Question

$2{\mathrm{H}}_2{\mathrm{O}}_2\to 2{\mathrm{H}}_2\mathrm{O}+{\mathrm{O}}_2$ is an example of a disproportionation reaction.

• A. True
• B. False

Answer 1

The correct option is A True

$2{\mathrm{H}}_2{\mathrm{O}}_2\to 2{\mathrm{H}}_2\mathrm{O}+{\mathrm{O}}_2$ is an example of a disproportionation reaction.

Disproportionation reactions: “In a disproportionation reaction an element in one oxidation state is simultaneously oxidized and reduced”.

Oxygen experiences a disproportionation reaction in the decomposition of hydrogen peroxide.
$\underset{\mathrm{Hydrogen}\mathrm{peroxide}}{2{\stackrel{+1}{\mathrm{H}}}_2{\stackrel{-1}{\mathrm{O}}}_2(\mathrm{aq}.)}\to \underset{\mathrm{Water}}{2{\stackrel{+1}{\mathrm{H}}}_2\stackrel{-2}{\mathrm{O}}\left(\mathrm{l}\right)}+\underset{\mathrm{Oxygen}}{{\stackrel{0}{\mathrm{O}}}_2\left(\mathrm{g}\right)}$

Here

The oxidation state of the oxygen present in peroxide is –1.

The oxidation state of oxygen present in the product is 0.

The oxidation state of oxygen present in ${\mathrm{H}}_2\mathrm{O}$. is –2

Thus, the given statement is true.