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Catalysts 2018, 8(9), 388; doi:10.3390/catal8090388
Rational Design of High Surface Area Mesoporous Ni/CeO2 for Partial Oxidation of Propane
Chemical Engineering Department, Catalyst and Advanced Materials Research Laboratory, Faculty of Engineering, University of Kashan, Kashan 8731751117, Iran
Chemical Engineering Department, Iran University of Science and Technology, Tehran 1684613114, Iran
Laboratory of Advanced Catalysis for Sustainability, School of Chemistry, University of Sydney, Sydney 2006, Australia
Authors to whom correspondence should be addressed.
Received: 4 August 2018 / Accepted: 2 September 2018 / Published: 10 September 2018
A Ni loaded catalyst on mesoporous ceria, with a large surface area, prepared through the surfactant-assisted precipitation and impregnation method was investigated as an efficient catalyst for propane partial oxidation to produce synthesis gas. The results show that 2.5 wt% Ni/CeO2 had the optimum Ni loading, exhibiting the highest catalytic propane conversion. It also showed excellent stability, with no obvious activity drop after a 10 h time-on-stream reaction and slightly decreased in H2 and CO yields. The investigation of the reactant composition effect on carbon formation showed that by decreasing the C/O2 ratio the content of accumulated carbon decreased and propane conversion increased. The good activity of the Ni/CeO2 can be ascribed to the high surface area and rich surface defects of the ceria support and a high dispersion of active sites (Ni nanoparticles).
Keywords:partial oxidation of propane; nickel catalysts; mesoporous ceria; coke deposition
The utilization of light hydrocarbon compounds, such as butane and propane, will become vital as liquid resources decrease in the future. Although abundant, resources including natural gas encounter difficulties such as storage and transportation. One effective strategy is to convert these light hydrocarbons into syngas (a mixture of CO and H2 with different ratios), which can be processed into chemicals (i.e., ammonia and methanol) by a variety of technologies [1,2,3]. Furthermore, light hydrocarbons can be readily stored, transported and distributed as a raw material for syngas production. In addition, propane has many benefits, it can be used worldwide as a fuel and is very abundant and it is compressible to a transportable liquid at a normal temperature [4,5]. The syngas can be produced through different routes, such as liquid and gaseous fuels by steam and combined reforming processes or non-catalytic and catalytic partial oxidation [6,7]. The steam reforming of hydrocarbons is a process with a high cost for operation and this process also needs high energy whereas catalytic partial oxidation (CPO) demands no external heat sources . However, the decline in catalytic activity during the reaction, because of carbon growth, is the main challenge [9,10,11]. Ni-catalysts have been widely used in CPO reactions due to their low cost and good performance, but they are not resistance against sintering and carbon formation [4,12,13]. Previous research shows that by using a catalyst support, the catalytic activity and the anti-coke-formation property can be significantly improved due to the high dispersion of the active phase [14,15,16]. CeO2 has been used as one of the most promising supports due to its special characteristics such as various interconvertible oxidation states and rich surface defects, which can assist the metal dispersion, carbon elimination, improve the metal-support interaction and minimize the metal sintering [17,18,19,20,21].
In this work, we have developed a nanocrystalline nickel catalyst loaded on mesostructured CeO2, with a high specific surface area for the propane partial oxidation reaction to produce syngas. This reaction system was well studied by evaluating the influences of the feed ratio and (gas hourly space velocity) GHSV on the catalytic performance of the optimized Ni/CeO2. Furthermore, the carbon deposition phenomenon on the as-prepared catalyst, under different reaction conditions, was investigated.
2. Results and Discussion
2.1. Textural Properties
The XRD measurements, carried out on the reduced catalysts (600 °C) with various Ni percentages, are illustrated in Figure 1. The diffractions located at 28.67, 33.22, 47.69, 56.6, 59.36, 69.75, 77.08 and 79.47° were attributed to the fingerprints of the standard cubic CeO2, which verified the pure phase of the prepared CeO2 supports. In the lower Ni loading samples (2.5Ni/CeO2), no apparent peaks related to the Ni crystal phase were found. As the nickel loading increased, diffraction peaks located at 44.5° and 51.8° were observed in the patterns, which are related to the plane (111) and (200) of the metal Ni (JCPDS. 004-0850), respectively. The XRD peaks of the Ni/CeO2 samples showed that along with the increase of nickel loading, the intensity of the ceria peaks decreased. The sizes of the nickel crystals are presented in Table 1. The size of nickel crystals grew from 8.8 to 15.6 nm by the increase in Ni loading.
The structural parameters of the ceria and reduced samples are reported in Table 1. CeO2 indicated a large specific surface area of 138 m2/g and the rise in nickel loading decreased the volume of pores and BET area because of the regional pore-blocking caused by the sintering nickel and/or the collapse of the mesopores at a relatively high reduction treatment. Increasing the nickel percentage did not notably affect the diameter of the pores. It is known that the appropriate Ni percentage results in the creation of nickel oxide particles with a high dispersion and surface area . The isotherm of N2 adsorb-desorption of the CeO2 and reduced Ni/CeO2 is presented in Figure 2a. It shows that all the samples exhibit the type IV isotherm, which is typical for powders containing mesopores. The CeO2 support possessed the H2 type hysteresis loop, which is generally attributed to a cylindrical-shaped channel structure. However, for the reduced Ni/CeO2 catalysts, the hysteresis loop changed to H1 type, which is assigned to pores with an ink-bottle shape . Furthermore, it can be seen from the pore size distributions in Figure 2b that all catalysts presented a porous texture with an average pore size of 4–15 nm. An increase in Ni content resulted to a narrower size distribution.
2.2. TPR Analysis
The results of the H2-TPR analysis are displayed in Figure 3. The H2-TPR profile of ceria as a support illustrated two reduction peaks. The first peak, at low temperatures, is referred to as the adsorbed oxygen on the surface defects of ceria and the second one, at around 600 °C, is attributed to the evolution of Ce4+ to Ce3+ in bulk. As shown in the Ni/CeO2 samples, three peaks can be seen in the H2-TPR profiles, which suggests the reduction of three types of reducible metal oxide species named as α, β and γ from low to high temperature. The α peak with low intensity, observed at low temperature (170–360 °C), was assigned to the surface oxygen located in the defects of the CeO2 surface. The β peak, observed around 400 °C, corresponded to the NiO species that interacted weakly with CeO2. The γ-peak, at about 500 °C, was caused by the reduction of NiO strongly interacting with the CeO2 substrate . It was seen that the rise in Ni percentage caused the shift of the γ peak towards higher temperatures due to the stronger interaction between NiO and CeO2. This indicated that a higher concentration of metallic nickel was achieved in catalysts with higher percentages of nickel. In addition, the area of reduction peaks in the TPR profile of the catalysts, with a higher percentage of nickel, was higher than the area detected for the catalysts with a lower Ni content, which was due to higher volume of hydrogen needed for the reduction of the catalyst with a higher Ni content [17,23].
2.3. Catalytic Characteristics
2.3.1. Influence of Operating Temperature and Ni Loading
The influence of the nickel percentage and temperature of the reaction on the catalytic performance was studied, as displayed in Figure 4a. C3H8 conversions increased when the temperature increased from 300 to 700 °C. As can be seen, the obtained Ni/CeO2 catalysts exhibited 35–45% conversion at low temperature (≤400 °C), while the propane partial oxidation was performed at a higher temperature in most of the previous works [4,24,25,26]. The results show that C3H8 conversion improved as the increment of nickel percentage was increased from 1.5 to 2.5 wt%, which is because of the increase in the total number of active sites (nickel) but a further increase results in a decrease in propane conversion. The 2.5% Ni/CeO2 exhibits the best activity among all samples (~80% conversion at 600 °C). In general, the molar ratio of H2/CO decreased with the rise in temperature of the reaction when the reverse water gas shift reaction (RWGS) occurred (Figure 4b) . Wang reported that the 2 wt% Ni-CeO2 possessed the best catalytic performance in the RWGS reaction and higher nickel loading resulted in a decrease in CO2 to CO conversion. Therefore, with an increasing nickel content, over 2.5% Ni, the RWGS reaction rate decreased, the CO2 and H2 yields increased, and the CO yield decreased . The yields of H2 and CO can be found in Figure 4c,d, which exhibited improvement with an increased temperature of 600 °C and then declined due to the formation of by-products at a temperature of 700 °C. When the Ni content was increased, the H2 yield increased and the CO yield decreased.
The by-product selectivity is illustrated in Figure 5a. The methane selectivity at different temperatures suggested that the 2.5% Ni/CeO2 catalyst shows the highest selectivity to methane. It is shown that this catalyst converts the carbonate intermediates on the surface of the catalyst to CH4 instead of CO2. The lowest methane selectivity is seen at 600 °C in all catalysts. A decrease in the selectivity to carbon dioxide was observed along with the rise in temperature (Figure 5b), which is caused by RWGS and CO2 consumption [26,29]. Ethane, ethylene, and propylene formation occurred at a temperature over 600 °C. The best operating temperature for C3H8 partial oxidation was selected as the temperature which yielded the highest amount of hydrogen and the least amount of the by-products. Thus, it indicated that the maximum hydrogen and minimum by-product production occurred at 600 °C for C3H8 .
The physical properties of the catalysts after the reaction are presented in Table 1. The specific surface area and volume of the pores were drastically affected by the reactivity sintering of the catalysts and the deposition of carbon at high temperatures. The deposited coke can fill the pores and decrease the BET surface area.
2.3.2. Influence of GHSV
Figure 6 shows how the GHSV influenced the conversion of C3H8 and yield of H2 and CO for the 2.5% Ni/CeO2 sample under normal conditions (600 °C, C3H8:O2 = 1:1.5, C3H8 = 10%). As the GHSV was increased from 15,000 to 90,000 mL/(gcat·h), the C3H8 conversion and CO yields increased. However, no obvious influence of GHSV variation was observed for the H2 yield. The reason can be attributed to the extra heat released from the reaction to the catalyst bed due to the increased feed flow. It has been reported in the literature that increasing the GHSV can raise the catalyst temperature .
2.3.3. Influence of Feed Gas Composition
The effect of the feed gas (C/O2) on the activity and selectivity of the sample has been studied as displayed in Figure 7. It shows that the O2 amount has a negligible influence on the propane conversion, rich O2 can promote the oxidation reaction. At lower C/O2 ratios, complete combustion was more favorable than partial oxidation. As a result, a high content of CO2 and H2O were generated. The selectivity of CO2 declined drastically while the selectivity of CH4 remained constant. The H2 and CO yields increased when the C/O2 increased, which was derived from the complete oxidation of propane. Therefore, the lower the C/O2 ratio, the lower the selectivity of hydrogen. Due to the small amount of CH4, H2 can be consumed by the extra oxygen, resulting in a higher H2O selectivity .
2.3.4. Stability Test
The stability of the 2.5% Ni/CeO2 catalyst was evaluated under the time-on-stream reaction at 700 °C for 600 min and the results can be seen in Figure 8. The sample possessed good catalytic stability with no obvious drop in C3H8 conversion. Figure 8 shows that the yields of CO and H2 decreased slightly, which arose due to the production of C2H4, C2H6, and C3H6 as by-products. The formation of by-products may occur by oxidation of the nickel metal or deposition of carbon on the active phase.
2.4. TPO Analysis
The influence of the C/O2 ratio and reaction temperature on the amount of accumulated carbon over 2.5% Ni/CeO2 was investigated by TPO analysis in Figure 9a,b. It indicates that as the ratio of C/O2 decreased, the carbon deposition decreased and no carbon species were detected at a low C/O2 ratio (1.33). It is well known that the rich oxygen adsorbed on surface defects of a cerium support can assist the decomposition of carbon deposition and prevent carbon formation. Also, thermodynamic calculations, based on the free energy minimization method, show that the possibility of carbon generation is maximized at a maximum C/O2 ratio [13,32]. From Figure 9b, one can observe that as the reaction temperature increases, the peak area of TPO drops. This means that carbon does not tend to form at higher temperatures, which is because the exothermic characteristic of CO disproportionation is unfavorable at high reaction temperatures from a thermodynamic viewpoint [33,34,35].
The SEM results of the used 2.5% Ni/CeO2 catalyst under various C/O2 ratios are shown in Figure 10. It shows that the decrease in C/O2 ratio reduces the content of whisker carbon. As observed in Figure 10, no detectable carbon was observed at C/O2 = 1.33. This has verified the TPO analysis, which shows a smaller amount of deposited carbon at a lower C/O2 ratio. Morphological properties of the used 2.5% Ni/CeO2 catalyst, as illustrated in Figure 11, were evaluated under different temperatures. As shown, the whisker carbon does not tend to form when the temperature is increased.
3. Experimental Section
3.1. Catalyst Synthesis
The CeO2 support with mesostructure was prepared using the surfactant-assisted precipitation method modified from our previous work . In summary, a precipitation agent was added dropwise to a prepared cerium and a cetyl trimethylammonium bromide) CTAB (mixed solution at ambient temperature. The pH value of the solution was adjusted to 11. Then, the slurry was aged, filtered, washed and finally calcinated. The nickel was loaded onto the CeO2 support through a simple impregnation route. The prepared CeO2 was immersed in a nickel nitrate solution, with the desired concentration, to prepare the nickel catalysts with a calculated nickel percentage. The suspension was stirred for 3 h, at ambient temperature, and was placed at 80 °C for drying prior to calcination at 600 °C for 3 h. The Ni/CeO2 with 2.5, 5, 7.5 and 10 wt% Ni content were defined as 2.5Ni/CeO2, 5Ni/CeO2, 7.5Ni/CeO2, and 10Ni/CeO2, respectively. The atomic absorption technique was used to compare the actual Ni loadings with theoretical values.
3.2. Catalytic Performance
The propane partial oxidation reaction was conducted in a constant flow-fixed bed microreactor, loaded with 100 mg catalyst. Each sample was initially pretreated in an H2 atmosphere at 600 °C for 3 h. In a typical reaction test, the feed gas consisted of the stoichiometric molar ratio of C3H8 and O2 (C/O2 = 2) balanced in He gas. The catalytic activity was evaluated from 300 to 700 °C. The continuous outlet gas with unreacted reactants and products was introduced to the gas chromatograph (Younglin) for analysis (HID detector and Carboxen 1010 column) after holding the catalyst for 90 min at each temperature. The test was repeated three times for each catalyst, and an average value of the results was used for calculating the conversions and selectivities. The desired reaction equation and the C3H8 conversions, CO and H2 yields, and selectivities of CO2, CH4, C2H6, C2H4 and C3H6 were calculated according to the following equations :where Fin and Fout represent the inlet and outlet flow rates of the mixed gas. A carbon balance was used to calculate Fout. n represents the molecular including CO, CO2, CH4, C2H6, C2H4 and C3H6.
The X-ray diffraction (XRD) pattern of the samples was measured on a PANalyticalX’Pert-Pro diffractometer with Cu Kα radiation (λ = 0.15406 nm) at 40 mA and 45 kV in the range of 10–80° (2θ). BET surface areas and pore size distributions were analyzed through N2 adsorption and desorption at −196 °C on a BELSORP-mini II adsorption analyzer. The mean pore diameter was calculated from D = 4VT/SBET. In this equation, V is the total pore volume and S is the specific surface area of the pore that is usually obtained using the BET model. Temperature programmed reduction and oxidation (TPR and TPO respectively) tests were performed on a Chemisorb 2750 Micromeritics instrument, with a thermal conductivity detector. The surface morphology of the used catalyst was investigated using a [email protected] scanning electron microscope (SEM). The actual nickel loading of catalysts was measured with a GBC atomic absorption spectrophotometer.
A series of mesoporous CeO2 catalysts with different nickel loadings were successfully fabricated and employed in propane partial oxidation. The reduced catalysts exhibited pore sizes in the mesoregion (4–15 nm). The catalytic results show that the prepared Ni/CeO2 catalysts possessed a high propane conversion at a temperature lower than 500 °C and the 2.5% Ni/CeO2 exhibited the best catalytic activity. The increase in nickel loading over the 2.5% Ni enhanced the H2 yield and suppressed the CO yield. The investigation of reaction temperature for propane partial oxidation confirms 600 °C as the optimal temperature. A total of 2.5% Ni/CeO2 exhibited a high stability during the long-term reaction. The post-reaction TPO and SEM results indicate that increasing the C/O2 ratio in feed and decreasing the reaction temperature led to surface carbon deposition on the catalyst.
M.P. performed catalyst synthesis, characterization and activity testing. S.M.A., H.A. and M.R. provided technical and scientific support as well as played a supervisory role in the research. The manuscript was prepared by M.P., H.A. and M.R., and revised by all the authors.
This research received no external funding.
Conflicts of Interest
The authors declare no conflict of interest.
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Figure 1. XRD profiles of the Ni/CeO2 catalysts.
Figure 2. (a) N2 adsorption-desorption isotherms and (b) pore size distributions of the reduced samples.
Figure 3. H2-TPR of as-obtained samples.
Figure 4. (a) C3H8 conversion. (b) Ratio of H2/CO, yield of (c) H2 and (d) CO versus reaction temperature. The reaction conditions follow: GHSV = 60,000 mL/(gcat·h), C/O2 = 2, C3H8 = 10%.
Figure 5. (a) CH4 selectivity and (b) CO2 selectivity, C/O2 = 2, GHSV = 60,000 mL/(gcat·h), C3H8 = 10%.
Figure 6. C3H8 conversion (XC3H8), yield of H2 (YH2) and yield of CO (YCO) of 2.5%Ni/CeO2 versus GHSV, T = 600 °C, C/O2 = 2, C3H8 = 10%.
Figure 7. Conversion yield of H2 and CO, and selectivity of H2 and CO of 2.5%Ni/CeO2 versus the C/O2 ratio. T = 600 °C, GHSV = 60,000 mL/(gcat·h), C3H8 = 10%.
Figure 8. Long-term reactivity test of 2.5%Ni/CeO2 at T = 700 °C, GHSV = 60,000 mL/(gcat·h), C/O2 = 2, C3H8 = 10%.
Figure 9. TPO results of 2.5% Ni/CeO2 show the effects of (a) C/O2 ratios (T = 600 °C, GHSV = 60,000 mL/(gcat·h), C3H8 = 10%) and (b) reaction temperatures (C/O2 = 2, GHSV = 60,000 mL/(gcat·h), C3H8 = 10%).
Figure 10. SEM results of used 2.5% Ni/CeO2 catalyst after an activity test under the condition of (a) C/O2 = 1.33; (b) C/O2 = 2 and (c) C/O2 = 4 (T = 600 °C, GHSV = 60,000 mL/(gcat·h), C3H8 = 10%, time = 10 h).
Figure 11. SEM results of spent 2.5% Ni/CeO2 catalyst after an activity test under a reaction temperature of (a) 500 °C, (b) 600 °C and (c) 700 °C (C/O2 = 2, GHSV = 60,000 mL/(gcat·h), C3H8 = 10%, time = 10 h).
Table 1. BET surfaces areas, pore volumes and crystal sizes of the support from reduced and spent catalysts.
|Sample||BET Surface Area (m2/g)||Pore Volume (cm3/g)||Pore Diameter (nm)||Ni Crystallite Size (nm)|
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