Viscosity models for mixtures

Short description: Mathematical models for calculating viscosity

The shear viscosity (or viscosity, in short) of a fluid is a material property that describes the friction between internal neighboring fluid surfaces (or sheets) flowing with different fluid velocities. This friction is the effect of (linear) momentum exchange caused by molecules with sufficient energy to move (or "to jump") between these fluid sheets due to fluctuations in their motion. The viscosity is not a material constant, but a material property that depends on temperature, pressure, fluid mixture composition, and local velocity variations. This functional relationship is described by a mathematical viscosity model called a constitutive equation which is usually far more complex than the defining equation of shear viscosity. One such complicating feature is the relation between the viscosity model for a pure fluid and the model for a fluid mixture which is called mixing rules. When scientists and engineers use new arguments or theories to develop a new viscosity model, instead of improving the reigning model, it may lead to the first model in a new class of models. This article will display one or two representative models for different classes of viscosity models, and these classes are:

* Elementary kinetic theory and simple empirical models[1][2][3] \- viscosity for dilute gas with nearly spherical molecules
* Power series[2][3] \- simplest approach after dilute gas
* Equation of state analogy[3] between PVT and TηP
* Corresponding state[2][3] model - scaling a variable with its value at the critical point
* Friction force theory[3] \- internal sliding surface analogy to a sliding box on an inclined surface
* Multi- and one-parameter version of friction force theory
* Transition state analogy - molecular energy needed to squeeze into a vacancy analogous to molecules locking into each other in a chemical reaction
* Free volume theory[3] \- molecular energy needed to jump into a vacant position in the neighboring surface
* Significant structure theory[3] \- based on Eyring's concept of liquid as a blend of solid-like and gas-like behavior / features

Selected contributions from these development directions is displayed in the following sections. This means that some known contributions of research and development directions are not included. For example, is the group contribution method applied to a shear viscosity model not displayed. Even though it is an important method, it is thought to be a method for parameterization of a selected viscosity model, rather than a viscosity model in itself.

The microscopic or molecular origin of fluids means that transport coefficients like viscosity can be calculated by time correlations which are valid for both gases and liquids, but it is computer intensive calculations. Another approach is the Boltzmann equation which describes the statistical behaviour of a thermodynamic system not in a state of equilibrium. It can be used to determine how physical quantities change, such as heat energy and momentum, when a fluid is in transport, but it is computer intensive simulations.

From Boltzmann's equation one may also analytically derive (analytical) mathematical models for properties characteristic to fluids such as viscosity, thermal conductivity, and electrical conductivity (by treating the charge carriers in a material as a gas). See also convection–diffusion equation. The mathematics is so complicated for polar and non-spherical molecules that it is very difficult to get practical models for viscosity. The purely theoretical approach will therefore be left out for the rest of this article, except for some visits related to dilute gas and significant structure theory.

## Contents

* 1 Use, definition and dependence
* 2 Dilute gas limit and scaled variables
* 2.1 Elementary kinetic theory
* 2.2 Kinetic theory
* 2.3 Empirical correlation
* 2.4 Kinetic theory with empirical extension
* 2.5 Trend functions and scaling
* 3 Classic mixing rules
* 3.1 Classic mixing rules for gas
* 3.2 Classic mixing rules for liquid
* 4 Power series
* 4.1 Mixture
* 4.2 Mixing rules
* 4.3 EOS
* 4.4 Dilute gas contribution
* 5 Corresponding state principle
* 5.1 Mixture
* 5.2 Mixing rules
* 5.3 Reference fluid
* 6 Equation of state analogy
* 6.1 Mixture
* 6.2 Mixing rules
* 7 Friction force theory
* 7.1 Multi-parameter friction force theory
* 7.1.1 Friction functions
* 7.1.2 Mixture
* 7.1.3 Mixing rules
* 7.2 One-parameter friction force theory
* 7.2.1 Reduced friction functions
* 7.2.2 Mixture
* 7.2.3 Mixing rules
* 7.2.4 Dilute gas limit
* 7.2.5 Light gases
* 8 Transition state analogy
* 8.1 Free volume theory
* 8.1.1 Mixture
* 8.1.2 Mixing rules
* 8.1.3 Trend functions
* 8.2 Significant structure theory
* 8.2.1 Gas-like contribution
* 8.2.2 Solid-like contribution
* 8.2.3 Mixture
* 8.2.4 Mixing rules
* 9 See also
* 10 References

## Use, definition and dependence

The classic Navier-Stokes equation is the balance equation for momentum density for an isotropic, compressional and viscous fluid that is used in fluid mechanics in general and fluid dynamics in particular:

ρ[∂𝐮∂t+𝐮⋅∇𝐮]=−∇P+∇[ζ(∇⋅𝐮)]+∇⋅[η(∇𝐮+(∇𝐮)T−23(∇⋅𝐮)𝐈)]+ρ𝐠

On the right hand side is (the divergence of) the total stress tensor σ which consists of a pressure tensor (−P𝐈) and a dissipative (or viscous or deviatoric) stress tensor τd. The dissipative stress consists of a compression stress tensor τc (term no. 2) and a shear stress tensor τs (term no. 3). The rightmost term ρ𝐠 is the gravitational force which is the body force contribution, and ρ is the mass density, and 𝐮 is the fluid velocity.

σ=−P𝐈+τd=−P𝐈+τc+τs

For fluids, the spatial or Eularian form of the governing equations is preferred to the material or Lagrangian form, and the concept of velocity gradient is preferred to the equivalent concept of strain rate tensor. Stokes assumptions for a wide class of fluids therefore says that for an isotropic fluid the compression and shear stresses are proportional to their velocity gradients, 𝐂 and 𝐒0 respectively, and named this class of fluids for Newtonian fluids. The classic defining equation for volume viscosity ζ and shear viscosity η are respectively:

τc=3ζ𝐂

τs=2η𝐒0

The classic compression velocity "gradient" is a diagonal tensor that describes a compressing (alt. expanding) flow or attenuating sound waves:

𝐂=13(∇⋅𝐮)𝐈

The classic Cauchy shear velocity gradient, is a symmetric and traceless tensor that describes a pure shear flow (where pure means excluding normal outflow which in mathematical terms means a traceless matrix) around e.g. a wing, propeller, ship hull or in e.g. a river, pipe or vein with or without bends and boundary skin:

𝐒0=𝐒−13(∇⋅𝐮)𝐈

where the symmetric gradient matrix with non-zero trace is

𝐒=12[∇𝐮+(∇𝐮)T]

How much the volume viscosity contributes to the flow characteristics in e.g. a choked flow such as convergent-divergent nozzle or valve flow is not well known, but the shear viscosity is by far the most utilized viscosity coefficient. The volume viscosity will now be abandoned, and the rest of the article will focus on the shear viscosity.

Another application of shear viscosity models is Darcy's law for multiphase flow.

𝐮a=−ηa−1𝐊ra⋅𝐊⋅(∇Pa−ρa𝐠) where a = water, oil, gas

and 𝐊 and 𝐊ra are absolute and relative permeability, respectively. These 3 (vector) equations models flow of water, oil and natural gas in subsurface oil and gas reservoirs in porous rocks. Although the pressures changes are big, the fluid phases will flow slowly through the reservoir due to the flow restriction caused by the porous rock.

The above definition is based on a shear-driven fluid motion that in its most general form is modelled by a shear stress tensor and a velocity gradient tensor. The fluid dynamics of a shear flow is, however, very well illustrated by the simple Couette flow. In this experimental layout, the shear stress τs and the shear velocity gradient 𝐒0 (where now 𝐒0=𝐒) takes the simple form:

τ=ηSwhereτ=FAandS=dudy=umaxymax

Inserting these simplifications gives us a defining equation that can be used to interpret experimental measurements:

FA=ηdudy=ηumaxymax

where A is the area of the moving plate and the stagnant plate, y is the spatial coordinate normal to the plates. In this experimental setup, value for the force F is first selected. Then a maximum velocity umax is measured, and finally both values are entered in the equation to calculate viscosity. This gives one value for the viscosity of the selected fluid. If another value of the force is selected, another maximum velocity will be measured. This will result in another viscosity value if the fluid is a non-Newtonian fluid such as paint, but it will give the same viscosity value for a Newtonian fluid such as water, petroleum oil or gas. If another parameter like temperature, T, is changed, and the experiment is repeated with the same force, a new value for viscosity will be the calculated, for both non-Newtonian and Newtonian fluids. The great majority of material properties varies as a function of temperature, and this goes for viscosity also. The viscosity is also a function of pressure and, of course, the material itself. For a fluid mixture, this means that the shear viscosity will also vary according to the fluid composition. To map the viscosity as a function of all these variables require a large sequence of experiments that generates an even larger set of numbers called measured data, observed data or observations. Prior to, or at the same time as, the experiments is a material property model (or short material model) proposed to describe or explain the observations. This mathematical model is called the constitutive equation for shear viscosity. It is usually an explicit function that contains some empirical parameters that is adjusted in order to match the observations as good as the mathematical function is capable to do.

For a Newtonian fluid, the constitutive equation for shear viscosity is generally a function of temperature, pressure, fluid composition:

η=f(T,P,𝐰)where𝐰=𝐱,𝐲,𝐳,1purefluid

where 𝐱 is the liquid phase composition with molfraction xi for fluid component i, and 𝐲 and 𝐳 are the gas phase and total fluid compositions, respectively. For a non-Newtonian fluid (in the sense of a generalized Newtonian fluid), the constitutive equation for shear viscosity is also a function of the shear velocity gradient:

η=f(T,P,𝐰,𝐒0)where𝐰=𝐱,𝐲,𝐳,1purefluid

The existence of the velocity gradient in the functional relationship for non-Newtonian fluids says that viscosity is generally not an equation of state, so the term constitutional equation will in general be used for viscosity equations (or functions). The free variables in the two equations above, also indicates that specific constitutive equations for shear viscosity will be quite different from the simple defining equation for shear viscosity that is shown further up. The rest of this article will show that this is certainly true. Non-Newtonian fluids will therefore be abandoned, and the rest of this article will focus on Newtonian fluids.

## Dilute gas limit and scaled variables

### Elementary kinetic theory

In textbooks on elementary kinetic theory[1] one can find results for dilute gas modeling that have widespread use. Derivation of the kinetic model for shear viscosity usually starts by considering a Couette flow where two parallel plates are separated by a gas layer. This non-equilibrium flow is superimposed on a Maxwell–Boltzmann equilibrium distribution of molecular motions.

Let σ be the collision cross section of one molecule colliding with another. The number density C is defined as the number of molecules per (extensive) volume C=N/V. The collision cross section per volume or collision cross section density is Cσ, and it is related to the mean free path l by

l=12Cσ

Combining the kinetic equations for molecular motion with the defining equation of shear viscosity gives the well known equation for shear viscosity for dilute gases:

η0=23π⋅mkBTσ=23π⋅MRTσNA

where

kB⋅NA=RandM=m⋅NA

where kB is the Boltzmann constant, NA is the Avogadro constant, R is the gas constant, M is the molar mass and m is the molecular mass. The equation above presupposes that the gas density is low (i.e. the pressure is low), hence the subscript zero in the variable η0. This implies that the kinetic translational energy dominates over rotational and vibrational molecule energies. The viscosity equation displayed above further presupposes that there is only one type of gas molecules, and that the gas molecules are perfect elastic hard core particles of spherical shape. This assumption of particles being like billiard balls with radius r, implies that the collision cross section of one molecule can be estimated by

σ=π(2r)2=πd2for monomolecular gases and monoparticle beam experiments

σij=π(ri+rj)2=π4(di+dj)2for binary collision in gas mixtures and dissimilar bullet / target particles

But molecules are not hard particles. For a reasonably spherical molecule the interaction potential is more like the Lennard-Jones potential or even more like the Morse potential. Both have a negative part that attracts the other molecule from distances much longer than the hard core radius, and thus models the van der Waals forces. The positive part models the repulsive forces as the electron clouds of the two molecules overlap. The radius for zero interaction potential is therefore appropriate for estimating (or defining) the collision cross section in kinetic gas theory, and the r-parameter (conf. r,ri) is therefore called kinetic radius. The d-parameter (where d=2r,di=2ri) is called kinetic diameter.

The macroscopic collision cross section σ⋅NA is often associated with the critical molar volume Vc, and often without further proof or supporting arguments, by

σNA∝Vc2/3orσNA=23π⋅Krv−1Vc2/3

where Krv is molecular shape parameter that is taken as an empirical tuning parameter, and the pure numerical part is included in order to make the final viscosity formula more suitably for practical use. Inserting this interpretation of σNA, and use of reduced temperature Tr, gives

η0=TrKrvDrvwhereTr=T/Tcand

Drv=(MRTc)1/2Vc−2/3=R1/2Dv

which implies that the empirical parameter Krv is dimensionless, and that Drv and η0 have the same units. The parameter Drv is a scaling parameter that involves the gas constant R and the critical molar volume Vc, and it used to scale the viscosity. In this article the viscosity scaling parameter will frequently be denoted by Dxyz which involve one or more of the parameters R, Vc, Pc in addition to critical temperature Tc and molar mass M. Incomplete scaling parameters, such as the parameter Dv above where the gas constant R is absorbed into the empirical constant, will often be encountered in practice. In this case the viscosity equation becomes

η0=TrKvDv

where the empirical parameter Kv is not dimensionless, and a proposed viscosity model for dense fluid will not be dimensionless if Dv is the common scaling factor. Notice that

η0=TrKrvDrv=TrKvDv⟹Kv=R1/2Krv

Inserting the critical temperature in the equation for dilute viscosity gives

η0c=KrvDrv=KvDv

The default values of the parameters Krv and Kv should be fairly universal values, although Kv depends on the unit system. However, the critical molar volume in the scaling parameters Drv and Dv is not easily accessible from experimental measurements, and that is a significant disadvantage. The general equation of state for a real gas is usually written as

PV=ZRT⟹PcVc=ZcRTc

where the critical compressibility factor Zc, which reflects the volumetric deviation of the real gases from the ideal gas, is also not easily accessible from laboratory experiments. However, critical pressure and critical temperature are more accessible from measurements. It should be added that critical viscosity is also not readily available from experiments.

Uyehara and Watson (1944)[4] proposed to absorb a universal average value of Zc (and the gas constant R) into a default value of the tuning parameter Kp as a practical solution of the difficulties of getting experimental values for Vc and/or Zc. The visocity model for a dilute gas is then

η0=TrKpDpwhereTr=T/Tcand

Dp=Tc−1/6Pc2/3M1/2

By inserting the critical temperature in the formula above, the critical viscosity is calculated as

η0c=KpDp

Based on an average critical compressibility factor of Z¯c=0.275 and measured critical viscosity values of 60 different molecule types, Uyehara and Watson (1944)[4] determined an average value of Kp to be

K¯p=7.7⋅1.013252/3≈7.77for[η0]=μPand[Pc]=bar

The cubic equation of state (EOS) are very popular equations that are sufficiently accurate for most industrial computations both in vapor-liquid equilibrium and molar volume. Their weakest points are perhaps molar volum in the liquid region and in the critical region. Accepting the cubic EOS, the molar hard core volume b can be calculated from the turning point constraint at the critical point. This gives

b=ΩbRTcPcwhich is similar toVc=Z¯cRTcPc

where the constant Ωb is a universal constant that is specific for the selected variant of the cubic EOS. This says that using Dp, and disregarding fluid component variations of Zc, is in practice equivalent to say that the macroscopic collision cross section is proportional to the hard core molar volume rather than the critical molar volume.

In a fluid mixture like a petroleum gas or oil there are lots of molecule types, and within this mixture there are families of molecule types (i.e. groups of fluid components). The simplest group is the n-alkanes which are long chains of CH2-elements. The more CH2-elements, or carbon atoms, the longer molecule. Critical viscosity and critical thermodynamic properties of n-alkanes therefore show a trend, or functional behaviour, when plotted against molecular mass or number of carbon atoms in the molecule (i.e. carbon number). Parameters in equations for properties like viscosity usually also show such trend behaviour. This means that

η0cj=KpjDpj≠K¯pDpjfor many or most fluid components j

This says that the scaling parameter Dp alone is not a true or complete scaling factor unless all fluid components have a fairly similar (and preferably spherical) shape.

The most important result of this kinetic derivation is perhaps not the viscosity formula, but the semi-empirical parameter Dp that is used extensively throughout the industry and applied science communities as a scaling factor for (shear) viscosity. The literature often reports the reciprocal parameter and denotes it as ξ.

The dilute gas viscosity contribution to the total viscosity of a fluid will only be important when predicting the viscosity of vapors at low pressures or the viscosity of dense fluids at high temperatures. The viscosity model for dilute gas, that is shown above, is widely used throughout the industry and applied science communities. Therefore, many researchers do not specify a dilute gas viscosity model when they propose a total viscosity model, but leave it to the user to select and include the dilute gas contribution. Some researchers do not include a separate dilute gas model term, but propose an overall gas viscosity model that cover the entire pressure and temperature range they investigated.

In this section our central macroscopic variables and parameters and their units are temperature T [K], pressure P [bar], molar mass M [g/mol], low density (low pressure or dilute) gas viscosity η0 [μP]. It is, however, common in the industry to use another unit for liquid and high density gas viscosity η [cP].

### Kinetic theory

From Boltzmann's equation Chapman and Enskog derived a viscosity model for a dilute gas.

η0×106=2.6693MTσ2Ω(T*)whereT*=kBT/ε

where ε is (the absolute value of) the energy-depth of the potential well (see e.g. Lennard-Jones interaction potential). The term Ω(T*) is called the collision integral, and it occurs as a general function of temperature that the user must specify, and that is not a simple task. This illustrates the situation for the molecular or statistical approach: The (analytical) mathematics gets incredible complex for polar and non-spherical molecules making it very difficult to achieve practical models for viscosity based on a statistical approach. The purely statistical approach will therefore be left out in the rest of this article.

### Empirical correlation

Zéberg-Mikkelsen (2001)[3] proposed empirical models for gas viscosity of fairly spherical molecules that is displayed in the section on Friction Force theory and its models for dilute gases and simple light gases. These simple empirical correlations illustrate that empirical methods competes with the statistical approach with respect to gas viscosity models for simple fluids (simple molecules).

### Kinetic theory with empirical extension

The gas viscosity model of Chung et alios (1988)[5] is combination of the Chapman–Enskog(1964) kinetic theory of viscosity for dilute gases and the empirical expression of Neufeld et alios (1972)[6] for the reduced collision integral, but expanded empirical to handle polyatomic, polar and hydrogen bonding fluids over a wide temperature range. This viscosity model illustrates a successful combination of kinetic theory and empiricism, and it is displayed in the section of Significant structure theory and its model for the gas-like contribution to the total fluid viscosity.

### Trend functions and scaling

In the section with models based on elementary kinetic theory, several variants of scaling the viscosity equation was discussed, and they are displayed below for fluid component i, as a service to the reader.

η0i=TriKrviDrviwhereDrvi=MiRTci⋅Vci−2/3

η0i=TriKviDvi whereDvi =MiTci⋅Vci−2/3

η0i=TriKpiDpi whereDpi =Mi1/2Pci2/3⋅Tci−1/6

Zéberg-Mikkelsen (2001)[3] proposed an empirical correlation for the Vci parameter for n-alkanes, which is

Vci−1=A+B⋅PciRTci⟺Vci=RTciARTci+BPci

A=0.000235751 mol/cm3andB=3.42770

The critical molar volume of component i Vci is related to the critical mole density ρnci and critical mole concentration cci by the equation Vci−1=ρnci=cci. From the above equation for Vci−1 it follows that

Zci=PciARTci+BPci⟺ZciRTciPciVci=1

where Zci is the compressibility factor for component i, which is often used as an alternative to Vci. By establishing a trend function for the parameter Vci for a homologous series, groups or families of molecules, parameter values for unknown fluid components in the homologous group can be found by interpolation and extrapolation, and parameter values can easily re-generateat at later need. Use of trend functions for parameters of homologous groups of molecules have greatly enhanced the usefulness of viscosity equations (and thermodynamic EOSs) for fluid mixtures such as petroleum gas and oil.[2]

Uyehara and Watson (1944)[4] proposed a correlation for critical viscosity (for fluid component i) for n-alkanes using their average parameter K¯p and the classical pressure dominated scaling parameter Dpi :

ηci=K¯pDpi

K¯p=7.7⋅1.013252/3≈7.77for[η0]=μPand[Pc]=bar

Zéberg-Mikkelsen (2001)[3] proposed an empirical correlation for critical viscosity ηci parameter for n-alkanes, which is

ηci=C⋅PciMiD

C=0.597556 μP/bar⋅(g/mol)−DandD=0.601652

The unit equations for the two constitutive equations above by Zéberg-Mikkelsen (2001) are

[Pc]=barand[Vc]=[RTc/Pc]=cm3/moland[T]=Kand[Zc]=1and[ηc]=μP

Inserting the critical temperature in the three viscosity equations from elementary kinetic theory gives three parameter equations.

ηci=KrviDrvi=KviDvi=KpiDpior

Krvi=ηciDrviandKvi=ηciDviandKpi=ηciDpi

The three viscosity equations now coalesce to a single viscosity equation

η0i=Triηci=TηciTci

because a nondimensional scaling is used for the entire viscosity equation. The standard nondimensionality reasoning goes like this: Creating nondimensional variables (with subscript D) by scaling gives

ηDi=η0iηciandTDi=TTci=Tri⟹ηDiηci=TDiKpiDpi

Claiming nondimensionality gives

KpiDpiηci=1⟺Kpi=ηciDpi⟹ηDi=TDi

The collision cross section and the critical molar volume which are both difficult to access experimentally, are avoided or circumvented. On the other hand, the critical viscosity has appeared as a new parameter, and critical viscosity is just as difficult to access experimentally as the other two parameters. Fortunately, the best viscosity equations have become so accurate that they justify calculation in the critical point, especially if the equation is matched to surrounding experimental data points.

## Classic mixing rules

### Classic mixing rules for gas

Wilke (1950)[7] derived a mixing rule based on kinetic gas theory

ηgmix=∑i=1Nηgi1+1yi∑j=1,j≠iNyjφij

φij=[1+η0iη0j2⋅MjMi4]24221+MiMj2

The Wilke mixing rule is capable of describing the correct viscosity behavior of gas mixtures showing a nonlinear and non-monotonical behavior, or showing a characteristic bump shape, when the viscosity is plotted versus mass density at critical temperature, for mixtures containing molecules of very different sizes. Due to its complexity, it has not gained widespread use. Instead, the slightly simpler mixing rule proposed by Herning and Zipperer (1936),[8] is found to be suitable for gases of hydrocarbon mixtures.

### Classic mixing rules for liquid

The classic Arrhenius (1887).[9] mixing rule for liquid mixtures is

ln⁡ηlmix=∑i=1Nxiln⁡ηli

where ηlmix is the viscosity of the liquid mixture, ηli is the viscosity (equation) for fluid component i when flowing as a pure fluid, and xi is the molfraction of component i in the liquid mixture.

The Grunberg-Nissan (1949)[10] mixing rule extends the Arrhenius rule to

ln⁡ηlmix=∑i=1Nxiln⁡ηli+∑i=1N∑j=1Nxixjdij

where dij are empiric binary interaction coefficients that are special for the Grunberg-Nissan theory. Binary interaction coefficients are widely used in cubic EOS where they often are used as tuning parameters, especially if component j is an uncertain component (i.e. have uncertain parameter values).

Katti-Chaudhri (1964)[11] mixing rule is

ln⁡(ηlmixVlmix)=∑i=1Nxiln⁡(ηliVli)

where Vli is the partial molar volume of component i, and Vlmix is the molar volume of the liquid phase and comes from the vapor-liquid equilibrium (VLE) calculation or the EOS for single phase liquid.

A modification of the Katti-Chaudhri mixing rule is

ln⁡(ηlmixV)=∑i=1Nziln⁡(ηliVli)+ΔGERT

ΔGE=∑i=1N∑j=1NzizjEij

where GE is the excess activation energy of the viscous flow, and Eij is the energy that is characteristic of intermolecular interactions between component i and component j, and therefore is responsible for the excess energy of activation for viscous flow. This mixing rule is theoretically justified by Eyring's representation of the viscosity of a pure fluid according to Glasstone et alios (1941).[12] The quantity ηliVli has been obtained from the time-correlation expression for shear viscosity by Zwanzig (1965).[13]

## Power series

Very often one simply selects a known correlation for the dilute gas viscosity η0, and subtracts this contribution from the total viscosity which is measured in the laboratory. This gives a residual viscosity term, often denoted Δη, which represents the contribution of the dense fluid, ηdf.

ηdf=η−η0⟺η=η0+ηdf

The dense fluid viscosity is thus defined as the viscosity in excess of the dilute gas viscosity. This technique is often used in developing mathematical models for both purely empirical correlations and models with a theoretical support. The dilute gas viscosity contribution becomes important when the zero density limit (i.e. zero pressure limit) is approached. It is also very common to scale the dense fluid viscosity by the critical viscosity, or by an estimate of the critical viscosity, which is a characteristic point far into the dense fluid region. The simplest model of the dense fluid viscosity is a (truncated) power series of reduced mole density or pressure. Jossi et al. (1962)[14] presented such a model based on reduced mole density, but its most widespread form is the version proposed by Lohrenz et al. (1964)[15] which is displayed below.

[ηdfDp+10−4]1/4=LBC

The LBC-function is then expanded in a (truncated) power series with empirical coefficients as displayed below.

LBC=LBC(ρnr)=∑i=15aiρnri−1

The final viscosity equation is thus

η=η0−10−4Dp+DpL4

η0=η0(T)

Dp=Tc−1/6Pc2/3Mn1/2

Local nomenclature list:

* ρn : mole density [mol/cm3]
* ρnr: reduced mole density [1]
* M : molar mass [g/mol]
* Pc : critical pressure [atm]
* T : temperature [K]
* Tc : critical temperature [K]
* Vc : critical molar volume [cm3/mol]
* η : viscosity [cP]

### Mixture

ηmix=η0mix−10−4Dpmix+DpmixLmix4

LBCmix=LBCmix(crmix)=∑i=15aicrmixi−1

Dpmix=Tcmix−1/6Pcmix2/3Mmix1/2

η0mix=η0mix(T)

The formula for η0 that was chosen by LBC, is displayed in the section called Dilute gas contribution.

LBC constants  i  | ai

|

1  | 0.10230
2  | 0.023364
3  | 0.058533
4  | −0.040758
5  | 0.0093324

### Mixing rules

Tcmix=∑iziTci

Mmix=Mn=∑iziMi

Pcmix=∑iziPci

ρncmix−1=Vcmix=∑iziVci+zC7+⋅VcC7+i<C7+

The subscript C7+ refers to the collection of hydrocarbon molecules in a reservoir fluid with oil and/or gas that have 7 or more carbon atoms in the molecule. The critical volume of C7+ fraction has unit ft3/lb mole, and it is calculated by

VcC7+=21.573+0.015122⋅MC7+−27.656⋅SGC7++0.070615⋅MC7+SGC7+

where SGC7+ is the specific gravity of the C7+ fraction.

Tcifori≥C7+orTcC7+is taken from EOS characterization

Mifori≥C7+orMC7+is taken from EOS characterization

Pcifori≥C7+orPcC7+is taken from EOS characterization

The molar mass Mi (or molecular mass) is normally not included in the EOS formula, but it usually enters the characterization of the EOS parameters.

### EOS

From the equation of state the molar volume of the reservoir fluid (mixture) is calculated.

Vmix=Vmix(T,P)for 1 mole fluid

The molar volume V is converted to mole density ρn (also called mole concentration and denoted c), and then scaled to be reduced mole density ρnr.

ρnmix=1/Vmixandρncmix=1/Vcmixandρnrmix=Vcmix/Vmix=ρnmix/ρncmix

### Dilute gas contribution

The correlation for dilute gas viscosity of a mixture is taken from Herning and Zipperer (1936)[8] and is

η0mix(T)=∑iziη0i(Tri)Mi1/2∑jzjMj1/2i,j<C7+

The correlation for dilute gas viscosity of the individual components is taken from Stiel and Thodos (1961)[16] and is

η0i(Tri)={34×10−5⋅DpiTri0.94ifTri⩽1.517.78×10−5⋅Dpi(4.58⋅Tri−1.67)5/8ifTri>1.5

where

Dpi=Tci−1/6Pci2/3Mi1/2i<C7+

Tri=TTcii<C7+

## Corresponding state principle

The principle of corresponding states (CS principle or CSP) was first formulated by van der Waals, and it says that two fluids (subscript a and z) of a group (e.g. fluids of non-polar molecules) have approximately the same reduced molar volume (or reduced compressibility factor) when compared at the same reduced temperature and reduced pressure. In mathematical terms this is

Va(Pra,Tra)Vca=Vz(Prz,Trz)Vcz⟺Va(Pa,Ta)=VcaVcz⋅Vz(Pz=PaPczPca,Tz=TaTczTca)

When the common CS principle above is applied to viscosity, it reads

η(P,T)=ηcηcz⋅ηz(Pz,Tz)≈KpDpKpzDpz⋅ηz(Pz,Tz)

Note that the CS principle was originally formulated for equilibrium states, but it is now applied on a transport property - viscosity, and this tells us that another CS formula may be needed for viscosity.

In order to increase the calculation speed for viscosity calculations based on CS theory, which is important in e.g. compositional reservoir simulations, while keeping the accuracy of the CS method, Pedersen et al. (1984, 1987, 1989)[17][18][2] proposed a CS method that uses a simple (or conventional) CS formula when calculating the reduced mass density that is used in the rotational coupling constants (displayed in the sections below), and a more complex CS formula, involving the rotational coupling constants, elsewhere.

### Mixture

The simple corresponding state principle is extended by including a rotational coupling coefficient α as suggested by Tham and Gubbins (1970).[19] The reference fluid is methane, and it is given the subscript z.

ηmix(P,T)=(TcmixTcz)−1/6⋅(PcmixPcz)2/3⋅(MmixMz)1/2⋅αcmixαcz⋅ηz(Pz,Tz)

Pz=P⋅PczαzPcmixαmix

Tz=T⋅TczαzTcmixαmix

### Mixing rules

The interaction terms for critical temperature and critical volume are

Tcij=(TciTcj)1/2

Vcij=18(Vci1/3+Vcj1/3)3

The parameter Vci is usually uncertain or not available. One therefore wants to avoid this parameter. Replacing Zci with the generic average parameter Z¯c for all components, gives

Vci=RZciTci/Pci=R¯zcTci/PciwhereR¯zc=RZ¯c

Vcij=18Rzc((TciPci)1/3+(TcjPcj)1/3)3

Tcmix=∑i∑jzizjVcijTcij∑i∑jzizjVcij

The above expression for Vcij is now inserted into the equation for Tcmix. This gives the following mixing rule

Tcmix=∑i∑jzizj((TciPci)1/3+(TcjPcj)1/3)3(TciTcj)1/2∑i∑jzizj((TciPci)1/3+(TcjPcj)1/3)3

Mixing rule for the critical pressure of the mixture is established in a similar way.

Pcmix=RzcTcmix/Vcmix

Vcmix=∑i∑jzizjVcij

Pcmix=8∑i∑jzizj((TciPci)1/3+(TcjPcj)1/3)3(TciTcj)1/2(∑i∑jzizj((TciPci)1/3+(TcjPcj)1/3)3)2

The mixing rule for molecular weight is much simpler, but it is not entirely intuitive. It is an empirical combination of the more intuitive formulas with mass weighting M‾w and mole weighting M‾n.

Mmix=1.304×10−4(M‾w2.303−M‾n2.303)+M‾n

M‾w=∑iziMi2∑jzjMjandM‾n=∑iziMi

The rotational coupling parameter for the mixture is

αmix=1+7.378×10−3ρrzα1.847Mmix0.5173

### Reference fluid

The accuracy of the final viscosity of the CS method needs a very accurate density prediction of the reference fluid. The molar volume of the reference fluid methane is therefore calculated by a special EOS, and the Benedict-Webb-Rubin (1940)[20] equation of state variant suggested by McCarty (1974),[21] and abbreviated BWRM, is recommended by Pedersen et al. (1987) for this purpose. This means that the fluid mass density in a grid cell of the reservoir model may be calculated via e.g. a cubic EOS or by an input table with unknown establishment. In order to avoid iterative calculations, the reference (mass) density used in the rotational coupling parameters is therefore calculated using a simpler corresponding state principle which says that

Pzα=P⋅PczPcmixandTzα=T⋅TczTcmix⇒Vzα=V(Tzα,Pzα)for 1 mole methane

The molar volume is used to calculate the mass concentration, which is called (mass) density, and then scaled to be reduced density which is equal to reciprocal of reduced molar volume because there is only on component (molecule type). In mathematical terms this is

ρzα=Mz/Vzαandρcz=Mz/Vcz⇒ρrzα=ρzα/ρcz=Vcz/Vzα

The formula for the rotational coupling parameter of the mixture is shown further up, and the rotational coupling parameter for the reference fluid (methane) is

αz=1+0.031ρrzα1.847

The methane mass density used in viscosity formulas is based on the extended corresponding state, shown at the beginning of this chapter on CS-methods. Using the BWRM EOS, the molar volume of the reference fluid is calculated as

Vz=V(Tz,Pz)for 1 mole methane

Once again, the molar volume is used to calculate the mass concentration, or mass density, but the reference fluid is a single component fluid, and the reduced density is independent of the relative molar mass. In mathematical terms this is

ρz=Mz/Vzandρcz=Mz/Vcz⇒ρrz=ρz/ρcz=Vcz/Vz

The effect of a changing composition of e.g. the liquid phase is related to the scaling factors for viscosity, temperature and pressure, and that is the corresponding state principle.

The reference viscosity correlation of Pedersen et al. (1987)[18] is

ηz(ρz,Tz)=η0(Tz)+η^1(Tz)ρz+F1Δη′(ρz,Tz)+F2Δη″(ρz,Tz)

The formulas for η0(Tz), η^1(Tz), Δη′(ρz,Tz) are taken from Hanley et al. (1975).[22]

The dilute gas contribution is

η0(Tz)=∑i=19giTzi−34

The temperature dependent factor of the first density contribution is

η^1(Tz)=h1−h2[h3−ln(Tzh4)]2

The dense fluid term is

Δη′(ρz,Tz)=ej1+j4/Tz×[exp[ρz0.1(j2+j3/Tz3/2)+θrzρz0.5(j5+j6/Tz+j7/Tz2)]−1]

where exponential function is written both as ex and as exp[x]. The molar volume of the reference fluid methane, which is used to calculate the mass density in the viscosity formulas above, is calculated at a reduced temperature that is proportional to the reduced temperature of the mixture. Due to the high critical temperatures of heavier hydrocarbon molecules, the reduced temperature of heavier reservoir oils (i.e. mixtures) can give a transferred reduced methane temperature that is in the neighborhood of the freezing temperature of methane. This is illustrated using two fairly heavy hydrocarbon molecules, in the table below. The selected temperatures are a typical oil or gas reservoir temperature, the reference temperature of the International Standard Metric Conditions for Natural Gas (and similar fluids) and the freezing temperature of methane (Tfz).

Transfer of reduced temperature  | Temp.  | Temp.  | n-decane  | n-eicosane  | methane  | Trc10h22 | Trc20h42

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Temperature  | deg C  | K  | Trc10h22 | Trc20h42 | Trc1h4 | ->Trc1h4 | ->Trc1h4
Tc(K) |  |  | 617.6  | 767  | 190.6  |  |
reservoir  | 95  | 368.15  | 0.60  | 0.48  | 1.93  | 0.60  | 0.48
ISMC-NG  | 15  | 288.15  | 0.47  | 0.38  | 1.51  | 0.47  | 0.38
Tfc1h4 | −182.45  | 90.7  | 0.15  | 0.12  | 0.48  |  |

Pedersen et al. (1987) added a fourth term, that is correcting the reference viscosity formula at low reduced temperatures. The temperature functions F1 and F2 are weight factors. Their correction term is

Δη″(ρz,Tz)=ek1+k4/Tz×[exp[ρz0.1(k2+k3/Tz3/2)+θrzρz0.5(k5+k6/Tz+k7/Tz2)]−1]
HCH and PF constants  i  | gi | hi | ji | ki

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1  | −2.090975E5  | 1.696985927  | −10.3506  | −9.74602
2  | 2.647269E5  | 0.133372346  | 17.5716  | 18.0834
3  | −1.472818E5  | 1.4  | −3019.39  | −4126.66
4  | 4.716740E4  | 168.0  | 188.730  | 44.6055
5  | −9.481872E3  |  | 0.0429036  | 0.976544
6  | 1.219979E3  |  | 145.290  | 81.8134
7  | −9.627993E1  |  | 6127.68  | 15649.9
8  | 4.274152E0  |  |  |
9  | −8.141531E-2  |  |  |

θrz=(ρz−ρcz)/ρcz=ρrz−1

F1=HTAN+12

F2=1−HTAN2

HTAN=tanh(ΔTz)=e(ΔTz)−e(−ΔTz)e(ΔTz)+e(−ΔTz)

ΔTz=Tz−Tfz

## Equation of state analogy

Phillips (1912)[23] plotted temperature T versus viscosity η for different isobars for propane, and observed a similarity between these isobaric curves and the classic isothermal curves of the PVT surface. Later, Little and Kennedy (1968)[24] developed the first viscosity model based on analogy between TηP and PVT using van der Waals EOS. Van der Waals EOS was the first cubic EOS, but the cubic EOS has over the years been improved and now make up a widely used class of EOS. Therefore, Guo et al. (1997)[25] developed two new analogy models for viscosity based on PR EOS (Peng and Robinson 1976) and PRPT EOS (Patel and Teja 1982)[26] respectively. The following year T.-M. Guo (1998)[27] [3] modified the PR based viscosity model slightly, and it is this version that will be presented below as a representative of EOS analogy models for viscosity.

PR EOS is displayed on the next line.

P=RTV−beos−aeosV(V+beos)+beos(V−beos)

The viscosity equation of Guo (1998) is displayed on the next line.

T=rPη−d−aη(η+b)+b(η−b)

To prepare for the mixing rules, the viscosity equation is re-written for a single fluid component i.

T=riPηi−di−aiηi(ηi+bi)+bi(ηi−bi)

Details of how the composite elements of the equation are related to basic parameters and variables, is displayed below.

ai=0.45724rci2Pci2Tci

bi=0.07780rciPciTci

ri=rciτi(Tri,Pri)

di=biϕi(Tri,Pri)

rci=ηciTciPciZci

ηci=KpDpiwhereKp=7.7⋅104andDpi=Tci−1/6Mi1/2Pci2/3

τi=τi(Tri,Pri)=(1+Q1i(TriPri−1))−2

ϕi=ϕi(Tri,Pri)=exp⁡[Q2i(Tri−1)]+Q3i(Pri−1)2

Q1i={0.829599+0.350857ωi−0.747680ωi2,if ωi<0.30.956763+0.192829ωi−0.303189ωi2,if ωi≥0.3

Q2i={1.94546−3.19777ωi+2.80193ωi2,if ωi<0.3−0.258789−37.1071ωi+20.5510ωi2,if ωi≥0.3

Q3i={0.299757+2.20855ωi−6.64959ωi2,if ωi<0.35.16307−12.8207ωi+11.0109ωi2,if ωi≥0.3

### Mixture

T=rmixPηmix−dmix−amixηmix(ηmix+bmix)+bmix(ηmix−bmix)

### Mixing rules

amix=∑i=1ziai

bmix=∑i=1zibi

dmix=∑i=1∑i=1zizididi(1−kij)

rmix=∑i=1ziri

## Friction force theory

### Multi-parameter friction force theory

The multi-parameter version of the friction force theory (short FF theory and FF model), also called friction theory (short F-theory), was developed by Quiñones-Cisneros et al. (2000, 2001a, 2001b and Z 2001, 2004, 2006),[28][29][30][3][31][32] and its basic elements, using some well known cubic EOSs, are displayed below.

It is a common modeling technique to accept a viscosity model for dilute gas (η0), and then establish a model for the dense fluid viscosity ηdf. The FF theory states that for a fluid under shear motion, the shear stress τ (i.e. the dragging force) acting between two moving layers can be separated into a term τ0 caused by dilute gas collisions, and a term τdf caused by friction in the dense fluid.

η=η0+ηdfandτ=τ0+τdf

The dilute gas viscosity (i.e. the limiting viscosity behavior as the pressure, normal stress, goes to zero) and the dense fluid viscosity (the residual viscosity) can be calculated by

τ0=η0dudyandτdf=ηdfdudy

where du/dy du/dy is the local velocity gradient orthogonal to the direction of flow. Thus

η0=τ0du/dyandηdf=τdfdu/dy

The basic idea of QZS (2000) is that internal surfaces in a Couette flow acts like (or is analogue to) mechanical slabs with friction forces acting on each surface as they slide past each other. According to the Amontons-Coulomb friction law in classical mechanics, the ratio between the kinetic friction force F and the normal force N is given by

ζ=FN=AτdfAσ=τdfσ

where ζ is known as the kinetic friction coefficient, A is the area of the internal flow surface, τ is the shear stress and σ is the normal stress (or pressure P) between neighboring layers in the Couette flow.

ηdf=τdfdu/dy=ζσdu/dy

The FF theory of QZS says that when a fluid is brought to have shear motion, the attractive and repulsive intermolecular forces will contribute to amplify or diminish the mechanical properties of the fluid. The friction shear stress term τdf of the dense fluid can therefore be considered to consist of an attractive friction shear contribution τdfatt and a repulsive friction shear contribution τdfrep. Inserting this gives us

ηdf=τdfrep+τdfattdu/dy=ζPdu/dy

The well known cubic equation of states (SRK, PR and PRSV EOS), can be written in a general form as

P=RTV−b−aV2+ubV+wb2

The parameter pair (u,w)=(1,0) gives the SRK EOS, and (u,w)=(2,-1) gives both the PR EOS and the PRSV EOS because they differ only in the temperature and composition dependent parameter / function a. Input variables are, in our case, pressure (P), temperature (T) and for mixtures also fluid composition which can be single phase (or total) composition 𝐳=[z1,⋯,zN], vapor (gas) composition 𝐲=[y1,⋯,yN] or liquid (in our example oil) composition 𝐱=[x1,⋯,xN]. Output is the molar volume of the phase (V). Since the cubic EOS is not perfect, the molar volume is more uncertain than the pressure and temperature values.

The EOS consists of two parts that are related to van der Waals forces, or interactions, that originates in the static electric fields of the colliding parts /spots of the two (or more) colliding molecules. The repulsive part of the EOS is usually modeled as a hard core behavior of molecules, hence the symbol (Ph), and the attractive part (Pa) is based on the attractive interaction between molecules (conf. van der Waals force). The EOS can therefore be written as

P=Ph−Pa

Assume that the molar volume (V) is known from EOS calculations, and prior vapor-liquid equilibrium (VLE) calculations for mixtures. Then the two functions Ph and Pa can be utilized, and these functions are expected to be a more accurate and robust than the molar volume (V) itself. These functions are

Ph=Ph(V,T,𝐰)=RTV−bwhere𝐰=𝐱,𝐲,𝐳,1purefluid

Pa=Pa(V,T,𝐰)=aV2+ubV+wb2where𝐰=𝐱,𝐲,𝐳,1purefluid

The friction theory therefore assumes that the residual attractive stress τfatt and the residual repulsive stress τfrep are functions of the attractive pressure term Pa and the repulsive pressure term Ph, respectively.

τdfatt=F(T,Pa,𝐰)andτdfrep=F(T,Ph,𝐰)and𝐰=𝐱,𝐲,𝐳,1purefluid

The first attempt is, of course, to try a linear function in the pressure terms / functions.

ηdf=KaPa+KhPh

All K coefficients are in general functions of temperature and composition, and they are called friction functions. In order to achieve high accuracy over a wide pressure and temperature ranges, it turned out that a second order term was needed even for non-polar molecules types such as hydrocarbon fluids in oil and gas reservoirs, in order to achieve a high accuracy at very high pressures. A test with a presumably difficult 3-component mixture of non-polar molecule types needed a third order power to achieve high accuracy at the most extreme super-critical pressures.

η=η0+KaPa+KhPh+Kh2Ph2+Kh3Ph3

This article will concentrate on the second order version, but the third order term will be included whenever possible in order to show the total set of formulas. As an introduction to mixture notation, the above equation is repeated for component i in a mixture.

ηi=η0i+KaiPai+KhiPhi+Kh2iPhi2+Kh3iPhi3

The unit equations for the central variables in the multi-parameter FF-model is

[Pc]=barand[T]=Kand[η]=μP

#### Friction functions

Friction functions for fluid component i in the 5 parameter model for pure n-alkane molecules are presented below.

Kai=Ba1iexp⁡(Γi−1)+Ba2i[exp⁡(2Γi−2)−1]

Khi=Bh1iexp⁡(Γi−1)+Bh2i[exp⁡(2Γi−2)−1]

Kh2i=Bh22i[exp⁡(2Γi)−1]

Γi=Tci/T

Friction functions for fluid component i in the 7- and 8-parameter models are presented below.

Kai=Ba0i+Ba1i[exp⁡(Γi−1)−1]+Ba2i[exp⁡(2Γi−2)−1]

Khi=Bh0i+Bh1i[exp⁡(Γi−1)−1]+Bh2i[exp⁡(2Γi−2)−1]

Kh2i=Bh22i[exp⁡(2Γi)−1]

Kh3i=Bh32i[exp⁡(2Γi)−1](Γi−1)3

Γi=Tci/T

The empirical constants in the friction functions are called friction constants. Friction constants for some n-alkanes in the 5 parameter model using SRK and PRSV EOS (and thus PR EOS) is presented in tables below. Friction constants for some n-alkanes in the 7 parameter model using PRSV EOS are also presented in a table below. The constant d2 for three fluid components are presented below in the last table of this table-series.

#### Mixture

Pdyn=P=RTVeos−beos−aeosVeos2+ubeosVeos+wbeos2

In the single phase regions, the mole volume of the fluid mixture is determined by the input variables are pressure (P), temperature (T) and (total) fluid composition 𝐳. In the two-phase gas-liquid region a vapor-liquid equilibrium (VLE) calculation splits the fluid into a vapor (gas) phase with composition 𝐲 and phase mixture molfraction ng and a liquid phase (in our example oil) with composition 𝐱 and phase mixture molfraction no. For liquid phase, vapor phase and single phase fluid the relation to VLE and EOS variables are

Phmix=Pheos(Veos,T,𝐰)=RTVeos−beoswhere𝐰=𝐱,𝐲,𝐳

Pamix=Paeos(Veos,T,𝐰)=aeosVeos2+ubeosVeos+wbeos2where𝐰=𝐱,𝐲,𝐳

In a compositional reservoir simulator the pressure is calculated dynamically for each grid cell and each timestep. This gives dynamic pressures for vapor and liquid (oil) or single phase fluid. Assuming zero capillary pressure between hydrocarbon liquid (oil) and gas, the simulator software code will give a single dynamic pressure Pdyn which applies to both the vapor mixture and the liquid (oil) mixture. In this case the reservoir simulator software code may use

Pamix=Phmix−PdynandPhmix=Pheos(Veos,T,𝐰)=RTVeos−beoswhere𝐰=𝐱,𝐲,𝐳

Phmix=Pdyn+PamixandPamix=Paeos(Veos,T,𝐰)=aeosVeos2+ubeosVeos+wbeos2where𝐰=𝐱,𝐲,𝐳

The friction model for viscosity of a mixture is

ηmix=η0mix+ηdfmix

ηmix=η0mix+KamixPamix+KhmixPhmix+Kh2mixPhmix2+Kh3mixPhmix3

The cubic power term is only needed when molecules with a fairly rigid 2-D structure are included in the mixture, or the user requires a very high accuracy at exemely high pressures. The standard model includes only linear and quadratic terms in the pressure functions.

#### Mixing rules

ln⁡(η0mix)=∑i=1Nziln⁡(η0i)orη0mix=∏i=1Nη0izi

Kqmix=∑i=1NWiKqiwhereq=a,h,h2

ln⁡(Kh3mix)=∑i=1Nziln⁡(Kh3i)orKh3mix=∏i=1NKh3izi

where the empirical weight fraction is

Wi=ziMiε⋅MMwhereMM=∑j=1NzjMjε

The recommended values for ε are

* ε=0.15 gave best performance for SRK EOS
* ε=0.075 gave best performance for PRSV EOS

These values are established from binary mixtures of n-alkanes using a 5-parameter viscosity model, and they seems to be used for 7- and 8-parameter models also. The motivation for this weight parameter Wi, and thus the ε-parameter, is that in asymmetric mixtures like CH4 \- C10H12, the lightest component tends to decrease the viscosity of the mixture more than linearly when plotted versus molfraction of the light component (or the heavy component).

The friction coefficients of some selected fluid components is presented in the tables below for the 5,7 and 8-parameter models. For convenience are critical viscosities also included in the tables.

FF5 for n-alkanes using SRK EOS  | Name  | Bh1 | Bh2 | Ba1 | Ba2 | Bh22 | ηc

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Formula  |  | μP/bar | μP/bar | μP/bar | μP/bar | μP/bar2 | μP
CH4 | Methane  | 0.0954878  | −0.0983074  | −0.424734  | 0.0598492  | 1.34730E-5  | 152.930
C2H6 | Ethane  | 0.0404072  | −0.241910  | −0.745442  | 0.0144118  | 1.53201E-5  | 217.562
C3H8 | Propane  | 0.322169  | −0.104459  | −0.692914  | 0.0515112  | 1.08144E-5  | 249.734
C4H10 | n-Butane  | 0.554315  | −0.0334891  | −0.577284  | 0.066969  | 1.03272E-5  | 257.682
C5H12 | n-Pentane  | 0.556934  | −0.143105  | −0.825295  | 0.0812198  | 1.67262E-5  | 258.651
C6H14 | n-Hexane  | 0.529445  | −0.262603  | −1.00295  | −0.00765227  | 2.76425E-5  | 257.841
C7H16 | n-Heptane  | 0.656480  | −0.0643520  | −0.964719  | 0.0485736  | 2.33140E-5  | 254.303
C8H18 | n-Octane  | 0.503808  | −0.114929  | −1.29910  | 0.0479385  | 3.88652E-5  | 256.174
C9H20 | n-Nonane  | 0.599863  | −0.0625962  | −1.40430  | 0.0220808  | 4.08108E-5  |
C10H22 | n-Decane  | 0.396401  | −0.345116  | −1.73836  | −0.178929  | 6.85603E-5  | 257.928
FF5 for n-alkanes using PRSV EOS  | Name  | Bh1 | Bh2 | Ba1 | Ba2 | Bh22 | ηc

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Formula  |  | μP/bar | μP/bar | μP/bar | μP/bar | μP/bar2 | μP
CH4 | Methane  | 0.0978603  | −0.0947431  | −0.347478  | 0.060992  | 1.09269E-5  | 152.930
C2H6 | Ethane  | 0.126032  | −0.180542  | −0.54886  | 0.033303  | 9.64845E-6  | 217.562
C3H8 | Propane  | 0.245709  | −0.164913  | −0.630638  | 0.0339251  | 1.13654E-5  | 249.734
C4H10 | n-Butane  | 0.478611  | −0.0819001  | −0.495743  | 0.0652985  | 1.07941E-5  | 257.682
C5H12 | n-Pentane  | 0.439938  | −0.232544  | −0.753537  | 0.0584165  | 1.82595E-5  | 258.651
C6H14 | n-Hexane  | 0.426605  | −0.335750  | −0.895709  | −0.00664088  | 2.69972E-5  | 257.841
C7H16 | n-Heptane  | 0.561799  | −0.137427  | −0.834083  | 0.0613722  | 2.33423E-5  | 254.303
C8H18 | n-Octane  | 0.406290  | −0.258599  | −1.14826  | 0.0283937  | 3.88084E-5  | 256.174
C9H20 | n-Nonane  | 0.484008  | −0.256690  | −1.24586  | −0.00934743  | 4.30254E-5  |
C10H22 | n-Decane  | 0.244111  | −0.760327  | −1.63800  | −0.311341  | 7.4966710E-5  | 257.928
FF7 for n-alkanes using PRSV EOS  | Name  | Bh0 | Bh1 | Bh2 | Ba0 | Ba1 | Ba2 | Bh22 | ηc

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Formula  |  | μP/bar | μP/bar | μP/bar | μP/bar | μP/bar | μP/bar | μP/bar2 | μP
CH4 | Methane  | 0.053816  | −0.124174  | 0.028406  | −0.430873  | −0.369093  | 0.116296  | 9.71321E-6  | 152.930
C2H6 | Ethane  | 0.210510  | 0.524279  | −0.226923  | −0.460617  | −0.010559  | −0.098116  | 6.97853E-6  | 217.562
C3H8 | Propane  | 0.275468  | 0.773038  | −0.191915  | −0.612507  | 0.020985  | −0.059749  | 8.98138E-6  | 249.734
C4H10 | n-Butane  | 0.024164  | 0.859899  | −0.828038  | −0.952995  | −0.327070  | −0.382722  | 3.02572E-5  | 257.682
C5H12 | n-Pentane  | 0.423099  | 0.519851  | −0.059803  | −0.765609  | −0.343983  | 0.095436  | 1.50614E-5  | 258.651
C6H14 | n-Hexane  | 0.375053  | 0.676194  | −0.153389  | −1.02588  | −0.121181  | −0.043562  | 2.04217E-5  | 257.841
C7H16 | n-Heptane  | 0.486876  | 0.357007  | −0.047235  | −0.962702  | −0.636737  | 0.035438  | 2.39889E-5  | 254.303
C8H18 | n-Octane  | 0.528242  | −0.272297  | 0.126597  | −1.08722  | −1.34905  | 0.209537  | 3.25271E-5  | 256.174
C9H20 | n-Nonane  |  |  |  |  |  |  |  |
C10H22 | n-Decane  | 1.36796  | −4.83660  | 1.35246  | −0.899394  | −4.82959  | 1.04980  | 4.49837E-5  | 257.928
C11H24 | n-Undecane  |  |  |  |  |  |  |  |
C12H26 | n-Dodecane  | 7.14537  | −18.9732  | 3.66800  | 4.49233  | −18.8211  | 3.36729  | 7.81348E-5  | 245.148
C13H28 | n-Tridecane  | 7.16560  | −15.4258  | 3.37122  | 6.20650  | −18.3811  | 3.35921  | 6.13474E-5  | 240.550
C14H30 | n-Tetradecane  | 19.1819  | −39.4083  | 7.32513  | 13.2010  | −33.8698  | 5.86977  | 8.23832E-5  | 232.314
C15H32 | n-Pentadecane  | 12.6811  | −31.3240  | 5.94936  | 8.42368  | −28.9591  | 5.08195  | 1.08073E-4  | 229.852
C16H34 | n-Hexadecane  | 20.0877  | −43.4274  | 7.11506  | 11.2682  | −35.3317  | 5.55183  | 1.55344E-4  | 217.100
C17H36 | n-Heptadecane  |  |  |  |  |  |  |  |
C18H38 | n-Octadecane  | 27.9413  | −61.8540  | 12.9142  | 17.5532  | −48.2830  | 9.13626  | 8.38258E-5  | 206.187
Bh32 using PR EOS  | Name  | Bh32 | ηc

|
|
|

Formula  |  | μP/bar3 | μP
C11H10 | 1-Methylnaphthalene  | 1.05763E-9  | 340.458
C13H28 | n-Tridecane  | 1.80168E-10  | 240.550
C16H34 | 2,2,4,4,6,8,8-Heptamethylnonane  | 2.14681E-7  | 580.515

### One-parameter friction force theory

The one-parameter version of the friction force theory (FF1 theory and FF1 model) was developed by Quiñones-Cisneros et al. (2000, 2001a, 2001b and Z 2001, 2004),[28][29][30][3][31] and its basic elements, using some well known cubic EOSs, are displayed below.

The first step is to define the reduced dense fluid (or frictional) viscosity for a pure (i.e. single component) fluid by dividing by the critical viscosity. The same goes for the dilute gas viscosity.

ηdfr=ηdfηcandη0r=η0ηc

The second step is to replace the attractive and repulsive pressure functions by reduced pressure functions. This will of course, affect the friction functions also. New friction functions are therefore introduced. They are called reduced friction functions, and they are of a more universal nature. The reduced frictional viscosity is

ηdfr=Kar(PaPc)+Khr(PhPc)+Kh2r(PhPc)2

Returning to the unreduced frictional viscosity and rephrasinge the formula, gives

ηdf=ηcKarPcPa+ηcKhrPcPh+ηcKh2rPc2Ph2

Critical viscosity is seldom measured and attempts to predict it by formulas are few. For a pure fluid, or component i in a fluid mixture, a formula from kinetic theory is often used to estimate critical viscosity.

ηci=KviDviwhereDvi=Mi1/2Tci1/2Vci−2/3

where Kvi is a constant, and critical molar volume Vci is assumed to be proportional to the collision cross section. The critical molar volume Vci is significantly more uncertain than the parameters Pci and Tci. To get rid of Vci, the critical compressibility factor Zci is often replaced by a universal average value. This gives

ηci=KpDpiwhereDpi=Mi1/2Pci2/3Tci−1/6

where Kp is a constant. Based on an average critical compressibility factor of Zc = 0.275 and measured critical viscosity values of 60 different molecule types, Uyehara and Watson (1944)[4] determined an average value of Kp to be

Kp=7.7⋅1.013252/3≈7.77

Zéberg-Mikkelsen (2001) proposed an empirical correlation for Vci, with parameters for n-alkanes, which is

Vci−1=A+B⋅PciRTci⟺Vci=RTciARTci+BPci

where Vci−1=ρnci=cci. From the above equation and the definition of the compressibility factor it follows that

Zci=PciARTci+BPci⟺ZciRTciPciVci=1

Zéberg-Mikkelsen (2001) also proposed an empirical correlation for ηci, with parameters for n-alkanes, which is

ηci=C⋅PciMiD

The unit equations for the two constitutive equations above by Zéberg-Mikkelsen (2001) are

[Pc]=barand[Vc]=[RTc/Pc]=cm3/moland[T]=Kand[ηc]=μP
Constants for n-alkanes  symbol  | value  | unit

|
|

A  | 0.000235751  | mol/cm3
B  | 3.42770  | 1
C  | 0.597556  | μP
D  | 0.601652  | 1

The next step is to split the formulas into formulas for well defined components (designated by subscript d) with respect critical viscosity and formulas for uncertain components (designated by subscript u) where critical viscosity is estimated using Dpi and the universal constant Kp which will be treated as a tuning parameter for the current mixture. The dense fluid viscosity (for fluid component i in a mixture) is then written as

ηdfi=ηdfdi+ηdfui=ηdfdi+KpuFui

The formulas from friction theory is then related to well defined and uncertain fluid components. The result is

ηdfdi=ηciKariPciPai+ηciKhriPciPhi+ηciKh2riPci2Phi2fori=1,…,m

Fui=DpiKariPciPai+DpiKhriPciPhi+DpiKh2riPci2Phi2fori=m+1,…,N

Dpi=Mi1/2Pci2/3Tci−1/6

However, in order to obtain the characteristic critical viscosity of the heavy pseudocomponents, the following modification of the Uyehara and Watson (1944) expression for the critical viscosity can be used. The frictional (or residual) viscosity is then written as

ηci=KpDpiwhereKp=7.9483

The unit equations are [η]=[ηc]=μP and [P]=[Pc]=bar and [T]=[Tc]=K.

#### Reduced friction functions

Kqri=Bqrc+Bqr00(Γi−1)+∑m=12∑n=0mBqrmnψin[exp⁡(mΓi−m)−1]whereq=a,h

Kh2ri=Bh2rc+Bh2r21ψi[exp⁡(2Γi)−1](Γi−1)2

ψi=RTciPciandΓi=TciT

The unit equation of ψi is [ψi]=cm3/mol.

The 1-parameter model have been developed based on single component fluids in the series from methane to n-octadecane (C1H4 to C18H38). The empirical parameters in the reduced friction functions above are treated as universal constants, and they are listed in the following table. For convenience are critical viscosities included in the tables for models with 5- and 7-parameters that was presented further up.

Universal constants in FF1  symbol  | SRK  | PR  | PRSV

|
|
|

Barc | −0.165302  | −0.140464  | −0.140464
Bhrc | 0.00699574  | 0.0119902  | 0.0119902
Bh2rc | 0.00126358  | 0.000855115  | 0.000855115
|  |  |
Bar00 | −0.114804  | −0.0489197  | 0.0261033
Bar10 | 0.246622  | 0.270572  | 0.194487
Bar11 | −1.15648E-4  | −1.10473E-4  | −1.00432E-4
Bar20 | −0.0394638  | −0.0448111  | −0.0401761
Bar21 | 4.18863E-5  | 4.08972E-5  | 3.94113E-5
Bar22 | −5.91999E-9  | −5.79765E-9  | −5.91258E-9
Bhr00 | −0.315903  | −0.357875  | −0.325026
Bhr10 | 0.566713  | 0.637572  | 0.586974
Bhr11 | −1.00860E-4  | −6.02128E-5  | −3.70512E-5
Bhr20 | −0.0729995  | −0.079024  | −0.0764774
Bhr21 | 5.17459E-5  | 3.72408E-5  | 3.38714E-5
Bhr22 | −5.68708E-9  | −5.65610E-9  | −6.32233E-9
Bh2r21 | 1.35994E-8  | 1.37290E-8  | 1.43698E-8

#### Mixture

The mixture viscosity is given by

ηmix=ηdmix+ηumix=ηdmix+KpuFumix

The mixture viscosity of well defined components is given by

ηdmix=η0dmix+KadmixPamix+KhdmixPhmix+Kh2dmixPhmix2+Kh3dmixPhmix3

The mixture viscosity function of uncertain components is given by

Fumix=η0umix+KaumixPamix+KhumixPhmix+Kh2umixPhmix2+Kh3umixPhmix3

The mixture viscosity can be tuned to measured viscosity data by optimizing (regressing) the parameter Kpu.

where the mixture friction coefficients are obtained by eq(I.7.45) through eq(I.7.47) and Pa and Ph are the attractive and repulsive pressure term of the mixture.

#### Mixing rules

The mixing rules for the well defined components are

ln⁡(η0dmix)=∑i=1mziln⁡(η0i)orη0mix=∏i=1mη0izi

Kqrdmix=∑i=1mWiηciKqriPciwhereq=a,h

Kqprdmix=∑i=1mWiηciKqrpiPcipwhereq=a,handp=2,3

QZS recommends to drop the dilute gas term for the uncertain fluid components which are usually the heavier (hydrocarbon) components. The formula is kept here for consistency. The mixing rules for the uncertain components are

ln⁡(η0umix)=∑i=m+1Nziln⁡(η0i)orη0mix=∏i=m+1Nη0izi

Kqrumix=∑i=m+1NWiDpiKqriPciwhereq=a,h

Kqprumix=∑i=m+1NWiDpiKqpriPcipwhereq=a,handp=2,3

ε=0.30when SRK, PR or PRSV EOS is used

#### Dilute gas limit

Zéberg-Mikkelsen (2001)[3] proposed an empirical model for dilute gas viscosity of fairly spherical molecules as follows

η0=dg1T+dg2Tdg3

η0=Dg1Tr+Dg2TrDg3

Dg1=dg1⋅TcandDg2=dg2⋅Tcdg3andDg3=dg3

The unit equations for viscosity and temperature are

[η0]=μPand[T]=K

The second term is a correction term for high temperatures. Note that most dg2 parameters are negative.

Parameters for light gas viscosity using PR EOS  chemical  | name  | dg1 | dg2 | dg3

|
|
|
|

formula  |  | μP/K0.5 | μP/Kdg3 | 1
Ar  | Argon  | 28.2638  | −80.5002  | 0.206762
He  | Helium  | 3.65477  | 1.80913  | 0.758601
H2 | Hydrogen  | −1.55199  | 2.92788  | 0.645731
Kr  | Krypton  | 37.0292  | −101.369  | 0.232700
CH2 | Methane  | 13.3919  | −47.9429  | 0.160913
Ne  | Neon  | 36.6876  | −49.5702  | 0.325255
N2 | Nitrogen  | 19.1275  | −53.0591  | 0.184743
O2 | Oxygen  | 23.7298  | −67.7604  | 0.192271

#### Light gases

Zéberg-Mikkelsen (2001) proposed a FF-model for light gas viscosity as follows

ηlg=η0+KaPa+KhPh+Kh2Ph2

The friction functions for light gases are simple

Ka=Ba0

Kh=Bh0

Kh2=Bh20Tr2

The FF-model for light gas is valid for low, normal, critical and super critical conditions for these gases. Although the FF-model for viscosity of dilute gas is recommended, any accurate viscosity model for dilute gas can also be used with good results.

The unit equations for viscosity and temperature are

[ηlg]=μPand[T]=K
Parameters for light gas viscosity using PR EOS  chemical  | name  | Ba0 | Bh0 | Bh20

|
|
|
|

formula  |  | μP/bar | μP/bar | μP/bar2
Ar  | Argon  | −0.727451  | 0.102756  | 1.50831E-4
He  | Helium  | −0.507319  | −0.0427035  | 2.72888E-2
H2 | Hydrogen  | −0.332575  | −0.00185308  | 1.35146E-4
Kr  | Krypton  | −0.941704  | 0.152164  | 1.43747E-4
CH2 | Methane  | −0.382909  | 0.0731796  | 6.63615E-5
Ne  | Neon  | −0.794717  | 0.0517444  | 7.44634E-4
N2 | Nitrogen  | −0.675406  | 0.0806720  | 2.81086E-4
O2 | Oxygen  | −0.643424  | 0.0633893  | 1.17249E-4
Parameters for light gas viscosity using SRK EOS  chemical  | name  | Ba0 | Bh0 | Bh20

|
|
|
|

formula  |  | μP/bar | μP/bar | μP/bar2
Ar  | Argon  | −0.835290  | 0.115788  | 1.78345E-4
He  | Helium  | −0.831727  | −0.0367788  | 2.64680E-2
H2 | Hydrogen  | −0.436199  | 0.00256407  | 2.29206E-4
Kr  | Krypton  | −0.992414  | 0.173573  | 2.36628E-4
CH2 | Methane  | −0.422054  | 0.0803060  | 9.48629E-5
Ne  | Neon  | −0.846085  | 0.0606315  | 1.00209E-3
N2 | Nitrogen  | −0.760370  | 0.0901145  | 3.50877E-4
O2 | Oxygen  | −0.714059  | 0.0724354  | 1.57748E-4
Parameters for light gas viscosity using PRSV EOS  chemical  | name  | Ba0 | Bh0 | Bh20

|
|
|
|

formula  |  | μP/bar | μP/bar | μP/bar2
Ar  | Argon  | −0.761658  | 0.0652867  | 1.67369E-4
He  | Helium  | −1.14514  | −0.0213745  | 1.48013E-2
H2 | Hydrogen  | −0.33798  | −0.00260014  | 1.38423E-4
Kr  | Krypton  | −0.957231  | 0.122511  | 1.58880E-4
CH2 | Methane  | −0.39996  | 0.0542854  | 7.52500E-5
Ne  | Neon  | −0.784327  | 0.0378022  | 7.95184E-4
N2 | Nitrogen  | −0.684294  | 0.0498357  | 3.03099E-4
O2 | Oxygen  | −0.662772  | 0.0378931  | 1.26928E-4
Parameters for light gas viscosity using SRKM EOS  chemical  | name  | Ba0 | Bh0 | Bh20

|
|
|
|

formula  |  | μP/bar | μP/bar | μP/bar2
Ar  | Argon  | −0.877401  | 0.0683988  | 2.03442E-4
He  | Helium  | −1.34900  | −0.0202833  | 1.83984E-2
H2 | Hydrogen  | −0.400596  | −0.00136468  | 2.22197E-4
Kr  | Krypton  | −1.01227  | 0.136152  | 2.56269E-4
CH2 | Methane  | −0.444138  | 0.056294  | 1.07892E-4
Ne  | Neon  | −0.825002  | 0.0431686  | 1.08049E-3
N2 | Nitrogen  | −0.765597  | 0.0540651  | 3.80282E-4
O2 | Oxygen  | −0.735723  | 0.0422321  | 1.71242E-4

## Transition state analogy

This article started with viscosity for mixtures by displaying equations for dilute gas based on elementary kinetic theory, hard core (kinetic) theory and proceeded to selected theories (and models) that aimed at modeling viscosity for dense gases, dense fluids and supercritical fluids. Many or most of these theories where based on a philosophy of how gases behaves with molecules flying around, colliding with other molecules and exchanging (linear) momentum and thus creating viscosity. When the fluid became liquid, the models started to deviate from measurements because a small error in the calculated molar volume from the EOS is related to a large change in pressure and vica versa, and thus also in viscosity. The article has now come to the other end where theories (or models) are based on a philosophy of how a liquid behaves and give rise to viscosity. Since molecules in a liquid are much closer to each other, one may wonder how often a molecule in one sliding fluid surface finds a free volume in the neighboring sliding surface that is big enough for the molecule to jump into it. This may be rephrased as: when do a molecule have enough energy in its fluctuating movements to squeeze into a small open volume in the neighboring sliding surface, similar to a molecule that collides with another molecule and locks into it in a chemical reaction, and thus creates a new compound, as modeled in the transition state theory (TS theory and TS model).

### Free volume theory

The free volume theory (short FV theory and FV model) originates from Doolittle (1951)[33] who proposed that viscosity is related to the free volume fraction fν in a way that is analogous to the Arrhenius equation. The viscosity model of Doolittle (1951) is

η=Aexp⁡[Bfν]wherefν=V−bb

where V is the molar volume and b is the molar hard core volume.

There where, however, little activity on the FV theory until Allal et al. (1996, 2001a)[34] [35] proposed a relation between the free volume fraction and parameters (and/or variables) at the molecular level of the fluid (also called the microstructure of the fluid). The 1996-model became the start of a period with high research activity where different models were put forward. The surviving model was presented by Allal et al. (2001b),[36] and this model will be displayed below.

The viscosity model is composed of a dilute gas contribution η0 (or ηdg ) and a dense-fluid contribution ηdf (or dense-state contribution ηds or Δη).

η=η0+ηdf

Allal et al. (2001b)[36] showed that the dense-fluid contribution to viscosity can be related to the friction coefficient ζ of the sliding fluid surface, and Dulliens (1963)[37] has shown that the self-diffusion coefficient D is related to the friction coefficient of an internal fluid surface. These two relations are shown here:

ηdf=ρNALp2ζMandD=kBTζ

By eliminating the friction coefficient ζ, Boned et al. (2004)[38] expressed the characteristic length Lp as

Lp2=DMηdfρNAkBT=DMηdfρRT

The right hand side corresponds to the so-called Dullien invariant which was derived by Dullien (1963, 1972).[37] [39] A result from this is that the characteristic length Lp is interpreted as the average momentum transfer distance to a molecule that will enter a free volume site and collide with a neighboring molecule.

The friction coefficient ζ is modeled by Allal et alios (2001b)[36] as

ζ=ζ0exp⁡[Bfν]andζ0=ENALd(M3RT)1/2

The free volume fraction is now related to the energy E by

fν=(RTE)3/2andE=E0+PVandE0=αρ
whereρ=MV

where E is the total energy a molecule must use in order to diffuse into a vacant volume, and PV is connected to the work (or energy) necessary to form or expand a vacant volume available for diffusion of a molecule. The energy E0 is the barrier energy that the molecule must overcome in order to diffuse, and it is modeled to be proportional to mass density in order to improve match of measured viscosity data. Note that the sensitive term V−b in the denominator of Doolittle's (1951) model has disappeared, making the viscosity model of Allal et alios (2001b) more robust to numerical calculations of liquid molar volume by an imperfect EOS. The pre-exponential factor A is now a function and becomes

A=Lcρ(αρ+PV)3MRTwhereLc=Lp2Ld

The viscosity model proposed by Allal et al.(2001b)[36] is thus

η=η0+Aexp⁡[B(αρ+PVRT)3/2]

A digression is that the self-diffusion coefficient of Boned et al. (2004)[38] becomes

D=RTLdαρ+PV3RTMexp⁡[−B(αρ+PVRT)3/2]

Local nomenclature list:

* B parameter that characterizes the free volume overlap or empirical tuning parameter [1]
* b molar hard core volume [m3/mol]
* E total energy which the molecule must use in order to diffuse [J/mole]
* E0 barrier energy which the molecule must overcome in order to diffuse [J/mole]
* Lp average momentum transfer distance for a molecular that transfer linear momentum (conf. hard core radius) and/or angular momentum (conf. radius of gyration) [Å]
* Ld dissipation length to the energy E [Å]
* Lc composite parameter that is characteristic for viscosity [Å]
* M molar mass, conf. molecular weight [kg/mol]
* NA Avogadros constant
* P pressure [MPa]
* R gas constant R = 8.31451 [K·J/mol]
* V molar volume [m3/mol]
* α characteristic parameter or empirical tuning parameter [1]
* η viscosity [Pas]
* ρ mass density [kg/m3]
* ζ friction coefficient of a molecule related to the mobility of the molecule [1]
* ζ0 friction coefficient for zero mass density i.e. for a dilute system / low pressure limit [1]

#### Mixture

The mixture viscosity is

ηmix=η0mix+ηdfmix

The dilute gas viscosity η0 is taken from Chung et al.(1988)[40] which is displayed in the section on SS theory. The dense fluid contribution to viscosity in FV theory is

ηdfmix=Lcmixρeos(αmixρeos+PVeos)3RTMmixexp⁡[Bmix(αmixρeos+PVeosRT)3/2]

where α,B,Lc are three characteristic parameters of the fluid w.r.t. viscosity calculations. For fluid mixtures are these three parameters calculated using mixing rules. If the self-diffusion coefficient is included in the governing equations, probably via the diffusion equation, use of four characteristic parameters (i.e. use of Lp and Ld instead of Lc) will give a consistent flow model, but flow studies that involves the diffusion equation belongs a small class of special studies.

The unit for the viscosity is [Pas], when all other units are kept in SI units.

#### Mixing rules

At the end of the intensive research period Allal et al. (2001c)[41] and Canet (2001)[42] proposed two different set of mixing rules, and according to Almasi (2015)[43] there has been no agreement in the literature about which are the best mixing rules. Almasi (2015) therefore recommended the classic linear mole weighted mixing rules which are displayed below for a mixture of N fluid components.

Mmix=Mn=∑i=1NziMi

αmix=∑i=1Nziαi

Bmix=∑i=1NziBi

Lcmix=∑i=1NziLci

The three characteristic viscosity parameters αi,Bi,Lci are usually established by optimizing the viscosity formula against measured viscosity data for pure fluids (i.e. single component fluids).

#### Trend functions

The three characteristic viscosity parameters α,B,Lc are usually established by optimizing the viscosity formula against measured viscosity data for pure fluids (i.e. single component fluids). Data for these parameters can then be stored in databases together with data for other chemical and physical material properties and information. This happens more often if use of the equation becomes widespread. Hydrocarbon molecules is a huge group of molecules that has several subgroups which itself contains molecules of the same basic structure, but with different lengths. The alkanes is the simplest of these groups. A material property of molecules in such a group normally shows up as a function when plotted against another material property. A mathematical function is then selected based physical/chemical knowledge, experience and intuition, and the empirical parameters (i.e. constants) in the function are determined by curve fitting. Such a function is called a trend or trend function, and the group of molecule types is called a homologous series. Llovell et al. (2013a, 2013b)[44] [45] proposed trend functions for the three FV parameters α,B,Lc for alkanes. Oliveira et al. (2014)[46] proposed trend functions for the FV parameters for fatty acid methyl esters (FAME) and fatty acid ethyl esters (FAEE), both including compounds with up to three unsaturated bonds, which are displayed below.

α=a0+a1M

B=b0+b1M+b2M2

Lc=c0+c1M

The molar mass M [g/mol] (or molecular mass / weight) associated with the parameters used in curve fitting process (where ai, bi, and ci are empirical parameters) corresponds to carbon numbers in the range 8-24 and 8-20 for FAME and FAEE respectively.

### Significant structure theory

Viscosity models based on significant structure theory, a designation originating from Eyring,[47] [48] (short SS theory and SS model) has in the first two decades of the 2000s evolved in a development relay. It starting with Macías-Salinas et al.(2003),[49] continued with a significant contribution from Cruz-Reyes et al.(2005),[50] followed by a third stage of development by Macías-Salinas et al.(2013),[51] whose model is displayed here. The SS theories have three basic assumptions:

* A liquid behaves similar to a solid in many aspects, e.g. a sensitive relation between molar volume (or mass density) and pressure; position and distance between molecules is like a quasi-lattice with "fluidized vacancies" of molecular size distributed randomly throughout the quazi-lattice. The vacancies are assumed to have molecular size and move freely throughout the quasi-lattise structure.
* The fluid viscosity is calculated from two components which is a gas-like and a solid-like contribution, and both contributions contain all molecule types occurring in the fluid phase. A molecule that jumps from one sliding surface to a vacant site in the neighboring surface, is said to display gas-like behavior. A molecule that remains on its site in the sliding surface for some time, is said to display solid-like behavior.
* Collisions between molecules from neighboring layers are equivalent to molecules jumping to vacant sites, and these events within viscosity modeling are analogous to chemical reactions between colliding molecules within TS theory.

The fraction of gas-like molecules Xgl and solid-like molecules Xsl are

Xgl=(V−Vs)/VandXsl=Vs/VandVs≈b

where V is the molar volume of the phase in question, Vs is the molar volume of solid-like molecules and b is the molar hard core volume. The viscosity of the fluid is a mixture of these two classes of molecules

η=Xglηgl+Xslηsl

#### Gas-like contribution

The gas-like viscosity contribution is taken from the viscosity model of Chung et al.(1984, 1988),[52][5] which is based on the Chapman–Enskog(1964) kinetic theory of viscosity for dilute gases and the empirical expression of Neufeld et al.(1972)[6] for the reduced collision integral, but expanded empirical to handle polyatomic, polar and hydrogen bonding fluids over a wide temperature range. The viscosity model of Chung et al.(1988) is

ηgl=40.785MT*Vc2/3Ω**Fcwith unit equation[ηgl]=μP

Ω*=1.16145(T*)0.14874+0.52487exp(0.7732T*)+2.16178exp(2.43787T*)−6.435×10−4(T*)0.14874*sin[18.0323(T*)0.7683−7.27371]

where

T*=1.2593*T/TcandFc=1−0.2756ω+0.059035μr4+κ

Local nomenclature list:

* Fc : factor for molecular shape and polarities of dilute gases [1]
* M : molar mass, conf. molecular weight [g/mol]
* T : temperature [K]
* Tc : critical temperature [K]
* Vc : molar critical volume [cm3/mol]
* ηgl : gas-like viscosity contribution [μP]
* κ : correction factor for hydrogen bonding effects [1]
* μr : reduced dipole moment [1]
* Ω* : reduced collision integral [1]
* ω : acentric factor [1]

#### Solid-like contribution

In the 2000s, the development of the solid-like viscosity contribution started with Macías-Salinas et al.(2003)[49] who used the Eyring equation in TS theory as an analogue to the solid-like viscosity contribution, and as a generalization of the first exponential liquid viscosity model proposed by Reynolds(1886).[53] The Eyring equation models irreversible chemical reactions at constant pressure, and the equation therefore uses Gibbs activation energy, ΔG‡, to model the transition state energy that the system uses to move matter (i.e. separate molecules) from the initial state to the final state (i.e. the new compound). In the Couette flow, the system moves matter from one sliding surface to another, due to fluctuating internal energy, and probably also due to pressure and the pressure gradient. Besides, the pressure effect on viscosity is somewhat different for systems in a medium pressure range than it is for systems in a very high pressure range. Cruz-Reyes et al.(2005)[50] uses Helmholtz energy (F = U-TS = G-PV) as potential in the exponential function. This gives

ηsl=A*exp[−ΔG‡−PVRT]

Cruz-Reyes et al.(2005)[50] states that the Gibbs activation energy is negative proportional to the internal energy of vaporization (and thus calculated at a point on the freezing curve), but Macías-Salinas et al.(2013)[51] changes that to be the residual internal energy, ΔUr, at the general pressure and temperature of the system. One could alternatively use the grand potential (Ω = U-TS-G = -PV, sometimes called Landau energy or potential) in the exponential function and argue that the Couette flow is not a homogeneous system, such that a term with the residual internal energy must be added. Both arguments gives the proposed solid-like contribution which is

ηsl=A*exp[−αΔUr−PVRT]=A*exp[−αΔUrRT+Z]

The pre-exponential factor A is taken as

A=RTV−b*1ν

The jumping frequency of a molecule that jumps from its initial position to a vacant site, ν, is made dependent on the number of vacancies, Xgl, and pressure in order to extend the applicability of ηsl to much wider ranges of temperature and pressure than a constant jumping frequency would do. The final jumping frequency model is

ν=Xgl−1*1012(ν0+ν1P)=VV−b*1012(ν0+ν1P)

A recurrent problem for viscosity models is the calculation of liquid molar volume for a given pressure using an EOS that is not perfect. This calls for introduction of some empirical parameters. Use of adjustable proportionality factors for both the residual internal energy and the Z-factor is a natural choice. The sensitivity of P versus V-b values for liquids makes it natural to introduce an empirical exponent (power) to the dimensionless Z-factor. The empirical power turns out to be very effective in the high pressure (high Z-factor) region. The solid-like viscosity contribution proposed by Macías-Salinas et al.(2013)[51] is then

ηsl=RTV*11012(ν0+ν1P)*exp[−αΔUrRT]*exp[β0Zβ1]

Local nomenclature list:

* b : molar hard core volume of the fluid phase [cm3/mol]
* P : pressure [bar]
* T : temperature [K]
* V : molar volume of the fluid phase [cm3/mol]
* Xjl : volume fraction of the j-like contribution j=g,s [1]
* Z : compressibility factor (Z-factor) [1]
* α : proportionality factor [1]
* βi : adjustable parameters i=0,1 [1]
* η : viscosity of the fluid phase [μPa·s]
* ηsl : solid-like viscosity contribution [μPa·s]
* νi : adjustable parameters i=0,1 [s−1] and [bar−1s−1]
* ΔG≠ : activation energy of the fluid [J/mol]
* ΔUr : residual internal energy of the fluid [J/mol]

#### Mixture

ηmix=Vmix−bmixVmix*ηglmix+bmixVmix*ηslmix

ηglmix=F(Tcmix,Mcmix,Vcmix,ωmix,μrmix;T)

ηslmix=F(Vmix,ΔUmixr,Zmix;P,T)

In order to clarify the mathematical statements above, the solid-like contribution for a fluid mixture is displayed in more details below.

ηslmix=RTVmix*11012(ν0+ν1P)*exp[−αΔUmixrRT]*exp[β0Zmixβ1]

#### Mixing rules

The variables Vmix,ΔUmixr,Zmix and all EOS parameters for a fluid mixture are taken from the EOS (conf. W) and the mixing rules used by the EOS (conf. Q). More details on this is displayed below.

A fluid of n mole in the single phase region where the total fluid composition is 𝐳 [molefractions]:

Qmix=Qeos(𝐳)andWmix=Weos(P,T,𝐳)

Gas phase of ng mole in two-phase region where the gas composition is 𝐲 [molefractions]:

Qmix=Qeos(𝐲)andWmix=Weos(P,T,𝐲)

Liquid phase of nl mole in two-phase region where the liquid composition is 𝐱 [molefractions]:

Qmix=Qeos(𝐱)andWmix=Weos(P,T,𝐱)

where

n=nl+ngandnzi=nlxi+ngyiandi=1,…,N

Q=Tc,M,Vc,ω,bandW=V,ΔUr,Z

Since nearly all input to this viscosity model is provided by the EOS and the equilibrium calculations, this SS model (or TS model) for viscosity should be very simple to use for fluid mixtures. The viscosity model also have some empirical parameters that can be used as tuning parameters to compensate for imperfect EOS models and secure high accuracy also for fluid mixtures.

## See also

* Collision theory
* Compressibility factor
* Concentration
* Conversion of units
* Curve fitting
* Dortmund Data Bank
* Ideal gas
* Ideal gas law
* Kinetic theory of gases
* List of thermodynamic properties
* Molar volume
* PSRK
* Real gas
* Real gas law
* Statistical mechanics
* Statistical physics
* Table of thermodynamic equations
* Transport phenomena
* Trend estimation
* VTPR

## References

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2. ↑ 2.0 2.1 2.2 2.3 2.4 Pedersen, K. S.; Fredenslund, Aa.; Thomassen, P. (1989). Properties of Oils and Natural Gases. 1989. Gulf Publishing Company, Houston. pp. 1–252. ISBN 9780872015883.
3. ↑ 3.00 3.01 3.02 3.03 3.04 3.05 3.06 3.07 3.08 3.09 3.10 3.11 3.12 3.13 Zéberg-Mikkelsen, C.K. (2001). "Viscosity study of hydrocarbon fluids at reservoir conditions - modeling and measurements". Ph.D. Thesis at the Technical University of Denmark. Department of Chemical Engineering June (2001): 1–271. ISBN 9788790142742.
4. ↑ 4.0 4.1 4.2 4.3 Uyehara, O. A.; Watson, K.M. (1944). "A Universal Viscosity Correlation". National Petroleum News 39 (October): R-714 - R-722.
5. ↑ 5.0 5.1 Chung, T.-H.; Ajlan, M.; Lee, L.L.; Starling, K.E. (1988). "Generalized Multiparameter Correlation for Nonpolar and Polar Fluid Transport Properties". Ind. Eng. Chem. Res. 27 (4): 671–679. doi:10.1021/ie00076a024.
6. ↑ 6.0 6.1 Neufeld, P.D.; Janzen, A.R.; Aziz, R.A. (1972). "Empirical Equations to Calculate 16 of the Transport Collision Integrals Ω (l,s)* for the Lennard-Jones (12-6) Potential". Journal of Chemical Physics 57 (3): 1100–1102. doi:10.1063/1.1678363. Bibcode: 1972JChPh..57.1100N.
7. ↑ Wilke, C.R. (1950). "A Viscosity Equation for Gas Mixtures". The Journal of Chemical Physics 18 (1950): 517–519. doi:10.1063/1.1747673. Bibcode: 1950JChPh..18..517W.
8. ↑ 8.0 8.1 Herning, F.; Zipperer, L. (1936). "German: Beitrag zur Berechnung der Zähigkeit Technischer Gasgemische aus den Zähigkeitswerten der Einzelbestandteile; English: Calculation of the Viscosity of Technical Gas Mixtures from Viscosity of the individual Gases". Das Gas- und Wasserfach 79 (1936): 49–54 and 69–73.
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12. ↑ Glasstone, S.; Laidler, K.J.; Eyring, H. (1941). The Theory of Rate Processes, the Kinetics of Chemical Reactions, Viscosity, Diffusion, and Electrochemical Phenomena. McGraw Hill, New York..
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15. ↑ Lohrenz, J.; Bray, B. G.; Clark, C. R. (1964). "Calculating Viscosities of Reservoir Fluids from Their Compositions". Journal of Petroleum Technology October (1964): 1171–1176. doi:10.2118/915-PA.
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19. ↑ Tham, M. J.; Gubbins, K.E. (1970). "Correspondence Principle for Transport Properties of Dense Fluids, Nonpolar Polyatomic Fluids". Ind. Eng. Chem. Fundam. 9 (1975): 63–70. doi:10.1021/i160033a010.
20. ↑ Benedict, W.; Webb, G.B.; Rubin, L.C. (1940). "An Empirical Equation for Thermodynamic Properties of Light Hydrocarbons and their Mixtures. I. Methane, Ethane. Propane, and Butane". J. Chem. Phys. 8 (4): 334–345. doi:10.1063/1.1750658. Bibcode: 1940JChPh...8..334B.
21. ↑ McCarty, R.D. (1974). "A Modified Benedict-Webb-Rubin Equation of State for Methane Using Recent Experimental Data". Cryogenics 14 (5): 276–280. doi:10.1016/0011-2275(74)90228-8. Bibcode: 1974Cryo...14..276M.
22. ↑ Hanley, H.J.M.; McCarty, R.D.; Haynes, W.M. (1975). "Equation for the Viscosity and Thermal Conductivity Coefficients of Methane". Cryogenics 15 (1975): 413–417. doi:10.1016/0011-2275(75)90010-7. Bibcode: 1975Cryo...15..413H.
23. ↑ Phillips, P. (1912). "The Viscosity of Carbon Dioxide". Proceedings of the Royal Society of London 87A (1912): 48–61. doi:10.1098/rspa.1912.0058. ISSN 0950-1207. Bibcode: 1912RSPSA..87...48P.
24. ↑ Little, J.E.; Kennedy, H.T. (1968). "A Correlation of the Viscosity of Hydrocarbon Systems with Pressure, Temperature and Composition". Society of Petroleum Engineers Journal 8 June (2): 157–162. doi:10.2118/1589-PA.
25. ↑ Guo, X.-Q.; Wang, L.-S.; Rong, S.-X.; Guo, T.-M. (1968). "Viscosity Model Based on Equations of State for Hydrocarbon Liquids and Gases". Society of Petroleum Engineers Journal 139 (1997): 405–421. doi:10.1016/S0378-3812(97)00156-8.
26. ↑ Patel, N.C.; Teja, A.S. (1982). "A New Cubic Equation of State for Fluids and Fluid Mixtures". Chemical Engineering Science 37 (1982): 463–473. doi:10.1016/0009-2509(82)80099-7. Bibcode: 1982ChEnS..37..463P.
27. ↑ Guo, X.-Q. (2001). "Private Communications with C.K. Zéberg-Mikkelsen". Ph.D. Thesis at the Technical University of Denmark. Department of Chemical Engineering June (2001): 1–271. ISBN 9788790142742.
28. ↑ 28.0 28.1 Quiñones-Cisneros, S.E.; Zéberg-Mikkelsen, C.K.; Stenby, E.H. (2000). "The Friction Theory (f-theory) for Viscosity Modeling". Fluid Phase Equilibria 169 (2000): 249–276. doi:10.1016/S0378-3812(00)00310-1.
29. ↑ 29.0 29.1 Quiñones-Cisneros, S.E.; Zéberg-Mikkelsen, C.K.; Stenby, E.H. (2001a). "One Parameter Friction Theory Models for Viscosity". Fluid Phase Equilibria 178 (2001a): 1–16. doi:10.1016/S0378-3812(00)00474-X.
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32. ↑ Quiñones-Cisneros, S.E.; Deiters, U.K. (2006). "Generalization of the friction theory for viscosity modeling". The Journal of Physical Chemistry B 110 (25): 12820–12834. doi:10.1021/jp0618577. PMID 16800618.
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34. ↑ Allal, A.; Montford, J.P.; Marin, G. (1996). "Molecular Rheology: Calculation of Viscoelastic Properties from the Microstructure of Polymers". Proceedings of the XIIth International Congress on Rheology, Edited by Ait Kadi A., Dealy J.M., James D.F., and Williams M.C. From Canadian Rheology Group 317. ISBN 9782980510908.
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36. ↑ 36.0 36.1 36.2 36.3 Allal, A.; Boned, C.; Baylaucq, A. (2001b). "Free-volume viscosity model for fluids in the dense and gaseous states". Phys. Rev. E 64 (1): 1203–. doi:10.1103/PhysRevE.64.011203. PMID 11461236. Bibcode: 2001PhRvE..64a1203A.
37. ↑ 37.0 37.1 Dullien, F.A.L. (1963). "New relationship between viscosity and the diffusion coefficients based on Lamm's theory of diffusion". Trans. Faraday Soc. 59: 856–868. doi:10.1039/TF9635900856.
38. ↑ 38.0 38.1 Boned, C.; Allal, A.; Baylaucq, A.; Zéberg-Mikkelsen, C.K.; Bessieres, D.; Quiñones-Cisneros, S.E. (2004). "Simultaneous free-volume modeling of the self-diffusion coefficient and dynamic viscosity at high pressure". Phys. Rev. E 69 (3): 1–6. doi:10.1103/PhysRevE.69.031203. PMID 15089276. Bibcode: 2004PhRvE..69c1203B. http://orbit.dtu.dk/files/4885724/Boned.pdf.
39. ↑ Dullien, F.A.L. (1972). "Predictive equations for self-diffusion in liquids: A different approach". AIChE J. 18 (1): 62–70. doi:10.1002/aic.690180113.
40. ↑ Chung1988
41. ↑ Allal, A.; Boned, C.; Daugé, P. (2001c). "A New Free Volume Model for Dynamic Viscosity of Dense Fluids Versus Pressure and Temperature. Extension to a Predictive Model for Not Very Associative Mixtures". Physics and Chemistry of Liquids 39 (5): 607–624. doi:10.1080/00319100108030681.
42. ↑ Canet, X. (2001). "Viscosité Dynamique et Masse Volumique sous Hautes Pressions de Mélanges Binaires et Ternaires d'Hydrocarbures Lourds et Légers". Thèse de Doctorant, Université de Pau, Pau, France.
43. ↑ Almasi, M. (2015). "Temperature dependence and chain length effect on density and viscosity of binary mixtures of nitrobenzene and 2-alcohols". Journal of Molecular Liquids 209: 346–351. doi:10.1016/j.molliq.2015.05.045.
44. ↑ Llovell, F.; Marcos, R.M.; Vega, L.F. (2013a). "Free-volume theory coupled with soft-SAFT for viscosity calculations: comparison with molecular simulation and experiment data". J. Phys. Chem. B 117 (27): 8159–8171. doi:10.1021/jp401307t. PMID 23789584.
45. ↑ Llovell, F.; Marcos, R.M.; Vega, L.F. (2013b). "Transport properties of mixtures by the soft-SAFT + free-volume theory: application to mixtures of n-alkanes and hydrofluorocarbons". J. Phys. Chem. B 117 (17): 5195–5205. doi:10.1021/jp401754r. PMID 23566079.
46. ↑ Oliveira, M.B.; Freitas, S.V.D.; Llovell, F.; Vega, L.F.; Coutinho, J.A.P. (2014). "Development of simple and transferable molecular models for biodiesel production with the soft-SAFT equation of state". Chemical Engineering Research and Design 92 (12): 2898–2911. doi:10.1016/j.cherd.2014.02.025.
47. ↑ Eyring, H.; Ree, T.; Hirai, N. (1958). "Significant Structures in the Liquid State". Proc. Natl. Acad. Sci. USA 44 (7): 683–691. doi:10.1073/pnas.44.7.683. PMID 16590259. Bibcode: 1958PNAS...44..683E.
48. ↑ Henderson, D. (2010). "Henry Eyring: Quantum Chemistry, Statistical Mechanics, Theory of Liquids, and Significant Structure Theory". Bull. Hist. Chem. 35 (2).
49. ↑ 49.0 49.1 Macías-Salinas, R.; Garcìa-Sánchez, F.; Hernàndez Garduza, O. (2003). "Viscosity Model for Pure Liquids Based on Eyring Theory and Cubic EoS". AIChE J. 49 (3): 799–804. doi:10.1002/aic.690490324.
50. ↑ 50.0 50.1 50.2 Cruz-Reyes, G.; Luna-Barcenas, G.; Alvarado, J.F.J.; Sánchez, I.C.; Macías-Salinas, R. (2005). "Simultaneous Correlation of Saturated Viscosities of Pure Gases and Liquids Using the Significant Structure Theory". Ind. Eng. Chem. Res. 44 (6): 1960–1966. doi:10.1021/ie049070v.
51. ↑ 51.0 51.1 51.2 Macías-Salinas, R.; Aquino-Olivos, M.A.; Garcìa-Sánchez, F. (2013). "Viscosity Modelling of Reservoir Fluids over Wide Temperature and Pressure Ranges". Chemical Engineering Transactions 32: 1573. doi:10.3303/CET1332263. ISBN 978-88-95608-23-5. ISSN 1974-9791.
52. ↑ Chung, T.-H.; Lee, L.L.; Starling, K.E. (1984). "Applications of Kinetic Gas Theories and Multiparameter Correlation for Prediction of Dilute Gas Viscosity and Thermal Conductivity". Industrial & Engineering Chemistry Fundamentals 23 (1): 8–13. doi:10.1021/i100013a002.
53. ↑ Reynolds, O. (1886). "On the Theory of Lubrication and Its Application to Mr. Beauchamp Tower's Experiments, Including an Experimental Determination of the Viscosity of Olive Oil". Phil. Trans. R. Soc. Lond. 177: 157–234. doi:10.1098/rstl.1886.0005.

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