Journal of Thermal Analysis and Calorimetry

, Volume 138, Issue 3, pp 2275–2282 | Cite as

The peculiarities of mayenite formation from synthetic katoite and calcium monocarboaluminate samples in temperature range 25–1150 °C

  • A. Eisinas
  • T. Dambrauskas
  • K. BaltakysEmail author
  • K. Ruginyte


In this work, the formation and thermal stability of mayenite by using two-step synthesis in a 25–1150 °C temperature range was examined. It should be indicated that, within 1 h of hydrothermal treatment (130 °C; CaO/Al2O3 = 1.714, w/s = 10), katoite and calcium monocarboaluminate were obtained. Meanwhile, the largest quantity of the latter compound was formed already after 4 h of isothermal curing. In the next stage of this work, the calcination of synthesis products was performed. It was observed that after 1 h of thermal treatment at 150 °C temperature, the crystal structure of calcium monocarboaluminate was destroyed and at a slightly higher temperature (240 °C), gibbsite was fully decomposed. Also, peaks of other calcium carbonate forms, aragonite, were observed. It should be indicated that katoite recrystallized to mayenite at 310 °C. The results of in situ XRD experiment showed that, when the temperature of calcination was increased to 600 °C, aragonite became metastable and started to recrystallize to calcite, which fully decomposed to calcium oxide at 900 °C. Besides, the intensity of diffraction maximums typical to mayenite increased in 850–1150 °C temperature range.


Mayenite Hydrothermal synthesis Calcination Calcium monocarboaluminate 



This research is funded by the European Social Fund under the No 09.3.3-LMT-K-712 “Development of Competences of Scientists, other Researchers and Students through Practical Research Activities” measure.


  1. 1.
    Rouchon L, Favergeon L, Pijolat M. Analysis of the kinetic slowing down during carbonation of CaO by CO2. J Therm Anal Calorim. 2013;113:1145–55.CrossRefGoogle Scholar
  2. 2.
    Decoupling of global emissions and economic growth confirmed. International Energy Agency (IEA). 16 March 2016 Paris. Accessed 21 April 2016.
  3. 3.
    Manovic V, Anthony EJ. CaO-based pellets supported by calcium aluminate cements for high-temperature CO2 capture. Environ Sci Technol. 2009;43:7117–22.CrossRefGoogle Scholar
  4. 4.
    Phromprasit J, et al. Metals (Mg, Sr and Al) modified CaO based sorbent for CO2 sorption/desorption stability in fixed bed reactor for high temperature application. Chem Eng J. 2016;284:1213.CrossRefGoogle Scholar
  5. 5.
    Fujita S, et al. Oxidative destruction of hydrocarbons on Ca12Al14-xSixO33 + 0.5x (0 <= x <= 4) with radical oxygen occluded in nanopores. Catal Lett. 2006;106:139–43.CrossRefGoogle Scholar
  6. 6.
    Kim SW, Shimoyama T, Hosono H. Solvated electrons in high-temperature melts and glasses of the room-temperatures table electride[Ca24Al28O64](4+).4e. Science. 2011;333:71–4.CrossRefGoogle Scholar
  7. 7.
    Proto A, et al. A study on the catalytic hydrogenation of aldehydes using mayenite as active support for palladium. Catal Commun. 2015;68:41–5.CrossRefGoogle Scholar
  8. 8.
    Chen GH. Mechanical activation of calcium aluminate formation from CaCO3–Al2O3 mixtures. J Alloy Compd. 2006;426:279–83.CrossRefGoogle Scholar
  9. 9.
    Iftekha S, et al. Phase formation of CaAl2O4 from CaCO3–Al2O3 powder mixtures. J Eur Ceram Soc. 2008;28:747–56.CrossRefGoogle Scholar
  10. 10.
    Martavaltzi CS, Lemonidou AA. Parametric study of the CaO–Ca12Al14O33 synthesis with respect to high CO2 sorption capacity and stability on multicycle operation. Ind Eng Chem Res. 2008;43:9537–43.CrossRefGoogle Scholar
  11. 11.
    Zhang X, et al. Investigation on a novel CaO–Y2O3 sorbent for efficient CO2 mitigation. Chem Eng J. 2014;243:297–304.CrossRefGoogle Scholar
  12. 12.
    Luo C, et al. Enhanced cyclic stability of CO2 adsorption capacity of CaO-based sorbents using La2O3 or Ca12Al14O33 as additives. Korean J Chem Eng. 2011;28:1042–6.CrossRefGoogle Scholar
  13. 13.
    Koirala R, Reddy GK, Smirniotis PG. Single nozzle flame-made highly durable metal doped Ca-based sorbents for CO2 capture at high temperature. Energy Fuels. 2012;26(5):3103–9.CrossRefGoogle Scholar
  14. 14.
    Kierzkowska AM, Poulikakos LV, Broda M, Müller CR. Synthesis of calcium-based, Al2O3-stabilized sorbents for CO2 capture using a co-precipitation technique. Int J Greenh Gas Control. 2013;15:48–54.CrossRefGoogle Scholar
  15. 15.
    Radfarnia HR, Sayari A. A highly efficient CaO-based CO2 sorbent prepared by a citrate-assisted sol–gel technique. Chem Eng J. 2015;262:913–20.CrossRefGoogle Scholar
  16. 16.
    Angeli SD, Martavaltzi CS, Lemonidou AA. Development of a novel-synthesized Ca-based CO2 sorbent for multicycle operation: parametric study of sorption. Fuel. 2014;127:62–9.CrossRefGoogle Scholar
  17. 17.
    Jeong YJ, Balamurugan C, Lee DW. Enhanced CO2 gas-sensing performance of ZnO nanopowder by La loaded during simple hydrothermal method. Sens Actuators, B. 2016;229:288–96.CrossRefGoogle Scholar
  18. 18.
    Baltakys K, Eisinas A, Dambrauskas T. The influence of aluminum additive on the α-C2S hydrate formation process. J Therm Anal Calorim. 2015;121:75–84.CrossRefGoogle Scholar
  19. 19.
    Iljina A, et al. The stability of formed CaF2 and its influence on the thermal behavior of C-S–H in CaO–silica gel waste-H2O system. J Therm Anal Calorim. 2017;127:221–8.CrossRefGoogle Scholar
  20. 20.
    Meller N, Kyritsis K, Hall C. The mineralogy of the CaO–Al2O3–SiO2–H2O (CASH) hydroceramic system from 200 to 350 & #xB0;C. Cem Concr Res. 2009;39:45–53.CrossRefGoogle Scholar
  21. 21.
    Baltakys K, Siauciunas R. Gyrolite formation in CaO–SiO2·nH2O–γ–Al2O3–Na2O–H2O system under hydrothermal conditions. Pol J Chem. 2007;81:103–14.Google Scholar
  22. 22.
    Chang YP, et al. Morphological and structural evolution of mesoporous calcium aluminate nanocomposites by microwave-assisted synthesis. Microporous Mesoporous Mater. 2014;183:134–42.CrossRefGoogle Scholar
  23. 23.
    Li C, Hirabayashi D, Suzuki K. Synthesis of higher surface area mayenite by hydrothermal method. Mater Res Bull. 2011;46:1307–10.CrossRefGoogle Scholar
  24. 24.
    Renaudin G, Francois M, Evrard O. Order and disorder in the lamellar hydrated tetracalcium monocarboaluminate compound. Cem Concr Res. 1999;29:63–9.CrossRefGoogle Scholar
  25. 25.
    Gabrovšek R, Vuk T, Kaučič V. The preparation and thermal behavior of calcium monocarboaluminate. Acta Chim Slov. 2008;55:942–50.Google Scholar
  26. 26.
    Francois M, Renaudin G, Evrard O. Cementitious compound with composition 3CaO.Al2O3.CaCO3.11H2O. Acta Cryst. 1998;54:1214–7.Google Scholar
  27. 27.
    Rivasmercury JM, Pena P, Aza AH, Turrillas X. Dehydration of Ca3Al2(SiO4)y(OH)4(3−y) (0 < y < 0.176) studied by neutron thermodiffractometry. J Eur Ceram Soc. 2008;28(9):1737–48.CrossRefGoogle Scholar
  28. 28.
    Eisinas A, Doneliene J, Baltakys K, Urbutis A. Hydrothermal synthesis of calcium aluminium hydrate-based adsorbent for the removal of CO2. J Therm Anal Calorim. 2018;131:537–44.CrossRefGoogle Scholar
  29. 29.
    Baltakys K, Eisinas A, Doneliene J, Dambrauskas T, Sarapajevaite G. The impact of Al2O3 amount on the synthesis of CASH samples and their influence on the early stage hydration of calcium aluminate cement. Ceram Int. 2019;45:2881–6.CrossRefGoogle Scholar

Copyright information

© Akadémiai Kiadó, Budapest, Hungary 2019

Authors and Affiliations

  • A. Eisinas
    • 1
  • T. Dambrauskas
    • 1
  • K. Baltakys
    • 1
    Email author
  • K. Ruginyte
    • 1
  1. 1.Department of Silicate TechnologyKaunas University of TechnologyKaunasLithuania

Personalised recommendations