# Performance of a Novel Hydrophobic Mesoporous Material for High Temperature Catalytic Oxidation of Naphthalene

Authors: Guotao Zhao; Zhenxiao Zhao; Junliang Wu; Daiqi Ye
Journal: Journal of Spectroscopy
 (2014)

---

## Abstract

A high surface area, hydrophobic mesoporous material, MFS, has been successfully synthesized by a hydrothermal synthesis method using a perfluorinated surfactant, SURFLON S-386, as the single template. N2 adsorption and TEM were employed to characterize the pore structure and morphology of MFS. Static water adsorption test indicates that the hydrophobicity of MFS is significantly higher than that of MCM-41. XPS and Py-GC/MS analysis confirmed the existence of perfluoroalkyl groups in MFS which led to its high hydrophobicity. MFS was used as a support for CuO in experiments of catalytic combustion of naphthalene, where it showed a significant advantage over MCM-41 and ZSM-5. SEM was helpful in understanding why CuO-MFS performed so well in the catalytic combustion of naphthalene. Experimental results indicated that MFS was a suitable support for catalytic combustion of large molecular organic compounds, especially for some high temperature catalytic reactions when water vapor was present.


---

## Body

## 1. Introduction

In recent years, more and more efforts have been focused on the catalytic removal of VOC or PAHs in ambient air and industrial emissions [1, 2]. However, traditional catalyst carriers have pore sizes that are too small to be used effectively in the catalytic combustion of large molecular organic pollutants [3]. Recently, many researchers have studied the catalytic removal process of VOC and PAHs on various mesoporous materials (refers to the kind of aperture between 2 and 50 nm porous materials) [4–7]. However, the presence of H2O molecules still has significant negative impacts on the decomposition of VOCs under these conditions [8]. Therefore, a popular, near-term research goal has been to develop hydrophobic carrier materials that will reduce the negative impacts of H2O on catalytic combustion.Currently, there are many methods for synthesizing hydrophobic mesoporous materials [9–12]. One of the most promising methods involves the use of fluorine-containing materials [13, 14]. If the method is optimized, the fluorine-containing groups are introduced onto the surface, even on the inner surfaces of the framework of the mesoporous materials, which enhances the hydrophobicity of the material [15–17] because of strong electronegativity of the fluorine-containing groups.This paper presents a new method for synthesizing mesoporous materials using the perfluorinated surfactant SURFLON S-386 (a polymeric perfluorocarboxylic acid) as the single template. The resulting mesoporous material (MFS) has a large surface area, high hydrophobiclity, and excellent hydrothermal stability for use in the catalytic combustion of naphthalene.


## 2. Experimental

### 2.1. Materials and Catalyst Preparation

SURFLON S-386 (99%) was received from Asahi Glass Company, Japan. TEOS (98%) was received from J&K Scientific Company, China. The chemicals were used without additional purification.The catalyst was prepared by mixing deionized water (120 mL) and SURFLON S-386 (0.8 g) in a 250 mL beaker. After stirring for 1 h at 40°C, a mixture of TEOS (10 g) and HCl (5 mL) was added drop by drop in a period of 30 min while stirring with a magnetic stirrer. After the mixture was added, the stirring was continuous for about 24 h. The mixture was then transferred into an autoclave and was heated for 48 h at 100°C. The resulting solid was centrifuged, washed (with water and alcohol), and dried in an oven at 100°C for 12 h. The final mesoporous material was calcined at 550°C for 6 h with the average heating rate of 1°C/min. The resulting product was marked as MFS.CuO was loaded on the MFS via the impregnation method by usingCu
(
N
O
3
)
2
·
3
H
2
O [18]. After evaporation and drying, the resulting solid material was calcined at 500°C for 4 h. After tableting and screening through with 40~60 mesh different concentrations of the catalyst were prepared by using different amounts of Cu
(
N
O
3
)
2
·
3
H
2
O. These catalysts were noted as CuO-MFS. The percentage of CuO ranged from 2 to 25%, expressed as the weight ratio of W
CuO
/
W
support.


### 2.2. Hydrophobicity Test

The hydrophobicities of the MFS samples were measured by the GBT6287-86 method (National Standards, China). The results obtained from the various materials were characterized by static adsorption rate.


### 2.3. Catalyst Activity Test

The catalytic activity test was performed with a continuous flow fixed-bed reactor with 8 mm ID, similar to that reported in the literature [19]. In each test run, 100 mg of catalyst was diluted with an appropriate amount of inert quartz beads (40~60 mesh) placed at the center of the reactor, above which a thermocouple was located to monitor the reaction temperatures. To create the stream containing naphthalene, a stream of pure dry air was passed through a U-shaped tube (contain naphthalene) at constant temperature (30°C) to produce a mixed gas containing a high concentration of naphthalene. The total flow rate was set at 180 mL min−1 with a concentration of 300 ppm naphthalene by adjusting the flow rate. The gas hourly space velocity (GHSV) in the tests was kept at 120000 h−1.An on-line gas chromatograph equipped with a FID detector was used to analyze the concentration of naphthalene in the inlet and outlet gas. Before each measurement, the temperature of the catalytic bed was raised to 200°C and stabilized at that temperature until the concentration of naphthalene became constant. No conversion of naphthalene was observed at this temperature. Then the temperature of catalyst bed was raised at 20°C/min until the experimental temperature was reached. Then the export concentration of naphthalene could be analyzed.


### 2.4. Materials Characterization

The specific surface areas (SSAs) of the catalysts (0.1–0.3 g) were determined with the BET method using an ASAP 2020 Micropore System (Micromeritics, USA). A vacuum pretreatment with vacuum at 300°C for 2 h was followed by nitrogen adsorption at −196°C. TEM (transmission electron microscopy) images were obtained using JEM-2010HR transmission electron microscope (Japan).The elements and their valances were measured by XPS (XML Paper Specification) using VG Multilab 2000 spectrometer (Germany) equipped with a hemispherical electron analyzer and Mg Ka radiation source(
h
ν
=
1253.6
eV
). All binding energies were referenced to the C
1
s line at 284.6 eV, which provided an accuracy of ±
0.48
eV within full scanning of 0~1000 eV.Py-GC/MS (pyrolysis-gas chromatography/mass spectrometry) analysis was carried out using a GC/MS-QP2010 PLUS pyrolysis gas chromatograph (Shimadzu, Japan) with a CDS (USA) cracker. SEM (scanning electron microscopy) images were obtained on a Philips FEIXL-30, operated with a 10 kV accelerating voltage after gold deposition.


## 2.1. Materials and Catalyst Preparation

SURFLON S-386 (99%) was received from Asahi Glass Company, Japan. TEOS (98%) was received from J&K Scientific Company, China. The chemicals were used without additional purification.The catalyst was prepared by mixing deionized water (120 mL) and SURFLON S-386 (0.8 g) in a 250 mL beaker. After stirring for 1 h at 40°C, a mixture of TEOS (10 g) and HCl (5 mL) was added drop by drop in a period of 30 min while stirring with a magnetic stirrer. After the mixture was added, the stirring was continuous for about 24 h. The mixture was then transferred into an autoclave and was heated for 48 h at 100°C. The resulting solid was centrifuged, washed (with water and alcohol), and dried in an oven at 100°C for 12 h. The final mesoporous material was calcined at 550°C for 6 h with the average heating rate of 1°C/min. The resulting product was marked as MFS.CuO was loaded on the MFS via the impregnation method by usingCu
(
N
O
3
)
2
·
3
H
2
O [18]. After evaporation and drying, the resulting solid material was calcined at 500°C for 4 h. After tableting and screening through with 40~60 mesh different concentrations of the catalyst were prepared by using different amounts of Cu
(
N
O
3
)
2
·
3
H
2
O. These catalysts were noted as CuO-MFS. The percentage of CuO ranged from 2 to 25%, expressed as the weight ratio of W
CuO
/
W
support.


## 2.2. Hydrophobicity Test

The hydrophobicities of the MFS samples were measured by the GBT6287-86 method (National Standards, China). The results obtained from the various materials were characterized by static adsorption rate.


## 2.3. Catalyst Activity Test

The catalytic activity test was performed with a continuous flow fixed-bed reactor with 8 mm ID, similar to that reported in the literature [19]. In each test run, 100 mg of catalyst was diluted with an appropriate amount of inert quartz beads (40~60 mesh) placed at the center of the reactor, above which a thermocouple was located to monitor the reaction temperatures. To create the stream containing naphthalene, a stream of pure dry air was passed through a U-shaped tube (contain naphthalene) at constant temperature (30°C) to produce a mixed gas containing a high concentration of naphthalene. The total flow rate was set at 180 mL min−1 with a concentration of 300 ppm naphthalene by adjusting the flow rate. The gas hourly space velocity (GHSV) in the tests was kept at 120000 h−1.An on-line gas chromatograph equipped with a FID detector was used to analyze the concentration of naphthalene in the inlet and outlet gas. Before each measurement, the temperature of the catalytic bed was raised to 200°C and stabilized at that temperature until the concentration of naphthalene became constant. No conversion of naphthalene was observed at this temperature. Then the temperature of catalyst bed was raised at 20°C/min until the experimental temperature was reached. Then the export concentration of naphthalene could be analyzed.


## 2.4. Materials Characterization

The specific surface areas (SSAs) of the catalysts (0.1–0.3 g) were determined with the BET method using an ASAP 2020 Micropore System (Micromeritics, USA). A vacuum pretreatment with vacuum at 300°C for 2 h was followed by nitrogen adsorption at −196°C. TEM (transmission electron microscopy) images were obtained using JEM-2010HR transmission electron microscope (Japan).The elements and their valances were measured by XPS (XML Paper Specification) using VG Multilab 2000 spectrometer (Germany) equipped with a hemispherical electron analyzer and Mg Ka radiation source(
h
ν
=
1253.6
eV
). All binding energies were referenced to the C
1
s line at 284.6 eV, which provided an accuracy of ±
0.48
eV within full scanning of 0~1000 eV.Py-GC/MS (pyrolysis-gas chromatography/mass spectrometry) analysis was carried out using a GC/MS-QP2010 PLUS pyrolysis gas chromatograph (Shimadzu, Japan) with a CDS (USA) cracker. SEM (scanning electron microscopy) images were obtained on a Philips FEIXL-30, operated with a 10 kV accelerating voltage after gold deposition.


## 3. Results and Discussion

### 3.1. Samples Characterization

#### 3.1.1. Nitrogen Adsorption

MFS sample was subjected to N2 adsorption studies [20]. The specific surface area was calculated according to the Brunauer-Emmett-Teller (BET) method and the average pore diameter was obtained according to the Barrett-Soyner-Halenda (BJH) method. A typical nitrogen adsorption isotherm is shown in Figure 1(a). Its BET surface area, Langmuir surface area, and pore volume were calculated to be 865.4 m2 g−1, 1205.1 m2 g−1, and 0.74 cm3 g−1, respectively. Its mesopore area and mesopore volume were 928.0 m2 g−1 and 0.7 cm3 g−1. In BJH differential pore volume plot, two sharp peaks are observed at about 2.9 nm and 4.9 nm for the MFS (Figure 1(b)), indicating a very narrow pore size for this mesoporous material.(a) N2 sorption isotherms of MFS 77 K and (b) pore size distribution in MFS as determined from the BJH model. P
/
P
o is the ratio of gas pressure (P) to saturation pressure (P
o
=
101.3
kPa).
(a)
(b)


#### 3.1.2. Transmission Electron Microscopy (TEM)

Figures2(a) and 2(b) show the TEM images of the MFS sample [20]. Some clear amorphous channel can be seen on the surface of the material. The light and dark stripes that are typical of mesoporous structures can also be observed in the MFS [16].TEM ((a) and (b)) images of the synthesized MFS.
(a)
(b)


#### 3.1.3. XML Paper Specification (XPS)

Figure3(a) shows the XPS full spectrum of MFS, which shows the electron energy states of five elements: Si
2
s, Si
2
p, C
1
s, O
1
s, and F
1
s, and content of fluoride element accounts for about 1% (At%). Figure 3(b) shows the XPS spectrum of F
1
s. F species were detected centered around 687.7 eV and are attributed to the –
CF
x bonds [21] which are related to the molecular structure of SURFLON S-386 (Figure 4). Therefore, it implies that a portion of the SURFLON S-386 fragments remain on the surface of MFS after calcination.(a) XPS full spectra of MFS and (b) XPS spectra ofF
1
s in MFS.
(a)
(b)Figure 4
Molecular structure of SURFLON S-386.


#### 3.1.4. Pyrolysis-Gas Chromatography/Mass Chromatogram (PY-GC/MS)

Pyrolysis-gas chromatography/mass spectrometry (Py-GC/MS) was employed to obtain structural information about MFS. The analytical procedure used in this study is similar to that reported previously [22]. The pyrolysis temperature was set at 800°C and held for 10 s from room temperature, with an average heating rate of 20°C/ms. The main pyrolytic products identified are listed in Table 1, and main peaks of the chromatogram are shown in Figure 5. The peak at 1.575 min is attributed to CO2, a combustion product of organic matter at high temperatures. Peak c at 1.950 min is attributed to the fluorine-containing decene according to the MS database, which is likely the residue of the template SURFLON S-386. Peak b at 1.742 min and other peaks from 2.10–4.05 min are also ascribed to the fragments of the template or intermediate species generated under high temperature. Peak d at 4.383 min is attributed to the fluorine-containing decanol according to MS database, which can be regarded as a new combination of SURFLON S-386 fragments with silicon-hydroxyl on the MFS surface. These findings indicate that fluorine-containing species exist on the MFS surface, which are a result of SURFLON S-386 fragments remaining on the surface of MFS after calcinations.Table 1
Main pyrolytic products of MFS according to Py-GC/MS.
Number
R. time(min)
Compound (matching)
Molecular weight
Peak
1
1.575
Carbon dioxide
44
a
2
1.742
Propanone
58
b
3
1.950
1-Decene,3,3,4,4,5,5,6,6,7,7,8,8,9,9,10,10,10-heptadecafluoro-
77
c
4
2.100
alpha-Methylfuran
82
—
5
2.308
2-Propanone
74
—
6
2.967
Propylene glycol
76
—
7
3.208
Succinaldehyde
86
—
8
3.892
Heptane
112
—
9
4.050
2-Cyclopenten-1-one
82
—
10
4.383
1-Decanol,3,3,4,4,5,5,6,6,7,7,8,8,9,9,10,10,10-heptadecafluoro-
464
dFigure 5
PY-GC/MS chromatogram of MFS.


### 3.2. Results of Hydrophobicity Test

A series adsorption of static water tests was conducted to investigate the hydrophobic properties of MFSs and MCM-41. Various MFS samples were synthesized with different amounts of SURFLON S-386(
g
SURFLON
S-
386
/
g
TEOS, m
/
m
) used during the process of synthesis. Different materials gave different static water adsorption rates as shown in Figure 6. Static water adsorption rate of MCM-41 is 74% (
g
water
/
g
adsorbent, m
/
m
), while the adsorption rate of MFS with 4% SURFLON S-386 is 46.3%. Then adsorption rate starts to decrease with the increase of the dosage. Adsorption rate dropped to 25.7%, when the dosage of SURFLON S-386 increased to 14%. Adsorption rate did not change significantly with increase of SURFLON S-386 dosage. Compared with MCM-41, the largest decrease of adsorption rate for SURFLON S-386 was greater than 50%. This means the hydrophobicity of MFS is significantly stronger than that of MCM-41. This behavior may be due to the existence of perfluoroalkyl groups remaining from SURFLON S-386 which reduces the surface tension and reduces the adsorption chances with water.Figure 6
Adsorption of static water on MFSs and MCM-41 (100% humidity).


### 3.3. Results of Catalytic Performance Experiments

Catalytic combustion of naphthalene has been investigated, and the results are shown in Figures7–9. Figure 7 shows the results of catalytic combustion of naphthalene with three catalysts: 10% CuO-ZSM-5, 10% CuO-MCM-41, and 10% CuO-MFS at temperatures from 300°C to 600°C.Figure 7
Conversion curves of naphthalene combustion over various materials.Figure 8
SEM of CuO-MFS and CuO-ZSM-5 before reaction and after reaction.Figure 9
Conversion curves of naphthalene combustion over CuO-FS-01.With 10% CuO-MCM-41, the conversion of naphthalene at first increases sharply, reaching a maximum conversion of 74.3% at 380°C and then decreasing at higher temperatures. A possible reason is that the hydrothermal stability of MCM-41 decreases at high temperature [23], which leads to the decrease in the conversion of naphthalene. Generally, MCM-41 is mainly used as a carrier for catalysts of combustion of small hydrocarbon molecules [24, 25]. If the temperature is higher than 400°C, the structure of MCM-41 may be disrupted due to the presence of water vapor.As for CuO-ZSM-5, its conversion also initially increases sharply, reaching a maximum conversion of 48% at 386°C and then decreasing at higher temperatures. One possible explanation for this behavior is that intermediate products generated in the reaction process block the channels of ZSM-5, which reduce the adsorption capacity for organic compounds, limiting the opportunities for naphthalene to enter the pores of ZSM-5. Hence, ZSM-5 is probably not appropriate for use as a catalyst carrier for catalytic combustion of large molecular organic compounds.Figure8 shows the SEM images of 10% CuO-ZSM-5 and 10% CuO-MFS before and after reaction. Comparing the paired images for 10% CuO-ZSM5-01A and for 10% CuO-ZSM5-02A, it can be seen that many stacked rod-like structures have formed on the surface of catalyst after reaction. The rod-like structure is probably the deposition of coke generated by the decomposition of naphthalene during the conversion process. When the catalytic reaction is going on, the larger incomplete oxidation products of naphthalene have difficulty entering the pores of ZSM-5. After continual accumulation and recombination, the rod-like structures start to form and grow at higher temperature.In contrast, Figure8 shows there is no significant change observed on the surface of MFS before and after reaction from the two images of MFS. However, for 10% CuO-MFS, the conversion of naphthalene increases slowly without maximum within the whole operation temperature range. The maximum conversion of 10% CuO-MFS is lower than 10% CuO-MCM-41, which may be due to the strong electronegativity of F, leading to the reduced activity of active species.The light-off curve of CuO-MFS for catalytic combustion of naphthalene is shown in Figure9. When the loading reaches 10%, the conversion reaches a maximum at all temperatures. Increasing the CuO loading further to 20%, results in a decline of the naphthalene conversion, which can be attributed to the agglomeration of the catalyst particles.


## 3.1. Samples Characterization

### 3.1.1. Nitrogen Adsorption

MFS sample was subjected to N2 adsorption studies [20]. The specific surface area was calculated according to the Brunauer-Emmett-Teller (BET) method and the average pore diameter was obtained according to the Barrett-Soyner-Halenda (BJH) method. A typical nitrogen adsorption isotherm is shown in Figure 1(a). Its BET surface area, Langmuir surface area, and pore volume were calculated to be 865.4 m2 g−1, 1205.1 m2 g−1, and 0.74 cm3 g−1, respectively. Its mesopore area and mesopore volume were 928.0 m2 g−1 and 0.7 cm3 g−1. In BJH differential pore volume plot, two sharp peaks are observed at about 2.9 nm and 4.9 nm for the MFS (Figure 1(b)), indicating a very narrow pore size for this mesoporous material.(a) N2 sorption isotherms of MFS 77 K and (b) pore size distribution in MFS as determined from the BJH model. P
/
P
o is the ratio of gas pressure (P) to saturation pressure (P
o
=
101.3
kPa).
(a)
(b)


### 3.1.2. Transmission Electron Microscopy (TEM)

Figures2(a) and 2(b) show the TEM images of the MFS sample [20]. Some clear amorphous channel can be seen on the surface of the material. The light and dark stripes that are typical of mesoporous structures can also be observed in the MFS [16].TEM ((a) and (b)) images of the synthesized MFS.
(a)
(b)


### 3.1.3. XML Paper Specification (XPS)

Figure3(a) shows the XPS full spectrum of MFS, which shows the electron energy states of five elements: Si
2
s, Si
2
p, C
1
s, O
1
s, and F
1
s, and content of fluoride element accounts for about 1% (At%). Figure 3(b) shows the XPS spectrum of F
1
s. F species were detected centered around 687.7 eV and are attributed to the –
CF
x bonds [21] which are related to the molecular structure of SURFLON S-386 (Figure 4). Therefore, it implies that a portion of the SURFLON S-386 fragments remain on the surface of MFS after calcination.(a) XPS full spectra of MFS and (b) XPS spectra ofF
1
s in MFS.
(a)
(b)Figure 4
Molecular structure of SURFLON S-386.


### 3.1.4. Pyrolysis-Gas Chromatography/Mass Chromatogram (PY-GC/MS)

Pyrolysis-gas chromatography/mass spectrometry (Py-GC/MS) was employed to obtain structural information about MFS. The analytical procedure used in this study is similar to that reported previously [22]. The pyrolysis temperature was set at 800°C and held for 10 s from room temperature, with an average heating rate of 20°C/ms. The main pyrolytic products identified are listed in Table 1, and main peaks of the chromatogram are shown in Figure 5. The peak at 1.575 min is attributed to CO2, a combustion product of organic matter at high temperatures. Peak c at 1.950 min is attributed to the fluorine-containing decene according to the MS database, which is likely the residue of the template SURFLON S-386. Peak b at 1.742 min and other peaks from 2.10–4.05 min are also ascribed to the fragments of the template or intermediate species generated under high temperature. Peak d at 4.383 min is attributed to the fluorine-containing decanol according to MS database, which can be regarded as a new combination of SURFLON S-386 fragments with silicon-hydroxyl on the MFS surface. These findings indicate that fluorine-containing species exist on the MFS surface, which are a result of SURFLON S-386 fragments remaining on the surface of MFS after calcinations.Table 1
Main pyrolytic products of MFS according to Py-GC/MS.
Number
R. time(min)
Compound (matching)
Molecular weight
Peak
1
1.575
Carbon dioxide
44
a
2
1.742
Propanone
58
b
3
1.950
1-Decene,3,3,4,4,5,5,6,6,7,7,8,8,9,9,10,10,10-heptadecafluoro-
77
c
4
2.100
alpha-Methylfuran
82
—
5
2.308
2-Propanone
74
—
6
2.967
Propylene glycol
76
—
7
3.208
Succinaldehyde
86
—
8
3.892
Heptane
112
—
9
4.050
2-Cyclopenten-1-one
82
—
10
4.383
1-Decanol,3,3,4,4,5,5,6,6,7,7,8,8,9,9,10,10,10-heptadecafluoro-
464
dFigure 5
PY-GC/MS chromatogram of MFS.


## 3.1.1. Nitrogen Adsorption

MFS sample was subjected to N2 adsorption studies [20]. The specific surface area was calculated according to the Brunauer-Emmett-Teller (BET) method and the average pore diameter was obtained according to the Barrett-Soyner-Halenda (BJH) method. A typical nitrogen adsorption isotherm is shown in Figure 1(a). Its BET surface area, Langmuir surface area, and pore volume were calculated to be 865.4 m2 g−1, 1205.1 m2 g−1, and 0.74 cm3 g−1, respectively. Its mesopore area and mesopore volume were 928.0 m2 g−1 and 0.7 cm3 g−1. In BJH differential pore volume plot, two sharp peaks are observed at about 2.9 nm and 4.9 nm for the MFS (Figure 1(b)), indicating a very narrow pore size for this mesoporous material.(a) N2 sorption isotherms of MFS 77 K and (b) pore size distribution in MFS as determined from the BJH model. P
/
P
o is the ratio of gas pressure (P) to saturation pressure (P
o
=
101.3
kPa).
(a)
(b)


## 3.1.2. Transmission Electron Microscopy (TEM)

Figures2(a) and 2(b) show the TEM images of the MFS sample [20]. Some clear amorphous channel can be seen on the surface of the material. The light and dark stripes that are typical of mesoporous structures can also be observed in the MFS [16].TEM ((a) and (b)) images of the synthesized MFS.
(a)
(b)


## 3.1.3. XML Paper Specification (XPS)

Figure3(a) shows the XPS full spectrum of MFS, which shows the electron energy states of five elements: Si
2
s, Si
2
p, C
1
s, O
1
s, and F
1
s, and content of fluoride element accounts for about 1% (At%). Figure 3(b) shows the XPS spectrum of F
1
s. F species were detected centered around 687.7 eV and are attributed to the –
CF
x bonds [21] which are related to the molecular structure of SURFLON S-386 (Figure 4). Therefore, it implies that a portion of the SURFLON S-386 fragments remain on the surface of MFS after calcination.(a) XPS full spectra of MFS and (b) XPS spectra ofF
1
s in MFS.
(a)
(b)Figure 4
Molecular structure of SURFLON S-386.


## 3.1.4. Pyrolysis-Gas Chromatography/Mass Chromatogram (PY-GC/MS)

Pyrolysis-gas chromatography/mass spectrometry (Py-GC/MS) was employed to obtain structural information about MFS. The analytical procedure used in this study is similar to that reported previously [22]. The pyrolysis temperature was set at 800°C and held for 10 s from room temperature, with an average heating rate of 20°C/ms. The main pyrolytic products identified are listed in Table 1, and main peaks of the chromatogram are shown in Figure 5. The peak at 1.575 min is attributed to CO2, a combustion product of organic matter at high temperatures. Peak c at 1.950 min is attributed to the fluorine-containing decene according to the MS database, which is likely the residue of the template SURFLON S-386. Peak b at 1.742 min and other peaks from 2.10–4.05 min are also ascribed to the fragments of the template or intermediate species generated under high temperature. Peak d at 4.383 min is attributed to the fluorine-containing decanol according to MS database, which can be regarded as a new combination of SURFLON S-386 fragments with silicon-hydroxyl on the MFS surface. These findings indicate that fluorine-containing species exist on the MFS surface, which are a result of SURFLON S-386 fragments remaining on the surface of MFS after calcinations.Table 1
Main pyrolytic products of MFS according to Py-GC/MS.
Number
R. time(min)
Compound (matching)
Molecular weight
Peak
1
1.575
Carbon dioxide
44
a
2
1.742
Propanone
58
b
3
1.950
1-Decene,3,3,4,4,5,5,6,6,7,7,8,8,9,9,10,10,10-heptadecafluoro-
77
c
4
2.100
alpha-Methylfuran
82
—
5
2.308
2-Propanone
74
—
6
2.967
Propylene glycol
76
—
7
3.208
Succinaldehyde
86
—
8
3.892
Heptane
112
—
9
4.050
2-Cyclopenten-1-one
82
—
10
4.383
1-Decanol,3,3,4,4,5,5,6,6,7,7,8,8,9,9,10,10,10-heptadecafluoro-
464
dFigure 5
PY-GC/MS chromatogram of MFS.


## 3.2. Results of Hydrophobicity Test

A series adsorption of static water tests was conducted to investigate the hydrophobic properties of MFSs and MCM-41. Various MFS samples were synthesized with different amounts of SURFLON S-386(
g
SURFLON
S-
386
/
g
TEOS, m
/
m
) used during the process of synthesis. Different materials gave different static water adsorption rates as shown in Figure 6. Static water adsorption rate of MCM-41 is 74% (
g
water
/
g
adsorbent, m
/
m
), while the adsorption rate of MFS with 4% SURFLON S-386 is 46.3%. Then adsorption rate starts to decrease with the increase of the dosage. Adsorption rate dropped to 25.7%, when the dosage of SURFLON S-386 increased to 14%. Adsorption rate did not change significantly with increase of SURFLON S-386 dosage. Compared with MCM-41, the largest decrease of adsorption rate for SURFLON S-386 was greater than 50%. This means the hydrophobicity of MFS is significantly stronger than that of MCM-41. This behavior may be due to the existence of perfluoroalkyl groups remaining from SURFLON S-386 which reduces the surface tension and reduces the adsorption chances with water.Figure 6
Adsorption of static water on MFSs and MCM-41 (100% humidity).


## 3.3. Results of Catalytic Performance Experiments

Catalytic combustion of naphthalene has been investigated, and the results are shown in Figures7–9. Figure 7 shows the results of catalytic combustion of naphthalene with three catalysts: 10% CuO-ZSM-5, 10% CuO-MCM-41, and 10% CuO-MFS at temperatures from 300°C to 600°C.Figure 7
Conversion curves of naphthalene combustion over various materials.Figure 8
SEM of CuO-MFS and CuO-ZSM-5 before reaction and after reaction.Figure 9
Conversion curves of naphthalene combustion over CuO-FS-01.With 10% CuO-MCM-41, the conversion of naphthalene at first increases sharply, reaching a maximum conversion of 74.3% at 380°C and then decreasing at higher temperatures. A possible reason is that the hydrothermal stability of MCM-41 decreases at high temperature [23], which leads to the decrease in the conversion of naphthalene. Generally, MCM-41 is mainly used as a carrier for catalysts of combustion of small hydrocarbon molecules [24, 25]. If the temperature is higher than 400°C, the structure of MCM-41 may be disrupted due to the presence of water vapor.As for CuO-ZSM-5, its conversion also initially increases sharply, reaching a maximum conversion of 48% at 386°C and then decreasing at higher temperatures. One possible explanation for this behavior is that intermediate products generated in the reaction process block the channels of ZSM-5, which reduce the adsorption capacity for organic compounds, limiting the opportunities for naphthalene to enter the pores of ZSM-5. Hence, ZSM-5 is probably not appropriate for use as a catalyst carrier for catalytic combustion of large molecular organic compounds.Figure8 shows the SEM images of 10% CuO-ZSM-5 and 10% CuO-MFS before and after reaction. Comparing the paired images for 10% CuO-ZSM5-01A and for 10% CuO-ZSM5-02A, it can be seen that many stacked rod-like structures have formed on the surface of catalyst after reaction. The rod-like structure is probably the deposition of coke generated by the decomposition of naphthalene during the conversion process. When the catalytic reaction is going on, the larger incomplete oxidation products of naphthalene have difficulty entering the pores of ZSM-5. After continual accumulation and recombination, the rod-like structures start to form and grow at higher temperature.In contrast, Figure8 shows there is no significant change observed on the surface of MFS before and after reaction from the two images of MFS. However, for 10% CuO-MFS, the conversion of naphthalene increases slowly without maximum within the whole operation temperature range. The maximum conversion of 10% CuO-MFS is lower than 10% CuO-MCM-41, which may be due to the strong electronegativity of F, leading to the reduced activity of active species.The light-off curve of CuO-MFS for catalytic combustion of naphthalene is shown in Figure9. When the loading reaches 10%, the conversion reaches a maximum at all temperatures. Increasing the CuO loading further to 20%, results in a decline of the naphthalene conversion, which can be attributed to the agglomeration of the catalyst particles.


## 4. Conclusion

A novel fluorine-containing, high surface area, hydrophobic mesoporous material, MFS, has been successfully synthesized by a hydrothermal synthesis method using a perfluorinated surfactant SURFLON S-386 as the single template. Some perfluoroalkyl groups from the SURFLON S-386 remain on the surface of MFS which leads to a high hydrophobicity of the material. MFS has significant advantages for use in the catalytic combustion of large molecular organic pollutants, especially those found in high temperature flue gases that contain water vapor. These advantages stem from MFS’s high hydrophobicity and larger pore diameter. Further work is needed to reduce the negative impacts of fluorine on the catalytic combustion reaction and to improve the naphthalene conversion at lower temperatures.



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*Source: 136067-2014-07-03.xml*