A metal plate of dimension (1 times 2 cm^2) | vedclass

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(B) Step $I$: Calculate the total volume of $Cu$ to be deposited.$V = 	ext{Area} 	imes 	ext{thickness} 	imes 2 	ext{ (for both sides)}$$V = (1

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$800$

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(B) Step $I$: Calculate the total volume of $Cu$ to be deposited.$V = 	ext{Area} 	imes 	ext{thickness} 	imes 2 	ext{ (for both sides)}$$V = (1 	imes 2 \ cm^2) 	imes 0.01 \ cm 	imes 2 = 0.04 \ cm^3$Step $II$: Calculate the mass of $Cu$ deposited.$m = 	ext{Volume} 	imes 	ext{Density}$$m = 0.04 \ cm^3 	imes 9 \ g/cm^3 = 0.36 \ g$Step $III$: Use Faraday's law of electrolysis to find time $t$.$m = Z 	imes i 	imes t$$0.36 \ g = 0.0003 \ g/C 	imes 1.5 \ A 	imes t$$t = \frac{0.36}{0.0003 	imes 1.5} = \frac{0.36}{0.00045} = 800 \ s$

$A$ metal plate of dimension $(1 \times 2 \ cm^2)$ has to be coated on both sides by $Cu$ metal. How long does it take to deposit $Cu$ of $0.01 \ cm$ thickness,if $1.5 \ A$ current is used (in $s$)? [Electrochemical equivalence of $Cu$ is $0.0003 \ g/C$ and the density of $Cu$ is $9 \ g/cm^3$]

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