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N.D. Cuong et al. / Journal of Alloys and Compounds 582 (2014) 83–87
are activated during the initial reaction period. Leng et al. [23] sug-
gested that the reaction induction period seemed to depend on the
catalytic activity. A high activity indicates a short induction period.
However, the function of iron oxides in active catalysts remains
unclear. In addition, the benzylation of benzene with BC over nano-
3. Results and discussion
3.1. Characterization of catalyst
The crystal structure of the as-prepared
were examined via powder XRD measurement, and the data is
a
-Fe2O3 nanoparticles
porous
a-Fe2O3 nanoparticles has not yet been explored. Thereby,
further study is needed to explicitly understand the catalytic per-
shown in Fig. 2. The observed pattern of the collected products
formance of nanoporous
benzene with BC.
a-Fe2O3 nanoparticles for benzylation of
exhibited all the expected peaks from the a-Fe2O3 structure with-
out any detectable peak from impurities and other phases. The dif-
In this article, we report the controlled synthesis of scalable
fraction peaks were well-indexed to the rhombohedral structure of
nanoporous
nanoporous
a
-Fe2O3 nanoparticles for benzene benzylation. The
a
-Fe2O3 [space group: R3c] with structural parameters of
a = b = 0.0356 Å, c = 13.7489 Å, = b = 90°, and = 120°, which
agree with the literature (JCPDS 33-0664). The average crystalline
size of the -Fe2O3 nanoparticles calculated from the XRD data by
using the Scherrer equation is about 35 nm.
The surface state of the synthesized
investigated via FTIR is shown in Fig. 3. The absorption peaks at
a-Fe2O3 nanoparticles were synthesized via a hydro-
a
c
thermal method, and their catalytic performances in the benzyla-
tion of benzene and other aromatics with BC were systematically
investigated. The results showed that the nanoporous hematite
nanoparticles are active and selective catalysts for the benzylation
of benzene with BC to yield DPM.
a
a
-Fe2O3 nanoparticles
474 and 544 cmÀ1 are original peaks from
a-Fe2O3 nanoparticles
[32], whereas the peaks at 1634 cmÀ1 and 3436 cmÀ1 are due to
the OH bending of water and the hydroxyl group (–OH), respec-
tively [33].
2. Experimental
2.1. Materials
The morphologies of the nanoporous
which were characterized from SEM and TEM images, are shown
in Fig. 4(A and B), respectively. The -Fe2O3 nanoparticles fabri-
a-Fe2O3 nanoparticles,
Urea, Fe(NO3)3Á9H2O, benzene, benzyl chloride, toluene, and p-xylene were pur-
chased from Merck. Cetyltrimethylammonium bromide (CTAB) was purchased from
Aldrich. All chemicals were used as received without further purification.
a
cated via hydrothermal synthesis have very homogenous morphol-
ogies with nearly spherical shapes and regular dispersion
(Fig. 4(A)). The average particle size of the nanoparticles is about
100 nm, which is larger than the average crystalline size estimated
from the Scherrer equation (35 nm). This result suggests that the
nanoparticle is not a single crystal but is a poly-crystal. The TEM
image also indicates that nanopores of about less than 10 nm are
2.2. Synthesis of nanoporous
a-Fe2O3 nanoparticles
Nanoporous -Fe2O3 nanoparticles were synthesized via a hydrothermal meth-
a
od by using urea and iron(III) nitrate nonahydrate as precursors and CTAB as a sur-
factant. Ferric nitrate (2 mmol), CTAB (1 g), and urea (15 mmol) were dissolved in
35 mL of distilled water via magnetic stirring at room temperature for 2 h to obtain
a slurry solution. The slurry solution was then transferred into a 100 mL Teflon-
lined autoclave for hydrothermal processing. The hydrothermal processing was car-
ried out at 80 °C for 36 h, and the solution was then cooled down to room temper-
ature. The products were collected by several cycles of centrifugation and washed
with distilled water and ethanol. The collected products were dried at 60 °C for
24 h and then heat-treated at 500 °C to remove organic residues.
randomly distributed inside the
a-Fe2O3 nanoparticles (Fig. 4(B)).
These nanopores are believed to be generated because of the pres-
ence of bubbles during the hydrothermal process. The water expul-
sion of iron oxyhydroxide via heat treatment at 500 °C may also
contribute to the formation of the nanopores. However, the XRD
pattern of as-hydrothermal
cal diffraction peaks of an
a
-Fe2O3 samples (Fig. S1) shows typi-
a
-Fe2O3 phase but not of iron oxyhy-
2.3. Material characterization
droxide. Therefore, the possibility of the formation of the
nanopores as a result of water expulsion could be eliminated.
Fig. 5 shows the N2 adsorption/desorption isotherms and pore
The crystal structure of the nanoporous
ized using an X-ray diffractometer (XRD, D8 Advance, Brucker, Germany) with Cu
(k = 1.54 nm) radiation. Infrared spectroscopy was performed to evaluate the
a-Fe2O3 nanoparticles was character-
Ka
size distributions of the a-Fe2O3 nanoparticles. The sample exhibits
surface state of the synthesized materials. The infrared spectra were obtained using
a Nicolet 6700 FTIR Spectrometer in the range of 400–4700 cmÀ1 with a spectral
resolution of 4 cmÀ1 in transmittance mode. The KBr pellet technique was used
for sampling with 1 wt.% of materials for infrared spectroscopy measurement.
The morphology and the average particle size of hematite nanoparticles were inves-
tigated via scanning electron microscopy (SEM, Model JSM-5300LV) and transmis-
sion electron microscopy (TEM, Model JEOLE-3432, Japan). The nitrogen adsorption/
desorption isotherms of the heat-treated samples were obtained using a Micromer-
itics at 77 K. The specific surface area of the sample was calculated using the Bru-
nauer–Emmett–Teller (BET) method, whereas the pore-size distribution was
determined from the desorption isotherm data by using the Barrett–Joyner–Ha-
lende (BJH) model.
a type IV N2 adsorption/desorption isotherm with the H1 hystere-
sis loop (Fig. 5), which indicates the presence of mesoporosity
within the nanoparticles [34]. The pore diameters (inset of Fig. 5)
calculated using the BJH method are about 81 nm, and the pores
are caused by the interparticle space that is formed by the aggrega-
tion of Fe2O3 nanocrystals upon calcination. The BET specific sur-
face area of the nanoporous
a
-Fe2O3 nanoparticles is 15 m2/g.
This value is relatively high considering the size of the nanoparti-
cles. The catalytic activity greatly depends on the morphologies
and specific surface area of the catalysts because they have differ-
ent fractions of atoms located at different corners and edges as well
as different defects that are caused by the loss of atoms at these
locations.
2.4. Friedel–Crafts type benzylation of benzene
A scheme that represents the proposed mechanism for the benzylation of ben-
zene over the nanoporous
a-Fe2O3 nanoparticles catalysts is shown in Fig. 1 [22,26].
The liquid phase Friedel–Crafts benzylation reactions over
a-Fe2O3 nanoparticle
catalysts were carried out in a mechanically stirred mode in a two-neck round-bot-
tomed flask (capacity: 100 mL), which was fitted with a reflux condenser and
heated in a precisely controlled oil bath. All the reactions were performed in air
atmosphere. Benzene (30.55 g, 391 mmol), benzyl chloride (1.1 g, 8.7 mmol), and
hematite catalyst (50 mg) were mixed and stirred at 358 K at a moderate speed
for at least 3 min. The liquid samples were extracted, filtered periodically, and ana-
lyzed via gas chromatography (GC-2010 Shimadzu series) equipped with a thermal
conductivity detector (TCD) to evaluate the catalytic activity. The catalytic conver-
sion was calculated from the amount of benzyl chloride that was consumed during
the reaction, and the products were confirmed via GC–MS. Details about the GC–MS
results can be found in the electronic supporting information (ESI).
3.2. Benzylation of benzene and other aromatic compounds
To evaluate the catalytic performance of the nanoporous
a-
Fe2O3 nanoparticles, the benzylation of benzene with BC was
investigated. The reaction was carried out at 358 K and 50 mg of
the catalyst was used. Fig. 6 shows the conversion of BC and prod-
uct distribution as a function of reaction time. The BC conversion
reached 100% in a very fast reaction time of about 3 min. The reac-
tion induction period depends on the catalytic activity [23], but the