As the volume of confined gas decreases at constant temperature, what happens to the pressure exerted by the gas?

The relationship between the volume of a confined gas and its pressure at constant temperature is described by Boyle's Law. According to Boyle's Law, if the temperature remains constant, the pressure of a gas is inversely proportional to its volume. This means that as the volume decreases, the gas molecules are forced closer together, leading to more frequent collisions with the walls of the container. Each collision exerts force, contributing to an increase in pressure.

Thus, when the volume of the gas decreases, the pressure increases. This principle is fundamental in understanding how gases behave under varying conditions and is critical in applications such as breathing mechanisms in the lungs and in various industrial processes involving gases.