Question

On passing a current of 1.0 ampere for 16 min and
5 sec through one litre solution of CuCl₂, all copper
of the solution was deposited at cathode. The
strength of CuCl₂ solution was (Molar mass of
Cu = 63.5; Faraday constant = 96,500 Cmol⁻¹)
(a) 0.01 N (b) 0.01 M
(c) 0.02 M (d) 0.2 N

Answer 1

Answer:

b. willbe the correct answer

Explanation:

Mark the answer brainliests

Answer 2

Answer:

Normality of the solution is 0.01N

Explanation:

Given current, $I= 1.0 A$

          time,  $t= 16 min 5 sec=16\times60+5=965 s$

          Molar mass of Cu = 63.5

          Faraday constant $C= 96,500 Cmol^{-1}$

From Faraday's first law of electrolysis, the ratio of mass(W) to the equivalent weight(E) of the substance is

                                    $\frac{W}{E} =\frac{Q}{C}$

Charge is given by current times time, therefore

                                     $Q=It=1\times965=965C$

Therefore, $\frac{W}{E} =\frac{965}{96500}=0.01$

Normality is given by the number of equivalent weights to the volume of solution, i.e.,

                      $N=\frac{W/E}{V} =\frac{0.01}{1}=0.01N$    

Therefore, the normality of the solution is 0.01N