In the context of gas laws, what is true about the volume of a gas under Boyle’s Law?

Under Boyle's Law, the relationship between the volume and pressure of a gas at constant temperature is fundamental. Boyle's Law states that the volume of a gas is inversely proportional to its pressure when the temperature remains constant. This means that as the pressure on a gas increases, the volume of that gas decreases, assuming no change in temperature.

This relationship can be expressed mathematically as ( P \times V = k ) (where ( k ) is a constant). If the pressure is increased, the volume must decrease to maintain the constant value of ( k ). This principle helps explain various real-world scenarios, such as how a syringe works: pushing the plunger increases the pressure inside the barrel, causing the volume of gas (or liquid) inside to decrease.

Understanding Boyle's Law is crucial for divers and those dealing with gases at varying pressures, as it affects how gases behave underwater.