According to Boyle's Law, how does pressure affect the volume of gas?

Boyle's Law states that for a given amount of gas at a constant temperature, the volume of the gas is inversely proportional to the pressure exerted on it. This principle means that as pressure increases, the volume of the gas decreases, provided the temperature remains constant. This is a fundamental concept in understanding gas behavior and is particularly important in diving, as changes in pressure occur with depth.

In practical terms, if a diver descends and experiences increased pressure, the volume of any trapped air in their buoyancy control device or in their lungs will decrease. This is a crucial consideration for divers to avoid issues such as barotrauma. Conversely, if a diver ascends and the pressure decreases, the volume of gas will expand, which could lead to overexpansion injuries if not managed properly.

Understanding this relationship is essential for divers to manage their buoyancy effectively and to prevent accidents associated with pressure changes during dives.