35 卷 6 期 2016. 6
结
构 化 学 (JIEGOU HUAXUE) Chinese J. Struct. Chem.
Vol. 35, No. 6 889─902
Pt/FeSnO(OH)5: A Novel Supported Pt Catalyst for Catalytic Oxidation of Benzene① YU Hana② CAO Zhou-Minga WEI Xiao-Fengb YU Yana② a
(Key Laboratory of Eco-materials Advanced Technology (Fuzhou University), Fujian Province University, College of Materials Science and Engineering, Fuzhou University, Fuzhou 350108, China)
b
(College of Chemical Engineering, Fuzhou University, Fuzhou 350108, China)
ABSTRACT Pt/FeSnO(OH)5 was synthesized as a novel catalyst for VOCs oxidation. Compared with Pt/γ-Al2O3 during catalytic oxidation of benzene, Pt/FeSnO(OH)5 showed better catalytic activity. After characterization of the catalysts by XRD, SEM, TEM, EDS, XPS, BET, TGA and DTA, we found most Pt could be reduced to metallic state when the hydroxyl catalyst was used as supporter, and the metallic Pt in Pt/FeSnO(OH)5 was more active than the oxidized Pt in Pt/γ-Al2O3 in catalytic oxidation of VOCs. Pt/FeSnO(OH)5 shows both good catalytic activity and high stability, which may be a promising catalyst. This study may also be helpful for the design and fabrication of new catalysts. Keywords: FeSnO(OH)5, supported Pt catalyst, catalytic oxidation of benzene; DOI: 10.14102/j.cnki.0254-5861.2011-1052 the most popular effective technologies because of
1 INTRODUCTION
its advantages such as low energy consumption, high At present, a growing number of researchers pay a close attention to the topic of removing the volatile
catalytic efficiency, relatively high flexibility and economical efficiency[2].
organic compounds (VOCs) because their extensive
Currently, supported noble metal catalysts, espe-
uses lead to water and air pollution. Among VOCs,
cially platinum (Pt) and palladium (Pd), despite their
benzene is a typical representative recognized as a
high costs, are often used in deep catalytic oxidation
[1]
major contributor to air pollution . Human and
of benzene because noble metal (Pt or Pd) can
animal are susceptible to benzene intoxication via
greatly improve the performance of catalysts for the
direct or indirect contact and will greatly increase
catalytic oxidation of benzene[1,
the risk of cancer if they live or stay in the benzene
doubt that a stable support can improve the per-
environment for a long period. Therefore, it is
formance of Pt-based catalysts[7-9]. And most of the
important to find an efficient method to get rid of
supported Pt catalysts are metal oxides, compounds
benzene. The catalytic oxidation of VOCs is one of
or nitrides as supports such as Al2O3[5, 10, 11], TiO2[1, 12, 13],
3-6]
. There is no
Received 16 November 2015; accepted 13 April 2016 ① This project was supported by the National Natural Science Foundation of China (No. 51102047, 51472050), the Natural Science Foundation of Fujian Province (No. 2013J05027) and the Fujian Province Education-science Project for Middle-aged and Young Teachers (No. JA13050) ② Corresponding author. Yu Han, Ph. D, Tel.: +86 591 22825732, Fax: +86 591 22866537. E-mails:
[email protected] and
[email protected]
892
YU H. et al.: Pt/FeSnO(OH)5: A Novel Supported Pt Catalyst for Catalytic Oxidation of Benzene [14]
zeolites
[3, 15]
and BN
No. 6
. These supports showed high
performances. On the basis of the characterizations,
thermal conductivity, temperature stability and
we have studied the oxidation states of Pt and the
[6, 7, 14]
oxidation resistance
. Moreover, the previous
relationship between the new support and the
researches have shown that metallic Pt nanoparticles
supported Pt for catalytic oxidation of benzene. This
have strong capacity for oxygen activation, and rich
study would be useful for the broadening of catalyst
chemisorbed oxygen on the surfaces of Pt nanopa-
supports and fabrication of efficient catalysts.
ticles is responsible for high catalytic activities for deep oxidation of benzene[1]. And a series of [3, 13]
lytic activities were observed in oxidized Pt catalysts and reduced Pt catalysts, of which the metallic species
EXPERIMENTAL
have demonstrated that different cata-
studies
[1, 2]
2
0
(Pt ) were more active than their oxidi2+
2. 1
Preparation of FeSnO(OH)5 nanocrystals
All of the chemical reagents were analytical grade from Sinopharm Chemical Reagent Co., Ltd. and
zed forms (PtO/ Pt ) for catalytic oxidation. In
used as received without further purification. The
addition, the dispersion of Pt on the supports’ sur-
solid FeSnO(OH)5 nanocrystals were prepared by an
face, the specific surface area of supports and the
ion-exchange method[20]. In a typical synthesis, 10
structure of the catalyst were also important factors
mmol of FeSO4·7H2O was added into 100 mL deio-
[1, 6, 16]
to affect the catalytic activity
.
nized water, and the solution was stirred at room
The surfaces of hydroxyl compounds possess
temperature until FeSO4·7H2O was dissolved com-
many hydroxyl (·OH) species and chemisorbed
pletely. Then, 20 mL of the solution containing 10
[17-19]
, and the rich hydroxyl species can make
mmol Na2SnO3·4H2O was poured into the FeSO4
the Pt nanoparticles strongly and balancedly loaded
solution. The mixed solution was cooled to 0 ℃
on the support surfaces, leading to better catalytic
and stirred for 6 h. After the reaction, the precipitates
activities. However, there is no report on using the
were collected by centrifugation and washed with
hydroxyl compounds as the carrier of catalysts as we
deionized water and ethanol for three times, res-
have known, because the poor thermal stability of
pectively. The final products were then dried in
most hydroxyl compounds prevents their applica-
vacuum at 70℃ for 12 h before use.
tions in catalysis. Therefore, if we can prepare a new
2. 2
oxygen
hydroxyl compound with better thermal stability
Preparation of the Pt/FeSnO(OH)5 composite catalysts
than the popular hydroxyl compounds, a new kind of
FeSnO(OH)5 loaded with 0.5 wt% Pt was fabri-
highly active supported Pt catalyst may be prepared.
cated via a simultaneous reduction-etching route[21].
However, how to achieve this target is a great
We used the L-ascorbic acid as reductant to reduce
challenge.
the H2PtCl6·6H2O in the water environment. 0.665
In this work, a new hydroxystannate compound
mL H2PtCl6·6H2O (0.019 M) was quickly added to a
(iron hydroxystannate, FeSnO(OH)5) has been
beaker of 10 mL ice water under strong stirring.
[20]
prepared via an ion exchange method
and loaded [21]
Then, 10 mL L-ascorbic acid ice-water solution (0.1
.
M) was slowly added into the solution. Next, 0.5 g
The catalyst (Pt/FeSnO(OH)5) was characterized in
as-synthesized FeSnO(OH)5 powder was dropped
detail by X-ray diffraction (XRD), infrared spec-
into the above mixed solution and stirred for 10
troscopy (FTIR), TG-DTA, field emission scanning
minutes. Subsequently, the beaker of mixture was
electron microscopy (FESEM), field emission trans-
placed in an ultrasonic cleaning instrument and
mission electron microscopy (FETEM), Brunauer-
treated for 1 h. Then the mixture was impregnated
Emmett-Teller (BET) and X-ray photoelectron spec-
and deposited for 24 h. The obtained products were
troscopy (XPS) for interpretation of its catalytic
collected by centrifugation and washed with deioni-
with Pt by simultaneous reduction-etching route
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zed water and ethanol for three times, respectively.
an atmospheric fixed bed reactor. 0.1 g portion of
The final products were then dried in vacuum at 70
Pt/FeSnO(OH)5 in 30~60 mesh was filled into a
℃ for 12 h.
U-type quartz tubular reactor equipped with a
For comparison, the Pt/γ-Al2O3 catalyst (0.5 wt%
temperature-programmed controller. Gaseous ben-
Pt) was also prepared by the above method. γ-Al2O3
zene (500 ppmv, Linde Gases (xiamen) Co., Ltd.)
was obtained by Shang Dong Aluminium Industry
balanced by synthetic air (20 vol% O2 and balanced
Co., Ltd.
N2, Linde Gases (xiamen) Co., Ltd.) was fed into the
2. 3
Characterization of the Pt/FeSnO(OH)5
reactor while the total flow rate was 100 mL/min
composite catalysts
and the gas pressure maintained 0.4 MPa, correspon-
X-ray diffraction (XRD) measurements of the
ding to a gas hourly space velocity (GHSV). The
powder samples were performed on a Panalytical
catalytic activity was measured while the tempe-
X’Pert spectrometer at a scanning rate of 10 deg/min
rature was raised from 50 to 200 ℃ at a rate of 3
in the 2θ range from 10° to 90°, with Fe filter Co-Kα
℃/min and the detailed heating and cooling pro-
radiation (λ = 0.178901 nm). The infrared spectro-
cesses are shown in Fig. 1. The benzene in the
scopy (FTIR) measurements were performed with a
stream was detected by an on-line GC (Huaai,
Nicolet 5700 spectrometer. The TG-DTA measure-
GC9560) equipped with flame ionization detector
ments were performed with USA TA (SDT-Q600) at
(FID). The GC (Huaai, GC9560) was also employed
a rate of 5 ℃/min in the temperature range from 0
for the quantitative and qualitative analyses of the
to 1000 ℃ under air atmosphere. The field emis-
products and by-products. Apart from the products
sion scanning electron microscopy (FESEM) images
such as CO2 and H2O, no other by-products were
of the samples were obtained by Hitachi S4800 field
found in all of the experiments. Thus the conversion
emission scanning electron microscopy. The field
was calculated based on the benzene consumption
emission transmission electron microscopy (FETEM)
Benzene conversion (%) = [(Cinlet – Coutlet)/Cinlet] × 100
images of the samples were obtained by FEI Tecnai
where Cinlet is the concentration of compound
G2 F20 S-TWIN with a field emission gun operated
benzene at the reactor inlet and Coutlet is that at the
at 200 kV. The energy dispersive spectrometer (EDS)
reactor outlet.
data were collected using an EDAX energy disper-
For comparison, the catalytic oxidation of ben-
sive spectrometer with the FETEM. N2 adsorption-
zene by the Pt/γ-Al2O3 catalyst was carried out under
desorption analysis was measured on a Microme-
the same conditions..
ritics ASAP 2020 instrument, and the multipoint Brunauer-Emmet-Teller (BET) surface area data
3 RESULTS AND DISCUSSION
were estimated from the relative pressure ranging from 0.06 to 0.3. X-ray photoelectron spectroscopy
3. 1
Characteristics of the catalysts
(XPS) measurements were performed with an
The XRD patterns of Pt/FeSnO(OH)5 catalysts are
ESCALab250-XI electron spectrometer from VG
shown in Fig. 2, in which the XRD pattern of pure
Scientific using 300 W AlKa radiation. The base
FeSnO(OH)5 is also included for comparison. In Fig. 2
-9
mbar and the binding
(a)~(e), all the diffraction peaks can be indexed to
energies were corrected by adjusting the binding
the standard cubic phase of FeSnO(OH)5 (JCPDS
energy of the C1s peak to 284.8 eV from adventi-
31-0654) without any unindexed peaks. However, no
tious carbon.
sharp peaks for Pt can be observed, indicating that
2. 4
Catalytic oxidation measurement
the loading amount of Pt (0.5 wt%) was too low or
of the Pt/FeSnO(OH)5 composite catalysts
the Pt nanoparticles might be uniformly dispersed
Catalytic oxidation of benzene was carried out on
and their crystal sizes were very small[1]. Moreover,
pressure was about 3×10
892
YU H. et al.: Pt/FeSnO(OH)5: A Novel Supported Pt Catalyst for Catalytic Oxidation of Benzene
No. 6
after the catalytic oxidation of benzene and the
talline structure of the sample was changed and
stability study at 150 and 180 ℃ for 80 h, respec-
became amorphous after the stability study at 200 ℃
tively, the crystal types of the supports did not
for 80 h (Fig. 2 (f)). Therefore, the Pt/FeSnO(OH)5
change, indicating that the Pt/FeSnO(OH)5 catalyst
catalyst can remain stable below 180 ℃.
is stable (Fig. 2(d) and (e)). Nevertheless, the crys-
Fig. 1.
Temperature-programmed pattern for the deep catalytic oxidation of benzene
Fig. 2. XRD patterns of the as-synthesized samples: (a) Pure FeSnO(OH)5; (b) and (c) Pt/FeSnO(OH)5 before and after catalytic oxidation of benzene; (d), (e) and (f) Pt/ FeSnO(OH)5 after the stability study at 150, 180 and 200 ℃ for 80 h, respectively
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The FTIR spectra of FeSnO(OH)5 and Pt/
vibration and the H2O-H2O hydrogen binding
FeSnO(OH)5 can provide more structural and sur-
absorption were also observed at 3400, 1635 and
face information about the prepared supports, which
775 cm−1[24,
are shown in Fig. 3. IR features of the samples are
could be found at 560 cm−1 which could be assigned
similar to the reported MSn(OH)6 (M = Cu, Mg,
to the stretching modes of Sn−OH[24,
[18]
26]
, respectively. Sn involved bonds 26]
. The
−1
. Thus, the formation of as-synthesized
absorption at around 2415 cm might be assigned to
samples can be further confirmed here by the FTIR
the stretching modes of Fe−OH. However, there are
result. In Fig. 3(a)~ (e), an intense broad band
no peaks at 3200, 2415 and 1190 cm−1 in Fig. 3(f),
centers at about 3200 cm−1 together with a sharp
indicating
Zn)
−1
that
the
surface
O−H
groups
in
absorption at 1190 cm , which can be attributed to
FeSnO(OH)5 disappeared after a long time at 200 ℃.
the
in
In other words, the crystal type of the support
and the
changed after the stability study at 200 ℃ for 80 h.
, respectively.
To sum up, the Pt/FeSnO(OH)5 catalyst was stable
The rich O−H groups in FeSnO(OH)5 are beneficial
below 200 ℃, corresponding to the results of XRD
for dispersion of the Pt nanoparticles on the support
patterns in Fig. 2.
stretching
vibration
of
O−H
groups [22, 23]
FeSnO(OH)5 or surface adsorbed H2O [24, 25]
-OH bending vibration of M−OH
surface. Moreover, the OH in-plane deformation
Fig. 3.
FTIR spectra of the As-synthesized samples: (a) Pure FeSnO(OH)5; (b) and (c) Pt/ FeSnO(OH)5 before and after catalytic oxidation of benzene; (d), (e) and (f) Pt/ FeSnO(OH)5 after the stability study at 150, 180 and 200 ℃ for 80 h, respectively
The thermal decomposition properties of the
℃ due to the loss of water upon FeSnO(OH)5 de-
synthesized FeSnO(OH)5 were investigated by TGA
composition. In addition, the phase transition
and DTA and the resulted curves are shown in Fig. 4.
temperature of FeSnO(OH)5 was 220 ℃, indicating
As shown in the TGA curve, a continuous and weak
that the thermal stability and the decomposition
weight loss ca. 2wt% from room temperature to 180
temperature of FeSnO(OH)5 were higher than the
℃ was observed. It was caused by the release of
reported MSn(OH)6 (M = Zn, Cu, Mg)[22]. There was
physically adsorbed water from FeSnO(OH)5.
no doubt that higher thermal stability of FeSnO-
Further increasing the temperature, a sharp decrease
(OH)5 would be good for the catalytic oxidation of
in mass appeared at ca. 180 ℃ and ended at ca. 250
benzene.
894
YU H. et al.: Pt/FeSnO(OH)5: A Novel Supported Pt Catalyst for Catalytic Oxidation of Benzene
Fig. 4.
No. 6
TGA and DTA curves of the As-synthesized FeSnO(OH)5 sample
The FESEM images of Pt/FeSnO(OH)5 are
change of FeSnO(OH)5 after the catalytic oxidation
present in Fig. 5(a~b), from which we can see that
of benzene, which is in agreement with the XRD
the samples are nanocubes with the sizes of about
data.
20~40 nm. There is no obvious morphological (b)
(a)
Fig. 5.
FESEM pictures of Pt/FeSnO(OH)5 before (a) and after (b) catalytic oxidation of benzene
of
surface area of the four samples at 160 m2/g in Table 2
Pt/FeSnO(OH)5 and Pt/γ-Al2O3 catalysts with their
because of the γ-Al2O3 support (159 m2/g) with a
corresponding EDS curves, respectively. The TEM
porous structure as shown in Fig. 7. Table 2 also
images and EDS curves prove that Pt nanoparticle
compared the BET surface areas of FeSnO(OH)5
was formed and attached to the FeSnO(OH)5 and
support and Pt/FeSnO(OH)5 catalyst. As presented in
γ-Al2O3 supporters, respectively, with similar size of
Table 2, the BET surface area of FeSnO(OH)5
about 5 nm.
support was 85 m2/g and that of Pt/FeSnO(OH)5
Fig.
6(a ~ d)
presents
TEM
images
Fig. 7 shows BET surface area, pore volume and
catalyst was 87 m2/g. Therefore, the negligible
size of Pt/FeSnO(OH)5 and Pt/γ-Al2O3 catalysts
differences between the BET surface areas indicated
measured by N2 adsorption and calculated from the
the insignificant effect of the supported Pt pro-
BET method. Pt/γ-Al2O3 exhibited the largest BET
cessing on the textural properties.
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Table 2. BET Surface Areas, Pt Particle Size and Comparison of Conversion Temperature for Benzene Oxidation over FeSnO(OH)5, Pt/FeSnO(OH)5, γ-Al2O3 and Pt/γ-Al2O3 Catalysts at the Flow Rate of 100 mL/min (T10, T50, T90, T100, Temperature at Which the Conversion of Benzene Reached 10%, 50%, 90%, and 100%, respectively) Name
BET surface area (m2/g)
Pt particle size (nm)
T10 (℃)
T50 (℃)
T90 (℃)
T100 (℃)
FeSnO(OH)5
85
—
180
>200
>200
>200
Pt/FeSnO(OH)5
87
~5
95
120
138
160
γ-Al2O3
159
—
190
>200
>200
>200
Pt/γ-Al2O3
160
~5
100
145
158
175
Fig. 6.
FETEM pictures of (a) Pt/FeSnO(OH)5 with the corresponding EDS curve inserted, (b) Partly enlarged of (a), (c) Pt/ γ-Al2O3 with the corresponding EDS curve inserted and (d) Partly enlarged of (c)
896
YU H. et al.: Pt/FeSnO(OH)5: A Novel Supported Pt Catalyst for Catalytic Oxidation of Benzene
Fig. 7.
No. 6
BET surface area, pore volume and size of Pt/FeSnO(OH)5 and Pt/γ-Al2O3 catalysts
XPS analyses of Pt 4d, Pt 4f, O 1s, Al 2s, Fe 2p
to Pt2+ and Pt4+ of Pt/γ-Al2O3[10].
and Sn 3d of Pt/FeSnO(OH)5 and Pt/γ-Al2O3
Fig. 8(b) shows that the O 1s peak (OI) on the
catalysts were carried out to identify the chemical
Pt/FeSnO(OH)5 catalyst appeared at 530.4 eV, which
states of the surface elements, as shown in Fig. 8. It
could be ascribed to the lattice oxygen in
0
was known that metallic Pt had relatively lower
FeSnO(OH)5. However, it was shifted to a higher BE
binding energies (BE) of 70.7~70.9 eV for 4f7/2
of about 530.8 eV for Pt/γ-Al2O3 catalyst. In addition,
and 74.0~74.1 eV for 4f5/2 electrons in Fig. 8(a),
a significant core level peak of O 1s (OII) is found at
2+
4+
and Pt oxidized states
about 531.5 and 531.9 eV for Pt/FeSnO(OH)5
exhibited much higher binding energies (72.8~73.1
catalyst, which could be ascribed to the adsorbed
respectively. However, Pt
2+
eV (4f7/2) and 76.3 ~ 76.4 eV (4f5/2) for Pt ;
oxygen. And the BE of adsorbed oxygen or
74.6~74.9 eV (4f7/2) and 78.1~78.2 eV (4f5/2) for
Pt/γ-Al2O3 catalyst appeared at 531.8 eV, while OI
4+ [1]
Pt ) . The peak of Pt 4f7/2 was concentrated upon
and OII atomic fractions of their O 1s peak were
70.2 (71.0) and the other was 73.3 (74.1) eV for the
different and Pt/FeSnO(OH)5 catalyst had higher OII
0
Pt/FeSnO(OH)5 catalyst, corresponding to Pt and 2+
atomic fraction, as shown in Table 1.
Pt , respectively. Nevertheless, it was positively
Fig. 8(c) shows that BE of Al in the Pt/γ-Al2O3
shifted to 73.7~75.3 eV for the Pt/γ-Al2O3 catalyst,
catalyst was single-peak appearing at 118.8 eV,
2+
and Pt oxidized
corresponding to Al3+ of γ-Al2O3. Sn 3d5 and Sn 3d3
states but far from the BE of metallic Pt0, indicating
for the Pt/FeSnO(OH)5 were recorded, which could
that Pt nanoparticles in Pt/γ-Al2O3 catalyst were not
be fitted by two peaks at the binding energies of
which was close to the BE of Pt
4+
0
reduced into metallic state (Pt ). This result could be
486.9 and 495.4 eV, corresponding to Sn4+ of
confirmed by Pt 4d5 and Pt 4d3 for Pt/γ-Al2O3 in Fig. 8(a)
FeSnO(OH)5[27]. Additionally, Fe 2p1 and Fe 2p3 for
which appeared at 314.3 nd 331.2 eV, corresponding
the Pt/FeSnO(OH)5 were also recorded, which could
2016
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be fitted by two peaks at the binding energies of 712.3 and 725.6 eV due to Fe
3+
of FeSnO(OH)5.
J.
Struct. Chem.
XPS data for Pt/FeSnO(OH)5 and Pt/γ-Al2O3 catalysts are listed in Table 1.
(a) Pt 4f Pt 4d
(b) O 1s
(c) Al 2s Fe 2p Sn 3d
Fig. 8.
897
XPS of Pt/FeSnO(OH)5 and Pt/γ-Al2O3 catalysts
898
YU H. et al.: Pt/FeSnO(OH)5: A Novel Supported Pt Catalyst for Catalytic Oxidation of Benzene
No. 6
Table 1.XPS Data for the Pt/FeSnO(OH)5 and Pt/γ-Al2O3 Catalysts Calculated from the Corresponding Areas of Fitted Peaks Done by XPSPEAK 4.1 with Shirley Background Pt/FeSnO(OH)5
Catalyst
Atomic (%)
BE (eV)
Atomic (%)
70.2
0.06
—
—
Pt
2+
74.1
0.01
73.7
0.05
Pt
4+
Pt0 4f Pt 4d
O 1s
Fe 2p
Sn 3d Al 2s
3. 2
Pt/γ-Al2O3
BE (eV)
—
—
75.3
0.02
Pt0
—
—
—
—
Pt2+
—
—
314.3
0.05
Pt4+
—
—
331.2
0.02
OⅠ
530.4
18.10
530.8
25.82
531.5
38.50
531.8
38.22
531.9
23.79
—
—
—
—
—
—
Fe
712.3
5.87
—
—
Sn 2+
—
—
—
—
486.9
13.67
—
—
—
—
118.8
35.89
OⅡ Fe2+ 3+
Sn
4+
Catalytic oxidation of benzene
was mainly influenced by the loading amount and
To be compared with the catalytic activity of the
oxidation state of active components (Pt). Moreover,
Pt/FeSnO(OH)5 catalyst, Pt/γ-Al2O3 was used as
Table 2 and Fig. 10 present the reaction temperature
catalyst. The light-off (or ignition) and complete
of 10% (T10), 50% (T50), 90% (T90) and 100% (T100)
combustion curves were used to compare the cata-
for benzene conversion (500 ppmv in air) over
lytic activities of the catalysts for benzene oxidation.
Pt/FeSnO(OH)5 and Pt/γ-Al2O3 catalysts. Fig. 9
The conversion was calculated on the basis of
clearly showed the benzene comparison plot of the
benzene consumption as described in Section 2.
reaction temperature for Pt/FeSnO(OH)5 and Pt/γ-
Before conducting the complete oxidation of
Al2O3 catalysts. These results clearly supported that
benzene by Pt/FeSnO(OH)5 and Pt/γ-Al2O3 catalysts,
Pt/FeSnO(OH)5 showed better catalytic activity than
a blank test was performed to check the existence of
the Pt/γ-Al2O3 catalyst.
homogeneous reactions. The blank test detected no
To study the effects of temperature cycling, the
thermal (or homogeneous) oxidation of benzene
stability of catalytic activity of the Pt/FeSnO(OH)5
below 600 ℃ in Fig. 9, which was in agree-
catalyst was detected when the catalytic temperature
[2]
ment with the previous studies . This result
was increased and then decreased, as shown in Fig. 11.
indicated that the employed system could be applied
The results also implied a good stability of the
for analyzing the catalytic oxidation of benzene. In
Pt/FeSnO(OH)5 catalyst. No other by-products
addition, pure FeSnO(OH)5 and γ-Al2O3 showed
(benzene-derived compounds or CO) were detected
poor catalytic activity for benzene oxidation and the
according to GC except the peaks for benzene and
former exhibited slightly better catalytic activity,
CO2 at different catalytic temperature over the
indicating that the supports had only small effect on
Pt/FeSnO(OH)5 catalyst.
the removal of benzene. Compared with pure
By comparing Table 2 with Fig. 9, we can see the
FeSnO(OH)5 and γ-Al2O3, the supported Pt catalysts
catalytic activity of Pt/FeSnO(OH)5 is better than
exhibited very high catalytic activities, especially for
Pt/γ-Al2O3. Good performance of the catalyst not
the Pt/FeSnO(OH)5 catalyst. Therefore, it could be
only depends on the intrinsic properties of the active
concluded that the catalytic activity of the catalyst
metal (electronic structure, etc.), but also on its
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crystal structure, particle size, specific surface area,
(Pt ) and 1/7 Pt exited as the oxidized forms (Pt2+).
pore structure and the dispersion states. However,
However, with the same condensation of Pt, all the
when the noble metal particles were presented in the
noble metal species exited as the oxidized forms in
form of nano-catalyst, the supported noble metal
Pt/γ-Al2O3, in which 5/7 Pt exited as Pt2+ and 2/7 Pt
catalysts exhibit a very high catalytic activity, indi-
exited as Pt4+. From above, we could conclude that
cating the performance of Pt was critical during
the metallic species were more active than their
catalysis.
of
oxidized forms for catalytic oxidation of benzene,
Pt/FeSnO(OH)5 was obviously smaller than Pt/γ-
which was in agreement with the previous resear-
Al2O3, as shown in Fig. 7, while the sizes of their
ches[1,
noble metal particles were similar, as shown in Fig. 5.
attached to both catalysts by the same method under
The most attractive difference between two catalysts
the same conditions, the difference of the Pt
was the oxidation state of Pt, as shown in Table 1. In
oxidation states could only be owed to the different
Pt/FeSnO(OH)5, 6/7 Pt exited as the reduced forms
structures of the supporters.
The
Fig. 9.
specific
surface
area
0
2]
. Considering that Pt was reduced and
Comparison plot of conversion temperatures of: (a) blank, (b) γ-Al2O3, (c) FeSnO(OH)5, (d) Pt/FeSnO(OH)5, and (e) Pt/γ-Al2O3
Fig. 10. Comparison plot of conversion temperature of T10, T50, T90 and T100 on Pt/FeSnO(OH)5 and Pt/γ-Al2O3
900
YU H. et al.: Pt/FeSnO(OH)5: A Novel Supported Pt Catalyst for Catalytic Oxidation of Benzene
Fig. 11.
3. 3
No. 6
Benzene conversion versus temperature over the Pt/FeSnO(OH)5 catalyst
Stability activity tests
possible that a bit of surface O−H groups in
A long catalytic test was performed in the reactor
FeSnO(OH)5 disappeared in a long time. Therefore,
operating at constant temperature in order to inves-
the Pt/FeSnO(OH)5 catalyst was cata- lytically
tigate the stability of the Pt/FeSnO(OH)5 catalyst.
stable.
The test was detected at the condition of 95% conversion in order to observe any deactivation
4
CONCLUSION
timely, as shown in Fig. 12. In addition, the benzene conversion versus on-stream reaction time over the
In conclusion, we synthesized Pt/FeSnO(OH)5 as
Pt/FeSnO(OH)5 catalyst is also shown in Fig. 12
a novel hydroxyl catalyst. Compared with Pt/γ-Al2O3
under the conditions of reaction temperature at 150
during
℃ for 80 h and 500 ppmv benzene in air with the
Pt/FeSnO(OH)5 showed better catalytic activity.
flow rate of 100 mL/min. The percentage of con-
After characterization of the catalysts by XRD, SEM,
version was analyzed at every time interval. It was
TEM, EDS, XPS and BET, we found most Pt could
found that during 80 h on stream, no obvious
be reduced to metallic state when the hydroxyl
decrease in catalytic activity was observed, that is,
catalyst was used as supporter and the metallic state
the Pt/FeSnO(OH)5 catalyst is catalytically stable.
of Pt was more active in catalytic oxidation of
This conclusion was confirmed by the result of XRD
benzene. Pt/FeSnO(OH)5 shows good catalytic
investigation in Fig. 2(d) and FTIR spectra in Fig. 3(d).
activity and high stability, which may be a promising
Although the degree of crystallinity was sli- ghtly
catalyst. This study may also be helpful for the
decreased, no significant change in Pt/FeSnO(OH)5
design and fabrication of new catalysts.
structure and crystal phase was detected. It was
catalytic
oxidation
of
benzene,
2016
Vol. 35
结
构
化
学(JIEGOU HUAXUE)Chinese
J.
Struct. Chem.
901
Fig. 12. Stability study of Pt/ FeSnO(OH)5 catalyst at 150 ℃ for 80 h under the condition of 500 ppmv benzene in air at the flow rate of 100 mL/min
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