Combustion - complete combustion of hydrocarbons results in CO2 and H2O. (results in forming the oxide of the elements of the compound) Gas Laws: Kinetic molecular Theory: Ideal: particles 0 volume no attraction, deviate from ideal at low particles in constant temperature and high pressure Van der Waal’s Equation random motion particles do not have volume particles do not attract ↑ ↑KE T with = ½m×v2 The Ideal Gas Law: PV = nRT (P = pressure in atm, V = volume in liters, n = moles, R = 0.08201 L*atm/mol*K, T = Combine Gas Law = temperature in Kelvin’s) P1V1 P2 V2 T1 T2 XA PA = Ptotal Ptotal = PA + PB +Pc + = …. moles A Mole fraction; X total moles Rate of Effusion: Boyle’s Law: PV = K Charles Law: V/T = K
Combustion - complete combustion of hydrocarbons results in CO2 and H2O. (results in forming the oxide of the elements of the compound) Gas Laws: Kinetic molecular Theory: particles in constant random motion particles do not have volume particles do not attract T ↑ with ↑KE = ½m×v2 Ideal: particles 0 volume no attraction, deviate from ideal at low temperature and high pressure Van der Waal’s Equation The Ideal Gas Law: (P = pressure in atm, V = volume in liters, n = moles, R = 0.08201 L*atm/mol*K, T = temperature in Kelvin’s) PV = nRT Combine Gas Law P1V1 = P2 V2 T1 T2 Mole fraction; X = moles A total moles PA = Ptotal XA Ptotal = PA + PB +Pc + …. Rate of Effusion: Boyle’s Law: PV = K Charles Law: V/T = K
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