Submitted Successfully!
To reward your contribution, here is a gift for you: A free trial for our video production service.
Thank you for your contribution! You can also upload a video entry or images related to this topic.
Version Summary Created by Modification Content Size Created at Operation
1
Janis Krumins
 + 2349 word(s) 2349 2022-03-23 08:41:40 |
2 format correct
Conner Chen
 Meta information modification 2349 2022-03-28 08:52:16 |

Video Upload Options

Do you have a full video?
Send video materials Upload full video

Confirm

Are you sure to Delete?
Yes No
Cite
If you have any further questions, please contact Encyclopedia Editorial Office.
Krumins, J. Carbon Dioxide Capture. Encyclopedia. Available online: https://encyclopedia.pub/entry/21039 (accessed on 04 July 2024).
Krumins J. Carbon Dioxide Capture. Encyclopedia. Available at: https://encyclopedia.pub/entry/21039. Accessed July 04, 2024.
Krumins, Janis. "Carbon Dioxide Capture" Encyclopedia, https://encyclopedia.pub/entry/21039 (accessed July 04, 2024).
Krumins, J. (2022, March 25). Carbon Dioxide Capture. In Encyclopedia. https://encyclopedia.pub/entry/21039
Krumins, Janis. "Carbon Dioxide Capture." Encyclopedia. Web. 25 March, 2022.
Carbon Dioxide Capture
Edit
This entry is adapted from the peer-reviewed paper 10.3390/min12030349

Carbon capture is among the most sustainable strategies to limit carbon dioxide emissions, which account for a large share of human impact on climate change and ecosystem destruction. This growing threat calls for novel solutions to reduce emissions on an industrial level. Carbon capture by amorphous solids is among the most reasonable options as it requires less energy when compared to other techniques and has comparatively lower development and maintenance costs. In this respect, the method of carbon dioxide adsorption by solids can be used in the long-term and on an industrial scale. Furthermore, certain sorbents are reusable, which makes their use for carbon capture economically justified and acquisition of natural resources full and sustainable. Clay minerals, which are a universally available and versatile material, are amidst such sorbents. These materials are capable of interlayer and surface adsorption of carbon dioxide. In addition, their modification allows to improve carbon dioxide adsorption capabilities even more. 

carbon dioxide emissions carbon sequestration carbon capture and storage technologies

1. Technologies for Carbon Dioxide Capture and Storage

The ever-increasing atmospheric CO2 concentration calls for immediate action to reduce possibilities for global catastrophic risks to the planet and to the very existence of civilization. This is why the development of technologies for carbon capture and storage (CCS) is crucial for preserving the future and the quality of life. During the last decades, the development of CCS technologies has been studied widely and intensively to find the balance among efficiency of use, production, and maintenance costs. Notably, the advancement of technologies for carbon capture is equally as important as the new options for carbon storage.
The reduction of CO2 emissions generally relies on its separation from flue gas from the combustion reactions. The technologies for CO2 separation include six major methods, which are [1]:
  • Absorption;
  • Adsorption;
  • Calcium looping;
  • Cryogenic separation;
  • Membrane separation;
  • Biological separation with microalgae.
The CO2 absorption technologies generally can be distinguished between chemical and physical absorption. The chemical absorption is then subdivided into formulation and operation. The chemical formulation involves a CO2 reaction with single amines (derivatives of ammonia), amine blends (solutions of two or more amines in varying compositions), and caustics (strong alkaline chemicals). At the same time, chemical operation is based on the use of a chemical adsorber or stripper and rotating columns to absorb CO2, where the rotation increases the chemical reactivity and the absorption efficiency [2]. The second absorption type, physical absorption of CO2, involves the use of units with various solvents and sorbents for gas separation, such as selexol, rectisol, fluor (econamine), purisol, and others [1][3][4][5][6].
Technologies for CO2 adsorption can be distinguished between adsorbent beds and the use of regeneration cycles. The fixed-bed adsorption generally utilizes activated carbon, alumina (synthetically produced Al2O3), silica, zeolites, metal organic frameworks (MOFs), hydrotalcites, amine supported adsorbents, and polymers [1][7][8][9][10][11][12][13][14]. Regeneration cycles, in turn, involve pressure swing adsorption, temperature swing adsorption, steam, or moisture adsorption [1][15][16][17].
The calcium looping technology uses the regenerative calcium cycle, where to separate CO2 from flue gas, a metal is reversibly reacted between its carbonate form and its oxide form. Within this approach for CO2 separation, the technology basically involves a loop of calcination and carbonation to remove CO2 from flue gas [1][18].
The cryogenic technology includes a set of conventional and unconventional methods. Among these, the cryogenic distillation is amidst the most common conventional approaches. In turn, most unconventional methods involve various cryogenic fluids, heat exchangers, and cryogenic packed beds to fix CO2 [1][19][20][21].
The membrane technology is based on gas separation using specially designed membranes, for instance, a polyphenylene oxide (PPE), poly dimethyl siloxane (PDMS) membrane, or polypropylene (PP) or ceramic bed systems to fix CO2 [1][22][23][24].
The technology behind the biological CO2 separation using microalgae involves carbon bio-fixation, for example, through enzyme-catalytic hydrolysis. The idea behind microbial bio-fixation involves CO2 fixation for microalgae cell growth [1][25][26][27].
Different technologies require divergent approaches; they are also characterized by different use and maintenance costs, as well as the range of applications and scale. Currently, among main technologies used for CO2 capture is [28][29][30][31][32][33]:
  • Cryogenic distillation;
  • Membrane purification;
  • Electrochemical separation;
  • Absorption with liquids;
  • Adsorption using solid materials.
Unfortunately, most of these approaches are expensive and high-energy demanding, which therefore limit widespread use of the given technology.
The cryogenic distillation is amongst most used technologies for CO2 adsorption and gas separation [29]. It is low-temperature CO2 capture technology, which relies on phase change. The technology can be applied to a range of CO2 concentrations. Regrettably, it is high-energy demanding and expensive, and thus the use on large industrial scale cannot be economically justifiable. At the same time, this technology can be recommended for smaller-scale applications [1].
The membrane purification involves CO2 capture in polymeric membranes. The membrane purification technology requires comparatively less energy than cryogenic distillation and is also much easier to operate; however, this technique is limited to minor CO2 concentrations and thus again cannot be justified for an industrial scale use [30][34].
The electrochemical reduction of CO2 is among promising future technologies; however, there are numerous challenges for large-scale production [35]. Separation of CO2 from flue gas using electrochemical cells is complex and energy demanding process. In this context, experiments have shown that this technology can be used to separate CO2 from flue gas streams produced by coal combustion for electricity generation; however, for this to happen, elevated temperature molten carbonate electrochemical cells would be required and the presence of any kind of contaminants would impact the electrolyte within the cell and thus also the effectiveness of CO2 separation. At the same time, experiments with low-temperature cells also continue and their applications are continuously advancing, which show comparatively higher work efficiency than the high-temperature cells [36].
Yet another approach—CO2 adsorption with liquids, in general with alkylamine solution or chilled ammonia, collides with an obstacle—is a complex, expensive, and high-energy demanding technique. Moreover, evaporation of these liquids eventually causes equipment corrosion, and thus this method may not be among long-term solutions [37].
In many aspects, the CO2 adsorption using solids is among the most reasonable options as this method demands the least energy, can be used in the long-term, and some of the materials can be reused and applied on a large industrial scale. In addition, organic or inorganic sorbents are available with high selectivity in respect to CO2, high efficiency, and stability during their exploitation [33][38][39]. Use of porous solid materials, such as clays, zeolites, activated carbon, MOFs, metal oxides, layered double hydroxides (LDHs), and porous silica have shown to be very effective for selective CO2 capture [40][41][42][43][44][45][46][47][48][49][50][51][52][53][54][55]. Notably, the majority of CO2 adsorption studies have been reported in high pressure and elevated temperatures as it is known that with increasing pressure, CO2 adsorption level would also increase [56]. However, in regard to GHG removal from the atmosphere, CO2 adsorption at atmospheric pressure also has to be accounted for, and therefore it is crucial to expand on this topic in further studies [57].
The most common technologies for CO2 capture from large stationary sources are generally based on a selective CO2 absorption using aqueous solutions of amines, such as monoethanolamine (MEA), diethanolamine (DEA), N-methyldiethanolamine (MDEA), diglycol-amine (DGA), and 2-amino-2-methyl-1-propanol (AMP) [58]. Regrettably, such an approach has several disadvantages over other equivalent solutions for carbon capture; for example, some known disadvantages are equipment corrosion or loss of amines due to evaporation. Moreover, solvent regeneration requires high energy consumption, and thus alternative approaches that are less energy demanding are necessary. In fact, this necessity has promoted the development of new strategies for CO2 capture that also involve the development of new appropriate solid material sorbents based on cheap substances, for instance, on clay minerals.

2. Materials for Carbon Dioxide Capture Technologies

It is reasonable to consider that several groups of sorbents, both representing solid and liquid phase materials, are suggested for the development of the CCS technologies due to their high efficiency and selectivity to CO2 capture, long-term applicability, and economic justifiability. In this regard, the materials with high potential for CO2 capture include a variety of porous materials and liquids of both natural and artificial origin, such as [59][60][61][62][63]:
  • Metal organic frameworks (MOFs);
  • Graphene organic frameworks (GOFs);
  • Covalent organic frameworks (COFs);
  • Metal oxides;
  • Homogenous porous silica;
  • Zeolites;
  • Activated carbon;
  • Clay minerals;
  • Molecular basket sorbents (MBSs);
  • Ionic liquids.
It has been reported that MOFs and GOFs form three-dimensional structures with narrow and homogenous pore size distribution, and this allows reversible retention of CO2 molecules [59][60][61][64][65]. A number of MOFs with designed pore and channel size and large surface area are viewed as materials for CO2 sorption and storage [32][66].While MOFs and GOFs show significant advantages in gas selectivity and separation in comparison to traditional adsorbents, the main disadvantages of these structures, however, are their relatively low thermal and hydrolytic stability, which are crucial for adsorbent regeneration and low yields. Yet another obstacle is the excessive cost, which is required to prepare these materials on a large industrial scale [59]. At the same time, properties of MOFs can be further improved by several means [67][68]. The main improvements that can be made to MOF composites are increased porosity and sorption capacity, as well as improved special functionality. Moreover, numerous structural modifications and improved kinetics in the synthesis of MOFs can be made, that all together can significantly improve their effectiveness towards CO2 sorption [69].
Other structures—COFs—are an equal alternative to MOFs and GOFs, as they can be either two- or three-dimensional highly porous organic solids, and they have already been used in the photocatalytic and electrocatalytic systems for large scale CO2 conversion to CO. However, such photocatalytic systems have poor overall CO2 selectivity and low effectiveness for CO2 adsorption [70][71][72][73][74][75]. Moreover, COF applications on an industrial scale are hampered by their low stability in the presence of water [76][77]. Simultaneously, studies show an effective CO2 adsorption on numerous metal oxides, such as Fe2O3, TiO2, ZrO2, or Al2O3 in the temperature below 0 °C, but unfortunately, the high energy support to maintain the required temperature is high, making this approach high-energy demanding [78]. Notably, the use of such solids as CaO, MgO, or mixed oxides coming from hydrotalcites generally is of low cost; they are highly available and have high overall capacity to capture CO2. However, use of these oxides is affected by the same complications as other metal oxides [79].
In the last several decades, experimentation with porous silica in regard to CO2 adsorption has been carried out. Experiments with porous silica with different textural parameters such as mesocellular foams—MCM-41, MCM-48, SBA-15, hexagonal mesoporous silica, and others—have shown that CO2 capacity is directly proportional to the microporosity [79][80][81]. However, in comparison, MOFs show much better CO2 adsorption capacity than silica [50][59][80][82][83][84][85].
Zeolites and activated carbon, among all materials, reach by far the highest CO2 adsorption values. In fact, inorganic zeolites were the first porous materials to be investigated for the ability to sequester CO2; however, their production is expensive, thus alternatives with similar properties are being sought [59][86][87][88][89]. Zeolites, activated carbon, and other solid porous sorbents are capable to capture CO2 via physical and chemical adsorption mechanisms [58]. Zeolites can bind CO2 either by chemical binding or by including both chemical and physical sorption pathways.
Clay minerals are a low-cost alternative with similar CO2 adsorption capacity to zeolites and activated carbon, thus their use on an industrial scale can be economically justifiable. Clays have high pore and channel size variability, large surface area, a wide variety of structures responsible for CO2 sorption, and large void volume for carbon storage. Furthermore, clays can be chemically modified to ensure high clay-based sorbent selectivity in respect to other gasses present in flue gas, such as H2N2, O2, CH4, or CO [32][59]. For instance, Wang et al. (2013) have reported that the support material accounts for over 70% of the total capital cost for sorbent preparation. In this respect, due to the easy availability, excellent thermal and chemical stability, surface properties that can be adjusted for various properties, and low cost, clay minerals can be considered one of the most justifiable materials for CCS [90]. For example, one of the top sequesters for CO2 is the exchanged fluorohectorite clay, which belongs to the smectite group [91]. In addition, clay minerals can be used as the base material for other technologies, such as MBSs. The concept of MBS is used to denote sorbents that may selectively capture CO2 onto a functional basket. Sorbents of this type are typically prepared by immobilizing an amine-functional polymer onto a porous carrier. Recent studies point to the benefits of MBS, such as, superior sorption–desorption characteristics, high sorption capacity, selectivity towards CO2, high regeneration abilities, and high stability. In addition, MBSs have much less corrosion potential and require much lower energy consumption when compared to the conventional methods, such as amine scrubbing [92]. It is worth mentioning that, while sorption processes have been studied in high detail and general regularities are known, desorption processes are not yet fully understood. At the same time, recent studies show that CO2 desorption in natural clays and clay modification products, including MBSs, can be controlled both by pore structures and by chemically functionalized groups [93]. However, understanding which factor prevails requires further investigation. Nevertheless, it is believed that desorption can be triggered by changes in clay properties that may endure pressure or temperature change, yet further studies are required.
The last considerable group of materials with a potential for CO2 fixation are ionic liquids. These are non-volatile liquids with modifiable structure and high CO2 uptake capacity [94]. Ionic liquids have been explored in various chemical and biological applications; however, use of them comes with a number of potential weaknesses in comparison to clay minerals; this includes weak thermodynamic properties, corrosivity, and toxicity [95]. One of the least substantial options for industrial-scale carbon capture is the precipitation of calcium carbonate in underground reservoirs. Crystallization of calcium carbonate requires a liquid, such as groundwater, thus this method can be viewed within the ionic fluids. However, the crystallization is slow geological process that is sensitive to pressure and temperature changes, and thus this approach is not an effective long-term or industrial-scale solution [96]. Therefore, the use of clay minerals and clay modification to support an increased level of CO2 fixation are both justifiable and welcomed in regard to reducing GHG emissions.

References

  1. Font-Palma, C.; Cann, D.; Udemu, C. Review of cryogenic carbon capture innovations and their potential applications. C 2021, 7, 58.
  2. Lin, C.-C.; Liu, W.-T.; Tan, C.-S. Removal of carbon dioxide by absorption in a rotating packed bed. Ind. Eng. Chem. Res. 2003, 42, 2381–2386.
  3. Dave, A.; Pathak, B.; Dave, M.; Rezvani, S.; Huang, Y.; Hewitt, N. Process design of CO2 desorption from physical solvent di-methyl-ether of poly-ethylene-glycol. Mater. Sci. Energy Technol. 2020, 3, 209–2017.
  4. Yang, S.; Qian, Y.; Yang, S. Development of a full CO2 capture process based on the rectisol wash technology. Ind. Eng. Chem. Res. 2016, 55, 6186–6193.
  5. Scherffius, J.R.; Reddy, S.; Klumpyan, J.P.; Armpriester, A. Large-scale CO2 capture demonstration plant using fluor’s econamine FG Plus technology at NRG’s WA parish electric generating station. Energy Procedia 2013, 37, 6553–6561.
  6. Hochgesand, G. Rectisol and purisol. Ind. Eng. Chem. 1970, 62, 37–43.
  7. Girimonte, R.; Testa, F.; Gallo, F.; Buscieti, R.; Leone, G.; Fromisani, B. Adsorption of CO2 on amine-modified silica particles in a confined-fluidized bed. Processes 2020, 8, 1531.
  8. Auta, M.; Amat Darbis, N.D.; Mohd Din, A.T.; Harmeed, B.H. Fixed-bed column adsorption of carbon dioxide by sodium hydroxide modified activated alumina. Chem. Eng. J. 2013, 233, 80–87.
  9. Casas, N.; Schell, J.; Pini, R.; Mazzotti, M. Fixed bed adsorption of CO2/H2 mixtures on activated carbon: Experiments and modelling. Adsorption 2012, 18, 143–161.
  10. Hauchhum, L.; Mahanta, P. Carbon dioxide adsorption on zeolites and activated carbon by pressure swing adsorption in a fixed bed. Int. J. Energy Environ. Eng. 2014, 5, 349–356.
  11. Bastin, L.; Barcia, P.S.; Hurtado, E.J.; Silva, J.A.C.; Rodrigues, A.E.; Chen, B. A microporous metal−organic framework for separation of CO2/N2 and CO2/CH4 by fixed-bed adsorption. J. Phys. Chem. C 2008, 112, 1575–1581.
  12. Moreira, R.F.P.M.; Soares, J.L.; Casarin, G.L.; Rodrigues, A.E. Adsorption of CO2 on hydrotalcite-like compounds in a fixed bed. Sep. Sci. Technol. 2006, 41, 341–357.
  13. Guo, Y.; Luo, L.; Zheng, Y.; Zhu, T. Optimization of CO2 adsorption on solid-supported Amines and thermal regeneration mode comparison. ACS Omega 2020, 5, 9641–9648.
  14. Yoro, K.O.; Singo, M.; Mulopo, J.L.; Daramola, M.O. Modelling and experimental study of the CO2 adsorption behaviour of polyaspartamide as an adsorbent during post-combustion CO2 capture. Energy Procedia 2017, 114, 1643–1664.
  15. Siqueira, R.M.; Freitas, G.R.; Peixoto, H.R.; do Nascimento, J.F.; Musse, A.P.S.; Torres, A.E.B.; Azevedo, D.C.S.; Bastos-Neto, M. Carbon dioxide capture by pressure swing adsorption. Energy Procedia 2017, 114, 2182–2192.
  16. Ntiamoah, A.; Ling, J.; Xiao, P.; Webley, P.A.; Zhai, Y. CO2 capture by temperature swing adsorption: Use of hot CO2-rich gas for regeneration. Ind. Eng. Chem. Res. 2016, 55, 703–713.
  17. Elliott, J.E.; Copeland, R.J.; Leta, D.P.; McCall, P.P.; Bai, C.; DeRites, B.A. Carbon Dioxide Separation Using Adsorption with Steam Regeneration. US Patent 9504955, 29 November 2016.
  18. Dean, C.C.; Blamey, J.; Florin, N.H.; Al-Jeboori, M.J.; Fennell, P.S. The calcium looping cycle for CO2 capture from power generation, cement manufacture and hydrogen production. Chem. Eng. Res. Des. 2011, 89, 836–855.
  19. Xu, J.; He, T.; Lin, W. Experimental and theoretical study of CO2 solubility in liquid CH4/H2 mixtures at cryogenic temperatures. J. Chem. Eng. Data 2021, 66, 2844–2855.
  20. Chang, H.-M.; Chung, M.J.; Park, S.B. Cryogenic heat-exchanger design for freeze-out removal of carbon dioxide from landfill gas. J. Therm. Sci. Technol. 2009, 4, 362–371.
  21. Babar, M.; Bustam, M.A.; Maulud, A.S.; Ali, A.; Mukhtar, A.; Ullah, S. Enhanced cryogenic packed bed with optimal CO2 removal from natural gas; a joint computational and experimental approach. Cryogenics 2020, 105, 103010.
  22. Zhimin, H.; Zhigang, T.; Ataeivarjovi, E.; Dong, G.; Zhijun, Z.; Hongwei, L. Study on polydimethylsiloxane desorption membrane of CO2-dimethyl carbonate system. Energy Procedia 2017, 118, 210–215.
  23. deMontigny, D.; Tontiwachwuthikul, P.; Chakma, A. Using polypropylene and polytetrafluoroethylene membranes in a membrane contactor for CO2 absorption. J. Membr. Sci. 2006, 277, 99–107.
  24. Drioli, E.; Brunetti, A.; Barbieri, G. Ceramic membranes in carbon dioxide capture: Applications and potentialities. Adv. Sci. Technol. 2010, 72, 105–118.
  25. Widayat, W.; Suzery, M.; Satriadi, H.; Wahyudi; Philia, J. Selection and cultivation of microalgae for CO2 biofixation. IOP Conf. Ser. Mater. Sci. Eng. 2021, 1053, 012132.
  26. Xu, X.; Kentish, S.E.; Martin, G.J.O. Direct air capture of CO2 by microalgae with buoyant beads encapsulating carbonic anhydrase. ACS Sustain. Chem. Eng. 2021, 9, 9698–9706.
  27. Pierre, A.C. Enzymatic carbon dioxide capture. Int. Sch. Res. Notices 2012, 2012, 753687.
  28. Choi, S.; Dresse, J.H.; Jones, C.W. Adsorbent materials for carbon dioxide capture from large anthropogenic point sources. ChemSusChem 2009, 2, 796–854.
  29. Pellegrini, L.A.; De Guido, G.; Ingrosso, S. Thermodynamic Framework for Cryogenic Carbon Capture. Comput. Aided Chem. Eng. 2020, 48, 475–480.
  30. Shah, S.; Shah, M.; Shah, A.; Shah, M. Evolution in the membrane-based materials and comprehensive review on carbon capture and storage in industries. Emerg. Mater. 2020, 3, 33–44.
  31. Zhang, X.; Song, Z.; Gani, R.; Zhou, T. Comparative economic analysis of physical, chemical, and hybrid absorption processes for carbon capture. Ind. Eng. Chem. Res. 2020, 59, 2005–2012.
  32. Ghanbari, T.; Abnisa, F.; Daud, W.M.A.W. A review on production of metal organic frameworks (MOF) for CO2 adsorption. Sci. Total Environ. 2020, 707, 135090.
  33. Sharma, H.; Dhir, A. Capture of carbon dioxide using solid carbonaceous and non-carbonaceous adsorbents: A review. Environ. Chem. Lett. 2021, 19, 851–873.
  34. Vilarrasa-Garcia, E.; Cecilia, J.A.; Azevedo, D.C.S.; Cavalcante, C.L.; Rodriguez-Castellon, E. Evaluation of porous clay heterostructures modified with amine species as adsorbent for CO2 capture. Microporous Mesoporous Mater. 2017, 249, 25–33.
  35. Park, S.; Wijaya, D.T.; Na, J.; Lee, C.W. Towards the large-scale electrochemical reduction of carbon dioxide. Catalysts 2021, 11, 253.
  36. Pennline, H.W.; Granite, E.J.; Luebke, D.R.; Kitchin, J.R.; Landon, J.; Weiland, L.M. Separation of CO2 from flue gas using electrochemical cells. Fuel 2010, 89, 1307–1314.
  37. Rinker, E.B.; Ashour, S.S.; Sandall, O.C. Absorption of carbon dioxide into aqueous blends of diethanolamine and methyldiethanolamine. Ind. Eng. Chem. Res. 2000, 39, 4346–4356.
  38. Siegelman, R.L.; Kim, E.J.; Long, J.R. Porous materials for carbon dioxide separations. Nat. Mater. 2021, 20, 1060–1072.
  39. Osman, A.I.; Hefny, M.; Abdel Maksoud, M.I.A.; Elgarahy, A.M.; Rooney, D.W. Recent advances in carbon capture storage and utilisation technologies: A review. Environ. Chem. Lett. 2021, 19, 797–849.
  40. Siriwardane, R.V.; Shen, M.-S.; Fisher, E.P.; Poston, J.A. Adsorption of CO2 on molecular sieves and activated carbon. Energy Fuels 2001, 15, 279–284.
  41. Soares, J.L.; Moreira, R.F.P.M.; Jose, H.J.; Grande, C.A.; Rodrigues, A.E. Hydrotalcite materials for carbon dioxide adsorption at high temperatures: Characterization and diffusivity measurements. Sep. Sci. Technol. 2004, 39, 1989–2010.
  42. Millward, A.R.; Yaghi, O.M. Metal-organic frameworks with exceptionally high capacity for storage of carbon dioxide at room temperature. J. Am. Chem. Soc. 2005, 127, 17998–17999.
  43. Walton, K.S.; Abney, M.B.; LeVan, M.D. CO2 adsorption in Y and X zeolites modified by alkali metal cation exchange. Microporous Mesoporous Mater. 2006, 91, 78–84.
  44. Bae, Y.-S.; Mulfort, K.L.; Frost, H.; Ryan, P.; Punnathanam, S.; Broadbelt, L.J.; Hupp, J.T.; Snurr, R.Q. Separation of CO2 from CH4 using mixed-ligand metal-organic frameworks. Langmuir 2008, 24, 8592–8598.
  45. Martavaltzi, C.S.; Lemonidou, A.A. Development of new CaO based sorbent materials for CO2 removal at high temperature. Microporous Mesoporous Mater. 2008, 110, 119–127.
  46. Shao, W.; Zhang, L.; Li, L. Adsorption of CO2 and N2 on synthesized NaY zeolite at high temperatures. Adsorption 2009, 15, 497.
  47. Huang, C.-M.; Hsu, H.-W.; Liu, W.-H.; Cheng, J.-Y.; Chen, W.-C.; Wen, T.-W.; Chen, W. Development of post-combustion CO2 capture with CaO/CaCO3 looping in a bench scale plant. Energy Procedia 2011, 4, 1268–1275.
  48. Bezzera, D.P.; da Silva, F.W.M.; de Moura, P.A.S.; Sousa, A.G.S.; Vieira, R.S.; Rodriguez-Castellon, E.; Azevedo, D.C.S. CO2 adsorption in amine-grafted zeolite 13X. Appl. Surf. Sci. 2014, 314, 314–321.
  49. Loganathan, S.; Tikmani, M.; Edubilli, S.; Mishra, A.; Ghoshal, A.K. CO2 adsorption kinetics on mesoporous silica under wide range of pressure and temperature. Chem. Eng. J. 2014, 256, 1–8.
  50. Pera-Titus, M. Porous Inorganic Membranes for CO2 Capture: Present and Prospects. Chem. Rev. 2014, 114, 1413–1492.
  51. Bhatta, L.K.G.; Subramanyam, S.; Chengala, M.D.; Olivera, S.; Venkatesh, K. Progress in hydrotalcite like compounds and metal-based oxides for CO2 capture: A review. J. Clean. Prod. 2015, 103, 171–196.
  52. Chang, S.-C.; Chien, S.-Y.; Chen, C.-L.; Chen, C.-K. Analysing adsorption characteristics of CO2, N2 and H2O in MCM-41 silica by molecular simulation. Appl. Surf. Sci. 2015, 331, 225–233.
  53. Montagnaro, F.; Silvestre-Albero, A.; Silvestre-Albero, J.; Rodriguez-Reinoso, F.; Erto, A.; Lancia, A.; Balsamo, M. Post-combustion CO2 adsorption on activated carbons with different textural properties. Microporous Mesoporous Mater. 2015, 209, 157–164.
  54. Vilarrasa-Garcia, E.; Cecilia, J.A.; Santos, S.M.L.; Cavalcante, C.L.; Jimenez-Jimenez, J.; Azevedo, D.C.S.; Rodriguez-Castellon, E. CO2 adsorption on APTES functionalized mesocellular foams obtained from mesoporous silicas. Microporous Mesoporous Mater. 2014, 187, 125–134.
  55. Vilarrasa-Garcia, E.; Moya, E.M.O.; Cecilia, J.A.; Cavalcante, C.L.; Jimenez-Jimenez, J.; Azevedo, D.C.S.; Rodriguez-Castellon, E. CO2 adsorption on amine modified mesoporous silicas: Effect of the progressive disorder of the honeycomb arrangement. Microporous Mesoporous Mater. 2015, 209, 172–183.
  56. Wang, Q.; Huang, L. Molecular insight into competitive adsorption of methane and carbon dioxide in montmorillonite: Effect of clay structure and water content. Fuel 2019, 239, 32–43.
  57. Stanly, S.; Jelmy, E.J.; Nair, C.P.R.; John, H. Carbon dioxide adsorption studies on modified montmorillonite clay/reduced graphene oxide hybrids at low pressure. J. Environ. Chem. Eng. 2019, 7, 103344.
  58. Samanta, A.; Zhao, A.; Shimizu, G.K.H.; Sarkar, P.; Gupta, R. Post-Combustion CO2 capture using solid sorbents: A Review. Ind. Eng. Chem. Res. 2012, 51, 1438–1463.
  59. Chouikhi, N.; Cecilia, J.A.; Vilarrasa-Garcia, E.; Besghaier, S.; Chlendi, M.; Duro, F.I.F.; Castellon, R.R.; Bagane, M. CO2 adsorption of materials synthesized from clay minerals: A review. Minerals 2019, 9, 514.
  60. Luedtke, Z.; Aro, M.; Sun, Z.; Toan, S. Carbon Capture Materials and Technologies: A Review. Cur. Res. Mater. Chem. 2021, 3, 108.
  61. Aniruddha, R.; Sreedhar, I.; Reddy, B.M. MOFs in carbon capture: Past, present and future. J. CO2 Util. 2020, 42, 101297.
  62. Mutch, G.A.; Shulda, S.; McCue, A.J.; Menart, M.J.; Ciobanu, C.V.; Ngo, C.; Anderson, J.A.; Richards, R.M.; Vega-Maza, D. Carbon capture by metal oxides: Unleashing the potential of the (111) facet. J. Am. Chem. Soc. 2018, 140, 4736–4742.
  63. 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, 6668–6681.
  64. Sumida, K.; Rogow, D.L.; Mason, J.A.; McDonald, T.M.; Bloch, E.D.; Herm, Z.R.; Bae, T.H.; Long, J.R. Carbon dioxide capture in metal-organic frameworks. Chem. Rev. 2012, 112, 724–781.
  65. Haque, E.; Islam, M.; Pourazadi, E.; Sarkar, S.; Harris, A.T.; Minett, A.I.; Yanmaz, E.; Alshehri, S.M.; Ide, Y.; Wu, K.C.-W.; et al. Boron functionalized graphene oxide-organic frameworks for highly efficient CO2 capture. Chem. Asian J. 2017, 12, 283–288.
  66. Elhenawy, S.E.M.; Khraisheh, M.; AlMomani, F.; Walker, G. Metal-organic frameworks as a platform for CO2 capture and chemical processes: Adsorption, membrane separation, catalytic-conversion, and electrochemical reduction of CO2. Catalysts 2020, 10, 1293.
  67. Wang, W.; Xiao, J.; Wei, X.; Ding, J.; Wang, X.; Song, C. Development of a new clay supported polyethyleneimine composite for CO2 capture. Appl. Energy 2014, 113, 334–341.
  68. Yang, L.; Zeng, X.; Wang, W.; Cao, D. Recent progress in MOF-derived, heteroatom-doped porous carbons as highly efficient electrocatalysts for oxygen reduction reaction in fuel cells. Adv. Funct. Mat. 2018, 28, 1704537.
  69. Ahmed, I.; Jhung, S.H. Composites of metal–organic frameworks: Preparation and application in adsorption. Mater. Today 2014, 17, 136–146.
  70. Inoue, T.; Fujishima, A.; Konishi, S.; Honda, K. Photo electrocatalytic reduction of carbon dioxide in aqueous suspensions of semiconductor powders. Nature 1979, 277, 637–638.
  71. Wang, S.; Yao, W.; Lin, J.; Ding, Z.; Wang, X. Cobalt imidazolate metal–organic frameworks photosplit CO2 under mild reaction conditions. Angew. Chem. Int. Ed. 2013, 23, 1034–1038.
  72. White, J.L.; Baruch, M.F.; Pander, J.E.; Hu, Y.; Fortmeyer, I.C.; Park, J.E.; Zhang, T.; Liao, K.; Gu, J.; Yan, Y.; et al. Light-driven heterogeneous reduction of carbon dioxide: Photocatalysts and photoelectrodes. Chem. Rev. 2015, 115, 12888–12935.
  73. Wang, S.; Wang, X. Imidazolium ionic liquids, imidazolylidene heterocyclic carbenes, and zeolitic imidazolate frameworks for CO2 capture and photochemical reduction. Angew. Chem. Int. Ed. 2016, 55, 2308–2320.
  74. Lanni, L.M.; Tilford, R.W.; Bharathy, M.; Lavigne, J.J. Enhanced hydrolytic stability of self-assembling alkylated two-dimensional covalent organic frameworks. J. Am. Chem. Soc. 2011, 133, 13975–13983.
  75. Uribe-Romo, F.J.; Doonan, C.J.; Furukawa, H.; Oisaki, K.; Yaghi, O.M. Crystalline covalent organic frameworks with hydrazone linkages. J. Am. Chem. Soc. 2011, 133, 11478–11481.
  76. Li, H.; Li, H.; Dai, Q.; Li, H.; Brédas, J.-L. Hydrolytic stability of boronate ester-linked covalent organic frameworks. Adv. Theory Sim. 2018, 1, 1700015.
  77. Zhang, B.; Wei, M.; Mao, H.; Pei, X.; Alshmimri, S.A.; Reimer, J.A.; Yaghi, O.M. Crystalline dioxin-linked covalent organic frameworks from irreversible reactions. J. Am. Chem. Soc. 2018, 140, 12715–12719.
  78. Ramis, G.; Busca, G.; Lorenzelli, V. Low-temperature CO2 adsorption on metal oxides: Spectroscopic characterization of some weakly adsorbed species. Mater. Chem. Phys. 1991, 29, 425–435.
  79. Cecilia, J.A.; Vilarrasa-García, E.; Cavalcante, C.L.; Azevedo, D.C.S.; Franco, F.; Rodríguez-Castellón, E. Evaluation of two fibrous clay minerals (sepiolite and palygorskite) for CO2 Capture. J. Environ. Chem. Eng. 2018, 6, 4573–4587.
  80. Sanz-Pérez, E.S.; Arencibia, A.; Calleja, G.; San, R. Tuning the textural properties of HMS mesoporous silica. Functionalization towards CO2 adsorption. Microporous Mesoporous Mater. 2018, 260, 235–244.
  81. Gomez-Pozuelo, G.; Sanz-Perez, E.S.; Arencibia, A.; Pizarro, P.; Sanz, R.; Serrano, D.P. CO2 adsorption on amine-functionalized clays. Microporous Mesoporous Mater. 2019, 282, 38–47.
  82. Hiyoshi, N.; Yogo, K.; Yashima, T. Adsorption characteristics of carbon dioxide on organically functionalized SBA-15. Microporous Mesoporous Mater. 2005, 84, 357–365.
  83. Vilarrasa-Garcia, E.; Cecilia, J.A.; Moya, E.M.O.; Cavalcante, C.L.; Azevedo, D.C.S.; Rodriguez-Castellon, E. “Low cost” pore expanded SBA-15 functionalized with amine groups applied to CO2 adsorption. Materials 2015, 8, 2495–2513.
  84. Cecilia, J.A.; Vilarrasa-García, E.; García-Sancho, C.; Saboya, R.M.A.; Azevedo, D.C.S.; Cavalcante, C.L.; Rodríuez-Castellón, E. Functionalization of hollow silica microspheres by impregnation or grafted of amine groups for the CO2 capture. Int. J. Greenh. Gas Control 2016, 52, 344–356.
  85. Yan, X.; Zhang, L.; Zhang, Y.; Qiao, K.; Yan, Z.; Komarnemi, S. Amine-modified mesocellular silica foams for CO2 capture. Chem. Eng. J. 2011, 168, 918–924.
  86. Li, G.; Xiao, P.; Webley, P.; Zhang, J.; Singh, R.; Marshall, M. Capture of CO2 from high humidity flue gas by vacuum swing adsorption with zeolite 13X. Adsorption 2008, 14, 415–422.
  87. Merel, J.; Clausse, M.; Meurier, F. Experimental investigation on CO2 post-combustion capture by indirect thermal swing adsorption using 13X and 5A zeolites. Ind. Eng. Chem. Res. 2008, 47, 209–215.
  88. Plaza, M.G.; Pevida, C.; Arenillas, A.; Rubiera, F.; Pis, J.J. CO2 capture by adsorption with nitrogen enriched carbons. Fuel 2007, 86, 2204–2212.
  89. Pevida, C.; Plaza, M.G.; Arias, B.; Fermoso, J.; Rubiera, F.; Pis, J.J. Surface modification of activated carbons for CO2 capture. Appl. Surf. Sci. 2008, 254, 7165–7172.
  90. Peng, J.; Sun, H.; Wang, J.; Qiu, F.; Zhang, P.; Ning, W.; Zhang, D.; Li, W.; Wei, C.; Miao, S. Highly stable and recyclable sequestration of CO2 using supported melamine on layered-chain clay mineral. Appl. Mater. Interfaces 2021, 13, 10933–10941.
  91. Cavalcanti, L.P.; Kalantzopoulos, N.G.; Eckert, J.; Knudsen, K.D.; Fossum, J.O. A nano-silicate material with exceptional capacity for CO2 capture and storage at room temperature. Sci. Rep. 2018, 8, 11827.
  92. Wang, W.; Wang, X.; Song, C.; Wei, X.; Ding, J.; Xiao, J. Sulfuric acid modified bentonite as the support of tetraethylenepentamine for CO2 capture. Energy Fuels 2013, 27, 1538–1546.
  93. Teng, Y.; Liu, Z.; Xu, G.; Zhang, K. Desorption kinetics and mechanisms of CO2 on amine-based mesoporous silica materials. Energies 2017, 10, 115.
  94. Shukla, S.K.; Khokarale, S.G.; Bui, T.Q.; Mikkola, J.-P.T. Ionic liquids: Potential materials for carbon dioxide capture and utilization. Front. Mater. 2019, 6, 42.
  95. Steinruck, H.-P.; Wasserscheid, P. Ionic liquids in catalysis. Catal. Lett. 2015, 145, 380–397.
  96. DePaolo, D.J.; Cole, D.R. Geochemistry of geologic carbon sequestration: An overview. Rev. Mineral. Geochem. 2013, 77, 1–14.
More
© Text is available under the terms and conditions of the Creative Commons Attribution (CC BY) license; additional terms may apply. By using this site, you agree to the Terms and Conditions and Privacy Policy.
Upload a video for this entry
Information
Subjects: Environmental Sciences
Contributor MDPI registered users' name will be linked to their SciProfiles pages. To register with us, please refer to https://encyclopedia.pub/register :
Janis Krumins
View Times: 575
Entry Collection: Environmental Sciences
Revisions: 2 times (View History)
Update Date: 28 Mar 2022
Table of Contents
    1000/1000
    Hot Most Recent
    Video Production Service
    Feedback