Boyle's Law -- Volume of a gas varies inversely with the pressure if temperature is held constant.

			Charles' Law -- Volume of gas varies directly with Absolute Temperature if pressure is held constant.

			Gay-Lussac's Law -- Pressure of a gas varies directly with the Absolute Temperature if volume is held constant.

			Ideal-Gas Law -- Putting it all together

			Our model of matter is that atoms and molecules are in constant motion that depends on the temperature.  In fact, what we call temperature is actually a measure of the kinetic energy of atoms and molecules.  The more kinetic energy atoms and molecules have the hotter we say they are.  Each time an atom or molecule in a gas enclosed in a container strikes the side of its container, it bounces off and imparts an impulse, changing its momentum and kinetic energy.  We detect this impulse as pressure, and the greater the number of atoms or molecules in the gas and the faster they are moving, the greater the pressure they exert.  There are so many atoms and molecules in a finite-sized container, that we can't possibly measure the momentum and kinetic energy of each one, but by using a statistical analysis, we can  show that the average translational kinetic energy of molecules in random motion in an ideal gas is directly proportional to the absolute temperature of the gas:  KEavg = (1/2)m(v2)avg = (3/2)kT.  In this same way, we can derive the ideal gas law:  PV = nRT = NkT.

			Read pp. 468-488 of the text.

			Answer the questions in HW 23 on WebAssign:  http://webassign.net/login.html