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The influence of the support on the properties of nickel
catalysts for edible oil hydrogenation
M. Gabrovska a,*, J. Krstic b, R. Edreva-Kardjieva a, M. Stankovic b, D. Jovanovic b
a Institute of Catalysis, Bulgarian Academy of Sciences, Acad. G. Bonchev str. bl. 11, 1113 Sofia, Bulgariab Institute of Chemisty, Technology and Metallurgy, Department of Catalysis and Chemical Engineering,
Njegoseva 12, 11000 Belgrade, Serbia and Montenegro
Received 1 July 2005; received in revised form 27 September 2005; accepted 4 October 2005
Available online 18 November 2005
Abstract
Two silica-containing materials, diatomite and waterglass, have been used as supports of nickel catalysts for edible oil hydrogenation. The
active phase has been deposited following the precipitation–deposition method. The textural and structural characteristics of the supports and
precursors have been studied by nitrogen sorption, scanning electron microscopy (SEM), infrared (IR) spectroscopy and X-ray powder diffraction
(XRD). The thermogravimetric (TG) analyses have been carried out under hydrogen flow at different heating rates. Chemisorption of hydrogen has
also been applied for precursor characterization and the metal particle size has been calculated from hydrogen adsorption isotherms at 25 8C. Thecatalysts have been tested in the soybean oil hydrogenation reaction. The differences in the textural and structural properties of the catalysts under
study have not been found to reflect on their activity and selectivity. However, the use of water glass as the support is considered to be preferable,
because of the lower economic cost of the catalyst, related to the elimination of the mechanical, chemical and thermal treatment of the crude
diatomite.
# 2005 Elsevier B.V. All rights reserved.
Keywords: Water glass; Diatomite; Precipitation–deposition; Textural and structural characterization; Reduction; Edible oil hydrogenation; Selectivity
www.elsevier.com/locate/apcata
Applied Catalysis A: General 299 (2006) 73–83
1. Introduction
The hydrogenation of vegetable oils is of special interest in
the process of modification of edible fats and oils. The first aim
of this process is to change the normal liquid oil into a semisolid
product with a desired consistency in a certain temperature
range. The second one is to reduce the diene and triene contents
of the product to a minimum, thus contributing to the stability
of the product against oxidative rancidity [1–3].
Nickel, copper, copper-chromite, platinum and palladium
are the most common metals used as active species in
heterogeneous catalysts for partial hydrogenation of poly-
unsaturated triglycerides [4,5]. The use of monolithic catalysts
in the hydrogenation of edible oils, as an alternative to slurry
systems, has received increasing interest throughout the last
* Corresponding author. Tel.: +359 2 9793578; fax: +359 2 9712967.
E-mail addresses: [email protected] (M. Gabrovska),
[email protected] (J. Krstic), [email protected]
(R. Edreva-Kardjieva), [email protected] (M. Stankovic),
[email protected] (D. Jovanovic).
0926-860X/$ – see front matter # 2005 Elsevier B.V. All rights reserved.
doi:10.1016/j.apcata.2005.10.011
years [6]. However, hydrogenation with nickel catalysts has
been the choice of industry, largely due to the availability, low
cost and inert nature of the metal relative to the oil. The typical
catalyst system for the hydrogenation of edible oils represents
reduced nickel in average concentration of 22 wt.%, deposited
on a suitable support and dispersed in the absence of air into
highly hydrogenated fat to stabilize it [4]. The choice and the
chemical preparation of the support, the technique of nickel and
promoter deposition, particle size, pore size and pore size
distribution of the precursor, as well as the activation procedure,
are known to be important for the activity and selectivity of the
catalyst. Kieselguhr (a diatomaceous earth), clay, silica, silica-
alumina, bentonite and palygorskite, as well as LTA-type
zeolites, have been used as supports of the nickel catalysts
[2–4,7–17].
Nickel supported on kieselguhr is the most widely used
catalyst in the industrial hydrogenation process. This support,
produced mainly from amorphous SiO2, has adequate textural,
thermal and chemical characteristics for the reaction under
study [4,12]. The crude diatomite, bentonite or palygorskite, as
natural silicon sources, contain large quantities of impurities.
M. Gabrovska et al. / Applied Catalysis A: General 299 (2006) 73–8374
Series of mechanical, chemical and thermal treatments of these
materials are necessary in order to obtain an activated support.
It is obvious that the establishment of a low-cost route for
producing the suitable support is opening the way for its
cheaper manufacture.
Water glass represents a viscous solution of sodium silicate
having a SiO2/Na2O molar ratio ranging from 3.75 to 1.5. Its
usage as a catalyst support for edible oil hydrogenation has
attracted our attention because a great number of laborious
steps would be avoided by its application as the source of silica,
instead of natural materials.
The number of papers about the application of water glass as
a catalyst support are rather scanty. For example, Tebben and
Weterings have reported that the silica carrier formed from
alkali water glass after neutralization and spray drying of the
material has no tendency to coalesce when used in processes
requiring precipitation of an insoluble nickel compound onto
the support [18].
The main support function is to keep up a fine dispersion of
nickel crystallites, making them available for reaction and also
to retard the growth or sintering of the small metal particles into
large agglomerates with a lower surface area and lower activity.
MgO is often used as a promoter in commercial nickel
catalysts, owing to its ability to stabilize the metal state and to
prevent the sintering of small nickel particles [19].
In this paper, we present the results from the comparative
study of two magnesium-promoted nickel catalysts. One of
them is supported on diatomite and the other one, on water
glass, both having been prepared by precipitation–deposition
technique. The aim was to elucidate the support influence on
the structure and catalytic properties of the catalysts in the
soybean oil hydrogenation reaction.
2. Experimental procedures
2.1. Supports
The diatomite, designated as D, is obtained from
Barosevac (the ‘‘Kolubara’’ Coal Basin—field B, Lazarevac,
Serbia and Montenegro). The crude diatomite is treated
mechanically, chemically (with an aqueous solution of HCl)
and thermally (at 800 8C) in order to obtain an activated
support [15].
The water glass material, designated as W, is a commercial
product with module (molar ratio) SiO2/Na2O = 3.0 (GALE-
NIKA—Magmasil A.D., Zemun (Belgrade, Serbia and
Montenegro).
2.2. Preparation of the precursors
All the chemicals used in the synthesis of the precursors
described in this paper, are of ‘‘pro analysis’’ purity grade.
The precursors, based on a diatomite (Ni–D) and on a
water glass (Ni-W), are obtained by the precipitation–dep-
osition method. Aqueous solutions of Ni(NO3)2�6H2O
(35.0 g dm�3 Ni), Mg(NO3)2�6H2O (1.4 g dm�3 Mg), Na2CO3
(110.0 g dm�3), an aqueous suspension containing 2.0 wt.% of
diatomite and an aqueous solution containing 2.0 wt.% of water
glass are prepared.
AvolumeofNi–Mgnitrate solution (molar ratioMg/Ni = 0.1)
is poured into a reaction vessel, equipped with a stirrer,
thermometer andpHelectrode. The solution is heated up to 90 8Cand co-precipitated with a ‘‘cold’’ Na2CO3 solution (20 8C)under vigorous stirring at constant value of pH 9.0� 0.2. A
peristaltic pump with defined flow rate is controlling the drop
wise addition of the Na2CO3 solution to the reaction vessel. The
obtained precipitate is aged for 30 min at 90 8C. The temperature
control and the constant stirring are performed with the
instrumentMR3001KandEKT3001, ‘‘Heidolph’’, respectively.
For the pH monitoring, a pH-meter 3320 ‘‘Jenway’’ with ATC
probe and pH Electrode C2401-8 ‘‘Radiometer’’ is used.
The water glass aqueous solution (20 8C) is added to the
aged precipitate in a quantity to satisfy the molar ratio SiO2/Ni
of 1.0 (Precursor Ni-W). The diatomite aqueous suspension
(20 8C) is added to the aged precipitate in a quantity to achievethe same SiO2/Ni molar ratio (Precursor Ni-D). The resulting
materials are aged again for 30 min at 90 8C under constant
stirring and than filtered and thoroughly washed with hot
(�90 8C) distilled water until absence of NO3� and Na+ ions is
obtained. The precursors are dried for 24 h in an oven at 105 8Cand ground to a powder.
2.3. Characterization of the supports and precursors
The silicate analysis is done by a classical chemical
procedure applicable in the analysis of sediment rocks. The
nickel content is determined gravimetrically by the dimethyl-
glyoxime method, while magnesium and other elements in
supports and precursors are determined on a Varian AA 775
spectrophotometer.
The X-ray diffraction (XRD) measurements are carried out
on a Philips PW 1710 powder diffractometer employing Cu Ka
radiation (l = 0.15148 nm), operated at U = 45 kV and 40
I = mA.
The infrared (IR) spectra of the supports and precursors are
recorded with a Perkin-Elmer 983 G spectrometer. The spectra
are performed using the KBr pellets technique: 1 mg of each
sample is mixed with 200 mg of KBr (KBr for spectroscopy
Uvasol, Merck, Germany). The spectral range of 4000–
250 cm�1 with a resolution of a 4 cm�1 is investigated. The
samples are dried at 105 8C before measurement.
The scanning electron microscopy (SEM) observations are
carried out on a JEOL Superprobe 733microscopewith a 25 kV
beam.
The nitrogen adsorption–desorption isotherms are deter-
mined at �196 8C on a Sorptomatic 1990 (Thermo Finnigan)
apparatus. The samples are out-gassed for 12 h at 110 8C and
degassed prior to the adsorption measurements. The specific
surface area, the total pore volume (Vp) at p/po = 0.998 and the
mean pore diameter are estimated with Win ADP (CE
Instruments) using the BET method [20].
The thermal analyses are performed using a LINSEIS device
(System 2000). The dried finely powdered precursors are
decomposed at heating rates of 2, 5, 10 and 20 8C min�1 under
M. Gabrovska et al. / Applied Catalysis A: General 299 (2006) 73–83 75
Table 1
The chemical composition of the supports
Support Chemical composition (wt.%)
SiO2 Al2O3 Fe2O3 CaO MgO Na2O K2O
Water glassa 74.51 – 0.50 – – 24.80 0.18
Diatomiteb 93.07 3.87 0.56 0.59 0.80 0.05 0.56
a Dry mass.b After activation.
hydrogen atmosphere. The H2 flow is introduced with a rate of 5
l h�1 to the thermogravimetric (TG) system after deoxygenat-
ing purifying.
The hydrogen chemisorption measurements are carried out
in a laboratory set-up using volumetric device. The samples are
previously reduced in the equipment for 5 h at 430 8C with a
gas mixture of H2/N2 (1:1, v/v, flow rate of 5 l h�1) at a heating
rate of 2 8C min�1. The adsorption isotherms are obtained
at 25 8C and pressures in the range of 0�100 Torr
(1 Torr = 133.3 Pa) after reduction. The hydrogen monolayer
coverage (adsorption capacity) is determined by extrapolation
of the linear part of the isotherm. The total amount of adsorbed
hydrogen is used to determine the metal nickel surface area and
metal nickel crystallite size. A ratio of 2 atoms of nickel per
molecule of chemisorbed hydrogen is assumed and the surface
density of a Ni atom is taken as 1.54 � 1019 atoms m�2Ni . The
crystallite size (dNi) is calculated assuming that the metallic
nickel presents in a cubic form and has metal density (rNi) of
8.9 � 106 g m�3 [21].
2.4. Reduction of the precursors
The activation of the precursors is performed in a laboratory
set-up by a dry reduction method. The reduction process is
accomplished with a gas mixture of H2/N2 (1:1, v/v) at a flow
rate of 5 l h�1. The reduction temperature is raised up to 430 8Cat a heating rate of 2 8C min�1 and held constant for 5 h. After
cooling down to room temperature, the reduced precursors,
denoted RNi-D and RNi-W, respectively, are passivated with a
mixture of 350 ppm O2 in nitrogen in order to reduce the
exceptional pyrophority of the metal nickel. The passivated
materials are impregnated with the pure paraffin oil.
2.5. Catalytic activity test
The partial hydrogenation of the edible soybean oil is
performed in a 7.5 dm3 reactor under the following conditions:
oil mass—5000 g; catalyst concentration—0.10 or 0.022 wt.%
Ni with respect to the amount of oil; initial hydrogenation
temperature—145 8C; final hydrogenation temperature—
180 8C; initial H2 pressure—0.08 MPa; final H2 pressure—
0.16 MPa; stirring rate—720 rpm.
A refined soybean oil with a composition of the fatty acids as
follows: palmitic (C16:0)—10.1%, stearic (C18:0)—4.1%,
oleic (C18:1)—23.2%, linoleic (C18:2)—52.8%, linolenic
(C18:3)—7.2%, is used as the starting material. The remaining
fatty acids: myristic (C14:0), palmitoleic (C16:1), arachidic
(C20:0), eicosenoic (C20:1) and behenic (C22:0) are in the total
concentration of 2.6%.
Taking a probe each 10 min follows the change in the fatty
acid composition of the soybean oil during the hydrogenation
reaction.
The hydrogenated products (triglycerides) are converted
into methyl esters using amethod described in detail by Christie
[22]. The analyses of the fatty acid methyl esters of the crude
soybean oil and hydrogenated products are performed by a
Hewlett–Packard HP 5890 gas chromatograph.
3. Results and discussion
3.1. Supports
The results of the chemical analysis of both supports are
summarized in Table 1.
The XRD pattern of diatomite (Fig. 1a) shows reflections
characteristic for amorphous silica (the broad peak centred at
2Q = 208) with a small amount of well-crystallized quartz
(2Q = 26.68; JCPDS file 46-1045). The XRD pattern of the
water glass reveals that the material is badly crystallized
(Fig. 1b).
The IR spectrum of diatomite (Fig. 2a) displays character-
istic bands of the amorphous hydrated SiO2. The broad
absorption band centred at 1100 cm�1 is attributed to the nasmode of Si–O stretching vibrations, while the sharp bands
centred at 800 and 470 cm�1 are attributed to the ns mode of Si–
O stretching vibrations. The peak at 1625 cm�1 is due to the
deformation mode (d) of H–O–H angle of the water molecules.
Some of the IR bands, characteristic of the amorphous hydrated
SiO2, are registered in the IR spectra of water glass, too
(Fig. 2b). They are of relatively low intensity and shifted to
lower wave numbers (the bands centred at 1050, 770 and
450 cm�1). A new band centred at 1450 cm�1 appears proving
the presence of CO32� ions [23,24].
SEM is used to investigate the morphology and the
uniformity of the particle shape, as well as to determine the
chemical homogeneity of the supports. The SEM image of
diatomite (Fig. 3) shows that this support consists of different
natural inorganic and biological products, differing in kind,
shape and size. In contrast, the SEM image of water glass
reveals very well pronounced habit of the angulated particles,
randomly distributed on the surface, ranging in effective
diameter from 8 to 170 mm.
The observed differences in the XRD and IR spectra and
SEM photography of the supports could be ascribed to their
different nature and different preliminary thermal treatments.
3.2. Precursors
3.2.1. Unreduced precursors
The results from the silicate and chemical analysis of both
precursors are summarized in the Table 2. An atomic ratio of
Mg/Ni about 0.1 is found in the both precursors that being
nearly equal to the Mg/Ni ratio in the synthesis solutions. The
obtained results demonstrate that the Ni2+ and Mg2+ ions are
quantitative precipitated.
M. Gabrovska et al. / Applied Catalysis A: General 299 (2006) 73–8376
Fig. 1. XRD patterns of the supports: (a) diatomite and (b) water glass.
The X-ray diffraction patterns of the precursors (Fig. 4) are
considerably differing from the spectrum of both supports. The
registered reflections are very broad and weak and indicate the
presence of poorly crystalline samples. The high background
below 2Q = 108 of the precursor Ni-W (Fig. 4c) indicates
advanced amorphization than in Ni-D. The XRD patterns of the
unsupported basic nickel carbonate (BNC) (Fig. 4a) disappear
in the patterns of both precursors (Fig. 4b and c). The observed
phenomenon proves that an interaction occurs between the
Fig. 2. IR profiles of the supports: (a) diatomite and (b) water glass.
basic nickel carbonate and the silica from the supports. As is
well known, when the nickel salt is precipitated with sodium
carbonate in the presence of silica, the synthesized compound is
the silica-supported basic nickel carbonate with a composition
of Ni(OH)x(CO3)y/SiO2�zH2O that varies considerably with the
changes in the precipitation conditions [23,25]. The tendency of
the silica support to react strongly with the Ni-containing
species has been reported in several studies [24,26,27]. This
strong interaction has been suggested to result in the formation
of nickel hydrosilicate layers on the surface of the silica
particles. The formed phases have been identified as nickel
antigorite [26,10,27,28], nickel chrysotiles [29], nickel
montomorillonite [26,28], nickel polygorskite [24], serpentine
[30] or even orthosilicate-type [24]. The poorly crystallized
nickel hydrosilicate compounds with imperfect nickel anti-
gorite and/or nickel montmorillonite-like structure are always
formed during the co-precipitation of nickel nitrate and alkali
silicate solutions at temperature under 100 8C [28].
The reflections characteristics of nickel silicate hydroxide
(2Q = 12�378; Ni3Si2O5(OH)4, JCPDS file #22-0754) and
antigorite-like phase appeared (2Q = 35�388; Ni3Si2O5(OH)4,
JCPDS file #21-0963). Theymay be observed as very broad and
weak reflections in both precursors (Fig. 4).
IR studies are used to prove the interactions of nickel species
with the silica from the supports. The IR spectrum of the
unsupported basic nickel carbonate exhibits characteristic
bands at 1640, 1380, 520, 465 and 360 cm�1 (Fig. 5a). The
band at 1625 cm�1, characteristic of a deformation mode (d) ofthe water molecules, and at 1380 cm�1 typical of the presence
of CO32� ions are still preserved in the spectra of the precursors
(Fig. 5), however with higher intensity. On the other hand, the
bands observed in the region 520–360 cm�1, characteristic of
lattice and stretching vibrations of Ni–O– in nickel basic
carbonate, disappeared. The IR spectra of both precursors do
not display the existence of free silica (bands at 1097 and
800 cm�1). The shift of the diatomite band at 1120 cm�1
(Fig. 2a) toward 1067 cm�1 in the Ni-D precursor (Fig. 5b), as
well as the shift of the water glass support from 1050 cm�1
(Fig. 2b) toward 1015 cm�1 in the Ni-W precursor (Fig. 5c), is
assigned to the vibrations of silicate species having interacted
with the basic nickel carbonate.
The SEM images of both precursors illustrate a change in the
morphology of the original supports (Fig. 3). It may be seen that
the preparation procedure leads to the formation of precursors
with smaller particles than the corresponding supports. The
SEM image of precursor Ni-D displays well-pronounced habit.
The surface consists of fragments different in shape and size.
The larger ones have an effective diameter of 3�7 mm. These
are covered with numerous fine particles with an effective
diameter of 0.5�3 mm. In contrast to Ni-D, the surface of the
Ni-W precursor appears to be composed of identical, smaller
and randomly distributed particles, similar to those of the
support structure. The particles are very fine with an effective
diameter of 0.25–1.5 mm, separated by craters.
The BET surface area and the textural characteristics of the
diatomite support and both precursors are represented in
Table 3. The table does not contain data for the water glass
M. Gabrovska et al. / Applied Catalysis A: General 299 (2006) 73–83 77
Fig. 3. SEM images of the samples.
support, because the dry material still contains a large amount
of water. Its presence makes the BET surface area and pore
volume measurements nonsense.
The increase in surface area from 17 m2 g�1 in fresh
diatomite (Table 3) up to 98 m2 g�1 in Ni-D may be explained
by the reaction between Ni- and Si-containing species. The
Table 2
The chemical composition of the precursors
Precursor The chemical composition of the precursors
Ni (wt.%) Mg (wt.%) Mg/Ni ratio S
Ni-D 41.93 1.80 0.10 4
Ni-W 42.21 1.70 0.09 4
formation of nickel hydrosilicate-type linkages (–Si–O–Ni–)
lead to a highly porous network [24]. This phenomenon is
more pronounced in precursor Ni-W and confirms the results
from XRD (Fig. 4c) and SEM (Fig. 3) analyses, revealing
respectively more poorly crystallized sample and smaller
particles.
iO2 (wt.%) NiO (wt.%) MgO (wt.%) SiO2/Ni ratio
3.70 53.32 2.98 1.02
3.48 53.70 2.82 1.01
M. Gabrovska et al. / Applied Catalysis A: General 299 (2006) 73–8378
Fig. 4. XRD patterns of the samples: (a) BNC; (b) Ni-D; and (c) Ni-W.
The nitrogen adsorption–desorption isotherms of the
diatomite and the precursors are represented in Fig. 6. The
isotherm of diatomite is close to type II characteristic for non-
porous or macroporous adsorbents according to the IUPAC
1985 classification [31]. The lack of full reversibility of the
adsorption–desorption isotherm, i.e. the presence of a hyster-
esis loop, indicates adsorption on an open and macroporous
Fig. 5. IR spectra of the samples: (a) BNC; (b) Ni-D; and (c) Ni-W.
stable surface. The isotherms of the precursor Ni-D changed in
shape, transforming into type IV characteristic for the
mesopores materials. The isotherm exhibits a hysteresis loop
close to type H4 [31]. Obviously, the modification of the
macroporous diatomite texture into the mesoporous one is
provoked by the reaction of nickel species with the support. The
isotherm of the Ni-W precursor is similar in shape to the Ni-D,
with more pronounced hysteresis loop, close to type H3.
Comparing the values of Vp and Vmes of both precursors, it
may be seen that they are six times higher in Ni-W than in Ni-D,
indicating higher access of the nitrogen molecule to the
corresponding pores of mesopore region (Table 3). The ratio
4Vp/SBET is used as a simple mode of the mean pore diameter
(dp) characterization [31]. The diatomite support possesses
large pores (dp = 60 nm). The formation of nickel silicate-like
phases reduces the pore size to 4.5 nm in the Ni-D sample. A
similar dp value is found in Ni-W.
In order to obtain a more comprehensive representation of
the texture of the diatomite and the precursors, the pore size
distribution (PSD) is estimated. The desorption branch of the
nitrogen isotherms at p/po from 0.2 to 0.998 is used, applying
the BHJ model and the standard isotherm of de Boer and co-
workers [32].
The PSD curve of the diatomite (Fig. 7) demonstrates a
texture with polydisperse type of distribution. The mean part of
the pores is situated at dp maximum equal to 47 nm. The PSD
curves of both precursors reveal a transformation from the
polydisperse to the monodisperse type of distribution in the
range of 3�5 nm with a dp maximum about 4 nm.
It may be concluded that the studied precursors are
composed of small particles but Ni-W sample possesses more
developed porous structure in the mesopore region.
It presents some interest to study whether the similarities in
the structure and texture of the precursors reflect on the
decomposition of the precursors under hydrogen atmosphere.
This activation procedure represents one of the most important
operations in the course of the catalyst synthesis, definitely
determining the characteristics and performance of the final
catalyst.
The differential thermal gravimetric (DTG) profiles of both
precursors, i.e. the first derivative of the weight losses,
measured at heating rates of 2, 5, 10 and 20 8C min�1 under
hydrogen flow, are studied.
The precursor Ni-D does not exhibit appreciable weight
losses in the low temperature region undergoing the same
weight losses (about 40%) at all heating rates studied. This is
easily explained by the high temperature (800 8C) calcinationof the support, prior to the precursor preparation. An analogous
behaviour of the precursor Ni-W is registered. This sample also
manifests the weight losses (about 30%) at all heating rates.
However, low temperature weight losses are observed with this
material. These peaks are not related to hydrogen consumption
but to the weight loss due to desorption of the adsorbed and
crystallization water in the samples. The higher temperature
weight loss peaks present broad minimum centered at 400 8Cfor the lowest heating rate (2 8C min�1) and at 500 8C for the
highest one (20 8C min�1).
M. Gabrovska et al. / Applied Catalysis A: General 299 (2006) 73–83 79
Table 3
The BET surface area, the textural characteristics and the type of isotherms of the samples
Sample Characteristics of the samples
SBET (m2 g�1) Vp (cm3 g�1) Vmes (cm
3 g�1) Max pore width (nm) dp (nm) Type of isotherm
D 17 0.25 0.10 2.20 58.8 II-like
Ni-D 98 0.11 0.10 3.82 4.49 IV-like
Ni-W 505 0.66 0.61 3.86 5.23 IV-like
Vp is total pore volume at p/p0 = 0.998; Vmes is cumulative pore volume of mesopore region; dp is mean pore diameter, dp = 4Vp/SBET.
Fig. 6. The nitrogen adsorption–desorption isotherms of the samples: (D)
adsorption and (~) desorption.
The temperature range of the intensive decomposition-
reduction is lower for the precursor Ni-D than Ni-W at all
heating rates. However, both precursors are reduced at a
considerably lower temperature at the heating rate of
2 8C min�1. The use the lowest heating rate in the activation
of the precursors by reduction has to be preferred.
Fig. 7. Pore size distribution of the samples.
M. Gabrovska et al. / Applied Catalysis A: General 299 (2006) 73–8380
Fig. 8. DTG profiles of the samples obtained at the heating rate of 2 8C min�1:
(a) Ni-D; (b) Ni-W; and (c) BNC.
Fig. 9. XRD patterns of the reduced precursors: (a) RNi-D and (b) RNi-W.
Table 4
The results from the measurements of H2 chemisorption
Precursor SNi ðm2Ni g
�1cat Þ SspNi ðm2
Ni g�1Ni Þ DNi (nm)
Ni-D 21.4 51.1 11.0
Ni-W 20.7 49.1 11.4
Basic nickel carbonate is used as a reference compound for
the TG experiments. The DTG profiles of the precursors
together with the profile of BNC determined at the heating rate
of 2 8C min�1 are shown in Fig. 8. The reduction of Ni2+ ions
to Ni0 in the reference compound starts at about 210 8C and
reaches a maximum at 255 8C (Fig. 8c). The DTG profile of the
Ni-D precursor (Fig. 8a) resembles that of the unsupported
basic nickel carbonate. The performance of the Ni-D sample
may be attributed to the reduction of the Ni2+ ions to Ni0
representing weak support interactions. The DTG profile of
the Ni-W precursor (Fig. 8b) demonstrates that the reduction
peak is shifted to a higher temperature, indicating that the
reduction of the Ni2+ ions to Ni0 is more difficult and exhibit
stronger interaction with the support. Consequently, it is clear
that stronger interaction between basic nickel carbonate and
SiO2 of the Ni-W precursor hampers the reduction of the Ni2+
ions to Ni0 due to the formation of nickel phyllosilicate
structures.
3.2.2. Reduced precursors
It is well known that the active phase in the vegetable oil
catalytic hydrogenation reaction is metallic nickel. The X-ray
diffraction patterns of the reduced and passivated precursors are
examined to determine the state of nickel in the reduced
materials. The XRD phase analysis shows that both reduced
samples exhibit similar reflections and consist of following
phases: metallic nickel, quartz and nickel silicate. However,
they are in different proportions (Fig. 9). The diffractogram of
RNi-D shows well-resolved reflections mainly of crystallized
metal nickel phase at d = 0.2036 and 0.1758 nm (JCPDS file
#4-850) and a reflection corresponding to quartz at
d = 0.3354 nm (JCPDS file #46-1045) (Fig. 9a). The XRD
patterns of RNi-W register one reflection characteristic to the
metal nickel phase at d = 0.2045 nm and a small signal
corresponding to the quartz phase (Fig. 9b). All reflections of
RNi-Wmaterial are broader and with lower intensity compared
to the RNi-D precursor. These results are in accordancewith the
total specific surface area of the reduced materials. The sample
RNi-W possesses a surface area of 132 m2 g�1 while the RNi-D
one – 11 m2 g�1.
The SEM images of both precursors demonstrate visible
changes in their morphology after reduction and passivating
(Fig. 3). The samples undergo significant packing in result of
water and CO2 removing. The large aggregates are covered
with small particles of similar size and shape in both reduced
precursors.
These results are confirmed by the hydrogen chemisorption
experiments after reduction of the samples at 430 8C. The tworeduced precursors demonstrate similar values of the metallic
nickel surface (SNi), specific nickel surface (SspNi) and nano-
sized nickel particles (DNi) (Table 4).
The observed similarity in the mean particle size of the
reduced precursors suggests identical dispersion of the metal
nickel crystallites on the surface. It may be concluded that the
reduction procedure of the precursors eliminates the differences
between the natural and synthetic siliceous supports.
M. Gabrovska et al. / Applied Catalysis A: General 299 (2006) 73–83 81
3.3. Catalytic activity and selectivity
The hydrogenation of soybean oil is represented by the
variation of the fatty acids content as a function of time
(Figs. 10 and 11). The data shows that the hydrogenation of
linolenic (C18:3) and linoleic (C18:2) acids on both catalysts
turns them almost entirely into the oleic acid (C18:1). Stearic
acid (C18:0) remains below 12 wt.%. If it exceeds this limit, the
edible oils acquire unpleasant taste. The final content of the
linoleic (C18:2) acid is less than 5 wt.%, which that is in
agreement with the general requirements for edible hydro-
genated oils. This low content also prevents the air oxidation
process. On the other hand, the linoleic acid is one of the
‘‘essential’’ fatty acids, e.g. its presence is necessary for human
nutrition. Therefore, small amounts of it are allowed in the
edible hydrogenated oils.
It may be concluded that both catalysts manifest similar
activity and the hydrogenated products fulfill all requirements
for the conventional partly hydrogenated edible oils.
Vegetable oil hydrogenation includes a series of side
processes (like the geometrical and position isomerization
reactions). However, evaluation of the catalyst selectivity by
first approximation indicates a reaction mechanism composed
by a series of consecutive reduction steps:
C3�!k3 C2�!k2 C1�!k1 C0;
Fig. 10. The fatty acids content as a function of time during the soybean
hydrogenation in the presence of the catalysts Ni-D, where (&) C18:0; (*)
C18:1; (D) C18:2; and (^) C18:3.
where C3, C2, C1 and C0 are the concentrations of linolenic,
linoleic, oleic and stearic acids, and k1, k2 and k3 are the
corresponding rate constants.
The rate constants k1, k2 and k3 are the cumulative constants
as previously emphasized [33]. All the geometric and positional
isomerization processes have been neglected. Solution of the
differential equations system, determining the rate of the above
process, may be explicitly expressed as the time (t) function of
all the system components concentration:
C3 ¼ A3 expð�k3tÞ (1)
C2 ¼�A2þ A3
k3k3 � k2
�expð�k2tÞ þ A3
k3k2 � k3
expð�k3tÞ
(2)
C1 ¼�A1þ A2
k2k2 � k1
þ A3k2k3
ðk2 � k1Þðk3 � k1Þ
�expð�k1tÞ
þ k2k1 � k2
�A2þ A3
k3k3 � k2
�expð�k2tÞ
þ A3k2k3
ðk1 � k3Þðk2 � k3Þexpð�k3tÞ
(3)
Fig. 11. The fatty acids content as a function of time during the soybean
hydrogenation in the presence of the catalysts Ni-W, where (&) C18:0; (*)
C18:1; (D) C18:2; and (^) C18:3.
M. Gabrovska et al. / Applied Catalysis A: General 299 (2006) 73–8382
Table 5
The rate constants and the selectivity of the studied catalysts
Catalyst Rate constants Selectivity
k1 � 10�4
(min�1)
k2 � 10�2
(min�1)
k3 � 10�2
(min�1)
SLn SLo
Ni-D 1.97 1.17 2.93 2.5 59.4
Ni-W 2.06 1.21 2.90 2.4 58.6
C ¼ C3t¼0 þC2t¼0 þC1t¼0 þC0t¼0 �C3 � C2 � C1 (4)
Relation (4) is actually representing the law of substance
preservation within this model. Since, based on the relation
(4), the system components are not all linearly independent, it is
sufficient to find the equations (1)–(3) by integrating, with the
fourth component being a linear combination of the first three.
The selectivity towards linolenic acid (C18:3) is denoted
SLn and it represents the relation k3/k2, while the selectivity
towards linoleic acid (C18:2) is denoted SLo = k2/k1. The rate
constants of the studied catalysts are determined by a numeric
minimization (Neadler–Mead method) of the square of
corresponding functions deviation from the experimental
values by subsequent fitting method [33]. The calculated
values of the rate constants are represented in Table 5.
It must be emphasized that the calculated selectivity,
regarding the mono- and polyunsaturated fatty acid hydro-
genation, is similar for both catalysts and corresponds to the
published data [34–40].
4. Conclusions
The use of siliceous supports considerably diverse in origin,
preliminary thermal treatments and morphology, lead to
preparation of precursors, also differing in morphology, texture
and structural properties, in spite of their identical composition.
The preparation procedure causes the formation of
precursors with small particles and poorly crystallized nickel
silicate hydroxide and antigorite-like structures. The establish-
ment of nickel hydrosilicate-type linkages is a precondition for
a highly porous material. This phenomenon is more pro-
nounced in the precursor supported on water glass, where more
developed mesopore region appears.
The reduction procedure eliminates the differences between
the natural and synthetic siliceous supports: both reduced
precursors demonstrate similar values of the metallic nickel
surface, specific nickel surface and nano-sized nickel particles.
Both catalysts manifest similar activity and selectivity under
the chosen reaction parameters when the observed differences
on the catalyst performance become negligible.
The advantage of water glass use as support is the lower
economic cost of the catalyst, as the procedures of mechanical,
chemical and thermal treatment of the crude diatomite may be
eliminated. The present study claims that water glass is a
suitable silica-containing support for the edible oil hydrogena-
tion catalyst.
Acknowledgements
The authors (M.G. and R.K.) are grateful to the National
Science Fund at the Ministry of Education and Science of
Bulgaria, for the partial financial support (Project X-1411). The
authors (J.K., M.S. and D.J.) greatly acknowledge the support
of the Serbian Ministry of Science and Environmental
Protection through the Project—TR 6712 B.
References
[1] R. Allen, Am. J. Oil Chem. Soc. 37 (1960) 521–523.
[2] H. Patterson, Hydrogenation of Fats and Oils, Applied Science Publishers,
London, 1983.
[3] M. Balakos, E. Hernandez, Catal. Today 35 (1997) 415–425.
[4] E. Draguez de Hault, A. Demoulin, J. Am. Oil Chem. Soc. 61 (1984) 195–
200.
[5] M. Fernandez, C. Piqueras, G. Tonetto, G. Crapiste, D. Damiani, J. Mol.
Catal. A: Chem. 233 (2005) 133–139.
[6] T. Boger, M. Zieverink, M. Kreutzer, F. Kapteijn, J. Moulijn, W. Addiego,
Ind. Eng. Chem. Res. 43 (2004) 2337–2344.
[7] J. Coenen, Ind. Eng. Chem. Fundam. 25 (1986) 43–52.
[8] S. Mendioroz, V. Munoz, Appl. Catal. 66 (1990) 73–90.
[9] M. Rodrigo, L. Daza, S. Mendioroz, Appl. Catal. A: Gen. 88 (1992) 101–
114.
[10] J. Anderson, M. Rodrigo, L. Daza, S. Mendioroz, Langmuir 9 (1993)
2485–2490.
[11] J. Ferreras, C. Pesquera, F. Gonzalez, I. Benito, C. Blanco, J. Renedo,
React. Kinet. Catal. Lett. 53 (1994) 1–6.
[12] J. Veldsink, M. Bouma, N. Schoon, Catal. Rev.-Sci. Eng. 39 (1997) 253–
318.
[13] M. Gonzalez-Marcos, J. Gutierrez-Ortiz, C. Gonzalez-Ortiz de Elguea, J.
Gonzalez-Velasco, J. Mol. Catal. A: Chem. 120 (1997) 185–196.
[14] M. Gonzalez-Marcos, J. Gutierrez-Ortiz, C. Gonzalez-Ortiz de Elguea, J.
Delgado, J. Gonzales-Velasco, Appl. Catal. A: Gen. 162 (1997) 269–
280.
[15] D. Jovanovic, R. Radovic, L. Mares, M. Stankovic, Br. Markovic, Catal.
Today 43 (1998) 21–28.
[16] I. Morawski, Przemysl Hemiczny 82 (2003) 1391–1394 (in Polish).
[17] M. Selim, I. Hamdy, A. ElMaksoud, Microporous Mesoporous Mater. 74
(2004) 79–85.
[18] J. Tebben, C. Weterings, US Patent 4,014,818 (1977).
[19] S. Narayanan, G. Sreekanth, J. Chem. Soc., Faraday Trans. 89 (1993) 943–
949.
[20] E. Barret, L. Joyner, P. Halenda, J. Am. Chem. Soc. 73 (1951) 373–380.
[21] J. Anderson, Structure of Metallic Catalysts, Academic Press, New York,
1975, p. 300.
[22] W. Christie, Advances in Lipid Methodology—Two, Oily Press, Dundee,
1993, pp. 69–111.
[23] G. Babu, A. Basrur, A. Bhat, R. Murthy, Ind. J. Chem. 29A (1990) 1094–
1097.
[24] K. Ghuge, A. Bhat, G. Babu, Appl. Catal. A: Gen. 103 (1993) 183–204.
[25] Y. Nitta, T. Imanaka, S. Teranishi, J. Catal. 96 (1985) 429–438.
[26] J. Coenen, B. Linsen, in: B. Linsen (Ed.), Physical and Chemical Aspects
of Adsorbents and Catalysts, Academic Press, New York, London, 1970,
pp. 471–479.
[27] J. Van Dillen, J. Gues, L. Hermans, J. Meijden, in: G. Bond, P. Wells, F.
Tompkins (Eds.), Proceedings of the 6th International Congress on
Catalysis, The Chemical Society, 1976, pp. 1–8.
[28] J.B. Van Eijk van Voorthuijsen, P. Franzen, Rec. Trav. Chim. 70 (1951)
793–812.
[29] C. Kibby, F. Massoth, H. Swift, J. Catal. 42 (1976) 350–357.
[30] P. Jacobs, H. Nijs, G. Poncelet, J. Catal. 64 (1980) 251–259.
[31] F. Rouquerol, J. Rouquerol, K. Sing, Adsorption by Powders and Porous
Solids, Principle, Methodology and Applications, Academic Press,
1999.
M. Gabrovska et al. / Applied Catalysis A: General 299 (2006) 73–83 83
[32] B. Lippens, B. Linsen, J. de Boer, J. Catal. 3 (1964) 32–37.
[33] D. Jovanovic, Br. Markovic, M. Stankovic, L. Rozic, T. Novakovic,
Z. Vukovic, M. Anic, S. Petrovic, Hem. Ind. 56 (2002) 147–
156.
[34] L. Albright, J. Am. Oil Chem. Soc. 40 (26) (1963) 28–29, 16–17.
[35] L. Albright, Chem. Eng. 74 (1967) 197–202.
[36] L. Albright, R. Allen, M. Moore, J. Am. Oil Chem. Soc. 47 (1970) 295–
298.
[37] J. Coenen, J. Am. Oil Chem. Soc. 53 (1976) 382–389.
[38] P. Puri, J. Am. Oil Chem. Soc. 55 (1978) 865–869.
[39] R. Allen, J. Am. Oil Chem. Soc. 58 (1981) 166–169.
[40] A. Chen, D.McIntire, R. Allen, J. Am. Oil Chem. Soc. 58 (1981) 816–818.