The approximate ratio of $A g, A l, C u$ deposited at the electrodes when these electrolytic cells are connected in series is :

6 : 2 : 3

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12 : 1 : 3.5

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4 : 1 : 2.4

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12 : 1 : 7

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Solution

The correct option is A $6 : 2 : 3$
The reaction equations are
$A g^{+} + e^{-} \to A g$
$A l^{3 +} + 3 e^{-} \to A l$
$C u^{2 +} + 2 e^{-} \to C u$
From the stoichiometry of these equations, one mole of electrons would deposit $1 m o l e$ of $A g$ in the electrolysis. As the cells are in series, the same current flows through all three cells and one mole of electrons would produce $\frac{1}{3} m o l e$ of $A l$ and $\frac{1}{2} m o l e$ of $C u$ from their solutions respectively. The ratio would be $A g : A l : C u = 1 : 1 / 3 : 1 / 2$ = $6 : 2 : 3$

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The approximate ratio of Ag,Al,Cu deposited at the electrodes when these electrolytic cells are connected in series is :

The approximate ratio of $A g, A l, C u$ deposited at the electrodes when these electrolytic cells are connected in series is :