# Removal of Polyvinyl Alcohol Using Photoelectrochemical Oxidation Processes Based on Hydrogen Peroxide Electrogeneration

Authors: Kai-Yu Huang; Chih-Ta Wang; Wei-Lung Chou; Chi-Min Shu
Journal: International Journal of Photoenergy
 (2013)

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## Abstract

This study investigates the removal efficiency of PVA from aqueous solutions using UV irradiation in combination with the production of electrogenerated hydrogen peroxide (H2O2) at a polyacrylonitrile-based activated carbon fiber (ACF) cathode. Three cathode materials (i.e., platinum, graphite, and ACF) were fed with oxygen and used for the electrogeneration of H2O2. The amount of electrogenerated H2O2 produced using the ACF cathode was five times greater than that generated using the graphite cathode and nearly 24 times greater than that from platinum cathode. Several parameters were evaluated to characterize the H2O2 electrogeneration, such as current density, oxygen flow rate, solution pH, and the supporting electrolyte used. The optimum current density, oxygen flow rate, solution pH, and supporting electrolyte composition were found to be 10 mA cm−2, 500 cm3 min−1, pH 3, and Na2SO4, respectively. The PVA removal efficiencies were achieved under these conditions 3%, 16%, and 86% using UV, H2O2 electrogeneration, and UV/H2O2 electrogeneration, respectively. A UV light intensity of 0.6 mW cm−2 was found to produce optimal PVA removal efficiency in the present study. A simple kinetic model was proposed which confirmed pseudo-first-order reaction. Reaction rate constant (kap) was found to depend on the UV light intensity.


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## Body

## 1. Introduction

Advanced oxidation processes (AOPs) have become very common for the treatment of industrial wastewater containing organic compounds. AOPs are based on the generation of highly reactive radicals such as hydroxyl(∙OH), a strong oxidant with E of 2.8 V, which can be strong enough to non-selectively oxidize most organic compounds through chain reactions at ambient temperature and pressure. Among these AOPs, electrochemical oxidation is thought to be one of the most promising methods for wastewater treatment; it is friendly to the environment, easy to control, and efficient for oxidation [1]. The electrochemical oxidation of organic pollutants is generally accompanied by side reactions such as oxygen or chlorine evolution due to the high voltage required to destroy the organic compounds in aqueous solutions. Thus, it may prove more efficient to combine electrochemical oxidation with other processes [2, 3]. Ultraviolet (UV) photolysis is another effective process. UV-based AOPs are characterized by the generation of strong oxidizing species, principally hydroxyl radicals, using combinations of strong oxidizing agents, such as ozone and hydrogen peroxide (H2O2) with UV radiation in the 200–280 nm range [4, 5].Hydrogen peroxide (H2O2) is an environmentally friendly chemical, because it leaves no hazardous residues. It is a powerful and versatile chemical, because it reacts as both a reductant and an oxidant [6]. However, the oxidative power of hydrogen peroxide is not strong enough to degrade organic compounds in some cases. Application in conjunction with UV irradiation and a metal catalyst can effectively increase the oxidative power of hydrogen peroxide due to the production of hydroxyl free radicals. The putative mechanism for the photolysis of H2O2 is the cleavage of the molecule into hydroxyl free radicals, which can then oxidize organic compounds (RH), yielding organic radicals that can in turn carry out further oxidation. The reactions that are accepted to occur during the UV/H2O2 oxidation process are as follows [7]:
(1)H2O2+UV⟶2OH•(2)RH+OH•⟶H2O+R•⟶furtheroxidationEmploying H2O2 with UV radiation for the removal of aqueous estrogens is one example of a homogeneous advanced oxidation process. The in situ electrochemical production of H2O2 via the reduction of oxygen on a cathode can reduce the costs and hazards associated with the transport and handling of concentrated H2O2. In recent years, some combinations of electrochemical oxidation and photolysis had been reported by various researchers [8, 9]. Most of these researchers concentrated on electro-Fenton technology in combination with UV irradiation, which may facilitate the photodecomposition of organic compounds, increase the generation of hydroxyl free radicals, and regenerate Fe2+ from Fe3+ species through a photoreduction mechanism [10–13]. However, there is little research on the combination of H2O2 electrogeneration with direct photolysis in the absence of added catalysts such as Fe2+ and TiO2.Electrochemical production of H2O2 has traditionally used graphite electrodes because of their low cost [14]. However, the poor solubility of oxygen in aqueous solutions causes mass transfer limitation, resulting in lower oxidation efficiency. Recently, activated carbon fiber (ACF) has been recognized as a promising carbon material with excellent characteristics for adsorption, conductivity, and catalysis [15]. Because of its large surface area, ACF also exhibits a high adsorption capacity and high adsorption rates. The excellent mechanical integrity of ACF makes it easy to configure as a stable electrode at which electrosorption processes can be conducted for the purpose of adsorptive removal of various organic pollutants in aqueous solutions. Furthermore, ACF electrodes may be used for the electrogeneration of H2O2 via the two-electron reduction of oxygen on its surface [16, 17]. The H2O2 electrogeneration rate significantly affects the treatment efficiency of any electro-Fenton technology. Several series processes affect the electrogeneration rate of H2O2 [15–17]. Oxygen gas must first be dissolved in solution. Second, it must be transferred to cathode surface, adsorbed onto the cathode, and finally reduced electrochemically to produce H2O2 in acidic media. Possible side reactions may occur simultaneously at the cathode and thus decrease the electrogeneration rate of H2O2 [14].Polyvinyl alcohol (PVA) is frequently used in the textile industry in blends with nylon and as a raw material for the production of PVA fibers. In addition, PVA is used as an ophthalmic lubricant in the pharmaceutical industry and is also widely used in the adhesives, emulsion paints, paper coating, and detergent-based industries. It is generally recognized that PVA is a high-k polymer with interesting properties such as good surface alignment effects, compatibility with water, low cost, and inexpensive processing [18]. The large amount of PVA discharged in industrial effluents is harmful to human health and to the environment [19]. It is often difficult to clean wastewaters containing PVA and to generate harmless end products such as water and carbon dioxide; thus, PVA adversely affects the ecosystem and accumulates in the human body through the food chain. PVA also creates environmental issues due to its ability to prevent the sedimentation of heavy metals in lakes and streams. Conventional biological technologies do not provide effective treatment of PVA because the degradation capacity of most microorganisms towards PVA is extremely low and specific to PVA [20]. The formation of foam in biological equipment for the treatment of wastewater containing PVA also makes stable operations and acceptable performance very difficult. A large number of scientific studies on the removal of PVA have been carried out, most of which have focused on photochemically initiated degradation processes [21]. Other physicochemical studies on the removal of PVA have focused on methods such as ultrasonic techniques [22], radiation-induced degradation [23], electro-Fenton [17], adsorption by activated carbon [24], and electrocoagulation [25, 26].To our knowledge so far, very little work, if any, has been reported in the literature to date on PVA removal by photoelectrochemical oxidation processes based on H2O2 electrogeneration. The main purpose of this study was to investigate the efficiency of H2O2 electrogeneration in acidic solutions using different cathodes fed with oxygen and to elucidate the removal efficiency of PVA via photoelectrochemical oxidation using an ACF cathode. The influences of several operating parameters such as current density, oxygen flow rate, solution pH, and different supporting electrolytes on the H2O2 electrogeneration were investigated. The effects of different processes (UV, H2O2 electrogeneration, and UV/H2O2 electrogeneration), and UV irradiation intensity on the rate of PVA removal from aqueous solutions were also investigated. In addition, a simple kinetic model for PVA removal by photoelectrochemical oxidation was proposed to calculate the reaction rate constant.


## 2.  Experimental

### 2.1. Material and Chemical Reagents

Polyvinyl alcohol (PVA, molecular weight in the range of 13,000 to 23,000 g mol−1) was obtained from Sigma-Aldrich (Saint Louis, MO 63103, USA) with a hydrolysis degree ranging from 98 to 99%. Na2SO4, NaNO3, and NaCl were purchased from Merck (Darmstadt, Germany) and used as supporting electrolyte in the aqueous solutions. Titanium(IV) sulfate [Ti(SO4)2] was purchased from SHOWA (Tokyo, Japan). Potassium iodide (KI) was obtained from Union Chemical Work Ltd. (Hsin-Chu, Taiwan), and iodine (I) was obtained from Toyobo Co. Ltd. (Osaka, Japan). Boric acid (H3BO3) was purchased from Merck (Darmstadt, Germany). Sulfuric acid (H2SO4, 3 M) was used to adjust the pH of the solution. All chemicals were analytical grade reagents and prepared by dilution with deionized water to the desired concentrations. The activated carbon fiber (ACF), PAN-based rigid composite carbon felt series, was obtained from Taiwan carbon Technology Co. Ltd. (Taichung, Taiwan).


### 2.2.  Apparatus

Figure1 is a schematic diagram of the photoelectrochemical system and the electrode assembly used in this work. The electrolytic reactor was a 1.0 L Pyrex glass vessel equipped with a water jacket and a magnetic stirrer. A magnetic stirrer bar (Suntex, SH-301, Taiwan) was spun at the center of the bottom of the reactor. The temperature of the electrolytic cell was controlled by continuously circulating water through the water jacket from a temperature controlled bath (Model BL-720, Taiwan). The assembly was connected to a direct current power source (PSM-6003, Taichung, Taiwan). A UV lamp (8 W, UV-C, λmax=254 nm, manufactured by Sankyo Denki, Tokyo, Japan) was used as a radiation source and placed above an electrolytic reactor. The UV-light intensity was measured by a Digital Ultraviolet Radiometer (Rixen Technology, Taipei, Taiwan).Figure 1
Schematic diagram of the photoelectrochemical oxidation equipment.


### 2.3.  Experimental and Analysis

The experiments were conducted in a close, and undivided glass vessel. For each test run, a circular container with 0.5 L of synthetic wastewater containing polyvinyl alcohol was used as the reactor. The ACF, graphite plate, and platinum were used as the cathodes and a platinum flat with an area of about 7.5 cm2 as the anode. The two electrodes were approximately 2 cm apart. The magnetic stirrer was turned on and set at 300 rpm. The ACF felt was saturated with 1000 mg L−1 PVA solution for 24 h to exclude the adsorption reaction of PVA on the ACF felt. During the electrolysis experiments, the cathode surface was fed with O2 for electrochemical reactions. Before the photoelectrochemical treatment, the pH of aqueous solution containing PVA was measured with pH meter. The photoelectrochemical treatment run lasted 120 min in all experiments. The H2O2 concentration was determined using the Ti(SO4)2 titration method and spectrophotometric analysis at λ=410 nm [27]. The PVA concentration in the aqueous solutions was determined using a HACH Model DR2800 spectrophotometer (HACH Company, USA) after addition of boric acid and iodine solutions according to the procedure described by Finley [28]. In order to calculate the normalized PVA concentration was performed using the following formula:
(3)NormalizedPVA=CC0,
where C0 is the initial concentration in mg L−1, C is the concentration value at time t in mg L−1. All samples were measured in duplicate to ensure data reproducibility, and an additional measurement was carried out if necessary.


## 2.1. Material and Chemical Reagents

Polyvinyl alcohol (PVA, molecular weight in the range of 13,000 to 23,000 g mol−1) was obtained from Sigma-Aldrich (Saint Louis, MO 63103, USA) with a hydrolysis degree ranging from 98 to 99%. Na2SO4, NaNO3, and NaCl were purchased from Merck (Darmstadt, Germany) and used as supporting electrolyte in the aqueous solutions. Titanium(IV) sulfate [Ti(SO4)2] was purchased from SHOWA (Tokyo, Japan). Potassium iodide (KI) was obtained from Union Chemical Work Ltd. (Hsin-Chu, Taiwan), and iodine (I) was obtained from Toyobo Co. Ltd. (Osaka, Japan). Boric acid (H3BO3) was purchased from Merck (Darmstadt, Germany). Sulfuric acid (H2SO4, 3 M) was used to adjust the pH of the solution. All chemicals were analytical grade reagents and prepared by dilution with deionized water to the desired concentrations. The activated carbon fiber (ACF), PAN-based rigid composite carbon felt series, was obtained from Taiwan carbon Technology Co. Ltd. (Taichung, Taiwan).


## 2.2.  Apparatus

Figure1 is a schematic diagram of the photoelectrochemical system and the electrode assembly used in this work. The electrolytic reactor was a 1.0 L Pyrex glass vessel equipped with a water jacket and a magnetic stirrer. A magnetic stirrer bar (Suntex, SH-301, Taiwan) was spun at the center of the bottom of the reactor. The temperature of the electrolytic cell was controlled by continuously circulating water through the water jacket from a temperature controlled bath (Model BL-720, Taiwan). The assembly was connected to a direct current power source (PSM-6003, Taichung, Taiwan). A UV lamp (8 W, UV-C, λmax=254 nm, manufactured by Sankyo Denki, Tokyo, Japan) was used as a radiation source and placed above an electrolytic reactor. The UV-light intensity was measured by a Digital Ultraviolet Radiometer (Rixen Technology, Taipei, Taiwan).Figure 1
Schematic diagram of the photoelectrochemical oxidation equipment.


## 2.3.  Experimental and Analysis

The experiments were conducted in a close, and undivided glass vessel. For each test run, a circular container with 0.5 L of synthetic wastewater containing polyvinyl alcohol was used as the reactor. The ACF, graphite plate, and platinum were used as the cathodes and a platinum flat with an area of about 7.5 cm2 as the anode. The two electrodes were approximately 2 cm apart. The magnetic stirrer was turned on and set at 300 rpm. The ACF felt was saturated with 1000 mg L−1 PVA solution for 24 h to exclude the adsorption reaction of PVA on the ACF felt. During the electrolysis experiments, the cathode surface was fed with O2 for electrochemical reactions. Before the photoelectrochemical treatment, the pH of aqueous solution containing PVA was measured with pH meter. The photoelectrochemical treatment run lasted 120 min in all experiments. The H2O2 concentration was determined using the Ti(SO4)2 titration method and spectrophotometric analysis at λ=410 nm [27]. The PVA concentration in the aqueous solutions was determined using a HACH Model DR2800 spectrophotometer (HACH Company, USA) after addition of boric acid and iodine solutions according to the procedure described by Finley [28]. In order to calculate the normalized PVA concentration was performed using the following formula:
(3)NormalizedPVA=CC0,
where C0 is the initial concentration in mg L−1, C is the concentration value at time t in mg L−1. All samples were measured in duplicate to ensure data reproducibility, and an additional measurement was carried out if necessary.


## 3. Results and Discussion

### 3.1.  Comparison of Electrogeneration of H2O2 on Different Electrodes

H2O2 is often used in the oxidation of organic pollutants because of its high oxidation reduction potential (ORP), which can facilitate the degradation of organic pollutants. The previous literature reports that electrodes made from carbon materials have been used to generate H2O2 with good yields, for example, graphite [29], gas diffusion electrodes [30], carbon felt [31], carbon nanotube-PTFE [32], glassy carbon mesh [33], and activated carbon fiber [34]. The amount of H2O2 generated by the two-electron reduction of O2 on the cathode surface is an important parameter in the electrogeneration process. Apparently, the cathode material strongly affects the rate of formation of hydrogen peroxide. Therefore, it is necessary to investigate the yield of H2O2 in photoelectrochemical oxidation processes using different cathode materials. To evaluate their comparative performance for H2O2 generation, several cathode materials were used, including ACF, graphite, and platinum. Figure 2 shows a comparison of the H2O2 generation rates achieved using different electrode materials. As shown in this figure, H2O2 production rates of 1 mg L−1, 4.9 mg L−1, and 24.3 mg L−1 were achieved after 120 min of electrolysis using platinum, graphite, and ACF electrodes, respectively. This finding is likely explained by the fact that the ACF electrode has a large specific surface area and a great number of mesopores, so that oxygen can be rapidly adsorbed and reduced on the cathode surface, thereby generating H2O2 at high rates. This observation was in agreement with another previous study [34].Figure 2
Effect of different electrode materials on the H2O2 electrogeneration. (Na2SO4 = 0.05 M, pH = 3, oxygen flow rate = 500 cm3 min−1, and current density = 10 mA cm−2).


### 3.2. Effect of Operational Parameters on the Generation of H2O2

#### 3.2.1.  Effect of Current Density

To confirm the effect of current density on the electrochemical generation of H2O2 on the ACF cathode, several current densities were used in acidic solutions containing 0.05 M Na2SO4. Figure 3 shows the effect of the current density on the generation of H2O2 for various electrolysis durations. As the duration of the electrolysis increased, concomitant increases in H2O2 generation were observed for all current densities (4):
(4)O2+2H++2e-⟶H2O2Figure 3
Effect of current density on the H2O2 electrogeneration as a function of time. (Na2SO4  = 0.05 M, pH = 3, and oxygen flow rate = 500 cm3 min−1).After 120 min of electrolysis, the H2O2 concentration gradually rose for all of the current densities, eventually reaching a steady state, as shown in Figure 3. An inspection of these results shows a clear maximum in the concentration of H2O2 generated at a current density of 10 mA cm−2. In the cases where current densities lower than 10 mA cm−2 were applied, the H2O2 concentration increased with increasing current density, likely because increasing the applied current density can enhance the production rate of H2O2. However, the findings indicated that the H2O2 concentration underwent a dramatic decrease when the current density reached 12.5 mA cm−2. This finding can be ascribed to the fact that higher applied current density reflects higher applied voltage on the electrochemical system, which induces the decomposition of H2O2, either on the electrode or directly in the solution (5) [35]. In addition, the electrode surface reactions such as the production of oxygen and hydrogen also retard the reactions generating H2O2 [36]. Furthermore, a portion of the H2O2 produced can be anodically oxidized to yield intermediate HO2• radicals [37]. Consequently, a current density of 10 mA cm−2 was chosen as the optimum current density for the subsequent experiments:
(5)H2O2+2e-⟶2OH-(6)H2O2⟶HO2•+H++e-(7)HO2•⟶O2+H++e-


#### 3.2.2.  Effect of Oxygen Flow Rate

The rate of H2O2 generation via oxygen reduction at the cathode significantly affects the treatment efficiency of photoelectrochemical oxidation processes. The effect of the oxygen flow rate on the rate of H2O2 electrogeneration was studied by varying the flow rate between 300 and 900 cm3 min−1 while keeping the current density, the initial pH, and supporting electrolyte at 10 mA cm−2, 3, and 0.05 M Na2SO4, as shown in Table 1. A significant increase in the H2O2 electrogeneration rate was observed with increases in the oxygen flow rate. After 120 min of electrolysis, the oxygen flow rate increased from 300 to 500, 700, and 900 cm3 min−1, and the H2O2 concentration increased from 13.7 mg L−1 to 24.3 mg L−1, 25.4 mg L−1, and 26.1 mg L−1, respectively. Table 1 illustrates that increasing the oxygen flow rate can increase the amount of dissolved oxygen in the solution, thereby accelerating the generation of hydrogen peroxide. Namely, increasing the oxygen flow rate can increase the dissolved oxygen concentration and the mass transfer rate of dissolved oxygen and finally increase the production of H2O2. However, above an oxygen flow rate of 500 cm3 min−1, the dissolved oxygen and hydrogen peroxide concentration followed a steady trend. The results implied that the electrochemical kinetics of the hydrogen peroxide production correlated well with the amount of oxygen solubility dissolved in aqueous solutions, in which the saturated solubility of oxygen in aqueous solutions was nearly achieved at the oxygen flow rate of 500 cm3 min−1 [38]. According to these results and economic considerations, an oxygen flow rate of 500 cm3 min−1 at an applied current density of 10 mA cm−2 was adequate for further study in the present work.Table 1
Effect of the oxygen flow rate and initial pH value on the H2O2 electrogeneration.
Oxygen flow rate (cm3 min−1)
pH
300
500
700
900
2
3
4
5
H2O2 generation concentration (mg L−1)
13.7
24.3
25.4
26.1
22.2
24.3
14.4
11


#### 3.2.3.  Effect of Initial pH

In an electrochemical oxidation process, the solution pH is a crucial factor for the electrogeneration of H2O2. In H2O2 production, a low pH is theoretically favorable for the production of H2O2 because the conversion of dissolved oxygen to H2O2 consumes protons in acidic solution. However, a low pH also promotes hydrogen evolution, reducing the number of active sites for generating H2O2. Therefore, the existence of an optimal solution pH might be expected. The effect of the initial pH value of the solution on the rate of H2O2 electrogeneration was investigated by varying the initial pH between 2 and 5 while keeping the current density, oxygen flow rate, and supporting electrolyte at 10 mA cm−2, 500 cm3 min−1, and 0.05 M Na2SO4, as shown in Table 1. From this table, it was shown that the maximum concentration of H2O2 (24.3 mg L−1) was obtained at an initial pH = 3 after 120 min of electrolysis. However, the accumulated concentration of H2O2 fell to 22.2 mg L−1 as the initial pH decreased to 2. This finding could be explained by the fact that the oxonium ion (H3O2+) can enhance the stability of H2O2 (8) [39]. At the same time, two side reactions occur at the cathode: the reduction of H2O2 to H2O (9) and hydrogen gas production (10) [40]. Therefore, these side reactions decreased the accumulation of H2O2 in the solution at lower pH values. Based on these results, a pH value of 3 was found to be the optimal condition for H2O2 electrogeneration:
(8)H2O2+H+⟶H3O2+(9)H2O2+2H++2e-⟶2H2O(10)2H++2e-⟶H2


#### 3.2.4. Effect of Different Supporting Electrolytes

In electrochemical processes that consist of heterogeneous ion and electron transfer reactions, the conductivity of the solution to be treated is a significant parameter. The most common method of adjusting this parameter is to add a supporting electrolyte, which increases the solution conductivity and thus reduces energy consumption during the electrochemical process. To investigate the effect of the supporting electrolyte species on the generation of H2O2, Na2SO4, NaNO3, and NaCl were used as supporting electrolytes under the same conditions, as shown in Figure 4. After 120 min of electrolysis, we observed that 24.3 mg L−1, 23.4 mg L−1, and 9.72 mg L−1 of H2O2 were generated using Na2SO4, NaNO3, and NaCl, respectively. As it can be seen from Figure 4, the concentration of electrogenerated H2O2 produced in NaCl solution was lower than the concentrations produced in NaNO3 and Na2SO4. This observation could likely be explained by the fact that Cl2 formation was observed as a result of chlorine oxidation at high anodic potentials during the electrolysis process, and further oxidation of chlorine can also occur to form HOCl [38]. Therefore, these side reactions likely decreased the accumulation of H2O2 in the solution. Furthermore, the electrical conductivities of SO42- and NO3- solutions were greater than that of equivalent-strength Cl- solution [41]; thus, these solutions yielded greater amounts of electrogenerated H2O2. In addition, Zhou et al. reported higher concentrations of sodium sulfate, which could accelerate the generation of H2O2 and increase the pollutant removal efficiency [39]. Consequently, Na2SO4 was considered to be the most suitable electrolyte tested for the generation of H2O2.Figure 4
Effect of supporting electrolyte on the H2O2 electrogeneration as a function of time. (pH = 3, oxygen flow rate = 500 cm3 min−1, and current density = 10 mA cm−2).


### 3.3.  Removal of PVA by Photoelectrochemical Oxidation

#### 3.3.1. Effect of UV Irradiation in the Presence of H2O2

Figure5 shows the PVA removal efficiency as a function of time for experiments conducted with UV irradiation only, H2O2 electrogeneration without UV irradiation, and H2O2 electrogeneration plus UV irradiation. It can be seen that there was no significant removal of PVA with UV irradiation alone or with H2O2 electrogeneration in the absence of UV irradiation; the removal efficiencies for these conditions were 3% and 16%, respectively. In the case of H2O2 electrogeneration with UV irradiation, the PVA removal efficiency increased to 86%. These results reveal that the electrogeneration of H2O2 in the presence of UV irradiation can form hydroxyl radicals capable of remediating solutions containing PVA. Consequently, this result proves that the photoelectrochemical oxidation method can effectively remove PVA from aqueous solutions.Figure 5
Effect of UV irradiation and H2O2 electrogeneration in photoelectrochemical oxidation of PVA. (PVA = 2 mg L−1, Na2SO4 = 0.05 M, pH = 3, oxygen flow rate = 500 cm3 min−1, Na2SO4 = 0.05 M, and I0=0.45 mW cm−2).


#### 3.3.2.  Effect of UV Irradiation Intensity

UV light intensity determines the concentration of hydroxyl radicals generated. To evaluate the influence of UV light intensity on the removal efficiency of PVA, reaction rates were measured for various UV light intensities from 0 to 0.6 mW cm−2. Figure 6 shows the effect of UV light intensity on the PVA removal efficiency. It appears that increasing UV light intensity increases the PVA removal efficiency. This result can be explained by the fact that higher UV light intensity can enhance the generation of hydroxyl radicals to remove PVA from the solution (1) [42, 43]. On the other hand, at low UV light intensity, the rate of photolysis of H2O2 is limited, resulting in decreased PVA removal efficiency.Figure 6
Derivation of pseudo-first-order kinetic model plot at different UV-light intensity. (PVA = 2 mg L−1, pH = 3, Na2SO4 = 0.05 M, oxygen flow rate = 500 cm3 min−1, and current density = 10 mA cm−2).The pseudo-first-order reaction constant is linearly correlated with UV light intensity (R2=0.9923), which is also directly proportional to the proposed model (18), as shown in Figure 7. Therefore, the intensity of UV light is linearly correlated with the efficiency of PVA removal in this study.Figure 7
Relation between light intensity and pseudo-first-order reaction rate constant.


#### 3.3.3. PVA Removal Kinetics of Photoelectrochemical Oxidation

The overall kinetics of PVA removal by photoelectrochemical oxidation is described by a pseudokinetic model in which the rate constant depends on the initial concentration and the UV light intensity. This model provides preliminary data for evaluating the reaction rate constant which is an important index. This constant is calculated using the following model [42]:
(11)PVA+OH•→k1product(12)Si+OH•→kiproducti
where Si are scavenger molecules such as intermediates, excess H2O2, OH•, and HO2•[44].The corresponding kinetic equations for PVA andOH• are
(13)d[PVA]dt=-k1[OH•][PVA],(14)d[OH•]dt=ϕIa-k1[OH•][PVA]-∑ki[OH•][Si].The steady state concentration of hydroxyl radicals can be described by (14), which is obtained by solving (13):
(15)[OH•]ss=ϕIak1[PVA]+∑iki[Si],Ia=I0fH2O2[1-exp(-2.3l(εH2O2[H2O2]+εPVA[PVA]))],fH2O2=εH2O2[H2O2]εH2O2[H2O2]+εPVA[PVA],
where I0 is the incident UV light intensity, l is the optical path length of the system, and εH2O2 and εPVA are the molar extinction coefficients for H2O2 and PVA, respectively. As PVA and H2O2 have high absorbances in the early stages of the process, we can write
(16)1-exp(-2.3l(εH2O2[H2O2]+εPVA[PVA]))≈1,[OH•]ss=ϕI0fH2O2k1[PVA]+∑iki[Si].By inserting the previous expression into (13), the following overall rate law is deduced:
(17)-d[PVA]dt=k1ϕI0fH2O2k1[PVA]+∑iki[Si][PVA].If the concentration of the substrate is high, so thatk1[PVA]≫∑iki[Si], the overall rate expression simplifies to a zero order reaction rate:
(18)-d[PVA]dt=ϕI0fH2O2.However, in the present study, the concentration of PVA is lower than that of H2O2; thus, ∑iki[Si]≫k1[PVA], and the overall rate expression simplifies to a pseudo-first-order reaction rate:
(19)-d[PVA]dt=k1ϕI0fH2O2∑iki[Si][PVA]or(20)-d[PVA]dt=kap[PVA].The previous equation corresponds to a pseudo-first-order reaction. The semilogarithmic graphs of PVA concentration versus time thus can be fitted with a straight line to obtain the apparent reaction rate constant (kap). The conformity between experimental data and the model values was evaluated by calculating correlation coefficients (R2). The apparent reaction rate constants and correlation coefficients calculated from the pseudo-first-order model are listed in Table 2. Table 2 also shows that as the UV light intensity is increased, the reaction rate constant increases, and thus, the removal efficiency of PVA increases.Table 2
Pseudo-first-order rate constants for PVA removal at various UV-light intensity.
UV-light intensity (mW cm−2)
Pseudo-first-order
k
ap
R
2
0
0.0024
0.9
0.2
0.0094
0.992
0.4
0.0152
0.994
0.6
0.0248
0.998


## 3.1.  Comparison of Electrogeneration of H2O2 on Different Electrodes

H2O2 is often used in the oxidation of organic pollutants because of its high oxidation reduction potential (ORP), which can facilitate the degradation of organic pollutants. The previous literature reports that electrodes made from carbon materials have been used to generate H2O2 with good yields, for example, graphite [29], gas diffusion electrodes [30], carbon felt [31], carbon nanotube-PTFE [32], glassy carbon mesh [33], and activated carbon fiber [34]. The amount of H2O2 generated by the two-electron reduction of O2 on the cathode surface is an important parameter in the electrogeneration process. Apparently, the cathode material strongly affects the rate of formation of hydrogen peroxide. Therefore, it is necessary to investigate the yield of H2O2 in photoelectrochemical oxidation processes using different cathode materials. To evaluate their comparative performance for H2O2 generation, several cathode materials were used, including ACF, graphite, and platinum. Figure 2 shows a comparison of the H2O2 generation rates achieved using different electrode materials. As shown in this figure, H2O2 production rates of 1 mg L−1, 4.9 mg L−1, and 24.3 mg L−1 were achieved after 120 min of electrolysis using platinum, graphite, and ACF electrodes, respectively. This finding is likely explained by the fact that the ACF electrode has a large specific surface area and a great number of mesopores, so that oxygen can be rapidly adsorbed and reduced on the cathode surface, thereby generating H2O2 at high rates. This observation was in agreement with another previous study [34].Figure 2
Effect of different electrode materials on the H2O2 electrogeneration. (Na2SO4 = 0.05 M, pH = 3, oxygen flow rate = 500 cm3 min−1, and current density = 10 mA cm−2).


## 3.2. Effect of Operational Parameters on the Generation of H2O2

### 3.2.1.  Effect of Current Density

To confirm the effect of current density on the electrochemical generation of H2O2 on the ACF cathode, several current densities were used in acidic solutions containing 0.05 M Na2SO4. Figure 3 shows the effect of the current density on the generation of H2O2 for various electrolysis durations. As the duration of the electrolysis increased, concomitant increases in H2O2 generation were observed for all current densities (4):
(4)O2+2H++2e-⟶H2O2Figure 3
Effect of current density on the H2O2 electrogeneration as a function of time. (Na2SO4  = 0.05 M, pH = 3, and oxygen flow rate = 500 cm3 min−1).After 120 min of electrolysis, the H2O2 concentration gradually rose for all of the current densities, eventually reaching a steady state, as shown in Figure 3. An inspection of these results shows a clear maximum in the concentration of H2O2 generated at a current density of 10 mA cm−2. In the cases where current densities lower than 10 mA cm−2 were applied, the H2O2 concentration increased with increasing current density, likely because increasing the applied current density can enhance the production rate of H2O2. However, the findings indicated that the H2O2 concentration underwent a dramatic decrease when the current density reached 12.5 mA cm−2. This finding can be ascribed to the fact that higher applied current density reflects higher applied voltage on the electrochemical system, which induces the decomposition of H2O2, either on the electrode or directly in the solution (5) [35]. In addition, the electrode surface reactions such as the production of oxygen and hydrogen also retard the reactions generating H2O2 [36]. Furthermore, a portion of the H2O2 produced can be anodically oxidized to yield intermediate HO2• radicals [37]. Consequently, a current density of 10 mA cm−2 was chosen as the optimum current density for the subsequent experiments:
(5)H2O2+2e-⟶2OH-(6)H2O2⟶HO2•+H++e-(7)HO2•⟶O2+H++e-


### 3.2.2.  Effect of Oxygen Flow Rate

The rate of H2O2 generation via oxygen reduction at the cathode significantly affects the treatment efficiency of photoelectrochemical oxidation processes. The effect of the oxygen flow rate on the rate of H2O2 electrogeneration was studied by varying the flow rate between 300 and 900 cm3 min−1 while keeping the current density, the initial pH, and supporting electrolyte at 10 mA cm−2, 3, and 0.05 M Na2SO4, as shown in Table 1. A significant increase in the H2O2 electrogeneration rate was observed with increases in the oxygen flow rate. After 120 min of electrolysis, the oxygen flow rate increased from 300 to 500, 700, and 900 cm3 min−1, and the H2O2 concentration increased from 13.7 mg L−1 to 24.3 mg L−1, 25.4 mg L−1, and 26.1 mg L−1, respectively. Table 1 illustrates that increasing the oxygen flow rate can increase the amount of dissolved oxygen in the solution, thereby accelerating the generation of hydrogen peroxide. Namely, increasing the oxygen flow rate can increase the dissolved oxygen concentration and the mass transfer rate of dissolved oxygen and finally increase the production of H2O2. However, above an oxygen flow rate of 500 cm3 min−1, the dissolved oxygen and hydrogen peroxide concentration followed a steady trend. The results implied that the electrochemical kinetics of the hydrogen peroxide production correlated well with the amount of oxygen solubility dissolved in aqueous solutions, in which the saturated solubility of oxygen in aqueous solutions was nearly achieved at the oxygen flow rate of 500 cm3 min−1 [38]. According to these results and economic considerations, an oxygen flow rate of 500 cm3 min−1 at an applied current density of 10 mA cm−2 was adequate for further study in the present work.Table 1
Effect of the oxygen flow rate and initial pH value on the H2O2 electrogeneration.
Oxygen flow rate (cm3 min−1)
pH
300
500
700
900
2
3
4
5
H2O2 generation concentration (mg L−1)
13.7
24.3
25.4
26.1
22.2
24.3
14.4
11


### 3.2.3.  Effect of Initial pH

In an electrochemical oxidation process, the solution pH is a crucial factor for the electrogeneration of H2O2. In H2O2 production, a low pH is theoretically favorable for the production of H2O2 because the conversion of dissolved oxygen to H2O2 consumes protons in acidic solution. However, a low pH also promotes hydrogen evolution, reducing the number of active sites for generating H2O2. Therefore, the existence of an optimal solution pH might be expected. The effect of the initial pH value of the solution on the rate of H2O2 electrogeneration was investigated by varying the initial pH between 2 and 5 while keeping the current density, oxygen flow rate, and supporting electrolyte at 10 mA cm−2, 500 cm3 min−1, and 0.05 M Na2SO4, as shown in Table 1. From this table, it was shown that the maximum concentration of H2O2 (24.3 mg L−1) was obtained at an initial pH = 3 after 120 min of electrolysis. However, the accumulated concentration of H2O2 fell to 22.2 mg L−1 as the initial pH decreased to 2. This finding could be explained by the fact that the oxonium ion (H3O2+) can enhance the stability of H2O2 (8) [39]. At the same time, two side reactions occur at the cathode: the reduction of H2O2 to H2O (9) and hydrogen gas production (10) [40]. Therefore, these side reactions decreased the accumulation of H2O2 in the solution at lower pH values. Based on these results, a pH value of 3 was found to be the optimal condition for H2O2 electrogeneration:
(8)H2O2+H+⟶H3O2+(9)H2O2+2H++2e-⟶2H2O(10)2H++2e-⟶H2


### 3.2.4. Effect of Different Supporting Electrolytes

In electrochemical processes that consist of heterogeneous ion and electron transfer reactions, the conductivity of the solution to be treated is a significant parameter. The most common method of adjusting this parameter is to add a supporting electrolyte, which increases the solution conductivity and thus reduces energy consumption during the electrochemical process. To investigate the effect of the supporting electrolyte species on the generation of H2O2, Na2SO4, NaNO3, and NaCl were used as supporting electrolytes under the same conditions, as shown in Figure 4. After 120 min of electrolysis, we observed that 24.3 mg L−1, 23.4 mg L−1, and 9.72 mg L−1 of H2O2 were generated using Na2SO4, NaNO3, and NaCl, respectively. As it can be seen from Figure 4, the concentration of electrogenerated H2O2 produced in NaCl solution was lower than the concentrations produced in NaNO3 and Na2SO4. This observation could likely be explained by the fact that Cl2 formation was observed as a result of chlorine oxidation at high anodic potentials during the electrolysis process, and further oxidation of chlorine can also occur to form HOCl [38]. Therefore, these side reactions likely decreased the accumulation of H2O2 in the solution. Furthermore, the electrical conductivities of SO42- and NO3- solutions were greater than that of equivalent-strength Cl- solution [41]; thus, these solutions yielded greater amounts of electrogenerated H2O2. In addition, Zhou et al. reported higher concentrations of sodium sulfate, which could accelerate the generation of H2O2 and increase the pollutant removal efficiency [39]. Consequently, Na2SO4 was considered to be the most suitable electrolyte tested for the generation of H2O2.Figure 4
Effect of supporting electrolyte on the H2O2 electrogeneration as a function of time. (pH = 3, oxygen flow rate = 500 cm3 min−1, and current density = 10 mA cm−2).


## 3.2.1.  Effect of Current Density

To confirm the effect of current density on the electrochemical generation of H2O2 on the ACF cathode, several current densities were used in acidic solutions containing 0.05 M Na2SO4. Figure 3 shows the effect of the current density on the generation of H2O2 for various electrolysis durations. As the duration of the electrolysis increased, concomitant increases in H2O2 generation were observed for all current densities (4):
(4)O2+2H++2e-⟶H2O2Figure 3
Effect of current density on the H2O2 electrogeneration as a function of time. (Na2SO4  = 0.05 M, pH = 3, and oxygen flow rate = 500 cm3 min−1).After 120 min of electrolysis, the H2O2 concentration gradually rose for all of the current densities, eventually reaching a steady state, as shown in Figure 3. An inspection of these results shows a clear maximum in the concentration of H2O2 generated at a current density of 10 mA cm−2. In the cases where current densities lower than 10 mA cm−2 were applied, the H2O2 concentration increased with increasing current density, likely because increasing the applied current density can enhance the production rate of H2O2. However, the findings indicated that the H2O2 concentration underwent a dramatic decrease when the current density reached 12.5 mA cm−2. This finding can be ascribed to the fact that higher applied current density reflects higher applied voltage on the electrochemical system, which induces the decomposition of H2O2, either on the electrode or directly in the solution (5) [35]. In addition, the electrode surface reactions such as the production of oxygen and hydrogen also retard the reactions generating H2O2 [36]. Furthermore, a portion of the H2O2 produced can be anodically oxidized to yield intermediate HO2• radicals [37]. Consequently, a current density of 10 mA cm−2 was chosen as the optimum current density for the subsequent experiments:
(5)H2O2+2e-⟶2OH-(6)H2O2⟶HO2•+H++e-(7)HO2•⟶O2+H++e-


## 3.2.2.  Effect of Oxygen Flow Rate

The rate of H2O2 generation via oxygen reduction at the cathode significantly affects the treatment efficiency of photoelectrochemical oxidation processes. The effect of the oxygen flow rate on the rate of H2O2 electrogeneration was studied by varying the flow rate between 300 and 900 cm3 min−1 while keeping the current density, the initial pH, and supporting electrolyte at 10 mA cm−2, 3, and 0.05 M Na2SO4, as shown in Table 1. A significant increase in the H2O2 electrogeneration rate was observed with increases in the oxygen flow rate. After 120 min of electrolysis, the oxygen flow rate increased from 300 to 500, 700, and 900 cm3 min−1, and the H2O2 concentration increased from 13.7 mg L−1 to 24.3 mg L−1, 25.4 mg L−1, and 26.1 mg L−1, respectively. Table 1 illustrates that increasing the oxygen flow rate can increase the amount of dissolved oxygen in the solution, thereby accelerating the generation of hydrogen peroxide. Namely, increasing the oxygen flow rate can increase the dissolved oxygen concentration and the mass transfer rate of dissolved oxygen and finally increase the production of H2O2. However, above an oxygen flow rate of 500 cm3 min−1, the dissolved oxygen and hydrogen peroxide concentration followed a steady trend. The results implied that the electrochemical kinetics of the hydrogen peroxide production correlated well with the amount of oxygen solubility dissolved in aqueous solutions, in which the saturated solubility of oxygen in aqueous solutions was nearly achieved at the oxygen flow rate of 500 cm3 min−1 [38]. According to these results and economic considerations, an oxygen flow rate of 500 cm3 min−1 at an applied current density of 10 mA cm−2 was adequate for further study in the present work.Table 1
Effect of the oxygen flow rate and initial pH value on the H2O2 electrogeneration.
Oxygen flow rate (cm3 min−1)
pH
300
500
700
900
2
3
4
5
H2O2 generation concentration (mg L−1)
13.7
24.3
25.4
26.1
22.2
24.3
14.4
11


## 3.2.3.  Effect of Initial pH

In an electrochemical oxidation process, the solution pH is a crucial factor for the electrogeneration of H2O2. In H2O2 production, a low pH is theoretically favorable for the production of H2O2 because the conversion of dissolved oxygen to H2O2 consumes protons in acidic solution. However, a low pH also promotes hydrogen evolution, reducing the number of active sites for generating H2O2. Therefore, the existence of an optimal solution pH might be expected. The effect of the initial pH value of the solution on the rate of H2O2 electrogeneration was investigated by varying the initial pH between 2 and 5 while keeping the current density, oxygen flow rate, and supporting electrolyte at 10 mA cm−2, 500 cm3 min−1, and 0.05 M Na2SO4, as shown in Table 1. From this table, it was shown that the maximum concentration of H2O2 (24.3 mg L−1) was obtained at an initial pH = 3 after 120 min of electrolysis. However, the accumulated concentration of H2O2 fell to 22.2 mg L−1 as the initial pH decreased to 2. This finding could be explained by the fact that the oxonium ion (H3O2+) can enhance the stability of H2O2 (8) [39]. At the same time, two side reactions occur at the cathode: the reduction of H2O2 to H2O (9) and hydrogen gas production (10) [40]. Therefore, these side reactions decreased the accumulation of H2O2 in the solution at lower pH values. Based on these results, a pH value of 3 was found to be the optimal condition for H2O2 electrogeneration:
(8)H2O2+H+⟶H3O2+(9)H2O2+2H++2e-⟶2H2O(10)2H++2e-⟶H2


## 3.2.4. Effect of Different Supporting Electrolytes

In electrochemical processes that consist of heterogeneous ion and electron transfer reactions, the conductivity of the solution to be treated is a significant parameter. The most common method of adjusting this parameter is to add a supporting electrolyte, which increases the solution conductivity and thus reduces energy consumption during the electrochemical process. To investigate the effect of the supporting electrolyte species on the generation of H2O2, Na2SO4, NaNO3, and NaCl were used as supporting electrolytes under the same conditions, as shown in Figure 4. After 120 min of electrolysis, we observed that 24.3 mg L−1, 23.4 mg L−1, and 9.72 mg L−1 of H2O2 were generated using Na2SO4, NaNO3, and NaCl, respectively. As it can be seen from Figure 4, the concentration of electrogenerated H2O2 produced in NaCl solution was lower than the concentrations produced in NaNO3 and Na2SO4. This observation could likely be explained by the fact that Cl2 formation was observed as a result of chlorine oxidation at high anodic potentials during the electrolysis process, and further oxidation of chlorine can also occur to form HOCl [38]. Therefore, these side reactions likely decreased the accumulation of H2O2 in the solution. Furthermore, the electrical conductivities of SO42- and NO3- solutions were greater than that of equivalent-strength Cl- solution [41]; thus, these solutions yielded greater amounts of electrogenerated H2O2. In addition, Zhou et al. reported higher concentrations of sodium sulfate, which could accelerate the generation of H2O2 and increase the pollutant removal efficiency [39]. Consequently, Na2SO4 was considered to be the most suitable electrolyte tested for the generation of H2O2.Figure 4
Effect of supporting electrolyte on the H2O2 electrogeneration as a function of time. (pH = 3, oxygen flow rate = 500 cm3 min−1, and current density = 10 mA cm−2).


## 3.3.  Removal of PVA by Photoelectrochemical Oxidation

### 3.3.1. Effect of UV Irradiation in the Presence of H2O2

Figure5 shows the PVA removal efficiency as a function of time for experiments conducted with UV irradiation only, H2O2 electrogeneration without UV irradiation, and H2O2 electrogeneration plus UV irradiation. It can be seen that there was no significant removal of PVA with UV irradiation alone or with H2O2 electrogeneration in the absence of UV irradiation; the removal efficiencies for these conditions were 3% and 16%, respectively. In the case of H2O2 electrogeneration with UV irradiation, the PVA removal efficiency increased to 86%. These results reveal that the electrogeneration of H2O2 in the presence of UV irradiation can form hydroxyl radicals capable of remediating solutions containing PVA. Consequently, this result proves that the photoelectrochemical oxidation method can effectively remove PVA from aqueous solutions.Figure 5
Effect of UV irradiation and H2O2 electrogeneration in photoelectrochemical oxidation of PVA. (PVA = 2 mg L−1, Na2SO4 = 0.05 M, pH = 3, oxygen flow rate = 500 cm3 min−1, Na2SO4 = 0.05 M, and I0=0.45 mW cm−2).


### 3.3.2.  Effect of UV Irradiation Intensity

UV light intensity determines the concentration of hydroxyl radicals generated. To evaluate the influence of UV light intensity on the removal efficiency of PVA, reaction rates were measured for various UV light intensities from 0 to 0.6 mW cm−2. Figure 6 shows the effect of UV light intensity on the PVA removal efficiency. It appears that increasing UV light intensity increases the PVA removal efficiency. This result can be explained by the fact that higher UV light intensity can enhance the generation of hydroxyl radicals to remove PVA from the solution (1) [42, 43]. On the other hand, at low UV light intensity, the rate of photolysis of H2O2 is limited, resulting in decreased PVA removal efficiency.Figure 6
Derivation of pseudo-first-order kinetic model plot at different UV-light intensity. (PVA = 2 mg L−1, pH = 3, Na2SO4 = 0.05 M, oxygen flow rate = 500 cm3 min−1, and current density = 10 mA cm−2).The pseudo-first-order reaction constant is linearly correlated with UV light intensity (R2=0.9923), which is also directly proportional to the proposed model (18), as shown in Figure 7. Therefore, the intensity of UV light is linearly correlated with the efficiency of PVA removal in this study.Figure 7
Relation between light intensity and pseudo-first-order reaction rate constant.


### 3.3.3. PVA Removal Kinetics of Photoelectrochemical Oxidation

The overall kinetics of PVA removal by photoelectrochemical oxidation is described by a pseudokinetic model in which the rate constant depends on the initial concentration and the UV light intensity. This model provides preliminary data for evaluating the reaction rate constant which is an important index. This constant is calculated using the following model [42]:
(11)PVA+OH•→k1product(12)Si+OH•→kiproducti
where Si are scavenger molecules such as intermediates, excess H2O2, OH•, and HO2•[44].The corresponding kinetic equations for PVA andOH• are
(13)d[PVA]dt=-k1[OH•][PVA],(14)d[OH•]dt=ϕIa-k1[OH•][PVA]-∑ki[OH•][Si].The steady state concentration of hydroxyl radicals can be described by (14), which is obtained by solving (13):
(15)[OH•]ss=ϕIak1[PVA]+∑iki[Si],Ia=I0fH2O2[1-exp(-2.3l(εH2O2[H2O2]+εPVA[PVA]))],fH2O2=εH2O2[H2O2]εH2O2[H2O2]+εPVA[PVA],
where I0 is the incident UV light intensity, l is the optical path length of the system, and εH2O2 and εPVA are the molar extinction coefficients for H2O2 and PVA, respectively. As PVA and H2O2 have high absorbances in the early stages of the process, we can write
(16)1-exp(-2.3l(εH2O2[H2O2]+εPVA[PVA]))≈1,[OH•]ss=ϕI0fH2O2k1[PVA]+∑iki[Si].By inserting the previous expression into (13), the following overall rate law is deduced:
(17)-d[PVA]dt=k1ϕI0fH2O2k1[PVA]+∑iki[Si][PVA].If the concentration of the substrate is high, so thatk1[PVA]≫∑iki[Si], the overall rate expression simplifies to a zero order reaction rate:
(18)-d[PVA]dt=ϕI0fH2O2.However, in the present study, the concentration of PVA is lower than that of H2O2; thus, ∑iki[Si]≫k1[PVA], and the overall rate expression simplifies to a pseudo-first-order reaction rate:
(19)-d[PVA]dt=k1ϕI0fH2O2∑iki[Si][PVA]or(20)-d[PVA]dt=kap[PVA].The previous equation corresponds to a pseudo-first-order reaction. The semilogarithmic graphs of PVA concentration versus time thus can be fitted with a straight line to obtain the apparent reaction rate constant (kap). The conformity between experimental data and the model values was evaluated by calculating correlation coefficients (R2). The apparent reaction rate constants and correlation coefficients calculated from the pseudo-first-order model are listed in Table 2. Table 2 also shows that as the UV light intensity is increased, the reaction rate constant increases, and thus, the removal efficiency of PVA increases.Table 2
Pseudo-first-order rate constants for PVA removal at various UV-light intensity.
UV-light intensity (mW cm−2)
Pseudo-first-order
k
ap
R
2
0
0.0024
0.9
0.2
0.0094
0.992
0.4
0.0152
0.994
0.6
0.0248
0.998


## 3.3.1. Effect of UV Irradiation in the Presence of H2O2

Figure5 shows the PVA removal efficiency as a function of time for experiments conducted with UV irradiation only, H2O2 electrogeneration without UV irradiation, and H2O2 electrogeneration plus UV irradiation. It can be seen that there was no significant removal of PVA with UV irradiation alone or with H2O2 electrogeneration in the absence of UV irradiation; the removal efficiencies for these conditions were 3% and 16%, respectively. In the case of H2O2 electrogeneration with UV irradiation, the PVA removal efficiency increased to 86%. These results reveal that the electrogeneration of H2O2 in the presence of UV irradiation can form hydroxyl radicals capable of remediating solutions containing PVA. Consequently, this result proves that the photoelectrochemical oxidation method can effectively remove PVA from aqueous solutions.Figure 5
Effect of UV irradiation and H2O2 electrogeneration in photoelectrochemical oxidation of PVA. (PVA = 2 mg L−1, Na2SO4 = 0.05 M, pH = 3, oxygen flow rate = 500 cm3 min−1, Na2SO4 = 0.05 M, and I0=0.45 mW cm−2).


## 3.3.2.  Effect of UV Irradiation Intensity

UV light intensity determines the concentration of hydroxyl radicals generated. To evaluate the influence of UV light intensity on the removal efficiency of PVA, reaction rates were measured for various UV light intensities from 0 to 0.6 mW cm−2. Figure 6 shows the effect of UV light intensity on the PVA removal efficiency. It appears that increasing UV light intensity increases the PVA removal efficiency. This result can be explained by the fact that higher UV light intensity can enhance the generation of hydroxyl radicals to remove PVA from the solution (1) [42, 43]. On the other hand, at low UV light intensity, the rate of photolysis of H2O2 is limited, resulting in decreased PVA removal efficiency.Figure 6
Derivation of pseudo-first-order kinetic model plot at different UV-light intensity. (PVA = 2 mg L−1, pH = 3, Na2SO4 = 0.05 M, oxygen flow rate = 500 cm3 min−1, and current density = 10 mA cm−2).The pseudo-first-order reaction constant is linearly correlated with UV light intensity (R2=0.9923), which is also directly proportional to the proposed model (18), as shown in Figure 7. Therefore, the intensity of UV light is linearly correlated with the efficiency of PVA removal in this study.Figure 7
Relation between light intensity and pseudo-first-order reaction rate constant.


## 3.3.3. PVA Removal Kinetics of Photoelectrochemical Oxidation

The overall kinetics of PVA removal by photoelectrochemical oxidation is described by a pseudokinetic model in which the rate constant depends on the initial concentration and the UV light intensity. This model provides preliminary data for evaluating the reaction rate constant which is an important index. This constant is calculated using the following model [42]:
(11)PVA+OH•→k1product(12)Si+OH•→kiproducti
where Si are scavenger molecules such as intermediates, excess H2O2, OH•, and HO2•[44].The corresponding kinetic equations for PVA andOH• are
(13)d[PVA]dt=-k1[OH•][PVA],(14)d[OH•]dt=ϕIa-k1[OH•][PVA]-∑ki[OH•][Si].The steady state concentration of hydroxyl radicals can be described by (14), which is obtained by solving (13):
(15)[OH•]ss=ϕIak1[PVA]+∑iki[Si],Ia=I0fH2O2[1-exp(-2.3l(εH2O2[H2O2]+εPVA[PVA]))],fH2O2=εH2O2[H2O2]εH2O2[H2O2]+εPVA[PVA],
where I0 is the incident UV light intensity, l is the optical path length of the system, and εH2O2 and εPVA are the molar extinction coefficients for H2O2 and PVA, respectively. As PVA and H2O2 have high absorbances in the early stages of the process, we can write
(16)1-exp(-2.3l(εH2O2[H2O2]+εPVA[PVA]))≈1,[OH•]ss=ϕI0fH2O2k1[PVA]+∑iki[Si].By inserting the previous expression into (13), the following overall rate law is deduced:
(17)-d[PVA]dt=k1ϕI0fH2O2k1[PVA]+∑iki[Si][PVA].If the concentration of the substrate is high, so thatk1[PVA]≫∑iki[Si], the overall rate expression simplifies to a zero order reaction rate:
(18)-d[PVA]dt=ϕI0fH2O2.However, in the present study, the concentration of PVA is lower than that of H2O2; thus, ∑iki[Si]≫k1[PVA], and the overall rate expression simplifies to a pseudo-first-order reaction rate:
(19)-d[PVA]dt=k1ϕI0fH2O2∑iki[Si][PVA]or(20)-d[PVA]dt=kap[PVA].The previous equation corresponds to a pseudo-first-order reaction. The semilogarithmic graphs of PVA concentration versus time thus can be fitted with a straight line to obtain the apparent reaction rate constant (kap). The conformity between experimental data and the model values was evaluated by calculating correlation coefficients (R2). The apparent reaction rate constants and correlation coefficients calculated from the pseudo-first-order model are listed in Table 2. Table 2 also shows that as the UV light intensity is increased, the reaction rate constant increases, and thus, the removal efficiency of PVA increases.Table 2
Pseudo-first-order rate constants for PVA removal at various UV-light intensity.
UV-light intensity (mW cm−2)
Pseudo-first-order
k
ap
R
2
0
0.0024
0.9
0.2
0.0094
0.992
0.4
0.0152
0.994
0.6
0.0248
0.998


## 4. Conclusions

In this study, the removal of PVA from aqueous solution via photoelectrochemical oxidation was investigated in a closed batch system. We compared the electrogeneration of H2O2 using three cathode materials (i.e., platinum, graphite, and activated carbon fiber (ACF)) fed with oxygen. The accumulation of electrogenerated H2O2 using the ACF electrode was greater than the concentrations obtained using other cathode materials. Several parameters were evaluated to characterize the H2O2 electrogeneration, such as current density, oxygen flow rate, solution pH, and the type of supporting electrolyte used. The results indicated that the optimal conditions for H2O2 electrogeneration were a current density of 10 mA cm−2, an oxygen flow rate of 500 cm3 min−1, and pH = 3. The addition of 0.05 M Na2SO4 as a supporting electrolyte also resulted in rapid H2O2 electrogeneration. The PVA removal efficiencies achieved under these conditions were 3%, 16%, and 86% using UV, H2O2 electrogeneration, and UV/H2O2 electrogeneration, respectively. A UV light intensity of 0.6 mW cm−2 was found to produce the highest rate of PVA removal in the present study. A simple kinetic model was proposed which confirmed the suitability of pseudo-first-order reaction. Reaction rate constant (kap) was dependent on the UV light intensity, and the pseudo-first-order constant was also directly proportional to UV light intensity. Under these conditions, the maximum PVA removal efficiency was found to be 91%.



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*Source: 841762-2013-09-01.xml*