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3) The corrosion of iron is an electrochemical process that involves the standard reduction potentials given...

3) 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– → 2H2O(l) E° = +1.23 V

a. Calculate the voltage for the standard cell based on the corrosion reaction. 2Fe(s) + O2(g) + 4H+ (aq) → 2Fe2+(aq) + 2H2O(l)

b. Calculate the voltage if the reaction in Part a occurs at pH = 4.00 but all other concentrations are maintained as they were in the standard cell.

c. For the reaction Fe(OH)2(s) + 2e– → Fe(s) + 2OH– (aq), E° = –0.88 V. Use this information with one of the given standard potentials in Appendix ** to calculate the Ksp of Fe(OH)2.

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