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Article

Hydroxymethylation of Furfural to HMF with Aqueous Formaldehyde over Zeolite Beta Catalyst

by
Shun Nishimura
* and
Atsuki Shibata
Graduate School of Advanced Science and Technology, Japan Advanced Institute of Science and Technology, 1-1 Asahidai, Nomi, Ishikawa 923-1292, Japan
*
Author to whom correspondence should be addressed.
Catalysts 2019, 9(4), 314; https://doi.org/10.3390/catal9040314
Submission received: 24 February 2019 / Revised: 14 March 2019 / Accepted: 28 March 2019 / Published: 31 March 2019
(This article belongs to the Special Issue Selected Papers from the 2nd Edition of Global Conference on Catalysis, Chemical Engineering and Technology (CAT 2018))
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Abstract

:
Hydroxymethylation of 2-furaldehyde (furfural) toward 5-hydroxymethyl-2-furaldehyde (HMF) was examined in this work among various zeolites with an aqueous formaldehyde as a reagent in a batch and a flow reactor system. It was found that the zeolite beta gave high activity and good reusability with calcination treatment before each run for the target reaction in the batch system. The unique stability of the HMF yield in the liquid-flow system was also observed only in the case of zeolite beta. The effect of the SiO2/Al2O3 ratio in the zeolite beta suggested that hydrophobicity would be an important factor in faster hydroxymethylation with an aqueous formaldehyde reagent. The highest turnover frequency (TOF) for HMF production was found to be 2.4 h−1 in the case of zeolite beta with SiO2/Al2O3 = 440 in the batch reactor system. An approximately 30% yield for HMF was achieved under optimum conditions for zeolite beta catalysts.

Graphical Abstract

1. Introduction

Catalytic biomass transformations towards highly value-added chemicals and materials have been an attractive research area in recent decades in relation to constructing a green and sustainable future society [1,2,3,4,5,6]. Furaldehydes are known as key platform compounds for biomass transformations in lignocellulosic biomass resources. In particular, 5-hydroxymethyl-2-furaldehyde (HMF) is the most important furaldehyde: it possesses two functionalities of formyl and hydroxyl groups on a furan ring at the second and fifth positions and this character enables various successive transformations to afford 2,5-furandicarboxylic acid [7,8], 2,5-diformylfuran [9,10], 2,5-bis(hydroxymethyl)furan (BHMF) [11,12], 2,5-dimethylfuran [13,14,15], 5-hydroxymethylfurfurylamine (HMFA) [16], 1,6-hexanediol [17], levulinic acid [18,19], aldol-adducts [20], and so on [21,22,23]. On the other hand, 2-furaldehyde (furfural), an abundant furaldehyde which is producible at the plant scale with a large quantity, has also permitted many conversions towards furoic acid [24,25], furfuryl alcohol [26,27], 2-methylfuran [28,29], furfuriyamine [30,31], 1,5-pentandiol [32,33], succinic acid [34], condensation products [35,36,37], cyclopentenones [38,39,40] and so on [41], as well as HMF reaction protocols. However, the number of possible derivatives of furfural and those impacts has been much less than those of HMF [1,6]. Apparently, the structural character of furfural, a formyl group linked on a furan ring at the second position, decreases its potential as a starting material in comparison with HMF.
To resolve this weakness of furfural, we have recently examined the direct hydroxymethylation of furfural and its derivatives (C5) with an aqueous formaldehyde reagent to produce the corresponding HMF-like derivatives (C6), a furan ring composed of two functional groups, by using a sulfuric functionalized resin catalyst in a batch and a liquid-flow reactor system [42]. The study carried out a survey of reactivity for the hydroxymethylation reaction among four types of Amberlyst resins constructed with a different acidity and/or surface nature. The Amberlyst-15 was found to be the best resin catalyst with a 43.1% yield and 57.5% selectivity for HMF production in a batch reaction system. It possessed significant reusability and applicability in the generation of furfural derivatives such as BHMF, HMFA, and 5-hydroxymethyl-2-furancarboxylic acid (HMFCA). However, there seems to be a great challenge in fabricating a resin-catalyzed system for the hydroxymethylation of furfural cost-effectively.
According to previous works, Moreau and co-workers have contributed important discussion on the direct hydroxymethylation of furaldehydes with 37% aqueous formaldehyde in the presence of dealuminated mordenite as a catalyst [43,44,45,46]. It is noteworthy that they revealed the importance of the hydrophobicity of highly dealuminated mordenite to the activity of hydroxymethylation of furfuryl alcohol towards BHMF by aqueous formaldehyde [46]. Because a lot of effort has been put into the synthesis of zeolite catalysts at the plant scale, it is likely that the development of zeolite-catalyzed hydroxymethylation of C5 to C6 furaldehydes has a fair chance of adding to sustainable technology in an economical manner.
In this work, we studied the hydroxymethylation of furfural to HMF in aqueous formaldehyde as a dual solvent and reagent (Scheme 1) with four different types of zeolite catalysts. The importance of the hydrophobic nature of the highly active zeolite beta catalyst composed of different SiO2/Al2O3 ratios was also investigated. This study is expected to be interesting and gives new insight into how to further the design of cheaper and/or more advanced systems for the upgrading of furaldehydes.

2. Results and Discussions

2.1. Catalyst Structure and Physicochemical Properties

During our initial survey of the effects of zeolite reactivity on HMF production through the hydroxymethylation of furfural, four conventional types of zeolites were investigated. The Japan Reference Catalyst (JRC) Committee of the Catalysis Society of Japan (Tokyo, Japan) kindly supplied four types of zeolites, and these were calcined at 823 K for 5 h before use. The results of the X-ray diffraction (XRD) analysis of the JRC supplied zeolites are shown in Figure 1a. In comparison with the international centre for diffraction data (ICDD) database obtained through a PDXL software (Rigaku Corp., Tokyo, Japan; ver.1.8.0.3) search and fitting function, JRC-Z-HB150(1) (SiO2/Al2O3 = 150), JRC-Z5-90H(1) (SiO2/Al2O3 = 90), JRC-Z-HM20(5) (SiO2/Al2O3 = 18.3), and JRC-Z-HY5.5 (SiO2/Al2O3 = 5.6) fitted well in accordance with the typical patterns of zeolite beta (card no. 00-056-0467), ZSM-5 (card no. 00-045-0120), mordenite (card no. 00-043-0171), and zeolite Y (card no. 00-040-0336), respectively. JRC-SAH-1 (SiO2/Al2O3 = 2.1) displayed a broad peak at around 25 degrees (at 2θ), indicating that it was amorphous SiO2-Al2O3. The zeolite beta samples composed of different SiO2/Al2O3 ratios were supplied by the JRC and Tosoh Corporation (Tokyo, Japan): JRC-Z-HB25(1) (SiO2/Al2O3 = 25), HSZ-941HOA (SiO2/Al2O3 = 42.2), HSZ-960HOA (SiO2/Al2O3 = 104), HSZ-980HOA (SiO2/Al2O3 = 440), and HSZ-990HOA (SiO2/Al2O3 = 1700). These also possessed clear beta structural forms in all cases, as determined by XRD (Figure 1b).
Pore size distribution and specific surface area were determined by Ar (>99.999 purity) adsorption isotherms at 87 K using BELSORP-max (BEL JAPAN, INC., Osaka, Japan). The samples (100 mg) were pretreated at 623 K for 6 h under vacuum before measurement. A micropore size distribution was estimated with the Saito-Foley (SF) method [47] using BELMaster7 software (MicrotracBEL Corp., Osaka, Japan; ver.7.0.18.8). The adsorption sectional area of Ar at 87 K was 0.1420 nm2. These results are listed in Table 1 (see also Figures S1 and S2 in the Supplementary Materials).
To ascertain the acidity of these samples, NH3-TPD was performed using Belcat II (MicrotracBEL Corp., Osaka, Japan). The sample (100 mg) was pretreated at 823 K for 1 h under an He flow before undergoing NH3 adsorption at 373 K. Thereafter, the vapor treatments were performed three times at 373 K under an He flow. The NH3 desorption was monitored using mass (m/e = 16) for the temperature range 373–873 K at a ramping rate at 10 K min-1 and 873 K for 20 min (const.). The obtained profiles are described in Figure 2. Zeolite beta (SiO2/Al2O3 = 150) had a single peak at around 630 K (acid amount: 0.20 mmol g−1) whereas ZSM-5 showed a peak at around 680 K (acid amount: 0.28 mmol g−1); in other words, the latter possessed a greater abundance and stronger acid sites. Mordenite exhibited humped peaks at 519 K and 800 K (acid amount: >0.65 mmol g−1 in total). Note that a further higher temperature in NH3-TPD seemed to be required to ascertain the full acidic nature in mordenite. However, application of such experimental conditions was limited because the calcination temperature was 823 K in this study. Zeolite Y and normal SiO2-Al2O3 gave a single peak at 582 K (acid amount: 0.38 mmol g−1) and a broad peak with the top of the peak at 557 K (acid amount: 0.42 mmol g−1), respectively. The NH3-TPD profiles for various zeolite beta samples with different SiO2/Al2O3 ratios are also shown in Figure 2b. The fundamental understanding is that a decrease in the SiO2/Al2O3 ratio would lead to an increase in the acid amounts of the zeolite [48,49]. However, the peak area for SiO2/Al2O3 = 25 (corresponding acid amount: 0.37 mmol g−1) was a little smaller than that for SiO2/Al2O3 = 42.2 (ibid.: 0.42 mmol g−1). From the viewpoint of the XRD patterns (Figure 1b) and pore size distribution (Figure S2), it was found that the crystallinity and pore volume of zeolite beta for SiO2/Al2O3 = 25 seemed to be slightly poorer than those of the other zeolite beta samples. Accordingly, we suppose that the BEA crystal imperfection in the case of SiO2/Al2O3 = 25 can lead to such disordering in the peak area in NH3-TPD, i.e., the acid amount, between SiO2/Al2O3 = 25 and 42.2. Estimated acid amounts for all samples are listed in Table 1.

2.2. Reactivity among Different Zeolite Structures

Figure 3 shows the time-based reaction progress of the hydroxymethylation of furfural with aqueous formaldehyde towards HMF production with zeolite beta, ZSM-5, mordenite, zeolite Y, and normal SiO2-Al2O3. Zeolite Y and normal SiO2-Al2O3 were inactive for HMF production. Linear increases in HMF yield were observed for ZSM-5 and mordenite. Notably, only zeolite beta had a significant impact on HMF production with a high conversion value (see Figure S3). The best catalyst studied for the reaction of furfural with a formaldehyde aqueous solution was zeolite beta (SiO2/Al2O3 = 150), which afforded the highest HMF yield of 29% with 82% conversion of furfural at 6 h in the batch reactor system.
Because these four types of zeolite were composed of different SiO2/Al2O3 ratios in this study, a simple discussion of structural impacts on the hydroxymethylation of furfural towards HMF in aqueous formaldehyde was difficult to achieve. However, interesting phenomena for zeolite beta were also observed in the flow reactor system. Figure 4 shows the results for the application of a continuous flow reactor system over the four types of zeolite catalysts for the hydroxymethylation of furfural towards HMF. As shown in Figure 4a, gradual decreases in furfural conversion value were detected for all zeolite samples during the progress of the flow reaction. From the viewpoint of the catalytic behavior affording HMF (yield) shown in Figure 4b, however, zeolite beta showed significantly different behavior. In the case of zeolite beta only, a gradual increase and constant yield were monitored within 3.5 h in the flow reaction, though the other three zeolites gave an inactive and/or decreasing yield for HMF. Such unique behavior of zeolite beta also appeared for various SiO2/Al2O3 cases (vide infra). Note that the initial induction period detected in a flow reactor system owes itself to the pelletizing treatment of the powder sample. Accordingly, the textural specialty of zeolite beta is an attractive subject of attention, even though the different SiO2/Al2O3 ratios were used for discussion of reactivity among four types of zeolite samples.
It was noted that zeolite beta, mordenite, and zeolite Y had large-pore structures of ~5.6 Å × 7.6 Å, ~6.5 Å × 7.0 Å, and ~7.4 Å × 7.4 Å, respectively, whereas ZSM-5 possessed a medium-pore structure of ~5.1 Å × 5.6 Å [50,51]. On the basis of the present Ar adsorption analytical approach, mordenite exhibited a middle pore diameter of 5.7 Å (Figure S1b), which was a smaller value than that mentioned above. Because mordenite is constructed with two types of ring, these being an 8-membered ring (~3.4 Å × 4.8 Å) and a 12-membered ring (~6.5 Å × 7.0 Å), such differences were expected. ZSM-5 is a 10-membered ring zeolite, whereas zeolite beta and zeolite Y are 12-membered ring zeolites. According to these properties, the size sensitivity and/or topology derived from each zeolite type would have scarcely contributed to the differences in reactivity for the target reaction. However, it was interesting to observe that the conversion values of furfural dramatically changed across the different zeolites (vide supra). There has been some discussion on the importance of acidity, i.e. the Brønsted/Lewis amount, to try to explain the different reactivities obtained for various types of zeolites in the presence of water [52,53].

2.3. Reusability of Zeolite Beta

The reusability of zeolite beta (SiO2/Al2O3 = 150) was investigated in a batch reactor. After the present reaction, the reaction media was centrifuged, and then the spent powder catalyst was washed with 0.5 L water and dried at 383 K overnight. Thereafter, the next recycling run was performed after re-calcination treatment at 823 K for 5 h. Because weight loss of catalyst powder could not be prohibited during the catalyst correction and reactivation procedures, different scales were applied for the recycling tests (see Table S1). As shown in Figure 5, high reusability for the above three recycling runs was achieved with zeolite beta. It should be noted that re-calcination treatment was necessary because a significant color change from white to dark gray after reaction occurred, i.e., strong carbon depositions onto the catalyst surface were expected during the reaction (see Figures S4 and S5). In the high performance liquid chromatography (HPLC) chart, some unidentified peaks were detected (Figure S6). However, the gas chromatography-time of flight mass (GC-TOFMS) spectrometry (JEOL Ltd., Tokyo, Japan; AccuTOFGCx) of the reaction mixture could not identify any appropriate side reactions, such as the self-resinification of furfural [45,54] and the dimerization of as-produced HMF [55,56], for the present situation; some of these products might be trapped on/in the zeolite, leading to color changes during the reaction.

2.4. Effect of SiO2/Al2O3 Ratio on Zeolite Beta

The effect of the SiO2/Al2O3 ratio on the target reaction was evaluated using fine zeolite beta samples fabricated with different SiO2/Al2O3 ratios. Figure 6 shows the time-based reaction progress of the hydroxymethylation of furfural towards HMF among zeolite beta samples composed of different SiO2/Al2O3 ratios in a batch reactor. Corresponding alterations of conversion and yield are also shown in Figure S7. Interestingly, SiO2/Al2O3 strongly influenced the reaction progress for the target reaction (Figure 6a). An increase in the SiO2/Al2O3 ratio from 25 to 42.2 led to a great increase in HMF yield, while similar progress of the reaction was obtained for the range 42.4–150. Thereafter, it seemed to gradually diminish in the cases from 440 to 1700. The highest yield of 31.6% with a 67.9% conversion rate was detected at 12 h during the reaction for SiO2/Al2O3 = 104.
To further discuss the details of the differences in reactivity derived from the SiO2/Al2O3 ratios, the initial rates of the reaction per acid amount and the TOF values were plotted in Figure 6b,c, respectively. It can be clearly observed that the SiO2/Al2O3 ratio was greatly associated with the reactivity of the target reaction. The reactivity had been heightened by increasing the SiO2/Al2O3 ratio from 25 to 440. The highest TOF value leached at 2.4 h−1, which was four times higher than that obtained using SiO2/Al2O3 = 25. In addition, a significantly large SiO2/Al2O3 value (1700) produced a drastic decrease in the TOF value, giving a value of 0.5 h−1.
In previous studies on zeolite catalysis, many researchers have insisted on the importance of the hydrophobic/hydrophilic nature of zeolites within the catalysis [57,58]. To anticipate the association of surface affinity with water, the main reaction media, the H2O (18.2 kΩ·cm) adsorption isotherm at 298 K was attempted using BELSORP-max. (BEL JAPAN, INC., Osaka, Japan). The samples (100 mg) were pretreated at 573 K for 6 h under vacuum before being measured. The adsorption sectional area of H2O at 298 K was 0.1250 nm2. Figure 7 shows the plot of the monolayer adsorption capacity density, which is the monolayer water adsorption capacity value (vm) (cm3(STP) g−1) divided by a specific surface area against Ar (m2 g−1) as a function of the SiO2/Al2O3 ratio in zeolite beta. According to previous papers [46,59], it was well-known that delamination treatment usually enhances the hydrophobic nature of zeolites. In fact, the SiO2/Al2O3 ratio for zeolite beta involved the monolayer water adsorption capacity, and the SiO2/Al2O3 = 440 ratio which exhibited the highest TOF value (vide superior) possessed the strongest hydrophobic nature among the zeolite beta samples used in this study. Note that the difference in tendencies observed in the cases of lower/higher SiO2/Al2O3 (= 25 and 1700) detected in Figure 7 would be owing to the poor crystallinity of the zeolite and/or the presence of extra SiO2 or Al2O3 species. A similar tendency between adsorption capacity and SiO2/Al2O3 ratio has been observed in the case of mordenite in a previous paper [60]. Accordingly, hydrophobicity was considered to be the one of key factors in accelerating the target reaction. It is notable that Moreau et al. also insisted that the hydrophobic character in mordenite was a predominant factor in the activity of hydroxymethylation of furfuryl alcohol by aqueous formaldehyde because the adsorption of organic substrates onto the catalyst in water as solvent determined the reaction constant for the reaction [46]. However, there still remains an open question about whether the relationship between the TOF value and the monolayer adsorption capacity density did not make a linear contribution. It is supposed that determination of the actual acid sites working in water solvent, e.g., the impact of water tolerance on Brønsted/Lewis acidity, would be helpful for further understanding the mechanism of zeolite beta-catalyzed hydroxymethylation of furfural to HMF with aqueous formaldehyde as a dual solvent and reagent. Notably, applications of various zeolite betas for the flow reactor system were also capable and showed good stability of HMF yield (see Figure S8).

3. Materials and Methods

3.1. Batch Reactor System

The reaction was performed in a Schlenk glass flask attached to a condensation cooler. As a general procedure, first, 37% aqueous formaldehyde solution (stabilized with 5–10% methanol, Wako Pure Chemical Ind. Ltd., Osaka, Japan) (5 mL) and solid catalyst (200 mg) were mixed well under vigorous stirring (500 rpm) at 363 K. Thereafter, the substrate of furfural (1 mmol) without purification treatment (Acros Organic, Geel, Belgium; 99% purity) was injected into the above mixture to initiate the target reaction. Then, after 12 h of reaction, the catalyst was filtered off with a Milex syringe filter (0.20 μm) (Merck, Darmstadt, Germany) and the obtained filtrate was analyzed using an HPLC equipped with a refractive index (RI) detector (Waters 2414). The column was an Aminex HPX-87H (Bio-Rad Laboratories Inc., Hercules, CA, USA) under 10 mM H2SO4 aq. flow (0.5 mL min−1). The retention times for HMF and furfural were 39.1 min and 60.0 min, respectively. Conversion and yield values were estimated with the standard lines adjusted by each reference compound.

3.2. Flow Reactor System

The liquid flow reaction was examined with a simple flow reactor system (MCR-1000; EYELA, Tokyo, Japan). A powdered zeolite sample was pressed (40 kPa for 30 min) into thin wafers, and then crushed and screened within a mesh size range of 26–42, before being installed into the reaction bed tube (φ5). The flow rate of the reaction mixture of furfural (10 mmol) and formalin (50 mL) was 0.2 mL min−1 and the reaction was performed at 363 K. The reactant was analyzed by HPLC using the same procedure mentioned above.

4. Conclusions

In summary, four types of typical zeolites and normal SiO2-Al2O3 were tentatively compared with regard to their reactivity for the hydroxymethylation of furfural towards HMF in a batch reactor system and a flow reactor system. Interestingly, the beta-type zeolite was found to be a highly-active, reusable, and uniquely stable catalyst. The effect of the SiO2/Al2O3 ratio for the various zeolite beta samples was examined using reactivity (TOF), NH3-TPD, and water adsorption capacity. The zeolite beta composed of SiO2/Al2O3 = 440 gave the highest TOF value of 2.4 h−1 in the batch reactor system and it possessed a strong hydrophobic nature. According to these results, it may be suggested that hydrophobicity plays a crucial role in the hydroxymethylation of furfural towards HMF using an aqueous formaldehyde reagent. In comparison to our previous report, which focused on a sulfuric functionalized resin catalyst [42], we have observed that there are a variety of ways of constructing morphology/affinity-controlled zeolite fabrications. Therefore, novel catalysis derived from zeolite beta in this report is expected to open up new possibilities for future research on the designs of zeolite-catalyzed hydroxymethylations, and in particular, the upgrading of C5 to C6 furaldehydes in biorefinery.

Supplementary Materials

The following are available online at https://www.mdpi.com/2073-4344/9/4/314/s1, Figure S1: Pore size distributions of ZSM-5, mordenite, zeolite Y, and normal SiO2-Al2O3 determined by Ar adsorption, Figure S2: Pore size distributions of zeolite beta with various SiO2/Al2O3 determined by Ar adsorption, Figure S3: Time-based reaction progression of furfural conversion for hydroxymethylation among four zeolites and normal SiO2-Al2O3 in a batch reactor, Table S1: Recycling experiments for the zeolite beta (SiO2/Al2O3 = 150) in a batch reactor, Figure S4: T Photographs of (a) fresh and (b) spent zeolite beta catalyst (SiO2/Al2O3 = 150), Figure S5: TG-DTA curves of spent zeolite beta (SiO2/Al2O3 = 150) in a batch reaction, Figure S6: Example of HPLC chromatograph for the hydroxymethylation of furfural to HMF in aqueous formaldehyde over zeolite beta, Figure S7: Time-based reaction progression of the hydroxymethylation of furfural to HMF among zeolite beta samples composed of different SiO2/Al2O3 ratios in a batch reactor: (a) furfural conversion and (b) HMF yield, Figure S8: Time-based reaction for HMF production in a flow reactor using f zeolite beta samples composed of various SiO2/Al2O3 ratios: (a) furfural conversion and (b) HMF yield.

Author Contributions

Conceptualization, S.N.; methodology, S.N. and A.S.; formal analysis, S.N. and A.S.; investigation, S.N. and A.S.; resources, S.N. and A.S.; data curation, S.N. and A.S.; writing—original draft preparation, S.N.; writing—review and editing, S.N.; visualization, S.N.; supervision, S.N.; project administration, S.N.; funding acquisition, S.N.

Funding

This work was supported by JSPS KAKENHI for Young Scientists (A) (grant no. 17H04966), Japan.

Acknowledgments

The authors would like to thank Prof. K. Ebitani (JAIST) for his encouragement of this research and Dr. D. Mott (Tohoku Univ.) for his careful reading of the manuscript.

Conflicts of Interest

The authors declare that they have no competing financial interest.

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Catalysts 09 00314 sch001 550
Scheme 1. Hydroxymethylation of furfural to 5-hydroxymethyl-2-furaldehyde (HMF) with a formaldehyde reagent.
Scheme 1. Hydroxymethylation of furfural to 5-hydroxymethyl-2-furaldehyde (HMF) with a formaldehyde reagent.
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Figure 1. X-ray diffraction (XRD) patterns of (a) four types of reference zeolites and normal SiO2-Al2O3 and (b) zeolite beta samples composed with various SiO2/Al2O3 ratios.
Figure 1. X-ray diffraction (XRD) patterns of (a) four types of reference zeolites and normal SiO2-Al2O3 and (b) zeolite beta samples composed with various SiO2/Al2O3 ratios.
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Figure 2. NH3-temperature programed desorption (NH3-TPD) of (a) four types of reference zeolites and normal SiO2-Al2O3 and (b) zeolite betas composed with various SiO2/Al2O3 ratios.
Figure 2. NH3-temperature programed desorption (NH3-TPD) of (a) four types of reference zeolites and normal SiO2-Al2O3 and (b) zeolite betas composed with various SiO2/Al2O3 ratios.
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Figure 3. Time-based reaction progression of the hydroxymethylation of furfural towards HMF among four zeolites and normal SiO2-Al2O3 in a batch reactor. Reaction conditions: furfural (1 mmol), formalin (5 mL), catalyst (200 mg), temperature (363 K), stirring (500 rpm).
Figure 3. Time-based reaction progression of the hydroxymethylation of furfural towards HMF among four zeolites and normal SiO2-Al2O3 in a batch reactor. Reaction conditions: furfural (1 mmol), formalin (5 mL), catalyst (200 mg), temperature (363 K), stirring (500 rpm).
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Figure 4. Time-based reaction for HMF production in a flow reactor using four different types of zeolites. Reaction conditions: furfural (10 mmol), formalin (50 mL), catalyst (500 mg), temperature (363 K), flow rate (0.2 mL min−1).
Figure 4. Time-based reaction for HMF production in a flow reactor using four different types of zeolites. Reaction conditions: furfural (10 mmol), formalin (50 mL), catalyst (500 mg), temperature (363 K), flow rate (0.2 mL min−1).
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Figure 5. Recycling tests on the hydroxymethylation of furfural towards HMF over zeolite beta in a batch reactor. Reaction conditions: furfural (1–3 mmol), formalin (5–15 mL), catalyst (600–200 mg), temperature (363 K), time (6 h), stirring (500 rpm). The catalyst was re-calcined at 823 K before each reuse.
Figure 5. Recycling tests on the hydroxymethylation of furfural towards HMF over zeolite beta in a batch reactor. Reaction conditions: furfural (1–3 mmol), formalin (5–15 mL), catalyst (600–200 mg), temperature (363 K), time (6 h), stirring (500 rpm). The catalyst was re-calcined at 823 K before each reuse.
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Figure 6. Time-based reaction progression of the hydroxymethylation of furfural to HMF among zeolite beta samples composed of different SiO2/Al2O3 ratios in a batch reactor: (a) HMF concentration and (b) initial rate for HMF production per acid amount. (c) Plot of turnover frequency (TOF) values as a function of SiO2/Al2O3 ratio on the basis of the dashed lines in (b) which represent the linear approximation results. Reaction conditions: furfural (1 mmol), formalin (5 mL), catalyst (200 mg), temperature (363 K), stirring (500 rpm).
Figure 6. Time-based reaction progression of the hydroxymethylation of furfural to HMF among zeolite beta samples composed of different SiO2/Al2O3 ratios in a batch reactor: (a) HMF concentration and (b) initial rate for HMF production per acid amount. (c) Plot of turnover frequency (TOF) values as a function of SiO2/Al2O3 ratio on the basis of the dashed lines in (b) which represent the linear approximation results. Reaction conditions: furfural (1 mmol), formalin (5 mL), catalyst (200 mg), temperature (363 K), stirring (500 rpm).
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Figure 7. Monolayer adsorption capacity density as a function of SiO2/Al2O3 ratio with zeolite beta. STP: standard ambient temperature and pressure.
Figure 7. Monolayer adsorption capacity density as a function of SiO2/Al2O3 ratio with zeolite beta. STP: standard ambient temperature and pressure.
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Table
Table 1. Physicochemical properties of catalysts used.
Table 1. Physicochemical properties of catalysts used.
EntryCatalyst aSBET b
(m2 g−1)		Average Pore Size b
(nm)		Acid Amount c
(mmol g−1)
1Beta (25)4940.690.37
2Beta (42.2)6390.680.42
3Beta (104)6130.710.24
4Beta (150)6070.730.20
5Beta (440)5710.710.076
6Beta (1700)5650.690.038
7ZSM-5 (90)4210.600.28
8Mordenite (18.3)4790.57>0.65
9Y (5.6)6510.720.38
10SiO2-Al2O3 (2.1)305N/A0.42
a Calcined at 823 K for 5 h; the numbers in parentheses are the SiO2/Al2O3 ratios. b Determined by Ar adsorption. SBET: a specific surface area determined by the Brunauer-Emmett-Teller theory. c Estimated by NH3-temperature programmed desorption (NH3-TPD) analysis.

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Nishimura, S.; Shibata, A. Hydroxymethylation of Furfural to HMF with Aqueous Formaldehyde over Zeolite Beta Catalyst. Catalysts 2019, 9, 314. https://doi.org/10.3390/catal9040314

AMA Style

Nishimura S, Shibata A. Hydroxymethylation of Furfural to HMF with Aqueous Formaldehyde over Zeolite Beta Catalyst. Catalysts. 2019; 9(4):314. https://doi.org/10.3390/catal9040314

Chicago/Turabian Style

Nishimura, Shun, and Atsuki Shibata. 2019. "Hydroxymethylation of Furfural to HMF with Aqueous Formaldehyde over Zeolite Beta Catalyst" Catalysts 9, no. 4: 314. https://doi.org/10.3390/catal9040314

APA Style

Nishimura, S., & Shibata, A. (2019). Hydroxymethylation of Furfural to HMF with Aqueous Formaldehyde over Zeolite Beta Catalyst. Catalysts, 9(4), 314. https://doi.org/10.3390/catal9040314

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