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

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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Question

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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