Question

In the electrolysis of $CuCl_{2}$ solution, the mass of cathode increased by $6.4g$ . What occurred at copper anode ?

• A. $0.224litre$ of $Cl_{2}$ was liberated
• B. $1.12litre$ of oxygen was liberated
• C. $0.05$ mole $Cu^{2 +}$ passed into the solution
• D. $0.1$ mole $Cu^{2 +}$ passed into the solution

Answer 1

Answer: (D)

$\left(CuCl\right)_{2}\left(\right.aq\left.\right)\rightleftharpoons\left(Cu\right)^{+ 2}+2\left(Cl\right)^{-}$

At both electrode $Cu$ will involve in the reaction
Thus $\left(g_{eq}\right)_{Anode }=\left(g_{eq}\right)_{Cathode }$
$\Rightarrow n\times 2=\frac{6 . 4}{64}\times 2$
$\Rightarrow n=0.1mole$ of $Cu^{+ 2}$ will form