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(C) Step $1$: Calculate the volume of the nickel layer.Volume = Area $	imes$ thickness = $100 \, cm^2 	imes 0.0001 \, cm = 0.01 \, cm^3$.Step $2$: C

Vedclass · Accepted Answer

$161$

Vedclass · Answer

(C) Step $1$: Calculate the volume of the nickel layer.Volume = Area $	imes$ thickness = $100 \, cm^2 	imes 0.0001 \, cm = 0.01 \, cm^3$.Step $2$: Calculate the mass of nickel required.Mass = Density $	imes$ Volume = $10 \, g \cdot cm^{-3} 	imes 0.01 \, cm^3 = 0.1 \, g$.Step $3$: Use Faraday's law of electrolysis: $W = \frac{M 	imes I 	imes t}{n 	imes F}$.Here,$W = 0.1 \, g$,$M = 60 \, g \cdot mol^{-1}$,$I = 2 \, A$,$n = 2$ (for $Ni^{2+} + 2e^- ightarrow Ni$),$F = 96500 \, C \cdot mol^{-1}$.Step $4$: Solve for $t$ (which is $x$):$0.1 = \frac{60 	imes 2 	imes x}{2 	imes 96500}$.$0.1 = \frac{60 	imes x}{96500}$.$x = \frac{0.1 	imes 96500}{60} = \frac{9650}{60} \approx 160.83 \, s$.Rounding to the nearest integer,$x = 161$.

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