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Such random mixing of solutions occurs if the interaction energies between unlike molecules are similar to the average interaction energies between like molecules. [2]: 149 [3] The value of the entropy corresponds exactly to random mixing for ideal solutions and for regular solutions, and approximately so for many real solutions. [3] [4]
An ideal solution or ideal mixture is a solution that exhibits thermodynamic properties analogous to those of a mixture of ideal gases. [1] The enthalpy of mixing is zero [2] as is the volume change on mixing by definition; the closer to zero the enthalpy of mixing is, the more "ideal" the behavior of the solution becomes.
This formula holds because there is no change in volume upon mixing for an ideal mixture. The molar entropy, in contrast, is given by = ( + ¯), where the term originates from the entropy of mixing of an ideal mixture.
A regular solution or mixture has a non-zero enthalpy of mixing with an ideal entropy of mixing. [ 9 ] [ 10 ] Under this assumption, Δ H m i x {\displaystyle \Delta H_{mix}} scales linearly with X 1 X 2 {\displaystyle X_{1}X_{2}} , and is equivalent to the excess internal energy.
Flory–Huggins solution theory is a lattice model of the thermodynamics of polymer solutions which takes account of the great dissimilarity in molecular sizes in adapting the usual expression for the entropy of mixing. The result is an equation for the Gibbs free energy change for mixing a polymer with a solvent. Although it makes simplifying ...
A special case of entropy increase, the entropy of mixing, occurs when two or more different substances are mixed. If the substances are at the same temperature and pressure, there is no net exchange of heat or work – the entropy change is entirely due to the mixing of the different substances.
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Raoult's law (/ ˈ r ɑː uː l z / law) is a relation of physical chemistry, with implications in thermodynamics.Proposed by French chemist François-Marie Raoult in 1887, [1] [2] it states that the partial pressure of each component of an ideal mixture of liquids is equal to the vapor pressure of the pure component (liquid or solid) multiplied by its mole fraction in the mixture.