What does the total pressure in kinetic gas theory depend on?

Total pressure in kinetic gas theory primarily depends on the frequency of collisions between gas molecules and the force of impact those molecules exert on the walls of their container. According to kinetic gas theory, gas particles are in constant, random motion and collide with each other and with the walls of the container. The pressure that a gas exerts is a result of these collisions.

As the gas molecules collide with the walls, they exert a force over a given area, which is what we measure as pressure. An increase in the number of collisions (which can happen with increased molecular speed due to higher temperatures or a greater number of gas molecules) will lead to an increase in pressure. Similarly, if the force of impact, which depends on the mass and speed of the molecules, increases, the pressure will also increase.

This relationship highlights that pressure is not solely defined by temperature or other singular factors but rather by the dynamic interactions among the gas molecules and their collisions with the container walls.