سلول فوتوالکتروشیمیایی

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سلول فوتوالکتروشیمیایی (به انگلیسی: Photoelectrochemical cell) یا PEC گونه‌ای سلول خورشیدی ست که از طیف نور شامل نور مرئی، انرژی الکتریکی تولید می‌کند. این دسته سلول‌ها علاوه بر تولید انرِژی، برای الکترولیز آب نیز بکار برده می‌شوند. تیتانیا (TiO2) ماده اصلی مورد کاربرد درین سلول‌هاست.

ساختار سلول[ویرایش]

تبدیل انرژی تژنور به الکتریسیته بوسیله دو الکترود (آند و کاتد) انجام می‌شود. سه نوع چیدمان برای ساختار این سلول‌ها وجود دارد:

  • فوتوآند نیمه‌رسانای نوع n و کاتد فلزی
  • فوتوآند نیمه‌رسانای نوع n و فوتوکاتد نیمه‌رسانای نوع p
  • آند فلزی و فوتوکاتد نیمه‌رسانای نوع p

جستارهای وابسته[ویرایش]

منابع[ویرایش]

Jenny Nelson, Physics of Sollar Cels', Imperial College Press

A "photoelectrochemical cell" is one of two distinct classes of device. The first produces electrical energy similarly to a dye-sensitized photovoltaic cell, which meets the standard definition of a photovoltaic cell. The second is a photoelectrolytic cell, that is, a device which uses light incident on a photosensitizer, semiconductor, or aqueous metal immersed in an electrolytic solution to directly cause a chemical reaction, for example to produce hydrogen via the electrolysis of water.

Both types of device are varieties of solar cell, in that a photoelectrochemical cell's function is to use the photoelectric effect (or, very similarly, the photovoltaic effect) to convert electromagnetic radiation (typically sunlight) either directly into electrical power, or into something which can itself be easily used to produce electrical power (hydrogen, for example, can be burned to create electrical power, see photohydrogen).

Two principles

The standard photovoltaic effect, as operating in standard photovoltaic cells, involves the excitation of negative charge carriers (electrons) within a semiconductor medium, and it is negative charge carriers (free electrons) which are ultimately are extracted to produce power. The classification of photoelectrochemical cells which includes Grätzel cells meets this narrow definition, albeit the charge carriers are often excitonic.

The situation within a photoelectrolytic cell, on the other hand, is quite different. For example, in a water-splitting photoelectrochemical cell, the excitation, by light, of an electron in a semiconductor leaves a hole which "draws" an electron from a neighboring water molecule:



This leaves positive charge carriers (protons, that is, H+ ions) in solution, which must then bond with one other proton and combine with two electrons in order to form hydrogen gas, according to:


A photosynthetic cell is another form of photoelectrolytic cell, with the output in that case being carbohydrates instead of molecular hydrogen.

Photoelectrolytic cell

Photoelectrolytic cell band diagram

A (water-splitting) photoelectrolytic cell electrolizes water into hydrogen and oxygen gas by irradiating the anode with electromagnetic radiation, that is, with light. This has been referred to as artificial photosynthesis and has been suggested as a way of storing solar energy in hydrogen for use as fuel.[1]

Incoming sunlight excites free electrons near the surface of the silicon electrode. These electrons flow through wires to the stainless steel electrode, where four of them react with four water molecules to form two molecules of hydrogen and 4 OH groups. The OH groups flow through the liquid electrolyte to the surface of the silicon electrode. There they react with the four holes associated with the four photoelectrons, the result being two water molecules and an oxygen molecule. Illuminated silicon immediately begins to corrode under contact with the electrolytes. The corrosion consumes material and disrupts the properties of the surfaces and interfaces within the cell.[2]

Two types of photochemical systems operate via photocatalysis. One uses semiconductor surfaces as catalysts. In these devices the semiconductor surface absorbs solar energy and acts as an electrode for water splitting. The other methodology uses in-solution metal complexes as catalysts.[3][4]

Photoelectrolytic cells have passed the 10 percent economic efficiency barrier. Corrosion of the semiconductors remains an issue, given their direct contact with water.[5] Research is now ongoing to reach a service life of 10000 hours, a requirement established by the United States Department of Energy.[6]

Other photoelectrochemical cells

The first photovoltaic cell ever designed was also the first photoelectrochemical cell. It was created in 1839, by Alexandre-Edmond Becquerel, at age 19, in his father's laboratory.[7]

The mostly commonly researched modern photoelectrochemical cell in recent decades has been the Grätzel cell, although much attention has recently shifted away from this topic to perovskite solar cells, due to relatively high efficiency of the latter and the similarity in vapor assisted deposition techniques commonly used in their creation.

Dye-sensitized solar cells or Grätzel cells use dye-adsorbed highly porous nanocrystalline titanium dioxide (nc-TiO
2
) to produce electrical energy.

Materials for photoelectrolytic cells

Water-splitting photoelectrochemical (PEC) cells use light energy to decompose water into hydrogen and oxygen within a two-electrode cell. In theory, three arrangements of photo-electrodes in the assembly of PECs exist:[8]

  • photo-anode made of a n-type semiconductor and a metal cathode
  • photo-anode made of a n-type semiconductor and a photo-cathode made of a p-type semiconductor
  • photo-cathode made of a p-type semiconductor and a metal anode

There are several requirements for photoelectrode materials in PEC production[9]:

  • light absorbance: determined by band gap and appropriate for solar irradiation spectrum
  • charge transport: photoelectrodes must be conductive (or semi-conductive) to minimize resistive losses
  • suitable band structure: large enough band gap to split water (1.23V) and appropriate positions relative to redox potentials for and
  • catalytic activity: high catalytic activity increases efficiency of the water-splitting reaction
  • stability: materials must be stable to prevent decomposition and loss of function

In addition to these requirements, materials must be low-cost and earth abundant for the widespread adoption of PEC water splitting to be feasible.

While the listed requirements can be applied generally, photoanodes and photocathodes have slightly different needs. A good photocathode will have early onset of the oxygen evolution reaction (low overpotential), a large photocurrent at saturation, and rapid growth of photocurrent upon onset. Good photoanodes, on the other hand, will have early onset of the hydrogen evolution reaction in addition to high current and rapid photocurrent growth. To maximize current, anode and cathode materials need to be matched together; the best anode for one cathode material may not be the best for another.

TiO
2

In 1967, Akira Fujishima discovered the Honda-Fujishima effect, (the photocatalytic properties of titanium dioxide).

TiO
2
and other metal oxides are still most prominent[10] catalysts for efficiency reasons. Including SrTiO
3
and BaTiO
3
,[11] this kind of semiconducting titanates, the conduction band has mainly titanium 3d character and the valence band oxygen 2p character. The bands are separated by a wide band gap of at least 3 eV, so that these materials absorb only UV radiation. Change of the TiO
2
microstructure has also been investigated to further improve the performance, such as TiO
2
nanowire arrays or porous nanocrystalline TiO
2
photoelectrochemical cells.[12]

GaN

GaN is another option, because metal nitrides usually have a narrow band gap that could encompass almost the entire solar spectrum.[13] GaN has a narrower band gap than TiO
2
but is still large enough to allow water splitting to occur at the surface. GaN nanowires exhibited better performance than GaN thin films, because they have a larger surface area and have a high single crystallinity which allows longer electron-hole pair lifetimes.[14] Meanwhile, other non-oxide semiconductors such as GaAs, MoS
2
, WSe
2
and MoSe
2
are used as n-type electrode, due to their stability in chemical and electrochemical steps in the photocorrosion reactions.[15]

Silicon

In 2013 a cell with 2 nanometers of nickel on a silicon electrode, paired with a stainless steel electrode, immersed in an aqueous electrolyte of potassium borate and lithium borate operated for 80 hours without noticeable corrosion, versus 8 hours for titanium dioxide. In the process, about 150 ml of hydrogen gas was generated, representing the storage of about 2 kilojoules of energy.[2][16]

Structured Materials

Structuring of absorbing materials has both positive and negative affects on cell performance. Structuring allows for light absorption and carrier collection to occur in different places, which loosens the requirements for pure materials and helps with catalysis. This allows for the use of non-precious and oxide catalysts that may be stable in more oxidizing conditions. However, these devices have lower open-circuit potentials which may contribute to lower performance.[17]

Hematite

Hematite structure

Researchers have extensively investigated the use of hematite (α-Fe2O3) in PEC water-splitting devices due to its low cost, ability to be n-type doped, and band gap (2.2eV). However, performance is plagued by poor conductivity and crystal anisotropy.[18] Some researchers have enhanced catalytic activity by forming a layer of co-catalysts on the surface. Co-catalysts include cobalt-phosphate[19] and iridium oxide[20], which is known to be a highly active catalyst for the oxygen evolution reaction.[17]

Tungsten Oxide

Tungsten(VI) Oxide (WO3) , which exhibits several different polymorphs at various temperatures, is of interest due to its high conductivity but has a relatively wide, indirect band gap (~2.7 eV) which means it cannot absorb most of the solar spectrum. Though many attempts have been made to increase absorption, they result in poor conductivity and thus WO3 does not appear to be a viable material for PEC water splitting.[17]

Bismuth Vanadate

With a narrower, direct band gap (2.4 eV) and proper band alignment with water oxidation potential, the monoclinic form of BiVO4 has garnered interest from researchers.[17] Over time, it has been shown that V-rich[21] and compact films[22] are associated with higher photocurrent, or higher performance. Bismuth Vanadate has also been studied for solar generation from seawater[23], which is much more difficult due to the presence of contaminating ions and a more harsh corrosive environment.

See also

References

  1. ^ John A. Turner; et al. (2007-05-17). "Photoelectrochemical Water Systems for H2 Production" (PDF). National Renewable Energy Laboratory. Archived from the original (PDF) on 2011-06-11. Retrieved 2011-05-02.
  2. ^ a b "Silicon/nickel water splitter could lead to cheaper hydrogen". Gizmag.com. Retrieved 2013-12-29.
  3. ^ Berinstein, Paula (2001-06-30). Alternative energy: facts, statistics, and issues. Greenwood Publishing Group. ISBN 1-57356-248-3. Another photoelectrochemical method involves using dissolved metal complexes as a catalyst, which absorbs energy and creates an electric charge separation that drives the water-splitting reaction.
  4. ^ Deutsch, T. G.; Head, J. L.; Turner, J. A. (2008). "Photoelectrochemical Characterization and Durability Analysis of GaInPN Epilayers". Journal of the Electrochemical Society. 155 (9): B903. doi:10.1149/1.2946478.
  5. ^ Brad Plummer (2006-08-10). "A Microscopic Solution to an Enormous Problem". SLAC Today. SLAC National Accelerator Laboratory. Retrieved 2011-05-02.
  6. ^ Wang, H.; Deutsch, T.; Turner, J. A. A. (2008). "Direct Water Splitting Under Visible Light with a Nanostructured Photoanode and GaInP2 Photocathode". ECS Transactions. 6: 37. doi:10.1149/1.2832397.
  7. ^ https://www.pveducation.org/pvcdrom/manufacturing/first-photovoltaic-devices
  8. ^ Tryk, D.; Fujishima, A; Honda, K (2000). "Recent topics in photoelectrochemistry: achievements and future prospects". Electrochimica Acta. 45 (15–16): 2363–2376. doi:10.1016/S0013-4686(00)00337-6.
  9. ^ Seitz, Linsey (26 February 2019), Lecture 13: Solar Fuels (Lecture Slides, Introduction to Electrochemistry CHE 395)|format= requires |url= (help), Northwestern University
  10. ^ A. Fujishima, K. Honda, S. Kikuchi, Kogyo Kagaku Zasshi 72 (1969) 108–113
  11. ^ De Haart, L.; De Vries, A. J.; Blasse, G. (1985). "On the photoluminescence of semiconducting titanates applied in photoelectrochemical cells". Journal of Solid State Chemistry. 59 (3): 291–300. Bibcode:1985JSSCh..59..291D. doi:10.1016/0022-4596(85)90296-8.
  12. ^ Cao, F.; Oskam, G.; Meyer, G. J.; Searson, P. C. (1996). "Electron Transport in Porous Nanocrystalline TiO2Photoelectrochemical Cells". The Journal of Physical Chemistry. 100 (42): 17021–17027. doi:10.1021/jp9616573.
  13. ^ Wang, D.; Pierre, A.; Kibria, M. G.; Cui, K.; Han, X.; Bevan, K. H.; Guo, H.; Paradis, S.; Hakima, A. R.; Mi, Z. (2011). "Wafer-Level Photocatalytic Water Splitting on GaN Nanowire Arrays Grown by Molecular Beam Epitaxy". Nano Letters. 11 (6): 2353–2357. Bibcode:2011NanoL..11.2353W. doi:10.1021/nl2006802. PMID 21568321.
  14. ^ Jung, Hye Song; Young Joon Hong, Yirui Li, Jeonghui Cho, Young-Jin Kim, Gyu-Chui Yi (2008). "Photocatalysis Using GaN Nanowires". ACS Nano. 2 (4): 637–642. doi:10.1021/nn700320y.CS1 maint: multiple names: authors list (link)
  15. ^ Kline, G.; Kam, K.; Canfield, D.; Parkinson, B. (1981). "Efficient and stable photoelectrochemical cells constructed with WSe2 and MoSe2 photoanodes". Solar Energy Materials. 4 (3): 301–308. doi:10.1016/0165-1633(81)90068-X.
  16. ^ Kenney, M. J.; Gong, M.; Li, Y.; Wu, J. Z.; Feng, J.; Lanza, M.; Dai, H. (2013). "High-Performance Silicon Photoanodes Passivated with Ultrathin Nickel Films for Water Oxidation". Science. 342 (6160): 836–840. Bibcode:2013Sci...342..836K. doi:10.1126/science.1241327. PMID 24233719.
  17. ^ a b c d Peter, Laurie; Lewerenz, Hans-Joachim (2 October 2013). Photoelectrochemical Water Splitting: Materials, Processes and Architectures. Cambridge: Royal Society of Chemistry. ISBN 978-1-84973-647-3.
  18. ^ Iordanova, N.; Dupuis, M.; Rosso, K. M. (8 April 2005). "Charge transport in metal oxides: A theoretical study of hematite α-Fe2O3". The Journal of Chemical Physics. 122 (14): 144305. doi:10.1063/1.1869492.
  19. ^ Zhong, Diane K.; Gamelin, Daniel R. (31 March 2010). "Photoelectrochemical Water Oxidation by Cobalt Catalyst ("Co−Pi")/α-FeO Composite Photoanodes: Oxygen Evolution and Resolution of a Kinetic Bottleneck". Journal of the American Chemical Society. 132 (12): 4202–4207. doi:10.1021/ja908730h.
  20. ^ Tilley, S. David; Cornuz, Maurin; Sivula, Kevin; Grätzel, Michael (23 August 2010). "Light-Induced Water Splitting with Hematite: Improved Nanostructure and Iridium Oxide Catalysis". Angewandte Chemie International Edition. 49 (36): 6405–6408. doi:10.1002/anie.201003110.
  21. ^ Berglund, Sean P.; Flaherty, David W.; Hahn, Nathan T.; Bard, Allen J.; Mullins, C. Buddie (16 February 2011). "Photoelectrochemical Oxidation of Water Using Nanostructured BiVO Films". The Journal of Physical Chemistry C. 115 (9): 3794–3802. doi:10.1021/jp1109459.
  22. ^ Su, Jinzhan; Guo, Liejin; Yoriya, Sorachon; Grimes, Craig A. (3 February 2010). "Aqueous Growth of Pyramidal-Shaped BiVO4 Nanowire Arrays and Structural Characterization: Application to Photoelectrochemical Water Splitting". Crystal Growth & Design. 10 (2): 856–861. doi:10.1021/cg9012125.
  23. ^ Luo, Wenjun; Yang, Zaisan; Li, Zhaosheng; Zhang, Jiyuan; Liu, Jianguo; Zhao, Zongyan; Wang, Zhiqiang; Yan, Shicheng; Yu, Tao; Zou, Zhigang (2011). "Solar hydrogen generation from seawater with a modified BiVO4 photoanode". Energy & Environmental Science. 4 (10): 4046. doi:10.1039/C1EE01812D.

External links