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Question

19 g fused SnCl2 was electrolysed using inert electrodes. 0.119g Sn was deposited at cathode. If nothing was given out during electrolysis, calculate the ratio of mass of SnCl2 and SnCl4 in fused state after electrolysis.(Round off to nearest integer)

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Solution

The Redox changes during electrolysis of SnCl2 are:
Anode: 2ClCl2+2e
Cathode:Sn2++2eSn
Also Cl2 formed at anode reacts with SnCl2 to give SnCl4
SnCl2+2eSnCl4
Now Eq. of SnCl2 lost during elecrolysis = Eq. of Cl2 formed during electrolysis=Eq. of Sn formed during electrolysis
=0.1190.119/2=2×103
Eq. of SnCl4 formed = 2×103
Total loss in eq. of SnCl2 during complete course=Eq. of SnCl2 lost during electorlysis + Eq. of SnCl2 lost during reaction with Cl2
= 2×103+2×103=4×103
Initial eq. of SnCl2 =\frac { 19 }{ 190/2 } =2\times { 10 }^{ -1 }
Eq.of SnCl2 left in solution
=2×1014×103 =0.196.
Also Eq. of SnCl4 formed= 2×103=0.002
=MassofSnCl2leftMassofSnCl4formed=0.196×(190/2)0.002×(261/2)=71.34
Hence, the ratio of mass of SnCl2 and SnCl4 in fused state after electrolysis is 71.34.

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