CHEM 1A Lecture Notes - Lecture 8: Kinetic Theory Of Gases, Ideal Gas, Ambient Pressure

• School: Berkeley
• Department: Chemistry
• Course: CHEM 1A
• Professor: Arnold John

Document Summary

Gases, whether trapped in various containers or in the open atmosphere, are literally all around us. We know this when we measure pressure of a gas in a container the force exerted by the gas on the walls of the container per unit surface area. Macroscopic properties such as temperature and pressure all derive from the random motion of gas molecules as described by the kinetic molecular theory of gases. The most remarkable observation is that to a first approximation, all gases, regardless of their identity, behave the same way in response to changes in volume, pressure, temperature, and the number of gas molecules. Explain the properties of gases in terms of the random motion of molecules. Relate volume, temperature, and pressure of a gas sample in both rigid and flexible containers. Explain why the pressure, temperature, and volume of an ideal gas do not depend on the identity of the gas.