Copper sulphate solution is electrolysed betw | vedclass

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(A) The reaction at the anode is: $2H_2O \rightarrow O_2 + 4H^+ + 4e^-$. The equivalent mass of $O_2$ is $E_{O_2} = \frac{32}{4} = 8 \ g/eq$.Number of

Vedclass · Accepted Answer

$6.36$

Vedclass · Answer

(A) The reaction at the anode is: $2H_2O ightarrow O_2 + 4H^+ + 4e^-$. The equivalent mass of $O_2$ is $E_{O_2} = \frac{32}{4} = 8 \ g/eq$.Number of equivalents of $O_2$ liberated = $\frac{1.6 \ g}{8 \ g/eq} = 0.2 \ eq$.According to Faraday's law,the number of equivalents of $Cu$ deposited at the cathode must be equal to the number of equivalents of $O_2$ liberated at the anode.Number of equivalents of $Cu = 0.2 \ eq$.The equivalent mass of $Cu$ is $E_{Cu} = \frac{63.6}{2} = 31.8 \ g/eq$.Mass of $Cu$ deposited = $	ext{Number of equivalents} 	imes E_{Cu} = 0.2 	imes 31.8 = 6.36 \ g$.Therefore,the correct option is $A$.

Copper sulphate solution is electrolysed between two platinum electrodes. $A$ current is passed until $1.6 \ g$ of oxygen is liberated at the anode. The amount of copper deposited at the cathode during the same period is .............. $g$ [At. mass of $Cu = 63.6$]

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