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 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 

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

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

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 pressure exerted by a mixture of 3.2 g of methane and 4.4 g of carbon dioxide contained in a 9 dm³ flask at 27 °C would be -

$1.$ $8.31$ $\times$ ${10}^4$ $\mathrm{Pa}$
$2.$ $7.43$ $\times$ ${10}^{-4}$ $\mathrm{Pa}$
$3.$ $6.87$ $\times$ ${10}^3$ $\mathrm{Pa}$
$4.$ $8.31$ $\times$ ${10}^6$ $\mathrm{Pa}$

The state of a gas can be described by quoting the relationship between:

1.  Pressure, volume, temperature

2.  Temperature, amount, pressure

3.  Amount, volume, temperature

4.  Pressure, volume, temperature, amount

A 2.24 L cylinder of oxygen at STP is found to develop a leakage. When the leakage was plugged, the pressure dropped to 570 mm of Hg. The number of moles of gas that escaped will be:

1. 0.050

2. 0.025

3. 0.075

4. 0.01

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

If an open container is heated from 300 K to 400 K, then the % of gas that remains in the container is-

1. 25%

2. 50%

3. 75%

4. 100%