A model-guided determination of Δdis G2 ∞ for slightly soluble gases in water using solubility data: From the solvent's freezing point to its critical point

There is continuing interest in the description of the solubility of nonpolar gases in water over a wide range of temperatures. On one hand, the solubility data are used in many fields of science and technology; and on the other hand, simulation and theoretical calculations require experimental data...

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Detalles Bibliográficos
Publicado: 2008
Materias:
Aqueous solutions
Solubility of gases
Thermodynamic properties
Acceso en línea:https://bibliotecadigital.exactas.uba.ar/collection/paper/document/paper_00959782_v37_n3_p433_Alvarez
http://hdl.handle.net/20.500.12110/paper_00959782_v37_n3_p433_Alvarez
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Biblioteca Digital - Facultad de Ciencias Exactas y Naturales (UBA) de Universidad de Buenos Aires
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spelling paper:paper_00959782_v37_n3_p433_Alvarez2023-06-08T15:09:45Z A model-guided determination of Δdis G2 ∞ for slightly soluble gases in water using solubility data: From the solvent's freezing point to its critical point Aqueous solutions Solubility of gases Thermodynamic properties There is continuing interest in the description of the solubility of nonpolar gases in water over a wide range of temperatures. On one hand, the solubility data are used in many fields of science and technology; and on the other hand, simulation and theoretical calculations require experimental data to test their results and predictions. For these reasons it is important to have a means of calculating from the experimental solubility data the Gibbs energy of dissolution of gases (Δdis G 2 ∞ ) and Henry's constant (k H) over all the temperature range of existence of liquid water. Under ambient conditions it is relatively easy to relate Δdis G 2 ∞ and, hence, k H to the solubility data of nonpolar gases. However, this simple procedure becomes increasingly complicated as the temperature approaches the critical temperature of the solvent and it is necessary to make important corrections to obtain the thermodynamic quantities for the dissolution process. This difficulty can be resolved with a procedure that employs a perturbation method applied to a simple model solvent to guide the correct determination of k H and Δdis G 2 ∞ . We describe in this work an iterative calculation procedure whose correctness was validated with a thermodynamic relationship that uses only experimental data, hence it is model-free. Unfortunately this relationship can be applied only to a few systems due to its data requirements. The iterative procedure described in this work can be extended to higher pressures, p≅50 MPa above the solvent's vapor pressure, and also to gases dissolved in nonaqueous solvents. © 2008 Springer Science+Business Media, LLC. 2008 https://bibliotecadigital.exactas.uba.ar/collection/paper/document/paper_00959782_v37_n3_p433_Alvarez http://hdl.handle.net/20.500.12110/paper_00959782_v37_n3_p433_Alvarez
institution Universidad de Buenos Aires
institution_str I-28
repository_str R-134
collection Biblioteca Digital - Facultad de Ciencias Exactas y Naturales (UBA)
topic Aqueous solutions
Solubility of gases
Thermodynamic properties
spellingShingle Aqueous solutions
Solubility of gases
Thermodynamic properties
A model-guided determination of Δdis G2 ∞ for slightly soluble gases in water using solubility data: From the solvent's freezing point to its critical point
topic_facet Aqueous solutions
Solubility of gases
Thermodynamic properties
description There is continuing interest in the description of the solubility of nonpolar gases in water over a wide range of temperatures. On one hand, the solubility data are used in many fields of science and technology; and on the other hand, simulation and theoretical calculations require experimental data to test their results and predictions. For these reasons it is important to have a means of calculating from the experimental solubility data the Gibbs energy of dissolution of gases (Δdis G 2 ∞ ) and Henry's constant (k H) over all the temperature range of existence of liquid water. Under ambient conditions it is relatively easy to relate Δdis G 2 ∞ and, hence, k H to the solubility data of nonpolar gases. However, this simple procedure becomes increasingly complicated as the temperature approaches the critical temperature of the solvent and it is necessary to make important corrections to obtain the thermodynamic quantities for the dissolution process. This difficulty can be resolved with a procedure that employs a perturbation method applied to a simple model solvent to guide the correct determination of k H and Δdis G 2 ∞ . We describe in this work an iterative calculation procedure whose correctness was validated with a thermodynamic relationship that uses only experimental data, hence it is model-free. Unfortunately this relationship can be applied only to a few systems due to its data requirements. The iterative procedure described in this work can be extended to higher pressures, p≅50 MPa above the solvent's vapor pressure, and also to gases dissolved in nonaqueous solvents. © 2008 Springer Science+Business Media, LLC.
title A model-guided determination of Δdis G2 ∞ for slightly soluble gases in water using solubility data: From the solvent's freezing point to its critical point
title_short A model-guided determination of Δdis G2 ∞ for slightly soluble gases in water using solubility data: From the solvent's freezing point to its critical point
title_full A model-guided determination of Δdis G2 ∞ for slightly soluble gases in water using solubility data: From the solvent's freezing point to its critical point
title_fullStr A model-guided determination of Δdis G2 ∞ for slightly soluble gases in water using solubility data: From the solvent's freezing point to its critical point
title_full_unstemmed A model-guided determination of Δdis G2 ∞ for slightly soluble gases in water using solubility data: From the solvent's freezing point to its critical point
title_sort model-guided determination of δdis g2 ∞ for slightly soluble gases in water using solubility data: from the solvent's freezing point to its critical point
publishDate 2008
url https://bibliotecadigital.exactas.uba.ar/collection/paper/document/paper_00959782_v37_n3_p433_Alvarez
http://hdl.handle.net/20.500.12110/paper_00959782_v37_n3_p433_Alvarez
_version_ 1768543745341390848

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