question_answer

(I) \[{{H}_{2}}{{O}_{2}}\,+{{O}_{3}}\,\xrightarrow{\,}\,{{H}_{2}}O\,+2{{O}_{2}}\]

(II) \[{{H}_{2}}{{O}_{2}}+A{{g}_{2}}O\to 2Ag+{{H}_{2}}O+{{O}_{2}}\]

Role of hydrogen peroxide in the above reactions is respectively                                                   [AIPMT 2014]

A)  oxidising in (I) and reducing in (II)

B)  reducing in (I) and oxidizing in (II)

C)  reducing in (I) and (II)

D)  oxidising in (I) and (II)

Correct Answer: A

Solution :

In the reaction,

Since \[{{H}_{2}}{{O}_{2}}\] oxidises, \[{{O}_{3}}\] into\[{{O}_{2}}\], thus it behaves as an oxidising agent.

Further, in the reaction,

Here \[{{H}_{2}}{{O}_{2}}\] reduces \[A{{g}_{2}}O\] into metallic silver [Ag] (as oxidation number is reducing from +1 to 0). Thus, \[{{H}_{2}}{{O}_{2}}\] behaves as a reducing agent.