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Applied Catalysis A: General 286 (2005) 1–10
0
d
Vanadium aluminium oxynitride catalysts for propane ammoxidation
reaction
Effect of the V/Al ratio on the structure and catalytic behaviour
Mihaela Florea a,b,1,*, Ricardo Prada Silvy b,1, Paul Grange b,1,�
a University of Bucharest, Faculty of Chemistry, B-dul Regina Elisabeta 4-12, 030016 Bucharest, Romaniab Universite Catholique de Louvain, Unite de Catalyse et Chimie des Materiaux Divises,
Croix du Sud 2, Boite 17, 1348 Louvain-la-Neuve, Belgium
Received 29 September 2004; received in revised form 15 February 2005; accepted 15 February 2005
Available online 5 April 2005
Abstract
The influence of the V/Al ratio composition on the physico-chemical and catalytic properties of the vanadium aluminium oxynitride
system was investigated. The samples were prepared by co-precipitation of vanadium and aluminium solutions containing different metal
compositions (0.1–0.9 V/Al) at pH 5.5 and characterized by XRD, XPS, Raman and BET surface area. Catalytic activity measurements for the
propane ammoxidation reaction were carried out under optimal acrylonitrile selectivity conditions.
X-ray diffraction pattern indicated that all the catalysts in both oxide precursor and nitride state show amorphous character. BET surface
area was higher for the sample with V/Al ratio of 0.25, before and after nitridation treatment. This sample showed optimal catalytic
performances, with 50% acrylonitrile selectivity and 60% propane conversion. The optimal nitridation degree, which induces an optimal
reduction degree of vanadium, would explain the maximal catalytic activity observed for the sample prepared using the V/Al ratio
composition of 0.25.
# 2005 Elsevier B.V. All rights reserved.
Keywords: Vanadium; Ammoxidation; Acrylonitrile
1. Introduction
Among the most significant examples of industrial
application in heterogeneous oxidation catalysis is the
production of acrylonitrile (ACN) through the propane
ammoxidation process. The advantages for replacing olefins
by alkanes in the current ammoxidation process are
essentially the lower price of propane with respect to
propylene and the risk of propylene shortage due to its
increasing consumption and the increasing worldwide
demand of nitriles and other derived products. Mixed
metal-oxides based on VMoMeOx [1,2] and VSbMeOx [3,4]
* Corresponding author. Tel.: +40 21 4103178; fax: +40 21 3159249.
E-mail address: [email protected] (M. Florea).1 Fax: +32 10 473649.� Deceased.
926-860X/$ – see front matter # 2005 Elsevier B.V. All rights reserved.
oi:10.1016/j.apcata.2005.02.032
are typical propane ammoxidation catalysts. Recently, Mo–
V–Te–Nb mixed oxides have been proposed as the most
active and selective catalysts in the ammoxidation of
propane to acrylonitrile, giving acrylonitrile yields up to
62% [5,6]. The active components of these catalysts have
been shown to be two phases called M1 and M2. The
respective roles of the two phases are not yet fully
understood but it has been reported that their concomitant
presence is needed to obtain effective catalysts. It has
recently been shown that these phases were presenting
orthorhombic and hexagonal type structures, respectively
and both contained the four metallic elements [6]. However,
this catalytic system has not yet provided a competitive
advantage in ACN productivity versus conventional
propylene ammoxidation catalysts, which explains why
the propane ammoxidation process has not yet been
commercially scaled up.
M. Florea et al. / Applied Catalysis A: General 286 (2005) 1–102
We have been investigating new catalytic materials for
alkane activation reaction. Vanadium aluminium oxynitride
(VAlON) catalysts show excellent properties for propane
ammoxidation and we have shown that the catalytic
properties strongly depend on the nitridation on the reaction
conditions [7] and on the preparation method [8]. The results
also indicated that the VAlON catalytic system has a high
ACN productivity at lower propane space–time relative to
VMoMeOx and VSbMeOx systems [9]. The dispersion of the
vanadium site at the surface has been recognized as the key
factor required for achieving high activity and, most
important, high acrylonitrile selectivity for vanadium-based
catalysts [10,11].
In this study, we investigate the influence of the
composition of the vanadium aluminium oxynitride, namely
the V/Al ratio, on the physico-chemical and catalytic
properties in propane ammoxidation.
Table 1
V/Al ratios and surface areas of VAlON catalysts
Catalyst V/Al
(theoretical)
V/Al
(experimental)
Surface
area before
test (m2/g)
Surface
area after
test (m2/g)
VAlON0.1 0.10 0.10 160 117
VAlON0.25 0.25 0.25 153 133
VAlON0.5 0.50 0.50 130 78
VAlON0.7 0.70 0.66 122 93
VAlON0.9 0.90 0.82 143 124
2. Experimental
Vanadium aluminium oxynitride catalyst with different
V/Al atomic ratios were prepared by thermal nitridation of a
co-precipitated V–Al oxide precursor. The preparation of the
oxide precursor is given elsewhere [8]. The nitridation of the
samples was carried out in a tubular rotating reactor under a
flow of pure ammonia (30 l h�1) at 500 8C for 5 h. The
system was subsequently cooled down to room temperature
under a flow of pure nitrogen.
The principle of the chemical analysis of total nitrogen
content is based on the reaction of the nitrogen species from
the catalyst with a strong base (KOH) at 450 8C and the
formation of ammonia which is then titrated with a standard
solution of sulphuric acid 10�2N (Grekov method). The
superficial nitrogen species were quantified by the Kjeldahl
method. The alkaline attack was realized using a KOH
saturated solution at 100 8C. The titrated ammonia
corresponds to the superficial NHx (NH and NH2) species.
Bulk nitrogen does not react under these conditions.
The BET surface area corresponding to oxynitride
catalysts before and after reaction was evaluated using a
Micromeritics Flow Sorb II 2300 apparatus.
Raman spectroscopy was performed with a DILOR-
JOBIN YVON-SPEX spectrometer, model OLYMPUS DX-
40, equipped with a He–Ne (l = 632.8 nm) laser. The
spectra were recorded in the 200–1600 cm�1 range.
XRD lines were recorded using a Siemens D-5000
powder diffractometer equipped with a Ni-filtered Cu Ka
radiation (l = 1.5418 A).
XPS spectra were collected with an SSX-100, model 206
Surface Science Instrument spectrometer at room tempera-
ture and under a vacuum of 1.33 mPa. Monochromatized Al
Ka radiation (hn = 1486.6 eV), obtained by bombarding the
Al anode with an electron gun operating at a beam current of
12 mA and an accelerating voltage of 10 kV was used. The
charge correction was made considering that the C 1s signal
of contaminating carbon (C–C or C–H bonds) was centered
at 284.8 eV. The C 1s, V 2p3, Al 2p, N 1s and O 1s levels
were chosen for characterization, since their signals are the
most intense and do not overlap.
Catalytic tests were performed in a fixed bed quartz
micro-reactor at atmospheric pressure and temperature of
500 8C, 0.1 g of catalyst and W/F = 8 g h/mol of C3H8. Feed
composition was 1.25:3:1 of C3H8:O2:NH3. The activity
results are reported after 24 h on stream. Feed and products
were analysed on-line using a gas chromatograph, equipped
with FID and TCD detectors and an on-line mass spectro-
meter was used to check the NOx formation. A carbon mass
balance of 80–90% was obtained, because of the condensa-
tion of the reaction products inside of the connection line
between the reactor and the gas chromatograph. To avoid the
condensation of acrylonitrile, the connection line was heated
at 150 8C.
Propane conversion is defined as the % ratio between the
mole of propane consumed per mole of propane in the feed;
the ACN selectivity as mole of ACN in the product per mole
of propane consumed; and the ACN yield as mole of ACN in
the product per mole of propane in the feed.
3. Results
3.1. Chemical composition, textural and structural
characteristics
Samples with V/Al atomic ratios in the range of 0.1–0.9
were prepared by the co-precipitation method followed by
nitridation in the presence of ammonia at 500 8C for 5 h. All
the samples are X-ray amorphous before and after the
catalytic test. Table 1 compiles the theoretical and
experimental V/Al ratios and the values of the surface
areas of the oxynitride powders before and after propane
ammoxidation.
The V/Al molar ratios in the obtained catalysts are lower
than the theoretical values for the ratios higher than 0.7. The
oxynitrides exhibit a specific area between 125 and 160 m2/g
and depend on the V/Al ratio, as seen in Table 1.
The surface area increases with the decreasing V/Al ratio,
with highest surface area of 160 m2/g being observed for
VAlON0.1 sample. The tested catalysts exhibit surface areas
15–25% lower than those of the corresponding fresh
M. Florea et al. / Applied Catalysis A: General 286 (2005) 1–10 3
Table 2
Nitrogen content before and after catalytic test as a function of the V/Al
ratio
Catalyst NT (%)a NK (%)b
Before test After test Before test After test
VAlON0.1 4.93 2.30 n.a.c n.a.
VAlON0.25 5.35 5.18 3.06 3.57
VAlON0.5 4.76 2.91 2.72 0.85
VAlON0.7 3.28 1.86 1.36 0.47
VAlON0.9 2.26 1.80 1.02 0.51
a Total nitrogen content determined by Grekov method.b Nitrogen content determined by Kjeldahl method.c Not analysed.
materials. The nitrogen contents of the nitrided powders
before and after the catalytic test are given in Table 2.
An increase of total and Kjeldahl nitrogen content was
observed with a decrease of the V/Al ratio until 0.25, below
this ratio, the nitrogen content slightly diminished. The
highest nitrogen content of 5.35% was obtained for
VAlON0.25. For all the samples, the total nitrogen content
diminished upon use in propane ammoxidation. For the used
catalysts, a slight increase of the surface nitrogen content
was observed only for the sample with V/Al of 0.25.
3.2. Raman spectroscopy
The Raman spectroscopy technique can discriminate
between different vanadium oxide species formed during the
preparation of the oxide precursor. The Raman spectra of the
oxide precursor with different V/Al ratios are presented in
Fig. 1.
The Raman results indicate that different vanadium
species are formed during the co-precipitation by changing
the V/Al ratio. The bands at 1050, 980 and 940 cm�1
confirm that there are both isolated and polymeric vanadium
oxide surface species formed as a function of the V/Al ratio.
For instance: (i) the band at 980 cm�1 is assigned to surface
decavanadate species [HnV10O28](6�n)� [12], (ii) the band at
Fig. 1. Raman spectra of vanadium aluminium oxide with various V/Al
ratios: 0.9 (a), 0.7 (b), 0.25 (c) and 0.1 (d).
940 cm�1 confirms the presence of [(VO3)n]n� metavana-
date species [13], and (iii) the band at 1050 cm�1 is assigned
to isolated VO4 vanadium oxide species [14] with one
terminal V O bond and three Raman inactive V–O–Al
bonds [15].
The highest concentration of isolated vanadium species is
found for the sample with a V/Al ratio of 0.1, as indicated by
the highest intensity of the Raman band at 1050 cm�1. With
increasing V/Al ratio, this band, assigned to isolated
vanadium species, diminished and disappeared for V/Al
of 0.7 and 0.9. The amount of polymeric species increased
with the V/Al ratio. The Raman band corresponding to the
V O terminal bond of surface decavanadate at 980 cm�1 is
characteristic for the V/Al ratios of 0.7 and 0.9.
It is worth mentioning that in the isolated species as well
in the metavanadate species (VO3)n, vanadium presents a
tetrahedral coordination, while in the decavanadate species
(HnV10O28), vanadium has an octahedral coordination.
Thus, the vanadium has a tetrahedral coordination for the
low vanadium loading and octahedral coordination for high
vanadium loading.
3.3. XPS characterization
The XPS technique provides information regarding the
nature of the surface nitrogen species before and after
catalytic test, as well as about the surface vanadium atoms.
Table 3 shows the binding energies corresponding to Al 2p,
O 1s, V 2p and N 1s levels.
The binding energy of the O 1s level was not modified by
changing the V/Al ratio nor by nitrogen insertion.
Concerning the Al 2p level, an increase of binding energy
was observed with increasing V/Al ratio, from 74.1 eV for
VAlON0.1 to 74.45 eV for VAlON0.9. However, the binding
energies of both O 1s and Al 2p levels diminished for the
used catalysts, indicating that changes in the structure of the
catalyst are induced by the reagents.
The XPS spectra of all the fresh samples are character-
ized by two values of the binding energy for the V 2p3/2
level, obtained at 517.1–517.5 and 515.5–516.3 eV (see
Table 3). There is controversy concerning the assignment of
these peaks, as it can be seen from the different results
reported in the literature [16–18].
The position of the first component agrees well with the V
2p3/2 binding energy in V2O5 and NH4VO3 (517.3 eV). Thus
we assign this component to the V5+ oxidation state.
Because of the wide variation in the reported binding
energies for all vanadium oxidation states, and since both
V3+ and V4+ are proposed in the literature, the components at
516.3–515.5 eV region cannot be readily assigned to a
specific oxidation state. An approximate estimation of the
atomic V5+/(V5+ + V4+) surface ratio can be made on the
basis of these results. The values for the fresh and used
catalysts are presented in Table 4.
The reduction degree increases with the V/Al ratio
and increases more upon propane ammoxidation for all
M. Florea et al. / Applied Catalysis A: General 286 (2005) 1–104
Table 3
Binding energy (eV) for VAlON catalysts
Sample Al 2p (eV) O 1s (eV) V 2p3/2 (eV) N 1s (eV)
VAlON0.1
Fresh 74.1 531.0 517.1 399.8
515.7
Used 73.5 530.3 516.4 399.2
515.2 402.8
VAlON0.25
Fresh 74.2 531.2 517.5 397.5
516.3 399.9
401.8
Used 73.9 530.8 517.5 400.3
516.4 398.5
VAlON0.5
Fresh 74.3 531.2 517.4 397.1
515.5 400.0
402.6
Used 73.6 530.2 516.8 399.3
515.3 402.3
VAlON0.7
Fresh 74.4 531.2 517.5 397.4
516.0 400.3
402.1
Used 72.9 530.7 516.9 398.6
515.5 401.7
VAlON0.9
Fresh 74.45 531.1 517.3 397.4
515.5 399.8
401.8
Used 74.3 530.9 517.2 399.0
515.8 400.6
Fig. 2. XPS spectra of the N 1s region.
samples, due to the presence of propane in the reaction
mixture. A higher reduction degree was observed for the V/
Al ratio of 0.1 and 0.25, of 42 and 65%, respectively while
Table 4
Atomic V5+/(V5+ + V4+) surface ratio for fresh and used catalysts
Sample V5+/(V5+ + V4+)
VAlON0.1
Fresh 0.72
Used 0.42
VAlON0.25
Fresh 0.76
Used 0.27
VAlON0.5
Fresh 0.79
Used 0.63
VAlON0.7
Fresh 0.80
Used 0.72
VAlON0.9
Fresh 0.81
Used 0.73
for higher V/Al ratios (0.5, 0.7 and 0.9) the reduction was
about 10–20%.
The formation of different nitrogen species depends on
the V/Al ratio. Fig. 2 presents the N 1s spectra of the fresh
catalysts as a function of the V/Al ratio.
The decomposition of the experimental signal led to three
types of nitrogen containing species. The less energetic one,
corresponding to binding energies in the range 397.1–
396.6 eV, is ascribed to nitride species (N3�) [19]. The
component at about 399.8–400.1 eV corresponds to NHx
groups (x = 1 or 2), and the peak at about 401.8–402.8 eV is
assigned to dinitrogenous species, M–NN–M (where M is V
or Al) [19].
Table 5 shows the atomic composition and the V/Al
surface ratio for the oxynitrides before and after the catalytic
test.
In all the cases, the V/Al surface ratios calculated from
the XPS data are smaller than the theoretical ones. An
increase of the amount of aluminium at the surface was
observed for the used catalyst, and, as a consequence, the V/
Al ratio diminished upon use in propane ammoxidation.
Moreover, an increase of surface nitrogen and a decrease of
the surface oxygen were observed for the used catalysts, due
to the substitution of oxygen by nitrogen during the catalytic
test. The surface nitrogen content increased with decreasing
V/Al ratio up to 0.25. For the VAlON0.1 sample, the
nitrogen content diminished. A similar evolution was
observed for the total nitrogen content (Table 2).
M. Florea et al. / Applied Catalysis A: General 286 (2005) 1–10 5
Table 5
Atomic compositions derived from the XPS analysis for the VAlON
catalysts
Sample N
(% bulka)
Al (%) O (%) V (%) N (%) V/Al
ratio
VAlON0.1
Fresh 4.93 32.95 62.36 1.90 1.77 0.06
Used 2.30 33.83 64.75 2.4 1.32 0.07
VAlON0.25
Fresh 5.35 28.7 65.45 4.20 2.64 0.15
Used 5.18 31.03 61.47 4.0 3.12 0.13
VAlON0.5
Fresh 4.76 21.73 68.02 7.02 2.40 0.31
Used 2.91 28.28 60.05 7.33 2.65 0.26
VAlON0.7
Fresh 3.28 20.94 66.80 8.90 1.18 0.42
Used 1.86 23.0 65.36 8.10 1.76 0.34
VAlON0.9
Fresh 2.26 23.34 67.80 8.20 1.64 0.35
Used 1.80 32.45 62.71 5.90 1.84 0.20
a Determined by Grekov method.
Fig. 4. XPS spectra of the N 1s region for VAlON0.9 for fresh and used
sample.
The comparison of the V 2p spectra for fresh and used
samples (Fig. 3) revealed a different participation of the
vanadium species in the reaction. The component at 515.5–
516.3 eV increased upon exposure to propane ammoxida-
tion, while the component at 517.1–517.5 eV diminished.
Modifications of the used catalyst compared with the
fresh catalyst were also observed in the N 1s region (Fig. 4).
A general trend is the diminution of the signal corresponding
to N3�. Moreover, for VAlON0.9 the components at 396.6–
397.1 and 401.8–402.8 eV corresponding to N3� and to
dinitrogenous species disappeared, as shown in Fig. 4.
However, the surface nitrogen content increased for the used
catalysts (see Table 4).
Fig. 3. XPS spectra of V 2p region for VAlON0.9 and VAlON0.25 for fresh
and used samples.
3.4. Catalytic activity
The catalytic tests were carried out in the optimal reaction
conditions, namely with C3H8:O2:NH3 molar ratio of
1.25:3:1 and 500 8C. No propylene and HCN were detected
in these reaction conditions. A carbon mass balance of 80–
90% was obtained, due to the condensation of acrylonitrile
inside of the connection line between the reactor and the gas
chromatograph.
Fig. 5 presents the conversion of propane and the
selectivity to the reaction products as a function of time on
stream for VAlON0.25.
Propane conversion was almost constant with time on
stream, while the selectivity and yield to acrylonitrile
increased in the first part of the reaction. The steady-state
conditions were reached after 4 h of time on stream.
After 24 h of time on stream the highest selectivity in
acrylonitrile was 50% for a conversion level of propane of
60%. In parallel, the selectivity to COx decreased with time
on stream leading to the idea that the total oxidation became
limited in time. Propylene formation was not observed
during the 24 h of reaction and no deactivation of the
catalyst was noted during this period. For the catalysts with
different V/Al ratios, the trends were similar to that
presented in Fig. 5.
The catalytic activity of the VAlON catalysts depends on
the V/Al ratio as observed from the results depicted in Fig. 6,
after 24 h of reaction.
The optimal V/Al ratio appeared to be 0.25, which
presents the highest ACN yield of 30%. In parallel, for
VAlON0.25, the selectivity to COx was the lowest. The
formation of COx and N2 was favoured over VAlON0.9 and
M. Florea et al. / Applied Catalysis A: General 286 (2005) 1–106
Fig. 5. Time on stream behaviour over VAlON0.25 catalyst, GHSV = 16.8 l/g h, propane:oxygen:ammonia = 1.25:3:1: (~) propane conversion; (&)
selectivity to ACN; (~) yield of ACN; (*) selectivity to AcCN; (*) selectivity to COx; (&) selectivity to N2.
VAlON0.7, with higher content of vanadium and lower
content of nitrogen.
4. Discussion
The study of the relation between structure and activity is
essential to understand the factors controlling the reactivity
and the key features of a catalyst. Particularly, for
ammoxidation catalysts, the role of different vanadium
species (V5+, V4+, V3+) and the role of different nitrogen
species are very important and are still under debate.
To answer these questions, the structural characteristics
of the vanadium aluminium oxynitride catalysts as a
function of the V/Al ratio will first be discussed, and then
related to their catalytic performances.
4.1. Structural changes induced by different compositions
in ‘‘VAlON’’ catalysts
The experimentally determined V/Al molar ratios were
lower than the theoretical values for the ratios higher than
0.7 (see Table 1), probably due to the poor precipitation of
Fig. 6. Catalytic behaviour over VAlON catalysts with different V/Al molar ratio,
propane conversion; (&) selectivity to ACN; (~) yield of ACN; (*) selectivity
vanadium with aluminium in the starting solution. This
appears to be an important parameter in the preparation of
the ‘‘VAlO’’ precursor.
The highest surface area is observed for VAlON0.1 with
the lowest content of vanadium (Table 1). By increasing the
V/Al ratio, the surface area diminished, and in addition, the
nitrogen content diminished as well, this suggesting that, for
higher V/Al ratios, nitrogen insertion was more difficult to
achieve. We observed the same tendency for the total
nitrogen content as for the surface nitrogen determined by
Kjeldahl method.
As indicated in Table 2, the nitrogen content changed for
the used catalysts. This obviously means that the nitridation,
for all the V/Al ratios, does not allow an optimal activation
of the catalysts and that the reduction–oxidation process
during the catalytic test allows to stabilize the solid.
Raman spectroscopy provides information about the
surface vanadium species of the vanadium aluminium oxide
precursor as a function of the V/Al ratio. The survey of the
literature [20] shows the following evolution of the
different vanadium oxide species with the increase of the
vanadium loading: orthovanadate (VO4) ! pyrovanadate
(V2O7) ! metavanadate (VO3)n ! decavanadate (V10O28)
GHSV = 16 800 ml/g h, propane:oxygen:ammonia = 1.25:3:1, 500 8C: (~)
to AcCN; (*) selectivity to COx; (&) selectivity to N2.
M. Florea et al. / Applied Catalysis A: General 286 (2005) 1–10 7
Fig. 7. Variation of different nitrogen component area determined by XPS
as a function of V/Al ratio: (*) N3�; (&) NHx; (~) dinitrogen.
Fig. 8. N3� species determined by differences of total nitrogen and surface
nitrogen (Kjedhal) (&); N3� species determined by XPS (~).
! vanadium pentoxide (V2O5). There are three possible
active bridging oxygen sites: terminal V O, binding surface
polymeric species V–O–V, and binding vanadium to support
V–O–S. The isolated vanadium oxide species have one
terminal V O bond and three V–O–Al bonds, while the
polymeric vanadium oxide species consist of a terminal V O
bond with one V–O-support and two bridging V–O–V bonds.
[21].
The spectra of the vanadium aluminium oxide precursor
presented in Fig. 1 as a function of vanadium loading are in
agreement with the literature data, meaning that higher
vanadium contents favour the formation of decavanadate
species (band at 980 cm�1). Besides, the decrease of the
vanadium loading increased the quantity of isolated
vanadium species (band at 1050 cm�1) and of metavanadate
species (band at 940 cm�1) formed.
A correlation can be made between the nature of the
vanadium oxide species and the nitrogen content. For the
higher V/Al ratios, the V–O–V bonds of polymeric
vanadium oxide species are predominant and at the same
time the nitrogen content decreases, while for the lower V/
Al ratios there is a predominance of the V–O–Al bonds of
isolated vanadium oxide species type and the nitrogen
content is higher. This suggests that, when increasing
concentration of the monomeric vanadium species, the
degree of nitridation increases and one may suppose that
the oxygen replaced by nitrogen during the nitridation
process could be the one bridged to V and Al. Thus, the
substitution of oxygen by nitrogen is favoured for the
lower V/Al ratios, for which we found a higher surface
concentration of isolated vanadium species. Also, if we
take in account the type of coordination of vanadium in
these different species, one can observe that the tetrahedral
coordination favours the substitution of oxygen by
nitrogen, while for the octahedral coordination the
nitridation is more difficult.
The XPS data also shows differences as a function of the
V/Al ratio, as for example: (i) generation of different
nitrogen species, and (ii) different reduction degree of
vanadium.
Fig. 7 points to a direct relation between the V/Al ratio
and the type of nitrogen species as determined by XPS
formed during the nitridation process.
This plot shows that the formation of nitride species
(N3�) is favoured at high V/Al ratio while the amount of
NHx species is favoured on the samples with low V/Al ratios.
However, the total amount of nitrogen species increased
with the decrease of the V/Al ratio.
Contradictory results are obtained from the chemical
analysis of the total and surface nitrogen content. If we admit
that the difference between the total nitrogen content
determined by Grekov method and the surface nitrogen
content determined by Kjeldahl method represent the
amount of N3� species from the bulk of the catalysts, one
can observe that the amount of N3� species increases with
decreasing V/Al ratio (Fig. 8).
The amount of bulk nitrogen species (N3�) determined
from the differences between total and surface nitrogen
contents (from chemical analysis), as well as N3�
determined by XPS, are plotted in Fig. 8.
It is seen that the bulk nitrogen determined by chemical
analysis and by XPS is the same for the VAlON0.9 sample,
indicating the homogeneity of this sample. It is well known
from the literature and supported by the RAMAN spectra of
the VAlO samples, that when the vanadium loading
increases, the possibility of formation of surface poly-
vanadates increases [22]. If we take into account that, in the
case of VAlON catalysts these polyvanadate species are
formed for the higher V/Al ratios, it indicates that the
nitridation of these species seems more difficult to achieve
and probably only the terminal V O species could be
nitrided. When the V/Al molar ratio diminishes, the
probability of formation of polyvanadate species diminishes,
and the nitridation is much deeper for lower V/Al ratio. The
increase of the total and surface nitrogen content with the V/
Al molar ratio is consistent with this hypothesis.
The fact that, after the catalytic test, the bulk nitrogen
content diminished compared with the bulk nitrogen content
for the fresh samples can be explained by the migration of
M. Florea et al. / Applied Catalysis A: General 286 (2005) 1–108
Fig. 9. Correlation between the bulk nitrogen and degree of reduction of
vanadium.
the nitride species to the surface of the catalyst during the
catalytic test in the presence of oxygen from the reaction
mixture. This phenomenon was also observed during the
oxidation of ‘‘AlGaPON’’ catalysts [23]. Moreover, in the
case of the VAlON0.9 catalysts, the component correspond-
ing to N3� disappeared after the reaction, as a consequence
of the consumption of these species during the reaction.
Another relevant aspect of the VAlON catalysts
determined from the XPS data is the reduction degree of
vanadium. The XPS spectra of the fresh catalysts present a
split of the V 2p3/2 level, observed at 517.1–517.5 and
515.5–516.3 eV (Table 3). Taking into account the limitation
in the assignment of these peaks, an approximate estimation
of the atomic V5+/(V5+ + V4+) surface ratio can be made
using the XPS technique (Table 4). For the ‘‘VAlON’’
samples, the atomic V5+/(V5+ + V4+) surface ratio decreases
with increasing V/Al ratio. Moreover, by decreasing the V/
Al ratio, the amount of nitrogen incorporated during the
nitridation process increases, and as consequence the
reduction degree of vanadium increased. The reduction
degree of vanadium as a function of bulk nitrogen is shown
in Fig. 9.
This dependence presented in Fig. 9 suggests that the
oxidation state of vanadium depends on the quantity of
nitrogen inserted by oxygen substitution. Thus, the highest
degree of reduction of vanadium (0.72) corresponds to the
highest content of bulk nitrogen inserted by nitridation
(2.73%). However, both the degree of nitridation and the
degree of reduction could be linked to the degree of
polymerisation of vanadium.
A diminution of atomic V5+/(V5+ + V4+) surface ratio is
observed for all the used catalysts, meaning that vanadium is
also reduced during the reaction (Table 5), due to the
presence of propane and ammonia in the gas feed. The
highest reduction occurring for the lower V/Al ratio, which
could be explained by the presence of isolated vanadium
species, are easier to reduce as compared with the polymeric
species [24].
The progressive and general decreasing trend of the
binding energies of Al 2p with the atomic nitrogen
percentage, as presented in Table 3, was explained by the
higher nucleophilic character of nitrogen compared to
oxygen, which reduces the positive charge around the
aluminium. The role of Al3+ ions in the VAlON system is not
yet well established. We believe that aluminium ions are not
directly involved in the catalytic reaction. However, they
could play an important role in increasing the surface
dispersion of vanadium.
In summary, the catalysts characterization showed the
following trends as a function of the V/Al ratio: (i) the
surface area increases with the decrease of the V/Al ratio, (ii)
the nitrogen content increases with the decrease of V/Al
ratio, (iii) the type of nitrogen species depends on the V/Al
ratio, higher content of bulk nitrogen was observed for the
lower V/Al ratio, (iv) higher degree of polymerisation of
vanadium oxide species for the higher V/Al ratio and (v) the
reduction degree is different as a consequence of the
nitrogen insertion during the nitridation step.
4.2. Study of the catalytic behaviour
The catalytic performances of ‘‘VAlON’’ as a function of
the V/Al ratio of the catalysts are presented in Fig. 6. The
increase of the V/Al ratio from 0.25 to 0.9 leads to: (i) a
decrease of the selectivity to acrylonitrile, (ii) an increase of
the selectivity to carbon oxides and (iii) an increase of the
amount of nitrogen formed by ammonia oxidation. It must
be stressed that regardless of the V/Al ratio, the conversion
of propane is nearly constant. The highest yield of
acrylonitrile is obtained over VAlON0.25.
Particular results were obtained for the VAlON0.1
sample, with the lowest vanadium content: (i) a decrease
of the selectivity to acrylonitrile is accompanied by (ii) a
decrease of propane conversion, indicating that under these
conditions there are not enough active sites for propane
activation.
As seen in Fig. 5, the steady-state conditions are achieved
after 4 h on stream. An explanation of this phenomenon
could be the fact that the degree of reduction of the catalyst
can increase with time on stream due to the presence of
propane and ammonia in the gas feed. Also, these results
correlate well with the increase of the nitrogen content as a
function of time on stream, until the steady state is reached.
Below, we shall attempt to correlate the catalytic
behaviour of the VAlON system with two important
parameters, which depend on the V/Al molar ratio: (i) the
reduction degree of vanadium and (ii) the quantity and type
of nitrogen species.
In order to establish a structure–activity relationship and to
understand the factors controlling the reactivity and the key
features of the catalyst, the role of different vanadium species
(V5+, V4+, V3+) in propane ammoxidation mechanism is often
under debate. Most of the studies attribute the activation of
propane to V5+ and V4+ centers [25]. However, a recent
publication stressed that V3+ may also have an effect on the
enhancement of the activity of an alkane molecule [26].
M. Florea et al. / Applied Catalysis A: General 286 (2005) 1–10 9
Fig. 10. Selectivity to ACN (&), nitrogen (&) and conversion of propane
(~) as a function of the V5+/(V5+ + V4+) ratio determined by XPS.
Fig. 10 depicts the catalytic results of the ‘‘VAlON’’
system as a function of the surface V5+/(V5+ + V4+) atomic
ratios measured after the catalytic test. With decreasing
surface V5+/(V5+ + V4+) atomic ratio, the selectivity to
acrylonitrile increased and reached a maximum for
VAlON0.25.
It should also be mentioned that the formation of nitrogen
from ammonia oxidation and the carbon oxides production
from total oxidation reaction increased with the increase of
the amounts of the V5+ species. These species enhance the
side reaction of ammonia oxidation to N2 (see Fig. 10). From
the literature, it is known that V2O5 is the active phase for the
oxidation of ammonia into nitrogen [27,28]. A maximum of
the catalytic activity is obtained for the V5+/(V5+ + V4+)
ratio of 0.27 (VAlON0.25 sample). Thus, the presence of V5+
species in large amounts on the surface has a negative effect
due to side reactions, but its role when present in lower
amounts is questionable. The most efficient sites of the
VAlON system for the acrylonitrile formation seems to be
the V4+ species, which agrees with the recent studies of
Millet and coworkers on the oxidation state of vanadium in
mixed vanadium and iron antimonite oxides [29].
By changing the V/Al ratio, the degree of the nitridation
is different, as it was observed from the XPS results. Since
the catalytic activity of the VAlON in propane ammoxida-
Fig. 11. Selectivities to ACN (&) and COx (*) as a funct
tion depends on the V/Al ratio, and that the nitrogen content
also depends on the V/Al ratio, we can admit that the
quantity of nitrogen generated by nitridation has an
influence on the catalytic behaviour. Indeed, the selectivity
to ACN as well as the formation of COx depends on the bulk
nitrogen content as well as on the surface nitrogen content,
illustrated in Fig. 11. The selectivity to acrylonitrile
increases with the nitrogen content, both for surface and
bulk nitrogen species, indicating the role of these species in
the N-insertion step to form acrylonitrile.
Changes in the concentration of nitrogen species were
observed upon use in propane ammoxidation, indicating the
participation of nitrogen species from the VAlON frame-
work in the N-insertion step to form acrylonitrile. Thus, it is
necessary to pay a special attention to the surface
restructuring phenomena during the catalytic reaction, as
a central aspect for the understanding of the surface
reactivity of the oxynitrides. On the vanadium aluminium
oxynitrides, this phenomenon is possible as the nitridation
process is a reversible one. This behaviour was observed also
on aluminium phosphate oxynitride catalysts, AlPON [23],
and should be confirmed on the case of VAlON.
Taking into account that (i) the total nitrogen content of
VAlON catalysts is modified upon use in propane
ammoxidation according to XPS and chemical analysis,
and (ii) the nitridation process is a reversible one, a Mars and
Van Krevelen mechanism applied to nitrogen could be
considered. Deeper investigations of this phenomenon are
the subject of others studies performed over VAlON
catalysts and will be published elsewhere [30].
As indicated by the above results, propylene formation as
an intermediate was not observed for all the series of VAlON
systems. Moreover, by performing propylene ammoxidation
on these catalysts a conversion of 100% was reached. This
observation, together with the fact that the VAlON system
shows a high acrylonitrile selectivity at very low space–time
value, suggests a different reaction mechanism as compared
with conventional metallic oxide ammoxidation systems. In
the case of VAlON, the catalytic behaviour can be explained
by a combination of different simultaneous effects: (i) a
better efficiency in the activation of the C–H bond of the
ion of the bulk nitrogen (a) and surface nitrogen (b).
M. Florea et al. / Applied Catalysis A: General 286 (2005) 1–1010
alkane due to a balanced redox capacity of vanadium
species, and (ii) a high nitrogen content which enhances the
nitrogen insertion rate for the acrylonitrile formation.
5. Conclusions
The results presented above show that the catalytic
performances depend on the V/Al ratio, with an optimal
selectivity to acrylonitrile obtained for V/Al of 0.25. These
results could be explained by an optimal degree of
polymerisation of vanadium species from oxide precursor,
which induces an optimal degree of nitridation and, further,
an optimal reduction degree of vanadium.
The prior nitridation of the V–Al oxide precursor with the
generation of the nitrogen species is beneficial for
ammoxidation of propane, indicating the positive role of
these species in this reaction. The results obtained in this
reaction established that these new compounds are important
catalytic materials, presenting tuneable properties by
variation of both the V/Al and N/O ratios.
Acknowledgements
The authors would like to thank the ‘‘Direction Generale
des Technologies, de la Recherche et de l’Energie’’ de la
Region Wallonne (GREDECAT) and ‘‘La Communaute
Francaise de Belgique’’ for financial support.
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