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

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

Maximum deviation from ideal gas is shown by-

1. H_2(g)   

2. N_2(g)

3. CH_4(g)

4. NH_3(g)

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

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

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

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

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

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