Use the density formula to elicit the effect on the density of a gas when the volume changes, the mass remaining constant. Discuss the compression of gas molecules and the effect the compression has on the volume and the pressure. Introduce the concept of diffusion, with molecules moving from areas of greater concentration into areas of less concentration. List the units in use when reporting the pressure a gas exerts.
Define solute and solvent. Indicate solutes may be solids, liquids, or gases. Elicit that solvents may also be any phase.

Use examples written on the board, along with molecular models, to demonstrate that empirical formulas are formulas based on the smallest whole number ratios of atoms in the compound. Analyze how two compounds can have the same empirical formula but be different compounds, for example, acetylene and benzene.

Discuss the factors which affect gas particle motion by using the kinetic molecular theory. Discuss using molecular models the effect of particle size, particle motion, and particle energy. Examine how the energy is affected by the particle mass and the velocity, arriving at the equation of K.E. = 1/2 MV squared.

Review Boyle's law and Charles law. Explain how they can be understood in terms of the kinetic molecular theory. Discuss the KM theory of gas particles, the directions of movement, how particle size and velocity affect the energy, and elastic collisions.

Set up and run a lab which demonstrates the relationship between the temperature of a gas and its volume. Determine, using Charle's law equation, the end volume of a gas when the temperature is decreased by a measurable amount. Run the experiment and compare the actual results with the mathematical theoretical results.

Discuss the effect of temperature on the volume of a gas. Use a graph of volume v temperature and elicit the direct relationship.
Explain in terms of the kinetic molecular theory. State the math relationship. Introduce the concept of Kelvin temperature and how to convert Centigrade to Kelvin. Work a problem to arrive at a final volume given an initial volume and change of temperature.

Review Boyle's law regarding the relationship between volume and pressure of a gas. Introduce the effect of temperature on the volume of a gas. Discuss the effect on the circumference on a sealed balloon when placed in a bucket of ice water. Introduce the kinetic molecular theory.

Show the effect of changing pressure on the volume of a gas by using a balloon inside a syringe. Complete the determination of volume problem from yesterday, and begin and complete a second problem. Demonstrate how to work the problems in a step by step fashion, insisting on each step being completed before continuing on to the next. Hypothesize the results of each problem prior to working it, and then analyze your findings

Outline an example of decreasing the gas pressure in an inflated balloon by placing it in ice water. Elicit the effect on the volume of the gas, and on the volume of the balloon. Elicit the pressure changes which would occur if a given volume of a gas was compressed into half then a quarter of its volume. Graph the results of a volume vs pressure experiment, and describe the inverse proportion seen. State Boyle's law based on the results.
State Boyle's law as a mathematical expression P1xV1=P2xV2.
Set up a practice problem in which a given sample of helium in a 1 liter container with a pressure of .998 atm is moved to a 2 liter container. Determine the new pressure.

Using the figures measured in last week's lab, determine the water of hydration for the copper sulfate compound. Determine the grams per mole of copper sulfate and water. Use that information to determine the number of moles of copper sulfate and water based on the grams measured from our sample.
Determine the mole ratio and then convert it to a whole number ratio. Write the formula for the hydrous copper sulfate based on the measured results.