Question

19 gms molten SnCl2 is electrolysed for sometime using inert electrode until 0.119 gms is deposited during cathode No substance is lost during electrolysis .Find the ratio of masse of SnCl2 and SnCl4 after electrolysis?

Answer 1

Solution:
The chemical reaction occurring during electrolysis is 
 2SnCl2 →  SnCl4 + Sn 
2×190 g 261 g 119 g 

119 g of Sn is deposited by the decomposition of 380 g of SnCl2

So, 0.119 g of SnCl2 of Sn is deposited by the decomposition of 
380/119×0.119=0.380 g of SnCl2
Remaining amount of SnCl2 = (19-0.380) = 18.62 g 

380 g of SnCl2 produce = 261 g of SnCl4
So 0.380 g of SnCl2 produce = 261/380×0.380=0.261 g of SnCl 
Thus, the ratio SnCl2 : SnCl4 =18.2/0.261 , i.e., 71.34 : 1 
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