How much electricity is required in coulomb for the oxidation of(i) 1 mol of H2O to O2?(ii) 1 mol of FeO to Fe2O3?

(i) The oxidation of 1 mol of H2O to O2 involves the following reaction:

2H2O → O2 + 4H+ + 4e-

This means that 4 moles of electrons are required for the oxidation of 2 moles of water. Therefore, for 1 mole of water, 2 moles of electrons are required.

The charge of 1 mole of electrons (also known as the Faraday constant) is approximately 96485.3 Coulombs. Therefore, the amount of electricity required for the oxidation of 1 mole of water is 2 * 96485.3 = 192970.6 Coulombs.

(ii) The oxidation of 1 mol of FeO to Fe2O3 involves the following reaction:

4FeO → 2Fe2O3 + 2e-

This means that 2 moles of electrons are required for the oxidation of 4 moles of FeO. Therefore, for 1 mole of FeO, 0.5 moles of electrons are required.

Again, using the Faraday constant, the amount of electricity required for the oxidation of 1 mole of FeO is 0.5 * 96485.3 = 48242.65 Coulombs.