A container of fixed volume holds an ideal gas at a pressure $P$ and temperature $T$. If the root mean square speed of the gas molecules is doubled while maintaining the same number density, what is the new pressure?

Some gas at 300 K is enclosed in a container. Now, the container is placed on a fast moving train. While the train is in motion, the temperature of the gas

8 g of ${{\rm{O}}_2},$ 14 g of ${{\rm{N}}_2}$ and 22 g of ${\rm{C}}{{\rm{O}}_2}$ is mixed in a container of 10 L capacity at 27$^ \circ C$. The pressure exerted by the mixture in terms of atmospheric pressure is

($R = 0.082\;{\rm{L}}\;{\rm{atm}}\;{{\rm{K}}^{ - 1}}\;{\rm{mo}}{{\rm{l}}^{ - 1}})$

The relation between the gas pressure $P$ and average kinetic energy per unit volume $E$ is

The de-Broglie wavelength of a neutron in thermal equilibrium with heavy water at a temperature $T$ (Kelvin) and mass $m$, is

At ${0^ \circ }C$ the density of a fixed mass of a gas divided by pressure is $x.$ At ${100^ \circ }C,$ the ratio will be

The ratio of mean kinetic energy of hydrogen and nitrogen at temperature $300\;K$ and $450\;K$ respectively is

The ideal gas equation connecting Pressure (P) Volume (V) and absolute temperature (T) is (Where ${K_B}$ is the Blotzmann Constant and N is the number of molecules)

For ideal gas, which statement is not true

If the mean free path of atoms is doubled then the pressure of gas will become

If number of molecules of ${H_2}$ are double than that of ${O_2},$ then ratio of kinetic energy of hydrogen and that of oxygen at $300\;K$ is