Open access peer-reviewed chapter - ONLINE FIRST

Cobalt-Based Catalysts for CO Preferential Oxidation

By Leticia E. Gómez and Alicia V. Boix

Submitted: October 30th 2018Reviewed: August 1st 2019Published: August 26th 2019

DOI: 10.5772/intechopen.88976

Downloaded: 41

Abstract

In this work, catalysts based on cobalt supported on ZrO2 and CeO2 and CoCeMnOx were studied for the CO preferential oxidation (COPrOx) in hydrogen-rich stream able to feed fuel cells. Among them, the CoCeMnOx formulation showed the highest CO conversion at low temperatures, while the cobalt oxide supported on ceria presented the best selectivity toward CO2. The Co3O4 spinel was the active phase for the CO preferential oxidation detected in all catalysts. However, the CoOx-CeO2 and CoCeMnOx catalysts resulted more active than cobalt oxide supported on zirconia. The presence of ceria close to cobalt species promotes the redox properties and enhances the catalytic activity. In the CoCeMnOx catalyst prepared by coprecipitation, the incorporation of Mn represented an additional positive effect. The presence of Mn promoted the reoxidation of Co2+ to Co3+ and, consequently, the activity increased at low temperature. By X-ray diffraction (XRD) of CoOx-ZrO2 and the CoOx-CeO2 catalysts, the Co3O4 spinel and ZrO2 or CeO2 were identified in agreement with laser-Raman spectra. At the same time, the CoCeMnOx catalyst, prepared by coprecipitation of precursor salts, showed an incipient development of a new phase (Mn,Co)3O4 mixed spinel, due to the intimate contact between elements.

Keywords

  • COPrOx
  • (Mn
  • Co)3O4 mixed spinel
  • redox couple
  • CoCeMnOx
  • CeO2 support
  • XPS
  • laser-Raman spectroscopy

1. Introduction

The global demand for energy has been inexorably growing in the last decades. The increasing use of fossil fuels in order to generate energy causes serious problems to the environment due to the gaseous emissions. This fact has produced a global movement toward trying to remove the contaminants from combustion effluents. Besides, the exploration for alternatives to fossil fuels, biofuels or hydrogen as an energy vector, has gained an immediate and future significance because this could contribute to the depletion of greenhouse gases [1, 2, 3].

Fuel cells are devices that are being actively developed, because they are power generation systems that can produce energy with significantly less impact on the environment. Among several types of fuel cells, proton exchange membrane fuel cells (H2-PEMC) are considered to be the most technically advanced for such application [4]. Hydrogen produced by means of the steam reforming or autothermal process of hydrocarbons or alcohols should contain less than 10 ppm of carbon monoxide before entering the cell since CO poisons the Pt anode of the fuel cells (Figure 1) [5, 6]. After the reforming step, the hydrogen production process continues with the water gas shift reaction (WGSR), where the stream is enriched in hydrogen and the CO content is diminished to 1%. As the CO concentration in the hydrogen stream is so high to enter to the cell, it is necessary to reduce it to the desired levels. Among various methods such as catalytic methanation, Pd-based membrane, and catalytic CO preferential oxidation (COPrOx), the latter is considered as the most adequate due to its simplicity and effectiveness. Thus, given the importance of the hydrogen purification process, the last few years have witnessed the surge of a renewed interest in the CO oxidation reaction, and several contributions dealing with this issue have recently been published [5, 6, 7].

Figure 1.

Schematic flow diagram of a typical fuel cell processor with COPrOx.

In our research group, catalysts for the removal of contaminants from vehicles, industrial facilities, and power-generating sources have been studied [8, 9]. In addition, catalysts and catalytic reactors have also been investigated for the production and purification of H2 to be used in fuel cells [10, 11, 12, 13].

On the other hand, due to their redox properties, cobalt-containing catalysts have been the object of numerous publications in the environmental catalysis field and in the purification of H2 stream, among other applications. For example, catalysts based on cobalt oxides have been studied for soot combustion [14], NOx selective reduction in oxygen excess [15], and CO preferential oxidation reaction [16].

The challenges involved in the design of successful COPrOx catalysts are the following: (i) high CO oxidation activity at low temperatures, (ii) high selectivity for CO oxidation against the undesired H2 oxidation, and (iii) good resistance to deactivation caused by the H2O and CO2 in the feed [5, 6, 17].

In order to reduce the CO concentration without consuming H2, several catalysts have been studied with promising results. Catalysts of Pt supported on bimetallic systems achieved excellent results [17, 18, 19], but the high cost of noble metals led the investigations toward the use of other active phases. For instance, CuO/CeOx catalysts have shown a catalytic performance in the COPrOx comparable to those based on noble catalysts [20, 21, 22].

In this vein, it has been shown that the combined effect of cobalt oxide and ceria strongly influences the morphological and redox properties of the composite oxides, by dispersing the Co3O4 phase and promoting the efficiency of the Co3+/Co2+ redox couple [23, 24]. Numerous publications have shown that the addition of other metals to a cerium-based mixed oxide (Zr or Mn) increases the oxygen storage capability of the ceria. This effect is originated by the increase in the surface oxygen mobility due to chemical interactions between cobalt, cerium, and other metals [25, 26, 27].

On the other hand, the use of structured catalysts as those supported onto honeycomb monoliths has long been considered in the chemical industry, and it has increased with the significance of environmental catalysis in pollution abatement applications due to catalysts with a high attrition resistance and a low pressure drop that are required. In addition the thin catalytic coating allows high efficiency and selectivity. Cordierite offers high mechanical strength, high resistance to elevated temperatures, and temperature shocks due to its low thermal expansion coefficient. Moreover, it presents great adhesion stability, which is a very important property for the monolithic catalysts [12, 13, 15, 16].

In our previous work with structured catalysts, we showed that cobalt supported on zirconia and ceria and CoCeMnOx mixed oxides resulted in efficient catalysts for the COPrOx. However, it is of great interest both to identify the cobalt species present in an active catalyst and to analyze the interactions with the support (CeO2 or ZrO2) and their influence on the catalytic behavior. It is also important to understand the role of cobalt in the CoCeMnOx mixed oxides. In the present work, a very detailed analysis of the species present in these complex systems was carried out. The catalysts were analyzed by X-ray diffraction (XRD) and temperature-programmed reduction (TPR). The X-ray photoelectron spectroscopy (XPS) and laser-Raman spectroscopy (LRS) were used to characterize the oxidation state, concentration, and chemical nature of species present on catalysts.

2. Materials and methods

2.1 Preparation of cobalt-based catalysts

Three main groups of Co-based catalysts with 10 wt.% of cobalt were prepared—CoOx/ZrO2, CoOx-CeO2, and CoCeMnOx—in order to study the cobalt species and their relation to the centers active in the CO preferential oxidation.

The CoOx-ZrO2 catalyst with 10 wt.% cobalt on ZrO2 was prepared by wet impregnation and labeled CoZ. A commercial zirconia support (6.8 m2/g, pore volume ca. 0.013 cm3/g) was impregnated with an aqueous solution of Co(NO3)2. The mixture was evaporated until achieving a paste, which was placed in the oven overnight at 120°C.

CoOx-CeO2 catalysts were prepared by two different methods. The CoCe-I sample was produced by the wet impregnation method with 10 wt.% of cobalt, using an aqueous solution of Co(NO3)2 and CeO2 powder as support which was obtained by precipitation of the Ce(NO3)3 solution with NH4(OH). The mixture was evaporated under continuous agitation until achieving a paste, which was placed in the oven overnight at 110°C. By means of the coprecipitation method, CoCe-P catalyst was obtained. The aqueous solution of Co(NO3)2 and Ce(NO3)3 was precipitated with NH4(OH) added drop by drop under vigorous stirring. The resulting precipitate was filtered and washed several times with distilled water and dried overnight at 110°C.

The CoCeMnOx oxide mixture catalyst with 10 wt.% of Co and Mn/Co molar ratio of 1/4 was prepared by the coprecipitation method, adding NH4(OH) to an aqueous solution of Co(NO3)2, Ce(NO3)3, and Mn(NO3)2. The mixture was kept 2 h under continuous stirring at room temperature. The precipitate obtained was washed several times with deionized water and then dried overnight at 110°C.

After drying, all obtained solids were calcined for 5 h at 500°C under flowing air (25 mL/min), and the temperature was ramped from room temperature up to 500°C at 10°C/min.

2.2 Characterization

2.2.1 Chemical composition quantification

Elemental analyzes were performed by inductively coupled plasma atomic emission spectroscopy (ICP-AES) on an ICP Optima 2100 DV PerkinElmer instrument.

2.2.2 Surface area measurement

The specific surface area was calculated by BET method from N2 adsorption isotherms at −196°C with a Micromeritics TriStar 3000 instrument. The powder samples (50 mg) were previously outgassed in vacuum at 300°C for 3 h in order to remove any adsorbed substance. The volume of adsorbed N2 was measured as the pressure was increased.

The surface area S of the catalysts was calculated as

S=vmNAVME1

where N is the Avogadro number, VM is the molar volume of a gas, A is the area of a molecule of nitrogen, and vm is the volume of an adsorbed monolayer of gas, which is obtained from the BET equation

PvP0P=1vmc+c1vmPP0E2

where P and P0 are the equilibrium and the saturation pressure of N2 at the temperature of adsorption, v is the adsorbed gas volume, vm is the volume of an adsorbed monolayer, and c is the BET constant.

2.2.3 X-ray diffraction (XRD)

The patterns of all samples were measured on a Shimadzu XD-D1 instrument with monochromator using Cu-Kα radiation at a scanning rate of 1°/min in the range of 2θ = 20°–80°.

2.2.4 Temperature-programmed reduction (H2-TPR)

The catalysts (100 mg) were pretreated in Ar flow heating up to 300°C and held 30 min in order to clean the catalytic surface. The reducing gas was a 5% H2/Ar mixture; the temperature was ramped up at 10°C/min to 900°C. The experiments were carried out using an Okhura TP-2002S instrument equipped with a thermal conductivity detector (TCD). The H2 uptake was registered as the temperature increased.

2.2.5 Laser-Raman spectroscopy (LRS)

The laser-Raman spectra of catalysts and CeO2 and ZrO2 supports disposed as pressed powder were measured with a LabRAM spectrometer (HORIBA Jobin Yvon) with an Olympus confocal microscope, equipped with a charge-coupled device (CCD) detector. The excitation wavelength was in all cases 532 nm. The laser power was set at 30 mW. In addition, a Linkam high-temperature cell was used for the in situ experiments, introducing into the cell 50 mg of powder catalysts. The reductive/oxidative treatments were carried out at different temperatures. The concentration and the caudal of gas reactants which entered to the cell were controlled by mass flow controllers. A thermocouple placed on the middle of the catalytic cell allowed the temperature control.

2.2.6 X-ray photoelectron spectroscopy

XPS analyses were performed in a multi-technique system (SPECS) equipped with AlKα X-ray source and operated at 100 W with pass energy of 30 eV. In addition, in order to avoid the spectral interference (Mn LMM with Ce 3d), the spectra of Ce 3d, O 1s, and C 1s were measured with MgKα X-ray source. The XPS analyses were performed on the calcined powders which were previously pressed. The data treatment was performed with the Casa XPS program (Casa Software Ltd., UK).

2.3 Assessment of the catalytic activity

CO preferential oxidation experiments were performed in a fixed-bed flow reactor at atmospheric pressure. The reaction mixture consisted of 1% CO, 1% O2, and 40% H2 and He balance. The weight/total flow ratio was adjusted to 2.1 mg∙min/mL. The CO conversion (XCO) and the oxygen selectivity toward CO2 (SO2) were defined as

XCO%=CCO0CCOCCO0×100E3
SO2%=0.5CCO0CCOCO20CO2×100E4

where CCO and CO2 were reactor exit concentrations of CO and O2, respectively, while CCO0 and CO20 represented the feed concentrations. The stream compositions were measured with a chromatograph GC-2014 Shimadzu equipped with a TCD cell. All catalysts were pretreated during 1 h in O2/He flow at 200°C before the catalytic test. In order to study the stability and a possible deactivation caused by the presence of CO2, the CoCeMnOx catalyst was tested during 75 h at 175°C, adding 20% CO2 in the reactant mixture.

3. Results and discussion

3.1 Prepared catalysts

The compositions of the cobalt-based catalysts, analyzed by the ICP technique, are presented in Table 1 and are in agreement with the predefined nominal values. The cobalt content (wt.%) resulted 9.2, 10.6, and 8.6 for CoZ, CoCe-I, and CoCe-P, respectively, while for the mixture of oxides CoCeMnOx, the concentrations of Co, Mn, and Ce were 11, 2.6, and 24.8 wt.%, respectively.

CatalystsPreparation methodCo (wt.%)Mn (wt.%)Molar ratio of Co/Zr or CeBET area (m2/g)
CoZwet impregnation9.20.157.5
CoCe-Iwet impregnation10.60.1493
CoCe-Pco-precipitation8.60.1492
CoCeMnOxco-precipitation11.02.61.06165

Table 1.

Co-based catalysts, compositions, and specific surface area.

The BET method was used to determine the surface specific area of each sample, and the values are also reported in Table 1. The surface area of the CoZ sample practically did not change with the impregnation of cobalt, showing BET value of 7.5 m2/g, close to the ZrO2 support. On the other hand, the surface area was similar for the CoOx-CeO2 catalysts, regardless of the impregnation or coprecipitation methods used. As it can be observed for CoMnCeOx, the addition of a small amount of manganese increased the specific surface with respect to the other samples, possibly due to the insertion of Mn in the ceria structure.

3.2 X-ray diffraction

The crystalline structures of the different Co-based catalysts and that of the ZrO2 and CeO2 supports were analyzed by means of XRD. Figure 2 shows the diffraction patterns of the samples.

Figure 2.

XRD patterns of CoZ, CoCe-I, CoCe-P, and CoCeMnOx catalysts and CeO2 and ZrO2 supports.

The CoOx-CeO2 catalysts (CoCe-I and CoCe-P) show patterns dominated by the characteristic CeO2 diffraction peaks, whose main signals appear at 2θ = 28.6°, 33.4°, 47.8°, and 56.6° (JCPDS34-0394). The peaks of Co3O4 at 2θ = 31.3°, 36.8°, 44.8°, 59.4°, and 65.3° (JCPDS 42-1467) do not seem to modify the structure of the CeO2 diffraction pattern. Despite the different preparation methods that were used, only two phases can be distinguished, i.e., Co3O4 spinel and CeO2 with fluorite structure.

On the other hand, the diffraction pattern of the CoZ catalyst shows the peaks associated with the monoclinic ZrO2 support and the main signal of Co3O4 at 2θ = 36.8°.

In the diffraction pattern of the CoCeMnOx catalyst, a broadening of peaks corresponding to the CeO2 phase can be observed. These results could indicate that the structure of CeO2 is distorted due to the insertion of manganese, although the type fluorite structure of CeO2 is still maintained [28]. It can be observed that in the main signal of CeO2 (2θ = 28.6°), an asymmetric broadening appears associated with an incipient formation of the (Mn,Co)3O4 phase, which has a characteristic peak at 29.4° (JCPDS 18-408). Likewise, the main peak of the (Mn,Co)3O4 phase (2θ = 36.4) appears at 36.9°, close to the main signal of the Co3O4 spinel.

3.3 Temperature-programmed reduction

Figure 3 exhibits the reduction peaks corresponding to cobalt-based catalyst. The reduction profile of the CoZ catalyst presents a peak, whose maximum is at 395°C, and a shoulder, at 370°C. The cobalt oxide reduction is completed at 440°C. It is known that the reduction of Co3O4 takes place in two steps that correspond to the subsequent reduction of the Co3+ and Co2+ species present in the spinel structure.

Figure 3.

Temperature-programmed reduction of CoZ, CoCe-I, CoCe-P, and CoCeMnOx catalysts.

The CoCe-P profile presents two intense peaks at 300 and 380°C belonging to Co3O4 reduction. The small signals at 471 and 850°C could be attributed to the reduction of the ceria support, superficial oxygen, and bulk species, respectively [29, 30]. On the other hand, in the CoCe-I sample, the peak at 471°C is a small shoulder. It is probable that for the coprecipitated catalysts, a more intimate contact between Co and Ce species takes place. This fact produces a synergistic effect promoting the reducibility of the species and the mobility of surface oxygen species in ceria support. The performance of Co3O4 phase on COPrOx reaction follows a redox mechanism which involves the reduction/oxidation of the Co3+ site. The presence of ceria and the synergism with cobalt would improve its reducibility. According to the H2 consumption of each sample, the H2/Co ratio close to 1.33 revealed that Co3O4 is the cobalt phase present on CoZ catalysts. In the case of CoOx-CeO2 catalysts, the H2/Co ratio values higher than 1.33 were calculated. This would indicate that a CeO2 fraction was reduced within the range of temperatures studied.

The profile of the CoCeMnOx catalyst shows three reduction zones at low (150–420°C), intermediate (420–620°C), and high (650–900°C) temperatures. As shown by XRD, the Co species seems preferentially to form the Co3O4 spinel (2θ = 36.9°) without distortion of the CeO2 structure, which is reduced at low temperature. The reduction of manganese species should also be considered in this zone, because there are multiple overlapping peaks [28]. Then, the cobalt species (Co3O4) and a fraction of the Mn4+/Mn3+ species incorporated to the ceria structure might be reduced below 420°C. The reduction temperatures of Co3O4 in the CoCeMnOx catalyst are lower than in the CoCe-I and CoCe-P samples. The other broad peak centered at 800°C is a typical reduction peak of bulk CeO2 and could also be associated with some difficult-to-reduce Mnn+ species.

3.4 Laser-Raman spectroscopy

The laser-Raman spectra of catalysts and CeO2 and ZrO2 supports are shown in Figure 4. The CeO2 spectrum shows a main band at 464 cm−1 (F2g mode) and other weaker signals at 259, 587, and 1173 cm−1 belonging to second-order (2 TA, D, and 2TO) Raman modes, respectively, which are associated to oxygen vacancies [31, 32, 33].

Figure 4.

Raman spectra of CoZ, CoCe-I, CoCe-P, and CoCeMnOx catalysts.

The Raman spectra of CoCe-I and CoCe-P show a single peak at 464 cm−1, which corresponds to CeO2, as well as the signals at 193, 484, 524, 615, and 680 cm−1 assigned to the vibrations of the Co3O4 spinel. The bands at 193, 524, and 615 cm−1 were attributed to the F2g mode, while the bands at 484 and 680 cm−1 were assigned to the Eg and A1g modes, respectively [34].

In the CoCeMnOx spectrum, the bands of Co3O4 oxide are not detected. However, a small peak at 666 cm−1 is observed, due to the possible formation of a Mn,Co mixed spinel. Nevertheless, the XRD patterns showed the main peak corresponding to the Co3O4 spinel Therefore, the co-existence of Co3O4 and (Mn,Co)3O4 phases could also be possible.

The Raman spectra of the CoZ catalysts and ZrO2 support are shown in Figure 4. The main bands at 680 and 520 cm−1 can be observed corresponding to cobalt oxides [35]. The other bands at 193, 475, and 615 cm−1 overlap with the bands of zirconia monoclinic phase.

In order to understand the change of the active phase under different atmospheres, the CoCe-I catalyst was subjected to different reductive/oxidative treatments at different temperatures. These experiments were followed by in situ Raman spectroscopy, recording spectra at each temperature. The catalyst was placed in a reaction chamber coupled to the spectrometer.

The first experiment consisted in reducing the catalysts with a 1% CO/Ar stream with the purpose of analyzing the CO reducing capacity. At room temperature the main signals corresponding to Co3O4 at 691, 521, and 484 cm−1, as well as the main signal of CeO2 at 463 cm−1, were detected (Figure 5A). As the temperature increased, the intensity of the Co3O4 bands decreased. However, a weak signal around 690 cm−1 was distinguished at 300°C, while at 325°C no signals of Co3O4 were detected, which implied that Co3O4 was completely reduced by CO from the gas phase. The catalyst was cooled to room temperature in 1% CO/Ar mixture and then maintained in Ar atmosphere.

Figure 5.

In situ Raman study of CoCe-I. (A) 1% CO/Ar flow, (B) 1% O2/Ar flow, and (C) under reaction conditions (1%CO, 1%O2, 40% H2, Ar).

The following experiment consisted in oxidizing the reduced catalyst with a 1% O2/Ar stream, and the spectra are exhibited in Figure 5B. In the spectrum at the bottom, recorded at room temperature, it is possible to observe the main signal of CeO2 at 463 cm−1, as well as a broad signal between 500 and 600 cm−1, which was assigned to oxygen vacancies. As the temperature increases, this broad band decreases due to the incorporation of oxygen from the gas phase into the structure. Moreover, at 200°C the signals corresponding to Co3O4 are observable due to the oxidation of Co metal particles. After the experiment, the catalyst was cooled in 1% O2/Ar flow at room temperature, and then it was treated in an Ar stream during several minutes. The corresponding spectrum registered at room temperature is shown in Figure 5C.

After that, the catalyst was again reduced at 350°C by a reducing stream (1% CO, 40% H2 in Ar), and then, it was cooled in the same stream. A new spectrum was recorded at room temperature, and it is only possible to observe the main signal of CeO2 at 464 cm−1. Then, the catalyst was treated in Ar stream during several minutes, and oxygen vacancies were again detected.

Subsequently, the catalyst was subjected to a stream composed of the COPrOx reactant mixed gas flow (1% CO, 1% O2, 40% H2 and Ar). At room temperature the CeO2 main signal was still observed. The temperature was increased, and at 150°C it was possible to detect a little band at 680 cm−1, which belongs to Co3O4, which indicates that the oxygen present in the reactant gas stream is capable of reoxidizing the reduced cobalt species. When the temperature continued increasing, the band at 680 cm−1 was well defined, but at 300°C, it started again to decrease. At 325°C, the signal completely disappeared.

3.5 X-ray photoelectron spectroscopy

The surface characterization of Co-based catalysts was analyzed by the XPS technique, and the spectra for Co 2p and O 1s core levels are presented in Figure 6. The Co 2p spectrum shows two peaks at 780.1 and 795.0 eV, corresponding to the Co 2p3/2-Co 2p1/2 spin-orbit splitting (Figure 6A). These binding energies (BE) could be assigned to Co2+ or Co3+ species, since the BE difference is negligible for both species. However, the presence of intense satellite peaks is distinctive of the Co2+ spectrum [36, 37]. The cobalt spectra present very small satellite peaks, or else, the absence of them would indicate that Co3+ species are dominant for all catalysts.

Figure 6.

XPS spectra of Co 2p3/2 (A) and O 1s (B) for CoZ, CoCe-I, CoCe-P, and CoCeMnOx catalysts.

Figure 6B shows the O 1s XP spectra for all of the catalysts studied. Broad and complex shape spectra are observed in this region. These spectra can be described as the result of the overlapping of two components corresponding to different species or groups of species. The first peak appears at 529.8 eV and the other at 532.3 eV. The oxygen signal at lower BE corresponds to bulk CeO2 oxide and to cobalt oxides [38, 39]. The other component is assigned to hydroxyl, water, and/or carbonate groups adsorbed on the solid surface [40].

3.6 Catalytic evaluation

The COPrOx reaction system can be described by the following two reactions; the first one corresponds to CO oxidation, while the second one is the undesirable H2 oxidation reaction.

CO+0.5O2CO2E5
H2+0.5O2H2OE6

Figure 7A presents CO conversion curves of different catalysts as a function of temperature. It can be observed that the catalyst which was prepared with ZrO2 support reached a conversion maximum (92%) lower than that reached by the catalysts prepared with cerium and at a higher temperature (200°C). CoCe-I and CoCe-P reached almost total CO conversion at 175 and 165°C, respectively, showing that CeO2 is a better catalytic support than ZrO2. Moreover, the small difference in catalytic performance which exists between CoCe-I and CoCe-P indicates that the coprecipitation method is slightly suitable to obtain an adequate catalyst for this reaction. When manganese was incorporated to the catalytic formulation, it could be observed that with the CoCeMnOx catalyst, complete CO conversion was reached at lower temperature than other catalysts. In addition, the temperature window of CO maxima conversion was maintained on a wide temperature range (150–200°C). Figure 7B shows the O2 to CO2 selectivity curves as a function of temperature. Selectivity curves exhibited a decreasing trend as the temperature increased. Since the H2 oxidation (reaction 2) had a higher apparent activation energy than the CO oxidation (reaction 1), as temperature increased, the hydrogen oxidation rate also increased so that CO conversion decreased and, consequently, the selectivity curve also decreased.

Figure 7.

COPrOx reaction on CoZ, CoCe-I, CoCe-P, and CoCeMnOx catalysts. (A) CO conversion (%). (B) O2 selectivity to CO2 (%). Reaction conditions: 1% CO, 1% O2, 40% H2 and He balance. W/F: 2.1 mg min/mL.

Moreover, the stability of CoCeMnOx and the effect of CO2 adding in the feed were studied at 175°C during 75 h under reaction conditions. The CO conversion was maintained at 95% while the selectivity increased from 50 to 60%. The used catalysts did not show carbon formation by LRS spectroscopy.

The CeO2 support with high mobility of surface lattice oxygen promotes the surface exchange between reduced and oxidized species Ce4+ + Co2+↔Ce3+ + Co3+. This process allows that the Co3+ species are available on the catalytic surface.

In the case of CoCeMnOx, which is the most active catalyst, the Co2+ species are oxidized by oxygen from Mn oxides or CeO2 support, and then they are oxidized by oxygen from the gas phase. The redox couples Co2+/Co3+ and Ce3+/Ce4+ are improved by the presence of MnOx.

The in situ Raman results suggest that the active phase participates in the chemical reaction by a redox mechanism, where Co3+ oxidizes CO and reduces itself to Co2+, but this cobalt species is permanently reoxidized by oxygen provided by CeO2 and/or the gas phase. These experiments also allow inferring that the reduction step limits the overall reaction while the reoxidation on the surface is very fast.

4. Conclusions

The nature of cobalt species observed on Co-based catalysts used on the COPrOx reaction was influenced by the constituent species of the environment.

The XRD, TPR, XPS, and LRS characterizations showed that the Co3O4 active phase was present in all catalysts. From diffraction patterns of CoOx-ZrO2 and the CoOx-CeO2 catalysts, the Co3O4 spinel and the signals corresponding to ZrO2 and CeO2 were identified in agreement with laser-Raman spectra.

The CoCeMnOx catalyst, prepared by coprecipitation of precursor salts, showed an incipient development of a new phase (Mn,Co)3O4 mixed spinel, due to the intimate contact between elements.

The reduction of cobalt oxides was completed below 400°C and was promoted by the oxygen vacancies of ceria. In contrast, in the CoZ catalysts, the cobalt species were totally reduced at 440°C. The profiles showed two reduction steps assigned to Co3+ to Co2+ and then Co2+ to Co0.

In situ laser-Raman spectroscopy revealed that cobalt species remained oxidized in spite of the reducing atmosphere of the reactant flow within the temperature range studied.

The XPS spectra showed the coexistence of Co2+ and Co3+ species according to the Co3O4 phase on the catalytic surface.

The CO conversion reached by the CoOx-CeO2 catalysts was higher than the CoOx-ZrO2 sample, due to redox properties of ceria. The manganese addition promoted the catalytic activity, widening the temperature window of maximum CO conversion.

Acknowledgments

The authors acknowledge the financial support received from UNL, ANPCyT, and CONICET. Thanks are given to Fernanda Mori for the XPS measurements.

Conflict of interest

The authors declare no conflict of interest with any person, institution, or organization for the publication of this chapter.

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Leticia E. Gómez and Alicia V. Boix (August 26th 2019). Cobalt-Based Catalysts for CO Preferential Oxidation [Online First], IntechOpen, DOI: 10.5772/intechopen.88976. Available from:

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