What relationship does Boyle's Law describe between volume and pressure at constant temperature?

Boyle's Law describes an inverse relationship between volume and pressure when the temperature of a gas is held constant. This means that as the volume of a gas decreases, the pressure exerted by that gas increases, and the reverse is also true: if the volume increases, the pressure decreases.

This principle can be observed in various real-life scenarios, such as when a syringe is used. When the plunger is pulled back (increasing the volume inside the syringe), the pressure inside the syringe drops, allowing a fluid to be drawn in. Conversely, pushing the plunger in decreases the volume, leading to an increase in pressure and forcing fluid out.

In summary, Boyle's Law effectively illustrates how gas behavior can be understood through the relationship between volume and pressure, with their involvement being inversely related under conditions of constant temperature.