A) action of \[{{H}_{2}}S{{O}_{4}}\]on barium peroxide
B) action of \[{{H}_{2}}S{{O}_{4}}\]on sodium peroxide
C) electrolysis of 50% \[{{H}_{2}}S{{O}_{4}}\]
D) burning hydrogen in excess of oxygen
Correct Answer: C
Solution :
[c] industrial preparation of \[{{H}_{2}}{{O}_{2}}:\] By the electrolysis of 50% \[{{H}_{2}}S{{O}_{4}}:\]50%\[{{H}_{2}}S{{O}_{4}}:\]solution is electrolyzed at \[0{}^\circ \]C between Pt electrodes. The perdisulphuric acid is formed. \[{{H}_{2}}S{{O}_{4}}\rightleftharpoons {{H}^{+}}+HS{{O}^{-}}_{4}\] At Anode: \[2HS{{O}^{-}}_{4}\to {{H}_{2}}{{S}_{2}}{{O}_{8}}+2e\] At Cathode: \[2{{H}^{+}}+2e\to {{H}_{2}}\] The obtained perdisulphuric acid gives \[{{H}_{2}}{{O}_{2}}\]on hydrolysis. \[{{H}_{2}}{{S}_{2}}{{O}_{8}}+2{{H}_{2}}O\rightleftharpoons {{H}_{2}}{{O}_{2}}+2{{H}_{2}}S{{O}_{4}}\] This \[{{H}_{2}}{{O}_{2}}\]is separated by distillation at reduced pressure and thus, 30% solution of \[{{H}_{2}}{{O}_{2}}\]is obtained.
You need to login to perform this action.
You will be redirected in
3 sec
