5 A current is passed through AgNO_3 solutio | vedclass

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(C) The reaction for the deposition of silver is: $Ag^+ + e^- \rightarrow Ag(s)$.Here,$n = 1$.Theoretical mass of $Ag$ deposited $(w_{th})$ is calcula

Vedclass · Accepted Answer

$90$

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(C) The reaction for the deposition of silver is: $Ag^+ + e^- ightarrow Ag(s)$.Here,$n = 1$.Theoretical mass of $Ag$ deposited $(w_{th})$ is calculated using Faraday's law: $w_{th} = \frac{M \cdot I \cdot t}{n \cdot F}$.Substituting the values: $w_{th} = \frac{108 \cdot 5 \cdot 193}{1 \cdot 96500} = 1.08 \ g$.Current efficiency is given by the ratio of actual mass to theoretical mass: $	ext{Efficiency} = \frac{	ext{Actual mass}}{	ext{Theoretical mass}} 	imes 100$.Efficiency = $\frac{0.972}{1.08} 	imes 100 = 90 \%$.

$5 \ A$ current is passed through $AgNO_3$ solution for $193 \ s$. If $0.972 \ g$ of $Ag$ is deposited,calculate the current efficiency (cell capacity) of the electrolytic cell. $[Ag = 108 \ u]$ (in $\%$)

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