Kinetic theory or kinetic theory of gases attempts to explain overall properties of gases, such as pressure, temperature, or volume, by considering their molecular composition and motion. The theory basically states that pressure is not caused by molecules pushing each other away, like earlier scientists thought. Instead, pressure is caused by the molecules colliding with each other and their container. Kinetic theory is also known as kinetic-molecular theory or collision theory.
There are three main components to kinetic theory:
- No energy is gained or lost when molecules collide
- The molecules in a gas take up a negligible (able to be ignored) amount of space in relation to the container they occupy
- The molecules are in constant, linear motion
Related pages[change | edit source]
References[change | edit source]
- The Mathematical Theory of Non-uniform Gases : An Account of the Kinetic Theory of Viscosity, Thermal Conduction and Diffusion in Gases, Sydney Chapman, T. G. Cowling
Other websites[change | edit source]
- Early Theories of Gases
- Thermodynamics - a chapter from an online textbook
- Temperature and Pressure of an Ideal Gas: The Equation of State on Project PHYSNET.
- Introduction to the kinetic molecular theory of gases, from The Upper Canada District School Board
- Java animation illustrating the kinetic theory from University of Arkansas
- Flowchart linking together kinetic theory concepts, from HyperPhysics
- Interactive Java Applets allowing high school students to experiment and discover how various factors affect rates of chemical reactions.
- Molecular kinetic theory fundamentals