Chem Lecture 11

Chem Lecture 11 - Sheet1 Page 1 Dalton's Law of Partial...

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Unformatted text preview: Sheet1 Page 1 Dalton's Law of Partial Pressure: For a mixture of gases in a container, the total pressure of grases is the sum of the pressure of each gas. Pt = P1 + P2 + P3 (t = total) Mole fraction (x(kai)i): The ratio of the number of mol of one component to the total number of mol of all components in the mixture. x(kai)1 = n1 / nT-Collecting a gas over water:->Total pressure = Pgas + Pwater-->Pwater = vapor pressure of water--- Kinetic Molecular Theory of Gases Postulates: 1. The voulme of the individual particles is very small (zero volume). The distance between particles is very large. 2. The particles are in continous random motion. THe pressure of a gas is due to collisions between the particles and the wall 3. The particles of a gas neither attract nor repel eachother (Not 100% true) 4. The average kinetic energy of a collection of gas particles is directly proportional to the absolute temperature, in Kelvin, of t 5. The collision between particles is elastic....
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This note was uploaded on 05/06/2008 for the course CHEM 151 taught by Professor Campbell during the Spring '08 term at Lansing.

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Chem Lecture 11 - Sheet1 Page 1 Dalton's Law of Partial...

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