Microwave-Assisted Catalytic Conversion of 5-HMF for Biofuel Additives by Molybdophosphoric Acid Encapsulated KCC-1

: In this work, the microwave-assisted reaction of 5-hydroxymethylfurfural (5-HMF) into valuable ether and acylated production formation was investigated with the help of molybdophosphoric acid encapsulated dendritic ﬁbrous silica (KCC-1) as a catalyst. XRD, N 2 adsorption-desorption, SEM, FT-IR, NH 3 -TPD, and TEM were used to analyze the physicochemical and structural properties of the synthesized catalysts. The microwave etheriﬁcation of 5-HMF with ethanol was tested using synthesized catalysts. The effects of the reaction temperature, reaction time, catalytic amount, and microwave power were investigated. The resulting MPA-KCC-1 and IMPA-KCC-1 catalysts demonstrated excellent activity for the etheriﬁcation of 5-HMF with ethanol, producing 5-(hydroxymethyl) furfural diethyl acetal (HMFDEA) and 5-(ethoxymethyl)furfural diethyl acetal (EMFDEA) products selectively. The signiﬁcant advantages of the work are the selective production of EMFDEA at 82%, the catalyst can be easily removed via ﬁltration, and the catalyst activity remains nearly intact even after ﬁve reaction cycles.


Introduction
Global warming is consistently growing due to the rapid consumption of fossil fuels, which creates a situation for researchers to find suitable alternative fuels. Biomass is considered one of the renewable energy sources and has received great attention among researchers, being sustainable to the environment and helping to reduce carbon footprints [1][2][3][4]. Moreover, biomass is a potential source for producing value-added chemicals, sustainable fuels, and renewable catalytic materials [5][6][7][8]. The organic compound 5-hydroxymethylfurfural (5-HMF) is derived from biomass carbohydrates, such as glucose and fructose, through acidcatalyzed dehydration. It is a versatile platform chemical with a wide range of applications, including as a fuel additive and as a precursor for the production of various chemicals and materials [8][9][10].
The 5-HMF can be upgraded through aldol condensation, esterification, etherification, amination, reduction, and oxidation [8,11]. The etherification or acetylation of 5-HMF are classes of reaction for biofuel additive synthesis with a high energy density, and they are also interesting for fundamental research [12,13]. Typically, the etherification of 5-HMF has been performed with ethanol and other lower-carbon alcohols in the presence of solid acid catalysts. Most of the solid acid catalysts have been reported for 5-EMF or 5-alkoxy methyl furfural synthesis from 5-HMF, including ambertlyst-15 [14,15], Al-MCM-41 [13,16], Figure 1 shows the XRD patterns of the unmodified pure KCC-1 and MPA-modified KCC-1 catalysts. The optimized amount of MPA was 20 wt.% from the reported literature and the same amount was taken to encapsulate in the KCC-1 silica material. The morphological structure of the KCC-1 silica materials collapsed if the increase in the encapsulation of MPA wt.% was more than 20 with KCC-1. The 20 wt.% impregnated on KCC-1 was synthesized to evaluate the catalytic activity with the encapsulated one [32,33]. All of the prepared Catalysts 2023, 13, 969 3 of 13 materials showed a large peak at 2θ degrees at 23 • in the X-ray diffraction, indicating the silica's characteristic amorphous nature ( Figure 1). In addition, the absence of MPA or its crystalline decomposition diffraction lines within the MPA-KCC-1 catalyst implied that the MPA molecules were distributed evenly in the silica matrix with Keggin units [34]. The primary XRD lines in the IMPA-KCC-1 were at 2θ, 13.8 • , 23.5 • , 26.3 • , 27.2 • , 34 • , and 39.2 • ; these peaks are aligned with the crystalline peaks of the pure MPA molecule. These peaks are typically assigned to cubic Keggin-type structures (the black color diffraction pattern in Figure 1). Due to the impregnation process, the intensity of IMPA was seen to be smaller than that of pure KCC-1 and MPA-KCC-1. Figure 1 shows the XRD patterns of the unmodified pure KCC-1 and MPA-modified KCC-1 catalysts. The optimized amount of MPA was 20 wt.% from the reported literature and the same amount was taken to encapsulate in the KCC-1 silica material. The morphological structure of the KCC-1 silica materials collapsed if the increase in the encapsulation of MPA wt.% was more than 20 with KCC-1. The 20 wt.% impregnated on KCC-1 was synthesized to evaluate the catalytic activity with the encapsulated one [32,33]. All of the prepared materials showed a large peak at 2θ degrees at 23° in the X-ray diffraction, indicating the silica's characteristic amorphous nature ( Figure 1). In addition, the absence of MPA or its crystalline decomposition diffraction lines within the MPA-KCC-1 catalyst implied that the MPA molecules were distributed evenly in the silica matrix with Keggin units [34]. The primary XRD lines in the IMPA-KCC-1 were at 2θ, 13.8°, 23.5°, 26.3°, 27.2°, 34°, and 39.2°; these peaks are aligned with the crystalline peaks of the pure MPA molecule. These peaks are typically assigned to cubic Keggin-type structures (the black color diffraction pattern in Figure 1). Due to the impregnation process, the intensity of IMPA was seen to be smaller than that of pure KCC-1 and MPA-KCC-1. The FT-IR spectra of the KCC-1 and MPA encapsulated and impregnated KCC-1 are shown in Figure 2. The broad peak at 3100 to 3600 cm −1 was assigned to the water molecules absorbed on the surface of the silica KCC-1. After the encapsulation and impregnation of MPA molecules with KCC-1 silica support, the broad peak was reduced due to the reduction of the absorbed water molecules or the interaction of -OH groups with loaded MPA molecules. The heteropoly acids of the MPA molecule bonds are generally located at 1060, 970, 875, and 760 cm −1 , corresponding to the stretching vibration of v(P-Oa), v(M-Od), v(M-Ob-M), and v(M-Oc-M) and also confirm the Keggin formations (M represents the Mo metal ions) [35]. Notably, most of the bands of the heteropoly anions overlapped with the SiO2 peaks and create difficulties in distinguishing the peaks between the heteropoly anions and SiO2. The FT-IR spectra of the KCC-1 and MPA encapsulated and impregnated KCC-1 are shown in Figure 2. The broad peak at 3100 to 3600 cm −1 was assigned to the water molecules absorbed on the surface of the silica KCC-1. After the encapsulation and impregnation of MPA molecules with KCC-1 silica support, the broad peak was reduced due to the reduction of the absorbed water molecules or the interaction of -OH groups with loaded MPA molecules. The heteropoly acids of the MPA molecule bonds are generally located at 1060, 970, 875, and 760 cm −1 , corresponding to the stretching vibration of v(P-Oa), v(M-Od), v(M-Ob-M), and v(M-Oc-M) and also confirm the Keggin formations (M represents the Mo metal ions) [35]. Notably, most of the bands of the heteropoly anions overlapped with the SiO 2 peaks and create difficulties in distinguishing the peaks between the heteropoly anions and SiO 2 .  Figure 3a,b depict the N2 sorption isotherms and BJH pore size distribution of the KCC-1, MPA-KCC-1, and IMPA-KCC-1 catalysts, and Table 1 provides the associated textural properties. The observed Type IV isotherms with H3 hysteresis loops in all synthe-  Table 1 provides the associated textural properties. The observed Type IV isotherms with H3 hysteresis loops in all synthesized materials can specify the mesoporous nature of those materials and can also confirm the formation of the mesoporous structures with large pores [36]. KCC-1, MPA-KCC-1, and IMPA-KCC-1 each had a surface area of 523, 320, and 380 m 2 /g, respectively (Table 1). In Figure 3b, the BJH pore size distribution (Figure 3b) adsorbed the volume in the range of 0.4 to 0.95 P/P o and was observed in all the catalysts, which confirms the presence of a large pore size distribution. The encapsulation strategy decreased the BET surface of MPA-KCC-1, (320 m 2 /g) and pore volume (0.65 cm 3 /g).  Figure 3a,b depict the N2 sorption isotherms and BJH pore size distribution of the KCC-1, MPA-KCC-1, and IMPA-KCC-1 catalysts, and Table 1 provides the associated textural properties. The observed Type IV isotherms with H3 hysteresis loops in all synthesized materials can specify the mesoporous nature of those materials and can also confirm the formation of the mesoporous structures with large pores [36]. KCC-1, MPA-KCC-1, and IMPA-KCC-1 each had a surface area of 523, 320, and 380 m 2 /g, respectively (Table 1). In Figure 3b, the BJH pore size distribution (Figure 3b) adsorbed the volume in the range of 0.4 to 0.95 P/Po and was observed in all the catalysts, which confirms the presence of a large pore size distribution. The encapsulation strategy decreased the BET surface of MPA-KCC-1, (320 m 2 /g) and pore volume (0.65 cm 3 /g).  The prepared samples' total acidity was evaluated using NH 3 -TPD, and their desorbed ammonia profiles are displayed in Figure 4. The total acidity of the pure siliceous KCC-1 was 0.022 mmol/NH 3 , which is negligible with the comparison of the total acidity of the MPA-KCC-1 and IMPA-KCC-1 catalysts (the acidic amounts are displayed in Table 1). In the NH 3 -TPD profile, the weak and moderate acidic sites of the MPA-KCC-1 and IMPA-KCC-1 can be observed at 80 to 150 • C and at 300 to 450 • C. The acidity of the IMPA-KCC-1 catalyst appears to be high, which is due to the impregnation method, which accommodated more heteropoly anions in the silica matrix as well as on the material's surface, resulting in a high acidic strength. The observed total acid value of the MPA-KCC-1 catalyst was considerably lower, indicating that its heteropoly anion was lost during the catalyst wash after synthesis [33].

Characterization Analysis
IMPA-KCC-1 can be observed at 80 to 150 °C and at 300 to 450 °C. The acidity of the IM KCC-1 catalyst appears to be high, which is due to the impregnation method, which commodated more heteropoly anions in the silica matrix as well as on the material's face, resulting in a high acidic strength. The observed total acid value of the MPA-KC catalyst was considerably lower, indicating that its heteropoly anion was lost during catalyst wash after synthesis [33]. The morphology of the synthesized catalysts was evaluated using SEM and T techniques; the related images are presented in Figures 5 and 6, respectively. Both the ( Figure 5a) and TEM ( Figure 6a) images of unmodified KCC-1 show the well-prese dendritic fibrous structure. The spherical morphology can be preserved during the M encapsulation strategy in KCC-1, allowing the MPA molecules to be filled evenly wi the fibrous natured pores that can be observed in the MPA-KCC-1 SEM image (Figure [33]. Furthermore, during synthesis, MPA is encapsulated in silica, transforming the m phology of the fibrous structure into a mesoporous sphere-shaped structure with the sistent distribution of pore sizes that can be observed in the MPA-KCC-1 TEM image ure 6b). Due to the accommodation of MPA molecules on the surface of the material fibrous-natured tiny pores are covered, generating homogeneous mesopores (12 nm) a dendritic spherical structure. The average particle size of the KCC-1 and MPA-KCC 0.4 ± 0.05 µm and 0.38 ± 0.05, respectively (calculated using ImageJ software). As a re the structure of the material and particle size is unaffected by the encapsulation techn [32]. The impregnation procedure had no impact on the morphology of the KCC-1 (Fi 6c) by the impregnation process, which can be observed in the TEM image of the IM The morphology of the synthesized catalysts was evaluated using SEM and TEM techniques; the related images are presented in Figures 5 and 6, respectively. Both the SEM ( Figure 5a) and TEM ( Figure 6a) images of unmodified KCC-1 show the well-preserved dendritic fibrous structure. The spherical morphology can be preserved during the MPA encapsulation strategy in KCC-1, allowing the MPA molecules to be filled evenly within the fibrous natured pores that can be observed in the MPA-KCC-1 SEM image ( Figure 5b) [33]. Furthermore, during synthesis, MPA is encapsulated in silica, transforming the morphology of the fibrous structure into a mesoporous sphere-shaped structure with the consistent distribution of pore sizes that can be observed in the MPA-KCC-1 TEM image (Figure 6b). Due to the accommodation of MPA molecules on the surface of the material, the fibrous-natured tiny pores are covered, generating homogeneous mesopores (12 nm) with a dendritic spherical structure. The average particle size of the KCC-1 and MPA-KCC-1 is 0.4 ± 0.05 µm and 0.38 ± 0.05, respectively (calculated using ImageJ software). As a result, the structure of the material and particle size is unaffected by the encapsulation technique [32]. The impregnation procedure had no impact on the morphology of the KCC-1 (Figure 6c) by the impregnation process, which can be observed in the TEM image of the IMPA-KCC-1. The impregnated KCC-1 and encapsulated MPA on KCC-1 catalysts were comprehensively characterized, and then its catalytic activity for the 5-HMF etherification with ethanol was assessed.

Catalytic Activity Study on HMF Etherification and Acylation with Ethanol
The prepared MPA encapsulated and impregnated KCC-1 catalysts were tested in the microwave etherification of 5-HMF with ethanol. Initially, the MPA-KCC-1 and IMPA-KCC-1 catalytic activities were evaluated for the 5-HMF etherification with ethanol at different temperatures for 30 min; the subsequent results are shown in Figure 7. The main products were 5-(hydroxymethyl) furfural diethyl acetal (HMFDEA), 5-(ethoxymethyl)furfural diethyl acetal (EMFDEA), and minor amounts of ethyl levulinate (EL) formations were noticed. In the temperature study, the 5-HMF conversion was increased until 120 °C, then dropped in at 140 °C due to the reverse reaction of HMFDEA to 5-HMF, where the EMFEDA and ethyl levulinate (EL) selectivity were increased [37]. The HMFDEA selectivity was high at a lower temperature of 80 °C and as the temperature increased, the selectivity of HMFDEA was reduced, while the EMFDEA selectivity increased gradually to 71% at 120 °C. Further, at a higher temperature of 140 °C, the EMFDEA slightly decreased instead of the EL selectivity increasing. The temperature study reveals that a high temperature favors more EL product formation. The maximum conversion of 5-HMF and EMFDEA selectivity was obtained at 120 °C and the temperature was considered the optimum for other parameter analysis. The IMPA-KCC-1 catalyst showed a higher conversion and selectivity due to its high total acidity (0.385 mmol NH3/g, Table 1). The surface area of both the MPA-KCC-1 and IMPA-KCC-1 catalysts was almost the same, which seemed to have no impact on the catalysis. Here, the acidity of the

Catalytic Activity Study on HMF Etherification and Acylation with Ethanol
The prepared MPA encapsulated and impregnated KCC-1 catalysts were tested in the microwave etherification of 5-HMF with ethanol. Initially, the MPA-KCC-1 and IMPA-KCC-1 catalytic activities were evaluated for the 5-HMF etherification with ethanol at different temperatures for 30 min; the subsequent results are shown in Figure 7. The main products were 5-(hydroxymethyl) furfural diethyl acetal (HMFDEA), 5-(ethoxymethyl)furfural diethyl acetal (EMFDEA), and minor amounts of ethyl levulinate (EL) formations were noticed. In the temperature study, the 5-HMF conversion was increased until 120 • C, then dropped in at 140 • C due to the reverse reaction of HMFDEA to 5-HMF, where the EMFEDA and ethyl levulinate (EL) selectivity were increased [37]. The HMFDEA selectivity was high at a lower temperature of 80 • C and as the temperature increased, the selectivity of HMFDEA was reduced, while the EMFDEA selectivity increased gradually to 71% at 120 • C. Further, at a higher temperature of 140 • C, the EMFDEA slightly decreased instead of the EL selectivity increasing. The temperature study reveals that a high temperature favors more EL product formation. The maximum conversion of 5-HMF and EMFDEA selectivity was obtained at 120 • C and the temperature was considered the optimum for other parameter analysis. The IMPA-KCC-1 catalyst showed a higher conversion and selectivity due to its high total acidity (0.385 mmol NH 3 /g, Table 1). The surface area of both the MPA-KCC-1 and IMPA-KCC-1 catalysts was almost the same, which seemed to have no impact on the catalysis. Here, the acidity of the catalyst and the temperature of the reaction play an important role. Even though the acidity of the IMPA-KCC-1 is higher than MPA-KCC-1, it was not considered for further studies because larger amounts of heteropoly anions were leached during the reaction, which was confirmed through ICP-OES analysis of the reacted solution. In our previous study, we observed the same effect for tungstophosphoric acid encapsulated KCC-1 silica for carbohydrates to 5-HMF conversion in a microwave assisted reaction condition [32]. The catalytic activity of pure molyptophosphoric acid was evaluated in 5-HMF with ethanol at 120 • C for 30 min with a microwave power of 100 W. The 5-HMF conversion was 100% but the total yield of products was 40 to 42%, instead of more humin products being observed. Due to the high acidity of the molyptophosphoric acid, more humin products were formed compared with heterogeneous MPA-KCC-1 and IMPA-KCC-1.
To compare the effect of microwave heating, we evaluated 5-HMF etherification with ethanol in conventional heating using an oil bath with a controlled temperature at 120 • C in an autoclave for 30 and 60 min, with the corresponding results shown in Figure 8. The autoclave was kept in the oil bath after reaching the desired temperature. After 30 or 60 min the autoclave was cooled in cold water immediately. The 5-HMF conversion was 59% and the selectivity of HMFDEA, EMFDEA, and EL was 33%, 61%, and 6%, respectively, for 30 min. However, the conversion was 65% after a 60 min reaction and the EL selectivity increased to 20%. It seems that conventional heating also favors the 5-HMF conversion with a longer time compared with microwave heating. As the time increased, there was noted the formation of humin or charred products. we observed the same effect for tungstophosphoric acid encapsulated KCC-1 silica for carbohydrates to 5-HMF conversion in a microwave assisted reaction condition [32]. The catalytic activity of pure molyptophosphoric acid was evaluated in 5-HMF with ethanol at 120 °C for 30 min with a microwave power of 100 W. The 5-HMF conversion was 100% but the total yield of products was 40 to 42%, instead of more humin products being observed. Due to the high acidity of the molyptophosphoric acid, more humin products were formed compared with heterogeneous MPA-KCC-1 and IMPA-KCC-1. To compare the effect of microwave heating, we evaluated 5-HMF etherification with ethanol in conventional heating using an oil bath with a controlled temperature at 120 °C in an autoclave for 30 and 60 min, with the corresponding results shown in Figure 8. The autoclave was kept in the oil bath after reaching the desired temperature. After 30 or 60 min the autoclave was cooled in cold water immediately. The 5-HMF conversion was 59% and the selectivity of HMFDEA, EMFDEA, and EL was 33%, 61%, and 6%, respectively, for 30 min. However, the conversion was 65% after a 60 min reaction and the EL selectivity increased to 20%. It seems that conventional heating also favors the 5-HMF conversion with a longer time compared with microwave heating. As the time increased, there was noted the formation of humin or charred products.  Reaction conditions: temperature 120 °C, ethanol 5 mL, 25 mg catalyst, 1 mmol of 5-HMF.
Reaction conditions: temperature 120 °C, microwave power 100 W, ethanol 5 mL, 25 mg catalyst, 1 mmol of HMF The effect of time on the 5-HMF conversion and the corresponding selectivity was evaluated at 120 °C; the results are shown in Figure 9. The 5-HMF conversion was increased as the time increased and the selective products of HMFDEA and EMFDEA were also increased. After 30 min, the 5-HMF conversion was decreased due to the reverse reaction of HMFDEA to 5-HMF. The maximum conversion of 75% 5-HMF with 20%, 71%, and 9% selectivity of HMFDEA, EMFDEA, and EL were formed, respectively, at 30 min. Further, the effect of the MPA-KCC-1 catalyst was studied at the different catalytic The effect of time on the 5-HMF conversion and the corresponding selectivity was evaluated at 120 • C; the results are shown in Figure 9. The 5-HMF conversion was increased as the time increased and the selective products of HMFDEA and EMFDEA were also increased. After 30 min, the 5-HMF conversion was decreased due to the reverse reaction of HMFDEA to 5-HMF. The maximum conversion of 75% 5-HMF with 20%, 71%, and 9% selectivity of HMFDEA, EMFDEA, and EL were formed, respectively, at 30 min. Further, the effect of the MPA-KCC-1 catalyst was studied at the different catalytic amounts at the optimum temperature of 120 • C; the results are displayed in Figure 10. The conversion of 5-HMF was 68%, 71%, and 82% for the catalytic amounts of 12.5, 25, and 37.5 mg of MPA-KCC-1, respectively. It reveals that as the catalytic amount increased, the selectivity of HMFDEA reduced from 42% to 12%, whereas the EMFDEA selectivity rose from 58% to 82%. These results suggest that an increase in catalytic amounts improves the EMFDEA selectivity due to more availability of acidic sites. In addition, the efficiency of microwave power was analyzed with varying microwave power ranges from 60 W to 100 W for the MPA-KCC-1 catalyst; the results are shown in Figure 11. The higher catalytic amount (37.5 mg) of MPA-KCC-1 was taken for different microwave power analyses and the reaction was carried out at 120 • C as the optimum temperature. It seems the different microwave powers had no great influence on the conversion of 5-HMF and the selectivity.      Reaction conditions: temperature 120 °C, time 30 min, ethanol 5 mL, 37.5 mg catalyst, 1 mmol of HMF.
The reusability of heterogeneous catalysts is an important industrial characteristic for evaluating the prepared catalyst's long-term catalytic performance. As a result, the reusability was further tested using five catalytic recycling experiments. The recycled experiment was conducted at an optimum parameter of 120 °C, 30 min, 100 W, 5 mL ethanol, and 37.5 mg catalyst with 1 mmol of 5-HMF. The 5-HMF conversion (82 to 75%) and the selectivity were gradually reduced in each cycle, but not too much. For reusability, the MPA-KCC-1 catalyst was filtered using 0.45-micron filter paper. The filtered catalyst was thoroughly washed three times (5 mL each time) with 70% ethanol and dried in an oven at 120 °C for 3 h, and tested for the next cycle. The recycled results are shown in Table 2. After the fifth cycle, the recovered catalyst was analyzed with ICP-OES to check the metal quantity and resulting in 5 to 6% reduced metal concentrations compared with the fresh catalyst. It is due to the metal loss in each cycle during the washing process. The recyclability of the catalyst revealed its superiority as a solid acid catalyst for potential acetylated and etherification reactions. Most researchers have reported the formation of 5-ethoxymethylfurfural (5-EMF) as a major ether product during the reaction of 5-HMF with ethanol [38]. However, in this work, we obtained acylated HMFDEA as a minor and etherified EMFDEA as a major product that would affect the acidic sites of MPA catalysts. Therefore, we generally say that the properties of the catalyst, the reaction conditions, and the acidic sites of the catalytic materials determine the distribution of the reaction products in the 5-HMF conversion.  HMFDEA  EMFDEA  EL  1  82  13  82  5  2  80  12  84  4  3  79  10  83  7  4  73  14  81  3  5  75  12  82  6 Reaction conditions: temperature 120 °C, time 30 min, microwave power 100 W, ethanol 5 mL, 1 mmol of 5-HMF. a The standard deviation of each cycle conversion is ± 2.5. b The standard deviation in the selectivity of each cycle is ±2.5. Reaction conditions: temperature 120 • C, time 30 min, microwave power 100 W, ethanol 5 mL, 1 mmol of HMF.
The reusability of heterogeneous catalysts is an important industrial characteristic for evaluating the prepared catalyst's long-term catalytic performance. As a result, the reusability was further tested using five catalytic recycling experiments. The recycled experiment was conducted at an optimum parameter of 120 • C, 30 min, 100 W, 5 mL ethanol, and 37.5 mg catalyst with 1 mmol of 5-HMF. The 5-HMF conversion (82 to 75%) and the selectivity were gradually reduced in each cycle, but not too much. For reusability, the MPA-KCC-1 catalyst was filtered using 0.45-micron filter paper. The filtered catalyst was thoroughly washed three times (5 mL each time) with 70% ethanol and dried in an oven at 120 • C for 3 h, and tested for the next cycle. The recycled results are shown in Table 2. After the fifth cycle, the recovered catalyst was analyzed with ICP-OES to check the metal quantity and resulting in 5 to 6% reduced metal concentrations compared with the fresh catalyst. It is due to the metal loss in each cycle during the washing process. The recyclability of the catalyst revealed its superiority as a solid acid catalyst for potential acetylated and etherification reactions. Most researchers have reported the formation of 5-ethoxymethylfurfural (5-EMF) as a major ether product during the reaction of 5-HMF with ethanol [38]. However, in this work, we obtained acylated HMFDEA as a minor and etherified EMFDEA as a major product that would affect the acidic sites of MPA catalysts. Therefore, we generally say that the properties of the catalyst, the reaction conditions, and the acidic sites of the catalytic materials determine the distribution of the reaction products in the 5-HMF conversion. Reaction conditions: temperature 120 • C, time 30 min, microwave power 100 W, ethanol 5 mL, 1 mmol of 5-HMF. a The standard deviation of each cycle conversion is ±2. 5. b The standard deviation in the selectivity of each cycle is ±2.5.

Synthesis Procedure of MPA Encapsulated KCC-1
In a 250 mL beaker, 0.0027 mol of cetyltrimethylammonium bromide (CTAB) and 0.01 mol of urea with 100 mL of deionized water were mixed and stirred until the CTAB was completely dissolved. In another 500 mL beaker, a mixed solution of 0.1 mol TEOS and 100 mL p-xylene was stirred for 30 min, then drop by drop, the urea and CTAB mixed solutions were added over 30 min. The mixture of TEOS, p-xylene, CTAB, and urea was stirred for another 25 min with the slow addition of 10 mL of n-pentanol while stirring. The entire solution mixture was exchanged into a 500 mL round-bottom flask. The reaction solution was stirred for 60 min at room temperature. Then the reaction solution was kept in an oil bath and refluxed at 120 • C for 5 h. Next, 1.25 g of MPA solution (20 wt%) was added during reflux and further stirred up for 2 h. After cooling to room temperature, 100 mL of ethanol was added, and the precipitated silica material was filtered using a vacuum with deionized water washing. The filtered product was dried at 100 • C for 12 h and afterward calcined at 450 • C in a tubular furnace with an air atmosphere at a rate of 5 • C min −1 and the calcined material was labeled as MPA-KCC-1. The pure KCC-1 material was synthesized using the same experimental procedure without MPA.
In addition, KCC1 impregnated with 20 wt% MPA was synthesized to compare the activity with that of encapsulated MPA-KCC-1. In a typical synthesis, 0.2 g of MPA was taken in 10 mL of deionized water and mixed with 1 g of KCC-1 in a small 100 mL beaker and stirred up for 20 h, then again heated at 100 • C until dried and kept in calcination at 450 • C in a tubular furnace with an air atmosphere for 10 h at a rate of 5 • C min −1 . After calcination, the obtained material was labeled as IMPA-KCC-1.

Characterizations
High-angle X-ray diffraction (XRD) of pure KCC-1, MPA-KCC-1, and IMPA-KCC-1 were recorded on a Rigaku D/max-2400 apparatus (Qingdao, China) with a step of 0.01 • using Cu-K radiation as the X-ray source. The texture parameters of the samples were analyzed by nitrogen physisorption measurements using a Micromeritics ASAP 2020 (Norcross, GA, USA) porosimeter at a temperature of liquid nitrogen. All the synthesized materials were degassed at 250 • C for 5 h before analysis. Brunauer-Emmett-Teller (BET) and Barrett-Joyner-Halenda (BJH) systems were used to calculate the specific surface area and pore size distributions. The energy dispersive X-ray spectroscopy (EDS) and scanning electron microscopy (SEM) analyses were conducted on a SU8010 scanning electron microscope (Tokyo, Japan) with a resolution of 10 kV. A JOEL 2100F (Tokyo, Japan) at 200 kV was used to obtain the transmission electron microscopy (TEM) images and EDS analysis was carried out with the instrument of Oxford X-MaxN 80 T IE250 (Oxford, UK). The ammonia temperature-programmed desorption analysis (NH 3 -TPD) was performed on a BELCAT B instrument (Osaka, Japan). Fourier transform infrared spectra (FT-IR) were measured, making KBr pellets in an IS10 FTIR spectrometer (ThermoScientific, Waltham, MA, USA). The elemental analysis of the synthesized and recycled catalysts was conducted on a Perkin Elmer spectrometer OES Optima 5300 DV (Wellesley, MA, USA) through inductively coupled plasma optical emission spectroscopy (ICP-OES).

Activity and Product Analysis of Catalysts
The 5-HMF etherification was conducted in a microwave tube (20 mL) with a mixing of 1 mmol 5-HMF and 5 mL ethanol as a reactant and as a solvent in the microwave reactor of a monomodal CEM Discover SP. The reactions were conducted in various catalytic amounts, times, temperatures, and microwave powers. All the reactions were performed in triplicate and the mean deviation of the conversion and selectivity were in the range of ±2 to 2.5. The internal temperature of the microwave was measured by an infrared sensor positioned underneath the microwave cavity. A small amount of the reaction solution was collected and quantitatively measured with gas chromatography linked with a mass spectrometer (GC-MS, Shimadzu QP2020, Kyoto, Japan) with a capillary column of SH-Rxi-5Sil MS (30 m 0.25 mm 0.25 m) at a predetermined period after the reaction had stopped. The program in the GC-MS was initially set to stable for 6 min at 40 • C and thereafter raised to 250 • C at 10 • C min −1 rate with the flow of 1.1 mL min −1 . The MS detector temperature was 230 • C with the electron ionization mode of 70 eV. The interval 35-450 m/z was used to record the MS spectra. The NIST Mass spectral library was utilized to identify the individual compounds.

Conclusions
This research demonstrated the synthesis of a heterogeneous catalyst of encapsulated molybdophosphoric acid in KCC-1 for the microwave etherification of 5-HMF with ethanol. TEM and SEM morphological studies proved the encapsulation of molybdophosphoric acid with KCC-1. The encapsulation of molybdophosphoric acid during synthesis did not affect the materials' spherical morphology and formed uniform unimodal pores (12 nm). The MPA encapsulated catalyst promoted 82% 5-HMF conversion with a 12% and 82% selectivity of HMFDEA and EMFDEA at the optimum conditions. Even the IMPA-KCC-1 catalyst outperformed the MPA-KCC-1 catalyst in terms of catalytic activity but lost the metal sites during reactions, limiting its use as a heterogeneous catalyst. The catalytic activity of 5-HMF with ethanol in the presence of pure MPA formed more humin products due to its high acidity and also the separation of MPA from the reaction mixture would be a tedious process due to its homogeneous nature. It concluded that the encapsulation method builds a highly heterogeneous catalyst and also selectively forms an EMFDEA ether product. The encouraging results obtained in this study will open up new possibilities for the use of 5-HMF to fuel additive synthesis in the biorefinery process using an encapsulated molybdophosphoric acid KCC-1 catalyst.