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In s. Gases will always flow from a region of higher partial pressure to one of lower pressure; the larger this difference, the faster the flow. Vapor Pressure is the pressure of a Vapor in equilibrium with its non-vapor phases (i.e., liquid or solid). Most often the term is used to describe a Liquid 's tendency to Evaporate . It is a measure of the tendency of Molecule s and Atom s to escape from a liquid or a Solid . A liquid's boiling point corresponds to the point where its vapor pressure is equal to the surrounding atmospheric pressure. Gases dissolve, diffuse, and react according to their partial pressures, and not necessarily according to their Concentration s in a gas mixture. DALTON'S LAW OF PARTIAL PRESSURES See Also: Dalton's law The pressure of an Ideal Gas in a mixture is equal to the pressure it would exert if it occupied the same volume alone at the same temperature. This is because ideal gas molecules are so far apart that they don't interfere with each other at all. Actual real-world gases come very close to this ideal. A consequence of this is that the total pressure of a mixture of ideal gases is equal to the sum of the partial pressures of the individual gases in the mixture as stated by (N2), Hydrogen (H2) and Ammonia (NH3): : IDEAL GAS MIXTURES The Mole Fraction of an individual gas component in an ideal gas mixture can be expressed in terms of the component's partial pressure or the Moles of the component: : and the partial pressure of an individual gas component in an ideal gas can be obtained using this expression: :
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| align | left= partial pressure of any individual gas component in a gas mixture |
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