Skip Content
You are currently on the new version of our website. Access the old version .
MDPIMDPI
Search all articles
CrystalsCrystals
Download PDF
  • Communication
  • Open Access

15 September 2020

Designer Synthesis of Ultra-Fine Fe-LTL Zeolite Nanocrystals

,
,
,
,
,
,
and
1
Institute of Applied Chemistry, Jiangxi Academy of Sciences, Nanchang 330096, China
2
College of Chemistry and Chemical Engineering, Jiangxi Normal University, Nanchang 330022, China
3
Institute of Chemistry, Chinese Academy of Sciences, Beijing 100190, China
*
Author to whom correspondence should be addressed.
Crystals2020, 10(9), 813;https://doi.org/10.3390/cryst10090813
This article belongs to the Special Issue Zeolites
Version Notes
Order Reprints

Abstract

Nanosized zeolites with larger external surface area and decreased diffusion pathway provide many potential opportunities in adsorption, diffusion, and catalytic applications. Herein, we report a designer synthesis of ultra-fine Fe-LTL zeolite nanocrystals under very mild synthesis conditions. We prepared Fe-LTL zeolite nanocrystals synthesized using L precursor. The precursor is aging at room temperature to obtain zeolite L nuclei. In order to investigate more details of Fe-LTL zeolite nanocrystals, various characterizations including X-ray diffraction (XRD), inductively coupled plasma (ICP), diffuse reflectance ultraviolet-visible (UV-Vis) spectroscopy, confirm the tetrahedral Fe3+ species in the zeolite framework. Besides, scanning electron microscope (SEM), Fourier transform infrared spectrometer (FT-IR), dynamic light scattering (DLS) indicate that the average particle size of Fe-LTL zeolite crystals is approximately 30 nm. Thus, ultra-fine Fe-LTL zeolite with large external surface area and shorter diffusion pathway to the active sites might have great potential in the near future.

1. Introduction

Zeolites as promising adsorbents, ion-exchangers, and catalysts have been widely used in the fields of catalysis, separations, and adsorption [1,2,3,4,5,6,7,8,9,10,11,12,13,14]. In particular, they have accelerated the development of heterogeneous catalysis and separation processes because of their large internal surface area, unique channel systems, high pore volume, and adjustable active sites. The chemical composition and pore architecture of zeolites are important, however, the precise control of their crystallite morphology also has a significant influence on their applications in catalysis and adsorption. As the crystal size decreases below 100 nm, the zeolite external surface area, which is distinct from the internal pore surface and is negligible for micron-sized zeolites, increases dramatically, resulting in zeolites with over 25% of the total surface area on the external surface [15]. Shorter diffusion path length of nanosized zeolites is another advantage compared to micron-sized zeolites. The improved properties of nanosized zeolites for adsorption and diffusion provide many potential opportunities for their applications in environmental catalysis, environmental remediation, decontamination, and drug delivery [16]. Thus, zeolite nanocrystals have been paid much attention because of their widespread applications, the strategies for the preparation of zeolite nanocrystals are necessary and important [17,18,19,20,21]. Nonetheless, designer synthesis of pure zeolite nanocrystals is still challenging at present.
The structure of zeolite LTL is hexagonal (space group P6/mmm) with unit cell constants a = 18.4 Å and c = 7.5 Å [22]. The linkages of the cancrinite cages by double 6-rings (D6R) lead to the formation of columns in the c-direction and thus give rise to 12-membered rings with a free diameter of 7.1 Å [23]. Over past 20 years, zeolite L has drawn much attention for their applications in catalytic processes [24,25,26,27], ion-exchange and separations [28,29], and photonic devices [30,31]. Notably, iron catalysts, supported on different solids, have been widely applied in Fischer-Tropsch reaction for many years. Combining the advantages of iron and LTL zeolites, it is very meaningful to synthesize ultra-fine Fe-LTL zeolite nanocrystals, which are potentially significant for catalytic applications.
Herein, we report a designer synthesis of ultra-fine Fe-LTL zeolite nanocrystals under very mild synthesis conditions. We prepared Fe-LTL zeolite nanocrystals synthesized using L precursor. The precursor is aging at room temperature to obtain zeolite L nuclei. Notably, the average crystal size of Fe-LTL zeolite nanocrystals we obtained is approximately 30 nm, which is smaller than the previous reports. In order to investigate more details of Fe-LTL zeolite nanocrystals, various characterizations including X-ray diffraction (XRD), diffuse reflectance ultraviolet-visible (UV-Vis) spectroscopy, confirm the tetrahedral Fe3+ species in the zeolite framework. Besides, scanning electron microscope (SEM), Fourier transform infrared spectrometer (FT-IR), dynamic light scattering (DLS) indicate the nanoscale of zeolite crystals. Ultra-fine Fe-LTL zeolite with large external surface area and shorter diffusion pathway to the active sites might have great potential in the near future.

2. Materials and Methods

2.1. Materials

The following chemicals were utilized: sodium aluminate (NaAlO2, 36.6% Na2O, and 43.3% Al2O3, Sinopharm Chemical Reagent Co., Ltd., Shanghai, China), sodium hydroxide (NaOH, AR, 96%, Sinopharm Chemical Reagent Co., Ltd., Shanghai, China), potassium hydroxide (KOH, AR, 85%, Sinopharm Chemical Reagent Co., Ltd., Shanghai, China), silica sol (LUDOX HS-40, 40% SiO2 in water, Sigma Aldrich, St. Louis, MO, USA), aluminum sulfate (Al2(SO4)3⋅18H2O, AR, 99%, Sinopharm Chemical Reagent Co., Ltd., Shanghai, China), sodium silicate solution (253.8 g/L SiO2, 77.8 g/L Na2O of 1 L sodium silicate solution), ferric chloride hexahydrate (FeCl3⋅6H2O, AR, Sinopharm Chemical Reagent Co., Ltd., Shanghai, China)

2.1.1. Synthesis of Zeolite L Precursor

As a typical run, zeolite L precursor was prepared by mixing 10 mL deionized H2O, 0.472 g sodium aluminate and 3.76 g potassium hydroxide under stirring for 10 min, 8.4 g silica sol was added later. After the solution was stirred for 1 h, 0.24 g sodium hydroxide was finally added, followed by aging at room temperature for 72 h, giving a clear solution. The molar ratio of the precursor is 3.0Na2O/14.3K2O/Al2O3/28SiO2/413H2O.

2.1.2. Synthesis of Fe-L Samples

Zeolite Fe-L nanocrystals were hydrothermally synthesized at the temperature of 80 °C for 3 days with 2.1Na2O/3.4K2O/Al2O3/15SiO2/0.6FeCl3/250H2O molar ratios of initial synthesis gels in the presence of zeolite L precursor. As a typical run, 1.16 g potassium hydroxide was added to 10.9 g sodium silicate solution, followed by introducing 1.4 g deionized H2O. After stirring for about 1 h, 1.665 g aluminum sulfate was added to the mixture, followed by the addition of 0.4 g FeCl3⋅6H2O, finally the last addition of 2.0 mL zeolite L precursor. After being stirred for 2 h at room temperature, the mixture was transferred into an autoclave to crystallize at 80 °C for 3 days. The products were collected by filtration, washed with deionized H2O, and dried in air, respectively. The H-form of the samples was prepared by triple ion-exchange with 1M of NH4NO3 solution at 80 °C for 1 h and calcination at 550 °C for 5 h.

2.1.3. Synthesis of Conventional Fe-L Zeolite

Conventional Fe-L crystal was hydrothermally synthesized at the temperature of 180 °C for 1 day with 1.56K2O/Al/6.25SiO2/0.25FeCl3/90H2O molar ratios of starting gels. The product was collected by filtration, washed with deionized H2O, and dried in air. The H-form of the sample was prepared by triple ion-exchange with 1M of NH4NO3 solution at 80 °C for 1 h and calcination at 550 °C for 5 h.

2.2. Methods

Powder X-ray diffraction (XRD) (Rigaku, Tokoyo, Japan) data were experimented at room temperature with a Rigaku Ultimate VI X-ray diffractometer (40 kV, 40 mA) using CuKα (λ = 1.5406 Å) radiation. Crystallinity of samples is calculated by area of peaks at 5.7°, 19°, 22°, and 28° from the XRD patterns. Scanning electron microscopy (SEM) (Hitachi, Tokoyo, Japan) experiments were carried out on Hitachi SU-8010 and SU-1510 electron microscopes. Dynamic light scattering (DLS) (Malvern, Malvern City, UK) experiments were measured using a Malvern Instrument Zetasizer Nano ZS90. Nitrogen sorption experiments (Micromeritics, Atlanta, GA, USA) were performed on a Micromeritics TriStar II at −196 °C. The pore volume and surface area were calculated using the t-plot and BET methods. UV-Vis analysis, using BaSO4 as the internal standard sample was performed on a Perkin-Elmer Lambda 20 spectrometer (Perkin Elmer, Waltham, MA, USA). Fourier transform infrared spectrometer (FT-IR) was measured on a FTIR 7600 Spectrometer (Lambda, Sydney, Australia). The sample composition was tested by ICP with a Perkin-Elmer 3300DV emission spectrometer.

3. Results and Discussion

Figure 1a–d shows the XRD patterns of as-synthesized and calcined Fe-LTL nanocrystals (Fe-LTL-N), conventional Fe-LTL (Fe-LTL-C), and calcined Fe-LTL-N, Fe-LTL-C samples. These samples give a series of characteristic peaks of the LTL framework structure. The peaks of Fe-LTL-N are broader than those of Fe-LTL-C, indicating the crystal size of Fe-LTL-N samples is nanoscale. After calcination, these peaks are basically remained, indicating their good thermal stability.
Figure 1. XRD patterns of (a) as-synthesized Fe-LTL-N, (b) calcined Fe-LTL-N, (c) as-synthesized Fe-LTL-C, (d) calcined Fe-LTL-C, respectively.
Figure 2 gives the SEM images of as-synthesized Fe-LTL-N, Fe-LTL-C samples. Figure 2a exhibits nanocylindrical morphology of Fe-LTL-N with size of 20–50 nm, while the morphology of Fe-LTL-C is micron cylindrical (Figure 2b). It is well consistent with the result from XRD testing of Fe-LTL-N and Fe-LTL-C samples. The particle size distribution (Figure 3) shows the average particle size of Fe-LTL-N is 30 nm. Notably, agglomeration of Fe-LTL-N is also exhibited in Figure 2a. Zeolite nanocrystals with smaller sizes have higher relative surface area and higher energy. To minimize its surface energy the nanocrystals create agglomeration.
Figure 2. SEM images of as-synthesized (a) Fe-LTL-N, (b) Fe-LTL-C.
Figure 3. DLS curve of as-synthesized Fe-LTL-N.
The porosity and specific surface area of Fe-LTL-N and Fe-LTL-C samples were characterized by nitrogen adsorption measurement (Figure 4a,b), which displays the related parameters, as shown in Table 1. Fe-LTL-N sample shows a mixed isotherm curve of Type I and IV with a large H1-type hysteresis. As the Table 1 shows, the total pore volume of Fe-LTL-N is 0.38 cm3g−1, while the conventional Fe-LTL zeolite shows relatively low pore volume at only 0.19 cm3g−1. The results are consistent with that of XRD patterns and SEM images.
Figure 4. N2 isotherm sorption of (a) Fe-LTL-N, (b) Fe-LTL-C.
Table 1. Textural parameters of Fe-LTL samples.
Figure 5 displays the UV-vis spectrum of Fe-LTL-N, exhibiting a strong absorption band at 220 nm with a distinct shoulder at 245 nm and weak bands at 379, 419, and 446 nm, which is in good agreement with the previously reported results [32]. Both bands in the 220–250 nm range correspond to tetrahedral Fe in the zeolite, where the band at 220 nm may be due to a different specific environment of Fe within the zeolite framework. The absorption bands located at 379, 419, and 446 nm are assigned to tetrahedral Fe3+ in the zeolite framework [33]. There were no obvious absorption peaks at near 320 nm, indicating the absence of aggregated FeOx species in the extra-framework.
Figure 5. UV-vis spectrum of as-synthesized Fe-LTL-N.
Table 2 presents a systematic investigation on crystallization of Fe-LTL zeolite nanocrystals at 80 °C from aluminosilicate gels in the presence of L precursor. Interestingly, when the K2O/SiO2 in the gels is optimized from 0.122 to 0.300, products of amorphous phase are obtained such as, a mixture of amorphous phase with LTL structure, pure LTL, a mixture of LTL and amorphous (Figure 6A). However, as the K2O/SiO2 ratio in the synthesis gel increases, there is significant broadening and a decrease in height for peaks. Notably, sample obtained under Run 6 with poorer crystallinity shows decrease in height of resolved IR spectrum compared with Fe-LTL-N sample (Figure S1). Combined with the XRD pattern of sample (Run 6), it is probably a mixture of LTL and amorphous [34]. Moreover, the suitable K2O/SiO2 ratio for crystallization of pure LTL structure is changed from 0.229 to 0.265. It is found that the SiO2/Al2O3 ratio has a great influence on the crystallization of LTL zeolite. When the SiO2/Al2O3 ratio is less than 15, it is normally amorphous phase. When this ratio is distributed in the range of 15–25, a pure phase of LTL structure is usually formed (Figure 6B). Figure S1 also shows resolved IR spectra of samples obtained under conditions of Run 10 and 11. Obviously, sample (Run 10) gives similar IR spectrum as that of sample (Run 6), while sample (Run 11) has a further decrease in height for the peaks. Therefore, the sample synthesized under Run 10 and 11 are probably mixture of LTL and amorphous. Furthermore, the FeCl3/SiO2 ratio also influences the crystallization of Fe-LTL zeolite. The Fe content and Si/Al ratios of samples is listed in Table 3. Clearly, samples obtained with more iron content in the initial gel are likely to exhibit higher iron content and Si/Al ratios. As the Figure 6C shows, the increase of iron content up to a certain amount in the initial synthesis gels tends to produce samples with lower crystallinity. When this ratio in the initial gel reaches to 0.07, it is formed a mixture of LTL with amorphous. It has been claimed that the presence of greater concentrations of iron in the gel inhibited the formation of the cancrinite cage due to the larger Fe-O bond length compared to Al-O [34]. Moreover, cancrinite cage is crucial in the formation of LTL zeolites. Thus, the amount of iron in the synthesis gels really has a major impact on crystallinity of Fe-LTL zeolites. Moreover, crystallization temperature has a great effect on the crystallization of zeolite crystals. Figure 7 shows the XRD patterns of Fe-LTL zeolite nanocrystals synthesized with the same ratios of Run 4 at different crystallization temperatures. Reasonably, higher crystallization of Fe-LTL zeolites tends to be obtained at higher crystallization temperatures.
Table 2. Impact of synthesis conditions on crystallization of Fe-LTL zeolite nanocrystals (Na2O/SiO2 = 0.14, H2O/SiO2 = 250, at 80 °C for 3 d).
Figure 6. XRD patterns of Fe-LTL zeolite crystals synthesized under various conditions in Table 2. (A) XRD patterns of Fe-LTL zeolite crystals synthesized with different K2O/SiO2 ratios; (B) XRD patterns of Fe-LTL zeolite crystals synthesized with different SiO2/Al2O3 ratios; (C) XRD patterns of Fe-LTL zeolite crystals synthesized with different FeCl3/SiO2 ratios.
Table 3. Fe/Si and Si/Al ratios of different samples.
Figure 7. XRD patterns of Fe-LTL zeolite crystals synthesized at (a) 80 °C, (b) 100 °C, (c) 120 °C, (d) 140 °C, (e) 160 °C, (f) 180 °C, respectively.
After the systematic synthesis, aluminosilicate gel for crystallization of Fe-LTL zeolites at 80 °C with molar ratio of 2.1Na2O/3.4K2O/Al2O3/15SiO2/0.6FeCl3/250H2O is suitable.

4. Conclusions

In summary, we have successfully synthesized ultra-fine Fe-LTL zeolite nanocrystals under very mild synthesis conditions. The average particle size of Fe-LTL zeolite nanocrystals is approximately 30 nm. Moreover, Fe-LTL-N zeolites that we obtained have advantages of larger external surface area, shorter diffusion pathway, good thermal stability, narrow particle distribution. Very importantly, tetrahedral Fe3+ is located in the zeolite framework of Fe-LTL-N. Designer synthesis of ultra-fine Fe-LTL zeolite nanocrystals in this work has significant potential applications for industrial catalysis in the near future.

Supplementary Materials

The following are available online at https://www.mdpi.com/2073-4352/10/9/813/s1, Figure S1: IR spectra of Fe-LTL zeolite crystals synthesized under various conditions in Table 2.

Author Contributions

Conceptualization and writing, F.Z.; methodology, Y.L., L.C. and G.C.; investigation, W.C., Y.H., S.Y., and W.S. All authors have read and agreed to the published version of the manuscript.

Funding

This research was funded by the Jiangxi Provincial Natural Science Foundation (20202ACB203003), the Science and Technology Program of Jiangxi Academy of Sciences (2020-YZD-3, 2019-XTPH1-09, 2019-YYB-09, 2018-YDHZ-01).

Conflicts of Interest

The authors declare no conflict of interest.

References

  1. Davis, M.E.; Lobo, R.F. Zeolite and molecular sieve synthesis. Chemistry of Materials. Chem. Mater. 1992, 4, 756–768. [Google Scholar] [CrossRef]
  2. Gies, H.; Marler, B. The structure-controlling role of organic templates for the synthesis of porosils in the system SiO2/template/H2O. Zeolite 1992, 12, 42–49. [Google Scholar] [CrossRef]
  3. Davis, M.E. Ordered porous materials for emerging applications. Nature 2002, 417, 813–821. [Google Scholar] [CrossRef]
  4. Cundy, C.S.; Cox, P.A. The hydrothermal synthesis of zeolites: History and development from the earliest days to the present time. Chem. Rev. 2003, 103, 663–702. [Google Scholar] [CrossRef] [PubMed]
  5. Zou, X.; Conradsson, T.; Klingstedt, M.; Dadachov, M.S.; O’Keeffe, M. A mesoporous germanium oxide with crystalline pore walls and its chiral derivative. Nature 2005, 437, 716–719. [Google Scholar] [CrossRef] [PubMed]
  6. Ma, S.Q.; Sun, D.F.; Wang, X.S.; Zhou, H.C. A mesh-adjustable molecular sieve for general use in gas separation. Angew. Chem. Int. Ed. 2007, 46, 2458–2462. [Google Scholar] [CrossRef] [PubMed]
  7. Shin, J.; Camblor, M.A.; Woo, H.C.; Miller, S.R.; Wright, P.A.; Hong, S.B. PST-1: A synthetic small-pore zeolite that selectively adsorbs H2. Angew. Chem. Int. Ed. 2009, 48, 6647–6650. [Google Scholar] [CrossRef] [PubMed]
  8. Lee, J.H.; Park, M.B.; Lee, J.K.; Min, H.K.; Song, M.K.; Hong, S.B. Synthesis and characterization of ERI-type UZM-12 zeolites and their methanol-to-olefin performance. J. Am. Chem. Soc. 2010, 132, 12971–12982. [Google Scholar] [CrossRef]
  9. Na, K.; Jo, C.; Kim, J.; Cho, K.; Jung, J.; Seo, Y.; Messinger, R.J.; Chmelka, B.F.; Ryoo, R. Directing zeolite structures into hierarchically nanoporous architectures. Science 2011, 333, 328–332. [Google Scholar] [CrossRef] [PubMed]
  10. Zhang, X.Y.; Liu, D.X.; Xu, D.D.; Asahina, S.; Cychosz, K.A.; Agrawal, K.V.; Al Wahedi, Y.; Bhan, A.; Al Hashimi, S.; Terasaki, O.; et al. Synthesis of self-pillared zeolite nanosheets by repetitive branching. Science 2012, 336, 1684–1687. [Google Scholar] [CrossRef]
  11. Goel, S.; Wu, Z.J.; Zones, S.I.; Iglesia, E. Synthesis and catalytic properties of metal clusters encapsulated within small-pore (SOD, GIS, ANA) zeolites. J. Am. Chem. Soc. 2012, 134, 17688–17695. [Google Scholar] [CrossRef]
  12. Jo, C.; Jung, J.; Shin, H.S.; Kim, J.; Ryoo, R. Capping with Multivalent Surfactants for Zeolite Nanocrystal Synthesis. Angew. Chem. Int. Ed. 2013, 52, 10014–10017. [Google Scholar] [CrossRef]
  13. Moller, K.; Bein, T. Mesoporosity-a new dimension for zeolites. Chem. Soc. Rev. 2013, 42, 3689–3707. [Google Scholar] [CrossRef] [PubMed]
  14. Bian, C.Q.; Wang, X.; Yu, L.; Zhang, F.; Zhang, J.; Fei, Z.X.; Qiu, J.P.; Zhu, L.F. Generalized methodology for inserting metal heteroatoms into the layered zeolite precursor RUB-36 by interlayer expansion. Crystals 2020, 10, 530. [Google Scholar] [CrossRef]
  15. Song, W.; Justice, R.E.; Jones, C.A.; Grassian, V.H.; Larsen, S.C. Size-dependent properties of nanocrystalline silicalite synthesized with systematically varied crystal sizes. Langmuir 2004, 20, 4696–4702. [Google Scholar] [CrossRef] [PubMed]
  16. Larsen, S.C. Nanocrystalline zeolites and zeolite structures: Synthesis, characterization, and applications. J. Phys. Chem. C 2007, 111, 18464–18474. [Google Scholar] [CrossRef]
  17. Choi, M.; Na, K.; Kim, J.; Sakamoto, Y.; Terasaki, O.; Ryoo, R. Stable single-unit-cell nanosheets of zeolite MFI as active and long-lived catalysts. Nature 2009, 461, 246–249. [Google Scholar] [CrossRef]
  18. Eng-Poh, N.; Chateigner, D.; Bein, T.; Valtchev, V.; Mintova, S. Capturing ultrasmall EMT zeolite from template-free systems. Science 2012, 335, 70–73. [Google Scholar]
  19. Feng, G.D.; Cheng, P.; Yan, W.F.; Boronat, M.; Li, X.; Su, J.H.; Wang, J.Y.; Li, Y.; Corma, A.; Xu, R.R. Accelerated crystallization of zeolites via hydroxyl free radicals. Science 2016, 351, 1188–1191. [Google Scholar] [CrossRef]
  20. Chen, W.; Fan, Z.L.; Pan, X.L.; Bao, X.H. Effect of confinement in carbon nanotubes on the activity of Fischer-Tropsch iron catalyst. J. Am. Chem. Soc. 2008, 130, 9414–9419. [Google Scholar] [CrossRef]
  21. Awala, H.; Gilson, J.-P.; Retoux, R.; Boullay, P.; Goupil, J.-M.; Valtchev, V.; Mintova, S. Template-free nanosized faujasite-type zeolites. Nat. Mater. 2015, 14, 447–451. [Google Scholar] [CrossRef] [PubMed]
  22. Ohsuna, T.; Horikawa, Y.; Hiraga, K.; Terasaki, O. Surface Structure of Zeolite L Studied by High-Resolution Electron Microscopy. Chem. Mater. 1998, 10, 688–691. [Google Scholar] [CrossRef]
  23. Laulus, O.; Valtchev, V.P. Crystal morphology control of LTL-type zeolite crystals. Chem. Mater. 2004, 16, 3381–3389. [Google Scholar]
  24. Davis, R.J. Aromatization on zeolite L-supported Pt clusters. Heterogen. Chem. Rev. 1994, 1, 41–53. [Google Scholar]
  25. Joshi, P.N.; Bandyopadhyay, R.; Awate, S.V.; Shiralkar, V.P.; Rao, B.S. Influence of physicochemical parameters on n-hexane dehydrocyclization over Pt/LTL zeolites. React. Kinet. Catal. Lett. 1994, 53, 231–236. [Google Scholar] [CrossRef]
  26. Jentoft, R.E.; Tsapatsis, M.; Davis, M.E.; Gates, B.C. Platinum clusters supported in zeolite LTL: Influence of catalyst morphology on performance in n-hexane reforming. J. Catal. 1998, 179, 565–580. [Google Scholar] [CrossRef]
  27. Miller, J.T.; Agrawal, N.G.B.; Lane, G.S.; Modica, F.S. Effect of pore geometry on ring closure selectivities in platinum L-zeolite dehydrocyclization catalysts. J. Catal. 1996, 163, 106–116. [Google Scholar] [CrossRef]
  28. Barrer, R.M.; Galabova, I.M. Ion-exchanged forms of zeolite L, erionite, and offretite and sorption of inert-gases. Adv. Chem. Ser. 1973, 356–373. [Google Scholar] [CrossRef]
  29. Lee, T.P.; Saad, B.; Ng, E.P.; Salleh, B. Zeolite linde type L as micro-solid phase extraction sorbent for the high performance liquid chromatography determination of ochratoxin A in coffee and cereal. J. Chromatogr. A 2012, 1237, 46–54. [Google Scholar] [CrossRef]
  30. Calzaferri, G.; Huber, S.; Maas, H.; Minkowski, C. Host–Guest Antenna Materials. Angew. Chem. Int. Ed. 2003, 42, 3732–3735. [Google Scholar] [CrossRef]
  31. Gigli, L.; Arletti, R.; Tabacchi, G.; Fabbiani, M.; Vitillo, J.G.; Martra, G.; Devaux, A.; Miletto, I.; Quartieri, S.; Calzaferri, G. Structure and host-guest interactions of perylene-diimide dyes in zeolite L nanochannels. J. Phys. Chem. C. 2018, 122, 3401–3418. [Google Scholar] [CrossRef]
  32. Goldfarb, D.; Bernado, M.; Strohmaier, K.G.; Vaughan, D.E.W.; Thomann, H. Characterization of iron in zeolites by X-band and Q-band ESR, pulsed ESR, and UV-visible spectroscopies. J. Am. Chem. Soc. 1994, 116, 6344–6353. [Google Scholar] [CrossRef]
  33. Zhang, H.; Chu, L.; Xiao, Q.; Zhu, L.; Yang, C.; Meng, X.; Xiao, F.-S. One-pot synthesis of Fe-Beta zeolite by an organotemplate-free and seed-directed route. J. Mater. Chem. A 2013, 1, 3254–3257. [Google Scholar] [CrossRef]
  34. Camblor, M.A.; Corma, A.; Mifsud, A.; Perez-Pariente, J. Valencia, Synthesis of nanocrystalline zeolite Beta in the absence of alkali metal cations. Stud. Surf. Sci. Catal. 1997, 105, 341–348. [Google Scholar]

Article Metrics

Citations

Article Access Statistics

Journal Statistics
Multiple requests from the same IP address are counted as one view.
Download PDF
Convective Transport of Fluid–Solid Interaction: A Study between Non-Newtonian Casson Model with Dust Particles
Previous
Effects of Highly Crystalized Nano C-S-H Particles on Performances of Portland Cement Paste and Its Mechanism
Next