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

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 43P

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Similar questions

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