How does the kinetic molecular theory explain the pressure exerted by gases

The kinetic molecular theory explains the pressure exerted by gases as the result of many collissions of the gas particles (atoms or molecules) with the walls of the vessel where they are contained.

The pressure is the perpendicular force per unit area exerted by the gas particles when they hit the walls of the container.

Explanation:

As per the kinetic molecular theory, gases consist on a large number of tiny particles (atoms or molecules) in continuous rapid random motion.

The particles are so small that they are considered to have a negligible volume compared with the volume of the vessel where they are confined.

Since the number of molecules is so large, statistical approach can be applied.

The rapidly moving particles constantly collide among them and with the walls of the container. The collisions are considered elastic, which means that there is no loss of energy after the coliisions.

Applying classical (Newtonian) mechanic and the statistical approach, the kinetic theory calculates the pressure exerted by gases as the force exerted by the particles when they hit the walls of the container per unit of area.