What is the relationship between the mean free path and the diameter of gas mole

What is the relationship between the mean free path and the diameter of gas molecules?

What is the relationship between the mean free path and the diameter of gas molecules?

Step 1: Understand what mean free path means. It is the average distance a gas molecule travels before colliding with another molecule.
Step 2: Know that gas molecules have a certain size, which is referred to as their diameter.
Step 3: Realize that if gas molecules are larger (have a bigger diameter), they take up more space.
Step 4: When gas molecules are larger, they are more likely to collide with each other more often.
Step 5: Because of these more frequent collisions, the distance a molecule can travel (mean free path) before hitting another molecule becomes shorter.
Step 6: Therefore, if the diameter of gas molecules increases, the mean free path decreases.
Step 7: This means that the mean free path is inversely proportional to the diameter of gas molecules.

No concepts available.