Question

Electrolysis of $50\%H_{2}S{O}_4$ produces:

• A. $H_2{S}_2{O}_8$ at anode
• B. $H_2$ at anode
• C. $H_{2}S{O}_5$ at cathode
• D. $H_2{O}_2$ at anode

Answer 1

The correct option is A $H_2{S}_2{O}_8$ at anode

Hydrogen peroxide can be produced by electrolysis of sulfuric acid. At the anode the following reaction takes place:
$H_{2}S{O}_4^{-}\to S_2{O}_8^{2-}+2H^{+}+2e^{-}$
The reaction of this ion with water serves as a commercial preparation of hydrogen peroxide:
$S_2{O}_8^{2-}(aq.)+H_{2}O\to H_2{O}_2(aq.)+2HS{O}_4^{-}$.