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Table 6. The mass and mole fractions of water in aqueous [Amim][HCOO]. Mass fraction mw 0.10 0.19 0.37 0.73 Mole fraction xw 0.509 0.687 0.846 0.962 Table 7. The parameters in equations (3) and (5). xw 0.509 0.687 0.846 0.962 kij -0.076 -0.070 -0.045 -0.0071 lij -0.50 -0.73 -1.3 -4.2 In order to illustrate the non-ideality of the aqueous [Amim][HCOO], the excess molar volume (VE) and viscosity deviation (Δη) were calculated according to the following equations: (6) (7) As shown in Fig. 2(a), the excess molar volumes of the aqueous [Amim][HCOO] exhibit negative deviations from ideality, thus indicating that the intermolecular interactions between the [Amim][HCOO] and H2O were strong and result in a volume contraction. Upon increasing temperatures, the magnitude of the negative value increased and can be attributed to the influence of the hydrogen bond. When comparing the mole volumes of dry [Amim][HCOO] (144.4 cm·mol- 1, 303.15 K) and pure water (18.21 cm·mol-1, 303.15 K), the excess molar volumes reported here were relatively small, but the density of the aqueous [Amim][HCOO] still needed to be adjusted in order to represent the experimental data well. As shown in Fig. 2(b), when the mole fraction of water was below 0.7, the viscosity of the aqueous [Amim][HCOO] gave rise strong negative deviations, at low temperatures. For example, when the mole fraction of water was 0.509, at 303.15, the magnitude of viscosity deviations reached 17.6% for the viscosity of dry [Amim][HCOO] (65.5 mPa·s). As a consequence, the ideal mixing rule cannot be used to study the viscosity of the aqueous [Amim][HCOO]. Upon increasing temperatures, the deviations were moderated and exhibited positive values. At high water concentrations (xw > 0.95), the viscosity deviations changed and gave a positive contribution. The same phenomenon was also observed by Rodriguez et al. for the ([emim][TFA] + H2O) system [19].PDF Image | CO2 Separation with Ionic Liquids
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