First slide

Hydrogen Peroxide

Question

Hydrogen peroxide is now generally prepared on industrial scale by the

Moderate

A

action of $H_{2} {SO}_{4}$ on barium peroxide
B

action of $H_{2} {SO}_{4}$ on sodium peroxide
C

electrolysis of 50% $H_{2} {SO}_{4}$
D

burning hydrogen in excess of oxygen

Solution

Industrial preparation of $H_{2} O_{2}$ :
(A) By the electrolysis of 50% $H_{2} {SO}_{4}$ : 50% $H_{2} {SO}_{4}$ solution is electrolyzed at $0^{0} C$ between Pt electrodes. The perdisulphuric acid is formed.
$H_{2} {SO}_{4} ⇌ H^{+} + {HSO}_{4}^{-}$
At Anode : $2 {HSO}_{4}^{-} ⇌ H_{2} S_{2} O_{8} + 2 e^{-}$
At Cathode: $2 H^{+} + 2 e^{-} \to H_{2}$
The obtained perdisulphuric acid gives $H_{2} O_{2}$ on hydrolysis.
$H_{2} S_{2} O_{8}^{} + 2 H_{2} O ⇌ H_{2} O_{2} + 2 H_{2} {SO}_{4}$
This $H_{2} O_{2}$ is separated by distillation at reduced pressure and thus, 30% solution of $H_{2} O_{2}$ is obtained.
(B) By the auto-oxidation of 2-ethyl-anthraquinol (Modern method): Anthraquinol, in a mixture of benzene and n-heptanol on treatment with air gives $H_{2} O_{2}$ and 2-ethyl-anthraquinone. This 2-ethyl-anthraquinone on hydrogenation gives 2-anthraquinol in presence of Pd catalyst.

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