Consider a galvanic cell with the following half-reactions: MnO4-+ 8 H†+5e¯ → Mn²+ + 4 H2O E° = 1.51 V I04 -+ 2 H* + 2e- → IO3 -+ H2O E° = 1.60 V i. Write the reduction half-reaction. ii. Write the oxidation half-reaction. iii. Write the balanced overall reaction.

Consider a galvanic cell with the following half-reactions: MnO4-+ 8 H†+5e¯ → Mn²+ + 4 H2O E° = 1.51 V I04 -+ 2 H* + 2e- → IO3 -+ H2O E° = 1.60 V i. Write the reduction half-reaction. ii. Write the oxidation half-reaction. iii. Write the balanced overall reaction.

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 a galvanic cell with the following half-reactions:
MnO4-+ 8 H* + 5e¯ → Mn²+ + 4 H2O
E° = 1.51 V
I04 -+ 2 H* + 2e → IO3 -+ H2O
E° = 1.60 V
i. Write the reduction half-reaction.
ii. Write the oxidation half-reaction.
iii. Write the balanced overall reaction.
iv. Calculate the standard cell potential, E°cell.
v. Which is the oxidizing agent?
vi. Which is the reducing agent?

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