Molar mass of `UF_(6)` is 176 times as high as that of `H_(2)`, yet at a particular temperature the average kinetic enegy of both is found to be the same-why?

Explanation

According to the kinetic theory of gas, the average kinetic energy of the molecules in a gas is directly proportional to the absolute temperature of the gas, and it does not depend upon the molar mass of the gas. The average kinetic energy of molecule of a gas at temperature TK is given by `(3)/(2)kT`, [k is Boltzmann constant]. since the value of `(3)/(2)kT` is constant at a given temperature and is independent of the mass of the gas molecule, the average kinetic energy of the molecule of a heavier gas will be the same as that of the molecule of a lighter gas. thus, at a givem temperature, the average kinetic energy of a `UF_(6)` molecule will be same as that of a `H_(2)` molecule.