What happens to the pressure when the volume of a gas decreases?

When the volume of a gas decreases, the pressure increases due to the principles outlined in Boyle's Law. Boyle's Law states that for a given mass of gas at constant temperature, the pressure of the gas is inversely proportional to its volume. This means that as the volume decreases, the molecules of the gas are squeezed closer together, which leads to more frequent collisions with the walls of the container. Since pressure is defined as the force exerted per unit area, more frequent collisions translate to an increase in pressure.

Mathematically, this relationship can be expressed by the equation ( PV = k ), where ( P ) is pressure, ( V ) is volume, and ( k ) is a constant corresponding to the specific amount of gas at a constant temperature. Therefore, as volume ( V ) decreases, pressure ( P ) must increase to keep the equation balanced.

Understanding this concept is crucial because it applies to various scenarios in real life, such as the operation of syringes, tire inflation, and even in biological systems involving respiration.