What does Boyle's Law state?

Boyle's Law describes the relationship between the pressure and volume of a gas at constant temperature. Specifically, it states that the volume of a given mass of gas is inversely proportional to its pressure when the temperature is held constant. This means that if the volume of the gas decreases, its pressure increases, and vice versa, as long as the temperature does not change. This relationship can be mathematically expressed as PV = k, where P is the pressure, V is the volume, and k is a constant.

In practical terms, if you were to compress a gas in a sealed container, you would find that as you decrease the volume of the container, the pressure inside the container increases. This principle is vital in various applications, including understanding how syringes function and how gases behave in different environments.

The other statements refer to different gas laws or principles. The first option relates to Gay-Lussac's Law, which connects pressure and temperature at constant volume. The third choice describes Avogadro's Law, which indicates the relationship between volume and the number of moles at constant temperature and pressure. The fourth option incorrectly suggests that a gas's volume is independent of both temperature and pressure, which is not consistent with the behavior of gases.