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a. Calculate Ecell and AG° (in kJ) and determine if the reaction is spontaneous. b. Calculate the equilibrium constant, K, at 298 K for the reaction using AG° = -RT In K. 4 Ag(s) + O2(g) + 4 H*(aq) → 4 Ag*(aq) + 2 H,O(1) O2(g) + 4 H*(aq) + 4 e +1.23 2 H2O(1) - +1.06 Br2(1) + 2 e 2 Br (aq) NO, (aq) + 4 H*(aq) + 3 e¯ Ag*(aq) + e - → NO(g) + 2 H,O(I) +0.96 +0.80 Ag(s) Do the signs/values of AG° and K make sense for this reaction given the cell potential?

a. Calculate Ecell and AG° (in kJ) and determine if the reaction is spontaneous. b. Calculate the equilibrium constant, K, at 298 K for the reaction using AG° = -RT In K. 4 Ag(s) + O2(g) + 4 H*(aq) → 4 Ag*(aq) + 2 H,O(1) O2(g) + 4 H*(aq) + 4 e +1.23 2 H2O(1) - +1.06 Br2(1) + 2 e 2 Br (aq) NO, (aq) + 4 H*(aq) + 3 e¯ Ag*(aq) + e - → NO(g) + 2 H,O(I) +0.96 +0.80 Ag(s) Do the signs/values of AG° and K make sense for this reaction given the cell potential?

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter17: Chemcial Thermodynamics
Section: Chapter Questions
Problem 17.59QE: Calculate G for the following reactions and state whether each reaction is spontaneous under...
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a. Calculate Ecell and AG° (in kJ) and determine if the reaction is spontaneous. b. Calculate the equilibrium constant, K, at 298 K for the reaction using AG° = -RT In K. 4 Ag(s) + O2(g) + 4 H*(aq) → 4 Ag*(aq) + 2 H,O(1) O2(g) + 4 H*(aq) + 4 e +1.23 2 H2O(1) - +1.06 Br2(1) + 2 e 2 Br (aq) NO, (aq) + 4 H*(aq) + 3 e¯ Ag*(aq) + e - → NO(g) + 2 H,O(I) +0.96 +0.80 Ag(s) Do the signs/values of AG° and K make sense for this reaction given the cell potential?
Transcribed Image Text:a. Calculate Ecell and AG° (in kJ) and determine if the reaction is spontaneous. b. Calculate the equilibrium constant, K, at 298 K for the reaction using AG° = -RT In K. 4 Ag(s) + O2(g) + 4 H*(aq) → 4 Ag*(aq) + 2 H,O(1) O2(g) + 4 H*(aq) + 4 e +1.23 2 H2O(1) - +1.06 Br2(1) + 2 e 2 Br (aq) NO, (aq) + 4 H*(aq) + 3 e¯ Ag*(aq) + e - → NO(g) + 2 H,O(I) +0.96 +0.80 Ag(s) Do the signs/values of AG° and K make sense for this reaction given the cell potential?
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