For a given sample of gas, Boyle's Law states the pressure is inversely proportional to what?

Boyle's Law specifically describes the relationship between the pressure and volume of a gas at constant temperature. According to Boyle's Law, for a given amount of gas at a constant temperature, the pressure of the gas is inversely proportional to its volume. This means that if the volume of the gas decreases, the pressure increases, as long as the temperature remains unchanged. Mathematically, this relationship can be expressed as (PV = k), where (P) represents the pressure, (V) is the volume, and (k) is a constant.

Understanding this inverse relationship is essential when analyzing how gases behave under varying conditions. As volume increases, the same amount of gas has more space to occupy, thereby exerting less pressure. Conversely, when the volume decreases, gas particles collide with the walls of the container more frequently, resulting in an increase in pressure.

The other options, such as temperature, molar mass, and density, do not describe this particular inverse relationship characterized by Boyle's Law. Temperature affects the pressure and volume in other gas laws, such as Charles' Law, while molar mass and density relate to different properties of gases but are not part of Boyle's Law's definition. Thus, the correct answer