Chem 1320 1st Edition Lecture 13 Outline of Last Lecture I. Daltons Law of Partial PressureII. Simple Model of a GasOutline of Current Lecture I. Average Molecular SpeedII. Real GassesIII. Van der Waals Equation of State Current LectureI. Average Molecular SpeedThe first thing you do is start with kinetic energy. Kinetic energy is the energy of motion and the model consumes no other energy. For single particles it is KE= 1/2mu2. For multiple particles it isKE= 1/2mu2. KE ɣ T 1/2mu2 ɣ T or ½mu2 = (constant) T Constant= 3R/2 for one particle (3R/2NA)R= 8.314J/(mol x K)U2=3RT/mNA = 3RT/M u= (3RT/M)1/2Example: Oxygen at room temperature (298K), M= 32.0g/molU= (3(8.14J/(mol x K) (298K)) 1/2 (0.032kg1mol) = 482m/sII. Real GasesThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.- Short comings of the ideal gas model1. Gas phase particles are not billiard balls and there are altercative forces between particles (P actual = P ideal- correction) 2. Gas phase particles have a finite volume (V ideal = V container- correction)Van der Waal’s Equation of StatePV = nRTZ= nRT/ PV (Z= compressibility factor) (P actual – constant)(V) = nRT(P actual – constant)(V- constant)= nRTEQUATION: (P-an2/v2)(v-bn)= nRT
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