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a. If the equilibrium constant (K) for water dissociation: H₂O(g) → H2(g) + 1/2O2(g) is 3. 4808x10+ at 2000 K, what is the equilibrium constant at room temperature? FYI: A,H° = 241.82 kJ/mol; you have to assume that it is temperature-invariant. b. What is the corresponding A.Gº? c. Why is there a slight difference in your answer in b. from -A-Gm=228.572 kJ/mol?

a. If the equilibrium constant (K) for water dissociation: H₂O(g) → H2(g) + 1/2O2(g) is 3. 4808x10+ at 2000 K, what is the equilibrium constant at room temperature? FYI: A,H° = 241.82 kJ/mol; you have to assume that it is temperature-invariant. b. What is the corresponding A.Gº? c. Why is there a slight difference in your answer in b. from -A-Gm=228.572 kJ/mol?

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy
Section: Chapter Questions
Problem 51GQ
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a. If the equilibrium constant (K) for water dissociation: H₂O(g) → H2(g) + ½/2O2(g) is 3. 4808×104 at 2000 K, what is the equilibrium constant at room temperature? FYI: A,H° = 241.82 kJ/mol; you have to assume that it is temperature-invariant. b. What is the corresponding 4,Gº? c. Why is there a slight difference in your answer in b. from -A-Gm-228.572 kJ/mol?
Transcribed Image Text:a. If the equilibrium constant (K) for water dissociation: H₂O(g) → H2(g) + ½/2O2(g) is 3. 4808×104 at 2000 K, what is the equilibrium constant at room temperature? FYI: A,H° = 241.82 kJ/mol; you have to assume that it is temperature-invariant. b. What is the corresponding 4,Gº? c. Why is there a slight difference in your answer in b. from -A-Gm-228.572 kJ/mol?
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