The average speed of gas molecules is v at pressure P. If by keeping the temperature constant, the pressure of the gas is doubled, then average speed will become:

(1) $\sqrt{2}v$

(2) v

(3) 2v

(4) $\frac{v}{\sqrt{2}}$

Four molecules of a gas have speeds of 1, 2, 3 and 4 km/s. The value of the r.m.s. speed of the gas molecules is:

(1) $\frac{1}{2}\sqrt{15} \mathrm{km}/\mathrm{s}$

(2) $\frac{1}{2}\sqrt{10} \mathrm{km}/\mathrm{s}$

(3) 2.5 km/s

(4) $\sqrt{\frac{15}{2}} \mathrm{km}/\mathrm{s}$

The rms speed of the molecules of an enclosed gas is \(v\). What will be the rms speed if the pressure is doubled, keeping the temperature constant?

The ratio of number of collisions per second at the walls of containers by He and O₂ gas molecules kept at the same volume and temperature is: (assume normal incidence on walls)

(1) 2: 1

(2) 1: 2

(3) $2\sqrt{2}$: 1

(4) 1: $2\sqrt{2}$

An ant is moving on a plane's horizontal surface. The number of degrees of freedom of the ant will be:
1. 1
2. 2
3. 3
4. 6

If a gas has 'f' degree of freedom, the ratio of the specific heats of the gases, $\frac{{\mathrm{C}}_{\mathrm{P}}}{{\mathrm{C}}_{\mathrm{V}}}$ is

(1) $\frac{1+\mathrm{f}}{2}$

(2) $1+\frac{\mathrm{f}}{2}$

(3) $1+\frac{1}{\mathrm{f}}$

(4) $1+\frac{2}{\mathrm{f}}$

Molar specific heat at constant volume, for a non-linear triatomic gas is: (vibration mode neglected)

(1) 3R

(2) 4R

(3) 2R

(4) R

A mixture of ideal gases has 2 moles of He, 4 moles of oxygen and 1 mole of ozone at absolute temperature T. The internal energy of the mixture is:

(1) 13RT

(2) 11RT

(3) 16RT

(4) 14RT

E₀ and E_H respectively represent the average kinetic energy of a molecule of oxygen and hydrogen. If the two gases are at the same temperature, which of the following statement is true?

(1) E₀  > E_H

(2) E₀  = E_H

(3) E₀  < E_H

(4) Data insufficient

14 g of CO at 27 ^oC is mixed with 16 g of O₂ at 47 ^oC. The temperature of the mixture is: (vibration mode neglected)

(1) - 5 ^oC

(2) 32 ^oC

(3) 37 ^oC

(4) 27 ^oC