The mass of copper that will be deposited at cathode in electrolysis of 0.2 M solution of copper sulphate when a quantity of electricity equal to that required to liberate 2.24 L of hydrogen from 0.1 M aqueous H2SO4 is passed (At. mass of Cu= 63.5) will be

Question

The mass of copper that will be deposited at cathode in electrolysis of 0.2 M solution of copper sulphate when a quantity of electricity equal to that required to liberate 2.24 L of hydrogen from 0.1 M aqueous H2SO4 is passed (At. mass of Cu= 63.5) will be (A) 1.59 g (B) 3.18 g (C) 6.35 g (D) 12.70 g

Tardigrade Admin · Accepted Answer

Wt. of substance liberated at electrodes are in ratio of their equivalent weights. ∴ (WCu/WH) = (ECu/EH) ⇒ WCu = (63.5/2) × (2.24/22.4) × (2/1) = 6.35 g

Q. The mass of copper that will be deposited at cathode in electrolysis of 0.2 M solution of copper sulphate when a quantity of electricity equal to that required to liberate 2.24 L of hydrogen from 0.1 M aqueous $H_{2} S O_{4}$ is passed (At. mass of Cu= 63.5) will be

1.59 g

3.18 g

6.35 g

12.70 g

Wt. of substance liberated at electrodes are in ratio of their equivalent weights.
$∴ \frac{W _{C u}}{W _{H}} = \frac{E _{C u}}{E _{H}}$
$\Rightarrow W_{C u} = \frac{63.5}{2} \times \frac{2.24}{22.4} \times \frac{2}{1}$
$= 6.35 g$

Q. The mass of copper that will be deposited at cathode in electrolysis of 0.2 M solution of copper sulphate when a quantity of electricity equal to that required to liberate 2.24 L of hydrogen from 0.1 M aqueous H2​SO4​ is passed (At. mass of Cu= 63.5) will be