# Investigation of Influential Parameters in Deep Oxidative Desulfurization of Dibenzothiophene with Hydrogen Peroxide and Formic Acid

Authors: Alireza Haghighat Mamaghani; Shohreh Fatemi; Mehrdad Asgari
Journal: International Journal of Chemical Engineering
 (2013)

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## Abstract

An effective oxidative system consisting of hydrogen peroxide, formic acid, and sulfuric acid followed by an extractive stage were implemented to remove dibenzothiophene in the simulated fuel oil. The results revealed such a great performance in the case of H2O2 in the presence of formic and sulfuric acids that led to the removal of sulfur compounds. Sulfuric acid was employed to increase the acidity of media as well as catalytic activity together with formic acid. The oxidation reaction was followed by a liquid-liquid extraction stage using acetonitrile as a polar solvent to remove produced sulfones from the model fuel. The impact of operating parameters including the molar ratio of formic acid to sulfur (nF/nS), hydrogen peroxide to sulfur (nO/nS), and the time of reaction was investigated using Box-Behnken experimental design for oxidation of the model fuel. A significant quadratic model was introduced for the sulfur removal as a function of effective parameters by the statistic analysis.


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## Body

## 1. Introduction

Deep desulfurization of diesel fuel has become an important issue due to the legislative regulations to reduce sulfur content in most countries (e.g., 15 ppmw since 2006 in the US and 10 wppm since 2008 in the EU) [1, 2]. Hydrodesulfurization (HDS) is the process most widely used in refineries to remove sulfur compounds from liquid hydrocarbons by transforming them to hydrogen sulfide. This process is catalytically carried out in the presence of hydrogen under severe reaction conditions such as high temperature and high pressure [3].However, it has been recognized that the achievement of almost zero values of sulfur in fuels has to be done through the combination of HDS process with complementary reactions. Studies reveal that sulfur compounds remaining in diesel fuel after HDS process, at sulfur level lower than 0.1% wt., are generally thiophene, benzothiophene, dibenzothiophene, and their derivatives. These compounds exhibit low HDS reactivity because of the strict hindrance for the interaction between sulfur and active sites on the catalyst [3]. As a result, to remove refractory sulfur compounds with HDS, more severe operating conditions are needed, including higher temperature and pressure, more active catalysts, and longer residence time, which lead to large hydrogen consumption and reduction of catalyst life. To solve the shortcomings of the HDS process to remove refractory sulfur compounds, several new processes including oxidative desulfurization (ODS), selective adsorption, and biodesulfurization have been developed as alternative or complementary technologies to HDS.Among these processes, oxidative desulfurization is regarded as one of the most promising methods to face the environmental regulation necessitating ultralow sulfur fuels. The greatest advantage of ODS is mild reaction conditions including ambient pressure and relatively low temperatures. Another crucial feature of ODS is that most refractory sulfur-containing compounds of HDS process such as dibenzothiophene (DBT) show high reactivity toward ODS process and are easily converted by oxidation. In addition, ODS does not use expensive and corrosive hydrogen. From chemical point of view, ODS process consists of two major steps. In the first step, sulfur-containing compounds are oxidized by an oxidizing agent such as hydrogen peroxide to their corresponding sulfones or sulfoxides. At the second stage, these highly polarized products are removed from the fuels by adsorption or liquid-liquid extraction [4, 5]. Various oxidation systems for ODS process with different oxidants and catalysts have been employed, such as H2O2/acetic acid [6–8], H2O2/formic acid [4, 9, 10], H2O2/heterogeneous catalysts [11–13], H2O2/ionic liquid [14, 15] oxygen/aldehyde [16], ozone/heterogeneous catalysts [17], and tert-butyl hydroperoxide/heterogeneous catalysts [18–20]. Hydrogen peroxide is the most common oxidant for ODS proces, because it is cheap, environmentally friendly, and commercially available. Another advantage of H2O2 is that it can be joined with various types of catalysts to oxidize sulfur compounds effectively. Zhu et al. [21] performed the oxidation of DBT with hydrogen peroxide, peroxotungsten and peroxomolybdenum complexes as catalyst. In another study, Napanang and Sooknoi [22] examined the oxidative extractive desulfurization of thiophene on titanosilicate-1 with different solvents in the presence of H2O2. Zhang et al. [23] also examined in situ production of hydrogen peroxide by oxidation of propanol to oxidize thiophene derivative compounds.Using hydrogen peroxide with an acid has been widely investigated by several researchers. However, to the best knowledge of the authors, there are few studies which are concerned with optimizing the process parameters. The objective of the present work is to develop an efficient system for oxidative desulfurization of model fuel. ODS of dibenzothiophene (DBT) inn-octane as simulated fuel was performed in the presence of H2O2, formic acid, and H2SO4 as the oxidation system. After the oxidation step, a two-step liquid-liquid extraction with acetonitrile was applied to remove the oxidated sulfur compounds from the model fuel. Influences of operating conditions including H2O2/S molar ratio, acid formic/S molar ratio, oxidation duration time, and medium acidity were examined. The extraction step was carried out at the same conditions in all experiments. Box-Behnken experimental design was implemented as a kind of response surface methodology (RSM) to arrange the experiments and develop a model to explain the relationships of sulfur removal and the studied parameters and finally optimize the operating conditions.


## 2. Experimental

### 2.1. Materials and Methods

All chemicals used in the present investigation, includingn-octane (99.9%), hydrogen peroxide (30% aqueous solution), dibenzothiophene (DBT), sulfuric acid (95–98%), formic acid (99%), and acetonitrile (98%), were used with no further treatment. Hydrogen peroxide and formic acid were implemented as oxidants, sulfuric acid was used to adjust pH in the desired range, acetonitrile was exploited as solvent to extract oxidized DBT from the organic phase, n-octane was used as a model fuel, and dibenzothiophene served as the model sulfur compound.An Agilent 6890 plus a gas chromatography system (GC) coupled with a flame ionization detector (GC-FID) using a HP-5 capillary column was applied to detect sulfur-containing compounds and identify their concentrations in model fuel and product. In this analysis, helium was used as a carrier gas with volumetric flow of 1.1 mL/min. The sample volume of 2μL was injected into the column without any further solvent dilution. The column temperature was first kept at 100°C for 2 minutes and then was heated from 100 to 280°C at 10°C/min with a final isothermal period of 10 minutes at 280°C.


### 2.2. Procedure

To prepare a solution which could behave as an appropriate sample of real fuel, the model fuel was prepared by dissolving calculated amount of DBT inn-octane, in order to obtain a solution with initial sulfur concentration of 250 ppmw. A typical set of experiments was designed and carried out as follows.A 100 mL three-necked glass was applied as the reactor in the present investigation. This vessel was also equipped with a magnetic stirrer, a thermometer, and a reflux condenser which was placed in a constant-temperature water bath (within ±0.1°C). At first, 50 mL of the sample fuel was poured into the reactor and heated to the desired temperature. In all experiments, the temperature was set at 65°C, as the optimal temperature for ODS in the presence of hydrogen peroxide [9]. Then, a proper amount of sulfuric acid (95–98%) was added to the system leisurely, and the mixture was stirred simultaneously. The pH of the solution was carefully measured by a digital pH meter and adjusted to the value of 1.5.After the solution was stirred vigorously for a few minutes, a suitable amount of hydrogen peroxide (30% aqueous solution) was added to the reaction mixture immediately. The value of added hydrogen peroxide was chosen in different levels as the experimental design. By addition of hydrogen peroxide, the reaction started. At the same time, an appropriate amount of formic acid (99%) was introduced to the reactor. Then the mixture was stirred at 700 RPM by a magnetic stirrer during reaction time. After a period of time, the solution was treated by means of liquid-liquid extraction. In each extraction stage, an equal amount of acetonitrile were employed to maintain extraction conditions identical for all cases. The extraction in each step was performed as follows: equal volume of the fuel, after oxidation step, and acetonitrile were decanted into a glass beaker. The beaker was shaken for 5 minutes at room temperature. After separating the aqueous and organic phases and replicating the second stage of extraction at the same condition, the final organic solution was analyzed by GC to detect the amount of DBT in the resulted model fuel. It should be mentioned that because the procedure of solvent extraction was kept identical in all experiments; any difference occurred in DBT detection of the resulted fuel would be related to the oxidation stage in different test runs.


### 2.3. Parameters

Efficiency of sulfur removal by an oxidative process is affected by various parameters. Some of these parameters were fixed from the previous studies to reduce the number of experiments. The amount of sulfuric acid, temperature of reaction, and solvent extraction were fixed according to the prior experiments and derived from the literature. However, the effects of acidity, temperature, and extraction are discussed below before applying for the variables of this work.


#### 2.3.1. Acidity

Sulfuric acid is a very strong acid in aqueous mediums. Using sulfuric acid reduces pH of the media considerably and enhances DBT conversion significantly. Decomposition rate of hydrogen peroxide to form hydroxyl radicals was reported to be related to the aqueous phase pH [10]. Due to these results, as aqueous phase pH value decreases from 5 to 1.5, DBT conversion enhances about 30%. Improvement in experimental results could be attributed to redox potential. Redox potential of H2O2 and hydroxyl radicals was influenced by pH media. At pH = 0, redox potential for H2O2 and HO was 1.77 and 2.8, respectively, whereas these values were 0.88 and 2 for H2O2 and HO at pH = 14, respectively [24]. Therefore, addition of sulfuric acid to the aqueous phase results in pH reduction and consequently increases redox potential of H2O2 and hydroxyl radicals. An experiment was designed and performed in order to investigate the effect of aqueous phase acidity on the oxidation of dibenzothiophene with H2O2/HCOOH system. In this experiment, the oxidative desulfurization was done with and without sulfuric acid, while all other parameters were kept identical. Table 1 shows the results of these two experiments. By comparing these results, it is obvious that aqueous phase acidity has a vital effect on sulfur removal. So, due to our preliminary experiments, the pH of the aqueous phase is maintained in the value of 1.5 in order to obtain better efficiency.Table 1
Effect of aqueous phase acidity.
Oxidative system
Sulfur removal (%)
H2O2/formic acid
75
H2O2/formic acid/acid sulfuric
97


#### 2.3.2. Temperature

Temperature plays an important role in the efficiency of a oxidative system. An increase in the reaction temperature results in a considerable increase in the reaction rate. However, carrying out the oxidation reaction at high temperatures causes thermal decomposition of hydrogen peroxide to undesirable products and reduces the quality of the fuel; therefore, an optimal temperature is required. Temperature and molar ratio of H2O2 have shown interactive effects [5, 6]. In this study, the temperature of reaction was fixed at 65°C but three levels of H2O2 molar ratios were examined and analyzed by the experimental design to obtain a better knowledge of the oxidant concentration effect.


#### 2.3.3. Solvent Extraction

During the oxidation reaction, dibenzothiophene (DBT) converts to sulfone and sulfoxide which are more polar components than DBT due to the presence of sulfur-oxygen bond in their structure. The oxidized-DBT compounds could be removed easily by contacting the treated fuel with a proper polar solvent. This process results in the transfer of oxidized sulfur compounds from model fuel to the more polar solvent which is highly favorable in the thermodynamic point of view. It is because during the transfer of oxidized sulfur compounds, such as DBT sulfones and DBT sulfoxides, from a nonpolar model fuel to a polar solvent, entropy increases sharply. But the important point is to choose a proper solvent in order to optimize the extraction process economically and technically. To choose a suitable solvent, not only the polarity of solvent should be considered, but also the boiling point, density, viscosity, surface tension, toxicity, price, and especially oil-recovery properties should be investigated. Considering these properties, acetonitrile was selected as the appropriate solvent for the extraction of oxidized-DBT compounds. It would be an appropriate choice because of its sulfone removal efficiency, oil recovery, and easy separation [7]. Furthermore, acetonitrile shows a high extraction activity for the sulfone which is a highly polarized and hydrophobic compound [6, 25]. On the other hand, a set of experiments was designed in order to validate the results of previous works.In addition, the amount of DBT in model fuel was measured, before and after extraction to find out the effect of extraction step on removal of DBT and sulfones, and it was revealed that negligible amount of DBT could be removed by the lonely process of extraction, whereas the most part of sulfur removal was due to the extraction of polar sulfones and/or sulfoxides by acetonitrile. Therefore, desulfurization by means of oxidative method followed by extraction should be applied as an appropriate method to treat the fuel [9].


## 2.1. Materials and Methods

All chemicals used in the present investigation, includingn-octane (99.9%), hydrogen peroxide (30% aqueous solution), dibenzothiophene (DBT), sulfuric acid (95–98%), formic acid (99%), and acetonitrile (98%), were used with no further treatment. Hydrogen peroxide and formic acid were implemented as oxidants, sulfuric acid was used to adjust pH in the desired range, acetonitrile was exploited as solvent to extract oxidized DBT from the organic phase, n-octane was used as a model fuel, and dibenzothiophene served as the model sulfur compound.An Agilent 6890 plus a gas chromatography system (GC) coupled with a flame ionization detector (GC-FID) using a HP-5 capillary column was applied to detect sulfur-containing compounds and identify their concentrations in model fuel and product. In this analysis, helium was used as a carrier gas with volumetric flow of 1.1 mL/min. The sample volume of 2μL was injected into the column without any further solvent dilution. The column temperature was first kept at 100°C for 2 minutes and then was heated from 100 to 280°C at 10°C/min with a final isothermal period of 10 minutes at 280°C.


## 2.2. Procedure

To prepare a solution which could behave as an appropriate sample of real fuel, the model fuel was prepared by dissolving calculated amount of DBT inn-octane, in order to obtain a solution with initial sulfur concentration of 250 ppmw. A typical set of experiments was designed and carried out as follows.A 100 mL three-necked glass was applied as the reactor in the present investigation. This vessel was also equipped with a magnetic stirrer, a thermometer, and a reflux condenser which was placed in a constant-temperature water bath (within ±0.1°C). At first, 50 mL of the sample fuel was poured into the reactor and heated to the desired temperature. In all experiments, the temperature was set at 65°C, as the optimal temperature for ODS in the presence of hydrogen peroxide [9]. Then, a proper amount of sulfuric acid (95–98%) was added to the system leisurely, and the mixture was stirred simultaneously. The pH of the solution was carefully measured by a digital pH meter and adjusted to the value of 1.5.After the solution was stirred vigorously for a few minutes, a suitable amount of hydrogen peroxide (30% aqueous solution) was added to the reaction mixture immediately. The value of added hydrogen peroxide was chosen in different levels as the experimental design. By addition of hydrogen peroxide, the reaction started. At the same time, an appropriate amount of formic acid (99%) was introduced to the reactor. Then the mixture was stirred at 700 RPM by a magnetic stirrer during reaction time. After a period of time, the solution was treated by means of liquid-liquid extraction. In each extraction stage, an equal amount of acetonitrile were employed to maintain extraction conditions identical for all cases. The extraction in each step was performed as follows: equal volume of the fuel, after oxidation step, and acetonitrile were decanted into a glass beaker. The beaker was shaken for 5 minutes at room temperature. After separating the aqueous and organic phases and replicating the second stage of extraction at the same condition, the final organic solution was analyzed by GC to detect the amount of DBT in the resulted model fuel. It should be mentioned that because the procedure of solvent extraction was kept identical in all experiments; any difference occurred in DBT detection of the resulted fuel would be related to the oxidation stage in different test runs.


## 2.3. Parameters

Efficiency of sulfur removal by an oxidative process is affected by various parameters. Some of these parameters were fixed from the previous studies to reduce the number of experiments. The amount of sulfuric acid, temperature of reaction, and solvent extraction were fixed according to the prior experiments and derived from the literature. However, the effects of acidity, temperature, and extraction are discussed below before applying for the variables of this work.


### 2.3.1. Acidity

Sulfuric acid is a very strong acid in aqueous mediums. Using sulfuric acid reduces pH of the media considerably and enhances DBT conversion significantly. Decomposition rate of hydrogen peroxide to form hydroxyl radicals was reported to be related to the aqueous phase pH [10]. Due to these results, as aqueous phase pH value decreases from 5 to 1.5, DBT conversion enhances about 30%. Improvement in experimental results could be attributed to redox potential. Redox potential of H2O2 and hydroxyl radicals was influenced by pH media. At pH = 0, redox potential for H2O2 and HO was 1.77 and 2.8, respectively, whereas these values were 0.88 and 2 for H2O2 and HO at pH = 14, respectively [24]. Therefore, addition of sulfuric acid to the aqueous phase results in pH reduction and consequently increases redox potential of H2O2 and hydroxyl radicals. An experiment was designed and performed in order to investigate the effect of aqueous phase acidity on the oxidation of dibenzothiophene with H2O2/HCOOH system. In this experiment, the oxidative desulfurization was done with and without sulfuric acid, while all other parameters were kept identical. Table 1 shows the results of these two experiments. By comparing these results, it is obvious that aqueous phase acidity has a vital effect on sulfur removal. So, due to our preliminary experiments, the pH of the aqueous phase is maintained in the value of 1.5 in order to obtain better efficiency.Table 1
Effect of aqueous phase acidity.
Oxidative system
Sulfur removal (%)
H2O2/formic acid
75
H2O2/formic acid/acid sulfuric
97


### 2.3.2. Temperature

Temperature plays an important role in the efficiency of a oxidative system. An increase in the reaction temperature results in a considerable increase in the reaction rate. However, carrying out the oxidation reaction at high temperatures causes thermal decomposition of hydrogen peroxide to undesirable products and reduces the quality of the fuel; therefore, an optimal temperature is required. Temperature and molar ratio of H2O2 have shown interactive effects [5, 6]. In this study, the temperature of reaction was fixed at 65°C but three levels of H2O2 molar ratios were examined and analyzed by the experimental design to obtain a better knowledge of the oxidant concentration effect.


### 2.3.3. Solvent Extraction

During the oxidation reaction, dibenzothiophene (DBT) converts to sulfone and sulfoxide which are more polar components than DBT due to the presence of sulfur-oxygen bond in their structure. The oxidized-DBT compounds could be removed easily by contacting the treated fuel with a proper polar solvent. This process results in the transfer of oxidized sulfur compounds from model fuel to the more polar solvent which is highly favorable in the thermodynamic point of view. It is because during the transfer of oxidized sulfur compounds, such as DBT sulfones and DBT sulfoxides, from a nonpolar model fuel to a polar solvent, entropy increases sharply. But the important point is to choose a proper solvent in order to optimize the extraction process economically and technically. To choose a suitable solvent, not only the polarity of solvent should be considered, but also the boiling point, density, viscosity, surface tension, toxicity, price, and especially oil-recovery properties should be investigated. Considering these properties, acetonitrile was selected as the appropriate solvent for the extraction of oxidized-DBT compounds. It would be an appropriate choice because of its sulfone removal efficiency, oil recovery, and easy separation [7]. Furthermore, acetonitrile shows a high extraction activity for the sulfone which is a highly polarized and hydrophobic compound [6, 25]. On the other hand, a set of experiments was designed in order to validate the results of previous works.In addition, the amount of DBT in model fuel was measured, before and after extraction to find out the effect of extraction step on removal of DBT and sulfones, and it was revealed that negligible amount of DBT could be removed by the lonely process of extraction, whereas the most part of sulfur removal was due to the extraction of polar sulfones and/or sulfoxides by acetonitrile. Therefore, desulfurization by means of oxidative method followed by extraction should be applied as an appropriate method to treat the fuel [9].


## 2.3.1. Acidity

Sulfuric acid is a very strong acid in aqueous mediums. Using sulfuric acid reduces pH of the media considerably and enhances DBT conversion significantly. Decomposition rate of hydrogen peroxide to form hydroxyl radicals was reported to be related to the aqueous phase pH [10]. Due to these results, as aqueous phase pH value decreases from 5 to 1.5, DBT conversion enhances about 30%. Improvement in experimental results could be attributed to redox potential. Redox potential of H2O2 and hydroxyl radicals was influenced by pH media. At pH = 0, redox potential for H2O2 and HO was 1.77 and 2.8, respectively, whereas these values were 0.88 and 2 for H2O2 and HO at pH = 14, respectively [24]. Therefore, addition of sulfuric acid to the aqueous phase results in pH reduction and consequently increases redox potential of H2O2 and hydroxyl radicals. An experiment was designed and performed in order to investigate the effect of aqueous phase acidity on the oxidation of dibenzothiophene with H2O2/HCOOH system. In this experiment, the oxidative desulfurization was done with and without sulfuric acid, while all other parameters were kept identical. Table 1 shows the results of these two experiments. By comparing these results, it is obvious that aqueous phase acidity has a vital effect on sulfur removal. So, due to our preliminary experiments, the pH of the aqueous phase is maintained in the value of 1.5 in order to obtain better efficiency.Table 1
Effect of aqueous phase acidity.
Oxidative system
Sulfur removal (%)
H2O2/formic acid
75
H2O2/formic acid/acid sulfuric
97


## 2.3.2. Temperature

Temperature plays an important role in the efficiency of a oxidative system. An increase in the reaction temperature results in a considerable increase in the reaction rate. However, carrying out the oxidation reaction at high temperatures causes thermal decomposition of hydrogen peroxide to undesirable products and reduces the quality of the fuel; therefore, an optimal temperature is required. Temperature and molar ratio of H2O2 have shown interactive effects [5, 6]. In this study, the temperature of reaction was fixed at 65°C but three levels of H2O2 molar ratios were examined and analyzed by the experimental design to obtain a better knowledge of the oxidant concentration effect.


## 2.3.3. Solvent Extraction

During the oxidation reaction, dibenzothiophene (DBT) converts to sulfone and sulfoxide which are more polar components than DBT due to the presence of sulfur-oxygen bond in their structure. The oxidized-DBT compounds could be removed easily by contacting the treated fuel with a proper polar solvent. This process results in the transfer of oxidized sulfur compounds from model fuel to the more polar solvent which is highly favorable in the thermodynamic point of view. It is because during the transfer of oxidized sulfur compounds, such as DBT sulfones and DBT sulfoxides, from a nonpolar model fuel to a polar solvent, entropy increases sharply. But the important point is to choose a proper solvent in order to optimize the extraction process economically and technically. To choose a suitable solvent, not only the polarity of solvent should be considered, but also the boiling point, density, viscosity, surface tension, toxicity, price, and especially oil-recovery properties should be investigated. Considering these properties, acetonitrile was selected as the appropriate solvent for the extraction of oxidized-DBT compounds. It would be an appropriate choice because of its sulfone removal efficiency, oil recovery, and easy separation [7]. Furthermore, acetonitrile shows a high extraction activity for the sulfone which is a highly polarized and hydrophobic compound [6, 25]. On the other hand, a set of experiments was designed in order to validate the results of previous works.In addition, the amount of DBT in model fuel was measured, before and after extraction to find out the effect of extraction step on removal of DBT and sulfones, and it was revealed that negligible amount of DBT could be removed by the lonely process of extraction, whereas the most part of sulfur removal was due to the extraction of polar sulfones and/or sulfoxides by acetonitrile. Therefore, desulfurization by means of oxidative method followed by extraction should be applied as an appropriate method to treat the fuel [9].


## 3. Experimental Design

A kind of response-surface methodology was used to design the experiments for studying the impact of molar ratios of hydrogen peroxide to sulfur, time of reaction, and ratio of acid formic to sulfur on desulfurization efficiency. The variable parameters, denoted byXi, were coded as −1, 0, and 1, for the low level, center point, and high level, respectively. A table with 15 test runs was made according to Box-Behnken experimental design for the three significant parameters. Those parameters are indicated in Table 2.Table 2
The amount and levels of the variables in experimental design.
Variable
Unit
Low level(−1)
Center point(0)
High level(+1)
H2O2/S (X1)
—
2
15
28
Time (X2)
min
50
100
150
Facid/S (X3)
—
2
20
38The experiments were performed in a random order to disperse the occurred random error in the whole region of the experiments. In addition, the center-point experiment was replicated twice to verify the reproducibility of the results. After running the experiments, the left amount of DBT and DBTO2 and the removal efficiency of sulfur was determined and presented in Table 3. Design Expert Software (version 8.0.5) was applied on the results to analyse the variance of the response with respect to the random error (ANOVA) to show the significant parameters and introduce a reliable model.Table 3
Coded and actual levels of variables with corresponding responses (initial sulfur concentration = 250 ppmw).
Experiment no.
Coded level of variables
Actual level of variables
Responses
X
1
X
2
X
3
X
1
X
2
X
3
S removal (%)
S (ppm)
1
−1
−1
0
2
50
20
95
12.5
2
1
−1
0
28
50
20
100
0
3
−1
1
0
2
150
20
85
37.5
4
1
1
0
28
150
20
100
0
5
−1
0
−1
2
100
2
91
22.5
6
1
0
−1
28
100
2
100
0
7
−1
0
1
2
100
38
93
17.5
8
1
0
1
28
100
38
100
0
9
0
−1
−1
15
50
2
98
5
10
0
1
−1
15
150
2
97
7.5
11
0
−1
1
15
50
38
99
2.5
12
0
1
1
15
150
38
100
0
13
0
0
0
15
100
20
100
0
14
0
0
0
15
100
20
100
0
15
0
0
0
15
100
20
100
0


## 4. Results and Discussion

### 4.1. Analysis of Variance

The impact of selected three parameters: hydrogen peroxide/S, formic acid/S molar ratio, and time of the reaction was investigated on sulfur removal efficiency, by the response-surface methodology using Box-Behnken statistical design. The weight fraction of sulfur removal was regarded as the response of the experiments. The effect of each variable was analyzed by analysis of variance with 90% confidence interval. A quadratic model was derived for sulfur conversion related to the variables shown in (1). The calculated Fischer values (F-test) and thereby the probability values (P value) were calculated, and the significance of each parameter was identified for P values of lower than 10%. The parameter X3 with P value of 21.8% was considered as the possibly significant parameter of the model, as can be seen in Table 4.Table 4
Effects and model coefficients for sulfur removal.
Terms
Mean sum of squares
Coefficients
F-value
P value
Significance*
Coded value
Actual value
Constant
41.8
99.8
92.32
17.01
0.000
HS
(H2O2/S) X1
162
4.5
0.62
65.93
0.000
HS
(Time)X2
12.5
−1.25
0.013
5.09
0.058
S
(Facid/S)X3
4.5
0.75
0.042
1.83
0.218
PS
X
1
X
2
25
2.5
0.0038
10.17
0.015
S
X
1
2
45.63
−3.7
−0.022
18.57
0.003
HS
X
2
2
4.8
−1.2
−0.0048
1.95
0.02
S
Residual
2.46
*
HS: highly significant, S: significant, and PS: possibly significant.ANOVA indicated that there is a linear relationship between the main effects (H2O2/S, formic acid/S, and time), as well as a quadratic relationship for H2O2/S and existence of binary interaction between time and H2O2/S molar ratio, for sulfur removal in oxidation reaction. The adjusted coefficient of determination was calculated sufficiently high (R2adj = 0.88), which shows a good agreement between the model and experiments. The final quadratic equation in terms of significant effects is presented below:
(1)SR(%)=92.32+0.62*X1+0.013*X2+0.042*X3-0.022*X12+0.004*X1*X2.The residual analysis of the model is presented in Figures1(a), 1(b), and 1(c). Figure 1(a) presents a standardized residual plot of the model response and experiment versus run order. The residuals are dispersed randomly around a line, and there has not been any outlier and leverage in the experiments. Figure 1(b) represents the normal probability plot of the residuals, which shows a linear relationship. It proves that the random error is independently and normally distributed. Figure 1(c) presents predicted model versus experimental response that shows a negligible scattering pattern around the bisector [26]. This informative approach implies that constructed model can predict the experiments with fairly well precision.Residual analysis of the predicted model for sulfur removal. (a) Residual versus the run number, (b) normal probability plot of residuals, and (c) predicted values against the actual values of response.
(a)
(b)
(c)Operational parameters are also optimized in such a way that oxidizing agent (i.e., H2O2) usage reaches its minimum. This value is selected as an oxidizing agent and is the most valuable and critical operating parameter in the set of experiments.The optimal operational conditions were determined at O/S = 15, formic acid/S = 22, and 56 min to achieve 100% sulfur removal from the fuel. In order to validate the optimization by statistical methods, an experiment was held in operating conditions which were obtained by statistical methods. Applying optimal conditions resulted in sulfur removal of 100% which verifies the accuracy of optimization by theoretical methods.


### 4.2. Influential Parameters

The effect of the studied parameters on sulfur removal is plotted in Figure2. It is obvious that increasing each parameter can significantly enhance the sulfur removal efficiency. A theoretical discussion will be described in the following sections.(a) Sulfur removal as a function of O/S, acid/S = 2, and time = 150 min. (b) Sulfur removal as a function of acid/S, O/S = 3, and time = 100 min. (c) Sulfur removal as a function of time, O/S = 28, and acid/S = 2 (oxidation condition:T = 65°C; aqueous phase pH = 1.5. Extraction condition: T = 22°C; solvent-to-oil phase volume ratio = 1; number of extraction stages = 2).
(a)
(b)
(c)


#### 4.2.1. Effect of O/S Molar Ratio

The effect of molar ratios of H2O2 to sulfur is exhibited in Figure 2(a). As indicated in Figure 2(a), sulfur removal initially increases, as the ratio of the oxidizing agent to sulfur-containing compound rises (i.e., the ratio of hydrogen peroxide to DBT). Then, after a specified level, the amount of oxidizing agent has no considerable effect on the sulfur removal anymore. Best results were obtained at the nO/nS = 18 at 65°C, and an increase in the O/S higher than 18 did not change the sulfur removal significantly. The initial molar H2O2/S concentration determines the initial hydrogen peroxide concentration in the reaction, which has an important impact on the formation of both hydroxyl radicals and performic acid. As mentioned before, according to the literature, these two species are the most effective agents of oxidation. So, it is obvious that by increasing the molar ratio of H2O2 to sulfur species, DBT conversion increases due to the formation of more hydroxyl radicals and performic acid. On the other hand, results have shown that high molar ratios of oxidizing agent to sulfur compound result in the decomposition of H2O2 into oxygen molecules, which eventually lead to loss of H2O2. Definitely this is not a desirable outcome. This means that greater amount of oxidizing agent beyond the proper level could have no affirmative impact on sulfur removal. The optimum value of O/S ratio is strongly dependent upon temperature because temperature can change the amount of decomposition rate significantly. At high temperature (50–70°C), the O/S molar ratio should be great enough (<10) to supply thermal decomposition of H2O2. However, for a temperature lower than 30–40°C, nO/nS can be closer to the stoichiometric ratio which is two [5, 6].Therefore, the initial H2O2/S molar ratio should be well controlled. It should be well noted that the stoichiometric ratio of H2O2 to DBT is two, whereas the excess amount of oxidant is usually required, which is more than the stoichiometric one. Several factors determine the necessity of extra amount of H2O2, including(1)
mass transfer problems between oil phase and aqueous phase;(2)
thermal decomposition of H2O2 to water and oxygen;(3)
parallel oxidation reactions of H2O2 [5].


#### 4.2.2. Formic Acid/S Molar Ratio

Figure2(b) shows the effect of molar ratios of formic acid to sulfur on the reactions while temperature and pH values of the solution are maintained at constant values of 65°C and 1.5, respectively. As it was expected, DBT conversion was promoted dramatically by increasing nF/nS. The results have shown an enhancement in DBT conversion by increasing the ratio of formic acid to sulfur from 2 to 20, whereas with a further increase in the ratio of formic acid to sulfur, the conversion rate did not increase remarkably. Formic acid could effectively enhance the oxidation because it acts as a cocatalyst in oxidation system and not only decreases the pH value of the aqueous phase, but also generates performic acid when it interacts with hydrogen peroxide. In addition to the polarization ability of O–O bond, oxidative catalytic feature of formic acid has been reported as an oxidizing agent by giving its oxygen atom to DBT and enhancing its conversion to sulfones and sulfoxides species [4, 5]. In addition, the small size of the formic acid molecule can facilitate its interaction with sulfur without any steric hindrance of alkyl groups. But like other oxidizing agents, it has an optimum value and increasing its amount to the upper level does not have any effect since its concentration would not act as a controlling parameter in the oxidation system anymore. So beyond an optimum level, increasing formic acid concentration could not enhance the oxidative desulfurization noticeably.


#### 4.2.3. Reaction Time

Figure2(c) shows sulfur removal as a function of reaction time. As it is indicated in this figure, the results were improved by increasing the time of the reaction initially and then slightly decrease. This could be explained by describing interaction of oxidizing agents as time proceeds. H2O2 and formic acid can interact with DBT to produce sulfones. This reaction like any other reaction needs enough time to complete and promotes as time goes on. Best results are observed at 125 min. After a particular reaction time, sulfur removal does not enhance by rising reaction time, which means there is an optimum time for oxidation system. Although it can be seen that after the optimum value as time proceeds sulfur removal value decreases, its decline is not sharp at all. This reduction in sulfur removal should be due to loss of hydrogen peroxide and performic acid and their decomposition which accelerates the conversion of oxidized sulfur compound to DBT. In other words, both the little amount of oxidizing agents and the long time of reaction result in the loss of all of the oxidizing agents, equilibrium change, and alteration of the reaction media from oxidizing to reducing one. But this trend never could be seen when the main oxidizing agent (i.e., hydrogen peroxide) exists in extra amount in solution. Because in such a condition there are excess amounts of hydroxyl and performic acid radicals over the whole reaction time, and the reaction medium remains as an oxidizing medium. So, carrying out the reaction in a long time especially whenever the oxidizing agent is in a little amount could have no benefit.


### 4.3. Interaction between H2O2/S Ratio and Time

The contour plot of H2O2/S and time is exhibited in Figure 3(a), which is very helpful in the study of the interactive effects of the factors of the sulfur removal. Figure 3(b) also represents a 3D plot of sulfur removal as a function of those two parameters. In both figures, the third factor (the ratio of formic acid to sulfur) was kept at a constant level of two. The interaction between time and O/S molar ratio arises at different time levels. When a high level of time is applied (150 minutes), sulfur removal increases by increasing O/S ratio because H2O2 and DBT have enough time to react with each other and produce sulfones. On the other hand, when the oxidative system does not have enough time (50 minutes) to interact with sulfur compounds, raising the O/S ratio not only causes side reactions involving the thermal decomposition of hydrogen peroxide, but also increases the amount of water in the reaction medium. These results show the balance of two opposing factors (i.e., the excess of oxidant increases the activity, while the water produced from ODS reaction and thermal decomposition hinders the ODS reaction). In addition, it is suggested that in the presence of excess hydrogen peroxide, it acts as a hydroxyl radical scavenger that leads to the generation of less active perhydroxyl radicals [27]. This effect eventually inhibited the oxidation of organic pollutants in the aqueous phase. The best results are found in the region where the ration is limited to 13 < O/S < 24 at a moderate level of time.(a) 2D contour plot and (b) 3D response surface curve of the constructed model displaying sulfur removal at different O/S and time. Oxidation condition:T = 65°C; aqueous phase pH = 1.5; acid/S = 20. Extraction condition: T = 22°C; solvent-to-oil volume ratio = 1; number of extraction stages = 2.
(a)
(b)


## 4.1. Analysis of Variance

The impact of selected three parameters: hydrogen peroxide/S, formic acid/S molar ratio, and time of the reaction was investigated on sulfur removal efficiency, by the response-surface methodology using Box-Behnken statistical design. The weight fraction of sulfur removal was regarded as the response of the experiments. The effect of each variable was analyzed by analysis of variance with 90% confidence interval. A quadratic model was derived for sulfur conversion related to the variables shown in (1). The calculated Fischer values (F-test) and thereby the probability values (P value) were calculated, and the significance of each parameter was identified for P values of lower than 10%. The parameter X3 with P value of 21.8% was considered as the possibly significant parameter of the model, as can be seen in Table 4.Table 4
Effects and model coefficients for sulfur removal.
Terms
Mean sum of squares
Coefficients
F-value
P value
Significance*
Coded value
Actual value
Constant
41.8
99.8
92.32
17.01
0.000
HS
(H2O2/S) X1
162
4.5
0.62
65.93
0.000
HS
(Time)X2
12.5
−1.25
0.013
5.09
0.058
S
(Facid/S)X3
4.5
0.75
0.042
1.83
0.218
PS
X
1
X
2
25
2.5
0.0038
10.17
0.015
S
X
1
2
45.63
−3.7
−0.022
18.57
0.003
HS
X
2
2
4.8
−1.2
−0.0048
1.95
0.02
S
Residual
2.46
*
HS: highly significant, S: significant, and PS: possibly significant.ANOVA indicated that there is a linear relationship between the main effects (H2O2/S, formic acid/S, and time), as well as a quadratic relationship for H2O2/S and existence of binary interaction between time and H2O2/S molar ratio, for sulfur removal in oxidation reaction. The adjusted coefficient of determination was calculated sufficiently high (R2adj = 0.88), which shows a good agreement between the model and experiments. The final quadratic equation in terms of significant effects is presented below:
(1)SR(%)=92.32+0.62*X1+0.013*X2+0.042*X3-0.022*X12+0.004*X1*X2.The residual analysis of the model is presented in Figures1(a), 1(b), and 1(c). Figure 1(a) presents a standardized residual plot of the model response and experiment versus run order. The residuals are dispersed randomly around a line, and there has not been any outlier and leverage in the experiments. Figure 1(b) represents the normal probability plot of the residuals, which shows a linear relationship. It proves that the random error is independently and normally distributed. Figure 1(c) presents predicted model versus experimental response that shows a negligible scattering pattern around the bisector [26]. This informative approach implies that constructed model can predict the experiments with fairly well precision.Residual analysis of the predicted model for sulfur removal. (a) Residual versus the run number, (b) normal probability plot of residuals, and (c) predicted values against the actual values of response.
(a)
(b)
(c)Operational parameters are also optimized in such a way that oxidizing agent (i.e., H2O2) usage reaches its minimum. This value is selected as an oxidizing agent and is the most valuable and critical operating parameter in the set of experiments.The optimal operational conditions were determined at O/S = 15, formic acid/S = 22, and 56 min to achieve 100% sulfur removal from the fuel. In order to validate the optimization by statistical methods, an experiment was held in operating conditions which were obtained by statistical methods. Applying optimal conditions resulted in sulfur removal of 100% which verifies the accuracy of optimization by theoretical methods.


## 4.2. Influential Parameters

The effect of the studied parameters on sulfur removal is plotted in Figure2. It is obvious that increasing each parameter can significantly enhance the sulfur removal efficiency. A theoretical discussion will be described in the following sections.(a) Sulfur removal as a function of O/S, acid/S = 2, and time = 150 min. (b) Sulfur removal as a function of acid/S, O/S = 3, and time = 100 min. (c) Sulfur removal as a function of time, O/S = 28, and acid/S = 2 (oxidation condition:T = 65°C; aqueous phase pH = 1.5. Extraction condition: T = 22°C; solvent-to-oil phase volume ratio = 1; number of extraction stages = 2).
(a)
(b)
(c)


### 4.2.1. Effect of O/S Molar Ratio

The effect of molar ratios of H2O2 to sulfur is exhibited in Figure 2(a). As indicated in Figure 2(a), sulfur removal initially increases, as the ratio of the oxidizing agent to sulfur-containing compound rises (i.e., the ratio of hydrogen peroxide to DBT). Then, after a specified level, the amount of oxidizing agent has no considerable effect on the sulfur removal anymore. Best results were obtained at the nO/nS = 18 at 65°C, and an increase in the O/S higher than 18 did not change the sulfur removal significantly. The initial molar H2O2/S concentration determines the initial hydrogen peroxide concentration in the reaction, which has an important impact on the formation of both hydroxyl radicals and performic acid. As mentioned before, according to the literature, these two species are the most effective agents of oxidation. So, it is obvious that by increasing the molar ratio of H2O2 to sulfur species, DBT conversion increases due to the formation of more hydroxyl radicals and performic acid. On the other hand, results have shown that high molar ratios of oxidizing agent to sulfur compound result in the decomposition of H2O2 into oxygen molecules, which eventually lead to loss of H2O2. Definitely this is not a desirable outcome. This means that greater amount of oxidizing agent beyond the proper level could have no affirmative impact on sulfur removal. The optimum value of O/S ratio is strongly dependent upon temperature because temperature can change the amount of decomposition rate significantly. At high temperature (50–70°C), the O/S molar ratio should be great enough (<10) to supply thermal decomposition of H2O2. However, for a temperature lower than 30–40°C, nO/nS can be closer to the stoichiometric ratio which is two [5, 6].Therefore, the initial H2O2/S molar ratio should be well controlled. It should be well noted that the stoichiometric ratio of H2O2 to DBT is two, whereas the excess amount of oxidant is usually required, which is more than the stoichiometric one. Several factors determine the necessity of extra amount of H2O2, including(1)
mass transfer problems between oil phase and aqueous phase;(2)
thermal decomposition of H2O2 to water and oxygen;(3)
parallel oxidation reactions of H2O2 [5].


### 4.2.2. Formic Acid/S Molar Ratio

Figure2(b) shows the effect of molar ratios of formic acid to sulfur on the reactions while temperature and pH values of the solution are maintained at constant values of 65°C and 1.5, respectively. As it was expected, DBT conversion was promoted dramatically by increasing nF/nS. The results have shown an enhancement in DBT conversion by increasing the ratio of formic acid to sulfur from 2 to 20, whereas with a further increase in the ratio of formic acid to sulfur, the conversion rate did not increase remarkably. Formic acid could effectively enhance the oxidation because it acts as a cocatalyst in oxidation system and not only decreases the pH value of the aqueous phase, but also generates performic acid when it interacts with hydrogen peroxide. In addition to the polarization ability of O–O bond, oxidative catalytic feature of formic acid has been reported as an oxidizing agent by giving its oxygen atom to DBT and enhancing its conversion to sulfones and sulfoxides species [4, 5]. In addition, the small size of the formic acid molecule can facilitate its interaction with sulfur without any steric hindrance of alkyl groups. But like other oxidizing agents, it has an optimum value and increasing its amount to the upper level does not have any effect since its concentration would not act as a controlling parameter in the oxidation system anymore. So beyond an optimum level, increasing formic acid concentration could not enhance the oxidative desulfurization noticeably.


### 4.2.3. Reaction Time

Figure2(c) shows sulfur removal as a function of reaction time. As it is indicated in this figure, the results were improved by increasing the time of the reaction initially and then slightly decrease. This could be explained by describing interaction of oxidizing agents as time proceeds. H2O2 and formic acid can interact with DBT to produce sulfones. This reaction like any other reaction needs enough time to complete and promotes as time goes on. Best results are observed at 125 min. After a particular reaction time, sulfur removal does not enhance by rising reaction time, which means there is an optimum time for oxidation system. Although it can be seen that after the optimum value as time proceeds sulfur removal value decreases, its decline is not sharp at all. This reduction in sulfur removal should be due to loss of hydrogen peroxide and performic acid and their decomposition which accelerates the conversion of oxidized sulfur compound to DBT. In other words, both the little amount of oxidizing agents and the long time of reaction result in the loss of all of the oxidizing agents, equilibrium change, and alteration of the reaction media from oxidizing to reducing one. But this trend never could be seen when the main oxidizing agent (i.e., hydrogen peroxide) exists in extra amount in solution. Because in such a condition there are excess amounts of hydroxyl and performic acid radicals over the whole reaction time, and the reaction medium remains as an oxidizing medium. So, carrying out the reaction in a long time especially whenever the oxidizing agent is in a little amount could have no benefit.


## 4.2.1. Effect of O/S Molar Ratio

The effect of molar ratios of H2O2 to sulfur is exhibited in Figure 2(a). As indicated in Figure 2(a), sulfur removal initially increases, as the ratio of the oxidizing agent to sulfur-containing compound rises (i.e., the ratio of hydrogen peroxide to DBT). Then, after a specified level, the amount of oxidizing agent has no considerable effect on the sulfur removal anymore. Best results were obtained at the nO/nS = 18 at 65°C, and an increase in the O/S higher than 18 did not change the sulfur removal significantly. The initial molar H2O2/S concentration determines the initial hydrogen peroxide concentration in the reaction, which has an important impact on the formation of both hydroxyl radicals and performic acid. As mentioned before, according to the literature, these two species are the most effective agents of oxidation. So, it is obvious that by increasing the molar ratio of H2O2 to sulfur species, DBT conversion increases due to the formation of more hydroxyl radicals and performic acid. On the other hand, results have shown that high molar ratios of oxidizing agent to sulfur compound result in the decomposition of H2O2 into oxygen molecules, which eventually lead to loss of H2O2. Definitely this is not a desirable outcome. This means that greater amount of oxidizing agent beyond the proper level could have no affirmative impact on sulfur removal. The optimum value of O/S ratio is strongly dependent upon temperature because temperature can change the amount of decomposition rate significantly. At high temperature (50–70°C), the O/S molar ratio should be great enough (<10) to supply thermal decomposition of H2O2. However, for a temperature lower than 30–40°C, nO/nS can be closer to the stoichiometric ratio which is two [5, 6].Therefore, the initial H2O2/S molar ratio should be well controlled. It should be well noted that the stoichiometric ratio of H2O2 to DBT is two, whereas the excess amount of oxidant is usually required, which is more than the stoichiometric one. Several factors determine the necessity of extra amount of H2O2, including(1)
mass transfer problems between oil phase and aqueous phase;(2)
thermal decomposition of H2O2 to water and oxygen;(3)
parallel oxidation reactions of H2O2 [5].


## 4.2.2. Formic Acid/S Molar Ratio

Figure2(b) shows the effect of molar ratios of formic acid to sulfur on the reactions while temperature and pH values of the solution are maintained at constant values of 65°C and 1.5, respectively. As it was expected, DBT conversion was promoted dramatically by increasing nF/nS. The results have shown an enhancement in DBT conversion by increasing the ratio of formic acid to sulfur from 2 to 20, whereas with a further increase in the ratio of formic acid to sulfur, the conversion rate did not increase remarkably. Formic acid could effectively enhance the oxidation because it acts as a cocatalyst in oxidation system and not only decreases the pH value of the aqueous phase, but also generates performic acid when it interacts with hydrogen peroxide. In addition to the polarization ability of O–O bond, oxidative catalytic feature of formic acid has been reported as an oxidizing agent by giving its oxygen atom to DBT and enhancing its conversion to sulfones and sulfoxides species [4, 5]. In addition, the small size of the formic acid molecule can facilitate its interaction with sulfur without any steric hindrance of alkyl groups. But like other oxidizing agents, it has an optimum value and increasing its amount to the upper level does not have any effect since its concentration would not act as a controlling parameter in the oxidation system anymore. So beyond an optimum level, increasing formic acid concentration could not enhance the oxidative desulfurization noticeably.


## 4.2.3. Reaction Time

Figure2(c) shows sulfur removal as a function of reaction time. As it is indicated in this figure, the results were improved by increasing the time of the reaction initially and then slightly decrease. This could be explained by describing interaction of oxidizing agents as time proceeds. H2O2 and formic acid can interact with DBT to produce sulfones. This reaction like any other reaction needs enough time to complete and promotes as time goes on. Best results are observed at 125 min. After a particular reaction time, sulfur removal does not enhance by rising reaction time, which means there is an optimum time for oxidation system. Although it can be seen that after the optimum value as time proceeds sulfur removal value decreases, its decline is not sharp at all. This reduction in sulfur removal should be due to loss of hydrogen peroxide and performic acid and their decomposition which accelerates the conversion of oxidized sulfur compound to DBT. In other words, both the little amount of oxidizing agents and the long time of reaction result in the loss of all of the oxidizing agents, equilibrium change, and alteration of the reaction media from oxidizing to reducing one. But this trend never could be seen when the main oxidizing agent (i.e., hydrogen peroxide) exists in extra amount in solution. Because in such a condition there are excess amounts of hydroxyl and performic acid radicals over the whole reaction time, and the reaction medium remains as an oxidizing medium. So, carrying out the reaction in a long time especially whenever the oxidizing agent is in a little amount could have no benefit.


## 4.3. Interaction between H2O2/S Ratio and Time

The contour plot of H2O2/S and time is exhibited in Figure 3(a), which is very helpful in the study of the interactive effects of the factors of the sulfur removal. Figure 3(b) also represents a 3D plot of sulfur removal as a function of those two parameters. In both figures, the third factor (the ratio of formic acid to sulfur) was kept at a constant level of two. The interaction between time and O/S molar ratio arises at different time levels. When a high level of time is applied (150 minutes), sulfur removal increases by increasing O/S ratio because H2O2 and DBT have enough time to react with each other and produce sulfones. On the other hand, when the oxidative system does not have enough time (50 minutes) to interact with sulfur compounds, raising the O/S ratio not only causes side reactions involving the thermal decomposition of hydrogen peroxide, but also increases the amount of water in the reaction medium. These results show the balance of two opposing factors (i.e., the excess of oxidant increases the activity, while the water produced from ODS reaction and thermal decomposition hinders the ODS reaction). In addition, it is suggested that in the presence of excess hydrogen peroxide, it acts as a hydroxyl radical scavenger that leads to the generation of less active perhydroxyl radicals [27]. This effect eventually inhibited the oxidation of organic pollutants in the aqueous phase. The best results are found in the region where the ration is limited to 13 < O/S < 24 at a moderate level of time.(a) 2D contour plot and (b) 3D response surface curve of the constructed model displaying sulfur removal at different O/S and time. Oxidation condition:T = 65°C; aqueous phase pH = 1.5; acid/S = 20. Extraction condition: T = 22°C; solvent-to-oil volume ratio = 1; number of extraction stages = 2.
(a)
(b)


## 5. Mechanism of Oxidation

An appropriate pathway is presented for better understanding the mechanism of oxidative sulfur removal by H2O2/acid system. As it is observed in Scheme 1, there are two competitive reactions for H2O2 that depend on the reaction temperature. The first reaction is the thermal decomposition of H2O2 that is an undesirable reaction because it increases the amount of water in the system and reduces the concentration of oxidant. Therefore, high temperature is not recommended for this reaction. In Reaction (2), hydroxyl radicals (HO∙) are produced which are strong oxidizing agents. In Reaction (3), DBT(s) are oxidized to their corresponding sulfoxide or sulfones [6].Scheme 1
ODS reaction of oxidative system and sulfur compound.In presence of acid (e.g., formic acid), H2O2 and acid interact and produce performic acid (CH2O3) (Reaction (4)). Then, performic acid gives its oxygen to dibenzothiophene and converts DBT into its sulfone (Reaction (5)).


## 6. Conclusion

This study focused on the oxidative reaction of DBT as a heavy sulfur compound with hydrogen peroxide in the liquid fuel. The model feed containing 250 ppmw sulfur was prepared by dissolving DBT inn-octane. A response surface methodology was used to study influential parameters in the removal efficiency of sulfur compounds. Among different types of effective parameters, that is, the fraction of sulfuric acid, temperature, type and fraction of the solvent were kept as sulfuric/S = 4 (mole), 65°C, volumetric ratio of acetonitrile/oil = 1, respectively. In addition, the impact of H2O2/S, formic acid/S ratio, and time of the reaction were studied by the experimental design to achieve the maximum removal of the sulfur. As a result, a reliable quadratic model was derived to describe the dependency of sulfur removal versus three parameters, quadratic form, and their interactions. Furthermore, the effect of each selected parameter and their interaction were investigated and described comprehensively. Also the operating condition, where best results could be taken, was obtained by statistical analyses (Box-Behnken method). According to the experiments and predicted results, the optimal operating conditions were determined at O/S = 15, formic acid/S = 22, and 56 min to achieve 100% sulfur removal from the fuel.



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*Source: 951045-2013-06-12.xml*