Unit 1-B By Jordan Rock and Garrett Schwarzman

PV = nRT P = Pressure (atm) P = Pressure (atm) V = Volume (Liters) V = Volume (Liters) n = # of moles n = # of moles T = Temperature (*K) T = Temperature (*K) R = R = (atm*L)/(moles*K) (atm*L)/(moles*K)

Gas Proportionalities Boyle’s Law  P = (1/V)*k Boyle’s Law  P = (1/V)*k Charles’ Law  V = kT Charles’ Law  V = kT Gay-Lussac’s Law  P = kT Gay-Lussac’s Law  P = kT Avogadro’s Law  n = kV Avogadro’s Law  n = kV Henry’s Law  P = kC Henry’s Law  P = kC

Partial Pressure Partial Pressure of a molecule is equal to the mole fraction of that molecule in the system multiplied by the total pressure of the system. Simply put: P a = (x a )(P system ) Where x a is the number of moles of (a) divided by the total number of moles in the system.

Van der Waals’ Equation [P + (n²a/V²)] [V-nb] = nRT a = molecular attraction (most likely given) a = molecular attraction (most likely given) b = molecular volume (most likely given) b = molecular volume (most likely given) R = (atm*L)/(mol*K) R = (atm*L)/(mol*K) This equation accounts for the absolute pressure and volume of the system. At high pressures and low temperatures, the system starts to shift from ideal This equation accounts for the absolute pressure and volume of the system. At high pressures and low temperatures, the system starts to shift from ideal

Kinetic Molecular Theory Gases contain large number of molecules in constant random motion Gases contain large number of molecules in constant random motion Molecules have negligible volume compared to the total volume it occupies Molecules have negligible volume compared to the total volume it occupies There are negligible attractive and repulsive forces between molecules There are negligible attractive and repulsive forces between molecules At a constant temp, the average KE of the molecules remains constant At a constant temp, the average KE of the molecules remains constant The molecule’s KE is proportional to its absolute temp The molecule’s KE is proportional to its absolute temp

Kinetic Energy KE = ½mu² KE = ½mu² where m = mass and u = RMS speed KE avg = 3/2RT KE avg = 3/2RT where R = J/(mol*K) U = √[(3RT)/M] U = √[(3RT)/M] where R = J/(mol*K) and M = molar mass in kg/mol.

Effusion Effusion Speed = Rate1/Rate2 = √ (M2/M1) Diffusion is when molecules move from high concentration to low concentration. Effusion is when they move through a small hole or somewhat-permeable barrier. Lighter molecules will effuse faster in comparison to heavier molecules.

The End.