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(B) The mean free path $\lambda$ of gas molecules 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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$P/2$

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(B) The mean free path $\lambda$ of gas molecules 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 temperature,$d$ is the molecular diameter,and $P$ is the pressure.From this relation,it is clear that the mean free path is inversely proportional to the pressure: $\lambda \propto \frac{1}{P}$.If the mean free path $\lambda$ is doubled (i.e.,$\lambda' = 2\lambda$),then the new pressure $P'$ must satisfy:$P' = \frac{P}{2}$.Therefore,if the mean free path is doubled,the pressure of the gas becomes half of its initial value.

If the mean free path of atoms is doubled,then the pressure of the gas will become:

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