Next Article in Journal
Fracture Toughness and Fatigue Crack Growth Analyses on a Biomedical Ti-27Nb Alloy under Constant Amplitude Loading Using Extended Finite Element Modelling
Next Article in Special Issue
Key Role of Corncob Based-Hydrochar (HC) in the Enhancement of Visible Light Photocatalytic Degradation of 2,4-Dichlorophenoxyacetic Acid Using a Derivative of ZnBi-Layered Double Hydroxides
Previous Article in Journal
A Joint Johnson–Cook-TANH Constitutive Law for Modeling Saw-Tooth Chip Formation of Ti-6AL-4V Based on an Improved Smoothed Particle Hydrodynamics Method
Previous Article in Special Issue
Heterogeneous Catalysts in N-Heterocycles and Aromatics as Liquid Organic Hydrogen Carriers (LOHCs): History, Present Status and Future
 
 
Search for Articles:
Title / Keyword
Author / Affiliation / Email
Journal
Article Type
 
 
Advanced Search
 
Section
Special Issue
Volume
Issue
Number
Page
 
Journals
Materials
Volume 16
Issue 12
10.3390/ma16124466
materials-logo
Submit to this Journal Review for this Journal Propose a Special Issue
► Article Menu

Article Menu

share Share announcement Help format_quote Cite question_answer Discuss in SciProfiles thumb_up
...
Endorse textsms
...
Comment
first_page
settings
Order Article Reprints
Font Type:
Arial Georgia Verdana
Font Size:
Aa Aa Aa
Line Spacing:
Column Width:
Background:
Article

The Relationship between the Structural Characteristics of α-Fe2O3 Catalysts and Their Lattice Oxygen Reactivity Regarding Hydrogen

by
Nadezhda Kirik
1,*,
Alexander Krylov
2,
Andrey Boronin
3,
Sergey Koshcheev
3,
Leonid Solovyov
1,
Evgenii Rabchevskii
1,
Nina Shishkina
1 and
Alexander Anshits
1,4,*
1
Federal Research Center “Krasnoyarsk Science Center of Siberian Branch of the Russian Academy of Sciences”, Institute of Chemistry and Chemical Technology, 50/24, Akademgorodok, 660036 Krasnoyarsk, Russia
2
Federal Research Center “Krasnoyarsk Science Center of Siberian Branch of the Russian Academy of Sciences”, Kirensky Institute of Physics, 50/38, Akademgorodok, 660036 Krasnoyarsk, Russia
3
Federal Research Center Boreskov Institute of Catalysis, 5, Ac. Lavrentieva Ave., 630090 Novosibirsk, Russia
4
Department of Chemistry, 79, Svobodny Ave., Siberian Federal University, 660041 Krasnoyarsk, Russia
*
Authors to whom correspondence should be addressed.
Materials 2023, 16(12), 4466; https://doi.org/10.3390/ma16124466
Submission received: 22 May 2023 / Revised: 8 June 2023 / Accepted: 16 June 2023 / Published: 19 June 2023
(This article belongs to the Special Issue The 15th Anniversary of Materials—Recent Advances in Catalytic Materials)
Browse Figures
Versions Notes

Abstract

:
In this paper, the relationship between the structural features of hematite samples calcined in the interval of 800–1100 °C and their reactivity regarding hydrogen studied in the temperature-programmed reaction (TPR-H2) was studied. The oxygen reactivity of the samples decreases with the increasing calcination temperature. The study of calcined hematite samples used X-ray Diffraction (XRD), Scanning Electron Microscopy (SEM), X-ray Photoelectron Spectroscopy (XPS), and Raman spectroscopy, and their textural characteristics were studied also. According to XRD results, hematite samples calcined in the temperature range under study are monophase, represented by the α-Fe2O3 phase, in which crystal density increases with increasing calcination temperature. The Raman spectroscopy results also register only the α-Fe2O3 phase; the samples consist of large, well-crystallized particles with smaller particles on their surface, having a significantly lower degree of crystallinity, and their proportion decreases with increasing calcination temperature. XPS results show the α-Fe2O3 surface enriched with Fe2+ ions, whose proportion increases with increasing calcination temperature, which leads to an increase in the lattice oxygen binding energy and a decrease in the α-Fe2O3 reactivity regarding hydrogen.

1. Introduction

Iron oxides are actively studied as catalysts in oxidation processes and as oxygen carriers in high-temperature chemical lopping processes, such as carbonaceous fuels combustion (CLC), reforming (CLR), hydrogen generation (CLGH), and partial methane oxidation (CLPO) [1,2,3,4,5,6,7]. Compared with other oxide systems, iron oxide-based materials have several advantages: the main ones are the possibility of modifying the reactivity, high oxygen capacity, high melting temperatures, mechanical strength characteristics, low cost, and natural compatibility.
High-temperature pretreatment of iron oxide-based catalysts affects not only the specific surface area, crystallite sizes, and mechanical properties, but also influences the surface atomic structure and structural characteristics of the oxides [8,9]. In particular, the temperature treatment of nanosized hematite samples in the range of 250–900 °C demonstrated the areas of structural disorder in the crystal lattice connected with the transformation of octahedral Fe3+ positions into tetrahedral Fe2+ ones after sample calcination at 900 °C [8]. During heat treatment of synthetic goethite up to 1100 °C, the formation of stoichiometric hematite after calcination at 500 °C occurs. For the structure of samples calcined up to 800 °C, the presence of flat defects in the basal plane is characteristic; with further increase in temperature, these defects disappear, and the formation of extended defects occurs, such as twins and surface steps, stabilizing in high-temperature (900–1100 °C) samples due to impurities [9].
The effect of high-temperature pretreatment (850–950 °C) of ore with a hematite content of 95 wt.% on the stabilization of activity during methane conversion in the CLC process is shown in [10]. The activity of calcined samples is maintained for 80 consecutive red-ox cycles, which is an important characteristic of oxygen carriers in cyclic processes.
In high-temperature CLC processes, at the first stage (in a fuel reactor) the fuel interacts with the oxygen carrier in the oxidized form [11,12,13], and the oxidation of hydrocarbons, hydrogen, and/or carbon monoxide occurs due to the lattice oxygen of the oxide, while the oxide crystal lattice at the initial stage transforms with the formation of surface vacancies in the anion sublattice [5,14,15]. The completely reduced oxygen carrier is then oxidized at the second stage (in an air or steam reactor) [11,12,13].
The high-temperature effect of obtaining hematite samples with α-Fe2O3 structure on the reactivity regarding hydrogen is found in several works [16,17,18,19]. With increasing calcination temperature in the range of 500–1200 °C of hematite samples obtained from different precursors, the initial reduction temperature (Tin) in the temperature-programmed reaction (TPR), in general, increases [16]. Samples synthesized from different precursors have different Tin after calcination at a fixed temperature. The difference also remains after high-temperature calcination (1100–1200 °C), which apparently relates to the differences in bulk and surface properties of α-Fe2O3 structure. It was also shown that the values of the activation energy vary during the reduction in the hydrogen of hematite samples with heat treatment (1200 °C) and without it [18].
Thus, the temperature pretreatment of α-Fe2O3 and its oxide-based systems is an essential factor affecting the red-ox properties, reducibility of oxides, and their reactivity to reducing agents (hydrogen, carbon monoxide, methane). Complex studies of the relationship between the calcination temperature, structural characteristics, and hematite oxidative reactivity have not been practically conducted. Previously, we showed [19] that increasing the calcination temperature of hematite samples with corundum structure in the range of 800–1100 °C leads to a consistent increase in the crystal density of the α-Fe2O3 phase, indicating a decrease in the degree of crystal lattice disorder and the growth of lattice oxygen binding energy, which manifests itself in a significant decrease in the α-Fe2O3 reactivity regarding hydrogen. The present work aimed to investigate the relationship between the structural features, surface state, and the lattice oxygen reactivity regarding H2 (as model reducing agent) of the α-Fe2O3 samples obtained using high-temperature (800–1100 °C) synthesis.

2. Materials and Methods

2.1. Chemicals and Materials

To prepare samples of α-Fe2O3, we used a powdered reagent of Fe2O3 (TC 6-09-1418-78, high purity qualification, heavy metal (Cu, Co, Sb) impurities < 5.0·10−3 wt. %). The reagent was dried at 200 °C for 2 h to remove hygroscopic moisture. The dried and fractionated material (˂40 μm), weighing 0.7–1.0 g, was pressed at 390 MPa with a holding time of 4 min into tablets of 16 mm diameter, about 1.0–1.5 mm thick, then calcined in air at 800, 900, 1000 and 1100 °C for 10 h and cooled to room temperature at a rate of ~8°/min. Sintered samples were milled, alternating crushing stages in a ball mill KM-1 (VEB, DDR) for 5 min and sieving on a vibratory drive VP/S-220 (Vibrotechnik, Russia) for 2 min, with selecting fractions of particle size class −0.2 + 0.1 mm. Marking of the samples used the values of calcination temperature; for example, sample Fe2O3-800 was calcined at 800 °C.

2.2. Characterization Techniques

The measurement of the texture characteristics of the obtained samples used a NOVA 3200e sorption analyzer (Quantachrome Instruments, USA) in the low-temperature nitrogen adsorption mode at −195.8 °C with samples degassed at 300 °C for 12 h to a residual pressure of <10−2 mm Hg. The specific surface area (SSA) calculation used a modified BET method [20,21], which makes it possible to consider the presence of micropores in the meso-macroporous material. The volume of micropores (Vmic) and mesopores (Vmeso) was analyzed by the comparative t-method using the de Boer equation to calculate the thickness of the statistical adsorbate layer [22]. The specific surface area and pore volume were averaged using the values of 4 independent measurements.
Morphologies of calcined hematite samples were studied using scanning electron microscopy (SEM) with a TM-4000 (Hitachi, Tokyo, Japan) instrument.
X-ray diffraction patterns were recorded on an X’Pert Pro MPD diffractometer (PANalytical, Almelo, The Netherlands) with a high-speed PIXcel detector in the angular interval of 23–153° 2Θ, in steps of 0.013° on Cu Kα radiation. The crystal lattice parameters of the hematite phase were determined and refined using the Rietveld full-profile approach using the derivative difference minimization (DDM) method [23,24,25], the XRD peak shift due to the sample surface misalignment was included in the Rietveld full-profile model and the respective displacement parameter was refined along with the lattice parameters to minimize the systematic errors. Owing to well-resolved diffraction peaks in the wide diffraction angle interval used, the lattice and peak shift parameters were correctly and precisely refined.
The Raman spectra were recorded in the wavenumbers range of 50–1600 cm−1 in the backscattering configuration on a T64000 triple spectrometer (HORIBA Jobin Yvon, Palaiseau, France) with a spectral resolution of 2 cm−1. To excite the sample, a diode-pumped solid-state Excelsior-532-300-CDRH laser (Spectra-Physics, Milpitas, CA, USA) with a wavelength of 532 nm and a power of 1 mW was used on the sample. The spectra were obtained in an air atmosphere from the sample located on a glass slide. The excitation radiation was focused on the sample using an Olympus BX41 microscope through a 50× Olympus MPlan objective with a numerical aperture of N.A = 0.75 into a spot 3 µm in diameter.

2.3. Examination of the State Surface of Calcined α-Fe2O3 Samples

The surface state of calcined hematite samples was examined using X-ray photoelectron spectroscopy on an ES300 photoelectron spectrometer (KRATOS Analytical, Manchester, UK) calibrated along Au4f7/2 and Cu2p3/2 lines with 84.0 and 932.7 eV binding energies for gold and copper metal foils, respectively [26]. A nonmonochromatized Mg Kα X-ray source with 1253.6 eV energy was used to record the spectra. To exclude the sample charging effect, the spectra were calibrated by shifting all recorded spectral lines by the value corresponding to the electrostatic charge using the C1s reference peak from amorphous carbon with Eb(C1s) = 285.0 eV. In the investigated samples, this value of Eb(C1s) plays the role of being an internal standard for binding energies of lines of other elements. A conductive adhesive tape specifically used for vacuum technologies provided the electrical contact of the samples with the metal holder. All samples were carefully grounded in an agate mortar before taping.
For the identification of lines and qualitative elemental composition of the surface, the survey spectrum in the range of 0–1200 eV was used. The detailed high-resolution spectra of lines Fe2p, O1s, C1s, etc. were registered to analyze the quantitative composition of samples and the chemical surface state. Calculations of sample composition were performed with the help of atomic sensitivity factors (ASF) [27,28].
Spectra were decomposed into individual components using the Gauss and Lorentz functions after subtracting the scattered electron background using the Shirley method. The spectra processing was performed using the original XPSCalc Software tested on oxide [29] and metal-oxide systems [30].

2.4. Temperature-Programmed Reduction of α-Fe2O3 Samples by Hydrogen

Temperature-programmed reduction measurements were carried out in a TG-DSC NETZSCH STA 449C (Germany) analyzer equipped with an Aeolos QMS 403C mass spectrometer, under 5%H2 + 95%Ar (H2 grade A, 99.99 vol.%, Ar grade 5.0, 99.999 vol.%) atmosphere at ambient pressure with heating in the range of 40–900 °C in Pt crucibles without lids (30.00 ± 0.01 mg, β = 5°/min, total flow 100 cm3/min). The qualitative composition of the gas phase was determined using on-line QMS in multiple ion detection mode from the intensity of ions of m/z = 18 (H2O), 32 (O2), 44 (CO2), and 28 (CO). Calibration of the sensor sensitivity by heat flow was performed by measuring the heat capacity of a standard sapphire disk using the method in [31]. The reduction degree of hematite was calculated from the mass loss with the recalculation of the removed lattice oxygen amount, the degree of 100% reduction corresponds to the oxygen removal from the lattice α-Fe2O3 when reduced to metal, the degrees of 11.1 and 33.3% reduction correspond to the reduction of hematite to magnetite and wüstite.

3. Results and Discussion

3.1. Reactivity of Calcined α-Fe2O3 Samples in the Temperature-Programmed Reduction by Hydrogen

The reactivity of monophase samples α-Fe2O3 preheated at 800–1100 °C significantly decreases with increasing treatment temperature in temperature-programmed reduction by hydrogen (TPR-H2). Table 1 shows the physicochemical characteristics of the calcined samples (specific surface area SSA, total pore volume Vpore, average particle size Dav, and crystal density DX) and the values of initial reduction temperature (Tin) and temperature of reaching 95% reduction degree (T95%). According to Table 1, the sample calcined at 800 °C shows the most activity and has the lowest temperatures of Tin and T95%.
The calcination temperature of α-Fe2O3 also determines the staging of the reduction process. Figure 1 shows the differential thermo-gravimetric (DTG) and water release (molecular ion mass spectrum with m/z = 18) curves during the reduction of Fe2O3-800 and Fe2O3-1100 samples.
The low-temperature peaks on the DTG and mass spectra (m/z = 18) curves (Figure 1) during the reduction of the Fe2O3-800 sample correspond to the stage of magnetite formation, confirmed by XRD results, according to which, after the reduction at the temperature up to 410 °C, the sample contains 98.8% of Fe3O4 and 1.2% of α-Fe. The second broad peak corresponds to the subsequent combined stages of oxides reduction to metal. Increasing the calcination temperature leads to forming of α-Fe2O3 samples whose reactivity regarding hydrogen significantly decreases; the reduction process of α-Fe2O3 begins at temperatures 50–100 °C higher (Table 1). The reduction of α-Fe2O3 samples calcined at 1000–1100 °C occurs without the magnetite formation stage and does not end at 900 °C (Figure 1).
It is known that it is possible to change the oxidizing ability of transition metal oxides by activating the Me-O bond. One of the methods is the modification of oxide by other cations to create a defective structure [32]. In our work, we used hematite samples from high-purity qualification reagents, and a change in their reactivity with respect to hydrogen is associated with structural features that are due to the temperature factor during the synthesis of samples. Considering that the hematite samples calcined at 800–1100 °C are monophase, we may assume that the decrease in oxygen reactivity regarding hydrogen is associated with the increase in lattice oxygen binding energy due to forming more ordered bulk crystal lattice and surface changes with increasing calcination temperature of α-Fe2O3.
To reveal the effect of calcination temperature of monophase α-Fe2O3 samples on the degree of disorder/violation of the near-order in the crystal lattice and the surface chemical state, the samples calcined in the range of 800–1100 °C were investigated using Raman spectroscopy and XPS.

3.2. Examination of Calcined α-Fe2O3 Samples using Raman Spectroscopy

Figure 2 shows images of α-Fe2O3 samples grains, calcined in the interval of 800–1100 °C, obtained with a microscope attachment in the Raman spectrometer. All samples are represented by particles of two types distinguishable by color under imaging conditions with assigned color codes “red” and “green.” Here, the ratio of particles changes with the calcination temperature. Smaller “red” particles practically completely cover the particles of the low-temperature Fe2O3-800 sample, under which one can see “green” particles.
As the calcination temperature increases, the size of “red” particles increases (Figure 2), their contribution significantly decreases (Figure 3), and mainly “green” particles represent the high-temperature Fe2O3-1100 sample. The proportion of surface “red” particles was calculated as the area of red regions relative to the sum of the red and green regions from the presented images. We can assume that the presence of two types of particles is due to different types of disorder in the crystal lattice of α-Fe2O3. To clarify the situation, we analyzed the Raman spectra taken from the “green” and “red” particles in the calcined samples of α-Fe2O3 (Figure 4).
The spectra of “green” and “red” particles are close, which indicates phase homogeneity, but as seen from Figure 4a,b, lines in the spectra significantly differ in intensity and magnitude of FWHM (full widths at half maximum), indicating a significant difference in the degree of crystallinity phase in particles. According to the literature data, all registered peaks are characteristic of α-Fe2O3. Thus, the calculated Raman spectrum of α-Fe2O3 in the region up to 700 cm−1 includes seven phonon lines related to transverse (TO) vibrational modes, two A1g modes, and five Eg modes [33,34], which correspond to peaks recorded, respectively, at 225–229 cm−1 and 498–500 cm−1 and at 245–249, 293–295, 298–302, 412–414, and 612–615 cm−1 in the experimental spectra [33,34,35,36]. In the experimental spectra of powder α-Fe2O3 samples, besides TO-mode lines, the lines belonging to the longitudinal (LO) modes are also registered at 660 and 1320 cm−1, respectively [33,35,36,37].
As seen from the spectra of “green” particles shown in Figure 4a, all calculated TO and LO lines of α-Fe2O3 are present with good resolution in all calcined samples in the range of 50–1600 cm−1. The spectrum of Fe2O3-800 contains lines (cm−1) at 226 (A1g), 246 (Eg), 293 (Eg), shoulder at 299 (Eg), 412 (Eg), 497 (A1g), 614 (Eg), 659 (LO), and 1318 (2*LO). Here, with increasing the calcination temperature of α-Fe2O3, the line positions do not change (Figure 4a, 5); however, changes in line intensities (cm−1) at 226 (A1g), 293 (Eg), and the shoulder at 299 (Eg) occur. Small, up to 1.3 times, variations in the intensities of the remaining lines are apparently due to the unequal contribution of different crystal planes on the surface and/or surface roughness [33,36]. In the spectra of “green” particles of low-temperature (800–900 °C) α-Fe2O3 samples, there is an asymmetric broadening of the peaks clearly visible for the peak at 226 cm−1 in the spectrum of the Fe2O3-800 sample (Figure 5). The asymmetry of the peaks practically disappears after the calcination of the samples at 1000–1100 °C. The broadening of the peaks may be due to the size factor observed in the Raman spectra of nanosized particles of α-Fe2O3 in film samples [36].
In the Raman spectra of α-Fe2O3, the line at 225–229 cm−1 (A1g) belongs to the vibrations of iron ions along the c crystallographic axis [35]. Calculation from X-ray diffraction data of the parameter c of the unit cell of α-Fe2O3 calcined samples showed a decrease from 13.7472(1) to 13.7416(1) Å when increasing the calcination temperature from 800 to 1000 °C, and further showed an increase to 13.7438(1) after calcination at 1100 °C [20], which is in inverse correlation with the change in line intensity at 226 cm−1. The ratio of this line intensity to the slightly variable line intensity at 246 cm−1, I226 cm−1/I246 cm−1, increases from 3.4 to 6 with increasing calcination temperature to 1000 °C and decreases to 2.5 after calcination at 1100 °C. The line at 293 cm−1 (Eg) refers to one of the two external vibrations [33]. Its decrease in intensity with increasing calcination temperature of α-Fe2O3 (Figure 5) probably relates to the decrease in surface/volume ratio with increasing crystallite size.
It is worth noting that in the spectra of “green” particles of all investigated α-Fe2O3 samples, the LO mode line at 659 cm−1 is registered (Figure 4a). This mode is prohibited in the Raman spectrum of α-Fe2O3, and the activation of this mode, as noted in several studies, is due to the presence of structural disorder/defectivity in the crystal lattice [33,35,36,37]. Note that in the 667–670 cm−1 region, the magnetite phase also has the Raman line (A1g) [36,37,38]. However, the authors of [37], based on comparing the spectra of the hematite and mixed magnetite with hematite samples, unambiguously attribute this line to the LO hematite mode activated due to the structural disorder. Considering the above data and the monophasic nature of the calcined samples α-Fe2O3 (by XRD), we can argue that the peak at 659 cm−1 in the Raman spectra of “green” particles of all samples is due to the disorder in the α-Fe2O3 crystal lattice. Registration in the spectra of an intense line at 1318 cm−1 (Figure 4a) (double the value of the LO mode wave number), which refers to the vibrational mode 2*LO, is consistent with the results of [33,38], in which the study of hematite samples also used green laser (514.5, 532.2 nm) for excitation and this intense line was recorded. The authors associate the significant intensity of this line with the resonance excitation effect.
The Raman spectra analysis of “red” particles (Figure 4b), as already mentioned, shows their correspondence also to the spectrum of α-Fe2O3 oxide, while there are features compared with the spectra of α-Fe2O3 “green” particles. All peaks have lower ~8–10-fold intensity and higher ~3–5-fold FWHM values, unresolved peaks in the 290 cm−1 region, and an observed shift of all peaks to lower values of wave numbers for high-temperature samples (except for the line at 662 cm−1) by 5–10 cm−1 and for low-temperature samples by 15–25 cm−1. The peak at 662 cm−1 attracts attention, being registered only in the spectra of high-temperature samples with the position shifted toward higher wave number values, unlike the other lines. Perhaps, the peak at 662 cm−1 is a superposition of the LO mode of hematite and the most intense in this region of the magnetite mode (A1g). The LO mode wave number of hematite based on 1306 cm−1 for the 2LO mode must have the value of 653 cm−1, i.e., the LO peak, as well as other peaks in the spectra of α-Fe2O3 “red” particles of high-temperature samples, is shifted to lower values of the wave number compared with the peaks of α-Fe2O3 “green” particles.
Thus, the study of α-Fe2O3 samples calcined in the interval of 800–1100 °C using Raman spectroscopy allows us to draw the following conclusions. All samples consist of two types of particles represented by the α-Fe2O3 phase differing in crystallite size, degree of crystallinity, and presence of disorder in the crystal lattice. “Red” particles that are smaller are located on the surface of larger “green” ones. In large particles, the α-Fe2O3 phase is well crystallized, and there is a disorder in the crystal lattice, as evidenced by the LO mode at 659 cm−1. Surface particles also consist of the α-Fe2O3 phase with a lower degree of crystallinity and smaller crystallites; the size of the particles increases with increasing sample calcination temperature with an overall decrease in their content. In the surface particles of high-temperature (1000–1100 °C) samples, along with the phase of α-Fe2O3, which has a disorder in the crystal lattice similar to large particles, traces of the magnetite phase are also possible.

3.3. Study of the α-Fe2O3 Surface in Calcined Samples

The influence of the calcination temperature on the surface state of α-Fe2O3 was also investigated using the XPS method. Analysis of the survey spectra lines in the 0–1150 eV range showed primary (Fe, O) and impurity (C, Si) elements, Si appeared due to the procedure of grinding sintered samples (see the footer Table 2) and C was revealed to be present as elementary carbon and carbonate species on the surface of the sample. Table 2 shows the calculated surface composition of the calcined samples of α-Fe2O3.
The valence states of the elements were estimated from the XPS spectra on the base of the peak position in the spectrum together with the elastic peak/satellite combination [39,40,41,42,43]. For this purpose, we decomposed the integral lines into elementary doublets in the case of Fe2p spectra and into individual singlet peaks in the case of O1s and C1s spectra. Considering the Raman results, we decomposed the Fe2p spectra using the literature data on the positions of the main doublets and their shake-up satellites for the Fe2+ and Fe3+ states, i.e., two doublets from Fe2+ with Eb(Fe2p3/2)~710 and 714 eV and two doublets from Fe3+ with Eb(Fe2p3/2)~711.5 and 719 eV. Table 3 shows the positions of the elementary components of the Fe2p spectra, which agree well with the literature data [39,40,41,42].
Figure 6 shows, as an example, the Fe2p spectra with their decomposition for samples Fe2O3-900 and Fe2O3-1100. Analysis of the Fe2p spectra showed that the characteristics of Fe2+ and Fe3+ ions are clearly visible in spectra for all samples. The calculation of the surface composition of hematite samples calcined at 800–1100 °C indicated the deviation from the stoichiometric composition of the Fe2O3 phase. The ratio of the integral intensity of doublets associated with the Fe2+ state to the total area of all doublets of the Fe2p line determined the proportion of Fe2+ ions on the surface of calcined hematite samples. In samples calcined at temperatures of 800–900 °C, the Fe2+/Fe ratio was 0.36–0.38 (0.37–0.42 at 1000–1100 °C), which is higher than the value of 0.33 for the stoichiometric composition of Fe3O4 oxide.
Knowing that iron oxide with the α-Fe2O3 structure has high structural stability, at high temperatures, there is a slight deviation from oxygen stoichiometry, and the hematite lattice is oxygen deficient: α-Fe2O3-ε, where ε is a positive value due to the preferential formation of anion vacancies [44,45]. At 1100 °C, ε is 2⋅10−5, and at 1300 °C—7.73⋅10−4, respectively, at lgPO2 (atm.) = −0.843 and −0.846 [44]. Compared with the bulk, the concentration of anionic vacancies in the surface/subsurface layers of hematite is higher [46], and the deviation from stoichiometry becomes present already at temperatures above 600 °C [47].
Based on the above data, the reason for the observed partial reduction in the surface/subsurface layers of α-Fe2O3 after calcination at temperatures of 800–1100 °C and the increase in the content of Fe2+ ions with increasing temperature is the process of removing oxygen from the α-Fe2O3 lattice, which leads to the formation of anion vacancies and stabilization of Fe2+ cations due to localization of electrons at Fe3d levels [45,48,49].
Enriching the surface of α-Fe2O3 calcined samples with low-valent iron ions should decrease the surface O/Fe ratio. However, the evaluation from XPS showed that the O/Fe ratio (when calculating the pure O/Fe ratio, the stoichiometry of O/Si was taken into account) on the surface of calcined samples increases with increasing calcination temperature up to 1000 °C, then slightly decreases (Figure 7a). Only for the low-temperature Fe2O3-800 sample, the O/Fe value is close to the composition of Fe2O3, for the rest samples, it is much higher.
The obtained O/Fe values testify to the presence of other oxygen forms in addition to the lattice oxygen, also confirmed by the complex shape of the O1s peak with a pronounced shoulder on the side of higher binding energies (Figure 8). To determine the fraction of out-of-lattice oxygen forms, the integral O1s spectra were decomposed into their components. Figure 8 shows the decomposition of the O1s XPS spectra for samples Fe2O3-900 and Fe2O3-1100. Here, the integral O1s peak shows a good decomposition into three elementary A, B, and C peaks with Eb(O1s)~529.7, 531.6, and 532.6 eV, respectively, with the positions shown in Table 3 for all samples. The peaks with Eb(O1s)~529.7 eV relate to the lattice oxygen in iron oxides, while peaks with higher Eb values relate to oxygen states of surface layers in which coordination and oxygen state differ from oxygen location in the bulk phase of oxide. The Eb values of these oxygen states correspond to the surface hydroxyl and carbonate groups [49,50], which can result from the interaction of water vapors and CO2 with the reactive surface centers in the post-synthetic period.
Hydroxylation of the α-Fe2O3(0001) surface occurs at low (~10−8 torr) water vapor pressures, forming several types of hydroxyl groups as known from [50]. According to calculations made in [49], the chemisorption of water vapor on a defective surface, specifically on anion vacancies, is preferable. The formation of mono- and bidentate carbonate and bicarbonate groups occurs during the carbon dioxide adsorption on the hematite surface according to [50,51,52], and this formation proceeds more efficiently in the presence of hydroxyl groups [51,52].
On the surface of the studied α-Fe2O3 calcined samples, the proportion of out-of-lattice oxygen forms was estimated from the ratio of the sum of the areas of peaks B and C to the total O1s spectrum area (O(B) + O(C)/Ototal). Figure 7b shows that the proportion of out-of-lattice oxygen forms significantly increases from 0.27 to 0.37 with increasing calcination temperature of α-Fe2O3 samples. There is a correlation between the content of surface out-of-lattice oxygen forms and the content of Fe2+ ions well explained by the change in the proportion of removed lattice oxygen from α-Fe2O3, which increases with increasing calcination temperature. Here, the concentration of surface defect centers increases, in particular, of anion vacancies, which are centers of water adsorption, localized Fe2+ ions, and specific centers of CO2 adsorption. Some decrease in the ratio of O(B) + O(C)/Ototal from 0.37 to 0.35 for the Fe2O3-1100 sample is likely due to partial ordering and crystallization of the surface phases.
Thus, investigating the surface of α-Fe2O3 samples calcined in the air in the temperature range of 800–1100 °C using the XPS method showed that the calcination temperature affects the surface chemical composition. With increasing calcination temperature, the surface enrichment with Fe2+ ions occurs, which agrees with the Raman results and the increase, compared with the stoichiometric value for the hematite phase, of the O/Fe ratio due to the significant contribution of the proportion of out-of-lattice (hydroxyl and carbonate) oxygen forms.
Based on the set of the obtained study results of α-Fe2O3 samples calcined in the interval of 800–1100 °C, the effect of high-temperature pretreatment on the morphological characteristics, chemical state of the surface, microstructural parameters, and the lattice oxygen reactivity regarding hydrogen was established.
According to X-ray diffraction data, all samples are represented by the α-Fe2O3 phase, in which crystal density value monotonically increases with increasing calcination temperature.
According to XPS results, on the surface of all α-Fe2O3 calcined samples, low-valent Fe2+ ions and out-of-lattice (hydroxyl and carbonate) forms of oxygen present, which proportion increases with increasing α-Fe2O3 calcination temperature.
According to Raman spectroscopy results, all samples consist of two types of particles represented by the α-Fe2O3 phase with differences in the size of crystallites, degree of crystallinity, and disorder of the crystal lattice. Small particles, consisting of crystallites with a lower degree of crystallinity, are on the surface of larger particles with a well-crystallized α-Fe2O3 phase. With increasing calcination temperature of α-Fe2O3 samples, the proportion of surface particles decreases, and their size increases. Traces of the magnetite phase are registered in the surface particles of the samples calcined at 1000–1100 °C. The crystal lattice of well-crystallized α-Fe2O3 crystallites of all the calcined samples has a disorder evidenced by activating the prohibited in the Raman spectra LO mode at 659 cm−1. For these crystallites, there is an inverse correlation between the intensity at the 226 cm−1 (A1g) line, which belongs to the vibrations of iron ions along the c crystallographic axis, and the unit cell parameter (c) calculated from X-ray diffraction data.
The observed differences in the structural features and the surface state of α-Fe2O3 samples calcined at 800–1100 °C make it possible to conclude that the main reason for the low reactivity of high-temperature α-Fe2O3 samples (Fe2O3-1000 and Fe2O3-1100) regarding hydrogen is due to the formation of α-Fe2O3 samples with a denser crystal lattice and with the surface enriched with Fe2+ iron ions, which deactivate Fe-O bond.

4. Conclusions

This paper studied the relationship between the textural and microstructural characteristics and the surface state of α-Fe2O3 samples calcined in the temperature range of 800–1100 °C with the activity of these samples regarding hydrogen in the TPR mode in the range of 40–900 °C.
It was found that the oxygen reactivity of α-Fe2O3 regarding hydrogen decreases with increasing calcination temperature of the samples.
All samples of hematite are monophase and represented by the α-Fe2O3 phase. With an increase in the calcination temperature from 800 to 1100 °C, the crystal density of the phase increases from 5.2704(1) to 5.2713(1) g/cm3.
According to the Raman spectroscopy results, all samples consist of two types of particles: large, with a well-crystallized α-Fe2O3 phase; and smaller particles, which are on the surface, also represented by the α-Fe2O3 phase with a significantly lower degree of crystallinity. Based on the registration of the line at 659 cm−1 (LO mode) prohibited in the Raman spectrum of α-Fe2O3, we can identify the presence of a close type of crystal lattice disorder in large particles of all calcined samples. There are traces of magnetite in small particles in the samples calcined at 1000–1100 °C.
According to the XPS results, on the surface of all calcined α-Fe2O3 samples, there are Fe2+ ions and out-of-lattice oxygen forms, whose concentrations increase with increasing calcination temperature of samples.
The study results indicate that by increasing the calcination temperature to 1100 °C, the α-Fe2O3 samples form a denser, less disordered crystal oxide lattice with more surface content of Fe2+ ions, which leads to an increase in the binding energy of oxygen (deactivation of the Fe-O bond) and decreased reactivity regarding hydrogen. These results can help develop catalytic systems and oxygen carriers based on α-Fe2O3 for high-temperature catalytic oxidation processes, cyclic processes of fuel combustion, hydrogen generation (CLC, CLGH), etc.

Author Contributions

Conceptualization, A.A.; data curation, E.R., S.K., L.S. and N.S.; investigation, A.K., L.S., S.K., E.R. and N.S.; methodology, N.K.; project administration, N.K.; supervision, A.A.; writing—original draft, N.K., A.K. and A.B.; writing—review & editing, N.K., A.B. and A.A. All authors have read and agreed to the published version of the manuscript.

Funding

This work was conducted within the framework of the budget project for the Institute of Chemistry and Chemical Technology of the Siberian Branch of the Russian Academy of Sciences, Federal Research Center KSC SB RAS, No. FWES–2021–0013.

Institutional Review Board Statement

Not applicable.

Informed Consent Statement

Not applicable.

Data Availability Statement

Not applicable.

Acknowledgments

The reported study was conducted by using the equipment of the Krasnoyarsk Regional Research Equipment Centre of SB RAS for The Raman experiments and SEM.

Conflicts of Interest

The authors declare no conflict of interest.

References

  1. Zhu, M.; Wachs, I.E. Iron-Based Catalysts for the High Temperature Water-Gas Shift (HT-WGS) Reaction: A Review. ACS Catal. 2016, 6, 722–732. [Google Scholar] [CrossRef]
  2. Wagloehner, S.; Reichert, D.; Leon-Sorzano, D.; Balle, P.; Geiger, B.; Kureti, S. Kinetic modeling of the oxidation of CO on Fe2O3 catalyst in excess of O2. J. Catal. 2008, 260, 305–314. [Google Scholar] [CrossRef]
  3. Wagloehner, S.; Kureti, S. Study on the mechanism of the oxidation of soot on Fe2O3 catalyst. Appl. Catal. B Environ. 2012, 125, 158–165. [Google Scholar] [CrossRef]
  4. Yu, Z.; Yang, Y.; Yang, S.; Zhang, Q.; Zhao, J.; Fang, Y.; Hao, X.; Guan, G. Iron-based oxygen carriers in chemical looping conversions: A review. Carbon Resour. Convers. 2019, 2, 23–34. [Google Scholar] [CrossRef]
  5. Cheng, Z.; Qin, L.; Guo, M.; Xu, M.; Fan, J.A.; Fan, L. Oxygen Vacancy Promoted Methane Partial Oxidation over Iron Oxide Oxygen Carrier in Chemical Looping Process. Phys. Chem. Chem. Phys. 2016, 18, 32418–32428. [Google Scholar] [CrossRef] [PubMed]
  6. Qin, L.; Cheng, Z.; Guo, M.; Xu, M.; Fan, J.A.; Fan, L.-S. Impact of 1% Lanthanum Dopant on Carbonaceous Fuel Redox Reactions with an Iron-Based Oxygen Carrier in Chemical Looping Processes. ACS Energy Lett. 2017, 2, 70–74. [Google Scholar] [CrossRef]
  7. Liu, X.; Wang, H. Hydrogen production from water decomposition by redox of Fe2O3 modified with single-or double-metal additives. J. Solid State Chem. 2010, 183, 1075–1082. [Google Scholar] [CrossRef]
  8. Bora, D.K.; Braun, A.; Erat, S.; Safonova, O.; Graule, T.; Constable, E.C. Evolution of structural properties of iron oxide nano particles during temperature treatment from 250 °C-900 °C: X-ray diffraction and Fe K-shell pre-edge X-ray absorption study. Curr. Appl. Phys. 2012, 12, 817–825. [Google Scholar] [CrossRef] [Green Version]
  9. Kryukova, G.N.; Tsybulya, S.V.; Solovyeva, L.P.; Sadykov, V.A.; Litvak, G.S.; Andrianova, M.P. Effect of heat treatment on microstructure evolution of haematite derived from synthetic goethite. Mater. Sci. Eng. A 1991, 149, 121–127. [Google Scholar] [CrossRef]
  10. Breault, R.W.; Yarrington, C.S.; Weber, J.M. The Effect of Thermal Treatment of Hematite Ore for Chemical Looping Combustion of Methane. J. Energy Resour. Technol. 2016, 138, 042202-1–042202-8. [Google Scholar] [CrossRef]
  11. Zhang, J.; Tao He, T.; Wang, Z.; Zhu, M.; Zhang, K.; Li, B.; Wu, J. The search of proper oxygen carriers for chemical looping partial oxidation of carbon. Appl. Energy 2017, 190, 1119–1125. [Google Scholar] [CrossRef]
  12. Riley, J.; Siriwardane, R.; Tian, H.; Benincosa, W.; Poston, J. Kinetic analysis of the interactions between calcium ferrite and coal char for chemical looping gasification applications: Identifying reduction routes and modes of oxygen transfer. Appl. Energy 2017, 201, 94–110. [Google Scholar] [CrossRef]
  13. Cheng, Z.; Qin, L.; Fan, J.A.; Fan, L.-S. New Insight into the Development of Oxygen Carrier Materials for Chemical Looping Systems. Engineering 2018, 4, 343–351. [Google Scholar] [CrossRef]
  14. Zhu, W.; Winterstein, J.; Maimon, I.; Yin, Q.; Yuan, L.; Kolmogorov, A.N.; Sharma, R.; Zhou, G. Atomic Structural Evolution during the Reduction of α-Fe2O3 Nanowires. J. Phys. Chem. C 2016, 120, 14854–14862. [Google Scholar] [CrossRef] [PubMed] [Green Version]
  15. Schöttner, L.; Nefedov, A.; Yang, C.; Heissler, S.; Wang, Y.; Wöll, C. Structural Evolution of α-Fe2O3(0001) Surfaces Under Reduction Conditions Monitored by Infrared Spectroscopy. Front. Chem. 2019, 7, 451. [Google Scholar] [CrossRef] [PubMed]
  16. Shimokawabe, M.; Furuichi, R.; Ishii, T. Influence of the preparation history of α-Fe2O3 on its reactivity for hydrogen reduction. Thermochim. Acta 1979, 28, 287–305. [Google Scholar] [CrossRef]
  17. Lamberov, A.A.; Dementieva, E.V.; Kuzmina, O.V.; Khazeev, B.R. Transformation of the structure of iron oxide (III) during thermal heating in air. Bull. Kazan Technol. Univ. 2013, 16, 37–41. (In Russian) [Google Scholar]
  18. Chen, Z.; Dang, J.; Hu, X.; Yan, H. Reduction Kinetics of Hematite Powder in Hydrogen Atmosphere at Moderate Temperatures. Metals 2018, 8, 751. [Google Scholar] [CrossRef] [Green Version]
  19. Kirik, N.P.; Yumashev, V.V.; Solovyov, L.A.; Rabchevskii, E.V.; Shishkina, N.N.; Anshits, A.G. Influence of Temperature and Duration of α-Fe2O3Calcination on Reactivity in Hydrogen Oxidation. J. Sib. Fed. Univ. Chem. 2023, 16, 66–77. [Google Scholar]
  20. Rouquerol, J.; Rouquerol, F.; Grillet, Y.; Triaca, M. Quasi-equilibrium nitrogen adsorption gravimetry: Comparison with volumetry for the determination of surface areas and pore size distributions. Thermochim. Acta 1986, 10, 89–96. [Google Scholar] [CrossRef]
  21. Lowell, S.; Shields, J.E.; Thomas, M.A.; Thommes, M. Characterization of Porous Solids and Powders: Surface Area, Pore Size, and Density; Springer Science + Business Media: New York, NY, USA, 2004. [Google Scholar] [CrossRef]
  22. de Boer, J.H.; Lippens, B.C.; Lippens, B.G.; Broekhoff, J.C.P.; van den Heuvel, A.; Osinga, T.V. The t-curve of multimolecular N2-adsorption. J. Colloid Interface Sci. 1966, 21, 405–414. [Google Scholar] [CrossRef]
  23. Solovyov, L.A. Full-profile refinement by derivative difference minimization. J. Appl. Crystallogr. 2004, 37, 743–749. [Google Scholar] [CrossRef]
  24. Anshits, A.G.; Bayukov, O.A.; Kondratenko, E.V.; Anshits, N.N.; Pletnev, O.N.; Rabchevskii, E.V.; Solovyov, L.A. Catalytic properties and nature of active centers of ferrospheres in oxidative coupling of methane. Appl. Catal. A General 2016, 524, 192–199. [Google Scholar] [CrossRef]
  25. Knyazev, Y.V.; Tarasov, A.S.; Platunov, M.S.; Trigub, A.L.; Bayukov, O.A.; Boronin, A.I.; Solovyov, L.A.; Rabchevskii, E.V.; Shishkina, N.N.; Anshits, A.G. Structural and electron transport properties of CaFe2O4 synthesized in air and in helium atmosphere. J. Alloys Compd. 2020, 820, 153073. [Google Scholar] [CrossRef]
  26. Seah, M.P. Quantification of AES and XPS. In Practical Surface Analysis, 2nd ed.; Briggs, D., Seah, M.P., Eds.; John Wiley & Sons: Chichester, UK, 1990; Volume 1, pp. 201–255. [Google Scholar]
  27. Wagner, C.D. Handbook of X-ray Photoelectron Spectroscopy; Wagner, C.D., Riggs, W.M., Davis, L.E., Moulder, J.F., Muilenberg, G.E., Eds.; Perkin-Elmer Corp., Physical Electronics Division: Eden Prairie, MN, USA, 1979; 190p. [Google Scholar] [CrossRef]
  28. Moulder, J.F.; Stickle, W.F.; Sobol, P.E.; Bomben, K.D. Handbook of X-ray Photoelectron Spectroscopy; Chastain, J., Ed.; Perkin-Elmer Corp., Physical Electronics Division: Eden Prairie, MN, USA, 1992; Corpus ID: 133719866. [Google Scholar]
  29. Baklanova, N.I.; Zima, T.M.; Boronin, A.I.; Kosheev, S.V.; Titov, A.T.; Isaeva, N.V.; Graschenkov, D.V.; Solntsev, S.S. Protective ceramic multilayer coatings for carbon fibers. Surf. Coat. Technol. 2006, 201, 2313–2319. [Google Scholar] [CrossRef]
  30. Ivanova, A.S.; Slavinskaya, E.M.; Gulyaev, R.V.; Zaikovskii, V.I.; Stonkus, O.A.; Danilova, I.G.; Plyasova, L.M.; Polukhina, I.A.; Boronin, A.I. Metal-support interactions in Pt/Al2O3 and Pd/Al2O3 catalysts for CO oxidation. Appl. Catal. B Environ. 2010, 97, 57–71. [Google Scholar] [CrossRef]
  31. DIN 51007:1994-06; Thermal Analysis; Differential Thermal Analysis. Principles, Deutsches Institut für Normung e. V.: Berlin, Germany, 1994.
  32. Sun, L.; Liang, X.; Liu, H.; Cao, H.; Liu, X.; Jin, Y.; Li, X.; Chen, S.; Wu, X. Activation of Co-O bond in (110) facet exposed Co3O4 by Cu doping for the boost of propane catalytic oxidation. J. Hazard. Mater. 2023, 15, 131319. [Google Scholar] [CrossRef]
  33. Massey, M.J.; Baier, U.; Merlin, R.; Weber, W.H. Effects of pressure and isotopic substitution on the Raman spectrum of a-Fe2O3: Identification of two-magnon scattering. Phys. Rev. B 1990, 41, 7822–7827. [Google Scholar] [CrossRef]
  34. Chamritski, I.; Burns, G. Infrared- and Raman-Active Phonons of Magnetite, Maghemite, and Hematite: A Computer Simulation and Spectroscopic Study. J. Phys. Chem. B 2005, 109, 4965–4968. [Google Scholar] [CrossRef]
  35. Chernyshova, I.V.; Hochella, M.F., Jr.; Madden, A.S. Size-dependent structural transformations of hematite nanoparticles. 1. Phase transition. Phys. Chem. Chem. Phys. 2007, 9, 1736–1750. [Google Scholar] [CrossRef]
  36. Jubb, A.M.; Allen, H.C. Vibrational Spectroscopic Characterization of Hematite, Maghemite, and Magnetite Thin Films Produced by Vapor Deposition. Appl. Mater. Interfaces 2010, 2, 2804–2812. [Google Scholar] [CrossRef]
  37. Bersani, D.; Lottici, P.P.; Montenero, A. Micro-Raman Investigation of Iron Oxide Films and Powders Produced by Sol–Gel Syntheses. J. Raman Spectrosc. 1999, 30, 355–360. [Google Scholar] [CrossRef]
  38. Hanesch, M. Raman spectroscopy of iron oxides and (oxy)hydroxides at low laser power and possible applications in environmental magnetic studies. Geophys. J. Int. 2009, 177, 941–948. [Google Scholar] [CrossRef]
  39. Parkinson, G.S. Iron oxide surfaces. Surf. Sci. Rep. 2016, 71, 272–365. [Google Scholar] [CrossRef] [Green Version]
  40. Wei, L.; Pang, X.; Liu, C.; Gao, K. Formation mechanism and protective property of corrosion product scale on X70 steel under supercritical CO2 environment. Corros. Sci. 2015, 100, 404–420. [Google Scholar] [CrossRef]
  41. Radu, T.; Iacovita, C.; Benea, D.; Turcu, R. X-Ray Photoelectron Spectroscopic Characterization of Iron Oxide Nanoparticles. Appl. Surf. Sci. 2017, 405, 337–343. [Google Scholar] [CrossRef]
  42. Yamashita, T.; Hayes, P. Analysis of XPS spectra of Fe2+ and Fe3+ ions in oxide materials. Appl. Surf. Sci. 2008, 254, 2441–2449. [Google Scholar] [CrossRef]
  43. Fujii, T.; de Groot, F.M.F.; Sawatzky, G.A.; Voogt, F.C.; Hibma, T.; Okada, K. In situ XPS analysis of various iron oxide films grown by NO2-assisted molecular-beam epitaxy. Phys. Rev. B 1999, 59, 3195–3202. [Google Scholar] [CrossRef] [Green Version]
  44. Deckmann, R. Point defects and transport in haematite (Fe2O3-Ɛ). Philos. Mag. 1993, 68, 725–745. [Google Scholar] [CrossRef]
  45. Lee, J.; Han, S. Thermodynamics of native point defects in α-Fe2O3: An ab initio study. Phys. Chem. Chem. Phys. 2013, 15, 18906–18914. [Google Scholar] [CrossRef]
  46. Warschkow, O.; Ellis, D.E. Defects and Charge Transport near the Hematite (0001) Surface: An Atomistic Study of Oxygen Vacancies. J. Am. Ceram. Soc. 2002, 85, 213–220. [Google Scholar] [CrossRef]
  47. Gieitzer, C.; Nowotny, J.; Rekas, M. Surface and Bulk Electrical Properties of the Hematite Phase Fe2O3. Appl. Phys. A 1991, 53, 310–316. [Google Scholar] [CrossRef]
  48. Ling, Y.; Wang, G.; Reddy, J.; Wang, C.; Zhang, J.Z.; Li, Y. The Influence of Oxygen Content on the Thermal Activation of Hematite Nanowires. Angew. Chem. 2012, 124, 4150–4155. [Google Scholar] [CrossRef]
  49. Ovcharenko, R.; Voloshina, E.; Sauer, J. Water adsorption and O-defect formation on Fe2O3 (0001) surfaces. Phys. Chem. Chem. Phys. 2016, 18, 25560–25568. [Google Scholar] [CrossRef] [PubMed] [Green Version]
  50. Yamamoto, S.; Kendelewicz, T.; Newberg, J.T.; Ketteler, G.; Starr, D.E.; Mysak, E.R.; Andersson, K.J.; Ogasawara, H.; Bluhm, H.; Salmeron, M.; et al. Water Adsorption on α-Fe2O3(0001) at near Ambient Conditions. J. Phys. Chem. C 2010, 114, 2256–2266. [Google Scholar] [CrossRef] [Green Version]
  51. Ismail, H.M.; Cadenhead, D.A.; Zaki, M.I. Surface Reactivity of Iron Oxide Pigmentary Powders toward Atmospheric Components: XPS, FESEM, and Gravimetry of CO and CO2 Adsorption. J. Colloid Interface Sci. 1997, 194, 482–488. [Google Scholar] [CrossRef]
  52. Ferretto, L.; Glisenti, A. Study of the surface acidity of an hematite powder. J. Mol. Catal. A Chem. 2002, 187, 119–128. [Google Scholar] [CrossRef]
Materials 16 04466 g001 550
Figure 1. TPR profiles of samples Fe2O3-800 and Fe2O3-1100: DTG curves and MS (m/z = 18) curves in the insert.
Figure 1. TPR profiles of samples Fe2O3-800 and Fe2O3-1100: DTG curves and MS (m/z = 18) curves in the insert.
Materials 16 04466 g001
Materials 16 04466 g002 550
Figure 2. Images of α-Fe2O3 samples calcined in the range of 800–1100 °C.
Figure 2. Images of α-Fe2O3 samples calcined in the range of 800–1100 °C.
Materials 16 04466 g002
Materials 16 04466 g003 550
Figure 3. The proportion of surface “red” particles in dependency of α-Fe2O3 calcination temperature.
Figure 3. The proportion of surface “red” particles in dependency of α-Fe2O3 calcination temperature.
Materials 16 04466 g003
Materials 16 04466 g004 550
Figure 4. Raman spectra of calcined (800–1100 °C) α-Fe2O3 samples, in the range of 50–1600 cm−1: (a) spectra of “green” particles with the phonon peak assignments and (b) spectra of “red” particles.
Figure 4. Raman spectra of calcined (800–1100 °C) α-Fe2O3 samples, in the range of 50–1600 cm−1: (a) spectra of “green” particles with the phonon peak assignments and (b) spectra of “red” particles.
Materials 16 04466 g004
Materials 16 04466 g005 550
Figure 5. Raman spectra of “green” particles, in the range of 180–350 cm−1.
Figure 5. Raman spectra of “green” particles, in the range of 180–350 cm−1.
Materials 16 04466 g005
Materials 16 04466 g006 550
Figure 6. The XPS spectra of Fe2p from the surface of hematite samples and the results of curve fitting procedure: (a) Fe2O3-900 and (b) Fe2O3-1100. The experimental data are shown as blue dots, the results of the spectra fitting are shown as solid green lines, the Fe2p spectra were decomposed with two doublets from Fe2+ (red lines) and two doublets from Fe3+ (black lines).
Figure 6. The XPS spectra of Fe2p from the surface of hematite samples and the results of curve fitting procedure: (a) Fe2O3-900 and (b) Fe2O3-1100. The experimental data are shown as blue dots, the results of the spectra fitting are shown as solid green lines, the Fe2p spectra were decomposed with two doublets from Fe2+ (red lines) and two doublets from Fe3+ (black lines).
Materials 16 04466 g006
Materials 16 04466 g007 550
Figure 7. Dependence of ratios of (a) O/Fe and (b) O(B)+O(C)/O on the α-Fe2O3 calcination temperature.
Figure 7. Dependence of ratios of (a) O/Fe and (b) O(B)+O(C)/O on the α-Fe2O3 calcination temperature.
Materials 16 04466 g007
Materials 16 04466 g008 550
Figure 8. The XPS spectra of O1s from the surface of hematite samples and the results of curve fitting procedure: (a) Fe2O3-900 and (b) Fe2O3-1100. The experimental data are shown as blue dots, the results of the spectra fitting are shown as solid green lines, the O1s spectra were decomposed with three elementary peaks (red, crimson and black lines).
Figure 8. The XPS spectra of O1s from the surface of hematite samples and the results of curve fitting procedure: (a) Fe2O3-900 and (b) Fe2O3-1100. The experimental data are shown as blue dots, the results of the spectra fitting are shown as solid green lines, the O1s spectra were decomposed with three elementary peaks (red, crimson and black lines).
Materials 16 04466 g008
Table
Table 1. Specific surface area, pore volume, average particle size, crystal density of α-Fe2O3, and the temperature values of the initial reduction and 95% reduction degree for calcined hematite samples.
Table 1. Specific surface area, pore volume, average particle size, crystal density of α-Fe2O3, and the temperature values of the initial reduction and 95% reduction degree for calcined hematite samples.
Tcal, °CSSA, m2/gVpore, × 10−4 cm3/gDav, μmDX, g/cm3Tin., °CT95%, °C
8002.1027.4~0.25.2704(1)337630
9000.8111.5-5.2707(1)385668
10000.213.1-5.2711(1)429737
11000.091.6~2.55.2713(1)435812
Vpore is the total pore volume at P/P0 = 0.95, Dav is the average size of crystal grains from SEM image analysis, and DX is the density of α-Fe2O3 from X-ray diffraction data.
Table
Table 2. The concentration of elements in calcined hematite samples (800–1100 °C), the ratios of elements are normalized for iron content.
Table 2. The concentration of elements in calcined hematite samples (800–1100 °C), the ratios of elements are normalized for iron content.
SamplesConcentration of Elements, Atomic Ratios
CΣC(CO3)OΣFeSi *
Fe2O3-8001.210.041.5210.08
Fe2O3-9001.770.131.8210.24
Fe2O3-10002.230.172.1010.21
Fe2O3-11001.590.141.8910.10
* Si is not registered in the sample of the initial hematite reagent, so in the calcined samples, the presence of Si is due to the procedure of grinding sintered samples in the mill to obtain the particle-size fraction.
Table
Table 3. Peak positions of the XPS lines Fe2p, O1s, and C1s (Eb in eV).
Table 3. Peak positions of the XPS lines Fe2p, O1s, and C1s (Eb in eV).
SamplesFe2p3/2O1sC1s
Fe2+Fe3+ABCABC
Fe2O3-800709.9714.1711.5719.0529.7531.6532.6285.0286288.5
Fe2O3-800709.9714.1711.4710.0529.7531.6532.5285.0-288.6
Fe2O3-800709.9714.1711.5718.8529.7531.6532.7284.9-288.6
Fe2O3-1100709.8714.1711.6718.9529.6531.5532.7285.0-288.7
Disclaimer/Publisher’s Note: The statements, opinions and data contained in all publications are solely those of the individual author(s) and contributor(s) and not of MDPI and/or the editor(s). MDPI and/or the editor(s) disclaim responsibility for any injury to people or property resulting from any ideas, methods, instructions or products referred to in the content.

Share and Cite

MDPI and ACS Style

Kirik, N.; Krylov, A.; Boronin, A.; Koshcheev, S.; Solovyov, L.; Rabchevskii, E.; Shishkina, N.; Anshits, A. The Relationship between the Structural Characteristics of α-Fe2O3 Catalysts and Their Lattice Oxygen Reactivity Regarding Hydrogen. Materials 2023, 16, 4466. https://doi.org/10.3390/ma16124466

AMA Style

Kirik N, Krylov A, Boronin A, Koshcheev S, Solovyov L, Rabchevskii E, Shishkina N, Anshits A. The Relationship between the Structural Characteristics of α-Fe2O3 Catalysts and Their Lattice Oxygen Reactivity Regarding Hydrogen. Materials. 2023; 16(12):4466. https://doi.org/10.3390/ma16124466

Chicago/Turabian Style

Kirik, Nadezhda, Alexander Krylov, Andrey Boronin, Sergey Koshcheev, Leonid Solovyov, Evgenii Rabchevskii, Nina Shishkina, and Alexander Anshits. 2023. "The Relationship between the Structural Characteristics of α-Fe2O3 Catalysts and Their Lattice Oxygen Reactivity Regarding Hydrogen" Materials 16, no. 12: 4466. https://doi.org/10.3390/ma16124466

Note that from the first issue of 2016, this journal uses article numbers instead of page numbers. See further details here.

Article Metrics

Back to TopTop