# A Facile Synthesis of Graphene-WO3 Nanowire Clusters with High Photocatalytic Activity for O2 Evolution

Authors: M.-J. Zhou; N. Zhang; Z. H. Hou
Journal: International Journal of Photoenergy
 (2014)

---

## Abstract

In the present work, graphene-WO3 nanowire clusters were synthesized via a facile hydrothermal method. The obtained graphene-WO3 nanowire clusters were characterized by X-ray diffraction (XRD), transmission electron microscopy (TEM), X-ray photoelectron spectroscopy (XPS), Fourier transform infrared spectroscopy (FT-IR), Raman spectroscopy, and ultraviolet-visible diffuse reflectance spectroscopy (DRS) techniques. The photocatalytic oxygen (O2) evolution properties of the as-synthesized samples were investigated by measuring the amount of evolved O2 from water splitting. The graphene-WO3 nanowire clusters exhibited enhanced performance compared to pure WO3 nanowire clusters for O2 evolution. The amount of evolved O2 from water splitting after 8 h for the graphene-WO3 nanowire clusters is ca. 0.345 mmol/L, which is more than 1.9 times as much as that of the pure WO3 nanowire clusters (ca. 0.175 mmol/L). The high photocatalytic activity of the graphene-WO3 nanowire clusters was attributed to a high charge transfer rate in the presence of graphene.


---

## Body

## 1. Introduction

Since Fujishima and Honda reported the evolution of oxygen and hydrogen from a TiO2 electrode under the irradiation of light in 1972 [1], photocatalysis is a very promising process to photodissociate water utilizing solar energy. Solar photolysis of water is one of the cleanest ways of producing hydrogen and oxygen, which has great potential in solving energy problem. Recently, tungsten oxide (WO3) as an important photocatalytic material with a wide band gap ranging from 2.4 to 2.8 eV has attracted considerable interest because it has the potential ability to promote photocatalytic reactions under visible light irradiation [2–4]. The photocatalytic applications of several types of WO3 nanomaterials have been reported, particularly for oxygen (O2) evolution in the presence of an electron accepter [5, 6]. However, WO3 nanomaterials are usually not efficient photocatalysts because of the high electron-hole recombination rate [7]. This is one of the biggest obstacles hindering the development of WO3 as a practical photocatalyst [8]. Recently, many attempts have been made to improve the efficiency of electron-hole pair separation in WO3, such as morphology control, doping, and composites [9].Recently, much effort has been focused on the synthesis of graphene- (GE-) based composites due to their potential application in the photocatalytic field [10–28]. The combination of GE with a well photocatalytic semiconductor is expected to result in a high performance in photocatalytic activity because GE has perfect two-dimensional carbon structure with high thermal conductivity and a large specific surface area [10]. GE is easy to produce from graphene oxide (GO). The presence of oxygen-containing functional group in GO and reduced GO makes it as excellent supporter to anchor photocatalytic semiconductors for the synthesis of GE-based composites. In general, these composites are prepared from the reduction of GO-based materials through a chemical method or heat treatment. However, these methods not only use toxic hydrazine hydrate, but also suffer from some harsh conditions.To the best of our knowledge, no investigation concerning the nanocomposite which consisted of WO3 nanowire clusters and GE nanosheets for water splitting has been reported. Guo et al. reported that WO3@GE composite showed improved photocatalytic activity to drive the water-splitting reaction to produce oxygen [25]. Ng et al. incorporated reduced graphene oxide with WO3 nanoparticles, achieving 1.6 times improvement in the photocurrent generation [26]. In the present work, GE-WO3 nanowire clusters were synthesizedvia a facile hydrothermal method. First, the structures and morphologies of the as-synthesized samples were characterized by X-ray diffraction (XRD), transmission electron microscopy (TEM), X-ray photoelectron spectroscopy (XPS), Fourier transform infrared spectroscopy (FT-IR), Raman spectroscopy, and ultraviolet-visible diffuse reflectance spectroscopy (DRS) techniques. Then, the photocatalytic O2 evolution properties of the samples were investigated by measuring the amount of evolved O2 from water splitting.


## 2. Experimental

### 2.1. Synthesis of GE-WO3 Nanowire Clusters

All of the chemical reagents were analytical grade and were used without further purification. GO was synthesized from natural graphite powder based on modified Hummers method [11]. GE-WO3 nanowire clusters were synthesizedvia a facile hydrothermal method. Typically, Na2WO4
· 2H2O and polyethylene glycol (PEG-4000) were directly dissolved in deionized water, and the pH value of the solution was adjusted to 1.5 adding HCl/NaOH solution. Different weight ratios between GO powders and WO3 nanowire clusters (at 1.0 wt%, 1.5 wt%, 2.0 wt%, 3.0 wt%, and 4.0 wt%) were dispersed rapidly in ethanol with ultrasonic. Then, the two solutions were mixed and transferred into the Teflon-lined stainless steel autoclave with a capacity of 100 mL. Hydrothermal treatments were carried out at 180°C for 30 h. After that, the autoclave was allowed to cool down naturally. Subsequently, the products were collected and washed with deionized water and ethanol several times and dried at 70°C for 12 h in air. Finally, the products were annealed at 400°C for 4 h under nitrogen atmosphere. Pure WO3 nanowire clusters were also obtained through a similar procedure only in the absence of GO.


### 2.2. Characterization

The XRD patterns obtained on a D/max-Ш X-ray diffractometer using Cu Kα radiation (λ
=
1.5418 Å) at a scan speed of 0.05° s−1 were used to determine phase structure. The morphologies of the samples were evaluated by transmission electron microscopy (TEM, JEOL JEM-2010 at 200 kV). Fourier transform infrared (FT-IR) spectroscopy was recorded on a Bruker VECTOR22 FT-IR spectrometer using KBr pellets. Chemical bonding between the functional groups and carbon atoms was confirmed by X-ray photoelectron spectroscopy (XPS, PHI 5000C ESCA System). Raman spectra were recorded on a microscopic confocal Raman spectrometer (Renishaw 1000 NR). The UV-vis spectra were obtainedvia UV-visible spectrophotometer (Shimadzu UV-2500, Japan).


### 2.3. Photocatalytic Oxygen Evolution Experiments

Photocatalytic oxidation reactions were carried out in a self-made Lab Solar gas photocatalysis system with external light irradiation. The reaction temperature was kept atca. 25°C using the temperature-controlled cooling water. The light source was a 150 W xenon lamp with λ
=
400~700 nm and was used as the simulated sunlight source (CEL-HXUV150, China). Before the photochemical reaction, 500 mL of deionized water was degassed by boiling it for 0.5 h and cooling to room temperature and then adding it to the reactor. Then, 2 g of the obtained photocatalysts and 100 mL of 0.1 mol/L Fe2(SO4)3 were added to the reactor under magnetic vigorous stirring to ensure the mixture suspense, using H2SO4 solution to adjust the pH of the mixture at 2. The amount of O2 evolved was determined using gas chromatography (TCD: thermal conductivity detector, nitrogen carrier gas).


## 2.1. Synthesis of GE-WO3 Nanowire Clusters

All of the chemical reagents were analytical grade and were used without further purification. GO was synthesized from natural graphite powder based on modified Hummers method [11]. GE-WO3 nanowire clusters were synthesizedvia a facile hydrothermal method. Typically, Na2WO4
· 2H2O and polyethylene glycol (PEG-4000) were directly dissolved in deionized water, and the pH value of the solution was adjusted to 1.5 adding HCl/NaOH solution. Different weight ratios between GO powders and WO3 nanowire clusters (at 1.0 wt%, 1.5 wt%, 2.0 wt%, 3.0 wt%, and 4.0 wt%) were dispersed rapidly in ethanol with ultrasonic. Then, the two solutions were mixed and transferred into the Teflon-lined stainless steel autoclave with a capacity of 100 mL. Hydrothermal treatments were carried out at 180°C for 30 h. After that, the autoclave was allowed to cool down naturally. Subsequently, the products were collected and washed with deionized water and ethanol several times and dried at 70°C for 12 h in air. Finally, the products were annealed at 400°C for 4 h under nitrogen atmosphere. Pure WO3 nanowire clusters were also obtained through a similar procedure only in the absence of GO.


## 2.2. Characterization

The XRD patterns obtained on a D/max-Ш X-ray diffractometer using Cu Kα radiation (λ
=
1.5418 Å) at a scan speed of 0.05° s−1 were used to determine phase structure. The morphologies of the samples were evaluated by transmission electron microscopy (TEM, JEOL JEM-2010 at 200 kV). Fourier transform infrared (FT-IR) spectroscopy was recorded on a Bruker VECTOR22 FT-IR spectrometer using KBr pellets. Chemical bonding between the functional groups and carbon atoms was confirmed by X-ray photoelectron spectroscopy (XPS, PHI 5000C ESCA System). Raman spectra were recorded on a microscopic confocal Raman spectrometer (Renishaw 1000 NR). The UV-vis spectra were obtainedvia UV-visible spectrophotometer (Shimadzu UV-2500, Japan).


## 2.3. Photocatalytic Oxygen Evolution Experiments

Photocatalytic oxidation reactions were carried out in a self-made Lab Solar gas photocatalysis system with external light irradiation. The reaction temperature was kept atca. 25°C using the temperature-controlled cooling water. The light source was a 150 W xenon lamp with λ
=
400~700 nm and was used as the simulated sunlight source (CEL-HXUV150, China). Before the photochemical reaction, 500 mL of deionized water was degassed by boiling it for 0.5 h and cooling to room temperature and then adding it to the reactor. Then, 2 g of the obtained photocatalysts and 100 mL of 0.1 mol/L Fe2(SO4)3 were added to the reactor under magnetic vigorous stirring to ensure the mixture suspense, using H2SO4 solution to adjust the pH of the mixture at 2. The amount of O2 evolved was determined using gas chromatography (TCD: thermal conductivity detector, nitrogen carrier gas).


## 3. Results and Discussion

Figure1 shows the XRD patterns of the as-synthesized samples. As for the GO, the sharp (001) diffraction peak at 10.46° illustrates that most of the natural graphite has been oxidized into GO. All the diffraction peaks of the pure WO3 nanowire clusters can be indexed to hexagonal WO3 (JCPDS card no. 33-1387). There are no peaks detected for other phases, indicating that single phase of WO3 with high purity has been synthesized. The main diffraction peaks of the GE-WO3 nanowire clusters with 2.0 wt% GE are similar to that of pure WO3 nanowire clusters; no diffraction peak of GO can be seen, indicating the great of GO has been reduced to GE on this occasion. However, no characteristic peaks of GE are presented in the WO3@GE nanocomposites because of the small content of GE used [28].Figure 1
XRD patterns of (a) GO, (b) WO3 nanowire clusters, and (c) GE-WO3 nanowire clusters.Raman spectra of the GO and GE-WO3 nanowire clusters are shown in Figure 2. The Raman spectrum of GO displays two prominent peaks at around 1595 cm−1 and 1346 cm−1, which correspond to the well-documented G and D bands. The G band corresponds to the E
2
g mode observed for sp2 carbon domains, whereas the D band is associated with sp3-hybridized carbon or structural defects. The Raman spectrum of GE in GE-WO3 nanowire clusters also contains both G and D bands (at around 1601 cm−1 and 1359 cm−1, resp.). However, an increased D/G intensity ratio is also observed in comparison with that of the GO spectrum. This change suggests a decrease in the average size of the sp2 domains upon reduction of the exfoliated GO and can be explained by the creation of numerous new graphitic domains that are smaller in size than the ones presented in exfoliated GO.Figure 2
Raman spectra of GO and GE-WO3 nanowire clusters.Figure3 shows the TEM images of WO3 nanowire clusters and GE-WO3 nanowire clusters with 2.0 wt% GE. It is apparent that the WO3 samples display nanowire cluster-like morphology. Careful examination of the TEM image reveals that many thinner nanowires assembled together along the axis direction form nanowire clusters. The morphology of the GE-WO3 nanowire clusters is consisting of WO3 nanowire clusters and thin stacked flakes. It is obvious that WO3 nanowire clusters are uniformly dispersed within the GE nanosheets. This nanostructure enables a multichannel environment to facilitate the efficient charge interaction.TEM images of (a) WO3 nanowire clusters and (b) GE-WO3 nanowire clusters.
(a)
(b)X-ray photoelectron spectroscopy (XPS) is an effective technique to analyze surface chemical states. The C1s XPS spectra of GO and the GE-WO3 nanowire clusters with 2.0 wt% GE are shown in Figure 4, respectively. For the GO, the peak with a binding energy of 284.6 eV can be attributed to the C–C and C–H bonds, while the other three peaks centered at the binding energies of 286.3, 287.7, and 289.2 eV can be assigned to the C–O, C=O, and O=C–OH functional groups, respectively. For the GE-WO3 nanowire clusters, the relative intensity of the sp2 carbon (C–C, 284.6 eV) shows a significant increase, suggesting a sufficient reduction of GO to GE.The C1s XPS spectra of (a) GO and (b) GE-WO3 nanowire clusters.
(a)
(b)Figure5 shows the FT-IR spectra of the GO and GE-WO3 nanowire clusters with 2.0 wt% GE. For the GO, the broad absorption band at 3430.11 cm−1 is related to the stretching peak of the C–OH group, and the characteristic absorption bands of GO are observed at 984.21 cm−1 (epoxy stretching), 1099.91 cm−1 (alkoxy C–O stretching), 1224.89 cm−1 (phenolic C–OH stretching), 1401.85 cm−1 (carboxyl O–H stretching), and 1723.76 cm−1 (C=O stretching vibrations of carboxyl or carbonyl groups). The peak at 1624.76 cm−1 is related to H–O–H bending band of the adsorbed H2O molecules or the in-plane vibrations of sp2 hybridized C–C bonding. For the GE-WO3 nanowire clusters, as compared to the peaks of the functional groups of GO, the broad absorption peak at 866.71 cm−1 is ascribed to the vibration of W–O–W bond. It is also found that the peaks at 1723.76 cm−1, 1224.89 cm−1, and 1089.91 cm−1 in the composites have disappeared, suggesting a sufficient reduction of GO to GE.Figure 5
FT-IR spectra of GO and GE-WO3 nanowire clusters.The UV-vis diffuse reflectance spectra of the WO3 nanowire clusters and GE-WO3 nanowire clusters with 2.0 wt% GE are shown in Figure 6. According to the spectrum, the WO3 nanowire clusters show a sharp edge at about ~465 nm, whereas the GE-WO3 nanowire clusters display an obvious red shift in the absorption edge. This result indicates that the GE-WO3 nanowire clusters can be excited in visible region because of the existence of W–O–C bond, similar to those reported in hybridization of Bi2WO6 with graphite-like carbon layers [14]. Therefore, we can infer that the introduction of GE in WO3 nanowire clusters is effective for the visible light response of the photocatalyst.Figure 6
UV-vis diffuse reflectance spectra of WO3 nanowire clusters and GE-WO3 nanowire clusters.The photocatalytic activities of the as-prepared GE-WO3 nanowire clusters with different weight ratios of GE in terms of evolved O2 from water splitting are measured, and the results are shown in Figure 7. For bare WO3 nanowire clusters, the amount of evolved O2 from water splitting after 8 h isca. 0.175 mmol/L. The photocatalytic activity of the GE-WO3 nanowire clusters can be enhanced with increasing the weight ratio of GO up to 2.0 wt%. This result indicates that the GE-WO3 nanowire clusters with 2.0 wt% GE exhibit the maximum evolved O2 from water splitting (ca. 0.345 mmol/L). This is attributed to GE which serves as an acceptor of the electrons generated in the WO3 and effectively decreases the recombination probability of the photogenerated electron-hole pairs. Further increasing the weight ratio of GO will lead to a decrease, especially in GE-WO3 nanowire clusters with 4.0 wt% GE. It is reasonable because the introduction of a large percentage of black GE leads to shielding of the active sites on the catalyst surface [19].Figure 7
Amount of evolved O2 for the different GE-WO3 nanowire clusters.The efficient charge separation and transfer are crucial for the enhanced photocatalytic activity of the GE-WO3 nanowire clusters. GE has a charge-carrier mobility of 200000 cm2 V−1 s−1 at room temperature, so it is very possible that the incorporation of GE may enhance the charge separation efficiency and suppress the charge recombination as suggested in Figure 8. Under visible light irradiation, electrons (e−) and holes (h+) are generated in the WO3 nanowire clusters (see (1)). WO3 is photocatalyst with weak reducing power, which prohibits the electron transfer to reduce H2O to H2. Therefore, only holes reaction with water to produce O2 can occur spontaneously by using the photocatalyst (see (2)). However, photogenerated electrons can transfer to carbon atoms on the graphene sheets and then react with Fe3+ ions as the scavenger to reduce the recombination of electron-hole pairs (see (3)). Thus, GE serves as the photogenerated electrons acceptor and effectively suppresses the charge recombination in the GE-WO3 nanowire clusters, leaving more positive charged holes on the WO3 surface and promoting the production of oxygen:
(1)
W
O
3
⟶
h
v
e
-
+
h
+
(2)
2
H
2
O
+
4
h
+
⟶
4
H
+
+
O
2
(3)
Fe
3
+
+
e
-
⟶
Fe
2
+Figure 8
The possible photocatalytic mechanism of the GE-WO3 nanowire clusters.


## 4. Conclusions

In summary, GE-WO3 nanowire clusters were synthesized by a facile hydrothermal method. The GE-WO3 nanowire clusters with 2.0 wt% GE exhibited enhanced performance compared to pure WO3 nanowire clusters for O2 evolution from water splitting. The sensitization of WO3 nanowire clusters by GE enhanced the visible light absorption property of GE-WO3 nanowire clusters. The chemical bonding between WO3 and GE reduced the recombination of the photogenerated electron-hole pairs, leading to improved photocatalytic activity.



---

*Source: 943537-2014-07-24.xml*