Two identical containers hold equal moles of different ideal gases, A and B, at the same temperature. Which of the following statements is true about the pressure exerted by the gases?

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

In the nuclear fusion reaction

${}_1^2{\rm{H}}\,\, + \,\,{}_1^3{\rm{H}} o {}_2^4{\rm{H}}e\,\, + \,\,n$

given that the repulsive potential energy between the two nuclei is $7.7\,\, imes \,\,{10^{ - 14}}{\rm{ J}}$, the temperature at which the gases must be heated to initiate the reaction is nearly [Boltzmann’s constant $k = 1.38\,\, imes \,\,{10^{ - 23}}\,\,{\rm{J}}{{\rm{K}}^{ - 1}}$]

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

For a diatomic gas change in internal energy for unit change in temperature for constant volume is ${U_1}$ and ${U_2}$ respectively. ${U_1}:{U_2}$ is

The temperature of a gas is -68$^ \circ C$. At what temperature will the average kinetic energy of its molecules be twice that of at -68$^ \circ C$?

The kinetic energy of one g-mole of a gas at normal temperature and pressure is ($R = 8.31\;J/mol - K$)

The ratio of mean kinetic energy of hydrogen and oxygen at a given temperature is

Air inside a closed container is saturated with water vapour. The air pressure is $p$ and the saturated vapour pressure of water is ${\bar p}$. If the mixture is compressed to one half of its volume by maintaining temperature constant, the pressure becomes

The average kinetic energy of a gas molecules is

Which of the following is NOT a postulate of the kinetic theory of gases?