1. Kinetic-Molecular Theory of Matter (KMT) 1.gases are mostly empty space 2.gas particles are in constant and random motion 3.collisions are elastic 4.gas pressure is caused by collisions of molecules with the walls of the container

2. IDEAL GAS LAW conventional formulaPV = nRT molar mass & densityMM = dRT / P helpful: number of moles mass / molar mass(n = m / MM)

3. Expression for Pressure (P) N = number of molecules m = mass of a molecule u = average speed N/V = concentration of gas molecules (  more molecules  more pressure more volume  less pressure mu 2 = measures energy of collision hence, equation predicts that pressure is directly proportional to mu 2.

4. Average Kinetic Energy (Et) From eq. for P & PV = nRT

5. Average Speed (u) Graham’s Law (Effusion/ Diffusion)

6. Distribution of Molecular Speeds