Lecture 6 PartII Chem 102SP

# Lecture 6 PartII Chem 102SP - Chapter 5 Gases Daltons Law...

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Chapter 5 Gases

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Dalton’s Law of Partial Pressures For a mixture of gases in a container, P Total = P 1 + P 2 + P 3 + . . . The total pressure exerted is the sum of the pressures that each gas would exert if it were alone. P 1 , P 2 , P 3 – partial pressure of individual gas Each gas behaves as ideal gas V RT n V RT n n P V RT n P V RT n P total total ) ( ,.... , 2 1 2 2 1 1 Note: temperature and volume are the same
Dalton’s Law of Partial Pressures Example 4. 27.4 L of oxygen gas at 25.0°C and 1.30 atm, and 8.50 L of helium gas at 25.0°C and 2.00 atm were pumped into a tank with a volume of 5.81 L at 25°C. Calculate the new partial pressure of oxygen . Calculate the new partial pressure of helium . Calculate the new total pressure of both gases .

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Dalton’s Law of Partial Pressures Find number of moles of each gass, n O2 and n He mol K mol K atm L L atm RT PV n mol K mol K atm L L atm RT PV n nRT PV He o 70 . 0 ) 298 ( * ) * / * 08206 . 0 ( 5 . 8 * 0 . 2 46 . 1 ) 298 ( * ) * / * 08206 . 0 ( 4 . 27 * 3 . 1 2
Find the partial pressure for each gas in new volume (tank), P O2 and P He Find total pressure of the mixture P total = 6.14 + 2.95= 6.09 atm atm L K mol K atm L mol V nRT P atm L K mol K atm L mol V nRT P O O 95 . 2 81 . 5 298 * ) * / * 08206 . 0 ( * 70 . 0 14 . 6 81 . 5 298 * ) * / * 08206 . 0 ( * 46 . 1 2 2 Dalton’s Law of Partial Pressures

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Mole Fraction and Partial Pressures The mole fraction (χ) is a dimensionless number total total P P P P P RT V P P RT V P n n 1 2 1 1 2 1 1 1 1 ) ( RT V P n V RT n P 1 1 1 1 , total n n 1 1 The partial pressure of a component of a gas mixture is equal to the mole fraction of that component times the total pressure of the mixture.
Example 5. The partial pressure of nitrogen in air is 592

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Lecture 6 PartII Chem 102SP - Chapter 5 Gases Daltons Law...

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