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Banana Fibers as Sorbent for Removal of Acid Green Dye from Water.

1. Introduction

There are various industries that use dyes as colouring agents, such as textile, paint, pharmaceuticals, beauty products, and food. The release of dyes to water is harmful to the aquatic lives as most dyes are complex in nature and of synthetic origin [1]. Moreover, dyes hinder sunlight from entering water and slowing photosynthesis for plants in water [2]. Some of the techniques used to treat dye-containing wastewater are Fenton oxidation, membrane filtration, photodegradation, coagulation-flocculation, biosorption, and adsorption [3-10]. Ease of use, low energy application, and simple operation are some of the advantages of using membrane and coagulation-flocculation [6, 7]. The drawbacks include searching for the right coagulants to maximize the process and membrane fouling. Chemical processes such as oxidation have high efficiency, though the high cost and disposal pose concern on the treatment process [11]. Adsorption is a physical process and has the advantages of simplicity, easy usage, and low energy consumption, similar to membrane and coagulation-flocculation [12]. The use of natural fibers as sorbents is an attractive option, as it is biodegradable and low cost.

The use of natural fibers has been studied over a wide range of water pollutants. The sorbents are used in natural or unmodified form, as activated carbon, as biochar, or modified with other chemicals. Modification of natural fibers as activated carbon has been demonstrated using pineapple waste [2], where the surface area of activated carbon was higher than 500 [m.sup.2]/g and the maximum adsorption capacity was found to be 288mg/g for adsorption of methylene blue. Biochar activated with microwave treatment was performed on P. juliflora species [13], where the surface area of adsorbents used was between 220 and 330 [m.sup.2]/g, and the maximum adsorption capacity increased compared to the non-microwave-treated biochar. The use of unmodified and modified-by-calcination rice bran revealed that calcination at high temperature had an adverse effect on the adsorption capacity of the adsorbents [1]. Using methylene blue and crystal violet dyes as model compounds, the adsorption capacity for uncalcined and calcined rice bran decreased from 325.9 to 172.5 mg/g and from 783.8 to 401.3 mg/g, respectively. The use of modification for natural fibers has to take into account the cost and environmental effects, as opposed to the increase (or decrease) in adsorption capacity.

Therefore, in this study, the natural form of banana is chosen as adsorbent. The banana plant used is taken from three parts of banana, which are the leaves, stem, and stalk. The three parts are used to remove acid green (AG) dye in aqueous solution.

2. Materials and Methods

2.1. Materials. The AG dye was purchased from Acros Organics. Analytical grade sodium hydroxide from Systerm (Malaysia) and 70.0% nitric acid from J.T. Baker (USA) were used to adjust the pH of solution. The acid and base were prepared at a concentration of 0.1 M. The sorbents were prepared by using banana plants collected from Samarahan, Sarawak, Malaysia. The dye stock solution of 10000 ppm was prepared by adding 10 g of the AG dye powder in 1000 mL of deionised water. The stock solution was diluted to the desired AG dye concentrations for experimental usage.

2.2. Preparation of Banana Fiber Sorbents. Three different parts of banana plant were used to prepare the sorbents, which were the leaves, stem, and stalk. The plants were scraped and the fibers extracted from the different parts. Next, the extracted fibers were cut to about 2 cm before they were washed several times with deionised water. The drying took place next, with room temperature drying for three days and oven drying at 60[degrees]C for 24 hours. After drying, the banana parts were ground and sieved using 500-micron mesh size. The prepared sorbents were then stored in dry, airtight containers before use.

2.3. Batch Adsorption Experiments. In kinetic study, the experimental conditions were temperature at 25[degrees]C, agitation speed of 200 rpm, adsorbent dosage of 60 g/L, and initial pH 2. The AG dye concentrations were varied at 750, 1000, and 1500 ppm. The experiments were carried out at predetermined experimental contact time, varying from 1 minute to 3 hours. After the predetermined contact time, the samples were filtered and the residual solutions were analysed using UV-Vis spectrophotometer (Thermo Scientific, model Evolution 201) at 624 nm of [[lambda].sub.max].

Adsorption isotherm study for the batch adsorption experiments was conducted at 25[degrees] C with agitation speed of 200 rpm, adsorbent dosage of 60 g/L, contact time of 3 hours, and initial solution pH of approximately 2. The initial AG dye concentrations were varied from 100 ppm to 2000 ppm. After 3 hours of experimental contact time, the samples were filtered and the residual solutions were analysed using the UV-Vis spectrophotometer at 624 nm of [[lambda].sub.max].

The solution pH effect study was performed for initial AG dye concentration of 1000 ppm at operating temperature of 25[degrees]C with agitation speed of 200 rpm, adsorbent dosage of 60 g/L, and total experimental contact time of 3 hours. The initial solution pH was varied between 2 and 12. After 3 hours of experimental contact time, the samples were filtered and the residual solutions were analysed using UV-Vis spectrophotometer (Thermo Scientific, model Evolution 201) at 624 nm of [[lambda].sub.max].

Each batch experiment was carried out in duplicate and theaverage valuewas tabulatedingraph form. Thepercentage removal was calculated using the following formula:

% removal = [C.sub.0] - [C.sub.t]/[C.sub.0] x 100%, (1)

where [C.sub.0] is the initial concentration and [C.sub.t] is the concentration at time interval.

The adsorption capacity, Q, was calculated using

Q = ([C.sub.0] - [C.sub.t])V/m, (2)

where [C.sub.0] is the initial concentration, [C.sub.t] is the concentration at time interval, V is the volume of solution used, and m is the mass of sorbent.

2.4. Characterisation of the Sorbents. The sorbents were characterised using scanning electron microscopy (SEM) (JEOL Analytical Scanning Microscope, model JSM-6390LA) to visualise the surface morphologies of the sorbents and Fourier Transform Infrared (FT-IR) to analyse the surface functional groups of the sorbents. The FT-IR spectra were recorded using Shimadzu ASC 7000 Autosampler in the range of 400-4000 [cm.sup.-1] with a resolution of 4 [cm.sup.-1].

3. Results and Discussion

3.1. Kinetic Batch Experiments. The interaction between sorbent and sorbate is generally seen in the contact time needed to remove the sorbate from water. The adsorption capacities of the three banana sorbents at different contact time were illustrated in Figure 1. In general, the adsorption capacity increases rapidly in the first 15 minutes and then increases gradually when nearing the equilibrium stage before becoming near constant at equilibrium. The rapid increase in adsorption at the initial stage is due to the availability of sorption sites. As the sorption sites are filled, the sorption becomes slower and causes the smaller increase in adsorption capacity. At equilibrium, the sorption sites are fully occupied with sorbate or there is nearly no sorbate to interact with. At different initial concentrations, the adsorption capacity is seen to increase with the increase in initial concentration. This can be attributed to the higher concentration difference, which can provide stronger driving force. For banana leaves sorbent, the adsorption capacities at 750, 1000, and 1500 ppm are 9.48, 11.01, and 18.40 mg/g, respectively. Lower adsorption capacities are found for banana stem sorbent (8.03, 10.54, and 17.02 mg/g) and banana stalk sorbent (7.28, 10.39, and 15.33 mg/g). Furthermore, at higher initial concentrations, longer contact time is needed to achieve equilibrium as there are higher amount of sorbates. At 1500 ppm for banana leaves, the equilibrium is achieved after 90 minutes, whereas the equilibrium is achieved after 25 minutes at 1000 ppm. Similar trend is exhibited with banana stem and banana stalk sorbents. At higher initial concentrations, there are more sorbate molecules to be sorbed. Therefore, longer time is needed to achieve the equilibrium state. Nevertheless, the sorption will be constant after equilibrium, indicating the saturation of sorption sites even with higher amount of sorbates. The equilibrium time for acid green dye was also found to be under 90 minutes using the Fenton method [5] and photodegradation with cobalt impregnated ZSM-5 catalyst [14].

3.2. The Effect of pH. Figure 2 shows the AG dye adsorption is greatly influenced by the acidic nature of solution. At highly acidic condition, with initial solution pH at approximately 2, the banana leaves, stem, and stalk sorbents produce the highest adsorption capacity of 28.7 mg/g, 18.5 mg/g, and 18.3 mg/g, respectively. For banana leaves and stalk sorbents, the adsorption capacity decreases to a constant value over a large range of initial solution pH (3 to 11). It can be seen in Figure 3 that, for these two sorbents, the final solution pH is equilibrated at around 6 for initial pH between 3 and 11, which explains why the adsorption capacity values became constant. For banana stem sorbent, the adsorption capacity is steadily decreasing as the solution pH increased. This could be due to the higher buffering value for this sorbent, which is at solution pH of 8 and 10. As this solution pH is basic, it gives a negative effect to the AG dye adsorption using the banana stem sorbent. The solution pH influences the interaction between the surface of the sorbent and the adsorbate [15, 16]. The AG dye is an anionic dye, and highly positive surface charge at initial solution pH 2 attracts the negative S[O.sub.3.sup.-] functional group in the AG dye.

3.3. Adsorption Kinetics. The data from the kinetic experiments was further analysed and fitted to kinetic model equations. The best fit model was selected based on correlation of coefficients, where higher correlation gives the best fit model to the kinetic data. Several kinetic models were used to model the rate of adsorption of AG dye on banana leaves, stem, and stalk sorbents.

The pseudo-first-order kinetic equation describes adsorption rate based on adsorption capacities, where it assumes that one adsorbate molecule is adsorbed onto one active site [16]. The linear pseudo-first-order equation is given as

ln ([q.sub.e] - [q.sub.t]) = ln [q.sub.e] - [k.sub.1]t, (3)

where [q.sub.e] and [q.sub.t] are the adsorption capacity of sorbent (mg/g) at equilibrium and time t, respectively. The pseudo-first-order rate constants [k.sub.1] ([min.sup.-1]) are determined from the slope of this equation.

Meanwhile, the pseudo-second-order equation is also used to describe adsorption rate based on adsorption capacities [17]. In this equation, one adsorbate molecule is assumed to be held onto two active sites. The linear form of this equation is given by

t/[q.sub.t] = 1/[k.sub.2][q.sup.2.sub.e] + [1/[q.sub.e]] t, (4)

where [q.sub.e] and [q.sub.t] are the adsorption capacity of sorbent (mg/g) at equilibrium and time t, respectively. The pseudo-second-order rate constants, [k.sub.2] (g/mg x min), are determined based on the slope of the equation.

The intraparticle diffusion model is used to explain the kinetics when pore diffusion is controlling the adsorption process. A common equation used to describe intraparticle diffusion is the Dunwald-Wagner equation:

log (1-[([q.sub.t]/[q.sub.e]).sup.2]) = -[k.sub.DW]t. (5)

The intraparticle diffusion equation will be crossing the origin if it is the only step that control the rate of adsorption [18, 19]. The parameters involved in the kinetic equations and the regression coefficients ([R.sup.2]) are given in Table 1.

The kinetics data fitted very well into the pseudo-second-order model, with the correlation coefficient, [R.sup.2], of more than 0.94 for all three sorbents. This indicates that sorption of AG dye on banana stem, stalk, and leaves sorbents may be controlled by chemisorption, through sharing of valence forces or ion exchange. The pseudo-first-order kinetic equation has lower [R.sup.2] values than pseudo-second-order one, although the correlation is still considered good with [R.sup.2] > 0.80. The pseudo-first-order plots in Figure 4 show the nonlinearity of sorption using the three sorbents at 750 and 1000 ppm. Moreover, calculated adsorption capacities using pseudo-first-order equation are not satisfactory in representing the experimental data compared to pseudo-second-order equation. Based on the pseudo-second-order plots in Figure 5, the experimental data conforms to the linear form of the equation well. The pseudo-second-order kinetics fits well with most systems of dye adsorption using natural fibers, such as adsorption of methylene blue and direct red using garlic straw [20, 21], adsorption of crystal violet dye using sugarcane bagasse [11], removal of tartrazine using Lantana camara [22], crystal violet dye removal using papaya seed [23], and adsorption of navy blue using powdered orange [24]. Comprehensive review on pseudo-second-order model has demonstrated that this model is clearly advantageous in predicting adsorption of pollutants in aqueous solution, as there is no need to know the equilibrium capacity from the experiment, as it can be calculated from the model [25]. The intraparticle diffusion model has similar correlation coefficient values with pseudo-first-order model, with [R.sup.2] > 0.80. Based on Figure 6, the linear line for the equation does not cross the origin, indicating that the intraparticle diffusion is not the primary rate-controlling step.

3.4. Adsorption Isotherm. Four isotherm equations were chosen to represent the adsorption of AG dye onto banana stem, stalk, and leaves sorbents. The isotherm experiments data were fitted with four isotherm equations, namely, Langmuir, Freundlich, Dubinin-Radushkevich, and Temkin.

The assumptions of Langmuir isotherm were homogeneous adsorption sites, where a single layer of adsorption occurs [26, 27]. Since the adsorption occurs in a monolayer, there are no further adsorption once the active site is occupied. The linear form of this model is written as

[C.sub.e]/[Q.sub.e] = 1/[Q.sub.m][K.sub.L] + [C.sub.e]/[Q.sub.m], (6)

where [C.sub.e] is the equilibrium concentration (mg/L), [Q.sub.e] is the equilibrium adsorption capacity (mg/g), [Q.sub.m] is the maximum adsorption capacity (mg/g), and [K.sub.L] is the Langmuir isotherm constant (L/mg). An important dimensionless constant that can be extracted from Langmuir isotherm is called the separation factor, [R.sub.L]. [R.sub.L] is a dimensionless constant that indicates whether the adsorption is favourable (0 < [R.sub.L] < 1), unfavourable ([R.sub.L] > 1), linear ([R.sub.L] = 1), or irreversible ([R.sub.L] = 0). [R.sub.L] can be expressed as

[R.sub.L] = 1/1 + [K.sub.L][C.sub.0], (7)

On the other hand, the Freundlich isotherm model was more commonly applied to explain adsorption that occurs in multiple layers, and there is interaction between adsorbed molecules [2, 27]. Unlike the Langmuir model, the adsorption sites in Freundlich model were heterogeneous, with the adsorption energy that declines exponentially as it nears the adsorption centers. The 1/n values indicate the degree of linearity of adsorption. When 1/n value is between 0 and 1, there exists some nonlinearity in the relationship between the solution concentration and adsorption. When 1/n value is 1, the adsorption is linear. The linear form of Freundlich isotherm is given as

ln [Q.sub.e] - ln [K.sub.F] + [1/n] ln [C.sub.e], (8)

where [C.sub.e] is the equilibrium concentration (mg/L), [Q.sub.e] is the equilibrium adsorption capacity (mg/g), [K.sub.F] is the Freundlich isotherm constant ([mg.sup.1-1/n] [L.sup.1/n] [g.sup.-1]), and n is the adsorption intensity.

In order to calculate the apparent free energy of adsorption, the Dubinin-Radushkevich model can be used [27, 28]. The Dubinin-Radushkevich model is given by this linear equation:

ln [Q.sub.e] - ln [Q.sub.m] - [K.sub.DR][[epsilon].sup.2], (9)

where [Q.sub.e] is the equilibrium adsorption capacity (mg/g), [Q.sub.m] is the saturation adsorption capacity (mg/g), [K.sub.DR] is Dubinin-Radushkevich isotherm constant related to adsorption energy ([mol.sup.2]/k[J.sup.2]), and [epsilon] is the Polanyi potential, which is defined as

[epsilon] = RT ln (1 + 1/[C.sub.e]), (10)

where R is the universal gas constant (8.314 J/mol x K) and T is the temperature in Kelvin.

Where the Freundlich isotherm assumes that the adsorption energy declines exponentially, the Temkin isotherm assumes that the heat of sorption declines linearly with temperature [27, 28] on the basis that the binding energies are uniformly distributed. The linear form of Temkin model is given as

[Q.sub.e] = [RT/B] ln ([A.sub.T]) + [RT/B] ln ([C.sub.e]), (11)

where [C.sub.e] is the equilibrium concentration (mg/L), [Q.sub.e] is the equilibrium adsorption capacity (mg/g), R is the universal gas constant (8.314 J/mol x K), T is the temperature in Kelvin, [A.sub.T] is the Temkin isotherm equilibrium binding constant (L/mg), and B is defined as

B = RT/[b.sub.T], (12)

where [b.sub.T] is the Temkin isotherm constant.

The parameters associated with adsorption isotherm models above are given in Table 2. For all three sorbents, the Freundlich isotherm model is the best fitting isotherm, with [R.sup.2] of 0.8934 for banana leaves sorbent, 0.9792 for banana stem sorbent, and 0.9079 for banana stalksorbent. This points to multilayer adsorption with interaction between adsorbed AG dye molecules. The isotherm is in line with kinetics, where the tendency for pseudo-second-order model indicates the interaction of one dye molecule to two adsorption sites. The three sorbents performed the worst for Langmuir isotherm model, with [R.sup.2] of less than 0.68. Nonetheless, the separation factor calculated using this model is between 0 and 1 for all three sorbents, showing that the adsorption is favourable under the conditions used. The maximum adsorption capacities calculated using Langmuir model are 79.36 mg/g for banana leaves sorbent, 157.73 mg/g for banana stem sorbent, and 48.08 mg/g using banana stalk sorbent. The Dubinin-Radushkevich isotherm fits satisfactorily for banana leaves and banana stem sorbent, with [R.sup.2] of 0.8688 and 0.8692, respectively. Using this model, the apparent free adsorption energy for each sorbent is calculated. The banana leaves sorbent has the highest free energy of 11.71 J/mol, the banana stalk sorbent is the next with 10.56 J/mol, and the banana stem sorbent has the lowest energy at 4.58 J/mol. All these energy values are very low, indicating physisorption nature of adsorption, as it is lower than 8.0 kJ/mol [29]. The experimental and calculated adsorption capacities were presented in Figure 7. The calculated adsorption capacities were close to the experimental ones at [C.sub.e] lower than 100 mg/L. At higher equilibrium concentrations, the calculated adsorption capacities were closely represented by using Langmuir and Temkin isotherms for banana leaves and stalk sorbents and by using Freundlich for banana stem sorbents.

3.5. Characterisation. The micrographs of SEM in Figure 8 show the surface morphologies of the sorbent after adsorption of the AG dye. The fibrillar structure in banana can be seen in the banana leaves, stem, and stalk sorbents, as has been reported in literature [30-32]. The stem and stalk sorbents are more homogeneous in structure, with smooth surface, compared to banana leaves sorbent. After the adsorption process, the AG dye molecules seem to cover part of the surface of the sorbents, as can be seen in Figures 8(a)-8(c) for the adsorption using 750 ppm of the AG dye and Figures 8(d)-8(f) for the adsorption using 1000 ppm of the AG dye. Similar morphologies were also found for the adsorption using 1500 ppm of the AG dye (not shown). The AG dye molecules were seen on the surface and inside the cavities of the sorbents.

FT-IR spectra after adsorption of the AG dye for the banana leaves, stem, and stalk sorbents are given in Figure 9. The surface functional groups found in the banana leaves, stem, and stalk sorbents are hydroxyl group at around 3400 [cm.sup.-1], C[H.sub.2] symmetric stretching at around 2900 [cm.sup.-1], overlapping peaks between 1600 and 1250 [cm.sup.-1] for C-C, C=C, OH, CO, C[H.sub.n], and C-O-C commonly found in polysaccharides, peak at around 1050 [cm.sup.-1] for C-O in alcohol group, and peaks between 550 and 430 [cm.sup.-1] for deformations of C-H groups in aromatic linkages, as described in our previous work [33]. The functional groups detected in AG dye (inset of Figure 9) are very similar to the ones in the sorbents used; thus, the FT-IR of the banana leaves, stem, and stalk sorbents remain the same after the adsorption. As can be seen, the peaks for functional groups at 3400 [cm.sup.-1], 2900 [cm.sup.-1], 1600-1250 [cm.sup.-1], 1050 [cm.sup.-1], and 550 to 430 [cm.sup.-1] are unshifted for all sorbents after the adsorption. Only the intensity of the hydroxyl group becomes less at concentration of 1500 ppm, though the peaks remain unshifted. This could indicate that the adsorption of these sorbents is more physical than chemical, as the functional groups are not strongly affected after adsorption took place.

4. Conclusions

The batch kinetics study for AG dye using banana leaves, stem, and stalk sorbents showed that the adsorption capacity for removal of AG dye is between 8 and 18 mg/g across all three concentrations used. The adsorption capacity increases with the increase in initial concentration in the range of concentrations tested. Sorption capacities of AG dye on banana leaves, stem, and stalk sorbents are higher at very low pH (initial pH = 2), whereas at higher pH the sorption capacities do not vary much, due to the buffering effect.

The sorption of all three sorbents follows closely pseudo-second-order kinetics, suggesting chemisorption involved as rate-controlling step. However, calculated mean free energy (using Dubinin-Radushkevich model) showed that the adsorption produces energy of less than 12 J/mol, which is much lower than chemisorption energy of 8 kJ/mol. The intraparticle diffusion model shows good conformity to the data, but all linear lines do not pass through origin, indicating that this is not the sole rate-limiting step. The adsorption of AG dye using banana stalk, stem, and leaves sorbents was found to fit into the Freundlich isotherm, suggesting multilayer adsorption.

http://dx.doi.org/ 10.1155/2016/9648312

Competing Interests

The authors declare that there is no conflict of interests regarding the publication of this paper.

Acknowledgments

The authors would like to thank Universiti Malaysia Sarawak for the use of laboratory facilities and equipment.

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Siti Kartina Abdul Karim, Soh Fong Lim, S. N. David Chua, Shanti Faridah Salleh, and Puong Ling Law

Faculty of Engineering, Universiti Malaysia Sarawak, Kota Samarahan 94300,

Malaysia

Correspondence should be addressed to Soh Fong Lim; sflim@unimas.my

Received 10 October 2016; Accepted 21 November 2016

Academic Editor: Wenshan Guo

Caption: FIGURE 1: Adsorption capacity of (a) banana leaves sorbent, (b) banana stem sorbent, and (c) banana stalk sorbent for AG dye removal ([??] 750 ppm; [??] 1000 ppm; [??] 1500 ppm). Experimental conditions: temperature = 25[degrees]C, agitation speed = 200 rpm, adsorbent dosage = 60g/L, and initial pH = 2.

Caption: FIGURE 2: Adsorption capacity of (a) banana leaves sorbent, (b) banana stem sorbent, and (c) banana stalk sorbent for AG dye removal. Experimental conditions: temperature = 25[degrees]C, agitation speed = 200 rpm, adsorbent dosage = 60 g/L, and initial concentration = 1000 ppm.

Caption: FIGURE 3: Initial versus final pH of (a) banana leaves sorbent, (b) banana stem sorbent, and (c) banana stalk sorbent for AG dye removal. Experimental conditions: temperature = 25[degrees]C, agitation speed = 200 rpm, adsorbent dosage = 60 g/L, and initial concentration = 1000 ppm.

Caption: FIGURE 4: The pseudo-first-order plots for adsorption of AG dye on (a) banana leaves sorbent, (b) banana stem sorbent, and (c) banana stalk sorbent ([??] 750 ppm; [??] 1000 ppm; [??] 1500 ppm).

Caption: FIGURE 5: The pseudo-second-order plots for adsorption of AG dye on (a) banana leaves sorbent, (b) banana stem sorbent, and (c) banana stalk sorbent ([??] 750ppm; [??] 1000 ppm; [??] 1500 ppm).

Caption: FIGURE 6: The intraparticle diffusion plots for adsorption of AG dye on (a) banana leaves sorbent, (b) banana stem sorbent, and (c) banana stalk sorbent ([??] 750ppm; [??] 1000 ppm; [??] 1500 ppm).

Caption: FIGURE 7: Experimental and calculated adsorption capacity of (a) banana leaves sorbent, (b) banana stem sorbent, and (c) banana stalk sorbent for CV dye removal. Experimental conditions: temperature = 25[degrees]C, agitation speed = 200 rpm, adsorbent dosage = 60 g/L, and initial pH = 2.

Caption: FIGURE 8: SEM images for (a) banana leaves sorbent, (b) banana stem sorbent, and (c) banana stalk sorbent, after adsorption using 750 ppm of AG dye, and (d) banana leaves sorbent, (e) banana stem sorbent, and (f) banana stalk sorbent, after adsorption using 1000 ppm of AG dye.

Caption: FIGURE 9: FT-IR spectra for (a) banana leaves sorbent, (b) banana stem sorbent, and (c) banana stalk sorbent, at (1) 1500 ppm, (2) 1000 ppm, and (3) 750 ppm. The inset in (c) is the FT-IR spectrum for AG dye.
TABLE 1: Adsorption kinetic parameters for banana stalk, stem, and
leaves sorbents based on pseudo-first-order, pseudo-second-order, and
intraparticle diffusion (Dunwald-Wagner) models.

Sorbent   Conc.    [Q.sub.e,           Pseudo-first-order
          (mg/L)     exp]        [k.sub.1]      [R.sup.2]   [Q.sub.e,
                    (mg/g)     ([min.sup.-1])                 cal]
                                                             (mg/g)

Banana     750      9.4752         0.1081        0.8724      3.1937
leaves     1000     11.0147        0.3026        0.8604      5.2204
           1500     18.4032       0.02602        0.8936      8.5605
Banana     750      8.0303         0.1382        0.8248      4.4066
stem       1000     10.5425        0.1635        0.7976      3.8107
           1500     17.0160        0.1350        0.8413      10.2612
Banana     750      7.2834         0.1069        0.9194      3.2984
stalk      1000     10.3923       0.05182        0.8444      2.9833
           1500     15.3295       0.08590        0.9470      6.8328

Sorbent                   Pseudo-second-order

               [k.sub.2]        [R.sup.2]   [Q.sub.e, cal]
             (g/mg x min)                       (mg/g)

Banana    1.195 x [10.sup.-3]    0.9993         9.3985
leaves    5.430 x [10.sup.-4]    0.9924        11.5473
          6.130 x [10.sup.-4]    0.9970        16.5837
Banana    3.492 x [10.sup.-3]    0.9657         8.1433
stem      5.994 x [10.sup.-4]    0.9897        10.1215
          4.118 x [10.sup.-4]    0.9471        16.8634
Banana    4.127 x [10.sup.-3]    0.9865         7.2046
stalk     9.971 x [10.sup.-4]    0.9984         9.8328
          5.152 x [10.sup.-4]    0.9957        15.4321

Sorbent          Dunwald-Wagner

            [k.sub.DW]     [R.sup.2]
          ([min.sup.-1])

Banana       0.09834        0.8937
leaves        0.2867        0.8529
              0.2188        0.9308
Banana        0.1283        0.8187
stem          0.1488        0.7922
              0.1198        0.8302
Banana       0.09742        0.9137
stalk        0.04721        0.8558
             0.07853        0.9445

TABLE 2: Isotherm parameters for banana stalk, stem, and leaves
sorbents based on Langmuir, Freundlich, Dubinin-Radushkevich, and
Temkin models.

                                    Langmuir

                        [K.sub.L]     [R.sub.L]      [R.sup.2]

Banana leaves sorbent   0.004508    0.09984-0.6893    0.2721
Banana stem sorbent     0.0002350   0.6802-0.9770     0.6735
Banana stalk sorbent    0.003708    0.1188-0.7295     0.6180

                                    Freundlich

                        [K.sub.F]    1/n     [R.sup.2]

Banana leaves sorbent    0.4025     0.9263    0.8934
Banana stem sorbent     0.005716    1.484     0.9792
Banana stalk sorbent     0.2654     0.8440    0.9079

                        Dubinin-Radushkevich

                        [K.sub.DR]   [R.sup.2]

Banana leaves sorbent    0.003644     0.8688
Banana stem sorbent      0.02380      0.8692
Banana stalk sorbent     0.004488     0.6996

                                    Temkin

                        [A.sub.T]   [b.sub.T]   [R.sup.2]

Banana leaves sorbent    0.1320       274.5      0.8881
Banana stem sorbent      0.01968      218.7      0.7699
Banana stalk sorbent     0.07441      338.3      0.8407
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Title Annotation:Research Article
Author:Karim, Siti Kartina Abdul; Lim, Soh Fong; Chua, S.N. David; Salleh, Shanti Faridah; Law, Puong Ling
Publication:Journal of Chemistry
Article Type:Technical report
Date:Jan 1, 2017
Words:5912
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