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(B) 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

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increase

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(B) 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 diameter of the molecule,and $P$ is the pressure of the gas.From the formula,it is clear that the mean free path $\lambda$ is inversely proportional to the pressure $P$ (i.e.,$\lambda \propto \frac{1}{P}$).Therefore,if the pressure $P$ is reduced,the mean free path $\lambda$ will increase because the molecules will travel a longer distance on average before colliding with another molecule.

If the pressure of a gas in a closed container is reduced,the mean free path of the molecules will ......

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