How much time would it take in minutes to deposit 1.18 g of metallic copper on a metal object when a current of 2.0 A is passed through the electrolytic cell containing `Cu^(2+)` ions?
[Molar mass of `Cu = 63.5 g mol^(-1), 1F = 96,500 Cmol^(-1)]`

Explanation

`m = Z xx I xx t`
`1.18 = (63.5)/(2 xx 96500) xx 2 xx t`
`t = (1.18 xx 2 xx96500)/(2 xx 63.5)`
`= 1793.23` sec
`= (1793.23)/(60) = 29.88` min.