Kinetics, Thermodynamics, and Isotherms of Methylene Blue Adsorption Study onto Cassava Stem Activated Carbon

: Water treatment using activated carbon is widely accepted, despite its high production cost. Therefore, this study was aimed to investigate the potential of cassava stem in activated carbon form for methylene blue (MB) dye uptake from water. Raw cassava stem (RCS) was also utilized to evaluate the difference between cassava stem in its raw form and after being converted to the activated carbon (ACS). The MB adsorption from water using the RCS and ACS was done in this study. The batch adsorption study showed fast MB uptake by ACS at 60 min contact time, while higher adsorbent dosage and higher pH contributed to higher adsorption percentage. The thermodynamic study showed positive values of ∆ H ◦ of ACS, indicating that the adsorption process of MB was endothermic. Meanwhile, the negative value of ∆ G ◦ showed that the adsorption processes of MB were spontaneous. The thermodynamic study showed higher ﬁtting to Langmuir isotherm, with data from the kinetic study showing better pseudo-second-order equation ﬁtting, which suggests the chemisorption process had happened. The highest adsorption recorded by ACS was 384.61 mg/g, indicating the possibility of cassava stem as the lower cost raw material for activated carbon production with excellent adsorption characteristics.


Introduction
Water pollution is considered a severe environmental issue that is harmful to all living things. Thus, numerous techniques have been discovered in order to clean the water from many types of dangerous pollutants. These techniques include reverse osmosis, ion exchange, dialysis or electrodialysis, cementation, electrolyte extraction, oxidationreduction, solvent extraction, evaporation, adsorption, dilution, filtration, and chemical precipitation. Among these techniques, adsorption has been widely practice [1]. Due to several advantages, such as low initial cost, non-complex design, less sensitivity to toxic substances, and ease of operation, the adsorption process was commonly adopted, considering its versatility and high cleaning effectiveness [2]. Focusing on the adsorption technique, the activated carbon has been widely used as the primary adsorption material (adsorbents) for the removal of a wide range of contaminants in liquid and gas phase application. Activated carbon is a useful material that contains a large surface area due to the high porosity level [3]. The increased production cost for producing activated carbon, however, is the main challenge. Researchers have started to find other lower-cost substitutes as precursors or raw materials to overcome this problem.
Biomass wastes, such as food and crops of the agricultural sector, agricultural crop by-products [4], wood industries wastes and residues [5], aquatic plants [6], animal byproducts and wastes [7], municipal wastes [8], and other unwanted materials, have been

Materials Preparation
The cassava stem was obtained from a local farmer in Raub, Pahang, Malaysia. Methylene Blue powder (C 16 H 18 ClN 3 S·xH 2 O) of analytical grade was acquired from Sigma-Aldrich, Selangor, Malaysia. The freshly obtained raw cassava stem (RCS) was cut into a smaller size, each around 1 cm to 2 cm, prior to drying in a convection oven (MEMMERT UN160) at 80 • C ± 3 overnight. The core part of the cassava stem was removed to ensure a homogenous sample part was used for the evaluation. The sample was ground, sieved, and passed through a mesh with a 500-µm to 1-mm size sieve. A portion of the RCS particles was used as control adsorbents in their natural form, while the others were used as the precursor of the activated carbon production. The RCS particles were placed inside a graphite reactor and tightly closed with a lid to minimize ash formation before being heated in a furnace with a temperature set at 787 • C for 146 min, based on the optimum condition found by the previous work by Sulaiman, Hashim, Mohamad Amini, Danish, and Sulaiman [26]. The produced activated carbon (AC) was cooled to room temperature and stored in closed containers for further use. The adsorbate preparation was completed by making 1000 mg/L MB dye stock solution by dissolving 1g of MB powder in a 1000 mL volumetric flask filled with distilled water. Serial dilution was made to prepare 100, 200, 300, and 400 mg/L stock solution, respectively. The absorbance value of MB was measured using a UV-vis spectrophotometer (Perkin Elmer Lambda 35, Waltham, MA, USA) before calculating the concentration of MB using the calibration curve.

Adsorption Equilibrium
Batch adsorption studies were used to investigate the adsorption equilibrium of methylene dye. Different parameters were tested, including the contact time, adsorbent dosage, pH of adsorbate, temperature of the reaction, and initial concentration of the adsorbate [27]. Each adsorbent with a calculated amount of 0.5 g/L, 1.5 g/L, 3.0 g/L, and 4.5 g/L was added to 250 mL conical flasks containing 50 mL of MB solution with a predetermined initial concentration of 100 mg/L, 200 mg/L, 300 mg/L, and 400 mg/L. These flasks were then placed in an orbital shaker operated at 100 rpm with computerized temperature-control, maintained at 25 • C, 35 • C, 45 • C, and 55 • C. After 60 min, 120 min, 240 min, 480 min, 720 min, and 1080 min, the solution was filtered through Whatman No. 2 filter paper. The filtrate was then analyzed using a UV-Vis spectrophotometer (Perkin Elmer Lambda 35) at a wavelength (lambda max) of 660.11 nm, and the lambda max was predetermined from the wavelength scan [28].

Thermodynamic Study
The thermodynamic study was conducted to evaluate the effect of temperature on the adsorption of MB on the cassava stem-activated carbon, while understanding the nature and feasibility of the reaction [29]. Adsorption was done at temperatures of 298.15 K, 308.15 K, 318.15 K, and 328.15 K with the adsorbate's initial concentrations of 100 mg/L, 200 mg/L, 300 mg/L, and 400 mg/L. Plots of the plot of lnKq versus 1/T (K −1 ) were completed where T is the absolute temperature in Kelvin. The changes in standard enthalpy (∆H) and standard entropy (∆S) were then calculated, according to the following Van't Hoff Equation (1): whereas ∆G was verified using the following equation: where R is defined as the universal gas constant (8.314 JK −1 mol −1 ), T represents the absolute temperature, and Kq is the thermodynamic equilibrium constant, it was measured as the ratio of adsorbate (MB) concentration at the surface of adsorbent to the adsorbate (MB) concentration remain in the residual solution.

Isothermic Study
A predetermined amount of adsorbate solution of different concentrations was mixed with 1.5 g of adsorbent in conical flasks and shaken at 100 rpm using the best contact time for adsorption to reach equilibrium in the previously done batch adsorption studies. Experiments were carried out at 25 • C, 35 • C, 45 • C, and 55 • C in triplicate. Mixtures were filtered, and the solutions obtained were analyzed using a UV-VIS spectrophotometer [30]. Langmuir and Freundlich isotherm models were used to fit the data obtained. The applicability of the isotherm equations to the adsorption iostherm was compared by the correlation coefficients, R-squared value (R 2 ). The general equation of the Langmuir isotherm is written as Equation (3): By plotting the graph, the parameters of the Langmuir adsorption can be determined from the linearized Equation (4): where Ce is the equilibrium concentration of the adsorbate (mg/L); qe is the adsorption capacity adsorbed at equilibrium (mg/g); qm is the maximum adsorption capacity (mg/g); and KL is the Langmuir adsorption constant that relates the energy of adsorption (L/mg). Freundlich isotherm, on the other hand, can be found by plotting ln qe versus ln Ce that yields a straight line with an intercept of ln Kf and a slope of 1/n, and the linear can be written as Equation (5): ln qe = ln Kf + 1/(n) ln Ce, where qe is the concentration of the adsorbed species, and Kf and n are empirical constants that are commonly temperature-dependent. The value 1/n represents the linearity of adsorption as the concentration change. The adsorption isotherm becomes more nonlinear as the n value getting larger [31,32].

Adsorption Kinetics
The kinetics studies were conducted to evaluate the adsorption dynamics in relation to time and quantify the rate of adsorption [33]. Fifty milliliters of 100 mg/L MB stock solution was added into a 250 mL conical flask containing 1.5 g/L dosages of the adsorbent. The adsorption kinetics was run at 25 • C with an agitation speed of 100 rpm at 60 min, 120 min, 240 min, 480 min, 720 min, and 1080 min time intervals. The mixture of adsorbent and MB stock solution was then filtered through Whatman No. 2 filter paper after each time interval. Finally, the filtrates were analyzed using UV-VIS spectrophotometer (Perkin Elmer Lambda 35) to determine the remaining MB dye in the solution.
Data from this experiment were fitted into the pseudo-first model, Equation (6): where qe and qt (mg/g) are the adsorption capacities at equilibrium and time t (min), respectively. The kp1 (min −1 ) is the pseudo-first-order rate constant for the kinetic model. A linear form of pseudo-second-order model was also applied Equation (7): where h = k 2 qe 2 . The parameters 'h' (mg/(g min)) means the initial adsorption rate and the constant (k 2 ) can be determined experimentally by plotting t/qt against t [34,35]. Other symbols represent the same as in pseudo-first-order.

Effect of Contact Time on the Adsorption
The adsorption capacity of both raw and activated carbon derived from the cassava stem was investigated. The results are illustrated in Figure 1. This figure showed that the concentration of MB dye decreased with an increase in contact time for both adsorbents. The high adsorption process was initially observed, starting from 120 min contact time for RCS. Meanwhile, a high percentage of removal was already observed at the first 60 min for ACS. Both samples showed a slight improvement in removal percentage at longer contact times and became almost constant at 24 h. The ease of accessibility of pores on the adsorbents caused a rapid adsorption process to occur at the initial contact time. There was a more minor improvement in adsorption percentage that occurred at longer contact time due to the bulky adsorbents that reduced the adhesion sites for adsorbates molecules [36].
It was observed that the adsorption capacity for ACS was higher than the RCS. The uptake amount increased by 55% at the initial 60 min after the cassava stem was converted into the activated carbon. This occurred as the high temperature in the activation process increased the pore size and volume of the cassava stem. Our previous study supports this fact, indicating a 0.765 m 2 /g surface area for raw cassava stem particles and a maximum surface area of 694.402 m 2 /g for cassava stem activated carbon [9]. Thus, the adhesion sites for adsorbates were increasing, which allowed more adsorbates molecules to be adsorbed onto the surface of the ACS. 21, 13, x FOR PEER REVIEW 5 of 17 time due to the bulky adsorbents that reduced the adhesion sites for adsorbates molecules [36]. It was observed that the adsorption capacity for ACS was higher than the RCS. The uptake amount increased by 55% at the initial 60 min after the cassava stem was converted into the activated carbon. This occurred as the high temperature in the activation process increased the pore size and volume of the cassava stem. Our previous study supports this fact, indicating a 0.765 m 2 /g surface area for raw cassava stem particles and a maximum surface area of 694.402 m 2 /g for cassava stem activated carbon [9]. Thus, the adhesion sites for adsorbates were increasing, which allowed more adsorbates molecules to be adsorbed onto the surface of the ACS.

Effect of Adsorbent Dosage on Adsorption of MB Dye
The capacity of adsorption percentage for a given initial concentration of MB dye can be measured by analyzing the effect of adsorbent dosage [37]. Figure 2 represents the effect of different dosages RCS and ACS on MB dye adsorption. The percentage of dye removal increased with higher adsorbent dosage until it achieved almost constant values after the critical dosage. The percentage of MB dye removal increased by 34.75% as RCS dosage was increased from 0.5 g/L to 4.5 g/L. Meanwhile, the additional dosage of ACS from 0.5 g/L to 4.5 g/L showed an increment of 16.37% for the removal of MB dye. When both RCS and ACS dosage was increased, the free sorption surface and adsorption sites will also be increased. Thus, more MB dye molecules will be adsorbed [38]. The increment of the percentage of removal, along with the increase in adsorbent dosage, for ACS was less than RCS. This happened as ACS already possessed a high percentage of removal at the lowest dosage (0.5 g/L). Therefore, the ACS had better efficiency in removal capacity and characteristics than the RCS. This is due to the nature of activated carbon which possessed larger surface area compared to raw sample. From the economic view, the ACS has better economic value than RCS since a small amount of ACS can remove a high amount of contaminant with the activation process records showing 38.7% in production yield [9].

Effect of Adsorbent Dosage on Adsorption of MB Dye
The capacity of adsorption percentage for a given initial concentration of MB dye can be measured by analyzing the effect of adsorbent dosage [37]. Figure 2 represents the effect of different dosages RCS and ACS on MB dye adsorption. The percentage of dye removal increased with higher adsorbent dosage until it achieved almost constant values after the critical dosage. The percentage of MB dye removal increased by 34.75% as RCS dosage was increased from 0.5 g/L to 4.5 g/L. Meanwhile, the additional dosage of ACS from 0.5 g/L to 4.5 g/L showed an increment of 16.37% for the removal of MB dye. When both RCS and ACS dosage was increased, the free sorption surface and adsorption sites will also be increased. Thus, more MB dye molecules will be adsorbed [38]. The increment of the percentage of removal, along with the increase in adsorbent dosage, for ACS was less than RCS. This happened as ACS already possessed a high percentage of removal at the lowest dosage (0.5 g/L). Therefore, the ACS had better efficiency in removal capacity and characteristics than the RCS. This is due to the nature of activated carbon which possessed larger surface area compared to raw sample. From the economic view, the ACS has better economic value than RCS since a small amount of ACS can remove a high amount of contaminant with the activation process records showing 38.7% in production yield [9].

Effect of pH Adsorbate on Adsorption of MB Dye
The adsorption of MB dye onto the RCS and ACS at different initial pH is shown in Figure 3. It demonstrated that the MB dye adsorption by the RCS was strongly pH-dependent, while, for the ACS, it was less affected by pH change. For RCS, the MB dye adsorption increased from 36.31% to 97.95% as the pH increased from pH 3 to pH 12. Meanwhile, ACS showed a slight increment of MB removal from 93.57% to 99.82% as pH increased. This showed that ACS could remove MB dye at any pH, but, still, more alkaline pH gave the best percentage of removal of MB dye. The H + ions were abundantly present at an acidic pH range that was likely to compete with the positively charged MB to attach to the adsorption sites. This explained the lowest adsorption percentage of MB at an acidic range of pH. Therefore, alkaline pH, especially a pH value of above 10, is more favorable due to the slight amount of H+ ions and the existence of negatively charged on the surface of the adsorbents. Hence, a more considerable amount of MB dye can be removed through the electrostatic force of attraction be-

Effect of pH Adsorbate on Adsorption of MB Dye
The adsorption of MB dye onto the RCS and ACS at different initial pH is shown in Figure 3. It demonstrated that the MB dye adsorption by the RCS was strongly pHdependent, while, for the ACS, it was less affected by pH change. For RCS, the MB dye adsorption increased from 36.31% to 97.95% as the pH increased from pH 3 to pH 12. Meanwhile, ACS showed a slight increment of MB removal from 93.57% to 99.82% as pH increased. This showed that ACS could remove MB dye at any pH, but, still, more alkaline pH gave the best percentage of removal of MB dye.

Effect of pH Adsorbate on Adsorption of MB Dye
The adsorption of MB dye onto the RCS and ACS at different initial pH is shown in Figure 3. It demonstrated that the MB dye adsorption by the RCS was strongly pH-dependent, while, for the ACS, it was less affected by pH change. For RCS, the MB dye adsorption increased from 36.31% to 97.95% as the pH increased from pH 3 to pH 12. Meanwhile, ACS showed a slight increment of MB removal from 93.57% to 99.82% as pH increased. This showed that ACS could remove MB dye at any pH, but, still, more alkaline pH gave the best percentage of removal of MB dye. The H + ions were abundantly present at an acidic pH range that was likely to compete with the positively charged MB to attach to the adsorption sites. This explained the lowest adsorption percentage of MB at an acidic range of pH. Therefore, alkaline pH, especially a pH value of above 10, is more favorable due to the slight amount of H+ ions and the existence of negatively charged on the surface of the adsorbents. Hence, a more considerable amount of MB dye can be removed through the electrostatic force of attraction be-  The H + ions were abundantly present at an acidic pH range that was likely to compete with the positively charged MB to attach to the adsorption sites. This explained the lowest adsorption percentage of MB at an acidic range of pH. Therefore, alkaline pH, especially a pH value of above 10, is more favorable due to the slight amount of H+ ions and the existence of negatively charged on the surface of the adsorbents. Hence, a more considerable amount of MB dye can be removed through the electrostatic force of attraction between the positively charged MB and the negatively surface of the adsorbents [39]. Moreover, at pH values higher than the zero-point charge, pHzpc, the surface of the adsorbents was supposed to possess a negative charge with a mainly strong electrostatic attraction towards the cationic MB [40]. The pHzpc values for RCS and ACS produced in this study were 6.53 and 9.20, respectively, measured according to solid addition method [41]. The initial pH of 50 mL, 0.03 M KNO 3 solution was adjusted to values between 1.5 and 11.5 by adding 0.1 M HCl or 0.1 M NaOH solutions. The same amount of adsorbents was added to each flask, and the final pH was measured after 24 h. The value of pHzpc was determined from the intersection of the plot pH initial versus pH final with line pH initial = pH final. Another possible mechanism may take place, as well, where the dispersive interactions of the π-π bond may be a response mechanism due to conjugate systems that exist in MB molecules. This mechanism can take place between the C=C, N=C, and aromatic rings system [42].

Effect of Temperature and Initial Concentration on the Adsorption of MB Dye
The effect of temperature as a function of the initial concentration of MB onto RCS and ACS is shown in Figure 4. These figures revealed that the adsorption of MB onto RCS and ACS was influenced by the temperature, in which high temperature gave a high adsorption percentage. This was due to the increment in the rate of diffusion of the solute through the liquid to the adsorption sites as the temperature increased, which led to the high adsorption capacity of the adsorbents.
These figures also show that the ACS has excellent adsorption characteristics since the ACS was capable of removing the high amount of MB dye (>99%) at low temperature (25 • C), up to the initial concentration of 200 mg/L. Additionally, ACS can remove MB dye at a high percentage (>99%) for the highest initial concentration (400 mg/L), at a set temperature of 55 • C only. The capability of the ACS as adsorbent was good enough as compared to the RCS since the RCS only has a high percentage of removal up to 98% for the lowest initial concentration (100 mg/L) and only at a high set temperature, which is 55 • C.
Additionally, high initial concentration did contribute to the relatively small amount of adsorption. This relies on the fact that a high initial concentration of MB possesses high driving forces that force the MB molecules to go into the pores onto the adsorbents. However, this factor is not strong enough to provide a high adsorption percentage of the MB, due to higher adsorbate ions: adsorption site ratio. Hence, another force from high temperature is required to complete the adsorption of MB, to a great extent in addition to the surface characteristic of these two adsorbents that favor the adsorption of MB.
Water 2021, 13, x FOR PEER REVIEW 7 of 17 tween the positively charged MB and the negatively surface of the adsorbents [39]. Moreover, at pH values higher than the zero-point charge, pHzpc, the surface of the adsorbents was supposed to possess a negative charge with a mainly strong electrostatic attraction towards the cationic MB [40]. The pHzpc values for RCS and ACS produced in this study were 6.53 and 9.20, respectively, measured according to solid addition method [41]. The initial pH of 50 mL, 0.03 M KNO3 solution was adjusted to values between 1.5 and 11.5 by adding 0.1 M HCl or 0.1 M NaOH solutions. The same amount of adsorbents was added to each flask, and the final pH was measured after 24 h. The value of pHzpc was determined from the intersection of the plot pHinitial versus pHfinal with line pHinitial = pHfinal. Another possible mechanism may take place, as well, where the dispersive interactions of the π-π bond may be a response mechanism due to conjugate systems that exist in MB molecules. This mechanism can take place between the C = C, N = C, and aromatic rings system [42].

Effect of Temperature and Initial Concentration on the Adsorption of MB Dye
The effect of temperature as a function of the initial concentration of MB onto RCS and ACS is shown in Figure 4. These figures revealed that the adsorption of MB onto RCS and ACS was influenced by the temperature, in which high temperature gave a high adsorption percentage. This was due to the increment in the rate of diffusion of the solute through the liquid to the adsorption sites as the temperature increased, which led to the high adsorption capacity of the adsorbents.
These figures also show that the ACS has excellent adsorption characteristics since the ACS was capable of removing the high amount of MB dye (>99%) at low temperature (25 °C), up to the initial concentration of 200 mg/L. Additionally, ACS can remove MB dye at a high percentage (>99%) for the highest initial concentration (400 mg/L), at a set temperature of 55 °C only. The capability of the ACS as adsorbent was good enough as compared to the RCS since the RCS only has a high percentage of removal up to 98% for the lowest initial concentration (100 mg/L) and only at a high set temperature, which is 55 °C.
Additionally, high initial concentration did contribute to the relatively small amount of adsorption. This relies on the fact that a high initial concentration of MB possesses high driving forces that force the MB molecules to go into the pores onto the adsorbents. However, this factor is not strong enough to provide a high adsorption percentage of the MB, due to higher adsorbate ions: adsorption site ratio. Hence, another force from high temperature is required to complete the adsorption of MB, to a great extent in addition to the surface characteristic of these two adsorbents that favor the adsorption of MB.

Thermodynamic Study
The thermodynamic study was done to evaluate the thermodynamic feasibility of the MB adsorption onto all adsorbent samples. The parameters calculated included standard change in enthalpy (∆H • ), standard change in entropy (∆S • ), and the standard change in Gibbs free energy (∆G • ). The primary consideration of the thermodynamic study is to determine the spontaneity of the adsorption process through the calculation of ∆G • . Figure 5 showed

Thermodynamic Study
The thermodynamic study was done to evaluate the thermodynamic feasibility of the MB adsorption onto all adsorbent samples. The parameters calculated included standard change in enthalpy (∆H°), standard change in entropy (∆S°), and the standard change in Gibbs free energy (∆G°). The primary consideration of the thermodynamic study is to determine the spontaneity of the adsorption process through the calculation of ∆G°. Figure  5 showed the plot of ln (Kq) versus 1/T (K −1 ) for all types of adsorbents, which gave the values of ∆H° and ∆S°. Parameters involved included temperatures of 298.15 K, 308.15 K, 318.15 K, and 328.15 K, adsorbate's initial concentrations of 100 mg/L, 200 mg/L, 300 mg/L, and 400 mg/L, 1.5 g/L of adsorbent dosage, and 1080 min of contact time. The linear equations, R-squared values, and thermodynamic parameters for the adsorption of MB dye onto all types of cassava stem adsorbents are summarized in Table 1. The RCS and ACS showed positive values of ∆H°, indicating that the adsorption process of MB by both adsorbents was endothermic [43]. Meanwhile, the positive values of ∆S° showed by all types of cassava stem adsorbent RCS and ACS indicated that the surface changes had happened due to the interaction of MB molecules with the active sites of cassava stem adsorbents, mainly hydroxyl groups in lignin and cellulose [44]. It also indicates increased randomness at the solid-solute interface during adsorption processes. The MB ions replaced the previously adsorbed water on the surface of the adsorbent, creating randomness in the system [45].
The negative value of ∆G° showed the spontaneous reaction of MB adsorption. Additionally, the ∆G° values for all types of adsorbents decreased when the reaction temperature was increased, indicating that high adsorption had been achieved at high temperatures [46]. Table 1 also reveals the adsorption process of MB onto the RCS was spontaneous at all temperatures for the initial concentration of 100 and 200 mg/L. For the initial concentration of 300 mg/L, a higher temperature was needed for the adsorption to be spontaneous. The ACS showed better thermodynamic properties than RCS in terms of The linear equations, R-squared values, and thermodynamic parameters for the adsorption of MB dye onto all types of cassava stem adsorbents are summarized in Table 1. The RCS and ACS showed positive values of ∆H • , indicating that the adsorption process of MB by both adsorbents was endothermic [43]. Meanwhile, the positive values of ∆S • showed by all types of cassava stem adsorbent RCS and ACS indicated that the surface changes had happened due to the interaction of MB molecules with the active sites of cassava stem adsorbents, mainly hydroxyl groups in lignin and cellulose [44]. It also indicates increased randomness at the solid-solute interface during adsorption processes. The MB ions replaced the previously adsorbed water on the surface of the adsorbent, creating randomness in the system [45].
The negative value of ∆G • showed the spontaneous reaction of MB adsorption. Additionally, the ∆G • values for all types of adsorbents decreased when the reaction temperature was increased, indicating that high adsorption had been achieved at high temperatures [46]. Table 1 also reveals the adsorption process of MB onto the RCS was spontaneous at all temperatures for the initial concentration of 100 and 200 mg/L. For the initial concentration of 300 mg/L, a higher temperature was needed for the adsorption to be spontaneous. The ACS showed better thermodynamic properties than RCS in terms of adsorption spontaneity. This was due to the result showing that spontaneous adsorption using ACS at an initial concentration of 300 mg/L can be achieved at low temperatures.

Isothermic Study
Isothermic studies characterize how adsorption molecules were dispersed in the solid and liquid phases to achieve the equilibrium state. The design optimization of an adsorption system is a vital key in studying the isotherm characteristics. The correlation between the adsorption capacity onto the adsorbent surface and adsorbate concentration at a particular temperature can be acquired. In this study, the Langmuir and Freundlich models were fitted to find the most appropriate relationship for the equilibrium curves. This fitting can be used to study the interactions between the adsorbate and adsorbent during adsorption.

Langmuir Isotherm Model
The Langmuir isotherm suggested the development of single layer coverage of adsorbate on the external surface of the adsorbent with no further adsorption taking place subsequently. The Langmuir isotherm implies that there is a fixed number of sites on the surface of the adsorbent for the adsorption process to happen, and all these sites are equal in terms of energy [47]. The linear equation of Langmuir isotherm is expressed as Ce/qe = 1/qmKL + Ce/qm, as described in the methodology part.). Figure 6 presents the plot of Ce/qe versus Ce for all types of cassava stem adsorbents. This plot gives slope 1/qm and intercepts 1/qmKL, which was used to calculate the qm and KL. adsorption spontaneity. This was due to the result showing that spontaneous adsorption using ACS at an initial concentration of 300 mg/L can be achieved at low temperatures.

Isothermic Study
Isothermic studies characterize how adsorption molecules were dispersed in the solid and liquid phases to achieve the equilibrium state. The design optimization of an adsorption system is a vital key in studying the isotherm characteristics. The correlation between the adsorption capacity onto the adsorbent surface and adsorbate concentration at a particular temperature can be acquired. In this study, the Langmuir and Freundlich models were fitted to find the most appropriate relationship for the equilibrium curves. This fitting can be used to study the interactions between the adsorbate and adsorbent during adsorption.

Langmuir Isotherm Model
The Langmuir isotherm suggested the development of single layer coverage of adsorbate on the external surface of the adsorbent with no further adsorption taking place subsequently. The Langmuir isotherm implies that there is a fixed number of sites on the surface of the adsorbent for the adsorption process to happen, and all these sites are equal in terms of energy [47]. The linear equation of Langmuir isotherm is expressed as Ce/qe = 1/qmKL + Ce/qm, as described in the methodology part.). Figure 6 presents the plot of Ce/qe versus Ce for all types of cassava stem adsorbents. This plot gives slope 1/qm and intercepts 1/qmKL, which was used to calculate the qm and KL.  Table 2 summarizes the parameters for the Langmuir isotherm, including linear equation, R 2 value, qm, KL, and RL. The maximum monolayer coverage capacity (qm) in this study increased with the rise in reaction temperature. At higher temperatures, there will be an increment in the diffusion rate of the adsorbate molecules within the pores and across the external boundary layer of the adsorbent [48]. In addition, the Langmuir constant, KL, in this study, increased with temperature, which confirmed the endothermic nature of the MB adsorption onto the cassava stem adsorbents [49]. Based on the regression coefficient (R 2 ) value, all types of cassava stem adsorbents were fit well with the Langmuir isotherm model at each temperature. This also indicated that the cassava stem adsorbents had a homogenous surface in nature [50].
Additionally, further analysis of the Langmuir isotherm can be conveyed using dimensionless separation factor, RL [51]. This separation factor is the essential characteristic of the Langmuir isotherm that describes the type of isotherm. It was expressed as RL = 1/(1 + KLCo), where Co is the initial concentration of adsorbate in solution (mg/L), and KL is the Langmuir constant. Accordingly, RL value is the positive numbers that determines the feasibility of the adsorption process to be either unfavorable if RL > 1; favorable if 0 < RL < 1; linear adsorption if RL = 1; and irreversible adsorption if RL = 0 [52]. In this study, the separation factor, RL, for all types of adsorbents is between 0 and 1, indicating that the equilibrium sorption was favorable.

Freundlich Isotherm Fitting
The multilayer adsorption characteristic onto the heterogeneous surface with irregular distribution of adsorption energy is described by the Freundlich isotherm model [53]. It was expressed in linear form as ln qe = ln Kf + 1 n ln Ce, where, qe is the adsorption capacity adsorbed at equilibrium (mg/g), Ce is the equilibrium concentration of adsorbate (mg/L), Kf is the Freundlich isotherm constant, and 1 n is the adsorption intensity that varies with the heterogeneity of the adsorbent. The constants n and Kf are determined from the slope and intercept of the graph of ln qe versus ln Ce, as shown in Figure 7. Table 3 presents the linear equation, R 2 value, and Freundlich parameters for the MB adsorption onto all types of cassava stem adsorbents. The adsorption coefficient that signifies the number of adsorbate molecules adsorbed can be determined from the Kf value. Results from this study showed the Kf value was increasing as the temperature increased from 25 • C to 55 • C, which can be explained by the increment of the diffusion rate of the MB into pores of the adsorbents at a higher temperature [54]. Thus, the high adsorption capacity of the MB onto the surface of the cassava stem adsorbents was obtained as the high temperature was utilized during the adsorption process.  Table 3 presents the linear equation, R 2 value, and Freundlich parameters for the MB adsorption onto all types of cassava stem adsorbents. The adsorption coefficient that signifies the number of adsorbate molecules adsorbed can be determined from the Kf value. Results from this study showed the Kf value was increasing as the temperature increased from 25 °C to 55 °C, which can be explained by the increment of the diffusion rate of the MB into pores of the adsorbents at a higher temperature [54]. Thus, the high adsorption capacity of the MB onto the surface of the cassava stem adsorbents was obtained as the high temperature was utilized during the adsorption process. The nature and strength of the sorption process, as well as the distribution of the active sites, is measured from the slopes . The partition between the two phases is independent of the concentration if = 1. Normal adsorption, which corresponds to the normal L-type Langmuir isotherm, is specified once values of < 1, and cooperatives adsorption that involve strong interaction between the molecules of adsorbate is specified  The nature and strength of the sorption process, as well as the distribution of the active sites, is measured from the slopes 1 n . The partition between the two phases is independent of the concentration if 1 n = 1. Normal adsorption, which corresponds to the normal L-type Langmuir isotherm, is specified once values of 1 n < 1, and cooperatives adsorption that involve strong interaction between the molecules of adsorbate is specified when the value 1 n > 1. The value of 1 n for all types of adsorbent samples in this study presented a value of less than 1. This revealed that the adsorption of the MB onto the surface of cassava stem adsorbents is normal in equivalents to the normal L-type of the Langmuir isotherm [52].
The value of n ranging from 1 to 10 indicates favorable adsorption. In this study, most of the cassava stem adsorbents displayed n value in the range of 1 to 10. Consequently, unsuitable adsorption parameters can be avoided in the adsorption of MB dye at an industrial scale. However, the R 2 value obtained from the linear plot of ln qe versus ln Ce for all types of cassava stem adsorbents showed poor agreement with the Freundlich isotherm model. Therefore, the adsorption of MB onto the adsorbent samples did not perform multilayer adsorption. Table 4 summarizes some recently researched adsorbents for MB adsorption. The ACS showed a considerably high adsorption percentage for MB with a maximum of 384.61 mg/g compared to other materials. Ease of acquisition, low cost, and high adsorption efficiency of ACS are among the advantages of this material.

Kinetic Studies
The rate uptake of MB molecules onto the adsorbents' surface was studied using pseudo-first-order and pseudo-second-order kinetic models. The correlation coefficient, R 2 , was used to verify the validity of the applied models. The kinetic studies were critical to optimize and design the handling of particular effluent [58].

Pseudo-First Order Kinetic Model
The pseudo-first-order equation was expressed as log(qe − qt) = log(qe) − (k 1 /2.303).t. Plots of log(qe − qt) against time for all types of cassava stem adsorbents are displayed in Figure 8. The parameters obtained from the plot of linearized equation, namely first-order rate constant, k 1 , and adsorption capacity at equilibrium, qe, are presented in Table 5, along with the linear equation and R 2 value for each cassava stem adsorbents. It was observed that the MB adsorption onto each type of cassava stem adsorbents did not fit well with the pseudo-first-order kinetic model.    A linear form of the pseudo-second-order kinetic model was expressed as t/qt = 1/h + (1/qe).t, where h is the initial sorption rate as qt/t = 0; thus, h = k 2 qe 2 . The plot of t/qt versus time for all types of cassava stem adsorbents is presented in Figure 9. The plots give the adsorption capacity at equilibrium (qe), as well as the second-order rate constant for each cassava stem adsorbents studied. Table 6 tabulates the pseudo-second-order parameters and the linear equation and corresponding correlation coefficients for each type of cassava stem adsorbents. The h value was much higher for the ACS sample. This simply indicated that the ACS samples have a higher initial rate of adsorption compared to RCS. The value of the correlation coefficient for both types of cassava stem adsorbents is near unity. This fact specified that the rate of MB adsorptions onto the cassava stem adsorbents was fit better by the pseudo-second-order kinetic model, which suggested the chemisorption process [59].

Conclusions
The MB adsorption from water using the RCS and ACS was done in this study. Batch adsorption study showed faster MB uptake by ACS (60 min contact time) than RCS (120 min contact time). Higher adsorbent dosage and higher pH contribute to a higher adsorption percentage. The pHzpc values for RCS and ACS produced in this study were 6.53 and 9.20. The thermodynamic study showed positive values of ∆H° of RCS and ACS, indicating that the adsorption process of MB by these two adsorbents is endothermic. The negative value of ∆G° shows that the adsorption processes of MB are spontaneous. The ad-

Conclusions
The MB adsorption from water using the RCS and ACS was done in this study. Batch adsorption study showed faster MB uptake by ACS (60 min contact time) than RCS (120 min contact time). Higher adsorbent dosage and higher pH contribute to a higher adsorption percentage. The pHzpc values for RCS and ACS produced in this study were 6.53 and 9.20. The thermodynamic study showed positive values of ∆H • of RCS and ACS, indicating that the adsorption process of MB by these two adsorbents is endothermic. The negative value of ∆G • shows that the adsorption processes of MB are spontaneous. The adsorption isotherm showed higher fitting to Langmuir isotherm for both samples, with the highest adsorption recorded by ACS (384.61 mg/g). The kinetic study showed higher R 2 by pseudo-second-order equation, which suggests the chemisorption process for both samples. Meanwhile, the RCS recorded 133.33 mg/g adsorption capacity for MB. Considering 2.88 times higher ACS adsorption capacity than RCS, it is a significant improvement of the material as an MB adsorbent. It can be concluded that producing activated carbon from cassava stem is worthwhile, taking into account the adsorption efficiency, year-round availability, and low cost of raw material.