Lec-23-Chap-10-3P

Lec-23-Chap-10-3P - Gas Mixtures Partial Pressures Daltons...

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Dalton Dalton ’s law of partial pressures s law of partial pressures “The total pressure of mixture of gases is the sum of the partial pressure of the individual gases in the mixture.” P total = P 1 + P 2 + P 3 + … Gas Mixtures & Partial Pressures Gas Mixtures & Partial Pressures
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Gas Mixtures & Partial Pressures Mole Fractions P total = P 1 + P 2 + … (P 1 = n 1 RT / V) = n 1 RT / V + n 2 RT / V + . .. = (n 1 + n 2 + . ..) RT / V P total = n total RT / V So P 1 / P total = n 1 /n total = X 1 P 2 / P total = n 2 /n total = X 2 etc. with X 1 = mole fraction mole fraction of gas 1 = ( n 1 / n total ) etc. Notice that: X 1 + X 2 + X 3 + …. . = 1
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A sample of gas is prepared by combining 14.1g O 2 (MM=32) and 42.5g N 2 (MM=28). The total pressure is 0.75 atm. What is the partial pressure of O 2 ? A: 0.250 atm B: 0.169 atm C: 1.96 atm D: 0.225 atm P(O 2 ) = X O2 * P tot = n O2 /n tot * 0.75 atm = (14.1/32) / (14.1/32 + 42.5/28) * 0.75 = 1.68 atm Partial Pressures Consider: 2 NO(g) + O 2 (g) 2 NO 2 (g) 4.0L, 1.00 atm 2.0L, 0.40 atm (a) The final composition and mole fractions of the mixture?
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This note was uploaded on 11/14/2010 for the course CHE 131 taught by Professor Kerber during the Spring '08 term at SUNY Stony Brook.

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Lec-23-Chap-10-3P - Gas Mixtures Partial Pressures Daltons...

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