# Preparation of Titanium Dioxide Nanoparticles Immobilized on Polyacrylonitrile Nanofibres for the Photodegradation of Methyl Orange

Authors: Pardon Nyamukamba; Omobola Okoh; Lilian Tichagwa; Corinne Greyling
Journal: International Journal of Photoenergy
 (2016)

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## Abstract

Herein, we describe the synthesis of titanium dioxide (TiO2) nanoparticles by the hydrolysis and condensation of titanium tetrachloride. The resulting nanoparticles were immobilized on polyacrylonitrile (PAN) based nanofibres by an electrospinning technique in order to allow simple isolation and reuse of titania semiconductor photocatalyst. The composite nanofibres were heat treated to convert the polymer nanofibres to carbon nanofibres and to convert amorphous TiO2 to crystalline TiO2. X-ray diffraction (XRD) analysis showed that the rutile phase was the major phase and the equatorial peaks of PAN disappeared after heat treatment at 600°C. Transmission electron microscopy (TEM) and scanning electron microscopy (SEM) analysis confirmed that some TiO2 nanoparticles were encapsulated whereas some were surface residing on the electrospun nanofibres. The TiO2 nanoparticles were found to lower the cyclization temperature of PAN as indicated by differential scanning colorimetry (DSC) and differential thermal analysis (DTA). Photocatalytic studies on the degradation of methyl orange dye under UV light irradiation showed that composite nanofibres were capable of degrading organic contaminants in water. The carbon nanofibres with surface residing titanium dioxide nanoparticles (TiO2/CNF-SR) showed the highest photocatalytic activity (59.35% after 210 minutes) due to direct contact between the TiO2 photocatalyst and methyl orange.


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## Body

## 1. Introduction

The pollution of water by dangerous industrial organic chemicals is a serious problem as it poses a health risk to humans and the environment. These organic contaminants need to be removed if the water is to be used in homes for human consumption. If these organics are not removed, they will react with chlorine during water treatment by chlorination forming by-products such as trihalomethanes, which increase the risk of cancer [1]. Conventional water treatment methods such as adsorption have a disadvantage of producing secondary pollutants that require disposal since it involves accumulation of pollutants on the surface. These disadvantages have prompted research interest into the development of new water treatment methods such as photocatalysis which makes use of a semiconductor photocatalyst that can oxidize organic compounds to harmless products such as water and carbon dioxide [2]. Photocatalysis started in 1972 when Fujishima and Honda discovered the photocatalytic splitting of water using titanium electrodes [3]. The interest in using TiO2 as a heterogeneous catalyst for wastewater and ground water remediation has increased tremendously [4, 5] because it is capable of degrading several organic and inorganic pollutants [6].TiO2 photocatalyst is ideal because it is photostable, relatively cheap, readily available, nontoxic and its photogenerated holes and electrons are highly oxidizing and reducing, respectively [7]. Several methods have been used for the synthesis of titania and these include gas phase pyrolysis [8], low temperature dissolution-reprecipitation process [9], sol-gel [10, 11], combustion synthesis [12], and ultrasonic spray pyrolysis [13]. In this study TiO2 photocatalyst was prepared using a simple sol-gel process.From a practical point of view, the use of a suspension of powdered TiO2 is very difficult due to filtration problems associated with the small size of the particles. Therefore, for easy isolation and reuse of the photocatalyst in water treatment, TiO2 has been immobilized on solid supports such as silica gel [2], polyester fabric [14], rigid substrates like glass, quartz, and stainless steel [15]. Methods such as electrophoretic deposition [15], dip-coating [9, 15], and electrospinning [16, 17] have been used to immobilize the TiO2 photocatalyst on supports. It was discovered that the photocatalytic activity of the supported TiO2 was influenced by the adsorption ability of supports to the pollutants, as the pollutants are concentrated around the photocatalyst [18]. In this study, the electrospinning technique was used to immobilize TiO2 photocatalyst on PAN based carbon nanofibres. It was found in other studies to be a unique and cost effective way of making high surface area nanofibres [19].Electrospinning involves the use of a high voltage, which causes electrostatic charging of the droplet of the polymer, drawing a jet towards the grounded collector [20] to produce an interconnected membrane like a web of small nanofibres. In a typical process, a high voltage is applied between polymer solution droplet at the tip of the capillary tube and a grounded collector. A charged jet of the polymer solution is ejected when the applied electric field overcomes the surface tension of the polymer droplet. The jet then travels to the grounded collector through spiralling loops. To convert the polymer nanofibres to carbon nanofibres, a stabilization process is vital in an oxygen environment to form a thermally stable structure, which can withstand high carbonization temperatures.


## 2. Materials and Methods

### 2.1. Preparation of TiO2 Embedded Carbon Nanofibres

About 37.54 mL of absolute ethanol was added dropwise to 12.46 mL of ice cold titanium tetrachloride solution in conical flask with vigorous stirring to form titanium ethoxide. An appropriate amount of ice cold ethanol/water mixture was then added to the titanium ethoxide dropwise with stirring to give a final concentration of Ti+4 0.322 M. A few drops of glacial acetic acid were added to control the rate of hydrolysis. The solution was stirred for 2 hours with heating at 60°C until the solution turned white and turbid. After the gelation process, about 2 g of PAN powder was added followed by centrifugation and washing with water and absolute ethanol. Washing with ethanol helped to prevent agglomeration between the precipitates [21]. The PAN/Ti(OH)4 complex was then air-dried and then dissolved in a suitable amount of DMF to give a 10% PAN solution followed by electrospinning. Electrospinning was done using a high voltage power supply and a glass pipette of diameter 0.5 mm inclined at 45° to minimize dripping of the PAN solution. A voltage of 20 kV was used and the distance between the grounded aluminium foil collectors was 20 cm. After electrospinning, the PAN/TiO2 composite was stabilized by heating at a rate of 1°C per minute up to 280°C in an oxygen environment and maintained at that temperature for 2 hours to stabilize the PAN nanofibres and also to remove adsorbed water and solvent. This was then followed by heating at a rate of 5°C per minute up to 600°C in a nitrogen environment to bring about carbonization of the polymer fibres and calcination of TiO2 particles. The flow rate of the nitrogen gas was 58.6 mL/min.


### 2.2. Preparation of Surface Residing TiO2 Carbon Nanofibres

About 0.5 mL of titanium tetrachloride was added to 18.96 mL of dimethyl formamide dropwise with vigorous stirring in ice bath. About 2 g of PAN was then added and stirred until a homogenous PAN solution was formed. The solution was electrospun using a voltage of 20 kV and the distance between the tip of pipette containing the PAN solution and the collector was 20 cm. After electrospinning, the resulting PAN nanofibres containing the TiO2 precursor were immersed in distilled water to bring about the hydrolysis of the titanium tetrachloride. The PAN/TiO2 nanofibre mats were air-dried at room temperature followed by stabilization and carbonization as reported in Section 2.1.


### 2.3. Characterization

XRD patterns were obtained using a Bruker AXS (Germany) instrument with a D8 Advance Diffractometer. The X-ray tube used a Cu-Kα radiation (λ = 1.5406 Å) and a gas positron sensitive detector, PSD Vantec-1, with 1600 channels. FTIR spectroscopy was used to determine the functional groups and nature of hydroxyl groups and examine the chemical structures of the polymer to identify the mechanism of the modification reaction during the heat treatment process. The nanofibres were cut into small pieces, mixed with potassium bromide, and then pressed into a disk for the FTIR analysis. The surface morphology of the composite nanofibres was obtained using a JOEL JSM-6390LV Scanning Electron Microscope fitted with a secondary electron detector.DSC analysis was performed at a heating rate of 10°C/minute in nitrogen atmosphere with sample weights of about 5 mg on a Perkin Elmer DSC 7 differential scanning calorimeter equipped with Pyris Software. The thermal stability analysis was done using thermogravimetric instrument supplied by MET-UED, South Africa. About 10 mg of the nanofibres was used for TGA analysis using a heating rate of 10°C/minute up to 900°C in a nitrogen environment. The change in concentration of the methyl orange during photocatalytic activity evaluation was determined using a Perkin Elmer Lambda 35 UV-Vis spectrophotometer.


### 2.4. Evaluation of Photocatalytic Activity

The photocatalytic activities of PAN/TiO2-EM, CNF/TiO2-EM, and CNF/TiO2-SR were investigated using 100 mL of 10 ppm methyl orange solution at a temperature of 25°C and pH 7 in a cylindrical glass vessel. About 1 g of the composite TiO2/nanofibres was immersed in methyl orange solution and put in the dark for an hour to allow adsorption and desorption equilibrium to take place. The solution was then irradiated with ultraviolet light of wavelength 365 nm using a 40 W, 220 V (50/60 Hz) lamp fixed at 20 cm above the solution. After every thirty minutes, aliquots of methyl orange were taken and the concentration was determined using a UV-Vis spectrometer.


### 2.5. Total Organic Content Measurement

During the photodegradation process, aliquots were taken after every 30 minutes for total organic content (TOC) analysis. This was done using the TOC Fusion which employs the UV/persulfate oxidation of organic matter into carbon dioxide which is then measured by an NDIR detector which uses the ratio 1 : 1 of carbon dioxide to organic matter in the solution. The other parameters used were as follows: sample volume 4.0 mL, dilution 1 : 2, acid volume 1.0 mL, reagent volume 1.0 mL, UV reactor prerinse volume 5.0 mL, ICS sparge time 1 min, and detector sweep flow 500 mL/min and the system flow was 200 mL/min.


## 2.1. Preparation of TiO2 Embedded Carbon Nanofibres

About 37.54 mL of absolute ethanol was added dropwise to 12.46 mL of ice cold titanium tetrachloride solution in conical flask with vigorous stirring to form titanium ethoxide. An appropriate amount of ice cold ethanol/water mixture was then added to the titanium ethoxide dropwise with stirring to give a final concentration of Ti+4 0.322 M. A few drops of glacial acetic acid were added to control the rate of hydrolysis. The solution was stirred for 2 hours with heating at 60°C until the solution turned white and turbid. After the gelation process, about 2 g of PAN powder was added followed by centrifugation and washing with water and absolute ethanol. Washing with ethanol helped to prevent agglomeration between the precipitates [21]. The PAN/Ti(OH)4 complex was then air-dried and then dissolved in a suitable amount of DMF to give a 10% PAN solution followed by electrospinning. Electrospinning was done using a high voltage power supply and a glass pipette of diameter 0.5 mm inclined at 45° to minimize dripping of the PAN solution. A voltage of 20 kV was used and the distance between the grounded aluminium foil collectors was 20 cm. After electrospinning, the PAN/TiO2 composite was stabilized by heating at a rate of 1°C per minute up to 280°C in an oxygen environment and maintained at that temperature for 2 hours to stabilize the PAN nanofibres and also to remove adsorbed water and solvent. This was then followed by heating at a rate of 5°C per minute up to 600°C in a nitrogen environment to bring about carbonization of the polymer fibres and calcination of TiO2 particles. The flow rate of the nitrogen gas was 58.6 mL/min.


## 2.2. Preparation of Surface Residing TiO2 Carbon Nanofibres

About 0.5 mL of titanium tetrachloride was added to 18.96 mL of dimethyl formamide dropwise with vigorous stirring in ice bath. About 2 g of PAN was then added and stirred until a homogenous PAN solution was formed. The solution was electrospun using a voltage of 20 kV and the distance between the tip of pipette containing the PAN solution and the collector was 20 cm. After electrospinning, the resulting PAN nanofibres containing the TiO2 precursor were immersed in distilled water to bring about the hydrolysis of the titanium tetrachloride. The PAN/TiO2 nanofibre mats were air-dried at room temperature followed by stabilization and carbonization as reported in Section 2.1.


## 2.3. Characterization

XRD patterns were obtained using a Bruker AXS (Germany) instrument with a D8 Advance Diffractometer. The X-ray tube used a Cu-Kα radiation (λ = 1.5406 Å) and a gas positron sensitive detector, PSD Vantec-1, with 1600 channels. FTIR spectroscopy was used to determine the functional groups and nature of hydroxyl groups and examine the chemical structures of the polymer to identify the mechanism of the modification reaction during the heat treatment process. The nanofibres were cut into small pieces, mixed with potassium bromide, and then pressed into a disk for the FTIR analysis. The surface morphology of the composite nanofibres was obtained using a JOEL JSM-6390LV Scanning Electron Microscope fitted with a secondary electron detector.DSC analysis was performed at a heating rate of 10°C/minute in nitrogen atmosphere with sample weights of about 5 mg on a Perkin Elmer DSC 7 differential scanning calorimeter equipped with Pyris Software. The thermal stability analysis was done using thermogravimetric instrument supplied by MET-UED, South Africa. About 10 mg of the nanofibres was used for TGA analysis using a heating rate of 10°C/minute up to 900°C in a nitrogen environment. The change in concentration of the methyl orange during photocatalytic activity evaluation was determined using a Perkin Elmer Lambda 35 UV-Vis spectrophotometer.


## 2.4. Evaluation of Photocatalytic Activity

The photocatalytic activities of PAN/TiO2-EM, CNF/TiO2-EM, and CNF/TiO2-SR were investigated using 100 mL of 10 ppm methyl orange solution at a temperature of 25°C and pH 7 in a cylindrical glass vessel. About 1 g of the composite TiO2/nanofibres was immersed in methyl orange solution and put in the dark for an hour to allow adsorption and desorption equilibrium to take place. The solution was then irradiated with ultraviolet light of wavelength 365 nm using a 40 W, 220 V (50/60 Hz) lamp fixed at 20 cm above the solution. After every thirty minutes, aliquots of methyl orange were taken and the concentration was determined using a UV-Vis spectrometer.


## 2.5. Total Organic Content Measurement

During the photodegradation process, aliquots were taken after every 30 minutes for total organic content (TOC) analysis. This was done using the TOC Fusion which employs the UV/persulfate oxidation of organic matter into carbon dioxide which is then measured by an NDIR detector which uses the ratio 1 : 1 of carbon dioxide to organic matter in the solution. The other parameters used were as follows: sample volume 4.0 mL, dilution 1 : 2, acid volume 1.0 mL, reagent volume 1.0 mL, UV reactor prerinse volume 5.0 mL, ICS sparge time 1 min, and detector sweep flow 500 mL/min and the system flow was 200 mL/min.


## 3. Results and Discussion

### 3.1. Fourier Transform Infrared (FTIR) Analysis

Figure1 shows the FTIR spectra of unstabilized PAN/TiO2, stabilized PAN/TiO2, and CNF/TiO2 composite nanofibres. The spectrum of the stabilized nanofibres clearly shows that the band at 2243 cm−1 which is assigned to –C≡N stretching decreased considerably (almost disappeared) compared to the same peak in the spectrum of the unstabilized PAN/TiO2 composite nanofibres. A new peak appeared at 1604 cm−1 in the spectrum of stabilized nanofibres indicating that –C=C– (aromatic) bonds were formed during the stabilization process. The peaks around 2941 cm−1 and 2892 cm−1 due to asymmetric and symmetric bending in CH, CH2, and CH3 groups and around 1457 cm−1 due to CH bending [22] reduced in intensity significantly in the spectrum of SNF/TiO2 when compared to the spectrum of unstabilized nanofibres. This indicates that cyclization and dehydrogenation reaction occurred during thermal oxidative stabilization of PAN nanofibres resulting in the formation of an aromatic heat-resistant structure. These peaks completely disappeared in the spectrum of CNF/TiO2 showing that almost all the hydrogen had been lost during the carbonization process. Some researchers [23, 24] reported that the peak around 1630 cm−1 indicates the presence of –C=C– bond and in this study this peak appeared in the spectrum of SNF/TiO2 and CNF/TiO2 but not in the spectrum of the unstabilized PAN nanofibres. The peak around 3457 cm−1 was due to OH group. Exposure of TiO2 to moisture causes hydroxylation of the surface by chemisorption of water molecules. The peak around 500 cm−1 corresponds to Ti-O and Ti-O-Ti bands [25]. The peaks at 1171 cm−1 (medium) and 1739 cm−1 (very sharp) were due to C=O of the residual DMF and these peaks disappeared in the spectrum of the stabilized nanofibres due to loss of the solvent.Figure 1
FTIR spectra of unstabilized PAN/TiO2, SNF/TiO2, and CNF/TiO2 composite nanofibres.


### 3.2. Scanning Electron Microscope Analysis

Figure2 shows the SEM images of neat PAN nanofibres, neat carbon nanofibres, TiO2 embedded PAN nanofibres (PAN/TiO2-EM), and TiO2 surface residing carbon nanofibres (CNF/TiO2-SR). The surfaces of neat PAN nanofibres (Figure 2(a)) were smooth but the surfaces of the composites, PAN/TiO2-EM nanofibres (Figure 2(c)) and CNF/TiO2-SR (Figure 2(d)) nanofibres, were rough due to the encapsulated and surface residing TiO2 nanoparticles, respectively. All the heat treated nanofibres were much darker in colour when compared to the PAN nanofibres which were not heat treated. The colour changes that were observed during the heat treatment were from white to brown after stabilization and black after carbonization. The TiO2 particles of the PAN/TiO2-EM nanofibres were dispersed fairly uniformly over the carbon nanofibres because the TiO2 nanoparticles were dispersed homogenously in the PAN solution before electrospinning. It was difficult to find the size of the TiO2 in PAN/TiO2-EM because the nanoparticles were encapsulated showing that the nanoparticles were far less than the diameter of the nanofibres ca. 150 to 200 nm.Figure 2
SEM images of (a) neat PAN nanofibres, (b) neat carbon nanofibres, (c) PAN/TiO2-EM, and (d) CNF/TiO2-SR nanofibres. The magnification was 50 000.
(a) (b) (c) (d)The EDS graph of the CNF/TiO2 composite nanofibres is shown in Figure 3 and it showed the presence of carbon, titanium, and oxygen as expected. The peak around 0.4, 4.5, and 5 keV corresponds to titanium.Figure 3
EDX spectrum of CNF/TiO2.


### 3.3. Thermal Properties

Thermogravimetric (TGA) and differential scanning calorimetry (DSC) analyses were done to get information about the changes that occur to PAN and TiO2 during calcination and stabilization processes. In order to obtain high performance commercial PAN based carbon fibres, it is vital to stabilize the nanofibres completely. Figure 4 shows the DSC of unstabilized neat PAN and stabilized neat PAN and PAN/TiO2 nanofibres. The onset temperature of the cyclization of PAN, glass transition temperature (Tg) of PAN, conversion of the remaining Ti(OH)4 to TiO2, and crystallization of TiO2 could be easily determined from the DSC thermogram.Figure 4
DSC curves of neat PAN and stabilized neat PAN and PAN/TiO2 nanofibres.There were minor discontinuities at the start of the thermograms which do not seem to be thermal events. These discontinuities are an undesired alteration in data related to the start of the DSC heating program [26]. In the thermogram of PAN/TiO2 nanofibres, an endothermic peak between 30°C and 150°C was due to the conversion (thermal decomposition) of the remaining Ti(OH)4 to TiO2, volatilization of some organic materials, and evaporation/desorption of physically adsorbed water and solvent [27, 28]. The exothermic peak between 310°C and 325°C was common to thermograms of both PAN/TiO2 nanofibres and unstabilized neat PAN nanofibres and can be attributed to the crosslinking and cyclization of the nitrile groups of PAN. The cyclisation reactions are extremely exothermic [29].The exothermic peak for the neat PAN was sharp and intense and it appeared at a higher temperature (ca. 322.3°C) compared to that of the composite nanofibres which was small and appeared at a lower temperature (ca. 313.4°C). The reason for the appearance of the exothermic peak of the composite nanofibres at a lower temperature than neat PAN could probably be the presence of titanium dioxide, which could have affected the exothermic reaction by initiating the stabilization reactions and facilitating the process. The endothermic peak at 548.1°C was due to amorphous to crystalline anatase phase transformation of TiO2 [30]. The presence of titanium in the PAN helped in the determination of the glass transition temperature easily as this was insignificant in the DSC curve of neat PAN. The literature value of the glass transition temperature (Tg) of pure PAN is 125°C and in this study as can be seen in the DSC curve of PAN containing titanium tetrahydroxide was 128.5°C which showed an increment of 3.5°C. This increment is probably due to the additive, titanium dioxide nanoparticles. The DSC curve for the stabilized PAN nanofibres was almost a straight line with no exothermic peaks showing that stabilization was basically complete and a heat-resistant ladder structure had formed; therefore in this work cyclization was complete at 280°C.The proposed stages in the conversion of PAN to carbon nanofibres are shown in Figure5. The reactions involved in the conversion are very complex but include the cyclization of the nitrile groups and crosslinking of the PAN straight chains forming a ladder polymer, which cannot melt during the carbonization process. Carbonization involves the removal of noncarbon elements in form of gases such as NH3, CO2, N, CO, and water vapour [31].Figure 5
Stages of the conversion of polymeric PAN to carbon nanofibres.Figure6 shows the TGA thermogram and DTA curves of polyacrylonitrile containing TiO2 using a heating rate of 10°C/minute in the temperature range of 25–900°C. A small weight loss of about 2.5% between 20°C and 100°C was due to the release of adsorbed water and solvents. Around 313.9°C the weight loss of 7% of the composite nanofibres was due to cyclization of the PAN, which is in agreement with the DSC analysis.Figure 6
TGA thermograms of PAN/TiO2 nanofibres.


### 3.4. Raman Analysis

Raman spectroscopy is a nondestructive, quick, and noncontacting technique that is commonly used to characterize and study the microstructural and phase information of carbon related materials. Figure7 shows the Raman spectra of the CNF/TiO2 and unstabilized and stabilized composite nanofibres using a laser with an excitation wavelength of 514.5 nm in the range of Raman shift of 949 to 2900 cm−1. Normally carbon fibres show two peaks, the D and G peaks around 1360 cm−1 and 1580 cm−1, respectively [32, 33]. In this study, the D peak of the CNF/TiO2 was found at 1362 cm−1 and the G peak appeared at 1564 cm−1. The presence of the G peak in the spectrum of CNF/TiO2 indicated the presence of Raman active sp2 carbon networks. The Raman spectra of the stabilized and unstabilized composite nanofibres did not give clear distinct D and G peaks. The unstabilized PAN/TiO2 composite fibres showed a small broad D peak compared to the heat treated fibres (stabilized and CNF/TiO2 composite nanofibers) and this agrees well with what was reported in literature [33]. The peak around 1865 cm−1 in the spectrum of unstabilized nanofibres was due to the presence of linear carbon chains [34]. As the temperature was increased, the intensity of the peaks increased. From these spectra, it can be observed that the G band is a feature for the highly ordered graphite structure, which was found in the carbonized nanofibres and this agrees well with what was reported in literature [34]. As the temperature was increased, the disordered carbon structure transformed into a more ordered graphitic carbon structure with good mechanical properties.Figure 7
Raman spectrum of (a) CNF/TiO2, (b1) unstabilized PAN/TiO2 nanofibres, and (b2) stabilized PAN/TiO2 nanofibres using 514.5 nm laser excitation.
(a) (b)Figure8 shows the XRD patterns of CNF/TiO2 and neat PAN nanofibres. In the XRD pattern of neat nanofibres, two equatorial peaks at 2θ values of 17.1° and 29.1° were observed. These peaks disappeared upon carbonization and after oxidation as these peaks could not appear in the XRD patterns of the CNF/TiO2. The peaks at 2θ values of 27.0°, 36.1°, 40.2°, 43.5°, 54.1°, and 68.6° indicate the presence of TiO2 in the rutile phase while small peaks at 2θ values of 25.1°, 47.2°, and 62.3° correspond to the diffraction of (101), (200), and (204) crystal faces of the anatase phase of TiO2 [35]. The major TiO2 phase was the rutile phase because of the heat treatment up to 600°C during the carbonization stage that transformed the anatase to rutile phase.Figure 8
XRD patterns of neat PAN nanofibres and CNF/TiO2.


### 3.5. Photocatalytic Activity Evaluation

Methyl orange was chosen as a model of the azo dyes that are mainly used in the chemical and textile industries. After an hour in the dark to allow desorption and adsorption equilibrium to take place on the composite nanofibres, it was observed that the absorbance which is proportional to the change in concentration was reduced from 0.512 to 0.489 by CNF/TiO2, to 0.462 by SNF/TiO2, and to 0.413 by PAN/TiO2 as shown in Figure 9. This showed that the PAN nanofibres were better adsorbents than heat treated polymer nanofibres. This is because PAN is polar and methyl orange is also polar; hence the interaction between the adsorbate and the surface sites of the adsorbent was enhanced.Figure 9
Change in absorbance of methyl orange due to adsorption by (A) initial (B) CNF/TiO2, (C) PAN/TiO2, and (D) SNF/TiO2.Figure10 shows the changes in concentration of methyl orange as a function of time under UV illumination for CNF/TiO2-EM, CNF/TiO2-SR, SNF/TiO2, and PAN/TiO2. The CNF/TiO2-SR showed the highest photocatalytic activity and it degraded 59.35% of methyl orange after 210 minutes followed by CNF/TiO2-EM, which degraded 25.48%, and SNF/TiO2 21.58% and PAN/TiO2 showed the least (16.44%). The reasons for the general higher photocatalytic activities of TiO2 in the CNF are that, during the carbonization of the polymer nanofibres, calcination of TiO2 occurred resulting in increased crystallinity and anatase to rutile phase transformation. Crystallinity increases the photocatalytic activity of the TiO2 nanoparticles. The anatase to rutile phase transformation that occurred resulted in a mixture of the two phases on the CNF. Although anatase has been reported to be more photocatalytically active than the rutile phase, a mixture of anatase and rutile with a ratio of 75 : 25 was found to be beneficial in reducing recombination of charge carriers resulting in a much higher photocatalytic activity than either pure anatase or pure rutile TiO2 photocatalyst [36, 37]. This shows that heat treatment is an important step in the preparation of a semiconductor photocatalyst. These results clearly indicate that polymer nanofibres are promising supports for semiconductor photocatalysts as they can adsorb pollutants bringing them closer to the photocatalyst to be degraded.Figure 10
Photodegradation curves of methyl orange concentration as a function of time using the composite nanofibres at 25°C and pH 7.The difference in the photocatalytic activities of the CNF/TiO2-EM and CNF/TiO2-SR was attributed to the total surface area of TiO2 nanoparticles in contact with methyl orange. In CNF/TiO2-EM, some of the nanoparticles were encapsulated meaning they were not in direct contact with the contaminant; hence its photocatalytic activity was lower than that of CNF/TiO2-SR.The stability of the nanofibre supports was checked by SEM analysis before and after the photocatalytic process. It was discovered that there was relatively no changes in nanofibre morphology that occurred indicating that the nanofibres were relatively stable.Table1 shows the TOC analysis results of methyl orange photodegradation catalyzed by CNF/TiO2-SR which was the best photocatalyst. The TOC could be quantified by measuring the carbon dioxide generated when the organic compounds were oxidized and according to Luo and coworkers (2015) it excludes the inorganic carbon compounds [38]. Generally there was a decrease in the TOC with increase in photodegradation time.Table 1
TOC analysis results of methyl orange photodegradation.
Time (minutes) TOC (mg/L) 0 73.5 30 66.3 60 61.1 90 52.3 150 46.3 180 44.5


## 3.1. Fourier Transform Infrared (FTIR) Analysis

Figure1 shows the FTIR spectra of unstabilized PAN/TiO2, stabilized PAN/TiO2, and CNF/TiO2 composite nanofibres. The spectrum of the stabilized nanofibres clearly shows that the band at 2243 cm−1 which is assigned to –C≡N stretching decreased considerably (almost disappeared) compared to the same peak in the spectrum of the unstabilized PAN/TiO2 composite nanofibres. A new peak appeared at 1604 cm−1 in the spectrum of stabilized nanofibres indicating that –C=C– (aromatic) bonds were formed during the stabilization process. The peaks around 2941 cm−1 and 2892 cm−1 due to asymmetric and symmetric bending in CH, CH2, and CH3 groups and around 1457 cm−1 due to CH bending [22] reduced in intensity significantly in the spectrum of SNF/TiO2 when compared to the spectrum of unstabilized nanofibres. This indicates that cyclization and dehydrogenation reaction occurred during thermal oxidative stabilization of PAN nanofibres resulting in the formation of an aromatic heat-resistant structure. These peaks completely disappeared in the spectrum of CNF/TiO2 showing that almost all the hydrogen had been lost during the carbonization process. Some researchers [23, 24] reported that the peak around 1630 cm−1 indicates the presence of –C=C– bond and in this study this peak appeared in the spectrum of SNF/TiO2 and CNF/TiO2 but not in the spectrum of the unstabilized PAN nanofibres. The peak around 3457 cm−1 was due to OH group. Exposure of TiO2 to moisture causes hydroxylation of the surface by chemisorption of water molecules. The peak around 500 cm−1 corresponds to Ti-O and Ti-O-Ti bands [25]. The peaks at 1171 cm−1 (medium) and 1739 cm−1 (very sharp) were due to C=O of the residual DMF and these peaks disappeared in the spectrum of the stabilized nanofibres due to loss of the solvent.Figure 1
FTIR spectra of unstabilized PAN/TiO2, SNF/TiO2, and CNF/TiO2 composite nanofibres.


## 3.2. Scanning Electron Microscope Analysis

Figure2 shows the SEM images of neat PAN nanofibres, neat carbon nanofibres, TiO2 embedded PAN nanofibres (PAN/TiO2-EM), and TiO2 surface residing carbon nanofibres (CNF/TiO2-SR). The surfaces of neat PAN nanofibres (Figure 2(a)) were smooth but the surfaces of the composites, PAN/TiO2-EM nanofibres (Figure 2(c)) and CNF/TiO2-SR (Figure 2(d)) nanofibres, were rough due to the encapsulated and surface residing TiO2 nanoparticles, respectively. All the heat treated nanofibres were much darker in colour when compared to the PAN nanofibres which were not heat treated. The colour changes that were observed during the heat treatment were from white to brown after stabilization and black after carbonization. The TiO2 particles of the PAN/TiO2-EM nanofibres were dispersed fairly uniformly over the carbon nanofibres because the TiO2 nanoparticles were dispersed homogenously in the PAN solution before electrospinning. It was difficult to find the size of the TiO2 in PAN/TiO2-EM because the nanoparticles were encapsulated showing that the nanoparticles were far less than the diameter of the nanofibres ca. 150 to 200 nm.Figure 2
SEM images of (a) neat PAN nanofibres, (b) neat carbon nanofibres, (c) PAN/TiO2-EM, and (d) CNF/TiO2-SR nanofibres. The magnification was 50 000.
(a) (b) (c) (d)The EDS graph of the CNF/TiO2 composite nanofibres is shown in Figure 3 and it showed the presence of carbon, titanium, and oxygen as expected. The peak around 0.4, 4.5, and 5 keV corresponds to titanium.Figure 3
EDX spectrum of CNF/TiO2.


## 3.3. Thermal Properties

Thermogravimetric (TGA) and differential scanning calorimetry (DSC) analyses were done to get information about the changes that occur to PAN and TiO2 during calcination and stabilization processes. In order to obtain high performance commercial PAN based carbon fibres, it is vital to stabilize the nanofibres completely. Figure 4 shows the DSC of unstabilized neat PAN and stabilized neat PAN and PAN/TiO2 nanofibres. The onset temperature of the cyclization of PAN, glass transition temperature (Tg) of PAN, conversion of the remaining Ti(OH)4 to TiO2, and crystallization of TiO2 could be easily determined from the DSC thermogram.Figure 4
DSC curves of neat PAN and stabilized neat PAN and PAN/TiO2 nanofibres.There were minor discontinuities at the start of the thermograms which do not seem to be thermal events. These discontinuities are an undesired alteration in data related to the start of the DSC heating program [26]. In the thermogram of PAN/TiO2 nanofibres, an endothermic peak between 30°C and 150°C was due to the conversion (thermal decomposition) of the remaining Ti(OH)4 to TiO2, volatilization of some organic materials, and evaporation/desorption of physically adsorbed water and solvent [27, 28]. The exothermic peak between 310°C and 325°C was common to thermograms of both PAN/TiO2 nanofibres and unstabilized neat PAN nanofibres and can be attributed to the crosslinking and cyclization of the nitrile groups of PAN. The cyclisation reactions are extremely exothermic [29].The exothermic peak for the neat PAN was sharp and intense and it appeared at a higher temperature (ca. 322.3°C) compared to that of the composite nanofibres which was small and appeared at a lower temperature (ca. 313.4°C). The reason for the appearance of the exothermic peak of the composite nanofibres at a lower temperature than neat PAN could probably be the presence of titanium dioxide, which could have affected the exothermic reaction by initiating the stabilization reactions and facilitating the process. The endothermic peak at 548.1°C was due to amorphous to crystalline anatase phase transformation of TiO2 [30]. The presence of titanium in the PAN helped in the determination of the glass transition temperature easily as this was insignificant in the DSC curve of neat PAN. The literature value of the glass transition temperature (Tg) of pure PAN is 125°C and in this study as can be seen in the DSC curve of PAN containing titanium tetrahydroxide was 128.5°C which showed an increment of 3.5°C. This increment is probably due to the additive, titanium dioxide nanoparticles. The DSC curve for the stabilized PAN nanofibres was almost a straight line with no exothermic peaks showing that stabilization was basically complete and a heat-resistant ladder structure had formed; therefore in this work cyclization was complete at 280°C.The proposed stages in the conversion of PAN to carbon nanofibres are shown in Figure5. The reactions involved in the conversion are very complex but include the cyclization of the nitrile groups and crosslinking of the PAN straight chains forming a ladder polymer, which cannot melt during the carbonization process. Carbonization involves the removal of noncarbon elements in form of gases such as NH3, CO2, N, CO, and water vapour [31].Figure 5
Stages of the conversion of polymeric PAN to carbon nanofibres.Figure6 shows the TGA thermogram and DTA curves of polyacrylonitrile containing TiO2 using a heating rate of 10°C/minute in the temperature range of 25–900°C. A small weight loss of about 2.5% between 20°C and 100°C was due to the release of adsorbed water and solvents. Around 313.9°C the weight loss of 7% of the composite nanofibres was due to cyclization of the PAN, which is in agreement with the DSC analysis.Figure 6
TGA thermograms of PAN/TiO2 nanofibres.


## 3.4. Raman Analysis

Raman spectroscopy is a nondestructive, quick, and noncontacting technique that is commonly used to characterize and study the microstructural and phase information of carbon related materials. Figure7 shows the Raman spectra of the CNF/TiO2 and unstabilized and stabilized composite nanofibres using a laser with an excitation wavelength of 514.5 nm in the range of Raman shift of 949 to 2900 cm−1. Normally carbon fibres show two peaks, the D and G peaks around 1360 cm−1 and 1580 cm−1, respectively [32, 33]. In this study, the D peak of the CNF/TiO2 was found at 1362 cm−1 and the G peak appeared at 1564 cm−1. The presence of the G peak in the spectrum of CNF/TiO2 indicated the presence of Raman active sp2 carbon networks. The Raman spectra of the stabilized and unstabilized composite nanofibres did not give clear distinct D and G peaks. The unstabilized PAN/TiO2 composite fibres showed a small broad D peak compared to the heat treated fibres (stabilized and CNF/TiO2 composite nanofibers) and this agrees well with what was reported in literature [33]. The peak around 1865 cm−1 in the spectrum of unstabilized nanofibres was due to the presence of linear carbon chains [34]. As the temperature was increased, the intensity of the peaks increased. From these spectra, it can be observed that the G band is a feature for the highly ordered graphite structure, which was found in the carbonized nanofibres and this agrees well with what was reported in literature [34]. As the temperature was increased, the disordered carbon structure transformed into a more ordered graphitic carbon structure with good mechanical properties.Figure 7
Raman spectrum of (a) CNF/TiO2, (b1) unstabilized PAN/TiO2 nanofibres, and (b2) stabilized PAN/TiO2 nanofibres using 514.5 nm laser excitation.
(a) (b)Figure8 shows the XRD patterns of CNF/TiO2 and neat PAN nanofibres. In the XRD pattern of neat nanofibres, two equatorial peaks at 2θ values of 17.1° and 29.1° were observed. These peaks disappeared upon carbonization and after oxidation as these peaks could not appear in the XRD patterns of the CNF/TiO2. The peaks at 2θ values of 27.0°, 36.1°, 40.2°, 43.5°, 54.1°, and 68.6° indicate the presence of TiO2 in the rutile phase while small peaks at 2θ values of 25.1°, 47.2°, and 62.3° correspond to the diffraction of (101), (200), and (204) crystal faces of the anatase phase of TiO2 [35]. The major TiO2 phase was the rutile phase because of the heat treatment up to 600°C during the carbonization stage that transformed the anatase to rutile phase.Figure 8
XRD patterns of neat PAN nanofibres and CNF/TiO2.


## 3.5. Photocatalytic Activity Evaluation

Methyl orange was chosen as a model of the azo dyes that are mainly used in the chemical and textile industries. After an hour in the dark to allow desorption and adsorption equilibrium to take place on the composite nanofibres, it was observed that the absorbance which is proportional to the change in concentration was reduced from 0.512 to 0.489 by CNF/TiO2, to 0.462 by SNF/TiO2, and to 0.413 by PAN/TiO2 as shown in Figure 9. This showed that the PAN nanofibres were better adsorbents than heat treated polymer nanofibres. This is because PAN is polar and methyl orange is also polar; hence the interaction between the adsorbate and the surface sites of the adsorbent was enhanced.Figure 9
Change in absorbance of methyl orange due to adsorption by (A) initial (B) CNF/TiO2, (C) PAN/TiO2, and (D) SNF/TiO2.Figure10 shows the changes in concentration of methyl orange as a function of time under UV illumination for CNF/TiO2-EM, CNF/TiO2-SR, SNF/TiO2, and PAN/TiO2. The CNF/TiO2-SR showed the highest photocatalytic activity and it degraded 59.35% of methyl orange after 210 minutes followed by CNF/TiO2-EM, which degraded 25.48%, and SNF/TiO2 21.58% and PAN/TiO2 showed the least (16.44%). The reasons for the general higher photocatalytic activities of TiO2 in the CNF are that, during the carbonization of the polymer nanofibres, calcination of TiO2 occurred resulting in increased crystallinity and anatase to rutile phase transformation. Crystallinity increases the photocatalytic activity of the TiO2 nanoparticles. The anatase to rutile phase transformation that occurred resulted in a mixture of the two phases on the CNF. Although anatase has been reported to be more photocatalytically active than the rutile phase, a mixture of anatase and rutile with a ratio of 75 : 25 was found to be beneficial in reducing recombination of charge carriers resulting in a much higher photocatalytic activity than either pure anatase or pure rutile TiO2 photocatalyst [36, 37]. This shows that heat treatment is an important step in the preparation of a semiconductor photocatalyst. These results clearly indicate that polymer nanofibres are promising supports for semiconductor photocatalysts as they can adsorb pollutants bringing them closer to the photocatalyst to be degraded.Figure 10
Photodegradation curves of methyl orange concentration as a function of time using the composite nanofibres at 25°C and pH 7.The difference in the photocatalytic activities of the CNF/TiO2-EM and CNF/TiO2-SR was attributed to the total surface area of TiO2 nanoparticles in contact with methyl orange. In CNF/TiO2-EM, some of the nanoparticles were encapsulated meaning they were not in direct contact with the contaminant; hence its photocatalytic activity was lower than that of CNF/TiO2-SR.The stability of the nanofibre supports was checked by SEM analysis before and after the photocatalytic process. It was discovered that there was relatively no changes in nanofibre morphology that occurred indicating that the nanofibres were relatively stable.Table1 shows the TOC analysis results of methyl orange photodegradation catalyzed by CNF/TiO2-SR which was the best photocatalyst. The TOC could be quantified by measuring the carbon dioxide generated when the organic compounds were oxidized and according to Luo and coworkers (2015) it excludes the inorganic carbon compounds [38]. Generally there was a decrease in the TOC with increase in photodegradation time.Table 1
TOC analysis results of methyl orange photodegradation.
Time (minutes) TOC (mg/L) 0 73.5 30 66.3 60 61.1 90 52.3 150 46.3 180 44.5


## 4. Conclusions

Titanium dioxide nanoparticles immobilized on carbon nanofibres via electrospinning and annealing the PAN/TiO2 composite were successfully prepared. The neat electrospun nanofibres displayed a very sharp exothermic peak at 322.3°C whereas the composite displayed it at 313.4°C. The titanium dioxide was found to lower the cyclization temperature of the polyacrylonitrile as indicated by DSC and DTA analysis. The CNF/TiO2-SR exhibited a higher photocatalytic activity than CNF/TiO2-EM, SNF/TiO2, and PAN/TiO2 nanofibres. Calcination at high temperatures is a way of improving the crystallinity and had a beneficial effect on the photocatalytic activity of TiO2. It was noted that polymer nanofibres have a high adsorption capacity compared to the heat treated polymer nanofibres.



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*Source: 3162976-2016-12-27.xml*