0.5 L of H₂ at 0.8 bar and 2.0 L of dioxygen at 0.7 bar are introduced in a 1L vessel at 27°C.

The pressure inside the vessel would be -

1. 3.6 bar

2. 1.8 bar

3. 4.1 bar

4. 0.7 bar

 

A student forgot to add the reaction mixture to the round-bottomed flask at 27 °C but instead, he placed the flask on the flame. After a lapse of time, he realized his mistake and using a pyrometer he found the temperature of the flask was 477 °C. The fraction of air that would  expel out would be :

1. 1/3

2. 4/5

3. 3/5

4. 2/3

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.