Juan I. Pardo

HmE, VmE, and GmE of {xCl2HCCHCl2 + (1 − x)C6H14} at several temperatures

Excess molar enthalpies, excess molar volumes, and vapour pressures of (1,1,2,2-tetrachloroethane + n-hexane) between 288.15 and 318.15 K (298.15 to 308.15 K for the vapour pressures) were determined. Activity coefficients and excess molar Gibbs free energies were calculated by Barkers method. Both the strong endothermic character and the positive excess entropy of the mixture suggest an orientational order in 1,1,2,2-tetrachloroethane that is destroyed in the mixing process.

Viscosities of the ternary mixture (2-butanol+n-hexane+1-butylamine) at 298.15 and 313.15 K

Abstract Viscosities of the ternary mixture (2-butanol+ n -hexane+1-butylamine) and of the binary mixtures (2-butanol+ n -hexane) at 298.15 and 313.15 K, and (2-butanol+1-butylamine) at 313.15 K have been measured at atmospheric pressure. Viscosity deviations and excess Gibbs energy of activation of viscous flow for the binary and ternary systems were fitted to Redlich–Kisters and Cibulkas equations, respectively. To correlate experimental data of ternary system from binary ones, different empirical and semiempirical equations have been used (Nissan and Grunberg, Hind, Frenkel, McAllister, Katti and Chaudhri, Heric and Iulan) and their parameters have been calculated. The “viscosity-thermodynamic” model (UNIMOD) has been applied to correlate experimental data for the binary mixtures and to predict the viscosity for the ternary system. The Group Contribution-Thermodynamic Viscosity model (GC-UNIMOD), and the group contribution method proposed by Wu have been employed to predict the viscosity for the binary and ternary systems.

Viscosities of the ternary mixture (1-butanol + n-hexane + 1-butylamine) at the temperatures 298.15 and 313.15 K

Abstract Viscosities of the ternary mixture {1-butanol + n -hexane + 1-butylamine} and the binary mixtures {1-butanol + n -hexane}, {1-butanol + 1-butylamine} and { n -hexane + 1-butylamine} have been measured at 298.15 and 313.15 K. Viscosity deviations for the binary and ternary systems were fitted to Redlich-Kisters and Cibulkas equations, respectively. The “viscosity-thermodynamic” model (UNIMOD) has been used to correlate experimental data for the binary mixtures and to predict the viscosities for the ternary system. The Group-Contribution Thermodynamic-Viscosity model (GC-UNIMOD), and the group contribution method proposed by Wu have been used to predict the viscosity of the binary and ternary systems.

Excess molar volumes VEm of (an alkanol + another alkanol) or (hexane + an alkanol) or (an alkanediol + an alkanol or another alkanediol) at the temperature 303.15 K

The excess molar volumes of (an isomer of butanol + another isomer of butanol or hexane or butan-1,3-diol) and (butan-1,3-diol + butan-2, 3-diol), measured at the temperature 303.15 K by a dilatometric method, are reported. Experimental excess volumes are negative over the whole composition range, except for mixtures with hexane in which excess volumes are positive and increase in the sequence normal

Viscosities of 1-chlorobutane and 1,4-dichlorobutane with isomeric butanols at 25 and 40°C

This paper reports viscosities and excess viscosities for binary systems of 1-chlorobutane and 1,4-dichlorobutane with isomeric butanols at 25 and 40°C. Results show negative deviations from ideal behavior. Viscosities and excess viscosities were correlated by means of the Grunberg-Nissan equation and the Redlich-Kister equation.

Experimental paperSolubility of gases in butanols. I. Solubilities of nonpolar gases in 1-butanol from 263.15 to 303.15 K at 101.33 kPa partial pressure of gas

Solubility measurements of 15 nonpolar gases (He, Ne, Ar, Kr, Xe, H2, D2, N2, O2, CH4, C2H4, C2H6, CF4, SF6 and CO2) in 1-butanol were carried out at 263.15, 273.15, 283.15, 293.15, and 303.15 K and partial pressure of gas of 101.33 kPa. Standard changes in thermodynamic functions for the solution process at 298.15 K (Gibbs energy, enthalpy and entropy) are derived from the experimental values of the solubility of gases and its variation with temperature. Lennard-Jones 6,12 pair potential parameters and the dependence of the effective hard-sphere diameter with respect to the temperature for 1-butanol have been estimated using the equations of scaled particle theory (SPT). Making use of SPT in the reverse direction, i.e., starting from the potential parameters found through it, theoretical solubilities and thermodynamic functions for the solution process have been calculated and compared with the experimental values.

Densities, speeds of sound and isentropic compressibilities of binary and ternary mixtures containing benzene, cyclohexane and hexane at 298.15 K

Abstract Densities, ϱ, and speeds of sound, u , have been measured for the ternary mixture {benzene + cyclohexane + hexane} and the corresponding binary mixtures {benzene + cyclohexane}, {benzene + hexane} and {cyclohexane + hexane}, at the temperature 298.15 K. Using these results, the isentropic compressibilities, κ s , the excess isentropic compressibilities, κ s E , and the speeds of sound deviations, Δu , have been calculated for both the binary mixtures and the ternary system. Excess isentropic compressibilities, κ s E , and the speeds of sound deviations, Δu , have been fitted to the Redlich-Kister equation in the case of binary mixtures, while the equation of Cibulka was used to fit the values relating to the ternary system. The empiric equations of Redlich-Kister, Tsao-Smith, Kohler and Colinet have been applied in order to predict the κ s E and Δu of ternary mixtures from the binary contributions.

Solubility of gases in butanols. III. Solubilities of non-polar gases in 2-butanol from 263.15 to 303.15 K at 101.33 kPa partial pressure of gas

Abstract Solubility measurements of 15 nonpolar gases (He, Ne, Ar, Kr, Xe, H2, D2, N2, O2, CH4, C2H4, C2H6, CF4, SF6 and CO2) in 1-butanol were carried out at 263.15, 273.15, 283.15, 293.15, and 303.15 K and partial pressure of gas of 101.33 kPa. Standard changes in thermodynamic functions for the solution process at 298.15 K (Gibbs energy, enthalpy and entropy) are derived from the experimental values of the solubility of gases and its variation with temperature. Lennard-Jones 6,12 pair potential parameters and the dependence of the effective hard-sphere diameter with respect to the temperature for 1-butanol have been estimated using the equations of scaled particle theory (SPT). Making use of SPT in the reverse direction, i.e., starting from the potential parameters found through it, theoretical solubilities and thermodynamic functions for the solution process have been calculated and compared with the experimental values.

Solubility of gases in butanols II. Solubilities of nonpolar gases in 2-methyl-1-propanol from 263.15 to 303.15 K at 101.33 kPa partial pressure of gas

Abstract Solubilities of 15 nonpolar gases (He, Ne, Ar, Kr, Xe, H2, D2, N2, O2, CH4, C2H4, C2H6, CF4, SF6 and CO2) in 2-methyl-1-propanol have been measured at 263.15, 273.15, 283.15, 293.15, and 303.15 K and at the partial pressure of gas 101.33 kPa. Standard changes in the thermodynamic properties for the solution process (enthalpies, entropies and Gibbs energies) at 298.15 K have been derived from the experimental data. The scaled particle theory (SPT) has been applied in order to estimate the Lennard-Jones 6,12 pair potential parameters at 298.15 K and the dependence of the effective hard-sphere diameter on the temperature for 2-methyl-1-propanol. Theoretical solubilities and values for the thermodynamic functions have been calculated using the SPT in the reverse direction starting from the potential parameters. Results for 2-methyl-1-propanol have been compared with those corresponding to 1-butanol.

Solubility of gases in butanols: IV. Solubilities of nonpolar gases in 2-methyl-2-propanol at 303.15 K and 101.33 kPa partial pressure of gas

Abstract Solubilities of 15 nonpolar gases (He, Ne, Ar, Kr, Xe, H 2 , D 2 , N 2 , O 2 , CH 4 , C 2 H 4 , C 2 H 6 , CF 4 , SF 6 , and CO 2 ) in 2-methyl-2-propanol ( tert -butanol) have been measured at the temperature 303.15 K and 101.33 kPa partial pressure of gas. Standard changes of the Gibbs energy of solution have been also determined from experimental data. The Lennard–Jones 6,12 pair potential parameters have been estimated for that solvent using the Scaled Particle Theory (SPT) and these parameters have been compared with those corresponding to the other isomers of butanol. It can be concluded that the derived energy parameters provide a measurement of the association of the alkanol. A version of the UNIFAC model has been applied and the corresponding interaction parameters for alkanes and alkanols have been determined.