The correct statement regarding the van der Waal constant of  N₂ & NH₃ is -

1. ${\mathrm{a}}_{{\mathrm{NH}}_3}> {\mathrm{a}}_{{\mathrm{N}}_2}, {\mathrm{b}}_{{\mathrm{NH}}_3}< {\mathrm{b}}_{{\mathrm{N}}_2}$

2. ${\mathrm{a}}_{{\mathrm{NH}}_3}< {\mathrm{a}}_{{\mathrm{N}}_2}, {\mathrm{b}}_{{\mathrm{NH}}_3}< {\mathrm{b}}_{{\mathrm{N}}_2}$

3. ${\mathrm{a}}_{{\mathrm{NH}}_3}> {\mathrm{a}}_{{\mathrm{N}}_2}, {\mathrm{b}}_{{\mathrm{NH}}_3}> {\mathrm{b}}_{{\mathrm{N}}_2}$

4. ${\mathrm{a}}_{{\mathrm{NH}}_3} < {\mathrm{a}}_{{\mathrm{N}}_2}, {\mathrm{b}}_{{\mathrm{NH}}_3}> {\mathrm{b}}_{{\mathrm{N}}_2}$

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. PV_m = RT

2. P(V_m-b) = RT

3. (P+a/V²_m) (V_m )= RT

4. P = RT/V_m + a/V²_m

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