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Use the Nernst equation to calculate the cell potential at 298K. Cu(s) + PtCl ² (aq) (0.10M) → Cu²+ (aq) (0.20 M) + PtCl4² (aq) (0.10M) + 2Cl(aq) (0.40M) • Ered Cu²+ (aq)/Cu(s) = +0.34 V • Eºred PtCl 6² (aq)/ PtCl4²(aq) + 2Cl¯ Oxidation: Cu(s)→→ Cu²+ (aq) + 2 e Reduction:PtCl6² (aq) + 2 e → PtCl 4² (aq) + 2Cl (a (aq) (aq) = +0.68 V Ex = -0.34 V Eº = +0.68 V red

Use the Nernst equation to calculate the cell potential at 298K. Cu(s) + PtCl ² (aq) (0.10M) → Cu²+ (aq) (0.20 M) + PtCl4² (aq) (0.10M) + 2Cl(aq) (0.40M) • Ered Cu²+ (aq)/Cu(s) = +0.34 V • Eºred PtCl 6² (aq)/ PtCl4²(aq) + 2Cl¯ Oxidation: Cu(s)→→ Cu²+ (aq) + 2 e Reduction:PtCl6² (aq) + 2 e → PtCl 4² (aq) + 2Cl (a (aq) (aq) = +0.68 V Ex = -0.34 V Eº = +0.68 V red

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 18.95QE
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Use the Nernst equation to calculate the cell potential at 298K. Cu(s) + PtCl ² (aq) (0.10M) → Cu²+ (aq) (0.20 M) + PtCl 4² (aq) (0.10M) + 2Cl(aq) (0.40M) • Ered Cu²+ (aq)/Cu(s) = +0.34 V • Eºred PtCl 6² (aq)/ PtCl4²(aq) + 2Cl¯ Oxidation: Cu(s)→→ Cu²+ (aq) + 2 e 2- Reduction: PtCl6² (aq) + 2 e → PtCl 4² (aq) + 2Cl(a (aq) √(aq) = ₁ = +0.68 V Ex = -0.34 V Eº = +0.68 V red
Transcribed Image Text:Use the Nernst equation to calculate the cell potential at 298K. Cu(s) + PtCl ² (aq) (0.10M) → Cu²+ (aq) (0.20 M) + PtCl 4² (aq) (0.10M) + 2Cl(aq) (0.40M) • Ered Cu²+ (aq)/Cu(s) = +0.34 V • Eºred PtCl 6² (aq)/ PtCl4²(aq) + 2Cl¯ Oxidation: Cu(s)→→ Cu²+ (aq) + 2 e 2- Reduction: PtCl6² (aq) + 2 e → PtCl 4² (aq) + 2Cl(a (aq) √(aq) = ₁ = +0.68 V Ex = -0.34 V Eº = +0.68 V red
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