The solubility of
1,4-dicyanobenzene
(DCB) in 17 neat solvents, that is, methanol, ethanol, n-propanol, isopropanol, acetone, ethyl acetate, ethyl formate, methyl
acetate, cyclohexanone, cyclopentanone, tetrahydrofuran, 2-butanone,
acetonitrile, chloroform, 2-pentanone, dichloromethane, and diethyl
ether, was measured via a gravimetric method from 272.95 to 324.15
K under ambient pressure. Within the experimental temperature range,
the mole fraction solubility of DCB increased with the rising temperature
in all selected solvents, and the order of magnitude is cyclopentanone
> dichloromethane > cyclohexanone ≈ tetrahydrofuran >
chloroform > (acetone, 2-butanone) > 2-pentanone ≈ methyl
acetate > ethyl formate > ethyl acetate > acetonitrile >
diethyl ether > methanol > ethanol > n-propanol
> isopropanol. The solubility of DCB in ketones was much higher
than that in ethers and alcohols. The Wilson model, nonrandom two-liquid
model, Apelblat equation, and λh equation were
employed to mathematically express the solid–liquid phase equilibrium
data of DCB. The maximum values of the root-mean-square and relative
average deviations were 9.83 × 10–5 and 5.21
× 10–3, respectively, which indicated that
good correlation was recorded between the experimental and calculated
data. The dissolution enthalpy, entropy, and Gibbs free energy were
calculated on the basis of thermodynamic relations and the Wilson
model, which revealed that the dissolution of DCB was a spontaneous
and endothermic process.