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.

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MysticalPoet MysticalPoet · Answer 1 · 2017-06-27T16:51:26+02:00

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

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shirleywashington shirleywashington · Answer 2 · 2019-03-22T11:14:20+01:00

Answer: Average distance between gas molecules become double.

Explanation :

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

[tex]\lambda=\dfrac{RT}{\sqrt{2}\pi d^2N_AP }}[/tex]

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, [tex]P=\dfrac{nRT}{V}[/tex]

So, [tex]\lambda\propto \dfrac{1}{P}[/tex]

So, [tex]\lambda \propto V[/tex]

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