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In which of the following reactions H(2)...

In which of the following reactions `H_(2)O_(2)` acts as reducing agent?
(A) `H_(2)O_(2)+2H^(+)+2e^(-) to 2H_(2)O`
(B) `H_(2)O_(2)-2e^(-) to O_(2)+2H^(+)`
(C ). `H_(2)O_(2)+2e^(-) to 2OH^(-)`
(D) `H_(2)O_(2)+2OH^(-)-2e^(-) to O_(2)+2H_(2)O`

A

A,C

B

B,D

C

A,B

D

C,D

Text Solution

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The correct Answer is:
To determine in which of the given reactions \( H_2O_2 \) acts as a reducing agent, we need to analyze each reaction and identify the oxidation states of the elements involved, particularly focusing on the oxidation state of oxygen in \( H_2O_2 \). ### Step-by-Step Solution: 1. **Understanding Reducing Agents**: A reducing agent is a substance that donates electrons in a chemical reaction and is oxidized in the process. This means that the reducing agent itself undergoes an increase in oxidation state. 2. **Analyzing Each Reaction**: We will analyze the oxidation states of oxygen in \( H_2O_2 \) for each reaction. **(A)** \( H_2O_2 + 2H^+ + 2e^- \rightarrow 2H_2O \) - In \( H_2O_2 \), oxygen is in the -1 oxidation state. - In \( H_2O \), oxygen is in the -2 oxidation state. - Since oxygen goes from -1 to -2, \( H_2O_2 \) is reduced, and therefore, it acts as an oxidizing agent. **(B)** \( H_2O_2 - 2e^- \rightarrow O_2 + 2H^+ \) - In \( H_2O_2 \), oxygen is in the -1 oxidation state. - In \( O_2 \), oxygen is in the 0 oxidation state. - Since oxygen goes from -1 to 0, \( H_2O_2 \) is oxidized, and therefore, it acts as a reducing agent. **(C)** \( H_2O_2 + 2e^- \rightarrow 2OH^- \) - In \( H_2O_2 \), oxygen is in the -1 oxidation state. - In \( OH^- \), oxygen is in the -2 oxidation state. - Since oxygen goes from -1 to -2, \( H_2O_2 \) is reduced, and therefore, it acts as an oxidizing agent. **(D)** \( H_2O_2 + 2OH^- - 2e^- \rightarrow O_2 + 2H_2O \) - In \( H_2O_2 \), oxygen is in the -1 oxidation state. - In \( O_2 \), oxygen is in the 0 oxidation state. - Since oxygen goes from -1 to 0, \( H_2O_2 \) is oxidized, and therefore, it acts as a reducing agent. 3. **Conclusion**: From the analysis, \( H_2O_2 \) acts as a reducing agent in reactions (B) and (D). ### Final Answer: **(B) and (D)** are the reactions in which \( H_2O_2 \) acts as a reducing agent.
To determine in which of the given reactions \( H_2O_2 \) acts as a reducing agent, we need to analyze each reaction and identify the oxidation states of the elements involved, particularly focusing on the oxidation state of oxygen in \( H_2O_2 \). ### Step-by-Step Solution: 1. **Understanding Reducing Agents**: A reducing agent is a substance that donates electrons in a chemical reaction and is oxidized in the process. This means that the reducing agent itself undergoes an increase in oxidation state. 2. **Analyzing Each Reaction**: ...
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Knowledge Check

  • In which of the following reactions H_(2)O_(2) acts as a reducing agent?

    A
    I and II
    B
    III and IV
    C
    I and III
    D
    II and IV

  • In which of the following reactions, H_(2)O_(2) acts as a reducing agent?

    A
    `PbO_(2)(s)+H_(2)O_(2)(aq)toPbO(s)+H_(2)O(l)+O_(2)(g)`
    B
    `Na_(2)SO_(3)(aq)+H_(2)O_(2)(aq)toNa_(2)SO_(4)(aq)+H_(2)O(l)`
    C
    `2KI(aq)+H_(2)O_(2)(aq)to2KOH(aq)+I_(2)(s)`
    D
    `KNO_(2)(aq)+H_(2)O_(2)(aq)toKNO_(2)(aq)+H_(2)O(l)`

  • In which of the following reactions, H_(2)O_(2) acts as a reducing agent?

    A
    `PbO_(2(s))+H_(2)O_(2(aq))toPbO_((s))+H_(2)O_((l))+O_(2(g))`
    B
    `Na_(2)SO_(3(aq))+H_(2)O_(2(aq))toNa_(2)SO_(4(aq))+H_(2)O_((l))`
    C
    `2KI_((aq))+H_(2)O_(2(aq))to2KOH_((aq))+I_(2(s))`
    D
    `KNO_(2(aq))+H_(2)O_(2(aq))toKNO_(3(aq))+H_(2)O_((l))`

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