Kinetic Study of the Bioadsorption of Methylene Blue on the Surface of the Biomass Obtained from the Algae D. antarctica.
Water pollution by various industries is the main problem the world is facing these times. Among these pollutants are the dyes [1, 2]; their world production per year is approximately 7 x [10.sup.5] MT, and around 10 to 15% of the dyes used are dumped in waste water . Synthetic dyes are more difficult to remove than natural dyes , and this is due to their complex aromatic structure, which gives them stability against air and light . They can easily transport within the aqueous environment due to their high solubility in water . They affect the aquatic autotrophs by restricting their photosynthetic efficiency because only limited sunlight is allowed to penetrate due to their colour; their toxic effect spreads along the food chain, and they are conserved for long periods deteriorating animal and human health .
Methylene blue (MB) is a cationic dye with broad applications such as dye for paper, hair, and cotton and filters for medical surgery  among others. This pollutant not only deteriorates water quality but also significantly affects the environment and human health . It has been shown that, in humans, it causes vomiting, lightheadedness, cyanosis, jaundice, tissue necrosis , increased heart rate, vomiting, shock, and tetraplegia . Therefore, there is a need to eliminate this dye present in wastewater or industrial effluents to ensure a safer environment . This and the other dyes are difficult to degrade biologically, so the studies aimed at removing these contaminants present in aqueous solution are important and must be carried out [8, 9] to reduce environmental damage and human health.
Various technologies, including adsorption, flocculation, membrane filtration, electrolysis, biological treatments, oxidation , sedimentation, membrane separation, reverse osmosis , and photocatalytic degradation , have been adopted to remove dyes from sewage water. Among the mentioned treatments, adsorption has some advantages because the adsorbents are inexpensive, are available, are simple to use, and have high efficiency  and their design is simple . However, the total removal of MB from the wastewater has not been achieved; therefore, it is necessary to continue with the studies to discover new bioadsorbents .
Many adsorbents have been studied to reduce the concentration of the dyes present in aqueous solutions, among which the activated carbon stands out for its high efficiency; however, its manufacture and regeneration involve a high cost. So, they have discovered and applied other natural adsorbents such as natural coal, chitin, chitosan, fly ash, wood sawdust, and rice husk .
Adsorption using biomass is considered a potential technique for the removal of contaminants present in water, and the advantage of using this adsorbent is that it is more economical than commercial adsorbents . The scope of this research is to perform the kinetic study of the MB adsorption on the surface of the biomass obtained from the algae D. antarctica and to determine the capacity of adsorption of the contaminant (MB) by the bioadsorbent. To understand the mechanism of adsorption of this process, different kinetic and adsorption models were applied to the obtained data. Additionally, traditional instrumental techniques were used to characterize the bioadsorbent.
2. Materials and Methods
2.1. Preparation of the Biomass. Biomass brown alga was collected from the Chilean coast, for preparing samples of fresh alga washed with distilled water to remove impurities, and dried at 40[degrees]C using an oven (Memmert, Germany) for 72 hours; once the drying process was finished, the material was cut into small pieces, before being grounded, and the dried biomass was sieved to a particle size of 500-1000 [micro]m. This material was used in all experiments .
2.2. Characterization. In order to evaluate the properties of the biomass surfaces obtained from the algae D. antarctica, which allow MB adsorption to be effective, this material was characterized by the techniques provided below.
2.2.1. Infrared Spectroscopy. The data of the IR spectra of the biomass before and after the adsorption of MB were recorded using an instrument SHIMADZU IRTracer-100. The pressed granules were prepared by grinding the biomass and mixing it with KBr in an agate mortar. The spectral data were recorded at wavenumber values between 4000 and 500 [cm.sup.-1].
2.2.2. Scanning Electron Microscopy. This technique was used to observe the morphology of the biomass surface before and after the MB adsorption process in a JEOL JSM-6490LV unit. For the SEM analysis, the sample obtained after the MB adsorption process was separated from the solution and dried at a temperature of 120[degrees]C for 5 h. Before carrying out this analysis, the surface of the biomass was coated with gold using the sputtering method to obtain a conductive surface.
2.3. Studies of the Biosorption of the Function of the pH. For the determination of the optimum pH of biosorption, methylene blue solutions of 50 ppm were prepared, whose pH was adjusted to values of 3, 5, 7, 9, and 11, after which the biomass was added in a ratio of 1 g/L, the samples were left in constant agitation for a period of 15 hours, and the MB concentration was determined at the beginning and end of the bioadsorption process by UV-Vis spectroscopy at a wavelength of 664 nm in a GENESYS 5 spectrophotometer.
2.4. Studies of Adsorption Kinetics. To prepare the kinetic studies, solutions of 25, 50, 100, 150, and 200 ppm of MB were prepared. According to the results obtained in Section 3.2, the optimum pH value of adsorption must be above 5; therefore, the pH of the solutions was adjusted to a value of 10 using 0.1 M x HCl and NaOH solutions. After this, the biomass was added in a ratio of 1 g/L, the samples were left in agitation, and aliquots were taken at 0, 5, 10, 15, 30, 60, 120, 240, 360, 480, and 560 minutes, to track the decrease in MB concentration present in the solution. Using (1), the values of [q.sub.t] were determined for the different kinetic experiments carried out:
[q.sub.t] = V([C.sub.0] - [C.sub.t])/m, (1)
where [q.sub.t] is the amount of MB adsorbed per gram of the sample (mg/g) in time (t) of the adsorption process, [C.sub.0] is the initial concentration of the solution (mg/L), [C.sub.t] is the concentration of the solution in time (t) of the adsorption process (mg/L), V is the initial volume of the solution, and m is the biomass added to the different solutions .
2.5. Studies of Equilibrium in the Solid-Liquid Interface. To understand the mechanism of adsorption of methylene blue on the surface of the biomass, solutions were prepared with initial concentrations of 25, 50, 100, 150, 200, 400, 600, 800, 100, and 1400 ppm of this contaminant; the pH of the solutions that were in the concentration range of 25 to 200 ppm was adjusted to a value of 10, and the pH value of the solutions that were in the concentration range of 400 to 1400 ppm was not adjusted since the pH value of these solutions was above 5. In Section 3.2, it was determined that, at basic pH values, the adsorption capacity of MB on the surface of the biomass is constant, so it was decided not to make adjustments to the pH value of these solutions.
The samples were left in agitation for 18 hours; using UV-Vis spectroscopy, the concentration of these solutions was determined at the beginning and at the end of the process. Using (2), the MB's adsorption capacity was determined by the biomass when the solution is in equilibrium at the end of this process:
[q.sub.e] = V([C.sub.0] - [C.sub.e])/m, (2)
where [q.sub.e] is the amount of MB adsorbed per gram of the sample (mg/g) at equilibrium and [C.sub.e] is the concentration of MB in equilibrium (mg/L). The data obtained were adjusted to the models of Freundlich, Langmuir, Redlich-Peterson, Sips, and Toth, to understand the mechanism of adsorption of MB which takes place on the surface of biomass .
2.6. Thermodynamic Studies of the Kinetics of Adsorption. Speed laws are essential in any study of biosorption because they provide an exact expression during the duration of the reaction . Then, the models used in the present study are described below.
2.6.1. Pseudo-First-Order and Pseudo-Second-Order Models. There are several models of kinetics, but in general, the most used and compared ones are the pseudo-first-order and pseudo-second-order kinetic models. The pseudo-first-order kinetic model was proposed for the first time at the end of the 19th century by Lagergren, and the speed constant when using this model is denoted as [K.sub.1] . The pseudo-second-order kinetic model was introduced for the first time in the mid-80s, but its recognition increased in the year of 1999 when Ho and McKay  took data from experiments reported in the literature and determined that the best fit to the data coming from all the systems studied was given by applying the pseudo-second-order model. After this publication came to light, the speed constant [K.sub.2] has become more popular since in most studies, it has been found that the data obtained fit this model; for this reason, the original article has more than 6000 citations, a figure that has increased exponentially over the course of the time , and the equations of these two models are presented below.
A pseudo-first-order model is given as follows:
log(1 - [q.sub.t]/[q.sub.e]) = [[k.sub.1]/2.303] t, (3)
where [q.sub.t] is the concentration of the adsorbed phase at a certain time of the adsorption process, [q.sub.e] is the concentration of the adsorbed phase at the end of equilibrium with the solid present in suspension, t is the time that has elapsed since the process of adsorption began, and [k.sub.L] is the Lagergren constant ([s.sup.-1]). The pollutant adsorption rate is proportional to the time that has elapsed since the adsorption process began; for T = 0, the value of [q.sub.t] = 0; once equilibrium has been reached, the value of [q.sub.t] [approximately equal to] [q.sub.e] .
A pseudo-second-order model is given as follows:
t/[q.sub.t] = 1/[k.sub.2][q.sup.2.sub.e] + [1/[q.sub.e]] t. (4)
When t approaches zero, the bioadsorption velocity [q.sub.t]/t becomes the initial bioadsorption velocity, and the data obtained in the kinetic study are adapted to the pseudo-second-order model by plotting the graph of t/[q.sub.t] versus t. The linear relationship obtained will allow the calculation of [q.sub.e], [k.sub.2], and [k.sub.2][q.sup.2.sub.e] without previously knowing any parameter .
2.6.2. Modified Pseudo-First-Order Model. This kinetic model is useful when the experimentally obtained data do not conform to the pseudo-first-order and pseudo-second-order kinetic models and the model of intraparticle diffusion. In this new model, the pseudo-first-order equation is modified by the speed constant as observed in the following equation :
ln(1 - ([q.sup.t]/[q.sub.e]) + [q.sub.t]/[q.sub.e] = -[k.sub.m]t. (5)
Since [q.sub.t] < [q.sub.e], this equation implies that the velocity constant [k.sub.1] is minimal when equilibrium has been reached .
2.6.3. Elovich Model. It has been found that Elovich's empirical adsorption model has broad applicability for numerous adsorption systems. This model is based on the assumption of energetic heterogeneity of the adsorption sites in the form of rectangular distribution .
The kinetic model of Elovich is reported as follows:
[q.sub.t] = [1/[beta]] ln([alpha][beta]) + [1/[beta]] ln t, (6)
where [alpha] is the initial adsorption rate of the Elovich equation (mg x [g.sup.-1] [min.sup.-1]) and [beta] is the adsorption constant of the model (mg x [mg.sup.-1]) ; it is related to the adsorption energy .
The Elovich equation can be linearized by assuming [alpha][beta]t [much greater than] t and that Q = 0 at t = 0 and that Q = [Q.sub.t] for a time t = [t.sub.t] . Under these conditions, a graph of [q.sub.t] versus ln (t) shows a linear relationship with a slope of (1/[beta]) and an intercept of (1/[beta]) ln ([alpha][beta]) .
This equation has been used by some authors to describe the kinetics of adsorption of contaminants in natural adsorbents, prepared or modified, which found that the best behavior of the data obtained is given when applying this model. But in spite of the utility of the Elovich equation in the estimation of the biosorption kinetics, the study of other kinetic models must be carried out, since these can present, in some cases, marginally superior correlation coefficients in the kinetics of adsorption of chemical substances .
This equation is also used to describe reaction mechanisms such as solute diffusion in the solution or interface phase, surface activation, and deactivation. It is adequate to elucidate the process with significant changes of activation energy. In addition, the Elovich equation can also reveal the irregularity of data that other dynamic equations have ignored .
2.6.4. Intraparticle Diffusion Model. According to chemical reaction fundamental theory, intraparticle diffusion becomes a limiting factor to the overall reaction rate when the catalyst particle size is too large and/or the intrinsic reaction rate is too fast compared to the diffusion rate of reacting molecules inside the catalyst pores. The degree of inhibition resulting from the overall velocity depends on the combination of particle size and shape, intrinsic reaction velocity, and diffusion rate .
According to literature , if the rate-limiting step is intraparticle diffusion, then the amount adsorbed at any time t should be directly proportional to the square root of the contact time t and pass through the origin.
The intraparticle diffusion model is reported as follows:
Log [q.sub.t] = log [k.sub.ip] + 0.5 log t, (7)
where [k.sub.ip] is the intraparticle diffusion rate constant (mg/g/[min.sub.-0.5]) .
The graph of [q.sub.t] against 0.5 log t should produce a straight line with a positive intercept for the adsorption process controlled by intraparticle diffusion. The constant K is determined from the intersection with the Y-axis, and the high values of this parameter are related to a great adsorption speed .
2.6.5. Film Diffusion Model. The film diffusion model is reported as follows:
ln(1 - [q.sub.t]/[q.sub.e]) = -[k.sub.F]t + A, (8)
where [k.sub.F] (1/min) and A are the constants of the film diffusion model .
In order to minimize the error distribution between experimental equilibrium data and values obtained by isotherm correlations, different error functions are generally applied. This goal of minimizing the error distribution is achieved by finding the minimum value of certain error functions or maximizing them depending on the definition of the selected error function. Therefore, choosing an error function seems indispensable in order to evaluate the best fit isotherm to the experimental equilibrium data . In the present investigation, five different error functions (Table 1) were used to establish with certainty the isotherm of the kinetic model that presents the best adjustment of the adsorption of methylene blue on the surface of the algae D. antarctica.
2.7. Thermodynamic Studies of Bioadsorption
2.7.1. Model of Freundlich. The Freundlich model is described by an empirical equation used for systems with a high degree of heterogeneity. In this model, it is assumed that adsorption occurs at different sites and the formation of multilayers occurs with different adsorption energies. This leads to an exponential decrease in energy as the coverage of the surface originates .
The model of the Freundlich isotherm is reported as follows:
[mathematical expression not reproducible], (14)
where [q.sub.e] (mg * [g.sup.-1]) is the capacity of bioadsorption of the metal by the algae D. antarctica in the balance, [C.sub.e] (mg * [L.sup.-1]) is the concentration of the metal in the equilibrium, and [mathematical expression not reproducible] and [n.sub.f] (dimensionless) are the constants of the Freundlich isotherm and are related to the capacity of biosorption and intensity, respectively; Freundlich's constant ([n.sub.f]) depends on the adsorption capacity, and it is used to evaluate the favouribility of adsorption. The values of [n.sub.f] between 2 and 10 indicate a high adsorption capacity, while values between 1 and 2 indicate a moderate adsorption capacity and values less than 1 indicate a small adsorption capacity .
2.7.2. Langmuir Model. The Langmuir model is based on the assumption that adsorption occurs on a surface with homogeneous sites, where each molecule of the adsorbate occupies an adsorption site, and maximum adsorption occurs with the formation of the complete monolayer, in which there is migration of the adsorbate molecules on the surface of the adsorbent .
The model of the Langmuir isotherm is reported as follows:
[q.sub.e] = [q.sub.m][K.sub.L][C.sub.e]/1 + [K.sub.L][C.sub.e] (15)
where [q.sub.m] (mg * [g.sup.-1]) is the maximum adsorption capacity of the bioadsorbent and [K.sub.L] (L * [mg.sup.-1]) is the Langmuir equilibrium counterrelated to bioadsorption energy.
2.7.3. Sips Model. The two models of previous isotherms have been widely used to analyze the biosorption of various pollutants present in aqueous solutions. The Sips model simultaneously involves the Freundlich and Langmuir models, has three parameters taken from the theory of these models , and has a greater capacity to describe the biosorption equilibrium.
The model of the Sips isotherm is reported as follows:
[mathematical expression not reproducible], (16)
where [K.sub.s] is the Sips count in equilibrium and [n.sub.s] (dimensionless) is the heterogeneity factor; a value of [n.sub.s] close to or equal to 1 is given in bioadsorbents with homogeneous active sites , while a value of [n.sub.s] close to 0 is given in biosorbents with heterogeneous active sites .
2.7.4. Toth Model. In the Toth model, an asymmetric quasi-Gaussian energy distribution is assumed, where most of the sites have a lower adsorption energy than the energy peak of maximum adsorption . Toth modifies the Langmuir equation in order to reduce the error between the experimental and predicted values of adsorption equilibrium. This model is best suited for heterogeneous systems in which multiple layer adsorption occurs. The exponent of the isotherm of Toth ([mathematical expression not reproducible]) is related to the heterogeneity of the surface; if it is equal to the unit, the Toth model is reduced to the Langmuir model. This correlation is applied for liquid-solid adsorption .
The model of the Toth isotherm is reported as follows:
[mathematical expression not reproducible], (17)
where [mathematical expression not reproducible] and [mathematical expression not reproducible] are constants of the model.
2.7.5. Redlich-Peterson Model. The Redlich-Peterson isotherm is an empirical model with no theoretical basis, which contains undefined empirical parameters ([K.sub.R] and [[alpha].sub.R]). This model can be applied for homogeneous and heterogeneous surfaces and does not follow the ideal monolayer adsorption; as a consequence, this model provides the best approximation of the experimental data. However, the main disadvantage of this model is the lack of estimation of the maximum adsorption capacity. Another disadvantage when applying this model is that it does not adjust to the experimental data; in the trials, the dose of some variables has varied, since the constant [[alpha].sub.R] depends on the dose of the variables studied . It should also be noted that this model includes the characteristics of the Langmuir and Freundlich isotherms in a single equation.
The Redlich-Peterson isotherm model is reported as follows:
[q.sub.e] = [K.sub.RP][C.sub.e]/1 + [[alpha].sub.RP][C.sub.g.sub.e], (18)
where [K.sub.RP] is the constant of the Redlich-Peterson model (L/g), [[alpha].sub.RP] is another constant of the Redlich-Peterson model [(mg/L).sup.-g], and g is the exponent of this model and must be between 0 < g [less than or equal to] 1.
When g = 1, the Redlich-Peterson equation becomes the Langmuir equation:
[q.sub.e] = [K.sub.RP][C.sub.e]/1 + [a.sub.RP][C.sub.e]. (19)
When g = 0, the Redlich-Peterson equation becomes Henry's law (20) :
[q.sub.e] = [K.sub.RP][C.sub.e]/1 + [a.sub.RP]. (20)
311. Infrared Spectroscopy. The FTIR spectra before and after MB adsorption can be seen in Figure 1. In this analysis, several peaks assigned to the vibrations of the biomass functional groups were detected. Some of them are involved in MB adsorption, while others did not disappear, or their wavenumber shifted when this process was completed. The appearance of new peaks after the bioadsorption process was also observed due to the interaction between the functional groups of the bioadsorbent and the MB.
The peaks at 3398 and 1613 [cm.sup.-1] of the biomass before the adsorption process correspond to antisymmetric OH stretch vibrations [36, 37] and to the C=O bond present in the acids [36, 38], the peak located at 1425 [cm.sup.-1] corresponds to primary alcohols , the peak at 2.936 [cm.sup.-1] is due to the stretching vibrations of OH of carboxylic acids , the biomass adsorption band before and after adsorption of MB at a wavenumber of 1035 [cm.sup.-1] is assigned to the CO present in the esters, and the peak at 1060 [cm.sup.-1] can also be assigned to CO stretches .
The IR peaks of the MB that appeared after the adsorption process are described as follows: the peaks at 1600 and 1394 [cm.sup.-1] correspond to vibrations of the aromatic ring and the CN bond, respectively, the peaks at 1336, 1141, and 1247 [cm.sup.-1] are attributed to symmetric deformation of -C[H.sub.3] and the CN bond, respectively , the peaks at 1653 [39,40], 1394,1336, and 1141 [cm.sup.-1] can be assigned to the vibrations of -C=C- of the stretch of the alkenes, to the C-C stretching in the aromatic ring, to the balancing of the CH alkanes, and to the wagging of the C-H (-C[H.sub.2]Cl) of alkyl halides, respectively, the peak at 1247 [cm.sup.-1] corresponds to the stretching of aliphatic amines , and the peak observed at 1150 [cm.sup.-1] belongs to the vibration stretch of -S[O.sub.3] .
These observations clearly showed that the MB molecules were adsorbed on the surface of the biomass obtained from the algae D. antarctica and that the active functional groups of the biomass that participated in the binding of the MB molecules were -OH, CO, C=O, and -COO- representing, respectively, hydroxyl group, inorganic carbonates, and cyclic anhydride and carboxylic groups .
31.2. Scanning Electron Microscopy. This analysis was carried out in order to obtain a view of the morphology of the biosorbent surface. The obtained micrographs are presented in Figure 2.
Using this technique, it was determined that the pores present in the surface of the biomass are homogeneously distributed; however, there are areas in the surface that are not porous, so it is valid to say that a percentage of the porosity is distributed heterogeneously and it is worth mentioning. In addition, the MB adsorption process did not modify the surface of the biomass. In Figure 2(a), a part of the nonporous surface of the biomass is observed, while in Figure 2(b), the porous part of the biomass is observed, which retained its texture after the MB adsorption process. This is attributed mainly to the size of the methylene blue molecule, which is 0.84 nm , since each molecule of this contaminant interacts with a single active site present on the surface of the biomass; therefore, the pores of the biomass, having a diameter size greater than 50 [micro]m, were not blocked during the biosorption process.
3.2. Determination of the Optimum pH for the Adsorption of Methylene Blue. The effect of pH on the adsorption of dyes is an important parameter. In Figure 3, the capacity of adsorption of MB by the biomass increased significantly when changing the pH value from 3 to 5, and this value was kept constant up to a basic pH corresponding to 11.
The chemical surface of an adsorbent has a great influence on the adsorption of an adsorbate, and this can be altered by modifying the initial pH value. Some authors have reported that, at low pH values, there is an electrostatic repulsion between the surface of the positively charged adsorbent and the cationic MB molecules, which inhibits the adsorption of this contaminant [4, 37, 43], because the ions of hydrogen compete with the MB molecule for the adsorption sites. As the pH increases, the surface of the biomass acquires a negative charge and a deprotonation of the surface is carried out which facilitates the adsorption of MB and therefore the capacity of adsorption of this pollutant by the biomass increases . This is mainly because in the solution, the MB is positively charged; hence, its adsorption is more effective when the surface charge presents a negative value [44,45]. Therefore, it was considered that a pH value of 10 was appropriate for carrying out the kinetic experiments.
3.3. Kinetics Models. In Figure 4, the larger the value of the initial concentration of MB, the more drastic the decrease in the value of its concentration, and as the time elapses, the change in concentration is less noticeable. In the first 180 minutes, the decrease in the MB concentration in the samples whose initial concentration was 200, 150, and 100 ppm is quite fast because the MB concentration remained above 20 ppm. However, after this time and smaller MB concentration values, the concentration changes are less noticeable. This is corroborated when observing that the decrease of the concentration of the contaminant in the solution whose initial concentration was 25 ppm is slow, in comparison with the other solutions.
Different models were applied to the results obtained in the kinetics of MB adsorption on the surface of the biomass studied. The pseudo-first-order model can describe the initial phase and the progress of the adsorption process; the pseudo-second-order equation describes that the chemisorption controls the speed of this process; According to the intraparticle diffusion model, several mechanisms are involved in the adsorption process, and this process can be described in three steps: external surface adsorption, intraparticle diffusion that is the speed-limiting step, and the final equilibrium that is very fast .
Next, the order in which the studied kinetic models were adjusted to the bioadsorption data obtained experimentally is mentioned.
Pseudo-second-order > Elovich > film diffusion = pseudo-first-order > intraparticle diffusion > modified pseudo-first-order.
Figure 5 shows the pseudo-second-order and Elovich isotherms obtained by adjusting the data kinetic experiments to these models; as can be seen, both models have a high correlation and therefore can describe the adsorption mechanism of methylene blue on the surface of D. antarctica algae.
In Table 2, it is observed that regardless of the value of the initial concentration of MB in the range studied, all bioadsorption data were adjusted to the pseudo-second-order model, this being the only model in which all the values of [R.sub.2] were above 0.95. P or which the initial adsorption rate depends exponentially on the concentration of methylene blue. The fact that this process is accurately described by a pseudo-second-order model further indicates that film diffusion, intraparticle diffusion, and surface adsorption coexisted during the adsorption of MB on the surface of the biomass, all of which factors affected the adsorption process and influence that the adsorption kinetics present the best fit when applying this model .
Given that the pseudo-second-order model presented the best fit of the data obtained, the value of [q.sub.e] was determined, using this model; as can be seen in Table 2, the adsorption capacity values obtained experimentally are quite close to the values obtained theoretically.
The Elovich model presents the second best fit to the data obtained; this model occurs when the adsorption processes involve the chemisorption in the solid surface, and the speed of adsorption decreases with time due to the coverage of the surface layer . The other models studied have a lower adjustment to the data studied, so it cannot explain with the same reliability the adsorption process that is being carried out.
To determine with greater precision the adjustment of the data obtained to the pseudo-second-order and Elovich kinetic models, five types of additional errors were determined. Table 3 reports the model that presents the best fit according to the type of error determined and the value of the initial concentration of methylene blue.
Regardless of the error studied, the best adjustment to the initial concentrations of MB of 200, 150, and 50 ppm is given in the pseudo-second-order model, while at 100 and 25 ppm, the Elovich model presents the best correlation. It can be deduced that, at high initial concentrations, the obtained data are adjusted to the pseudo-second-order model given that the adsorption speed is related to the value of the initial concentration.
3.4. Bioadsorption Isotherms. Figure 6 shows the data of [C.sub.e] and [q.sub.e] obtained when determining the bioadsorption capacity of MB on the surface of the biomass obtained from the algae D. antarctica; in this figure, the graphs are obtained by adjusting the data of bioadsorption to the models of Freundlich, Langmuir, Redlich-Peterson, Sips, and Toth.
The best fit to the data obtained by the bioadsorption of MB on the surface of the biomass obtained from the algae D. antarctica is given by applying the Toth model, which indicates that the adsorption occurs on a heterogeneous surface that consists of multiple layers. This also agrees with the good fit presented by the kinetic data when applying the Elovich model since this model also describes the adsorption of the contaminant on a heterogeneous surface.
The values of the parameters obtained by adjusting the methylene blue adsorption data on the surface of D. antarctica biomass to the bioadsorption models studied are presented in Table 4.
The Langmuir model presented the second best fit to the data obtained in this biosorption process, and this equation is valid for systems where the biosorption occurs on a homogeneous surface.
The best fit to the obtained data is in a three-parameter model that describes that the adsorption occurs on a heterogeneous surface in multiple layers and in a model of two parameters that describe an adsorption process on a homogeneous surface. It is mainly due to the fact that the surface of the biomass has an irregular surface in which there are areas where the pores are homogeneously distributed and others in which the surface has no porosity; this agrees with the analysis of the SEM micrographs that were presented in Section 3.1.
The value of [Q.sub.e] when applying the Toth model is 702.91 mg/g. This shows that the capacity of bioadsorption of MB on the surface of the biomass is high in comparison with other works reported in the literature. The exponent of the isotherm of this model ([mathematical expression not reproducible]) is related to the heterogeneity of the surfaces, and if it is equal to unity, the Toth model is reduced to the Langmuir model . In these biosorption experiments, it was found that the value of this constant is 2.63; this value is different from one, which corroborates that this adsorption does not conform to the Langmuir model, and therefore, the majority of active sites are distributed heterogeneously. The Sips and Redlich-Peterson models are of three parameters and present characteristics of the models of Langmuir (homogeneous) and Freundlich (heterogeneous). The correlation coefficient when adjusting these statistical models to the bioadsorption data obtained was 0.873 and 0.989, respectively; these values are below the value of the correlation coefficient when applying the Toth and Langmuir models corresponding to 0.995 and 0.980, respectively. However, the value of [R.sup.2] when applying the Redlich-Peterson model is high, which suggests that the adsorption does not occur in an ideal monolayer, corroborating that this adsorption process occurred in multilayers as described by the Toth model.
Although the value of [R.sup.2] when applying the Sips model is small (0.873), the value of the constant ns corresponding to 0.266 is closer to zero than to one, which corroborates that most active sites on the surface of the biomass which are involved in this adsorption process are distributed heterogeneously.
The value of [R.sup.2] when applying the Freundlich model was 0.873. This value is small; however, it should be noted that the value of the constant [n.sub.f] when applying this model was 3.76, and according to the theory of this model, when the value of this constant is between 2 and 10, the adsorption capacity of the contaminant by the adsorbent is high . This statement is corroborated when comparing the values of the methylene blue adsorption capacity presented in Table 5 for some adsorbents reported in the literature and the biomass obtained from the algae D. antarctica.
The bioadsorption capacity of the contaminant on the surface of the biomass increases with increasing pH, always when working at acid pH value intervals. Since the MB solution is at basic pH values, the MB adsorption capacity remains constant; in addition to this, it was determined that, in initial MB concentrations above 400 ppm, the initial pH value of these solutions is basic, which is why it is necessary to make modifications of the pH value which increase the efficiency of this process.
The pseudo-second-order model presented the best fit to the data obtained from the adsorption kinetics of MB on the surface of the biomass obtained from algae D. antarctica, which shows that the adsorption speed of this process is proportional to the exponential form of the initial concentration of MB present in the solution and to the time that has elapsed since the beginning of this process, as long as it is not greater than 540 min.
The Toth model presented the best fit to the data obtained from bioadsorption. By this model, it was determined that the adsorption capacity of MB on the surface of the biomass is 702.9 mg/g; this demonstrates the high efficiency that this material possesses to adsorb this contaminant.
Some data used to support the findings of this study are included in the tables and graphs within the article. More data (Origin and Excel files, as well as unedited images) are available from the corresponding author upon request.
Conflicts of Interest
The authors declare that there are no conflicts of interest.
The authors thank the Framework Agreement between the Universidad de los Andes and the Universidad Nacional de Colombia and the act of agreement established between the Chemistry Departments of the two universities. The authors also appreciate the grant for the funding of research programs for Associate Professors, Full Professors, and Emeritus Professors, announced by the Faculty of Sciences of the Universidad de los Andes (Colombia), 11-28-2017, 2018-2019, according to the project "Thermodynamic Characterization of the Adsorption of Contaminants on Porous Adsorbents." This work was financed by the Department of Chemistry and the Faculty of Sciences of the Andes University.
 F. Marrakchi, W. A. Khanday, M. Asif, and B. H. Hameed, "Cross-linked chitosan/sepiolite composite for the adsorption of methylene blue and reactive orange 16," International Journal of Biological Macromolecules, vol. 93, pp. 1231-1239, 2016.
 S. Thakur, S. Pandey, and O. A. Arotiba, "Development of a sodium alginate-based organic/inorganic superabsorbent composite hydrogel for adsorption of methylene blue," Carbohydrate Polymers, vol. 153, pp. 34-46, 2016.
 D. Pathania, S. Sharma, and P. Singh, "Removal of methylene blue by adsorption onto activated carbon developed from Ficus carica bast," Arabian Journal of Chemistry, vol. 10, pp. S1445-S1451, 2017.
 F. Marrakchi, M. J. Ahmed, W. A. Khanday, M. Asif, and B. H. Hameed, "Mesoporous-activated carbon prepared from chitosan flakes via single-step sodium hydroxide activation for the adsorption of methylene blue," International Journal of Biological Macromolecules, vol. 98, pp. 233-239, 2017.
 M. Heidarizad and S. S. Sengor, "Synthesis of graphene oxide/ magnesium oxide nanocomposites with high-rate adsorption of methylene blue," Journal of Molecular Liquids, vol. 224, pp. 607-617, 2016.
 S. Aslam, J. Zeng, F. Subhan et al., "In situ one-step synthesis of [Fe.sub.3][O.sub.4]@MIL-100(Fe) core-shells for adsorption of methylene blue from water," Journal of Colloid and Interface Science, vol. 505, pp. 186-195, 2017.
 S. M. Miraboutalebi, S. K. Nikouzad, M. Peydayesh, N. Allahgholi, L. Vafajoo, and G. McKay, "Methylene blue adsorption via maize silk powder: kinetic, equilibrium, thermodynamic studies and residual error analysis," Process Safety and Environmental Protection, vol. 106, pp. 191-202, 2017.
 H. Aysan, S. Edebali, C. Ozdemir, M. Celik Karakaya, and N. Karakaya, "Use of chabazite, a naturally abundant zeolite, for the investigation of the adsorption kinetics and mechanism of methylene blue dye," Microporous and Mesoporous Materials, vol. 235, pp. 78-86, 2016.
 Q. Huang, M. Liu, J. Chen et al., "Marrying the mussel inspired chemistry and Kabachnik-Fields reaction for preparation of Si[O.sub.2] polymer composites and enhancement removal of methylene blue," Applied Surface Science, vol. 422, pp. 17-27, 2017.
 X.-P. Luo, S.-Y. Fu, Y.-M. Du, J.-Z. Guo, and B. Li, "Adsorption ofmethylene blue and malachite green from aqueous solution by sulfonic acid group modified MIL-101," Microporous and Mesoporous Materials, vol. 237, pp. 268-274,2017.
 F. Wang, L. Zhang, Y. Wang, X. Liu, S. Rohani, and J. Lu, "[Fe.sub.3][O.sub.4]@Si[O.sub.2]@CS-TETA functionalized graphene oxide for the adsorption of methylene blue (MB) and Cu(II)," Applied Surface Science, vol. 420, pp. 970-981, 2017.
 N. Tahir, H. N. Bhatti, M. Iqbal, and S. Noreen, "Biopolymers composites with peanut hull waste biomass and application for Crystal Violet adsorption," International Journal of Biological Macromolecules, vol. 94, pp. 210-220, 2017.
 H. Cid, C. Ortiz, J. Pizarro et al., "Characterization of copper (II) biosorption by brown algae Durvillaea antarctica dead biomass," Adsorption, vol. 21, no. 8, pp. 645-658, 2015.
 M. A. Hossain, H. H. Ngo, W. S. Guo, and T. Setiadi, "Adsorption and desorption of copper(II) ions onto garden grass," Bioresource Technology, vol. 121, pp. 386-395, 2012.
 H. I. Inyang, A. Onwawoma, and S. Bae, "The Elovich equation as a predictor of lead and cadmium sorption rates on contaminant barrier minerals," Soil and Tillage Research, vol. 155, pp. 124-132, 2016.
 S. Lagergren, "About the theory of so-called adsorption of soluble substances, Kungliga Svenska Vetenskapsakad," Handlingar, vol. 24, pp. 1-39, 1898.
 Y. S. Ho and G. McKay, "Pseudo-second order model for sorption processes," Process Biochemistry, vol. 34, no. 5, pp. 451-465, 1999.
 J.-P. Simonin, "On the comparison of pseudo-first order and pseudo-second order rate laws in the modeling of adsorption kinetics," Chemical EngineeringJournal, vol. 300, pp. 254-263, 2016.
 A. E. Rodrigues and C. M. Silva, "What's wrong with Lagergreen pseudo first order model for adsorption kinetics?," Chemical Engineering Journal, vol. 306, pp. 1138-1142, 2016.
 A. E. Ofomaja, E. B. Naidoo, and S. J. Modise, "Dynamic studies and pseudo-second order modeling of copper(II) biosorption onto pine cone powder," Desalination, vol. 251, no. 1-3, pp. 112-122, 2010.
 X. Yang and B. Al-Duri, "Kinetic modeling of liquid-phase adsorption of reactive dyes on activated carbon," Journal of Colloid and Interface Science, vol. 287, no. 1, pp. 25-34, 2005.
 M. Baghdadi, "UT (University of Tehran) isotherm as a novel and useful adsorption isotherm for investigation of adsorptive removal of pollutants," Journal of Environmental Chemical Engineering, vol. 5, no. 2, pp. 1906-1919, 2017.
 C. Rill, Z. I. Kolar, G. Kickelbick, H. T. Wolterbeek, and J. A. Peters, "Kinetics and thermodynamics of adsorption on hydroxyapatite of the [160Tb] terbium complexes of the bone-targeting ligands DOTP and BPPED," Langmuir, vol. 25, no. 4, pp. 2294-2301, 2009.
 H. Uslu and S. Majumder, "Adsorption studies of lactic acid by polymeric adsorbent amberlite XAD-7: equilibrium and kinetics," Journal of Chemical & Engineering Data, vol. 62, no. 4, pp. 1501-1506, 2017.
 H. Zhang, Y. Wang, P. Bai, X. Guo, and X. Ni, "Adsorptive separation of acetic acid from dilute aqueous solutions: adsorption kinetic, isotherms, and thermodynamic studies," Journal of Chemical & Engineering Data, vol. 61, no. 1, pp. 213-219, 2015.
 J. Chen, H. Yang, and Z. Ring, "Study of intra-particle diffusion effect on hydrodesulphurization of dibenzothiophenic compounds," Catalysis Today, vol. 109, no. 1-4, pp. 93-98, 2005.
 A. Okoye, P. Ejikeme, and O. Onukwuli, "Lead removal from wastewater using fluted pumpkin seed shell activated carbon: adsorption modeling and kinetics," International Journal of Environmental Science & Technology, vol. 7, no. 4, pp. 793800, 2010.
 E. M. Kalhori, T. J. Al-Musawi, E. Ghahramani, H. Kazemian, and M. Zarrabi, "Enhancement of the adsorption capacity of the light-weight expanded clay aggregate surface for the metronidazole antibiotic by coating with MgO nanoparticles: studies on the kinetic, isotherm, and effects of environmental parameters," Chemosphere, vol. 175, pp. 8-20, 2017.
 N. Barka, K. Ouzaouit, M. Abdennouri, and M. E. Makhfouk, "Dried prickly pear cactus (Opuntia ficus indica) cladodes as a low-cost and eco-friendly biosorbent for dyes removal from aqueous solutions," Journal of the Taiwan Institute of Chemical Engineers, vol. 44, no. 1, pp. 52-60, 2013.
 M. Brdar, M. Sciban, A. Takaci, and T. Dosenovic, "Comparison of two and three parameters adsorption isotherm for Cr(VI) onto Kraft lignin," Chemical Engineering Journal, vol. 183, pp. 108-111, 2012.
 G. McKay, A. Mesdaghinia, S. Nasseri, M. Hadi, and M. Solaimany Aminabad, "Optimum isotherms of dyes sorption by activated carbon: fractional theoretical capacity & error analysis," Chemical Engineering Journal, vol. 251, pp. 236-247, 2014.
 F. Deniz and E. T. Ersanli, "Simultaneous bioremoval of two unsafe dyes from aqueous solution using a novel green composite biosorbent," Microchemical Journal, vol. 128, pp. 312-319, 2016.
 S. Chatterjee, M. W. Lee, and S. H. Woo, "Adsorption of congo red by chitosan hydrogel beads impregnated with carbon nanotubes," Bioresource Technology, vol. 101, no. 6, pp. 1800-1806, 2010.
 A. Bera, T. Kumar, K. Ojha, and A. Mandal, "Adsorption of surfactants on sand surface in enhanced oil recovery: isotherms, kinetics and thermodynamic studies," Applied Surface Science, vol. 284, pp. 87-99, 2013.
 S. Rangabhashiyam, N. Anu, M. S. Giri Nandagopal, and N. Selvaraju, "Relevance of isotherm models in biosorption of pollutants by agricultural byproducts," Journal of Environmental Chemical Engineering, vol. 2, no. 1, pp. 398-414, 2014.
 D.-q Li, J. Wang, Z.-g Guo, J. Li, and J. Shuai, "Pectin gels cross-linked by [Ca.sup.2+]: an efficient material for methylene blue removal," Journal of Molecular Liquids, vol. 238, pp. 36-42, 2017.
 J. Pang, F. Fu, Z. Ding, J. Lu, N. Li, and B. Tang, "Adsorption behaviors of methylene blue from aqueous solution on mesoporous birnessite," Journal of the Taiwan Institute of Chemical Engineers, vol. 77, pp. 168-176, 2017.
 F. Marrakchi, M. Auta, W. A. Khanday, and B. H. Hameed, "High-surface-area and nitrogen-rich mesoporous carbon material from fishery waste for effective adsorption of methylene blue," Powder Technology, vol. 321, pp. 428-434, 2017.
 S. Anisuzzaman, C. G. Joseph, D. Krishnaiah, A. Bono, and L. Ooi, "Parametric and adsorption kinetic studies of methylene blue removal from simulated textile water using durian (Durio zibethinus Murray) skin," Water Science and Technology, vol. 72, no. 6, pp. 896-907, 2015.
 D. L. Postai, C. A. Demarchi, F. Zanatta, D. C. C. Melo, and C. A. Rodrigues, "Adsorption of rhodamine B and methylene blue dyes using waste of seeds of Aleurites moluccana, a low cost adsorbent," Alexandria Engineering Journal, vol. 55, no. 2, pp. 1713-1723, 2016.
 A. Naskar and R. Majumder, "Understanding the adsorption behaviour of acid yellow 99 on Aspergillus niger biomass," Journal of Molecular Liquids, vol. 242, pp. 892-899, 2017.
 L. Giraldo, V. Garcia, and J. C. Moreno, "Caracterizacion superficial en fase gas y liquida de carbones activados," Revista de Ingenieria, vol. 27, pp. 07-16, 2008.
 R. Pandimurugan and S. Thambidurai, "Synthesis of seaweed-ZnO-PANI hybrid composite for adsorption of methylene blue dye," Journal of Environmental Chemical Engineering, vol. 4, no. 1, pp. 1332-1347, 2016.
 S. Zhang, Z. Wang, Y. Zhang, H. Pan, and L. Tao, "Adsorption of methylene blue on organosolv lignin from rice straw," Procedia Environmental Sciences, vol. 31, pp. 3-11, 2016.
 W. Gao, S. Zhao, H. Wu, W. Deligeer, and S. Asuha, "Direct acid activation of kaolinite and its effects on the adsorption of methylene blue," Applied Clay Science, vol. 126, pp. 98-106, 2016.
 L.-g. Yan, L.-l. Qin, H.-q. Yu, S. Li, R.-r. Shan, and B. Du, "Adsorption of acid dyes from aqueous solution by CTMAB modified bentonite: kinetic and isotherm modeling," Journal of Molecular Liquids, vol. 211, pp. 1074-1081, 2015.
 S. Fan, Y. Wang, Z. Wang, J. Tang, J. Tang, and X. Li, "Removal of methylene blue from aqueous solution by sewage sludge-derived biochar: adsorption kinetics, equilibrium, thermodynamics and mechanism," Journal of Environmental Chemical Engineering, vol. 5, no. 1, pp. 601-611, 2017.
 J. S. Piccin, G. L. Dotto, M. L. Vieira, and L. A. Pinto, "Kinetics and mechanism of the food dye FD&C Red 40 adsorption onto chitosan," Journal of Chemical & Engineering Data, vol. 56, no. 10, pp. 3759-3765, 2011.
 M. A. Islam, M. J. Ahmed, W. A. Khanday, M. Asif, and B. H. Hameed, "Mesoporous activated coconut shell-derived hydrochar prepared via hydrothermal carbonization-NaOH activation for methylene blue adsorption," Journal of Environmental Management, vol. 203, pp. 237-244, 2017.
 P. Chen, Z.-f. Cao, X. Wen et al., "In situ nano-silicate functionalized graphene oxide composites to improve MB removal," Journal of the Taiwan Institute of Chemical Engineers, vol. 81, pp. 87-94, 2017.
 G. Wang, S. Wang, Z. Sun, S. Zheng, and Y. Xi, "Structures of nonionic surfactant modified montmorillonites and their enhanced adsorption capacities towards a cationic organic dye," Applied Clay Science, vol. 148, pp. 1-10, 2017.
 X. Yang, H. Liu, F. Han, S. Jiang, L. Liu, and Z. Xia, "Fabrication of cellulose nanocrystal from Carex meyeriana Kunth and its application in the adsorption of methylene blue," Carbohydrate Polymers, vol. 175, pp. 464-472, 2017.
 Z. Anfar, R. El Haouti, S. Lhanafi, M. Benafqir, Y. Azougarh, and N. El Alem, "Treated digested residue during anaerobic co-digestion of Agri-food organic waste: methylene blue adsorption, mechanism and CCD-RSM design," Journal of Environmental Chemical Engineering, vol. 5, no. 6, pp. 5857-5867, 2017.
 M. Yang, X. Liu, Y. Qi, W. Sun, and Y. Men, "Preparation of K-carrageenan/graphene oxide gel beads and their efficient adsorption for methylene blue," Journal of Colloid and Interface Science, vol. 506, pp. 669-677, 2017.
 V. J. Vilar, C. M. Botelho, and R. A. Boaventura, "Methylene blue adsorption by algal biomass based materials: biosorbents characterization and process behaviour," Journal of hazardous materials, vol. 147, no. 1-2, pp. 120-132, 2007.
 T. S. Chandra, S. Mudliar, S. Vidyashankar et al., "Defatted algal biomass as a non-conventional low-cost adsorbent: surface characterization and methylene blue adsorption characteristics," Bioresource technology, vol. 184, pp. 395-404, 2015.
 H. Shao, Y. Li, L. Zheng, T. Chen, and J. Liu, "Removal of methylene blue by chemically modified defatted brown algae Laminaria japonica," Journal of the Taiwan Institute of Chemical Engineers, vol. 80, pp. 525-532, 2017.
Jhonatan R. Guarin, (1) Juan Carlos Moreno-Pirajan (iD), (1) and Liliana Giraldo (2)
(1) Department of Chemistry, Sciences Faculty, Research Group in Porous Solids and Calorimetry, University of the Andes, Bogota 111711, Colombia
(2) Departamento de Qumica, Facultad de Ciencias, Universidad Nacional de Colombia, Bogota 111321, Colombia
Correspondence should be addressed to Juan Carlos Moreno-Pirajan; firstname.lastname@example.org
Received 9 March 2018; Revised 17 April 2018; Accepted 22 April 2018; Published 14 June 2018
Academic Editor: Carlos A. Martinez-Huitle
Caption: Figure 1: Infrared spectrum of the biomass of D. antarctica before and after the bioadsorption of MB.
Caption: Figure 2: SEM micrographs of the biomass (a) before and (b) after the biosorption process of MB.
Caption: Figure 3: Effect of pH on bioadsorption of MB on the surface of the biomass of D. antarctica.
Caption: Figure 4: Effect of the concentration on the adsorption speed of MB on the surface of the biomass of D. antarctica.
Caption: Figure 5: Result of applying the kinetic models used in the adsorption of MB on the surface of the biomass: (a) modified pseudo-first-order model; (b) Elovich model.
Caption: Figure 6: Bioadsorption models of methylene blue in D. antarctica biomass at 18 hours.
Table 1: The names and equations of applied error functions . Error function Definition Equation RMSE [square root of ((1/n-2) (9) [[summation].sup.N.sub.I=1] [([q.sub.e,exp] - [q.sub.e,isotherm]).sup.2])] [X.sup.2] [X.sup.2] = [[summation].sup.N.sub.1] (10) [([q.sub.e,exp] - [q.sub.e,isotherm]).sup.2]/ [q.sub.e,isotherm] ERRSQ [[summation].sup.N.sub.i=1] (11) [([q.sub.e,exp] - [q.sub.e,isotherm]).sup.2.sub.i] HYBRD [[summation].sup.N.sub.i=1] (12) ][[([q.sub.e,exp] - [q.sub.e,isotherm]).sup.2]/ [q.sub.e,exp]].sub.i] MPSD [[summation].sup.N.sub.i=1] (13) [[(([q.sub.e,exp] - [q.sub.e,isotherm]).sup.2]/ [q.sub.e,exp])].sup.2.sub.i] Table 2: Adsorption kinetic parameters obtained by adsorption of MB onto D. antarctica. Kinetic model Initial concentration of MB (mg/L) Parameter r 25 50 Pseudo-first-order [K.sub.1] 0.00967 0.00783 [R.sup.2] 0.986 0.952 Pseudo-second-order [K.sub.2] 0.00178 0.000287 [q.sub.e], exp. 22.565 41.221 [q.sub.e], cal. 22.402 40.003 [R.sup.2] 0.999 0.972 Modified pseudo-first-order [K.sub.m] 0.008 0.0059 [R.sup.2] 0.985 0.875 Elovich [alpha] 3.908 1.634 [beta] 0.272 0.122 [R.sup.2] 0.991 0.943 Intraparticle diffusion [k.sub.I] 4.547 2.212 [R.sup.2] 0.963 0.996 Film diffusion A 0.346 0.0591 [k.sub.f] 0.0097 0.0078 [R.sup.2] 0.986 0.952 Kinetic model Initial concentration of MB (mg/L) Parameter r 100 150 Pseudo-first-order [K.sub.1] 0.00967 0.00921 [R.sup.2] 0.893 0.937 Pseudo-second-order [K.sub.2] 0.000385 0.000234 [q.sub.e], exp. 87.754 141.763 [q.sub.e], cal. 86.024 140.955 [R.sup.2] 0.995 0.999 Modified pseudo-first-order [K.sub.m] 0.0081 0.0074 [R.sup.2] 0.839 0.971 Elovich [alpha] 15.783 11.672 [beta] 0.0733 0.0356 [R.sup.2] 0.992 0.967 Intraparticle diffusion [k.sub.I] 17.519 13.766 [R.sup.2] 0.949 0.914 Film diffusion A 0.212 0.416 [k.sub.f] 0.0096 0.0092 [R.sup.2] 0.893 0.937 Kinetic model Initial concentration of MB (mg/L) Parameter r 200 Pseudo-first-order [K.sub.1] 0.00990 [R.sup.2] 0.992 Pseudo-second-order [K.sub.2] 0.0000730 [q.sub.e], exp. 191.294 [q.sub.e], cal. 196.349 [R.sup.2] 0.994 Modified pseudo-first-order [K.sub.m] 0.0078 [R.sup.2] 0.991 Elovich [alpha] 7.450 [beta] 0.0224 [R.sup.2] 0.970 Intraparticle diffusion [k.sub.I] 3.259 [R.sup.2] 0.897 Film diffusion A 0.0664 [k.sub.f] 0.01 [R.sup.2] 0.992 Table 3: Kinetic model that presents the best adjustment according to the initial concentration of MB and the type of error determined. Error function Initial concentration of MB (mg/L) 25 50 100 RMSE Elovich Pseudo-second-order Elovich [X.sup.2] Elovich Pseudo-second-order Elovich ERRSQ Elovich Pseudo-second-order Elovich HYBRD Elovich Pseudo-second-order Elovich MPSD Elovich Pseudo-second-order Elovich Error function Initial concentration of MB (mg/L) 150 200 RMSE Pseudo-second-order Pseudo-second-order [X.sup.2] Pseudo-second-order Pseudo-second-order ERRSQ Pseudo-second-order Pseudo-second-order HYBRD Pseudo-second-order Pseudo-second-order MPSD Pseudo-second-order Pseudo-second-order Table 4: Parameters of the models of the Freundlich, Redlich-Peterson, Sips, and Toth isotherms for the adsorption of MB on the surface of D. antarctica. Models Parameters MB Freundlich [K.sub.f] 148.309 [n.sub.f] 3.762 [R.sup.2] 0.873 Langmuir [Q.sub.m] 765.750 K 0.064 [R.sup.2] 0.980 Redlich-Peterson [K.sub.RP] 38.133 [[alpha].sub.RP] 0.022 g 1.139 [R.sup.2] 0.989 Sips [Q.sub.m] 148.311 [K.sub.s] -31.367 [n.sub.s] 0.266 [R.sup.2] 0.873 Toth [Q.sub.m] 702.911 [mathematical expression not 3735.703 reproducible] [mathematical expression not 2.633 reproducible] [R.sup.2] 0.995 Table 5: Comparison of the adsorption capacity of MB on the surface of the biomass obtained from the algae D. antarctica and other compounds. Compound [q.sub.e] T ([degrees]C) (mg/g) Mesoporous activated carbon 200.0 30 GO/silicates 230 20 Nonionic surfactant modified 740.7 25 montmorillonite [Fe.sub.3][O.sub.4]@Si[O.sub.2]@CS- 529.1 30 TETA-GO Cellulose nanocrystal 217.4 30 TDAW 285.7 25 [kappa]-carrageenan/graphene oxide gel 658.4 25 beads Chitosan flakes 143.5 50 Algae Gelidium 171 Defatted algal biomass 7.8 25 Defatted Laminaria japonica biomass 549.45 35 modified by sulfuric acid Durvillaea antarctica 702.9 25 Compound Concentration range (mg/L) Mesoporous activated carbon 25-250 GO/silicates 40-120 Nonionic surfactant modified 100 montmorillonite [Fe.sub.3][O.sub.4]@Si[O.sub.2]@CS- 1000 TETA-GO Cellulose nanocrystal 50-400 TDAW 40-1000 [kappa]-carrageenan/graphene oxide gel 100-800 beads Chitosan flakes 25-400 Algae Gelidium 40-800 Defatted algal biomass 1-5 Defatted Laminaria japonica biomass 20-250 modified by sulfuric acid Durvillaea antarctica 25-1400 Compound Time (min) Reference Mesoporous activated carbon 1440  GO/silicates 100  Nonionic surfactant modified 180  montmorillonite [Fe.sub.3][O.sub.4]@Si[O.sub.2]@CS- 20  TETA-GO Cellulose nanocrystal 300  TDAW 120  [kappa]-carrageenan/graphene oxide gel 1440  beads Chitosan flakes 420  Algae Gelidium 160  Defatted algal biomass 60  Defatted Laminaria japonica biomass 60  modified by sulfuric acid Durvillaea antarctica 540 This work
|Printer friendly Cite/link Email Feedback|
|Title Annotation:||Research Article|
|Author:||Guarin, Jhonatan R.; Moreno-Pirajan, Juan Carlos; Giraldo, Liliana|
|Publication:||Journal of Chemistry|
|Date:||Jan 1, 2018|
|Previous Article:||Optimization of Preparation Conditions of Novel Adsorbent from Sugar Scum Using Response Surface Methodology for Removal of Methylene Blue.|
|Next Article:||Critical Effects of Smoking Parameters on the Levels of Polycyclic Aromatic Hydrocarbons in Traditionally Smoked Fish and Meat Products in Finland.|