**Andoni Choya , Beatriz de Rivas, Jose Ignacio Gutiérrez-Ortiz and Rubén López-Fonseca \***

Chemical Technologies for Environmental Sustainability Group, Department of Chemical Engineering, Faculty of Science and Technology, University of the Basque Country UPV/EHU, P.O. Box 644, E-48080 Bilbao, Spain; andoni.choya@ehu.eus (A.C.); beatriz.derivas@ehu.eus (B.d.R.); joseignacio.gutierrez@ehu.eus (J.I.G.-O.) **\*** Correspondence: ruben.lopez@ehu.es; Tel.: +34-94-601-5985

Received: 19 June 2020; Accepted: 7 July 2020; Published: 8 July 2020

**Abstract:** Spinel-type cobalt oxide is a highly active catalyst for oxidation reactions owing to its remarkable redox properties, although it generally exhibits poor mechanical, textural and structural properties. Supporting this material on a porous alumina can significantly improve these characteristics. However, the strong cobalt–alumina interaction leads to the formation of inactive cobalt aluminate, which limits the activity of the resulting catalysts. In this work, three different strategies for enhancing the performance of alumina-supported catalysts are examined: (i) surface protection of the alumina with magnesia prior to the deposition of the cobalt precursor, with the objective of minimizing the cobalt–alumina interaction; (ii) coprecipitation of cobalt along with nickel, with the aim of improving the redox properties of the deposited cobalt and (iii) surface protection of alumina with ceria, to provide both a barrier effect, minimizing the cobalt–alumina interaction, and a redox promoting effect on the deposited cobalt. Among the examined strategies, the addition of ceria (20 wt % Ce) prior to the deposition of cobalt resulted in being highly efficient. This sample was characterized by a notable abundance of both Co3<sup>+</sup> and oxygen lattice species, derived from the partial inhibition of cobalt aluminate formation and the insertion of Ce4<sup>+</sup> cations into the spinel lattice.

**Keywords:** cobalt oxide; methane oxidation; modified alumina; magnesium oxide; nickel cobaltite; ceria; lattice distortion; oxygen mobility

#### **1. Introduction**

The commercialization of vehicles driven by natural gas engines is a widely accepted strategy to mitigate the emissions associated with transport, which is one of the largest emitting sectors of greenhouse effect gases, due to their reduced CO2, NOx, particles and hydrocarbons emissions [1,2]. However, the consolidation of this type of vehicles in the automotive fleet requires the control of the residual (around 1%) unburned methane (the main component of natural gas) emissions from the engine, since this pollutant possesses a powerful greenhouse effect potential (around 25 times that of CO<sup>2</sup> in a 100 years period). Owing to the high chemical stability of this compound and its low concentration in the flue gases (<1% vol.), the low-temperature catalytic oxidation appears as an attractive solution for this purpose. In order for this treatment not to significantly increase the cost of the engine, the selected catalyst must present a high activity with a reasonable economic investment.

Traditionally, the most commonly applied catalysts have been based on noble metals such as palladium or platinum [3,4]. However, this type of catalyst is generally expensive, due to the high cost of the noble metals and their relatively high metallic loading (2–4 wt %), and is prone to deactivation by sintering [5,6]. Spinel oxides based on transition metals can be a promising catalytic system for the oxidation of lean methane, due to their lower cost, higher availability and relatively good activity for the oxidation of CO and light hydrocarbons [7,8]. More specifically, bulk spinel-type cobalt oxide (Co3O4) is regarded as a highly interesting substitute to noble metals for catalytic oxidation of trace amounts of methane on the basis of its excellent redox properties [9–12]. However, when prepared by conventional synthesis methodologies [13,14], the textural and structural properties of this oxide tend to be poor. Although some routes can partially overcome this problem, they are normally too complex and difficult to scale up to the industrial operation [15,16].

One possible alternative could be to use a porous media as a support for cobalt oxide, in order to increase the amount of active surface area available for reaction. This generally translates into and enhancement of the physico-chemical properties of the resulting catalyst, but the probability of the occurrence a strong cobalt–support interaction, causing a negative effect on the redox properties of the deposited cobalt, is high. More specifically, when the selected support is high surface gamma alumina, this interaction provokes the formation of a cobalt aluminate phase (CoAl2O4), which is characterized by a poor reducibility and a consequent low specific activity for oxidation reactions [17,18].

A proposed solution would be the modification of the properties of the alumina with the aim of tuning its affinity for the Co3O<sup>4</sup> deposited over it. This can be carried out by incorporating some chemical promoters to the alumina before the deposition of Co3O4, or by adding the promoters after the formation of the final Co/Al2O<sup>3</sup> catalyst. In this sense, Liotta et al. [19] reported that adding Ba during the sol–gel synthesis of Al2O<sup>3</sup> decreased diffusion of the Co2<sup>+</sup> ions into the structure of the alumina after Co deposition. Similarly, Park et al. [20] and Park et al. [21], on different studies, observed that adding phosphorus to Al2O<sup>3</sup> resulted in the formation of a mixed AlPO<sup>4</sup> phase that partially suppressed the formation of CoAl2O4. On the other hand, Cheng et al. [22] found out that the addition of Mn or Fe during the synthesis of a Cu-Co/Al2O<sup>3</sup> catalyst improved the redox properties of both active metals. In addition, El-Shobaky et al. [23] reported an increased activity for CO oxidation of Co3O4/Al2O<sup>3</sup> catalysts doped with small amounts of Mn and/or La.

Similarly, an attractive strategy to improve the performance of this type of catalyst could be using magnesium as a modifier. In this sense, Riad [24] observed that alumina coated with magnesium and prepared by coprecipitation presented better properties than bare alumina. Cobalt catalysts can also be supported over pure magnesium oxide, which results in systems with enhanced activity due to the magnesium–cobalt interaction, as reported by Ulla et al. [25] and Ji et al. [26].

Considering this background, in the present paper various enhancing strategies for γ-alumina-supported cobalt catalysts were examined in order to determine their efficiency for improving the activity of the resulting catalysts for the complete oxidation of methane under lean conditions with respect to an unmodified reference Co/Al2O<sup>3</sup> catalyst (Co/Al sample). The three investigated approaches were the following:


#### **2. Results**

#### *2.1. Physico-Chemical Characterization*

Along with their chemical composition as determined by Wavelength dispersive X-ray fluorescence (WDXRF), the textural properties of the synthesized catalysts in terms of the BET (Brunauer–Emmett–Teller) surface and pore volume are listed in Table 1. Additionally, the properties of

0.35 cm3 g−1.

bare alumina and the modified supports with MgO and CeO<sup>2</sup> are included for comparative purposes. All supports and catalysts exhibited type IV adsorption–desorption isotherms (Figure 1) with H2 type hysteresis cycles, characteristic of mesoporous materials with a relatively broad size distribution. The addition of ceria provoked an appreciable decrease (16%) in the surface area whereas the effect of MgO deposition was virtually negligible. After incorporating the active metallic oxide, the surface area decreased by around 19–32%. Hence, the specific surface area of the catalysts varied in the 93–113 m<sup>2</sup> g −1 range while the pore volume was between 0.27 and 0.35 cm<sup>3</sup> g −1 . *Catalysts* **2020**, *10*, x FOR PEER REVIEW 3 of 18


**Table 1.** Physico-chemical properties of the supported cobalt catalysts. Along with their chemical composition as determined by Wavelength dispersive X‐ray fluorescence (WDXRF), the textural properties of the synthesized catalysts in terms of the BET

Me stands for Mg, Ni or Ce.

**Figure 1.** N2 physisorption isotherms of the supported cobalt catalysts. **Figure 1.** N<sup>2</sup> physisorption isotherms of the supported cobalt catalysts.

**Table 1.** Physico‐chemical properties of the supported cobalt catalysts. **Sample Co Loading, wt % Me Loading, wt % Me/Co Molar Ratio BET Surface, m2 g−<sup>1</sup> Pore Volume, cm3 g−<sup>1</sup> Cophase Crystallite Size, nm** Al2O3 ‐ ‐ ‐ 139 0.56 ‐ The pore size distributions of the supports and the cobalt catalysts are shown in Figure 2. The blank alumina exhibited a bimodal distribution with maxima at 110 and 150 Å, while the distributions were unimodal, centered at 110 Å, over the MgO- and CeO<sup>2</sup> modified supports, thereby showing that the promoter oxides were preferentially deposited on the larger pores of the alumina. On the other hand, all cobalt catalysts exhibited unimodal distributions centered at 90 Å, thus evidencing that cobalt was also massively located on the larger pores of the supports.

Mg‐Al ‐ 6.7 ‐ 145 0.50 ‐ Ce‐Al ‐ 20.6 ‐ 117 0.42 ‐ Co/Al 27.9 0.0 0 108 0.29 29 Co/Mg‐Al 28.7 3.0 0.25 99 0.27 23 Co‐Ni/Al 23.2 4.8 0.21 113 0.35 21 Co/Ce‐Al 29.5 12.4 0.18 93 0.30 23

Me stands for Mg, Ni or Ce.

distributions were unimodal, centered at 110 Å, over the MgO‐ and CeO2 modified supports, thereby showing that the promoter oxides were preferentially deposited on the larger pores of the alumina. On the other hand, all cobalt catalysts exhibited unimodal distributions centered at 90 Å, thus

evidencing that cobalt was also massively located on the larger pores of the supports.

respectively.

range.

**Figure 2.** Pore size distributions of the supported cobalt catalysts. **Figure 2.** Pore size distributions of the supported cobalt catalysts.

The structural characterization of the catalysts was performed by XRD. The diffractograms in Figure 3 revealed signals of a cubic spinel phase (2θ = 19.1°, 31.3°, 37.0°, 45.1°, 59.4° and 65.3°) in the four cobalt catalysts that could be assigned to the presence of both Co3O4 (ICDD 00‐042‐1467) and CoAl2O4 (ICDD 00‐044‐0160) formed by the interaction of the deposited cobalt with the alumina [29,30]. The relative occurrence of these two phases could not be determined since both oxides essentially exhibit the same diffraction signals at similar positions. The structural characterization of the catalysts was performed by XRD. The diffractograms in Figure 3 revealed signals of a cubic spinel phase (2θ = 19.1◦ , 31.3◦ , 37.0◦ , 45.1◦ , 59.4◦ and 65.3◦ ) in the four cobalt catalysts that could be assigned to the presence of both Co3O<sup>4</sup> (ICDD 00-042-1467) and CoAl2O<sup>4</sup> (ICDD 00-044-0160) formed by the interaction of the deposited cobalt with the alumina [29,30]. The relative occurrence of these two phases could not be determined since both oxides essentially exhibit the same diffraction signals at similar positions. *Catalysts* **2020**, *10*, x FOR PEER REVIEW 5 of 18

**Figure 3.** XRD patterns of the supported cobalt catalysts. **Figure 3.** XRD patterns of the supported cobalt catalysts.

On the other hand, weak signals from a cubic phase with low crystallinity were detected at 2θ = 37.7, 45.9 and 66.9◦ that could be attributed to the gamma-alumina (ICDD 01-074-2206). Additionally, various signals from a fluorite-like phase of CeO<sup>2</sup> were detected at 2θ = 28.5◦ , 33.3◦ , 47.5◦ and 56.4◦ for

**Figure 4.** Close up view of the XRD patterns of the supported cobalt catalysts in the 2θ = 36–38°

amount of nickel cobaltite present in this catalyst was probably low.

A closer inspection of the position and width of the A1g mode of the modified catalysts could be helpful in determining a possible distortion of the Co3O4 lattice due to the insertion of cations of the promoters. This influence was analyzed in terms of the shift and the FWHM value of this signal (Figure 5). The shift of the A1g signal of the modified catalysts with respect to the reference Co/Al sample ranged between 4 and 17 cm−1, with the Co‐Ni/Al catalyst exhibiting the largest shift. In addition, the FWHM for the modified catalysts was between 26 and 30 cm−1, while it was 13 cm−<sup>1</sup> for the unmodified catalyst. These results revealed that the most marked lattice distortion occurred over the Co‐Ni/Al catalyst, in line with the results from XRD. However, the Raman spectra of this sample did not show any detectable signals related to the presence of NiCo2O4 in contrast to what the observed the enlargement of the cell size of the crystalline spinel phase suggested. Therefore, the the Co/Ce-Al catalyst. Due to the lower amount of Mg and Ni (<5 wt %), no signals attributable to MgO and NiO were noticed over the Co/Mg-Al and the Co-Ni/Al samples, respectively.

*Catalysts* **2020**, *10*, x FOR PEER REVIEW 5 of 18

The average crystallite size of the cobalt spinel phase was estimated from the full width half maximum (FWHM) of the characteristic peak located at 37.1◦ , assignable to the (311) crystalline plane, by applying the Scherrer equation (Table 1). The crystallite size for the catalyst supported over bare alumina was 29 nm, while it was slightly smaller (21–23 nm) over the modified catalysts. It must be noted that sizes calculated from the refinement were not substantially different from those obtained from single peak data. Furthermore, a close-up view of this signal (Figure 4) revealed a significant 2θ shift towards lower angle values, thus denoting an enlargement of the cell size of the spinel due to the insertion of cations of the promoters into its lattice. In this sense, the Co-Ni/Al catalyst showed the largest growth (a<sup>0</sup> = 8.122 Å) with respect to the catalyst supported over bare alumina (a<sup>0</sup> = 8.096 Å). This remarkable growth may indicate the presence of the nickel cobaltite mixed spinel (NiCo2O4) in this sample [28,31]. **Figure 3.** XRD patterns of the supported cobalt catalysts.

**Figure 4.** Close up view of the XRD patterns of the supported cobalt catalysts in the 2θ = 36–38° **Figure 4.** Close up view of the XRD patterns of the supported cobalt catalysts in the 2θ = 36–38◦ range.

range. A closer inspection of the position and width of the A1g mode of the modified catalysts could be helpful in determining a possible distortion of the Co3O4 lattice due to the insertion of cations of the promoters. This influence was analyzed in terms of the shift and the FWHM value of this signal (Figure 5). The shift of the A1g signal of the modified catalysts with respect to the reference Co/Al sample ranged between 4 and 17 cm−1, with the Co‐Ni/Al catalyst exhibiting the largest shift. In addition, the FWHM for the modified catalysts was between 26 and 30 cm−1, while it was 13 cm−<sup>1</sup> for the unmodified catalyst. These results revealed that the most marked lattice distortion occurred over the Co‐Ni/Al catalyst, in line with the results from XRD. However, the Raman spectra of this sample did not show any detectable signals related to the presence of NiCo2O4 in contrast to what the observed the enlargement of the cell size of the crystalline spinel phase suggested. Therefore, the A closer inspection of the position and width of the A1g mode of the modified catalysts could be helpful in determining a possible distortion of the Co3O<sup>4</sup> lattice due to the insertion of cations of the promoters. This influence was analyzed in terms of the shift and the FWHM value of this signal (Figure 5). The shift of the A1g signal of the modified catalysts with respect to the reference Co/Al sample ranged between 4 and 17 cm−<sup>1</sup> , with the Co-Ni/Al catalyst exhibiting the largest shift. In addition, the FWHM for the modified catalysts was between 26 and 30 cm−<sup>1</sup> , while it was 13 cm−<sup>1</sup> for the unmodified catalyst. These results revealed that the most marked lattice distortion occurred over the Co-Ni/Al catalyst, in line with the results from XRD. However, the Raman spectra of this sample did not show any detectable signals related to the presence of NiCo2O<sup>4</sup> in contrast to what the observed the enlargement of the cell size of the crystalline spinel phase suggested. Therefore, the amount of nickel cobaltite present in this catalyst was probably low.

amount of nickel cobaltite present in this catalyst was probably low.

**Figure 5.** Raman spectra of the supported cobalt catalysts. **Figure 5.** Raman spectra of the supported cobalt catalysts.

Figure 6 shows the Co2p3/2 XPS spectra of the samples. The spectra of all catalysts were composed of five different signals. As for the Co/Al sample the two features with the lowest binding energies, located at 779.5 and 781.0 eV, were assigned to Co3+ and Co2+ ions, respectively, while the signal centered at 783.2 eV was attributed to the presence of CoO in the surface of the samples [32,33]. The two signals with the highest binding energies (786.2 and 790.1 eV) were identified as the satellite signals from Co3+ and Co2+ ions, respectively. The position of the main signal of the Co2p3/2 spectra can be used as an indication of the predominant cobalt species on the surface of each sample. Thus, higher binding energy values suggested a higher abundance of Co2+ cations, while lower binding energies pointed out a favored presence of Co3+ cations. In this sense, the position of the main signal of the unmodified catalyst was 781.1 eV, thereby evidencing a significant presence of Co2+ ions, in line with its higher CoAl2O4 content as deduced by Raman spectroscopy. Conversely, the main signal for the Co/Mg‐Al sample was centered at 780.8 eV assignable to a slightly lower Co2+ content. This observation was not coherent with the results from Raman spectroscopy that evidenced that the presence of CoAl2O4 in this sample was appreciably limited. For this reason, the increased Co2+ presence was not attributed to the presence of cobalt aluminate, but rather to the probable formation of a Co‐Mg solid solution, as already reported elsewhere [34,35]. Figure 6 shows the Co2p3/<sup>2</sup> XPS spectra of the samples. The spectra of all catalysts were composed of five different signals. As for the Co/Al sample the two features with the lowest binding energies, located at 779.5 and 781.0 eV, were assigned to Co3<sup>+</sup> and Co2<sup>+</sup> ions, respectively, while the signal centered at 783.2 eV was attributed to the presence of CoO in the surface of the samples [32,33]. The two signals with the highest binding energies (786.2 and 790.1 eV) were identified as the satellite signals from Co3<sup>+</sup> and Co2<sup>+</sup> ions, respectively. The position of the main signal of the Co2p3/<sup>2</sup> spectra can be used as an indication of the predominant cobalt species on the surface of each sample. Thus, higher binding energy values suggested a higher abundance of Co2<sup>+</sup> cations, while lower binding energies pointed out a favored presence of Co3<sup>+</sup> cations. In this sense, the position of the main signal of the unmodified catalyst was 781.1 eV, thereby evidencing a significant presence of Co2<sup>+</sup> ions, in line with its higher CoAl2O<sup>4</sup> content as deduced by Raman spectroscopy. Conversely, the main signal for the Co/Mg-Al sample was centered at 780.8 eV assignable to a slightly lower Co2<sup>+</sup> content. This observation was not coherent with the results from Raman spectroscopy that evidenced that the presence of CoAl2O<sup>4</sup> in this sample was appreciably limited. For this reason, the increased Co2<sup>+</sup> presence was not attributed to the presence of cobalt aluminate, but rather to the probable formation of a Co-Mg solid solution, as already reported elsewhere [34,35].

On the other hand, the main signals of the Co‐Ni/Al and Co‐Ce/Al catalysts exhibited a significant shift towards lower binding energies with respect to the Co/Al sample. Thus, both catalysts displayed their main signal centered at about 780.1 eV, thus evidencing their higher content in Co3+ cations. Additionally, the Ni2p3/2 spectra of the Co‐Ni/Al catalyst (not shown) were deconvoluted into five signals. Hence, three main contributions at 853.7, 855.3 and 857.3 eV were attributed to the presence of Ni2+ as NiO, Ni2+ belonging to a spinel lattice and Ni3+ cations, respectively, while the signals at 861.2 and 866.5 eV were assigned to the satellites of Ni2+ and Ni3+ cations, respectively. The relatively low binding energy of the signal associated with the presence of Ni2+ cations in a spinel lattice (855.3 eV) also denoted that these species were mainly a part of the NiCo2O4 spinel instead of the NiAl2O4, for which the binding energy of that signal would be expectedly higher (ca. 856.0 eV), as shown by other studies [36,37]. On the other hand, the main signals of the Co-Ni/Al and Co-Ce/Al catalysts exhibited a significant shift towards lower binding energies with respect to the Co/Al sample. Thus, both catalysts displayed their main signal centered at about 780.1 eV, thus evidencing their higher content in Co3<sup>+</sup> cations. Additionally, the Ni2p3/<sup>2</sup> spectra of the Co-Ni/Al catalyst (not shown) were deconvoluted into five signals. Hence, three main contributions at 853.7, 855.3 and 857.3 eV were attributed to the presence of Ni2<sup>+</sup> as NiO, Ni2<sup>+</sup> belonging to a spinel lattice and Ni3<sup>+</sup> cations, respectively, while the signals at 861.2 and 866.5 eV were assigned to the satellites of Ni2<sup>+</sup> and Ni3<sup>+</sup> cations, respectively. The relatively low binding energy of the signal associated with the presence of Ni2<sup>+</sup> cations in a spinel lattice (855.3 eV) also denoted that these species were mainly a part of the NiCo2O<sup>4</sup> spinel instead of the NiAl2O4, for which the binding energy of that signal would be expectedly higher (ca. 856.0 eV), as shown by other studies [36,37].

**Figure 6.** Co2p3/2 XPS spectra of the supported cobalt catalysts. **Figure 6.** Co2p3/<sup>2</sup> XPS spectra of the supported cobalt catalysts.

The deconvolution and integration of the XPS spectra allowed for a quantitative analysis of the composition of the surface, as shown in Table 2. Firstly, it must be noticed that the surface cobalt loading of the Co/Al sample and particularly Co/Mg‐Al sample was significantly lower than their bulk content, which, on one hand, suggested that a notable fraction of Co species was as CoAl2O4 and, on the other hand, evidenced a marked formation of the aforementioned Co‐Mg solid solution. These results would be in agreement with the relatively low Co3+/Co2+ molar ratios of these catalysts (0.67 and 0.94, respectively). The deconvolution and integration of the XPS spectra allowed for a quantitative analysis of the composition of the surface, as shown in Table 2. Firstly, it must be noticed that the surface cobalt loading of the Co/Al sample and particularly Co/Mg-Al sample was significantly lower than their bulk content, which, on one hand, suggested that a notable fraction of Co species was as CoAl2O<sup>4</sup> and, on the other hand, evidenced a marked formation of the aforementioned Co-Mg solid solution. These results would be in agreement with the relatively low Co3+/Co2<sup>+</sup> molar ratios of these catalysts (0.67 and 0.94, respectively).


On the other hand, a substantial surface cobalt enrichment was noticed for the Co‐Ni/Al and Co/Ce‐Al catalysts, thus pointing out that deposited cobalt was preferentially located on the external **Table 2.** Surface composition of the supported cobalt catalysts.

Krevelen mechanism [38,39]. As revealed by our results, its abundance was optimized over the The values in brackets correspond to the bulk composition. Me stands for Mg, Ni or Ce.

Co/Ce‐Al catalyst. It is quite reasonable to expect that the Ce3+/Ce4+ relative abundance can play a role in controlling the activity of the Co/Ce‐Al. Unfortunately, since the amount of Ce at the surface of the catalyst is very low, a proper deconvolution of the Ce3d XPS spectrum devoted to the evaluation of the Ce3+/Ce4+ molar ratio was not possible. In this sense, we have shown elsewhere [40] that an inverse relationship between the Ce3+/Ce4+ and the Co3+/Co2+ molar ratios, as determined by XPS, for a series of Ce‐doped bulk Co3O4 catalysts with a Ce/Co molar ratio between 0.03 and 0.14 (corresponding to 5–20 wt % Ce). These results could be explained in terms of the equilibrium Ce3+ + Co3+ ↔ Ce4+ + Co2+, established by the requirement of charge balance within the cations of the spinel lattice. Since our XRD and Raman measurements suggested the insertion of Ce cations into the Co3O4 lattice in the Co/Ce‐Al sample, the aforementioned effect could also be occurring in this catalyst. This would explain the higher surface Co3+/Co2+ molar ratio among all the samples. **Table 2.** Surface composition of the supported cobalt catalysts. **Catalyst Co, wt % Me, wt % Co3+/Co2+ Molar Ratio Oads/Olatt Molar Ratio** On the other hand, a substantial surface cobalt enrichment was noticed for the Co-Ni/Al and Co/Ce-Al catalysts, thus pointing out that deposited cobalt was preferentially located on the external surface and it did not tend to strongly interact with the support. This in turn was in good agreement with the higher Co3+/Co2<sup>+</sup> molar ratios of these samples (1.21 and 1.38, respectively). It is worth pointing out that this higher abundance of Co3<sup>+</sup> species at the surface was accompanied by a more notable presence of lattice oxygen species in the Co-Ni/Al and Co/Ce-Al catalysts, as shown in Table 2. This type of oxygen species is usually involved in the oxidation of methane by a Mars-van Krevelen mechanism [38,39]. As revealed by our results, its abundance was optimized over the Co/Ce-Al catalyst. It is quite reasonable to expect that the Ce3+/Ce4<sup>+</sup> relative abundance can play a role in controlling the activity of the Co/Ce-Al. Unfortunately, since the amount of Ce at the surface of the catalyst is very low, a proper deconvolution of the Ce3d XPS spectrum devoted to the evaluation of the Ce3+/Ce4<sup>+</sup> molar ratio was not possible. In this sense, we have shown elsewhere [40] that an inverse relationship between the Ce3+/Ce4<sup>+</sup> and the Co3+/Co2<sup>+</sup> molar ratios, as determined by XPS, for a series of Ce-doped bulk Co3O<sup>4</sup> catalysts with a Ce/Co molar ratio between 0.03 and 0.14 (corresponding to 5–20 wt % Ce).

Co/Al 22.6 (27.9) ‐ 0.67 1.41

These results could be explained in terms of the equilibrium Ce3<sup>+</sup> <sup>+</sup> Co3<sup>+</sup> <sup>↔</sup> Ce4<sup>+</sup> <sup>+</sup> Co2+, established by the requirement of charge balance within the cations of the spinel lattice. Since our XRD and Raman measurements suggested the insertion of Ce cations into the Co3O<sup>4</sup> lattice in the Co/Ce-Al sample, the aforementioned effect could also be occurring in this catalyst. This would explain the higher surface Co3+/Co2<sup>+</sup> molar ratio among all the samples. Co/Mg‐Al 13.3 (28.7) 4.4 (3.0) 0.94 1.02 Co‐Ni/Al 25.4 (23.2) 8.2 (4.8) 1.21 0.94 Co/Ce‐Al 32.9 (29.5) 3.2 (12.4) 1.38 0.77 The values in brackets correspond to the bulk composition. Me stands for Mg, Ni or Ce. The redox properties of the cobalt catalysts were investigated by temperature‐programmed

The redox properties of the cobalt catalysts were investigated by temperature-programmed reduction with hydrogen (H2-TPR) and temperature-programmed reaction with methane in the absence of oxygen (CH4-TPRe). As widely accepted, the H2-TPR profile of the base alumina-supported Co3O<sup>4</sup> catalyst (Figure 7) evidenced a two-step reduction process [41,42]. A first H<sup>2</sup> uptake at low temperatures (<550 ◦C) was associated with the reduction of Co3O4, which in turn could be subdivided into two contributions located at around 270–310 ◦C, assignable to the reduction of Co3<sup>+</sup> ions into Co2+, and at 350–400 ◦C, attributable to the subsequent reduction of Co2<sup>+</sup> into metallic cobalt. This second H<sup>2</sup> uptake did not take the shape of a single peak, but instead was formed of at least two different contributions, which suggested the presence of Co2<sup>+</sup> species with varying reducibilities. The presence of this type of species was much more noticeable for the Co/Mg-Al catalysts, where the temperature window for this second reduction event extended from 300 to 550 ◦C. On the other hand, the marked H<sup>2</sup> consumption located at high temperatures (>600 ◦C) over the four catalysts was attributed to the reduction of cobalt aluminate [43]. reduction with hydrogen (H2‐TPR) and temperature‐programmed reaction with methane in the absence of oxygen (CH4‐TPRe). As widely accepted, the H2‐TPR profile of the base alumina‐supported Co3O4 catalyst (Figure 7) evidenced a two‐step reduction process [41,42]. A first H2 uptake at low temperatures (<550 °C) was associated with the reduction of Co3O4, which in turn could be subdivided into two contributions located at around 270–310 °C, assignable to the reduction of Co3+ ions into Co2+, and at 350–400 °C, attributable to the subsequent reduction of Co2+ into metallic cobalt. This second H2 uptake did not take the shape of a single peak, but instead was formed of at least two different contributions, which suggested the presence of Co2+ species with varying reducibilities. The presence of this type of species was much more noticeable for the Co/Mg‐Al catalysts, where the temperature window for this second reduction event extended from 300 to 550 °C. On the other hand, the marked H2 consumption located at high temperatures (>600 °C) over the four catalysts was attributed to the reduction of cobalt aluminate [43].

**Figure 7.** Temperature‐programmed reduction with hydrogen (H2‐TPR) profiles of the supported cobalt catalysts. **Figure 7.** Temperature-programmed reduction with hydrogen (H<sup>2</sup> -TPR) profiles of the supported cobalt catalysts.

The relative amount of each type of Co species present in the various catalysts was estimated by deconvolution of the experimental TPR profiles. The threshold temperature of 550 °C was taken as a criterion to distinguish between easily reducible cobalt species (low‐temperature uptake), namely free Co3O4 (200–450 °C) and some mixed cobalt‐metal species (450–550 °C) such as cobalt‐magnesium species, and hardly reducible cobalt species (high‐temperature uptake) in the form of cobalt aluminate (>550 °C). The results are summarized in Table 3. The relative amount of each type of Co species present in the various catalysts was estimated by deconvolution of the experimental TPR profiles. The threshold temperature of 550 ◦C was taken as a criterion to distinguish between easily reducible cobalt species (low-temperature uptake), namely free Co3O<sup>4</sup> (200–450 ◦C) and some mixed cobalt-metal species (450–550 ◦C) such as cobalt-magnesium species, and hardly reducible cobalt species (high-temperature uptake) in the form of cobalt aluminate (>550 ◦C). The results are summarized in Table 3.

**Table 3.** Characterization by H2‐TPR and temperature‐programmed reaction with methane in the absence of oxygen (CH4‐TPRe) of the supported cobalt catalysts.

> **High‐Temperature H2 Uptake, mmol gCo−<sup>1</sup>**

**Catalyst Low‐Temperature H2**

**Uptake, mmol gCo−<sup>1</sup>**

**H2‐TPR CH4‐TPRe**

**Low‐Temperature O2 Consumption, mmol gCo−<sup>1</sup>**

**Onset Reduction Temperature, °C**


**Table 3.** Characterization by H<sup>2</sup> -TPR and temperature-programmed reaction with methane in the absence of oxygen (CH<sup>4</sup> -TPRe) of the supported cobalt catalysts.

Firstly, it must be noticed that the H<sup>2</sup> uptake at low temperatures, associated with species with a high reducibility, mainly free of Co3O4, was larger for the three modified catalysts with respect to the Co/Al sample. The increase in H<sup>2</sup> uptake was 5% for the Co/Mg-Al, 28% for the Co-Ni/Al and 39% for the Co/Ce-Al, thus showing that nickel and cerium were efficient redox promoters for cobalt. On one hand, for the Co-Ni/Al catalyst, the increase in H<sup>2</sup> uptake at a low temperature could be due to the presence of the NiCo2O<sup>4</sup> spinel, which possesses a higher specific H<sup>2</sup> uptake than Co3O4. On the other hand, for the Co/Ce-Al sample, the increase could be related to the reduction of the surface of the ceria, which is known to occur at around 450–500 ◦C [44], and also the improved reducibility of cobalt oxide due to the insertion of cerium cations into its lattice. Additionally, the onset reduction temperature of the three modified catalysts was clearly lowered. The most noticeable temperature shift occurred for the catalyst modified with nickel (50 ◦C), which could be due to the presence of nickel cobaltite, while it was much less significant for the Co/Ce-Al catalyst (5 ◦C).

On the other hand, the H<sup>2</sup> uptake assignable to the presence of CoAl2O<sup>4</sup> was only lower for the Co/Ce-Al catalyst (8.5 mmol gCo −1 ) with respect to the Co/Al sample (10.2 mmol gCo −1 ); while it was notably higher (12.9 mmol gCo −1 ) over the Co-Ni/Al catalyst. This could be due to ceria acting as a physical barrier between cobalt and alumina, whereas both cobalt and nickel were directly deposited on the alumina in the case of the Co-Ni/Al sample. Therefore, the cobalt–alumina interaction was not apparently limited over this sample. Alternatively, given that the Co/Mg-Al catalyst showed a comparable H<sup>2</sup> uptake at high temperatures (10.4 mmol gCo −1 ), it could be thought that such a barrier effect could be ruled out in this catalyst as well. However, it must be noticed that a certain fraction of this H<sup>2</sup> uptake would probably be due to the partial reduction of a Co-MgO solid solution. Therefore, the total H<sup>2</sup> uptake associated with the presence of cobalt aluminate was probably lower than that of the Co/Al sample.

As a complement of the H2-TPR analysis, the reactivity of oxygen species present in the examined catalysts was also analyzed by temperature-programmed reaction with methane in the absence of oxygen (CH4-TPRe). The evolution of evolved CO2, CO and H<sup>2</sup> was monitored by mass spectrometry. In general, the CO<sup>2</sup> profiles evidenced a two-step reaction process, as depicted in Figure S1, Supplementary Material. The low-temperature reaction step was attributed to the complete oxidation of methane by lattice oxygen species associated with Co3<sup>+</sup> ions. No CO or H<sup>2</sup> formation was detected at this temperature interval. The amount of CO<sup>2</sup> evolved from the complete oxidation reaction was barely perceptible over the Co/Al sample. Above 525–550 ◦C the methane partial oxidation occurred, where methane reacted with low-mobility oxygen species associated with Co2<sup>+</sup> ions, yielding significant amounts of CO and H<sup>2</sup> along with CO<sup>2</sup> [14]. It must be noted that the occurrence of this second process was not observed over the Co/Al catalyst, thus suggesting that it could only take place at temperatures higher than 600 ◦C.

The comparatively larger formation of CO<sup>2</sup> above 500 ◦C made the proper analysis of the obtained results in the low-temperature range rather difficult. For this reason, Figure 8 only focuses on the evolution of the CO<sup>2</sup> yield between 100 and 550 ◦C. It was thus clearly evidenced that the three investigated enhancing strategies were efficient for increasing the amount of reactive oxygen in the resulting cobalt catalysts. More specifically, the O<sup>2</sup> consumption at low temperatures (Table 3) increased from 0.28 mmol gCo −1 for the Co/Al sample up to 0.61–0.88 mmol gCo −1 for the modified catalysts,

with the Co/Ce-Al achieving the highest value. Note that the amount of reacted O<sup>2</sup> was relatively limited over the Co/Mg-Al sample in spite of its higher Me/Co molar ration (0.25). Additionally, this low-temperature step peaked at lower temperatures with respect to the reference cobalt catalyst. The temperature shift was as high as 67 ◦C for the Co-Ni/Al catalyst. Such remarkable improvement could be due to the presence of NiCo2O<sup>4</sup> in this sample, which has been already reported to be highly reducible and active for methane oxidation elsewhere [27,45]. *Catalysts* **2020**, *10*, x FOR PEER REVIEW 10 of 18

**Figure 8.** Close up view of the CH4‐TPRe profiles of the supported cobalt catalysts in the 100–550 °C temperature range. **Figure 8.** Close up view of the CH<sup>4</sup> -TPRe profiles of the supported cobalt catalysts in the 100–550 ◦C temperature range.

Given the notable redox behavior of the Co‐Ni/Al and Co/Ce‐Al catalysts, these were examined by high angle annular dark field—scanning transmission electronic microscopy (HAADF–STEM) coupled with electron energy loss spectroscopy (EELS) or energy dispersive X‐ray spectrometry (EDX), respectively. Elemental maps (Figure 9 and Figure S2, Supplementary Material) were generated for certain areas in each sample to allow studying the spatial distribution of cobalt and nickel or cerium in the bimetallic catalysts. These results evidenced that both Ni and Ce were homogenously present over the supported nanoparticles. In the case of nickel, this probably means that it was forming nickel cobaltite. The Co/Ce‐Al sample also contained small nanoparticles of cerium species (as ceria) of around 10–20 nm. Given the notable redox behavior of the Co-Ni/Al and Co/Ce-Al catalysts, these were examined by high angle annular dark field—scanning transmission electronic microscopy (HAADF–STEM) coupled with electron energy loss spectroscopy (EELS) or energy dispersive X-ray spectrometry (EDX), respectively. Elemental maps (Figure 9 and Figure S2, Supplementary Material) were generated for certain areas in each sample to allow studying the spatial distribution of cobalt and nickel or cerium in the bimetallic catalysts. These results evidenced that both Ni and Ce were homogenously present over the supported nanoparticles. In the case of nickel, this probably means that it was forming nickel cobaltite. The Co/Ce-Al sample also contained small nanoparticles of cerium species (as ceria) of around 10–20 nm.

#### *2.2. Catalytic Performance*

**20 nm**

Three consecutive light-off tests were carried out for each catalyst. The second and third cycles were characterized by an identical light-off curve. Hence, the light-off curves corresponding to the third cycle of each catalyst are shown in Figure 10. It must be noticed that all four samples presented 100% selectivity towards CO2. It was clear that the three modified catalysts resulted were remarkably more efficient than the base Co/Al catalyst. In this sense, the corresponding T<sup>50</sup> value (Table 4) was lowered by 15 (Co/Mg-Al), 50 (Co-Ni/Al) and 70 ◦C (Co/Ce-Al). Note that the intrinsic activity of the Co-free alumina supports (pure Al2O3, Mg-Al and Ce-Al) was negligible at 600 ◦C.

**Figure 9.** High angle annular dark field–scanning transmission electron microscopy (HAADF–STEM) images of the Co‐Ni/Al (**left**) and Co/Ce‐Al (**right**) catalysts coupled to electron cerium species (as ceria) of around 10–20 nm.

temperature range.

**Figure 8.** Close up view of the CH4‐TPRe profiles of the supported cobalt catalysts in the 100–550 °C

Given the notable redox behavior of the Co‐Ni/Al and Co/Ce‐Al catalysts, these were examined by high angle annular dark field—scanning transmission electronic microscopy (HAADF–STEM) coupled with electron energy loss spectroscopy (EELS) or energy dispersive X‐ray spectrometry (EDX), respectively. Elemental maps (Figure 9 and Figure S2, Supplementary Material) were generated for certain areas in each sample to allow studying the spatial distribution of cobalt and nickel or cerium in the bimetallic catalysts. These results evidenced that both Ni and Ce were homogenously present over the supported nanoparticles. In the case of nickel, this probably means

**Figure 9.** High angle annular dark field–scanning transmission electron microscopy (HAADF–STEM) images of the Co‐Ni/Al (**left**) and Co/Ce‐Al (**right**) catalysts coupled to electron **Figure 9.** High angle annular dark field–scanning transmission electron microscopy (HAADF–STEM) images of the Co-Ni/Al (**left**) and Co/Ce-Al (**right**) catalysts coupled to electron energy loss spectroscopy (EELS; Co (red) and Ni (blue)) and energy dispersive X-ray spectrometry (EDX; Co (red) and Ce (green)) elemental distribution. 100% selectivity towards CO2. It was clear that the three modified catalysts resulted were remarkably more efficient than the base Co/Al catalyst. In this sense, the corresponding T50 value (Table 4) was lowered by 15 (Co/Mg‐Al), 50 (Co‐Ni/Al) and 70 °C (Co/Ce‐Al). Note that the intrinsic activity of the Co‐free alumina supports (pure Al2O3, Mg‐Al and Ce‐Al) was negligible at 600 °C.

**Figure 10.** Light off curves of the supported cobalt catalysts. **Figure 10.** Light off curves of the supported cobalt catalysts.



Co/Ce‐Al 480 3.2 80 ± 2

energies were around 80–84 kJ mol−1, a value comparable to those reported in other studies for methane oxidation over Co3O4‐based catalysts [48,49]. Thus, it could be concluded that the main

On the other hand, the specific reaction rates of the various catalysts were estimated by the differential method (for methane conversions lower than 20%). In this analysis, for the sake of proper comparison, the specific activity of the various catalysts were calculated at the same temperature (400 °C) and normalized per gram of cobalt. The results are shown in Table 4. All three

active species in all four catalysts was free of Co3O4.

The apparent activation energy of the four evaluated catalysts (Table 4) were estimated by the

The apparent activation energy of the four evaluated catalysts (Table 4) were estimated by the integral method, assuming that the reaction kinetics followed a pseudo-order one for methane and a zeroth order for oxygen, as it is usual for the Mars–van Krevelen mechanism in the presence of excess oxygen [46,47]. The corresponding linearized plots are depicted in Figure S2. The activation energies were around 80–84 kJ mol−<sup>1</sup> , a value comparable to those reported in other studies for methane oxidation over Co3O4-based catalysts [48,49]. Thus, it could be concluded that the main active species in all four catalysts was free of Co3O4.

On the other hand, the specific reaction rates of the various catalysts were estimated by the differential method (for methane conversions lower than 20%). In this analysis, for the sake of proper comparison, the specific activity of the various catalysts were calculated at the same temperature (400 ◦C) and normalized per gram of cobalt. The results are shown in Table 4. All three modified samples achieved higher reaction rates (1.5–3.2 mmol CH<sup>4</sup> gCo <sup>−</sup><sup>1</sup> h −1 ) with respect to the unmodified counterpart (1.2 mmol CH<sup>4</sup> gCo <sup>−</sup><sup>1</sup> h −1 ). The catalyst promoted with ceria (Co/Ce-Al), in particular, presented the highest reaction rate, which was almost three times higher than that of the catalyst supported over bare alumina. *Catalysts* **2020**, *10*, x FOR PEER REVIEW 12 of 18 modified samples achieved higher reaction rates (1.5–3.2 mmol CH4 gCo−<sup>1</sup> h−1) with respect to the unmodified counterpart (1.2 mmol CH4 gCo−<sup>1</sup> h−1). The catalyst promoted with ceria (Co/Ce‐Al), in particular, presented the highest reaction rate, which was almost three times higher than that of the catalyst supported over bare alumina.

In view of these results, modifying the alumina support with ceria prior to the deposition of cobalt would be a quite promising strategy to be developed for improving the activity of cobalt catalysts. Interestingly, when cobalt was deposited over the Ce-modified support, a dual beneficial effect was evidenced. On one hand, ceria was found to act as a physical barrier between alumina and deposited cobalt, limiting the cobalt–alumina interaction and the subsequent cobalt aluminate formation. On the other hand, the interaction between cobalt and ceria led to a partial incorporation of cerium ions into the lattice of Co3O4. Both phenomena in turn led to a larger abundance of Co3<sup>+</sup> and therefore to a promoted mobility of the lattice oxygen species at low temperatures with ceria loading as shown in Figure 11. In view of these results, modifying the alumina support with ceria prior to the deposition of cobalt would be a quite promising strategy to be developed for improving the activity of cobalt catalysts. Interestingly, when cobalt was deposited over the Ce‐modified support, a dual beneficial effect was evidenced. On one hand, ceria was found to act as a physical barrier between alumina and deposited cobalt, limiting the cobalt–alumina interaction and the subsequent cobalt aluminate formation. On the other hand, the interaction between cobalt and ceria led to a partial incorporation of cerium ions into the lattice of Co3O4. Both phenomena in turn led to a larger abundance of Co3+ and therefore to a promoted mobility of the lattice oxygen species at low temperatures with ceria loading as shown in Figure 11.

**Figure 11.** Relationship among specific reaction rate and: surface Co3+/Co2+ and Oads/Olatt molar ratios (**left**); low‐temperature H2 uptake from H2‐TPR and low‐temperature O2 consumption from CH4‐TPRe (**right**). **Figure 11.** Relationship among specific reaction rate and: surface Co3+/Co2<sup>+</sup> and Oads/Olatt molar ratios (**left**); low-temperature H<sup>2</sup> uptake from H<sup>2</sup> -TPR and low-temperature O<sup>2</sup> consumption from CH<sup>4</sup> -TPRe (**right**).

#### **3. Materials and Methods 3. Materials and Methods**

followed by a calcination step (600 °C for 4 h).

and/or Ni) was fixed at 30 wt %.

#### *3.1. Catalyst Preparation*

*3.1. Catalyst Preparation* A commercial γ‐alumina kindly provided by Saint Gobain was used as the base support. Alternatively, the alumina was modified with MgO (Mg‐Al) or CeO2 (Ce‐Al), which were incorporated by precipitation, starting with magnesium nitrate and cerium nitrate, respectively, A commercial γ-alumina kindly provided by Saint Gobain was used as the base support. Alternatively, the alumina was modified with MgO (Mg-Al) or CeO<sup>2</sup> (Ce-Al), which were incorporated by precipitation, starting with magnesium nitrate and cerium nitrate, respectively, followed by a calcination step (600 ◦C for 4 h).

Afterwards, the precipitates were thoroughly washed with deionized water in order to remove the residual sodium ions that are known to be detrimental for the activity of the resulting catalysts [40]. The washed precipitates were dried at 110 °C for 16 h and then subjected to calcination at 600 °C for 4 h in static air. The Me/Co molar ratio (where M = Mg, Ni or Ce) of the modified catalysts was 0.20 for the Co‐Ni/Al and Co/Ce‐Al samples and 0.25 for the Co/Mg‐Al catalyst, as dictated from a previous optimization for this type of cobalt catalysts [51,52]. The total amount of active metal (Co

Four alumina supported cobalt oxide catalysts, namely Co/Al, Co‐Ni/Al, Co/Mg‐Al and Co/Ce‐Al, were prepared following a simple precipitation route as detailed elsewhere [50]. This

Four alumina supported cobalt oxide catalysts, namely Co/Al, Co-Ni/Al, Co/Mg-Al and Co/Ce-Al, were prepared following a simple precipitation route as detailed elsewhere [50]. This methodology consisted of the precipitation of aqueous solutions of cobalt nitrate hexahydrate and eventually nickel nitrate hexahydrate with adjusted concentrations by the drop-by-drop addition of a sodium carbonate 1.2 M solution at a constant temperature of 80 ◦C until pH 8.5 was achieved. Afterwards, the precipitates were thoroughly washed with deionized water in order to remove the residual sodium ions that are known to be detrimental for the activity of the resulting catalysts [40]. The washed precipitates were dried at 110 ◦C for 16 h and then subjected to calcination at 600 ◦C for 4 h in static air. The Me/Co molar ratio (where M = Mg, Ni or Ce) of the modified catalysts was 0.20 for the Co-Ni/Al and Co/Ce-Al samples and 0.25 for the Co/Mg-Al catalyst, as dictated from a previous optimization for this type of cobalt catalysts [51,52]. The total amount of active metal (Co and/or Ni) was fixed at 30 wt %.

#### *3.2. Characterisation Techniques*

Wavelength dispersive X-ray fluorescence (WDXRF) determined the composition of the synthesized catalysts. Previously, a boron pearl glass was obtained by mixing the corresponding catalyst with a commercial flux agent (Spectromelt A12) with a 1:20 mass ratio. This mixture was then melted at 1200 ◦C. Measurements were performed under vacuum with PANalytical AXIOS sequential WDXRF spectrometer equipped with a Rh tube and three different detectors (gas flow, scintillation and Xe sealed).

Specific surface area (BET method), pore volume (BJH method) and pore size distribution (BJH method) were estimated by low-temperature (−196 ◦C) N<sup>2</sup> physisorption with a Micromeritics TriStar II instrument. The samples were submitted to degassing before analysis with flowing N<sup>2</sup> in a Micromeritics SmartPrep sample preparation system at 300 ◦C for 10 h.

Powder X-ray diffraction (XRD) and Raman spectroscopy were used for the structural characterization of the cobalt catalysts. XRD data were collected on an X'PERT-PRO X-ray diffractometer using Cu Kα radiation (λ = 1.5406 Å) and a Ni filter at 40 kV and 40 mA. The patterns were collected with the 2θ range from 10 to 80◦ with a step size of 0.026◦ and a counting time of 2.0 s. The cell size of the Co-spinel phase was calculated by profile matching of the whole diffractogram using FullProf.2k software. Raman measurements were performed on a Renishaw InVia Raman spectrometer using a 514 nm laser source (ion-argon laser, Modu-Laser), scanning from 150 to 1200 cm−<sup>1</sup> . For each analysis, 20 s were employed and 5 scans were accumulated

X-ray photoelectron spectroscopy (XPS) was employed for characterizing the structure and chemical composition and the electronic structure at the surface level. The analysis was carried out with a SPECS system coupled to a Phoibos 150 1D analyzer and a DLD (Delay−Line Detector)-monochromatic radiation source.

The redox behavior of the cobalt catalysts was examined by temperature-programmed reduction with hydrogen (H2-TPR) with a Micromeritics Autochem 2920 equipment with a 5%H2/Ar stream. The samples were first conditioned at 300 ◦C for 30 min with a flowing 5% O2/He mixture. Next, they were cooled down to 50 ◦C in an inert stream. The reduction process was conducted up to 600 ◦C with a heating rate of 10 ◦C min−<sup>1</sup> . In addition, the reducibility of the samples was also examined by temperature-programmed reaction with methane (CH4-TPRe) with a 5% CH4/He mixture.

Elemental maps of Co, Ni and Ce were obtained by electron energy loss spectroscopy (EELS) or energy dispersive X-ray spectrometry (EDX), both in the scanning transmission electron microscopy—high angle annular dark field (STEM–HAADF) mode (FEI Titan Cubed operating at 300 kV and Philips CM200 operating at 200 kV), with a Tridiem Energy Filter (Gatan) and Super-X detector (ChemiSTEM) as detectors, respectively. The Co-Ni/Al and Co/Ce-Al samples were characterized by EELS-STEM and EDS-STEM, respectively.
