Equal weights of CH₃ and H₂ are mixed in an empty container at 25°C. the fraction of the total pressure exerted by H₂ is:

• 1/9

• 1/2

• 8/9

• 16/17

Four gases P, Q, R and S have almost same values of 'b' but their 'a' values (a, b are van der Waals' constants) are in the order Q < R < S < P. At a particular temperature, among the four gases, the most easily liquefiable one is

• P

• Q

• R

• S

Maximum deviation from ideal gas is expected from

• H₂(g)

• N₂(g)

• CH₄(g)

• NH₃(g)

The value of $∆$H for cooling 2 mole of an ideal monoatomic gas from 225°C to 125°C at constant pressure will be [given C_p = $\frac{5}{2}\mathrm{R}$].

• 250 R

• -500 R

• 500 R

• -250 R

The compressibility factor (Z) of one mole of a van der Waals' gas of negligible 'a' value is

• 1

• $\frac{\mathrm{bp}}{\mathrm{RT}}$

• $1 + \frac{\mathrm{bp}}{\mathrm{RT}}$

• $1-\frac{\mathrm{bp}}{\mathrm{RT}}$

Calculate the ratio of the rate of diffusion of oxygen to the rate of diffusion of hydrogen at constant temperature and pressure.

At identical temperature and pessure, the ratio of diffusion of hydrogen gas is $\sqrt[3]{3}$ times that of a hydrocarbon having molecular formula C_nH_2n-2. What is the value of 'n'?

• 1

• 4

• 3

• 8

Which of the following compounds shows evidence of the strongest hydrogen bonding?

• Propan-1-ol

• Propan-2-ol

• Propan-1,2-diol

• Propan-1,2,3-triol

Unusually high boiling point of water is result of

• intermolecular hydrogen bonding

• intramolecular hydrogen bonding

• both intra and inter molecular hydrogen bonding

• high specific heat

The rms velocity of an ideal gas at constant pressure varies with density (d) as

• $\frac{1}{\sqrt{\mathrm{d}}}$

• d

• $\sqrt{\mathrm{d}}$

• d²