Dalton's Law of Partial Pressures

The total pressure of a mixture of gases, which do not interact chemically, is equal to the sum of the partial pressures. The sum of the pressures that each gas would exert if it alone occupied the volume containing the mixture.

Example
Dry oxygen gas at 713 torr is saturated with water vapour at 25 torr, the pressure of the wet gas is 738 torr.

See also: Avogadro′s Law, Boyles Gas Law, Charles Gas Law, Dalton, John, Ideal Gas Law, Partial Pressures.

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Subjects: Thermodynamics