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  4. Three electrolytic cells A, B, C containing solutions of ZnSO4, AgNO3 and CuSO4, 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?

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Q. 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?

Electrochemistry

Solution:

$I = 1.5 \,A, W = 1.45 \,g\, Ag, t = ?, E = 108, n = 1$
Using Faraday’s $1^{st}$ law of electrolysis $W = ZIt$
or, $W = \frac{E}{F} It$
or, $1.45 \,g = \frac{108}{96500} \times 1.5\,t$
or, $t = \frac{1.45 \times 96500}{1.5 \times 108}$
$ = 863.73$ seconds