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Experimental and Modeling Study of Organic Chloride Compounds Removal from Naphtha Fraction of Contaminated Crude Oil Using Sintered # -Al2O3 Nanoparticles: Equilibrium, Kinetic and Thermodynamic Analysis Samad Arjang, Kazem Motahari, and Majid Saidi Energy Fuels, Just Accepted Manuscript • DOI: 10.1021/acs.energyfuels.7b03845 • Publication Date (Web): 19 Feb 2018 Downloaded from http://pubs.acs.org on February 25, 2018

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Experimental and Modeling Study of Organic Chloride Compounds Removal from Naphtha Fraction of Contaminated Crude Oil Using Sintered γ−Al2O3 Nanoparticles: Equilibrium, Kinetic and Thermodynamic Analysis Samad Arjang a, Kazem Motahari a*, Majid Saidi b† a

b

Department of Chemical Engineering, Arak University, Arak, 38156−8−8349, Iran

School of Chemistry, College of Science, University of Tehran, PO Box 14155−6455, Tehran, Iran

Abstract Because of destructive effects of organic chlorides, elimination of these compounds from contaminated crude oil and its distillates is very crucial for oil refiners. Despite the importance of the subject, limited researches in this field are performed and most of the proposed removal methods are operationally difficult and costly. In the present study, adsorption process as an efficient technology is proposed and employed to eliminate the organic chlorides compounds from naphtha fraction of contaminated crude oil. The γ−Al2O3 nanoparticles as an adsorbent is prepared and characterized by XRD, SEM−EDS, and BET analyses. Adsorption experiments are carried out at different operating temperatures and also various initial organic chloride concentrations. The experimental results indicated that the adsorption efficiency reaches to more than 96%, when the initial concentration of the organic chloride in the sample is 8.5 mg/L. The adsorption equilibrium analysis revealed that the Freundlich isotherm model provided the best fit and prediction of experimental data. It was * †

Corresponding Author: (Kazem Motahari) [email protected] Corresponding Author: (Majid Saidi) Email: [email protected] , [email protected]

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also found that for all of verified samples, the adsorption kinetic followed pseudo−second order equation well. According to experimental investigations reported in the present work, the sintered γ−Al2O3 nanoparticles would be an effective adsorbent for elimination of organic chloride as a hazardous material from the naphtha distillate of crude oil. Keywords: Organic chloride; Adsorption; Crude oil; Naphtha distillate; γ−Al2O3 nanoparticles.

1. Introduction Due to harmful effects of crude oil impurities on the refinery processes and facilities, elimination of these contaminants and control of their level in the crude oil samples is very important. Recently, according to environmental and technical regulations, the concentration of organic chlorides as one of the most important impurities should be monitored and the crude oil containing high amount of these compounds do not be allowed to enter as feed to refineries. Therefore, this type of impurity could make a considerable additional cost for oil producers and consumers. There are two types of chloride compounds in the crude oil including inorganic and organic chlorides

1, 2

. Both of these compounds could be harmful and cause many problems for

refining processes and facilities 1 such as corrosion of equipments including crude distillation unit (CDU) overhead 3, 4, heat exchangers and other downstream facilities 5, 6. Fouling in the processing vessels 7, catalyst poisoning and deactivation

8, 9

and equipment blockage

1

are

some other important problems caused by these compounds. The most important refinery units reported to be damaged by organic chlorides are distillation towers

1, 10

, naphtha

hydro−treating (NHT) units 11, catalytic reforming units 12 and catalytic cracking units 13. 2 ACS Paragon Plus Environment

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Inorganic chlorides are mainly separated using an electric desalting unit

2, 14

. But separation

of organic chlorides is very difficult because most of them have more solubility in the crude oil with respect to water and also they could not be easily extracted 2. This type of chloride compounds reacts and forms hydrogen chloride (HCl) under high temperature and pressure operating conditions during refining processes 1, 15-17. Dissolution of HCl in small amount of water in the distillation towers overhead leads to serious acidic corrosion in the downstream facilities

1, 2, 18

. In addition, in some other units like diesel and fuel hydrogenation, these

dangerous compounds hydrolyzed and form HCl

18

. In another situation, the chemical

reaction of this acid and nitrogen compounds leads to formation of NH4Cl via hydrogenation process 19. The presence of ammonium chloride causes the blockage of heat exchangers and serious under−deposit corrosion in some units like Fluid Catalytic Cracking Unit (FCCU) 13. Also the presence of organic chlorides contamination in the final refinery products like fuels will be harmful for the last user equipment (like engines) and also leads to environment pollution 18. It is well documented that even trace amounts of these compounds could disturb processes and facilities 1, 8, 10, 18. Therefore, as the first strategy these compounds must not be allowed to enter or form in the crude oil. It is obvious that elimination, controlling or mitigation of the main sources of these compounds at production and primary processing plants are much easier than separation or elimination of them from contaminated crude oil. It is necessary to mention that under some operating conditions and also during production, storage and transportation processes, crude oil could be contaminated with these harmful compounds. In this case, these compounds must be removed from the crude oil in order to reach the allowable concentration for refining processes which is below 1.0 mg/L in the naphtha fraction of the crude (Initial Boiling Point, IBP, to 477.59 K)

20, 21

. Some previous works were performed to eliminate the organic


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chlorides from the contaminated crude oil samples containing high amount of these compounds

18, 22-24

. But all of these proposed methods are very difficult and costly. Many of

them focused on breaking C−Cl bond and convert these compounds to harmless molecules. It is known that this bond is very strong and its average bond dissociation energy is about 83.0 kcal mole-1

25, 26

. Therefore, all of these methods need sever operating conditions

27

and also

catalytic processes are required for cleavage of this bond and convert them to other harmless compounds

28, 29

. A few other methods are based on the separation and removal of organic

chloride compounds from crude oil and its distillates, especially naphtha important methods of these proposed techniques are hydrogenation

29-32

. The most

29, 33

, nucleophilic

substitution 31 and adsorption 18, 32, 34, 35. In hydrogenation process, different forms of organic chlorides are converted to HCl over a specific hydrogenation catalyst 9. It is important to note that this removal method needs high temperature and pressure operating conditions and also this method has high operating cost because of its catalytic reactions 29. The most important problem of this method is the formation of hydrochloric acid which could make considerable corrosion in the reactor vessel and other facilities of this process. In the substitution method, the nucleophilic reagent such as sodium cyanide, sodium thiocyanate or sodium hydroxide reacts with organic chlorides to substitute chloride atom in the presence of phase transfer catalyst, like polyethylene glycol or dimethyl sulfoxide

31, 36-38

. This method also has some

drawbacks such as long reaction time and high temperature condition and operating cost. Considering the previous proposed methods represents that the mentioned converting methods could not be industrially applicable because of high operating and investment costs. Meanwhile, adsorption method 18, 35, 39, 40 does not need sever operating conditions and also it can be executed easily 41. Ma et al.

18

employed Na−LSX zeolite as an adsorbent of organic

chlorides from a model jet fuel. Although their results indicated that Na−LSX zeolite could


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act as an appropriate adsorbent for 5−chloro−2−methylaniline, but the main limitation of their work is high operating time of adsorption process (about 12 hours) 18. Also they performed their experiments only for a simple model sample not a real industrial one. In a few researches, it is reported that alumina could absorb some organohalide compounds 42

. Also it is well documented that when the adsorbent grain size decreases to nano order, the

adsorption capacity of the adsorbent increases significantly

43

. Alumina has perfectly

controlled mesoporosity associated with hardness, hydrolytic stability, amphoteric character, and thermal stability of the γ−transition−oxide phases

44, 45

. On the other hand, γ−phase of

alumina shows better characteristics and higher specific surface area for adsorption process 46

. Thus, in the present research, sintered γ−Al2O3 nanoparticles are employed for the first

time as the adsorbent of organic chloride compounds from naphtha distillate as a hydrocarbon media. Sintering temperature affects the final characteristics of sintered alumina. In this case the sintering temperature must be lower than 1023 K in order to prevent any phase transition of γ−Al2O3

47

and also must not be too high for maintaining the basic characteristics of

alumina nanoparticles

48

. Also, in the present study, the adsorption of different types of

organic chloride compounds from the industrial naphtha distillates of contaminated crude oil samples by sintered γ−Al2O3 is investigated. For this purpose, five crude oil samples containing different initial concentration of organic chlorides in the range of 8.5 to 105 mg/L are selected. The adsorption performance of prepared adsorbents for removal of these compounds from naphtha distillates at seven adsorption times in the range of 1 to 10 h and seven different constant temperatures including 298, 308, 318, 328, 338, 348 and 358 K are considered. 2. Experimental Methods 2.1. Materials 5 ACS Paragon Plus Environment

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All of the nanoparticles were used as received. Alumina nanoparticles (γ−Al2O3) basically produced by SSNano (Sky Spring Nano) Inc. were bought with the specified characterizations as: Average Particle Size (APS), 20 nm; Specific Surface Area (SSA), 230−400 m2/g and Purity, 99.9%. The basic characteristics of crude oil used in this research are summarized in Table 1. These industrial samples were contaminated with organic chloride compounds during production or primary processing. The initial concentration of the organic chlorine compounds in the crude oil samples varied from 8.5 to 105 mg/L. Table 1

2.2. Alumina Nanoparticles Sintering and Adsorbent Preparation To prepare the adsorbent for the main experiments, 10 g of γ−Al2O3 nanoparticles was placed in the porcelain and let it to be sintered at temperature of 773 K in an enclosed furnace for about 4 hours. Then, it is allowed to be cooled slowly to room temperature. Thirty five same adsorbents were prepared based on this procedure and each of them is used for a specified sample at a certain temperature. Also, in order to investigate the effect of adsorbent quantity on the adsorption process, different amount of adsorbents including 10, 15, 20, 25, 30 and 35 g of alumina nanoparticles were employed.

2.3. Apparatus In this study, a batch reactor was designed to verify the effect of time and temperature on the adsorption performance of sintered alumina nanoparticles. A schematic diagram of the set−up is shown in Figure S−1 (Supporting Information). This reactor contains a batch 1200 ml 6 ACS Paragon Plus Environment

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volumetric flask vessel, electrical heating jacket, temperature sensor (one platinum resistance thermometer (Pt 100) with a precision of ±0.1 K), pressure sensor, flanged sealing door and temperature controller. Due to safety consideration during the experiments, the entire set−up was placed on an electrically insulated platform.

2.4. Measurement Methods 2.4.1. Characterization of Adsorbent X−Ray−Diffraction (XRD) pattern for sintered γ−Al2O3 nanoparticles was obtained using Philips diffractometer model PW 1800. Scanning−Electron−Microscopy (SEM) Philips model XL30 was used for taking SEM micrograph and Energy Dispersive X−ray Spectroscopy (EDS) was employed to analyze the nano−adsorbent. The Brunauer–Emmett– Teller (BET) specific surface area, pore size, pore volume and micropore volume for the sintered alumina nanoparticles sample were determined by nitrogen adsorption using ASAP2010 instrument.

2.4.2. Measuring Method for Organic Chlorides Concentration 2.4.2.1. Measuring analyzers Organic chloride concentration of all samples measured using two different methods to ensure about the accuracy of final experimental results. The first method of measurement was based on coulometery while the second one was done with X−Ray fluorescence (XRF). Coulometery method was performed with Analytik Jena model multi EA 5000 analyzer while XRF method was done with CLORA 2XP model XOS instrument with a measurement range 7 ACS Paragon Plus Environment

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of 0−3000 mg/L. Both of these methods lead to the same results and confirmed each other. But the coulometery technique is more precise than XRF method for low concentration especially for concentrations below 1 mg/L. In both measurement methods, the final result of each sample was recorded based on arithmetic mean calculated from five different measurements.

2.4.2.2. Preparation of naphtha distillate samples In order to measure the concentration of organic chloride in the crude oil samples, naphtha distillate of these samples must be prepared according to the standard procedure. At the first step, the crude oil sample was distilled and its naphtha cut at temperature of 477 K was obtained based on ASTM D86 standard method

49

. Then, according to ASTM D4929

standard procedure, this distillate was washed three times with equal volume of caustic solution (1 M KOH) followed by equal volume of washing water for each time. The washing process with caustic solution removes hydrogen sulfide, while the washing with water removes traces of inorganic chlorides either originally present in the crude oil or from impurities in the caustic solution 50. Finally, the organic chloride concentration of the washed distillate was measured using two different analyzers based on the methods mentioned in the above section.

2.5. Experimental Procedure In this study, five crude oil samples with different initial organic chloride concentration were selected. These samples were taken from the outlet stream of same primary process plant at different times through two months (eight weeks). In fact, samples were taken at week 1, 3, 5, 8 ACS Paragon Plus Environment

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7 and 8, respectively. For each time, about 1000 liters processed crude oil was taken from the outlet stream of industrial plant to check the repeatability of experiments. The organic chloride concentrations of these five samples were measured using the mentioned methods and reported in Table 2. Based on reported data in this table, it seems that an unwanted source of organic chlorides entered the crude oil and then decreased gradually. Table 2 As presented in Table 2, for simplicity of the samples verification, they were named and ordered from the maximum organic chloride level to the minimum one. Therefore, samples with initial organic chloride concentration of 105, 82, 55, 27 and 8.5 mg/L were named sample no. 1, 2, 3, 4 and 5, respectively. Adsorption experiments were done at seven different constant temperatures of 298, 308, 318, 328, 338, 348 and 358 K and seven adsorption time intervals including 1, 2, 4, 6, 8, 9 and 10 h. For each sample and adsorption temperature, the adsorbent bed was made by sintering 10 g of alumina nanoparticles. In each experiment, 2200 ml of the sample was distilled based on ASTM D86 procedure and its naphtha distillate was obtained at 477 K. Then, the prepared adsorbent was placed in the reactor vessel and in the following, 280 ml of the obtained naphtha fraction was directly poured in the vessel. The vessel was completely sealed and temperature was adjusted on the determined adsorption temperature. After elapsing specified adsorption time interval, the electrical heating jacket was turned off and the vessel and its content let to be cooled to the room temperature. Organic chlorides concentration of treated sample was measured and reported based on the mentioned procedures. In order to recycle the adsorbent for repeating the experiments, it was heated to 478 K for 25 minutes to vaporize the remaining of naphtha distillate and adsorbed species. The recovery temperature was selected based on the final boiling point of naphtha distillate. To ensure the complete evaporation of the distillate compounds adsorbed on the 9 ACS Paragon Plus Environment

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sintered alumina nanoparticles, this temperature was adjusted one degree higher than boiling point of the obtained naphtha fraction which was 477 K.

3. Modeling The amount of adsorbed organic chlorides, qt (mg/g) at time t, was calculated by the following equation 51, 52:

=

− m

(1)

where C0 is the initial concentration of the organic chloride (mg/L), Ct is the concentration of the organic chloride at specified time t (mg/L), V is the volume of naphtha fraction (L), and m is the mass of adsorbent (g). Also, the adsorption capacity of sintered γ−Al2O3 nanoparticles at equilibrium condition, qe (mg/g), was calculated by the following mass balance equation 5356

:

=

− m

(2)

where Ce is the equilibrium concentration of the organic chloride compounds in the naphtha fraction (mg/L). The removal percentage (%) of organic chloride compounds from naphtha distillate by adsorption process can be calculated using the following equation 54, 57:

% =

− × 100%

3.1. Adsorption Equilibrium Modeling


(3)

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In order to investigate the adsorption equilibrium, the most famous isotherm models including Langmuir, Temkin, Freundlich and Dubinin–Radushkevich isotherms were selected to describe the relationship between the adsorbed amount of organic chloride compounds and its equilibrium concentration in the naphtha distillate.

3.1.1. Langmuir Isotherm Model Langmuir model was proposed by Hall et al. 58. The main characteristic of this model is the monolayer adsorption of the solute on a homogenous surface. In fact, in Langmuir model it is assumed that the adsorption process occurred at uniform adsorption energies and there is no transmigration on the adsorbent surface. This model was described by the following equation 59-61

:

=

! 1 + !

(4)

This equation could be rewritten as the following linear form 55, 62, 63:

1 =

1 1 1 . + !

(5)

where qe (mg/g) is the adsorptive capacity of sintered γ−Al2O3 nanoparticles at equilibrium condition, and k (L/mg) is the Langmuir adsorption equilibrium constant.

3.1.2. Temkin Isotherm Model In this model, the effect of indirect interaction of adsorbent−adsorbate on the adsorption isotherm process was considered

64-66

. This interaction involves the linear decrease of 11

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Page 12 of 68

adsorption heat with increasing the adsorption coverage. The following equation describes the linear form of Temkin isotherm model 67, 68:

%& %& = $ ( ) + $ ( ) ' '

(6)

where b and A are Temkin constants. This isotherm model was based on two important assumptions. Firstly, the heat of adsorption of all the molecules in the layer decreases linearly with coverage due to adsorbent–adsorbate interaction, and secondly, the adsorption is characterized by a uniform distribution of binding energies, up to some maximum binding energy 64, 69 .

3.1.3. Freundlich Isotherm Model Freundlich model is more realistic than Langmuir isotherm model. In this model, it is assumed that the adsorbent surface is heterogeneous and adsorption sites are different with each other. But all of these sites obey the Langmuir isotherm

51, 67

. In fact this model

describes the multilayer adsorption of adsorbate on the adsorbent surface 67. The describing equation for this model is as follows 70:

=

*

+

(7)

where kF and n are the capacity and the intensity of adsorption, respectively. This formula can be reformed to the following linear equation 71-73:

) = )

*

+ )

(8)

3.1.4. Dubinin−Radushkevich Isotherm Model 12 ACS Paragon Plus Environment

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Dubinin−Radushkevich isotherm model is generally applied to express the adsorption mechanism with a Gaussian energy distribution instead of heterogeneous surface

74, 75

. Also,

the present model described the adsorption process performance as a pore filling mechanism instead of an energetically non−uniform surface of the adsorbent

76

. The basic equation of

this isotherm model is as follows 74: 3

(9)

0%& )1 + 1⁄ 2 = exp / 6 −25 3

where R is the gas constant (8.314 J/mol K), T (K) is the absolute temperature and E is the adsorption energy (kJ/mol). The linear form of Dubinin−Radushkevich equation is as follow 77, 78

:

) = ) − 78 3

(10)

where,

8 = %& ) $1 + 7=

1 25 3

1 (

(11)

(12)

3.2. Kinetic Modeling To evaluate the efficiency and mechanism of the adsorption process, kinetic investigation is necessary 54, 79. In this study, the adsorption kinetic model was developed based on the most popular

models.

Pseudo−first

order

66,

80

,

pseudo−second


order

81,

82

and

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intra−particle−diffusion

83

Page 14 of 68

as the most widely used models were employed to investigate the

kinetic mechanism of organic chloride adsorption on sintered γ−Al2O3 nanoparticles.

3.2.1. Pseudo−First Order Model Lagergren presented the first order rate equation for the adsorption of oxalic acid and malonic acid into charcoal to explain the kinetics of adsorption process on solid surfaces. The pseudo−first order kinetic model is expressed as follows 80, 84, 85:

=

9

(13)

−

where k1 is the equilibrium rate constant of pseudo−first order kinetic (1/min). After integration and by applying the boundary conditions (qt=0 at t=0), Eq. (13) can be rewritten as 63, 86-88:

) − = ) −

9

(14)

3.2.2. Pseudo−Second Order Model The equation of pseudo−second order kinetic model is written as follow 70, 81, 89:

=

3

(15)

− 3

By integrating the above equation, the linear form of this equation is obtained as below 55, 62, 90, 91

:


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=

1 1 + 3 3

(16)

where k2 (g/ (mg .min)) is the pseudo−second order rate constant for the adsorption process.

3.2.3. Intra−Particle Diffusion Model 83

This model proposed by Weber and Morris

can explain the possibility of intra particle

diffusion in an adsorption process. The adsorbate transport from the solution phase to the surface of the adsorbent particles occurs in several steps. The overall adsorption process may be controlled either by one or more steps, e.g. film or external diffusion, pore diffusion, surface diffusion and adsorption on the pore surface, or a combination of more than one step 84

. The equation of this model is expressed as below 83, 84:

= :;+

9< 3

(17)

+=

where kint is the intra−particle diffusion rate constant (mg g−1min−0.5). According to this equation, after plotting qt versus t1/2, if the fitting line passes through the origin (i.e., Intercept I=0), it means that the controlling step of adsorption process would be intra−particle diffusion mechanism, unless otherwise, the intra−particle diffusion would not be the only rate−controlling step mechanism, indeed other factors may affect the rate of adsorption process and it is called hybrid control mechanism 92, 93.

3.3. Thermodynamic of Adsorption Process To investigate the possibility and the type of adsorption process, thermodynamic analysis should be performed. For this purpose, Gibbs free energy change, ∆G0, which is the most 15 ACS Paragon Plus Environment

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important thermodynamic parameter, was employed. The describing equation for Gibbs free energy is as follows 88, 94, 95:

∆? = −%& ):

(18)

where Ke (L/g) is obtained by the below equation 60, 94:

: =

(19)

The relationship between other thermodynamic parameters including enthalpy change (∆H0) and entropy change (∆S0) with Gibbs free energy change (∆G0) can be described as the following equation 72, 96, 97:

∆? = ∆@ − &∆A

(20)

and this equation can be rewritten as 60, 95, 98, 99:

): = −

∆@ ∆A + %& %

(21)

Based on Eq. 21, ∆S0 and ∆H0 can be obtained from the intercept and slope of linear fitting line of Ln Ke plot versus 1/T, respectively.

4. Results and Discussion 4.1. Characterization of Sintered Alumina Nanoparticles XRD pattern for sintered γ−Al2O3 nanoparticles is presented in Figure S−2 (Supporting Information). This pattern represents the high pure alumina existence in the final calcined

adsorbent without any phase change. The diffractograms for the sample display three distinct 16 ACS Paragon Plus Environment

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reflections at 38.3o (311 reflection), 45.7o (400) and 66.6o (440) which is in agreement with the database standard (JCPDS reference no.00−010−0425) and also with the reported results in the literatures for gamma alumina 100-103. SEM micrograph of this nano−adsorbent is shown in Figure S−3 (Supporting Information). Analysis of this image with Image J 1.51j8 software revealed that the adsorbent surface covered by fine nanoparticles with an average particle size less than 90 nm. According to the EDS analysis which is reported in Table S−1 (Supporting Information), the mass content of Al and O in this nano−adsorbent is 51.81% and 48.19% respectively. The BET analysis of surface area for this adsorbent indicated that the average specific surface area of this sample is 287.32 m2/g. Also its average pore size, pore volume and micropore volume were 1.23 nm, 0.42 cm3/g and 0.36 cm3/g, respectively.

4.2. Adsorbent Surface Characterization after Adsorption Process and after Regeneration It is well documented that there are different kinds of organic chlorides in the crude oil

10, 19

and some of these compounds enter this fluid during production, primary processing, storage and transportation 2. Wu et al. 1, 10 reported the existence of 17 kinds of organic chlorides in a specific crude oil in china including carbon tetrachloride, trichlorethylene, tetrachlorethylene, 1,2,3−trichloropropene, hexachloroethane, 1,1−dichloroethane,

1,1,2,2−tetrachloroethane,

methylene

chloride,

1,2−dichloropropane,

1,1,1,3−

tetrachloropropane,

2−chloropropane,

1,2−dichloroethane,

2,3−dichlorobutane,

1,2−dichlorobutane,

1,2,3−trichloropropane, 1,2−dichlorobenzene, and 1,2,4−trichlorobenzene. In this study, in order to ensure about the adsorption of organic chlorides on the prepared adsorbent, the EDS 17 ACS Paragon Plus Environment

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analysis of adsorbent was performed after the adsorption process. The analysis of sample no.1 (with average initial organic chloride concentration of 105 mg/L) was performed at 308 K and adsorption time of 10 h. The results reported in Table 3 confirmed the adsorption of such compounds on sintered alumina nanoparticles. Table 3 After the regeneration process, the EDS analyses of absorbents were performed. The EDS analyses of adsorbents surfaces after regeneration process indicated the complete elimination of organic chlorides via the evaporation process. In fact, no elements other than aluminum and oxygen were detected by this qualitative analysis after heating the adsorbents. The results of adsorbents analysis after regeneration process were the same with the analysis taken before adsorption process. These results also revealed that the adsorption process of organic chloride compounds on sintered γ−Al2O3 nanoparticles is a physisorption type, because the adsorbate−adsorbent bond cleaved at low temperature 104, 105.

4.3. Effect of Initial Adsorbate Concentration and Adsorption Time The organic chloride concentrations of final processed distillates after contacting with the adsorbent plotted as a function of adsorption time at constant adsorption temperatures in Figure 1. According to Figure 1, it is deduced that the sintered γ−Al2O3 nanoparticles could act as an appropriate adsorbent for the organic chloride compounds adsorption in the crude oil naphtha distillate. For each sample, the organic chlorides content of final processed naphtha fractions (after adsorption process) via the adsorption time showed the same behavior. According to this figure, the organic chloride content of samples continuously


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decreased with increasing the adsorption time to reach the equilibrium point where no considerable change observed in the organic chlorides content of naphtha distillates. Figure 1 It seemed that for the first and second samples, adsorption equilibrium obtained after 8 h, because according to the experimental results plotted in Figure 1 (a, b and c) no considerable change in the organic chlorides concentration of final processed samples observed after 480 min. The equilibrium time decreased to 360 min for sample no. 4 and it reached to 240 min for sample no. 5. In all of these experiments, the amount of adsorbent and subsequently, the number of vacant sites of adsorption kept constant. It can be concluded that for the samples with lower organic chlorides concentration, the required time to reach the equilibrium condition is shorter than the samples with higher concentration.

4.3. Effect of Adsorption Temperature Temperature is an important parameter for the adsorption process 106-109. The organic chloride concentration of each sample at a certain adsorption time was plotted as a function of process temperature as shown in Figure 2 (sample no.1 and 5) and Figure S−4 (samples no.2 to 4). Figure 2 According to EDS analyses presented in the previous section, we inferred that due to physisorption adsorption, the chemical bond between adsorbent surface and adsorbate is a Wan der Waals type 110, 111. Therefore the higher temperature leads to higher liquid mobility. It means that the activation of liquid molecules increases and subsequently, the contact of these molecules with adsorbent surface enhances. This phenomenon could improve the 19 ACS Paragon Plus Environment

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physical adsorption process. But, according to Figure 2, increase the distillate temperature more than a certain value has a negative effect on the adsorption process performance and some adsorbed organic chloride compounds desorbed from adsorbent. For naphtha distillates with lower initial organic chlorides content, this optimum condition occurred at higher temperatures, because for these samples, the chlorides molecules must be more energetic to reach the adsorbent surface and this is occurred at higher temperatures. The optimum temperature for the samples with initial concentration of 105, 82 and 55 mg/L was 318 K while this temperature rose to 328 K for the sample with initial concentration of 27 mg/L, and 338 K for the sample with initial organic chlorides concentration of 8.5 mg/L.

4.4. Adsorption Performance The amount of organic chlorides adsorption qt (mg/g) from naphtha distillate at different temperatures is presented in Figure 3 (sample no.1 and 5) and Figure S−5 (samples no.2 to 4). According to the obtained results, it is concluded that when the initial concentration of organic chlorides increased from 8.5 to 105 mg/L, the organic chloride adsorption per unit mass of sintered γ−Al2O3 nanoparticles enhanced. For example, qt increased from 0.22 to 1.51 mg/g as the initial organic chloride concentration increased from 8.5 to 105 mg/L at temperature of 298 K and adsorption time of 10 h. This manner is related to enhancement of mass transfer driving force due to higher concentration of organic chloride compounds in the naphtha distillate. In fact, with increasing the initial concentration of organic chloride in the naphtha fraction, the mass transfer driving force increased and therefore more organic chloride molecules transferred from the solution to the surface of the adsorbent. As shown in Figure 3 and Figure S−5, it can be seen that the highest qt value was obtained at the optimum temperature. Also, the maximum adsorption percentages of organic chloride compounds are 20 ACS Paragon Plus Environment

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shown in Figure 4. It can be observed that at the constant amount of adsorbent, the final removal percentage increased with decreasing the initial organic chloride concentration from 105 to 8.5 mg/L. Figure 3 Figure 4 Figure S−6 (Supporting Information) illustrates the percentage removal of organic chloride compounds at different adsorption times and temperatures. According to this figure, the rate of organic chloride compounds removal from naphtha distillate was high at the beginning of adsorption process which is related to the large number of available adsorption sites. By passing the time, the repulsive force between organic chloride molecules on the surface of adsorbent and in the liquid phase enhances, and this phenomenon leads to difficult adsorption of organic chloride molecules on the remaining vacant sites of adsorbent. Therefore, in the following of process, the adsorption rate slowed down gradually.

4.5. Effect of Adsorbent Quantity The amount of sintered alumina nanoparticles is a determinative parameter on the adsorbent capacity and adsorption equilibrium. In this section, the sample with initial concentration of 105 mg/L was selected to investigate the effect of adsorbent quantity on the adsorption process. Six different quantities of γ−Al2O3 nanoparticles including 10, 15, 20, 25, 30 and 35 g were used. As shown in Figure 5 at different temperatures, the removal percentage of organic chloride compounds improved with increasing the amount of adsorbent. For example, the removal percentage of organic chloride compounds increased from 51.3% to a considerable value of 91.5% with increasing the amount of adsorbent from 10 to 35 g at 21 ACS Paragon Plus Environment

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temperature of 298 K. Also, this increasing trend was observed for other adsorption temperatures. Especially, the maximum removal percentage was seen at optimum temperature of 318 K and the adsorbent amount of 35 g. Figure 5 Figure 6 shows the equilibrium adsorption capacity of the adsorbent, qe versus the amount of adsorbent at different temperatures. According to the plotted data in Figure 6, the equilibrium adsorption capacity of organic chloride per unit mass of sintered γ−Al2O3 nanoparticles decreased with increasing the amount of adsorbent. Indeed, the adsorption efficiency enhances with increasing the amount of adsorbent, due to increasing the effective absorbent surface area. Figure 6

4.6. Adsorption Isotherms Adsorption isotherms of organic chloride compounds on sintered γ−Al2O3 nanoparticles were determined for adsorption experimental data of five samples with initial organic chloride concentration of 8.5, 27, 55, 82 and 105 mg/L at different adsorption temperatures. The Langmuir, Temkin, Freundlich and Dubinin–Radushkevich (D–R) isotherm parameters for adsorption of organic chloride compounds on sintered γ−Al2O3 nanoparticles were obtained by linear fitting the experimental data. Figure 7 illustrates the fitting line for each of these models at different temperatures. Figure 7


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As presented in Figure 7, at adsorption temperature of 298 K, the correlation coefficient R2 was 0.9409, 0.9793, 0.8547 and 0.7386 for Langmuir model, Freundlich isotherm model, Temkin isotherm model and Dubinin−Radushkevich model, respectively. The model with R2 parameter closer to 1.0 has the better performance to fit the experimental data 112, therefore it can be concluded that Dubinin−Radushkevich isotherm model exhibited the weakest fitting for the experimental data with respect to other used isotherm models. Normalized standard deviation (SD) is another important parameter that could be obtained using the following equation 113, 114: (22)

3

AB =

,GHI. − ,JKL. M N ,GHI. C∑ E −1

where qe,exp is the adsorption capacity of organic chloride at equilibrium (mg/g) derived from the experimental results, qe,cal is the adsorption capacity calculated by the corresponding models and n is the number of data. For better comparison between the isotherm models, their basic parameters were calculated according to the fitted lines shown in Figure 7 and the results reported in Table 4. Based on the calculated parameters of adsorption isotherms in Table 4, it can be deduced that Freundlich isotherm seemed to be the best one to fit the experimental data due to its largest R2 and the smallest SD values than that of Langmuir and Temkin isotherm models. This result is also obviously confirmed by Figure 8 for temperatures of 298 and 358 K, where the calculated equilibrium adsorption capacities qe,calc, of each isotherm model were compared with respect to experimental values, qexp. It is necessary to mention that the plots for the other five temperatures including 308, 318, 328, 338 and 348 K were shown in Figure S−7 (Supporting Information). As shown in these figures, the nearest qe,calc. values to experimental ones were obtained with Freundlich 23 ACS Paragon Plus Environment

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isotherm model. Therefore, Freundlich adsorption isotherm model could be used to predict the adsorption of organic chloride compounds onto sintered γ−Al2O3 nanoparticles well. Table 4 Figure 8 4.7. Adsorption Kinetics The adsorption mechanism could be deeply understood using kinetic studies 79, 115. Eqs. (14), (16)

and

(17)

express

the

pseudo−first−order,

pseudo−second−order

and

intra−particle−diffusion kinetic models, respectively. Based on their linearized equations form, the experimental data were fitted and the final results were presented in Figures 9 for sample no. 1 with different initial organic chloride concentration of 105 mg/L. These graphs were plotted for the rest of the samples and shown in the Supporting Information file (Figures S−8 to S−11). Figure 9 When the pseudo−first−order kinetic model was employed to describe the experimental data, the values of qe, k1 and the correlation coefficient R2 were calculated from the linear plot of ln(qe− qt) versus t. Whereas, for fitting kinetic data using the linear form of the pseudo−second−order kinetic model, t/qt must be plotted versus t. According to the equation of this model, qe, k2 and correlation coefficient R2 could be calculated from the slope and intercept of the straight line obtained from the fitting line. In the case of intra−particle−diffusion model, qt plotted versus t1/2 and model parameters including Kint and I and also correlation coefficient R2 could be determined based on the fitted line to the experimental data. The mentioned kinetic models parameters and correlation coefficients R2 were calculated for different samples with different initial organic chloride concentration at 24 ACS Paragon Plus Environment

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various temperatures and the results were reported in Table 5. As reported in this table, the correlation coefficients R2, for intra−particle diffusion model and pseudo−second−order model are greater and closer to number 1.0 than that of pseudo−first−order kinetic model. For instance, for sample with initial organic chloride concentration of 55 mg/L, the correlation coefficients of intra−particle−diffusion model and pseudo−second−order model are 0.9772 and 0.9532 respectively, while this parameter is 0.8851 for pseudo−first−order kinetic model. Therefore, it can be resulted that for all of the samples, the intra−particle diffusion and pseudo−second−order kinetic models could better describe the kinetic of organic chloride adsorption on the sintered alumina nanoparticles. Based on the calculated results, for samples with lower initial concentrations, the pseudo−second−order model could better predict kinetic behavior of organic chloride compounds adsorption. Also, the reported parameters of intra−particle−diffusion kinetic model for the samples with different initial organic chloride concentrations showed that this diffusion model is not the only controlling step of organic chloride adsorption on sintered alumina nanoparticles. This is resulted from the fact that intra−particle−diffusion model intercept (I) is not zero for all of the samples data. Therefore, it can be said eventually that the kinetic of this adsorption process could not be described with only one kinetic model. Table 5

4.8. Adsorption Thermodynamics The thermodynamic parameters were calculated based on Eq. 21 using the slope and intercept of Ln Ke versus 1/T at different temperatures. More details about calculation procedure of thermodynamic parameters are presented in the Supporting Information. The final results were


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reported in Table 6. The negative ∆G0 values implied that adsorption process of organic chloride onto the sintered γ−Al2O3 nanoparticles was possible and spontaneous. Moreover, the values of Gibbs free energy for physisorption change between −20 and 0 kJ/mole, while chemical adsorption ∆G0 is between −400 and −80 kJ/mole

116, 117

. Therefore, it can be

concluded that the organic chloride compounds were adsorbed physically to the surface of sintered alumina nanoparticles that is in accordance with experimental results. The enthalpy change for physical adsorption was reported to be in the range of -20 to 40 kJ/mol 118. Hence, the values of -1.05 to -4.98 kJ/mol for ∆H0 showed that physisorption is the dominant mechanism for the adsorption process of organic chloride compounds on the sintered alumina nanoparticles. This important conclusion confirmed the previous results. Furthermore, the negative value of ∆H0 for this process revealed that it is an exothermic process that is in agreement with the decreasing adsorption capacity with increasing temperature. The positive values of ∆S0 implied that the molecular randomness of the solution increased during adsorption of organic chloride compounds that probably caused by the increased mobility of organic chloride on the surface of adsorbent compared with that of naphtha distillate. Table 6

5. Conclusions In this research, the removal of organic chlorides compounds from naphtha fraction of contaminated crude oil via adsorption process onto sintered γ−Al2O3 nanoparticles was investigated. Different crude oil samples with various initial concentrations of organic chlorides were taken from an industrial processing plant. The adsorption process performed at different adsorption time and temperatures. The EDS analyses before and after 26 ACS Paragon Plus Environment

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regeneration of nano−alumina adsorbent showed that the adsorption of organic chlorides is a physisorption type. Thermodynamic calculation of Gibbs free energy and enthalpy change also confirmed the physical adsorption of organic chloride compounds on the adsorbent. In order to investigate the effect of adsorbent dosage, different quantities of sintered alumina nanoparticles were employed. The results indicated that with increasing the amount of adsorbent, the removal percentage enhanced considerably while adsorption capacity, qe, decreased. Application of different adsorption isotherm models revealed that based on the correlation coefficients factor (R2) and standard deviation (SD), the Freundlich isotherm model could best describe the adsorption equilibrium of organic chloride compounds. Also, the kinetic mechanism of organic chloride adsorption process was investigated using the most applicable kinetic models including pseudo−first−order, pseudo−second−order and intra−particle−diffusion models. The correlation coefficients R2 of fitting these models to the experimental data indicated that intra−particle−model exhibited the best fitting for all of the verified samples. Finally, according to the experimental and theoretical interpretation results of this study, it can be concluded that sintered γ−Al2O3 nanoparticles could act as an effective adsorbent for adsorption removal of organic chloride compounds from naphtha fraction of crude oil.


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Energy & Fuels

List of Tables: Table 1. Main characteristics of the verified crude oil. Table 2. Organic chloride concentration of five different contaminated crude oil samples. Table 3. EDS analysis of adsorbent surface after adsorption process for sample no.1 after adsorption time of 10 h for sample no. 1. Table 4. Calculated Langmuir, Temkin and Freundlich isotherm models parameters. Table 5. Comparison of the pseudo−first−order, pseudo−second−order and intra particle diffusion kinetic models for the adsorption of organic chloride onto sintered γ−Al2O3 nanoparticles for various initial concentrations and temperatures. Table 6. Thermodynamic parameters for adsorption process of organic chloride compounds onto sintered γ−Al2O3 nanoparticles under different temperatures.


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Table 1 Characteristics

Units

Result

Test Method

Specific Gravity @ 15.56°C

−−−

0.8750

ASTM D5002

API Gravity

°API

31

ASTM D4294

Sulfur Content(Total)

wt.%

1.83

IP 170

H2S Content

ppm

1

UOP 163

Mercaptan Content

ppm

185

ASTM D5762

Nitrogen Content (Total)

wt.%

0.23

ASTM D4007

Water & Sediment

vol.%

Equilibrium, Kinetic, and Thermodynamic Analysis - Energy & Fuels

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