Electrolysis of an aqueous solution of copper sulphate using copper electrodes gives A. Copper at cathode and oxygen at anode B. Copper at anode and oxygen at cathode. C. Copper at cathode and anodes dissolve to give copper D. Hydrogen at cathode and oxygen at anode

The correct answer is: Copper at cathode and oxygen at anode.

When an aqueous solution of copper sulphate is electrolysed using copper electrodes, the following reaction occurs at the cathode:

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

This means that copper ions are reduced to copper metal at the cathode.

The following reaction occurs at the anode:

$2H_2O \to O_2 + 4H^+ + 4e^-$

This means that water is oxidised to oxygen gas and hydrogen ions at the anode.

The overall reaction is:

$Cu^{2+} + 2H_2O \to Cu + O_2 + 4H^+$

This reaction shows that copper is deposited at the cathode and oxygen gas is evolved at the anode.

The other options are incorrect because:

• Option B is incorrect because copper is deposited at the cathode, not the anode.
• Option C is incorrect because the anodes do not dissolve to give copper.
• Option D is incorrect because hydrogen gas is not produced at the cathode.