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334 Y. Xie et al. / Applied Energy 136 (2014) 325–335 Fig. 12. The amount of ILs and energy consumption for pressure- and temperature-swing CO2 separation process. 4. Conclusion In this work, in order to carry out the energy consumption for a CO2 separation process using ILs as liquid absorbents based on the available experimental data, the experimental CO2 solubility in imidazolium-based ILs at pressures below 10 MPa was evaluated by NRTL-RK model firstly. It is found that most of the data is reli- able, and the data from three sources is inconsistent with those from other sources. The reliable CO2 solubilities were further rep- resented by the NRTL-RK model, and the CO2 absorption enthalpy was then calculated based on the thermodynamic model. The results show that the CO2 absorption enthalpy in ILs is dominated by the CO2 dissolution enthalpy. The magnitude of CO2 absorption enthalpy decreases with increasing chain length in cation and strongly depends on the anion of ILs. The energy consumption of a CO2 separation process was esti- mated. The energy consumption for separating 1 mol of CO2 using different ILs was calculated and compared. If the solvent is regen- erated by releasing pressure, the CO2 desorption enthalpy contrib- utes mostly to the total energy consumption; If CO2 is absorbed at 298 K and 1 MPa and IL is regenerated by decreasing the pressure to 0.1MPa at the same temperature, among the studied ILs, [emim][EtSO4] is the solvent with the lowest energy consumption of 9.840 kJ/mol CO2. If the solvent is regenerated by increasing temperature, the sensible enthalpy has a significant influence on the total energy consumption for a CO2 separation process because of the high heat capacity of ILs; If CO2 is absorbed at (298 K, 0.1 MPa) and desorbed at (323 K, 0.1 MPa), [emim][PF6] is the solvent with the lowest energy demand of 888.9 kJ/mol CO2. If the solvent is regenerated by both releasing pressure and increas- ing temperature, both the Henry’s constant of CO2 in ILs and the heat capacity of ILs are important factors for analyzing the energy consumption; If CO2 is absorbed at 298 K and 1 MPa and IL is regenerated at 0.1 MPa and 323 K, [bmim][Tf2N] is the solvent with the lowest energy consumption of 57.71 kJ/mol CO2. Acknowledgement We’d like to thank the Interreg IVA North programme, the County Administrative Board of Norrbotten Sate in Sweden and the Swedish research council for the financial support. References [1] Haszeldine RS. Carbon capture and storage: how green can black be? Science 2009;325:1647–52. [2] Schach MO, Schneider Rd, Schramm H, Repke JU. Techno-economic analysis of postcombustion processes for the capture of carbon dioxide from power plant flue gas. Ind Eng Chem Res 2010;49:2363–70. [3] Gough C, Upham P. Biomass energy with carbon capture and storage (BECCS or Bio-CCS). Greenhouse Gases: Sci Technol 2011;1:324–34. [4] Chen Z, Deng S, Wei H, Wang B, Huang J, Yu G. Activated carbons and amine- modified materials for carbon dioxide capture—a review. Front Environ Sci Eng 2013;7:326–40. [5] Han K, Ahn CK, Lee MS, Rhee CH, Kim JY, Chun HD. Current status and challenges of the ammonia-based CO2 capture technologies toward commercialization. Int J Greenhouse Gas Control 2013;14:270–81. [6] Hedin N, Andersson L, Bergström L, Yan J. Adsorbents for the post-combustion capture of CO2 using rapid temperature swing or vacuum swing adsorption. Appl Energy 2013;104:418–33. [7] Song CF, Kitamura Y, Li SH. Evaluation of Stirling cooler system for cryogenic CO2 capture. Appl Energy 2012;98:491–501. [8] Zhao WY, Sprachmann G, Li ZS, Cai NS, Zhang XH. Effect of K2CO31.5H2O on the regeneration energy consumption of potassium-based sorbents for CO2 capture. Appl Energy 2013;112:381–7. [9] Blanchard LA, Hancu D, Beckman EJ, Brennecke JF. Green processing using ionic liquids and CO2. Nature 1999;399:28–9. [10] Ramdin M, de Loos TW, Vlugt TJ. State-of-the-art of CO2 capture with ionic liquids. Ind Eng Chem Res 2012;51:8149–77. [11] Zhang X, Zhang X, Dong H, Zhao Z, Zhang S, Huang Y. Carbon capture with ionic liquids: overview and progress. Energy Environ Sci 2012;5:6668–81. [12] Kumar S, Cho JH, Moon I. Ionic liquid-amine blends and CO2 BOLs: prospective solvents for natural gas sweetening and CO2 capture technology—a review. Int J Greenhouse Gas Control 2014;20:87–116. [13] Shiflett MB, Drew DW, Cantini RA, Yokozeki A. Carbon dioxide capture using ionic liquid 1-Butyl-3-methylimidazolium acetate. Energy Fuels 2010;24:5781–9. [14] Shiflett MB, Kasprzak DJ, Junk CP, Yokozeki A. Phase behavior of mixtures. J Chem Thermodyn 2008;40:25–31. [15] Basha OM, Heintz YJ, Keller MJ, Luebke DR, Resnik KP, Morsi BI. Development of a conceptual process for selective capture of CO2 from fuel gas streams using two TEGO ionic liquids as physical solvents. Ind Eng Chem Res 2014;53:3184–95. [16] Basha OM, Keller MJ, Luebke DR, Resnik KP, Morsi BI. Development of a conceptual process for selective CO2 capture from fuel gas streams using [hmim][Tf2N] ionic liquid as a physical solvent. Energy Fuels 2013;27:3905–17. [17] Huang Y, Zhang X, Zhang X, Dong H, Zhang S. Thermodynamic modeling and assessment of ionic liquid-based CO2 capture processes. Ind Eng Chem Res 2014;53:11805–17. [18] Zhang Y, Que H, Chen CC. Thermodynamic modeling for CO2 absorption in aqueous MEA solution with electrolyte NRTL model. Fluid Phase Equilib 2011;311:67–75. [19] Zhang Y, Chen CC. Thermodynamic modeling for CO2 absorption in aqueous MDEA solution with electrolyte NRTL model. Ind Eng Chem Res 2010;50:163–75. [20] Yan Y, Chen CC. Thermodynamic modeling of CO2 solubility in aqueous solutions of NaCl and Na2SO4. J Supercrit Fluids 2010;55:623–34.PDF Image | CO2 Separation with Ionic Liquids
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