The volume $V$ of an enclosure contains a mixture of three gases: $16 g$ of oxygen, $28 g$ of nitrogen and $44 g$ of carbon dioxide at absolute temperature $T$ . Consider $R$ as universal gas constant. The pressure of the mixture of gases is:

\frac{4 R T}{V}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

\frac{88 R T}{V}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

\frac{5}{2} \frac{R T}{V}

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

\frac{3 R T}{V}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is C $\frac{5}{2} \frac{R T}{V}$
No. of moles of $O_{2} : n_{1} = \frac{16}{32} = 0.5 moles$
No. of moles of $N_{2} : n_{2} = \frac{28}{28} = 1 mole$
No. of moles of $C O_{2} : n_{3} = \frac{44}{44} = 1 mole$

Total no. of moles in container: $n = n_{1} + n_{2} + n_{3}$
$∴ n = 0.5 + 1 + 1 = \frac{5}{2} moles$

From ideal gas equation $P V = n R T$
$P = \frac{n R T}{V}$
$∴ P = \frac{5}{2} \frac{R T}{V}$
Hence option (c) is correct.

Suggest Corrections

Similar questions

An enclosure of volume V contains a mixture of 8g of oxygen, 14g of nitrogen and 22g of carbon dioxide at absolute temperature T. The pressure of the mixture of gases is (R is universal gas constant)

Q. An enclosure of volume

4 l i t r e s

contains a mixture of

8 g

of oxygen,

14 g

of nitrogen and

22 g

of carbon dioxide. If the temperature of the mixture is

27^{\circ} C

find the pressure of the mixture of gases. Given

R = 8.315 K J^{- 1} m o l^{- 1}

Q. A vessel contains a mixture of nitrogen (

m_{1} =

7.0 g) and carbon dioxide (

m_{2} =

11 g) at a temperature T

=

290 K and pressure

p_{0} =

1.0 atm. Find the density of this mixture, assuming the gases to be ideal.

Q. A mixture of gases at

760

torr contains

55.0 %

nitrogen,

25.0 %

oxygen and

20.0 %

carbon dioxide by volume. What is the partial pressure of each gas in torr?

Join BYJU'S Learning Program

The volume V of an enclosure contains a mixture of three gases: 16 g of oxygen, 28 g of nitrogen and 44 g of carbon dioxide at absolute temperature T. Consider R as universal gas constant. The pressure of the mixture of gases is:

The correct option is C 52RTVNo. of moles of O2:n1=1632=0.5 moles No. of moles of N2:n2=2828=1 mole No. of moles of CO2:n3=4444=1 mole Total no. of moles in container: n=n1+n2+n3 ∴n=0.5+1+1=52 moles From ideal gas equation PV=nRT P=nRTV ∴P=52RTV Hence option (c) is correct.

The volume $V$ of an enclosure contains a mixture of three gases: $16 g$ of oxygen, $28 g$ of nitrogen and $44 g$ of carbon dioxide at absolute temperature $T$ . Consider $R$ as universal gas constant. The pressure of the mixture of gases is: