{"id":30,"date":"2006-09-01T20:04:23","date_gmt":"2006-09-02T01:04:23","guid":{"rendered":"http:\/\/www.jmcampbell.com\/tip-of-the-month\/?p=30"},"modified":"2011-06-13T14:05:17","modified_gmt":"2011-06-13T19:05:17","slug":"how-to-determine-k-values","status":"publish","type":"post","link":"http:\/\/www.jmcampbell.com\/tip-of-the-month\/2006\/09\/how-to-determine-k-values\/","title":{"rendered":"How to determine K-Values?"},"content":{"rendered":"

Modeling and design of many types of equipment for separating gas and liquids such as flash separators at the well head, distillation columns and even a pipeline are based on the phases present being in vapor-liquid equilibrium. The thermodynamic equilibrium between vapor and liquid phases is expressed in terms equality of fugacity of component i in the vapor phase, fi<\/sub>V<\/sup>, and the fugacity of component i in the liquid phase, fi<\/sub>L<\/sup>, is written as<\/p>\n

\"Equation<\/a><\/div>\n

Equation (1) is the foundation of vapor-liquid equilibrium calculations; however, we rarely use it in this form for practical applications. For calculation purposes, Eq. (1) is transformed to a more common expression which is<\/p>\n

\"Equation<\/a><\/div>\n

Ki is called the vapor\u2013liquid equilibrium ratio, or simply the K-value, and represents the ratio of the mole fraction in the vapor, yi, to the mole fraction in the liquid, xi. Equation (2) is also called “Henry\u2019s law” and K is referred to as Henry\u2019s constant.\u00a0For the more volatile components the Kvalues are greater than 1.0, whereas for the less volatile components they are less than 1.0.
\nDepending on the system under study, any one of several approaches may be used to determine K-values. Obviously, experimental measurement is the most desirable; however, it is expensive and time consuming. Alternatively, there are several graphical or numerical tools that are used for determination of K-values. This \u201cTip of the Month\u201d presents a history of many of those graphical methods and numerical techniques.<\/p>\n

In general K-values are function of the pressure, temperature, and composition of the vapor and liquid phases. The components making up the system plus temperature, pressure, composition, and degree of polarity affect the accuracy and applicability, and hence the selection, of an approach. The widely used approaches are K-value charts, Raoult\u2019s law, the equation of state (EoS) approach (f), activity coefficient approach (?) or combination of EoS and the EoS and ? approaches [1-5]. EoS approach requires use of a digital computer.<\/p>\n

K-Value Charts<\/strong><\/p>\n

There are several forms of K-value charts. One of the earliest K-value charts for light hydrocarbons is presented in reference [1]. In these charts, K-values for individual components are plotted as a function of temperature on the x-axis with pressure as a parameter. In each chart the pressure range is from 70 to 7000 kPa (10 to 1000 psia) and the temperature range is from 5 to 260 \u00baC (40 to 500 \u00baF).<\/p>\n

Early high pressure experimental work revealed that, if a hydrocarbon system of fixed overall composition were held at constant temperature and the pressure varied, the K-values of all components converged toward a common value of unity (1.0) at some high pressure. This pressure was termed the \u201cConvergence Pressure\u201d of the system and has been used to correlate the effect of composition on K-values, thus permitting generalized K-values to be presented in a moderate number of charts.<\/p>\n

In more recent publications [2], the K-values are plotted as a function of pressure on the x-axis with temperature and Convergence Pressure as parameters. In order to use these charts, one should determine the Convergence Pressure first. The determination of convergence Pressure is a trial-and-error procedure and can be found elsewhere [6].<\/p>\n

For computer use, later in 1958 these K-Value charts were curve fitted to the following equations by academic and industrial experts collaborating through the Natural Gas Association of America [7].<\/p>\n

\"Equation<\/a><\/div>\n

In Eq (3) T is temperature in \u00baR, P is pressure in psia and the fitted values of the bij coefficients are reported in an NGAA publication [7].
\nA relatively simple nomograph is normally presented in undergraduate thermodynamics and unit operations text books. In the nomograph, the K-values of light hydrocarbons, normally methane through n-decane, are plotted on one or two pages. Charts of this type do allow for an average effect of composition, but the essential basis is Raoult\u2019s law and equilibrium constants derived from them are useful only for teaching and academic purposes.<\/p>\n

Raoult\u2019s Law<\/strong><\/p>\n

Raoult\u2019s Law is based on the assumptions that the vapor phase behaves as an ideal gas and the liquid phase is an ideal solution. Under these conditions the fugacities are expressed as<\/p>\n

\"Equation<\/a><\/div>\n

The saturation pressure of a component is represented by Pi<\/sub>Sat <\/sup>and the pressure of the system is represented by P. Substituting from Eqs (4) and (5) in Eq (1) gives<\/p>\n

\"Equation<\/a><\/div>\n

The vapor pressure may be read from a Cox chart or calculated from a suitable equation in terms of temperature. A typical Cox chart may be found in reference [8]. The Antoine [5] equation is recommended for calculating vapor pressure:<\/p>\n

\"Equation<\/a><\/div>\n

Values of A, B, and C for several compounds are reported in the literature [5]. Complex vapor pressure equations such as presented by Wagner [5], even though more accurate, should be avoided because they can not be used to extrapolate to temperatures beyond the critical temperature of each component. Raoult\u2019s law is applicable to low pressure systems (up to about 50 psia or 0.35 MPa) or to systems whose components are very similar such as benzene and toluene. This method is simple but it suffers when the temperature of the system is above the critical temperature of one or more of the components in the mixture. At temperatures above the critical point of a component, one must extrapolate the vapor pressure which frequently results in erroneous K-values. In addition, this method ignores the fact that the K-values are composition dependent.
\n<\/strong><\/p>\n

Correlation Method<\/strong><\/p>\n

As mentioned earlier, determination of K-values from charts is inconvenient for computer calculations. Therefore, scientists and engineers have developed numerous curve fitted expressions for calculation of K-values. However, these correlations have limited application because they are specific to a certain system or applicable over a limited range of conditions. Some of these are polynomial or exponential equations in which K-values are expressed in terms of pressure and temperature. One of these correlations presented by Wilson [9], is:<\/p>\n

\"Equation<\/a><\/div>\n

where Tci, critical temperature, in \u00baR or K, Pci<\/sub>, critical pressure, in psi, kPa or bar, ?i<\/sub> is the acentric factor, P is the system pressure, in psi, kPa or bar, T is the system temperature, in \u00baR or K. (P and Pc, T and Tc must be in the same units.) This correlation is applicable to low and moderate pressure, up to about 3.5 MPa (500 psia), and the K-values are assumed to be independent of composition.<\/p>\n

EoS Approach<\/p>\n

The fugacity of each component is determined by an EoS. In other words, both phases are described by only one EoS. It is a powerful tool and relatively accurate if used appropriately. This approach is widely used in industry for light hydrocarbon and non polar systems. Under these conditions the fugacities are expressed by<\/p>\n

\"Equation<\/a><\/div>\n

The fugacity coefficients for each component in the vapor and liquid phases are represented by ?i<\/sub>V<\/sup> and ?i<\/sub>L<\/sup>
\n, respectively. Substitution of fugacities from Eqs (9) and (10) in Eq (1) gives<\/p>\n

\"Equation<\/a><\/div>\n

The EoS method has been programmed in the GCAP for Volumes 1 & 2 of Gas Conditioning and Processing Software to generate K-values using the SRK EoS [10].<\/p>\n

EoS-Activity Coefficient Approach<\/p>\n

The approach is based on an EoS which describes the vapor phase non-ideality through the fugacity coefficient and an activity coefficient model which accounts for the non-ideality of the liquid phase. This approach is widely used in industry for polar systems exhibiting highly non-ideal behavior. Under these conditions the fugacities are expressed by<\/p>\n

\"Equation<\/a><\/div>\n

The fugacity coefficients for each component in the vapor phase are represented by fi<\/sub>V<\/sup> . The saturation fugacity coefficient for a component in the system, fi<\/sub>Sat<\/sup> is calculated for pure component i at the temperature of the system but at the saturation pressure of that component. Normally, an EoS is used to calculate both fi<\/sub>V <\/sup>and fi<\/sub>Sat<\/sup> . Substitution of fugacities from Eqs (12) and (13) in Eq (1) gives<\/p>\n

\"Equation<\/a><\/div>\n

Activity coefficients are calculated by an activity coefficient model such as that of Wilson [11] or the NRTL (Non-Random Two Liquid) model [12]. In order to calculate K-values by equation 14, the mole fractions in both phases in addition to the pressure and temperature must be known. Normally not all of these variables are known. As is the case for the EoS approach, calculations are trial and error. This approach is applicable to polar systems such as water \u2013 ethanol mixtures from low to high pressures.<\/p>\n

Normally, for low pressures, we can assume that the vapor phase behaves like an ideal gas; therefore both ?i<\/sub>V<\/sup> and ?i<\/sub>Sat<\/sup> are set equal to 1.0. Under such circumstances, Eq (14) is reduced to<\/p>\n

\"Equation<\/a><\/div>\n

Eq (15) is applicable for low pressure non-ideal and polar systems. Assuming the liquid phase is an ideal solution, ? i becomes unity and Eq (15) is reduced further to a simple Raoult\u2019s law.<\/p>\n

The JMC K-Values<\/p>\n

Two sets of K-values are summarized in Appendices 5A and 5B at the end of Chapter 5 of Gas Conditioning and Processing, Vol. 1. Appendix 5A is a series of computer-generated charts using SRK EoS. The values shown are useful particularly for calculations of vapor liquid equilibrium wherein liquid being condensed from gas systems. Appendix 5B is based on the data obtained from field tests and correlations on oil-gas separators. The data set was based on over 300 values. This correlation has bee used for often for oil separation calculations.<\/p>\n

To learn more on applications of K-values and their impact on facilities calculation, design and surveillance, refer to JMC books [12-13] and enroll in our\u00a0G4 (Gas Conditioning and Processing)<\/a> and G5 (Gas Conditioning and Processing – Special)<\/a> courses.<\/p>\n

By Dr. Mahmood Moshfeghian<\/em><\/p>\n

Reference:<\/p>\n

    \n
  1. Natural Gasoline Supply Men\u2019s Association, 20th Annual Convention, April 23-25, 1941.<\/li>\n
  2. Engineering Data Book, 10th and 11th Editions, Gas Processors and Suppliers Association Data Book, Tulsa, Oklahoma, (1998).<\/li>\n
  3. Prausnitz, J. M.; R. N. Lichtenthaler, E. G. de Azevedo, \u201cMolecular Thermodynamics of Fluid Phase Equilibria,\u201d, 3rd Ed., Prentice Hall PTR, New Jersey, NY, 1999.<\/li>\n
  4. Maddox, R. N. and L. L. Lilly, \u201cGas conditioning and processing, Volume 3: Advanced Techniques and Applications,\u201d John M. Campbell and Company, Norman, Oklahoma, USA, 1994.<\/li>\n
  5. Reid, R. C.; J. M. Prausnitz, and B. E. Poling, \u201cThe properties of Gases and liquids,\u201d 4th Ed., McGraw Hill, New York, 1987.<\/li>\n
  6. Engineering Data Book, 7th Edition, Natural Gas Processors Suppliers Association, Tulsa, Oklahoma, 1957.<\/li>\n
  7. Equilibrium Ratio Data for Computers, Natural Gasoline Association of America, Tulsa, Oklahoma, (1958).<\/li>\n
  8. Natural Gasoline and the Volatile Hydrocarbons, Natural Gasoline Association of America, Tulsa, Oklahoma, (1948).<\/li>\n
  9. Wilson, G., \u201cA modified Redlich-Kwong equation of state applicable to general physical data calculations,\u201d Paper No15C, 65th AIChE National meeting, May, (1968).<\/li>\n
  10. G. Soave, Chem. Eng. Sci. 27, 1197-1203, 1972.<\/li>\n
  11. Wilson, G. M., J. Am. Chem. Soc. Vol 86, pp.127-120, 1964<\/li>\n
  12. Campbell, J. M. \u201cGas conditioning and processing, Volume 1: Fundamentals,\u201d John M. Campbell and Company, Norman, Oklahoma, USA, 2001.<\/li>\n
  13. Campbell, J. M., \u201cGas conditioning and processing, Volume 2: Equipment Modules,\u201d John M. Campbell and Company, Norman, Oklahoma, USA, 2001.<\/li>\n<\/ol>\n","protected":false},"excerpt":{"rendered":"

    Modeling and design of many types of equipment for separating gas and liquids such as flash separators at the well head, distillation columns and even a pipeline are based on the phases present being in vapor-liquid equilibrium. The thermodynamic equilibrium between vapor and liquid phases is expressed in terms equality of fugacity of component i […]<\/p>\n","protected":false},"author":23,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"nf_dc_page":"","_monsterinsights_skip_tracking":false,"_monsterinsights_sitenote_active":false,"_monsterinsights_sitenote_note":"","_monsterinsights_sitenote_category":0,"_jetpack_newsletter_access":"","_jetpack_dont_email_post_to_subs":false,"_jetpack_newsletter_tier_id":0,"_jetpack_memberships_contains_paywalled_content":false,"_jetpack_feature_clip_id":0,"_jetpack_memberships_contains_paid_content":false,"footnotes":"","jetpack_publicize_message":"","jetpack_publicize_feature_enabled":true,"jetpack_social_post_already_shared":false,"jetpack_social_options":{"image_generator_settings":{"template":"highway","default_image_id":0,"font":"","enabled":false},"version":2},"jetpack_post_was_ever_published":false},"categories":[3],"tags":[],"coauthors":[],"class_list":["post-30","post","type-post","status-publish","format-standard","hentry","category-gas-processing"],"jetpack_publicize_connections":[],"jetpack_featured_media_url":"","jetpack_shortlink":"https:\/\/wp.me\/p1pQc4-u","jetpack_sharing_enabled":true,"_links":{"self":[{"href":"http:\/\/www.jmcampbell.com\/tip-of-the-month\/wp-json\/wp\/v2\/posts\/30","targetHints":{"allow":["GET"]}}],"collection":[{"href":"http:\/\/www.jmcampbell.com\/tip-of-the-month\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"http:\/\/www.jmcampbell.com\/tip-of-the-month\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"http:\/\/www.jmcampbell.com\/tip-of-the-month\/wp-json\/wp\/v2\/users\/23"}],"replies":[{"embeddable":true,"href":"http:\/\/www.jmcampbell.com\/tip-of-the-month\/wp-json\/wp\/v2\/comments?post=30"}],"version-history":[{"count":3,"href":"http:\/\/www.jmcampbell.com\/tip-of-the-month\/wp-json\/wp\/v2\/posts\/30\/revisions"}],"predecessor-version":[{"id":1127,"href":"http:\/\/www.jmcampbell.com\/tip-of-the-month\/wp-json\/wp\/v2\/posts\/30\/revisions\/1127"}],"wp:attachment":[{"href":"http:\/\/www.jmcampbell.com\/tip-of-the-month\/wp-json\/wp\/v2\/media?parent=30"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"http:\/\/www.jmcampbell.com\/tip-of-the-month\/wp-json\/wp\/v2\/categories?post=30"},{"taxonomy":"post_tag","embeddable":true,"href":"http:\/\/www.jmcampbell.com\/tip-of-the-month\/wp-json\/wp\/v2\/tags?post=30"},{"taxonomy":"author","embeddable":true,"href":"http:\/\/www.jmcampbell.com\/tip-of-the-month\/wp-json\/wp\/v2\/coauthors?post=30"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}