The compressibility factor of an ideal gas is:

1. zero                         

2. infinite

3. 1                               

4. -1

The compressibility factor of a gas is less than unity at STP. The correct statement among the following is -

1. ${\mathrm{V}}_{\mathrm{m}}$  > 22.4 L

2. ${\mathrm{V}}_{\mathrm{m}}$ < 22.4 L

3. ${\mathrm{V}}_{\mathrm{m}}$ = 22.4 L

4. ${\mathrm{V}}_{\mathrm{m}}$ = 44.8 L

Consider the following graph:

The curve that represents CO₂ gas is - 

1. X

2. Y

3. Both X and Y 

4. Cannot predict from the graph

At high pressure, the compressibility factor 'Z' is equal to -

1.  Unity

$2.$ $1-\frac{\mathrm{Pb}}{\mathrm{RT}}$
$3.$ $1+\frac{\mathrm{Pb}}{\mathrm{RT}}$

4.  Zero

 In the given figure, the curve representing an ideal gas is-

1.  B only

2.  C and D only

3.  E and F only 

4.  A and B only

The compressibility factor for 1 mol of a van der Waals gas at $0°\mathrm{C}$ and 100 atmospheric pressure is found to be 0.5. The volume of gas is-

1. 2.0224 L

2. 1.4666 L

3. 0.8542 L

4. 0.1119 L

The compressibility factor for H₂ and He is usually-

1. >1                                     

2. =1

3. <1                                     

4.  Zero

The density of a gaseous substance at 1 atm pressure and 773 K is 0.4 g/L. If the molecular weight of the substance is 30, the dominant force existing among gas molecules is/are-