The porosity and water vapor sorption property of commercially available hydrophobic SiO2beads were investigated. The hydrophobic SiO2 beads, the surface of which has been modified by trimethylsilyl functional groups, with a surface area of 70.7 m2/g, a mesopore diameter of about 36 nm and a mesopore volume of about 0.91 cm3/g showed lower water vapor sorption property as compared to the unmodified SiO2 beads; the amount of monolayer water adsorbed were estimated to be 2.94×10-3 and 5.12×10-3 g(H2O)/g(adsorbent) for hydrophobic and unmodified SiO2 beads, respectively. The evaluation of the heat of water vapor sorption suggests that the suppression of water cluster formation by trimethylsilyl groups is attributed to the hydrophobic property

古藤 健司

宗像 健三

杉山 貴彦

森田 洋平

田中 将裕

田口 明

application/pdfThe porosity and water vapor sorption property of commercially available hydrophobic SiO2beads were investigated. The hydrophobic SiO2 beads, the surface of which has been modified by trimethylsilyl functional groups, with a surface area of 70.7 m2/g, a mesopore diameter of about 36 nm and a mesopore volume of about 0.91 cm3/g showed lower water vapor sorption property as compared to the unmodified SiO2 beads; the amount of monolayer water adsorbed were estimated to be 2.94×10-3 and 5.12×10-3 g(H2O)/g(adsorbent) for hydrophobic and unmodified SiO2 beads, respectively. The evaluation of the heat of water vapor sorption suggests that the suppression of water cluster formation by trimethylsilyl groups is attributed to the hydrophobic property.Article富山大学水素同位体科学研究センター研究報告, 33巻, 2014.06.30, pp.45-51departmental bulletin pape

田口, 明

杉山, 貴彦

森田, 洋平

田中, 将裕

古藤, 健司

宗像, 健三

University of Toyama Repository

 5HVHDUFK1RWH&(&( ゐ፹⏝␯Ỉᛶࢩࣜ࢝ࣅ࣮ࢬࡢ⣽Ꮝᵓ㐀ཬࡧỈ⵨Ẽ྾╔≉ᛶ⏣ཱྀ ᫂ 1䠈ᮡᒣ㈗ᙪ 2䠈᳃⏣ὒᖹ 2䠈⏣୰ᑗ⿱ 3䠈ྂ⸨೺ྖ 4䠈᐀ീ೺୕ 5  1ᐩᒣ኱ᏛỈ⣲ྠ఩య⛉Ꮫ◊✲䝉䞁䝍䞊㻌   ᐩᒣᕷ஬⚟ ྡྂᒇ኱Ꮫ኱Ꮫ㝔ᕤᏛ◊✲⛉ྡྂᒇᕷ༓✀༊୙⪁⏫᰾⼥ྜ⛉Ꮫ◊✲ᡤᒱ㜧┴ᅵᒱᕷୗ▼⏫㸱㸰㸰Ѹ㸴஑ᕞ኱Ꮫ኱Ꮫ㝔ᕤᏛ◊✲㝔 ⚟ᒸᕷす༊ඖᒸ㸵㸲㸲␒ᆅ⛅⏣኱ᏛᕤᏛ㈨※Ꮫ㒊 ⛅⏣ᕷᡭᙧᏛᅬ⏫㸯㸫㸯Porosity and water vapor sorption property of new hydrophobic silica beads  for CECE catalyst support Akira Taguchi1, Takahiko Sugiyama2, Yohei Morita2, Masahiro Tanaka3, Kenji Kotoh4,  Kenzo Munakata5  1Hydrogen Isotope Research Center, University of Toyama  Gofuku 3190, Toyama 930-8555 2Graduate School of Engineering and School of Engineering, Nagoya University Furo-cho, Chikusa-ku, Nagoya 464-8603 3National Institute for Fusion Science Oroshi-Cho 322-6, Toki 509-5292 4Graduate School of Engineering, Kyushu University Motooka Nishi-ku 744, Fukuoka 819-0395 ᐩᒣ኱ᏛỈ⣲ྠ఩య⛉Ꮫ◊✲ࢭࣥࢱ࣮◊✲ሗ࿌33㸸㸪 5Department Faculty of Engineering and Resource Science, Akita University Tegata gakuen-machi 1-1, Akita 010-8502  (Received December 17, 2013; May 23, 2014)  	The porosity and water vapor sorption property of commercially available hydrophobic SiO2 beads were investigated. The hydrophobic SiO2 beads, the surface of which has been modified by trimethylsilyl functional groups, with a surface area of 70.7 m2/g, a mesopore diameter of about 36 nm and a mesopore volume of about 0.91 cm3/g showed lower water vapor sorption property as compared to the unmodified SiO2 beads; the amount of monolayer water adsorbed were estimated to be 2.94×10-3 and 5.12×10-3 g(H2O)/g(adsorbent) for hydrophobic and unmodified SiO2 beads, respectively. The evaluation of the heat of water vapor sorption suggests that the suppression of water cluster formation by trimethylsilyl groups is attributed to the hydrophobic property.  	  The combined electrolysis catalytic exchange (CECE) method is a practical process for the enrichment of heavy water and the extraction of tritium from light and heavy water mixtures.[1-3] From the development of the CECE process and afterwards, much effort has been devoted to improve the catalytic activity, design of the catalyst bed, and operation parameters.[1,4,5] One of the CECE catalysts commercially available at the present is the styrene-divinylbenzene copolymer supported Pt catalyst which has been known as the Kogel catalyst.[1,3-5] Although the superior activity and life time with satisfactory operating results of the Kogel catalyst have been well known, one problem is the difficulty in its mass production and hence a high price. Therefore, the development of a new preparation method with improved activity is still an interesting task.   From these backgrounds, we started our attempt at preparing a new CECE catalyst from commercially available, relatively cheap materials such as SiO2, Al2O3 and activated carbon. Among the several physical and chemical properties required for a CECE catalyst support, such as porosity, water resistance, and hardness, one of the most important properties is hydrophobicity.[1,4,5] Although the hydrophobic/hydrophilic property is difficult to define quantitatively [6], it has been known that hydrophilic CECE catalysts easily cause pore blocking due to the condensation of water vapor, resulting in the decrease in catalytic activity.[1,4,5] We ⏣ཱྀ࣭᫂ᮡᒣ㈗ᙪ࣭᳃⏣ὒᖹ࣭⏣୰ᑗ⿱࣭ྂ⸨೺ྖ࣭᐀ീ೺୕ have chosen hydrophobic SiO2 beads (Fuji Silysia Chemical Ltd., Aichi), denoted as SiO2B, for use as the catalyst support in a new CECE catalyst system. In this note, we report some fundamental properties of SiO2B, especially focusing on water vapor sorption properties in addition to other pore structural properties. As a reference material, SiO2 beads (CARiACT-Q50, Fuji Silysia, denoted as SiO2BH2O) were used in this study. This SiO2BH2O was the parent material for SiO2B, which had trimethylsilyl functional groups grafted on the surface (grafting density of 1.2 – 1.8 groups/nm2 in catalog). It should be noted that SiO2BH2O also shows hydrophobicity, since it is composed of pure silica [6], which excludes Al3+ or related counter-cations of Na+ or Ca2+ as is the case with hydrophilic silica gel or zeolite molecular sieves.   Fig. 1 shows the SEM image of SiO2B and the optical photo of SiO2B and SiO2BH2O. The color of these beads was white and the diameter was about 2.4 – 4.1 mm (Fig.1 inset). The SEM measurements (JSM-6701F, JEOL) revealed that SiO2B possessed textural pores with the diameter of several tens of nanometers. These pores existed as continuous wormhole-like structures in a SiO2 framework.   Nitrogen sorption isotherms were measured by using Autosorb-1MP (Quantachrome) at -196 ºC. The samples were evacuated previously at 200 ºC for more than 12 h. Brunauer–Emmett–Teller surface area (S.A.) were found to be 70.7 and 76.2 m2/g for SiO2B and SiO2BH2O, respectively. Both SiO2B and SiO2BH2O showed a type V isotherm as shown in Fig. 2 [7]; the sorption capacity was small in low and middle P/P0 ranges, and then suddenly increased at higher P/P0. This suggested that unrestricted monolayer-multilayer adsorption could occur.[7,8] Indeed, the micropore volumes (Vpmicro) below a P/P0 of 0.205, corresponding to the pore  N2 sorption isotherm of SiO2B and SiO2BH2O. Inset: Barrett-Joyner-Halenda (BJH) pore size distribution of SiO2B and SiO2BH2O evaluated from the desorption branch. Symbols are circle for SiO2B and triangle for SiO2BH2O, respectively.   SEM image of SiO2B. Inset: Appearance of SiO2B and SiO2BH2O.  &(&(ゐ፹⏝␯Ỉᛶࢩࣜ࢝ࣅ࣮ࢬࡢ⣽Ꮝᵓ㐀ཬࡧỈ⵨Ẽ྾╔≉ᛶ diameter of 2.1 nm, were 0.030 and 0.034 cm3/g for SiO2B and SiO2BH2O, respectively (Table 1). On the other hand, the pore volume in the region between 0.205 and 0.957, corresponding to the mesopore diameter of 2.1 to 47 nm (Vpmeso), were found to be 0.176 and 0.187 cm3/g, respectively, and larger than Vpmicro. The Barrett-Joyner-Halenda (BJH) pore size distribution curve (desorption branch) also revealed that most of the pores had sizes in the range of 30 – 60 nm (Fig. 2, inset), which was consistent with SEM measurements. The pore diameter (Dp) was found to be 49.0 and 63.3 nm for SiO2B and SiO2BH2O, respectively. However, these high P/P0 region is excluded from the applicability of the N2 sorption study [8]. Therefore, we investigated the pore size distribution using mercury porosimetry (AutoPore IV 9510, Micromeritics). Fig. 3 shows the pore size distribution curves of SiO2B and SiO2BH2O and the cumulative intrusion of Hg (inset). It is clearly seen that both SiO2B and SiO2BH2O possess mesopores with the pore diameter of 36 and 37 nm, respectively, which are smaller than the ones from the BJH pore size distribution [8]. The pore volumes of the mesopore (Vpmeso, 2.0 – 50 nm) and macropore (Vpmacro, 50  414 nm) regions were listed in Table 1. It was revealed that both SiO2B and SiO2BH2O were mesopore-rich materials. This finding is consistent with the SEM image (Fig. 1). From these data, we have determined the S.A., Dp and Vpmeso of SiO2B were 70.7 m2/g, 36 nm, and 0.909 cm3/g, respectively.   Water vapor sorption isotherms were measured with Hydrosorb1000 (Quantachrome). The samples were previously heated in vacuum at 200 ºC for more than 12 h. Water vapor sorption isotherms (25 ºC) are shown in Fig. 4 and corresponding BET plots are shown in Fig. 4 inset. The adsorption capacity close to saturation was about 0.50 mmol/g for SiO2B, while it was   Pore size distribution of (circle) SiO2B and (triangle) SiO2BH2O obtained by mercury porosimetry. Inset: cumulative intrusion of Hg.  Table 1 Summary of sorption study of SiO2B and SiO2BH2O. SiO2BSiO2BH2ON2 sorption Hg porosimetryH2O vapor sorption25 ºC (BET constant)S.A.[m2/g]70.776.2Dp[nm]49.063.3Vpmicro[cm3/g]0.0300.034Vpmeso[cm3/g]0.1760.187Dp[nm]3637Vpmeso[cm3/g]0.9090.934Vpmacro[cm3/g]0.0590.050wm[g(H2O)/g]2.94  10-35.12  10-3C[]7.675.36⏣ཱྀ࣭᫂ᮡᒣ㈗ᙪ࣭᳃⏣ὒᖹ࣭⏣୰ᑗ⿱࣭ྂ⸨೺ྖ࣭᐀ീ೺୕ more than 1.94 mmol/g for SiO2BH2O. For SiO2BH2O, the amount of water vapor increased gradually at P/P0 < 0.7, and the amount adsorbed steeply increased at P/P0 larger than 0.8. Such a steep increase can be attributed to the formation of water clusters as will discuss below. Also, substantial hysteresis was observed in the desorption branch of SiO2BH2O. The presence of hysteresis suggests an interaction between the adsorbent (SiO2BH2O) and water molecules. The silica surface mainly consists of siloxane bridges (Si-O-Si) and fewer silanol groups.[6,9] These surface siloxane bridges are hydrolyzed by adsorbed water molecules to form silanols, which are considered to cause the decrease in water molecules desorbed.   On the other hand, for SiO2B, the amount of water vapor adsorption is limited; the water adsorption ability was lower than that of SiO2BH2O over the whole range of P/P0, and the steep increase at high P/P0 was absent. The amount of water adsorbed at P/P0 =0.99 was less than one-fourth of that for SiO2BH2O. These findings demonstrated the hydrophobicity of SiO2B as expected. The decrease in water adsorption property was also confirmed by the significant reduction of the hysteresis loop in the desorption branch. These data clearly shows the hydrophobic property of SiO2B.   The surface property on water vapor sorption was evaluated using the BET plots (Fig. 4 inset). The amount of monolayer water adsorbed (wm) can be estimated to be 2.94×10-3 and 5.12×10-3 (g(H2O)/g(adsorbent)) for SiO2B and SiO2BH2O, corresponding to 0.163 and 0.284 mmol/g, respectively (Table 1). The BET constant (C) of SiO2B was slightly larger than that of SiO2BH2O, suggesting an interaction in this early stage. By using the surface area (S.A.) evaluated from N2 sorption study (Table 1) and Avogadro’s number (NA), the number of water molecule per unit surface area (Nwater) can be calculated from the following equation:  	 The Nwater for SiO2B and SiO2BH2O was 1.39 and 2.24 (molecules/nm2), respectively. Assuming the geometrical closest packing of H2O molecules (0.125 nm2/molecule), corresponding to 8 molecules/nm2, it seems that the surface coverage by water molecules was low.    Water vapor sorption isotherm of SiO2B and SiO2BH2O. Inset; BET plots by water sorption. Symbols are circle for SiO2B and triangle for SiO2BH2O, respectively. &(&(ゐ፹⏝␯Ỉᛶࢩࣜ࢝ࣅ࣮ࢬࡢ⣽Ꮝᵓ㐀ཬࡧỈ⵨Ẽ྾╔≉ᛶ  The differential heat of water vapor adsorption was shown in Fig. 5. For SiO2B, a high heat evolution (about 60 kJ/mol) was seen in the initial stage of water adsorption, and then it decreased to less than 44 kJ/mol, which is the heat of liquefaction of water [10], at the adsorption amount of 0.05 mmol/g. This large exothermic effect is probably due to the strong interaction between water and unreacted silanol groups (Si-OH), which were left during the grafting of bulky trimethylsilane.[9,11,12] The heat of adsorption reached a minimum at around 0.2 - 0.3 mmol/g, which is close to the value of wm (0.163). Then, the heat of adsorption slightly increased with an increase in the adsorption amount. However, the formation of water clusters was not detectable (below 44 kJ/mol), obviously preventing the additional adsorption of water molecules to grow the water clusters.  On the other hand, for SiO2BH2O, the heat of adsorption was low at the initial stage, indicating less interaction between siloxane and water molecules and hence suggesting the hydrophobic character of the surface.[6,9] The minimum value of the heat of adsorption was observed at the adsorption amount of around 0.20  0.30 mmol/g, which is close to the wm (0.284 mmol/g). Then, the released heat increased gradually as the adsorption proceeded, attaining about 44 kJ/mol at the adsorption amount of about 1.65 mmol/g. These findings support the idea that after formation of monolayers, additional water molecules coordinate to the water molecules to form water clusters in the pores. The hydrolysis of siloxane bonds to generate silanol groups probably takes place during water uptake, which may explain the large hysteresis in the desorption isotherm. An FT-IR study may help us obtain more detailed understanding of the hydrolysis process, but it would be out of the scope of this paper.   In conclusion, we have investigated the porosity and water vapor sorption properties of trimethylsilane grafted hydrophobic silica beads (SiO2B), which we have chosen as a catalyst support for CECE reaction. The low water vapor sorption capacity and restricted interaction for water cluster formation of this SiO2B demonstrated a desired feature for a catalyst support: prevention of pore blocking due to water condensation. Preparation and characterization of Pt-loaded catalysts and the CECE reaction activity of resultant catalysts will be reported elsewhere.    Differential heat of adsorption of water vapor on (circle) SiO2B and (triangle) SiO2BH2O.  ⏣ཱྀ࣭᫂ᮡᒣ㈗ᙪ࣭᳃⏣ὒᖹ࣭⏣୰ᑗ⿱࣭ྂ⸨೺ྖ࣭᐀ീ೺୕ 	The authors thank to Fuji Silysia Chemical Ltd., Aichi, for their kindly supply of SiO2 beads. This work is performed with the support and under the auspices of the NIFS Collaboration Research program (NIFS13KOBA029).   	  [1] J. P. Butler, Sep. Sci. Technol.  (1980) 371.  [2] G. Vsaru, “Tritium Isotope Separation”, CRC press, Boca Raton, Florida, (1993).  [3] A. Matsushima, T. Haneda, S. Hayashi, S. Kiyota, JNC Technical Review (Saikuru Kiko Giho), No.20s1 (2003) 73, (in Japanese). [4] T. Sugiyama, Y. Asakura, T. Uda, Y. Abe, T. Shiozaki, Y. Enokida, I. Yamamoto, J. Nucl. Sci. Technol.  (2004) 696.  [5] T. Sugiyama, E. Suzuki, M. Tanaka, I. Yamamoto, Fus. Sci. Technol.  (2011) 1323.  [6] E.-P. Ng, S. Mintova, Micropor. Mesopor. Mat.  (2008) 1.  [7] K. S. W. Sing, Pure Appl. Chem.  (1982) 2201. [8] S. Lowell, J. E. Shields, M. A. Thomas, M. Thommes, “Characterization of Porous Solids and Powders: Surface Area, Pore Size and Density”, Kluwer Academic Publishers, Dordrecht, The Netherlands (2004).  [9] L. T. Zhuravlev, Colloids Surf. A.   (2000) 1.  [10] D. R. Lide, H. V. Kehiaian, “CRC Handbook of Thermophysical and Thermochemical Data”, CRC press, Boca Raton, Florida, (1994).  [11] X. S. Zhao, G. Q. Lu, J. Phys. Chem. B,  (1998) 1556.  [12] R. Anwander, I. Nagl, M. Widenmeyer, G. Engelhardt, O. Groeger, C. Palm, T. Röser, J.Phys. Chem. B,  (2000) 3532. &(&(ゐ፹⏝␯Ỉᛶࢩࣜ࢝ࣅ࣮ࢬࡢ⣽Ꮝᵓ㐀ཬࡧỈ⵨Ẽ྾╔≉ᛶ

CECE触媒用疎水性シリカビーズの細孔構造及び水蒸気吸着特性

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Porosity and water vapor sorption property of new hydrophobic silica beads for CECE catalyst support

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