Watching this resources will notify you when proposed changes or new versions are created so you can keep track of improvements that have been made.
Favoriting this resource allows you to save it in the “My Resources” tab of your account. There, you can easily access this resource later when you’re ready to customize it or assign it to your students.
By the late 19th century, scientists had begun accepting the atomic theory of matter started relating it to individual molecules. The Kinetic Molecular Theory of Gases comes from observations that scientists made about gases to explain their macroscopic properties. The following are the basic assumptions of the Kinetic Molecular Theory:
The volume occupied by the individual particles of a gas is negligible compared to the volume of the gas itself.
Gas particles are in a constant state of random motion and move in straight lines until they collide with another body.
The collisions exhibited by gas particles are completely elastic; when two molecules collide, total kinetic energy is conserved.
The average kinetic energy of gas molecules is directly proportional to absolute temperature only; this implies that all molecular motion ceases if the temperature is reduced to absolute zero.
Applying Kinetic Theory to Gas Laws
Charles' Law states that at constant pressure, the volume of a gas increases or decreases by the same factor as its temperature. This can be written as:
According to Kinetic Molecular Theory, an increase in temperature will increase the average kinetic energy of the molecules. As the particles move faster, they will likely hit the edge of the container more often. If the reaction is kept at constant pressure, they must stay farther apart, and an increase in volume will compensate for the increase in particle collision with the surface of the container.
Boyle's Law states that at constant temperature, the absolute pressure and volume of a given mass of confined gas are inversely proportional. This relationship is shown by the following equation:
At a given temperature, the pressure of a container is determined by the number of times gas molecules strike the container walls. If the gas is compressed to a smaller volume, then the same number of molecules will strike against a smaller surface area; the number of collisions against the container will increase, and, by extension, the pressure will increase as well. Increasing the kinetic energy of the particles will increase the pressure of the gas.
The Kinetic Molecular Theory of Gas (part 1) - YouTube
Reviews kinetic energy and phases of matter, and explains the kinetic-molecular theory of gases.
The Kinetic Molecular Theory of Gas (part 2) - YouTube
Uses the kinetic theory of gases to explain properties of gases (expandability, compressibility, etc. )
gas molecules increase in kinetic energy, thus increasing the pressure, gas molecules experience greater intermolecular forces, thus decreasing the pressure, gas molecules increase in temperature, thus increasing the pressure, and gas molecules collide with the container more often, thus increasing the pressure
Source: Boundless. “Kinetic Molecular Theory and Gas Laws.” Boundless Chemistry. Boundless, 01 Jul. 2015. Retrieved 01 Jul. 2015 from https://www.boundless.com/chemistry/textbooks/boundless-chemistry-textbook/gases-5/kinetic-molecular-theory-55/kinetic-molecular-theory-and-gas-laws-263-8284/