The overall reaction of the oxidation of iron(II) with oxygen in acidic solutions proceeds as follows:...

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The overall reaction of the oxidation of iron(II) with oxygen in acidic solutions proceeds as follows: 4Fe(g) + O2(g) +4H(aq) ⇒4Fe(a) +2H₂O(1) a) Determine the cell potential for the above reation at a pH of 7. Assume standard state conditions for all chemical species whose concentrations are not specified. b) Determine the effect of precipitation of Fe(III) involved in the oxidation-reduction reaction on the cell potential obtained in a) by comparing it to the cell potential when iron(III) is in equilibrium with iron(III) hydroxide, Fe(OH)3. The solubility product constant for iron(III) hydroxide is 6x10-38. The overall reaction of the oxidation of iron(II) with oxygen in acidic solutions proceeds as follows: 4Fe(g) + O2(g) +4H(aq) ⇒4Fe(a) +2H₂O(1) a) Determine the cell potential for the above reation at a pH of 7. Assume standard state conditions for all chemical species whose concentrations are not specified. b) Determine the effect of precipitation of Fe(III) involved in the oxidation-reduction reaction on the cell potential obtained in a) by comparing it to the cell potential when iron(III) is in equilibrium with iron(III) hydroxide, Fe(OH)3. The solubility product constant for iron(III) hydroxide is 6x10-38.