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Article

Electrocatalytic Performance of Carbon Supported WO3-Containing Pd–W Nanoalloys for Oxygen Reduction Reaction in Alkaline Media

by
Nan Cui
,
Wenpeng Li
*,
Zengfeng Guo
,
Xun Xu
and
Hongxia Zhao
Key Lab of Fine Chemicals in Universities of Shandong, Institute of Advanced Energy Materials and Chemistry, School of Chemistry and Pharmaceutical Engineering, Qilu University of Technology (Shandong Academy of Sciences), Daxue Road, Changqing District, Jinan 250353, China
*
Author to whom correspondence should be addressed.
Catalysts 2018, 8(6), 225; https://doi.org/10.3390/catal8060225
Submission received: 7 April 2018 / Revised: 16 May 2018 / Accepted: 21 May 2018 / Published: 24 May 2018
(This article belongs to the Special Issue Catalysts for Oxygen Reduction Reaction)
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Versions Notes

Abstract

:
In this paper, we report that WOx containing nanoalloys exhibit stable electrocatalytic performance in alkaline media, though bulk WO3 is easy to dissolve in NaOH solution. Carbon supported oxide-rich Pd–W alloy nanoparticles (PdW/C) with different Pd:W atom ratios were prepared by the reduction–oxidation method. Among the catalysts, the oxide-rich Pd0.8W0.2/C (Pd/W = 8:2, atom ratio) exhibits the highest catalytic activity for the oxygen reduction reaction. The X-ray photoelectron spectroscopy data shows that ~40% of Pd atoms and ~60% of the W atoms are in their oxide form. The Pd 3d5/2 binding energy of the oxide-rich Pd–W nanoalloys is higher than that of Pd/C, indicating the electronic structure of Pd is affected by the strong interaction between Pd and W/WO3. Compare to Pd/C, the onset potential of the oxygen reduction reaction at the oxide-rich Pd0.8W0.2/C shifts to a higher potential. The current density (mA·mg Pd−1) at the oxide-rich Pd0.8W0.2/C is ~1.6 times of that at Pd/C. The oxide-rich Pd0.8W0.2/C also exhibits higher catalytic stability than Pd/C, which demonstrates that it is a prospective candidate for the cathode of fuel cells operating with alkaline electrolyte.

Graphical Abstract

1. Introduction

The study of the oxygen reduction reaction (ORR) has a history of more than one century since Grove fabricated the earliest hydrogen–oxygen fuel cell with Pt as the catalyst for ORR in 1839. In recent years, the studies of ORR have been promoted by the increasing demand of clean energy technology like fuel cells. As the energy efficiency and battery voltage of electrochemical cells are limited by the slow kinetics of the ORR [1,2], there is a great need for highly efficient catalysts for ORR. Various electrocatalysts for ORR have been developed, including but not limited to Pt-based catalysts [3,4,5], Pd-based catalysts [6,7], catalysts based on non-precious metals [8,9], catalysts based on carbon nanostructure/nanocomposites [10,11,12,13], catalysts based on metal oxides [14,15], catalysts based on metal–organic frameworks [16,17], catalysts based on complexes [18,19], enzyme-based catalysts [20,21,22,23,24], metal carbides [25,26,27,28], and so on. Among the catalysts for ORR, Pt-based catalysts are regarded as the most active catalysts [29]. However, platinum’s scarcity limits the large scale application of Pt-based electrocatalysts. Palladium has been used as one of the alternative candidates being about 200 times more abundant in the earth than platinum. There have been some reviews about Pd-based electrocatalysts [30,31,32]. The ORR [33] can be performed under both acid conditions and alkaline conditions in fuel cells. It has been reported that alkaline media are a benefit for the kinetics of ORR [34]. In alkaline solutions, the oxygen can be reduced through a four-electron pathway or a two-electron pathway [35]. A lot of novel Pd-based electrocatalysts for ORR exist, including carbon or metal supported Pd alloys [36,37,38], nitrogen and sulfur co-doped carbon supported PdNi catalyst (PdNi-NS/C) [39], Pd supported on TiO2 with oxygen vacancy (Pd/TiO2–Vo) [40], PdW nanoparticles supported on sulfur-doped graphene (PdW/SG) [41], PdNiCu/PdNiCo supported on nitrogen dope graphene [42], PdSnCo/nitrogen-doped-graphene [43], electrochemically reduced graphene-oxide supported Pd-Mn2O3 nanoparticles [44], AuPd@PdAu alloy nanocrystals [45], three-dimensional nitrogen-doped graphene supports for palladium nanoparticles (Pd-N/3D-GNS) [46], and so on. Most of the research above on Pd-based electrocatalysts for ORR in alkaline media is supported on graphene specially treated (doping, modifying, and so on). Although carbon black is the most used support for noble metal electrocatalysts in fuel cells, Pd-based electrocatalysts supported on carbon black (C) for ORR in alkaline media have been rarely reported over the past few years. Besides the boom of novel support materials like doped graphene, one of the possible reasons is the high activity of Pd/C for ORR in alkaline media. It was found that Pd/C exhibits significantly high activity close to Pt/C in alkaline solutions [37,38], therefore it is difficult for other electrocatalysts for ORR in alkaline media to exhibit much higher activity than Pd/C. The new studies about carbon-black supporting Pd based catalysts for ORR in alkaline media have to face the difficult situation of being compared to the ultra-high active catalyst Pd/C.
After their calculations based on quantum mechanics, Goddard et.al. [47] predicted that Pd3W was a prospective catalyst for ORR, which was confirmed by our previous work for Pd0.7W0.3 in acid media [48]. To date, Pt-based electrocatalysts are commonly used in commercially available electric vehicles powered by fuel cells. Goddard and his coworkers examined the critical barriers of the ORR with Pd3W and compared them to the analogous barriers for Pd and Pt. The results demonstrated that Pd3W exhibits ORR properties greatly improved over pure Pd and close to that of pure Pt. Since the cost of Pd3W is six times less than that of pure Pt, a highly efficient Pd–W system is a promising candidate for future application. In this work, we attempt to fabricate high performance Pd–W/C systems for ORR in alkaline media. Most of the noble metal electrocatalysts used in fuel cells are in the form of naonoparticles supported on carbon. Since the surface of metal nanoparticles is easy to be oxidized by ambient air, the effect of oxides in the Pd-based catalysts for ORR in alkaline media should be discussed. There have been some state-of-art electrocatalysts based on oxides such as Fe3O4@NiFexOy [49]. However, as the resistance of semiconductor oxides is higher than that of metals, the output voltage will decrease when the oxides are directly used as electrode materials in fuel cells or metal–air batteries. Combining the oxide with a high-conductive metal in each of the nanoparticles of catalysts is a solution for avoiding the decrease. The interaction of metal and metal oxides in catalysts has attracted research interests for decades [50,51,52,53]. It has been reported recently that metal and metal oxides interactions are greatly affected by the catalytic consequence of electrocatalysis reactions such as the oxygen reduction reaction [54] and the ethanol oxidation reaction [55,56]. Bulk WO3 crystal can be dissolved in strong NaOH solutions, which limits its direct application in fuel cells operating with alkaline electrolytes. To solve this problem, we started by separating the W atoms with noble metals such as Pd in the atomic scale before their oxidation. Therefore the chemical bonds attached to most of the W atoms are not W–O–W bonds but Pd–W metallic bonds, which are more stable than W–O–W bonds in alkaline solutions. According to the Monte Carlo simulation [57,58], alloy clusters at the surface of nano-materials sometimes exhibit higher stability. Then, we fabricated WOx-containing Pd–W nanoalloys with the reduction– oxidation method (Scheme 1). The onset potential of ORR at the as prepared oxide-rich Pd0.8W0.2/C (Pd/W = 8:2, metal atomic ratio) is close to the Pd/C and Pt/C fabricated with the chemical reduction method [36]. The ORR stability and current density (mA·mg Pd−1) of the oxide-rich Pd0.8W0.2/C are higher than those of Pd/C, which indicates that the oxide-rich Pd0.8W0.2/C is a prospective candidate for the cathode of fuel cells.

2. Results and Discussion

2.1. Characterization of Oxide-Rich PdW/C Catalysts

The X-ray diffraction (XRD) patterns of Pd/C (a), oxide-rich Pd0.6W0.4/C (b), Pd0.7W0.3/C (c), Pd0.8W0.2/C (d), Pd0.9W0.1/C (e) are shown in Figure 1. Five typical diffraction peaks of the catalysts are observed at about 24.8°, 40°, 46°, 68°, 82° in the diffractogram. The five peaks correspond to the Vulcan XC-72R carbon (002) crystal face, face centered cubic (fcc) metal Pd (111), (200), (220) and (311) crystal plane diffraction, respectively. The XRD patterns do not show any diffraction peaks corresponding to W (fcc) or WO3 indicating that most of the W atoms do not exist as an individual phase, but have entered into the lattice of the Pd crystal. The absence of peaks for tungsten also was found in our previous reported Pd0.7W0.3 catalyst [59] used in acid conditions. The diffraction angle of (220) or (311) crystal plane diffraction peaks of the Pd in the PdW/C catalysts is higher than that of the corresponding Pd/C catalyst. The XRD peaks shift to a higher angle indicating compression in the direction perpendicular to the tensile stress [60,61]. The size of catalyst metal particles can be estimated with Scherrer’s equation [62]. The estimated particle size of Pd/C, Pd0.6W0.4/C, Pd0.7W0.3/C, Pd0.8W0.2/C and Pd0.9W0.1/C were 5.6 nm, 4.8 nm, 4.5 nm, 4.3 nm, and 5.2 nm, respectively. The particle size of the oxide-rich Pd–W/C nanoparticles is smaller than that of Pd/C.
The morphology and particle distribution (Figure 2) of Pd/C (a, b) and oxide-rich Pd0.8W0.2/C (c, d) were characterized by transmission electron microscope (TEM). The oxide-rich Pd0.8W0.2 nanoparticles are more uniformly dispersed on the carbon surface than Pd. The average diameter of Pd nanoparticles is 5.6 nm while the average metal particle diameter of oxide-rich Pd0.8W0.2 is 4.3 nm which are consistent with the XRD results. Figure 3a–c shows high resolution transmission electron microscopy (HRTEM) of oxide-rich Pd0.8W0.2/C catalyst. The lattice spacing in Figure 3a–c is 0.224 nm, 0.193 nm and 0.263 nm which respectively correspond to the (111), (200) crystal planes of face-centered cubic Pd and (220) plane of WO3. The lattice fringes of WO3 can be found in a few nanoparticles, which supports the existence of WOx in the Pd0.8W0.2/C catalysts. Although the WO3 phase is found in a few nanoparticles, there is no W phase or WO3 phase in most of the Pd–W alloy nanoparticles, which is consistent with the XRD patterns. It indicates that most of the W atoms have been mixed with the Pd atoms during the preparation of Pd–W alloy nanoparticles from the uniform mixtures of Pd salt and W salt, thus the separate W or WO3 phase is rare. Besides, the W atoms on the surface of Pd–W nanoparticles are easily oxidized by ambient air, therefore it is difficult to find the W phase on the surface of Pd–W nanoparticles. Although there is no diffraction peak corresponding to W in the XRD patterns mentioned above, the energy dispersive spectrum (EDS) of the as prepared oxide-rich Pd0.8W0.2/C (Figure 3d) shows the content of W in the Pd–W nanoalloys.
Figure 4 shows the X-ray photoelectron spectroscopy (XPS) spectra of oxide-rich Pd0.6W0.4/C, Pd0.7W0.3/C, Pd0.8W0.2/C, Pd0.9W0.1/C. The XPS spectra of Pd/C was published in our recent works [63]. All XPS curves were fitted using the Gaussian–Lorentzian (20%) method after subtracting the background with Shirley’s method. The surface composition ratios of the Pd:W elements in oxide-rich Pd0.6W0.4/C, Pd0.7W0.3/C, Pd0.8W0.2/C and Pd0.9W0.1/C are Pd0.57W0.43, Pd0.70W0.30, Pd0.79W0.21, Pd0.87W0.23, respectively. In Figure 4a, the peaks of Pd 3d5/2 and Pd 3d3/2 correspond to Pd and PdOy (0 < 2 < y), and the Pd element is present in all the samples as Pd metal and PdOy. The binding energy of Pd 3d5/2 peaks of PdW/C catalysts respectively shifted +0.21 eV, +0.28 eV, +0.36 eV, +0.52 eV compared with that of Pd/C (335.6 eV, the solid line) which indicates a decrease of Pd 3d electronic cloud densities. The change of the electronic structure is due to the formation of high-valency oxides. Figure 4b is the peak of W4f. The two peaks at 35.5 and 37.5 eV correspond to WO3. With the decrease of tungsten content in the Pd–W nanoalloy, the atom ratio of W(0):W(VI) increases. The W(0):W(VI) in Pd0.9W0.1/C, Pd0.8W0.2/C, Pd0.7W0.3/C and Pd0.8W0.2/C is W(0)0.40:W(VI)0.60, W(0)0.42:W(VI)0.58, W(0)0.48:W(VI)0.52, W(0)0.55:W(VI)0.45, respectively. The oxides play a key role in the oxide-rich Pd–W/C electrocatalysts. It was found that the PdO exhibits higher electrocatalytic activity and stability for ORR than Pd in alkaline solutions [64]. WO3 nanoarray supported on carbon cloth has been regarded as a state-of-art catalyst for the oxygen evolution reaction (OER) [65] operating in alkaline media. Zhang et al. [66] reported that Pd supported on WO3/C exhibits a higher ORR activity in acid solution than Pd/C. The strong interaction between Pd and WO3 effectively promotes the direct 4-electron pathway of the ORR at Pd. In this work, the performance of the as prepared oxide-rich Pd–W/C catalyst is enhanced by both the high ORR activity of PdO and the synergistic effect of W/WO3.

2.2. Electrochemical Performance

Figure 5 shows the cyclic voltammograms (CV) of Pd/C (a), oxide-rich Pd0.6W0.4/C (b), Pd0.7W0.3/C(c), Pd0.8W0.2/C (d), Pd0.9W0.1/C (e); all the CVs were measured in 1 M NaOH solution at a scan rate of 10 mV·s−1. All the potentials in this paper are quoted with respect to reversible hydrogen electrode (RHE). All potentials vs. the Hg/HgO electrode were converted to values referring to the RHE using the following equation: E(RHE) = E(Hg/HgO) + 0.098 V + 0.0591 × pH. The peak of hydrogen adsorption/desorption is at about 0.23 V. The peak of OH− adsorbed on the surface of the electrocatalyst is in the range from 0.33 V to 0.53 V. The oxidation of the surface metal and the resulting reduction of the oxide are in the range of 0.33 V to 1.13 V. The peak at ~0.7 V vs. RHE changed dramatically depending on the ratio of Pd and W. There are several factors affecting the current. As mentioned above, the size/diameter of the nanoparticles changed with the content of W. In a smaller nanoparticle, more metal atoms locate at the surface, which is a benefit for the electrochemical reaction. Besides, the peak at ~0.7 V vs. RHE corresponds to the reduction of PdO at the surface of Pd–W bimetallic nanoparticles. The surface Pd content in the oxide-rich Pd–W nanoalloys changes with the Pd:W ratios. Furthermore, the peak current could also be affected by other known/unknown physical properties of the bimetallic nanoparticles. For example, as mentioned above, the addition of W changed the electron structure of Pd atoms. The electrochemical active surface area (EASA) can be calculated by the amount of charge corresponding to the hydrogen adsorption/desorption region in the cyclic voltammetric characteristic curve. However, Pd based catalysts supported on carbon have poor clarity for hydrogen because hydrogen can penetrate into the Pd-based alloy structure. So the reduction charge of PdO was chosen to calculate the EASA. The EASA value of the catalyst was calculated by the following equation:
EASA = Q/QMR
where Q is the coulombs of the reduction of palladium oxide over a range of 0.47 V to 0.87 V, and QMR is the charge required to reduce a monolayer of PdO. The single-layer palladium oxide reduction charge was 4.05 C/m2. The EASA of Pd/C (a), oxide-rich Pd0.6W0.4/C (b), oxide-rich Pd0.7W0.3/C (c), oxide-rich Pd0.8W0.2/C (e) and oxide-rich Pd0.9W0.1/C (d) were 7.85 cm2, 8.75 cm2, 9.91 cm2, 11.8 cm2, and 19.9 cm2 respectively.
Figure 6 displays the linear sweep voltammetry (LSV) of Pd/C (a), oxide-rich Pd0.6W0.4/C (b), Pd0.7W0.3/C (c), Pd0.8W0.2/C (d), Pd0.9W0.1/C (e) catalysts. The LSV curves were measured at a rotating disk electrode (RDE) with a rotating speed of 2000 r/min and a scan rate of 1 mV·s−1. The electrolyte is 0.1 M NaOH solution saturated with O2. Compared with Pd/C, the onset potential at the oxide-rich Pd0.8W0.2/C shifted toward a higher potential. Which is consistent with the prediction of the high activity of Pd3W [47]. As mentioned above, the Pd0.8W0.2 nanoparticles exhibit the smallest size and the largest EASA, which is a benefit for their electrocatalytic performance of ORR.
Chronoamperometry (CA) curves are often used to evaluate the stability of electrocatalysts [67,68]. Electrocatalytic stability of Pd/C and oxide-rich Pd0.8W0.2C catalysts were characterized by CA at 0.57 V vs. RHE in 0.1 M NaOH solution (Figure 7). At the beginning the CA current decreased rapidly, then the current density of each catalyst became relatively stable. The rapid decrease in the initial 1 or 2 s may be the charging current at the working electrode (WE). At the beginning of the CA measurements, the potential at the WE rapidly shifted to the set potential (0.57 V vs. RHE). The rapid shift of potential caused a charging current at the WE. Although the oxide-rich Pd0.8W0.2/C catalyst exhibits higher electrocatalytic stability than Pd/C, it is still difficult to draw a conclusion of whether the composition of the catalyst is unchanged during the ORR measurements. Catalysts with constant compositions such as pure Pd [69] or pure Pt [70] sometimes exhibit poor electrocatalytic stability. Therefore the high electrocatalytic stability does not mean constant composition. It can be seen from Figure 6 that Pd0.9W0.1/C also exhibits high activity. That means even if a half of the W/WO3 de-alloyed from the Pd0.8W0.2 nanoalloys, the Pd–W catalysts still maintain high activity. The current density (mA·mg Pd−1) at the oxide-rich Pd0.8W0.2/C is more than 1.6 times of that at Pd/C.
Figure 8 shows the electrochemical impedance spectroscopy (EIS) of Pd/C and oxide-rich Pd0.8W0.2/C catalysts. EIS measurements were performed from 1 Hz to 100 kHz with 5 mV signals. The semicircle arc radius in the high-frequency region represents the charge transfer resistance (RCT). It can be seen that the charge transfer resistance of the oxide-rich Pd0.8W0.2/C is similar to that of Pd/C.
Figure 9 shows the Koutecky–Levich plots of oxide-rich Pd0.8W0.2/C catalyst, the transferred electron numbers of O2 in ORR were determined by the Koutecky–Levich equation:
B = 0.2   n F   ( D O 2 ) 2 / 3 ν − 1 / 6 C O 2
where B is the reciprocal of the slope of the Koutecky–Levich plots, n is the number of electrons transferred, F is the Faraday constant, D is the diffusion coefficient of O2 in 0.1 M NaOH, ν is the viscosity of the electrolyte, and C is the saturated concentration of O2 in 0.1 M NaOH [71]. Based on the Koutecky–Levich plots and the Koutecky–Levich equation, the calculated number of electrons transferred is 3.8. Thus there is mainly a 4-electron mechanism for the ORR at the oxide-rich Pd0.8W0.2/C catalyst.

3. Materials and Methods

3.1. Preparation and Characterization of the Catalysts

PdCl2 was purchased from Sinopharm Chemical Reagent Co., Ltd. (Shanghai, China). The Vulcan carbon powder XC-72R was obtained from Cabot Corporation (Cabot Corp., Billerica, MA, USA). Nafion solution (5%) was obtained from DuPont (Delaware, DE, USA). All other chemicals were of analytical grade and used as acquired. Triple-distilled water was used through-out. The WO3 containing Pd–W catalysts were prepared with the reduction–oxidation procedures, schematically illustrated in Scheme 1.
Pd/C and PdW/C catalysts with a metal loading of 20 wt% were prepared by the NaBH4 chemical reduction method (Scheme 1, step 1) that we used before [72]. PdCl2 and Na2WO4 were used as the precursors. Electrocatalysts with different atomic ratios were controlled by the molar ratio of metal precursors. The Pd–W nanoalloys are easily oxidized in ambient air and formed the WO3-contained Pd–W/C catalysts (Scheme 1, step 2).
The XRD was carried out by a Bruker D8 advance X-ray diffractometer (BRUKER AXS GMBH, Karlsruhe, Germany) operating at 40 keV and 30 mA with Cu Kα radiation source, λ = 0.15406 nm. The TEM/HRTEM images were obtained on a JEOL JEM-2100 transmission electron microscope (JEOL, Tokyo, Japan). The content of metal elements on the surface of the samples was analyzed by EDS. The presence of the metal was excited by X-ray photoelectron spectroscopy (XPS) using Al Kα X-ray radiation on an ESCALAB 250 (Thermo Fisher SCIENTIFIC, Waltham, MA, USA) spectrometer. Peak fitting using Gaussian/Lorentzian (20% Gaussian) method after background subtraction using Shirley’s method [73].

3.2. Electrochemical Measurements

The electrochemical measurements were performed with CHI832B and CHI660E electrochemical workstations (CHI Instruments, Austin, TX, USA) and a conventional three-electrode electrochemical cell. A carbon-rod was used as the auxiliary electrode. A Hg/HgO electrode was used as the reference electrode. The working electrode was prepared by the following procedure: The glassy carbon electrode (GCE, 3 mm in diameter, LANLIKE, Tianjin, China) was carefully polished with 0.05 μm alumina (Al2O3) powder, and washed with triple-distilled water before use. Ten mg of the catalyst powder in a mixture of 0.5 mL water and 0.5 mL ethanol was ultrasonicated for 15 min to prepare the ink for catalysts. Twenty μL (2 μL× 10 times) of the ink was dropped on the GCE. Three μL of Nafion solution (5 wt.%) was dropped on the surface after the ink was dried in air.

4. Conclusions

The WO3 containing oxide-rich Pd–W/C catalysts were successful fabricated by reduction–oxidation procedures. The as prepared oxide-rich Pd0.8W0.2/C catalysts exhibit high electrocatalytic activity and stability. This demonstrates that the as prepared oxide-rich Pd0.8W0.2/C is a prospective candidate for the cathode of fuel cells operating with alkaline electrolyte.

Author Contributions

The corresponding author W.L. is the director of the other authors. W.L. and N.C. designed the experiments. N.C. and Z.G. carried out the experiments; X.X. and H.Z. analyzed the experimental results.

Acknowledgments

This work was supported by the Natural Science Foundation of Shandong Province (ZR2016BM31). We are greatly appreciate the contributions of Guang Dong, Xin Han, Haoquan Zhang, Shuzheng Xu, Peipei Yu and Mingchen Qin for their kindly repeated the experiments to make sure the data is repeatable, and proofreading the spellings.

Conflicts of Interest

The authors declare no conflict of interest.

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Catalysts 08 00225 sch001 550
Scheme 1. Schematic illustration of the formation of catalyst. Dimensions are not to scale.
Scheme 1. Schematic illustration of the formation of catalyst. Dimensions are not to scale.
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Figure 1. X-ray diffraction (XRD) patterns of Pd/C (a), oxide-rich Pd0.6W0.4/C (b), oxide-rich Pd0.7W0.3/C (c), oxide rich Pd0.8W0.2/C (d), and oxide rich Pd0.9W0.1/C (e).
Figure 1. X-ray diffraction (XRD) patterns of Pd/C (a), oxide-rich Pd0.6W0.4/C (b), oxide-rich Pd0.7W0.3/C (c), oxide rich Pd0.8W0.2/C (d), and oxide rich Pd0.9W0.1/C (e).
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Figure 2. The morphology and particle distribution of Pd/C (a,b) and oxide-rich Pd0.8W0.2/C (c,d).
Figure 2. The morphology and particle distribution of Pd/C (a,b) and oxide-rich Pd0.8W0.2/C (c,d).
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Figure 3. High resolution transmission electron microscopy (HRTEM) (a–c) images and energy dispersive spectroscopy (EDS) spectra (d) of the oxide-rich Pd0.8W0.2/C catalyst.
Figure 3. High resolution transmission electron microscopy (HRTEM) (a–c) images and energy dispersive spectroscopy (EDS) spectra (d) of the oxide-rich Pd0.8W0.2/C catalyst.
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Figure 4. X-ray photoelectron spectroscopy (XPS) spectra of (a) Pd 3d and (b) W 4f) of oxide-rich PdW/C catalysts.
Figure 4. X-ray photoelectron spectroscopy (XPS) spectra of (a) Pd 3d and (b) W 4f) of oxide-rich PdW/C catalysts.
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Figure 5. Cyclic voltammograms (CV) of Pd/C (a), oxide-rich Pd0.6W0.4/C (b), oxide-rich Pd0.7W0.3/C (c), oxide-rich Pd0.8W0.2/C (d), oxide-rich Pd0.9W0.1/C (e) in 1 M NaOH solution. Scan rate 10 mV·s−1.
Figure 5. Cyclic voltammograms (CV) of Pd/C (a), oxide-rich Pd0.6W0.4/C (b), oxide-rich Pd0.7W0.3/C (c), oxide-rich Pd0.8W0.2/C (d), oxide-rich Pd0.9W0.1/C (e) in 1 M NaOH solution. Scan rate 10 mV·s−1.
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Figure 6. Linear sweep voltammetry (LSV) of Pd/C (a), oxide-rich Pd0.6W0.4/C (b), oxide-rich Pd0.7W0.3/C (c), oxide-rich Pd0.8W0.2/C (d), oxide-rich Pd0.9W0.1/C (e) in 0.1 M NaOH solution saturated with O2. Rotating speed 2000 r/min. Scan rate 1 mV·s−1.
Figure 6. Linear sweep voltammetry (LSV) of Pd/C (a), oxide-rich Pd0.6W0.4/C (b), oxide-rich Pd0.7W0.3/C (c), oxide-rich Pd0.8W0.2/C (d), oxide-rich Pd0.9W0.1/C (e) in 0.1 M NaOH solution saturated with O2. Rotating speed 2000 r/min. Scan rate 1 mV·s−1.
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Figure 7. Electrocatalytic stability of Pd/C (a) and oxide-rich Pd0.8W0.2/C (b) in 0.1 mol/L NaOH solution saturated with O2. Potential 0.57 V vs. RHE. Rotating speed 2000 r/min.
Figure 7. Electrocatalytic stability of Pd/C (a) and oxide-rich Pd0.8W0.2/C (b) in 0.1 mol/L NaOH solution saturated with O2. Potential 0.57 V vs. RHE. Rotating speed 2000 r/min.
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Figure 8. EIS of Pd/C and oxide-rich Pd0.8W0.2/C catalysts.
Figure 8. EIS of Pd/C and oxide-rich Pd0.8W0.2/C catalysts.
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Figure 9. Koutecky–Levich plots of oxide-rich Pd0.8W0.2/C catalyst.
Figure 9. Koutecky–Levich plots of oxide-rich Pd0.8W0.2/C catalyst.
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MDPI and ACS Style

Cui, N.; Li, W.; Guo, Z.; Xu, X.; Zhao, H. Electrocatalytic Performance of Carbon Supported WO3-Containing Pd–W Nanoalloys for Oxygen Reduction Reaction in Alkaline Media. Catalysts 2018, 8, 225. https://doi.org/10.3390/catal8060225

AMA Style

Cui N, Li W, Guo Z, Xu X, Zhao H. Electrocatalytic Performance of Carbon Supported WO3-Containing Pd–W Nanoalloys for Oxygen Reduction Reaction in Alkaline Media. Catalysts. 2018; 8(6):225. https://doi.org/10.3390/catal8060225

Chicago/Turabian Style

Cui, Nan, Wenpeng Li, Zengfeng Guo, Xun Xu, and Hongxia Zhao. 2018. "Electrocatalytic Performance of Carbon Supported WO3-Containing Pd–W Nanoalloys for Oxygen Reduction Reaction in Alkaline Media" Catalysts 8, no. 6: 225. https://doi.org/10.3390/catal8060225

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