# Brilliant Green Dye Biosorption Using Activated Carbon Derived from Guava Tree Wood

Authors: R. A. Mansour; Abeer El Shahawy; A. Attia; Mokhtar S. Beheary
Journal: International Journal of Chemical Engineering
 (2020)

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## Abstract

The removal of brilliant green (BG) dye from an aqueous solution using activated carbon (AC) derived from guava tree wood is conducted in batch conditions. The influence of different factors such as contact time, pH, adsorbent dosage, initial dye concentration, and temperature on the adsorption of BG onto AC was investigated. FTIR, BET, and SEM analyses were performed to determine the characteristics of the material. The isotherm results were analyzed using the Langmuir, Freundlich, Temkin, and Dubinin–Radushkevich isotherms. Linear regression was used to fit the experimental data. It was found that the equilibrium data are best represented by the Freundlich isotherm, and the adsorption capacity (qe) was 90 mg dye/g AC. The values of the free energy (∆G), enthalpy (∆H), and entropy (∆S) were −86.188 kJ/mol, 43.025 kJ/mol, and 128 J/mol.K, respectively, at pH 7 for the BG dye. The kinetics of BG dye adsorption were analyzed using pseudo-first-order and pseudo-second-order models, and it was found that the pseudo-second-order model was suitable for the behavior of the BG dye at R2 = 0.999.


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## Body

## 1. Introduction

Dyes are widely used in several industrial applications such as in textiles, plastics, printing, rubber, cosmetics, paper and pulp, leather, and pharmaceutical [1–3]. The effluents of these industries are usually discharged into the water stream body which may cause harmful effects to the human and aquatic life beings due to their carcinogenic, toxic, and mutagenic effects [1].Brilliant green is a basic dye in various industrial and medical applications, e.g., biological stain, dermatological agent, veterinary medicine, an additive to poultry feed to prevent the spread of mold, intestinal parasites, and fungus [2], and also used in paper printing and textile dying. BG dye is dangerous in case of skin contact, eye contact, and swallowing. It is toxic to the lungs, through inhalation. During its degradation, it may form carbon dioxide, nitrogen oxide, and sulfur oxides. Therefore, there is an urgent need to separate this dye from the wastewater [3–8].Different treatment techniques (physical, chemical, and biological) have been used to separate colored compounds from wastewater. Biological degradation, photochemical degradation, flocculation, coagulation, reverse osmosis, chemical oxidation, floatation, and adsorption are widely used [9–11]. Adsorption on activated carbon (AC) is commonly used owing to its high efficiency and ability to remove many chemical compounds [12], simplicity of design [13], and economic feasibility. Nevertheless, the large-scale usage of AC is restrained when it is produced from expensive and nonrenewable precursors [14].Although activated carbon as an adsorbent for dye removal is commercially available, it is not cost effective and has some environmental concerns. It is commonly produced from very expensive materials such as lingocellulosic materials and coal, which are not renewable. This increases the preparation cost considerably. This has motivated researchers to find and test alternative sources with feasible methods for the preparation of AC compared to the currently available techniques. One of the viable and promising methods of producing AC is ant wastes or agricultural byproducts such as saw dust, wood, banana pith, fruit stones, and coconut husks. Because of their merits of low cost, availability, and ecofriendliness [15], anion-exchange resins such as IRA 402 and IRA-400 have been applied in the aqueous medium for both batch and column adsorption processes. Sinha et al. [16] have examined the sorption of the Congo Red (CR) azo dye from aqueous solutions using the Amberlite IRA-400 resin in batch and fixed bed reactors.As mentioned above, it is economical to prepare high-quality AC from abundant, cheap, renewable, and sustainable precursors such as biomass-based agroindustrial byproducts [17, 18]. Guava tree wood is an important source of activated carbon and is widely used in turnery and carpentry. In addition, this wood is excellent as a fuel and a valuable resource for charcoal.In this study, AC prepared from guava tree wood is used for the adsorption of the BG dye from an aqueous solution. The adsorption efficiency of AC can be identified by different factors such as pH, AC dose, contact time, temperature, and initial dye concentration. Textural characterization of the prepared AC was carried out by BET, FTIR, and SEM. Additionally, the kinetic, thermodynamic, and isotherm studies were carried out.


## 2. Experimental Work

### 2.1. Brilliant Green Dye and Solutions

BG was purchased from Merck Company (Germany) and was used without any further purification. It is an organic compound that is classified as a basic cationic dye. It has a molecular formula as C27H33N2O4S, and its molecular weight is 482.64 g/g.mol. One gram of the BG dye was dissolved in a liter of distilled water to get a dye concentration of 1000 mg/l. The concentration of the other solutions tested in the current study can be changed by the diluting method. The pH value was adjusted with sodium hydroxide or hydrochloric acid solutions (0.1 M).


### 2.2. Preparation of Adsorbent

AC was prepared from the guava tree wood, which was collected from Damietta city, Egypt. A given amount of crushed guava wood was heated at 700–900°C for one hour. After that, it was allowed for cooling to room temperature (25 ± 4°C). The powder was treated with 1 M HCl solution to eliminate the ash content and then washed with distilled deionized water. Further, the treated powder was dried at 105°C for 24 h. The final product was stored in closed glass containers. The prepared AC was screened by a 40 mesh sieve and was used as an adsorbent [19].


### 2.3. Batch Adsorption Studies

Batch technique was used in this study. A polluted water sample (50 ml) containing a known concentration of the BG dye (varied from 5 to 100 ppm) was transferred to a glass stoppered bottle (250 ml). The flasks were kept in a thermostatic water bath shaker at a constant speed of 240 rpm for 20 min. The batch experiments were carried out at 293 K to determine the retention kinetic of BG on activated carbon. 0.8 g of activated carbon dissolved in 50 ml dye solution (pH 7) was shaken for different times to attain equilibrium distribution, and the batch experiment was repeated twice, and the data were averaged for the dye. The retention capacity of the BG dye adsorbed by AC was determined from the difference between the initial and final dye concentration in the aqueous solution before and after retention. The concentration of the BG dye was analyzed using a spectrophotometer (UV/Vis spectrophotometer) atλmax (625 nm). The amount of dye retained per unit mass of the adsorbent and the percent removal (% R) of the dye were calculated by(1)%R=Ci−CfCi∗100,qe=Ci−Ce∗vm,where qe is the adsorption capacity (mg/g), Ci is the initial concentration of the dye in (mg/l), Ce is the concentration of the BG dye (mg/l) at equilibrium, Ci and Cf are the initial and final concentrations of the BG dye (mg/l) respectively, v is the volume of the solution (l), and m is the amount of the adsorbent (g).


### 2.4. Equilibrium Studies and Adsorption Isotherm

The most commonly used representation of the adsorbate concentration and quantity of the pollutant adsorbed is the adsorption isotherm. The equilibrium adsorption isotherm is fundamental in describing the interactive behavior between the solute and the adsorbent and is important for the design of an adsorption system equilibrium of BG dye adsorption. It was modeled by the following important isotherms.


#### 2.4.1. Langmuir Isotherm

The Langmuir adsorption model describes monolayer adsorption of the adsorbate onto a homogeneous adsorbent surface [20]. This model also determines the maximum capacity of the adsorbent [21]:(2)Ceqe=1qmCe+1qmkL,where qe is the amount of the dye at equilibrium (mg/g), qm is the maximum adsorption capacity (mg/g), and kL is the Langmuir constant (L/mg).


#### 2.4.2. Freundlich Isotherm

The Freundlich isotherm model is often used for heterogeneous surface energy systems and is represented by the following equation:(3)lnqe=1nlnCe+lnkf,where Ce is the equilibrium concentration in the liquid phase (mg/l), qe is the adsorption capacity (mg/g), kf is the Freundlich constant representing adsorption capacity, and “n” is the empirical parameter representing the energetic heterogeneity of the adsorption sites.


#### 2.4.3. Temkin Isotherm

The nonlinear form of the Temkin equation is given by(4)qe=qmlnKtCe.This equation can be linearized as given by(5)qe=qmlnKt+qmlnCe,where qm is a constant related to the heat of adsorption (J/mole) and kt is the equilibrium binding constant (l/g) corresponding to the maximum binding energy. The isotherm constants kt and qm are determined by the slope and intercept from a plot of qe versus ln(Ce).


#### 2.4.4. Dubinin–Radushkevich Isotherm

Dubinin isotherm can be expressed in the linear form as follows:(6)lnqe=lnqm−Dε2,ε=RTln1+1Ce,where D is a constant related to the transfer energy, R is the gas constant (kJmol−1K−1), qm is the Dubinin constant (mgg−1), and T is the absolute temperature in (K) [22, 23].


### 2.5. Kinetic Studies

The adsorption of the BG dye was characterized by two kinetic models as follows:


#### 2.5.1. Pesudo-First Order

The pseudo-first-order kinetic model can be written as follows:(7)logqe−qt=logqe−K1t2.303,where qe and qt are the amount of dye sorbed per mass of the sorbent at equilibrium (mg g−1) and at any time (t), respectively, and k1 is the rate constant (min−1).


#### 2.5.2. Pseudo-Second Order

This model is represented by(8)tqt=1k2qe2+1qet,where k2 is the rate constant and qt is the dye uptake capacity at any time t.


### 2.6. Thermodynamic Study

Thermodynamic parameters for the adsorption of BG on the adsorbent are evaluated by the equilibrium experimental data observed at different temperatures from 298.15 to 358.18 K. There is a set of thermodynamic parameters that can be used to describe the adsorption process which are the change of enthalpy (ΔH, kJ mol−1), Gibbs energy (ΔG, kJ mol−1), and entropy (ΔS, kJ mol−1K−1) [24]. These parameters were calculated using the Van’t Hoff equations [25, 26]. This is given as follows:(9)ΔG=−RTlnK,(10)K=qece,(11)ΔG=ΔH−TΔS,where K is the equilibrium constant (g−1), T is the temperature (K), R is the universal gas constant (8.314 J/mol.K), and qe is the adsorption capacity (mg g−1). By plotting the graph between 1/T and ln(k), the values of ΔH and ΔS of the adsorption process were estimated from the slope and the intercept.


## 2.1. Brilliant Green Dye and Solutions

BG was purchased from Merck Company (Germany) and was used without any further purification. It is an organic compound that is classified as a basic cationic dye. It has a molecular formula as C27H33N2O4S, and its molecular weight is 482.64 g/g.mol. One gram of the BG dye was dissolved in a liter of distilled water to get a dye concentration of 1000 mg/l. The concentration of the other solutions tested in the current study can be changed by the diluting method. The pH value was adjusted with sodium hydroxide or hydrochloric acid solutions (0.1 M).


## 2.2. Preparation of Adsorbent

AC was prepared from the guava tree wood, which was collected from Damietta city, Egypt. A given amount of crushed guava wood was heated at 700–900°C for one hour. After that, it was allowed for cooling to room temperature (25 ± 4°C). The powder was treated with 1 M HCl solution to eliminate the ash content and then washed with distilled deionized water. Further, the treated powder was dried at 105°C for 24 h. The final product was stored in closed glass containers. The prepared AC was screened by a 40 mesh sieve and was used as an adsorbent [19].


## 2.3. Batch Adsorption Studies

Batch technique was used in this study. A polluted water sample (50 ml) containing a known concentration of the BG dye (varied from 5 to 100 ppm) was transferred to a glass stoppered bottle (250 ml). The flasks were kept in a thermostatic water bath shaker at a constant speed of 240 rpm for 20 min. The batch experiments were carried out at 293 K to determine the retention kinetic of BG on activated carbon. 0.8 g of activated carbon dissolved in 50 ml dye solution (pH 7) was shaken for different times to attain equilibrium distribution, and the batch experiment was repeated twice, and the data were averaged for the dye. The retention capacity of the BG dye adsorbed by AC was determined from the difference between the initial and final dye concentration in the aqueous solution before and after retention. The concentration of the BG dye was analyzed using a spectrophotometer (UV/Vis spectrophotometer) atλmax (625 nm). The amount of dye retained per unit mass of the adsorbent and the percent removal (% R) of the dye were calculated by(1)%R=Ci−CfCi∗100,qe=Ci−Ce∗vm,where qe is the adsorption capacity (mg/g), Ci is the initial concentration of the dye in (mg/l), Ce is the concentration of the BG dye (mg/l) at equilibrium, Ci and Cf are the initial and final concentrations of the BG dye (mg/l) respectively, v is the volume of the solution (l), and m is the amount of the adsorbent (g).


## 2.4. Equilibrium Studies and Adsorption Isotherm

The most commonly used representation of the adsorbate concentration and quantity of the pollutant adsorbed is the adsorption isotherm. The equilibrium adsorption isotherm is fundamental in describing the interactive behavior between the solute and the adsorbent and is important for the design of an adsorption system equilibrium of BG dye adsorption. It was modeled by the following important isotherms.


### 2.4.1. Langmuir Isotherm

The Langmuir adsorption model describes monolayer adsorption of the adsorbate onto a homogeneous adsorbent surface [20]. This model also determines the maximum capacity of the adsorbent [21]:(2)Ceqe=1qmCe+1qmkL,where qe is the amount of the dye at equilibrium (mg/g), qm is the maximum adsorption capacity (mg/g), and kL is the Langmuir constant (L/mg).


### 2.4.2. Freundlich Isotherm

The Freundlich isotherm model is often used for heterogeneous surface energy systems and is represented by the following equation:(3)lnqe=1nlnCe+lnkf,where Ce is the equilibrium concentration in the liquid phase (mg/l), qe is the adsorption capacity (mg/g), kf is the Freundlich constant representing adsorption capacity, and “n” is the empirical parameter representing the energetic heterogeneity of the adsorption sites.


### 2.4.3. Temkin Isotherm

The nonlinear form of the Temkin equation is given by(4)qe=qmlnKtCe.This equation can be linearized as given by(5)qe=qmlnKt+qmlnCe,where qm is a constant related to the heat of adsorption (J/mole) and kt is the equilibrium binding constant (l/g) corresponding to the maximum binding energy. The isotherm constants kt and qm are determined by the slope and intercept from a plot of qe versus ln(Ce).


### 2.4.4. Dubinin–Radushkevich Isotherm

Dubinin isotherm can be expressed in the linear form as follows:(6)lnqe=lnqm−Dε2,ε=RTln1+1Ce,where D is a constant related to the transfer energy, R is the gas constant (kJmol−1K−1), qm is the Dubinin constant (mgg−1), and T is the absolute temperature in (K) [22, 23].


## 2.4.1. Langmuir Isotherm

The Langmuir adsorption model describes monolayer adsorption of the adsorbate onto a homogeneous adsorbent surface [20]. This model also determines the maximum capacity of the adsorbent [21]:(2)Ceqe=1qmCe+1qmkL,where qe is the amount of the dye at equilibrium (mg/g), qm is the maximum adsorption capacity (mg/g), and kL is the Langmuir constant (L/mg).


## 2.4.2. Freundlich Isotherm

The Freundlich isotherm model is often used for heterogeneous surface energy systems and is represented by the following equation:(3)lnqe=1nlnCe+lnkf,where Ce is the equilibrium concentration in the liquid phase (mg/l), qe is the adsorption capacity (mg/g), kf is the Freundlich constant representing adsorption capacity, and “n” is the empirical parameter representing the energetic heterogeneity of the adsorption sites.


## 2.4.3. Temkin Isotherm

The nonlinear form of the Temkin equation is given by(4)qe=qmlnKtCe.This equation can be linearized as given by(5)qe=qmlnKt+qmlnCe,where qm is a constant related to the heat of adsorption (J/mole) and kt is the equilibrium binding constant (l/g) corresponding to the maximum binding energy. The isotherm constants kt and qm are determined by the slope and intercept from a plot of qe versus ln(Ce).


## 2.4.4. Dubinin–Radushkevich Isotherm

Dubinin isotherm can be expressed in the linear form as follows:(6)lnqe=lnqm−Dε2,ε=RTln1+1Ce,where D is a constant related to the transfer energy, R is the gas constant (kJmol−1K−1), qm is the Dubinin constant (mgg−1), and T is the absolute temperature in (K) [22, 23].


## 2.5. Kinetic Studies

The adsorption of the BG dye was characterized by two kinetic models as follows:


### 2.5.1. Pesudo-First Order

The pseudo-first-order kinetic model can be written as follows:(7)logqe−qt=logqe−K1t2.303,where qe and qt are the amount of dye sorbed per mass of the sorbent at equilibrium (mg g−1) and at any time (t), respectively, and k1 is the rate constant (min−1).


### 2.5.2. Pseudo-Second Order

This model is represented by(8)tqt=1k2qe2+1qet,where k2 is the rate constant and qt is the dye uptake capacity at any time t.


## 2.5.1. Pesudo-First Order

The pseudo-first-order kinetic model can be written as follows:(7)logqe−qt=logqe−K1t2.303,where qe and qt are the amount of dye sorbed per mass of the sorbent at equilibrium (mg g−1) and at any time (t), respectively, and k1 is the rate constant (min−1).


## 2.5.2. Pseudo-Second Order

This model is represented by(8)tqt=1k2qe2+1qet,where k2 is the rate constant and qt is the dye uptake capacity at any time t.


## 2.6. Thermodynamic Study

Thermodynamic parameters for the adsorption of BG on the adsorbent are evaluated by the equilibrium experimental data observed at different temperatures from 298.15 to 358.18 K. There is a set of thermodynamic parameters that can be used to describe the adsorption process which are the change of enthalpy (ΔH, kJ mol−1), Gibbs energy (ΔG, kJ mol−1), and entropy (ΔS, kJ mol−1K−1) [24]. These parameters were calculated using the Van’t Hoff equations [25, 26]. This is given as follows:(9)ΔG=−RTlnK,(10)K=qece,(11)ΔG=ΔH−TΔS,where K is the equilibrium constant (g−1), T is the temperature (K), R is the universal gas constant (8.314 J/mol.K), and qe is the adsorption capacity (mg g−1). By plotting the graph between 1/T and ln(k), the values of ΔH and ΔS of the adsorption process were estimated from the slope and the intercept.


## 3. Results and Discussion

### 3.1. Characterization of AC

In order to obtain information about the mode of interaction of the brilliant green dye with activated carbon, different physicochemical measurements were done, which are presented below.


#### 3.1.1. Scanning Electron Microscopy (SEM)

Figures1(a) and 1(b) show the SEM image of AC and adsorbed BG onto AC, respectively. The SEM image of the AC sample before dye adsorption (Figure 1(a)) obviously shows the surface morphology with an irregular texture and high surface roughness and different levels of porosity in AC, which provides possible sites for adsorption of the dye. The surface roughness and the macropores which are important factors for the dye adsorption were responsible for the high surface area, making AC a good adsorbent. After adsorption with the dye, a large area of AC was covered with dye molecules in the form of flakes, and thus the SEM image of AC after adsorption showed a smooth surface because the BG molecules were trapped and sorbed on the surface of AC.Figure 1
SEM images of the AC adsorbent. (a) AC only and (b) AC + BG dye.


#### 3.1.2. Fourier-Transform Infrared (FTIR) Spectra

A substantial part of the knowledge concerning the mode of the bonding in the dye compound can be gained by applying infrared spectra. In such a case, the spectrum of AC is usually compared with that of the AC-dye species to get an idea about the function groups which react with the dye. The IR spectra of the sorbed species and AC are depicted in Figure2.Figure 2
FTIR for (a) activated carbon and (b) activated carbon with brilliant green dye.
(a)(b)Figure2 represents the FTIR spectrum of the adsorbent (AC) before and after adsorption. The FTIR spectrum of AC showed different bands at 3440, 2918, 1598, 1452, and 782 cm−1assigned to O-H, -CH aliphatic, -C=C, -CH2 bending, and -C=S. The FTIR spectrum of AC-BG compared with that of AC showed that there are bands at 3442, 2920, 1583, 1440, and 811 cm−1 assigned to O-H, -CH aliphatic, -C=C, -CH2 bending, and -C=S. The FTIR spectrum of the AC-BG showed shifts in bands to higher and/or to lower with appearance or disappearance of other bands, which indicate the complete adsorption of the BG dye.


#### 3.1.3. BET

The specific surface area of the prepared AC was obtained by the nitrogen adsorption/desorption isotherm at 77 K using the high-speed gas sorption analyzer (NOVA 1000, Version 6.11, Quanta Chrome Corporation) employing the Brunauer–Emmett–Teller (BET) method (activation temperature of 900°C and activation time 0.5 hr.). The specific surface area was found to be equal to 310 m2/g. This area can provide many active sites that increase the chances of adsorption.


### 3.2. Affecting Parameters on Adsorption

#### 3.2.1. Effect of pH

The pH value is an important parameter in controlling the adsorption process due to the ionization of surface functional groups in the solution [27]. To study the influence of pH on the adsorption of the BG dye onto AC, experiments were performed using various initial pH values varying from 2 to 12. The results indicate that the percentage removal of the BG dye increases with the increase in pH up to a pH value of 7 (Figure 3), after which the removal of BG dye decreases with the increase in pH. At lower pH values, the BG removal was reduced, probably as a result of the competition between hydrogen ions and the dye cations for the sorption sites of AC [28]. The surface of the AC may get negatively charged at higher pH, which increases the chances of attraction force with the cationic dye through electrostatic force of attraction [29]. Generally, the net positive charge decreases with increasing pH value leading to the decrease in the repulsion force between the adsorbent surface and the dye, thus improving the adsorption capacity.Figure 3
Effect of pH on the adsorption of the BG dye using AC.


#### 3.2.2. Effect of Adsorbent Dose

Figure4 shows the influence of AC mass on the removal of BG dye from aqueous solutions. With an increase in the amount of the adsorbent material, the uptake of the dye increases. The adsorption of the BG dye increases significantly (from 83% to 99%) when the adsorbent dose increases from 0.1 g to 0.8 g, but the removal efficiency of the dye does not change significantly when the adsorbent dose is increased above 0.8 g. So, 0.8 g of the adsorbent (AC) can be considered the optimal dose for the adsorption of the BG dye. For the brilliant green dye, it is clear that the percentage removal increased gradually as the adsorbent mass increased. This effect can be attributed to the increase in the surface area and the active sites of the adsorbent [30].Figure 4
Effect of adsorbent dosage on the adsorption of the BG dye using AC.


#### 3.2.3. Effect of Initial Dye Concentration

The influence of initial dye concentration (Ci) was studied in the range (5–100 mg/l) at temperature 25°C, 240 rpm, and 20 min contact time, and the results are shown in Figure 5. From Figure 5, the removal efficiency of the activated carbon decreased with increasing initial dye concentration. There will be unoccupied active sites on the AC surface at low dye concentration, and the active sites required for adsorption of the BG molecules will be lacking when the initial dye concentration increases [31].Figure 5
Effect of initial dye concentration on the adsorption onto AC.


### 3.3. Adsorption Isotherm

The adsorption isotherms were determined by shaking 0.8 g of the AC with 50 ml of 5 to 100 mg/l of BG solutions for 20 min. The adsorption isotherms are used to relate the adsorbed amount at the interface and the adsorbent concentration in the bulk solution [32] and is important for the design of an adsorption system. The correlation coefficient values (R2) were used as a criterion to infer the most appropriate isotherm equation that can be selected to describe the adsorption process.


#### 3.3.1. Langmuir Isotherm

The linear form can be used for the linearization of experimental data by plottingCe/qe against Ce (Figure 6). The Langmuir constant qm (mg/g) which is a measure of the maximum adsorption capacity of AC is obtained as 90 mg/g. Km is the Langmuir constant which relating to adsorption energy is found to be 0.14 mg−1 for the brilliant green dye. The feasibility of the process can be evaluated by a separation factor (dimensionless constant) “RL” which is given in the following equation:(12)RL=11+KLCi,where “Ci” is the initial dye concentration (mg/L) and the “RL” value is between zero and one for favorable adsorption, whereas (RL > 1), (RL = 1), and (RL = zero) for unfavorable, linear, and irreversible adsorption, respectively [7].Figure 6
Langmuir model for brilliant green dye onto AC.


#### 3.3.2. Freundlich Isotherm

By plotting the graph between ln(qe) and ln(ce) (Figure 7), the Freundlich constants (KF and n) can be obtained from the slope and the intercept of the linear plot of the experimental data. The values of Kf and n are 0.427 and 1.326, respectively. The value of n indicates the degree of nonlinearity between solution concentration and adsorption; if n = 1, then adsorption is linear; if n < 1, then adsorption is a chemical process; if n > 1, then adsorption is a physical process [33]. The n value was found to be 1.326 for AC. Since n > 1, the adsorption of the BG dye onto AC is a physical process. It is found that the correlation coefficient value (R2) obtained from the Freundlich isotherm model for AC is 0.975 for the dye.Figure 7
Freundlich model for brilliant green dye onto AC.


#### 3.3.3. Temkin Isotherm

The Temkin model suggested that the heat of adsorption of all the molecules in the layer would decrease linearly with coverage, and the distribution of binding energy is uniform during the adsorption process [34].A plot of ln(Ce) versus qe (Figure 8) at 25°C is used to calculate the Temkin isotherm constants (qm and Kt). The constants qm and Kt are 5.18 and 1.48, respectively. The obtained R2 for the Temkin isotherm model is 0.863 for the dye.Figure 8
Temkin model for brilliant green dye onto AC.


#### 3.3.4. Dubinin–Radushkevich Isotherm

The plot between ln(qe) and ε2 (Figure 9) at 25°C is used to calculate the constants qm and D whose values are 2.31 and 0.53, respectively. The value of R2 is 0.732.Figure 9
Dubinin model for brilliant green dye onto AC.The isotherm constants andR2 which were computed from the above four isotherms are tabulated in Table 1. From the values of R2, it is strongly suggested that the adsorption of BG onto AC data fits well with the Freundlich isotherm. Finally, the adsorption is a multilayer adsorption and takes place on heterogeneous surfaces.Table 1
Isotherm models and their linearized expression with their parameters for adsorption of the BG dye on AC.
Adsorption isothermParametersR21Langmuirqm = 900.959Km = 0.142FreundlichKf = 0.4270.975n = 1.3263Temkinqm = 5.180.863Kt = 1.484Dubinin–Radushkevichqm = 2.310.732D = 0.53


### 3.4. Adsorption Kinetics

The influence of contact time on the adsorption of BG onto AC was studied to detect the equilibrium time and to investigate the adsorption process. Plots of the change in contact time (5–60 min) versus dye removal percent are presented in Figure10. The removal of BG by sorption onto AC was found to be rapid at the initial period of contact time and then to become slow with the increase in contact time. This is probably due to the larger surface area being available at the beginning for the adsorption of BG dye onto AC. The adsorption of the dye on the AC reaches equilibrium after 20 min. Therefore, a contact time of 20 min for the dye was applied for the further studies as the adsorption equilibrium time. At any time t, the amount of dye taken (qt, mg/g) on the adsorbent was computed by the following model [35]:(13)qt=C0−Ctvm.Figure 10
Effect of contact time on the adsorption of BG dye onto AC.In order to investigate the mechanism of the adsorption and potential rate-controlling steps such as mass transfer and chemical reaction, the kinetics of BG sorption onto AC were investigated by using two different models: the pseudo-first-order and pseudo-second-order kinetic models [36].


#### 3.4.1. Pseudo-First-Order Kinetics

The slope and intercept of the plot log (qe − qt) versus t (Figure 11) give a straight line which represents the pseudo-first-order rate constants (k1 and qe). The values of k1 and qe for the initial dye concentration are listed in Table 2. The value of R2 is found to be 0.932 for the dye.Figure 11
Pseudo-first order for adsorption of brilliant green dye onto AC.Table 2
Kinetic parameters for the adsorption of BG onto AC.
No.ParametersR21Pseudo-first orderk1 × 103 = −0.05 qe = −0.920.9322Pseudo-second orderk2 × 103 = 1.65 qe = 1.110.999


#### 3.4.2. Pseudo-Second-Order Kinetics

The slope of the straight line and intercept resulted by plottingt/qt against t is shown in Figure 12 and presented in Table 2. The value of R2 is found to be 0.999 for the dye. The BG adsorption on AC is well convenient with pseudo-second-order kinetics (R2 = 0.999). Thus, the pseudo-second-order kinetic expression can be used to predict successfully the amount of BG dye adsorbed at equilibrium using the kinetic experimental data.Figure 12
Pseudo-second order for adsorption of brilliant green dye onto AC.


### 3.5. Thermodynamic Studies

The influence of temperature on the adsorption of BG onto AC was investigated in the temperature range of 25–95°C (Figure13). The uptakes of BG dye by AC increase on increasing the temperature, confirming the endothermic nature of the retention step.Figure 13
Effect of temperature on the adsorption of dye onto AC.To understand more the effect of temperature on the adsorption process, the thermodynamic parameters, including the change in enthalpy (∆H, KJ mol−1), Gibbs free energy (∆G, KJ mol−1), and entropy (∆S, J mol−1K−1), were determined. The inherent energy, structural changes, orientation, and feasibility of the adsorption reaction are associated with these parameters [37].The thermodynamic parameters ∆H, ∆S, and ∆G of the dye sorption from the aqueous solution onto the AC were calculated employing equations (9)–(11). The plot of qe/Ce versus 1/T was linear over the temperature range of 298.15–368.15 K. The values of ∆H, ∆S, and ∆G computed from the slope and the intercept (Figure 14) and (Table 3) were found equal to 43.025 kJ/mol, −128 J/mol.K, and 86.188 kJ/mol, respectively. The value of ∆H confirms the endothermic nature of the brilliant green dye. This conclusion was consistent with the results obtained earlier where the adsorption of BG onto AC increased with increasing temperature. The negative values of ∆G demonstrate the spontaneous nature of the adsorption process under study at the limits of the temperatures used. The value of ∆G became more negative with increasing temperature; this showed that the adsorption process was favorable with increasing the temperature. The positive value of ∆S showed the increasing randomness at the solid/liquid interface during the adsorption of the BG dye onto AC.Figure 14
Thermodynamic parameters for the adsorption of dye onto AC.Table 3
Thermodynamic parameters for the adsorption of the BG dye onto AC.
T (K)∆G (kJmol−1)∆H (kJmol−1)∆S (Jmol−1K−1)298−81.18843.025128308−82.468318−83.108328−84.388338−85.668348−86.948358−88.228368−89.508


### 3.6. Comparison with Different Experimental Studies

The results concluded that green dye (BG) removal by adsorption was controlled by the nature of the adsorbent material which can be detected by the change in surface characteristics of the adsorbents with SEM and FTIR, pH, adsorbent dosage, contact time, and the initial concentration of BG in contaminated water. Maximum removal of BG was obtained with activated carbon derived from guava tree wood (99%) in the first 20 min at a dosage of 0.8 g with an adsorption potential of 90 mg/g. In the future, column scale and pilot plant experiments can be implemented to be applied in the wastewater treatment plant for cationic and anionic textile dye removal from wastewater. Authors reported studies on the adsorption of brilliant green dye (BG) from water as illustrated in Table4 with the different optimum conditions.Table 4
Comparison between the present study and previous studies for the biosorption of the brilliant green dye from point of view of the operating parameters.
TypeMaterialVariables pH, temperature, COD conc., water typeRemoval (%)Ref.EDTA-modified magnetic sawdust carbon nanocomposites (EDTA@Fe3O4/SC ncs)pH = 7, room temperature (27°C), dye conc. 10 mg/l, 0.5 g/l, 0.5 h96.7[38]Cotton shell powder (CSP)At optimum dosage (2 g/L), room temperature, dye conc. 80 mg/l, and pH = 8CSPMC > MLMC > CSP > ML (98.8–86.6% > 98.2–82.0% > 92.3–70.7% > 89.0–57.4%)[39]Moringa oleifera leaves (ML)Magnetite-assisted composites ofMoringa oleifera leaves (MLMC)Cotton shell powder (CSPMC)Hydroxyapatite/chitosan nanocompositepH = 7, room temperature (25oC), dye conc. 5 mg/l, 0.9 g/l, 1 h99.5[40]Cu 0.5 Mn 0.5 Fe2O4 nanospinelpH = 2–12, room temperature (25oC), dye conc. 100 mg/l, 3.3 g/l, 2 h92[41]MnO2-loaded activated carbonpH = 7, room temperature (25oC), dye conc. 6 mg/l, 0.44 g/l, 0.06 h99[42]Kaolin90 min, dye concentrations of 20 mg/L, pH = 7, adsorbent dose = 1 g/l91[2]Activated carbon materials were prepared from the Brazilian pine-fruit shell (Araucaria angustifolia)Chemically activated carbon (CAC)5 h at 323 K, pH 5.5; adsorbent mass 50.0 mgThe maximum adsorption capacities were 273.9 and 335.8 mg/g for CAC and CPAC, respectively[43]Chemically and physically activated carbon (CPAC)NaOH-treated saw dustpH = 2.9, contact time = 3 h and adsorbent dose = 4 g/l.T = 3 h, temperature 303 K96[44]Red claypH = 7, RC particle size = 58μm, contact time = 4 h and adsorbent dose = 0.4 g/L and temperature 25°C, dye conc. 20 ppm96[7]ZnS-NP-AC 142.9pH = 6, adsorbent dose = 0.015 g, time = 35 min, temperature: 27 ± 2°C, BG conc. 5 mg/L98[45]ZnS-NP-AC-BG 250Zinc sulfide nanoparticles loaded on activated carbon (ZnS-NPs-AC)pH = 5, 20 mg of ZnS-NP-AC, 7 mg L−1 of BG after 4 min sonication95% adsorption capacity 258 mg g−1[46]ZnO nanoparticlesDye conc. 10–100 mg/L, temp. −27 ± 1 ̊C, adsorbent dose 0.04 g and time 120 min., pH 6.5 ± 0.590[47]Activated carbon derived from guava tree woodTime (qt) is 20 minutes, pH 7, initial BG dye of 25 mg/l and AC dosage greater than 0.8 g99This study


## 3.1. Characterization of AC

In order to obtain information about the mode of interaction of the brilliant green dye with activated carbon, different physicochemical measurements were done, which are presented below.


### 3.1.1. Scanning Electron Microscopy (SEM)

Figures1(a) and 1(b) show the SEM image of AC and adsorbed BG onto AC, respectively. The SEM image of the AC sample before dye adsorption (Figure 1(a)) obviously shows the surface morphology with an irregular texture and high surface roughness and different levels of porosity in AC, which provides possible sites for adsorption of the dye. The surface roughness and the macropores which are important factors for the dye adsorption were responsible for the high surface area, making AC a good adsorbent. After adsorption with the dye, a large area of AC was covered with dye molecules in the form of flakes, and thus the SEM image of AC after adsorption showed a smooth surface because the BG molecules were trapped and sorbed on the surface of AC.Figure 1
SEM images of the AC adsorbent. (a) AC only and (b) AC + BG dye.


### 3.1.2. Fourier-Transform Infrared (FTIR) Spectra

A substantial part of the knowledge concerning the mode of the bonding in the dye compound can be gained by applying infrared spectra. In such a case, the spectrum of AC is usually compared with that of the AC-dye species to get an idea about the function groups which react with the dye. The IR spectra of the sorbed species and AC are depicted in Figure2.Figure 2
FTIR for (a) activated carbon and (b) activated carbon with brilliant green dye.
(a)(b)Figure2 represents the FTIR spectrum of the adsorbent (AC) before and after adsorption. The FTIR spectrum of AC showed different bands at 3440, 2918, 1598, 1452, and 782 cm−1assigned to O-H, -CH aliphatic, -C=C, -CH2 bending, and -C=S. The FTIR spectrum of AC-BG compared with that of AC showed that there are bands at 3442, 2920, 1583, 1440, and 811 cm−1 assigned to O-H, -CH aliphatic, -C=C, -CH2 bending, and -C=S. The FTIR spectrum of the AC-BG showed shifts in bands to higher and/or to lower with appearance or disappearance of other bands, which indicate the complete adsorption of the BG dye.


### 3.1.3. BET

The specific surface area of the prepared AC was obtained by the nitrogen adsorption/desorption isotherm at 77 K using the high-speed gas sorption analyzer (NOVA 1000, Version 6.11, Quanta Chrome Corporation) employing the Brunauer–Emmett–Teller (BET) method (activation temperature of 900°C and activation time 0.5 hr.). The specific surface area was found to be equal to 310 m2/g. This area can provide many active sites that increase the chances of adsorption.


## 3.1.1. Scanning Electron Microscopy (SEM)

Figures1(a) and 1(b) show the SEM image of AC and adsorbed BG onto AC, respectively. The SEM image of the AC sample before dye adsorption (Figure 1(a)) obviously shows the surface morphology with an irregular texture and high surface roughness and different levels of porosity in AC, which provides possible sites for adsorption of the dye. The surface roughness and the macropores which are important factors for the dye adsorption were responsible for the high surface area, making AC a good adsorbent. After adsorption with the dye, a large area of AC was covered with dye molecules in the form of flakes, and thus the SEM image of AC after adsorption showed a smooth surface because the BG molecules were trapped and sorbed on the surface of AC.Figure 1
SEM images of the AC adsorbent. (a) AC only and (b) AC + BG dye.


## 3.1.2. Fourier-Transform Infrared (FTIR) Spectra

A substantial part of the knowledge concerning the mode of the bonding in the dye compound can be gained by applying infrared spectra. In such a case, the spectrum of AC is usually compared with that of the AC-dye species to get an idea about the function groups which react with the dye. The IR spectra of the sorbed species and AC are depicted in Figure2.Figure 2
FTIR for (a) activated carbon and (b) activated carbon with brilliant green dye.
(a)(b)Figure2 represents the FTIR spectrum of the adsorbent (AC) before and after adsorption. The FTIR spectrum of AC showed different bands at 3440, 2918, 1598, 1452, and 782 cm−1assigned to O-H, -CH aliphatic, -C=C, -CH2 bending, and -C=S. The FTIR spectrum of AC-BG compared with that of AC showed that there are bands at 3442, 2920, 1583, 1440, and 811 cm−1 assigned to O-H, -CH aliphatic, -C=C, -CH2 bending, and -C=S. The FTIR spectrum of the AC-BG showed shifts in bands to higher and/or to lower with appearance or disappearance of other bands, which indicate the complete adsorption of the BG dye.


## 3.1.3. BET

The specific surface area of the prepared AC was obtained by the nitrogen adsorption/desorption isotherm at 77 K using the high-speed gas sorption analyzer (NOVA 1000, Version 6.11, Quanta Chrome Corporation) employing the Brunauer–Emmett–Teller (BET) method (activation temperature of 900°C and activation time 0.5 hr.). The specific surface area was found to be equal to 310 m2/g. This area can provide many active sites that increase the chances of adsorption.


## 3.2. Affecting Parameters on Adsorption

### 3.2.1. Effect of pH

The pH value is an important parameter in controlling the adsorption process due to the ionization of surface functional groups in the solution [27]. To study the influence of pH on the adsorption of the BG dye onto AC, experiments were performed using various initial pH values varying from 2 to 12. The results indicate that the percentage removal of the BG dye increases with the increase in pH up to a pH value of 7 (Figure 3), after which the removal of BG dye decreases with the increase in pH. At lower pH values, the BG removal was reduced, probably as a result of the competition between hydrogen ions and the dye cations for the sorption sites of AC [28]. The surface of the AC may get negatively charged at higher pH, which increases the chances of attraction force with the cationic dye through electrostatic force of attraction [29]. Generally, the net positive charge decreases with increasing pH value leading to the decrease in the repulsion force between the adsorbent surface and the dye, thus improving the adsorption capacity.Figure 3
Effect of pH on the adsorption of the BG dye using AC.


### 3.2.2. Effect of Adsorbent Dose

Figure4 shows the influence of AC mass on the removal of BG dye from aqueous solutions. With an increase in the amount of the adsorbent material, the uptake of the dye increases. The adsorption of the BG dye increases significantly (from 83% to 99%) when the adsorbent dose increases from 0.1 g to 0.8 g, but the removal efficiency of the dye does not change significantly when the adsorbent dose is increased above 0.8 g. So, 0.8 g of the adsorbent (AC) can be considered the optimal dose for the adsorption of the BG dye. For the brilliant green dye, it is clear that the percentage removal increased gradually as the adsorbent mass increased. This effect can be attributed to the increase in the surface area and the active sites of the adsorbent [30].Figure 4
Effect of adsorbent dosage on the adsorption of the BG dye using AC.


### 3.2.3. Effect of Initial Dye Concentration

The influence of initial dye concentration (Ci) was studied in the range (5–100 mg/l) at temperature 25°C, 240 rpm, and 20 min contact time, and the results are shown in Figure 5. From Figure 5, the removal efficiency of the activated carbon decreased with increasing initial dye concentration. There will be unoccupied active sites on the AC surface at low dye concentration, and the active sites required for adsorption of the BG molecules will be lacking when the initial dye concentration increases [31].Figure 5
Effect of initial dye concentration on the adsorption onto AC.


## 3.2.1. Effect of pH

The pH value is an important parameter in controlling the adsorption process due to the ionization of surface functional groups in the solution [27]. To study the influence of pH on the adsorption of the BG dye onto AC, experiments were performed using various initial pH values varying from 2 to 12. The results indicate that the percentage removal of the BG dye increases with the increase in pH up to a pH value of 7 (Figure 3), after which the removal of BG dye decreases with the increase in pH. At lower pH values, the BG removal was reduced, probably as a result of the competition between hydrogen ions and the dye cations for the sorption sites of AC [28]. The surface of the AC may get negatively charged at higher pH, which increases the chances of attraction force with the cationic dye through electrostatic force of attraction [29]. Generally, the net positive charge decreases with increasing pH value leading to the decrease in the repulsion force between the adsorbent surface and the dye, thus improving the adsorption capacity.Figure 3
Effect of pH on the adsorption of the BG dye using AC.


## 3.2.2. Effect of Adsorbent Dose

Figure4 shows the influence of AC mass on the removal of BG dye from aqueous solutions. With an increase in the amount of the adsorbent material, the uptake of the dye increases. The adsorption of the BG dye increases significantly (from 83% to 99%) when the adsorbent dose increases from 0.1 g to 0.8 g, but the removal efficiency of the dye does not change significantly when the adsorbent dose is increased above 0.8 g. So, 0.8 g of the adsorbent (AC) can be considered the optimal dose for the adsorption of the BG dye. For the brilliant green dye, it is clear that the percentage removal increased gradually as the adsorbent mass increased. This effect can be attributed to the increase in the surface area and the active sites of the adsorbent [30].Figure 4
Effect of adsorbent dosage on the adsorption of the BG dye using AC.


## 3.2.3. Effect of Initial Dye Concentration

The influence of initial dye concentration (Ci) was studied in the range (5–100 mg/l) at temperature 25°C, 240 rpm, and 20 min contact time, and the results are shown in Figure 5. From Figure 5, the removal efficiency of the activated carbon decreased with increasing initial dye concentration. There will be unoccupied active sites on the AC surface at low dye concentration, and the active sites required for adsorption of the BG molecules will be lacking when the initial dye concentration increases [31].Figure 5
Effect of initial dye concentration on the adsorption onto AC.


## 3.3. Adsorption Isotherm

The adsorption isotherms were determined by shaking 0.8 g of the AC with 50 ml of 5 to 100 mg/l of BG solutions for 20 min. The adsorption isotherms are used to relate the adsorbed amount at the interface and the adsorbent concentration in the bulk solution [32] and is important for the design of an adsorption system. The correlation coefficient values (R2) were used as a criterion to infer the most appropriate isotherm equation that can be selected to describe the adsorption process.


### 3.3.1. Langmuir Isotherm

The linear form can be used for the linearization of experimental data by plottingCe/qe against Ce (Figure 6). The Langmuir constant qm (mg/g) which is a measure of the maximum adsorption capacity of AC is obtained as 90 mg/g. Km is the Langmuir constant which relating to adsorption energy is found to be 0.14 mg−1 for the brilliant green dye. The feasibility of the process can be evaluated by a separation factor (dimensionless constant) “RL” which is given in the following equation:(12)RL=11+KLCi,where “Ci” is the initial dye concentration (mg/L) and the “RL” value is between zero and one for favorable adsorption, whereas (RL > 1), (RL = 1), and (RL = zero) for unfavorable, linear, and irreversible adsorption, respectively [7].Figure 6
Langmuir model for brilliant green dye onto AC.


### 3.3.2. Freundlich Isotherm

By plotting the graph between ln(qe) and ln(ce) (Figure 7), the Freundlich constants (KF and n) can be obtained from the slope and the intercept of the linear plot of the experimental data. The values of Kf and n are 0.427 and 1.326, respectively. The value of n indicates the degree of nonlinearity between solution concentration and adsorption; if n = 1, then adsorption is linear; if n < 1, then adsorption is a chemical process; if n > 1, then adsorption is a physical process [33]. The n value was found to be 1.326 for AC. Since n > 1, the adsorption of the BG dye onto AC is a physical process. It is found that the correlation coefficient value (R2) obtained from the Freundlich isotherm model for AC is 0.975 for the dye.Figure 7
Freundlich model for brilliant green dye onto AC.


### 3.3.3. Temkin Isotherm

The Temkin model suggested that the heat of adsorption of all the molecules in the layer would decrease linearly with coverage, and the distribution of binding energy is uniform during the adsorption process [34].A plot of ln(Ce) versus qe (Figure 8) at 25°C is used to calculate the Temkin isotherm constants (qm and Kt). The constants qm and Kt are 5.18 and 1.48, respectively. The obtained R2 for the Temkin isotherm model is 0.863 for the dye.Figure 8
Temkin model for brilliant green dye onto AC.


### 3.3.4. Dubinin–Radushkevich Isotherm

The plot between ln(qe) and ε2 (Figure 9) at 25°C is used to calculate the constants qm and D whose values are 2.31 and 0.53, respectively. The value of R2 is 0.732.Figure 9
Dubinin model for brilliant green dye onto AC.The isotherm constants andR2 which were computed from the above four isotherms are tabulated in Table 1. From the values of R2, it is strongly suggested that the adsorption of BG onto AC data fits well with the Freundlich isotherm. Finally, the adsorption is a multilayer adsorption and takes place on heterogeneous surfaces.Table 1
Isotherm models and their linearized expression with their parameters for adsorption of the BG dye on AC.
Adsorption isothermParametersR21Langmuirqm = 900.959Km = 0.142FreundlichKf = 0.4270.975n = 1.3263Temkinqm = 5.180.863Kt = 1.484Dubinin–Radushkevichqm = 2.310.732D = 0.53


## 3.3.1. Langmuir Isotherm

The linear form can be used for the linearization of experimental data by plottingCe/qe against Ce (Figure 6). The Langmuir constant qm (mg/g) which is a measure of the maximum adsorption capacity of AC is obtained as 90 mg/g. Km is the Langmuir constant which relating to adsorption energy is found to be 0.14 mg−1 for the brilliant green dye. The feasibility of the process can be evaluated by a separation factor (dimensionless constant) “RL” which is given in the following equation:(12)RL=11+KLCi,where “Ci” is the initial dye concentration (mg/L) and the “RL” value is between zero and one for favorable adsorption, whereas (RL > 1), (RL = 1), and (RL = zero) for unfavorable, linear, and irreversible adsorption, respectively [7].Figure 6
Langmuir model for brilliant green dye onto AC.


## 3.3.2. Freundlich Isotherm

By plotting the graph between ln(qe) and ln(ce) (Figure 7), the Freundlich constants (KF and n) can be obtained from the slope and the intercept of the linear plot of the experimental data. The values of Kf and n are 0.427 and 1.326, respectively. The value of n indicates the degree of nonlinearity between solution concentration and adsorption; if n = 1, then adsorption is linear; if n < 1, then adsorption is a chemical process; if n > 1, then adsorption is a physical process [33]. The n value was found to be 1.326 for AC. Since n > 1, the adsorption of the BG dye onto AC is a physical process. It is found that the correlation coefficient value (R2) obtained from the Freundlich isotherm model for AC is 0.975 for the dye.Figure 7
Freundlich model for brilliant green dye onto AC.


## 3.3.3. Temkin Isotherm

The Temkin model suggested that the heat of adsorption of all the molecules in the layer would decrease linearly with coverage, and the distribution of binding energy is uniform during the adsorption process [34].A plot of ln(Ce) versus qe (Figure 8) at 25°C is used to calculate the Temkin isotherm constants (qm and Kt). The constants qm and Kt are 5.18 and 1.48, respectively. The obtained R2 for the Temkin isotherm model is 0.863 for the dye.Figure 8
Temkin model for brilliant green dye onto AC.


## 3.3.4. Dubinin–Radushkevich Isotherm

The plot between ln(qe) and ε2 (Figure 9) at 25°C is used to calculate the constants qm and D whose values are 2.31 and 0.53, respectively. The value of R2 is 0.732.Figure 9
Dubinin model for brilliant green dye onto AC.The isotherm constants andR2 which were computed from the above four isotherms are tabulated in Table 1. From the values of R2, it is strongly suggested that the adsorption of BG onto AC data fits well with the Freundlich isotherm. Finally, the adsorption is a multilayer adsorption and takes place on heterogeneous surfaces.Table 1
Isotherm models and their linearized expression with their parameters for adsorption of the BG dye on AC.
Adsorption isothermParametersR21Langmuirqm = 900.959Km = 0.142FreundlichKf = 0.4270.975n = 1.3263Temkinqm = 5.180.863Kt = 1.484Dubinin–Radushkevichqm = 2.310.732D = 0.53


## 3.4. Adsorption Kinetics

The influence of contact time on the adsorption of BG onto AC was studied to detect the equilibrium time and to investigate the adsorption process. Plots of the change in contact time (5–60 min) versus dye removal percent are presented in Figure10. The removal of BG by sorption onto AC was found to be rapid at the initial period of contact time and then to become slow with the increase in contact time. This is probably due to the larger surface area being available at the beginning for the adsorption of BG dye onto AC. The adsorption of the dye on the AC reaches equilibrium after 20 min. Therefore, a contact time of 20 min for the dye was applied for the further studies as the adsorption equilibrium time. At any time t, the amount of dye taken (qt, mg/g) on the adsorbent was computed by the following model [35]:(13)qt=C0−Ctvm.Figure 10
Effect of contact time on the adsorption of BG dye onto AC.In order to investigate the mechanism of the adsorption and potential rate-controlling steps such as mass transfer and chemical reaction, the kinetics of BG sorption onto AC were investigated by using two different models: the pseudo-first-order and pseudo-second-order kinetic models [36].


### 3.4.1. Pseudo-First-Order Kinetics

The slope and intercept of the plot log (qe − qt) versus t (Figure 11) give a straight line which represents the pseudo-first-order rate constants (k1 and qe). The values of k1 and qe for the initial dye concentration are listed in Table 2. The value of R2 is found to be 0.932 for the dye.Figure 11
Pseudo-first order for adsorption of brilliant green dye onto AC.Table 2
Kinetic parameters for the adsorption of BG onto AC.
No.ParametersR21Pseudo-first orderk1 × 103 = −0.05 qe = −0.920.9322Pseudo-second orderk2 × 103 = 1.65 qe = 1.110.999


### 3.4.2. Pseudo-Second-Order Kinetics

The slope of the straight line and intercept resulted by plottingt/qt against t is shown in Figure 12 and presented in Table 2. The value of R2 is found to be 0.999 for the dye. The BG adsorption on AC is well convenient with pseudo-second-order kinetics (R2 = 0.999). Thus, the pseudo-second-order kinetic expression can be used to predict successfully the amount of BG dye adsorbed at equilibrium using the kinetic experimental data.Figure 12
Pseudo-second order for adsorption of brilliant green dye onto AC.


## 3.4.1. Pseudo-First-Order Kinetics

The slope and intercept of the plot log (qe − qt) versus t (Figure 11) give a straight line which represents the pseudo-first-order rate constants (k1 and qe). The values of k1 and qe for the initial dye concentration are listed in Table 2. The value of R2 is found to be 0.932 for the dye.Figure 11
Pseudo-first order for adsorption of brilliant green dye onto AC.Table 2
Kinetic parameters for the adsorption of BG onto AC.
No.ParametersR21Pseudo-first orderk1 × 103 = −0.05 qe = −0.920.9322Pseudo-second orderk2 × 103 = 1.65 qe = 1.110.999


## 3.4.2. Pseudo-Second-Order Kinetics

The slope of the straight line and intercept resulted by plottingt/qt against t is shown in Figure 12 and presented in Table 2. The value of R2 is found to be 0.999 for the dye. The BG adsorption on AC is well convenient with pseudo-second-order kinetics (R2 = 0.999). Thus, the pseudo-second-order kinetic expression can be used to predict successfully the amount of BG dye adsorbed at equilibrium using the kinetic experimental data.Figure 12
Pseudo-second order for adsorption of brilliant green dye onto AC.


## 3.5. Thermodynamic Studies

The influence of temperature on the adsorption of BG onto AC was investigated in the temperature range of 25–95°C (Figure13). The uptakes of BG dye by AC increase on increasing the temperature, confirming the endothermic nature of the retention step.Figure 13
Effect of temperature on the adsorption of dye onto AC.To understand more the effect of temperature on the adsorption process, the thermodynamic parameters, including the change in enthalpy (∆H, KJ mol−1), Gibbs free energy (∆G, KJ mol−1), and entropy (∆S, J mol−1K−1), were determined. The inherent energy, structural changes, orientation, and feasibility of the adsorption reaction are associated with these parameters [37].The thermodynamic parameters ∆H, ∆S, and ∆G of the dye sorption from the aqueous solution onto the AC were calculated employing equations (9)–(11). The plot of qe/Ce versus 1/T was linear over the temperature range of 298.15–368.15 K. The values of ∆H, ∆S, and ∆G computed from the slope and the intercept (Figure 14) and (Table 3) were found equal to 43.025 kJ/mol, −128 J/mol.K, and 86.188 kJ/mol, respectively. The value of ∆H confirms the endothermic nature of the brilliant green dye. This conclusion was consistent with the results obtained earlier where the adsorption of BG onto AC increased with increasing temperature. The negative values of ∆G demonstrate the spontaneous nature of the adsorption process under study at the limits of the temperatures used. The value of ∆G became more negative with increasing temperature; this showed that the adsorption process was favorable with increasing the temperature. The positive value of ∆S showed the increasing randomness at the solid/liquid interface during the adsorption of the BG dye onto AC.Figure 14
Thermodynamic parameters for the adsorption of dye onto AC.Table 3
Thermodynamic parameters for the adsorption of the BG dye onto AC.
T (K)∆G (kJmol−1)∆H (kJmol−1)∆S (Jmol−1K−1)298−81.18843.025128308−82.468318−83.108328−84.388338−85.668348−86.948358−88.228368−89.508


## 3.6. Comparison with Different Experimental Studies

The results concluded that green dye (BG) removal by adsorption was controlled by the nature of the adsorbent material which can be detected by the change in surface characteristics of the adsorbents with SEM and FTIR, pH, adsorbent dosage, contact time, and the initial concentration of BG in contaminated water. Maximum removal of BG was obtained with activated carbon derived from guava tree wood (99%) in the first 20 min at a dosage of 0.8 g with an adsorption potential of 90 mg/g. In the future, column scale and pilot plant experiments can be implemented to be applied in the wastewater treatment plant for cationic and anionic textile dye removal from wastewater. Authors reported studies on the adsorption of brilliant green dye (BG) from water as illustrated in Table4 with the different optimum conditions.Table 4
Comparison between the present study and previous studies for the biosorption of the brilliant green dye from point of view of the operating parameters.
TypeMaterialVariables pH, temperature, COD conc., water typeRemoval (%)Ref.EDTA-modified magnetic sawdust carbon nanocomposites (EDTA@Fe3O4/SC ncs)pH = 7, room temperature (27°C), dye conc. 10 mg/l, 0.5 g/l, 0.5 h96.7[38]Cotton shell powder (CSP)At optimum dosage (2 g/L), room temperature, dye conc. 80 mg/l, and pH = 8CSPMC > MLMC > CSP > ML (98.8–86.6% > 98.2–82.0% > 92.3–70.7% > 89.0–57.4%)[39]Moringa oleifera leaves (ML)Magnetite-assisted composites ofMoringa oleifera leaves (MLMC)Cotton shell powder (CSPMC)Hydroxyapatite/chitosan nanocompositepH = 7, room temperature (25oC), dye conc. 5 mg/l, 0.9 g/l, 1 h99.5[40]Cu 0.5 Mn 0.5 Fe2O4 nanospinelpH = 2–12, room temperature (25oC), dye conc. 100 mg/l, 3.3 g/l, 2 h92[41]MnO2-loaded activated carbonpH = 7, room temperature (25oC), dye conc. 6 mg/l, 0.44 g/l, 0.06 h99[42]Kaolin90 min, dye concentrations of 20 mg/L, pH = 7, adsorbent dose = 1 g/l91[2]Activated carbon materials were prepared from the Brazilian pine-fruit shell (Araucaria angustifolia)Chemically activated carbon (CAC)5 h at 323 K, pH 5.5; adsorbent mass 50.0 mgThe maximum adsorption capacities were 273.9 and 335.8 mg/g for CAC and CPAC, respectively[43]Chemically and physically activated carbon (CPAC)NaOH-treated saw dustpH = 2.9, contact time = 3 h and adsorbent dose = 4 g/l.T = 3 h, temperature 303 K96[44]Red claypH = 7, RC particle size = 58μm, contact time = 4 h and adsorbent dose = 0.4 g/L and temperature 25°C, dye conc. 20 ppm96[7]ZnS-NP-AC 142.9pH = 6, adsorbent dose = 0.015 g, time = 35 min, temperature: 27 ± 2°C, BG conc. 5 mg/L98[45]ZnS-NP-AC-BG 250Zinc sulfide nanoparticles loaded on activated carbon (ZnS-NPs-AC)pH = 5, 20 mg of ZnS-NP-AC, 7 mg L−1 of BG after 4 min sonication95% adsorption capacity 258 mg g−1[46]ZnO nanoparticlesDye conc. 10–100 mg/L, temp. −27 ± 1 ̊C, adsorbent dose 0.04 g and time 120 min., pH 6.5 ± 0.590[47]Activated carbon derived from guava tree woodTime (qt) is 20 minutes, pH 7, initial BG dye of 25 mg/l and AC dosage greater than 0.8 g99This study


## 4. Conclusion

The removal of the brilliant green dye from wastewater using activated carbon derived from guava tree wood has been investigated under different experimental conditions in the batch mode. The FTIR results reveal that a large amount of chemical functional groups were well maintained and created on the surface of AC, which might improve its adsorptive properties due to the functional groups O-H, -CH aliphatic, -C=C, -CH2 bending, and -C=S. It also showed that the SEM analysis exhibited approval of the adsorption process due to the surface texture of the examined plant. The adsorbent (AC) can completely remove the BG dye from an aqueous solution at the following conditions: pH 7, initial BG dye of 25 mg/l, and contact time 20 minutes. The adsorption efficiency increases with increasing dose, and the optimum dose is 0.8 g with the removal efficiency of 99% and adsorption capacity (qe) of 90 mg BG dye/g AC. The sorption of dye follows the Freundlich isotherm, indicating the heterogeneous adsorption surface with multilayer adsorption taking place on the heterogeneous AC from the guava tree surface’s innumerous adsorption sites. This was also supported by the results of the kinetic study for BG dye removal, which were obtained following the pseudo-second-order model. This model, used to clarify the probability of overall adsorption properties, was suited to the chemical adsorption mechanism. From the values of thermodynamic parameters, the adsorption process is spontaneous and endothermic. AC from the guava tree can be effectively used as an adsorbent comparable with the other commercial adsorbents used. AC from the guava tree wood is economically cheap, and so regeneration is not necessary.



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