Chemistry - Redox Reactions Question with Solution | TestHub

$\stackrel{\left(0\right)}{3\mathrm{B}{\mathrm{r}}_2}+6\mathrm{O}{\mathrm{H}}^{-}\to 5\mathrm{B}{\mathrm{r}}^{-}+\mathrm{B}\mathrm{r}{\mathrm{O}}_3^{-}+3{\mathrm{H}}_2\mathrm{O}$
In this reaction, O.S. of bromine changes from (i) to 0 to -1 and (ii) 0 to +5. Hence,$\mathrm{B}{\mathrm{r}}_2$is reduced to$\mathrm{B}{\mathrm{r}}^{-}$and also oxidized to$\mathrm{B}\mathrm{r}{\mathrm{O}}_3^{-}$. Thus,$\mathrm{B}{\mathrm{r}}_2$is oxidised as well as reduced. In other words,$\mathrm{B}{\mathrm{r}}_2$undergoes disproportionation.