Carbon dioxide pressure-temperature phase diagram
This video shows the property of carbon dioxide to go into a supercritical state with increasing temperature

Supercritical carbon dioxide (sCO
2) is a fluid state of carbon dioxide where it is held at or above its critical temperature and critical pressure.

Carbon dioxide usually behaves as a gas in air at standard temperature and pressure (STP), or as a solid called dry ice when cooled and/or pressurised sufficiently. If the temperature and pressure are both increased from STP to be at or above the critical point for carbon dioxide, it can adopt properties midway between a gas and a liquid. More specifically, it behaves as a supercritical fluid above its critical temperature (304.128 K, 30.9780 °C, 87.7604 °F)[1] and critical pressure (7.3773 MPa, 72.808 atm, 1,070.0 psi, 73.773 bar),[1] expanding to fill its container like a gas but with a density like that of a liquid.

Supercritical CO
2 is becoming an important commercial and industrial solvent due to its role in chemical extraction, in addition to its relatively low toxicity and environmental impact. The relatively low temperature of the process and the stability of CO
2 also allows compounds to be extracted with little damage or denaturing. In addition, the solubility of many extracted compounds in CO
2 varies with pressure,[2] permitting selective extractions.

Applications

Solvent

Main article: Supercritical fluid extraction

Carbon dioxide is gaining popularity among coffee manufacturers looking to move away from classic decaffeinating solvents. sCO
2 is forced through green coffee beans which are then sprayed with water at high pressure to remove the caffeine. The caffeine can then be isolated for resale (e.g., to pharmaceutical or beverage manufacturers) by passing the water through activated charcoal filters or by distillation, crystallization or reverse osmosis. Supercritical carbon dioxide is used to remove organochloride pesticides and metals from agricultural crops without adulterating the desired constituents from plant matter in the herbal supplement industry.[3]

Supercritical carbon dioxide can be used as a solvent in dry cleaning.[4]

Supercritical carbon dioxide is used as the extraction solvent for creation of essential oils and other herbal distillates.[5] Its main advantages over solvents such as hexane and acetone in this process are that it is non-flammable and does not leave toxic residue. Furthermore, separation of the reaction components from the starting material is much simpler than with traditional organic solvents. The CO
2 can evaporate into the air or be recycled by condensation into a recovery vessel. Its advantage over steam distillation is that it operates at a lower temperature, which can separate the plant waxes from the oils.[6]

In laboratories, sCO
2 is used as an extraction solvent, for example for determining total recoverable hydrocarbons from soils, sediments, fly-ash, and other media,[7] and determination of polycyclic aromatic hydrocarbons in soil and solid wastes.[8] Supercritical fluid extraction has been used in determining hydrocarbon components in water.[9]

Processes that use sCO
2 to produce micro and nano scale particles, often for pharmaceutical uses, are under development. The gas antisolvent process, rapid expansion of supercritical solutions, and supercritical antisolvent precipitation (as well as several related methods) process a variety of substances into particles.[10]

Due to its ability to selectively dissolve organic compounds and assist enzyme functioning, sCO
2 has been suggested as a potential solvent to support biological activity on Venus- or super-Earth-type planets.[11]

Manufactured products

Environmentally beneficial, low-cost substitutes for rigid thermoplastic and fired ceramic are made using sCO
2 as a chemical reagent. The sCO
2 in these processes is reacted with the alkaline components of fully hardened hydraulic cement or gypsum plaster to form various carbonates.[12] The primary byproduct is water.

sCO
2 is used in the foaming of polymers. Supercritical carbon dioxide can saturate the polymer with solvent. Upon depressurization and heating, the carbon dioxide rapidly expands, causing voids within the polymer matrix, i.e., creating a foam. Research is ongoing on microcellular foams.

An electrochemical carboxylation of a para-isobutylbenzyl chloride to ibuprofen is promoted under sCO
2.[13]

Working fluid

sCO
2 is chemically stable, reliable, low-cost, non-flammable and readily available, making it a desirable candidate working fluid for transcritical cycles.[14]

Supercritical CO2 is used as the working fluid in domestic water heat pumps. Manufactured and widely used, heat pumps are available for domestic and business heating and cooling.[14] While some of the more common domestic water heat pumps remove heat from the space in which they are located, such as a basement or garage, CO2 heat pump water heaters are typically located outside, where they remove heat from the outside air.[14]

Power generation

The unique properties of sCO
2 present advantages for closed-loop power generation and can be applied to power generation applications. Power generation systems that use traditional air Brayton and steam Rankine cycles can use sCO
2 to increase efficiency and power output.

The relatively new Allam power cycle uses sCO2 as the working fluid in combination with fuel and pure oxygen. The CO2 produced by combustion mixes with the sCO2 working fluid. A corresponding amount of pure CO2 must be removed from the process (for industrial use or sequestration). This process reduces atmospheric emissions to zero.

sCO2 promises substantial efficiency improvements. Due to its high fluid density, sCO2 enables compact and efficient turbomachinery. It can use simpler, single casing body designs while steam turbines require multiple turbine stages and associated casings, as well as additional inlet and outlet piping. The high density allows more compact, microchannel-based heat exchanger technology.[15]

For concentrated solar power, carbon dioxide critical temperature is not high enough to obtain the maximum energy conversion efficiency. Solar thermal plants are usually located in arid areas, so it is impossible to cool down the heat sink to sub-critical temperatures. Therefore, supercritical carbon dioxide blends, with higher critical temperatures, are in development to improve concentrated solar power electricity production.

Further, due to its superior thermal stability and non-flammability, direct heat exchange from high temperature sources is possible, permitting higher working fluid temperatures and therefore higher cycle efficiency. Unlike two-phase flow, the single-phase nature of sCO
2 eliminates the necessity of a heat input for phase change that is required for the water to steam conversion, thereby also eliminating associated thermal fatigue and corrosion.[16]

The use of sCO
2 presents corrosion engineering, material selection and design issues. Materials in power generation components must display resistance to damage caused by high-temperature, oxidation and creep. Candidate materials that meet these property and performance goals include incumbent alloys in power generation, such as nickel-based superalloys for turbomachinery components and austenitic stainless steels for piping. Components within sCO
2 Brayton loops suffer from corrosion and erosion, specifically erosion in turbomachinery and recuperative heat exchanger components and intergranular corrosion and pitting in the piping.[17]

Testing has been conducted on candidate Ni-based alloys, austenitic steels, ferritic steels and ceramics for corrosion resistance in sCO
2 cycles. The interest in these materials derive from their formation of protective surface oxide layers in the presence of carbon dioxide, however in most cases further evaluation of the reaction mechanics and corrosion/erosion kinetics and mechanisms is required, as none of the materials meet the necessary goals.[18][19]

In 2016, General Electric announced a sCO2-based turbine that enabled a 50% efficiency of converting heat energy to electrical energy. In it the CO2 is heated to 700 °C. It requires less compression and allows heat transfer. It reaches full power in 2 minutes, whereas steam turbines need at least 30 minutes. The prototype generated 10 MW and is approximately 10% the size of a comparable steam turbine.[20] The 10 MW US$155-million Supercritical Transformational Electric Power (STEP) pilot plant was completed in 2023 in San Antonio. It is the size of a desk and can power around 10,000 homes.[21]

Other

Work is underway to develop a sCO
2 closed-cycle gas turbine to operate at temperatures near 550 °C. This would have implications for bulk thermal and nuclear generation of electricity, because the supercritical properties of carbon dioxide at above 500 °C and 20 MPa enable thermal efficiencies approaching 45 percent. This could increase the electrical power produced per unit of fuel required by 40 percent or more. Given the volume of carbon fuels used in producing electricity, the environmental impact of cycle efficiency increases would be significant.[22]

Supercritical CO
2 is an emerging natural refrigerant, used in new, low carbon solutions for domestic heat pumps. Supercritical CO
2 heat pumps are commercially marketed in Asia. EcoCute systems from Japan, developed by Mayekawa, develop high temperature domestic water with small inputs of electric power by moving heat into the system from the surroundings.[23]

Supercritical CO
2 has been used since the 1980s to enhance recovery in mature oil fields.

"Clean coal" technologies are emerging that could combine such enhanced recovery methods with carbon sequestration. Using gasifiers instead of conventional furnaces, coal and water is reduced to hydrogen gas, carbon dioxide and ash. This hydrogen gas can be used to produce electrical power In combined cycle gas turbines, CO
2 is captured, compressed to the supercritical state and injected into geological storage, possibly into existing oil fields to improve yields.[24][25][26]

Supercritical CO
2 can be used as a working fluid for geothermal electricity generation in both enhanced geothermal systems[27][28][29][30] and sedimentary geothermal systems (so-called CO
2 Plume Geothermal).[31][32] EGS systems utilize an artificially fractured reservoir in basement rock while CPG systems utilize shallower naturally-permeable sedimentary reservoirs. Possible advantages of using CO
2 in a geologic reservoir, compared to water, include higher energy yield resulting from its lower viscosity, better chemical interaction, and permanent CO
2 storage as the reservoir must be filled with large masses of CO
2. As of 2011, the concept had not been tested in the field.[33]

Aerogel production

Supercritical carbon dioxide is used in the production of silica, carbon and metal based aerogels. For example, silicon dioxide gel is formed and then exposed to sCO
2. When the CO
2 goes supercritical, all surface tension is removed, allowing the liquid to leave the aerogel and produce nanometer sized pores.[34]

Sterilization of biomedical materials

Supercritical CO
2 is an alternative for thermal sterilization of biological materials and medical devices with combination of the additive peracetic acid (PAA). Supercritical CO
2 does not sterilize the media, because it does not kill the spores of microorganisms. Moreover, this process is gentle, as the morphology, ultrastructure and protein profiles of inactivated microbes are preserved.[35]

Cleaning

Supercritical CO
2 is used in certain industrial cleaning processes.

See also

References

  1. ^ a b Span, Roland; Wagner, Wolfgang (1996). "A New Equation of State for Carbon Dioxide Covering the Fluid Region from the Triple-Point Temperature to 1100 K at Pressures up to 800 MPa". Journal of Physical and Chemical Reference Data. 25 (6): 1509–1596. Bibcode:1996JPCRD..25.1509S. doi:10.1063/1.555991.
  2. ^ Discovery - Can Chemistry Save The World? - BBC World Service
  3. ^ Department of Pharmaceutical Analysis, Shenyang Pharmaceutical University, Shenyang 110016, China
  4. ^ Stewart, Gina (2003), Joseph M. DeSimone; William Tumas (eds.), "Dry Cleaning with Liquid Carbon Dioxide", Green Chemistry Using Liquid and SCO
    2    : 215–227
  5. ^ Aizpurua-Olaizola, Oier; Ormazabal, Markel; Vallejo, Asier; Olivares, Maitane; Navarro, Patricia; Etxebarria, Nestor; Usobiaga, Aresatz (1 January 2015). "Optimization of supercritical fluid consecutive extractions of fatty acids and polyphenols from Vitis vinifera grape wastes". Journal of Food Science. 80 (1): E101–107. doi:10.1111/1750-3841.12715. ISSN 1750-3841. PMID 25471637.
  6. ^ Mendiola, J.A.; Herrero, M.; Cifuentes, A.; Ibañez, E. (2007). "Use of compressed fluids for sample preparation: Food applications". Journal of Chromatography A. 1152 (1–2): 234–246. doi:10.1016/j.chroma.2007.02.046. hdl:10261/12445. PMID 17353022.
  7. ^ "Test Methods | Wastes - Hazardous Waste | US EPA". wayback.archive-it.org. Archived from the original on 17 December 2008. Retrieved 5 February 2018.((cite web)): CS1 maint: bot: original URL status unknown (link)
  8. ^ U.S.EPA Method 3561 Supercritical Fluid Extraction of Polycyclic Aromatic Hydrocarbons.
  9. ^ Use of Ozone Depleting Substances in Laboratories. TemaNord 2003:516.
  10. ^ Yeo, S.; Kiran, E. (2005). "Formation of polymer particles with supercritical fluids: A review". J. Supercrit. Fluids. 34 (3): 287–308. doi:10.1016/j.supflu.2004.10.006.
  11. ^ Budisa, Nediljko; Schulze-Makuch, Dirk (8 August 2014). "Supercritical Carbon Dioxide and Its Potential as a Life-Sustaining Solvent in a Planetary Environment". Life. 4 (3): 331–340. Bibcode:2014Life....4..331B. doi:10.3390/life4030331. PMC 4206850. PMID 25370376.
  12. ^ Rubin, James B.; Taylor, Craig M. V.; Hartmann, Thomas; Paviet-Hartmann, Patricia (2003), Joseph M. DeSimone; William Tumas (eds.), "Enhancing the Properties of Portland Cements Using Supercritical Carbon Dioxide", Green Chemistry Using Liquid and Supercritical Carbon Dioxide: 241–255
  13. ^ Sakakura, Toshiyasu; Choi, Jun-Chul; Yasuda, Hiroyuki (13 June 2007). "Transformation of Carbon dioxide". Chemical Reviews. 107 (6): 2365–2387. doi:10.1021/cr068357u. PMID 17564481.
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  15. ^ "Supercritical CO2 Power Cycle Developments and Commercialization: Why sCO2 can Displace Steam" (PDF).
  16. ^ "Supercritical Carbon Dioxide Power Cycles Starting to Hit the Market". Breaking Energy.
  17. ^ "Corrosion and Erosion Behavior in sCO
    2     Power Cycles"     (PDF). Sandia National Laboratories.
  18. ^ "THE EFFECT OF TEMPERATURE ON THE sCO2 COMPATIBILITY OF CONVENTIONAL STRUCTURAL ALLOYS" (PDF). The 4th International Symposium - Supercritical CO2 Power Cycles. Archived from the original (PDF) on 23 April 2016.
  19. ^ J. Parks, Curtis. "Corrosion of Candidate High Temperature Alloys in Supercritical Carbon Dioxide" (PDF). Ottawa-Carleton Institute for Mechanical and Aerospace Engineering.
  20. ^ Talbot, David (11 April 2016). "Desk-Size Turbine Could Power a Town". MIT Technology Review. Retrieved 13 April 2016.
  21. ^ Blain, Loz (1 November 2023). "Supercritical CO2 pilot aims to make steam turbines obsolete". New Atlas. Retrieved 4 November 2023.
  22. ^ V. Dostal, M.J. Driscoll, P. Hejzlar, "A Supercritical Carbon Dioxide Cycle for Next Generation Nuclear Reactors" (PDF). Retrieved 20 November 2007. MIT-ANP-Series, MIT-ANP-TR-100 (2004)
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  24. ^ "The Hydrogen Economy: Opportunities, Costs, Barriers, and R&D Needs", p. 84 (2004)
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  28. ^ Donald W. Brown(2000), "On the feasibility of using sCO
    2     as heat transmission fluid in an engineered hot dry rock geothermal system"     Archived 2006-09-04 at the Wayback Machine
  29. ^ K Pruess(2007)Enhanced Geothermal Systems (EGS) comparing water with CO
    2     as heat transmission fluids"
  30. ^ J Apps(2011), "Modeling geochemical processes in enhanced geothermal systems with CO
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  31. ^ Randolph, Jimmy B.; Saar, Martin O. (2011). "Combining geothermal energy capture with geologic carbon dioxide sequestration". Geophysical Research Letters. 38 (L10401): n/a. Bibcode:2011GeoRL..3810401R. doi:10.1029/2011GL047265.
  32. ^ Adams, Benjamin M.; Kuehn, Thomas H.; Bielicki, Jeffrey M.; Randolph, Jimmy B.; Saar, Martin O. (2015). "A comparison of electric power output of CO2 Plume Geothermal (CPG) and brine geothermal systems for varying reservoir conditions". Applied Energy. 140: 365–377. doi:10.1016/j.apenergy.2014.11.043.
  33. ^ http://earthsciences.typepad.com/blog/2011/06/achieving-carbon-sequestration-and-geothermal-energy-production-a-win-win.html ESD News and Events "Achieving Carbon Sequestration and Geothermal Energy Production: A Win-Win!"
  34. ^ "Aerogel.org » Supercritical Drying".
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