Mutual Solubilities Of Hydrocarbons Research Articles

Estimation of water-hydrocarbon mutual solubility in gas processing operations using an intelligent model

ABSTRACTAn accurate prediction of the mutual solubilities of hydrocarbons and water is extremely useful in oil, gas, and chemical industries. Estimating the solubility of hydrocarbons in water is required to describe their phase distribution through the removal process and also in the design of separation equipment. The current study plays emphasis on applying the predictive model based on the least square support vector machine (LSSVM) to estimate mutual water-hydrocarbon solubility at a wide range of conditions. A genetic algorithm (GA) was employed to choose and optimize hyperparameters (γ and σ2), which are embedded in LSSVM model. Utilization of this model showed high competence of the applied model in terms of coefficient of determination (R2) of 0.9998 and 0.9994, Average absolute relative deviation (AARD) of 1.1378 and 1.12459 from experimental values for predicted water solubility in hydrocarbons and hydrocarbon solubility in water, correspondingly. Using this method is quite simple and accurate to determine the mutual water-hydrocarbon solubility with negligible uncertainty.

Mutual solubilities of hydrocarbons and water with the CPA EoS

The knowledge of hydrocarbon/water phase equilibria is important in the design and operation of equipment for petroleum transport and refining and petrochemical plants. The presence of water in a hydrocarbon mixture can affect the product quality and damage the operation equipment due to corrosion and formation of gas hydrates. Tracing the concentration of hydrocarbons in aqueous media is also important for technical purposes like preventing oil spills and for ecological concerns such as predicting the fate of these organic pollutants in the environment. In spite of its huge interest there was no model able for a qualitative description of the mutual solubility of water and hydrocarbons for a broad range of systems in a wide range of thermodynamic conditions. In this work it is shown that an equation of state incorporating association known as the CPA EoS is able to produce an excellent description of the mutual solubilities of water and several aliphatic and aromatic hydrocarbons in a broad range of pressures and temperatures.

Prediction of the mutual solubilities of hydrocarbons and water with COSMO-RS

A critical collection of data for the mutual solubilities of water and hydrocarbons (HC) recently presented by Tsonopoulos is used for careful analysis of the ability of a priori prediction method conductor-like screening model–real solvents (COSMO-RS) to predict the infinite dilution activity coefficients in such dissimilar systems. Although only few data of hydrocarbon–water mixtures had been used in the parameterization of COSMO-RS, the mutual solubilities of hydrocarbons ( n-alkanes, 1-alkenes, alkylbenzenes, and alkylcyclohexanes) and water are quite well predicted by COSMO-RS. All trends of the solubilities with respect to carbon number (CN) of the hydrocarbons are very well reproduced. Some moderate deviations are observed for the temperature dependence (solvation enthalpy) of hydrocarbon solubility in water, while the temperature dependence of the water solubility in various hydrocarbons is reproduced almost within the experimental error up to temperatures of about 473 K. The good qualitative and even satisfactory quantitative prediction of the solubilities of hydrocarbons in water proves that COSMO-RS correctly reflects the physics of the hydrophobic solvation, i.e. the fact that the largest part of the free energy of solution of hydrocarbons in water is of entropic nature due to the re-organization of the water molecules around non-polar compounds. This is especially unexpected, because the COSMO-RS method does not takes into account the 3D-geometry of solute–solvent arrangements. An explanation is given, how the physics of water re-organization around non-polar surface is nevertheless described by COSMO-RS. Some ideas for further improvement of COSMO-RS regarding the mutual solubilities of hydrocarbons and water are discussed.

Modeling of gas solubility in brine

Cubic equations of state (EOS) are widely used to represent the phase behavior of gas–oil-systems, whereas different types of models have traditionally been used to describe gas solubility in aqueous mixtures. Since formation water is often produced together with gas and oil, it is also desirable to model gas solubility in formation water using an EOS. It has previously been shown that the mutual solubility of hydrocarbons and pure water can be well represented by a cubic EOS by applying a non-classical mixing rule for the a-parameter. However, formation water produced together with gas and oil will often have a considerable content of salts, which must be accounted for in gas solubility calculations. It is shown that the mixing rule of Huron and Vidal can be stretched to account for the presence of the salts NaCl, KCl and CaCl 2 in the water phase. This is done by assigning hypothetical critical properties to the salts, and estimating interaction parameters for gas-salt interactions based on experimental gas solubility data. This model concept gives a fair representation of the gas solubility in salt water.

Mutual solubilities of hydrocarbons and water: III. 1‐hexene; 1‐octene; C10C12 hydrocarbons

AbstractThis article completes the analysis of high‐temperature mutual solubilities of hydrocarbons and water. Part I (Tsonopoulos and Wilson, 1983) presented benzene, cyclohexane, and n‐hexane, while Part II (Heidman et al., 1985) extended the investigation to ethylbenzene, ethylcyclohexane, and n‐octane. Part III presents experimental data up to the three‐phase critical end point for C6, C8, and C10 1‐alkenes, n‐decane, n‐butylcyclohexane, m‐diethylbenzene, p‐diisopropylbenzene, cis‐decalin, tetralin, 1‐methylnaphthalene, and 1‐ethylnaphthalene. The thermodynamic analysis of Henry's constants for hydrocarbons in water is extended to the critical temperature of water, while the solubility and volatility of water in hydrocarbons are successfully correlated with several modifications of the Redlich‐Kwong equation of state.

High‐temperature mutual solubilities of hydrocarbons and water. Part II: Ethylbenzene, ethylcyclohexane, and n‐octane

AbstractIn Part I (Tsonopoulos and Wilson, 1983), the mutual solubilities of three C6 hydrocarbons (benzene, cyclohexane, n‐hexane) and water were experimentally investigated and, together with critically selected literature data, were correlated up to the three‐phase critical end point. The present paper extends this analysis to the mutual solubilities of three C8 hydrocarbons (ethylbenzene, ethylcyclohexane, n‐octane) and water, which have been measured at the three‐phase equilibrium pressure up to the critical temperatures (568, 561 and 539 K, respectively). A thermodynamic analysis of these new measurements and of available literature data has been performed up to the three‐phase critical end point. Information is also provided on vapor‐phase equilibrium compositions. The solubility of hydrocarbons in water has been used to calculate Henry's constants, while the solubility and volatility of water in hydrocarbons has been successfully correlated with several modifications of the Redlich‐Kwong equation of state.

High‐temperature mutual solubilities of hydrocarbons and water. Part I: Benzene, cyclohexane andn‐hexane

AbstractThe mutual solubilities at the three‐phase equilibrium pressure of three C6hydrocarbons (benzene, cyclohexane andn‐hexane) and water have been experimentally investigated up to 482 K. A thermodynamic analysis of these new measurements and of critically selected literature data has been carried out to the three‐phase critical end point. Information is also provided on the two‐phase critical locus. The solubility of hydrocarbons in water has been used to calculate Henry's constants, while the solubility of water in the hydrocarbons has been correlated with a modified version of the Redlich‐Kwong equation of state. Consideration is also given to the effect of pressure on the mutual solubilities.

Mutual Solubilities of Hydrocarbons and Water at 0 and 25 °C

Mutual solubilities of 14 paraffinic and 6 aromatic hydrocarbons and water were determined experimentally at 0 and 25 °C. The solubilities are generally smaller at 0 than at 25 °C except the solubilities of paraffins in water which are larger at 0 than at 25 °C. The coefficients of the Redlich–Kister equation were evaluated from the experimental data and correlated as a function of molar volume of liquid hydrocarbons and group contributions. The correlation allows calculation of the mutual solubilities of paraffinic and aromatic hydrocarbons and water at 0 and 25 °C from the knowledge of the molar volume of liquid and the contribution of their component groups.

Mutual Solubilities of Hydrocarbons. III. Systems cis-Decahydronaphthalene—trans-Decahydronaphthalene, cis-Dehydronaphthalene—Tetracosane, cis-Decahydronaphthalene—Dotriacontane

ADVERTISEMENT RETURN TO ISSUEPREVArticleNEXTMutual Solubilities of Hydrocarbons. III. Systems cis-Decahydronaphthalene—trans-Decahydronaphthalene, cis-Dehydronaphthalene—Tetracosane, cis-Decahydronaphthalene—DotriacontaneWilliam F. Seyer, Sun Yip, and Gordon PyleCite this: J. Am. Chem. Soc. 1950, 72, 7, 3162–3164Publication Date (Print):July 1, 1950Publication History Published online1 May 2002Published inissue 1 July 1950https://doi.org/10.1021/ja01163a098RIGHTS & PERMISSIONSArticle Views42Altmetric-Citations4LEARN ABOUT THESE METRICSArticle Views are the COUNTER-compliant sum of full text article downloads since November 2008 (both PDF and HTML) across all institutions and individuals. These metrics are regularly updated to reflect usage leading up to the last few days.Citations are the number of other articles citing this article, calculated by Crossref and updated daily. Find more information about Crossref citation counts.The Altmetric Attention Score is a quantitative measure of the attention that a research article has received online. Clicking on the donut icon will load a page at altmetric.com with additional details about the score and the social media presence for the given article. Find more information on the Altmetric Attention Score and how the score is calculated. Share Add toView InAdd Full Text with ReferenceAdd Description ExportRISCitationCitation and abstractCitation and referencesMore Options Share onFacebookTwitterWechatLinked InReddit PDF (332 KB) Get e-Alerts Get e-Alerts

The Mutual Solubilities of Hydrocarbons. I. The Freezing Point Curves of Dotriacontane (Dicetyl) in Propane and Butane

The Mutual Solubilities of Hydrocarbons. I. The Freezing Point Curves of Dotriacontane (Dicetyl) in Propane and Butane