Question

The reaction $2{H_2}{O_2} \to 2{H_2}O + {O_2}$ is:
a.) A redox reaction
b.) A hydrolysis reaction
c.) A solvolysis reaction
d.) Disproportionation.

Answer 1

Hint: In this question, we will be learning about the disproportionation reaction. What happens under this reaction and how to state that a reaction is under the disproportionation reaction.

Complete step by step answer:
$2{H_2}{O_2} \to 2{H_2}O + {O_2}$ is a disproportionation reaction wherein the oxygen goes through oxidation and decreases all the while. The correct answer is option “D” .

Additional Information :
What is the disproportionation reaction?
In a disproportionation response, a similar element is all the while oxidized and reduced.
Definition:
The responses wherein single reactant is oxidized and decreased is known as Disproportionation responses
The disproportionation response is given beneath
$2{H_2}O \to 2{H_2}O + {O_2}$
is likewise a disproportionation response since O is decreased in framing ${H_2}O$ and oxidized in shaping ${O_2}$
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 What are oxidation and reduction reactions?
An oxidation-reduction (redox) reaction is a sort of chemical reaction that includes an exchange of electrons between two species. An oxidation-reduction reaction is any compound response where the oxidation number of a particle, molecule, or particle changes by picking up or losing an electron. Redox responses are normal and fundamental to a portion of the essential elements of life, including photosynthesis, breath, burning, and erosion or rusting.
- Oxidation is the addition of oxygen.
- Reduction is the loss of oxygen.


Note: Redox responses include two sections, a reduced half and an oxidized half, that consistently happen together. The reduced half picks up electrons and the oxidation number decreases, while the oxidized half loses electrons and the oxidation number increments. Straightforward approaches to recall this incorporate the memory helpers OIL RIG, signifying "oxidation is shortfall" and "decrease is increase," and LEO says GER, signifying "loss of e-= oxidation" and "addition of e-= reduced." There is no net change in the quantity of electrons in a redox response. Those emitted in the oxidation half response are taken up by another species in the decreased half response.