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

The volume of 2.8 g of carbon monoxide at 27°C and 0.821 atm pressure is- 

$(\mathrm{R}=0.0821$ $\mathrm{lit}$ $\mathrm{atm}$ ${\mathrm{K}}^{-1}$ ${\mathrm{mol}}^{-1})$

1. 0.3 litre

2. 1.5 litre

3. 3 litre

4. 30 litre

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

The volume of 0.0168 mol of O₂ obtained by decomposition of KClO₃ and collected by displacement of water is 428 ml at a pressure of 754 mm Hg at 25°C. The pressure of water vapour at 25°C is- 

1. 18 mm Hg

2. 20 mm Hg

3. 22 mm Hg

4. 24 mm Hg

The partial pressure of H₂ in a flask containing 2 g of H₂, 14 g of N_2, and 16 g of O₂ is-

1. 1/2 of the total pressure

2. 1/3 of the total pressure

3. 1/4 of the total pressure

4. 1/16 of the total pressure

Equal weights of methane and oxygen are mixed in an empty container at 25°C. The fraction of the total pressure exerted by oxygen is- 

1. 1/3

2. 1/2

3. 2/3

4. $\frac{1}{3}\times \frac{273}{298}$  

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

Density ratio of O₂ and H₂ is 16 : 1. The ratio of their r.m.s. velocities will be- 

1. 4 : 1

2. 1 : 16

3. 1 : 4

4. 16 : 1