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
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B
False
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Solution

## 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. $\underset{\mathrm{Hydrogen}\mathrm{peroxide}}{2{\stackrel{+1}{\mathrm{H}}}_{2}{\stackrel{-1}{\mathrm{O}}}_{2}\left(\mathrm{aq}.\right)}\to \underset{\mathrm{Water}}{2{\stackrel{+1}{\mathrm{H}}}_{2}\stackrel{-2}{\mathrm{O}}\left(\mathrm{l}\right)}+\underset{\mathrm{Oxygen}}{{\stackrel{0}{\mathrm{O}}}_{2}\left(\mathrm{g}\right)}$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.

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