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(A) The mean free path $\lambda$ of a gas molecule is given by the formula $\lambda = \frac{k_B T}{\sqrt{2} \pi d^2 P}$,where $k_B$ is the Boltzmann c

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Directly proportional to temperature

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(A) The mean free path $\lambda$ of a gas molecule is given by the formula $\lambda = \frac{k_B T}{\sqrt{2} \pi d^2 P}$,where $k_B$ is the Boltzmann constant,$T$ is the absolute temperature,$d$ is the molecular diameter,and $P$ is the pressure.Assuming the pressure $P$ remains constant,the mean free path $\lambda$ is directly proportional to the absolute temperature $T$ (i.e.,$\lambda \propto T$).

How does the mean free path of a gas depend on temperature?

Similar Questions

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