Next Article in Journal
Emerging Trends of Electrochemical Sensors in Food Analysis
Previous Article in Journal
Impact of Ni Content on the Electrochemical Performance of the Co-Free, Li and Mn-Rich Layered Cathode Materials
 
 
Search for Articles:
Title / Keyword
Author / Affiliation / Email
Journal
Article Type
 
 
Advanced Search
 
Section
Special Issue
Volume
Issue
Number
Page
 
Journals
Electrochem
Volume 4
Issue 1
10.3390/electrochem4010003
electrochem-logo
Submit to this Journal Review for this Journal Propose a Special Issue
► Article Menu

Article Menu

share Share announcement Help format_quote Cite question_answer Discuss in SciProfiles thumb_up
...
Endorse textsms
...
Comment
first_page
settings
Order Article Reprints
Font Type:
Arial Georgia Verdana
Font Size:
Aa Aa Aa
Line Spacing:
Column Width:
Background:
Review

Environment-Friendly Ascorbic Acid Fuel Cell

by
Md. Mahmudul Hasan
Research Organization for Nano and Life Innovation, Waseda University, Shinjuku, Tokyo 162-0041, Japan
Electrochem 2023, 4(1), 31-41; https://doi.org/10.3390/electrochem4010003
Submission received: 10 January 2023 / Revised: 24 January 2023 / Accepted: 28 January 2023 / Published: 30 January 2023
Browse Figures
Review Reports Versions Notes

Abstract

:
Recently, ascorbic acid (AA) has been studied as an environment-friendly fuel for energy conversion devices. This review article has deliberated an overview of ascorbic acid electrooxidation and diverse ion exchange types of AA-based fuel cells for the first time. Metal and carbon-based catalysts generated remarkable energy from environment-friendly AA fuel. The possibility of using AA in a direct liquid fuel cell (DLFC) without emitting any hazardous pollutants is discussed. AA fuel cells have been reviewed based on carbon nanomaterials, alloys/bimetallic nanoparticles, and precious and nonprecious metal nanoparticles. Finally, the obstacles and opportunities for using AA-based fuel cells in practical applications have also been incorporated.

1. Introduction

The current energy system is predominately fossil-fuel-based and contributes to alarming greenhouse emissions. This resulted in a greater need for alternative energy sources due to rising global energy demands driven by population increase and economic expansion. Modern wind and solar power technologies have developed quickly to provide sustainable and clean energy to meet energy demands. The geographical reliance, irregularity, and high starting costs of these energy generation methods put them at a competitive and economic disadvantage. Battery and fuel cell technologies that use renewable energy are receiving widespread attention in academia and business to overcome fossil fuel dependency [1].
In comparison to other sustainable energy sources, fuel cells are rapidly replacing gas, oil, coal, petroleum, etc. A fuel cell generates electricity from chemical energy and oxygen [2]. Direct liquid fuel cells (DLFCs) provide sustainable, carbon-neutral, and efficient power generation prospects. Transportation, permanent and mobile equipment, as well as a secondary power source are examples of DLFCs application [3]. The energy density of methanol is high, and it is also simple to store and distribute compared to hydrogen. Thus, a direct acidic methanol fuel cell (DMFC) is a preferable alternative for proton exchange membrane fuel cells (PEMFCs), where a cation exchange membrane (CEM) is used. The moderate toxicity of methanol and the catalyst poisoning (CO adsorption) that occurs in acidic DMFCs necessitate the use of expensive anode catalysts [4]. Direct formic acid fuel cells (DFAFCs) are gaining popularity because they have a lower fuel crossover and are less hazardous than methanol [3]. Conversely, it has less energy density and required costly Pt catalysts [3]. Furthermore, DFAFCs are highly vulnerable to CO poisoning on noble metals (Pt and Pd) during long-time operations [5]. Since ethanol is renewable and has a low level of toxicity, direct ethanol fuel cells (DEFCs) have been studied. However, even with precious metals, the ethanol oxidation rate is quite low in acidic environments [6].
Since the invention of anion exchange membranes (AEMs), many fuels can be oxidized efficiently in alkaline conditions compared to an acidic environment. In AEMs, hydroxyl ions are moved from cathode to anode over the membrane with lowered fuel crossover. In addition, the alkaline environment of AEM has benefits for water management, minimal overpotential requirements, and oxidation and reduction. Significantly reducing the cost of operation is made possible by nonprecious metal (Cu) catalysts in alkaline fuel cells [7]. This ensures the feasibility of DLFCs, as costly noble metals could be replaced. In terms of environmental considerations, the release of CO2 makes commercialization more challenging for alcohol-based DLFC, in both cases of acidic and alkaline. Figure 1 shows the schematic diagram of alcohol-based DLFC fuel cells. An environment-friendly fuel source is highly desirable to generate clean energy. Ascorbic acid (AA) could be used for clean energy generation. This review will provide more information and explore the feasibility of using AA as an alternative environmentally benign fuel for energy conversion.

2. An Overview of Ascorbic Acid

AA (vitamin C) is a water-soluble antioxidant that is present in foods and biological systems [8,9]. The molecular formula for AA is C6H8O6 and its molar mass is 176.14 g per mol [10]. Vitamin C or AA is the L-enantiomer of ascorbate; the D-enantiomer is the reverse and has no physiological importance. The same chemical structure exists in each of its forms, which are exact replicas of one another. Figure 2a illustrates the chemical structure of AA. One of the most pervasive vitamins ever identified is AA. It must be consumed from outside fruits and vegetables because it cannot be produced in the human body. AA is largely present in citrus fruits and vegetables [11]. AA is widely used in the chemical sector and cosmetic and medical applications due to its antioxidant properties. The mechanism and kinetics of AA oxidation have been extensively studied during the past few decades [8,12,13]. Two e− and two H+ are released during AA oxidation to create dehydroascorbic acid (DHA). As seen in Figure 2b, AA and DHA form an irreversible redox pair [11]. It has been established that the production of DHA requires two e- and two H+ during the oxidation of AA [14,15].

3. Catalysts for Ascorbic Acid Electrooxidation

Research output has increased in several application fields as a result of the development of nanomaterial technology. The incorporation of nanomaterials into electrocatalyst technology improves catalysis performance by increasing sensitivity, selectivity, stability, and repeatability. The discovery of novel catalysts enables comprehensive catalyst downsizing, improve stability, and enhanced specificity. The noble metals are more stable at room temperature and have better catalytic activity and biocompatibility when compared to other nanoscale systems. Numerous applications, such as electrocatalysis, environmental monitoring, and biosensing, have previously demonstrated the value of noble metals. Numerous nanomaterials (noble metal nanoparticles, carbon nanocomposites, transition metals oxides and hydroxides, and conducting polymers) have been used in the electrocatalysis of AA [16]. The electrocatalysis of AA has been carried out using noble metals (gold, ruthenium, etc.) through high selectivity and low overpotential [17,18,19,20,21]. Noble-metal-modified electrochemical surfaces have a greater electrochemically active surface area, which results in a faster electron transfer rate, faster current responsiveness, and a lower overpotential required for electrochemical reactions. Pt has drawn more interest because it has better mass transport characteristics and allows for rapid electron transmission. Pt has been applied for the electrocatalysis of AA [22,23,24,25]. There are several sites for AA oxidation, hydrogen adsorption, reverse adsorption, and dissociative side-chain adsorption in the nanostructured Pt. The exorbitant price of the Pt catalysts might prevent commercialization. The use of Au nanoparticles in electrocatalysis is frequently widespread because of its electron-rich core, biocompatibility, constrained size, and several surface functions [26]. Many studies have discussed the use of Au-modified electrodes for AA electrooxidation [11,13,17,27,28]. However, the performance of Au nanoparticles for AA electrooxidation is insufficient for practical applications. Pd has high catalytic activity for electrochemical reactions. Several Pd-based catalysts for AA electrooxidation have been reported [9,11,29,30]. Ag has been employed for AA electrooxidation because of its unique electrical and chemical characteristics [8,31,32,33,34,35,36]. Non-noble catalyst Cu has been employed for AA oxidation [19,37]. Nonmetallic catalysts, such as carbon catalysts, showed prominent results for AA electrooxidation [38,39,40,41,42,43,44].

4. Ascorbic Acid as Fuel

AA, generally referred to as vitamin C, has been a subject of interest in a variety of scientific disciplines. In particular, AA has been used for DLFCs throughout the past few decades. It is a tiny organic molecule that is plentiful in living things and is, therefore, a sustainable fuel source. Additionally, AA can be produced commercially by fermenting D-glucose or from biomass waste [45]. AA is oxidized effectively on a variety of carbon black materials, making it a desirable fuel choice for DLFCs [41,44]. Thus, the potential of carbon electrodes for the AA fuel cell is worth investigating. As mentioned above, the primary end product of the AA oxidation reaction has been identified as DHA, regardless of catalyst [46,47]. The creation of DHA from AA fuel and solid carbon catalyst benefits the environment and creates a complete zero-emissions energy-harvesting system. These advantages have significant effects on AA’s capacity to be used in implantable medical devices. Additionally, it has been demonstrated that DHA can be enzymatically converted to AA via a variety of pathways, suggesting effective recovery of fuel from waste [48].

4.1. Acidic Fuel Cell

Combining thin-film and microelectromechanical systems (MEMS), AA could be used in portable or small acidic fuel cells. According to Mogi et al., direct AA fuel cells (DAAFCs) with microchannels made of polyimide (PI) substrates have been produced [49]. On the PI substrate, aluminum electrodes were created using photolithography and screen printing. Porous carbon was deposited on the Al electrode using screen printing to improve surface area to produce 1.83 μW/cm2 power density. These devices showed excellent versatility and endurance while serving as examples of micropower sources for in vivo sensing [49]. Falk et al. demonstrated an AA-based biofuel cell without a membrane for glucose sensing [50]. The cell produced electricity using AA and oxygen from the human lachrymal fluid. Tetrathiafulvalene (TTF) and tetracyanoquinodimethane (TCNQ) were added to nanostructured microelectrodes to act as the anode catalysts for AA oxidation and a redox enzyme called bilirubin oxidase (BOx) as the cathode catalyst. The device generated a peak power density of 0.72 µW/cm2 and a current density of 0.55 µA/cm2. This technology demonstrated a secure, dependable source of power for noninvasive glucose testing [50]. Wu et al. demonstrated a small silicon wafer fuel cell where a thin polymer electrolyte separator was used between AA and air reactants. The anodic catalyst for the electrooxidation of AA was a thin Pt layer (0.43 mg/cm2) deposited by sputtering on a silicon surface. Using DuPont’s Nafion®117, the maximum output power density was 1.95 mW/cm2 at a current density of 10 mA/cm2 [51].
In contrast to fuels like ethanol, methanol, and/or polyalcohol fuels, investigations have shown that the electrooxidation of AA fuel may be carried out on a cheap, non-noble metal catalyst. Using a CEM and several anode catalysts, including carbon black (Vulcan XC72) [44,45], Pt [45,47], Ru [45,47], Pd [44,45,46,47], Ir [45,47], Rh [45,47], and PtRu [45,47], Fujiwara et al. showed an operational DAAFC. Pd black metal catalyst displayed excellent power production of 7 mW/cm2 among various precious metal catalysts. The highest power density was generated using Vulcan XC72 (16 mW/cm2), as shown in Figure 3. Variations in fuel cell performance on each anodic catalyst are caused by differences in the electrochemically active surface area of electrodes. According to Mondal et al., a polyaniline (PANI) catalyst might be employed for DAAFC without a platinum-group catalyst. The DAAFC generated a peak power density of 4.3 mW/cm2 and a current density of 15 mA/cm2 at 70 °C. Kaneto et al. reported single-walled carbon nanotubes (SWCNTs) and poly(3,4-ethylene dioxythiophene) polystyrene sulfonate (PEDOT*PSS) (* denotes charge transfer complex) composite anode catalyst for DAAFC. Coating SWCNT with PEDOT*PSS enhanced peak power density to 11.3 mW/cm2 higher than SWCNT (4.9 mW/cm2) alone [52]. The OCV was 0.55 V. Uhm et al. found that electrochemically oxidized carbon electrodes had a considerably higher electrocatalytic performance for AA oxidation than unmodified carbon. Furthermore, the carbon paper-based electrode structure is much more effective in generating a power density of 18 mW/cm2 at 60 °C without the need for an extra powder-based valuable catalyst layer [38]. To produce an anodic electrocatalyst with better hydrophilicity for AA oxidation, Qiu et al. demonstrated that BP 2000 carbon black treated with 4 M nitric acid yielded a peak power density of 31 mW/cm2 at 80 °C [43]. A hydrophilic carbon produced 1.72 times the power density of the previously reported carbon catalyst. In contrast to platinum group metals, Choun et al. found that carbon surfaces with high oxygen-to-carbon ratios (O/C) demonstrated exceptional electrocatalytic activity toward AA oxidation. They discovered that acid-treated carbon on the Toray-060 catalyst produced a maximum power output of about 53 µW/cm2 at 36.5 °C (implantable medical technology) [39].

4.2. Alkaline Fuel Cell

The AEM used in alkaline DLFCs has benefits over the CEM (e.g., Nafion) [53]. Alkaline DLFCs produce water at the anode, minimizing the need for water management, and fuel cell performance does not affect the cathode. They have faster reaction kinetics, lower activation overpotential requirement, and a lower corrosive environment for metal catalysts of the fuel cell. Lastly, compared to hydrogen, alkaline DLFCs are easier to store, handle, and transfer [54]. According to Muneeb et al., ascorbate is more effectively oxidized in alkaline media when used with an alkaline DAAFC. The initial direct alkaline DAAFC was operated by Muneeb et al. using an anion exchange membrane. The DAAFC showed a peak power density of 27 mW/cm2 at room temperature using Pd black and Pt black catalysts, higher than the acidic AA fuel cell previously described. At 60 °C, this DAAFC generated a maximum power density of 73 mW/cm2 and a current density of 497 mA/cm2, as shown in Figure 4 [55]. Additionally, Muneeb et al. discovered that the use of a Pd28Cu72/C catalyst further improves the performance of alkaline DAAFC, followed by a maximum power density of 89 mW/cm2. This is because of the bimetallic advantage of the electrical and bifunctional effects [37]. This is very important because, by substituting roughly 3/4 of the Pd with Cu, higher performance and lower fuel cell material costs were also attained. The current work examines the idea of using a carbon-supported Cu catalyst in place of precious metal catalysts at the anode entirely.

4.3. Split-pH (Alkaline–Acid) Fuel Cells

The split-pH DLFC was proposed by An and Zhao et al. They investigated the DEFC with an alkaline ethanol fuel in anode and an acidic oxidant flow (H2O2 and H2SO4) on the cathode side with a CEM (Nafion) as an electrolyte [56]. A proton usually migrates from the anode to the cathode in DLFCs with a CEM. However, protons in CEM are replaced by Na+ (or K+) ions in split-pH fuel cells, allowing CEMs to be employed in an alkaline condition (NaOH), as shown in Figure 5a. It has been demonstrated that the oxidation of several fuels, such as methanol, ethanol, formate, and ascorbate, happens most effectively in alkaline media, but AEMs have many drawbacks when compared to CEMs. AEMs are less thermally stable and have around half or 1/3 lower ionic conductivity than CEMs [57]. As a result, the split-pH fuel cell integrates the conductivity advantages of CEM and the kinetic benefits of alkaline fuel conditions into a single system. Additionally, the use of H2O2 (oxidant) in DLFC extended for use in space and underwater travel [58]. In alkaline conditions, H2O2 also has a larger reduction potential than O2 (+0.48 V higher), which rises to +0.91 V by the acidic oxidant. As a result, split-pH fuel cells have a thermodynamic advantage of greatly enhanced theoretical cell potential. The fuel showed a significantly large oxidation potential at pH 14 and a high reduction potential of H2O2 at pH 0 [59]. Li et al. tuned a formate–peroxide DLFC to achieve a peak power density of 591 mW/cm2 (highest until now) having 1.69 V OCV at 60 °C by Pd/C anode catalyst and Pt/C cathode catalyst [60]. With a high power density of 33 mW/cm2 at 60 °C, they also demonstrated that an AEM-based formate–oxygen DLFC might run without extra hydroxide [61]. Formate–oxygen DLFC and formate–peroxide DLFC have a significant power density difference, which highlights the excellent efficiency of split-pH fuels.
Muneeb et al. showed that a split-pH DAAFC (ascorbate–peroxide) operated by carbon anode and cathode generated a peak power density of 40 mW/cm2 at 60 °C using 1 M H2SO4 and 3% H2O2 [41]. This was carried out to reduce the price of fuel cell components. In addition, using 30% H2O2, this fuel cell produces the highest power density of 158 mW/cm2 shown in Figure 5b. They also showed that, using the same catalyst, an alkaline ascorbate fuel cell using an AEM generated 4.7 mW/cm2 peak power density with O2 and 16 mW/cm2 with 30% H2O2 at 60 °C. This demonstrated the performance advantages of a split-pH DAAFC over an alkaline DAAFC where the carbon electrode could be used on both sides of the fuel cell. The first nonprecious metal split-pH ascorbate–peroxide fuel cell was demonstrated by Keramati et al. They used Cu/C (anode), and carbon (cathode) as catalysts and the oxidant was H2O2 in H2SO4. It attained an OCV of 1.05 V and a maximum power density of 51 mW/cm2 [59]. An alkaline environment may speed up ascorbate (A2−) oxidation to DHA by reducing nonredox steps compared to AA oxidation at normal pH. They propose the fuel cell reaction as follows [59]:
  • Anode: A2− = DHA + 2e−; Eanode = −0.42 V
  • Cathode: H2O2 + 2H+ +2e− = 2H2O; Ecathode= +1.78 V
  • Overall: A2− + H2O2 = DHA + 2H2O; Eoverall= +2.18 V
The reported AA-based fuel cells are all listed in Table 1. The order is based on the highest performance.

5. Challenges and Future Scope

AA is a natural, plentiful, and eco-friendly fuel source. However, the performance of fuel cells is still far behind for commercial use. AA functioned as a proton conductor for acidic DAAFC, much like the proton exchange ionomer Nafion. Increasing the thickness and/or mass of the Nafion ionomer reduced the AA oxidation rate by preventing AA’s mass transfer towards the electrode surface [44,46]. AA is a water-based fuel. Therefore, increasing the hydrophilicity of the membrane electrode assembly (MEA) is crucial for improving fuel cell performance. The water management process might be enhanced by alkaline DAAFC. Thus, fuel cell performance was improved. However, the AEM deterioration could be troublesome for long-time operations. The benefits of the alkaline anode side and acidic cathode side in split-pH DAAFC showed the highest performance, similar to the alcohol-based DLFC. Although split-pH DAAFC significantly improved the catholyte, the higher corrosivity brought by utilizing a more concentrated H2O2 solution may cause fuel cell components to prematurely degrade. Therefore, to produce a higher amount of power density for the practical use of environmentally friendly DAAFC, the best conditions paired with a suitable anode catalyst, such as Pd- and/or Cu-based carbon catalysts, need to be further explored.

6. Conclusions

This review paper covered the operation of the DAAFC and the possibility that AA might be used as a renewable alternative fuel. Numerous studies demonstrated that the DAAFC produced clean energy without emitting any hazardous materials into the environment. As an alternate power source to alcohol-based DLFC, split-pH DAAFC offers similar performance. Thus, this review may provide future academics with a chance to draw attention to DAAFC improvement and build a sustainable society for the next generation.

Funding

This research received no external funding.

Institutional Review Board Statement

Not applicable.

Informed Consent Statement

Not applicable.

Data Availability Statement

Not applicable.

Conflicts of Interest

The author declares no conflict of interest.

References

  1. Zaman, S.; Huang, L.; Douka, A.I.; Yang, H.; You, B.; Xia, B.Y. Oxygen Reduction Electrocatalysts toward Practical Fuel Cells: Progress and Perspectives. Angew. Chem. Int. Ed. 2021, 133, anie.202016977. [Google Scholar] [CrossRef]
  2. Debe, M.K. Electrocatalyst Approaches and Challenges for Automotive Fuel Cells. Nature 2012, 486, 43–51. [Google Scholar] [CrossRef] [PubMed]
  3. Ong, B.C.; Kamarudin, S.K.; Basri, S. Direct Liquid Fuel Cells: A Review. Int. J. Hydrogen Energy 2017, 42, 10142–10157. [Google Scholar] [CrossRef]
  4. Basri, S.; Kamarudin, S.K.; Daud, W.R.W.; Yaakub, Z. Nanocatalyst for Direct Methanol Fuel Cell (DMFC). Int. J. Hydrogen Energy 2010, 35, 7957–7970. [Google Scholar] [CrossRef]
  5. Haan, J.L.; Stafford, K.M.; Masel, R.I. Effects of the Addition of Antimony, Tin, and Lead to Palladium Catalyst Formulations for the Direct Formic Acid Fuel Cell. J. Phys. Chem. C 2010, 114, 11665–11672. [Google Scholar] [CrossRef]
  6. Antolini, E. Catalysts for Direct Ethanol Fuel Cells. J. Power Sources 2007, 170, 1–12. [Google Scholar] [CrossRef]
  7. Ferriday, T.B.; Middleton, P.H. Alkaline Fuel Cell Technology—A Review. Int. J. Hydrogen Energy 2021, 46, 18489–18510. [Google Scholar] [CrossRef]
  8. Hasan, M.M.; Rakib, R.H.; Hasnat, M.A.; Nagao, Y. Electroless Deposition of Silver Dendrite Nanostructure onto Glassy Carbon Electrode and Its Electrocatalytic Activity for Ascorbic Acid Oxidation. ACS Appl. Energy Mater. 2020, 3, 2907–2915. [Google Scholar] [CrossRef]
  9. Hasan, M.M.; Nagao, Y. Christmas-Tree-Shaped Palladium Nanostructures Decorated on Glassy Carbon Electrode for Ascorbic Acid Oxidation in Alkaline Condition. ChemistrySelect 2021, 6, 5885–5892. [Google Scholar] [CrossRef]
  10. Cathcart, R.F. A Unique Function for Ascorbate. Med. Hypotheses 1991, 35, 32–37. [Google Scholar] [CrossRef]
  11. Pisoschi, A.M.; Pop, A.; Serban, A.I.; Fafaneata, C. Electrochemical Methods for Ascorbic Acid Determination. Electrochim. Acta 2014, 121, 443–460. [Google Scholar] [CrossRef]
  12. Prieto, F.; Coles, B.A.; Compton, R.G. Mechanistic Determination Using Arrays of Variable-Sized Channel Microband Electrodes: The Oxidation of Ascorbic Acid in Aqueous Solution. J. Phys. Chem. B 1998, 102, 7442–7447. [Google Scholar] [CrossRef]
  13. Rueda, M.; Aldaz, A.; Sanchez-Burgos, F. Oxidation of L-Ascorbic Acid on a Gold Electrode. Electrochim. Acta 1978, 23, 419–424. [Google Scholar] [CrossRef]
  14. Hu, I.F.; Kuwana, T. Oxidative Mechanism of Ascorbic Acid at Glassy Carbon Electrodes. Anal. Chem. 1986, 58, 3235–3239. [Google Scholar] [CrossRef]
  15. Tu, Y.J.; Njus, D.; Schlegel, H.B. A Theoretical Study of Ascorbic Acid Oxidation and HOO˙/O2˙− Radical Scavenging. Org. Biomol. Chem. 2017, 15, 4417–4431. [Google Scholar] [CrossRef]
  16. Dhara, K.; Debiprosad, R.M. Review on Nanomaterials-Enabled Electrochemical Sensors for Ascorbic Acid Detection. Anal. Biochem. 2019, 586, 113415. [Google Scholar] [CrossRef]
  17. Kuss, S.; Compton, R.G. Electrocatalytic Detection of Ascorbic Acid Using N,N,N′,N′-Tetramethyl-Para-Phenylene-Diamine (TMPD) Mediated Oxidation at Unmodified Gold Electrodes; Reaction Mechanism and Analytical Application. Electrochim. Acta 2017, 242, 19–24. [Google Scholar] [CrossRef]
  18. Zhang, X.; Yu, S.; He, W.; Uyama, H.; Xie, Q.; Zhang, L.; Yang, F. Electrochemical Sensor Based on Carbon-Supported NiCoO2 Nanoparticles for Selective Detection of Ascorbic Acid. Biosens. Bioelectron. 2014, 55, 446–451. [Google Scholar] [CrossRef]
  19. Xi, L.; Ren, D.; Luo, J.; Zhu, Y. Electrochemical Analysis of Ascorbic Acid Using Copper Nanoparticles/Polyaniline Modified Glassy Carbon Electrode. J. Electroanal. Chem. 2010, 650, 127–134. [Google Scholar] [CrossRef]
  20. Raoof, J.B.; Ojani, R.; Baghayeri, M. A Selective Sensor Based on a Glassy Carbon Electrode Modified with Carbon Nanotubes and Ruthenium Oxide/Hexacyanoferrate Film for Simultaneous Determination of Ascorbic Acid, Epinephrine and Uric Acid. Anal. Methods 2011, 3, 2367. [Google Scholar] [CrossRef]
  21. Lee, Y.G.; Liao, B.X.; Weng, Y.C. Ruthenium Oxide Modified Nickel Electrode for Ascorbic Acid Detection. Chemosphere 2017, 173, 512–519. [Google Scholar] [CrossRef] [PubMed]
  22. Thiagarajan, S.; Chen, S. Preparation and Characterization of PtAu Hybrid Film Modified Electrodes and Their Use in Simultaneous Determination of Dopamine, Ascorbic Acid and Uric Acid. Talanta 2007, 74, 212–222. [Google Scholar] [CrossRef] [PubMed]
  23. Zhao, D.; Yu, G.; Tian, K.; Xu, C. A Highly Sensitive and Stable Electrochemical Sensor for Simultaneous Detection towards Ascorbic Acid, Dopamine, and Uric Acid Based on the Hierarchical Nanoporous PtTi Alloy. Biosens. Bioelectron. 2016, 82, 119–126. [Google Scholar] [CrossRef] [PubMed]
  24. Xing, X.; Bae, I.T.; Shao, M.; Liu, C.C. Electro-Oxidation of l-Ascorbic Acid on Platinum in Acid Solutions: An In-Situ FTIRRAS Study. J. Electroanal. Chem. 1993, 346, 309–321. [Google Scholar] [CrossRef]
  25. Oko, D.N.; Garbarino, S.; Zhang, J.; Xu, Z.; Chaker, M.; Ma, D.; Guay, D.; Tavares, A.C. Dopamine and Ascorbic Acid Electro-Oxidation on Au, AuPt and Pt Nanoparticles Prepared by Pulse Laser Ablation in Water. Electrochim. Acta 2015, 159, 174–183. [Google Scholar] [CrossRef]
  26. Islam, M.T.; Hasan, M.M.; Shabik, M.F.; Islam, F.; Nagao, Y.; Hasnat, M.A. Electroless Deposition of Gold Nanoparticles on a Glassy Carbon Surface to Attain Methylene Blue Degradation via Oxygen Reduction Reactions. Electrochim. Acta 2020, 360, 136966. [Google Scholar] [CrossRef]
  27. Raj, C.R.; Ohsaka, T. Electroanalysis of Ascorbate and Dopamine at a Gold Electrode Modified with a Positively Charged Self-Assembled Monolayer. J. Electroanal. Chem. 2001, 496, 44–49. [Google Scholar] [CrossRef]
  28. Alonso-Lomillo, M.A.; Domínguez-Renedo, O.; Saldaña-Botín, A.; Arcos-Martínez, M.J. Determination of Ascorbic Acid in Serum Samples by Screen-Printed Carbon Electrodes Modified with Gold Nanoparticles. Talanta 2017, 174, 733–737. [Google Scholar] [CrossRef]
  29. Wu, G.; Wu, Y.; Liu, X.; Rong, M.; Chen, X.; Chen, X. An Electrochemical Ascorbic Acid Sensor Based on Palladium Nanoparticles Supported on Graphene Oxide. Anal. Chim. Acta 2012, 745, 33–37. [Google Scholar] [CrossRef]
  30. Jiang, J.; Du, X. Sensitive Electrochemical Sensors for Simultaneous Determination of Ascorbic Acid, Dopamine, and Uric Acid Based on Au@Pd-Reduced Graphene Oxide Nanocomposites. Nanoscale 2014, 6, 11303–11309. [Google Scholar] [CrossRef]
  31. Noroozifar, M.; Khorasani-Motlagh, M.; Taheri, A. Preparation of Silver Hexacyanoferrate Nanoparticles and Its Application for the Simultaneous Determination of Ascorbic Acid, Dopamine and Uric Acid. Talanta 2010, 80, 1657–1664. [Google Scholar] [CrossRef] [PubMed]
  32. Majari Kasmaee, L.; Gobal, F. A Preliminary Study of the Electro-Oxidation of l-Ascorbic Acid on Polycrystalline Silver in Alkaline Solution. J. Power Sources 2010, 195, 165–169. [Google Scholar] [CrossRef]
  33. Khalilzadeh, M.A.; Borzoo, M. Green Synthesis of Silver Nanoparticles Using Onion Extract and Their Application for the Preparation of a Modified Electrode for Determination of Ascorbic Acid. J. Food Drug Anal. 2016, 24, 796–803. [Google Scholar] [CrossRef] [PubMed]
  34. Gobal, F.; Majari Kasmaee, L. Silver Selenide as a Potential Electro-Catalyst for l-Ascorbic Acid Electro-Oxidation in Alkaline Solution. Electrocatalysis 2011, 2, 331–336. [Google Scholar] [CrossRef]
  35. Harraz, F.A.; Faisal, M.; Al-Salami, A.E.; El-Toni, A.M.; Almadiy, A.A.; Al-Sayari, S.A.; Al-Assiri, M.S. Silver Nanoparticles Decorated Stain-Etched Mesoporous Silicon for Sensitive, Selective Detection of Ascorbic Acid. Mater. Lett. 2019, 234, 96–100. [Google Scholar] [CrossRef]
  36. Tashkhourian, J.; Nezhad, M.R.H.; Khodavesi, J.; Javadi, S. Silver Nanoparticles Modified Carbon Nanotube Paste Electrode for Simultaneous Determination of Dopamine and Ascorbic Acid. J. Electroanal. Chem. 2009, 633, 85–91. [Google Scholar] [CrossRef]
  37. Muneeb, O.; Do, E.; Boyd, D.; Perez, J.; Haan, J.L. PdCu/C Anode Catalysts for the Alkaline Ascorbate Fuel Cell. Appl. Energy 2019, 235, 473–479. [Google Scholar] [CrossRef]
  38. Uhm, S.; Choi, J.; Chung, S.T.; Lee, J. Electrochemically Oxidized Carbon Anode in Direct L-Ascorbic Acid Fuel Cells. Electrochim. Acta 2007, 53, 1731–1736. [Google Scholar] [CrossRef]
  39. Choun, M.; Lee, H.J.; Lee, J. Positively Charged Carbon Electrocatalyst for Enhanced Power Performance of L-Ascorbic Acid Fuel Cells. J. Energy Chem. 2016, 25, 793–797. [Google Scholar] [CrossRef]
  40. Sathe, B.R. A Scalable and Facile Synthesis of Carbon Nanospheres as a Metal Free Electrocatalyst for Oxidation of l -Ascorbic Acid: Alternate Fuel for Direct Oxidation Fuel Cells. J. Electroanal. Chem. 2017, 799, 609–616. [Google Scholar] [CrossRef]
  41. Muneeb, O.; Chino, I.; Saenz, A.; Haan, J.L. An Ascorbate Fuel Cell with Carbon Black Nanoparticles as Anode and Cathode. J. Power Sources 2019, 413, 216–221. [Google Scholar] [CrossRef]
  42. Zhang, M.; Liu, K.; Xiang, L.; Lin, Y.; Su, L.; Mao, L. Carbon Nanotube-Modified Carbon Fiber Microelectrodes for In Vivo Voltammetric Measurement of Ascorbic Acid in Rat Brain. Anal. Chem. 2007, 79, 6559–6565. [Google Scholar] [CrossRef]
  43. Qiu, C.; Chen, H.; Liu, H.; Zhai, Z.; Qin, J.; Lv, Y.; Gao, Z.; Song, Y. The Hydrophilicity of Carbon for the Performance Enhancement of Direct Ascorbic Acid Fuel Cells. Int. J. Hydrogen Energy 2018, 43, 21908–21917. [Google Scholar] [CrossRef]
  44. Fujiwara, N.; Yamazaki, S.; Siroma, Z.; Ioroi, T.; Yasuda, K. Direct Oxidation of L-Ascorbic Acid on a Carbon Black Electrode in Acidic Media and Polymer Electrolyte Fuel Cells. Electrochem. Commun. 2006, 8, 720–724. [Google Scholar] [CrossRef]
  45. Fujiwara, N.; Yamazaki, S.; Siroma, Z.; Ioroi, T.; Yasuda, K. L-Ascorbic Acid as an Alternative Fuel for Direct Oxidation Fuel Cells. J. Power Sources 2007, 167, 32–38. [Google Scholar] [CrossRef]
  46. Fujiwara, N.; Siroma, Z.; Ioroi, T.; Yasuda, K. Rapid Evaluation of the Electrooxidation of Fuel Compounds with a Multiple-Electrode Setup for Direct Polymer Electrolyte Fuel Cells. J. Power Sources 2007, 164, 457–463. [Google Scholar] [CrossRef]
  47. Fujiwara, N.; Yasuda, K.; Ioroi, T.; Siroma, Z.; Miyazaki, Y.; Kobayashi, T. Direct Polymer Electrolyte Fuel Cells Using L-Ascorbic Acid as a Fuel. Electrochem. Solid-State Lett. 2003, 6, A257. [Google Scholar] [CrossRef]
  48. Du, J.; Cullen, J.J.; Buettner, G.R. Ascorbic Acid: Chemistry, Biology and the Treatment of Cancer. Biochim. Biophys. Acta Rev. Cancer 2012, 1826, 443–457. [Google Scholar] [CrossRef] [Green Version]
  49. Mogi, H.; Fukushi, Y.; Koide, S.; Sano, R.; Sasaki, T.; Nishioka, Y. A Flexible Ascorbic Acid Fuel Cell with a Microchannel Fabricated Using MEMS Techniques. J. Phys. Conf. Ser. 2013, 476, 012065. [Google Scholar] [CrossRef]
  50. Falk, M.; Andoralov, V.; Blum, Z.; Sotres, J.; Suyatin, D.B.; Ruzgas, T.; Arnebrant, T.; Shleev, S. Biofuel Cell as a Power Source for Electronic Contact Lenses. Biosens. Bioelectron. 2012, 37, 38–45. [Google Scholar] [CrossRef]
  51. Wu, J.; Xiao, Z.; Ying, Y.; Chan, P.C.H. Development of a Miniature Silicon Wafer Fuel Cell Using L-Ascorbic Acid as Fuel. J. Zhejiang Univ. A 2008, 9, 955–960. [Google Scholar] [CrossRef]
  52. Kaneto, K.; Nishikawa, M.; Uto, S. Characteristics of Ascorbic Acid Fuel Cells Using SWCNT and PEDOTPSS Composite Anodes. Chem. Lett. 2019, 48, 1533–1536. [Google Scholar] [CrossRef]
  53. Bianchini, C.; Shen, P.K. Palladium-Based Electrocatalysts for Alcohol Oxidation in Half Cells and in Direct Alcohol Fuel Cells. Chem. Rev. 2009, 109, 4183–4206. [Google Scholar] [CrossRef] [PubMed]
  54. Zalineeva, A.; Serov, A.; Padilla, M.; Martinez, U.; Artyushkova, K.; Baranton, S.; Coutanceau, C.; Atanassov, P.B. Self-Supported PdxBi Catalysts for the Electrooxidation of Glycerol in Alkaline Media. J. Am. Chem. Soc. 2014, 136, 3937–3945. [Google Scholar] [CrossRef]
  55. Muneeb, O.; Do, E.; Tran, T.; Boyd, D.; Huynh, M.; Ghosn, G.; Haan, J.L. A Direct Ascorbate Fuel Cell with an Anion Exchange Membrane. J. Power Sources 2017, 351, 74–78. [Google Scholar] [CrossRef]
  56. An, L.; Zhao, T.S.; Chen, R.; Wu, Q.X. A Novel Direct Ethanol Fuel Cell with High Power Density. J. Power Sources 2011, 196, 6219–6222. [Google Scholar] [CrossRef]
  57. Shang, Z.; Wycisk, R.; Pintauro, P. Electrospun Composite Proton-Exchange and Anion-Exchange Membranes for Fuel Cells. Energies 2021, 14, 6709. [Google Scholar] [CrossRef]
  58. Pan, Z.; Zhuang, H.; Bi, Y.; An, L. A Direct Ethylene Glycol Fuel Cell Stack as Air-Independent Power Sources for Underwater and Outer Space Applications. J. Power Sources 2019, 437, 226944. [Google Scholar] [CrossRef]
  59. Keramati, A.; Hendrix, K.; Nguyen, D.; Gonzales, F.; Waters, K.; Fry-Petit, A.; Haan, J.L. A Non-Precious Metal Ascorbate Fuel Cell. Int. J. Energy Res. 2021, 45, 1–11. [Google Scholar] [CrossRef]
  60. Li, Y.; Wu, H.; He, Y.; Liu, Y.; Jin, L. Performance of Direct Formate-Peroxide Fuel Cells. J. Power Sources 2015, 287, 75–80. [Google Scholar] [CrossRef]
  61. Li, Y.; Feng, Y.; Sun, X.; He, Y. A Sodium-Ion-Conducting Direct Formate Fuel Cell: Generating Electricity and Producing Base. Angew. Chem. Int. Ed. 2017, 56, 5734–5737. [Google Scholar] [CrossRef]
  62. Mondal, S.K.; Raman, R.K.; Shukla, A.K.; Munichandraiah, N. Electrooxidation of Ascorbic Acid on Polyaniline and Its Implications to Fuel Cells. J. Power Sources 2005, 145, 16–20. [Google Scholar] [CrossRef]
Electrochem 04 00003 g001 550
Figure 1. Alcohol fuel cells using (a) CEM and (b) AEM.
Figure 1. Alcohol fuel cells using (a) CEM and (b) AEM.
Electrochem 04 00003 g001
Electrochem 04 00003 g002 550
Figure 2. (a) Chemical structure of ascorbic acid and (b) ascorbic acid oxidation to produce dehydroascorbic acid.
Figure 2. (a) Chemical structure of ascorbic acid and (b) ascorbic acid oxidation to produce dehydroascorbic acid.
Electrochem 04 00003 g002
Electrochem 04 00003 g003 550
Figure 3. The relationship between power density and current density for DAAFCs using Vulcan XC72, Pt, Ru, Pd, Ir, Rh, and PtRu anode catalysts and Pt-PTFE black as cathode catalysts at room temperature using Nafion 117 membrane. Reproduced with permission [45]. Copyright 2007 Elsevier B.V.
Figure 3. The relationship between power density and current density for DAAFCs using Vulcan XC72, Pt, Ru, Pd, Ir, Rh, and PtRu anode catalysts and Pt-PTFE black as cathode catalysts at room temperature using Nafion 117 membrane. Reproduced with permission [45]. Copyright 2007 Elsevier B.V.
Electrochem 04 00003 g003
Electrochem 04 00003 g004 550
Figure 4. Voltage–current plots of alkaline DAAFC at 60 °C with 1 M ascorbate + 1 M KOH (anode) and oxygen (cathode). Reproduced with permission [37]. Copyright 2018 Elsevier Ltd.
Figure 4. Voltage–current plots of alkaline DAAFC at 60 °C with 1 M ascorbate + 1 M KOH (anode) and oxygen (cathode). Reproduced with permission [37]. Copyright 2018 Elsevier Ltd.
Electrochem 04 00003 g004
Electrochem 04 00003 g005 550
Figure 5. (a) Working principle of the split-pH DAAFC, (b) VI plots of the split-pH DAAFC with anode fuel 1 M ascorbate + 1 M NaOH (pH 14) and cathode oxidant is 3 or 30% H2O2 + 1 M H2SO4 (pH 0). Reproduced with permission [41]. Copyright 2018 Elsevier B.V.
Figure 5. (a) Working principle of the split-pH DAAFC, (b) VI plots of the split-pH DAAFC with anode fuel 1 M ascorbate + 1 M NaOH (pH 14) and cathode oxidant is 3 or 30% H2O2 + 1 M H2SO4 (pH 0). Reproduced with permission [41]. Copyright 2018 Elsevier B.V.
Electrochem 04 00003 g005
Table
Table 1. Summarized data of AA-based fuel cell.
Table 1. Summarized data of AA-based fuel cell.
Anode (Catalyst Loading)Anode FuelFlow (mL/min)Cathode (Catalyst Loading)Cathode FuelFlow (mL/min)MembraneTemp. (°C)Peak Power Density (mW/cm2)Current Density (mA/cm2)Ref.
Acid-treated Vulcan XC-72 (2 mg/cm2)1 M AA and 1 M NaOH2Acid-treated Vulcan XC-72 (2 mg/cm2)30% H2O2 and 1 M H2SO45NaOH treated Nafion 115 CEM60158~475[41]
PdCu/C (2 mg/cm2)1 M AA and 1 M KOH1Pt black (4 mg/cm2)O2100Tokuyama A201 AEM6089~560[37]
Pd catalyst (4 mg/cm2)1 M AA and 1 M KOH5Pt black (2 mg/cm2)O2100Tokuyama A201 AEM6073497[55]
Cu/C (5 mg/cm2)1 M AA and 2 M NaOH1Carbon (5 mg/cm2)3% H2O2 and 1 M H2SO42NaOH treated Nafion 115 CEM6051~240[59]
Acid treated carbon (1 mg/cm2)1 mM AA + 0.5 M H2SO415Pt/C (1 mg/cm2)O2200Nafion 2118031~180[43]
Oxidized Carbon (SGL 35AA) (no metal loading)1 M AA5Pt on Carbon (SGL 35BC GDL) (3 mg/cm2)O2200Nafion 115 CEM6018~90[38]
Vulcan XC72 on PTFE sheet (3 mg/cm2)0.5 M AA4Pt black on PTFE sheet (3 mg/cm2)O2100Nafion 117 CEM2516~115[45]
Vulcan XC72 (0.3 mg/cm2)0. 5 M AA + 0.5 M H2SO44Pt–PTFE black (3 mg/cm2)O2100Nafion-117 CEM2515~85[44]
aSWCNT@PEDOT*PSS (1 mg/cm2)0.5 M AA2Pt black (3 mg/cm2)O2100Nafion 117 CEM2511.3~60[52]
Poly aniline on TGPH 090 (35 mg/cm2)1 M AA in 0.5 M H2SO4-Pt on TGPH 090 (no information)O2-Nafion 117 CEM704.315[62]
Acid treated Carbon on Toray-060 (1 mg/cm2)0.5 M AA4Pt/C on (SGL, 10BC) (1 mg/cm2)O2100Nafion 115 CEM36.5~0.053~0.66[39]
Disclaimer/Publisher’s Note: The statements, opinions and data contained in all publications are solely those of the individual author(s) and contributor(s) and not of MDPI and/or the editor(s). MDPI and/or the editor(s) disclaim responsibility for any injury to people or property resulting from any ideas, methods, instructions or products referred to in the content.

Share and Cite

MDPI and ACS Style

Hasan, M.M. Environment-Friendly Ascorbic Acid Fuel Cell. Electrochem 2023, 4, 31-41. https://doi.org/10.3390/electrochem4010003

AMA Style

Hasan MM. Environment-Friendly Ascorbic Acid Fuel Cell. Electrochem. 2023; 4(1):31-41. https://doi.org/10.3390/electrochem4010003

Chicago/Turabian Style

Hasan, Md. Mahmudul. 2023. "Environment-Friendly Ascorbic Acid Fuel Cell" Electrochem 4, no. 1: 31-41. https://doi.org/10.3390/electrochem4010003

Article Metrics

Back to TopTop