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When an aqueous solution of copper sulphate is electrolysed using copper electrodes the reaction at the anode is represented by

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${Cu}^{2 +} + 2 e^{-} \to Cu$

${Cu}_{(s)} \to {Cu}^{2 +}_{(aq)} + 2 e^{-}$

${SO}_{4}^{2 -} (aq) \to {SO}_{4} + 2 e^{-}$

$H^{+} + e^{-} \to H$

answer is D.

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Detailed Solution

Cupper electrode is an attacking electrode , so the reactions are

Anode: ${Cu}_{(s)} \to {Cu}_{(aq)}^{2 +} + 2 e^{-}$

Cathode : ${Cu}_{(aq)}^{2 +} + 2 e^{-} \to {Cu}_{(s)}$

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