CHEM 1125Q 1st Edition Lecture 6 Outline of Last Lecture (Ch. 11)I. Pressure, Gas Laws: Boyle’s, Charles’s, Avogadro’s, Combined Gas Law, and Ideal Gas EquationOutline of Current Lecture (Ch. 11)II. Ideal Gas EquationA. FlawsIII. Van der Waals EquationIV. Dalton’s LawV. Mole FractionsA. Mole FractionsB. Stoichiometric CalculationsCurrent LectureII. Ideal Gas EquationA. Flawsa. According to the Ideal Gas Equation (PV=nRT), particles have no mass or attractive forces, which in turn would mean that the particles couldnot transform from a gas to a liquid or solid state. Since gases are in fact capable of changing states, this equation is flawedb. At high pressure and low temperature, molecules are extremely close to each other and moving slower, so their individual volumes become insignificantIII. Van der Waals EquationA. Van der Waals Equation, also known as the Virial Equation after the virial coefficients (a and b) that it contains, is useful for solving for gases that do not behave ideally, and could not be solved with the Ideal Gas Equationa. (P + an2/V2)(V – nb) = nRTP = Experimental measured pressurea = A virial coefficient unique to each gasV = Volume of the containerb = A virial coefficient specific to each gasIV. Dalton’s LawA. Dalton’s Law of Partial Pressure states that when two or more gases are in a container, each gas behaves as if it was in the container by itselfThese 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.a. Each gas has its own pressure, independent of those of the other gases presentb. The total pressure of the mixture is the sum of each gas’s individual pressure. Therefore a gas’s individual pressure in a mixture is known as its partial pressurec. Px + Py = PTotalV. Mole FractionsA. Mole Fractionsa. Mole fractions determine the relative amount of a substance in a gaseous mixtureb. Χi = ni / nTotalΧi = Pi / PTotalB. Stoichiometric Calculationsa. Stoichiometric equations can help determine mole relationships whensolving for partial
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