How long will it take to produce 5.4 g of Ag | vedclass

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(B) The reaction for the deposition of $Ag$ is: $Ag^+ + e^- \rightarrow Ag(s)$.Here,$n = 1$ (number of electrons involved).Using Faraday's law of elec

Vedclass · Accepted Answer

$965$

Vedclass · Answer

(B) The reaction for the deposition of $Ag$ is: $Ag^+ + e^- ightarrow Ag(s)$.Here,$n = 1$ (number of electrons involved).Using Faraday's law of electrolysis: $W = \frac{M 	imes I 	imes t}{n 	imes F}$.Given: $W = 5.4 \ g$,$M = 108 \ g \ mol^{-1}$,$I = 5 \ A$,$F = 96500 \ C \ mol^{-1}$.Substituting the values: $5.4 = \frac{108 	imes 5 	imes t}{1 	imes 96500}$.$t = \frac{5.4 	imes 96500}{108 	imes 5}$.$t = \frac{521100}{540} = 965 \ s$.

How long will it take to produce $5.4 \ g$ of $Ag$ from molten $AgCl$ by passing $5 \ A$ current (in $s$)? (Molar mass $Ag = 108 \ g \ mol^{-1}$)

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