Copper–chlorine cycle

The copper–chlorine cycle (Cu–Cl cycle) is a four-step thermochemical cycle for the production of hydrogen. The Cu–Cl cycle is a hybrid process that employs both thermochemical and electrolysis steps. It has a maximum temperature requirement of about 530 degrees Celsius.[1]

Simplified diagram of the Copper–Chlorine cycle

The Cu–Cl cycle involves four chemical reactions for water splitting, whose net reaction decomposes water into hydrogen and oxygen. All other chemicals are recycled. The Cu–Cl process can be linked with nuclear plants or other heat sources such as solar and industrial waste heat to potentially achieve higher efficiencies, lower environmental impact and lower costs of hydrogen production than any other conventional technology.

The Cu–Cl cycle is one of the prominent thermochemical cycles under development within the Generation IV International Forum (GIF). Through GIF, over a dozen countries around the world are developing the next generation of nuclear reactors for highly efficient production of both electricity and hydrogen.

Process description

The four reactions in the Cu–Cl cycle are listed as follows:[2][3]

  1. 2 Cu + 2 HCl(g) → 2 CuCl(l) + H2(g) (430–475 °C)
  2. 2 CuCl2 + H2O(g) → Cu2OCl2 + 2 HCl(g) (400 °C)
  3. 2 Cu2OCl2 → 4 CuCl + O2(g) (500 °C)
  4. 2 CuCl → CuCl2(aq) + Cu (ambient-temperature electrolysis)
Net reaction: 2 H2O → 2 H2 + O2
Legend: (g)—gas; (l)—liquid; (aq)—aqueous solution; the balance of the species are in a solid phase.

Atomic Energy of Canada Limited has demonstrated experimentally a CuCl electrolyzer in which hydrogen is produced electrolytically at the cathode and Cu(I) is oxidized to Cu(II) at the anode, thereby combining above steps 1 and 4 to eliminate the intermediate production and subsequent transport of solid copper.[4]

Approximately 50% of the heat required to drive this reaction can be captured from the reaction itself. The other heat can be provided by any suitable process. Recent research has focused on a cogeneration scheme using the waste heat from nuclear reactors, specifically the CANDU supercritical water reactor.[4]

Advantages and disadvantages

Advantages of the copper–chlorine cycle include lower operating temperatures, the ability to use low-grade waste heat to improve energy efficiency, and potentially lower cost materials. In comparison with other thermochemical cycles, the Cu–Cl process requires relatively low temperatures of up to 530 °C (990 °F).

Another significant merit of this cycle is a relatively low voltage (thus low electrical energy expenditure) that is required for the electrochemical step (0.6 to 1.0 V, perhaps even 0.5 if lower current density can be achieved).[5] The overall efficiency of the Cu–Cl cycle has been estimated to be just over 43%,[6] excluding the additional potential gains of utilizing waste heat in the cycle.

Solids handling between processes and corrosive working fluids present unique challenges for the engineering equipment development. Among others, the following materials are being currently used: spray coatings, nickel alloys, glass-lined steel, refractory materials, and other advanced materials.[7]

gollark: I used to, but the bees making up my computational substrate were replaced with directly manipulated apions for higher clock rate.
gollark: It might need gmp or something.
gollark: Hey, what if I allow length-terminated strings to have length-terminated lengths represented as strings *to arbitrary depths*?
gollark: Poe's law applies to reality, evidently.
gollark: PRs welcome!

See also

References
  1. Solar power for thermochemical production of hydrogen
  2. Rosen, M.A., Naterer, G.F., Sadhankar, R., Suppiah, S., "Nuclear-Based Hydrogen Production with a Thermochemical Copper-Chlorine Cycle and Supercritical Water Reactor", Canadian Hydrogen Association Workshop, Quebec, October 19 – 20, 2006. (PDF) Archived 2011-07-06 at the Wayback Machine.
  3. Lewis, M. and Masin, J., "An Assessment of the Efficiency of the Hybrid Copper-Chloride Thermochemical Cycle", Argonne National Laboratory, University of Chicago, 2 November 2005. (PDF).
  4. Naterer, G. F.; et al. (2009). "Recent Canadian Advances in Nuclear-Based Hydrogen Production and the Thermochemical Cu-Cl Cycle". International Journal of Hydrogen Energy. 34 (7): 2901–2917. doi:10.1016/j.ijhydene.2009.01.090.
  5. Dokiya, M.; Kotera, Y. (1976). "Hybrid Cycle with Electrolysis Using Cu-Cl System" (PDF). International Journal of Hydrogen Energy. 1 (2): 117–121. doi:10.1016/0360-3199(76)90064-1. Archived from the original (PDF) on 2011-07-06. Retrieved 2009-02-27.
  6. Chukwu, C., Naterer, G. F., Rosen, M. A., "Process Simulation of Nuclear-Produced Hydrogen with a Cu-Cl Cycle", 29th Conference of the Canadian Nuclear Society, Toronto, Ontario, Canada, June 1–4, 2008. "Archived copy" (PDF). Archived from the original (PDF) on 2012-02-20. Retrieved 2013-12-04.CS1 maint: archived copy as title (link)
  7. Hydrogen Website of UOIT (University of Ontario Institute of Technology) Archived 2011-05-22 at the Wayback Machine
This article is issued from Wikipedia. The text is licensed under Creative Commons - Attribution - Sharealike. Additional terms may apply for the media files.