Precision Methods for the Determination of the Solubility of Gases in Liquids

Wilhelm, Emmerich; Battino, Rubin

doi:10.1080/10408348508542786

Cited by 11 publications

(21 citation statements)

References 249 publications

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“…f i cannot be determined experimentally (Wilhelm, 1985(Wilhelm, ,1986. f i cannot be determined experimentally (Wilhelm, 1985(Wilhelm, ,1986.…”

mentioning

confidence: 98%

Prediction of the solubility of hydrogen in naphtha reformate using the modified UNIFAC group contribution method

Fahim¹,

Elkilani²

1991

Ind. Eng. Chem. Res.

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The solubility of hydrogen in the naphtha reformate cut (423-473 K) was estimated by using the UNIFAC group contribution method. Functional group concentrations, estimated from analytical data, and interactions parameters, predicted in this work, were used to provide reasonable estimates of hydrogen solubility. The predicted solubility data were compared favorably with experimental values obtained by the pulse response technique using gas chromatography within 10% error. 13, 185-197.

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“…f i cannot be determined experimentally (Wilhelm, 1985(Wilhelm, ,1986. f i cannot be determined experimentally (Wilhelm, 1985(Wilhelm, ,1986.…”

mentioning

confidence: 98%

Prediction of the solubility of hydrogen in naphtha reformate using the modified UNIFAC group contribution method

Fahim¹,

Elkilani²

1991

Ind. Eng. Chem. Res.

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“…In this case, the unsymmetric convention is usually selected: it has the advantage that Henry fugacities and hence activity coefficients HL 2 T, P, x 2 are unambiguously accessible via an experimental procedure (cf. Equation 301) [17,66,169,216,219]. The figure was reproduced from E. Wilhelm, J.…”

Section: Henry's Law: An Alternative Ideal-solution Model For Liquid Systemsmentioning

confidence: 99%

“…Equation 300a summarizes Henry's law; it defines the Henry fugacity h π i,j (T, P) of component i dissolved in component j for any phase π (L or V) and identifies the limiting slope of the curve f π i vs. x π i at constant T and P as h π i,j (T, P) . Henry's law is a limiting law, and for real solutions it is approximately valid for small values of x π i , with the experimental precision determining the observed apparent validity range [17,66,169,216,219].…”

Section: Henry's Law: An Alternative Ideal-solution Model For Liquid Systemsmentioning

confidence: 99%

“…Equation 300b summarizes the Lewis-Randall rule; it valid in any phase (L or V) and shows that in the limit x π i → 1 both f i and the limiting slope of the curve f π i vs. x π i at constant T and P become equal to the fugacity of pure i in phase . The Lewis-Randall rule is a limiting law, and for real solutions it is approximately valid for values of x π i near unity, with the experimental precision determining the observed apparent validity range [17,66,169,216,219].…”

Section: Henry's Law: An Alternative Ideal-solution Model For Liquid Systemsmentioning

confidence: 99%

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Solutions, in Particular Dilute Solutions of Nonelectrolytes: A Review

Wilhelm¹

2021

J Solution Chem

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The liquid state is one of the three principal states of matter and arguably the most important one; and liquid mixtures represent a large research field of profound theoretical and practical interest. This topic is of importance in many areas of the applied sciences, such as in chemical engineering, geochemistry, the environmental sciences, biophysics and biomedical technology. First, I will concisely present a review of important concepts from classical thermodynamics of nonelectrolyte solutions; this will be followed by a survey of (semi-)empirical approaches to representing the composition and temperature dependence of selected thermodynamic mixture properties, and finally the focus will be on dilute binary nonelectrolyte solutions where one component, a supercritical solute, is present in much smaller quantity than the other component, called the solvent. Partial molar properties in the limit of infinite dilution (indicated by a superscript ∞) are of particular interest. For instance, activity coefficients (Lewis–Randall (LR) convention) are customarily used to characterize mixing behavior, and infinite-dilution values $$\gamma_{i}^{{{\text{LR,}}\infty }}$$ γ i LR, ∞ provide a convenient route for obtaining binary parameters for several popular solution models. When discussing solute (j)—solvent (i) interactions in solutions where the solute is supercritical, the Henry fugacity $$h_{j,i} \left( {T,P} \right)$$ h j , i T , P , also known as Henry’s law (HL) constant, is a measurable thermodynamic key quantity. Its temperature dependence yields information on the partial molar enthalpy change on solution $$\Delta H_{j}^{\infty } \left( {T,P} \right)$$ Δ H j ∞ T , P , while its pressure dependence yields information on the partial molar volume $$V_{j}^{{{\text{L,}}\infty }} \left( {T,P} \right)$$ V j L, ∞ T , P of solute j in the liquid phase (superscript L). I will clarify issues frequently overlooked, touch upon solubility data reduction and correlation, report a few recent high-precision experimental results on dilute aqueous solutions of supercritical nonelectrolytes, and show the equivalency of results for caloric quantities (e.g. $$\Delta H_{j}^{\infty }$$ Δ H j ∞ ) obtained via van ’t Hoff analysis of high-precision solubility data with directly measured calorimetric data.

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“…Of practical and theoretical importance is the partial molar volume at infinite dilution, [103][104][105][106] which is defined by (7:30) and the excess partial molar volume at infinite dilution…”

Section: @H @Pmentioning

confidence: 99%