Non-random two-liquid model

VLE of the mixture of Chloroform and Methanol plus NRTL fit and extrapolation to different pressures

The non-random two-liquid model^[1] (short NRTL equation) is an activity coefficient model that correlates the activity coefficients γ_i of a compound i with its mole fractions x_i in the liquid phase concerned. It is frequently applied in the field of chemical engineering to calculate phase equilibria. The concept of NRTL is based on the hypothesis of Wilson that the local concentration around a molecule is different from the bulk concentration. This difference is due to a difference between the interaction energy of the central molecule with the molecules of its own kind U_ii and that with the molecules of the other kind U_ij. The energy difference also introduces a non-randomness at the local molecular level. The NRTL model belongs to the so-called local-composition models. Other models of this type are the Wilson model, the UNIQUAC model, and the group contribution model UNIFAC. These local-composition models are not thermodynamically consistent due to the assumption that the local composition around molecule i is independent of the local composition around molecule j. This assumption is not true, as was shown by Flemmer in 1976.^[2]

Equations for a binary mixture

For a binary mixture the following equations^[3] are used:

$\left\{\begin{matrix} \ln\ \gamma_1=x^2_2\left[\tau_{21}\left(\frac{G_{21}}{x_1+x_2 G_{21}}\right)^2 +\frac{\tau_{12} G_{12}} {(x_2+x_1 G_{12})^2 }\right] \\ \\ \ln\ \gamma_2=x^2_1\left[\tau_{12}\left(\frac{G_{12}}{x_2+x_1 G_{12}}\right)^2 +\frac{\tau_{21} G_{21}} {(x_1+x_2 G_{21})^2 }\right] \end{matrix}\right.$

with

$\left\{\begin{matrix} \ln\ G_{12}=-\alpha_{12}\ \tau_{12} \\ \ln\ G_{21}=-\alpha_{21}\ \tau_{21} \end{matrix}\right.$

In here τ₁₂ and τ₂₁ are the dimensionless interaction parameters, which are related to the interaction energy parameters Δg₁₂ and Δg₂₁ by:

$\left\{\begin{matrix} \tau_{12}=\frac{\Delta g_{12}}{RT}=\frac{U_{12}-U_{22}}{RT} \\ \tau_{21}=\frac{\Delta g_{21}}{RT}=\frac{U_{21}-U_{11}}{RT} \end{matrix}\right.$

Here R is the gas constant and T the absolute temperature, and U_ij is the energy between molecular surface i and j. U_ii is the energy of evaporation. Here U_ij has to be equal to U_ji, but Δg_ij is not necessary equal to Δg_ji.

The parameters α₁₂ and α₂₁ are the so-called non-randomness parameter, for which usually α₁₂ is set equal to α₂₁. For a liquid, in which the local distribution is random around the center molecule, the parameter α₁₂ = 0. In that case the equations reduce to the one-parameter Margules activity model:

$\left\{\begin{matrix} \ln\ \gamma_1=x^2_2\left[\tau_{21} +\tau_{12} \right]=Ax^2_2 \\ \ln\ \gamma_2=x^2_1\left[\tau_{12}+\tau_{21} \right]=Ax^2_1 \end{matrix}\right.$

In practice, α₁₂ is set to 0.2, 0.3 or 0.48. The latter value is frequently used for aqueous systems. The high value reflects the ordered structure caused by hydrogen bonds. However in the description of liquid-liquid equilibria the non-randomness parameter is set to 0.2 to avoid wrong liquid-liquid description. In some cases a better phase equilibria description is obtained by setting α₁₂ = − 1^[4]. However this mathematical solution is impossible from a physical point of view, since no system can be more random than random (α₁₂ =0). In general NRTL offers more flexibility in the description of phase equilibria than other activity models due to the extra non-randomness parameters. However in practice this flexibility is reduced in order to avoid wrong equilibrium description outside the range of regressed data.

The limiting activity coefficients, aka the activity coefficients at infinite dilution, are calculated by:

$\left\{\begin{matrix} \ln\ \gamma_1^\infty=\left[\tau_{21} +\tau_{12} exp{(-\alpha_{12}\ \tau_{12})} \right] \\ \ln\ \gamma_2^\infty=\left[\tau_{12} +\tau_{21}exp{(-\alpha_{12}\ \tau_{21})}\right] \end{matrix}\right.$

The expressions show that at α₁₂ = 0 the limiting activity coefficients are equal. This situation that occurs for molecules of equal size, but of different polarities.
It also shows, since three parameters are available, that multiple sets of solutions are possible.

General equations

The general equation for ln(γ_i) for species i in a mixture of n components is^[5]:

$\ln(\gamma_i)=\frac{\displaystyle\sum_{j=1}^{n}{x_{j}\tau_{ji}G_{ji}}}{\displaystyle\sum_{k=1}^{n}{x_{k}G_{ki}}}+\sum_{j=1}^{n}{\frac{x_{j}G_{ij}}{\displaystyle\sum_{k=1}^{n}{x_{k}G_{kj}}}}{\left ({\tau_{ij}-\frac{\displaystyle\sum_{m=1}^{n}{x_{m}\tau_{mj}G_{mj}}}{\displaystyle\sum_{k=1}^{n}{x_{k}G_{kj}}}}\right )}$

with

$G_{ij}=\text{exp}\left ({-\alpha_{ij}\tau_{ij}}\right )$

$\alpha_{ij}=\alpha_{ij_{0}}+\alpha_{ij_{1}}T$

$\tau_{ij}=A_{ij}+\frac{B_{ij}}{T}+\frac{C_{ij}}{T^{2}}+D_{ij}\ln{\left ({T}\right )}+E_{ij}T^{F_{ij}}$

There are several different equations forms for α_ij and τ_ij, the most general of which are shown above.

Temperature dependent parameters

To describe phase equilibria over a large temperature regime, i.e. larger than 50 K, the interaction parameter has to be made temperature dependent. Two formats are frequently used. The extended Antoine equation format:

$\tau_{ij}=f(T)=a_{ij}+\frac{b_{ij}}{T}+c_{ij}\ \ln\ T+d_{ij}T$

Here the logarithmic term is mainly used in the description of liquid-liquid equilibria (miscibility gap).

The other format is a third-order polynomial format:

$\Delta g_{ij}=f(T)=a_{ij}+b_{ij}\cdot T +c_{ij}T^{2}$

Parameter determination

The NRTL parameters are fitted to activity coefficients that have been derived from experimentally determined phase equilibrium data (vapor–liquid, liquid–liquid, solid–liquid) as well as from heats of mixing. The source of the experimental data are often factual data banks like the Dortmund Data Bank. Other options are direct experimental work and predicted activity coefficients with UNIFAC and similar models. Noteworthy is that for the same liquid mixture several NRTL parameter sets might exist. The NRTL parameter set to use depends on the kind of phase equilibrium (i.e. solid–liquid, liquid–liquid, vapor–liquid). In the case of the description of a vapor–liquid equilibria it is necessary to know which saturated vapor pressure of the pure components was used and whether the gas phase was treated as an ideal or a real gas. Accurate saturated vapor pressure values are important in the determination or the description of an azeotrope. The gas fugacity coefficients are mostly set to unity (ideal gas assumption), but for vapor-liquid equilibria at high pressures (i.e. > 10 bar) an equation of state is needed to calculate the gas fugacity coefficient for a real gas description.

Literature

1. ^ Renon H., Prausnitz J. M., "Local Compositions in Thermodynamic Excess Functions for Liquid Mixtures", AIChE J., 14(1), S.135–144, 1968
2. ^ McDermott (Fluid Phase Equilibrium 1(1977)33) and Flemr (Coll. Czech. Chem.Comm., 41 (1976) 3347)
3. ^ Reid R. C., Prausnitz J. M., Poling B. E., The Properties of Gases & Liquids, 4th Edition, McGraw-Hill, 1988
4. ^ Effective Local Compositions in Phase Equilibrium Correlations, J. M. Marina, D. P. Tassios Ind. Eng. Chem. Process Des. Dev., 1973, 12 (1), pp 67–71
5. ^ http://users.rowan.edu/~hesketh/0906-316/Handouts/Pages%20from%20SimBasis%20appendix%20A%20property%20packages.pdf