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(D) The mean free path $\lambda$ of gas molecules is given by the formula: $\lambda = \frac{1}{\sqrt{2} \pi d^2 n_V}$.Here, $d$ is the diameter of the

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gas constant $R$

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(D) The mean free path $\lambda$ of gas molecules is given by the formula: $\lambda = \frac{1}{\sqrt{2} \pi d^2 n_V}$.Here, $d$ is the diameter of the molecule and $n_V$ is the number density of the molecules (number of molecules per unit volume).$1$. The mean free path depends on the number density $(n_V)$.$2$. The mean free path depends on the size (diameter $d$) of the molecule, which is related to the volume of the molecule.$3$. In terms of pressure $P$ and temperature $T$, using the ideal gas law $P = n_V k_B T$, we can write $n_V = \frac{P}{k_B T}$. Thus, $\lambda = \frac{k_B T}{\sqrt{2} \pi d^2 P}$. This shows that the mean free path depends on the temperature $T$ of the gas.$4$. The gas constant $R$ is a universal constant and does not appear in the expression for the mean free path of gas molecules.Therefore, the mean free path is independent of the gas constant $R$.

Mean free path of molecules in a polyatomic gas is independent of

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