# Redlich–Kwong equation of state

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In physics and thermodynamics, the Redlich–Kwong equation of state is an empirical, algebraic equation that relates temperature, pressure, and volume of gases. It is generally more accurate than the van der Waals equation and the ideal gas equation at temperatures above the critical temperature. It was formulated by Otto Redlich and Joseph Neng Shun Kwong in 1949.[1][2] It showed that a two-parameter, cubic equation of state could well reflect reality in many situations, standing alongside the much more complicated Beattie–Bridgeman model and Benedict–Webb–Rubin equation that were used at the time. The Redlich–Kwong equation has undergone many revisions and modifications, in order to either improve its accuracy in terms of predicting gas-phase properties of more compounds, as well as in better simulating conditions at lower temperatures, including vapor–liquid equilibria.

## Equation

The Redlich–Kwong equation is formulated as:[1]

$P = \frac{R\,T}{V_m-b} - \frac{a}{\sqrt{T}\; V_m\, (V_m+b)},$

where:

The constants are different depending on which gas is being analyzed. The constants can be calculated from the critical point data of the gas:[1]

$a = \frac{1}{9(\sqrt[3]{2}-1)}\, \frac{R^2\, {T_c}^{5/2}}{P_c} = 0.42748\, \frac{R^2\, {T_c}^{5/2}}{P_c},$
$b = \frac{\sqrt[3]{2}-1}{3}\, \frac{R\, T_c}{P_c} = 0.08664\, \frac{R\, T_c}{P_c},$

where:

• Tc is the temperature at the critical point, and
• Pc is the pressure at the critical point.

The Redlich–Kwong equation is adequate for calculation of gas phase properties when the ratio of the pressure to the critical pressure (reduced pressure) is less than about one-half of the ratio of the temperature to the critical temperature (reduced temperature):

$\frac{p}{p_c} < \frac{T}{2T_c}.$

The Redlich–Kwong equation can also be represented as an equation for the compressibility factor of a gas, as a function of temperature and pressure:[2]

$Z = \frac{P\, V_m}{R\, T} = \frac{1}{1-h}\ - \frac{A^2}{B} \frac{h}{1+h}$

where:

• $A^2 = \frac{a}{R^2\, T^{5/2}} = \frac{0.42748\, {T_c}^{5/2}}{P_c\, T^{5/2}}$
• $B = \frac{b}{R\, T} = \frac{0.08664\, T_c}{P_c\, T}$
• $h = \frac{B\, P}{Z} = \frac{b}{V_m}$

This equation only implicitly gives Z as a function of pressure and temperature, but is easily solved numerically, originally by graphical interpolation, or now, more easily by computer.

For all Redlich–Kwong gases:

$Z_c={1 \over 3}$

where:

• Zc is the compressibility factor at the critical point

From the Redlich–Kwong equation, the fugacity coefficient of a gas can be estimated:[2]

$\ln \phi = \int_0^P {\frac{Z - 1}{p} dP} = Z - 1 - \ln {(Z-B\, P)} - \frac{A^2}{B}\, \ln {(1+\frac{B\, P}{Z})}$

The Redlich–Kwong equation was developed with an intent to also be applicable to mixtures of gases. In a mixture, the b term, representing the volume of the molecules, is an average of the b values of the components, weighted by the mole fractions:

$b = \sum_i {x_i\, b_i}$, or
$B = \sum_i {x_i\, B_i}$

where:

• xi is the mole fraction of the ith component of the mixture,
• bi is the b value of the ith component of the mixture, and
• Bi is the B value of the ith component of the mixture

The constant representing the attractive forces, a, is not linear with respect to mole fraction, but rather depends on the square of the mole fractions. That is:

$a = \sum_i {\sum_j {x_i\, x_j\, a_{i\, j}}}$

where:

• ai j is the attractive term between a molecule of species i and species j,
• xi is the mole fraction of the ith component of the mixture, and
• xj is the mole fraction of the jth component of the mixture.

It is generally assumed that the attractive cross terms are the geometric average of the individual a terms, that is:

$a_{i\, j} = ({a_i\, a_j})^{1/2}$

In this case, the following equation for the attractive term is furnished:

$A = \sum_i {x_i\, A_i}$

where Ai is the A term for the i'th component of the mixture.

## History

The Van der Waals equation, formulated in 1873 by Johannes Diderik van der Waals, is generally regarded as the first somewhat realistic equation of state (beyond the ideal gas law):

$p = \frac{RT}{V_\mathrm{m}-b}-\frac{a}{V_\mathrm{m}^2}$

However, its modeling of real behavior is not sufficient for many applications, and by 1949, had fallen out of favor, with the Beattie–Bridgeman and Benedict–Webb–Rubin equations of state being used preferentially, both which contain more parameters than the Van der Waals equation.[3] The Redlich–Kwong equation was developed by Redlich and Kwong while they were both working for the Shell Development Company at Emeryville, California. Kwong had begun working at Shell in 1944, where he met Otto Redlich when he joined the group in 1945. The equation arose out of their work at Shell - they wanted an easy, algebraic way to relate the pressures, volumes, and temperatures of the gasses they were working with - mostly non-polar and slightly polar hydrocarbons (the Redlich–Kwong equation is less accurate for hydrogen-bonding gasses). It was presented jointly in Portland, Oregon at the Symposium on Thermodynamics and Molecular Structure of Solutions in 1948, as part of the 14th Meeting of the American Chemical Society.[4] The success of the Redlich–Kwong equation in modeling many real gasses accurately demonstrate that a cubic, two-parameter equation of state can give adequate results, if it is properly constructed. After they demonstrated the viability of such equations, many others created equations of similar form to try to improve on the results of Redlich and Kwong.

## Derivation

The equation is essentially empirical - the derivation is neither direct nor rigorous. The Redlich–Kwong equation is very similar to the Van der Waals equation, with only a slight modification being made to the attractive term, giving that term a temperature dependence. At high pressures, the volume of all gases approaches some finite volume, largely independent of temperature, that is related to the size of the gas molecules. This volume is reflected in the b in the equation. It is empirically true that this volume is about 0.26Vc (where Vc is the volume at the critical point). This approximation is quite good for many small, non-polar compounds – the value ranges between about 0.24Vc and 0.28Vc.[5] In order for the equation to provide a good approximation of volume at high pressures, it had to be constructed such that

$b = 0.26\ V_c$

The first term in the equation represents this high-pressure behavior.

The second term corrects for the attractive force of the molecules to each other. The functional form of a with respect to the critical temperature and pressure is empirically chosen to give the best fit at moderate pressures for most relatively non-polar gasses.[4]

## Modification

The Redlich–Kwong equation was designed largely to predict the properties of small, non-polar molecules in the vapor phase, which it generally does well. However, it has been subject to various attempts to refine and improve it. In 1975, Redlich himself published an equation of state adding a third parameter, in order to better model the behavior of both long-chained molecules, as well as more polar molecules. His 1975 equation was not so much a modification to the original equation as a re-inventing of a new equation of state, and was also formulated so as to take advantage of computer calculation, which was not available at the time the original equation was published.[5] Many others have offered competing equations of state, either modifications to the original equation, or equations quite different in form. It was recognized by the mid 1960s that to significantly improve the equation, the parameters, especially a, would need to become temperature dependent. As early as 1966, Barner noted that the Redlich–Kwong equation worked best for molecules with an acentric factor (ω) close to zero. He therefore proposed a modification to the attractive term:

$a = \alpha + \gamma\,T^{-1.5}$

where

• α is the attractive term in the original Redlich–Kwong equation
• γ is a parameter related to ω, with γ = 0 for ω = 0 [6]

It soon became desirable to obtain an equation that would also model well the Vapor–liquid equilibrium (VLE) properties of fluids, in addition to the vapor-phase properties.[3] Perhaps the best known application of the Redlich–Kwong equation was in calculating gas fugacities of hydrocarbon mixtures, which it does well, that was then used in the VLE model developed by Chao and Seader in 1961.[3][7] However, in order for the Redlich–Kwong equation to stand on its own in modeling vapor–liquid equilibria, more substantial modifications needed to be made. The most successful of these modifications is the Soave modification to the equation, proposed in 1972.[8] Soave's modification involved replacing the T1/2 power found in the denominator attractive term of the original equation with a more complicated temperature-dependent expression. He presented the equation as follows:

$P = \frac{R\,T}{V_m-b} - \frac{a\,\alpha}{V_m\left(V_m+b\right)}$

where

• $\alpha = \left(1 + \left(0.480 + 1.574\,\omega - 0.176\,\omega^2\right) \left(1-T_r^{\,0.5}\right)\right)^2$,
• Tr is the reduced temperature of the compound, and
• ω is the acentric factor

The Peng–Robinson equation of state further modified the Redlich–Kwong equation by modifying the attractive term, giving

$p=\frac{R\,T}{V_m-b} - \frac{a\,\alpha}{V_m\, (V_m + b) + b\, (V_m - b)}$

the parameters a, b, and α are slightly modified, with

$a = \frac{0.457235\,R^2\,T_c^2}{p_c}$
$b = \frac{0.077796\,R\,T_c}{p_c}$
$\alpha = \left(1 + \left(0.37464 + 1.54226\,\omega - 0.26992\,\omega^2\right) \left(1-T_r^{\,0.5}\right)\right)^2$ [9]

The Peng–Robinson equation typically gives similar VLE equilibria properties as the Soave modification, but often gives better estimations of the liquid phase density.[3]

Several modifications have been made that attempt to more accurately represent the first term, related to the molecular size. The first significant modification of the repulsive term beyond the Van der Waals equation's

$P_{hs}=\frac{R\, T}{V_m - b} = \frac{R\, T}{V_m}\, \frac{1}{1 - \frac{b}{V_m}}$

(where Phs represents a hard spheres equation of state term.) was developed in 1963 by Thiele:[10]

$P_{hs}= \frac{R\, T}{V_m}\, \frac{1 - \eta^3}{(1 - \eta)^4}$

where

$\eta = \frac{b}{4\, V_m}$, and

This expression was improved by Carnahan and Starling to give [11]

$P_{hs}= \frac{R\, T}{V_m}\, \frac{1 + \eta + \eta^2 - \eta^3}{(1 - \eta)^3}$

The Carnahan-Starling hard-sphere equation of state has term been used extensively in developing other equations of state,[3] and tends to give very good approximations for the repulsive term.[12]

Beyond improved two-parameter equations of state, a number of three parameter equations have been developed, often with the third parameter depending on either Zc, the compressibility factor at the critical point, or ω, the acentric factor. Schmidt and Wenzel proposed an equation of state with an attractive term that incorporates the acentric factor:[13]

$P = \frac{R\, T}{V_m - b} - \frac{a}{V_m^2 + (1 + 3\, \omega)\, b\, V_m - 3\, \omega\, b^2}$

This equation reduces to the original Redlich–Kwong equation in the case when ω = 0, and to the Peng–Robinson equation when ω = 1/3.

## References

1. ^ a b c Murdock, James W. (1993), Fundamental fluid mechanics for the practicing engineer, CRC Press, pp. 25–27, ISBN 0-8247-8808-7
2. ^ a b c Redlich, Otto; Kwong, J. N. S. (1949). "On The Thermodynamics of Solutions". Chem. Rev. 44 (1): 233–244. doi:10.1021/cr60137a013. PMID 18125401.
3. Tsonopoulos, C.; Heidman, J. L. (1985). "From Redlich–Kwong to the Present". Fluid Phase Equilibria 24: 1–23. doi:10.1016/0378-3812(85)87034-5.
4. ^ a b Reif-Acherman, Simón (2008). "Joseph Neng Shun Kwong: A Famous and Obscure Scientist". Quim. Nova. 31 (7): 1909–1911. doi:10.1590/S0100-40422008000700054.
5. ^ a b Redlich, Otto (1975). "On the Three-Parameter Representation of the Equation of State". Industrial & Engineering Chemistry Fundamentals 14 (3): 257–260. doi:10.1021/i160055a020. Retrieved 6 May 2012.
6. ^ Barner, H. E.; Pigford, R. L.; Schreiner, W. C. (1966). "A Modified Redlich–Kwong Equation of State". 31st Midyear Meeting, API Div Refining.
7. ^ Chao, K. C.; Seader, J. D. (1961). "A general correlation of vapor-liquid equilibria in hydrocarbon mixtures". AIChE Journal 7 (4): 598–605. doi:10.1002/aic.690070414. Retrieved 6 May 2012.
8. ^ Soave, Giorgio. "Equilibrium constants from a modified Redlich–Kwong equation of state". Chemical Engineering Science 27 (6): 1197–1203. doi:10.1016/0009-2509(72)80096-4. Retrieved 6 May 2012.
9. ^ Peng, Ding-Yu; Robinson, Donald (1985). "A New Two-Constant Equation of State". Industrial & Engineering Chemistry Fundamentals 15 (1): 59–64. doi:10.1021/i160057a011. Retrieved 6 May 2012.
10. ^ Thiele, Everett (1963). "Equation of State for Hard Spheres". Journal of Chemical Physics 39 (2): 474–479. Bibcode:1963JChPh..39..474T. doi:10.1063/1.1734272. Retrieved 6 May 2012.
11. ^ Carnahan, Norman; Starling, Kenneth (1969). "Equation of State for Nonattracting Rigid Spheres". Journal of Chemical Physics 51 (2): 635–636. Bibcode:1969JChPh..51..635C. doi:10.1063/1.1672048. Retrieved 6 May 2012.
12. ^ Song, Yuhua; Mason, E. A.; Stratt, Richard (1989). "Why does the Carnahan-Starling equation work so well?". The Journal of Physical Chemistry 93 (19): 6916–6919. doi:10.1021/j100356a008. Retrieved 6 May 2012.
13. ^ Schmidt, G.; Wenzel, H. (1980). "A modified van der Waals type equation of state". Chemical Engineering Science 35 (7): 1503–1512. doi:10.1016/0009-2509(80)80044-3. Retrieved 6 May 2012.