$A$ mixture of $2$ moles of oxygen and $4$ moles of argon is kept at temperature $T$. Neglecting all internal vibrations,the total internal energy of the system is: (in $, RT$)

Two moles of a monoatomic gas are mixed with six moles of a diatomic gas. The molar specific heat of the mixture at constant volume is:

If $2 \text{ mole}$ of an ideal monoatomic gas at temperature $T$ is mixed with $6 \text{ mole}$ of another ideal monoatomic gas at temperature $2T$, then the temperature of the mixture is:

$A$ gaseous mixture has $2$ moles of oxygen and $4$ moles of Argon at a temperature $T$. Neglecting all vibrational modes of the molecules,the total internal energy of the system is ($R$ = Universal gas constant). (in $RT$)

One mole of a monoatomic ideal gas is mixed with one mole of a diatomic ideal gas. The molar specific heat of the mixture at constant volume is

$A$ vessel contains a mixture of one mole of oxygen and two moles of nitrogen at $300 K$. The ratio of the average rotational kinetic energy per $O_2$ molecule to that per $N_2$ molecule is