CHM 121 Lecture Notes - Lecture 4: Lead Dioxide, Ideal Gas Law, Atmospheric Pressure

• School: University of Miami
• Department: Chemistry
• Course: CHM 121
• Professor: Leslie Knecht

Document Summary

Physical characteristics of gases: gases assume the volume and shape of their containers, gases are the most compressible state of matter, gases will mix evenly and completely when confined to the same container. No portioned out gases: gases have much lower densities than liquids and solids, density is measure as g/l because they have a low density, volume of the gas = volume of container. The pressure of a gas: the pressure of a gas depends on several factors, number of gas particles in a given volume. More collisions= more particles= more pressure: volume of the container larger volume = decreased pressure, average speed of the gas particles. Measuring air pressure: 1 pascal (pa) = 1 n/m2, 1 atm = 760 mmhg = 760 torr, 1 atm = 101,325 pa = 14. 7 psi, pressure= force/ area. Boyles law: as p increases, v decreases, not directly proportional, inversely proportional, graph of p and 1/v is directly proportional.