Wei Shi,
Lianyang Zhang,
Zheming Ni*,
Shengjie Xia and
Xuechun Xiao
Laboratory of Advanced Catalytic Materials, College of Chemical Engineering, Zhejiang University of Technology, Hangzhou 310032, Zhejiang, China. E-mail: jchx@zjut.edu.cn; nzm@zjut.edu.cn; Tel: +86 0571 88320373
First published on 7th October 2014
The adsorption behavior and the selective hydrodesulfurization mechanism of thiophene on a Pd(111) surface were elucidated by density functional theory (DFT). All the pertinent species of different pathways were gathered to obtain their preferred adsorption sites. The activation energy and reaction energy of each step in different pathways were also calculated. The results show that the adsorption at the hollow site was the most stable when the thiophene was parallel to the Pd(111) surface with a ring plane. In the process of hydrodesulfurization, the heat of reaction was almost negative; therefore, reducing the temperature is helpful for the removal of S atom. The mechanism of direct hydrodesulfurization has a low activation energy, but the reaction has more than one possible product and is difficult to control. The mechanism of indirect hydrodesulfurization was the best fit for the 1,2-cis-hydrogenation process. The most feasible reaction pathway is (1) C4H4S + H2 → α,β-C4H6S; (2) α,β-C4H6S + H2 → C4H8S; (3) C4H8S + H2 → C4H10 + S. Among these steps, the formation of C4H8S is the rate-determining step.
At present, on comparison with the non-hydrodesulfurization (NHDS) method for sulfur removal, the method of hydrodesulfurization (HDS) is more mature, effective and economical.1,8,9 Most of the previous studies focused on the application of precious metal catalysts in the HDS of thiophene, which has superior catalytic activity and milder reaction conditions.10,11 Among these catalysts, palladium (Pd) nanoparticles are one of the most effective precious metal catalysts, which are characterized by a high degree of dispersion and small average particle size,12,13 and have been widely applied in the hydrogenation reactions of thiophene. Badano et al.14 compared the sulfur resistance of different catalysts; the result shows that the Pd catalyst had the highest activity. Vit et al.15 synthesized Pd/silica–alumina, and the result suggests that the higher acidity and surface area could improve the activities of Pd catalyst in the HDS of thiophene. In addition, they also found that the PdHx phase most likely served as a storage medium during the hydrogenation reaction.16 Although there has been extensive experimental research on the hydrogenation reaction of thiophene, there are only a few reports on its adsorption process and hydrogenation mechanism due to the complexity of the experiments and the limitations of the characterization methods.
Density functional theory17,18 has been widely used to calculate the adsorption energy, structure parameters, activation energy and reaction energy in the process of different reactions. Liao et al.19 made comparisons among different Mo-catalysts during the C–S cleavage of thiophene in order to find the most active catalyst species. Moreover, by DFT, Zhu et al.20,21 researched the hydrogenation reaction of thiophene over Pt(110) and Pt(111) surfaces to present the most efficient reaction route. Our previous work22 predicted the most favorable mechanism for thiophene catalyzed on an Au(111) surface, and found that the hydroisomerization process is dominant.
In this work, we studied the adsorption process and hydrogenation mechanism of thiophene on a clean Pd(111) surface by the DFT method using the Dmol3 program package. The properties of different adsorption sites were also elucidated, which include structure parameters and adsorption energy. Furthermore, the possible reaction pathways of thiophene hydrogenation were discussed in detail to discover the primary HDS mechanism. The aim of this work is to provide a better understanding of the structural, energetic, catalytic and selective properties of Pd catalysts for the hydrodesulfurization of thiophene.
Eads = E(A/surface) − (EA + Esurface) |
According to previous works,22,30 the thiophene plane would interact with the metal surface through the S atom. In addition, the vertical adsorption sites would be converted to parallel adsorption sites; this implies that the model of parallel adsorption is more stable. As a result, we chose twelve highly symmetric parallel adsorption sites on the Pd(111) surface for calculations, as shown in Fig. 1. These adsorption sites include top (0°, 30°, 60°), hcp (0°, 30°, 60°), fcc (0°, 30°, 60°) and bridge (0°, 30°, 60°) sites. As can be seen in Fig. 1, 0°, 30° and 60° represent the adsorption sites with the symmetry axis rotating 0°, 30° and 60° from the horizontal direction.
The adsorption energies and geometric parameters of different sites were calculated and are listed in Table 1; only those in stable adsorption configurations were summarized. Moreover, the most stable structure of thiophene adsorbed on the Pd(111) surface is shown in Fig. 2. As can be seen from Table 1 and Fig. 2, a thiophene molecule is adsorbed on the Pd(111) surface with an energy of −176 to −186 kJ mol−1, and preferentially adsorbed in a parallel way through the ring plane. Among different initial adsorption sites, the Eads of the Bri-0° site is −185.3 kJ mol−1, and the distance between the Pd atom and S atom is 0.1461 nm. The maximum of Eads and the least value of dPd–S suggest that the position of Bri-0° is the most stable. During the process of adsorption, the S atom and H atoms of thiophene move upward, and the axial rotation of the ring plane is clockwise. Finally, the S atom of thiophene is transferred to the hollow site and interacted with the Pd(111) surface.
Adsorption site | Eads/(kJ mol−1) | dPd–S nm−1 | Adsorption site | Eads/(kJ mol−1) | dPd–S nm−1 |
---|---|---|---|---|---|
a The adsorption positions in Table 1 represent the initial adsorption sites of thiophene. | |||||
Top-0° | −176.0 | 0.1559 | Fcc-0° | −182.4 | 0.1578 |
Top-30° | −184.6 | 0.1587 | Fcc-30° | −179.8 | 0.1516 |
Top-60° | −176.8 | 0.1560 | Fcc-60° | −183.2 | 0.1562 |
Hcp-0° | −181.6 | 0.1542 | Bri-0° | −185.3 | 0.1461 |
Hcp-30° | −184.7 | 0.1584 | Bri-30° | −184.5 | 0.1577 |
Hcp-60° | −182.1 | 0.1558 | Bri-60° | −184.7 | 0.1551 |
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Fig. 2 The most stable configurations of thiophene on the Pd(111) surface (A) represented thiophene; (B) represented top view; (C) represented side view. |
In order to analyze the structure parameter of the most stable adsorption site of a thiophene molecule on a Pd(111) surface, Table 2 lists the adsorption energy and bond lengths of the thiophene molecule at the initial site of Bri-0°. On comparing the data in Table 2, it can be seen that the calculation of bond length for free thiophene is in good agreement with the experimental values.30 After adsorption, there is an elongation in the range of 0.0013–0.0112 nm for the bond lengths of d1–d5, while the energy of thiophene decreases. This phenomena suggests that the adsorption of thiophene on a Pd(111) surface could promote the hydrogenation reaction. In addition, the greatest change in d1 implies that the H atom is more likely to attack the α-C of thiophene.
Model | Eads/(kJ mol−1) | d1/nm | d2/nm | d3/nm | d4/nm | d5/nm |
---|---|---|---|---|---|---|
Thiophene (expt) | — | 0.1730 | 0.1370 | 0.1420 | 0.1370 | 0.1730 |
Thiophene (calc) | — | 0.1729 | 0.1372 | 0.1422 | 0.1372 | 0.1727 |
Thiophene/Au(111) | −185.3 | 0.1841 | 0.1424 | 0.1435 | 0.1482 | 0.1801 |
|Δd| | — | 0.0112 | 0.0052 | 0.0013 | 0.0110 | 0.0074 |
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Fig. 3 Different reaction pathways for the hydrogenation of thiophene. A, B, C, D, E and F represent mechanisms A, B, C, D, E and F. |
Table 3 provides six possible hydrogenation mechanisms of thiophene on a Pd(111) surface. The mechanisms of A–E represent the HYD pathway, and the mechanism of F represents the DDS pathway. Among the hydrogenation mechanisms of A–F, the major difference is the diversity of the hydrogenation position of the α-C and β-C in the thiophene molecule. According to the mechanisms of A–F in Table 3, we optimized the structures of the reactants (IS) and products (FS), and then searched the TS between them. The activation energies and reaction energies at the TS are tabulated in Table 4. Among different hydrogenation mechanisms, the initial step is the coadsorption of thiophene and atomic H, thus we only compared the intermediate steps of the hydrogenation process in Table 3 (Step 1–4).
Step | Mechanism A | Mechanism B | Mechanism C |
---|---|---|---|
a aα,β represent hydrogenation of α-C or β-C. | |||
1 | C4H4S* + H* → α-C4H5S* + * | ||
2 | α-C4H5S* + H* → α,β-C4H6S* + * | α-C4H5S* + H* → α,α-C4H6S* + * | |
3 | α,β-C4H6S* + H* → α,β,α-C4H7S* + * | α,β-C4H6S* + H* → α,β,β-C4H7S* + * | α,α-C4H6S* + H* → α,α,β-C4H7S* + * |
4 | α,β,α-C4H7S* + H* → C4H8S* + * | α,β,β-C4H7S* + H* → C4H8S* + * | α,α,β-C4H7S* + H* → C4H8S* + * |
5 | C4H8S* + H* → C4H9S* + * | ||
6 | C4H9S* + H* → C4H10* + S* |
Step | Mechanism D | Mechanism E | Mechanism F |
---|---|---|---|
1 | C4H4S* + H* → β-C4H5S* + * | C4H4S* + H* → C4H5S* + * | |
2 | β-C4H5S* + H* → β,α-C4H6S* + * | C4H5S* + H* → C4H6* + S* | |
3 | β,α-C4H6S* + H* → β,α,β-C4H7S* + * | β,α-C4H6S* + H* → β,α,α-C4H7S* + * | |
4 | β,α,β-C4H7S* + H* → C4H8S* + * | β,α,α-C4H7S* + H* → C4H8S* + * | |
5 | C4H8S* + H* → C4H9S* + * | ||
6 | C4H9S* + H* → C4H10* + S* |
Intermediates | Reaction | Ea/(kJ mol−1) | ΔE/(kJ mol−1) |
---|---|---|---|
TS1 | C4H4S* + H* → α-C4H5S* + * | 41.6 | −54.6 |
TS2 | C4H4S* + H* → β-C4H5S* + * | 85.6 | −50.7 |
TS3 | α-C4H5S* + H* → α,β-C4H6S* + * | 142.1 | −22.9 |
TS4 | α-C4H5S* + H* → α,α-C4H6S* + * | 185.6 | 21.3 |
TS5 | α,β-C4H6S* + H* → α,β,α-C4H7S* + | 124.2 | 85.3 |
TS6 | α,β-C4H6S* + H* → α,β,β-C4H7S* + | 110.1 | −36.6 |
TS7 | α,β,β-C4H7S* + H* → C4H8S* + * | 229.9 | 11.3 |
TS8 | C4H8S* + H* → C4H9S* + * | 198.8 | −37.8 |
TS9 | C4H9S* + H* → C4H10* + S* | 169.1 | −48.3 |
TS10 | C4H4S* + H* → C4H5S* + * | 62.5 | −54.6 |
TS11 | C4H5S* + H* → C4H6* + S* | 58.6 | −90.1 |
C4H4S* + H* → C4H5S* (FS1 or FS2) |
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Fig. 4 The IS, TS, FS, activation energy and reaction energy (kJ mol−1) of mechanisms A–E(1) on the Pd(111) surface A–C(1): Ea = 41.6; ΔE = −54.6 D–E(1): Ea = 85.6; ΔE = −50.7. |
For the reaction of C4H4S* + H* → α-C4H5S* (FS1), we calculated the coadsorption of thiophene and atomic H as IS1. After complete optimization, the thiophene adsorbed with the S atom downwardly bonded to the Pd(111) surface at the original hollow site; moreover, the C2 and C3 atoms of thiophene moved upward. The atomic H transferred from the fcc site to the neighboring bridge site. In TS1, the reacted α-C tilted by 38.4° from the horizontal plane, and the atomic H moved to the hcp site with an α-C–H distance of 0.1756 nm. When FS1 formed, the reacted H of α-C continued to tilt upward until it was perpendicular to the Pd(111) surface. Finally, the FS1 was adsorbed at the hollow site through the unreacted double bond of CC to the surface. The bond length of the reacted α-C–H decreased from 0.2729 nm to 0.1095 nm, and d1 was elongated to 0.1841 nm. This reaction was exothermic by −54.6 kJ mol−1, and the corresponding Ea was 41.6 kJ mol−1.
For the reaction of C4H4S* + H* → β-C4H5S* (FS2), the IS of the first step is exactly the same as the IS1. In TS2, the S atom tilted upward slightly, and the atomic H gradually moved away from the surface at the same time. The bond length of the reacted β-C–H decreased from 0.2366 nm in IS1 to 0.1597 nm. When FS2 formed, the reacted H of β-C continued to tilt upward until it was perpendicular to the Pd(111) surface; moreover, the S atom moved upward noticeably. This reaction was exothermic by −50.7 kJ mol−1, and the corresponding Ea was 85.6 kJ mol−1.
As can be seen from Table 4 and Fig. 4, the relative energies of FS1 and FS2 are exothermic with negative values, which indicates that reducing the temperature is helpful for the reaction in step 1. In addition, the formation of FS1 is more favorable because of the comparably lower activation energy of 41.6 kJ mol−1. Therefore, the hydrogenation process of α-C in thiophene occurs more easily in step 1, and this result is in good agreement with the analysis of the structure parameters in Section 3.1.
α-C4H5S* + H* → C4H6S* (FS3 or FS4) |
α-C4H5S* is regarded as the dominant product in step 1, and the further hydrogenation process would occur on the basis of α-C4H5S*. The Ea, ΔE and the corresponding TS structures for the mechanism of A–C(2) are shown in Fig. 5.
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Fig. 5 The IS, TS, FS, activation energy and reaction energy (kJ mol−1) of mechanisms A–C(2) on the Pd(111) surface A–B(2): Ea = 142.1; ΔE = −22.9 C(2): Ea = 185.6; ΔE = 21.3. |
For the reaction of α-C4H5S* + H* → α,β-C4H6S* (FS3), we calculated the coadsorption of α-C4H5S and atomic H as IS2. When the reaction occurred, the methylene of α-C4H5S tilted upward and other C atoms lay flush with each other. The atomic H got transferred from the fcc site to the neighboring hcp site. In TS3, the reacted β-C–H moved upward, and the atomic H moved close to the ring plane. The product α,β-C4H5S* (FS3) was generated after the atomic H reached the reacted β-C and settled at the hollow site through the double bond. The d1 was elongated to 0.1852 nm. This reaction was exothermic by −22.9 kJ mol−1, and the corresponding Ea was 142.1 kJ mol−1.
For the reaction of α-C4H5S* + H* → α,α-C4H6S* (FS4), the reactant is the same as in IS2. In TS4, the reacted α-C moved upward, and the atomic H got transferred to the adjacent hcp site in order to move close to the reacted α-C with an α-C–H distance of 0.2200 nm. Additionally, the C2 and C3 atoms are electron-rich because of the hydrogenation process of α-C; as a result, the double bond between C2 and C3 was formed during the reaction. Once FS4 was produced, the H atoms of α-C retained almost the same structure, both of which had a tilting angle of 109.5°. Finally, the FS4 was adsorbed at the bridge site via the double bond of C2 and C3. This reaction was endothermic by 21.3 kJ mol−1, and the corresponding Ea was 185.6 kJ mol−1.
Compared with the calculation results in step 2, the formation of α,β-C4H5S* is exothermic, while the formation of α,α-C4H5S* is endothermic. The hydrogenation process of C4H5S* to α,β-C4H5S* seems more liable to take place due to its lower energy barrier (142.1 kJ mol−1). Hence, the α,β-C4H5S* species is selected as the species for further hydrogenation below.
α,β-C4H6S* + H* → C4H7S* (FS5 or FS6) |
α,β-C4H6S* is considered as the most favorable product in step 2, and the further hydrogenation process of α,β-C4H6S leads to α,β,α-C4H6S or α,β,β-C4H6S. The Ea, ΔE and the corresponding TS structures for the mechanism of A–B(3) are illustrated in Fig. 6.
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Fig. 6 The IS, TS, FS, activation energy and reaction energy (kJ mol−1) of mechanisms A–B(3) on the Pd(111) surface A(3): Ea = 124.2; ΔE = 85.3 B(3): Ea = 110.1; ΔE = −36.6. |
The reaction of α,β-C4H6S* + H* → α,β,α-C4H7S* (FS5) starts from the coadsorption of α,β-C4H6S and atomic H. In the initial state, the structure of α,β-C4H6S remained the same as in FS3, and was located at the hollow site through the double bond. The atomic H got transferred to the adjacent hcp site. In TS5, the atomic H left its hcp site and moved to the adjacent hcp site, and the ring plane rotated anticlockwise to meet the attacking H atom. The forming α-C–H distance decreased from 0.3582 nm to 0.2531 nm. Once FS5 was formed, the S atom moved away from the Pd surface, and the ring plane tilted downwards. The bond length of the reacted α-C–H decreased to 0.1225 nm. This reaction was endothermic by 85.3 kJ mol−1, and the corresponding Ea was 124.2 kJ mol−1.
For the reaction of α,β-C4H6S* + H* → α,β,β-C4H7S* (FS6), the reactant was the same as what was described in IS3. In TS6, the atomic H got transferred from the hcp site to the neighboring top site. At the same time, the C2 and C3 atoms moved upwards. The distance between the atomic H and reacted β-C was decreased to 0.2128 nm from 0.2929 nm. While FS6 was produced, the C2 and C3 atoms further moved upward. Subsequently, the β-C–H bond was activated with a distance of 0.1102 nm and d1 was elongated to 0.1860 nm. This reaction was exothermic by −36.6 kJ mol−1, and the corresponding Ea was 110.1 kJ mol−1.
As can be seen from the data mentioned above, the reactant α,β-C4H6S prefers hydrogenation on β-C rather than α-C. The formation of FS5 is endothermic, while the formation of FS6 is exothermic. Furthermore, a low barrier of 110.1 kJ mol−1 as well as a short bond length of 0.1102 nm are present for the β-C–H bond formed in FS6. Therefore, the formation of FS6 from α,β-C4H6S is likely to occur.
α,β,β-C4H7S* + H* → C4H8S* (FS7) |
From the previous discussion, the mechanism B is regarded as the most favorable pathway. There is only one possibility for the further hydrogenation of α,β,β-C4H6S to form the saturated product of C4H8S. The Ea, ΔE, and the corresponding TS structures for the mechanism of B(4) are illustrated in Fig. 7.
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Fig. 7 The IS, TS, FS, activation energy and reaction energy (kJ mol−1) of mechanism B(4) on the Pd(111) surface B(4): Ea = 229.9; ΔE = 11.3. |
The reaction of α,β,β-C4H7S* + H* → α,β,β,α-C4H8S* (FS7) began with the coadsorption of α,β,β-C4H7S and atomic H, as can be seen in IS4. For IS4 adsorption on the Pd surface, the preferential adsorption site was where the atomic H got transferred to the nearby hcp site, and the α,β,β-C4H7S molecule was bound at the hollow site via the S atom, where the adsorption configuration is the same as in FS6. In TS7, the unsaturated α-C moved upward and the atomic H got transferred to the adjacent hollow site in order to form the saturated bond of α-C–H. The distance between the atomic H and unsaturated α-C was decreased from 0.3466 to 0.2011 nm. Once FS7 was adsorbed at the top site through the S atom, the C atoms of the ring plane lay flush with each other parallel to the Pd surface. The d1 was elongated to 0.1866 nm. This reaction was exothermic by 11.3 kJ mol−1, and the corresponding Ea was 229.9 kJ mol−1.
C4H8S* + 2H* → C4H10* + S* (FS8 and FS9) |
In the final step, C4H8S* is further hydrogenated to n-butane and an S atom with the help of atomic H. The Ea, ΔE and the corresponding TS structures for the mechanism of B(5–6) are illustrated in Fig. 8.
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Fig. 8 The IS, TS, FS, activation energy and reaction energy (kJ mol−1) of mechanisms B(5–6) on the Pd(111) surface B(5): Ea = 198.8; ΔE = −37.8 B(6): Ea = 169.1; ΔE = −48.3. |
The reaction of C4H8S* + H* → C4H9S* (FS8) was exothermic by −37.8 kJ mol−1, with the corresponding Ea of 198.8 kJ mol−1. In the initial state, the C4H8S molecule bound at the top site through the S atom, and the atomic H got transferred from the fcc site to the adjacent bridge site. In TS8, the atomic H moved close to the reacted α-C, resulting in a shortening of the distance between the α-C and atomic H from 0.3020 nm to 0.2257 nm. Moreover, one of the C–S bonds broke up, and the S atom moved downward to the Pd surface. The formed FS8 was adsorbed at the hcp site via the S atom and d5 was elongated to 0.1879 nm; moreover, the distance between the α-C and the atomic H was further reduced to 0.1110 nm to form the bond of α-C–H.
For the reaction C4H9S* + H* → C4H10* + S* (FS9), we calculated the coadsorption of C4H9S and atomic H as IS6. After adsorption, the atomic H was located at the original fcc site. The C3 and C4 atoms of C4H9S tilted upwards, compared with the structure in FS8. From the TS9 shown in Fig. 8, the atomic H was located at the nearby top site with an α-C–H distance of 0.3756 nm; moreover, the S atom was separated from C4H9S. Once FS9 was produced, the dissociated S settled at the fcc site, and the C4H10 molecule was adsorbed on the Pd surface through the H atoms of C2 and C4, whose structure was perpendicular to the Pd surface. This phenomenon is similar to previous results reported in the literature.36 This reaction was exothermic by −48.3 kJ mol−1, and the corresponding Ea was 169.1 kJ mol−1.
C4H4S* + H* → C4H5S* (FS10) |
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Fig. 9 The IS, TS, FS, activation energy and reaction energy (kJ mol−1) of mechanism F(1) on the Pd(111) surface F(1): Ea = 62.5; ΔE = −54.6. |
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Fig. 10 The IS, TS, FS, activation energy and reaction energy (kJ mol−1) of mechanism F(2) on the Pd(111) surface F(2): Ea = 58.6; ΔE = −90.1. |
For the reaction of C4H4S* + H* → C4H5S* (FS10), the configuration of the reactant is the same as described in IS1. In TS10, d5 decreased from 0.1820 nm to 0.1805 nm. This phenomena caused the d1 bond to break, which was accompanied by migration of the atomic H to the top site and upward migration of C3 and C4. While FS10 was formed, the C3 atom moved downward, which made the C1–C3 atoms parallel to the Pd surface. Finally, FS10 was adsorbed at the hollow site on the Pd surface via the double bond of C1 and C2. This reaction was exothermic by −54.6 kJ mol−1, and the corresponding Ea was 62.5 kJ mol−1.
C4H5S* + H* → C4H6* + S* (FS11) |
The reaction C4H5S* + H* → C4H6S* (FS11) started with the coadsorption of C4H4S and atomic H. During the process, the atomic H migrated to the hcp site from the initial fcc site, and the structure of C4H5S remained the same as in FS10. Moreover, the d5 bond was elongated to 0.1843 nm. In TS11, the atomic H moved to the adjacent fcc site to form the bond of α-C–H, leading to the breaking of the C–S bond. Then, the dissociated S got transferred to the hcp site. When FS11 produced, the dissociated S got located at the hcp site, and the molecule of butadiene was parallely adsorbed at bridge sites on the Pd surface through the double bonds of C1C2 and C3
C4. This reaction was exothermic by −90.1 kJ mol−1, and the corresponding Ea was 58.6 kJ mol−1.
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Fig. 11 Sketch for potential relative energy (ER) of reaction mechanisms F and B on the Pd(111) surface. |
Our results show that the parallel adsorption of thiophene at the hollow site through the ring plane is the most stable adsorption structure on the Pd(111) surface. After thiophene gets adsorbed, all the bond lengths increase, and the H atom is most liable to attack the α-C of thiophene when the hydrogenation reaction occurs.
No matter what kind of mechanism it follows, the hydrogenation of thiophene is almost exothermic; therefore, reducing the temperature is beneficial for desulfurization. For the DDS mechanism, the reaction has a lower energy of activation as compared with the HDS reaction, but the hydrogenated product has more than one possibility and is difficult to control. For the HDS mechanism, it is found that 1,2-cis-hydrogenation is predominant. During the reaction, the C–S bond length in thiophene increases gradually, while the bond energy of C–S decreases. All of these changes facilitate the cleavage of C–S. The reaction path of HYD is found to proceed as follows: C4H4S → α-C4H6S → α,β-C4H6S → α,β,β-C4H6S → C4H8S → C4H9S → C4H10 + S. The formation of C4H8S is considered as the rate-limiting step, which has the highest energy barrier.
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