SciELO - Scientific Electronic Library Online

 
vol.59 issue4EMQAL: ERASMUS MUNDUS MASTER IN QUALITY IN ANALYTICAL LABORATORIESPREPARATION OF MOLECULARLY IMPRINTED POLYMERS FOR DIPHENYLAMINE REMOVAL FROM ORGANIC GUNSHOT RESIDUES author indexsubject indexarticles search
Home Pagealphabetic serial listing  

Services on Demand

Journal

Article

Indicators

Related links

  • On index processCited by Google
  • Have no similar articlesSimilars in SciELO
  • On index processSimilars in Google

Share


Journal of the Chilean Chemical Society

On-line version ISSN 0717-9707

J. Chil. Chem. Soc. vol.59 no.4 Concepción Dec. 2014

http://dx.doi.org/10.4067/S0717-97072014000400020 

 

CATALYTIC COMBUSTION OF SOOT ON Ce-DOPED LANTHANUM COBALTITES

 

GINA PECCHI1*, RUDDY MORALES1, EDUARDO J. DELGADO1, ROMEL JIMENEZ2, MARCO FRAGA3

1: Departamento Físico-Química, Facultad Ciencias Químicas;
2
: Departamento Ingeniería Química, Facultad de Ingeniería, Universidad de Concepción, Concepción, Chile.
3
: Instituto Nacional de Tecnologia/MCTI, Rio de Janeiro, Brasil.
* e-mail:
gpecchi@udec.cl


ABSTRACT

Substituted La1-xCexCoO3 perovskite-type oxides (0.0x0.9), prepared by the self-combustion method, have been investigated as catalysts in soot combustion. The characterization results indicate modification in the specific surface area, crystal structure, oxygen mobility and reducibility of cobaltite upon cerium substitution. Cobaltite structure does not tolerate more than 50% substitution of La by Ce. For higher Ce substitution the perovskite structure is lost and mixed oxides are detected. Further destruction of the perovskite structure in a reductive process indicates a lower catalytic role of the perovskite structure in the catalytic combustion of soot regarding to the chemical composition of the La1-xCexCoO3 system. After the reductive process, only a slight increase in the catalytic activity of the samples with low Ce content (x0.3) while a larger increased was detected for those with larger amount of Ce(x0.5). These results suggest that the activity of these materials for soot combustion is improved by two factors: i) the increasing of CeO2 content, closely related to higher material capacity for oxygen transfer from catalyst to carbonaceous surface and ii) the formation of larger CeO2 crystals in the higher-Ce-content samples after H2 reduction, responsible of the improvement of the oxygen exchange and number of contact points between catalyst and soot.

Key words: cobalt, ceria, lanthanum, perovskite, soot, combustion.


 

1. INTRODUCTION

Diesel engines play a vital role in the modern society since they are widely used in heavy-duty transportation and power generation. The application of diesel engines in these fields is motivated because of the high efficiency of the engines, their low-operating costs, high durability and reliability. However, the diesel engine is one of the largest contributors to environment pollution problems worldwide, and will remain so, with large increases expected in vehicle population causing ever-increasing global emissions of diesel particulate matter and nitrogen oxides. Particulate matter consists mostly of carbonaceous soot with minor components of volatile organic fraction, from unburned fuel, and inorganic compounds such as ash and sulphur compounds. The particulate material is responsible for serious adverse effects on human health, physiology of plants, environment, building materials and global warming. For these reasons, legislative restrictions for emission levels have stimulated the development of new catalysts and technologies for the abatement of soot particulates. Among the traditional catalytic systems for soot combustions such as noble metals[1], oxides and mixed oxides[2], alkali based materials[3]; perovskite-type mixed oxides have received recently considerable attention for this purpose[4-8]. Perovskite-type oxides are represented by the general formula ABO3, where the A-site metal is usually a rare earth element, and the B-site metal is a first row transition metal. Due to the number of possible combinations of metals for the A and B-sites, perovskites can be tailored to create a wide family of catalysts, by varying either the A-site and/or the B-site metal ion. Thus, pure and doped lanthanum chromites, manganites and cobaltites, have been tested with mixed results in the catalytic combustion of soot [9]. Recently, a Pr0.7Sr0.2K0.1MnO3perovskite type catalyst on a ceramic filter has been point out has a promising soot catalyst and that more detailed investigations must be carried out to understand their catalytic behavior [10]. Cerium is usually reported as a good promoter in perovskite lattice. Partial substitution of lanthanum by cerium or strontium on cobalt based perovskites leads to an increase in catalytic oxidation [11]. When perovskite-type oxides are submitted to a reduction process, the low thermal behavior of these materials under reductor atmosphere allow to produce nanometric metal particles, in a high dispersion degree [12] modifying the oxygen storage capacity of the catalyst. The substitution of the lanthanum cation La3+ by an oxygen storage cation as cerium, with the capacity of the redox Ce3+/Ce4+ couple, must have a direct effect in the reducibility of the perovskite structure and dispersion degree of the pure or mixed La2O3 and CeO2 oxides.

In this article it is proposed to use calcined and reduced Ce-doped lanthanum cobaltite's; LaxCe1-xCoO3,x=0.10.9 on the catalytic combustion of soot. The synthesis, characterization and the effect of reduction and substitution degree on the catalytic activity is reported.

2. MATERIAL AND METHODS

2.1 Preparation

Pure cobaltite (LaCoO3) and substituted La1-xCexCoO3 (x=0.1, 0.3, 0.5, 0.7, 0.9) catalysts were prepared by the self-combustion method [13]. Glycine (H2NCH2CO2H), used as ignition promoter, was added to an aqueous solution of metal nitrates with the appropriate stoichiometry in order to get a NO3-/ NH2 (molar ratio) = 1. The resulting dissolution was slowly evaporated until a vitreous green gel was obtained. The gel was heated up to around 250°C, temperature at which the ignition reaction occurs producing a powdered precursor. The solids were crushed and sieved to obtain the required particle size (<200 μm) prior to calcination at 700°C in air for 10 h to eliminate the remaining carbon. Even though in some of the calcined solids the perovskite structure is not reached, for uniformity it has been maintained the nomenclature La1-xCex-CoO3. To study the thermal stability in hydrogen, the calcined perovskites were reduced under pure hydrogen flow (50 mLmin-1) at 500°C for 2 h. After, the reactor was purged with nitrogen and cooled down to room temperature, placed in a cryostatic bath and a flow of 5%O2/Ar was admitted into the reactor for 1 h. Afterwards, it was purged for 30 min with N2 under the same cryostatic conditions and finally the bath was removed and the catalysts were stabilized at room temperature. These materials are referred as reduced samples in this paper.

2.2 Characterization

Chemical analysis of the samples was carried out by atomic absorption spectroscopy (AAS) using a Perkin Elmer instrument model 3100. Samples were dissolved in HCl and HNO3 acids dissolutions and then appropriately diluted to get concentrations of lanthanum, cerium and cobalt within the calibration range of the instrument. Specific surface (SS) areas were calculated using the BET method from the nitrogen adsorption isotherms, recorded at 77 K on a Micromeritics apparatus Model ASAP 2010. X-ray powder diffraction (XRD) patterns were obtained with nickel-filtered CuKα1 radiation (λ = 1.5418 Å) using a Rigaku diffractometer controlled by a computer. TPD-O2experiments were performed in a TPR/TPD 2900 Micromeritics system with a thermal conductivity detector. The samples were exposed to oxygen for 1 h at 600°C, followed by cooling to room temperature in the same atmosphere. After switching the atmosphere to a helium flow, the sample was heated at a constant rate of 10°Cmin-1 and the desorbed oxygen was monitored with a thermal conductivity detector. Temperature programmed reduction (TPR) experiments were performed in a TPR/TPD 2900 Micromeritics system with a thermal conductivity detector. Samples were placed in a U-shape quartz tube and purged in a synthetic air stream of 50 mLmin-1 at 500°C for 1 h and then cooled to ambient temperature. A cold-trap was placed just before the TCD of the instrument to remove the water from the exit stream.

2.3 Catalytic activity

The catalytic activity of the solids was investigated using carbon black (CB) as model of soot. The catalyst-CB mixture for the assessment of the catalytic activity was prepared mixing 4 mg of CB and 16 mg of catalyst in tight contact. The catalytic oxidation of the CB was carried out in a thermogravimetric apparatus (Netzch 409 PC) with 7.5 mg of the mixture heated in 180 mLmin-1 flow of air at 10°Cmin-1 up to 800°C. The combustion rate was normalized dividing by the initial weight of CB in each sample. The temperature at which combustion occurs at the maximum rate, denoted as Tm, and the catalytic activity index (CAI) defined as the difference between the temperatures for the catalyzed and uncatalyzed reaction, that is: CAI=(Tm)uncat - (Tm)cat was taken as a measure of catalytic activity[14].

3. RESULTS

3.1 Catalytic Activity

Figure 1 shows the DTG curves for CB combustion of the calcined (solid line) and reduced (dotted line) solids. The catalytic activity is estimated from the temperature corresponding to the maximum of DTG curve, Tm. Higher values for Tm means lower catalytic activity. The Tm for the uncatalized CB combustion is 650°C, so all tested samples exhibit a significant catalytic activity; even the less active solid, LaCoO3, decreases the Tm value in about 200°C. It is also observed that the catalytic activity of calcined samples (solid lines) increases with the increase of the cerium content in the catalyst, and the higher CAI is observed for La0.1Ce0.9CoO3, which is the sample with the highest Ce/La mass ratio (Fig. 1).

 

Figure 1. Thermogravimetric assays for the catalytic
combustion of CB. (—) calcined, () reduced.

 

In order to evaluate the effect of perovskite-type structure on CB combustion reaction rate, the calcined samples were reduced in H2 at 700°C to destroy the perovskite structure. After that, the samples were again tested as catalyst for CB combustion (Fig. 1, dotted lines). It is observed that the reduction process did not significantly affect the catalytic activity of low-Ce-content samples (x = 0, 0.1, 0.3), while an important decrease of Tm value was observed for those samples with higher Ce content, which burned the soot at temperatures as lower as 354°C. Fig. 1 also shows that for the reduced samples with higher Ce content (x = 0.5, 0.7, 0.9) not only the Tm values decrease but also the maximum reaction rate for CB combustion increases. On the other hand, the lower La content in the catalysts the higher CAI value for both calcined and reduced samples (Fig.1, Table 1).

 

Table 1: Tm for La1-xCexCoO3 catalysts. Tm = 650°C for uncatalyzed
CB combustion.

 

3.2 Elemental composition

The Atomic Absorption Spectroscopy composition of the La1-xCexCoO-3samples shown in Table 2 indicatesthat experimental lanthanum, cerium and cobalt contents approach to the nominal ones.

 

Table 2: Bulk composition (wt%) and SS area for La1-xCexCoO3 catalysts.

1 Estimated error is below 1% (Nominal values are in parentheses)

 

3.3 Specific area

The BET areas of the calcined and reduced solids are summarized in Table 2. It can be seen that the reduction process decreases the surface area of the solids. The reduced cobaltite and the one with lower Ce content (x=0.1) exhibits the lowest SBET, of 7 m2g-1, and a progressive increase is observed for larger cerium-content samples, till the highest value of 14 m2g-1 for the highest Ce-content sample (x=0.9) is achieved. The obtained values for BET area of the calcined solids are in the range of previously reported for other lanthanum perovskites-type oxides [15, 16]. It is worth mentioning, that not always a direct relation between BET surface area of the catalyst and the combustion rate of carbon black have been previously observed for this type of heterogeneous catalytic reaction [2, 7, 17], since the catalytic combustion of soot takes place in the so-called triple contact point (catalyst-carbon black-O2), where the solid catalyst, the solid soot and the gaseous reactant meet together.

3.4 X-ray diffraction (XRD)

The samples calcined at 700°C (Fig.2, solid lines) with lower Ce content (LaCoO3, La0.9Ce0.1CoO3) show well defined perovskite crystal structure, with sharp reflections and absence of any other crystalline phases. Cobaltite (LaCoO3) belongs to a well crystallized rhombohedral structure ( JC-PDF-480123) in agreement with previous results [18]. Moreover, two different behaviors can be detected as a function of the Ce content in the solids. For samples with lower Ce content (x = 0.1, 0.3, 0.5) the diffraction profiles indicate presence of the rhombohedral structure of LaCoO3 perovskite, with the appearance of a diffraction peak at 2θ=28.7°, attributed to segregated CeO2 phase. Only for the higher Ce content, 0.5 it is also detected Co3O4 as segregated phase. It can be seen that the diffraction lines corresponding to CeO2 increases in line with the decrease of the diffraction peak at 2θ=33° corresponding to the perovskite-type structure. Moreover, the decrease in intensity of the line at 2θ=33° is accompanied with the disappearance of the characteristic doublet of the rhombohedral structure (2θ of 33°). It is noticeable no shift of the 20 values, indicating no distortion of the perovskite structure upon Ce substitution, an expected result due to the similar ionic radii of La3+ and Ce3+; 0.136 and 0.134 nm respectively. The diffraction patterns of larger Ce-content sample (x = 0.7, 0.9) show: i) absence of diffraction peaks attributed to the perovskite structure, which suggests that thermodynamic stability of perovskite structure is limited by the substitution degree of La by Ce, regardless of the similarity between ionic radii of La3+ and Ce3+; ii) absence of diffraction peaks attributed to single or mixed lanthanum oxides; iii) appearance of two new crystalline phases that corresponds to CeO2 (JC-PDF 340394) and Co3O4 (JC-PDF 421467). The lack of lanthanum diffraction patterns can be taken as indicative of highly dispersed lanthanum oxide formation as a consequence of calcination at 700°C; also the La oxide phase can be in an amorphous form or incorporated to CeO2. The XRD patterns of the calcined (solid lines) and the reduced (dotted lines) solids can be compared in Figure 2. Larger structure changes after H2 treatment at 700°C were observed for samples with lower Ce content (x0.3), while calcined and reduced samples with higher Ce content (x = 0.7, 0.9) show very similar XRD patterns. For the samples with lower Ce content (x = 0.1, 0.3, 0.5) the most intense diffraction peak of the perosvkite-type structure (2θ=33°) fully disappears after reductive treatment, indicating a low thermal stability in H2 atmosphere. The diffraction lines of the reduced solids indicate the presence of La2O3, La2CoO4, CeO2 as segregated phases as well as Co°, which appears in the two broad peaks at 2θ=44.3° and 51.5°, probably in a high dispersion degree. For x0.5, a careful inspection of the diffraction profiles reveals no significant changes in the crystalline structure after hydrogen treatment and absence of diffraction lines belonging to single or mixed lanthanum oxides. Since the reduced samples with higher Ce content showed the higher catalytic activity for soot combustion, the effect of reductive treatment on the CeO2 mean crystal size was evaluated by using the Debye Scherrer equation. The diffraction line at 2θ=28.7° was used to calculate the mean crystallite size of CeO2 and the results are shown in Figure 3. It is observed no effect of reductive treatment on the CeO2crystal size for samples with low Ce content. Moreover, for calcined samples the CeO2 crystal size seems to be independent of the Ce content. On the contrary, the CeO2 particle size increases with the Ce content for higher-Ce-content samples after H2 treatment at 500°C.

 

Figure 2. XRD profiles for La1-xCexCoO3 catalysts: a) calcined; b) reduced.

 

Figure 3. CeO2 mean particle size for La1-xCexCoO3
catalysts. (Δ) calcined; () reduced

 

Besides surface area and crystalline structure characterizations, the surface redox properties of the catalysts, i.e., reducibility (TPR) and surface oxygen stability (TPD-O2) were also measured, since these properties have shown to be closely related with the catalytic activity for soot combustion [19].

3.5 Temperature-Programmed Reduction (TPR)

The temperature-programmed reduction profiles (TPR) shown in Figure 4 indicate that for pure LaCoO3 the reduction process does not occur in a single step. The first reduction peak at 365°C corresponds to an intermediate oxygen-deficient perovskite structure (LaCoO3-6) and the complete reduction of the perovskite, with formation of La2O3, La(OH)3, H2O and Co° corresponds to the second reduction peak at 530°C [20]. The one at lower temperatures is attributed to surface oxygen species, while the reduction of the cobaltite structure (LaCoO3 = 1/2 La2O3 + CoO + 1/4 O2) occurs at higher reduction temperature. Upon Ce content, broader peaks with a progressive decrease in the reduction temperature of cobalt with the reduction of cerium between the two reduction peaks of cobalt can be clearly seen in Figure 4. The shift of the reduction peaks to lower temperatures implies an increase in the reducibility of the catalysts. Since soot oxidation, is a redox reaction, it is expected that the enhancement of the low-reducibility of the catalysts must have a positive effect in the catalytic activity to the soot combustion.

 

Figure 4. Temperature-programmed reduction profiles
for La1-xCexCoO3 catalysts.

 

3.6 Oxygen-Temperature Programmed Desorption (O2-TPD)

The evolution of oxygen during temperature-programmed desorption (O2-TPD) experiments are also closely related to the redox properties of the catalysts[21]. It is well known that depending on the oxygen desorption temperatures, physical, α-oxygen's and β-oxygen's can be detected. Physical oxygen's correspond to the low desorption peak centered at □80°C, which comes likely from weakly held oxygen species. The namely α-oxygen's are ascribed to adsorbed oxygen at oxygen vacancies that desorbs between 200°C to 500°C [22] and the so-called β-oxygen associated with the lattice oxygen desorbs up to 600°C with partial reduction of the B site metal to lower oxidation state[23]. These desorbed oxygen species are of less importance in soot combustion since the reaction occurs at lower temperature. Figure 5 displays the obtained O2-TPD profiles. The large desorption peaks located at ~90°C indicates the presence of weakly physisorbed oxygen species, with no dependence of the Ce content and not related with catalytic activity. Meanwhile, a beneficial effect in the α-oxygen's can be related with the Ce content. The importance of the surface oxygen's species is their close relation with the oxygen vacancies in the perovskite structure, that can activate the molecular oxygen forming active oxygen species in the ABO3 structure[24]. Since TPD-MS experiments confirm that the evolved gas and the He flow only contain oxygen, the deconvolution of the oxygen desorption curves using a Lorentzian peak shape allow to calculate the amount of desorbed oxygen. The obtained profiles were deconvoluted and only the desorbed oxygen corresponding to the α-oxygens are displayed in Table 3. It can be seen a continuous increase with Ce content. The larger activity of the higher Ce substituted catalysts indicates availability of reactive oxygen species on the catalytic surface, attributed to the weaker oxygen binding [25]. In this way, it is proposed that the gaseous oxygen may be dissociatively adsorbed on the surface of the metal oxide forming an oxygen adsorbed species that can react with the reactive free carbon site to give a highly reactive oxygen-carbon intermediate which can react either with the Oads or gaseous O2 to form CO or CO2[26]. In the catalytic oxidation reaction using mixed oxides or perovskites types oxides as catalysts, the oxygen surface oxygen species (O-, O2-, O2-) involved in the catalytic process may come from the molecular oxygen in gas phase, surface oxygen's or lattice oxygen. The promotional effect of ceria on cobaltite explain the catalytic effect in these catalysts, in line with previous results reporting that structural defects and oxygen mobility are important factors controlling the catalytic activity of these type of crystalline structures [27].The larger catalytic activity of the two catalysts with larger Ce content (x=0.7 and 0.9) is in agreement with previous result of the enhanced in the catalytic soot oxidation by lattice oxygen via La3+-doped CeO2 in the CeO2/soot interface [28-30].

 

Table 3: Detected XRD phases and desorbed oxygen for La1-xCexCoO3 catalysts.

 

Figure 5. Oxygen desorption profiles for La1-xCexCoO3 catalysts.

 

4. DISCUSSION

All samples tested in this study show significant catalytic activity for soot combustion. Perovskite LaCoO3 and low-Ce-content samples (x0.5) with well-defined perovskite-type structure (Fig 2) reduce the Tm value in more than 200°C. However, this catalytic activity practically did not change after perovskite structure destruction with sample reductive treatment at 500°C (Fig 1). These results are inconsistent with the catalytic role attributed to perovskite-type structures and hardly support the recently proposed mechanism for soot combustion on lanthanoid perovskites, in which the oxidation of soot particles is attributed to the surface oxygen species, which migrate from the perovskite structure [31, 32]. Moreover, Fig 1 shows a higher catalytic activity for calcined samples with higher Ce content (x=0.7, 0.9), in which XRD patterns show CeO2 and Co3O4 crystal phases instead of perovskite-type structure. These results suggest that CeO2 is playing the main role in soot combustion, which is in agreement with the higher catalytic activity of ceria oxide reported for soot combustion [33]. Moreover, the oxygen storage capacity of samples increases with Ce content as observed in Fig 5. Since XRD patterns (Fig 2) show an increase in the intensity of CeO2 peaks with Ce content, it is inferred that CeO2 crystals directly participates in the oxygen storage and exchange process. It is also important to note that H2 reduction process (destruction of perovskite-type structure) increases the catalytic activity for all the samples but in a different degree; samples with low CeO2 content (x0.5) slightly increased their activity while samples with higher amount of CeO2(x=0.7, 0.9) strongly increased the activity for soot combustion after reductive process. Also, reduced samples with higher Ce content (x=0.7-0.9) show an increase in CeO2 mean crystal size as shown in Fig 3. The same phenomenon was not observed for the calcined samples, in which the CeO2 particle size was insensible to Ce sample content increasing. These results suggest that the activity of these materials for soot combustion is improved by two factors: i) the increasing of CeO2 content and ii) the formation of larger CeO2 crystals in the higher-Ce-content samples after H2 reduction. In fact, it was observed a similar CeO2 mean particle size for all calcined samples, while the catalytic activity increases with the Ce content as a consequence of a larger CeO2 total surface, in which the oxygen can be activated and transferred to CB surface through more abundant catalyst-CB contact points. In the same way, the catalytic activity of reduced samples is improved by the increasing of CeO2 amount, but additionally, larger CeO2 crystals were formed in the samples with higher Ce content (x=0.7-0.9), which could explain the stronger decrease of Tm values when these samples were used as catalyst for soot combustion. Catalytic activity for soot combustion is closely related to higher material capacity for oxygen transfer from catalyst to carbonaceous surface[34]. Thus, the higher amount of CeO2 crystals in the sample, the higher oxygen storage in the catalytic surfaces and more contact point between catalyst and CB, through which active oxygen species attack the carbon material. This explains the reducing of Tm value with the increasing of CeO2 content for all the tested samples. Since XRD patterns (Fig. 2) show the presence of Co3O4 in calcined samples with higher Ce content (x=0.7-0.9), the effect of cobalt oxide is not disregarded, however, the cobalt oxide composition in both samples is the same, so this work does not provides evidences to attribute the observed catalytic activity for soot combustion to this specific phase. The reduction processes with H2 neither reduce the CeO2 to metallic Ce nor affect the Ce material composition; however, this treatment did cause dissimilar increasing of catalytic activity as a function of sample Ce content. Fig. 1 demonstrates that reduced samples with lower Ce content (x0.5) showed a minor improvement of catalytic activity than high-Ce-content samples (x=0.7-0.9) (Fig. 1), as a result of the increasing of CeO2 crystal size in these samples (Fig. 3). These results confirm that cerium oxide represents the main active phase in these materials, so the higher catalytic activity for soot combustion is related to an increase in the CeO2 sample content, which improves the oxygen exchange and number of contact points between catalyst and soot. Additionally, our results provide evidences of structural sensitivity of active oxygen species formation over CeO2, since larger CeO2 crystals showed higher activity for CB combustion than smaller ones, for comparison between samples with the same CeO2 composition. Afterward, the formation of active oxygen species and their transfer from CeO2 to carbonaceous material seems to be favored in large crystals rather than small ones, since a higher availability of lattice oxygen for oxygen exchange with gas phase is expected in larger crystal faces than in edges and corner, the later proportionally more abundant in small particles. Moreover, the transfer of oxygen species from edges and corners of CeO2 crystals would be affected by the stronger binding of oxygen atoms. Bueno-López et al.[29, 30] used labeled (O18) in gas phase and non labeled (O16) in catalysts to probe that the gas-phase labeled oxygen replaces non labeled lattice oxygen, creating the highly active non labeled oxygen, which reacts with soot, giving CO and CO2. In this sense, our results not only indicate that this highly active oxygen is more abundant in those samples with higher CeO2 content, but also suggest that the reactivity of this oxygen species increase with the CeO2 crystal size. Bueno-López et al.[30] observed an important improvement of catalytic activity when CeO2 was doped with La. The authors relate this result with a decrease in the onset temperature at which Ce4+ is reduced to Ce3+, i.e. the doping with La increases Ce reducibility. The effect of La doping on CeO2 catalytic activity for soot combustion is not disregarded in this work, since La is present in smaller amount in those samples with higher catalytic activity (reduced x > 0.5). However, our results do not have strong evidences to support this idea.

5. CONCLUSIONS

La1-xCexCoO3 catalysts were synthesized, characterized and evaluated for the soot combustion. It was found an increase in the specific area upon Ce content. Since the ionic radii of cerium is similar to lanthanum, cerium can be introduced to the lattice for the substitution x0.5, while for larger Ce content (x0.7) formation of CeO2 phase is detected. The destruction of the perovskite-type structure in a reductive process increases the catalytic activity in a different degree; a slightly increased in the samples with low CeO2 content (x0.5) while those with higher amount of CeO2 (x=0.7, 0.9) strongly increased their activity for soot combustion. These results suggest that the activity of these materials for soot combustion is improved by two factors: i) the increasing of CeO2 content, closely related to higher material capacity for oxygen transfer from catalyst to carbonaceous surface and ii) the formation of larger CeO2 crystals in the higher-Ce-content samples after H2 reduction, responsible for the improvement of the oxygen exchange and number of contact points between catalyst and soot.

ACKNOWLEDGEMENTS

The authors thank CONICYT (Fondecyt Grant 1130005), Red Doctoral REDOC, MINEDUC project UCO1202 and Grant PFB-27.

 

REFERENCES

[1] J.O. Uchisawa, A. Obuchi, Z. Zhao, S. Kushiyama, Applied Catalysis B-Environmental, 18 (1998) L183-L187.         [ Links ]

[2] R. Jimenez, X. Garcia, T. Lopez, A.L. Gordon, Fuel Processing Technology, 89 (2008) 1160-1168.         [ Links ]

[3] M.A. Peralta, V.G. Milt, L.M. Cornaglia C.A. Querini, Journal of Catalysis, 242 (2006) 118-130.         [ Links ]

[4] Q. Li, M. Meng, F.F. Dai, Y.Q. Zha, Y.N. Xie, T.D. Hu, J. Zhang, Chemical Engineering Journal, 184 (2012) 106-112.         [ Links ]

[5] Z.Q. Li, M. Meng, F.F. Dai, T.D. Hu, Y.N. Xie, J. Zhang, Fuel, 93 (2012) 606-610.         [ Links ]

[6] G. Pecchi, B. Cabrera, A. Buljan, E.J. Delgado, A.L. Gordon, R. Jimenez, Journal of Alloys and Compounds, 551 (2013) 255-261.         [ Links ]

[7] G. Pecchi, B. Cabrera, E.J. Delgado, X. Garcia, R. Jimenez, Applied Catalysis a-General, 453 (2013) 341-348.         [ Links ]

[8] K. Taniguchi, N. Okinaka, T. Akiyama, Journal of Alloys and Compounds, 509 (2011) 4084-4088.         [ Links ]

[9] D. Fino, N. Russo, G. Saracco, V. Speechia, Journal of Catalysis, 217 (2003) 367-375.         [ Links ]

[10] P. Doggali, H. Kusaba, S. Rayalu, Y. Teraoka, N. Labhsetwar, Topics in Catalysis, 56 (2013) 457-461.         [ Links ]

[11] R.D. Zhang, N. Luo, B.H. Chen, S. Kaliaguine, Energy & Fuels, 24 (2010) 3719-3726.         [ Links ]

[12] G. Pecchi, C. Campos, O. Pena, Materials Research Bulletin, 44 (2009) 846-853.         [ Links ]

[13] L.A. Chick, L.R. Pederson, G.D. Maupin, J.L. Bates, L.E. Thomas, G.J. Exarhos, Materials Letters, 10 (1990) 6-12.         [ Links ]

[14] B. Jankovic, B. Adnadevic, S. Mentus, Chemical Engineering Science, 63 (2008) 567-575.         [ Links ]

[15] N. Russo, D. Fino, G. Saracco, V. Specchia, Journal of Catalysis, 229 (2005) 459-469.         [ Links ]

[16] N.A. Merino, B.P. Barbero, P. Grange, L.E. Cadús, Journal of Catalysis, 231 (2005) 232-244.         [ Links ]

[17] D. Fino, P. Fino, G. Saracco, V. Specchia, Applied Catalysis B-Environmental, 43 (2003) 243-259.         [ Links ]

[18] K. Poplawski, J. Lichtenberger, F.J. Keil, K. Schnitzlein, M.D. Amiridis, Catalysis Today, 62 (2000) 329-336.         [ Links ]

[19] D. Fino, N. Russo, E. Cauda, G. Saracco, V. Specchia, Catalysis Today, 114 (2006) 31-39.         [ Links ]

[20] G. Pecchi, C. Campos, O. Pena, L.E. Cadus, Journal of Molecular Catalysis a-Chemical, 282 (2008) 158-166.         [ Links ]

[21] H.M. Zhang, Y. Shimizu, Y. Teraoka, N. Miura, N. Yamazoe, Journal of Catalysis, 121 (1990) 432-440.         [ Links ]

[22] S. Ifrah, A. Kaddouri, P. Gelin, G. Bergeret, Catalysis Communications, 8 (2007) 2257-2262.         [ Links ]

[23] R.D. Zhang, A. Villanueva, H. Alamdari, S. Kaliaguine, Journal of Catalysis, 237 (2006) 368-380.         [ Links ]

[24] G. Pecchi, P. Reyes, R. Zamora, C. Campos, L.E. Caduus, B.P. Barbero, Catalysis Today, 133 (2008) 420-427.         [ Links ]

[25] D.V. Ivanov, L.G. Pinaeva, E.M. Sadovskaya, L.A. Isupova, Kinetics and Catalysis, 52 (2011) 401-408.         [ Links ]

[26] M.J. Illan-Gomez, C.S.M. de Lecea, A. Linares-Solano, L.R. Radovic, Energy & Fuels, 12 (1998) 1256-1264.         [ Links ]

[27] L. Marchetti, L. Forni, Applied Catalysis B-Environmental, 15 (1998) 179-187.         [ Links ]

[28] M. Machida Y. Murata, K. Kishikawa, D.J. Zhang, K. Ikeue, Chemistry of Materials, 20 (2008) 4489-4494.         [ Links ]

[29] A. Bueno-Lopez, K. Krishna, M. Makkee, J. Moulijn, Catalysis Letters,  99 (2005) 203-205.         [ Links ] 

[30] A. Bueno-Lopez, K. Krishna, M. Makkee, J.A. Moulijn, Journal of  Catalysis, 230 (2005) 237-248.         [ Links ]

[31] M.L. Fu, X.H. Yue, D.Q. Ye, J.H. Ouyang, B.C. Huang, J.H. Wu, H. Liang, Catalysis Today, 153 (2010) 125-132.         [ Links ]

[32] X.H. Yue, X. Zhang, M.L. Fu, B.C. Huang, H. Liang, D.Q. Ye, Chinese Journal of Inorganic Chemistry, 25 (2009) 1170-1176.         [ Links ]

[33] E. Aneggi, J. Llorca, C. de Leitenburg, G. Dolcetti, A. Trovarelli, Applied  Catalysis B-Environmental, 91 (2009) 489-498.         [ Links ]

[34] R. Jimenez, R. Zamora, G. Pecchi, X. Garcia, A.L. Gordon, Fuel Processing  Technology, 91 (2010) 546-549.         [ Links ]

 

Creative Commons License All the contents of this journal, except where otherwise noted, is licensed under a Creative Commons Attribution License