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(B) The aqueous solution of $K_2SO_4$ dissociates as: $K_2SO_4(aq) \rightarrow 2K^+(aq) + SO_4^{2-}(aq)$.Water also undergoes self-ionization: $H_2O(l

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$H_2, O_2$

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(B) The aqueous solution of $K_2SO_4$ dissociates as: $K_2SO_4(aq) \rightarrow 2K^+(aq) + SO_4^{2-}(aq)$.Water also undergoes self-ionization: $H_2O(l) \rightleftharpoons H^+(aq) + OH^-(aq)$.At the cathode,the reduction potential of $H^+$ is higher than that of $K^+$,so $H^+$ ions are reduced: $2H^+(aq) + 2e^- \rightarrow H_2(g)$.At the anode,the oxidation potential of $OH^-$ (or $H_2O$) is higher than that of $SO_4^{2-}$,so $H_2O$ is oxidized: $2H_2O(l) \rightarrow O_2(g) + 4H^+(aq) + 4e^-$.Therefore,$H_2$ gas is produced at the cathode and $O_2$ gas is produced at the anode.

The products obtained at the cathode and anode respectively during the electrolysis of aqueous $K_2SO_4$ solution using platinum electrodes are

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