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Table 4.1. Sources of experimental CO2 solubility in imidazolium-based ILs. ILs [emim][BF4] [bmim][BF4] [hmim][BF4] [omim][BF4] [bmim][PF6] [hmim][PF6] [emim][Tf2N] [bmim][Tf2N] [hmim][Tf2N] T,K Ref. 298-343 [51-54] 278-383 [22, 55-61] 293-373 [22, 51, 303-363 [21-23] 283-413 [20, 21, 298-373 [51, 63, 293-450 [51, 57, 273-450 [56, 58, 282-413 [51, 55, 54, 62, 63] 25, 26, 51, 56, 60, 64-67] 68] 69-73] 69, 71, 74-77] 63, 71, 73, 78-82] Figure 4.1. CO2 solubility in [emim][BF4]. Symbols: experimental data. Curve: correlations with NRTL-RK model. The evaluation shows that most of available experimental data is reliable. The data from three groups [21, 54, 69] is unreliable and excluded in parameter fitting. In addition, it is found that the Henry’s constant is sensitive to the experimental CO2 solubility data. Since the Henry’s constant is of great importance in predicting the CO2 absorption enthalpy (eq. 3.32), it is important to determine the CO2 solubility accurately. 4.1.2 CO2 absorption enthalpy The CO2 absorption enthalpy consists of CO2 dissolution enthalpy and excess enthalpy. The CO2 dissolution enthalpy is calculated from the Henry’s constant of CO2, and the excess enthalpy is calculated from activity coefficient of CO2 in the liquid phase. The CO2 22PDF Image | CO2 Separation with Ionic Liquids
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