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

(a) The oxidation reaction is :
`underset("1 mole")(H_(2)O) rarr 1/2 O_(2) +2H^(+) + underset("2 mole")(2e^(-))`
`Q=2xxF`
`=2xx96500=193000` coulomb
(b) The oxidation reaction is :
`FeO+1/2 H_(2)O rarr 1/2 Fe_(2)O_(3) +H^(+) +e^(-)`
`Q=F=96500` coulomb