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How much sulphur is to be burnt to produce $0.224$ lit of ${SO}_{2}$ at NTP?

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$32 g$

$0.03 g$

$3.2 g$

$0.32 g$

answer is B.

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Detailed Solution

The balanced equation for ${SO}_{2}$ formation is

$S + O_{2} ⟶ {SO}_{2}$

From the above equation it is considered that $32 g$ of sulphur produces $22.4 L$ of ${SO}_{2}$ . Then for the production of $0.224$ lit of ${SO}_{2}$ at NTP it requires $32 / 22.4 \times 0.224 = 0.32 g$

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