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

Boyle's law states that the pressure of a gas is inversely proportional to its volume when the temperature and the amount of gas remain constant. This means that as the volume of a gas increases, the pressure exerted by that gas decreases.

When the volume increases, the gas molecules have more space to move around, which leads to fewer collisions with the walls of the container. Since pressure is defined as the force exerted by these collisions divided by the area of the walls, a larger volume results in a lower frequency of collisions, hence a decrease in pressure. This principle is fundamental in understanding gas behavior and is widely applicable in various scientific and real-world contexts, such as in breathing mechanics or when manipulating gas in laboratory settings.

In summary, an increase in volume directly leads to a decrease in pressure, making the correct answer an essential aspect of understanding gas laws in the context of human anatomy and physiology.