Question

$H_2{O}_2+H_2{O}_2\to 2H_{2}O+O_2$, is an example of disproportionation because:

• A. oxidation number of oxygen only decreases
• B. oxidation number of oxygen only increases
• C. oxidation number of oxygen decreases as well as increase
• D. oxidation number of oxygen neither decreases nor increases

Answer 1

Answer: (C)

oxidation number of oxygen decreases as well as increase

The reaction $H_2{O}_2+H_2{O}_2\to 2H_{2}O+O_2$, is an example of disproportionation (or auto oxidation reduction) reaction as the oxidation number of oxygen increases as well decreases.

The oxidation number of oxygen increases from $-1$ $($in $H_2{O}_2)$ to $0$ $($in $O_2)$ and decreases from $-1$ $($in $H_2{O}_2)$ to $-2$ $($in $H_{2}O)$.