Chem 1320 1st Edition Lecture 13Outline of Last Lecture I. EquationsII. ExamplesIII. Gas StoichiometryOutline of Current Lecture I. Daltons Law of Partial PressureII. Simple Model of a GasCurrent LectureI. Daltons Law of Partial PressureThis law explains the pressure of individual gasses are additive. Some assumptions are that gases mix homogeneously and do not react. Since gases are so far apart on average, we can assume that they behave independently. Some consequences are that moles of gas are adaptive, independent. Also, if volume and temperature are fixed gases, pressures are adaptive.PT= P1+P2+P3……PT= n1RT/V + n2RT/V…Example: A gas sample has 8.24 mol of CH4, 0.421 mol of C2H6, and 0.116 mol of C3H8. If the totalpressure equals 1.37atm, what is the pressure of C3H8? - 8.24 mol CH4, 0.421 mol C2H6, 0.166 mol C3H8, PT= 1.37atm, Pc3H8 =? - Pi= XPT- NT= 8.24+ 0.421+0.166= 8.78 mol- Pc3H8 = (0.166/8.78) (1.37atm)= 0.0181atm- Sum of the individual pressures should equal total pressure II. Simple Model of a GasThese 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.Some behaviors are that a gas appears to be independent of the identity of a gas, is a good assumption. Also, there are deviations from ideal behavior and we want to understand why. Some assumptions are that non- interacting particles have no attraction between them. Also, allof the particles are in constant random motion. Lastly, volume of a gas particles are small compared to the system. Some consequences are that magnitude of the pressure given by how often and how hard the molecules strike. Gas molecules have an average kinetic energy and that each molecule has a different energy. Also that there is a spread of individual energies of gas molecules in any sample of gas. Lastly, as temperature increases, average kinetic energy of gas molecules
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