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Catalysts 2017, 7(9), 255; doi:10.3390/catal7090255

Article
Continuous-Flow Monolithic Silica Microreactors with Arenesulphonic Acid Groups: Structure–Catalytic Activity Relationships
Agnieszka Ciemięga 1, Katarzyna Maresz 1, Janusz J. Malinowski 1 and Julita Mrowiec-Białoń 1,2,*
1
Institute of Chemical Engineering Polish Academy of Sciences, Bałtycka 5, 44-100 Gliwice, Poland
2
Department of Chemical Engineering and Process Design, Silesian University of Technology, Ks. M. Strzody 7, 44-100 Gliwice, Poland
*
Correspondence: Tel.: +48-32-231-08-11
Academic Editors: Tian-Yi Ma, Jian-Rong (Jeff) Li and Cláudia Gomes Silva
Received: 11 July 2017 / Accepted: 28 August 2017 / Published: 30 August 2017

Abstract

:
The performance of monolithic silica microreactors activated with sulphonic acid groups and a packed bed reactor with Amberlyst 15 resin were compared in the esterification of acetic acid with n-butanol. The monolithic microreactors were made of single silica rods with complex pore architecture, differing in the size of mesopores, and in particular, flow-through macropores which significantly affected the flow characteristic of the continuous system. The highest ester productivity of 105.2 mol·molH+−1·h−1 was achieved in microreactor M1 with the largest porosity, characterized by a total pore volume of 4 cm3·g−1, mesopores with 20 nm diameter, and large flow-through macropores 30–50 μm in size. The strong impact of the permeability of the monoliths on a reaction kinetics was shown.
Keywords:
silica monoliths; continuous-flow microreactors; acid centres; structure/catalytic activity relationships

1. Introduction

Synthesis of most fine and specialty chemical—particularly pharmaceuticals—is typically carried out in a liquid phase and batch operation, despite the fact that batch processes cause a number of problems, especially with scaling up and producing within homogeneous processing conditions [1]. Flow reactors have many advantages over batch reactors: continuous production, better process control, easier automation, and reduced operation costs. Moreover, continuous-flow heterogeneous catalytic processes offer higher selectivity, productivity, and elimination of costly catalyst separation from the reaction media [2,3]. The application of reactors involving solid catalysts in the form of either stationary or moving particles often leads to serious operational problems associated with mass and heat transfer limitations, excessive backpressure, thermal instabilities in stationary beds, etc. [4]. The replacement of a continuous flow reactor by monolithic microreactor-based technology appeared to be promising for the effective production of fine chemicals.
Continuous microreactors allow a miniaturization of the apparatus, which is of particular importance in fine chemical synthesis, and in the pharmaceutical and chemical industries [2]. A high surface to volume ratio of the rectors enables high concentrations of active sites per unit volume and provides better heat and mass transfer. Furthermore, precise control of the reaction temperature and residence time has a beneficial effect on the productivity and selectivity.
Microreactors can be made from a wide range of materials, and a variety of fabrication techniques have been proposed [5,6], often requiring special equipment and skills. Continuous-flow monolithic polymeric microreactors which have a well-defined system of flow-through pores show important advantages over packed bed reactors [7,8,9], but suffer from low thermal stability and a tendency to swell. More recently, however, it was shown [8] that highly cross-linked polymer monoliths do not suffer from the latter effects. In recent years, among the various types of microreactor, much attention has been paid to the reactors with reactive cores made of inorganic carriers—especially of monolithic silica. The silica-based microreactors were first proposed by the Montpellier group, and were made from a single monolith (MonoSil), the surface of which was functionalized with -NH2 or -HSO3 groups. Innovation of this approach stems from a unique hierarchical pore structure of the monolith in which flow-through macropores are connected to an extensive network of meso- and micropores present in the silica skeleton [10,11]. Owing to the unique hierarchical pore structure, the flow resistance could be reduced, permeability increased, and the accessibility of substrates to catalytic sites improved, giving an overall better performance compared to packed column [12]. The silica monoliths with hierarchical porosity were obtained by combining the phase separation method elaborated by Nakanishi [13,14] with pseudomorphic synthesis [15,16], to ensure an ordered mesoporous morphology of materials.
Hierarchically structuring both the porosity and the architecture of a material over a different length scale provides an opportunity to synthesize materials suitable for different applications, including catalysis and separation [17,18]. Recently, the synthesis strategies and catalytic performances exhibited by the hierarchically porous catalysts have been thoroughly reviewed [18].
Silica-based materials are extensively used in heterogeneous catalysis as an active site support due to the abundance of surface silanols, which allows the grafting of a wide variety of active species to meet specific catalytic demands [19] posed for the synthesis of fine chemicals [10]. Consequently, silica monoliths have been activated with organic groups [11,20], enzymes [21,22], or metal complexes [23], and successfully applied as active cores of continuous-flow microreactors.
In this work, we compare the performance of continuous-flow reactors fabricated using silica monoliths featuring different pore structure with that of the packed bed reactor filled with Amberlyst 15 resin. The reactors were tested in the esterification of acetic acid with n-butanol. The n-butyl acetate is the product of the model reaction which is of practical interest, being used as a solvent in the manufacturing of lacquer, artificial perfume, plastics, and safety glass, and also as a synthetic fruit flavouring in foods [24]. The silica monoliths were synthesized using four synthesis protocols to obtain carriers with significantly different structural parameters on both the meso- and macroscale. Subsequently, monoliths were functionalized with arenesulphonic acid groups in order to obtain monolithic microreactors with Brönsted acid centres. A strong impact of the macroporous structure on the flow characteristic of the microreactors was found, while the amount of anchored active groups correlated well with mesostructural properties (i.e., significant increase was recorded with increasing values of specific surface area). However, the structure of monoliths at macroscale decisively influenced the overall performance of the microreactors. The highest productivity was achieved in the monolith with the largest porosity, and not the largest surface area, which also offered the lowest pressure drop. The latter finding is also of major practical importance, and correlates very well with the observation most recently reported in [25].

2. Results

2.1. Characterization of the Silica Monoliths

Three silica monoliths designated as M1, M2, and M3 were fabricated using different synthesis protocols (see the Materials and Methods, Table 5). The monolith structure—in both the meso- and macropore scales—strongly depended on the composition of the reaction mixture and the synthesis process parameters thereof. The scanning electron microscopy images of the monoliths are displayed in Figure 1.
The images confirmed the presence of the bi-continuous, foam-like structure of the macropores in the monoliths. The characterization of the materials by low-temperature nitrogen adsorption and mercury porosimetry (Figure 2) revealed pore system architecture in different size scales. Structural properties of the materials are summarized in Table 1.
Monolith M1 synthesized in the presence of surfactant and hydrothermally treated in ammonia solution at 90 °C featured bimodal mesopore structure (small mesopores with diameters of 2–4 nm and larger ones in the size of 10–35 nm) and large macropores with diameters in the range of 30–50 μm. The bimodal mesopore structure originated from the presence of a micelle-forming surfactant. Monolith M2 hydrothermally treated in ammonia solution at 80 °C had a uniform mesopore structure in the range of 10–20 nm and macropores with diameters ca. 5 μm. As reported earlier [26,27], the size of the macropores decreased with the increase in the value of polyethylene glycol (PEG)/Si ratio (Table 1, Figure 2). In turn, the use of a higher concentration of nitric acid in the synthesis of monolith (sample M3) resulted in the formation of smaller macropores with a small effect on the volume of the macropores. This phenomenon was interpreted as an effect of a faster hydrolysis and slower condensation of siliceous species in acidic conditions [28]. The pore structure in the nanometer range was tailored by a post-gelation treatment of the silica monoliths in ammonia solution, as well as an application of a cationic surfactant. The total pore volume (VT) of the monoliths was very large (in the range of 3–4 cm3·g−1), while the mesopore volume (Vpmes) was comparable (ca. 1.1 cm3·g−1). Monolith M3 was characterized by the largest specific surface area (575 m2·g−1), which is associated with the presence of small mesopores. Monoliths M1 and M2 also differed in the structure of the silica skeleton. Monolith M2 was characterized by a uniform wall thickness (about 5 μm), while in monolith M1 there were visible structural elements of different thicknesses ranging from a few to tens of micrometers. Ion-exchange resin Amberlyst 15 exhibited large mesopores (cf. inset to Figure 2) of volume ca. 0.3 cm3·g−1 (i.e., four times smaller than in the synthesized monoliths).
Thermal stability of the catalyst is of primary importance—particularly when it contains organic groups. The thermal stability of arenesulphonic acid groups attached to the monoliths’ surface and their amount were determined by thermogravimetric method. The results are shown in Figure 3 and in Table 1. All samples were stable up to 350 °C. The sharp weight loss below 120 °C corresponds to physisorbed water. The amount of incorporated acidic groups was calculated from mass loss in the range of 300–700 °C, resulting from thermal decomposition of functional groups. A strong relationship between specific surface area of silica skeleton and chemically bonded acidic groups was observed. Monolith M3 with the largest specific surface area had the highest amount of anchored acidic groups (Table 1), which correlates very well with the content of hydroxyls employed to attach functional groups [29].
The identification of acid sites and their strength were studied using pyridine (Py) adsorption combined with Fourier transform infrared (FTIR) studies. The spectra recorded before and after the adsorption and desorption at different temperatures for M1 are depicted in Figure 4. The bands at 1488, 1542, and 1634 cm−1 derive from pyridinium ions bonded to Brönsted acid sites (BAS). The fact that the characteristic bands still remained after evacuation at 150 °C and 200 °C confirmed the presence of strong BAS. The band at 1443 cm−1—visible after adsorption—disappeared at 150 °C, and it corresponds to hydrogen-bonded pyridine. The relative acid strength was calculated based on the intensity of the adsorption band centered at 1542 cm−1. The ratio of the integrated area of the peaks obtained at 200 °C and 150 °C represents the fraction of acid sites still containing chemisorbed Py after evaluation at these temperatures and reduced pressure. The data in Table 1 confirmed that strength of BAS is comparable for all the samples. The value of A200/A150 nearly close to unity is characteristic of strong acid sites [30,31].
The relationship between the pressure drop and the flow rate is of practical significance, providing additional knowledge which is useful in assessing process economics. Thus, the pressure drop was measured for all monolithic microreactors and the packed bed reactor equipped with the Amberlyst 15 resin. It was found that it strongly depended on the size of the flow-through macropores, and a significant increase in pressure was recorded in the order M1 << M2 < M3 (Figure 5), which correlates very well with the decreasing pore size. The reduction in the size of the flow-through macropores (from ca. 50 μm to 1 μm) resulted in the increase in pressure drop of a few orders of magnitude. In the packed bed reactor, the pressure drop was twice as large as that recorded in the M1 microreactor.
The permeability of the monoliths and the packed bed reactor (Amberlyst) was calculated using Darcy equation [25], and the results obtained are shown in Table 2. The permeability coefficient was three orders of magnitude lower in M3 than in M1, in perfect agreement with the smaller size of macropores in that material.

2.2. Catalytic Performance

The performance of continuous-flow monolithic microreactors and the packed bed reactor with Amberlyst 15 resin was compared in the esterification of acetic acid with n-butanol. Catalytic tests were performed for at least 6 h, at a flow rate of 0.06 cm3·min−1 (representative graph for M1-A is shown in Figure 6). The flow rate was selected to achieve conversion smaller than 50% to discriminate efficacy of different structure.
One of the key factors in continuous flow reactors’ performance is the residence time (τ) of a reactant molecule in the active zone. According to Sachse et al. [32], for the monolithic reactor τ may be determined from the following expression:
τ = xmVT/F,
where x is monolith length, m is a weight per cm (g·cm−1), and F is the flow rate (cm3·min−1).
Thus, the more open the structure (as found in M1), the longer the residence time (Table 2) for the same flow rate.
The productivity—expressed in mol of product formed per kg of catalyst per h—was calculated from conversion (Conv) and initial concentration of reactant (C0) using the equation:
P = C0ConvVT/τ.
The value of productivity calculated for all microreactors was similar and of ca. 68 mol·kgcat−1·h−1 (Table 3). However, if the productivity was related to the concentration of active centers (mmol of product per mmol of active centers per hour), the M1-A microreactor showed superior performance. This can be ascribed to: (i) enhanced mass transfer from a core of reactants to the skeleton’s surface, and (ii) easier access of reactants to active sites embedded in much larger mesopores of M1-A than in M2-A and M3-A. On the other hand, a greater density of active sites in M2-A and M3-A enabled compensation for the higher activity of the M1-A catalytic sites. However, M1 monoliths revealed the largest permeability of liquids (Table 2), and this bears directly on pressure drop and hence power/energy input and also safety. Thus, bearing in mind all factors, we consider the M1-A microreactor as the most effective solution.
The productivity in the reactor packed with Amberlyst 15 was about 86% of the M1-A microreactor, despite a similar conversion as in M-type reactors. It is important to emphasize that in the case of monolithic microreactors, higher conversions can be achieved by increasing the length of the microreactor or by applying numbering-up approach [5]. For example, by connecting two the M1-A reactors in series, a conversion of 62% was reached (data not shown here).
The M1-A performance also most favourably compares with other studies reported previously (Table 4).

3. Materials and Methods

3.1. Monoliths Synthesis and Activation

Three silica monoliths (M1–M3) in the form of rods with diameter of 4.5 mm were prepared using Nakanishi approach [13,14] with minor modifications [26,27]. In brief, polyethylene glycol (PEG 35000, Sigma-Aldrich, St. Louis, MO, USA) was dissolved in aqueous HNO3 (Avantor, 65%, Gliwice, Poland), after which tetraethoxysilane (TEOS, ABCR, 99%, Karlsruhe, Germany) was added slowly to the PEG solution in an ice bath followed by the addition of cetyltrimethylammonium bromide (CTAB, Sigma-Aldrich) (sample M1). Details of the composition of the reagents are given in Table 5.
After treatment with ammonia (Avantor, 25%), the samples were washed with deionized water and dried for 3 days at 40 °C. Finally, the samples were calcined at 550 °C for 8 h (ramp 1 °C·min−1).
Single silica rods (ca. 4 cm long) were embedded into heat-shrinkable Teflon tubes, equipped with connectors to obtain a microreactor suitable for a continuous operation. Subsequently, silica monoliths were functionalized under flow (48 h, 60 °C) with arenesulphonic acid groups using solution of 2-(4-chlorosulfonylphenyl)ethyltrimethoxysilane (CSPTMS; 50 wt % solution in CH2Cl2, ABCR) dissolved in anhydrous ethanol. The functionalized monoliths were designated as M1-A, M2-A, and M3-A. The nominal content of organic groups was 1.5 mmol·g−1. After activation, the material was washed extensively with ethanol (Avantor, 99.8%) to remove a non-bonding precursor.

3.2. Characterization of Materials

The mesoporous textural properties of the materials were determined from low-temperature nitrogen sorption (Micromeritics ASAP 2020, Norcross, GA, USA). The samples were outgassed in a vacuum for 24 h at 200 °C prior to the analysis. The specific surface area SBET was determined using a standard BET method [36]. The mesopore volume and pore size distribution were calculated from the desorption branch of the isotherm using BJH model [37]. The macroporous network of pores in the silica monoliths was investigated by mercury porosimetry (PoreMaster 60, Quantachrome, Boynton Beach, FL, USA) and by scanning electron microscopy (TM 30000, Hitachi, Tokyo, Japan). Thermal properties and the amount of acidic groups attached to the silica carrier were studied by thermogravimetric analysis (STAR 853, Mettler Toledo, Greifensee, Switzerland). The type and strength of acid centres were determined using pyridine as a probe molecule and a FTIR-DRIFT spectrometer (NICOLET 6700, Thermo Fisher Scientific, Waltham, MA, USA) equipped with high temperature/vacuum chamber with ZnSe windows.

3.3. Catalytic Tests

The catalytic tests were performed in the esterification of acetic acid (Avantor, p.a) with n-butanol (Avantor, p.a) in a continuous-flow monolithic microreactor fabricated using monoliths M1–M3 and a packed bed reactor filled with Amberlyst 15 resin (particle size of 0.7 ± 0.1 mm, Sigma-Aldrich). The esterification process was examined for the molar ratio of substrates 1:1 and at 75 °C using flow rate of 0.06 cm3·min−1. The catalytic tests were carried out for 6 h. The progress of the reaction was monitored by gas chromatography (Agilent 7890 A; FID detector; HP-5 column, Agilent Technologies, Palo Alto, CA, USA).

4. Conclusions

The presented studies clearly showed that the performance of the continuous-flow monolithic microreactors strongly depended on the silica structure both on meso- and macro-scale. It was shown that slight changes in the synthesis procedure strongly affected the structure of monoliths, which translated directly into a significant effect of their flow characteristic. The extremely high pressure drop was recorded when decreasing the size of the macropores from ca. 50 μm to 1.3 μm. Furthermore, smaller mesopores were detected in monoliths with small macropores, which resulted in a considerable increase (ca. 60% of specific surface area). Consequently, a larger concentration of arenesulphonic groups (up to 50%) was identified in these monoliths. However, the microreactors with much larger macroporosity appeared to be the most effective; i.e., they were characterized by a lower pressure drop and higher productivity in the esterification process despite the smaller concentration of active groups. The studied microreactors have strong Brönsted acid sites and they can operate up to 300 °C. Moreover, the performance of the best microreactor appeared to be significantly better than that found for the reactor packed with Amberlyst 15.

Acknowledgments

This work was financed by the National Science Centre Project no DEC-2014/15/N/ST8/03171.

Author Contributions

A.C., K.M. and J.M.-B. conceived and designed the experiments, analysed the data and wrote the paper; J.J.M. wrote part of the manuscript.

Conflicts of Interest

The authors declare no conflict of interest.

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Figure 1. SEM images of (a) M1, (b) M2, and (c) M3 monoliths.
Figure 1. SEM images of (a) M1, (b) M2, and (c) M3 monoliths.
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Figure 2. (a) N2 adsorption/desorption isotherms and pore size distribution in monoliths and Amberlyst 15; (b) Cumulative pore volume curves determined by mercury porosimetry.
Figure 2. (a) N2 adsorption/desorption isotherms and pore size distribution in monoliths and Amberlyst 15; (b) Cumulative pore volume curves determined by mercury porosimetry.
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Figure 3. Thermogravimetric (TG) curves of the functionalized silica monoliths.
Figure 3. Thermogravimetric (TG) curves of the functionalized silica monoliths.
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Figure 4. Fourier transform infrared (FTIR) spectra of M1-A: (a) before and (b) after pyridine adsorption, and after evacuation at (c) 150 °C and (d) 200 °C.
Figure 4. Fourier transform infrared (FTIR) spectra of M1-A: (a) before and (b) after pyridine adsorption, and after evacuation at (c) 150 °C and (d) 200 °C.
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Figure 5. Pressure drop vs. flow rate in microreactors and the packed bed reactor with Amberlyst 15.
Figure 5. Pressure drop vs. flow rate in microreactors and the packed bed reactor with Amberlyst 15.
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Figure 6. Conversion vs. time in the M1-A microreactor.
Figure 6. Conversion vs. time in the M1-A microreactor.
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Table 1. Structural and acidic properties of the materials.
Table 1. Structural and acidic properties of the materials.
SampleSBET
(m2·g−1)
Vpmes
(cm3·g−1)
VT
(cm3·g−1)
Dmac
(μm)
Dmes 1
(nm)
H+
(mmol·g−1)
A200/A150 4
M13281.15430–502.5/200.650.9
(245) 2(0.91)(3.72)(30–50)(20)
M24131.123.274–6150.850.9
(316)(0.91)3.014–6(14.9)
M35751.042.981.38.70.970.8
(427)(0.74)2.651.3(7.9)
Amberlyst400.33--314.7 3n/a
1 a maximum of the pore size distribution curve by BJH; 2 in parentheses, texture parameters after functionalization with acidic groups; 3 manufacturer’s data; 4 relative strength of Brönsted acid sites (BAS).
Table 2. Permeability of silica monoliths and Amberlyst 15.
Table 2. Permeability of silica monoliths and Amberlyst 15.
SamplePermeability K·1012 (m2)
M111.3
M20.27
M30.025
Amberlyst 155.4
Table 3. Results from catalytic experiments.
Table 3. Results from catalytic experiments.
SampleConversion
(%)
τ
(min)
Productivity
(mol·kgcat−1·h−1)
Productivity
(mol·molH+−1·h−1)
M1-A421068.4105.2
M2-A41867.279.2
M3-A427.568.470.8
Amberlyst 15384.261.813.2
Table 4. Comparison of acetic acid esterification with n-butanol in flow (entries 1–2) and batch (entries 3–5) reactors.
Table 4. Comparison of acetic acid esterification with n-butanol in flow (entries 1–2) and batch (entries 3–5) reactors.
EntryCatalystConversion (%)Productivity
(mol·kgcat−1·h−1)
Temp.
(°C)
Time
(min)
Ref.
1M1-A4268.47510 2This work
2Amberlyst 15 170308010 2[33]
3Al-MCM-415029.4150360[34]
4H-USY-203513.875360[35]
5Smopex-1016537.875360[35]
1 packed-bed column; 2 residence time; molar ratio of substrates—1:1.
Table 5. Composition of reagents for monolith synthesis and conditions during ammonia aqueous solution treatment of monoliths prior to drying. PEG: polyethylene glycol.
Table 5. Composition of reagents for monolith synthesis and conditions during ammonia aqueous solution treatment of monoliths prior to drying. PEG: polyethylene glycol.
SampleTEOS
(cm3)
PEG
(g)
H2O
(cm3)
HNO3
(cm3)
CTAB
(g)
Aging
(Days)
Ammonia Treatment
Conc.
(M)
Time
(h)
Temp.
(°C)
M126.12.7330.102.181.271890
M226.13.3131.442.040312480
M326.13.3232.052.39030.12040
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