JEE Main 2026 — Electrochemistry Question with Solution

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: ${\mathrm{Cu}}^{2+}(\mathrm{aq})+2{\mathrm{e}}^{-}\to \mathrm{Cu}(\mathrm{s}){\mathrm{E}}_{\text{red }}^{\mathrm{o}}=+0.34\mathrm{V}$
${\mathrm{O}}_2(\mathrm{g})+4{\mathrm{H}}^{+}+4{\mathrm{e}}^{-}\to 2{\mathrm{H}}_2\mathrm{O}{\mathrm{E}}_{\text{red }}^{\mathrm{o}}=+1.23\mathrm{V}$
Molar mass of $\mathrm{Cu}=63.54\mathrm{g}{\mathrm{mol}}^{-1}$
Molar mass of ${\mathrm{O}}_2=32\mathrm{g}{\mathrm{mol}}^{-1}$
Faraday Constant $=96500\mathrm{C}{\mathrm{mol}}^{-1}$
Molar volume at $\mathrm{STP}=22.4\mathrm{L}$]