The weight of $Z n S$ required to produce 22.4 lits of $S O_{2}$ at STP is:
$[S = 32, Z n = 65, O = 16]$

97 g

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65 g

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124 g

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78 g

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Solution

The correct option is A 97 g
When Zinc Blende ( $Z n S$ ) is roasted in air, the following chemical reaction takes place:
$Z n S + O_{2} \to Z n + {S O}_{2} ↑$

Molecular mass of $Z n S$ = 97 g
Molecular mass of oxygen = 32 g
Molecular mass of ${S O}_{2}$ = 64 g

Given: Amount of ${S O}_{2}$ produced = 22.4 litre (at STP)
Number of moles of ${S O}_{2}$ = 1 mole
Number of moles of $Z n S$ = 1 mole
Weight of $Z n S$ consumed = moles x molecular mass of $Z n S$ = $1 \times 97$ = 97 g

Hence, answer is $A$ .

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