4. a. Write a balanced equation to represent the overall reaction you would expect to occur in the electrolysis of molten NaBr. b. Write a balanced equation to represent the overall reaction you would expect to occur in the electrolysis of molten NaBr in the presence of molten MgF2. State clearly which ion is oxidized at the anode and which ion is reduced at the cathode. c. Write a balanced equation to represent the overall reaction you would expect to occur in the electrolysis of aqueous NaBr. Hint: remember overvoltage: 2H2O(1) → O2(g) + 4H*(aq)+ 4e¯ 2H2O(1) + 2e¯ → H2(g) + 2OH´(aq) E° = 0.82V, ~1.4V with overvoltage (oxidation) E° = -0.42V, ~ -1V with overvoltage (reduction) d. Clearly explain why the products of the three processes are not the same.

4. a. Write a balanced equation to represent the overall reaction you would expect to occur in the electrolysis of molten NaBr. b. Write a balanced equation to represent the overall reaction you would expect to occur in the electrolysis of molten NaBr in the presence of molten MgF2. State clearly which ion is oxidized at the anode and which ion is reduced at the cathode. c. Write a balanced equation to represent the overall reaction you would expect to occur in the electrolysis of aqueous NaBr. Hint: remember overvoltage: 2H2O(1) → O2(g) + 4H*(aq)+ 4e¯ 2H2O(1) + 2e¯ → H2(g) + 2OH´(aq) E° = 0.82V, ~1.4V with overvoltage (oxidation) E° = -0.42V, ~ -1V with overvoltage (reduction) d. Clearly explain why the products of the three processes are not the same.

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

4.
a. Write a balanced equation to represent the overall reaction you would expect to occur in the electrolysis
of molten NaBr.
b. Write a balanced equation to represent the overall reaction you would expect to occur in the electrolysis
of molten NaBr in the presence of molten MgF2. State clearly which ion is oxidized at the anode and which
ion is reduced at the cathode.
c. Write a balanced equation to represent the overall reaction you would expect to occur in the electrolysis
of aqueous NaBr. Hint: remember overvoltage:
2H2O(1) → O2(g) + 4H*(aq)+ 4e¯
2H2O(1) + 2e* → H2(g) + 20H´(aq)
E° = 0.82V, ~1.4V with overvoltage (oxidation)
E° = -0.42V, ~ -1V with overvoltage (reduction)
d. Clearly explain why the products of the three processes are not the same.

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