Calcium looping

From Wikipedia, the free encyclopedia
Jump to: navigation, search

Calcium looping (CaL), or the regenerative calcium cycle (RCC), is a second-generation carbon capture technology. It is the most developed form of carbonate looping, where a metal (M) is reversibly reacted between its carbonate form (MCO3) and its oxide form (MO) to separate carbon dioxide from other gases coming from either power generation or an industrial plant. In the calcium looping process, the two species are calcium carbonate (CaCO3) and calcium oxide (CaO). The carbon dioxide can then be transported to a storage site, used in enhanced oil recovery or used as a chemical feedstock. Calcium oxide is often referred to as the sorbent.

Calcium looping is being developed as it is a more efficient, less toxic alternative to current post-combustion capture processes such as amine scrubbing.[1] It also has interesting potential for integration with the cement industry.[2][3]

Basic concept[edit]

CaCO_3 \leftrightharpoons CaO + CO_2 \qquad\qquad \Delta H = +178kJ/mol

There are two main steps in CaL:[4]

  • Calcination: Solid calcium carbonate is fed into a calciner, where it is heated to 850-950 °C to cause it to thermally decompose into gaseous carbon dioxide and solid calcium oxide (CaO). The almost-pure stream of CO2 is then removed and purified so that it is suitable for storage or use. This is the 'forward' reaction in the equation above.
  • Carbonation: The solid CaO is removed from the calciner and fed into the carbonator. It is cooled to approximately 650 °C and is brought into contact with a flue gas containing a low to medium concentration of CO2. The CaO and CO2 react to form CaCO3, thus reducing the CO2 concentration in the flue gas to a level suitable for emission to the atmosphere. This is the 'backward' reaction in the equation above.

Note that carbonation is calcination in reverse.

Whilst the process can be theoretically performed an infinite amount of times, the calcium oxide sorbent degrades as it is cycled.[4] For this reason, it is necessary to remove (purge) some of the sorbent from the system and replace it with fresh sorbent (often in the carbonate form). The size of the purge stream compared with the amount of sorbent going round the cycle affects the process considerably.[5]

Benefits of CaL compared with other post-combustion capture processes[edit]

Process description[edit]

CaL is usually designed using a dual fluidised bed system to ensure sufficient contact between the gas streams and the sorbent.[4][6][7][8][9] The calciner and carbonator are fluidised beds with associated process equipment for separating the gases and solids attached (such as cyclones). Calcination is an endothermic process and as such requires the application of heat to the calciner. The opposite reaction, carbonation, is exothermic and heat must be removed. Since the exothermic reaction happens at about 650 °C and the endothermic reaction at 850-950 °C, the heat from the carbonator cannot be directly used to heat the calciner.

The fluidisation of the solid bed in the carbonator is achieved by passing the flue gas through the bed. In the calciner, some of the recovered CO2 is recycled through the system.[4] Some oxygen may also be passed through the reactor if fuel is being burned in the calciner to provide energy.

Provision of energy to the calciner[edit]

Heat can be provided for the endothermic calcination step either directly or indirectly.

Direct provision of heat involves the combustion of fuel in the calciner itself (fluidised bed combustion). This is generally assumed to be done under oxy-fuel conditions; i.e. oxygen rather than air is used to burn the fuel to prevent dilution of the CO2 with nitrogen. The provision of oxygen for the combustion uses lots of electricity; other air separation processes are being developed.[10]

Indirect provision of heat to the calciner involves either:

  • Combustion of fuel outside the vessel and conduction of energy in to the vessel[11]
  • Combustion of fuel in another vessel and use of a heat transfer medium.[6]

Indirect methods are generally less efficient but do not require the provision of oxygen for combustion within the calciner to prevent dilution. The flue gas from the combustion of fuel in the indirect method could be mixed with the flue gas from the process that the CaL plant is attached to and passed through the carbonator to capture the CO2.

Recovery of energy from the carbonator[edit]

Although the heat from the carbonator is not at a high enough temperature to be used in the calciner, the high temperatures involved (>600 °C) mean that a relatively efficient Rankine cycle for generating electricity can be operated.[12]

Note that the waste heat from the market-leading amine scrubbing CO2 capture process is emitted at a maximum of 150 °C.[10] The low temperature of this heat means that it contains much less exergy and can generate much less electricity through a Rankine or organic Rankine cycle.

This electricity generation is one of the main benefits of CaL over lower-temperature post-combustion capture processes as the electricity is an extra revenue stream (or reduces costs).

Sorbent degradation[edit]

It has been shown that the activity of the sorbent reduces quite markedly in laboratory, bench-scale and pilot plant tests. This degradation has been attributed to three main mechanisms, as shown below.[4]


Calcium oxide is friable, that is, quite brittle. In fluidised beds, the calcium oxide particles can break apart upon collision with the other particles in the fluidised bed or the vessel containing it. [REF] The problem seems to be greater in pilot plant tests[13] than at a bench scale.


Sulfation is a relatively slow reaction (several hours) compared with carbonation (<10 minutes); thus it is more likely that SO2 will come into contact with CaCO3 than CaO. However, both reactions are possible, and are shown below.

Indirect sulfation:  CaO + SO_2 + 1/2 O_2 \Rightarrow CaSO_4
Direct sulfation:  CaCO_2 + SO_2 + 1/2 O_2 \Rightarrow CaSO_4 + CO_2

Because calcium sulfate has a greater molar volume than either CaO or CaCO3 a sulfated layer will form on the outside of the particle, which can prevent the uptake of CO2 by the CaO further inside the particle.[4] Furthermore, the temperature at which calcium sulfate dissociates to CaO and SO2 is relatively high, precluding sulfation's reversibility at the conditions present in CaL.

Disposal of waste sorbent[edit]

Properties of waste sorbent[edit]

After cycling several times and being removed from the calcium loop, the waste sorbent will have attrited, sulfated and become mixed with the ash from any fuel used. The amount of ash in the waste sorbent will depend on the fraction of the sorbent being removed and the ash and calorific content of the fuel. The size fraction of the sorbent is dependent on the original size fraction but also the number of cycles used and the type of limestone used.[14]

Disposal routes[edit]

Proposed disposal routes of waste sorbent include:

  • Landfill;
  • Disposal at sea;
  • Use in cement manufacture;
  • Use in flue gas desulfurisation (FGD).

The lifecycle CO2 emissions for power generation with CaL and the first three disposal techniques have been calculated.[15] Before disposal of the CaO coal power with CaL has a similar level of lifecycle emissions as amine scrubbing but with the CO2-absorbing properties of CaO CaL becomes significantly less polluting. Ocean disposal was found to be the best, but current laws relating to dumping waste at sea prevent this. Next best was use in cement manufacture, reducing emissions over an unabated coal plant by 93%.

Use in cement manufacture[edit]

Portland cement is approximately two-thirds calcium oxide by mass and its manufacture is responsible for approximately 8% of the world's CO2 emissions. 60% of this CO2 comes from the calcination of calcium carbonate as shown earlier in this article, and the other 40% from fossil fuel combustion. By replacing some or all of the calcium carbonate entering the plant with waste calcium oxide, the CO2 caused from calcination can be avoided, as well as some of the CO2 from fossil fuel combustion.

This calcium oxide could be sourced from other point sources of CO2 such as power stations, but most effort has been focussed on integrating calcium looping with Portland cement manufacture. By replacing the calciner in the cement plant with a calcium looping plant, it should be possible to capture 90% or more of the CO2 relatively inexpensively. There are alternative set-ups such as placing the calcium looping plant in the preheater section so as to make the plant as efficient as possible.

Some work has been undertaken into whether calcium looping affects the quality of the Portland cement produced, but results so far seem to suggest that the production of strength-giving phases such as alite are similar for calcium looped and non-calcium looped cement.[16]


  1. ^ Ahn, Hyungwoong; Luberti, Mauro; Liu, Zhengyi; Brandani, Stefano (August 2013). "Process configuration studies of the amine capture process for coal-fired power plants". International Journal of Greenhouse Gas Control 16: 29–40. doi:10.1016/j.ijggc.2013.03.002. 
  2. ^ Dean, C.C.; Blamey, J.; Florin, N.H.; Al-Jeboori, M.J.; Fennell, P.S. (June 2011). "The calcium looping cycle for CO2 capture from power generation, cement manufacture and hydrogen production". Chemical Engineering Research and Design 89 (6): 836–855. doi:10.1016/j.cherd.2010.10.013. 
  3. ^ Dean, Charles C.; Dugwell, Denis; Fennell, Paul S. (2011). "Investigation into potential synergy between power generation, cement manufacture and CO2 abatement using the calcium looping cycle". Energy & Environmental Science 4 (6): 2050. doi:10.1039/C1EE01282G. 
  4. ^ a b c d e f Blamey, J.; Anthony, E.J.; Wang, J.; Fennell, P.S. (April 2010). "The calcium looping cycle for large-scale CO2 capture". Progress in Energy and Combustion Science 36 (2): 260–279. doi:10.1016/j.pecs.2009.10.001. 
  5. ^ Rodriguez, N.; Alonso, M.; Grasa, G.; Abanades, J. Carlos (May 2008). "Heat requirements in a calciner of CaCO3 integrated in a CO2 capture system using CaO". Chemical Engineering Journal 138 (1-3): 148–154. doi:10.1016/j.cej.2007.06.005. 
  6. ^ a b Rodríguez, N.; Alonso, M.; Grasa, G.; Abanades, J. Carlos (15 September 2008). "Process for Capturing CO2 Arising from the Calcination of the CaCO3 Used in Cement Manufacture". Environmental Science & Technology 42 (18): 6980–6984. doi:10.1021/es800507c. 
  7. ^ Shimizu, T.; Hirama, T.; Hosoda, H.; Kitano, K.; Inagaki, M.; Tejima, K. (January 1999). "A Twin Fluid-Bed Reactor for Removal of CO2 from Combustion Processes". Chemical Engineering Research and Design 77 (1): 62–68. doi:10.1205/026387699525882. 
  8. ^ Fennell, Paul S.; Pacciani, Roberta; Dennis, John S.; Davidson, John F.; Hayhurst, Allan N. (July 2007). "The Effects of Repeated Cycles of Calcination and Carbonation on a Variety of Different Limestones, as Measured in a Hot Fluidized Bed of Sand". Energy & Fuels 21 (4): 2072–2081. doi:10.1021/ef060506o. 
  9. ^ Florin, Nicholas H.; Blamey, John; Fennell, Paul S. (19 August 2010). "Synthetic CaO-Based Sorbent for CO2 Capture from Large-Point Sources". Energy & Fuels 24 (8): 4598–4604. doi:10.1021/ef100447c. 
  10. ^ a b Boot-Handford, Matthew E.; Abanades, Juan C.; Anthony, Edward J.; Blunt, Martin J.; Brandani, Stefano; Mac Dowell, Niall; Fernández, José R.; Ferrari, Maria-Chiara; Gross, Robert; Hallett, Jason P.; Haszeldine, R. Stuart; Heptonstall, Philip; Lyngfelt, Anders; Makuch, Zen; Mangano, Enzo; Porter, Richard T. J.; Pourkashanian, Mohamed; Rochelle, Gary T.; Shah, Nilay; Yao, Joseph G.; Fennell, Paul S. (2014). "Carbon capture and storage update". Energy & Environmental Science 7 (1): 130. doi:10.1039/C3EE42350F. 
  11. ^ "Catalytic Flash Calcination (CFC) Technology". Calix Limited. Retrieved 21 March 2014. 
  12. ^ Romeo, Luis M.; Abanades, J. Carlos; Escosa, Jesús M.; Paño, Jara; Giménez, Antonio; Sánchez-Biezma, Andrés; Ballesteros, Juan C. (October 2008). "Oxyfuel carbonation/calcination cycle for low cost CO2 capture in existing power plants". Energy Conversion and Management 49 (10): 2809–2814. doi:10.1016/j.enconman.2008.03.022. 
  13. ^ Lu, Dennis Y.; Hughes, Robin W.; Anthony, Edward J. (December 2008). "Ca-based sorbent looping combustion for CO2 capture in pilot-scale dual fluidized beds". Fuel Processing Technology 89 (12): 1386–1395. doi:10.1016/j.fuproc.2008.06.011. 
  14. ^ González, Belén (May 2010). Comportiamento de CaO Como Sorbente Regenerable para la Captura de CO2 (in Spanish). Spain: Universidad de Oviedo. 
  15. ^ Hurst, Thomas F.; Cockerill, Timothy T.; Florin, Nicholas H. (2012). "Life cycle greenhouse gas assessment of a coal-fired power station with calcium looping CO2 capture and offshore geological storage". Energy & Environmental Science 5 (5): 7132. doi:10.1039/C2EE21204H. 
  16. ^ Dean, Charles.; Hills, Thomas.; Florin, Nick.; Dugwell, Denis.; Fennell, Paul S. (2013). "Integrating Calcium Looping CO2 Capture with the Manufacture of Cement". Energy Procedia 37: 7078–7090. doi:10.1016/j.egypro.2013.06.644.