When a liquid that is immiscible with water was steam distilled at 95.2°C at a total pressure of 99.652 kPa. The distillate contained 1.27 g of the liquid per gram of water. What will be the molar mass of the liquid if the vapour pressure of water is 85.140 kPa at 95.2°C?

• 99.65 g mol^-1

• 18 g mol^-1

• 134.1 g mol^-1

• 105.74 g mol^-1

Van der waals' real gas, acts as an ideal gas at which condition?

• High temperature, low pressure

• Low temperature, high pressure

• High temperature, high pressure

• Low temperature, low pressure

Which of the following type of forces are present in vulcanised rubber?

• Weakest intermolecular forces

• Hydrogen bonding

• Three dimensional network of bonds

• Metallic bonding

Match the following

List I	List II
(A) Viscosity	(I) Critical temperature
(B) Ideal gas behaviour	(II) Isobar
(C) Liquefaction of gases	(III) Compressibility factor
(D) Charles'law	(IV) kg s-2
	(V) kgm-1s-1

The correct answer

• A-IV, B-III, C-I, D-II

• A-V, B-III, C-I, D-II

• A-V, B-III, C-II, D-I

• A-IV, B-III, C-II, D-I

The most probable speed of O₂, molecules at T(K) is

• $\sqrt{\frac{\mathrm{RT}}{4\mathrm{\pi }}}$

• $\sqrt{\frac{\mathrm{RT}}{16\mathrm{\pi }}}$

• $\sqrt{\frac{\mathrm{RT}}{16}}$

• $\sqrt{\frac{3\mathrm{RT}}{32}}$

If the kinetic energy in J, of CH₄ (molar mass =16 g mol^-1) at T(K) is X, the kinetic energy in J, of O₂, (molar mass = 32 g mol^-1) at the same temperature is

• X

• 2X

• X²

• X/2

The given figure shows the Maxwell distribution of molecular speeds of a gas at three different temperatures T_1,T_2, and T₃. The correct order of temperature is

• T₁ > T₂ > T₃

• T₁ > T₃ > T₂

• T₃ > T₂ > T₁

• T₂ > T₃ > T₁

At low pressure and high temperature, the van der Waal's equation is finally reduced (simplified) to

• $\left(\mathrm{p} + \frac{\mathrm{a}}{{\mathrm{V}}_{\mathrm{m}}^2}\right)({\mathrm{V}}_{\mathrm{m}} - \mathrm{b}) = \mathrm{RT}$

• $\mathrm{p}({\mathrm{V}}_{\mathrm{m}} - \mathrm{b}) = \mathrm{RT}$

• $\left(\mathrm{p} + \frac{\mathrm{a}}{{\mathrm{V}}_{\mathrm{m}}^2}\right){\mathrm{V}}_{\mathrm{m}} = \mathrm{RT}$

• pV_m = RT

At a given temperature T, gases Ne, Ar, Xe and Kr are found to deviate from ideal gas behaviour. Their equation of state is given as p = $\frac{\mathrm{RT}}{\mathrm{V} - \mathrm{b}}$ at T. Here, b is the van der Waals constant. Which gas will exhibit steepest increase in the plot of Z (compression factor) vs p?

• Ne

• Xe

• Ar

• Kr

Consider the following table:

Gas	a/(kPa dm6mol-1)	b/(dm3mol-1)
A	642.32	0.05196
B	155.21	0.04136
C	431.91	0.05196
D	155.21	0.4382

And b are vander walls contants . The correct statement a Bout the gases is :

• Gas A will occupy than gas D  Compressible than gas D Gas C will Occupy more volume than

• gas A gas B will be more compressible than gas D Gas C will Occupy Lesser volume than

• Gas A gas B will be more compressible than gas D Gas C will Occupy Lesser volume than

• Gas A: gas B will be lesser Compressble than gas D