Question

For ${H_2}{O_2}$ is:
A.An oxidising agent
B.Both oxidising and reducing agent
C.Reducing agent
D.None of the above

Answer 1

Firstly we have to mention the fact regarding the reducing / oxidising nature of the ${H_2}{O_2}$ . Then we have to mention the change regarding the oxidising state and then finally the reactions like ${H_2}{O_2} + 2{H^ + } + 2{e^ + } \to 2{H_2}O$ that would state the fact.

Complete step by step answer:
For the case of oxidising agents.
Whenever in any reaction, ${H_2}{O_2}$ acts as an oxidizing agent, there would be a change in the evident oxidising state of the oxygen atom of the compound. In the change, the oxidation state of the oxygen of hydrogen peroxide will get reduced from $- 1$ to $- 2$ .
The reaction for the given chemical change would be :
${H_2}{O_2} + 2{H^ + } + 2{e^ + } \to 2{H_2}O$
Now for the case of the reducing agent.
Whenever in any reaction, ${H_2}{O_2}$ acts as an reducing agent, there would be a change in the evident oxidising state of the oxygen atom of the compound. In the change, the oxidation state of the oxygen of hydrogen peroxide will get reduced from $- 1$ to $0$ .
The reaction for the given chemical change would be :
$2KMn{O_4} + 5{H_2}{O_2} + 3{H_2}S{O_4} \to {K_2}S{O_4} + 5{O_2} + 2MnS{O_4} + 8{H_2}O$
So we can say that the hydrogen peroxide would act both as a reducing and oxidising agent as per the requirements.
Therefore the option B, both oxidising and reducing agent.

Note:
In its pure form, it is a very pale blue liquid, slightly more viscous than water. Hydrogen peroxide is the simplest peroxide (a compound with an oxygen–oxygen single bond). It is used as an oxidizer, bleaching agent, and antiseptic. Concentrated hydrogen peroxide, or "high-test peroxide", is a reactive oxygen species.