# Effect of the Reduction Temperature of PdAg Nanoparticles during the Polyol Process in the Ethanol Electrooxidation Reaction

Authors: R. Carrera-Cerritos; C. Salazar-Hernandez; I. R. Galindo-Esquivel; R. Fuentes-Ramirez
Journal: Journal of Nanomaterials
 (2018)

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## Abstract

This work reports the effect of reduction temperature during the synthesis of PdAg catalysts through the polyol process and their evaluation in the ethanol electrooxidation reaction (EOR). The characterization was performed using Transmission Electron Microscopy (TEM) and X-Ray Diffraction (XRD). The electrochemical evaluation for the ethanol electrooxidation reaction was implemented in alkaline medium using chronoamperometry (CA) and cyclic voltammetry (CV). An important effect of the reduction temperature on electroactivity and catalytic stability was observed: both the maximum current density and the catalytic stability were higher in the catalyst synthesized at the highest temperature (135°C). This performance was associated with the extent of the interaction between Pd and Ag which was measured in terms of the structural expansion of Pd.


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## Body

## 1. Introduction

Researchers concerned in current environmental pollution problems and the depletion of fossil fuels have found interest in new sources of renewable and clean energy. Ethanol is an alcohol with high energy density (8 KW-h/kg), which can be renewable if obtained from biomass. Ethanol is also nontoxic and has characteristics that allow it to be stored and transported easily and safely [1]. These properties make ethanol an attractive power source for fuel cells used to produce electricity for mobile devices and transport applications [2, 3]. However, the ethanol electrooxidation reaction (EOR) that occurs at the anode has slow kinetics in the catalysts currently used, so the development of anodic materials with high electroactivity and stability is still a challenge [4, 5].Among the pure elements, palladium has been identified as the most suitable catalyst for the EOR in alkaline solutions due to its high activity and stability during the reaction [6, 7]. For this reason, several attempts have been made to improve its catalytic performance through a combination with other elements, since bimetallic and multimetallic catalysts synthesized at nanoscale contribute to the enhancement of the catalytic activity [8–10]. A criterion usually used to qualitatively determine surface reactivity is the use of the d-band center. According to this model, a shift in the position of thed-band center towards the Fermi level indicates an improvement in the chemisorption properties, which are then associated with the reactivity of the material. The Density of States (DOS) for thed-band of the metal varies from metal to metal, and it can be modified by several factors such as ligand and geometric effects. This then leads to a variation of the electronic properties of the metal. According to Hammer and Nørskov calculation, the center of thed-band of Pd (3.89 Å) will shift when combined with Ag (a=4.09 Å) [11]. As a result, and because silver is a much cheaper and abundant metal than Pd, the bimetallic nanoparticles of PdAg are receiving great attention. These materials may be able to potentiate various reactions such as Oxygen Electro-Reduction and the electrooxidation of small chain alcohols [12, 13].The polyol method is a very fast method that does not require extreme conditions or sophisticated equipment and can be scaled up to produce larger amounts of nanoparticles. Due to these properties, this method has been used for the synthesis of many metal nanoparticles. In fact, the polyol method has been extrapolated for the synthesis of PdAg nanoparticles of different shapes and sizes [14, 15]. The evaluation of the PdAg nanoparticles as catalysts for EOR in alkaline medium has shown that the synergistic interaction between the Pd and Ag atoms not only produces materials that exhibit excellent catalytic activity but also promotes tolerance towards the adsorbed CO, thus improving the catalytic stability during EOR [16]. However, the activation energy for the EOR reaction has not been sufficiently reduced [17, 18]. In addition, the effect of alloy grade and particle size on the catalytic activity has not been explored in detail. Considering the above, interesting catalytic properties could be inferred when manipulating the temperature of reduction during the polyol process in order to modify the degree of interaction between the palladium and the silver. Thus, the synthesis of the PdAg nanoparticles supported on carbon vulcan at three different temperatures was performed. The catalysts were characterized by TEM and XRD. Also, the electrocatalytic activity of the nanoparticles in the EOR was evaluated in alkaline solutions using CV and CA.


## 2. Materials and Methods

### 2.1. Synthesis of PdAg Catalysts

The previously reported polyol method to obtain pure Pd-based nanobars was modified in order to obtain bimetallic nanoparticles of PdAg [14, 15]. This process is described as follows: 5 ml of ethylenglycol (EG, 99.9%, J.T. Baker) were added to a 25 ml three-necked flask coupled to a reflux system. The flask was then heated to 105°C (PdAg-a), 120°C (PdAg-b), and 135°C (PdAg-c) with constant stirring. Two solutions were prepared separately: (1) 0.0486 g of Na2PdCl4 (98%, Sigma-Aldrich) and 0.6 g of KBr (99%, Sigma-Aldrich) were dissolved in 1 ml of deionized water, and (2) 0.0916 g of PVP (99%, Sigma-Aldrich) and 0.005 g of AgNO3 (99%, Sigma-Aldrich) were added in 3 ml of EG. The solution with the Pd precursor (1) was added to the three-necked flask and, after three minutes, the silver solution (2) was incorporated. The mixture was allowed to react for 1 h at a fixed temperature. Vulcan at a ratio 20/80 Pd/C was added during the reaction; this support was preheated at 277°C for 3 h. At the end of the reaction time, the product was cooled down to room temperature. Subsequently, it was separated by centrifugation with acetone (99.9%, JT Baker) and then washed with deionized water 8 to 10 times. The speed used for the first separation was 4000 rpm, while 60000 rpm was used for rinsing. Finally, the product was dried at 100°C for 12 h.


### 2.2. Catalyst Characterization

The visualization of the synthesized nanoparticles was carried out in a JEOL Transmission Electron Microscope, model JEM-1010 equipped with a tungsten filament. It was operated with 80 kV and a magnification of 200000x. The microscope has a model ORIUS digital camera and was operated with the GATAN software. The crystallinity of the catalysts was analyzed in powder using a Rigaku Miniflex instrument. The radiation emitted by the X-ray tubes of this diffractometer corresponded to the Cu Kα (1.5406 Å). The patterns were collected from 2θ=5 to 80°, with a step of 0.02°, and a count time of 0.06 s per point. The experimental data of the Pd(2 0 0) reflection was fitted to a Gaussian distribution using the OriginPro 9 software. In all cases, the coefficient of determination (R-square) was higher than 0.95. The center maximum and the FWHM were obtained from the adjusted peak to perform the calculations of lattice parameter and crystal size.


### 2.3. Electrochemical Characterization

The electrochemical analysis was done in a model SP-150 Biologic Science Instruments potentiostat/galvanostat controlled by a Ec-Lab Software (V10.19) and a cell of three electrodes. A saturated calomel electrode (SCE) was used as the reference electrode, while a platinum electrode was used as the counterelectrode. The working electrode consisted of a glassy carbon disc which was previously polished with alumina powder (0.05μm), then sonicated for 10 minutes, and washed with deionized water. For the electrochemical measurements, a mixture of 1.0 mg of the electrocatalyst and 73 μl of isopropyl alcohol (99%, J.T. Baker) was prepared by sonication for 20 minutes. Then, 7 μl of Nafion® solution (5% isopropyl alcohol, Sigma-Aldrich) was added to the mixture and sonicated for 20 minutes in order to obtain a homogeneous ink. 2.2 μl of the catalyst ink was placed on the working electrode. Then, it was dried using air at room temperature to obtain a thin film of catalyst. Cyclic voltammetry was carried out in an aqueous solution of 1 M KOH (98%, Sigma-Aldrich) with and without 1 M ethanol (99%, J.T. Baker). A potential window from −1 to 0.4 V (versus SCE) was scanned at 0.05 Vs−1. Chronoamperometry measurements were performed in an aqueous solution of 1 M KOH with 1 M ethanol at a potential of −0.3 V (versus SCE) for 2400 s.


## 2.1. Synthesis of PdAg Catalysts

The previously reported polyol method to obtain pure Pd-based nanobars was modified in order to obtain bimetallic nanoparticles of PdAg [14, 15]. This process is described as follows: 5 ml of ethylenglycol (EG, 99.9%, J.T. Baker) were added to a 25 ml three-necked flask coupled to a reflux system. The flask was then heated to 105°C (PdAg-a), 120°C (PdAg-b), and 135°C (PdAg-c) with constant stirring. Two solutions were prepared separately: (1) 0.0486 g of Na2PdCl4 (98%, Sigma-Aldrich) and 0.6 g of KBr (99%, Sigma-Aldrich) were dissolved in 1 ml of deionized water, and (2) 0.0916 g of PVP (99%, Sigma-Aldrich) and 0.005 g of AgNO3 (99%, Sigma-Aldrich) were added in 3 ml of EG. The solution with the Pd precursor (1) was added to the three-necked flask and, after three minutes, the silver solution (2) was incorporated. The mixture was allowed to react for 1 h at a fixed temperature. Vulcan at a ratio 20/80 Pd/C was added during the reaction; this support was preheated at 277°C for 3 h. At the end of the reaction time, the product was cooled down to room temperature. Subsequently, it was separated by centrifugation with acetone (99.9%, JT Baker) and then washed with deionized water 8 to 10 times. The speed used for the first separation was 4000 rpm, while 60000 rpm was used for rinsing. Finally, the product was dried at 100°C for 12 h.


## 2.2. Catalyst Characterization

The visualization of the synthesized nanoparticles was carried out in a JEOL Transmission Electron Microscope, model JEM-1010 equipped with a tungsten filament. It was operated with 80 kV and a magnification of 200000x. The microscope has a model ORIUS digital camera and was operated with the GATAN software. The crystallinity of the catalysts was analyzed in powder using a Rigaku Miniflex instrument. The radiation emitted by the X-ray tubes of this diffractometer corresponded to the Cu Kα (1.5406 Å). The patterns were collected from 2θ=5 to 80°, with a step of 0.02°, and a count time of 0.06 s per point. The experimental data of the Pd(2 0 0) reflection was fitted to a Gaussian distribution using the OriginPro 9 software. In all cases, the coefficient of determination (R-square) was higher than 0.95. The center maximum and the FWHM were obtained from the adjusted peak to perform the calculations of lattice parameter and crystal size.


## 2.3. Electrochemical Characterization

The electrochemical analysis was done in a model SP-150 Biologic Science Instruments potentiostat/galvanostat controlled by a Ec-Lab Software (V10.19) and a cell of three electrodes. A saturated calomel electrode (SCE) was used as the reference electrode, while a platinum electrode was used as the counterelectrode. The working electrode consisted of a glassy carbon disc which was previously polished with alumina powder (0.05μm), then sonicated for 10 minutes, and washed with deionized water. For the electrochemical measurements, a mixture of 1.0 mg of the electrocatalyst and 73 μl of isopropyl alcohol (99%, J.T. Baker) was prepared by sonication for 20 minutes. Then, 7 μl of Nafion® solution (5% isopropyl alcohol, Sigma-Aldrich) was added to the mixture and sonicated for 20 minutes in order to obtain a homogeneous ink. 2.2 μl of the catalyst ink was placed on the working electrode. Then, it was dried using air at room temperature to obtain a thin film of catalyst. Cyclic voltammetry was carried out in an aqueous solution of 1 M KOH (98%, Sigma-Aldrich) with and without 1 M ethanol (99%, J.T. Baker). A potential window from −1 to 0.4 V (versus SCE) was scanned at 0.05 Vs−1. Chronoamperometry measurements were performed in an aqueous solution of 1 M KOH with 1 M ethanol at a potential of −0.3 V (versus SCE) for 2400 s.


## 3. Results and Discussion

### 3.1. Synthesis of PdAg Catalysts

Figure1 shows the micrographs of the three synthesized catalysts. A mixture of square and spherical nanoparticles of different sizes was obtained in the three temperatures. The appearance of nanobars was expected because the technique used in this work is a modification of the one used by our work group to obtain PdAg nanobars [15]. 200 PdAg nanoparticles of both spheroidal and rectangular shapes were measured and percentage frequency was calculated. The formation of PdAg nanobars was 29.5%, 15.5%, and 17.5% for the PdAg-a, PdAg-b, and PdAg-c catalysts, respectively. The average size (width × length, nm × nm) for the PdAg-a catalyst was 5 × 15, 10 × 30 for PdAg-b, and 10 × 40 for PdAg-c. It was observed that the percentage frequency of nanobars in the three catalysts was low in comparison to other reports [15, 25, 26]. This result was associated with (a) the lower amount of water used in this work, which decreases the molding of the nanoparticle through oxidative etching and (b) the high reaction temperatures that speed up the reduction kinetics of the precursors. The combination of these conditions provides a stronger reduction environment that favors the morphological transformation from a nanobar towards a spheroidal nanoparticle [15, 25, 26]. Figure 1 also shows the spheroidal nanoparticle size distributions. A monomodal and narrow size distribution was observed for the PdAg-a and PdAg-c catalysts, while the PdAg-b catalyst displayed a bimodal and wide size distribution. The mean sizes of 6.2, 9.7, and 11.3 nm correspond to the catalysts PdAg-a, PdAg-b, and PdAg-c, respectively. This result showed that the mean particle size increased with the increase of the reduction temperature during the polyol process.Figure 1
TEM micrographs and particle size distribution for (a) PdAg-a, (b) PdAg-b, and (c) PdAd-c catalysts.
(a) (b) (c)Figure2 shows the diffractograms for the PdAg-a, PdAg-b, and PdAg-c catalysts. An XRD pattern of a Pd catalyst was also plotted as a reference. In the aforementioned pattern, the characteristic planes of Pd(1 1 1), (2 0 0), and (2 2 0) were observed at angles of 40.1, 46.6, and 68.1°, respectively (Card JCPDS 46-1043 for Pd, long dash lines). These XRD reflections are similar to those observed in the PdAg catalysts, indicating that they have a face-centered cubic structure. Additionally, reflections corresponding to AgBr (Card JCPS 06-0438 for AgBr, dotted lines) were distinguished in the PdAg-a catalyst. These reflections of impurities were due to softer reduction conditions constituted by the lower reaction temperature that does not act in favor of the reduction of the AgBr. This compound has a more negative reduction potential than the rest of the Pd and Ag species in the reaction mixture [14, 15]. Therefore, the reaction temperature used to obtain the PdAg-b (120°C) and PdAg-c (135°C) catalysts was sufficient to hinder the formation of AgBr crystals.Figure 2
XRD patterns for the catalysts and their comparison with a pure Pd catalyst.Regarding the pure Pd pattern, a slight shift towards lower angles was observed in the PdAg-a, PdAg-b, and PdAg-c catalysts. This angular shift was associated with the expansion of the palladium crystalline lattice due to the inclusion of Ag atoms with atomic radius greater than that of Pd (see lattice parameters in Table1). The angular shift is more noticeable in the zoomed in graph between 45 and 48° that shows the Pd(2 0 0) reflection. The absence of reflections in the pure-Ag angles (solid lines of the diffraction pattern) suggests that the Ag was integrated in the crystalline Pd network. This avoids the formation of silver-rich regions detectable by XRD. A gradual increase in angular displacement was observed while elevating the reaction temperature. This is indicative of a higher degree of alloying between Pd and Ag when the temperature is elevated during the polyol process. Similar angular shifts have been reported in the literature, which have been obtained by increasing the concentration of the silver precursor in the PdAg system during reduction with hydrogen gas [18].Table 1
Structural parameters obtained from XRD for the PdAg-a, PdAg-b, and PdAg-c catalysts.
Electrocatalyst Crystal size (2 0 0)(nm) Lattice parametera  (nm) Pd 7.3 0.3846 PdAg-a 6.8 0.3891 PdAg-b 7.3 0.3892 PdAg-c 7.6 0.3898The average crystal size was calculated using the Full Width at Half Maximum of the peak (2 0 0) and the Scherrer equation [18]. The results are shown in Table 1. A discrepancy between the sizes obtained by XRD and TEM techniques was observed since the TEM particle size is greater than that calculated by XRD. This difference between particle and crystal size indicates that the nanoparticles in the catalysts have a polycrystalline structure.


### 3.2. Electrochemical Characterization

Figure3 shows the voltammograms for the PdAg-a, PdAg-b, and PdAg-c catalysts in 1 M KOH at room temperature. Four regions were observed in the anodic scan (Figure 3(a)). The first region at potentials lower than −0.7 V (versus SCE) was associated with the desorption of hydrogen from the catalyst surface (region I). The second region, (II) from −0.7 to −0.2 V, was assigned to the formation of palladium hydroxides. The peaks observed in regions III and IV (−0.2 to 0.4 V) were related to the palladium and silver oxidation, respectively [14]. The inverted processes were observed in the cathodic direction: the adsorption of hydrogen appeared at potentials near −0.8 V, while the reduction of palladium oxide to Pd0 and the reduction of silver oxide (peaks III and IV) were observed at −0.34 and 0.03 V, respectively. The voltammogram in Figure 3(a) suggests that a high amount of Ag may be at the surface in the PdAg-a electrocatalyst. On the other hand, the weak signal in region IV for the PdAg-b and PdAg-c catalysts suggests that the surface of the nanoparticles is poor in Ag atoms. These results complement the observations made with XRD and indicated that Ag atoms PdAg-b and PdAg-c did not remain on the surface or in crystalline agglomerates in the form of AgBr. As a consequence, the Ag atoms were properly integrated into the Pd structure in the catalysts that were synthesized at higher temperatures.Figure 3
Cyclic voltammograms for the (a) PdAg-a, (b) PdAg-b, and (c) PdAg-c catalyst in 1 M KOH at room temperature. The solid line indicates the first cycle while the dashed line corresponds to cycle ten.
(a) (b) (c)Figure3 shows the evolution of the peaks’ intensity of the electrocatalysts during the first ten cycles. An increase in the intensity of the hydrogen adsorption-desorption, hydroxyl, and PdO reduction signals was observed on the three catalysts. However, the peaks associated with the oxidation-reduction of silver in the PdAg-a catalyst decreased during the first 10 cycles, probably due to the removal of Ag atoms from the catalyst surface. This indicated that the silver on the surface of this material has a weak anchorage with the rest of the nanoparticle.The electrochemical active surface area (ECSA) was determined by integrating the palladium oxide reduction (zone III in Figure3) and using the following formula [27]:(1)ECSA=QQref,where Q is the coulombic charge resulting from the integration of reduction peak III and Qref is the electric charge necessary for the reduction of a PdO monolayer and is equal to 405 μC cm−2 [27]. The ECSAs of the PdAg-a, PdAg-b, and PdAg-c electrocatalysts are shown in Table 2. These results were used to normalize the electric currents obtained by the cyclic voltammetry and the chronoamperometry in the presence of ethanol. A lower electroactive area was noticed in the highest temperature PdAg-c catalyst compared to the PdAg-a and PdAg-b catalysts. This result was associated with the larger particle and crystal sizes in this catalyst when compared to the others. According to XRD and TEM results, a high electroactive area would be expected in the lowest temperature catalyst (PdAg-a) due to its smaller particle and crystal sizes. However, the ECSA was the smallest of the three catalysts. This discrepancy was due to the high concentration of Ag at the surface (Figure 3), which was not considered in the ECSA calculation.Table 2
Electrochemical active surface areas for PdAg-a, PdAg-b, and PdAg-c electrocatalysts after ten cycles.
Electrocatalyst ECSA (cm2/mg) PdAg-a 33.3 PdAg-b 124 PdAg-c 17.3Cyclic voltammograms in the presence of ethanol correspond to the ethanol electrooxidation reaction. Figure4 shows the voltammogram cycles of the PdAg-a, PdAg-b, and PdAg-c electrocatalysts in 1 M ethanol + 1 M KOH solution. All voltammograms showed two characteristic peak currents: one in the anodic and the other one in the cathodic direction. In the anodic scan, the peak is associated with the oxidation of chemisorbed species derived from fresh-ethanol adsorption, while the oxidation peak in the reversed scan is related to the removal of carbon species that were not completely oxidized during the course in the positive direction. The PdAg-a catalyst (−0.18 V) showed the most negative oxidation potential, as well as a better thermodynamic performance compared to the PdAg-b (−0.12 V) and PdAg-c (−0.13 V) catalysts. This effect could be associated with the higher nanobar content in this catalyst (see TEM results) which exposes Pd(2 0 0) faces that favor the adsorption and oxidation of ethanol at low potentials [28]. In kinetic terms, it was observed that the maximum current densities for the PdAg-a, PdAg-b, and PdAg-c catalysts were 4.6, 2.6, and 12.9 mAcm−2, respectively. The current densities of the PdAg-a and PdAg-b catalysts showed low values, while the higher temperature catalyst (PdAg-c) showed the best kinetic performance. Table 3 shows the results reported for the PdAg and other representative catalytic systems for comparative purposes. A similar catalytic activity in terms of onset potential (OP) and maximum peak potential (MPP) was observed in the three catalysts in comparison to the PdAg systems in Table 3 (OP = −0.75 V versus SCE or −0.649 versus Hg/HgO 1 M NaOH; MPP = −0.079, −0.019, and −0.029 V versus Hg/HgO 1 M NaOH for PdAg-a, PdAg-b, and PdAg-c catalysts, resp.). However, the peak current for the PdAg-c catalyst is higher than practically all the catalysts presented in the table (with the exception of the PdAg nanowires).Table 3
Potential at peak maximum (PPM), onset potential (OP), and peak current density for some Pd-based catalysts reported for ethanol electrooxidation in alkaline solutions.
Catalytic system MPP (V) OP (V) Peak current density Comments Pd92Ag8  Pd79Ag21  Pd66Ag34 −0.302 (vs SCE)−0.244  −0.291 −0.8 (vs SCE)−0.8  −0.8 3.46 mA cm−2  5.17  2.44 Reaction conditions: 1.0 M NaOH + 1 M ethanol, scan rate of 20 mVs−1Catalysts synthesized by electroless deposition [19] 10%Pd-5%Ag∗ −0.09 (vs Hg/HgO) −0.65 (vs Hg/HgO) 2.5 mA Reaction conditions: 1.0 M KOH + 1 M ethanol, 50 mVs−1, 24°C.Carbon-supported catalyst synthesized by co-reduction of silver and palladium nitrate with Na3C6H5O7 + NaBH4 [17] P d 3 A g 1  ∗ −0.1 (vs Hg/HgO) −0.65 (vs Hg/HgO) 8 mA cm−2 Carbon-supported catalysts synthesized by an impregnation-reduction method using hydrogen gas at high temperature. P d 2 A g 1  ∗ −0.05 (vs Hg/HgO) −0.65 (vs Hg/HgO) 7 mA cm−2 Reaction conditions: 1 M NaOH + 1 M ethanol, 10 mVs−1 at room temperature [18] P d A g  ∗ −0.15 (vs Hg/HgO) −0.6 (vs Hg/HgO) 6 mA cm−2 Catalyst supported on Nb0.2-doped-Ti0.8O2 by polyol process.Reaction condition: 1 M KOH + 1 M ethanol, 50 mVs−1 [20] PdAg Nanotube −0.09 (vs Hg/HgO) −0.77 (vs Hg/HgO) 13.58 mA cm−2 Catalyst synthesized by polyol process and used without support.Reaction condition: 1 M KOH + 1 M ethanol, 50 mVs−1 [21]. P d 4 N i 5  ∗ −0.1 (vs Hg/HgO) 0.801 (vs Hg/HgO) 800 mAmgPd-1 Carbon-supported catalyst synthesized through a solution phase-nanocapsule method.Reaction conditions: 1 M NaOH + 1 M ethanol, 50 mVs−1, room temperature [22] Pd nanowire∗ −0.15 (vs Hg/HgO) −0.6 (vs Hg/HgO) 63 mA cm−2 Pd loading: 0.24 mg cm−2, 1M KOH, 1 M ethanol, scan rate: 50 mVs−1 [23] Pd-(Ni-Zn-P)∗ 0.9 (vs RHE) 0.35 (vs RHE) 3 mAμgPd-1 Carbon-supported catalyst.Reaction conditions: 2.0 M KOH + 10 wt% ethanol, scan rate of 50 mVs−1, room temperature [24] D a t a   ∗ obtained from its corresponding voltammogram.Figure 4
Cyclic voltammograms for the PdAg-a, PdAg-b, and PdAg-c electrocatalysts in 1 M KOH + 1 M ethanol solutions.According to Oliveira et al., there is a difference of 0.2 Å between the lattice parameter of pure Pd/C and Ag/C catalysts. They reported that the lattice parameter of Pd increases linearly with the Ag concentration in the PdAg alloy obtained by electroless method [19]. The highest electroactivity for ethanol electrooxidation was observed in the Pd79Ag21 catalyst with aPdAg = 3.925 Å, with a lattice expansion of aPdAg-aPd=Δa=0.035 Å [19]. In addition, the lineal increase of the lattice parameter with Ag concentration has also been reported by Li et al. for PdAg catalysts synthesized by impregnation-reduction with the hydrogen gas method [18]. A “volcano” behavior of the catalytic activity in terms of current density versus lattice parameter was reported, with a maximum activity when the Ag content was within 25–33%, which corresponds to a lattice expansion in the range of Δa = 0.04–0.05 Å [18]. Taking into account the fact that the concentration of Ag remained constant (at 20%) in all the syntheses performed in this study, the results showed that manipulating the reaction temperature allowed modifying the lattice expansion of PdAg catalysts during the polyol process. The lattice expansion obtained was Δa=0.045, 0.046, and 0.052 Å, for the PdAg-a, PdAg-b, and PdAg-c catalysts, respectively. Our results agree with those reported by Li and coworkers, as the higher activity and stability among the catalyst evaluated were close to the upper limit of lattice expansion (0.05 Å). This suggests that the lattice expansion of the PdAg catalyst is a critical parameter for the ethanol electrooxidation reaction.This research shows that the temperature change during the catalyst synthesis brings about a different degree of interaction between Pd and Ag, which causes modifications in the electroactivity of the catalysts. Based on thed-band center theory and the mechanism proposed by Hammer and Nørskov, deformation in the Pd-surface structure moves up the center of band d of the Pd [29]. This promotes an increase in the concentration of OH− species over the surface of the electrocatalyst that improves the elimination of ethoxyl intermediates, thus maintaining the EOR reaction [17]. Interestingly, larger particle and crystal sizes were observed in the PdAg-c catalyst, which would suggest that the reduced performance of this catalyst is related to its small electrochemical active area. However, the higher integration of the Ag atoms into the Pd network observed by VC and XRD (in the PdAg-c catalyst) indicates that the structural modification of the Pd with the presence of Ag plays an important role in carrying out the EOR in alkaline medium.Chronoamperometry tests were performed to analyze the stability of the catalysts at a potential of −0.3 V versus ECS. Figure5 shows the behavior of the current density as a function of time. A noticeable decrease in current density was observed during the first seconds in the three catalysts. Subsequently, the current density presented a gradual decrease for all the catalysts. This behavior indicated that the current density followed the Cottrell equation. According to this model, the active sites are initially free of adsorbed/oxidized ethanol molecules. As the reaction takes place, the rate of adsorption of a new ethanol molecule will depend on the availability of active sites in the catalyst. This makes the process governed by the diffusion of reagents and products. It can be observed that the catalysts produce different current densities at the start of the perturbation, where the PdAg-c catalyst holds the highest value and is followed by the PdAg-a and PdAg-b catalysts. The PdAg-b catalyst showed a faster decrease in the current density with respect to the other catalysts studied. The PdAg-c electrocatalyst maintained the highest current density (about 2.5 mA cm−2) after 240 s at −0.3 V versus ECS, indicating that this catalyst was the most stable under these reaction conditions. The PdAg-b electrocatalyst was the least stable as its current density was the lowest after the same reaction time. This indicates that the catalyst synthesized at a higher temperature is not only the most active (according to VC), but also the most stable.Figure 5
Chronoamperometry results for PdAg-a, PdAg-b, and PdAg-c electrocatalysts 1 M KOH + 1 M ethanol solutions at −0.3 V versus SCE.


## 3.1. Synthesis of PdAg Catalysts

Figure1 shows the micrographs of the three synthesized catalysts. A mixture of square and spherical nanoparticles of different sizes was obtained in the three temperatures. The appearance of nanobars was expected because the technique used in this work is a modification of the one used by our work group to obtain PdAg nanobars [15]. 200 PdAg nanoparticles of both spheroidal and rectangular shapes were measured and percentage frequency was calculated. The formation of PdAg nanobars was 29.5%, 15.5%, and 17.5% for the PdAg-a, PdAg-b, and PdAg-c catalysts, respectively. The average size (width × length, nm × nm) for the PdAg-a catalyst was 5 × 15, 10 × 30 for PdAg-b, and 10 × 40 for PdAg-c. It was observed that the percentage frequency of nanobars in the three catalysts was low in comparison to other reports [15, 25, 26]. This result was associated with (a) the lower amount of water used in this work, which decreases the molding of the nanoparticle through oxidative etching and (b) the high reaction temperatures that speed up the reduction kinetics of the precursors. The combination of these conditions provides a stronger reduction environment that favors the morphological transformation from a nanobar towards a spheroidal nanoparticle [15, 25, 26]. Figure 1 also shows the spheroidal nanoparticle size distributions. A monomodal and narrow size distribution was observed for the PdAg-a and PdAg-c catalysts, while the PdAg-b catalyst displayed a bimodal and wide size distribution. The mean sizes of 6.2, 9.7, and 11.3 nm correspond to the catalysts PdAg-a, PdAg-b, and PdAg-c, respectively. This result showed that the mean particle size increased with the increase of the reduction temperature during the polyol process.Figure 1
TEM micrographs and particle size distribution for (a) PdAg-a, (b) PdAg-b, and (c) PdAd-c catalysts.
(a) (b) (c)Figure2 shows the diffractograms for the PdAg-a, PdAg-b, and PdAg-c catalysts. An XRD pattern of a Pd catalyst was also plotted as a reference. In the aforementioned pattern, the characteristic planes of Pd(1 1 1), (2 0 0), and (2 2 0) were observed at angles of 40.1, 46.6, and 68.1°, respectively (Card JCPDS 46-1043 for Pd, long dash lines). These XRD reflections are similar to those observed in the PdAg catalysts, indicating that they have a face-centered cubic structure. Additionally, reflections corresponding to AgBr (Card JCPS 06-0438 for AgBr, dotted lines) were distinguished in the PdAg-a catalyst. These reflections of impurities were due to softer reduction conditions constituted by the lower reaction temperature that does not act in favor of the reduction of the AgBr. This compound has a more negative reduction potential than the rest of the Pd and Ag species in the reaction mixture [14, 15]. Therefore, the reaction temperature used to obtain the PdAg-b (120°C) and PdAg-c (135°C) catalysts was sufficient to hinder the formation of AgBr crystals.Figure 2
XRD patterns for the catalysts and their comparison with a pure Pd catalyst.Regarding the pure Pd pattern, a slight shift towards lower angles was observed in the PdAg-a, PdAg-b, and PdAg-c catalysts. This angular shift was associated with the expansion of the palladium crystalline lattice due to the inclusion of Ag atoms with atomic radius greater than that of Pd (see lattice parameters in Table1). The angular shift is more noticeable in the zoomed in graph between 45 and 48° that shows the Pd(2 0 0) reflection. The absence of reflections in the pure-Ag angles (solid lines of the diffraction pattern) suggests that the Ag was integrated in the crystalline Pd network. This avoids the formation of silver-rich regions detectable by XRD. A gradual increase in angular displacement was observed while elevating the reaction temperature. This is indicative of a higher degree of alloying between Pd and Ag when the temperature is elevated during the polyol process. Similar angular shifts have been reported in the literature, which have been obtained by increasing the concentration of the silver precursor in the PdAg system during reduction with hydrogen gas [18].Table 1
Structural parameters obtained from XRD for the PdAg-a, PdAg-b, and PdAg-c catalysts.
Electrocatalyst Crystal size (2 0 0)(nm) Lattice parametera  (nm) Pd 7.3 0.3846 PdAg-a 6.8 0.3891 PdAg-b 7.3 0.3892 PdAg-c 7.6 0.3898The average crystal size was calculated using the Full Width at Half Maximum of the peak (2 0 0) and the Scherrer equation [18]. The results are shown in Table 1. A discrepancy between the sizes obtained by XRD and TEM techniques was observed since the TEM particle size is greater than that calculated by XRD. This difference between particle and crystal size indicates that the nanoparticles in the catalysts have a polycrystalline structure.


## 3.2. Electrochemical Characterization

Figure3 shows the voltammograms for the PdAg-a, PdAg-b, and PdAg-c catalysts in 1 M KOH at room temperature. Four regions were observed in the anodic scan (Figure 3(a)). The first region at potentials lower than −0.7 V (versus SCE) was associated with the desorption of hydrogen from the catalyst surface (region I). The second region, (II) from −0.7 to −0.2 V, was assigned to the formation of palladium hydroxides. The peaks observed in regions III and IV (−0.2 to 0.4 V) were related to the palladium and silver oxidation, respectively [14]. The inverted processes were observed in the cathodic direction: the adsorption of hydrogen appeared at potentials near −0.8 V, while the reduction of palladium oxide to Pd0 and the reduction of silver oxide (peaks III and IV) were observed at −0.34 and 0.03 V, respectively. The voltammogram in Figure 3(a) suggests that a high amount of Ag may be at the surface in the PdAg-a electrocatalyst. On the other hand, the weak signal in region IV for the PdAg-b and PdAg-c catalysts suggests that the surface of the nanoparticles is poor in Ag atoms. These results complement the observations made with XRD and indicated that Ag atoms PdAg-b and PdAg-c did not remain on the surface or in crystalline agglomerates in the form of AgBr. As a consequence, the Ag atoms were properly integrated into the Pd structure in the catalysts that were synthesized at higher temperatures.Figure 3
Cyclic voltammograms for the (a) PdAg-a, (b) PdAg-b, and (c) PdAg-c catalyst in 1 M KOH at room temperature. The solid line indicates the first cycle while the dashed line corresponds to cycle ten.
(a) (b) (c)Figure3 shows the evolution of the peaks’ intensity of the electrocatalysts during the first ten cycles. An increase in the intensity of the hydrogen adsorption-desorption, hydroxyl, and PdO reduction signals was observed on the three catalysts. However, the peaks associated with the oxidation-reduction of silver in the PdAg-a catalyst decreased during the first 10 cycles, probably due to the removal of Ag atoms from the catalyst surface. This indicated that the silver on the surface of this material has a weak anchorage with the rest of the nanoparticle.The electrochemical active surface area (ECSA) was determined by integrating the palladium oxide reduction (zone III in Figure3) and using the following formula [27]:(1)ECSA=QQref,where Q is the coulombic charge resulting from the integration of reduction peak III and Qref is the electric charge necessary for the reduction of a PdO monolayer and is equal to 405 μC cm−2 [27]. The ECSAs of the PdAg-a, PdAg-b, and PdAg-c electrocatalysts are shown in Table 2. These results were used to normalize the electric currents obtained by the cyclic voltammetry and the chronoamperometry in the presence of ethanol. A lower electroactive area was noticed in the highest temperature PdAg-c catalyst compared to the PdAg-a and PdAg-b catalysts. This result was associated with the larger particle and crystal sizes in this catalyst when compared to the others. According to XRD and TEM results, a high electroactive area would be expected in the lowest temperature catalyst (PdAg-a) due to its smaller particle and crystal sizes. However, the ECSA was the smallest of the three catalysts. This discrepancy was due to the high concentration of Ag at the surface (Figure 3), which was not considered in the ECSA calculation.Table 2
Electrochemical active surface areas for PdAg-a, PdAg-b, and PdAg-c electrocatalysts after ten cycles.
Electrocatalyst ECSA (cm2/mg) PdAg-a 33.3 PdAg-b 124 PdAg-c 17.3Cyclic voltammograms in the presence of ethanol correspond to the ethanol electrooxidation reaction. Figure4 shows the voltammogram cycles of the PdAg-a, PdAg-b, and PdAg-c electrocatalysts in 1 M ethanol + 1 M KOH solution. All voltammograms showed two characteristic peak currents: one in the anodic and the other one in the cathodic direction. In the anodic scan, the peak is associated with the oxidation of chemisorbed species derived from fresh-ethanol adsorption, while the oxidation peak in the reversed scan is related to the removal of carbon species that were not completely oxidized during the course in the positive direction. The PdAg-a catalyst (−0.18 V) showed the most negative oxidation potential, as well as a better thermodynamic performance compared to the PdAg-b (−0.12 V) and PdAg-c (−0.13 V) catalysts. This effect could be associated with the higher nanobar content in this catalyst (see TEM results) which exposes Pd(2 0 0) faces that favor the adsorption and oxidation of ethanol at low potentials [28]. In kinetic terms, it was observed that the maximum current densities for the PdAg-a, PdAg-b, and PdAg-c catalysts were 4.6, 2.6, and 12.9 mAcm−2, respectively. The current densities of the PdAg-a and PdAg-b catalysts showed low values, while the higher temperature catalyst (PdAg-c) showed the best kinetic performance. Table 3 shows the results reported for the PdAg and other representative catalytic systems for comparative purposes. A similar catalytic activity in terms of onset potential (OP) and maximum peak potential (MPP) was observed in the three catalysts in comparison to the PdAg systems in Table 3 (OP = −0.75 V versus SCE or −0.649 versus Hg/HgO 1 M NaOH; MPP = −0.079, −0.019, and −0.029 V versus Hg/HgO 1 M NaOH for PdAg-a, PdAg-b, and PdAg-c catalysts, resp.). However, the peak current for the PdAg-c catalyst is higher than practically all the catalysts presented in the table (with the exception of the PdAg nanowires).Table 3
Potential at peak maximum (PPM), onset potential (OP), and peak current density for some Pd-based catalysts reported for ethanol electrooxidation in alkaline solutions.
Catalytic system MPP (V) OP (V) Peak current density Comments Pd92Ag8  Pd79Ag21  Pd66Ag34 −0.302 (vs SCE)−0.244  −0.291 −0.8 (vs SCE)−0.8  −0.8 3.46 mA cm−2  5.17  2.44 Reaction conditions: 1.0 M NaOH + 1 M ethanol, scan rate of 20 mVs−1Catalysts synthesized by electroless deposition [19] 10%Pd-5%Ag∗ −0.09 (vs Hg/HgO) −0.65 (vs Hg/HgO) 2.5 mA Reaction conditions: 1.0 M KOH + 1 M ethanol, 50 mVs−1, 24°C.Carbon-supported catalyst synthesized by co-reduction of silver and palladium nitrate with Na3C6H5O7 + NaBH4 [17] P d 3 A g 1  ∗ −0.1 (vs Hg/HgO) −0.65 (vs Hg/HgO) 8 mA cm−2 Carbon-supported catalysts synthesized by an impregnation-reduction method using hydrogen gas at high temperature. P d 2 A g 1  ∗ −0.05 (vs Hg/HgO) −0.65 (vs Hg/HgO) 7 mA cm−2 Reaction conditions: 1 M NaOH + 1 M ethanol, 10 mVs−1 at room temperature [18] P d A g  ∗ −0.15 (vs Hg/HgO) −0.6 (vs Hg/HgO) 6 mA cm−2 Catalyst supported on Nb0.2-doped-Ti0.8O2 by polyol process.Reaction condition: 1 M KOH + 1 M ethanol, 50 mVs−1 [20] PdAg Nanotube −0.09 (vs Hg/HgO) −0.77 (vs Hg/HgO) 13.58 mA cm−2 Catalyst synthesized by polyol process and used without support.Reaction condition: 1 M KOH + 1 M ethanol, 50 mVs−1 [21]. P d 4 N i 5  ∗ −0.1 (vs Hg/HgO) 0.801 (vs Hg/HgO) 800 mAmgPd-1 Carbon-supported catalyst synthesized through a solution phase-nanocapsule method.Reaction conditions: 1 M NaOH + 1 M ethanol, 50 mVs−1, room temperature [22] Pd nanowire∗ −0.15 (vs Hg/HgO) −0.6 (vs Hg/HgO) 63 mA cm−2 Pd loading: 0.24 mg cm−2, 1M KOH, 1 M ethanol, scan rate: 50 mVs−1 [23] Pd-(Ni-Zn-P)∗ 0.9 (vs RHE) 0.35 (vs RHE) 3 mAμgPd-1 Carbon-supported catalyst.Reaction conditions: 2.0 M KOH + 10 wt% ethanol, scan rate of 50 mVs−1, room temperature [24] D a t a   ∗ obtained from its corresponding voltammogram.Figure 4
Cyclic voltammograms for the PdAg-a, PdAg-b, and PdAg-c electrocatalysts in 1 M KOH + 1 M ethanol solutions.According to Oliveira et al., there is a difference of 0.2 Å between the lattice parameter of pure Pd/C and Ag/C catalysts. They reported that the lattice parameter of Pd increases linearly with the Ag concentration in the PdAg alloy obtained by electroless method [19]. The highest electroactivity for ethanol electrooxidation was observed in the Pd79Ag21 catalyst with aPdAg = 3.925 Å, with a lattice expansion of aPdAg-aPd=Δa=0.035 Å [19]. In addition, the lineal increase of the lattice parameter with Ag concentration has also been reported by Li et al. for PdAg catalysts synthesized by impregnation-reduction with the hydrogen gas method [18]. A “volcano” behavior of the catalytic activity in terms of current density versus lattice parameter was reported, with a maximum activity when the Ag content was within 25–33%, which corresponds to a lattice expansion in the range of Δa = 0.04–0.05 Å [18]. Taking into account the fact that the concentration of Ag remained constant (at 20%) in all the syntheses performed in this study, the results showed that manipulating the reaction temperature allowed modifying the lattice expansion of PdAg catalysts during the polyol process. The lattice expansion obtained was Δa=0.045, 0.046, and 0.052 Å, for the PdAg-a, PdAg-b, and PdAg-c catalysts, respectively. Our results agree with those reported by Li and coworkers, as the higher activity and stability among the catalyst evaluated were close to the upper limit of lattice expansion (0.05 Å). This suggests that the lattice expansion of the PdAg catalyst is a critical parameter for the ethanol electrooxidation reaction.This research shows that the temperature change during the catalyst synthesis brings about a different degree of interaction between Pd and Ag, which causes modifications in the electroactivity of the catalysts. Based on thed-band center theory and the mechanism proposed by Hammer and Nørskov, deformation in the Pd-surface structure moves up the center of band d of the Pd [29]. This promotes an increase in the concentration of OH− species over the surface of the electrocatalyst that improves the elimination of ethoxyl intermediates, thus maintaining the EOR reaction [17]. Interestingly, larger particle and crystal sizes were observed in the PdAg-c catalyst, which would suggest that the reduced performance of this catalyst is related to its small electrochemical active area. However, the higher integration of the Ag atoms into the Pd network observed by VC and XRD (in the PdAg-c catalyst) indicates that the structural modification of the Pd with the presence of Ag plays an important role in carrying out the EOR in alkaline medium.Chronoamperometry tests were performed to analyze the stability of the catalysts at a potential of −0.3 V versus ECS. Figure5 shows the behavior of the current density as a function of time. A noticeable decrease in current density was observed during the first seconds in the three catalysts. Subsequently, the current density presented a gradual decrease for all the catalysts. This behavior indicated that the current density followed the Cottrell equation. According to this model, the active sites are initially free of adsorbed/oxidized ethanol molecules. As the reaction takes place, the rate of adsorption of a new ethanol molecule will depend on the availability of active sites in the catalyst. This makes the process governed by the diffusion of reagents and products. It can be observed that the catalysts produce different current densities at the start of the perturbation, where the PdAg-c catalyst holds the highest value and is followed by the PdAg-a and PdAg-b catalysts. The PdAg-b catalyst showed a faster decrease in the current density with respect to the other catalysts studied. The PdAg-c electrocatalyst maintained the highest current density (about 2.5 mA cm−2) after 240 s at −0.3 V versus ECS, indicating that this catalyst was the most stable under these reaction conditions. The PdAg-b electrocatalyst was the least stable as its current density was the lowest after the same reaction time. This indicates that the catalyst synthesized at a higher temperature is not only the most active (according to VC), but also the most stable.Figure 5
Chronoamperometry results for PdAg-a, PdAg-b, and PdAg-c electrocatalysts 1 M KOH + 1 M ethanol solutions at −0.3 V versus SCE.


## 4. Conclusions

The ethanol electrooxidation reaction on PdAg catalysts was analyzed as a function of the reduction temperature in the polyol process. The increase of the reduction temperature favors the growth of the particle and crystal sizes due to the increase of the reduction kinetics of the precursors. The angular displacement of the diffraction pattern was greater when the reduction temperature increased. This behavior points to a high interaction between palladium and silver. The maximum current density for the PdAg-a, PdAg-b, and PdAg-c electrocatalysts was 4.6, 2.6, and 12.9 mA cm−2, respectively. The PdAg-c catalyst maintained the highest current density after 40 min at −0.3 V versus SCE. Finally, the catalyst synthesized at a higher temperature (PdAg-c) showed higher electrocatalytic activity in terms of the maximum current density, as well as a higher catalytic stability under the reaction conditions used. The improvement in catalytic performance was associated with the higher interaction between PdAg observed by XRD and cyclic voltammetry studies.



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