A $0.5$ $d m^{3}$ flask contains gas $A$ and 1 $d m^{3}$ flask contains gas $B$ at the same temperature. If density of $A = 3 g / d m^{3}$ and that of $B = 1.5 g / d m^{3}$ and the molar mass of $A = 1 / 2$ of $B$ , the ratio of pressure exerted by gases is:

\frac{P_{A}}{P_{B}} = 2

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\frac{P_{A}}{P_{B}} = 1

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\frac{P_{A}}{P_{B}} = 4

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\frac{P_{A}}{P_{B}} = 3

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Solution

The correct option is C $\frac{P_{A}}{P_{B}} = 4$
The ideal gas equation is:

$P M = D R T$

At constant temperature:

$\frac{P_{A}}{P_{B}} = \frac{D_{A} M_{B}}{M_{A} D_{B}}$

$= \frac{3 \times M_{B}}{1.5 \times 0.5 M_{B}} = 4$

Hence, the ratio of the pressure exerted by the gases A and B is $4 : 1$ .

Hence, the correct answer is option $C$ .

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A V ${d m}^{3}$ flask contains gas A and another flask of 2V ${d m}^{3}$ contains gas B at the same temperature. If density of gas A is 3.0 g ${d m}^{- 3}$ and of gas B is 1.5 g ${d m}^{- 3}$ and mol. Wt. Of A = $\frac{1}{2}$ mol. Wt. Of B, then the ratio of pressure exerted by gases is