At absolute zero temperature, the kinetic energy of gas molecules theoretically becomes:

Vessel $A$ is filled with hydrogen while vessel $B,$ whose volume is twice that of $A,$ is filled with the same mass of oxygen at the same temperature. The ratio of the mean kinetic energies of hydrogen and oxygen is

The temperature of an ideal gas is increased from ${27^ \circ }C$ to ${127^ \circ }C,$ then percentage increase in ${V_{rms}}$ is

At constant volume, temperature is increased. Then

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

A sealed container with negligible coefficient of volumetric expansion contains helium (a monoatomic gas). When it is heated from $300\;K$ to $600\;K$ the average K.E. of helium atoms is

The molecular weights of ${O_2}$ and ${N_2}$ are 32 and 28 respectively. At ${15^ \circ }C,$ the pressure of $1\;g\;{O_2}$ will be the same as that of $1\;g\;{N_2}$ in the same bottle at the temperature

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

If the average kinetic energy of gas molecules increases, the temperature of the gas will:

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