This question tests the understanding of Faraday's laws of electrolysis and the stoichiometry of electrode reactions. The key principle is that the amount of electricity required depends on the number of electrons transferred in the oxidation reaction. From the context, we know that charge on one electron is $1.6021 \times 10$⁻¹⁹ C, and one mole of electrons (1 Faraday) equals approximately 96500 C. For each reaction, we must first write the balanced oxidation half-reaction and determine the number of moles of electrons involved per mole of substance oxidized.