In the case of hydrogen and oxygen at N.T.P., | vedclass

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(B) The average kinetic energy of a gas molecule is given by the formula $K = \frac{3}{2} k_B T$,where $k_B$ is the Boltzmann constant and $T$ is the

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average kinetic energy per molecule

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(B) The average kinetic energy of a gas molecule is given by the formula $K = \frac{3}{2} k_B T$,where $k_B$ is the Boltzmann constant and $T$ is the absolute temperature.Since both hydrogen and oxygen are at the same $N.T.P.$ (Normal Temperature and Pressure),their temperatures $T$ are identical.Because the average kinetic energy depends only on the temperature,it remains the same for both gases.However,the average momentum depends on the mass of the molecules $(p = \sqrt{3mk_B T})$,which differs for hydrogen and oxygen.Similarly,the kinetic energy per unit volume depends on the number density of the molecules,which varies for different gases at the same $N.T.P.$ if the pressure is defined by the ideal gas law $P = n k_B T$.Therefore,only the average kinetic energy per molecule is the same for both.

In the case of hydrogen and oxygen at $N.T.P.$,which of the following quantities is/are the same?

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