Question

Assertion(A): The decomposition of hydrogen peroxide to form water and oxygen is an example of disproportionation reaction.

Reason(R): The oxygen of peroxide is in $-1$ oxidation state and it is converted to zero oxidation state in $O_2$ and $-2$ oxidation states in $H_{2}O$.

• A. A is true but R is false
• B. Both A and R are false
• C. Both A and R are true and R is not the correct explanation of A
• D. Both A and R are true and R is the correct expalanation of A.

Answer 1

The correct option is D Both A and R are true and R is the correct expalanation of A.

Assertion:
Disproportionation reaction

Reactions in which same species undergo oxidation and reduction simultaneously are called disproportionation reaction.

$2H_2{O}_2\to 2H_{2}O+O_2$
Here, $H_2{O}_2$ is getting reduced to $H_{2}O$, as oxidation state of oxygen is decreasing from $-1$to $-2$, While $H_2{O}_2$ is also getting oxidized to $O_2$ as the oxidation state of oxygen is increasing from $-1$ to $0$.

Since, $H_2{O}_2$ is undergoing reduction and oxidation simultaneously , this reaction is an example for disproportionation reaction.


Reasons

$2H_2{O}_2\to 2H_{2}O+O_2$

In this reaction, the oxygen of peroxide is in $-1$ oxidation state and it is converted to zero oxidation state in $O_z$ and $-2$
oxidation in $H_{2}O$.

The given assertion and reason are correct and reason is the correct explanation for assertion.

Hence, the correct option is (A).