What results from increasing the amount of gas in a confined space?

Increasing the amount of gas in a confined space leads to increased pressure, as described by Boyle’s Law and the Ideal Gas Law (PV=nRT). According to the Ideal Gas Law, pressure (P) is directly proportional to the number of moles of gas (n) when the volume (V) and temperature (T) are held constant. This means that if you add more gas molecules to the container, they will collide more frequently with the walls of the container, which raises the overall pressure.

In a confined space, as more gas is introduced, the crowded conditions cause the gas particles to exert more force against the walls of the container during their collisions, resulting in an increase in pressure. This relationship is fundamentally tied to the behavior of gases in confined volumes and reflects the kinetic molecular theory of gases, which states that gas pressure arises from collisions of gas particles with the walls of their container.

Therefore, increasing the amount of gas in a confined space consistently results in increased pressure, assuming other factors such as temperature and volume remain unchanged.