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  3. Chemistry
  4. 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

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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 $H_2SO_4$ is passed (At. mass of Cu= 63.5) will be

Electrochemistry

Solution:

Wt. of substance liberated at electrodes are in ratio of their equivalent weights.
$\therefore \frac{W_{Cu}}{W_H} = \frac{E_{Cu}}{E_H}$
$\Rightarrow W_{Cu} = \frac{63.5}{2} \times \frac{2.24}{22.4} \times \frac{2}{1}$
$ = 6.35\,g$