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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.
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 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.
The pure component's molar volume and molar enthalpy are equal to the corresponding partial molar quantities because there is no volume or internal energy change on mixing for an ideal solution. The molar volume of a mixture can be found from the sum of the excess volumes of the components of a mixture:
JPMorgan Chase, Bank of America and Citigroup reminded employees that they can take paid time off to vote in Tuesday's U.S. presidential election, while underscoring the need to work across ...
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.
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