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(a) Calculate the half-cell potential for the reaction O2(g) + 4 H3O* (aq) + 4 e¯ → 6 H;0(€) at pH 7 with the oxygen pressure at 1 atm. (b) Explain why aeration of solutions of I- leads to their decomposition. Write a balanced equation for the redox reaction that occurs. (c) Will the same problem arise with solutions containing Br or CI? Explain. (d) Will decomposition be favored or opposed by increas- ing acidity?

(a) Calculate the half-cell potential for the reaction O2(g) + 4 H3O* (aq) + 4 e¯ → 6 H;0(€) at pH 7 with the oxygen pressure at 1 atm. (b) Explain why aeration of solutions of I- leads to their decomposition. Write a balanced equation for the redox reaction that occurs. (c) Will the same problem arise with solutions containing Br or CI? Explain. (d) Will decomposition be favored or opposed by increas- ing acidity?

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 88AP
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(a) Calculate the half-cell potential for the reaction O2(g) + 4 H3O* (aq) + 4 e¯ → 6 H;0(€) at pH 7 with the oxygen pressure at 1 atm. (b) Explain why aeration of solutions of I- leads to their decomposition. Write a balanced equation for the redox reaction that occurs. (c) Will the same problem arise with solutions containing Br or CI? Explain. (d) Will decomposition be favored or opposed by increas- ing acidity?
Transcribed Image Text:(a) Calculate the half-cell potential for the reaction O2(g) + 4 H3O* (aq) + 4 e¯ → 6 H;0(€) at pH 7 with the oxygen pressure at 1 atm. (b) Explain why aeration of solutions of I- leads to their decomposition. Write a balanced equation for the redox reaction that occurs. (c) Will the same problem arise with solutions containing Br or CI? Explain. (d) Will decomposition be favored or opposed by increas- ing acidity?
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