How much electricity is required in coulomb for the oxidation of
(i) 1 mol of `H_2O ` to `O_2` ?
(ii) 1 mol of FeO to `Fe_2O_3` ?

Explanation

(i) The electrode reaction for 1 mol of `H_(2)O` is represented as:
`H_(2)O to H_(2) + 1/2 O_(2)`
i.e., `O^(2-) to 1/2O_(2) + 2e^(-)`
`therefore` Quantity of electricity required = `2F= 2 xx 96500 C = 193000 C`
(ii) The electrode reaction for 1 mol of FeO is represented as:
`FeO to 1/2O_(2)`
i.e. `Fe^(2+) to Fe^(3+) +e^(-)`
`therefore` Quantity of electricity required = 1F = 96500 C