CHM 1311 Lecture Notes - Lecture 8: Kinetic Theory Of Gases, Ideal Gas Law, Ideal Gas

• School: University of Ottawa
• Department: Chemistry
• Course: CHM 1311
• Professor: Wendy Pell

Document Summary

Ideal gas law is empirical (based on observations of macroscopic behaviour of gases; theoretical model. Pressure is the momentum and rate at which particles hit the walls; how many you have and how fast they are. Assumptions: gas molecules are in constant, random, straight line motion, volume of individual particles is approx. Unit for energy is joules (1kgm2/s2), therefore mass (m) is converted to kg i. e m for h2 most probable speed (v) for h2 gas molecules at 300k is 1. 57 x 103m/s. Diffusion: gradual mixing of molecules of different gases. Effusion: escape of a gas from its container through a small hole. Rates for both effusion and diffusion are proportional to the root mean square of the speeds of the particles involved. Increase temperature = increase pressure (more collusions and force per collision) Determination of molar mass from rearranging the ideal gas equation. Heavier gas = denser b/c assumed all gases have same volume.