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International Journal of Photoenergy
Volume 2012 (2012), Article ID 901907, 6 pages
http://dx.doi.org/10.1155/2012/901907
Research Article

Photocatalytic Activity of Titanate Nanotube Powders in a Hybrid Pollution Control System

1Faculty of Nanotechnology and Advanced Materials Engineering, Sejong University, Seoul 143-747, Republic of Korea
2Department of Fine Chemical Engineering and Applied Chemistry, Chungnam National University, Daejeon 305-764, Republic of Korea
3Department of Dental Materials, School of Dentistry, Chosun University, Gwangju 501-759, Republic of Korea
4Department of Civil and Environmental Engineering, Chonnam National University, Yosu 550-749, Republic of Korea
5Department of Environmental Engineering, Sunchon National University, Sunchon 540-742, Republic of Korea

Received 26 January 2012; Revised 21 February 2012; Accepted 24 February 2012

Academic Editor: Weifeng Yao

Copyright © 2012 Sun-Jae Kim et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

Abstract

The photocatalytic activity on decomposition of Rhodamine B (RB) of titanate nanotubes (TNTs) synthesized by alkali hydrothermal treatment method was evaluated using a microwave/UV/photocatalyst hybrid system. The effects of each element technique as well as the synergy effects on decomposition of organic material were investigated. When TNTs were ion-exchanged with HCl, Na+ content was reduced from 8.36 wt% to 0.03 wt%, whereas the TNTs calcined at 723 K was phase-transformed into anatase structure. The RB decomposition rate increased with TNTs dosage as well as with microwave intensity. Effect of addition of auxiliary oxidants on photocatalytic decomposition of RB was also investigated. When ozone was added, the decomposition rate increased with the amount of ozone added. When H2O2 was used as the auxiliary oxidant, however, addition of H2O2 exceeding a threshold amount caused reduction of decomposition rate. A synergy effect was observed when H2O2 addition was combined with microwave-assisted photocatalysis.

1. Introduction

Titanate nanotube (TNT), having unique properties, for example, tubular structure, large surface area, strong ion exchange, and high sedimentation rate, is a material with high potential in various applications such as supports, ion exchange, adsorption, and dye sensitized solar cells. Among others, application as photocatalyst is of special interest because of its material property combined with nanoscale structure. Nevertheless, data reported for the photocatalytic activity of synthesized TNTs are inconsistent. According to Yu et al. [1], who used TNT synthesized hydrothermally at 423 K with 48 h of treatment time to enhance the photocatalytic oxidation of acetone in air, TNT showed no photocatalytic activity before calcination. It has been reported that nanotubes do not have photocatalytic activity towards amaranth degradation regardless of its sodium content. Yu et al. [2] synthesized hydrogen titanate nanowires at various heat treatment temperatures and investigated their phase structure, crystallite size, morphology, specific surface area, pore structure, and photocatalytic activity. Baiju et al. [3] investigated the photocatalytic activity of a mixed nanobelts-nanotubes titanate obtained through hydrothermal method at 423 K with 30 h of treating time on degradation of methylene blue. They reported that photocatalytic activity of the catalyst was very low although it exhibited high adsorptivity towards methylene blue. On the other hand, Nakahira et al. [4] reported a significantly high activity of TNT on degradation of HCHO under UV light. Xiao et al. [5] also found that TNT synthesized hydrothermally at 403 K with 24 h of treating time had a high photocatalytic activity on degradation of Rhodamine B (referred to as RB hereafter), with the degradation efficiency similar to that of P25. This inconsistency found in the literature may be attributed, at least partly, to different precursors used (amorphous TiO2, anatase, rutile, and their mixture) and reaction conditions applied (temperature and time). Another possibility is that the produced TNT may have contained unreacted anatase phase which could have provided unexpected photocatalytic activity.

It is of growing interest to use microwave energy for synthetic organic chemistry because it can accelerate reactions and improve yields and selectivity. Many researchers have reported improved photocatalytic performance achieved by microwave irradiation. For example, Kataoka et al. [6] reported that microwave irradiation increased the photocatalytic oxidation rate of ethylene by 83.9%. Horikoshi et al. [7] found from their experiments using electron spin resonance (ESR) that generation of OH radicals during photocatalytic reaction was enhanced by about 20% by microwave irradiation. One difficulty in combining UV light source and microwave irradiation is electrode spoilage. This problem can be solved if microwave electrodeless lamp is used as the light source. Furthermore, microwave electrodeless lamp brings additional benefits: good photochemical efficiency, long lifetime, low cost, and simple equipment setup [8]. Horikoshi et al. [9] argued that photocatalysis with electrodeless lamp (a double quartz cylindrical plasma photoreactor) was about 10-times more efficient than the photocatalysis using traditional lamp.

In a previous study of ours, the TNTs were calcined at several different temperatures and their photocatalytic activities were compared with those of Degussa P-25 powders [10]. The TNT calcined at 673 K showed a lower activity than P-25, whereas the activity of the TNT calcined at 698 K was similar to that of P-25. On the other hand, all the TNTs calcined at 723 K or higher exhibited higher photocatalytic activities than P-25. In this study, the photocatalytic activity of the TNT calcined at 723 K was evaluated using a novel microwave/UV/photocatalyst hybrid system. A microwave-assisted electrodeless lamp is used as the UV source. The effect of microwave irradiation on photocatalytic reaction efficiency is investigated. To improve the pollutant removal rate further, two auxiliary oxidants, O3 and H2O2, are added in the reaction and their effects on the reaction efficiency are investigated based on the experimental results. The role of each element technique and interaction among them are discussed.

2. Experimental

Commercial TiO2 P25 (Evonik, former Degussa, Germany), composed of 75% of anatase and 25% of rutile, was used as raw material for TNT production. The BET surface area and the anatase crystallite size of P25 are about 50 m2/g and 25 nm, respectively. P25 was put into a Teflon-lined autoclave containing 10-M NaOH. The suspension was treated ultrasonically for 1 h to have TiO2 particles dispersed well. Then the autoclave was heated to maintain the temperature at 423 K for 48 h. After the reaction was completed, nanotube precipitate with a high pH level was washed repeatedly using distilled water to remove NaOH. The washed precipitate had 8.36 wt% of Na+ at pH = 7.0. It was then again dispersed in 0.1-N HCI solution at 333 K and stirred for a long time to allow Na+ ions trapped on the surface and interior of the particles during the hydrothermal reaction to be ion-exchanged with H+ and then removed. During the ion-exchange processing, precipitate was sampled to measure the Na+ content. It was confirmed by the analysis of the precipitate that the Na+ content of the precipitate was 0.03 wt% at pH = 7.0. The precipitate sample was dried for 24 h using a freeze-dryer to remove moisture from the sample. The ion-exchanged nanotubes were calcined in air at 723 K for 30 min and then were ground in an agate mortar before being used in the photocatalytic experiments. Scanning electron microscope (S-4700, Hitachi) and transmission electron microscope (JEM-2010F, JEOL) observations showed that the powders had nanotubular shape. The Na+ ion content was analyzed by EDX (Oxford INCA energy detector, equipped with SEM). Crystal structure of the powder was analyzed using X-ray diffractometer (D/MAX-2500/PC, Rigaku) and ambient Raman Spectroscopy (inVia Raman macroscope, Renishow).

Photocatalytic activity of TNT prepared in this way on decomposition of RB in its aqueous solution was evaluated using a microwave/UV/photocatalyst hybrid process system. RB (Junsei Chem. Co., Ltd.) was chosen because it is not adsorbed well on TNT powders. Refer to our previous paper [11] for detailed description on the experimental apparatus. Microwave irradiation was created by a microwave/UV system manufactured by Korea microwave instrument Co., Ltd. It is composed of a microwave generator (frequency, 2.45 GHz; maximal power, 1 kW), a three-stub tuner, a power monitor, and a reaction cavity. Microwave (actual power used, 200~600 W) irradiated on the RB aqueous solution ( mM, 1 L) containing TNT powders (loading, 0.05~0.15 g) was delivered through a wave guide. Microwave irradiation was continuous and its intensity was controlled by a power monitor. Optimal low reflection of the microwave radiation was achieved using the three-stub tuner. The UV source and the microwave generator were located on the right-hand and left-hand sides, respectively, of the device. A stirrer was installed on the back side in the reaction cavity to enhance the microwave transfer.

A double-tube type microwave discharge electrodeless lamp (referred to as MDEL hereafter), with 170 mm length, 44 mm inner diameter, and 60 mm outer diameter, emitting UV upon irradiation of microwave was used in this study. It was made of quartz to maximize the reaction efficiency. Small amount of mercury was doped between the tubes inside the double-tube UV lamp that was kept vacuumed. The lamp used in this study is UV-C type lamp although a little amount of UV-A and UV-B wavelength lights is emitted as well.

Because microwave irradiation heats up the reactant solution, the reaction temperature could not be maintained at a constant without a cooling system. Therefore, the reactant solution was put in a stainless steel beaker installed in a constant-temperature equipment. The heated reactant solution was circulated through a cooling system by a roller pump to keep the reaction temperature constant at 298 K. To investigate the effect of addition of auxiliary oxidants on the decomposition organic compounds, ozone and hydrogen peroxide were added. Ozone was produced by feeding oxygen with the flow rate of 500 cc/min to an ozone generator (Lab-1, Ozone Tech Co., Ltd). The ozone production rate was controlled between 0.75 and 3.26 g/hr. The reactant solution was prepared using double distilled water. The decomposition rate of RB was calculated from the change in its concentration measured at the reactor outlet as a function of reaction time. The RB concentration was determined by measuring absorbance at 550 nm using a spectrophotometer (UV-1601, Shimadzu).

3. Results and Discussion

Figure 1(a) shows the XRD results for TNT powders calcined at 723 K for 30 min in O2 atmosphere. Characteristic peaks of anatase TiO2 phase at 2θ = 25.35, 37.84, 48.14, 53.97, and 55.18° are clearly observed due to transformation of the titanate into anatase phase. This is in good agreement with Raman spectra shown in Figure 1(b) that demonstrates anatase characteristic peaks at 145, 390, 506, and 638 cm−1. It is clearly shown in Figure 1 that the titanate phase transformation was almost complete at 723 K although trace of the titanate phase was detected at 280 cm−1, which is not clearly shown in normal scale.

fig1
Figure 1: X-ray diffraction pattern (a) and Raman spectra (b) of TNT powders calcined for 30 min at 723 K in O2 atmosphere.

Figure 2(a) shows an SEM image of calcined TNT powders. The powders are shown to be nanotubes growing along axial direction. The tubular shape of the powder is observed from a TEM image as well (Figure 2(b)). It is also observed that the powders were broken into nanorods and then became nanoparticles. Figure 2 shows that thermal treatment for 30 minutes at 723 K in O2 atmosphere did not destroy the nanotubular structure of TNT.

fig2
Figure 2: SEM and TEM images of TNT powders calcined for 30 min at 723 K in O2 atmosphere.

Figure 3 shows the decay in RB concentration obtained with three different TNT powder dosages. For all experiments, initial concentration of RB was about 5.0 × 10−6 mM and 1 L of solution was circulated into the reactor with a flow rate of 400 cc/min. The intensity of microwave irradiation was 0.4 kW. It is shown that the RB decomposition rate increases with TNT powder dosage. The results for the three cases were all fitted well by linear lines indicating that decomposition of RB over TNT catalyst can be approximated by a pseudo-first-order reaction model: where is the RB concentration, the initial concentration, the over-all reaction rate constant, and the reaction time. is determined from the slope of the lines shown in Figure 3.

901907.fig.003
Figure 3: Effect of TNT powder dosages on decomposition of RB.

Figure 4 compares the RB concentration decay obtained with three different microwave intensities: 0.2, 0.4, and 0.6 kw. For all experiments shown in this figure, 0.1 g of TNT powders was used. It is clearly shown in this figure that the degradation rate increases with microwave intensity. Microwave irradiation contributes to enhancing the pollutant degradation rate in two ways [7]. It increases temperature selectively, quickly, and uniformly leading to higher reaction rate (thermal effect). Microwave also increases the collision frequency between reactants (nonthermal effect). In addition, microwave intensity affects UV intensity as well in this study because the UV irradiation was created by MDEL upon the irradiation of microwave: higher microwave intensity results in a higher UV intensity. UV, which carries intense energy, enhances the photocatalytic reaction rate by exciting photo-catalyst. Therefore, it was not possible to identify the mechanism by which microwave irradiation contributed to enhancing the photocatalytic reaction rate in this study. It can be either one of the effects described above or combination of two or all of them.

901907.fig.004
Figure 4: Effect of microwave intensity on photocatalytic degradation of RB.

Ozone is a strong oxidant with the electric potential difference of 2.07 V. It has widely been used in water treatment because it can effectively remove taste, odor and precursors of trihalomethanes (THMs). The effect of ozone in oxidation of organic compounds is, however, relatively selective because ozone has very low reactivity on single-bond chemicals and aromatic compounds with specific functional groups such as –COOH and –NO2. On the contrary, the hydroxyl radical (OH), which has a higher oxidation potential (2.80 V) than ozone, can react with organic compounds unselectively. Large attention has been given to the advanced oxidation processes (AOPs), in which the organic compounds decomposition is enhanced by OH radicals. One of the strengths of the microwave/UV/TiO2 hybrid system used in this study is that combined microwave and UV irradiations activate photo-catalyst to maximize the formation of OH radicals when ozone is introduced.

Figure 5 compares the reaction rate constants obtained with three different combinations of element techniques, that is, ozone injection only, ozone injection combined with microwave irradiation, and ozone injection combined with microwave-assisted UV photocatalysis, with four different ozone injection levels: 0, 0.75, 1.78, and 3.26 g/hr. For all the experiments shown in this figure, TNT powder dosage and microwave irradiation intensity were 0.1 g and 0.4 kW, respectively, when they were applied.

901907.fig.005
Figure 5: Effect of ozone injection on decomposition of RB.

The RB decomposition rate was highest when ozone was injected to the microwave/UV/TiO2 photocatalyst system. The reaction rate increased with ozone dosage. Even the ozone-only experiments showed high RB decomposition rate with the rate constant of 0.1354, which was a little higher than that obtained by microwave/UV/TiO2 photocatalyst system without ozone injection (0.1284). When microwave irradiation combined with ozone injection was used, the reaction rate constant was in between the results of the other two conditions. When only microwave irradiation was used, very little RB decomposition was obtained (not shown).

Reports on the effect of H2O2 on pollutant removal are abundant in the literature. There is a general consensus that addition of H2O2 enhances the photocatalytic degradation of organic pollutants [12]. The increased reaction rate caused by H2O2 addition can be explained by a couple of reasons. First, it takes surface-trapped electrons, and hence reduces the electron-hole recombination rate and makes more holes available for reactions creating OH radicals (e.g., OH + h+ → OH). Second, H2O2 may split into two OH radicals directly by photocatalytic reaction. Because H2O2 can be an efficient electron acceptor in TiO2 photocatalytic systems, its effect on photocatalytic pollutant degradation was evaluated [13]. Figure 6 compares the reaction rate constants obtained with different amount of H2O2 added to the microwave-assisted photocatalytic system. H2O2 addition increased the reaction rate while the added amount was smaller than a threshold value, 1.16 × 10−2 here, but further addition of H2O2 exceeding the threshold reduced the reaction rate. This is in good agreement with the results reported in the literature [14]. H2O2 is known to form a surface complex on TiO2 [15], which can cause blocking of surface sites of catalysts if the amount of H2O2 is too large. Another possible reason for the reduction of photocatalytic reaction rate due to excessive H2O2 is OH radical scavenging by H2O2 (H2O2 + OH → HO2 + H2O). In order to examine the function of H2O2 as the scavenger of OH radicals, it is required to observe the change in OH radicals. For instance, Xiang et al. [16] quantitatively measured the hydroxyl radicals produced from various semiconductor photocatalysts contained in aqueous solutions using the photoluminescence technique. Unfortunately, however, quantitative measurement of the hydroxyl radicals was not possible in this study due to the difficulty of installation of a sensor in the microwave cavity.

901907.fig.006
Figure 6: Effect of injection H2O2 for decomposition of RB in aqueous solutions.

Figure 7 compares the decomposition rate constants obtained under different experimental conditions. The results of eight different experiments are shown in this figure: microwave irradiation only (M), ozone injection only (O), H2O2 injection only (H), microwave irradiation combined with ozone injection (MO), microwave irradiation combined with H2O2 injection (MH), microwave-assisted photocatalysis by MDEL (MUP), MUP combined with ozone injection (MUPO), and MUP combined with H2O2 injection (MUPH). For all the experiments shown in this figure, TNT powder dosage of 0.1 g, microwave irradiation intensity of 0.4 kW, circulation flow rate of 400 mL/min, ozone injection rate of 0.75 g/h, and H2O2 addition amount of 1 mL  mol) were used. A relatively low ozone injection rate of 0.75 g/h was used because the reaction proceeded too fast under some conditions with a higher ozone injection rate.

901907.fig.007
Figure 7: Reaction rate constants obtained under various experimental conditions.

As shown in Figure 7, RB was hardly decomposed under M and H conditions. The reaction constant was low also under MH condition . When these element techniques were all combined (MUPH), however, the reaction rate was about six times that obtained under MH condition . Completely different results were obtained with addition of ozone. While the reaction rate constants of condition O and condition MO were high compared to those obtained with other element techniques, the reaction rate obtained under MUPO in which all these techniques were combined was not very high showing no synergy effect.

Microwave, which is an electromagnetic wave with a very short wavelength, excites polar molecules to cause them to rotate and vibrate back and forth rapidly. For example, water molecules can vibrate about times every second upon microwave irradiation. The original objective of this study was to enhance the decomposition reaction rate by exciting pollutant molecules using microwave irradiation. According to the experimental results shown above (M), however, the effect of excitement of pollutant molecules was negligible. Nevertheless, when the microwave-assisted photocatalysis was combined with addition of auxiliary oxidant such as H2O2, a synergy effect enhancing the reaction rate considerably was observed. This result suggests that microwave irradiation may promote the production of active intermediate products, for example, OH radicals, by exciting the auxiliary oxidant molecules. It should be noted, however, that this hypothesis cannot be proved based only on the limited experimental results of this study. Further studies under different conditions, including different pollutants and different auxiliary oxidants, are required to validate the hypothesis further.

4. Conclusion

To use hybrid pollution control system for advanced treatment of RB, a series of experiments were performed in which the effects of microwave irradiation and auxiliary oxidants were evaluated. The conclusions obtained from the experimental results are as follows.(1)When TNTs was ion-exchanged with HCl, Na+ content was reduced from 8.36 wt% to 0.03 wt%, whereas the TNTs calcined at 723 K was phase-transformed into anatase structure.(2)The RB decomposition rate increased with TNTs dosage as well as with microwave intensity.(3)When ozone was added, the decomposition rate increased with the amount of ozone added.(4)When H2O2 was used as the auxiliary oxidant, however, addition of H2O2 exceeding a threshold amount caused reduction of decomposition rate.(5)When the microwave-assisted photocatalysis was combined with addition of auxiliary oxidant such as H2O2, a synergy effect enhancing the reaction rate considerably was observed.

Acknowledgment

This research was supported by Basic Science Research Program through the National Research Foundation of Korea (NRF) funded by the Ministry of Education, Science, and Technology (2010-0007412 and 2011-0016699).

References

  1. J. Yu, H. Yu, B. Cheng, and C. Trapalis, “Effects of calcination temperature on the microstructures and photocatalytic activity of titanate nanotubes,” Journal of Molecular Catalysis A, vol. 249, no. 1-2, pp. 135–142, 2006. View at Publisher · View at Google Scholar · View at Scopus
  2. H. Yu, J. Yu, and B. Cheng, “Photocatalytic activity of the calcined H-titanate nanowires for photocatalytic oxidation of acetone in air,” Chemosphere, vol. 66, no. 11, pp. 2050–2057, 2007. View at Publisher · View at Google Scholar · View at Scopus
  3. K. V. Baiju, S. Shukla, S. Biju, M. L. P. Reddy, and K. G. K. Warrier, “Hydrothermal processing of dye-adsorbing one-dimensional hydrogen titanate,” Materials Letters, vol. 63, no. 11, pp. 923–926, 2009. View at Publisher · View at Google Scholar · View at Scopus
  4. A. Nakahira, W. Kato, M. Tamai, T. Isshiki, and K. Nishio, “Synthesis of nanotube from a layered H2Ti4O9· H2O in a hydrothermal treatment using various titania sources,” Journal of Materials Science, vol. 39, no. 13, pp. 4239–4245, 2004. View at Publisher · View at Google Scholar · View at Scopus
  5. M. W. Xiao, L. S. Wang, X. J. Huang, Y. D. Wu, and Z. Dang, “Synthesis and characterization of WO3/titanate nanotubes nanocomposite with enhanced photocatalytic properties,” Journal of Alloys and Compounds, vol. 470, no. 1-2, pp. 486–491, 2009. View at Publisher · View at Google Scholar · View at Scopus
  6. S. Kataoka, D. T. Tompkins, W. A. Zeltner, and M. A. Anderson, “Photocatalytic oxidation in the presence of microwave irradiation: observations with ethylene and water,” Journal of Photochemistry and Photobiology A, vol. 148, no. 1–3, pp. 323–330, 2002. View at Publisher · View at Google Scholar · View at Scopus
  7. S. Horikoshi, H. Hidaka, and N. Serpone, “Environmental remediation by an integrated microwave/UV-illumination method. 1. Microwave-assisted degradation of rhodamine-B dye in aqueous TiO2 dispersions,” Environmental Science and Technology, vol. 36, no. 6, pp. 1357–1366, 2002. View at Publisher · View at Google Scholar
  8. J. Literak and P. Klan, “The electrodeless discharge lamp: a prospective tool for photochemistry. Part 2. Scope and limitation,” Journal of Photochemistry and Photobiology A, vol. 137, no. 1, pp. 29–35, 2000.
  9. S. Horikoshi, H. Hidaka, and N. Serpone, “Environmental remediation by an integrated microwave/UV illumination technique VI. A simple modified domestic microwave oven integrating an electrodeless UV-Vis lamp to photodegrade environmental pollutants in aqueous media,” Journal of Photochemistry and Photobiology A, vol. 161, no. 2-3, pp. 221–225, 2004. View at Publisher · View at Google Scholar
  10. N. H. Lee, H. J. Oh, S. C. Jung, W. J. Lee, D. H. Kim, and S. J. Kim, “Photocatalytic properties of nanotubular-shaped TiO2 powders with anatase phase obtained from titanate nanotube powder through various thermal treatments,” International Journal of Photoenergy, vol. 2011, Article ID 327821, 7 pages, 2011. View at Publisher · View at Google Scholar
  11. S. H. Park, S. J. Kim, S. G. Seo, and S. C. Jung, “Assessment of microwave/UV/O3 in the photo-catalytic degradation of bromothymol blue in aqueous nano TiO2 particles dispersions,” Nanoscale Research Letters, vol. 5, no. 10, pp. 1627–1632, 2010. View at Publisher · View at Google Scholar · View at Scopus
  12. M. Harir, A. Gaspar, B. Kanawati et al., “Photocatalytic reactions of imazamox at TiO2 , H2O2 and TiO2/H2O2 in water interfaces: kinetic and photoproducts study,” Applied Catalysis B, vol. 84, no. 3-4, pp. 524–532, 2008. View at Publisher · View at Google Scholar · View at Scopus
  13. R. N. Rao and N. Venkateswarlu, “The photocatalytic degradation of amino and nitro substituted stilbenesulfonic acids by TiO2/UV and Fe2+/H2O2/UV under aqueous conditions,” Dyes and Pigments, vol. 77, no. 3, pp. 590–597, 2008. View at Publisher · View at Google Scholar · View at Scopus
  14. S. Kim, H. Park, and W. Choi, “Comparative study of homogeneous and heterogeneous photocatalytic redox reactions: PW12O40v3s TiO2,” Journal of Physical Chemistry B, vol. 108, no. 20, pp. 6402–6411, 2004. View at Scopus
  15. J. Q. Chen, D. Wang, M. X. Zhu, and C. J. Gao, “Photocatalytic degradation of dimethoate using nanosized TiO2 powder,” Desalination, vol. 207, no. 1–3, pp. 87–94, 2007. View at Publisher · View at Google Scholar
  16. Q. Xiang, J. Yu, P. K. Wong, and M. Chen, “Facile fabrication of mechanochromic-responsive colloidal crystal films,” Journal of Colloid and Interface Science, vol. 357, no. 1, pp. 163–168, 2011. View at Publisher · View at Google Scholar · View at Scopus