A solution of copper sulphate $\left(\mathrm{CuSO}_4\right)$ is electrolysed for $10$ minutes with a current…

A solution of copper sulphate $\left(\mathrm{CuSO}_4\right)$ is electrolysed for $10$ minutes with a current of $1.5$ amperes. The mass of copper deposited at the cathode (at. mass of $\mathrm{Cu}=63 \mathrm{u}$ ) is :
  1. $0.3892 \mathrm{~g}$
  2. $0.2938 \mathrm{~g}$
  3. $0.2398 \mathrm{~g}$
  4. $0.3928 \mathrm{~g}$

Solution

$\mathrm{W}=\mathrm{Zit}$ where $\mathrm{Z}$ = Electrochemical equivalent Eq. wt. of copper $=\frac{63}{2}=31.5$ $\begin{aligned} & \mathrm{Z}=\frac{31.5}{96500} \\ & \mathrm{~W}=\mathrm{Zit}=\frac{31.5}{96500} \times 1.5 \times 10 \times 60=0.2938 \mathrm{~g} \end{aligned}$

Asked in: JEE Main 2013 (25 Apr Online)

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