# The Photocatalytic Oxidation of 4-Chlorophenol Using Bi2WO6 under Solar Light Irradiation

Authors: Lorean Madriz; José Tatá; Ronald Vargas
Journal: International Journal of Photochemistry
 (2014)

---

## Abstract

This report discusses the effects of the initial concentration of 4-chlorophenol (4-CP) on its solar light photoinduced oxidation/mineralization kinetics on Bi2WO6 catalyst. Photocatalytic degradation followed the Langmuir-Hinshelwood (L-H) mechanism. From the kinetic data the Langmuir adsorption equilibrium constant of 4-CP on the Bi2WO6 surface and the L-H maximum reaction rate for 4-CP oxidation have been evaluated. Chromatographic and spectroscopy studies show the presence of p-benzoquinone and maleic acid as the main reaction products; these compounds first increase and then decay until they disappear. Chemical oxygen demand (COD) and produced CO2 measurement show that photocatalytic mineralization of the phenolic compound was readily possible in a wide concentration range.


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## Body

## 1. Introduction

In recent years, a large number of investigations have focused on the development of visible light induced heterogeneous photocatalyst for its applications in solar energy conversion and environmental wastewater purification [1–4]. In this sense, efforts have been directed to developing nanostructures based on Bi2WO6, the simplest member in the Aurivillius family [5–10]. This compound was first studied by Kudo and Hijii [11] and Zou and coworkers [12]; their works revealed that Bi2WO6 could perform as an excellent photocatalytic material, because it presents enhanced activities for the oxidative water splitting reaction. As a result, the solar light photocatalytic degradation of many pollutants as rhodamine B [13], green malachite [14], benzene [15], and 2,4-dichlorofenoxiacetic acid (2,4-D) [16] has been studied.The photoinduced degradation of 4-chlorophenol (a water soluble hazardous material widely used in paper, pharmaceutical, pesticide, and coal industries) [17–19] with Bi2WO6 nanocatalysts under visible light irradiation has been tested [20, 21]. This method induces an important decrease in the organic load and toxicity of wastewater; however, these authors have considered that the photodegradation reaction follows first order kinetics [22], thus obtaining the overall oxidation rate constant from linear plots of ln
⁡
(
c
(
t
)
/
c
0
) versus t. Nonetheless, this constant does not describe each of the steps of the overall reaction mechanism; hence, its value will depend in general on the detailed conditions under which the experiments are carried out. However, less effort has been expended on measuring the kinetic parameters of environmental pollutant degradation and mineralization according to a heterogeneous catalysis model like Langmuir-Hinshelwood kinetics. Knowledge of these parameters permits investigators to establish the reaction mechanisms and optimal reaction conditions needed to properly describe the process for use in designing chemical reactors at large scales.In the present work, we discuss the kinetics of 4-CP solar light photoinduced oxidation/mineralization kinetics on Bi2WO6 catalyst. Our results show that mineralization kinetics of this phenolic compound is determined by their surface concentration according to the Langmuir-Hinshelwood mechanism. The kinetic parameters of this model are reported and mechanistic implications are discussed.


## 2. Material and Methods

### 2.1. Materials

The following reactants were used without further purification: 4-chlorophenol, C6H5OCl, 99%, Merck; bismuth (III) nitrate pentahydrate, Bi(NO3)3·5H2O, 99%, Merck; sodium tungstate dihydrate, Na2WO4·2H2O, 99%, Riedel de Häen; titanium dioxide, TiO2, Anatase, Riedel de Haën; potassium monobasic phosphoric acid, KH2PO4, 99%, Riedel de Haën; potassium dibasic phosphoric acid, K2HPO4, 98%, Riedel de Haën; potassium phosphate K3PO4·H2O, 95%, Riedel de Haën; sulfuric acid, H2SO4, 95–97%, Riedel de Haën; potassium dichromate, K2Cr2O7, 99.5%, Merck; potassium hydrogen phthalate, C8H5KO4, 99.5%, Riedel de Haën; mercury (II) sulfate, HgSO4, ≥99%, Merck; silver sulfate, Ag2SO4, ≥99%, Merck; water, H2O, 17.7 MΩ/cm, Nanopure.


### 2.2. Equipment

A Solar Light Co. solar light simulator with a 1000 W xenon lamp and the appropriate filters for producing solar light (290–900 nm) was used in the experiments. Solar light radiometer and Ocean Optics fiber optic spectrometer model S1024dw were used to determine the radiation intensity and simulated spectra during each trial. Solutions pH was recorded using a digital pH-meter, model P211, Hanna Instruments. Millipore filtration equipment with 0.05μm membrane filters was used to separate the photocatalyst from the sample solutions. A diode arrangement UV-Vis spectrophotometer by Hewlett Packard (model HP8452A) was used to obtain the 4-CP UV-Vis spectrum. Waters Association HPLC with model M6000A pump, Rheodyne injector, model 484 UV detector, and model 745B data recorder was used to identify the intermediates formed during the reaction.


### 2.3. Methods

#### 2.3.1. Synthesis and Characterization of the Bi2WO6 Photocatalyst

Bi2WO6 nanocrystals were fabricated according to the widely reported hydrothermal synthesis [6, 7, 13, 14, 23, 24]. As a typical process, aqueous solutions of Na2WO4·2H2O (5 mM) and Bi(NO3)3·5H2O (10 mM) were mixed together (maintained the 1 : 2 molar ratio) until they reached 200 mL. White precipitate appeared immediately and was put in ultrasonic bath for 10 min in order to complete the precipitation. The solution pH was adjusted to 7.0 and the final solution was added into a 300 mL stainless steel Parr autoclave; the experimental conditions were established in 160°C and 70 psig for 24 h. Then, the reactor was cooled to room-temperature naturally; the resulting sample was collected and washed with deionized water. Finally, the obtained powder was dried at 80°C in air.The characterization of the obtained photocatalyst according to the described procedure has been reported by our group; for details see [10, 25, 26]. The main results for the Bi2WO6 powder are nanocrystals with orthorhombic phase, semiconductor band gap energy of 2.55 eV, B.E.T. specific surface area of 48 m2/g, and internal pore diameter of 7 nm. These values are typically reported for the highly active bismuth tungstate photocatalytic materials [6, 7, 10, 13, 14, 23–26].


#### 2.3.2. Photocatalytic Oxidation of 4-Chlorophenol Using Bi2WO6 under Solar Light Irradiation

The photocatalytic probes for 4-CP degradation were evaluated in a well-mixed batch configuration. In a beaker of 600 mL with magnetic agitation, a suspension of 500 mL of 4-CP and phosphate buffer solution (pH = 7) with 100 mg L−1 of the Bi2WO6 photocatalyst was prepared. This suspension remained in the dark for 30 min in order to establish the reactant-Bi2WO6 adsorption/desorption equilibrium. After this time, the system was placed under solar simulator cannon (diameter ca. 20 cm) in such a way that the distance between the end of the cannon and the beaker was 15 cm. The simulator was turned on, and the reaction was monitored by taking aliquots (3 mL) at different times. The aliquots were filtered with Millipore membranes, and the UV-Vis spectrum of the filtered solution was recorded. 4-CP analytical quantification was performed with the UV-Vis spectroscopy. The UV-Vis spectra obtained for the multicomponent solution (reactant + products) were deconvoluted using Matlab v 7.0 software, and the concentrations of the different compounds present in solution were determined according to the Lambert-Beer law, with molar absorption coefficients at the wavelengths of maximum absorption for each compound [27]. Simulator radiation was measured with a radiometer. Values of 100(±5) mW cm−2 were typically measured for solar visible radiation. The temperature of the reactor was kept at 22(±1)°C by maintaining the temperature of the room where the simulator was located.


#### 2.3.3. Mineralization

Mineralization during 4-CP photocatalytic oxidation was followed by measuring the chemical oxygen demand (COD). In a typical reaction, aliquots (3 mL) were taken at different reaction times and the COD of each aliquot was measured with a colorimetric method [28, 29] in which the total organic sample content was oxidized for 2 h at 150°C in a closed system with sulfuric acid and potassium dichromate. The solution absorbance at 420 and 600 nm was then measured. From this absorbance, the solution COD was obtained from a potassium hydrogen phthalate calibration curve. Mineralization was confirmed by direct CO2 measurement using an OxyGuard portable dissolved CO2 analyzer based on nondispersive infrared spectrometry (NDIR).


#### 2.3.4. HPLC Studies

Liquid chromatography was carried out with a Waters Association HPLC system composed of a model M6000A pump, a Rheodyne injector, a model 484 UV detector, and a model 745B data recorder. Aμ Bondapack CN (RP) 3.9 mm × 150 mm column was used to determine the intermediaries, with 70/30 water/methanol solution as mobile phase, at 0.9 mL/min flow rate and 254 nm UV-Vis detection. Maleic acid was analysed with an Aminex HPX-87, 7.8 mm × 300 mm column, using 8 × 10−4 M sulphuric acid aqueous solution as mobile phase at 0.5 mL/min flow rate, with detection at 210 nm.


## 2.1. Materials

The following reactants were used without further purification: 4-chlorophenol, C6H5OCl, 99%, Merck; bismuth (III) nitrate pentahydrate, Bi(NO3)3·5H2O, 99%, Merck; sodium tungstate dihydrate, Na2WO4·2H2O, 99%, Riedel de Häen; titanium dioxide, TiO2, Anatase, Riedel de Haën; potassium monobasic phosphoric acid, KH2PO4, 99%, Riedel de Haën; potassium dibasic phosphoric acid, K2HPO4, 98%, Riedel de Haën; potassium phosphate K3PO4·H2O, 95%, Riedel de Haën; sulfuric acid, H2SO4, 95–97%, Riedel de Haën; potassium dichromate, K2Cr2O7, 99.5%, Merck; potassium hydrogen phthalate, C8H5KO4, 99.5%, Riedel de Haën; mercury (II) sulfate, HgSO4, ≥99%, Merck; silver sulfate, Ag2SO4, ≥99%, Merck; water, H2O, 17.7 MΩ/cm, Nanopure.


## 2.2. Equipment

A Solar Light Co. solar light simulator with a 1000 W xenon lamp and the appropriate filters for producing solar light (290–900 nm) was used in the experiments. Solar light radiometer and Ocean Optics fiber optic spectrometer model S1024dw were used to determine the radiation intensity and simulated spectra during each trial. Solutions pH was recorded using a digital pH-meter, model P211, Hanna Instruments. Millipore filtration equipment with 0.05μm membrane filters was used to separate the photocatalyst from the sample solutions. A diode arrangement UV-Vis spectrophotometer by Hewlett Packard (model HP8452A) was used to obtain the 4-CP UV-Vis spectrum. Waters Association HPLC with model M6000A pump, Rheodyne injector, model 484 UV detector, and model 745B data recorder was used to identify the intermediates formed during the reaction.


## 2.3. Methods

### 2.3.1. Synthesis and Characterization of the Bi2WO6 Photocatalyst

Bi2WO6 nanocrystals were fabricated according to the widely reported hydrothermal synthesis [6, 7, 13, 14, 23, 24]. As a typical process, aqueous solutions of Na2WO4·2H2O (5 mM) and Bi(NO3)3·5H2O (10 mM) were mixed together (maintained the 1 : 2 molar ratio) until they reached 200 mL. White precipitate appeared immediately and was put in ultrasonic bath for 10 min in order to complete the precipitation. The solution pH was adjusted to 7.0 and the final solution was added into a 300 mL stainless steel Parr autoclave; the experimental conditions were established in 160°C and 70 psig for 24 h. Then, the reactor was cooled to room-temperature naturally; the resulting sample was collected and washed with deionized water. Finally, the obtained powder was dried at 80°C in air.The characterization of the obtained photocatalyst according to the described procedure has been reported by our group; for details see [10, 25, 26]. The main results for the Bi2WO6 powder are nanocrystals with orthorhombic phase, semiconductor band gap energy of 2.55 eV, B.E.T. specific surface area of 48 m2/g, and internal pore diameter of 7 nm. These values are typically reported for the highly active bismuth tungstate photocatalytic materials [6, 7, 10, 13, 14, 23–26].


### 2.3.2. Photocatalytic Oxidation of 4-Chlorophenol Using Bi2WO6 under Solar Light Irradiation

The photocatalytic probes for 4-CP degradation were evaluated in a well-mixed batch configuration. In a beaker of 600 mL with magnetic agitation, a suspension of 500 mL of 4-CP and phosphate buffer solution (pH = 7) with 100 mg L−1 of the Bi2WO6 photocatalyst was prepared. This suspension remained in the dark for 30 min in order to establish the reactant-Bi2WO6 adsorption/desorption equilibrium. After this time, the system was placed under solar simulator cannon (diameter ca. 20 cm) in such a way that the distance between the end of the cannon and the beaker was 15 cm. The simulator was turned on, and the reaction was monitored by taking aliquots (3 mL) at different times. The aliquots were filtered with Millipore membranes, and the UV-Vis spectrum of the filtered solution was recorded. 4-CP analytical quantification was performed with the UV-Vis spectroscopy. The UV-Vis spectra obtained for the multicomponent solution (reactant + products) were deconvoluted using Matlab v 7.0 software, and the concentrations of the different compounds present in solution were determined according to the Lambert-Beer law, with molar absorption coefficients at the wavelengths of maximum absorption for each compound [27]. Simulator radiation was measured with a radiometer. Values of 100(±5) mW cm−2 were typically measured for solar visible radiation. The temperature of the reactor was kept at 22(±1)°C by maintaining the temperature of the room where the simulator was located.


### 2.3.3. Mineralization

Mineralization during 4-CP photocatalytic oxidation was followed by measuring the chemical oxygen demand (COD). In a typical reaction, aliquots (3 mL) were taken at different reaction times and the COD of each aliquot was measured with a colorimetric method [28, 29] in which the total organic sample content was oxidized for 2 h at 150°C in a closed system with sulfuric acid and potassium dichromate. The solution absorbance at 420 and 600 nm was then measured. From this absorbance, the solution COD was obtained from a potassium hydrogen phthalate calibration curve. Mineralization was confirmed by direct CO2 measurement using an OxyGuard portable dissolved CO2 analyzer based on nondispersive infrared spectrometry (NDIR).


### 2.3.4. HPLC Studies

Liquid chromatography was carried out with a Waters Association HPLC system composed of a model M6000A pump, a Rheodyne injector, a model 484 UV detector, and a model 745B data recorder. Aμ Bondapack CN (RP) 3.9 mm × 150 mm column was used to determine the intermediaries, with 70/30 water/methanol solution as mobile phase, at 0.9 mL/min flow rate and 254 nm UV-Vis detection. Maleic acid was analysed with an Aminex HPX-87, 7.8 mm × 300 mm column, using 8 × 10−4 M sulphuric acid aqueous solution as mobile phase at 0.5 mL/min flow rate, with detection at 210 nm.


## 2.3.1. Synthesis and Characterization of the Bi2WO6 Photocatalyst

Bi2WO6 nanocrystals were fabricated according to the widely reported hydrothermal synthesis [6, 7, 13, 14, 23, 24]. As a typical process, aqueous solutions of Na2WO4·2H2O (5 mM) and Bi(NO3)3·5H2O (10 mM) were mixed together (maintained the 1 : 2 molar ratio) until they reached 200 mL. White precipitate appeared immediately and was put in ultrasonic bath for 10 min in order to complete the precipitation. The solution pH was adjusted to 7.0 and the final solution was added into a 300 mL stainless steel Parr autoclave; the experimental conditions were established in 160°C and 70 psig for 24 h. Then, the reactor was cooled to room-temperature naturally; the resulting sample was collected and washed with deionized water. Finally, the obtained powder was dried at 80°C in air.The characterization of the obtained photocatalyst according to the described procedure has been reported by our group; for details see [10, 25, 26]. The main results for the Bi2WO6 powder are nanocrystals with orthorhombic phase, semiconductor band gap energy of 2.55 eV, B.E.T. specific surface area of 48 m2/g, and internal pore diameter of 7 nm. These values are typically reported for the highly active bismuth tungstate photocatalytic materials [6, 7, 10, 13, 14, 23–26].


## 2.3.2. Photocatalytic Oxidation of 4-Chlorophenol Using Bi2WO6 under Solar Light Irradiation

The photocatalytic probes for 4-CP degradation were evaluated in a well-mixed batch configuration. In a beaker of 600 mL with magnetic agitation, a suspension of 500 mL of 4-CP and phosphate buffer solution (pH = 7) with 100 mg L−1 of the Bi2WO6 photocatalyst was prepared. This suspension remained in the dark for 30 min in order to establish the reactant-Bi2WO6 adsorption/desorption equilibrium. After this time, the system was placed under solar simulator cannon (diameter ca. 20 cm) in such a way that the distance between the end of the cannon and the beaker was 15 cm. The simulator was turned on, and the reaction was monitored by taking aliquots (3 mL) at different times. The aliquots were filtered with Millipore membranes, and the UV-Vis spectrum of the filtered solution was recorded. 4-CP analytical quantification was performed with the UV-Vis spectroscopy. The UV-Vis spectra obtained for the multicomponent solution (reactant + products) were deconvoluted using Matlab v 7.0 software, and the concentrations of the different compounds present in solution were determined according to the Lambert-Beer law, with molar absorption coefficients at the wavelengths of maximum absorption for each compound [27]. Simulator radiation was measured with a radiometer. Values of 100(±5) mW cm−2 were typically measured for solar visible radiation. The temperature of the reactor was kept at 22(±1)°C by maintaining the temperature of the room where the simulator was located.


## 2.3.3. Mineralization

Mineralization during 4-CP photocatalytic oxidation was followed by measuring the chemical oxygen demand (COD). In a typical reaction, aliquots (3 mL) were taken at different reaction times and the COD of each aliquot was measured with a colorimetric method [28, 29] in which the total organic sample content was oxidized for 2 h at 150°C in a closed system with sulfuric acid and potassium dichromate. The solution absorbance at 420 and 600 nm was then measured. From this absorbance, the solution COD was obtained from a potassium hydrogen phthalate calibration curve. Mineralization was confirmed by direct CO2 measurement using an OxyGuard portable dissolved CO2 analyzer based on nondispersive infrared spectrometry (NDIR).


## 2.3.4. HPLC Studies

Liquid chromatography was carried out with a Waters Association HPLC system composed of a model M6000A pump, a Rheodyne injector, a model 484 UV detector, and a model 745B data recorder. Aμ Bondapack CN (RP) 3.9 mm × 150 mm column was used to determine the intermediaries, with 70/30 water/methanol solution as mobile phase, at 0.9 mL/min flow rate and 254 nm UV-Vis detection. Maleic acid was analysed with an Aminex HPX-87, 7.8 mm × 300 mm column, using 8 × 10−4 M sulphuric acid aqueous solution as mobile phase at 0.5 mL/min flow rate, with detection at 210 nm.


## 3. Results and Discussion

Figure1(a) shows that the degradation of 4-CP on Bi2WO6 under solar irradiation is able to generate a dramatic COD diminution of the wastewater. The total COD diminution implies that efficient conversion to CO2 occurred during solar irradiation. This result was confirmed by the direct measurement by NDIR of the CO2 produced during 30 mg L−1 of 4-CP photocatalytic oxidation; the final concentration of dissolved carbon dioxide (1.1
±
0.2 mM) corresponds very well with the predicted stoichiometrically assuming that all 4-CP was oxidized completely (1.4 mM). It should be noted that COD remains a constant value when the suspension is in the dark. Figure 1(b) shows the influence of the initial concentration of 4-CP on the diminution of the COD. It should be noted that the COD decrease is assessment in a wide range for the initial quantity of organic compound and follows a pseudo first order kinetic decay.(a) COD diminution during the photocatalytic oxidation of the 4-CP on Bi2WO6. (b) Effect of the initial concentration of 4-CP on COD diminution during the visible light photocatalytic oxidation of the 4-CP on Bi2WO6. (—) Pseudo first order kinetics decay.
(a)
(b)Figure2(a) shows deconvoluted UV-Vis spectra of 15 ppm of 4-CP, after 30 min of solar light irradiation in presence of 100 ppm of Bi2WO6 at neutral pH. It should be noted that the bands between 200–240 nm (I) and 260–300 nm (II) are associated with the starting compound, and the 4-CP absorption band with its maximum at 280 nm decreases continuously with the irradiation time. The band between 225 and 260 nm (III) increases as 4-CP is oxidized. This band arises from the oxidation of the phenolic compound to ap-benzoquinone compound. This has been reported as the principal reaction intermediate during oxidation of several phenolic compounds [27, 30, 31] and was verified with high performance liquid chromatography (HPLC). In general, the chromatographic and spectroscopy analysis indicated that the more stable intermediaries observed during the photooxidation of 4-CP are thep-benzoquinone (PBQ) and the maleic acid (MA), where in all intermediaries there was an increase in concentration at first and then they decreased until they disappeared (see Figure 2(b)). It should be noted that these compounds are the main intermediates reported during the reaction between 4-CP and hydroxyl radicals in other advanced photooxidation process like TiO2/UV [27, 31, 32]. However, these intermediates have UV spectra; therefore, to obtain the 4-CP concentration a determination involving numerical deconvolution of the spectra data according to the Lambert-Beer law for multicomponent mixtures is required [27]. Figure 2(b) showed the result obtained for the photocatalytic oxidation of 4-CP. The concentration of the initial compound decreases continuously until it reaches low values, and the concentration of the more stable intermediates (PBQ and MA) first increases and then decays.(a) Deconvoluted UV-Vis spectra of 15 ppm of 4-CP, after 30 min of solar light irradiation in presence of 100 mg/L of Bi2WO6 at neutral pH. Intensities of deconvoluted absorption bands ((—) 4-CP, (- - -) PBQ, and (– – –) MA). (b) Concentration versus irradiation time curves during the 4-CP degradation.
(a)
(b)Chromatographic and spectroscopy studies show that the mechanism of oxidative mineralization of phenolic compounds involves first the formation of highly toxic quinones and then the subsequent opening of the aromatic rings leading to formation of aliphatic acids and finally to carbon dioxide [27, 30, 31]. In Scheme 1, the principal oxidation reaction pathways (intermediates detected) during the 4-CP oxidation after the consecutive hydroxyl radicals attack are shown. However, chemical analysis indicated that at large irradiation time this intermediate is not accumulated leading to the completed mineralization of the initial 4-CP in solution.Scheme 1
Principal reaction pathways (intermediates detected) during the 4-CP oxidation after the consecutive hydroxyl radicals attack.According to many researchers [31, 33–38], the influence of the initial concentration of the solute on the photocatalytic degradation rate of the most organic compounds is described by the Langmuir-Hinshelwood model
(1)
r
=
k
K
C
(
1
+
K
C
+
∑
K
i
C
i
)
,
where r (mg L−1 min−1) is the reaction rate of disappearance of 4-CP, C (mg L−1) is the concentration of the organic compound, K (L mg−1) represents the equilibrium adsorption constant of the organic compound on the photocatalyst, and k  (mg L−1 min−1) reflects the limiting reaction rate at maximum coverage for the experimental conditions. In this case the 4-CP adsorbs fast at the Bi2WO6 and then reacts consecutively with the OH
∙, in order to produce the p-hydroquinone (PHQ), PBQ, MA, and finally CO2. As pointed out [35], the initial rate method should be used to validate the kinetic model, with assumption of no competition with reaction byproducts, because when t
→
0, it results in ∑
K
i
C
i
≪
1
+
K
4
-CP
C
4
-CP. Then the simplest representation for the initial rate of disappearance of 4-CP on Bi2WO6 is given by
(2)
r
0
=
k
K
C
0
(
1
+
K
C
0
)
.
The r
0 were determined by linear fit from the 4-CP concentration versus irradiation time curves at the initial times; then the L-H model was verified according to the linear representation of (2); that is, a plot of the inverse initial rate (1/r
0) as a function of the inverse initial concentration (1/C
0) should be linear.As indicated in Figure3, the 1/r
0 versus 1/C
0 plot yields a straight line. From the linear fit the L-H kinetic constants for the 4-CP photooxidation using Bi2WO6 under solar light irradiation arek = 0.78 mg L−1 min−1 andK = 0.02 L mg−1. In order to compare the kinetic efficiency of this system, the maximum value for the first order kinetic constant (k
obs
=
k
K) was estimated (for L-H model k
obs
=
k
K
/
(
1
+
K
C
) and if K
C
≪
1, the maximum k
obs becomeskK) [35]. In this work we find k
obs = 0.02 min−1 for 4-CP on Bi2WO6 + solar light and Theurich and coworkers report k
obs
=
0.08 min−1 for 4-CP on TiO2 + UV light [31]. It should be noted that the catalytic efficiency observed in Bi2WO6/solar light degradation of 4-chlorophenol is slightly lower but in the same order of magnitude for the well-known TiO2/UV advanced oxidation process. Therefore, the use of solar light makes the Bi2WO6 a promising material towards the decontamination of polluted water.Figure 3
Langmuir-Hinshelwood kinetic linear representation of the solar light photooxidation/mineralization of 4-CP on Bi2WO6. Inset: graphical representation of the L-H model. (◆) Experimental data and (—) equation (1) withk = 0.78 mg L−1 min−1,K = 0.02 L mg−1.


## 4. Conclusions

Photocatalytic degradation of 4-chlorophenol (4-CP) on Bi2WO6 under solar irradiation followed the Langmuir-Hinshelwood mechanism; the respective kinetic constants arek = 0.78 mg L−1 min−1 and K
=
0.02 L mg−1. Studies performed by several techniques show the presence ofp-benzoquinone and maleic acid as the main reaction products; these compounds disappear to form carbon dioxide. Chemical oxygen demand and produced CO2 measurements show that photocatalytic mineralization of the phenolic compound was readily possible in a wide concentration range. The results obtained for the solar light photoinduced oxidation/mineralization of 4-chlorophenol on Bi2WO6 catalyst demonstrate the use of this semiconductor as material potential for decontamination of polluted water take advantage of solar energy.



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*Source: 387536-2014-08-05.xml*