What is the relationship between pressure and volume in Boyle’s Law?

Boyle's Law describes the relationship between the pressure and volume of a gas when the temperature and the amount of gas are held constant. According to Boyle's Law, pressure and volume are inversely proportional, which means that as the volume of a gas decreases, the pressure increases, and vice versa. This relationship can be expressed mathematically as P1V1 = P2V2, where P is the pressure and V is the volume of the gas at two different states.

The underlying principle of this relationship is based on the kinetic molecular theory, which asserts that gas particles are in constant motion. When the volume is reduced, gas particles have less space to move around, resulting in more frequent collisions with the walls of the container. This increased frequency of collisions leads to higher pressure. Conversely, if the volume is increased, gas particles have more space to move, resulting in fewer collisions and therefore lower pressure.

This inverse relationship is a fundamental concept in gas laws and is crucial for understanding how gases behave under varying conditions.