Adsorptive removal of anionic dye from aqueous solutions using powdered and calcined vegetables wastes as low-cost adsorbent

Abstract

In this study, we describe a behaviour comparison between powdered and calcined adsorbents prepared from vegetables waste of Persea species to remove Eriochrome Black T as anionic dye from aqueous solutions. Potential capabilities of these two adsorbents have been evaluated by studying some experimental parameters such as solution pH, adsorbent dosage, initial dye concentration, contact time and temperature. Kinetic study has been achieved by the application of pseudo-first and second orders and Elovich model. Results found agreed well with the pseudo-second order model. The experimental data were analysed using Langmuir, Freundlich and Tempkin isotherms models. The equilibrium data fitted well with the Freundlich isotherm and the adsorption capacities were calculated to be 120.50 mg/g and of 96.15 mg/g for calcined and powdered adsorbents, respectively. Thermodynamic study was also undertaken and provided important results indicating a spontaneous reaction and feasibility on the two adsorbents. The two adsorbents have been characterized via spectroscopic data such infrared spectrum, X-ray and by emission scanning electron microscopy.

Keywords:

• Persea species
• powdered adsorbent
• calcined adsorbent
• anionic dye
• removal

1. Introduction

Adsorption is one of the most used tools for the removal of pollutant chemicals species. Every day researchers describe new ways and elaborate a new adsorbent on the basis of good selectivity for a chemical species, or for the low cost of the process. Among the chemical species removed by adsorption are industrial dyes. It is already known that dyes are very toxic and cause undesirable effects when discharged to aqueous media by preventing the penetration of sunlight, depleting dissolved oxygen and affecting human and animal health (Abuzer, Mehmet, & Huseyin, 2009; Chakraborty, Basak, Dutta, Bhunia, & Dey, 2013).

A number of conventional methods are used for textile wastewater treatment, generally classified as biological, chemical and physical treatments (Nethaji, Sivasamy, Thennarasu, & Saravanan, 2010; El Haddad et al., 2012; Azizian, 2004; Mittal, Mittal, Malviya, & Gupta, 2010; Gupta, Jain, Nayak, Agarwal, & Shrivastava, 2011; Saravan et al., 2013a, 2013b, 2013c; Saravanan et al., 2015). The current study focuses on the adsorption technique as it is an effective and inexpensive treatment option. The adsorption process can be carried out using various inexpensive and renewable adsorbents, making the treatment even more inexpensive.

Activated carbon is the most preferred adsorbent for the removal of dyes because of its excellent adsorption ability. However, widespread use of activated carbon is restricted because of its high cost. An alternative adsorbent is considered to be of low cost when minimal processing is required, it is abundant in nature, or it is derived from industrial by-products (Sonai, de Souza, de Oliveira, & de Souza, 2016). Among these, different sorts of materials have been studied as potential adsorbents for the removal of dyes by a number of researchers. Some that are commonly used include Cerastoderma lamarcki shell (Kazemi, Biparva, & Ashtiani, 2016), Partherium hysterophorus (Chatterjee, Kumar, Basu, & Dutta, 2012), sugar beet pulp (Malekbala, Hosseini, Kazemi Yazdi, Masoudi Soltani, & Malekbala, 2012), animal bones (Slimani et al., 2011), mussel shells (El Haddad et al., 2014), pistachio shell (Deniz and Kepekci, 2016), orange peel powder (Munagapati and Kim, 2016), peanut hull waste (Tahira, Bhatti, Iqbal, & Noreen, 2017), mango stone (Shoukat, Bhatti, Iqbal, & Noreen, 1987), clay/MnFe₂O₄ composite (Kanwal, Bhatti, Iqbal, & Noreen, 2017), native acidic and composite clay (Ehsan, Bhatti, Iqbla, & Noreen, 2017) and calcined bones (El Haddad, Mamouni, Saffaj, & Lazar, 2016).

The chromophores in anionic and non-ionic dyes mostly consist of anthraquinone or azo groups. Due to fused aromatic rings, anthraquinone-based dyes are particularly resistant to degradation, and their persistence in wastewaters is growing at the present time. In this fact, the presence of an azo group (N = N) on Eriochrome Black T (EBT) and its low biodegradability makes it a concern for environmental study. The removal of EBT dye from aqueous solutions is very important due to its toxicity, and it was selected in this study as representative anionic dye.

In our research plan, we have already undertaken many studies for the removal anionic and cationic dyes from aqueous media using calcined mussel shells and bones and sawdust.

We describe here the ability of powdered Persea americana nuts and Persea americana nuts calcined and activated under acidic conditions for the adsorption of an azo anionic dye such as EBT contained in aqueous solution. A comparative study was made for the evaluation of the potentialities of the two prepared adsorbents for removing dye from aqueous solutions. The adsorption experiments were performed in batch mode, and studies such as isotherms models, kinetics forms, and thermodynamic calculations were evaluated and discussed. Finally, the reusability efficiency of the two adsorbents was enhanced.

2. Materials and methods

2.1. Adsorbents preparation

Persea americana nuts were washed several times with distilled water to remove adhered impurities from their surface. The resulting material was dried at 105 °C for 24 h, crushed and sieved. This is abbreviated as P – PAN for powdered Persea americana nuts.

The activation of P – PAN was carried out using an appropriate weight and 25 mL of concentrated phosphoric acid (1:4) and completed by carbonization at temperature 500 °C for 2 hours, producing a black carbonaceous residue. The activated carbon was repeatedly washed with distilled water until neutral pH was achieved. The resulting adsorbent was dried at 105 °C for 2 hours, and was abbreviated as C – PAN, for carbon Persea americana nuts.

The characterization of P – PAN and C – PAN adsorbents was achieved by Fourier-transform infrared spectroscopy (FT–IR) applied to investigate the surface characteristic functional groups and scanning electronic microscopy (SEM) images for studying the morphology of surface texture.

2.2. Preparation of Eriochrome Black T solution

The chemical structure of the studied dye EBT is shown in Figure 1, and its characteristics are summarized in Table 1. The stock of EBT dye solution (1000 mg/L) was prepared by dissolving 100 mg of EBT dye in 1L of distilled water. Experimental solutions of the desired concentrations were prepared by successive dilutions. The pH zero point charge (pH_ZPC) of the P – PAN and C – PAN adsorbents was determined using the pH drift method (Foo and Hameed, 2012).

Figure 1. Chemical structure of EBT.

Table 1. Some properties of Eriochrome Black T dye.

Dye class	Anionic azo
Molecular formula	C20H12N3NaO7S
Molecular weight	461.38 g/mol
Maximum wavelength (λmax)	530 nm
Solubility in water (20 °C)	50 g/L
Solubility in ethanol (20 °C)	2 g/L
Colour	Black

2.3. Experimentation conditions of adsorption studies

The adsorption isotherm and kinetics experiments were performed by batch mode. An aliquot of 50 mL of EBT dye solution of known initial concentration (60 mg/L) was used. The mixture solution was stirred at 1500 rpm, with a required dose of adsorbents (10–25 mg) for a specific period of contact time (5–60 min) using a magnetic stirrer, after noting down the initial pH of the solution to the optimum pH. The pH of the solutions was adjusted to the required value by adding either 0.1 M HCl or 0.1 M NaOH solution.

After equilibrium, the final concentration (C_e) was measured using absorbance values with a UV/Visible spectrophotometer (JANWAY 6300) and compared with the absorbance values of the initial solutions. The absorbance was measured at 530 nm. Experiments were carried out in duplicate and mean values are presented. The percent removal (%) of dyes was calculated using the following equation: $$\text{\% Removal dye}=\mathrm{ }\frac{C_0-C_e}{C_0}\times 100$$

where C₀ is the initial dye concentration and C_e (mg/L) is the concentrations of EBT dye at equilibrium.

The amount of dye adsorption per unit mass of P – PAN and C – PAN adsorbents at equilibrium, q_e (mg/g) was calculated by the following equation: $$q_e=\mathrm{ }\frac{C_0-\mathrm{ }{C}_e}{W}\mathrm{ }V$$

where C_e (mg/L) is the liquid concentration of dye at equilibrium, C₀ (mg/L) is the initial concentration of the EBT dye in solution. V is the volume of the solution (L) and W is the mass of dye adsorbent (g).

3. Results and discussion

3.1. Characterization of P – PAN and C – PAN adsorbents

The FT–IR spectra of the unmodified and modified P – PAN were obtained to determine the surface functional groups and are shown in Figure 2(a) and (b).

Figure 2. FT–IR spectra of C – PAN and P – PAN adsorbents.

From Figure 2(a) the peaks were also found at frequencies: 876, 1074, 1149, 1563, 2916 and 3415 cm⁻¹. The absorption band at 3415 cm⁻¹ is attributed to the hydroxyl groups (OH) vibration (Liang, Guo, & Tian, 2011). The bands at 2916 cm⁻¹, 1563 cm⁻¹ and 1381 cm⁻¹ correspond, respectively, to unsymmetrical aliphatic C–H stretching, C=C stretching of aromatic rings and aromatic C=C stretching vibration. The band at 1149 cm⁻¹ is ascribed to C–O stretching in alcohol or ether or hydroxyl group (He, Ma, He, Zhao, & Yu, 2002; Pavia, Lampman, & Kaiz, 1987).

From Figure 2(b), the peaks at 3275.13 cm⁻¹ and 2924.09 cm⁻¹ indicate the presence of hydroxyl (OH) group. The peak around 1635 cm⁻¹ is due to the C=C stretching that can be attributed to the aromatic C–C bond, while bands at 1021 cm⁻¹ and 1454 cm⁻¹ are due, respectively, to C–O–C, P–O or P–OH stretching.

SEM has been a primary tool for characterizing the surface morphology and fundamental physical properties of the adsorbent. SEM images of C – PAN and P – PAN are shown in Figure 3. As can be seen from this figure, a lot of large pores were clearly found on the surface of C – PAN relative to the surface of P – PAN.

Figure 3. SEM image of C – PAN and P – PAN adsorbents.

3.2. Effect of adsorbent dosage

The effect of adsorbent dosage of P – PAN and C – PAN adsorbents was studied at different amounts of adsorbents (10, 15, 20, and 25 mg); analyses were conducted using 50 mL of EBT solutions at 60 mg/L at ambient temperature and at pH 2. In the light of these results, it appears that equilibrium of P – PAN and C – PAN adsorbents was attained above 60 min. Before this time, the % adsorption increases from 43% to 51% for P – PAN and from 48% to 69% for C – PAN, when the adsorbent dosage was increased from 10 to 25 mg. It was observed that the uptake of the EBT dye increased by the amount of adsorbents added and that the maximum dye removal was achieved within the amount 25 mg. This implied that the number of adsorption sites increased as the adsorbents’ mass increases (see Figure 4). This can be attributed to the increase in the adsorbent surface area and availability of more adsorption sites (Mahmoodi, Hayati, Arami, & Lan, 2011). Finally, % removal efficiency of EBT was better onto C – PAN than onto P – PAN. These results can be explained by the higher affinity for C – PAN making many pores on the adsorbent area.

Figure 4. Effects of P – PAN and C – PAN adsorbent amounts on the % removal efficiency of EBT dye. Experimental conditions: C₀ = 60 mg/L, pH = 2, V = 50 mL, ambient temperature.

3.3. Effect of pH

pH plays an important role in the determination of significant adsorption capacity of an adsorbent. This study explores the variation of % adsorption of EBT dye onto P – PAN and C – PAN adsorbents versus pH (2 – 10). All results of this study are shown in Figure 5. It is observed that uptake decreases from 50.65 to 4.01% for P – PAN and from 68.87 to 31.23% for C – PAN with increasing pH from 2 to 10. In explaining this behaviour, the determination of pH_ZPC plays an important role. Thus, pH_ZPC of P – PAN is 5 and is of 2.1 for C – PAN, as depicted in Figure 6. The pH_ZPC of P – PAN indicated that the surface of the adsorbent was positively charged at pH less than 5 and negatively charged at pH values above 5. At this pH, a significantly high electrostatic attraction phenomenon exists between the negatively charged anionic dye and the positively charged surface of adsorbent, resulting in a higher uptake of EBT dye. For P – PAN, greater adsorption was found under pH 6 and this decreases clearly at pH greater than 6. By comparison, from the results of % adsorption of EBT dye from the two adsorbents, it appears that C – PAN provides a better response than P – PAN.

Figure 5. Effect of pH on % removal of EBT dye onto P – PAN and C – PAN adsorbents. Experimental conditions: C₀ = 60 mg/L, W = 25 mg, pH = 2, V = 50 mL, ambient temperature.

Figure 6. Values of pH_ZPC for P – PAN and C – PAN adsorbents.

3.4. Effect of initial dye concentration

The effect of initial dye concentration depends on the immediate relation between the concentration of the dye and the available sites on an adsorbent surface. The effect of the initial dye concentration was investigated as follows: a 25 mg sample of P – PAN and C – PAN was added to 50 mL solution of EBT dye with initial concentrations varying from 60 to 100 mg/L. Figure 7 shows the effect of initial dye concentration and nature of the adsorbent on the adsorption capacity of EBT dye at pH 2. An increase in initial EBT dye concentration leads to an increase in the adsorption capacity for P – PAN and C – PAN adsorbents. As the initial dye concentration increases from 40 mg/L to 100 mg/L, the adsorption capacity of dye changes from 47.52 to 95.81 mg/g for P – PAN and from 61.14 to 119.3 mg/g for C – PAN. This indicates that the initial dye concentration plays an important role in the adsorption capacity of dye, as described by other research (Regti, Laamari, Stiriba, & El Haddad, 2017). From these results, C – PAN was considered better than P – PAN as an adsorbent.

Figure 7. Effect of Erichrome Black T dye concentrations on dye removal by P – PAN and C – PAN. Experimental conditions: m = 25 mg, pH = 2, V = 50 mL and ambient temperature.

3.5. Kinetic studies

The linearized integral form of the pseudo-first order model is generally expressed as $$\text{log}\left(q_e-\mathrm{ }{q}_t\right)=\text{log}\left(q_e\right)-\frac{k_1}{2.303\mathrm{ }}\mathrm{ }t$$

where q_e and q_t are the adsorption capacities (mg/g) at equilibrium and time t, respectively, and k₁ is the pseudo-first order rate constant (min⁻¹) (Li, Yue, & Gao, 2010).

The calculated equilibrium adsorption capacity q_e (cal) and q_e (exp) values have shown large deviation at various initial EBT dye concentrations onto P – PAN and C – PAN adsorbents (see Table 2). The pseudo-first order kinetic model rate law failed to explain the adsorption of EBT dye onto P – PAN and C – PAN adsorbents, with poor fit at various concentrations.

Table 2. Kinetic parameters for EBT dye removal onto P – PAN and C – PAN adsorbents.

Dye concentration (mg/L)			Pseudo-first order			Pseudo-second order			Elovich model
		qe,exp	qe,cal	k1	R^2	qe,cal	k2	R^2	α	β	R^2
P – PAN	40	47.53	10.96	0.068	0.756	47.62	0.029	0.999	2.95 10^9	0.546	0.943
	60	60.78	11.04	0.069	0.654	61.35	0.027	0.999	3.7 10^11	0.493	0.879
	80	77.34	17.38	0.064	0.656	77.51	0.017	0.999	1.5 10^14	0.481	0.763
	100	95.81	19.05	0.073	0.777	96.15	0.018	0.999	3.9710^12	0.345	0.902
C – PAN	40	61.14	26.43	0.073	0.891	62.11	0.01	0.998	7652	0.184	0.949
	60	82.64	59.83	0.074	0.730	84.03	0.0004	0.994	915.7	0.107	0.958
	80	99.92	53.17	0.054	0.902	102.1	0.0003	0.993	1677	0.095	0.876
	100	119.28	54.17	0.054	0.898	120.5	0.0003	0.996	10320	0.094	0.932

The pseudo-second order model is based on the assumption that the rate-limiting step involves chemisorptions (Qin, Ma, & Liu, 2009). The pseudo-second order rate equation is given as $$\frac{t}{q_t}=\mathrm{ }\frac{1}{k_2\mathrm{ }{q}_e^2}+\mathrm{ }\frac{1}{q_e}\mathrm{ }t$$

where q_e is the maximum adsorption capacity (mg/g), k₂ the rate constant of the pseudo-second order equation (g/mg.min) and q_t is the amount of dye adsorbed on adsorbed per unit mass of the adsorbent (mg/g).

The results of the pseudo-second order plot at various initial EBT dye concentrations are given in Table 2. The equilibrium adsorption capacity q_e(cal) and q_e(exp) values are in close agreement at various concentrations. From the results it is clear that the equilibrium capacity increases with increasing initial EBT dye concentration. The adsorption of EBT dye onto P – PAN and C – PAN adsorbents is explained well by the pseudo-second order model kinetics, with a very high correlation coefficient. The uptake of EBT dye indicates that the rate-determining step could be chemisorption in nature (Kadirvelu, Karthika, Vennilamani, & Pattabhi, 2005; Karthikeyan, Rajgopal, & Iranda, 2005). By comparing the adsorption capacity data for P – PAN and C – PAN adsorbents, it appears the C – PAN adsorbent shows better results than those of P – PAN.

The Elovich equation is often used when the adsorbing surface is heterogeneous. The linear form of the Elovich equation is given as described by Elovich: $$q_t=\frac{1}{\beta }\text{ ln }\left(\alpha \mathrm{ }\beta \right)+\frac{1}{\beta }\text{ ln }\left(t\right)$$

where α (mg/g.min) is the initial adsorption rate constant and the parameter β (g/mg) is related to the extent of surface coverage and activation energy for chemisorption. The values of α and β can be calculated from the plot of q_t against ln (t). The values of the constants α and β are given in Table 2. For any adsorbent, values of α and β increase with increasing EBT dye concentration. Despite the fact that the correlation factor is not close to unity, important suggestions can be deduced, like the values of α are much higher for P – PAN than those for C – PAN, suggesting a slow reaction onto P – PAN. Similarly, values of β are higher for P – PAN than those for C – PAN. This is a logical result because the adsorption reaction occurs very slowly. Through this model, we confirm that the adsorption of EBT dye is more favourable onto C – PAN adsorbent than P – PAN adsorbent.

3.6. Adsorption isotherms

The adsorption isotherm is significant for explaining how the adsorbent will interact with the adsorbate, and giving an idea of adsorption capacity. This plays an important role in understanding the mechanism of adsorption. In this study, Langmuir, Freundlich and Tempkin adsorption isotherms were studied.

The Langmuir adsorption model is established on the following hypotheses: uniformly energetic adsorption sites, monolayer coverage, and no lateral interaction between adsorbed molecules (Langmuir, 1918). A mathematical expression of the Langmuir isotherm is given by the following equation: $$\frac{C_e}{q_e}= \frac{1}{q_{m\hspace{0.17em}}{K}_L}+ \frac{1}{q_m} C_e$$

where q_e (mg/g) is the amount of dye adsorbed on the solid adsorbent at equilibrium, q_m (mg/g) is the maximum adsorption capacity, K_L (L/mg) is the Langmuir equilibrium constant, and C_e (mg/L) is the EBT dye concentration at equilibrium. The essential characteristic of the Langmuir isotherm can be expressed by the dimensionless constant called equilibrium parameter, R_L, defined by $$R_L=\mathrm{ }\frac{1}{1+\mathrm{ }{K}_L\mathrm{ }{C}_0}$$

where C₀ is the initial EBT dye concentration (mg/L). Values of R_L indicate the possibility type of the request isotherm which may be $$\text{Irreversible}\text{:} R_L=0;\text{Favorable}\text{:} 0<R_L<1;\text{Linear}\text{:}{R}_L=1;\text{Unfavorable}\text{:} R_L>1.$$

The values of the maximum adsorption capacity q_m and the adsorption constant K_L were obtained by plotting C_e/q_e versus C_e and are presented in Table 3. Firstly, values of R_L are 0.45 and 0.22 for P – PAN and C – PAN, respectively, suggesting the favourable adsorption of EBT dye onto both dyes.

Table 3. Isotherm constants for Eriochrome Black T biosorption onto P – PAN and C – PAN.

Adsorbent	Langmuir			Freundlich			Temkin
	qmax (mg/g)	RL	R^2	Kf	n	R^2	BT	KT	R^2
P – PAN	178.57	0.45	0.853	8.89	1.7	0.965	39.28	0.185	0.919
C – PAN	166.67	0.22	0.978	22.16	2.22	0.996	38.58	0.488	0.976

The Freundlich isotherm endorses the heterogeneity of the surface and assumes that the adsorption occurs at sites with different energy of adsorption. The energy of adsorption varies as a function of surface coverage (Freundlich, 1906). This equation is also applicable to multilayer adsorption and is expressed by the following linear form: $$\log \mathrm{ }\left(q_e\right)=\log \mathrm{ }\left(K_f\right)+\mathrm{ }\frac{1}{n}\mathrm{ log}\mathrm{ }\left(C_e\right)$$

where K_F (L/mg) is the Freundlich constant and n is the heterogeneity factor. The K_F value is related to the adsorption capacity; while the 1/n value is related to the adsorption intensity, values of 1/n indicate the type of isotherm to be Irreversible: 1/n = 0; Favourable: 0 < 1/n < 1; Unfavourable: 1/n > 1.

Therefore, a plot of log (q_e) versus log (C_e) should be a straight line of slope 1/n and intercept log (K_f). Figure 8 shows the plot of Freundlich isotherm for EBT dye onto P – PAN and C – PAN adsorbents, showing an acceptable linearity straight line. Values of n parameter are 1.7 for P – PAN and 2.22 for C – PAN, suggesting values of 1/n comprised between 0 and 1, indicating a favourable adsorption of EBT dye onto both dyes.

Figure 8. Plot Curve of linear equation Freundlich model for the adsorption of EBT dye onto P – PAN and C – PAN adsorbents.

Tempkin considered the effects of some indirect adsorbate/adsorbate interactions on adsorption isotherms and suggested that, because of these interactions, the heat of adsorption of all the molecules in the layer would decrease linearly with coverage. The Tempkin equation is given as described in Tempkin and Pyzhev (1940): $$q_{\mathrm{e}}=B_T\text{Ln }\left(K_T\right)+B_T\mathrm{L}\mathrm{n}\left(C_e\right)$$

where $$B_T=\frac{RT}{b}.$$

A plot of q_e versus ln (C_e) enables the determination of the isotherm constants B_T and K_T from the slope and the intercept, respectively. K_T is the equilibrium binding constant (L/mol) corresponding to the maximum binding energy and constant B_T is related to the heat of adsorption.

The isotherm constants of each model were calculated and presented in Table 3. Examination of the linear isotherm parameters show that the correlation coefficients (R²) obtained from the Freundlich isotherm model were higher in comparison with the other models.

Therefore, the Freundlich equation represents better the adsorption process, which proves that the heterogeneous adsorption surface with sites that have different energies of adsorption as the model assumes.

3.7. Thermodynamic studies

The thermodynamic parameters such as standard enthalpy (ΔH⁰), the standard entropy (ΔS⁰) and free standard energy (ΔG⁰) have been calculated using the following equations: $$\Delta G^0=-RT\text{ ln }\left(K_C\right)$$

$$\Delta G^0=\Delta H^0-T\mathrm{ }\Delta S^0$$$$\text{ln }\left(K_C\right)=\frac{\Delta S^0}{R}-\frac{\Delta H^0}{RT}$$

where R is the universal gas constant (8.314 J/mol K), T is the temperature (K) and K_C is the distribution coefficient of EBT dye for adsorption mechanism. The parameter K_C can be calculated using the following equation as described in Han et al. (2006): $$K_C=\mathrm{ }\frac{q_e}{C_e}$$

where C_e is the equilibrium EBT dye concentration on the adsorbent (mg/L) and q_e is the solid phase concentration (mg/g).

The values of ΔH⁰ and ΔS⁰ were calculated from the slope of the linear plot of ln (K_C) versus 1/T (see Figure 9) and the free energy change ΔG⁰ was calculated at different temperatures and is given in Table 4. We consider firstly the adsorption of EBT dye onto P – PAN adsorbent; the negative values of ΔG⁰ have decreased from –2.72 to –7.48 kJ/mol with increases in temperature from 298 K to 328 K. This behaviour indicates the spontaneous nature of adsorption favourable at higher temperatures. On the other hand, the positive value of ΔH⁰ (44.514 kJ/mol) suggests that the process was endothermic in nature, and the positive value of ΔS⁰ (158.51 J/mol K) indicates that the entropy of the system increased during the adsorption.

Figure 9. Van’t Hoff plot for the adsorption of EBT dye onto P – PAN and C – PAN adsorbents.

Table 4. Thermodynamic parameters for the adsorption of EBT dye onto P – PAN and C – PAN adsorbents.

Adsorbent	Temperature (K)	ΔG^0 (kJ/mol)	ΔH^0 (kJ/mol)	ΔS^0 (J/mol K)
P – PAN	298	−2.722	44.514	158.51
	308	−4.307
	318	−5.892
	328	−7.477
C – PAN	298	−3.435	−10.087	−22.32
	308	−3.212
	318	−2.989
	328	−2.766

Secondly, in the adsorption of EBT dye onto C – PAN adsorbent, the increased values of ΔG⁰ from –3.43 kJ/mol to –2.76 kJ/mol with the increasing temperature from 298 to 328 K indicate a decrease in feasibility of adsorption at higher temperatures. The negative value ΔH⁰ –10.087 kJ/mol shows that the adsorption is exothermic in nature. The negative value of change of entropy ΔS⁰ –22.32 J/mol K suggests that the adsorption onto C – PAN adsorbent occurs by a decreasing randomness at the solid/liquid interface.

3.7. Comparison study

Table 5 depicts some results of the uptake of EBT dye onto some adsorbents cited in the literature. The comparison shows that C – PAN adsorbent gives a better adsorption capacity, and it is above 120 mg/g.

Table 5. Comparison of adsorption capacity of the uptake EBT dye onto other adsorbents.

Adsorbent	Adsorption capacity (mg/g)	Reference
Peanut shell	40.81	Boumchita et al. (2017)
Bottom ash	89.90	Mittal and Gupta (2010)
NiFe2O4 magnetic nanoparticles	47.00	Moeinpour, Alimoradi, & Kazemi (2014)
Acid-Modified Graphene	102.04	Arsalan and Mukarram (2018)
C – PAN	120.50	This study

3.8. Regeneration and reusability of P – PAN and C – PAN adsorbents

The economic and environmental aspects of the use of adsorbent materials make their re-use important. Figure 10 displays the difference in percent removal of first and fifth cycles. The adsorption efficiency was reduced from 51% to 35% for P – PAN adsorbent, and from 69% to 38% for C – PAN adsorbent. This result can be explained by the reduction in the specific surface of this material following the heat treatment carried out.

Figure 10. Reusability of P – PAN and C – PAN adsorbents. Experimental conditions: C₀ = 60 mg/L, m = 25 mg, pH =2, V = 50 mL, ambient temperature.

5. Conclusion

In this study, we have achieved the removal of EBT from aqueous solutions onto P – PAN and C – PAN as adsorbents. The best adsorption capacity was found with C – PAN at different concentrations, and showed that for the removal of EBT dye C – PAN acts as a better adsorbent than P – PAN. The equilibrium adsorption data obtained at different concentrations fitted well with the requirements of the Freundlich isotherm model, indicating multilayer adsorption on a heterogeneous surface. Kinetic studies show that the EBT adsorption demonstrates pseudo-second order chemical reaction kinetics.

The adsorption of the dye on modified P – PAN is spontaneous and exothermic, as evidenced by negative values of the changes in free energy and enthalpy, while the adsorption at P – PAN is spontaneous and endothermic as indicated by the negative values of the changes in free energy and positive values of enthalpy.

Disclosure statement

No potential conflict of interest was reported by the authors.