What is the key assumption of the Kinetic Model of Gases regarding the size of gas molecules?

The Kinetic Model of Gases is built on several assumptions that help to describe the behavior of gases in a simplified manner. One of the key assumptions is that the size of the gas molecules is negligible compared to the distances between them. This means that when considering the motion and interactions of gas particles, their individual sizes do not significantly affect their overall behavior as a gas.

This assumption allows for the simplification of calculations involving gas pressure and volume. Essentially, it treats gas molecules as point particles, which can move freely and collide elastically with one another and with the walls of their container without considering the volume occupied by the molecules themselves. By ignoring the volume of the molecules, the model can effectively describe gas behavior using the Ideal Gas Law and other fundamental principles.

In real-world applications, while gas molecules do have size, at typical conditions (such as low pressure and high temperature), this assumption holds true for most gases, making it a practical and crucial aspect of the kinetic theory.