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Article

Commercial Gold Complexes Supported on Functionalised Carbon Materials as Efficient Catalysts for the Direct Oxidation of Ethane to Acetic Acid

by
Ana P. C. Ribeiro
1,
Inês A. S. Matias
1,
Sónia A. C. Carabineiro
1,2,3,* and
Luísa M. D. R. S. Martins
1,*
1
Centro de Química Estrutural, Institute of Molecular Sciences, Departamento de Engenharia Química, Instituto Superior Técnico, Universidade de Lisboa, Av. Rovisco Pais, 1049-001 Lisboa, Portugal
2
Laboratory of Catalysis and Materials (LCM), Associate Laboratory LSRE-LCM, Faculty of Engineering, University of Porto, 4200-465 Porto, Portugal
3
LAQV-REQUIMTE, Department of Chemistry, NOVA School of Science and Technology, Universidade NOVA de Lisboa, 2829-516 Caparica, Portugal
*
Authors to whom correspondence should be addressed.
Catalysts 2022, 12(2), 165; https://doi.org/10.3390/catal12020165
Submission received: 7 January 2022 / Revised: 21 January 2022 / Accepted: 24 January 2022 / Published: 28 January 2022
(This article belongs to the Special Issue Catalytic Oxidation of Hydrocarbons)
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Abstract

:
The single-pot efficient oxidation of ethane to acetic acid catalysed by Au(I) or Au(III) compounds, chlorotriphenylphosphinegold(I) (1), chlorotrimethylphosphinegold(I) (2), 1,3-bis(2,6-diisopropylphenyl)imidazol-2-ylidenegold(I) chloride (3), dichloro(2-pyridinecarboxylato)gold(III) (4), homogenous and supported on different carbon materials: activated carbon (AC), multi-walled carbon nanotubes (CNT) and carbon xerogel (CX), oxidised with nitric acid followed by treatment with NaOH (-ox-Na), is reported. The reactions were performed in water/acetonitrile. The materials were selective for the production of acetic acid, with no trace of by-products being detected. The best homogenous catalysts were complexes 2 and 3 which showed the highest ethane conversion and an acetic acid yield of ca. 21%, followed by 4 and 1. The heterogenised materials showed much better activity than the homogenous counterparts, with acetic acid yields up to 41.4% for 4@CNT-ox-Na, and remarkable selectivity (with acetic acid being the only product detected). The heterogenised catalysts with the best results were reused up to five cycles, with no significant loss of activity, and maintaining high selectivity for acetic acid. 4@CNT-ox-Na showed not only the best catalytic activity but also the best stability during the recycling runs.

Graphical Abstract

1. Introduction

Direct ethane oxidation is difficult to achieve due to the low reactivity of the C-H bond. The kinetic labile products also increase the difficulty of this potentially rewarding reaction [1]. Economically speaking, this reaction is important, as several bulk chemicals rely on the ethane oxidation products. Among them, acetic acid is the most sought product [2]. It is commercially produced mainly from methanol carbonylation [3], which gives rise to several environmental problems. Methanol carbonylation is responsible for 65% of the world capacity, the remaining 35% being distributed between oxidation of n-butane, acetaldehyde, naphtha and fermentation of hydrocarbons [4].
A new commercial procedure to obtain acetic acid that can replace the carbonylation of methanol is needed. It is important to avoid the use of corrosive chemicals and consequent waste disposal. The economy related to general commodities makes the possibility of new procedures to produce acetic acid a key challenge for catalysis research.
The development of an environmental awareness for catalysis research led to emerging legislation for the impact of chemicals, such as CO2 and methane emission. In addition, the decrease in oil reserves provided the opportunity for exploring alternative feedstocks to produce several commodities. Despite the gas synthesis route of acetic acid being currently an economically appealing process for the production of acetic acid in large-scale (CativaTM process) [3], many energy-demanding intermediate steps augment the total costs of production. Thus, simpler and more economical procedures to produce acetic acid are needed.
The most reported catalysts for the oxidation of ethane are mixtures of calcinated oxides with selectivities up to 96%; however, neither the conversion nor the yield are high. Some reviews can be found on the subject [5,6,7]. The pioneer work of Thorsteinson et al. [8] reports on the selective oxidation of ethane to produce acetic acid on oxide-based catalysts containing Mo, V, and other elements (Nb, Sb, Ti, Ta, Sn, As, W, Fe). These authors stated that ethylene is produced as a principal product, and acetic acid was formed only at higher pressures as a result of subsequent oxidation of ethylene. Several researchers used Mo-V oxides [9,10], sometimes doped with Al [11,12], Nb [13,14,15,16,17,18,19], Pd [16,19] or Nb and Pd [20,21]. Mo-V with redox elements (Pd, Ni, Ti) and acid elements (K, Cs, Te) were also reported, with acetic acid yield maximised for a Mo8V2Nb1Ti0.005Te1 catalyst [22]. Mo-V-M-O (M = Al, Fe, Cr or Ti) complex metal oxide catalysts were also tested [23]. Mo-V materials, frequently doped with other elements, supported on silica [24] and titania [25,26,27,28,29,30] were also described. Molybdo(vanado)phosphoric heteropoly acids with Keggin structure on oxide supports (SiO2, Al2O3, TiO2) are found in the literature [31]. V-P-O oxides were tested [13,32,33], sometimes doped with Mo [32] or supported on titania [25,33]. In addition, titania has been used as a support for VOx catalysts [33,34], along with zirconia [34]. It is not easy to determine which is the actual active and selective phase, as recently stated by Bordes-Richard [7].
Zeolites, such as H-ZSM-5 [35], iron and copper containing ZSM-5 [36,37], Fe/ZSM-5 [37,38], Rh/HZSM-5 [39], platinum and zinc containing LTA zeolite catalysts [40] were used towards the oxidation of ethane, but selectivities do not go beyond 80%, and yields and conversions are still low.
Other catalysts include the iridium clusters and atomically dispersed iridium catalysts on nanodiamond support [41], pyrazole and tris(pyrazolyl)methane rhenium complexes (with a remarkable 40% acetic acid yield) [42,43], or silica, graphite or nafion supported mu-nitrido diiron phthalocyanines [44].
Recently, a highly selective oxidation of ethane to acetic acid was achieved by us [45], using a Fe3O4/TiO2/[FeCl2{κ3-HC(pz)3}] composite, where the C-scorpionate iron(II) catalyst was immobilised at the magnetic core–shell (Fe3O4/TiO2) support.
Gold catalysts have been widely used in many reactions as shown by several reviews [46,47,48,49]. However, the only references found in the literature for the use of gold in ethane oxidation are from the work of Wang et al., dealing with non-supported Au-Pd nanoparticles in water, but the main product obtained was ethyl hydroperoxide [50] and our own work dealing with homogeneous N-heterocyclic carbene and oxo-carbene Au(I) compounds [51]. Therefore, to the best of our knowledge, the present work reports the first use of commercial gold complexes supported on carbon nanomaterials in the oxidation of ethane to produce acetic acid. These complexes had already been used in the oxidation of alcohols and alkanes, in a previous work of ours, with good results [52]. Herein, the one-step oxidation of ethane to acetic acid using a supported catalyst and a mixture of solvents (water and acetonitrile) is reported as a new procedure for ethane oxidation. The present method uses an environmentally sustainable approach, with milder conditions and some commercial catalysts, with good activity and a selectivity of 100% to acetic acid. This is an important step that will contribute considerably to the efficient use of feedstocks.

2. Results and Discussion

2.1. Carbon Supports Characterisation

The carbon-based materials used were activated carbon (AC), multi-walled carbon nanotubes (CNT) and carbon xerogel (CX), oxidised with HNO3 and afterwards treated with NaOH (-ox-Na). Table 1 and Figure 1 show the characterisation results of the original supports and after the treatment.
AC has a high surface area and a great deal of micropores, as expected [52,53,54,55,56,57,58]. However, CX is mainly mesoporous, also as expected [53,57,58,59]. Carbon nanotubes are cylindrical, and the porosity comes from the free spaces of the bundles, which results in a lower surface area [53,57,58,59]. The ox-Na treatment causes the collapse of the pores of AC and CX, decreasing the surface area and pore volume. On CX, the average mesopore width is increased. For CNT, an increase in area is found, possibly due to the opening of some CNT tips with the harsh oxidative treatment.
Figure 1 shows the temperature programmed desorption (TPD) profiles before and after the treatment. It is not surprising that the -ox-Na treatment largely increased the CO and CO2 quantities desorbed (Table 1). The carboxylic acids (that decompose around 200–350 °C as CO2 [53,54,55,56,60] largely increase in treated samples (Figure 1b,d,f). Concerning the CO profiles (Figure 1a,c,e), desorption starts around 350 °C for the AC-ox-Na and CX-ox-Na samples, but only at around 500 °C for the CNT-ox-Na material. This is caused by the decomposition of stable carboxylates and phenolates [59] that desorb as CO at that range of temperatures [53,54,55,56,60].
Catalysts 12 00165 g001 550
Figure 1. TPD results for AC (a,b), CX (c–e) and CNT (e,f). Desorption as CO (a,c,e) and CO2 (b,d,f). The colour bars show the expected temperature ranges for the desorption of the diverse groups (adapted from [52,61]).
Figure 1. TPD results for AC (a,b), CX (c–e) and CNT (e,f). Desorption as CO (a,c,e) and CO2 (b,d,f). The colour bars show the expected temperature ranges for the desorption of the diverse groups (adapted from [52,61]).
Catalysts 12 00165 g001
Table
Table 1. Carbon samples characterisation: surface area (SBET), average mesopore width (L), total pore volume (Vp), micropore volume (Vmicro), determined by adsorption of N2 at −196 °C, and quantities of CO and CO2 desorbed, obtained by TPD. Adapted from [52,61].
Table 1. Carbon samples characterisation: surface area (SBET), average mesopore width (L), total pore volume (Vp), micropore volume (Vmicro), determined by adsorption of N2 at −196 °C, and quantities of CO and CO2 desorbed, obtained by TPD. Adapted from [52,61].
SampleSBET (m2/g)Vp (cm3/g)L (nm)Vmic (cm3/g)CO (µmol/g)CO2 (µmol/g)
AC9740.67-0.34643179
AC-ox-Na6100.35-0.25150122883
CNT2572.89 ~014289
CNT-ox-Na3501.45-~01079838
CX6040.9113.7~0492135
CX-ox-Na5600.7517.60.03637203793

2.2. Heterogenisation Efficiency

The readily available Au(I) and Au(III) commercial complexes chlorotriphenylphosphinegold(I) (1), chlorotrimethylphosphinegold(I) (2), 1,3-bis(2,6-diisopropylphenyl)imidazol-2-ylidenegold(I) chloride (3) and dichloro(2-pyridinecarboxylato)gold(III) (4) (Figure 2) were used as catalysts towards the conversion of ethane into acetic acid. These materials had already been used in the oxidation of alcohols and alkanes in a previous work of ours [52].
The Au compounds were anchored on the different functionalised carbon materials. The intended value was 2% Au loading, but several amounts were obtained on the different carbon materials (Table 2). As shown above, the treatment affects the porous structure and surface properties of the carbon supports. However, all of them were able to anchor the complexes, but with different efficiencies (Table 2). Functionalisation of the supports leads to an increase the amount of surface groups that can “anchor” the compounds [59,61,62,63]. Complex 4 heterogenises similarly on all supports. The other complexes, in general, anchor better on AC-ox-Na. Nevertheless, the values obtained for complexes 2–4 are similar in all carbon materials, showing that the phenolates and carboxylate groups present in these supports (known to be more stable and help anchorage of complexes on the carbon materials [59,61,62,63]) have a larger effect on heterogenisation than the nature of the support itself. Complex 1 has a slightly worse behaviour on CX-ox-Na, but similar results are found for the other complexes. Complex 3 has the lowest heterogenisation amounts. It is possible that the steric effect caused by its large diisopropylphenyl moieties prevents a larger heterogenisation degree.

2.3. Oxidation of Ethane to Acetic Acid

The commercial Au(I) and Au(III) complexes 1–4 (Figure 2) were used as catalysts for the oxidation of ethane to acetic acid. The reaction was carried out using potassium peroxodisulfate as oxidant, in several reaction media/conditions (Table 3). The optimised conditions were found to be the use of aqueous acetonitrile, at 80 °C, during 20 h. All the Au compounds exhibited significant selectivity (acetic acid being the only product detected) and good activity (Figure 3). Blank runs in the presence of ethane and potassium peroxodisulfate (metal-free, determined by ICP) were carried out under the found optimised conditions, which allowed for confirmation that acetic acid was only detected when a gold catalyst was present in the reaction mixture.
The gold(I) catalysts chlorotrimethylphosphinegold(I) (2) and 1,3-bis(2,6-diisopropylphenyl)imidazol-2-ylidenegold(I) chloride (3) afforded the highest ethane conversion with an acetic acid yield of ca. 21% (Figure 3 and Table 3), followed by dichloro(2-pyridinecarboxylato)gold(III) (4) and chlorotriphenylphosphinegold(I) (1). The electronic withdrawing ligand PPh3 associated to its steric hindrance, appears to contribute for the achievement of a lower yield of acetic acid relative to catalysts 2–4, although maintaining the oxidative selectivity. The herein obtained yields (up to 21%) are lower than the recently reported (33–39.8%) for homogeneous N-heterocyclic carbene and oxo-carbene gold(I) catalysts [51]. However, we should keep in mind the advantageous availability of the commercial Au compounds relative to harder-to-prepare and less stable carbene complexes.
The literature common solvent for ethane oxidation, trifluoroacetic acid (TFA) [64,65], was also tested with the gold complexes 1–4. As presented in Figure 3, the performance of all catalysts decreases considerably in TFA when compared with the exhibited in the greener aqueous mixture: a maximum of 14.2% yield of acetic acid is attained for complex 3, whereas for complexes 1, 2 and 4, an even more marked yield reduction (Table 3) is observed.
Despite the above promising results in the water/acetonitrile mixture, the major drawback presented by the homogeneous catalysts 1–4 is their lack of recyclability. Therefore, the gold complexes 1–4 were supported on functionalised carbon materials (Section 2.2) and applied as heterogeneous catalysts for the oxidation of ethane to produce acetic acid (Scheme 1). The selected carbon supports were oxidised with nitric acid and subsequently treated with sodium hydroxide (-ox-Na).
The reactions were performed using potassium peroxodisulfate as an oxidant in several reaction media/conditions (selected results presented in Table 4) to reach the optimised heterogeneous catalytic systems. As found in homogeneous conditions (see above), aqueous acetonitrile, at 80 °C, for 20 h, provided the best results (Table 4). Blank runs in the presence of ethane, potassium peroxodisulfate and each carbon material were carried out under the found optimised conditions, which allowed for confirmation that acetic acid was only detected when a gold catalyst was present in the reaction mixture.
All hybrid catalysts obtained by immobilisation of the gold complexes on the carbon materials exhibited an amazing selectivity (only acetic acid was detected) and a clearly improved catalytic performance relative to the homogeneous analogues (compare Table 3 and Table 4). Indeed, under optimised conditions, the hybrid catalysts allowed for attainment of up to 41.4% yield of acetic acid (entry 32 of Table 3, for catalyst 4@CNT-ox-Na), whereas a maximum of 20.9% yield was reached under homogeneous conditions (entry 10 of Table 3, for catalyst 3). Moreover, an increase of 10 times on the catalyst amount (from 1.5 to 15 μmol Au) did not impart a significant changing of the acetic acid formed (compare e.g., entries 12 and 14, Table 4). It is possible that a larger amount of catalyst can lead to mixing problems and possible agglomeration of material (which decreases the number active catalyst sites). Thus, the lower loading (1.5 μmol Au) was chosen as the optimum amount. It is worth highlighting the low catalyst amount used in this oxidation reaction.
As expected from the results in homogeneous conditions, the performance of all catalysts decreased considerably in TFA (Figure 4) when compared with the ones exhibited in the greener aqueous mixture (a maximum of 14.2% yield of acetic acid is attained for 1@CNT-ox-Na, entry 7, Table 3).
The type of support also played a role on the catalytic activity of complexes 1–4 towards the formation of acetic acid, as depicted in Figure 4. CNT-ox-Na was the best support. The phenolate and carboxylate groups (formed by the -ox-Na treatment) might act as coordinating sites [59] for the complexes. The good performance of CNT might be caused by a textural effect (as CNT are nonporous, the reactants easily access the active), or an electronic effect (due to the graphitic structure of CNT), which can increase the interactions with the reactants or the intermediate radicals, as proposed by us on previous papers [52,62]. The Au(III) catalyst 4@CNT-ox-Na led to the highest acetic acid yield (41.4%), among the commercial gold complexes 1–4 heterogenised at functionalised carbon nanotubes (Figure 5).
The stability of the catalysts supported on functionalised carbon nanotubes that exhibited the highest catalytic performances (acetic acid yields above 30%, Figure 5) was investigated towards recycling experiments. Thus, each hybrid catalyst was recovered from the oxidation medium, and consecutive catalytic oxidation cycles with fresh reagents were run (see Experimental section). These catalysts were effortlessly recovered and reused up to five cycles with no significant loss of activity, while maintaining their selectivity towards the formation of acetic acid (Figure 6). Again, catalyst 4@CNT-ox-Na presented the best behaviour; its stability was less affected by the consecutive oxidative runs.
The possible gold leaching from the support as well as the formation of gold nanoparticles was accessed at the end of each catalytic cycle for catalyst 4@CNT-ox-Na. The analysis for the gold loading by inductively coupled plasma atomic emission spectroscopy (ICP-AES) of the remaining liquid phase, after the catalytic test up to the fifth run, did not show the presence of any gold. Therefore, we can assume that there was no catalyst leaching from the support. In addition, the formation of Au(0) nanoparticles from a possible decomposition of the gold complexes to form free gold ions was investigated by performing UV–vis spectra of the remaining liquid phase, after each catalytic cycle. No UV–plasmon band was observed in the usual region of 500–550 nm, indicating the absence of Au(0) nanoparticles formation.

3. Materials and Methods

3.1. General Reagents

All solvents and reagents were purchased from commercial companies and used as received.

3.2. Gold Complexes

Different Au(I) and Au(III) complexes were used (Figure 1). The Au(I) complexes, chlorotriphenylphosphinegold(I) (1), chlorotrimethylphosphinegold(I) (2) and 1,3-bis(2,6-diisopropylphenyl)imidazol-2-ylidenegold(I) chloride (3) were obtained from Strem Chemicals. The dichloro(2-pyridinecarboxylato)gold(III) (4), used for the first time as catalyst by Hashmi et al. [66], was purchased from Aldrich.

3.3. Carbon Supports

Activated carbon Norit® RO 0.8 (AC) was purchased from Sigma-Aldrich, multi-walled carbon nanotubes NC3100 (CNT) were obtained from NanocylTM. Carbon xerogel (CX) prepared by the condensation of resorcinol and formaldehyde, as already described [56,67]. The supports were functionalised with 5 M nitric acid solution and subsequently treated with NaOH, as reported elsewhere [61,62,63,68,69,70,71,72].

3.4. Supports Characterisation

The carbon materials were characterised by N2 adsorption (−196 °C) on a Quantachrome Nova 4200e device and by temperature programmed desorption (TPD) with an Altamira AMI-300 apparatus. Further details can be found elsewhere [52].

3.5. Heterogenisation Procedure

The complexes were supported onto each carbon materials to obtain ~2% Au per mass of carbon using methanol. The Au loading was determined by inductively coupled plasma atomic emission spectroscopy (ICP-AES) at the IST Analysis Lab.

3.6. Catalytic Tests

The catalytic oxidation of ethane to acetic acid was performed in a stainless-steel reactor. First, 4.33 mmol of oxidant (K2S2O8) and 1.50 μmol of catalyst (1–4) were added to 6 mL of H2O/CH3CN (or 5.5 mL of trifluoroacetic acid). After closing the reactor, it was flushed thrice with ethane and pressurised at 3 atm (0.78 mmol), heated at 80 °C (higher temperatures lead to a decrease in the solubility of ethane and decomposition of the oxidant) [73] for 20 h. Then, the reactor was cooled to room temperature, degassed, and opened. Then, 5 mL of diethyl ether (to cause precipitation of the homogeneous gold catalysts and extract the organic products) and 90 μL de n-butyric acid (internal standard) were added to 1 mL of mixture and stirred for 30 min. After filtration, the liquid was analysed by gas chromatography (GC) using a FISONS Instruments GC 8000 with an FID detector and a DB-WAX capillary column (internal diameter 0.32 mm, length 30 m) software using He as a carrier, with an injection temperature of 240 °C. The values were obtained by average from several runs with similar results.
Concerning the recycling experiments, each hybrid catalyst was recovered from the oxidation medium of the first catalytic cycle by separating it from the liquid phase medium by gravity filtration. The solid was washed 5 times with water/acetonitrile mixture and then 3 times with diethyl ether. Then, it was dried in an oven at 50 °C overnight. The 2nd catalytic cycle was initiated by placing the dried recovered catalyst and all fresh reagents into the reactor and repeating the conditions of the first catalytic cycle. The following consecutive catalytic oxidation cycles, up to the 5th one, were run in the same way.
The occurrence of leaching during the catalytic reaction or the catalyst recovery process was investigated by UV measurements of the remaining liquid phase, performed in a lambda 35, Perkin Elmer (Waltham, MA, USA).

4. Conclusions

The single-pot oxidation of ethane to acetic acid was studied using Au(I) or Au(III) compounds, in their homogenous forms and supported on AC-ox-Na, CX-ox-Na and CNT-ox-Na, as catalysts. The heterogenised catalysts showed outstanding selectivity (with acetic acid being the only product detected) and much better activity than the homogenous counterparts, with acetic acid yields up to 41.4% for 4@CNT-ox-Na. The presence of TFA was detrimental for the catalytic activity, showing that aqueous (green) conditions are more adequate. The best support was CNT-ox-Na. The phenolate and carboxylate groups (formed by the -ox-Na treatment) seemed to be beneficial. Selected heterogenised catalysts were easily recovered and reused up to five cycles, with no significant loss of activity, maintaining a high selectivity for acetic acid 4@CNT-ox-Na showed not only the best catalytic performance, but also the best stability in the recycling tests.

Author Contributions

Conceptualisation, A.P.C.R. and L.M.D.R.S.M.; investigation, I.A.S.M. and S.A.C.C.; writing, L.M.D.R.S.M. and S.A.C.C.; supervision, A.P.C.R. and L.M.D.R.S.M.; funding acquisition, L.M.D.R.S.M. and S.A.C.C. All authors have read and agreed to the published version of the manuscript.

Funding

This research was funded by Fundação para a Ciência e Tecnologia (FCT), projects UIDB/00100/2020 and UIDP/00100/2020 of Centro de Química Estrutural and IMS—LA/P/0056/2020. APCR thanks Instituto Superior Técnico for the Scientific Employment contract IST-ID/119/2018. IASM is thankful to FCT for her PhD fellowship (SFRH/BD/146426/2019). It was also funded by national funds though FCT, under the Scientific Employment Stimulus–Institutional Call (CEEC-INST/00102/2018). We also acknowledge the Associate Laboratory for Green Chemistry—LAQV financed by national funds from FCT/MCTES (UIDB/50006/2020 and UIDP/50006/2020) and Base-UIDB/50020/2020 and Programmatic-UIDP/50020/2020 funding of the Associate Laboratory LSRE-LCM.

Institutional Review Board Statement

Not applicable.

Informed Consent Statement

Not applicable.

Data Availability Statement

Data will be made available upon request.

Conflicts of Interest

The authors declare no conflict of interest.

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Catalysts 12 00165 g002 550
Figure 2. Structures of commercial chlorotriphenylphosphinegold(I) (1), chlorotrimethylphosphinegold(I) (2), 1,3-bis(2,6-diisopropylphenyl)imidazol-2-ylidenegold(I) chloride (3) and dichloro(2-pyridinecarboxylato)gold(III) (4).
Figure 2. Structures of commercial chlorotriphenylphosphinegold(I) (1), chlorotrimethylphosphinegold(I) (2), 1,3-bis(2,6-diisopropylphenyl)imidazol-2-ylidenegold(I) chloride (3) and dichloro(2-pyridinecarboxylato)gold(III) (4).
Catalysts 12 00165 g002
Catalysts 12 00165 g003 550
Figure 3. Acetic acid yields obtained by oxidation of ethane catalysed by the commercial gold complexes 1–4, using K2S2O8, under optimised conditions.
Figure 3. Acetic acid yields obtained by oxidation of ethane catalysed by the commercial gold complexes 1–4, using K2S2O8, under optimised conditions.
Catalysts 12 00165 g003
Catalysts 12 00165 sch001 550
Scheme 1. Acetic acid formation by selective oxidation of ethane catalysed by the commercial gold complexes 1–4 immobilised on carbon materials, using K2S2O8.
Scheme 1. Acetic acid formation by selective oxidation of ethane catalysed by the commercial gold complexes 1–4 immobilised on carbon materials, using K2S2O8.
Catalysts 12 00165 sch001
Catalysts 12 00165 g004 550
Figure 4. Acetic acid yields for the direct oxidation of ethane catalysed by the commercial gold complexes 1–4 heterogenised at carbon materials, by K2S2O8, under optimised conditions (1.5 μmol of Au, 80 °C).
Figure 4. Acetic acid yields for the direct oxidation of ethane catalysed by the commercial gold complexes 1–4 heterogenised at carbon materials, by K2S2O8, under optimised conditions (1.5 μmol of Au, 80 °C).
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Catalysts 12 00165 g005 550
Figure 5. Acetic acid yields achieved by direct oxidation of ethane catalysed by the commercial gold complexes 1–4 heterogenised at functionalised carbon nanotubes, using K2S2O8, under optimised conditions (1.5 μmol of Au, 80 °C).
Figure 5. Acetic acid yields achieved by direct oxidation of ethane catalysed by the commercial gold complexes 1–4 heterogenised at functionalised carbon nanotubes, using K2S2O8, under optimised conditions (1.5 μmol of Au, 80 °C).
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Catalysts 12 00165 g006 550
Figure 6. Recycling assays (at optimised conditions) using the commercial gold complexes 1, 2 and 4 heterogenised at functionalised carbon nanotubes.
Figure 6. Recycling assays (at optimised conditions) using the commercial gold complexes 1, 2 and 4 heterogenised at functionalised carbon nanotubes.
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Table
Table 2. Gold loading (mmol/g) of the complexes 1–4 heterogenised on carbon materials (data from [52]).
Table 2. Gold loading (mmol/g) of the complexes 1–4 heterogenised on carbon materials (data from [52]).
@AC-ox-Na@CX-ox-Na@CNT-ox-Na
10.200.010.17
20.050.060.04
30.030.020.03
40.100.100.10
Table
Table 3. Results for the direct oxidation of ethane to acetic acid catalysed by compounds 1–4 in homogenous conditions a.
Table 3. Results for the direct oxidation of ethane to acetic acid catalysed by compounds 1–4 in homogenous conditions a.
EntryCatalystTemperature (°C)SolventYield b (%)TON cTOF d
1180TFA4.9543
280ACN/H2O12.71417
350TFA000
450ACN/H2O0.100
5280TFA4.4493
680ACN/H2O20.422611
750TFA3.2352
850ACN/H2O5.3593
9380TFA14.21578
1080ACN/H2O20.923112
1150TFA000
1250ACN/H2O0.200
13480TFA8.9985
1480ACN/H2O15.71749
1550TFA3.1342
1650ACN/H2O5.2583
a Reaction conditions (unless otherwise stated): p C2H6 3 atm, 1.5 mmol of catalyst (1–4), K2S2O8 (4.33 mmol), 20 h. Reactions were performed in 5.5 mL of TFA or 6 mL of water/acetonitrile mixture. b Yield (%) = mol of acetic acid/100 mol of ethane. c TON = mol of acetic acid/mol of catalyst (1–4). d TOF = (mol of acetic acid/mol of catalyst (1–4))/time.
Table
Table 4. Direct oxidation of ethane to acetic acid catalysed by compounds 1–4 heterogenised on selected carbon materials a.
Table 4. Direct oxidation of ethane to acetic acid catalysed by compounds 1–4 heterogenised on selected carbon materials a.
EntryCatalystCatalyst Amount
(μmol Au)		Temperature (°C)SolventYield b (%)TON cTOF d
11@CNT-ox-Na1.580TFA7.2804
21@CNT-ox-Na1.580ACN/water33.437019
31@CNT-ox-Na1580TFA6.980
41@CNT-ox-Na1580ACN/water36.5402
51@CNT-ox-Na1.550TFA0.220
61@CNT-ox-Na1.550ACN/water000
71@CX-ox-Na1.580TFA14.21578
81@CX-ox-Na1.580ACN/water21.223512
91@AC-ox-Na1.580TFA8.9985
101@AC-ox-Na1.580ACN/water16.21799
112@CNT-ox-Na1.580TFA8.3925
122@CNT-ox-Na1.580ACN/water32.732216
132@CNT-ox-Na1580TFA10.1111
142@CNT-ox-Na1580ACN/water31.6352
152@CNT-ox-Na1.550TFA0.670
162@CNT-ox-Na1.550ACN/water1.1121
172@CX-ox-Na1.580TFA1.5171
182@CX-ox-Na1.580ACN/water23.225713
192@AC-ox-Na1.580TFA0.890
202@AC-ox-Na1.580ACN/water25.328014
213@CNT-ox-Na1.580TFA13.21467
223@CNT-ox-Na1.580ACN/water26.329115
233@CX-ox-Na1.580TFA12.736218
243@CX-ox-Na1.580ACN/water21.623912
253@CX-ox-Na1580TFA14.3161
263@CX-ox-Na1580ACN/water29.4332
273@CX-ox-Na1.550TFA000
283@CX-ox-Na1.550ACN/water000
293@AC-ox-Na1.580TFA11.41266
303@AC-ox-Na1.580ACN/water20.722911
314@CNT-ox-Na1.580TFA12.81427
324@CNT-ox-Na1.580ACN/water41.445823
334@CNT-ox-Na1580TFA11.3131
344@CNT-ox-Na1580ACN/water39.7442
354@CNT-ox-Na1.550TFA0.9101
364@CNT-ox-Na1.550ACN/water1.3141
374@CX-ox-Na1.580TFA13.81538
384@CX-ox-Na1.580ACN/water33.437019
394@AC-ox-Na1.580TFA7.2804
404@AC-ox-Na1.580ACN/water13.41488
a Reaction conditions (unless stated otherwise): p C2H6 3 atm, K2S2O8 (4.33 mmol), 20 h. Reactions were performed in 5.5 mL of TFA or 6 mL of water/acetonitrile mixture. b Yield (%) = mol of acetic acid/100 mol of ethane. c TON = mol of acetic acid/mol of Au. d TOF = (mol of acetic acid/mol of catalyst (1–4))/time.
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Ribeiro, A.P.C.; Matias, I.A.S.; Carabineiro, S.A.C.; Martins, L.M.D.R.S. Commercial Gold Complexes Supported on Functionalised Carbon Materials as Efficient Catalysts for the Direct Oxidation of Ethane to Acetic Acid. Catalysts 2022, 12, 165. https://doi.org/10.3390/catal12020165

AMA Style

Ribeiro APC, Matias IAS, Carabineiro SAC, Martins LMDRS. Commercial Gold Complexes Supported on Functionalised Carbon Materials as Efficient Catalysts for the Direct Oxidation of Ethane to Acetic Acid. Catalysts. 2022; 12(2):165. https://doi.org/10.3390/catal12020165

Chicago/Turabian Style

Ribeiro, Ana P. C., Inês A. S. Matias, Sónia A. C. Carabineiro, and Luísa M. D. R. S. Martins. 2022. "Commercial Gold Complexes Supported on Functionalised Carbon Materials as Efficient Catalysts for the Direct Oxidation of Ethane to Acetic Acid" Catalysts 12, no. 2: 165. https://doi.org/10.3390/catal12020165

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