19 g of molten `SuCl_(2)` is electrolysed for some time using inert electrodes until 0.119 g of Sn is deposited at the cathode. No substance is lost during electrolysis. Find the ratio of the masses of `SnCl_(2) : SnCl_(4)` after electrolysis.

Explanation

The chemical reaction occuring during electrolysis is :
`underset(2xx190 g)(2SnCl_(2)) rarr underset(261 g)(SnCl_(4))+underset(119 g)(Sn)`
119 g of Sn is deposited by the decomposition of 380 g of `SnCl_(2)`.
So, 0.119 g of Sn is deposited by the decomposition of
`380/119xx0.119=0.380 g` of `SnCl_(2)`
Remaining amount of `SnCl_(2)=(19-0.380)=18.62 g`
380 g of `SnCl_(2)` produce `=261 g` of `SnCl_(4)`
So, 0.380 g of `SnCl_(2)` produce `=261/380xx0.380=0.261 g` of `SnCl_(4)`
Thus, the ratio `SnCl_(2) : SnCl_(4)=18.62/0.261`, i.e., `71.34 : 1`