Next Article in Journal
Sulfonate Ionic Liquid as a Stable and Active Catalyst for Levoglucosenone Production from Saccharides via Catalytic Pyrolysis
Next Article in Special Issue
Carbon-Supported PtRuMo Electrocatalysts for Direct Alcohol Fuel Cells
Previous Article in Journal
Application of Photocatalysts and LED Light Sources in Drinking Water Treatment
Previous Article in Special Issue
Nanostructured Carbon Materials as Supports in the Preparation of Direct Methanol Fuel Cell Electrocatalysts

Catalysts 2013, 3(3), 744-756; doi:10.3390/catal3030744

Article
PtRu Nanoparticles Deposited by the Sulfite Complex Method on Highly Porous Carbon Xerogels: Effect of the Thermal Treatment
Cinthia Alegre 1, David Sebastián 1, María Elena Gálvez 2, Rafael Moliner 3, Alessandro Stassi 1, Antonino Salvatore Aricò 1, María Jesús Lázaro 3 and Vincenzo Baglio 1,*
1
Institute for Advanced Energy Technologies “Nicola Giordano”, CNR-Consiglio Nazionale della Ricerca, Vía Salita Santa Lucía sopra Contesse, 5; 98126 Messina, Italy; E-Mails: alegre@itae.cnr.it (C.A.); sebastian@itae.cnr.it (D.S.); stassi@itae.cnr.it (A.S.); arico@itae.cnr.it (A.S.A.)
2
Swiss Federal Institute of Technology, ETH Zurich, Sonneggstrasse 3; 8092 Zürich, Switzerland; E-Mail: megalvez@ethz.ch
3
Institute of Carbochemistry, CSIC-Spanish National Research Council, C/. Miguel Luesma Castán, 4, 50018 Zaragoza, Spain; E-Mails: rmoliner@icb.csic.es (R.M.); mlazaro@icb.csic.es (M.J.L.)
*
Author to whom correspondence should be addressed; E-Mail: baglio@itae.cnr.it; Tel.: +39-90-624237; Fax: +39-90-624247.
Received: 16 July 2013; in revised form: 6 September 2013 / Accepted: 10 September 2013 /
Published: 23 September 2013

Abstract

: Highly porous carbon xerogels (CXGs) were synthesized to be used as support for PtRu nanoparticles. Metal particles were deposited on CXGs by means of the sulfite complex method for the first time. Catalysts so-obtained were submitted to thermal treatment in H2, at different temperatures, in order to increase the particle size and thus the intrinsic activity. Physico-chemical characterizations included N2 physisorption, X-Ray diffraction, X-ray photoelectron spectroscopy and transmission electron microscopy. Highly dispersed alloyed PtRu particles were obtained, with crystal sizes ranging from 1.6 to 2.0 nm. PtRu-catalysts were tested in half-cell for the methanol oxidation reaction (MOR). The resulting thermal treatment was effective in increasing both particle size and catalytic activity toward MOR.
Keywords:
carbon xerogel; platinum-ruthenium catalyst; methanol oxidation reaction; sulfite complex method

1. Introduction

Pt–Ru catalysts are well known for their high activity towards the electro-oxidation of methanol [1,2,3,4,5]. Nevertheless, drawbacks such as slow oxidation kinetics and methanol crossover make the efficiency of the Direct Methanol Fuel Cells (DMFC) still insufficient for practical applications [1]. Therefore, further optimizations of the anode material and the membrane are necessary for the development and commercialization of DMFC. In this context, an attractive approach for the anode, which appears as a possible solution to reduce metal loading and increase the catalytic efficiency, is the use of novel carbonaceous materials as electrocatalyst supports [6,7,8,9]. The nature of the support, as well as the interaction between the latter and the metal, has been demonstrated to be extremely important, given that it determines the physico-chemical properties of catalysts, such as dispersion, stability and morphology of metallic crystallites [10,11,12]. In addition, characteristics of the support can also determine the electrochemical properties of catalysts by altering mass transport, active electrochemical area and metal nanoparticle stability during the cell operation [13,14].

Among the numerous new carbon materials that can be found in the literature, carbon xerogels, cryogels and aerogels constitute an interesting alternative to carbon blacks [15,16]. These materials are obtained either by supercritical drying or evaporative drying of organic gels, followed by pyrolysis. Their texture is fully controllable within a wide range of pore sizes and distribution via the synthesis process of the organic gel [14]. The use of carbon gels as catalysts supports has been previously reported. Catalysts supported on carbon gels (aerogels, cryogels and xerogels) showed higher activities towards methanol oxidation and oxygen reduction, in comparison to catalysts supported on commercial carbon blacks, such as Vulcan [12,15,16,17,18]. Vulcan XC-72R, with a surface area of ca. 250 m2 g−1, has been commonly used as a catalyst support, especially in DMFC anode catalyst preparation. However, an accessible and sufficiently large surface for maximum catalyst dispersion has been argued to be a necessary but insufficient condition for obtaining optimized carbon-supported catalysts. First of all, Vulcan has a preponderance of small pores that cannot be filled with polymer molecules. This portion inside the micropores has less or even no electrochemical activity due to the difficulty in reactant accessibility. Besides, the poor surface chemistry of this carbon material makes its impregnation with the metallic precursor difficult.

Some studies have dealt with different preparation methods of catalysts onto this kind of supports. Arbizzani et al. developed PtRu catalysts, prepared by both chemical and electrochemical routes, on mesoporous cryo- and xerogel carbons [18]. Their results were compared to those obtained with Vulcan-supported PtRu, resulting in almost double specific catalytic activity when Vulcan was substituted by the former carbons. Job et al. reported the use of the ‘Strong Electrostatic Adsorption’ (SEA) method to prepare Pt/carbon xerogel catalysts, exhibiting high Pt dispersion at high metal content [15]. Figueiredo et al. prepared Pt catalysts supported on carbon xerogels by impregnation with H2PtCl6, studying the effect of different reduction protocols [12].

Carbon xerogels have also been employed as catalyst supports in previous studies of our group [19,20,21]. Carbon xerogels were used as support for Pt and PtRu nanoparticles, synthesized by an impregnation and reduction with sodium borohydride method. Catalysts performed higher activities than commercial catalysts Pt/C, ETEK and PtRu/C, ETEK, that are supported on Vulcan carbon black [19]. In another paper, we reported the synthesis of two carbon xerogels of different textural properties, which were subsequently functionalized through several oxidation treatments. These carbon xerogels were used as supports in the preparation of several Pt catalysts which were characterized and tested for CO and methanol electro-oxidation, performing higher activities than Pt supported on Vulcan [20]. In another work, PtRu catalysts were prepared using a highly mesoporous carbon xerogel submitted to different oxygen functionalization treatments: diluted and concentrated nitric acid as well as gas-phase 5% O2−N2 oxidation. Catalysts with 20 wt% loading and equimolar Pt:Ru metallic phase were prepared using an impregnation procedure involving chemical reduction with formic acid. Catalysts supported on the carbon xerogel presented higher activities towards methanol oxidation than the catalyst supported on Vulcan prepared by the same procedure [21]. In comparison to the commercial carbon black Vulcan, carbon xerogel doubles the SBET value determined for Vulcan. Such features favour diffusion of reagents and products to and from active sites when using carbon xerogels as catalysts supports, instead of Vulcan, making catalysts more active. Although catalysts supported on carbon xerogels showed higher performances than when supported on Vulcan, not proper dispersion was achieved in these works for any of the methods assayed (impregnation and reduction with different reduction protocols), pointing out the need for further research in synthesis methods providing low crystallite size and high metallic dispersion.

In general, the Pt/carbon gel catalysts are classically obtained via deposition from the liquid phase; in most cases, impregnation of the support by H2PtCl6 solutions is used and followed by various post-treatments, such as liquid phase reduction or drying followed by gas phase reduction under hydrogen [15]. Nevertheless, it has been noticed that the presence of chloride ions during the deposition can have a negative effect on the later performance of the catalysts for methanol oxidation [15]. In this paper a sulfite-complex based method is used for the first time for carbon xerogels, in order to avoid the use of chloride species. This preparation method presents an advantage over the straight reduction of chloride salts since no chloride ions are present during the deposition of the metals onto the support. Further, given that this method leads to small metallic particles, with a high dispersion, two thermal treatments at different temperatures were carried out, in order to slightly increase crystal and particle size, favoring catalytic activity towards methanol oxidation reaction (MOR).

2. Results and Discussion

2.1. Textural Properties of Carbon Xerogels and PtRu-Catalysts

Carbon xerogel (CXG) was synthesized by a sol-gel method consisting on the polymerization and pyrolysis of resorcinol and formaldehyde. Subsequently, this carbon material was used as support for PtRu nanoparticles deposited by a sulfite complex method, based on the formation of colloids. PtRu metallic loading was calculated to obtain a 20 wt.% on the carbon support. Catalysts so obtained were divided in three aliquots: one as-prepared and the other two were treated under a H2 stream for 1 h at 200 °C and 400 °C, respectively.

Carbon xerogel shows a high surface area (see Table 1), and can be mainly considered as a mesoporous carbon, with 89% of its pore volume corresponding to mesopores, and average pore sizes of 23 nm. Textural properties of PtRu catalysts are also shown in Table 1. Catalysts were named as follows: PtRu/CXG-COL (given that the sulfite complex method is based on colloids), followed by TT-200 or TT-400 (standing for thermal treatment at 200 °C or 400 °C, respectively). Upon metallic loading, surface area and pore volume decrease considerably, but still carbon materials conserve a highly developed porous structure. Note that mean pore size slightly decreases after metallic introduction but there is no significant selectivity regarding the deposition on micropores nor mesopores, indicating the presence of PtRu nanoparticles all over the CXG surface. It is also worthy of note that the porosity increases with thermal treatment in terms of both Brunauer-Emmet-Teller (BET) surface area and pore volume, maybe attributable to some carbon gasification from the CXG.

Table Table 1. Brunauer-Emmet-Teller (BET) surface area and pore volumes obtained from N2 adsorption isotherms for the carbon xerogel and the PtRu-catalysts prepared.

Click here to display table

Table 1. Brunauer-Emmet-Teller (BET) surface area and pore volumes obtained from N2 adsorption isotherms for the carbon xerogel and the PtRu-catalysts prepared.
SampleSBET (m2 g−1)Vpore p/p0 ≈ 1 (cm3 g−1)Vmeso BJH (cm3 g−1)Vmicro (cm3 g−1)Mean pore size (nm)
CXG5281.791.660.1423
PtRu/CXG-COL2710.510.590.0819
PtRu/CXG-COL-TT2002780.570.460.0918
PtRu/CXG-COL-TT4003320.660.550.1118

2.2. PtRu-Catalysts Characterization

PtRu crystal sizes, shown in Table 2, were calculated from the XRD patterns (shown in Figure 1) and using the Debye-Scherrer equation on the Pt (220) reflection. PtRu crystal size ranges from 1.6 to 2.0 nm.

Table Table 2. PtRu crystal size obtained by XRD and PtRu concentration in the synthesized catalysts.

Click here to display table

Table 2. PtRu crystal size obtained by XRD and PtRu concentration in the synthesized catalysts.
Sample% w/w PtRuAtomic ratio Pt:RuPtRu crystal sizeLattice parameterXRu in PtRu alloy
TGAXRFnmnmVegard’s lawAntolini’s equation [22]
PtRu/CXG-COL251.61.60.3860.350.49
PtRu/CXG-COLTT200251.61.80.3870.390.37
PtRu/CXG-COLTT400251.62.00.3850.430.50

The highly developed surface area of these carbon materials is the controlling parameter determining such a low crystal size. Thermal treatment proved to be effective in increasing the catalysts crystal size. The amount of Ru alloyed with Pt ranges from 0.35 to 0. 43 when calculated using Vegard’s law, and slightly higher when using Antolini`s equation [22]. Antolini and co-workers [22] obtained similar values of XRu, however, a little smaller. The higher XRu in the alloy in comparison to Antolini’s work, might be due to the small crystal size, favoring inclusion of Ru in the fcc structure of Pt. This is confirmed by the lattice parameter that decreases from 0.392 nm (from pure Pt) to ca. 0.385 due to the contraction of the lattice, indicating the formation of the alloy between Pt and Ru. In the case of PtRu/CXG-COL-TT200 and PtRu/CXG-COL-TT400 catalysts, it is possible that H2 treatment favored the further inclusion of Ru in the fcc network. The metallic loading was slightly higher than the nominal 20 wt.% in all cases. X-ray fluorescence analysis yields similar to Pt/Ru ratios for all catalysts prepared.

Catalysts 03 00744 g001 1024
Figure 1. Diffractograms obtained by XRD for the synthesized PtRu catalysts.

Click here to enlarge figure

Figure 1. Diffractograms obtained by XRD for the synthesized PtRu catalysts.
Catalysts 03 00744 g001 1024

TEM images, shown in Figure 2, were acquired for PtRu catalysts in order to analyze the metal dispersion obtained. A uniform distribution of the active phase is obtained in all cases. The remarkably enhanced dispersion of the metal compounds achieved through this sulfite complex method lead us to conclude that, in terms of active phase dispersion, the surface of the carbon support is optimally covered by the metallic particles. Histograms obtained confirmed the results obtained from XRD. Catalysts submitted to subsequent thermal treatment produced larger particle sizes (around 2.4 nm and 3.1 nm for PtRu/CXG-COL-TT200 and PtRu/CXG-COL-TT400, respectively) as a consequence of the intended metallic particle sintering to a certain extent, in comparison to the untreated catalyst, PtRu/CXG-COL, with a particle size distribution centered at 1.9 nm.

Catalysts 03 00744 g002 1024
Figure 2. Representative TEM micrographs of the PtRu electrocatalysts (a) PtRu/CXG-COL; (b) PtRu/CXG-COL-TT200 and (c) PtRu/CXG-COL-TT400.

Click here to enlarge figure

Figure 2. Representative TEM micrographs of the PtRu electrocatalysts (a) PtRu/CXG-COL; (b) PtRu/CXG-COL-TT200 and (c) PtRu/CXG-COL-TT400.
Catalysts 03 00744 g002 1024

XPS was used to identify the oxidation state of Pt and Ru on the surface of the different catalysts prepared. Pt and Ru peaks were deconvoluted as described in [23]. Figure 3 shows an example of the deconvolution of Pt 4f7/2 and Ru 3p3/2 signals for the catalyst PtRu/CXG-COL, whereas Table 3 shows the results of this deconvolution.

Catalysts 03 00744 g003 1024
Figure 3. XPS signals for (a) Pt and (b) Ru for the catalyst PtRu/CXG-COL.

Click here to enlarge figure

Figure 3. XPS signals for (a) Pt and (b) Ru for the catalyst PtRu/CXG-COL.
Catalysts 03 00744 g003 1024

For all the catalysts studied, Pt0 was found to be the predominant species on their surface. There is, however, an important contribution of oxidized Pt2+, as well as of Pt4+, to a lower extent. In contrast, RuO2 is the predominant species in all catalysts, followed by Ru0. Catalysts submitted to thermal treatment in reducing atmosphere present higher amounts of reduced metals, as expected, increasing with treatment temperature. Pt/Ru atomic ratios determined by XPS are similar, and in all cases superior, to the values obtained by XRF, showing a surface particularly enriched in Pt.

Table Table 3. Binding energies of the Pt 4f7/2 and Ru 3p3/2 signals for catalysts prepared, determined by XPS.

Click here to display table

Table 3. Binding energies of the Pt 4f7/2 and Ru 3p3/2 signals for catalysts prepared, determined by XPS.
SamplePt 4f7/2Ru 3p3/2Pt/Ru
SpeciesIntensity (%)SpeciesIntensity (%)
PtRu/CXG- COLPt46.8Ru34.62.2
PtO44.7RuO253.0
PtO28.5RuO2·xH2O12.4
PtRu/CXG-COL-TT200Pt54.2Ru38.22.2
PtO36.6RuO250.2
PtO29.2RuO2·xH2O11.6
PtRu/CXG-COL-TT400Pt63.9Ru48.11.9
PtO21.1RuO244
PtO215RuO2·xH2O7.9

2.3. Catalytic Activity towards MOR

Electrochemical surface areas were determined by CO stripping for the three catalysts under study, as shown in Table 4.

Table Table 4. Electrochemical active surface area (ECSA) for PtRu catalysts, determined by CO stripping.

Click here to display table

Table 4. Electrochemical active surface area (ECSA) for PtRu catalysts, determined by CO stripping.
SampleECSA/m2·g−1 PtRu
PtRu/CXG-COL56.9
PtRu/CXG-COLTT20035.9
PtRu/CXG-COLTT40030.4

ECSA decreases when catalysts are submitted to thermal treatment, due to the increase in the particle size and the agglomeration of the metallic particles.

Methanol electro-oxidation polarization curves, obtained at room temperature, are shown in Figure 4. PtRu/CXG-COL-TT400 presents the highest mass activity towards methanol oxidation, as a result of its higher crystal size and amount of reduced metals, Pt0 and Ru0. It is clear that crystal/particle size has a huge influence on the electrocatalytic activity. Methanol electro-oxidation is in fact a structure-sensitive process. Several studies point to a loss of effective surface area as particle size increases, resulting in lower catalytic activity. However, other authors state that there is an optimal particle size for achieving maximal catalytic activity, in a certain system. Frelink et al. [24] evaluated different Pt/Vulcan carbon black supported catalysts prepared through different methods and stated that for Pt particle sizes (determined by TEM) in the range 1.2–4.5 nm, a decrease in size resulted in a decrease in methanol oxidation activity, whereas for sizes larger than 4.5 nm, the methanol oxidation activity remained almost constant. They explained this fact in terms of a high affinity towards oxygen of very small particles, resulting in a largely covered Pt-OH surface which left insufficient sites for methanol adsorption. Even if it is also true that higher particle sizes may offer a higher amount of exposed crystal active phases—(111) planes have been claimed to be the most active [25]—differences in catalytic activity towards methanol oxidation may not only be related to the effect of particle size, but also to surface chemistry in the different catalytic systems [26]. Pt and Ru oxidation state can strongly determine the catalytic activity. In fact, Garcia and co-workers [26] proved that the presence of Pt and Ru oxides do not permit the dehydrogenation step, i.e., breaking of C–H bonds, in the molecule of methanol.

The results of chronoamperometric tests of methanol oxidation are shown in Figure 5. The results at constant 0.60 V vs. RHE follow the same trend as the one observed in the methanol oxidation polarization curves. The catalyst PtRu/CXG-COL-TT400 shows the highest catalytic activity, followed by the catalyst PtRu/CXG-COL-TT200 and PtRu/CXG-COL; this is, in increasing order of PtRu particle size. Taking into account the decrease of electrochemical surface area from both the increase of PtRu particle size and the slight degree of agglomeration, the increase of MOR activity is attributed to the better intrinsic activity of the biggest particles, in this study 2.0 nm according to XRD and 3.1 nm according to TEM analysis [26].

Catalysts 03 00744 g004 1024
Figure 4. Polarization curves for the electro-oxidation of methanol in a 2 M CH3OH + 0.5 M H2SO4 solution at room temperature for the PtRu carbon-supported catalysts. Scan rate = 0.02 V s−1.

Click here to enlarge figure

Figure 4. Polarization curves for the electro-oxidation of methanol in a 2 M CH3OH + 0.5 M H2SO4 solution at room temperature for the PtRu carbon-supported catalysts. Scan rate = 0.02 V s−1.
Catalysts 03 00744 g004 1024
Catalysts 03 00744 g005 1024
Figure 5. Current density vs. time curves recorded in a 2 M CH3OH + 0.5 M H2SO4 solution at room temperature for the PtRu carbon-supported catalysts at E = 0.60 V vs. RHE.

Click here to enlarge figure

Figure 5. Current density vs. time curves recorded in a 2 M CH3OH + 0.5 M H2SO4 solution at room temperature for the PtRu carbon-supported catalysts at E = 0.60 V vs. RHE.
Catalysts 03 00744 g005 1024

3. Experimental Section

3.1. Carbon Xerogel Synthesis

CXG was synthesized as described in [27] by the pyrolysis at 800 °C of an organic gel obtained by the polycondensation of resorcinol and formaldehyde in stoichiometric ratio (2 mol of formaldehyde per mol of resorcinol). The gelation and curing process took place at an initial pH of 6.0 and using sodium carbonate as catalyst (0.04 mol% with respect to total content of resorcinol + formaldehyde). Curing of the organic gel was carried out for 24 h at room temperature, 24 h at 50 °C and 120 h at 85 °C. Subsequently, remaining water was exchanged with acetone and the gel was dried under subcritical conditions before its pyrolysis. Pyrolysis took place at 800 °C under a nitrogen atmosphere for 3 h.

3.2. Catalysts Preparation

PtRu nanoparticles were deposited on the synthesized carbon xerogels by the sulfite complex method (a type of colloidal method) never reported before for carbon xerogels. A 20 wt.% nominal metal concentration on CXGs was chosen. Sulfite complexes of Pt and Ru, in appropriate amounts, were decomposed by hydrogen peroxide to form aqueous colloidal solutions of Pt-Ru oxides. These particles were adsorbed on CXGs. The amorphous oxides on CXGs were thus reduced in a hydrogen stream to form metallic particles. The reduction process was considered complete when no significant H2 consumption was detected in the outlet stream by using a thermal conductive detector (TCD). Two aliquots of this catalyst were further treated in hydrogen atmosphere at 200 °C and 400 °C for 1 h, with the aim of evaluating the effect of this thermal and reducing treatment in the features of the catalysts, mostly in terms of increased metallic crystal size. These catalysts were named PtRu/CXG-COL-TT200 and PtRu/CXG-COL-TT400, respectively.

3.3. Physico-Chemical Characterization

The textural and morphological features of the different carbon supports and catalysts prepared were determined by means of nitrogen physisorption at −196 °C (Micromeritics ASAP 2020). Textural properties such as specific surface area, pore volume and pore size distribution were calculated from each corresponding nitrogen adsorption-desorption isotherms applying the Brunauer-Emmet-Teller (BET) equation, Barrett-Joyner-Halenda (BJH) and t-plot methods. Thermogravimetric complete oxidation in air of both the carbon support and PtRu catalysts was used to determine the total amount of metal deposited, in a Setaram Setsys evolution thermogravimetric analyzer at atmospheric pressure, with a temperature program from room temperature to 950 °C with a constant rate of 5 °C min−1. X-ray fluorescence (XRF) measurements were also used to determine the Pt:Ru atomic ratio, by using a Bruker AXS S4 Explorer spectrometer. Catalysts were as well characterized by X-Ray Diffraction (XRD), using a Bruker AXS D8 Advance diffractometer, with a θ-θ configuration and using Cu-Kα radiation. Crystallite sizes were calculated from the Scherrer’s equation on the (220) peak for platinum. X-ray photoelectron spectrometry (XPS) analysis were performed using a ESCAPlus Omicron spectrometer equipped with a Mg (1253.6 eV) anode, 150 W (15 mA, 10 kV) power, over an area of sample of 1.75 × 2.75 mm. C 1s (280–295 eV), O 1s (526–540 eV) and Pt 4f (65–84 eV) signals were obtained at 0.1 eV step, 0.5 s dwell and 20 eV pass energy. Spectra were deconvoluted using CasaXPS software. Particle sizes were evaluated from TEM images obtained in a JEOL 2100F microscope operated with an accelerating voltage of 200 kV and equipped with a field emission electron gun providing a point resolution of 0.19 nm. The standard procedure involved dispersing 3 mg of the sample in ethanol in an ultrasonic bath for 15 min. The sample was then placed in a Cu carbon grid where the liquid phase was evaporated.

3.4. Electrochemical Experiments

A cell with a three-electrode assembly and an AUTOLAB potentiostat-galvanostat were used to carry out the electrochemical characterization. The counter electrode consisted on a pyrolytic graphite rod, while the reference electrode was a reversible hydrogen electrode (RHE). Therefore, all potentials in the text are referred to the latter. The working electrode consisted of a pyrolytic graphite disk (7 mm) with a thin layer of the electrocatalyst under study deposited onto it. For the preparation of this layer, an aqueous suspension consisting of 3.6 mg of PtRu/CXG catalyst was obtained by ultrasonically dispersing it in Nafion solution 10% w/w (Sigma-Aldrich, St. Louis, MO, USA) (14.7 μL) and a mixture of ultrapure water (240 μL) (Millipore) and ethanol (240 μL) (Merck). Subsequently an aliquot of 40 μL of the dispersed suspension was deposited on top of the graphite disk and dried under inert atmosphere prior its use.

Polarization curves were performed to study the electro-oxidation of methanol, in a 2 M CH3OH + 0.5 M H2SO4 solution, at scan rate of 20 mV·s−1, between 0.05 and 0.8 V vs. RHE. Chronoamperometries were performed at 0.60 V vs. RHE in a 2 M CH3OH + 0.5 M H2SO4 solution, in order to evaluate the evolution of the electrocatalytic activity with time of the prepared catalysts in the electro-oxidation of methanol. All the experiments were carried out at room temperature, and current was normalized with respect to each catalyst metal amount (A/g PtRu).

4. Conclusions

PtRu nanoparticles were deposited on a highly mesoporous carbon xerogel for the first time by a sulfite complex method. Thermal treatments at 200 °C and 400 °C in H2 for 1 h were carried out, in order to increase the crystal size. This sulfite complex method led to catalysts with low crystal sizes (from 1.6 to 2.0 nm). Thermal treatment proved to be effective increasing the catalysts crystal size and the extent of metallic phase reduction.

It was observed, by means of XRF and XPS, that Pt segregated towards the surface of the metallic crystallites deposited on the carbon xerogel.

A certain extent of pore blockage was observed upon the loading of the active phase, but catalysts still maintained the initial mesopore-enriched structure of the carbon xerogel.

Methanol electro-oxidation was found to be dependent mainly on the crystal size and the extent of reduced metals (Pt0 and Ru0) on the composition of the catalyst. The most active catalysts were those treated at 400 °C, PtRu/CXG-COL-TT400, with the highest crystal size and the highest amount of reduced metals. The high segregation extent of Pt towards the surface of the particles/crystallites deposited, on the surface of the carbon xerogel, may have resulted in an optimal combination of Pt and Ru atoms enhancing the progress of the different controlling steps of methanol electro-oxidation mechanism at room temperature; starting from methanol dehydrogenation and completing the oxidation of the intermediate COads species by means of nearby OHads on Ru sites.

Acknowledgments

The authors wish to thank the Spanish Ministry of Economy and Competitiveness (Secretaría de Estado de I+D+I) and FEDER for financial support under the project CTQ2011-28913-C02-01. Authors also thank the financial support of the bilateral CNR (Italy)—CSIC (Spain) joint agreement 2011–2012 (project Baglio/Lazaro 2010IT0026). CNR-ITAE authors acknowledge the financial support of PRIN 2010-11 project “Advanced nanocomposite membranes and innovative electrocatalysts for durable polymer electrolyte membrane fuel cells (NAMED-PEM)”.

Conflicts of Interest

The authors declare no conflict of interest.

References

  1. Aricó, A.S.; Baglio, V.; Antonucci, V. Direct Methanol Fuel Cells; Nova Publishers: New York, NY, USA, 2010. [Google Scholar]
  2. Antolini, E. Effect of the Structural Characteristics of Binary Pt–Ru and Ternary Pt–Ru–M Fuel Cell Catalysts on the Activity of Ethanol Electrooxidation in Acid Medium. ChemSusChem. [CrossRef]
  3. Petrii, O.A. Pt-Ru electrocatalysts for fuel cells: A representative review. J. Solid State Electrochem. 2008, 12, 609–642. [Google Scholar] [CrossRef]
  4. Antolini, E. Formation of carbon-supported PtM alloys for low temperature fuel cells: A review. Mater. Chem. Phys. 2003, 78, 563–573. [Google Scholar] [CrossRef]
  5. Viva, F.A.; Bruno, M.M.; Jobbagy, M.; Corti, H.R. Electrochemical Characterization of PtRu Nanoparticles Supported on Mesoporous Carbon for Methanol Electrooxidation. J. Phys. Chem. C 2012, 116, 4097–4104. [Google Scholar]
  6. Sharma, S.; Pollet, B.G. Support materials for PEMFC and DMFC electrocatalysts—A review. J. Power Sources 2012, 208, 96–119. [Google Scholar] [CrossRef]
  7. Monteverde Videla, A.H.A.; Zhang, L.; Kim, J.; Zeng, J.; Francia, C.; Zhang, J.; Specchia, S. Mesoporous carbons supported non-noble metal Fe-N X electrocatalysts for PEM fuel cell oxygen reduction reaction. J. Appl. Electrochem. 2013, 43, 159–169. [Google Scholar] [CrossRef]
  8. Baglio, V.; di Blasi, A.; D’Urso, C.; Antonucci, V.; Aricò, A.S.; Ornelas, R.; Morales-Acosta, D.; Ledesma-Garcia, J.; Godinez, L.A.; Arriaga, L.G.; et al. Development of Pt and Pt -Fe Catalysts Supported on Multiwalled Carbon Nanotubes for Oxygen Reduction in Direct Methanol Fuel Cells. J. Electrochem. Soc. 2008, 155, B829–B833. [Google Scholar] [CrossRef]
  9. Park, S.J.; Kim, B.J.; Lee, S.Y. Effect of surface modification of mesoporous carbon supports on the electrochemical activity of fuel cells. J. Colloid Interface Sci. 2013, 405, 150–156. [Google Scholar] [CrossRef]
  10. Cui, Z.; Liu, C.; Liao, J.; Xing, W. Highly active PtRu catalysts supported on carbon nanotubes prepared by modified impregnation method for methanol electro-oxidation. Electrochim. Acta 2008, 53, 7807–7811. [Google Scholar] [CrossRef]
  11. Zhou, W.J.; Li, W.Z.; Song, S.Q.; Zhou, Z.H.; Jiang, L.H.; Sun, G.Q.; Xin, Q.; Poulianitis, K.; Kontou, S.; Tsiakaras, P. Bi- and tri-metallic Pt-based anode catalysts for direct ethanol fuel cells. J. Power Sources 2004, 131, 217–223. [Google Scholar] [CrossRef]
  12. Figueiredo, J.L.; Pereira, M.F.R.; Serp, P.; Kalck, P.; Samant, P.V.; Fernandes, J.B. Development of carbon nanotube and carbon xerogel supported catalysts for the electro-oxidation of methanol in fuel cells. Carbon 2006, 44, 2516–2522. [Google Scholar] [CrossRef]
  13. Yu, X.; Ye, S. Recent advances in activity and durability enhancement of Pt/C catalytic cathode in PEMFC: Part I. Physico-chemical and electronic interaction between Pt and carbon support, and activity enhancement of Pt/C catalyst. J. Power Sources 2007, 172, 133–144. [Google Scholar] [CrossRef]
  14. Kim, M.; Park, J.N.; Kim, H.; Song, S.; Lee, W.H. The preparation of Pt/C catalysts using various carbon materials for the cathode of PEMFC. J. Power Sources 2006, 163, 93–97. [Google Scholar] [CrossRef]
  15. Job, N.; Chatenet, M.; Berthon-Fabry, S.; Hermans, S.; Maillard, F. Efficient Pt/carbon electrocatalysts for proton exchange membrane fuel cells: Avoid chloride-based Pt salts! J. Power Sources 2013, 240, 294–305. [Google Scholar] [CrossRef]
  16. Arbizzani, C.; Beninati, S.; Soavi, F.; Varzi, A.; Mastragostino, M. Supported PtRu on mesoporous carbons for direct methanol fuel cells. J. Power Sources 2008, 185, 615–620. [Google Scholar] [CrossRef]
  17. Job, N.; Lambert, S.; Chatenet, M.; Gommes, C.J.; Maillard, F.; Berthon-Fabry, S.; Regalbuto, J.R.; Pirard, J.P. Preparation of highly loaded Pt/carbon xerogel catalysts for Proton Exchange Membrane fuel cells by the Strong Electrostatic Adsorption method. Catal. Today 2010, 150, 119–127. [Google Scholar] [CrossRef]
  18. Arbizzani, C.; Beninati, S.; Manferrari, E.; Soavi, F.; Mastragostino, M. Electrodeposited PtRu on cryogel carbon–Nafion supports for DMFC anode. J. Power Sources 2006, 161, 826–830. [Google Scholar] [CrossRef]
  19. Alegre, C.; Calvillo, L.; Moliner, R.; González-Expósito, J.A.; Guillén-Villafuerte, O.; Huerta, M.V.M.; Pastor, E.; Lázaro, M.J. Pt and PtRu electrocatalysts supported on carbon xerogels for direct methanol fuel cells. J. Power Sources 2011, 196, 4226–4235. [Google Scholar] [CrossRef]
  20. Alegre, C.; Gálvez, M.E.; Baquedano, E.; Pastor, E.; Moliner, R.; Lázaro, M.J. Influence of support’s oxygen functionalization on the activity of Pt/carbon xerogels catalysts for methanol electro-oxidation. Int. J. Hydrogen Energy 2012, 37, 7180–7191. [Google Scholar]
  21. Alegre, C.; Gálvez, M.E.; Baquedano, E.; Moliner, R.; Pastor, E.; Lázaro, M.J. Oxygen-Functionalized Highly Mesoporous Carbon Xerogel Based Catalysts for Direct Methanol Fuel Cell Anodes. J. Phys. Chem. C 2013, 117, 13045–13058. [Google Scholar]
  22. Antolini, E.; Cardellini, F. Formation of carbon supported PtRu alloys: An XRD analysis. J. Alloys Compd. 2001, 315, 118–122. [Google Scholar] [CrossRef]
  23. De la Fuente, J.L.G.; Martínez-Huerta, M.V.; Rojas, S.; Fierro, J.L.G.; Peña, M.A. Methanol electrooxidation on PtRu nanoparticles supported on functionalised carbon black. Catal. Today 2006, 116, 422–432. [Google Scholar] [CrossRef]
  24. Frelink, T.; Visscher, W.; van Veen, J.A.R. Particle size effect of carbon-supported platinum catalysts for the electrooxidation of methanol. J. Electroanal. Chem. 1995, 382, 65–72. [Google Scholar] [CrossRef]
  25. Chrzanowski, W.; Wieckowski, A. Surface Structure Effects in Platinum/Ruthenium Methanol Oxidation Electrocatalysis. Langmuir 1998, 14, 1967–1970. [Google Scholar] [CrossRef]
  26. Garcia, G.; Baglio, V.; Stassi, A.; Pastor, E.; Antonucci, V.; Aricò, A.S. Investigation of Pt–Ru nanoparticle catalysts for low temperature methanol electro-oxidation. J. Solid State Electrochem. 2007, 11, 1229–1238. [Google Scholar] [CrossRef]
  27. Alegre, C.; Sebastián, D.; Baquedano, E.; Gálvez, M.E.; Moliner, R.; Lázaro, M.J. Tailoring Synthesis Conditions of Carbon Xerogels towards Their Utilization as Pt-Catalyst Supports for Oxygen Reduction Reaction (ORR). Catalysts 2012, 2, 466–489. [Google Scholar] [CrossRef]
Catalysts EISSN 2073-4344 Published by MDPI AG, Basel, Switzerland RSS E-Mail Table of Contents Alert