A) \[{{H}_{2}}S\]
B) \[S{{O}_{3}}\]
C) \[{{H}_{2}}{{O}_{2}}\]
D) \[{{F}_{2}}\]
E) \[{{H}_{2}}S{{O}_{4}}\]
Correct Answer: C
Solution :
Hydrogen peroxide\[({{H}_{2}}{{O}_{2}})\]can act as an oxidising as well as a reducing agent. \[{{H}_{2}}{{O}_{2}}\]as a reducing agent: \[A{{g}_{2}}O+{{H}_{2}}{{O}_{2}}\xrightarrow[{}]{{}}2Ag+{{H}_{2}}O+{{O}_{2}}\] \[{{H}_{2}}{{O}_{2}}\]as a oxidising agent: \[PbS+4{{H}_{2}}{{O}_{2}}\xrightarrow{{}}PbS{{O}_{4}}+4{{H}_{2}}O\]
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