# Nanoporous PdCo Catalyst for Microfuel Cells:  Electrodeposition and Dealloying

Authors: Satoshi Tominaka; Tetsuya Osaka
Journal: Advances in Physical Chemistry
 (2011)

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## Abstract

PdCo alloy is a promising catalyst for oxygen reduction reaction of direct methanol fuel cells because of its high activity and the tolerance to methanol. We have applied this catalyst in order to realize on-chip fuel cell which is a membraneless design. The novel design made the fuel cells to be flexible and integratable with other microdevices. Here, we summarize our recent research on the synthesis of nanostructured PdCo catalyst by electrochemical methods, which enable us to deposit the alloy onto microelectrodes of the on-chip fuel cells. First, the electrodeposition of PdCo is discussed in detail, and then, dealloying for introducing nanopores into the electrodeposits is described. Finally, electrochemical response and activities are fully discussed.


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## Body

## 1. Introduction

Recent progress in microelectrochemical devices, for example, on-chip fuel cells    [1–6], microbatteries    [7, 8], and on-chip sensors    [9, 10], inevitably requires developments of both electrode materials with a large surface area and processes for depositing such materials precisely onto the tiny current collectors. For such selective deposition, we regard that electrodeposition is attractive, because this technique enables us to selectively synthesize metals onto conductive materials, even onto microelectrodes and to directly synthesize alloys without thermal treatment    [11–13]. Moreover, its possible control of morphology by tuning applied current densities appears applicable to the synthesis of nanostructured materials    [12–14]. Thus, electrodeposition is an important technique for synthesizing electrode materials for microelectrochemical devices. In view of this, we electrodeposited electrocatalysts for on-chip fuel cells, for example, Pt black, PtRu alloy, and PdCo alloy    [1, 2, 11, 15].In order to increase surface area of electrode of interest, nanostructured materials, for example, nanoparticles, have been widely used. Moreover, since each of the devices needs electrode with a different porosity appropriate to its own requirements for reactant and product transportations, synthesis of nanoporous structures with defined porosity is beneficial. For example, nanoporous Pt electrodes synthesized using soft or hard templates    [16–19]. Though such templating processes are useful for synthesizing well-organized nano- and microstructures, they are generally time consuming and need hazardous chemicals to remove the templates. Therefore, we considered that more versatile methods for synthesizing nanostructured electrodes for microelectrochemical devices need to be developed.Contrary to such templating methods, the dealloying method can form metals with sponge-like nanoporous structures without any templates    [20, 21]. Dealloying refers to the selective dissolution of one or more components out of an alloy. The unique porous structure is formed by a competition of two processes: dissolution of less-noble component (i.e., pore formation) and surface diffusion of more noble component to aggregate into two-dimensional clusters (i.e., surface passivation)    [20–24]. Their surface area can reach a value comparable to those of nanoparticles when the pore size is a nanoscale [25].Here, we summarize our recent research on the synthesis of nanostructured PdCo catalyst by electrochemical methods, which enable us to deposit the alloy onto microelectrodes of the on-chip fuel cells [1]. We have used the combination of electrodeposition and dealloying in order to synthesize sponge-like nanoporous thin films    [26–28] and coral-reef-like nanostructures [29] selectively onto current collectors as illustrated in Figure 1.Electrochemical synthesis of nanostructured PdCo catalyst selectively on Au layer by (i) electrodeposition and (ii) dealloying. (a) Sponge-like nanoporous thin film and (b) nanoporous dendrites. Such three-dimensional porosity is beneficial in terms of diffusion inside.
(a)(b)Pd-based alloys such as PdCo are attractive as oxygen reduction reaction (ORR) catalysts for direct methanol fuel cells (DMFCs) because of its high activity comparable to Pt catalyst and its high tolerance to methanol    [30–35]. Based on the latter property, we have used this catalyst for realizing a tiny on-chip DMFC of a membraneless design [1]. Since Pd-based catalyst may not be sufficiently stable in acidic media at such a positive potential for oxygen reduction reaction for practical use [36], we have tested the use of neutral pH atmosphere for the on-chip fuel cell system    [1, 3]. For the reasonable comparison with data reported by others, we used sulfuric acid as the supporting electrolyte for evaluating catalytic activity in this paper.Figure2 is a phase diagram of PdCo alloy with an indication of composition range enhancing ORR (PdxCo1−x, x=0.7-0.9)    [30–35, 37–41]. This alloy system mainly forms solid solution phase, but in some composition range, ordered phases of intermetallic compounds such as L12 phase (i.e., Pd3Co1) and L10 phase (i.e., Pd1Co1) can be formed    [42, 43]. In the potential range where high ORR activities were obtained, L12 type Pd3Co1 phase may exist. Since those ordered phases were detectable only by electron diffraction, we have to be careful on such. The surface composition was reported to be Pd-rich after reduction in H2 and Co-rich after oxidation. This surface segregation is typical for this type of alloys as supported by the alloy segregation theory [44].Figure 2
Phase diagram of PdCo system showing the composition range where oxygen reduction reaction is enhanced. The diagram was based on the figure reported in the literature [43]. Mainly, the phase is an fcc solid solution. In specific composition range, the alloy contains ordered fcc phase (L12 type) or ordered face-centered tetragonal phase (L10 type).In order to use PdCo catalyst for fuel cells, understanding of electrochemistry is needed. Mallet et al. reported linear sweep voltammograms of PdCo alloys scanned in acidic solution [42]. Figure 3(a) shows that the disordered phases did not exhibit any anodic current associated with Co dissolution, but this does not mean high stability of them, because the authors reported that these samples lost some portion of Co atoms just after dipping into the solution. It is reasonable that the redox potential of Co is more negative than the hydrogen evolution potential in the acid solution. The removal of Co atoms probably resulted in the formation of a passive Pd layer.Linear seep voltammograms of PdCo powders (positive scans) in nitrogen-saturated 0.5 M sulfuric acid solution: (a) Before heat treatment: Curve (a) Pd3Co1, curve  (b) Pd1Co1, and curve  (c) Pd1Co3. (b–d) After heat treatment at 500°C: Curve  (a) first sweep and curve  (b) second sweep after reduction with hydrogen. Reproduced with permission from [42]. Copyright 1986, Elsevier.
(a)(b)(c)(d)Since, from the viewpoint of thermodynamics, Co atoms in the ordered phases are considered more stable than those in disordered phases, the Pd-rich ordered phases of L12 type are considered the most stable in acidic media. Anodic current attributable to Co dissolution was observed for an ordered phase of Pd3Co1 above ~0.8 V, which is more negative than fuel cell cathode potential. This result indicates the stability may not be sufficient even for this phase. Considering that the charge associated with the dissolution was roughly in the same level as oxide formation current and that such dissolution was observed only in the first scan, only the surface Co atoms were considered to be dissolved. The same thing holds true for the other ordered phases. These results indicate that the surface of PdCo alloys is stabilized in the fuel cell condition by the formation of Pd skin layer.


## 2. Synthesis of PdCo Alloys by Electrodeposition

Electrodeposition of PdCo alloys was investigated by Abys et al. [45], and their aqueous bath was in a mixed ligand system. The first ligand, that is, ammonia, forms strong complexes with palladium and weak complexes with cobalt. The second ligand, that is, an organic molecule containing carboxylic acid group(s), forms strong complexes with cobalt, because cobalt complexes (octahedral with coordination number 6 [46]) bind favorably to oxygen containing ligands rather than to nitrogen containing ligands. These complex formations bring the deposition potentials of Pd and Co closer. Moreover, pH control of the solution (<10.58) is important to obtain a stable bath. They investigated numerous ligands consisting of mono-, di-, and tetracarboxylic acid.Figure4 shows typical scanning electron microscope images of PdCo alloy synthesized by electrodeposition. By applying a low current density, a flat film with granular surface with ca. 10-nm particles was obtained (Figure 4(a)), while dendritic deposits with ca. 50-nm particles were obtained by applying a high current density (Figure 4(b)). The pores between dendritic deposits were expected to make the entire surface readily accessible by the reactants. The deposition condition and the solution were adjusted to obtain active catalyst for ORR (details are available in Section 6) [11]. The particle size is quite large compared to that of typical fuel cell catalysts, that is, <10 nm, reasonably leading to the conclusion that further improvement in nanostructure is needed for fuel cell applications. Thus, the surface was modified with additional PdCo deposits with smaller particles, which were deposited at a similar condition as the flat PdCo film. As shown in Figure 4(c), the surface of the dendrites was successfully covered with small particles in the 5–10 nm range. This treatment increased the surface area by ca. 30% as summarized in Table 1.Table 1
Oxygen reduction reaction characteristics of the PdCo catalysts evaluated in 0.5 M H2SO4 compared with those of Pt electrode and Pd electrode.
Electrode performanceb/mA cm−2Specific activitye/μA cm−2Onset potentiala/V0.65 V versus Ag/AgCl0.60 V  versus Ag/AgCl0.65 V versus Ag/AgCl0.60 V versus Ag/AgClTafel slope/mV decade−1Roughness factor/−Ref.Pt electrodef0.723.5 × 10−21.1 × 10−18.42.7 × 10171c, 116d4.2[60]Pd thin filmg0.581.0 × 10−4 h5.8 × 10−4 h3.4 × 10−2 h1.9 × 10−1 h673.1[11]PdCo thin filmf0.662.4 × 10−22.6 × 10−11.51.6 × 1014416[60]PdCo dendriteg0.685.7 × 10−26.2 × 10−1 h4.44.7 × 101 h4813[15]Modified PdCo dendriteg0.711.9 × 10−11.6h1.1 × 1019.2 × 101 h5517[15]Nanoporous PdCo thin filmf0.693.5 × 10−12.58.66.2 × 1014341[60]Nanoporous PdCo dendriteg0.723.9 × 10−1 i—1.3i——290[29]aat the current density of 1 μA cm−2 (electrochemically active surface area). bbased on the geometrical surface area. c0.7–0.75 V. d0.55–0.65 V. ebased on the electrochemically active surface area. fmeasured by hydrodynamic voltammetry at room temperature (22°C). gmeasured by linear sweep voltammetry at (30°C). hestimated by extrapolating the Tafel slope. iwith a slight mass-transfer limitation.SEM images of PdCo alloys synthesized by electrodeposition: (a) at a low current density, (b) at a high current density, and (c) modification of the sample “b” by additional deposition. Left: cross-sectional view. Right: plan view. Reproduced with permission from [15]. Copyright 2007, The Electrochemical Society.
(a)(b)(c)The dendritic one was a substitutional solid solution of Pd75Co25, which is in the composition range active in the ORR [11] (cf. Figure 2). The X-ray photoelectron spectroscopy (XPS) results (Figure 5) indicate that the surface Pd and Co were metallic, not oxide, by comparing the binding energies of the deposits (Pd 3d5/2: 334.7 eV, Co 2p3/2: 777.4 eV) to those of a metallic Pd and a metallic Co reported in the literature (Pd 3d5/2: 335.1 eV, Co 2p3/2: 778.3 eV [47]). The spectra also suggest that the surface composition was apparently Pd-rich by comparing the peak intensities with taking the sensitivity factors into consideration (the factor of Pd 3d is ~1.5 times larger than Co 2p [47]). That is, Pd-skin was formed as often reported for Pt alloy catalysts of fuel cells    [48, 49]. The skin was probably formed by the dissolution of surface Co by air or Pd ions in the solution.Core-level XPS of PdCo thin film of Pd 3d and Co 2p. The vertical dotted lines refer to Pd 3d5/2 of pure Pd and Co 2p3/2 of pure Co. The data of PdCo dendrites is consistent with this data. Reproduced with permission from [11]. Copyright 1986, Elsevier.
(a)(b)Figure6 shows the electrochemical response of the PdCo film in an acid solution, compared with that of a pure Pd film. The cyclic voltammogram (CV) of PdCo is similar to that of Pd, except for the sharp peaks obtained in the hydrogen region (−0.2 to +0.1 V). Since this CV trace of the PdCo film is similar to that of a nanostructured Pd (Pd-black), we assigned the peaks located in the hydrogen region in accordance with a report on nanostructured Pd [50]:(i)
Peak 1 (0.05 V): hydrogen adsorption/desorption for the surface Pd (strongly bound),(ii)
Peak 2 (−0.05 V): hydrogen absorption/desorption for the subsurface Pd (α and β phases),(iii)
Peak 3 (−0.2 V): hydrogen adsorption/desorption for the surface Pd or hydrogen evolution/oxidation reactions (less-strongly bound).Cyclic voltammograms of the electrodeposited PdCo catalyst scanned at 50 mV s−1 in 0.5 M H2SO4 deaerated with N2 at lower (a) and at higher (b) expansion of current axis scale. The dotted line is a voltammogram of the electrodeposited Pd. The current density was normalized by electrochemical surface areas. Reproduced with permission from [11]. Copyright 1986, Elsevier.
(a)(b)From this identification, it is found that the sharp peaks of PdCo (Peaks 1 and 3) strongly indicate the presence of Pd-skin. Compared with pure Pd, the hydrogen absorption was found to be prevented by alloying with Co.In the oxide region, the current densities from the PdCo are almost the same as that from the Pd, this meaning that the amount of sites binding with oxygen atoms is the same. However, the potential of oxide formation/deformation of the PdCo alloy was shifted to more negative potential, and this means that the Pd-skin is easily oxidized compared with pure Pd. This tendency was reported also by other groups [31]. Interestingly, this effect of the alloying on the oxide region is opposite to that of Pt alloys    [51, 52] and to the prediction based on the shift of d-band center to a larger binding energy and the result of first-principle consideration    [31, 53]. Since the CV behavior in the potential region was dominated by adsorption of oxygenated species and desorption of sulfate anions, we speculate that the apparent negative shift of oxidation potential was probably due to the negative shift of sulfate desorption potential.The current densities of the CVs were based on electrochemically active area (Aec). Such area of Pt electrode has been calculated on the basis of hydrogen adsorption charge    [54, 55], and that of Au electrode has been calculated on the basis of oxide reduction charge    [55, 56]; however, on Pd electrode, hydrogen absorption in hydrogen region and Pd dissolution in the oxide region make such charges unclear    [36, 57]. In view of this, we assumed that the double-layer capacitance (Cdl) per Aec for Pd was the same as that for Pt. This assumption is acceptable, because the adsorbed-sulfate structure on a Pd electrode is similar to a Pt electrode. In detail, the adsorbed-sulfate structure was reported to be the same on (111) surface and slightly different on (100) surface    [58, 59]. We measured such capacitance for Pt by cyclic voltammetry, and a value of 86 μF cm−2 was obtained. Using this value, the electrochemically active surface areas of PdCo alloys were calculated.For the successful improvement of microfuel cell performance, large surface area of catalyst is needed [5]. General direct methanol fuel cells require Pt loading of about 2.5 mg cm−2. This loading is translated into a roughness factor (a ratio of actual electrode surface area divided by geometrical one) of 2000 (80 m2 g−1) [39]. The value of the PdCo dendrite described above was 13.3. Even though longer deposition time was used, the value was limited to less than 100. This large gap is because the particles of the electrodeposited dendrites were more than ten times as big as the nanoparticles generally used for fuel cells. Thus, in order to increase the surface area of such electrodeposits, we have introduced nanopores into the electrodeposits by dealloying.


## 3. Electrochemical Dealloying for Introducing Nanopores into Electrodeposits

In order to increase the surface area of electrodeposited PdCo catalyst, we used dealloying technique as illustrated in Figure1(a). First, a Co-rich PdCo alloy was electrodeposited, and then, the deposit was partially dealloyed by applying more positive potential in a sulfuric acid solution. A thin film of nanoporous PdCo catalyst was thus synthesized. Figure 7 shows that the dealloyed PdCo thin film was highly porous sponge-like film with <50-nm thick ligaments. The TEM images show crystalline ligaments whose lattice spacing was observed to be ca. 0.22 nm, which is close to that of Pd(111) plane (0.226 nm). Interestingly, Figure 7(D) indicates that the ligament was formed by large crystal domains; namely, the ligaments were not composed of small particles, but of a long single crystal domain.Figure 7
Electron micrographs of the dealloyed PdCo film. Cross-sectional (A) and (B) plan-view SEM images. (C, D) TEM images. (a-c) High-resolution images of lattice fringes with a lattice distance of 2.2 Å. Reproduced with permission from [27]. Copyright 2010, RSC.The as-deposited PdCo alloy of a nonporous fcc Pd30Co70 film became the sponge-like nanoporous Pd93Co7. In accordance with Vegard’s law, since the peak angles of XRD pattern were shifted to higher angles [60], the crystal domains of the dealloyed PdCo alloy were found to be a substitutional solid solution of Pd92Co8. This degree of lattice contraction seems of great promise as ORR catalyst, because such a 8% lattice contraction was reported to endow Pd alloys with a high ORR activity [53].The XPS results (Figure8) show that the surface of this dealloyed thin film was Pd-rich, suggesting the formation of a Pd-skin layer as those of electrodeposited PdCo catalyst. The presence of Pd-skin was confirmed by CV measurement as shown in Figure 11. Compared with those of electrodeposited PdCo catalyst (Figure 5) and the as-deposited one (Figure 8), the dealloyed one had the Pd 3d5/2 peak located at a slightly higher energy. Since the Pd 3d5/2 peak energy located at 335.5 eV is close to that of a metallic Pd (335.1 eV) rather than those of Pd oxides (PdO at 336.3 eV and PdO2 at 337.9 eV) [47], the Pd skin of the dealloyed one was still metallic. The slight shift toward higher energy probably suggested that the lattice of the Pd skin layer was contracted by the presence of subsurface PdCo alloy.Core-level XPS of the nanoporous PdCo thin film of Pd 3d and Co 2p. The vertical dotted lines refer to Pd 3d5/2 of pure Pd and Co 2p3/2 of pure Co. Reproduced with permission from [27]. Copyright 2010, RSC.
(a)(b)Since there was a concern about that, for use as an electrode for fuel cells, reactant transports seem hampered by their small and tortuous pores. On this point, we conceived that the macropores between dendrites formed by electrodeposition can compensate for the limitation. In this view, we proposed a simple method to synthesize a unique nanostructure with both a hierarchical porosity and a large surface area, that is nanoporous dendrites, which have macropores between dendrites formed by electrodeposition and nanopores formed by dealloying (Figure1(b)).Likewise, the dealloying of dendritic structures resulted in the nanoporous dendrites as shown in Figures9 and 10. Compared with as-deposited ones, the nanopores were found to be formed without changing the macroscopic morphology of dendrites (Figure 9(b)). The dendrites consisted of 100–300 nm nanoparticles having ~10 nm nanopores. The sponge-like porous structure is typical for the metal architecture prepared by dealloying. Since the lattice fringes were observed to be aligned over nanopores (Figure 10(c)), the crystallites were found to be larger than the ligaments. The whole deposited layer was thin enough (4-5 μm) for use as a catalyst for on-chip fuel cells [1]. The macropores between the deposits are expected to make the entire surface of the dendrites readily accessible by oxygen.SEM images of nanoporous PdCo dendrites: (a–c) plan view, and (d) cross-sectional. The sample shown in “a” and “b” was electrodeposited at a constant current of –50 mA cm−2 for 600 s followed by the immersion in an air-saturated 0.5 M sulfuric acid solution for ~15 h at 60°C. The sample shown in “c” and “d” was prepared by galvanic pulse deposition and dealloying. Reproduced with permission from [29]. Copyright 2010, Elsevier.
(a)(b)(c)(d)TEM images (a–c) and selected-area electron diffraction pattern (d) of nanoporous PdCo dendrites synthesized by the combination of electrodeposition and dealloying. The parallel lines in “c” show the direction of lattice fringes. The diffraction pattern was collected at 200 kV with a camera length of 1.0 m. The inset in “d” is another diffraction pattern. Reproduced with permission from [29]. Copyright 2010, RSC.
(a)(b)(c)(d)Figure 11
Comparison of cyclic voltammograms of the PdCo dendrite (dashed red line), nanoporous PdCo thin film (dotted blue line), and  nanoporous PdCo dendrite (black solid line) scanned in 0.5 M H2SO4 deaerated with N2 at 50 mV s−1. The inset shows voltammogram of the nanoporous dendrite scanned at 5 mV s−1.The bulk composition and crystal structure were changed from amorphous Pd24Co76 (as-deposited one) to a polycrystalline fcc crystals of Pd79Co21, whose XRD pattern was well consistent with that of a pure fcc Pd. The surface composition was determined to be nearly pure metallic Pd by XPS, which corresponds to the results shown in Figure 5. This layer probably protected the residual Co atoms in the subsurface alloy phases from leaching out. As we described above, Pd atoms in some easily dissolvable phases, for example, solid solutions and intermetallic compounds of PdCo3 (L12 phase) [42], probably resulted in thick Pd skin layers that incorporated some relatively stable phases, for example, fcc Pd3Co (L12 phase) and fct Pd1Co1 (L10 phase).Electron diffraction (Figure10(d)) reveals such presence of alloy domains. The diffraction pattern is assignable to a face-centered tetragonal structure with lattice parameters of a = 4.9 Å and c = 2.5 Å, or a hexagonal close packing (hcp) structure with lattice parameters of a = 2.8 Å and c = 4.1 Å, observed at [111] direction (for determining details, further investigation is needed). Compared with fcc Pd (a = 3.90 Å), fcc Co (a = 3.54 Å) and  hcp Co (a = 2.51 Å and c = 4.09 Å), whichever, this pattern can be assignable to an alloy phase. In addition, we could obtain weak polycrystalline fcc ED pattern as shown in the inset, this might be assignable to the surface Pd skin layer, considering the fact that a fcc pattern was obtained by XRD. Thus, we can conclude that the nanoporous dendrites contained both crystalline pure Pd skin layer and fct or hcp PdCo alloy phase.


## 4. Comparison as Catalyst Layers for Microfuel Cells

Figure11 compares CVs of the PdCo catalysts synthesized. Electrochemical response of the nanoporous dendrite was apparently larger than nanoporous thin film and nonporous dendrite. The roughness factor of the nanoporous dendrite was determined to be ca. 290. This value is more than twentyfold of the value of the PdCo dendrite without nanopores (ca. 13), indicating a positive effect of the formation of nanopores even though the nanoporous one is a few times thicker than the nonporous one (ca. 1.5 μm). This quite large surface area is expected to improve the electrode performance. The roughness factors were compared also in Table 1.ORR activities of the PdCo catalysts synthesized are compared in Table1. Apparently, the electrode performances of the nanoporous catalysts are higher than those of nonporous ones, and the nanoporous dendrite exhibited the best performance. This is simply because of its large surface area. The onset potentials were ~0.7 V versus Ag/AgCl, which is by 0.1 V more positive than pure Pd catalyst and comparable to pure Pt catalyst. In terms of specific activity, most of PdCo alloys were comparable to Pt catalyst at 0.65 V and became better at 0.60 V. Thus, we confirmed positive effect of alloying.The activity of nanoporous PdCo thin film was ~200 times higher than that of pure Pd catalyst and still a few times higher than the PdCo alloys which did not exhibit the apparent peak shift of Pd 3d XPS (i.e., PdCo dendrite, PdCo thin film and nanoporous PdCo dendrite). Therefore, we conclude that the lattice contraction of the surface Pd-skin is the most important, and the nanoporous PdCo thus obtained had an active surface as well as the large surface area.The higher activity than Pt catalyst is because of the preferably small Tafel slope, which indicates that the rate-determining step of ORR on the nanoporous PdCo thin film was different from Pt catalyst. As discussed previously [60], all of the PdCo catalysts synthesized by electrochemical methods had small Tafel slopes as shown in Table 1. Those values are apparently smaller than those of PdCo catalysts synthesized by other techniques (60–70 mV decade−1). This unique property of such PdCo catalysts synthesized by electrochemical techniques is of significant importance for developing effective catalysts.


## 5. Conclusions

We have synthesized PdCo catalysts for microfuel cells by electrodeposition and electrochemical dealloying. The former technique successfully synthesized PdCo alloys selectively onto conductive Au substrates, and by changing the potential applied, morphologies of the deposits were tuned into thin films or dendrites. The latter technique successfully increased the electrochemically active surface area by roughly ten times. Thus, such combination of electrodeposition and dealloying was proved effective for synthesizing high-performance electrodes for microsystems.In terms of fuel cell catalyst, the PdCo nanostructures exhibited better activity for oxygen reduction reaction than Pt catalyst, especially in the potential range of interest for actual fuel cell operation (0.8 V versus NHE). This is because of the smaller Tafel slope value of our PdCo catalysts. We believe that detailed analyses on such unique Tafel slope values, which have been obtained only for such PdCo catalysts synthesized by electrochemical methods, are needed and of quite importance for developing effective fuel cell catalysts.


## 6. Experimental

### 6.1. Synthesis

PdCo thin film was electrodeposited at −10 mA cm−2 for 60 s, and PdCo dendrite was deposited at −200 mA cm−2 for 5 s. The dendrite was modified by further deposition at −0.75 V versus Ag/AgCl for 10 s. This potential was consistent with the deposition potential of the PdCo thin film at −10 mA cm−2. The deposition bath contained 76 mM [Pd(NH3)4]Cl2, 34 mM CoCl2, 78 mM NH4Cl and 120 mM malonic acid (pH = 9.1, adjusted by NH4OH).Nanoporous PdCo flat film was synthesized as follows. First, Co-rich PdCo thin film was electrodeposited at −0.9 V versus Ag/AgCl for 10 min in a solution containing 34 mM [Pd(NH3)4]Cl2, 76 mM CoCl2, 76 mM NH4Cl and 268 mM malonic acid at 14 ± 2°C. This solution was prepared by mixing (i) a Pd solution containing 68 mM [Pd(NH3)4]Cl2 and 152 mM NH4Cl (pH = 10 adjusted by NH4OH) and (ii) a Co solution containing 152 mM CoCl2 and 536 mM malonic acid (pH = 10 adjusted by NH4OH), in a volume ratio of 1 : 1. Then, the solution was aged for 3 days at 14°C. The PdCo film thus obtained was electrochemically dealloyed for 6 h at 0.6 V in 0.5 M H2SO4 deaerated with N2 (~22°C).Nanoporous PdCo dendrites with hierarchical porosity were synthesized as follows. First, Co-rich PdCo dendrites were electrodeposited by applying a galvanic pulse (on: −40 mA cm−2 for 1 s; off: 2 s; 500 cycles) in a bath of the same composition for synthesizing nanoporous thin film but without the aging treatment. Then, the electrodeposits were dealloyed by immersing in an air-saturated 0.5 M H2SO4 at 60°C overnight (~15 h).For these deposition experiments, a conventional three-electrode cell was used. The reference and the counter electrodes were a Ag/AgCl (KCl-saturated) electrode and a Pt coil, respectively. The working electrode was a flat Au thin film (200 nm thick), which was deposited on silicon substrate with 20-nm Ti adhesion layer by electron-beam evaporation [11].


### 6.2. Characterization

The morphology was observed using a high-resolution scanning electron microscope (HR-SEM) (S-5500, Hitachi). The composition was determined by energy dispersive X-ray fluorescence spectroscopy or by inductively coupled plasma atomic emission spectroscopy. The surface composition and the surface elemental state were evaluated by X-ray photoelectron spectroscopy (XPS) using an Mg target. The crystal structure was examined by means of X-ray diffractometry (XRD) using a Cu Kα radiation.The surfaces of the synthesized catalysts were electrochemically cleaned by scanning in a 0.5 M H2SO4 solution deaerated with N2 in the potential range of +0.2 to 1.0 V versus Ag/AgCl at 50 mV s−1. The electrochemical response was evaluated by cyclic voltammetry (CV) in a 0.5 M H2SO4 deaerated with N2 in the potential range of −0.2 to +1.0 V versus Ag/AgCl at 50 mV s−1. The roughness factor was calculated based on the double-layer capacitance in the CVs (8.6 mF cm−2) [11]. The activity for the oxygen reduction reaction was evaluated by linear sweep voltammetry (LSV) in an oxygen-saturated 0.5 M H2SO4 solution from the open circuit potential.


## 6.1. Synthesis

PdCo thin film was electrodeposited at −10 mA cm−2 for 60 s, and PdCo dendrite was deposited at −200 mA cm−2 for 5 s. The dendrite was modified by further deposition at −0.75 V versus Ag/AgCl for 10 s. This potential was consistent with the deposition potential of the PdCo thin film at −10 mA cm−2. The deposition bath contained 76 mM [Pd(NH3)4]Cl2, 34 mM CoCl2, 78 mM NH4Cl and 120 mM malonic acid (pH = 9.1, adjusted by NH4OH).Nanoporous PdCo flat film was synthesized as follows. First, Co-rich PdCo thin film was electrodeposited at −0.9 V versus Ag/AgCl for 10 min in a solution containing 34 mM [Pd(NH3)4]Cl2, 76 mM CoCl2, 76 mM NH4Cl and 268 mM malonic acid at 14 ± 2°C. This solution was prepared by mixing (i) a Pd solution containing 68 mM [Pd(NH3)4]Cl2 and 152 mM NH4Cl (pH = 10 adjusted by NH4OH) and (ii) a Co solution containing 152 mM CoCl2 and 536 mM malonic acid (pH = 10 adjusted by NH4OH), in a volume ratio of 1 : 1. Then, the solution was aged for 3 days at 14°C. The PdCo film thus obtained was electrochemically dealloyed for 6 h at 0.6 V in 0.5 M H2SO4 deaerated with N2 (~22°C).Nanoporous PdCo dendrites with hierarchical porosity were synthesized as follows. First, Co-rich PdCo dendrites were electrodeposited by applying a galvanic pulse (on: −40 mA cm−2 for 1 s; off: 2 s; 500 cycles) in a bath of the same composition for synthesizing nanoporous thin film but without the aging treatment. Then, the electrodeposits were dealloyed by immersing in an air-saturated 0.5 M H2SO4 at 60°C overnight (~15 h).For these deposition experiments, a conventional three-electrode cell was used. The reference and the counter electrodes were a Ag/AgCl (KCl-saturated) electrode and a Pt coil, respectively. The working electrode was a flat Au thin film (200 nm thick), which was deposited on silicon substrate with 20-nm Ti adhesion layer by electron-beam evaporation [11].


## 6.2. Characterization

The morphology was observed using a high-resolution scanning electron microscope (HR-SEM) (S-5500, Hitachi). The composition was determined by energy dispersive X-ray fluorescence spectroscopy or by inductively coupled plasma atomic emission spectroscopy. The surface composition and the surface elemental state were evaluated by X-ray photoelectron spectroscopy (XPS) using an Mg target. The crystal structure was examined by means of X-ray diffractometry (XRD) using a Cu Kα radiation.The surfaces of the synthesized catalysts were electrochemically cleaned by scanning in a 0.5 M H2SO4 solution deaerated with N2 in the potential range of +0.2 to 1.0 V versus Ag/AgCl at 50 mV s−1. The electrochemical response was evaluated by cyclic voltammetry (CV) in a 0.5 M H2SO4 deaerated with N2 in the potential range of −0.2 to +1.0 V versus Ag/AgCl at 50 mV s−1. The roughness factor was calculated based on the double-layer capacitance in the CVs (8.6 mF cm−2) [11]. The activity for the oxygen reduction reaction was evaluated by linear sweep voltammetry (LSV) in an oxygen-saturated 0.5 M H2SO4 solution from the open circuit potential.



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*Source: 821916-2011-08-18.xml*