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South African Journal of Chemistry

versão On-line ISSN 1996-840X
versão impressa ISSN 0379-4350

S.Afr.j.chem. (Online) vol.71  Durban  2018 



Transition metal oxide supported on alumina catalysts: a comparative study for the hydrogenation of octanal



Jignesh Valand ; Venkata D.B.C. Dasireddy; Abdul S. Mahomed; Holger B. Friedrich*

Catalysis Research Group, School of Chemistry and Physics, University of KwaZulu-Natal, Private BagX45001, Durban, 4000, South Africa




Monometallic (10 wt.%) Co, Ni and Cu nanoparticles supported on alumina catalysts were prepared using an ultrasonic impreg-nation-cavitation method and characterized using ICPP XRD, physisorption, chemisorption and temperature programmed techniques. The copper catalyst showed higher metal dispersion and greater hydrogen and CO chemisorption capacity when compared to the nickel and cobalt catalysts. Hydrogenation of octanal carried out in a continuous flow high pressure fixed bed reactor showed that the rate of reaction and turnover number of octanol depended on the amount of hydrogen chemisorbed. The copper catalyst showed the lowest activation energy, as well as best catalytic activity. The Cu-Al catalyst which showed higher metal dispersion and low acidity, showed the highest selectivity towards octanol with no C24 acetal formation, when compared to the Ni-Al and Co-Al catalysts.

Keywords: Octanal hydrogenation, octanol, copper, nickel, cobalt.



1. Introduction

Linear α-olefins (LAOs) are an important feedstock for the chemical industry.1 These compounds are produced from catalytic cracking, resulting in a large number of different types of 1-alkenes as the primary products, together with alkanes.2 These valuable terminal alkenes are also produced by the dehydration of primary alcohols. These alcohols, in turn, can be prepared by the hydrogenation of carbonyl compounds formed, e.g. in the hydroformylation reaction.3 Catalytic conversion of carbonyl compounds to alcohols is one of the more demanding reactions in organic synthesis and also is used in the production of fine chemicals.

From the early 1930s, triglycerides, primarily vegetable oils, have been transformed to fatty alcohols by hydrogenation over Cr-containing Adkins catalysts.4 The use of chromium is known to cause concern regarding health and environmental issues, as a result the search for environmentally friendly and benign hydrogenation catalysts is continuing.3,5 Reports on the selective hydrogenation of aldehydes to alcohols in continuous flow liquid phase systems, under mild conditions are limited.6 There are reports on using group VIII metals on oxide supports for the hydrogenation of aldehydes.3,7 Catalysts with metals such as nickel,8 palladium9 or rhodium10 are not selective towards unsaturated alcohols, whereas ruthenium has moderate activity and similar or better selectivities are achieved with platinum, iridium or osmium catalysts.11 Those metals, however, are rare and expensive.

It has been shown that hydrogenation depends on the surface area, pore volume and acid-base character of the support.11-12 High surface area enhances dispersion of supported metals, whereas porosity of the support affects intraparticle diffusion of reactants and products. The acid-base nature of the support is a key parameter to allow or restrict the formation of acetals and diols in the hydrogenation of aldehydes.1,11a Hydrogenation of a long chain aldehyde, e.g. octanal is one of the interesting topics of research in the field of catalysis. In the present study, we report the hydrogenation of 1-octanal to 1-octanol, an important step in an industrial process which ultimately gives 1-octene, over the comparatively inexpensive transition metals cobalt, nickel and copper supported on alumina, prepared by an ultrasonication process.


2. Experimental

The ultrasonic cavitation-impregnation method13 was used for preparing the supported catalysts. These materials were made by dissolving the required amounts of the metal precursors, cobalt nitrate (Cu(NO3)2-3H2O, Sigma-Aldrich), nickel nitrate (Ni(NO3)2-6H2O, Sigma-Aldrich), and copper nitrate (Co(NO3)2-6H2O, ACE ) in distilled water, then adding the solutions to high surface area 1-alumina (1-Al2O3 Alfa-Aesar). Magnetic stirring at 300 rpm, combined with ultrasonic cavita-tion (MRC Ultrasonic System, D150H Model) at 43 kHz were applied at room temperature (25 ± 1 °C) to obtain a homogeneous mixture and uniform dispersion. The slurry was dried by evaporation at 70 °C while stirring continuously. The materials then were dried in an oven for 16 h at 110 °C. The catalysts then were calcined for 5 h at 550 °C to give the 10 wt.% of cobalt, nickel and copper catalysts, denoted as Cu-Al, Ni-Al and Co-Al, respectively.

The Brunauer-Emmett-Teller (BET) surface area was measured using a Micromeritics Tristar II instrument. Inductively coupled plasma (ICP) analyses were carried out with a Perkin Elmer Optical Emission Spectrometer Optima 5300 DV. Powder X-ray diffraction (XRD) was conducted using a Bruker D8 Advance diffractometer equipped with a Cu radiation source (1 = 1.5406 A). NH3-temperature programmed desorption (NH3-TPD) was done on a Micromeritics 2920 Autochem II Chemi-sorption Analyser. In these analyses a mixture of5%NH3 in helium was passed over the reduced catalyst for 60 min. Thereafter, the temperature was increased slowly to 950 °C by ramping at 10 °C min-1 under helium flow.14 The dispersion of metals, crystallite size, hydrogen and CO uptake were determined with the use of a Micromeritics ASAP 2020 Chemisorption Analyser. The metal dispersion is expressed as the ratio between hydrogen uptake and the metal on the surface of the support. It was calculated assuming a 1:1 H:M (M = Co, Ni and Cu) chemisorption stoichiometry.3 The equations used to establish dispersion and metal surface area can be found in the supplementary information. A Jeol JEM-1010 electron microscope was used to obtain TEM images of the catalysts.

The hydrogenation reactions were performed in a fixed bed continuous flow reactor in down-flow mode. The catalyst bed (4 mL volume, pellet sizes ranged between 300 and 600 μm) was diluted with an equal volume of carborundum (24 grit). Prior to the catalytic testing, to ensure that the reactor is free from physical transport limitations, the reactor set-up was checked with varying flows of octanal, pressures and pellet sizes of catalysts. The feed used for all reactions was 10 wt.% octanal in octanol, the latter serving as thermal diluent. Octanol does not affect the reaction. There was no decrease in octanal conversion with increasing dilution, which shows the absence of diluent effects during the reaction.15 The feed entered the reactor via aLab Alliance Series II hplc pump. The liquid products were collected in a 500 mL catchpot and the excess hydrogen gas exited through a wet gas flow meter (Ritter Drum-type). The liquid products were collected at regular intervals. They were identified and quantified using a PerkinElmer Clarus 500 GC, with an FID and a Petrolite column. All the reported data points were obtained in duplicate after steady state was achieved. The mass balances for all samples were 100 ± 1 %.

TON, also called turnover number, was defined as the molecules reacting per active site per gram of catalyst. The number of reacting molecules of octanal was calculated using the conversion and mass flow rate data at corresponding reaction temperatures; and the available number of active sites was obtained from the metal dispersion data, measured from chemisorption. The apparent activation energy was calculated using the Arrhenius plot, details of which are found in the supplementary information.


3. Results and Discussion

3.1. Characterisation of the Catalysts

Table 1 shows the results of the physisorption experiments and the elemental analyses of the catalysts. The ICP data of the catalysts showed that the desired metal wt.% was loaded on the alumina. All the catalysts show Type IV adsorption desorption isotherms with a H1 hysteresis loop, which demonstrated the mesoporous nature of the catalysts.14 By impregnating the metal oxides on alumina, the surface area and pore volume decreased, likely due to the blocking of the narrow pores of alumina with the metal oxides. Powder XRD (Fig. 1) shows the alumina pattern which is in agreement with the literature2 and with JCPDS File No. 10-425. The d-spacing values for the 20 angles between 30 ° to 50 ° correlate with the JCPDS File Nos. 41-254, 47-1049,42-1467 for copper oxide, nickel oxide and cobalt oxide, respectively.4b Among all the catalysts, Co-Al showed the largest crystallite size compared to Cu-Al and Ni-Al (Table 2). In general, the larger crystallite size of the metals leads to lower dispersion of the metal on the surface of the support.15c The same trend is observed in this study. The amount of hydrogen chemisorbed on the surface of the catalysts was in the inverse order to crystallite size.

In the TPD analysis data, all catalysts showed three types of acidic sites, i.e. weak (<400 °C), moderate (400-600 °C) and strong (600-900 °C).2 In all the catalysts, weak acidic sites are dominant and Co-Al showed the highest Lewis acidity, whereas Ni-Al showed the highest total and specific acidity (Table 3). Cu-Al showed the lowest acidity when compared to other catalysts, but slighter higher acidity than the alumina support. In the TEM images (Fig. S1, supplementary information), alumina appears as irregular-shaped agglomerations of elongated particles. When the Cu, Ni and Co oxides were impregnated, no difference in the overall morphology of the catalysts was observed.

3.2. Catalytic Results

The hydrogenation of octanal was conducted in a continuous flow fixed bed reactor with an octanal to hydrogen molar ratio of 1:2. GHSV and LHSV were maintained at 460 h-1 and 18 h-1, respectively, at temperatures of 110 °C, 150 °C and 180 °C. With an increase in temperature, all the catalysts showed the expected increase in conversion of octanal and also an increased selectivity towards octanol.

Figure 2 shows the conversion of octanal and selectivity towards products at 110 °C. The conversion profile of the catalysts correlates with the amount of hydrogen chemisorbed on the surface of the catalysts (Table 2), which suggests the conversion of the octanal depends on the disassociation of hydrogen on the surface of the catalyst.16 The copper-containing catalyst is significantly more active than other catalysts, due to high metal dispersion and acidic site distribution (Fig. 2). The selectivity profile of octanol is proportional to the quantity of CO chemisorbed on the surface of the catalysts in chemisorption studies, which might imply a correlation with carbonyl group (octanal) adsorption.

The desired reaction in this study is the hydrogenation of octanal to produce octanol. However, some side reactions do occur to produce the C16 diol and C24 acetal. The C16 diol is produced over the Cu-Al catalyst and occurs through an acid-base catalyzed aldol condensation of two octanal molecules to form the C16 aldol, which is further hydrogenated to form the C16 diol.17 The C24 acetal formation is mainly an acid catalyzed reaction and is produced by the Ni-Al and Co-Al catalysts, which showed relatively high specific acidity. Here, the reaction between octanal and octanol tales place over the acidic sites to form C16 hemi acetals which upon dehydration with octanol produces the C24 acetal. The C24 acetal selectivity decreased with increase in temperature. In addition to octanol, C24 acetal and C16 diols, other products (2-hexyl decanol, octanoic acid, octyloctanoate) also formed in small quantities.

Figure 3 shows the product selectivity at an iso-conversion of 95 %, at a temperature of 150 °C and an octanal to hydrogen molar ratio of 2. The product selectivity at iso-conversion is influenced by the metal dispersion and acidic site distribution of the catalysts. The Cu-Al catalyst which showed higher metal dispersion and low acidity, showed the highest selectivity towards octanol with no C24 acetal formation, when compared to the Ni-Al and Co-Al catalysts. No significant difference is seen in the selectivities towards products for the Ni-Al and Co-Al catalysts, probably due to their similar specific acidities and high acidity when compared to the Cu-Al catalyst.

3.3. Kinetics of the Reaction

To gain insight into the reaction mechanism in this study, the rate of the reaction of octanal hydrogenation and turnover number toward octanol were calculated. Since all reactions were carried out at 50 bar pressure, it is assumed that there would be no mass transfer limitations of gaseous hydrogen to the liquid phase. It was also assumed that adsorbed hydrogen was effectively at equilibrium and that the rate limiting step of the reaction is the addition of the second hydrogen atom to the organic moiety.15 As a result, the rate expression was determined to be first order in both aldehyde concentration and hydrogen partial pressure.1,6 The rate of the reaction of catalytic hydrogenation of octanal was found to be proportional to the metal dispersion of the catalysts (Table 4). The catalyst with highest metal dispersion and lowest acidity, i.e Cu-Al, showed the highest rate and the lowest activation energy. The turnover number toward octanol was greater over the Cu-Al catalyst, than over both the Ni-Al and Co-Al catalysts.



4. Conclusion

All three catalysts showed good catalytic hydrogenation activity, however, the Cu-Al catalyst performed better when compared to the Ni-Al and Co-Al catalysts. Cu-Al showed the highest metal dispersion, whereas Co-Al showed the lowest metal dispersion which directly affects the catalyst performance under hydrogenation. Octanal conversion was dependent on the dispersion of metal on the catalysts. The selectivity profiles match the acidic site distributions of the catalysts at iso-conversion. In addition to octanol, other products such as the C16 diol and the C24 acetal were observed in small amounts, which formed via acid-base catalysis on the surface. Octanal hydrogenation follows first-order kinetics and the rate of the reaction is also dependent on the metal dispersion of the catalysts. Among all the catalysts, Cu-Al showed the lowest activation energy and thus highest activity.


Supplementary Material

Supplementary information is provided in the online supplement.



We would like to thank THRIP (Grant TP1208035643), the NRF and SASOL and for financial support. We also thank Dr. N. Prinsloo (SASOL) and the Electron Microscopy Unit at UKZN (Westville campus).



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Received 6 March 2018
Revised 20 August 2016
Accepted 20 August 2018



A.S. Mahomed: © H.B. Friedrich: ©
Present address: Department of Materials Science, Sardar Patel University, Vallabh Vidyanagar-388120, Gujarat, India.
* To whom correspondence should be addressed. E-mail:



Supplementary Data

The supplementary data is available in pdf: [Supplementary data]

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