Yongbiao Zhaiab,
Yingying Xueab,
Zheng Chenab,
Min Chenac,
Buhuan Wangab and
Jiangang Chen*a
aState Key Laboratory of Coal Conversion, Institute of Coal Chemistry, Chinese Academy of Sciences, Taiyuan, 030001, P. R. China. E-mail: Chenjg@sxicc.ac.cn
bUniversity of Chinese Academy of Sciences, Beijing, 100049, P. R. China
cCollege of Environmental Engineering, Shanghai University, Shanghai, 200444, P. R. China
First published on 10th October 2016
To further understand the role of Fe–Co alloys in Fischer–Tropsch synthesis, a series of RANEY® Fe–Co mono/bimetallic catalysts were prepared through alkali leaching solidified Fe–Co–Al alloy. There are three advantages about these catalysts: (i) RANEY® structure can provide certain surface area for catalytic reaction; (ii) these catalysts avoid the influence of the metal–support interaction due to the absence of support; (iii) the composition of active phase can be determined easily. The FT results showed that not all the Fe–Co alloy could enhance the C5+ selectivity, only when the ratio of Fe/Co is 3:
7 can C5+ selectivity be promoted effectively. Besides, we also found that Fe–Co alloy did not show intended synergy effects on the FT activity, instead, Co-dominant catalysts exhibited a higher CO conversion.
Iron and cobalt are the typical active metals used in FT synthesis. Co-Based catalysts show high catalytic activity and are suitable for the production of long-chain paraffins.11 The comparatively less expensive Fe-based catalysts exhibit high selectivity toward lower olefins and catalyze the water gas shift (WGS) reaction, which can be used to adjust H2/CO ratio in syngas and make the FT synthesis more flexible to different types of feedstocks.12 We therefore focus on bimetallic Fe–Co catalysts in this work. In most studies on bimetallic systems, Fe–Co active phase was dispersed on the surface of supports through a variety of methods.13–16 Supported catalysts displayed high specific surface area and enhanced dispersion of active phase. However, numerous researches on supported catalysts met limited success because of the presence of strong metal–support interaction that prevented the reduction of oxide precursor.17,18 Ma et al. had observed that the performance of Fe–Co catalysts depended on the type of support materials used.7 Support materials such as SiO2, TiO2 and MgO have been shown to react with Fe or Co to give Co2SiO4, Co2TiO4 and FeO–MgO during catalysts preparation, thermal treatment or catalytic reaction. Unfortunately, these mixed compounds are not active in FT synthesis.19 In this case, carbonaceous materials are widely used as a promising support, but there are still some uncertainties. It is difficult to determine the active phase because Fe, Co or Fe–Co alloy may be coexistent in the catalysts.20–22
To avoid these shortcomings, RANEY® Fe–Co catalysts were prepared in this work through alkali leaching of a rapid quenched (Fe1−xCox)50Al50 alloy. Firstly, RANEY® structure can provide a large surface area for catalytic reaction;23,24 secondly, these catalysts effectively prevent the effect of metal–support interaction due to the absence of support; thirdly, the Fe–Co alloy can be formed easily during the high-temperature melting stage. Besides, the rapid quenching could produce refined and uniform microstructures, which lead to improvements in catalytic performance. Fan et al. had shown that Fe–Mn catalysts leached from rapid quenched Fe–Mn–Al alloy displayed superior activity, selectivity to alkenes and longer hydrocarbons.25
The bimetallic Fe–Co catalysts were prepared by adding Fe–Co–Al alloy into the NaOH solution (6.0 mol L−1) at 70 °C for alkali leaching. The black powders were washed thoroughly with distilled water and absolute ethanol. The as-prepared catalysts were stored in ethanol before characterization and catalytic testing.
The reaction products passed through a 130 °C hot trap and a 5 °C cold trap at working pressure, and then the gaseous products were analyzed on-line by gas chromatography (GC 920). A carbon molecular sieve column connected with a thermal conductivity detector was used to separate and quantify H2, N2, CH4, CO and CO2, whereas C1–C8 hydrocarbons were separated in a capillary Porapack-Q column and detected in a flame ionization detector.
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Fig. 1 (a and b) XRD patterns of the mono/bimetallic RANEY® Fe1−xCox catalysts. (c) Amplified XRD patterns of the RANEY® Fe1−xCox catalysts near 2θ = 45°. |
Fig. 1c shows amplified XRD patterns of the R-Fe1−xCox catalysts (x range from 0.1 to 0.07) near 2θ = 45°, in which an obvious shift toward higher angle zone can be found with the increase of Co content. This can be attributed to the difference in atomic radius between Fe and Co, since the atomic radius of Co is smaller than that of Fe.
The bulk compositional and textural properties of as-prepared mono/bimetallic R-Fe1−xCox catalysts are summarized in Table 1. After alkali leaching, the Al content decreased drastically from 50% to no more than 4.5%, which agrees to the disappearance of Fe–Co–Al phase in Fig. 1. Although these catalysts were prepared by the same experimental method, the content of Co significantly influenced the surface area and crystallite size. As inferred from Table 1, the surface area rises from 29.6 m2 g−1 to 57.5 m2 g−1 when the Co content increases from 0 to 90%, while the mean crystallite size decreases from 16.9 nm to 12.6 nm. This trend has also been reported elsewhere.6 For example, the studies on FeCo catalysts reported a decrease in particle size for bimetallic catalysts compare to the monometallic catalysts, and particle size decreased with the increase of Co content.
Catalyst | Ala wt% | SBET (m2 g−1) | Vpore (cm3 g−1) | Dpore (nm) | dFe–Cob (nm) |
---|---|---|---|---|---|
a Bulk composition determined by ICP-OES analysis.b Mean crystallite size calculated from the XRD of Fe(110), Co(111) and Fe–Co(110) using the Scherrer equation. | |||||
R-Fe | 3.9 | 29.6 | 0.121 | 19.9 | 16.9 |
R-Fe0.8Co0.2 | 3.7 | 37.1 | 0.149 | 16.4 | 16.1 |
R-Fe0.5Co0.5 | 4.4 | 46.7 | 0.196 | 12.7 | 14.8 |
R-Fe0.3Co0.7 | 4.0 | 51.8 | 0.209 | 12.1 | 13.5 |
R-Fe0.2Co0.8 | 3.7 | 55.3 | 0.214 | 11.8 | 13.1 |
R-Fe0.1Co0.9 | 3.3 | 57.5 | 0.253 | 11.5 | 12.6 |
R-Co | 4.1 | 31.4 | 0.155 | 19.8 | 15.6 |
The catalysts were also characterized by SEM, and the typically SEM micrographs were presented in Fig. 2. Compared to the spongy morphology of RANEY® Fe and Co (Fig. 2a and b) characteristic, we note that the average particle size of bimetallic R-Fe0.2Co0.8 and Fe0.1Co0.9 (Fig. 2c and d) decreases obviously with the increase of Co content. This trend is consistent with the results of average crystallite size in Table 1.
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Fig. 2 Representative SEM micrographs of RANEY® Fe (a), RANEY® Co (b), RANEY® Fe0.2Co0.8 (c) and RANEY® Fe0.1Co0.9 (d). |
The catalytic performance of mono/bimetallic R-Fe1−xCox catalysts were evaluated by using a fixed-bed reactor at 240 °C and 20 bar (GHSV = 2000 h−1, H2/CO = 2). The CO conversion of the catalysts as a function of time on stream is presented in Fig. 3. It was observed that all the catalysts investigated in this study were stable within 100 h. For the monometallic catalysts, R-Co has a higher CO conversion than that of R-Fe under the same reaction conditions. This result was consistent with available literature data. For the bimetallic catalysts, the addition of Co (x ≤ 0.7) to Fe-based catalysts did not yield any drastic effect on CO conversion compared to the monometallic R-Fe catalyst. This result suggests that Fe–Co alloy does not possess any additive properties compared to the pure Fe catalysts. This observation is agreement with conclusions drawn from other literature studies.16,20 Notably, Co-rich samples (x ≥ 0.8) significantly improved the CO conversion, and the R-Fe0.1Co0.9 sample had the highest conversion (72.5%) among all the catalysts. According to the foregoing discussions, Co could be separated out from supersaturated Fe0.1Co0.9 melt (Fe0.1Co0.9 → 2/3Co + 1/3Fe0.3Co0.7), thus we can assume that the structure of supersaturated Fe0.1Co0.9 may similar to the Fe0.3Co0.7-supported Co catalyst. Besides, the average crystallite size of precipitated-Co is smaller than that of monometallic R-Co and the surface area is larger than monometallic R-Co (Table 1). These combined factors result in the highest CO conversion of R-Fe0.1Co0.9.28 The similar results has also been demonstrated elsewhere.9
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Fig. 3 CO conversion as a function of time in FT synthesis for the mono/bimetallic RANEY® Fe1−xCox catalysts (T = 240 °C, P = 20 bar, GHSV = 2000 h−1, H2/CO = 2). |
The steady-state CO conversions and product selectivity of mono/bimetallic R-Fe1−xCox catalysts are summarized in Table 2. C5+ selectivity and CO conversion are shown in Fig. 4. As expected, monometallic R-Fe exhibited comparatively lower selectivity to C5+ hydrocarbons than that of R-Co catalyst. Monometallic Co catalysts can be typically evaluated in the temperature range of 220 °C to 240 °C to achieve a high selectivity to long-chain paraffins. But the Fe catalysts need alkali metal promoters to enhance the long-chain hydrocarbons selectivity. For the bimetallic R-Fe1−xCox catalysts, the selectivity of C5+ hydrocarbons increased slightly with the increase of Co content when the value of x is smaller than 0.7. Surprisingly, the selectivity of C5+ hydrocarbons rises sharply to 62.7% from 33.3% when the value of x is 0.7, and the relatively high selectivity (55–62%) is maintained when the value of x is greater than 0.7. These results indicated that not all the Fe–Co alloy can enhance the C5+ selectivity effectively. In fact, the ratio of Fe/Co is very critical in Fe–Co alloy. On the basis of our results, Fe0.3Co0.7 is the most crucial phase to enhance the selectivity of C5+ hydrocarbons. Coville and co-worker also reported that Co2Fe alloy may be the main component to improve the selectivity of long-chain paraffins.29 Combining CO conversion and C5+ selectivity, R-Fe0.2Co0.8 and R-Fe0.1Co0.9 displayed the best catalytic performance, because their C5+ selectivity was about 60% and CO conversion remained at a high level (58.4% and 72.5%).
Catalyst | CO conversion (%) | Hydrocarbon selectivity (%) | CO2 selectivity (%) | ||
---|---|---|---|---|---|
CH4 | C2–C4 | C5+ | |||
R-Fe | 33.6 | 25.7 | 44.8 | 29.2 | 16.7 |
R-Fe0.8Co0.2 | 36.1 | 21.3 | 48.1 | 30.6 | 14.3 |
R-Fe0.5Co0.5 | 33.7 | 20.2 | 43.5 | 33.3 | 12.9 |
R-Fe0.3Co0.7 | 38.8 | 12.8 | 24.5 | 62.7 | 12.3 |
R-Fe0.2Co0.8 | 58.4 | 14.7 | 24.0 | 61.3 | 8.5 |
R-Fe0.1Co0.9 | 72.5 | 17.1 | 24.1 | 58.8 | 5.4 |
R-Co | 63.7 | 13.9 | 36.8 | 49.3 | 3.8 |
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Fig. 4 The steady-state CO conversion (line) and C5+ selectivity (column) on the mono/bimetallic RANEY® Fe1−xCox catalysts (T = 240 °C, P = 20 bar, GHSV = 2000 h−1, H2/CO = 2). |
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