Abstract
The solid-liquid equilibrium solubility of 2-phenylacetamide in sixteen pure solvents, i.e. methanol, ethanol, n-propanol, isopropanol, n-butanol, isobutanol, n-pentanol, isopentanol, acetone, ethyl acetate, acetonitrile, 2-butanone, 2-pentanone, methyl acetate, ethyl formate and tetrahydrofuran was obtained over a temperature range from 273.75 K to 324.95 K by a gravimetric method under atmospheric pressure. For all the solvents investigated, the equilibrium solubility of 2-phenylacetamide increases with augmented temperature. The statistical correlations were correlated by the modified Apelblat model, λh equation, non-random two-liquid (NRTL) equation and the Wilson equation. On the basis of thermodynamic relations and the Wilson model, the dissolution enthalpy, entropy, and Gibbs free energy were calculated. The results demonstrate that the dissolution of 2-phenylacetamide is a spontaneous and entropy-driven process in the selected solvents. The solubility data, correlation models and derived dissolution properties would promote the development of the separation and reaction of 2-phenylacetamide in industry.
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