What is the relationship between Boyle's law and the kinetic theory?

Question

Avery Adams · Accepted Answer

In qualitative terms, the relationship is the following.
According to the Kinetic Theory, the pressure of a gas is due to the elastic collisions of its molecules upon the container's wall. If the temperature is kept constant the average speed of molecules is constant, thus the pressure can change only if the frequency of the collisions changes.
This is what happens by reducing the volume (the molecules become more crowded, thus making the rate of collisions and pressure increasing) or expanding the container (the molecules become more rarefied, so the rate of collisions and pressure decrease).

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Jose Ayala · Answer

undefined Boyle's law describes the inverse relationship between the pressure and volume of a gas at constant temperature. According to the kinetic theory of gases, gases consist of particles in constant, random motion. Boyle's law can be explained by the kinetic theory as follows: When the volume of a gas decreases, the gas particles have less space to move, so they collide more frequently with the walls of the container, leading to an increase in pressure. Conversely, when the volume increases, the gas particles have more space to move, resulting in fewer collisions with the walls and a decrease in pressure.