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Catalysts 2012, 2(2), 264-280; doi:10.3390/catal2020264
Abstract: Magnesium nickel silicate (MNS) has been investigated as a catalyst to convert tars and light hydrocarbons to syngas (CO and H2) by steam reforming and CO2 reforming in the presence of H2S for biomass gasification process at NexTech Materials. It was observed that complete CH4 conversion could be achieved on MNS catalyst granules at 800–900 °C and a space velocity of 24,000 mL/g/h in a simulated biomass gasification stream. Addition of 10–20 ppm H2S to the feed had no apparent impact on CH4 conversion. The MNS-washcoated monolith also showed high activities in converting methane, light hydrocarbons and tar to syngas. A 1200 h test without deactivation was achieved on the MNS washcoated monolith in the presence of H2S and/or NH3, two common impurities in gasified biomass. The results indicate that the MNS material is a promising catalyst for removal of tar and light hydrocarbons from biomass gasified gases, enabling efficient use of biomass to produce power, liquid fuels and valuable chemicals.
As renewable energy, biomass conversion has gained more interest in recent years because of concerns related to global warming, gradual decreases in the known reserves of fossil fuels and increases in fossil fuel consumption. Gasification is an attractive route to convert biomass to syngas (CO + H2), which can be used in internal/external combustion engines, gas turbines and fuel cells for power generation, or further converted into hydrogen and liquid fuels such as methanol, dimethyl ether, ethanol, gasoline and diesel [1,2]. For biomass gasification, efficient cleaning and conditioning of the derived syngas is a significant barrier to commercializing this technology. Raw syngas contains impurities, such as sulfur, ammonia, tars, light hydrocarbons and methane. The methane and light hydrocarbons comprise un-used biomass carbon and hydrogen, which decrease the energy utilization efficiency. The tars mainly consist of polycyclic aromatic compounds with high boiling points, which will condense in the downstream process equipment. Therefore, these contaminants (e.g., tars) need to be removed from the gasification product gases.
Currently, two approaches are widely used for cleaning tars from biomass gasification product gases: liquid scrubbing and catalytic reforming. Liquid scrubbing removes tar in a condensed form. This approach requires the gasification products to be cooled to low temperatures, resulting in a loss of thermal efficiency. It also creates a liquid waste which needs to be further treated for disposal. In comparison, catalytic reforming of tar to syngas at high temperatures is a promising approach from an economic standpoint as it can utilize the sensible heat in the syngas, decrease the capital cost with simpler cooling systems, and enhance overall energy efficiency. It also converts the tar, methane and light hydrocarbons to syngas, increasing the fuel value.
Many catalysts have been reported to be active for tar reforming in the literature [3,4,5,6,7,8,9,10,11,12,13,14,15,16,17,18,19,20,21,22,23,24,25,26,27,28,29,30,31,32,33,34,35]. The types of catalysts depend on whether the catalysts are located within the gasifier, or in a secondary bed after the gasifier exit. For the former approach, particulate catalysts such as dolomite (a calcium carbonate based mineral) have been used in fluidized bed gasifiers [3,4,5,6,7]. Issues encountered include attrition of dolomite into smaller particles (which cannot be retained in the fluidized bed) and deactivation of the dolomite via carbon deposition. More recently, olivine-based minerals (modified with nickel) have been utilized for the same purpose [8,9,10,11,12,13,14,15], with benefits being the higher attrition resistance of olivine and its relatively high catalytic activity for tar reforming. A challenge in this case is that the chemical composition (and thus catalytic performance) of olivine mineral varies widely depending on location of the mine. This issue can be addressed by modifying the olivine composition in a separate step, but this would add cost and could potentially compromise the attrition resistance property of the olivine.
Alternatively, synthetic catalysts, especially Ni, Fe and Co, have been widely investigated for tar reforming due to the higher activity than the minerals [13,16,17,19,20,23,25,26,27,28,29,30,31,32,33,34,35,36,37]. It is known that Ni-based catalysts have been commercialized for steam methane reforming to produce CO and H2. These catalysts were also found to be very active for the tar reforming. For instance, Caballero et al. investigated several commercial Ni catalysts from ICI, UCI, BASF and Haldor-Topsoe for tar reforming and found that nearly 100% tar conversion could be achieved at 840 °C and 0.2–0.3 s residence time [27,28]. Other commercial Ni-based catalysts were also tested for biomass tar reforming . For Ni-based catalysts, it is likely that the use of support plays an important role in tar conversion. In many cases, Al2O3 is used as the main support. Addition of MgO to Al2O3 is found to enhance catalyst activity and stability. On a series of supported Ni catalysts, such as Ni/MgO, Ni/γ-Al2O3, Ni/α-Al2O3, Ni/SiO2 and Ni/ZrO2, the activity of CO2 reforming of toluene (a model tar compound) was found to depend on Ni particle size, which is related to the interaction between Ni and the support . The best catalytic performance was obtained on the Ni/MgO due to the strong interaction between NiO and MgO within the NiO-MgO solid solution. Precious metals are also active for the tar reforming reaction. On a series of precious metal supported CeO2-SiO2 catalysts, Tomishige et al. reported that the activity decreased in a sequence of Rh > Pt > Pd (≈Ni) > Ru . However, precious metal catalysts are expensive, making them less practical for tar reforming applications.
Although transition metal and precious metal based catalysts are active in converting tar to syngas, most of the testing data in the literature were reported in the absence of sulfur [2,33]. It is known that sulfur exists in biomass gasification gases. Tolerance to H2S is critical for tar reforming catalysts because sulfur is difficult to be removed at gasification temperatures. In this work, we have developed a magnesium nickel silicate (MNS) catalyst for reforming of biomass gasification products at NexTech Materials. This MNS catalyst is found to be tolerant to H2S and immune to NH3. This MNS catalyst can convert tars and light hydrocarbons to syngas by steam reforming and CO2 reforming at high temperatures in the presence of sulfur, enabling efficient use of biomass to produce power, liquid fuels and valuable chemicals.
2. Results and Discussion
2.1. Properties of MNS Catalyst
The XRD profile of MNS catalyst is shown in Figure 1. Only orthorhombic magnesium silicate phase was detected in the catalyst. NiO was not observed as a separate phase, suggesting NiO was dissolved in the magnesium silicate phase and/or dispersed well on the magnesium silicate surface.
The catalyst reducibility was determined by H2-TPR. As shown in Figure 2, The MNS sample exhibited a low temperature reduction peak near 460 °C and a high temperature reduction peak near 740 °C. Since MgO and SiO2 are difficult to be reduced below 800 °C, the two peaks can be attributed to the reduction of nickel oxides at two different sites. It is reported that, when NiO is deeply dissolved in MgO to form a solid solution  or reacts with SiO2 to generate nickel silicate compound , its reduction temperature is generally above 700–900 °C. Hence, the higher temperature peak is probably related to the NiO deeply dissolved in the magnesium silicate phase, while the lower temperature peak is due to the NiO on the magnesium silicate surface with a weaker interaction.
2.2. Methane Reforming on Granulated Catalyst
The MNS catalyst was tested for methane reforming with a simulated straw gasification stream of 3.7% H2, 8.4% CO, 13.8% CO2, 7.8% CH4, 43.3% N2 and 23.0% H2O (mole percent basis) . As shown in Figure 3, the MNS exhibited nearly 100% initial CH4 conversion at 800 °C and a GHSV of 24,000 mL/g/h, indicating this catalyst is highly active in steam reforming and dry reforming of methane to syngas under the testing conditions. CO selectivity was approximately 38% and H2/CO ratio was 5.2. H2 concentration in the product was 65%. At 340 h, the reaction temperature was increased to 900 °C. CO selectivity was increased slightly to 42%, while CH4 conversion remained at 100%. H2/CO ratio was decreased to 4.4 correspondingly. The increase in CO selectivity with temperature is because reverse water gas shift reaction is more favorable at higher temperature. No change in methane reforming activity was observed during the initial 400 h testing.
At 400 h, 10 ppm H2S was added to the feed at 900 °C. The catalytic performance was unchanged for another approximately 200 h on stream (Figure 4). At 600 h, the H2S concentration was increased to 20 ppm while keeping the other conditions unchanged. A slight initial decrease in CH4 conversion and CO selectivity was observed, but no further change was seen in additional 200 h testing (Figure 4). CH4 conversion remained at 98%, while CO selectivity remained at 40%. The above data indicated that the MNS catalyst was stable for 800 h during the testing under the conditions with H2S and without H2S. It is noted that there are some data gaps during the activity testing for baking out GC columns.
2.3. Catalytic Performance of MNS Extruded Monolith
Monolith catalysts, located at the tail end of gasifier, have been suggested for tar removal via steam reforming at elevated temperatures. Identified advantages of this include: (1) reduction of pressure drops associated with fixed/fluidized bed reactors; (2) reduction of carbon deposition (and clogging) of reactors that often occurs in fixed bed reactors; (3) potential for additional functionality (i.e., reforming of residual hydrocarbons into H2 and CO); (4) the ability to use high activity catalysts that are not cost effective when used in fixed beds. The MNS catalyst was extruded to form a monolith with 400 CPSI, followed by calcination 1300 °C for one hour. Figure 5a shows a fresh MNS-extruded monolith with dark green color. Under the conditions of 850 °C and a space velocity of 10,000 h−1, less than 25% CH4 conversion was obtained on the extruded monolith in flowing 3.7% H2, 7.6% CH4, 8.5% CO, 13.9% CO2, 23.4% H2O, and 42.9% N2. A BET surface area analysis confirmed that the cause for the low performance was the low surface area of the monolith material. After calcination at 1300 °C during monolith manufacturing, the surface area of the MNS was decreased to only 0.13 m2/g from the previous 4.0 m2/g.
To increase the monolith activity, fine-scale MNS powder were washcoated onto the extruded monolith. It was observed that, under the same reaction conditions, approximately 90–100% CH4 conversion was achieved at 900 °C, while CO selectivity was 60–65% (Figure 6). H2 concentration in the product was 55% and H2/CO ratio was approximately 1.8. As compared to the granule catalyst (Figure 4), the higher CO selectivity on the monolith catalyst might be due to more CO2 reforming at the lower space velocity. At 70 h, the reaction temperature was decreased to 850 °C. An initial decrease in CH4 conversion was observed, but it recovered to nearly 100% slowly. This observation suggests an activation process for the catalyst during the testing. When more active sites are available on the surface with time, the catalyst exhibits higher reforming activity. CO selectivity also decreased to approximately 58%. The monolith catalyst achieved 90–100% methane conversion in 600-h testing. This result demonstrated that washcoating of MNS catalyst powders on the extruded monolith increased its reforming activity significantly.
2.4. Catalytic Performance of MNS Washcoated Cordierite Monolith
The MNS catalyst was also washcoated on a cordierite monolith (400 CPSI). The color of the MNS-washcoated monolith is light green (Figure 5b), similar to the catalyst color. The monolith was tested for reforming of oak wood gasification products  under the conditions of 900 °C, 14.4% H2, 10.4% CO, 9.8% CO2, 5.8% CH4, 13.2% N2, 44.6% H2O, 1.6% C2H6 and C2H4, 0.2% C3H8 and C3H6, 30 ppm naphthalene (when used), 22 ppm H2S and GHSV = 10,000 h−1. H2S, naphthalene, C2 and C3 hydrocarbons were added to the feed for this testing.
As shown in Figure 7, C2+ hydrocarbon conversion reached 87% on the MNS-washcoated cordierite monolith in the presence of H2S, while CH4 conversion was approximately 20%. CO selectivity was 55%. H2 concentration in the product was 35% and H2/CO ratio was approximately 1.8. For the C2+ hydrocarbons, propane and propylene were not detected in the product, indicating complete conversions. Approximately 85% of ethane and ethylene conversion was obtained. The above data indicate that, for reforming of the light hydrocarbons, the activity decreased in a sequence of C3 hydrocarbons (100%) > C2 hydrocarbons (85%) > methane (20%) on the MNS-washcoated monolith in the presence of sulfur. This is likely due to the difference in C-H bond dissociation energy in these hydrocarbons. For example, the C-H bond energy in the hydrocarbons decreases in a sequence of CH4 (103 kcal/mol) > C2H6 (98 kcal/mol) > C3H8 (95 kcal/mol), which is in reverse order of their reforming activity. In a separate test under the same conditions but without H2S, almost complete CH4 and C2+ hydrocarbon conversions were achieved (not shown), suggesting the presence of H2S decreased monolith catalyst reforming activity.
At 165 h, 30 ppm naphthalene (a model tar compound) was added to the feed with sulfur, the catalytic performance did not change. Naphthalene was not detected in the exhaust by a mass spectrometer, suggesting that the catalyst was effective in breaking down the double ringed structure and converting it into syngas. The MNS catalyst was tested for 500 h in the presence of H2S and no deactivation was seen (Figure 7). This indicates that the catalyst was stable in the presence of H2S.
Beyond the initial 500 h testing, additional conditions were investigated to determine the monolith’s performance at different temperatures. The feed flow rate was adjusted to obtain complete C2+ hydrocarbon conversion at 900 °C, 875 °C, and 850 °C in the presence of H2S. A summary of this testing is provided in Table 1. At 900 °C, complete C2+ hydrocarbon conversion could be obtained at a gas space velocity of 5000 h−1. A decrease in reaction temperature decreased catalyst activity and required progressively lower gas flow rate to achieve near complete C2+ hydrocarbon conversion. At 875 °C, complete C2+ hydrocarbon conversion was obtained at a gas space velocity of 3000 h−1. When the temperature was decreased to 850 °C, nearly complete C2+ hydrocarbon conversion could be obtained at 1800 h−1. CH4 conversion also changed with the reaction temperature and gas flow rate (Table 1).
|Monolith Temperature (°C)||Space Velocity (h−1)||C2+ Conversion (%)||Methane Conversion (%)|
Feed gas composition: 14.4% H2, 10.4% CO, 9.8% CO2, 5.8% CH4, 13.2% N2, 44.6% H2O, 1.6% C2H6 and C2H4, 0.2% C3H8 and C3H6, and 22 ppm H2S.
After concluding the study summarized by Table 1, the reaction conditions were returned to the initial conditions: 900 °C and GHSV = 10,000 h−1. As shown in Figure 8, C2+ hydrocarbon conversion was maintained at approximately 87%, while CH4 conversion decreased slightly to 18%. After the MNS-washcoated monolith was tested for 1000 h, 1000 ppm NH3 was added to the feed while the other conditions were kept the same. It can be seen that the addition of NH3 did not impact the performance of the catalyst. All major exhaust compositions were shown to be consistent before and after the NH3 addition. This suggests that the catalyst was stable in the presence of both H2S and NH3, two major impurities in biomass gasification products.
At 1145 h, H2S was removed from the feed stream while maintaining NH3 concentration at 1000 ppm. C2+ hydrocarbon and CH4 conversions were increased to about 100% and above 95%, respectively (Figure 9). CO selectivity did not change significantly. H2 concentration in the product was increased to 53% and H2/CO ratio was approximately 2.7. The catalyst activity was almost identical to that in the absence of sulfur and ammonia. This further supports the conclusion that NH3 did not impact the reforming activity of this catalyst. Additionally, the quick increase in C2+ hydrocarbon and methane conversions also suggests that H2S has a reversible degradation effect on the catalyst. Upon H2S removal, the catalytic performance was recovered quickly.
After the ammonia tolerance testing, the feed gas was changed back to the original conditions with 22 ppm H2S at 1200 h. 87% C2+ hydrocarbon conversion and 18% CH4 conversion were still obtained. The testing data have proven that the MNS catalyst is robust for reforming of biomass gasification products. It is stable in the presence of H2S and NH3, which are impurities in biomass gasification gases.
The above testing data have indicated that the magnesium nickel silicate is highly active in reforming of tar and light hydrocarbons to syngas for biomass gasification process in the presence of sulfur and ammonia. In the catalyst, NiO phase was not detected by XRD, indicating it is highly dispersed on the magnesium silicate surface and/or dissolved in the phase, which is considered to be beneficial to the reforming activity in the literature [27,28,29,30,31,32,33,34,35]. Consequently, the MNS catalyst granules achieved complete methane conversion at 900 °C and a space velocity of 24,000 mL/g/h. The addition of 10–20 ppm H2S to the feed had no apparent impact on the performance (both methane conversion and CO selectivity) (Figure 4). In comparison, CH4 and C2+ hydrocarbon conversions were decreased by H2S on the MNS washcoated monoliths. It is likely that the total amount of active sites on the granules is more than enough for complete hydrocarbon reforming under the testing conditions. When the catalyst is partially poisoned by H2S, the amount of the active sites is still enough to convert all of the hydrocarbons. Hence the addition of H2S did not have “apparent” impact on methane conversion on the granule catalyst. This might not be the case for the MNS washcoated catalyst, resulting in a decrease in activity. Moreover, this MNS catalyst has shown excellent stability over hundreds of hours of testing. Deactivation was not observed in 800 h of testing of the granulated catalyst (Figure 3 and Figure 4) and not seen in 1200 h of testing of the monolithic catalyst (Figure 7–Figure 9) in the absence/presence of H2S and NH3. Complete light hydrocarbon conversion was achieved on the MNS-washcoated monolith in the presence of H2S at 900 °C and GHSV = 5000 h−1 (Table 1). In the literature, some Ni-based catalysts are reported to deactivate in steam reforming of tar due to coking and sulfur poisoning. On Ni/Al2O3  and Ni/CeO2-ZrO2 , carbon deposition is reported to result in loss of tar reforming activity. Typical characteristics of deactivation by coking are that the catalyst activity drops and pressure drop increases continuously with time until the catalyst surface is fully covered by carbon deposition or the reactor channel is blocked by the coke. In this work, our MNS catalyst was continuously tested without deactivation and without discernible increases in pressure drop for 800–1200 h, suggesting that the catalyst was not coked during the testing. In fact, coke was not detected on the used catalyst by SEM analysis. It is reported that NiO can dissolve in MgO and form solid NiXMg1-XO solution, resulting in excellent anti-coking property in reforming methane and other hydrocarbons . It is likely that the NiO in the MNS catalyst is also dissolved in the magnesium silicate phase to form solid solution for the anti-coking purpose, as evidenced by no NiO phase detected in the XRD analysis (Figure 1).
For sulfur poisoning, it is known that H2S in the reaction gas tends to react with Ni in the catalysts to form non-active surface Ni-S . Consequently most of the Ni-based reforming catalysts are poisoned by sulfur, resulting in activity loss irreversibly. It is reported that doping a sulfur-resistant promoter WO3 onto Ni/MgO-CaO catalyst has enhanced the tolerance to sulfur because tungsten promotes sulfur dissociation via the reactions NiSX + W = WSX + Ni and WSX + xH2 = W + xH2S . On a nickel calcium aluminum catalyst (Ni/Ca12Al14O33), Li et al. also reports an initial sulfur resistance compared to the commercial Ni/Al2O3 and Ni/CaO-MgO catalysts . The catalyst can sustain sulfur poisoning without loss of tar reforming activity for approximately one hour under the testing conditions due to the presence of O2− and O22− adsorbed species on the surface. The “free oxygen” in the catalyst structure can be substituted preferably by sulfur and thus prolongs Ni lifetime. However, the adsorbed S atom is hardly re-substituted by O2, resulting in a permanent deactivation late. In this work, the MNS catalyst lost some activity in the presence of sulfur, suggesting the catalyst is partially poisoned by the sulfur. However, no further deactivation was observed over 1200 h of testing (Figure 7–Figure 9), indicating the catalyst is stable in the presence of sulfur. Further, the sulfur poisoning effect is reversible. After sulfur was removed from the feed gas, the catalyst activity was fully recovered quickly (Figure 9). This indicates that the sulfur adsorption on the MNS catalyst is relatively weak. It can be removed by steam and H2 under the testing conditions. Consequently, after the H2S is removed from the feed, the reforming activity is restored. For the MNS catalyst, the reason for the tolerance to sulfur poisoning is not clear at present time. It might be related to the solid solution formation and interaction between the NiO and magnesium silicate, resulting in a weaker adsorption of sulfur on the Ni surface.
The addition of 1000 ppm NH3 did not impact the catalytic performance at 900 °C in the presence and absence of H2S (Figure 8), indicating the MNS catalyst is immune to NH3. The resistance to NH3 poisoning is possibly due to the weak adsorption of ammonia and nitrogen atom on the MNS catalyst surface. In fact, Ni-supported materials have been investigated as catalysts for NH3 decomposition for biomass gasification process. Ni-based catalysts are reported to be active in decomposing NH3 to N2 and H2 at high temperatures (>800 °C) and the ammonia conversion increases with Ni content in the catalysts . As a result, the addition of NH3 to the feed does not impact the activity of the MNS catalyst. Overall, the present testing data suggests that this MNS material is a promising catalyst for reforming of tar and light hydrocarbons to CO and H2 for biomass gasification process in the presence of H2S and NH3, enabling efficient use of biomass to produce power, liquid fuels and valuable chemicals.
3. Experimental Section
3.1. Catalyst Preparation and Characterization
Magnesium nickel silicate (MNS) catalyst was prepared by solid-state reaction. The as-prepared material had a BET surface area of 4 m2/g. For catalyst activity testing, the powders were pressed, crushed and sieved to 35–60 mesh.
In addition, the MNS catalyst was extruded to form a 0.75 in (O.D.) × 1.5 in (length) monolith with 400 cells per square inch (CPSI), followed by calcination 1300 °C for 1 h. The formed monolith had strength of 82.5 MPa/cm. The MNS powders were washcoated on the MNS-extruded monolith and a cordierite monolith (400 CPSI, 0.75 in (O.D.) × 1.5 in (length), obtained from Applied Ceramics) by dip coating. The washcoated monoliths were calcined at 1000 °C for 4 h. The catalyst loading in the monolith was 180 g per liter.
BET surface area was measured with a Micromeritics TriStar system. X-ray diffraction (XRD) analysis was performed with a Scintag XDS2000 instrument. Catalyst reducibility was analyzed by H2-TPR (temperature programmed reduction), using a Micromeritics AutoChem 2910 system. 50 mg sample was heated to 850 °C at 10 °C/min in 5% H2/Ar at a flow rate of 50 SCCM. A thermal conductivity detector (TCD) was used to measure H2 consumption amount during heating.
3.2. Catalyst Performance Testing
Catalyst granules (35–60 mesh) were evaluated for reforming of methane to CO + H2 in a simulated biomass gasification product stream. The feed gas had a composition of 3.7% H2, 8.4% CO, 13.8% CO2, 7.8% CH4, 43.3% N2, 23.0% H2O and 10–20 ppm H2S (when used). 0.5 g catalyst was loaded in a 0.25 inch stainless steel reactor. The total gas flow rate was 200 mL/min and the gas hourly space velocity was 24,000 mL/g/h.
The MNS extruded monolith and washcoated monoliths were tested for reforming of methane, light hydrocarbons and tar (using naphthalene as a model compound) to syngas in a simulated biomass gasification product stream. The monoliths were loaded in one inch (OD) stainless steel reactors for the testing. A vaporizer produced steam from a liquid feed supplied by an Eldex 2HM pump. The vaporizer consisted of an initial section operated at 150 °C and second section held at 300 °C. After exit of the second section, the steam was mixed with CO, CO2, CH4, H2 and N2. The mixed feed was then introduced into a pre-heater that operated at 900 °C. A 0.25 inch stainless steel Tee between the pre-heater and the reactor furnace allowed for various hydrocarbons, ammonia, and H2S to be added into the synthetic biomass composition. All of these components were controlled by Sierra MFCs. The complete feed then entered the monolith reactor. The exit of the reactor fed into a condenser to knock out the water from the gaseous stream. The condenser was operated at 6 °C and the condensate accumulation was released by a level controlled solenoid valve. Removing the water from the stream enabled more accurate and consistent data to be taken using a gas chromatograph (GC). A scheme of the catalyst performance testing system is shown in Figure 10.
The GC for analyzing the gas compositions was an SRI 8610C Multiple Gas Analyzer No. 1. This instrument contained a 6-foot silica gel column and a 6-foot 13× molecular sieve column to separate a wide range of molecules. The GC had a thermal conductivity detector and a flame ionization detector with a methanation system. The standard setup was modified by adding copper before the methanation system to prevent H2S from poisoning the methanation catalyst. The carrier gas was Argon at a pressure of 28 PSIG. For each injection, the column temperature was held at 30 °C for 6 min and then increased to 300 °C at 10 °C/min heating rate. Finally the temperature was held at 300 °C for 20 min to bake out all gases. The GC was calibrated prior to each testing using standard mixing gases. CH4 and C2+ hydrocarbon conversions were calculated by the difference in their flow rates before the reaction and after the reaction. CO selectivity was determined as [CO]/([CO] + [CO2]) in the product. The carbon balance in this work was 100 ± 5%.
Based on the above testing data, it can be concluded that:
Granulated MNS catalysts achieved complete methane conversion at 900 °C and a space velocity of 24,000 mL/g/h in a simulated biomass gasification stream. Addition of 10–20 ppm H2S to the stream did not significantly change the catalyst performance.
The MNS-extruded monolith exhibited poor activity in biomass reforming, which was attributed to a significant decrease in surface area during the monolith manufacturing process.
The MNS catalyst washcoated on MNS-extruded monolith achieved 90–100% CH4 conversion at 850–900 °C and a space velocity of 10,000 h−1 in a simulated biomass gasification stream without H2S.
On a MNS-washcoated cordierite monolith, the addition of 22 ppm H2S to a simulated biomass gasification stream decreased the initial activity at 900 °C, but the activity was constant for 1200 h in the presence of H2S.
On the MNS washcoated monolith, the reforming activity decreased in a sequence of C3 hydrocarbons > C2 hydrocarbons > methane.
On the MNS-washcoated monolith, complete C2+ hydrocarbon conversion could be achieved at 900 °C and a GHSV of 5000 h−1 in the presence of H2S.
The addition of 1000 ppm NH3 did not impact the catalytic performance at 900 °C in the presence and absence of H2S, indicating the MNS catalyst was immune to NH3.
This work was supported by the U.S. Department of Energy (Contract No. DE-FG36-04GO14314) and by the National Science (Contract Numbers 0740809 and IIP-0848877).
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