| Amagat's law of additive volumes | states that the volume of a gas mixture is equal to the sum of the volumes each gas would occupy if it existed alone at the mixture temperature and pressure.
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| Apparent gas constant | of a mixture is the universal gas constant divided by the apparent molar mass of the mixture.
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| Apparent molar mass | of a mixture can be expressed as the sum of the products of the mole fraction and molar mass of each component in the mixture.
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| Average gas constant | (see apparent gas constant)
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| Average molar mass | (see apparent molar mass)
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| Chemical potential | is the change in the Gibbs function of the mixture in a specified phase when a unit amount of a given component of the mixture in the same phase is added as pressure and temperature and the amounts of all other components are held constant. The chemical potential of a component of an ideal gas mixture depends on the mole fraction of the components as well as the mixture temperature and pressure, and is independent of the identity of the other constituent gases.
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| Component pressure | is the pressure a component in a gas mixture would have if it existed alone at the volume and temperature of the mixture.
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| Component volume | is the volume a component in a gas mixture would occupy if it existed alone at the temperature and pressure of the mixture.
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| Dalton's law of additive pressures | states that the pressure of a gas mixture is equal to the sum of the pressures each gas would exert if it existed alone at the mixture temperature and volume.
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| Extensive properties | of a nonreacting ideal-or real-gas mixture are obtained by just adding the contributions of each component of the mixture.
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| Gibbs-Dalton law | an extension of Dalton's law of additive pressures, states that under the ideal-gas approximation, the properties of a gas in a mixture are not influenced by the presence of other gases, and each gas component in the mixture behaves as if it exists alone at the mixture temperature and mixture volume.
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| Gravimetric analysis | is one way to describe the composition of a mixture that is accomplished by specifying the mass of each component.
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| Ideal mixture or ideal solution | is a mixture where the effect of dissimilar molecules in a mixture on each other is negligible and the chemical potential of a component in such a mixture is simply taken to be the Gibbs function of the pure component.
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| Intensive properties | of a nonreacting ideal-or real-gas mixture are obtained by dividing the extensive properties by the mass or the mole number of the mixture in the gas mixture. The internal energy, enthalpy, and entropy of a gas mixture per unit mass or per unit mole of the mixture can be determined by summing the products of the mass fractions and the specific property or summing the products of the mole fractions and the molar specific property. That is, the intensive properties of a gas mixture are determined by either a mass weighted or a mole weighted average of the properties.
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| Kay's rule | proposed by W. B. Kay in 1936, predicts the P-v-T behavior of a gas mixture by determining the compressibility factor for a gas mixture at the reduced pressure and reduced temperature defined in terms of the pseudocritical pressure (the sum of the products of the mole fraction and critical pressure of each component) and pseudocritical temperature (the sum of the products of the mole fraction and critical temperature of each component).
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| Mass fraction | is the ratio of the mass of one component in a mixture to the total mass of the mixture.
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| Molar analysis | is one way to describe the composition of a mixture that is accomplished by specifying the number of moles of each component.
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| Mole fraction | is the ratio of the number of moles of one component in a mixture to the total moles of the mixture. Note that for an ideal-gas mixture, the mole fraction, the pressure fraction, and the volume fraction of a component are identical.
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| Nonreacting gas mixture | is a mixture of gases not undergoing a chemical reaction and can be treated as a pure substance since it is usually a homogeneous mixture of different gases.
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| Osmotic pressure | is the pressure difference across a semipermeable membrane that separates fresh water from the saline water under equilibrium conditions.
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| Osmotic rise | is the vertical distance saline water would rise when separated from the fresh water by a membrane that is permeable to water molecules alone at equilibrium.
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| Partial pressure | of a component in a gas mixture is the product of the mole fraction and the mixture pressure. The partial pressure is identical to the component pressure for ideal gas mixtures.
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| Partial volume | of a component in a gas mixture is the product of the mole fraction and the mixture volume. The partial volume is identical to the component volume for ideal gas mixtures.
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| Pressure fraction | of a gas component in a gas mixture is the ratio of the component pressure to the mixture pressure. Note that for an ideal-gas mixture, the mole fraction, the pressure fraction, and the volume fraction of a component are identical.
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| Volume fraction | of a gas component in a gas mixture is the ratio of the component volume to the mixture volume. Note that for an ideal-gas mixture, the mole fraction, the pressure fraction, and the volume fraction of a component are identical.
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