CHEM 1A Lecture Notes - Lecture 15: Kinetic Theory Of Gases, Billiard Ball, Intermolecular Force
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Movement of substances from an area of high concentration to one of lower concentration. Ability of a gas to spread out and fill a container. In theory this is how they would behave. The collisions of the particles with the walls of the container are the cause of pressure exerted by the gas. Gas particles are in continuous, rapid, random motion. Increase in temperature increases the movement of the molecules and thus the pressure exerted by the gas. The particles are assumed to exert no forces on each other; they are assumed to neither attract nor repel each other. The particles are so small compared with distances between them that the value of the individual particles can be assumed to be negligible (zero). Volume occupied by the molecules is inconsequential. The average kinetic energy of a collection of gas particle is assumed to be directly proportional to the kelvin temperature of a gas.
