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Article

Synthesis, Characterization and Shape-Dependent Catalytic CO Oxidation Performance of Ruthenium Oxide Nanomaterials: Influence of Polymer Surfactant

by
Antony Ananth
1,
Duncan H. Gregory
2 and
Young Sun Mok
1,*
1
Department of Chemical and Biological Engineering, Jeju National University, Jeju 690-756, Korea
2
School of Chemistry, University of Glasgow, Glasgow G12 8QQ, UK
*
Author to whom correspondence should be addressed.
Appl. Sci. 2015, 5(3), 344-358; https://doi.org/10.3390/app5030344
Submission received: 26 June 2015 / Revised: 26 July 2015 / Accepted: 5 August 2015 / Published: 11 August 2015
(This article belongs to the Special Issue Nano-Catalysts and Their Applications)
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Abstract

:
Ruthenium oxide nano-catalysts supported on mesoporous γ-Al2O3 have been prepared by co-precipitation method and tested for CO oxidation. The effect of polyethylene glycol (PEG) on the properties of the catalyst was studied. Addition of the PEG surfactant acted as a stabilizer and induced a change in the morphology of ruthenium oxide from spherical nanoparticles to one-dimensional nanorods. Total CO conversion was measured as a function of morphology at 175 °C and 200 °C with 1.0 wt.% loading for PEG-stabilized and un-stabilized catalysts, respectively. Conversion routinely increased with temperature but in each case, the PEG-stabilized catalyst exhibited a notably higher catalytic activity as compared to the un-stabilized equivalent. It can be assumed that the increase in the activity is due to the changes in porosity, shape and dispersion of the catalyst engendered by the use of PEG.

Graphical Abstract

1. Introduction

Ruthenium oxide (RuOx) is a promising-material both in the context of catalysis [1,2] and energy [3]. For instance, combinations and composites based on metallic ruthenium/ruthenium oxides are notable for coupling reaction catalysis [4], catalyzing the photochemical reduction of water [5], as thin film resistors for inkjet printing [6] and as catalysts for N2O decomposition [7], selective oxidation of alcohol [8] and oxidation of carbon monoxide (CO) [9,10,11]. Among the above chemical processes, CO oxidation is an attractive one for study since it is both an industrially important reaction and relatively uncomplicated to model experimentally and computationally. The impact of CO on environmental air quality is considerable and as a toxic gas an exposure of 800 ppm for 1 h is fatal to human life [12]. Noble metal catalysts such as Pt and Pd exhibit good CO oxidation activity but concerns over cost and abundance have compelled researchers to develop metal oxides as a viable alternative [13,14,15,16]. The catalytic activity of candidate metal oxide systems is heavily dependent on oxidation state and for example in the Ru-O system, when a RuO2 catalyst is used under a high partial pressure of O2, it exhibits a superior CO oxidation performance than metallic Ru catalysts [10,17]. Moreover, the performance of such catalysts can be greatly improved when stabilized or uniformly dispersed on the surface of a suitable support [18,19,20].
Dispersion is a critical step in furthering an effective reaction between the reactants [21]. Conventional methods of catalyst dispersion on support materials by wet impregnation often yield aggregated structures [22]. Polymers can be used in nanomaterial syntheses as stabilizers, surfactants or growth-directing agents [23,24] in which they control the particle aggregation, pore characteristics and in a catalysis context, the stability and poisoning resistance of the support [25]. Polyethylene glycol (PEG) is one of the most widely-used polymers in the design of heterogeneous catalysts [26] and can increase the interaction between the catalyst and the support by altering the physicochemical properties. Polymer additives need to be chosen carefully so as not to hinder the catalytic process and need to be removed by heat treatment prior to the experiment. Even though many surfactant materials are commercially available, PEG is an attractive choice as an additive since its oxidation products contain no nitrogen, sulfur or phosphorous thus precluding catalyst poisoning during heat treatment [27]. There are several reports describing the use of polymer stabilizers for the preparation of the catalysts [28,29,30], but very few detailed studies on the surfactant-induced morphological changes and subsequent correlations with activity are reported. A fuller understanding of such relationships provides a useful means to improve catalyst performance. In this study, the CO oxidation performance (both in wet and dry conditions) of a PEG-stabilized RuOx/γ-Al2O3 catalyst is compared with an un-stabilized equivalent. Detailed physical and chemical characterization of the materials has allowed us to begin to understand the connectivity between surfactant-mediated RuOx catalyst design and activity.

2. Experimental Section

2.1. Materials

Alumina (Al2O3) powder (Sigma-Aldrich, St. Louis, Missouri, USA), RuCl3·xH2O (Sigma-Aldrich), NH3 solution (Junsei Chemical Co. Ltd., Tokyo, Japan), tetraethyl orthosilicate (TEOS, Sigma-Aldrich), polyethylene glycol (PEG, average molecular weight 20,000 g/mol, Sigma-Aldrich) and ethyl alcohol (Daejung Chemical and Metals Co., Shiheung, Korea) were used as received.

2.2. Syntheses of Catalysts

The amount of 1 wt.% RuOx supported on mesoporous γ-Al2O3 (hereafter referred to as RAWOS) was prepared using the following homogeneous precipitation procedure. Firstly, a known quantity of RuCl3·xH2O (0.155 g) and TEOS (0.25 wt.%, also containing ethanol and water) solution were prepared and mixed (previously it has been suggested that the in situ formation of a minor amount of SiO2 could improve the hardening of the oxidation catalyst without affecting its performance [31]). The solution was reacted with 25 mL, 1 M NH3 solution (acting as a precipitating agent) at 75 °C. After 2 h, the required amount of Al2O3 powder (9.9 g irreducible support) was added and the mixture was stirred for a further 1 h. Following the reaction, the product was washed repeatedly with deionized water in order to remove the by-product and then heat-treated at 115 °C. The resulting powder was pressed into a pellet (approximately 8 ton weight for 1 cm diameter) and calcined at 650 °C for 24 h. In order to investigate the role of stabilizer/surfactant, a separate sample (hereafter referred to as RAWS) was prepared as above with the addition of a synthesis step in which PEG (0.5 g) was added prior to the addition of the NH3 solution. The calcination step converted amorphous Ru(OH)3 into RuOx and removed PEG completely. Unmodified γ-Al2O3 was also prepared as a reference sample (hereafter referred to as ALVIR). Following the calcination, each of the pellets were crushed and sieved to obtain 2–3 mm size granules.

2.3. Catalyst Characterization

The phase purity and crystallinity of the catalysts were studied by a powder X-ray diffractometer (XRD, D/Max Ultima IIIdiffractometer, Rigaku Corporation, Tokyo, Japan) equipped with monochromatic Cu Kα radiation (wavelength, λ = 0.154 nm) operated at 40 mA and 40 kV. The surface morphology was analyzed using field emission scanning electron microscope (FESEM, JEM 1200 EX II, JEOL, Tokyo, Japan) and transmission electron microscopy with EDX attachment (TEM, TECNAI F20, Philips Corp., Eindhoven, The Netherlands). Identification of the basic chemical functional groups (and quantification of CO2 during CO oxidation experiment) was performed by FTIR spectroscopy (IFS 66/S spectrometer, Bruker, Billerica, MA, USA). In addition, the surface of the catalysts was also characterized by using an X-ray photoelectron spectroscopy (XPS, ESCA 2000, VG Microtech, West Sussex, UK) with monochromatic Mg Kα X-ray radiation (1253.6 eV) operated at 13 kV and 15 mA as an excitation source. The Quantachrome software (version 2.11, Quantachrome Instruments, Boynton Beach, FL, USA) was used to determine the surface area and pore characteristics of the catalysts. Chemisorption measurements (temperature programmed reduction (TPR) experiments) were conducted using a gas sorption analyzer (Autosorb iQ, Quantachrome Instruments, Boynton Beach, FL, USA) to predict the catalyst dispersion. In this test, 100 mg of catalyst and a mixture of H2 and Ar (10%) were used. The samples were pretreated and the TPR profile was recorded from room temperature to 600 °C at a steady ramping.
Exactly 10 g of the catalyst prepared as above was loaded in a tubular reactor (diameter: 1.5 cm) and then fixed inside a furnace equipped with a temperature controller. The feed gas was prepared by mixing CO, oxygen and nitrogen. The concentration of CO was fixed at 2000 ppm (parts per million, volumetric), and the oxygen concentration was varied from 0.5 to 2.5 vol.% with the total flow rate kept at 1 L·min−1. The volume of the catalyst inside the reactor was 11.48 cm3, corresponding to a space velocity of 5226 h−1 at a feed gas flow rate of 1 L·min−1. All experiments were performed under isothermal conditions (the feed gases were introduced immediately after the required temperature was attained). The difference between the temperature measured at the catalyst using a thermocouple and that recorded by the temperature controller was negligible. The concentration of CO at the outlet was measured by using the FTIR spectrometer after 1 h of the reaction.

3. Results

3.1. Characterization

Figure 1 shows the FESEM micrographs of the RAWOS and RAWS catalysts. The RAWOS samples showed the presence of aggregated structures of RuOx nanomaterials inside and on the surface of the γ-Al2O3 support. By contrast, the PEG-stabilized RAWS sample exhibited a finger-like protrusion of RuOx on the surface of the γ-Al2O3. The TEM image of RAWOS sample (Figure 2a) clearly displayed the distinction between γ-Al2O3 (gray) and small size RuOx (black) which is non-uniform in shape and size. EDX analysis was also performed in the above locations, which confirmed the particular morphological feature was due to RuOx. At the same time, RAWS clearly showed the presence of rod-like structures with a length and width of ca. 200 and 75 nm, respectively (Figure 2b). Assemblies of nanorods like this were widespread throughout catalyst samples. The approximate elemental composition measured by EDX for the corresponding catalysts can be seen in the right side of the figures. The RAWOS catalyst contains 58.34% oxygen and 9.78% Ru, whereas RAWS contains 46.49% oxygen and 50.94% Ru (atomic percentage). The observed one dimensional (1D) growth found in RAWS is proposed to originate from the formation of micelles in PEG solution, which further directs the growth of the catalyst. As noted previously in the literature, the formation of 1D structure is achieved due to the effect of PEG acting as a capping and growth directing agent. The ordered chain structure of PEG (mainly arising from oxygen in the C-O-C chains) is anticipated to adsorb easily on a ruthenium-rich surface, coordinating with the ruthenium ions, forming PEG-Ru+3 complexes in the colloidal state and confining growth at specific crystal faces [32,33]. Subsequent neutralization with alkaline solution (ammonia) produces PEG-Ru(OH)3. Finally heat treatment at high temperature (650 °C) removes PEG and water which results in the ruthenium oxide nanomaterials. This process is shown schematically in Figure 3.
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Figure 1. The FESEM surface morphological images of RAWOS (a) and RAWS; (b) catalysts. (Abbreviations: RAWOS: RuOx/γ-Al2O3 without polymer stabilizer; RAWS: PEG stabilized RuOx/γ-Al2O3).
Figure 1. The FESEM surface morphological images of RAWOS (a) and RAWS; (b) catalysts. (Abbreviations: RAWOS: RuOx/γ-Al2O3 without polymer stabilizer; RAWS: PEG stabilized RuOx/γ-Al2O3).
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Figure 2. The TEM images of (a) RAWOS and (b) RAWS catalysts, and the EDX spectra of (c) RAWOS and (d) RAWS catalysts along with the elemental composition.
Figure 2. The TEM images of (a) RAWOS and (b) RAWS catalysts, and the EDX spectra of (c) RAWOS and (d) RAWS catalysts along with the elemental composition.
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Figure 3. Formation mechanism of 1-D RuOx in the presence of PEG.
Figure 3. Formation mechanism of 1-D RuOx in the presence of PEG.
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The phase and crystal structure of the ALVIR, RAWOS and RAWS catalysts were analyzed by using XRD and given in Figure S1. The diffraction pattern of the as-received alumina shows prominent diffraction peaks at 2θ = 36.7, 45.8 and 66.9° corresponding to the (311), (400) and (440) reflections of γ-Al2O3, respectively (cf. JCPDS card no. 00-010-0425). Commonly, commercial γ-Al2O3 is mesoporous with a higher surface area and is the most thermodynamically stable phase of alumina [34,35,36]. The XRD diffractograms of both the synthesized and heat-treated catalyst materials displayed identical peaks although reflections corresponding to RuOx could not be observed clearly, which may due to the inclusion of Ru atoms in the interstitial sites of alumina or it may simply due to the lesser amount of RuOx (1 wt.%) [37]. In case of the X-ray diffractometer employed in this work, it was found that the catalyst loading should be greater than 7 wt.% to clearly identify RuOx diffraction peaks and to calculate the lattice parameters.
The FTIR spectra of the ALVIR, RAWOS and RAWS catalysts are shown in Figure S2a–c, respectively. As-received alumina exhibited prominent bands at 550 cm−1 and 790 cm−1 corresponding to the Al ions in octahedral and tetrahedral surrounding (Al-O vibrations), respectively [38]. The band at 1635 cm−1 can be associated with physisorbed water (from exposure prior to analysis), and a broad peak between 3200 cm−1 and 3600 cm−1 indicates OH stretching exhibited by hydroxyl functional groups [39,40]. The FTIR spectra of the RAWOS and RAWS catalysts displayed similar peaks to those observed in spectra for ALVIR. Ru-O vibrations are expected to occur between 600 and 800 cm−1 and thus a distinction between Al-O and Ru-O bands could not be clearly made. Bands originating from the functional groups associated with PEG (the main C-O-C band at 1094 cm−1) in the RAWS sample were not observed, which implies that the PEG was removed by the heat treatment.
The RAWOS and RAWS supported catalysts were additionally characterized using XPS (Figure 4). The spectra were de-convoluted by using a Gauss-Laurentzian peak fitting program. The respective high resolution core level Al 2p, Ru 3d and Ru 3p spectra are given for the catalyst RAWOS (Figure 4a–c) and RAWS (Figure 4d–f). The binding energy values observed in the Al 2p spectra of both catalysts correspond to Al2O3 as expected [41]. Spectra also contained peaks corresponding to carbon (284.5 eV) and Ru 3d peaks typical for ruthenium oxides (286.2 and 286.0 eV) [42]. Since the Ru 3d and C 1s peaks are very close in terms of binding energy values, spectra in the Ru 3p binding energy region were recorded to clarify the ruthenium oxidation state and bonding environment. From the positions and relative intensity of the observed peaks, the RAWOS sample surface consisted of approximately 68 at.% Ru (IV) (typical of RuO2; 462.4 eV) and approximately 32 at.% RuO3 (465.0 eV) [42,43]. By comparison, Ru 3p peaks for the RAWS sample surface reflected an approximate composition of 62 at.% RuOx (i.e., higher oxides of Ru, where x = 3 mostly) at 464.3 eV and 38 at.% elemental Ru°, (461.8 eV) [42]. It has been reported that RuO3 is found in all of the surfaces of RuO2 and it plays a main role in the stability of RuO2 [42]. It is clearly seen that when the sample was prepared with a polymer stabilizer such as PEG (as is the case for the RAWS), formation of metallic Ru is induced through the reducing activity of the stabilizer [44].
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Figure 4. High resolution core level Al 2p, Ru 3d and Ru 3p spectra corresponding to RAWOS (a–c) and RAWS (d–f) catalysts.
Figure 4. High resolution core level Al 2p, Ru 3d and Ru 3p spectra corresponding to RAWOS (a–c) and RAWS (d–f) catalysts.
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The adsorption capacity of gas molecules within the pores of the catalyst is an important step towards understanding the catalyst reaction. This can be determined from the surface and pore-characteristics of the catalyst. Figure 5 shows the N2 adsorption-desorption isotherm (Figure 5a–c) and the multipoint Brunauer-Emmet-Teller (BET) plots (Figure 5d–f) for the ALVIR, RAWOS and RAWS materials, respectively. From the sorption profiles it is evident that the catalysts exhibit mesoporous type IV isotherm behavior in which the intake of adsorbate increases at high pressure. The pore volume and pore radius of the catalysts during adsorption and desorption process calculated by Barrett-Joyner-Halenda (BJH) method are listed in Table 1, which confirmed the standard values of the pore size (1.5–100 nm) reported [45]. The linearity of the data (indicating a strong interaction of the ruthenium oxide catalyst with N2) in the relative pressure (P/P0) range of 0.0–0.3 reinforces the suitability of applying the BET model in determining the specific surface area of the catalysts. The BET surface area is generally used for practical purposes. The ALVIR, RAWOS and RAWS catalysts exhibit BET surface area values of ca. 112.2, 138.3 and 128.1 m2·g−1, respectively. From a comparison of the RAWS and RAWOS sorption isotherm results, the addition of the polymer stabilizer apparently leads to an increase in the pore volume and pore radius and a decrease in the surface area values by 10.2 m2·g−1. A similar trend has been reported previously for Ni-Al2O3 catalyst stabilized by cetyltrimethylammonium bromide [30].
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Figure 5. Nitrogen adsorption-desorption isotherms (a)–(c) and the multipoint BET plots; (d)–(f) corresponding to ALVIR, RAWOS and RAWS catalysts.
Figure 5. Nitrogen adsorption-desorption isotherms (a)–(c) and the multipoint BET plots; (d)–(f) corresponding to ALVIR, RAWOS and RAWS catalysts.
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Table
Table 1. Physisorption results of the catalysts measured by Barrett-Joyner-Halenda (BJH) method.
Table 1. Physisorption results of the catalysts measured by Barrett-Joyner-Halenda (BJH) method.
Catalyst NameProcessSurface Area (m2/g)Pore Volume (cc/g)Pore Radius (Mode Dv(r)) (Å)
ALVIRAdsorption102.90.232230.72
Desorption140.70.248028.18
RAWOSAdsorption120.50.247530.58
Desorption168.70.269424.40
RAWSAdsorption119.00.253230.76
Desorption164.80.272324.54

3.2. CO Oxidation Performance of the Catalysts

Oxygen concentration and temperature were varied in the range of 0.5–2.5 vol.% and 50–250 °C, respectively, in a series of CO oxidation experiments. The inlet concentration of CO was fixed at 2000 ppm. The conversion of CO into CO2 obtained with as received γ-Al2O3 (ALVIR) under steady state conditions showed a maximum of 5.6% at reactor temperature of 175 °C. The CO conversion percentages using the RAWOS and RAWS catalyst materials are shown in Figure 6a–c for oxygen concentrations of 0.5. 1.5 and 2.5 vol.%. The plots clearly demonstrate a gradual increase in CO conversion from <10% at 50 °C to 100% at 200 °C. Generally, varying the oxygen content at low temperature did not affect the overall conversion process significantly but its influence at high temperature is clear. The RAWOS catalyst exhibits substantial activity above 100 °C. Similar behavior was observed on repeating the oxidation experiments with the PEG-stabilized RAWS catalyst, but the CO conversion percentage at each experimental temperature was notably higher. Moreover, total conversion was achieved at 175 °C as compared to 200 °C observed for the equivalent RAWOS catalyst. At low temperature (50 °C and 75 °C), the difference between the materials is almost negligible but when the temperature is increased, a remarkable difference can be noted. An increase in the CO conversion efficiency of about 33% by RAWS catalyst was observed in experiments at 125 °C with an O2 concentration of 1.5%. Above and below this temperature, a gradual decrease in the conversion efficiency can be noted with a slight variation depending on the oxygen concentration. The stability of the catalysts was also confirmed by conducting the experiments continuously for 7 h at 125 °C. These extended experiments showed the repeatability of the performance observed above without any significant change.
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Figure 6. The CO oxidation performance of RAWOS and RAWS catalysts with different concentrations of oxygen. (a) 0.5 vol.%, (b) 1.5 vol.% and (c) 2.5 vol.%.
Figure 6. The CO oxidation performance of RAWOS and RAWS catalysts with different concentrations of oxygen. (a) 0.5 vol.%, (b) 1.5 vol.% and (c) 2.5 vol.%.
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In order to investigate the performance of the catalysts under real working conditions, water vapor was added to the reactant gas (i.e., CO + H2O + O2). The experiments were thus performed in the presence of 2.5% and 5% water (by volume) at different temperature. The results of these CO oxidation experiments are represented in Figure 7. The CO conversion efficiency increased depending upon the temperature. For a water content of 2.5%, full conversion was achieved at 275 °C for the RAWOS catalyst. By contrast, the rod type RAWS catalysts exhibited 100% CO oxidation at a reduced temperature of 225 °C (Figure 7a). Increasing the water content from 2.5% to 5% resulted in the shift of temperature to 300 °C for the RAWOS material and 250 °C for the RAWS catalyst, respectively (Figure 7b). In addition, it is very clear that at every reaction temperature, the RAWS catalyst showed an improved conversion performance over the RAWOS equivalent. As compared to the results obtained under dry conditions, the increase in the effective temperature required for full conversion can be understood in terms of the competition between CO and H2O adsorption in the reactive sites of the catalysts. This is also consistent with the finding that pre-oxidized RuOx catalysts are very active in dry conditions, similar to the phenomena exhibited by oxides of copper and cobalt [46,47].
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Figure 7. Effect of (a) 2.5 vol.% and (b) 5 vol.% water content on the CO oxidation performance using RAWS and RAWOS catalyst. The inlet oxygen concentration was fixed at 1.5 vol.%.
Figure 7. Effect of (a) 2.5 vol.% and (b) 5 vol.% water content on the CO oxidation performance using RAWS and RAWOS catalyst. The inlet oxygen concentration was fixed at 1.5 vol.%.
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4. Discussion

The reason for the enhancement of the catalytic activity in the PEG-stabilized materials results from a combination of factors. First, the increase in the pore volume and pore size would appear to be the dominant effect (Table 1) [30]. Second, the stoichiometric and non-stoichiometric ruthenium oxides (and hence variable ruthenium oxidation states) states might be expected to contribute to the catalyst activity as is seen, for example, for MnOx (where x ≤ 2) [48]. Arguments in the literature suggest that metallic Ru, as observed in the RAWS material (and as found by XPS), forms bonds with adsorbed ad-layers of oxygen (as a transient surface oxide) in situ during CO oxidation and is catalytically more active below 500 K [49,50,51,52]. Third, metallic catalysts such as Pd and Rh on oxide supports show structure-sensitive (size) catalytic activity [46] and favor towards high CO adsorption. Zhou et al., have reported that an increase in the CO oxidation capability of Pt nanowires over zero dimensional Pt nanoparticles is due to the large crystal facets and a small density of defect sites [53]. This means that the synergistic effect rendered by rod-structured RuOx (as a manifestation of shape dependent catalytic activity) also partly explain such improvements [54]. It is reported that the difference in the geometry of nanomaterials occurs due to the changes in the surface atomic arrangement, thus exhibiting different electronic structures [55]. The binding strength between the catalyst surface and the adsorbed species (interaction) depends on such atomic arrangements (defect structures), which in turn influences the catalytic activity and selectivity [28,56,57]. The open coordination sites rendered by the edge and corner atoms [58] usually found in tetrahedral nanomaterials (in case of this work, Ru exhibits rutile-type structure with Ru atoms located in the corner) might significantly affect adsorption energy (activation energy) and bond enthalpy [59]. In addition, the flat sides of RuOx containing large number of surface atoms would result in an increase in the contact area with the catalyst support, which can provide additional sites for the adsorption of reactant molecules [60].
Finally, the catalyst dispersion engendered in the PEG-stabilized catalysts contributes significantly to catalyst activity. Figure 8 shows the TPR profiles of the RAWOS and RAWS catalysts. The H2 consumption profiles exhibit a number of maxima at different temperatures, implying the existence of various Ru species on γ-Al2O3. The H2-TPR for RAWOS shows reduction peaks between 100–300 °C. The narrow peaks at ca. 168 °C and 225 °C (and 266 °C) correspond to the reduction of RuO3 and RuO2 [61,62]. Low temperature peak at 110 °C refers to the formation of ruthenium from tiny RuO2 particles (Figure 8a). By comparison, the RAWS catalyst exhibited a smooth and well defined ruthenium reduction peak with large peak area at a lower temperature (95.5 °C). The high temperature peak at 522 °C is the result of the reduction of the mesoporous γ-Al2O3 support [63,64] and the peak observed as a shoulder at 331 °C should be due to the reduction of large RuO2 nanorod structures. Comparing the peak areas, the amount of H2 gas consumed by the RAWS catalyst is higher than the un-stabilized catalyst and the reduction events are shifted consistently to lower temperature (by between 35–170 °C). One might infer therefore that since the rod-structured catalyst is well dispersed the formation of oxygen vacancies throughout the RuOx is facilitated via the facile interaction of gaseous species, which ultimately leads to an enhancement of CO oxidation. Such a size and shape dependent reduction behavior was also reported for CeO2 catalysts in the literature [63].
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Figure 8. The H2 consumption (TPR) profiles of the RAWOS (a) and RAWS (b) catalysts.
Figure 8. The H2 consumption (TPR) profiles of the RAWOS (a) and RAWS (b) catalysts.
Applsci 05 00344 g008

5. Conclusions

The preparation of nano-sized RuOx catalysts on mesoporous γ-Al2O3 support was achieved following a chemical co-precipitation route. Two predominant types of catalyst nanomaterial were synthesized; aggregated spheres and dispersed rods. The addition of PEG surfactant was essential in achieving the latter catalyst morphology. Subsequent characterization showed that polymeric surfactant used for stabilization could be removed by heat treatment and did not lead to catalyst poisoning. The surfactant played the principal role in controlling the morphology and pore characteristics of the catalysts. It was observed that the PEG-stabilized rod type nanomaterials showed superior conversion over un-stabilized spherical-shaped materials in the catalytic oxidation of CO. The use of PEG in mediating the shape, size, surface structure and transition metal oxidation state is crucial in tailoring catalyst performance.

Supplementary Materials

The XRD and FTIR spectrum of the ALVIR, RAWOS and RAWS catalysts are provided.

Acknowledgments

This research was supported by Basic Science Research Program through the National Research Foundation of Korea (NRF) funded by the Ministry of Science, ICT and future Planning (Grant No. 2013R1A2A2A01067961).

Author Contributions

Antony Ananth performed the experimental work and analyzed the data; Duncan H. Gregory helped prepare the first draft of the manuscript and provided advice on the discussion; Young Sun Mok supervised all the study and participated in the interpretation of the results.

Conflicts of Interest

The authors declare no conflict of interest.

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MDPI and ACS Style

Ananth, A.; Gregory, D.H.; Mok, Y.S. Synthesis, Characterization and Shape-Dependent Catalytic CO Oxidation Performance of Ruthenium Oxide Nanomaterials: Influence of Polymer Surfactant. Appl. Sci. 2015, 5, 344-358. https://doi.org/10.3390/app5030344

AMA Style

Ananth A, Gregory DH, Mok YS. Synthesis, Characterization and Shape-Dependent Catalytic CO Oxidation Performance of Ruthenium Oxide Nanomaterials: Influence of Polymer Surfactant. Applied Sciences. 2015; 5(3):344-358. https://doi.org/10.3390/app5030344

Chicago/Turabian Style

Ananth, Antony, Duncan H. Gregory, and Young Sun Mok. 2015. "Synthesis, Characterization and Shape-Dependent Catalytic CO Oxidation Performance of Ruthenium Oxide Nanomaterials: Influence of Polymer Surfactant" Applied Sciences 5, no. 3: 344-358. https://doi.org/10.3390/app5030344

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