What happens to the volume of a gas in a sealed container when the pressure increases, according to Boyle's Law?

According to Boyle's Law, the relationship between the pressure and volume of a gas in a sealed container is inverse; as the pressure increases, the volume of the gas decreases. This principle is based on the fact that gas particles are in constant motion and occupy space. When the pressure in the container rises—perhaps due to the addition of more gas or a decrease in volume—the gas particles are forced closer together.

The mathematical expression of Boyle's Law, which states that pressure multiplied by volume equals a constant (P1V1 = P2V2), supports this relationship. If the pressure increases (P2 > P1), the volume (V2) must decrease to keep the equation balanced. This fundamental principle of physics is critical for understanding how gases behave under different conditions as it applies to many practical scenarios in scuba diving and other fields involving gases.