What does Boyle’s Law describe about pressure and volume?

Boyle’s Law states that at constant temperature, the pressure of a gas is inversely proportional to its volume. This relationship indicates that as the volume of a gas decreases, the pressure increases, provided the temperature remains constant. This principle is critical for understanding how gases behave under different conditions, particularly in diving, where changes in depth can affect pressure and volume of gases in a diver's lungs and equipment.

For example, if a diver ascends to shallower depths, the volume of air in their lungs will expand due to the decrease in external pressure, which can result in potential complications if not managed properly, such as pulmonary barotrauma. This is why diver training emphasizes the significance of Boyle's Law in planning ascents and managing air consumption effectively while underwater.

Understanding the inverse relationship underscores the importance of proper ascent rates and equalization techniques, ensuring divers can safely manage pressure changes during their underwater activities.