Next Article in Journal
Identification of Marker Compounds and In Vitro Toxicity Evaluation of Two Portuguese Asphodelus Leaf Extracts
Next Article in Special Issue
Solid–Liquid Equilibrium in Co-Amorphous Systems: Experiment and Prediction
Previous Article in Journal
Total Synthesis of Lineaflavones A, C, D, and Analogues
Previous Article in Special Issue
Simultaneous Predictions of Chemical and Phase Equilibria in Systems with an Esterification Reaction Using PC-SAFT
 
 
Search for Articles:
Title / Keyword
Author / Affiliation / Email
Journal
Article Type
 
 
Advanced Search
 
Section
Special Issue
Volume
Issue
Number
Page
 
Journals
Molecules
Volume 28
Issue 5
10.3390/molecules28052371
molecules-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

Density Functional Study on Adsorption of NH3 and NOx on the γ-Fe2O3 (111) Surface

by
Wei Huang
1,
Liang Wang
2,
Lu Dong
1,3,*,
Hongyun Hu
1,3 and
Dongdong Ren
4
1
State Key Laboratory of Coal Combustion, School of Energy and Power Engineering, Huazhong University of Science and Technology, Wuhan 430074, China
2
China Power Hua Chuang (Suzhou) Electricity Technology Research Company Ltd., Suzhou 215125, China
3
Research Institute, Huazhong University of Science and Technology in Shenzhen, Wuhan 430074, China
4
School of Environmental and Municipal Engineering, Qingdao University of Technology, Qingdao 266555, China
*
Author to whom correspondence should be addressed.
Molecules 2023, 28(5), 2371; https://doi.org/10.3390/molecules28052371
Submission received: 8 February 2023 / Revised: 26 February 2023 / Accepted: 1 March 2023 / Published: 4 March 2023
(This article belongs to the Special Issue Exclusive Feature Papers in Physical Chemistry)
Browse Figures
Versions Notes

Abstract

:
γ-Fe2O3 is considered to be a promising catalyst for the selective catalytic reduction (SCR) of nitrogen oxide (NOx). In this study, first-principle calculations based on the density function theory (DFT) were utilized to explore the adsorption mechanism of NH3, NO, and other molecules on γ-Fe2O3, which is identified as a crucial step in the SCR process to eliminate NOx from coal-fired flue gas. The adsorption characteristics of reactants (NH3 and NOx) and products (N2 and H2O) at different active sites of the γ-Fe2O3 (111) surface were investigated. The results show that the NH3 was preferably adsorbed on the octahedral Fe site, with the N atom bonding to the octahedral Fe site. Both octahedral and tetrahedral Fe atoms were likely involved in bonding with the N and O atoms during the NO adsorption. The NO tended to be adsorbed on the tetrahedral Fe site though the combination of the N atom and the Fe site. Meanwhile, the simultaneous bonding of N and O atoms with surface sites made the adsorption more stable than that of single atom bonding. The γ-Fe2O3 (111) surface exhibited a low adsorption energy for N2 and H2O, suggesting that they could be adsorbed onto the surface but were readily desorbed, thus facilitating the SCR reaction. This work is conducive to reveal the reaction mechanism of SCR on γ-Fe2O3 and contributes to the development of low-temperature iron-based SCR catalysts.

1. Introduction

The SCR (selective catalytic reduction) NOx removal technology originated in the 1950s and has realized industrial operation since the 1970s [1]. Nowadays, SCR technology has become the most important and efficient method for NOx removal from flue gas in the industrial field [2]. The SCR reaction is a process of selective reduction of NOx to non-toxic and harmless N2 and H2O by reducing agents, including NH3, CH4, H2, and CO, under specific temperature conditions [3,4]. A catalyst is crucial in the SCR process, which determines the layout and catalytic efficiency of the whole reactor. At present, commercial vanadium–titanium catalysts with good NOx removal efficiency and thermal stability are widely used in the SCR process, in which the V2O5 served as the primary active component. However, the operating temperature of vanadium–titanium catalysts is relatively high (about 330–400 °C), and the V2O5 is toxic, resulting in secondary pollution [5]. Therefore, the development of low-operating-temperature and high-efficiency SCR catalysts has attracted extensive attention from researchers [6,7].
Iron-based SCR catalysts have attracted an increasing amount of attention owing to their remarkable capability to reduce NOx at lower temperatures [8,9,10,11,12]. As early as 1981, Kato et al. [13,14] prepared Fe2O3-TiO2 catalysts by using meta titanic acid (TiO(OH)2·nH2O) and ferric sulfate as precursors. The NOx elimination efficiency of Fe2O3-TiO2 catalysts was over 90%, with a good N2 selectivity at the temperature range from 350 °C to 450 °C. Liu et al. [15,16,17] prepared iron–titanium composite oxide catalysts (FeTiOx) by co-precipitation method with ferric nitrate and titanium sulfate as precursors. The FeTiOx catalyst could remove more than 90% of NOx in flue gas during 250–400 °C and exhibited good resistance to sulfur poisoning and water. Yang et al. [18,19] prepared a Fe-Ti spinel structure catalyst ((Fe3−χTiχ)1−δO4) via the co-precipitation method and tested its NOx removal efficiency. The results showed that the Fe/Ti catalyst exhibited excellent NOx removal performance and good resistance to sulfur poisoning and water. Some researchers have reported that Fe2O3 exhibited a relatively high SCR denitrification activity. Supported Fe2O3 was prepared by Bai et al. [20]; the NOx purification efficiency of this sample with a “tube in tube” structure was higher than 98% at 200–250 °C. Yao et al. [8,9] investigated the NOx elimination characteristics of γ-Fe2O3 in a fluidized bed, and the experiment results indicated that γ-Fe2O3 exhibited an excellent denitrification ability in the temperature range between 200 and 290 °C. Yang et al. [21] confirmed that γ-Fe2O3 exhibited a better de-NOx performance than α-Fe2O3 by denitrification experiments. Liang et al. [22] synthesized nano-γ-Fe2O3 particles for NOx removal and found that more than 85% NOx could be eliminated at 180–330 °C, and the temperature played a positive role in the range of 90–180 °C. Moreover, about 98% NOx could be removed at 240 °C under the aerobic condition. Up to now, there is still much controversy about the mechanism of SCR reaction. Ramis et al. [23,24] and Qi et al. [25] found that the active component in the catalysts responsible for NH3 adsorption might be Lewis acid sites, and the adsorption product would be dehydrogenated to form NH2 species. The NH2 acted as an intermediate species and subsequently reacted with NO to form another intermediate species, and finally N2 and H2O were produced after the intermediate species decomposition. However, Gilardoni et al. [26,27] inferred that NH3 was adsorbed onto the B-acid sites on the V2O5 catalyst surface primarily to generate ammonium ion based on the DFT calculation. Furthermore, Rethwisch et al. [28] discovered that the active sites on the catalyst surface could adsorb NO, as well, resulting in the formation of complex adsorption products. The method of in situ infrared diffuse reflectance spectroscopy was applied to investigate the SCR reaction involved in the γ-Fe2O3 catalyst surface. The results indicated that the L-acid and B-acid sites served as the activate sites which dominated the NH3 and NO adsorption. NH3 was preferentially attracted by the L-acid sites, and NOx underwent an affinity reaction, with the active sites forming complex N-containing species. Therefore, the following conclusion can be drawn that the study of the Fe-based SCR denitrification mechanisms has recently expanded to include research on the NH3 SCR reaction on catalysts. However, as a result of the complexity of the real flue gases, the mechanism of heterogeneous catalytic reaction still lacks a convincing explanation. It is known that the catalytic reaction of the catalyst can always be treated as a “black box” as a result of the difficulty of experimental measurement [29]. In order to comprehend the characteristics of the γ-Fe2O3 catalyst surface and SCR reaction and to identify the active sites responsible for attracting NH3/NOx, a computational study of the interaction between flue gas, such as NH3 and NO, and the γ-Fe2O3 (111) surface, using DFT calculations, was performed in the present work.
It has been agreed that, in the NH3-SCR reaction, the reactants must first be adsorbed onto the catalyst surface and then activated before the reaction. Therefore, there must be two steps during the SCR-NOx eliminating process: the gas molecules must be adsorbed on the catalyst surface, and the reaction must occur between the reactants. The popularly accepted SCR reaction is known as 4NO + 4NH3 + O2 → 4N2 + 6H2O. During the process, the adsorption of reactants such as NH3, NO, and O2, will firstly occur on the catalyst’s surface, and then the oxidation–reduction reaction can take place. Hence, the adsorption of reactants might play a big part in the de-NOx reaction. The formation of N2 and H2O during the SCR process underscores the significance of investigating the adsorption of these molecules onto the catalyst surface, making it an intriguing and worthwhile research avenue to explore. With the improvement of theoretical models used in computational chemistry, a growing number of researchers are applying computational chemistry to simulate the surface mechanism of SCR catalysts and to develop new low-temperature SCR catalysts [30,31]. By DFT simulation, parameters of different adsorption configurations on different catalysts, such as adsorption energy, bond length, and bond angle, can be obtained. The optimal adsorption mode of NOx on the catalyst can thus be obtained, as well, which can provide guidance for the SCR reaction mechanism. As reported in our previous studies, tentative research has been performed to explore the adsorption characteristics of denitration reactants and products on the γ-Fe2O3 (001) surface, indicating that the affinity of these gas molecules varied significantly at different sites on the surface [32]. It has been reported that the γ-Fe2O3 (111) surface is also considered to be a stable and active catalytic surface, which could have a significant impact on the de-NOx process [33]. As far as we know, the adsorption mechanism of the reactants and products in the SCR reaction on the γ-Fe2O3 (111) surface has rarely been investigated.
In this study, the adsorption of reactants (NH3, NOx, and O2), and products (N2 and H2O) over γ-Fe2O3 (111) surface was investigated by using the DFT calculation. The potential active sites on the surface of γ-Fe2O3 (111) were determined, and the corresponding adsorption energies were calculated. By analyzing the electronic transfer and electronic orbitals interaction between gas molecules and the catalyst surface before and after the SCR reaction, we explored the mechanisms of different gas molecules binding with the γ-Fe2O3 (111) surface.

2. Results

2.1. Adsorption of NH3 onto γ-Fe2O3 (111) Surface

NH3, as a reducing agent, plays a big part in the SCR reaction. The adsorption of NH3 could affect the NOx removal activity over the catalyst. The N atom in NH3 molecule contains unbonded lone-pair electrons; thus, NH3 can easily lose electrons and be oxidized. Fe2O3 crystal, with 3d orbitals that have enough space to accept electrons, tends to adsorb reducing gas molecules, such as NH3.
The adsorption configurations of the perfect γ-Fe2O3 (111) surface-adsorbing NH3 are shown in Figure 1. The parameters of optimized configurations of the γ-Fe2O3 (111) surface-adsorbed NH3 molecule, such as adsorption energy, Hirshfeld charge, and Bond length, are showed in Table 1. NH3 could be bonded to the surface with the N atom and H atom. The octahedral and tetrahedral Fe cations served as the main adsorption sites. Figure 1a,b show that the N atom of NH3 was bonded to the tetrahedral Fe site (Fetet) and octahedral Fe site (Feoct), sequentially. Figure 1c shows that the H atom was bonded to the surface via bonding with surface O atom site (Lattice O).
The adsorption energy of configurations (a) and (b) were −8.935 kJ/mol and −90.729 kJ/mol, respectively. It could be found that the octahedral Fe cations were the most active sites, as evidenced by the significantly higher adsorption energy observed in configuration (b), as compared to configuration (a). The Hirshfeld charge of configuration (b) was 0.15 e, suggesting that a large number of electrons were transferred from NH3 to the surface atoms. The octahedral Fe cations could attract more electrons than the tetrahedral Fe cations. Hence, the NH3 was preferred to be adsorbed by octahedral Fe cations, forming stable bonds. The bond length of Fe-N was 2.130 Å, and the bond angle of H-N-H of NH3 was 107.351°, indicating that the bond angle of the NH3 molecule was not changed much after adsorption.
The formation of the hydrogen bond was observed between H atom of NH3 and lattice oxygen on the surface in configuration (c). The adsorption energy was −34.620 kJ/mol, which was less than that in configuration (b), suggesting that a stable hydrogen bond could be formed between the NH3 molecule and γ-Fe2O3 (111) surface, but it was weaker than the Fe-N bond. By analyzing the Hirshfeld charge, we found that the surface lattice oxygen donated electrons to the NH3 molecule, resulting in a net charge of −0.09 e. The bond length of O-H was 1.851 Å, and the bond angle of H-N-H of NH3 was 107.949°, indicating that the bond angle of NH3 was not changed much after adsorption.
To investigate the mechanism of the Fe-N bond formation, the partial density of state (PDOS) of the NH3 and the adjacent Fe atom before and after NH3 adsorption were determined. The PDOS of the most stable configuration (b) was determined as exhibited in Figure 2. It can be found that the NH3 peak underwent a reduction in intensity and a downward shift in energy level as a result of adsorption, which was consistent with the Hirshfeld charge results that NH3 obtains electrons during the adsorption process. An analysis of the NH3 and Fe orbitals revealed that the N atom strongly hybridized with the Fe cation with a resonance peak around −7 eV, and this is indicative of the formation of a stable chemical bond. Effective hybridization between the Fe and N atoms is compelling evidence for the formation of a stable chemical bond, specifically the Fe-N bond, which is responsible for the remarkable adsorption strength of NH3 on the γ-Fe2O3 (111) surface.

2.2. Adsorption of NO onto γ-Fe2O3 (111) Surface

For the SCR reaction over γ-Fe2O3, it is crucial for NO to adsorb onto the surface as the first step. The NO adsorption patterns on the γ-Fe2O3 (111) surface were optimized geometrically, and the resulting parameters can be found in Table 2, with a visual representation in Figure 3. In the configurations 1A, 1B, 1C, and 1D, NO was bonded to the Fe cations with one of its atoms, whereas both N and O atoms were bonded to the surface Fe atoms in the configurations 1E and 1F. The bonding of a nitrogen atom and oxygen atom with tetrahedral Fe cations occurred in configurations 1A and 1B, while configurations 1C and 1D showed bonding between a nitrogen atom and oxygen atom and octahedral Fe cations. In configuration 1E, the N atom bonded with an octahedral Fe cation, while the O atom was linked with a tetrahedral Fe cation. An opposite phenomenon was observed in configuration 1F, as the nitrogen atom and oxygen atom were combined with the tetrahedral Fe cation and the octahedral Fe cation, respectively.
In the configurations 1A–1D, the adsorption energy follows 1A > 1B > 1C > 1D. It can be seen that the N atom preferred to be adsorbed onto both of the two Fe cations to form a stable configuration, which is known as the nitroso acyl compound [34]. When NO was close to the surface, it attracted electrons due to its oxidizability, as the Hirshfeld charge change of NO was negative in these four configurations. The higher electronegativity of the O atom in configurations 1B and 1D resulted in a stronger electron attraction compared to the N atom. The length of the Fe-O bond was longer than that of the Fe-N bond because the N atom radio was smaller than the O atom radio, which could explain the fact that the Fe-N was more stable. In addition, compared with octahedral Fe, NO would attract more electrons when it was adsorbed on the tetrahedral Fe. Thus, more electrons will enter the bonding orbital and form a more stable chemical bond, resulting in a shorter Fe-N bond.
For the purpose of explaining the mechanism of bond formation, the PDOS for configurations 1A–1F was also analyzed, as exhibited in Figure 4. After NO adsorption, it is evident from Figure 4a that the NO molecule orbitals were moved to a less energetic state. Hybrid peaks were observed between the NO orbital and the Fe atom’s p and d orbitals at approximately −6 eV to −8 eV, indicating the formation of a stable adsorption configuration. The same results could be found in configuration 1C. However, compared with Figure 4a, the hybrid peaks were weaker, which could be attributed to the lower adsorption energy of configuration 1C. It could thus be concluded that NO preferred to be adsorbed onto the tetrahedral Fe cation. After adsorption onto configuration 1B, the orbitals of the NO molecule underwent a shift to a less energetic state. The orbital of NO was hybridized with the p and d orbitals of Fe atom at approximately −6 eV~−7 eV. The hybrid peaks were lower in configuration 1B when compared with configuration 1A, suggesting that the Fe-N bond was more stable than the Fe-O bond.
In configurations 1E and 1F, there were two bonds formed. Thus, their adsorption was more stable than that of the configurations 1A and 1B. The adsorption energy of configuration 1F was higher than that of configuration 1E due to the bond between the N atom and tetrahedral Fe being stronger in configuration 1F. As indicated in the PDOS (shown in Figure 4e,f), the orbital of NO atom shift downward, its energy was lowered, and the appearance of hybrid peaks around −6 eV to −8 eV suggested the formation of a chemical bond between the NO and Fe site.

2.3. Adsorption of NO2 onto γ-Fe2O3 (111) Surface

During the SCR process, NO could react with O2 to produce NO2, which could also be adsorbed onto the catalyst’s surface, and then participated in the reaction. Hence, it is also necessary to study the adsorption of NO2 over γ-Fe2O3.
All possible orientations (parallel and perpendicular) and adsorption sites were taken into consideration for the NO2 molecule adsorbed onto the γ-Fe2O3 (111) surface. The optimized and stable configurations are demonstrated in Figure 5. It can be seen that configurations 2A and 2B are linear configurations, in which the NO2 molecule bonded to the surface through one of its O atoms, which was linked to the octahedral Fe and tetrahedral Fe cations separately, and this can be identified as monodentate nitrite [34]. The adsorption energy of configurations 2A and 2B was −250.395 kJ/mol and −240.995 kJ/mol, respectively. NO2 preferred to be adsorbed onto the octahedral Fe cation in linear configurations, but there was not much difference between configurations 2A and 2B. In configuration 2C, both of the two O atoms in the NO2 molecule were connected with the octahedral Fe and tetrahedral Fe cations of the γ-Fe2O3 simultaneously, and this configuration was named bridging bidentate nitrite [29]. The adsorption energy of configuration 2C was −295.858 kJ/mol, which was higher than that of configurations 2A and 2B because two bonds were formed.
In configuration (d), the N atom formed a bond with the octahedral Fe site, with an adsorption energy of −262.002 kJ/mol, which was higher than that of configurations 2A and 2B but still lower than that of configuration 2C. It could be concluded that the Fe-N bond was easily formed, and it was more stable compared with the Fe-O bond. The N-containing compound formed in configuration 2D could be ascribed to the nitro compound [22]. As for configurations 2E and 2F, the N atom and one of the O atoms formed bonds with two Fe atoms, and these kinds of configuration are known as chelating nitro compounds [34]. In configuration 2E, the O atom was bonded to the octahedral Fe cation, and the N atom was bonded to the tetrahedral Fe cation. In configuration 2F, however, the O atom formed a bond with the tetrahedral Fe site, while the N atom was bonded to the octahedral Fe cation. The adsorption energy of configurations 2E and 2F were −329.365 kJ/mol and −345.194 kJ/mol, respectively, which were much higher than those of configurations 2A and 2B. This can be attributed to the fact that there were two bonds formed, in which one bond was the stable Fe-N bond and the other one was the Fe-O bond. The adsorption energy of configuration 2F was a little higher than that of 2E, and this indicated that the octahedral Fe cation had a higher activity to bond to the N atom and formed a stable configuration.
To further understand the mechanism of NO2 adsorption, the PDOS of the corresponding configurations after adsorption (listed in Figure 5) were analyzed, as presented in Figure 6.
In configurations 2A and 2B, the O atom bonded with the Fe cation, and it can be seen that the orbital of the NO2 molecule hybridized with the adjacent Fe atoms at about −7.5 eV and −2.5 eV after adsorption, resulting in a stable chemical bond between NO2 and the catalyst’s surface. In configuration 2C, hybrid peaks between NO2 and both tetrahedral and octahedral Fe sites appeared at −7.5 eV and −2.0 eV, suggesting that the chemical bond was formed between two kinds of Fe cations and NO2 molecules. In configuration 2D, the hybrid peak was also formed because the nitrogen atom of NO2 could also form a stable chemical bond with the Fe atom. As seen from configurations 2E and 2F, both of the N and O atoms were connected with the adjacent Fe atoms simultaneously, and the hybrid peak between the NO2 molecule and tetrahedral and octahedral Fe cations also appeared. It can be seen that NO2 could be attracted by the γ-Fe2O3 (111) surface, with both N and O atoms bonding to the Fe cation and forming a stable chemical bond.
To sum up, the adsorption of NOx, including NO and NO2, can be completed on the γ-Fe2O3 (111) surface. Both NO and NO2 could be attracted by the surface’s active sites, and the N atom and O atom could both bond to the Fe cation on the surface since the orbital of the molecule could be hybridized with the iron oxide surface. In the NOx adsorption process, a number of electrons were transferred from the catalyst’s surface to the gas species because of the oxidizability of NOx. The adsorbed NOx could be formed as the N-related species, such as nitrate, bidentate nitrate, monodentate nitrate, and monodentate nitrite, on the γ-Fe2O3 (111) surface, and this was in accordance with the in situ infrared results in the previous study [22]. According to the analysis of NOx and NH3 adsorption, it can be deduced that the L-H reaction mechanism is suitable for describing the SCR reaction process [35], suggesting that the simultaneous adsorption of ammonia and NO on the γ-Fe2O3 (111) surface existed during the de-NOx reaction. Thus, the SCR denitration process over the γ-Fe2O3 catalyst can easily occur under a lower temperature [27].

2.4. Adsorption of Other Molecules onto the γ-Fe2O3 (111) Surface

In the SCR process, O2, an important reactant, plays an important role, which could promote the NOx removal activity. Studying the adsorption of O2 is conducive to understanding the entire SCR reaction. The configurations of the O2 adsorption onto the γ-Fe2O3 (111) surface were optimized as shown in Figure 7.
Figure 7a depicts the stable configuration in which O2 adsorbed onto the tetrahedral Fe cation, and Figure 7b depicts the stable adsorption of O2 on the octahedral Fe atom. Meanwhile, in the Figure 7c, the two O atoms of the O2 molecule were connected with the tetrahedral and octahedral Fe atoms simultaneously. The adsorption energy of the configurations in Figure 7a–c is −133.470 kJ/mol, −174.754 kJ/mol, and −285.242 kJ/mol, respectively. The adsorption energy of the configuration in Figure 7c is much higher than that of configurations in Figure 7a,b because two chemical bonds were formed in this configuration, as listed in Figure 7c. The adsorption energy of the configuration in Figure 7b was higher than that of configuration in Figure 7a, thus indicating that the octahedral Fe sites were more active than tetrahedral Fe cations during the O2 adsorption process. The Hirshfeld charge analysis showed that the O2 molecule could obtain a lot of electrons from the surface atoms. The Hirshfeld charge calculated in these three configurations was −0.27, −0.25, and −0.32, respectively. It is easy to know that the adsorption mechanism of O2 was identical to that of NO since they were both diatomic molecules. During the process of O2 adsorption, O2 acquired a number of electrons from the γ-Fe2O3 (111) surface, and a stable chemical bond was formed. The results showed that energy was released during the adsorption process, indicating that O2 could be easily adsorbed onto the γ-Fe2O3 (111) surface and that the γ-Fe2O3 (111) surface should exhibit good NOx removal activity.
According to the SCR reaction, N2 and H2O will be generated on the catalyst surface, and their desorption behavior would affect the SCR process. Thus, it is important to study the desorption of N2 and H2O.
The N2 adsorption patterns on the γ-Fe2O3 (111) surface were optimized as illustrated in Figure 8, and the resulting parameters can be found in Table 3. The stable adsorption configurations in Figure 8a,b showed that N2 was adsorbed onto the tetrahedral Fe and octahedral Fe cations, respectively. It could be seen that the Fe cation was the active site for the N2 adsorption process, and the N atom could be bonded with the Fe cation to form a stable chemical bond, such as O2 and NO. The configuration in Figure 8b obtained a much higher adsorption energy (−123.374 kJ/mol) than obtained in Figure 8a, with an adsorption energy of −86.538 kJ/mol, indicating that the octahedral Fe site was more active than the tetrahedral Fe site in relation to N2 adsorption. The Hirshfeld charge of N2 in both configurations was negative, suggesting that electrons were transferred from the catalyst to the N2 atom since the oxidation of N2 occurred. However, compared with the adsorption of NO and O2, we observed that fewer electrons were transferred from N2, and this could be ascribed to the lower oxidizability of the N2 molecule. Therefore, the chemical bond formed during the N2 adsorption onto the γ-Fe2O3 (111) surface was weaker, and the adsorption energy was lower, indicating that N2 could not easily be adsorbed compared with O2 and NO, even though their molecular structures were very similar. In other words, N2, as a product in the SCR process, could be easily desorbed from the γ-Fe2O3 (111) surface, hence contributing to the positive progress of the SCR reaction.
The adsorption configuration of H2O on the γ-Fe2O3 (111) surface was also optimized, as exhibited in Figure 9. The adsorption parameters of these two configurations are shown in Table 4. It is obvious that the O atom of H2O was bonded with the Fe cation on the γ-Fe2O3 (111) surface; the configuration in Figure 9a was H2O adsorbed onto the tetrahedral Fe, and configuration in Figure 9b was H2O adsorbed onto the octahedral Fe cation. Unlike other molecules, a H2O molecule is a nonlinear molecule composed of three atoms. Among the three atoms, the O atoms isolated pairs of electrons, making it easy to lose electrons in the process of adsorption, exhibiting strong reducibility, and showing similar characteristics to ammonia molecule. The Hirshfeld charge results also verified that only a few electrons were transferred from H2O to the γ- Fe2O3 (111) surface in both configurations. The adsorption energy of configurations (a) and (b) were −75.266 kJ/mol and −112.224 kJ/mol, respectively, indicating that H2O could be easily desorbed from the γ-Fe2O3 (111) surface, and this was also beneficial to the positive progress of the SCR reaction.

3. Discussion

It has been verified that both the (001) crystal surface and (111) crystal surface are exposed to the surface of γ-Fe2O3 at the same time, they are the main crystal surfaces of the γ-Fe2O3 catalyst [22]. During the SCR reaction, the relevant gas molecules can be adsorbed and subsequently be reacted on these two surfaces, so both of these two crystal surfaces need to be investigated. The adsorption of gas molecules participating in NH3-SCR reaction on the γ-Fe2O3 (0011) surface has been analyzed in detail in our previous research [32]. Hence, in this study, the adsorption of the reactants (NH3, NOx, and O2), and the products (N2 and H2O) over the γ-Fe2O3 (111) surface was investigated.
On the surface of γ-Fe2O3 (111), the stable adsorption configurations and adsorption energy were determined. Possible binding mechanisms of various gas molecules on γ-Fe2O3 (111) surface after the adsorption reaction were also deduced. As compared with results of the NH3 and NOx molecules adsorbing on the γ-Fe2O3 (001) surface [32], the adsorption energies of N2 and H2O adsorbed on the γ-Fe2O3 (111) surface were smaller than those adsorbed on the γ-Fe2O3 (001) surface, which indicated that the products N2 and H2O generated after NH3-SCR reaction were easier to desorption. This means that the SCR reaction on the γ-Fe2O3 (111) surface should occur more easily.
It should be noted that, after cutting the surface of the γ-Fe2O3 crystal, the surface Fe and O atoms have the possibility of adsorbing hydrogen or hydroxyl groups. It is undeniable that the hydrogen atom or hydroxyl functional group on the surface will affect the adsorption of NOx, NH3, and other gas molecules. In this work, the pre-adsorption of hydroxyl on octahedral Fe and tetrahedral Fe sites was calculated, and its effect on NH3, NOx, and O2 adsorbing onto the γ-Fe2O3 (111) surface was studied. The hydroxyl group was first placed on the γ-Fe2O3 (111) surface, with the oxygen atom close to the octahedral Fe and tetrahedral Fe atoms perpendicular to the surface, and then optimized calculations were performed. The stable configurations are obtained as illustrated in Figure 10.
After the adsorption of -OH, the NH3, NO, NO2, and O2 gas molecules were placed above the other iron atom site on the γ-Fe2O3 (111) surface that was not occupied by -OH. The stable adsorption configurations (3A–3H) are presented in Figure 11, and the adsorption energy of the corresponding configurations are also listed. It can be seen that the pre-adsorption of -OH had an obvious promoting effect on the adsorption of NH3 (configurations 3A and 3B), and the adsorption energy increased from 8.935 and 90.729 kJ/mol of unabsorbed -OH cases to 114.660 and 169.653 kJ/mol of pre-adsorbed -OH cases. For the adsorption of NO (configurations 3C and 3D), NO2 (configurations 3E and 3F), and O2 (configurations 3G and 3H), -OH pre-adsorption has a certain inhibitory effect on the adsorption of these molecules. In particular, the adsorption energy of NO2 and O2 decreased significantly. Therefore, it can be found that the adsorption of hydroxyl groups on the surface has a complex effect on the adsorption of gas molecules participating in the NH3-SCR reaction, and this needs to be further considered in future research.

4. Materials and Methods

The γ-Fe2O3 is generally accepted as a maghemite, as it possesses a spinel-type structure, which bears a striking resemblance to magnetite. The crystal structure of the γ-Fe2O3 unit cell is exhibited in Figure 12, which can be formulated as Fe21.33O32, with a space group of Fd-3m [29,36]. The cubic unit cell has a lattice constant of 0.834 nm and contains 32 O2− anions and 211/3 Fe3+ cations. The Fe cations associated with the octahedral sites are regarded as Feoct, and the Fe cations associated with the tetrahedral sites are regarded as Fetet. Eight Fe3+ cations are located at eight tetrahedral sites, and an additional 131/3 Fe3+ cations are located among sixteen octahedral sites. In addition, every O site in the crystal is occupied [32].
The γ-Fe2O3 (001) and γ-Fe2O3 (111) surfaces are the most widespread surfaces that exist in the γ-Fe2O3 catalyst. During the SCR reaction, these two surfaces could determine the SCR efficiency, the reactants (NH3, NOx, and O2), and the products (N2, H2O) that could be adsorbed on these two surfaces. However, there are few studies about the adsorption of NH3/NOx on the γ-Fe2O3 (111) surface. In our previous studies, the γ-Fe2O3 (001) surface was investigated in detail for the adsorption behaviors of SCR reactants [32,37]. In the present work, the unit cell was firstly optimized, and then, after that, the (111) crystal surface of the γ-Fe2O3 with Feoct and Fetet active sites was identified and treated as the adsorption surface [38]. A p (1 × 1) 7-layer γ-Fe2O3 (111) slab model was built and separated by a vacuum layer of 20 Å to eliminate the interactions between slabs, as shown in Figure 13.
All spin-polarized DFT calculations were performed using the CASTEP (Cambridge Sequential Total Energy Package) program [39]. The generalized gradient approximation (GGA) with the Perdew–Burke–Ernzerhof (PBE) functional was adopted to estimate the exchange–correlation effects [40]. Ionic cores were described by the ultra-soft pseudopotential method. The electronic wave function was expanded in a plane wave basis set with an energy cutoff of 300 eV. The k-point of the Brillouin zone was 4 × 4 × 1 for all calculations [41]. During the calculation, the first 3 layers were totally relaxed, and the remaining layers were fixed for all the structure optimization and energy calculations.
Adsorption energy is generally considered to be a key criterion for evaluating the adsorption ability. A larger adsorption energy indicates a more stable adsorption. The adsorption energy (Eads) of different molecules on the γ-Fe2O3 (111) surface was calculated based on the following expression:
Eads = E(surface+molecule) − (Esurface + Emolecule)
where E(surface+molecule), Esurface, and Emolecule are the total energies of the γ-Fe2O3 (111) surface plus molecule surface system, the pristine γ-Fe2O3 (111) surface, and gas phase molecule, respectively. The reactants (NH3, NOx, and O2) and products (N2 and H2O) were optimized in a 10 Å × 10 Å × 10 Å cell to obtain the corresponding energy (Emolecule). The PDOS and the Hirshfeld charge distribution of different adsorption configurations were performed to uncover the bonding mechanisms.

5. Conclusions

The present work focused on the adsorption mechanism of reactants (NH3, NOx, and O2) and products (N2 and H2O) over the γ-Fe2O3 (111) surface, which is of great significance for the catalytic oxidation of NO. DFT calculations were performed to investigate the adsorption characteristics of these molecules on the γ-Fe2O3 (111) surface. The results indicated that NH3, NO, and NO2 can be effectively adsorbed on the γ-Fe2O3 (111) surface, which is conducive to the de-NOx process. Two kinds of Fe cations, Fetet cation and Feoct cation, existed on the surface, and both of them exhibited a certain reactivity in the case of the adsorption of gas molecules participating in the SCR reaction.
During the NH3 adsorption process, the octahedral Fe site is the most active site, and the N atom has the ability to bind with the two Fe cations to form a stable chemical bond, as demonstrated by the fact that the N atom was strongly hybridized with Fe cation. During the NO adsorption process, both N and O atoms could be bonded to Fetet and Feoct cations. In this case, the N atom exhibits a more stable bond interaction with surface Fe sites than the O atom, and several N-containing species, such as nitrate, bidentate nitrate, etc., are formed. O2 could also establish stable bonds with surface Fe cations by transferring electrons from the iron oxide surface to O2 in three configurations. The adsorption energy of N2 and H2O on γ-Fe2O3 (111) is inferior to that of NH3 and NOx on γ-Fe2O3 (111), which enables H2O and N2, as products, to be easily desorbed from the surface, thus contributing to the positive progress of the SCR reaction.
In addition, the impact of the pre-adsorbed hydroxyl group on the adsorption of molecules such as NH3, NO, NO2, and O2 on the γ-Fe2O3 (111) surface was also investigated. It was found that -OH can be stably bonded to surface Fe cations, which was beneficial to the adsorption of NH3. However, the adsorption of NO, NO2, and O2 molecules was inhibited by -OH to a certain extent. The impact of -OH on the SCR reaction in relation to the γ-Fe2O3 (111) surface would be an interesting research topic in the future.

Author Contributions

Conceptualization, investigation, software, and writing, W.H.; investigation and data curation, L.W.; methodology, software, supervision, writing—review and editing, and fund acquisition, L.D.; supervision, data curation, and validation, H.H.; software and validation, D.R. All authors have read and agreed to the published version of the manuscript.

Funding

This research was funded by the National Natural Science Foundation of China (52206141), Key Projects of Shenzhen Technology Research (JSGG20220831101202005), Key Research and Development Program in Hubei Province (2021BCA157).

Institutional Review Board Statement

Not applicable.

Informed Consent Statement

Not applicable.

Data Availability Statement

Data are available upon request.

Conflicts of Interest

The authors declare no conflict of interest.

References

  1. Nakatsuji, T.; Miyamoto, A. Removal technology for nitrogen oxides and sulfur oxides from exhaust gases. Catal. Today 1991, 10, 21–31. [Google Scholar] [CrossRef]
  2. Bauerle, G.; Wu, S.; Nobe, K. Parametric and durability studies of NOx reduction with NH3 on V2O5 catalysts. Ind. Eng. Chem. Prod. Res. Dev. 1978, 17, 117–122. [Google Scholar] [CrossRef]
  3. Busca, G.; Lietti, L.; Ramis, G.; Berti, F. Chemical and mechanistic aspects of the selective catalytic reduction of NOx by ammonia over oxide catalysts: A review. Appl. Catal. B Environ. 1998, 18, 1–36. [Google Scholar] [CrossRef]
  4. Liu, Z.; Ihl Woo, S. Recent advances in catalytic DeNOx science and technology. Catal. Rev. 2006, 48, 43–89. [Google Scholar] [CrossRef]
  5. Thirupathi, B.; Smirniotis, P. Co-doping a metal (Cr, Fe, Co, Ni, Cu, Zn, Ce, and Zr) on Mn/TiO2 catalyst and its effect on the selective reduction of NO with NH3 at low-temperatures. Appl. Catal. B Environ. 2011, 110, 195–206. [Google Scholar] [CrossRef]
  6. Zhang, L.; Wang, D.; Liu, Y.; Kamasamudram, K.; Li, J.; Epling, W. SO2 poisoning impact on the NH3-SCR reaction over a commercial Cu-SAPO-34 SCR catalyst. Appl. Catal. B Environ. 2014, 156, 371–377. [Google Scholar] [CrossRef]
  7. Li, J.; Chang, H.; Ma, L.; Hao, J.; Yang, R. Low-temperature selective catalytic reduction of NOx with NH3 over metal oxide and zeolite catalysts—A review. Catal. Today 2011, 175, 147–156. [Google Scholar] [CrossRef]
  8. Yao, G.; Wang, F.; Wang, X.; Gui, K. Magnetic field effects on selective catalytic reduction of NO by NH3 over Fe2O3 catalyst in a magnetically fluidized bed. Energy 2010, 35, 2295–2300. [Google Scholar] [CrossRef]
  9. Yao, G.; Gui, K.; Wang, F. Low-Temperature De-NOx by Selective Catalytic Reduction Based on Iron-Based Catalysts. Chem. Eng. Technol. 2010, 33, 1093–1098. [Google Scholar] [CrossRef]
  10. Ramis, G.; Yi, L.; Busca, G.; Turco, M.; Kotur, E.; Willey, R. Adsorption, activation, and oxidation of ammonia over SCR catalysts. J. Catal. 1995, 157, 523–535. [Google Scholar] [CrossRef]
  11. Apostolescu, N.; Geiger, B.; Hizbullah, K.; Jan, M.; Kureti, S.; Reichert, D.; Schotta, F.; Weisweiler, W. Selective catalytic reduction of nitrogen oxides by ammonia on iron oxide catalysts. Appl. Catal. B Environ. 2006, 62, 104–114. [Google Scholar] [CrossRef]
  12. Liu, C.; Yang, S.; Ma, L.; Peng, Y.; Hamidreza, A.; Chang, H.; Li, J. Comparison on the performance of α-Fe2O3 and γ-Fe2O3 for selective catalytic reduction of nitrogen oxides with ammonia. Catal. Lett. 2013, 143, 697–704. [Google Scholar] [CrossRef]
  13. Kato, A.; Matsuda, S.; Nakajima, F.; Imanari, M.; Watanabe, Y. Reduction of nitric oxide with ammonia on iron oxide-titanium oxide catalyst. J. Phys. Chem. 1981, 85, 1710–1713. [Google Scholar] [CrossRef]
  14. Kato, A.; Matsuda, S.; Kamo, T.; Nakajima, F.; Kuroda, H.; Narita, T. Reaction between nitrogen oxide (NOx) and ammonia on iron oxide-titanium oxide catalyst. J. Phys. Chem. 1981, 85, 4099–4102. [Google Scholar] [CrossRef]
  15. Liu, F.; Asakura, K.; He, H.; Liu, Y.; Shan, W.; Shi, X.; Zhang, C. Influence of calcination temperature on iron titanate catalyst for the selective catalytic reduction of NOx with NH3. Catal. Today 2011, 164, 520–527. [Google Scholar] [CrossRef]
  16. Liu, F.; He, H. Structure− Activity Relationship of Iron Titanate Catalysts in the Selective Catalytic Reduction of NOx with NH3. J. Phys. Chem. C 2010, 114, 16929–16936. [Google Scholar] [CrossRef]
  17. Liu, F.; He, H.; Zhang, C. Novel iron titanate catalyst for the selective catalytic reduction of NO with NH3 in the medium temperature range. Chem. Commun. 2008, 17, 2043–2045. [Google Scholar] [CrossRef] [PubMed]
  18. Yang, S.; Guo, Y.; Yan, N.; Wu, D.; He, H.; Qu, Z.; Yang, C.; Zhou, Q.; Jia, J. Nanosized cation-deficient Fe−Ti spinel: A novel magnetic sorbent for elemental mercury capture from flue gas. ACS Appl. Mater. Interfaces 2011, 3, 209–217. [Google Scholar] [CrossRef] [PubMed]
  19. Yang, S.; Li, J.; Wang, C.; Chen, J.; Ma, L.; Chang, H.; Chen, L.; Peng, Y.; Yan, N. Fe–Ti spinel for the selective catalytic reduction of NO with NH3: Mechanism and structure–activity relationship. Appl. Catal. B: Environ. 2012, 117, 73–80. [Google Scholar] [CrossRef]
  20. Bai, S.; Zhao, J.; Du, G.; Zheng, J.; Zhu, Z. In situ modifying of carbon tube-in-tube nanostructures with highly active Fe2O3 nanoparticles. Nanotechnology 2008, 19, 205605. [Google Scholar] [CrossRef]
  21. Yang, S.; Liu, C.; Chang, H.; Ma, L.; Qu, Z.; Yan, N.; Wang, C.; Li, J. Improvement of the activity of γ-Fe2O3 for the selective catalytic reduction of NO with NH3 at high temperatures: NO reduction versus NH3 oxidization. Ind. Eng. Chem. Res. 2013, 52, 5601–5610. [Google Scholar] [CrossRef]
  22. Liang, H.; Gui, K.; Zha, X. DRIFTS study of γFe2O3 nano-catalyst for low-temperature selective catalytic reduction of NOx with NH3. Can. J. Chem. Eng. 2016, 94, 1668–1675. [Google Scholar] [CrossRef]
  23. Ramis, G.; Larrubia, M. An FT-IR study of the adsorption and oxidation of N-containing compounds over Fe2O3/Al2O3 SCR catalysts. J. Mol. Catal. A Chem. 2004, 215, 161–167. [Google Scholar] [CrossRef]
  24. Larrubia, M.; Ramis, G.; Busca, G. An FT-IR study of the adsorption and oxidation of N-containing compounds over Fe2O3-TiO2 SCR catalysts. Appl. Catal. B Environ. 2001, 30, 101–110. [Google Scholar] [CrossRef]
  25. Qi, G.; Yang, R.; Chang, R. MnOx-CeO2 mixed oxides prepared by co-precipitation for selective catalytic reduction of NO with NH3 at low temperatures. Appl. Catal. B Environ. 2004, 51, 93–106. [Google Scholar] [CrossRef]
  26. Gilardoni, F.; Weber, J.; Baiker, A. Mechanism of the vanadium oxide-catalyzed selective reduction of NO by NH3. A quantum chemical modeling. J. Phys. Chem. A 1997, 101, 6069–6076. [Google Scholar] [CrossRef]
  27. Gilardoni, F.; Weber, J.; Baiker, A. Density functional investigation of the mechanism of the selective catalytic reduction of NO by NH3 over vanadium oxide model clusters. Int. J. Quantum Chem. 1997, 61, 683–688. [Google Scholar] [CrossRef]
  28. Rethwisch, D.; Dumesic, J. Adsorptive and catalytic properties of supported metal oxides. 2. Infrared spectroscopy of nitric oxide adsorbed on supported iron oxides. J. Phys. Chem. 1986, 90, 1625–1630. [Google Scholar] [CrossRef]
  29. Guo, P.; Guo, X.; Zheng, C. Roles of γ-Fe2O3 in fly ash for mercury removal: Results of density functional theory study. Appl. Surf. Sci. 2010, 256, 6991–6996. [Google Scholar] [CrossRef]
  30. Rohrbach, A.; Hafner, J. Molecular adsorption of NO on NiO (100): DFT and DFT+ U calculations. Phys. Rev. B 2005, 71, 045405. [Google Scholar] [CrossRef]
  31. Liu, Z.; Ma, L.; Junaid, A. NO and NO2 adsorption on Al2O3 and Ga modified Al2O3 surfaces: A density functional theory study. J. Phys. Chem. C 2010, 114, 4445–4450. [Google Scholar] [CrossRef]
  32. Ren, D.; Gui, K. Study of the adsorption of NH3 and NOx on the nano-γFe2O3 (001) surface with density functional theory. Appl. Surf. Sci. 2019, 487, 171–179. [Google Scholar] [CrossRef]
  33. Bowker, M.; Hutchings, G.; Davies, P.; Edwards, D.; Davies, R.; Shaikhutdinov, S.; Freund, H. Surface structure of γ-Fe2O3 (111). Surf. Sci. 2012, 606, 1594–1599. [Google Scholar] [CrossRef]
  34. Hadjiivanov, K. Identification of neutral and charged NxOy surface species by IR spectroscopy. Catal. Rev. 2000, 42, 71–144. [Google Scholar] [CrossRef]
  35. Yang, Y.; Liu, J.; Du, X.; Ding, J.; Liu, F. Metal–Metal Interactions of Ternary Spinel for Efficient NH3 Selective Catalytic Reduction of NOx at a Low Temperature. Energy Fuels 2020, 34, 15424–15432. [Google Scholar] [CrossRef]
  36. Yang, Y.; Wang, Z.; Miao, S.; Liu, J.; Yu, Y.; Ding, J. Mechanistic landscape of HCl-mediated Hg0 capture by magnetite. J. Phys. Chem. C 2019, 123, 30434–30442. [Google Scholar] [CrossRef]
  37. Ren, D.; Gui, K.; Gu, S. Quantum chemistry study of SCR-NH3 nitric oxide reduction on Ce-doped γFe2O3 catalyst surface. Mol. Catal. 2021, 502, 111373. [Google Scholar] [CrossRef]
  38. Baetzold, R.; Yang, H. Computational study on surface structure and crystal morphology of γ-Fe2O3: Toward deterministic synthesis of nanocrystals. J. Phys. Chem. B 2003, 107, 14357–14364. [Google Scholar] [CrossRef]
  39. Payne, M.; Teter, M.; Allan, D.; Arias, T.; Joannopoulos, J. CASTEP 4.2 Academic version, licensed under the UKCP-MSI Agreement. Rev. Mod. Phys. 1992, 64, 1045–1097. [Google Scholar] [CrossRef] [Green Version]
  40. White, J.; Bird, D. Implementation of gradient-corrected exchange-correlation potentials in Car-Parrinello total-energy calculations. Phys. Rev. B 1994, 50, 4954. [Google Scholar] [CrossRef]
  41. Nayak, S.; Nooijen, M.; Bernasek, S.; Blaha, P. Electronic structure study of CO adsorption on the Fe (001) surface. J. Phys. Chem. B 2001, 105, 164–172. [Google Scholar] [CrossRef]
Molecules 28 02371 g001 550
Figure 1. Stable adsorption configurations of NH3 on Fetet site (a), Feoct site (b), and Lattice O site (c) of the γ-Fe2O3 (111) surface (N, blue; Fe, purple; H, white; O, red).
Figure 1. Stable adsorption configurations of NH3 on Fetet site (a), Feoct site (b), and Lattice O site (c) of the γ-Fe2O3 (111) surface (N, blue; Fe, purple; H, white; O, red).
Molecules 28 02371 g001
Molecules 28 02371 g002 550
Figure 2. The PDOS for the system before and after NH3 adsorption onto the γ-Fe2O3 (111) surface.
Figure 2. The PDOS for the system before and after NH3 adsorption onto the γ-Fe2O3 (111) surface.
Molecules 28 02371 g002
Molecules 28 02371 g003 550
Figure 3. Stable adsorption configurations of NO on the γ-Fe2O3 (111) surface (N, blue; Fe, purple; O, red).
Figure 3. Stable adsorption configurations of NO on the γ-Fe2O3 (111) surface (N, blue; Fe, purple; O, red).
Molecules 28 02371 g003
Molecules 28 02371 g004 550
Figure 4. The PDOS for the system before and after NO adsorption onto the γ-Fe2O3 (111) surface. PDOS of configuration 1A (a), PDOS of configuration 1B (b), PDOS of configuration 1C (c), PDOS of configuration 1D (d), PDOS of configuration 1E (e), PDOS of configuration 1F (f).
Figure 4. The PDOS for the system before and after NO adsorption onto the γ-Fe2O3 (111) surface. PDOS of configuration 1A (a), PDOS of configuration 1B (b), PDOS of configuration 1C (c), PDOS of configuration 1D (d), PDOS of configuration 1E (e), PDOS of configuration 1F (f).
Molecules 28 02371 g004
Molecules 28 02371 g005 550
Figure 5. Stable adsorption configurations of NO2 onto the γ-Fe2O3 (111) surface (N, blue; Fe, purple; O, red).
Figure 5. Stable adsorption configurations of NO2 onto the γ-Fe2O3 (111) surface (N, blue; Fe, purple; O, red).
Molecules 28 02371 g005
Molecules 28 02371 g006 550
Figure 6. The PDOS for the system before and after NO2 adsorption on the γ-Fe2O3 (111) surface. PDOS of configuration 2A (a), PDOS of configuration 2B (b), PDOS of configuration 2C (c), PDOS of configuration 2D (d), PDOS of configuration 2E (e), PDOS of configuration 2F (f).
Figure 6. The PDOS for the system before and after NO2 adsorption on the γ-Fe2O3 (111) surface. PDOS of configuration 2A (a), PDOS of configuration 2B (b), PDOS of configuration 2C (c), PDOS of configuration 2D (d), PDOS of configuration 2E (e), PDOS of configuration 2F (f).
Molecules 28 02371 g006
Molecules 28 02371 g007 550
Figure 7. Stable adsorption configurations of O2 onto Fetet site (a), Feoct site (b), and Fetet site + Feoct site (c) of the γ-Fe2O3 (111) surface (N, blue; Fe, purple; O, red).
Figure 7. Stable adsorption configurations of O2 onto Fetet site (a), Feoct site (b), and Fetet site + Feoct site (c) of the γ-Fe2O3 (111) surface (N, blue; Fe, purple; O, red).
Molecules 28 02371 g007
Molecules 28 02371 g008 550
Figure 8. Stable adsorption configurations of N2 onto Fetet site (a), Feoct site (b) of the γ-Fe2O3 (111) surface (N, blue; Fe, purple; O, red).
Figure 8. Stable adsorption configurations of N2 onto Fetet site (a), Feoct site (b) of the γ-Fe2O3 (111) surface (N, blue; Fe, purple; O, red).
Molecules 28 02371 g008
Molecules 28 02371 g009 550
Figure 9. Stable adsorption configurations of H2O onto Fetet site (a), Feoct site (b) of the γ-Fe2O3 (111) surface (Fe, purple; H, white; O, red).
Figure 9. Stable adsorption configurations of H2O onto Fetet site (a), Feoct site (b) of the γ-Fe2O3 (111) surface (Fe, purple; H, white; O, red).
Molecules 28 02371 g009
Molecules 28 02371 g010 550
Figure 10. Stable adsorption configurations of -OH onto Feoct site (a), Fetet site (b) of the γ-Fe2O3 (111) surface (Fe, purple; H, white; O, red).
Figure 10. Stable adsorption configurations of -OH onto Feoct site (a), Fetet site (b) of the γ-Fe2O3 (111) surface (Fe, purple; H, white; O, red).
Molecules 28 02371 g010
Molecules 28 02371 g011 550
Figure 11. Stable adsorption configurations of NH3 on the -OH pre-adsorbed γ-Fe2O3 (111) surface (N, blue; Fe, purple; H, white; O, red).
Figure 11. Stable adsorption configurations of NH3 on the -OH pre-adsorbed γ-Fe2O3 (111) surface (N, blue; Fe, purple; H, white; O, red).
Molecules 28 02371 g011
Molecules 28 02371 g012 550
Figure 12. The unit cell of γ-Fe2O3, showing the Fe cations (in purple) and oxygen ions (in red).
Figure 12. The unit cell of γ-Fe2O3, showing the Fe cations (in purple) and oxygen ions (in red).
Molecules 28 02371 g012
Molecules 28 02371 g013 550
Figure 13. The side view of γ-Fe2O3 (111) (a) and the top view of γ-Fe2O3 (111) surface (b) (N, blue; Fe, purple; O, red).
Figure 13. The side view of γ-Fe2O3 (111) (a) and the top view of γ-Fe2O3 (111) surface (b) (N, blue; Fe, purple; O, red).
Molecules 28 02371 g013
Table
Table 1. The parameters of optimized configurations of the γ-Fe2O3 (111) surface-adsorbed NH3 molecule.
Table 1. The parameters of optimized configurations of the γ-Fe2O3 (111) surface-adsorbed NH3 molecule.
Adsorption SiteAdsorption Energy (kJ/mol)Hirshfeld Charge (e)Bond Length (Å)
aFeoct−8.9350.102.101
bFetet−90.7290.152.130
cLattice O−34.620−0.091.851
Table
Table 2. The parameters of optimized configurations of the γ-Fe2O3 (111) surface-adsorbed NO molecule.
Table 2. The parameters of optimized configurations of the γ-Fe2O3 (111) surface-adsorbed NO molecule.
Adsorption SiteAdsorption Energy
(kJ/mol)		Hirshfeld Charge
(e)		Fe-N Bond
Length (Å)		Fe-O Bond
Length (Å)
1AFeoct−287.159−0.141.697
1BFeoct−177.547−0.18 1.811
1CFetet−195.665−0.101.701
1DFetet−70.593−0.14 1.802
1EFetet-Feoct−237.602−0.181.9411.851
1DFetet-Feoct−316.855−0.161.7182.002
Table
Table 3. The parameters of optimized configurations of the γ-Fe2O3 (111) surface-adsorbed N2 molecule.
Table 3. The parameters of optimized configurations of the γ-Fe2O3 (111) surface-adsorbed N2 molecule.
Adsorption SiteAdsorption Energy (kJ/mol)Hirshfeld Charge (e)
aFeoct−86.538−0.10
bFetet−123.374−0.08
Table
Table 4. The parameters of optimized configurations of the γ-Fe2O3 (111) surface-adsorbed H2O molecule.
Table 4. The parameters of optimized configurations of the γ-Fe2O3 (111) surface-adsorbed H2O molecule.
Adsorption SiteAdsorption Energy (kJ/mol)Hirshfeld Charge (e)
aFeoct−75.2660.09
bFetet−112.2240.11
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

Huang, W.; Wang, L.; Dong, L.; Hu, H.; Ren, D. Density Functional Study on Adsorption of NH3 and NOx on the γ-Fe2O3 (111) Surface. Molecules 2023, 28, 2371. https://doi.org/10.3390/molecules28052371

AMA Style

Huang W, Wang L, Dong L, Hu H, Ren D. Density Functional Study on Adsorption of NH3 and NOx on the γ-Fe2O3 (111) Surface. Molecules. 2023; 28(5):2371. https://doi.org/10.3390/molecules28052371

Chicago/Turabian Style

Huang, Wei, Liang Wang, Lu Dong, Hongyun Hu, and Dongdong Ren. 2023. "Density Functional Study on Adsorption of NH3 and NOx on the γ-Fe2O3 (111) Surface" Molecules 28, no. 5: 2371. https://doi.org/10.3390/molecules28052371

Article Metrics

Back to TopTop