Search tips
Search criteria 


Logo of nanomatLink to Publisher's site
Nanomaterials (Basel). 2016 December; 6(12): 238.
Published online 2016 December 9. doi:  10.3390/nano6120238
PMCID: PMC5302713

Nano Copper Oxide-Modified Carbon Cloth as Cathode for a Two-Chamber Microbial Fuel Cell

Thomas Nann, Academic Editor


In this work, Cu2O nanoparticles were deposited on a carbon cloth cathode using a facile electrochemical method. The morphology of the modified cathode, which was characterized by scanning electron microscopy (SEM) and Brunauer-Emmett-Teller (BET) tests, showed that the porosity and specific surface area of the cathode improved with longer deposition times. X-ray photoelectron spectroscopy (XPS) and cyclic voltammetry (CV) results showed that cupric oxide and cuprous oxide coexisted on the carbon cloth, which improved the electrochemical activity of cathode. The cathode with a deposition time of 100 s showed the best performance, with a power density twice that of bare carbon cloth. Linear sweep voltammetry (LSV) and electrochemical impedance spectroscopy (EIS) results revealed that moderate deposition of nano copper oxide on carbon cloth could dramatically reduce the charge transfer resistance, which contributed to the enhanced electrochemical performance. The mediation mechanism of copper oxide nanocatalyst was illustrated by the fact that the recycled conversion between cupric oxide and cuprous oxide accelerated the electron transfer efficiency on the cathode.

Keywords: microbial fuel cells, nanocatalyst, electrodeposition, cathode, copper

1. Introduction

Microbial fuel cells (MFCs) harness the power of a microorganism and convert energy released in metabolic reactions into electrical energy. This environmentally-friendly process produces electricity without the combustion of fossil fuels. Catalysts used to fabricate MFC cathodes are mostly noble metals, such as platinum (Pt). However, the high cost of noble metals inhibits their use in large-scale production of MFCs [1].

Copper is considered to be an important element for cathode catalysis in fuel cells due to its low cost and high stability. Previous studies have demonstrated that the electron-catalytic activity of copper deposited on a carbon cathode for oxygen reduction reaction was fairly good at low oxygen pressure [2]. Recently, it has also been found that Cu2O exhibited excellent electron-catalytic activity for the reduction of oxygen. Cathodes decorated by alloys containing copper and other elements, such as Pt, Pd, Mn, and Ir, were developed to replace costly platinum cathodes and showed high power output [3,4,5,6]. In addition, a Pt cathode modified by copper oxide was reported to have the potential for oxygen reduction, and the oxidation state of Cu enables the Cu to act as an adsorption site of oxygen [7]. In addition to oxygen reduction, nitrates and nitrites can be electrochemically reduced by the catalytic activity of copper. Other metals, such as nickel [8], tin [9], zinc [10,11], palladium [12], and rhodium [13] have the same effect. Even carbon monoxide and carbon dioxide have been reported to be the objects of electrocatalytic reduction using cathodes decorated by copper-containing material [14] or copper electrodes [15]. The above-mentioned research indicated the extensive and profound usefulness of copper for improving the efficiency of substrate reduction at the cathode.

However, there is little research about the performance and mechanism of treated carbon cloth by electrodeposited copper in MFC. In this work, a carbon cloth cathode modified by nano copper oxide was prepared using a simple electrochemical method. The effects of deposition time on morphology and catalytic activity of copper oxide were also examined. MFC with potassium ferricyanide as an electron acceptor has high voltage, low internal resistance, and good stability, and it is suited for research purposes [16,17,18]. Baker’s yeast, Saccharomyces cerevisiae, has been studied as a biocatalyst for use in biofuel cells [19,20,21], because it has many attractive features, i.e., nonpathogenic, inexpensive, easy mass cultivation, and can be maintained for a long time in a dried state. Therefore, we utilized potassium ferricyanide as an electron acceptor and yeast as a biocatalyst in this study.

2. Results and Discussion

2.1. Scanning Electron Microscopy (SEM) and Brunauer-Emmett-Teller (BET) Characterization

Figure 1 showed the size of copper oxide particles on the surface of the carbon cloth increased as the deposition time increased. No Cu2O particles were found on the bare carbon cloth. The particles with deposition time of 50 s were irregular in shape and sizes and were distributed normally with a diameter of approximately 100 nm, whereas more homogeneous and larger sized (approximately 200 nm) particles were found with a deposition time of 100 s. As the Cu deposition time increased, the size of the particles increased, and the spaces between them became smaller, leading to smaller specific surface areas. As shown in Figure 1, particles with a deposition time of 150 s stood ‘shoulder to shoulder’, which decreased the porosity and the specific surface area of the modified electrode. The corresponding Brunauer-Emmett-Teller (BET) results showed that the specific surface area of the modified electrodes, with deposition times of 50, 100 and 150 s, were 0.1630, 0.2841 and 0.2673 m2/g, respectively, indicating that the specific surface area of the cathode improved with longer deposition times, but excessive deposition time led to decreasing specific surface area.

Figure 1
Scanning electron microscopy (SEM) images of the surface of copper oxide-coated carbon cloth. These carbon cloths were modified with deposition times of 0 (a), 50 (b), 100 (c), and 150 s (d), respectively.

2.2. X-ray Photoelectron Spectroscopy Results

X-ray photoelectron spectroscopy (XPS) was used to determine the state of the copper on the cathode. Wide-scan XPS survey spectra were obtained from the modified carbon cloth (Figure 2a) and the bare carbon cloth (Figure 2a inset), and the modified carbon cloth was applied as cathode in the MFC for a period of time. The spectra showed that Cu and Fe appeared on the modified carbon cloth in addition to C, O and N and the distributions are shown in Table 1. The presence of Fe and the increase in N on the modified carbon cloth may be attributed to adsorption on the cathode of the ferricyanide in the solution. This result is supported by the measured ratio of Fe to N on the modified carbon cloth being 5.14%:30.13%, which is similar to the ratio in ferricyanide (1:6). Figure 2b shows the core-level Cu 2p region of an XPS spectrum acquired from the modified carbon cloth and a curve-fit to the spectrum. Spectrum noise was attributed to the short acquisition time that was used to avoid the photo-reduction of Cu(II) ions by the action of X-rays [22]. The presence of the well-known shake-up peak indicated the presence of Cu(II) species [23]. Other states of Cu are also present, based on the wide shake-up peak type [24,25]. The large asymmetric mean peak could be decomposed into three contributions at 933.00 eV, 934.7 eV and 935.78 eV (Table 1). The contributions at 934.7 eV and 935.78 eV, according to the literature [23], are due to CuO and Cu(OH)2 [26,27], respectively. The first peak at 933.00 eV cannot be specifically identified due to the presence of statistically similar binding energy (BE) values for Cu metal and Cu (I) oxide species. Auger peak position has been used to identify the oxidation state of copper. Previous reports [28,29] had noted a distinctive Cu LMM (L-inner level-M-inner level-M-inner level electron transition) peak at 569.99 eV for Cu2O, which is in accord with the Cu LMM Auger peak position of this result (Cu LMM peak at 569.89 eV). Therefore, based on the observed oxidative states of copper, our results indicate that Cu(I) and Cu(II) coexist on the cathode. Thus, the major components deposited on the carbon cloth electrode were Cu in different oxidative states.

Figure 2
X-ray photoelectron spectroscopy (XPS) spectra of the cathode materials. (a) Wide-scan XPS survey spectra of the modified carbon cloth after being applied as cathode in the microbial fuel cell (MFC) for a period of time. Inset: bare carbon cloth. (b) ...
Table 1
Assignments of main spectral bands for carbon cloth and modified carbon cloth. The bands are based on their binding energies (BE) and atomic concentration (AC).

XPS spectra, showing Cu 2p and Cu LMM regions, from the electrodeposited carbon cloth that had not been used in the MFC were showed in Figure 2c. The material was dried in a holder at room temperature for 24 h. The figure showed characteristics typical of CuO: The binding energy of Cu 2p being 934.7 eV; the strong shake-up peak of the Cu 2p spectrum; and he peak kinetic energy of Cu LMM spectrum being 916.8 eV. So CuO alone was present on the carbon cloth after electrodeposition. Cu(OH)2 was not found on this electrodeposited carbon cloth, and this may be caused by the long drying process, during which the Cu(OH)2 converted to CuO.

The following mechanism has been proposed for the formation of CuO on the carbon cloth [30].

Electrodeposition of Cu:

Cu2+ + 2e → Cu,

Formation of Cu(OH)2:

Cu + 2OH → Cu(OH)2 + 2e,

Formation of CuO:

Cu(OH)2 → CuO + H2O,

The proposed mechanism suggests that there is initial formation of Cu(OH)2 which then converts into CuO. However, as mentioned above, CuO and Cu2O coexist on the cathode after this carbon cloth was applied in the MFC for a period of time. The conversion between the two oxidation states of copper on the carbon cloth cathode may initiate different electrochemical performance which is displayed next.

2.3. Performance of MFCs Equipped with the Modified Carbon Cloth Cathodes

Tests of MFCs with the modified cathodes were conducted to determine the influence of the deposition on the MFC power generation. Upon variation of the deposition time, the power density curves were also obtained (Figure 3).

Figure 3
Power densities of four microbial fuel cells (MFCs) with different deposition times.

As shown in Figure 3, The open circuit voltages (OCV) observed here were approximately 600 mV, which were higher than the values in a previous report [31], but were in accord with Hubenova’s research [32]. The maximum power density of the MFC with a deposition time of 100 s was found to be 308.69 mW/m2, over two times higher than that of the bare cathode (121.51 mW/m2). The maximum power density of the bare cathode was on the same level as other reports [32,33]. MFCs of modified cathodes with deposition times of 50 s (252 mW/m2) and 150 s (237 mW/m2) also displayed higher power density than the bare carbon cloth cathode did.

From slopes of the polarization curves in Figure 3, the internal resistances (Rint) of the cell were estimated: 948.88 Ω (0 s), 585.81 Ω (50 s), 374.15 Ω (100 s), and 464.07 Ω (150 s). The Rint of MFCs with modified cathodes were significantly lower than that of the bare cathode, and the Rint of the MFC with a deposition time of 100 s was less than half of the bare cathode MFC’s Rint. This reduction in Rint may be the result of catalysis by the deposited material. The better performance of the modified carbon cloth also found expression in a higher short circuit current density of 0.94 A/m2 in comparison with 0.50 A/m2 for the bare carbon cloth.

These results clearly showed that modification of the carbon cloth could enhance the MFC power output performance, which corresponded with catalysis by copper [34,35]. The best performance was observed with the deposition time of 100 s. This phenomenon was due to the electroactivity being affected by deposition time [30].

2.4. Electrochemical Characterization of Cu Oxide-Coated Carbon Cloth Cathode

To provide further insight into the role of coated Cu oxide in the catalysis process, different electrochemical characterizations were conducted. Figure 4 showed the cyclic voltammograms (CVs) of the Cu oxide-coated carbon cloths with different deposition times in a potassium ferricyanide solution (50 mM). The peaks of one distinct redox couple with potentials of about −0.1 V and 0.6 V are clearly seen both for the modified carbon cloths and the bare carbon cloth. These redox peaks are related to the oxidation and reduction of ferrocyanide and ferricyanide at the surface of the carbon cloth [36]. In contrast, another redox couple was found with potentials of approximately 0.6 V and 1 V only for the modified carbon cloths. These results show that there is another redox couple that occurs on the modified carbon cloths besides the ferrocyanide and ferricyanide redox. This is consistent with the XPS results that indicate that there are only two oxidative states of Cu present, corresponding to this redox couple. This reductive peak is due to the reduction of CuO to Cu2O on the surface of the electrode, which is easier than the reduction of ferricyanide, whose reductive potential was more negative. A similar result had been reported before [35], with CuO nanoparticles playing a role in the increase of the electroactive surface area, but the mechanism had not been explained.

Figure 4
Cyclic voltammetry (CV) of copper-coated carbon cloths. These carbon cloths had deposition times of 0, 50, 100 and 150 s, respectively.

Theoretically, in a potassium ferricyanide solution with high oxidative ability, the Cu2O could be easily oxidized to form CuO [30]:

2CuO + 2H++ 2e → Cu2O + H2O,

[Fe(CN)6]3 + e → [Fe(CN)6]4,

According to equations 4 and 5, the total reaction was:

2[Fe(CN)6]3 + Cu2O + H2O → 2[Fe(CN)6]4 + 2CuO + 2H+,

Figure 5 shows the linear sweep voltammetry (LSV) polarization curves of Cu oxide-coated cathodes. The slopes of the cathode voltage–current densities are different with the increasing order of 0 s (bare carbon cloth) < 50 s < 150 s < 100 s. The polarization degree of the bare carbon cloth cathode is much greater than that of Cu oxide-coated carbon cloths, indicating that the Cu oxide-coated cathodes have better electrochemical property, which is consistent with the CV results.

Figure 5
Linear sweep voltammetry (LSV) curves of the bare carbon cloth and the Cu oxide-coated carbon cloths with different deposition times in a 50 mM potassium ferricyanide solution.

Figure 6 shows the Nyquist plot for Cu oxide-coated carbon cloths. The total resistance includes the ohmic resistance (Ro), charge transfer resistance (Rct) and diffusion resistance (Rd). Rct is the major kinetic limitation due to slow activation reaction rates on the cathode. Rct of the cathodes have an apparent trend, with the order of: 0 s (bare carbon cloth) > 50 s > 150 s >100 s. The Rct of bare carbon cloth was 1309 Ω, which was 59.23 times as much as that of cathode with deposition time of 100 s (22.10 Ω) (Table 2).

Figure 6
Nyquist plots of electrochemical impedance spectroscopy (EIS) by the Cu oxide-coated carbon cloths with different deposition times.
Table 2
Electrochemical impedance fitting results of different cathodes.

Cu oxide deposited on the surface of carbon cloth can enhance the electron transfer rate between the current collector and ferricyanide, leading to the decrease of charge transfer resistance. Hence, Rct decreases with the increase in deposition time from 0 s to 100 s. However, too much coating of Cu oxide may reduce the specific surface area (Figure 1) and leads to decreased mass transport, which will reduce the cell performance. That is the reason why an optimum deposition time of 100 s exists. These results are consistent with those of CV and LSV tests.

2.5. Catalytic Mechanism of Copper Oxide Nanocatalyst

As mentioned before, the CuO on the MFC cathode is first reduced to Cu2O by the electrons from the anode; and then, Cu2O is oxidized to CuO by the ferricyanide, and this constitutes a redox cycle mediated on the cathode [37,38]. A schematic diagram of the mechanism is shown in Figure 7. Therefore, the improvement in performance of the MFCs may be the result of the mediation mechanism associated with the Cu oxide film interacting with the ferricyanide solution. It has been reported that copper behaves as a charge mediator for electrocatalytic reduction of nitrite species under neutral conditions [39], which is the same mechanism as has been presented in this paper.

Figure 7
The mechanism of Cu oxide’s intermediation functions on the cathode in ferricyanide solution. The CuO on the cathode surface is first reduced to Cu2O by the electrons from the anode, and then Cu2O is oxidized to CuO by the ferricyanide. This redox ...

The MFC performances and electrochemical characterization results indicate that the Cu oxide-coated carbon cloth with an intermediate deposition time (100 s) had the highest electrochemical activity. Patake et al. [30] have reported that the electrochemical activity of copper oxide increases with increasing deposition time and with increasing film thickness. The Cu oxide film with a deposition time of 100 s led to better MFC performance, corresponding to reduced charge transfer resistance and increased porosity of surface structure. These results are similar to those observed by other researchers [40]. Thus, improvement of the MFC performance is attributed to the enhanced kinetics and the porosity of the copper oxide film on the electrode.

It should also be mentioned that BET results were not completely consistent with the maximum power densities. Although 100 s and 150 s have almost same surface area, their peak power densities are different, which indicated that the specific surface was not the only factor affecting the performance of MFC. There should be other factors such as the impact of the quantity of deposited copper on carbon cloth, the catalytic activity of copper oxide, and so on. Although the electrochemical characterization and cell performance evaluation of the nano Cu oxide-modified cathodes have been conducted in this work, some other issues, such as long-term stability and use of different electron acceptors, should also be considered in further study in order to advance its practical application.

3. Materials and Methods

3.1. Electrode Materials and Chemicals

Carbon cloth was employed as the cathode material. The carbon cloth was purchased from Heshen, Inc. (Shanghai, China). Modified carbon cloth was prepared by electrodeposition using a potentiostatic plating technique. The surface area of the carbon cloth was 1 cm2. It was hooked onto the titanium wire and then immersed into the electrolyte used for electrodeposition, which contained CuSO4 (50 mM), sodium citrate (5 mM), and glucose (20 mM). All chemicals were of analytical grade and were used without further purification. The electrodeposition was performed in a conventional three-electrode cell with platinum wire as a counter electrode and Ag/AgCl as a reference electrode using a Corrtest CS120 model electrochemical workstation (Wuhan, China). The electroplating bath temperature was kept constant at 25 °C by thermostat. The polarization potential of the applied potentiostatic regimes was −0.65 V [41].

3.2. MFC Construction and Operation

The catalytic effects of the electrodeposited carbon cloth cathodes were investigated by using them as cathodes in a double-chamber mediatorless yeast-biofuel cell. The cathodic electrolyte was prepared using 50 mM potassium ferricyanide in phosphate buffer solution (PBS) and refreshed every three days. To prepare the PBS, we dissolved 0.27 g KH2PO4, 1.42 g Na2HPO4, 8 g NaCl and 0.2 g KCl in 800 mL of H2O. Then adjusted the pH to 7.4 with HCl, and added H2O until the final volume was 1.00 L. The anode was a round carbon felt with a diameter of 3 cm. Titanium wire was used to connect both the anode and the cathode to the external circuit in order to avoid corrosion of wires due to the electrolyte. The electrodes were fixed in the corresponding anodic and cathodic plastic chamber, each with a volume of 14 cm3, and separated from the other by a proton-exchange membrane. The carbon cloth that was to be tested was hooked onto the titanium wire and then immersed into the ferricyanide solution.

Saccharomyces cerevisiae was cultivated in yeast peptone medium (YP medium) in an incubator at 30 °C for 16 h to increase the cell biomass. The YP medium was composed of 0.5% yeast extract, 0.8% peptone and 1% glucose, and the pH was maintained at approximately 7 by dissolving these substrates in PBS. After 16 h of cultivation, the medium was injected into the anode chamber, with the biomass of the microorganism having reached a maximum value according to a previous test. Fed-batch MFC operation was performed with a constant load resistance (1 K) as external resistance. After 24 h of operation, half of the anolyte was substituted with yeast-free YP medium.

3.3. Electrochemical and Physical Measurements

CVs were measured using a three-electrode conventional cell with the Corrtest CS120 model electrochemical workstation [42]. LSV and EIS were conducted on a CHI 660E electrochemical workstation (Shanghai Chen Hua Instrument Co., Ltd., Shanghai, China). The carbon cloth cathode, Pt electrode, and Ag/AgCl electrode (0.207 V vs. SHE) were used as working, counter, and reference electrode, respectively. CV was measured at a scan rate of 2 mV/s. The current density was calculated based on the cathode area in accordance with Ohm’s law. LSV was measured from the open circuit potential (OCP) to 0 V at a scan rate of 0.1 mV·s−1. EIS test was conducted at a frequency range of 100 kHz to 10 mHz with amplitude of 5 mV.

Power density measurements were made using a resistance box at various resistances (10 K to 100 Ω). The cell voltage was recorded using a multimeter [32]. Power density was estimated for each voltage-current density pair on the basis of Joule’s law P = U × I and the corresponding power density curves were also drawn as power density vs. current density plots.

XPS (Axis Ultra DLD, Shimadzu, Kyoto, Japan) was used to evaluate elemental compositions and the chemical states of the copper. The analyzed area of the sample was approximately 0.25 cm2. An overview spectrum (0–1200 eV) and narrow regions corresponding to Cu 2p (928–990 eV) were recorded. Deconvolution of the main Cu 2p peaks was performed using Casa XPS software. The cathode material, which was used in the MFC, was removed and washed with distilled water for the test. In addition, electrodeposited carbon cloth that had not been used in the MFC was also tested.

Scanning electron microscopy (SEM, Nanosem 430, FEI, Eindhoven, Netherlands) was used to analyze the morphology of the modified and the bare carbon cloth surface. 5 × 20 mm pieces of the carbon cloth were attached to a piece of glass by conductive tape and were prepared for SEM analysis. Magnifications of 20000× and 100000× were used to inspect the state of the entire film and individual particles, respectively. Specific surface area determination was performed using the BET method with an adsorption meter (ASAP 2020/Tristar 3000, MICROMERITICS, Norcross, GA, USA).

4. Conclusions

In summary, copper oxide-coated carbon cloth, which had porous surfaces and an intermediation function, was used for cathodes in MFCs with ferricyanide as an electron acceptor. Cu oxide-coating improved the performance of carbon cloth cathodes. The maximum power density of the MFC with copper oxide-coated carbon cloth with 100 s of deposition reached 308.69 mW/m2, more than doubled when compared with bare carbon cloth of 121.51 mW/m2. The copper oxide is first reduced by the electrons from the anode to cuprous oxide in the microbial fuel cell, then the cuprous oxide is oxidized to copper oxide by potassium ferricyanide, which forms a redox cycle in the cathode. This redox cycle actually improved the performance of MFC. The improved performance was mainly attributed to the porous surface of the cathode and to the fast and reversible redox reactions between the oxidation states of Cu(II) and Cu(I). With the prolongation of the deposition time, the mass of the deposited copper oxide and the specific surface area of the electrode gradually increased. However, too long of a deposition time leads to the decrease of specific surface area, which reduced the electrocatalytic performance of the electrode and the performance of the fuel cell. This phenomenon was observed for the first time and the corresponding mechanism was identified. This work can help to improve our understanding of the reduction mechanisms of catalytic agents on cathodes.


This work was partially supported by the Natural Science Foundation of Tianjin City (No. 15JCYBJC21400).


The following abbreviations are used in this manuscript:

microbial fuel cell
scanning electron microscopy
X-ray photoelectron spectroscopy
cyclic voltammetry
linear sweep voltammetry
electrochemical impedance spectroscopy
open circuit voltage

Author Contributions

Author Contributions

Xianhua Liu, Kexun Li, and Pingping Zhang conceived and designed the experiments; Feng Dong and Peng Zhang performed the experiments, analyzed the data, and wrote the paper.

Conflicts of Interest

Conflicts of Interest

The authors declare no conflict of interest.


1. Zhang P., Liu X.H., Li K.X., Song Z.Q. Optimization of Fabrication Parameters to Enhance the Performance of Activated Carbon Air-Cathode. J. Electrochem. Soc. 2015;162:F1347–F1355. doi: 10.1149/2.0501512jes. [Cross Ref]
2. Nabae Y., Yamanaka I., Otsuka K. Electro-catalysis of the Cu/carbon cathode for the reduction of O2 during fuel-cell reactions. Appl. Catal. A. 2005;280:149–155. doi: 10.1016/j.apcata.2004.10.050. [Cross Ref]
3. You D.J., Jin S.A., Lee K.H., Pak C., Choi K.H., Chang H. Improvement of activity for oxygen reduction reaction by decoration of Ir on PdCu/C catalyst. Catal. Today. 2012;185:138–142. doi: 10.1016/j.cattod.2011.08.024. [Cross Ref]
4. Xu Z., Zhang H.M., Liu S.S., Zhang B.S., Zhong H.X., Su D.S. Facile synthesis of supported Pt-Cu nanoparticles with surface enriched Pt as highly active cathode catalyst for proton exchange membrane fuel cells. Int. J. Hydrogen Energy. 2012;37:17978–17983. doi: 10.1016/j.ijhydene.2012.09.050. [Cross Ref]
5. Xiong L., Kannan A.M., Manthiram A. Pt-M (M = Fe, Co, Ni and Cu) electrocatalysts synthesized by an aqueous route for proton exchange membrane fuel cells. Electrochem. Commun. 2002;4:898–903. doi: 10.1016/S1388-2481(02)00485-X. [Cross Ref]
6. Alia S.M., Jensen K., Contreras C., Garzon F., Pivovar B., Yan Y. Platinum Coated Copper Nanowires and Platinum Nanotubes as Oxygen Reduction Electrocatalysts. ACS Catal. 2013;3:358–362. doi: 10.1021/cs300664g. [Cross Ref]
7. Tsujimura S., Miura Y., Kano K. CueO-immobilized porous carbon electrode exhibiting improved performance of electrochemical reduction of dioxygen to water. Electrochim. Acta. 2008;53:5716–5720. doi: 10.1016/j.electacta.2008.03.037. [Cross Ref]
8. Mattarozzi L., Cattarin S., Comisso N., Guerriero P., Musiani M., Vazquez-Gomez L., Verlato E. Electrochemical reduction of nitrate and nitrite in alkaline media at CuNi alloy electrodes. Electrochim. Acta. 2013;89:488–496. doi: 10.1016/j.electacta.2012.11.074. [Cross Ref]
9. Macova Z., Bouzek K., Serak J. Electrocatalytic activity of copper alloys for NO3 reduction in a weakly alkaline solution-Part 2: Copper-tin. J. Appl. Electrochem. 2007;37:557–566. doi: 10.1007/s10800-006-9287-8. [Cross Ref]
10. Li M., Feng C., Zhang Z., Shen Z., Sugiura N. Electrochemical reduction of nitrate using various anodes and a Cu/Zn cathode. Electrochem. Commun. 2009;11:1853–1856. doi: 10.1016/j.elecom.2009.08.001. [Cross Ref]
11. Fan N., Li Z., Zhao L., Wu N., Zhou T. Electrochemical denitrification and kinetics study using Ti/IrO2-TiO2-RuO2 as the anode and Cu/Zn as the cathode. Chem. Eng. J. 2013;214:83–90. doi: 10.1016/j.cej.2012.10.026. [Cross Ref]
12. Gauthard F., Epron F., Barbier J. Palladium and platinum-based catalysts in the catalytic reduction of nitrate in water: effect of copper, silver, or gold addition. J. Catal. 2003;220:182–191. doi: 10.1016/S0021-9517(03)00252-5. [Cross Ref]
13. Comisso N., Cattarin S., Fiameni S., Gerbasi R., Mattarozzi L., Musiani M., Vazquez-Gomez L., Verlato E. Electrodeposition of Cu-Rh alloys and their use as cathodes for nitrate reduction. Electrochem. Commun. 2012;25:91–93. doi: 10.1016/j.elecom.2012.09.026. [Cross Ref]
14. Huang T.-J., Chou C.-L. Electrochemical CO2 reduction with power generation in SOFCs with Cu-added LSCF-GDC cathode. Electrochem. Commun. 2009;11:1464–1467. doi: 10.1016/j.elecom.2009.05.031. [Cross Ref]
15. Kortlever R., Tan K.H., Kwon Y., Koper M.T.M. Electrochemical carbon dioxide and bicarbonate reduction on copper in weakly alkaline media. J. Solid State Electrochem. 2013;17:1843–1849. doi: 10.1007/s10008-013-2100-9. [Cross Ref]
16. Chen S.L., Chen Y., He G.H., He S.J., Schroder U., Hou H.Q. Stainless steel mesh supported nitrogen-doped carbon nanofibers for binder-free cathode in microbial fuel cells. Biosens. Bioelectron. 2012;34:282–285. doi: 10.1016/j.bios.2011.10.049. [PubMed] [Cross Ref]
17. Tamakloe R.Y. Effect of COD and H2O2 concentration on DC-MFC. Renew Energ. 2015;83:1299–1304. doi: 10.1016/j.renene.2015.04.046. [Cross Ref]
18. Wetser K., Sudirjo E., Buisman C.J.N., Strik D.P.B.T.B. Electricity generation by a plant microbial fuel cell with an integrated oxygen reducing biocathode. Appl. Energ. 2015;137:151–157. doi: 10.1016/j.apenergy.2014.10.006. [Cross Ref]
19. Kaneshiro H., Takano K., Takada Y., Wakisaka T., Tachibana T., Azuma M. A milliliter-scale yeast-based fuel cell with high performance. Biochem. Eng. J. 2014;83:90–96. doi: 10.1016/j.bej.2013.12.011. [Cross Ref]
20. Raghavulu S.V., Goud R.K., Sarma P.N., Mohan S.V. Saccharomyces cerevisiae as anodic biocatalyst for power generation in biofuel cell: Influence of redox condition and substrate load. Bioresource Technol. 2011;102:2751–2757. doi: 10.1016/j.biortech.2010.11.048. [PubMed] [Cross Ref]
21. Sayed E.T., Tsujiguchi T., Nakagawa N. Catalytic activity of baker’s yeast in a mediatorless microbial fuel cell. Bioelectrochemistry. 2012;86:97–101. doi: 10.1016/j.bioelechem.2012.02.001. [PubMed] [Cross Ref]
22. Poulston S., Parlett P., Stone P., Bowker M. Surface oxidation and reduction of CuO and Cu2O studied using XPS and XAES. Surf. Interface Anal. 1996;24:811–820. doi: 10.1002/(SICI)1096-9918(199611)24:12<811::AID-SIA191>3.0.CO;2-Z. [Cross Ref]
23. Biesinger M.C., Lau L.W.M., Gerson A.R., Smart R.S.C. Resolving surface chemical states in XPS analysis of first row transition metals, oxides and hydroxides: Sc, Ti, V, Cu and Zn. Appl. Surf. Sci. 2010;257:887–898. doi: 10.1016/j.apsusc.2010.07.086. [Cross Ref]
24. Chusuei C.C., Brookshier M.A., Goodman D.W. Correlation of relative X-ray photoelectron spectroscopy shake-up intensity with CuO particle size. Langmuir. 1999;15:2806–2808. doi: 10.1021/la9815446. [Cross Ref]
25. Velu S., Suzuki K., Okazaki M., Kapoor M.P., Osaki T., Ohashi F. Oxidative steam reforming of methanol over CuZnAl(Zr)-oxide catalysts for the selective production of hydrogen for fuel cells: Catalyst characterization and performance evaluation. J. Catal. 2000;194:373–384. doi: 10.1006/jcat.2000.2940. [Cross Ref]
26. Dubal D.P., Dhawale D.S., Salunkhe R.R., Jamdade V.S., Lokhande C.D. Fabrication of copper oxide multilayer nanosheets for supercapacitor application. J. Alloys Compd. 2010;492:26–30. doi: 10.1016/j.jallcom.2009.11.149. [Cross Ref]
27. Al-Kuhaili M.F. Characterization of copper oxide thin films deposited by the thermal evaporation of cuprous oxide (Cu2O) Vacuum. 2008;82:623–629. doi: 10.1016/j.vacuum.2007.10.004. [Cross Ref]
28. Goh S.W., Buckley A.N., Lamb R.N., Rosenberg R.A., Moran D. The oxidation states of copper and iron in mineral sulfides, and the oxides formed on initial exposure of chalcopyrite and bornite to air. Geochim. Cosmochim. Acta. 2006;70:2210–2228. doi: 10.1016/j.gca.2006.02.007. [Cross Ref]
29. Le M., Ren M., Zhang Z., Sprunger P.T., Kurtz R.L., Flake J.C. Electrochemical Reduction of CO2 to CH3OH at Copper Oxide Surfaces. J. Electrochem. Soc. 2011;158:E45–E49. doi: 10.1149/1.3561636. [Cross Ref]
30. Patake V.D., Joshi S.S., Lokhande C.D., Joo O.-S. Electrodeposited porous and amorphous copper oxide film for application in supercapacitor. Mater. Chem. Phys. 2009;114:6–9. doi: 10.1016/j.matchemphys.2008.09.031. [Cross Ref]
31. Gunawardena A., Fernando S., To F. Performance of a Yeast-mediated Biological Fuel Cell. Int. J. Mol. Sci. 2008;9:1893–1907. doi: 10.3390/ijms9101893. [PMC free article] [PubMed] [Cross Ref]
32. Hubenova Y.V., Rashkov R.S., Buchvarov V.D., Arnaudova M.H., Babanova S.M., Mitov M.Y. Improvement of Yeast–Biofuel Cell Output by Electrode Modifications. Ind. Eng. Chem. Res. 2010;50:557–564. doi: 10.1021/ie1000949. [Cross Ref]
33. Hubenova Y., Rashkov R., Buchvarov V., Babanova S., Mitov M. Nanomodified NiFe- and NiFeP-carbon felt as anode electrocatalysts in yeast-biofuel cell. J. Mater. Sci. 2011;46:7074–7081. doi: 10.1007/s10853-011-5502-z. [Cross Ref]
34. Yin M., Wu C.K., Lou Y.B., Burda C., Koberstein J.T., Zhu Y.M., O’Brien S. Copper oxide nanocrystals. J. Am. Chem. Soc. 2005;127:9506–9511. doi: 10.1021/ja050006u. [PubMed] [Cross Ref]
35. Ping J.F., Ru S.P., Fan K., Wu J.A., Ying Y.B. Copper oxide nanoparticles and ionic liquid modified carbon electrode for the non-enzymatic electrochemical sensing of hydrogen peroxide. Microchim. Acta. 2010;171:117–123. doi: 10.1007/s00604-010-0420-3. [Cross Ref]
36. Wang C.-H., Shih H.-C., Tsai Y.-T., Du H.-Y., Chen L.-C., Chen K.-H. High methanol oxidation activity of electrocatalysts supported by directly grown nitrogen-containing carbon nanotubes on carbon cloth. Electrochim. Acta. 2006;52:1612–1617. doi: 10.1016/j.electacta.2006.03.102. [Cross Ref]
37. Abbaspour A., Ghaffarinejad A. Copper Oxide Nanoparticle Modified Sol-Gel-Derived Carbon Ceramic by Microwave Irradiation, and Its Application for Determination of Adenine at Very Low Potential. Electroanalysis. 2011;23:651–661. doi: 10.1002/elan.201000473. [Cross Ref]
38. Aita T., Watanabe Y., Higuchi T., Sato S. Electrocatalytic Properties of CuO Immobilized on Conductive Carbon Particles in Alkaline Surfactant Solution. J. Chem. Eng. Jpn. 2008;41:279–283. doi: 10.1252/jcej.07WE203. [Cross Ref]
39. Guzman-Vargas A., Oliver-Tolentino M.A., Lima E., Flores-Moreno J. Efficient electrocatalytic reduction of nitrite species on zeolite modified electrode with Cu-ZSM-5. Electrochim. Acta. 2013;108:583–590. doi: 10.1016/j.electacta.2013.07.030. [Cross Ref]
40. Joo S., Liang H. Tribo-electrochemical characterization of copper thin films. Electrochim. Acta. 2013;99:133–137. doi: 10.1016/j.electacta.2013.03.109. [Cross Ref]
41. Matsushima H., Bund A., Plieth W., Kikuchi S., Fukunaka Y. Copper electrodeposition in a magnetic field. Electrochim. Acta. 2007;53:161–166. doi: 10.1016/j.electacta.2007.01.043. [Cross Ref]
42. Hao M.Q., Liu X.H., Feng M.N., Zhang P.P., Wang G.Y. Generating power from cellulose in an alkaline fuel cell enhanced by methyl viologen as an electron-transfer catalyst. J. Power Sources. 2014;251:222–228. doi: 10.1016/j.jpowsour.2013.11.013. [Cross Ref]

Articles from Nanomaterials are provided here courtesy of Multidisciplinary Digital Publishing Institute (MDPI)