Law of Equipartition of Energy

Rigid diatomic molecules of gas have how many rotational degrees of freedom?

The total number of degrees of freedom for a non-rigid diatomic molecule is equal to:

The number of translational degrees of freedom for a diatomic gas is 

Two ideal monatomic gases $\mathrm{A}$ and $\mathrm{B}$ at $27 \mathrm{℃}$ and $37 \mathrm{℃}$ are mixed. The number of moles in gas $\mathrm{A}$ is $2$ and number of moles in gas $\mathrm{B}$ is $3$. What will be the temperature of the mixture?

According to the kinetic theory of gases, for a diatomic molecule

Molecule of a gas can be modelled as three sphere connected through three rigid rods as to make triangle like structure. A gas containing such molecules performs 25 J of work when it expands at constant pressure. Heat given to gas is –

Five grams of helium having rms speed of molecules $1000 \mathrm{m} {\mathrm{s}}^{-1}$ and $24 \mathrm{g}$ of oxygen having rms of $1000 \mathrm{m} {\mathrm{s}}^{-1}$ are introduced into a thermally isolated vessel. Find the rms speed of helium and oxygen individually when thermal equilibrium is attained. Neglect the heat capacity of the vessel.

If the temperature of $3$ moles of helium gas is increased by $2 \mathrm{K}$., then the change in the internal energy of helium gas is

In a model of chlorine (${\mathrm{Cl}}_2$), two $\mathrm{Cl}$ atoms are rotated about their centre of mass as shown. Here the two '$\mathrm{Cl}$' atoms are $2\times {10}^{-10} \mathrm{m}$ apart and angular speed $\omega =2\times 10^{12} \mathrm{rad} {\mathrm{s}}^{-1}$. If the molar mass of chlorine is $70 \mathrm{g} {\mathrm{mol}}^{-1}$, then the rotational kinetic energy of one ${\mathrm{Cl}}_2$ molecule is


                        

Find the temperature of the mixture, if two perfectly monoatomic gases at absolute temperatures $T_1$ and $T_2$ number of moles in the gases are $n_1$ and $n_2$, respectively are mixed. Assume no loss of energy

If at a pressure of $106 \mathrm{dyne} {\mathrm{cm}}^{-2}$, $1 \mathrm{gram}$ mole of nitrogen occupies $2\times {10}^4 {\mathrm{cm}}^3$ volume, then calculate the average energy of nitrogen molecules in $\mathrm{erg}$
(Given : Avogadro's number = $6\times {10}^{23}$)