What is the mass of 2 liters of nitrogen at 22.4 atmospheric pressure and 273 K?

1. 28 g               

2. 14$\times 22.4$ g

3. 56 g               

4. None of these

Which one of the following graphs represent the behaviour of an ideal gas at constant temperature?

1.		2.
3.		4.

PV versus T graphs of equal masses of \(H_2\), \(He\) and \(O_2\)${\mathrm{}}_{}$ are shown in the figure. Choose the correct alternative:               

The figure shows two connected flasks. The volume of flask-1 is twice that of flask-2. The system is filled with an ideal gas at temperatures of \(100\) K and \(200\) K, respectively. If the mass of the gas in flask-1 is \(m,\) what is the mass of the gas in flask-2 when the system reaches equilibrium?

      
1. \(m\)         
2. \(m/2\)    
3. \(m/4\)    
4. \(m/8\)

An ideal gas is found to obey an additional law $V{P}^2$= constant. The gas is initially at temperature T and volume V. When it expands to a volume 2 V, the temperature becomes:

1. T $\sqrt{2}$         

2. 2T       

3. 2T$\sqrt{2}$           

4. 4T

The molecular weight of two gases is \(M_1\) and \(M_2.\) At any temperature, the ratio of root mean square velocities \(v_1\) and \(v_2\) will be:
1. \(\sqrt{\frac{M_1}{M_2}}\)
2. \(\sqrt{\frac{M_2}{M_1}}\)
3. \(\sqrt{\frac{M_1+M_2}{M_1-M_2}}\)
4. \(\sqrt{\frac{M_1-M_2}{M_1+M_2}}\)

If the degree of freedom of gas are f, then the ratio of two specific heats $C_P/C_V$ is given by:

[MP PET 1995; BHU 1997; MP PMT 2001, 04]

1. $\frac{2}{f}+1$                 

 2. $1-\frac{2}{f}$

3. $1+\frac{1}{f}$                   

4. $1-\frac{1}{f}$

The root mean square speed of the molecules of an enclosed gas is V.  What will be the root mean square speed if the pressure is doubled, the temperature remaining the same?

1. $\frac{v}{2}$     

2. v         

3. 2       

4. 4 v

From the T-P graph, what conclusion can be drawn?

1. $V_2=V_1$

2. $V_2<V_1$

3. $V_2>V_1$

4. Nothing can be predicted

The equation of state for 5 g of oxygen at a pressure P and temperature T, when occupying a volume V, will be: (where R is the constant)

1. PV = 5RT

2. PV = $\left(\frac{5}{2}\right)RT$

3. PV = $\left(\frac{5}{16}\right)RT$

4. PV = $\left(\frac{5}{32}\right)RT$