Electrochemistry - Result Question 25
####27. On passing a current of 1.0 ampere for $16 min$ and $5 sec$ through one litre solution of $CuCl_2$, all copper of the solution was deposited at cathode. The strength of $CuCl_2$ solution was (Molar mass of $Cu=63.5 ;$ Faraday constant $=96,500 Cmol^{-1}$ )
[1996]
(a) $0.01 N$
(b) $0.01 M$
(c) $0.02 M$
(d) $0.2 N$
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Solution:
- (a) By Faraday’s Ist Law, $\frac{W}{E}=\frac{q}{96500}$ (where $q=it=$ total electric charge) we know that no of equivalent
$=\frac{W}{E}=\frac{i t}{96500}=\frac{1 \times 965}{96500}=\frac{1}{100}$
(where $i=1 A, t=16 \times 60+5=965 sec$.)
Since, we know that
Normality $=\frac{\text{ no. of equivalent }}{\text{ Volume (in litre) }}=\frac{\frac{1}{100}}{1}=0.01 N$
