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liquid and crystalline compounds in both chloroform and 1,2-dichloroethane. The
experimental values were determined by either direct calorimetric methods or calculated
based on the temperature dependence of the measured infinite dilution activity
coefficients or solubilities. The retrieved enthalpy of solution values were converted to
gas-to-organic solvent enthalpies of transfer by
Liquid solutes: AHsolv = AHsoln - AHVap,298K (7)
Crystalline solutes: AHsolv = AHsoln - AHSub,298 (8)
subtracting the solute's standard molar enthalpy of vaporization [66], AHVap,298K, or
standard molar enthalpy of sublimation [67], AHSub,298K , at 298.15 K. For purposes of
the this study we have considered enthalpies of solvation, AHsolv, and what will be called
"inner energies", AUsolv,, to be equivalent. Goss [68] discusses the difference between the
AHsolv, and AUsolv, in terms of the concentration units used in expressing the gas-phase
concentrations of the Henry's law constant. At 298 K the difference between the
quantities amounts to about 2.5 kJ/mole [68], which is less than the experimental
uncertainty associated with many of the observed values. Given the slight numerical
difference between the two values under normal environmental conditions, we have
combined both sets of numerical values into a single database, as has been done in the
past by most research groups that have developed predictive methods for enthalpies of
solvation. Most of our tabulated values are enthalpies of solvation; however, there may
be a few "inner energies" listed in Tables 1 and 2 that that were mislabeled as enthalpies
in the original data source.
Based on an initial assessment of the available experimental data, we eliminated
from consideration all experimental data that pertained to temperatures outside of the
