerted HȮ2 elimination reaction
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
15
Intermediate temperature chemistrymdash Concerted eliminations are not well known ndash quantum chemistry
mdash Quelch et al1 first proposed Ċ2H5 + O2 = C2H4 + HȮ2 cyclic TS via concerted elimination
mdash Miyoshi23 variational TST and RRKMmaster equation (Ċ2iĊ3n‐s‐t‐Ċ4 + O2)
mdash Villano et al45 calculated 23 different straight and branched alkyl‐peroxyl radicals
mdash Goldsmith et al6 for the propyl + O2 system
Need for further studies of these reactions due to their high importance
1GE Quelch MM Gallo M Shen Y Xie HF Schaefer III D Moncrieff J Am Chem Soc 116 (1994) 4953ndash49622A Miyoshi J Phys Chem A 115 (2011) 3301ndash33253A Miyoshi A Int J Chem Kinet 44 (2012) 59ndash744SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 115 (2011) 13425ndash134425SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 116 (2012) 5068ndash50896CF Goldsmith WH Green SJ Klippenstein J Phys Chem A 2012 116 3325ndash3346
16
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
17
Few direct measurements of H‐atom abstraction by HȮ2 ndash lack of suitable precursors mdash CH2O + HȮ2 Jemi‐Alade et al1 using flash photolysismdash Walker et al23 made indirect relative rate measurementsmdash Scott and Walker4 review of alkanes aromatics and related compounds in 2002
Recent developments in quantitative measurements of HȮ2 radicals mdash Fluorescence assay by Gas Expansion by Blocquet et al5 (2013)mdash Dual‐modulation Faraday Spectroscopy67 (2014 2015)mdash Cavity ring‐down spectroscopy8 (2014)
These measurements are very useful in assessing mechanism performance1AA Jemi‐Alade PD Lightfoot R Lesclaux Chem Phys Lett 195 (1992) 25ndash302RR Baldwin RW Walker Proc Combust Inst 17 (1979) 525ndash5333RW Walker C Morley in Comprehensive Chem Kinetics (M J Pilling Ed) Elsevier Amsterdam 351 (1997)4M Scott RW Walker Combust Flame 129 (2002) 365ndash3775M Blocquet C Schoemaecker D Amedro O Herbinet F Battin‐Leclerc C Fittschen Proc Natl Acad Sci U S A 110 (2013) 20014ndash200176B Brumfield WT Sun Y Wang Y Ju G Wysocki Opt Lett 39 (2014) 1783ndash17867N Kurimoto B Brumfield X Yang T Wada P Dieacutevart G Wysocki Y Ju Proc Combust Inst 35(1) (2015) 457ndash4648M Djehiche NL Le Tan CD Jain G Dayma P Dagaut C Chauveau L Pillier A Tomas J Am Chem Soc 136 (2014) 16689ndash16694
93
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
18
CH3OH oxidation 855 O2 p = 40 atm and T = 885 K
Sensitivity to ignition delay timeU Burke WK Metcalfe SM Burke KA Heufer P Dagaut HJ Curran Combust Flame 165 (2016) 125ndash13694
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
19
CH3OH + HȮ2 = ĊH2OH + H2O2
05 10 15 20104
105
106
107
108
109
1010
1011
1012
rate
con
stan
t (k)
cm
3 mol
-1 s
-1
1000 K T
Altarawneh (2011) Olm et al (2017) Alecu and Truhlar (2011) Klippenstein (2011)
104
105
106
107
108
109
1010
1011
1012
2000 1500 1000 500T K
20
Klippenstein et al1 reported high sensitivity to CH3OH + HȮ2 also calculated k Altarawneh et al2 and Alecu and Truhlar3
Olm et al4 via computer optimization using direct and indirect measurements Alecu and Truhlar attributed differences with Klippenstein et al calculations to
differences in treatment of anharmonicity
Possible chemically activated reactions involving HȮ2 radicals
1SJ Klippenstein LB Harding MJ Davis AS Tomlin RT Skodje Proc Combust Inst 33 (2011) 351ndash3572M Altarawneh AH Al‐Muhtaseb BZ Dlugogorski EM Kennedy JC Mackie J Comp Chem 32 (2011) 1725ndash17333IM Alecu DG Truhlar J Phys Chem A 115 (2011) 14599ndash146114C Olm T Varga Eacute Valkoacute HJ Curran T Turaacutenyi Combust Flame 186 (2017) 45ndash64
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
21
Carstensen and Dean12 for CH4 C2H6 C3H8 C4H10 + HȮ2
Aguilera‐Iparraguirre et al3 CH4 C2H6 C3H8 nC4H10 iC4H10 + HȮ2
mdashAgree well with the determinations of Walker et al
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash1573J Aguilera‐Iparraguirre HJ Curran W Klopper JM Simmie J Phys Chem A 112 (2008) 7047ndash7054
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
22ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
RH + CH3Ȯ2 = R + CH3O2H can also be important
HJ Curran P Gaffuri WJ Pitz CK WestbrookCombustion and Flame 129253ndash280 (2002)
iC8H18 oxidationφ = 10 in air p = 40 atm
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
23
RH + CH3Ȯ2 = R + CH3O2HĊH3 + O2 = CH3Ȯ2
RH + CH3Ȯ2 = R + CH3O2HCH3O2H = CH3Ȯ + ȮH
Carstensen and Dean1 for CH4C2H6 + ḢCH3Ȯ2C2H5Ȯ2
CarstensenDeanDeutschmann2 for CH4 C2H6 C3H8 C4H10 + HȮ2 CH3Ȯ2 C2H5Ȯ2 C3H7Ȯ2 C3H7Ȯ2 HC(O)Ȯ2 CH3C(O)Ȯ2
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash157
24ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
25
Rate rules for large molecular weight molecules
bull High temperature mechanismReaction class 1 Unimolecular fuel decompositionReaction class 2 H atom abstractions from fuelReaction class 3 Alkyl radical decompositionReaction class 4 Alkyl radical + O2 = olefin + HȮ2
Reaction class 5 Alkyl radical isomerizationReaction class 6 H atom abstraction from olefinsReaction class 7 Addition of radical species to olefinsReaction class 8 Alkenyl radical decompositionReaction class 9 Olefin decomposition
26Slide Courtesy of Dr William Pitz
Reaction rate rules for higher MW species
27Slide Courtesy of Dr William Pitz
Reaction classes for low temperature reactionsLow temperature mechanismReaction class 10 Alkyl radical addition to O2 (R + O2)Reaction class 11 R + RrsquoO2 = RȮ + RrsquoȮReaction class 12 Alkylperoxy radical isomerizationReaction class 13 RȮ2 + HȮ2 = ROOH + O2Reaction class 14 RȮ2 + H2O2 = ROOH + HȮ2Reaction class 15 RȮ2 + CH3Ȯ2 = RȮ + CH3Ȯ +O2Reaction class 16 RȮ2 + RrsquoȮ2 = RȮ + RrsquoȮ + O2Reaction class 17 ROOH = RȮ + ȮHReaction class 18 RȮ DecompositionReaction class 19 QOOH = Cyclic Ether + ȮHReaction class 20 QOOH = Olefin + HȮ2Reaction class 21 QOOH = Olefin + Aldehyde or Carbonyl + ȮHReaction class 22 Addition of QOOH to molecular oxygen O2Reaction class 23 Ȯ2QOOH isomerization to carbonylhydroperoxide + ȮHReaction class 24 Carbonylhydroperoxide decompositionReaction class 25 Reactions of cyclic ethers with ȮH and HȮ2
28
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
9
Flame images taken by a CH-filtered digital stillcamera (a) Normal flame (U = 40 cms) (b) FREI (U= 20 cms) and (c) weak flames (U = 30 cms) Computed profiles of major species at U = 20 cms
Vertical dotted lines indicate the locations of HRR peaks
Akira Yamamoto Hiroshi Oshibe Hisashi Nakamura Takuya Tezuka Susumu Hasegawa Kaoru Maruta
Proceedings of the Combustion Institute vol 33 pp 3259‐3266 (2011)
Three distinct temperature regimes nC7H16
0
300
600
900
1200
1500
000 020 040 060 080 100
Tem
pera
ture
-K
Time - seconds
n-heptane RON = 0
heat release rateTemperature
Slide courtesy of Dr Charles Westbrook10
Three distinct temperature regimes nC7H16
11ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
Intermediate TḢ + O2 (+M) = HȮ2 (+M)RH + HȮ2 = R+ H2O2
H2O2 (+M) = ȮH + ȮH (+M)R + O2harr RȮ2
RȮ2 rarr olefin + HȮ2
High TFuel = R + Rprime
R = olefin + ĊH3 or ḢḢ + O2 = Ouml + ȮH
ĊH3 + O2 = CH2O + ȮH
22
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
12
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Ḣ + O2 (+M) = HȮ2 (+M)RH + HȮ2 = R+ H2O2
H2O2 (+M) = ȮH + ȮH (+M)R + O2harr RȮ2
RȮ2 rarr olefin + HȮ2
Three distinct temperature regimes
13
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
14ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Importance of concerted HȮ2 elimination reaction
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
15
Intermediate temperature chemistrymdash Concerted eliminations are not well known ndash quantum chemistry
mdash Quelch et al1 first proposed Ċ2H5 + O2 = C2H4 + HȮ2 cyclic TS via concerted elimination
mdash Miyoshi23 variational TST and RRKMmaster equation (Ċ2iĊ3n‐s‐t‐Ċ4 + O2)
mdash Villano et al45 calculated 23 different straight and branched alkyl‐peroxyl radicals
mdash Goldsmith et al6 for the propyl + O2 system
Need for further studies of these reactions due to their high importance
1GE Quelch MM Gallo M Shen Y Xie HF Schaefer III D Moncrieff J Am Chem Soc 116 (1994) 4953ndash49622A Miyoshi J Phys Chem A 115 (2011) 3301ndash33253A Miyoshi A Int J Chem Kinet 44 (2012) 59ndash744SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 115 (2011) 13425ndash134425SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 116 (2012) 5068ndash50896CF Goldsmith WH Green SJ Klippenstein J Phys Chem A 2012 116 3325ndash3346
16
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
17
Few direct measurements of H‐atom abstraction by HȮ2 ndash lack of suitable precursors mdash CH2O + HȮ2 Jemi‐Alade et al1 using flash photolysismdash Walker et al23 made indirect relative rate measurementsmdash Scott and Walker4 review of alkanes aromatics and related compounds in 2002
Recent developments in quantitative measurements of HȮ2 radicals mdash Fluorescence assay by Gas Expansion by Blocquet et al5 (2013)mdash Dual‐modulation Faraday Spectroscopy67 (2014 2015)mdash Cavity ring‐down spectroscopy8 (2014)
These measurements are very useful in assessing mechanism performance1AA Jemi‐Alade PD Lightfoot R Lesclaux Chem Phys Lett 195 (1992) 25ndash302RR Baldwin RW Walker Proc Combust Inst 17 (1979) 525ndash5333RW Walker C Morley in Comprehensive Chem Kinetics (M J Pilling Ed) Elsevier Amsterdam 351 (1997)4M Scott RW Walker Combust Flame 129 (2002) 365ndash3775M Blocquet C Schoemaecker D Amedro O Herbinet F Battin‐Leclerc C Fittschen Proc Natl Acad Sci U S A 110 (2013) 20014ndash200176B Brumfield WT Sun Y Wang Y Ju G Wysocki Opt Lett 39 (2014) 1783ndash17867N Kurimoto B Brumfield X Yang T Wada P Dieacutevart G Wysocki Y Ju Proc Combust Inst 35(1) (2015) 457ndash4648M Djehiche NL Le Tan CD Jain G Dayma P Dagaut C Chauveau L Pillier A Tomas J Am Chem Soc 136 (2014) 16689ndash16694
93
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
18
CH3OH oxidation 855 O2 p = 40 atm and T = 885 K
Sensitivity to ignition delay timeU Burke WK Metcalfe SM Burke KA Heufer P Dagaut HJ Curran Combust Flame 165 (2016) 125ndash13694
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
19
CH3OH + HȮ2 = ĊH2OH + H2O2
05 10 15 20104
105
106
107
108
109
1010
1011
1012
rate
con
stan
t (k)
cm
3 mol
-1 s
-1
1000 K T
Altarawneh (2011) Olm et al (2017) Alecu and Truhlar (2011) Klippenstein (2011)
104
105
106
107
108
109
1010
1011
1012
2000 1500 1000 500T K
20
Klippenstein et al1 reported high sensitivity to CH3OH + HȮ2 also calculated k Altarawneh et al2 and Alecu and Truhlar3
Olm et al4 via computer optimization using direct and indirect measurements Alecu and Truhlar attributed differences with Klippenstein et al calculations to
differences in treatment of anharmonicity
Possible chemically activated reactions involving HȮ2 radicals
1SJ Klippenstein LB Harding MJ Davis AS Tomlin RT Skodje Proc Combust Inst 33 (2011) 351ndash3572M Altarawneh AH Al‐Muhtaseb BZ Dlugogorski EM Kennedy JC Mackie J Comp Chem 32 (2011) 1725ndash17333IM Alecu DG Truhlar J Phys Chem A 115 (2011) 14599ndash146114C Olm T Varga Eacute Valkoacute HJ Curran T Turaacutenyi Combust Flame 186 (2017) 45ndash64
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
21
Carstensen and Dean12 for CH4 C2H6 C3H8 C4H10 + HȮ2
Aguilera‐Iparraguirre et al3 CH4 C2H6 C3H8 nC4H10 iC4H10 + HȮ2
mdashAgree well with the determinations of Walker et al
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash1573J Aguilera‐Iparraguirre HJ Curran W Klopper JM Simmie J Phys Chem A 112 (2008) 7047ndash7054
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
22ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
RH + CH3Ȯ2 = R + CH3O2H can also be important
HJ Curran P Gaffuri WJ Pitz CK WestbrookCombustion and Flame 129253ndash280 (2002)
iC8H18 oxidationφ = 10 in air p = 40 atm
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
23
RH + CH3Ȯ2 = R + CH3O2HĊH3 + O2 = CH3Ȯ2
RH + CH3Ȯ2 = R + CH3O2HCH3O2H = CH3Ȯ + ȮH
Carstensen and Dean1 for CH4C2H6 + ḢCH3Ȯ2C2H5Ȯ2
CarstensenDeanDeutschmann2 for CH4 C2H6 C3H8 C4H10 + HȮ2 CH3Ȯ2 C2H5Ȯ2 C3H7Ȯ2 C3H7Ȯ2 HC(O)Ȯ2 CH3C(O)Ȯ2
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash157
24ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
25
Rate rules for large molecular weight molecules
bull High temperature mechanismReaction class 1 Unimolecular fuel decompositionReaction class 2 H atom abstractions from fuelReaction class 3 Alkyl radical decompositionReaction class 4 Alkyl radical + O2 = olefin + HȮ2
Reaction class 5 Alkyl radical isomerizationReaction class 6 H atom abstraction from olefinsReaction class 7 Addition of radical species to olefinsReaction class 8 Alkenyl radical decompositionReaction class 9 Olefin decomposition
26Slide Courtesy of Dr William Pitz
Reaction rate rules for higher MW species
27Slide Courtesy of Dr William Pitz
Reaction classes for low temperature reactionsLow temperature mechanismReaction class 10 Alkyl radical addition to O2 (R + O2)Reaction class 11 R + RrsquoO2 = RȮ + RrsquoȮReaction class 12 Alkylperoxy radical isomerizationReaction class 13 RȮ2 + HȮ2 = ROOH + O2Reaction class 14 RȮ2 + H2O2 = ROOH + HȮ2Reaction class 15 RȮ2 + CH3Ȯ2 = RȮ + CH3Ȯ +O2Reaction class 16 RȮ2 + RrsquoȮ2 = RȮ + RrsquoȮ + O2Reaction class 17 ROOH = RȮ + ȮHReaction class 18 RȮ DecompositionReaction class 19 QOOH = Cyclic Ether + ȮHReaction class 20 QOOH = Olefin + HȮ2Reaction class 21 QOOH = Olefin + Aldehyde or Carbonyl + ȮHReaction class 22 Addition of QOOH to molecular oxygen O2Reaction class 23 Ȯ2QOOH isomerization to carbonylhydroperoxide + ȮHReaction class 24 Carbonylhydroperoxide decompositionReaction class 25 Reactions of cyclic ethers with ȮH and HȮ2
28
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
0
300
600
900
1200
1500
000 020 040 060 080 100
Tem
pera
ture
-K
Time - seconds
n-heptane RON = 0
heat release rateTemperature
Slide courtesy of Dr Charles Westbrook10
Three distinct temperature regimes nC7H16
11ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
Intermediate TḢ + O2 (+M) = HȮ2 (+M)RH + HȮ2 = R+ H2O2
H2O2 (+M) = ȮH + ȮH (+M)R + O2harr RȮ2
RȮ2 rarr olefin + HȮ2
High TFuel = R + Rprime
R = olefin + ĊH3 or ḢḢ + O2 = Ouml + ȮH
ĊH3 + O2 = CH2O + ȮH
22
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
12
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Ḣ + O2 (+M) = HȮ2 (+M)RH + HȮ2 = R+ H2O2
H2O2 (+M) = ȮH + ȮH (+M)R + O2harr RȮ2
RȮ2 rarr olefin + HȮ2
Three distinct temperature regimes
13
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
14ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Importance of concerted HȮ2 elimination reaction
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
15
Intermediate temperature chemistrymdash Concerted eliminations are not well known ndash quantum chemistry
mdash Quelch et al1 first proposed Ċ2H5 + O2 = C2H4 + HȮ2 cyclic TS via concerted elimination
mdash Miyoshi23 variational TST and RRKMmaster equation (Ċ2iĊ3n‐s‐t‐Ċ4 + O2)
mdash Villano et al45 calculated 23 different straight and branched alkyl‐peroxyl radicals
mdash Goldsmith et al6 for the propyl + O2 system
Need for further studies of these reactions due to their high importance
1GE Quelch MM Gallo M Shen Y Xie HF Schaefer III D Moncrieff J Am Chem Soc 116 (1994) 4953ndash49622A Miyoshi J Phys Chem A 115 (2011) 3301ndash33253A Miyoshi A Int J Chem Kinet 44 (2012) 59ndash744SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 115 (2011) 13425ndash134425SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 116 (2012) 5068ndash50896CF Goldsmith WH Green SJ Klippenstein J Phys Chem A 2012 116 3325ndash3346
16
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
17
Few direct measurements of H‐atom abstraction by HȮ2 ndash lack of suitable precursors mdash CH2O + HȮ2 Jemi‐Alade et al1 using flash photolysismdash Walker et al23 made indirect relative rate measurementsmdash Scott and Walker4 review of alkanes aromatics and related compounds in 2002
Recent developments in quantitative measurements of HȮ2 radicals mdash Fluorescence assay by Gas Expansion by Blocquet et al5 (2013)mdash Dual‐modulation Faraday Spectroscopy67 (2014 2015)mdash Cavity ring‐down spectroscopy8 (2014)
These measurements are very useful in assessing mechanism performance1AA Jemi‐Alade PD Lightfoot R Lesclaux Chem Phys Lett 195 (1992) 25ndash302RR Baldwin RW Walker Proc Combust Inst 17 (1979) 525ndash5333RW Walker C Morley in Comprehensive Chem Kinetics (M J Pilling Ed) Elsevier Amsterdam 351 (1997)4M Scott RW Walker Combust Flame 129 (2002) 365ndash3775M Blocquet C Schoemaecker D Amedro O Herbinet F Battin‐Leclerc C Fittschen Proc Natl Acad Sci U S A 110 (2013) 20014ndash200176B Brumfield WT Sun Y Wang Y Ju G Wysocki Opt Lett 39 (2014) 1783ndash17867N Kurimoto B Brumfield X Yang T Wada P Dieacutevart G Wysocki Y Ju Proc Combust Inst 35(1) (2015) 457ndash4648M Djehiche NL Le Tan CD Jain G Dayma P Dagaut C Chauveau L Pillier A Tomas J Am Chem Soc 136 (2014) 16689ndash16694
93
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
18
CH3OH oxidation 855 O2 p = 40 atm and T = 885 K
Sensitivity to ignition delay timeU Burke WK Metcalfe SM Burke KA Heufer P Dagaut HJ Curran Combust Flame 165 (2016) 125ndash13694
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
19
CH3OH + HȮ2 = ĊH2OH + H2O2
05 10 15 20104
105
106
107
108
109
1010
1011
1012
rate
con
stan
t (k)
cm
3 mol
-1 s
-1
1000 K T
Altarawneh (2011) Olm et al (2017) Alecu and Truhlar (2011) Klippenstein (2011)
104
105
106
107
108
109
1010
1011
1012
2000 1500 1000 500T K
20
Klippenstein et al1 reported high sensitivity to CH3OH + HȮ2 also calculated k Altarawneh et al2 and Alecu and Truhlar3
Olm et al4 via computer optimization using direct and indirect measurements Alecu and Truhlar attributed differences with Klippenstein et al calculations to
differences in treatment of anharmonicity
Possible chemically activated reactions involving HȮ2 radicals
1SJ Klippenstein LB Harding MJ Davis AS Tomlin RT Skodje Proc Combust Inst 33 (2011) 351ndash3572M Altarawneh AH Al‐Muhtaseb BZ Dlugogorski EM Kennedy JC Mackie J Comp Chem 32 (2011) 1725ndash17333IM Alecu DG Truhlar J Phys Chem A 115 (2011) 14599ndash146114C Olm T Varga Eacute Valkoacute HJ Curran T Turaacutenyi Combust Flame 186 (2017) 45ndash64
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
21
Carstensen and Dean12 for CH4 C2H6 C3H8 C4H10 + HȮ2
Aguilera‐Iparraguirre et al3 CH4 C2H6 C3H8 nC4H10 iC4H10 + HȮ2
mdashAgree well with the determinations of Walker et al
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash1573J Aguilera‐Iparraguirre HJ Curran W Klopper JM Simmie J Phys Chem A 112 (2008) 7047ndash7054
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
22ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
RH + CH3Ȯ2 = R + CH3O2H can also be important
HJ Curran P Gaffuri WJ Pitz CK WestbrookCombustion and Flame 129253ndash280 (2002)
iC8H18 oxidationφ = 10 in air p = 40 atm
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
23
RH + CH3Ȯ2 = R + CH3O2HĊH3 + O2 = CH3Ȯ2
RH + CH3Ȯ2 = R + CH3O2HCH3O2H = CH3Ȯ + ȮH
Carstensen and Dean1 for CH4C2H6 + ḢCH3Ȯ2C2H5Ȯ2
CarstensenDeanDeutschmann2 for CH4 C2H6 C3H8 C4H10 + HȮ2 CH3Ȯ2 C2H5Ȯ2 C3H7Ȯ2 C3H7Ȯ2 HC(O)Ȯ2 CH3C(O)Ȯ2
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash157
24ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
25
Rate rules for large molecular weight molecules
bull High temperature mechanismReaction class 1 Unimolecular fuel decompositionReaction class 2 H atom abstractions from fuelReaction class 3 Alkyl radical decompositionReaction class 4 Alkyl radical + O2 = olefin + HȮ2
Reaction class 5 Alkyl radical isomerizationReaction class 6 H atom abstraction from olefinsReaction class 7 Addition of radical species to olefinsReaction class 8 Alkenyl radical decompositionReaction class 9 Olefin decomposition
26Slide Courtesy of Dr William Pitz
Reaction rate rules for higher MW species
27Slide Courtesy of Dr William Pitz
Reaction classes for low temperature reactionsLow temperature mechanismReaction class 10 Alkyl radical addition to O2 (R + O2)Reaction class 11 R + RrsquoO2 = RȮ + RrsquoȮReaction class 12 Alkylperoxy radical isomerizationReaction class 13 RȮ2 + HȮ2 = ROOH + O2Reaction class 14 RȮ2 + H2O2 = ROOH + HȮ2Reaction class 15 RȮ2 + CH3Ȯ2 = RȮ + CH3Ȯ +O2Reaction class 16 RȮ2 + RrsquoȮ2 = RȮ + RrsquoȮ + O2Reaction class 17 ROOH = RȮ + ȮHReaction class 18 RȮ DecompositionReaction class 19 QOOH = Cyclic Ether + ȮHReaction class 20 QOOH = Olefin + HȮ2Reaction class 21 QOOH = Olefin + Aldehyde or Carbonyl + ȮHReaction class 22 Addition of QOOH to molecular oxygen O2Reaction class 23 Ȯ2QOOH isomerization to carbonylhydroperoxide + ȮHReaction class 24 Carbonylhydroperoxide decompositionReaction class 25 Reactions of cyclic ethers with ȮH and HȮ2
28
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
11ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
Intermediate TḢ + O2 (+M) = HȮ2 (+M)RH + HȮ2 = R+ H2O2
H2O2 (+M) = ȮH + ȮH (+M)R + O2harr RȮ2
RȮ2 rarr olefin + HȮ2
High TFuel = R + Rprime
R = olefin + ĊH3 or ḢḢ + O2 = Ouml + ȮH
ĊH3 + O2 = CH2O + ȮH
22
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
12
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Ḣ + O2 (+M) = HȮ2 (+M)RH + HȮ2 = R+ H2O2
H2O2 (+M) = ȮH + ȮH (+M)R + O2harr RȮ2
RȮ2 rarr olefin + HȮ2
Three distinct temperature regimes
13
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
14ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Importance of concerted HȮ2 elimination reaction
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
15
Intermediate temperature chemistrymdash Concerted eliminations are not well known ndash quantum chemistry
mdash Quelch et al1 first proposed Ċ2H5 + O2 = C2H4 + HȮ2 cyclic TS via concerted elimination
mdash Miyoshi23 variational TST and RRKMmaster equation (Ċ2iĊ3n‐s‐t‐Ċ4 + O2)
mdash Villano et al45 calculated 23 different straight and branched alkyl‐peroxyl radicals
mdash Goldsmith et al6 for the propyl + O2 system
Need for further studies of these reactions due to their high importance
1GE Quelch MM Gallo M Shen Y Xie HF Schaefer III D Moncrieff J Am Chem Soc 116 (1994) 4953ndash49622A Miyoshi J Phys Chem A 115 (2011) 3301ndash33253A Miyoshi A Int J Chem Kinet 44 (2012) 59ndash744SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 115 (2011) 13425ndash134425SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 116 (2012) 5068ndash50896CF Goldsmith WH Green SJ Klippenstein J Phys Chem A 2012 116 3325ndash3346
16
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
17
Few direct measurements of H‐atom abstraction by HȮ2 ndash lack of suitable precursors mdash CH2O + HȮ2 Jemi‐Alade et al1 using flash photolysismdash Walker et al23 made indirect relative rate measurementsmdash Scott and Walker4 review of alkanes aromatics and related compounds in 2002
Recent developments in quantitative measurements of HȮ2 radicals mdash Fluorescence assay by Gas Expansion by Blocquet et al5 (2013)mdash Dual‐modulation Faraday Spectroscopy67 (2014 2015)mdash Cavity ring‐down spectroscopy8 (2014)
These measurements are very useful in assessing mechanism performance1AA Jemi‐Alade PD Lightfoot R Lesclaux Chem Phys Lett 195 (1992) 25ndash302RR Baldwin RW Walker Proc Combust Inst 17 (1979) 525ndash5333RW Walker C Morley in Comprehensive Chem Kinetics (M J Pilling Ed) Elsevier Amsterdam 351 (1997)4M Scott RW Walker Combust Flame 129 (2002) 365ndash3775M Blocquet C Schoemaecker D Amedro O Herbinet F Battin‐Leclerc C Fittschen Proc Natl Acad Sci U S A 110 (2013) 20014ndash200176B Brumfield WT Sun Y Wang Y Ju G Wysocki Opt Lett 39 (2014) 1783ndash17867N Kurimoto B Brumfield X Yang T Wada P Dieacutevart G Wysocki Y Ju Proc Combust Inst 35(1) (2015) 457ndash4648M Djehiche NL Le Tan CD Jain G Dayma P Dagaut C Chauveau L Pillier A Tomas J Am Chem Soc 136 (2014) 16689ndash16694
93
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
18
CH3OH oxidation 855 O2 p = 40 atm and T = 885 K
Sensitivity to ignition delay timeU Burke WK Metcalfe SM Burke KA Heufer P Dagaut HJ Curran Combust Flame 165 (2016) 125ndash13694
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
19
CH3OH + HȮ2 = ĊH2OH + H2O2
05 10 15 20104
105
106
107
108
109
1010
1011
1012
rate
con
stan
t (k)
cm
3 mol
-1 s
-1
1000 K T
Altarawneh (2011) Olm et al (2017) Alecu and Truhlar (2011) Klippenstein (2011)
104
105
106
107
108
109
1010
1011
1012
2000 1500 1000 500T K
20
Klippenstein et al1 reported high sensitivity to CH3OH + HȮ2 also calculated k Altarawneh et al2 and Alecu and Truhlar3
Olm et al4 via computer optimization using direct and indirect measurements Alecu and Truhlar attributed differences with Klippenstein et al calculations to
differences in treatment of anharmonicity
Possible chemically activated reactions involving HȮ2 radicals
1SJ Klippenstein LB Harding MJ Davis AS Tomlin RT Skodje Proc Combust Inst 33 (2011) 351ndash3572M Altarawneh AH Al‐Muhtaseb BZ Dlugogorski EM Kennedy JC Mackie J Comp Chem 32 (2011) 1725ndash17333IM Alecu DG Truhlar J Phys Chem A 115 (2011) 14599ndash146114C Olm T Varga Eacute Valkoacute HJ Curran T Turaacutenyi Combust Flame 186 (2017) 45ndash64
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
21
Carstensen and Dean12 for CH4 C2H6 C3H8 C4H10 + HȮ2
Aguilera‐Iparraguirre et al3 CH4 C2H6 C3H8 nC4H10 iC4H10 + HȮ2
mdashAgree well with the determinations of Walker et al
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash1573J Aguilera‐Iparraguirre HJ Curran W Klopper JM Simmie J Phys Chem A 112 (2008) 7047ndash7054
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
22ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
RH + CH3Ȯ2 = R + CH3O2H can also be important
HJ Curran P Gaffuri WJ Pitz CK WestbrookCombustion and Flame 129253ndash280 (2002)
iC8H18 oxidationφ = 10 in air p = 40 atm
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
23
RH + CH3Ȯ2 = R + CH3O2HĊH3 + O2 = CH3Ȯ2
RH + CH3Ȯ2 = R + CH3O2HCH3O2H = CH3Ȯ + ȮH
Carstensen and Dean1 for CH4C2H6 + ḢCH3Ȯ2C2H5Ȯ2
CarstensenDeanDeutschmann2 for CH4 C2H6 C3H8 C4H10 + HȮ2 CH3Ȯ2 C2H5Ȯ2 C3H7Ȯ2 C3H7Ȯ2 HC(O)Ȯ2 CH3C(O)Ȯ2
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash157
24ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
25
Rate rules for large molecular weight molecules
bull High temperature mechanismReaction class 1 Unimolecular fuel decompositionReaction class 2 H atom abstractions from fuelReaction class 3 Alkyl radical decompositionReaction class 4 Alkyl radical + O2 = olefin + HȮ2
Reaction class 5 Alkyl radical isomerizationReaction class 6 H atom abstraction from olefinsReaction class 7 Addition of radical species to olefinsReaction class 8 Alkenyl radical decompositionReaction class 9 Olefin decomposition
26Slide Courtesy of Dr William Pitz
Reaction rate rules for higher MW species
27Slide Courtesy of Dr William Pitz
Reaction classes for low temperature reactionsLow temperature mechanismReaction class 10 Alkyl radical addition to O2 (R + O2)Reaction class 11 R + RrsquoO2 = RȮ + RrsquoȮReaction class 12 Alkylperoxy radical isomerizationReaction class 13 RȮ2 + HȮ2 = ROOH + O2Reaction class 14 RȮ2 + H2O2 = ROOH + HȮ2Reaction class 15 RȮ2 + CH3Ȯ2 = RȮ + CH3Ȯ +O2Reaction class 16 RȮ2 + RrsquoȮ2 = RȮ + RrsquoȮ + O2Reaction class 17 ROOH = RȮ + ȮHReaction class 18 RȮ DecompositionReaction class 19 QOOH = Cyclic Ether + ȮHReaction class 20 QOOH = Olefin + HȮ2Reaction class 21 QOOH = Olefin + Aldehyde or Carbonyl + ȮHReaction class 22 Addition of QOOH to molecular oxygen O2Reaction class 23 Ȯ2QOOH isomerization to carbonylhydroperoxide + ȮHReaction class 24 Carbonylhydroperoxide decompositionReaction class 25 Reactions of cyclic ethers with ȮH and HȮ2
28
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
12
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Ḣ + O2 (+M) = HȮ2 (+M)RH + HȮ2 = R+ H2O2
H2O2 (+M) = ȮH + ȮH (+M)R + O2harr RȮ2
RȮ2 rarr olefin + HȮ2
Three distinct temperature regimes
13
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
14ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Importance of concerted HȮ2 elimination reaction
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
15
Intermediate temperature chemistrymdash Concerted eliminations are not well known ndash quantum chemistry
mdash Quelch et al1 first proposed Ċ2H5 + O2 = C2H4 + HȮ2 cyclic TS via concerted elimination
mdash Miyoshi23 variational TST and RRKMmaster equation (Ċ2iĊ3n‐s‐t‐Ċ4 + O2)
mdash Villano et al45 calculated 23 different straight and branched alkyl‐peroxyl radicals
mdash Goldsmith et al6 for the propyl + O2 system
Need for further studies of these reactions due to their high importance
1GE Quelch MM Gallo M Shen Y Xie HF Schaefer III D Moncrieff J Am Chem Soc 116 (1994) 4953ndash49622A Miyoshi J Phys Chem A 115 (2011) 3301ndash33253A Miyoshi A Int J Chem Kinet 44 (2012) 59ndash744SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 115 (2011) 13425ndash134425SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 116 (2012) 5068ndash50896CF Goldsmith WH Green SJ Klippenstein J Phys Chem A 2012 116 3325ndash3346
16
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
17
Few direct measurements of H‐atom abstraction by HȮ2 ndash lack of suitable precursors mdash CH2O + HȮ2 Jemi‐Alade et al1 using flash photolysismdash Walker et al23 made indirect relative rate measurementsmdash Scott and Walker4 review of alkanes aromatics and related compounds in 2002
Recent developments in quantitative measurements of HȮ2 radicals mdash Fluorescence assay by Gas Expansion by Blocquet et al5 (2013)mdash Dual‐modulation Faraday Spectroscopy67 (2014 2015)mdash Cavity ring‐down spectroscopy8 (2014)
These measurements are very useful in assessing mechanism performance1AA Jemi‐Alade PD Lightfoot R Lesclaux Chem Phys Lett 195 (1992) 25ndash302RR Baldwin RW Walker Proc Combust Inst 17 (1979) 525ndash5333RW Walker C Morley in Comprehensive Chem Kinetics (M J Pilling Ed) Elsevier Amsterdam 351 (1997)4M Scott RW Walker Combust Flame 129 (2002) 365ndash3775M Blocquet C Schoemaecker D Amedro O Herbinet F Battin‐Leclerc C Fittschen Proc Natl Acad Sci U S A 110 (2013) 20014ndash200176B Brumfield WT Sun Y Wang Y Ju G Wysocki Opt Lett 39 (2014) 1783ndash17867N Kurimoto B Brumfield X Yang T Wada P Dieacutevart G Wysocki Y Ju Proc Combust Inst 35(1) (2015) 457ndash4648M Djehiche NL Le Tan CD Jain G Dayma P Dagaut C Chauveau L Pillier A Tomas J Am Chem Soc 136 (2014) 16689ndash16694
93
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
18
CH3OH oxidation 855 O2 p = 40 atm and T = 885 K
Sensitivity to ignition delay timeU Burke WK Metcalfe SM Burke KA Heufer P Dagaut HJ Curran Combust Flame 165 (2016) 125ndash13694
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
19
CH3OH + HȮ2 = ĊH2OH + H2O2
05 10 15 20104
105
106
107
108
109
1010
1011
1012
rate
con
stan
t (k)
cm
3 mol
-1 s
-1
1000 K T
Altarawneh (2011) Olm et al (2017) Alecu and Truhlar (2011) Klippenstein (2011)
104
105
106
107
108
109
1010
1011
1012
2000 1500 1000 500T K
20
Klippenstein et al1 reported high sensitivity to CH3OH + HȮ2 also calculated k Altarawneh et al2 and Alecu and Truhlar3
Olm et al4 via computer optimization using direct and indirect measurements Alecu and Truhlar attributed differences with Klippenstein et al calculations to
differences in treatment of anharmonicity
Possible chemically activated reactions involving HȮ2 radicals
1SJ Klippenstein LB Harding MJ Davis AS Tomlin RT Skodje Proc Combust Inst 33 (2011) 351ndash3572M Altarawneh AH Al‐Muhtaseb BZ Dlugogorski EM Kennedy JC Mackie J Comp Chem 32 (2011) 1725ndash17333IM Alecu DG Truhlar J Phys Chem A 115 (2011) 14599ndash146114C Olm T Varga Eacute Valkoacute HJ Curran T Turaacutenyi Combust Flame 186 (2017) 45ndash64
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
21
Carstensen and Dean12 for CH4 C2H6 C3H8 C4H10 + HȮ2
Aguilera‐Iparraguirre et al3 CH4 C2H6 C3H8 nC4H10 iC4H10 + HȮ2
mdashAgree well with the determinations of Walker et al
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash1573J Aguilera‐Iparraguirre HJ Curran W Klopper JM Simmie J Phys Chem A 112 (2008) 7047ndash7054
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
22ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
RH + CH3Ȯ2 = R + CH3O2H can also be important
HJ Curran P Gaffuri WJ Pitz CK WestbrookCombustion and Flame 129253ndash280 (2002)
iC8H18 oxidationφ = 10 in air p = 40 atm
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
23
RH + CH3Ȯ2 = R + CH3O2HĊH3 + O2 = CH3Ȯ2
RH + CH3Ȯ2 = R + CH3O2HCH3O2H = CH3Ȯ + ȮH
Carstensen and Dean1 for CH4C2H6 + ḢCH3Ȯ2C2H5Ȯ2
CarstensenDeanDeutschmann2 for CH4 C2H6 C3H8 C4H10 + HȮ2 CH3Ȯ2 C2H5Ȯ2 C3H7Ȯ2 C3H7Ȯ2 HC(O)Ȯ2 CH3C(O)Ȯ2
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash157
24ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
25
Rate rules for large molecular weight molecules
bull High temperature mechanismReaction class 1 Unimolecular fuel decompositionReaction class 2 H atom abstractions from fuelReaction class 3 Alkyl radical decompositionReaction class 4 Alkyl radical + O2 = olefin + HȮ2
Reaction class 5 Alkyl radical isomerizationReaction class 6 H atom abstraction from olefinsReaction class 7 Addition of radical species to olefinsReaction class 8 Alkenyl radical decompositionReaction class 9 Olefin decomposition
26Slide Courtesy of Dr William Pitz
Reaction rate rules for higher MW species
27Slide Courtesy of Dr William Pitz
Reaction classes for low temperature reactionsLow temperature mechanismReaction class 10 Alkyl radical addition to O2 (R + O2)Reaction class 11 R + RrsquoO2 = RȮ + RrsquoȮReaction class 12 Alkylperoxy radical isomerizationReaction class 13 RȮ2 + HȮ2 = ROOH + O2Reaction class 14 RȮ2 + H2O2 = ROOH + HȮ2Reaction class 15 RȮ2 + CH3Ȯ2 = RȮ + CH3Ȯ +O2Reaction class 16 RȮ2 + RrsquoȮ2 = RȮ + RrsquoȮ + O2Reaction class 17 ROOH = RȮ + ȮHReaction class 18 RȮ DecompositionReaction class 19 QOOH = Cyclic Ether + ȮHReaction class 20 QOOH = Olefin + HȮ2Reaction class 21 QOOH = Olefin + Aldehyde or Carbonyl + ȮHReaction class 22 Addition of QOOH to molecular oxygen O2Reaction class 23 Ȯ2QOOH isomerization to carbonylhydroperoxide + ȮHReaction class 24 Carbonylhydroperoxide decompositionReaction class 25 Reactions of cyclic ethers with ȮH and HȮ2
28
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
13
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
14ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Importance of concerted HȮ2 elimination reaction
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
15
Intermediate temperature chemistrymdash Concerted eliminations are not well known ndash quantum chemistry
mdash Quelch et al1 first proposed Ċ2H5 + O2 = C2H4 + HȮ2 cyclic TS via concerted elimination
mdash Miyoshi23 variational TST and RRKMmaster equation (Ċ2iĊ3n‐s‐t‐Ċ4 + O2)
mdash Villano et al45 calculated 23 different straight and branched alkyl‐peroxyl radicals
mdash Goldsmith et al6 for the propyl + O2 system
Need for further studies of these reactions due to their high importance
1GE Quelch MM Gallo M Shen Y Xie HF Schaefer III D Moncrieff J Am Chem Soc 116 (1994) 4953ndash49622A Miyoshi J Phys Chem A 115 (2011) 3301ndash33253A Miyoshi A Int J Chem Kinet 44 (2012) 59ndash744SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 115 (2011) 13425ndash134425SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 116 (2012) 5068ndash50896CF Goldsmith WH Green SJ Klippenstein J Phys Chem A 2012 116 3325ndash3346
16
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
17
Few direct measurements of H‐atom abstraction by HȮ2 ndash lack of suitable precursors mdash CH2O + HȮ2 Jemi‐Alade et al1 using flash photolysismdash Walker et al23 made indirect relative rate measurementsmdash Scott and Walker4 review of alkanes aromatics and related compounds in 2002
Recent developments in quantitative measurements of HȮ2 radicals mdash Fluorescence assay by Gas Expansion by Blocquet et al5 (2013)mdash Dual‐modulation Faraday Spectroscopy67 (2014 2015)mdash Cavity ring‐down spectroscopy8 (2014)
These measurements are very useful in assessing mechanism performance1AA Jemi‐Alade PD Lightfoot R Lesclaux Chem Phys Lett 195 (1992) 25ndash302RR Baldwin RW Walker Proc Combust Inst 17 (1979) 525ndash5333RW Walker C Morley in Comprehensive Chem Kinetics (M J Pilling Ed) Elsevier Amsterdam 351 (1997)4M Scott RW Walker Combust Flame 129 (2002) 365ndash3775M Blocquet C Schoemaecker D Amedro O Herbinet F Battin‐Leclerc C Fittschen Proc Natl Acad Sci U S A 110 (2013) 20014ndash200176B Brumfield WT Sun Y Wang Y Ju G Wysocki Opt Lett 39 (2014) 1783ndash17867N Kurimoto B Brumfield X Yang T Wada P Dieacutevart G Wysocki Y Ju Proc Combust Inst 35(1) (2015) 457ndash4648M Djehiche NL Le Tan CD Jain G Dayma P Dagaut C Chauveau L Pillier A Tomas J Am Chem Soc 136 (2014) 16689ndash16694
93
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
18
CH3OH oxidation 855 O2 p = 40 atm and T = 885 K
Sensitivity to ignition delay timeU Burke WK Metcalfe SM Burke KA Heufer P Dagaut HJ Curran Combust Flame 165 (2016) 125ndash13694
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
19
CH3OH + HȮ2 = ĊH2OH + H2O2
05 10 15 20104
105
106
107
108
109
1010
1011
1012
rate
con
stan
t (k)
cm
3 mol
-1 s
-1
1000 K T
Altarawneh (2011) Olm et al (2017) Alecu and Truhlar (2011) Klippenstein (2011)
104
105
106
107
108
109
1010
1011
1012
2000 1500 1000 500T K
20
Klippenstein et al1 reported high sensitivity to CH3OH + HȮ2 also calculated k Altarawneh et al2 and Alecu and Truhlar3
Olm et al4 via computer optimization using direct and indirect measurements Alecu and Truhlar attributed differences with Klippenstein et al calculations to
differences in treatment of anharmonicity
Possible chemically activated reactions involving HȮ2 radicals
1SJ Klippenstein LB Harding MJ Davis AS Tomlin RT Skodje Proc Combust Inst 33 (2011) 351ndash3572M Altarawneh AH Al‐Muhtaseb BZ Dlugogorski EM Kennedy JC Mackie J Comp Chem 32 (2011) 1725ndash17333IM Alecu DG Truhlar J Phys Chem A 115 (2011) 14599ndash146114C Olm T Varga Eacute Valkoacute HJ Curran T Turaacutenyi Combust Flame 186 (2017) 45ndash64
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
21
Carstensen and Dean12 for CH4 C2H6 C3H8 C4H10 + HȮ2
Aguilera‐Iparraguirre et al3 CH4 C2H6 C3H8 nC4H10 iC4H10 + HȮ2
mdashAgree well with the determinations of Walker et al
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash1573J Aguilera‐Iparraguirre HJ Curran W Klopper JM Simmie J Phys Chem A 112 (2008) 7047ndash7054
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
22ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
RH + CH3Ȯ2 = R + CH3O2H can also be important
HJ Curran P Gaffuri WJ Pitz CK WestbrookCombustion and Flame 129253ndash280 (2002)
iC8H18 oxidationφ = 10 in air p = 40 atm
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
23
RH + CH3Ȯ2 = R + CH3O2HĊH3 + O2 = CH3Ȯ2
RH + CH3Ȯ2 = R + CH3O2HCH3O2H = CH3Ȯ + ȮH
Carstensen and Dean1 for CH4C2H6 + ḢCH3Ȯ2C2H5Ȯ2
CarstensenDeanDeutschmann2 for CH4 C2H6 C3H8 C4H10 + HȮ2 CH3Ȯ2 C2H5Ȯ2 C3H7Ȯ2 C3H7Ȯ2 HC(O)Ȯ2 CH3C(O)Ȯ2
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash157
24ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
25
Rate rules for large molecular weight molecules
bull High temperature mechanismReaction class 1 Unimolecular fuel decompositionReaction class 2 H atom abstractions from fuelReaction class 3 Alkyl radical decompositionReaction class 4 Alkyl radical + O2 = olefin + HȮ2
Reaction class 5 Alkyl radical isomerizationReaction class 6 H atom abstraction from olefinsReaction class 7 Addition of radical species to olefinsReaction class 8 Alkenyl radical decompositionReaction class 9 Olefin decomposition
26Slide Courtesy of Dr William Pitz
Reaction rate rules for higher MW species
27Slide Courtesy of Dr William Pitz
Reaction classes for low temperature reactionsLow temperature mechanismReaction class 10 Alkyl radical addition to O2 (R + O2)Reaction class 11 R + RrsquoO2 = RȮ + RrsquoȮReaction class 12 Alkylperoxy radical isomerizationReaction class 13 RȮ2 + HȮ2 = ROOH + O2Reaction class 14 RȮ2 + H2O2 = ROOH + HȮ2Reaction class 15 RȮ2 + CH3Ȯ2 = RȮ + CH3Ȯ +O2Reaction class 16 RȮ2 + RrsquoȮ2 = RȮ + RrsquoȮ + O2Reaction class 17 ROOH = RȮ + ȮHReaction class 18 RȮ DecompositionReaction class 19 QOOH = Cyclic Ether + ȮHReaction class 20 QOOH = Olefin + HȮ2Reaction class 21 QOOH = Olefin + Aldehyde or Carbonyl + ȮHReaction class 22 Addition of QOOH to molecular oxygen O2Reaction class 23 Ȯ2QOOH isomerization to carbonylhydroperoxide + ȮHReaction class 24 Carbonylhydroperoxide decompositionReaction class 25 Reactions of cyclic ethers with ȮH and HȮ2
28
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
14ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Importance of concerted HȮ2 elimination reaction
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
15
Intermediate temperature chemistrymdash Concerted eliminations are not well known ndash quantum chemistry
mdash Quelch et al1 first proposed Ċ2H5 + O2 = C2H4 + HȮ2 cyclic TS via concerted elimination
mdash Miyoshi23 variational TST and RRKMmaster equation (Ċ2iĊ3n‐s‐t‐Ċ4 + O2)
mdash Villano et al45 calculated 23 different straight and branched alkyl‐peroxyl radicals
mdash Goldsmith et al6 for the propyl + O2 system
Need for further studies of these reactions due to their high importance
1GE Quelch MM Gallo M Shen Y Xie HF Schaefer III D Moncrieff J Am Chem Soc 116 (1994) 4953ndash49622A Miyoshi J Phys Chem A 115 (2011) 3301ndash33253A Miyoshi A Int J Chem Kinet 44 (2012) 59ndash744SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 115 (2011) 13425ndash134425SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 116 (2012) 5068ndash50896CF Goldsmith WH Green SJ Klippenstein J Phys Chem A 2012 116 3325ndash3346
16
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
17
Few direct measurements of H‐atom abstraction by HȮ2 ndash lack of suitable precursors mdash CH2O + HȮ2 Jemi‐Alade et al1 using flash photolysismdash Walker et al23 made indirect relative rate measurementsmdash Scott and Walker4 review of alkanes aromatics and related compounds in 2002
Recent developments in quantitative measurements of HȮ2 radicals mdash Fluorescence assay by Gas Expansion by Blocquet et al5 (2013)mdash Dual‐modulation Faraday Spectroscopy67 (2014 2015)mdash Cavity ring‐down spectroscopy8 (2014)
These measurements are very useful in assessing mechanism performance1AA Jemi‐Alade PD Lightfoot R Lesclaux Chem Phys Lett 195 (1992) 25ndash302RR Baldwin RW Walker Proc Combust Inst 17 (1979) 525ndash5333RW Walker C Morley in Comprehensive Chem Kinetics (M J Pilling Ed) Elsevier Amsterdam 351 (1997)4M Scott RW Walker Combust Flame 129 (2002) 365ndash3775M Blocquet C Schoemaecker D Amedro O Herbinet F Battin‐Leclerc C Fittschen Proc Natl Acad Sci U S A 110 (2013) 20014ndash200176B Brumfield WT Sun Y Wang Y Ju G Wysocki Opt Lett 39 (2014) 1783ndash17867N Kurimoto B Brumfield X Yang T Wada P Dieacutevart G Wysocki Y Ju Proc Combust Inst 35(1) (2015) 457ndash4648M Djehiche NL Le Tan CD Jain G Dayma P Dagaut C Chauveau L Pillier A Tomas J Am Chem Soc 136 (2014) 16689ndash16694
93
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
18
CH3OH oxidation 855 O2 p = 40 atm and T = 885 K
Sensitivity to ignition delay timeU Burke WK Metcalfe SM Burke KA Heufer P Dagaut HJ Curran Combust Flame 165 (2016) 125ndash13694
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
19
CH3OH + HȮ2 = ĊH2OH + H2O2
05 10 15 20104
105
106
107
108
109
1010
1011
1012
rate
con
stan
t (k)
cm
3 mol
-1 s
-1
1000 K T
Altarawneh (2011) Olm et al (2017) Alecu and Truhlar (2011) Klippenstein (2011)
104
105
106
107
108
109
1010
1011
1012
2000 1500 1000 500T K
20
Klippenstein et al1 reported high sensitivity to CH3OH + HȮ2 also calculated k Altarawneh et al2 and Alecu and Truhlar3
Olm et al4 via computer optimization using direct and indirect measurements Alecu and Truhlar attributed differences with Klippenstein et al calculations to
differences in treatment of anharmonicity
Possible chemically activated reactions involving HȮ2 radicals
1SJ Klippenstein LB Harding MJ Davis AS Tomlin RT Skodje Proc Combust Inst 33 (2011) 351ndash3572M Altarawneh AH Al‐Muhtaseb BZ Dlugogorski EM Kennedy JC Mackie J Comp Chem 32 (2011) 1725ndash17333IM Alecu DG Truhlar J Phys Chem A 115 (2011) 14599ndash146114C Olm T Varga Eacute Valkoacute HJ Curran T Turaacutenyi Combust Flame 186 (2017) 45ndash64
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
21
Carstensen and Dean12 for CH4 C2H6 C3H8 C4H10 + HȮ2
Aguilera‐Iparraguirre et al3 CH4 C2H6 C3H8 nC4H10 iC4H10 + HȮ2
mdashAgree well with the determinations of Walker et al
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash1573J Aguilera‐Iparraguirre HJ Curran W Klopper JM Simmie J Phys Chem A 112 (2008) 7047ndash7054
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
22ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
RH + CH3Ȯ2 = R + CH3O2H can also be important
HJ Curran P Gaffuri WJ Pitz CK WestbrookCombustion and Flame 129253ndash280 (2002)
iC8H18 oxidationφ = 10 in air p = 40 atm
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
23
RH + CH3Ȯ2 = R + CH3O2HĊH3 + O2 = CH3Ȯ2
RH + CH3Ȯ2 = R + CH3O2HCH3O2H = CH3Ȯ + ȮH
Carstensen and Dean1 for CH4C2H6 + ḢCH3Ȯ2C2H5Ȯ2
CarstensenDeanDeutschmann2 for CH4 C2H6 C3H8 C4H10 + HȮ2 CH3Ȯ2 C2H5Ȯ2 C3H7Ȯ2 C3H7Ȯ2 HC(O)Ȯ2 CH3C(O)Ȯ2
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash157
24ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
25
Rate rules for large molecular weight molecules
bull High temperature mechanismReaction class 1 Unimolecular fuel decompositionReaction class 2 H atom abstractions from fuelReaction class 3 Alkyl radical decompositionReaction class 4 Alkyl radical + O2 = olefin + HȮ2
Reaction class 5 Alkyl radical isomerizationReaction class 6 H atom abstraction from olefinsReaction class 7 Addition of radical species to olefinsReaction class 8 Alkenyl radical decompositionReaction class 9 Olefin decomposition
26Slide Courtesy of Dr William Pitz
Reaction rate rules for higher MW species
27Slide Courtesy of Dr William Pitz
Reaction classes for low temperature reactionsLow temperature mechanismReaction class 10 Alkyl radical addition to O2 (R + O2)Reaction class 11 R + RrsquoO2 = RȮ + RrsquoȮReaction class 12 Alkylperoxy radical isomerizationReaction class 13 RȮ2 + HȮ2 = ROOH + O2Reaction class 14 RȮ2 + H2O2 = ROOH + HȮ2Reaction class 15 RȮ2 + CH3Ȯ2 = RȮ + CH3Ȯ +O2Reaction class 16 RȮ2 + RrsquoȮ2 = RȮ + RrsquoȮ + O2Reaction class 17 ROOH = RȮ + ȮHReaction class 18 RȮ DecompositionReaction class 19 QOOH = Cyclic Ether + ȮHReaction class 20 QOOH = Olefin + HȮ2Reaction class 21 QOOH = Olefin + Aldehyde or Carbonyl + ȮHReaction class 22 Addition of QOOH to molecular oxygen O2Reaction class 23 Ȯ2QOOH isomerization to carbonylhydroperoxide + ȮHReaction class 24 Carbonylhydroperoxide decompositionReaction class 25 Reactions of cyclic ethers with ȮH and HȮ2
28
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
15
Intermediate temperature chemistrymdash Concerted eliminations are not well known ndash quantum chemistry
mdash Quelch et al1 first proposed Ċ2H5 + O2 = C2H4 + HȮ2 cyclic TS via concerted elimination
mdash Miyoshi23 variational TST and RRKMmaster equation (Ċ2iĊ3n‐s‐t‐Ċ4 + O2)
mdash Villano et al45 calculated 23 different straight and branched alkyl‐peroxyl radicals
mdash Goldsmith et al6 for the propyl + O2 system
Need for further studies of these reactions due to their high importance
1GE Quelch MM Gallo M Shen Y Xie HF Schaefer III D Moncrieff J Am Chem Soc 116 (1994) 4953ndash49622A Miyoshi J Phys Chem A 115 (2011) 3301ndash33253A Miyoshi A Int J Chem Kinet 44 (2012) 59ndash744SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 115 (2011) 13425ndash134425SM Villano LK Huynh HH Carstensen AM Dean J Phys Chem A 116 (2012) 5068ndash50896CF Goldsmith WH Green SJ Klippenstein J Phys Chem A 2012 116 3325ndash3346
16
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
17
Few direct measurements of H‐atom abstraction by HȮ2 ndash lack of suitable precursors mdash CH2O + HȮ2 Jemi‐Alade et al1 using flash photolysismdash Walker et al23 made indirect relative rate measurementsmdash Scott and Walker4 review of alkanes aromatics and related compounds in 2002
Recent developments in quantitative measurements of HȮ2 radicals mdash Fluorescence assay by Gas Expansion by Blocquet et al5 (2013)mdash Dual‐modulation Faraday Spectroscopy67 (2014 2015)mdash Cavity ring‐down spectroscopy8 (2014)
These measurements are very useful in assessing mechanism performance1AA Jemi‐Alade PD Lightfoot R Lesclaux Chem Phys Lett 195 (1992) 25ndash302RR Baldwin RW Walker Proc Combust Inst 17 (1979) 525ndash5333RW Walker C Morley in Comprehensive Chem Kinetics (M J Pilling Ed) Elsevier Amsterdam 351 (1997)4M Scott RW Walker Combust Flame 129 (2002) 365ndash3775M Blocquet C Schoemaecker D Amedro O Herbinet F Battin‐Leclerc C Fittschen Proc Natl Acad Sci U S A 110 (2013) 20014ndash200176B Brumfield WT Sun Y Wang Y Ju G Wysocki Opt Lett 39 (2014) 1783ndash17867N Kurimoto B Brumfield X Yang T Wada P Dieacutevart G Wysocki Y Ju Proc Combust Inst 35(1) (2015) 457ndash4648M Djehiche NL Le Tan CD Jain G Dayma P Dagaut C Chauveau L Pillier A Tomas J Am Chem Soc 136 (2014) 16689ndash16694
93
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
18
CH3OH oxidation 855 O2 p = 40 atm and T = 885 K
Sensitivity to ignition delay timeU Burke WK Metcalfe SM Burke KA Heufer P Dagaut HJ Curran Combust Flame 165 (2016) 125ndash13694
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
19
CH3OH + HȮ2 = ĊH2OH + H2O2
05 10 15 20104
105
106
107
108
109
1010
1011
1012
rate
con
stan
t (k)
cm
3 mol
-1 s
-1
1000 K T
Altarawneh (2011) Olm et al (2017) Alecu and Truhlar (2011) Klippenstein (2011)
104
105
106
107
108
109
1010
1011
1012
2000 1500 1000 500T K
20
Klippenstein et al1 reported high sensitivity to CH3OH + HȮ2 also calculated k Altarawneh et al2 and Alecu and Truhlar3
Olm et al4 via computer optimization using direct and indirect measurements Alecu and Truhlar attributed differences with Klippenstein et al calculations to
differences in treatment of anharmonicity
Possible chemically activated reactions involving HȮ2 radicals
1SJ Klippenstein LB Harding MJ Davis AS Tomlin RT Skodje Proc Combust Inst 33 (2011) 351ndash3572M Altarawneh AH Al‐Muhtaseb BZ Dlugogorski EM Kennedy JC Mackie J Comp Chem 32 (2011) 1725ndash17333IM Alecu DG Truhlar J Phys Chem A 115 (2011) 14599ndash146114C Olm T Varga Eacute Valkoacute HJ Curran T Turaacutenyi Combust Flame 186 (2017) 45ndash64
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
21
Carstensen and Dean12 for CH4 C2H6 C3H8 C4H10 + HȮ2
Aguilera‐Iparraguirre et al3 CH4 C2H6 C3H8 nC4H10 iC4H10 + HȮ2
mdashAgree well with the determinations of Walker et al
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash1573J Aguilera‐Iparraguirre HJ Curran W Klopper JM Simmie J Phys Chem A 112 (2008) 7047ndash7054
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
22ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
RH + CH3Ȯ2 = R + CH3O2H can also be important
HJ Curran P Gaffuri WJ Pitz CK WestbrookCombustion and Flame 129253ndash280 (2002)
iC8H18 oxidationφ = 10 in air p = 40 atm
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
23
RH + CH3Ȯ2 = R + CH3O2HĊH3 + O2 = CH3Ȯ2
RH + CH3Ȯ2 = R + CH3O2HCH3O2H = CH3Ȯ + ȮH
Carstensen and Dean1 for CH4C2H6 + ḢCH3Ȯ2C2H5Ȯ2
CarstensenDeanDeutschmann2 for CH4 C2H6 C3H8 C4H10 + HȮ2 CH3Ȯ2 C2H5Ȯ2 C3H7Ȯ2 C3H7Ȯ2 HC(O)Ȯ2 CH3C(O)Ȯ2
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash157
24ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
25
Rate rules for large molecular weight molecules
bull High temperature mechanismReaction class 1 Unimolecular fuel decompositionReaction class 2 H atom abstractions from fuelReaction class 3 Alkyl radical decompositionReaction class 4 Alkyl radical + O2 = olefin + HȮ2
Reaction class 5 Alkyl radical isomerizationReaction class 6 H atom abstraction from olefinsReaction class 7 Addition of radical species to olefinsReaction class 8 Alkenyl radical decompositionReaction class 9 Olefin decomposition
26Slide Courtesy of Dr William Pitz
Reaction rate rules for higher MW species
27Slide Courtesy of Dr William Pitz
Reaction classes for low temperature reactionsLow temperature mechanismReaction class 10 Alkyl radical addition to O2 (R + O2)Reaction class 11 R + RrsquoO2 = RȮ + RrsquoȮReaction class 12 Alkylperoxy radical isomerizationReaction class 13 RȮ2 + HȮ2 = ROOH + O2Reaction class 14 RȮ2 + H2O2 = ROOH + HȮ2Reaction class 15 RȮ2 + CH3Ȯ2 = RȮ + CH3Ȯ +O2Reaction class 16 RȮ2 + RrsquoȮ2 = RȮ + RrsquoȮ + O2Reaction class 17 ROOH = RȮ + ȮHReaction class 18 RȮ DecompositionReaction class 19 QOOH = Cyclic Ether + ȮHReaction class 20 QOOH = Olefin + HȮ2Reaction class 21 QOOH = Olefin + Aldehyde or Carbonyl + ȮHReaction class 22 Addition of QOOH to molecular oxygen O2Reaction class 23 Ȯ2QOOH isomerization to carbonylhydroperoxide + ȮHReaction class 24 Carbonylhydroperoxide decompositionReaction class 25 Reactions of cyclic ethers with ȮH and HȮ2
28
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
16
1) Ḣ + O2 rarr Ouml + ȮHOuml + H2 rarr Ḣ + ȮH High T ( 1100 K)
OumlH + H2 rarr H2O + ḢNet 2H2 + O2 rarr ȮH + Ḣ + H2O
2) Ḣ + O2 (+M) rarr HȮ2 (+M) Intermediate TRH + HȮ2 rarr R + H2O2 (850 1100 K)H2O2 (+M) rarr ȮH + ȮH (+M) chain branching
RȮ2 rarr olefin + HȮ2 (NTC)QOOH rarr cyclic ether + ȮH (NTC)
3) R + O2 harr RȮ2 Low T (~500 850 K)
RȮ2 QOOH harr Ȯ2QOOH RȮ + ȮH + ȮH
Three distinct chain branching pathways
17
Few direct measurements of H‐atom abstraction by HȮ2 ndash lack of suitable precursors mdash CH2O + HȮ2 Jemi‐Alade et al1 using flash photolysismdash Walker et al23 made indirect relative rate measurementsmdash Scott and Walker4 review of alkanes aromatics and related compounds in 2002
Recent developments in quantitative measurements of HȮ2 radicals mdash Fluorescence assay by Gas Expansion by Blocquet et al5 (2013)mdash Dual‐modulation Faraday Spectroscopy67 (2014 2015)mdash Cavity ring‐down spectroscopy8 (2014)
These measurements are very useful in assessing mechanism performance1AA Jemi‐Alade PD Lightfoot R Lesclaux Chem Phys Lett 195 (1992) 25ndash302RR Baldwin RW Walker Proc Combust Inst 17 (1979) 525ndash5333RW Walker C Morley in Comprehensive Chem Kinetics (M J Pilling Ed) Elsevier Amsterdam 351 (1997)4M Scott RW Walker Combust Flame 129 (2002) 365ndash3775M Blocquet C Schoemaecker D Amedro O Herbinet F Battin‐Leclerc C Fittschen Proc Natl Acad Sci U S A 110 (2013) 20014ndash200176B Brumfield WT Sun Y Wang Y Ju G Wysocki Opt Lett 39 (2014) 1783ndash17867N Kurimoto B Brumfield X Yang T Wada P Dieacutevart G Wysocki Y Ju Proc Combust Inst 35(1) (2015) 457ndash4648M Djehiche NL Le Tan CD Jain G Dayma P Dagaut C Chauveau L Pillier A Tomas J Am Chem Soc 136 (2014) 16689ndash16694
93
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
18
CH3OH oxidation 855 O2 p = 40 atm and T = 885 K
Sensitivity to ignition delay timeU Burke WK Metcalfe SM Burke KA Heufer P Dagaut HJ Curran Combust Flame 165 (2016) 125ndash13694
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
19
CH3OH + HȮ2 = ĊH2OH + H2O2
05 10 15 20104
105
106
107
108
109
1010
1011
1012
rate
con
stan
t (k)
cm
3 mol
-1 s
-1
1000 K T
Altarawneh (2011) Olm et al (2017) Alecu and Truhlar (2011) Klippenstein (2011)
104
105
106
107
108
109
1010
1011
1012
2000 1500 1000 500T K
20
Klippenstein et al1 reported high sensitivity to CH3OH + HȮ2 also calculated k Altarawneh et al2 and Alecu and Truhlar3
Olm et al4 via computer optimization using direct and indirect measurements Alecu and Truhlar attributed differences with Klippenstein et al calculations to
differences in treatment of anharmonicity
Possible chemically activated reactions involving HȮ2 radicals
1SJ Klippenstein LB Harding MJ Davis AS Tomlin RT Skodje Proc Combust Inst 33 (2011) 351ndash3572M Altarawneh AH Al‐Muhtaseb BZ Dlugogorski EM Kennedy JC Mackie J Comp Chem 32 (2011) 1725ndash17333IM Alecu DG Truhlar J Phys Chem A 115 (2011) 14599ndash146114C Olm T Varga Eacute Valkoacute HJ Curran T Turaacutenyi Combust Flame 186 (2017) 45ndash64
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
21
Carstensen and Dean12 for CH4 C2H6 C3H8 C4H10 + HȮ2
Aguilera‐Iparraguirre et al3 CH4 C2H6 C3H8 nC4H10 iC4H10 + HȮ2
mdashAgree well with the determinations of Walker et al
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash1573J Aguilera‐Iparraguirre HJ Curran W Klopper JM Simmie J Phys Chem A 112 (2008) 7047ndash7054
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
22ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
RH + CH3Ȯ2 = R + CH3O2H can also be important
HJ Curran P Gaffuri WJ Pitz CK WestbrookCombustion and Flame 129253ndash280 (2002)
iC8H18 oxidationφ = 10 in air p = 40 atm
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
23
RH + CH3Ȯ2 = R + CH3O2HĊH3 + O2 = CH3Ȯ2
RH + CH3Ȯ2 = R + CH3O2HCH3O2H = CH3Ȯ + ȮH
Carstensen and Dean1 for CH4C2H6 + ḢCH3Ȯ2C2H5Ȯ2
CarstensenDeanDeutschmann2 for CH4 C2H6 C3H8 C4H10 + HȮ2 CH3Ȯ2 C2H5Ȯ2 C3H7Ȯ2 C3H7Ȯ2 HC(O)Ȯ2 CH3C(O)Ȯ2
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash157
24ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
25
Rate rules for large molecular weight molecules
bull High temperature mechanismReaction class 1 Unimolecular fuel decompositionReaction class 2 H atom abstractions from fuelReaction class 3 Alkyl radical decompositionReaction class 4 Alkyl radical + O2 = olefin + HȮ2
Reaction class 5 Alkyl radical isomerizationReaction class 6 H atom abstraction from olefinsReaction class 7 Addition of radical species to olefinsReaction class 8 Alkenyl radical decompositionReaction class 9 Olefin decomposition
26Slide Courtesy of Dr William Pitz
Reaction rate rules for higher MW species
27Slide Courtesy of Dr William Pitz
Reaction classes for low temperature reactionsLow temperature mechanismReaction class 10 Alkyl radical addition to O2 (R + O2)Reaction class 11 R + RrsquoO2 = RȮ + RrsquoȮReaction class 12 Alkylperoxy radical isomerizationReaction class 13 RȮ2 + HȮ2 = ROOH + O2Reaction class 14 RȮ2 + H2O2 = ROOH + HȮ2Reaction class 15 RȮ2 + CH3Ȯ2 = RȮ + CH3Ȯ +O2Reaction class 16 RȮ2 + RrsquoȮ2 = RȮ + RrsquoȮ + O2Reaction class 17 ROOH = RȮ + ȮHReaction class 18 RȮ DecompositionReaction class 19 QOOH = Cyclic Ether + ȮHReaction class 20 QOOH = Olefin + HȮ2Reaction class 21 QOOH = Olefin + Aldehyde or Carbonyl + ȮHReaction class 22 Addition of QOOH to molecular oxygen O2Reaction class 23 Ȯ2QOOH isomerization to carbonylhydroperoxide + ȮHReaction class 24 Carbonylhydroperoxide decompositionReaction class 25 Reactions of cyclic ethers with ȮH and HȮ2
28
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
17
Few direct measurements of H‐atom abstraction by HȮ2 ndash lack of suitable precursors mdash CH2O + HȮ2 Jemi‐Alade et al1 using flash photolysismdash Walker et al23 made indirect relative rate measurementsmdash Scott and Walker4 review of alkanes aromatics and related compounds in 2002
Recent developments in quantitative measurements of HȮ2 radicals mdash Fluorescence assay by Gas Expansion by Blocquet et al5 (2013)mdash Dual‐modulation Faraday Spectroscopy67 (2014 2015)mdash Cavity ring‐down spectroscopy8 (2014)
These measurements are very useful in assessing mechanism performance1AA Jemi‐Alade PD Lightfoot R Lesclaux Chem Phys Lett 195 (1992) 25ndash302RR Baldwin RW Walker Proc Combust Inst 17 (1979) 525ndash5333RW Walker C Morley in Comprehensive Chem Kinetics (M J Pilling Ed) Elsevier Amsterdam 351 (1997)4M Scott RW Walker Combust Flame 129 (2002) 365ndash3775M Blocquet C Schoemaecker D Amedro O Herbinet F Battin‐Leclerc C Fittschen Proc Natl Acad Sci U S A 110 (2013) 20014ndash200176B Brumfield WT Sun Y Wang Y Ju G Wysocki Opt Lett 39 (2014) 1783ndash17867N Kurimoto B Brumfield X Yang T Wada P Dieacutevart G Wysocki Y Ju Proc Combust Inst 35(1) (2015) 457ndash4648M Djehiche NL Le Tan CD Jain G Dayma P Dagaut C Chauveau L Pillier A Tomas J Am Chem Soc 136 (2014) 16689ndash16694
93
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
18
CH3OH oxidation 855 O2 p = 40 atm and T = 885 K
Sensitivity to ignition delay timeU Burke WK Metcalfe SM Burke KA Heufer P Dagaut HJ Curran Combust Flame 165 (2016) 125ndash13694
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
19
CH3OH + HȮ2 = ĊH2OH + H2O2
05 10 15 20104
105
106
107
108
109
1010
1011
1012
rate
con
stan
t (k)
cm
3 mol
-1 s
-1
1000 K T
Altarawneh (2011) Olm et al (2017) Alecu and Truhlar (2011) Klippenstein (2011)
104
105
106
107
108
109
1010
1011
1012
2000 1500 1000 500T K
20
Klippenstein et al1 reported high sensitivity to CH3OH + HȮ2 also calculated k Altarawneh et al2 and Alecu and Truhlar3
Olm et al4 via computer optimization using direct and indirect measurements Alecu and Truhlar attributed differences with Klippenstein et al calculations to
differences in treatment of anharmonicity
Possible chemically activated reactions involving HȮ2 radicals
1SJ Klippenstein LB Harding MJ Davis AS Tomlin RT Skodje Proc Combust Inst 33 (2011) 351ndash3572M Altarawneh AH Al‐Muhtaseb BZ Dlugogorski EM Kennedy JC Mackie J Comp Chem 32 (2011) 1725ndash17333IM Alecu DG Truhlar J Phys Chem A 115 (2011) 14599ndash146114C Olm T Varga Eacute Valkoacute HJ Curran T Turaacutenyi Combust Flame 186 (2017) 45ndash64
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
21
Carstensen and Dean12 for CH4 C2H6 C3H8 C4H10 + HȮ2
Aguilera‐Iparraguirre et al3 CH4 C2H6 C3H8 nC4H10 iC4H10 + HȮ2
mdashAgree well with the determinations of Walker et al
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash1573J Aguilera‐Iparraguirre HJ Curran W Klopper JM Simmie J Phys Chem A 112 (2008) 7047ndash7054
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
22ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
RH + CH3Ȯ2 = R + CH3O2H can also be important
HJ Curran P Gaffuri WJ Pitz CK WestbrookCombustion and Flame 129253ndash280 (2002)
iC8H18 oxidationφ = 10 in air p = 40 atm
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
23
RH + CH3Ȯ2 = R + CH3O2HĊH3 + O2 = CH3Ȯ2
RH + CH3Ȯ2 = R + CH3O2HCH3O2H = CH3Ȯ + ȮH
Carstensen and Dean1 for CH4C2H6 + ḢCH3Ȯ2C2H5Ȯ2
CarstensenDeanDeutschmann2 for CH4 C2H6 C3H8 C4H10 + HȮ2 CH3Ȯ2 C2H5Ȯ2 C3H7Ȯ2 C3H7Ȯ2 HC(O)Ȯ2 CH3C(O)Ȯ2
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash157
24ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
25
Rate rules for large molecular weight molecules
bull High temperature mechanismReaction class 1 Unimolecular fuel decompositionReaction class 2 H atom abstractions from fuelReaction class 3 Alkyl radical decompositionReaction class 4 Alkyl radical + O2 = olefin + HȮ2
Reaction class 5 Alkyl radical isomerizationReaction class 6 H atom abstraction from olefinsReaction class 7 Addition of radical species to olefinsReaction class 8 Alkenyl radical decompositionReaction class 9 Olefin decomposition
26Slide Courtesy of Dr William Pitz
Reaction rate rules for higher MW species
27Slide Courtesy of Dr William Pitz
Reaction classes for low temperature reactionsLow temperature mechanismReaction class 10 Alkyl radical addition to O2 (R + O2)Reaction class 11 R + RrsquoO2 = RȮ + RrsquoȮReaction class 12 Alkylperoxy radical isomerizationReaction class 13 RȮ2 + HȮ2 = ROOH + O2Reaction class 14 RȮ2 + H2O2 = ROOH + HȮ2Reaction class 15 RȮ2 + CH3Ȯ2 = RȮ + CH3Ȯ +O2Reaction class 16 RȮ2 + RrsquoȮ2 = RȮ + RrsquoȮ + O2Reaction class 17 ROOH = RȮ + ȮHReaction class 18 RȮ DecompositionReaction class 19 QOOH = Cyclic Ether + ȮHReaction class 20 QOOH = Olefin + HȮ2Reaction class 21 QOOH = Olefin + Aldehyde or Carbonyl + ȮHReaction class 22 Addition of QOOH to molecular oxygen O2Reaction class 23 Ȯ2QOOH isomerization to carbonylhydroperoxide + ȮHReaction class 24 Carbonylhydroperoxide decompositionReaction class 25 Reactions of cyclic ethers with ȮH and HȮ2
28
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
18
CH3OH oxidation 855 O2 p = 40 atm and T = 885 K
Sensitivity to ignition delay timeU Burke WK Metcalfe SM Burke KA Heufer P Dagaut HJ Curran Combust Flame 165 (2016) 125ndash13694
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
19
CH3OH + HȮ2 = ĊH2OH + H2O2
05 10 15 20104
105
106
107
108
109
1010
1011
1012
rate
con
stan
t (k)
cm
3 mol
-1 s
-1
1000 K T
Altarawneh (2011) Olm et al (2017) Alecu and Truhlar (2011) Klippenstein (2011)
104
105
106
107
108
109
1010
1011
1012
2000 1500 1000 500T K
20
Klippenstein et al1 reported high sensitivity to CH3OH + HȮ2 also calculated k Altarawneh et al2 and Alecu and Truhlar3
Olm et al4 via computer optimization using direct and indirect measurements Alecu and Truhlar attributed differences with Klippenstein et al calculations to
differences in treatment of anharmonicity
Possible chemically activated reactions involving HȮ2 radicals
1SJ Klippenstein LB Harding MJ Davis AS Tomlin RT Skodje Proc Combust Inst 33 (2011) 351ndash3572M Altarawneh AH Al‐Muhtaseb BZ Dlugogorski EM Kennedy JC Mackie J Comp Chem 32 (2011) 1725ndash17333IM Alecu DG Truhlar J Phys Chem A 115 (2011) 14599ndash146114C Olm T Varga Eacute Valkoacute HJ Curran T Turaacutenyi Combust Flame 186 (2017) 45ndash64
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
21
Carstensen and Dean12 for CH4 C2H6 C3H8 C4H10 + HȮ2
Aguilera‐Iparraguirre et al3 CH4 C2H6 C3H8 nC4H10 iC4H10 + HȮ2
mdashAgree well with the determinations of Walker et al
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash1573J Aguilera‐Iparraguirre HJ Curran W Klopper JM Simmie J Phys Chem A 112 (2008) 7047ndash7054
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
22ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
RH + CH3Ȯ2 = R + CH3O2H can also be important
HJ Curran P Gaffuri WJ Pitz CK WestbrookCombustion and Flame 129253ndash280 (2002)
iC8H18 oxidationφ = 10 in air p = 40 atm
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
23
RH + CH3Ȯ2 = R + CH3O2HĊH3 + O2 = CH3Ȯ2
RH + CH3Ȯ2 = R + CH3O2HCH3O2H = CH3Ȯ + ȮH
Carstensen and Dean1 for CH4C2H6 + ḢCH3Ȯ2C2H5Ȯ2
CarstensenDeanDeutschmann2 for CH4 C2H6 C3H8 C4H10 + HȮ2 CH3Ȯ2 C2H5Ȯ2 C3H7Ȯ2 C3H7Ȯ2 HC(O)Ȯ2 CH3C(O)Ȯ2
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash157
24ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
25
Rate rules for large molecular weight molecules
bull High temperature mechanismReaction class 1 Unimolecular fuel decompositionReaction class 2 H atom abstractions from fuelReaction class 3 Alkyl radical decompositionReaction class 4 Alkyl radical + O2 = olefin + HȮ2
Reaction class 5 Alkyl radical isomerizationReaction class 6 H atom abstraction from olefinsReaction class 7 Addition of radical species to olefinsReaction class 8 Alkenyl radical decompositionReaction class 9 Olefin decomposition
26Slide Courtesy of Dr William Pitz
Reaction rate rules for higher MW species
27Slide Courtesy of Dr William Pitz
Reaction classes for low temperature reactionsLow temperature mechanismReaction class 10 Alkyl radical addition to O2 (R + O2)Reaction class 11 R + RrsquoO2 = RȮ + RrsquoȮReaction class 12 Alkylperoxy radical isomerizationReaction class 13 RȮ2 + HȮ2 = ROOH + O2Reaction class 14 RȮ2 + H2O2 = ROOH + HȮ2Reaction class 15 RȮ2 + CH3Ȯ2 = RȮ + CH3Ȯ +O2Reaction class 16 RȮ2 + RrsquoȮ2 = RȮ + RrsquoȮ + O2Reaction class 17 ROOH = RȮ + ȮHReaction class 18 RȮ DecompositionReaction class 19 QOOH = Cyclic Ether + ȮHReaction class 20 QOOH = Olefin + HȮ2Reaction class 21 QOOH = Olefin + Aldehyde or Carbonyl + ȮHReaction class 22 Addition of QOOH to molecular oxygen O2Reaction class 23 Ȯ2QOOH isomerization to carbonylhydroperoxide + ȮHReaction class 24 Carbonylhydroperoxide decompositionReaction class 25 Reactions of cyclic ethers with ȮH and HȮ2
28
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
19
CH3OH + HȮ2 = ĊH2OH + H2O2
05 10 15 20104
105
106
107
108
109
1010
1011
1012
rate
con
stan
t (k)
cm
3 mol
-1 s
-1
1000 K T
Altarawneh (2011) Olm et al (2017) Alecu and Truhlar (2011) Klippenstein (2011)
104
105
106
107
108
109
1010
1011
1012
2000 1500 1000 500T K
20
Klippenstein et al1 reported high sensitivity to CH3OH + HȮ2 also calculated k Altarawneh et al2 and Alecu and Truhlar3
Olm et al4 via computer optimization using direct and indirect measurements Alecu and Truhlar attributed differences with Klippenstein et al calculations to
differences in treatment of anharmonicity
Possible chemically activated reactions involving HȮ2 radicals
1SJ Klippenstein LB Harding MJ Davis AS Tomlin RT Skodje Proc Combust Inst 33 (2011) 351ndash3572M Altarawneh AH Al‐Muhtaseb BZ Dlugogorski EM Kennedy JC Mackie J Comp Chem 32 (2011) 1725ndash17333IM Alecu DG Truhlar J Phys Chem A 115 (2011) 14599ndash146114C Olm T Varga Eacute Valkoacute HJ Curran T Turaacutenyi Combust Flame 186 (2017) 45ndash64
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
21
Carstensen and Dean12 for CH4 C2H6 C3H8 C4H10 + HȮ2
Aguilera‐Iparraguirre et al3 CH4 C2H6 C3H8 nC4H10 iC4H10 + HȮ2
mdashAgree well with the determinations of Walker et al
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash1573J Aguilera‐Iparraguirre HJ Curran W Klopper JM Simmie J Phys Chem A 112 (2008) 7047ndash7054
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
22ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
RH + CH3Ȯ2 = R + CH3O2H can also be important
HJ Curran P Gaffuri WJ Pitz CK WestbrookCombustion and Flame 129253ndash280 (2002)
iC8H18 oxidationφ = 10 in air p = 40 atm
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
23
RH + CH3Ȯ2 = R + CH3O2HĊH3 + O2 = CH3Ȯ2
RH + CH3Ȯ2 = R + CH3O2HCH3O2H = CH3Ȯ + ȮH
Carstensen and Dean1 for CH4C2H6 + ḢCH3Ȯ2C2H5Ȯ2
CarstensenDeanDeutschmann2 for CH4 C2H6 C3H8 C4H10 + HȮ2 CH3Ȯ2 C2H5Ȯ2 C3H7Ȯ2 C3H7Ȯ2 HC(O)Ȯ2 CH3C(O)Ȯ2
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash157
24ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
25
Rate rules for large molecular weight molecules
bull High temperature mechanismReaction class 1 Unimolecular fuel decompositionReaction class 2 H atom abstractions from fuelReaction class 3 Alkyl radical decompositionReaction class 4 Alkyl radical + O2 = olefin + HȮ2
Reaction class 5 Alkyl radical isomerizationReaction class 6 H atom abstraction from olefinsReaction class 7 Addition of radical species to olefinsReaction class 8 Alkenyl radical decompositionReaction class 9 Olefin decomposition
26Slide Courtesy of Dr William Pitz
Reaction rate rules for higher MW species
27Slide Courtesy of Dr William Pitz
Reaction classes for low temperature reactionsLow temperature mechanismReaction class 10 Alkyl radical addition to O2 (R + O2)Reaction class 11 R + RrsquoO2 = RȮ + RrsquoȮReaction class 12 Alkylperoxy radical isomerizationReaction class 13 RȮ2 + HȮ2 = ROOH + O2Reaction class 14 RȮ2 + H2O2 = ROOH + HȮ2Reaction class 15 RȮ2 + CH3Ȯ2 = RȮ + CH3Ȯ +O2Reaction class 16 RȮ2 + RrsquoȮ2 = RȮ + RrsquoȮ + O2Reaction class 17 ROOH = RȮ + ȮHReaction class 18 RȮ DecompositionReaction class 19 QOOH = Cyclic Ether + ȮHReaction class 20 QOOH = Olefin + HȮ2Reaction class 21 QOOH = Olefin + Aldehyde or Carbonyl + ȮHReaction class 22 Addition of QOOH to molecular oxygen O2Reaction class 23 Ȯ2QOOH isomerization to carbonylhydroperoxide + ȮHReaction class 24 Carbonylhydroperoxide decompositionReaction class 25 Reactions of cyclic ethers with ȮH and HȮ2
28
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
20
Klippenstein et al1 reported high sensitivity to CH3OH + HȮ2 also calculated k Altarawneh et al2 and Alecu and Truhlar3
Olm et al4 via computer optimization using direct and indirect measurements Alecu and Truhlar attributed differences with Klippenstein et al calculations to
differences in treatment of anharmonicity
Possible chemically activated reactions involving HȮ2 radicals
1SJ Klippenstein LB Harding MJ Davis AS Tomlin RT Skodje Proc Combust Inst 33 (2011) 351ndash3572M Altarawneh AH Al‐Muhtaseb BZ Dlugogorski EM Kennedy JC Mackie J Comp Chem 32 (2011) 1725ndash17333IM Alecu DG Truhlar J Phys Chem A 115 (2011) 14599ndash146114C Olm T Varga Eacute Valkoacute HJ Curran T Turaacutenyi Combust Flame 186 (2017) 45ndash64
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
21
Carstensen and Dean12 for CH4 C2H6 C3H8 C4H10 + HȮ2
Aguilera‐Iparraguirre et al3 CH4 C2H6 C3H8 nC4H10 iC4H10 + HȮ2
mdashAgree well with the determinations of Walker et al
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash1573J Aguilera‐Iparraguirre HJ Curran W Klopper JM Simmie J Phys Chem A 112 (2008) 7047ndash7054
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
22ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
RH + CH3Ȯ2 = R + CH3O2H can also be important
HJ Curran P Gaffuri WJ Pitz CK WestbrookCombustion and Flame 129253ndash280 (2002)
iC8H18 oxidationφ = 10 in air p = 40 atm
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
23
RH + CH3Ȯ2 = R + CH3O2HĊH3 + O2 = CH3Ȯ2
RH + CH3Ȯ2 = R + CH3O2HCH3O2H = CH3Ȯ + ȮH
Carstensen and Dean1 for CH4C2H6 + ḢCH3Ȯ2C2H5Ȯ2
CarstensenDeanDeutschmann2 for CH4 C2H6 C3H8 C4H10 + HȮ2 CH3Ȯ2 C2H5Ȯ2 C3H7Ȯ2 C3H7Ȯ2 HC(O)Ȯ2 CH3C(O)Ȯ2
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash157
24ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
25
Rate rules for large molecular weight molecules
bull High temperature mechanismReaction class 1 Unimolecular fuel decompositionReaction class 2 H atom abstractions from fuelReaction class 3 Alkyl radical decompositionReaction class 4 Alkyl radical + O2 = olefin + HȮ2
Reaction class 5 Alkyl radical isomerizationReaction class 6 H atom abstraction from olefinsReaction class 7 Addition of radical species to olefinsReaction class 8 Alkenyl radical decompositionReaction class 9 Olefin decomposition
26Slide Courtesy of Dr William Pitz
Reaction rate rules for higher MW species
27Slide Courtesy of Dr William Pitz
Reaction classes for low temperature reactionsLow temperature mechanismReaction class 10 Alkyl radical addition to O2 (R + O2)Reaction class 11 R + RrsquoO2 = RȮ + RrsquoȮReaction class 12 Alkylperoxy radical isomerizationReaction class 13 RȮ2 + HȮ2 = ROOH + O2Reaction class 14 RȮ2 + H2O2 = ROOH + HȮ2Reaction class 15 RȮ2 + CH3Ȯ2 = RȮ + CH3Ȯ +O2Reaction class 16 RȮ2 + RrsquoȮ2 = RȮ + RrsquoȮ + O2Reaction class 17 ROOH = RȮ + ȮHReaction class 18 RȮ DecompositionReaction class 19 QOOH = Cyclic Ether + ȮHReaction class 20 QOOH = Olefin + HȮ2Reaction class 21 QOOH = Olefin + Aldehyde or Carbonyl + ȮHReaction class 22 Addition of QOOH to molecular oxygen O2Reaction class 23 Ȯ2QOOH isomerization to carbonylhydroperoxide + ȮHReaction class 24 Carbonylhydroperoxide decompositionReaction class 25 Reactions of cyclic ethers with ȮH and HȮ2
28
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
21
Carstensen and Dean12 for CH4 C2H6 C3H8 C4H10 + HȮ2
Aguilera‐Iparraguirre et al3 CH4 C2H6 C3H8 nC4H10 iC4H10 + HȮ2
mdashAgree well with the determinations of Walker et al
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash1573J Aguilera‐Iparraguirre HJ Curran W Klopper JM Simmie J Phys Chem A 112 (2008) 7047ndash7054
Intermediate temperature chemistry RH + HȮ2 = R + H2O2
22ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
RH + CH3Ȯ2 = R + CH3O2H can also be important
HJ Curran P Gaffuri WJ Pitz CK WestbrookCombustion and Flame 129253ndash280 (2002)
iC8H18 oxidationφ = 10 in air p = 40 atm
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
23
RH + CH3Ȯ2 = R + CH3O2HĊH3 + O2 = CH3Ȯ2
RH + CH3Ȯ2 = R + CH3O2HCH3O2H = CH3Ȯ + ȮH
Carstensen and Dean1 for CH4C2H6 + ḢCH3Ȯ2C2H5Ȯ2
CarstensenDeanDeutschmann2 for CH4 C2H6 C3H8 C4H10 + HȮ2 CH3Ȯ2 C2H5Ȯ2 C3H7Ȯ2 C3H7Ȯ2 HC(O)Ȯ2 CH3C(O)Ȯ2
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash157
24ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
25
Rate rules for large molecular weight molecules
bull High temperature mechanismReaction class 1 Unimolecular fuel decompositionReaction class 2 H atom abstractions from fuelReaction class 3 Alkyl radical decompositionReaction class 4 Alkyl radical + O2 = olefin + HȮ2
Reaction class 5 Alkyl radical isomerizationReaction class 6 H atom abstraction from olefinsReaction class 7 Addition of radical species to olefinsReaction class 8 Alkenyl radical decompositionReaction class 9 Olefin decomposition
26Slide Courtesy of Dr William Pitz
Reaction rate rules for higher MW species
27Slide Courtesy of Dr William Pitz
Reaction classes for low temperature reactionsLow temperature mechanismReaction class 10 Alkyl radical addition to O2 (R + O2)Reaction class 11 R + RrsquoO2 = RȮ + RrsquoȮReaction class 12 Alkylperoxy radical isomerizationReaction class 13 RȮ2 + HȮ2 = ROOH + O2Reaction class 14 RȮ2 + H2O2 = ROOH + HȮ2Reaction class 15 RȮ2 + CH3Ȯ2 = RȮ + CH3Ȯ +O2Reaction class 16 RȮ2 + RrsquoȮ2 = RȮ + RrsquoȮ + O2Reaction class 17 ROOH = RȮ + ȮHReaction class 18 RȮ DecompositionReaction class 19 QOOH = Cyclic Ether + ȮHReaction class 20 QOOH = Olefin + HȮ2Reaction class 21 QOOH = Olefin + Aldehyde or Carbonyl + ȮHReaction class 22 Addition of QOOH to molecular oxygen O2Reaction class 23 Ȯ2QOOH isomerization to carbonylhydroperoxide + ȮHReaction class 24 Carbonylhydroperoxide decompositionReaction class 25 Reactions of cyclic ethers with ȮH and HȮ2
28
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
22ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
RH + CH3Ȯ2 = R + CH3O2H can also be important
HJ Curran P Gaffuri WJ Pitz CK WestbrookCombustion and Flame 129253ndash280 (2002)
iC8H18 oxidationφ = 10 in air p = 40 atm
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
23
RH + CH3Ȯ2 = R + CH3O2HĊH3 + O2 = CH3Ȯ2
RH + CH3Ȯ2 = R + CH3O2HCH3O2H = CH3Ȯ + ȮH
Carstensen and Dean1 for CH4C2H6 + ḢCH3Ȯ2C2H5Ȯ2
CarstensenDeanDeutschmann2 for CH4 C2H6 C3H8 C4H10 + HȮ2 CH3Ȯ2 C2H5Ȯ2 C3H7Ȯ2 C3H7Ȯ2 HC(O)Ȯ2 CH3C(O)Ȯ2
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash157
24ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
25
Rate rules for large molecular weight molecules
bull High temperature mechanismReaction class 1 Unimolecular fuel decompositionReaction class 2 H atom abstractions from fuelReaction class 3 Alkyl radical decompositionReaction class 4 Alkyl radical + O2 = olefin + HȮ2
Reaction class 5 Alkyl radical isomerizationReaction class 6 H atom abstraction from olefinsReaction class 7 Addition of radical species to olefinsReaction class 8 Alkenyl radical decompositionReaction class 9 Olefin decomposition
26Slide Courtesy of Dr William Pitz
Reaction rate rules for higher MW species
27Slide Courtesy of Dr William Pitz
Reaction classes for low temperature reactionsLow temperature mechanismReaction class 10 Alkyl radical addition to O2 (R + O2)Reaction class 11 R + RrsquoO2 = RȮ + RrsquoȮReaction class 12 Alkylperoxy radical isomerizationReaction class 13 RȮ2 + HȮ2 = ROOH + O2Reaction class 14 RȮ2 + H2O2 = ROOH + HȮ2Reaction class 15 RȮ2 + CH3Ȯ2 = RȮ + CH3Ȯ +O2Reaction class 16 RȮ2 + RrsquoȮ2 = RȮ + RrsquoȮ + O2Reaction class 17 ROOH = RȮ + ȮHReaction class 18 RȮ DecompositionReaction class 19 QOOH = Cyclic Ether + ȮHReaction class 20 QOOH = Olefin + HȮ2Reaction class 21 QOOH = Olefin + Aldehyde or Carbonyl + ȮHReaction class 22 Addition of QOOH to molecular oxygen O2Reaction class 23 Ȯ2QOOH isomerization to carbonylhydroperoxide + ȮHReaction class 24 Carbonylhydroperoxide decompositionReaction class 25 Reactions of cyclic ethers with ȮH and HȮ2
28
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
23
RH + CH3Ȯ2 = R + CH3O2HĊH3 + O2 = CH3Ȯ2
RH + CH3Ȯ2 = R + CH3O2HCH3O2H = CH3Ȯ + ȮH
Carstensen and Dean1 for CH4C2H6 + ḢCH3Ȯ2C2H5Ȯ2
CarstensenDeanDeutschmann2 for CH4 C2H6 C3H8 C4H10 + HȮ2 CH3Ȯ2 C2H5Ȯ2 C3H7Ȯ2 C3H7Ȯ2 HC(O)Ȯ2 CH3C(O)Ȯ2
1H‐H Carstensen AM Dean Proc Combust Inst 30 (2005) 995ndash10032H‐H Carstensen AM Dean O Deutschmann Proc Combust Inst 31 (2007) 149ndash157
24ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
25
Rate rules for large molecular weight molecules
bull High temperature mechanismReaction class 1 Unimolecular fuel decompositionReaction class 2 H atom abstractions from fuelReaction class 3 Alkyl radical decompositionReaction class 4 Alkyl radical + O2 = olefin + HȮ2
Reaction class 5 Alkyl radical isomerizationReaction class 6 H atom abstraction from olefinsReaction class 7 Addition of radical species to olefinsReaction class 8 Alkenyl radical decompositionReaction class 9 Olefin decomposition
26Slide Courtesy of Dr William Pitz
Reaction rate rules for higher MW species
27Slide Courtesy of Dr William Pitz
Reaction classes for low temperature reactionsLow temperature mechanismReaction class 10 Alkyl radical addition to O2 (R + O2)Reaction class 11 R + RrsquoO2 = RȮ + RrsquoȮReaction class 12 Alkylperoxy radical isomerizationReaction class 13 RȮ2 + HȮ2 = ROOH + O2Reaction class 14 RȮ2 + H2O2 = ROOH + HȮ2Reaction class 15 RȮ2 + CH3Ȯ2 = RȮ + CH3Ȯ +O2Reaction class 16 RȮ2 + RrsquoȮ2 = RȮ + RrsquoȮ + O2Reaction class 17 ROOH = RȮ + ȮHReaction class 18 RȮ DecompositionReaction class 19 QOOH = Cyclic Ether + ȮHReaction class 20 QOOH = Olefin + HȮ2Reaction class 21 QOOH = Olefin + Aldehyde or Carbonyl + ȮHReaction class 22 Addition of QOOH to molecular oxygen O2Reaction class 23 Ȯ2QOOH isomerization to carbonylhydroperoxide + ȮHReaction class 24 Carbonylhydroperoxide decompositionReaction class 25 Reactions of cyclic ethers with ȮH and HȮ2
28
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
24ldquoDeveloping detailed chemical kinetic mechanisms for fuel combustionrdquo
nC5H12 in air p = 20 atm
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
Three distinct temperature regimes
6 8 10 12 141E-3
001
01
1
10 = 05 = 10 = 20
Igni
tion
dela
y tim
e (m
s)
10000 K T
1667 1250 1000 833 714Temperature (K)
Low TR + O2rarr RȮ2 QOOH QOOH + O2rarrȮ2QOOH RȮ + ȮH + ȮH
25
Rate rules for large molecular weight molecules
bull High temperature mechanismReaction class 1 Unimolecular fuel decompositionReaction class 2 H atom abstractions from fuelReaction class 3 Alkyl radical decompositionReaction class 4 Alkyl radical + O2 = olefin + HȮ2
Reaction class 5 Alkyl radical isomerizationReaction class 6 H atom abstraction from olefinsReaction class 7 Addition of radical species to olefinsReaction class 8 Alkenyl radical decompositionReaction class 9 Olefin decomposition
26Slide Courtesy of Dr William Pitz
Reaction rate rules for higher MW species
27Slide Courtesy of Dr William Pitz
Reaction classes for low temperature reactionsLow temperature mechanismReaction class 10 Alkyl radical addition to O2 (R + O2)Reaction class 11 R + RrsquoO2 = RȮ + RrsquoȮReaction class 12 Alkylperoxy radical isomerizationReaction class 13 RȮ2 + HȮ2 = ROOH + O2Reaction class 14 RȮ2 + H2O2 = ROOH + HȮ2Reaction class 15 RȮ2 + CH3Ȯ2 = RȮ + CH3Ȯ +O2Reaction class 16 RȮ2 + RrsquoȮ2 = RȮ + RrsquoȮ + O2Reaction class 17 ROOH = RȮ + ȮHReaction class 18 RȮ DecompositionReaction class 19 QOOH = Cyclic Ether + ȮHReaction class 20 QOOH = Olefin + HȮ2Reaction class 21 QOOH = Olefin + Aldehyde or Carbonyl + ȮHReaction class 22 Addition of QOOH to molecular oxygen O2Reaction class 23 Ȯ2QOOH isomerization to carbonylhydroperoxide + ȮHReaction class 24 Carbonylhydroperoxide decompositionReaction class 25 Reactions of cyclic ethers with ȮH and HȮ2
28
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
25
Rate rules for large molecular weight molecules
bull High temperature mechanismReaction class 1 Unimolecular fuel decompositionReaction class 2 H atom abstractions from fuelReaction class 3 Alkyl radical decompositionReaction class 4 Alkyl radical + O2 = olefin + HȮ2
Reaction class 5 Alkyl radical isomerizationReaction class 6 H atom abstraction from olefinsReaction class 7 Addition of radical species to olefinsReaction class 8 Alkenyl radical decompositionReaction class 9 Olefin decomposition
26Slide Courtesy of Dr William Pitz
Reaction rate rules for higher MW species
27Slide Courtesy of Dr William Pitz
Reaction classes for low temperature reactionsLow temperature mechanismReaction class 10 Alkyl radical addition to O2 (R + O2)Reaction class 11 R + RrsquoO2 = RȮ + RrsquoȮReaction class 12 Alkylperoxy radical isomerizationReaction class 13 RȮ2 + HȮ2 = ROOH + O2Reaction class 14 RȮ2 + H2O2 = ROOH + HȮ2Reaction class 15 RȮ2 + CH3Ȯ2 = RȮ + CH3Ȯ +O2Reaction class 16 RȮ2 + RrsquoȮ2 = RȮ + RrsquoȮ + O2Reaction class 17 ROOH = RȮ + ȮHReaction class 18 RȮ DecompositionReaction class 19 QOOH = Cyclic Ether + ȮHReaction class 20 QOOH = Olefin + HȮ2Reaction class 21 QOOH = Olefin + Aldehyde or Carbonyl + ȮHReaction class 22 Addition of QOOH to molecular oxygen O2Reaction class 23 Ȯ2QOOH isomerization to carbonylhydroperoxide + ȮHReaction class 24 Carbonylhydroperoxide decompositionReaction class 25 Reactions of cyclic ethers with ȮH and HȮ2
28
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
bull High temperature mechanismReaction class 1 Unimolecular fuel decompositionReaction class 2 H atom abstractions from fuelReaction class 3 Alkyl radical decompositionReaction class 4 Alkyl radical + O2 = olefin + HȮ2
Reaction class 5 Alkyl radical isomerizationReaction class 6 H atom abstraction from olefinsReaction class 7 Addition of radical species to olefinsReaction class 8 Alkenyl radical decompositionReaction class 9 Olefin decomposition
26Slide Courtesy of Dr William Pitz
Reaction rate rules for higher MW species
27Slide Courtesy of Dr William Pitz
Reaction classes for low temperature reactionsLow temperature mechanismReaction class 10 Alkyl radical addition to O2 (R + O2)Reaction class 11 R + RrsquoO2 = RȮ + RrsquoȮReaction class 12 Alkylperoxy radical isomerizationReaction class 13 RȮ2 + HȮ2 = ROOH + O2Reaction class 14 RȮ2 + H2O2 = ROOH + HȮ2Reaction class 15 RȮ2 + CH3Ȯ2 = RȮ + CH3Ȯ +O2Reaction class 16 RȮ2 + RrsquoȮ2 = RȮ + RrsquoȮ + O2Reaction class 17 ROOH = RȮ + ȮHReaction class 18 RȮ DecompositionReaction class 19 QOOH = Cyclic Ether + ȮHReaction class 20 QOOH = Olefin + HȮ2Reaction class 21 QOOH = Olefin + Aldehyde or Carbonyl + ȮHReaction class 22 Addition of QOOH to molecular oxygen O2Reaction class 23 Ȯ2QOOH isomerization to carbonylhydroperoxide + ȮHReaction class 24 Carbonylhydroperoxide decompositionReaction class 25 Reactions of cyclic ethers with ȮH and HȮ2
28
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
27Slide Courtesy of Dr William Pitz
Reaction classes for low temperature reactionsLow temperature mechanismReaction class 10 Alkyl radical addition to O2 (R + O2)Reaction class 11 R + RrsquoO2 = RȮ + RrsquoȮReaction class 12 Alkylperoxy radical isomerizationReaction class 13 RȮ2 + HȮ2 = ROOH + O2Reaction class 14 RȮ2 + H2O2 = ROOH + HȮ2Reaction class 15 RȮ2 + CH3Ȯ2 = RȮ + CH3Ȯ +O2Reaction class 16 RȮ2 + RrsquoȮ2 = RȮ + RrsquoȮ + O2Reaction class 17 ROOH = RȮ + ȮHReaction class 18 RȮ DecompositionReaction class 19 QOOH = Cyclic Ether + ȮHReaction class 20 QOOH = Olefin + HȮ2Reaction class 21 QOOH = Olefin + Aldehyde or Carbonyl + ȮHReaction class 22 Addition of QOOH to molecular oxygen O2Reaction class 23 Ȯ2QOOH isomerization to carbonylhydroperoxide + ȮHReaction class 24 Carbonylhydroperoxide decompositionReaction class 25 Reactions of cyclic ethers with ȮH and HȮ2
28
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
28
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
29
Class 12
RȮ2 QOOH isomerization reactions
6-membered ring isomerization k6 = 25times1010 exp(ndash20450RT)
5-membered ring isomerization k5 = 20times1011 exp(ndash26450RT)
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
30
primarytertiary
5-member TS 6-member TS
tertiaryprimary
RO
OH
O
OHR
secondary
Class 12
Activation energy depends on ring size and overall thermochemistryAmenable to rule generation
S M Villano L K Huynh H ndashH Carstensen A M DeanJ Phys Chem A 2011 115 13425ndash13442
Correlations between structure and reactivity
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
31
Pentane isomers
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
32
n‐Pentane
(RON = 617)
iso‐Pentane
neo‐Pentane
Success of reaction rate rules eg pentane isomers
J Bugler et al Combust Flame 163(1) (2016) 138ndash156
(RON = 923)
(RON = 855)
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air p = 10 bar
Temperature (K)
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
33
Rate rules applied to larger alkanes
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
34
Expanded for other classes eg Alcohols
Alcohols are less reactive than their corresponding alkanemdash n‐pentanol (RON = 80) slower to ignite compared to pentane (RON = 617)mdash Carbon alpha to ndashOH alcohol functional group is weakest mdash Da Silva et al1 showed concerted elimination reaction Ea = 114 kcal molndash1
1G da Silva JW Bozzelli L Liang JT Farrell J Phys Chem A 113 (2009) 8923ndash8933
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
35
Software for automatic mechanism development Semi‐detailed mechanisms using automatic reaction generator
MAMOX code (Ranzi and Faravelli 1995mdash1997)
Computer‐aided automatic generation for large aliphatic HC moleculesmdash Chevalier et al 1990 (did not include reaction rate details)mdash REACTION (Morley and Blurock 1993mdash1995)
Enhanced by Moreacuteac ndash generated nC7H16 nC10H22
mdash EXGAS ndash Battin‐Leclerc et al (2005) (initial work by Haux et al 1985mdash1988)
Comprehensive C0ndashC2 base with lumped secondary mechanism from KINGAS Thermodynamic parameters from THERGAS
mdash Genesys12 ndash Van Geem 2012mdash2015 (Ghent University) mdash Reaction Mechanism Generator (RMG) ndash Green and West (MITNorthwestern)
Mechanisms include elementary reaction steps Include species identifiers
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
8 10 12 14
01
1
10
100 = 10 RCM = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1200 1000 800
Temperature (K)
Neopentane oxidation in air at 10 atm
36
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
7 8 9
01
1
10 = 10 ST
Igni
tion
Del
ay T
ime
(ms)
104 T (K-1)
1400 1300 1200 1100
Temperature (K)
Neopentane oxidation in air at 10 atm
37
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
10 12 141
10
100
= 10 RCMIg
nitio
n D
elay
Tim
e (m
s)
104 T (K-1)
1000 900 800 700
Temperature (K)Neopentane oxidation in air at 10 atm
38
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Neopentane oxidation in an engine
39
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
40
Neopentane oxidation in an engine
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Model vs Experiments
n‐Pentane
iso‐Pentane
neo‐Pentane
41
7 8 9 10 11 12 13 14
01
1
10
100
104 T (K-1)
Igni
tion
Del
ay T
ime
(ms)
1400 1200 1000 800
= 05 in air
Temperature (K)
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
High Temperature Mechanism
(Eapp 30000 calmol)
Intermediate Temperature Mechanism
(Eapp 19000 calmol)
+ O2
OHbull + Cyclic Ethers
OHbull + bullRCHO + CnH2n
HO2bull + nC7H14
‐Decomposition Products
NTC
conv
ersi
on
Reactor Temperature
nC7H16
nC7H15
+ O2
R7OO
Q7OOH
+ O2
OOQ7OOH
DegenerateBranching Path
OQ7OOH + OHbull
Oxidation of alkanes
Courtesy of Prof Tiziano Faravelli Politecnico di Milano42
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Mechanism competitionTransition from the LT to the HT mechanism ruled by the decomposition of peroxy radicals
kadd= 109 [Lmols]kdec= 1013 exp (-28000RT) [1s]R + O2 ROO
Competitive pathways at high temperatures alkyl radicals are favored over the peroxy radicals or pyrolysis is favored over oxidation
Ceiling Temperature is the transition temperature from one mechanism to the other
At equilibrium the addition (forward) and the decomposition (reverse) reaction rates are equal
radd = rdec kadd [R][O2]=kdec [ROO]
Courtesy of Prof Tiziano Faravelli Politecnico di Milano43
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
R + O2 RO2
Ceiling temperature vs pressure
2
13
9
2800010 exp( )
10O
RT RTPx
2
13
92
2800010 exp( )
10dec
addO
R k RTPROO k O x
RT
001
01
1
10
100
1000
800 900 1000 1100 1200 1300Tceiling
p
Ceiling temperature increases with pressure higher oxygen concentration favors direct reaction of peroxy radical formation NTC region moves toward higher temperatures
Courtesy of Prof Tiziano Faravelli Politecnico di Milano44
R + O2 RO2
p in atm R = 00821 L atm K‐1 mol‐1
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
nC7H16
R7
R7OO
+O2
+
Kinetic Modelling of Hydrocarbon Pyrolysis and Oxidation
Tceiling
10E+02
10E+03
10E+04
08 09 10 11 12 13 14 15
Ignitio
n Delay Tim
e (s)
1000T [1K]
n‐heptaneair φ=10
45 atm
13 atm
Pelucchi et al Energy amp Fuels 2014Ciezki et al Combustion and Flame 1993
Ceiling temperature vs pressure
Bugler et al Journal of Physical Chemistry A 2015
Goldsmith et al Journal of Physical Chemistry A 2012
45Courtesy of Dr Matteo Pelucchi Politecnico di Milano
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Example data n‐Heptane
φ = 10 τ = 20 s 106 bar 05 fuelHerbinet et al Combust Flame 159 (2012) 3455-3471
46
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Hydrogen ignition delay times
47
Simulated using mechanism fromJ Li Z Zhao A Kazakov FL Dryer Int J Chem Kinet 36 (2004) 566ndash575
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
65 70 75 80
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s
10000 K T
ndash Butanol isomers (STRCM) (Dr Kenji Yasunaga Ministry of Defense)
bull T = 1150-1750 K p = 35 atm
K Yasunaga T Mikajiri SM Sarathy T Koike F Gillespie T Nagy JM Simmie H J Curran ldquoA Shock Tube and Chemical Kinetic Modeling Study of the Pyrolysis and Oxidation of Butanolsrdquo Combust Flame 159(6) (2012) 2009ndash2027
sec‐Butanol p = 35 atm iso‐Butanol p = 35 atm
60 65 70 75 80 85
100
1000 = 20 3 O2
= 10 6 O2
= 05 12 O2
Igni
tion
dela
y tim
e
s10000 K T
Lean Mixtures faster at High TLow p
48
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
75 80 85 90 95 100 105
100
1000
= 05 = 10 = 20
Igni
tion
dela
y tim
e
s
10000 K T
Rich Mixtures faster at Low THigh p
T Tsujimura W J Pitz F Gillespie H J Curran B W Weber Y Zhang C‐J Sung Development of isopentanol reaction mechanism reproducing autoignition character at high and low temperatures Energy Fuels 26(8) (2012) 4871ndash4886
iso‐Pentanol p = 21 barDr Taku TsujimuraAdvanced Industrial Science Technology
49
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
NG Effect of Equivalence Ratio
06 07 08 09 10 11 12 13 14
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s
1000 K T07 08 09 10 11 12 13 14
001
01
1
10
100
RCM = 05 STD = 05 RCM = 10 RCM = 20 STD = 20
Igni
tion
dela
y tim
e m
s1000 K T
625 CH4200 C2H6100 C3H850 nC4H1025 nC5H12
8125 CH4100 C2H650 C3H8
25 nC4H10125 nC5H12
p = 20 atm
50
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
75 80 85 90 95 100
100
Igni
tion
dela
y tim
e
s
104 K T
=03 =05 =10 =20
n‐PB Effect of Equivalence Ration‐Propylbenzene at 30 atm
51
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Ignition of C3H8O2 in closed adiabatic system
- One or two stage ignition
‐ NTC between 650‐700 K
600
650
700
750
800
850
900
950
1000
time
Tempe
rature (K
)
No heat exchangeNo mass exchange
Courtesy of Prof Tiziano Faravelli Politecnico di Milano52
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
NTC Behavior
07 08 09 10 11 12 13 14
001
01
1
10
100
Wales 20 atm Wales 40 atm NUIGRCM 30 atm Duisberg 30 atm in Ar Duisberg 30 atm in N2
TAMU 30 atm Model prediction
Igni
tion
Del
ay ti
me
(ms)
1000 K T
1400 1300 1200 1100 1000 900 800 70021 C3H8 = 05
53
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
High p low T iC8H18 = 10 in air p = 40 atm
Reduced reactivity
54
H + O2 + (M) = HO2 + (M)H + O2 = O + OH
CH3 + HO2 = CH3O + OHCH3 + HO2 = CH4 + O2
RO2 = QOOHQOOH = CYCLIC ETHER + OH
FUEL + OH = XC8H17 + H2OH2O2 + (M) = OH + OH + (M)
RO2 =gt QOOHQOOH + O2 =gt O2QOOH
O2QOOH = KET + OHFUEL+CH3O2 =XC8H17+CH3O2H
R + O2 =gt RO2FUEL + RO2 = XC8H17 + RO2HFUEL + HO2 = XC8H17 + H2O2
HO2 + HO2 = H2O2 + O2R = BETA-SCISSION
-30 -20 -10 0 10 20 30 40 50 60 70
Sensitivity
725 K 825 K 1000 K
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Assign reaction rate rules by reaction classes
bull High temperature mechanismbull Reaction class 1 Unimolecular fuel decompositionbull Reaction class 2 H atom abstractions from fuelbull Reaction class 3 Alkyl radical decompositionbull Reaction class 4 Alkyl radical + O2 = olefin + HȮ2bull Reaction class 5 Alkyl radical isomerizationbull Reaction class 6 H atom abstraction from olefinsbull Reaction class 7 Addition of radical species to olefinsbull Reaction class 8 Alkenyl radical decompositionbull Reaction class 9 Olefin decomposition
55
Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Test molecule 4‐methyl heptane
Bond dissociation energies
Primary ~ 1015 kcalmol Secondary ~ 985 kcalmol Tertiary ~ 960 kcalmol
56
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
1 Unimolecular fuel decomposition
Very important for ignition delay times in a STndash High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
Usually need to account for fall‐off in rate constant
57
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
High p limit usually estimated in the reverse (exothermic) direction radical‐radical recombination with no Ea
58
1 Unimolecular fuel decomposition
k = 1014 cm3 mol-1 s-1
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
59
1 Unimolecular fuel decomposition
Very high activation energies are required (85‐95 kcalmol for CmdashC bond scission)
There are many unique bond scissions available in 4‐methylheptane
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
The geometric mean rule relates the selfcombination rate coefficients of two radicalsand their cross combination rate coefficient
kAB = 2(kAAkBB)05
Where kAB is the rate coefficient for the cross reaction and kAA and kBB are the rate coefficients for the self reactions
60
Klippenstein et al Phys Chem Chem Phys 2006 8 1133‐1147
1 Unimolecular fuel decomposition
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
2 H‐atom abstraction from fuel Abstraction of H atoms from the fuel by radical species (eg Ḣ ȮH HȮ2
ĊH3 etc) H atoms can be abstracted from primary (1o) secondary (2o) or tertiary
(3o) carbon sites The rate constant depends on the radical species and the type of H atom
being abstracted Primary H atoms have the strongest bond CmdashH energies are the most difficult to abstract while tertiary H atoms are the weakest and most easily abstracted
61
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Reaction rate rules make the assignment of reaction rate constants manageable
C-H type A (cm3 mol-1 s-1) n EA (cal)
1 222E+05 254 6756
Ḣ 2 650e+05 240 4471
3 602E+05 240 2583
1 176E+09 097 1586
ȮH 2 234E+07 161 -35
3 573E+10 051 63
1 151E-01 365 7154
ĊH3 2 755E-01 346 5481
3 601E-10 636 893
1 680E+00 359 17160
HȮ2 2 316E+01 337 13720
3 650E+02 301 12090
H‐ atom abstraction rate rules for alkanes
Fuel + (Ḣ ȮH ĊH3 HȮ2) =gt fuel radical + (H2 H2O CH4 H2O2) Class 2
62Courtesy of Dr William Pitz Lawrence Livermore National Laboratory
Orme et al J Phys Chem A 2006
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Ea in kJ mol-1
Allylic H Vinylic H
Primary Secondary Tertiary Secondary Tertiary
lgA b E lgA b E lgA b E lgA b E lgA b E
Radical
108 07 25 106 07 13 105 07 5 107 07 36 108 07 32bullObull
48 25 10 44 25 -7 44 25 -12 56 25 51 56 25 41bullH
60 2 -1 62 2 -6 61 2 -11 60 2 12 60 2 6bullOH
-13 35 24 119 0 29 119 0 22 -17 35 54 -17 35 50bullCH3
35 26 58 35 26 52 42 26 45bullHO2
H‐abstractions RH + X R + HX
H
H
C C C CH
H
H
H
H H
There are more complex correlations of incremental type depending on the nature of RH and X (Atkinson 1986 Ranzi et al 1994)
Courtesy of Dr Pierre-Alexandre Glaude63
Correlations between structure and reactivity
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
ȮH and Ḣ are the most reactive
Ouml radical is also very reactive but usually is in small concentration
HȮ2 is notably less reactive but leads to H2O2 which decomposes into two ȮH radicals
64
2 H‐atom abstraction from fuel
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
65
2 H‐atom abstraction by ȮH radials
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
2 H‐atom abstraction by ȮH radials Finer considerations take into account next‐nearest‐neighbour (NNN)
configurations and different types of H atoms
66
Sivaramakrishnan et al J Phys Chem A 2009 113(17) 5047‐5060
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Uncertainty in fuel + HȮ2 rate
67
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Need more accurate rates constants for HȮ2 + alkanesUncertainty in rate of a factor of 3 ‐ 6
NUIG
CSM
C3H8+HȮ2 lt=gt iĊ3H7 + H2O2
Ignition very sensitive to this rate constant under RCM
conditions
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Uncertainty in fuel + HȮ2 rateEffect on shock tube ignition delay time
69
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Evans‐Polanyi type correlations Empirical relationships linking the activation energy to the internal energy of the reaction (chemical driving force) and to an intrinsic energy barrier E0 (chemical inertia)
LFER relationships
DaggerG = DaggerG0 + arG0
Allow to calculate k (Hammet equation)
Evans‐Polanyi relationships
Ea = DaggerH0 + a rH0
Valid for reactions going through the same reaction channel (similar structures of the TSs) Hazardous extrapolations
Courtesy of Dr Pierre-Alexandre Glaude70
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Correlation for H‐abstractions on a C‐atom or a N‐atom (Dean and Bozzelli 1999)
k = nH A Tn exp (ndashE0 ndashf(H0 ndashH)RT) cm3 mol‐1 s‐1nH number of equivalent abstractable H‐atoms
RH + X R + HX
Formation of a radical center on C‐atom reference ethane
O
O
CH2
H
H
HH
CH2H
978 990
857943
926
839
987
8721002
8261009 699Importance of thermo data and BDE
Courtesy of Dr Pierre-Alexandre Glaude71
Evans‐Polanyi type correlations
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
3 Alkyl radical decomposition Alkyl radicals undergo ‐scission of C C and C H bonds to form a radical and an alkene
Bond once removed (ie ) from the radical site breaks to form a stable molecule and radical
‐scissions of C H bonds are negligible compared to C C bond scission at T≲ 2000 K
How many ‐scissions are possible
72
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Correlation for the decomposition of alkyl free radicals by ‐scissiondetermined from the theoretical calculation (CBS‐QB3 level of theory) of a series of reference reactions (Sirjean 2007)
Ea = 060 rH0 + 143 kcalmolR Rrsquo + alkene
R H + alkene
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
bullC3H7 rarr bullCH3 + C2H4 228 289bullC4H9 rarr bullC2H5 + C2H4 220 278bullC5H11 rarr bullC3H7 + C2H4 228 282bullC6H13 rarr bullC4H9 + C2H4 227 280bullC7H15 rarr bullC5H11 + C2H4 227 280
1-hexen-6-ylerarr1-buten-4-yle+C2H4 228 2781-hexen-3-ylerarr13-butadiene+bullC2H5 157 250
Reactions ΔrHdeg(kcalmol)
Ea(kcalmol)
1-penten-5-ylerarrbullC3H5+C2H4 74 192bullC3H7 rarr C3H6 + H 320 340bullC4H9 rarr C4H8 + H 326 344
bullC5H11 rarr C5H10 + H 325 344bullC6H13 rarr C6H12 + H 324 344bullC7H15 rarr C7H14+ H 324 342
Reactions of acyclic radicals used to built the correlation
Courtesy of Dr Pierre-Alexandre Glaude73
Evans‐Polanyi type correlations
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
‐scission alkyl free radicals Correlation adapted to a large number of -scissions but not to some ring opening
60
50
40
30
20
10
0
Ea
(kca
lmol
)
6040200-20-40rH (kcalmol)
-scissions of acyclic radicals (C-C and C-H bonds) -scissions C-H of cycloalkyl radicals -scissions of alkyl groups on the cycle exo ring opening (all cycles) endo ring opening of C3 endo ring opening of C4 endo ring opening of C5 endo ring opening of C6 endo ring opening of C7 Evans-Polanyi correlation
Ea = 060 (plusmn 002) rH + 143 (plusmn 06) (kcalmol-1)
(1)
(2)
(3)
Courtesy of Dr Pierre-Alexandre Glaude74
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Alkyl radical decomposition
H3C CH2 CH2 OH -H
H3C CH2 CH OH
H3C CH CH2 OH
H2C CH2 CH2 OH
H3C CH2 CH2 O
75
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
76
n‐Propanol ‐radical decomposition
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
ldquoEnols Are Common Intermediates in Hydrocarbon OxidationrdquoCraig A Taatjes et al Science 308 1887 (2005)
Photoionization mass spectrometry of flames
ndash Detected substantial quantities of 2 3 amp 4‐carbon enols
ndash Ethenol detected for allene propyne benzene cyclohexane 13‐butadiene ethanol propene cyclopentene ethene and 1‐propanol
ndash Ethenol below detection for ethane methane propane and 2‐propanol flames
77
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Alkyl radical decomposition
H
EFER
C2H5C2H4 + H
78
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
79
n‐Propanol ‐radical decomposition
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Alkyl radical decomposition
Reaction A‐factor Tn Ea (calmol)C2H4 + H = C2H5 170 1010 107 1450C3H6 + H = iC3H7 424 1011 051 1230C3H6 + H = nC3H7 250 1011 051 2620C2H4 + CH3 = nC3H7 176 104 248 6130C2H4 + C2H5 = nC4H9 132 104 248 6130C3H6 + CH3 = sC4H9 176 104 248 6130C3H6 + CH3 = iC4H9 189 103 267 6850
iC4H8 + CH3 = neoC5H11 130 103 248 8520
80
HJ Curran Int J Chem Kinet 28(4) (2006) 250‐275
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Hydrogen addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 065 131 145
CH2=CH(CH3) 081 123
CH2=CH(OH) 072
CH(CH3)=CH2 196 234 262
CH(OH)=CH2 351 368
81
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Methyl addition
ReactionHoDagger kcal molndash1 Ea kcal molndash1
CBS‐QB3 CBS‐APNO 2006 Study
CH2=CH2 614 638 613
CH2=CH(CH3) 590 624 613
CH2=CH(OH) 641 662
CH(CH3)=CH2 731 753 685
CH(OH)=CH2 870 891
82
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Ethyl addition
ReactionHoDagger kcal molndash1
CBS‐QB3 CBS‐APNOCH2=CH(OH) 628 633CH(OH)=CH2 774 786
83
JM Simmie HJ Curran J Phys Chem A (2009) 113(27) 7834ndash7845
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
84
CH3CH2CHOH = products
Reaction Ar nr EarCH3CH2CH=O + H 800 1012 000 9500CH2=CHOH + CH3 176 104 248 6130CH3CH=CHOH + H 250 1011 051 2620
Af nf EafA 703 1009 099 32590B 501 1010 104 30450C 546 1011 034 35630
H3C CH2 CH OH CH2 CH OH + CH3
+H3C CH2 CH O H
HH3C CH CH OH +
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
CH3CH2CHOH = products
05 06 07 08 09 10 11 12 13
103
104
105
106
107
108
109
1010
1011k
s-1
1000 K T
C2H
3OH + CH
3
C2H
5CHO + H
CH3CHCHOH + H
85
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
05 06 07 08 09 10 11 12 13
105
106
107
108
109
1010
k s
-1
1000 K T
C3H
6 + OH
C2H
3OH + CH
3
H2C CCH3
H + OH H3C CCH2
HOH
H2C CH
OH + CH3
iC3H6OH = products
86
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
3 Alkyl radical decomposition
87
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
4 Alkyl radical isomerization
88
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
4 Alkyl radical isomerization The rate constant for these reactions depends on the nature of the
broken C‐H bond (ie primary secondary or tertiary) and on the ring strain energy barrier
Isomerization reactions involving 5‐member 6‐member and 7‐member transition state ring are most important
Radical isomerizations involving fewer than five and greater than seven members are much slower
How many unique isomerizations are there
89
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
4 Alkyl radical isomerization
90
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Isomerization of free radicals activation energy
CH
CH3
R
CH2
R
HCH 2H
R
Ea = Ering + Eabstr
Eabstr Energy contribution of the internal H-abstraction
Ering Strain energy of the ring created in the TS
Atoms in the cyclic TS 4 5 6 7 8 9
Ering 26000 6300 1000 6400 9900 12800
Hp Hs Ht
Eabstr 13500 11000 9000Data for the isomerization of an
alkyl radical
91Courtesy of Dr Pierre-Alexandre Glaude
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
So where are we now
92
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
H atom abstraction from alkenes
93
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Allylic radical decomposition Allylic radicals either undergo ‐scission or react with HȮ2 radicals to
generate allyloxy and ȮH radicals Allyloxy radicals decompose via ‐scission to generate an aldehyde and
a vinylic radical
94
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
C = C double bonds reduce low T reactivity
s s a v v a s s‐ C ndash C ndash C ndash C = C ndash C ndash C ndash C ‐s s a a s s
Inserting one C=C double bonds changes the reactivity of 4 carbons atoms in the C chain
Allylic C ndash H bond sites are weaker than most others Therefore they are preferentially abstracted by radicals O2 is also very weakly bound at allylic sites and falls off rapidly
inhibiting low T reactivity
95
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Two double bonds make a huge difference
96
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Observed reactivity effect in hexene fuels
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
3-Hexene
2-Hexene
1-Hexene0
20
40
60
80
100
650 700 750 800 850 900T [K]
Igni
tion
dela
y tim
e [m
s]
Ignition delay times in a rapid compression machine of hexene isomers
(086‐109 MPa Φ=1)
C = C - C - C - C - C 1-hexene
C - C = C - C - C - C 2-hexene
C - C - C = C - C - C 3-hexene
RO2 isomerization initiates low temperature reactivity
Moving the double bond towards the center of the molecule ldquoinhibitsrdquo RO2 kinetics
Experimental data Vanhove et al PCI 2005Simulations Mehl Vanhove Pitz Ranzi Combustion and Flame 2008
97
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
Reaction Co‐ordinate Diagram
A + B
CE
D + F
reaction coordinate
energy
High pressure collisional stabilization dominates
C
DEF are lsquoProducts ofChemical Activationrsquo
98
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability
99
Outlook Kinetic mechanisms for ever larger fuel molecules are being
developed due to increasing computational ability
Lack of focus on accurate thermochemistry ATcT is a very good start but we need more than
Experimental measurements and accurate quantum chemistry calculations of important reactions involved in the C0ndashC4 system are vital for accurate predictions of ALL fuels
Rate rules are useful in building mechanisms for large molecular weight fuelsmdash ks for larger molecules can be calculated with increasing accuracy
due to increasing computational ability