Submitted Successfully!
To reward your contribution, here is a gift for you: A free trial for our video production service.
Thank you for your contribution! You can also upload a video entry or images related to this topic.
Version Summary Created by Modification Content Size Created at Operation
1
Matthew Asmussen
 + 1980 word(s) 1980 2021-12-15 04:57:01 |
2 The format is correct.
Yvaine Wei
 -11 word(s) 1969 2021-12-28 02:40:22 |

Video Upload Options

Do you have a full video?
Send video materials Upload full video

Confirm

Are you sure to Delete?
Yes No
Cite
If you have any further questions, please contact Encyclopedia Editorial Office.
Asmussen, M. Reducing Chlorine Evolution through Transitional Metal Dopants. Encyclopedia. Available online: https://encyclopedia.pub/entry/17574 (accessed on 25 July 2024).
Asmussen M. Reducing Chlorine Evolution through Transitional Metal Dopants. Encyclopedia. Available at: https://encyclopedia.pub/entry/17574. Accessed July 25, 2024.
Asmussen, Matthew. "Reducing Chlorine Evolution through Transitional Metal Dopants" Encyclopedia, https://encyclopedia.pub/entry/17574 (accessed July 25, 2024).
Asmussen, M. (2021, December 27). Reducing Chlorine Evolution through Transitional Metal Dopants. In Encyclopedia. https://encyclopedia.pub/entry/17574
Asmussen, Matthew. "Reducing Chlorine Evolution through Transitional Metal Dopants." Encyclopedia. Web. 27 December, 2021.
Reducing Chlorine Evolution through Transitional Metal Dopants
Edit
This entry is adapted from the peer-reviewed paper 10.3390/app112411911

Electrocatalytic water splitting is a possible route to the expanded generation of green hydrogen; a long-term challenge is the requirement of fresh water as an electrolyzer feed. The use of seawater as a direct feed for electrolytic hydrogen production would alleviate fresh water needs and potentially open an avenue for locally generated hydrogen from marine hydrokinetic or off-shore power sources. One environmental limitation to seawater electrolysis is the generation of chlorine as a competitive anodic reaction. 

electrolysis chlorine evolution oxygen evolution seawater

1. Introduction

The electrocatalytic splitting of water to produce hydrogen can be used to store renewable electricity as either a chemical fuel or as a feedstock. However, this process currently requires an ultra-pure water feed [1], which would thus strain drinking water supplies at hydrogen production levels required for a fleet of fuel cell vehicles [2]. Seawater presents an abundant water resource, but it is yet to be utilized for hydrogen production due to the complexity it presents as an electrolyte and energy-intensive purification processes. If the associated challenges were overcome, seawater electrolysis could generate H2 fuel from green electricity at coastal sites, on board marine vessels or platforms, or submersed at marine hydrokinetic platforms [3].
The kinetics of the oxygen evolution reaction (OER) are generally slower relative to chlorine evolution reaction (CER) due to the requirement for the transfer of four electrons and protons per oxygen molecule, while the CER is a two-electron process. At pH > 3, chloride can be oxidized to form hypochlorous acid (HOCl, pH 3–7), and at pH > 7, hypochlorite is formed (OCl−) [4]. Most research on maximizing oxygen evolution activity to date has focused on highly acidic [5][6][7][8] or alkaline [9][10][11][12] media, and information regarding the selectivity toward chlorine evolution often stems from the chlor-alkali industry in acidic environments where CER is preferred [13]. Although precious metal oxides (e.g., IrO2) are highly active for OER in acidic media, such materials are similarly highly active for CER in chloride-containing media [14][15].
In the neutral conditions of seawater [16][17][18], electrolysis studies are scarce and, instead, often incorporate additional buffering [19]. Historically, research in such media has focused on metal oxides primarily composed of Mn [20][21][22], Ni [16][23], and Co [19][20][24], often with additional elements, such as Fe or W. Considering abundance and a promising price point [24], here Mn-based oxides are focused, which are stable and have demonstrated good Faradaic efficiency in a wide range of electrolyte pH. MnOx electrocatalysts (often supported on an IrO2/Ti substrate [25]) have demonstrated good selectivity (>90%) toward OER in chlorine-containing electrolyte, with the remainder of the current going toward CER and oxidative dissolution in the form of MnO4− [21]. However, these electrodes suffered from mechanical instability during cycling at appreciable current densities. The incorporation of Mo6+ improved durability and Faradaic efficiency [26]. The further incorporation of W6+ maintained this performance while improving OER activity (lowering overpotential), which has been attributed in part to its enhancement of oxide conductivity [23]. However, numerous other potential metals may serve a similar role, perhaps with better efficacy and stability.

2. Electrode Fabrication and Structure

The electrodeposition process produced electrodes with a cracked mud structure, with the Mn-Mo-X catalyst deposited on top of a sub-layer of thermal decomposition-produced IrO2. The IrO2 layer prevents insulation of the titanium substrate by oxidation [25]. The thermal decomposition process deposited ~0.0020 g/cm2 of IrO2. To ensure the complete coverage of, first, the IrO2 layer on the Ti and, then, the Mn-Mo catalyst, important for analysis of Faradaic efficiency toward OER, deposition conditions were tailored to achieve complete attenuation by EDS (information depth on the order of ~microns). Three sequential electrodeposition cycles of 20 min each at 80 °C were used to generate a homogenous catalyst layer. Figure 1 shows the resulting catalyst layer yielding complete coverage of the electrode surface by EDS, similar to prior work [22]. Electrodeposition at room temperature or with a continuous deposition at 80 °C generated incomplete and heterogeneous catalyst layers on the electrode surface. Beyond three cycles, flaking from over-deposition was observed. The deposition cycles resulted in ~0.0500 g/cm2 of catalyst deposited.
Applsci 11 11911 g001 550
Figure 1. (a) SEM micrograph and the corresponding EDS maps for (b) Mn and (c) Mo for a 0.2 M Mn-0.003 M Mo catalyst with three 20 min electrodeposition cycles at 80 °C. There was no signal from the underlying Ti or Ir layers.
The inclusion of dopants at various levels in the Mn-Mo-X catalyst did not distort the overall cracked mud structure. Some heterogeneous distribution of the catalyst elements was observed as small “bumps” on the catalyst surface. EDS mapping highlighted the variations in element distribution through the catalysts. As an example, Figure 2a shows the SEM image of a Mn-Mo-0.006 M Ru electrode. While the composition appeared generally uniform across the film, there is also a Mn-rich region (Figure 2b) that is depleted in Mo (Figure 2c) and Ru (Figure 2d). The “cracks” in the microstructure gave a stronger Mn signal, suggesting the Mn distribution may vary with electrode thickness. While the distribution of the Ru in Figure 2d appeared homogenous, magnification of the catalyst surface in Figure 2e showed “bumps” on the catalyst surface. EDS spot analysis showed that the flat region contained only Mn and Mo, whereas the bumps also contained Ru (Table 1). As a result of this heterogenous composition profile, the quantification of the dopant level and Mn/Mo/X ratios was limited with EDS. Thus, electrodes are referred to by the starting electrodeposition solution concentration, where increased solution concentration results in increased electrode dopant concentration.
Applsci 11 11911 g002 550
Figure 2. (a) SEM micrograph and corresponding EDS maps for (b) Mn, (c) Mo, and (d) Ru showing a Mn-rich region. (e) SEM micrograph at higher resolution on the Mn-Mo-0.006 M Ru electrode showing the heterogeneous bumps on the sample surface. The red boxes denote the regions quantified in Table 1.
Table 1. Composition of the regions analyzed by EDS in Figure 2e.
Spectrum O (at%) Mn (at%) Mo (at%) Ru (at%)
1 58.23 41.49 0.28 0.00
2 58.17 41.29 0.40 0.15
The XRD pattern of both the Mn-Mo-0.006 M Ru and Mn-Mo-0.009 M Ru electrodes showed the majority of the pattern arising from MnO2 with a strong signal from the underlying IrO2 layer (Figure 3). The low concentration of Ru and the overlap in the XRD features of its oxides make it challenging to assess potential phase segregation.
Applsci 11 11911 g003 550
Figure 3. XRD patterns of the Mn-Mo-0.006 M Ru and Mn-Mo-0.009 M Ru electrodes and associated peak fits. CPS = counts per second.

3. OER Efficiency in Saline and Seawater Environments

The performance of the electrodes was assessed on efficiency toward the OER over the CER, represented as the faradaic efficiency (FE) for OER, and the overall catalytic performance, represented as total charge passed at a given applied potential for 30 min (normalized by electrode geometric area). Electrodes that suppress the CER while facilitating the rate of OER are promising candidates for further development. In a 30 min exposure at 1.4 V vs. Ag/AgCl, an IrOx had a faradaic efficiency of only 18% toward OER (14.7 C/cm2), while a Mn-Mo electrode measured 91% faradaic efficiency (31 C/cm2).
The influence of various dopant levels on the Mn-Mo electrodes on OER faradaic efficiency in neutral chloride (0.5 M NaCl) environments is shown in Figure 4. In Figure 4a, the addition of Co to the Mn-Mo provided efficiencies >95% relatively consistently for the tested compositions, with the exception being 0.009 M Co. Increasing to Mn-Mo-0.1 M Co created a more physically stable electrode. For the inclusion of Fe (Figure 4b), the best performance was measured for electrodes Mn-Mo-0.01 M Fe, Mn-Mo-0.1 M Fe, and Mn-Mo-0.02 M Fe. Below 0.01 M Fe addition, stability and efficiency were compromised. A Mn-Mo-0.003 M W electrode was the best performing of the W set with consistent >94% efficiency for OER (Figure 4d). A drop in pH over time was observed in the unbuffered neutral chloride electrolyte, possibly due to the inability of the Nafion® membrane to exchange the protons at the proton generation/consumption rate. The Ru electrodes with >0.003 M Ru addition all had strong OER efficiency (Figure 4c). The Mn-Mo-0.001 M Ru electrodes had poor physical stability leading to the large deviation between runs. The addition of Sn as a dopant led to a decrease in OER compared with the other dopants, with the Mn-Mo-0.003 M Sn electrode providing ~88% efficiency (Figure 4e). Out of the electrodes evaluated, the inclusion of Ru provided the best efficiency toward OER in 0.5 M NaCl (Figure 4). 
Applsci 11 11911 g005 550
Figure 4. Comparison of the average OER faradaic efficiencies (3 subsequent measurements) following 30 min at 1.5 V (vs. Ag/AgCl) in 0.5 M NaCl for electrodes doped with (a) Co, (b) Fe, (c) Ru, (d) W, and (e) Sn.
When testing in filtered raw seawater, most of the electrodes saw a slight decrease in OER faradaic efficiency compared with the neutral chloride solution. The differences may originate from the increased ionic concentration in seawater and the application from a higher kinetic overpotential (V vs. RHE) given the increased buffering in seawater and, correspondingly, the higher pH in the anolyte compared to 0.5 M NaCl. A summary of these tests is shown in Figure 5. The inclusion of Co (Figure 5a) generally maintained high OER faradaic efficiency, somewhat greater for the Mn-Mo-0.2 M Co electrode. Surprisingly, for Fe-containing electrodes (Figure 5b), the OER faradaic efficiency in seawater was notably greater than in 0.5 M NaCl for 0.001 M Fe, generally decreasing with Fe content and reaching OER efficiencies notably lower than in 0.5 M NaCl. This switch may be due to buffering occurring in seawater improving the Fe’s stability in the electrode. Elucidation of this behavior change at low Fe doping levels will be a focus of future work. The Ru electrodes also performed well, >90% efficiency for the electrodes at 0.003 M Ru and 0.009 M Ru (Figure 5c). For W-containing electrodes, OER faradaic efficiencies were also somewhat higher in seawater, marginally greater for the Mn-Mo-0.003 M W (Figure 6d), which also had similar performance in artificial seawater. The Mn-Mo-0.003 M Sn electrode again had the best performance from the Sn set (Figure 5e).
Applsci 11 11911 g006 550
Figure 5. Comparison of the OER faradaic efficiency for replicate electrode samples following 30 min at 1.5 V (vs. Ag/AgCl) in raw filtered seawater for electrodes doped with (a) Co, (b) Fe, (c) W, (d) Ru, and (e) Sn.

4. The Effectiveness of Doping Transition Metals on CER Suppression

The doping transition metals into Mn-Mo-X catalysts can effectively suppress the CER and improve overall catalytic activity. The best-performing dopant was Ru in terms of efficiency for OER over CER and catalytic activity. However, despite previous reports of this doping approach being successful for CER suppression, little mechanistic discussion is present in the literature. With the similar response of multiple dopants (Fe, Sn, W, and Co) and the enhanced activity of a known catalytically active species, Ru, dopants may play a role in manipulating the coating density and stability in addition to serving as active catalytic sites. Evidence on both mechanistic roles exists. Ru and Ir are industrial benchmark catalysts for efficient oxygen and chlorine evolution (in the chlor-alkali process), sitting high on the volcano curve for both OER [27] and CER [28]. In the case of IrOx, the OER is not suppressed or influenced by the CER occurring on the same surface, showing scaling between the two reactions on active catalysts [29]. Targeting selective OER over CER can present a challenge but may be realized through a combination of processes.

The adsorbed intermediates generated for the CER can also influence selectivity. Surfaces that form a M-Cl intermediate can efficiently sustain the CER, while the generation of the M-OCl intermediate will suppress the CER [30]. The OCl intermediate route further suppresses the CER on RuO2 with increasing pH due to the change in Gibbs free energy loss. Studies of preferential OER in halide-containing environments on NiB and CoP catalysts suggest that the edge sites on the metalate clusters are crucial to sustaining the OER, as H2O will out compete halides for these sites, increasing the likelihood of OER over CER. With the small locations and disordered distribution of the Ru dopants, a higher number of edge sites may dictate an added preference to OER over CER via oxygen-containing intermediates [31]. 

References

  1. Tong, W.; Forster, M.; Dionigi, F.; Dresp, S.; Sadeghi Erami, R.; Strasser, P.; Cowan, A.J.; Farràs, P. Electrolysis of low-grade and saline surface water. Nat. Energy 2020, 5, 367–377.
  2. Webber, M.E. The water intensity of the transitional hydrogen economy. Environ. Res. Lett. 2007, 2, 034007.
  3. Dresp, S.R.; Dionigi, F.; Klingenhof, M.; Strasser, P. Direct electrolytic splitting of seawater: Opportunities and challenges. ACS Energy Lett. 2019, 4, 933–942.
  4. Hansen, H.A.; Man, I.A.; Studt, F.; Abild-Pedersen, F.; Bligaard, T.; Rossmeisl, J. Electrochemical chlorine evolution at rutile oxide (110) surfaces. Phys. Chem. Chem. Phys. 2010, 12, 283–290.
  5. El-Moneim, A.A.; Bhattarai, J.; Kato, Z.; Izumiya, K.; Kumagai, N.; Hashimoto, K. Mn-Mo-Sn oxide anodes for oxygen evolution in seawater electrolysis for hydrogen production. ECS Trans. 2010, 25, 127.
  6. El-Moneim, A.A.; Kumagai, N.; Asami, K.; Hashimoto, K. Nanocrystalline manganese-molybdenum-tungsten oxide anodes for oxygen evolution in acidic seawater electrolysis. Mater. Trans. 2005, 46, 309–316.
  7. Vos, J.; Koper, M. Measurement of competition between oxygen evolution and chlorine evolution using rotating ring-disk electrode voltammetry. J. Electroanal. Chem. 2018, 819, 260–268.
  8. Vos, J.G.; Wezendonk, T.A.; Jeremiasse, A.W.; Koper, M.T. MnOx/IrOx as selective oxygen evolution electrocatalyst in acidic chloride solution. J. Am. Chem. Soc. 2018, 140, 10270–10281.
  9. Amikam, G.; Nativ, P.; Gendel, Y. Chlorine-free alkaline seawater electrolysis for hydrogen production. Int. J. Hydrogen Energy 2018, 43, 6504–6514.
  10. Kuang, Y.; Kenney, M.J.; Meng, Y.; Hung, W.-H.; Liu, Y.; Huang, J.E.; Prasanna, R.; Li, P.; Li, Y.; Wang, L. Solar-driven, highly sustained splitting of seawater into hydrogen and oxygen fuels. Proc. Natl. Acad. Sci. USA 2019, 116, 6624–6629.
  11. Juodkazytė, J.; Šebeka, B.; Savickaja, I.; Petrulevičienė, M.; Butkutė, S.; Jasulaitienė, V.; Selskis, A.; Ramanauskas, R. Electrolytic splitting of saline water: Durable nickel oxide anode for selective oxygen evolution. Int. J. Hydrogen Energy 2019, 44, 5929–5939.
  12. Dresp, S.R.; Dionigi, F.; Klingenhof, M.; Merzdorf, T.; Schmies, H.; Drnec, J.; Poulain, A.; Strasser, P. Molecular Understanding of the Impact of Saline Contaminants and Alkaline pH on NiFe Layered Double Hydroxide Oxygen Evolution Catalysts. ACS Catal. 2021, 11, 6800–6809.
  13. Karlsson, R.K.; Cornell, A. Selectivity between oxygen and chlorine evolution in the chlor-alkali and chlorate processes. Chem. Rev. 2016, 116, 2982–3028.
  14. Exner, K.S.; Over, H. Beyond the rate-determining step in the oxygen evolution reaction over a single-crystalline IrO2 (110) model electrode: Kinetic scaling relations. ACS Catal. 2019, 9, 6755–6765.
  15. Exner, K.S. Controlling stability and selectivity in the competing chlorine and oxygen evolution reaction over transition metal oxide electrodes. ChemElectroChem 2019, 6, 3401–3409.
  16. Zheng, J. Seawater splitting for high-efficiency hydrogen evolution by alloyed PtNix electrocatalysts. Appl. Surf. Sci. 2017, 413, 360–365.
  17. Zheng, J. Pt-free NiCo electrocatalysts for oxygen evolution by seawater splitting. Electrochim. Acta 2017, 247, 381–391.
  18. Cheng, F.; Feng, X.; Chen, X.; Lin, W.; Rong, J.; Yang, W. Synergistic action of Co-Fe layered double hydroxide electrocatalyst and multiple ions of sea salt for efficient seawater oxidation at near-neutral pH. Electrochim. Acta 2017, 251, 336–343.
  19. Hsu, G.-S.W.; Lu, Y.-F.; Hsu, S.-Y. Effects of electrolysis time and electric potential on chlorine generation of electrolyzed deep ocean water. J. Food Drug Anal. 2017, 25, 759–765.
  20. Fujimura, K.; Izumiya, K.; Kawashima, A.; Akiyama, E.; Habazaki, H.; Kumagai, N.; Hashimoto, K. Anodically deposited manganese-molybdenum oxide anodes with high selectivity for evolving oxygen in electrolysis of seawater. J. Appl. Electrochem. 1999, 29, 769–775.
  21. Fujimura, K.; Matsui, T.; Izumiya, K.; Kumagai, N.; Akiyama, E.; Habazaki, H.; Kawashima, A.; Asami, K.; Hashimoto, K. Oxygen evolution on manganese–molybdenum oxide anodes in seawater electrolysis. Mater. Sci. Eng. A 1999, 267, 254–259.
  22. El-Moneim, A. Mn–Mo–W-oxide anodes for oxygen evolution during seawater electrolysis for hydrogen production: Effect of repeated anodic deposition. Int. J. Hydrogen Energy 2011, 36, 13398–13406.
  23. Dionigi, F.; Reier, T.; Pawolek, Z.; Gliech, M.; Strasser, P. Design criteria, operating conditions, and nickel-iron hydroxide catalyst materials for selective seawater electrolysis. ChemSusChem 2016, 9, 962–972.
  24. Vesborg, P.C.; Jaramillo, T.F. Addressing the terawatt challenge: Scalability in the supply of chemical elements for renewable energy. Rsc Adv. 2012, 2, 7933–7947.
  25. Kato, Z.; Sato, M.; Sasaki, Y.; Izumiya, K.; Kumagai, N.; Hashimoto, K. Electrochemical characterization of degradation of oxygen evolution anode for seawater electrolysis. Electrochim. Acta 2014, 116, 152–157.
  26. Fujimura, K.; Matsui, T.; Habazaki, H.; Kawashima, A.; Kumagai, N.; Hashimoto, K. The durability of manganese–molybdenum oxide anodes for oxygen evolution in seawater electrolysis. Electrochim. Acta 2000, 45, 2297–2303.
  27. Yu, J.; He, Q.; Yang, G.; Zhou, W.; Shao, Z.; Ni, M. Recent Advances and Prospective in Ruthenium-Based Materials for Electrochemical Water Splitting. ACS Catal. 2019, 9, 9973–10011.
  28. Exner, K.S. Beyond thermodynamic-based material-screening concepts: Kinetic scaling relations exemplified by the chlorine evolution reaction over transition-metal oxides. Electrochim. Acta 2020, 334, 135555.
  29. Trasatti, S. Electrocatalysis in the anodic evolution of oxygen and chlorine. Electrochim. Acta 1984, 29, 1503–1512.
  30. Exner, K.S. Design criteria for the competing chlorine and oxygen evolution reactions: Avoid the OCl adsorbate to enhance chlorine selectivity. Phys. Chem. Chem. Phys. 2020, 22, 22451–22458.
  31. Keane, T.P.; Nocera, D.G. Selective Production of Oxygen from Seawater by Oxidic Metallate Catalysts. ACS Omega 2019, 4, 12860–12864.
More
© Text is available under the terms and conditions of the Creative Commons Attribution (CC BY) license; additional terms may apply. By using this site, you agree to the Terms and Conditions and Privacy Policy.
Upload a video for this entry
Information
Subjects: Chemistry, Applied
Contributor MDPI registered users' name will be linked to their SciProfiles pages. To register with us, please refer to https://encyclopedia.pub/register :
Matthew Asmussen
View Times: 490
Entry Collection: Environmental Sciences
Revisions: 2 times (View History)
Update Date: 29 Dec 2021
Table of Contents
    1000/1000
    Hot Most Recent
    Video Production Service
    Feedback