Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Ag+ (aq) + Fe(s) → 2Ag(s) + Fe²+ (aq) Ag (aq) + e → Ag(s) E 0.799 V red Fe2+ (aq) + 2e wwww Fe(s) E :-0.440 V red Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at 298 K: AGO for this reaction would be than zero.

Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Use standard reduction potentials to calculate the equilibrium constant
for the reaction:
2Ag (aq) + Fe(s) → 2Ag(s) + Fe²+ (aq)
Ag+ (aq) + e → Ag(s) E
red
Fe2+ (aq) + 2e → Fe(s) E
red
www
0.799 V
-0.440 V
Hint: Carry at least 5 significant figures during intermediate calculations
to avoid round off error when taking the antilogarithm.
Equilibrium constant at 298 K:
AGO for this reaction would be
than zero.
Transcribed Image Text:Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Ag (aq) + Fe(s) → 2Ag(s) + Fe²+ (aq) Ag+ (aq) + e → Ag(s) E red Fe2+ (aq) + 2e → Fe(s) E red www 0.799 V -0.440 V Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at 298 K: AGO for this reaction would be than zero.
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