The reaction involved is:
\[2\text{NH}_4\text{Cl} + \text{MnO}_2 + 2\text{H}_2\text{SO}_4 \xrightarrow{\Delta} \text{MnSO}_4 + (\text{NH}_4)_2\text{SO}_4 + 2\text{H}_2\text{O} + \text{Cl}_2 \uparrow\]
In this reaction, chlorine gas (\( \text{Cl}_2 \)) is liberated, which has a greenish-yellow color.
$\mathrm{KMnO}_{4}$ 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