Redox Reactions and Electrochemistry: JEE Main 2026 Chemistry question

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 mg of Cu metal. However, a current of 600 mA was continued to pass through the same solution for another 28 minutes by keeping the total volume of the solution fixed at 200 mL. The total volume of oxygen evolved at STP during the entire process is ______ mL. (Nearest integer) [Given: $\mathrm{Cu^{2+}(aq) + 2e^- \rightarrow Cu(s)}$ $E^\circ_{red} = +0.34$ V; $\mathrm{O_2(g) + 4H^+ + 4e^- \rightarrow 2H_2O}$ $E^\circ_{red} = +1.23$ V; Molar mass of Cu = 63.54 g mol$^{-1}$; Molar mass of $\mathrm{O_2}$ = 32 g mol$^{-1}$; Faraday Constant = 96500 C mol$^{-1}$; Molar volume at STP = 22.4 L]