The condition of SATP refers to:

1. 25 $°$C and 2 atm             

2. 25 $°$C  and 1 atm

3. 0 $°$C  and 2 atm             

4. 25 $°$C  and 1 bar

The condition that favour a pure sample of an ideal gas to have pressure of 1 atm and a concentration of

1 mol L^-1  is -

(R=0.082 L atm mol^-1K^-1)                                     

1. At STP

2. When V = 22.4 L

3. When T = 12 K

4. Impossible under any conditions

The van der Waals' equation for real gas is:

1. (P + a/V²)(V-b) = RT

2. (P+n²a/V²)(V-nb) = nRT

3. \(P=\frac{nRT}{V-nb}-\frac{an^2}{V^2}\)

4. All of the above

The gas among the following that can be most steadily liquefied is -

1. NH₃                           

2. Cl₂

3. SO₂                           

4. CO₂

The correct statement for an ideal gas equation is -

1. n is the number of molecules of a gas.

2. V denotes the volume of 1 mole of the gas.

3. n moles of a gas has a volume V.

4. p is the pressure of the gas when only one mole of the gas is present.

An ideal gas expands according to PV=constant. On expansion, the temperature of the gas:

1. Will rise.

2. Will drop.

3. Will remain constant.

4. Cannot be determined because the external pressure is not known.

The deviation of a gas from ideal behavior is expected to be minimum at -                                    

1. 350 K and 3 atm                   

2. 550 K and 1 atm

3. 250 K and 4 atm                   

4. 450 K and 2 atm

The curve that can not represent Boyle's law is -

1.   

2.  

3.  

4.  

The compressibility factor of an ideal gas is:

1. zero                         

2. infinite

3. 1                               

4. -1

A gas cannot be liquefied if:

1. Forces of attraction are low under ordinary conditions

2. Forces of attraction are high under ordinary conditions

3. Forces of attraction are zero under ordinary conditions

4. Forces of attraction are either high or low under ordinary conditions