question_answer

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

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

Role of hydrogen peroxide in the above reactions is respectively

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

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

C)  reducing in (I) and (II)

D)  oxidizing 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.