19 g of molten `SnCl_(2)` is electrolysed for same tine, using inert electrodes. 0.119 g of Sn is deposited at the cathode. No substance is lost during the electrolysis. Find the ratio of the weight of `SnCl_(2)` and `SnCl_(2)` after electrolysis (Sn = 119)

Explanation

To solve the problem, we need to find the ratio of the weight of `SnCl2` before and after electrolysis. Here’s a step-by-step breakdown of the solution:

### Step 1: Calculate the molar mass of `SnCl2`
The molar mass of `SnCl2` can be calculated as follows:
- Atomic mass of Sn = 119 g/mol
- Atomic mass of Cl = 35.5 g/mol
- Therefore, molar mass of `SnCl2` = 119 + 2(35.5) = 119 + 71 = 190 g/mol

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