# Ordered Mesoporous Carbons as Novel and Efficient Adsorbent for Dye Removal from Aqueous Solution

Authors: Phuong T. Dang; Hoa T. H. Nguyen; Canh D. Dao; Giang H. Le; Quang K. Nguyen; Kien T. Nguyen; Hoa T. K. Tran; Tuyen V. Nguyen; Tuan A. Vu
Journal: Advances in Materials Science and Engineering
 (2016)

---

## Abstract

Ordered mesoporous carbons (OMCs) were successfully synthesized by using hard template and soft template methods. These materials were characterized by XRD, TEM, and N2 adsorption-desorption Brunauer-Emmett-Teller (BET). From the obtained results, it is revealed that the obtained OMCs samples showed high surface area (>1000 m2/g) with high pore volume, mainly mesopore volume (1.2–2.4 cm3/g). Moreover, OMCs samples had similar structure of the SBA-15 silica and exhibited high MB adsorption capacity with q
m of 398 mg·g−1 for OMCs synthesis with hard template and 476 mg·g−1 for OMCs synthesis with soft template, respectively. From kinetics investigation, it is confirmed that MB adsorption from aqueous solution obeys the pseudo-second-order kinetic equation.


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## Body

## 1. Introduction

In recent years, the synthesis of porous carbon materials with ordered mesopore array owing to their unique characteristics including highly periodic pore arrangement, uniform nanosize, high surface area, and large pore volume has received a great interest of researchers. Porous carbons [1–3] are widely used in many applications such as gas storage [4, 5], gas separation [6], catalysis [7, 8], electrochemical energy storage [9], and adsorption [10–12]. These materials showed high specific surface area with the contributions of both micropores and mesopores. Among porous carbon materials, carbon nanotubes have been intensively investigated. However, synthesis of carbon nanotubes with mesopores raised problems such as purity of products (removal catalyst) and mixture structure (single and multiwalls) [13, 14]. Ghaedi et al. [13] compared the efficiency of activated carbon (AC) and multiwalled carbon nanotube (MWCNT) for the removal of Eriochrome Cyanine R (ECR) molecules from aqueous solutions. They claimed that the sorption processes followed the pseudo-second-order in addition to intraparticle diffusion kinetics models with a good correlation coefficient with the overall entire adsorption of ECR on both adsorbents. Equilibrium data fit well with the Langmuir and Temkin models with a maximum sorption capacity based on the Langmuir equation of 40.6 and 95.2 mg/g for AC and MWCNT, respectively. Ordered mesoporous carbons (OMCs) are still rarely explored as adsorbent for dye removal. Ordered mesoporous carbons are mainly synthesized by the hard template method using ordered mesoporous silica like Si-MCM-41 and Si-SBA-15 as stating material and following the carbonization process [15]. Recently, a few papers described the preparation of OMCs using soft template methods [15–17]. Libbrecht et al. [15] reported the mesoporous carbons synthesized by both soft and hard template methods and compared them to a commercial powder activated carbon (PAC) for the adsorption ability of bisphenol-A (BPA) from an aqueous solution. The maximum observed adsorption capacity (
q
m
) of CMK-3 was the highest with 474 mg·g−1, compared to that of 290 mg·g−1 for PAC and 154 mg·g−1 for SMC. The difference in adsorption capacities was attributed to the specific surface area and hydrophobicity of the adsorbents.In the case of soft template method, the advantage is that the template contained in ordered mesoporous silica can be directly used as carbon source. Scheme of OMCs synthesis by the soft template is described as in Scheme1.Scheme 1In this paper, we report the synthesis of OMCs using both hard template and soft template method and their application as highly efficient adsorbents for methylene blue (MB) removal from aqueous solution. The effects of pH, MB, and OMCs concentration and the influence of OMCs pore structures as well as kinetics of MB over these OMCs materials were investigated.


## 2. Experimental

### 2.1. OMC-H Preparation

SBA-15 silica following synthesis procedure was reported by Nie et al. [26]. OMCs were synthesized by calcinations of SBA-15 impregnated with aqueous solution of carbon sources with sulfuric acid. Typically, 2 g of sucrose was mixed with 1 g SBA-15 and then added to a solution obtained by dissolving 0.14 g of H2SO4 in 5 g of H2O. The mixture was placed in a drying oven for 6 h at 100°C, and subsequently the oven temperature was increased to 160°C and maintained there for 6 h. The sample turned dark brown or black during the treatment in the oven. We repeated this step at 100 and 160°C using the same oven after the addition of 1 g of carbon, 0.14 g of H2SO4, and 5 g of H2O. The carbonization was completed by pyrolysis with heating at typically 900°C under nitrogen flow. The carbon-silica composite obtained after pyrolysis was immerged in HF 40% solution and then washed with H2O before being washed with mixture of 50 vol% ethanol + 50 vol% H2O. Final product was dried at 100°C for 3 h.


### 2.2. OMCs-S Preparation

OMCs-S was synthesized as follows: 3 g of F127 dissolved in 30 g ethanol and then to this mixture HCl 0.2 M solution was added and stirred at 40°C for 1 h. Next, 3.9 g of tetraethyl orthosilicate (TEOS) and resols solution (25% wt) with molar ratio resol/F127 by 0.85 is added and the mixture is kept stirring for 2 h, at 40°C. After 2 hours of stirring at 40°C, the obtained clear solution is poured out to disk for ethanol evaporation at room temperature for 24 h. Thin film was obtained by dried sample at 120°C for polymerization in 24. This thin film is heated in N2 flow from room temperature to 350°C in 1 h, then continued to raise the calcinations temperature up to 700°C, and keeps at this temperature in 2 h (carbonization). The obtained sample was washed in HF 10% solution and dried at 50°C for 4 h. Finally, sample was washed with H2O before being washed with ethanol-water mixture with a volume ratio of 50 : 50 before being dried at 80°C in 3 h.


### 2.3. Characterization

The powder X-ray diffraction (XRD) patterns of the samples were recorded on a Shimadzu XRD-6100 analyzer with CuK
α radiation (l
=
1.5417 Å). Transmission electron microscopy (TEM) was recorded using JEOL 1010 instrument operating at 80 kV with magnification of 25,000–100,000. Surface area of samples was determined on Quantachrome Instruments version 3.0 at 77 K and using nitrogen adsorbent. pH was investigated using microprocessor pH/Ion Meter pMX3000 (Germany) (scale ±0.03).


### 2.4. Adsorption Experiments

The methylene blue (C16H18N3SCl, 95% of purity) was purchased from Merck (Germany). MB adsorption was performed in liquid phase at room temperature under stirring condition. Batch experiments were carried out in a set of 250 mL Erlenmeyer flasks, in which a 100 mL aliquot of each MB solution with initial concentrations in the range of 100–300 ppm was added. Equal masses (W) of 0.05 g adsorbent were added to the MB solutions (V). The pH values of the solutions were adjusted using HCl 0.1 M or NaOH 0.1 M. Removal efficiency (H
%) of MB is defined as follows:(1)
H
%
=
C
o
-
C
e
C
o
×
100
%
,where C
o and C
e (ppm) are initial and equal MB concentration.


## 2.1. OMC-H Preparation

SBA-15 silica following synthesis procedure was reported by Nie et al. [26]. OMCs were synthesized by calcinations of SBA-15 impregnated with aqueous solution of carbon sources with sulfuric acid. Typically, 2 g of sucrose was mixed with 1 g SBA-15 and then added to a solution obtained by dissolving 0.14 g of H2SO4 in 5 g of H2O. The mixture was placed in a drying oven for 6 h at 100°C, and subsequently the oven temperature was increased to 160°C and maintained there for 6 h. The sample turned dark brown or black during the treatment in the oven. We repeated this step at 100 and 160°C using the same oven after the addition of 1 g of carbon, 0.14 g of H2SO4, and 5 g of H2O. The carbonization was completed by pyrolysis with heating at typically 900°C under nitrogen flow. The carbon-silica composite obtained after pyrolysis was immerged in HF 40% solution and then washed with H2O before being washed with mixture of 50 vol% ethanol + 50 vol% H2O. Final product was dried at 100°C for 3 h.


## 2.2. OMCs-S Preparation

OMCs-S was synthesized as follows: 3 g of F127 dissolved in 30 g ethanol and then to this mixture HCl 0.2 M solution was added and stirred at 40°C for 1 h. Next, 3.9 g of tetraethyl orthosilicate (TEOS) and resols solution (25% wt) with molar ratio resol/F127 by 0.85 is added and the mixture is kept stirring for 2 h, at 40°C. After 2 hours of stirring at 40°C, the obtained clear solution is poured out to disk for ethanol evaporation at room temperature for 24 h. Thin film was obtained by dried sample at 120°C for polymerization in 24. This thin film is heated in N2 flow from room temperature to 350°C in 1 h, then continued to raise the calcinations temperature up to 700°C, and keeps at this temperature in 2 h (carbonization). The obtained sample was washed in HF 10% solution and dried at 50°C for 4 h. Finally, sample was washed with H2O before being washed with ethanol-water mixture with a volume ratio of 50 : 50 before being dried at 80°C in 3 h.


## 2.3. Characterization

The powder X-ray diffraction (XRD) patterns of the samples were recorded on a Shimadzu XRD-6100 analyzer with CuK
α radiation (l
=
1.5417 Å). Transmission electron microscopy (TEM) was recorded using JEOL 1010 instrument operating at 80 kV with magnification of 25,000–100,000. Surface area of samples was determined on Quantachrome Instruments version 3.0 at 77 K and using nitrogen adsorbent. pH was investigated using microprocessor pH/Ion Meter pMX3000 (Germany) (scale ±0.03).


## 2.4. Adsorption Experiments

The methylene blue (C16H18N3SCl, 95% of purity) was purchased from Merck (Germany). MB adsorption was performed in liquid phase at room temperature under stirring condition. Batch experiments were carried out in a set of 250 mL Erlenmeyer flasks, in which a 100 mL aliquot of each MB solution with initial concentrations in the range of 100–300 ppm was added. Equal masses (W) of 0.05 g adsorbent were added to the MB solutions (V). The pH values of the solutions were adjusted using HCl 0.1 M or NaOH 0.1 M. Removal efficiency (H
%) of MB is defined as follows:(1)
H
%
=
C
o
-
C
e
C
o
×
100
%
,where C
o and C
e (ppm) are initial and equal MB concentration.


## 3. Results and Discussion

### 3.1. X-Ray Diffraction (XRD)

XRD patterns of OMCs and SBA-15 samples are shown in Figure1. XRD pattern of SBA-15 showed three sharp peaks which are assigned to the (100), (110), and (200) reflections, characteristic of the 2D hexagonal space groupp6mm.In the case of OMCs-H sample, only an intense peak at 2θ of 1.2° assigned to (100) reflection was observed. This result confirmed that OMCs-H had the same structure of SBA-15 but not well-ordered structure as compared to that of SBA-15. Similarly, the XRD pattern of OMCs-S showed an intense peak at 2θ of 1.2° but the intensity of this peak is much lower, indicating the less ordered structure of this material.Figure 1
XRD patterns of SBA-15, OMCs-H, and OMCs-S.


### 3.2. Transmission Electron Microscopy (TEM)

The TEM images in Figure2 show that SBA-15 and OMCs-H have the same morphology. These results confirm that the synthesis method of OMCs-H does not change the SBA-15 structure. However, the pores of SBA-15 are uniform with diameters of approximately 6-7 nm, larger than those of OMCs-H (4-5 nm); this can explain that OMCs-H was formed inside the SBA-15 pores walls narrowing the pore size. In contrast, OMCs-S was formed from direct structure template (copolymer F127), located within the pores of Si-SBA-15; therefore it is difficult to control the distribution and size of the pores.Figure 2
TEM images of SBA-15 (a), OMCs-S (b), and OMCs-H (c).
(a)
(b)
(c)


### 3.3. N2 Adsorption-Desorption (BET) Isotherms

N2 adsorption-desorption isotherms and pore-sized distribution of OMCs-H and OMCs-S are presented in Figure 3. As observed in Figure 3, both OMCs showed the isotherm curves of type IV with the hysteresis loop, characteristic for capillary condensation which is often noted for mesoporous material. Textural characteristics of samples are given in Table 1. As observed in Table 1, both OMCs-H and OMCs-S showed higher surface area as compared to that of SBA-15. Thus, surface area of OMCs-S is 1693 m2/g which is much higher than OMCs-H (1041 m2/g) and SBA-15 (650 m2/g). Pore size of OMCs-H is narrow distributed with the size of 4-5 nm while pore size of OMCs-S is also narrow distributed but with larger size, ranging from 5 to 10 nm. Moreover, from Table 1, it is noted that both OMCs exhibited very high pore volumes of 1.2–2.3 cm3/g which are much higher than that reported for ordered mesoporous materials [15]. Interestingly, in the case of OMCs-S synthesis by using soft template method, the new mesopores during carbonization are created. This can be rationalized by the fact that, during decomposition of copolymer F127 (copolymer of ethylene oxide and propylene oxide) in the inert gas flow, H2O formation plays the role of steaming activation to develop the new pore systems as observed on the active carbon activated by steaming [27, 28].Table 1
Textural properties of samples.
Samples
Textural properties
Surface area (m2/g)
Pore diameter (nm)
Pore volume (cm3/g)
Micropore volume (cm3/g)
Mesopore volume (cm3/g)
SBA-15
6-7
1.134
0.3471
0.787
650
OMCs-H
4-5
1.237
0.3615
0.875
1041
OMCs-S
5–10
2.374
0.1205
2.253
1693Figure 3
N2 adsorption-desorption isotherms (a) and pore-size distribution (b) of OMCs-H and OMCs-S.
(a)
(b)


### 3.4. Effect of pH

It is well known that the adsorption capacity of dyes is dominated by surface area and the interaction between the adsorbate molecules and the adsorbent surface through the electrostatic attraction. The charge of adsorbent surface depends on pH point of zero charge (p
H
p
z
c). Figure 4 plotted the surface charge as a function of pH value for OMCs-S and OMCs-H. Methylene blue is a cationic dye, when p
H
<
p
H
p
z
c, surface of the adsorbent positively charged, due to the expulsive force MB adsorption capacity decreased. In contrast, when p
H
>
p
H
p
z
c the adsorbent surface negatively charged due to the attraction force MB adsorption capacity increased. Moreover, at low pH (strong acidic medium) or high pH (high alkaline medium), the cations are rejected due to the affinity being weaker as compared to the proton and hydroxyl group affinity. From Figure 4, p
H
p
z
c of OMCs-S and OMCs-H is 6.0 and 5.5, respectively. The effect of pH solution on the adsorption equilibrium of OMCs-S and OMCs-H is shown in Figure 5. As noted in Figure 5, at pH of 8 (alkaline medium), MB adsorption efficiency reached the value of 98% and 95% for OMCs-S and OMCs-H, respectively. At pH of 7 (neutral medium), the efficiency also reached high value of 95% for OMCs-S and 93% for OMCs-H. At pH of 4 the efficiency decreased considerably (87% for OMCs-S and 70% for OMCs-H). In the MB adsorption process, all experiments were carried out at pH of 7 because of high MB removal efficiency and the appropriate application practice.Figure 4
p
H
p
z
c plot of OMC-S and OMC-H.Figure 5
Effect of pH solution on the adsorption equilibrium of OMC-S and OMC-H at [MB] = 200 ppm,W
/
V = 0.5 g/L, and T = 298 K.


### 3.5. Methylene Blue Adsorption

MB adsorption capacities at different concentrations on OMCs-H (a) and OMCs-S (b) are presented in Figure6 and Langmuir and Freundlich isotherm constants of OMCs-H and OMCs-S are given in Table 2. From Table 2 and Figure 6, both OMCs-H and OMCs-S showed high MB adsorption capacities. However, higher adsorption capacities over OMCs-S (q
m of 476 mg·g−1) as compared to that of OMCs-H (q
m of 398 mg/g) were observed. This can be explained by the fact that OMCs-S had higher surface area (1693 m2/g) as compared to that of OMCs-H (1041 m2/g). Note that both OMCs samples exhibited much higher MB adsorption capacities as compared to those of the same materials (OMCs) or related materials which have been reported in the literature. Thus, Yuan et al. [18] investigated MB adsorption ability on OMCs and obtained only the MB maximum adsorption capacity (
q
m
) of 200 mg·g−1. Moreover, in comparison to other related materials like activated carbon and carbon nanotubes, MB adsorption capacity of OMCs synthesized in our laboratory also showed higher value (see Table 2).Table 2
Comparison of MB adsorption capacity for different adsorbents.
Adsorbent
Template
q
m (mg/g)
Adsorbate
References
CFY
NaY
80
Methylene blue (MB)
[18]⁢
OMC-40
SBA-15
200
OMC-70
SBA-15
200
OMC-100
SBA-15
196
Fe-CMK-3
SBA-15
316
Methylene blue (MB)
[19]
MCSG60
Silica gel
200
Methylene blue (MB)
[20]
Graphene/c-MWCNT
—
191
Methylene blue (MB)
[21]
Date stone based AC
—
316
Methylene blue (MB)
[22]
Activated carbon produced from Venezuelan bituminous coal
—
380
Methylene blue (MB)
[23]
Activated sludge biomass
—
256
Methylene blue (MB)
[24]
Rice husk
—
312
Methylene blue (MB)
[25]
OMCs-S
—
476
Methylene blue (MB)
This study
OMCs-H
SBA-15
398Figure 6
Comparison of MB adsorption capacity at different concentrations of OMCs-H (a) and OMCs-S (b).
(a)
(b)


### 3.6. Langmuir and Freundlich Isotherm Models

Two experiment equations, Langmuir and Freundlich isotherms models, were often used to analyze the experimental data [29, 30].The Langmuir equation is expressed as follows:(2)
C
e
q
e
=
1
q
m
K
L
+
1
q
m
C
e
.The Freundlich equation is expressed as follows:(3)
log
⁡
q
e
=
log
⁡
K
F
+
1
n
log
⁡
C
e
,where q
m and K
L in the Langmuir equation represent the maximum adsorption capacity of adsorbents (mg·g−1) and Langmuir adsorption constant related to the free energy of adsorption, respectively. K
F and n are Freundlich constants related to adsorption capacity and adsorption intensity, respectively. The parameters of the Langmuir and Freundlich models were presented in Figure 7 and Table 3.Table 3
Langmuir and Freundlich isotherm constants of OMCs-H and OMCs-S.
Langmuir isotherm
Freundlich isotherm
OMCs-H
q
m (mg⋅g−1)
398
1
/
n
0.097
K
L (L⋅mg−1)
2.51
K
F [(
m
g
g
-
1
)
(
m
g
-
1
)
1
/
n]
283.59
R
2
0.9999
R
2
0.674
OMCs-S
q
m (mg⋅g−1)
476
1
/
n
0.143
K
L (L⋅mg−1)
5.25
K
F [(
m
g
g
-
1
)
(
m
g
-
1
)
1
/
n]
265.44
R
2
0.9999
R
2
0.495Figure 7
Langmuir plot for the adsorption of MB onto the OMCs-H and OMCs-S.The Langmuir isotherm models for the adsorption of MB on OMCs-H and OMCs-S are presented in Figure7. From Figure 7, it can be confirmed that the MB adsorption data on OMC-H and OMC-S fit well with Langmuir isotherm model.As observed in Table3, the value of R
2
=
0.9999 for Langmuir model with both of samples is higher than that of R
2
=
0.674 and 0.495 for Freundlich model with OMCs-H and OMCs-S, respectively. This was indicating that the Langmuir model fits much better than the Freundlich model for both samples.It is well accepted that the Langmuir isotherm assumes a surface with homogeneous binding sites, whereas the Freundlich isotherm is based on an exponential distribution of adsorption sites and adsorption onto heterogeneous surfaces. Moreover,R
L values are too small (Table 4), so we can confirm that MB adsorption process on OMCs samples is mainly monolayer adsorption process.Table 4
R
L equilibrium parameter value with MB adsorption on OMCs-S and OMCs-H.
C
o (mg/L)
100
150
200
300
400
500
R
L (OMCs-S)
0.00015
0.00010
0.000075
0.000050
0.000038
0.000030
R
L (OMCs-H)
0.0015
0.00075
0.00040
0.00030
0.000200
0.00020


### 3.7. MB Adsorption Kinetics

#### 3.7.1. Pseudo-First-Order Equation

The rate constant of adsorption is determined from the pseudo-first-order equation given by Langergren [31]:(4)
ln
⁡
q
e
-
q
t
=
ln
⁡
q
e
-
k
1
t
,where q
e and q
t are the amounts of MB adsorbed (mg·g−1) at equilibrium and at time t, respectively, and k
1 is the rate adsorption constant.Figure8 presents plots of ln
⁡
q
e
-
q
t versus time t for different MB concentrations. Values of k
1 were calculated from the plots of ln
⁡
q
e
-
q
t versus t for different concentrations of MB on OMCs samples and given in Table 5.Table 5
Rate adsorption constants and MB adsorption capacities calculated according to pseudo-first-order equation of OMCs-S and OMCs-H.
C
o (mg/L)
R
2
k
1 (h−1)
q
e
,
e
x
p (mg/g)
q
e
,
c
a
l (mg/g)
OMCs-S
100
0.0791
0.558
166.56
0.040
150
0.9777
1.389
249.84
3.890
200
0.9492
0.689
332.58
89.828
OMCs-H
100
0.0791
0.558
197.29
0.1579
150
0.9777
1.389
292.94
19.222
200
0.9492
0.689
397.94
42.798
q
e
,
e
x
p: q
e experimental.
q
e
,
c
a
l: q
e calculated.Figure 8
Plots ofln
⁡
(
q
e
-
q
t
) versus time t for different MB concentrations on OMCs-S (a) and OMCs-H (b).
(a)
(b)As observed in Table5, the low value of R
2 and large difference in q
e
,
e
x
p experimental and q
e
,
c
a
l calculated values indicate that the MB adsorption on OMCs does not obey the pseudo-first-order equation.


#### 3.7.2. Pseudo-Second-Order Equation

On the other hand, a pseudo-second-order equation based on equilibrium adsorption [32] is expressed as(5)
t
q
t
=
1
k
2
q
e
2
+
1
q
t
t
,where k
2 (g/mg·min) is the rates constant of pseudo-second-order adsorption. If pseudo-second-order kinetics is applicable, the plot of t
/
q
t versus t should show a linear relationship. There is no need to know any parameter beforehand and q
e and k
2 can be determined from the slope and intercept of the plot. Also, this procedure is more likely to predict the behavior over the whole range of adsorption. The linear plots of t
/
q
t versus t are presented in Figure 9.Figure 9
Linear plots oft
/
q
t versus time t for different MB concentrations of OMCs-S (a) and OMCs-H (b).
(a)
(b)Correlation coefficients,q
e
,
e
x
p experimental and q
e
,
c
a
l calculated values according to the pseudo-second-order kinetic equation, are shown in Table 6. As noted in Table 6, the high R
2 values of 0.9999–1 as well as the coincidence between q
e
,
e
x
p experimental and q
e
,
c
a
l calculated values can confirm that the MB adsorption in aqueous solution obeys the pseudo-second-order kinetic equation.Table 6
Rate adsorption constants and MB adsorption capacities calculated according to pseudo-second-order equation of OMCs-H and OMCs-S.
C
o (mg/L)
R
2
k
2 (g/mg⋅h)
q
e
,
e
x
p (mg/g)
q
e
,
c
a
l (mg/g)
OMCs-H
100
1
3.599
166.56
166.67
150
1
0.2
249.84
250
200
1
0.09
332.58
333.33
OMCs-S
100
1
3.599
197.29
197.23
150
1
0.2
292.94
296.73
200
0.9999
0.09
397.94
396.82


## 3.1. X-Ray Diffraction (XRD)

XRD patterns of OMCs and SBA-15 samples are shown in Figure1. XRD pattern of SBA-15 showed three sharp peaks which are assigned to the (100), (110), and (200) reflections, characteristic of the 2D hexagonal space groupp6mm.In the case of OMCs-H sample, only an intense peak at 2θ of 1.2° assigned to (100) reflection was observed. This result confirmed that OMCs-H had the same structure of SBA-15 but not well-ordered structure as compared to that of SBA-15. Similarly, the XRD pattern of OMCs-S showed an intense peak at 2θ of 1.2° but the intensity of this peak is much lower, indicating the less ordered structure of this material.Figure 1
XRD patterns of SBA-15, OMCs-H, and OMCs-S.


## 3.2. Transmission Electron Microscopy (TEM)

The TEM images in Figure2 show that SBA-15 and OMCs-H have the same morphology. These results confirm that the synthesis method of OMCs-H does not change the SBA-15 structure. However, the pores of SBA-15 are uniform with diameters of approximately 6-7 nm, larger than those of OMCs-H (4-5 nm); this can explain that OMCs-H was formed inside the SBA-15 pores walls narrowing the pore size. In contrast, OMCs-S was formed from direct structure template (copolymer F127), located within the pores of Si-SBA-15; therefore it is difficult to control the distribution and size of the pores.Figure 2
TEM images of SBA-15 (a), OMCs-S (b), and OMCs-H (c).
(a)
(b)
(c)


## 3.3. N2 Adsorption-Desorption (BET) Isotherms

N2 adsorption-desorption isotherms and pore-sized distribution of OMCs-H and OMCs-S are presented in Figure 3. As observed in Figure 3, both OMCs showed the isotherm curves of type IV with the hysteresis loop, characteristic for capillary condensation which is often noted for mesoporous material. Textural characteristics of samples are given in Table 1. As observed in Table 1, both OMCs-H and OMCs-S showed higher surface area as compared to that of SBA-15. Thus, surface area of OMCs-S is 1693 m2/g which is much higher than OMCs-H (1041 m2/g) and SBA-15 (650 m2/g). Pore size of OMCs-H is narrow distributed with the size of 4-5 nm while pore size of OMCs-S is also narrow distributed but with larger size, ranging from 5 to 10 nm. Moreover, from Table 1, it is noted that both OMCs exhibited very high pore volumes of 1.2–2.3 cm3/g which are much higher than that reported for ordered mesoporous materials [15]. Interestingly, in the case of OMCs-S synthesis by using soft template method, the new mesopores during carbonization are created. This can be rationalized by the fact that, during decomposition of copolymer F127 (copolymer of ethylene oxide and propylene oxide) in the inert gas flow, H2O formation plays the role of steaming activation to develop the new pore systems as observed on the active carbon activated by steaming [27, 28].Table 1
Textural properties of samples.
Samples
Textural properties
Surface area (m2/g)
Pore diameter (nm)
Pore volume (cm3/g)
Micropore volume (cm3/g)
Mesopore volume (cm3/g)
SBA-15
6-7
1.134
0.3471
0.787
650
OMCs-H
4-5
1.237
0.3615
0.875
1041
OMCs-S
5–10
2.374
0.1205
2.253
1693Figure 3
N2 adsorption-desorption isotherms (a) and pore-size distribution (b) of OMCs-H and OMCs-S.
(a)
(b)


## 3.4. Effect of pH

It is well known that the adsorption capacity of dyes is dominated by surface area and the interaction between the adsorbate molecules and the adsorbent surface through the electrostatic attraction. The charge of adsorbent surface depends on pH point of zero charge (p
H
p
z
c). Figure 4 plotted the surface charge as a function of pH value for OMCs-S and OMCs-H. Methylene blue is a cationic dye, when p
H
<
p
H
p
z
c, surface of the adsorbent positively charged, due to the expulsive force MB adsorption capacity decreased. In contrast, when p
H
>
p
H
p
z
c the adsorbent surface negatively charged due to the attraction force MB adsorption capacity increased. Moreover, at low pH (strong acidic medium) or high pH (high alkaline medium), the cations are rejected due to the affinity being weaker as compared to the proton and hydroxyl group affinity. From Figure 4, p
H
p
z
c of OMCs-S and OMCs-H is 6.0 and 5.5, respectively. The effect of pH solution on the adsorption equilibrium of OMCs-S and OMCs-H is shown in Figure 5. As noted in Figure 5, at pH of 8 (alkaline medium), MB adsorption efficiency reached the value of 98% and 95% for OMCs-S and OMCs-H, respectively. At pH of 7 (neutral medium), the efficiency also reached high value of 95% for OMCs-S and 93% for OMCs-H. At pH of 4 the efficiency decreased considerably (87% for OMCs-S and 70% for OMCs-H). In the MB adsorption process, all experiments were carried out at pH of 7 because of high MB removal efficiency and the appropriate application practice.Figure 4
p
H
p
z
c plot of OMC-S and OMC-H.Figure 5
Effect of pH solution on the adsorption equilibrium of OMC-S and OMC-H at [MB] = 200 ppm,W
/
V = 0.5 g/L, and T = 298 K.


## 3.5. Methylene Blue Adsorption

MB adsorption capacities at different concentrations on OMCs-H (a) and OMCs-S (b) are presented in Figure6 and Langmuir and Freundlich isotherm constants of OMCs-H and OMCs-S are given in Table 2. From Table 2 and Figure 6, both OMCs-H and OMCs-S showed high MB adsorption capacities. However, higher adsorption capacities over OMCs-S (q
m of 476 mg·g−1) as compared to that of OMCs-H (q
m of 398 mg/g) were observed. This can be explained by the fact that OMCs-S had higher surface area (1693 m2/g) as compared to that of OMCs-H (1041 m2/g). Note that both OMCs samples exhibited much higher MB adsorption capacities as compared to those of the same materials (OMCs) or related materials which have been reported in the literature. Thus, Yuan et al. [18] investigated MB adsorption ability on OMCs and obtained only the MB maximum adsorption capacity (
q
m
) of 200 mg·g−1. Moreover, in comparison to other related materials like activated carbon and carbon nanotubes, MB adsorption capacity of OMCs synthesized in our laboratory also showed higher value (see Table 2).Table 2
Comparison of MB adsorption capacity for different adsorbents.
Adsorbent
Template
q
m (mg/g)
Adsorbate
References
CFY
NaY
80
Methylene blue (MB)
[18]⁢
OMC-40
SBA-15
200
OMC-70
SBA-15
200
OMC-100
SBA-15
196
Fe-CMK-3
SBA-15
316
Methylene blue (MB)
[19]
MCSG60
Silica gel
200
Methylene blue (MB)
[20]
Graphene/c-MWCNT
—
191
Methylene blue (MB)
[21]
Date stone based AC
—
316
Methylene blue (MB)
[22]
Activated carbon produced from Venezuelan bituminous coal
—
380
Methylene blue (MB)
[23]
Activated sludge biomass
—
256
Methylene blue (MB)
[24]
Rice husk
—
312
Methylene blue (MB)
[25]
OMCs-S
—
476
Methylene blue (MB)
This study
OMCs-H
SBA-15
398Figure 6
Comparison of MB adsorption capacity at different concentrations of OMCs-H (a) and OMCs-S (b).
(a)
(b)


## 3.6. Langmuir and Freundlich Isotherm Models

Two experiment equations, Langmuir and Freundlich isotherms models, were often used to analyze the experimental data [29, 30].The Langmuir equation is expressed as follows:(2)
C
e
q
e
=
1
q
m
K
L
+
1
q
m
C
e
.The Freundlich equation is expressed as follows:(3)
log
⁡
q
e
=
log
⁡
K
F
+
1
n
log
⁡
C
e
,where q
m and K
L in the Langmuir equation represent the maximum adsorption capacity of adsorbents (mg·g−1) and Langmuir adsorption constant related to the free energy of adsorption, respectively. K
F and n are Freundlich constants related to adsorption capacity and adsorption intensity, respectively. The parameters of the Langmuir and Freundlich models were presented in Figure 7 and Table 3.Table 3
Langmuir and Freundlich isotherm constants of OMCs-H and OMCs-S.
Langmuir isotherm
Freundlich isotherm
OMCs-H
q
m (mg⋅g−1)
398
1
/
n
0.097
K
L (L⋅mg−1)
2.51
K
F [(
m
g
g
-
1
)
(
m
g
-
1
)
1
/
n]
283.59
R
2
0.9999
R
2
0.674
OMCs-S
q
m (mg⋅g−1)
476
1
/
n
0.143
K
L (L⋅mg−1)
5.25
K
F [(
m
g
g
-
1
)
(
m
g
-
1
)
1
/
n]
265.44
R
2
0.9999
R
2
0.495Figure 7
Langmuir plot for the adsorption of MB onto the OMCs-H and OMCs-S.The Langmuir isotherm models for the adsorption of MB on OMCs-H and OMCs-S are presented in Figure7. From Figure 7, it can be confirmed that the MB adsorption data on OMC-H and OMC-S fit well with Langmuir isotherm model.As observed in Table3, the value of R
2
=
0.9999 for Langmuir model with both of samples is higher than that of R
2
=
0.674 and 0.495 for Freundlich model with OMCs-H and OMCs-S, respectively. This was indicating that the Langmuir model fits much better than the Freundlich model for both samples.It is well accepted that the Langmuir isotherm assumes a surface with homogeneous binding sites, whereas the Freundlich isotherm is based on an exponential distribution of adsorption sites and adsorption onto heterogeneous surfaces. Moreover,R
L values are too small (Table 4), so we can confirm that MB adsorption process on OMCs samples is mainly monolayer adsorption process.Table 4
R
L equilibrium parameter value with MB adsorption on OMCs-S and OMCs-H.
C
o (mg/L)
100
150
200
300
400
500
R
L (OMCs-S)
0.00015
0.00010
0.000075
0.000050
0.000038
0.000030
R
L (OMCs-H)
0.0015
0.00075
0.00040
0.00030
0.000200
0.00020


## 3.7. MB Adsorption Kinetics

### 3.7.1. Pseudo-First-Order Equation

The rate constant of adsorption is determined from the pseudo-first-order equation given by Langergren [31]:(4)
ln
⁡
q
e
-
q
t
=
ln
⁡
q
e
-
k
1
t
,where q
e and q
t are the amounts of MB adsorbed (mg·g−1) at equilibrium and at time t, respectively, and k
1 is the rate adsorption constant.Figure8 presents plots of ln
⁡
q
e
-
q
t versus time t for different MB concentrations. Values of k
1 were calculated from the plots of ln
⁡
q
e
-
q
t versus t for different concentrations of MB on OMCs samples and given in Table 5.Table 5
Rate adsorption constants and MB adsorption capacities calculated according to pseudo-first-order equation of OMCs-S and OMCs-H.
C
o (mg/L)
R
2
k
1 (h−1)
q
e
,
e
x
p (mg/g)
q
e
,
c
a
l (mg/g)
OMCs-S
100
0.0791
0.558
166.56
0.040
150
0.9777
1.389
249.84
3.890
200
0.9492
0.689
332.58
89.828
OMCs-H
100
0.0791
0.558
197.29
0.1579
150
0.9777
1.389
292.94
19.222
200
0.9492
0.689
397.94
42.798
q
e
,
e
x
p: q
e experimental.
q
e
,
c
a
l: q
e calculated.Figure 8
Plots ofln
⁡
(
q
e
-
q
t
) versus time t for different MB concentrations on OMCs-S (a) and OMCs-H (b).
(a)
(b)As observed in Table5, the low value of R
2 and large difference in q
e
,
e
x
p experimental and q
e
,
c
a
l calculated values indicate that the MB adsorption on OMCs does not obey the pseudo-first-order equation.


### 3.7.2. Pseudo-Second-Order Equation

On the other hand, a pseudo-second-order equation based on equilibrium adsorption [32] is expressed as(5)
t
q
t
=
1
k
2
q
e
2
+
1
q
t
t
,where k
2 (g/mg·min) is the rates constant of pseudo-second-order adsorption. If pseudo-second-order kinetics is applicable, the plot of t
/
q
t versus t should show a linear relationship. There is no need to know any parameter beforehand and q
e and k
2 can be determined from the slope and intercept of the plot. Also, this procedure is more likely to predict the behavior over the whole range of adsorption. The linear plots of t
/
q
t versus t are presented in Figure 9.Figure 9
Linear plots oft
/
q
t versus time t for different MB concentrations of OMCs-S (a) and OMCs-H (b).
(a)
(b)Correlation coefficients,q
e
,
e
x
p experimental and q
e
,
c
a
l calculated values according to the pseudo-second-order kinetic equation, are shown in Table 6. As noted in Table 6, the high R
2 values of 0.9999–1 as well as the coincidence between q
e
,
e
x
p experimental and q
e
,
c
a
l calculated values can confirm that the MB adsorption in aqueous solution obeys the pseudo-second-order kinetic equation.Table 6
Rate adsorption constants and MB adsorption capacities calculated according to pseudo-second-order equation of OMCs-H and OMCs-S.
C
o (mg/L)
R
2
k
2 (g/mg⋅h)
q
e
,
e
x
p (mg/g)
q
e
,
c
a
l (mg/g)
OMCs-H
100
1
3.599
166.56
166.67
150
1
0.2
249.84
250
200
1
0.09
332.58
333.33
OMCs-S
100
1
3.599
197.29
197.23
150
1
0.2
292.94
296.73
200
0.9999
0.09
397.94
396.82


## 3.7.1. Pseudo-First-Order Equation

The rate constant of adsorption is determined from the pseudo-first-order equation given by Langergren [31]:(4)
ln
⁡
q
e
-
q
t
=
ln
⁡
q
e
-
k
1
t
,where q
e and q
t are the amounts of MB adsorbed (mg·g−1) at equilibrium and at time t, respectively, and k
1 is the rate adsorption constant.Figure8 presents plots of ln
⁡
q
e
-
q
t versus time t for different MB concentrations. Values of k
1 were calculated from the plots of ln
⁡
q
e
-
q
t versus t for different concentrations of MB on OMCs samples and given in Table 5.Table 5
Rate adsorption constants and MB adsorption capacities calculated according to pseudo-first-order equation of OMCs-S and OMCs-H.
C
o (mg/L)
R
2
k
1 (h−1)
q
e
,
e
x
p (mg/g)
q
e
,
c
a
l (mg/g)
OMCs-S
100
0.0791
0.558
166.56
0.040
150
0.9777
1.389
249.84
3.890
200
0.9492
0.689
332.58
89.828
OMCs-H
100
0.0791
0.558
197.29
0.1579
150
0.9777
1.389
292.94
19.222
200
0.9492
0.689
397.94
42.798
q
e
,
e
x
p: q
e experimental.
q
e
,
c
a
l: q
e calculated.Figure 8
Plots ofln
⁡
(
q
e
-
q
t
) versus time t for different MB concentrations on OMCs-S (a) and OMCs-H (b).
(a)
(b)As observed in Table5, the low value of R
2 and large difference in q
e
,
e
x
p experimental and q
e
,
c
a
l calculated values indicate that the MB adsorption on OMCs does not obey the pseudo-first-order equation.


## 3.7.2. Pseudo-Second-Order Equation

On the other hand, a pseudo-second-order equation based on equilibrium adsorption [32] is expressed as(5)
t
q
t
=
1
k
2
q
e
2
+
1
q
t
t
,where k
2 (g/mg·min) is the rates constant of pseudo-second-order adsorption. If pseudo-second-order kinetics is applicable, the plot of t
/
q
t versus t should show a linear relationship. There is no need to know any parameter beforehand and q
e and k
2 can be determined from the slope and intercept of the plot. Also, this procedure is more likely to predict the behavior over the whole range of adsorption. The linear plots of t
/
q
t versus t are presented in Figure 9.Figure 9
Linear plots oft
/
q
t versus time t for different MB concentrations of OMCs-S (a) and OMCs-H (b).
(a)
(b)Correlation coefficients,q
e
,
e
x
p experimental and q
e
,
c
a
l calculated values according to the pseudo-second-order kinetic equation, are shown in Table 6. As noted in Table 6, the high R
2 values of 0.9999–1 as well as the coincidence between q
e
,
e
x
p experimental and q
e
,
c
a
l calculated values can confirm that the MB adsorption in aqueous solution obeys the pseudo-second-order kinetic equation.Table 6
Rate adsorption constants and MB adsorption capacities calculated according to pseudo-second-order equation of OMCs-H and OMCs-S.
C
o (mg/L)
R
2
k
2 (g/mg⋅h)
q
e
,
e
x
p (mg/g)
q
e
,
c
a
l (mg/g)
OMCs-H
100
1
3.599
166.56
166.67
150
1
0.2
249.84
250
200
1
0.09
332.58
333.33
OMCs-S
100
1
3.599
197.29
197.23
150
1
0.2
292.94
296.73
200
0.9999
0.09
397.94
396.82


## 4. Conclusion

Ordered mesoporous carbons were successfully synthesized by using hard template and soft template methods. From XRD, TEM, and N2 adsorption-desorption (BET) results, it is revealed that the obtained OMCs-S sample had higher surface area (1693 m2/g) and pore volume (2.374 cm3/g) as compared to those of OMCs-H sample (1041 m2/g and 1.237 cm3/g). At pH of 7-8, MB adsorption capacity reached q
m of 476 mg·g−1 for OMCs-S and 398 mg·g−1 for OMCs-H, respectively. This opens high application potential of OMCs materials as novel and efficient adsorbents for dye removal from aqueous solution.



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*Source: 6528315-2016-09-22.xml*