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where DHabs is the CO2 absorption enthalpy per mol CO2, Hdis is the enthalpy of CO2 dissolution and depends on the Henry’s constant as shown in Eq. (10), Hex is the excess enthalpy for a solution with 1 mol of CO2 and m mol of ILs at saturation state (equilibrium state). m depends on temperature, pressure and the type of ILs. Hex can be calculated from the activity coefficient in the liquids phase as shown in Eq. (11). 2.2. Energy consumption for a CO2 separation process The CO2 separation process generally consists of the absorber, desorber and heat exchanger as shown in Fig. 1. Most of the energy consumption required in a separation process is from the solvent regeneration, therefore, only the energy consumed for the solvent regeneration was accounted in this work. Depending on the type of solvents, the regeneration can be a pressure swing (solvent regen- eration by pressure decrease) or temperature swing (solvent regeneration by temperature increase) process. As the imidazoli- um-based ILs studied in this work belong to physical absorbents, both options can be operated. Based on the CO2 absorption enthalpy and other thermody- namic properties, the energy consumption for a CO2 separation process can be estimated. In the energy consumption analysis, for the convenience, in this work, it was assumed that 1 mol of CO2 is separated and out of the desorber at temperature of T2 and pressure of P2, and n mol of CO2 is left in the solvent (ILs). In the absorber, it was assumed that (1 + n) mol of CO2 is absorbed by m mol of ILs at temperature of T1 and pressure of P1. The energy consumption Q for the solvent regeneration can be calculated as: Q 1⁄4 DH2 DH1 ð12Þ where DH2 1⁄4mHaqðT2;P2ÞþnHaq ðT2;P2ÞþðnþmÞHexðT2;P2ÞþHg ðT2;P2Þ IL CO2 2 CO2 DH1 1⁄4mHaqðT1;P1Þþð1þnÞHaq ðT1;P1Þþð1þnþmÞHexðT1;P1Þ IL CO2 1 For the pressure swing process, the temperature is a constant (T1 = T2), and the energy consumption was simplified as: Qdes is the energy consumption in order to vaporize CO2 from liquid to vapor phase, which is termed as the desorption enthalpy. Hex is 1 the excess enthalpy of the solution at T1 and P1, Hex is the excess 2 enthalpy of the solution at T2 and P2, and Qex is the energy consump- tion due to the difference of excess enthalpy between the streams. For the temperature swing process, it was assumed that the heat duty of heat exchanger is zero, and the energy consumption reaches the maximum that can be calculated as: Q 1⁄4Qsen þQdes þQex ð14Þ where Qsen 1⁄4 mCP;ILðT2 T1Þ þ nCP;CO2;gðT2 T1Þ Qsen is the sensible heat due to the increase of temperature, and Cp is the heat capacity. The heat capacity of gaseous CO2 is temperature- dependent and described as the following equation: CP;CO2 ;g 1⁄4 0:0416T þ 25:048 ð15Þ In this work, it was assumed that the pressure effect on the sensible heat was negligible due to the limited knowledge of the pressure effect on the enthalpy of ILs. 3. Results and discussions 3.1. Evaluation of CO2 solubility in imidazolium-based ILs To develop IL technology for CO2 separation, the CO2 solubility in ILs is an important knowledge. The CO2 solubility in imidazoli- um-based ILs has been measured extensively by different research groups with different methods. The experimental data has been surveyed, but the experimental data evaluation has not been car- ried out. Meanwhile, the CO2 absorption enthalpy and excess enthalpy have not been studied well experimentally, and the energy consumption analysis for a CO2 separation process can only be estimated based on the thermodynamic model with the param- eters obtained from the fitting of the CO2 solubility in ILs. Our preliminary research shows that the CO2 absorption enthalpy is very sensitive to the experimental solubility data, which makes it crucial to evaluate the experimental CO2 solubility data and choose the reliable data to obtain the parameters of the thermodynamic model. Therefore, the experimental data evaluation was the first step in energy consumption analysis. In general, CO2 separation process is operated at pressures less than 5 MPa [24], therefore, Q 1⁄4 Qdes þ Qex where Qdes 1⁄4HdisðT2;P2Þ1⁄4Hg CO2 CO2 Qex 1⁄4DHex 1⁄4ðnþmÞHexðT2;P2Þð1þnþmÞHexðT1;P1Þ 21 ð13Þ Haq Y. Xie et al. / Applied Energy 136 (2014) 325–335 327 Fig. 1. The schematic of CO2 separation process by ILs.PDF Image | CO2 Separation with Ionic Liquids
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