Chemistry - Electrochemistry Question with Solution | TestHub

During electrolysis of an aqueous solution of Na₂SO₄, the following reactions occur at the electrodes:

Anode: $4O{H}^{-}⟶2H_{2}O+O_2+4e^{-}$

Cathode: $2H^{+}+2e^{-}⟶H_2$

Number of Faradays needed to liberate 1 mole of O₂ = 4.

Charge = $\frac{2.4\times 4}{22.4}F$

Number of moles of H₂ liberated by 1 F of charge =$1/2$.

Number of moles of H₂ = $\frac{2.4\times 4}{2\times 22.4}$.

Volume of H₂ at STP = $\frac{2.4\times 4\times 22.4}{2\times 22.4}=4.8L$