Chemistry - Redox Reactions Question with Solution | TestHub

In the given reaction, bromine ($B{r}_2$) undergoes disproportionation, meaning it is both oxidized and reduced. To find the equivalent weight of $B{r}_2$, we need to consider the change in oxidation state. $B{r}_2$ is converted to $B{r}^{-}$ and $Br{O}_3^{-}$. The change in oxidation number helps determine the n-factor. The equivalent weight is then calculated as $EquivalentWeight=\frac{MolecularWeight}{n-factor}$. In this specific reaction, the n-factor for $B{r}_2$ is $\frac{5}{3}$, so the equivalent weight of $B{r}_2$ is $\frac{3M}{5}$.