The total pressure of a mixture that contains 8 g of O₂ and 4 g of H₂ confined in a vessel of 1 dm³ at 27^°C would be -

(R = 0.083 bar dm³ K^-1mol^-1)

1. 45.67 bar

2. 56.02 bar

3. 34.67 bar

4. 67.13 bar  

 

Find the mass of payload of a balloon of radius 10 m, if a mass of 100 kg is filled with helium at 1.66 bar and 27°C temperature.

(Density of air = 1.2 kg m^–3 and R = 0.083 bar dm³ K^–1 mol^–1).

1. 2905 Kg

2. 3811 Kg 

3. 2721 Kg

4. 4201 Kg                                                                                                                

2.9 g of a gas at 95^°C occupies the same volume as 0.184 g of dihydrogen at 17^°C, at the same pressure. The molar mass of the gas is -

1. 20 g mol^-1

2. 40 g mol^-1

3. 34 g mol^-1

4. 14 g mol^-1

A mixture of dihydrogen and dioxygen at one bar pressure contains 20% by weight of dihydrogen. The partial pressure of dihydrogen is -

1. 0.2 bar

2. 0.7 bar

3. 0.8 bar

4. 0.6 bar

Van der Waals parameter 'a' signifies -

1.The magnitude of intermolecular attractive forces.

2. The magnitude of intermolecular repulsive forces.

3. The volume of a gas molecule.

4. All of the above.

A plot of volume versus temperature (T) for a gas at constant pressure is a straight line passing through the origin. The plots at different values of pressure are shown in the figure given below.

       

The correct order of pressure is -

         Temperature (K) 

1. ${\mathrm{p}}_1>{\mathrm{p}}_2>{\mathrm{p}}_3>{\mathrm{p}}_4$

2. ${\mathrm{p}}_1={\mathrm{p}}_2={\mathrm{p}}_3={\mathrm{p}}_4$

3. ${\mathrm{p}}_1<{\mathrm{p}}_2<{\mathrm{p}}_3<{\mathrm{p}}_4$

4. ${\mathrm{p}}_1<{\mathrm{p}}_2={\mathrm{p}}_3<{\mathrm{p}}_4$

The interaction energy of London force is inversely proportional to sixth power of the distance between two interacting particles. Their magnitude depends upon-

1. Charge of interacting particles.

2. Mass of interacting particles.

3. Polarizability of interacting particles.

4. Strength of permanent dipoles in the particles.

Dipole-dipole forces act between the molecules possessing permanent dipole. Ends of dipoles possess 'partial charges'.

The partial charge will be-

1. More than unit electronic charge.

2. Equal to unit electronic charge.

3. Less than unit electronic charge.

4. Double the unit electronic charge.

As the temperature increases, average kinetic energy of molecules increases. With increase in temperature at constant volume, the pressure -  

1. Increases

2. Decreases

3. Remains same

4. Becomes half

Gases possess characteristic critical temperature which depends upon the magnitude of intermolecular forces between the particles. Following are the critical temperatures of some gases.

From the above data, the order of liquefaction of the given gases is-
(write the order from the gas liquefying first)
1. ${\mathrm{H}}_2,$ $\mathrm{He},$ ${\mathrm{O}}_2,$ ${\mathrm{N}}_2$
2. $\mathrm{He},$ ${\mathrm{O}}_2,$ ${\mathrm{H}}_2,$ ${\mathrm{N}}_2$
3. ${\mathrm{N}}_2,$ ${\mathrm{O}}_2,$ $\mathrm{He,}$ ${\mathrm{H}}_2$
4. ${\mathrm{O}}_2,$ ${\mathrm{N}}_2,$ ${\mathrm{H}}_2,$ $\mathrm{He}$