A copper strip having $3 c m$ length and $4 c m$ breadth is coated with silver of $2 m m$ thickness.
Calculate the quantity of electricity (in coloumb) required for the above process.
(Density of $A g = 10.5$ g cm $^{- 3})$ .

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Solution

amount of silver deposited:
$m = d e n s i t y \times v o l u m e$
Volume of silver sheet deposited:
$V = l \times b \times t$
Given: $l = 3 c m, b = 4 c m, t = 2 m m = 0.2 c m$
$V = 3 \times 4 \times 0.2 = 2.4 c m^{3}$
Given density of silver $= 10.5 g / c m^{3}$
$∴ m = 0.24 \times 10.5 = 2.52 g$
Reaction involved is $A g^{+} + e^{-} \to A g$
Atomic wt of $A g$ is $108 g / m o l$
Using the relation:
$m = Z Q$
where $Z = 108 / F, m = 2.52 g$
amount of electricity passed/required is:
$Q = m / Z$
$Q = 2252 C$

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