What does kinetic molecular theory explain regarding gas pressure?

The kinetic molecular theory provides a framework for understanding the behavior of gases, particularly how gas pressure arises from the motion of particles. According to this theory, gas particles are in constant, rapid motion and travel in straight lines until they collide with other particles or the walls of their container.

When gas particles collide with the walls of their container, they exert a force on those walls. The cumulative effect of many particles colliding with the walls leads to the observable pressure exerted by the gas. Therefore, gas pressure is directly related to the frequency and force of collisions between gas particles and the surfaces they encounter. This explanation aligns with the understanding that increases in gas temperature, volume, or the number of particles can also affect pressure, but the core principle hinges on the nature of the collisions as described by the kinetic molecular theory.

In contrast, pressure being caused by the weight of gas, resulting solely from temperature changes, or being unrelated to particle motion does not accurately reflect the principles outlined in the kinetic molecular theory. These aspects do not capture how the energy and motion of particles contribute to gas pressure.