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absorption enthalpy in imidazolium-based ILs was estimated, and the contribution of each part was further analysed. Figure 4.2 illustrates the CO2 dissolution enthalpy and excess enthalpy in [bmim][BF4], [hmim][BF4] and [omim][BF4] at 298 K. The excess enthalpy contributes less than 5 % to the overall of CO2 absorption enthalpy at pressures lower than 1 MPa. Therefore, it is reasonable to neglect the excess enthalpy when the CO2 separation is operated at low pressure. Figure 4.2. CO2 dissolution enthalpy and excess enthalpy at 298 K in [bmim][BF4], [hmim][BF4] , [omim][BF4]. The influences of cation and anion on the CO2 absorption enthalpy were investigated. The corresponding CO2 loading was depicted in order to check the capacity (loading) and the corresponding enthalpy simultaneously. As shown in Figure 4.3, both the CO2 loading and the magnitude of CO2 absorption enthalpy in [BF4]-based ILs decreases with increasing chain length of cation. The same tendency is also observed for [PF6]- and [Tf2N]-series of ILs. Therefore, the trend of CO2 absorption enthalpy in ILs can be predicted from the CO2 loading. Figure 4.4 illustrates the CO2 loading and CO2 absorption enthalpy in [bmim]-based ILs at 298 K and pressures up to 6 MPa. The CO2 loading in [bmim]-based ILs with the order [NO3] < [DCA] ≈ [BF4] < [PF6] < [TfO] < [Tf2N], while the magnitude of CO2 absorption enthalpy in [bmim]-based ILs at 1 MPa decreases in the order: [TfO] > [BF4] > [NO3] > [PF6] > [DCA] > [Tf2N]. Therefore, the influence of anion is more complicated, and the CO2 absorption enthalpy cannot be estimated from the knowledge of CO2 loading. 23PDF Image | CO2 Separation with Ionic Liquids
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