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Catalysts 2013, 3(3), 656-670; doi:10.3390/catal3030656

Article
Investigation on the Stability of Supported Gold Nanoparticles
Michela Signoretto 1,*, Federica Menegazzo 1, Valentina Trevisan 1, Francesco Pinna 1, Maela Manzoli 2 and Flora Boccuzzi 2
1
Department of Molecular Sciences and Nanosystems, Ca’ Foscari University Venice, Consortium INSTM RU Ve, Dorsoduro 2137, 30123 Venice, Italy; E-Mails: fmenegaz@unive.it (F.M.); valentina.trevisan@unive.it (V.T.); pinna@unive.it (F.P.)
2
Department of Chemistry, University of Turin, NIS Centre of Excellence, P. Giuria 7, 10125 Torino, Italy; E-Mails: maela.manzoli@unito.it (M.M.); flora.boccuzzi@unito.it (F.B.)
*
Author to whom correspondence should be addressed; E-Mail: miky@unive.it; Tel.: +39-41-2348-650; Fax: +39-41-2348-917.
Received: 19 June 2013; in revised form: 1 August 2013 / Accepted: 12 August 2013 /
Published: 21 August 2013

Abstract

: The procedures leading to the preservation of catalytic performances of Au/ZrO2 samples have been investigated. The three potential causes of deactivation, namely the particle growth by sintering of gold nanoparticles, the metal leaching and the formation of un-reactive species which inhibit the reaction, have been evaluated. In particular, this paper deals with the stability of gold nanoparticles: (1) under storage conditions; (2) with time on stream for a gas phase reaction (LT-WGSR); (3) with time on stream for a liquid phase reaction (furfural oxidative esterification).
Keywords:
gold nanoparticles; stability; sulfated zirconia; FTIR spectroscopy; LT-WGS reaction; oxidative esterification; furfural

1. Introduction

The good catalytic activity displayed by highly dispersed gold in many reactions was not expected, considering that gold is the most noble of all metals and it is the least reactive metal towards atoms or molecules at the interface with gases or liquids. The surprise was enormous when Professor Haruta and co-workers discovered in the late 80s [1] that suitable prepared gold supported on a metal oxide showed high activity in the CO oxidation reaction at temperatures as low as 200 K. This discovery initiated extensive activity in both applied and fundamental research concerning gold. The range of reactions catalyzed by gold as well as the suitability of different support materials and the influence of the preparation conditions were widely explored and optimized in applied research [2]. Gold catalysts appeared to be very different from the other noble metal-based catalysts, due to their marked dependence on the preparation method which is crucial for the genesis of the catalytic activity. A very general phenomenon related to gold samples is the extreme dependence of the catalytic activity on the size of the Au particles, which also implies that sintering is very crucial for the long-term stability of the catalysts. These features make Au very different from classical catalysts based on transition metals such as Pt or Pd, which are also active as larger particles and even as macroscopic single crystals. The achievement of a small particles size is not always an easy task, because of the low melting point of gold (1336 K, as compared to 1823 K for Pd and 2042 K for Pt). Another relevant aspect that must be considered, looking at the application of gold catalysts, is that both activity and stability of these systems strongly depend on the structure of the support as well as on the specific interaction between the gold and the support, giving rise to a synergistic effect.

We present here an investigation of a series of gold-based catalysts over zirconia and sulfated zirconia. In particular, we have focused our attention to procedures leading to the preservation of their catalytic performances. Significantly, one of the main drawbacks in the industrial exploitation of a catalyst lies in a poor stability; for commercial usage the catalysts need to be stable and should not deteriorate with the elapse of time and with use. The principal causes of catalyst deactivation are well recognized and include:

1.1. Metal Sintering

A first reason for the decrease of catalytic performances can be associated with the sintering of gold clusters during reaction. In fact, an opportune gold dispersion is the key factor which determines the high performances of Au-based catalysts. We have shown [3,4] that CO chemisorption by a pulse flow technique and Fourier transform infrared (FTIR) measurements of adsorbed CO in well-defined and controlled conditions of temperature and pressure can be taken as effective methods for the quantitative determination of the gold active sites. Therefore, we have investigated metal sintering by HRTEM, CO chemisorption and FTIR analyses.

1.2. Metal Leaching

Working in solvent medium, metal leaching cannot, in principle, be excluded and the heterogeneity of the catalytic reaction may always be questionable. Therefore, we have investigated gold leaching through chemical analysis by atomic absorption of the disintegrated exhausted samples of a liquid phase reaction.

1.3. Fouling of the Active Sites

For poisoning we mean any deactivation mechanism involving prevention of reactants from reaching the active sites. From a practical point of view, the reason for catalyst deactivation is due to the blocking of gold active sites by deposition of poisons; the reaction inhibition by the reaction substrate, products or by-products; or even to deposition of polymeric material as a result of side or consecutive reactions. In our work, in order to verify the presence of carbon-based residues, the exhausted catalysts were subjected to temperature programmed oxidations (TPO) and FTIR analyses of adsorbed CO.

2. Results and Discussion

2.1. Features of Gold Supported on Zirconia and Sulfated Zirconia

Zirconia and sulfated zirconia [5] were used as supports for gold-based catalysts. We choose zirconia because it is of particular interest in a large field of applications, as it possesses desirable characteristics such as tunable surface acidity/basicity, redox properties, porosity, and surface area. In particular, sulfating zirconia causes not only modifications of the acid properties, but also affects surface features: sulfates retard crystallization, stabilize the tetragonal phase, improve surface area and pores size [6]. Au/ZrO2 materials are of significant interest as catalysts for CO oxidation [7], butadiene hydrogenation [8], epoxidation of styrene [9], low-temperature water–gas shift (LT-WGS) reaction [10,11,12]. Supports and gold samples were analyzed by physisorption analyses and ion exchange chromatography, and the results are reported in Table 1. As already known, the effect of sulfate addition on zirconium oxide is to increase its surface area and reduce the mean pore size, shifting crystallization processes towards higher temperatures during calcination treatment [13]. Surface area and porosity are very similar for the supports and the corresponding catalysts, proving that they are not modified by the gold DP technique.

As regards the amount of sulfates on the supports, it is due to the maximum value of anions that the oxide can keep under the calcination conditions [14]. In fact, it is known that the elimination of sulfates occurs during the calcination step, and that the SO42− amount that remains at the end of this process is strictly connected with both the initial charged SO42− amount and the calcination conditions. Conversely, the final catalysts no longer contain sulfates [15,16]. This is not unexpected, since the methodology of gold DP on the support has been carried out at a basic pH, and the detachment of sulfate groups has occurred. Such SO42− dissolution had been previously demonstrated by quantitative IC analyses [17].

However, we have previously demonstrated [16] that sulfate addition to zirconia means a twofold advantage: (i) higher surface area; (ii) higher gold dispersion due to the positive role of SO4= groups that address the deposition of Au in the form of highly dispersed clusters in close contact with the support.

Table Table 1. Textural properties of the supports.

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Table 1. Textural properties of the supports.
SampleNominal SO42− (wt%)Found SO42− (wt%)Surface area (m2/g)Pore diameter (nm)
Z004021
SZ111.07911
SZ222.0938.9
SZ443.61157.0
SZ884.01196.7

2.2. Stability of the Catalysts under Storage Conditions

Conditions of storage are critical for gold-based catalysts, as has been already discussed [18,19,20,21]. Two predominant effects have been identified: (i) the effect of light, which during storage as well as during synthesis can cause photodecomposition of cationic gold to Au0; (ii) the effect of temperature, which can cause a slow aggregation of precursor species, giving large particles of Au0 when reduction occurs. Therefore it is well known that storage in the dark and in a refrigerator is recommended for gold-based samples. In our work we have always used these devices. We have furthermore investigated the effect of calcination on stability under storage condition. HRTEM analysis was performed on both calcined at 453 K and not calcined 1AuSZ2 samples, as reported in Figure 1a,b, by collecting a representative total number of images (45 and 46 images, respectively) in order to describe accurately the morphology of the samples. More precisely, the measurements revealed that, due to the very high dispersion, Au particles were not easily recognized, especially in the case of non-calcined 1AuSZ2. However, small roundish gold nanoparticles, whose presence is highlighted by red harrows in Figure 1, have been observed in both cases and, quite interestingly, these particles are stable under the electron beam maintaining a high dispersion during the whole measurement on both samples. As shown in Figure 1c, the particle size distribution obtained for calcined 1AuSZ2 is narrower than that of the not calcined sample, despite a similar mean gold particle size (1.3 nm and 1.4 nm, respectively), pointing out an effect of the calcination pretreatment on gold dispersion after four months.

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Figure 1. HRTEM representative images of calcined (a) and not calcined (b) 1AuSZ2 sample. Gold particles size distribution (c) obtained by HRTEM measurements performed on calcined (grey histogram) and not calcined (red histogram) 1AuSZ2 sample after 4 months. Both images have been taken at an original instrumental magnification of 400,000×.

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Figure 1. HRTEM representative images of calcined (a) and not calcined (b) 1AuSZ2 sample. Gold particles size distribution (c) obtained by HRTEM measurements performed on calcined (grey histogram) and not calcined (red histogram) 1AuSZ2 sample after 4 months. Both images have been taken at an original instrumental magnification of 400,000×.
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However, the presence of gold species even more dispersed that escape from HRTEM detection has been demonstrated by CO chemisorption (Figure 2a). The results of the as-soon-as-prepared samples indicate that calcination leads to a small decrease of metal surface area. This is reasonably compatible with the heat treatment. However, an opposite trend is observed after four months: in fact the calcined catalyst preserves a higher dispersion than the not calcined one. This is rationally due to the exceptional gold dispersion of the not calcined sample, which leads to an outstanding gold mobility. On the contrary, calcination induces a stronger interaction among the gold nanoparticles and the zirconia support, therefore arresting gold mobility. Hence, the calcination procedure guarantees the stabilization of gold nanoparticles.

Moreover, these data have been compared with those deriving from the activity in the LT-WGS reaction. The WGS reaction:

CO + H2O = CO2 + H2  ∆H 0298= −41 kJ/mol, ∆G0298 = −28.6 kJ/mol
is one of the oldest catalytic processes employed in the chemical industry, since it provides an economical route to hydrogen production. It usually proceeds in two distinct steps with two types of catalyst: a high temperature (HT) stage over an iron oxide promoted with chromium oxide catalyst, and a low temperature (LT) stage, on a catalyst composed of copper, zinc oxide, and alumina. Recently, there has been a renewed interest in this reaction because it is one of the key steps in important applications such as pure H2 production for fuel-cell power systems and in the automobile exhaust processes, since the hydrogen produced is a very effective reductant for NOx removal. However, in these applications heterogeneous catalysts with high activity as well as good structural stability in air and in cyclic operation are required, but this target is not met by the commercially available LT-WGS catalysts. The catalysis of this reaction by gold nanoparticles supported over metal oxides has been the subject of numerous investigations [22,23]. Recently, it has been found that zirconia [10] and sulfated zirconia [11] are very efficient supports of gold-based catalyst for the LT-WGS reaction.

As reported in Figure 2b, it is evident that the calcination led to an enhancement of the stability of catalytic activity, and there is a good correlation between chemisorption and conversion data. These results put in evidence that the calcination procedure allowed the stabilization of highly dispersed gold, possibly by a strong interaction between the gold species and the zirconia support, blocking gold mobility on the support and therefore allowing the preservation of very high metal dispersion. As a consequence, the catalytic performances decrease to a lesser extent. In conclusion, for optimal storage conditions, particular attention must be paid to avoid the exposition to the solar light and to keep the samples already calcined at a proper temperature in the refrigerator.

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Figure 2. Trends of chemisorption (a) and conversion in LT-WGS reaction; (b) for 1AuSZ2 catalyst.

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Figure 2. Trends of chemisorption (a) and conversion in LT-WGS reaction; (b) for 1AuSZ2 catalyst.
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2.3. Stability of the Catalysts with Time on Stream in a Gas Phase Reaction (LT-WGSR)

In this paragraph, we will discuss the stability of gold nanoparticles with time on stream for a gas phase reaction, i.e., the LT-WGS reaction. We have previously demonstrated [4] that the CO molecule is adsorbed on the very small clusters on Au supported over zirconia, in intimate contact with the oxide. On these surface sites, a close contact between the activated water and the CO probe can be realized. Moreover, we have found [15] that the catalyst prepared on sulfated zirconia is more stable than that supported on plain zirconia under LT-WGSR conditions. On sulfated zirconia, gold sintering is inhibited in some extent as a consequence of the surface structural disorder left after sulfate removal, allowing a lower mobility of gold atoms on the zirconia surface [15]. As discussed and illustrated in [16], an active role of sulfates is played during the gold deposition, producing highly dispersed gold species grafted to zirconia. Afterwards, we investigated the effect of both gold and sulfates on the catalytic performances. Conversions are reported in Figure 3, while Table 2 reports catalytic results normalized for the dispersion data.

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Figure 3. Conversion obtained for the LT-WGS reaction at 453 K for the 1 wt%Au (a) and 3 wt% Au (b).

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Figure 3. Conversion obtained for the LT-WGS reaction at 453 K for the 1 wt%Au (a) and 3 wt% Au (b).
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Table Table 2. Catalytic performances after 24 h.

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Table 2. Catalytic performances after 24 h.
Sample103 * Converted molCO/h chemisorption data *Sample103 * Converted molCO/h chemisorption data *
1AuSZ1153AuSZ116
1AuSZ2163AuSZ219
1AuSZ4143AuSZ418
1AuSZ8153AuSZ817

* Chemisorption data = chemisorbed molCO/mol Au.

Firstly, an effect of the gold loading is evident if contrasting the results coming from the samples with 1 wt% to those containing 3 wt% Au: an increase of the quantity of the active species implies an increase of the catalytic activity. However, the expected increase of catalytic performance by enhancing the gold loading from 1 wt% up to 3 wt% Au does not occur and the activity observed on the two series of samples is comparable. This apparently contradictory result is due to the fact that in our experimental conditions it was not possible to maintain the same gold dispersion by increasing the gold loading. In fact, some Au agglomeration occurs when increasing the Au content, as demonstrated by the particle size distributions of the fresh samples reported in Figure 4 that will be discussed later on.

Both catalysts supported on SZ1 perform worst, indicating that a 1 wt% amount of sulfates is not enough to keep the gold active phase dispersed and it negatively affects catalytic performances. In regards to stability, the curves referring to catalysts with 1 wt% Au denote a very similar profile: the conversion decrease is more noticeable during the first 24 h, while at a later stage the profiles tend to get flat. SZ2 results to have an adequate amount of sulfates to achieve good catalytic results for the 1 wt% Au catalysts.

The curves related to the samples with 3 wt% Au follow a similar trend than those of samples containing 1 wt%, but the conversion values for 3AuSZ4 and 3AuSZ8 are almost coincident and higher than 3AuSZ2. For the 3 wt% Au samples a further increase in the sulfates amount (from 4 wt% to 8 wt%) has no evident effect on the activity and stability of the catalysts.

Moreover, it is interesting to note that for the 3 wt% Au catalysts, the loss of activity in 72 h is substantially smaller than for the series with 1 wt% Au, indicating that 3 wt% Au > 1 wt% Au, as for gold stability, too.

This feature can be related to the lower gold sintering observed in the samples with the higher percentage of Au, as confirmed by comparing the particles size distributions of the fresh (grey histograms) and used (blue histograms) 1AuSZ2 and 3AuSZ2 samples reported in section a and b of Figure 4. Gold particles with diameter >2 nm are present after reaction in the distribution of 1AuSZ2 (blue histogram), whilst the particle size distribution of the gold particles present on the 3AuSZ2 is slightly shifted towards higher sizes after reaction, and the average size is almost identical before and after the catalytic tests. On the other hand, the distribution of the used 3AuSZ4 catalyst (blue histogram in Figure 4c) is fixed in the same range of sizes of the distribution related to the fresh sample. In agreement with the trends displayed by the 3 wt % catalysts and shown in Figure 3, gold nanoparticles present on 3AuSZ4 seem more stable than those on 3AuSZ2, indicating that the sulfate amount has to be modulated depending on the Au content to obtain samples with the optimal metal dispersion.

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Figure 4. Gold particle size distributions of 1AuSZ2 (a); 3AuSZ2 (b) and 3AuSZ4 (c) fresh (grey histograms) and used (blue histograms) catalysts.

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Figure 4. Gold particle size distributions of 1AuSZ2 (a); 3AuSZ2 (b) and 3AuSZ4 (c) fresh (grey histograms) and used (blue histograms) catalysts.
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Figure 5. FTIR difference spectra of CO adsorbed at 157 K on fresh (grey curves) and used (blue curves) 3AuSZ2 (a) and 3AuSZ4 (b) catalysts precovered previously by water.

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Figure 5. FTIR difference spectra of CO adsorbed at 157 K on fresh (grey curves) and used (blue curves) 3AuSZ2 (a) and 3AuSZ4 (b) catalysts precovered previously by water.
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In order to investigate more deeply this point, FTIR spectroscopic measurements of adsorbed CO have been carried out at low temperature either on the fresh samples or on the used ones (Figure 5). In fact, all gold exposed sites, also the highly dispersed ones thatescape from the HRTEM detection, can be monitored by employing this technique.

An intense band centered at 2,094 cm−1 whose position is close to that typically observed for metallic Au nanoparticles, but broader and more symmetrical in shape, is present on both samples (sections a and b, grey curves). Looking at the behavior observed during outgassing at 157 K and/or upon heating at r.t., as well as at the different absorption coefficient, 1.8 cm−1 mol−1 (×104) vs. 3.2 cm−1 mol−1 (×104) determined for Au nanoparticles, this band is due to the presence of mutually interacting Au corner sites exposed at the surface of non metallic neutral clusters [15,24]. In these clusters a large fraction of the gold atoms is uncoordinated and exposed at the surface, where almost all Au atoms are in corner or interface positions.

After use, the band at 2094 cm−1 displays a less symmetric shape (Figure 5a,b, blue curves). In particular, the component at about 2115 cm−1 is almost totally depleted, indicating that a partial sintering process occurred during reaction.

Sintering is well evident on 3AuSZ2, in fact the CO band related to the used sample is less intense than that associated to the fresh one. On the contrary, the highly dispersed gold clusters present on 3AuSZ4 undergo only minor sintering, as demonstrated by the small change in shape of the band as well as by the fact that it has the same intensity if compared to the band related to the fresh sample. These data are in agreement with HRTEM findings and further confirm our hypotheses on the effect of an opportune sulfate amount ruling the gold dispersion and stability.

2.4. Stability of the Catalysts with Time on Stream in a Liquid Phase Reaction (Furfural Oxidative Esterification)

The stability with time on stream for a liquid phase reaction, i.e., the furfural oxidative esterification to methyl furoate, will be discussed in this section. In Scheme 1 is reported the reaction of the furfural oxidative esterification to methyl furoate.

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Scheme 1. Furfural oxidative esterification to methyl furoate.

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Scheme 1. Furfural oxidative esterification to methyl furoate.
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The catalytic tests have been performed at 393 K in methanol under pressure and stirring at 1000 rpm for many hours. Very recently, we have found [25,26] good catalytic performances of highly dispersed Au/ZrO2 samples, due to the presence of highly dispersed Au clusters able to produce atomic oxygen by reaction with the oxygen molecule. Unfortunately the catalysts, after the first catalytic run, filtration and washing in methanol, did not restore starting performances [26]: selectivity collapses from 98% to 29%. Firstly, we investigated if gold leaching occurred during tests in the liquid phase. In fact, metal leaching can never be excluded for a reaction working in solvent medium for many hours. Exhausted samples were disaggregated and chemical analysis by atomic absorption of gold was carried out. Catalysts that have been discharged after three hours of reaction in methanol and stirred at 1000 rpm have shown the same Au content of the as-prepared samples (1.5 wt% vs. 1.5 wt%).

Another reason for the selectivity decrease of Au/ZrO2 catalysts can be associated with the sintering of gold clusters during the reaction [26]. Therefore, the increase in size of the Au nanoparticles was investigated by HRTEM. The mean Au particle size is the same before and after the catalytic test (2.8 nm vs. 2.7 nm). From these findings, gold sintering problems throughout the reaction time can be excluded. This is plausible, as we have previously shown that calcination at a proper temperature results in stable gold nanoparticles. Moreover, the reaction was performed at only 393 K, a temperature which is quite lower than the calcination temperature (773 K).

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Figure 6. TPO of the 1.5AuSZ2 sample after reaction.

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Figure 6. TPO of the 1.5AuSZ2 sample after reaction.
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After ruling out both Au leaching and sintering, we investigated fouling of the active sites [26]. In order to verify the presence of any carbon-based residues, the catalysts were subjected to temperature programmed oxidation (TPO). The profile of the as-prepared catalyst does not present CO2 evolution, indicating the absence of organic residues in the material. On the contrary, as shown in Figure 6, the TPO profile of the sample after reaction, presents one broad band due to CO2 evolution.

Therefore, the catalyst has been reoxidated at 723 K in order to completely remove the carbon residue. Moreover, the TPO profile of the reoxidated sample is flat, meaning the complete elimination of carbon species on the material.

Hence, we further performed catalytic reaction on the reoxidized catalyst. As reported in Figure 7, it is possible to restore the initial conversion and almost fully the selectivity [26].

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Figure 7. Comparison of activity data of the 1.5AuSZ2 sample.

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Figure 7. Comparison of activity data of the 1.5AuSZ2 sample.
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3. Experimental Section

3.1. Catalysts’ Preparation

The supports were prepared by precipitation from ZrOCl2 8H2O (Fluka) at constant pH (pH = 8.6), aged under reflux conditions for 20 h [27,28], washed free from chloride (AgNO3 test) and dried at 383 K overnight. Part of the Zr(OH)4 was sulfated with (NH4)2SO4 (Merck, Padua, Italy) by incipient wetness impregnation (1,2,4,8 wt% SO4=/ZrO2). Then un-sulfated (Z) and sulfated (SZ1, SZ2, SZ4, SZ8) supports were heated (90 K/h) up to 923 K in flowing air (50 mL/min STP) and kept at this temperature for 6 h, followed by slow cooling to room temperature.

Gold was deposited on the calcined supports by deposition precipitation at pH = 8.6 using a NaOH aqueous solution (0.5 M) (Riedel-de Haen, Padua, Italy). A proper amount of HAuCl4 aqueous solutions was used in order to give different nominal Au contents. After filtration, the catalysts were dried at 308 K for 15 h. Part of the materials was finally calcined in air for 1 h at different temperatures (453 or 773 K). The samples will be hereafter denoted as XAuZY or XAuSZY, where X represents the Au wt% loading, and Y the amount of sulfates.

Oxidative treatments of the exhausted catalysts were carried out for 1 h at 723 K in a 5% O2/He flow (40 mL/min).

3.2. Methods

Surface area and pore size distribution were obtained from N2 adsorption/desorption isotherm at 77 K (using a Micromeritics ASAP 2000 Analyser, (Milan, Italy). Calcined samples (400 mg) were pretreated at 573 K for 2 h under vacuum, while non-calcined samples (300 mg) were pretreated at 298 K for 6 h under vacuum. Surface area was calculated from the N2 adsorption isotherm by the BET equation, and the pore size distribution was determined by the BJH method also applied on the adsorption branch [29]. Total pore volume was taken at p/p0 = 0.99.

The amount of sulfate was determined by ion chromatography (IEC) after dissolution of the materials [17]. Sulfate concentration was calculated as the average of two independent sample analyses, and each analysis included two chromatographic determinations.

The gold amount was determined by atomic adsorption spectroscopy. Dried samples (typically 100 mg) were dispersed in water acidified with HF and aqua regia and disgregated by microwaves.

CO pulse chemisorption measurements were performed at 157 K with a previously reported procedure [30]. Before chemisorption the following pretreatment was applied: the sample (200 mg) was reduced in H2 flow (40 mL/min) at 423 K for 60 min, cooled in H2 to ambient temperature, purged in He flow and finally hydrated at ambient temperature. The hydration treatment was performed by contacting the sample with a He flow (10 mL/min) saturated with water. The sample was then cooled in He flow to the temperature chosen for CO chemisorption (157 K).

HRTEM analysis was performed on all catalysts using a Jeol 3010 EX electron microscope (300 kV, Milan, Italy) equipped with a side entry stage and a LaB6 filament. The powdered samples were deposited on a copper grid, coated with a porous carbon film. All digital micrographs were acquired by an Ultrascan 1000 camera and the images were processed by Gatan digital micrograph. A statistically representative number of gold particles was counted in order to obtain the particle size distribution.

FTIR spectra were taken on a Perkin–Elmer 1760 spectrometer (equipped with a MCT detector, Milan, Italy) with the samples in self-supporting pellets introduced in a cell allowing thermal treatments in controlled atmospheres and spectrum scanning at controlled temperatures (from 120 to 300 K). From each spectrum, the spectrum of the sample before the inlet of CO was subtracted. The spectra were normalized with respect to the gold content of each pellet. The pretreatment of the samples was: (i) reduction in H2 at 423 K; (ii) cooling in H2 to room temperature (r.t.) outgassing at the same temperature; and (iii) hydration at room temperature.

TPO measurements were carried out in lab-made equipment: samples (100 mg) were heated with a temperature rate of 10 K/min from 298 K to 873 K in a 5% O2/He flow (40 mL/min). The effluent gases were analyzed by a TCD detector and by a Genesys 422 quadrupole mass analyzer (QMS).

3.3. Catalytic Activity Measurement

WGSR was performed in a fixed-bed flow reactor at atmospheric pressure and in the temperature range from 453 to 423 K. The following conditions were applied: space velocity = 9400 h−1; catalyst volume = 0.5 cm3 (35–50 mesh) diluted to 1.5 cm3 with quartz sand (Carlo Erba; 35–50 mesh); the feed mixture contained 1.9% vol. CO, 39.7% vol. H2, 9.5% vol. CO2, 11.4% vol. N2, 37.5% vol. H2O. Samples were previously subjected to a slow (50 K/h) thermal activation in nitrogen (50 mL/min) up to 453 K and kept at this temperature for 17 h in the same N2 flow. The progress of the reaction was followed by gas–chromatographic analysis of the converted mixture at the reactor outlet.

Furfural oxidative esterification with oxygen and methanol was investigated at 393 K, without NaCH3O addition, using a mechanical stirred autoclave fitted with an external jacket. Catalyst (100 mg), furfural (300 μL) and n-octane (150 μL), used as internal standard, were added to the solvent (150 mL of methanol). The reactor was charged with oxygen (6 bar) and stirred at 1000 rpm. The progress of the reaction was determined after 3 h by gas–chromatographic analysis of the converted mixture (capillary column HP-5, FID detector). Preliminary experiments showed that the system works in a strictly kinetic regime.

4. Conclusions

If gold-based catalysts are ever to find commercial applications on a large scale, their long-term stability must be improved. Au/ZrO2 samples are active and selective, and this is due to the presence of highly dispersed Au clusters, that are able, for example, to produce atomic oxygen by reaction with O2. However, the performances of these catalysts must be maintained for longer periods of time.

Gold sintering is inhibited to some extent on sulfated zirconia as a consequence of the surface structural disorder left after sulfate removal during gold deposition, allowing a lower mobility of gold clusters grafted on the zirconia surface. In fact, even if sulfates are not present in the final catalyst, they act in the synthesis step, increasing both surface area and gold dispersion.

However, the sulfates amount has to be modulated depending on the Au content to obtain samples with the optimal metal dispersion. As a consequence, an opportune sulfates amount rules both gold dispersion and stability.

Moreover, we have shown that the calcination pretreatment is an essential procedure to be followed for improving stability of Au/ZrO2 samples. Calcination causes stronger interaction between gold and zirconia, blocks gold mobility on the support and therefore allows the preserving of very high dispersion. Therefore, storage conditions must provide the appropriate levels of dark and refrigeration, and storing samples already calcined at a proper temperature. Calcination is essential also for liquid phase reactions. In fact, it allows gold stability in regard to both leaching and sintering. In this case, gold stability is involved by its tendency to adsorb organic species in the reaction ambient. However, we have shown that deactivation is reversible and after heating in oxygen atmosphere at a proper temperature, the catalyst surface is cleaned by evolution of carbon dioxide, and it is possible to fully recover the initial performances.

Acknowledgments

We thank Tania Fantinel for technical assistance.

Conflicts of Interest

The authors declare no conflict of interest.

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