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.

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.

The condition of SATP refers to:

1. 25 $°$C and 2 atm             

2. 25 $°$C  and 1 atm

3. 0 $°$C  and 2 atm             

4. 25 $°$C  and 1 bar

If 300 ml of a gas at 27°C is cooled to 7°C at constant pressure, its final volume will be:

Boyle's law is applicable in :

1. Isobaric process

2. Isochoric process

3. Isothermal process

4. Adiabatic process

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

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

V versus T curves at constant pressure P₁ and P₂ for an ideal gas are as shown in the figure. The correct statement is-

1. P₁>P₂

2. P₁<P₂

3. P₁=P₂

4. All of the above

At 0^°C, the density of a certain oxide of a gas at 2 bar is the same as that of dinitrogen at 5 bar.

The molecular mass of the oxide would be -

1. 35 g/mol

2. 45 g/mol

3. 70 g/mol

4. 60 g/mol

A 200 mL flask having oxygen at 220 mm and a 300 mL flask having nitrogen at 100 mm are connected in such a way that ${\mathrm{O}}_2<mspace\; width="1em"></mspace>\mathrm{and}<mspace\; width="1em"></mspace>{\mathrm{N}}_2$ may combine in their volumes if temperature is kept constant. The total pressure of the gaseous mixture is-

1. 158 mm

2. 138 mm

3. 148 mm

4. 168 mm