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Effect of Collisions on Pressures

 

From the assumptions of the kinetic theory of gases, gas molecules collide with themselves and with the walls of the container. The collisions with the walls of the container produce the pressure in the vessel. Therefore, the greater the rate of collision at constant volume, the higher the pressure generated and vice versa.

Notice that temperature directly affect the rate of collisions at constant volume. The higher the temperature of the system at constant volume, the greater the kinetic energy of the gas molecules, therefore, the greater the rate of collision of the molecules with the walls of the container - the greater the pressure and vice versa.

Related Tutorials

The Kinetic Theory of Matter
Deviations from Ideal Gas Behavior
Limitations of the Kinetic Theory
Application of the Kinetic Theory of Matter 

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