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 correct relation between density ($\mathrm{\rho }$) and pressure of gas (P) is-

1. $\mathrm{P}$ $\mathrm{\alpha }$ ${\mathrm{d}}^2$

2. $\mathrm{P}$ $\mathrm{\alpha }$ $\frac{1}{\mathrm{d}}$

3. $\mathrm{P}$ $\mathrm{\alpha }$ $\mathrm{d}$

4. None of the above

The number of moles of H₂ in 0.224 litre of hydrogen gas at STP (273 K, 1 atm.) is-

1. 1

2. 0.1

3. 0.01

4. 0.001

The temperature of 4.0 mole of a gas occupying 5 dm³ at 3.32 bar is -
(R = 0.083 bar dm³ K^–1 mol^–1).

1. 40 K 

2. 30 K 

3. 20 K

4. 50 K 

7.0 g of gas occupies 5.6 L of volume at STP. The gas is-

1. NO

2. ${\mathrm{N}}_2\mathrm{O}$

3. CO

4. ${\mathrm{CO}}_2$ 

Flask X is filled with 20 g of ${\mathrm{CH}}_4$ gas at 100 °C and another identical flask Y with 40 g ${\mathrm{O}}_2$ gas at the same temperature. The correct statement among the following is –

1. The pressure of the gases in the two flasks is identical

2. The pressure of ${\mathrm{CH}}_4$ in flask X is higher than that of ${\mathrm{O}}_2$ in flask Y

3. The pressure of ${\mathrm{CH}}_4$ in flask X is lower than that of ${\mathrm{O}}_2$ in flask Y

4. The pressure of ${\mathrm{CH}}_4$ in flask X is half that of ${\mathrm{O}}_2$ in flask Y

2.9 g of a gas at 95^°C occupies the same volume as 0.184 g of dihydrogen at 17^°C, at the same pressure. The molar mass of the gas is -

1. 20 g mol^-1

2. 40 g mol^-1

3. 34 g mol^-1

4. 14 g mol^-1

The volume occupied by 1.8 g of water vapour at 374 ${}^{\mathrm{o}}\mathrm{C}$ and 1 bar pressure will be -

[Use R=0.083 bar ${\mathrm{LK}}^{-1}$ ${\mathrm{mol}}^{-1}$]

1. 96.66 L

2. 55.87 L

3. 3.10 L

4. 5.31 L

Two flasks of equal volume are connected by a narrow tube (of negligible volume) at 27ºC and contain 0.70 mole of ${\mathrm{H}}_2$ at 0.5 atm. One of the flasks is then immersed in a hot bath, kept at 127 ºC, while the other remains at 27 ºC. The final pressure is -

1. 5.714 atm                   

2. 0.5714 atm

3. 2.5214 atm                 

4. 5.5114 atm

The volume occupied by 8.8 g of CO₂ at 31.1°C and 1 bar pressure is:

(R = 0.083 bar L K^–1 mol^–1)

1. 4.05 L 

2. 3.05 L 

3. 6.05 L 

4. 5.05 L