An aqueous solution of potassium permanganate (KMN04) appears deep purple. The permanganate ion can be reduced to the pale-pink manganese(II) ion (Mn²+) in aqueous acidic solutions. The standard reduction potential of an MnO, Mn²+ half-cell is Eell with a Zn²+ |Zn half-cell in a galvanic cell, with [Zn²+] = [MnO,] = [Mn²+] = [H;O*] = 1 M. = 1.49 V. Suppose this half-cell is combined (a) Write equations for the reactions at the anode and the cathode. (b) Write a balanced equation for the overall cell reaction. (c) Calculate the standard cell potential difference, AE 'cell

An aqueous solution of potassium permanganate (KMN04) appears deep purple. The permanganate ion can be reduced to the pale-pink manganese(II) ion (Mn²+) in aqueous acidic solutions. The standard reduction potential of an MnO, Mn²+ half-cell is Eell with a Zn²+ |Zn half-cell in a galvanic cell, with [Zn²+] = [MnO,] = [Mn²+] = [H;O*] = 1 M. = 1.49 V. Suppose this half-cell is combined (a) Write equations for the reactions at the anode and the cathode. (b) Write a balanced equation for the overall cell reaction. (c) Calculate the standard cell potential difference, AE 'cell

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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