1. IntroductionCurrent energy infrastructures which mostly depend on fossil fuels release greenhouse gases (GHG) and lead to the global warming. According to Wallington et al., 30 billions of tons CO2 emissions were released every year generally for the electricity and heat production [1] . Besides that, the global energy demand is forecasted to increase in the future with the growth by roughly double in 2050 and triple by the end of this century [2] . Therefore, meeting the current energy demand and reducing the impact of global warming are two global issues that really need an appropriate solution. Nowadays, the alternative solutions in carbon management are Carbon Capture and Storage (CCS) and Carbon capture and Utilization (CCU). The CCS is known as the long term solutions but it has a high potential hazard due to CO2 leakage and high equipment cost [3] . The CCU method reuses the captured CO2 but it is only applicable for a high purity of CO2 waste. Therefore, the new alternative was introduced, the Carbon Capture and Conversion (CCC) method. This CCC method will convert the captured CO2 into a renewable energy product such as methane, ethane, ethylene and methanol. This new alternative is promptly able to meet the global energy demand without any fossil fuels shortages and has a high potential energy source since CO2 is green, abundant, nontoxic and an inexpensive feedstock [4] [5] . Since this method is new and not commercial yet, some improvements need to be done. The highly efficient CCC materials synthesized via a green method with a low equipment cost and simple experimental steps are the ultimate goals in this research work.
The morphological change such as surface area and the crystallinity phase will affect the photocatalytic efficiency in each composite and this morphological change is actually related to the synthesis method [6] . According to Rosa M. et al., highly efficient CCC materials with a longer lifespan can be synthesized by focusing on the synthesis method [7] . According to Dong et al., although the chemical modification of TiO2-carbon composite can enhance the capability to absorb in the visible range and improve its photocatalytic performance, it can also decrease the surface area and thereby decrease the absorptive power and photocatalytic performance. That is because of the weak interfacial contact GO and severe aggregation of TiO2 particles on the graphene sheets, causing the development of highly efficient photocatalyst remains challenging until today.
There were various synthesis methods that had been reported such as simple liquid phase deposition method [8] , thermal hydrolysis of suspension [9] , simple wet impregnation method [10] , microwave-hydrothermal treatment [11] , simple solvothermal method [12] and modified hydrothermal method [13] [14] which were using different raw material, equipment needed and also different experimental step. Based on our study, we found that the solvothermal and hydrothermal method are the good synthesis method due to their availability and low raw material cost, low equipment cost and also the simple and scalable experimental step. The differences between the solvothermal and hydrothermal synthesis methods are only the solvent used. The solvothermal typically using an acid such as acetic acid while hydrothermal using alkaline water or distilled water as a solvent. Solvent is important aspect in both morphological growths since it will control the state of active Ti species during the growth. According to Shen, et al., the obtained rGO-TiO2 composite via a modified hydrothermal method are pure, with less defects compared to others synthesized method, controllable structure and quite high CO2 conversion rate [6] . Wang et al. reported that, the in-situ hydrothermal method can ensure the strong interaction between the semiconductor nanocomposites which makes their work synergistically [15] . Besides that, Zhang et al. reported that, the hydrothermal method to synthesize the TiO2-GO is the simple and efficient method [16] . According to the Fan and co, the TiO2-rGO composites which prepared by the hydrothermal method shows the most efficient photocatalyst for the evolution of H2 compare to others synthesize method; UV-assisted photoreduction and chemical reduction using a hydrazine [17] . In contrast, [12] reported that the solvothermal method is economically and practically feasible method. Ali et al., reported that the solvothermal method are the most effective, cleaner route, economic and environmentally friendly [18] .
The effects of synthesis method on the growth of reduced graphene oxide-Titanium (rGO-TiO2) as a Carbon Capture and Conversion (CCC) composite will be studied. The rGO-TiO2 composites in this research works were synthesized via solvothermal and hydrothermal methods. The CCC composite will then be analyzed by using a UV-Vis and XRD. By focusing on the synthesizing method of this CCC composite, it will give a great contribution and beneficiaries to the renewable energy fields.
2. Material and Method2.1. MaterialsThe raw material been used to prepare the rGO-TiO2 composites are Graphite Oxide (GO) powder, Tetrabutyl Titanate powder (TBT), commercial TiO2 Anatase powder, ethylene glycol (EG), acetic acid (HAc) and Ammonium hydroxide (NaOH).
2.2. CharacterizationThere are several characterizations equipment had been used such as Field Emission Scanning Electron Microscopy(FESEM) to check the surface morphology, X-ray Diffractometry (XRD) to check the crystallinity, UV-Vis spectrophotometer to identify the optical properties, Electrochemical Impedance Spectroscopy (EIS) to check the electrical properties, Fluorescent spectrometer (PL) to check the recombination rate of the photogenerated electron-hole pairs and lastly is the Gas Chromatograph (GC) to testing the photo reduction and conversion. In this paper, the results obtained from the XRD and UV-Vis were focused on.
The crystallinity of the samples, rGO-TiO2 composites will be examine by using XRD with the radiation (wavelength, λ = 0.15406 nm) at 0.02˚ s−1 a scan rate (2θ). The absorbance spectra were analyzed by using a UV-Vis spectroscope under ambient temperature in the wavelength ranging from 200 - 800 nm. The band gap energies of the photocatalyst were estimated from the Kubelka-Munk (KM) function F(R) and the extrapolation of the Tauc plot [F(R) ∙ hv]1/2 to the abscissa of photon energy, hv. The raw data were analyzed by using the OriginPro 9.1 and excel software to tabulate and plotting the graphs. Four samples will be compared; pure TiO2, rGO-TiO2 (S), rGO-TiO2 (H1) and rGO-Anatase TiO2 (H2). The rGO-TiO2 (S) was synthesized by solvothermal while rGO-TiO2 (H1) and rGO-Anatase TiO2 (H2) were synthesized by hydrothermal method.
2.3. Synthesis MethodThe solvothermal method (S) were using a step reported by [10] , the hydrothermal method 1 (H1) were using a modification of method reported by [10] . The modification of step [10] is followed by [19] . The hydrothermal method 2 (H2) are followed the method reported by [20] . The (H1) method is originally proposed in this research work to synthesize the rGO-TiO2 composite for photocatalyst reduction applications. To the best of our knowledge, there is no reported paper which synthesized the rGO-TiO2 composite by using this H1 method. The solvent used in the (S) method are the ethylene glycol (EG) and acetic acid (HAc) as per [10] while the (H1) method are NaOH and distilled water as the alkaline solvent before heated in autoclave at 180˚C temperature. The 8 hours treatment time in autoclave and 180˚C temperature were fixed conditions for both solvothermal and hydrothermal methods. The effect of synthesis method on the crystallinity, recombination rate of electron-hole pairs and photocatalytic activities in each synthesized composites will be study and discuss further.
2.4. Synthesis of Graphene Oxide (GO)Figure 1 shows the synthesizing process of graphene oxide (GO) from the graphite powder by using a modified Hummers method [12] . Graphite powder were added into concentrated H2SO4, P2O5 and K2S2O8 then undergo the mixture, filter and wash process and dried overnight. On the next day, the pre-oxidized graphite was dispersed into cold (0˚C) concentrated H2SO4. KMnO4 were added slowly until thick green paste was observed. The residue then was filtered, washed, and kept overnight. The solution was then centrifuged at 14000rpm for 30 min each time to obtain the GO powder.
2.5. Synthesis of rGO-TiO<sub>2</sub> Composite via Solvothermal Method, rGO-TiO<sub>2</sub> (S)Figure 2 shows the synthesizing process of rGO-TiO2 (S) via a solvothermal method by using a Teflon-Lined autoclave. The TiO2 precursor was synthesized from the TBT powder. The GO sheet was prepared by dispersing the GO into distilled water and ultrasonicated for 1 hour at ambient temperature. The GO sheet solution was chilled until to ≈5˚C in an ice bath and labelled as solution A. The titanium solution was prepared by adding the TiO2 precursor, ethylene glycol (Eg) and acetic acid (HAc) together. The TiO2 solution was then chilled to ≈5˚C in an ice bath and labelled as solution B. Consequently, the solution B was added dropwise into the chilled solution A under vigorous stirring. The mixture of solution A and B was then transferred into 200 mL Teflon Lined stainless steel autoclave and was heated for 8hours. The resultant solid was dried in air oven overnight. Before the characterization stage, the precipitate was annealed for 60 minutes.
2.6. Synthesis of rGO-TiO<sub>2</sub> Composite via Hydrothermal Method, rGO-TiO<sub>2</sub> (H1) and rGO-Anatase TiO<sub>2</sub> (H2)Figure 3 shows the synthesizing process of rGO-TiO2 (H1) and rGO-TiO2 (H2) via a Hydrothermal Method by using a Teflon-Lined autoclave. The rGO-TiO2 (H1) was synthesized from the TBT powder while rGO-TiO2 (H2) from the P90 TiO2 powder. The GO sheet was prepared by sonicating the GO mixture which consist of GO and deionized water for 1 hour. Then, add TiO2 precursor powder dropwise into the stirring GO mixture. The mixture was further stirred for 1 hour to ensure complete mixing. Next, the NaOH was then added into the mixture. The solution was then transferred into 200 mL Teflon-Lined autoclave and heated under static condition for 8hours. The gray colored gel product was then washed with 0.1M HCl solution and stirred overnight at room temperature. Subsequently, the final product was washed with deionized water several times, centrifuged at 5000 rpm for 30 minutes and dried overnight. Before the characterization stage, the precipitate was annealed 300˚C for 60 minutes.
3. Results and DiscussionThe crystallinity of chemical composition and the crystalline size of composites can be determined by using XRD. Higher the crystallinity and smaller the crystalline size will lead to the better photocatalytic performance.
The interaction between rGO and TiO2 can be analyze in the diffuse reflectance of UV-Vis result. The wavelength (nm) in the absorption edge was indicate the elemental band gap absorption of TiO2 from the electron transitions from VB to the CB [18] . The higher the wavelength (nm) in the absorption edge means lower the elemental band gap absorption of its TiO2 which lead to the better photocatalytic performance because the electron at the VB do not need to absorb high energy from the UV light to excite and escape to the CB. Besides that, by using the Tauc plot of the modified Kubelka-Munk (KM) function with a linear extrapolation, we can determine the optical bandgap of each composite.
3.1. XRDFigure 4 shows the XRD patterns of (S), (H1) and (H2). The note A means the TiO2 in anatase phase while R means in rutile phase. The XRD pattern of (S) above shows the significant peaks at 25.3˚, 27.439˚, 37.8˚ and 48˚ which can be indexed to the (101A), (101R), (004) and (200) crystal planes of a tetragonal anatase phase (JCPDS no. 21-1272) [12] . The XRD patterns of the (H2) above shows the significant peaks at 25.3˚ and 48˚ which are match with the titanium anatase pattern (ICSD ref no. 00-004-0477) with the lattice constants a = 3.7830 Å and c = 9.5100 Å. Besides that, there is another peak at 27.439˚ which was matched with the titanium rutile pattern (ICSD ref no. 01-078-1508) with the lattice constants a = 4.5933 Å and c = 2.9580 Å. It means that the composite are consist of both anatase and rutile phase TiO2. However, the crystallinity peak of this composite shows the lowest peak compare to the other composites (S) and (H1) which lead to the lowest crystallinity and biggest crystalline size.
The XRD patterns of the (H1) above shows several peaks at 25.3˚ (101), 37.8˚ (004), 48˚ (200), 53.9˚ (105), 62.7˚ (204), 70.3˚ (116) and 75˚ (215) which match with the pure tetragonal anatase phase (JCPDS ref no. 21-1272) with the lattice constants a = 3.78 Å and c = 9.50 Å. The diffraction peak of rGO-TiO2 (H1) showed a strong and sharp diffraction peak which lead to the highest crystallinity and the smallest crystalline size. Referring to the XRD result reported by Wenqing et al., the rGO diffraction peak are at 24.5˚ with the very broad peak and looks disappear [13] . The rGO were stacked together with the TiO2 nanoparticles to form the undetectable graphite structure [13] . Therefore, we assume that our undetectable rGO diffraction peak was being shielded by the main peak of anatase TiO2 at 25.3˚. We can conclude that, all composites were pure and well crystallized due to no diffraction peak was detected from the impurities compositions. The rGO-TiO2 composites prepared by the other methods showed similar XRD patterns [12] [13] .
The broad diffraction peaks are indicating the big crystallite size while the sharp and strong diffraction peaks determine the small crystallite size. As mention earlier, the smaller the crystalline size, the better its photocatalytic performance. That is because, the small crystallite size will provide a big surface area which is the most important for the photocatalytic activity to occur. By using the Scherrer’s equation as shown in Equation (1) below, we calculate the average crystal size of the TiO2 particles in each composite for further analyzation. The λ is the CuKα radiation (λ = 0.15406 nm), β is the full width at half maximum (FWHM) intensity of the peak in radians and θ is the Bragg’s diffraction angle.
D = 0.9 λ β cos θ
Equation (1): Scherrer’s equation [15] .
Figure 5 shows the average crystal size of the TiO2 particles in (S), (H1) and (H2) composite by using a Scherrer’s equation. The average crystal size of the TiO2 particles in the (S), (H1) and (H2) composites are 86.57 nm, 107.05 nm and 42.14 nm respectively. Clearly shows that the crystallinity and the crystal size of TiO2 were affected by the synthesizing method. The crystallinity and the better crystallite size was at (H1) composite. The smallest crystallite size means the biggest surface area for a better photocatalytic performance.
3.2. UV-VisFigure 6 shows the UV Vis diffuse reflectance spectra of titanium (TiO2), (H2), (S) and (H1). As shown in Figure 4, the estimated wavelength in absorption edge for the spectra (TiO2), (H2), (S) and (H1) are 390 nm, 410 nm, 420 nm and 490 nm respectively. Notably that the synthesized rGO-TiO2 composites (H2), (S) and (H1) were shifted to the higher wavelength in the absorption edge compare to the pure titanium (TiO2).
Figure 7 shows the Kubelka-Munk function plot of (TiO2), (H2), (S) and (H1). We can see the approximated band gaps of (TiO2), (H2), (S) and (H1)
are 3.40 eV, 3.10 eV, 2.90 eV, 2.60 eV respectively. Due to some researchers, the band gap narrowing occurs because of the formation of strong Ti-O-C bond between the TiO2 and rGO composites [21] [22] . The smaller the band gap, the better the formation of Ti-O-C bond due to the strong contact between TiO2 and rGO. Based on this result, the formation of Ti-O-C bond in (H1) is the strongest compare to (S) and (H2) can be concluded. The formation of Ti-O-C bond leads to improve the absorption edge and resulting a better electron transitions from the VB to the CB for a better photocatalytic performance.
3.3. DiscussionAs we can see from the UV Vis spectroscopy result, the band gap narrowing was showed for all three composites compare to pure TiO2. The (H1) shows the lowest band gap with 2.60 eV compare to the (S) with 2.90 eV and (H2) with 3.10 eV. Hence, the possibility of (H1) composite to perform a better photocatalytic reduction is high compare (H2) and (S) due to its wider absorption light range and potentially to produce a multiple photogenerated electron-hole pairs. The strong interaction/contact between TiO2 and rGO will form a better Ti-O-C bond and lead to the band gap narrowing [21] [22] . Perera et al. stated that, the presence of rGO can help to separate the photogenerated electron-hole pairs and without them, the possibility of the photogenerated electron-hole pairs to recombine is high [14] .
In addition, according to the Liang et al., and Fan W. et al., the formation of Ti-O-C chemical bonding in the graphene-TiO2 composites lead to control the morphology of TiO2 nanoparticles on the graphene sheets [21] [22] . The best formation of Ti-O-C chemical bonding in (H1) caused it has the best morphology (less agglomerate and high crystallinity). The (H1) composite also shows the best crystallinity and smallest crystallite size with ~42 nm compare to the other composites, (H2) with ~107 nm and (S) with ~86 nm. The smallest crystal size of (H1) composite means it provide the biggest surface area which leads to the better photoreduction performance.
Even though this research study is only study two synthesis conditions, but it still means a lot to the wider photocatalyst field especially for this new rGO-TiO2 composite as a photocatalyst reduction of CO2 into CH4 applications. The synthesis method that we used to synthesis the (H1) is originally propose by us and not yet reported by previous researchers. This method only uses the GO powder, TBT powder and NaOH as a raw material. The NaOH and distilled water as the solvent prove that this method are green and environmentally friendly since it do not produce any acidic waste which can harm our environment after the synthesis process compare to the solvothermal method which need some acetic acid (HAc) as the solvent. This method also use a low equipment cost since it only need an autoclave for its simple experimental steps. This project could make a great contribution in investigating the best synthesizing method to synthesis a high efficient CCC composite via a green raw material, low equipment cost and simple experimental step.
4. ConclusionThe growth and properties of rGO-TiO2 composites which were synthesized by three different conditions: (S), (H1) and (H2) have been successfully studied. The effect of synthesizing method via solvothermal and hydrothermal methods was examined and analyzed by UV Vis and XRD. The results show that the samples had different growth, purity, crystallite size and band gap, leading to different photocatalyst performances. From the results obtained, the (H1) composite has a strongest interaction between TiO2 and rGO sheets in the composite due to its significant strong Ti-O-C peak and lowest band gap (2.60 eV) compared to the (H2) and (S). The intimate contact between the TiO2 and rGO may accelerate the transfer of photogenerated electrons on TiO2 to rGO and decelerate the recombination of charge carriers. The synthesis method and a pure TBT TiO2 are the main reasons of its better performance compared to other samples. Several characterizations are suggested in further work in order to strengthen these findings. The future characterizations are such as Field Emission Scanning Electron Microscopy (FESEM) to check the surface morphology, Electrochemical Impedance Spectroscopy (EIS) to check the electrical properties, Fluorescent spectrometer (PL) to check the recombination rate of the photogenerated electron-hole pairs and lastly the Gas Chromatograph (GC) to test the photo reduction and conversion. We believe that, this approach could help to produce a high grade of rGO-TiO2 at a large scale in the future due to its green and environmentally friendly raw material, low equipment cost and also simple and efficient experimental works.