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Open AccessArticle

Mesoporous Adsorbents for Desulfurization of Model Diesel Fuel: Optimization, Kinetic, and Thermodynamic Studies

Catalysis and Chemical Reaction Engineering Laboratories, Department of Chemical and Biological Engineering, University of Saskatchewan, Saskatoon, SK S7N 5A9, Canada
Syncrude Edmonton Research Centre, Edmonton, AB T6N 1H4, Canada
Author to whom correspondence should be addressed.
Fuels 2020, 1(1), 47-58;
Received: 14 October 2020 / Revised: 10 November 2020 / Accepted: 13 November 2020 / Published: 14 November 2020


Mesoporous alumina-based adsorbents consisting of a π-electron acceptor complexing agent (2,7-dinitro-9-fluorenone) were synthesized and characterized. Adsorbents were screened for the removal of sulfur compounds from a model ultra-low-sulfur diesel fuel via a charge transfer complex (CTC) mechanism. The sulfur adsorption isotherms and kinetics were examined. The kinetics of sulfur adsorption followed a pseudo-second-order model with the CTC adsorbents. Among the three adsorbents screened, a commercial γ-Al2O3 CTC adsorbent showed the highest desulfurization in a short-run period. The regeneration of spent adsorbent was studied with three different polar solvents, namely chloroform, dichloromethane, and carbon tetrachloride. Dichloromethane was found to be the most suitable solvent for extracting a major portion of sulfur compounds occupied in the pores of the spent adsorbent. γ-Al2O3 CTC adsorbent can be reused after regeneration. Thermodynamic parameters such as Ea, ΔG, ΔH, and ΔS provided a better insight into the adsorption process.
Keywords: mesoporous adsorbent; desulfurization; charge transfer complex; adsorption; kinetics and thermodynamics mesoporous adsorbent; desulfurization; charge transfer complex; adsorption; kinetics and thermodynamics

1. Introduction

The world’s population has exponentially increased over the last few decades with a corresponding increase in demand for different resources, including fossil fuel. Over the last two decades, fossil fuel consumption has increased worldwide due to fast-growing economies. The burning of fossil fuel causes air pollution, which has been of great global concern, as it becomes a precursor for many health and environmental problems. Emissions of air pollutants, such as sulfur oxides, nitrogen oxides, carbon monoxide, particulate matter, and volatile organic compounds, come from various sources, notably among them is the combustion of fuels in internal combustion engines. To control these emissions, governments around the world have established certain limits on the allowable concentration of certain compounds in fuels that are being used for transportation. Particularly, sulfur compounds present in fossil fuels have a major impact on the environment when they are not under regulations. Oil refineries usually employ hydrotreatment to reduce the amounts of sulfur, nitrogen, oxygen, aromatics present in fuels. Since the removal of refractory sulfur compounds beyond certain thresholds through the conventional hydrotreating process is still challenging, several alternative methods have been studied to reduce levels of the recalcitrant species in fuels [1,2,3,4,5,6].
Among the alternative methods, adsorptive desulfurization (ADS) has the attention of many researchers around the world since it is a very promising and cost-effective route [7,8,9,10,11]. Unlike hydrotreating, ADS is a low-temperature process and does not require costly hydrogen gas [12]. The adsorptive desulfurization process can be physical or chemical. The physical adsorption pathway does not involve the formation of any new compounds, rather it results from van der Waals forces leading to mild attractions between molecules of sulfur compounds (adsorbate) and an adsorbent [13]. In the chemical adsorption route, the adsorbate-adsorbent interaction involves chemical reactions resulting from the sharing of electrons. The key factors influencing adsorptive desulfurization are the textural properties (large surface area, pore size, and pore volume) of the adsorbents and their affinity towards organic nitrogen compounds. Recently, we have reported 2,7-Dinitro-9-fluorenone (DNF) functionalized mesoporous Al2O3, Ti-substituted mesoporous Al2O3, and commercial γ-Al2O3 mesoporous alumina for desulfurization of liquid fuels [14]. For an adsorbent to be considered feasible for commercial and industrial applications, several investigations, including process parameters optimization, kinetic evaluations, as well as thermodynamics, need to be studied. The objective of this study is to investigate the optimum sulfur adsorption conditions of mesoporous charge-transfer complex (CTC) adsorbents and test their regeneration and reusability. Besides, the kinetic and thermodynamic behaviors were also investigated to elucidate their possible adsorptive desulfurization mechanisms.

2. Experimental

2.1. Materials and Chemicals

Poly (ethylene oxide)-block poly (propylene oxide)-block poly (ethylene oxide) (P123), carbon tetrachloride (CCl4) and dichloromethane were sourced from Sigma Aldrich (Oakville, ON, Canada). ACS grade nitric acid, methanol, toluene, and acetic acid were obtained from Fisher Chemical, Saskatoon, Canada. 2,7-Dinitro-9-fluorenone was sourced from the Tokyo chemical industry. Aluminum isopropoxide and ethylenediamine with purities of 98 and 99%, respectively, were supplied from Alfa Aesar, Canada. ACS grade titanium (IV) isopropoxide and hydrochloric acid (37% solution in water) were purchased from Acros Organics, Canada. Ethanol (anhydrous) was obtained from the Commercial Alcohols, Canada.

2.2. Preparation of Adsorbents

The synthesis method of the charge transfer adsorbents used in this study was described in detail in our previous publication [14]. In brief, the mesoporous Al2O3, titanium substituted mesoporous Al2O3 and commercial γ-Al2O3 were used as supports for the preparation of adsorbents A, B, and C, respectively. The syntheses of adsorbents involved (i) preparation of supports, (ii) anchoring of a linker, ethylenediamine on supports, and (iii) immobilization of a π-acceptor, 2,7-dinitro-9-fluorenone on supports.

2.2.1. Synthesis of Mesoporous Al2O3 and Titanium Substituted Mesoporous Al2O3 Supports

The mesoporous Al2O3 support was synthesized by a sol-gel technique. Solution A was prepared by dissolving aluminum isopropoxide and titanium isopropoxide in ethanol under mechanical agitation. Similarly, solution B was prepared by dissolving P123 in ethanol. A sol-gel solution was prepared by mixing solutions A and B. The resulting sol-gel solution was aged at 65 °C for 108 h before calcination at 600 °C for 5 h.

2.2.2. Functionalization of Supports with Ethylenediamine

Ethylenediamine (EDA) was used as a linker to anchor the π-acceptor on supports. EDA was immobilized on supports by mixing a methanol solution of EDA and the support. The resulting mixture was filtered, washed with methanol, and dried at 70 °C for 6 h in a vacuum oven.

2.2.3. Incorporation of π-Acceptor on Supports

DNF π-acceptor was dissolved in toluene and acetic acid solution by mechanical mixing. To this, ethylenediamine functionalized support was added and refluxed for three days. The π-acceptor loaded adsorbent was filtered and washed with toluene. Finally, the material was dried under vacuum prior to characterizations and adsorptive studies using a model ultra-low-sulfur diesel fuel.

2.3. Process Parameter Optimization

To investigate the influence of process parameters and their combined interactions on the adsorptive desulfurization process, a set of experiments was designed by varying process parameters, such as temperature and time, as well as the adsorbent loadings. The model feed concentration was kept constant. Experiments were designed by the Central Composite Design (CCD) approach using the Design Expert® software (version 6.0.11, State-Ease Inc., Minneapolis, MN, USA). Table 1 shows the ranges of variables for the experimental design. As given in Table 2, a set of 19 experiments (14 unique) was designed, with the center point experiment replicated five times. Experiments were repeated to check reproducibility under the same set of conditions. The model feed used in this study contained 541 ppm of sulfur, which was prepared by dissolving thiophene in ultra-low sulfur diesel (ULSD). Sulfur compounds mainly existing in diesel fuel are thiophene, benzothiophene (BT), dibenzothiophene (DBT). The CTC adsorbent used in this study removes organosulfur compounds through the π-complexation mechanism. The removal mechanism is the same for thiophene, benzothiophene, and dibenzothiophene and thus similar adsorption result is expected with all three organosulfur compounds. Besides, like thiophene, no internal diffusional barriers to benzothiophene and dibenzothiophene are expected since pores of CTC adsorbents are mesopores with diameters between 6 and 8 nm [14]. The typical adsorption experiment was carried out with 0.5 g of the adsorbent and 2.5 g of the model feed in a batch set up at required process conditions. The adsorbent was separated by filtration and the liquid product was analyzed with an Antek N/S analyzer for the total sulfur content.

2.4. Adsorption Kinetics

Kinetic studies were conducted in a stirred batch system consisting of a 15 mL glass vial in which a mixture of the adsorbent and the model feed was stirred at 400 rpm. The adsorbent to feed ratio was maintained at 1:5. To determine the minimum time required for the adsorbent to reach adsorption equilibrium, the experiments were carried out at different times ranging from 15 min to 72 h. To investigate the adsorption mechanism, the temperature was kept constant at 22 °C.
After the duration for adsorption was elapsed, the adsorbent was recovered under vacuum and the treated oil product was collected and stored in vials for total sulfur and nitrogen analysis. Following the N/S analysis, the adsorption efficiency was calculated using the formula shown below:
S   removal   efficiency   ( % ) =   S   in   the   feed   ( ppm ) S   in   the   product   liquid S   in   the   feed   ( ppm ) × 100
The equilibrium adsorption capacities were calculated using the following formula:
q e =   C 0 C e m V
where C0 and Ce are the initial and equilibrium concentrations of sulfur (mg·L−1), respectively, V is the volume of the feed used (L), and m is the mass of the adsorbent (g).

2.5. Adsorption Thermodynamics

Using the reaction rate constant of the pseudo-second-order model, the activation energies of ADS on three adsorbents were calculated following a method reported by Laidler [15]. Using the Arrhenius equation, the activation energy, E2, was calculated as shown below:
ln E 2 = E a RT + ln A
Moreover, using the data obtained from the adsorption experiments, the free activation energy (ΔG0) was determined by assuming that the adsorption process happened spontaneously. The changes in enthalpy (ΔH0) and entropy (ΔS0) were also calculated using the equations shown below:
Δ G 0 = RT ln K D
Δ G 0 = RT ln K D
ln K D = Δ S 0 R Δ H 0 RT
where ΔG0 (kJ·mol−1) was calculated using the Van’t Hoff equation, R is the universal gas constant, 8.314 J.mol−1, T is the absolute adsorption temperature in K, KD is the adsorption equilibrium constant. Using the slope and intercept of the plot (ln KD vs. 1/T), ΔH0 and ΔS0 were calculated.

2.6. Regeneration and Reusability Studies

The reusability study of the best adsorbent (adsorbent C) was carried out at the optimum process conditions (adsorbent loading = 30%, time = 27 min, temperature = 22 °C, and 400 rpm), which were identified from the screening study. After the 24 h adsorption reaction, the adsorbent was regenerated with three different solvents, namely chloroform, dichloromethane, and carbon tetrachloride, using a Soxhlet extraction set-up. Chlorinated solvents have been reported in the literature to eliminate and dissolve oil-based and organic substances [16,17,18]. The spent adsorbent was placed inside the soxhlet apparatus in a cellulose thimble and extracted with 150 mL of solvent. During the Soxhlet extraction, the solvent was placed in a 250 mL round-bottom flask connected to a reflux condenser in an immersed heated oil bath maintained at the boiling point of each solvent. The extraction was carried out for 8 h, and then adsorbent was dried and tested for reusability.

3. Result and Discussion

3.1. Adsorption Parameters Optimization

The CTC adsorbents used in this study were comprehensively characterized using BET, FTIR, XRD, TGA, and XPS techniques. The results of characterization were reported in our previous publication [14]. These adsorbents belong to the category of charge-transfer complex (CTC) adsorbent. As given in Figure 1, they adsorb organosulfur compounds selectively through the π-complexation mechanism, which involves interactions between the π orbitals of organic sulfur compounds and 2,7-Dinitro-9-fluorenone (DNF).
The effects of time, temperature, and adsorbent loadings on sulfur removal were determined by plotting a three-dimensional (3D) response surface and control graphs, as shown in Figure 2. Adsorbent A shows its highest adsorption activity with 76.3% of sulfur removal at an adsorbent loading of 20%, 41 °C and a reaction time of 43 min. However, at a temperature of 22 °C, an adsorbent loading of 30%, and a reaction time of 27 min, adsorbent A shows 74.0% sulfur removal. In terms of energy requirements, ADS at 41 °C might not be ideal as compared to 22 °C. Besides, raising the adsorption temperature by 20 °C increased the sulfur removal only by 2 wt.%. Adsorbent B showed a maximum sulfur removal of 57.2 wt.% at an adsorbent loading of 10% (0.25 g), a temperature of 60 °C and an adsorption time of 27 min. Similarly, adsorbent C reached its maximum adsorption capacity at an adsorbent loading of 30% (0.75 g), a temperature of 22 °C and an adsorption time of 27 min, resulting a sulfur removal of 83 wt.%. To fit the response function on sulfur removal, regression analysis was performed. The model equation for sulfur removal for adsorbents A, B, and C is shown in Table 3. The individual effect of each of the process parameters, such as temperature (X), time (Y) and adsorbent loading (Z), and combined effects of two of the process parameters on sulfur adsorption can be distinguished by using equations given in Table 3. For example, the interaction effects of X-Y, X-Z, and Y-Z are not as significant as the individual effect of X, Y, and Z on the sulfur adsorption capacity of the adsorbent A. The typical steps of adsorption on a CTC adsorbent involve (i) external diffusion, which involves the transfer of sulfur compounds to the external surface of adsorbent due to the occurrence of a concentration gradient, (ii) internal diffusion of sulfur compounds into pores of the CTC adsorbent, and (iii) adsorption of sulfur compounds through interacting with 2,7-Dinitro-9-fluorenone (π-acceptor) on the adsorbent. Although all are mesoporous materials, they differ in surface area, pore volume, and pore diameter [14]. Besides the number of active sites (π-acceptor) on these adsorbents is also expected to differ from each other. Because of these structural differences, along with the change in the number of active sites, the optimum process parameters of adsorption were changed among CTC adsorbents.

3.2. Kinetic Studies

To analyze the kinetic data of adsorption experiments, two conventional kinetic models, such as pseudo-first, and pseudo-second-order models, were investigated [4,19]. Figure 3 shows the adsorption kinetic curves for the pseudo-first-order model of adsorbents A, B, and C for adsorptive desulfurization. The pseudo-first-order model formula is shown below:
ln ( q e q t ) =   ln q e     k 1 * t
where qe and qt are amounts of sulfur compounds adsorbed at equilibrium (qe) and at different times (qt) calculated in (mg·g−1) and k1 is the pseudo-first-order model rate constant (min−1). The values of qe and k1 can be determined from the intercept and slope of the linear plot of ln (qe −qt) versus t. For the pseudo-first-order model, calculated values of qe and k1 are shown in Table 4, along with other kinetic parameters and correlation coefficients. The experimental data deviated considerably from the theoretical data. Moreover, the theoretical qe values found from the first-order kinetic model did not give reasonable values.
The kinetic parameters of the pseudo-second-order model are also presented in Table 4. From the table, it can be seen that the pseudo-second-order model given in Equation (8) adequately fits the adsorption experimental data for all three adsorbents.
t q t = 1 k 2 q e 2 + t q e
This observation was corroborated by the correlation coefficient R2 values obtained from this model. For adsorbents A and C, the R2 values were higher than its counterpart, however, the pseudo-first-order model did not show R2 higher than 0.5. However, with the pseudo-second-order model, both adsorbents A and C showed R2 values greater than 0.99, suggesting a better correlation of the experimental data to the kinetic model, as depicted in Figure 4.
The comparatively inferior performance of adsorbent B can also be observed from the kinetic studies. As reported in our earlier study [14], adsorbent B was inferior in textural properties that are critical to be a desirable adsorbent for adsorption [20,21,22]. Furthermore, this poor performance was also observed in consecutive parameter optimization experiments. Due to the inferior performance of adsorbent B, thermodynamic and regeneration studies were only carried out for adsorbents A and C.

3.3. Adsorption Thermodynamic

As part of this study, the activation energy (Ea) was calculated to get an insight into adsorption mechanisms. Using the Arrhenius equation, the activation energies were calculated for adsorbents A and C in the temperature range of 295–314 K. The activation energy values of 8.27 and 8.29 kJ·mol−1 were calculated by plotting ln k2 vs. 1/T for adsorbents A and C (Figure 5). It is known that lower activation energies (Ea) in the range of 5 to 40 kJ·mol−1 correspond to physical adsorption, while higher activation energies (40–800 kJ·mol−1) correspond to chemical adsorption [23]. The calculated activation energy values for adsorbents A and C shown in Table 5 suggest that sulfur compounds removal from the model fuel proceeded via the physical adsorption pathway. This means that the adsorption process is not associated with chemical reactions, instead, sulfur molecules are attracted to the adsorbent via the weak van der Waals forces or hydrogen bonding [4].
The free activation energy (ΔG0), enthalpy (ΔH0), and entropy (ΔS0) are usually involved in an adsorption process. To evaluate if the adsorption process of an adsorbate is spontaneous or not, the above-mentioned parameters have to be determined. As presented in Table 6, the free activation energy (ΔG0) values at 295 K were found to be 9.6 and 7.5 kJ·mol−1 for adsorbents A and C, respectively. At 318 K, these values were 10.1 and 7.9 kJ·mol−1. At 333 K these values were 10.6 and 8.4 kJ·mol−1. The positive values of ΔG0 mean that adsorption of sulfur compounds on adsorbents A and C is a slow process [24]. Using ln KD vs. 1/T values, (Figure not shown), enthalpy and entropy values were calculated using the intercept and slope.
As given in Table 5, the adsorption enthalpies (ΔH0) with adsorbents A and C were calculated to be 15.5 and 15.3 kJ·mol−1, respectively. The positive values of ΔH0 indicate that the adsorption process is endothermic [25]. The change of entropy (ΔS0) values in the adsorption system were −85.2 and −77.1 J·mol−1 K−1 for adsorbents A and C, respectively. The negative entropy values among adsorbents A and C indicate that the internal structure of these adsorbents hardly changes during the adsorption process [26].

4. Regeneration and Reusability

The spent adsorbent was regenerated by solvent washing with chloroform, dichloromethane, and carbon tetrachloride. These solvents were used since they are polar and suitable for the extraction of polar organosulfur compounds. Since these solvents have lower boiling points than sulfur compounds present in the petroleum feedstocks, they were completely removed from the extract solution by a rotary evaporator, and concentrated extracts were analyzed for their sulfur levels. The sulfur extraction efficiencies of chloroform, carbon tetrachloride, and dichloromethane with adsorbent C are shown in Figure 6. The highest sulfur removal was achieved using dichloromethane. It removed 80% of sulfur molecules that were adsorbed on the adsorbent C. The reusability of adsorbent C was studied three times. After each run, the spent adsorbent was regenerated by solvent washing with DCM. The residual solvent molecules on the adsorbent were removed by drying at 100 °C. The results are shown in Figure 7. The fresh adsorbent showed 83.8% sulfur removal. After the first regeneration, the sulfur removal efficiency dropped by only 7%. A significant drop was noted when the adsorbent C was reused for the third time. The nitrogen analysis of the solvent extract was carried out to determine the leaching of the immobilized EDA linker and π-acceptor during regeneration with DCM. The solvent extract of first and second regeneration contained 36 and 193 ppm of nitrogen, respectively, due to leaching of EDA and DNF. The leaching of DNF from the adsorbent C caused the drop in the number of available adsorption sites and thus its adsorption capacity after successive regenerations.

5. Conclusions

In this study, optimization, regeneration, and kinetic evaluations were carried out for three CTC adsorbents for adsorptive desulfurization of a model feed. The parameter optimization study showed optimum adsorption at ambient conditions. Adsorbent C had the highest sulfur removal capacity in a shorter period. The pseudo-second-order model had the best fit with the kinetic data of all three adsorbents. The activation energy (Ea) values indicated physical adsorption of sulfur compounds on adsorbents A and C. The values of free activation energy and enthalpy suggested that the adsorption of sulfur compounds on adsorbents A and C is a slow endothermic process. Entropy values evidenced that adsorbent A and C experienced no significant change in the internal structure during adsorption of sulfur compounds. The results of regeneration showed that dichloromethane is an effective solvent for regeneration, and the adsorbent C can be used at least two times.

Author Contributions

Conceptualization, A.B.-d.l.C. and S.V.; methodology, A.B.-d.l.C.; and S.V.; software, A.B.-d.l.C.; validation, P.E.B., S.V., J.A. and A.K.D.; formal analysis, A.B.-d.l.C.; investigation, A.B.-d.l.C.; resources, A.K.D.; data curation, A.B.-d.l.C.; writing—original draft preparation, A.B.-d.l.C. and S.V.; writing—review and editing, S.V., A.K.D. and P.E.B.; supervision, A.K.D. and J.A.; All authors have read and agreed to the published version of the manuscript.


This research received no external funding.


The authors thank the Natural Sciences and Engineering Research Council of Canada (NSERC), and the Canada Research Chair Program for funding the project.

Conflicts of Interest

The authors declare no conflict of interest.


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Figure 1. Mechanism of formation of electron-donor acceptor complex on CTC mesoporous adsorbent.
Figure 1. Mechanism of formation of electron-donor acceptor complex on CTC mesoporous adsorbent.
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Figure 2. The three-dimensional response surfaces: Effects of temperature and adsorbent loading on desulfurization activity of adsorbents (AC).
Figure 2. The three-dimensional response surfaces: Effects of temperature and adsorbent loading on desulfurization activity of adsorbents (AC).
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Figure 3. Pseudo first-order adsorption kinetics of adsorbents A, B, and C. Temperature = 22 °C, feed to adsorbent ratio = 5. The solid line is the kinetic model, the dash line is pseudo first-order-model simulation.
Figure 3. Pseudo first-order adsorption kinetics of adsorbents A, B, and C. Temperature = 22 °C, feed to adsorbent ratio = 5. The solid line is the kinetic model, the dash line is pseudo first-order-model simulation.
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Figure 4. Pseudo-second order adsorption kinetics of adsorbents A, B, and C at 22 °C using 1:5 adsorbent to feed ratio. The solid line is the results for the kinetic model, the dashed line is a pseudo-second order model simulation.
Figure 4. Pseudo-second order adsorption kinetics of adsorbents A, B, and C at 22 °C using 1:5 adsorbent to feed ratio. The solid line is the results for the kinetic model, the dashed line is a pseudo-second order model simulation.
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Figure 5. The activation energy (Ea) plot for adsorbents A and C.
Figure 5. The activation energy (Ea) plot for adsorbents A and C.
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Figure 6. Sulfur removal from the spent adsorbent C after 8 h of regeneration with chloroform, carbon tetrachloride, and dichloromethane.
Figure 6. Sulfur removal from the spent adsorbent C after 8 h of regeneration with chloroform, carbon tetrachloride, and dichloromethane.
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Figure 7. Reusability of adsorbent C after regeneration with dichloromethane.
Figure 7. Reusability of adsorbent C after regeneration with dichloromethane.
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Table 1. Optimization parameters and their corresponding range for the central composite design.
Table 1. Optimization parameters and their corresponding range for the central composite design.
Temperature (°C)A12260
Time (min)B11560
Adsorbent loading (g)C10.250.75
Table 2. Design of experiments for adsorption of sulfur.
Table 2. Design of experiments for adsorption of sulfur.
Run NumberAdsorbent Loading (g)Temperature (°C)Time (min)
Table 3. Linear equations for adsorbents A, B, and C from Composite Design Expert based on the proposed set of experiments.
Table 3. Linear equations for adsorbents A, B, and C from Composite Design Expert based on the proposed set of experiments.
AdsorbentLinear Equation
ATotal S removal = −5.37+0.17X + 111.04Y + 68.99Z − 0.60XY − 0.44XZ − 75.31YZ
BTotal S removal = 50.73 + 0.34X – 55.31Y – 19.13Z + 0.30XY – 0.17XZ + 48.46 YZ
CTotal S removal = 103.46 – 0.01X – 1.63Y – 104.90Z – 0.54XY + 0.27XZ + 116.77YZ
Note: Where X, Y, and Z are temperature (°C), time (h), and adsorbent loading (wt.%), respectively.
Table 4. Kinetic parameters for pseudo-first and pseudo-second-order model.
Table 4. Kinetic parameters for pseudo-first and pseudo-second-order model.
Adsorbentqe (exp) (mg·g−1)Pseudo-First Order ModelPseudo-Second Order Model
qe(cal) (mg·g−1)K1 (min−1)R2qe (cal) (mg·g−1)K2 (g·mg−1·min−1)R2
A2.79−0.001123.5 × 10−40.391.011.59 × 10−20.99
B2.08−0.000213.4 × 10− × 10−20.92
C2.78−0.00117−9.0 × 10−40.331.039.21 × 10−30.99
Table 5. Activation energy calculated values for adsorbents A and C.
Table 5. Activation energy calculated values for adsorbents A and C.
AdsorbentActivation Energy (Ea) (kJ/mol)ΔH (kJ/mol)ΔS (J/mol K)
Table 6. Free activation energy (ΔG) values for adsorbents A and C.
Table 6. Free activation energy (ΔG) values for adsorbents A and C.
Temperature (K)ΔG (kJ/mol)
Adsorbent AAdsorbent C
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