The kinetic energy of translation of the molecules in $50 \text{ g}$ of $\text{CO}_2$ gas at $17^{\circ}\text{C}$ is: (in $\text{ J}$)

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:

If $10^{22}$ gas molecules,each of mass $10^{-26} \ kg$,collide with a surface (perpendicular to it) elastically per second over an area of $1 \ m^2$ with a speed of $10^4 \ m/s$,the pressure exerted by the gas molecules will be of the order of:

If the average translational kinetic energy of a molecule in a gas is equal to the kinetic energy of an electron accelerating from rest through $10 \,V$, then the temperature of the gas molecule is (Boltzmann constant $= 1.38 \times 10^{-23} \,JK^{-1}$)

$A$ gas at a pressure ${P_0}$ is contained in a vessel. If the masses of all the molecules are halved and their speeds are doubled,the resulting pressure $P$ will be equal to:

If the mass of each molecule of a gas kept at a constant pressure $P$ in a container is halved and their speed is doubled,what will be the resulting pressure of the gas?