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Use standard reduction potentials to calculate the equilibrium constant for the reaction: Pb2+ (aq) + Sn(s) → Pb(s) + Sn'(aq) Pb + (aq) + 2e → Pbs) Erd - -0.126 V Sn+ (ag) + 2e → Sn(s) E° red = -0.140 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: AG° for this reaction would be

Use standard reduction potentials to calculate the equilibrium constant for the reaction: Pb2+ (aq) + Sn(s) → Pb(s) + Sn'(aq) Pb + (aq) + 2e → Pbs) Erd - -0.126 V Sn+ (ag) + 2e → Sn(s) E° red = -0.140 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: AG° for this reaction would be

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
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 18.48QE: The standard potential of the cell reaction Ag+(aq)+Eu2+(aq)Ag(s)+Eu3+(aq) is E = +1.23 V. Use the...
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Use standard reduction potentials to calculate the equilibrium constant for the reaction:

Pb2+ (aq) + Sn(s) → Pb(s) + Sn'(aq)

Pb + (aq) + 2e → Pbs) Erd - -0.126 V

Sn+ (ag) + 2e → Sn(s) E°

red = -0.140 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:

AG° for this reaction would be

 

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