Question

On electrolysis of aqueous $CuS{O}_4$ with $Cu$ electrodes, the reduced $Cu$ gets deposited on:

• A. sides of the container
• B. negative terminal electrode
• C. half of positive terminal and half of negative terminal electrodes
• D. positive terminal electrode

Answer 1

The correct option is B negative terminal electrode

The process of using an electric current ​to drive a ​non-spontaneous​ chemical reaction is called electrolysis.
The electrolyte used can be in fused (or molten) state or in aqueous state. It should conduct electricity.

Electrolysis of $CuS{O}_4$ with $Cu$ electrode:
Two copper strips are dipped in an aqueous solution of $CuS{O}_4$ ​

When the DC voltage is applied,
At cathode: $C{u}^{2+}$ ions get discharged as $Cu$ atoms​
Reaction: $C{u}^{2+}+2e^{-}\to Cu$

At anode: $Cu$ atoms get dissolved as $C{u}^{2+}$ ions​
Reaction: $Cu\to C{u}^{2+}+2e^{-}$

Thus, $Cu$ is deposited at cathode.
Cathode is negative in electrolytic cell because it connects to the negative terminal of battery.
Hence, $Cu$ gets deposited at negative terminal electrode.