(I)\[{{H}_{2}}{{O}_{2}}+{{O}_{3}}\xrightarrow{{}}{{H}_{2}}O+2{{O}_{2}}\] |
(II)\[{{H}_{2}}{{O}_{2}}+A{{g}_{2}}O\xrightarrow{{}}2Ag+{{H}_{2}}O+{{O}_{2}}\] |
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.You need to login to perform this action.
You will be redirected in
3 sec