Chemistry Question from JEE Main 2026 · 24 January, Shift 1

Electricity is passed through an acidic solution of $\mathrm{Cu}^{2+}$ till all the $\mathrm{Cu}^{2+}$ was exhausted, leading to the deposition of $300 \, \text{mg}$ of Cu metal. However, a current of $600 \, \text{mA}$ was continued to pass through the same solution for another $28 \, \text{minutes}$ by keeping the total volume of the solution fixed at $200 \, \text{mL}$. The total volume of oxygen evolved at STP during the entire process is _____ $\text{mL}$. (Nearest integer)

Given: $\mathrm{Cu}^{2+} + 2e^- \rightarrow \mathrm{Cu}(s)$ $\mathrm{O_2} + 4H^+ + 4e^- \rightarrow 2H_2O$

Molar mass of $\mathrm{Cu}$ = $63.54 \, \text{g mol}^{-1}$

Faraday constant = $96500 \, \text{C mol}^{-1}$

Molar volume at STP = $22.4 \, \text{L}$