# Enhanced Photocatalytic Activity of Reduced Graphene Oxide/Bismuth Sulfide Nanostructure Composites for the Degradation of Methylene Blue

Authors: Bayisa Meka Chufa; Bedasa Abdisa Gonfa; Teketel Yohannes Anshebo
Journal: Journal of Nanomaterials
 (2021)

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## Abstract

Today, the issue of the environment is the concern of scientists worldwide. Aside from developed countries, developing countries are revolutionizing their economy from agriculture to industries, aggravating the discharge of pollutants. Textile industries are the main sources of pollutant dyes such as methylene blue (MB). In this study, a simple and green synthesis method was used to manufacture a nanostructure heterogeneous photocatalyst, rGO-Bi2S3, for the degradation of MB. Bi2S3 and rGO were synthesized separately using Vernonia amygdalina (VA) plant extract. rGO-Bi2S3 was synthesized using a single-step refluxed hydrothermal method. The products were characterized by XRD, FT-IR, UV-Vis, DTA, TGA, and visual techniques. The comparative degradability degree of the dye under visible light irradiation with and without the presence of the catalyst was studied. The performance test results showed 99% degradation of MB in the presence and 7% in the absence of the catalyst under the same condition for the duration of 25 minutes. The durability and reusability tests for the catalyst were also studied for five cycles. The maximum decrease in the degradation capacity of the catalyst for the duration of 25 minutes was 0.5%. Hence, rGO-Bi2S3 is found to be the ideal material for the degradation of MB, for environmental protection.


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## Body

## 1. Introduction

Nanosized materials are materials exhibiting unique physical, chemical, mechanical, electrical, biological, and thermal properties than their bulk counter parts due to their high surface area, small particle size, and possible quantum confinement effects [1–3]. Semiconductor materials are solid materials having an energy band gap lying in between a conductor and an insulator. Semiconductor materials manufactured to the nanoscale shares the above described nanomaterial properties. The development of these materials necessitates the progress of sciences: chemistry, physics engineering, and technology of the materials [4, 5]. A bismuth sulfide nanostructure (Bi2S3) is a semiconductor material with unique features such as favorable energy band gap, high absorption coefficient, and environmentally friendly elemental composition than the other known semiconductor [6–8]. Bi2S3 has a direct narrow band gap energy of 1.34 eV and finds application in photodiode arrays, photovoltaic convertors, and thermoelectric cooling devices based on Peltier effects [4, 9–13].The 21st century is termed as the century of the environment [14]. The world population is growing at the fastest rate, and this resulted in the intensification of industrial activities which in turn resulted in the contamination of the environment. For instance, textile industries are the main sources of dyes, which are the top pollutants of water bodies [15–17], and Bi2S3 has been attracting significant attention of researchers owing to its interesting band gap in the photocatalysis application for water purification [18–20]. However, the small band gap of Bi2S3 is subjected to the risk of charge carrier recombination and inefficient light response range, but it is still very effective and efficient if composited with graphene-based nanomaterials, forming a heterojunction, which stabilizes the band gap and optimizes its light absorption range [21–23]. Heterojunctions play a great role in mitigating the aforementioned drawbacks [24–26].Different synthesis methods of Bi2S3 have been reported so far; however, many of them are chemical methods that discharge hazardous pollutants to the environment [19, 27]. Because of its nontoxicity, energy band gap, light absorption potential, and ease of fabrication, Bi2S3 has been the preferred and widely used semiconductor [28–30]. Hence, the safe, cheap, and simple synthesis method of Bi2S3 semiconductors should be devised by researchers.As indicated in many recent research works, different approaches such as constructing heterostructured photocatalysts for the charge separation efficiency and extending the light response range by coupling the suitable band gap structure of materials are the most promising to promote photocatalytic efficiency of Bi2S3 [31, 32]. Owing to their unique electronic properties for application of photovoltaic devices, graphene has attracted interest of researchers recently [31]. Graphene possesses properties such as a high specific surface area (2600 m2 g-1), electrical conductivity (550 S cm-1), electron mobility at room temperature (200,000 cm2 v-1 s-1), and current density up to six orders of magnitude higher than copper [33] which are important for the application of photocatalytic activities. Therefore, the combination of the delocalized electron-rich materials like rGO and semiconductor Bi2S3 to form the heterostructure nanocomposite rGO-Bi2S3 allows the stability of the band gap of the semiconductor and modifies the light harvesting capacity of the heterostructure [34, 35].In this work, we presented a cheap, simple, and green synthesis method of Bi2S3 using methanol extracted compounds of Vernonia amygdalina at a low temperature below 100°C. Bitter leaf (Vernonia amygdalina, VA) is a soft wood shrub tree commonly found naturally in tropical Africa and Asia. It is a promising plant in research and development and often used as a traditional medicine and for nutritional purposes [36, 37]. The plant extract was used as a capping agent for the stabilization of the product nanostructure. Graphene oxide (GO) was synthesized using the improved method with a slight modification, and it was reduced to produce reduced graphene oxide (rGO) by the green synthesis method. The rGO-Bi2S3 composite was synthesized from the mixture of rGO and Bi2S3 under a single-step refluxed hydrothermal method. This method of synthesis is a solution reaction-based approach. The hydrothermal autoclave reactor is used to carry the hydrothermal reaction at a high pressure and temperature [38]. The enhanced photocatalytic activity of Bi2S3 using rGO for the degradation of methylene blue (MB) was studied thoroughly. The durability and reusability of the heterogeneous catalyst were also explored exhaustively.


## 2. Materials and Methods

### 2.1. Materials

Thiourea (CH4N2S), bismuth chloride (BiCl3), methanol (99.8%), ethanol (98%), and distilled water were used directly as purchased without further treatment, and bitter leaf plant extract was synthesized in the lab. 100 microns of graphite powder (99.5% purity), sulfuric acid (98%), phosphoric acid (75%), hydrogen peroxide (35%), hydrochloric acid (37%), potassium permanganate (99.5%), barium chloride (99%), and deionized water were also used to synthesize the catalyst as rGO [39].


### 2.2. Synthesis of Bi2S3

1.5 g of bismuth chloride (BiCl3) and 1.2 g of thiourea (CH4N2S) were dissolved in 50 ml of distilled water each and mixed while continuously stirring using a heater with magnetic stirrer at 100°C. After 5 minutes of heating, add 10 ml of methanol extracted compounds of Vernonia amygdalina into the solution. Then, the mixture was set on indirect heating using a water bath under continuous stirring for six hours. Then finally, the black powder was obtained after being washed using distilled water and ethanol several times and oven dried at 60°C for 12 hours.


### 2.3. Synthesis of rGO

The green synthesis method was used to obtain the catalyst, rGO, by using a bitter leaf plant extract as a reducing agent. The leaf extract was prepared by taking 10 g of the ground powder and adding into a 500 ml borosilicate beaker. Then, 10 grams of the powder was dissolved in 100 ml of methanol, and the mixture was heated on a heater with a magnetic stirrer to the boiling point of methanol until the complete removal of the solvent. The hot solution was taken off and cooled naturally at room temperature. And then, the extract was filtered using Whatman number 1 filter paper. The resulting filtrates were further concentrated over a water bath at 40-50°C for solvent removal. The stock solutions of crude extracts were prepared, and desired working concentrations were made by appropriate techniques. The concentrated extracts were made ready and stored in a fridge at 4°C for further use. Then, a 1 : 10 ratio by volume of the extract-graphene oxide was mixed in a flask and heated at 70°C for an hour with continuous stirring using a magnetic stirrer. The jelly-like black solution was taken of the heater and cooled at room temperature. Then, the black structure floating in the clear solution was separated by Whatman number 1 filter paper and washed with distilled water several times. The black paste was dried in the oven at 50°C for 5 hours. The dried sample was finely ground and stored for further use [39].


### 2.4. Synthesis of Bi2S3-rGO Composite

All reagents used in this experiment were analytical grade and used directly without further purification. A simple hydrothermal rout under reflux was used to synthesize rGO-Bi2S3. 1.43 g of the Bi2S3 powder was thoroughly dissolved in 50 ml of distilled water, and 2 g of rGO was dissolved in the same volume of distilled water in a separate flask. Both mixtures were poured into a 500 ml beaker and sonicated for two hours at room temperature. Then, the mixture was heated under reflux at 100°C for 12 hours. The black precipitate was filtered by using Whatman number 1 filter paper and purified by washing with distilled water and ethanol several times. The black paste was dried into a black powder in an oven under 120°C for 18 hours.


### 2.5. Photocatalysis Study

The photocatalysts were prepared by a simple hydrothermal method, and its performance was tested against the degradation of methylene blue (MB) under visible light irradiation using a 500 W xenon lamp in the wavelength rangeλ>42nm. 125 ml of methylene blue and 5 mg of the catalyst rGO-Bi2S3 (1 : 25 ratios) were placed in a glass cup reactor (100 ml). The mixture was continuously stirred with ultrasonication for 30 minutes at room temperature to maintain the adsorption-desorption equilibrium. Then after, at a given time interval of irradiation, 5 ml of the reaction mixture liquid was taken out and placed in centrifuge tubes which were later on centrifuged to remove any residual catalyst. The centrifugation and washing of the reaction liquid were done repeatedly using ethanol and water. The UV-Vis spectroscopy analyses were done against the concentrations of residual MB to check the performance of the catalyst.


### 2.6. Characterization Techniques

The confirmations of the formation of reduced graphene oxide from graphene oxide and the spectral positions of Bi2S3-GO were determined by Fourier transform infrared spectroscopy (FTIR, Perkin Elmer, USA). GO-Bi2S3 and rGO pellet were prepared using KBr as a mulling agent, and the sample was analyzed in the range between 400 cm-1 and 4000 cm-1. X-ray diffraction (XRD) of Bi2S3, Bi2S3-GO, and rGO was recorded on a Panalytical PW 3040 X’Pert MPD X-ray diffractometer with Cu-Kα X-ray radiation sources at 40 keV and 30 mA. XRD spectra were recorded to determine the purity and crystallinity of the samples. The optical absorption property of rGO was examined by ultraviolet-visible spectroscopy (UV-Vis, SM, UV-1600 Maadab-India). The thermogravimetric-differential thermal analysis (TGA-DTA) was performed with a differential thermal analyzer (DTG-60H, Beijing, China). These tests were operated under a nitrogen atmosphere with a platinum cell at 50 ml/min flow rate.


## 2.1. Materials

Thiourea (CH4N2S), bismuth chloride (BiCl3), methanol (99.8%), ethanol (98%), and distilled water were used directly as purchased without further treatment, and bitter leaf plant extract was synthesized in the lab. 100 microns of graphite powder (99.5% purity), sulfuric acid (98%), phosphoric acid (75%), hydrogen peroxide (35%), hydrochloric acid (37%), potassium permanganate (99.5%), barium chloride (99%), and deionized water were also used to synthesize the catalyst as rGO [39].


## 2.2. Synthesis of Bi2S3

1.5 g of bismuth chloride (BiCl3) and 1.2 g of thiourea (CH4N2S) were dissolved in 50 ml of distilled water each and mixed while continuously stirring using a heater with magnetic stirrer at 100°C. After 5 minutes of heating, add 10 ml of methanol extracted compounds of Vernonia amygdalina into the solution. Then, the mixture was set on indirect heating using a water bath under continuous stirring for six hours. Then finally, the black powder was obtained after being washed using distilled water and ethanol several times and oven dried at 60°C for 12 hours.


## 2.3. Synthesis of rGO

The green synthesis method was used to obtain the catalyst, rGO, by using a bitter leaf plant extract as a reducing agent. The leaf extract was prepared by taking 10 g of the ground powder and adding into a 500 ml borosilicate beaker. Then, 10 grams of the powder was dissolved in 100 ml of methanol, and the mixture was heated on a heater with a magnetic stirrer to the boiling point of methanol until the complete removal of the solvent. The hot solution was taken off and cooled naturally at room temperature. And then, the extract was filtered using Whatman number 1 filter paper. The resulting filtrates were further concentrated over a water bath at 40-50°C for solvent removal. The stock solutions of crude extracts were prepared, and desired working concentrations were made by appropriate techniques. The concentrated extracts were made ready and stored in a fridge at 4°C for further use. Then, a 1 : 10 ratio by volume of the extract-graphene oxide was mixed in a flask and heated at 70°C for an hour with continuous stirring using a magnetic stirrer. The jelly-like black solution was taken of the heater and cooled at room temperature. Then, the black structure floating in the clear solution was separated by Whatman number 1 filter paper and washed with distilled water several times. The black paste was dried in the oven at 50°C for 5 hours. The dried sample was finely ground and stored for further use [39].


## 2.4. Synthesis of Bi2S3-rGO Composite

All reagents used in this experiment were analytical grade and used directly without further purification. A simple hydrothermal rout under reflux was used to synthesize rGO-Bi2S3. 1.43 g of the Bi2S3 powder was thoroughly dissolved in 50 ml of distilled water, and 2 g of rGO was dissolved in the same volume of distilled water in a separate flask. Both mixtures were poured into a 500 ml beaker and sonicated for two hours at room temperature. Then, the mixture was heated under reflux at 100°C for 12 hours. The black precipitate was filtered by using Whatman number 1 filter paper and purified by washing with distilled water and ethanol several times. The black paste was dried into a black powder in an oven under 120°C for 18 hours.


## 2.5. Photocatalysis Study

The photocatalysts were prepared by a simple hydrothermal method, and its performance was tested against the degradation of methylene blue (MB) under visible light irradiation using a 500 W xenon lamp in the wavelength rangeλ>42nm. 125 ml of methylene blue and 5 mg of the catalyst rGO-Bi2S3 (1 : 25 ratios) were placed in a glass cup reactor (100 ml). The mixture was continuously stirred with ultrasonication for 30 minutes at room temperature to maintain the adsorption-desorption equilibrium. Then after, at a given time interval of irradiation, 5 ml of the reaction mixture liquid was taken out and placed in centrifuge tubes which were later on centrifuged to remove any residual catalyst. The centrifugation and washing of the reaction liquid were done repeatedly using ethanol and water. The UV-Vis spectroscopy analyses were done against the concentrations of residual MB to check the performance of the catalyst.


## 2.6. Characterization Techniques

The confirmations of the formation of reduced graphene oxide from graphene oxide and the spectral positions of Bi2S3-GO were determined by Fourier transform infrared spectroscopy (FTIR, Perkin Elmer, USA). GO-Bi2S3 and rGO pellet were prepared using KBr as a mulling agent, and the sample was analyzed in the range between 400 cm-1 and 4000 cm-1. X-ray diffraction (XRD) of Bi2S3, Bi2S3-GO, and rGO was recorded on a Panalytical PW 3040 X’Pert MPD X-ray diffractometer with Cu-Kα X-ray radiation sources at 40 keV and 30 mA. XRD spectra were recorded to determine the purity and crystallinity of the samples. The optical absorption property of rGO was examined by ultraviolet-visible spectroscopy (UV-Vis, SM, UV-1600 Maadab-India). The thermogravimetric-differential thermal analysis (TGA-DTA) was performed with a differential thermal analyzer (DTG-60H, Beijing, China). These tests were operated under a nitrogen atmosphere with a platinum cell at 50 ml/min flow rate.


## 3. Result and Discussion

### 3.1. Synthesis of Bi2S3

#### 3.1.1. Visual Observations

As can be seen in Figure1, three different colors (a, b, and c) were dominantly displayed during the stepwise synthesis of bismuth sulfide. Immediately as the solutions of white crystalline salt BiCl3 and the white fine powder CH4N2S were mixed, a corn yellow-colored solution was formed as indicated in Figure 1(a). This is the initial step and indication of the generation of sulfide ion as a result of hydrolysis reaction by the action of OH- in the aqueous solution as shown by the following equation [40]:
(1)NH22CS+2H2O⟶2NH3+2CO32−+S2−+2H2OFigure 1
The color change observed during the stepwise synthesis of bismuth sulfide.
(a)(b)(c)(d)(e)Upon the addition ofVernonia amygdalina plant extract and heating under continuous stirring, the deep black color was formed as shown in Figure 1(c), through the royal yellow color solution (Figure 1(b)). The brown oily supernatant (Figure 1(d)) was decanted, and a black paste was collected from which the black powder was obtained by oven drying at 100°C overnight as depicted in Figure 1(d).


#### 3.1.2. X-Ray Diffraction (XRD)

Figure2 shows the XRD patterns of the as-synthesized Bi2S3 nanostructure. All the reflections in the diffraction peaks can be indexed as the orthorhombic structured Bi2S3 with lattice constants (of standard data) a=11.150A, b=11.303A, and c=3.981A (JCPDS No. 17-0320). The intensities and positions of the peaks are in good agreement with literature values [7, 8, 28]. Some of the major peaks are ascribed to 020, 120, 220, 101, 130, 021, 211, 221, 301, and 311 facets, etc.Figure 2
XRD pattern of Bi2S3 synthesized from CH4N2S and BiCl3 sources.


#### 3.1.3. Thermal Analysis

Figure1 shows the DTA and TGA curves of the Bi2S3 single crystal run from 0 to 1000 K under N2 gas atmosphere. As can be seen from the graph of TGA in Figure 3, the sample is slightly stable for the temperature range of 0 to 680 K with a weight loss of ~1-2% due to the decomposition of some compounds. The significant decomposition of the material with a severe weight loss was observed at around 700 K increasing continuously with rising temperature up to 1000 K. The maximum weight loss recorded at 1000 K is 21% [41, 42]. This weight loss is attributed to the decomposition of sulfur dioxide (SO2), and the remaining product finally turns into Bi2O3 residue which is confirmed from DTA analysis (Figure 3) that gives the endothermic peak at around 910 K. Following the severe weight loss at 700-1000 K, two exothermic peaks and two endothermic peaks were observed from the DTA curve. The maximum endothermic peak at around 910 K means that this temperature is the melting point of Bi2S3 which is supposed to be reduced from 1036 K due to the lowered particle size to the nanoscale.Figure 3
DTA (left side) and TGA (right side) curves of single crystal Bi2S3.


### 3.2. Synthesis of Reduced Graphene Oxide (rGO)

#### 3.2.1. Visual Observations

As shown in Figures4(a)–4(c), three main different colors were observed during the stepwise synthesis of rGO. The dark green-colored thick solution as shown in Figure 4(a) is due to the formation of the high oxidizing agent dimanganese heptoxide (Mn2O7) [43, 44] from the reaction of MnO+3 and MnO-4, and in the meanwhile, the temperature of the solution was increased to 45°C.Figure 4
Different colors observed during the stepwise synthesis of rGO.
(a)(b)(c)(d)The brown color as indicated in Figure4(b) was obtained which is one of the confirmations of the formation of the graphene oxide nanostructure. The dark black suspension formed as shown in Figure 4(c) is the sign of GO reduction to produce rGO. The image of powders depicted in Figure 4(d) is rGO.


#### 3.2.2. UV-Vis

As a result of the reduction reaction, GO is deoxygenated and converted into rGO. Less amount of oxygen is detected on rGO, and this is confirmed by the red shift of the peak as shown in Figure5. Hence, there is a less number of n−π∗ transition in rGO which corresponds to the transition due C=O which is very low on rGO. This product is later used to synthesize the bismuth sulfide-reduced graphene oxide nanostructure composite.Figure 5
UV-Vis spectra record of rGO.The chromatograph profile of the heterostructure rGO-Bi2S3 recorded by GC-MS is shown in Figure6. It revealed to be a complex mixture of compounds. The interpretation of the GC-MS spectrum was done based on the NIST library.Figure 6
GC-MS chromatogram of rGO-Bi2S3.In the UV-Vis analysis of Bi2S3 and rGO-Bi2S3 as shown in Figure 7, the peak observed at around 400 and 680 λ due to sulfide and bismuth disappeared in the case of the heterostructure composite.Figure 7
UV-Vis spectra record of Bi2S3 and rGO-Bi2S3.


#### 3.2.3. XRD

Besides the structural arrangement, the X-RD characterization technique is used to monitor the extent of oxidation and purity of the material under examination. As shown in Figure8, a peak was observed at around 2θ=43° in rGO which resulted due to the crystal structure from basal planes slipping out of the alignments. With the green reduction using methanol extracts of Vernonia amygdalina (in Afaan Oromo, it is called Dhebicha) of GO to produce graphene/(rGO), there was a shift in the d-spacing and 2θ values to 0.36 nm and 24.5°, respectively, and this result confirmed the successful reduction of GO to graphene/rGO. We have reported the synthesis and green reduction of GO using “Dhebicha” to rGO in our preceding work.Figure 8
X-ray diffraction pattern of rGO.


#### 3.2.4. FT-IR

As shown in Figure9, the structure of the prepared rGO was characterized using FT-IR spectroscopy. The FT-IR record displayed a broad stretching peak at 3408 cm-1 which was attributed to the –OH of the intercalated residual water molecules and the peak at 1634 cm-1 by the same molecules but due to bending vibration [44] disappeared in rGO. As the oxygen-containing functional groups were removed by the reducing agent, the characteristic absorption peaks of oxide groups decreased significantly, and the CO2 peak at around 2640 cm-1 vanished indicating the successful reduction of GO. The compounds obtained from Vernonia amygdalina (VA) by solvent extraction using methanol as a solvent were used to reduce GO to rGO. Most of the peaks related to carbonyl, carboxyl, and hydroxyl of water disappeared in the spectra of rGO. The sharp band formed at 1570 cm-1 was attributed to C=C stretching. The absorption peak formed at 1222 and 1051 cm-1 as a result of the stretching vibration of the epoxide and alkoxy (C-O) groups, respectively, in GO is not observed in rGO which is also the indicator of the successful reduction of GO. Hence, the FT-IR spectra record shown in Figure 7 confirms the complete reduction of GO to rGO, and the synthesized rGO was used to manufacture the rGO-Bi2S3 nanostructure composite for the decomposition of methylene blue in the presence of visible light irradiation.Figure 9
FT-IR spectra record of rGO obtained by reduction of GO by VA.


### 3.3. Bi2S3-rGO Synthesis

#### 3.3.1. XRD

Here, the powder X-ray diffraction (XRD) is used to determine the phase structure of the as-prepared rGO-Bi2S3 composite. Figure 10 shows the XRD patterns of rGO-Bi2S3 composites.Figure 10
XRD pattern of rGO-Bi2S3 nanostructure composite.The result obtained for rGO-Bi2S3 is similar to the XRD pattern of Bi2S3 which implies that the weak XRD spectra of rGO at 2θ=24.5° is shielded by the strong peak intensities of Bi2S3 at around 2θ=25°. The peaks observed at 2θ>40° in Bi2S3 disappeared in the case of composites but get relatively narrower which is attributed to the degree of crystallinity and purity of rGO-Bi2S3. As determined from TGA analysis, the amount of rGO in the composite is lower that its peak is dominated by the peak of Bi2S3. In Figure 11, the XRD results of Bi2S3 and rGO-Bi2S3 were stacked vertically to compare their crystallinity.Figure 11
XRD pattern of Bi2S3 and rGO-Bi2S3 stacked vertically.


#### 3.3.2. Thermal Analysis

From the differential thermogravimetric analysis result shown in Figure9 (black line), the oxidative decomposition temperature of rGO-Bi2S3 is 450 K. This value is less than the DTA value of pure rGO which is equal to 570 K [45]. The decomposition of rGO is enhanced when a metal sulfide is bonded to it because of the catalytic effects of the metal sulfide nanoparticles. Hence, the lower decomposition temperature of rGO in the composite is attributed to the catalytic effects of the Bi2S3 which confirms the anchoring of Bi2S3 to the surface of rGO to form the rGO-Bi2S3 composite. The decomposition peak observed from the DTA graph for rGO-Bi2S3 is 450 K. As can be seen from the TGA analysis of Bi2S3 (Figure 3), maximum decomposition of the materials started at 700 K which is much greater than the value for the composite rGO-Bi2S3 which is equal to 430 K (Figure 12, red line). The lowered decomposition temperature in the case of the composite is attributed to the presence of oxygen that favors the decomposition rate with low temperature.Figure 12
Thermal analysis results of rGO-Bi2S3 NSs composite.


#### 3.3.3. FT-IR

As shown in Figure13, the relatively smaller band unlike that of the broad peak in GO formed at 3460 cm-1 is attributed to the O-H functional group of the residual water stretching, and the band observed at 1640 cm-1 is due to the bending vibration of the same group [46]. The relatively wide absorption peak formed at 1090 cm-1 is attributed to the interaction between the rGO and the Bi2S3 nanostructure composite [47].Figure 13
FT-IR spectral records of the composite NSs and rGO-Bi2S3.


### 3.4. Photocatalytic Activity

#### 3.4.1. Photocatalytic Degradation of Methylene Blue

One of the organic dyes most extensively used in almost all textile industries is methylene blue (MB), but it often pollutes the environment [48]. Thus, in this study, we tried to examine the photocatalytic degradation performance of as-prepared rGO-Bi2S3 against this important as well as serious pollutant MB under simulated visible light irradiation. The photocatalytic degradation of methylene blue (MB) was investigated in the absence and presence of as-synthesized rGO-Bi2S3 composite nanostructure (NS) catalyst under visible light irradiation. As shown in Figure 11 in the photodegradation spectra of MB, there is no significant change observed in the intensity of MB in the absence of the catalyst. The maximum wavelength (λmax) of MB is 664 nm, and the red- and blueshifts were not observed with the prolonged irradiation in the absence of rGO-Bi2S3, but there was insignificant intensity change (with a maximum decrease of 7%) at 20 minutes. Hence, the dye does not degrade when exposed to the light in the absence of a catalyst. The decrease in the intensity of the spectra is not consistent with the time of irradiation in the absence of the catalyst as can be observed in Figure 14. Hence, the use of a catalyst is mandatory to degrade dyes to prevent pollution in the environment.Figure 14
Degradation tests of MB in the absence of the catalyst under visible light.It has been reported that graphene oxide (GO) significantly enhanced the efficiency of Bi2S3 in the degradation of dyes (methylene blue) [32]. As shown below in Figure 15, rGO displayed superior enhancement for the dye degradation in this study. The degradations started immediately as a 1 : 25 ratio of the catalyst-to-dye mixture was subjected to visible radiation. The study was carried for a total of 25 minutes.Figure 15
Degradation tests of MB in the presence of the catalyst under visible light.The maximum intensity of MB after 5 minutes of irradiation was decreased to 0.43561. The degradation efficiency was recorded to be 84%, 86%, 95%, 97%, and 99% at 5, 10, 15, 20, and 25 minutes, respectively. Hence, rGO-Bi2S3 is the best composite with 99% degradation efficiency. Figure 16 shows the degradation percentage of the pollutant versus the time taken. It is reported in many works that the activity of the photocatalyst depends on the separation and transfer of charge carriers generated by irradiation that provoke the formation of active species of hydroxyl (⋅OH) and superoxide (⋅O2-) radicals. These facilitate degradation of the organic pollutant adhered onto the photocatalyst surface [27, 49]. According to kinetics analysis, the photocatalytic degradation of organic pollutants obeys a Langmuir isotherm mechanisms and follows a quasi-first-order reaction with the photocatalytic degradation rate defined by the following equation:
(2)r=−dCtdt=KobsCt.Figure 16
The degradation of methylene blue under visible light irradiation with and without a catalyst at different time intervals.The durability and reusability are also another way of measuring the performance of a catalyst.The photocatalyst after each run was collected, washed with distilled water, dried at 80°C, and used for the successive new run. The photocatalytic activity of rGO-Bi2S3 nanostructure composites exhibited insignificant change (decrease) after running for five cycles as shown in Figure 17 for a 25-minute retention time, confirming that the potentials of rGO-Bi2S3 to be a stable catalyst that can be used several times.Figure 17
The cyclic degradation efficiency of rGO-Bi2S3 composite against MB.


### 3.5. Mechanism of Photodegradation of Dyes

The generation of the charge carriers (electron hole) by the semiconductor during irradiation by visible light was the initiator of the photodegradation reaction. The charge intertransfer mechanism through the rGO-Bi2S3 composite nanostructure during the degradation of the MB dye is shown in Figure 18. When the semiconductor is irradiated by sunlight, it generates an e--h+ pair which is stabilized by the electron acceptor rGO. This graphene material prevents the recombination of the charge carrier by accepting an electron from Bi2S3 favoring the continuous generation of the charge carrier. Reduced graphene oxide accepts the electron from the semiconductor by two different ways unlike GO. One is by using its peripheral residual oxygen and the second is by the positive polarity formed at its edges due to the delocalized electron on the materials.Figure 18
Mechanisms of Photodegradation by rGO-Bi2S3.rGO inhibits charge carrier recombination by reducing the band gap so that the energy absorption efficiency of rGO-Bi2S3 is increased which in turn results in the accelerated generation of the e--h+ pair. Therefore, with the effective separation of charge carriers upon the irradiation of the rGO-Bi2S3 composite with visible light, the continuously generated electrons participated in the decomposition of O2 and H2O2 to generate the active species such as O2⋅- and ⋅OH for the degradation of the dyes.


## 3.1. Synthesis of Bi2S3

### 3.1.1. Visual Observations

As can be seen in Figure1, three different colors (a, b, and c) were dominantly displayed during the stepwise synthesis of bismuth sulfide. Immediately as the solutions of white crystalline salt BiCl3 and the white fine powder CH4N2S were mixed, a corn yellow-colored solution was formed as indicated in Figure 1(a). This is the initial step and indication of the generation of sulfide ion as a result of hydrolysis reaction by the action of OH- in the aqueous solution as shown by the following equation [40]:
(1)NH22CS+2H2O⟶2NH3+2CO32−+S2−+2H2OFigure 1
The color change observed during the stepwise synthesis of bismuth sulfide.
(a)(b)(c)(d)(e)Upon the addition ofVernonia amygdalina plant extract and heating under continuous stirring, the deep black color was formed as shown in Figure 1(c), through the royal yellow color solution (Figure 1(b)). The brown oily supernatant (Figure 1(d)) was decanted, and a black paste was collected from which the black powder was obtained by oven drying at 100°C overnight as depicted in Figure 1(d).


### 3.1.2. X-Ray Diffraction (XRD)

Figure2 shows the XRD patterns of the as-synthesized Bi2S3 nanostructure. All the reflections in the diffraction peaks can be indexed as the orthorhombic structured Bi2S3 with lattice constants (of standard data) a=11.150A, b=11.303A, and c=3.981A (JCPDS No. 17-0320). The intensities and positions of the peaks are in good agreement with literature values [7, 8, 28]. Some of the major peaks are ascribed to 020, 120, 220, 101, 130, 021, 211, 221, 301, and 311 facets, etc.Figure 2
XRD pattern of Bi2S3 synthesized from CH4N2S and BiCl3 sources.


### 3.1.3. Thermal Analysis

Figure1 shows the DTA and TGA curves of the Bi2S3 single crystal run from 0 to 1000 K under N2 gas atmosphere. As can be seen from the graph of TGA in Figure 3, the sample is slightly stable for the temperature range of 0 to 680 K with a weight loss of ~1-2% due to the decomposition of some compounds. The significant decomposition of the material with a severe weight loss was observed at around 700 K increasing continuously with rising temperature up to 1000 K. The maximum weight loss recorded at 1000 K is 21% [41, 42]. This weight loss is attributed to the decomposition of sulfur dioxide (SO2), and the remaining product finally turns into Bi2O3 residue which is confirmed from DTA analysis (Figure 3) that gives the endothermic peak at around 910 K. Following the severe weight loss at 700-1000 K, two exothermic peaks and two endothermic peaks were observed from the DTA curve. The maximum endothermic peak at around 910 K means that this temperature is the melting point of Bi2S3 which is supposed to be reduced from 1036 K due to the lowered particle size to the nanoscale.Figure 3
DTA (left side) and TGA (right side) curves of single crystal Bi2S3.


## 3.1.1. Visual Observations

As can be seen in Figure1, three different colors (a, b, and c) were dominantly displayed during the stepwise synthesis of bismuth sulfide. Immediately as the solutions of white crystalline salt BiCl3 and the white fine powder CH4N2S were mixed, a corn yellow-colored solution was formed as indicated in Figure 1(a). This is the initial step and indication of the generation of sulfide ion as a result of hydrolysis reaction by the action of OH- in the aqueous solution as shown by the following equation [40]:
(1)NH22CS+2H2O⟶2NH3+2CO32−+S2−+2H2OFigure 1
The color change observed during the stepwise synthesis of bismuth sulfide.
(a)(b)(c)(d)(e)Upon the addition ofVernonia amygdalina plant extract and heating under continuous stirring, the deep black color was formed as shown in Figure 1(c), through the royal yellow color solution (Figure 1(b)). The brown oily supernatant (Figure 1(d)) was decanted, and a black paste was collected from which the black powder was obtained by oven drying at 100°C overnight as depicted in Figure 1(d).


## 3.1.2. X-Ray Diffraction (XRD)

Figure2 shows the XRD patterns of the as-synthesized Bi2S3 nanostructure. All the reflections in the diffraction peaks can be indexed as the orthorhombic structured Bi2S3 with lattice constants (of standard data) a=11.150A, b=11.303A, and c=3.981A (JCPDS No. 17-0320). The intensities and positions of the peaks are in good agreement with literature values [7, 8, 28]. Some of the major peaks are ascribed to 020, 120, 220, 101, 130, 021, 211, 221, 301, and 311 facets, etc.Figure 2
XRD pattern of Bi2S3 synthesized from CH4N2S and BiCl3 sources.


## 3.1.3. Thermal Analysis

Figure1 shows the DTA and TGA curves of the Bi2S3 single crystal run from 0 to 1000 K under N2 gas atmosphere. As can be seen from the graph of TGA in Figure 3, the sample is slightly stable for the temperature range of 0 to 680 K with a weight loss of ~1-2% due to the decomposition of some compounds. The significant decomposition of the material with a severe weight loss was observed at around 700 K increasing continuously with rising temperature up to 1000 K. The maximum weight loss recorded at 1000 K is 21% [41, 42]. This weight loss is attributed to the decomposition of sulfur dioxide (SO2), and the remaining product finally turns into Bi2O3 residue which is confirmed from DTA analysis (Figure 3) that gives the endothermic peak at around 910 K. Following the severe weight loss at 700-1000 K, two exothermic peaks and two endothermic peaks were observed from the DTA curve. The maximum endothermic peak at around 910 K means that this temperature is the melting point of Bi2S3 which is supposed to be reduced from 1036 K due to the lowered particle size to the nanoscale.Figure 3
DTA (left side) and TGA (right side) curves of single crystal Bi2S3.


## 3.2. Synthesis of Reduced Graphene Oxide (rGO)

### 3.2.1. Visual Observations

As shown in Figures4(a)–4(c), three main different colors were observed during the stepwise synthesis of rGO. The dark green-colored thick solution as shown in Figure 4(a) is due to the formation of the high oxidizing agent dimanganese heptoxide (Mn2O7) [43, 44] from the reaction of MnO+3 and MnO-4, and in the meanwhile, the temperature of the solution was increased to 45°C.Figure 4
Different colors observed during the stepwise synthesis of rGO.
(a)(b)(c)(d)The brown color as indicated in Figure4(b) was obtained which is one of the confirmations of the formation of the graphene oxide nanostructure. The dark black suspension formed as shown in Figure 4(c) is the sign of GO reduction to produce rGO. The image of powders depicted in Figure 4(d) is rGO.


### 3.2.2. UV-Vis

As a result of the reduction reaction, GO is deoxygenated and converted into rGO. Less amount of oxygen is detected on rGO, and this is confirmed by the red shift of the peak as shown in Figure5. Hence, there is a less number of n−π∗ transition in rGO which corresponds to the transition due C=O which is very low on rGO. This product is later used to synthesize the bismuth sulfide-reduced graphene oxide nanostructure composite.Figure 5
UV-Vis spectra record of rGO.The chromatograph profile of the heterostructure rGO-Bi2S3 recorded by GC-MS is shown in Figure6. It revealed to be a complex mixture of compounds. The interpretation of the GC-MS spectrum was done based on the NIST library.Figure 6
GC-MS chromatogram of rGO-Bi2S3.In the UV-Vis analysis of Bi2S3 and rGO-Bi2S3 as shown in Figure 7, the peak observed at around 400 and 680 λ due to sulfide and bismuth disappeared in the case of the heterostructure composite.Figure 7
UV-Vis spectra record of Bi2S3 and rGO-Bi2S3.


### 3.2.3. XRD

Besides the structural arrangement, the X-RD characterization technique is used to monitor the extent of oxidation and purity of the material under examination. As shown in Figure8, a peak was observed at around 2θ=43° in rGO which resulted due to the crystal structure from basal planes slipping out of the alignments. With the green reduction using methanol extracts of Vernonia amygdalina (in Afaan Oromo, it is called Dhebicha) of GO to produce graphene/(rGO), there was a shift in the d-spacing and 2θ values to 0.36 nm and 24.5°, respectively, and this result confirmed the successful reduction of GO to graphene/rGO. We have reported the synthesis and green reduction of GO using “Dhebicha” to rGO in our preceding work.Figure 8
X-ray diffraction pattern of rGO.


### 3.2.4. FT-IR

As shown in Figure9, the structure of the prepared rGO was characterized using FT-IR spectroscopy. The FT-IR record displayed a broad stretching peak at 3408 cm-1 which was attributed to the –OH of the intercalated residual water molecules and the peak at 1634 cm-1 by the same molecules but due to bending vibration [44] disappeared in rGO. As the oxygen-containing functional groups were removed by the reducing agent, the characteristic absorption peaks of oxide groups decreased significantly, and the CO2 peak at around 2640 cm-1 vanished indicating the successful reduction of GO. The compounds obtained from Vernonia amygdalina (VA) by solvent extraction using methanol as a solvent were used to reduce GO to rGO. Most of the peaks related to carbonyl, carboxyl, and hydroxyl of water disappeared in the spectra of rGO. The sharp band formed at 1570 cm-1 was attributed to C=C stretching. The absorption peak formed at 1222 and 1051 cm-1 as a result of the stretching vibration of the epoxide and alkoxy (C-O) groups, respectively, in GO is not observed in rGO which is also the indicator of the successful reduction of GO. Hence, the FT-IR spectra record shown in Figure 7 confirms the complete reduction of GO to rGO, and the synthesized rGO was used to manufacture the rGO-Bi2S3 nanostructure composite for the decomposition of methylene blue in the presence of visible light irradiation.Figure 9
FT-IR spectra record of rGO obtained by reduction of GO by VA.


## 3.2.1. Visual Observations

As shown in Figures4(a)–4(c), three main different colors were observed during the stepwise synthesis of rGO. The dark green-colored thick solution as shown in Figure 4(a) is due to the formation of the high oxidizing agent dimanganese heptoxide (Mn2O7) [43, 44] from the reaction of MnO+3 and MnO-4, and in the meanwhile, the temperature of the solution was increased to 45°C.Figure 4
Different colors observed during the stepwise synthesis of rGO.
(a)(b)(c)(d)The brown color as indicated in Figure4(b) was obtained which is one of the confirmations of the formation of the graphene oxide nanostructure. The dark black suspension formed as shown in Figure 4(c) is the sign of GO reduction to produce rGO. The image of powders depicted in Figure 4(d) is rGO.


## 3.2.2. UV-Vis

As a result of the reduction reaction, GO is deoxygenated and converted into rGO. Less amount of oxygen is detected on rGO, and this is confirmed by the red shift of the peak as shown in Figure5. Hence, there is a less number of n−π∗ transition in rGO which corresponds to the transition due C=O which is very low on rGO. This product is later used to synthesize the bismuth sulfide-reduced graphene oxide nanostructure composite.Figure 5
UV-Vis spectra record of rGO.The chromatograph profile of the heterostructure rGO-Bi2S3 recorded by GC-MS is shown in Figure6. It revealed to be a complex mixture of compounds. The interpretation of the GC-MS spectrum was done based on the NIST library.Figure 6
GC-MS chromatogram of rGO-Bi2S3.In the UV-Vis analysis of Bi2S3 and rGO-Bi2S3 as shown in Figure 7, the peak observed at around 400 and 680 λ due to sulfide and bismuth disappeared in the case of the heterostructure composite.Figure 7
UV-Vis spectra record of Bi2S3 and rGO-Bi2S3.


## 3.2.3. XRD

Besides the structural arrangement, the X-RD characterization technique is used to monitor the extent of oxidation and purity of the material under examination. As shown in Figure8, a peak was observed at around 2θ=43° in rGO which resulted due to the crystal structure from basal planes slipping out of the alignments. With the green reduction using methanol extracts of Vernonia amygdalina (in Afaan Oromo, it is called Dhebicha) of GO to produce graphene/(rGO), there was a shift in the d-spacing and 2θ values to 0.36 nm and 24.5°, respectively, and this result confirmed the successful reduction of GO to graphene/rGO. We have reported the synthesis and green reduction of GO using “Dhebicha” to rGO in our preceding work.Figure 8
X-ray diffraction pattern of rGO.


## 3.2.4. FT-IR

As shown in Figure9, the structure of the prepared rGO was characterized using FT-IR spectroscopy. The FT-IR record displayed a broad stretching peak at 3408 cm-1 which was attributed to the –OH of the intercalated residual water molecules and the peak at 1634 cm-1 by the same molecules but due to bending vibration [44] disappeared in rGO. As the oxygen-containing functional groups were removed by the reducing agent, the characteristic absorption peaks of oxide groups decreased significantly, and the CO2 peak at around 2640 cm-1 vanished indicating the successful reduction of GO. The compounds obtained from Vernonia amygdalina (VA) by solvent extraction using methanol as a solvent were used to reduce GO to rGO. Most of the peaks related to carbonyl, carboxyl, and hydroxyl of water disappeared in the spectra of rGO. The sharp band formed at 1570 cm-1 was attributed to C=C stretching. The absorption peak formed at 1222 and 1051 cm-1 as a result of the stretching vibration of the epoxide and alkoxy (C-O) groups, respectively, in GO is not observed in rGO which is also the indicator of the successful reduction of GO. Hence, the FT-IR spectra record shown in Figure 7 confirms the complete reduction of GO to rGO, and the synthesized rGO was used to manufacture the rGO-Bi2S3 nanostructure composite for the decomposition of methylene blue in the presence of visible light irradiation.Figure 9
FT-IR spectra record of rGO obtained by reduction of GO by VA.


## 3.3. Bi2S3-rGO Synthesis

### 3.3.1. XRD

Here, the powder X-ray diffraction (XRD) is used to determine the phase structure of the as-prepared rGO-Bi2S3 composite. Figure 10 shows the XRD patterns of rGO-Bi2S3 composites.Figure 10
XRD pattern of rGO-Bi2S3 nanostructure composite.The result obtained for rGO-Bi2S3 is similar to the XRD pattern of Bi2S3 which implies that the weak XRD spectra of rGO at 2θ=24.5° is shielded by the strong peak intensities of Bi2S3 at around 2θ=25°. The peaks observed at 2θ>40° in Bi2S3 disappeared in the case of composites but get relatively narrower which is attributed to the degree of crystallinity and purity of rGO-Bi2S3. As determined from TGA analysis, the amount of rGO in the composite is lower that its peak is dominated by the peak of Bi2S3. In Figure 11, the XRD results of Bi2S3 and rGO-Bi2S3 were stacked vertically to compare their crystallinity.Figure 11
XRD pattern of Bi2S3 and rGO-Bi2S3 stacked vertically.


### 3.3.2. Thermal Analysis

From the differential thermogravimetric analysis result shown in Figure9 (black line), the oxidative decomposition temperature of rGO-Bi2S3 is 450 K. This value is less than the DTA value of pure rGO which is equal to 570 K [45]. The decomposition of rGO is enhanced when a metal sulfide is bonded to it because of the catalytic effects of the metal sulfide nanoparticles. Hence, the lower decomposition temperature of rGO in the composite is attributed to the catalytic effects of the Bi2S3 which confirms the anchoring of Bi2S3 to the surface of rGO to form the rGO-Bi2S3 composite. The decomposition peak observed from the DTA graph for rGO-Bi2S3 is 450 K. As can be seen from the TGA analysis of Bi2S3 (Figure 3), maximum decomposition of the materials started at 700 K which is much greater than the value for the composite rGO-Bi2S3 which is equal to 430 K (Figure 12, red line). The lowered decomposition temperature in the case of the composite is attributed to the presence of oxygen that favors the decomposition rate with low temperature.Figure 12
Thermal analysis results of rGO-Bi2S3 NSs composite.


### 3.3.3. FT-IR

As shown in Figure13, the relatively smaller band unlike that of the broad peak in GO formed at 3460 cm-1 is attributed to the O-H functional group of the residual water stretching, and the band observed at 1640 cm-1 is due to the bending vibration of the same group [46]. The relatively wide absorption peak formed at 1090 cm-1 is attributed to the interaction between the rGO and the Bi2S3 nanostructure composite [47].Figure 13
FT-IR spectral records of the composite NSs and rGO-Bi2S3.


## 3.3.1. XRD

Here, the powder X-ray diffraction (XRD) is used to determine the phase structure of the as-prepared rGO-Bi2S3 composite. Figure 10 shows the XRD patterns of rGO-Bi2S3 composites.Figure 10
XRD pattern of rGO-Bi2S3 nanostructure composite.The result obtained for rGO-Bi2S3 is similar to the XRD pattern of Bi2S3 which implies that the weak XRD spectra of rGO at 2θ=24.5° is shielded by the strong peak intensities of Bi2S3 at around 2θ=25°. The peaks observed at 2θ>40° in Bi2S3 disappeared in the case of composites but get relatively narrower which is attributed to the degree of crystallinity and purity of rGO-Bi2S3. As determined from TGA analysis, the amount of rGO in the composite is lower that its peak is dominated by the peak of Bi2S3. In Figure 11, the XRD results of Bi2S3 and rGO-Bi2S3 were stacked vertically to compare their crystallinity.Figure 11
XRD pattern of Bi2S3 and rGO-Bi2S3 stacked vertically.


## 3.3.2. Thermal Analysis

From the differential thermogravimetric analysis result shown in Figure9 (black line), the oxidative decomposition temperature of rGO-Bi2S3 is 450 K. This value is less than the DTA value of pure rGO which is equal to 570 K [45]. The decomposition of rGO is enhanced when a metal sulfide is bonded to it because of the catalytic effects of the metal sulfide nanoparticles. Hence, the lower decomposition temperature of rGO in the composite is attributed to the catalytic effects of the Bi2S3 which confirms the anchoring of Bi2S3 to the surface of rGO to form the rGO-Bi2S3 composite. The decomposition peak observed from the DTA graph for rGO-Bi2S3 is 450 K. As can be seen from the TGA analysis of Bi2S3 (Figure 3), maximum decomposition of the materials started at 700 K which is much greater than the value for the composite rGO-Bi2S3 which is equal to 430 K (Figure 12, red line). The lowered decomposition temperature in the case of the composite is attributed to the presence of oxygen that favors the decomposition rate with low temperature.Figure 12
Thermal analysis results of rGO-Bi2S3 NSs composite.


## 3.3.3. FT-IR

As shown in Figure13, the relatively smaller band unlike that of the broad peak in GO formed at 3460 cm-1 is attributed to the O-H functional group of the residual water stretching, and the band observed at 1640 cm-1 is due to the bending vibration of the same group [46]. The relatively wide absorption peak formed at 1090 cm-1 is attributed to the interaction between the rGO and the Bi2S3 nanostructure composite [47].Figure 13
FT-IR spectral records of the composite NSs and rGO-Bi2S3.


## 3.4. Photocatalytic Activity

### 3.4.1. Photocatalytic Degradation of Methylene Blue

One of the organic dyes most extensively used in almost all textile industries is methylene blue (MB), but it often pollutes the environment [48]. Thus, in this study, we tried to examine the photocatalytic degradation performance of as-prepared rGO-Bi2S3 against this important as well as serious pollutant MB under simulated visible light irradiation. The photocatalytic degradation of methylene blue (MB) was investigated in the absence and presence of as-synthesized rGO-Bi2S3 composite nanostructure (NS) catalyst under visible light irradiation. As shown in Figure 11 in the photodegradation spectra of MB, there is no significant change observed in the intensity of MB in the absence of the catalyst. The maximum wavelength (λmax) of MB is 664 nm, and the red- and blueshifts were not observed with the prolonged irradiation in the absence of rGO-Bi2S3, but there was insignificant intensity change (with a maximum decrease of 7%) at 20 minutes. Hence, the dye does not degrade when exposed to the light in the absence of a catalyst. The decrease in the intensity of the spectra is not consistent with the time of irradiation in the absence of the catalyst as can be observed in Figure 14. Hence, the use of a catalyst is mandatory to degrade dyes to prevent pollution in the environment.Figure 14
Degradation tests of MB in the absence of the catalyst under visible light.It has been reported that graphene oxide (GO) significantly enhanced the efficiency of Bi2S3 in the degradation of dyes (methylene blue) [32]. As shown below in Figure 15, rGO displayed superior enhancement for the dye degradation in this study. The degradations started immediately as a 1 : 25 ratio of the catalyst-to-dye mixture was subjected to visible radiation. The study was carried for a total of 25 minutes.Figure 15
Degradation tests of MB in the presence of the catalyst under visible light.The maximum intensity of MB after 5 minutes of irradiation was decreased to 0.43561. The degradation efficiency was recorded to be 84%, 86%, 95%, 97%, and 99% at 5, 10, 15, 20, and 25 minutes, respectively. Hence, rGO-Bi2S3 is the best composite with 99% degradation efficiency. Figure 16 shows the degradation percentage of the pollutant versus the time taken. It is reported in many works that the activity of the photocatalyst depends on the separation and transfer of charge carriers generated by irradiation that provoke the formation of active species of hydroxyl (⋅OH) and superoxide (⋅O2-) radicals. These facilitate degradation of the organic pollutant adhered onto the photocatalyst surface [27, 49]. According to kinetics analysis, the photocatalytic degradation of organic pollutants obeys a Langmuir isotherm mechanisms and follows a quasi-first-order reaction with the photocatalytic degradation rate defined by the following equation:
(2)r=−dCtdt=KobsCt.Figure 16
The degradation of methylene blue under visible light irradiation with and without a catalyst at different time intervals.The durability and reusability are also another way of measuring the performance of a catalyst.The photocatalyst after each run was collected, washed with distilled water, dried at 80°C, and used for the successive new run. The photocatalytic activity of rGO-Bi2S3 nanostructure composites exhibited insignificant change (decrease) after running for five cycles as shown in Figure 17 for a 25-minute retention time, confirming that the potentials of rGO-Bi2S3 to be a stable catalyst that can be used several times.Figure 17
The cyclic degradation efficiency of rGO-Bi2S3 composite against MB.


## 3.4.1. Photocatalytic Degradation of Methylene Blue

One of the organic dyes most extensively used in almost all textile industries is methylene blue (MB), but it often pollutes the environment [48]. Thus, in this study, we tried to examine the photocatalytic degradation performance of as-prepared rGO-Bi2S3 against this important as well as serious pollutant MB under simulated visible light irradiation. The photocatalytic degradation of methylene blue (MB) was investigated in the absence and presence of as-synthesized rGO-Bi2S3 composite nanostructure (NS) catalyst under visible light irradiation. As shown in Figure 11 in the photodegradation spectra of MB, there is no significant change observed in the intensity of MB in the absence of the catalyst. The maximum wavelength (λmax) of MB is 664 nm, and the red- and blueshifts were not observed with the prolonged irradiation in the absence of rGO-Bi2S3, but there was insignificant intensity change (with a maximum decrease of 7%) at 20 minutes. Hence, the dye does not degrade when exposed to the light in the absence of a catalyst. The decrease in the intensity of the spectra is not consistent with the time of irradiation in the absence of the catalyst as can be observed in Figure 14. Hence, the use of a catalyst is mandatory to degrade dyes to prevent pollution in the environment.Figure 14
Degradation tests of MB in the absence of the catalyst under visible light.It has been reported that graphene oxide (GO) significantly enhanced the efficiency of Bi2S3 in the degradation of dyes (methylene blue) [32]. As shown below in Figure 15, rGO displayed superior enhancement for the dye degradation in this study. The degradations started immediately as a 1 : 25 ratio of the catalyst-to-dye mixture was subjected to visible radiation. The study was carried for a total of 25 minutes.Figure 15
Degradation tests of MB in the presence of the catalyst under visible light.The maximum intensity of MB after 5 minutes of irradiation was decreased to 0.43561. The degradation efficiency was recorded to be 84%, 86%, 95%, 97%, and 99% at 5, 10, 15, 20, and 25 minutes, respectively. Hence, rGO-Bi2S3 is the best composite with 99% degradation efficiency. Figure 16 shows the degradation percentage of the pollutant versus the time taken. It is reported in many works that the activity of the photocatalyst depends on the separation and transfer of charge carriers generated by irradiation that provoke the formation of active species of hydroxyl (⋅OH) and superoxide (⋅O2-) radicals. These facilitate degradation of the organic pollutant adhered onto the photocatalyst surface [27, 49]. According to kinetics analysis, the photocatalytic degradation of organic pollutants obeys a Langmuir isotherm mechanisms and follows a quasi-first-order reaction with the photocatalytic degradation rate defined by the following equation:
(2)r=−dCtdt=KobsCt.Figure 16
The degradation of methylene blue under visible light irradiation with and without a catalyst at different time intervals.The durability and reusability are also another way of measuring the performance of a catalyst.The photocatalyst after each run was collected, washed with distilled water, dried at 80°C, and used for the successive new run. The photocatalytic activity of rGO-Bi2S3 nanostructure composites exhibited insignificant change (decrease) after running for five cycles as shown in Figure 17 for a 25-minute retention time, confirming that the potentials of rGO-Bi2S3 to be a stable catalyst that can be used several times.Figure 17
The cyclic degradation efficiency of rGO-Bi2S3 composite against MB.


## 3.5. Mechanism of Photodegradation of Dyes

The generation of the charge carriers (electron hole) by the semiconductor during irradiation by visible light was the initiator of the photodegradation reaction. The charge intertransfer mechanism through the rGO-Bi2S3 composite nanostructure during the degradation of the MB dye is shown in Figure 18. When the semiconductor is irradiated by sunlight, it generates an e--h+ pair which is stabilized by the electron acceptor rGO. This graphene material prevents the recombination of the charge carrier by accepting an electron from Bi2S3 favoring the continuous generation of the charge carrier. Reduced graphene oxide accepts the electron from the semiconductor by two different ways unlike GO. One is by using its peripheral residual oxygen and the second is by the positive polarity formed at its edges due to the delocalized electron on the materials.Figure 18
Mechanisms of Photodegradation by rGO-Bi2S3.rGO inhibits charge carrier recombination by reducing the band gap so that the energy absorption efficiency of rGO-Bi2S3 is increased which in turn results in the accelerated generation of the e--h+ pair. Therefore, with the effective separation of charge carriers upon the irradiation of the rGO-Bi2S3 composite with visible light, the continuously generated electrons participated in the decomposition of O2 and H2O2 to generate the active species such as O2⋅- and ⋅OH for the degradation of the dyes.


## 4. Conclusions

The heterogeneous photocatalyst rGO-Bi2S3 was synthesized from Bi2S3 and rGO by a single-step refluxed hydrothermal method. Bi2S3 was synthesized from thiourea and bismuth chloride in the presence of methanol extracted VA. The reduction of GO to rGO was also done by using these multifunctional compounds obtained from VA by the methanol extraction method. All the synthesized materials were characterized, and their formations were confirmed. With two groups of samples, comparative studies were performed on the degradation rate of MB under visible light irradiation. Samples with and without the presence of the catalyst were considered. A group of samples with the presence of a catalyst were prepared by adding 5 mg of rGO-Bi2S3 to 125 ml of the MB (1 : 25) ratio and sonicated for 30 minutes to obtain the adsorption desorption equilibrium. After being subjected to visible light, 5 ml of the sample was taken at 5-minute intervals and collected in a centrifuge tube, which was later on centrifuged, and UV-Vis analysis was done for the performance test. 2%, 84%, 86%, 95%, 97%, and 99% degradations were recorded for 0, 5, 10, 15, 20, and 25 minutes, respectively. This degradation performance capacity is confirmed to be constant by repeating the test for five times, and the maximum average is 99% for a 25-minute retention time. The maximum degradation value recorded under visible light irradiation of MB in the absence of a catalyst was 7%. The reusability and durability test made confirmed that the catalyst can be reused continuously for several times without decrease in capacity. The catalyst regenerated from the solution by washing with distilled water several times was reused for catalysis of MB for five cycles with the insignificant decrease in the degradation capacity. From the result obtained, the maximum decrease in the degradation capacity by percent for a 25-minute retention time was 7%.



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*Source: 1309961-2021-09-15.xml*