How much electricity is required in coulomb for the oxidation of :
(a) `1` mol of `H_(2)O` to `O_(2)`,
(b) `1` mole of `FeO` to `Fe_(2)O_(3)` ?

Explanation

(i). The electrode reaction for 1 mol of `H_(2)O` is
`H_(2)OtoH_(2)+(1)/(2)O_(2)`
i.e., `O^(2-)to(1)/(2)O_(2)+2e^(-)`
`therefore` Quantity of electricity required
`=2F=2xx96500C=193000C`.
(ii). The electrode reaction for 1 mol of FeO is
`FeO+(1)/(2)O_(2)to(1)/(2)Fe_(2)O_(3)`
i.e., `Fe^(2+)toFe^(3+)+e^(-)`
`therefore` Quantity of electricity required `=1F=96500C`.