What does Boyle's Law state regarding gas volume and pressure when temperature remains constant?

Boyle's Law states that at constant temperature, the volume of a gas is inversely proportional to its pressure. This means that as the pressure of a gas increases, its volume decreases, and vice versa. The relationship can be mathematically expressed as PV = k, where P is pressure, V is volume, and k is a constant for a given amount of gas at a constant temperature.

In practical terms, if you compress a gas into a smaller volume (increasing the pressure), the molecules have less space to move and collide, resulting in an increase in pressure. Conversely, if the gas expands, the pressure decreases as the molecules have more space to move, allowing for a larger volume. This fundamental principle is crucial in various fields, including aviation and medicine, as it helps explain how gases behave under different atmospheric conditions. Understanding this concept is essential for comprehending how changes in altitude affect the pressure and volume of gases in the human body and in aircraft cabins.