chemistry. chemical thermodynamics-ii session objectives
TRANSCRIPT
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Chemistry
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Chemical thermodynamics-II
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Session Objectives
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Session objectives
1. Enthalpy
2. Various types of enthalpy of reactions
3. Heat capacities of gases
4. Adiabatic process
5. Hess’s law
6. Bond energy
7. Lattice energy
8. Limitation of first law of thermodynamics
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EnthalpyEnthalpy is the total heat contentsof the system at constant pressure. Enthalpy is shown by ‘H’.
H = E + PV
H2 – H1 = E2 – E1 + P(V2 – V1)
Where H1, E1 and V1 are the enthalpy, internal energy and volume respectively in initial state while H2, E2 and V2
are the enthalpy, internal energy and volume respectively in final state.
H = E + P V
Enthalpy change at constant pressure
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Enthalpy
Enthalpy is a state function
At constant pressurePV1 = n1RT (for initial state)
PV2 = n2RT (for final state)
P(V2 – V1) = RT(n2 – n1)
gP V = n RT
Where ng = np–nr (gaseous moles only)
gH = E + n RT
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Enthalpy of formation
It is the change in enthalpy when one mole of a compound is formed
from its elements in their naturally occuring physical states.
2 2 4 f2C(s) 2H (g) C H H 52kJ
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Enthalpy of combustion
4 2 2 2CH g 2O g CO g 2H O(g) ; H 890.3 kJ
2 6 2 2 2
1
2C H g 7O g 4CO g 6H O l
H 745.6K calmole
1745.6– 372.8 Kcal mol
2
It is the change in enthalpy when one mole of the substance undergoes complete combustion.
Heat of combustion
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Application of heat of combustion
Amount of heat produced per gram of a substance (food or fuel) is completely burnt.
Calorific value
4 2 2 2CH g 2O CO g 2H O l
Calorific value of CH4 (g) =– 890
– 55.6 kJ / g16
Hydrogen has the highest calorific value (150 kJ/g)
H = -890.3 kJ /mol
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Enthalpy of neutralization
Difference in energy is used to ionize weak base.
4 4 2weak basestrong acid
HCl aq NH OH aq NH Cl aq H O l
H – 12.3Kcal
2HCl (aq) + NaOH (aq) NaCl (aq) + H O
H = -13.7 Kcal
Strong acid and strong base
Ionization energy of NH4OH =
What is the Ionization energy of NH4OH?
13.7 12.3 1.4KCal.
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Enthalpy of solution
Amount of heat evolved or absorbed per mole of the substance in excess of water,
2
2
KCl s H O KCl aq H – 4.4 Kcal
KOH s H O KOH aq H – 13.3 Kcal
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Enthalpy of fusion
One mole of solid substance changes
to its liquid state at its melting point.
Melting2 2
Freezing2 2
H O s H O l H 1.44Kcal
H O l H O s H – 1.44 Kcal
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Enthalpy of vaporization
One mole of the substance changesfrom liquid state to gaseous state atits boiling point.
Boiling2 2
Cooling2 2
H O l H O g H 10.5 Kcal
H O g H O l H – 10.5 Kcal
Enthalpy change per mole of a solid converts directly to its vapours
Enthalpy of sublimation
sublimation4 4NH Cl (s) NH Cl g H 14.9 Kcal
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Heat capacity
Quantity of heat required to raise thetemperature of the system by one degree.
Heat capacity = dq
dT
Heat capacity at constant pressure
pp
HC
T
(Since at constant pressure dq = dH)
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Heat capacity
V
V
EC
T
(Since at constant volume dq = dE)
The difference between Cp and Cv is equal to the work done by 1 mole of gas in expansion when heated through 1° C.
Heat capacity at constant volume
p vC -C = R
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Heat capacity
Specific heat capacity is the heatrequired to raise the temperature ofunit mass by one degree.
q = c × m × T
m = Mass of the substance
q = Heat required
= Temperature difference
c = Specific heat capacity. Specific heat capacity of water is 4.18 J/g K.
T
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Adiabatic work
For adiabatic process, q = 0 it means no heat is exchanged with the surrounding.
v
v
E q w
i.e. E w q 0
For a finite change of an ideal gas,
E C . T
w E C T
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Reversible Adiabatic expansion
Relations for reversible adiabatic expansion of an ideal gas
1
1
v
2 1v
PV cons tant ...(i)
TV cons tant ...(ii)
T V cons tant ...(iii)
Now, considering this relation
Work done, W C T
R R(T T ) [ 1]
( 1) C
(For 1 mole of gas)
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Irreversible Adiabatic expansion
(i) For free expansion, w = 0. Since Pext = 0
(ii) For intermediate expansion,
ext 2 1
2 1ext
2 1
2 1v 2 1 ext
2 1
w P (V V )
T TP R
P P
T Ti.e. w C (T T ) R P
P P
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Hess’s Law
Cq1 q2
A Bq
According to Hess’s law
q = q1 + q2
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Applications of Hess’s law
Determination of heat changes of
transformation of rhombic sulphur
into monoclinic sulphur.Given
Subtracting (ii) from (i), we get
S (rhombic) – S (monoclinic)
H = +2.5 kJ
2 2
2 2
S (rhombic) + O (g) SO (g); H = - 297.5 kJ -----(i)
S (monoclinic) + O (g) SO (g); H = - 300.0 kJ -----(ii)
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Resonance energy
Resonance energy = Enthalpy of formation calculated from bond energy – Experimental value of enthalpy
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Question
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Illustrative example
Calculate resonance energy of benzene from the following data:
(i) benzene = –358.5 kJ mol–1
(ii) Heat of atomization of carbon is 716.8 kJ mol-1
(iii) Bond energies of C–H, C–C, C = C and H–H bonds are 490, 340, 620 and 436.9 kJ mol–1 respectively.
0fH
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Solution
The required equation is
2 6 66C(s) + 3H (g) C H , H = -358.5 kJ
Bond energies of reactants – Bond energies of products
fH =
= {6 [ HC(s) c(g)] + 3 ( HH–H) – 3{[ HC–C] + 3 ( HC =C) + 6 ( HC–H )
=6716.8 + (3 436.9) – (3 340) – (3620) – (6490) kJ mol–1
Resonance energy = Hf (obs.) – Hf (cal)
= – 358.5 – ( – 208.5)
= – 150.0 kJ mol–1
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Determination of lattice energy
sub diss X M X MXMX M 2
1H H ( H ) (IP) ( EA) ( U)
2
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Figure
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Determination of bond energies or bond enthalpiesEnergy required to break the bondor energy released during the bond formation is called bond energy.
2H S H g SH g H 100 kJ / mole
SH g S g H g H 200 kJ / mole
The average of these two bond dissociation energies gives the value of bond energy of S — H.
Bond energy of S — H bond100 200
150 kJ / mole2
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Limitations of first law
1. The first law of thermodynamics states that one form of energy disappears, an equivalent amount of another form of energy is produced. But it is salient about the extent to which such conversion can take place.
2. It does not tell about the direction of flow of heat.
3. It does not tell about spontaneity of reaction.
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Class exercise
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Class exercise 1
For the reaction
for the reaction will be
(a) – 781.80 Kcal (b) – 780.009 Kcal
(c) – 780.75 Kcal (d) 780.05 Kcal
= -780.9 Kcal, E
6 6 2 2 21
C H (l) 7 O (g) 6CO (g) 3H O(l)2
0, H(27 )
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SolutionH = E + nRT
15 3n 6 1.5
2 2
E = H - nRT
= –780.9 – (–1.5 RT)
1.5 1.987 300780.9
1000
= – 780.9 + 0.891
= – 780.009 Kcal
Hence, the answer is (b).
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Class exercise 2
When 1 gram of methane (CH4) burnsin O2 the heat evolved (measured under standard conditions) is 13.3 kcal. What is the heat of combustion?
(a) –13.3 k cals (b) +213 k cals
(c) – 213 k cals (d) – 416 k cals
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Solution
13.3 Kcal/gm evolved
ocombH 13.3 16 Kcal / mol
= – 213 Kcal/mol
Hence, the answer is (c).
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Class exercise 3
When 4.184 J of heat is transferred to 1 g of water at 20° C, its temperature rises to 21° C. The molar heat capacity at this temperature is
(a) 18 JK–1 (b)
(c) 75.4 JK–1 (d) 4.184 JK–1
18
4 1841
.JK
-
C = (4.184) × 18 = 75.4 J/K
n C T = 4.184
Hence, the answer is (c).
Solution:
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Class exercise 4
When 0.532 g of benzene (B.P 80° C) is burnt in a constant volume systemwith an excess of oxygen, 22.3 kJ of heat is given out. for the combustion process is given by
(a) – 21 kJ (b) – 1234.98 kJ
(c) – 221 kJ (d) – 3273.26 kJ
H
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Solution
6 6Mol. wt C HH 22.3
0.532
22.3 780.532
= – 3269.5 kJ
Hence, the answer is (d).
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Class exercise 5
Consider the reaction
2 2 31
SO (g) O (g) SO (g) H2
= – 98.3 kJ. If the enthalpy of formation of SO3(g) is – 395.4 kJ, then the enthalpy of formation of SO2(g) is
(a) 297.1 kJ (b) 493.7 kJ
(c) – 493.7 kJ(d) – 297.1 kJ
3 2
o of SO f SO
H H 98.3 kJ
2
of SO
H 98.3 395.4 kJ 297.1 kJ
Solution:
Hence, the answer is (d).
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Class exercise 6
Calculate the heat change for the following reaction:
4 2 2 2CH (g) + 2O (g) CO (g) + 2H O(l)
for CH4 , H2O and CO2 are –17.89, –68.3 and–94.05 kcal/mole.
0fH
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Solution
4 2 2 2CH g 2O g CO g 2H O l
2 2 4 2
o o o o oreaction f H O f CO f CH f OH 2 H H H 2 H
= – 2 × 68.3 – 94.05 + 17.89 – 0
= – 212.76 kcal/mol
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Class exercise 7
Calculate the heat of combustion of benzene from the following data:
2 6 66C (s) + 3H (g) C H (l)
2 2 21
H (g) + O (g) H O(l)2
2 2C(s) + O (g) CO (g)
H = 11720 cal
H = -68320 cal
H =-93050 cal
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Solution
The required reaction is
6 6 2 2 215
C H O 3H O 6CO (1)2
2 6 66C + 3H C H (2)
2 2C + O CO (3)
2 2 21
H O H O2
3 × (4) + 6 × (3) – (2) o o o o1 4 3 2H 3 H 6 H H
= 3(– 68320) + 6(– 93050) – (1720 Cal)
= – 774.980 kcal/mol
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Class exercise 8
Calculate for the following reaction at 27o C.
Given = – 337 kcal R= 1.987 cal deg–1 mole–1
2 4 2 2 2C H (g) + 3O (g) 2CO (g) + 2H O(l)
H
H
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Solution
H = E + PV
3=– 337 – (–2)(1.987)(300) × 10
E = H - nRT
= – 335.8078 kcal/mol
= E + nRT { n = -2}
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Class exercise 9
Calculate the heat of combustion of acetic acid at 25o C if the heat of formation of CH3COOH(l),CO2(g) and H2O(l) are –116.4, –94.0 and –68.3 kcal mole–1 respectively.
3 2 2 2CH COOH l 3O g 2CO g 2H O l
reactions f 2 f 2
f 3 f 2
H = 2 . H (CO ) + 2 . H (H O)
- H (CH COOH) - 3 H (O )
= 2(– 94.0) + 2(– 68.3) – (–116.4)
= – 208.2 Kcal/mol
Solution:
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Thank you