# Effect of Al-Cu Bimetallic Components in a TiO2 Framework for High Hydrogen Production on Methanol/Water Photo-Splitting

Authors: A-Young Kim; Misook Kang
Journal: International Journal of Photoenergy
 (2012)

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## Abstract

This study investigated the production of hydrogen over TiO2, Cu-TiO2, Ag-TiO2, and Cu-Ag-TiO2 photocatalysts incorporated with Cu and Ag ions by a solvothermal method. The Ag metal (200, 220, and 311 plane) peaks at 2θ=44.50, 64.00, and 77.60ο were presented in the Ag-incorporated TiO2 catalysts. The CuO component (Cu2p3/2 and Cu2p1/2 at 930.4 and 949.5 eV) was exhibited in the X-ray photon spectroscopy (XPS) band of the Cu-incorporated TiO2 photocatalyst. All the absorption plots in the Cu-, Ag-, and Cu-Ag-incorporated catalysts showed excitation characteristics; an asymmetric tail was observed towards a higher wavelength due to scattering. The intensity of the photoluminescence (PL) curves of Cu-Ag-TiO2s was smaller, with the smallest case being observed for Cu(0.05)-Ag(0.05)Ti(0.9)O2 and Cu(0.03)-Ag(0.07)Ti(0.9)O2. Based on these optical characteristics, the production of H2 from methanol/water photodecomposition over the Cu(0.03)-Ag(0.07)Ti(0.9)O2 photocatalyst at 8,750 mmol after 8 h was greater than that over the other photocatalysts.


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## Body

## 1. Introduction

The technology for generating hydrogen by the splitting of water using a photocatalyst has attracted much attention. The principle of photocatalytic water decomposition is based on the conversion of light energy into electricity in a semiconductor on exposure to light [1–3]. Semiconductor materials such as MTiO3 [4, 5] and TiOxNy [6, 7] have been widely investigated due to their low band gap and high corrosion resistance. However, the photocatalytic decomposition of water on a TiO2 photocatalyst is ineffective as the amount of hydrogen produced is limited by the rapid recombination of holes and electrons, resulting in the formation of water. Recently, the production of hydrogen has been extended to the photodecomposition of methanol (CH3OH), which has a lower splitting energy than water. The following overall methanol decomposition reaction was proposed [8, 9]:(1)MeOH(l)↔HCHO(g)+H2(g),G1°=64.1kJmol-1,(2)HCHO(g)H2O(l)↔HCO2H(l)+H2(g),G2°=47.8kJmol-1,(3)HCO2H(l)⟷CO2(g)+H2(g),G3°=-95.8kJmol-1.(4)Finally,MeOH(l)+H2O(l)↔CO2(g)+3H2(g),ΔG°=16.1KJmol-1.The decomposition energy for methanol is smaller than 0.7 eV, compared to 1.2 eV for water splitting. Most investigations on the production of hydrogen via methanol photodecomposition have focused onMxOy (M = Cd or Zn) [10, 11] and noble metal (Cu, Ag, Pd, Pt, Au)-doped TiO2 [12–16], which can be used to activate the photocatalysts using UV light with longer wavelengths. However, the number of known photocatalysts is limited, and their activities remain low. New photocatalysts possessing greater hydrogen-producing activity under visible light irradiation need to be developed. Moreover, hydrogen-based energy offers the significant advantage of being environmentally friendly. In our previous study [17], a new material, Cu-TiO2, where CuxO was substituted into the TiO2 framework, was investigated as a conducting component to reduce the large band gap of pure TiO2. The structural effect of the catalyst on photocatalysis was also evaluated using Cu-incorporated TiO2 photocatalysts with anatase and rutile structures. The production reached 16,000 μmol after 24 h over Cu-TiO2 with a rutile structure for water/methanol decomposition. Additionally, in our other paper [18], we reported about the synthesis and characterization of AgxO and found that the hydrogen production from methanol photodecomposition over a mixture of AgxO and TiO2 was remarkably increased. Moreover, it was further enhanced when AgxO thermally treated at 100°C was added, and the production peaked at 17,000 μmol after 24 h. However, the economic evaluation of this hydrogen production process remained poor, and any Ag and Cu metals remaining after the reaction showed a tendency to precipitate at the bottom of the reactor, where they were rapidly reduced. Subsequently the catalyst was rapidly deactivated.Therefore, in order to overcome these disadvantages, we prepared a new catalyst in which two metals with different reduction/oxidation abilities were embedded into the TiO2 framework. We investigated the production of hydrogen from the methanol/water photodecomposition over TiO2, Cu(0.1)-Ti(0.9)O2, Ag(0.1)-Ti(0.9)O2, Cu(0.05)-Ag(0.05)Ti(0.9)O2, Cu(0.03)-Ag(0.07)Ti(0.9)O2,  and Cu(0.07)-Ag(0.03)Ti(0.9)O2 photocatalysts in which Cu and Ag ions were incorporated into the TiO2 framework with an anatase structure, prepared using a solvothermal method. To determine the relationship between Cu and Ag species and the catalytic performance for the production of H2, these photocatalysts were examined using X-ray diffraction analysis (XRD), X-ray photon spectroscopy (XPS), and UV-visible and photoluminescence (PL) spectroscopy.


## 2. Experimental

### 2.1. Preparation of Photocatalysts

The photocatalysts were prepared using the conventional solvothermal method, as shown in Figure1. To prepare the sol mixture, titanium tetraisopropoxide (TTIP, 99.95%), copper nitrate (Cu(NO3)2, 99.9%), and silver nitrate (AgNO3, 99.9%), all supplied by Junsei Chemical (Tokyo, Japan), were used as the titanium, copper, and silver precursors, respectively. After 0.9 mol TTIP was added slowly to 250 mL ethanol, Ag and Cu nitrate (totally 10 mol-% per titanium mole) dissolved with ethanol were added into the titanium solution. The mixture was stirred homogeneously for 1 h, and the pH was maintained at 3.0. The final solution was stirred homogeneously and moved to an autoclave for the thermal treatment. TTIP, silver, and copper nitrates were hydrolyzed via the OH groups during thermal treatment at 473 K for 8 h under a nitrogen environment at a pressure of approximately 10 atm. The resulting precipitate was washed with distilled water until pH = 7.0 and then dried at 353 K for 24 h. The six photocatalysts were pure TiO2, Cu(0.1)-Ti(0.9)O2, Ag(0.1)-Ti(0.9)O2,Cu(0.05)-Ag(0.05)Ti(0.9)O2, Cu(0.03)-Ag(0.07)Ti(0.9)O2,  and Cu(0.07)-Ag(0.03)Ti(0.9)O2.Figure 1
The preparation of six photocatalysts, pure TiO2, Cu(0.1)-Ti(0.9)O2, Ag(0.1)-Ti(0.9)O2, Cu(0.05)-Ag(0.05)Ti(0.9)O2, Cu(0.03)-Ag(0.07)Ti(0.9)O2, and Cu(0.07)-Ag(0.03)Ti(0.9)O2 using a solvothermal method.


### 2.2. Characteristics of the Photocatalysts

The powders for the six synthesized photocatalysts were examined by XRD (MPD, PANalytical, at Yeungnam University Instrumental Analysis Center) with nickel-filtered CuKα radiation (30 kV, 30 mA) at 2θ angles ranging from 10 to 80°, a scan speed of 10° min−1, and a time constant of 1 s. The sizes and shapes of the particles were measured by transmission electron spectroscopy (TEM; H-7600, Hitachi, at Yeungnam University Instrumental Analysis Center) operated at 120 kV. The UV-visible spectra were obtained using a Cary 500 spectrometer with a reflectance sphere over the special range of 200 to 800 nm. PL spectroscopy was also performed to determine the number of photo-excited electron hole pairs using a PL mapping system (LabRamHR, Jobin Yvon, at Korea Photonics Technology Institute Material Characterization Center). It was also used to examine the number of photo-excited, electron-hole pairs for all samples. Samples of 1.0-mm diameter pellets were measured at room temperature using a He-Cd laser source at 325 nm in the reflection mode. XPS measurements of Cu2p,Ag3d, Ti2p, and O1s were recorded with an ESCA 2000 (VZ MicroTech, Oxford, UK) system, equipped with a nonmonochromatic AlK (1486.6 eV) X-ray source. The powders were pelletized at 1.2 × 104 kPa for 1 min, and the 1.0-mm pellets were then maintained overnight in a vacuum (1.0 × 10−7Pa) to remove the water molecules from the surface prior to the measurement. The base pressure of the ESCA system was below 1 × 10−9Pa. Experiments were recorded with a 200-W source power and an angular acceptance of ±5°. The analyzer axis made an angle of 90° with the specimen surface. Wide scan spectra were measured over a binding energy range of 0 to 1200 eV, with pass energy of 100.0 eV. The Ar+ bombardment of the photocatalysts was performed with an ion current of 70 to 100 nA, over an area of 10.0 × 10.0 mm, with a total sputter time of 2400 s divided into 60 s intervals. A Shirley function was used to subtract the background in the XPS data analysis. The O1s, Ti2p, Ag3d, and Cu2p XPS signals were fitted using mixed Lorentzian-Gaussian curves.


### 2.3. H2 Production from Methanol/Water Photo Decomposition over Photocatalysts

The photodecomposition of methanol/water was performed using a liquid photoreactor designed in our laboratory (Figure2). For methanol/water photodecomposition, 0.5 g of the powdered photocatalysts was added to 2.0 L of a 1.0 : 1.0 methanol/water mixture in a 3.0-L Pyrex reactor. UV-lamps (6 × 3 Wcm−2 = 18 Wcm−2, 30 cm length × 2.0 cm diameter; Shinan, Sunchun, Korea), emitting radiation at 365 nm, were used. The methanol/water decomposition was conducted for 30 h, with stirring, with the hydrogen evolution determined after 1 h. The hydrogen (H2) produced during the methanol/water photodecomposition was analyzed using a thermal-conductivity-detector- (TCD-) type gas chromatograph (GC, model DS 6200; Donam Instruments Inc., Gyeonngi-do, Korea). To determine the products and intermediates, the GC was directly connected to the methanol/water decomposition reactor. The GC conditions were as follows: column: Carbosphere (Alltech, Deerfield, IL, USA), injection temp.: 160°C, initial temp.: 100°C, final temp.: 100°C, and detector temp.: 200°C.Figure 2
The liquid photoreactor used for H2 production via methanol/water photodecomposition. Reaction conditions: volumetric ratio of CH3OH/H2O = 1; catalyst weight per 2.0 L solution, 0.5 g; UV intensity at 365 nm, 18 W m−2; batch system.


## 2.1. Preparation of Photocatalysts

The photocatalysts were prepared using the conventional solvothermal method, as shown in Figure1. To prepare the sol mixture, titanium tetraisopropoxide (TTIP, 99.95%), copper nitrate (Cu(NO3)2, 99.9%), and silver nitrate (AgNO3, 99.9%), all supplied by Junsei Chemical (Tokyo, Japan), were used as the titanium, copper, and silver precursors, respectively. After 0.9 mol TTIP was added slowly to 250 mL ethanol, Ag and Cu nitrate (totally 10 mol-% per titanium mole) dissolved with ethanol were added into the titanium solution. The mixture was stirred homogeneously for 1 h, and the pH was maintained at 3.0. The final solution was stirred homogeneously and moved to an autoclave for the thermal treatment. TTIP, silver, and copper nitrates were hydrolyzed via the OH groups during thermal treatment at 473 K for 8 h under a nitrogen environment at a pressure of approximately 10 atm. The resulting precipitate was washed with distilled water until pH = 7.0 and then dried at 353 K for 24 h. The six photocatalysts were pure TiO2, Cu(0.1)-Ti(0.9)O2, Ag(0.1)-Ti(0.9)O2,Cu(0.05)-Ag(0.05)Ti(0.9)O2, Cu(0.03)-Ag(0.07)Ti(0.9)O2,  and Cu(0.07)-Ag(0.03)Ti(0.9)O2.Figure 1
The preparation of six photocatalysts, pure TiO2, Cu(0.1)-Ti(0.9)O2, Ag(0.1)-Ti(0.9)O2, Cu(0.05)-Ag(0.05)Ti(0.9)O2, Cu(0.03)-Ag(0.07)Ti(0.9)O2, and Cu(0.07)-Ag(0.03)Ti(0.9)O2 using a solvothermal method.


## 2.2. Characteristics of the Photocatalysts

The powders for the six synthesized photocatalysts were examined by XRD (MPD, PANalytical, at Yeungnam University Instrumental Analysis Center) with nickel-filtered CuKα radiation (30 kV, 30 mA) at 2θ angles ranging from 10 to 80°, a scan speed of 10° min−1, and a time constant of 1 s. The sizes and shapes of the particles were measured by transmission electron spectroscopy (TEM; H-7600, Hitachi, at Yeungnam University Instrumental Analysis Center) operated at 120 kV. The UV-visible spectra were obtained using a Cary 500 spectrometer with a reflectance sphere over the special range of 200 to 800 nm. PL spectroscopy was also performed to determine the number of photo-excited electron hole pairs using a PL mapping system (LabRamHR, Jobin Yvon, at Korea Photonics Technology Institute Material Characterization Center). It was also used to examine the number of photo-excited, electron-hole pairs for all samples. Samples of 1.0-mm diameter pellets were measured at room temperature using a He-Cd laser source at 325 nm in the reflection mode. XPS measurements of Cu2p,Ag3d, Ti2p, and O1s were recorded with an ESCA 2000 (VZ MicroTech, Oxford, UK) system, equipped with a nonmonochromatic AlK (1486.6 eV) X-ray source. The powders were pelletized at 1.2 × 104 kPa for 1 min, and the 1.0-mm pellets were then maintained overnight in a vacuum (1.0 × 10−7Pa) to remove the water molecules from the surface prior to the measurement. The base pressure of the ESCA system was below 1 × 10−9Pa. Experiments were recorded with a 200-W source power and an angular acceptance of ±5°. The analyzer axis made an angle of 90° with the specimen surface. Wide scan spectra were measured over a binding energy range of 0 to 1200 eV, with pass energy of 100.0 eV. The Ar+ bombardment of the photocatalysts was performed with an ion current of 70 to 100 nA, over an area of 10.0 × 10.0 mm, with a total sputter time of 2400 s divided into 60 s intervals. A Shirley function was used to subtract the background in the XPS data analysis. The O1s, Ti2p, Ag3d, and Cu2p XPS signals were fitted using mixed Lorentzian-Gaussian curves.


## 2.3. H2 Production from Methanol/Water Photo Decomposition over Photocatalysts

The photodecomposition of methanol/water was performed using a liquid photoreactor designed in our laboratory (Figure2). For methanol/water photodecomposition, 0.5 g of the powdered photocatalysts was added to 2.0 L of a 1.0 : 1.0 methanol/water mixture in a 3.0-L Pyrex reactor. UV-lamps (6 × 3 Wcm−2 = 18 Wcm−2, 30 cm length × 2.0 cm diameter; Shinan, Sunchun, Korea), emitting radiation at 365 nm, were used. The methanol/water decomposition was conducted for 30 h, with stirring, with the hydrogen evolution determined after 1 h. The hydrogen (H2) produced during the methanol/water photodecomposition was analyzed using a thermal-conductivity-detector- (TCD-) type gas chromatograph (GC, model DS 6200; Donam Instruments Inc., Gyeonngi-do, Korea). To determine the products and intermediates, the GC was directly connected to the methanol/water decomposition reactor. The GC conditions were as follows: column: Carbosphere (Alltech, Deerfield, IL, USA), injection temp.: 160°C, initial temp.: 100°C, final temp.: 100°C, and detector temp.: 200°C.Figure 2
The liquid photoreactor used for H2 production via methanol/water photodecomposition. Reaction conditions: volumetric ratio of CH3OH/H2O = 1; catalyst weight per 2.0 L solution, 0.5 g; UV intensity at 365 nm, 18 W m−2; batch system.


## 3. Results and Discussion

### 3.1. Characteristics of the Photocatalysts

Figure3 shows the XRD patterns for the six as-synthesized photocatalysts. Generally, TiO2 and metal-TiO2 photocatalysts with an anatase structure are known to perform well in the decomposition of various organic compounds. The diffraction peaks for the anatase and rutile phases are labeled A and R with the corresponding diffraction planes given in parentheses, respectively [19]. Both pure TiO2 and metal-incorporated TiO2 catalysts showed well-developed anatase structures as synthesized. The Ag metal (200, 220, and 311 plane) peaks at 2θ=44.50, 64.00, and 77.60° were presented in the Ag-incorporated TiO2 catalysts [20] and the intensities increased with increasing amount of loaded Ag. These results indicated that the Ag components partially existed on the external surface of TiO2 and were unlikely to be incorporated into the framework of the anatase structure. However, the Cu component did not appear in any of the catalysts, which indicated its complete insertion into the TiO2 framework. Interestingly, the structural stability of anatase increased when bimetallic two metals, Cu and Ag, were inserted into the TiO2 framework at the same time, compared with when one kind of metal, Cu or Ag, that was inserted. Generally, crystalline domain sizes decrease with increasing line broadening of the peaks. The line broadening of the [101] peak is related to the size of the hexagonal crystalline phase. Scherrer’s equation [21], t=0.9λ/βcosθ, where λ  is the wavelength of the incident X-rays,  β   is the full width at half maximum height (FWHM) in radians, and  θ   is  the diffraction angle, was used to estimate the crystalline domain size. The estimated crystalline domain sizes were 15.04, 13.71, 17.00, 11.80, 15.82, and 15.25 nm for pure TiO2, Cu(0.1)-Ti(0.9)O2, Ag(0.1)-Ti(0.9)O2,Cu(0.05)-Ag(0.05)Ti(0.9)O2, Cu(0.03)-Ag(0.07)Ti(0.9)O2, and Cu(0.07)-Ag(0.03)Ti(0.9)O2 powders, respectively. The results indicated that the grain growths increased and decreased according to incorporation of Ag and Cu, respectively.Figure 3
The XRD patterns of six photocatalysts as-synthesized. (a) TiO2, (b) Cu(0.1)-Ti(0.9)O2, (c) Cu(0.07)-Ag(0.03)Ti(0.9)O2, (d) Cu(0.05)-Ag(0.05)Ti(0.9)O2, (e) Cu(0.03)-Ag(0.07)Ti(0.9)O2, and (f) Ag(0.1)-Ti(0.9)O2.Figure4 shows TEM images of the particle shapes of the six photocatalysts. A relatively uniform mixture of rhombic and cubic particles was observed with sizes ranging from 10 to 20 nm. The particles were slightly decreased in size when Cu was added but enlarged with Ag addition. The size was the smallest in Cu(0.05)-Ag(0.05)Ti(0.9)O2, which corresponds to the XRD patterns shown in Figure 3.The TEM images of six photocatalysts as-synthesized.
(a)(b)(c)(d)(e)(f)Table1 summarizes the atomic composition of the six photocatalysts. The compositions were estimated using energy dispersive X-ray (EDAX) analysis. The ratios of metal(mono or bimetal)/Ti were 0.20, 0.10, 0.16, 0.10, and 0.11 in Cu(0.1)-Ti(0.9)O2, Ag(0.1)-Ti(0.9)O2,  Cu(0.05)-Ag(0.05)Ti(0.9)O2, Cu(0.03)-Ag(0.07)Ti(0.9)O2,  and Cu(0.07)-Ag(0.03)Ti(0.9)O2 powders, respectively. Similar to the XRD results, the incorporation of Ag component into the TiO2 framework was more difficult than that of Cu component.Table 1
The atomic composition of the six photocatalysts.
Atomic composition (%)SamplesMetal/TiOTiCuAgTiO2—7.16728.33——Cu(0.1)-Ti(0.9)O20.2076.9919.113.89—Ag(0.1)-Ti(0.9)O20.1074.0323.56—2.41Cu(0.05)-Ag(0.05)Ti(0.9)O20.1169.8527.242.110.79Cu(0.03)-Ag(0.07)Ti(0.9)O20.1670.7825.252.031.94Cu(0.07)-Ag(0.03)Ti(0.9)O20.1071.6425.270.861.74Figure5 shows the UV-visible spectra of the six photocatalysts. The absorption of the Ti4+ tetrahedral symmetry normally appears at around 350 nm [22], which is assigned to L-L   (P→π or P→π* ) transitions localized on the oxygen. In the figure, the absorption bands are around 350 nm for all the photocatalysts, but the intensity of absorption for pure TiO2 is stronger than for metal-incorporated TiO2. The Cu-incorporated materials broadly absorbed at around 650 nm with remarkable intensity, which is allowed by the large spin-orbit coupling constant of the d-d transfer of copper, and the band observed in the visible region can be rationalized in terms of symmetry arguments. Otherwise, the broad band in the Ag-incorporated catalysts at 380~600nm was attributed to Ag→O metal-to-ligand charge transfer (MLCT) transitions. The two broad bands observed in the wavelength interval 350–600 nm were therefore assigned to the MLCT and d-d transitions, which indicated that the band gap was narrowed in the Ag- and Cu-inserted TiO2 catalysts, leading to higher photocatalytic performance.Figure 5
The UV-visible spectra of six photocatalysts as-synthesized. (a) TiO2, b) Cu(0.1)-Ti(0.9)O2, (c) Cu(0.07)-Ag(0.03)Ti(0.9)O2, (d) Cu(0.05)-Ag(0.05)Ti(0.9)O2, (e) Cu(0.03)-Ag(0.07)Ti(0.9)O2, and (f) Ag(0.1)-Ti(0.9)O2.Figure6 shows the PL spectra of the six photocatalysts. The PL curve suggests that the electrons in the valence band were transferred to the conduction band, after which the excited electrons were stabilized by photoemission. In general, it is very important that the PL intensity increases with the increasing number of emitted electrons resulting from the recombination between excited electrons and holes, and, consequently, that the photoactivity decreases [23]. In particular, the PL intensity decreases to a greater extent in the presence of a metal that can capture excited electrons or exhibit conductivity, via the relaxation process. The PL curve of pure TiO2 showed emission at 370–450 nm as a curve type. The band broadening was attributed to the overlapped emission from the higher and lower excited states to the ground states. The pattern of the Ag- or Cu-incorporated catalysts showed two curves—at 360 nm and 400 nm—which were attributed to the band gap between the incorporated metals, Ag or Cu, respectively, and that of pure anatase TiO2. Additionally the curves were shifted to a lower wavelength, and the PL intensity decreased significantly with decreasing metal insertion, probably due to the electron-capturing actions of the metal atoms from conduction band of TiO2. Particularly when Ag component was inserted into the TiO2 framework, the PL intensity was largely reduced. Consequently, the PL intensity varied according to whether the added metal acted as an electron capturer or not. If the incorporated metals existed on the surface or in the framework of TiO2, they attracted the excited electrons from TiO2, so that the recombination of an electron and a hole was difficult, thus increasing the number of holes over the valence band and generating more OH radicals.Figure 6
The PL spectra of six photocatalysts as-synthesized. (a) TiO2, (b) Cu(0.1)-Ti(0.9)O2, (c) Cu(0.07)-Ag(0.03)Ti(0.9)O2, (d) Cu(0.05)-Ag(0.05)Ti(0.9)O2, e) Cu(0.03)-Ag(0.07)Ti(0.9)O2, and (f) Ag(0.1)-Ti(0.9)O2.


### 3.2. H2 Production from Methanol/Water Decomposition over the Six Photocatalysts

Figure7 summarizes the evolution of H2 from methanol/water decomposition over the six photocatalysts in a batch-type, liquid photosystem. Over pure anatase TiO2, 200 mmol of H2 were only collected after methanol/water photodecomposition for 8 h, however the amount of H2 gas more increased in the Ag- or Cu-incorporated photocatalysts linearly with increasing time. The H2production was the highest in Cu(0.03)-Ag(0.07)Ti(0.9)O2 at 8,750 mmol and finally reached 20,000 mmol after 30 h. therefore, the simultaneously bimetallic addition of Ag and Cu components had a greater influence on the H2 production during methanol/water photodecomposition than the mono metals, Cu- or Ag-incorporated TiO2. Particularly, metal chunks were observed to be deposited in the reactor after the reaction. These results are evidence for the continuing oxidation/reduction actions between Cu and Ag during the reaction.The evolution of H2 from methanol/water decomposition over the six photocatalysts in a batch-type liquid photosystem. (A) accumulated amount of hydrogen gas and (B) accumulated amount of oxygen gas.  (a) TiO2, (b) Cu(0.1)-Ti(0.9)O2, (c) Cu(0.07)-Ag(0.03)Ti(0.9)O2, (d) Cu(0.05)-Ag(0.05)Ti(0.9)O2, (e) Cu(0.03)-Ag(0.07)Ti(0.9)O2, and f) Ag(0.1)-Ti(0.9)O2.The Cu(0.03)-Ag(0.07)Ti(0.9)O2 particles underwent quantitative XPS analyses before and after the reaction, with the typical survey and high-resolution spectra shown in Figure 8. The Ti2p1/2 and Ti2p3/2 spin-orbital splitting photoelectrons for anatase TiO2s were located at binding energies of 462.0 and 456.4 eV, respectively, and were assigned to the presence of typical Ti4+ [24]. The measured FWHM of the Ti2p3/2 peak was larger before reaction than after the reaction. However, there was no subsequent change. In general, a greater FWHM implies a greater amount of less-oxidized metals. The Cu2p3/2 and Cu2p1/2 spin-orbital splitting photoelectrons for the anatase Cu(0.03)-Ag(0.07)Ti(0.9)O2 photocatalyst before the reaction were located at binding energies of 930.4 and 949.5 eV, respectively, and these bands were assigned to CuO. However, these bands were separated into two peaks at binding energies of 932.5 eV of Cu2p3/2and 952.5 eV of Cu2p1/2, and these bands were assigned to Cu2O [24]. On the other hand, the fresh photocatalyst showed Ag3d5/2 and Ag3d3/2 spin-orbital splitting photoelectrons at binding energies of 366.1 and 372.0 eV, respectively, which were assigned to AgO, but the peak intensities were dramatically decreased after the reaction. This result indicated that the oxidation state of Cu was reduced and the amount of AgO was decreased during the reaction, which enabled their strong involvement in methanol/water decomposition. The O1s region was decomposed into two contributions: metal (Ti4+ or Ti3+)-O (527.5 eV) in the metal oxide and metal-OH (529.5.0 eV). The ratios of metal-OH/metal-O in the O1s peaks were decreased after the reaction compared to that before the reaction. Additionally, the measured FWHM of the O1s peak was larger after reaction than that before, which was attributed to the exposure of Ag or Cu ions from the surface of TiO2.Figure 8
The XPS for Cu2p, Ag3d, Ti2p, and O1s of Cu(0.03)-Ag(0.07)Ti(0.9)O2 before and after the methanol/water photodecomposition reaction: (A) before reaction and (B) after reaction.


## 3.1. Characteristics of the Photocatalysts

Figure3 shows the XRD patterns for the six as-synthesized photocatalysts. Generally, TiO2 and metal-TiO2 photocatalysts with an anatase structure are known to perform well in the decomposition of various organic compounds. The diffraction peaks for the anatase and rutile phases are labeled A and R with the corresponding diffraction planes given in parentheses, respectively [19]. Both pure TiO2 and metal-incorporated TiO2 catalysts showed well-developed anatase structures as synthesized. The Ag metal (200, 220, and 311 plane) peaks at 2θ=44.50, 64.00, and 77.60° were presented in the Ag-incorporated TiO2 catalysts [20] and the intensities increased with increasing amount of loaded Ag. These results indicated that the Ag components partially existed on the external surface of TiO2 and were unlikely to be incorporated into the framework of the anatase structure. However, the Cu component did not appear in any of the catalysts, which indicated its complete insertion into the TiO2 framework. Interestingly, the structural stability of anatase increased when bimetallic two metals, Cu and Ag, were inserted into the TiO2 framework at the same time, compared with when one kind of metal, Cu or Ag, that was inserted. Generally, crystalline domain sizes decrease with increasing line broadening of the peaks. The line broadening of the [101] peak is related to the size of the hexagonal crystalline phase. Scherrer’s equation [21], t=0.9λ/βcosθ, where λ  is the wavelength of the incident X-rays,  β   is the full width at half maximum height (FWHM) in radians, and  θ   is  the diffraction angle, was used to estimate the crystalline domain size. The estimated crystalline domain sizes were 15.04, 13.71, 17.00, 11.80, 15.82, and 15.25 nm for pure TiO2, Cu(0.1)-Ti(0.9)O2, Ag(0.1)-Ti(0.9)O2,Cu(0.05)-Ag(0.05)Ti(0.9)O2, Cu(0.03)-Ag(0.07)Ti(0.9)O2, and Cu(0.07)-Ag(0.03)Ti(0.9)O2 powders, respectively. The results indicated that the grain growths increased and decreased according to incorporation of Ag and Cu, respectively.Figure 3
The XRD patterns of six photocatalysts as-synthesized. (a) TiO2, (b) Cu(0.1)-Ti(0.9)O2, (c) Cu(0.07)-Ag(0.03)Ti(0.9)O2, (d) Cu(0.05)-Ag(0.05)Ti(0.9)O2, (e) Cu(0.03)-Ag(0.07)Ti(0.9)O2, and (f) Ag(0.1)-Ti(0.9)O2.Figure4 shows TEM images of the particle shapes of the six photocatalysts. A relatively uniform mixture of rhombic and cubic particles was observed with sizes ranging from 10 to 20 nm. The particles were slightly decreased in size when Cu was added but enlarged with Ag addition. The size was the smallest in Cu(0.05)-Ag(0.05)Ti(0.9)O2, which corresponds to the XRD patterns shown in Figure 3.The TEM images of six photocatalysts as-synthesized.
(a)(b)(c)(d)(e)(f)Table1 summarizes the atomic composition of the six photocatalysts. The compositions were estimated using energy dispersive X-ray (EDAX) analysis. The ratios of metal(mono or bimetal)/Ti were 0.20, 0.10, 0.16, 0.10, and 0.11 in Cu(0.1)-Ti(0.9)O2, Ag(0.1)-Ti(0.9)O2,  Cu(0.05)-Ag(0.05)Ti(0.9)O2, Cu(0.03)-Ag(0.07)Ti(0.9)O2,  and Cu(0.07)-Ag(0.03)Ti(0.9)O2 powders, respectively. Similar to the XRD results, the incorporation of Ag component into the TiO2 framework was more difficult than that of Cu component.Table 1
The atomic composition of the six photocatalysts.
Atomic composition (%)SamplesMetal/TiOTiCuAgTiO2—7.16728.33——Cu(0.1)-Ti(0.9)O20.2076.9919.113.89—Ag(0.1)-Ti(0.9)O20.1074.0323.56—2.41Cu(0.05)-Ag(0.05)Ti(0.9)O20.1169.8527.242.110.79Cu(0.03)-Ag(0.07)Ti(0.9)O20.1670.7825.252.031.94Cu(0.07)-Ag(0.03)Ti(0.9)O20.1071.6425.270.861.74Figure5 shows the UV-visible spectra of the six photocatalysts. The absorption of the Ti4+ tetrahedral symmetry normally appears at around 350 nm [22], which is assigned to L-L   (P→π or P→π* ) transitions localized on the oxygen. In the figure, the absorption bands are around 350 nm for all the photocatalysts, but the intensity of absorption for pure TiO2 is stronger than for metal-incorporated TiO2. The Cu-incorporated materials broadly absorbed at around 650 nm with remarkable intensity, which is allowed by the large spin-orbit coupling constant of the d-d transfer of copper, and the band observed in the visible region can be rationalized in terms of symmetry arguments. Otherwise, the broad band in the Ag-incorporated catalysts at 380~600nm was attributed to Ag→O metal-to-ligand charge transfer (MLCT) transitions. The two broad bands observed in the wavelength interval 350–600 nm were therefore assigned to the MLCT and d-d transitions, which indicated that the band gap was narrowed in the Ag- and Cu-inserted TiO2 catalysts, leading to higher photocatalytic performance.Figure 5
The UV-visible spectra of six photocatalysts as-synthesized. (a) TiO2, b) Cu(0.1)-Ti(0.9)O2, (c) Cu(0.07)-Ag(0.03)Ti(0.9)O2, (d) Cu(0.05)-Ag(0.05)Ti(0.9)O2, (e) Cu(0.03)-Ag(0.07)Ti(0.9)O2, and (f) Ag(0.1)-Ti(0.9)O2.Figure6 shows the PL spectra of the six photocatalysts. The PL curve suggests that the electrons in the valence band were transferred to the conduction band, after which the excited electrons were stabilized by photoemission. In general, it is very important that the PL intensity increases with the increasing number of emitted electrons resulting from the recombination between excited electrons and holes, and, consequently, that the photoactivity decreases [23]. In particular, the PL intensity decreases to a greater extent in the presence of a metal that can capture excited electrons or exhibit conductivity, via the relaxation process. The PL curve of pure TiO2 showed emission at 370–450 nm as a curve type. The band broadening was attributed to the overlapped emission from the higher and lower excited states to the ground states. The pattern of the Ag- or Cu-incorporated catalysts showed two curves—at 360 nm and 400 nm—which were attributed to the band gap between the incorporated metals, Ag or Cu, respectively, and that of pure anatase TiO2. Additionally the curves were shifted to a lower wavelength, and the PL intensity decreased significantly with decreasing metal insertion, probably due to the electron-capturing actions of the metal atoms from conduction band of TiO2. Particularly when Ag component was inserted into the TiO2 framework, the PL intensity was largely reduced. Consequently, the PL intensity varied according to whether the added metal acted as an electron capturer or not. If the incorporated metals existed on the surface or in the framework of TiO2, they attracted the excited electrons from TiO2, so that the recombination of an electron and a hole was difficult, thus increasing the number of holes over the valence band and generating more OH radicals.Figure 6
The PL spectra of six photocatalysts as-synthesized. (a) TiO2, (b) Cu(0.1)-Ti(0.9)O2, (c) Cu(0.07)-Ag(0.03)Ti(0.9)O2, (d) Cu(0.05)-Ag(0.05)Ti(0.9)O2, e) Cu(0.03)-Ag(0.07)Ti(0.9)O2, and (f) Ag(0.1)-Ti(0.9)O2.


## 3.2. H2 Production from Methanol/Water Decomposition over the Six Photocatalysts

Figure7 summarizes the evolution of H2 from methanol/water decomposition over the six photocatalysts in a batch-type, liquid photosystem. Over pure anatase TiO2, 200 mmol of H2 were only collected after methanol/water photodecomposition for 8 h, however the amount of H2 gas more increased in the Ag- or Cu-incorporated photocatalysts linearly with increasing time. The H2production was the highest in Cu(0.03)-Ag(0.07)Ti(0.9)O2 at 8,750 mmol and finally reached 20,000 mmol after 30 h. therefore, the simultaneously bimetallic addition of Ag and Cu components had a greater influence on the H2 production during methanol/water photodecomposition than the mono metals, Cu- or Ag-incorporated TiO2. Particularly, metal chunks were observed to be deposited in the reactor after the reaction. These results are evidence for the continuing oxidation/reduction actions between Cu and Ag during the reaction.The evolution of H2 from methanol/water decomposition over the six photocatalysts in a batch-type liquid photosystem. (A) accumulated amount of hydrogen gas and (B) accumulated amount of oxygen gas.  (a) TiO2, (b) Cu(0.1)-Ti(0.9)O2, (c) Cu(0.07)-Ag(0.03)Ti(0.9)O2, (d) Cu(0.05)-Ag(0.05)Ti(0.9)O2, (e) Cu(0.03)-Ag(0.07)Ti(0.9)O2, and f) Ag(0.1)-Ti(0.9)O2.The Cu(0.03)-Ag(0.07)Ti(0.9)O2 particles underwent quantitative XPS analyses before and after the reaction, with the typical survey and high-resolution spectra shown in Figure 8. The Ti2p1/2 and Ti2p3/2 spin-orbital splitting photoelectrons for anatase TiO2s were located at binding energies of 462.0 and 456.4 eV, respectively, and were assigned to the presence of typical Ti4+ [24]. The measured FWHM of the Ti2p3/2 peak was larger before reaction than after the reaction. However, there was no subsequent change. In general, a greater FWHM implies a greater amount of less-oxidized metals. The Cu2p3/2 and Cu2p1/2 spin-orbital splitting photoelectrons for the anatase Cu(0.03)-Ag(0.07)Ti(0.9)O2 photocatalyst before the reaction were located at binding energies of 930.4 and 949.5 eV, respectively, and these bands were assigned to CuO. However, these bands were separated into two peaks at binding energies of 932.5 eV of Cu2p3/2and 952.5 eV of Cu2p1/2, and these bands were assigned to Cu2O [24]. On the other hand, the fresh photocatalyst showed Ag3d5/2 and Ag3d3/2 spin-orbital splitting photoelectrons at binding energies of 366.1 and 372.0 eV, respectively, which were assigned to AgO, but the peak intensities were dramatically decreased after the reaction. This result indicated that the oxidation state of Cu was reduced and the amount of AgO was decreased during the reaction, which enabled their strong involvement in methanol/water decomposition. The O1s region was decomposed into two contributions: metal (Ti4+ or Ti3+)-O (527.5 eV) in the metal oxide and metal-OH (529.5.0 eV). The ratios of metal-OH/metal-O in the O1s peaks were decreased after the reaction compared to that before the reaction. Additionally, the measured FWHM of the O1s peak was larger after reaction than that before, which was attributed to the exposure of Ag or Cu ions from the surface of TiO2.Figure 8
The XPS for Cu2p, Ag3d, Ti2p, and O1s of Cu(0.03)-Ag(0.07)Ti(0.9)O2 before and after the methanol/water photodecomposition reaction: (A) before reaction and (B) after reaction.


## 4. Conclusions

TiO2 photocatalysts inserted with Ag, Cu, and Cu-Ag were prepared for the production of H2 gas from methanol/water photodecomposition in a batch-type liquid photosystem. Compared to monometal-incorporated TiO2, the H2 production via methanol/water photodecomposition was markedly enhanced in bimetal-incorporated photocatalyst and reached 8,750 mmol after methanol/water photodecomposition for 8 h over Cu(0.03)-Ag(0.07)Ti(0.9)O2 photocatalyst. These results confirmed that the simultaneous presence of Cu and Ag components in the framework of the TiO2 anatase structure improved the H2 production via methanol/water photodecomposition. Here, we suggested that any Cu or Ag components present in the TiO2 framework are reduced or decreased by attracting the excited electrons from the valence band of TiO2, because of the greater reduction potential of CuO or AgO than that of pure TiO2. This hinders the recombination of an electron and a hole because the CuO or AgO component captures electrons, thereby increasing the number of holes over the valence band and allowing methanol decomposition to continue. The simultaneous insertion of the two ions into the TiO2 framework induced an increased synergistic effect.



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*Source: 618642-2012-03-29.xml*