Consider the corrosion of copper at 30°C using the overall reaction: Cu(s) + 0.5 O₂(g) + 2 H3O+ (aq) → Cu²+ (aq) + 3 H₂O(l) If the partial pressure of oxygen is 0.88 bar, and the concentration of Cu²+ (aq) is 5.1 M, at what pH does the reaction become spontaneous?

Consider the corrosion of copper at 30°C using the overall reaction: Cu(s) + 0.5 O₂(g) + 2 H3O+ (aq) → Cu²+ (aq) + 3 H₂O(l) If the partial pressure of oxygen is 0.88 bar, and the concentration of Cu²+ (aq) is 5.1 M, at what pH does the reaction become spontaneous?

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 corrosion of copper at 30°C using the overall reaction:
Cu(s) + 0.5 O₂(g) + 2 H3O+ (aq) → Cu²+ (aq) + 3 H₂O(l)
If the partial pressure of oxygen is 0.88 bar, and the concentration of Cu²+ (aq)
is 5.1 M, at what pH does the reaction become spontaneous?

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