The ratio of the mean kinetic energy of hydrogen and nitrogen at temperatures $300 \, K$ and $450 \, K$ respectively is:

In an ideal gas at temperature $T$,the average force that a molecule applies on the walls of a closed container depends on $T$ as $T^{x}$. The value of $x$ is

The pressure exerted by a gas is $P_0$. If the mass of the molecules is halved and their velocity is doubled,the pressure will become .......

An ideal gas in a container of volume $500 \text{ c.c.}$ is at a pressure of $2 \times 10^5 \text{ N/m}^2$. The average kinetic energy of each molecule is $6 \times 10^{-21} \text{ J}$. The number of gas molecules in the container is:

Consider a gas with density $\rho$ and $\bar{c}$ as the root mean square velocity of its molecules contained in a volume. If the system moves as a whole with velocity $v$,then the pressure exerted by the gas is

Pressure of an ideal gas is increased by keeping temperature constant. What is the effect on the kinetic energy of molecules?