Hydrothermally Treated Banana Empty Fruit Bunch Fiber Activated Carbon for Pb(II) and Zn(II) Removal
Ganiyu Abimbola Adebisi, Zaira Zaman Chowdhury,* Sharifah Bee Abd Hamid, and Eaqub Ali
Activated carbon was produced by chemical activation of hydrothermally carbonized (HTC) banana empty fruit bunch (BEFB), using phosphoric acid (H3PO4) as the activating agent. The activation process was optimized using a Box-Behnken factorial design (BBD), with an outcome of 17 different experiments under the predefined conditions. Three different parameters (activation temperature (x1), activation time (x2), and the concentration of activating acid (x3)) were analyzed with respect to their influence on maximum adsorption percentage for divalent cations, Pb(II) (Y1) and Zn(II) (Y2), and carbon yield (Y3). All process parameters had strong positive effects on adsorption capacity up to a certain limit. The specific surface area of the hydrochar (HTC) was enhanced substantially after the activation process. Scanning electron microscopy (SEM) revealed that the morphology of the BEFB-based char changed noticeably after the acid impregnation and activation process. The Langmuir maximum monolayer adsorption capacity for Pb (II) and Zn (II) cations was 74.62 mg/g and 77.51 mg/g, respectively. Equilibrium isotherm data were in agreement with the Langmuir model. Thermodynamic characterization revealed that the equilibrium system was endothermic and spontaneous.
Keywords: Hydrothermal carbonization (HTC); Langmuir monolayer adsorption capacity; Box-Behnken Design (BBD); Hydrochar; Isotherm Model; Thermodynamics
Contact information: Nanotechnology & Catalysis Research Centre (NANOCAT), University of Malaya, Institute of Post Graduate Studies, 50603 Kuala Lumpur, Malaysia;
* Corresponding authors: email@example.com; firstname.lastname@example.org
The global demand for activated carbon (AC) has prompted research investigating new precursors and production methods to obtain micro- and nano-structured carbon for versatile applications. The AC is manufactured by chemical or physical activation methods; frequently, lignocellulosic biomass residues are the starting materials (Chowdhury et al. 2013). During physical activation, the biomass sample is first pyrolyzed (> 500 °C) and treated with an activating agent (air, carbon dioxide, and water or steam) at a high temperature (700 to 900 °C). For chemical activation, the residues are impregnated with chemicals and then pyrolyzed at moderate to high temperatures. Overall, the process can be made more energy-efficient by modifying the carbonization step, which decreases the production costs (Roman et al. 2013). The combination of hydrothermal and chemical activation methods functionalizes the carbon with tunable surface chemistry (Roman et al. 2013).
A hydrothermal carbonization technique (HTC) has been used to produce carbonaceous char (Titirici et al. 2007a; Sevilla and Fuertes 2009). During hydrothermal pretreatment, a lignocellulosic residue is carbonized under a mild temperature range (150 to 250 °C) and self-generated pressures using deionized water as the “green” solvent. The HTC process is very popular because of its simplicity in design, cost savings, and energy efficiency. Furthermore, it is a “green method,” as it does not employ organic solvents, corrosive catalysts, or surfactants (Titirici et al. 2007b). During hydrothermal carbonization, linkages between the carbohydrate-rich fractions, i.e., cellulose and hemicellulose, are broken and dissolved in water. Consequently, a complex aldol reaction, cycloaddition, and condensation process yield carbonaceous hydrochar. The liquid phase contains some sugars or lignin-based oligomers, which can be used to extract value-added products including bioplastics and biofuels. Overall, the process is energy efficient and uses milder conditions than classical pyrolysis. Moreover, it does not require drying of the raw biomass, and the process is exothermic, releasing heat that contributes one-third of the energy needed for the complete carbonization process (Roman et al. 2013). In addition, the process does not produce toxic gases and tar-like pyrolysis (Xiu et al. 2010). Hydrothermal carbonization of biomass can provide a new type of starting material to produce activated carbon. HTC char is chemically similar to peat and lignite and can be further transformed to functional activated carbon (Hao et al. 2014). HTC char has good self-binding properties, which is advantageous for pelletisation (Amaya et al. 2007). Finally, the HTC process does not require gas flow, making it economically feasible, and most of the generated carbon is confined to the carbonaceous hydrochar (Amaaya et al. 2007). Hydrochar prepared from biomass residues has certain porosity, with special morphological features like nano-spheres or nano-fibers (Titirici et al. 2008). Its surface functional groups are hydrophilic. Thus, hydrochar can be the precursor to activated carbon with the appropriate surface chemistry to adsorb heavy metals from water. The activation of HTC materials with different activating agents and the physiochemical characteristics of the porous activated carbon have not been thoroughly studied. HTC contains a cross-linked polyfuranic structure, and the connections between the furan rings are composed of an aliphatic chain with oxygen groups. A small fraction of aromatic arene-like structures are observed after processing the biomass at 180 °C. With increasing temperature, the aromaticity increases, but the aliphatic and oxygen-containing groups decrease (Falco et al. 2013). This effect was attributed to oxygenated linking groups inside the final carbon matrix, which contains many reactive functional groups and hydrophilic structures than the pyrolyzed material.
In this report, hydrochar prepared from banana empty fruit bunch (BEFB) was used to prepare activated carbon for the removal of Pb(II) and Zn(II) cations from wastewater. The activation parameters were optimized with a 3-level factorial design based on Box-Behnken (BBD) modeling, which concurrently investigates the interdependence of several factors (Baskan and Pala 2010). The experimental variables are typically varied between two levels. This approach is systematic and describes nonlinear dependencies for a particular variable and interactions between variables. Compared with other response surface designs, BBD is slightly more efficient than the central composite design but much more efficient than the three-level full factorial designs (Ferreira et al. 2007). In this research, BBD design was applied to the parameters of temperature, time, and H3PO4 acid concentration for the activation of HTC obtained from BEFB. The resultant AC was used to absorb Pb(II) and Zn(II) from wastewater. The experimental data was analyzed using Langmuir, Freundlich, and Temkin Isotherm models. Thermodynamic characterization of the system determined the Gibb’s Free energy (∆G°), enthalpy (∆H°), and entropy (∆S°) values.
Preparation of feedstock (BEFB)
Banana empty fruit bunch (BEFB; Bangladesh Scientific Institute of Research (BCSIR), Dhaka, Bangladesh) was used as the primary biomass feedstock. BEFB sample was vigorously washed with hot deionized water to remove dust and dried in an oven at 80 °C for 24 h. To promote effective homogeneous mixing and stirring, the sample was crushed using a ball mill. The powdered sample was sieved to remove large particles, washed, dried, and stored in a sealed container for further processing.
Preparation of hydrochar (BEFBC)
To prepare hydrochar, 5.0 g of residues was mixed with 50 mL of deionized water and stirred until it was homogeneously mixed. The sample was transferred into a Teflon-lined autoclave (100 mL) and carbonized for 12 h at 220 °C. The resulting char sample (BEFBC) was washed several times with deionized water until a neutral pH was obtained. The obtained BEFBC was not initially activated and was stored in air-tight containers for preliminary characterization studies.
Preparation of activated carbon (BEFBAC)
BEFBC (20 g) was impregnated with H3PO4 (100 mL, variable concentration) at 90 to 100 °C for 4 h. The sample was dried completely overnight at 90 °C. The dried sample was further pyrolyzed to enhance the surface area of the final product. The secondary stage of pyrolysis was carried out in the presence of nitrogen gas flow at varying temperatures, based on the basic design matrix (Tables 1 and 2).
Table 1. Independent Variables for Box Behnken Design
The activated carbon samples (BEFBAC) were washed vigorously to remove unreacted acid. The final samples were dried and stored for further characterization.
Isotherm and thermodynamic characterization for the single solute system
Pb(II) and Zn(II) ions were prepared by dissolving Pb(NO3)2.2H2O or ZnCl2·2H2O salts in de-ionized water to a final concentration of 1000 mg/L. A batch adsorption test was carried out by varying the concentration from 150, 200, 250, 300 and 350 mg/L, where the concentration gap was kept at 50 mg/L for each sample. The stock solution was further diluted to obtain the required concentration for isotherm studies. To calculate the removal percentage, the highest solution concentration of 350 mg/L was used. Adsorption experiments were carried out at 30, 60, and 80 °C for thermodynamic characterization of the equilibrium system. The loading of Pb(II) and Zn(II) ions onto the BEFBAC was calculated using Eq. 1 (Chowdhury et al. 2011a, 2014),
where qe represents the amount of ion adsorbed at equilibrium (mg/g), C0 is the initial concentration of the targeted cation (mg/L), Ce is the liquid-phase concentrations of metal ions at equilibrium conditions (mg/L), V is the volume of the single solute solution (L), and W is the mass of BEFBAC used (g). For calculating the removal percentages at different experimental conditions (Table 2), the following equation was used:
The RSM technique was used to examine the impact of the major operating factors on Pb(II) and Zn(II) cation removal. The number of experiments (N) required for the BBD design is expressed by Eq. 3,
N = 2k (k − 1) + C0 (3)
where k is number of factors and Co is the number of central points. The method is less time consuming as a lower number of experimental runs is needed, when k is not too large (Ferreira et al. 2007). The Box Behnken Design (BBD) with three factors, including five replicates at the center point for appraisal of errors, was used to estimate the main and interaction effects of the variables and to develop a second-order polynomial model with linear, interaction, and quadratic terms. For equilibrium adsorption studies, three important effective parameters—temperature (x1), time (x2), and activating agent concentration (x3)—were the independent variables, while Pb(II) removal (Y1), Zn(II) (Y2) removal, and carbon yield (Y3) were the response variables (dependent variables). The variations were as follows: temperature, 500 to 800 °C; time, 1 to 3 h; and concentration of acid, 25 to 50%. The low, middle, and high levels of each variable were indicated as -1, 0, and +1, respectively. The order of the experimental runs was randomized, and the responses were used to develop empirical models using a second-degree polynomial equation (Gunaraj and Murugan 1999) Eq. 4,
where Y is the predicted response, b0 is the constant coefficient, bi is the linear coefficient, bij isthe interaction coefficients, bii is the quadratic coefficient, and xi, and xj are the coded values of adsorption. For the three variables, the suggested number of experiments at the center point was five, and the total number of experiments (N) required was 17 (Table 2). Table 2 summarizes the coded and actual levels of the three independent variables together with the responses obtained from the BBD experimental run represented by the design matrix.
Surface morphological changes in the BEFB, BEFBC, and BEFBAC were characterized using field emission scanning electron microscopy (FE-SEM; model SUPRA 35VP, Zeiss, Germany, UK). The Brunauer-Emmett-Teller (BET) surface area, micropore volume, mesopore volume, and pore size distribution of the samples were analyzed using a TriStar II BET Surface Area Analyzer (Micromeritics, USA). Prior to the nitrogen gas adsorption procedure, the samples were outgassed under a vacuum at 300 °C for 4 h to remove excess moisture content. The surface area and pore diameter were calculated using the BET method, whereas the micropore volume was obtained through the t-plot method (Storck et al. 1998). Carbon, hydrogen, and nitrogen contents were determined using an Elemental Analyzer (Series II 2400, PerkinElmer Inc., Japan).
RESULTS AND DISCUSSION
Development of the Regression Model
Linear, interactive, quadratic, and cubic functions were applied to the analytical data for ion removal and yield to develop regression equations. To check the adequacy of the models, three different tests were used: sequential model sum of squares, lack of fit, and model summary statistics. A cubic model was not suggested for the removal percentage and yield because of insufficient points for the calculation of the coefficients. Based on the sequential model sum of the squares and model summary statistics models, the quadratic model showed the best fit with the experimental data, having the lowest standard deviation and the highest correlation coefficient and adjusted R2 values, including the lowest P-value for Pb(II) and Zn(II) removal. A linear model was chosen for the carbon yield calculation. The experimental data were used for developing the models shown in Eqs. 5 through 7.
The coefficients containing independent variables of temperature (x1), time (x2), and concentration of H3PO4 acid (x3) denote the effects of the individual parameters on the response variables of Pb(II) removal (Y1), Zn(II) removal (Y2), and carbon yield (Y3). Multiplication values between the two factors and others with second order terms exhibited the interaction and quadratic effect, respectively (Chowdhury et al. 2011b; Arami-Niya et al. 2012). A positive sign in front of the constant terms indicates a synergistic effect, whereas a negative sign indicates an antagonistic effect (Montgomery 2001). Figures 1(a), 1(b), and 1(c) show the experimental data versus the predicted values. The high values of the regression coefficient for all response variables indicated that the model predictions fit reasonably well with the experimental observations (Table 3).
Table 2. Experimental Responses from the Preparation of Banana Empty Fruit Bunch Activated Carbon (BEFBAC)
|Sample ID||Run||Type of Point||Reaction Variables
Fig. 1. Predicted versus actual (a) % removal, of Pb (II), Y1 (b) % removal of Zn(II), Y2 and (c) % yield of BEFBAC, Y3
For further assessment, studentized residuals were plotted versus experimental runs for all of the responses. The experimental points for residuals were randomly scattered around zero (Fig. 2). Most of the standard residuals fell within the interval range of ± 3.00, which indicated that no response transformation was needed for the experimental design.
Fig. 2. Studentized residuals versus experimental run (a) % removal, of Pb(II), Y1 (b) % removal of Zn(II), Y2 and (c) % yield of BEFBAC, Y3
Standard deviation was calculated to validate the quality of the models (Table 3). The experimental R2 values were in reasonable agreement with the adjusted R2. The values obtained for the coefficient of variation (CV) and standard deviation were small, suggesting reproducibility of the developed models. The values of adequate precision were calculated based on the signal-to-noise ratio. For effective model simulation, adequate precision should be greater than 4; the adequate precision observed for Pb(II) removal, Zn(II) removal, and carbon yield were 18.49, 22.81, and 26.65, respectively. Thus, the experimental data was statistically significant to confirm the experimental layout of the design.
Table 3. Statistical Parameters for Model Verification
Statistical analysis for the developed models for all three responses was analyzed using analysis of variance (ANOVA). The analysis results are summarized in Tables 4, 5, and 6.
Table 4. Analysis of Variance (ANOVA) and Lack of Fit Test for the Removal of Pb(II) from BEFBAC (Y1)
Based on model F-values, it can be concluded that temperature (x1) had the greatest influence on the response of removal percentage of Pb(II) cations, Y1, time (x2), and ratio (x3) had moderate influences on the removal percentage (Table 4). However, between time and H3PO4concentration, the concentration of H3PO4 acid played vital role to enhance the quality of the prepared activated carbon. The interaction influences of temperature and time (x1x2) was more prominent than the other interaction factor associated with the percentage removal of Pb(II) cation, Y1. In this case, x1, x3, the quadratic terms of x12, x22, x32 including interaction terms of x1x2 are significant model terms (Table 4).
Table 5. Analysis of Variance (ANOVA) and Lack of Fit test for the Removal of Zn(II) from BEFBAC (Y2)
For Zn(II) removal percentage, Y2, temperature (x1) and time (x2) had larger influence than ratio (x3), whereas the cumulative effect of temperature and ratio (x1x3) had greatest impact on removal percentages. In this case, x1, x2, x3, the quadratic terms of x12, x22, x32 including interaction terms of x1x2 and x1x3 were significant model terms (Table 5)
For yield percentage (Y3), x1, x2 and x3 were significant model terms. Table 6 reveals that temperature (x1) and H3PO4 acid concentration (x3) had more dominating effect for yield calculation. The F-test values representing the variation in the data about the mean were determined to check the competence of the models. Based on a 95% confidence interval, the model F-values for Pb(II) removal, Zn(II) removal, and carbon yield were 33.54, 64.87, and 73.52, respectively, which implied that these models were significant. However, the P-values for all three responses were less than 0.05, which indicated that the model terms considered for the response analysis were significant.
Table 6. Analysis of Variance (ANOVA) and Lack of Fit test for the Percent Yield of BEFBAC (Y3)
Effect of Process Parameters on Removal Percentages
Figure 3(a) demonstrates the three-dimensional response surface plots of the collective impact of temperature (x1) and time (x2) on the removal of Pb(II) cations (Y1) by BEFBAC, when the H3PO4 concentration (x3) was fixed at the center point (37.50%). Figure 3(b) displays the influence of temperature (x1) and H3PO4 acid concentration (x3) on the removal of Pb(II) cations, when the activation time for the hydrochar BEFBC was kept at the center point (2 h). Figures 4(a) and 4(b) are constructed to reveal the interaction of temperature and time or temperature and concentration on the removal of Zn(II) cations (Y2) by BEFBAC. In both cases, the third variable was fixed at the center point.
Fig. 3. Three dimensional response surface contour plots of the combined effects of (a) temperature (x1) and time (x2) and (b) temperature (x1) and H3PO4 acid concentration (x3) on the percent removal of Pb(II) cations by BEFBAC (Y1), when the third variable was fixed at the center point
Fig. 4. Three-dimensional response surface contour plots of the combined effects of (a) temperature (x1) and time (x2) and (b) temperature (x1) and H3PO4 acid concentration (x3) on the percent removal of Zn(II) cations by BEFBAC (Y2), when the third variable was fixed at the center point
The curvature observed in Figs. 3 and 4 represents the prominent effect of the activation temperature on the removal of both cations, irrespective of the time and concentration of H3PO4. The plots revealed that the temperature and concentration of the impregnating acid was proportional to the percentage removal. Up to a certain limit, increasing of temperature and acid concentration enhanced the reaction, resulting in more surface area with a porous texture, which is desirable for adsorption. ANOVA also showed that the activation temperature had the highest impact on ion removal. In previous studies, the activation time exhibited a moderate to minimal impact on the development of the surface area and pore structure of the activated carbon prepared from cassava peel, whereas the pore distribution in terms of micropore and mesopore percentages were strongly influenced by the activating KOH impregnation ratio and the temperature (Sudaryanto et al. 2006). A short activation time and very low temperature might not be sufficient to enhance the surface area (Cao et al. 2006). After a certain limit, increasing the temperature and concentration both exhibited a detrimental effect on the percentage removal; high temperature or acid concentration might destroy some surface functional groups. In addition, these conditions might compromise the integrity of the porous texture of AC by thermal annealing, which destroys the walls of the micropores to form more mesopores, which are suitable for liquid phase adsorption. However, in that case, the pore size distribution is not suitable, because larger mesopores fail to adsorb and retain smaller cations, resulting in lower removal efficiency (Chowdhury et al. 2012). At very high temperatures and longer residence times with highly concentrated acid, the carbon skeleton might burn into ash, which also compromises removal efficiency. A very long activation time is not beneficial, as it increases the liquid yield and reduces the carbon yield, with successive decreases in the removal efficiency. This trend was also observed during the preparation of activated carbon from oil palm fronds for the removal of Zn(II) cations (Zahangir et al. 2008).
Effect of Process Parameters on Carbon Yield
Figure 5a reveals the cumulative influence of two independent factors, temperature and time, on percentage yield of carbon when the H3PO4 concentration was fixed at the center point (37.50%). Figure 5b shows the combined impact of temperature and H3PO4 concentration over yield percentage, where time was kept at the center point of 2 h. All three parameters exhibited a synergistic effect on percentage yield.
In general, the yield decreased with increasing temperature, time, and acid concentration. Temperature had the highest impact on the yield percentage, which was earlier shown by the highest F-value of 684.69 (Table 6), whereas the activation time was not as noteworthy compared to the temperature and acid concentration. Temperature was the dominant factor relative to the yield, as supported by the ANOVA data (Table 6). The lowest yield was obtained at 800 °C for 3 h with 37.50% acid (Sample B-11, Table 2). With increased temperature, the contact time and concentration intensified the diffusion of acidic solution inside the hydrochar matrix, leading to conversion of carbon to ash. This effect initiated the disintegration of the crystalline region of hydrochar and formed amorphous carbon, which is desirable for adsorbent preparation. Thus, the optimum reaction condition should be determined to enhance the surface area of the carbon sample with the highest possible yield. Consequently, the removal efficiency would also be higher.
This observation is consistent with the previous work on cassava peel (Sudaryanto et al. 2006), where activation temperature was the most important factor, role, and activation time had the least impact on the carbon yield. Increasing the temperature beyond a certain point enhanced dehydration and elimination reactions to release additional volatile organic fractions from the hydrochar matrix as gaseous and aqueous products, rather than as solid activated carbon.
Fig. 5. Three-dimensional response surface contour plots of the combined effects of (a) temperature (x1) and time (x2) and (b) temperature (x1) and H3PO4 acid concentration (x3) on the percent yield of BEFBAC (Y2), when the third variable was fixed at the center point
Model Validation and Confirmation
For the robustness of experimental design to manufacture carbon, relatively high removal efficiencies, along with satisfactory carbon yields were expected for targeting pollutants under optimum conditions. When the independent variables of temperature, time, and acid concentration were increased, the percentage removal increased up to a certain point, whereas the yield decreased. The converse effects were also observed. To optimize the char activation process, maximum values for removal were set as the targets, while the three variables (temperature, time, and acid concentration) were set within the studied ranges. A 1.0-g sample was used as the input for each parameter to control the desirability function (Amini et al. 2008). The desirability function for optimization and error percentage were estimated (Table 7).
The obtained hydrochar was brown in color and consistent with partially carbonized products. SEM images of the raw lignocellulosic residues (BEFB) showed a smooth, nonporous texture without cracks (Fig. 6a), but after carbonization (BEFBC and BEFBAC), there were substantial changes in the surface morphology and texture. Many sphere-like microparticles were deposited over the larger particles (BEFBC). Cellulose and hemicellulose were degraded during hydrothermal carbonization, producing carbon microspheres (Liu and Guo 2015). However, the more chemically stable non-saccharide components of biomass (lignin) were only partially degraded, which preserved the original skeleton of the particles (Sevilla and Fuertes 2009; Gao et al. 2012; Falco et al. 2013). After activation, BEFBAC particle surfaces were characterized by large conchoidal cavities with smooth surface structures (Fig. 6c). Thus, acid activation caused drastic morphological changes, as previously reported for eucalyptus wood-based hydrochar (Sevilla and Fuertes 2011).
Table 7. Process Parameter Optimization for BEFBAC
The XRD patterns of BEFB, along with hydrochar (BEFBC) and activated carbon (BEFBAC), obtained in the 2θ range of 10 to 35° are shown in Fig. 7. Sharp peaks were observed around 16° and 22° for the original biomass (BEFB) and hydrochar (BEFBC), indicating crystalline regions of cellulose (Keiluweit et al. 2010). The biomass and the hydrochar samples showed similar XRD patterns, reflecting that the hydrothermal carbonization did not disrupt crystalline cellulose.
After activation, the peak intensity became lower and broader, reflecting a decrease in crystallinity. Therefore, the carbon content present in hydrochar-based activated carbon (BEFBAC) was mainly amorphous in texture. This result was expected, as amorphous materials show better absorbance due to their high surface area and greater number of active sites (Tchomgui-Kamga et al. 2010). Previous findings also demonstrated the presence of amorphous carbon in coconut coir-based activated carbon (Sharma and Gode 2010).
Fig. 7. XRD pattern of banana empty fruit bunch (BEFB), hydrochar (BEFBC), and hydrochar activated carbon (BEFBAC)
The texture of hydrochar (BEFBC) and hydrochar carbon (BEFBAC) were analyzed by means of nitrogen physi-sorption (Table 8). The BEFBC sample exhibited less surface area with poor porosity, which was attributed to incomplete carbonization. Thus, the obtained hydrochar material obtained virtually no framework of confined pores. Its surface area arises only from inter-particle voids (Sun et al. 2015).
The biomass type and temperature play a vital role in hydrochar surface area by controlling the amount of pores by cracking the basal structural sheets of hydrochar (Novak et al. 2009; Mumme et al. 2011). After chemical activation with H3PO4, the surface area and pore volume increased substantially. The reaction between H3PO4 and hydrochar structural compounds led to further depolymerization, which enhanced pore volume (Fernandez et al. 2015).
Table 8. Physico-Chemical Characteristics of BEFBC and Activated BEFBAC
Table 9 lists the ultimate analysis of biomass, hydrochar, and hydrochar activated carbon. After hydrothermal carbonization, the carbon content of the char increased, whereas the hydrogen and oxygen contents decreased (Saqib et al. 2015). After activation, the carbon content increased substantially. Both the H/C and O/C ratios decreased after carbonization and activation. The H/C ratio decreased due to aromatization that occurred during hydrothermal carbonization. The O/C ratio decreased as a result of decarboxylation, whereas both the H/C and O/C ratios decreased via dehydration (Liu and Guo 2015).
Table 9. Ultimate Analysis of BEFB, BEFBC, and BEFBAC
Equilibrium Isotherm Studies
Isotherm parameters were evaluated using three types of linear model equations, namely Langmuir, Freundlich, and Temkin. Results are listed in Table 11. Maximum monolayer adsorption capacity, qm (mg/g), and Langmuir’s constant, KL (L/mg), demonstrated the binding energy for adsorption uptake under optimum conditions, as determined from Langmuir’s model in Eq. 8 (Langmuir 1918):
Equation 8 was linearized to give Eq. 9:
The dimensionless factor, RL, of the Langmuir’s model can be calculated using Eq. 10:
RL values were calculated for the highest initial concentration (350 mg/L). The separation factor, RL, was determined to elucidate the types of isotherms (Table 10; Chowdhury et al. 2015).
Table 10. Types of Isotherms Based on the Separation Factor, RL
The surface heterogeneity, to show the multilayer adsorption properties of BEFBAC, can be observed using Freundlich’s isotherm. The empirical equation shows that the reactive sites over the carbon sample are scattered exponentially with the heat of the adsorption process (Freundlich 1906). The nonlinear form of Freundlich’s equation is given by:
The above equation was linearized to determine the parameters (Eq. 11),
where Kf is the affinity factor of the cations towards the carbon sample (BEFBAC) (mg/g) and 1/n represents the intensity of the adsorption.
The equilibrium data were further analyzed by the Temkin isotherm and are
expressed by Eq. (13) (Temkin and Pyzhev 1940):
Equation 13 can be linearized as,
where RT/b = B denotes the Temkin constant (J/mol), which depicts the heat of the sorption process, whereas KT reflects the equilibrium binding constant (L/g), R is the universal gas constant (8.314 J/mol·K), and T° is the absolute solution temperature (K) (Temkin and Pyzhev 1940).
Table 11. Langmuir, Freundlich, and Temkin Model Parameters at Different Temperatures
In this work, relatively better linearity for the Langmuir model was observed for Pb(II) and Zn(II) cations at temperatures of 30, 60, and 80 °C. The Langmuir separation factor, RL, and the Freundlich exponent, 1/n, were below 1.0 percent for all the temperatures, suggesting a favorable adsorption processes. Similar observations for RL and 1/n were reported for Mn(II) sorption onto raw- and acid-treated corncob biomass and mangostene fruit peel-based activated carbon (Abideen et al. 2011; Chowdhury et al. 2014).
The thermodynamic characterization of the equilibrium system provides the values of Gibbs free energy (∆G°), enthalpy (∆H°), and entropy (∆S°) of the sorption process. The following linear equations were used to interpret the equilibrium data (Chowdhury et al. 2011a),
where the constant, KL was determined from the Langmuir equation at three different temperatures (L/mg; Table 11), R is the universal gas constant (8.314 J/mol·K), and T is the absolute temperature (K) (Ahmad 2006).
The thermodynamic parameters Gibbs free energy (∆G°), enthalpy (∆H°), and entropy (∆S°) were calculated (Table 12). The enthalpy (∆H°) calculated for both the cations showed a positive magnitude, indicating that the process was endothermic (Chowdhury et al. 2014). Thus, the removal of both cations was improved by increased temperature.
A positive value of entropy (∆S°) reflected an increase in the degrees of freedom for the equilibrium system. Similar phenomena were reported for the removal of divalent lead cations from synthetic water using activated palm ash residues (Chowdhury et al. 2011a). The Gibbs free energy change (∆G°) estimated for all of the temperatures was negative, indicating the feasible and spontaneous nature of sorption (Chowdhury et al. 2011c, d).
Table 12. Thermodynamic Parameters of Pb(II) and Zn(II) Sorption by BEFBAC
- AC preparation factors were optimized using response surface methodology based on a Box Behnken Design. The activation temperature, time, and concentration of acid substantially influenced each response variable.
- Model validation was conducted under optimum conditions. The developed models were significant enough to calculate the values of the responses reasonably well. The deviation errors between the predicted and experimental results for Pb(II) removal, Zn(II) removal, and AC yield were 5.68%, 5.38%, and 3.16%, respectively.
- The surface area and carbon content of the prepared hydrochar were enhanced by activation
- The equilibrium data and linear regression analysis at room temperature using Langmuir, Freundlich, and Temkin isotherms exhibited a maximum monolayer sorption capacity of 74.62 mg/g and 77.51 mg/g for Pb(II) and Zn(II) cations, respectively.
- Equilibrium thermodynamic studies showed that the process was endothermic, spontaneous, and feasible for the temperature ranges investigated.
The authors thank the University of Malaya for financial support (HIR grant H-21001-F0032) andBKP (BK054-2015).
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Article submitted: October 19, 2015; Peer review completed: March 30, 2016; Revised version received and accepted: May 4, 2016; Published: September 28, 2016.