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**Hint:**To solve this question, you must recall the formula for mean free path of gas particles. It is the average distance travelled by a gas particle between two successive collisions. We shall calculate the number of molecules present at the given pressure and then substitute the values in the given formula.

**Formula used:**The number of molecules per unit volume is given by,

$N = \dfrac{n}{V} \times {N_A}$

The mean free path is given by:

$\lambda = \dfrac{1}{{\sqrt 2 \pi {\sigma ^2}N}}$

Where, $\lambda $ is the mean free path

$\sigma $ is the molecular diameter

And $N$ is the number of molecules per unit molar volume of the gas.

**Complete step by step solution:**

We can write, ${10^{ - 6{\text{ }}}}{\text{mmHg}} \approx \dfrac{{{\text{1}}{{\text{0}}^{ - 9}}}}{{1.01325}}{\text{ bar}}$

The number of molecules per unit volume is given by,

$N = \dfrac{n}{V} \times {N_A}$

We know from the ideal gas equation, $PV = nRT$

Thus we get, $\dfrac{n}{V} = \dfrac{P}{{RT}}$

So we have the number of molecules per unit volume as,

$N = \dfrac{P}{{RT}} \times {N_A}$

Substituting the values, we get,

$N = \dfrac{{{{10}^{ - 9}}}}{{1.01325 \times 0.0821 \times 300}} \times 6.023 \times {10^{23}}$

$ \Rightarrow N = 2.4 \times {10^{10}}{\text{ molecules/c}}{{\text{m}}^3}$

The mean free path is given by,

$\lambda = \dfrac{1}{{\sqrt 2 \pi {\sigma ^2}N}}$

Substituting the values, we get,

$\lambda = \dfrac{1}{{1.414 \times 3.14 \times {{\left( {460 \times {{10}^{ - 10}}} \right)}^2} \times 2.4 \times {{10}^{10}}}}$

$\therefore \lambda = 4.435 \times {10^3}{\text{cm}}$.

**Additional information:**

The kinetic theory of gases provides an explanation for various experimental observations about a gas. Its postulates are:

a)Each gas is made up of large number of tiny particles

b)The volume of a molecule is negligible as compared to the volume of the gas.

c)There are no attractive forces present between the molecules of the gas.

d)The molecules are never stationary and keep moving in straight line motion until it collides.

e)All collisions are assumed to be completely elastic

**Note:**

a)Based on the kinetic theory of gases, the mean free path is directly proportional to temperature and inversely proportional to the pressure.

b)Larger is the size of a molecule, smaller is the mean free path.

c) Greater the number of molecules per unit volume, smaller is the mean free path

d)Larger the temperature, larger the mean free path

e)And, larger the pressure, lesser is the mean free path.

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