Pt | H₂ (0.50 atm) | H+ (0.10 M) || MnO4- (0.10 M), Mn²+ (1.0 M), H* (0.10 M) | Pt 2H+ + 2e →→ H₂ Eº = 0.00 V Eº = -0.80 V MnO4 + 8H+ + 5e-→Mn²+ + 4H₂O a. Write the balanced chemical equation for the above redox reaction. Calculate the cell potential of the cell. b. C. Determine the free energy change for the overall redox reaction in the cell.

Pt | H₂ (0.50 atm) | H+ (0.10 M) || MnO4- (0.10 M), Mn²+ (1.0 M), H* (0.10 M) | Pt 2H+ + 2e →→ H₂ Eº = 0.00 V Eº = -0.80 V MnO4 + 8H+ + 5e-→Mn²+ + 4H₂O a. Write the balanced chemical equation for the above redox reaction. Calculate the cell potential of the cell. b. C. Determine the free energy change for the overall redox reaction in the cell.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.ACP

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