CHEM 1A Lecture Notes - Elastic Energy, Effusion, Root Mean Square

• School: UC-Irvine
• Department: Chemistry
• Course: CHEM 1A
• Professor: Amanda Brindley

Document Summary

Kinetic theory of gases - assume molecules are point masses (no volume, even though there s mass) Constant random motion, collisions are completely elastic. Energy can be transferred, but total energy remains the same. Gas molecules are neither attracted nor repulsed. Average kinetic energy is proportional to temperature. At a given temperature, 2 different gas molecules will have the same ke. Same ke, different masses => velocity changes. Increase mass => decrease velocity // heavier molecules are slower. Pressure - created by collisions between molecules and the container. The faster the molecules hit the container => the more pressure. If molecules move faster => higher temperature. The more frequent molecules hit the container => the more pressure. Increase temperature or increase the number of molecules. Molecular speed curves - particular amount of molecules at particular speeds. Temperature - y axis: # of particles and x axis: molecular speed m/s. Raise temperature => wider curve => more speeds.