Calculate the volume of $O_2$ gas liberated at the anode when a current of $2.5 \ A$ is passed for $1 \ hour$ through an aqueous solution of $Na_2SO_4$ using inert electrodes at $1 \ bar$ pressure and $300 \ K$ temperature. (Assume $1 \ mole$ of gas occupies $24.6 \ L$ at $1 \ bar$ and $300 \ K$) (in $mL$)
- A$573.93$
- B$286.96$
- C$1147.86$
- D$143.48$
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