As always… Lon-Capa assignments Lecture videos Textbook Read Do text homework

The Partial Pressure of each Gas in a Mixture of Gases in a Container Depends on the Number of Moles of that Gas

Kinetic Molecular Theory Gases consist of particles in constant random motion. Temperature is a measure of average kinetic energy. Pressure is due to collisions of gas particles with the container.

KMT (assumptions) Assume gas particles exert no forces on each other. Assume the volume of the individual gas particles is negligible (zero). Identity of the gas doesn’t matter!

PV/nRT vs. P

a) Person 3 b) Person 4 c) Person 5 d) Person 6 e) Person 7 Clicker Question You are standing in a line with 9 other friends, evenly spaced apart. You are at one end of the line (we will call you person #1). You release laughing gas (N2O) at the exact same time the person at the other end of the line (person #10) releases the tear gas commonly referred to as CS gas (C10H5ClN2).   Assuming ideal behavior, which person is the first person to simultaneously laugh and cry? a) Person 3 b) Person 4 c) Person 5 d) Person 6 e) Person 7

Diffusion of NH3(g) and HCl(g)

Effusion

Egg in a Bottle Using liquid nitrogen to cool the bottle. What factors are changing? What factors are staying constant?

Clicker Question As you increase the temperature of a sample of an ideal gas at constant pressure and volume, what happens to the number of moles of gas? a) The number of moles of gas increases. b) The number of moles of gas decreases. c) The number of moles of gas does not change. d) I do not know.

Egg in a Bottle Placing a burning cotton ball in the bottle. What factors are changing? What factors are staying constant?