CHEM 1125Q Lecture Notes - Lecture 2: Gas Laws, Molar Mass, Gas Constant
Document Summary
A sample of gas assumes both the shape and volume of the container. The densities of gases are much smaller than those of liquids and solids and are highly variable depending on temperature and pressure. Gases form homogeneous mixtures (solutions) with one another in any proportion. The kinetic molecular theory explains how the molecular nature of gases gives rise to their macroscopic properties. The basic assumptions of the kinetic molecular theory are as follows. A gas is composed of particles that are separated by large distances. The volume occupied by individual molecules is negligible. Gas molecules are constantly in random motion, moving in straight paths, colliding with perfectly elastic collisions. Gas molecules do not exert attractive or repulsive forces on one another. The average kinetic energy of a gas molecule in a sample is proportional to the absolute temperature. Gases are compressible because molecules in the gas phase are separated by large distances. (first assumption)
