Photoelectrochemical reduction of carbon dioxide

Photoelectrochemical reduction of carbon dioxide, also known as photoelectrolysis of carbon dioxide, is a chemical process whereby carbon dioxide is reduced to carbon monoxide or hydrocarbons by the energy of incident light. This process requires catalysts, most of which are semiconducting materials. The feasibility of this chemical reaction was first theorised by Giacomo Luigi Ciamician, an Italian photochemist. Already in 1912 he stated that "[b]y using suitable catalyzers, it should be possible to transform the mixture of water and carbon dioxide into oxygen and methane, or to cause other endo-energetic processes."

This article is about the photoelectrochemical system. For related systems, see Electrochemical reduction of carbon dioxide and Photochemical reduction of carbon dioxide.

Furthermore, the reduced species may prove to be a valuable feedstock for other processes. If the incident light utilized is solar then this process also potentially represents energy routes which combine renewable energy with CO2 reduction.

Thermodynamics

Thermodynamic potentials for the reduction of CO2 to various products is given in the following table versus NHE at pH = 7. Single electron reduction of CO2 to CO2●− radical occurs at E° = −1.90 V versus NHE at pH = 7 in an aqueous solution at 25 °C under 1 atm gas pressure. The reason behind the high negative thermodynamically unfavorable single electron reduction potential of CO2 is the large reorganization energy between the linear molecule and bent radical anion. Proton-coupled multi-electron steps for CO2 reductions are generally more favorable than single electron reductions, as thermodynamically more stable molecules are produced.[1]

Summary of thermodynamic potentials of CO2 reduction to various products
CO
2   +   2 H+
   +   2 e−   →   CO   +   H
2O		E0 = −0.53 V
CO
2   +   2 H+
   +   2 e−   →   HCOOH		E0 = −0.61 V
CO
2   +   4 H+
   +   4 e−   →   HCHO   +   H
2O		E0 = −0.48 V
CO
2   +   6 H+
   +   6 e−   →   CH
3OH   +   H
2O		E0 = −0.38 V
CO
2   +   8 H+
   +   8 e−   →   CH
4   +   2 H
2O		E0 = −0.24 V
CO
2   +   e−   →   CO−
2		E0 = −1.90 V

Kinetics
Figure 3 Position of conduction and valence band of several semiconductors at pH = 1 shown vs NHE. Thermodynamic potentials for CO2 reduction to different products at pH = 1 vs NHE is shown beside the band edge positions of semiconductors.

Thermodynamically, proton coupled multiple-electron reduction of CO2 is easier than single electron reduction. But to manage multiple proton coupled multiple-electron processes is a huge challenge kinetically. This leads to a high overpotential for electrochemical heterogeneous reduction of CO2 to hydrocarbons and alcohols. Even further heterogeneous reduction of singly reduced CO2●− radical anion is difficult because of repulsive interaction between negatively biased electrode and negatively charged anion.

Figure 2 shows that in case of a p-type semiconductor/liquid junction photo generated electrons are available at the semiconductor/liquid interface under illumination. The reduction of redox species happens at less negative potential on illuminated p-type semiconductor compared to metal electrode due to the band bending at semiconductor/liquid interface. Figure 3 shows that thermodynamically, some of the proton-coupled multi-electron CO2 reductions are within semiconductors band gap. This makes it feasible to photo-reduce CO2 on p-type semiconductors. Various p-type semiconductors have been successfully employed for CO2 photo reduction including p-GaP, p-CdTe, p-Si, p-GaAs, p-InP, and p-SiC. Kinetically, however, these reactions are extremely slow on given semiconductor surfaces; this leads to significant overpotential for CO2 reduction on these semiconductor surfaces. Apart from high overpotential; these systems have a few advantages including sustainability (nothing is consumed in this system apart from light energy), direct conversion of solar energy to chemical energy, utilization of renewable energy resource for energy intensive process, stability of the process (semiconductors are really stable under illumination) etc. A different approach for photo-reduction of CO2 involves molecular catalysts, photosensitizers and sacrificial electron donors. In this process sacrificial electron donors are consumed during the process and photosensitizers degrade under long exposure to illumination.

Solvent effect

The photo-reduction of CO2 on p-type semiconductor photo-electrodes has been achieved in both aqueous and non-aqueous media. Main difference between aqueous and non-aqueous media is the solubility of CO2. The solubility of CO2 in aqueous media at 1 atm. of CO2 is around ≈ 35 mM; whereas solubility of CO2 in methanol is around 210 mM and in acetonitrile is around 210 mM.

Aqueous media

Photoreduction of CO2 to formic acid was demonstrated on an p-GaP photocathode in aqueous media.[2] Apart from several other reports of CO2 photoreduction on p-GaP, there are other p-type semiconductors like p-GaAs,[3] p-InP, p-CdTe,[4] and p+/p-Si[5] have been successfully used for photoreduction of CO2. The lowest potential for CO2 photoreduction was observed on p-GaP. This may be due to high photovoltage excepted from higher band gap p-GaP (2.2 eV) photocathode. Apart from formic acid, other products observed for CO2 photoreduction are formaldehyde, methanol and carbon monoxide. On p-GaP, p-GaAs and p+/p-Si photocathode, the main product is formic acid with small amount of formaldehyde and methanol. However, for p-InP and p-CdTe photocathode, both carbon monoxide and formic acid are observed in similar quantities. Mechanism proposed by Hori[6] based on CO2 reduction on metal electrodes predicts formation of both formic acid (in case of no adsorption of singly reduced CO2●− radical anion to the surface) and carbon monoxide (in case of adsorption of singly reduced CO2●− radical anion to the surface) in aqueous media. This same mechanism can be evoked to explain the formation of mainly formic acid on p-GaP, p-GaAs and p+/p-Si photocathode owing to no adsorption of singly reduced CO2●− radical anion to the surface. In case of p-InP and p-CdTe photocathode, partial adsorption of CO2●− radical anion leads to formation of both carbon monoxide and formic acid. Low catalytic current density for CO2 photoreduction and competitive hydrogen generation are two major drawbacks of this system.

Non-aqueous media

Maximum catalytic current density for CO2 reduction that can be achieved in aqueous media is only 10 mA cm−2 based solubility of CO2 and diffusion limitations.[7] The integrated maximum photocurrent under Air Mass 1.5 illumination, in the conventional Shockley-Quiesser limit for solar energy conversion for p-Si (1.12 eV), p-InP (1.3 eV), p-GaAs (1.4 eV), and p-GaP (2.3 eV) are 44.0 mA cm−2, 37.0 mA cm−2, 32.5 mA cm−2 and 9.0 mA cm−2, respectively.[8] Therefore, non-aqueous media such as DMF, acetonitrile, methanol are explored as solvent for CO2 electrochemical reduction. In addition, Methanol has been industrially used as a physical absorber of CO2 in the Rectisol method.[9] Similarly to aqueous media system, p-Si, p-InP, p-GaAs, p-GaP and p-CdTe are explored for CO2 photoelectrochemical reduction. Among these, p-GaP has lowest overpotential, whereas, p-CdTe has moderate overpotential but high catalytic current density in DMF with 5% water mixture system.[10] Main product of CO2 reduction in non-aqueous media is carbon monoxide. Competitive hydrogen generation is minimized in non-aqueous media. Proposed mechanism for CO2 reduction to CO in non-aqueous media involves single electron reduction of CO2 to CO2●− radical anion and adsorption of radical anion to surface followed by disproportionate reaction between unreduced CO2 and CO2●− radical anion to form CO32− and CO.

See also

References
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  2. Halmann, M. (1978). "Photoelectrochemical reduction of aqueous carbon dioxide on p-type gallium phosphide in liquid junction solar cells". Nature. 275 (5676): 115–116. Bibcode:1978Natur.275..115H. doi:10.1038/275115a0. S2CID 4257841.
  3. Aurian-Blajeni, B.; Halmann, M.; Manassen, J. (1983). "Electrochemical measurement on the photoelectrochemical reduction of aqueous carbon dioxide on p-Gallium phosphide and p-Gallium arsenide semiconductor electrodes". Solar Energy Materials. 8 (4): 425–440. doi:10.1016/0165-1633(83)90007-2.
  4. Yoneyama, Hiroshi; Sugimura, Kenji; Kuwabata, Susumu (1988). "Effects of electrolytes on the photoelectrochemical reduction of carbon dioxide at illuminated p-type cadmium telluride and p-type indium phosphide electrodes in aqueous solutions". J. Electroanal. Chem. Interfacial Electrochem. 249 (1–2): 143–153. doi:10.1016/0022-0728(88)80355-3.
  5. Junfu, Liu; Baozhu, ChunYu (1992). "Photoelectrochemical reduction of carbon dioxide on a p+/p-Si photocathode in aqueous electrolyte". J. Electroanal. Chem. 324 (1–2): 191–200. doi:10.1016/0022-0728(92)80045-6.
  6. Hori, Yoshio; Wakebe, Hidetoshi; Tsukamoto, Toshio; Koga, Osamu (1994). "Electrocatalytic process of CO selectivity in electrochemical reduction of CO2 at metal electrodes in aqueous media". Electrochim. Acta. 39 (11–12): 1833–1839. doi:10.1016/0013-4686(94)85172-7.
  7. Kumar, Bhupendra; Smieja, Jonathan M.; Kubiak, Clifford P. (2010). "Photoreduction of CO2 on p-type Silicon Using Re(bipy-But)(CO)3Cl: Photovoltages Exceeding 600 mV for the Selective Reduction of CO2 to CO". J. Phys. Chem. C. 114 (33): 14220-14223. doi:10.1021/jp105171b.
  8. Walter, Michael G.; Warren, Emily L.; McKone, James R.; Boettcher, Shannon W.; Mi, Qixi; Santori, Elizabeth A.; Lewis, Nathan S. (2010). "Solar Water Splitting Cells". Chem. Rev. 110 (11): 6446–6473. doi:10.1021/cr1002326. PMID 21062097.
  9. Kaneco, Satoshi; Katsumata, Hideyuki; Suzuki, Tohru; Ohta, Kiyohisa (2006). "Photoelectrochemical reduction of carbon dioxide at p-type gallium arsenide and p-type indium phosphide electrodes in methanol". Chemical Engineering Journal. 116 (3): 227–231. doi:10.1016/j.cej.2005.12.014.
  10. Taniguchi, I.; Aurian-Blajeni, B.; Bockris, J. O'M. (1984). "The reduction of carbon dioxide at illuminated p-type semiconductor electrodes in nonaqueous media". Electrochim. Acta. 29 (7): 923–932. doi:10.1016/0013-4686(84)87137-6.
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