Assertion: Decomposition of hydrogen peroxide is an example of disproportionation reaction. Reason: In a disproportionation reaction, an element in one oxidation state is simultaneously oxidised and reduced.

Question

Assertion: Decomposition of hydrogen peroxide is an example of disproportionation reaction. Reason: In a disproportionation reaction, an element in one oxidation state is simultaneously oxidised and reduced. (A) If both assertion and reason are true and reason is the correct explanation of assertion. (B) If both assertion and reason are true but reason is not the correct explanation of assertion. (C) If assertion is true but reason is false. (D) If both assertion and reason are false.

Tardigrade Admin · Accepted Answer

The oxidation states are overset+1-12 H 2 O 2 (aq) arrow overset+1-22 H 2 O(l) + overset0O 2(g) Oxidation State of Oxygen of peroxide increases to o from -1 in O 2 and decreases to -2 in H 2 O..

Q. Assertion: Decomposition of hydrogen peroxide is an example of disproportionation reaction.
Reason : In a disproportionation reaction, an element in one oxidation state is simultaneously oxidised and reduced.

If both assertion and reason are true and reason is the correct explanation of assertion.

If both assertion and reason are true but reason is not the correct explanation of assertion.

If assertion is true but reason is false.

If both assertion and reason are false.

The oxidation states are
$2 H_{2} O_{2} (a q) + 1 - 1 \to 2 H_{2} O_{(l)} + 1 - 2 + O_{2} (g) 0$
Oxidation State of Oxygen of peroxide increases to o from $- 1$ in $O_{2}$ and decreases to $- 2$ in $H_{2} O$ ..

Q. Assertion: Decomposition of hydrogen peroxide is an example of disproportionation reaction. Reason : In a disproportionation reaction, an element in one oxidation state is simultaneously oxidised and reduced.