Solubility of carbon dioxide in water–t-butanol solutions

1985 ◽  
Vol 63 (12) ◽  
pp. 3403-3410 ◽  
Author(s):  
Peeter Kruus ◽  
Catherine A. Hayes
Keyword(s):  
Carbon Dioxide ◽  
Activity Coefficient ◽  
Mole Fraction ◽  
Scaled Particle Theory ◽  
Gas Solubility ◽  
Particle Theory ◽  
Temperature Dependent ◽  
Solution Composition ◽  
Governing Factor ◽  
Tertiary Butanol

The solubility of carbon dioxide has been determined in tertiary butanol – water mixtures over the temperature range 1–25 °C. The solubility exhibits a sharp, temperature-dependent minimum in water-rich solutions corresponding to a maximum in the activity coefficient of t-butanol, which has also been determined. The activity coefficient of t-butanol has a prominent temperature-dependent maximum (γ > 7.0) at a solution composition of about 0.06 mole fraction alcohol. Application of the scaled particle theory indicates that volume effects are a governing factor in the gas solubility, but are insufficient to explain the total effect. The pH of t-butanol–water and t-butanol–water–CO2 mixtures reveals no major anomalous solvation effect.

Scaled particle theory of gas solubility — inclusion of the temperature dependent hard sphere term

1982 ◽  
Vol 60 (14) ◽  
pp. 1896-1900 ◽  
Author(s):  
Bruce A. Cosgrove ◽  
John Walkley
Keyword(s):  
Temperature Dependence ◽  
Hard Sphere ◽  
Inert Gases ◽  
Scaled Particle Theory ◽  
Sphere Diameter ◽  
Gas Solubility ◽  
Particle Theory ◽  
Temperature Dependent ◽  
Limiting Behaviour ◽  
Self Consistency

The limiting behaviour of the scaled particle theory (spt) of gas solubility has been examined for the inert gases in a range of solvents. The hard sphere limit is shown to exhibit thermodynamic self-consistency only with the inclusion of an effective hard sphere diameter temperature dependence whereas the original spt (exclusion of a temperature dependence) fails to extrapolate to the correct hard sphere limit. Furthermore, inclusion of the temperature dependence yields correct thermodynamic properties for gases of small atomic diameter (and well depth potential) as would be expected from a hard sphere based theory.

Solubility of nonpolar gases in 2-methylcyclohexanone between 273.15 and 303.15 K at 101.32 kPa partial pressure of gas

1989 ◽  
Vol 67 (5) ◽  
pp. 809-811 ◽  
Author(s):  
Maria Asuncion Gallardo ◽  
Maria del Carmen Lopez ◽  
Jose Santiago Urieta ◽  
Celso Gutierrez Losa
Keyword(s):  
Partial Pressure ◽  
Thermodynamic Functions ◽  
Solution Process ◽  
Pair Potential ◽  
Scaled Particle Theory ◽  
Sphere Diameter ◽  
Gas Solubility ◽  
Particle Theory ◽  
Potential Parameters ◽  
Solubility Of Nonpolar Gases

Solubility measurements of several nonpolar gases (He, Ne, Ar, Kr, Xe, H2, D2, N2, CH4, C2H4, C2H6, CF4, SF6, and CO2) in 2-methylcyclohexanone at 273.15–303.15 K and a partial pressure of gas of 101.32 kPa are reported. Thermodynamic functions (Gibbs energy, enthalpy, and entropy) for the solution process at 298.15 K and 101.32 kPa partial pressure of gas are evaluated. Use is made of the Scaled Particle Theory applied to gas solubility for determining Lennard-Jones (6, 12) pair-potential parameters and temperature dependence of the effective hard-sphere diameter of the solvent. The values that this theory predicts for the solution thermodynamic functions are also calculated. Keywords: 2-methylcyclohexanone, gas solubility, thermodynamic functions of solution, Henry coefficient, scaled particle theory.

An analysis of the thermodynamics of transfer of polar non-electrolytes from water to aqueous concentrated salt solutions

1977 ◽  
Vol 30 (12) ◽  
pp. 2597 ◽  
Author(s):  
RF Cross ◽  
PT McTigue
Keyword(s):  
Activity Coefficient ◽  
Scaled Particle Theory ◽  
Enthalpies Of Solution ◽  
Polar Group ◽  
Methyl Ethyl ◽  
Particle Theory ◽  
Salt Solutions ◽  
Thermodynamics Of Transfer ◽  
Alkyl Side Chains ◽  
Alkyl Acetates

A calorimeter has been constructed and used to determine the limiting enthalpies of solution (ΔHS) of a series of alkyl acetates (methyl, ethyl, propyl, butyl and t-butyl) in water and aqueous solutions of some of the following salts: LiCl, NaCl, KCl, CsCl, KF, KBr, NaNO3 and NaClO4. These measurements are combined with previous activity coefficient determinations to obtain the thermodynamics of transfer for the esters. In the case of transfer to NaCl solutions, scaled-particle theory calculations are used to determine the thermodynamics of cavity transfer, which, when combined with the experimental total-transfer quantities, give rise to a set of quantities that we have called the interaction transfer quantities. These quantities indicate that the predominant factors in the transfer of neutral molecules containing both polar and non-polar segments from water to NaCl solutions are the transfer of the cavity and of the interactions of the polar group. The interactions of the alkyl side chains are shown to be similar to those of alkane molecules.

Solubility of nonpolar gases in 2,6-dimethylcyclohexanone

1990 ◽  
Vol 68 (3) ◽  
pp. 435-439 ◽  
Author(s):  
Maria Asuncion Gallardo ◽  
Maria Del Carmen Lopez ◽  
Jose Santiago Urieta ◽  
Celso Gutierrez Losa
Keyword(s):  
Gibbs Energy ◽  
Thermodynamic Functions ◽  
Pair Potential ◽  
Scaled Particle Theory ◽  
Gas Solubility ◽  
Particle Theory ◽  
Lennard Jones ◽  
Enthalpy And Entropy ◽  
Potential Parameters ◽  
Solubility Of Nonpolar Gases

Solubility measurements of He, Ne, Ar, Kr, Xe, H2, D2, N2, CH4, C2H4, C2H6, CF4, SF6, and CO2 in 2,6-dimethylcyclohexanone at temperatures 273.15 to 303.15 K and at a gas partial pressure of 101.33 kPa are reported. Standard changes in Gibbs energy, enthalpy, and entropy for the dissolution process at 298.15 K are also presented. Results for both solubility and thermodynamic functions are compared with those for cyclohexanone and 2-methylcyclohexanone. The scaled particle theory is used to obtain the effective Lennard–Jones (6,12) pair potential parameters for 2,6-dimethylcyclohexanone and, from these, the values it predicts for the solubility of the studied gases in the solvent are obtained. Keywords: gas solubility, Henry coefficient, 2,6-dimethylcyclohexanone, thermodynamic functions of solution, non-polar gases.

scholarly journals Use of scaled-particle theory in the assessment of the Ph4As+/Ph4B− assumption for single ions

1979 ◽  
Vol 57 (1) ◽  
pp. 71-76 ◽  
Author(s):  
Michael H. Abraham ◽  
Asadollah Nasehzadeh
Keyword(s):  
Free Energy ◽  
Recent Work ◽  
Scaled Particle Theory ◽  
Cavity Formation ◽  
Energy Term ◽  
Free Energies ◽  
Particle Theory ◽  
Novel Method ◽  
Energy Of Interaction ◽  
Solvent Molecules

A novel method for the assessment of the Ph4As+/Ph4B− assumption for free energies of transfer of single ions has recently been suggested by Treiner, and used by him to deduce that the assumption is not valid for transfers between water, propylene carbonate, sulpholane, dimethylsulphoxide, N-methyl-2-pyrrolidone, and perhaps also dimethylformamide. The basis of the method is the estimation of the free energy of cavity formation by scaled-particle theory, together with the hypothesis that the free energy of interaction of Ph4As+ (or Ph4B−) with solvent molecules is the same in all solvents, ΔGt0(int) = 0. It is shown in the present paper that (a) whether or not the Ph4As+/Ph4B− assumption applies to transfer to a given solvent depends on which other solvent is taken as the reference solvent in Treiner's method, (b) the calculation of the cavity free energy term by scaled-particle theory and by the theory of Sinanoglu – Reisse – Moura Ramos (SRMR) yields values so different that the method cannot be considered reliable, (c) the calculation of cavity enthalpies and entropies for Ph4As+ or Ph4B− by scaled-particle theory yields results that are chemically not reasonable, (d) the hypothesis that ΔGt0(int) = 0 conflicts with SRMR theory, and (e) the conclusions reached by Treiner are not in accord with recent work that in general supports the Ph4As+/Ph4B− assumption for solvents that are rejected by Treiner.

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