Vapor–liquid equilibria (VLE)
of benzene and acetone in
the selected eight imidazole ionic liquids (ILs) was studied with
a static method. VLE measurements were carried out over an extremely
low concentration range and at temperatures ranging from 303.2 to
333.2 K. On the basis of the solubility data, the infinite dilution
activity coefficient (γ
∞
)
and Henry’s constant (H) were derived and
described formally by using the nonrandom two-liquid equation. The
obtained results indicated that the anion species of ionic liquids
play a great role in determining the solubility of benzene and acetone
relative to cationic species, and increase following the sequence
[Tf2N] > [PF6] > [BF4]. The
difference
of solubility between acetone and benzene mainly depends on the difference
of their chemical and structural properties. Additionally, the partial
molar excess enthalpies at infinite dilution (H
i
E,∞
) have been derived from the temperature
dependence of the limiting activity coefficients, and partial molar
enthalpies and entropies at infinite dilution for benzene and acetone
absorbed in ILs have also been derived from the temperature dependence
of the Henry’s constant.
By using the dual vessel equilibrium
method, the solubility of
oxygen in toluene and acetic acid was experimentally investigated
with pressure ranging from 0.1 to 1.0 MPa at temperatures from 293.1
to 383.1 K. The results show that the oxygen solubility either in
toluene or in acetic acid increases with a rise in temperature. On
the basis of the experimental data, Henry coefficients were derived
and expressed as a function of temperature. At the same temperature,
Henry coefficient for the oxygen–toluene system is lower than
that for the oxygen–acetic acid system. Through analysis of
the Gibbs energy (ΔG
0), partial
molar enthalpy (ΔH
0), and the partial
molar entropy (ΔS
0) of the solvation,
we can know that solubilization of oxygen either in toluene or in
acetic acid is an endothermic process. To correlate the experimental
data, the Peng–Robinson equation of state with the quadratic
mixing rule was used for the two systems.
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