According to Boyle's law, what happens to the volume of a gas as pressure increases?

Boyle's law states that for a given mass of gas at constant temperature, the volume of the gas is inversely proportional to the pressure applied to it. This means that as the pressure increases, the volume of the gas decreases, provided that the temperature remains constant. This relationship can be mathematically expressed as PV = k, where P represents pressure, V represents volume, and k is a constant for a given amount of gas.

When pressure is applied to a gas, the molecules are forced closer together, leading to a decrease in volume. In practical terms, when divers descend underwater, they experience increased pressure, which causes the air in their lungs and equipment to compress, reducing volume. Understanding this principle is crucial for divers to manage their buoyancy and avoid issues like barotrauma, which occurs when air-filled spaces in the body, such as ears and lungs, cannot equalize with the surrounding pressure.