Next Article in Journal
A Stretchable Alternating Current Electroluminescent Fiber
Previous Article in Journal
Dielectric, Piezoelectric, and Vibration Properties of the LiF-Doped (Ba0.95Ca0.05)(Ti0.93Sn0.07)O3 Lead-Free Piezoceramic Sheets
 
 
Font Type:
Arial Georgia Verdana
Font Size:
Aa Aa Aa
Line Spacing:
Column Width:
Background:
Article

Effective Capture of Carbon Dioxide Using Hydrated Sodium Carbonate Powders

1
School of Chemistry and Chemical Engineering, China Key Laboratory of Enhanced Heat Transfer and Energy Conservation of the Ministry of Education, South China University of Technology, Guangzhou 510640, Guangdong, China
2
Polymer Program, Institute of Materials Science, University of Connecticut, Storrs, CT 06269, USA
3
Department of Chemical and Biomolecular Engineering, University of Connecticut, Storrs, CT 06269, USA
4
Department of Biomedical Engineering, University of Connecticut, Storrs, CT 06269, USA
*
Authors to whom correspondence should be addressed.
Materials 2018, 11(2), 183; https://doi.org/10.3390/ma11020183
Submission received: 27 December 2017 / Revised: 19 January 2018 / Accepted: 20 January 2018 / Published: 24 January 2018

Abstract

:
The emission of CO2 has been considered a major cause of greenhouse effects and global warming. The current CO2 capture approaches have their own advantages and weaknesses. We found that free-flowing hydrated sodium carbonate (Na2CO3) powders with 30 wt % water can achieve a very high CO2 sorption capacity of 282 mg/g within 60 min and fast CO2 uptake (90% saturation uptake within 16 min). The results suggest that the alkaline solution resulting from the dissolution of partial Na2CO3 can freely attach onto the hydrated Na2CO3 particles, which provides an excellent gas–liquid interface for CO2 capture, leading to significantly enhanced CO2 sorption capacity and kinetics.

1. Introduction

Emission of CO2 is identified as the main contributor to global climate change. Reducing the levels of CO2 in the atmosphere has become a pressing issue worldwide, and capturing and sequestrating CO2 as an option to decrease levels of CO2 has been widely explored [1,2,3,4].
A number of promising materials for CO2 capture were reported [5,6,7,8,9,10]. The best developed are probably aqueous amines [11,12], including monoethanolamine (MEA) [13,14] and diethanolamine (DEA) [15,16]. However, liquid amines have some serious disadvantages, including amine evaporation [17,18], corrosion to equipment [19], and high energy cost for regeneration [20,21]. A feasible way to reduce the corrosivity and the regeneration energy is to use supported amine adsorbents [22,23,24,25,26], but the raw materials are currently too expensive to be applied in large-scale industrial settings [27].
As an alternative to supported amine sorbents, alkali metal carbonates such as K2CO3 and Na2CO3 as solid sorbents have received wide attention with both high sorption capacity and low cost [28,29,30,31,32]. However, the main problem of using carbonates is their slow reaction kinetics [33,34,35]. Cooper and co-workers reported that dry K2CO3 solution (K2CO3 aqueous solution coated with hydrophobic silica powders) exhibited significantly increased CO2 uptakes [36], but the recyclability of this sorbent was poor. It has been generally accepted that K2CO3 is superior to Na2CO3 in terms of both CO2 uptake capacity and kinetics [37,38,39]. However, using Na2CO3 will be more competitive for large-scale industrial applications because of its lower cost, especially if one can dramatically promote the rate of the key reaction:
Na2CO3 + H2O + CO2 ⇌ 2NaHCO3
One of the most common approaches to tackle this problem is to disperse Na2CO3 powders on solid supports [40,41], but such a strategy also reduces CO2 sorption capacity because the inclusion of the supports greatly decreases the amount of active components per unit mass [42].
In this report, we demonstrate that support-free hydrated sodium carbonate powders (HSCPs) prepared by simply mixing a certain amount of water and Na2CO3 powders exhibit effective CO2 capture. The alkaline solution resulting from the dissolution of partial Na2CO3 can freely attach into hydrated Na2CO3 particles, which provides an excellent gas–liquid interface for CO2 capture, leading to significantly enhanced CO2 sorption capacity and kinetics. The elimination of supports not only reduces the overall cost of raw materials, but also increases the CO2 sorption capacity, both of which are critical for large-scale applications.

2. Experimental

2.1. Preparation of HSCPs

Na2CO3 (99.8%) was purchased from Tianjin Qilun Chemical Technology Co. Ltd., Tianjin, China. Na2CO3·H2O (99%) was purchased from Aladdin Co. Ltd., Shanghai, China. MEA (99%) was purchased from Jiangsu Yonghua Chemical Technology Co. Ltd., Changshu, China. CO2 (99.9%) was supplied by Zhuozheng Gas Co. Ltd., Guangzhou, China. All the chemicals were used as received without further purification. A series of HSCPs with different Na2CO3 contents were prepared by thoroughly mixing an appropriate amount of Na2CO3 and deionized water at room temperature.

2.2. Characterization

X-ray diffraction (XRD) patterns of the samples were recorded using a Bruker D8 diffractometer (Bruker, Karlsruhe, Germany) with Bragg–Brentano θ−2θ geometry (20 kV and 5 mA), using a graphite monochromator with Cu Kα radiation.
To measure the CO2 capture capacity of the HSCP samples, 5.0 g HSCP was charged into a 50 mL container, which was exposed to CO2 using a balloon containing a sufficient amount of CO2 gas (ca. 5 L with a pressure of ca. 1.05 bar). The amount of CO2 captured by each HSCP sample was measured using a balance. A muffle furnace (Luoyang BSK Electronic Materials Co. Ltd., Luoyang, China) was used to regenerate the sorbents at 250 °C for 1 h, which was mixed with water to reform HSCPs.

3. Results and Discussion

Figure 1a shows the CO2 uptake kinetic curves using various HSCPs (labelled as HSCP-X, where X is the mass percentage of Na2CO3 in the mixture) as a sorbent at 30 °C. It was found that HSCP-10 to HSCP-60 had a very low CO2 sorption capacity (<32 mg/g of HSCP). The CO2 uptake capacity rapidly rose to 156 mg/g when the mass fraction of Na2CO3 was increased to 65 wt %, i.e., HSCP-65, but it still suffered from low sorption kinetics. Further increasing mass fraction of Na2CO3 led to another significant increase in term of both sorption capacity and kinetics. At the optimum concentration of 70 wt % (i.e., HSCP-70), the CO2 uptake capacity reached 282 mg/g within 60 min, and the t90 (the time to achieve 90% of this capacity) was only 16 min. This capacity is much higher than that of other Na2CO3-based CO2 sorbents reported in the literature, which varies between 32 and 140 mg/g [43,44]. Although HSCP-75 achieved the highest capacity (286 mg/g), its CO2 sorption rate was relatively slow and t90 was about 45 min.
It was found that too high a concentration of Na2CO3 in HSCP would actually lower the CO2 uptake capacity. When the concentration of Na2CO3 in HSCP reached 80 and 85 wt %, the CO2 uptake capacity decreased to 124 and 46 mg/g, respectively. Theoretically, the CO2 sorption capacity is directly related to the amount of Na2CO3 in HSCPs when the content of water is more than 14.5 wt % according to Equation (1). Thus, the conversion ratio of Na2CO3 is a good indicator of the CO2 sorption behaviour. As shown in Figure 1b, with an increasing mass fraction of Na2CO3, the conversion ratio of Na2CO3 decreased initially, then dramatically increased to a maximum value close to 100% before declining again. After 60 min of reaction, HSCP-70 exhibited the highest conversion rate (97.1%), which suggested that most of Na2CO3 was consumed. The HSCPs with a low mass fraction of Na2CO3, such as HSCP-10, also showed a high conversion ratio, in which Na2CO3 dissolved in water to form a solution, due to its high degree of hydrolysis [45]. However, their corresponding CO2 uptake capacity is low because of the limited amount of Na2CO3 presented (Figure 1a). The other two sets of data in Figure 1b represent the conversion ratios of Na2CO3 after five and 15 min of reaction. For HSCP-70, its conversion ratio increased rapidly from 5 to 15 min, but changed little from 15 to 60 min, which suggested that most of Na2CO3 was consumed within 15 min, thus showing a high reaction rate.
Overall, the above results show that the concentration of Na2CO3 in HSCPs has a great influence on CO2 capture, which can be explained by the fact that the morphology of HSCPs varies from aqueous solution and slurry, to powders with an increasing Na2CO3 concentration. At low Na2CO3 concentrations, the HSCPs exist as an aqueous solution or slurry as shown in Figure 1b (inset), which is not ideal for CO2 capture because of the low gas–liquid contact surface area. However, HSCP-70 is a sample of free-flowing powders (Figure 2) with a much higher gas–liquid contact surface area. This is why it has a rapid reaction rate and a high CO2 uptake capacity.
In order to better understand the mechanism of CO2 sorption by HSCPs, the XRD patterns (Figure 3) of various Na2CO3-based compounds were collected, including the reaction products of HSCP-70 after 0, 5, 15, and 60 min of sorption reaction at 30 °C. The XRD pattern of HSCP-70 was very close to the standard pattern of Na2CO3·H2O, which contains only 14.5 wt % water. This indicates that HSCP-70 contains extra water. As such, we also studied the CO2 sorption by pure Na2CO3·H2O, but it exhibited a low CO2 sorption capacity and rate (Figure 4). This suggests that the extra water contained in the sorbent plays a significant role in CO2 sorption. It indicates that the reaction proceeds most rapidly and effectively when Na2CO3, H2O, and CO2 are present simultaneously. Based on the above results, we propose that the extra water on the surface of HSCPs helps to form a basic alkaline aqueous environment. When CO2 diffuses to the surface of HSCPs, it reacts with the basic aqueous media. Since the reaction is exothermic, the generated heat triggers the decomposition of sodium carbonate hydrates, meanwhile releasing water to drive the reaction to proceed continuously. In addition, along the reaction of HSCP-70 and CO2, we also found that the characteristic peaks of Na2CO3 disappeared gradually, then intermediate structures, such as Na3H(CO3)2·2H2O (i.e., Na2CO3·NaHCO3·2H2O) and Na2CO3·3NaHCO3, appeared after reacting for five and 15 min, respectively. Eventually, virtually pure NaHCO3 formed after 60 min of reaction, which is expected.
The amine-based CO2 capture system is a proven technology that is already commercialized. To prevent excessive corrosion, typically 30 wt % MEA aqueous solution is used [11]. As shown in Figure 4, a 30 wt % MEA aqueous solution showed similar CO2 uptake kinetics initially, but its overall sorption capacity was relatively low (111 mg/g versus 282 mg/g for HSCP-70). We also studied the CO2 sorption capacity of pure water as a control, whose CO2 uptake capacity was ca. 0.7 mg/g (Figure 4).
We also studied the CO2 uptake kinetics at different temperatures and the recyclability of HSCP-70. The suitable temperature range for CO2 capture was determined to be 30–50 °C (Figure 5). A higher temperature will cause excessive evaporation of water in HSCP-70, and a lower temperature will cause the formation of Na2CO3·7H2O (as shown in Figure 6), both of which lead to a lower CO2 uptake of HSCP-70. HSCP-70 also exhibited excellent recyclability with little deterioration in CO2 sorption capacity and reaction rate after recycling (Figure 7).

4. Conclusions

In summary, we have demonstrated that support-free HSCPs can be used as effective sorbents for CO2 capture with a high capacity (282 mg/g) and fast sorption rate (90% saturation uptake within 16 min). The elimination of support and the low cost of Na2CO3 make this technology more competitive for large-scale applications. In addition, based on the reaction principles, HSCPs should also have high potential in capturing other acid gases, including SOx, NOx, H2S, and Cl2.

Acknowledgments

This research is sponsored by the National Natural Science Foundation of China (21176093 and 21676107). L.S. acknowledges the partial support by the Air Force Office of Scientific Research (Grant FA9550-12-1-0159). The authors acknowledge Pinzhen Lin, Haoxin Huang, and Zhuyan Tan for their assistance for this research.

Author Contributions

Weixing Wang and Luyi Sun conceived and designed the experiments. Yuanhao Cai, Liang Li, Weilin Wang, Suying Wang, and Hao Ding performed the experiments and/or analyzed the data. Zhaofeng Wang, Zhengguo Zhang, and Hao Ding discussed the experiments and data. Weixing Wang, Luyi Sun, Yuanhao Cai, Weilin Wang, Zhaofeng Wang, and Hao Ding wrote the manuscript. All authors discussed the results and commented on the manuscript.

Conflicts of Interest

The authors declare no conflict of interest.

References

  1. Bender, M.L.; Ho, D.T.; Hendricks, M.B.; Mika, R.; Battle, M.O.; Tans, P.P.; Conway, T.J.; Sturtevant, B.; Cassar, N. Atmospheric O2/N2 changes, 1993–2002: Implications for the partitioning of fossil fuel CO2 sequestration. Glob. Biogeochem. Cycles 2008, 19, 4057–4061. [Google Scholar]
  2. Rubin, E.S.; Chen, C.; Rao, A.B. Cost and performance of fossil fuel power plants with CO2 capture and storage. Energy Policy 2007, 35, 4444–4454. [Google Scholar] [CrossRef]
  3. Wolsky, A.M.; Daniels, E.J.; Jody, B.J. CO2 capture from the flue gas of conventional fossil-fuel-fired power plants. Environ. Prog. Sustain. Energy 1994, 13, 214–219. [Google Scholar] [CrossRef]
  4. Wang, W.; Ma, C.; Lin, P.; Sun, L.; Cooper, A.I. Gas storage in renewable bioclathrates. Energy Environ. Sci. 2012, 6, 105–107. [Google Scholar] [CrossRef]
  5. Cullinane, J.T.; Rochelle, G.T. Carbon dioxide absorption with aqueous potassium carbonate promoted by piperazine. Chem. Eng. Sci. 2004, 59, 3619–3630. [Google Scholar] [CrossRef]
  6. Macdowell, N.; Florin, N.; Buchard, A.; Hallett, J.; Galindo, A.; Jackson, G.; Adjiman, C.S.; Williams, C.K.; Shah, N.; Fennell, P. An overview of CO2 capture technologies. Energy Environ. Sci. 2010, 3, 1645–1669. [Google Scholar] [CrossRef] [Green Version]
  7. Drage, T.C.; Snape, C.E.; Stevens, L.A.; Wood, J.; Wang, J.; Cooper, A.I.; Dawson, R.; Guo, X.; Satterley, C.; Irons, R. Materials challenges for the development of solid sorbents for post-combustion carbon capture. J. Mater. Chem. 2011, 22, 2815–2823. [Google Scholar] [CrossRef]
  8. Goeppert, A.; Czaun, M.; Prakash, G.K.S.; Olah, G.A. ChemInform Abstract: Air as the Renewable Carbon Source of the Future: An Overview of CO2 Capture from the Atmosphere. Energy Environ. Sci. 2012, 44, 7833–7853. [Google Scholar] [CrossRef]
  9. Xu, Y.; Zhou, Y.; Liu, J.; Sun, L. Coassembled Ionic Liquid/Laponite Hybrids as Effective CO2 Adsorbents. J. Energy Chem. 2017, 26, 1026–1029. [Google Scholar] [CrossRef]
  10. Zhou, Y.; Liu, J.; Min, X.; Meng, Y.; Sun, L. Designing Supported Ionic Liquids (ILs) within Inorganic Nanosheets for CO2 Capture Applications. ACS Appl. Mater. Interfaces 2016, 8, 5547–5555. [Google Scholar] [CrossRef] [PubMed]
  11. Rochelle, G.T. Amine scrubbing for CO2 capture. Science 2009, 325, 1652–1654. [Google Scholar] [CrossRef] [PubMed]
  12. Rao, A.B.; Rubin, E.S. A technical, economic, and environmental assessment of amine-based CO2 capture technology for power plant greenhouse gas control. Environ. Sci. Technol. 2002, 36, 4467–4475. [Google Scholar] [CrossRef] [PubMed]
  13. Alie, C.; Backham, L.; Croiset, E.; Douglas, P.L. Simulation of CO2 capture using MEA scrubbing: A flowsheet decomposition method. Energy Convers. Manag. 2005, 46, 475–487. [Google Scholar] [CrossRef]
  14. And, I.J.U.; Idem, R.O. Studies of SO2 and O2-Induced Degradation of Aqueous MEA during CO2 Capture from Power Plant Flue Gas Streams. Ind. Eng. Chem. Res. 2007, 46, 2558–2566. [Google Scholar]
  15. Wang, R.; Li, D.F.; Zhou, C.; Liu, M.; Liang, D.T. Impact of DEA solutions with and without CO2 loading on porous polypropylene membranes intended for use as contactors. J. Membr. Sci. 2004, 229, 147–157. [Google Scholar] [CrossRef]
  16. Filburn, T.; And, J.J.H.; Weiss, R.A. Development of Supported Ethanolamines and Modified Ethanolamines for CO2 Capture. Ind. Eng. Chem. Res. 2005, 44, 1542–1546. [Google Scholar] [CrossRef]
  17. Hasib-Ur-Rahman, M.; Siaj, M.; Larachi, F. Ionic liquids for CO2 capture—Development and progress. Chem. Eng. Process. 2010, 49, 313–322. [Google Scholar] [CrossRef]
  18. Aparicio, S.; Atilhan, M. A computational study on choline benzoate and choline salicylate ionic liquids in the pure state and after CO2 adsorption. J. Phys. Chem. B 2012, 116, 9171–9185. [Google Scholar] [CrossRef] [PubMed]
  19. Aaron, D.; Tsouris, C. Separation of CO2 from Flue Gas: A Review. Sep. Sci. Technol. 2011, 40, 321–348. [Google Scholar] [CrossRef]
  20. Duke, M.C.; Ladewig, B.; Smart, S.; Rudolph, V.; Costa, J.C.D.D. Assessment of postcombustion carbon capture technologies for power generation. Front Chem. Sci. Eng. 2010, 4, 184–195. [Google Scholar] [CrossRef]
  21. Tuwati, A.; Fan, M.; Russell, A.G.; Wang, J.; Dacosta, H.F. New CO2 Sorbent Synthesized with Nanoporous TiO(OH)2 and K2CO3. Energy Fuels 2013, 27, 7628–7636. [Google Scholar] [CrossRef]
  22. Khatri, R.A.; Chuang, S.S.; Soong, Y.; Gray, M. Thermal and chemical stability of regenerable solid amine sorbent for CO2 capture. Energy Fuels 2006, 20, 1514–1520. [Google Scholar] [CrossRef]
  23. Chen, C.; Yang, S.T.; Ahn, W.S.; Ryoo, R. Amine-impregnated silica monolith with a hierarchical pore structure: Enhancement of CO2 capture capacity. Chem. Commun. 2009, 24, 3627–3629. [Google Scholar] [CrossRef] [PubMed]
  24. Bollini, P.; Didas, S.A.; Jones, C.W. Amine-oxide hybrid materials for acid gas separations. J. Mater. Chem. 2011, 21, 15100–15120. [Google Scholar] [CrossRef]
  25. Brunelli, N.A.; Didas, S.A.; Venkatasubbaiah, K.; Jones, C.W. Tuning cooperativity by controlling the linker length of silica-supported amines in catalysis and CO2 capture. J. Am. Chem. Soc. 2012, 134, 13950–13953. [Google Scholar] [CrossRef] [PubMed]
  26. Kuwahara, Y.; Kang, D.Y.; Copeland, J.R.; Brunelli, N.A.; Didas, S.A.; Bollini, P.; Sievers, C.; Kamegawa, T.; Yamashita, H.; Jones, C.W. Dramatic enhancement of CO2 uptake by poly(ethyleneimine) using zirconosilicate supports. J. Am. Chem. Soc. 2012, 134, 10757–10760. [Google Scholar] [CrossRef] [PubMed]
  27. Xu, X.; Zhao, X.; Sun, L.; Liu, X. Adsorption separation of carbon dioxide, methane and nitrogen on monoethanol amine modified β-zeolite. J. Nat. Gas Chem. 2009, 18, 167–172. [Google Scholar] [CrossRef]
  28. Zhao, C.; Chen, X.; Zhao, C. Multiple-Cycles Behavior of K2CO3/Al2O3 for CO2 Capture in a Fluidized-Bed Reactor. Energy Fuels 2010, 24, 1009–1012. [Google Scholar] [CrossRef]
  29. Seo, Y.; Jo, S.H.; Ryu, C.K.; Yi, C.K. Effects of water vapor pretreatment time and reaction temperature on CO2 capture characteristics of a sodium-based solid sorbent in a bubbling fluidized-bed reactor. Chemosphere 2007, 69, 712–718. [Google Scholar] [CrossRef] [PubMed]
  30. Liang, Y.; Harrison, D.; Gupta, R.; Green, D.; McMichael, W. Carbon dioxide capture using dry sodium-based sorbents. Energy Fuels 2004, 18, 569–575. [Google Scholar] [CrossRef]
  31. Wang, Q.; Yu, J.; Liu, J.; Guo, Z.; Umar, A.; Sun, L. Na+ and K+-Exchanged Zirconium Phosphate (ZrP) as High-Temperature CO2 Adsorbents. Sci. Adv. Mater. 2013, 5, 469–474. [Google Scholar] [CrossRef]
  32. Borhani, T.N.G.; Azarpour, A.; Akbari, V.; Alwi, S.R.W.; Manan, Z.A. CO2 Capture with Potassium Carbonate Solutions: A State-of-the-Art Review. Int. J. Greenh. Gas Control 2015, 41, 142–162. [Google Scholar] [CrossRef]
  33. Lee, S.C.; Kim, J.C. Dry Potassium-Based Sorbents for CO2 Capture. Catal. Surv. Asia 2007, 11, 171–185. [Google Scholar] [CrossRef]
  34. Charitos, A.; Rodríguez, N.; Hawthorne, C.; Alonso, M.; Zieba, M.; Arias, B.; Kopanakis, G.; Scheffknecht, G.; Abanades, J.C. Experimental Validation of the Calcium Looping CO2 Capture Process with Two Circulating Fluidized Bed Carbonator Reactors. Ind. Eng. Chem. Res. 2011, 50, 9685–9695. [Google Scholar] [CrossRef] [Green Version]
  35. Borhani, T.N.G.; Akbari, V.; Hamid, M.K.A.; Manan, Z.A. Rate-based simulation and comparison of various promoters for CO2 capture in industrial DEA-promoted potassium carbonate absorption unit. J. Ind. Eng. Chem. 2015, 22, 306–316. [Google Scholar] [CrossRef]
  36. Dawson, R.; Stevens, L.A.; Williams, O.S.A.; Wang, W.; Carter, B.O.; Sutton, S.; Drage, T.C.; Blanc, F.; Adams, D.J.; Cooper, A.I. ‘Dry bases’: carbon dioxide capture using alkaline dry water. Energy Environ. Sci. 2014, 7, 1786–1791. [Google Scholar] [CrossRef]
  37. Lee, S.C.; Choi, B.Y.; Lee, S.J.; Jung, S.Y.; Chong, K.R.; Kim, J.C. CO2 Absorption and Regeneration using Na and K Based Sorbents. Stud. Surf. Sci. Catal. 2004, 153, 527–530. [Google Scholar]
  38. Choi, B.S. Sorption of Carbon Dioxide onto Sodium Carbonate. Sep. Sci. Technol. 2006, 41, 515–525. [Google Scholar]
  39. Park, S.W.; Sung, D.H.; Choi, B.S.; Lee, J.W.; Kumazawa, H. Carbonation kinetics of potassium carbonate by carbon dioxide. J. Ind. Eng. Chem. 2006, 12, 522–530. [Google Scholar]
  40. Dutcher, B.; Fan, M.; Leonard, B. Use of multifunctional nanoporous TiO(OH)2 for catalytic NaHCO3 decomposition-eventually for Na2CO3/NaHCO3 based CO2 separation technology. Sep. Purif. Technol. 2011, 80, 364–374. [Google Scholar] [CrossRef]
  41. Kondakindi, R.R.; Mccumber, G.; Aleksic, S.; Whittenberger, W.; Abraham, M.A. Na2CO3 -based sorbents coated on metal foil: CO2 capture performance. Int. J. Greenh. Gas Control 2013, 15, 65–69. [Google Scholar] [CrossRef]
  42. Choi, S.; Drese, J.H.; Jones, C.W. Adsorbent materials for carbon dioxide capture from large anthropogenic point sources. ChemSusChem 2009, 2, 796–854. [Google Scholar] [CrossRef] [PubMed]
  43. Lee, S.C.; Choi, B.Y.; Ryu, C.K.; Ahn, Y.S.; Lee, T.J.; Kim, J.C. The effect of water on the activation and the CO2 capture capacities of alkali metal-based sorbents. Korean J. Chem. Eng. 2006, 23, 374–379. [Google Scholar] [CrossRef]
  44. Zhao, C.; Chen, X.; Anthony, E.J.; Jiang, X.; Duan, L.; Wu, Y.; Dong, W.; Zhao, C. Capturing CO2 in flue gas from fossil fuel-fired power plants using dry regenerable alkali metal-based sorbent. Prog. Energy Combust. Sci. 2013, 39, 515–534. [Google Scholar] [CrossRef]
  45. Nakayama, F. Hydrolysis of sodium carbonate. J. Chem. Educ. 1970, 47, 67. [Google Scholar] [CrossRef]
Figure 1. (a) CO2 sorption kinetics of various HSCPs at 30 °C; (b) conversion ratio of Na2CO3 in various HSCPs and different reaction time.
Figure 1. (a) CO2 sorption kinetics of various HSCPs at 30 °C; (b) conversion ratio of Na2CO3 in various HSCPs and different reaction time.
Materials 11 00183 g001
Figure 2. Free-flowing HSCP-70 from a glass funnel.
Figure 2. Free-flowing HSCP-70 from a glass funnel.
Materials 11 00183 g002
Figure 3. XRD patterns of various Na2CO3 based compounds and the reaction products of HSCP-70 after 0, 5, 15, and 60 min of CO2 sorption reaction at 30 °C.
Figure 3. XRD patterns of various Na2CO3 based compounds and the reaction products of HSCP-70 after 0, 5, 15, and 60 min of CO2 sorption reaction at 30 °C.
Materials 11 00183 g003
Figure 4. CO2 sorption kinetics of HSCP-70, pure water, 30 wt % MEA aqueous solution, and Na2CO3·H2O at 30 °C.
Figure 4. CO2 sorption kinetics of HSCP-70, pure water, 30 wt % MEA aqueous solution, and Na2CO3·H2O at 30 °C.
Materials 11 00183 g004
Figure 5. CO2 sorption kinetics of HSCP-70 at different temperatures.
Figure 5. CO2 sorption kinetics of HSCP-70 at different temperatures.
Materials 11 00183 g005
Figure 6. XRD patterns of HSCP-70 at 10 and 30 °C.
Figure 6. XRD patterns of HSCP-70 at 10 and 30 °C.
Materials 11 00183 g006
Figure 7. Recycling performance of HSCP-70 after regeneration at 250 °C.
Figure 7. Recycling performance of HSCP-70 after regeneration at 250 °C.
Materials 11 00183 g007

Share and Cite

MDPI and ACS Style

Cai, Y.; Wang, W.; Li, L.; Wang, Z.; Wang, S.; Ding, H.; Zhang, Z.; Sun, L.; Wang, W. Effective Capture of Carbon Dioxide Using Hydrated Sodium Carbonate Powders. Materials 2018, 11, 183. https://doi.org/10.3390/ma11020183

AMA Style

Cai Y, Wang W, Li L, Wang Z, Wang S, Ding H, Zhang Z, Sun L, Wang W. Effective Capture of Carbon Dioxide Using Hydrated Sodium Carbonate Powders. Materials. 2018; 11(2):183. https://doi.org/10.3390/ma11020183

Chicago/Turabian Style

Cai, Yuanhao, Weilin Wang, Liang Li, Zhaofeng Wang, Suying Wang, Hao Ding, Zhengguo Zhang, Luyi Sun, and Weixing Wang. 2018. "Effective Capture of Carbon Dioxide Using Hydrated Sodium Carbonate Powders" Materials 11, no. 2: 183. https://doi.org/10.3390/ma11020183

Note that from the first issue of 2016, this journal uses article numbers instead of page numbers. See further details here.

Article Metrics

Back to TopTop