# TiO2/Diazonium/Graphene Oxide Composites: Synthesis and Visible-Light-Driven Photocatalytic Degradation of Methylene Blue

Authors: Nguyen Thi Vuong Hoan; Nguyen Ngoc Minh; Thoi Thi Kim Nhi; Nguyen Van Thang; Vu Anh Tuan; Vo Thang Nguyen; Nguyen Mau Thanh; Nguyen Van Hung; Dinh Quang Khieu
Journal: Journal of Nanomaterials
 (2020)

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## Abstract

In the present article, the synthesis of TiO2/diazonium/graphene oxide and its photocatalytic activity for methylene blue (MB) degradation have been demonstrated. The functionalization of graphene oxide (GO) with diazonium salt (diazonium-GO) was conducted for enhancing the dispersibility of GO in distilled water. TiO2 was highly dispersed in diazonium-GO to form TiO2/diazonium/graphene. The obtained specimens were characterized by X-ray diffraction, FT-IR spectroscopy, Raman spectroscopy, UV-Vis spectroscopy, scanning electron microscope, transmission electron microscopy, and X-ray photoelectron spectroscopy. It was found that the TiO2 phase in TiO2/diazonium/GO composites can be controlled by adjusting the amount of ethanol or titanium oxide in the reactant mixture. The obtained composites exhibited photocatalytic activities for methylene blue degradation (MB). The composite with ac. 70% anatase can provide the highest MB degradation efficiency. The studying of some intermediates for MB photocatalytic degradation using LC-MS showed that structure of MB by the cleavage and oxidation of one or more of the methyl group substituent on the amine groups lead to form compounds with low molecular masses. Total organic carbon studies confirmed a complete mineralization of MB. The present catalyst was stable and recyclable after three times with a negligible loss of catalytic activity. In addition, the TiO2/diazonium/GO can also photocatalyze for the degradation of some other dyes (phenol, methyl red, and Congo red).


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## Body

## 1. Introduction

Titanium oxide-based materials in several types and forms have exhibited excellent potential as powerful photocatalysts for various reactions thanks to their chemical stability, nontoxicity, and high reactivity and interesting materials with nonline optical properties for applications in ultrafast optical information processing, optical switching, and optical limiting for protection against strong laser radiation [1]. In particular, titanium oxide has been used for such significant applications as the solar photons for the photocatalytic depollution [2], energy conversion [3], and purification of polluted water and air [4]. It is well known that three polymorphs of titania are brokite, anatase, and rutile. Rutile is a stable phase while brokite and anatase are metaphases. Because of the difficulty in the synthesis, the catalytic activity of brokite is seldom reported. Anatase exhibits higher catalytic activities compared with those of rutile [5, 6]. However, detailed mechanisms and factors influencing different activities of these polymorphs are controversial. During the photocatalytic process, the photo-induced electrons and holes are generated because the electrons are excited from the valence band (VB) of TiO2 to the conduction band (CB). The holes and electrons will react with water and oxygen to form free radicals which can oxidize and decompose the organic compounds [7]. However, the fast recombination of excited state CB electrons and VB holes without initiating the photocatalytic activity limits TiO2 in catalytic applications. Many approaches of preventing the photo-induced electron-hole recombination have been reported, such as using TiO2 composites with transition metal oxides [8, 9], noble metals [10, 11], and carbon nanotubes (CNT) [12, 13].Graphene is an interesting material because of its unique electronic property [14], high mobility and transparency [15], flexible structure, and high surface area [16]. Graphene oxide (GO) could be considered as graphene functionalized by hydroxyl, carboxylic acid, and epoxide groups [17, 18], and their properties are sensitive to chemical doping, adsorbed or bound species [19]. Generally, an electron energy gap could be varied by oxidation of graphene, and the value of the energy gap depends on oxidization degree of graphene and species of oxygen-containing groups. It means that GO could change from conducting to insulating by tuning the C/O ratios [20, 21].The combination of TiO2 with GO is considered as the versatile composite for photocatalyst due to the excellent absorbability and conductivity of GO. Much attempt on investigation into the synthesis and application of TiO2/GO composites as photocatalyst has been reported. Chen et al. [22] reported the synthesis of visible-light-driven graphene oxide/TiO2 composites with p/n heterojunction from TiCl3 source, and these semiconductors could be excited by visible light and acted as a sensitizer in graphene oxide/TiO2 composites. TiO2 nanorods are self-assembled on the graphene oxide sheets at the water/toluene interface [23]. During the preparation of GO–TiO2 composites by sonicating the dispersed TiO2 nanoparticles and GO in ethanol, Williams et al. [24] found that GO can be reduced photocatalytically by TiO2 under UV light irradiation. However, the formation of homogeneous mixture of TiO2 and GO is often a problem because the easy formation of agglomeration of both titania and GO prevents the effective dispersion of these metal oxide nanoparticles in a GO matrix. In order to overcome this experimental hinderance, several GO derivatives have been prepared by grafting new functional groups such as ethylenediamine [25], EDTA [26], and diazonium of sulfanilic acid [27] through a GO backbone to form the water soluble GO; as a result, nanooxide particles are effectively dispersed in a GO matrix. Continuing this idea, in the present paper, GO was modified by the diazonium salt of sulfanilic acid prior to dispersion of TiO2 on GO with an idea to enhancing the possibility of inserting active oxygen-containing polarization groups between graphite layer in graphene oxide, which adjusts the semiconductivity of graphene oxide in the obtained composite. The photocatalytic activity of the TiO2/diazonium/GO composite material was evaluated by the degradation of methylene blue (MB) in the visible light region.


## 2. Experimental

### 2.1. Materials

Graphite powder (C, 99%), titanium tetrachloride (TiCl4, 99%), potassium permanganate (KMnO4, 99.5%), sodium nitrate (NaNO3, 99%), sulfuric acid (H2SO4, 98%), and ethanol (C2H5OH, 99.5%) were purchased from Merck. Hydrogen peroxide (H2O2, 30%), sulfanilic acid ((H2N)C6H4SO3H, 99.8%), ammonia solution (NH4OH, 25%), hydrochloric acid (HCl, 37%), 1,4-benzoquinone (C6H4O2, ≥99%, BQ), dimethyl sulfoxide ((CH3)2SO, 99.9%, DMSO), diamonium oxalate ((NH4)2C2O4·H2O), ≥99.5%, AO), tert-Butanol ((CH3)3COH, ≥99%, TB), and methylene blue (C16H18N3SCl, MB) were obtained from Sigma-Aldrich. All chemicals used were of analytical grade and were used as received without any further purification.


### 2.2. Synthesis of Graphene Oxide

GO was synthesized by a modified Hummers’ method [28]. In a typical synthesis, 1.0 g of graphite powder was added into 2.5 g of NaNO3 and 100 mL of concentrated H2SO4 under magnetic stirring. Then, 3.0 g of KMnO4 was slowly added to this mixture at 10°C under stirring for 2 h before adding 100 mL of distilled water and heating up to 98°C under stirring for another 2 h. After that, 10 mL of H2O2 was poured into the mixture with stirring for 2 h. As the result, the color of the mixture changed to bright yellow. Finally, the mixture was filtered and washed with a 5% HCl aqueous solution to remove metal ions, followed by distilled water for removal of the acid. The brown-black solid obtained was separated by ultrasonic treatment in water and then dried at 60°C for 12 h.


### 2.3. Synthesis of TiO2/Diazonium/GO Composites

The preparation of modified graphene oxide was carried out as follows. Firstly, the diazonium salt was prepared by dissolving 46 mg of sulfanilic acid in 10 mL of distilled water containing 30 mg of Na2CO3 in ice bath, then heating gently for sulfanilic acid to dissolve completely [27]. Next, 18 mg of NaNO2 was dissolved into 5 mL of distilled water before being added to the prepared sulfanilic acid solution. A 1 N HCl solution (2.4 mL) was added dropwise to the above mixture and stirred to obtain diazotized sulfanilic acid. Next, 75 mg of GO was added to the diazonium solution and stirred continuously for 2 hours. The solid was separated by filtering and drying. The samples were diazotized sulfanilic acid-GO (denoted as Dia-GO). Sulfanilic acid contains a sulfo group (SO3H) and an amino group (NH2). The amino group can react with cold nitrous acid to produce diazotized sulfanilic acid which can be used to synthesize the sulfonated graphene oxide composite.The reactions are assumed as follows:The composite of TiO2/Dia-GO was prepared as described elsewhere [29]. Firstly, the effect of TiCl4 concentration on the phase formation of TiO2 phases was studied. 15 mg of Dia-GO was dissolved in 120 mL solvent (40 mL ethanol/80 mL distilled water) under ultrasonication for 2 hours. The mixture was cooled down at 0-5°C. Then, 2 mL TiCl4 was added slowly at different concentration to Dia-GO suspension under vigorous stirring to obtain the brown suspension. The resulting suspension was added to an autoclave at 180°C for 12 hours. The obtained solid was separated by filter and washed by distilled water for several times and then dried at 60°C for 6 hours. The obtained samples are denoted as Tx-y/Dia-GO: T0.05-40/Dia-GO, T0.15-40/Dia-GO, T0.45-40/Dia-GO, and T1.35-40/Dia-GO with the symbol of x=0.05, 0.15, 0.45, and 1.35 representing the concentration in mole of titanium chloride and y of 40 representing the mL ethanol in 120 mL mixture. Subsequently, the effect of ethanol/water ratio (v/v) used for the hydrolysis on the titania phases was investigated. The procedure was similar to the one mentioned above but only 120 mL mixture with the amount of ethanol differed from 20 to 120 mL. The sample as denoted as T0.05-20/Dia-GO, T0.05-40/Dia-GO, T0.05-60/Dia-GO, T0.05-80/Dia-GO, T0.05-100/Dia-GO, and T0.05-120/Dia-GO corresponding to the ethanol/distilled water (v/v) being 20/100, 40/80, 60/60, 80/40, 100/20, and 120/0.


### 2.4. Characterization of Materials

The X-ray diffraction (XRD) data of all samples were collected in a D8 Advanced Bruker anode X-ray Diffractometer with Cu Kα. The quantitative analysis of mixture of anatase-rutile was performed using the XRD method as previously proposed [30]. Particle diameters smaller 5 microns are desirable to ensure adequate reproducibility of diffraction intensity measurement.
(1)XR=11+0.8IA/IR⋅100%,XA=11+1.26IR/IA⋅100%,where IA and IB, respectively, are the intensity of diffraction at (110) for rutile phase and (101) for anatase phase; XR and XA are the percentage of rutile and anatase, respectively; the experimental parameters of 0.80 and 1.26 are obtained from the regression of the relative given amount of anatase and rutile versus IR/IA.Transmission electron microscope (TEM) images were obtained by JEOL JEM-2100F. FT-Infrared (IR) spectra for the samples were recorded on an IR Prestige-21 spectrophotometer (Shimadzu). X-ray photoelectron spectrometry (XPS) was used for surface analysis with an ESCALAB 250 (Thermo VG, UK) spectrometer with X-ray source monochromated Al Kα radiation (1486.6 eV). DRS-UV-Vis spectra were recorded with Jasco-V670 instrument. The measurement of photoluminescence (PL) was conducted by means of a spectrometer Horiba Jobin-Yvon HR800 LabRam using UV excitation. The identification of MB degradation was performed using a liquid chromatography-mass spectrometry (LC-MS) method (Ultimate 3000 plus, Hypersil GOLD C18 (150×2.1 mm, 2.0 μm), Thermo, MA, USA).


### 2.5. Photocatalytic Activity

In this study, the photocatalytic activities of obtained materials were investigated via the degradation of methylene blue (MB) in an aqueous solution under the irradiation of 75 W-220 V filament lamps (Dien Quang) with a UV cut off filter (λ<390 nm, d=77 mm).The experiments were carried out with a 500 mL dye solution at various concentrations containing 100 mg of catalyst. The mixture was stirred continuously for 2 hours in the dark to establish an adsorption-desorption equilibrium before turning on the lamp. Three millites of solution were withdrawn after a certain time and centrifuged to remove the solid. The concentration of MB in solution was determined by its absorption atλmax=664nm. Each experiment was in triplicate.The performance of MB mineralization was calculated based on TOC (total organic carbon) measurements from(2)M=100×TOC0–TOCtTOC0,where TOC0 and TOCt are the MB concentrations at the initial and time t of the reaction, respectively. The concentration of TOC was determined using a TOC analyzer (model: Multi N/C®2100 S, Analytik Jena, Germany).


## 2.1. Materials

Graphite powder (C, 99%), titanium tetrachloride (TiCl4, 99%), potassium permanganate (KMnO4, 99.5%), sodium nitrate (NaNO3, 99%), sulfuric acid (H2SO4, 98%), and ethanol (C2H5OH, 99.5%) were purchased from Merck. Hydrogen peroxide (H2O2, 30%), sulfanilic acid ((H2N)C6H4SO3H, 99.8%), ammonia solution (NH4OH, 25%), hydrochloric acid (HCl, 37%), 1,4-benzoquinone (C6H4O2, ≥99%, BQ), dimethyl sulfoxide ((CH3)2SO, 99.9%, DMSO), diamonium oxalate ((NH4)2C2O4·H2O), ≥99.5%, AO), tert-Butanol ((CH3)3COH, ≥99%, TB), and methylene blue (C16H18N3SCl, MB) were obtained from Sigma-Aldrich. All chemicals used were of analytical grade and were used as received without any further purification.


## 2.2. Synthesis of Graphene Oxide

GO was synthesized by a modified Hummers’ method [28]. In a typical synthesis, 1.0 g of graphite powder was added into 2.5 g of NaNO3 and 100 mL of concentrated H2SO4 under magnetic stirring. Then, 3.0 g of KMnO4 was slowly added to this mixture at 10°C under stirring for 2 h before adding 100 mL of distilled water and heating up to 98°C under stirring for another 2 h. After that, 10 mL of H2O2 was poured into the mixture with stirring for 2 h. As the result, the color of the mixture changed to bright yellow. Finally, the mixture was filtered and washed with a 5% HCl aqueous solution to remove metal ions, followed by distilled water for removal of the acid. The brown-black solid obtained was separated by ultrasonic treatment in water and then dried at 60°C for 12 h.


## 2.3. Synthesis of TiO2/Diazonium/GO Composites

The preparation of modified graphene oxide was carried out as follows. Firstly, the diazonium salt was prepared by dissolving 46 mg of sulfanilic acid in 10 mL of distilled water containing 30 mg of Na2CO3 in ice bath, then heating gently for sulfanilic acid to dissolve completely [27]. Next, 18 mg of NaNO2 was dissolved into 5 mL of distilled water before being added to the prepared sulfanilic acid solution. A 1 N HCl solution (2.4 mL) was added dropwise to the above mixture and stirred to obtain diazotized sulfanilic acid. Next, 75 mg of GO was added to the diazonium solution and stirred continuously for 2 hours. The solid was separated by filtering and drying. The samples were diazotized sulfanilic acid-GO (denoted as Dia-GO). Sulfanilic acid contains a sulfo group (SO3H) and an amino group (NH2). The amino group can react with cold nitrous acid to produce diazotized sulfanilic acid which can be used to synthesize the sulfonated graphene oxide composite.The reactions are assumed as follows:The composite of TiO2/Dia-GO was prepared as described elsewhere [29]. Firstly, the effect of TiCl4 concentration on the phase formation of TiO2 phases was studied. 15 mg of Dia-GO was dissolved in 120 mL solvent (40 mL ethanol/80 mL distilled water) under ultrasonication for 2 hours. The mixture was cooled down at 0-5°C. Then, 2 mL TiCl4 was added slowly at different concentration to Dia-GO suspension under vigorous stirring to obtain the brown suspension. The resulting suspension was added to an autoclave at 180°C for 12 hours. The obtained solid was separated by filter and washed by distilled water for several times and then dried at 60°C for 6 hours. The obtained samples are denoted as Tx-y/Dia-GO: T0.05-40/Dia-GO, T0.15-40/Dia-GO, T0.45-40/Dia-GO, and T1.35-40/Dia-GO with the symbol of x=0.05, 0.15, 0.45, and 1.35 representing the concentration in mole of titanium chloride and y of 40 representing the mL ethanol in 120 mL mixture. Subsequently, the effect of ethanol/water ratio (v/v) used for the hydrolysis on the titania phases was investigated. The procedure was similar to the one mentioned above but only 120 mL mixture with the amount of ethanol differed from 20 to 120 mL. The sample as denoted as T0.05-20/Dia-GO, T0.05-40/Dia-GO, T0.05-60/Dia-GO, T0.05-80/Dia-GO, T0.05-100/Dia-GO, and T0.05-120/Dia-GO corresponding to the ethanol/distilled water (v/v) being 20/100, 40/80, 60/60, 80/40, 100/20, and 120/0.


## 2.4. Characterization of Materials

The X-ray diffraction (XRD) data of all samples were collected in a D8 Advanced Bruker anode X-ray Diffractometer with Cu Kα. The quantitative analysis of mixture of anatase-rutile was performed using the XRD method as previously proposed [30]. Particle diameters smaller 5 microns are desirable to ensure adequate reproducibility of diffraction intensity measurement.
(1)XR=11+0.8IA/IR⋅100%,XA=11+1.26IR/IA⋅100%,where IA and IB, respectively, are the intensity of diffraction at (110) for rutile phase and (101) for anatase phase; XR and XA are the percentage of rutile and anatase, respectively; the experimental parameters of 0.80 and 1.26 are obtained from the regression of the relative given amount of anatase and rutile versus IR/IA.Transmission electron microscope (TEM) images were obtained by JEOL JEM-2100F. FT-Infrared (IR) spectra for the samples were recorded on an IR Prestige-21 spectrophotometer (Shimadzu). X-ray photoelectron spectrometry (XPS) was used for surface analysis with an ESCALAB 250 (Thermo VG, UK) spectrometer with X-ray source monochromated Al Kα radiation (1486.6 eV). DRS-UV-Vis spectra were recorded with Jasco-V670 instrument. The measurement of photoluminescence (PL) was conducted by means of a spectrometer Horiba Jobin-Yvon HR800 LabRam using UV excitation. The identification of MB degradation was performed using a liquid chromatography-mass spectrometry (LC-MS) method (Ultimate 3000 plus, Hypersil GOLD C18 (150×2.1 mm, 2.0 μm), Thermo, MA, USA).


## 2.5. Photocatalytic Activity

In this study, the photocatalytic activities of obtained materials were investigated via the degradation of methylene blue (MB) in an aqueous solution under the irradiation of 75 W-220 V filament lamps (Dien Quang) with a UV cut off filter (λ<390 nm, d=77 mm).The experiments were carried out with a 500 mL dye solution at various concentrations containing 100 mg of catalyst. The mixture was stirred continuously for 2 hours in the dark to establish an adsorption-desorption equilibrium before turning on the lamp. Three millites of solution were withdrawn after a certain time and centrifuged to remove the solid. The concentration of MB in solution was determined by its absorption atλmax=664nm. Each experiment was in triplicate.The performance of MB mineralization was calculated based on TOC (total organic carbon) measurements from(2)M=100×TOC0–TOCtTOC0,where TOC0 and TOCt are the MB concentrations at the initial and time t of the reaction, respectively. The concentration of TOC was determined using a TOC analyzer (model: Multi N/C®2100 S, Analytik Jena, Germany).


## 3. Results and Discussion

### 3.1. Characterization of Materials

#### 3.1.1. Preparation of Diazonium/GO (Dia-GO)

Figure1 presents XRD patterns of graphite, GO, and Dia-GO. The sharp peak around 26.5° is characteristic of graphite [31] (the inset of Figure 1). The peak at around 11.4° of GO can be attributed to the introduction of oxygen-containing functional groups into the graphite sheets to form of graphene oxide [32]. These functional groups, especially the -SO3H group between the layers of GO, interact strongly with polarizing groups on GO, leading to a shift of a 2θ angle to the smaller value in GO [33, 34], resulting in an increase in dspacing from 7.82 Å for GO to 8.11 Å for Dia-GO (Figures 1(a) and 1(b)). The similar results have been also obtained in the reported papers [34–36] in which GO is chemically functionalized with diazonium of sulfanilic acid.Figure 1
X-ray diffraction patterns for GO (a), Dia-GO (b), and the inset present the XRD pattern of graphite.From Figure2, it can be seen that the GO shows characteristic bands of oxygen-containing functional group vibrations: hydroxyl group (-OH) over the range of 3400-3500 cm-1, C=O vibration (-COOH) at 1636-1700 cm-1, and C-O vibration at 1229 cm-1 and 1060 cm-1 [37–39]. In addition, there are also characteristic peaks for the oscillation of the O=S=O (group -SO3H) bond at 1620-1650 cm-1, 1400 cm-1, and 1100 cm-1 [40–43] in Dia-GO. These results confirmed the formation of diazonium/graphene oxide.Figure 2
FTIR spectra of GO (a), Dia-GO (b).


#### 3.1.2. The Preparation of TiO2/Diazonium/GO

The effect of TiCl4 concentration on the phase formation of TiO2 was investigated by XRD studies (Figure 3).Figure 3
XRD patterns of TiO2/Dia-GO samples.It can be seen that the obtained samples all exhibit characteristic diffraction peaks of titanium oxide. As seen in Figure3, the formation of titanium oxide phases (rutile or anatase) depended on titanium chloride concentration. The rutile phase was formed primarily as the titanium chloride concentration was high. T1.35-40/Dia-GO composed of mainly rutile phase with characteristic peaks at 2θ angles of 27.4°, 36.1°, and 41.3° indexed as (110), (101), and (111), respectively (JCPDS: No 21-1276), whereas anatase phase increased with a decrease in titanium chloride concentration. The characteristic peaks with increasing intensity of anatase phase were observed at angles 2θ of 25.5°, 37°, 53.9°, 56.5°, and 62.5° indexed as (101), (004), (200), (105), and (211), respectively (JCPDS: No 21-1272). Primary estimation of catalytic activity for the obtained composite revealed that the use of T0.05-40/Dia-GO led to the highest yield of MB degradation. Therefore, T0.05-40/Dia-GO was selected to further study the effect of ethanol/distilled water ratio on the formation of titanium oxide.The composition of titanium oxide depends not only on titanium chloride concentration but also on the amount of ethanol used in the hydrolysis step. Figure4 shows XRD patterns of T0.05-y/Dia-GO composite materials synthesized at various amounts of ethanol y (y: 20-120 mL of ethanol used).Figure 4
X-ray diffraction patterns for T0.05-y/Dia-GO samples (y=20, 40, 60, 80, 100, and 120 mL ethanol).For T0.05-120/Dia-GO, TiO2 phase existed mainly in anatase form with the characteristic diffraction peaks at 2θ angle of 25.5° with high intensity. The intensity of this characteristic peak decreased with the decrease of ethanol/distilled water ratio. Meanwhile, the intensity of characteristic diffractions at 27.4° and 36.1° for rutile increased significantly with the decrease of the ethanol/distilled ratio. The quantitative analysis of titanium oxide phase showed that when the amount of ethanol increased from 20 mL to 120 mL, the anatase TiO2 phase composition increased from 15.25% to 100%, corresponding to the reduction of rutile phase composition from 84.75% to 0%. Thus, in the samples of synthetic materials, titanium oxide existed in both forms, anatase and rutile.The results of photocatalytic activity of TiO2/Dia-GO nanocomposite are listed in Table 1. It can be seen that photocatalytic activity depended significantly on titania phase composition. Composite with 100% TiO2 in rutile phase exhibited the lowest photocatalytic activity on MB degradation (around 23.4%). The photocatalytic activity increased with an increase in the amount of anatase phase. The MB degradation efficiency peaked at 69.8% as the anatase phase growed to around 73.4% (corresponding to T0.05-100/Dia-GO) before slightly reducing when the amount of anatase phase kept increasing. It is well-known that anatase has lower absorbance ability towards visible light than rutile due to the larger band gap (3.2 eV) than that (3.0 eV) of rutile. However, its indirect band gap provides a longer lifetime of photoinduced electron/hole pairs than direct band gap in rutile because the direct recombination of photoexcited electrons from the conduction band to valence band of anatase TiO2 is impossible [6]. The mixture with an appropriate ratio of anatase and rutile should provide the more superior photocatalytic activity than that of individual rutile or anatase. Then, T0.05-100/Dia-GO was selected for further experiments.Table 1
Phase composition and methylene blue conversion (%) of TiO2/Dia-GO composites (C0,MB=100mg/L, V=100mL, mCat=100mg, and time=120min).
Notation
Phase composition (%)
MB conversion (%)
Anatase
Rutile
T1.35-40/Dia-GO
0
100
23.41
T0.45-40/Dia-GO
0
100
24.84
T0.15-40/Dia-GO
15.25
84.75
45.28
T0.05-40/Dia-GO
40.25
59.75
48.73
T0.05-60/Dia-GO
58.89
41.11
54.23
T0.05-80/Dia-GO
62.19
37.81
57.05
T0.05-100/Dia-GO
73.45
26.55
69.82
T0.05-120/Dia-GO
100
0
63.55The morphologies of T0.05-100/Dia-GO observed by TEM are shown in Figure5. The TiO2 nanoparticles were dispersed highly over the Dia-GO sheet with an average particle size of 5-15 nm (Figure 5(a)). The crystallite size of 11.7 nm obtained by Debye-Scherrer analysis at (101) diffraction is close to the average size of TiO2 particles observed by TEM indicated that the morphology of T0.05-100/Dia-GO consists of single crystals of TiO2 highly dispersed on Dia-GO. Elemental analysis for composite surface showed that T0.05-100/Dia-GO consisted of N, S, and Ti (Figure 5(b)) as an additional evidence of the successful synthesis of the composite of TiO2/diazonium/GO.Figure 5
(a) TEM observation and (b) EDX spectrum of T0.05-100/Dia-GO.
(a)
(b)Based on the band theory of semiconductors, the conduction band (CB) of TiO2 is mainly determined by the Ti 3d orbital energy levels, while the valence band (VB) is mainly formed from the O2p orbitals. As compared to the O2p orbital, other nonmetal elements such as N and S, P possess 2p orbitals locating at more negative energy levels; hence, the partial substitution of the impurity dopants N and S will result in the formation of new energy bands above the TiO2 valence band, thus providing the photocatalytic activity over the visible light region of TiO2 [44].The textural property of the obtained composite was estimated by means of the nitrogen adsorption/desorption isotherms (Figure6). The isotherm curve is the type IV and H3 according to IUPAC classification. The hysteresis loop at the high relative pressure in the range of 0.5 to 0.9 indicated the existence of micromesoposity. The specific surface area of materials based on BET calculation was 152 m2·g-1.Figure 6
The nitrogen adsorption/desorption isotherms of T0.05-100/Dia-GO.DRS-UV-Vis spectra of TiO2/GO (1), Dia-GO (2), and T0.05-100/Dia-GO (3) are presented in Figure 7(a). Bulk TiO2 is considered as an indirect semiconductor [45]. In nanoparticles, the lattice periodicity is lost over a length-scale comparable to the nanoparticle size so the effectiveness of this selection rule breaks down and direct transitions can actually be expected to take place [46, 47]. We used the classical relation near the band-edge optical absorption in a semiconductor to calculate the energy of band-band transition
(3)α=Ahν−Egnhν,where α is the absorption coefficient, Eg is the energy gap, hν is the photon energy, and n is equal to 1/2 for direct transitions and 2 for indirect ones. The Eg value can be calculated from the linear plot of αhν1/n or αhν2vs. hν by extrapolating at zero the linear portion near the band-edge. (Figures 7(b) and 7(c)). Both types of plots exhibit the highly linearity with R2=0.97–0.99 indicating direct or indirect transition that likely occur. The value for types of band gap energy is listed in Table 2. It is obvious that the value of indirect band energy tends to be lower than direct band energy that is similar to some previous reports [45, 46]. It is found that the indirect band gap energy decreased in the order TiO2/GO (2.71 eV) > Dia-GO (2.62 eV) > T0.05-100/Dia-GO (2.35 eV) and these TiO2-based materials exhibit the indirect band gap energy smaller than that of pure TiO2 (3-3.2 eV) [45–47]. The absorption edge shifts towards a visible region due to the possible interaction of between TiO2 and modifiers (N and S). This shift is assigned to the generation of intermediate gap energy levels near the valence band of titania. Consequently, narrowing the band gap energy and minimizing the recombination of photoexited electron/hole pairs are considered for the obtained composite T0.05-100/Dia-GO.Figure 7
(a) DRS-UV-Vis spectra of TiO2/GO (1), Dia-GO (2), and T0.05-100/Dia-GO (3); (b) Tauc’s plots of (αhν)1/2 vs. hν and (c) of (αhν)2 vs. hν for TiO2/GO (1), Dia-GO (2), and T0.05-100/Dia-GO (3).
(a)
(b)
(c)Table 2
Eg values for direct and indirect transitions of the investigated samples.
Sample
Eg (indirect) (eV)
Eg (direct) (eV)
TiO2/GO
2.71
3.15
Dia-GO
2.62
3.12
T0.05-100/Dia-GO
2.35
3.09Raman spectroscopy is a useful approach for the characterization of the physicochemical properties of graphene-based composites. It is known that in Raman spectroscopy, the G band is assigned to the first-order scattering of the sp2 C atoms (∼1600 cm−1), and the D band is attributed to a breathing mode of k-point photons (∼1300 cm−1). At the same time, an increase in ID/IG ratio arises from a lower degree of crystallinity in the graphitic structure. Two bands in the Raman spectra of GO and T0.05-100/Dia-GO located at approximately 1300 and 1600 cm−1 attributed to the D band and G band, respectively (Figure 8(a)). The ID/IG ratio increased from 1.42 for GO to 1.45 for T0.05-100/Dia-GO suggesting a decrease in the size of the in-plane sp2 domains and the partially ordered crystal structure of graphene oxide. These results provided more evidence for the insert of titania and diazonium salt into graphene oxide.Figure 8
(a) Raman spectra of GO and T0.05-100/Dia-GO; (b) photoluminescence (PL) spectra of rutile (1), anatase (2), Dia-GO (3), TiO2-GO (4), and T0.05-100/Dia-GO (5).
(a)
(b)PL spectra of obtained samples are shown in Figure8(b). It can be seen that the luminescent intensity of rutile was the highest, followed by anatase, Dia-GO, and TiO2/GO, and the lowest one belonged to T0.05-100/Dia-GO. It is well known that low PL intensity means low recombination of electron and holes; then, the opposite would be high PL intensity would increase recombination rate and reduce photocatalytic activity. These results demonstrate that the dispersion of TiO2 on graphene reduces the recombination of photonic electrons and photogenic holes, which may increase the photocatalytic activity of the material.Figure9(a) shows the XPS spectrum of T0.05-100/Dia-GO composite, indicating the presence of the four main elements at 162, 284.6, 529.8, and 458.6 eV corresponding to sulfur (S2p), carbon (C1s), oxygen (O1s), and titanium (Ti2p), respectively. Figure 9(b) shows the XPS Ti2p core level. It can be seen that characteristic peaks are at around 457.6 eV for Ti2p3/2 and 463.4 eV for Ti2p1/2, indicating a successful loading of Ti on the surface of GO [5, 48]. Figure 9(c) represents the S2p doublet core peak locating at 160.8-169 eV, associated with a sulfonate type [49]. N1s spectrum is shown in Figure 9(d). The binding energy of around 399.6 eV can be assigned to tertiary amine [50]. The C1s spectrum of GO in Figure 9(e) can be deconvoluted into three peaks at 284.6, 286.7, and 288.5 eV, respectively. Two main peaks at 284.6 and 286.7 eV are usually attributed to adventitious carbon and graphitic carbon from GO, and hydroxyl carbon (C-OH), respectively [51]. The other peak at 288.5 eV can be assigned to carboxyl carbon (O-C=O) [51].Figure 9
XPS spectra of T0.05-100/Dia-GO: (a) survey spectrum; (b) Ti2p; (c) S2p; (d) N1s; (e) C1s.
(a)
(b)
(c)
(d)
(e)


### 3.2. Photocatalytic Performance of TiO2/Diazonium/GO Composites for MB Degradation in a Visible-Light Region

#### 3.2.1. Leaching Experiment

The kinetics of decolorization of MB in several conditions are shown in Figure10. It was found that the decolorization of MB was not observed if visible light was irradiated in the absence of T0.05-100/Dia-GO suggesting that MB was stable and did not undergo photolysis. A leaching experiment was also conducted in which the T0.05-100/Dia-GO was filtered by centrifugation after 60 min. of irradiation. The MB decolorization was quenched even when the light was still irradiated. This indicates that there was no leaching of the active species into the reaction solution from the heterogeneous catalyst. The above experimental results confirmed that T0.05-100/Dia-GO acted as a heterogeneous catalyst in the degradation reaction of MB.Figure 10
Leaching experiment (V=500mL, C0=100mg·L−1; mass of catalyst: 100 mg).Figure11(a) presents the adsorption kinetics and photocatalytic decolorization of MB on TiO2/Dia-GO catalyst. This catalyst presented a low adsorption capacity of MB. The adsorption was saturated from 100 min to 120 min depending on the initial MB concentration. In this study, the light illumination was carried out only when the dark adsorption reached adsorption/desorption equilibrium.Figure 11
(a) The adsorption and photodegradation kinetics of MB on T0.05-100/Dia-GO catalyst; (b) the plots of the1/KlnC+C against t different initial MB concentration.
(a)
(b)


#### 3.2.2. Adsorption Isotherm

The equilibrium adsorption capacity,qe, can be expressed as follows:
(4)qe=V⋅C0−Cem,where C0 and Ce are the MB concentration at initial and equilibrium time (mg·L-1); V is the volume of the MB solution (L); m is the mass of catalyst (g).The relationship betweenCe and qe is expressed by the Langmuir isotherm model as equation (5) and the Freundlich model as equation (6):
(5)qe=ΚL⋅qm⋅Ce1+KL⋅Ce,(6)qe=KF⋅Ce1/n,where qm is the maximum monolayer adsorption capacity (mg·L-1); KL is the Langmuir adsorption equilibrium constant (mg-1·L); KF and n are Freundlich parameters.The calculated parameters can be obtained from nonlinear regression of equations (5) and (6) and are listed in Table 3. A high determination coefficient (R2=0.99) for Langmuir model and Freundlich model indicated that the equilibrium data was well fitted in both models. It implies a monolayer adsorption and the existence of heterogeneous surface in the adsorbents.Table 3
The parameters of Langmuir and Freundlich model.
Langmuir model
Freundlich model
KL (L·mg-1)
qm (mg·g-1)
R2
KF
N
R2
3.2.10-2
138.12
0.99
5.837
1.35
0.99


### 3.3. Decomposition Kinetics

Based on the Langmuir-Hinshelwood model, the overall reaction could be illustrated as follows:(7)T0.05−100/GO−Dia+MB⇄k−1k1T0.05−100/GO−Dia⋯MB∗→k2degradationproductswhere k1 and k–1 are the forward/back adsorption rate constant, respectively; k2 is the kinetic rate coefficient of the degradation process.The law rate is expressed as follows:(8)r=−dCdt=kMLH⋅θ,where C is the dye concentration (mg·L−1) at time t; kMLH is the kinetic rate coefficient (mg·L−1·min−1); θ is the fraction of the surface covered by MB. θ is expressed in the Langmuir model as [37]
(9)θ=ΚL⋅C1+KL⋅C.Substituting (8) to (6) gives
(10)dCdt=−kMLH⋅KL⋅C1+KL⋅C.Then,(11)∫1+KL⋅CKL⋅C⋅dC=−∫kMLH⋅dt.Integrating equation (11) with the boundary conditions t⟶0 and C⟶C0e gives
(12)1KL⋅lnC+C=−kMLH⋅t+I0,when t=0, then
(13)I0=1KL⋅lnC0e+C0e.Substituting (13) into (12) gives
(14)1KL⋅lnC+C=−kMLH⋅t+1KL⋅lnC0e+C0e,where C0e (mg·L−1) is the equilibrium concentration of adsorbate at time t (min) taken from light illumination.The plot of the (1/KlnC+C) against t gives a straight line with slope kMLH (Figure 11(b)).For the kinetics of unimolecular reaction on heterogeneous catalyst the Langmuir-Hinshelwood model is widely used. In this study, the Langmuir-Hinshelwood was also applied to calculate the kinetic data for the sake of comparison. This model is as follows:(15)lnCtC0=−kLH⋅t,where kLH is the rate constant of the degradation process (min−1); C0 and Ct are MB initial concentration and concentration at time t (mg·L−1).The values ofkMHL at different initial MB concentrations for both models are listed in Table 4.Table 4
The value ofkMLH and kLH at different initial MB concentration over T0.05-100/Dia-GO.
Concentration (mg·L−1)
Modified Langmuir-Hinshelwood model
Langmuir-Hinshelwood model
kMLH (mg·L−1·min–1)
R2
kLH (min-1)
R2
20
0.121
0.99
0.160
0.98
40
0.180
0.99
0.019
0.97
60
0.242
0.99
0.207
9.96
80
0.310
1
0.235
0.97
100
0.411
1
0.289
0.98The determination coefficients of the straight lines derived from the modified Langmuir-Hinshelwood model are significantly higher than those of the conventional Langmuir-Hinshelwood model, demonstrating that the proposed modified Langmuir-Hinshelwood model fitted better for the experimental data. The comparison of rate constant calculated by the Langmuir-Hinshelwood model of the present catalyst with published literature is listed in Table5. The results show that the photocatalytic activity of TiO2/diazonium/GO was relatively high compared with previous reports.Table 5
Comparison of rate constant of the present catalyst with published literature.
Catalyst
BET-specific surface area (m2·g-1)
Light source (nm, powder)
C0 (mg·L-1)/volume (mL)/mcatalyst (mg)
kLH (min-1)
References
ZnO
8.21
UV, 20 W
10/100/50
0.022
[52]
ZnO/graphene oxide
31.58
UV, 20 W
10/100/50
0.098
[52]
Pristine TiO2 (P25)
—
254, 11 W
10/100/50
0.009
[53]
Graphene-like carbon/TiO2
—
254, 11 W
10/100/50
0.248
[53]
Pristine TiO2 (P25)
51
≤370, 18 W
9.60/100/50
0.050
[54]
Sm-TiO2
46
370, 18 W
9.60/100/50
0.030
[54]
Ce-TiO2
46
370, 18 W
9.60/100/50
0.025
[55]
TiO2
50
340, 125 W
23/2750/375
0.025
[56]
CdS
111.2
>420, 500w
25/200/80
0.008
[56]
g-C3N4
9.8
>420, 500w
25/200/80
0.004
[56]
g-C3N4-CdS
166.5
>420, 500w
25/200/80
0.012
[56]
Ag/ZnO
—
>570, (high pressure sodium lamp)
5/-/150
0.005
[57]
Ta-ZnO
36
>420, 300
10/50/50
0.040
[58]
Eu-TiO2
—
(400-800 nm), 60 W, halogen lamp
3.19/100/100
0.008
[59]
TiO2/diazonium/GO
151.4
75 W - 220 V
20/100/100
0.160
The present work


#### 3.3.1. The Proposed Mechanism of MB Degradation

Figure12 presents the UV-Vis spectra of MB solution at different reaction time.Figure 12
TOC of MB solution in the photocatalytic degradation (V=100mL; C0=100ppm; mcatalyst=100mg; reaction time is 30 min).The MB solution after 30 minutes of photocatalytic oxidation were analyzed by mass spectroscopic LC-MS studies (see FiguresS1, 2, 3, 4, and 5). The finding showed that the intermediates with the retention time of 1.88, 1.90, 1.93, 2.13, and 2.21 have m/z, respectively, 91.00259, 153.06585, 139.05020, 103.07536, and 167.08150. The molecular formulae were HOOC-COOH, CH3-CH2-CH2-CH2-COOH, H2N-C6H4-O-N=O, CH3-HN-C6H4-O-N=O, and (CH3)2N-C6H4-O-N=O (see Schemes S1, 2, 3, 4, and 5). These results indicate that phenothiazine structure and benzene were possibly attacked by the hydroxyl or superoxide radicals which were formed with the presence of photoinduced hole/electron pairs. As the results, they were oxidized and opened the ring to form the intermediates during photocatalytic oxidation. The time dependence of the total organic carbon (TOC) in MB solution during photocatalytic degradation is presented in Figure 12 showing that the TOC value reduced with an increase in irradiation time (13.12 mg·L-1 for initial time and 0.67 mg·L-1 for 600 min. of photocatalytic degradation). TOC reduced to 95% after 600 minutes which implied that almost all MB is mineralized.It is well known that the mechanism of photocatalytic reaction in the intermediate phase involves the formation of free radicals, the photoluminescent electrons, and the clear optical holes [60]. In order to understand the mechanism of the reaction, the effect of some quenchers during the catalyst degradation of MB was investigated. In this work, we used benzoquinone (BQ) as a quenching agent for ⋅O-2, ammonium oxalate (AO) as the optical h+ hole scavenger, tert-Butanol (TB) to quench ⋅OH, and dimethyl sulfoxide (DMSO) to quench electron, e-. The solution was quenched with an initial concentration of quencher of 1 mM, for an initial TB concentration of 10 mM. The results are presented in Figure 13.Figure 13
Photocatalytic degradation of MB by T0.05-100/Dia-GO using quencher AO, BQ, TB, DMSO, and without quencher (WQ) under visible light irradiation for 420 min (condition: concentration of MB,C0=100ppm; V=100mL).The research results showed that the presence of a quencher reduced the optical decomposition efficiency of MB compared to the nonquenching system (WQ). The most obvious effect was DMSO where the degradation efficiency only decreased to 18%, followed by AO with a decrease to 37% and then BQ with a drop in the efficiency to 42%. Meanwhile, TB scavenger did not show significant effect on the degradation efficiency. From the contents discussed above, it can be concluded that the original superoxide anion (⋅O-2), photogenic electrons, e-, and photogenic holes, h+, all contribute to the MB decomposition process. Among the three determinants of the photocatalytic process performance of the study material are photoluminescence and photonic hole, the most important is the presence of photogenic electrons.Proposed mechanism for the degradation of MB under visible light-illumination in the presence of the TiO2/Dia-GO photocatalyst is as follows:
(16)TiO2/Dia−GO+hv⟶Dia/GOe−CB+TiO2h+VBDia/GOe−CB+O2⟶Dia/GO+•O−2⟶Dia/GO+•OHTiO2e−CB+O2⟶TiO2+•O−2⟶TiO2+•OHTiO2h+VB+OH−⟶•OH+TiO2•O−2,•OH,e−CB,h+VB+MB⟶Degradationproducts


#### 3.3.2. Recyclability

The T0.05-100/Dia-GO catalyst was reused for several times. After each run, it was separated by centrifugation, then washed with water and ethanol for three times to remove any dye residual, and finally dried at 120°C for 15 h. The photocatalytic degradation efficiency of T0.05-100/Dia-GO decreased from 100% to 92.72% after three cycles (Figure14(a)). The XRD patterns of the recycled TiO2/Dia-GO samples stayed unaltered; therefore, it can be inferred that TiO2/Dia-GO remained stable during photocatalytic degradation reactions (Figure 14(b)).Figure 14
(a) Photocatalytic degradation efficiency of used catalysts; (b) XRD patterns of T0.05-100/Dia-GO after three cycles of catalysis (V=1000mL, C0=10ppm, mcatalyst=500mg; adsorption time is 120 min; light-illumination time is 120 min).
(a)
(b)In addition, the obtained catalyst manifested excellent photocatalytic degradation of several other dyes, including phenol, methyl orange, and Congo red. As can be seen in Figure15, T0.05-100/Dia-GO composite exhibited superior visible-light-responsive photocatalytic degradation of MB compared with single TiO2 and TiO2/GO.Figure 15
Visible-light-driven photocatalytic degradation of several dyes over TiO2, TiO2/GO and T0.05-100/Dia-GO composite (condition: concentration of dyes=100mg/L; V=100mL; mcatalyst=100mg; illumination time is 300 min).


## 3.1. Characterization of Materials

### 3.1.1. Preparation of Diazonium/GO (Dia-GO)

Figure1 presents XRD patterns of graphite, GO, and Dia-GO. The sharp peak around 26.5° is characteristic of graphite [31] (the inset of Figure 1). The peak at around 11.4° of GO can be attributed to the introduction of oxygen-containing functional groups into the graphite sheets to form of graphene oxide [32]. These functional groups, especially the -SO3H group between the layers of GO, interact strongly with polarizing groups on GO, leading to a shift of a 2θ angle to the smaller value in GO [33, 34], resulting in an increase in dspacing from 7.82 Å for GO to 8.11 Å for Dia-GO (Figures 1(a) and 1(b)). The similar results have been also obtained in the reported papers [34–36] in which GO is chemically functionalized with diazonium of sulfanilic acid.Figure 1
X-ray diffraction patterns for GO (a), Dia-GO (b), and the inset present the XRD pattern of graphite.From Figure2, it can be seen that the GO shows characteristic bands of oxygen-containing functional group vibrations: hydroxyl group (-OH) over the range of 3400-3500 cm-1, C=O vibration (-COOH) at 1636-1700 cm-1, and C-O vibration at 1229 cm-1 and 1060 cm-1 [37–39]. In addition, there are also characteristic peaks for the oscillation of the O=S=O (group -SO3H) bond at 1620-1650 cm-1, 1400 cm-1, and 1100 cm-1 [40–43] in Dia-GO. These results confirmed the formation of diazonium/graphene oxide.Figure 2
FTIR spectra of GO (a), Dia-GO (b).


### 3.1.2. The Preparation of TiO2/Diazonium/GO

The effect of TiCl4 concentration on the phase formation of TiO2 was investigated by XRD studies (Figure 3).Figure 3
XRD patterns of TiO2/Dia-GO samples.It can be seen that the obtained samples all exhibit characteristic diffraction peaks of titanium oxide. As seen in Figure3, the formation of titanium oxide phases (rutile or anatase) depended on titanium chloride concentration. The rutile phase was formed primarily as the titanium chloride concentration was high. T1.35-40/Dia-GO composed of mainly rutile phase with characteristic peaks at 2θ angles of 27.4°, 36.1°, and 41.3° indexed as (110), (101), and (111), respectively (JCPDS: No 21-1276), whereas anatase phase increased with a decrease in titanium chloride concentration. The characteristic peaks with increasing intensity of anatase phase were observed at angles 2θ of 25.5°, 37°, 53.9°, 56.5°, and 62.5° indexed as (101), (004), (200), (105), and (211), respectively (JCPDS: No 21-1272). Primary estimation of catalytic activity for the obtained composite revealed that the use of T0.05-40/Dia-GO led to the highest yield of MB degradation. Therefore, T0.05-40/Dia-GO was selected to further study the effect of ethanol/distilled water ratio on the formation of titanium oxide.The composition of titanium oxide depends not only on titanium chloride concentration but also on the amount of ethanol used in the hydrolysis step. Figure4 shows XRD patterns of T0.05-y/Dia-GO composite materials synthesized at various amounts of ethanol y (y: 20-120 mL of ethanol used).Figure 4
X-ray diffraction patterns for T0.05-y/Dia-GO samples (y=20, 40, 60, 80, 100, and 120 mL ethanol).For T0.05-120/Dia-GO, TiO2 phase existed mainly in anatase form with the characteristic diffraction peaks at 2θ angle of 25.5° with high intensity. The intensity of this characteristic peak decreased with the decrease of ethanol/distilled water ratio. Meanwhile, the intensity of characteristic diffractions at 27.4° and 36.1° for rutile increased significantly with the decrease of the ethanol/distilled ratio. The quantitative analysis of titanium oxide phase showed that when the amount of ethanol increased from 20 mL to 120 mL, the anatase TiO2 phase composition increased from 15.25% to 100%, corresponding to the reduction of rutile phase composition from 84.75% to 0%. Thus, in the samples of synthetic materials, titanium oxide existed in both forms, anatase and rutile.The results of photocatalytic activity of TiO2/Dia-GO nanocomposite are listed in Table 1. It can be seen that photocatalytic activity depended significantly on titania phase composition. Composite with 100% TiO2 in rutile phase exhibited the lowest photocatalytic activity on MB degradation (around 23.4%). The photocatalytic activity increased with an increase in the amount of anatase phase. The MB degradation efficiency peaked at 69.8% as the anatase phase growed to around 73.4% (corresponding to T0.05-100/Dia-GO) before slightly reducing when the amount of anatase phase kept increasing. It is well-known that anatase has lower absorbance ability towards visible light than rutile due to the larger band gap (3.2 eV) than that (3.0 eV) of rutile. However, its indirect band gap provides a longer lifetime of photoinduced electron/hole pairs than direct band gap in rutile because the direct recombination of photoexcited electrons from the conduction band to valence band of anatase TiO2 is impossible [6]. The mixture with an appropriate ratio of anatase and rutile should provide the more superior photocatalytic activity than that of individual rutile or anatase. Then, T0.05-100/Dia-GO was selected for further experiments.Table 1
Phase composition and methylene blue conversion (%) of TiO2/Dia-GO composites (C0,MB=100mg/L, V=100mL, mCat=100mg, and time=120min).
Notation
Phase composition (%)
MB conversion (%)
Anatase
Rutile
T1.35-40/Dia-GO
0
100
23.41
T0.45-40/Dia-GO
0
100
24.84
T0.15-40/Dia-GO
15.25
84.75
45.28
T0.05-40/Dia-GO
40.25
59.75
48.73
T0.05-60/Dia-GO
58.89
41.11
54.23
T0.05-80/Dia-GO
62.19
37.81
57.05
T0.05-100/Dia-GO
73.45
26.55
69.82
T0.05-120/Dia-GO
100
0
63.55The morphologies of T0.05-100/Dia-GO observed by TEM are shown in Figure5. The TiO2 nanoparticles were dispersed highly over the Dia-GO sheet with an average particle size of 5-15 nm (Figure 5(a)). The crystallite size of 11.7 nm obtained by Debye-Scherrer analysis at (101) diffraction is close to the average size of TiO2 particles observed by TEM indicated that the morphology of T0.05-100/Dia-GO consists of single crystals of TiO2 highly dispersed on Dia-GO. Elemental analysis for composite surface showed that T0.05-100/Dia-GO consisted of N, S, and Ti (Figure 5(b)) as an additional evidence of the successful synthesis of the composite of TiO2/diazonium/GO.Figure 5
(a) TEM observation and (b) EDX spectrum of T0.05-100/Dia-GO.
(a)
(b)Based on the band theory of semiconductors, the conduction band (CB) of TiO2 is mainly determined by the Ti 3d orbital energy levels, while the valence band (VB) is mainly formed from the O2p orbitals. As compared to the O2p orbital, other nonmetal elements such as N and S, P possess 2p orbitals locating at more negative energy levels; hence, the partial substitution of the impurity dopants N and S will result in the formation of new energy bands above the TiO2 valence band, thus providing the photocatalytic activity over the visible light region of TiO2 [44].The textural property of the obtained composite was estimated by means of the nitrogen adsorption/desorption isotherms (Figure6). The isotherm curve is the type IV and H3 according to IUPAC classification. The hysteresis loop at the high relative pressure in the range of 0.5 to 0.9 indicated the existence of micromesoposity. The specific surface area of materials based on BET calculation was 152 m2·g-1.Figure 6
The nitrogen adsorption/desorption isotherms of T0.05-100/Dia-GO.DRS-UV-Vis spectra of TiO2/GO (1), Dia-GO (2), and T0.05-100/Dia-GO (3) are presented in Figure 7(a). Bulk TiO2 is considered as an indirect semiconductor [45]. In nanoparticles, the lattice periodicity is lost over a length-scale comparable to the nanoparticle size so the effectiveness of this selection rule breaks down and direct transitions can actually be expected to take place [46, 47]. We used the classical relation near the band-edge optical absorption in a semiconductor to calculate the energy of band-band transition
(3)α=Ahν−Egnhν,where α is the absorption coefficient, Eg is the energy gap, hν is the photon energy, and n is equal to 1/2 for direct transitions and 2 for indirect ones. The Eg value can be calculated from the linear plot of αhν1/n or αhν2vs. hν by extrapolating at zero the linear portion near the band-edge. (Figures 7(b) and 7(c)). Both types of plots exhibit the highly linearity with R2=0.97–0.99 indicating direct or indirect transition that likely occur. The value for types of band gap energy is listed in Table 2. It is obvious that the value of indirect band energy tends to be lower than direct band energy that is similar to some previous reports [45, 46]. It is found that the indirect band gap energy decreased in the order TiO2/GO (2.71 eV) > Dia-GO (2.62 eV) > T0.05-100/Dia-GO (2.35 eV) and these TiO2-based materials exhibit the indirect band gap energy smaller than that of pure TiO2 (3-3.2 eV) [45–47]. The absorption edge shifts towards a visible region due to the possible interaction of between TiO2 and modifiers (N and S). This shift is assigned to the generation of intermediate gap energy levels near the valence band of titania. Consequently, narrowing the band gap energy and minimizing the recombination of photoexited electron/hole pairs are considered for the obtained composite T0.05-100/Dia-GO.Figure 7
(a) DRS-UV-Vis spectra of TiO2/GO (1), Dia-GO (2), and T0.05-100/Dia-GO (3); (b) Tauc’s plots of (αhν)1/2 vs. hν and (c) of (αhν)2 vs. hν for TiO2/GO (1), Dia-GO (2), and T0.05-100/Dia-GO (3).
(a)
(b)
(c)Table 2
Eg values for direct and indirect transitions of the investigated samples.
Sample
Eg (indirect) (eV)
Eg (direct) (eV)
TiO2/GO
2.71
3.15
Dia-GO
2.62
3.12
T0.05-100/Dia-GO
2.35
3.09Raman spectroscopy is a useful approach for the characterization of the physicochemical properties of graphene-based composites. It is known that in Raman spectroscopy, the G band is assigned to the first-order scattering of the sp2 C atoms (∼1600 cm−1), and the D band is attributed to a breathing mode of k-point photons (∼1300 cm−1). At the same time, an increase in ID/IG ratio arises from a lower degree of crystallinity in the graphitic structure. Two bands in the Raman spectra of GO and T0.05-100/Dia-GO located at approximately 1300 and 1600 cm−1 attributed to the D band and G band, respectively (Figure 8(a)). The ID/IG ratio increased from 1.42 for GO to 1.45 for T0.05-100/Dia-GO suggesting a decrease in the size of the in-plane sp2 domains and the partially ordered crystal structure of graphene oxide. These results provided more evidence for the insert of titania and diazonium salt into graphene oxide.Figure 8
(a) Raman spectra of GO and T0.05-100/Dia-GO; (b) photoluminescence (PL) spectra of rutile (1), anatase (2), Dia-GO (3), TiO2-GO (4), and T0.05-100/Dia-GO (5).
(a)
(b)PL spectra of obtained samples are shown in Figure8(b). It can be seen that the luminescent intensity of rutile was the highest, followed by anatase, Dia-GO, and TiO2/GO, and the lowest one belonged to T0.05-100/Dia-GO. It is well known that low PL intensity means low recombination of electron and holes; then, the opposite would be high PL intensity would increase recombination rate and reduce photocatalytic activity. These results demonstrate that the dispersion of TiO2 on graphene reduces the recombination of photonic electrons and photogenic holes, which may increase the photocatalytic activity of the material.Figure9(a) shows the XPS spectrum of T0.05-100/Dia-GO composite, indicating the presence of the four main elements at 162, 284.6, 529.8, and 458.6 eV corresponding to sulfur (S2p), carbon (C1s), oxygen (O1s), and titanium (Ti2p), respectively. Figure 9(b) shows the XPS Ti2p core level. It can be seen that characteristic peaks are at around 457.6 eV for Ti2p3/2 and 463.4 eV for Ti2p1/2, indicating a successful loading of Ti on the surface of GO [5, 48]. Figure 9(c) represents the S2p doublet core peak locating at 160.8-169 eV, associated with a sulfonate type [49]. N1s spectrum is shown in Figure 9(d). The binding energy of around 399.6 eV can be assigned to tertiary amine [50]. The C1s spectrum of GO in Figure 9(e) can be deconvoluted into three peaks at 284.6, 286.7, and 288.5 eV, respectively. Two main peaks at 284.6 and 286.7 eV are usually attributed to adventitious carbon and graphitic carbon from GO, and hydroxyl carbon (C-OH), respectively [51]. The other peak at 288.5 eV can be assigned to carboxyl carbon (O-C=O) [51].Figure 9
XPS spectra of T0.05-100/Dia-GO: (a) survey spectrum; (b) Ti2p; (c) S2p; (d) N1s; (e) C1s.
(a)
(b)
(c)
(d)
(e)


## 3.1.1. Preparation of Diazonium/GO (Dia-GO)

Figure1 presents XRD patterns of graphite, GO, and Dia-GO. The sharp peak around 26.5° is characteristic of graphite [31] (the inset of Figure 1). The peak at around 11.4° of GO can be attributed to the introduction of oxygen-containing functional groups into the graphite sheets to form of graphene oxide [32]. These functional groups, especially the -SO3H group between the layers of GO, interact strongly with polarizing groups on GO, leading to a shift of a 2θ angle to the smaller value in GO [33, 34], resulting in an increase in dspacing from 7.82 Å for GO to 8.11 Å for Dia-GO (Figures 1(a) and 1(b)). The similar results have been also obtained in the reported papers [34–36] in which GO is chemically functionalized with diazonium of sulfanilic acid.Figure 1
X-ray diffraction patterns for GO (a), Dia-GO (b), and the inset present the XRD pattern of graphite.From Figure2, it can be seen that the GO shows characteristic bands of oxygen-containing functional group vibrations: hydroxyl group (-OH) over the range of 3400-3500 cm-1, C=O vibration (-COOH) at 1636-1700 cm-1, and C-O vibration at 1229 cm-1 and 1060 cm-1 [37–39]. In addition, there are also characteristic peaks for the oscillation of the O=S=O (group -SO3H) bond at 1620-1650 cm-1, 1400 cm-1, and 1100 cm-1 [40–43] in Dia-GO. These results confirmed the formation of diazonium/graphene oxide.Figure 2
FTIR spectra of GO (a), Dia-GO (b).


## 3.1.2. The Preparation of TiO2/Diazonium/GO

The effect of TiCl4 concentration on the phase formation of TiO2 was investigated by XRD studies (Figure 3).Figure 3
XRD patterns of TiO2/Dia-GO samples.It can be seen that the obtained samples all exhibit characteristic diffraction peaks of titanium oxide. As seen in Figure3, the formation of titanium oxide phases (rutile or anatase) depended on titanium chloride concentration. The rutile phase was formed primarily as the titanium chloride concentration was high. T1.35-40/Dia-GO composed of mainly rutile phase with characteristic peaks at 2θ angles of 27.4°, 36.1°, and 41.3° indexed as (110), (101), and (111), respectively (JCPDS: No 21-1276), whereas anatase phase increased with a decrease in titanium chloride concentration. The characteristic peaks with increasing intensity of anatase phase were observed at angles 2θ of 25.5°, 37°, 53.9°, 56.5°, and 62.5° indexed as (101), (004), (200), (105), and (211), respectively (JCPDS: No 21-1272). Primary estimation of catalytic activity for the obtained composite revealed that the use of T0.05-40/Dia-GO led to the highest yield of MB degradation. Therefore, T0.05-40/Dia-GO was selected to further study the effect of ethanol/distilled water ratio on the formation of titanium oxide.The composition of titanium oxide depends not only on titanium chloride concentration but also on the amount of ethanol used in the hydrolysis step. Figure4 shows XRD patterns of T0.05-y/Dia-GO composite materials synthesized at various amounts of ethanol y (y: 20-120 mL of ethanol used).Figure 4
X-ray diffraction patterns for T0.05-y/Dia-GO samples (y=20, 40, 60, 80, 100, and 120 mL ethanol).For T0.05-120/Dia-GO, TiO2 phase existed mainly in anatase form with the characteristic diffraction peaks at 2θ angle of 25.5° with high intensity. The intensity of this characteristic peak decreased with the decrease of ethanol/distilled water ratio. Meanwhile, the intensity of characteristic diffractions at 27.4° and 36.1° for rutile increased significantly with the decrease of the ethanol/distilled ratio. The quantitative analysis of titanium oxide phase showed that when the amount of ethanol increased from 20 mL to 120 mL, the anatase TiO2 phase composition increased from 15.25% to 100%, corresponding to the reduction of rutile phase composition from 84.75% to 0%. Thus, in the samples of synthetic materials, titanium oxide existed in both forms, anatase and rutile.The results of photocatalytic activity of TiO2/Dia-GO nanocomposite are listed in Table 1. It can be seen that photocatalytic activity depended significantly on titania phase composition. Composite with 100% TiO2 in rutile phase exhibited the lowest photocatalytic activity on MB degradation (around 23.4%). The photocatalytic activity increased with an increase in the amount of anatase phase. The MB degradation efficiency peaked at 69.8% as the anatase phase growed to around 73.4% (corresponding to T0.05-100/Dia-GO) before slightly reducing when the amount of anatase phase kept increasing. It is well-known that anatase has lower absorbance ability towards visible light than rutile due to the larger band gap (3.2 eV) than that (3.0 eV) of rutile. However, its indirect band gap provides a longer lifetime of photoinduced electron/hole pairs than direct band gap in rutile because the direct recombination of photoexcited electrons from the conduction band to valence band of anatase TiO2 is impossible [6]. The mixture with an appropriate ratio of anatase and rutile should provide the more superior photocatalytic activity than that of individual rutile or anatase. Then, T0.05-100/Dia-GO was selected for further experiments.Table 1
Phase composition and methylene blue conversion (%) of TiO2/Dia-GO composites (C0,MB=100mg/L, V=100mL, mCat=100mg, and time=120min).
Notation
Phase composition (%)
MB conversion (%)
Anatase
Rutile
T1.35-40/Dia-GO
0
100
23.41
T0.45-40/Dia-GO
0
100
24.84
T0.15-40/Dia-GO
15.25
84.75
45.28
T0.05-40/Dia-GO
40.25
59.75
48.73
T0.05-60/Dia-GO
58.89
41.11
54.23
T0.05-80/Dia-GO
62.19
37.81
57.05
T0.05-100/Dia-GO
73.45
26.55
69.82
T0.05-120/Dia-GO
100
0
63.55The morphologies of T0.05-100/Dia-GO observed by TEM are shown in Figure5. The TiO2 nanoparticles were dispersed highly over the Dia-GO sheet with an average particle size of 5-15 nm (Figure 5(a)). The crystallite size of 11.7 nm obtained by Debye-Scherrer analysis at (101) diffraction is close to the average size of TiO2 particles observed by TEM indicated that the morphology of T0.05-100/Dia-GO consists of single crystals of TiO2 highly dispersed on Dia-GO. Elemental analysis for composite surface showed that T0.05-100/Dia-GO consisted of N, S, and Ti (Figure 5(b)) as an additional evidence of the successful synthesis of the composite of TiO2/diazonium/GO.Figure 5
(a) TEM observation and (b) EDX spectrum of T0.05-100/Dia-GO.
(a)
(b)Based on the band theory of semiconductors, the conduction band (CB) of TiO2 is mainly determined by the Ti 3d orbital energy levels, while the valence band (VB) is mainly formed from the O2p orbitals. As compared to the O2p orbital, other nonmetal elements such as N and S, P possess 2p orbitals locating at more negative energy levels; hence, the partial substitution of the impurity dopants N and S will result in the formation of new energy bands above the TiO2 valence band, thus providing the photocatalytic activity over the visible light region of TiO2 [44].The textural property of the obtained composite was estimated by means of the nitrogen adsorption/desorption isotherms (Figure6). The isotherm curve is the type IV and H3 according to IUPAC classification. The hysteresis loop at the high relative pressure in the range of 0.5 to 0.9 indicated the existence of micromesoposity. The specific surface area of materials based on BET calculation was 152 m2·g-1.Figure 6
The nitrogen adsorption/desorption isotherms of T0.05-100/Dia-GO.DRS-UV-Vis spectra of TiO2/GO (1), Dia-GO (2), and T0.05-100/Dia-GO (3) are presented in Figure 7(a). Bulk TiO2 is considered as an indirect semiconductor [45]. In nanoparticles, the lattice periodicity is lost over a length-scale comparable to the nanoparticle size so the effectiveness of this selection rule breaks down and direct transitions can actually be expected to take place [46, 47]. We used the classical relation near the band-edge optical absorption in a semiconductor to calculate the energy of band-band transition
(3)α=Ahν−Egnhν,where α is the absorption coefficient, Eg is the energy gap, hν is the photon energy, and n is equal to 1/2 for direct transitions and 2 for indirect ones. The Eg value can be calculated from the linear plot of αhν1/n or αhν2vs. hν by extrapolating at zero the linear portion near the band-edge. (Figures 7(b) and 7(c)). Both types of plots exhibit the highly linearity with R2=0.97–0.99 indicating direct or indirect transition that likely occur. The value for types of band gap energy is listed in Table 2. It is obvious that the value of indirect band energy tends to be lower than direct band energy that is similar to some previous reports [45, 46]. It is found that the indirect band gap energy decreased in the order TiO2/GO (2.71 eV) > Dia-GO (2.62 eV) > T0.05-100/Dia-GO (2.35 eV) and these TiO2-based materials exhibit the indirect band gap energy smaller than that of pure TiO2 (3-3.2 eV) [45–47]. The absorption edge shifts towards a visible region due to the possible interaction of between TiO2 and modifiers (N and S). This shift is assigned to the generation of intermediate gap energy levels near the valence band of titania. Consequently, narrowing the band gap energy and minimizing the recombination of photoexited electron/hole pairs are considered for the obtained composite T0.05-100/Dia-GO.Figure 7
(a) DRS-UV-Vis spectra of TiO2/GO (1), Dia-GO (2), and T0.05-100/Dia-GO (3); (b) Tauc’s plots of (αhν)1/2 vs. hν and (c) of (αhν)2 vs. hν for TiO2/GO (1), Dia-GO (2), and T0.05-100/Dia-GO (3).
(a)
(b)
(c)Table 2
Eg values for direct and indirect transitions of the investigated samples.
Sample
Eg (indirect) (eV)
Eg (direct) (eV)
TiO2/GO
2.71
3.15
Dia-GO
2.62
3.12
T0.05-100/Dia-GO
2.35
3.09Raman spectroscopy is a useful approach for the characterization of the physicochemical properties of graphene-based composites. It is known that in Raman spectroscopy, the G band is assigned to the first-order scattering of the sp2 C atoms (∼1600 cm−1), and the D band is attributed to a breathing mode of k-point photons (∼1300 cm−1). At the same time, an increase in ID/IG ratio arises from a lower degree of crystallinity in the graphitic structure. Two bands in the Raman spectra of GO and T0.05-100/Dia-GO located at approximately 1300 and 1600 cm−1 attributed to the D band and G band, respectively (Figure 8(a)). The ID/IG ratio increased from 1.42 for GO to 1.45 for T0.05-100/Dia-GO suggesting a decrease in the size of the in-plane sp2 domains and the partially ordered crystal structure of graphene oxide. These results provided more evidence for the insert of titania and diazonium salt into graphene oxide.Figure 8
(a) Raman spectra of GO and T0.05-100/Dia-GO; (b) photoluminescence (PL) spectra of rutile (1), anatase (2), Dia-GO (3), TiO2-GO (4), and T0.05-100/Dia-GO (5).
(a)
(b)PL spectra of obtained samples are shown in Figure8(b). It can be seen that the luminescent intensity of rutile was the highest, followed by anatase, Dia-GO, and TiO2/GO, and the lowest one belonged to T0.05-100/Dia-GO. It is well known that low PL intensity means low recombination of electron and holes; then, the opposite would be high PL intensity would increase recombination rate and reduce photocatalytic activity. These results demonstrate that the dispersion of TiO2 on graphene reduces the recombination of photonic electrons and photogenic holes, which may increase the photocatalytic activity of the material.Figure9(a) shows the XPS spectrum of T0.05-100/Dia-GO composite, indicating the presence of the four main elements at 162, 284.6, 529.8, and 458.6 eV corresponding to sulfur (S2p), carbon (C1s), oxygen (O1s), and titanium (Ti2p), respectively. Figure 9(b) shows the XPS Ti2p core level. It can be seen that characteristic peaks are at around 457.6 eV for Ti2p3/2 and 463.4 eV for Ti2p1/2, indicating a successful loading of Ti on the surface of GO [5, 48]. Figure 9(c) represents the S2p doublet core peak locating at 160.8-169 eV, associated with a sulfonate type [49]. N1s spectrum is shown in Figure 9(d). The binding energy of around 399.6 eV can be assigned to tertiary amine [50]. The C1s spectrum of GO in Figure 9(e) can be deconvoluted into three peaks at 284.6, 286.7, and 288.5 eV, respectively. Two main peaks at 284.6 and 286.7 eV are usually attributed to adventitious carbon and graphitic carbon from GO, and hydroxyl carbon (C-OH), respectively [51]. The other peak at 288.5 eV can be assigned to carboxyl carbon (O-C=O) [51].Figure 9
XPS spectra of T0.05-100/Dia-GO: (a) survey spectrum; (b) Ti2p; (c) S2p; (d) N1s; (e) C1s.
(a)
(b)
(c)
(d)
(e)


## 3.2. Photocatalytic Performance of TiO2/Diazonium/GO Composites for MB Degradation in a Visible-Light Region

### 3.2.1. Leaching Experiment

The kinetics of decolorization of MB in several conditions are shown in Figure10. It was found that the decolorization of MB was not observed if visible light was irradiated in the absence of T0.05-100/Dia-GO suggesting that MB was stable and did not undergo photolysis. A leaching experiment was also conducted in which the T0.05-100/Dia-GO was filtered by centrifugation after 60 min. of irradiation. The MB decolorization was quenched even when the light was still irradiated. This indicates that there was no leaching of the active species into the reaction solution from the heterogeneous catalyst. The above experimental results confirmed that T0.05-100/Dia-GO acted as a heterogeneous catalyst in the degradation reaction of MB.Figure 10
Leaching experiment (V=500mL, C0=100mg·L−1; mass of catalyst: 100 mg).Figure11(a) presents the adsorption kinetics and photocatalytic decolorization of MB on TiO2/Dia-GO catalyst. This catalyst presented a low adsorption capacity of MB. The adsorption was saturated from 100 min to 120 min depending on the initial MB concentration. In this study, the light illumination was carried out only when the dark adsorption reached adsorption/desorption equilibrium.Figure 11
(a) The adsorption and photodegradation kinetics of MB on T0.05-100/Dia-GO catalyst; (b) the plots of the1/KlnC+C against t different initial MB concentration.
(a)
(b)


### 3.2.2. Adsorption Isotherm

The equilibrium adsorption capacity,qe, can be expressed as follows:
(4)qe=V⋅C0−Cem,where C0 and Ce are the MB concentration at initial and equilibrium time (mg·L-1); V is the volume of the MB solution (L); m is the mass of catalyst (g).The relationship betweenCe and qe is expressed by the Langmuir isotherm model as equation (5) and the Freundlich model as equation (6):
(5)qe=ΚL⋅qm⋅Ce1+KL⋅Ce,(6)qe=KF⋅Ce1/n,where qm is the maximum monolayer adsorption capacity (mg·L-1); KL is the Langmuir adsorption equilibrium constant (mg-1·L); KF and n are Freundlich parameters.The calculated parameters can be obtained from nonlinear regression of equations (5) and (6) and are listed in Table 3. A high determination coefficient (R2=0.99) for Langmuir model and Freundlich model indicated that the equilibrium data was well fitted in both models. It implies a monolayer adsorption and the existence of heterogeneous surface in the adsorbents.Table 3
The parameters of Langmuir and Freundlich model.
Langmuir model
Freundlich model
KL (L·mg-1)
qm (mg·g-1)
R2
KF
N
R2
3.2.10-2
138.12
0.99
5.837
1.35
0.99


## 3.2.1. Leaching Experiment

The kinetics of decolorization of MB in several conditions are shown in Figure10. It was found that the decolorization of MB was not observed if visible light was irradiated in the absence of T0.05-100/Dia-GO suggesting that MB was stable and did not undergo photolysis. A leaching experiment was also conducted in which the T0.05-100/Dia-GO was filtered by centrifugation after 60 min. of irradiation. The MB decolorization was quenched even when the light was still irradiated. This indicates that there was no leaching of the active species into the reaction solution from the heterogeneous catalyst. The above experimental results confirmed that T0.05-100/Dia-GO acted as a heterogeneous catalyst in the degradation reaction of MB.Figure 10
Leaching experiment (V=500mL, C0=100mg·L−1; mass of catalyst: 100 mg).Figure11(a) presents the adsorption kinetics and photocatalytic decolorization of MB on TiO2/Dia-GO catalyst. This catalyst presented a low adsorption capacity of MB. The adsorption was saturated from 100 min to 120 min depending on the initial MB concentration. In this study, the light illumination was carried out only when the dark adsorption reached adsorption/desorption equilibrium.Figure 11
(a) The adsorption and photodegradation kinetics of MB on T0.05-100/Dia-GO catalyst; (b) the plots of the1/KlnC+C against t different initial MB concentration.
(a)
(b)


## 3.2.2. Adsorption Isotherm

The equilibrium adsorption capacity,qe, can be expressed as follows:
(4)qe=V⋅C0−Cem,where C0 and Ce are the MB concentration at initial and equilibrium time (mg·L-1); V is the volume of the MB solution (L); m is the mass of catalyst (g).The relationship betweenCe and qe is expressed by the Langmuir isotherm model as equation (5) and the Freundlich model as equation (6):
(5)qe=ΚL⋅qm⋅Ce1+KL⋅Ce,(6)qe=KF⋅Ce1/n,where qm is the maximum monolayer adsorption capacity (mg·L-1); KL is the Langmuir adsorption equilibrium constant (mg-1·L); KF and n are Freundlich parameters.The calculated parameters can be obtained from nonlinear regression of equations (5) and (6) and are listed in Table 3. A high determination coefficient (R2=0.99) for Langmuir model and Freundlich model indicated that the equilibrium data was well fitted in both models. It implies a monolayer adsorption and the existence of heterogeneous surface in the adsorbents.Table 3
The parameters of Langmuir and Freundlich model.
Langmuir model
Freundlich model
KL (L·mg-1)
qm (mg·g-1)
R2
KF
N
R2
3.2.10-2
138.12
0.99
5.837
1.35
0.99


## 3.3. Decomposition Kinetics

Based on the Langmuir-Hinshelwood model, the overall reaction could be illustrated as follows:(7)T0.05−100/GO−Dia+MB⇄k−1k1T0.05−100/GO−Dia⋯MB∗→k2degradationproductswhere k1 and k–1 are the forward/back adsorption rate constant, respectively; k2 is the kinetic rate coefficient of the degradation process.The law rate is expressed as follows:(8)r=−dCdt=kMLH⋅θ,where C is the dye concentration (mg·L−1) at time t; kMLH is the kinetic rate coefficient (mg·L−1·min−1); θ is the fraction of the surface covered by MB. θ is expressed in the Langmuir model as [37]
(9)θ=ΚL⋅C1+KL⋅C.Substituting (8) to (6) gives
(10)dCdt=−kMLH⋅KL⋅C1+KL⋅C.Then,(11)∫1+KL⋅CKL⋅C⋅dC=−∫kMLH⋅dt.Integrating equation (11) with the boundary conditions t⟶0 and C⟶C0e gives
(12)1KL⋅lnC+C=−kMLH⋅t+I0,when t=0, then
(13)I0=1KL⋅lnC0e+C0e.Substituting (13) into (12) gives
(14)1KL⋅lnC+C=−kMLH⋅t+1KL⋅lnC0e+C0e,where C0e (mg·L−1) is the equilibrium concentration of adsorbate at time t (min) taken from light illumination.The plot of the (1/KlnC+C) against t gives a straight line with slope kMLH (Figure 11(b)).For the kinetics of unimolecular reaction on heterogeneous catalyst the Langmuir-Hinshelwood model is widely used. In this study, the Langmuir-Hinshelwood was also applied to calculate the kinetic data for the sake of comparison. This model is as follows:(15)lnCtC0=−kLH⋅t,where kLH is the rate constant of the degradation process (min−1); C0 and Ct are MB initial concentration and concentration at time t (mg·L−1).The values ofkMHL at different initial MB concentrations for both models are listed in Table 4.Table 4
The value ofkMLH and kLH at different initial MB concentration over T0.05-100/Dia-GO.
Concentration (mg·L−1)
Modified Langmuir-Hinshelwood model
Langmuir-Hinshelwood model
kMLH (mg·L−1·min–1)
R2
kLH (min-1)
R2
20
0.121
0.99
0.160
0.98
40
0.180
0.99
0.019
0.97
60
0.242
0.99
0.207
9.96
80
0.310
1
0.235
0.97
100
0.411
1
0.289
0.98The determination coefficients of the straight lines derived from the modified Langmuir-Hinshelwood model are significantly higher than those of the conventional Langmuir-Hinshelwood model, demonstrating that the proposed modified Langmuir-Hinshelwood model fitted better for the experimental data. The comparison of rate constant calculated by the Langmuir-Hinshelwood model of the present catalyst with published literature is listed in Table5. The results show that the photocatalytic activity of TiO2/diazonium/GO was relatively high compared with previous reports.Table 5
Comparison of rate constant of the present catalyst with published literature.
Catalyst
BET-specific surface area (m2·g-1)
Light source (nm, powder)
C0 (mg·L-1)/volume (mL)/mcatalyst (mg)
kLH (min-1)
References
ZnO
8.21
UV, 20 W
10/100/50
0.022
[52]
ZnO/graphene oxide
31.58
UV, 20 W
10/100/50
0.098
[52]
Pristine TiO2 (P25)
—
254, 11 W
10/100/50
0.009
[53]
Graphene-like carbon/TiO2
—
254, 11 W
10/100/50
0.248
[53]
Pristine TiO2 (P25)
51
≤370, 18 W
9.60/100/50
0.050
[54]
Sm-TiO2
46
370, 18 W
9.60/100/50
0.030
[54]
Ce-TiO2
46
370, 18 W
9.60/100/50
0.025
[55]
TiO2
50
340, 125 W
23/2750/375
0.025
[56]
CdS
111.2
>420, 500w
25/200/80
0.008
[56]
g-C3N4
9.8
>420, 500w
25/200/80
0.004
[56]
g-C3N4-CdS
166.5
>420, 500w
25/200/80
0.012
[56]
Ag/ZnO
—
>570, (high pressure sodium lamp)
5/-/150
0.005
[57]
Ta-ZnO
36
>420, 300
10/50/50
0.040
[58]
Eu-TiO2
—
(400-800 nm), 60 W, halogen lamp
3.19/100/100
0.008
[59]
TiO2/diazonium/GO
151.4
75 W - 220 V
20/100/100
0.160
The present work


### 3.3.1. The Proposed Mechanism of MB Degradation

Figure12 presents the UV-Vis spectra of MB solution at different reaction time.Figure 12
TOC of MB solution in the photocatalytic degradation (V=100mL; C0=100ppm; mcatalyst=100mg; reaction time is 30 min).The MB solution after 30 minutes of photocatalytic oxidation were analyzed by mass spectroscopic LC-MS studies (see FiguresS1, 2, 3, 4, and 5). The finding showed that the intermediates with the retention time of 1.88, 1.90, 1.93, 2.13, and 2.21 have m/z, respectively, 91.00259, 153.06585, 139.05020, 103.07536, and 167.08150. The molecular formulae were HOOC-COOH, CH3-CH2-CH2-CH2-COOH, H2N-C6H4-O-N=O, CH3-HN-C6H4-O-N=O, and (CH3)2N-C6H4-O-N=O (see Schemes S1, 2, 3, 4, and 5). These results indicate that phenothiazine structure and benzene were possibly attacked by the hydroxyl or superoxide radicals which were formed with the presence of photoinduced hole/electron pairs. As the results, they were oxidized and opened the ring to form the intermediates during photocatalytic oxidation. The time dependence of the total organic carbon (TOC) in MB solution during photocatalytic degradation is presented in Figure 12 showing that the TOC value reduced with an increase in irradiation time (13.12 mg·L-1 for initial time and 0.67 mg·L-1 for 600 min. of photocatalytic degradation). TOC reduced to 95% after 600 minutes which implied that almost all MB is mineralized.It is well known that the mechanism of photocatalytic reaction in the intermediate phase involves the formation of free radicals, the photoluminescent electrons, and the clear optical holes [60]. In order to understand the mechanism of the reaction, the effect of some quenchers during the catalyst degradation of MB was investigated. In this work, we used benzoquinone (BQ) as a quenching agent for ⋅O-2, ammonium oxalate (AO) as the optical h+ hole scavenger, tert-Butanol (TB) to quench ⋅OH, and dimethyl sulfoxide (DMSO) to quench electron, e-. The solution was quenched with an initial concentration of quencher of 1 mM, for an initial TB concentration of 10 mM. The results are presented in Figure 13.Figure 13
Photocatalytic degradation of MB by T0.05-100/Dia-GO using quencher AO, BQ, TB, DMSO, and without quencher (WQ) under visible light irradiation for 420 min (condition: concentration of MB,C0=100ppm; V=100mL).The research results showed that the presence of a quencher reduced the optical decomposition efficiency of MB compared to the nonquenching system (WQ). The most obvious effect was DMSO where the degradation efficiency only decreased to 18%, followed by AO with a decrease to 37% and then BQ with a drop in the efficiency to 42%. Meanwhile, TB scavenger did not show significant effect on the degradation efficiency. From the contents discussed above, it can be concluded that the original superoxide anion (⋅O-2), photogenic electrons, e-, and photogenic holes, h+, all contribute to the MB decomposition process. Among the three determinants of the photocatalytic process performance of the study material are photoluminescence and photonic hole, the most important is the presence of photogenic electrons.Proposed mechanism for the degradation of MB under visible light-illumination in the presence of the TiO2/Dia-GO photocatalyst is as follows:
(16)TiO2/Dia−GO+hv⟶Dia/GOe−CB+TiO2h+VBDia/GOe−CB+O2⟶Dia/GO+•O−2⟶Dia/GO+•OHTiO2e−CB+O2⟶TiO2+•O−2⟶TiO2+•OHTiO2h+VB+OH−⟶•OH+TiO2•O−2,•OH,e−CB,h+VB+MB⟶Degradationproducts


### 3.3.2. Recyclability

The T0.05-100/Dia-GO catalyst was reused for several times. After each run, it was separated by centrifugation, then washed with water and ethanol for three times to remove any dye residual, and finally dried at 120°C for 15 h. The photocatalytic degradation efficiency of T0.05-100/Dia-GO decreased from 100% to 92.72% after three cycles (Figure14(a)). The XRD patterns of the recycled TiO2/Dia-GO samples stayed unaltered; therefore, it can be inferred that TiO2/Dia-GO remained stable during photocatalytic degradation reactions (Figure 14(b)).Figure 14
(a) Photocatalytic degradation efficiency of used catalysts; (b) XRD patterns of T0.05-100/Dia-GO after three cycles of catalysis (V=1000mL, C0=10ppm, mcatalyst=500mg; adsorption time is 120 min; light-illumination time is 120 min).
(a)
(b)In addition, the obtained catalyst manifested excellent photocatalytic degradation of several other dyes, including phenol, methyl orange, and Congo red. As can be seen in Figure15, T0.05-100/Dia-GO composite exhibited superior visible-light-responsive photocatalytic degradation of MB compared with single TiO2 and TiO2/GO.Figure 15
Visible-light-driven photocatalytic degradation of several dyes over TiO2, TiO2/GO and T0.05-100/Dia-GO composite (condition: concentration of dyes=100mg/L; V=100mL; mcatalyst=100mg; illumination time is 300 min).


## 3.3.1. The Proposed Mechanism of MB Degradation

Figure12 presents the UV-Vis spectra of MB solution at different reaction time.Figure 12
TOC of MB solution in the photocatalytic degradation (V=100mL; C0=100ppm; mcatalyst=100mg; reaction time is 30 min).The MB solution after 30 minutes of photocatalytic oxidation were analyzed by mass spectroscopic LC-MS studies (see FiguresS1, 2, 3, 4, and 5). The finding showed that the intermediates with the retention time of 1.88, 1.90, 1.93, 2.13, and 2.21 have m/z, respectively, 91.00259, 153.06585, 139.05020, 103.07536, and 167.08150. The molecular formulae were HOOC-COOH, CH3-CH2-CH2-CH2-COOH, H2N-C6H4-O-N=O, CH3-HN-C6H4-O-N=O, and (CH3)2N-C6H4-O-N=O (see Schemes S1, 2, 3, 4, and 5). These results indicate that phenothiazine structure and benzene were possibly attacked by the hydroxyl or superoxide radicals which were formed with the presence of photoinduced hole/electron pairs. As the results, they were oxidized and opened the ring to form the intermediates during photocatalytic oxidation. The time dependence of the total organic carbon (TOC) in MB solution during photocatalytic degradation is presented in Figure 12 showing that the TOC value reduced with an increase in irradiation time (13.12 mg·L-1 for initial time and 0.67 mg·L-1 for 600 min. of photocatalytic degradation). TOC reduced to 95% after 600 minutes which implied that almost all MB is mineralized.It is well known that the mechanism of photocatalytic reaction in the intermediate phase involves the formation of free radicals, the photoluminescent electrons, and the clear optical holes [60]. In order to understand the mechanism of the reaction, the effect of some quenchers during the catalyst degradation of MB was investigated. In this work, we used benzoquinone (BQ) as a quenching agent for ⋅O-2, ammonium oxalate (AO) as the optical h+ hole scavenger, tert-Butanol (TB) to quench ⋅OH, and dimethyl sulfoxide (DMSO) to quench electron, e-. The solution was quenched with an initial concentration of quencher of 1 mM, for an initial TB concentration of 10 mM. The results are presented in Figure 13.Figure 13
Photocatalytic degradation of MB by T0.05-100/Dia-GO using quencher AO, BQ, TB, DMSO, and without quencher (WQ) under visible light irradiation for 420 min (condition: concentration of MB,C0=100ppm; V=100mL).The research results showed that the presence of a quencher reduced the optical decomposition efficiency of MB compared to the nonquenching system (WQ). The most obvious effect was DMSO where the degradation efficiency only decreased to 18%, followed by AO with a decrease to 37% and then BQ with a drop in the efficiency to 42%. Meanwhile, TB scavenger did not show significant effect on the degradation efficiency. From the contents discussed above, it can be concluded that the original superoxide anion (⋅O-2), photogenic electrons, e-, and photogenic holes, h+, all contribute to the MB decomposition process. Among the three determinants of the photocatalytic process performance of the study material are photoluminescence and photonic hole, the most important is the presence of photogenic electrons.Proposed mechanism for the degradation of MB under visible light-illumination in the presence of the TiO2/Dia-GO photocatalyst is as follows:
(16)TiO2/Dia−GO+hv⟶Dia/GOe−CB+TiO2h+VBDia/GOe−CB+O2⟶Dia/GO+•O−2⟶Dia/GO+•OHTiO2e−CB+O2⟶TiO2+•O−2⟶TiO2+•OHTiO2h+VB+OH−⟶•OH+TiO2•O−2,•OH,e−CB,h+VB+MB⟶Degradationproducts


## 3.3.2. Recyclability

The T0.05-100/Dia-GO catalyst was reused for several times. After each run, it was separated by centrifugation, then washed with water and ethanol for three times to remove any dye residual, and finally dried at 120°C for 15 h. The photocatalytic degradation efficiency of T0.05-100/Dia-GO decreased from 100% to 92.72% after three cycles (Figure14(a)). The XRD patterns of the recycled TiO2/Dia-GO samples stayed unaltered; therefore, it can be inferred that TiO2/Dia-GO remained stable during photocatalytic degradation reactions (Figure 14(b)).Figure 14
(a) Photocatalytic degradation efficiency of used catalysts; (b) XRD patterns of T0.05-100/Dia-GO after three cycles of catalysis (V=1000mL, C0=10ppm, mcatalyst=500mg; adsorption time is 120 min; light-illumination time is 120 min).
(a)
(b)In addition, the obtained catalyst manifested excellent photocatalytic degradation of several other dyes, including phenol, methyl orange, and Congo red. As can be seen in Figure15, T0.05-100/Dia-GO composite exhibited superior visible-light-responsive photocatalytic degradation of MB compared with single TiO2 and TiO2/GO.Figure 15
Visible-light-driven photocatalytic degradation of several dyes over TiO2, TiO2/GO and T0.05-100/Dia-GO composite (condition: concentration of dyes=100mg/L; V=100mL; mcatalyst=100mg; illumination time is 300 min).


## 4. Conclusion

The synthesis of TiO2/diazonium/GO and an application to MB photocatalytic degradation in a visible region have been studied. Rutile or anatase phase in TiO2/diazonium/GO composites can be controlled by adjusting the amount of TiCl4 in the reaction mixture or ethanol/water ratio for hydrolysis. TiO2/diazonium/GO with ac. 70% anatase in titania phase provided the highest MB degradation efficiency. The photocatalytic oxidation exhibited a complete decomposition of MB by the cleavage and oxidation of one or more of the methyl substituents on the amine groups. We have proposed a kinetic model by the combination of classical Langmuir-Hinshelwood kinetic model and Langmuir isotherm model. The experimental data fit well the proposed model. In addition, TiO2/diazonium/GO composite can catalyze for photodegradation of several dyes such as phenol, Congo red, and methyl red. The present catalyst with its stability and recyclable advantages is promising for application in the treatment of dye wastes.



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