(C) The balanced chemical equation for the oxidation of $PbS$ by $O_3$ is:$PbS + 4 O_3 \rightarrow PbSO_4 + 4 O_2$From the balanced equation,we can se

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(C) The balanced chemical equation for the oxidation of $PbS$ by $O_3$ is:$PbS + 4 O_3 \rightarrow PbSO_4 + 4 O_2$From the balanced equation,we can see that $1$ mole of $PbS$ reacts with $4$ moles of $O_3$ to produce $4$ moles of $O_2$.Therefore,$X = 4$ and $Y = 4$.The value of $X + Y = 4 + 4 = 8$.

Class 11 Chemistry Redox Reactions Redox reaction and Method for balancing Redox reaction

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$1$ mole of $PbS$ is oxidised by "$X$" moles of $O_3$ to get "$Y$" moles of $O_2$. $X + Y = $ . . . . . . .

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A
$4$
B
$3$
C
$8$
D
$7$

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Redox reaction and Method for balancing Redox reaction

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$1$ mole of $PbS$ is oxidised by "$X$" moles of $O_3$ to get "$Y$" moles of $O_2$. $X + Y = $ . . . . . . .

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