The mean free path of the molecules of a certain gas at `300 K` is `2.6xx10^(-5)m`. The collision diameter of the molecule is `0.26m`. Calculate (`a`) the pressure of the gas and (`b`) the number per unit volume of the gas.

Explanation

To solve the problem step by step, we will calculate the pressure of the gas and the number of molecules per unit volume using the given mean free path and collision diameter.

### Given Data:
- Mean free path, \( \lambda = 2.6 \times 10^{-5} \, \text{m} \)
- Collision diameter, \( \sigma = 0.26 \, \text{m} \)
- Temperature, \( T = 300 \, \text{K} \)
- Boltzmann constant, \( k = 1.38 \times 10^{-23} \, \text{J/K} \)

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