Furfural Oxidation on Gold Supported on MnO₂: Influence of the Support Structure on the Catalytic Performances

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The catalysts developed in this work could be potentially used industrially for green oxidations of bio-based compounds.

Abstract

A series of catalysts consisting of gold nanoparticles supported on MnO₂ presenting different morphologies were synthesized and tested in the base-free oxidation of furfural. Ultra-small Au particles (less than 3 nm) were deposited on low (commercial MnO₂) and high (NF, nanoflowers and NW, nanowires MnO₂) surface area supports. High activity was observed for Au/MnO₂-NF material with very high selectivity to furoic acid. The X-ray photoelectron spectroscopy (XPS) study confirmed the presence of a significant amount of highly active Au^δ+ species on the surface of the Au/MnO₂-NF catalyst. These species seem to be responsible for the high activity in oxidation of furfural under mild conditions (air as oxidant, 110 °C).

1. Introduction

In recent decades, supported gold nanoparticles have been extensively studied because of their unusual catalytic properties [1,2,3,4]. It is well recognized that the size of gold nanoparticles determines both the activity and the selectivity of the final catalyst [4,5]. It is also considered that the drastic change of the catalytic properties of nanoparticles is due to their new properties (physical and chemical) which are created when their size decreases, mainly due to the significant increase in the number of atoms on the surface [5,6,7]. However, when working with supported gold nanoparticles (NPs), the support also plays a very important role. Supported gold nanoparticles should be well dispersed to be able to interact with the support. Appropriate support can increase the dispersion of gold NPs, and hence improve the overall catalytic activity [8]. For Au catalysts supported on reducible supports, such as Fe₂O₃, TiO₂, CeO₂, and MnO₂, the dominant reaction pathway is expected to involve adsorption of a molecular oxygen species on the support, its dissociation at the interface, and then its reaction with the substrate [9]. In the case of Au supported on inert oxides (SiO₂ or Al₂O₃), the oxygen supply most likely proceeds via direct dissociative adsorption on the Au particles. The influence of the support on the catalytic activity strongly depends on the type of catalyzed reaction [10]. Ishida et al. [11] studied the effect of supported gold catalyst on the catalytic oxidation of glucose. They found that compared to gas phase catalytic oxidation reactions (such as for instance oxidation of CO), in the liquid phase oxidation, the influence of gold particle size is more important than the nature of the support. Commoti et al. [12] observed similar results. They have also stated that the size of the Au particles appears to be the most important parameter. However, in these studies, the oxidation was always performed at high pH [12]. Indeed, the majority of works in the literature deal with the oxidation of sugars or of other bio-based compounds at controlled basic pH. At this pH, the substrates were almost always completely converted [13]. Moreover, several papers reported the need for a basic medium to perform the selective oxidation [12,13,14,15]. According to them, the presence of a base allows higher reaction rates, higher feed concentrations, better product solubility and lower adsorption of the products on the catalyst surface. However, oxidation in the liquid phase may occur at the interface between Au particles and the support. In this case, the activation energy would be different, depending on the nature of the support. Metal-oxide support interactions might affect Au clusters electronically and lead to weaker rate dependencies than those observed for unsupported Au nanoparticles. Obviously, the metal-support interactions depend on the nature of the support and of its structure [16]. It would be preferable to study the support effects without using basic conditions. Indeed, in the high pH range, the base used for the reaction governs the mechanism of the reaction. There is no systematic study in the literature which establishes a correlation between the support structure interacting with gold nanoparticles and their catalytic activity and selectivity. Therefore, we attempted to study the catalytic performance of supported gold nanoparticles for the base-free oxidation of furfural, using different manganese oxide structures (MnO₂) as supports. Firstly, the oxidation of furfural can lead to interesting products, such as 2-furoic [17] or maleic acid [18]. Indeed, 2-furoic acid can undergo a C-H carboxylation with CO₂ to form 2,5-furanodicarboxylic acid (FDCA) [19]. Secondly, MnO₂ is one of the most attractive materials because of its technological importance and possible application in different catalytic and electrochemical processes [20]. Moreover, the properties of MnO₂ are significantly influenced by its structure and morphology, which permits the study of the effect of the support structure on the catalytic activity. Therefore, we report herein about catalysts composed of MnO₂ with different structures modified with very small gold nanoparticles. Prepared materials were studied in the liquid phase oxidation of furfural using air (or oxygen) as the oxidant and water as the solvent.

2. Materials and Methods

2.1. Materials

Analytical grade chemicals chloroauric acid trihydrate (HAuCl₄·3H₂O, 99.9%, Sigma-Aldrich, St. Louis, MO, USA), manganese sulfate monohydrate (MnSO₄·H₂O, 99%, Sigma-Aldrich, St. Louis, MO, USA), potassium permanganate (KMnO₄, 99%, Sigma-Aldrich, St. Louis, MO, USA), ethylene glycol (EG, 99,8%, Sigma Aldrich, St. Louis, MO, USA), sodium borohydride (NaBH₄, 98%, Sigma-Aldrich, St. Louis, MO, USA), polyvinylpyrrolidone (PVP, Sigma-Aldrich, St. Louis, MO, USA, M.W. 55,000 g/mol), manganese oxide (MnO₂, ReagentPlus^®, St. Louis, MO, USA, ≥99%, Sigma-Aldrich—further noted MnO₂-Comm), furfural (C₅H₄O₂, > 99%, Sigma-Aldrich, St. Louis, MO, USA) were used as received. All solutions were prepared using deionized water (18.2 MΩ).

The MnO₂ nanoflowers (MnO₂-NF) and nanowires (MnO₂-NW) were obtained by a hydrothermal approach, as described elsewhere [21]. In a typical procedure for the synthesis of nanoflowers, 0.4 g of MnSO₄. H₂O and 1.0 g of KMnO₄ were dissolved in 30 mL of deionized water. This solution was transferred to a 100 mL Teflon-lined stainless-steel autoclave. The autoclave was heated and stirred at 140 °C for 1 h and then allowed to cooled down to room temperature. For the synthesis of MnO₂ nanowires, the same procedure was employed, but the autoclave was heated and stirred at 140 °C for 18 h. The products were collected by centrifugation and washed three times with ethanol (15 mL) and three times with water (15 mL) by successive rounds of centrifugation and removal of the supernatant. As-prepared materials were then dried at 80 °C for 6 h in air.

The supported gold nanoparticles were prepared as follow: Typically, 200 mg of MnO₂ support and 260 mg of PVP were added to 200 mL of EG. The obtained suspension was transferred to a 25 mL round-bottom flask and kept under vigorous stirring at 90 °C for 20 min. Then, 3.0 mL of a 120 mM NaBH_4(aq) and 3 mL of a 24 mM AuCl₄^-_(aq) solutions were sequentially added to the reaction flask. This mixture was kept under vigorous stirring for another 1 h to produce Au/MnO₂. After cooling down to room temperature, the Au/MnO₂ materials were isolated by centrifugation and washed three times with acetic acid (15 mL), three times with ethanol (15 mL), and three times with water (15 mL) by successive rounds of centrifugation at 6000 rpm for 5 min and removal of the supernatant. After washing, the Au/MnO₂ materials were dried at 120 °C for 6 h in air.

2.2. Characterization

The transmission electron microscopy (TEM) and high-resolution transmission electron microscopy (HRTEM) images were obtained with a JEOL JEM2100 microscope (JEOL USA, Peabody, MA, USA) operated at 200 kV. High angle annular dark field (HAADF) and energy dispersive X-ray spectroscopy (EDS) images were acquired using a FEI TECNAI G2 F20 (The Ames Laboratory, Ames, IA, USA) operated at 200 kV. Samples for HRTEM, HAADF-STEM (High-angle annular dark-field scanning transmission electron microscopy), and EDX-STEM (Energy-dispersive X-ray spectroscopy scanning transmission electron microscopy) were prepared by drop-casting an aqueous suspension of the nanostructures over a carbon-coated copper grid, followed by drying under ambient conditions. The Au atomic percentage was measured by flame atomic absorption spectrometry (FAAS) with a Shimadzu spectrophotometer, model AA-6300 (Shimadzu Corp., Kyoto, Japan), equipped with an air-acetylene flame. Leaching tests were performed using ICP-OES (Inductively Coupled Plasma Optical Emission Spectrometry). An Agilent 720-ES ICP-OES (Agilent Technologies, Santa Clara, CA, USA) was used for determining the elemental composition of the reactant solutions.

Temperature-programmed reduction with hydrogen (H₂-TPR) was carried out in a Micrometrics Chemisorb 2705. Usually, 0.1 g of a catalyst was dried with N₂ flow at 125 °C for 1 h. Then, the sample was cooled down to room temperature, and then reduced up to 1000 °C (ramp 5·°C·min⁻¹) under H₂ flow (30 mL·min⁻¹). X-ray photoelectron spectroscopy (XPS) data of the samples were obtained with a SPECSLAB II (Phoibos-Hsa 3500 150, 9 channeltrons) SPECS spectrometer, with Al Kα source (E = 1486.6 eV) operating at 12 kV, pass energy (Epass) = 40 eV, 0.1 eV energy step and an acquisition time of 1 s per point. The samples were placed on stainless-steel sample-holders, transferred under inert atmosphere to the XPS pre-chamber and held there for 2 h in a vacuum. The residual pressure inside the analysis chamber was ~1×10⁻¹ Torr. The binding energies (BE) of the Mn 2p, Au 4f and C 1s spectral peaks were referenced to the C 1s peak at 284.5 eV, providing accuracy within ± 0.2 eV. Textural characteristics of the catalysts were determined from nitrogen adsorption isotherms, recorded at −196 °C in a Quantachrome Nova 1000. The samples (ca. 100 mg) were degassed for 3 h at 150 °C before analysis. Specific surface areas were determined by the Brunauer-Emmett-Teller equation (BET method) from an adsorption isotherm generated in a relative pressure range 0.07 < P/Po < 0.3. The total pore volume was calculated from the amount of N₂ adsorbed at a relative pressure close to unity. The average pore diameter was determined by the Barrett-Joyner-Halenda (BJH) method, from the N₂ desorption isotherms.

2.3. Catalytic Tests

Furfural oxidation was carried out on the REALCAT platform [22] in a Screening Pressure Reactors system (SPR) from Unchainedlabs, equipped with 24 parallel batch reactors for high-throughput screening of the catalytic materials. The catalysts (10 mg) were placed in each reactor. Then, 3 mL of an aqueous solution of furfural (1.0 wt %) was injected. The catalytic tests were performed under air (12 bar) for 2 h at 110 °C under acidic pH (pH = 3). After the reactions, the reactors were cooled down to room temperature. The liquid products were analyzed by High Performance Liquid Chromatography (HPLC, Waters 2410 RJ) equipped with RI and UV detectors and a Shodex SUGARSH-1011 column (8 × 300 mm). Diluted H₂SO₄ (5 mM, 1 mL/min) was used as a mobile phase. Commercial standards (furoic acid, furfural) were used for calibration of the HPLC set up. The recyclability tests were done in the same reaction conditions. Temperature, initial pressure, air atmosphere, duration of the reaction, catalyst amount and initial reactant concentration were set as follow: 110 °C, 12 bar, air, 2 h, furfural:Au ratio of 100:1. After the first run, the reactant solution was taken out from the reactor using a syringe. The catalyst was recovered by centrifugation, and then dried at 100 °C overnight. The next day, the second run was performed. The same amount of catalyst was weighed and added to the reactor. After that, the reactor was closed, and the test was performed again in the same conditions as previously used.

3. Results

In order to characterize the materials, several techniques have been used: HRTEM, FAAS and XPS. It is already well established that the catalytic activity of the supported gold catalysts strongly depends on the average Au particle size. HRTEM measurements were applied to determine the exact size distribution of the synthesized gold nanoparticles. In our case, the strategy was to prepare, on different supports, ultra-dispersed gold nanoparticles with similar average particle size, using PVP as a stabilizer and NaBH₄ as a reductant. Indeed, this method is generally applied for the synthesis of nanometric metallic nanoparticles [23].

3.1. Structural properties

TEM images of the Au/MnO₂-MF, Au/MnO₂-NW and Au/MnO₂-Comm materials obtained by this route are shown in Figure 1. The Au NPs deposited on the different supports were monodispersed, and had very small sizes of about 2.6 nm (±0.8 nm) in all cases. Moreover, as could be seen, Au nanoparticles were uniformly dispersed onto the MnO₂ surfaces. In addition, no significant agglomeration of gold nanoparticles was detected.

The different morphologies of the three different MnO₂ supports used were clearly observed in the TEM images. Moreover, significant differences were also observed in the specific surface areas of these materials, as can be seen in

Table 1. Au wt %, Au gold particle size, BET surface area, pore volume and pore diameter determined by FAAS, TEM and BET - N₂ adsorption, respectively.

Catalyst	Au (wt %)	Particle size (nm)	Surface Area (m2/g)	Pore Volume (cm3/g)	Pore Diameter (Å)
Au/MnO2-NF	1.3	2.6	196	0.42	6.1
MnO2 NF	-	-	194	0.41	6.1
Au/MnO2-NW	1.3	3.2	125	0.16	6.9
MnO2-NW	-	-	122	0.16	6.8
Au/MnO2-Comm	1.4	2.6	15	0.05	17.8
MnO2-Comm	-	-	14	0.05	17.8

.

The specific surface areas of both homemade MnO₂ supports (MnO₂-NF and MnO₂-NW) are roughly ten times as high as that of the commercial oxide (MnO₂-Comm). The nanoflowers MnO₂ presented the highest surface, and also pore volume (Table 1). These characteristics could strongly influence the activity of this material. Moreover, the modification of the MnO₂ materials with gold nanoparticles did not change the structural and morphological properties of the bare support. Indeed, as could be expected, high dispersion of the gold nanoparticles permitted a slight increase in the overall specific surface areas of the prepared catalysts. It is interesting to note that the huge differences in the surface areas of the commercial support and the homemade samples did not impact the average particle size of the gold nanoparticles (Table 1). Indeed, this was one of the objectives of this work, and it is due to the method of preparation of the Au particles using PVP as a stabilizer. Taking into account the same average Au particle size and metal loading, it seems that the catalytic performances should be governed mostly by the structure and the morphology of the support.

Interesting results were obtained from H₂-TPR studies (Figure 2). The reducibility of the MnO₂ support represents an important parameter in the context of catalytic applications. This is because Au NPs (active phase) can strongly interact with metal oxides and change their redox properties. This, in turn, can affect catalytic activity.

The TPR profile for MnO₂ nanoflowers displayed two peaks, centred at 284 and 323 °C, assigned to the reduction of MnO₂ to Mn_xO_y (displaying lower oxidation states) [24]. After the deposition of the ultra-small Au NPs at the nanoflowers’ surface, a marked change in the TPR profile was observed. Indeed, the reduction of MnO₂ was shifted to lower temperatures, and three main reduction peaks corresponding to the reduction of Mn₃O₄ to MnO (113 °C), Mn₂O₃ to Mn₃O₄ (252 °C), and MnO₂ to Mn₂O₃ (287 °C) could be observed [24,25]. This effect may be due to strong metal-support interactions. Previous investigations suggested that the presence of small Au NPs can also facilitate the MnO₂ reduction [25]. Results obtained from H₂-TPR showed that high surface area support (MnO₂-NF) and smaller Au NPs led to stronger metal-support interactions, due to the higher interfacial perimeter between Au and the oxide support. The reduction of MnO₂ occurred, in this case, at lower temperature. In contrast, the low surface area support (MnO₂-comm) presents lower interaction between metal and oxide, and the presence of gold does not significantly change the high reduction temperature of this support.

3.2. Catalytic Activity

All prepared samples and bare supports were tested in the aqueous phase oxidation of furfural to furoic acid. Supports alone showed, already, a significant activity for this reaction (up to 55% furfural conversion in case of MnO₂-NF). However, the selectivity to furoic acid was much lower than in the case of Au-modified samples (c.a. 80%). It reached only 25% in the case of the MnO₂-NF sample at a furfural iso-conversion of 55%. It is well established that MnO₂ materials are good catalysts for oxidation reactions. Generally, oxidation of furfural to furoic acid is carried out in the presence of hazardous oxidants [26,27] or heterogeneous catalysts in a strong alkaline solution [28]. However, at alkaline pH, degradation of furfural can occur, resulting in a drop of selectivity. Furthermore, instead of leading to furoic acid salt, the oxidation reaction can yield mixtures of low and high molecular weight products. The basic medium is also related to degradation of furfural and the formation of other furan derivates (such as 5-HMF) under reaction conditions. Tests in absence of catalyst showed conversion without any detection of oxidation products. In addition, a colour change was noticed in the reaction mixture from yellow to brownish, with the formation of a black precipitate [29,30]. This precipitate was attributed to the formation of humic acids, which are a mixture of many different acids that can be formed during dehydration, and also arise from the condensation of furfural. The present study showed that working in base-free conditions is possible using highly selective supported gold nanoparticles. Figure 3 presents the results obtained for furfural oxidation with air at 110 °C. After only 2 h of reaction, Au/MnO₂-NF catalyst reached 86% of furfural conversion (

Table 2. Screening of the catalytic conditions using Au/MnO₂-NF catalyst. P = 12 bar (air), furfural:Au molar ratio = 100:1.

Entry	T [°C]	Time [min]	XFUR [%]	SFA [%]	CB [%]
1	110	30	45	82	93
2	110	70	61	80	93
3	110	120	86	72	92
4	110	240	100	82	93
5	80	120	31	92	92
6	80	240	65	89	96
7	150	120	100	67	75

, Entry 3). At the same time, Au supported on commercial MnO₂ oxide showed only 69% of conversion. In the case of both homemade catalysts (Au/MnO₂-NF and Au/MnO₂-NW), very high selectivity to furoic acid was obtained (more than 80%), and the carbon balance values indicated that no degradation of furfural occurred.

The most active Au/MnO₂-NF catalyst was tested in different reaction conditions, to optimize the furoic acid yield. As could be seen from Table 2, full furfural conversion was reached after 4 h of reaction at 110 °C (Entry 4). In addition, this catalyst was already active at lower temperatures, and 65% of conversion was obtained at 80 °C after 4 h of reaction. The best results were obtained at 110 °C and after 4 h of reaction. In these conditions, furoic acid can be produced with a yield of 82% (Entry 4).

The reaction temperature strongly affects the catalytic properties of the supported gold nanoparticles. Indeed, at low temperature, high selectivity could be obtained, whereas high temperature favoured the degradation of furfural. Full conversion was observed at 150 °C (Entry 7), but only 67% of selectivity to furoic acid and a very low carbon balance, ascribed to the formation of undetected degradation products. Alternatively, for all the tests carried out in the 80–110 °C temperature range, high values of carbon balance were observed, which suggests that no degradation of furfural took place (Entries 1–6). In addition, ICP analysis of post-reactant mixtures confirmed that no Au leaching occurred. However, a low quantity of Mn²⁺ was detected in the solution, indicating low Mn²⁺ leaching (12–14 ppm). Taking into account the Mn²⁺ leaching, recycling tests were performed. Spent catalysts were also studied by TEM, as reported in the next section.

Catalyst reuse was tested on all catalysts. The results are given in

Table 3. Recycling tests. P = 12 bar (air), T = 110 °C, reaction time 2 h, furfural:Au molar ratio = 100:1.

Entry	Catalyst	XFUR [%]	SFA [%]	CB [%]
1	Au/MnO2 -NF	82	74	92
2	Au/MnO2-NW	75	64	93
3	Au/MnO2-Comm	53	37	91

.

As can be seen, no significant decrease of the activity was observed. Only in the case of the Au/MnO₂-comm sample was the decrease of furfural conversion about 20%. This could be due to the increase of the Au particle size observed in TEM after the tests (section below). In the case of the Au/MnO₂-MF and Au/MnO₂-NW samples, no changes were observed as compared to the results reported in Figure 3.

3.3. Post-Test Characterization

In order to check the mechanical and textural stability of the catalysts, TEM studies were also carried out on spent catalysts (Figure 4A–F).

As can be seen from Figure 4C–F, the structure of the Au/MnO₂-NW and Au/MnO₂-Comm samples are preserved. However, an increase in the Au particle size was observed in both cases. Specifically, the Au NPs sizes corresponded to 3.3 ± 0.9 nm and 16 ± 4 nm in diameter in the catalyst containing MnO₂ nanowires and commercial MnO₂, respectively. In the case of the Au/MnO₂-NF sample (Figure 4A,B), the structure of the support and average Au particle size were conserved. This indicates a better stability of this catalyst when compared to commercial and NW-based samples.

4. Discussion

As can be seen from the results presented above, the activity of the Au-based catalysts supported on MnO₂ strongly depends on the structure and morphology of the MnO₂ oxide used for the synthesis. It seems that it is not only the differences in surface area and pore volume that are responsible for the high activity of the MnO₂-NF catalyst. Even if, as could be seen from Table 1, the Au/MnO₂-NF material has significantly higher surface area than the MnO₂-Comm catalyst, the Au particle size did not change at all in both cases. This result differs from that observed in the literature. Indeed, Zhu et al. [31] studied different Au/MnO₂ materials in 5-HMF oxidation in an organic solvent. They observed that higher surface area was beneficial to obtain smaller Au particle sizes. However, in that case, the Au particle sizes were quite large (between 6 and 20 nm), which could explain the differences in the activity observed by the authors. In our study, all materials have similar Au particle size (about 3 nm), which suggests that only the structure of the support governs the catalytic activity. To better understand the differences, we decided to study in more detail the Mn and Au surface species present in the catalysts. X-ray photoelectron spectroscopy (XPS) is a powerful tool to study the external surface of catalysts, and is able to determine the chemical composition and oxidation states of the components present on the catalyst surface. In the case of the MnO₂ nanoflowers support, one main photoelectron peak at the Mn 2p_3/2 region centred at 642.6 eV, which can be assigned to the presence of Mn⁴⁺ species, was observed. Moreover, after the deposition of small gold nanoparticles, changes in the oxidation state of the Mn species occurred (

Table 4. Binding energies measured by XPS before and after the deposition of Au NPs at the surface of the different MnO₂ supports (OL—lattice oxygen species, OS—oxygen ions).

Sample	BE of Mn 2p3/2 (eV)	BE of O 1s (eV)		Au 4f (eV)
		OL	OS	Auδ+
Au/MnO2-NW	641.7	530.1 (46) *	532.0 (39) *	85.4 (20) *
MnO2-NW	642.6	529.5 (52) *	531.5 (34) *	no signal
Au/MnO2-comm	642.0	530.1 (56) *	532.0 (30) *	86.5 (18) *
MnO2-comm	642.7	530.0 (56) *	532.2 (29) *	no signal
Au/MnO2-NF	641.7	529.8 (41) *	531.6 (47) *	85.5 (26) *
MnO2-NF	642.6	530.0 (61) *	532.0 (28) *	no signal

* % of O or Au species.

). The main peak in the Mn 2p_3/2 region was broadened and shifted to 641.7 eV. This could indicate the partial reduction of Mn⁴⁺ to Mn^δ+ (δ < 4) at the surface. Concerning the O 1s XPS region, three different surface oxygen species could be identified. The binding energy between 529.9–529.5 eV was characteristic of the lattice oxygen (denoted as O_L), the binding energies between 532.0–531.4 eV were assigned to oxygen vacancies or the surface oxygen ions (denoted as O_s), and the binding energies around 533.9 eV were characteristic of adsorbed water. In addition, incorporation of Au NPs to the MnO₂ nanoflowers material led to a more significant decrease in the O_L/O_s ratio as compared to the pure MnO₂ nanoflowers. This demonstrates that the enrichment of oxygen vacancies or the surface oxygen ions was induced by the partial reduction of Mn⁴⁺ species during the Au NPs deposition step. At the same time, the extent of Au^δ+ species increases for the MnO2-NF sample, indicating higher numbers of gold active sites.

At the same time, the XPS Au 4f region displayed broad peaks (Figure 5C), suggesting the presence of different oxidation states of gold (Au⁰ and Au^δ+ species).

As observed in Table 4, the deposition of Au NPs on MnO₂ supports led to the formation of a significant amount of Au^δ+ species. Specifically, the Au^δ+ species ratio was ~26 % in Au/MnO₂-NF, which is a higher proportion in comparison with the other supports. This could be responsible for the enhanced catalytic activity of this catalyst. Indeed, previous works on supported Au nanoparticles has indicated surface Au^δ+ species as being the most catalytically active sites in oxidation reactions [25,32].

5. Conclusions

We have studied different Au/MnO₂ systems in the base-free oxidation of furfural to furoic acid. Small Au nanoparticles of the same size were deposited on three different MnO₂ materials, which permitted the study of the effects of the morphology and metal-support interaction on catalytic activity. The best results were obtained using a homemade nanostructured support (MnO₂-NF). This catalyst showed not only the best morphological properties (high surface area, high pore volume), but also excellent catalytic properties (high furfural conversion, optimal selectivity). The differences in the catalytic results were assigned to the presence of a significant amount of Au^δ+ species on the surface, as shown by XPS. Indeed, the Au^δ+ species present in MnO₂-NF material are indicated as being the most catalytically active sites in oxidation reactions.