drill: calculate the volume of gas released at 227 o c under 83.1 kpa pressure when 320 kg of nh 4...
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Drill: Calculate the volume of gas released
at 227oC under 83.1 kPa pressure when 320 kg of
NH4NO3 is exploded forming N2, O2, & H2O:
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Thermo-chemistry
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AP Chm
Chapter 8
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Chm II
Chapter 15
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Thermochemistry
•The study of heat transfer in
chemical reactions
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Thermochemistry Topics
•Heat change
•Calorimetry
•Thermo-Chm-Eq
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Thermo-chemical
Terms
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Heat (H)•A form of energy
that can flow between samples of
matter
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Heat cannot be measured directly; thus, we measure heat change (H)
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Enthalpy•Another name for
heat
H
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Enthalpy Change•Heat that can flow
in/out of a system
H
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System•That part of nature upon which attention
is focused
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Surroundings•That part of nature
around the part upon which we are
focused
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Reaction Coordinate
•A graph of energy change versus time in a chemical reaction
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Time
Ene
rgy
RP
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Exothermic Rxn•Chemical reactions
that release, give off heat, or lose
heat
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Exothermic Rxn•Products will
contain less heat than the reactants
H < 0
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Endothermic Rxn
•Chemical reactions that absorb, take in heat, or gain heat
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Endothermic Rxn•Products will
contain more heat than the reactants
H > 0
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Topic: Heat
Change
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Specific Heat•The heat required to raise one gram of a substance 1oC
•C: (J/goC, J/kgoK)
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Specific Heat Formula
H = mCT
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Heat of Fusion•The heat required to melt one gram of a substance at its normal MP
•Hf: (J/g or J/kg)
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Heat of Fusion Formula
H = mHf
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Heat of Vaporization
•The heat required to boil one gram of a substance at its normal BP
•Hv: (J/g or J/kg)
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Heat of Vap. Formula
H = mHv
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AP CHM HW•Read: Chapter 8•Work problems:
5 & 17•Page: 234
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CHM II HW•Read: Chapter 9•Work problems:
•Page:
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Calculate the heat change when 10.0 g H2O goes from –100.0oC to 200oC.MP = 0oC BP = 100oCHf = 334 J/g HV = 2260 J/g
Cice = 2.06 J/gKCwater = 4.18 J/gK Csteam = 2.02 J/gK
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Drill: Calculate the heat required to change 25 g
of water from 140.0oC to 60.0oC
MP = 0oC BP = 100oCHf = 334 J/g HV = 2260 J/g
Cice = 2.06 J/gKCwater = 4.18 J/gK Csteam = 2.02 J/gK
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Topic: Calorimetry
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Calorimetry•A method to measure the
experimental heat transfer in a system
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Calorimeter•Device used to measure heat transfer
•A calorimeter is an adiabatic system
•Experimental yield
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Adiabatic System•A system that exchanges zero heat with its surroundings
Hsystem = 0
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H (J or kJ)H = q = the heat or enthalpy change in a system
Hsys = mcTsys parts
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CalorimetryHsystem = 0
Hsys = Hcal + Hrxn
Hrxn = -Hcal
Hrxn = -mcTcal
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When Q reacts in a 1.5 kg calorimeter containing 2.5 kg water the temp changes from
22.5oC to 26.5oC.Calculate Hrxn. Cwater = 4.18 J/gK Ccal = 2.00 J/gK
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Chm II HW
Problems: 64 & 65
Page: 641-641
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AP Chm HW
Problems: 8 & 9
Page: 234
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When X reacts in a 2.0 kg calorimeter containing 1.5 kg water, the temp changes
from 22.5oC to 30.5oC. Calculate Hrxn. Cwater = 4.18 J/gK Ccal = 1.50 J/gK
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When Z reacts in a 1.0 kg calorimeter containing 2.0 kg water, T = 22.5oC to 32.5oC. Calculate Hrxn.
Cwater = 4.18 J/gK Ccal = 2.00 J/gK
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Drill: When 40.0 g NH4NO3 dissolves in
460.0 g water at 25.0oC, the temp. falls to 22.5.oC.
Calculate the Hosoln for
NH4NO3. Csoln = 4.00 J/gK
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Topic: Thermochemical
Equation (TCE)
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Thermo-chemical Equation
Terms
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Heat of Reaction•The heat or enthalpy change of a chemical reaction
Hrxn
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Typical Reaction
•HCl + NaOH NaCl + HOH
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Heat of Solution
•The heat or enthalpy change when a substance is dissolved
Hsoln
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Typical Ionization
KCl
K+(aq) + Cl-
(aq)
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Heat of Combustion•The heat or enthalpy change when a substance is burned
Hcombustion
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Combustion Reaction
•CxHy + O2
CO2 + HOH
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Heat of Formation•The heat required to form one mole of a compound from pure elements
Hfo (kJ/mole)
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Rxn Making Cpds from ele
H2 + ½ O2 H2O
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The Degree Symbol•Indicates standard conditions & molar
quantities by itself or from a balanced
equation.
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AP Chm HW•Problem: 41
On page 236
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Chm II HW•Problem: 37
On page 638
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Gibb’s Free Energy•Energy of a system that can be converted to work
•Determines spontaneity
G
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Energy of Formation•The energy required to form one mole of a compound from pure elements
Gfo (kJ/mole)
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Exergonic Reaction•A reaction in which free energy is given off
G < 0
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Endergonic Reaction
•A reaction in which free energy is absorbed
G > 0
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Exergonic Reaction•A reaction which can be spontaneous
G < 0
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Endergonic Reaction
•A reaction which cannot be spontaneous
G > 0
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Reaction at Equilibrium
G = 0
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Interrelation Term (G)
G interrelates thermochemistry,
chemical equilibria,
& electrochemistry
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Entropy•A measure of disorder
So
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Entropy of Formation•The entropy of one mole of a substance
•Sfo (J/moleoK)
•Sfo (kJ/moleoK)
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Drill: Define:• Heat of reaction
• Heat of solution
• Heat of formation
• Energy of formation
• Entropy of formation
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Drill: Identify type of rxn when:
G > 0G < 0G = 0
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Thermochemical Equation
•An equation that shows changes in heat, energy, etc
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Thermochemical Equation
Ho
rxn Hf
o
productsHf
o
reactants
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Thermochemical Equation
Go
rxn Gf
o
productsGf
o
reactants
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Thermochemical Equation
So
rxnSf
o
products
Sfo
reactants
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Thermochemical Equation
•Stoichiometry of heat change
•Solves theoretical yield
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Interrelating Equation
GH
S
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Drill: Define:•Heat of Rxn
•Heat of Solution
•Heat of Combustion
•Heat of Formation
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In stoichoimetric calculations, the TCE
is used for molar conversions from
mole to heat or heat to moles
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Calculate H, G, & S when 13.6 g of CaSO4 is changed
into CaO + SO2 + O2 at 25oC
Cmpd CaSO4 SO2 CaO
Hf
o -1434.1 -296.8 -635.1
Gf
o -1321.8 -300.2 -604.0
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AP Homework•Problem: 41b
On page 236
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Chm II HW•Problem: 36
On page 638
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Calculate H, G, & S when 19.7 kg of BaCO3 is decomposed into BaO + CO2
Cmpd BaCO3 CO2 . BaO
Hf
o -1216.3 -393.5 -553.5
Gf
o -1137.6 -394.4 -525.1
Sf
o 112.1 213.6 70.4
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Drill: Calculate Ho
rxn for:A + B2C3 AC2 + B
Compd B2C3 AC2
Hfo(kJ/mole) -150 -250
Gfo(kJ/mole) -175 -225
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Calculate the potential H, G, & S for the reaction & Sf
o for
O2 when burning 8.8 kg of C3H8 Cpd C3H8 CO2 H2O
Hf
o-103.8 -393.5 -241.8
Gf
o- 23.5 -394.4 -228.6
Sf
o269.9 213.6 188.7
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AP CHM HW•Work problem 45 on page 236
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Lab Results: Cup H2O NaOH Thermo
5.0 g 50.0 g 4.0 g 15.0 g Ti = 22.0
oC Tf = 27.0
oC
Cmpd NaOH Na+ OH-
Hf
o -425.6 -240.1 -230.0
Determine: theoretical and experimental heat changes
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Drill: Calculate Ho, Go, & So when P + QR PR2 + QCompd QR PR2
Hfo(kJ/mole) -250 -450
Gfo(kJ/mole) -225 -425
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Chm II HW•Problem: 63
•Page: 640
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Review Quiz
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Heat Change•Calculate the heat change when the temperature of 1.0 kg H2O is changed from –100.0oC to 200.0oC.
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When 2.00 g NaOH dissolves in a 1.0 L water in a 2.5 kg calorimeter, the temp. went
from 22.5oC to 26.5oC. Calculate: Ho
soln Cwater = 4.18 J/gK Ccal = 2.00 J/gK
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Bond Energy•The energy change
when one mole of bonds are broken
Ho
bond
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Bond Equation
Hbondo
rxnHbond
o
products
Hbondo
reactants)
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Bond Energies (kJ/mole)
C-C 347 O=O
C-H 414 498
O-H 464
C=O 715
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Calculate the heat change when 1.00
mole of C2H6 is burned.
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Drill:Calculate H, G, & S in the production of 831mL
ammonia at 227oC under
250.0 kPa pressureCompd NH3
Hfo -46.1
Gfo -16.5
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1st Law Thermodynamics
•Total energy change = heat + work
E = q + W
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Work•W = Fd
•P = F/A
•V = Ad
•W = PV = nRT
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2nd Law Thermodynamics
•Total entropy in a system always increases assuming no energy is added to the system
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Thermodynamic Rxns are State
Rxns
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State Reaction•Reactions that are independent of the
path; thus not dependent on intermediates
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Lab 8:•Thermochemistry•HW: P 49•Page: 236
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Drill: Calculate Ho, Go, So, & solve Teq when:
A + BC AC2 + BCompd BC AC2
Hfo(kJ/mole) -150 -250
Gfo(kJ/mole) -125 -225
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Hess’s LawHrxn is the same
whether it occurs in a single step or a series
of steps.
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Calculate Ho & Go, & S & Teq at -23oC when:
A + BC AC + BCompd BC ACHf
o(kJ/mole) -150 -250Gf
o(kJ/mole) -175 -225
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Write TE for the process2 A + B C + D
C + A H
D + B 2 K
H + K M + B
K + M Product
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Write TE for the process2 A + B C + D
C + A H
D + B 2 K
H + K M + B
K + M Product
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AP Homework•Problem: 32 & 33
On page 235
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Write TE for the process2 A + 2 B C + D
C + A 2 H
D + B 2 K
H + K P + B
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Write TE for the process2 A + 2 B C + D
C + A 2 H
D + B 2 K
2 H + 2 K 2 P + 2 B
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Drill: Calculate Horxn for
the production of CaCO3 from CaO & CO2
Hf
o
(kJ/mole)
CaCO3 CaO CO2
-1206.9 -635.1 -393.5
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When 25.0 g CaCO3 is made
from CaO & CO2 in a 500. g calorimeter (C = 1.50 J/gK) containing 250 g of water
(C = 4.18 J/gK), the water changes from 25.0oC to 45.0oC. Calculate Hrxn/mole of CaCO3
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Calculate the % yield from the
results of the last two slides
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Bond Equation
Hbondo
rxnHbond
o
products
Hbondo
reactants)
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Bond Energies (kJ/mole)
C-C 347 O=O
C-H 414 685
O-H 464
C=O 715
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Calculate the heat change when 6.0
kg of ethane (C2H6) is burned
in excess oxygen.
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Substance Hof(kJ/mole)
S Hof S Ho
f
A -100 H -150B -150 K -200C -50 P -250D -125 Q -300
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Solve Horxn for TE
A + B 2 C + 2 D
C + A 2 H + P
D + B 2 K + P
H + K P + Q
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Solve Horxn for TE
A + B 2 C + 2 D
2C + 2A 4 H + 2P
2D + 2B 4K + 2P
4H + 4K 4P + 4Q
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Test on Thermochemistry
on Tuesday
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Review
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What does each symbol represent?
Define what is represents:
H:G:S:
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Calculate Htotal, when 40.0 g of
H2O is changed from - 25oC to
125oC. FPw = 0.0oC
BPw = 100.0 oC Hv = 2260 J/gCice = 2.06 (J/g K) Hf = 334 J/gCwater = 4.18 (J/g K)Csteam = 2.02 (J/g K)
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Calculate Ho, Go, & So for N2O5 + H2O HNO3
Cpd N2O5 H2O HNO3 Hf
o -11.3 -285.8 -174.1
Gfo -10.4 -237.2 -151.5
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Solve Ho for TE X + Y 2 W + 2 Z 60 kJ
W + X 2 R + P 40 kJ
2 S + P Z + Y 50 kJ
R + S P + Q 80 kJ
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Ho for TE X + Y 2 W + 2 Z 60 kJ
2W + 2X 4 R + 2P 80 kJ
2Z + 2Y 4 S + 2P -100 kJ
4 R + 4S 4P + 4Q 320 kJ
3X + 3Y 8P + 4Q 360 kJ
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Calculate Ho, G
o, & S for
AD2 + BC AC2 + BD
at (-23oC)
Cpd BC AD2 AC2 BD
Hf
o -150 -250 -300 -175
Gf
o -125 -225 -250 -150
Sf
o 75 50 80 ?
Determine Sf
o
BD
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Calculate Ho, Go, & So for PbO2 + CO CO2 + Pb
Cpd PbO2 CO CO2 Hf
o -277.4 -110.5 -393.5
Gfo -217.4 -137.2 -394.4
Calculate: Teq & H of 48 g PbO2
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Test Tomorrow
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When 4.20 g MgCO3 is decomposed to MgO & CO2 in a 2500.0 g calorimeter (C = 2.00 J/gK) containing 1.0.kg of water (C = 4.18 J/gK), the water changes from 23.00oC to 13.00oC. Calculate the heat of rxn/mole of MgCO3
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AP Homework:Read: Chapter 9Power Point: 17
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Chm II Homework:Read: Chapter 16Power Point: 19