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(D) According to Faraday's laws of electrolysis,the mass $m$ of a substance deposited is given by $m = ZIt = \frac{E}{F} It$,where $E$ is the equivale

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$3.5$

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(D) According to Faraday's laws of electrolysis,the mass $m$ of a substance deposited is given by $m = ZIt = \frac{E}{F} It$,where $E$ is the equivalent weight and $F$ is Faraday's constant.Since the voltameters are connected in series,the charge $Q = It$ passed through both is the same.Therefore,the ratio of the masses deposited is equal to the ratio of their equivalent weights: $\frac{m_{Ag}}{m_{Zn}} = \frac{E_{Ag}}{E_{Zn}}$.Given $m_{Zn} = W$,we have $m_{Ag} = W 	imes \frac{E_{Ag}}{E_{Zn}}$.The equivalent weight of silver $(Ag)$ is approximately $108$ and the equivalent weight of zinc $(Zn)$ is approximately $\frac{65.4}{2} = 32.7$.Thus,$m_{Ag} = W 	imes \frac{108}{32.7} \approx 3.3 W$.Comparing this with the given options,the closest value is $3.5 W$.

$A$ silver and zinc voltameter are connected in series and a current $i$ is passed through them for a time $t$ liberating $W \, g$ of zinc. The weight of silver deposited is nearly ..............$W$.

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