Lecture 13_092608 - In a mixture of gases, total pressure...

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Unformatted text preview: In a mixture of gases, total pressure equals sum of partial pressures P Total = P 1 + P 2 + P 3 At constant V and T Each gas acts independently Where n = n +n +n + = + + + = n V RT P P P P ... 3 2 1 total Daltons Law of Partial Pressures V RT n P 1 1 = V RT n P 3 3 = V RT n P 2 2 = Daltons Law of Partial Pressures Examples Exactly 2.0 moles of Ne and 3.0 moles of Ar were placed in a 40.0 L container at 25 o C. What are the partial pressures of each gas and the total pressure? A sample of natural gas contains 6.25 moles of methane (CH 4 ), 0.500 moles of ethane (C 2 H 6 ), and 0.100 moles of propane (C 3 H 8 ). If the total pressure of the gas is 1.50 atm, what are the partial pressures of the gases? Daltons Law of Partial Pressure For a two-component system, the moles of components A and B can be represented by the mole fractions (X A and X B )....
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This note was uploaded on 08/29/2010 for the course CHM 2045 taught by Professor Brant during the Fall '08 term at University of South Florida - Tampa.

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Lecture 13_092608 - In a mixture of gases, total pressure...

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