A $0.5 {dm}^{3}$ flask contains gas A and a $1 {dm}^{3}$ flask contains gas B at the same temperature.
If the density of $A = 3 {g.dm}^{- 3}$ , that of $B = 1.5 {g.dm}^{- 3}$ and the molar mass of $A = \frac{1}{2}$ B, the ratio of pressures exerted by the 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 $\frac{P_{A}}{P_{B}} = 4$
$Pressure = \frac{ρ R T}{M}$
where, $ρ$ is the density of the gas.
Given,
Density of the gas A, $ρ_{A} = 3 {g.dm}^{- 3}$
Density of the gas B, $ρ_{B} = 1.5 {g.dm}^{- 3}$
$molar mass of A = \frac{1}{2} \times molar mass of B$
Hence,
$P_{A} = \frac{3 R T}{M_{A}}; P_{B} = \frac{1.5 R T}{M_{B}}$

$\frac{P_{A}}{P_{B}} = \frac{2 M_{B}}{M_{A}} = \frac{2 \times 2 M_{A}}{M_{A}} = 4$

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Similar questions

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

Q. 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

B

, the ratio of pressure exerted by gases is:

If A and B are any two events such that P (A) + P (B) − P (A and B) = P (A), then

(A) P (B|A) = 1 (B) P (A|B) = 1

IF A and B are any two events such that P(A) + P(B) - P (A and B ) = P(A), then
(a) $P (\frac{B}{A}) = 1$
(b) $P (\frac{A}{B}) = 1$
(c) $P (\frac{B}{A}) = 0$
(d) $P (\frac{A}{B}) = 0$

Q. If

A

and

B

are two events such that

A \subset B

and

P (B) \neq 0

, then which of the following is correct?

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A 0.5 dm3 flask contains gas A and a 1 dm3 flask contains gas B at the same temperature. If the density of A=3 g.dm−3, that of B=1.5 g.dm−3 and the molar mass of A=12 B, the ratio of pressures exerted by the gases is:

The correct option is C PAPB=4Pressure=ρRTM where, ρ is the density of the gas. Given, Density of the gas A, ρA=3 g.dm−3 Density of the gas B, ρB=1.5 g.dm−3 molar mass of A=12×molar mass of B Hence, PA=3RTMA;PB=1.5RTMB PAPB=2MBMA=2×2MAMA=4

A $0.5 {dm}^{3}$ flask contains gas A and a $1 {dm}^{3}$ flask contains gas B at the same temperature.
If the density of $A = 3 {g.dm}^{- 3}$ , that of $B = 1.5 {g.dm}^{- 3}$ and the molar mass of $A = \frac{1}{2}$ B, the ratio of pressures exerted by the gases is: