1 Partial Pressure Pressure of individual gases in a mixture.

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Presentation transcript:

1 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

2 atm 1 atm 3 atm 6 atm

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?

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 Mole Fraction

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. Example

Gas Collection 8

9 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 P tot = P gas + P water P gas = P tot - P water

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

Example 11 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?