Three electrolytic cells A,B,C containing solutions of `ZnSO_(4),AgNO_(3) and CuSO_(4)`, passed through them until 1.45g of silver deposited at the cathode of cell B. How long did the current flow? What mass of copper and zinc were deposited?

Answer

`863.7s,0.426g of Cu, 0.438g Zn`

Explanation

`Ag^(o+)+e^(-) rarr Ag, i.e., 108g` of `Ag` are deposited by `1F=96500C`
`:. 1.45g of Ag` will be deposited by `(96500)/(108)xx1.45C`
`=1295.C`
`Q=Ixxt or t=Q//I=1295.6//1.50=863.7s=14 mi n 24s`
`Cu^(2+)+2e^(-) rarr Cu`
`i.e., 2xx96500C` deposits `Cu=63.5g`
`=(63.5)/(2xx96500)xx1295.6=0.426g`
`:. Zn` deposited `=(63.5)/(2xx96500)xx1295.6=0.438g`