# MCAT Chemistry

 Factors that affect the rate of reaction
 Catalysts, Medium, Temperature, Concentration of Reactants
 Homogeneous catalysts
 Catalysts are in the same phase as the reactant
 Heterogeneous Catalysts
 Catalysts are in a different phase from the reactants
 Enthalpy
 is the heat absorbed or evolved by a system at constant pressure
 kinetic molecular theory
 no volume, no attractions or repulsions, ave KE is proportional to abs temp, elastic collisions, continuous random motion
 KE formula
 1/2 mv^2 = 3/2kT
 Diffusion
 The flow of gas particles through a mixture e.g. the smell from an open bottle of perfume diffusing across the room. Isobaric and Isothermal. r1/r2 = (mr2/mr1)^1/2
 Effusion
 the flow of gas particles under pressure from one compartment to another through a small opening. isothermal. r1/r2 = (mr2/mr1)^1/2
 Boyle’s Law
 P1V1=P2V2
 Charles’s Law
 V1/T1 = V2/T2
 n1/V1 = n2/V2
 Ideal Gas Equation and Encompassing Gas Eqtn
 PV = nRTP1V1/T1 = P2V2/T2
 Density
 m/V
 STP
 273.15K. 1 atm amd 22.4L/molKinetics
 Standard ConditionsState functions
 293.15K and 1 atmEnthalpy, Entropy, Gibb’s free energy
 Ideal gas behaviour – exception
 seen at low pressure and high temperature. Exception = high pressure and low temperature bc molecular volume and intermolecular attraction become important
 Dalton’s Law of Partial Pressure
 Pa = XaPt where X = mole fraction & Pt = total pressure
 Mole Fraction
 Xa = na (moles of A) /nt (total moles)
 Root mean square
 is the speed which corresponds to the ave. KE per particle. Urms = (3RT/mr)^1/2
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