Ruthenium Catalyst Supported on Multi-Walled Carbon Nanotubes for CO Oxidation


This work proposes the synthesis of the 5%wt Ru on MWCNT catalyst and the influence of feed rate and testing variables for low-temperature oxidation affecting the CO2 yield. Morphology and incorporation of the nanoparticles in carbon nanotubes were investigated by specific surface area (BET method); thermogravimetric analyses (TGA); X-ray diffraction; Raman spectroscopy, transmission electron microscopy (TEM) and XPS. The conversions of CO and O2 were mostly 100% in groups C1 and C2 (temperature between 200 and 500°C with low WHSV). In order to assess the effect of mass on catalytic activity, condition C3 was tested at even lower temperatures. In the tested catalyst, high activity (100% CO and O2 conversion) was observed, keeping it active under reaction conditions, suggesting oxi-reduction of the RuO2 at surface without affecting the MWCNT but Lewis acid influencing the CO2 yield.

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Kozonoe, C. , Giudici, R. and Schmal, M. (2021) Ruthenium Catalyst Supported on Multi-Walled Carbon Nanotubes for CO Oxidation. Modern Research in Catalysis, 10, 73-91. doi: 10.4236/mrc.2021.103005.

1. Introduction

Gaseous pollutants are released into the atmosphere, such as carbon monoxide (CO), causing great damage to the environment, and are known to stay in the Earth’s atmosphere for a long time [1].

There are several studies concerning the CO oxidation of different metals and supports, as reported in the review by Lui and Corma [2]. In fact, the catalytic oxidation of CO is the most effective process, as reported in the literature [3] [4] [5] [6] [7], using predominantly alumina-support and noble metals (Pt, Ru, Rh, and Pd) [8] - [13] and zeolite-supported platinum [13] [14] [15]. The metal-support interface on oxides and mixed oxides has also demonstrated great effect on the CO oxidation. Mixed oxide cobalt ferrite (CoFe2O4) nanoparticles exhibited also high CO conversion and good stability [16]. Liu et al. [17] studied the CO oxidation of the Pd doping in Ce-Zr oxides as one of the most efficient.

However, among the noble metal catalysts, ruthenium has had an unusual catalytic behavior for CO oxidation [18] - [27]. The Ru single crystal was less active among noble metals under ultrahigh vacuum conditions [18], but highly active under oxidizing and high-pressure conditions [19]. Studies of supported Ru NP catalysts for this reaction have only been sporadically reported [24] [25] [26] [27]. Joo et al. [28] studied the influence of crystal sizes of ruthenium nanoparticles supported on alumina for the CO oxidation activity, which increased with increasing particle sizes. In addition, Soliman [29] studied optimal conditions of the CO oxidation and the influence of the reaction conditions on the nanostructure of the catalyst.

In fact, oxide supports are not inert materials due to the presence of hydroxyls and large pore sizes. Unlike, the carbon nanotubes (CNT) are inert materials and have been proposed as supports for different reactions, due to the high surface area, allowing the insertion or deposition of the nano-metals or nano metal-oxides, favoring the dispersion and the accessibility of the molecules on the metallic particles. Basically, the nanotube structures have covalent C-C bonds formed by layers of graphite. These carbon nanostructures have also uniform pore size distribution, and are resistant at high temperatures. Multi-walled nanotubes (MWCNT) have been used for greatly minimizing the limitations imposed by mass transfer.

However, the synthesized carbon nanotubes need pretreatment for anchoring metallic sites, promoting higher dispersion of the metallic particles [30]. Zeng et al. [31] found that the hydrophilic functional groups of hydroxyl and carboxyl are favorable for the insertion of the metal oxide into the tubes of the MWCNTs. Kozonoe et al. [32] synthesized recently the Ni@MWCNT/Ce catalyst and evaluated the influence of testing variables on reaction performance and nanostructure of the catalyst.

The objective of this work is to synthesize ruthenium oxide NP on multi-walled carbon nanotubes (Nanocyl), the distribution and sizes of nano particles, as well as the nature of both materials on the external walls and the influence of reaction conditions for the CO oxidation on the activity and CO2 yield, the effect of the reaction on the MWCNT and Ru NP structure and size and surface mechanism.

2. Materials and Methods

2.1. Synthesis of Ruthenium Nanoparticles Supported on Carbon Nanotubes

Initially, 0.11 g of Ruthenium (Ruthenium (III) chloride hydrate) was prepared. 3 ml of water was added by dripping to 1 g of multi-walled carbon nanotubes (purchased as Nanocyl-3100). Then, 1.32 ml of ethylene glycol was added to the carbon nanotube and soaked. Finally, the ruthenium solution in ethylene glycol solution was added, and the paste formed was dried under vacuum during three days. The calcination was performed under airflow at 100 ml∙min−1, raising the temperature from 30˚C to 350˚C at 10˚C/min, and held for 2 hours. The reduction was performed with hydrogen flow at 100 ml∙min−1 from 30˚C to 400˚C, at 10˚C/min, and kept for 2 h. The catalyst was denoted as 5%Ru/MWCNT.

We also prepared and functionalized CNT sample that was impregnated with the same metallic precursors, according to the procedure reported previously [32].

2.2 Catalyst Characterization

The specific surface area of the catalyst was determined using nitrogen physisorption at −196˚C in the NOVA 1200 equipment (Surface Area & Pore Size Analyzer) of Quantachrome Instruments. Prior to the physisorption analysis, the materials were pretreated under vacuum at 200˚C for 17 h. The specific surface area was determined using the BET methodology.

Transmission Electronic Microscopy (TEM) analyses were performed in a JEOL JEM 2100 Microscope, with maximum acceleration voltage 200 kV, and resolution of 0.23 nm at the point and 0.14 nm on the network, with maximum magnification of 1,500,000 times.

X-ray diffraction (XRD) analyses were performed in a Rigaku equipment with an acquisition in the radiation incidence angle range of 2˚ < 2θ < 90˚. Identification phases in the sample were obtained using the PDF (Powder Diffraction File PDF2-2003) datasheets as database through the Search-Match program, comparing to their positions in the experimental data.

The Raman spectra were acquired in the range of 100 - 3500 cm−1 with a Renishaw in Via confocal Raman microscope in backscattering geometry equipped with a CCD detector (−70˚C) and HeNe laser supplying the photon at 532 nm. The laser excitation power was kept below 10 mW on the sample surface to minimize the local heating. The total acquisition time was 300s. All the spectra of the samples after reaction were recorded under identical conditions at room temperature.

The surface of the catalysts was studied using X-ray photoelectron spectroscopy (XPS). X-ray photoelectron spectra were recorded on a Leybold-Heraeus LHS 10 spectrometer using a non-monochromatized Al-K-α source (1486.7 eV).

Thermal analyses of the samples before and after reaction were performed on a DTG-60H Shimadzu with a TG-DTG simultaneous analyses accessory. The measurements were conducted under a flow of nitrogen/oxygen mixture (55 mL/min N2/8 mL/min O2) from 25 to 1000˚C at a heating rate of 10˚C/min.

2.3. Activity Tests

The tests were performed in a Microactivity-Effi (PID company) with a Hastelloy X tubular reactor of 9.1 mm diameter and length of 370 mm at atmospheric pressure, varying the temperature range and weight hourly space velocities (WHSV). The feed flows downwards through the catalytic bed and a condenser before running the test. The temperature was measured with a thermocouple and a PID controller. The total mass was 100 mg (20 mg of catalyst and 80 mg of carbide). Prior, the catalyst was reduced in-situ with pure H2 flow (99.999%, Air Products) for 120 min, at 10˚C∙min−1 up to 450˚C. After purging with N2 flow, the gas was switched to the feed mixture (CO2:O2:N2). The exit gases were measured online in a gas chromatograph (GC2010 Plus Shimadzu) with a Carboxen 1010 plot column.

3. Results

3.1. Specific Surface Area (BET Method)

The specific surface area of the catalyst Ru/MWCNT was 285 m2/g, and the pore volume 1.33 cm3/g. The surface area of the functionalized sample 5% Ru/MWCNTf (functionalized) was 371.8 m2/g. The isotherms of the Nanocyl sample and the corresponding pore size distribution are shown in Figure 1. It displays a type IV adsorption curve with hysteresis, which is associated with the development of a pore network. The MWCNTf displayed similar profiles (not shown).

The pore size distribution curves suggest various types of pore sizes. The small pores around 4 nm are aggregated pores of CNTs. Regarding the pore size distribution, mostly can be considered bimodal (micro and mesopores) types, which agreed with Ma et al. [30].

3.2. Transmission Electron Microscopy (TEM)

The images of the transmission electron microscopy (TEM) in Figure 2 show that the impregnation of ruthenium nanoparticles over carbon nanotubes was well succeeded, using this preparation method, as proposed in this work.

Figure 1. Nitrogen adsorption-desorption isotherms, the corresponding pore size distribution of the Ru/MWCNT catalyst.

Noteworthy is that the depositions of Ru particles (Figures A and B) are well dispersed on the external wall of the CNT.

In fact, transmission electron microscopic analyses generate two-dimensional images, allowing determining the location of the particles in some selected regions.

We calculated the average diameter of the nanotubes and particles from the images using the ImageJ software and obtained the particle size distribution from a representative group of 12 images.

The average diameter for the Ru located at the external wall of the carbon nanotubes was 2.3 ± 0.6 nm, very close to the calculated by the X-ray diffraction, XRD (1.7 nm).

Figure 3 displays the average external and internal diameter of the carbon nanotubes, 13.4 ± 2.7 and 6.8 ± 1.6 nm, respectively. The sample space presents 32 tubes.

Figure 2. Images of transmission electron microscopy (TEM) of the carbon nanotubes decorated with Ru (5%Ru/MWCNT) ((a), (b)).

Figure 3. The capture of a carbon nanotube with external impregnation with 50 nm resolution.

3.3. X-Ray Analyses (XRD)

Figure 4 shows the X-ray diffractograms for the MWCNT and of the catalyst. According to the literature [33], the MWCNT present characteristic peaks at 2θ ≈ 26.2˚, 43.0˚, 55.0˚, and 77.0˚, which represent, respectively, the (002), (100), (004) and (110) planes. The first peak indicates the presence of the effect of different overlapping graphene sheets, in a concentric mode [34], characteristic of multi-layered carbon nanotubes.

The profile obtained for MWCNT (Figure 4) showed the peaks of the planes (002) and (100) at 2θ equal to 26.05˚ and 43.03˚, respectively. In addition, such peaks are broad, characteristic of amorphous materials, as expected for carbon nanotubes.

The diffractogram of the catalyst with ruthenium showed the presence of two peaks with low intensity at 34.8˚ and 54.8˚, which are assigned to RuO2 (Ref. code 40-1290 and overlap identified by “*” in Figure 5) present at the external surface of the MWCNT, in agreement with the images of electron transmission microscopy analyses. For comparison, the XRD of the functionalized MWCNTf diffractogram is presented in supplementary information S1.

The crystallite size of ruthenium was calculated using Scherrer’s equation [35]. For this, the peak of 34.8˚ was used, which resulted in a crystallite size of 1.7 nm in agreement with TEM result of 2.3 ± 0.6 nm. Rojas et al. [36] found metallic Ru particles of 2.5 nm on the Ru/MWCNT sample.

3.4. Thermogravimetric Analyses (TGA)

The thermogravimetric analyses (TGA) and their derivate (DTG) profiles of the Ru/MWCNT catalysts are shown in Figure 6, presenting the weight loss of the pure carbon nanotube (MWCNT) and of the catalyst (Ru/MWCNT).

Figure 4. XRD of the carbon nanotubes (MWCNT) and the carbon nanotubes 5% Ru/MWCNT catalyst.

Figure 5. Diffractogram for the carbon nanotube impregnated with ruthenium externally.

Figure 6. TGA and DTA curve of the MWCNT sample (a) and 5% Ru/MWCNT catalyst (b).

The TGA analysis (red curve) shows that the support (MWCNT) and the catalyst (5% Ru/MWCNT) present slightly different profiles. For the support, the mass loss was approximately 84% at 515˚C, and for the catalyst, was 92% at approximately 600˚C, which indicates decomposition of the carbonyl and carboxylic groups present in carbon nanotubes, in accordance with Saleh et al. [37].

3.5. Raman Spectroscopy

Raman spectroscopic analyses provide information about the chemical composition and crystalline structure of the sample [38]. Figure 7 shows the spectra of the carbon nanotube and the catalyst. The spectrum of the MWCNT showed the peaks at bands D (≈1340 cm−1), G (≈1572 cm−1), 2D (≈2663 cm−1), G + D (≈2919 cm−1), in accordance with Zdrojek et al. [39] and noise bands between 100 and

Figure 7. Raman spectra take from pure carbon nanotubes and the MWCNT covered with Ru (5% Ru/MWCNT) at λ = 532 nm.

200 cm−1, as observed by Ivanova et al. [40]. However, the spectrum of the catalyst sample showed extra peaks, which could be correlated to impurities (≈2330 cm−1, 800 cm−1 and 270 cm−1).

The band G (graphite) corresponds to the vibrations of the sp2 bonds between the carbons in the same plane and the band D to the disorder in the carbon structure, that is, the sp3 bonds between the carbons. The ratio between the areas of these peaks (ID/IG) allows determining the quality of carbon nanotubes [41], representing the density of structural defects. The higher the ratio, the more defects (sp3 connections) are present in relation to the expected (sp2 connections). The ratio of the pure support was 1.98.

This ratio increased after the addition of ruthenium (2.80). In fact, it indicates that there is an exchange of double bond for single bond in the carbons, with the formation of new covalent bonds. Figure 7 shows the peaks in the region at lower wavenumbers, indicating the presence of the metal oxide, probably ruthenium oxide, RuO2 (set of 2 small peaks, between 510 and 1300 cm−1) as indicated in the figure and in accordance with the literature [42]. In fact, RuO2 is probably the main oxide present at the external surface of the MWCNT. Literature reported different oxidation states of the Ru, but in particular the Ru+4 and Ru+8, besides other oxidation states that were reported in literature. For comparison, the Raman spectrum of the functionalized MWCNTf is also presented in supplementary information S1.

3.6. X-Ray Spectroscopy (XPS) of Ru/MWCNT

The XPS analyses were performed for identifying the oxidation state of ruthenium oxide deposited on the outer surface of the CNT, and also identifying the functional groups of the MWCNT. All binding energies were corrected, referencing the C1s (284.6 eV) peak of the contamination carbon as an internal standard. The XPS experiments were obtained for the functionalized MWCNT with the same content of 5%Ru. The XPS results are important to explain the presence of the RuO2 at the surface, not well seen in the XRD and Raman spectra. In fact, Figure 8(a) shows the screening spectrum of carbon, ruthenium and have oxygen.

Figure 8(b) shows the deconvolution of C1s peak. Results showed graphitic carbon at 284.3 eV [41]. Peaks at 284.5 and 290.5 eV are assigned to the carbon atoms (C-C) attached to groups containing oxygen (C=O) in their structure [43]. The electronic transition of orbitals π → π* was associated with the peak at 290.5 eV. These results indicate the external surface and also that the graphite layers retained their original structure [28] [31].

The spectrum the Ru 3d is characterized by a pair corresponding to the 5/2 and 3/2 spin-orbit components located at 281.4 and 285.6 eV, respectively (not

Figure 8. XPS spectra of the Ru/MWCNTt (a) screening, (b) Carbon C and (c) Oxygen O1s.

shown). Figure 8(c) displays the O 1s core level spectrum of the RuO2 on distinct maxima located at 530.1 eV, associated with oxygen adsorbed on the surface and 532.0, 532.8 and 534.0 eV, assigned carboxylic and hydroxyl groups. These peaks were related to the metallic oxides on the external surface of the CNTs.

3.7. Catalytic Activity

The catalyst (5% Ru/MWCNT) was tested in the CO oxidation reaction, for different conditions (3 groups), as presented in Table 1, to show the influence of temperature and space velocity. The conversion and selectivity results are presented in this table and illustrated in Figure 9. Each experiment was carried out in triplicate with the same sample and conditions, and constant mass.

Tests for condition C3 were obtained at WHSV 13,285 (mL/min.g) and mass of 20 mg, consequently, low contact time. The CO and O2 conversions with temperatures between 50 and 270˚C are displayed in Figure 9. In fact, the conversions of CO and O2 increased, from 50˚C, reaching the maximum conversions of 75% and 100%, respectively, at 150˚C, but the selectivity of CO2 was around 85%.

The results for condition C1, for lower space velocity (WHSV) 2000 (mL/min∙g)

Table 1. Conversion and selectivity results for different experimental conditions of the CO oxidation using 5%Ru/MWCNT catalyst.

Figure 9. Conversions of CO and O2, selectivity and yield of CO2 for the 5%Ru/MWCNT catalyst in the evaluation of the effects of the space velocity and temperature.

and CO:O2 = 1:0.5, and temperatures between 300˚C and 500˚C, showed conversions of carbon monoxide 100%, and of O2 around 95%. However, the CO2 yield was higher than 100%.

Conditions C2 were tested, diluting the reagents at the feed entrance (CO:O2:N2 = 1:0.47:5.91), by increasing the volume of the inert gas N2 and the space velocity of 2657 mL/min.g, and increasing the temperature from 200˚C to 400˚C. The carbon monoxide and O2 reached maximum conversions of 100%, suggesting total oxidation of CO; however, the CO2 selectivity was 88%.

We calculated the yield, using equation: Y(j) = X(CO) × S(j), and results are shown in Figure 9(d), with increasing conversion. As shown yield increased linearly with the conversion.

4. Discussion

In fact, these results may indicate the concomitant occurrence of reactions. In experiments C1 occurred the Bourdouard reaction with the formation of Carbon and CO2, besides the partial oxidation of C formed at higher temperature. Under this temperature range without combustion of the CNT, as evidenced in the TGA and DTG results in Figure 6 or partial decomposition of the carbon support:

2CO C + CO 2 (1)

C + O 2 CO 2 (2)

Noteworthy are the experiments C3, showing that between 50˚C and 150˚C at a space velocity 13,285 mL/min.g, the conversion of O2 is higher than of CO with simultaneous CO2 formation, indicating that besides the CO oxidation it consumes more oxygen for the oxidation of RuO2 to higher oxidation state. However, between 150˚C and 270˚C, the oxygen conversion is 100% while the CO2 selectivity is lower, varying from 84% to 88%, besides higher conversion of CO, reaching 75%, which suggests the reduction of RuO2 to metallic Ru0, with simultaneous formation of carbonate as shown below. So, there is a simultaneous reduction and oxidation process during the reaction, noted on experiments C1 and C2. For higher temperatures, the CNT is partially decomposed or oxidized.

In fact, these experiments suggest that CO probably reduces the RuO2 in the metallic Ru or form carbonate according to the literature [44]:

RuO 2 + CO Ru 0 + CO 3 (3)

RuO 2 + CO Ru 2 CO 3 C 3 O 9 Ru 2 (4)

In conclusion, these results evidenced high performance like the reducible oxide supports and depend mainly on the distribution of particle sizes, but not on their sizes. The selectivity of CO2 depends on the temperature range and on the oxidative-reductive cycle of the metal oxide-metal. For the MWCNT support we found particle sizes of Ru oxide around 2.3 nm, which resulted in very high CO and O2 conversions, but influencing also the CO2 selectivity.

Liu et al. [4] studied the CO oxidation on Pd-Ce0.8Zr0.2O2 (mixed oxide) with Pd that presented the high activity and complete CO conversion at 110˚C. Due to the metal−support interface interaction with oxide support, they claimed that the introduction of Pd promoted the formation of oxygen vacancy. Authors suggested that the CO molecule directly reacts with a surface O atom neighboring the Pd dopant, leading to the formation of CO2 and a surface O vacancy, without any activation energy. Ananth et al. [43] studied the CO oxidation on RuO2/Al2O3 catalyst, and showed complete CO oxidation at 200˚C, 225˚C, and 300˚C, similar to these results obtained for the same temperature range and at space velocity between 2000 and 2657 (mL/min.g). Therefore, it can be attributed to the high distribution and dispersion of metal oxide over an MWCNT, due to the high surface area, which influences the CO2 selectivity. In fact, condition C3 showed for 74.8% CO conversion and 100% oxygen conversion at 150˚C, and 84.5% CO2 selectivity (Table 1).

The CO oxidation activity depends on the surface property, high surface areas, and mesoporous structure of the catalyst. Park et al. [45] observed that the H2 pretreatment of meso-RuO2 results in the collapse of the mesostructure and a change RuO2 phase, as discussed above, which corroborates our results. The catalytic activity at low temperature is high for Ru/MWCNT, which may also be attributed to the high distribution of RuO2-based catalysts anchored on the MWCNT due to the high surface area 285 m2/g.

According to Joo et al. [28] the size of Ru nanoparticles affects the CO oxidation, and with increasing particle size the activity. The particle sizes of this work are of the order of 2.3 nm and showed high activity. They observed for Ru/SiO2 for 3 and 5% particle sizes between 2 and 6 nm and energy of activations of 22.2 and 22.5 kcal/mol, suggesting a low barrier, which increases the activity in the presence of Ru NP.

The activity can be determined for the half-time reaction of CO and oxygen conversion. In Figure 9 we observe the temperature for 50% conversion of CO and O2 are 120˚C and 80˚C, respectively, which compared to Reddy et al. [46], who observed for the copper catalysts supported on alumina the same temperature around 120˚C, for a CO conversion around 60%. The light-off temperature of the Ru catalyst around 110˚C - 120˚C is also in good agreement with the Ru on Al2O3.

However, there may occur structural changes due to the reaction. Joo et al. [28] showed through in situ spectroscopic analyses the as-prepared metallic Ru nanoparticle transformed into core-shell structure (Ru@RuO2) under reaction conditions, and the fraction of RuO2 overlayer was related to the particle size. Therefore, the size-dependent redox properties of Ru nanoparticles may account the CO oxidation.

4.1. Thermogravimetric Analysis of Spent Catalyst

The thermogravimetric analysis (TGA) was performed after reaction in air atmosphere (Figure 10). Noteworthy is that the profile shows gain of mass from 250˚C up to 700˚C, and the DTG profile shows a maximum peak at 320˚C, decreasing then up to 750˚C, and afterwards increases without mass alteration. It evidences an oxidation step of the metallic particles starting at 450˚C up to 700˚C. According to these results, the mass gain is suggested to be attributed to the carbon formation, and principally to the oxidation of Ru species [11]. These last results may explain the phase transformation without decomposition of the CNT.

The thermogravimetric analysis (TGA and DTA) results indicate between 200˚C and 400˚C the reduction besides the oxidation of RuO2 to RuO4 due to the gain of mass, as shown in Figure 9, that is:

RuO 2 + O 2 RuO 4 (5)

In fact, it supports the original hypothesis of spectroscopic analyses that the metallic Ru nanoparticle are transformed into core-shell structure (Ru@RuO2) under reaction conditions, according to Joo et al. [28].

Figure 10. TGA and DTG curves of the Ru/MWCNT catalyst after reaction.

Moreover, Figure 10 shows gain of mass between 450˚C and 720˚C and DTA profile evidence transformation of phases attributed mainly the oxidation of RuO2 with a gain of mass to RuO4, in good agreement with TGA and DTA results of the original catalyst in Figure 6(b) and in accordance with the XPS results. The O1s core level spectrum of the RuO2 displays oxygen adsorbed on the surface, which is associated with oxygen from Ruthenium oxides. There are no references reported in the literature concerning this behavior.

4.2. Reaction Mechanism

According to the literature [45] authors suggested that the mechanism of CO oxidation on the RuO2 surface is explained by the adsorption and reaction of atomic oxygen species on the coordinative unsaturated Ru atoms and bridge position surface oxygen atoms as verified by Mars-van Krevelan.

Therefore, we propose a reaction mechanism that follows the scheme presented below. In the first stage the RuO2 present as nanoparticles can be reduced in the presence of CO molecule, with the formation of Ru0 metallic. Besides this RuO2 can also be reduced with the formation of a carbonate specie ( Ru 2 CO 3 ) and in sequence to the formation of Ruthenium carbonate (C3O9Ru2) that is inert, but can be decomposed. Then the metallic Ru0 is oxidized regenerating the RuO2, which completes the oxi-reduction stage. However, the MWCNT present OH hydroxyls as evidenced by XPS, which can combine with the carbonate and formation of CO 3 + OH HCO 3 + O , releasing O at the surface of the CNT and react with CO to form CO2, which was observed in all experiments, indicating higher yields than realeased from the direct oxidation of CO with oxygen.

The following scheme represents the mechanism of the CO oxidation on RuO supported on MWCNT:

RuO 2 + CO Ru 0 + CO 3 (3)

RuO 2 + CO Ru 2 CO 3 C 3 O 9 Ru 2 (4)

RuO 2 + O 2 RuO 4 (5)

Ru 0 + O 2 RuO 2 (6)

CO 3 + OH HCO 3 + O (7)

CO + O CO 2 (8)

Therefore, this agrees with Park et al. [45], suggesting the mechanism of CO oxidation on the RuO2 surface through the adsorption and reaction of atomic oxygen species (O), as identified by XPS, which can be attributed to the coordinative unsaturated Ru atoms.

However, for higher temperatures 300˚C - 400˚C one observed higher release of CO2, which can be explained by the Bourdourd reaction and carbon oxidation ( 2CO C + CO 2 ; C + O 2 CO 2 ), that were observed by TGA analysis too.

In fact, this support MWCNT does not supply oxygen like the reducible mixed oxides support. But, it can be attributed to the presence of Lewis sites (Equation (7)) with the adsorption of molecular oxygen and release of atomic oxygen for the reaction with CO (Equation (8)), but depending also on the temperature range can influence the CO2 yield.

5. Conclusion

In this work, the ruthenium catalyst added on outside multi-walled carbon nanotubes (MWCNT) was synthesized. The BET surface area results revealed that the catalyst exhibited a high specific surface area of about 285 m2/g. The TEM studies confirm the presence of Ru nanoparticles impregnated on the outside of the carbon nanotubes and have excellent distribution. The X-ray diffraction revealed the sub-tile presence of the ruthenium. Thermogravimetric analysis of the synthesized sample indicated that the prepared catalyst is thermally stable up to 500˚C, showing a peak of degradation at 600˚C. The activity for CO oxidation reaction was studied considering different feed conditions and temperatures. In the tested catalyst, high activity (100% CO and O2 conversion) were observed, keeping the catalyst active under reaction conditions, suggesting that the RuO2 surface provides oxygen species to react with CO, thereby regenerating the consumed oxygen atoms. XPS results displayed oxygen adsorbed on the surface, which are associated with oxygen from Ruthenium oxides and Lewis acid sites on the MWCNT with caption of molecular oxygen and formation of atomic oxygen, influencing the activity and CO2 selectivity.


The authors gratefully acknowledge the support of the RCGI, Research Centre for Gas Innovation, hosted by the University of São Paulo (USP) and sponsored by FAPESP, São Paulo Research Foundation (2014/50279-4). This study was financed in part by the Coordenação de Aperfeiçoamento de Pessoal de Nível Superior, Brasil (CAPES), Finance Code 001. Many thanks to graduate students in chemical engineering (Giovanna Merces, Fabio Chirumpolo and Clara Ferreira) for their help with catalyst characterization analyzes. We thank collaboration of Technische Universität München (Germany) for XPS measurements.

Conflicts of Interest

The authors declare no conflicts of interest.


[1] Weaver, L.K. (1999) Carbon Monoxide Poisoning. Critical Care Clinics, 15, 297-317.
[2] Liu, L. and Corma, A. (2018) Metal Catalysts for Heterogeneous Catalysis: From Single Atoms to Nanoclusters and Nanoparticles. Chemical Reviews, 118, 4981-5079.
[3] Cole, K.J., Carley, A.F., Crudace, M.J., Clarke, M., Taylor, S.H. and Hutchings, G.J. (2010) Copper Manganese Oxide Catalysts Modified by Gold Deposition: The Influence on Activity for Ambient Temperature Carbon Monoxide Oxidation. Catalysis Letters, 138, 143-147.
[4] Harrison, P.G., Ball, I.K., Azelee, W., Daniell, W. and Goldfarb, D. (2000) Nature and Surface Redox Properties of Copper(II)-Promoted Cerium(IV) Oxide CO-Oxidation Catalysts. Chemistry of Materials, 12, 3715-3725.
[5] Rynkowski, J.M. and Dobrosz-Gómez, I. (2009) Ceria-Zirconia Supported Gold Catalysts. In: Annales Universitatis Mariae Curie-Sklodowska, De Gruyter Poland, Vol. 64, 197-217.
[6] Yoshida, T., Murayama, T., Sakaguchi, N., Okumura, M., Ishida, T. and Haruta, M. (2018) Carbon Monoxide Oxidation by Polyoxometalate-Supported Gold Nanoparticulate Catalysts: Activity, Stability, and Temperature-Dependent Activation Properties. Angewandte Chemie International Edition, 57, 1523-1527.
[7] Kaneti, Y.V., Tanaka, S., Jikihara, Y., Nakayama, T., Bando, Y., Haruta, M., Hossain, M.S.A., Golberg, D. and Yamauchi, Y. (2018) Room Temperature Carbon Monoxide Oxidation Based on Two-Dimensional Gold-Loaded Mesoporous Iron Oxide Nanoflakes. Chemical Communications, 54, 8514-8517.
[8] Brown, M., Green, A., Cohn, G. and Andersen, H. (1960) Purifying Hydrogen by Selective Oxidation of Carbon Monoxide. Industrial & Engineering Chemistry, 52, 841-844.
[9] Oh, S.H. and Sinkevitch, R.M. (1993) Carbon Monoxide Removal from Hydrogen-Rich Fuel Cell Feedstreams by Selective Catalytic Oxidation. Journal of Catalysis, 142, 254-262.
[10] Kahlich, M.J., Gasteiger, H.A. and Behm, R.J. (1997) Kinetics of the Selective CO Oxidation in H2-Rich Gas on Pt/Al2O3. Journal of Catalysis, 171, 93-105.
[11] Korotkikh, O. and Farrauto, R. (2000) Selective Catalytic Oxidation of CO in H2: Fuel Cell Applications. Catalysis Today, 62, 249-254.
[12] Manasilp, A. and Gulari, E. (2002) Selective CO Oxidation over Pt/alumina Catalysts for Fuel Cell Applications. Applied Catalysis B: Environmental, 37, 17-25.
[13] Igarashi, H., Uchida, H., Suzuki, M., Sasaki, Y. and Watanabe, M. (1997) Removal of Carbon Monoxide from Hydrogen-Rich Fuels by Selective Oxidation over Platinum Catalyst Supported on Zeolite. Applied Catalysis A: General, 159, 159-169.
[14] Watanabe, M., Uchida, H., Igarashi, H. and Suzuki, M. (1995) Pt Catalyst Supported on Zeolite for Selective Oxidation of CO in Reformed Gases. Chemistry Letters, 24, 21-22.
[15] Igarashi, H., Uchida, H. and Watanabe, M. (2000) Mordenite-Supported Noble Metal Catalysts for Selective Oxidation of Carbon Monoxide in a Reformed Gas. Chemistry Letters, 29, 1262-1263.
[16] Chagas, C.A., De Souza, E.F., De Carvalho, M.C.N.A., Martins, R.L. and Schmal, M. (2016) Cobalt Ferrite Nanoparticles for the Preferential Oxidation of CO. Applied Catalysis A: General, 519, 139-145.
[17] Liu, J., Liu, B., Fang, Y., Zhao, Z., Wei, Y., Gong, X.Q., Xu, C., Duan, A. and Jiang, G. (2014) Preparation, Characterization and Origin of Highly Active and Thermally Stable Pd-Ce0.8Zr0.2O2 Catalysts via Sol-Evaporation Induced Self-Assembly Method. Environmental Science & Technology, 48, 12403-12410.
[18] Lee, H.I. and White, J.M. (1980) Carbon Monoxide Oxidation over Ru (001). Journal of Catalysis, 63, 261-264.
[19] Goodman, D.W. and Peden, C.H.F. (1986) Carbon Monoxide Oxidation over Rhodium and Ruthenium: A Comparative Study. The Journal of Physical Chemistry, 90, 4839-4843.
[20] Kim, Y.D., Over, H., Krabbes, G. and Ertl, G. (2000) Identification of RuO2 as the Active Phase in CO Oxidation on Oxygen-Rich Ruthenium Surfaces. Topics in Catalysis, 14, 95-100.
[21] Over, H. and Muhler, M. (2003) Catalytic CO Oxidation over Ruthenium: Bridging the Pressure Gap. Progress in Surface Science, 72, 3-17.
[22] Assmann, J., Narkhede, V., Breuer, N.A., Muhler, M., Seitsonen, A.P., Knapp, M., Crihan, D., Farkas, A., Mellau, G. and Over, H. (2008) Heterogeneous Oxidation Catalysis on Ruthenium: Bridging the Pressure and Materials Gaps and Beyond. Journal of Physics: Condensed Matter, 20, Article ID: 184017.
[23] Gao, F., McClure, S.M., Cai, Y., Gath, K.K., Wang, Y., Chen, M.S., Guo, Q.L. and Goodman, D.W. (2009) CO Oxidation Trends on Pt-Group Metals from Ultrahigh Vacuum to near Atmospheric Pressures: A Combined in Situ PM-IRAS and Reaction Kinetics Study. Surface Science, 603, 65-70.
[24] Cant, N.W., Hicks, P.C. and Lennon, B.S. (1978) Steady-State Oxidation of Carbon Monoxide over Supported Noble Metals with Particular Reference to Platinum. Journal of Catalysis, 54, 372-383.
[25] Kiss, J.T. and Gonzalez, R.D. (1984) Catalytic Oxidation of Carbon Monoxide over Rhodium/Silicon Dioxide. An in Situ Infrared and Kinetic Study. The Journal of Physical Chemistry, 88, 898-904.
[26] Assmann, J., Narkhede, V., Khodeir, L., Löffler, E., Hinrichsen, O., Birkner, A., Over, H. and Muhler, M. (2004) On the Nature of the Active State of Supported Ruthenium Catalysts Used for the Oxidation of Carbon Monoxide: Steady-State and Transient Kinetics Combined with in Situ Infrared Spectroscopy. The Journal of Physical Chemistry B, 108, 14634-14642.
[27] Assmann, J., Crihan, D., Knapp, M., Lundgren, E., Löffler, E., Muhler, M., Narkhede, V., Over, H., Schmid, M., Seitsonen, A.P. and Varga, P. (2005) Understanding the Structural Deactivation of Ruthenium Catalysts on an Atomic Scale under both Oxidizing and Reducing Conditions. Angewandte Chemie International Edition, 44, 917-920.
[28] Joo, S.H., Park, J.Y., Renzas, J.R., Butcher, D.R., Huang, W. and Somorjai, G.A. (2010) Size Effect of Ruthenium Nanoparticles in Catalytic Carbon Monoxide Oxidation. Nano Letters, 10, 2709-2713.
[29] Soliman, N.K. (2019) Factors Affecting CO Oxidation Reaction over Nanosized Materials: A Review. Journal of Materials Research and Technology, 8, 2395-2407.
[30] Ma, Q., Wang, D., Wu, M., Zhao, T., Yoneyama, Y. and Tsubaki, N. (2013) Effect of Catalytic Site Position: Nickel Nanocatalyst Selectively Loaded inside or outside Carbon Nanotubes for Methane Dry Reforming. Fuel, 108, 430-438.
[31] Zeng, S., Zhang, L., Jiang, N., Gao, M., Zhao, X., Yin, Y. and Su, H. (2015) Multi-Wall Carbon Nanotubes as Support of Copper-Cerium Composite for Preferential Oxidation of Carbon Monoxide. Journal of Power Sources, 293, 1016-1023.
[32] Kozonoe, C.E., Brito, R.M. and Schmal, M. (2020) Influence of Feed Rate and Testing Variables for Low-Temperature Tri-Reforming of Methane on the Ni@MWCNT/Ce Catalyst. Fuel, 281, Article ID: 118749.
[33] Zhao, X. and Ando, Y. (1998) Raman Spectra and X-Ray Diffraction Patterns of Carbon Nanotubes Prepared by Hydrogen Arc Discharge. Japanese Journal of Applied Physics, 37, 4846-4849.
[34] Abdulrazzak, F.H., Alkiam, A.F. and Hussein, F.H. (2019) Behavior of X-Ray Analysis of Carbon Nanotubes. In: Saleh, H.E.D. and El-Sheikh, S.M.M., Eds., Chapter 7 Perspective of Carbon Nanotubes, BoD-Books on Demand, 109-124.
[35] Bond, G.C. (1987) Heterogeneous Catalysis: Principles and Applications (Oxford Chemistry). 2nd Edition, Oxford University Press, New York.
[36] Rojas, J.V., Toro-Gonzalez, M., Molina-Higgins, M.C. and Castano, C.E. (2016) Facile Radiolytic Synthesis of Ruthenium Nanoparticles on Graphene Oxide and Carbon Nanotubes. Materials Science & Engineering B: Solid-State Materials for Advanced Technology, 205, 28-35.
[37] Saleh, T.A. (2011) The Influence of Treatment Temperature on the Acidity of MWCNT Oxidized by HNO3 or a Mixture of HNO3/H2SO4. Applied Surface Science, 257, 7746-7751.
[38] Santos, A.R., Menezes, D.B., Ellena, J. and Andrade, M.B. (2019) Aplicação da espectroscopia Raman na caracterização de minerais pertencentes a uma geocoleção. Química Nova, 42, 489-496.
[39] Zdrojek, M., Gebicki, W., Jastrzebski, C., Melin, T. and Huczko, A. (2004) Studies of Multiwall Carbon Nanotubes Using Raman Spectroscopy and Atomic Force Microscopy. In: Solid State Phenomena, Trans Tech Publications Ltd., Stafa-Zurich, 265-268.
[40] Foldvari, M., et al. (2012) Pharmaceutical Characterization of Solid and Dispersed Carbon Nanotubes as Nanoexcipients. International Journal of Nanomedicine, 2012, 403-415.
[41] Shih, Y.T., Lee, K.Y. and Huang, Y.S. (2014) Electrochemical Capacitance Characteristics of Patterned Ruthenium Dioxide-Carbon Nanotube Nanocomposites Grown onto Graphene. Applied Surface Science, 294, 29-35.
[42] Schmal, M. (2016) Heterogeneous Catalysis and Its Industrial Applications. Springer, Berlin.
[43] Ananth, A., Jeong, R.H. and Boo, J.-H. (2020) Preparation, Characterization and CO Oxidation Performance of Ag2O/γ-Al2O3 and (Ag2O+RuO2)/γ-Al2O3 Catalysts. Surfaces, 3, 251-264.
[44] Her, J.H., Kennon, B.S., Shum, W.W., Stephens, P.W. and Miller, J.S. (2008) Structure and Magnetic Properties of LnIII[Ru2(CO3)4]ܮH2O. Inorganica Chimica Acta, 361, 3462-3464.
[45] Park, J.N., Kuk Shon, J., Jin, M., Sung Kong, S., Moon, K., Ok Park, G., Boo, J.H. and Man Kim, J. (2011) Room-Temperature CO Oxidation over a Highly Ordered Mesoporous RuO2 Catalyst. Reaction Kinetics, Mechanisms and Catalysis, 103, 87-99.
[46] Reddy, B.M., Rao, K.N. and Bharali, P. (2009) Copper Promoted Cobalt and Nickel Catalysts Supported on Ceria-Alumina Mixed Oxide: Structural Characterization and CO Oxidation Activity. Industrial & Engineering Chemistry Research, 48, 8478-8486.

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