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;IF=96,500 Cmol^-1]

Explanation

m=Z xx I xx t
L .18=63.5/2 xx 96500 xx 2 x t
t=1.18 xx 2 xx 96500/2 xx 63.5=1793.23 sec
quad=1793.23/60=29.88 ~min
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