Which gas law indicates that the pressure of a gas is inversely proportional to its volume at constant temperature?

Boyle's law is the correct choice as it specifically states that the pressure of a gas is inversely proportional to its volume when the temperature is held constant. This means that as the volume of a gas decreases, the pressure increases, and vice versa. This relationship can be mathematically represented as (PV = k), where (P) is the pressure, (V) is the volume, and (k) is a constant for a given sample of gas at a constant temperature.

Understanding this principle is fundamental in various applications, especially in fields like medicine and aviation, where pressure changes can occur in environments such as flight. Boyle's law is a result of the kinetic molecular theory, which explains that gas particles are in constant motion and that their collisions with the walls of a container result in pressure.

In contrast, Dalton's law pertains to the total pressure exerted by a mixture of gases being equal to the sum of the partial pressures of individual gases, Graham's law describes the rates at which gases effuse or diffuse relative to their molar masses, and Henry's law focuses on the amount of gas that dissolves in a liquid being proportional to the partial pressure of that gas above the liquid. Each of these laws addresses