Which gas law describes the relationship between volume and pressure of a gas?

Boyle's Law describes the relationship between the volume and pressure of a gas, indicating that at constant temperature, the pressure of a gas is inversely proportional to its volume. This means that if the volume of a gas decreases, its pressure increases, and vice versa, as long as the temperature remains unchanged. This relationship can be mathematically expressed as ( P_1V_1 = P_2V_2 ), where ( P ) represents pressure and ( V ) represents volume. Boyle's Law is fundamental in understanding how gases behave under changing conditions.

In contrast, Charles's Law deals with the relationship between volume and temperature, stating that gas volume increases with increasing temperature when pressure is held constant. Avogadro's Law pertains to the volume of gas and the amount of substance, emphasizing how volume relates to the number of moles when the temperature and pressure are constant. Graham's Law focuses on the rates of effusion and diffusion of gases, illustrating how these rates relate to molar mass. Each of these laws describes different aspects of gas behavior, but Boyle's Law specifically targets the inverse relationship between volume and pressure.