Joule-Thomson coefficient ($\partial \mathrm{T}/\partial \mathrm{P}$)_H for an ideal gas is:

1. zero                                 

2. +ve

3. -ve                                   

4. none of these

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

The correct statement regarding the van der Waal constant of  N₂ & NH₃ is -

1. ${\mathrm{a}}_{{\mathrm{NH}}_3}> {\mathrm{a}}_{{\mathrm{N}}_2}, {\mathrm{b}}_{{\mathrm{NH}}_3}< {\mathrm{b}}_{{\mathrm{N}}_2}$

2. ${\mathrm{a}}_{{\mathrm{NH}}_3}< {\mathrm{a}}_{{\mathrm{N}}_2}, {\mathrm{b}}_{{\mathrm{NH}}_3}< {\mathrm{b}}_{{\mathrm{N}}_2}$

3. ${\mathrm{a}}_{{\mathrm{NH}}_3}> {\mathrm{a}}_{{\mathrm{N}}_2}, {\mathrm{b}}_{{\mathrm{NH}}_3}> {\mathrm{b}}_{{\mathrm{N}}_2}$

4. ${\mathrm{a}}_{{\mathrm{NH}}_3} < {\mathrm{a}}_{{\mathrm{N}}_2}, {\mathrm{b}}_{{\mathrm{NH}}_3}> {\mathrm{b}}_{{\mathrm{N}}_2}$

Maximum deviation from ideal gas is shown by-

1. H_2(g)   

2. N_2(g)

3. CH_4(g)

4. NH_3(g)

The critical volume of a gas is $0.072 \mathrm{lit}. {\mathrm{mol}}^{–1}$. The radius of the molecule will be , in cm

1. ${\left(\frac{3}{4\mathrm{\pi }}\mathrm{x}{10}^{-23}\right)}^{\frac{\mathbf{1}}{\mathbf{3}}}$                           

2. ${\left(\frac{4\mathrm{\pi }}{3}\mathrm{x}{10}^{-23}\right)}^{\frac{\mathbf{1}}{\mathbf{3}}}$

3. ${\left(\frac{3\mathrm{\pi }}{4}\mathrm{x}{10}^{-23}\right)}^{\frac{\mathbf{1}}{\mathbf{3}}}$                           

4. $\left(\frac{3}{4\mathrm{\pi }}\mathrm{x}{10}^{-8}\right)$