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Partial Pressures

Partial Pressures. Dalton’s Law of Partial Pressures & Air Pressure. 8 mm Hg. P. 590 mm Hg. Ar. P. P. P. P. P. N 2. P. = + + +. Total. O 2. N 2. CO 2. Ar. 149 mm Hg. P. P. O 2.

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Partial Pressures

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  1. Partial Pressures

  2. Dalton’s Law of Partial Pressures & Air Pressure 8 mm Hg P 590 mm Hg Ar P P P P P N2 P = + + + Total O2 N2 CO2 Ar 149 mm Hg P P O2 149 590 3 8 mm Hg = + + + Total 3 mm Hg P CO2 PTotal = 750 mm Hg EARTH

  3. Dalton’s Partial Pressures Zumdahl, Zumdahl, DeCoste, World of Chemistry2002, page 421

  4. Dalton’s Law Zumdahl, Zumdahl, DeCoste, World of Chemistry2002, page 422

  5. Dalton’s Law Applied Suppose you are given four containers – three filled with noble gases. The first 1 L container is filled with argon and exerts a pressure of 2 atm. The second 3 liter container is filled with krypton and has a pressure of 380 mm Hg. The third 0.5 L container is filled with xenon and has a pressure of 607.8 kPa. If all these gases were transferred into an empty 2 L container…what would be the pressure in the “new” container? PKr = 380 mm Hg Ptotal = ? PAr = 2 atm Pxe 607.8 kPa V = 1 liter V = 3 liters V = 0.5 liter V = 2 liters

  6. …just add them up PKr = 380 mm Hg Ptotal = ? PAr = 2 atm Pxe 607.8 kPa V = 1 liter V = 3 liters V = 0.5 liter V = 2 liters Dalton’s Law of Partial Pressures “Total Pressure = Sum of the Partial Pressures” PT = PAr + PKr + PXe + … P1 x V1 = P2 x V2 P1 x V1 = P2 x V2 (0.5 atm) (3L) = (X atm) (2L) (6 atm) (0.5 L) = (X atm) (2L) PKr = 0.75 atm Pxe = 1.5 atm PT = 1 atm + 0.75 atm + 1.5 atm PT = 3.25 atm

  7. Same Gas, Volume, and Temperature, but… Dorin, Demmin, Gabel, Chemistry The Study of Matter , 3rd Edition, 1990, page 316

  8. Same Gas, Volume, and Temperature, but…different numbers of moles Dorin, Demmin, Gabel, Chemistry The Study of Matter , 3rd Edition, 1990, page 316

  9. Adding and Removing Gases

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