The balanced chemical equation for the oxidation of PbS by ozone is:
\(\text{PbS} + 4\text{O}_3 \rightarrow \text{PbSO}_4 + 4\text{O}_2\)
From the equation:
- 1 mole of PbS reacts with 4 moles of \( \text{O}_3 \), so \( X = 4 \).
- 4 moles of \( \text{O}_2 \) are produced, so \( Y = 4 \).
Therefore:
\(X + Y = 4 + 4 = 8\)
The Correct answer is: 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