The temperature of a gas is $-73^{\circ}C$. To what temperature in $^{\circ}C$ should the gas be heated so that the average kinetic energy of its molecules becomes doubled?

$A$ flask contains argon and chlorine in the ratio of $2:1$ by mass. The temperature of the mixture is $27^{\circ} C$. The ratio of average kinetic energies of two gases per molecule is (in $:1$)

The initial average kinetic energy of the molecules was $E$,when a gas sample is at $27^{\circ} C$. When the gas is heated to $327^{\circ} C$,then the final average kinetic energy will be

The internal energy of a monoatomic ideal gas molecule is

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:

The pressure exerted by the gas on the walls of the container is because: