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(D) The average kinetic energy $(K_{avg})$ of an ideal gas molecule is given by the formula: $K_{avg} = \frac{3}{2} k_B T$,where $k_B$ is the Boltzman

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Both $(B)$ and $(C)$

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(D) The average kinetic energy $(K_{avg})$ of an ideal gas molecule is given by the formula: $K_{avg} = \frac{3}{2} k_B T$,where $k_B$ is the Boltzmann constant and $T$ is the absolute temperature.From this formula,it is clear that the average kinetic energy depends only on the absolute temperature $(T)$.It does not depend on the nature of the gas (e.g.,whether it is monoatomic or diatomic) or the pressure $(P)$ or volume $(V)$ of the gas.Therefore,the average kinetic energy of gas molecules does not depend on the nature of the gas or the pressure.

Average kinetic energy of gas molecules does not depend on which factors?

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