Standard Enthalpy of Formation' for Various CompoundsCompoundДН (kJ/mol)CompoundAHr (kJ/mol)CompoundAH´r (kJ/mol)CompoundAH'¡ (kJ/mol)Ag,0(s)-30.6C,H;OH(1)-277.6HCI(g)-92.3NH,CI(s)-315.4Ag2S(s)-31.8C¿H6(g)-84.7HF(g)-268.6ΝΗNO; (s)-365.1AgBr(s)-99.5C3H$(g)-103.8HgO(s)-90.7NiO(s)-244.3AgCl(s)-127.0n-C4H10(g)-124.7HgS(s)-58.2NO(g)+90.4AgI(s)-62.4n-C3H12(1)-173.1HI(g)+25.9NO2(g)+33.9Al»O3(s)-1669.8CO(g)-110.5HNO;(1)-173.2Pb3O4(s)-734.7BaCl2(s)-860.1CO2(g)-393.5KBr(s)-392.2PbBr2(s)-277.0BaCO3(s)-1218.8CoO(s)-239.3KCI(s)-435.9PbCl2(s)-359.2BaO(s)-558.1Cr2O3(s)-1128.4KC1O;(s)-391.4PbO(s)-217.9BaSO4(s)-1465.2Cu,O(s)-166.7KF(s)-562.6P6O2(s)-276.6Cа(ОН)2(s)-986.6CuO(s)-155.2Mg(OH)2(s)-924.7PCI;(g)-306.4CaCl2(s)-795.0CuS(s)-48.5MgCl2(s)-641.8PCI5(g)-398.9CACO3(s)-1207.0CUSO4(s)-769.9MgCO3(s)-1113SiO2(s)-859.4CaO(s)-635.5Fe2O3(s)-822.2MgO(s)-601.8SnCl2(s)-349.8CASO4(s)-1432.7Fe;O4(s)-1120.9MgSO4(s)-1278.2SNCL4(1)-545.2CCL(1)-139.5H,O(g)-241.8MnO(s)-384.9SnO(s)-286.2CH;OH(1)-238.6H2O(1)-285.8MNO2(s)-519.7SnO2(s)-580.7CH4(g)-74.8H,O2(1)-187.6NaCl(s)-411.0SO-(g)-296.1CHCI;(1)-131.8H2S(g)-20.1NaF(s)-569.0SO3(g)-395.2C2H2(g)+226.7H2SO4(1)-811.3NaOH(s)-426.7ZnO(s)-348.0C¿H4(g)+52.3HBr(g)-36.2NH3(g)-46.2ZnS(s)-202.9* All standard enthalpy values are at 25°C and 1 atmosphere of pressure.Standard Enthalpy of Formation' for Atomic and Molecular lonsCationsAH°¡ (kJ/mol)CationsAH'r (kJ/mol)AnionsAH° (kJ/mol)AnionsAH' (kJ/mol)Ag°(aq)+105.9K*(aq)-251.2Br (aq)-120.9H2PO4 (aq)-1302.5Al*(aq)Li"(aq)CI (aq)НРО (аg)-524.7-278.5-167.4-1298.7Ba (aq)-538.4Mg²"(aq)ClO; (aq)-462.0-98.3Гад)-55.9Са (aq)Mn"(aq)2+CIO, (aq)Co? (aq)-543.0-218.8-131.4MnO4 (aq)-518.4Cd²*(aq)Na"(aq)NO3 (aq)-72.4-239.7-676.3-206.6Cu²*(aq)NH4*(aq)-132.8CrO2² (aq)ОН (аq)+64.4-863.2-229.9Fe2*(aq)-87.9"(aq)-64.0F (aq)-329.1PO (aq)-1284.1Fe*(aq)Pb²*(aq)НСО, (аq)-691.1s? (aq)-47.7+1.6+41.8H*(aq)0.0Sn²*(aq)so?" (aq)-10.0-907.5Zn*(aq)* All standard enthalpy values are at 25°C, 1 molar concentration, and 1 atmosphere of pressure.-152.4 4. Using ethanol as a fuel reduces greenhouse gas emissions by 40-50% when compared directly togasoline. Calculate the enthalpy change for the combustion of ethanol, using the enthalpies offormation for C2H5OH), CO2(g), and H2Ou, located on the chart provided for the following reaction:C2H5OH(1) + 302(g) → 2CO2(g) + 3H2O1)

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enthalpy change for

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.

Question

Standard Enthalpy of Formation' for Various Compounds
Compound
ДН (kJ/mol)
Compound
AHr (kJ/mol)
Compound
AH´r (kJ/mol)
Compound
AH'¡ (kJ/mol)
Ag,0(s)
-30.6
C,H;OH(1)
-277.6
HCI(g)
-92.3
NH,CI(s)
-315.4
Ag2S(s)
-31.8
C¿H6(g)
-84.7
HF(g)
-268.6
ΝΗNO; (s)
-365.1
AgBr(s)
-99.5
C3H$(g)
-103.8
HgO(s)
-90.7
NiO(s)
-244.3
AgCl(s)
-127.0
n-C4H10(g)
-124.7
HgS(s)
-58.2
NO(g)
+90.4
AgI(s)
-62.4
n-C3H12(1)
-173.1
HI(g)
+25.9
NO2(g)
+33.9
Al»O3(s)
-1669.8
CO(g)
-110.5
HNO;(1)
-173.2
Pb3O4(s)
-734.7
BaCl2(s)
-860.1
CO2(g)
-393.5
KBr(s)
-392.2
PbBr2(s)
-277.0
BaCO3(s)
-1218.8
CoO(s)
-239.3
KCI(s)
-435.9
PbCl2(s)
-359.2
BaO(s)
-558.1
Cr2O3(s)
-1128.4
KC1O;(s)
-391.4
PbO(s)
-217.9
BaSO4(s)
-1465.2
Cu,O(s)
-166.7
KF(s)
-562.6
P6O2(s)
-276.6
Cа(ОН)2(s)
-986.6
CuO(s)
-155.2
Mg(OH)2(s)
-924.7
PCI;(g)
-306.4
CaCl2(s)
-795.0
CuS(s)
-48.5
MgCl2(s)
-641.8
PCI5(g)
-398.9
CACO3(s)
-1207.0
CUSO4(s)
-769.9
MgCO3(s)
-1113
SiO2(s)
-859.4
CaO(s)
-635.5
Fe2O3(s)
-822.2
MgO(s)
-601.8
SnCl2(s)
-349.8
CASO4(s)
-1432.7
Fe;O4(s)
-1120.9
MgSO4(s)
-1278.2
SNCL4(1)
-545.2
CCL(1)
-139.5
H,O(g)
-241.8
MnO(s)
-384.9
SnO(s)
-286.2
CH;OH(1)
-238.6
H2O(1)
-285.8
MNO2(s)
-519.7
SnO2(s)
-580.7
CH4(g)
-74.8
H,O2(1)
-187.6
NaCl(s)
-411.0
SO-(g)
-296.1
CHCI;(1)
-131.8
H2S(g)
-20.1
NaF(s)
-569.0
SO3(g)
-395.2
C2H2(g)
+226.7
H2SO4(1)
-811.3
NaOH(s)
-426.7
ZnO(s)
-348.0
C¿H4(g)
+52.3
HBr(g)
-36.2
NH3(g)
-46.2
ZnS(s)
-202.9
* All standard enthalpy values are at 25°C and 1 atmosphere of pressure.
Standard Enthalpy of Formation' for Atomic and Molecular lons
Cations
AH°¡ (kJ/mol)
Cations
AH'r (kJ/mol)
Anions
AH° (kJ/mol)
Anions
AH' (kJ/mol)
Ag°(aq)
+105.9
K*(aq)
-251.2
Br (aq)
-120.9
H2PO4 (aq)
-1302.5
Al*(aq)
Li"(aq)
CI (aq)
НРО (аg)
-524.7
-278.5
-167.4
-1298.7
Ba (aq)
-538.4
Mg²"(aq)
ClO; (aq)
-462.0
-98.3
Гад)
-55.9
Са (aq)
Mn"(aq)
2+
CIO, (aq)
Co? (aq)
-543.0
-218.8
-131.4
MnO4 (aq)
-518.4
Cd²*(aq)
Na"(aq)
NO3 (aq)
-72.4
-239.7
-676.3
-206.6
Cu²*(aq)
NH4*(aq)
-132.8
CrO2² (aq)
ОН (аq)
+64.4
-863.2
-229.9
Fe2*(aq)
-87.9
"(aq)
-64.0
F (aq)
-329.1
PO (aq)
-1284.1
Fe*(aq)
Pb²*(aq)
НСО, (аq)
-691.1
s? (aq)
-47.7
+1.6
+41.8
H*(aq)
0.0
Sn²*(aq)
so?" (aq)
-10.0
-907.5
Zn*(aq)
* All standard enthalpy values are at 25°C, 1 molar concentration, and 1 atmosphere of pressure.
-152.4

4. Using ethanol as a fuel reduces greenhouse gas emissions by 40-50% when compared directly to
gasoline. Calculate the enthalpy change for the combustion of ethanol, using the enthalpies of
formation for C2H5OH), CO2(g), and H2Ou, located on the chart provided for the following reaction:
C2H5OH(1) + 302(g) → 2CO2(g) + 3H2O1)

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