Maxwell's velocity distribution curve is given for two different temperatures. For the given curves-
                    

1. $T_1>T_2$
2. $T_1<T_2$
3. $T_1\le T_2$
4. $T_1=T_2$

${\mathrm{n}}_1$ mole of monoatomic gas is mixed with ${\mathrm{n}}_2$ mole of diatomic gas such that ${\gamma }_{mix}=1.5$, then:

1. ${\mathrm{n}}_1=2{\mathrm{n}}_2$

2. ${\mathrm{n}}_2=2{\mathrm{n}}_1$

3. $n_1=n_2$

4. $n_1=3n_2$

$\mathrm{Molar}<mspace\; width="1em"></mspace>\mathrm{heat}<mspace\; width="1em"></mspace>\mathrm{capacity}<mspace\; width="1em"></mspace>\mathrm{of}<mspace\; width="1em"></mspace>\mathrm{the}<mspace\; width="1em"></mspace>\mathrm{process}<mspace\; width="1em"></mspace>\mathrm{P}<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>\frac{\mathrm{a}}{\mathrm{T}}<mspace\; width="1em"></mspace>\mathrm{for}<mspace\; width="1em"></mspace>\mathrm{a}<mspace\; width="1em"></mspace>\mathrm{monoatomic}<mspace\; width="1em"></mspace>\mathrm{gas},<mspace\; width="1em"></mspace>\text{'}\mathrm{a}\text{'}<mspace\; width="1em"></mspace>\mathrm{being}<mspace\; width="1em"></mspace>\mathrm{positive}<mspace\; width="1em"></mspace>\mathrm{constant}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>is-$

1.  $\frac{7}{2}<mspace\; width="1em"></mspace>\mathrm{R}<mspace\; width="1em"></mspace>$

2.  $\frac{5}{2}<mspace\; width="1em"></mspace>\mathrm{R}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>$

3.  $\frac{3}{2}<mspace\; width="1em"></mspace>\mathrm{R}$

4.  None of these

A rocket is propelled by a gas which is initially at a temperature of 4000 K. The temperature of the gas falls to 1000 K as it leaves the exhaust nozzle. The gas which will acquire the largest momentum while leaving the nozzle is:

1. Hydrogen

2. Helium

3. Nitrogen

4. Argon

The variation of density (p) of gas with its absolute temperature (T) at constant pressure is best represented by the graph

1.		2.
3.		4.

The variation of pressure versus temperature of an ideal gas is shown in the given diagram. From this diagram, one can conclude that

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

1.  $\frac{P}{2}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>$

2.  $P<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>$

3.  $<mspace\; width="1em"></mspace>\frac{3P}{2}<mspace\; width="1em"></mspace>$

4.  $<mspace\; width="1em"></mspace>2P$

The root mean square speed of oxygen molecules (O2) at a certain absolute temperature is v. If the temperature is doubled and oxygen gas dissociates into oxygen atom, the rms speed would be :

1.  $\mathrm{v}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>$

2.  $\sqrt{2}\mathrm{v}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>$

3.  $2\mathrm{v}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>$

4.  $2\sqrt{2}\mathrm{v}$

A gas mixture consist of 2 moles of $O_2$ and 4 moles of Ar at temperature T. Neglecting all vibrational modes, the total internal energy of the system is:

1. 4RT 

2. 15RT

3. 9RT

4. 11RT

One mole of an ideal monatomic gas undergoes a process described by the equation $P{V}^3=$ constant. The heat capacity of the gas during this process is:

1. $\frac{3}{2}R$           

2. $\frac{5}{2}R$

3. $2R$             

4. $R$