UNIQUAC (universal quasichemical) is an activity coefficient model used in description of phase equilibria.  The model is a so-called lattice model and has been derived from a first order approximation of interacting molecule surfaces in statistical thermodynamics. The model is however not fully thermodynamically consistent due to its two liquid mixture approach. In this approach the local concentration around one central molecule is assumed to be independent from the local composition around another type of molecule.
The UNIQUAC model can be considered a second generation activity coefficient because its expression for the Excess Gibbs energy consists of an entropy term in addition to an enthalpy term. Earlier activity coefficient models such as the Wilson equation and the Non-random two-liquid model (NRTL model) only consist of enthalpy terms.
Today the UNIQUAC model is frequently applied in the description of phase equilibria (i.e. liquid–solid, liquid–liquid or liquid–vapor equilibrium). The UNIQUAC model also serves as the basis of the development of the group contribution method UNIFAC, where molecules are subdivided into functional groups. In fact, UNIQUAC is equal to UNIFAC for mixtures of molecules, which are not subdivided; e.g. the binary systems water-methanol, methanol-acryonitrile and formaldehyde-DMF.
In the UNIQUAC model the activity coefficients of the ith component of a two component mixture are described by a combinatorial and a residual contribution.
The first is an entropic term quantifying the deviation from ideal solubility as a result of differences in molecule shape. The latter is an enthalpic [nb 1] correction caused by the change in interacting forces between different molecules upon mixing.
The combinatorial contribution accounts for shape differences between molecules and affects the entropy of the mixture and is based on the lattice theory. The excess entropy γC is calculated exclusively from the pure chemical parameters, using the relative Van der Waals volumes ri and surface areas qi [nb 2] of the pure chemicals.
With the volume fraction per mixture mole fraction, Vi, for the ith
component given by:
And the surface area fraction per mixture molar fraction, Fi, for the ith component is given by:
The first 3 terms on the right hand side of the combinatorial term form the Flory-Huggins contribution, while the remaining term, the Guggenhem-Staverman correction, reduce this because connecting segments cannot be placed in all direction in space. This spatial correction shifts the result of the Flory-Huggins term about 5% towards an ideal solution. The coordination number, z, i.e. the number of close interacting molecules around a central molecule, is frequently set to 10. It can be regarded as an average value that lies between cubic (z=6) and hexagonal packing (z=12) of molecules that are simplified by spheres.
In the case of infinite dilution for a binary mixture, the equations for the combinatorial contribution reduce to:
This pair of equations show that molecules of same shape, i.e. same r and q parameters, have
The residual, enthalpic term contains an empirical parameter, , which is determined from the binary interaction energy parameters. The expression for the residual activity coefficient for molecule i is:
[J/mol] is the binary interaction energy parameter. Theory defines , and , where is the interaction energy between molecules and . The interaction energy parameters are usually determined from activity coefficients, vapor-liquid, liquid-liquid, or liquid-solid equilibrium data.
Usually , because the energies of evaporation (i.e. ), are in many cases different, while the energy of interaction between molecule i and j is symmetric, and therefore . If the interactions between the j molecules and i molecules is the same as between molecules i and j, there is no excess energy of mixing, . And thus
Alternatively, in some process simulation software can be expressed as follows :
The "C", "D", and "E" coefficients are primarily used in fitting liquid–liquid equilibria data (with "D" and "E" rarely used at that). The "C" coefficient is useful for vapor-liquid equilibria data as well. The use of such an expression ignores the fact that on a molecular level the energy, Δuij, is temperature independent. It is a correction to repair the simplifications, which were applied in the derivation of the model.
Applications (Phase Equilibrium Calculations)
Activity coefficients can be used to predict simple phase equilibria (vapour–liquid, liquid–liquid, solid–liquid), or to estimate other physical properties (e.g. viscosity of mixtures). Models such as UNIQUAC allow chemical engineers to predict the phase behavior of multicomponent chemical mixtures. They are commonly used in process simulation programs to calculate the mass balance in and around separation units.
UNIQUAC requires two basic underlying parameters: Relative surface and volume fractions are chemical constants, which must be known for all chemicals (r(i) and q(i) parameters, respectively). Empirical parameters between components that describes the intermolecular behaviour. These parameters must be known for all binary pairs in the mixture. In a quaternary mixture there are six such parameters (1–2,1–3,1–4,2–3,2–4,3–4) and the number rapidly increases with additional chemical components. The empirical parameters are obtained by a correlation process from experimental equilibrium compostions or activity coefficients, or from phase diagrams, from which the activity coefficients themselves can be calculated. An alternative is to obtain activity coefficients with a method such as UNIFAC, and the UNIFAC parameters can then be simplified by fitting to obtain the UNIQUAC parameters. This method allows for the more rapid calculation of activity coefficients, rather than direct usage of the more complex method.
Remark that the determination of parameters from LLE data can be difficult depending on the complexity of the studied system. For this reason it is necessary to confirm the consistency of the obtained parameters in the whole range of compositions (including binary subsystems, experimental and calculated lie-lines, Hessian matrix, etc.). 
UNIQUAC has been extended by several research groups. Some selected derivatives are: UNIFAC, a method which permits the volume, surface and in particular, the binary interaction parameters to be estimated. This eliminates the use of experimental data to calculate the UNIQUAC parameters, extensions for the estimation of activity coefficients for electrolytic mixtures, extensions for better describing the temperature dependence of activity coefficients, and solutions for specific molecular arrangements.
- Chemical equilibrium
- Chemical thermodynamics
- MOSCED, a model for estimating limiting activity coefficients at infinite dilution
- NRTL, an alternative to UNIQUAC of the same local composition type
- Here it is assumed that the enthalpy change upon mixing can be assumed to be equal to the energy upon mixing, since the liquid excess molar volume is small and Δ Hex=ΔUex+Vex ΔP ≈ ΔU
- Here it is assumed that all molecules have the same coordination number as the methylene group of an alkane, which is the reference to calculate the relative volume and surface area.
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- Marcilla, Antonio; Reyes-Labarta, Juan A.; Olaya, M.Mar (2017). "Should we trust all the published LLE correlation parameters in phase equilibria? Necessity of their Assessment Prior to Publication". Fluid Phase Equilibria. 433: 243–252. doi:10.1016/j.fluid.2016.11.009.
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- "The Extended UNIQUAC model".
- Wisniewska-Goclowska B., Malanowski S.K., “A new modification of the UNIQUAC equation including temperature dependent parameters”, Fluid Phase Equilib., 180, 103–113, 2001
- Andreas Klamt, Gerard J. P. Krooshof, Ross Taylor “COSMOSPACE: Alternative to conventional activity-coefficient models”, AIChE J., 48(10), 2332–2349,2004