In the electrolysis of $\mathrm{CuCl}_{2}$ solution, the mass of the cathode increased by $3.2 \mathrm{~g}$.…

In the electrolysis of $\mathrm{CuCl}_{2}$ solution, the mass of the cathode increased by $3.2 \mathrm{~g}$. What occured at the copper anode?
  1. $0.12$ litre of $\mathrm{Cl}_{2}$ was liberated
  2. $0.56$ litre of $\mathrm{O}_{2}$ was liberated
  3. $0.1 \mathrm{~mol} \mathrm{Cu}^{2+}$ passed into the solution.
  4. $0.05 \mathrm{~mol}$ of $\mathrm{Cu}^{2+}$ passed into the solution.

Solution

The amount. of copper deposited at cathode by reduction of $\mathrm{Cu}^{2+}$ ions is $\frac{3.2}{63}=0.05$ moles.
The same amount $0.05$ mole of $\mathrm{Cu}^{2+}$ must pass into solution from anode by oxidation

Asked in: JEE-TOPICTESTS-CHEMISTRY

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