At $27^{0} C$ temperature 20 gm. $H_{2}$ , 220 gm $C O_{2}$ and 140 gm $N_{2}$ are filled in a vessel having volume 2 litre. Find the total pressure in bar unit which gas is removed from the vessel so that pressure can be reduced by 50%.

Open in App

Solution

No. of moles of $H_{2} = \frac{20}{2} = 10$ moles
No. of moles of $C O_{2} = \frac{220}{44} = 5$ moles
No. of moles of $N_{2} = \frac{140}{28} = 5$ moles
So, according to Dalton's law of partial pressure,
pressure $\propto$ mole fraction of $H_{2}$
So, as mole fraction is 0.5, when hydrogen is removed half of the pressure is removed.

Suggest Corrections

Similar questions

A closed vessel contains 8 gm of oxgen 7 gm of nitrogen and 1 gm of hydrogen. The total pressure is 8 atmospheres at a given temperature. If now oxygen is removed without change in temperature the pressure of the remaining gas is

Q. Ina

13

litres vessel initially following reaction occur

C (s) + S_{2} (g) \to C S_{2}

(g) by

12

gm C, 64 gm

S_{2}

76

C S_{2}

1027

temperature, then total pressure is:

Q. 12 g

N_{2}

, 4 gm

H_{2}

and 9 gm

O_{2}

are put into a one litre container at

27^{\circ} C

. What is the total pressure?

Q. A vessel contains 1.6 gm of oxygen gas at 1 atm and 273 K. The gas is transferred to another container. The temperature of which is double to that of initial temperature. The new pressure of the gas is 0.20 atm. The volume (in litre) of the new vessel is:

Q. The pressure exerted by

12 gm

of an ideal gas at

t^{\circ} C

in a vessel of volume v litre is one atm. When the temperature is increased by

10^{\circ} C

at the same volume, the pressure increases by 10%. Calculate the temperature t (in K) (Mol. Wt. of gas = 120)

Join BYJU'S Learning Program

At 270C temperature 20 gm. H2, 220 gm CO2 and 140 gm N2 are filled in a vessel having volume 2 litre. Find the total pressure in bar unit which gas is removed from the vessel so that pressure can be reduced by 50%.

No. of moles of H2=202=10 molesNo. of moles of CO2=22044=5 molesNo. of moles of N2=14028=5 molesSo, according to Dalton's law of partial pressure,pressure ∝ mole fraction of H2 So, as mole fraction is 0.5, when hydrogen is removed half of the pressure is removed.

At $27^{0} C$ temperature 20 gm. $H_{2}$ , 220 gm $C O_{2}$ and 140 gm $N_{2}$ are filled in a vessel having volume 2 litre. Find the total pressure in bar unit which gas is removed from the vessel so that pressure can be reduced by 50%.