Chapter 11 (Gases): Kinetic Molecular Theory: Conversion between units of pressure: (Atm to mmHg and back) Boyle’s Law: P1V1 = P2V2 • Relationship between volume & pressure is inversely proportional • Assumes constant temperatureCharles’ Law: V1/T1 = V2/T2 (assumes constant pressure) (* temperature MUST be given in Kelvins*) P1/T1 = P2/T2 (assumes constant volume) • Relationship is directly proportional Combined Gas Law: P1V1/T1 = P2V2/T2 (* temperature MUST be given in Kelvins*) • Relationship between volume/pressure & temperature is directly proportional • Used when no “measurables” (ie: P, V, & T) are constant. Avogadro’s Law: V1/n1 = V2/ n2 (n = moles) • Relationship between volume & number of moles is directly proportional • Assumes constant pressure & temperatureIdeal Gas Law: PV = nRT (Ties V, T, P, & n together into a single law) • Gas Constant R = 0.082 L·Atm/mol· K • * Pressure must be in Atm, Volume in L, Temp. in Kelvins* • Assumes Ideal Conditions o High Temp; Low Pressure o These conditions allow minimal interactions between gas particles Derivations of the ideal gas law: Molar mass Density gRT=(molar mass)PV d =(molar mass)PRT Gases in Chemical Reactions: • Uses the Moles term (n) in the ideal Gas Law to convert from P, V, & T to quantities in chemical equations: Molar Volume at Standard Temperature and Pressure (STP) • STP = 0oC and 1 atm (At STP, 1 mole of an ideal gas occupies 22.4 L) • Ideal Gas Law reduces to a per expression under these conditions (1mol/22.4L) Partial Pressures of gas mixtures: Ptot = Pa + Pb + Pc +