For 10 minutes each, at `0^(@)C`, from two identical holes nitrogen and an unknown gas are leaked into a common vessel of 4 litre capacity. The resulting pressure is 2.8 atm and the mixture contains 0.4 mole of nitrogen. What is the molar mass of unknown gas ? (Take `R = 0.821 "L-atm mol"^(-1)K^(-1)`]

For 10 minutes each at 27^(@)C from two identical holes nitrogen and an unknow gas are leaked into a common vessel of 3 litre capacity The resulting pressure is 4.18 bar and the mixture contains 0.4 mole of nitrogen What is the molar mass of the unknown gas ? .

From two identical holes, nitrogen and an unknown gas are leaked into a common vessel of 3 L capacity for 10 min , at 27^(@)C . The resulting pressure is 4.18 bar and the mixture contains 0.4 mol of nitrogen. What is the molar mass of the unknown gas?

The constant motion and high velocities of gas particles lead to some important practical consequences One such consequence is that is mixing rapidly when they come in contact. The mixing of different gases by random molecular motion and with frequent collisions is called diffusion.A similar process in which gas molecules escape through a tiny hole into vaccum is called effusion. For 10 min each at 27^(@) C from two identical bulbs helium and an unknown gas X at equal pressure are leaked into a common vessel of 3L capacity. The resulting pressure is 4.1 atm and the mixture contains 0.4 mol of helium The molar mass of gas X is

At 27^(@) C , hydrogen is leaked through a tiny hole into a vessel for 20 min . Another unknown gas at the same T and P as that of H_(2) , is leaked through the same hole for 20 min. After the effusion of the gases the mixture exerts a pressure of 6 atm. The hydrogen content of the mixture is 0.7 mole. If the volume of the container is 3 litre, what is molecular weight of unknown gas ? ("Use" : R = 0.821 "L atm K"^(-1) "mole"^(-1))

Density of ideal gas at 2.46 atm and 300 K is 0.8 g//L Hence g-molar mass of gas is : [R = 0.082 "L-atm/mol-K"]

If two moles of an ideal gas at 500 K occupies a volume of 41 litres, the pressure of the gas is (R = 0.082 L atm K^(-1) mol^(-1))

The osmotic pressure of 0.2 molar solution of urea at 300 K(R = 0.082) litre atm mol^(-1)K^(-1) is

Kinetic energy of 0.3 mole of 'He' gas in a container of maximum capacity of 4 litre at 5 atm, must be : (R = 0.821"atm litre mol"^(-1) K^(-1))