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Journal of Nanotechnology
Volume 2018, Article ID 3803969, 9 pages
https://doi.org/10.1155/2018/3803969
Research Article

Fabrication of CuOx-Pd Nanocatalyst Supported on a Glassy Carbon Electrode for Enhanced Formic Acid Electro-Oxidation

1Department of Chemical Engineering, Faculty of Engineering, The British University in Egypt, Cairo 11837, Egypt
2Chemistry Department, Faculty of Science, Cairo University, Cairo 12613, Egypt

Correspondence should be addressed to Ahmad M. Mohammad; ge.ude.uc@dammahomma and Mohamed S. El-Deab; moc.oohay@86adaasm

Received 27 August 2018; Revised 17 October 2018; Accepted 13 November 2018; Published 2 December 2018

Guest Editor: Abdellatif Ait Lahcen

Copyright © 2018 Islam M. Al-Akraa et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

Abstract

Formic acid (FA) electro-oxidation (FAO) was investigated at a binary catalyst composed of palladium nanoparticles (PdNPs) and copper oxide nanowires (CuOxNWs) and assembled onto a glassy carbon (GC) electrode. The deposition sequence of PdNPs and CuOxNWs was properly adjusted in such a way that could improve the electrocatalytic activity and stability of the electrode toward FAO. Several techniques including cyclic voltammetry, chronoamperometry, field-emission scanning electron microscopy, energy dispersive X-ray spectroscopy, and X-ray diffraction were all combined to report the catalyst’s activity and to evaluate its morphology, composition, and structure. The highest catalytic activity and stability were obtained at the CuOx/Pd/GC electrode (with PdNPs directly deposited onto the GC electrode followed by CuOxNWs with a surface coverage, Г, of ca. 49%). Such enhancement was inferred from the increase in the peak current of direct FAO (by ca. 1.5 fold) which associated a favorable negative shift in its onset potential (by ca. 30 mV). The enhanced electrocatalytic activity and stability (decreasing the loss of active material by ca. 1.5-fold) of the CuOx/Pd/GC electrode was believed originating both from facilitating the direct oxidation (decreasing the time needed to oxidize a complete monolayer of FA, increasing turnover frequency, by ca. 2.5-fold) and minimizing the poisoning impact (by ca. 71.5%) at the electrode surface during FAO.

1. Introduction

The growing petition for a clean fuel and the awareness of environmental problems have drawn the attention of the global community to substitute fossil fuels with other sources of clean energy [1, 2]. Of these, fuel cells were encouraging as they have been verified competent, consistent, sustainable, noiseless, long-lasted, and simply installed and moved; hence, they were excellent for transportation and suburban uses as well as portable electronics [37]. To date, the direct formic acid fuel cells (DFAFCs) have shown more preferred than hydrogen fuel cells (HFCs) and direct methanol fuel cells (DMFCs) in providing electricity for portable electronics [614]. In fact, the transportation and storage of formic acid (FA, the energy carrier in DFAFCs) was much easier than H2, and it could exhibit, moreover, a lower crossover than methanol through Nafion-based membranes. This permitted a higher practical energy density because of allowing the usage of thinner membranes and more concentrated fuel solutions [15, 16]. In addition, FA can be sustainably manufactured by CO2 electrochemical reduction utilizing excess clean electrical power sources such as solar farms and wind turbines [17].

With the revolution of nanotechnology, several nanostructures have been recommended for applications of multidiversity [1821]. Platinum-based catalysts have been commonly used as for the electro-oxidation of formic acid (FAO) [22, 23]. On Pt-based materials, FAO proceeded in two pathways at the same time: the direct (favorable—in which FA is converted to CO2 at a low anodic potential) [9, 1517] and the indirect (unfavorable—in which FA is converted to poisoning CO that is then oxidized at higher potentials by platinum hydroxide species) [24]. Unluckily, CO adsorption in the low potential domain at the Pt surface deactivated its catalytic activity, which finally impeded the direct pathway of FAO [2426]. Scheme 1 represents the dehydrogenation and dehydration pathways of FAO at Pt surfaces.

Scheme 1: Dehydrogenation and dehydration pathways of FAO.

Compared with Pt, Pd can catalyze the FAO through a more facile direct path to produce CO2 with less vulnerability to CO poisoning [27, 28]. However, Pd-based catalysts used to be subjected to a potential deactivation with time that originated typically from the adsorption of some CO-like poisoning species [29, 30]. The catalytic performance of Pd catalysts toward FAO was recently enhanced by doping with other metals and/or metal oxides that have the capacity to reduce the adsorption of these poisoning intermediates [3134]. In the previous study [12], MnOx was able to enhance the electrocatalytic performance of Pd in such a way that minimized the adsorption of poisoning species depicted from calculating the long-term poisoning rate (δ). This modification reduced δ to 0.11, 0.08, and 0.05%·s−1 at the Pd/MnOx/GC, MnOx/Pd/GC, and Pd-MnOx/GC electrodes, respectively.

Doping platinum and palladium with nonprecious copper or copper oxide has not only exhibited outstanding improvement in the catalytic activities and stability of several potential electrochemical reactions [3538], but also it offers a very effective way that could reduce the loading of noble metals. Hence, a motivation to report on the enhanced efficiency of a CuOx/Pd/GC nanocatalyst (in which PdNPs was directly electrodeposited onto a GC surface followed by CuOxNWs) toward FAO exists. The electrodeposition technique is utilized as it attracted particular attention due to the ease of preparation, suitability for special-shaped electrodes, and low-cost requirement. The influence of deposition sequence and loading level of CuOxNWs was examined to maximize the catalytic performance toward FAO.

2. Experimental

2.1. Electrochemical Measurements

After cleaning with conventional procedures, the electrode was mechanically polished with No. 2000 emery paper and then with aqueous slurries of successively finer alumina powder (down to 0.06 µm) with the help of a polishing microcloth. Next, the polished electrode was rinsed thoroughly with distilled water, and glassy carbon (GC, d = 3.0 mm) electrode was served as a working electrode. A spiral Pt wire and an Ag/AgCl/KCl (sat.) were used as counter and reference electrodes, respectively. All potentials in this investigation were measured in reference to Ag/AgCl/KCl (sat.).

The electrochemical measurements were performed at room temperature (25 ± 1°C) in a two-compartment three-electrode glass cell. The measurements were performed using EG&G potentiostat (model 273A). Current densities were calculated on the basis of the real surface area of the working electrodes. The electrocatalytic activity of the modified electrodes toward FAO was examined in an aqueous solution of 0.3 M FA solution (pH = 3.5, pH was adjusted by adding a proper amount of NaOH) at a scan rate of 100 mV·s−1 (first cycle is recorded). At this pH, the polarization resistance will be reduced, thus the solution ionic conductivity was enhanced [39].

2.2. Electrodeposition of PdNPs and CuOxNWs

The electrodeposition of PdNPs was carried out in 0.1 M H2SO4 solution containing 1.0 mM Pd(CH3COO)2 at a constant potential electrolysis at 0 V for 300 s. The PdNPs loading was estimated from Faraday’s law using the charge associated in the i-t curve obtained during deposition to be ca. 18 µg·cm−2. Alternatively, the electrode’s modification with CuOxNWs was carried out in 0.1 M H2SO4 solution containing 1.0 mM CuSO4 at a constant potential electrolysis at −0.2 V for various durations [38]. These durations were set to control the amount of the electrodeposited Cu. The experimental protocol used for the surface modification of GC electrode with PdNPs and CuNWs is shown in Scheme 2.

Scheme 2: The experimental protocol used for the surface modification of GC electrode with PdNPs and CuNWs.
2.3. Materials Characterization

A field-emission scanning electron microscope, FE-SEM, (QUANTA FEG 250) coupled with an energy dispersive X-ray spectrometer (EDS) was served to determine the morphology and composition of the investigated electrodes. An X-ray diffraction (XRD, PANalytical, X’Pert PRO) operated with Cu target (λ = 1.54 Å) revealed the crystallographic structure of the modified catalysts. The inductively coupled plasma optical emission spectrometry, ICP-OES, (Perkin Elmer, Optima 8000) has been utilized to specify if there was a loss in the catalysts’ materials (Pd&Cu) after the prolonged electrolysis and to determine the amounts lost.

3. Results and Discussion

3.1. Electrochemical and Materials Characterization

Cyclic voltammograms (CVs) for (a) Pd/GC, (b) CuOx/GC, (c) Pd/CuOx/GC, and (d) CuOx/Pd/GC electrodes measured in 0.5°M H2SO4 are shown in Figure 1. Figure 1(a) depicts the characteristic response of Pd surfaces where its oxidation started between 0.6 and 1.2 V was combined with this oxide reduction at ca. 0.4 V [33]. Besides that, the peaks that appeared in the potential range from 0 to −0.2 V were assigned to the hydrogen adsorption/desorption (Hads/des). For the CuOx/GC electrode (Figure 1(b)), a main oxidation peak appeared at ca. 0.15 V coupled with a reduction peak after ca. 0 V corresponding to the CuOx formation and reduction [27, 29]. After the deposition of PdNPs onto the CuOx/GC electrode (Pd/CuOx/GC electrode, Figure 1(c)), the intensity of the Pd oxide reduction peak increased coinciding with the increase in the intensity of the Pd oxide and the Hads/des peaks. This is expected as the loading of CuOxNWs on the GC surface can offer more active sites for the deposition of PdNPs; therefore, the Pd surface area could be seen increased. On the contrary, upon modifying the Pd/GC electrode with CuOxNWs (Figure 1(d)), two new features were noticed:(i)A significant decrease in the intensities of the Pd oxide reduction and the Hads/des peaks. This suggests a significant decrease in the PdNPs surface area as a result of CuOxNWs deposition.(ii)A redox couple at ca. 0.25 V corresponding to the Cu oxidation and reduction [2730].

Figure 1: CVs obtained at (a) Pd/GC, (b) CuOx/GC, (c) Pd/CuOx/GC, and (d) CuOx/Pd/GC electrodes in 0.5 M H2SO4. Potential scan rate: 100 mVs−1.

These new features of the CuOx/Pd/GC catalyst confirmed the surface exposure of both PdNPs and CuOxNWs to the electrolyte.

Figure 2 displays FE-SEM images of the Pd/GC (Figure 2(a)), CuOx/GC (Figure 2(b)), Pd/CuOx/GC (Figure 2(c)), and CuOx/Pd/GC (Figure 2(d)) electrodes. It illustrates that Pd was electrodeposited onto the GC electrode in a well-dispersed spherical lumps with an average particle size of ca. 75°nm (Figures 2(a), 2(c), and 2(d)), whereas CuOx has been electrodeposited as hair-like nanowires (Figures 2(b) and 2(d)). The disappearance of the CuOx morphology for the Pd/CuOx/GC electrode (Figure 2(c)), in contrast to the case for CuOx/Pd/GC (Figure 2(d)), infers that it has been covered during Pd deposition. This difference in morphology may affect the electrocatalytic parameters of FAO which will be displayed in the next section.

Figure 2: FE-SEM images of (a) Pd/GC, (b) CuOx/GC, (c) Pd/CuOx/GC, and (d) CuOx/Pd/GC electrodes. The electrodeposition conditions are listed in the experimental section.

The EDS analysis of the Pd/GC, CuOx/GC, and CuOx/Pd/GC electrodes confirmed the deposition of the different ingredients in the catalyst and assisted in calculation of their relative ratios (Figures 3(a)3(c)). Moreover, the crystal structure of the Pd/GC, CuOx/GC, and CuOx/Pd/GC electrodes was investigated utilizing the XRD technique. In fact, the XRD analysis of the Pd/GC and CuOx/Pd/GC electrodes (Figures 4(a) and 4(c)) displayed several diffraction peaks at ca. 39.7°, 43.2°, 67.2°, and 78° corresponding, respectively, to the (1 1 1), (2 0 0), (2 2 0), and (3 1 1) planes of Pd face-centered cubic (fcc) lattice [40, 41]. However, in Figures 4(b) and 4(c), a very small diffraction peak appeared at ca. 43.3° corresponding to Cu (1 1 1) plane. There were also two broad diffraction peaks for C (0 0 2) and (1 0 0) planes between 21–28° and 42–46°, respectively [42]. The C (1 0 0) peak was much higher and broader than those of Pd (200) and Cu (111) and that is why they appeared like a single peak.

Figure 3: EDS analysis of (a) Pd/GC, (b) CuOx/GC, and (c) CuOx/Pd/GC electrodes. The electrodeposition conditions are listed in the experimental section.
Figure 4: XRD patterns of (a) Pd/GC, (b) CuOx/GC, and (c) CuOx/Pd/GC electrodes. The electrodeposition conditions are listed in the experimental section.
3.2. Electrocatalytic Activity toward FAO
3.2.1. Effect of Deposition Sequence

Figure 5 shows CVs of FAO at the Pd/GC, CuOx/GC, Pd/CuOx/GC, and CuOx/Pd/GC electrodes in a 0.3 M aqueous solution of FA (pH = 3.5). It is important to consider the inactivity of the unmodified GC electrode toward FAO [25, 43]. Inspection of Figure 5 reveals few interesting remarks:(i)The reaction pathway of FAO on the Pd/GC electrode (Figure 5(a)) proceeded exclusively via the dehydrogenation route in which CO2 was the only oxidation product with insignificant contribution of Pd poisoning by CO [44, 45]. This was evident from the appearance of a single oxidation peak around ca. 0 V, which assigned the direct oxidation of FA to CO2 [33].(ii)The electrodeposition of CuOx directly at GC electrode surface did not show any activity for FAO (Figure 5(b)) to confirm the inertness of CuOx as well as the GC substrate toward FAO.(iii)The deposition of PdNPs at GC electrode surface modified with CuOx to obtain Pd/CuOx/GC electrode (Figure 5(c)) a little bit shifts the current density of the oxidation peak (Ip) to a higher value as compared to the Pd/GC electrode (Figure 5(a)). This was likely because it had a higher surface area of PdNPs (as discussed before in Figure 1).(iv)The electrodeposition of CuOxNWs at the GC electrode surface previously modified with PdNPs (Pd/GC) to obtain CuOx/Pd/GC electrode (Figure 5(d)) exhibited an enhanced performance toward FAO with an increase of Ip (ca. 1.5 fold) and a negative shift (ca. 30 mV) in the onset potential (Eonset) of FAO. Recalling the smaller surface area of Pd in the CuOx/Pd/GC electrode than in the Pd/GC electrode (compare Figures 1(a) and 1(d)), one may exclude the geometrical factor in the catalytic enhancement to suggest rather an electronic influence for CuOxNWs that could presumably promote the charge transfer of the direct FAO at the electrode surface [17, 29, 46].

Figure 5: CVs obtained at (a) Pd/GC, (b) CuOx/GC, (c) Pd/CuOx/GC, and (d) CuOx/Pd/GC electrodes in 0.3 M FA (pH = 3.5). Potential scan rate: 100 mVs−1.
3.2.2. Effect of Loading Level of CuOxNWs at Pd/GC Electrode

Optimization of the loading level of CuOxNWs onto the Pd/GC electrode toward FAO has been investigated. A gradual decrease in the surface area of PdNPs reflected by a decrease in the intensity of the Pd oxide reduction and the Hads/des peaks with the loading of CuOxNWs have been observed. Table 1 summarizes the variation of the surface coverage (Г) of CuOxNWs electrodeposited onto the Pd/GC electrode with time and its effect on the peak current of FAO, Ip. As obviously seen, the Ip increased systematically to a certain value with Г and then decreased. This makes sense as the catalytic activity of the CuOx/Pd/GC electrode is expected to increase with the loading level of CuOxNWs as long as the accessible surface area of PdNPs is sufficient to sustain the adsorption of FA. However, beyond certain coverage (ca. 49%), the accessible surface area of PdNPs becomes limiting in estimating the overall rate of FAO.

Table 1: Variation of the surface coverage (Г) of CuOxNWs electrodeposited onto Pd/GC electrode with deposition time and its effect on Ip of FAO.
3.3. Stability of CuOx/Pd/GC Electrode

Stability of the Pd-based catalysts is another important parameter in the practical use of DFAFCs. Figure 6 shows current transients of the Pd/GC, Pd/CuOx/GC, and CuOx/Pd/GC electrodes in a 0.3 M aqueous solution of FA (pH = 3.5) at −0.1 V. We did not include the data of the CuOx/GC electrode as it did not show any activity toward FAO (Figures 5(b), 6(a), and 6(b)) (Pd/GC and Pd/CuOx/GC electrodes, respectively) depicting a poor stability toward FAO, as can be obtained from the fast current drop with time, which agreed with other investigations in the literature [33, 46]. Interestingly, the CuOx/Pd/GC electrode (Figure 6(c)) exhibited a higher current density in the activation polarization region, and its final current density was 1.6 mA·cm−2 (compare it with 0.07 and 0.3 mA·cm−2 obtained at the Pd/GC and Pd/CuOx/GC electrodes). This may be assigned to the difference in the degree of poisoning of the three electrodes. The long-term poisoning rate (δ) could be calculated by measuring the linear decay of the current at intervals longer than 500°s using the following equation [47]:where is the slope of the linear portion of the current decay and is the current at the start of polarization back-extrapolated from the linear current decay, respectively. Fascinatingly, the CuOx/Pd/GC electrode showed a lower poisoning rate (ca. 0.002%·s−1) if compared to those obtained at both the Pd/GC (ca. 0.007%·s−1) and Pd/CuOx/GC electrodes (ca. 0.005%·s−1). This also infers about how CuOx promoted FAO at the Pd-CuOx modified catalysts.

Figure 6: Current transients of (a) Pd/GC, (b) Pd/CuOx/GC, and (c) CuOx/Pd/GC electrodes in 0.3 M FA (pH = 3.5) at −0.1 V.

Furthermore, some important electrocatalytic parameters, calculated from pseudosteady state current, such as time needed to oxidize a complete monolayer of FA and turnover frequency (TOF), have been estimated for the modified electrodes. Utilizing the charge associated with oxidation of a complete monolayer of FA, the complete oxidation of a FA monolayer at the Pd/GC and Pd/CuOx/GC electrodes, respectively, needed 0.86 and 0.82 s on the basis of a two-site adsorption model, and the corresponding TOF was estimated as 2.33 and 2.44 s−1 [48], respectively. Interestingly, based on the same adsorption model, the complete oxidation of a FA monolayer at the CuOx/Pd/GC electrode needed 0.35 s, and the corresponding TOF was 5.71 s−1. These parameters could infer about the superior catalytic activity of the as-prepared CuOx/Pd/GC electrode. Table 2 summarizes the electrochemical parameters, extracted from Figures 5 and 6, of the CuOx/Pd/GC compared with Pd/GC and Pd/CuOx/GC electrodes. It also compares the data obtained in this investigation with the same data obtained from other previous investigations at which Pt surface was modified with nano-NiOx and IrNPs [49, 50].

Table 2: Electrochemical parameters, extracted from Figures 5 and 6, of the CuOx/Pd/GC compared with Pd/GC, Pd/CuOx/GC electrodes in this study and other previously reported catalysts.

Further, the inductively coupled plasma optical emission spectrometry (ICP-OES) has been utilized to specify if there was a loss in the catalysts’ materials (Pd and Cu) after the prolonged electrolysis and to determine the amounts lost. A minor loss was obtained after 2 h of electrolysis in FA. Importantly, the loss of the active material toward FAO (Pd) in the Pd/GC electrode was ca. 1.5 of that obtained at the modified CuOx/Pd/GC electrode confirming once again the superiority of the CuOx/Pd/GC electrode toward FAO (Table 3).

Table 3: Inductively coupled plasma optical emission spectrometry (ICP-OES) measured after 2 h of electrolysis in FA for CuOx/Pd/GC and Pd/GC electrodes.

4. Conclusion

A novel binary catalyst composed of PdNPs and CuOxNWs has been assembled onto the GC electrode for the efficient FAO. The deposition sequence of both PdNPs and CuOxNWs onto the GC electrode influenced, to a great extent, the catalytic efficiency. The highest catalytic activity and stability were obtained at the CuOx/Pd/GC electrode (in which CuOxNWs were partially deposited, Г ≈ 49%, onto the Pd/GC electrode). The enhancement in the electrocatalytic activity (increasing Ip of direct FAO by ca. 1.5-fold and decreasing Eonset by ca. 30 mV) and stability (decreasing both current decay and loss of active metal, by ca. 1.5-fold, during prolonged electrolysis) of the CuOx/Pd/GC electrode was believed originating both from facilitating the direct oxidation of FA (increasing turnover frequency by ca. 2.5-fold) and minimizing the adsorption of poisoning species (by ca. 71.5%) at the electrode surface.

Data Availability

The data used to support the findings of this study are available from the corresponding author upon request.

Conflicts of Interest

The authors declare that there are no conflicts of interest regarding the publication of this paper.

References

  1. M. Carmo, G. Doubek, R. C. Sekol, M. Linardi, and A. D. Taylor, “Development and electrochemical studies of membrane electrode assemblies for polymer electrolyte alkaline fuel cells using FAA membrane and ionomer,” Journal of Power Sources, vol. 230, pp. 169–175, 2013. View at Publisher · View at Google Scholar · View at Scopus
  2. S. Nishimura, N. Ikeda, and K. Ebitani, “Selective hydrogenation of biomass-derived 5-hydroxymethylfufural (HMF) to 2,5-dimethyl furfural (DMF) under atmospheric hydrogen pressure over carbon supported PdAu bimetallic catalyst,” Catalysis Today, vol. 232, pp. 89–98, 2014. View at Publisher · View at Google Scholar · View at Scopus
  3. A. M. Abdullah, A. M. Mohammad, T. Okajima, F. Kitamura, and T. Ohsaka, “Effect of load, temperature and humidity on the pH of the water drained out from H2/air polymer electrolyte membrane fuel cells,” Journal of Power Sources, vol. 190, no. 2, pp. 264–270, 2009. View at Publisher · View at Google Scholar · View at Scopus
  4. B. Braunchweig, D. Hibbitts, M. Neurock, and A. Wieckowski, “Electrocatalysis: a direct alcohol fuel cell and surface science perspective,” Catalysis Today, vol. 202, pp. 197–209, 2013. View at Publisher · View at Google Scholar · View at Scopus
  5. M. Bron and C. Roth, in Chapter 10-Fuel Cell Catalysis from a Materials Perspective New and Future Developments in Catalysis, Elsevier, Amsterdam, Netherlands, 2013.
  6. J. P. Stempien and S. H. Chan, “Comparative study of fuel cell, battery and hybrid buses for renewable energy constrained areas,” Journal of Power Sources, vol. 340, pp. 347–355, 2017. View at Publisher · View at Google Scholar · View at Scopus
  7. P. Y. You and S. K. Kamarudin, “Recent progress of carbonaceous materials in fuel cell applications: an overview,” Chemical Engineering Journal, vol. 309, pp. 489–502, 2017. View at Publisher · View at Google Scholar · View at Scopus
  8. S. Zhang, Y. Shao, G. Yin, and Y. Lin, “Facile synthesis of PtAu alloy nanoparticles with high activity for formic acid oxidation,” Journal of Power Sources, vol. 195, no. 4, pp. 1103–1106, 2010. View at Publisher · View at Google Scholar · View at Scopus
  9. I. M. Al-Akraa, A. M. Mohammad, M. S. El-Deab, and B. E. El-Anadouli, “Development of tailor-designed gold-platinum nanoparticles binary catalysts for efficient formic acid electrooxidation,” International Journal of Electrochemical Science, vol. 7, no. 5, pp. 3939–3946, 2012. View at Google Scholar
  10. M. S. El-Deab, A. M. Mohammad, G. A. El-Nagar, and B. E. El-Anadouli, “Impurities contributing to catalysis: enhanced electro-oxidation of formic acid at Pt/GC electrodes in the presence of vinyl acetate,” Journal of Physical Chemistry C, vol. 118, no. 39, pp. 22457–22464, 2014. View at Publisher · View at Google Scholar · View at Scopus
  11. G. A. El-Nagar, A. M. Mohammad, M. S. El-Deab, T. Ohsaka, and B. E. El-Anadouli, “Acrylonitrile-contamination induced enhancement of formic acid electro-oxidation at platinum nanoparticles modified glassy carbon electrodes,” Journal of Power Sources, vol. 265, pp. 57–61, 2014. View at Publisher · View at Google Scholar · View at Scopus
  12. I. M. Al-Akraa, “Efficient electro-oxidation of formic acid at Pd-MnOx binary nanocatalyst: effect of deposition strategy,” International Journal of Hydrogen Energy, vol. 42, no. 7, pp. 4660–4666, 2017. View at Publisher · View at Google Scholar · View at Scopus
  13. M. S. El-Deab, G. A. El-Nagar, A. M. Mohammad, and B. E. El-Anadouli, “Fuel blends: enhanced electro-oxidation of formic acid in its blend with methanol at platinum nanoparticles modified glassy carbon electrodes,” Journal of Power Sources, vol. 286, pp. 504–509, 2015. View at Publisher · View at Google Scholar · View at Scopus
  14. A. M. Mohammad, G. A. El-Nagar, I. M. Al-Akraa, M. S. El-Deab, and B. E. El-Anadouli, “Towards improving the catalytic activity and stability of platinum-based anodes in direct formic acid fuel cells,” International Journal of Hydrogen Energy, vol. 40, no. 24, pp. 7808–7816, 2015. View at Publisher · View at Google Scholar · View at Scopus
  15. Y. W. Rhee, S. Y. Ha, and R. I. Masel, “Crossover of formic acid through Nafion® membranes,” Journal of Power Sources, vol. 117, no. 1-2, pp. 35–38, 2003. View at Publisher · View at Google Scholar · View at Scopus
  16. X. Wang, J.-M. Hu, and I.-M. Hsing, “Electrochemical investigation of formic acid electro-oxidation and its crossover through a Nafion® membrane,” Journal of Electroanalytical Chemistry, vol. 562, no. 1, pp. 73–80, 2004. View at Publisher · View at Google Scholar · View at Scopus
  17. S. Hu, L. Scudiero, and S. Ha, “Electronic effect of Pd-transition metal bimetallic surfaces toward formic acid electrochemical oxidation,” Electrochemistry Communications, vol. 38, pp. 107–109, 2014. View at Publisher · View at Google Scholar · View at Scopus
  18. A. M. Mohammad, S. Dey, K. K. Lew, J. M. Redwing, and S. E. Mohney, “Fabrication of cobalt silicide nanowire contacts to silicon nanowires,” Journal of the Electrochemical Society, vol. 150, no. 9, pp. G577–G580, 2003. View at Publisher · View at Google Scholar · View at Scopus
  19. S. M. Dilts, A. Mohmmad, K. K. Lew, and J. M. Redwing, “Mohney SE fabrication and electrical characterization of silicon nanowire arrays,” in Proceedings of MRS Fall Meeting, L. Tsybeskov, D. J. Lockwood, C. Delerue, and M. Ichikawa, Eds., pp. 287–292, Boston, MA, USA, November 2004.
  20. D. Shir, B. Z. Liu, A. M. Mohammad, K. K. Lew, and S. E. Mohney, “Oxidation of silicon nanowires,” Journal of Vacuum Science & Technology B: Microelectronics and Nanometer Structures, vol. 24, no. 3, pp. 1333–1336, 2006. View at Publisher · View at Google Scholar · View at Scopus
  21. A. M. Abdullah, T. Okajima, A. M. Mohammad, F. Kitamura, and T. Ohsaka, “Temperature gradients measurements within a segmented H2/air PEM fuel cell,” Journal of Power Sources, vol. 172, no. 1, pp. 209–214, 2007. View at Publisher · View at Google Scholar · View at Scopus
  22. G. A. El-Nagar and A. M. Mohammad, “Enhanced electrocatalytic activity and stability of platinum, gold, and nickel oxide nanoparticles-based ternary catalyst for formic acid electro-oxidation,” International Journal of Hydrogen Energy, vol. 39, no. 23, pp. 11955–11962, 2014. View at Publisher · View at Google Scholar · View at Scopus
  23. J. K. Yoo and C. K. Rhee, “Formic acid oxidation on Bi-modified Pt surfaces: Pt deposits on Au versus bulk Pt,” Electrochimica Acta, vol. 216, pp. 16–23, 2016. View at Publisher · View at Google Scholar · View at Scopus
  24. I. M. Al-Akraa, A. M. Mohammad, M. S. El-Deab, and B. E. El-Anadouli, “Electrooxidation of formic acid at platinum gold nanoparticle-modified electrodes,” Chemistry Letters, vol. 40, no. 12, pp. 1374-1375, 2011. View at Publisher · View at Google Scholar · View at Scopus
  25. G. A. El-Nagar, A. M. Mohammad, M. S. El-Deab, and B. E. El-Anadouli, “Electrocatalysis by design: enhanced electrooxidation of formic acid at platinum nanoparticles-nickel oxide nanoparticles binary catalysts,” Electrochimica Acta, vol. 94, pp. 62–71, 2013. View at Publisher · View at Google Scholar · View at Scopus
  26. G. Cabello, R.-rA. Davoglio, F. W. Hartl et al., “Microwave-assisted synthesis of Pt-Au nanoparticles with enhanced electrocatalytic activity for the oxidation of formic acid,” Electrochimica Acta, vol. 224, pp. 56–63, 2017. View at Publisher · View at Google Scholar · View at Scopus
  27. L. Dai and S. Zou, “Enhanced formic acid oxidation on Cu-Pd nanoparticles,” Journal of Power Sources, vol. 196, no. 22, pp. 9369–9372, 2011. View at Publisher · View at Google Scholar · View at Scopus
  28. L. Feng, J. Chang, K. Jiang et al., “Nanostructured palladium catalyst poisoning depressed by cobalt phosphide in the electro-oxidation of formic acid for fuel cells,” Nano Energy, vol. 30, pp. 355–361, 2016. View at Publisher · View at Google Scholar · View at Scopus
  29. S. Li, D. Cheng, X. Qiu, and D. Cao, “Synthesis of Cu@Pd core-shell nanowires with enhanced activity and stability for formic acid oxidation,” Electrochimica Acta, vol. 143, pp. 44–48, 2014. View at Publisher · View at Google Scholar · View at Scopus
  30. R. Ojani, Z. Abkar, E. Hasheminejad, and J.-B. Raoof, “Rapid fabrication of Cu/Pd nano/micro-particles porous-structured catalyst using hydrogen bubbles dynamic template and their enhanced catalytic performance for formic acid electrooxidation,” International Journal of Hydrogen Energy, vol. 39, no. 15, pp. 7788–7797, 2014. View at Publisher · View at Google Scholar · View at Scopus
  31. G. Chen, M. Liao, B. Yu et al., “Pt decorated PdAu/C nanocatalysts with ultralow Pt loading for formic acid electrooxidation,” International Journal of Hydrogen Energy, vol. 37, no. 13, pp. 9959–9966, 2012. View at Publisher · View at Google Scholar · View at Scopus
  32. Y.-H. Qin, Y. Jiang, D.-F. Niu et al., “Carbon nanofiber supported bimetallic PdAu nanoparticles for formic acid electrooxidation,” Journal of Power Sources, vol. 215, pp. 130–134, 2012. View at Publisher · View at Google Scholar · View at Scopus
  33. I. M. Al-Akraa, A. M. Mohammad, M. S. El-Deab, and B. E. El-Anadouli, “Electrocatalysis by design: synergistic catalytic enhancement of formic acid electro-oxidation at core-shell Pd/Pt nanocatalysts,” International Journal of Hydrogen Energy, vol. 40, no. 4, pp. 1789–1794, 2015. View at Publisher · View at Google Scholar · View at Scopus
  34. Y. Jin, J. Zhao, F. Li et al., “Nitrogen-doped graphene supported palladium-nickel nanoparticles with enhanced catalytic performance for formic acid oxidation,” Electrochimica Acta, vol. 220, pp. 83–90, 2016. View at Publisher · View at Google Scholar · View at Scopus
  35. F. Gobal and R. Arab, “A preliminary study of the electro-catalytic reduction of oxygen on Cu–Pd alloys in alkaline solution,” Journal of Electroanalytical Chemistry, vol. 647, no. 1, pp. 66–73, 2010. View at Publisher · View at Google Scholar · View at Scopus
  36. F. Wang and G. Lu, “Hydrogen feed gas purification over bimetallic Cu–Pd catalysts – effects of copper precursors on CO oxidation,” International Journal of Hydrogen Energy, vol. 35, no. 13, pp. 7253–7260, 2010. View at Publisher · View at Google Scholar · View at Scopus
  37. P. Mani, R. Srivastava, and P. Strasser, “Dealloyed binary PtM3 (M=Cu, Co, Ni) and ternary PtNi3M (M=Cu, Co, Fe, Cr) electrocatalysts for the oxygen reduction reaction: performance in polymer electrolyte membrane fuel cells,” Journal of Power Sources, vol. 196, no. 2, pp. 666–673, 2011. View at Publisher · View at Google Scholar · View at Scopus
  38. G. A. El-Nagar, A. M. Mohammad, M. S. El-Deab, and B. E. El-Anadouli, “Propitious dendritic Cu2O-Pt nanostructured anodes for direct formic acid fuel cells,” ACS Applied Materials & Interfaces, vol. 9, no. 23, pp. 19766–19772, 2017. View at Publisher · View at Google Scholar · View at Scopus
  39. G. A. El-Nagar, A. M. Mohammad, M. S. El-Deab, and B. E. El-Anadouli, “Facilitated electro-oxidation of formic acid at nickel oxide nanoparticles modified electrodes,” Journal of The Electrochemical Society, vol. 159, no. 7, pp. F249–F254, 2012. View at Publisher · View at Google Scholar · View at Scopus
  40. T. Teranishi and M. Miyake, “Size control palladium nanoparticles and their crystal structures,” Chemistry of Materials, vol. 10, no. 2, pp. 594–600, 1998. View at Publisher · View at Google Scholar · View at Scopus
  41. B. Zhang, D. Ye, J. Li, X. Zhu, and Q. Liao, “Electrodeposition of Pd catalyst layer on graphite rod electrodes for direct formic acid oxidation,” Journal of Power Sources, vol. 214, pp. 277–284, 2012. View at Publisher · View at Google Scholar · View at Scopus
  42. F. Alardin, H. Wullens, S. Hermans, and M. Devillers, “Mechanistic and kinetic studies on glyoxal oxidation with Bi- and Pb-promoted Pd/C catalysts,” Journal of Molecular Catalysis A: Chemical, vol. 225, no. 1, pp. 79–89, 2005. View at Publisher · View at Google Scholar · View at Scopus
  43. L. Lu, L. Shen, Y. Shi et al., “New insights into enhanced electrocatalytic performance of carbon supported Pd-Cu catalyst for formic acid oxidation,” Electrochimica Acta, vol. 85, pp. 187–194, 2012. View at Publisher · View at Google Scholar · View at Scopus
  44. J.-H. Choi, K.-J. Jeong, Y. Dong et al., “Electro-oxidation of methanol and formic acid on PtRu and PtAu for direct liquid fuel cells,” Journal of Power Sources, vol. 163, no. 1, pp. 71–75, 2006. View at Publisher · View at Google Scholar · View at Scopus
  45. S. M. Baik, J. Han, J. Kim, and Y. Kwon, “Effect of deactivation and reactivation of palladium anode catalyst on performance of direct formic acid fuel cell (DFAFC),” International Journal of Hydrogen Energy, vol. 36, no. 22, pp. 14719–14724, 2011. View at Publisher · View at Google Scholar · View at Scopus
  46. L. Wang, J.-J. Zhai, K. Jinag, K.-Q. Wang, and W.-B. Cai, “Pd-Cu/C electrocatalysts synthesized by one-pot polyol reduction toward formic acid oxidation: structural characterization and electrocatalytic performance,” International Journal of Hydrogen Energy, vol. 40, no. 4, pp. 1726–1734, 2015. View at Publisher · View at Google Scholar · View at Scopus
  47. J. Jiang and A. Kucernak, “Electrooxidation of small organic molecules on mesoporous precious metal catalystsI: CO and methanol on platinum,” Journal of Electroanalytical Chemistry, vol. 533, no. 1-2, pp. 153–165, 2002. View at Publisher · View at Google Scholar · View at Scopus
  48. M. Osawa, K. Komatsu, G. Samjeske et al., “The role of bridge-bonded adsorbed formate in the electrocatalytic oxidation of formic acid on platinum,” Angewandte Chemie International Edition, vol. 50, no. 5, pp. 1159–1163, 2011. View at Publisher · View at Google Scholar · View at Scopus
  49. I. M. Al-Akraa, A. M. Mohammad, M. S. El-Deab, and B. E. El-Anadouli, “Electrocatalysis by nanoparticle: enhanced electro-oxidation of formic acid at NiOx–Pd binary nanocatalysts,” Journal of The Electrochemical Society, vol. 162, no. 10, pp. F1114–F1118, 2015. View at Publisher · View at Google Scholar · View at Scopus
  50. I. M. Al-Akraa, A. M. Mohammad, M. S. El-Deab, and B. E. El-Anadouli, “Advances in direct formic acid fuel cells: fabrication of efficient Ir/Pd nanocatalysts for formic acid electro-oxidation,” International Journal of Electrochemical Science, vol. 10, no. 4, pp. 3282–3290, 2015. View at Google Scholar