In the kinetic theory of gases,a molecule of mass $m$ of an ideal gas collides with a wall of a vessel with velocity $V$. The change in the linear momentum of the molecule is

The average force applied on the walls of a closed container depends as $T^{x}$ where $T$ is the temperature of an ideal gas. The value of $x$ 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:

The relation between the pressure $(P)$,volume $(V)$,and average kinetic energy $(E)$ of a gas 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

At which of the following temperatures would the molecules of a gas have twice the average kinetic energy they have at $20^{\circ}C$ (in $^{\circ}C$)?