Three electrolytic cells `A, B, C` containing solutions of `ZnSO_4, AgNO_3` and `CuSO_4`, respectively are connected in series. A steady current of `1.5` amperes was passed through them until `1.45 g` of silver deposited at the cathode of cell B. How long did the current flow? What mass of copper and zinc were deposited?

Explanation

Atomic mass of `C u=63.5 . Z n=65.3 . A g doteq` 108,
`Ag^*+e^- Ag`
ie. `108 ~g` of `Ag` are deposited by `IF=96.500 C` `therefore 1.45 ~g` of. `Ag` will be deposited by `96,500/108 xx 1.45 C=1295.6 C_1: Q=1 xx t`
or `t=Q/1=1295.6/1.5=863.75=14 ~mm .24 sec`
Now `Cu^2++2 e^- Cu`
ie. `2 xx 96.500` deposif `Cu=63.5`
will deposit `Cu=therefore 63.5+/2 xx 96,500 xx 1295.6`
`=0.426 ~g`
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