Reduction Half Reaction:
\[ 2\text{MnO}_4^- \rightarrow 2\text{MnO}_2 \] \[ 2\text{MnO}_4^- + 4\text{H}_2\text{O} + 6e^- \rightarrow 2\text{MnO}_2 + 8\text{OH}^- \]
Oxidation Half Reaction:
\[ 2\text{I}^- \rightarrow \text{I}_2 + 2e^- \] \[ 6\text{I}^- \rightarrow 3\text{I}_2 + 6e^- \]
Adding the oxidation half and reduction half, we get the net reaction as:
\[ 2\text{MnO}_4^- + 6\text{I}^- + 4\text{H}_2\text{O} \rightarrow 3\text{I}_2 + 2\text{MnO}_2 + 8\text{OH}^- \]
Thus, \( z = 8 \).
$\mathrm{KMnO}_{4}$ acts as an oxidising agent in acidic medium. ' X ' is the difference between the oxidation states of Mn in reactant and product. ' Y ' is the number of ' d ' electrons present in the brown red precipitate formed at the end of the acetate ion test with neutral ferric chloride. The value of $\mathrm{X}+\mathrm{Y}$ is _______ .
Match List-I with List-II: List-I