$19 g$ of molten $S n C l_{2}$ is electrolysed for some time using inert electrodes until $0.119 g$ of $S n$ is deposited at the cathode. No substance is lost during electrolysis. Find the ratio of the masses of $S n C l_{2} : S n C l_{4}$ after electrolysis.

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Solution

The chemical reaction occurring during electrolysis is:
$2 S n C l_{2} 2 \times 190 g \to S n C l_{4} 261 g + S n 119 g$
$119 g$ of $S n$ is deposited by the decomposition of $380 g$ of $S n C l_{2}$ .
So, $0.119 g$ of $S n$ is deposited by the decomposition of
$\frac{380}{119} \times 0.119 = - .380 g$ of $S n C l_{2}$
Remaining amount of $S n C l_{2} = (19 - 0.380) = 18.62 g$
$380 g$ of $S n C l_{2}$ produce $= 261 g$ of $S n C l_{4}$
So, $0.380 g$ of $S n C l_{2}$ produce $= \frac{261}{380} \times 0.380 = 0.261 g$ of $S n C l_{4}$
Thus, the ratio $S n C l_{2} : S n C l_{4} = \frac{18.62}{0.261}$ , i.e., $71.34 : 1$ .

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