Zn2+(aq) + 2e → Zn (s) E°red = -O.76 V½ O2 (g)+ H2O + 2e¯ → 2 OH (aq) Eºred =+0.40 VUse the reduction potential above tosolve for the cell potential E°cell in voltsfor the corrosion of copper:Zn (s) + ½ O2 (g) + H2O → Zn²* (aq) +20H (aq) From the result above, the cell potentialfor the corrosion of Zinc is higher thaniron. The oxidation/corrosion of copperis a MORE spontaneous reactioncompared to the oxidation/corrosion ofiron. Therefore, zinc is more prone tooxidation compared to iron. We can saythat zinc is a more active metal thaniron.Using the result for Nail D:Does wrapping Zinc strip prevented theIron nail from undergoingoxidation/rusting/corrosion?

The cell reaction for corrosion of zinc is as below: Zn(s) + 1/2 O2 (g) + H2O (l) -------> Zn2+…

Answered: Use the reduction potential above to…

Use the reduction potential above to solve for the cell potential E°cell in volts for the corrosion of copper: Zn (s) + ½ O2 (g) + H2O → Zn²* (aq) + 20H (aq)

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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