In a 10 litre vessel, the total pressure of a gaseous mixture containing $H_{2}, N_{2} a n d C O_{2}$ is 9.8 atm, The partial pressures of $H_{2} a n d N_{2}$ are 3.7 and 4.2 atm respectively. Find the partial pressure of $C O_{2}$ .

Q. One litre of oxygen at a pressure of

1 a t m

and two litres of nitrogen at a pressure of

0.5 a t m

, are introduced into a vessel of volume

1 L

. If there is no change in temperature, the final pressure of the mixture of gas (in atm) is

Q. Choose the correct option for the total pressure (in atm.) in a mixture of

4 g O_{2} and 2 g H_{2}

confined in a total volume of one litre at

0^{\circ} C

is :

[Given R = 0.082 L atm m o l^{1} K^{- 1}, T = 273 K]

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5 litre of N2 under a pressure of 2 atm, 2 litre of O2 at 5.5 atm and 3 litre of CO2 at 5 atm are mixed. The resultant volume of the mixture is 15 litre. Calculate the total pressure of the mixture and partial pressure of each constituent.

The correct option is A 2.06 atmFrom the equation Pv=nRT for the two gases. We can writenN2=5×2RTnO2=2×5.5RTnCO2=3×5RTWhen introduced in 1L vessel, thenP×15L=(nN2+nO2+nCO2)RTPutting the values, we getP=2.06barHence, the total pressure of the gaseous mixture in the vessel is 1.8 bar

5 litre of $N_{2}$ under a pressure of 2 atm, 2 litre of $O_{2}$ at 5.5 atm and 3 litre of $C O_{2}$ at 5 atm are mixed. The resultant volume of the mixture is 15 litre. Calculate the total pressure of the mixture and partial pressure of each constituent.