The curve between absolute temperature and \(\mathrm{v}^2_{rms}\)${\mathrm{}}^{}$ is:

1.		2.
3.		4.

The root-mean-square (RMS) speed of oxygen molecules $\left(O_2\right)$ at a certain absolute temperature is v. If the temperature is doubled and the oxygen gas dissociates into atomic oxygen, the RMS speed would be:

1. V                       

2. $\sqrt{2}v$

3. 2 v                     

4. 2 $\sqrt{2}v$

At what temperature is the root mean square speed of molecules of hydrogen twice as that at STP?
1. \(273\) K
2. \(546\) K
3. \(819\) K
4. \(1092\) K

 Volume, pressure, and temperature of an ideal gas are \(V,\) \(P,\) and \(T\) respectively. If the mass of its molecule is \(m\), then its density is: [\(k\)=Boltzmann's constant]

In the adjacent V-T diagram what is the relation between $P_{1 }and P_2$ ?

1. $P_2=P_1$                               

2. $P_2>P_1$

3. $P_2<P_1$                                 

4. cannot be predicated
 

Which one of the following graph is correct at constant pressure?

1.		2.
3.		4.

The equation $\left(p+\frac{a}{v^2}\right)\left(v-b\right)=RT$ is known as:

1. Perfect gas equation

2. Joule Thomson's equation

3. Vander Waal's equation

4. Maxwell's equation

The temperature of an ideal gas is increased from $27°$ to $927°C$. The r.m.s. speed of its molecules becomes-

1. twice           

2. half           

3. four times         

4. one fourth

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

Molecular weight of two gases are \(M_1\) 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. \(\sqrt{\frac{M_1-M_2}{M_1+M_2}}\)