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Article

Promotional Effect of Pt-Doping on the Catalytic Performance of Pt−CeO2 Catalyst for CO Oxidation

by
Angran Jiang
1,
Zhibo Ren
2,
Yaqi Qu
1,
Yanjun Zhang
1 and
Jianwei Li
1,*
1
State Key Laboratory of Chemical Resources Engineering, Beijing University of Chemical Technology, Beijing 100029, China
2
Huaneng Clean Energy Research Institute, Beijing 102209, China
*
Author to whom correspondence should be addressed.
Catalysts 2022, 12(5), 529; https://doi.org/10.3390/catal12050529
Submission received: 13 March 2022 / Revised: 16 April 2022 / Accepted: 27 April 2022 / Published: 9 May 2022
(This article belongs to the Section Catalytic Materials)
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Abstract

:
Growing interest in the development of a hydrogen economy means that CO oxidation is increasingly important for upgrading H2-rich fuel gas streams for fuel cells. CeO2-supported catalysts are the most promising candidates for the catalytic oxidation of CO because of their high activity. In the present work, DFT+U calculations were performed to investigate the stability and CO oxidation reactivity of Ptn (n = 1−4) clusters supported on CeO2(111) (Pt/CeO2) and Pt-doped CeO2(111) (Pt/(Pt−Ce)O2) surfaces. The Pt clusters showed similar nucleation behavior on both CeO2 and (Pt−Ce)O2 surfaces. Further, the formation of oxygen vacancies (Ov) was facilitated because of surface charge depletion caused by the dopant Pt. Our DFT results suggest that the interfacial OV plays an important role in the CO oxidation reaction cycle, and the calculated energy barrier for the CO oxidation reaction on the Pt/(Pt−Ce)O2 surface is approximately 0.43 eV lower than that on the surface of the undoped catalyst, suggesting enhanced CO oxidation reactivity. Therefore, the chemical modification of the CeO2 support via doping is an effective strategy for improving the catalytic performance of Pt/CeO2.

1. Introduction

Cerium oxide (CeO2)-based catalysts have been widely used in many catalytic processes, such as the water–gas shift reaction [1], methanol synthesis [2], and CO oxidation [3]. CO oxidation is becoming increasingly important to remove CO from reformate streams to obtain fuel-cell-grade hydrogen [4,5]. Pt-group metals supported on reducible oxides, such as TiO2 [6] and CeO2, are regarded as promising low-temperature CO removal catalysts [7]. Thus, CeO2-supported Pt catalysts and their role in CO oxidation have drawn extensive interest both experimentally and theoretically. Boronin et al. synthesized Pt/CeO2 catalysts having a range of Pt loadings, and the 8 and 20 wt% Pt catalysts were found to convert 60% and 90% of CO below 0 °C because of the synergistic reaction between ionic platinum and nanostructured ceria [8]. The superior activity of high Pt loading catalyst was attributed to a high concentration of Pt ions, with a fraction of the ionic Pt content aggregated into clusters. Liu et al. investigated CO oxidation on CeO2(111)-supported Pd-based bimetallic nanorods using density functional theory (DFT) and found that the formation of a bimetallic system having complementary chemical properties was effective for tuning the catalytic activity [9]. In particular, the superior activity of CeO2-supported catalysts lies in their high oxygen storage capacities [10] and strong metal–support interactions [11], which not only lowers the oxygen vacancy formation energy (Evac) on the CeO2 surface but also facilitates CO oxidation via the Mars–Van Krevelen (M-VK) mechanism [12]. On the other hand, the metal–support interaction can stabilize the metal clusters on the surface of the support [13], which results in excellent anti-sintering performance under reactive conditions.
As previously reported, small Pt clusters supported on the CeO2 surface provide active sites for CO oxidation and show higher activity than atomically supported Pt atoms [14,15]. In particular, the surface oxygen atoms at the Pt/CeO2 interface play an extremely important role during the CO oxidation process. Lu et al. found that CO adsorbs strongly on Pt clusters, whereas the highly active lattice oxygen sites near the Pt clusters overcome the strong bonds of CO adsorbed on the Pt cluster [16]. Many attempts have been made to enhance the activity of the metal–oxide interface, for example, by adjusting the size of metal clusters and creating surface oxide defects near the clusters [17]. Recently, computational evidence has suggested that the doping of the CeO2 support is a promising way to accelerate CO oxidation at the metal–support interface [18].
The doping of the CeO2 surface with metals is reported to reduce the oxygen vacancy formation energy of nearby surface oxygen atoms significantly [19]. The oxygen vacancy formation energy varies with the position of the dopant in the periodic table [20]—when low-valence metals are doped on the surface of CeO2, fewer electrons are transferred to the surrounding oxygen atoms than from Ce4+, which results in electron depletion in the CeO2 support. This further weakens the bonds between electrophilic oxygen atoms and the surface atoms and reduces the oxygen vacancy formation energy, Evac [21]. Hu et al. [22] studied the effects that reduce the oxygen vacancy formation energy on the insertion of metal atoms on the surface of CeO2 and found that the doping of the CeO2 support with low-valence metals, such as Y and La, can reduce the oxygen vacancy formation energy in the long range. In contrast, the high valence dopants, such as Pt and Zr, just create a weak electron deficit in the CeO2(111) surface, and the oxygen vacancy formation energy is only reduced near the surface [23].
In the present work, the influence of doping Pt/CeO2 catalyst with a heterometal (Pt) was investigated using DFT calculations. Firstly, we identified the most stable Pt-doped CeO2(111) surface structure. Secondly, the adsorption and nucleation of the supported Ptn (n = 1−4) clusters were explored. Finally, the structural changes and energies of oxygen vacancy formation and CO oxidation on the Pt-support interface were studied to gain insights into the catalytic activity of the small CeO2-supported Pt clusters.

2. Results

2.1. Structures of Pristine and Pt-doped CeO2(111) Surface

A model of the CeO2(111) surface doped with Pt was obtained by replacing a single surface Ce4+ ion with a Pt4+ ion. Two stable structures were then found, namely (Pt−Ce)O2_I, in which the dopant Pt atom has a square planar structure, and (Pt−Ce)O2_II, in which the Pt atom has a regular octahedral structure (Figure 1); these structures are similar to those reported by Su et al. [24]. In fact, the total energy of the (Pt−Ce)O2_II structure is 0.54 eV lower than that of the (Pt−Ce)O2_I structure, indicating the (Pt−Ce)O2_II structure is thermodynamically more favorable [25]. The radii of the Pt4+ (0.77Å) is a little smaller than that of the Ce4+ (0.97Å) [12]; thus, the dopant Pt is more inclined to form an octahedral structure. Therefore, the (Pt−Ce)O2_II model structure was used in the following studies and is denoted as (Pt−Ce)O2 in subsequent sections.

2.2. Stability of Ptn Clusters

Next, in the computational model, Pt1–4 clusters were loaded onto the perfect CeO2 and (Pt−Ce)O2 surfaces to enable the investigation of the interaction between Pt clusters and different support surfaces. The doped Pt cations were supposed to be a nucleation center for supported Pt nanoparticles and Pt clusters formed at positions where Pt2+ is doped into the framework. Once acting as a nucleation center for supported metal nanoparticles, dopants such as Ni, Pd, Pt, and Rh cannot activate lattice O atoms [24]. Therefore, Pt clusters were deposited on the neighboring site of Pt dopant to study its short range doping effect as in the previous study [18]. The most stable adsorption structures in terms of thermodynamics for each composition and adsorption energies are shown in Figure 2. As shown, a single Pt atom preferentially adsorbs close to O-hollow site between two O anions on both CeO2(111) and the (Pt−Ce)O2 surfaces, having adsorption energies of −2.84 and −3.06 eV, respectively. Consistent with the results of previous studies, the adsorption of the Pt2 dimer on the O-O bridge site is more stable than that of an isolated Pt atom on both support surfaces [26]. The adsorption energy of Pt2 on clean CeO2(111) is −2.97 eV, which is larger than that on the (Pt−Ce)O2 surface. For Pt3 on both surfaces, a flat triangular Pt cluster in which each Pt atom forms a close interaction with the surface O atoms of CeO2 is the most relatively stable structure. However, in the triangular structure, one of the Pt atoms forms a shorter Pt-O bond, 1.84 Å (the others are 1.92 and 1.95 Å). The adsorption energies of the supported Pt3 cluster on both surfaces are lower (by about 1 eV) than that of the Pt2 cluster adsorbed on the same surfaces. When we modeled the adsorption of four Pt atoms on both surfaces, a tetrahedral configuration was formed; in this structure on both surfaces, three Pt atoms interact with the surfaces through Pt-O bonds, and the remaining Pt atom is located at the top vertex pointing away from the support surface.
The DFT calculations show that the Ptn (n = 1–4) clusters adsorbed on the CeO2(111) and (Pt−Ce)O2 surfaces have similar adsorption energies, but that on the doped surface is slightly lower than that on the pristine surface. In addition, as the number of Pt atoms in the Ptn cluster increases, the difference between the adsorption energies on the CeO2(111) and (Pt−Ce)O2 surfaces gradually decreases. These results suggest that the metal dopants do not significantly affect the stability of the supported Pt clusters.
As shown in Figure 3, the nucleation energy with respect to the size of the Ptn (n = 1–4) clusters adsorbed on both CeO2 and (Pt−Ce)O2 surfaces show similar trends. The negative nucleation energy indicates an exothermic process, and the cluster tends to aggregate. As seen in the Figure 3, Pt clusters supported on CeO2(111) surface showed an aggregation trend with negative nucleation energy, which has been observed in previous study on Cu/CeO2 system [26]. Furthermore, the nucleation energy of the Ptn (n = 1–4) clusters adsorbed on CeO2(111) surface is slightly higher than that of the Ptn (n = 1–4) clusters adsorbed on the (Pt−Ce)O2 surface, and, at n = 4, the difference reaches the maximum, 0.43 eV. Therefore, the dopant of Pt has no obvious effect on the nucleation of clusters. Pt4 is the smallest three-dimensional cluster and is also a typical model in theoretical calculations, so the Pt4/CeO2 and Pt4/(Pt−Ce)O2 models were used for subsequent calculations.

2.3. Oxygen Vacancy Formation

To explore the change in the activity of the surface oxygen atoms before and after Pt atom doping, the oxygen vacancy formation energies on the Pt4/CeO2 and Pt4/(Pt−Ce)O2 interfaces were calculated. The position of the surface vacancy is indicated by way of a dotted circle in Figure 4, and those formation energies on the Pt4/(Pt−Ce)O2 and Pt4/CeO2 surfaces were calculated to be 0.37 and 2.19 eV, respectively. Thus, the insertion of Pt atoms facilitates the formation of oxygen vacancies at the metal–support interface and enhances the activity of the surface oxygen atoms.
Next, Bader charge analysis of both the Pt4/CeO2 and Pt4/(Pt−Ce)O2 surfaces was performed to explore the differences in the charge distribution caused by doping with Pt. A detailed charge distribution diagram of both surfaces loaded with a single Pt4 cluster is shown in Figure 4. For the Pt4/(Pt−Ce)O2 system, the oxidation state of the doped Pt atoms is +1.50e, whereas that of the Ce atoms at the same position without the Pt dopant is +2.41e. This is because the amount of positive charge carried by the doped Pt atoms is significantly less than that of the subsurface Ce atoms replaced by Pt atoms. On the insertion of a Pt atom, the surface oxygen atoms associated with it (indicated by a dotted circle) have an oxidation state of −1.01e, whereas the other surface oxygen atoms have an oxidation state between −1.10e and −1.20e. Therefore, Pt doping results in charge redistribution at the CeO2 surface. The total Bader charge of Pt1, Pt2, Pt3, and Pt4 supported on CeO2 surface is 0.05e, 0.02e, 0.03 e, and 0.05e, respectively. After the Pt doping, it can be observed that the total Bader charge of Ptn (n = 1–4) will increase to 0.19e, 0.10e, 0.12e, and 0.15e, respectively. In particular, the surface charge depletion caused by doping with Pt reduces the charge of the nearby surface oxygen atoms, which makes detachment from the surface easier, thus resulting in the formation of oxygen vacancies.
It can be observed from the results of Bader charge analysis and adsorption energy of both Pt4/CeO2 and Pt4/(Pt−Ce)O2 surfaces that Pt clusters near the doped site have slightly more positive charges and stronger adsorption energies. The charge depletion caused by Pt dopant enhances the interaction between Pt cluster and support surface. As mentioned in Liu’s work [27], the adsorption energy of CO varies with clusters’ oxidation state. Therefore, the dopant of Pt increases the oxidation state of the Pt clusters on the nearby surface, thereby weakening the CO adsorption.

2.4. CO Oxidation on the Pt4/(Pt−Ce)O2 and Pt4/CeO2 Surfaces

The oxygen atom activity, which is affected by the charge transfer from the Pt dopant atom, plays an important role in improving the catalytic CO oxidation activity of the Pt clusters adsorbed nearby on the surface. To explore this, the energies of each elementary step in the CO oxidation reaction occurring on the Pt4/CeO2 and Pt4/(Pt−Ce)O2 surfaces were calculated based on the M-VK mechanism. The corresponding models and energies of the CO oxidation reaction are shown in Figure 5 and Figure 6, respectively.
In the CO oxidation process at the Pt4/CeO2 interface, CO is first adsorbed with an adsorption energy of 2.89 eV near the Pt atoms at the Pt–support interface. The lengths of the Pt-C and C-O bonds in the adsorbed CO were calculated to be 1.84 and 1.16 Å, respectively (IM1). In the next step, CO combines with oxygen atoms on the support surface to form a triangular reaction intermediate (denoted TRI, IM2) in an endothermic process, having an energy of 0.32 eV. Here, the Pt-C bond length in IM2 lengthens to 2.06 Å.
Next, the oxygen atom at the active site is attracted by the C atom in CO to form a C-O bond having a length of 1.31 Å, and one of the O-Ce bonds formed with this oxygen atom is broken, and the length of the other Ce-O bond is elongated to 2.51 Å. The decomposition of the first TRI structure to produce a gaseous CO2 molecule requires 0.89 eV, and this process can lead to the formation of an oxygen vacancy (IM3).
In the next step, O2 is adsorbed on the surface with an adsorption energy of −1.70 eV and fills the oxygen vacancy (IM4). The length of the elongated O-O length in the O2 molecule is 1.46 Å. Further, a second CO molecule is adsorbed on the Pt atom with an adsorption energy of 1.83 eV, and the C atom of the CO molecule forms three Pt-C bonds, whose bond lengths range from 2.05 to 2.06 Å (IM5). Subsequently, the adsorbed CO combines with the O2 adsorbed on the oxygen vacancy to form a second TRI structure (IM6). In this process, the O-Ce bond of adsorbed O2 breaks, as does the O-O bond in molecular oxygen, and two of the three Pt-C bonds formed with the C atom of adsorbed CO break; the remaining Pt-C bond is thus shortened to 2.01 Å. The shift from IM5 to IM6 is strongly exothermic, having an energy of −1.43 eV. Finally, the TRI structure decomposes to form a second molecule of CO2 with an energy change of 0.23 eV (FS), resulting in the catalyst regaining its original structure.
The energy profile of the reaction shows that the formation of the TRI structure is the key step of the reaction. One of the reasons for this is the strong adsorption of CO on the Pt atoms, and the other is the lack of high activity of oxygen atoms at the interface of Pt4/CeO2. Both of these factors lead to a higher reaction energy barrier, about 1.21 eV.
For the CO oxidation reaction on the surface of Pt4/(Pt−Ce)O2, the first molecule of CO is adsorbed on the Pt atom close to the dopant Pt atom. This process leads to an energy change of −2.08 eV, suggesting the weaker adsorption of CO on the Pt cluster as a result of the insertion of a Pt atom on the nearby surface. In this structure, the C-O bond length is 1.16 Å, and the Pt-C bond length is 1.85 Å. Clearly, the bond length of the adsorbed CO is longer than that of the adsorbed CO at the Pt4/CeO2 interface. Next, IM2 is formed by the adsorbed CO moving towards and combining with a surface O atom. In IM2, the Pt-C bond length is 2.07 Å, and a C-O bond between the oxygen atom at the active site and the C atom of the adsorbed CO is formed at the Pt4/(Pt−Ce)O2 interface, having a bond length of 1.28 Å. In addition, one of the O-Ce bonds between the reactive oxygen atom and the two Ce atoms is also broken, as for the process occurring at the Pt4/CeO2 interface. However, the Ce-O bond length of the other is 2.46 Å, which is slightly shorter than the 2.51 Å bond at the Pt4/CeO2 interface. The transition from IM1 to IM2 is an exothermic process, having an energy change of −0.5 eV, and the energy barrier is only 0.78 eV. The decomposition of TRI in IM3 adsorbs 0.44 eV energy, making it the rate-determining step. This energy is much less than that adsorbed in the same process on the Pt4/CeO2 surface (0.9 eV). In IM4, O2 is adsorbed on the oxygen vacancy between Pt4 and the support, yielding an O-O bond length of 1.43 Å and an adsorption energy of −1.66 eV; further, when CO is adsorbed on the Pt4 clusters in IM5 with an adsorption energy of 1.40 eV, the C-O bond length is 1.20 Å. In the second TRI structure, the O-O bond in the adsorbed O2 molecule is broken, and O atom simultaneously bonds with the C atom of the adsorbed CO and a surface Ce atom, forming bonds having lengths of 2.43 and 1.26 Å, respectively. In this structure, the Pt-C bond length changes to 2.08 Å. Notably, the formation of the TRI structure releases 1.09 eV of energy and has a low energy barrier of 0.04 eV. The key step of the reaction is the decomposition of IM3, which is endothermic by 0.44 eV. The relatively weaker adsorption of CO and more active surface oxygen atoms can be attributed to the lower energy barrier of the reaction.
A comparison of the energy profiles of the CO oxidation reaction over the Pt4/CeO2 and Pt4/(Pt−Ce)O2 surfaces shows that the lattice oxygen atom activity is significantly enhanced, but the adsorption of CO is significantly weakened when the CeO2 surface is doped with Pt. Crucially, the insertion of Pt atoms reduces the energy of CO oxidation, that is, the rate-limiting step of the reaction, and Evac decreases from 1.21 to 0.78 eV.

3. Computation Details

All spin-polarized periodic DFT calculations were performed using the Vienna Ab initio Simulation Package (VASP 5.4) [28,29]. The electron exchange and correlation were treated within the generalized gradient approximation (GGA) using the Perdew–Burke-Ernzerhof (PBE) functional [30]. The core electrons of all the atoms were described by the projector-augmented wave (PAW) pseudopotential with a cut-off energy of 450 eV [31]. A spin-polarized DFT+U calculations with a value of U = 4.5 eV was used for the description of Ce 4f states [32]. The lattice parameter for bulk CeO2 is set to our previously calculated DFT+U value (5.44 Å) [33]. The CeO2(111) surface was modeled containing a (4 × 3) unit cell with three Ce-O-Ce layers and the Pt doped surface was constructed by substituting a surface Ce atom with a Pt atom. During geometry optimization, the bottom Ce-O-Ce layer were fixed, while the other layers and adsorbates were fully relaxed. The k-points sampling was generated by the Monkhorst Pack procedure with a (4 × 4 × 1) mesh and a 15 Å vacuum region was introduced to eliminate the interaction between Z-axis atoms. The electronic self-consistent field was converged to 10−5 eV and the forces on all atoms were converged to less than 0.02 eV/ Å. Bader charge provides a good approximation to the total electronic charge of atoms in computational system. Bader analysis was performed with the code developed by Henkelman et al. to quantify charge transfer between atoms [34]. The adsorption energy (Eads) of Ptn clusters was calculated by:
Eads = E(Ptn/Slab) − E(Slab)− E(Ptn)
The nucleation energy (Enuc) of Ptn (n = 1–4) clusters was calculated to quantify the nucleation processes of small Ptn cluster on the support surface.
Enuc = E(Ptn/Slab) − nE(Pt1/Slab) + (n−1)E(Slab)
The TS of surface reactions were searched using the climbing image nudged elastic band (CI-NEB) method [35] and the maximum force was converged to less than 0.05 eV/ Å. The stretching frequencies were analyzed to characterize a transition state with single imaginary frequency along the reaction coordinate. The activation energy was determined as the energy difference between the corresponding TS and initial states (IS) and the reaction energy was defined as the corresponding FS and IS energy difference.

4. Conclusions

In this study, using DFT calculations, we investigated the effect of dopant Pt atoms on (1) the energy of Ptn (n = 1−4) clusters with respect to size on pristine and doped CeO2(111) surfaces, (2) the activity of the surface O atoms, and (3) the CO oxidation cycle at the Pt−CeO2 interface. By calculating the nucleation energies of the Pt clusters on the undoped and Pt-doped surfaces, we found that the dopant had a negligible effect on the stability of the Pt clusters with respect to size. In addition, we found that the doping of metal atoms can enhance the surface oxygen atom activity via charge depletion on the oxide surface, thus lowering the oxygen formation energy. The dopant Pt atoms facilitate the key step in CO oxidation at the metal–substrate interface by lowering the energy required for the formation of TRI, which subsequently yields CO2. Moreover, the energy barrier for the reaction of CO with surface oxygen atoms is reduced, thereby improving the reaction activity. This study also illustrates that the combination of Pt dopant atoms and Pt clusters on the dopant surface can significantly improve the catalytic performance. Our theoretical computation results provide important insights for developing thermally stable and active Pt/CeO2 catalysts for CO oxidation.

Author Contributions

Conceptualization, A.J. and Z.R.; methodology, A.J. and Z.R.; software, A.J.; validation, A.J.; formal analysis, A.J. and Z.R.; investigation, A.J. and Z.R.; resources, J.L; data curation, A.J.; writing—original draft preparation, A.J.; writing—review and editing, Y.Q. and Y.Z.; supervision, J.L. All authors have read and agreed to the published version of the manuscript.

Funding

This research received no external funding.

Data Availability Statement

Not applicable.

Acknowledgments

Not applicable.

Conflicts of Interest

The authors declare no conflict of interest.

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Figure 1. Top views of the optimized configurations of the support surface: (a) CeO2(111), (b) (Pt−Ce)O2_I, and (c) (Pt−Ce)O2_II. The inset in (b) and (c) show the detailed configuration of the doped Pt. Ce (pale yellow), O (red), and Pt (cyan).
Figure 1. Top views of the optimized configurations of the support surface: (a) CeO2(111), (b) (Pt−Ce)O2_I, and (c) (Pt−Ce)O2_II. The inset in (b) and (c) show the detailed configuration of the doped Pt. Ce (pale yellow), O (red), and Pt (cyan).
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Figure 2. Top views of the optimized configurations of Ptn clusters on the CeO2 surface (up) and (Pt−Ce)O2 surface (down).
Figure 2. Top views of the optimized configurations of Ptn clusters on the CeO2 surface (up) and (Pt−Ce)O2 surface (down).
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Figure 3. Nucleation energies as a function of the number of Pt atoms in the Ptn cluster on CeO2 and (Pt−Ce)O2 surface.
Figure 3. Nucleation energies as a function of the number of Pt atoms in the Ptn cluster on CeO2 and (Pt−Ce)O2 surface.
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Figure 4. Bader charge analysis of (a) Pt4/CeO2 and (b) Pt4/(Pt−Ce)O2. The dotted circle represents the removed O atom to form oxygen vacancy.
Figure 4. Bader charge analysis of (a) Pt4/CeO2 and (b) Pt4/(Pt−Ce)O2. The dotted circle represents the removed O atom to form oxygen vacancy.
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Figure 5. Top view of CO oxidation on the (a) Pt4/CeO2 and (b) Pt4/(Pt−Ce)O2 surfaces. (IM: intermediate; TS: transition state; FS: final state).
Figure 5. Top view of CO oxidation on the (a) Pt4/CeO2 and (b) Pt4/(Pt−Ce)O2 surfaces. (IM: intermediate; TS: transition state; FS: final state).
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Figure 6. Calculated energy profiles for CO oxidation on the Pt4/CeO2 and Pt4/(Pt−Ce)O2 surfaces. The activation energy (Eact) is the energy of the transition state relative to the previous stage.
Figure 6. Calculated energy profiles for CO oxidation on the Pt4/CeO2 and Pt4/(Pt−Ce)O2 surfaces. The activation energy (Eact) is the energy of the transition state relative to the previous stage.
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Jiang, A.; Ren, Z.; Qu, Y.; Zhang, Y.; Li, J. Promotional Effect of Pt-Doping on the Catalytic Performance of Pt−CeO2 Catalyst for CO Oxidation. Catalysts 2022, 12, 529. https://doi.org/10.3390/catal12050529

AMA Style

Jiang A, Ren Z, Qu Y, Zhang Y, Li J. Promotional Effect of Pt-Doping on the Catalytic Performance of Pt−CeO2 Catalyst for CO Oxidation. Catalysts. 2022; 12(5):529. https://doi.org/10.3390/catal12050529

Chicago/Turabian Style

Jiang, Angran, Zhibo Ren, Yaqi Qu, Yanjun Zhang, and Jianwei Li. 2022. "Promotional Effect of Pt-Doping on the Catalytic Performance of Pt−CeO2 Catalyst for CO Oxidation" Catalysts 12, no. 5: 529. https://doi.org/10.3390/catal12050529

APA Style

Jiang, A., Ren, Z., Qu, Y., Zhang, Y., & Li, J. (2022). Promotional Effect of Pt-Doping on the Catalytic Performance of Pt−CeO2 Catalyst for CO Oxidation. Catalysts, 12(5), 529. https://doi.org/10.3390/catal12050529

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