Reduction Process of Iron Catalyst Precursors for Ammonia Synthesis Doped with Lithium Oxide

Iron catalyst precursors promoted with oxides of calcium, aluminum, and lithium were prepared by a fusion method. Using XRD analysis, it was found that catalyst precursors had a magnetite structure. Lithium oxide, which is dependent on the Fe2+/Fe3+ molar ratio in a catalyst, was built into the magnetite structure as a solid solution and/or formed a separate Li2Fe3O4 phase. Lithium oxide forming the solid solution in magnetite accelerated the magnetite phase reduction. However, it was observed that magnetite, in the presence of lithium oxide, was not reduced to iron directly, but to a transient phase, Li2O·xFeO, where x < 3 was formed, which meant that the reduction to iron was much slower. Activity of the catalysts promoted with lithium oxide increased, while the degree of reduction increased.


Introduction
Iron catalyst is used in industrial processes of ammonia synthesis. The discovery of the iron-fused catalyst for the synthesis of ammonia has created the foundations for our current understanding of heterogeneous catalysis [1][2][3][4][5]. Today, iron-based catalysts are tested in hydrogen gas processes e.g., water gas shift reaction and ammonia decomposition [6][7][8][9][10]. Due to huge energy consumption in the process of ammonia synthesis, research into the creation of a new catalyst that enables running the synthesis at lower temperatures and pressures is still required.
On the basis of previous results it can be concluded that iron is the most effective catalyst in the ammonia synthesis among elements.
An iron catalyst precursor is obtained by melting magnetite and promoters. An oxidized form of the magnetite-based catalyst is composed mainly of iron oxide Fe 3 O 4 ; other metal oxides play the role of promoters. Oxides of aluminum, calcium, and potassium (Al 2 O 3 , CaO, and K 2 O) are most frequently used. Oxides of aluminum and calcium are structure-building promoters, and they influence the catalyst structure, its specific surface area, and thermal resistance under reaction conditions [11][12][13][14]. Potassium oxide is an activating promoter that changes iron sorption properties by the modification of iron surface. The nature of the potassium-activating role is not unambiguously clarified. According to Ertl [15,16], lattice planes, differing in Miller indices, showed differences in dissociative nitrogen chemisorption. The addition of potassium on the iron surface caused an equalization of activities of various lattice planes and, at the same time, made the activities much higher. Another mechanism has been proposed by Samorjai [17,18]. According to Samorjai, the presence of potassium eased desorption of the ammonia adsorbed on the catalyst surface and, as a result, more active sites were available.

Results and Discussion
Two catalyst precursors promoted with oxides of calcium, aluminum, and lithium were prepared by a fusion method. Chemical composition and molar ratio Fe 2+ /Fe 3+ of the prepared precursors are given in (Table 1). A characteristic of the industrial iron catalyst (PS-3-INS Grupa Azoty) for the ammonia synthesis promoted with potassium oxide, marked as KAT-K 2 O, was also given in Table 1. That catalyst was used as a reference point. Contents of calcium, aluminum, and lithium oxides were similar in the prepared lithium catalysts. However, these catalysts differed in molar ratio R. X-ray patterns of the obtained precursors are presented in (Figure 1). Contents of calcium, aluminum, and lithium oxides were similar in the prepared lithium catalysts. However, these catalysts differed in molar ratio R. X-ray patterns of the obtained precursors are presented in (Figure 1). Fe3O4, FeO, and CaFe3O5 phases were identified in the catalyst precursor KAT-K2O promoted with potassium oxide. In the catalyst precursor KAT1-Li2O, in that Li2O was an activating promoter and R = 0.68, the FeO phase did not occur in spite of an excess of Fe 2+ ions in comparison to magnetite. The CaFe3O5 phase was not visible either. Peaks of magnetite and Li2Fe3O4 phases (according to ICDD: 37-1432 card) were identified. Both Li2Fe3O4 and Fe3O4 crystallized similarly in a cubic crystal system with the same space group, Fd-3 m, and space group number 227. In the X-ray pattern of KAT2-Li2O catalyst, there were peaks belonging tomagnetite. No other peaks were observed in that precursor.
Authors of the previous work [33] found that potassium oxide in the iron magnetite-structure catalyst precursor was completely located within grain boundaries and not bound with iron oxides. The distribution of structural promoters (CaO, Al2O3) in an iron catalyst precursor depended on the molar ratio of iron ions R [34]. The distribution of promoters in the structure of an iron catalyst promoted with Li2O was presented in the paper [35]. The authors concluded that lithium oxide was bound with iron oxides and formed a separate Li2Fe3O4 phase.
On the basis of the X-ray diffraction, it was stated that lithium oxide in the iron catalyst precursor may have occurred as the separate phase Li2Fe3O4 (KAT1-Li2O) or formed the solid solution in magnetite (KAT2-Li2O). Using the selective etching [35] it was found thatlithium oxide in the catalyst KAT1-Li2O in the amount of 14% formed the solid solution with magnetite while the rest formed the Li2Fe3O4 phase.
The reduction process of catalyst precursors in a hydrogen atmosphere was examined in a differential reactor with a thermogravimetric measurement device. The dependence of mass change on the precursor reduction time is shown in (Figure 2).  Authors of the previous work [33] found that potassium oxide in the iron magnetite-structure catalyst precursor was completely located within grain boundaries and not bound with iron oxides. The distribution of structural promoters (CaO, Al 2 O 3 ) in an iron catalyst precursor depended on the molar ratio of iron ions R [34]. The distribution of promoters in the structure of an iron catalyst promoted with Li 2 O was presented in the paper [35]. The authors concluded that lithium oxide was bound with iron oxides and formed a separate Li 2 Fe 3 O 4 phase.
On the basis of the X-ray diffraction, it was stated that lithium oxide in the iron catalyst precursor may have occurred as the separate phase Li 2 Fe 3 O 4 (KAT1-Li 2 O) or formed the solid solution in magnetite (KAT2-Li 2 O). Using the selective etching [35] it was found thatlithium oxide in the catalyst KAT1-Li 2 O in the amount of 14% formed the solid solution with magnetite while the rest formed the Li 2 Fe 3 O 4 phase.
The reduction process of catalyst precursors in a hydrogen atmosphere was examined in a differential reactor with a thermogravimetric measurement device. The dependence of mass change on the precursor reduction time is shown in (Figure 2).
The reduction was carried out according to the procedure: polythermal heating from 25 • C to 420 • C at a heating rate of 10 • C/min, next the isothermal reduction at a temperature of 420 • C until a sample mass was constant, polythermal heating from 420 • C to 470 • C at a heating rate of 3.5 • C/min, and the isothermal reduction at 470 • C. The reduction was not completed at any case. The aim of the procedure was to determine the reduction run at the initial stage for catalysts of different phase contents. The reduction was carried out according to the procedure: polythermal heating from 25 °C to 420 °C at a heating rate of 10 °C/min, next the isothermal reduction at a temperature of 420 °C until a sample mass was constant, polythermal heating from 420 °C to 470 °C at a heating rate of 3.5 °C/min, and the isothermal reduction at 470 °C. The reduction was not completed at any case. The aim of the procedure was to determine the reduction run at the initial stage for catalysts of different phase contents.
Only the precursor of the catalyst promoted with potassium oxide (KAT-K2O), in which the wustite phase was present, started being reduced at a temperature of 420 °C. On the basis of literature [1], it was known that the FeO phase started being reduced at a temperature of 380 °C. The catalyst precursor promoted with lithium oxide characterized with R = 0.68 (KAT1-Li2O) had a similar molar ratio Fe 2+ /Fe 3+ as the precursor promoted with potassium oxide. However, the reduction process of that precursor as well as the catalyst promoted with lithium oxide started at a higher temperature In the initial stage, the reductions of KAT-K2O and KAT2-Li2O precursors were similar. The reduction of KAT1-Li2O ran slower ( Figure 3). In the case of KAT2-Li2O, for which only the magnetite phase was identified in the X-ray pattern, the highest reduction rate was observed at 571 °C. For KAT-K2O and KAT1-Li2O catalyst precursors the highest reduction rate was observed at 587 °C and 600 °C respectively. The inflection at a temperature of about 680 °C was visible on the DTA curve made for KAT2-Li2O. It may have pointed out the reduction of the harder reducible phase required higher temperature. It was confirmed by further results. Only the precursor of the catalyst promoted with potassium oxide (KAT-K 2 O), in which the wustite phase was present, started being reduced at a temperature of 420 • C. On the basis of literature [1], it was known that the FeO phase started being reduced at a temperature of 380 • C. The catalyst precursor promoted with lithium oxide characterized with R = 0.68 (KAT1-Li 2 O) had a similar molar ratio Fe 2+ /Fe 3+ as the precursor promoted with potassium oxide. However, the reduction process of that precursor as well as the catalyst promoted with lithium oxide started at a higher temperature.
In the initial stage, the reductions of KAT-K 2 O and KAT2-Li 2 O precursors were similar. The reduction of KAT1-Li 2 O ran slower ( Figure 3). The reduction was carried out according to the procedure: polythermal heating from 25 °C to 420 °C at a heating rate of 10 °C/min, next the isothermal reduction at a temperature of 420 °C until a sample mass was constant, polythermal heating from 420 °C to 470 °C at a heating rate of 3.5 °C/min, and the isothermal reduction at 470 °C. The reduction was not completed at any case. The aim of the procedure was to determine the reduction run at the initial stage for catalysts of different phase contents.
Only the precursor of the catalyst promoted with potassium oxide (KAT-K2O), in which the wustite phase was present, started being reduced at a temperature of 420 °C. On the basis of literature [1], it was known that the FeO phase started being reduced at a temperature of 380 °C. The catalyst precursor promoted with lithium oxide characterized with R = 0.68 (KAT1-Li2O) had a similar molar ratio Fe 2+ /Fe 3+ as the precursor promoted with potassium oxide. However, the reduction process of that precursor as well as the catalyst promoted with lithium oxide started at a higher temperature In the initial stage, the reductions of KAT-K2O and KAT2-Li2O precursors were similar. The reduction of KAT1-Li2O ran slower ( Figure 3). In the case of KAT2-Li2O, for which only the magnetite phase was identified in the X-ray pattern, the highest reduction rate was observed at 571 °C. For KAT-K2O and KAT1-Li2O catalyst precursors the highest reduction rate was observed at 587 °C and 600 °C respectively. The inflection at a temperature of about 680 °C was visible on the DTA curve made for KAT2-Li2O. It may have pointed out the reduction of the harder reducible phase required higher temperature. It was confirmed by further results. In the case of KAT2-Li 2 O, for which only the magnetite phase was identified in the X-ray pattern, the highest reduction rate was observed at 571 • C. For KAT-K 2 O and KAT1-Li 2 O catalyst precursors the highest reduction rate was observed at 587 • C and 600 • C respectively. The inflection at a temperature of about 680 • C was visible on the DTA curve made for KAT2-Li 2 O. It may have pointed out the reduction of the harder reducible phase required higher temperature. It was confirmed by further results.
Results on the polythermal reduction of the industrial catalyst KAT-K 2 O precursor in an XRK 900 reaction chamber are presented in (Figure 4). Changes of peak intensities, given as peak areas (they are depicted by the Is symbols), of individual phases in dependence on temperature are presented.
Results on the polythermal reduction of the industrial catalyst KAT-K2O precursor in an XRK 900 reaction chamber are presented in (Figure 4). Changes of peak intensities, given as peak areas (they are depicted by the Is symbols), of individual phases in dependence on temperature are presented. Results on the polythermal reduction of the catalyst precursor promoted with potassium oxide were in a good accordance with literature data [1]. At first, the wustite phase reduction took place (380-410 °C), then the magnetite phase (440-550 °C) was reduced.
The reduction of the industrial catalyst precursor KAT-K2O was examined in-situ under isothermal conditions at a temperature of 470 °C (Supplementary Materials Figures S1 and S2).
The dependence of peak intensity changes on reduction temperature of the catalyst precursors KAT1-Li2O and KAT2-Li2O are shown in (Figures 5 and 6). In the initial stage (from a temperature of 410 °C) the magnetite phase of the KAT1-Li2O was reduced ( Figure 5). An increase in the area of Li2Fe3O4 phase peak was visible at the same time. In the KAT2-Li2O, of R = 0.54, lithium was only in the form of a solid solution in magnetite. The reduction process was noticeable at temperatures close to 450 °C ( Figure 6). Results on the polythermal reduction of the catalyst precursor promoted with potassium oxide were in a good accordance with literature data [1]. At first, the wustite phase reduction took place (380-410 • C), then the magnetite phase (440-550 • C) was reduced.
The reduction of the industrial catalyst precursor KAT-K 2 O was examined in-situ under isothermal conditions at a temperature of 470 • C (Supplementary Materials Figures S1 and S2).
The dependence of peak intensity changes on reduction temperature of the catalyst precursors KAT1-Li 2 O and KAT2-Li 2 O are shown in (Figures 5 and 6).
Results on the polythermal reduction of the industrial catalyst KAT-K2O precursor in an XRK 900 reaction chamber are presented in (Figure 4). Changes of peak intensities, given as peak areas (they are depicted by the Is symbols), of individual phases in dependence on temperature are presented. Results on the polythermal reduction of the catalyst precursor promoted with potassium oxide were in a good accordance with literature data [1]. At first, the wustite phase reduction took place (380-410 °C), then the magnetite phase (440-550 °C) was reduced.
The reduction of the industrial catalyst precursor KAT-K2O was examined in-situ under isothermal conditions at a temperature of 470 °C (Supplementary Materials Figures S1 and S2).
The dependence of peak intensity changes on reduction temperature of the catalyst precursors KAT1-Li2O and KAT2-Li2O are shown in (Figures 5 and 6). In the initial stage (from a temperature of 410 °C) the magnetite phase of the KAT1-Li2O was reduced ( Figure 5). An increase in the area of Li2Fe3O4 phase peak was visible at the same time. In the KAT2-Li2O, of R = 0.54, lithium was only in the form of a solid solution in magnetite. The reduction process was noticeable at temperatures close to 450 °C ( Figure 6). In the initial stage (from a temperature of 410 • C) the magnetite phase of the KAT1-Li 2 O was reduced ( Figure 5). An increase in the area of Li 2 Fe 3 O 4 phase peak was visible at the same time. In the KAT2-Li 2 O, of R = 0.54, lithium was only in the form of a solid solution in magnetite. The reduction process was noticeable at temperatures close to 450 • C ( Figure 6).
The reduction process of Li 2 Fe 3 O 4 in the KAT1-Li 2 O catalyst did not run directly to iron in. On X-ray patterns in (Supplementary Materials, Figure S3), it may have been observed that the peak of the Li 2 Fe 3 O 4 phase was asymmetric (it was broadened at lower scattering angles), what showed that a new phase was formed. It may have been supposed that the new phase was Li 2 O·xFeO, where x > 3. During the reduction process, a precise analysis of intensities and shapes of peaks belonging to Fe 3 O 4 and Li 2 Fe 3 O 4 phases was carried out. The X-ray pattern, in the scattering angle range 2Θ from 41 • to 44 • , taken in the reduction stage when the intensity of the Li 2 Fe 3 O 4 peak was maximal, and the intensity of Fe 3 O 4 peak decreased of 50%, are presented in (Figure 7).
The reduction process of Li2Fe3O4 in the KAT1-Li2O catalyst did not run directly to iron in. On X-ray patterns in (Supplementary Materials, Figure S3), it may have been observed that the peak of the Li2Fe3O4 phase was asymmetric (it was broadened at lower scattering angles), what showed that a new phase was formed. It may have been supposed that the new phase was Li2O·xFeO, where x > 3. During the reduction process, a precise analysis of intensities and shapes of peaks belonging to Fe3O4 and Li2Fe3O4 phases was carried out. The X-ray pattern, in the scattering angle range 2Θ from 41° to 44°, taken in the reduction stage when the intensity of the Li2Fe3O4 peak was maximal, and the intensity of Fe3O4 peak decreased of 50%, are presented in (Figure 7).  Deconvolution of that peak confirmed that during the reduction of the Li2Fe3O4 phase a new transient phase occurred. Much better fitting was found when an additional peak at the angle 2θ of 42.1° was inserted (left of the phase Li2Fe3O4 phase, 2θ = 42.45°). The peak could not be ascribed to the FeO phase because it would occur at the lower angle-2θ = 41.80° and at a temperature of 460 °C it would be reduced rapidly (Supplementary Materials Figure S1).
The analysis of the maximum position of the Li2Fe3O4 peak during the reduction process is shown in (Figure 8).
In the initial stage of the magnetite phase reduction, a new additional compound Li2O·xFeO was formed. It shifted the peak maximum of Li2Fe3O4 towards lower angles (the increase in lattice constant). After the reduction of the new phase Li2O·xFeO, the maximum shifted towards higher angles (the decrease in lattice constant). Shifts towards higher angles were connected with non- X-ray patterns in (Supplementary Materials, Figure S3), it may have been observed that the peak of the Li2Fe3O4 phase was asymmetric (it was broadened at lower scattering angles), what showed that a new phase was formed. It may have been supposed that the new phase was Li2O·xFeO, where x > 3. During the reduction process, a precise analysis of intensities and shapes of peaks belonging to Fe3O4 and Li2Fe3O4 phases was carried out. The X-ray pattern, in the scattering angle range 2Θ from 41° to 44°, taken in the reduction stage when the intensity of the Li2Fe3O4 peak was maximal, and the intensity of Fe3O4 peak decreased of 50%, are presented in (Figure 7).  Deconvolution of that peak confirmed that during the reduction of the Li2Fe3O4 phase a new transient phase occurred. Much better fitting was found when an additional peak at the angle 2θ of 42.1° was inserted (left of the phase Li2Fe3O4 phase, 2θ = 42.45°). The peak could not be ascribed to the FeO phase because it would occur at the lower angle-2θ = 41.80° and at a temperature of 460 °C it would be reduced rapidly (Supplementary Materials Figure S1).
The analysis of the maximum position of the Li2Fe3O4 peak during the reduction process is shown in (Figure 8).
In the initial stage of the magnetite phase reduction, a new additional compound Li2O·xFeO was formed. It shifted the peak maximum of Li2Fe3O4 towards lower angles (the increase in lattice constant). After the reduction of the new phase Li2O·xFeO, the maximum shifted towards higher angles (the decrease in lattice constant). Shifts towards higher angles were connected with non-  Figure S1).
The analysis of the maximum position of the Li 2 Fe 3 O 4 peak during the reduction process is shown in (Figure 8).
In the initial stage of the magnetite phase reduction, a new additional compound Li 2 O·xFeO was formed. It shifted the peak maximum of Li 2 Fe 3 O 4 towards lower angles (the increase in lattice constant). After the reduction of the new phase Li 2 O·xFeO, the maximum shifted towards higher angles (the decrease in lattice constant). Shifts towards higher angles were connected with non-stoichiometry of Li 2 O·xFeO, where x < 3. During the reduction, FeO was reduced to Fe. The presence of lithium caused that magnetite was not reduced directly to Fe, but to FeO at a temperature of 460 • C. That oxide combined with Li 2 O forming the additional phase Li 2 O·xFeO. It is known from literature [36] that magnetite was reduced only at temperatures over 570 • C through wustite to iron. The authors' views on the direct reduction of magnetite to metallic iron are divided. Authors of the work [1], on the basis of "in situ" examinations carried out in a reaction chamber, made with the aid of XRD method, confirmed the presence of wustite after the reduction at a temperature of 413 • C. Other authors on the ground of chemical analysis and Mössbauer investigations [37,38] made the wustite formation impossible during the reduction of the magnetite precursor. Results of our research confirmed that magnetite was reduced to iron through the wustite phases. The same phenomenon was observed for KAT-Li 2 O in which lithium formed a solid solution in magnetite. Regarding temperature shifts connected with a lattice constant extend, isothermal examinations gave more information (Supplementary Materials Figure S4). stoichiometry of Li2O·xFeO, where x < 3. During the reduction, FeO was reduced to Fe. The presence of lithium caused that magnetite was not reduced directly to Fe, but to FeO at a temperature of 460 °C. That oxide combined with Li2O forming the additional phase Li2O·xFeO. It is known from literature [36] that magnetite was reduced only at temperatures over 570 °C through wustite to iron. The authors' views on the direct reduction of magnetite to metallic iron are divided. Authors of the work [1], on the basis of "in situ" examinations carried out in a reaction chamber, made with the aid of XRD method, confirmed the presence of wustite after the reduction at a temperature of 413 °C. Other authors on the ground of chemical analysis and Mössbauer investigations [37,38] made the wustite formation impossible during the reduction of the magnetite precursor. Results of our research confirmed that magnetite was reduced to iron through the wustite phases. The same phenomenon was observed for KAT-Li2O in which lithium formed a solid solution in magnetite. Regarding temperature shifts connected with a lattice constant extend, isothermal examinations gave more information (Supplementary Materials Figure S4). The change of Fe3O4 peak position, during the isothermal reduction, in the dependence on time was presented in (Figure 9). Similarly to the KAT1-Li2O catalyst, the shift of the peak maximum towards lower angles was observed what may have been attributed to a new phase Li2O·xFeO (where x < 3) formation. After The change of Fe 3 O 4 peak position, during the isothermal reduction, in the dependence on time was presented in (Figure 9). stoichiometry of Li2O·xFeO, where x < 3. During the reduction, FeO was reduced to Fe. The presence of lithium caused that magnetite was not reduced directly to Fe, but to FeO at a temperature of 460 °C. That oxide combined with Li2O forming the additional phase Li2O·xFeO. It is known from literature [36] that magnetite was reduced only at temperatures over 570 °C through wustite to iron. The authors' views on the direct reduction of magnetite to metallic iron are divided. Authors of the work [1], on the basis of "in situ" examinations carried out in a reaction chamber, made with the aid of XRD method, confirmed the presence of wustite after the reduction at a temperature of 413 °C. Other authors on the ground of chemical analysis and Mössbauer investigations [37,38] made the wustite formation impossible during the reduction of the magnetite precursor. Results of our research confirmed that magnetite was reduced to iron through the wustite phases. The same phenomenon was observed for KAT-Li2O in which lithium formed a solid solution in magnetite. Regarding temperature shifts connected with a lattice constant extend, isothermal examinations gave more information (Supplementary Materials Figure S4). The change of Fe3O4 peak position, during the isothermal reduction, in the dependence on time was presented in (Figure 9). Similarly to the KAT1-Li2O catalyst, the shift of the peak maximum towards lower angles was observed what may have been attributed to a new phase Li2O·xFeO (where x < 3) formation. After Similarly to the KAT1-Li 2 O catalyst, the shift of the peak maximum towards lower angles was observed what may have been attributed to a new phase Li 2 O·xFeO (where x < 3) formation. After the maximum of asymmetry had been attained it started getting smaller causing the shift of total peak towards higher angles.
The average size of iron crystallites formed during the reduction processes of the examined catalysts was also compared (Figure 10). the maximum of asymmetry had been attained it started getting smaller causing the shift of total peak towards higher angles.
The average size of iron crystallites formed during the reduction processes of the examined catalysts was also compared ( Figure 10). Sizes of iron crystallites formed during the reduction of KAT-K2O and KAT2-Li2O catalysts were very similar for both catalysts. It was found that the industrial catalyst of the magnetite structure and promoted with potassium oxide was fully reduced at 500 °C. The average size of iron crystallites was around 30 nm. The further increase in reduction temperature caused the recrystallization process and increase in size of iron crystallites.
Catalysts promoted with lithium oxide reached the full reduction only at a temperature of 600 °C. Under these conditions, the iron recrystallization process run; the average size of crystallites was in the range of 40 nm to 60 nm.
The catalyst KAT1-Li2O containing the additional phase Li2Fe3O4 was reduced faster and formed crystallites of iron that recrystallized easily while temperature rose. Structural promoters calcium and aluminum oxides, protecting iron against sintering, were released during the magnetite phase reduction, and formed a three-dimensional (3-D) structure; it means they formed bridges between iron crystallites. Significantly bigger iron crystallites were observed for the catalyst KAT1-Li2O than for the catalysts KAT2-Li2O that contained only magnetite.
Arrhenius curves for the tested catalyst reduced at a temperature of 500 °C and after reduction at 650 °C are shown in Figure 11.
Apparent activation energies were calculated from slopes of straights for catalysts reduced at various temperatures, Table 2.
Catalysts promoted with lithium oxide and reduced at a temperature of 650 °C showed lower activity compared to the catalyst KAT-K2O promoted with potassium oxide. However, properties of the catalyst promoted with lithium oxide after reduction at 650 °C were very interesting-their activity rose. Sizes of iron crystallites formed during the reduction of KAT-K 2 O and KAT2-Li 2 O catalysts were very similar for both catalysts. It was found that the industrial catalyst of the magnetite structure and promoted with potassium oxide was fully reduced at 500 • C. The average size of iron crystallites was around 30 nm. The further increase in reduction temperature caused the recrystallization process and increase in size of iron crystallites.
Catalysts promoted with lithium oxide reached the full reduction only at a temperature of 600 • C. Under these conditions, the iron recrystallization process run; the average size of crystallites was in the range of 40 nm to 60 nm.
The catalyst KAT1-Li 2 O containing the additional phase Li 2 Fe 3 O 4 was reduced faster and formed crystallites of iron that recrystallized easily while temperature rose. Structural promoters calcium and aluminum oxides, protecting iron against sintering, were released during the magnetite phase reduction, and formed a three-dimensional (3-D) structure; it means they formed bridges between iron crystallites. Significantly bigger iron crystallites were observed for the catalyst KAT1-Li 2 O than for the catalysts KAT2-Li 2 O that contained only magnetite.
Arrhenius curves for the tested catalyst reduced at a temperature of 500 • C and after reduction at 650 • C are shown in Figure 11.   Apparent activation energies were calculated from slopes of straights for catalysts reduced at various temperatures, Table 2. Catalysts promoted with lithium oxide and reduced at a temperature of 650 • C showed lower activity compared to the catalyst KAT-K 2 O promoted with potassium oxide. However, properties of the catalyst promoted with lithium oxide after reduction at 650 • C were very interesting-their activity rose.
The completed reduction at that temperature caused releasing of lithium oxide onto the iron surface. It was found [35] from TPD-H 2 tests that the amount of hydrogen sorption sites on the surface of catalysts promoted with lithium oxide and reduced at 650 • C were significantly increased in comparison with the reduction at 500 • C when the total surface area was taken into account. As a result of the increase in the catalyst reduction degree at 650 • C, the catalyst absolute activity increased while lithium oxide concentration on the catalyst surface increased. However, the average size of crystallites was bigger at the same temperature as a result of the sintering, Figure 10.

Materials and Methods
Precursors of catalysts for the ammonia synthesis were obtained by a fusing method in a laboratory plant for fused catalysts, Scheme 1 [39]. Feeding mixtures for the melting of catalysts were made of magnetite ore and oxide of calcium, aluminum, and lithium hydroxide. Molar ratio Fe 2+ /Fe 3+ was adjusted using a proper amount of reducer, added during the melting process. With this technique, catalysts with various Fe 2+ /Fe 3+ ratios were prepared. Precursors of catalyst with a constant ratio of the mass of promoter oxides to mass of iron (Al 2 O 3 -0.027, CaO-0.015, and Li2O-0.011) were studied. These catalysts were signed as KAT1-Li 2 O and KAT2-Li 2 O. The reduction of catalyst precursors was studied in a differential reactor equipped with a thermogravimetric measurement, in a hydrogen atmosphere at a flow of 80 dm 3. h −1. g −1 under iso-(470 °C) and polythermal conditions during a heating from 350 °C to 750 °C at a rate of 3.5 °C/min.
In situ studies of the reduction of the catalysts were carried out in reaction chamber XRK900 (Antor Paar, Blankenfelde-Mahlow, German), connected with X-ray diffraction apparatus Philips X'Pert PRO (Almelo, The Netherland) using Cu-Kα radiation (λ = 1.54 Å). The reduction was carried Chemical compositions of catalyst precursors were determined with the aid of inductively coupled plasma atomic emission spectroscopy (ICP-AES) using the PerkinElmer Optima 5300 DV (Waltham, MA, USA) spectrometer.
The ratio Fe 2+ /Fe 3+ was determined with the manganometric titration method and denoted with an R letter in the whole paper.
The reduction of catalyst precursors was studied in a differential reactor equipped with a thermogravimetric measurement, in a hydrogen atmosphere at a flow of 80 dm 3. h −1. g −1 under iso-(470 • C) and polythermal conditions during a heating from 350 • C to 750 • C at a rate of 3.5 • C/min.
In situ studies of the reduction of the catalysts were carried out in reaction chamber XRK900 (Antor Paar, Blankenfelde-Mahlow, German), connected with X-ray diffraction apparatus Philips X'Pert PRO (Almelo, The Netherland) using Cu-Kα radiation (λ = 1.54 Å). The reduction was carried out in a hydrogen atmosphere at a flow of 60 dm 3. h −1. g −1 at a heating rate of 2.5 • C/min. The same diffractometer was used to determine a phase composition of the examined catalysts. Taken X-ray patterns were analyzed with the X'Pert HighScore Plus software (version 2.2, PANalytical, Almelo, The Netherland) and compared with the ICDD database.
The catalytic activity was measured in a six-channel integral reactor at the pressure of 10 MPa. A detailed description of the method has been reported previously in this work [34]. Before activity tests, samples of the oxidized form of the catalysts were reduced polythermally in the temperature range of 350-500 • C, at a pressure of 0.1 MPa, by means of a nitrogen-hydrogen mixture using space velocity of about 20,000 h −1 . The final stage of reduction was executed at a pressure of 10 MPa and at a temperature of 500 • C. The activity studies were carried out under the same pressure in the temperature range of 350-500 • C. The rate constant calculated from the Temkin-Pyzhew equation was accepted as a measure of the activity. Subsequently, the catalysts were reduced polythermally into 650 • C, at a pressure of 0.1 MPa. When reduction was completed, the determination of the catalyst activities was performed again.

Conclusions
Lithium oxide was built into the magnetite structure during the melting process of the iron catalyst precursor and/or it formed the separate phase with iron(II) oxide. The form of lithium oxide binding depended on reduction-oxidation conditions during the fusing process. In the excess of Fe 2+ ions of the additional phase, Li 2 Fe 3 O 4 occurred. That phase was reduced at a lower temperature in comparison with the solid solution of lithium in iron.
Lithium oxide forming the solid solution in the magnetite accelerated the reduction process of the magnetite phase. It was observed that magnetite in the presence of lithium oxide was not reduced to iron directly, however, a new intermediate phase occurred, of which the reduction was much slower.
Fused catalysts promoted with lithium oxide showed lower activity in comparison with catalysts promoted with potassium oxide because the lithium promoted catalysts needed to be reduced at higher temperatures, which was the reason of the sintering of iron crystallites.

Supplementary Materials:
The following are available online at http://www.mdpi.com/2073-4344/8/11/494/s1, Figure S1. Demonstration X-ray patterns of the industrial catalyst precursor KAT-K 2 O taken after various reduction times at a temperature of 470 • C, Figure S2. Dependence of peak intensities of Fe 3 O 4 , FeO, and Fe on the reduction time for the industrial catalyst precursor KAT-K 2 O (T = 470 • C). For better view the peak intensity of Fe phase was divided by 4, Figure S3. X-ray patterns taken after various times of KAT1-Li 2 O catalyst precursor reduction at a temperature of 520 • C, Figure S4. X-ray patterns of the KAT2-Li 2 O catalyst after various time of the reduction at 520 • C.
Funding: This research received no external funding.