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Methane combustion on some perovskite-like mixed oxides
Davide Ferri, Lucio Forni*
Dipartimento di Chimica Fisica ed Elettrochimica, UniversitaÁ di Milano, Via C. Golgi 19, I-20133 Milan, Italy
Received 18 May 1997; received in revised form 18 July 1997; accepted 18 July 1997
Abstract
Some perovskite-like mixed oxides of general formula La1ÿxA0xBO3 were prepared by the amorphous citrate method and
tested for methane combustion within the 300±6008C temperature range. Substitution at A-site with a bivalent (Eu, Sr) or
tetravalent (Ce) metal cation led to a decrease or increase of catalytic activity, respectively. La0.9Ce0.1CoO3 proved to be the
most active catalyst, showing complete conversion at 5008C. The nature of the metal cation introduced modi®es the oxidation
state of cobalt, which leads to the formation of cationic or anionic vacancies. TPD-MS analysis con®rmed that the catalytic
activity is related to the oxygen storage properties of the catalyst. The substitution at B-site (B � Fe, Co, Ni) allowed to ®nd
interesting correlations between catalytic activity and the temperature Tmax of maximum oxygen desorption rate. # 1998
Elsevier Science B.V.
Keywords: Perovskite as catalyst; Methane combustion; Oxygen mobility
1. Introduction
In the past decades, the interest for catalytic com-
bustion has grown increasingly [1] due to increasing
legislative restrictions on gaseous emissions from
either fossil fuel burners or vehicles. At low tempera-
ture, when the combustion is ¯ameless, the formation
of harmful species such as CO or NOx is limited or
virtually absent. Traditional catalysts for methane
combustion are: supported noble metals, such as
Pd=Al2O3 and Pt=Al2O3 or their combination with
Rh or Ir as in the three-way converters. The main
advantage of noble metals is their ability to activate
both the C±H and O±O bonds. These materials show
high activity even below 3508C [2], but their com-
mercial exploitation is hampered by the relatively high
volatility of oxides, sintering ease above 5008C and
mainly by cost [3]. Hence, much effort has been
devoted to the substitution of noble metal catalysts
with mixtures of selected metal oxides. Perovskite-
like mixed oxides, with general formula ABO3,
showed suitable catalysts for oxidation of light hydro-
carbons and, in particular, of methane [4±7].
Perovskite-like oxides can be tailored to create a
wide family of catalysts, by varying either the A-site
or the B-site metal ion, or both. Indeed, the catalytic
activity of a perovskite can be modi®ed by inserting
proper transition metal ions. Moreover, partial sub-
stitution at A-site with another A0 metal cation to give
A1ÿxA0xBO3�d can strongly affect catalytic activity,
due to stabilisation of unusual oxidation states of the B
Applied Catalysis B: Environmental 16 (1998) 119±126
*Corresponding author. Tel.: +39-2-26603289; Fax: +39-2-
70638129; E-mail: [email protected]
0926-3373/98/$19.00 # 1998 Elsevier Science B.V. All rights reserved.
P I I S 0 9 2 6 - 3 3 7 3 ( 9 7 ) 0 0 0 6 5 - 9
component and to simultaneous formation of struc-
tural defects created by such a substitution. Catalytic
activity is admittedly ascribed to the B-site cation, the
lanthanide ion at A-site being considered responsible
for thermal endurance of the catalyst. However, the
size of this cation seems to play a role [7,8], since the
ionic radii of both A and B cations are important for
conferring stability to the perovskitic structure [9].
Structural defects are responsible not only for part
of the catalytic activity, but also for oxygen mobility
within crystal lattice of the solid, due to the non-
stoichiometry created by substituting A0 for A. The
presence of ionic vacancies affects catalytic activity
by favouring or non-favouring the adsorption of reac-
tant from the gas phase.
In the present work, different sets of perovskite-type
mixed oxides, of general formula La1ÿxSrxCoO3
(x�0, 0.2 and 0.4), La0.8Sr0.2BO3 (B�Fe and Ni)
and La0.9A0CoO3 (A0 � Eu and Ce), were prepared,
characterised and tested as catalysts for methane oxi-
dation under ¯ameless conditions. The aim of the
work was to analyse the in¯uence on catalytic activity
of the nature of B-site metal cation and of the substi-
tution of bivalent or tetravalent cations, such as Sr, Eu
or Ce for La. A study of the oxygen storage properties
of these perovskites was also carried out, in order to
correlate these properties with catalytic activity.
2. Experimental
2.1. Materials
Starting nitrates of metal constituents were pur-
chased from ACROS and MERCK. All materials were
pro-analysi reagents, with >98% purity, except nickel
nitrate (97%). For testing catalytic activity a S.I.A.D.
certi®ed gas mixture of 1.00 vol% CH4 in nitrogen was
used, mixed with S.A.P.I.O. �99.999% pure air. Pure
helium (S.I.A.D. �99.999 vol%) was used both as
carrier and as auxiliary gas for gas chromatographic
(GC) analysis. Ultrapure helium carrier gas (S.I.A.D.
�99.9999%) and oxygen (S.A.P.I.O. �99.999 vol%)
were employed for TPD-MS experiments.
2.2. Catalysts preparation
Catalysts were prepared by the so-called citrate
method [10]. Aqueous solutions of starting nitrates
were mixed with an aqueous solution of citric acid.
The molar ratio between the total amount of nitrates
and citric acid was 1 : 1. The resulting solution was
evaporated at 708C and then completely dried in a
vacuum oven overnight at 708C. The spongy material
thus obtained was crushed and calcined for 2 h in
¯owing air at the temperature determined by thermo-
gravimetric analysis (TGA, vide infra). The main
characteristics of the catalysts prepared are sum-
marised in Table 1.
2.3. Catalysts characterisation
TGA analysis of catalysts precursors was carried
out by means of a Mettler Toledo TA 8000 instrument,
on ca. 10 mg samples, with a temperature ramp of
108C=min from room temperature up to 10008C. XRD
patterns were obtained by a Siemens D-500 diffract-
ometer, using the Cu Ka (�1.5148 AÊ ) radiation, Ni-
®ltered, for all solids, except LaCoO3, for which the
Co Ka (�1.79026 AÊ ) radiation was used. Reference
spectra were compared with the J.C.P.D.S. data [11]
for structure assignment. Surface areas were deter-
mined by nitrogen sorption±desorption (B.E.T.
method), by a Carlo Erba Sorptomatic-1800 instru-
ment.
2.4. Catalytic activity tests
Methane oxidation was carried out in a quartz ®xed-
bed reactor (I.D.�0.6 cm, L�45 cm). The catalyst
powder (ca. 200 mg) was pelleted, crushed, sieved to
60±100 mesh (0.02±0.04 mm) and mixed with ca.
Table 1
Main characteristics of the catalysts employed
Catalyst Code Tc
(8C)
Phase(s) a S.A.
(m2=g)
LaCoO3 Co 640 P (�La2CO5) 11
La0.8Sr0.2CoO3 02-Co 580 P (�SrCO3) 19
La0.6Sr0. 4CoO3 04-Co 580 P (�SrCO3) 8
La0.9Eu0.1CoO3 Eu01-Co 600 P 16
La0.9Ce0.1CoO3 Ce01-Co 580 P (�CeO2) 22
La0.8Sr0.2FeO3 02-Fe 680 P (�SrCO3) 21
La0.8Sr0.2NiO3 02-Ni 800 P (�SrCO3�NiOx) b 5
a P� perovskite. In parentheses, the phases forming in minor
amounts.b NiOx � various Ni oxides.
120 D. Ferri, L. Forni / Applied Catalysis B: Environmental 16 (1998) 119±126
1.3 g of quartz (60±100 mesh). The catalyst bed was
inserted in the reactor tube between quartz beads (20±
60 mesh), to favour gas mixing and heat transfer
between gas and solid. A detailed sketch of the
apparatus was given in a previous work [6].
Catalytic tests were carried out by feeding the
reactor with a total ¯ow of 40 N cm3=min of CH4
in nitrogen gas mixture and air, so as to have 0.5 vol%
of methane. The catalysts were previously activated
overnight in 40 N cm3=min ¯owing air at 508C below
the calcination temperature. After cooling down to
3008C in air, feeding of methane gas mixture was
started (20 N cm3=min), reducing the air ¯ow to
20 N cm3=min. A 28C=min ramp was then begun,
from 3008C up to 6008C, while analysing the ef¯uent
gas every 12 min, by on-line GC.
2.5. TPD-MS analysis
Oxygen TPD-MS analysis was carried out using the
apparatus described in detail in a previous paper [12].
The quartz micro-reactor was loaded with ca. 100 mg
of catalyst. The catalyst was activated in ultrapure
helium (20 N cm3=min) overnight at proper tempera-
ture, 508C below the calcination temperature. The
¯owing gas was then swept to 15 N cm3=min oxygen
for 15 min and the sample cooled down to 508C in
¯owing oxygen. At 508C, O2 was swept to He and,
after attaining the steady state conditions, a 108C=min
temperature ramp was started from 508C up to 8008C,
while continuously monitoring by the quadrupolar MS
the fragments with m=z � 18, 28, 32 and 44, corre-
sponding to water, CO, oxygen and CO2, respectively.
3. Results
3.1. Catalysts characterisation
TGA analysis of citrates showed three decomposi-
tion steps, as also described by other authors [13]. The
temperature chosen for calcining the catalysts was ca.
208C higher than that corresponding to the third step
of the TGA thermogram, i.e. ca. 208C above the lowest
temperature needed for the formation of perovskite-
like structure. This temperature is well below that
usually needed for the preparation of perovskites by
the traditional route, so that B.E.T. surface area of the
present ®nished samples is up to one order of magni-
tude higher.
XRD patterns (Fig. 1) con®rm the formation of the
pure perovskite-like structure for the Eu-containing
system. In Ce01±Co, calcined both at 5808C and
8008C, CeO2 was hardly detected, since very weak
re¯ections attributable to that phase were observable
(Fig. 1g and h, respectively). In a previous work [12],
it was shown that the solubility of cerium in
La1ÿxCexCoO3 is limited to x�0.05, probably due
to that preparation method and to the high calcination
temperature needed for forming the perovskite-like
structure. Tabata et al. [14] and Nitadori et al. [15]
found CeO2 in their La1ÿxCexCoO3 samples; they
used also high calcination temperature for synthesis.
As for the Sr-containing catalysts (Fig. 1b,c) XRD
analysis showed a small amount of SrCO3, besides the
perovskite-like structure. Co, the only sample ana-
lysed by the Co Ka radiation, showed a small amount
of La2CO5 phase and probably also a trace of Co3O4
(Fig. 1a), as already observed by Daturi et al. [16] for
a similar catalyst. The 02±Ni (Fig. 1e) and 04±Co
(Fig. 1c) samples showed more complex diffracto-
grams, the SrCO3 phase seeming more abundant than
in other catalysts. Some of the re¯ections could be
attributed also to other oxides. In fact, Zhao et al. [17]
reported the presence of mixed oxides such as the
La2NiO4 of K2NiF4 structure or LaNiO3 phases for the
La1ÿxSrxNiO3 series. Finally, for 04±Co the SrCO3
phase seems to be the most abundant secondary
compound.
3.2. Catalytic activity and TPD results
Catalytic activity data for methane combustion are
presented in Fig. 2. They are in accordance with
literature data [14,18]. By expressing the activity
through the light-off temperature (T50) at which
50% of methane conversion is reached, Ce01±Co
appears the most active catalyst.
In the series La1ÿxSrxCoO3 (x�0, 0.2 and 0.4),
the maximum activity is for x�0.2 and the order is
02±Co>Co>04±Co, as it was also found by Tabata et
al. [19]. On the other hand, in the series La0.8Sr0.2BO3
(B�Fe, Co and Ni) the Co-based system proved more
active than the other two catalysts, for which T50
showed practically the same value. At T>T50 02±Ni
appeared more active than 02±Fe and 100% conver-
D. Ferri, L. Forni / Applied Catalysis B: Environmental 16 (1998) 119±126 121
sion was attained around 5508C. Ce01±Co was
more active than the corresponding Eu-containing
system.
CO was never detected in the products for any
catalyst, and for every catalyst methane combustion
took place within the 300±6008C temperature range,
Fig. 1. XRD patterns. (a) Co; (b) 02-Co; (c) 04-Co; (d) 02-Fe; (e) 02-Ni; (f) Eu01±Co; (g) Ce01±Co; and (h) Ce01±Co calcined at 8008C. Cu
Ka radiation, Ni filtered, except for sample (a), for which the Co Ka radiation was used. (*) Perovskite; (*) SrCO3; and (5) CeO2.
122 D. Ferri, L. Forni / Applied Catalysis B: Environmental 16 (1998) 119±126
whereas for the Ce-containing cobaltate catalyst, full
conversion was achieved at 5008C.
TPD spectra (Fig. 3) show that all the present
catalysts release more oxygen than the corresponding
Mn-based perovskites [6]. The spectra present two or
three desorption peaks within the 200±8008C tem-
perature range. The high-temperature peak is, how-
ever, less important for methane combustion, since the
reaction takes place at much lower temperature. The
low-temperature peak has been attributed to supraf-
acial adsorbed oxygen, while the oxygen released
around 5008C may be considered as coming from
the bulk of the solid. This oxygen species occupy
the inner vacancies created by substitution of Sr for La
or by segregation of La-containing phases (as in the
present Co sample) [20].
At almost the same temperature Ce01±Co released
a larger amount of oxygen with respect to Eu01±Co,
but its high-temperature peak is shifted to lower
temperature (<6008C). In the La1ÿxSrxCoO3 series
the amount of oxygen released is larger for x�0.4,
while for x�0 and 0.2 the catalysts behaved compar-
ably from this point of view. For the La0.8Sr0.2BO3
series the order for oxygen desorption was 02±Ni>02±
Fe�02±Co. The Fe- and Ni-perovskites showed only
two desorption peaks, while all the Co-perovskites
showed three, at ca. 250, 600 and 8008C, respectively.
This means that oxygen mobility is higher than in the
corresponding manganites [6] which released oxygen
only at 6008C.
These results lead to the conclusion that activation
of the oxygen molecule is possible at low temperature
Fig. 2. Methane conversion for the series (a) La0:9A00:1CoO3
(A0 � Ce, Eu); (b) La1ÿxSrxCoO3 (x�0, 0.2, 0.4); and (c) ±
La0.8Sr0.2BO3 (B�Fe, Co, Ni).
Fig. 3. TPD spectra after O2 saturation. (a) Ce01±Co; (b) Eu01±
Co; (c) 04±Co; (d) 02±Co; (e) Co; (f) 02±Ni; and (g) 02±Fe.
D. Ferri, L. Forni / Applied Catalysis B: Environmental 16 (1998) 119±126 123
(ca. 2008C), whereas activation of the C±H bond
appears to be more dif®cult, the reaction starting in
any case only above 3008C.
4. Discussion
It is well known that in perovskite-like mixed
oxides substitution of the trivalent A-site metal ion
with a bivalent or tetravalent metal cation (A0) is
accompanied by a modi®cation of the oxidation
state of B-site metal cation, thus modifying catalytic
activity. Moreover, modi®cation of the oxidation
state of B-site metal cation by insertion of A0 may
be accompanied by the formation of structural
defects, thus leading to non-stoichiometry. In the
Co-containing perovskites this usually means
oxygen defects, while in Mn-perovskites it results
in oxygen excess [9]. Fe [18] and Ni-based perovskites
[21] were shown to have an intermediate behaviour. In
the latter, formation of anionic vacancies seems to be
easier than oxidation of Ni3� to Ni4�, since the ionic
radius of oxidised species does not ®t the perovskitic
structure.
In Ce01±Co and in Eu01±Co the low calcination
temperature leads to pure perovskite, and CeO2 was
hardly detected. The presence of a small amount of
this phase means that not all of Ce4� has been
incorporated within the perovskitic structure. This
results in either partial reduction and oxidation of
Co, Co3� being the average oxidation state in these
perovskites. In fact, cation vacancies are created at A-
site by the insertion of Eu2�, resulting in the oxidation
of Co3� to Co4�, while the insertion of Ce4� brings
about the reduction to Co2�.
The case of Sr2�-catalysts is similar to that of Eu-
containing ones. Sr substitution for La leads to higher
oxidation states for Co, so that the higher the amount
of Sr, the higher is the concentration of Co4�. How-
ever, since Co4� is particularly unstable, then some
oxygen release can take place, ending in the formation
of oxygen vacancies. Furthermore, XRD patterns of
this series show the formation of SrCO3, very likely
accompanied by the formation of cation vacancies.
This is in line with TPD data of La1ÿxSrxCoO3 sam-
ples (Fig. 3) showing that by increasing x the con-
centration of Co4� increases, as the amount of
desorbing oxygen increases accordingly.
By contrast, as previously shown [6], Mn-based
perovskites released oxygen in the opposite order,
i.e. by increasing x the amount of released oxygen
decreases, due to a decrease of cation vacancies con-
centration. It can be concluded that the substitution of
a bivalent cation for La3� is accompanied by oxidation
of the B cation. On the contrary, insertion of Ce4�
leads to partial reduction of the B-site metal cation.
According to Wu [18] and Tabata [19], by increas-
ing x in La1ÿxSrxCoO3 more oxygen is released. In the
present case, the maximum activity falls at 20%
substitution of Sr for La. 04±Co is less active than
02±Co, though it releases a larger amount of oxygen,
as shown by TPD measurements (Fig. 3). Indeed,
oxygen vacancies are directly connected with oxygen
mobility. The higher the amount of anion defects (the
higher the value of x), the higher is the oxygen
mobility. However, a too high oxygen release is
accompanied by a dif®cult surface reoxidability
[22], so leading to a less active catalyst.
Oxygen TPD signals for perovskite-like oxides are
usually attributed to release of oxygen species situated
at structural defects, i.e. essentially oxygen from the
bulk [23]. However, since a relatively large amount of
structural defects is present in these catalysts, a part of
desorbing oxygen can be due to surface species too.
The high-temperature peak (Fig. 3) is surely attribu-
table to more tightly bound oxygen, i.e. to structural
bulk oxygen. However, the low-temperature peaks
(200±6008C) correspond to oxygen originated by
the reduction process involving the B-site metal
[24] and the formation of anionic vacancies. At low
temperatures, methane combustion on these catalysts
is a suprafacial reaction [25] involving oxygen coming
from the gas phase or sitting in the anion vacancies of
the catalyst [20]. In fact, it has been shown [4] that
methane combustion rate depends on CH4 partial
pressure only at low temperature, whereas at high
temperature CH4 reacts with the oxygen supplied
by the catalyst and coming from the bulk (intrafacial
mechanism [25]). Our data con®rm these ®ndings,
showing that for all the catalysts (Fig. 2) the rate of
methane oxidation boosts when bulk oxygen becomes
available.
Fig. 2a data show also that Ce01±Co is more active
than Eu01±Co. Besides the larger amount of oxygen
available for methane oxidation, as indicated by the
TPD patterns (Fig. 3), XPS data (not reported here) for
124 D. Ferri, L. Forni / Applied Catalysis B: Environmental 16 (1998) 119±126
Ce01±Co indicate the presence of Co2�, generated by
the insertion of Ce4� for La3�. This leads to the
presence of a larger amount of active sites for oxygen
adsorption from gas phase, i.e. an easier reoxidability
of the catalyst.
In our La0.8Sr0.2BO3 series, where B is Fe, Co or Ni,
Sr substitution for La is accompanied by oxidation of
part of B species up to Fe4�, Co4� or Ni4�, respec-
tively. 02±Co proved more active than 02±Fe and 02±
Ni. It released oxygen at ca. 2508C, while 02±Fe and
02±Ni at ca. 3608C and 4008C, respectively (Fig. 3).
Formation of oxygen defects promotes oxygen
adsorption from gas phase. Therefore, in the 02±Co
sample the formation of defects due to cobalt reduc-
tion to Co3� is enhanced, resulting in a higher activity
since that temperature. The difference in activity of
these catalysts can also be ascribed to the different
stability of the mentioned uncommon oxidation states
created by substituting Sr2� for La3�.
Finally, the activity data here obtained allow us to
compare the two families of cobaltates and manga-
nites, which have been taken as reference catalysts for
a wide number of reactions [2,20,26±30]. It is clear
that Co- and Mn-based perovskites behave in an
opposite way and that, by substituting A0 (Sr, Eu or
Ce) for A, different situations are encountered. Co-
based perovskites are oxygen de®cient and charac-
terised by the presence of anionic vacancies, favouring
oxidation catalysis. On the other hand, in Mn-based
catalysts an excess of oxygen and cationic vacancies
are present and anionic vacancies seem to appear only
beyond a given value of x [6,31]. As a consequence,
substitution of Eu or Ce for La brings about a different
behaviour towards methane combustion. Ce01±Co is
more active than Eu01-Co while Eu01-Mn is more
active than Ce01-Mn [6]. The Co-based catalysts
release more oxygen, while the manganites release
less oxygen and only at ca. 6008C. Oxygen mobility is
thus higher for the former and the activity for methane
oxidation increases accordingly from Mn- to Co-based
perovskites. However, it must be kept in mind that also
the stability of the B-site metal cation affects the
activity. In manganites the introduction of Sr2� leads
to Mn4� and to cationic vacancies, since Mn4� is more
stable than Mn3� [22]. In the cobaltates Co4� is less
stable than Co3�, thus leading to reduction, oxygen
release and creation of oxygen vacancies. Hence, the
different stability of the oxidation state of B-site cation
may reduce the difference in activity between the two
series of catalysts.
Acknowledgements
We are grateful to M. Catti and A. Sironi for XRD
analysis and to A. Lunghi of the Stazione Sperimen-
tale per i Combustibili, S. Donato Milanese, for TGA
analysis. Thanks are due also to R. Revilla for his help
in experimental work.
References
[1] J. Saint-Just, J. der Kinderen, Catal. Today 29 (1996) 387.
[2] R. Doshi, C.B. Alcock, N. Gunasekaran, J.J. Carberry, J.
Catal. 140 (1993) 557.
[3] M.F.M. Zwinkels, S.G. JaÈraÊs, P.Govind Menon, T.A. Griffin,
Catal. Rev.-Sci. Eng. 35(3) (1993) 319.
[4] H. Arai, T. Yamada, K. Eguchi, T. Seiyama, Appl. Catal. 26
(1986) 265.
[5] Y. Teraoka, H.M. Zhang, N. Yamazoe, Proc. 9th Intern.
Congress in Catalysis, Calgary, (1988) (M.J. Phillips, M.
Ternan Eds.), The Chemical Institute of Canada, Ottawa, vol.
4, p. 1984.
[6] L. Marchetti, L. Forni, Appl. Catal. B Environ. (1997) in
press..
[7] A. Baiker, P.E. Marti, P. Keusch, E. Fritsch, A. Reller, J.
Catal. 146 (1994) 268.
[8] P.E. Marti, A. Baiker, Catal. Lett. 26 (1994) 71.
[9] L.G. Tejuca, J.L.G. Fierro, J.M.D. TascoÂn, Adv. in Catal. 36
(1989) 237.
[10] M.S.G. Baythoun, F.R. Sale, J. Mater. Sci. 17 (1982) 2757.
[11] Selected Powder Diffraction Data, Miner. DBM (1-40),
J.C.P.D.S., Swarthmore, PA, 1974±1992.
[12] L. Forni, C. Oliva, F.P. Vatti, M.A. Kandala, A.M. Ezerets,
A.V. Vishniakov, Appl. Catal., B: Environmental 7 (1996)
269.
[13] H.M. Zhang, Y. Teraoka, N. Yamazoe, Chem. Lett., (1987)
665.
[14] K. Tabata, I. Matsumoto, S. Kohiki, M. Misono, J. Mater. Sci.
22 (1987) 4031.
[15] T. Nitadori, M. Misono, J. Catal. 93 (1985) 459.
[16] M. Daturi, G. Busca, R.J. Willey, Chem. Mater. 7 (1995)
2115.
[17] Z. Zhao, X. Yang, Y. Wu, Appl. Catal., B: Environmental 8
(1996) 281.
[18] Y. Wu, T. Yu, B.S. Dou, C.X. Wang, X.F. Xie, Z.L. Yu, S.R.
Fan, Z.R. Fan, L.C. Wang, J. Catal. 120 (1989) 88.
[19] K. Tabata, I. Matsumoto, S. Kohiki, J. Mater. Sci. 22 (1987)
1882.
[20] K.S. Chan, J. Ma, S. Jaenicke, G.K. Chuah, J.Y. Lee, Appl.
Catal. A: General 107 (1994) 201.
[21] Z. Yu, L. Gao, S. Yuan, Y. Wu, J. Chem. Soc. Faraday Trans.
88(21) (1992) 3245.
D. Ferri, L. Forni / Applied Catalysis B: Environmental 16 (1998) 119±126 125
[22] N. Yamazoe, Y. Teraoka, Catal. Today 8 (1990) 175.
[23] N. Yamazoe, Y. Teraoka, T. Seiyama, Chem. Lett., (1981)
1767.
[24] Y. Teraoka, M. Yoshimatsu, N. Yamazoe, T. Seiyama, Chem.
Lett., (1984) 893.
[25] J.L.G. Fierro, Catal. Today 8 (1990) 153.
[26] L.A. Isupova, V.A. Sadykov, V.P. Ivanov, A.A. Rar, S.V.
Tsybulya, M.P. Andrianova, V.N. Kolomilchuk, A.N. Petrov,
O.F. Kononchuk, React. Kinet. Catal. Lett. 53(1) (1994) 223.
[27] N. Gunasekaran, J.J. Carberry, R. Doshi, C.B. Alcock, J.
Catal. 146 (1994) 583.
[28] R.J.H. Voorhoeve, J.P. Remeika, L.E. Trimble, A.S. Cooper,
F.J. Disalvo, P.K. Gallagher, J. Solid State Chem. 14 (1975)
395.
[29] Y. Teraoka, H. Fukuda, S. Kagawa, Chem. Lett., (1990) 1.
[30] J. Lentmaier, S. Kemmler-Sack, G. Knell, P. Kessler, E. Plies,
Mater. Res. Bull. 31(10) (1996) 1269.
[31] T. Nitadori, S. Kurihara, M. Misono, J. Catal. 98 (1986) 221.
126 D. Ferri, L. Forni / Applied Catalysis B: Environmental 16 (1998) 119±126