29.The corrosion of iron is an electrochemical process that involves thestandard reduction potentials given here at 25 °C:Fe2*(aq) + 2eFe(s) E° = -0.44 VO2(g) + 4H*(aq) + 4e¯2H20(1) E° = 1.23 V%3DCalculate the voltage if the reaction occurs at pH = 4.00 but all otherconcentrations are maintained as they would be in a standard cell.-1.67 V1.43 V1.91 V1.67 V-1.91 V

Voltage can be calculated as follows

The corrosion of iron is an electrochemical process that involves the standard reduction potentials given here at 25 °C: Fe2*(aq) + 2e → Fe(s) E° = -0.44 V O2(g) + 4H*(aq) + 4e¯ → 2H20(1) E° = 1.23 V Calculate the voltage if the reaction occurs at pH = 4.00 but all other concentrations are maintained as they would be in a standard cell. -1.67 V 1.43 V 1.91 V 1.67 V O -1.91 V

The corrosion of iron is an electrochemical process that involves the standard reduction potentials given here at 25 °C: Fe2(aq) + 2e → Fe(s) E° = -0.44 V O2(g) + 4H(aq) + 4e¯ → 2H20(1) E° = 1.23 V Calculate the voltage if the reaction occurs at pH = 4.00 but all other concentrations are maintained as they would be in a standard cell. -1.67 V 1.43 V 1.91 V 1.67 V O -1.91 V

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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