onsider the voltaic cell made from the following redox couples: Sb2O5(s) / Sb2O3(s) E°red = +0.69 V & InO4'(aq) / MnO4²(aq) E°red = +0.58 V %3D Write the balanced half-reaction that occurs in the anode under basic conditions. (Use the 1 action method to balance.) Write the balanced half-reaction that occurs in the cathode under basic conditions. (Use the action method to balance.)

onsider the voltaic cell made from the following redox couples: Sb2O5(s) / Sb2O3(s) E°red = +0.69 V & InO4'(aq) / MnO4²(aq) E°red = +0.58 V %3D Write the balanced half-reaction that occurs in the anode under basic conditions. (Use the 1 action method to balance.) Write the balanced half-reaction that occurs in the cathode under basic conditions. (Use the action method to balance.)

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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Question

Consider the voltaic cell made from the following redox couples:
Sb2O5(s) / Sb2O3(s)
E°red =
+0.69 V
&
MnO4 (aq) / MnO42 (aq)
E°red = +0.58 V
a) Write the balanced half-reaction that occurs in the anode under basic conditions. (Use the 1/2
reaction method to balance.)
b) Write the balanced half-reaction that occurs in the cathode under basic conditions. (Use the 1/2
reaction method to balance.)
c) Write the balanced overall cell reaction.
d) Calculate the standard cell potential.
e) Calculate the cell potential at 25°C when the cathode and anode are at pH = 8.50 and the
[MnO4] = [Mn042] = 0.0025 M. (Hint: What concentrations can you find given pH?)

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