On the basis of the kinetic theory of gases, one compares \(1~\text{gm}\) of hydrogen with \(1~\text{gm}\) of argon both at \(0^\circ \text{C}.\) Then:

1.	the same temperature implies that the average kinetic energy of the molecules is the same in both cases.
2.	the same temperature implies that the average potential energy of the molecules is the same in both cases.
3.	the internal energies in both cases are equal.
4.	when both the samples are heated by \(1^\circ \text{C},\) the total energy added to both of them is the same.

Consider a mole of a sample of hydrogen gas at NTP. Then:

Consider the following statements for air molecules in an airtight container:

The true statements are:

An ideal gas is confined in a closed container and slowly heated. As the temperature rises, which of the following statements are correct?

Consider a gas of triatomic molecules. The molecules are assumed to be triangular, composed of massless rigid rods with atoms at the vertices.  The internal energy of a mole of the gas at temperature \(T\) is:

Match the \(C_p/C_V\)  ratio for ideal gases with different type of molecules :
 

The pressure of an ideal gas is written as \(p=\dfrac{2E}{3V},\) where \(E\) is the total kinetic energy, and \(V\) is the volume.
This statement is: