BaFe1−xCuxO3 Perovskites as Active Phase for Diesel (DPF) and Gasoline Particle Filters (GPF)

BaFe1−xCuxO3 perovskites (x = 0, 0.1, 0.3 and 0.4) have been synthetized, characterized and tested for soot oxidation in both Diesel and Gasoline Direct Injection (GDI) exhaust conditions. The catalysts have been characterized by BET, ICP-OES, SEM-EDX, XRD, XPS, H2-TPR and O2-TPD and the results indicate the incorporation of copper in the perovskite lattice which leads to: (i) the deformation of the initial hexagonal perovskite structure for the catalyst with the lowest copper content (BFC1), (ii) the modification to cubic from hexagonal structure for the high copper content catalysts (BFC3 and BFC4), (iii) the creation of a minority segregated phase, BaOx-CuOx, in the highest copper content catalyst (BFC4), (iv) the rise in the quantity of oxygen vacancies/defects for the catalysts BFC3 and BFC4, and (v) the reduction in the amount of O2 released in the course of the O2-TPD tests as the copper content increases. The BaFe1−xCuxO3 perovskites catalyze both the NO2-assisted diesel soot oxidation (500 ppm NO, 5% O2) and, to a lesser extent, the soot oxidation under fuel cuts GDI operation conditions (1% O2). BFC0 is the most active catalysts as the activity seems to be mainly related with the amount of O2 evolved during an. O2-TPD, which decreases with copper content.


Introduction
The high toxicity of particulate matter (PM) or soot, mainly produced by internal combustion engines, is well established. As in Europe the transport sector generates a 14% of PM2.5 (particulates with a size lesser than 2.5 m, the most hazardous portion), the actual European emissions legislation (Euro 6c) for new passengers vehicles meet or decreases the Particulates Numbers (PN) generated by Gasoline Direct Injection (GDI) to the level corresponding to Diesel engines [1]. GDI engines are considered more effective than diesel engines due to the substantial decrease of fuel intake and CO 2 emissions [2]. Consequently, a growth in the US and European market of GDI cars is being observed. To attend the actual European emission legislation, the use of Gasoline Particulate Filter (GPF) is necessary for GDI vehicles, as the Diesel Particulate Filter (DPF) was for Diesel vehicles. In both filters, periodic regeneration is demanded to avoid soot accumulation in the channels of the filter [3][4][5].
In Diesel engine, as NO 2 promotes soot oxidation, a catalyst able to oxidize NO to NO 2 is incorporated into the DPF to carry out the NO 2 -assisted soot oxidation. In fact, several systems (most of them containing Platinum Group Metals, PGM) were developed and implemented in diesel cars to oxidize soot. However, recently, the EU [6] has highlighted that the use of critical raw materials (such as PGM) must be optimized.
Based on the success of DPF in diesel engines, GPF is proposed as a solution for GDI engines. The operating requirements of GPF differ largely from those of the DPF, as NO 2 is not present and a very low amount of O 2 is available in the GDI exhaust downstream the TWC [7][8][9]. Thus, active catalysts to oxidize soot in poor (or even null) oxygen conditions must be developed. However, even though it is a challenging issue, the soot oxidation reaction in the severe GDI exhaust requirements (i.e., <10,000 ppm of O 2 ) has been scarcely studied [8][9][10].
Considering this background, and taking into account the promising performance previously featured by a BaFe 1−x Cu x O 3 catalysts series for soot oxidation in the most severe GDI exhaust requirements (regular stoichiometric GDI operation, i.e., 0% O 2 ) [35], the objective of this research is to further study the influence of the partial replacement of iron by copper in the properties of a BaFeO 3 perovskite which will define its catalytic performance for soot oxidation. Therefore, BaFe 1−x Cu x O 3 catalysts (x = 0, 0.1, 0.3 and 0.4) were synthetized, characterized and tested for soot oxidation in both diesel and "fuel cuts" GDI exhaust conditions (i.e., 1% O 2 ).

Catalyst Preparation
BaFe 1−x Cu x O 3 catalysts (x = 0, 0.1, 0.3, 0.4) have been obtained using a citrate sol-gel method [26]. Ba(CH 3 COOH) 2 (Sigma-Aldrich, 99%), Fe(NO 3 ) 2 ·9H 2 O (Sigma-Aldrich, 97%) and Cu(NO 3 ) 2 ·3H 2 O (Panreac, 99%) have been employed as metal precursors. Briefly, a 1M citric acid solution, with a 1:2 molar ratio with respect to barium has been heated to 60 • C. The solution pH has been raised to 8.5 with ammonia solution. Subsequently, the corresponding amounts of barium, iron, and copper precursors have been incorporated, and the pH value has been readjusted to 8.5 with ammonia solution. The solution was hold at 65 • C during 5 h and later dried at 90 • C for 48 h. The dried gel has been calcined at 150 • C for 1 h and then, at 850 • C 6 h [26]. Table 1 includes the catalysts nomenclature.

Characterization
To measure the metal content in the samples by Inductively Coupled Plasma Atomic Emission Spectroscopy (ICP-OES), a Perkin-Elmer equipment (Optima 4300 DV) has been used. For the analysis, copper was extracted dissolving the samples with magnetic stirring in 8M HCl solution by reflux heating.
An Autosorb-6B instrument (Quantachrome Instruments, Boynton Beach, FL, USA) was used to determine, by N 2 adsorption at −196 • C, the Brunauer Emmet Teller (BET) surface area of the samples, which were previously degasified at 250 • C for 4 h.
X-ray diffraction (XRD) tests were performed between 20-80 • 2θ angles with a step rate of 1.5 • /2 min and using CuKα (0.15418 nm) radiation in a Bruker D8-Advance device. The Rietveld analysis of XRD data was developed with the Automatic Rietveld Refinement (HIGHScore Plus from PANalytical program).
A ZEISS Merlin VP Compact Field Emission Scanning Electron Microscopy (FESEM) equipment (Quantax 400 from Bruker, Berlin, Germany) was employed to analyze the morphology of the catalysts and to determine the elemental composition of the catalysts (by Energy Dispersive X-Ray analysis, EDX).
X-Ray Photoelectron Spectroscopy (XPS) was used to obtain the surface composition. To register the XPS spectra, a K-Alpha photoelectron spectrometer by Thermo-Scientific, with an Al Kα (1486.6 eV) radiation source, was used in the following conditions: 5 × 10 −10 mbar pressure in the chamber and setting the C1s transition at 284.6 eV. The binding energy (BE) and kinetic energy (KE) values were then determined with the peak-fit software of the spectrophotometer, to regulate the BE and KE scales.
Reducibility of the catalysts was evaluated by Temperature Programmed Reduction with H 2 (H 2 -TPR). The experiments were developed in a Pulse Chemisorb 2705 device from Micromeritics fitted with a Thermal Conductivity Detector (TCD to find out the outlet gas composition changes. 20 mg of the sample was heated at 10 • C/min from room temperature to 1000 • C in 5% H 2 /Ar atmosphere (40 mL/min, P t = 1 atm). The H 2 consumption amount was determined using a CuO sample supplied by Micromeritics.

Activity Tests
The catalytic activity for NO to NO 2 oxidation and NO 2 -assisted diesel soot oxidation was established by Temperature Programmed Reaction (NOx-TPR) using of a gas mixture composed of 500 ppm NOx and 5% O 2 , balanced with N 2 (500 mL/min gas flow). For NO oxidation experiments, 80 mg of the catalyst were mixed with SiC, in a 1:4 mass ratio, and warmed from 25 to 800 • C, at 10 • C/min, in a quartz fixed-bed reactor. The activity for diesel soot oxidation was evaluated adding 20 mg of Printex U from Degussa (employed as surrogated soot, which represents the least reactive fraction of particulate matter [8][9][10]16,26,[34][35][36][37][38]), in loose contact with the catalyst. For the catalyst with the highest activity, isothermal soot oxidation reactions at 450 • C were also performed. The gas composition was monitored by specific Non-dispersive Infrared Ultraviolet NDIR-UV gas analyzers for NO, NO 2 , CO, CO 2 , and O 2 (Rosemount Analytical Model BINOS 1001, 1004 and 100). The NO 2 generation, soot conversion and CO 2 selectivity percentages were calculated using Equations (1), (2), and (3), respectively: where NO 2,out and NO x , out are the NO 2 and NOx concentrations determined at the reactor exit, t 0 CO 2 + CO is the quantity of CO 2 and CO evolved at a time t, and and (CO 2 + CO) total are the CO and CO 2 + CO evolved during all the experiment time.
To determine the catalysts performance for soot oxidation in GDI exhaust conditions, a gas mixture with 1% O 2 in He was used as it is the typical O 2 concentration at the turbine-GDI engine exit, i.e., upstream the TWC [8], but also because it simulates the fuel cut GDI operation conditions (<20% O 2 ) [7]. These experiments were developed as Temperature Programmed Reactions (6 • C/min from Nanomaterials 2019, 9, 1551 4 of 22 150 • C temperature till 900 • C, 500 mL/min gas flow) in a quartz fixed-bed reactor using 80 mg of the catalysts and 20 mg of Printex-U (1:4 soot/catalyst ratio in loose contact) mixed with SiC. A Gas Chromatograph (Hewlet Packard 8690) with two packed columns (Porapak Q and Molecular Sieve 5a) connected to a Thermal Conductivity Detector (TCD) was used for the measure of the gas composition. Previous to the soot oxidation reaction, the catalysts were preheated in the reaction mixture (1% O 2 in He) at 150 • C during 1 hour. The soot conversion and CO 2 selectivity percentages were calculated using Equations (2) and (3), respectively.

Characterization of the Fresh Catalysts
3.1.1. Chemical, Morphological, and Structural Properties Table 1 features the real copper content and BET surface area of the BaFe 1−x Cu x O 3 (x = 0, 0.1, 0.3, 0.4) perovskites obtained by ICP-OES and N 2 adsorption, respectively. All the BaFe 1−x Cu x O 3 catalysts present a very low surface area, as it corresponds to mixed oxides with perovskite structure [19]. The data of the real copper content (very close to the nominal corresponding to the stoichiometric formula) reveal that nearly all the copper used in the synthesis appears in the catalysts. Concerning morphology, FESEM images ( Figure S1 in Supplementary Information) show that catalysts are formed by highly agglomerated irregular grains with a size in the range of micrometer. The presence of a low amount of copper (BFC1 and BFC3) does not significantly change the morphology of the bare perovskite; however, for the catalyst with highest copper content (BFC4), a different type of grains is detected which could correspond to a new phase. The EDX data (see Table S1 in Supplementary Information) reveal an identical atomic percentage of Ba and Fe for BFC0, as expected according to perovskite composition (BaFeO 3 ). However, for BFC4, in addition to the presence of Cu, larger atomic percentages of Ba and O are detected. This fact supports the existence of a new phase composed by barium, oxygen, and copper in the surface of this catalyst. Figure 1 features the XRD profiles, showing (as expected according to the calculated t values shown in Table 1) a perovskite structure as an almost unique crystalline phase for all catalysts. Additionally, a Fe(III) and Fe(IV) mixed-oxide with triclinic structure is identified as a minority phase for BFC0 and BFC1, while, for BFC4, a BaO x -CuO x phase (with a suggested stoichiometry of BaCuO 2 ) appears. This oxide could correspond to the different type of grains observed by FESEM for BFC4 catalyst (Figure S1d in Supplementary Information) and justifies the EDX data (Table S1 in Supplementary Information) for this catalyst.  Table 1 features the real copper content and BET surface area of the BaFe1-xCuxO3 (x = 0, 0.1, 0.3, 0.4) perovskites obtained by ICP-OES and N2 adsorption, respectively. All the BaFe1-xCuxO3 catalysts present a very low surface area, as it corresponds to mixed oxides with perovskite structure [19]. The data of the real copper content (very close to the nominal corresponding to the stoichiometric formula) reveal that nearly all the copper used in the synthesis appears in the catalysts. Concerning morphology, FESEM images ( Figure S1 in Supplementary Information) show that catalysts are formed by highly agglomerated irregular grains with a size in the range of micrometer. The presence of a low amount of copper (BFC1 and BFC3) does not significantly change the morphology of the bare perovskite; however, for the catalyst with highest copper content (BFC4), a different type of grains is detected which could correspond to a new phase. The EDX data (see Table S1 in Supplementary Information) reveal an identical atomic percentage of Ba and Fe for BFC0, as expected according to perovskite composition (BaFeO3). However, for BFC4, in addition to the presence of Cu, larger atomic percentages of Ba and O are detected. This fact supports the existence of a new phase composed by barium, oxygen, and copper in the surface of this catalyst. * In the range of experimental detection limit. ** Calculated as: = √ ((( ) ) ) Figure 1 features the XRD profiles, showing (as expected according to the calculated t values shown in Table 1) a perovskite structure as an almost unique crystalline phase for all catalysts. Additionally, a Fe(III) and Fe(IV) mixed-oxide with triclinic structure is identified as a minority phase for BFC0 and BFC1, while, for BFC4, a BaOx-CuOx phase (with a suggested stoichiometry of BaCuO2) appears. This oxide could correspond to the different type of grains observed by FESEM for BFC4 catalyst (Figure S1d in Supplementary Information) and justifies the EDX data (Table S1 in Supplementary Information) for this catalyst.  For BFC0 and BFC1 catalysts, the diffraction peaks are assigned to a hexagonal perovskite structure; however, for BFC3 and BFC4, the peaks are consistent with a cubic structure. These results agree with the decrease in the t parameter values (Table 1), which becoming closer to 1 (corresponding to an ideal cubic structure) as the copper content increases. This structural modification (which has been verified by the Rietveld analysis presented in Figure 2 was previously noticed for other barium-based perovskites [26,34,38] and also for Sn-doped BaFeO 3 perovskites [39], and supports that Cu has been introduced into the perovskite lattice. Concerning BFC1, the reduction in the intensity of the main perovskite peak (at. 31.5 • ) evidences that copper has been inserted into the perovskite structure [26,34,38]. Moreover, except for the catalyst with a highest copper content (BFC4), peaks corresponding to a copper segregated phase are not clearly identified, revealing that copper species are not segregated or, if they are, they would present a size under the detection limit of XRD. Finally, for BFC4, the presence of the BaO x -CuO x phase as minority segregated phase shows a limit in the amount of copper introduced into the perovskite framework [26,34,35,38]. For BFC0 and BFC1 catalysts, the diffraction peaks are assigned to a hexagonal perovskite structure; however, for BFC3 and BFC4, the peaks are consistent with a cubic structure. These results agree with the decrease in the t parameter values (Table 1), which becoming closer to 1 (corresponding to an ideal cubic structure) as the copper content increases. This structural modification (which has been verified by the Rietveld analysis presented in Figure 2 was previously noticed for other barium-based perovskites [26,34,38] and also for Sn-doped BaFeO3 perovskites [39], and supports that Cu has been introduced into the perovskite lattice. Concerning BFC1, the reduction in the intensity of the main perovskite peak (at. 31.5°) evidences that copper has been inserted into the perovskite structure [26,34,38]. Moreover, except for the catalyst with a highest copper content (BFC4), peaks corresponding to a copper segregated phase are not clearly identified, revealing that copper species are not segregated or, if they are, they would present a size under the detection limit of XRD. Finally, for BFC4, the presence of the BaOx-CuOx phase as minority segregated phase shows a limit in the amount of copper introduced into the perovskite framework [26,34,35,38].  Rietveld analysis for (minority phase not included in the analysis): a) BFC0: in red the original XRD pattern, in blue the Rietveld simulation corresponding to hexagonal perovskite structure and in green the residual data corresponding to triclinic structure; b) BFC1: in red the original XRD pattern, in blue the Rietveld simulation corresponding to hexagonal perovskite structure and in green the residual data corresponding to triclinic structure; c) BFC3: in red the original XRD pattern, in blue the Rietveld simulation corresponding to cubic perovskite structure and in green the residual data corresponding to BaCuO2; d) BFC4: in red the original XRD pattern, in blue the Rietveld simulation corresponding to cubic perovskite structure and in green the residual data corresponding to BaCuO2.
The average crystal size for the catalyst has been determined from the Full Width at Half Maximum (FWHM) of the main perovskite XRD peak (in hexagonal or cubic structure) applying the Scherrer equation [40]; data are included in Table 2. The average crystal size is smaller for the catalyst containing copper with hexagonal structure (BFC1) than for the bare perovskite (BFC0). On the contrary, for catalysts with cubic structure (BFC3 and BFC4), the average crystal size increases with the copper content. The lattice parameter for hexagonal (a and c) and cubic (a) perovskites have also been estimated from XRD data ( Table 2). As the average crystal size, the decrease in a and c values is observed in the presence of copper for the catalyst with hexagonal structure (BFC1), Rietveld analysis for (minority phase not included in the analysis): (a) BFC0: in red the original XRD pattern, in blue the Rietveld simulation corresponding to hexagonal perovskite structure and in green the residual data corresponding to triclinic structure; (b) BFC1: in red the original XRD pattern, in blue the Rietveld simulation corresponding to hexagonal perovskite structure and in green the residual data corresponding to triclinic structure; (c) BFC3: in red the original XRD pattern, in blue the Rietveld simulation corresponding to cubic perovskite structure and in green the residual data corresponding to BaCuO 2 ; (d) BFC4: in red the original XRD pattern, in blue the Rietveld simulation corresponding to cubic perovskite structure and in green the residual data corresponding to BaCuO 2 .
The average crystal size for the catalyst has been determined from the Full Width at Half Maximum (FWHM) of the main perovskite XRD peak (in hexagonal or cubic structure) applying the Scherrer equation [40]; data are included in Table 2. The average crystal size is smaller for the catalyst containing copper with hexagonal structure (BFC1) than for the bare perovskite (BFC0). On the contrary, for catalysts with cubic structure (BFC3 and BFC4), the average crystal size increases with the copper content. The lattice parameter for hexagonal (a and c) and cubic (a) perovskites have also been estimated from XRD data ( Table 2). As the average crystal size, the decrease in a and c values is observed in the presence of copper for the catalyst with hexagonal structure (BFC1), confirming that copper has been inserted into the lattice. However, as the ionic radii of copper (as Cu 2+ , 0.73 Å) is larger than the Fe 3+ ionic radii (0.65 Å) or Fe 4+ (0.59 Å), an increase in the lattice parameters would be expected if this was the unique factor affecting the values. Nevertheless, it has been reported that a modification in the amount of the oxygen vacancies affects the lattice parameter [41], thus, it seems that the amount of oxygen vacancies is also being affected by copper incorporation into the BaFeO 3 perovskite framework. For cubic perovskites (BFC3 and BFC4), the lattice parameter is almost constant but larger than the corresponding to a reference BaFeO 3 with cubic structure (4.012 Å) [39], again supporting that copper has been inserted into the lattice. Summarizing, from XRD data, it can be concluded that copper is inserted into the perovskite structure causing: (i) the distortion of the original hexagonal perovskite structure for the catalyst with the lowest copper content (BFC1), (ii) the modification from hexagonal to cubic structure for the catalysts with high copper content (BFC3 and BFC4), (iii) the formation of a BaOx-CuOx oxide as minority segregated phase for BFC4 catalyst, and iv) a possible increase in the amount of oxygen vacancies/defects.

Surface Properties
XPS analysis provides data about the surface composition of the BaFe 1−x Cu x O 3 perovskite catalysts. The XPS profiles corresponding to the Cu 2p 3/2 transition are presented in Figure 3. Reduced copper species, such as metallic copper or Cu 2 O, usually appear at a binding energy (BE) close to 933 eV, while, for Cu(II) species, the Cu 2p 3/2 transition appears above 933 eV [36,[42][43][44]. In Figure 3, the BE maximum of the main XPS band appears slightly above 933 eV in the three catalysts containing copper, suggesting the presence of Cu(II) species. Moreover, Cu(I) and Cu(II) species can be distinguished by the presence of a satellite peak at 942-945 eV, due to an electron transfer from Cu 2p 3/2 to 3d free level in Cu(II) [45]. The existence of the satellite peak for the three copper-content catalysts, that reveals the presence of Cu(II) species [45], confirms that copper is present as Cu(II) species. Additionally, based on the use of Auger data (Cu LMM) [45], the existence of Cu(II) species has been verified as reveals the Wagner (chemical state) plot shown in Figure S2 (Supplementary information). The deconvolution of the normalized Cu 2p 3/2 bands reveals two contributions with maxima at around 933 eV and 935 eV, which seem to correspond to two different Cu(II) species [42][43][44]: (i) the band at lower BE, assignable to copper species with a weak electronic interaction with perovskite, that is, to CuO species located on the surface (Cu S ) and (ii) the band at higher BE, corresponding to copper species with a strong electronic interaction with perovskite (Cu L ), i.e., copper inserted in the lattice, near the surface. As the percentage of the area for the XPS band at 935 eV (Cu L band) increases with the copper content from 26% to 33%, it seems that the presence of copper with a strong electronic interaction with perovskite is favored as copper content increases. However, a slight decrease of this value is observed for the BFC4 catalyst with respect to BFC3 (33% versus 35%), confirming that a limit for the copper insertion has been achieved. In fact, a comparison between the Cu/Cu+Fe+Ba ratio calculated by XPS and the corresponding nominal ratio (both data included in Table 3) confirms that copper has been inserted into the perovskite structure, as the XPS ratio are lower (for BFC1 and BFC3) or similar than (for BCF4) the nominal ratio [25,[34][35][36][37][38]. It is remarkable that the smallest difference between these two values is presented by BFC4 catalyst, supporting, again, the limit in the copper insertion. Therefore, the copper which is not introduced into the lattice has to be dispersed on the surface forming the BaOx-CuOx phase, which was detected by XRD and EDX, as copper content is higher for BFC4 (Table 1). Nanomaterials 2019, 9,1551 8 of 22 into the lattice has to be dispersed on the surface forming the BaOx-CuOx phase, which was detected by XRD and EDX, as copper content is higher for BFC4 (Table 1).   Figure 4 features the XPS spectra of the Fe 2p3/2 for BaFe1-xCuxO3 catalysts and the corresponding to a Fe2O3 commercial sample use as reference. The maximum of the main XPS band for the four catalysts does not appear at exactly the same (BE) value than the corresponding to the reference suggesting the presence of Fe species with a different oxidation state or with the same oxidation state but in different proportion. The deconvolution of the main band shows two significant contributions at around 709 eV and 711 eV. Even though the identification of iron oxidation states by XPS is very difficult [46], according to literature [39,[46][47][48][49][50], the first peak corresponds to Fe(III) species, and the second one could be assigned to Fe(IV) species [48][49][50]. It has been established that the position of the satellite peak is the key finger to detect the oxidation state of Fe [46,48]. Thus, the shake-up peak observed at 717 eV (which corresponds to the satellite peak of Fe(III)) supports the existence of this oxidation state [39,46,48,51]. However, the presence of Fe(IV) seems not to be supported by the XPS data, as the high BE peak at approximately 711 eV is not always unequivocally assigned to this oxidation state [46,48]. Thus, more evidence from other characterization techniques is needed to assume that Fe(IV) exits. The TPR-H2 results (see below) indicate that Fe(IV) and Fe(III) oxidation states co-exist in the BaFe1-xCuxO3 catalysts, as it is observed that the experimental H2 consumption is in between the nominal (calculated) H2 consumption expected, considering that iron as Fe(III) or Fe(IV) is reduced to Fe(II). The presence of Fe(IV) in BaFe1-xCuxO3 catalysts is   Figure 4 features the XPS spectra of the Fe 2p 3/2 for BaFe 1−x Cu x O 3 catalysts and the corresponding to a Fe 2 O 3 commercial sample use as reference. The maximum of the main XPS band for the four catalysts does not appear at exactly the same (BE) value than the corresponding to the reference suggesting the presence of Fe species with a different oxidation state or with the same oxidation state but in different proportion. The deconvolution of the main band shows two significant contributions at around 709 eV and 711 eV. Even though the identification of iron oxidation states by XPS is very difficult [46], according to literature [39,[46][47][48][49][50], the first peak corresponds to Fe(III) species, and the second one could be assigned to Fe(IV) species [48][49][50]. It has been established that the position of the satellite peak is the key finger to detect the oxidation state of Fe [46,48]. Thus, the shake-up peak observed at 717 eV (which corresponds to the satellite peak of Fe(III)) supports the existence of this oxidation state [39,46,48,51]. However, the presence of Fe(IV) seems not to be supported by the XPS data, as the high BE peak at approximately 711 eV is not always unequivocally assigned to this oxidation state [46,48]. Thus, more evidence from other characterization techniques is needed to assume that Fe(IV) exits. The TPR-H 2 results (see below) indicate that Fe(IV) and Fe(III) oxidation states co-exist in the BaFe 1−x Cu x O 3 catalysts, as it is observed that the experimental H 2 consumption is in between the nominal (calculated) H 2 consumption expected, considering that iron as Fe(III) or Fe(IV) is reduced to Fe(II). The presence of Fe(IV) in BaFe 1−x Cu x O 3 catalysts is additionally supported by the well-known stabilization of high oxidation state for B cation, as Fe(IV), in perovskites [19,39,[48][49][50]. On the basis of the BaFeO 3 stoichiometric formula, Fe(IV) must be the oxidation state for Fe in the perovskite, and, in the presence of copper, a rise in the Fe(IV) amount and /or the generation of additional oxygen vacancies into the perovskite structure would be expected to compensate the deficiency of positive charge due to the partial iron substitution [19]. In fact, the decrease in the lattice parameter observed by XRD for BFC1 with respect to BFC0 (Table 2) suggests an increase in the Fe(IV), which presents a lower ionic ratio that Fe(III). However, for BFC2 and BFC3, the lattice parameter ( Table 2) increases revealing that the amount of Fe(IV) cannot be higher; thus, the generation of additional oxygen vacancies should be observed to balance the positive charge deficiency due to the increase of the copper content in the catalyst. This larger amount of oxygen vacancies has to cause the lattice expansion detected [41]. additionally supported by the well-known stabilization of high oxidation state for B cation, as Fe(IV), in perovskites [19,39,[48][49][50]. On the basis of the BaFeO3 stoichiometric formula, Fe(IV) must be the oxidation state for Fe in the perovskite, and, in the presence of copper, a rise in the Fe(IV) amount and /or the generation of additional oxygen vacancies into the perovskite structure would be expected to compensate the deficiency of positive charge due to the partial iron substitution [19].
In fact, the decrease in the lattice parameter observed by XRD for BFC1 with respect to BFC0 ( Table  2) suggests an increase in the Fe(IV), which presents a lower ionic ratio that Fe(III). However, for BFC2 and BFC3, the lattice parameter ( Table 2) increases revealing that the amount of Fe(IV) cannot be higher; thus, the generation of additional oxygen vacancies should be observed to balance the positive charge deficiency due to the increase of the copper content in the catalyst. This larger amount of oxygen vacancies has to cause the lattice expansion detected [41].  Figure 5 presents the XPS spectra of the O1s transition for all catalysts, where three contributions are usually observed [36,[42][43][44] : i) at low BE (around 528 eV), corresponding to lattice oxygen (OL) in metal oxides, ii) at intermediate BE (between 529 and 531 eV), assigned to adsorbed oxygen species such as, O2 −2 , surface CO3 −2 , and/or OH − groups, and iii) at high BE (533 eV approximately) due to oxygen in adsorbed water [52][53][54][55]. The intensity of the bands is modified in the presence of copper revealing changes in the amount of oxygen species on the catalysts surface. The values of OL/Cu+Ti+Ba ratio in Table 3 (determined from the peak area of OL, Fe2p 3/2 , Ba3d 3/2 , and Cu2p 3/2 transitions) is higher for BFC1 than for the bare BFC0 perovskite, which means a lower amount of surface oxygen vacancies. This fact supports that the oxidation of Fe(III) to Fe(IV) occurs in the BFC1 perovskite to compensate the positive charge deficiency due to copper incorporation. However, for BFC3 and BFC4 catalysts, the lower OL/Cu+Ti+Ba ratio with respect to the nominal value confirms the generation of additional oxygen vacancies to balance the positive charge   Table 3 (determined from the peak area of O L , Fe2p 3/2 , Ba3d 3/2 , and Cu2p 3/2 transitions) is higher for BFC1 than for the bare BFC0 perovskite, which means a lower amount of surface oxygen vacancies. This fact supports that the oxidation of Fe(III) to Fe(IV) occurs in the BFC1 perovskite to compensate the positive charge deficiency due to copper incorporation. However, for BFC3 and BFC4 catalysts, the lower O L /Cu+Ti+Ba ratio with respect to the nominal value confirms the generation of additional oxygen vacancies to balance the positive charge deficiency due to partial iron substitution by copper. Additionally, these results justify the change in the values of lattice parameters observed, that is: (i) the lower lattice parameters values for BFC1 catalyst with respect to BFC0 (Table 2) are due to the decrease in the amount of oxygen vacancies (Table 3), as, for this catalysts, the oxidation of Fe(III) to Fe(IV) takes place and (ii) the larger values for BFC3 and BFC4 (Table 2) are due to the rise in the amount of oxygen vacancies with respect to BFC0 (Table 3).
Nanomaterials 2019, 9, 1551 10 of 22 deficiency due to partial iron substitution by copper. Additionally, these results justify the change in the values of lattice parameters observed, that is: i) the lower lattice parameters values for BFC1 catalyst with respect to BFC0 (Table 2) are due to the decrease in the amount of oxygen vacancies (Table 3), as, for this catalysts, the oxidation of Fe(III) to Fe(IV) takes place and ii) the larger values for BFC3 and BFC4 (Table 2) are due to the rise in the amount of oxygen vacancies with respect to BFC0 (Table 3).

Redox Properties
Reducibility and redox properties of the fresh BaFe1-xCuxO3 catalysts were analyzed by Temperature Programmed Reduction with H2 (H2-TPR), which are the H2 consumption profiles shown in Figure 6. In Figure 7, the nominal (calculated) H2 consumption (mL of H2 per gram of catalysts) expected considering that iron, as Fe(III) or Fe(IV) in the perovskite, is reduced to Fe(II), is compared with the experimental H2 consumption determined from the H2-TPR profiles ( Figure 6). It is observed that the experimental H2 consumption is in between both nominal values revealing that Fe(IV) and Fe(III) oxidation states co-exist in the BaFe1-xCuxO3 catalysts. Furthermore, the experimental H2 consumption data indicates that the amount of Fe(IV) increases in the presence of copper.
In the complex H2 consumption profiles shown in Figure 6, three regions can be established [56][57][58]: a) At low temperature, between approximately 200 °C and 550 °C, a broad H2 consumption signal is observed for all the catalyst that, according to literature, can be ascribed to different reduction processes: i) the Cu(II) [34,38] reduction, ii) the Fe(IV) and Fe(III) reduction to Fe(III) and Fe(II), as was observed for Fe3O4, and iii) the reduction of weakly chemisorbed oxygen upon surface oxygen vacancies of perovskite (α-oxygen) [34].

Redox Properties
Reducibility and redox properties of the fresh BaFe 1−x Cu x O 3 catalysts were analyzed by Temperature Programmed Reduction with H 2 (H 2 -TPR), which are the H 2 consumption profiles shown in Figure 6. In Figure 7, the nominal (calculated) H 2 consumption (mL of H 2 per gram of catalysts) expected considering that iron, as Fe(III) or Fe(IV) in the perovskite, is reduced to Fe(II), is compared with the experimental H 2 consumption determined from the H 2 -TPR profiles ( Figure 6). It is observed that the experimental H 2 consumption is in between both nominal values revealing that Fe(IV) and Fe(III) oxidation states co-exist in the BaFe 1−x Cu x O 3 catalysts. Furthermore, the experimental H 2 consumption data indicates that the amount of Fe(IV) increases in the presence of copper.
In the complex H 2 consumption profiles shown in Figure 6, three regions can be established [56][57][58]: a) At low temperature, between approximately 200 • C and 550 • C, a broad H 2 consumption signal is observed for all the catalyst that, according to literature, can be ascribed to different reduction processes: (i) the Cu(II) [34,38] reduction, (ii) the Fe(IV) and Fe(III) reduction to Fe(III) and Fe(II), as was observed for Fe 3 O 4 , and iii) the reduction of weakly chemisorbed oxygen upon surface oxygen vacancies of perovskite (α-oxygen) [34]. b) From around 550 • C to 700 • C, the H 2 consumption peaks correspond to both the reduction of Fe(III) to Fe(II) as detected for the reduction of Fe 3 O 4 to FeO and to the decomposition of surface oxygen species formed on oxygen vacancies (called α'-oxygen) [34], more strongly bonded to the perovskite than α-oxygen.

c)
At high temperatures (T > 700 • C), broad TCD signals assigned to the reduction of Fe(II) to Fe(0) (causing the consequent destruction of the perovskite structure) could be found [56][57][58]. Nevertheless, the XRD data for catalysts after H 2 -TPR (not shown) reveal that the perovskite structure is still present, thus, the reduction to Fe(0) is not taking place and, consequently, H 2 consumption is hardly observed at T > 700 • C. Therefore, the most relevant information related to the redox properties of the BaFe 1−x Cu x O 3 catalysts is located at T < 700 • C.
BFC0 profile shows two peaks at temperature lower than 700 • C: a broad peak with maximum at ca 300 • C and a more defined peak with a maximum at around 670 • C. The H 2 consumption detected at temperature lower than 300 • C is usually related to the presence of Fe(IV) [56][57][58], supporting the existence of this oxidation state. The second H 2 consumption peak, with a maximum at 670 • C, corresponds to the reduction of Fe(III) to Fe(II) and to desorption/reduction of oxygen surface species formed on oxygen vacancies (α'-oxygen) [34]. b) From around 550 °C to 700 °C, the H2 consumption peaks correspond to both the reduction of Fe(III) to Fe(II) as detected for the reduction of Fe3O4 to FeO and to the decomposition of surface oxygen species formed on oxygen vacancies (called α'-oxygen) [34], more strongly bonded to the perovskite than α-oxygen.

c) At high temperatures (T > 700 °C), broad TCD signals assigned to the reduction of Fe(II) to Fe(0)
(causing the consequent destruction of the perovskite structure) could be found [56][57][58].
Nevertheless, the XRD data for catalysts after H2-TPR (not shown) reveal that the perovskite structure is still present, thus, the reduction to Fe(0) is not taking place and, consequently, H2 consumption is hardly observed at T > 700 °C. Therefore, the most relevant information related to the redox properties of the BaFe1-xCuxO3 catalysts is located at T < 700 °C.
BFC0 profile shows two peaks at temperature lower than 700 °C: a broad peak with maximum at ca 300 °C and a more defined peak with a maximum at around 670 °C. The H2 consumption detected at temperature lower than 300 °C is usually related to the presence of Fe(IV) [56][57][58], supporting the existence of this oxidation state. The second H2 consumption peak, with a maximum at 670 °C, corresponds to the reduction of Fe(III) to Fe(II) and to desorption/reduction of oxygen surface species formed on oxygen vacancies (α'-oxygen) [34].   b) From around 550 °C to 700 °C, the H2 consumption peaks correspond to both the reduction of Fe(III) to Fe(II) as detected for the reduction of Fe3O4 to FeO and to the decomposition of surface oxygen species formed on oxygen vacancies (called α'-oxygen) [34], more strongly bonded to the perovskite than α-oxygen. c) At high temperatures (T > 700 °C), broad TCD signals assigned to the reduction of Fe(II) to Fe(0) (causing the consequent destruction of the perovskite structure) could be found [56][57][58].
Nevertheless, the XRD data for catalysts after H2-TPR (not shown) reveal that the perovskite structure is still present, thus, the reduction to Fe(0) is not taking place and, consequently, H2 consumption is hardly observed at T > 700 °C. Therefore, the most relevant information related to the redox properties of the BaFe1-xCuxO3 catalysts is located at T < 700 °C.
BFC0 profile shows two peaks at temperature lower than 700 °C: a broad peak with maximum at ca 300 °C and a more defined peak with a maximum at around 670 °C. The H2 consumption detected at temperature lower than 300 °C is usually related to the presence of Fe(IV) [56][57][58], supporting the existence of this oxidation state. The second H2 consumption peak, with a maximum at 670 °C, corresponds to the reduction of Fe(III) to Fe(II) and to desorption/reduction of oxygen surface species formed on oxygen vacancies (α'-oxygen) [34].   In the H 2 consumption profile of BFC1 catalyst, a broad peak with two maxima, at approximately 350 • C and 450 • C, is identified. The first maximum is ascribed to the Cu(II) to Cu(0) reduction (appearing at lower temperature than the CuO used as a reference [38]) and also to the consumption due to the partial Fe(IV) and Fe(III) reduction to Fe(III) and Fe(II), respectively. The second maximum of this broad peak at 450 • C seems to correspond to: i) the reduction of Fe(III) to Fe(II), taking place at lower temperature than for the BaFeO 3 catalyst, due to the presence of reduced copper [26] and ii) the desorption/reduction of strongly bonded oxygen species ('-oxygen) [34].
In the H 2 -TPR profile of the BFC3 catalyst, a broad peak between 300 and 500 • C is detected with a well-defined maximum at 320 • C, followed by a shoulder around 380 • C. The first maximum corresponds to the reduction of Cu(II) to Cu(0) and it is better defined than the corresponding to BFC1 due to the higher copper content. As for BFC1, the low H 2 consumption at T < 300 • C confirms the presence of Fe(IV). The shoulder at 380 • C has to be related with the reduction of Fe(III) to Fe(II) that seems to take place at lower temperature than for BFC1. This fact supports that the formation of metallic copper (which is more easily reduced than iron) promotes the reduction of Fe(III) to Fe(II), as was previously observed for the reduction of manganese species in BaMn 1−x Cu x O 3 catalysts series [26].
Concerning BFC4, a sharp H 2 consumption peak with a maximum at 315 • C is found, followed by a low intensity peak with a maximum at around 475 • C. The presence of this well-defined peak, which is ascribed to Cu(II) to Cu(0) reduction, confirms the existence of copper oxide (II) species [34]. In fact, for this catalyst, BaO x -CuO x oxide has been detected by XRD and FESEM, thus, the sharp peak corresponds to the reduction of this copper oxide. The second peak has to be due to the Fe(III) reduction to Fe(II) that, for BFC1 and BFC3 catalysts, takes place at lower temperature that for BFC0.
After the analysis of the H 2 -TPR profiles for three catalysts, it can be concluded that the Fe(III) reduction to Fe(II) takes place at similar temperature for BFC1 and BFC4 (450 • C and 475 • C, respectively); this happens at lower a temperature (380 • C) for the BFC3 catalyst, probably due to its higher content of lattice copper (see Table 3).
Concluding, H 2 -TPR results indicate the co-existence of Fe(III) and Fe(IV) and suggest that copper incorporation promotes the reduction of Fe(III) to Fe(II).

O 2 Release During Heat-Treatment in He (O 2 -TPD)
In the O 2 profiles evolved by perovskite mixed oxides during a heat treatment in He (O 2 -TPD), three regions are usually observed [26,39,[59][60][61][62][63][64][65][66][67][68]. The lower temperature region, at T < 400 • C corresponds to weakly chemisorbed oxygen upon surface-oxygen vacancies (denoted as oxygen). The intermediate region, between 400 • C and 700 • C, is ascribed to near-surface oxygen associated to lattice defects such as dislocations and grains frontiers (designed as α' oxygen). Therefore, the presence of α and α'-oxygen is directly linked with the presence of surface vacancies/defects of oxygen in the structure [64][65][66]. Finally, the oxygen evolved at temperature higher than 700 • C, named β oxygen, is generally related with the lattice oxygen (which comes from the reduction of B cation (Fe in this case) of the perovskite [66]) and it is related with the oxygen mobility and with the inner bulk oxygen vacancies. Figure 8 shows the O 2 profiles for the BaFe 1−x Cu x O 3 catalysts. The O 2 -TPD profiles show that α and α'-oxygen are mainly evolved by most of the BaFe 1−x Cu x O 3 catalysts [8,9]. BFC0, BFC3, and BFC4 exhibit a higher oxygen signals than BFC1 and, therefore, higher quantity of surface oxygen vacancies, agreeing with the XPS results (lower O L /Cu+Ti+Ba ratio). Regarding α'-oxygen, BFC1 presents the highest signal, which evidences the great structure distortion (as exhibited by XRD) promoted by a small Cu incorporation. The total quantity of O 2 , calculated from the area under the O 2 profiles, diminishes as copper content grows: 424 µmol/g cat (BFC0) > 333 µmol/g cat (BFC1) > 282 µmol/g cat (BFC3) > 275 µmol/g cat (BFC4). Thus, as it has been previously published [39], the addition of a dopant seems to stabilize the oxygen bonded to Fe and leads to a decrease in the desorbed O 2 . For BFC4, a grown in the β oxygen has been detected, probably related to the structural modification and the presence of the BaOx-CuOx phase identified by XRD. The phase composition of BaFe1-xCuxO3 catalysts after the O2-TPD has been determined by XRD ( Figure S3 in Supplementary Information). For BFC0 and BFC1 catalysts, the hexagonal perovskite structure is replaced by a monoclinic BaFeO2.5 phase (with ordered oxygen vacancies) after losing a fraction of the lattice oxygen. On the contrary, BFC3 and BFC4 catalysts preserve the cubic perovskite structure after O2 release. This founding agrees with the conclusions of Huang et al. [39], who pointed out the increase in the structure stability due to the presence of a dopant (copper in our case). Note that the most stable catalysts (BFC3 and BFC4) are those with ideal (cubic) perovskite structure. The higher structural stability in the presence of copper could be relevant for catalytic applications at high temperature. Figure 9 shows the NO2 generation profiles obtained in TPR conditions for BaFe1-xCuxO3 catalysts including, as reference, the thermodynamic equilibrium profile. As observed for other perovskite-based catalysts [26,[34][35][36][37][38]64,67], the thermodynamic equilibrium limits the NO2 percentage at T > 500 °C. All catalysts accelerate the NO to NO2 oxidation at temperature lower than 500 °C, being the copper-free catalyst (BFC0) the most active. In general terms, the NO2 generation follows the same sequence than the amount of oxygen evolved during O2-TPD, except for BFC4 catalyst. Note that the two catalysts evolving large amount of and '   -oxygen, that is, BFC0 and BFC1, are also the catalysts generating more NO2 at low temperature (T < 300 °C). This is in agreement with the relationship found by Onrubia et al. [64] between the amount of and ' oxygen evolved by the catalysts (Sr-doped LaBO3 (B = Mn or Co perovskites) and the activity for the NO to NO2 oxidation. Note that BFC4 shows a slightly higher NO2 generation capacity than BFC3, which has to be related with the presence of copper species on the surface (BaOx-CuOx) that also catalyze the NO2 production [34]. The phase composition of BaFe 1−x Cu x O 3 catalysts after the O 2 -TPD has been determined by XRD ( Figure S3 in Supplementary Information). For BFC0 and BFC1 catalysts, the hexagonal perovskite structure is replaced by a monoclinic BaFeO 2.5 phase (with ordered oxygen vacancies) after losing a fraction of the lattice oxygen. On the contrary, BFC3 and BFC4 catalysts preserve the cubic perovskite structure after O 2 release. This founding agrees with the conclusions of Huang et al. [39], who pointed out the increase in the structure stability due to the presence of a dopant (copper in our case). Note that the most stable catalysts (BFC3 and BFC4) are those with ideal (cubic) perovskite structure. The higher structural stability in the presence of copper could be relevant for catalytic applications at high temperature. Figure 9 shows the NO 2 generation profiles obtained in TPR conditions for BaFe 1−x Cu x O 3 catalysts including, as reference, the thermodynamic equilibrium profile. As observed for other perovskite-based catalysts [26,[34][35][36][37][38]64,67], the thermodynamic equilibrium limits the NO 2 percentage at T > 500 • C. All catalysts accelerate the NO to NO 2 oxidation at temperature lower than 500 • C, being the copper-free catalyst (BFC0) the most active. In general terms, the NO 2 generation follows the same sequence than the amount of oxygen evolved during O 2 -TPD, except for BFC4 catalyst. Note that the two catalysts evolving large amount of and '-oxygen, that is, BFC0 and BFC1, are also the catalysts generating more NO 2 at low temperature (T < 300 • C). This is in agreement with the relationship found by Onrubia et al. [64] between the amount of and ' oxygen evolved by the catalysts (Sr-doped LaBO 3 (B = Mn or Co perovskites) and the activity for the NO to NO 2 oxidation. Note that BFC4 shows a slightly higher NO 2 generation capacity than BFC3, which has to be related with the presence of copper species on the surface (BaOx-CuOx) that also catalyze the NO 2 production [34]. To evaluate the activity of the catalysts for NO2-assisted diesel soot oxidation, Temperature Programmed Reactions in a NO/O2 atmosphere (see Experimental Section for details) were carried out, and the TPR-NOx soot conversion profiles (calculated based on the amount of CO and CO2 evolved) are featured in Figure 10. Relevant data, such as the ignition temperature (T5%), the temperature required to reach 50% of soot conversion (T50%), and the selectivity to CO2, are included in Table 4. It can be concluded that all the catalysts shift the soot conversion profiles to lower temperatures compared to the uncatalyzed reaction (blank corresponding to bare soot) and, consequently, the T5% and the T50% are lower. In agreement with the NO2 profiles (Figure 9), BFC0 is the most active catalyst for diesel soot oxidation as the addition of copper decreases the catalyst activity for soot conversion. Moreover, for BFC0 the T50% value is close to 500 °C, thus, this perovskite could be used as potential catalyst for the soot removal from diesel engine exhaust [69]. The decrease in the activity for soot oxidation after the addition of a dopant (copper in our catalysts) was also observed by Huang et al. [39] for Ag-doped LaFeO3 catalysts. These authors related the lower activity of Ag-perovskites for soot oxidation with the reduction in the amount of surface oxygen vacancies due to the anchorage of Ag nanoparticles. Furthermore, the reaction rate for methane combustion of a series of oxygen deficient SrFeO3 perovskites was related with the quantity of oxygen vacancies in the structure [58]. In fact, a relationship between soot oxidation performance and oxygen vacancies has been published [70]. Thus, in BaFe1-xCuxO3 catalysts, the decrease in the total amount of O2 evolved as copper content increases apparently leads to a decrease in the activity for both NO to NO2 and soot oxidation. Note that BFC4 does not match this trend as it shows the lowest T5% y T50% values among the catalysts containing copper (BFC1, BFC3, and BFC4). This catalyst presents the highest fraction of surface copper species, which also catalyzes the NO2/soot oxidation reaction [26,34,36], and hence, improves its catalytic performance. Therefore, the activity for NO2 generation and the amount of surface copper species seem to determine the catalytic performance. Thus, the highest NO2 generation capacity of BFC0 catalyst seems to justify its highest soot oxidation activity, while it is the largest fraction of surface copper species present in BFC4, which seems to justify its higher soot oxidation activity compared to BFC3.

NO 2 Generation and Diesel Soot Oxidation
Additionally, the data in Table 4 reveal that, as could be expected [26,34,36,37], all the catalysts show a higher CO2 selectivity than the uncatalyzed reaction (bare soot), with BFC4 being the most selective. Thus, CO2 selectivity increases with the amount of surface copper species (Table 3) as this metal is a well-known catalyst for CO to CO2 oxidation. To evaluate the activity of the catalysts for NO 2 -assisted diesel soot oxidation, Temperature Programmed Reactions in a NO/O 2 atmosphere (see Experimental Section for details) were carried out, and the TPR-NOx soot conversion profiles (calculated based on the amount of CO and CO 2 evolved) are featured in Figure 10. Relevant data, such as the ignition temperature (T 5% ), the temperature required to reach 50% of soot conversion (T 50% ), and the selectivity to CO 2 , are included in Table 4. It can be concluded that all the catalysts shift the soot conversion profiles to lower temperatures compared to the uncatalyzed reaction (blank corresponding to bare soot) and, consequently, the T 5% and the T 50% are lower. In agreement with the NO 2 profiles (Figure 9), BFC0 is the most active catalyst for diesel soot oxidation as the addition of copper decreases the catalyst activity for soot conversion. Moreover, for BFC0 the T 50% value is close to 500 • C, thus, this perovskite could be used as potential catalyst for the soot removal from diesel engine exhaust [69]. The decrease in the activity for soot oxidation after the addition of a dopant (copper in our catalysts) was also observed by Huang et al. [39] for Ag-doped LaFeO 3 catalysts. These authors related the lower activity of Ag-perovskites for soot oxidation with the reduction in the amount of surface oxygen vacancies due to the anchorage of Ag nanoparticles. Furthermore, the reaction rate for methane combustion of a series of oxygen deficient SrFeO 3 perovskites was related with the quantity of oxygen vacancies in the structure [58]. In fact, a relationship between soot oxidation performance and oxygen vacancies has been published [70]. Thus, in BaFe 1−x Cu x O 3 catalysts, the decrease in the total amount of O 2 evolved as copper content increases apparently leads to a decrease in the activity for both NO to NO 2 and soot oxidation. Note that BFC4 does not match this trend as it shows the lowest T 5% y T 50% values among the catalysts containing copper (BFC1, BFC3, and BFC4). This catalyst presents the highest fraction of surface copper species, which also catalyzes the NO 2 /soot oxidation reaction [26,34,36], and hence, improves its catalytic performance. Therefore, the activity for NO 2 generation and the amount of surface copper species seem to determine the catalytic performance. Thus, the highest NO 2 generation capacity of BFC0 catalyst seems to justify its highest soot oxidation activity, while it is the largest fraction of surface copper species present in BFC4, which seems to justify its higher soot oxidation activity compared to BFC3.  Due to its high activity, the performance of the BFC0 catalyst was deeply analyzed and five consecutives TPR-NOx soot oxidation cycles were carried out using the same portion of catalyst. As the T50% values for the first (543 °C) and fifth cycle (561 °C) are still under those corresponding to the uncatalyzed reaction (612 °C), it can be concluded that the catalyst is not significantly deactivated. In fact, the XRD data (shown in Figure S4 in Supplementary Information) of this used catalyst (after five TPR-NOx cycles) reveal that the hexagonal perovskite structure is not significantly modified. This means that, in the presence of oxygen in the reaction atmosphere, the catalyst keeps its structure and, consequently, its activity for soot oxidation in TPR conditions. Finally, to complete the BFC0 evaluation, its catalytic performance for NO2-assisted diesel soot oxidation in isothermal conditions was determined by carrying out two consecutive soot oxidation experiments at 450 °C. The soot oxidation profiles at 450 °C (featured in Figure S5 in Supplementary Information) show that BFC0 catalyst is able to oxide soot without a significant deactivation and showing a high CO2 selectivity (close to 80%). The soot oxidation rate was calculated at the beginning of the reaction, in order to avoid the effect of high soot consumption, as being 1.2 min −1 , which is not too far from a commercial model Pt/Al2O3 catalyst (1.8 min −1 ) used in the same experimental conditions. Thus, it seems that BaFeO3 perovskite could be a potential catalyst for diesel soot oxidation and, consequently, it could be used as an active phase for DPF.

Soot Oxidation in GDI Conditions
A preliminary study about the use of BaFe1-xCuxO3 perovskites to catalyze the oxidation reaction of soot under the highest demanding GDI exhaust requirements (regular stoichiometric GDI operation, i.e., 0% O2) revealed that these oxides could be used as active phase for GPF [35]. It  Additionally, the data in Table 4 reveal that, as could be expected [26,34,36,37], all the catalysts show a higher CO 2 selectivity than the uncatalyzed reaction (bare soot), with BFC4 being the most selective. Thus, CO 2 selectivity increases with the amount of surface copper species (Table 3) as this metal is a well-known catalyst for CO to CO 2 oxidation.
Due to its high activity, the performance of the BFC0 catalyst was deeply analyzed and five consecutives TPR-NOx soot oxidation cycles were carried out using the same portion of catalyst. As the T 50% values for the first (543 • C) and fifth cycle (561 • C) are still under those corresponding to the uncatalyzed reaction (612 • C), it can be concluded that the catalyst is not significantly deactivated. In fact, the XRD data (shown in Figure S4 in Supplementary Information) of this used catalyst (after five TPR-NOx cycles) reveal that the hexagonal perovskite structure is not significantly modified. This means that, in the presence of oxygen in the reaction atmosphere, the catalyst keeps its structure and, consequently, its activity for soot oxidation in TPR conditions. Finally, to complete the BFC0 evaluation, its catalytic performance for NO 2 -assisted diesel soot oxidation in isothermal conditions was determined by carrying out two consecutive soot oxidation experiments at 450 • C. The soot oxidation profiles at 450 • C (featured in Figure S5 in Supplementary Information) show that BFC0 catalyst is able to oxide soot without a significant deactivation and showing a high CO 2 selectivity (close to 80%). The soot oxidation rate was calculated at the beginning of the reaction, in order to avoid the effect of high soot consumption, as being 1.2 min −1 , which is not too far from a commercial model Pt/Al 2 O 3 catalyst (1.8 min −1 ) used in the same experimental conditions. Thus, it seems that BaFeO 3 perovskite could be a potential catalyst for diesel soot oxidation and, consequently, it could be used as an active phase for DPF.

Soot Oxidation in GDI Conditions
A preliminary study about the use of BaFe 1−x Cu x O 3 perovskites to catalyze the oxidation reaction of soot under the highest demanding GDI exhaust requirements (regular stoichiometric GDI operation, i.e., 0% O 2 ) revealed that these oxides could be used as active phase for GPF [35]. It was concluded that the copper content has an essential role on the performance of the BaFe 1−x Cu x O 3 catalysts for soot oxidation, agreeing with previous reports focused on diesel soot removal [10,26,34,[36][37][38] and with the report for copper-supported ceria-zirconia catalysts for soot oxidation in GDI conditions [10]. These results confirm that the higher soot conversion presented by BFC4 with respect to the catalysts with lower copper content (BFC1 and BFC3) is linked both to the largest amount of β oxygen evolved by this catalyst, and with the presence of surface copper species (as BaO x -CuO x ) [10,34,[36][37][38].
To further analyze the performance of these BaFe 1−x Cu x O 3 perovskites in GDI exhaust conditions, a study using 1% O 2 in He (which represents the named "fuel cuts" GDI exhaust conditions) has been developed [9]. Figure 12 shows the profiles of CO 2 and CO evolved during temperature programmed reaction experiments, including the profiles for the uncatalyzed reaction (blank corresponding to bare soot), as reference. Note that in the presence of BaFe 1−x Cu x O 3 catalysts, the amount of CO decreases and the amount of CO 2 increases. This means that, as could be expected [26,34,36,37], and as was observed during soot conversion reaction in NOx atmosphere, the catalysts increase the selectivity to CO 2 from 56% for bare soot to 93% for BFC0, 70% for BFC1, 79% for BFC3, and 87% for BFC4. As for NO 2 assisted diesel soot oxidation, the BFC0 catalyst is the most active and the addition of copper seems to decrease the ability of the catalysts to improve the CO 2 selectivity. Additionally, as it has been deduced from soot conversion results in NOx atmosphere (see Table 4) that BFC4 presents the highest CO 2 selectivity among the copper containing catalysts due to the presence of the surface copper species. Nanomaterials 2019, 9, 1551 16 of 22 was concluded that the copper content has an essential role on the performance of the BaFe1-xCuxO3 catalysts for soot oxidation, agreeing with previous reports focused on diesel soot removal [10,26,34,[36][37][38] and with the report for copper-supported ceria-zirconia catalysts for soot oxidation in GDI conditions [10]. These results confirm that the higher soot conversion presented by BFC4 with respect to the catalysts with lower copper content (BFC1 and BFC3) is linked both to the largest amount of β oxygen evolved by this catalyst, and with the presence of surface copper species (as BaOx-CuOx) [10,34,[36][37][38].
To further analyze the performance of these BaFe1-xCuxO3 perovskites in GDI exhaust conditions, a study using 1% O2 in He (which represents the named "fuel cuts" GDI exhaust conditions) has been developed [9]. Figure 11 shows the profiles of CO2 and CO evolved during temperature programmed reaction experiments, including the profiles for the uncatalyzed reaction (blank corresponding to bare soot), as reference. Note that in the presence of BaFe1-xCuxO3 catalysts, the amount of CO decreases and the amount of CO2 increases. This means that, as could be expected [26,34,36,37], and as was observed during soot conversion reaction in NOx atmosphere, the catalysts increase the selectivity to CO2 from 56% for bare soot to 93% for BFC0, 70% for BFC1, 79% for BFC3, and 87% for BFC4. As for NO2 assisted diesel soot oxidation, the BFC0 catalyst is the most active and the addition of copper seems to decrease the ability of the catalysts to improve the CO2 selectivity. Additionally, as it has been deduced from soot conversion results in NOx atmosphere (see Table 4) that BFC4 presents the highest CO2 selectivity among the copper containing catalysts due to the presence of the surface copper species.  Figure 11. CO2 a) and CO b) profiles during TPR soot oxidation in 1% O2 for BaFe1-xCuxO3 catalysts. Figure 12 shows the soot conversion profiles in 1% O2, calculated based on the amount of evolved CO and CO2 featured in Figure 11. In general terms, and in agreement with previous results for BaMn1-xCuxO3 catalysts [26], the catalytic effect is less relevant than the observed for NO2-assisted diesel soot oxidation. Thus, only BFC0 and BFC1 catalyze the soot oxidation with oxygen as the conversion profiles are shifted to lower temperature with respect to bare soot for these two catalysts. As observed for NO2 generation (see previous section), and in agreement with published conclusions [39,58,70], the soot conversion with oxygen follows the same trend than the amount of oxygen evolved during O2-TPD (Figure 8) as the most active catalysts (BFC0 and BFC1) are those generating the largest amount of oxygen. In fact, the highest activity of BFC1 at low temperature, i.e., at T < 600 °C approximately, seems to be related with the largest amount of and ' evolved ( Figure 8).    Thus, it seems that a similar reaction pathway is followed by soot oxidation with oxygen and with NO2-assisted diesel soot oxidation,  Figure 13 shows the soot conversion profiles in 1% O 2 , calculated based on the amount of evolved CO and CO 2 featured in Figure 12.  Figure 12 shows the soot conversion profiles in 1% O2, calculated based on the amount of evolved CO and CO2 featured in Figure 11. In general terms, and in agreement with previous results for BaMn1-xCuxO3 catalysts [26], the catalytic effect is less relevant than the observed for NO2-assisted diesel soot oxidation. Thus, only BFC0 and BFC1 catalyze the soot oxidation with oxygen as the conversion profiles are shifted to lower temperature with respect to bare soot for these two catalysts. As observed for NO2 generation (see previous section), and in agreement with published conclusions [39,58,70], the soot conversion with oxygen follows the same trend than the amount of oxygen evolved during O2-TPD (Figure 8) as the most active catalysts (BFC0 and BFC1) are those generating the largest amount of oxygen. In fact, the highest activity of BFC1 at low temperature, i.e., at T < 600 °C approximately, seems to be related with the largest amount of and ' evolved ( Figure 8).    Thus, it seems that a similar reaction pathway is followed by soot oxidation with oxygen and with NO2-assisted diesel soot oxidation, In general terms, and in agreement with previous results for BaMn 1−x Cu x O 3 catalysts [26], the catalytic effect is less relevant than the observed for NO 2 -assisted diesel soot oxidation. Thus, only BFC0 and BFC1 catalyze the soot oxidation with oxygen as the conversion profiles are shifted to lower temperature with respect to bare soot for these two catalysts. As observed for NO 2 generation (see previous section), and in agreement with published conclusions [39,58,70], the soot conversion with oxygen follows the same trend than the amount of oxygen evolved during O 2 -TPD ( Figure 8) as the most active catalysts (BFC0 and BFC1) are those generating the largest amount of oxygen. In fact, the highest activity of BFC1 at low temperature, i.e., at T < 600 • C approximately, seems to be related with the largest amount of and ' evolved ( Figure 8). Thus, it seems that a similar reaction pathway is followed by soot oxidation with oxygen and with NO 2 -assisted diesel soot oxidation, even though the catalytic effect is more relevant for the latter reaction than for the former. Hence, it could be concluded that the BaFe 1−x Cu x O 3 perovskites catalyze more effectively the NO 2 -soot reaction than the O 2 -soot reaction. Additionally, the comparison of these results with the obtained in the most demanding GDI conditions (0% O 2 ) [35] reveals that copper has an essential role on the performance of the BaFe 1−x Cu x O 3 catalysts for soot oxidation only in the absence of oxygen in the reaction atmosphere.
Summarizing, the activity data above discussed reveals that the BaFe 1−x Cu x O 3 perovskites catalyze both, the NO 2 -assisted diesel soot oxidation (500 ppm NO, 5% O 2 ) and, to a lesser extent, the soot oxidation in the "fuel cut" GDI exhaust conditions (1% O 2 ). BFC0 is the most active catalyst as the activity seems to be mainly related with the amount of O 2 evolved during an O 2 -TPD, which decreases with copper content.

Conclusions
The results obtained for the BaFe 1−x Cu x O 3 (x = 0, 0.1, 0.3 and 0.4) catalyst series allows us to conclude that: • Partial substitution of iron by copper in the lattice of a BaFeO 3 perovskite generates a distortion of the hexagonal perovskite structure for the lowest copper content catalyst (BFC1), and a change to cubic structure for the catalysts with higher copper content (BFC3 and BFC4).

•
The amount of copper inserted into the perovskite framework achieve a maximum for the highest copper content catalyst (BFC4), which provokes the presence of BaOx-CuOx as a minority segregated phase.

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The positive charge deficiency due to the partial substitution of Fe by Cu seems to be balanced by the oxidation of Fe(III) to Fe(IV) in the BFC1 perovskite and by the generation of additional oxygen vacancies/defects, for BFC3 and BFC4 catalysts. • BaFe 1 -xCuxO 3 perovskite catalyze both the NO 2 -assisted diesel soot oxidation (500 ppm NO, 5% O 2 ) and, to a lesser extent, the soot oxidation in the high demanding GDI exhaust conditions (1% O 2 ) • BFC0 is the most active catalyst for both oxidation reactions. The activity seems to be mainly related with the amount of O 2 evolved during an O 2 -TPD, which decreases with the copper content of the catalyst.