Guest Editor: S. Walia
Beilstein J. Nanotechnol. 2019, 10, 848–855. https://doi.org/10.3762/bjnano.10.85
Received 10 Jan 2019, Accepted 29 Mar 2019, Published 11 Apr 2019
MnO2–CuO–Fe2O3/CNTs catalysts, as a low-dimensional material, were fabricated by a mild redox strategy and used in denitration reactions. A formation mechanism of the catalysts was proposed. NO conversions of 4% MnO2–CuO–Fe2O3/CNTs catalyst of 43.1–87.9% at 80–180 °C were achieved, which was ascribed to the generation of amorphous MnO2, CuO and Fe2O3, and a high surface-oxygen (Os) content.
Keywords: amorphous materials; carbon nanotubes; low-dimensional materials; low-temperature catalysis; SCR activity
Nitrogen oxides, NOx (x = 1, 2), contribute to acid rain, photochemical smog, greenhouse effect and ozone depletion [1-3]. The selective catalytic reduction of NO with NH3 (SCR), as a commercialized NOx abatement technology, has received a great deal of attention [4,5]. However, the catalyst of the SCR reaction, V2O5+WO3(MoO3)/TiO2, has some drawbacks, such as the toxic V-based material and the high operating temperature window (300–400 °C) [6-8]. Additionally, this kind of catalyst is easily influenced by ash and SO2, which makes it necessary to be installed downstream of electrostatic precipitator and desulfurizer, where the flue gas temperature is normally below 200 °C . Therefore, it is of importance to develop a SCR catalyst with high catalytic activity below 200 °C.
Carbon nanotubes (CNTs), a low-dimensional material, exhibit a one-dimensional tubular structure and outstanding chemical and physical properties. Hence, they are extensively studied for the application in SCR, e.g., in MnOx/CNTs , Mn–CeOx/CNTs  and CuOx/carbonaceous-materials catalysts . However, the working temperature window of these SCR catalysts is still between 200 and 300 °C.
A series of Cu-based [12,13] and (Mn + Fe)-based [14,15] catalysts have been applied in the SCR reaction and presented good catalytic activity. Nevertheless, the preparation procedures of the catalysts always need high-temperature calcination or high-pressure hydrothermal reactions, which are uneconomic and unsafe. Our previous studies, including MnO2–Fe2O3–CeO2–Ce2O3/CNTs  and Ce2O3–CeO2–CuO–MnO2/CNTs  catalysts, have reported a simple and mild redox method for the preparation of ternary and quaternary catalysts, and the resultant catalysts show outstanding denitration activity at 80–180 °C. The mechanisms of above preparation method are redox reactions between MnO4− (from KMnO4) and Cl− (from FeCl3 and CeCl3), or Mn7+ and O2− (from KMnO4) as well as MnO4− (from the KMnO4) and Cl− (from CeCl3). The generation of Cl− anions in the preparation process can result in corrosion of the equipment. On the basis of the above issues, a redox method with the formation of HNO3 between Mn7+ and O2− (only from KMnO4) was developed, and the passivation through HNO3 can protect the metal equipment. This redox method yielded MnO2–CuO–Fe2O3/CNTs catalysts, and the as-synthesized catalysts were applied in the SCR reaction at 80–180 °C.
Figure 1 shows the NO conversion as a function of temperature for the CNT-based catalysts. As shown in Figure 1, the NO conversion of MnO2–CuO–Fe2O3/CNTs prepared by the mild method was better than that of Mn–Cu–FeOx/CNTs-IWIM fabricated through incipient wetness impregnation, except for the 1% MnO2–CuO–Fe2O3/CNTs, and reached 69.9–87.9% between 140 to 180 °C. The SCR activity over 4% MnO2–CuO–Fe2O3/CNTs reached maximum values of 43.1–87.9% at 80–180 °C at a weight hourly space velocity of 280 L·gcat−1·h−1.
Figure 2 shows the XRD patterns of the acid-treated CNTs and the as-synthesized catalysts. All samples present the characteristic diffraction peaks at 26.3°, 42.6° and 53.7°, corresponding to the (002), (100), and (004) planes of graphite, respectively . For MnO2–CuO–Fe2O3/CNTs, only a weak peak of MnO2 (PDF#53-0633) can be observed when the loading was greater than or equal to 4%, whereas no diffraction peaks of metal oxides could be found, suggesting the formation of amorphous metal oxide phases. Amorphous catalytic materials are conducive to SCR activity , which is also shown in the results of NO conversion (Figure 1) and our previous studies [6,16,17]. In the case of Mn–Cu–FeOx/CNTs-IWIM, a series of peaks corresponding to Mn3O4 (PDF#18-0803) can be seen. Metal oxide catalysts with higher crystallinity show a smaller catalytic activity . This is corroborated by the results of NO conversion. Besides, the intensities of the graphite peaks declines with increased loading, which is due to the interaction between the metal oxide catalysts and CNTs [21-25].
The morphologies of the acid-treated CNTs and the catalysts were investigated by TEM and HRTEM (Figure 3). The acid-treated CNTs have a smooth external surface (Figure 3a) that becomes coarse after being loaded with active metal oxide (Figure 3b). Additionally, the HRTEM images show the presence of catalysts nanoflakes, also verifying the generation of metal oxide catalysts on the CNT surface. The EDX spectrum (Figure 3d) shows signals of Mn, Cu, Fe, O and C. Clear lattice fringes of the metal oxides cannot be observed in the HRTEM images, indicating the generation of amorphous materials, which is consistent with the results of XRD (Figure 2).
The XPS spectra of the as-prepared catalysts are given in Figure 4. The elements Mn, Cu, Fe, C, and O were detected in the XPS full-scan spectrum of Figure 4A. For the Mn 2p spectrum of 4% MnO2–CuO–Fe2O3/CNTs (Figure 4B), the binding energies at 654.2 and 642.4 eV, attributed to Mn 2p1/2 and Mn 2p3/2, respectively, can be observed. These values together with the energy separation of 11.8 eV demonstrate the formation of MnO2 . The high oxidation state of MnO2 is advantageous to the SCR reaction , which is in accordance with the results of XRD and NO conversion measurements. The binding energies of Cu 2p1/2 and Cu 2p3/2 of the 4% MnO2–CuO–Fe2O3/CNTs catalyst (Figure 4C) are located at 954.3 and 934.4 eV, respectively, along with satellites at higher energies, indicating the formation of CuO . The energy separation between Cu 2p1/2 and Cu 2p3/2 is 19.9 eV, also demonstrating the generation of CuO . The Auger spectrum of Cu (Figure 4D) presents a peak at 917.2 eV, typical for CuO [30,31].
In the Fe 2p spectra of 4% MnO2–CuO–Fe2O3/CNTs and Mn–Cu–FeOx/CNTs-IWIM (Figure 4E, spectrum a), the Fe 2p1/2 and Fe 2p3/2 peaks at 724.7 and 711.2 eV, respectively, can be attributed to Fe2O3 . The energy separation of 13.5 eV is typical for Fe2O3 . The two satellites at 732.7 and 718.4 eV also verify the formation of Fe2O3 . In spectrum b of Figure 4E, the binding energies of Fe 2p1/2 and Fe 2p3/2 (724.4 and 711.0 eV) of the Mn–Cu–FeOx/CNTs-IWIM catalyst appear at lower energies than those of 4% MnO2–CuO–Fe2O3/CNTs catalyst, revealing the formation of Fe3O4 . Moreover, the absence of any satellites further proved the presence of Fe3O4. It is noteworthy that Fe2O3 exhibits a better low-temperature SCR activity than Fe3O4 , which is corroborated by the NO conversion measurements.
The O 1s peak can be divided into three peaks (Figure 4F). The peak at 529.9 eV is attributed to lattice oxygen (designated as OL), while the binding energies at 530.5–534.0 eV are ascribed to surface oxygen (labeled as OS). The OS content (Table S2, Supporting Information File 1) of the 4% MnO2–CuO–Fe2O3/CNTs catalyst is 66.7%, whereas it is 36.8% in Mn–Cu–FeOx/CNTs-IWIM catalyst. OS has a higher mobility than OL, which is in favor of the oxidation of NO to NO2, accelerating the SCR reaction . This was also confirmed by the results of NO conversion and of previous studies [6,16,17].
STEM and element mapping were adopted to further investigate the morphology of the catalyst. As shown in Figure 5a, bright dots associated to the metal elements can be found, indicating the formation of metal oxide catalysts on CNTs. The STEM-EDX mappings (Figure 5b–g) exhibit a series of columnar element-distribution images, further proving that the metal oxide catalysts have been successfully loaded on the CNTs.
In SCR reaction, the redox performance of the catalyst plays a significant role in the catalytic cycle. Therefore, the reducibility of the as-obtained catalysts was evaluated by using hydrogen temperature-programmed reduction (H2-TPR). The results are listed in Figure 6. The catalysts exhibits three reduction peaks. For 4% MnO2–CuO–Fe2O3/CNTs catalyst (Figure 6a), the peaks at 150–300 °C (centered at 249 °C) are overlapping reduction peaks of MnO → Mn2O3  and CuO → Cu2O [12,38,39]. The reduction peaks between 300–380 °C are overlapping peaks of Mn2O3 → Mn3O4 → MnO  and Cu2O → Cu . Moreover, a reduction peak could be found at 580 °C, which is attributed to the oxygen groups on the CNT surface. For the Mn–Cu–FeOx/CNTs-IWIM catalyst (Figure 6b), the centers of the first and second reduction peaks (257 and 454 °C) were all at higher temperatures than those of 4% MnO2–CuO–Fe2O3/CNTs catalyst. This means that the reducibility is lower compared with that of 4% MnO2–CuO–Fe2O3/CNTs.
The chemisorption and activation of NH3 on the surface acid sites of a catalyst are generally viewed as the primary processes in the SCR of NO. Therefore, ammonia temperature-programmed desorption (NH3-TPD) measurements were carried out and the results are shown in Figure 7. The two catalysts presents three desorption peaks of NH3 corresponding to weak, intermediate and strong acid sites. For 4% MnO2–CuO–Fe2O3/CNTs catalyst, the centers of the three desorption peaks of NH3 are located at 165, 267 and 391 °C. These values are higher than those of Mn–Cu–FeOx/CNTs-IWIM catalyst (158, 259 and 387 °C), which means that the acid sites are stronger in 4% MnO2–CuO–Fe2O3/CNTs catalyst . In addition, the number of Brønsted acid sites and Lewis acid sites at low and high temperature of the 4% MnO2–CuO–Fe2O3/CNTs catalyst is higher than that of the MnO2–CuO–Fe2O3/CNTs catalyst . In general, stronger acid sites and a higher number of acid sites are advantageous to the SCR reaction , which is corroborated by the results of the NO conversion.
In practical applications, the cyclic and long-term stability of a catalyst are crucial factors. The cyclic and long-term stability of the optimal 4% MnO2–CuO–Fe2O3/CNTs catalyst are listed in Figure 8. Figure 8A shows that the catalytic activity of 4% MnO2–CuO–Fe2O3/CNTs in run 2 and run 3 reaches 44.5–88.4% at 80–180 °C, which is similar with to the catalytic activity of 4% MnO2–CuO–Fe2O3/CNTs in run 1 (43.1–87.9%), suggesting an excellent cyclic stability of the catalyst. Figure 8B shows that the catalytic activity of 4% MnO2–CuO–Fe2O3/CNTs exhibits no obvious changes and reaches up to 87.9% at 180 °C during a test of 6 h, revealing the outstanding long-term stability. In view of the above favorable properties, the 4% MnO2–CuO–Fe2O3/CNTs catalyst will be potentially applicable in the low-temperature NO reduction with NH3.
Table 1 shows three catalysts with excellent performance in the low-temperature NO reduction with NH3, but the chemical reactions during preparation are different. The 6% Ce2O3–CeO2–CuO–MnO2/CNTs and 4% MnO2–Fe2O3–CeO2–Ce2O3/CNT catalysts present outstanding denitration efficiency values over the test temperature range, but Cl− anions are formed in the preparation process, which might lead to a corrosion of metal equipment. The 4% MnO2–CuO–Fe2O3/CNTs catalyst reaches NO conversions of 43.1–87.9% at 80–180 °C, which is similar to two catalysts in our previous papers. Moreover, HNO3 is formed in the preparation process, which leads to an inactivation of the metal equipment.
Table 1: Catalytic performance of three catalysts.
A reaction mechanism of the synthesis of the MnO2–CuO–Fe2O3/CNTs catalystis proposed. Based on the results of XRD and XPS, active components of MnO2, CuO, and Fe2O3 are formed. The following formation mechanism was inferred: Cu2+ and Fe3+ ions are first adsorbed on the surface of acid-treated CNTs via electrostatic interaction. Then the Cu(NO3)2 and Fe(NO3)3 are partly hydrolyzed in situ into Cu(OH)2, Fe(OH)3, and HNO3 on the CNTs. Afterwards, MnO2 is formed through the reaction between KMnO4 and HNO3, and the hydrolysis process is accelerated. MnO2–Cu(OH)2–Fe(OH)3/CNTs samples are obtained, and the MnO2–CuO2–Fe2O3/CNTs catalysts are prepared through thermal dehydration of the MnO2–Cu(OH)2–Fe(OH)3/CNTs samples [42,43]. The detailed reaction equations are:
MnO2–CuO–Fe2O3/CNTs catalysts were synthesized via a mild preparation method. The 4% MnO2–CuO–Fe2O3/CNTs catalyst showed the optimum low-temperature catalytic activity at 80–180 °C with a weight hourly space velocity of 280 L·gcat−1·h−1, benefitting from its amorphous metal oxide catalysts as well as high surface-oxygen content. The mild preparation conditions of the MnO2–CuO–Fe2O3/CNTs catalyst, can also provide a promising application in other catalytic fields.
The raw CNTs (multi-wall) of 60–100 nm in diameter were purchased from Shenzhen Nanoport Company (China). KMnO4 (AR), Cu(NO3)2·3H2O (AR), Fe(NO3)·9H2O (AR) and ethanol (AR) were purchased from Shanghai Chemical Reagent Ltd. All chemical were used without further purification. Deionized water with a resistivity above 18.0 MΩ·cm was obtained from a JL-RO100 Millipore-Q Plus.
The raw CNTs were first treated with HNO3 (65–68%) for 4 h at 140 °C, and then washed with deionized water and ethanol until pH 7. Finally, the solid product was dried at 70 °C for 12 h and grinded in an agate mortar.
First, acid-treated CNTs, Cu(NO3)2·3H2O, and Fe(NO3)·9H2O were dispersed in 40 mL deionized water under stirring for 12 h. Afterward, 40 mL of KMnO4 solution was added under continuous stirring at room temperature for another 12 h. Subsequently, the solid product was obtained by filtration, and washed with deionized water and ethanol until pH 7. Finally, the product was dried at 105 °C in air for 10 h. The as-prepared catalyst is denoted as y MnO2–CuO–Fe2O3/CNTs, where y represents the molar ratio of [KMnO4 + Cu(NO3)2 + Fe(NO3)3]/CNTs. For further details see . The detailed molar ratios of precursors of 4% MnO2–CuO–Fe2O3/CNTs catalyst were obtained as follows: A molar ratio of 16 KMnO4:4Fe(NO3)3:2Cu(NO3)2 is obtained from Equations 1–3, and the molar ratio of [KMnO4 + Cu(NO3)2 + Fe(NO3)3]/CNTs = 4%. The mass of CNTs is 0.3 g (0.025 mol). The total amount of substance is then [KMnO4 + Cu(NO3)2 + Fe(NO3)3] = 4% × 0.025 mol = 0.001 mol. The amount of substance of KMnO4, Cu(NO3)2, and Fe(NO3)3 is 0.0007273 mol KMnO4, 0.0000909 mol Cu(NO3)2, and 0.0001818 mol Fe(NO3)3. For a comparative experiment, incipient wetness impregnation [44,45], as a common preparation method of catalysts, was applied to fabricate the Mn–Cu–FeOx/CNTs-IWIM catalyst with an optimal load of 4%.
X-ray diffraction (XRD) was measured with an X'Pert Pro MPD X-ray diffractometer using Cu Kα radiation (λ = 0.15406 nm) with a 2θ range from 5° to 80°. Transmission electron microscopy (TEM) was performed on a JEOL model JEM 2010 EX instrument. Temperature-programmed reduction by H2 (H2-TPR) was assessed by using a custom-built TCD apparatus. Before the H2-TPR test, 50 mg catalyst was firstly purged in N2 at 200 °C for 1.5 h. The test was carried out in N2 (containing 6% H2) with a heating rate of 10 °C/min. X-ray photoelectron spectroscopy (XPS) was carried on a Thermo Scientific ESCALAB 250 spectrometer equipped with a dual Al/Mg anode (0.6 eV resolution).
The SCR activity tests were carried out in a fixed-bed quartz reactor using 0.15 g catalyst in each test. The reaction gas consisted of [O2] = 5%, [NO] = [NH3] = 400 ppm, balanced by N2 gas. The total flow rate was 700 mL/min equivalent to a weight hourly space velocity (WHSV) of 280 L·gcat−1·h–1. A flue-gas analyzer (Kane International Limited, KM950) equipped with the NO, NO2, SO2, and O2 sensors was used to monitor the gas concentration. All data were recorded after 30 min till the catalytic reaction reached a steady state.
|Supporting Information File 1: Additional experimental data.|
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