The total internal energy of $4$ moles of a diatomic gas at a temperature of $27^{\circ} C$ is (Universal gas constant $R = 8.31 \ J \ mol^{-1} \ K^{-1}$) (in $kJ$)

The average kinetic energy of a gas at $-23^{\circ}C$ and $75 \, cm$ pressure is $5 \times 10^{-14} \, erg$ for $H_2$. The mean kinetic energy of $O_2$ at $227^{\circ}C$ and $150 \, cm$ pressure will be:

$A$ gas is contained in a vessel at pressure $P_0$. If the mass of all molecules is halved and their speed is doubled,what will be the final pressure?

Discuss the main points to be considered while deriving the equation of pressure on the basis of the kinetic theory of gases.

At what temperature is the kinetic energy of a gas molecule double that of its value at $27^{\circ}C$?

$E_0$ and $E_H$ respectively represent the average kinetic energy of a molecule of oxygen and hydrogen. If the two gases are at the same temperature,which of the following statements is true?