At constant temperature, 200 cm3 of N2 at 720 mm and 400 cm3 of O2 at 750 mm pressure are put together in a one-litre flask. The final pressure of the mixture is-
1. 111 mm
2. 222 mm
3. 333 mm
4. 444 mm
The temperature at which the r.m.s velocity of carbon dioxide becomes the same as that of nitrogen at 210C is-
1. 462 oC
2. 273 K
3. 189 oC
4. 546 K
The density of O2(g) is maximum at-
1. STP
2. 273 K and 2 atm
3. 546 K and 1 atm
4. 546 K and 2 atm
In van der Waal's equation of state for a non-ideal gas, the term that accounts for the intermolecular force is-
1. V-b
2. (P+a/V2)
3. RT
4. (RT)-1
The gas among the following that can be most readily liquified is-
( Value of 'a' for NH3 = 4.17, CO2 = 3.59, SO2 = 6.71, Cl2 = 6.49)
1. NH3
2. Cl2
3. SO2
4. CO2
At moderate pressure, the van der Waal's equation becomes:
1. PVm = RT
2. P(Vm-b) = RT
3. (P+a/V2m) (Vm )= RT
4. P = RT/Vm + a/V2m
Which among the following mixtures of gases at room temperature does not obey Dalton's law of partial pressure-
1. He and O2
2. NH3 and HCl
3. H2 and He
4. N2 and He
1.6 g O2 gas and 0.1 g H2 gas are placed in a 1.12 L flask at 0 oC. The total pressure of the gas mixture will be-
1. 2 atm
2. 3 atm
3. 4 atm
4. 1 atm
An open flask containing air is heated from 300 K to 500 K. The percentage of air that will escape into the atmosphere if pressure is kept constant is-
1. 80
2. 40
3. 60
4. 20
V versus T curves at constant pressure P1 and P2 for an ideal gas are as shown in the figure. The correct statement is-
1. P1>P2
2. P1<P2
3. P1=P2
4. All of the above