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International Journal of Environment Science and Technology
Center for Environment and Energy Research and Studies (CEERS)
ISSN: 1735-1472 EISSN: 1735-2630
Vol. 8, Num. 2, 2011, pp. 351-362

International Journal of Environment Science and Technology, Vol. 8, No. 2, 2011, pp. 351-362

Iron and chromium doped titanium dioxide nanotubes for the degradation of environmental and industrial pollutants

*S. T. Hussain; A. Siddiqa

Nano Science and Catalysis Division, National Center for Physics, Quaid-i-Azam University Complex, Islamabad, Pakistan

*Corresponding Author Email: Tel.: +9251 2077 308; Fax: +9251 2077 395

Received 25 June 2010; revised 12 October 2010; accepted 12 February 2011

Code Number: st11032


Pure titanate nanotubes and titanate nanotubes doped with iron (III) and chromium (III) were fabricated by the hydrothermal treatment in methanol and sodium hydroxide mixture. The fabricated nano tubes have high surface area, high aspect ratio, consisted of very good surface morphology and high metals dispersion. The morphology, crysralline phase, composition were characterized by powdered X-ray diffraction, scanning electron microscopy, transmission electron microscopy, BarrettJoynerHalenda methods and X-ray photoelectron spectroscopy. The results showed that nanotubes possess anatase phase and are composed up of 8-12 nm in diameter and 360-400 nm in length. The band gap of the titanium dioxide nanotubes was determined using transformed diffuse reflectance spectroscopy according to the Kubelka-Munk theory, showed pronounced band gap decrease on doped titanium dioxide nanotubes. The photocatalytic activity of doped nanotubes were evaluated in terms of degradation of phenol and photoreduction of carbon dioxide into methanol and ethanol under Ultra violet and Infra red irradiation. It was found that with iron (III) and chromium (III) doped titanium dioxide nanotubes exhibited much higher photocatalytic activity than undoped titanate nanotubes.

Keywords: Titanium dioxide; Hydrothermal method; Infra red;Phenol degradation; Photocatalyst; Sun irradiation


Following the discovery of nanotube morphology in carbon, many studies have been devoted to the preparation and characterization of various inorganic nanotubular materials (Mohapatra et al., 2007; Goyal et al., 2008). Among these nanostructures, the titanium dioxide nanotubalar materials are of high interest due to chemical inertness, strong oxidizing power, large surface area, non toxicity, high photocatalytic activitry, high cation exchange capacity, strong oxidizer, low cost of production and relatively good stability at elevated temperatures (Khan et al., 2006; Samarghandi et al., 2007; Liang and Li, 2009). This material extensively explored as a catalyst for water splitting and for the production of solar hydrogen (Chen et al., 2005). As a catalyst for the conversion of green house gases into energy producing products for methane and methanol (Chen et al., 2005; Khan et al., 2006). Moreover these nanotubes are widely exploited in lithium ions batteries, electrochemical devices, gas sensors, photoluminescence ion exchange and in photovoltaic dye sensitized solar cells (Kuang et al., 2008).

Recent research on Titanium dioxide (TiO2) nanotubes is mainly focused on the understanding of its strong photocatalytic activity which is useful in environmental pollution remediations, such as air purification, hazardous waste remediation and water purification (Qamar, 2008; Sekabira et al., 2010). The presence of pollutants CO2 , NO2 in air, organic dyes (methylene blue, reactive blue, methyl red etc) and many other organic hydrocarbons (phenol, formaldehyde and gasoline), produced as a result of many industrial processes (manufacture of dyes, food processing, pesticides, polymers) in industrial wastes, have caused the sever environmental problems (Chein and shih, 2007; Ismael et al., 2007; Qamar, 2008). Titanium dioxide material has sufficient band gap energies for specifically promoting or catalyzing a wide range of chemical reactions of environmental interest (Ismael et al., 2007). In particular, it has been used to oxidize industrial pollutants and its conversion into products like of H2O, alcohols and other useful hydrocarbons.

However, powdered photocatalyst have limitations. It needs post treatment separation in a slurry system after photocatalyst reaction. Though this can be overcome by converting TiO2 into nanotubes which resulted in increase surface area and catalytic activity (Fujishima et al., 2006; Khanfekr et al., 2009; Zhu et al., 2009; Rafati et al.,2010). Interest in TiO2 nanotubes photocatalysis increased after the pioneering study of Fujishma and Honda in 1972. Kochkar et al. (2009) discovered the photocatalytic splitting of water on TiO2 electrodes. Furthermore, Coating the nanotubes with transition metals resulted in boosting of their activity (Dmitry et al., 2005; Kochkar et al., 2009).

TiO2 nanotubes were reported first time by Hoyer via template assisted method. Latter on TiO2 based nanotubes (TNTs) of different geometrical shapes and microstructures have been developed through various approaches, for example the electrochemical anodic oxidation of Ti, assisted tempelate method and alkaline hydrothermal treatment (Wang et al., 2004; Khan et al., 2006; Mohapatra et al., 2007; Liang and Li 2009). There are advantages and limitations in each of above mentioned methods like attaining uniform inner diameter of titanium dioxide nanotubes and controlling the morphology, shape and length of the synthesized nanotubes (Wang et al., 2004; Liang and Li 2009).

The most widely usedtemplate-assisted method which utilizes porous alumina, carbon nanotubes or polymer membrane and amphiphilic surfactant as template to construct material with a regular morphology (Macak et al., 2007) also has the disadvantage in pre-fabrication and removal of template and usually results in impurities encapsulation. The highly ordered and self assembled TiO2 nanotubes were discovered by Grimes in 2001 via anodization of Ti foil in fluoride based electrolyte. This method has limitations because it results in low yield and involvement of highly expense fabrication apparatus (Wang et al., 2004; Macak et al., 2007).

Hydrothermal method was reported first time by Kasuga et al. (1998) for preparation of TiO2 nanotubes in one step without use of template, by treating TiO2 with concentrated NaOH at elevated temperature in a tightly closed vessel.

Titanium dioxide nanotube produced by this method have good uniformity, controllable size, large surface area, high reactivity and in the amorphous state (Yury et al., 2000; Liang and Li 2009). The hydrothermal process too has problems for its extensive production, due to low yield. This method could also not produce well separated and crystallized nanotubes.

The mechanism of formation and the morphology (diameter and length, wall thickness, size distribution and size of nanotube agglomerates) of nanotubes are still an issue of debate (Yury et al., 2000; Chen et al., 2002a; Sun and Li 2003). Hydrothermal methods of TNTs formation using TiO2 as raw material (in the range of temperature between 110oC-180oC and time of 24-96 h) under high molar concentration of aqueous NaOH (10 M), has been reported earlier. In the present study, the limitation of long reaction time, high temperature, and highly alkali concentration have been overcome using NaOH and methanol mixture rather than water. This resulted in nanotubes formation at low temperature (90 oC), reaction time (8 h) and at stirring rate of 300 rpm

In the present study a new synthesis procedure for the production of Fe/Cr doped and undoped TiO2 nanotubes via hydrothermal synthesis from TiO2 nanoparticles and its application for the degradation of organic waste, like phenol and carbon dioxide conversion to alcohol using UV radiation, is reported. The effect of dopant on degradation of phenol, conversion of carbon dioxide to alcohols and on its optical properties were also studied, the results compared with other studies described above. The data suggest the improvement not only in the synthesis, but also in its industrial applications. The study was carried out in January-March , 2010 at the Nanoscience Catalysis Division, National Centre for Physics, Quaid-i-Azam University, Islamabad, Pakistan.



Titanium dioxide, anatase, sodium hydroxide (NaOH), Methanol, Hydrochloric acid (HCl), phenol, FeCl3 and CrCl3 were obtained from Aldrich and were used without further purification. Ultra pure water was used without purification in the whole experiment.

Preparation of Titanium dioxide nanotubes

Titanium dioxide nanotubes were produced using hydrothermal method similar to that described in literature (Yury et al., 2000) with the modification of using methanol than water. In typical nanotube preparation, 3 g of the TiO2 powder was mixed with 300 mL of 2M NaOH in methanol, followed by hydrothermal treatment in a Teflon-lined autoclave high-pressure stainless steel at 90 °C for 8 h and at stirring speed of 300 rpm. After hydrothermal treatment the precipitates were separated through filteration and washed with 0.1M HCl and distilled water numerous times until the pH of the filterate turned to 7. The resulting sample was dried in oven at 100 °C overnight to get TNTs (titanium dioxide nanotubes) and labelled as A-TNTs for undoped titanium dioxide nanotubes.

Prepration of Fe/Cr doped Titanium nanotubes

Fe/Cr-codoped TiO2 nanotubes were prepared as follows: The synthesized titanium dioxide nanotube (A-TNTs), 1 g, was stirred with 100 mL aqueous solutions containing 0.1 g each of FeCl3, CrCl3 for 10 min. The solution was transferred into a stainless steel autoclave with a Teflon lined autoclave, which was sealed and maintained at 90 °C for 2 h under H2-pressure of 25 bar to dope titanium dioxide nanotubes by ion exchange treatment. The H+ ion existing within nanotubes was ion exchanged with above referred metal ions. Subsequently, the resultant materials were centrifuged, washed and dried at 60 °C for 4 h to get modified titanium dioxide nanotubes. These samples were labelled as B-TNTs for Fe/Cr co-doped titanium dioxide nanotubes.

Photocatalytic activity

The degradation of phenol and conversion of CO2 were investigated in photocatalytic batch reactor setup as shown in Fig. 1a and b. In two separate experiments 0.5 g of A-TNTs and B-TNTs were added in 0.01M phenol for phenol degradation while for conversion of CO2, 0.2 g of A-TNTs and B-TNTs were suspended into 0.2 N NaOH solution with pure CO2 bubbling at the rate of 100 mls/min. In both systems a mercury lamp (Ultra-Violet Products Inc., USA; LF-204.LS), UVC (254 nm) was placed on the top of reactor. The reaction was carried out for 1-2 h with vigorous stirring (300 rpm) at room temperature. After completion of reaction TNTs were separated through filteration using milipore filter paper (with the pore size of 125mm). The filterate analyzed using GC/MS after the chloroform extraction method.


The microstructures and morphology of the A-TNTs and B-TNTs were observed using Transmission Electron Microscope S-3500 N with Absorbed Electron Detector S-6542 (Hitachi Science System Ltd) and SEM scanning electron microscopy with energy dispersive X-ray spectrometer (SEM-EDX, Philips XL30, EDAX DX4). XRD patterns were recorded using a Scintag XDS 2000 D8 diffractometer equipped with CuKá radiation of wavelength of 1.5406 A° in the 2è range 20°80°with a step size of 0.02° to evaluate the crystallinity, phase and structure. Brunauer Emmett Teller (BET) measurements were done to determine specific surface area nitrogen adsorptiondesorption and average pore volume was also evaluated from the data using the BarretJoynerHalender (BJH) method. EDX (Inca Energy, Oxford Instrument Microanalysis, Ltd) were used to determine the surface comparison of samples under specified conditions of 20 keV, 25 mm working distance and magnification varying from x 300-1000.

Diffuse reflectance spectroscopy (DRS) was used for the optical characterization of TiO2 nanotubes. All spectra were taken at room temperature in the range of 200-1000 nm on Lambda-950 Perkin-Elmer.

The chemical status and shift of the catalyst surface due to doping were analyzed by X-ray photoelectron spectroscopy (XPS) using a VG Microtech MT500 spectrometer, operated with a constant pass energy of 50 eV and with Mg Ká radiation as the excitation source (= 1253.6 eV). The catalyst was pressed into a pellet, and then adhered on sample holder by carbon tape.


The use of H2O in the previous study results in the formation of rutile/anatase nanotubes mixture with low yield. The staring TiO2 nanoparticles with mixed phases on anatase and rutile could be separated well into TiO6 octahedra in the NaOH basic solution and methanol which has boiling point of 64.7 °C as compared to H2O. This is reason that in our process nanotubes are formed at much lower temperature, lower pressure and in considerably less time. For the rearrangement of TiO6 octahedra, methanol molecules play the role of bridges between surface OH groups of different octahedral which share only one common yertex, using the two lone pairs of electrons on the oxygen. The deprotonated methylate produced from methanol can chelate TiO6, that is beneficial to the edge-sharing polycondesation between TiO6 octahedra to form anatase phase rather than rutile phase nanotubes in the hydrothermal conditions.

The phase and crystal structure of TNTs before and after calcinations in air at 450 °C for 2 h were investigated by XRD pattern and shown in Fig. 2a and b for undoped and doped TNTs. The intensities and positions of the observed peaks are in agreement with literature values (Zhuang et al., 2007). The XRD peaks were sharp which suggests that synthesized nanotubes have relatively high crystallinity and attributable to the anatase phase (indicated by peak 24). The peaks became sharper and broader after doping which demonstrates that cryatallanity of nanotubes enhances with the doping.

BET specific surface area of doped and undoped TNTs is much higher to the TiO2 nanoparticles. BET surface area has no effect on the phase of the TNTs but has an effect on the photcatalytic degradation reaction (Hussain et al., 2009). Doping on titanium dioxide nanotubes with metals resulted in increase in BET surface area and pore volume. Larger surface area increased adsorption/ desorption capacity and consequently good photocatalytic activity (Diebold, 2002; Hussain et al., 2009). Table 1 presents the measured surface area of the prepared titanium dioxide nanotubes; the surface area of the commercial TiO2 is also included for comparison. Fig. 3a and b and Fig. 4a and b shows the SEM and TEM image of doped and undoped TNTs. As seen in the SEM image, TiO2 nanotubes have had obvious tubular and uniform morpholgy with an average diameter of 8-12 nm and with narrow size distribution.. The dispersion of Fe/Cr on the nanotubes is uniform as depicted in Fig. 3b .

TEM analysis verified that tubes were hollow with an open end having needle shape structures. Furthermore, TEM pattern shows that these tubes are uniform, single walled and are upto several hundred nm in length. No TiO2 nanoparticles exist around the nanotubes, proving high conversion of nanoparticles into nanotubes under employed experimental conditions. Moreover, the chemical composition and respective percentage of each atom present in the samples, was analyzed by EDX. Table 2 presents the percentages of O, Ti, Na, Fe and Cr elements confirming the formation of doped and undoped TNTs.

The DRS studies

The band gap of samples was measured by Kubelka-Munk function F(R) which is related to the the diffuse reflectance, R, of the sample according to the following relation (Diebold 2002; Hussain et al., 2009).

F (R) = (1-R)2/ 2R

Where ÌR´Ì is the absolute value of reflectance. The energy bandgap of the doped and Fe/Cr doped TNTs were calculated from their diffuse-reflectance spectra by plotting the square of the Kubelka-Munk function F(R)2 vs energy in electron volts. The linear part of the curve was extrapolated to F(R)2 = 0 to get the direct energy bandgap. The optical band gap of all samples was determined by the above method.

Fig. 5 shows the comparative the UVvis diffuse reflectance spectrum of A-TNTs, B-TNTs taken at room temperature in the range of 200-800 nm. It is clear from Fig. 4 that doping transition metals into titanium dioxide nanotubes tune the optical band gap in comparison to undoped TNTs, thus shifting UV absorption to visible-light absorption and band gap narrowing. The band gap is reduced with doping of TNTs with Fe and Cr (Quan et al., 2005; Xu et al., 2005a; Kochkar et al., 2009) which was determined by K-Munk function. The narrower band gap, the more easily an electron is excited from the valence band to the conduction band. The differences in the band gap and light absorption property lead to different photocatalytic behavior. The UVvis diffuse reflectance spectra are in good agreement with the observed photocatalytic activity (Kubo et al., 2006).

Fig. 6a and b show the bandgap calculation of A-TNTs, B-TNTs from K-Munk function, respectively. The direct band gap energies estimated from the intercept of the tangents to the plots are 3.25 eV and 1.85 eV for the samples A-TNTs and B-TNTs, respectively. The decrease in band gap energy of B-TNTs can be ascribed to Fe/ Cr atom incorporated into the lattice of titanium dioxide. Thus, it induces a larger red-shift and bandgap narrowing thus changing the crystalline and electronic structures (Xu et al., 2005a; Kochkar et al., 2009).

It was also found, that constitution of the titanium dioxide nanotubes (doped and undoped TiO2) also plays an important role in its photoactivity This change in energy bandgap is directly reflected in the photocatlytic activity studies, where appreciable change is observed due doping (Dmitry et al., 2005; Xu et al., 2005b).

TiO2 nanoparticles were transformed to TNTs after hydrothermal treatment. However, the exact mechanism of formation and the morphology of TNTs is still subject of debate. There are few reports about the growth mechanism of titanium dioxide (Kubo et al., 2006). Kasuga et. al. (1998) proposed that TNTs are formed during the acid washing step (Chen et al., 2002a; Kubo et al., 2006). The nanotubes obtained after hydrothermal synthesis, showing very clear morphology and well defined structure. The nanotubes grow extensively with the length of several hundred nanometers with smooth tubular surfaces (Zhang et al., 2004).

From the results of present work and previous reports we proposed a plausible mechanism of formation of nanotubes. Certain Ti-O-Ti building units in titanium dioxide are broken down via alkali hydrothermal treatment of titanium dioxide with NaOH, resulting in the formation of new co-ordination i.e.,TiONa and TiOH , lateron. Some of Na+ ions were expected to be exchanged with H+ ions during acid treatment and at this stage titanate sheets were exfoliated into layered nanosheets which subsequently scroll and form nanotubes at high temperature and high pressure to avoid electrostatic repulsions within the charges and to minimize the steric repulsions between the sheet edges while the tubular morphology is retained (Chen et al., 2002b; Liu et al., 2002; Zhang et al., 2004). These H+ ions were then exchanged with Fe3+/Cr3+ while reaction of titanium dioxide nanotubes with their respective salts to obtain doped titanium dioxide nanotubes (Zhang et al., 2004).

To study the surface composition and chemical states of the synthesized nanotubes, the doped and undoped TNTs (A-TNTs and B-TNTs) were also analyzed by XPS and its XPS spectra are shown in Fig. 7a and b. The individual peaks of O1s at 529.5 eV and Ti 2p at 458.2 and 463.9 eV (Liu et al., 2002; Huogen et al., 2007) can be clearly seen in the high-resolution spectra (Fig. 7a and b), which mean that chemical state of the sample is Ti4+ bonded with oxygen (Ti4+ O), which has been modified by iron and chromium doping. The binding energy of the Ti 2p3/2 and 2p1/2 band in case of doped Cr2O3/Fe2O3 TiO2 samples was found to be higher than that of the pure TiO2. This shift towards higher side, could be attributed to an atomic dispersion of iron and chromium on TiO2, and the formation of a TiOCr/ TiOFe bond (Chen et al., 2002b; Kim et al., 2006; Huogen et al., 2007).

Photocatalytic degradation of phenol

The TiO2 anatase is the main catalyst used in the contaminants photodegradation. However, the photocatalytic activity of TiO2 nanotubes has been little explored in the literature (Kim et al., 2006; Huogen et al., 2007). Thus, a detailed study of the photocatalytic properties of TiO2 nanotubes is needed. In this study, photocatalytic activity of the mesoporous titanium dioxide nanotube composites was evaluated by photocatalytic phenol degradation, the results are shown in Fig. 8, under infra-red (IR) and visible light illumination. The degradation kinetics was computed after every 30 min by the change in phenol concentration (1 g/L) employing UVvisible spectrometry as a function of irradiation time. The phenol conversion is estimated using the following equation (Hou et al., 2007).

Phenol Conversion (%) = [Phenol]0 - [Phenol]t / [Phenol]0 x100

Where [Phenol]0 is the initial concentration of phenol, [Phenol]t is the concentration of phenol after time "t". The study of Fig. 8 indicates that Fe/Cr doped nanotubes decompose phenol more rapidly than does titanium dioxide nanotubes alone under UV light. Similar trend is observed in case of IR irradiation.

The photocatalytic decomposition of phenol is remarkably accelerated by the doped-TNTs photocatalysts prepared in the present work. This may be due to the inhibition of a spontaneous recombination between the hole and electron occurring on the surface of excited TNTs (Xu et al., 2005b) by the metals deposited on the TNTs surface. The photodegradation efficiency of titanate nanotubes is 35 %±3, while after doping the efficiency increased to 75 %±3 under IR irradiation. Metal ion doping influence the photoactivity of TiO2 by electron or hole traps. Where the trap causes the formation of some active species that benefit degradation of phenol, here the electron scavenger effect of Cr3+/Fe3+ prevents the recombination of electron and hole pairs thus resulting in increase of the efficiency of photodegradation process (Kim et al., 2006; Hou et al., 2007). In Fe/Cr- doped samples, electrons are either directly trapped at Ti (IV) surface sites (form Ti3+) or in deeper Fe (III)/ Cr (III) sites (form Cr2+/Fe2+). In this case, the trapped electron can be easily transferred from Cr2+/Fe2+ to a neighboring surface Ti4+ because of the proximity of the energy levels (Dmitry et al., 2005; Huogen et al., 2007; Hou et al., 2007). As a result, the photocatalytic activity is improved after the doping. The proposed mechanism of process is presented in Fig. 9. The titanium dioxide nanotubes fabricated through hydrothermal method showed large surface are and high reactivity. Moreover, doping of titanium dioxide nanotubes with transition metals like chromium and iron, resulted in the enhanced photocatalytic properties because of the decrease bandgap. These materials provide sufficient negative and positive redox potential, which accelerate the degradation process.

Conversion of CO2 + H2O by solar energy

The conversion of CO2+H2O into alcohol by the synthesized undoped and doped titanium dioxide nanotubes was evaluated under UV and IR radiation, respectively and presented in Fig. 10a and b. The comparative stdudy of Fig. 10a and b reveals that the doped TNTs show considerably higher conversion of CO2 + H2O in comparison with the undoped nanotubes under both IR and UV irradiation. CO2 conversion is calculated using the following formula (Huogen et al., 2007).

CO2 conversion (%) = [CO2]t/[CH3OH] t x 100

Where, [CO2]t = CO2 conversion at time t. [CH3 OH]t= Formation of CH3OH at time t. When titanium dioxide absorbs UV radiation from sunlight or illuminated light source, it will produce pair of electrons and holes. The electrons of valence band are excited when illuminated by light. The excess energy of this excited electro promoted the electron to the conduction band of titanium dioxide therefore producing the negative electron (e-) and positive hole (h+) pair within the catalyst (Xu et al., 2005a). A portion of this photo-excited electron-hole pairs diffuse to the surface of the catalytic particle (electron hole pairs are trapped at the surface) and take part in the chemical reaction with the adsorbed donor (D) or acceptor (A) molecules (Syoufian et al., 2007). The positive holes can oxidize donor molecules i.e., break apart water molecules to form hydrogen gas and hydroxyl radicals which combines with carbon to form alcohol, whereas the negative electrons can reduce appropriate electron acceptor molecules i.e., react with oxygen molecules to form super oxide anion (Fig. 9), illuminated TiO2 photocatalysts can decompose and mineralize organic compounds by participating in a series of oxidation reactions leading to carbon dioxide to harmless substance that can be released to the environment (Xu et al., 2005b; Syoufian et al., 2007). This cycle continue when the sun light is available. The energy needed to activate TNTs is 3.2 eV or more, which nearly corresponds to UV radiation wavelength of 380 nm or less. This makes it possible to use the sun as illumination source, since about 4-6 % of the solar energy that reaches the earth's surface is less than 400 nm. This process is referred to as heterogeneous photocatalysis or more specifically, photocatalysis oxidation (PCO). The energy difference between valence band and conduction band is referred as band gap (Jin and Shiraishi, 2004).

Hereby it is proposed that the Fe3+ and Cr3+ presence inside the lattice of TiO2 nanotubes, induces a delocalized electron density within CO2+H2O structure that promotes the adsorption of the molecule on to the surface. This effect could support the reaction pathway to the mineralization on to TiO2 surface with consequent yields of intermediate species and creates extra energy due to presence of dopand which results in the breakage of H-OH and C-O bonds. It is speculated that molecules can adsorb through the formation of Ti+4 (surface) ð electron or OH (surface) ð electron type complex and latter is related to the production of products. For both type of adsorption, the nature of promoter related to their withdrawing or donor capacity played a major role. All types of Lewis and Bronsted-Lowry sites are generally present at various extents on the lattice of TiO2 nanotubes (Jin and Shiraishi, 2004; Syoufian et al., 2007). In the CO2 + H2O conversion to alcohol, two important species are involved in the process: H+ (hydrogen radical) and CO2- (carbon dioxide anion radical). The incident photons are observed by TiO2 and photoexcited electron (e-) and positive hole (h+) are formed in the catalyst due to presence of Fe3+ and Cr3+ ( i.e., by a charge transfer to the excited site of Fe-Cr-Ti-O). Furthermore, the photoexcited electrons and holes in the lattice are separated and trapped by appropriate sites of Fe-TiO2 and Cr-TiO2. The whole react with H2O adsorbed on the surface of the catalyst giving rise to oxygen and H+. The H+ ions interact with excited electrons, resulting the formation of H+ radical. This is enhanced by the presence of multiple active sites of Fe and Cr coupled with TiO2. The interaction of all these species results in the formation of alcohol. The role that which types of sites are responsible for the photocataytic reaction is difficult to assess. This study is under way at present and will be published later.


In this work, mesoporous nanotubes by hydrothermal treatment in aqueous sodium hydroxide solution have been synthesized. Direct hydrothermal synthesis method is easy and efficient to synthesize pure and titanate nanotubes doped with transition metals. Using methanol and sodium hydroxide mixture, the considerable decrease in reaction time and reaction temperature was achieved.

High aspect ratio of TiO2 undoped and doped TiO2 nanotubes of homogenous length were synthesized. XRD result suggests that cryatallanity enhanced after annealing, while the band gap and BET surface area increased after doping. TNTs revealed a larger specific surface area and a higher pore volume than that of nanoparticles, leading to an obvious enhancement of the photocatalytic activity for the photocatalytic degradation of pollutants (CO2 and phenol) under UV and IR irradiation. Doping of metals, such as iron and chromium on the surface of TNTs resulted in enhanced rate of the photocatalytic decomposition of organic compounds in aqueous solutions.

In conclusion, TiO2 nanotubes are found to be feasible and attractive to be used in further investigation of CO2 reduction for CO2 environment management. The first three conclusion points exclusively explained the scientific achievement. The low temperature, low pressure with homogeneous tube length, very good aspect ratio and high surface area with band gap in the UV range will directly affect the economics of all the process.


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