A car tyre is filled with nitrogen gas at 35 psi at 27 °C. It will burst if pressure exceeds 40 psi. The temperature in °C at which the car tyre will burst is-

(Rounded-off to the nearest integer)
(Hint: psi is unit of pressure)

1. 65

2. 70

3. 75

4. 77

3.12 g of oxygen is adsorbed on 1.2 g of platinum metal. The volume of oxygen adsorbed per gram of the

adsorbent at 1 atm and 300 K in L is:

[R = 0.0821 L atm K^–1 mol^–1]

1. 4 L

2. 3 L

3. 1 L

4. 2 L

Among the following, the graph not correctly representing an ideal gas is:

d = Density , P = Pressure, T = Temperature 

1.  II
2.  III
3.  I
4.  IV

A mixture of one mole of H₂, He, and O₂ each are enclosed in a cylinder of volume V at temperature T. If the partial pressure of H₂ is 2 atm, the total pressure of the gases in the cylinder is-
1. 14 atm
2. 22 atm
3. 38 atm
4. 6 atm

Consider the van der Waals constants, a and b, for the following gases.
       Gas                     Ar            Ne       Kr     Xe
a/(atm dm⁶ mol^–2)      1.3          0.2      5.1    4.1
b/(10^–2dm³ mol^–1)      3.2          1.7      1.0    5.0
Which gas is expected to have the highest critical temperature?

1.  Xe

2.  Ne

3.  Kr 

4.  Ar 

'a' and 'b' are van der Waals' constants for gases. Chlorine is more easily liquefied than ethane because:

If 10⁻⁴ dm³ of water is introduced into a 1.0 dm³ flask at 300 K, then the total number of moles of water in the vapour phase (equilibrium is established) are-

(Given: Vapour pressure of H₂O at 300 K is 3170 Pa; R = 0.0821 atm L K⁻¹ mol⁻¹; 1 Pa = 9.9 × 10^-6 atm )

1. 1.26 x 10⁻³ mol 

2. 5.56 x 10⁻³ mol 

3. 1.53 x10⁻² mol 

4. 4346 x 10-² mol

Which one of the following statements is not true about the effect of an increase in temperature on the distribution of molecular speeds in a gas?

1. The area under the distribution curve remains the same as under the lower temperature

2. The distribution becomes broader

3. The fraction of the molecules with the most probable speed increases

4. The most probable speed increases

The volume of hydrogen gas at 273 K and 1 atm pressure that will be consumed in obtaining 21.6 g of elemental boron ( atomic mass = 10.8) from the reduction of boron trichloride by hydrogen is-

1. 89.6 L 

2. 67.2 L 

3. 44.8 L 

4. 22.4 L