Sulfur-containing compounds are undesirable in gasoline and diesel fuels because of the emission of SOx gases leading to air pollution. In order to protect the human health and reduce the environmental hazards, environmental regulations that tend to limit the sulfur levels to very lower ones have already been introduced in many countries during the last few decades (1). The specifications present a new and challenging task for the crude oil and its derivation refining industry. Much attention has been paid to low level sulfur approaching requirements for the deep desulfurization technologies currently (2-4). Hydrodesulfurization (HDS) can remove aliphatic and acyclic sulfur compounds quite efficiently when adopted at an industrial scale. HDS is a catalyticchemical process to obtain ultra-low sulfur fuel which needs high temperature and pressure, large reactor tower and more active catalysts (5-7). Because of high hydrogen consumption, decreased catalysts life and low yield of products, HDS is very costly. Therefore, alternative desulfurization techniques have been investigated widely, among which oxidative desulfurization (ODS) is considered to be one of the promising new methods for super high desulfurization of petroleum oil. As a part of our ongoing efforts for developing the synthesis and application of POMs (8-12), herein we report the synthesis of TBA-PV2Mo10@PVA nanocomposite as a high-performance nanocatalyst for the elimination of organic sulfur compounds. To the best of our knowledge, it is the first reported results of the application of this catalyst for desulfurization of gasoline.
Polyoxometalates (POMs) are well-defined oxoanionic clusters of early transition metals that have attracted growing interest for the development of advanced functional materials (13-16). POMs are a type of intriguing catalysts that can be applied for a wide range of technologically relevant applications owing to reasonably high thermal stability, and reversible electron transfer ability under mild conditions (14). Furthermore, polyoxometalates have several advantages, including high flexibility in the modification of the acid strength, non-toxicity, environmental compatibility, ease of handling, and experimental simplicity (14-16). Keggin-type of POMs have been widely studied as heterogeneous and homogeneous catalyst for the oxidation of organic compounds (16,17). However, the application of this type of catalysts still suffers from some drawbacks, mainly the low surface area (1–10 m2/g) leading to the low efficiency and the high solubility, causing recycling difficulty and environmental problem (18). To overcome these disadvantages there is a need to invent a supported and heterogeneously active forms of POM (18,19). Organic polymers due to their excellent toughness and durability are suitable candidates as matrices for assembling polyoxometalates (20).
In this investigation, polyvinyl alcohol (PVA) is used to play this important and useful role as great matrices. TBA-PV2Mo10@PVA has lipophilic cation which acts as a good phase transfer agent and transfers the peroxometal anion into organic phase. A phase transfer between the aqueous phase containing the oxidants and catalyst and the organic phase containing the oil limits the overall efficiency. This aspect of the process can be improved by using a phase transfer agent that facilitates the transfer of reagents between the two immiscible phases. A new approach to phase transfer catalysis uses surfactant based or amphiphilic catalysts, which combine together a polyoxoanion and a quaternarnary ammonium cation. However, the organic-inorganic hybrid nanocomposite is successfully designed by reaction of TBA-PV2Mo10 and PVA via sol gel method under oil-bath condition as a phase transfer catalyst for ODS of gasoline. In typical oxidation reactions, the mixture of H2O2/CH3COOH is used as oxidant and polar CH3CN applied as an extraction solvent for removing the oxidized products. In addition, the influences of different parameters on the desulfurization efficiency are investigated in detail.
MATERIALS AND METHODS
Materials and characterization methods
All chemicals and solvents were commercially available and used as received. Benzothiophene (BT) and thiophene (Th), n-heptane, hydrogen peroxide (H2O2, 30 vol.%), and acetic acid (CH3COOH, 99.7%), acetonitrile (CH3CN), sodium tungstate dihydrate (Na2WO4.2H2O), disodium hydrogen phosphate (Na2HPO4) and tetrabutylammonium bromide (TBAB) were purchased from Sigma–Aldrich company. Several heteropolyoxometalates catalysts were prepared according to procedures published in literature (11, 12). Typical real gasoline was used with the following specification: density 0.7863 g/mL at 15 °C, total sulfur content 0.287 wt.%.
Fourier transform infrared spectroscopy (FT-IR) studies were done on a Thermo-Nicolet-is 10 spectrometer, using KBr disks in the range 400–4000 cm−1. Ultraviolet–visible (UV–vis) spectra were measured with a double beam Thermo-Heylos spectrometer in the range of 200-400 nm. Measurements were performed by using quartz cuvettes. Powder X-ray diffraction (XRD) analysis were collected between 2θ = 5°-80° at room temperature on a Bruker D8 advance powder X-ray diffractometer with a Cu-Kα (λ = 0.154 nm) radiation source. The surface morphologies were examined by scanning electron microscope (SEM) by LEO 1455 VP equipped with an energy dispersive X-ray (EDX) spectroscopy apparatus. 31P NMR spectrums were recorded on Bruker Ultra Shield 250 MHz. The total sulfur and mercaptan content in gasoline before and after treatment were determined using X-ray fluorescence with a TANAKA X-ray fluorescence spectrometer RX-360 SH.
Synthesis of tetrabutylammonium divanadodeca-molibdophosphate (TBA-PV2Mo10)
H5PV2Mo10O40 was synthesized according to published literature . In summary, in 50 mL of boiling water sodium metavanadate (12.2 g, 100 mmol) was dissolved and mixed with (3.55 g, 25 mmol) of Na2HPO4 in 50 mL of water. The solution was cooled and 5 mL of concentrated sulfuric acid (17M, 85 mmol) was added to it. The solution was developed a red color. Na2MoO4.2H2O (60.5 g, 250 mmol) was dissolved in 100 mL of water and added to the red solution with vigorous stirring. Concentrated sulfuric acid (42 mL, 17 M, 714 mmol) was added to it, slowly. The hot solution was cooled to room temperature. The 10-molybdo-2-vanadophosphoric acid was extracted with 500 mL of ethyl ether. Air was passed through the heteropoly etherate (bottom layer) to free it of ether. The solid remaining behind was dissolved in water, concentrated to first crystal formation, as already described. The large red crystals that formed were filtered, washed with water, and air dried. By addition of solid potassium carbonate, the pH is adjusted between 6 and 7. By addition of solid potassium chloride (2.2 g, 40 mmol) an orange potassium salt (2.5 g, 45 mmol) is precipitated and recrystallized in water. Then, the remaining solid was dissolved in 55 mL of warm distilled water. Then, aqueous solution of tetrabutylammonium bromide (Bu4NBr) (1.8 mmol) was added drop-wise, with vigorous stirring. The solid formed was filtered off, recrystallized with acetonitrile, ether and air dried (Fig. 1). The resultant (((n- C4H9)4N)4K[PMo10V2O40]) solid is designated as TBA-PV2Mo10.
Synthesis of the TBA-PV2Mo10@PVA nanocatalyst
Preparation of TBA-PV2Mo10@PVA via sol–gel method under oil-bath condition is as follows: 0.1 g of PVA was dissolved in 35 mL of hot distilled water and the temperature was fixed at 60 °C. Then, aqueous solution of 0.04 g mL-1of TBA-PV2Mo10 in water was added drop wise in it. The mixture was stirred to dissolve any solid. Then, the sol was heated to 65 °C under oil bath condition until a hydrogel TBA-PV2Mo10@PVA was formed. Finally, the gel was filtered, washed with deionized water-acetone and dried in oven at 50 °C for 2 h. (Fig. 2).
ODS of model fuel
The ODS process of model fuel was carried out in a round-bottom flask equipped with a magnetic stirrer and a thermometer. Some of the MSCs such as BT or Th was dissolved in n-heptane as a model fuel to evaluate the catalytic performance of TBA-PV2Mo10@PVA and the reactivity of mercaptans in the oxidation reaction. First, the water bath was heated and stabilized to a certain temperature (25-40 °C). 4 mL CH3COOH/H2O2 in the volume ratio of 1/1 was added and mixed with 50 mL of the model sulfur compound (Th or BT). 0.1 g of TBA-PV2Mo10@PVA was added to the flask as a catalyst. The flask was immersed in a heating bath and stirred at 500 rpm for 2 h. The biphasic was formed and separated by decantation. After the decantation, the upper phase (model fuel) was withdrawn and the remained MSCs in model fuel were analyzed by GC-FID (Agilent 6890). The conversion of BT in the model fuel was used to calculate the removal of MSCs. The oxidized MSCs was characterized by GC-MS (Varian cp-1200 quadrupole MS), HP5890 Series II with 5972 Series MS detector. The results indicated a perfect match of the mass spectrum of the product with the standard benzothiophene sulfone. Also the total sulfur concentration of the model gasoline before and after ODS was determined using a Tanaka Scientific RX-360 SH X-ray fluorescence spectrometer (ASTM D-4294 method). The desulfurization (%) of real gasoline fuel was calculated by the following equation, where S0 is the sulfur concentration in the original fuel, and St is the sulfur concentration in the treated oil.
% Desulfurization = (S0–St)/S0 × 100 (1)
The concentrations of the MSCs (BT) in the treated model fuel were determined from their peak areas in the GC‐FID chromatograms using a calibration curve obtained with the peak areas of their standard concentrations. The change in concentration was calculated as conversion (%) using equation (2), in which C0 is initial concentration of BT, and Ct is the final concentration of BT after time t.
% Conversion = (C0–Ct)/C0 × 100 (2)
ODS of real gasoline
For ODS of real fuel, 50 mL gasoline was added to two-necked round bottom flask. The temperature of solution fixed at 35°C. Then, 0.1 g of TBA-PV2Mo10@PVA was added to the solution and strongly stirred by a magnetic stirrer. A mixture of CH3COOH: H2O2 (4 mL) in ratio of 1/1 was added drop wise in 2 h, while it has been stirring vigorously. When the ODS has been finished the mixture was cooled down to room temperature and then 10 mL of CH3CN was added to extract the oxidized MSCs. The acetonitrile/oil ratio used was 1/5 by volume. The biphasic mixture was separated by decantation. The oil phase was separated and weighed to calculate present of gasoline (for three times reaction: 98, 97 and 96%). The total sulfur and mercaptan content in gasoline before and after ODS were determined using standard test method (ASTM D-4294 and D-3227). Results are showed in Table 1.
RESULTS AND DISCUSSION
Characterization of materials
The identification of specific chemical bands and functional groups of the synthesized samples was characterized using FT-IR spectroscopy to confirm their successful incorporation. The FT-IR spectra of different POMs salts showed the common characteristic absorption peaks ranging from 500 to 1100 cm–1 corresponded to POM anion configurations, and the peaks ranging from 1450 to 3000 cm–1 showed the pattern of quaternary ammonium salts (Fig. 3). The peaks of POM in 560-590 cm–1, 765-796 cm–1, 860-885 cm–1, 940-965 cm–1, and 1060-1075 cm–1 related to the symmetric vibrations of O–Mo–O, octahedral bridge/edge sharing Mo–Oc–Mo, octahedral corner sharing Mo–Ob–Mo, terminal Mo–Od, and P–O configurations, respectively (14-16). These configurations collectively account for the Keggin type POMs. The absorption peaks in the range of 1450-1475 cm–1 indicated the C–H bending vibrations for CH2 and the peaks at 640 cm–1 showed N–H bending vibrations. The adoption bands at 2850 and 2915 cm–1 represented the stretching vibrations of C–H for CH2 and CH3 (16). From FT-IR spectra shown in Fig. 3, it can understand that there is a clear and notable difference among TBA-PV2Mo10 powder, PVA and TBA-PV2Mo10@PVA nanocomposite. As presented in Table 2, characteristic bands of TBA-PV2Mo10 on PVA, compared to pure TBA-PV2Mo10, which shows a blue- or red-shift indicate the electrostatic and hydrogen-bond interactions between TBA-PV2Mo10 and PVA. According to this table Mo-O corner-sharing band experiences a red shift and show it is involved in the interaction with hydrogen on the PVA and formed a hydrogen bond.
Fig. 4 shows the UV-vis spectra of pure PVA, TBA-PV2Mo10 and TBA-PV2Mo10@PVA as comparative data to confirm the changes on pure TBA-PV2Mo10 after introducing PVA. The UV–vis spectra of PVA (a), TBA-PV2Mo10 (b), and TBA-PV2Mo10@PVA (c) (Fig. 4), showed strong absorption peak at 214 nm which assigned to oxygen-to-vanadium or O-2 to Mo+6 charge-transfer transition of PV2Mo10, 213 nm for TBA-PV2Mo10@PVA and 270 nm for PVA which indicated TBA-PV2Mo10@PVA blue shift towards PVA and red shift towards TBA-PV2Mo10. Excitation of the oxygen to metal charge transfer band of TBA-PV2Mo10 in near UV light region results in the charge transfer from an O-2 to Mo+6, forming the O-1 and Mo+5. By introducing TBA-PV2Mo10 on PVA, corresponding to (a, b), the intensity of bands decreased so can persuade us that interaction between them completed and spectra of PVA overlapped TBA-PV2Mo10. This confirmative state made us to use TBA-PV2Mo10@PVA during the ODS process of gasoline.
The surface morphology of TBA-PV2Mo10@PVA nanocomposite was investigated by SEM. A typical SEM picture of the as prepared TBA-PV2Mo10@PVA catalyst is shown in Fig. 5. From Fig. 5(a), the blank PVA film is observed to be relatively flat surface and Fig. 5(b) shows TBA-PV2Mo10 consist of very small agglomerated nanoparticle. This picture (Fig. 5 c) shows non regular morphology. Nanocomposite TBA-PV2Mo10@PVA is made and the estimated particle sizes are seen to be nano-scale. The SEM images, Fig. 5(c), of TBA-PV2Mo10@PVA present the self- assembly of TBA-PV2Mo10 with PVA. The structures of the nanocomposite TBA-PV2Mo10@PVA conform that the rate of stirring as well as the given temperature is optimum, which led to appropriate nanoshape. The presence of Keggin type of TBA-PV2Mo10 on PVA, as substrate, indicates an interaction between them that was according to our expectations and can satisfy to be as an efficient catalyst for next project.
The powder nanostructures were investigated by X-ray diffraction (XRD) measurement (25). XRD patterns of TBA-PV2Mo10, PVA and TBA-PV2Mo10@PVA are shown in Fig. 6 and were collected in the range 2θ = 5°–70° and continuous scan mode. XRD patterns (a), (b) and (c) in Fig. 6 corresponded to TBA-PV2Mo10, PVA and TBA-PV2Mo10@PVA respectively. It is obviously seen that in the XRD patterns of keggin type POM special peak has appeared. The existence of sharp peaks in 5°-10° can prove the structure of synthesized TBA-PV2Mo10 as a Keggin type POM. Besides, the peaks at 15°-20° and 30° are important to be sure about the structure. According to previous reporting, the XRD pattern of pure PVA must have a sharp peak in 19.8° (21). Fig. 6 consists of required information of PVA and TBA-PV2Mo10. It can be seen that the diffraction of PVA is overlapped by TBA-PV2Mo10 so the intensity around 20° is decreased. Therefore, TBA-PV2Mo10 has immobilized on PVA with a good interaction between them. Scherer equation (D = 0.89λ/βcosθ) was used to calculate the nano crystallite size by XRD radiation of wavelength from measuring full width at half maximum of peaks in radian located at any 2θ in the pattern. The mean crystal size obtained was around 21 nm.
Nuclear magnetic resonance (NMR) of the different active nuclei constituting POM is considered to be a very powerful method to clear their molecular structures both in solution and in the solid state. The 31P NMR spectrum of TBA-PV2Mo10 and TBA-PV2Mo10@PVA in DMSO at ~25 °C was a clear single line spectrum at -3.9 ppm due to the internal phosphorus atom, thereby confirming the compound's purity (it suggested that no other P-related impurities present), as shown in Fig. 7. According to Fig. 1-5 it is proved that TBA-PV2Mo10 is put on polymer matrixes thus the useful nanocatalyst is synthesized in its efficient way for developing the next step which is desulfurization of gasoline.
General desulfurization process
A model oil was made by adding Th and BT into n-heptane solvent, with a total sulfur concentration of 500 mg/L. The MSCs are mixed with CH3OOH/H2O2 and TBA-PV2Mo10@PVA then the ODS takes place at 35 °C under atmospheric pressure. This is followed by a polar liquid extraction (CH3COOH) to obtain gasoline with low sulfur. H2O2 first reacts with organic acid (CH3COOH) quickly and generates peracid (CH3COOOH). CH3COOOH can efficiency converts MSCs to sulfones without forming a substantial amount of residual product. The nanocatalyst accepted the active oxygen from the oxidant H2O2 to form new oxoperoxo species mediate. The role of the metal atoms, W or V, is to form peroxo-metal species which are able to activate the H2O2 and peracid molecules. The cation with carbon chain transferred oxoperoxo species to the substrates (Th or BT) and made the ODS process accomplish completely. This mechanism involves in the first step the easy formation of the peroxometalate species (27).
ODS of real gasoline
From the results of Table 1, after oxidation process, total sulfur content (Entry 4) and content of mercaptans (Entry 6) were very low, while other properties of gasoline remained unaffected. Also, it was demonstrated that the mercaptan scavenger, TBA-PV2Mo10@PVA, can catalyze the ODS process in 2 h and reduce total sulfur content of gasoline from 0.398 wt.% to 0.012 wt.% and also, reduce content of mercaptans from 87 ppm to 3 ppm.
Effect of the catalyst structure
As determined in previous work, the catalytic activity of the catalysts depends on the polyoxometalate anion and cation (6,7). The effect of the nature of the catalyst on the oxidative desulfurization of gasoline using CH3COOH/H2O2 as the oxidant is shown in Tables 1 and 4. The amount of each catalyst was constant throughout the series. Blank experiment was performed in the absence of catalyst. Under these conditions, percent conversion was very low (22% in 2 h) at 35 °C (Table 3, entry 9). The results show that the catalytic activity of TBA-PV2Mo10@PVA nanocomposite has presented much higher than other unsupported polyoxometalates (Fig. 8). Also in Fig. 8, the catalytic activity of supported and unsupported catalyst with H2O2 (3 and 4) and without H2O2 (1 and 2) were compared. The supported keggin type polyoxometalate catalyst TBA-PV2Mo10 was very active systems for the oxidation of BT, while other studied polyoxometalates systems were very less active. This system TBA-PV2Mo10@PVA with a phase transfer or emulsion catalyst comprising a quaternary ammonium salt-based polyoxometalate is shown to be very active system for ODS of BT and real gasoline. This quaternary ammonium Keggin type which has lipophilic cation act as phase transfer agent and transfer the peroxometal anion into organic phase. That is, the oxidation reactivity of the catalysts depends on the type of countercation: ((C4H9)4N)+ > NH4+ > K+. Also, the vanadium-substituted Keggin type polyoxometalate catalyst was very active systems for the ODS of gasoline.
Effect of Catalyst dosage
Another factor that should be concerned is the catalyst dosage. It was found that the catalyst dosage has a marked influence on the efficiency of process (Table 4). Under oxidation, without catalyst TBA-PV2Mo10@PVA (blank), 24% of the Th, 23% of the BT and 23% of real gasoline are removed from the n-heptane phase in 120 min. Percent conversion of real gasoline in the presence of TBA-PV2Mo10@PVA were found to be 68%, 88% and 97%, corresponding to catalyst amount of 0.06, 0.08 and 0.1 gr respectively. Desulfurization efficiency increased rapidly with the increase of catalyst dosage (Fig. 9). The results indicate that, increasing the dosage of catalyst, more peroxo-polyoxo compound species can be formed and therefore deepens reaction. The increasing catalyst quantity (TBA-PV2Mo10@PVA) enhances the removal rate of sulfur because the concentration of the catalytically active species (Mo (O2)n−Q+) increased. Results revealed that TBA-PV2Mo10@PVA is active for the oxidation of sulfur compounds and more than 97% of the total sulfur removal was obtained during the ODS process. The results are summarized in Table 4.
Effect of temperature
The reaction was carried out at different temperatures under the same conditions by TBA-PV2Mo10@PVA as a catalysts and CH3COOH/H2O2 as oxidant. The results are shown in Table 5 and Fig. 10. The results show that yields of products are a function of temperature. Percent conversion of sulfur in model fuel and in real gasoline has increased with temperature and time (Fig. 10). Percent conversion of sulfur in simulated fuel at 35 ºC is higher than at 30 ºC. 97% conversion of sulfur was obtained at 35 ºC in 120 min. The effects of reaction time and temperature on benzothiophene oxidation are shown in Fig. 10 (a). At low temperature, the oxidative conversion of BT was very low, which increased gradually with increase in reaction time. At 25 and 30 °C, the BT conversion reached 72% and 84% after 120 min of reaction time, respectively. The oxidation rate of BT increased rapidly with increase in temperature. At 35 °C, 97% conversion was attained in 2 h. The oxidation of Th was also found to increase with temperature and reaction time (Fig. 10(b)). At 25 and 30 °C, maximum conversions of 74% and 89% were attained in 2 h, while at 35 °C, more than 98% conversion of BT was achieved in 120 min reaction time.
Effect of different oxidative system on the ODS process
Effect of oxidative system on the ODS of gasoline was studied (Table 6). Hydrogen peroxide, KMnO4 and K2Cr2O5 were selected as oxidizing agents which were used in the presence of organic or inorganic acids such as; acetic acid, oxalic acid, benzoic acid, H2SO4 and H2CO3 to acidify the system. The results in Table 6 showed oxidation reactivity in inorganic acids, H2SO4 and H2CO3, are lower than organic acids. H2SO4 and H2CO3 cannot dissolve in real gasoline; therefore % sulfur removal of gasoline in inorganic acid/H2O2 was lower than organic acid/H2O2 system. Among these acids, HCOOH and CH3COOH are inexpensive reagents. CH3COOH has lesser toxicity than HCOOH. Thus, in the current study for ODS of gasoline the H2O2 in the presence of organic acid (CH3COOH) were used as oxidants. The results are shown in Table 6, which indicates that the oxidation of real gasoline carried out in the presence of H2O2 without acetic acid resulted in a maximum of 78% conversion of all the sulfur compounds (entry 6). In the presence of acetic acid but no H2O2, the maximum conversion was 49% (entry 7). These results indicated that the oxidation of the sulfur compounds is governed by peracetic acid (CH3COOOH), which is formed by the reaction of H2O2 and CH3COOH. In the absence of CH3COOH or H2O2, no peracetic acid was formed and only H2O2 or CH3COOH resulted in a low removal of total sulfur or mercaptan of real gasoline (entry 6 and 7).
Effect of the amount of acetic acid
Effect of the amount of acetic acid on the ODS of different sulfur compounds was studied and the results are given in Table 7. In the acetic acid catalyzed reaction, the acetic acid can interact with sulfur without any steric hindrance from alkyl groups. Therefore, the reactivity trend obtained in the acetic acid catalyzed reactions reflects the intrinsic oxidation reactivity of the BT. The percent sulfur removal of the mode fuel increased with increasing acetic acid. A mixture of acetic acid: H2O2 in ratio of 1:1 was better than the other mole ratio. Therefore, in all the subsequent experiments, this acetic acid/ H2O2 mole ratio was used. The gasoline mixed with acetic acid/H2O2 (peracetic acid) and the oxidative reaction occurred below 40 °C under atmospheric pressure.
Mechanism of the oxidative desulfurization reaction
The mechanism of sulfide oxidation to sulfoxides using H2O2-organic acid is not studied sufficiently; however, the potential mechanism is a heterolytic electrophyl interaction where H+X- is a polar solvent (23). Based on this mechanism, hydrogen peroxide fist reacts with organic acid (acetic acid) and produces peroxide acid (CH3COOOH), and then the acid reacts with nonpolar sulfur compounds and generates relative sulfone or sulfoxide. The role of the metal atoms in TBA-PV2Mo10@PVA, M = W or Mo, is to form peroxo-metal species which are able to activate the H2O2 and peracid molecules. During the ODS process, the H2O2 can efficiency convert organic sulfur to sulfones without forming a substantial amount of residual product. TBA-PV2Mo10@PVA accepted the active oxygen from the oxidant H2O2 to form new oxoperoxo species mediate. The cation with carbon chain transferred oxoperoxo species to the substrates (Th or BT) and made the oxidation reaction accomplish completely (Fig. 11).
Kinetics of BT oxidation
For better understand the catalytic oxidation of BT, reaction kinetics was examined. To the apparent consumption of BT, the constant rate was gained from the ﬁrst-order kinetic model (Eq. (3)) as follows:
Constant rate of BT was calculated using their initial concentrations at time zero (Co) and time t reaction (Ct) in the plot of ln(C/C0) or C/C0 against t with use of Eq. (5), an exponential line (C/C0) with slope k was gained (Fig. 12). The relationship between C and t can be applied to describe rate equations. With increasing reaction temperature from 25 to 35 °C removal of BT and thiophene and the constant rate reaction also increasing in 2 h (Table 8). The affiliation of the rate constant k on the reaction temperature can be expressed with the Arrhenius equation (Eq. (6)). A is the pre-exponential factor, Ea the apparent activation energy, R and T are gas constant and the reaction temperature (K), respectively (21,28). Fig. 13 shown the Arrhenius plots and the calculated Ea values for the oxidation of BT and Th are 61.21 and 54.7 kJ/mol, respectively.
Influence of recycle times on oxidative desulfurization
At the end of the ODS of the MSCs and real gasoline, the catalyst was filtered and washed with dichloromethane. In order to determine whether TBA-PV2Mo10@PVA would succumb to poisoning and lose its catalytic activity during the reaction, the reusability of TBA-PV2Mo10@PVA was investigated. For this purpose, we carried out the desulfurization reaction of gasoline and model compounds in the presence of fresh and recovered TBA-PV2Mo10@PVA. The catalyst recovered after the reactions were characterized, in order to check the catalysts stability. Fig. 14 illustrates XRD pattern and IR spectra of TBA-PV2Mo10@PVA after five catalytic cycles. Even after five runs for the reaction, the catalytic activity of TBA-PV2Mo10@PVA was almost the same as that of freshly used catalyst. The results are summarized in Table 9.
In conclusion, the TBA-PV2Mo10@PVA nano-composite has been successfully prepared by immobilization of TBA-PV2Mo10 on PVA as a new nanocatalyst for ODS of gasoline. The catalytic activity of the catalyst was carried out on various MSCs and real gasoline. The organic sulfur compounds were removed using the peroxo-metal intermediate complex as a catalytic enhancer in the present of H2O2/CH3COOH as oxidant. The comparative experimental results were demonstrated that the desulfurization efficiency depended on the structure of the catalyst, nature of the sulfur molecules, reaction temperature, and dosage of the nanocatalyst. At the end, the heterogeneous nanocatalyst was reused up to five regeneration cycles. This work was introduced as a facile method for the synthesized phase transfer nanocatalyst TBA-PV2Mo10@PVA and its application in the ODS treatment to promote the quality of gasoline fuel. The TBA-PV2Mo10@PVA nanoparticle was very active catalyst system for desulfurization of the models compound, while unmodified TBA-PV2Mo10 showed much lower activity. This TBA-PV2Mo10/PVA/H2O2/CH3COOH system provides an efficient, convenient and practical method for oxidative desulfurization of gasoline and the advantages of this method are nontoxic, mild condition and environmentally friendly.
CONFLICT OF INTERESTS
The authors declare that there is no conflict of interests regarding the publication of this paper.
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