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Lecture 13_092608

# Lecture 13_092608 - Daltons Law of Partial Pressures In a...

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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 Σ n = n 1 +n 2 +n 3 + … = + + + = n V RT P P P P ... 3 2 1 total Dalton’s Law of Partial Pressures V RT n P 1 1 = V RT n P 3 3 = V RT n P 2 2 =

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Dalton’s 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?
Dalton’s 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 ). Mole fraction is related to the total pressures by: B A A A n n n X + = to t i i P X P = B A B B n n n X + = 1 B A = + Ξ Ξ

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Dalton’s Law of Partial Pressures
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Lecture 13_092608 - Daltons Law of Partial Pressures In a...

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