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A mixture of ${CH}_{4}$ , $N_{2} and O_{2}$ is enclosed in a vessel of one litre capacity at O° C.
The ratio of partial pressures of gases is I : 4 :2. Total pressure of the gaseous mixture is 2660 mm. The number of molecules of oxygen present in the vessel is

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$\frac{6.02 \times 10^{23}}{22.4}$

$6.02 \times 10^{23}$

$22.4 \times 10^{22}$

1000

answer is A.

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Detailed Solution

$Partial pressure of oxygen = \frac{2}{1 + 4 + 2} \times 2660 = 760 mm$

$Thus, 1 L oxygen gas is present at 0 ° C and 760 mm pressure$

$∴ Number of oxygen molecules = \frac{6.023 \times 10^{23}}{22.4}$

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