As per Charles's law ,–273° C is the lowest possible temperature because:

1.	All gases get liquefied before reaching a temperature of – 273° C.
2.	All gases get liquefied after reaching a temperature of – 273° C.
3.	All gases have a critical temperature of –273° C.
4.	None of the Above.

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 minimum pressure required to compress 500 dm³ of air at 1 bar to 200 dm³ at 30°C is :

1. 3.6 bar

2. 3.2 kbar

3. 2.5 bar

4. 2.8 kbar

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 

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 

34.05 mL of phosphorus vapour weighs 0.0625 g at 546 °C and 0.1 bar pressure. The molar mass of phosphorus would be -

$1.$ $1247.5$ $\mathrm{g}$ ${\mathrm{mol}}^{-1}$
$2.$ $2234.7$ $\mathrm{g}$ ${\mathrm{mol}}^{-1}$
$3.$ $3126.9$ $\mathrm{g}$ ${\mathrm{mol}}^{-1}$
$4.$ $1134.6$ $\mathrm{g}$ ${\mathrm{mol}}^{-1}$

The density of a gas is found to be 5.46 g/dm³ at 27^°C at 2 bar pressure. The density of gas at STP would be -

$1. 2.0 \mathrm{g} {\mathrm{dm}}^{-3}$
$2. 3.0 \mathrm{g} {\mathrm{dm}}^{-3}$
$3. 4.5 \mathrm{g} {\mathrm{dm}}^{-3}$
$4. 1.5 \mathrm{g} {\mathrm{dm}}^{-3}$

Van der Waals parameter 'a' signifies -

1.The magnitude of intermolecular attractive forces.

2. The magnitude of intermolecular repulsive forces.

3. The volume of a gas molecule.

4. All of the above.

A mixture of dihydrogen and dioxygen at one bar pressure contains 20% by weight of dihydrogen. The partial pressure of dihydrogen is -

1. 0.2 bar

2. 0.7 bar

3. 0.8 bar

4. 0.6 bar

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