Xin Gaoab,
Ling Lib,
Lihong Songab,
Ting Lub,
Jiaxin Zhaob and
Zhi Liu*ab
aInstitute of Chemistry for Functionalized Materials, Faculty of Chemistry and Chemical Engineering, Liaoning Normal University, Dalian 116029, China. E-mail: zhiliu@lnnu.edu.cn; Fax: +86 411 82156858; Tel: +86 411 82156989
bFaculty of Chemistry and Chemical Engineering, Liaoning Normal University, Dalian, Liaoning 116029, China
First published on 18th March 2015
In this paper, we report a novel nanocomposite of MnOx nanoparticles supported by three-dimensionally ordered macroporous carbon (MnOx/3DOMC) fabricated by means of a simple multi-component infiltration of three-dimensional templates and its use as a catalyst for low-temperature selective catalytic reduction (SCR) of NOx with NH3. Several techniques, including scanning electron microscopy, X-ray diffraction, N2-sorption, transmission electron microscopy, X-ray photoelectron spectroscopy, NH3 temperature-programmed desorption, and H2 temperature-programmed reduction, are employed to characterize the MnOx/3DOMC nanocomposite. The results demonstrate that MnOx/3DOMC possesses a highly ordered macroporous structure with hierarchical mesopores in the walls of the macroporous skeleton. MnOx nanoparticles of 2–4 nm are observed to be highly dispersed on the 3DOM carbon scaffold. Compared with the MnOx/NAC and MnOx/TiO2 catalysts prepared by a conventional impregnation method, the MnOx/3DOMC catalyst exhibits better low-temperature NH3-SCR activity, stability, and water vapor and/or SO2 resistance ability. Such material represents a promising exploratory direction for enhancing the catalytic performance of metal oxide-based NH3-SCR catalysts.
Three-dimensionally ordered macroporous (3DOM) materials, with uniform pore size and well-defined periodic structure, have triggered increasing interests due to their widespread applications in separation, catalysis, energy storage/conversion systems, and solar cells, etc.19–25 Conventionally, the colloidal crystal templating strategy (CCTS) is employed to prepare 3DOM materials.26 Briefly, uniform monodispersed microspheres, such as polymethyl methacrylate (PMMA), polystyrene (PS) or silica spheres, can assemble into ordered three-dimensional array in densified packing. These ordered arrays offer a 3D scaffold in which a variety of precursors can be infiltrated. After subsequent solidification of the precursors and removal of the colloidal microspheres, periodic 3D framework structures can be obtained successfully. However, the single macroporous size distributions and relatively low surface areas are greatly disadvantageous to the efficient application of the 3DOM materials especially when they are used as supports in catalysis field. In order to address the problems, a upgraded dual ‘hard-soft’ colloidal crystal templating strategy (dual-CCTS) has been recently proposed to prepare hierarchically porous structure 3DOM materials, in which PMMA or PS microspheres were used as the hard template to create macropores and some surfactants or organics were introduced into the precursors as the soft template to form mesopores.27–33 It is widely accepted that the metal-support interaction and active species dispersion are important factors in the determination of catalytic performances for metal-loaded catalysts. And a larger specific surface area of the support permits higher dispersion of the active phase, which consequently leads to promotional catalytic performance.34–36 Obviously supports such as hierarchical 3DOM materials not only possess high surface area for good active species dispersion, but it can also reduce the diffusion resistance and permit facile transport, thus allowing for the efficient mass transport of the reactant and the product molecules. Moreover, desired active species can be directly introduced into the 3DOM solid-state architecture through using the corresponding metal salt solution(s) as precursor(s) to infiltrate the template. Different from the traditional impregnation, deposit or (co-)precipitation, such a 3DOM catalyst would not only yield intimate contact and strong interaction between the active species and the 3DOM support matrix, but it also make the active species highly dispersed in the 3DOM support matrix, which will potentially give rise to superior catalytic performance.
In the present work, we have successfully prepared a MnOx/3DOM carbon nanocomposite (MnOx/3DOMC) by means of a simple multi-component (manganous nitrate, phenol-formaldehyde resol, and triblock copolymer F127) infiltration of 3D PMMA templates followed by a direct pyrolysis process. The NH3-SCR of NOx was used as a probe reaction to evaluate the catalytic performance of the MnOx/3DOMC. The results showed that the MnOx nanoparticles prepared with the dual-CCTS were highly dispersed in the 3DOM carbon scaffold, and the new nanocomposite presented a higher catalytic activity than those of the others MnOx-based catalysts prepared by the conventional impregnation method in the NH3-SCR of NOx.
For comparison, commercial Norit activated carbon (NAC) and TiO2 were used as supports for preparing the MnOx/NAC and MnOx/TiO2 catalysts by a conventional impregnation method. Briefly, 0.2 g of NAC or TiO2 was dispersed in a certain amount of Mn(NO3)2 solution (50 wt%). The mixture was ultrasonicated for 1 h and then dried overnight at 80 °C. Then, the catalysts were calcined under flowing N2 at 500 °C for 3 h. The total loading amounts of manganese on MnOx/NAC and MnOx/TiO2 were 7.3 wt% and 7.4 wt% (ICP analysis), respectively.
XRD results of the MnOx/3DOMC, MnOx/NAC, and MnOx/TiO2 catalysts are compared in Fig. 2. For the MnOx/3DOMC, only two broad diffraction peaks at 22.5° and 43.5° characteristic of amorphous carbon appeared,40,41 and no any crystalline phases of MnOx were observed, suggesting their possible high dispersion in the 3DOM carbon matrices. For the MnOx/NAC, in addition to the diffraction peaks of amorphous carbon, two diffraction peaks at 43.2° and 50.5°, ascribed to the characteristics diffraction peaks of tetragonal symmetry of α-MnO2 (JCPDS 44-0141), were observed clearly, indicating the presence of MnOx with larger particle sizes in this catalyst than in the MnOx/3DOMC. In addition, no diffraction peaks for other manganese oxides were detected. For the MnOx/TiO2, the different diffraction peaks, assignable to the anatase TiO2 (JCPDS 21-1272), MnO2 (JCPDS 44-0141) and Mn2O3 (JCPDS 41-1442), respectively, could be found easily.
Fig. 3 presents the N2 adsorption–desorption isotherms and pore size distributions (PSDs) of the MnOx/3DOMC, MnOx/NAC, and MnOx/TiO2 catalysts. For the MnOx/3DOMC, the isotherm belonged to a mixed type combining macropores with certain meso- and micropores, which exhibited a type II isotherm with an H3-type hysteresis loop and three N2 uptake phases. Below the very low relative pressure of P/P0 = 0.1, there was a significant quick rise of adsorption branch, indicating the presence of some micropores generated possibly from the carbonization of P-F resol. With the increase of the relative pressure from P/P0 = 0.1 to P/P0 = 0.8, the N2 adsorption amounts increased gradually accompanying with a slight H2-type hysteresis loop related to the capillary condensation taking place, implying the existence of some mesopores of a variety of sizes. At high relative pressures of P/P0 = 0.8–1.0, an obvious H3-type hysteresis loop, which had no clear adsorption plateau at P/P0 ≈ 1.0, indicative of a macroporous size distribution, was observed. Such a phenomenon was also observed in the others surfactants-assisted preparation of 3DOM materials,42–49 feature of combination of macro-mesopore structure. The PSD of the MnOx/3DOMC, which centered at ∼5 nm and ∼60 nm, respectively, also confirmed this point. In comparison with the MnOx/3DOMC, the hysteresis loops of the MnOx/NAC and MnOx/TiO2 at the low and high relative pressure ranges varied from sample to sample, reflecting their discrepancy in PSD with the MnOx/3DOMC. For the MnOx/NAC, three peaks centering at ∼3.0, 4.1, and 6.5 nm were observed in the PSD curve. Moreover, broad peaks between 20–60 nm were also observed, implying the inhomogeneity of its PSD. For the MnOx/TiO2, a wide PSD from 20 to 300 nm with two small bimodal distributions centering at ∼30 and ∼110 nm was observed, which possibly originated from the interstitial spaces between agglomerated particles. Table 1 lists the corresponding textural properties of the three catalysts. The MnOx/NAC possessed a BET surface area of 659 m2 g−1 and a Vp of 0.38 cm3 g−1. Its Vmeso and Vmic were 0.10 and 0.26 cm3 g−1, respectively, indicating that substantial micropores were present and contributed to the major surface area of the catalyst. On the contrary, despite the fact that the MnOx/3DOMC had a similar BET surface area of 656 m2 g−1 to the MnOx/NAC, the Vmeso strikingly increased to 0.36 cm3 g−1 accompanying with a distinct decrease of corresponding Vmic to 0.04 cm3 g−1, suggesting that the introduction of F127 during the preparation process could substantially increase the mesoporosity, which favored the significant enhancement in surface area of the obtained MnOx/3DOMC catalyst. In addition, the MnOx/TiO2 had the smallest the BET surface area of 68 m2 g−1 and the pore volume of 0.11 cm3 g−1 among the catalysts.
![]() | ||
Fig. 3 Nitrogen adsorption–desorption isotherms and corresponding pore size distributions of the MnOx/3DOMC, MnOx/NAC, and MnOx/TiO2 catalysts. |
Catalyst | SBET (m2 g−1) | Vmeso (cm3 g−1) | Vmicro (cm3 g−1) | Vp (cm3 g−1) | Mn content (wt%) |
---|---|---|---|---|---|
MnOx/3DOMC | 656 | 0.36 | 0.04 | 0.43 | 7.1 |
MnOx/NAC | 659 | 0.10 | 0.26 | 0.38 | 7.3 |
MnOx/TiO2 | 68 | 0.05 | 0.01 | 0.11 | 7.4 |
Since the incomplete certain of manganese valence, XPS was adopted to further identify the components, oxidation states of manganese, and corresponding surface atomic concentration information of the MnOx/3DOMC, MnOx/NAC, and MnOx/TiO2 catalysts, as shown in Fig. 4. For the MnOx/3DOMC, the binding energies (BEs) of Mn 2p3/2 and 2p1/2 located at 642.1 and 653.8 eV, respectively, with a spin-energy separation of 11.7 eV, suggesting that the predominant oxidation state of manganese is +4.50 For the MnOx/NAC, the BEs of Mn 2p3/2 and 2p1/2 located at about 642.0 and 653.9 eV, respectively, which can be considered to be identical to those of the MnOx/3DOMC with a Mn4+ oxide phase. Unlike the MnOx/3DOMC and MnOx/NAC, the distinctive Mn 2p3/2 shoulder-peak of the MnOx/TiO2 could be deconvoluted into three characteristic peaks at BEs of 643.4 eV, 642.0 eV, and 640.3 eV, which were attributed to Mn4+, Mn3+, and Mn2+ oxide phases, respectively.51 Table 2 summarizes the surface atomic concentrations of manganese and the relative concentration ratios of Mn4+, calculated from the XPS spectra. The concentration ratio of Mn4+ over the MnOx/3DOMC, MnOx/NAC and MnOx/TiO2 catalysts were presented as 96%, 76%, and 49%. According to the total surface manganese concentrations over the catalysts, 1.65 at.% for the MnOx/3DOMC, 1.00 at.% for the MnOx/NAC, and 1.60 at.% for the MnOx/TiO2, the concentrations of Mn4+ over the catalysts were calculated to be 1.50 at.%, 0.76 at.% and 0.78 at.%, respectively. Evidently, the molar concentration of Mn4+ on the MnOx/3DOMC was much higher than that on the other two catalysts. Such discrepancy was presumably associated with the difference in catalyst preparation. In our case, the MnOx/3DOMC catalyst prepared by the dual-CCTS possessed higher manganese precursor (Mn(NO3)2) dispersion and exposed more manganese atoms on the surface than the other two catalysts prepared by the impregnation method. During the pyrolysis process, these exposed active atoms were thus easier to decompose directly into the high valence. Furthermore, the well developed interconnected networks of the ordered macro-mesopore structures of the 3DOM carbon would potentially afford much more internal surface to expose the active atoms. It was much reported that Mn4+ species and their redox processes were responsible for the high activity over the manganese-based catalysts in the low temperature NH3-SCR reaction. And a high Mn4+ ratio would enhance the oxidation of NO to NO2, which was beneficial to promote the low-temperature SCR activity.17,52–55 Therefore, the higher atomic concentration of Mn4+ would play an important role in obtaining better low-temperature NOx removal ability for the MnOx/3DOMC catalyst than for the other two catalysts. On the other hand, the O 1s spectrum is frequently used to identify the types of surface oxygen species in a particular oxide. The chemical environment of oxygen in metal oxide catalysts often has an important effect on their catalytic properties. Fig. 4 also shows the O 1s spectra of the three catalysts. For all the catalysts, three deconvoluted peaks were observed, which were attributed to three types of oxygen species: the peak at BE of 529–530 eV was assigned to the lattice oxygen O2− in Mn–O–Mn (denoted as Oβ), the peak at BE of 531–532 eV was ascribed to the surface oxygen ions with low coordination (denoted as Oα), such as O− or O22− belonging to the hydroxide (Mn–OH) or defective oxides, and the peak at a higher BE of above 533 eV corresponded to adsorbed water.53,56–59 It was established that the Oα were more active than the Oβ due to its higher mobility than the Oβ.60 As a result, the higher Oα/(Oα + Oβ) ratio was favorable to the NH3-SCR reaction owing to the enhanced oxidation of NO to NO2. Based on the XPS, the concentrations of Oα/(Oα + Oβ) over the MnO2/3DOMC, MnOx/NAC, and MnOx/TiO2 catalysts were calculated to be 14.1%, 3.8% and 10.1%, respectively (Table 2). Considering these results, as well as the manganese valence analysis, it was therefore reasonable to expect that the MnOx/3DOMC catalyst would potentially achieve better activity than the other two catalysts in the NH3-SCR reaction at low temperature.
Catalyst | Mn4+/(Mn2+ + Mn3+ + Mn4+) (%) | Mn (at.%) | Mn4+ (at.%) | Mn (wt%) | Oα/(Oα + Oβ) (%) | O (at.%) | Oα (at.%) |
---|---|---|---|---|---|---|---|
MnOx/3DOMC | 91 | 1.65 | 1.50 | 6.8 | 80.4 | 17.55 | 14.1 |
MnOx/NAC | 76 | 1.00 | 0.76 | 4.2 | 29.3 | 13.10 | 3.8 |
MnOx/TiO2 | 49 | 1.60 | 0.78 | 2.5 | 26.1 | 38.6 | 10.1 |
Fig. 5 illustrates typical TEM images of the MnOx/3DOMC, MnOx/NAC, and MnOx/TiO2 catalysts. It was clearly seen in Fig. 5a that the MnOx/3DOMC possessed a high-quality 3DOM structure containing interconnected networks with overlapped pores. The macroporous diameter of the MnOx/3DOMC was ∼200 nm, in good agreement with its SEM observation. A clearer observation in the partial magnified image in Fig. 5b revealed that MnOx nanoparticles were highly distributed on the macropore walls of the 3DOM carbon scaffold. The sizes of MnOx nanoparticles fell in the range of 2–4 nm, as seen by the tiny black spots. From the high-resolution TEM image in Fig. 5c, the high dispersion MnOx on 3DOM carbon was much easier to be observed. Two crystal lattice fringes with a d-spacing of 0.239 and 0.418 nm corresponding to the (110) and (211) planes of MnO2 respectively can be clearly observed as well, whereas no significant crystalline plane of carbon was found, substantiating its amorphous nature. In addition, there were numerous mesopores with an average size of 5 nm randomly distributed in the macropore walls of the 3DOM carbon scaffold. The emergence of the mesopores could potentially enhance the capability of absorption and activation for gas reactant. Similar formation pathways have been discussed by other groups.42,61 Differing greatly from the MnOx/3DOMC, the TEM image in Fig. 5d displayed a relatively low dispersion of the MnOx particles with sizes of 20–100 nm in the MnOx/NAC. Similarly for the MnOx/TiO2, as shown in Fig. 5e, a large number of aggregates were formed.
![]() | ||
Fig. 5 TEM images of: (a) (b) the MnOx/3DOMC catalyst at low and high magnification; (c) the MnOx/NAC catalyst; (d) the MnOx/TiO2 catalyst. |
The NH3-TPD technique is often employed to determine the surface acid amount and strength of catalysts. The area of desorption peak is directly proportional to the acid amount and the peak position is correlated with the acid strength. Fig. 6 shows the NH3-TPD profiles of the MnOx/3DOMC, MnOx/NAC, and MnOx/TiO2 catalysts. For the MnOx/3DOMC, the NH3 desorption profile exhibited three distinct desorption peaks centered at 247 °C, 365 °C, and 562 °C, assignable to the NH3 desorbed by weak, medium and strong acid sites, respectively.62,63 It was well accepted that the coordinated NH3 molecular bound to the Lewis (L) acid sites was more thermally stable than the NH4+ ions fixed on the Brønsted (B) acid sites.64 It was therefore conjectured that the desorption peak at low temperature was assigned to physisorbed NH4+ ions bound to the B acid sites, while the desorption peak at high temperature was associated with NH3 molecular originating from the L acid sites.65 On the other hand, pyridine is commonly used as a basic probe molecule for characterization of both B and L acidic sites by FTIR spectroscopy. In order to ascertain the type of B or L acid, we further characterized the MnOx/3DOMC by pyridine-DRIFTS. As shown in Fig. S3,† the band at 1446 cm−1 was typically attributed to pyridine bound to L acid sites, the band at 1487 cm−1 was assigned to the L or B acid sites, and the band at 1540 cm−1 was generally assigned to pyridine bound to B acid sites.66,67 Evidently, the strong and medium L acid sites were the main acid sites in the MnOx/3DOMC, whereas the peak belonging to B acid sites was relatively weak, indicating that only a small number of B acid sites were formed. For the MnOx/NAC, there were two major NH3 desorption peaks centered at 354 °C and 546 °C. Moreover, the overall curve shifted towards the low temperature region, indicating that the strength of acid sites on MnOx/NAC became weaker than that on MnOx/3DOMC. Meanwhile, the smaller area of desorption peaks of MnOx/NAC also implied a lower number of acid sites on this catalyst. For the MnOx/TiO2, the NH3 desorption peaks were relatively weak as compared with the other two samples, suggesting its shortage of acid sites. Such results indicated that the preparation method has a significant effect on the amount and the strength of the acidic sites on the catalysts. In our case, the MnOx/3DOMC was derived from P-F phenolic resin, which contained various aromatic structures supplying enough strong acid sites.68 On the other hand, it was reported that some oxides could increase the acidity of support remarkably.69 The largest area of the desorption peaks of the MnOx/3DOMC implied the most Brønsted and Lewis acid sites it possessed, which could be attributed to 3DOM carbon itself and the MnOx nanoparticles on 3DOM carbon.
H2-TPR is an ideal tool for investigating the reducibility of the MnOx over the different supports. Fig. 7 records the H2-TPR profiles of the MnOx/3DOMC, MnOx/NAC, and MnOx/TiO2 catalysts. It was reported that the reduction process of MnOx took place in the following stepwise order: MnO2 → Mn2O3 → Mn3O4 → MnO.57,70 For the MnOx/3DOMC, there was one strong reduction peak centered at 233 °C, assigned to the reduction of major MnO2. For the MnOx/NAC, the reduction peak of MnO2 shifted to a higher temperature of 270 °C accompanying with the emergence of another obvious broad peak at 341 °C, which was correlated to the reduction of Mn2O3 phase. For the MnOx/TiO2, in addition to the peaks of the reduction of MnO2 to Mn2O3 (281 °C) and Mn2O3 to Mn3O4 (376 °C), the third peak at 464 °C, indicative of the reduction Mn3O4 to MnO, was observed. Apparently, the reduction temperature of MnO2 in the MnOx/3DOMC catalyst was found to be lower than those in the MnOx/NAC and MnOx/TiO2 catalysts, indicating the strongest reducibility of MnO2 in the MnOx/3DOMC catalyst. Furthermore, the larger area of the reduction peak of the MnOx/3DOMC catalyst meant the higher consumption of H2, suggesting that more active species were exposed in the MnOx/3DOMC catalyst than in the other two catalysts. This was in very good agreement with the TEM observation and XPS analysis.
![]() | ||
Fig. 8 NO conversions over the MnOx/3DOMC, MnOx/NAC, and MnOx/TiO2 catalysts. Reaction conditions: 1000 ppm of NO, 1000 ppm of NH3, 5% of O2, He balance. |
Catalyst | Mn content (wt%) by XPS | Composition of feed gas | GHSV (h−1) | Calculation temperature (°C) | TOF (s−1) | References | |
---|---|---|---|---|---|---|---|
NO + NH3 (ppm) | O2 (vol%) | ||||||
MnOx/3DOMC | 6.8 | 1000 + 1000 | 5 | 36![]() |
100 | 3.81 × 10−4 | This work |
MnOx/NAC | 4.2 | 1000 + 1000 | 5 | 36![]() |
100 | 1.79 × 10−4 | This work |
MnOx/TiO2 | 2.5 | 1000 + 1000 | 5 | 40![]() |
100 | 1.31 × 10−4 | This work |
MnZ-3 | 16.76 | 600 + 600 | 4.5 | 36![]() |
100 | 7.98 × 10−5 | 11 |
MnOx/TiO2 | 5 | 500 + 500 | 2 | 75![]() |
100 | 4.08 × 10−5 | 14 |
MnOx/MWCNTs | 10 | 1000 + 1000 | 5 | 40![]() |
100 | 2.57 × 10−4 | 17 |
Mn-MA/Ti-CVC | 23.4 | 500 + 500 | 5 | 30![]() |
100 | 4.89 × 10−6 | 71 |
MnCBV | 3.5 | 500 + 500 | 5 | 80![]() |
150 | 9.34 × 10−5 | 72 |
MnOx/Al2O3–TiO2 | 8.2 | 500 + 500 | 5 | 80![]() |
100 | 2.49 × 10−5 | 72 |
MnOx/CZO | 25.74 | 1000 + 1000 | <5 | 6000 | 100 | 2.29 × 10−5 | 73 |
MnOx/CeO2 | 7.22 | 600 + 660 | 6 | 45![]() |
100 | 1.65 × 10−4 | 74 |
MnOx/CeO2–ZrO2 | 9.4 | 600 + 600 | 3 | 30![]() |
100 | 1.39 × 10−4 | 75 |
MnOx/MWCNTs | 10 | 1000 + 1000 | 5 | 40![]() |
100 | 5.90 × 10−5 | 76 |
MnOx/CeO2 | 20 | 1000 + 1000 | 3 | 50![]() |
100 | 2.04 × 10−4 | 77 |
MnOx/CeO2–TiO2 | 20 | 200 + 200 | 8 | 60![]() |
120 | 2.63 × 10−5 | 78 |
(Ca)MnOx/TiO2 | 23.58 | 650 + 650 | 3 | 75![]() |
100 | 7.39 × 10−5 | 79 |
Long-term stability is an important merit for catalysts. Meanwhile, since water vapor and/or SO2 are inevitable components of exhaust gas and may cause severe deactivation of catalysts for the NH3-SCR reaction, it is also necessary to study the water vapor resistance and/or SO2 tolerance of catalysts. Fig. 9 indicates the stability and the effects of water vapor and/or SO2 on NO conversion over the MnOx/3DOMC, MnOx/NAC, and MnOx/TiO2 catalysts. During a 48 h period at 190 °C (Fig. 9a), the MnOx/3DOMC preserved a high NO conversion at ∼98% with almost negligible activity decay. Unfortunately, the NO conversions over the MnOx/NAC and MnOx/TiO2 gradually faded with reaction time. After the continuous 48 h reaction, the 3DOM structure of the MnOx/3DOMC catalyst was still well-maintained with partial pore collapse to some extent, and the whole structural integrity remained considerably (Fig. 9e), implying that the long-term reaction did not spoil the structure of the catalyst and the high NO conversion could be further well preserved. The NH3-TPD profile after the long-term test shown in Fig. S4† also verified that there were indiscernible changes of the amount of acid sites and acid strength in the MnOx/3DOMC catalyst. When 5 v% water vapor was introduced into the feed gases (Fig. 9b), all the NO conversions over the three catalysts decreased during the test period. The fall range was ∼3.4% for MnOx/3DOMC, ∼5.0% for MnOx/NAC, and ∼9.3% for MnOx/TiO2, respectively, suggesting that the MnOx/3DOMC had a higher capacity for water vapor-resistance. After the water vapor was discontinued from the feed gases, all the NO conversions were almost restored to their originals, indicating that the inhibition effect of water vapor over the three catalysts was reversible. This was in good line with the reported results that the inhibition of water vapor resulted from the competitive adsorption between water and ammonia on the active sites of the catalyst's surface, which was reversible.80,81 When 200 ppm of SO2 was added to the feed gases (Fig. 9c), the NO conversion over the MnOx/3DOMC decreased slightly from initial 99% to 94%, then presented a gradually recovery trend during the test period. By contrast, the presence of SO2 caused a significant decrease of NO conversion over the MnOx/NAC and MnOx/TiO2 by 9 and 15%, respectively. After excluding SO2 in the feed gases, the conversions of NO over the MnOx/NAC and MnOx/TiO2 gradually restored to a certain extent, but still were less than their initial values, and finally returned to 81 and 58%, respectively. This substantiated that the MnOx/3DOMC had a stronger resistance to SO2. The NH3-TPD profile after the SO2-resistance test shown in Fig. S4† confirmed the remarkable increases in the amount of acid sites and acid strength in the MnOx/3DOMC catalyst. This was likely due to the increasing acidity of the catalyst by potential SO2 sulfuration, and implied that the acidity was not the only factor for the MnOx/3DOMC catalyst to determine the SCR performance. It was reported that the SO2 poisoning and deactivation to catalyst was usually related to the generation of ammonium sulfate species and deposition on the catalyst surface, blocking the active sites of the catalyst surface. And some MnOx-based catalysts resistance to SO2 could be enhanced due to the strong interaction between MnOx and the support with the inhibition of manganese sulfate formation on catalyst surface.82,83 In our case, the present MnOx nanoparticles formed with the dual-CCTS were mainly imbedded in or anchored on the carbon walls, which would not only produce highly dispersed MnOx nanoparticles in the 3DOMC matrix, but it could also create intimate contacts and strong interactions between the MnOx nanoparticles and the carbon support. Based on this point, such unique feature of the MnOx/3DOMC obviously helped to improve its SO2 resistance ability. In addition, the effect of coexistence of water vapor and SO2 was investigated. When 5 v% water vapor and 200 ppm SO2 were together introduced into the feed gases (Fig. 9d), the variation of NO conversion of the three catalysts were similar as those in the SO2-existence model. All the NO conversions exhibited a trend of first decease, then gradual recovery to a certain extent but less than their initial values, and finally returned to some stable values during the test period. This was likely stemmed from the synergistic inhibition effect of water vapor and SO2.
The excellent catalytic performance of the MnOx/3DOMC catalyst was approximately described as the Fig. 10 demonstrating. In the macro aspect, the MnOx/3DOMC was hierarchically porous structure. There were numerous additional mesopores in the macropore walls of the well-developed interconnected monolithic MnOx/3DOMC framework. Moreover, the MnOx nanoparticles were highly dispersed in the macropore walls where intimate contacts and strong interactions between the MnOx nanoparticles and the carbon support could be well yielded. These features were favorable to provide easier mass transport and more accessible internal surface area for the reaction, increase the number of active sites, and prevent the MnOx nanoparticles aggregation and growth during reaction. Meanwhile in the microcosmic aspect, the NH3-SCR of NOx over the MnOx/3DOMC catalyst was possibly described as the following five underlying reactions (Fig. 10). Reaction (1) was the adsorption of gaseous ammonia on the acid sites (i.e. B acid sites and L acid sites) to form adsorbed ammonia species including ionic NH4+ and coordinated NH3. Reaction (2) was the activation of adsorbed ammonia species by Mn4+ to form amide species (–NH2). Reaction (3) was the oxidation of NO to NO2. Then, gaseous NO and NO2 were reduced by –NH2 on the surface to form N2 and H2O via reaction (4). Reaction (5) was the re-oxidization of formed Mn3+.
Footnote |
† Electronic supplementary information (ESI) available. See DOI: 10.1039/c4ra16141f |
This journal is © The Royal Society of Chemistry 2015 |