Consider the following redox half-reaction at 25 °C: MnO4 (aq) + 8 H* (aq) + 5 e¯ → Mn²* (aq) + 4 H2O (I) E° = +1.51 V For a ratio of [Mn²*] : [MnO4¯]] = 1000:1, what must the pH of the solution be to give a value of the cell potential of E = +1.45 V? R = 8.314 J/mol.K F = 96485 C/mol Data needed:

Consider the following redox half-reaction at 25 °C: MnO4 (aq) + 8 H* (aq) + 5 e¯ → Mn²* (aq) + 4 H2O (I) E° = +1.51 V For a ratio of [Mn²*] : [MnO4¯]] = 1000:1, what must the pH of the solution be to give a value of the cell potential of E = +1.45 V? R = 8.314 J/mol.K F = 96485 C/mol Data needed:

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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