A gas occupied a volume of 250 ml at 700 mm Hg pressure and 25°C. An additional pressure is required to reduce the gas volume to its 4/5^th value at the same temperature is-

1. 225 mm Hg

2. 175 mm Hg

3. 150 mm Hg

4. 265 mm Hg

When the temperature of 23 ml of dry CO₂ gas is increased from 10° to 30°C at a constant pressure of 760 mm, the volume of gas becomes-

1. 7.7 ml

2. 25.5 ml

3. 24.6 ml

4. 69 ml

The volume of a gas is 100 ml at 100°C. If the pressure remains constant then the temperature at which the volume becomes 200 ml is-

1. 200°C

2. 473°C

3. 746°C

4. 50°C

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

According to Charle’s law, at constant pressure, 100 ml of a given mass of a gas with 10°C rise in temperature will become $\left(\frac{1}{273}=0.00366\right)$ ,T initial = Zero °C

1. 100.03

2. 99.96

3. 103.66

4. 100.36

A sealed tube which can withstand a pressure of 3 atmosphere is filled with air at ${27}^{o}C$ and 760 mm pressure. The tube will burst at - 

1. 900°C

2. 627°C

3. 726°C

4. 1173°C

The pressure of 2 moles of an ideal gas at 546 K having volume 44.8 L is:

1. 2 atm

2. 3 atm

3. 4 atm

4. 1 atm

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

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