One litre of gas A and two litres of gas B, both having the same temperature 100$°$C and the same pressure 2.5 bar will have the ratio of kinetic energies of their molecules as:

(1) 1:1       (2) 1:2       (3) 1:4         (4) 4:1

An ideal gas is filled in a vessel, then

(1) If it is placed inside a moving train, its temperature increases

(2) Its centre of mass moves randomly

(3) Its temperature remains constant in a moving car

(4) None of these

If P is the pressure of the gas then the KE per unit volume of the gas is:

1.  $\frac{P}{2}$

2.  $P$

3.  $\frac{3P}{2}$

4.  $2P$

A gas mixture consists of 2 moles of oxygen and 4 moles of argon at temperature T. Neglecting all vibrational modes, the total internal energy of the system is

1.  4RT

2.  15RT

3.  9RT

4.  11RT

For an ideal gas V-T curves at constant pressure ${\mathrm{P}}_1$ and ${\mathrm{P}}_2$ are shown in figure. From the figure

1. ${\mathrm{P}}_1>{\mathrm{P}}_2$

2. ${\mathrm{P}}_1<{\mathrm{P}}_2$

3. ${\mathrm{P}}_1={\mathrm{P}}_2$

4. ${\mathrm{P}}_1\le {\mathrm{P}}_2$

\(4.0 ~\text g\) of a gas occupies \(22.4~\text L\) at NTP. The specific heat capacity of the gas at constant volume is \(5.0 ~\text{J K}^{-1}\text{mol}^{-1}.\) If the speed of sound in this gas at NTP is \(952~\text{m/s}\) then the heat capacity at constant pressure is:
(Take gas constant \(R=8.3 ~\text{J K}^{-1}\text{mol}^{-1}\))
1.  \(8 ~\text{J K}^{-1}\text{mol}^{-1}\)
2.  \(7.5 ~\text{J K}^{-1}\text{mol}^{-1}\)
3.  \(7.0 ~\text{J K}^{-1}\text{mol}^{-1}\)
4.  \(8.5 ~\text{J K}^{-1}\text{mol}^{-1}\)

The mean free path of gas A, with molecular diameter equal to 4 Å, contained in a vessel, at a pressure of ${10}^{–6}$ torr, is 6990 cm. The vessel is evacuated and then filled with gas B, with molecular diameter, equal to 2 Å, at a pressure of ${10}^{–3}$ torr, the temperature remaining the same. The mean free path of gas B will be

(A) 28 cm                       

(B) 280 cm

(C) 7 cm                         

(D) 14 cm

The mean free path of gas molecules depends on:
(\(d=\) molecular diameter)
1. \(d\)
2. \(d^2\)
3. \(d^{-2}\)
4. \(d^{-1}\)

A gas at 27°C temperature and 30 atmospheric pressure is allowed to expand to the atmospheric pressure. If the volume becomes 10 times its initial volume, then the final temperature becomes

1.  100°C                             

2.  173°C

3.  273°C                             

4.  – 173°C

The equation of state for 5 g of oxygen at a pressure P and temperature T, when occupying a volume V, will be

1. $\mathrm{PV}=\left(5/32\right)\mathrm{RT}$                               

2. $\mathrm{PV}=5\mathrm{RT}$

3. $\mathrm{PV}=\left(5/2\right)\mathrm{RT}$                                 

4. $\mathrm{PV}=\left(5/16\right)\mathrm{RT}$

(where R is the gas constant)