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Partial Pressure

Partial Pressure. Pressure of individual gases in a mixture. Daltons’ Law of Partial Pressures. The total pressure inside a container is equal to the partial pressure due to each gas. The partial pressure is the contribution by that gas. P Total = P 1 + P 2 + P 3. 6 atm. 1 atm. 2 atm.

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Partial Pressure

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  1. Partial Pressure • Pressure of individual gases in a mixture

  2. Daltons’ Law of Partial Pressures • The total pressure inside a container is equal to the partial pressure due to each gas. • The partial pressure is the contribution by that gas. • PTotal = P1 + P2 + P3

  3. 6 atm 1 atm 2 atm 3 atm

  4. Examples • What is the total pressure in a balloon filled with air if the pressure of the oxygen is 170 mm Hg and the pressure of nitrogen is 620 mm Hg? • In a second balloon the total pressure is 1.3 atm. What is the pressure of oxygen if the pressure of nitrogen is 720 mm Hg?

  5. More Examples • What pressure is exerted by a mixture of 2.00 g of hydrogen gas and 8.00 g of nitrogen gas at 273 K and in a 10.0 L vessel? • If a .20 L sample of oxygen at 0°C and 1 atm and a .10 L sample of nitrogen at 0°C and 2.0 atm are both placed in a .40 L container at 0°C, what is the total pressure of the mixture?

  6. Mole Fraction • Ratio of the number of moles of a component in a mixture to the total number of moles in the mixture • Numerically equal to the ratio of the partial pressure of a component gas to the total pressure of the gas mixture

  7. Example • The partial pressure of oxygen was observed to be 156 torr in air with a total atmospheric pressure of 743 torr. Calculate the mole fraction of oxygen in the sample.

  8. Gas Collection

  9. Gas Collection • When a gas is collected over water, water vapor ends up in the gas • The pressure of the pure gas is the total pressure minus the pressure of the water vapor Ptot = Pgas + Pwater Pgas = Ptot - Pwater

  10. Water Vapor Pressure • Pressure of the water vapor depends on the temperature at which the gas is collected

  11. Example • Carbon dioxide gas is collected over water at a temperature of 18°C. The barometric pressure reads 775 mm Hg. What is the pressure of the carbon dioxide?

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