# Dynamic Hydrogen Production from Methanol/Water Photo-Splitting Using Core@Shell-Structured CuS@TiO2 Catalyst Wrapped by High Concentrated TiO2 Particles

Authors: Younghwan Im; Sora Kang; Kang Min Kim; Taeil Ju; Gi Bo Han; No-Kuk Park; Tae Jin Lee; Misook Kang
Journal: International Journal of Photoenergy
 (2013)

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## Abstract

This study focused on the dynamic hydrogen production ability of a core@shell-structured CuS@TiO2 photocatalyst coated with a high concentration of TiO2 particles. The rectangular-shaped CuS particles, 100 nm in length and 60 nm in width, were surrounded by a high concentration of anatase TiO2 particles (>4~5 mol). The synthesized core@shell-structured CuS@TiO2 particles absorbed a long wavelength (a short band gap) above 700 nm compared to that pure TiO2, which at approximately 300 nm, leading to easier electronic transitions, even at low energy. Hydrogen evolution from methanol/water photo-splitting over the core@shell-structured CuS@TiO2 photocatalyst increased approximately 10-fold compared to that over pure CuS. In particular, 1.9 mmol of hydrogen gas was produced after 10 hours when 0.5 g of 1CuS@4TiO2 was used at pH = 7. This level of production was increased to more than 4-fold at higher pH. Cyclic voltammetry and UV-visible absorption spectroscopy confirmed that the CuS in CuS@TiO2 strongly withdraws the excited electrons from the valence band in TiO2 because of the higher reduction potential than TiO2, resulting in a slower recombination rate between the electrons and holes and higher photoactivity.


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## Body

## 1. Introduction

In recent years, hydrogen has been highlighted as a next-generation energy source because of its environmentally friendly nature and high-energy efficiency. Therefore, hydrogen production has recently become the most active research topic globally. In particular, the technology for generating hydrogen by the splitting of water using a photocatalyst has attracted considerable attention. In the early days, the photocatalytic formation of hydrogen and oxygen focused extensively on metal-loaded or incorporated-TiO2 semiconductors due to the low band gap and high corrosion resistance of these materials [1–5]. On the other hand, hydrogen production from water photo-splitting using TiO2-based photocatalysts is ineffective because the amount of hydrogen produced is limited by the rapid recombination of holes and electrons over TiO2, resulting in the reformation of water [6]. In addition, more than 1.2 eV is needed to decompose water [7], which means that the photodecomposition of water should be performed at UV wavelengths of approximately 260 nm. Therefore, there is urgent need for the development of new and inexpensive photocatalysts that are both environmentally friendly and possess greater hydrogen-producing activity under visible light irradiation. Recently, studies of metal sulfide photocatalysts, such as ZnS- [8], CuS- [9, 10], FeS- [11], Bi2S3- [12], Sb2S3- [13], or CdS-loaded TiO2 [14], have covered topics ranging from synthesis to applications in new photocatalytic reaction mechanisms. Narrow band gaps make it possible to absorb longer wavelengths compared to wide band gaps of conventional metal oxide semiconductor systems. A previous study reported high photocatalytic activity on the ZnS-loaded TiO2 composite system for hydrogen production [15]. In that study, the evolution of H2 from methanol/water (1 : 1) photo-splitting over the ZnS/TiO2 composite was enhanced dramatically compared to that over pure TiO2 and ZnS. In particular, 1.2 mmol of H2 gas was produced after 10 h when 0.5 g of a 5.0 wt% ZnS-loaded TiO2 composite was used. Recently, many studies began to focus their attention on bimetallic sulfides photocatalysts, such as CdZnS [16], CuZnS [17], ZnInS [18], and AgZnS [19]. These studies have been extended to trimetallic sulfide photocatalysts, such as CuAgInS [20], ZnCuCdS [21], CuInZnS [22], and AgGaInS [23]. On the other hand, most papers are based on metal sulfides loaded on the surface of TiO2 particles. Few studies have examined TiO2 nanoparticles loaded on the surface of large-sized metal sulfide particles.This study focused on the CuS core material with a shorter band-gap of 1.56 eV and a higher reduction potential [24] than those of pure TiO2. Cu materials are widely used as catalysts for methanol steam reforming because of their excellent redox properties despite vulnerable to water. The potential (Cu2+ + 2e− = Cu0, E° = −0.224 V) is slightly lower than the conduction band (−0.26 V) of anatase TiO2 but is higher than the reduction potential of H+ (2H+ + 2e− = H2, E° = −0.000 V), which favors electron transfer from the conduction band of TiO2 to Cu2+, and the reduction of H+, thereby enhancing the photocatalytic H2-production activity [25, 26]. In this study, CuS was synthesized by a hydrothermal method with sodium sulfate as the sulfur source. A Ti precursor at a high concentrated molar ratio was then coated on the surface of the CuS like a core-shell structure. The relationship between the spectroscopic properties and the catalytic performance for the hydrogen production over the core@shell-structured CuS@TiO2 was examined by X-ray diffraction (XRD), transmission electron microscopy (TEM), UV-visible absorption spectroscopy, Brunauer, Emmett, and Teller (BET) surface areas, cyclic voltammetry (CV), and zeta potential measurements using an electrophoresis measurement apparatus.


## 2. Experimental

### 2.1. Synthesis of CuS and Core@Shell-Structured CuS@TiO2

The TiO2, CuS, and core@shell-structured CuS@TiO2 photocatalysts were prepared using hydrothermal and impregnation methods, respectively. In the first step for TiO2, titanium tetra-isopropoxide (TTIP, 99.99%, Junsei Chemical, Japan) as a titanium precursor was added dropwise to an aqueous solution and stirred homogeneously for 2 h. The pH of the final solution was set to pH = 3.0 using acetic acid to induce mild hydrolysis, and the resulting solution was transferred to an autoclave for thermal treatment. The thermal treatment at 200°C was kept for 12 h, and the resulting precipitates were obtained, washed with distilled water, and dried at 80°C for 24 h. In the second step of CuS synthesis, CuSO4·5H2O (99.99%, Junsei Chemical, Japan) and Na2S2O3·5H2O (99.99%, Junsei Chemical, Japan) were used as the Cu and S precursors to prepare the sol mixture, respectively. Copper sulfate and sodium sulfate were dissolved sequentially in distilled water and stirred to homogeneity for 2 h. The final solution was transferred to an autoclave for thermal treatment. Cu ions were sulfurized during the thermal treatment at 180°C for 12 h. The resulting precipitates were obtained, washed with distilled water, and dried at 80°C for 24 h. Finally the dried powders were treated at 400°C for 4 h to obtain crystallized CuS. Finally, 4.0 and 5.0 moles of TTIP (titanium tetraisopropoxide, 99.99%, Aldrich) for each 1.0 mole of CuS were added slowly to an ethanol solution containing the dispersed CuS particles during stirring to coat the CuS surface. The pH of the colloidal solution was kept at 4.0, and the solution was stirred homogeneously for 18 h. The final solution was evaporated at 80°C for 5 h and calcined at 400°C for 4 h to induce the anatase TiO2. Finally, three types of materials, CuS and the core@shell-structured 1CuS@4TiO2 and 1CuS@5TiO2, were examined. Three samples of pure TiO2 (by hydrothermal method), CuS, and physically mixed TiO2/CuS were also prepared for comparison.


### 2.2. Characteristics of Synthesized CuS and Core@Shell-Structured CuS@TiO2

The synthesized CuS and core@shell-structured CuS@TiO2 photocatalysts were examined by XRD (X’Pert Pro MPD PANalytical 2-circle diffractometer) using nickel-filtered CuKα radiation (30 kV and 30 mA). The sizes and shapes of the CuS and core@shell-structured CuS@TiO2 photocatalysts were examined by TEM (JEOL 2000EX). The BET surface areas of catalysts were measured using a Belsorp II instrument. All the catalysts were degassed under vacuum at 150°C for 30 min before the BET surface measurements. The catalysts were measured through the nitrogen gas adsorption using a continuous flow method with a mixture of nitrogen and helium as the carrier gas. The UV-visible absorption spectra of CuS and core@shell-structured CuS@TiO2 powders were obtained using a Cary 500 spectrometer with a reflectance sphere. The CV measurements of the CuS and core@shell-structured CuS@TiO2 pellets were obtained using a BAS 100B potentiostat at room temperature in 0.1 M KCl solution. A platinum wire as the counter electrode and Ag/AgCl as the reference electrode were used. The zeta potential of CuS and core@shell-structured CuS@TiO2 particles was determined by the electrophoretic mobility using an electrophoresis measurement apparatus (ELS 8000, Otsuka Electronics, Japan) with a plate sample cell. Electrophoretic light scattering (ELS) was performed in reference beam mode using a laser light source of 670 nm, a modular frequency of 250 Hz, and a scattering angle of 15°. The standard error of the zeta potential, converted from the experimentally determined electrophoretic mobility, was typically <1.5%, and the percentage error was <5%. To measure the zeta potentials, 0.1 wt% of each sample was dispersed in deionized water, and the pH of the solution was adjusted with HCl or NaOH. The relative molecular diameter size distributions of the various solutions were also measured using this equipment.


### 2.3. Hydrogen Production from Photo-Splitting of Methanol/Water over CuS and Core@Shell-Structured CuS@TiO2

Photo-splitting in methanol/water using CuS and core@shell-structured CuS@TiO2 photocatalysts was carried out using a liquid photoreactor designed in house, as shown in Figure 1. For methanol/water photo-splitting, 0.5 g of a photocatalyst was added to 1.0 L distilled water in a 2.0 L Pyrex reactor. UV-lamps (6 × 3 W cm−2 = 18 W cm−2, 30 cm length × 2.0 cm diameter; Shinan Co.) emitting radiation with a wavelength of 365 nm were used. Methanol/water photo-splitting was carried out for 10 h with constant stirring, and the level of hydrogen evolution was measured at 1 h intervals. The hydrogen gas (H2) produced during methanol/water photo-splitting was analyzed by TCD-type gas chromatography (GC, model DS 6200; Donam Instruments Inc., Republic of Korea). To determine the products and intermediates, the GC was connected directly to the methanol/water photo-splitting reactor. The following GC conditions were used: TCD detector; Carbosphere column (Alltech, Deerfield, IL, USA); and an injection, initial, final, and detector temperature of 413 K, 393 K, 393 K, and 423 K, respectively.Figure 1
Apparatus of a liquid photoreactor for the methanol/water photo-splitting using CuS and core@shell-structured CuS@TiO2 photocatalysts.


## 2.1. Synthesis of CuS and Core@Shell-Structured CuS@TiO2

The TiO2, CuS, and core@shell-structured CuS@TiO2 photocatalysts were prepared using hydrothermal and impregnation methods, respectively. In the first step for TiO2, titanium tetra-isopropoxide (TTIP, 99.99%, Junsei Chemical, Japan) as a titanium precursor was added dropwise to an aqueous solution and stirred homogeneously for 2 h. The pH of the final solution was set to pH = 3.0 using acetic acid to induce mild hydrolysis, and the resulting solution was transferred to an autoclave for thermal treatment. The thermal treatment at 200°C was kept for 12 h, and the resulting precipitates were obtained, washed with distilled water, and dried at 80°C for 24 h. In the second step of CuS synthesis, CuSO4·5H2O (99.99%, Junsei Chemical, Japan) and Na2S2O3·5H2O (99.99%, Junsei Chemical, Japan) were used as the Cu and S precursors to prepare the sol mixture, respectively. Copper sulfate and sodium sulfate were dissolved sequentially in distilled water and stirred to homogeneity for 2 h. The final solution was transferred to an autoclave for thermal treatment. Cu ions were sulfurized during the thermal treatment at 180°C for 12 h. The resulting precipitates were obtained, washed with distilled water, and dried at 80°C for 24 h. Finally the dried powders were treated at 400°C for 4 h to obtain crystallized CuS. Finally, 4.0 and 5.0 moles of TTIP (titanium tetraisopropoxide, 99.99%, Aldrich) for each 1.0 mole of CuS were added slowly to an ethanol solution containing the dispersed CuS particles during stirring to coat the CuS surface. The pH of the colloidal solution was kept at 4.0, and the solution was stirred homogeneously for 18 h. The final solution was evaporated at 80°C for 5 h and calcined at 400°C for 4 h to induce the anatase TiO2. Finally, three types of materials, CuS and the core@shell-structured 1CuS@4TiO2 and 1CuS@5TiO2, were examined. Three samples of pure TiO2 (by hydrothermal method), CuS, and physically mixed TiO2/CuS were also prepared for comparison.


## 2.2. Characteristics of Synthesized CuS and Core@Shell-Structured CuS@TiO2

The synthesized CuS and core@shell-structured CuS@TiO2 photocatalysts were examined by XRD (X’Pert Pro MPD PANalytical 2-circle diffractometer) using nickel-filtered CuKα radiation (30 kV and 30 mA). The sizes and shapes of the CuS and core@shell-structured CuS@TiO2 photocatalysts were examined by TEM (JEOL 2000EX). The BET surface areas of catalysts were measured using a Belsorp II instrument. All the catalysts were degassed under vacuum at 150°C for 30 min before the BET surface measurements. The catalysts were measured through the nitrogen gas adsorption using a continuous flow method with a mixture of nitrogen and helium as the carrier gas. The UV-visible absorption spectra of CuS and core@shell-structured CuS@TiO2 powders were obtained using a Cary 500 spectrometer with a reflectance sphere. The CV measurements of the CuS and core@shell-structured CuS@TiO2 pellets were obtained using a BAS 100B potentiostat at room temperature in 0.1 M KCl solution. A platinum wire as the counter electrode and Ag/AgCl as the reference electrode were used. The zeta potential of CuS and core@shell-structured CuS@TiO2 particles was determined by the electrophoretic mobility using an electrophoresis measurement apparatus (ELS 8000, Otsuka Electronics, Japan) with a plate sample cell. Electrophoretic light scattering (ELS) was performed in reference beam mode using a laser light source of 670 nm, a modular frequency of 250 Hz, and a scattering angle of 15°. The standard error of the zeta potential, converted from the experimentally determined electrophoretic mobility, was typically <1.5%, and the percentage error was <5%. To measure the zeta potentials, 0.1 wt% of each sample was dispersed in deionized water, and the pH of the solution was adjusted with HCl or NaOH. The relative molecular diameter size distributions of the various solutions were also measured using this equipment.


## 2.3. Hydrogen Production from Photo-Splitting of Methanol/Water over CuS and Core@Shell-Structured CuS@TiO2

Photo-splitting in methanol/water using CuS and core@shell-structured CuS@TiO2 photocatalysts was carried out using a liquid photoreactor designed in house, as shown in Figure 1. For methanol/water photo-splitting, 0.5 g of a photocatalyst was added to 1.0 L distilled water in a 2.0 L Pyrex reactor. UV-lamps (6 × 3 W cm−2 = 18 W cm−2, 30 cm length × 2.0 cm diameter; Shinan Co.) emitting radiation with a wavelength of 365 nm were used. Methanol/water photo-splitting was carried out for 10 h with constant stirring, and the level of hydrogen evolution was measured at 1 h intervals. The hydrogen gas (H2) produced during methanol/water photo-splitting was analyzed by TCD-type gas chromatography (GC, model DS 6200; Donam Instruments Inc., Republic of Korea). To determine the products and intermediates, the GC was connected directly to the methanol/water photo-splitting reactor. The following GC conditions were used: TCD detector; Carbosphere column (Alltech, Deerfield, IL, USA); and an injection, initial, final, and detector temperature of 413 K, 393 K, 393 K, and 423 K, respectively.Figure 1
Apparatus of a liquid photoreactor for the methanol/water photo-splitting using CuS and core@shell-structured CuS@TiO2 photocatalysts.


## 3. Results and Discussion

### 3.1. Properties of Synthesized CuS and Core@Shell-Structured CuS@TiO2

Figure2 shows XRD patterns of the TiO2, CuS, and CuS@TiO2 photocatalysts. All the peaks in CuS were indexed to the hexagonal phase CuS (P63/mmc space, cell constants a=3.8Å, b=3.8 Å, and c=16.43 Å; JCPDS Card no. 02-0820). The XRD patterns showed the main peaks at 26.75, 27.51, 29.36, 31.82, 33.03, 38.96, 43.04, 44.60, 52.88, 59.18, 63.69, 67.86, 69.58, 74.00, and 79.08° 2θ, which were assigned to the (100), (101), (102), (103), (006), (105), (106), (008), (110), (114), (116), (1010), (0012), (207), (208), and (213) planes, respectively. In the case of CuS@TiO2, the peaks for crystalline CuS almost disappeared except for a very small peak at 33.03° 2θ (006). This result coincides with the fact that in general if the core-shell structure formed completely in a core-shell material, the XRD peaks for the core do not appear; only the diffraction patterns for the shell are observed [27]. Otherwise, the XRD patterns for crystalline TiO2 (anatase, tetragonal crystal system, I41/amd space, JCPDS Card no. 02-0387) in CuS@TiO2 were observed at 25.35, 37.93, 48.10, 53.89, 55.30, 68.99, 70.18, and 75.37° 2θ, which were assigned to the (101), (004), (200), (105), (211), (116), (220), and (215) planes, respectively. The locations were the same as the hydrothermally prepared pure TiO2 in (b). The peaks in CuS@TiO2 were slightly larger according to the loaded Ti concentration. The XRD peak intensities that were assigned to anatase TiO2 in 1CuS@5TiO2 were slightly sharper than those of CuS@TiO2 loaded with 4.0 mol-concentrated Ti. Generally, the line widths of the XRD peaks were broad, which indicated a smaller crystallite size. The Scherrer equation, t=0.9λ/βcosθ, where λ is the wavelength of incident X-rays, β is the full width at half maximum (FWHM) in radians, and θ is the diffraction angle, was used to determine the crystallite size. The loaded TiO2 crystallite sizes of 1CuS@4TiO2 and 1CuS@5TiO2 based on the 25.35° 2θ peak were 17.50 and 17.90 nm, respectively.Figure 2
XRD patterns of the CuS and CuS@TiO2 photocatalysts.Figure3 shows TEM images of the CuS and CuS@TiO2 powders. Rectangular-shaped particles with 100 nm long and 60 nm wide sides were observed in the CuS sample, and 10 nm sized TiO2 particles were also observed in TiO2 samples. Here, the nanosized TiO2 particles were synthesized hydrothermally for comparison. Interestingly, the huge CuS particles were surrounded by nanosized TiO2 particles with high concentrations (4~5 moles compared to 1 mole of core CuS). This is in good agreement with the XRD patterns. This is a reliable result in that, when the loaded TiO2 amounts increased, the shell composed of TiO2 particles was thicker. TEM confirmed that the obtained CuS@TiO2 sample had a core@shell structure.TEM images of the CuS and CuS@TiO2 photocatalysts.
(a)
CuS
(b)
TiO2
(c)
CuS@TiO2 (1 : 4)
(d)
CuS@TiO2 (1 : 5)Figure4 shows the adsorption-desorption isotherm curves of N2 at 77 K for the fresh powder samples and core@shell-structured CuS@TiO2. The isotherms belonged to the IV type in the IUPAC classification [28]. Generally, this hysteresis slope has been observed in the presence of large mesopores. Here, the mesopores are considered to be bulk pores formed between TiO2 particles in the shell. This suggests that the reaction of the catalyst with a high surface area facilitates adsorption, which can improve the catalytic activity. Therefore, it is expected that the methanol or water molecules are adsorbed more easily on the surfaces of the core@shell-structured CuS@TiO2 than those of pure TiO2 or CuS particles during methanol/water photo-splitting. The surface area increased from 17.88 to 27.97 m2 g−1 according to the change in TiO2 concentration from 4.0 to 5.0 mol. Generally, the specific surface area increases with decreasing particle size. Here, the loaded TiO2 particle sizes in the two samples were similar. Therefore, the surface area in this study possibly depends on the bulk pores formed by aggregation between the TiO2 particles in the shell. The total bulk-pore volumes increased from 0.029 (4 mol TiO2 loading) to 0.038 (5 mol TiO2 loading) cm3g−1. Eventually, the specific surface area increased with increasing pore volume.Adsorption-desorption isotherm curves of N2 at 77 K for the core@shell-structured CuS@TiO2.
(a)
(b)
(c)Figure5 shows the UV-visible absorption spectra of the CuS and core@shell-structured CuS@TiO2 powders. The absorption edges of Ti4+ and Cu2+ with octahedral symmetries normally appear at a maximum of approximately 300 and 700 nm in pure TiO2 and CuS, respectively [29, 30]. The band gap in a semiconductor material is closely related to the wavelength range absorbed, where the band gap decreases with increasing absorption wavelength. Consequently, a material with a narrow band gap can be extended readily to utilize visible light, whereas a narrow band gap can reduce photocatalytic activity by increasing the recombination rate between the electrons and holes. Based on the Tauc equation [31], the band gaps obtained by extrapolation at the cross-section point of the two tangents were approximately 1.35 and 3.19 eV for pure CuS and TiO2, respectively.Figure 5
UV-visible absorption spectra of the CuS and core@shell-structured CuS@TiO2 powders.Figure6 presents the CV measurements of CuS and the core@shell-structured CuS@TiO2, indicating high dependence on the analytic conditions being studied, which must be redox active within the experimental potential window. A reversible wave that provides the following information is desirable: reversible reactions will show a ratio of the peak currents passed at reduction (Epc) and oxidation (Epa). When such reversible peaks are observed, thermodynamic information in the form of a half cell potential E1/2°(Epc+Epa/2) can be determined. In particular, when the waves are semireversible, such as when Epa/Epc≥1, it can be possible to induce even more information, particularly in kinetic processes. Recently, some studies reported a useful equation that can determine the energy levels of the HOMO and LUMO using a CV method [32]. In the synthesized CuS, the Cu(II) → Cu(0) redox process appeared to be a reversible reaction, and the absolute potential in the reduction (Epc) was observed at −0.732 V. The onset potentials in the core@shell-structured CuS@TiO2 samples might be used to determine the thermodynamic E1/2° as −1.255 and −2.59 V in 1CuS@4TiO2 and 1CuS@5TiO2, respectively. The CV curves were observed at two locations, and there might be two factors from TiO2 (front) and CuS (back), −1.79 and −0.712 V, respectively. Therefore, the corresponding LUMO energy levels were calculated to be −3.65 (for CuS), −3.12 (for 1CuS@4TiO2), and −3.668 (for 1CuS@5TiO2) eV, respectively.Cyclic voltammetry for the CuS and core@shell-structured CuS@TiO2.
(a)
CuS
(b)
CuS@TiO2 (1 : 4)
(c)
CuS@TiO2 (1 : 5)Figure7 summarizes the hydrogen evolution from methanol/water photo-splitting over the CuS, TiO2, and two types of core@shell-structured CuS@TiO2 photocatalysts in a batch-type liquid photosystem, and the catalytic performance of a physically mixed CuS+TiO2 sample was also evaluated for comparison. The catalytic activities of the core@shell-structured CuS@TiO2 photocatalysts were enhanced considerably compared to the pure CuS or TiO2. In Figure 7(a), a very small amount of hydrogen was collected over CuS (0.2 mmol) and TiO2 (0.09 mmol) after methanol/water photo-splitting for 10 h. A significant amount of hydrogen gas was collected over CuS@TiO2, and the amount of hydrogen produced reached 1.9 mmol over 0.5 g 1CuS@4TiO2. On the other hand, the amount produced was significantly lower on the core@shell-structured 1CuS@5TiO2 catalyst with higher Ti incorporation. Here, CuS absorbs longer wavelengths easily, but recombination between the excited electrons and the holes also causes rapid catalytic deactivation. In contrast, the core@shell-structured CuS@TiO2 has stronger oxidation-reduction ability than pure CuS. Here, the CuS core acts as a good electron collector excited from TiO2 and transporter, resulting in the retardation of electron-hole recombination, leading to an increase in photocatalytic performance. On the other hand, the collected hydrogen did not increase significantly over the physically mixed CuS+TiO2 sample. The catalytic performance of methanol/water destruction over the core@shell-structured 1CuS@4TiO2 was enhanced more under the alkali electrolytes solution, as shown in Figure 7(b). When OH− ions are present in the alkali solution, the subsequent reaction occurs: OH-+hole→OH∙ in the valence band. Therefore, a large number of OH radicals are generated in the alkali solution, resulting in an increase in hydrogen evolution. Hydrogen production was increased dramatically in the alkali solution by generating more OH ions, reaching up to 8.0 mmol after 10 h in a KOH (pH = 11) solution. In an acidic solution, however, the level of production was decreased due to SO42- ions formed after the reaction. The S ions inside the CuS catalyst appear to dissolve in the acidic solution, followed by a reaction with O ions in water to form SO42- ions. Eventually, the sulfate ions combine with the hydrogen ions generated during the methanol/water photo-splitting process, which occurs during the formation of H2SO4.Evolution of H2 from methanol/water photo-splitting over the CuS, TiO2, and two types of core@shell-structured CuS@TiO2 photocatalysts in a batch-type liquid photosystem. (a) Hydrogen production according to the catalysts and (b) hydrogen production according to the pH for 1CuS@4TiO2.
(a)
(b)Figure8 shows the influence of pH on the zeta potential distribution in the CuS, TiO2, and two types of core@shell-structured CuS@TiO2. The adjacent table summarizes the aggregated particle sizes in the aqueous solution. The zeta potential of the 1CuS@4TiO2 suspensions decreased significantly with increasing pH. The surface charges in all samples changed from a positive value in an acidic solution to a larger negative value in an alkali solution. The isoelectric points, meaning the large aggregation of particles, were different: 5.8, 7.9, 7.0, and 7.7 for CuS, TiO2, 1CuS@4TiO2, and 1CuS@5TiO2, respectively. At pH = 11.0, the surface charges in all samples showed the highest absolute value. This suggests that the colloidal samples were stable [33] with high mobility, which is closely related to the reaction sites over the photocatalyst surface. This result matches the results in Figure 6 well.Figure 8
Zeta potential distributions of the CuS, TiO2, and two types of core@shell-structured CuS@TiO2 according to the pH.The CV curves, UV-visible absorption spectra, and their photocatalytic performance suggest a photocatalysis model over the core@shell-structured CuS@TiO2, as shown in Scheme 1. The TiO2 shells covered the core CuS completely, which means that the electrons on the valence band of TiO2 will be transferred to the conduction band. The excited electrons are moved to the valence band in CuS because of its higher reduction potential than TiO2. In this study the core CuS acted as a good electron collector and transporter, similar to reduced graphene oxide reported in another paper [34]. Therefore, the recombination of electrons and holes was reduced, and finally more OH radicals were generated easily at the holes in the valence band of TiO2. Radicals with strong oxidative power attack CH3OH molecules, and CO2, H2, and H2O are produced by the complete oxidation of methanol. In addition, if the core CuS also absorbs the radiation (if it does not have a complete core@shell structure), the electrons would be excited more easily from the valence band of CuS. Overall, the catalytic activity of CuS@TiO2 is performed more effectively in the methanol/water photo-splitting reaction. This also means that the electrons excited from the valence band over CuS@TiO2 recombine slowly with the holes during photocatalysis. Therefore, the hole effect at the valence band continues for a longer time than those in pure CuS or TiO2. In addition, according to the UV-visible spectra, the CuS@TiO2 samples exhibited enhanced absorbance over the entire visible-light region. Therefore, the CuS core can also absorb visible radiation compared to the TiO2 shell, which can only absorb UV light. Consequently, the photocatalytic activity is enhanced over the core@shell-structured CuS@TiO2 photocatalysts.Scheme 1
Supposed photocatalysis model over the core@shell-structured CuS@TiO2.


## 3.1. Properties of Synthesized CuS and Core@Shell-Structured CuS@TiO2

Figure2 shows XRD patterns of the TiO2, CuS, and CuS@TiO2 photocatalysts. All the peaks in CuS were indexed to the hexagonal phase CuS (P63/mmc space, cell constants a=3.8Å, b=3.8 Å, and c=16.43 Å; JCPDS Card no. 02-0820). The XRD patterns showed the main peaks at 26.75, 27.51, 29.36, 31.82, 33.03, 38.96, 43.04, 44.60, 52.88, 59.18, 63.69, 67.86, 69.58, 74.00, and 79.08° 2θ, which were assigned to the (100), (101), (102), (103), (006), (105), (106), (008), (110), (114), (116), (1010), (0012), (207), (208), and (213) planes, respectively. In the case of CuS@TiO2, the peaks for crystalline CuS almost disappeared except for a very small peak at 33.03° 2θ (006). This result coincides with the fact that in general if the core-shell structure formed completely in a core-shell material, the XRD peaks for the core do not appear; only the diffraction patterns for the shell are observed [27]. Otherwise, the XRD patterns for crystalline TiO2 (anatase, tetragonal crystal system, I41/amd space, JCPDS Card no. 02-0387) in CuS@TiO2 were observed at 25.35, 37.93, 48.10, 53.89, 55.30, 68.99, 70.18, and 75.37° 2θ, which were assigned to the (101), (004), (200), (105), (211), (116), (220), and (215) planes, respectively. The locations were the same as the hydrothermally prepared pure TiO2 in (b). The peaks in CuS@TiO2 were slightly larger according to the loaded Ti concentration. The XRD peak intensities that were assigned to anatase TiO2 in 1CuS@5TiO2 were slightly sharper than those of CuS@TiO2 loaded with 4.0 mol-concentrated Ti. Generally, the line widths of the XRD peaks were broad, which indicated a smaller crystallite size. The Scherrer equation, t=0.9λ/βcosθ, where λ is the wavelength of incident X-rays, β is the full width at half maximum (FWHM) in radians, and θ is the diffraction angle, was used to determine the crystallite size. The loaded TiO2 crystallite sizes of 1CuS@4TiO2 and 1CuS@5TiO2 based on the 25.35° 2θ peak were 17.50 and 17.90 nm, respectively.Figure 2
XRD patterns of the CuS and CuS@TiO2 photocatalysts.Figure3 shows TEM images of the CuS and CuS@TiO2 powders. Rectangular-shaped particles with 100 nm long and 60 nm wide sides were observed in the CuS sample, and 10 nm sized TiO2 particles were also observed in TiO2 samples. Here, the nanosized TiO2 particles were synthesized hydrothermally for comparison. Interestingly, the huge CuS particles were surrounded by nanosized TiO2 particles with high concentrations (4~5 moles compared to 1 mole of core CuS). This is in good agreement with the XRD patterns. This is a reliable result in that, when the loaded TiO2 amounts increased, the shell composed of TiO2 particles was thicker. TEM confirmed that the obtained CuS@TiO2 sample had a core@shell structure.TEM images of the CuS and CuS@TiO2 photocatalysts.
(a)
CuS
(b)
TiO2
(c)
CuS@TiO2 (1 : 4)
(d)
CuS@TiO2 (1 : 5)Figure4 shows the adsorption-desorption isotherm curves of N2 at 77 K for the fresh powder samples and core@shell-structured CuS@TiO2. The isotherms belonged to the IV type in the IUPAC classification [28]. Generally, this hysteresis slope has been observed in the presence of large mesopores. Here, the mesopores are considered to be bulk pores formed between TiO2 particles in the shell. This suggests that the reaction of the catalyst with a high surface area facilitates adsorption, which can improve the catalytic activity. Therefore, it is expected that the methanol or water molecules are adsorbed more easily on the surfaces of the core@shell-structured CuS@TiO2 than those of pure TiO2 or CuS particles during methanol/water photo-splitting. The surface area increased from 17.88 to 27.97 m2 g−1 according to the change in TiO2 concentration from 4.0 to 5.0 mol. Generally, the specific surface area increases with decreasing particle size. Here, the loaded TiO2 particle sizes in the two samples were similar. Therefore, the surface area in this study possibly depends on the bulk pores formed by aggregation between the TiO2 particles in the shell. The total bulk-pore volumes increased from 0.029 (4 mol TiO2 loading) to 0.038 (5 mol TiO2 loading) cm3g−1. Eventually, the specific surface area increased with increasing pore volume.Adsorption-desorption isotherm curves of N2 at 77 K for the core@shell-structured CuS@TiO2.
(a)
(b)
(c)Figure5 shows the UV-visible absorption spectra of the CuS and core@shell-structured CuS@TiO2 powders. The absorption edges of Ti4+ and Cu2+ with octahedral symmetries normally appear at a maximum of approximately 300 and 700 nm in pure TiO2 and CuS, respectively [29, 30]. The band gap in a semiconductor material is closely related to the wavelength range absorbed, where the band gap decreases with increasing absorption wavelength. Consequently, a material with a narrow band gap can be extended readily to utilize visible light, whereas a narrow band gap can reduce photocatalytic activity by increasing the recombination rate between the electrons and holes. Based on the Tauc equation [31], the band gaps obtained by extrapolation at the cross-section point of the two tangents were approximately 1.35 and 3.19 eV for pure CuS and TiO2, respectively.Figure 5
UV-visible absorption spectra of the CuS and core@shell-structured CuS@TiO2 powders.Figure6 presents the CV measurements of CuS and the core@shell-structured CuS@TiO2, indicating high dependence on the analytic conditions being studied, which must be redox active within the experimental potential window. A reversible wave that provides the following information is desirable: reversible reactions will show a ratio of the peak currents passed at reduction (Epc) and oxidation (Epa). When such reversible peaks are observed, thermodynamic information in the form of a half cell potential E1/2°(Epc+Epa/2) can be determined. In particular, when the waves are semireversible, such as when Epa/Epc≥1, it can be possible to induce even more information, particularly in kinetic processes. Recently, some studies reported a useful equation that can determine the energy levels of the HOMO and LUMO using a CV method [32]. In the synthesized CuS, the Cu(II) → Cu(0) redox process appeared to be a reversible reaction, and the absolute potential in the reduction (Epc) was observed at −0.732 V. The onset potentials in the core@shell-structured CuS@TiO2 samples might be used to determine the thermodynamic E1/2° as −1.255 and −2.59 V in 1CuS@4TiO2 and 1CuS@5TiO2, respectively. The CV curves were observed at two locations, and there might be two factors from TiO2 (front) and CuS (back), −1.79 and −0.712 V, respectively. Therefore, the corresponding LUMO energy levels were calculated to be −3.65 (for CuS), −3.12 (for 1CuS@4TiO2), and −3.668 (for 1CuS@5TiO2) eV, respectively.Cyclic voltammetry for the CuS and core@shell-structured CuS@TiO2.
(a)
CuS
(b)
CuS@TiO2 (1 : 4)
(c)
CuS@TiO2 (1 : 5)Figure7 summarizes the hydrogen evolution from methanol/water photo-splitting over the CuS, TiO2, and two types of core@shell-structured CuS@TiO2 photocatalysts in a batch-type liquid photosystem, and the catalytic performance of a physically mixed CuS+TiO2 sample was also evaluated for comparison. The catalytic activities of the core@shell-structured CuS@TiO2 photocatalysts were enhanced considerably compared to the pure CuS or TiO2. In Figure 7(a), a very small amount of hydrogen was collected over CuS (0.2 mmol) and TiO2 (0.09 mmol) after methanol/water photo-splitting for 10 h. A significant amount of hydrogen gas was collected over CuS@TiO2, and the amount of hydrogen produced reached 1.9 mmol over 0.5 g 1CuS@4TiO2. On the other hand, the amount produced was significantly lower on the core@shell-structured 1CuS@5TiO2 catalyst with higher Ti incorporation. Here, CuS absorbs longer wavelengths easily, but recombination between the excited electrons and the holes also causes rapid catalytic deactivation. In contrast, the core@shell-structured CuS@TiO2 has stronger oxidation-reduction ability than pure CuS. Here, the CuS core acts as a good electron collector excited from TiO2 and transporter, resulting in the retardation of electron-hole recombination, leading to an increase in photocatalytic performance. On the other hand, the collected hydrogen did not increase significantly over the physically mixed CuS+TiO2 sample. The catalytic performance of methanol/water destruction over the core@shell-structured 1CuS@4TiO2 was enhanced more under the alkali electrolytes solution, as shown in Figure 7(b). When OH− ions are present in the alkali solution, the subsequent reaction occurs: OH-+hole→OH∙ in the valence band. Therefore, a large number of OH radicals are generated in the alkali solution, resulting in an increase in hydrogen evolution. Hydrogen production was increased dramatically in the alkali solution by generating more OH ions, reaching up to 8.0 mmol after 10 h in a KOH (pH = 11) solution. In an acidic solution, however, the level of production was decreased due to SO42- ions formed after the reaction. The S ions inside the CuS catalyst appear to dissolve in the acidic solution, followed by a reaction with O ions in water to form SO42- ions. Eventually, the sulfate ions combine with the hydrogen ions generated during the methanol/water photo-splitting process, which occurs during the formation of H2SO4.Evolution of H2 from methanol/water photo-splitting over the CuS, TiO2, and two types of core@shell-structured CuS@TiO2 photocatalysts in a batch-type liquid photosystem. (a) Hydrogen production according to the catalysts and (b) hydrogen production according to the pH for 1CuS@4TiO2.
(a)
(b)Figure8 shows the influence of pH on the zeta potential distribution in the CuS, TiO2, and two types of core@shell-structured CuS@TiO2. The adjacent table summarizes the aggregated particle sizes in the aqueous solution. The zeta potential of the 1CuS@4TiO2 suspensions decreased significantly with increasing pH. The surface charges in all samples changed from a positive value in an acidic solution to a larger negative value in an alkali solution. The isoelectric points, meaning the large aggregation of particles, were different: 5.8, 7.9, 7.0, and 7.7 for CuS, TiO2, 1CuS@4TiO2, and 1CuS@5TiO2, respectively. At pH = 11.0, the surface charges in all samples showed the highest absolute value. This suggests that the colloidal samples were stable [33] with high mobility, which is closely related to the reaction sites over the photocatalyst surface. This result matches the results in Figure 6 well.Figure 8
Zeta potential distributions of the CuS, TiO2, and two types of core@shell-structured CuS@TiO2 according to the pH.The CV curves, UV-visible absorption spectra, and their photocatalytic performance suggest a photocatalysis model over the core@shell-structured CuS@TiO2, as shown in Scheme 1. The TiO2 shells covered the core CuS completely, which means that the electrons on the valence band of TiO2 will be transferred to the conduction band. The excited electrons are moved to the valence band in CuS because of its higher reduction potential than TiO2. In this study the core CuS acted as a good electron collector and transporter, similar to reduced graphene oxide reported in another paper [34]. Therefore, the recombination of electrons and holes was reduced, and finally more OH radicals were generated easily at the holes in the valence band of TiO2. Radicals with strong oxidative power attack CH3OH molecules, and CO2, H2, and H2O are produced by the complete oxidation of methanol. In addition, if the core CuS also absorbs the radiation (if it does not have a complete core@shell structure), the electrons would be excited more easily from the valence band of CuS. Overall, the catalytic activity of CuS@TiO2 is performed more effectively in the methanol/water photo-splitting reaction. This also means that the electrons excited from the valence band over CuS@TiO2 recombine slowly with the holes during photocatalysis. Therefore, the hole effect at the valence band continues for a longer time than those in pure CuS or TiO2. In addition, according to the UV-visible spectra, the CuS@TiO2 samples exhibited enhanced absorbance over the entire visible-light region. Therefore, the CuS core can also absorb visible radiation compared to the TiO2 shell, which can only absorb UV light. Consequently, the photocatalytic activity is enhanced over the core@shell-structured CuS@TiO2 photocatalysts.Scheme 1
Supposed photocatalysis model over the core@shell-structured CuS@TiO2.


## 4. Conclusions

Core@shell-structured CuS@TiO2 was synthesized using hydrothermal/impregnation methods. Based on the UV-visible absorption and CV results, the band gap of the pure CuS was estimated to be approximately 1.35 eV, respectively, and the corresponding LUMO energy level was −3.65 eV. ELS showed that the core@shell-structured 1CuS@4TiO2 particles were stable in an alkali solution. A significant amount of hydrogen gas was collected over 0.5 g of the core@shell-structured 1CuS@4TiO2 photocatalyst, and the amount reached 1.9 mmol with a maximum yield of 8.0 mmol after 10 h in a KOH solution. This was due most likely to the slower recombination between the electrons and a hole, which enables higher catalytic performance over the core@shell-structured 1CuS@4TiO2. These results are expected to play a significant role in the development of new photocatalysts with a core@shell structure for dramatic hydrogen production.



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*Source: 452542-2013-09-03.xml*