Bo Penga,
Shuoyang Liangb,
Zheng Yanc,
Hao Wangad,
Zhao Mengd and
Mei Zhang*a
aState Key Laboratory of Advanced Metallurgy, School of Metallurgical and Ecological Engineering, University of Science and Technology Beijing, Beijing 100083, PR China. E-mail: zhangmei@ustb.edu.cn
bSchool of Environmental Science and Engineering, Southern University of Science and Technology, Shenzhen, 518055, PR China
cCollege of Energy & Environment, Shenyang Aerospace University, Shenyang, 110136, PR China
dSchool of Materials Science and Engineering, Peking University, Beijing 100871, PR China
First published on 7th February 2022
Multi-valence CuxO has been demonstrated to have high activity in the low-temperature selective catalytic reduction of NOx with NH3 (NH3-SCR). Here, CuxO was loaded onto activated semi-coke (ASC) for SCR, which has shown satisfactory low-temperature SCR activity. By virtue of the reduction property of carbon, the valence of Cu was regulated by simply adjusting the calcination temperature. The high concentration of Cu+ generated from the reduction of CuO by ASC during calcination can collaborate to form Cu2+/Cu+ circulation. After systematic characterization by XPS, H2-TPD, and NH3-TPR, it is revealed that abundant acidic sites and surface reactive oxygen species are formed on the surface of the catalysts. Further investigation with in situ DRIFTS confirms that the NH3-SCR over the as-prepared CuO|Cu2O-ASC catalysts simultaneously follows the Langmuir–Hinshelwood (L–H) and Eley–Rideal (E–R) pathways, attributed to the synergistic effects of Cu2+ and Cu+.
Various investigations have demonstrated that transition metal oxides are ideal candidates for low-temperature SCR, such as CuxO, MnxOy, and FexOy.5–8 Among the potential metal oxides that have been employed as active ingredients for low-temperature SCR catalysts, CuxO can offer high redox capacity and suitable acidic sites, which are significant for LT SCR performance. It was found that the valence of Cu directly affected the surface acidity and redox capacity of the catalysts, which are vital for their catalytic performance.9 Redox cycles of Cu2+/Cu+ and Cu+/Cu0 are considered to play a governing role during LT SCR.10 Although it has been well demonstrated that the appearance of a large number of Cu+ merits superior catalytic performance, pure Cu2O or CuO oxide catalysts show poor activity in a narrow temperature window.11 Hence, CuxO has usually been loaded onto a support, such as carbon,10,12–14 alumina,15 and molecular sieve.16 CuxO can be highly dispersed on the surface of the supports to expose more active sites. Meanwhile, the defects on the substrate are favorable during the creation of multi-valence CuxO. In comparison with alumina and other supports, carbonaceous materials are not only able to provide high surface area for the active sites but are also equipped with a large amount of functional groups.10,13 Close interactions have been observed during the loading of CuxO onto carbonaceous materials, which can regulate the valence distribution of copper species by virtue of their surface oxygen vacancy storage/release capacities and facilitate electron transfer among different Cu species.17–19 Li et al. prepared CuxO-carbon nanotubes (CNTs), CuxO-activated carbon (AC) and CuxO-graphite catalysts by wet impregnation methods to probe the effect of carbonaceous material supports and the nature of CuxO species. It was found that the good de-NOx of the Cu-CNTs catalyst originated from the good dispersion of CuxO, the existence of Cu+ and the strong acid sites on the catalyst surface. However, the interaction between Cu2+ and Cu+ was not discussed in detail.20 Zhu et al. loaded CuO on activated carbon and the catalysts showed high activities for NO reduction with NH3 at temperatures above 180 °C. They found that calcination temperature and Cu loading of the catalyst strongly influence the activity and structure of the catalyst. During the NO–NH3–O2 reaction, Cu2O can be easily oxidized into active CuO and results in increased activity.14 Wu et al. fabricated a series of CuAl-layered double oxide/carbon nanotubes-x (CuAl-LDO/CNTs-x) nanocatalysts with a tunable valence distribution of highly dispersed CuxO, which further demonstrated the synergistic catalytic mechanism of Cu2O and CuO.21 Herein, it is of great importance to regulate the distribution of Cu2+ and Cu+ in a convenient way. Xue et al. has reported the pretreatment of activated carbon using several methods, including air oxidation or wet oxidation in HNO3, H2O2, H2SO4 or H3PO4 aqueous solution. The de-NOx efficiencies of the as-prepared catalysts treated by HNO3 or H2O2 were greatly improved, contributed by the high concentration of acidic oxygen groups.10 This study presents the influence of the surface properties of the substrate, but the correlation between Cu2+/Cu+ and the reaction pathways is still ambiguous.
Based on previous research ideas, we employed activated semi-coke (an economical industrial carbonaceous material22), as the substrate to load CuxO, followed by regulating the calcination condition to obtain multi-valence Cu oxides. The abundant oxygen-containing groups on the surface of activated semi-coke can enhance the production of multi-valence Cu. The influence of the calcination temperature and atmosphere on the physical and chemical properties was further examined to probe the role of Cu2+/Cu+ circulation and the oxygen vacancies during LT SCR. Reaction mechanisms were further investigated with in situ diffuse reflectance infrared Fourier transform spectroscopy (in situ DRIFTS).
The calcination temperature was varied in the range of 250–450 °C, and the samples were denoted as Cu1.0-Y, in which Y stands for the calcination temperature (250, 300, 400, and 450 °C).
The calcination atmosphere was regulated as well, including pure Ar and the Ar flow containing 10% O2.
(1) |
The morphologies of CuX catalysts are shown in Fig. 2. As illustrated in Fig. 2(a), the surface of the sample ASC presents a porous structure, which can provide high surface area and is suitable for the subsequent loading of active composites. When the Cu precursor concentration is 0.3 mol L−1, large CuxO sheets with a size of ∼10 μm are observed. With the rising of Cu precursor concentration, the sheets begin to splinter into small pieces (Fig. 2(c)) and then form rod morphologies (Fig. 2(d–f)). At a concentration of 2.0 mol L−1, the rods accumulate and the surface of ASC is completely covered, which coincides with the variation of loading amount exhibited in Fig. 1(b). In addition, the EDS characterization results show that the element distribution in the catalyst surface is very uniform (Fig. S1†).
Fig. 2 Morphologies of CuX samples prepared with different precursor concentrations, (a) 0, (b) 0.3 mol L−1, (c) 0.6 mol L−1, (d) 1.0 mol L−1, (e) 1.5 mol L−1, (f) 2.0 mol L−1 Cu0.3. |
The textural properties of as-prepared catalysts are illustrated in Table 1. The pore size distributions and N2 adsorption isotherms are shown in Fig. S2.† The treatment with HNO3 greatly improved the specific surface area from 27 m2 g−1 to 357 m2 g−1, which can expose more effective surface. After loading CuxO, the surface areas of catalysts present an initial increase and then a decreasing trend in the range of 260–290 m2 g−1, among which Cu1.0 achieves the largest surface area (289.5 m2 g−1). Meanwhile, the pore diameters of all CuX samples decreases to ∼2 nm. Therefore, the formation of CuxO can influence the textural properties, which is also consistent with the morphology analyses. Nevertheless, overdose of active components usually causes obvious accumulation and block the pores. Hence, the precursor concentration has a great influence on the catalytic activity.
Samples | Specific surface area (m2 g−1) | Pore volume (cm3 g−1) | Average pore diameter (nm) |
---|---|---|---|
SC | 27 | 0.028 | 4.008 |
ASC | 357 | 0.164 | 3.787 |
Cu0.3 | 262.5 | 0.146 | 2.139 |
Cu0.6 | 269.3 | 0.152 | 2.143 |
Cu1.0 | 289.5 | 0.151 | 2.170 |
Cu1.5 | 278.1 | 0.150 | 2.168 |
Cu2.0 | 267.7 | 0.143 | 2.141 |
It can be observed from Fig. 3 that the activities of as-prepared samples increase along with the rising temperature. Taking the loading amount into account, the catalysts present an initial increase and then decreasing tendency, in which sample Cu1.0 has the highest efficiency in the whole conducted range. At 150 °C, sample Cu1.0 presents about 90% NOx removal efficiency and achieves 100% efficiency at 180–210 °C. Furthermore, at a higher temperature range (180 and 210 °C), the advantages that originated from the high loading amount are reduced. Combined with the characterization of textural properties in Table 1 and the morphologies in Fig. 2, we proposed that when the precursor concentration is lower than 1.0 mol L−1, the main limitation is the absence of abundant active sites, but a higher loading amount may result in the loss of surface area. Therefore, we choose Cu1.0 as the best load condition for the next exploration. The N2 selectivity of these catalysts can be seen in Fig. S4,† which indicates high values close to 100%.
The catalytic activities of the sample calcinated at 350 °C were compared as shown in Fig. 4(a). Activities of the sample treated in Ar atmosphere is more than the one treated with O2, particularly at a temperature lower than 150 °C. The XRD patterns were thus examined and are illustrated in Fig. 4(b). For the sample treated with protection of Ar, the main phases of CuxO are Cu2O, CuO, and even elemental Cu, resulted from the reduction by C after decomposition of Cu(NO3)2. However, when limited oxygen (10%) was introduced (Ar as the balancing gas), only CuO species can be found. Therefore, it can be deduced that the existence of O2 can effectively restrain the appearance of high content of Cu+ and Cu, which is not beneficial for the production of multi-valence Cu. From the morphologies demonstrated in Fig. 4(c), we can observe that with Ar atmosphere, the CuO grown on the surface of ASC mainly presents a sheet morphology with a size of 20–50 μm. When O2 is involved, the CuxO presents flocculent morphology, resulting from the erosion reaction by O2, indicating the transformation of Cu+ and Cu0 to high valence Cu2+. Combined with the de-NOx performance in Fig. 4(a) and the XRD patterns in Fig. 4(b), we can further draw the conclusion that the appearance of multi-valence Cu is favorable for low temperature SCR, owing to the synergistic effect of CuO/Cu2O.18
Considering that the precursors of samples with different loads are consistent, we choose the samples with better performance to study the thermal stability of precursors. Thermal analyses of sample Cu1.0 with Ar were performed to probe the production process of multi-valence Cu and the results are shown in Fig. 5. The weight loss is slow due to the inert atmosphere. The initial weight loss stage (to 2.1%) takes place at a temperature of ∼100 °C, resulting from the evaporation of water from the sample. Then, a rapid loss of weight observed below 200 °C is usually ascribed to the formation of Cu2(OH)3NO3, originating from Cu(NO3)2·3H2O. The decomposition of Cu2(OH)3NO3 over 200 °C results in the mixture of CuO and Cu2O. On further increasing the temperature, the weight loss rate becomes slow again, and the wide endothermic peak centered around 330 °C is assigned to the transformation of Cu2O to Cu.24 Herein, the decomposition reactions of Cu(NO3)2·3H2O on ASC can be described as Cu(NO3)2·5H2O → Cu2(OH)3NO3 → CuO → Cu2O → Cu.
Another important proposal that should be also noted is the properties of the carbonaceous support, which not only provides a high surface area to load the active sites, but also affects the loading process of the metal oxides since the carbon element can reduce the high valence metal ion, and oxygen functional groups usually display synergistic effect accompanied with the active sites.18,21,22,25
To further investigate the roles of CuO and Cu2O, characterizations for sample Cu1.0 before and after the NH3-SCR were carried out, and the results are shown in Fig. 6. As shown in Fig. 6(a), the XPS spectra of sample Cu1.0 before and after SCR have Cu 2p peaks. In detail, Fig. 6(b) exhibits the spectra of deconvoluted Cu 2p peaks. The peak located at 934.4 eV is assigned to the binding energy of Cu2+ and the one centered around 932.6 eV is attributed to Cu+.27 It can be seen that the intensity of Cu2+ increases after the SCR reactions, and meanwhile, the peak presenting Cu+ is weaker, indicating the transformation of Cu+ to Cu2+ during SCR reactions. In Fig. 6(c), one can observe a stronger peak of O 1s after SCR reactions, which confirms the existence of higher valence of CuxO. The XRD patterns in Fig. 6(d) furthermore evidences that the intensity of peaks ascribed to CuO increases and Cu2O decreases after SCR reactions, which agrees well with the XPS spectra.28 Hence, it is concluded that the redox cycle of Cu2+/Cu+ might play the main role during the NH3-SCR reactions, especially the existence of Cu+. Wu et al. proposed the different roles of CuO and Cu2O during SCR reactions. CuO active center can function as the dominant adsorption site of NO and NH3 to promote the formation of NO+ active species and the dehydrogenation activation of NH3. The Cu2O active center can act as the adsorption site for O, promoting the formation of active oxygen species O−.18 Herein, it is of great importance to regulate the distribution of Cu2+ and Cu+ with an easy and convenient approach.
Fig. 6 The properties of Cu1.0 before and after SCR reactions: (a) XPS spectra, (b) XPS spectra of Cu 2p, (c) XPS spectra of O 1s, (d) XRD patterns. |
The de-NOX performances of the above samples were conducted to further verify the relationships between the distribution of Cu valence and the reaction mechanisms (Fig. 8 and S6†). With the increase in calcination temperature, activities of catalysts reveal an initial increase and then a decreasing trend, and the one treated at 350 °C (Cu1.0-350) shows the best performance, which implies an optimal proportion of Cu2+ and Cu+. Hence, several different characterization methods are employed to systematically discuss the influence of Cu valence distribution.
X-ray photoelectron spectroscopy (XPS) was used to probe the surface states and atomic concentration of Cu, as illustrated in Fig. 9(a). The XPS spectrum of Cu 2p was deconvoluted into several peaks by fitting the Gaussian peaks. The peaks detected at 934.3 eV and 932.6 eV can be assigned to Cu2+ and Cu+ respectively, evidencing the co-existence of multi-valence Cu ions. The peak area ratios of Cu2+ and Cu+ are listed in Table 2. When the calcination temperature was 250 °C, the peak was totally composed of Cu2+. By increasing the calcination temperature, the value of Cu2+/Cu+ remarkably decreases from 6.9 (300 °C) to 0.8 (450 °C), further evidencing that the composition of Cu ions can be manipulated via the calcination process. Meanwhile, the collaboration of Cu2+ and Cu+ facilitates the oxidation–reduction process during NH3-SCR reactions.17 The synergistic effect of Cu2+ and Cu+ can also result in changes in the active oxygen. The O 1s peaks are displayed in Fig. 9(b). The peak around 530.37 eV corresponds to lattice oxygen (Oα), whereas the one at 531.96 eV is attributed to the surface adsorbed oxygen species O2− or O− (Oβ). The peak that originates from the hydroxyl-like groups, including chemisorbed water, is denoted as Oγ. It has been well demonstrated that Oβ species can flexibly adsorb and release oxygen and transfer the lattice oxygen atoms to the surface of the catalysts.18 Thus, a higher relative concentration of Oβ is beneficial to the formation of adsorbed NO2 and favors the fast SCR reaction. Meanwhile, with the increasing temperature, the binding energies become higher, demonstrating a better transfer capability of lattice oxygen atoms to the surface of the catalysts.21,30
Calcination temperature | Peak area ratio (Cu2+:Cu+) | Oα ratio | Oβ ratio | Oβ/(Oα + Oβ) (%) |
---|---|---|---|---|
250 °C | — | 7.9 | 60 | 88.4 |
300 °C | 6.9 | 8.3 | 67.2 | 89.0 |
350 °C | 1.7 | 7.2 | 62.1 | 89.6 |
400 °C | 1.3 | 7.5 | 66.5 | 89.9 |
450 °C | 0.8 | 6.3 | 62.5 | 90.8 |
The relative content of Oα and Oβ of each sample are compared in Table 2. It can be seen that Oβ is the dominant of the O species, and the ratio of Oβ increases along with the increased Cu+ content, consistent with the study conducted by Wu et al.21 Combined with the value of Cu2+/Cu+, it is found that a certain ratio of Cu+ is beneficial to the SCR activity, and the oxygen vacancies are closely related to the Cu2+/Cu+circulation. Consequently, surface active oxygen species with better mobility account for one of the key factors that permits a high SCR activity.31 Nevertheless, the SCR activities are not completely in conformity with the Oβ variation, which implies acidic sites that influence the adsorption of NH3 might also play a significant role during NH3-SCR.32
Another factor that triggers the SCR reactions is the adsorption of NH3 on acidic sites.34 Herein, NH3-TPD technology is used to determine the surface acidity of the catalysts. Trends of NH3-TPD patterns along with the variation of calcination temperature are shown in Fig. 10(b). Two obvious sections can be observed in the desorption temperature range for all samples. One section corresponded to the desorption of weakly bound NH3 around 100 °C, which is derived from the breakage of fairly weak hydrogen bonds between adsorbed NH3 and surface acidic groups.35 The other part in a wide range of 600–900 °C is attributed to the desorption of NH3 from the strong acid sites, specifically Lewis acid sites. One small peak around 385 °C, owing to the existence of Brønsted acid sites can be found for the sample calcinated at 250 and 350 °C. It has been demonstrated that Brønsted and Lewis acid sites on catalysts can greatly affect the adsorption states of NH3 and the reaction pathway. It can be seen that the sample treated at 350 °C has abundant acidic sites. Thus, we propose that the NH3-SCR activities of as-prepared catalysts should take the integrated effect of oxygen vacancies and acidic sites into consideration.36 Herein, it is of great importance to systematically conduct the NH3-SCR process for better understanding.
The adsorptions of NH3 were conducted with the inlet gas of 500 ppm NH3/N2, which occurred after pretreatment in an N2 atmosphere at 300 °C and background collection at 180 °C. As shown in Fig. 11(a), the NH3 adsorption on CuxO/ASC was performed. As shown in Fig. 11(a), the NH3 adsorption on the catalyst resulted in the formation of several peaks originating from the NH4+ bound to Brønsted acid sites (1681–1900 cm−1, 1452 cm−1), NH3 coordinated on Lewis acid sites (1630–1070 cm−1), and weakly adsorbed NH3 (970 and 927 cm−1).21,37 In detail, the peak at 1681 and 1452 cm−1 present symmetric and asymmetric bending vibrations of NH4+ species after reaction with Brønsted acid sites.25,38 Peaks at 1627 and 1241 reveal the existence of NH3 coordinated to the Lewis acid sites. A strong peak is centered around 1525 cm−1, which can be assigned to the amide species (–NH2) and intermediates from the partial oxidation of NH3.39 Peaks at 970 and 927 cm−1 can be assigned to either gas phase or weakly adsorbed NH3.40 It has been demonstrated from NH3-TPD that Lewis acid sites are in the majority among acid sites, which is consistent with the in situ DRIFTS analyses.
Fig. 11 In situ DRIFTS spectra of the catalyst pre-treated in different flowing gas at 180 °C for various times: (a) 500 ppm NO/N2 + 3% O2 and (b) 500 ppm NH3/N2. |
The adsorptions of NO and O2 were conducted with the inlet gas of 500 ppm NO/N2 + 3% O2, which occurred after pretreatment in an N2 atmosphere at 300 °C and background collection at 180 °C. The absorption spectrum is shown in Fig. 11(b). After NO + O2 was purged in, the peak at 973 cm−1 assigned to C–O vibration in primary C–OH appears, owing to the ASC support.25 Due to gaseous or weakly adsorbed NO, one peak at 1882 cm−1 was found. The peak surrounding 1697 cm−1 reveals the weakly adsorbed NO2 molecules.41 The peak at 1523 cm−1 reveals the appearance of bidentate nitrate, and the one at 1427 cm−1 can be attributed to monodentate nitrate. The band observed at 1168 cm−1 can be assigned to cis-N2O22−, suggesting the improved oxidation of NO to NO2.42
In situ DRIFTS transient reactions were further performed. First, NH3/N2 flow was purged for 30 min and then shut down. Afterwards, NO + O2/N2 was switched on over the NH3-adsorbed samples to further probe the reaction mechanisms. The spectra are shown in Fig. 12(a). After NH3 pre-adsorption for 30 min, one can observe several NH3 adsorption species as described above, including NH4+ bound to Brønsted acid sites (1681–1900 cm−1, 1452 cm−1), NH3 coordinated on Lewis acid sites (1630–1070 cm−1), and weakly adsorbed NH3 (970 and 927 cm−1). After the reaction with NO + O2, an obvious change can be noticed. It is found that the peaks at 970 and 927 cm−1 corresponding to weakly adsorbed NH3 gradually disappeared after the inlet of NH3, which are active for NH3-SCR.11,38 The peaks at 1681 and 1452 cm−1 corresponding to NH4+ species after reaction with Brønsted acid sites also disappeared immediately after the purge of NO + O2, indicating the high reactivity of Brønsted acid sites. Instead, the peaks at 1627, 1525, and 1241 cm−1 remain stable, which is attributed to the intermediates related to the Lewis acid sites. Herein, we can speculate that Brønsted acid sites play a key role during NH3-SCR.
The order of purged flow was reversed to further evaluate the reactivity of the adsorbed nitrogen oxide species. The catalysts were first treated with NO + O2 for 30 min, and then NH3 was introduced for 30 min to observe the reactions among NO and the NH3-originated intermediates. The results are shown in Fig. 12(b). The pretreatment with NO + O2 results in the form of adsorbed NO2 (1697 cm−1), nitrate (1523 and 1427 cm−1), and nitrite (1168 cm−1) on the catalyst surface. After NH3 is switched in, most peaks of the NO-related species vanish immediately, suggesting that adsorbed NOx species on the catalyst surface participate in the SCR reaction. Meanwhile, new peaks at 1621, 1357, 1064, and 943 cm−1 can be observed, which represent the NH3 coordinated on Lewis acid sites, and weakly adsorbed NH3, respectively. Therefore, one can conclude that the adsorbed NO2, bridge nitrates, and nitrite are quite active during the SCR reactions of the prepared catalysts.
Footnote |
† Electronic supplementary information (ESI) available. See DOI: 10.1039/d1ra07647g |
This journal is © The Royal Society of Chemistry 2022 |