Given an electrochemical half-cell by mixing 0.01 M MnO4" solution with 0.02 M Mn2+ solution. Solution pH was set at pH 2.0. Compute potential of this half reaction at 25 °C. Given the half reaction as below. MnO4(eg) + 8H+(ag) + 5e → Mn2+lag) + 4H2O1) E° = 1.51V

Given an electrochemical half-cell by mixing 0.01 M MnO4" solution with 0.02 M Mn2+ solution. Solution pH was set at pH 2.0. Compute potential of this half reaction at 25 °C. Given the half reaction as below. MnO4(eg) + 8H+(ag) + 5e → Mn2+lag) + 4H2O1) E° = 1.51V

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter17: Electrochemistry And Its Applications

Section: Chapter Questions

Problem 92QRT

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Question

Given an electrochemical half-cell by mixing 0.01 M MnO4 solution with 0.02 M Mn2+ solution.
Solution pH was set at pH 2.0. Compute potential of this half reaction at 25 °C. Given the half
reaction as below.
Mn04(ag) + 8H+(ag) + 5e > Mn2+(ag) + 4H2O1) E° = 1.51v

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