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Article

Ozone-Assisted Hydrothermal Synthesis Method of Sb-Doped SnO2 Conductive Nanoparticles for Carbon-Free Oxygen-Reduction-Reaction Catalysts of Proton-Exchange-Membrane Hydrogen Fuel Cells

by
Takeshi Fukuda
1,
Kenji Iimura
2,
Takanori Yamamoto
1,
Ryuki Tsuji
1,
Maito Tanabe
1,
Seiji Nakashima
3,
Naoki Fukumuro
2 and
Seigo Ito
1,*
1
Department of Materials and Synchrotron Radiation Engineering, Graduate School of Engineering, University of Hyogo, 2167 Shosha, Himeji 671-2280, Hyogo, Japan
2
Department of Chemical Engineering and Materials Science, Graduate School of Engineering, University of Hyogo, 2167 Shosha, Himeji 671-2280, Hyogo, Japan
3
Department of Electronics and Computer Science, Graduate School of Engineering, University of Hyogo, 2167 Shosha, Himeji 671-2280, Hyogo, Japan
*
Author to whom correspondence should be addressed.
Crystals 2024, 14(5), 462; https://doi.org/10.3390/cryst14050462
Submission received: 7 June 2023 / Revised: 9 May 2024 / Accepted: 11 May 2024 / Published: 15 May 2024
(This article belongs to the Special Issue New Materials for Electrochemical Energy Storage Systems and Catalysis)
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Abstract

:
Proton-exchange-membrane hydrogen fuel cells (PEMFCs) are an important energy device for achieving a sustainable hydrogen society. Carbon-based catalysts used in PEMFCs’ cathode can degrade significantly during operation-voltage shifts due to the carbon deterioration. The longer lifetime of the system is necessary for the further wide commercialization of PEMFCs. Therefore, carbon-free catalysts are required for PEMFCs. In this study, highly crystallized conducting Sb-doped SnO2 (Sb-SnO2) nanoparticles (smaller than 7 nm in size) were synthesized using an ozone-assisted hydrothermal synthesis. Pt nanoparticles were loaded on Sb-SnO2 supporting particles by polyol method to be “Pt/Sb-SnO2 catalyst”. The Pt/Sb-SnO2 catalyst showed a high oxygen reduction reaction (ORR) mass activity (178.3 A g-Pt−1 @ 0.9 V), compared to Pt/C (149.3 A g-Pt−1 @ 0.9 V). In addition, the retention ratio from the initial value of electrochemical surface area (ECSA) during 100,000-voltage cycles tests between 1.0 V and 1.5 V, Pt/SnO2 and Pt/Sb-SnO2 catalyst exhibited higher stability (90% and 80%), respectively, than that of Pt/C catalyst (47%). Therefore, the SnO2 and Sb-SnO2 nanoparticles synthesized using this new ozone-assisted hydrothermal method are promising as carbon-free catalyst supports for PEMFCs.

Graphical Abstract

1. Introduction

Proton-exchange-membrane hydrogen fuel cells (PEMFCs) are clean generator devices with multiple advantages, such as small size, lightweight, low noise, and high power density. They have been used as power sources for automobiles and stationary fuel cells. However, since the lifetime of PEMFCs for automotive applications is 2500–3000 h [1], the operation stability should be extended for further application. In PEMFCs, a Pt carbon (Pt/C) catalyst, which consists of platinum (Pt) nanoparticles supported on porous carbon, is used for the cathode. The carbon can be degraded with the voltage variation at the starting-up and shutting-down [2,3,4,5,6,7]. In addition, it has been reported that when a portion of the anode is exposed to air, the voltage at the cathode jumps up to 1.4–2.0 V [8,9,10]. Under such conditions, carbon is easily oxidized to CO2, resulting in the deterioration of PEMFC performance. Hence, various studies have been conducted to develop materials that can be replaced with carbon.
In order to replace the carbon support, metal oxides have been studied intensively because they are chemically stable and conductive, such as titanium oxide (TiOx) [11], titanium carbide (TiC) [12], tungsten oxide (WOx) [13], iridium oxide (IrOx) [14], ruthenium oxide (RuOx) [14], cerium oxide (CeOx) [15], manganese oxide (MnOx) [16] and tin oxide (SnOx) [17,18,19,20,21,22,23,24,25,26,27,28,29,30,31,32,33,34,35,36,37,38,39,40,41,42,43,44,45,46,47]. Among these, SnO2 is one of the most actively studied materials because it is very stable under the operating voltage of PEMFCs [23,25]. Moreover, it exhibits very high electrical conductivity when doped with other elements. For the dopants, antimony (Sb), niobium (Nb), and tantalum (Ta) are typical elements that have been reported as PEMFC catalyst supports and showed high activity and durability as Pt-supporting catalysts [17,19,21,22,24,25,26,27,32,33,34,35,36,37,38,39,40,41,42,43,44,45,46,47]. In addition, SnO2 can be produced at a low cost. Moreover, SnO2 is a transition metal-oxide semiconductor, and it is not only utilized in fuel cells but also in various devices such as solar cells [48], displays [49], and gas sensors [50].
There are multiple reports about synthesis methods of SnO2 as Pt (or another catalyst) supports for PEMFCs: sol–gel (including precipitation) methods with annealing [17,18,19,20,21,22,23,24,25,26,27], polyol crystallization without annealing [28], hydrothermal synthesis with annealing [29] and without annealing [30,31], flame oxide-forming [32,33,34,35,36,37,38,39,40,41,42,43,44], electrospinning with annealing [45,46], and atomic layer deposition (ALD) [47]. There is also the problem of additives, such as surfactants, which can cause contamination. The organic additives can be eliminated by high-temperature annealing, resulting in the formation of a large and stable aggregation of SnO2 nanoparticles.
To solve these problems, a method using ozone bubbling has been recently developed at the University of Hyogo, Japan [51]. This is a method that converts the precursors into SnO2 nanoparticles using the strong oxidizing power of ozone. This method is quite useful because SnO2 nanoparticles are synthesized reproducibly by very simple control without surfactant. Moreover, there is no report on synthesizing conductive SnO2 nanoparticles by doping using this ozone method.
In this study, we developed a new method (ozone-assisted hydrothermal method) that combines an ozone-based synthesis followed by hydrothermal crystallization (without annealing). Using this new combination, well-crystallized Sb-doped SnO2 (Sb-SnO2) nanoparticles were synthesized without surfactant and annealing procedure. The Sb doping ratios into SnO2 for the PEMFC catalyst support were selected as 5 at.% and 10 at.%, according to previous publications [17,22,24,25,26,27,32,33,44,52,53]. For the application, these SnO2 and Sb-doped SnO2 (Sb-SnO2) nanoparticles prepared by the ozone-assisted hydrothermal method were synthesized, and their material and electrochemical properties were evaluated for cathode catalyst supports in PEMFCs.

2. Experiment

2.1. Materials

All chemicals were used as purchased, without further purification: tin(II) fluoride (SnF2, 90.0%, FUJIFILM Wako Pure Chemical Corporation, Osaka, Japan), antimony trichloride (SbCl3, FUJIFILM Wako Pure Chemical Corporation), 25% tetramethylammonium hydroxide solution ((CH3)4NOH, FUJIFILM Wako Pure Chemical Corporation), methanol (CH3OH, 99.8%, KANTO CHEMICAL Co., Inc., Tokyo, Japan), ethylene glycol (EG, HOCH2CH2OH, FUJIFILM Wako Pure Chemical Corporation), hydrogen hexachloroplatinate(IV) 6-hydrate, 98.5%, KISHIDA CHEMICAL Co., Ltd., Osaka, Japan), ethanol (C2H5OH, 99.5%, KANTO CHEMICAL Co., Inc.), 2-propanol ((CH3)2CHOH, 99.7%, KANTO CHEMICAL Co., Inc.), nafion® perfluorinated resin solution (5 wt.% in lower aliphatic alcohols and water, contains 15–20% water, Sigma-Aldrich Japan, Tokyo, Japan), perchloric acid 70% (HClO4, 70%, KISHIDA CHEMICAL Co., Ltd., Osaka, Japan), platinum carbon catalyst (46.8% Pt loading Pt/C, TEC10E50E, TANAKA Precious Metals., Tokyo, Japan).

2.2. Preparation Method of SnO2 and Sb-SnO2 Nanoparticles

The synthesis method is summarized in Figure 1. The amount of Sb (5 at.% and 10 at.%) in SnO2 is the mixed ratio for the synthesis, not the resulting doped amount. The exact doped values were measured by XRF, shown in the Section 3. Figure 1 shows a block chart of the synthesis method for 5 at.% Sb-doped SnO2. A total of 0.784 g of tin fluoride (SnF2) in 10 mL H2O and 0.060 g of antimony chloride (SbCl3) in 37.5 mL H2O were mixed and stirred with a magnetic stirring bar until the solution became transparent (for 10 at.% doping, the amount of SbCl3 was doubled to be 0.120 g). A solution of 4.3 mL of tetramethylammonium hydroxide (TMAH) was added and sonicated for 1 min, and the solution became milky white. Ozone bubbling was performed for 1 h using an ozone generator (OZONE WAVE, SYOKEN Corporation, Tokyo, Japan) with stirring at 850 rpm at 70 °C. The ozone flow rate was set at 3 L min−1 (Lpm), and the applied power was 80% of the system. During the ozone bubbling, the milky-white solution gradually turns yellow and transparent. Using a rotary evaporator, the reacted solution was densified until the solution volume was reduced to 20 mL. The solution was transferred to a Teflon-internal-vessel and stainless-steel-out jacket autoclave (Model 4744, General Purpose Acid Digestion Vessel, 45 mL, Parr Instrument Company, Moline, IL, USA) and placed in an electric furnace at 240 °C for 12 h. The dark blue precipitate was obtained by centrifugation. The precipitate was dispersed in H2O and centrifuged to remove the supernatant liquid with impurities 3 times. And then, the precipitation was dispersed in methanol using an ultrasonic homogenizer. Finally, the solution was transferred to a Petri dish and dried on a hot plate at 60 °C to be named “ozone-hydrothermal Sb-SnO2”. Each 10 at.% Sb-SnO2 was synthesized by changing the amount of SbCl3. Each pure SnO2 (without Sb dopant) was prepared in the same way without SbCl3.

2.3. Preparation Method of Thin Films of SnO2 and Sb-SnO2

To evaluate conductivity, absorption spectra, and XRD patterns, SnO2, 5 at.% Sb-SnO2, and 10 at.% Sb-SnO2 thin films were prepared by spin-coating on glass substrates. Glass substrates were 25 × 25 mm in size. Substrates were ultrasonically cleaned with ethanol and distilled water for 30 min, and then surface organics were removed with UV-O3 cleaner (Tabletop UV/Ozone Processor, SEN LIGHTS Corporation, Osaka, Japan). Methanol was used as the solvent of Sb-SnO2 dispersion. It was thoroughly dispersed using an ultrasonic homogenizer. The concentration of the solution was 30 wt.%. A total of 120 μL of the solution was dropped onto the glass substrate using a micropipette and spun at 2500 rpm for 20 s. To increase the thickness, the spin coating was repeated four times. Finally, the substrate was annealed at 450 °C for 2 h.

2.4. Preparation Method of Pt/SnO2 and Pt/5 at.% Sb-SnO2

Pt catalyst nanoparticles were prepared using a polyol method, as reported elsewhere [54]. As a platinum precursor solution, 1 g hexachloroplatinic acid hexahydrate was dissolved in 50 mL ethanol. A total of 81 mg of Sb-SnO2 powder was placed in a flask and mixed with 135 mL of EG/water (2:1) mixture at room temperature. While the solution was stirred with a magnetic stirring bar at room temperature, 2.69 mL of the platinum precursor solution was added. After sonication, the mixture was stirred for 12 h at room temperature. It was transferred to an oil bath and heated at 125 °C for 2 h with stirring to reduce platinum. The reactants were centrifuged with distilled water and dried in an oven at 60 °C overnight to be the Pt/5 at.% Sb-SnO2 powder. The targeting Pt amount at the synthesis was 20 wt%, and the XRF measured Pt amount was ca. 17 wt% in Pt/5 at.% Sb-SnO2. Pt/SnO2 was prepared in the same way as above. In order to confirm the merit of the ozone-assisted hydrothermal method, a catalyst without the hydrothermal method (named “Pt/ozone Sb-SnO2” in Figure 1) was prepared and compared. The “ozone Sb-SnO2” was the colloidal nanoparticle after ozone bubbling in Figure 1, which was obtained by centrifugation and 60 °C drying.

2.5. Materials Characterizations

The atomic ratio of Sn/Sb in prepared Sb-SnO2 was measured by X-ray fluorescence (XRF, XGT-1000WR, HORIBA, Ltd., Kyoto, Japan). The crystal structure of Sb-SnO2 powder was evaluated by X-ray diffraction (XRD, MiniFlexⅡ, Rigaku, Tokyo, Japan). The morphologies of (Sb-)SnO2 and Pt/(Sb-)SnO2 were observed by transmission electron microscope and high-angle annular dark field scanning transmission electron microscope (TEM and HAADF-STEM, Talos F200i, Thermo Fisher Scientific Japanese Grous, Tokyo, Japan). The average crystallite size was calculated using the Scherrer’s equation. The average nanoparticle size of SnO2 and Sb-SnO2 was evaluated using the TEM images. The aggregation size of nanoparticles dispersed in methanol was measured using dynamic light scattering (DLS, nanoSAQLA, Otsuka Electronics Co., Ltd., Osaka, Japan). X-ray photoelectron spectroscopy (XPS, PHI5000, ULVAC-PHI, Inc., Chigasaki, Japan) was performed to evaluate the constituent elements of the obtained SnO2 and Sb-SnO2. The optical absorbance of thin films was evaluated by a UV/vis spectrometer (LAMBDA 750 UV/VIS Spectrometer, PerkinElmer Japan, Yokohama, Japan). The sheet resistance of thin films was measured using a resistivity meter (Lonerta-EP MCP-T360, Mitsubishi Chemical Corporation, Tokyo, Japan). Film thickness was measured using a scanning electron microscope (SEM, JSM-6510, JEOL, Tokyo, Japan). Conductivity was calculated from the obtained sheet resistance and film thickness.

2.6. Electrochemical Characterization of Pt/SnO2 and Pt/Sb-SnO2

Electrochemical measurements and catalyst evaluation were performed based on the reported method [43]. Electrochemical measurements were performed at room temperature using a rotating disk electrode system (RDE, HR-500, Meiden Hokuto Corporation, Tokyo, Japan) and a three-electrode cell. A reference electrode (reverse hydrogen electrode, RHE), a working electrode (glassy carbon disk electrode, electrode surface area 0.196 cm2), a counter electrode (platinum wire electrode), and an electrolyte solution (0.1 M HClO4) were used. Catalyst ink was prepared by mixing 12 mg of Pt/(Sb-)SnO2, 5358 μL of distilled water, 1692 μL of isopropanol, and 28.2 μL of 5% Nafion dispersion followed by sonication for 2 min using an ultrasonic homogenizer. A total of 10 μL of catalyst ink was applied on the surface of the glassy carbon disk electrode using a micropipette. And then, it dried in an oven at 60 °C for 20 min. The amount of Pt loaded on the electrode was 17.3 μg-Pt cm−2. For cyclic voltammetry (CV) and linear sweep voltammetry (LSV) measurements, a potentiostat (HZ-7000, Hokuto Denko Corporation, Tokyo, Japan) was used.
For the electrochemical surface area (ECSA), CV measurements were performed by sweeping the potential between 0.05 V and 1.2 V at 50 mV s−1 in HClO4 without rotating WE. Before the measurement, N2 gas was bubbled in the solution for 10 min. After 50 cycles of voltage sweeping and the confirmation of no variational result, the CV data were acquired. ECSA was determined by integrating the area of the hydrogen adsorption region (0.4–0.05 V) at the 50th cycle of CV voltammograms. Following the former research, the hydrogen adsorption electric capacitance per unit area of Pt was decided to be 0.21 mC cm−2 [55].
To evaluate the oxygen reduction reaction (ORR) activity, the mass activity (MA) of the catalyst was evaluated by liner-sweep voltammetry (LSV) measurements performed while rotating WE. LSV was recorded by sweeping a potential range of 0.05 to 1.2 V at a scan rate of 10 mV s−1. Before the measurement, O2 gas was bubbled in the solution for 30 min. The rotational speeds of the working electrode were 100, 400, 900, 1600, and 2500 rpm. The Koutecky–Levich equation was applied to calculate the mass activity (MA) at 0.9 V vs. RHE.
The catalyst durability of ECSA was evaluated using a start-stop protocol (10,000 cycles of voltage sweeping with 0.5 V s−1 from 1.0 to 1.5 V) to check the durability of supporting material (carbon or SnO2) [7] and a load cycle protocol (10,000 cycles of voltage steps kept at 1.0 V for 3 s and at 0.6 V for 3 s, alternatively) to check the durability of Pt nanoparticles on the supporting material [7]. Before the durability test, the LSV measurements were performed under oxygen saturation, and then, for the stability test, N2 gas was bubbled in the electrolyte solution for 20 min, and the initial ECSA data were measured by CV. To determine the retention rate of ECSA, the 5 cycles of CV measurements were measured after every 1000 cycles. The ECSA data were acquired at the 5th cycle of CV.

3. Result and Discussion

3.1. Material Characteristics of SnO2 and Sb-SnO2

To confirm the concentration of doped antimony, XRF measurements were performed on the Sb-SnO2 powders (Table 1). The 5 at.% Sb-SnO2 shows that the Sb/Sn ratio at the synthesis was kept in the resulting SnO2 powder. In contrast, the 10 at.% Sb-SnO2 had only 8 at.% Sb, and not all Sb ions are present in the SnO2 lattice, which will be due to the limitation of doping amounts. Although 10 at.% of Sb doping was not in the SnO2 lattice, this sample will continue to be referred to as “10 at.% Sb-SnO2” in this study. The detailed research of another concentration will be discussed in a future paper.
Figure 2a shows XRD measurements of SnO2 powders synthesized by ozone-assisted process [51] and ozone-assisted hydrothermal process (this work). In order to express the crystallinity, the y-axis of Figure 2a shows the measured-XRD raw data, which are not the arbitrary unit (a.u.) because the arbitrary unit (a.u.) cannot be compared about the largeness of the y-axis. As a result of the hydrothermal treatment, the crystalline of SnO2 was significantly improved compared to only the ozone-assisted process. Figure 2b shows XRD measurements of Sb-SnO2 powders with different antimony synthesis concentrations. Peaks showed tetragonal rutile structure derived from SnO2 in all Sb-SnO2 at 0, 5, and 10 at.%. In addition, no additional peaks by Sb doping appeared (such as Sb2O3). Figure 2c shows a magnified view of the (101) peak of Sb-SnO2. A slight shift of the peak position to a lower angle was observed with increasing Sb doping concentration, resulting in the SnO2 lattice expansion. Therefore, it can be concluded that Sb was doped in the SnO2 lattice effectively.
As the doping concentration was increased from 0, 5, and 10 at.%, the peak became broader and the full width at half maximum (FWHM) widened, and the crystallite size calculated by Scherrer’s equation decreased (Table 2). It has been previously reported that Sb doping decreases the SnO2 crystallite size [56], which is generally consistent with the results of the present measurements.
Figure 3 shows the TEM images of SnO2 nanoparticles with/without Sb doping. The average particle sizes were summarized in Table 2, compared with the crystal sizes obtained by XRD data (using Sherre’s equation). The “crystal/shape-sizes ratio (=(crystallite size from XRD [nm])/(average particle size from TEM [nm]))” was shown. The higher crystal/shape-sizes ratio means higher crystallinity. On the contrary, the lower crystal/shape-sizes ratio means lower crystallinity with an amorphous phase. The SnO2 by ozone-assisted method is a few nm particles with poor crystallinity (Figure 3a). The average particle size, crystal size, and crystal/shape size ratio were 3.99 nm, 1.44 nm, and 0.361, respectively. These results mean that the ozone-assisted SnO2 has lower crystallinity with a thick amorphous phase as the shell. In contrast, it can be confirmed that the SnO2 nanoparticle by ozone-hydrothermal method shows high crystallinity with 11.19 nm of the average particle size (Figure 3b), 8.56 nm of the crystal size, and 0.765 of the crystal/shape size ratio, which is due to the hydrothermal treatment after the ozone peptization method. Also, the SnO2 nanoparticle has a very angular shape, and the crystalline surface can be clearly seen. Figure 3c,d are TEM images of 5 and 10 at.% of Sb-doped SnO2 by ozone-assisted hydrothermal method, respectively. As with pure SnO2, the presence of nanoparticles with high crystallinity can be confirmed because of the high value of the crystal/shape size ratio (>0.88). The particle size decreases with increasing doping concentration (Table 2), which corresponds to the crystallite size calculated from XRD.
Figure 4a shows the results of the survey scan of XPS. For both SnO2 and 5 at.% Sb-SnO2 samples, the distinct peaks for Sn and O were detected. The magnified views of O1s and Sb 3d3/2 and of Sn 4d were shown in Figure 4b,c, respectively. In Figure 4b, the peak of Sb 3d3/2 was detected, and the O1s peak of 5 at.% Sb-SnO2 is slightly broadened compared to the peak of SnO2, which is due to the increasing energy distribution in the oxygen atom. Moreover, in Figure 4c, the Sn 4d peak of 5 at.% Sb-SnO2 also widened the binding energy compared to the peak of SnO2. By the above results of XRF, XRD, and XPS measurements, it was confirmed that the Sb is appropriately doped in the SnO2 lattice with the expansion and squeezing of the SnO2 lattice.
To observe the dispersing condition of nanoparticles in solution, dynamic light scattering (DLS) measurements were performed in water (Figure 5). The average particle sizes calculated from the DLS measurement were 106.5 nm and 87.5 nm for pure SnO2 and 5 at.% Sb-SnO2, respectively. Since the average crystallite size of SnO2 was 11.19 nm by TEM results, SnO2 exists as an aggregate of approximately nine particles in diameter in an aqueous solution. The average aggregate of 5 at.% Sb-SnO2 nanoparticle was smaller than that of SnO2. This may be due to the smaller nanoparticle size of 5 at.% Sb-SnO2 than that of pure SnO2. Hence, there is no variation by Sb doping about the dispersibility.
Conductivities of the SnO2 films, 5 at.% Sb-SnO2, and 10 at.% Sb-SnO2 were measured and prepared by spin-coating and annealing on glass substrates. Table 3 shows the sheet resistance, film thickness, and conductivity of each film. The sheet resistance of the SnO2 was more than 107 Ω sq−1 (over the range of the measurement system). Although the accurate value could not be obtained, it can be said that the pure SnO2 was an insulating material. In contrast, 5 at.% Sb-SnO2 had a sheet resistance of 4.03 ± 2.8 × 104 Ω sq−1 and a conductivity of 0.25 S cm−1. Hence, the doping of Sb significantly improves conductivity. On the other hand, the excess addition of Sb to “10 at.% Sb-SnO2” depressed the conductivity to 0.11 S cm−1. So, it was confirmed that excessive Sb doping could be a hindrance to carrier conduction.
UV/VIS measurements were performed on the thin films of SnO2, 5 at.% Sb-SnO2, and 10 at.% Sb-SnO2. Figure 6 shows the absorbance (y-axis) of the thin films with the plot on energy (x-axis). Each layer has a band gap of around 3.9 eV. Focus on the infrared region (<1 eV), absorption zones were observed in the Sb-SnO2 films. This shows the formation of donor levels in Sb-SnO2 thin films due to the Sb doping. Thus, it was confirmed that the enhanced conductivity of the Sb-SnO2 is due to the formation of donor levels.

3.2. Electrochemical Characteristics of Pt/SnO2 and Pt/Sb-SnO2

For the application of the Sb-SnO2 nanoparticles synthesized via this ozone-assisted hydrothermal method, we have measured the Pt-catalyst-supporting ability using RDE for proton-exchange-membrane fuel cell (PEMFC) as “carbon-support-free PEMFC”. For the Pt/Sb-SnO2, the sample of 5 at.% Sb-SnO2 was used because of better conductivity than 10 at.% Sb-SnO2. Hence, instead of writing the catalyst as “Pt/5 at.% Sb-SnO2”, it will be written as “Pt/Sb-SnO2” in short, below. The PEMFC abilities of prepared Pt/SnO2 and Pt/Sb-SnO2 were evaluated by comparison with the commercial Pt/C (TEC10E50E, TANAKA Precious Metals).
Cyclic voltammetry (CV) results for the fabricated Pt/Sb-SnO2 catalyst are shown in Figure 7a. Both Pt/SnO2 and Pt/Sb-SnO2 showed similar voltammograms as Pt/C derived from Pt peaks. A peculiar peak was detected in Pt/Sb-SnO2 around 0.65 V (not in the CV curve of Pt/C and Pt/SnO2). As the first possibility, it can be thought that the 0.65 V peak is attributed to the oxidation of dissolved Sb atom on Pt [44,47]. However, in the literature, the oxidation peaks of Sb and Sn can be observed at 0.47–0.48 V and 0.61–0.8 V, respectively [24,26]. Hence, as the second possibility, it is thought that the 0.65 V peak is due to Sn oxidation, which can be enhanced by the addition of Sb doping in the SnO2 lattice. The details of the phenomena will be discussed in our future paper, along with the results of XPS, TEM, and additional electrochemical results, considering the effects of strong metal-support interaction (SMSI) [19,28,57,58]. The electrochemical surface area (ECSA) value calculated from the CVs (Figure 7a) is shown in Figure 7b. ECSA was 82.3, 60.3, and 61.7 m2g−1-Pt for Pt/C, Pt/SnO2, and Pt/Sb-SnO2, respectively. Hence, the ECSA of Pt on carbon (Pt/C) was better than that on SnO2 and Sb-SnO2.
Figure 7c,d show the results of LSV and the resulting oxygen reduction reaction (ORR) activity. The onset potential of Pt/Sb-SnO2 is located on the slightly higher voltage side compared to Pt/C and Pt/SnO2. This shows that the ORR activity is enhanced by Sb doping. The mass activity was 149.3, 98.2, and 173.3 A g-Pt−1 for Pt/C, Pt/SnO2, and Pt/Sb-SnO2, respectively. The Pt/Sb-SnO2 recorded the highest mass activity in this work, which would be due to the high conductivity of Sb-SnO2 and SMSI of Pt/Sb-SnO2. This MA value of Pt/Sb-SnO2 (173.3 A g-Pt−1) is one of the highest results in published Sb-SnO2. In Pt/SnO2 catalysts, on the contrary, the lower conductivity of pure SnO2 results in lower mass activity. However, since the LSV curve of Pt/SnO2 shows a high current close to Pt/C and Pt/Sb-SnO2. Hence, Pt/SnO2 is also promising for the PEMFC catalyst.
Figure 8 is the comparison of Pt/Sb-SnO2 with different synthesizing methods (ozone and ozone-hydrothermal methods, shown in Figure 1). The catalysts without hydrothermal treatment exhibited lower catalytic performance. On the other hand, in the CV measurements (Figure 8a), the catalysts with hydrothermal treatment showed clear Pt peaks. In the LSV (Figure 8b), the hydrothermal-treated catalyst performed a high current below 0.9 V for the oxygen reduction reaction.
In order to discuss the catalytic activity, TEM observations were performed. Figure 9 shows STEM/High angle annular dark-field (HAADF) STEM images of Pt/SnO2 and Pt/Sb-SnO2. In HAADF-STEM images, the white parts show the position of Pt nanoparticles on SnO2 and/or Sb-SnO2. Without the hydrothermal method (Pt/ozone SnO2 in Figure 9a and Pt/ozone Sb-SnO2 in Figure 9b), the size of Pt nanoparticles was not so homogeneous (large and small particles), and each Pt nanoparticles were not so much connected.
With the ozone-assisted hydrothermal method without Sb doping (Pt/ozone-hydrothermal SnO2 in Figure 9c), the Pt nanoparticles were significantly connected to each other on the SnO2 surface. This Pt network may be formed due to the redox reaction from H2PtCl6 to Pt nanoparticles on the surface of the SnO2 crystal. The Pt nanoparticles network on the crystal surface of ozone-hydrothermal SnO2 may enhance the ORR.
With the Sb-doping and ozone-assisted hydrothermal method (Pt/ozone-hydrothermal Sb-SnO2 in Figure 9d), the small Pt nanoparticles were dispersed on the SnO2 surface and a bit connected to each other. The conducting ozone-hydrothermal Sb-SnO2 shows high ORR activity with small Pt nanoparticles forming small aggregation (in Figure 9d).
Figure 10 summarizes the images of catalysts in this work. In Figure 10a, the surface of ozone (Sb-)SnO2 particles is an amorphous phase (not crystal). Pt nanoparticles were not deposited without connecting to each other. Moreover, ozone (Sb-)SnO2 does not have the conductivity. Hence, there is not a good pathway for the electrons from graphite electrodes to the reaction site (the surface of Pt nanoparticles). Contrary, in Figure 10b for ozone-hydrothermal SnO2, the Pt nanoparticles made a network as a “nanowire” on the Rutile crystal surface of ozone-hydrothermal SnO2. Although the ozone-hydrothermal SnO2 does not have the conductivity itself, the Pt nanowire can work the pathway for electrons to the surface of Pt nanoparticles for ORR activation [59,60]. On the other hand, in Figure 10c, the ozone-hydrothermal Sb-SnO2 has conductivity for the pathway for electrons to the surface of Pt nanoparticles for ORR. Hence, without such long Pt connections, Pt/ozone-hydrothermal Sb-SnO2 can perform the high ORR activity. Due to the conductivity of the ozone-hydrothermal Sb-SnO2, it may not be necessary for Pt nanoparticles to connect each other at the Pt nanoparticle formation with the redox reaction (from H2PtCl6 to Pt nanoparticles).

3.3. Stability of Pt/SnO2 and Pt/Sb-SnO2 as ORR Catalyst

The durability of the catalyst was evaluated using a start-stop protocol. The start-stop protocol is a widely known method for evaluating the durability of catalyst supports in PEMFC [5,6,7]. At first, the durability of the supporting material (carbon or SnO2) was checked by a start-stop protocol (10,000 cycles of voltage sweeping with 0.5 V s−1 between 1.0 V and 1.5 V) [7] (Figure 11a). Figure 11b shows the transition of ECSA value up to 100,000 cycles, and Figure 11c shows the retention rate of ECSA when the initial value is normalized to 100%. The ECSA retention after 100,000 cycles were 46, 80, and 90% from the initial value of Pt/C, Pt/Sb-SnO2, and Pt/SnO2, respectively. Pt/SnO2 and Pt/Sb-SnO2 showed high durability compared to Pt/C. In Figure 10b, there are crossing points between the ECSA of Pt/C and those of Pt/SnO2 and Pt/Sb-SnO2, around 20,000 cycles. This suggests that Pt/SnO2 and Pt/Sb-SnO2 outperform Pt/C in long-term utilization from the viewpoint of application. In order to think about the application probability, we have considered the catalytic stability (CS) against Pt/C.
CS = [the final ECSA value of Pt/Sb-SnO2]/[the start ECSA value of Pt/C].
If CS can be very good, the catalyst can be considered for commercial application because of the stability issue of Pt/C. The CS values of Pt/SnO2 and Pt/Sb-SnO2 at 10,000 cycles were 79.3% and 83.2%, respectively, which are quite high values compared to other publications.
At the second, as another type of durability test, the protocol to accelerate Pt degradation was conducted (in Figure 12a with voltage steps kept at 1.0 V for 3 s and at 0.6 V for 3 s, alternatively [7]). Figure 12b shows the transition of ECSA value up to 100,000 cycles. Since the ESCA of Pt/C in Figure 12 was kept higher than that in Figure 11, there was no crossing point between Pt/C and Pt/(Sb-)SnO2, and ECSA of Pt/C was any time better than Pt/(Sb-)SnO2. Figure 12c shows the retention rate of ECSA when the initial value is normalized to 100%. The ECSA retention rate of Pt/C, Pt/Sb-SnO2, and Pt/SnO2 after 100,000 cycles were 63, 70, and 81% from the initial value, respectively. Although the catalysts using SnO2 as a support showed higher durability than Pt/C in Figure 12c, the degradation speed of Pt/Sb-SnO2 was similar to Pt/C up to 20,000 cycles. So, the Sb-SnO2 can work on the durability as supporting material (voltage sweeping with 0.5 V s−1 from 1.0 to 1.5 V), but not so much for Pt durability (voltage steps kept at 1.0 V for 3 s and at 0.6 V for 3 s). The higher durability of Pt/SnO2 may be due to the platinum linkage structure of Pt/SnO2 shown in the STEM and HAADF-STEM images. The linked platinum may work to suppress the migration of platinum during operation under degraded conditions like Pt nanowire. Moreover, the SMSI between Pt and SnO2 supports is also thought to contribute to the realization of high durability. The electronic structure can be changed by SMSI, which suppresses the migration and desorption of platinum. The details will be published in our future paper.

4. Conclusions

SnO2, 5 at.% Sb-SnO2, and 10 at.% Sb-SnO2 were prepared using an ozone-assisted hydrothermal method, which is a simple combination of ozone bubbling and hydrothermal treatment. In XRF, XRD, and XPS results revealed that the Sb is appropriately doped in the SnO2 lattice at 5 at.% of Sb mixing, but some Sb remained out of the lattice at 10 at.% of Sb mixing. In conductivity of films, 5 at.% Sb-SnO2 recorded the conductivity of 0.25 ± 0.12 S cm−1, which would be a significant help for the higher MA value (178.3 A g-Pt−1) than that of Pt/C. The durability of Pt/SnO2 and Pt/5 at.% Sb-SnO2 (voltage sweeping with 0.5 V s−1 from 1.0 to 1.5 V) were much higher than Pt/C and recorded the ECSA retention of 90% and 80% at 100,000 cycles. Therefore, Pt/SnO2 and Pt/5 at.% Sb-SnO2 synthesized using this new ozone-hydrothermal method is a promising carbon-free catalyst support for the long-lifetime PEMFC system. The system electricity generation cost from hydrogen fuel cells can be calculated as [(catalyst cost + another device cost) + (hydrogen cost) ]/[(energy conversion efficiency) × (lifetime)]. If the catalyst and system can survive forever, the cost of the catalyst and system can be negligible. Hence, although the cost of Pt is quite high at any time, the lifetime of the catalyst is much more important.
In summary, the high catalytic activity can be attributed to three reasons: (1) improved conductivity due to antimony doping [39], (2) the platinum linkage structure (like platinum nanowire [59,60]), and (3) strong metal support interaction (SMSI) between Pt and Sb-doped SnO2 [19,28,57,58]. We have measured XPS spectra of Pt 4f orbital in the catalysts (Pt/C, Pt/SnO2, and Pt/5 at.% Sb-SnO2) to discuss the SMSI. However, due to limitations of the paper length and the number of figures, the future paper will be submitted with detailed discussions about SMSI. The origin of the CV peak at 0.65 V will also be discussed in the next paper.

Author Contributions

Conceptualization, T.F., T.Y. and S.I.; methodology, T.F. (electrochemistry), T.Y. (hydrothermal), M.T. (Pt deposition), R.T. (dispersion, electrochemistry), K.I. (ozone synthesis), S.N. (XPS) and N.F. (TEM); data curation, T.F.; writing—original draft preparation, T.F.; writing—review and editing, T.F. and S.I.; supervision, S.I.; project administration, S.I.; funding acquisition, S.I. All authors have read and agreed to the published version of the manuscript.

Funding

This woks has been supported by Himeji City, Hyogo, Japan, funding number: Himesanshindai R5-3 gou.

Data Availability Statement

The original contributions presented in the study are included in the article, further inquiries can be directed to the corresponding author.

Conflicts of Interest

The authors declare no conflict of interest.

Correction Statement

This article has been republished with a minor correction to the abstract, figure content and text. This change does not affect the scientific content of the article.

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Crystals 14 00462 g001
Figure 1. Synthesis method of Pt-deposited Sb-SnO2 nanoparticles.
Figure 1. Synthesis method of Pt-deposited Sb-SnO2 nanoparticles.
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Crystals 14 00462 g002
Figure 2. X-ray diffraction (XRD) spectra of SnO2 and Sb-SnO2: (a) ozone-assisted process [51] and ozone-assisted hydrothermal process, (b) Sb-SnO2 with different antimony concentration (Sb/Sn = 0, 5, 10 at.%), and (c) enlarged view of (101) in Figure 2b.
Figure 2. X-ray diffraction (XRD) spectra of SnO2 and Sb-SnO2: (a) ozone-assisted process [51] and ozone-assisted hydrothermal process, (b) Sb-SnO2 with different antimony concentration (Sb/Sn = 0, 5, 10 at.%), and (c) enlarged view of (101) in Figure 2b.
Crystals 14 00462 g002
Crystals 14 00462 g003
Figure 3. TEM images of SnO2: (a) pure SnO2 synthesizing by ozone-assisted method, (b) pure SnO2 synthesizing by ozone-assisted hydrothermal method, (c) 5 at.% Sb-doped SnO2 synthesizing by ozone-assisted hydrothermal method, and (d) 10 at.% Sb-doped SnO2 synthesizing by ozone-assisted hydrothermal method.
Figure 3. TEM images of SnO2: (a) pure SnO2 synthesizing by ozone-assisted method, (b) pure SnO2 synthesizing by ozone-assisted hydrothermal method, (c) 5 at.% Sb-doped SnO2 synthesizing by ozone-assisted hydrothermal method, and (d) 10 at.% Sb-doped SnO2 synthesizing by ozone-assisted hydrothermal method.
Crystals 14 00462 g003
Crystals 14 00462 g004
Figure 4. X-ray photoelectron spectroscopy (XPS) spectra of pure SnO2 and 5 at.% Sb-SnO2: (a) survey spectra, (b) O1s and Sb 3d spectra, and (c) Sn 4d spectra.
Figure 4. X-ray photoelectron spectroscopy (XPS) spectra of pure SnO2 and 5 at.% Sb-SnO2: (a) survey spectra, (b) O1s and Sb 3d spectra, and (c) Sn 4d spectra.
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Crystals 14 00462 g005
Figure 5. Dynamic light scatting (DLS) size distribution plot of pure SnO2 and 5 at.% Sb-SnO2.
Figure 5. Dynamic light scatting (DLS) size distribution plot of pure SnO2 and 5 at.% Sb-SnO2.
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Crystals 14 00462 g006
Figure 6. Absorption spectra of SnO2, 5 at.% Sb-SnO2, and 10 at.% Sb-SnO2.
Figure 6. Absorption spectra of SnO2, 5 at.% Sb-SnO2, and 10 at.% Sb-SnO2.
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Crystals 14 00462 g007
Figure 7. Electrochemical measurements of commercial Pt/C, Pt/SnO2, and Pt/5 at.% Sb-SnO2 catalysts using RDE: (a) cyclic voltammograms with N2 saturation (rotation speed at 0 rpm), (b) ECSA calculated from Figure 7a, (c) linear sweep voltammograms with O2 saturation (rotation speed at 2500 rpm), and (d) MA calculated from Figure 7c.
Figure 7. Electrochemical measurements of commercial Pt/C, Pt/SnO2, and Pt/5 at.% Sb-SnO2 catalysts using RDE: (a) cyclic voltammograms with N2 saturation (rotation speed at 0 rpm), (b) ECSA calculated from Figure 7a, (c) linear sweep voltammograms with O2 saturation (rotation speed at 2500 rpm), and (d) MA calculated from Figure 7c.
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Crystals 14 00462 g008
Figure 8. Electrochemical measurements of Pt/Sb-SnO2 catalyst activity with different synthesizing methods using RDE of (a) cyclic voltammograms with N2 saturation (rotation speed at 0 rpm) and (b) linear sweep voltammograms with O2 saturation (rotation speed at 2500 rpm).
Figure 8. Electrochemical measurements of Pt/Sb-SnO2 catalyst activity with different synthesizing methods using RDE of (a) cyclic voltammograms with N2 saturation (rotation speed at 0 rpm) and (b) linear sweep voltammograms with O2 saturation (rotation speed at 2500 rpm).
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Crystals 14 00462 g009aCrystals 14 00462 g009b
Figure 9. STEM and HAADF-STEM images of Pt/SnO2 and Pt/5 at.% Sb-SnO2 with different synthesizing method: (a) Pt/SnO2 by ozone method, (b) Pt/5 at.% Sb-SnO2 by ozone method, (c) Pt/SnO2 by ozone-hydrothermal method, and (d) Pt/5 at.% Sb-SnO2 by ozone-hydrothermal method.
Figure 9. STEM and HAADF-STEM images of Pt/SnO2 and Pt/5 at.% Sb-SnO2 with different synthesizing method: (a) Pt/SnO2 by ozone method, (b) Pt/5 at.% Sb-SnO2 by ozone method, (c) Pt/SnO2 by ozone-hydrothermal method, and (d) Pt/5 at.% Sb-SnO2 by ozone-hydrothermal method.
Crystals 14 00462 g009aCrystals 14 00462 g009b
Crystals 14 00462 g010aCrystals 14 00462 g010b
Figure 10. Working and activation image of catalysts: (a) ozone (Sb-)SnO2, (b) ozone-hydrothermal SnO2, and (c) ozone-hydrothermal Sb-SnO2.
Figure 10. Working and activation image of catalysts: (a) ozone (Sb-)SnO2, (b) ozone-hydrothermal SnO2, and (c) ozone-hydrothermal Sb-SnO2.
Crystals 14 00462 g010aCrystals 14 00462 g010b
Crystals 14 00462 g011
Figure 11. Durability of commercial Pt/C, Pt/SnO2, and Pt/5 at.% Sb-SnO2 as a start-stop protocol potential cycles up to 100,000 cycles with voltage sweeping with 0.5 V s−1 from 1.0 to 1.5 V) to check the durability of supporting material (carbon or SnO2) [7]: (a) the applied voltage pattern for the stability test; (b) the transition of ECSA value and (c) ECSA retention rate.
Figure 11. Durability of commercial Pt/C, Pt/SnO2, and Pt/5 at.% Sb-SnO2 as a start-stop protocol potential cycles up to 100,000 cycles with voltage sweeping with 0.5 V s−1 from 1.0 to 1.5 V) to check the durability of supporting material (carbon or SnO2) [7]: (a) the applied voltage pattern for the stability test; (b) the transition of ECSA value and (c) ECSA retention rate.
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Crystals 14 00462 g012
Figure 12. Durability of commercial Pt/C, Pt/SnO2, and Pt/5 at.% Sb-SnO2 as an accelerating Pt degradation protocol potential cycles up to 100,000 cycles with voltage steps kept at 1.0 V for 3 s and at 0.6 V for 3 s, alternatively, to check the durability of Pt nanoparticles [7]: (a) the applied voltage pattern for the stability test; (b) the transition of ECSA value and (c) ECSA retention rate.
Figure 12. Durability of commercial Pt/C, Pt/SnO2, and Pt/5 at.% Sb-SnO2 as an accelerating Pt degradation protocol potential cycles up to 100,000 cycles with voltage steps kept at 1.0 V for 3 s and at 0.6 V for 3 s, alternatively, to check the durability of Pt nanoparticles [7]: (a) the applied voltage pattern for the stability test; (b) the transition of ECSA value and (c) ECSA retention rate.
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Table 1. Sn/Sb atomic ratio measured by XRF.
Table 1. Sn/Sb atomic ratio measured by XRF.
SampleSn/Sb Ratio/at.%
SnSb
5 at.% Sb-SnO295.05.01
10 at.% Sb-SnO292.17.94
Table 2. Crystal and average particle sizes of ozone-assisted SnO2 with/without hydrothermal treatment with different Sb concentrations. The “crystal/shape size ratio” shows the value of (crystallite size from XRD [nm])/(average particle size from TEM [nm]).
Table 2. Crystal and average particle sizes of ozone-assisted SnO2 with/without hydrothermal treatment with different Sb concentrations. The “crystal/shape size ratio” shows the value of (crystallite size from XRD [nm])/(average particle size from TEM [nm]).
Sb Synthesizing Concentration (at.%)Crystallite Size
from XRD/nm		Average Particle Size from TEM/nmCrystal/Shape Size Ratio
Ozone SnO21.443.990.361
Ozone-hydrothermal SnO28.5611.190.765
Ozone-hydrothermal 5 at.%-Sb-SnO25.866.630.884
Ozone-hydrothermal 10 at.%-Sb-SnO24.304.850.887
Table 3. Sheet resistance, film thickness, and conductivity of SnO2, 5 at.% Sb-SnO2, and 10 at.% Sb-SnO2.
Table 3. Sheet resistance, film thickness, and conductivity of SnO2, 5 at.% Sb-SnO2, and 10 at.% Sb-SnO2.
Sb Synthesizing Concentration
(at.%)		Sb Concentration by XRF
(at.%)		Sheet Resistance
(Ω·sq−1)		Film Thickness
(nm)		Conductivity
(S·cm−1)
0->107 (over range)939 ± 54-
55.014.03 ± 2.8 × 1041150 ± 2310.25 ± 0.12
107.941.68 ± 0.8 × 105950 ± 310.11 ± 0.05
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Fukuda, T.; Iimura, K.; Yamamoto, T.; Tsuji, R.; Tanabe, M.; Nakashima, S.; Fukumuro, N.; Ito, S. Ozone-Assisted Hydrothermal Synthesis Method of Sb-Doped SnO2 Conductive Nanoparticles for Carbon-Free Oxygen-Reduction-Reaction Catalysts of Proton-Exchange-Membrane Hydrogen Fuel Cells. Crystals 2024, 14, 462. https://doi.org/10.3390/cryst14050462

AMA Style

Fukuda T, Iimura K, Yamamoto T, Tsuji R, Tanabe M, Nakashima S, Fukumuro N, Ito S. Ozone-Assisted Hydrothermal Synthesis Method of Sb-Doped SnO2 Conductive Nanoparticles for Carbon-Free Oxygen-Reduction-Reaction Catalysts of Proton-Exchange-Membrane Hydrogen Fuel Cells. Crystals. 2024; 14(5):462. https://doi.org/10.3390/cryst14050462

Chicago/Turabian Style

Fukuda, Takeshi, Kenji Iimura, Takanori Yamamoto, Ryuki Tsuji, Maito Tanabe, Seiji Nakashima, Naoki Fukumuro, and Seigo Ito. 2024. "Ozone-Assisted Hydrothermal Synthesis Method of Sb-Doped SnO2 Conductive Nanoparticles for Carbon-Free Oxygen-Reduction-Reaction Catalysts of Proton-Exchange-Membrane Hydrogen Fuel Cells" Crystals 14, no. 5: 462. https://doi.org/10.3390/cryst14050462

APA Style

Fukuda, T., Iimura, K., Yamamoto, T., Tsuji, R., Tanabe, M., Nakashima, S., Fukumuro, N., & Ito, S. (2024). Ozone-Assisted Hydrothermal Synthesis Method of Sb-Doped SnO2 Conductive Nanoparticles for Carbon-Free Oxygen-Reduction-Reaction Catalysts of Proton-Exchange-Membrane Hydrogen Fuel Cells. Crystals, 14(5), 462. https://doi.org/10.3390/cryst14050462

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