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International Journal of Photoenergy
Volume 2013 (2013), Article ID 595031, 12 pages
http://dx.doi.org/10.1155/2013/595031
Research Article

Supported Zinc Oxide Photocatalyst for Decolorization and Mineralization of Orange G Dye Wastewater under UV365 Irradiation

Institute of Environmental Engineering, Hungkuang University, No. 34 Chung-Chie Road, Shalu, Taichung 433, Taiwan

Received 18 August 2013; Revised 24 September 2013; Accepted 25 September 2013

Academic Editor: Jiaguo Yu

Copyright © 2013 Ming-Chin Chang et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

Abstract

To solve the environmental challenge of textile wastewater, a UV/ZnO photocatalytic system was proposed. The objective of this study was to prepare a photocatalytic system by utilizing both cold cathode fluorescent light (CCFL) UV irradiation and steel mesh supported ZnO nanoparticles in a closed reactor for the degradation of azo dye C.I. Orange G (OG). Various operating parameters such as reaction time, preparation temperature, mixing speed, ZnO dosage, UV intensity, pH, initial dye concentration, and service duration were studied. Results presented efficient color and total organic carbon (TOC) removal of the OG azo dye by the designed photocatalytic system. The optimal ZnO dosage for color removal was 60 g m−2. An alkaline pH of 11.0 was sufficient for photocatalytic decolorization and mineralization. The rate of color removal decreased with the increase in the initial dye concentration. However, the rate of color removal increased with the increase in the UV intensity. The steel mesh supported ZnO can be used repeatedly over 10 times without losing the color removal efficiency for 120 min reaction time. Results of Fourier transform infrared (FTIR) and ion chromatography (IC) indicated the breakage of N=N bonds and formation of sulfate, nitrate, and nitrite as the major and minor products. The observation indicated degradation of dye molecules.

1. Introduction

In the last few decades, the textile industry is one of the most important industries, which make contribution toward Taiwan’s economic development. Wastewater effluents from textile and dye manufacturing industries receive much attention from public and governmental enforcements, because this type of wastewater can hardly meet the national discharge standards. In Taiwan, the national effluent standard (NES) has enforced the criteria of textile dyeing industries that chemical oxygen demand (COD) meets <100 to 160 mg/L and American Dye Manufacturers Institute (ADMI) color index meets <550 unit by the year 2003. On the other hand, most dyestuffs from the effluent of textile dyeing and finishing industry are complicated organic compounds with high color intensity, are recalcitrant to conventional biological wastewater treatment, and cause major environmental concerns [14]. To resolve the wastewater treatment problem, textile industrial treatment plants usually employ chemical coagulation integrated with activated sludge process. Unfortunately, these traditional treatment processes cannot meet the increasingly stringent criteria of color in dye wastewater treatment in Taiwan [5]. Under this situation, textile dyeing industries should pursue a more efficient technique to be the pretreatment or polishing processes to decolorize the highly colored wastewater. In this category of wastewater, azo dyes with nitrogen double bond (–N=N–) are the largest class of commercial dyestuffs used in the textile industries. Thus, many studies focused on decolorizing azo dye compounds by various techniques [68].

Advanced oxidation processes (AOPs), such as ozonation, UV/H2O2, UV/O3, Fe2+/H2O2, and UV/O3/H2O2, are widely used to decompose organic products in industrial wastewater and groundwater. The extensive literatures of these technologies have been reviewed by Venkatadri and Peters [9]. These processes have the potential ability to mineralize most of the organic contaminants into carbon dioxide and water. There were reports of successful color removal with final mineralization from azo dye wastewater using advanced oxidation processes (AOPs) such as UV/H2O2 [1012], UV/O3 [13, 14], or the Fenton reaction [15, 16]. Additionally, it has been reported that photocatalytic processes such as UV/ZnO system can also be effective in treating dye wastewaters [1719]. The preparation of ZnO catalyst can be demonstrated by hydrothermal synthesis [20] and the doping of carbon on ZnO can improve its visible light application [21]. Much research focused on slurry type reactor. However, the limitation on the need of further separation of ZnO particles made the process more complicate and expensive. Therefore, fixing the ZnO particles onto supported materials such as glass plate, silica plate can avoid the particle separation step and can enable the easy operation of heterogeneous ZnO photocatalysis [2224]. The aim of this work was to study the degradation of azo dye C.I. Orange G (OG) using a batch photocatalytic reactor in which the photocatalytic ZnO particles were supported on steel mesh and six cold cathode fluorescent lamps (CCFL) were used (wavelength of 365 nm) to provide UV irradiation. Operating parameters such as preparation temperature, mixing speed, ZnO dosage, UV intensity, pH, initial dye concentration, and reaction time that may affect the degree of the dye degradation were studied. Changes in color intensity, total organic carbon (TOC), pH, oxidation reduction potential (ORP) were monitored in addition to the analysis of reaction products by Fourier transform infrared (FTIR) and ion chromatography (IC).

2. Materials and Methods

2.1. Materials and Apparatus

A mono-azo dye, C.I. Orange G (OG), was selected as target compound for this photocatalytic decolorization study. OG (C16H10N2Na2O7S2, 60% purity) with a characteristic wavelength () of 479 nm and a molecular weight of 452.38 g mole−1 was purchased from Sigma-Aldrich, Inc. and used as received without further purification. The chemical structure of OG can be obtained from our previous study [25]. The commercial available nanosized zinc oxide (ZnO), with a specific surface area of 25.68 m2 g−1 from Aldrich, was used as the photocatalyst. The steel mesh (mesh size no.140, 0.106 mm) was purchased from a local hardware store and trimmed into pieces with a gross area of 252 cm2 (36 × 7 cm). A dip coating technique was used to prepare ZnO-coated steel meshes. The trimmed steel mesh was washed, dried, and weighted first, then dipped into a designed concentration of ZnO mixed liquid for 30 minutes, and then dried in a 105°C oven for 30 minutes. The coating process was repeated three times. After all, the ZnO-coated steel mesh was weighted to measure the amount of ZnO on steel mesh. The detailed preparation procedure was reported in our previous work with the replacement of TiO2 with ZnO nanoparticles [25]. Table 1 shows the steel mesh with specific surface. ZnO concentration of 8–67 g m−2 can be obtained by dip coating 0.20–1.67 g of ZnO nanoparticles on the given steel mesh with gross area of 252 cm2. Based on images obtained with the field emission scanning electron microscope (FESEM), model JEOL 6330CF, the bare steel mesh showed smooth surface with no particles attached as shown in Figures 1(a) and 1(b). As for ZnO-coated steel mesh, it is seen that ZnO particles were uniformly coated on the steel mesh surface and the particles were of cylindrical shape as shown in Figures 1(c) and 1(d). The crystallinity of ZnO particles was provided by Aldrich as wurtzite structure. The photocatalytic reactor setup was also presented in our previous work [25]. The reactor was a 36 cm (L) × 7 cm (W) × 7.8 cm (H) black acrylics container fixed on a horizontal shaker with 75 rpm mixing speed. At the upper cover of the reactor, six cold cathode fluorescent lamps (CCFL), each of which has a diameter of 0.25 cm, length of 30 cm, light intensity of 4 W, and irradiation wavelength of 365 nm, were equipped which yielded a total light energy of 2.1 mW cm−2 measured at the surface of the solution. In each experimental run, 200 mL dye solution was introduced to the photocatalytic reactor. At the bottom of the reactor, there was ZnO-coated steel mesh with total gross surface area 252 cm2 placed.

tab1
Table 1: The ZnO-coated weight on the steel meshes.
fig1
Figure 1: The morphology of ZnO powder coated on steel mesh at 150°C was identified by a JEOL 6330CF field emission scanning electron microscope (FESEM). (a) Bare steel mesh, 50 times enlargement. (b) Bare steel mesh, 100,000 times enlargement. (c) ZnO-coated steel mesh, 50 times enlargement. (d) ZnO-coated steel mesh, 50,000 times enlargement.
2.2. Experimental Procedure and Analysis

OG azo dye solution at various concentrations was prepared with deionized water. The experimental variables studied included reaction time, preparation temperature, mixing speed, ZnO dosage, UV intensity, pH, initial dye concentration, and application duration of ZnO. At a predetermined reaction time, an aliquot of the solution was withdrawn and analyzed for residual dye concentration, TOC, and color.

Dye concentration was determined by measuring the absorbance at a wavelength of 479 nm using Hitachi U-2000 spectrophotometer. Color intensity was determined based on the American Dye Manufacturers Institute (ADMI) standard color measurement by applying the Adams-Nickerson color difference formula following method 2120E of the standard methods. The pH and redox potential (ORP) were monitored by a Eutech PH5500 dual channel pH/ion meter with specific probes. TOC was obtained with a total organic carbon analyzer from O.I. Analytical Aurora, model 1030. Besides, the degradation products were identified using Perkin Elmer FTIR spectrophotometer model, Spectrum One. Ions such as sulfate, nitrate, and nitrite were identified with ion chromatography (IC), Dionex ICS-1000.

3. Results and Discussion

3.1. Synergic Effect of Combining CCFL UV 365 Irradiation and ZnO Catalyst

The color removal was first compared for various systems, that is, UV/ZnO, UV alone, and ZnO alone, at the initial OG concentration of 50 mg L−1, ZnO dosage of 60 g m−2, and 6 CCFL lamps with total light intensity of 24 W and at wavelength of 365 nm in 120 min of reaction in the closed reactor. Figure 2(a) shows results of color removal by various systems. Results indicated that the system of UV alone and ZnO alone could not remove color at any significant level. The UV/ZnO system removed color effectively with 100% removal, in 120 min. It was also observed that the pH remained relatively constant from 5.5 to 5.0 with time. This was expected as ZnO is a known photocatalyst that, upon radiation with light whose wavelength is shorter than that of its bandgap, can generate electron-hole pair and hydroxyl radicals, strong oxidation agents that can oxidize a wide group of organic compounds nonspecifically. Figure 2(b) shows the UV spectra of OG at different reaction time periods. There were three major absorption peaks for OG dye, that is, 248, 330, and 479 nm. During the photocatalytic reaction, all three major absorption peaks were diminished. For example, at the wavelengths of 479, 330, and 248 nm, the original absorbance was 1.8514, 1.1891, and 2.4417, respectively. After 120 min of reaction, the absorbance of 479, 330, and 248 nm changed to 0, 0, and 0.0145, respectively. The figure illustrates the total removal of color by UV/ZnO system.

fig2
Figure 2: (a) Synergic effect of UV and ZnO on UV/ZnO photocatalytic system. (b) UV spectra of OG under UV/ZnO decolorization. The conditions were initial dye concentration of 50 mg L−1, ZnO loading of 60 g m−2, light intensity of 2.1 mW cm−2, and reaction time during 120 min.
3.2. Effect of Preparation Temperature and Mixing Speed

The effect of steel mesh supported ZnO preparation temperature on color removal was studied at the initial OG concentration of 50 mg L−1, ZnO load dosage of 60 g m−2, and 6 CCFL lamps in 120 min in the closed reactor. Figure 3(a) shows insignificant color removal differences in the range of 100–300°C. It was noted that pH remained unchanged at around 5 to 6. The reaction kinetics of UV/ZnO photocatalytic system was suggested to follow the Langmuir-Hinshelwood (L-H) reaction kinetics. And, in most of the designed reaction conditions, the L-H kinetic model of the UV/ZnO system can be further simplified into pseudo-first-order reaction kinetics. Therefore, the color removal of this study was treated using pseudo-first-order reaction as follows: where denotes the pseudo-first-order reaction rate constant (min−1), is the reaction time (min), designates the initial concentration (mg L−1) of OG, and is the concentration (mg L−1) of OG at time . The curve fitting of experimental results by (1) was shown in the figures as solid lines to demonstrate the consistence of kinetic model and experimental data. The calculated rate constants (from curve fitting) were 4.44, 4.37, 3.68, 4.32, and 4.57 (10−2) (min−1) at 100, 150, 200, 250, and 300°C, respectively. The preparation temperature shows neglected effect on OG color removal. Preparation temperature of 150°C was chosen as the working condition for its low energy consumption and fast dyeing speed. Figure 3(b) shows the effect of mixing speed on color removal under UV/ZnO photocatalytic system. Mixing speed is definitely an important factor that affects the color removal efficiency. From the results, the higher the mixing speed is, the faster the decolorizing reaction can be obtained. The calculated rate constants (from curve fitting) were 0.60, 2.78, 4.44, and 4.32 (10−2) (min−1) at 0, 50, 75, and 100 rpm, respectively. Therefore, the mixing speed was fixed at 75 rpm for further experimental runs. Since the photocatalytic degradation of OG happened on the surface of ZnO catalyst, the mass transfer of OG molecules from aqueous solution to the surface of ZnO catalyst was rather important to affect the reaction rate. The higher mixing speed caused better contact of OG molecules and ZnO catalyst and presented higher degradation rate of OG. However, when the mixing speed increased to higher than 75 rpm, the limited surface of ZnO cannot provide enough active sites for OG molecules. Therefore, the degradation rate of OG under UV/ZnO system hardly increased while the mixing speed was adjusted to higher than 75 rpm.

fig3
Figure 3: Effect of (a) preparation temperature and (b) mixing speed. The conditions were initial dye concentration of 50 mg L−1, ZnO loading of 60 g m−2, light intensity of 2.1 mW cm−2, and reaction time during 120 min.
3.3. Effect of ZnO Load Dosage

Figure 4(a) shows the removal of color as a function of load dosage of ZnO under 1.05 mW cm−2 of UV irradiation. Results indicated that the color removal increased from 89 to 98.5% in 60 min when the surface loading of ZnO particles increased from 8 to 60 g m−2. The color removal then decreased from 98.9 to 98.5% when the surface loading of ZnO increased from 60 to 67 g m−2. An optimal ZnO loading for color removal occurred at 60 gm−2. However, the differences of color removal rate between various ZnO loads were not significant. The rate constants followed similar trend to percent color removal; the observed rate constants were 0.66, 0.67, 1.25, 2.94, and 2.98 (10−2 min−1) at surface ZnO loading dosages of 8, 15, 30, 60, and 67 g m−2, respectively. From Figure 4(b), the TOC removal was 67.2% for ZnO loading of 8 g m−2 and increased up to 88.3% for ZnO loading of 60 g m−2. Results indicated that the TOC removal was highly affected by various ZnO loading dosages. On the other hand, ZnO dosage presented insignificant effect on color removal. To decolorize and mineralize simultaneously, one should choose higher ZnO loading to both color and TOC removal requirements.

fig4
Figure 4: Effect of surface loading of ZnO. The conditions were initial dye concentration of 50 mg L−1, light intensity of 1.05 mW cm−2, and reaction time during 120 min.
3.4. Effect of UV Light Intensity

Theoretically, the higher the UV light intensity applied to a photocatalytic system, the faster the electron-hole pairs and OH• free radical form to obtain the higher dye decolorization and mineralization rate. Thus, the rate constant increases by UV intensity increase, while the same ZnO catalyst surface is loading. Since the photolysis of ZnO catalyst is enhanced to produce abundant electron-hole pairs and OH• in the dye solution to be used for decolorization, it is obvious that the more UV intensity employed to the system is, the faster the dye is decolorized.

Figure 5(a) shows the removal of color as a function of UV intensity. Results indicated that the color removal increased from 71.6 to 98.8% in 60 min when the UV intensity increased from 20 to 120 W L−1. The rate constants followed similar trend to percent color removal; the observed rate constants were 2.01, 3.42, and 4.82 (10−2 min−1) at UV intensity which increased from 20, 60, and 120 W L−1, respectively, as shown in Table 2. Figure 5(b) presents the mineralization of OG in solution as a function of UV intensity. Results denote that the TOC removal increased from 38.2 to 88.3% in 120 min when the UV intensity increased from 20 to 120 W L−1. Therefore, applying sufficient UV intensity with ZnO photocatalyst can fairly mineralize portion of TOC to reach almost total mineralization.

tab2
Table 2: The first-order reaction rate constant k (102 min−1) for operating parameter of UV intensity and initial concentration.
fig5
Figure 5: Effect of UV light intensity on OG (a) decolorization and (b) mineralization by UV/ZnO photocatalytic system. The conditions were initial dye concentration of 50 mg L−1, ZnO-coated amounts of 60 g m−2, and UV light intensity of 20 to 120 W L−1 (120 W L−1 measured as 2.1 mW cm−2).

Figure 6 shows the relationship between pseudo-first-order rate constants and UV light intensity that a linear relationship can be obtained. This presents that the UV light intensity is an important operating parameter which linearly affects the decolorization of OG under UV/ZnO photocatalytic system. In this work, the maximum UV light intensity was 120 W L−1, which can be transferred into photo flux density as 2.1 mW cm−2. From previous studies, photocatalytic reaction rate constant is linearly increased with UV intensity while operating in low region of UV intensity, that is, between 0 and 20 mW cm−2 [17, 20]. The degradation of OG under UV/ZnO system was major caused by formation of OH• free radicals. From a previous study by Xiang et al., ZnO had the third highest formation rate of OH• free radicals following P25 and anatase TiO2 [26]. Under higher UV irradiation intensity, the formation rate of OH• free radicals was higher. This caused faster degradation reaction of OG under UV/ZnO system.

595031.fig.006
Figure 6: Effect of UV light intensity on pseudo-first-order rate constant of OG decolorization by UV/ZnO photocatalytic system. The conditions were the same as in Figure 5.
3.5. Effect of Dye Initial Concentration

To present the validity of L-H model on our CCFL/ZnO system, the effect of initial dye concentrations on the photodegradation of azo OG dye was studied at initial concentrations of 12.5–75 mg L−1, ZnO dosage of 60 gm−2, and 6 CCFL lamps for a period of 120 min in the closed reactor. Figure 7 shows results of dye photodegradation as a function of reaction time at various initial dye concentrations. Results indicated that the rate of dye removal decreased from 20.1 to 5.95 (10−2 min−1) when the initial dye concentration was increased from 12.5 to 50 mg L−1, as shown in Table 2. The rate constant then remained constant and independent of the dye concentration as the initial dye concentration increased to greater than 50 mg L−1. This is typical Langmuir-Hinshelwood (L-H) reaction kinetics which is generally capable of modeling UV/ZnO photocatalytic oxidation process [2730]. According to the L-H reaction kinetics, the rate of dye degradation can be described by the following equation: where is the degradation rate of dye (mg L−1 min−1) and , , and are the rate constant (mg L−1 min−1), equilibrium adsorption constant (L mg−1), and residual dye concentration (mg L−1), respectively. According to the above equation, at high dye concentration, that is, , the rate equation is Likewise, at low dye concentration, that is, , the above equation (2) becomes That is, as the initial concentration increases, the reaction no longer follows the first-order expression; it rather becomes independent of the dye concentration as shown in (3). By rearranging (2), one has where and are the initial rate (mg L−1 min−1) and initial dye concentration (mg L−1), respectively. A plot of the reciprocals of initial rate and initial concentration yields the rate constant, , and the adsorption constant, (Figure 8). The initial rate was calculated by the first 2 min of Figure 7 with ZnO loading dosage of 60 g m−2. From the slope () and the intercept () of Figure 8, the calculated and were 54.35 mg L−1 min−1 and 0.0055 mg−1 for ZnO loading dosage of 60 g m−2. The rate constants () obtained in this work of 54.35 mg L−1 min−1 were higher than that of previous works [2730] such as 1.66, 1.67, 0.95, and 0.17 mg L−1 min−1 for various dyes such as direct red 16, Remazol Black 5, Procion Red MX-5B, and indigo carmine, respectively. Similarly, the equilibrium adsorption constants () of 0.0055 L mg−1 from this work were in the range of previous studies, such as 0.0093, 0.072, 0.071, and 0.78 L mg−1, for various dyes as above. The results indicate that the photocatalytic degradation of Orange G by CCFL/ZnO process followed the Langmuir-Hinshelwood kinetic model with fairly good prediction of .

fig7
Figure 7: Effect of initial concentration on (a) ADMI color and (b) TOC removal. The conditions were ZnO-coated amounts of 60 gm−2, light intensity of 2.1 mW cm−2, and reaction time during 0–120 min.
595031.fig.008
Figure 8: Langmuir-Hinshelwood kinetic model (ZnO loading dosage of 60 g m−2 with light intensity of 2.1 mW cm−2).
3.6. Effect of pH

The effect of pH on the degradation of azo dye was conducted by adjusting the initial pH value of 5.0 to the range of 2 to 11 using HCl and/or NaOH with initial OG dye concentration of 50 mg L−1 and 60 g m−2 of ZnO dosage. Figure 9(a) shows OG dye removal as a function of time at various pH values. Results indicated that, at original pH, the color removal reached 78.5% in 30 min of photocatalytic reaction. At acidic pH of 2 and 3, the color removal rates of 76.7 and 76.1% were obtained, respectively. This implies that acidic pH provides no benefit for OG decolorization under UV/ZnO system. On the other hand, at alkaline pH of 11, the color removal rate sharply increased up to 95.6%. Figure 9(b) shows the TOC removal as a function of time at various pH values. Results indicated that, at original pH, the TOC removal reached 88.3% in 120 min of photocatalytic reaction. At acidic pH of 2 and 3, the color removal rates of 70.1 and 82.8% were obtained, respectively. At alkaline pH of 11, TOC removal rate was 87.8%. This implies that the TOC removal rate is rather stable in the range of 82.8–88.3 for pH range 3–11. And for pH 2, an extremely acidic condition, the TOC removal dropped from 12–18% to 70.1%. Extremely acidic pH has disadvantage for TOC removal under UV/ZnO system for OG solution, since 0.1 N HCl solution was used to adjust solution pH value to 2-3. At this operating condition, there were abundant amounts of high concentration chloride ions in the solution to play the role of free radical scavenger. Chloride ions competed with OG molecules to consume free radicals. Therefore, the decolorization and mineralization rate of OG by UV/ZnO system decreased. The observed rate constants for various pH values were summarized in Table 3.

tab3
Table 3: The first-order reaction rate constant k (102 min−1) for operating parameter of pH and duration.
fig9
Figure 9: Effect of initial pH on (a) decolorization and (b) mineralization of OG under UV/ZnO system. The conditions were initial dye concentration of 50 mg L−1, ZnO-coated amounts of 60 g m−2, light intensity of 2.1 mW cm−2, and reaction time during 120 min.
3.7. The Product Analysis by FTIR and IC

The change of functional groups of azo dye after photocatalytic treatment was surveyed. The initial dye concentration was 50 mg L−1 and was treated with a ZnO dosage of 60 g m−2 and reaction time of 120 min. The scan spectra (Figure 10(a)) for the functional groups are SO3Na of 1150~1250 cm−1, N=N of 1426, 1462 and 1495 cm−1, C=O of 1690~1760 cm−1, and C–H and N–H of 3300~3500 cm−1. After the photocatalytic oxidation (Figure 10(b)), a new double bond C=O at 1637 cm−1 was produced. Meanwhile, the N=N from dye at 1426, 1463, and 1496 cm−1 disappeared due to attack by the hydroxyl radicals that cleaved the double bond N=N. Accordingly, the dye molecule was degraded and decolorized. The ions such as sulfate, chloride, nitrite, and nitrate were determined. Figure 11(a) shows that the major ion concentration of sulfate significantly increased to 16 mg L−1 over time. The chloride ion produced due to the impurity of OG dye was as low as 1.5 mg L−1. The nitrate ion concentration was about from 1.0 to 4.5 mg L−1, and nitrite concentration was less than 0.5 mg L−1 as shown in Figure 11(b).

fig10
Figure 10: FTIR spectra for OG decolorization and demineralization (a) before and (b) after UV/ZnO photocatalytic degradation. The operating conditions were the same as in Figure 2.
fig11
Figure 11: The product analysis by IC, (a) and Cl, and (b) and . The conditions were initial dye concentration of 50 mg L−1, ZnO-coated amounts of 60 g m−2, and light intensity of 2.1 mW cm−2 at 120 min.
3.8. Application Duration

The steel mesh supported ZnO catalyst was used repeatedly to treat the OG solution. Figure 12 shows the system performance over 10 cycles. Results indicated that, although the rate of OG degradation decreased as the reuse cycle of catalyst increased, the total amount of dye removal remained relatively unchanged at 100% in the treatment time range of 100–120 min, however. Instead of ADMI color, the TOC removal decreased from 90 to 78% after ten experimental runs. In the meantime, there was nearly neglected loss (0.04%) of ZnO in each operation even after 10 cycles according to the solution Zn concentration analysis by atomic absorption. The observed rate constants declined with more reuse cycles as shown in Table 3 from 0.0441 to 0.0231 min−1, however. This can be attributed to potential surface poisoning of the photocatalyst, ZnO, due to adsorption of reaction products.

fig12
Figure 12: Duration test on (a) color and (b) TOC removal. The conditions were initial dye concentration of 50 mg L−1, ZnO-coated amounts of 60 gm−2, light intensity of 2.1 mW cm−2, and reaction time during 120 min.

4. Conclusions

Steel mesh supported ZnO catalyst illuminated with cold cathode fluorescent light (CCFL) UV was effective in the removal of ADMI color and TOC from the OG azo dye solution. Preparation temperature showed insignificant effect on color and TOC removal. An optimal ZnO surface loading or dosage of 60 g m−2 exhibited the highest color removal as well as the fastest rate; further increase in surface ZnO loading had no benefit in increasing the color removal, however. An alkaline pH of 11 had the best photocatalytic oxidation rate; the rate of color removal was stable in the range from pH 3 to 9. At pH 2, the TOC removal rate was the lowest among all pH range. The rate of color removal decreased with initial dye concentration as was expected by the Langmuir-Hinshelwood kinetics. The rate of color removal increased with UV intensity linearly. The ZnO-coated steel mesh can be repeatedly used over 10 cycles without significant loss of catalyst mass; the percent dye removal remained close to 100% in 10 cycles except for about 50% decrease in reaction rate constants apparently due to possible surface poisoning. Based on FTIR analysis, there was decrease of N=N bonding which indicated chemical transformation of the dye OG compound. Results of analyzing the inorganic byproducts revealed that sulfate production was predominant; nitrite and nitrate were produced at minor quantities.

Acknowledgments

The authors appreciate the research funding granted by the Taiwan National Science Foundation (NSC 98-2221-E-241-006-MY3) as well as the analysis by NSC Instrumental Center of the National Chung Hsing University and the National Tsing Hua University.

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