120 g of an ideal gas of molecular weight 40 g mole^–1 are confined to a volume of 20 L at 400 K. The pressure of the gas is- 

 ($R=0.0821$ $L$ $atm$ $K^{-1}$ $mol{e}^{-1}$)

1. 3.90 atm

2. 4.92 atm

3. 6.02 atm

4. 2.96 atm

3.2 g of oxygen  and 0.2 g of hydrogen are placed in a 1.12 litre flask at 0°C.

The total pressure of the gas mixture will be-

1. 1 atm

2. 4 atm

3. 3 atm

4. 2 atm

The density of methane at 2.0 atmosphere pressure and 27°C is- 

1. 0.13 gL^–1

2. 0.26 gL^–1

3. 1.30 gL^–1

4. 2.60 gL^–1

In a flask of volume V litres, 0.2 mol of oxygen, 0.4 mol of nitrogen, 0.1 mol of ammonia and 0.3 mol of helium are enclosed at ${27}^{o}C$. If the total pressure exerted by these non-reacting gases is one atmosphere, the partial pressure exerted by nitrogen is-

1. 1 atm

2. 0.1 atm

3. 0.2 atm

4. 0.4 atm

A gaseous mixture contains 56 g of N₂, 44 g of CO₂ and 16 g of CH₄. The total pressure of the mixture is 720 mm Hg. The partial pressure of CH₄ is-

1. 180 mm

2. 360 mm

3. 540 mm

4. 720 mm

Maximum deviation from ideal gas is shown by-

1. H_2(g)   

2. N_2(g)

3. CH_4(g)

4. NH_3(g)

If 300 ml of a gas at 27°C is cooled to 7°C at constant pressure, its final volume will be:

The kinetic energy for 14 grams of nitrogen gas at 127°C is nearly -

(mol. mass of nitrogen = 28 and gas constant = 8.31JK^–1mol^–1) 

1. 1.0 J

2. 4.15 J

3. 2493 J

4. 3.3 J

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

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