Influence of the Synthesis Method for Pt Catalysts Supported on Highly Mesoporous Carbon Xerogel and Vulcan Carbon Black on the Electro-Oxidation of Methanol

Abstract

Platinum catalysts supported on carbon xerogel and carbon black (Vulcan) were synthesized with the aim of investigating the influence of the characteristics of the support on the electrochemical performance of the catalysts. Three synthesis methods were compared: an impregnation method with two different reducing agents, sodium borohydride and formic acid, and a microemulsion method, in order to study the effect of the synthesis method on the physico-chemical properties of the catalysts. X-ray diffraction and transmission electron microscopy were applied. Cyclic voltammetry and chronoamperometry were used for studying carbon monoxide and methanol oxidation. Catalysts supported on carbon xerogel presented higher catalytic activities towards CO and CH₃OH oxidation than catalysts supported on Vulcan. The higher mesoporosity of carbon xerogel was responsible for the favored diffusion of reagents towards catalytic centers.

1. Introduction

Carbon materials such as charcoals, activated carbons, carbon blacks and graphite have been widely used as support in the synthesis of catalysts with important applications in the chemical industry [1]. The properties of such supports, as well as their porous structure and surface chemistry, influence the dispersion and stability of the metal employed as active phase, determining the activity of the catalyst [2,3].

In the field of fuel cells, electrocatalysts are responsible for the oxidation of the fuel (hydrogen, methanol, etc.) at the anode, and the reduction of oxygen at the cathode, thus generating electrical power. In PEMFC the catalysts are usually based on Pt and supported on carbon black with high surface area. In the last few decades, growing literature has appeared concerning new carbon supports such as carbon nanotubes [3], carbon nanofibers [4], ordered mesoporous carbons and carbon xerogels and aerogels [2,5,6]. These materials could lead to the production of more stable and highly active catalysts, with low platinum loadings (<0.1 mg·cm⁻²) and therefore low cost [7].

Direct methanol fuel cells (DMFCs) are very promising for portable devices [2], given the ease of use of a liquid fuel, which is easily storable and transportable. However the commercialization of DMFCs is still hindered by some technical challenges, mainly: (1) slow kinetics of both the oxygen reduction and the methanol oxidation and (2) methanol crossover [2]. For these reasons, improved catalysts are required. Research is mainly focusing on (i) the development of new catalyst syntheses taking into account alloy composition, nanometric dimensions and uniform distribution of the catalyst and (ii) the development of new carbon supports with high electric conductivity, high surface area and high mesoporosity in the pore size range of 20–40 nm [5].

Carbon gels are materials with interesting properties to be used as electrocatalyst supports in fuel cells (FC). Carbon xerogels in particular are attracting much attention for their unique and controllable properties (high surface area and mesoporosity with narrow pore size distribution as well as high purity (>99.5% C)) which, in turn, are attributed to the mechanism reaction, being similar to the sol-gel process [8].

In a previous work [9], Pt and PtRu catalysts supported on carbon xerogels (CXGs) were synthesized. Carbon supports presented high surface area and pore volume values, 577 m²·g⁻¹ and 1.82 cm³·g⁻¹ respectively, with pore size equal to 7.1 nm. Pt/CXG and PtRu/CXG catalysts presented higher catalytic activities than commercial ones, namely Pt/C and PtRu/C from E-TEK. The present work involves the synthesis of a carbon xerogel with improved properties (higher surface area, 660 m²·g⁻¹ and larger pore size, 23 nm), to be used as Pt support. In order to compare the results obtained, Pt nanoparticles were also deposited on a commercial carbon black (Vulcan-XC-72R). Also, three different synthetic methods were assessed given that the catalyst preparation procedure has a strong influence on its final properties. It is necessary to optimize each synthesis method, taking into consideration the particular characteristics of the support, in order to obtain a properly dispersed active phase, with the most appropriate crystal size.

2. Results and Discussion

2.1. Textural and Chemical Characterization

2.1.1. Characterization of the Carbon Supports

Table 1 presents the textural properties of the carbon supports, determined from their corresponding nitrogen adsorption isotherms. Carbon supports were called “CXG” for carbon xerogels and “Vulcan”, for the commercial carbon black. Significantly higher values of surface area (660 m²·g⁻¹) and pore volume (1.79 cm³·g⁻¹) were obtained for the carbon xerogel, in comparison to those determined for Vulcan carbon black (224 m²·g⁻¹), pointing to a more developed porous structure in the case of the CXG.

Table 1. Carbon support textural properties.

Sample	SBET (m2·g−1)	Total pore volume (0.7–180 nm) (cm3·g−1)	Micropore volume (cm3·g−1)			Mesopore volume (cm3·g−1)			Average pore size (nm)
			Vmicro (0–0.7 nm)	Vmicro (0.7–2 nm)	Vmicro (0–2 nm)	Vmeso (2–25 nm)	Vmeso (25–300 nm)	VBJH (1.5–300 nm)
Vulcan	224	0.47	0.01	0.03	0.04	0.24	0.17	0.41	11.0
CXG	660	1.79	0.06	0.07	0.13	0.97	0.69	1.66	23.3

Table 1. Carbon support textural properties.

Sample	SBET (m2·g−1)	Total pore volume (0.7–180 nm) (cm3·g−1)	Micropore volume (cm3·g−1)			Mesopore volume (cm3·g−1)			Average pore size (nm)
			Vmicro (0–0.7 nm)	Vmicro (0.7–2 nm)	Vmicro (0–2 nm)	Vmeso (2–25 nm)	Vmeso (25–300 nm)	VBJH (1.5–300 nm)
Vulcan	224	0.47	0.01	0.03	0.04	0.24	0.17	0.41	11.0
CXG	660	1.79	0.06	0.07	0.13	0.97	0.69	1.66	23.3

Table 2. Catalysts textural properties.

Sample	SBET (m2·g−1)	Total pore volume (0.7–180 nm) (cm3·g−1)	Micropore volume (cm3·g−1)			Mesopore volume (cm3·g−1)			Average pore size (nm)
			Vmicro (0–0.7 nm)	Vmicro (0.7–2 nm)	Vmicro (0–2 nm)	Vmeso (2–25 nm)	Vmeso (25–300 nm)	VBJH (1.5–300 nm)
Pt/Vulcan-SBM	187	0.47	0.02	0.01	0.03	0.21	0.21	0.42	14.8
Pt/Vulcan-FAM	191	0.38	0.02	0.01	0.03	0.20	0.13	0.33	11.9
Pt/Vulcan-ME	177	0.35	0.02	0.01	0.03	0.17	0.15	0.32	10.3
Pt/CXG-SBM	475	1.34	0.07	0.05	0.12	0.45	0.77	1.22	24.5
Pt/CXG-FAM	478	1.08	0.09	0.05	0.14	0.34	0.59	0.93	23.5
Pt/CXG-ME	349	1.27	0.06	0.04	0.10	0.38	0.77	1.15	25.5

Table 2. Catalysts textural properties.

Sample	SBET (m2·g−1)	Total pore volume (0.7–180 nm) (cm3·g−1)	Micropore volume (cm3·g−1)			Mesopore volume (cm3·g−1)			Average pore size (nm)
			Vmicro (0–0.7 nm)	Vmicro (0.7–2 nm)	Vmicro (0–2 nm)	Vmeso (2–25 nm)	Vmeso (25–300 nm)	VBJH (1.5–300 nm)
Pt/Vulcan-SBM	187	0.47	0.02	0.01	0.03	0.21	0.21	0.42	14.8
Pt/Vulcan-FAM	191	0.38	0.02	0.01	0.03	0.20	0.13	0.33	11.9
Pt/Vulcan-ME	177	0.35	0.02	0.01	0.03	0.17	0.15	0.32	10.3
Pt/CXG-SBM	475	1.34	0.07	0.05	0.12	0.45	0.77	1.22	24.5
Pt/CXG-FAM	478	1.08	0.09	0.05	0.14	0.34	0.59	0.93	23.5
Pt/CXG-ME	349	1.27	0.06	0.04	0.10	0.38	0.77	1.15	25.5

Although the average pore size measured for the carbon xerogel, 23.3 nm, is higher than the value obtained for the carbon black, 11 nm, both carbon materials are predominantly mesoporous. BJH-mesopore volumes are 1.66 cm³·g⁻¹ (for the CXG) and 0.41 cm³·g⁻¹ (for Vulcan), much more relevant than their respective micropore contributions, which become almost negligible in the case of the carbon black. In carbon aerogels and xerogels, micropores are related to the stacking arrangement of the aromatic layers that compose the primary particles of their structure, with a particle size of 3–25 nm [10]. In their three-dimensional arrangement, mesopores appear as a consequence of the void space and interconnections among these primary particles [6]. As shown in Table 1, t-plot analysis of the adsorption isotherms yielded similar values for mesopore volume in the range of 2 to 25 nm as for wider mesopores and macropores, 25–300 nm, in the case of the carbon black. However, for the synthesized carbon xerogel, narrow mesopores (in the range of 2 to 25 nm) represent a relatively higher fraction of the total mesopore volume. Abundance of mesopores in the structure of these materials favors, in principle, their application as supports in the preparation of Pt-based electrocatalysts. Pores in the range of wide mesopores ensure an adequate deposition of the active phase, avoiding pore blockage, and facilitating both the access of the reactants to the metallic sites and the diffusion of the products out of the porous structure of the catalyst [5,11,12].

2.1.2. Catalyst Characterization

Table 2 shows the textural properties obtained from their corresponding nitrogen adsorption isotherms for the several catalysts prepared, using both the carbon black Vulcan and the carbon xerogel, and following the different synthetic routes for Pt deposition. Impregnation and microemulsion synthetic methods were employed to support Pt nanoparticles on the different carbon materials. Impregnation and reduction with formic acid (FAM) or sodium borohydride (SBM) were employed as general synthetic methods, whereas a microemulsion based method (ME) was introduced as a new synthetic route not previously used for carbon xerogels. In general, surface area decreases notably after Pt-loading, as a consequence of partial blockage of the porous structure of the carbon materials. In spite of this, the prepared electrocatalysts show areas in the 177–478 m²·g⁻¹ range, higher in the case of the ones prepared using the carbon xerogel in comparison to Vulcan, due to the more developed porous structure of the starting carbon material.

Micropore volume remains almost constant upon the introduction of the metallic component, with a slight reduction in the amount of wide micropores, which become partially blocked by the deposition of Pt particles of lower size. On the other hand, metal loading affects mostly the mesopore volume of the carbon supports, depending on the initial porous structure of each material and the synthesis method employed for the preparation of the catalyst. Mesopore volume decreases as a consequence of the introduction of the active phase, but this decrease is more noticeable in the case of the catalysts prepared using formic acid as a reducing agent. Following the borohydride synthesis route, Pt-deposition using carbon black as support results in only a slight blockage of narrow mesoporosity. The use of formic acid results in a more extensive pore blockage, either in the case of employing the Vulcan carbon black or the carbon xerogel as supports. A wider range of mesopore sizes, 30–60 nm, was affected by introduction of the metallic active phase when following the formic acid synthesis route, vis-á-vis the use of sodium borohydride as reducing agent. On the other hand, pore volume and surface area decrease dramatically in the case of the catalysts prepared through the microemulsion method. In this last case, micropore volume is totally blocked upon active phase loading. This can be due to the presence of some remains of the surfactant employed within the synthesis of this catalyst, which remain bonded to the carbon surface, as evidenced in TGA oxidation of this catalyst (not shown). The presence of this material, even upon extensive washing, still blocks part of the porous structure of the support.

Figure 1 shows the X-Ray patterns for the prepared electrocatalysts. Peaks observed indicate the presence of the face-centered cubic (fcc) structure typical of Pt and represented by the (111), (200), (220) facets.

Figure 1. XRD patterns for the assessed catalysts.

Figure 1. XRD patterns for the assessed catalysts.

Scherrer’s equation was applied to (220) reflectances for the calculation of Pt particle size in each case. Crystallite sizes obtained range from 3.4 to 4.6 nm, as presented in Table 3. Broader peaks correspond, according to Scherrer’s law, to small average crystal sizes. The broadening of the peaks evidences also lower crystallinity, typical of small particles having lattice strain [13]. Pt crystal size increases for the catalysts prepared using sodium borohydride as reducing agent in the case of using CXG as support, whereas the opposite effect is encountered for the carbon black support.

Table 3. Crystallite size obtained by XRD and percentage of metal (weight) deposited measured by ICP-AES.

Catalysts	Pt crystal size (nm)	% Pt (ICP-AES)
Pt/CXG-SBM	4.2	20.2
Pt/CXG-FAM	3.6	17.9
Pt/CXG-ME	3.9	17.1
Pt/Vulcan-SBM	3.4	16.8
Pt/Vulcan-FAM	4.6	16.7
Pt/Vulcan-ME	4.4	17.4

Table 3. Crystallite size obtained by XRD and percentage of metal (weight) deposited measured by ICP-AES.

Catalysts	Pt crystal size (nm)	% Pt (ICP-AES)
Pt/CXG-SBM	4.2	20.2
Pt/CXG-FAM	3.6	17.9
Pt/CXG-ME	3.9	17.1
Pt/Vulcan-SBM	3.4	16.8
Pt/Vulcan-FAM	4.6	16.7
Pt/Vulcan-ME	4.4	17.4

Pt catalysts were characterized by ICP-AES (Table 3) to determine the percentage of metal deposited. The metallic loading ranges from 16% to 20% (weight). As can be seen in the micrographs obtained by TEM (Figure 2), catalysts present different particle distribution. In principle, the synthetic route using formic acid provides the catalysts with a more adequate Pt-distribution, independently from the support (Figure 2b,d) with average particle sizes centered at 2.7 nm in both cases (see histograms). Synthesis by means of the borohydride route, Figure 2a,e, shows the presence of both isolated particles of lower size and agglomerates of particles in the case of the CXG, where a bimodal particle size distribution is observed: one peak is centered around 3.2 nm and another about 4.5 nm. In the case of Vulcan, there is also some presence of particle agglomerates, with particle size distribution centered around 2.8 nm. The microemulsion route leads to Pt-particles that tend to agglomerate, forming chain-like structures (Figure 2c,f) although particles appear to be individually slightly smaller than in the other cases, with an average size centered at 3.6 nm for Vulcan and at 4.3 nm for the CXG.

Figure 2. TEM images and corresponding histograms for (a) Pt/CXG-SBM; (b) Pt/CXG-FAM; (c) Pt/CXG-ME; (d) Pt/Vulcan-SBM; (e) Pt/Vulcan-FAM; and (f) Pt/Vulcan-ME.

Figure 2. TEM images and corresponding histograms for (a) Pt/CXG-SBM; (b) Pt/CXG-FAM; (c) Pt/CXG-ME; (d) Pt/Vulcan-SBM; (e) Pt/Vulcan-FAM; and (f) Pt/Vulcan-ME.

2.2. Electrochemical Characterization

Pt catalysts were characterized by cyclic voltammetry, and CO stripping was performed in order to establish the influence of the support on the potential for its oxidation. Figure 3 shows the CO-stripping voltammograms obtained for the assessed catalysts. Two scans were performed: during the first one, CO was oxidized; whereas the second one is equivalent to the voltammogram in the base electrolyte.

The COads oxidation peak potential of Pt supported onto both carbon supports was obtained around 0.81–0.83 V vs. RHE, for the catalysts synthesized by impregnation methods. However, for the catalysts synthesized by the microemulsion method, the COads oxidation peak potential occurred at more negative potentials, (0.78 V vs. RHE) along with another oxidation peak at low potentials (0.70 V vs. RHE). Maillard and co-workers [14] investigated the performance of carbon black supported catalysts with different degrees of metallic agglomeration towards the electro-oxidation of CO. They observed that in fact CO monolayer oxidation was strongly influenced by Pt particle size. They reported remarkable activity for Pt agglomerates in comparison to isolated Pt particles or polycrystalline Pt, catalysing CO oxidation at considerably lower overpotentials.

Figure 3. CO stripping voltammograms for (a) Pt/CXG-SBM; (b) Pt/CXG-FAM; (c) Pt/CXG-ME; (d) Pt/Vulcan-SBM; (e) Pt/Vulcan-FAM; and (f) Pt/Vulcan-ME.

Figure 3. CO stripping voltammograms for (a) Pt/CXG-SBM; (b) Pt/CXG-FAM; (c) Pt/CXG-ME; (d) Pt/Vulcan-SBM; (e) Pt/Vulcan-FAM; and (f) Pt/Vulcan-ME.

CO stripping was also employed to determine the electrochemical Pt active areas (ECSA) as shown in Table 4. Catalysts show similar ECSA values between 36.5 and 47.9 m²·g⁻¹, except for Pt/Vulcan-ME, which shows a much lower ECSA, 14.7 m²·g⁻¹. As previously shown in TEM micrographs, this catalyst showed the worst particle distribution, which is responsible for this low ECSA. Contrary to expectations, catalysts with the lowest crystal size do not present the highest ECSA.

Table 4. ECSA obtained from CO stripping and peak mass activity for methanol oxidation.

Catalysts	Pt crystal size (nm)	ECSA (m2·g−1)	Peak mass activity (A·g−1 Pt)	Peak specific activity (mA·cm−2 Pt)
Pt/CXG-SBM	4.2	47.9	363	0.96
Pt/CXG-FAM	3.6	38.6	367	1.13
Pt/CXG-ME	3.9	36.5	470	1.29
Pt/Vulcan-SBM	3.4	39.2	330	0.84
Pt/Vulcan-FAM	4.6	41.4	300	0.47
Pt/Vulcan-ME	4.4	14.7	232	1.58

Table 4. ECSA obtained from CO stripping and peak mass activity for methanol oxidation.

Catalysts	Pt crystal size (nm)	ECSA (m2·g−1)	Peak mass activity (A·g−1 Pt)	Peak specific activity (mA·cm−2 Pt)
Pt/CXG-SBM	4.2	47.9	363	0.96
Pt/CXG-FAM	3.6	38.6	367	1.13
Pt/CXG-ME	3.9	36.5	470	1.29
Pt/Vulcan-SBM	3.4	39.2	330	0.84
Pt/Vulcan-FAM	4.6	41.4	300	0.47
Pt/Vulcan-ME	4.4	14.7	232	1.58

The behavior of the electrocatalysts towards the oxidation of methanol was studied in a deaerated 2 M CH₃OH + 0.5 M H₂SO₄ solution. Resulting cyclic voltammograms recorded are shown in Figure 4. Table 4 also shows the peak activities towards the oxidation of methanol, expressed both in terms of mass activity (A·g⁻¹·Pt) and specific activity (mA·cm⁻²·Pt).

Figure 4. Cyclic voltammograms in a 2M CH₃OH + 0.5M H₂SO₄ solution for the assessed catalysts. Scan rate = 0.02 V·s⁻¹.

Figure 4. Cyclic voltammograms in a 2M CH₃OH + 0.5M H₂SO₄ solution for the assessed catalysts. Scan rate = 0.02 V·s⁻¹.

The highest mass activity value is obtained with Pt/CXG-ME catalyst. This higher activity might be due to its higher activity towards the oxidation of CO, an intermediate of CH₃OH oxidation reaction. Since this catalyst presents the highest activity towards CO oxidation, CH₃OH oxidation becomes also speeded up. Catalysts supported on carbon xerogels, whatever the synthetic method employed, are more active than catalysts supported on Vulcan. The higher mesopore volume of carbon xerogels, allowing an optimal diffusion of reagents towards the catalytic centres, is responsible for the higher catalytic activity. Among the different methods, both impregnation routes (FAM and SBM) lead to catalysts with similar behaviours, particularly when using CXG as catalyst support. Pt/CXG-FAM and Pt/Vulcan-SBM present very similar crystal sizes. Pt/Vulcan-SBM presents a better metal dispersion, (due to its lower crystal size) and so a slightly higher ECSA. In spite of this, its performance is lower, due to the higher mesopore volume of the carbon xerogel in comparison to the carbon black Vulcan. In the CXG, Pt particles are better located within the three phase boundaries, where Pt is in contact with both the ionomer, nafion, and CH₃OH, favoring a higher catalytic activity. The catalyst Pt/Vulcan-ME, showed the poorest activity, probably due to its bad metallic distribution, as could be seen in TEM micrographs. Regarding the specific activity, calculated dividing mass activity by the ECSA, catalysts with the lower ECSA show the higher specific activity, as a result of dividing by a lower value.

The activity of these catalysts towards methanol oxidation was also analyzed by chronoamperometric tests at 600 mV as shown in Figure 5. As in the CV tests, Pt/CXG-ME showed the highest activity. Nevertheless, this activity did not seem very stable with time, given the certain activity decay observed during the experiment.

Figure 5. Chroamperometric tests performed at 0.6 V vs. RHE in a 2 M CH₃OH + 0.5 M H₂SO₄ solution for the assessed catalysts.

Figure 5. Chroamperometric tests performed at 0.6 V vs. RHE in a 2 M CH₃OH + 0.5 M H₂SO₄ solution for the assessed catalysts.

3. Experimental Section

3.1. Synthesis of Carbon Xerogels

Resorcinol (1,3-dihydroxybenzoic acid)-formaldehyde organic gels were synthesized by the sol-gel method first proposed by Pekala et al. [8]. The necessary amounts of resorcinol (R) (98% Sigma-Aldrich, St. Louis, MO, USA) and sodium carbonate deca-hydrated (Panreac, Castellar del Vallès (Barcelona, Spain)) (C) (molar ratio R/C = 800) were dissolved in deionised water under stirring. Subsequently, the required volume of formaldehyde (F) (37 wt.% in H₂O, contains 10%–15% Methanol as stabilizer, Sigma-Aldrich, St. Louis, MO, USA) (molar ratio resorcinol/formaldehyde R/F = 0.5, and dilution rate equal 5.7, as described elsewhere [15]) was added to the former mixture and pH was adjusted to 6 with an aqueous solution of 2 M HNO₃. The mixture was stirred for 30 min and then poured into sealed flasks, followed by curing for 24 h at room temperature, 24 h at 50 °C and 3 days at 85 °C until curing was complete as described elsewhere [16]. Afterwards gels were washed with acetone for three days to exchange the initial solvent, water. Acetone was daily replaced after vacuum filtration. This procedure allows keeping the original gel structure, as surface tension caused by evaporation of the solvent is lower for acetone than for water [6]. Finally wet gels were sub-critically dried at 110 °C for 5 h. Organic xerogels are grinded prior to the treatment with acetone and after the drying process, in an agate mortar until a fine powder is obtained. Xerogels were pyrolyzed with the following heating program steps: (1) 2 h at 150 °C; (2) 1 h at 300 °C; (3) 1 h at 600 °C; and (4) 2 h at 800 °C as described elsewhere [17].

3.2. Pt catalysts Synthesis

Pt was deposited on former carbon supports by impregnation and reduction with two different reducing agents: sodium borohydride and formic acid. The amount of metallic precursor was calculated to obtain a metal loading of 20% w/w. An aqueous solution of H₂PtCl₆ (Sigma-Aldrich, St. Louis, MO, USA) was slowly added to a dispersion of the carbon support in ultrapure water. Mixture was sonicated during the addition of the metallic precursor. pH was adjusted to 5 with a solution of NaOH. Subsequently, sodium borohydride was added in excess to reduce the metallic precursor, maintaining temperature under 18 °C. Finally, catalyst was filtered and thoroughly washed with deionized water, and dried overnight at 60 °C. The catalyst so obtained was named Pt/C-SBM, being C, CXG or Vulcan.

When using formic acid as reducing agent, a dispersion of the carbon support in a 2M solution of formic acid was prepared and heated at 80°C. Then an aqueous solution of H₂PtCl₆ (Sigma-Aldrich, St. Louis, MO, USA) was slowly added under magnetic stirring. Catalyst were filtered and thoroughly washed with ultrapure water, and dried overnight at 60 °C. The catalyst so obtained was named Pt/C-FAM.

The microemulsion route consisted on the synthesis of Pt nanoparticles by means of a water in oil microemulsion [18]. The microemulsion was composed of a commercial surfactant, n-heptane as the non-polar phase and 2-propanol as co-surfactant. A commercial surfactant (Brij30, Sigma-Aldrich, St. Louis, MO, USA) and n-heptane were mixed and stirred, before adding dropwise an aqueous solution of H₂PtCl₆ (8 mM). The co-surfactant, 2-propanol was added until an optically transparent mixture was observed, indicating the formation of the microemulsion. The whole mixture was stirred for 4 h, after which an 0.1 M aqueous solution of the reducing agent (NaBH₄) was slowly added to the microemulsion under continuous stirring. Finally this suspension was slowly added to a suspension of the carbon support in ethanol under sonication. The catalyst was thoroughly washed with ethanol and water and subsequently dried overnight at 60 °C [19]. The catalyst so obtained was named Pt/C-ME.

3.3. Carbon Supports and Catalysts Textural, Structural and Morphological Characterization

The nature and characteristics of the carbon supports were characterized using nitrogen physisorption. Textural properties such as specific surface area, pore volume and mesoporosity were calculated from nitrogen adsorption-desorption isotherms, measured at −196 °C using a Micromeritics (Norcross, GA, USA) ASAP 2020. Total surface area and pore volume were determined using the Brunauer-Emmet-Teller (BET) equation and the single point method, respectively. Microporosity was determined using the t-plot method and mesopore volume and medium pore size were calculated by applying the Barret-Joyner-Hallenda method. Catalysts were characterized by X-Ray Diffraction (XRD), and XRD patterns were performed using a Bruker (Billerica, MA, USA) AXS D8 Advance diffractometer, with a θ–θ configuration and using Cu Kα radiation. Particle sizes were evaluated using TEM images obtained in a JEOL (Tokyo, Japan) 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 Characterization

Catalyst electrochemical activity towards the oxidation of carbon monoxide and methanol was studied using cyclic voltammetry and chronoamperometry. A flow cell with a three-electrode assembly at room temperature and an AUTOLAB (Utrecht, The Netherlands) potentiostat-galvanostat were used to carry out the electrochemical characterization. The counter electrode consisted of a pyrolytic graphite bar and the reference electrode was a reversible hydrogen electrode (RHE). All potentials in the text refer to the latter. The working electrode consisted of a pyrolytic graphite disk with a thin layer of the different electrocatalysts deposited onto it. For the preparation of this layer, an aqueous suspension of Pt/CXG or Pt/Vulcan catalysts was obtained by ultrasonically dispersing it in Nafion and ultrapure water (Merck-Millipore, Billerica, MA, USA). Subsequently, an aliquot of 40 μL of the dispersed suspension was deposited on top of the graphite disk (7 mm) and dried under inert atmosphere prior its use. After preparation, the electrode was immersed into deaerated 0.5 M H₂SO₄ electrolyte, prepared from high purity reagents (Merck-Millipore, Billerica, MA, USA) and ultrapure water (Merck-Millipore, Billerica, MA, USA). The electrolyte was saturated with pure N₂ or CO (99.997%, Air Liquide, Madrid, Spain), depending on the experiments. Activation of the electrode was performed by potential cycling solution between 0.05 and 1.10 V at a scan rate of 0.5 V·s⁻¹ until a stable voltammogram in the base electrolyte (0.5 M H₂SO₄) was obtained.

CO stripping voltammograms were obtained after bubbling this gas in the cell for 10 min at 0.20 V, followed by electrolyte exchange and nitrogen purging to remove the excess of CO, and oxidation by scanning the potential up to the upper limit previously established for Pt catalysts. The admission potential was selected considering that, for this value, maximum adsorbate coverage is achieved for CO adsorption on Pt. Electrochemical Pt active areas were determined from the integration of the current involved in the oxidation of a CO monolayer taking into account that CO adsorbs on Pt and assuming 420 μC·cm⁻². Cyclic voltammograms for the electrooxidation of methanol were carried out in a 2 M CH₃OH + 0.5 M H₂SO₄ solution, at scan rate of 0.02 V·s⁻¹, between 0.0 and 1.10 V. Chronoamperometries were performed at 0.60 V vs. RHE in a 2 M CH₃OH + 0.5 M H₂SO₄ solution in order to evaluate the performance of the electrocatalysts for the oxidation of methanol. Every experiment was carried out at room temperature (25 °C ± 1 °C).

4. Conclusions

A highly mesoporous carbon xerogel was synthesized as support for Pt nanoparticles. Three different synthetic methodologies were employed for the synthesis of Pt-based catalysts: two impregnation methods and a microemulsion method. These methods were also applied to a commercial carbon black, Vulcan.

Carbon xerogel showed a high developed surface area and high mesoporosity, much greater than the one shown for the commercial support.

Catalysts supported on carbon xerogel provided lower crystal sizes and good metallic distribution, particularly when using formic acid as reducing agent.

Pt-based catalysts were tested for CO oxidation and the CH₃OH oxidation. Pt synthesized by the microemulsion method supported on the carbon xerogel was the highest active catalyst for the oxidation of CH₃OH. This fact was explained by the higher activity of this catalyst towards the oxidation of CO, an intermediate of the oxidation of methanol.

Catalysts supported on carbon xerogels were more active than catalysts supported on the commercial carbon black support, Vulcan, due to the higher mesoporosity of the former, favoring the diffusion of reagents to and from the catalytic centers.