Original Article
Phys Chem Ind J, Volume: 12( 1)

Significant CO2 Adsorption Ability of Nanoscale BaTiO3 Ceramics Fabricated by Carbon-Template-Solvothermal Reactions

*Correspondence:
Ohba T, Graduate School of Science, Chiba University, 1-33 Yayoi, Inage, Chiba 2638522, Japan, E-mail: [email protected]

Received: March 29, 2017; Accepted: April 21, 2017; Published: April 28, 2017

Citation: Watanabe T, Md Khan S, Kanoh H, et al. Significant CO2 Adsorption Ability of Nanoscale BaTiO3 Ceramics Fabricated by Carbon-Template-Solvothermal Reactions. Phys Chem Ind J. 2017;S1:101.

Abstract

Separation of CO2 using adsorption and membrane separations can be performed under moderate conditions for carbon capture and release processes. Although porous media work well for this purpose, these novel materials must be fabricated with high CO2 separation ability. We propose the use of nanoscale BaTiO3 crystals as separators for CO2 adsorption. Although BaTiO3 is a conventional ceramic, it exhibits high dielectric properties and shows potential for a strong interaction with the quadrupole moment of CO2. However, this high adsorption potential is reduced by the extremely small surface area of BaTiO3. Here, we fabricated nanoscale BaTiO3 crystals with high surface area and nanopores, and demonstrated their excellent CO2 adsorption performance with large adsorption hysteresis. The CO2 adsorbed in the nanoscale BaTiO3 crystals could be perfectly released under vacuum conditions. The structure of adsorbed CO2 was similar to CO2 solid at 1 GPa. The unique adsorption properties of CO2 in these nanoscale BaTiO3 crystals are of interest for the development of materials with high CO2 adsorption ability.

Keywords

CO2 adsorption; Adsorption hysteresis; Barium titanate; Carbon storage; Nanoceramics; Chemisorption

Introduction

The effects of global warming and climate change are receiving increasing attention [1,2]. In particular, emphasis has been placed on the control of CO2 emissions, the main source of which is generally fossil fuel combustion [3,4]. The selection of an appropriate technology for CO2 capture depends on many factors such as the partial pressure of CO2 in the gas stream, recyclability, sensitivity to impurities, capital and operating costs, and environmental impact [2]. Based on the methods used for the separation of the components of a gas stream, absorption, adsorption, cryogenic distillation, or membrane purification can be applied for CO2 capture [5]. Liquid absorbents need to be changed and may be corrosive and toxic, cryogenic distillation is a costly process, and membranes are efficient for the separation of relatively high concentrations of adsorbate. Therefore, of these four technologies, we focused on adsorption, which is desirable because of the easy recovery of the adsorbent using temperature or pressure fluctuations, thereby reducing the cost and energy consumption [5-8]. Suitable adsorbents should exhibit high adsorption capacity, fast adsorption and desorption kinetics, recovery capabilities, and stability under various operating conditions [6,8,9]. In recent decades, adsorption using porous materials has been investigated. Porous materials are generally used for CO2 capture because of their large surface area, and these materials are sometimes modified using functional groups, such as zeolites [10], activated carbon [11,12], and metal–organic frameworks [13], to increase the CO2 adsorption capacity. Amine-modified silica is also used as an adsorbent that functions based on chemical interaction such as chemisorption [14].

Barium titanate (BaTiO3) is a representative advanced ceramic and exhibits electronic properties that are useful for capacitors and sensors. BaTiO3 is also a ferroelectric and thus exhibits spontaneous polarization; in addition, its surface has strong electrostatic interaction with several types of adsorbates, described by Coulomb’s law for partial charges. Zhao et al. investigated the effect of ferroelectric polarization on the adsorption of 2-fluoroethanol and ethanol on BaTiO3 , suggesting reaction sites on polarized surfaces of BaTiO3 [15,16]. Higai proposed dissociative adsorption of H2O, and both H2O and CO2 were greatly stabilized on nanoscale BaTiO3 according to first-principles calculations [17-19]. Baniecki et al. experimentally evaluated the CO2 adsorption observed in defective surfaces of BaTiO3 -defective surfaces, they have received considerable attention not only for their use in electronic devices but also as adsorbents. Many researchers have investigated methods to reduce the size of BaTiO3 using hydrothermal methods [20-22], sol-gel solvothermal methods [23,24], and template synthesis [24,25]. We previously fabricated nanoscale BaTiO3 crystals using carbon template-solvothermal reactions [26].

In this study, we adopted nanoscale BaTiO3 crystals as CO2 adsorbents and evaluated the performance of CO2 adsorption on various sized BaTiO3 crystals. In addition, the CO2 adsorption mechanism and structures were investigated using adsorption isotherms at 273 K to 363 K and X-ray diffraction (XRD).

Materials and Methods

BaTiO3 crystals of three different scales were prepared using solid-state, solvothermal, and carbon template-solvothermal reactions, and the resulting crystals were labeled macro-, meso-, and nano-BaTiO3 crystals, respectively. The reagents used for the solid-state reaction were barium carbonate (>98%, Wako Pure Chemical Industries, Co. Ltd., Osaka, Japan) and rutile-type titanium dioxide (>99%, Wako Pure Chemical Industries, Co. Ltd.) A stoichiometric mixture of barium carbonate and titanium dioxide was pelletized under more than 60 MPa for 1 h, and the pellet obtained was heated at 1073 K for 24 h and subsequently heated at 1473 K for 48 h after grinding and pelletizing. In the solvothermal and carbon-template solvothermal reactions, barium ethoxide (>99%, Kojundo Chemical Laboratory Co. Ltd., Saitama, Japan) and titanium tetraisopropoxide (>99%, Kojundo Chemical Laboratory Co. Ltd.) were mixed with methanol (>99%, Wako Pure Chemical Industries, Co. Ltd.) and methoxyethanol (>99%, Wako Pure Chemical Industries, Ltd.). The volume ratio of methanol and methoxyethanol was 3:2. This solution was stirred vigorously for 3 h. After stirring, water or activated carbon fiber (W15, Ad’all Co. Ltd., Kyoto, Japan) adsorbed water was added into the precursor and heated at 400 K for 24 h for the solvothermal or carbon-template solvothermal reaction, respectively. Here, water-adsorbed activated carbon fibers were prepared by exposure to water vapor at 85–89% humidity. The meso-BaTiO3 crystal after the solvothermal reaction was collected by centrifugation at 10000 rpm for 20 min. Nano-BaTiO3 crystal was obtained by heat removal of the activated carbon fibers in an O2 atmosphere at 673 K for 48 h. The products were purified by filtration using hot water to remove the precursors and impurities. Two concentrations of Ba and Ti ions, 0.2 and 0.4 mol L-1, were selected for both the solvothermal and carbon-template solvothermal reactions.

The structures of the BaTiO3 crystals were evaluated using XRD (UltimaIV, Rigaku Co., Tokyo, Japan) with Cu Kα radiation (λ=0.1541 nm) at 40 kV and 40 mA and N2 adsorption measurements at 77 K (Autosorb-1, Quantachrome Co., Florida, USA). The crystallite sizes of the BaTiO3 crystals were determined using the Scherrer equation based on the XRD results [27]. The specific surface areas and micropore volumes were analyzed using the Brunauer-Emmett-Teller and Dubinin-Radushkevich equations, respectively [28,29]. The pore size distributions of the BaTiO3 crystals were evaluated using non-local density functional theory calculations using the software package (Autosorb-1) [30,31]. The particle size was evaluated based on the spherical assumption. Particle structures were evaluated using transmission electron microscopy (TEM; JEM-2100F, JEOL Co., Tokyo, Japan) at 200 kV. Finally, the CO2 sorption performances at 273, 303, 333, and 363 K were evaluated using adsorption measurements.

Results and Discussion

The crystal structure of the macro-BaTiO3 crystal shown in Figure 1a, matched well with that previously reported for BaTiO3 (JCPDS Card #50626). The XRD patterns for the meso-BaTiO3 crystal in Figure 1a, perfectly correspond with those of the macro-BaTiO3 crystal but were broadened because of the reduced crystallite size. Further broadening was observed for the nano-BaTiO3 crystal, indicating nano-crystallization. The crystallite sizes of the macro-, meso-, and nano-BaTiO3 crystals were calculated to be 370 nm, 13 nm ± 1 nm, and 6.4 nm ± 0.2 nm, respectively, using the Scherrer equation. Crystallite size evaluation using the Scherrer equation is known to be erroneous for crystals larger than 100 nm; the crystal size of the macro-BaTiO3 evaluated using SEM in our preceding paper was approximately 1000 nm [26]. The N2 adsorption isotherms at 77 K in Figure 1b, were used to evaluate the specific surface areas and micropore volumes, which were determined to be 2 m2 g-1, 71 m2 g-1, and 266 m2 g-1 and 0.000 mL g-1, 0.019 mL g-1, and 0.060 mL g-1 for the macro-, meso-, and nano-BaTiO3 crystals, respectively. The particle sizes, which were evaluated under the spherical assumption using the specific surface areas, were determined to be 650 nm, 14 nm, and 4 nm for the macro-, meso-, and nano-BaTiO3 crystals, respectively. The particle size of the nano-BaTiO3 crystals was the smallest because of restriction by carbon nanopores of activated carbon fibers. Figure 1c, demonstrates that the particle size approximately corresponded to the crystallite size, indicating that the particles were roughly composed of single nanocrystals. The TEM images are shown in Figure 1d. Nanoparticles of nano-BaTiO3 were observed on a TEM grid and the particle size was 2 nm to 10 nm. The particle sizes of meso- and macro-BaTiO3 was 10 nm to 20 nm and more than 0.5 μm, respectively. Those direct observations of particle sizes approximately agreed with the particle and crystallite size evaluations from the N2 adsorption isotherms and XRD analyses. In addition, interparticle spaces could form nanopores for those nanoparticles. The nanopore size distribution determined based on non-local density functional theory calculations [30,31] suggested that the nanopores of the nano-BaTiO3 crystals were smaller than those of the meso-BaTiO3 crystals, as observed in Figure 1e; however, narrow micropores were formed in both the meso- and nano-BaTiO3 crystals. The average nanopore sizes were unexpectedly larger than the particle sizes. Therefore, aggregation of the BaTiO3 crystals occurred and those assemblages then formed relatively large nanopores.

physical-chemistry-Structural-evaluation

Figure 1: Structural evaluation of nano-BaTiO3 (red), meso-BaTiO3 (blue), and macro-BaTiO3 (green) crystals. (a) XRD patterns of nano-, meso-, and macro-BaTiO3 crystals. (b) N2 adsorption isotherms of BaTiO3 crystals at 77 K for adsorption (filled symbols) and desorption courses (open symbols). Meso-BaTiO3 crystals synthesized using 200 (?) and 400 (?) mM concentrations and nano-BaTiO3 crystals synthesized using 200 (?) and 400 (?) mM concentrations. (c) Comparison of particle size and crystallite size. (d) TEM images of BaTiO3 crystals. (e) Nanopore size distributions of BaTiO3 crystals.

Figure 2, presents the CO2 adsorption isotherms at 273 K, 303 K, 333 K, and 363 K. The macro-BaTiO3 crystal exhibited typical ceramic crystallinity and CO2 was rarely adsorbed on the macro-BaTiO3 crystal surfaces. However, the meso- and nano-BaTiO3 crystals adsorbed substantial amounts of CO2 because of the nanocrystallization. Surprisingly, adsorption hysteresis was observed even at 303 K and 333 K, and CO2 was perfectly released in vacuo at these temperatures. Reversible CO2 physical adsorption and desorption on porous media were typically observed; however, adsorption hysteresis was observed for adsorbents with chemisorbing species such as amine groups. Therefore, the nano-BaTiO3 crystals exhibited weak chemisorption of CO2 .

physical-chemistry-adsorption-isotherms

Figure 2: CO2 adsorption isotherms of nano- (red), meso- (blue), and macro-BaTiO3 (green) crystals at 273 (a), 303 (b), 333 (c), and 363 K (d) for adsorption (filled symbol) and desorption courses (open symbol). Meso-BaTiO3 crystals synthesized using 200 (?) and 400 (?) mM concentrations and nano-BaTiO3 crystals synthesized using 200 (?) and 400 (?) mM concentrations.

Considerable adsorption hysteresis of CO2 adsorption in the nano-BaTiO3 crystals was observed, as mentioned above, especially for the 200 mM concentration. Figure 3a, shows the adsorption hysteresis areas evaluated based on the difference between the integrals of the adsorption and desorption amounts. The adsorption hysteresis for the nano-BaTiO3 crystals is clearly larger than that for the meso-BaTiO3 crystals. The adsorption hysteresis loop shrunk with increasing temperature except for the nano-BaTiO3 crystals synthesized using the 200 mM concentration. The adsorption hysteresis area for the nano-BaTiO3 crystals had a maximum at 303 K to 333 K. The ratio of the adsorption hysteresis is defined as the adsorption hysteresis area divided by the integral of the adsorption amount, as shown in Figure 3b. The ratio of the adsorption hysteresis reached a maximum at 333 K, suggesting that the activation energy of CO2 capture and/or weak CO2 chemisorption was 333 K. These quasi-irreversible adsorption properties have rarely been observed for CO2 adsorption on typical porous media.

physical-chemistry-Adsorption-hysteresis

Figure 3: Adsorption hysteresis in CO2 adsorption isotherms at 273 K to 363 K (a) and ratios of adsorption hysteresis areas (b). Meso-BaTiO3 crystals synthesized using 200 (?) and 400 (?) mM concentrations and nano-BaTiO3 crystals synthesized using 200 (?) and 400 (?) mM concentrations.

Figure 4, shows the adsorption density changes at various temperatures. Here, the adsorption densities were calculated based on the adsorption amounts and micropore volumes. The results for microporous media are also shown for comparison because CO2 could be mainly adsorbed in the micropores. The meso- and nano-BaTiO3 crystals had extremely high adsorbed densities compared with the other microporous media. The adsorbed densities were somewhat maintained even at temperatures above 333 K. The mesopores of the meso-BaTiO3 crystals partially adsorbed CO2 , thereby increasing the adsorbed density. The adsorbed densities in the meso- and nano-BaTiO3 crystals were sufficiently high; the CO2 solid density at 195 K and liquid density at 236 K were 1560 mg/cm-3 and 1100 mg/cm-3, respectively. The specific surface areas and micropore volumes of the meso- and nano-BaTiO3 crystals were relatively smaller than those of typical microporous media. To improve the adsorption performance of CO2 , aggregation of nanocrystals must be prevented.

physical-chemistry-adsorption-densities

Figure 4: CO2 adsorption densities in nanopores of BaTiO3 crystals and other porous materials at 100 kPa. The nano-BaTiO3 crystals synthesized at concentrations of 200 and 400 mM are depicted by blue circles and diamonds, respectively. The meso-BaTiO3 crystals synthesized at concentrations of 200 and 400 mM are depicted by red triangles and squares, respectively. The macro-BaTiO3 crystal is depicted by green crosses. (?): carbon materials S32], ?: metal-organic frameworks [9,13,33,34], ?: zeolites [10], and ?: porous silica [32].

Figure 5, presents the XRD patterns of the CO2 -adsorbed meso- and nano-BaTiO3 crystals at 100 kPa, and the meso- and nano-BaTiO3 crystals in vacuo. The XRD pattern of the CO2 solid is also shown for comparison [32-35]. The differences between the BaTiO3 crystals with and without CO2 originate from the correlation between CO2 -CO2 and CO2 -BaTiO3 crystals. The differential broad peaks were assigned to the CO2 solid. Thus, the solid-like structure of CO2 adsorbed in the nanopores of the nano-BaTiO3 crystals was formed. The solid-like structure formation of CO2 resulted in high adsorption density in the nanopores.

physical-chemistry-XRD-patterns

Figure 5: XRD patterns of meso-BaTiO3 crystal (dark blue), meso-BaTiO3 crystal adsorbing CO2 (light blue), nano-BaTiO3 crystal (red), nano-BaTiO3 crystal adsorbing CO2 (orange), and CO2 solid (black) at 1 GPa [33].

Conclusions

In this work, we demonstrated the anomalous CO2 adsorption properties of nanoscale BaTiO3 crystals. BaTiO3 is a conventional ceramic that exhibits almost non-existent adsorption performance. However, nanocrystallization of BaTiO3 induced high CO2 adsorption performance associated with adsorption hysteresis and the formation of a solid-like CO2 structure. BaTiO3 crystals inherently exhibit strong dielectric properties and interact with the partial charges of CO2 , forming a quadrupole moment. The quasi-irreversible adsorption properties on the nano-BaTiO3 crystals are important to adsorb and release CO2 efficiently, because typical porous solids have weak adsorption potential of CO2 and chemisorption by amine-functionalized media is too strong to release CO2 . Thus, the fabrication of nanoscale BaTiO3 crystals revealed their excellent CO2 adsorption performance. However, some nanoscale BaTiO3 crystals became aggregated, and this aggregation reduced the surface areas. Further study is thus necessary to prevent the aggregation of nanoscale BaTiO3 crystals.

Acknowledgements

We thank Dr. S. Kawaguchi for his help in recording the XRD data at SPring-8. TEM observations were performed at the Chemical Analysis Center, Chiba University. This research was supported by the Japan Society for the Promotion of Science KAKENHI (Grant Numbers 26706001 and 15K12261), research fellowships from the New Energy and Industrial Technology Development Organization (NEDO), Japan, and the Futaba Electronics Memorial Foundation.

References