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(C) During the electrolysis of aqueous $H_2SO_4$ using $Pt$ electrodes,the following ions are present: $H^+$,$SO_4^{2-}$,and $OH^-$ (from water).At th

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$O_2$

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(C) During the electrolysis of aqueous $H_2SO_4$ using $Pt$ electrodes,the following ions are present: $H^+$,$SO_4^{2-}$,and $OH^-$ (from water).At the anode,oxidation occurs. The competing reactions are:$1$) $2H_2O(l) \rightarrow O_2(g) + 4H^+(aq) + 4e^-$,$E^o = +1.23 \ V$$2$) $2SO_4^{2-}(aq) \rightarrow S_2O_8^{2-}(aq) + 2e^-$,$E^o = +1.96 \ V$Since the oxidation potential of water is higher (or the reduction potential of $O_2$ is lower),water is preferentially oxidized at the anode.Therefore,$O_2$ gas is evolved at the anode.

The product obtained at the anode on electrolysis of aqueous $H_2SO_4$ in the presence of $Pt$ electrodes is:

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