Question

A container with a specific volume “V” changes to “2V.” What happens to the average distance between gas molecules? Assume that pressure and temperature of the gas remain constant.

Answer 1

As the volume increases, there is more space so the average distance between the gas molecules also increases.

Answer 2

Answer: Average distance between gas molecules become double.

Explanation :

Average distance or mean free path of a gas molecule is given as :

`\lambda=(RT)/(√(2)\pi d^2N_AP )}`

Where,

R is gas constant

T is temperature

d is the radius of the gas molecule

P is the pressure

We know that all values except P are constant.

Also,
`P=(nRT)/(V)`

So,
`\lambda\propto (1)/(P)`

So,
`\lambda \propto V`

When a container with a specific volume “V” changes to “2V. Then the average distance between the gas molecules become double