1. Tardigrade
  2. Question
  3. Chemistry
  4. 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 C mol -1 )

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Q. 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 $=96,500\, C\,mol ^{-1}$ )

BITSATBITSAT 2018

Solution:

By Faraday's $I^{s t}$ Law, $\frac{W}{E}=\frac{q}{96500}$
(where $q=$ it $=$ charge of ion)
$=\frac{W}{E}=\frac{i t}{69500}=\frac{1 \times 965}{96500}=\frac{1}{100}$
(where $i=1 A, t=16 \times 60+5=965$ sec.)
Since, we know that
Normality $=\frac{\text { no- of equivalent }}{\text { Volume (in litre) }}$
$=\frac{\frac{1}{100}}{1}=0.01 \,N$