What fundamental principle explains the behavior of gasses in a closed container?

The behavior of gases in a closed container is primarily explained by Boyle's Law, which states that the pressure of a gas is inversely proportional to its volume when the temperature is held constant. This means that if the volume of the gas decreases, the pressure increases, and vice versa. This principle emerges from the kinetic theory of gases, which asserts that gas particles are in constant motion, colliding with the walls of their container and exerting pressure.

In a closed container, if the volume decreases (for instance, if the container is compressed), the gas particles have less space to move around, leading to more frequent collisions with the walls, thus increasing the pressure. The relationship described by Boyle's Law allows us to predict how gases will behave under varying conditions of pressure and volume, making it fundamental to understanding gas dynamics in closed systems.

While other laws such as Charles's Law evaluate how temperature affects gas volume, and the conservation of mass pertains to the total mass remaining constant in a closed system, they do not specifically address the pressure-volume relationship under constant temperature. Newton's Third Law concerns the action-reaction principle, which, while relevant in some contexts, does not explain the behavior of gases in this specific scenario. Thus, Boyle's Law