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Mole Concept

What volume o...

Question

What volume of air at $1 a t m$ and $273 K$ containing 21% of oxygen by volume is required to completely burn sulphur $(S_{8})$ present in $200 g$ of sample, which contains $20 %$ inert material which does not burn. Sulpur burns according to the reaction
$\frac{1}{8} S_{8} (s) + O_{2} (g) \to S O_{2} (g)$

23.52 L

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320 L

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112 L

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533.33 L

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Solution

The correct option is D $533.33 L$
$Weight of S_{8} in sample = 160 g$
$Moles of S_{8} = \frac{160}{32 \times 8} = 0.625$
$Number of moles of O_{2} required = 0.625 \times 8$
$Volume of O_{2} required at S T P = 22.4 \times 5$
$∴ Volume of air required at S T P = 22.4 \times 5 \times \frac{100}{21} = 533.33 L$

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273 K

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\frac{1}{8} S_{8} (s) + O_{2} (g) \to S O_{2} (g)

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\frac{1}{8} S_{8} (s) + O_{2} (g) \to S O_{2} (g)

What volume of 21% oxygen by volume is required of air at NTP to completely burn 1000 gram of sulphur containing 4% incombustible matter ?

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