CarbonΔHof (kJ/mol)ΔGof (kJ/mol)So (J/mol K)C (s, graphite)005.7C (s, diamond)1.92.92.4C (g)716.7671.3158.1CCl4 (l)-135.4-65.2216.4CCl4 (g)-102.9-60.6309.9CHCl3 (l)-134.5-73.7201.7CHCl3 (g)-103.1-70.3295.7CH4 (g)-74.8-50.7186.3CH3OH (g)-200.7-162.0239.8CH3OH (l)-238.7-166.3126.8H2CO (g)-116.0-110.0219.0HCOOH (g)-363.0-351.0249.0HCN (g)135.1125.0202.0C2H2 (g)226.7209.2200.9C2H4 (g)52.368.2219.6CH3CHO (g, acetaldehyde)-166.0-129.0250.0C2H4O (g, ethylene oxide)-53.0-13.0242.0CH3CH2OH (l)-277.7-174.8160.7CH3CH2OH (g)-235.1-168.5282.7CH3COOH (l)-484.0-389.0160.0C2H6 (g)-84.7-32.8229.6C3H6 (g)20.962.7266.9C3H8 (g)-103.8-23.5269.9CH2=CHCN (l)152.0190.0274.0C6H6 (l)49.0124.5172.8C6H12O6 (s)-1275.0-911.0212.0CO (g)-110.5-137.2197.7CO2 (g)-393.5-394.4213.7CS2 (g)117.467.1237.8COCl2 (g)-218.8-204.6283.5 HydrogenΔHof (kJ/mol)ΔGof (kJ/mol)So (J/mol K)H2 (g)00130.7H (g)218.0203.2114.7H+ (g)1536.2 H+ (aq)0 OH- (aq)-230.0-157.0-11.0H2O (l)-285.8-237.169.9H2O (g)-241.8-228.6188.8H2O2 (l)-187.8-120.4109.6 Consider the reaction:CO(g) + H2O(1)→CO2(g)+ H2(g)Using standard thermodynamic data at 298K, calculate the free energy change when 2.30 moles of CO(g) react at standard conditions.AG°rxnkJ

Gibbs energy is a significant quantity that tells us the useful work performed by a system. It is…

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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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Carbon	ΔH^o_f (kJ/mol)	ΔG^o_f (kJ/mol)	S^o (J/mol K)
C (s, graphite)	0	0	5.7
C (s, diamond)	1.9	2.9	2.4
C (g)	716.7	671.3	158.1
CCl₄(l)	-135.4	-65.2	216.4
CCl₄ (g)	-102.9	-60.6	309.9
CHCl₃ (l)	-134.5	-73.7	201.7
CHCl₃ (g)	-103.1	-70.3	295.7
CH₄ (g)	-74.8	-50.7	186.3
CH₃OH (g)	-200.7	-162.0	239.8
CH₃OH (l)	-238.7	-166.3	126.8
H₂CO (g)	-116.0	-110.0	219.0
HCOOH (g)	-363.0	-351.0	249.0
HCN (g)	135.1	125.0	202.0
C₂H₂ (g)	226.7	209.2	200.9
C₂H₄ (g)	52.3	68.2	219.6
CH₃CHO (g, acetaldehyde)	-166.0	-129.0	250.0
C₂H₄O (g, ethylene oxide)	-53.0	-13.0	242.0
CH₃CH₂OH (l)	-277.7	-174.8	160.7
CH₃CH₂OH (g)	-235.1	-168.5	282.7
CH₃COOH (l)	-484.0	-389.0	160.0
C₂H₆ (g)	-84.7	-32.8	229.6
C₃H₆ (g)	20.9	62.7	266.9
C₃H₈ (g)	-103.8	-23.5	269.9
CH₂=CHCN (l)	152.0	190.0	274.0
C₆H₆ (l)	49.0	124.5	172.8
C₆H₁₂O₆ (s)	-1275.0	-911.0	212.0
CO (g)	-110.5	-137.2	197.7
CO₂ (g)	-393.5	-394.4	213.7
CS₂ (g)	117.4	67.1	237.8
COCl₂ (g)	-218.8	-204.6	283.5

Hydrogen	ΔH^o_f (kJ/mol)	ΔG^o_f (kJ/mol)	S^o (J/mol K)
H₂ (g)	0	0	130.7
H (g)	218.0	203.2	114.7
H⁺ (g)	1536.2
H⁺ (aq)	0
OH^- (aq)	-230.0	-157.0	-11.0
H₂O (l)	-285.8	-237.1	69.9
H₂O (g)	-241.8	-228.6	188.8
H₂O₂ (l)	-187.8	-120.4	109.6

Consider the reaction:
CO(g) + H2O(1)→CO2(g)+ H2(g)
Using standard thermodynamic data at 298K, calculate the free energy change when 2.30 moles of CO(g) react at standard conditions.
AG°rxn
kJ

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