# Application of Recycled Zero-Valent Iron Nanoparticle to the Treatment of Wastewater Containing Nitrobenzene

Authors: Heon Lee; Byung-Hoon Kim; Young-Kwon Park; Sun-Jae Kim; Sang-Chul Jung
Journal: Journal of Nanomaterials
 (2015)

---

## Abstract

Zero-valent iron (ZVI) was synthesized using iron oxide, a byproduct of pickling line at a steel work. ZVI with a mean particle size of 500 nm was synthesized. The reaction activity of the synthesized ZVI was much higher than commercial ZVI. When applied to the decomposition of nitrobenzene (NB), the ZVI particles underwent corrosion and passivation oxide film formation, resulting in particle size decrease. The NB decomposition rate increased with increasing ZVI dosage level and with decreasing pH. The solution pH increased monotonously with increasing reaction duration, whereas the aniline concentration showed a maximum at 50 min. Based on the GC/MS analysis, NB is presumed to be reduced into aniline via reductive intermediates such as azobenzene and azoxybenzene. When combined with a subsequent biological process, the synthesized ZVI will be able to decompose NB in wastewater effectively.


---

## Body

## 1. Introduction

Nitrobenzene (NB) is an important feedstock material used widely for the production of various chemical products such as aniline, pharmaceuticals, dyes, and pesticides [1]. When disposed inadequately, however, NB can be a dangerous pollutant contaminating surface water and groundwater and hence endangering aquatic organisms and humans [2]. NB can be a significant threat to environment even at low concentrations [3]. Conventional biological treatment is often not effective in removing NB contained in water because of the electron-deficient character of nitro-groups that make NB resistant to the decomposition by microorganisms [4, 5]. A number of different advanced oxidation processes have been examined for the treatment of NB-containing wastewater: ozonation and O3/UV processes [6], photocatalysis [7], photoassisted Fenton oxidation [8], supercritical oxidation [9], and other processes [10]. However, these processes are either expensive or ineffective.Zero-valent iron (ZVI) is a mild reducing agent with a reduction potential of −0.440 V. It has been widely used as a reactive medium to reduce nitro compounds contained in groundwater because the reduced products (amido compounds) are much less toxic and can be biodegraded easily [11–13]. However, ZVI has an important drawback: high production cost. The production of ZVI from waste iron oxide generated in steel works is one way to reduce the production cost.In the steel industry, the oxide scale layer formed on the surface of carbon steel is removed using acid pickling process, during which waste acid is generated as a byproduct. Acid stock solution is recovered from this waste acid using roasting process, during which iron oxide (Fe2O3) is generated as a byproduct. Depending on the content of impurities, the iron oxide generated from the roasting process is divided into high-grade and low-grade iron oxides. High-grade iron oxide is used as ferrite, whereas low-grade iron oxide is used as pigment. Recent rapid growth of Chinese steel market has caused oversupply of low-grade iron oxide. Landfilling of iron oxide can cause the contamination of soil and groundwater. Therefore, finding new applications of low-grade iron oxide is in urgent need. Low-grade iron oxide was used in this study. Under the assumption that the price of low-grade iron oxide, which is mostly disposed as waste, is zero, the total cost of the synthesis of S-ZVI using transfer type reactor was calculated to be about 7 us$/kg. Hot-air dryers are installed in the pickling lines of steel works for drying iron oxide. Therefore, using these hot-air dryers can decrease the operation cost of transfer type reactor. In addition, the use of reducing gases, which are produced in the steel works as byproducts, can decrease further the cost of the synthesis of S-ZVI, making it virtually zero. Therefore, the S-ZVI production process is highly economical mass manufacturing process.We have reported the generation of ZVI from low-grade iron oxide using fixed-bed and transfer type reductor [14–16]. In this study, ZVI was applied to the degradation of NB contained in water. The activity of ZVI generated from low-grade iron oxide was compared with that of commercial ZVI. The effects of pH and ZVI dose on the NB degradation efficiency were investigated. The morphology, size, and composition of ZVI particles were observed using a transmission electron microscope (TEM) before and after the degradation experiments. The reductive products were analyzed using GC/MS measurements to suggest the mechanism for the degradation of NB in the presence of ZVI.


## 2. Materials and Methods

### 2.1. Zero-Valent Iron

ZVI was synthesized by reducing iron oxide obtained from the pickling line of a steel work located in Gwangyang city, South Korea. This ZVI will be referred to as S-ZVI hereafter. A transfer type reductor and H2 gas were used to reduce iron oxide. The physicochemical characteristics of iron oxide were reported in a previous study [14]. The characteristics and detailed synthesis procedure of S-ZVI were also reported previously [16]. Commercial iron powder (C-ZVI hereafter) with 98% purity and the particle diameter of 120~150 μm was purchased from Kanto Chemical Co. for the purpose of comparison.


### 2.2. Degradation Experiments

Nitrobenzene (C6H5NO2) purchased from Junsei Chemical Co. Ltd. was used as the target pollutant. The pH of reaction solution was adjusted using hydrochloric acid (Daejung Chemicals & Metals Co., Ltd.). Only reagent-grade chemicals and pure water (Daejung Chemicals & Metals Co., Ltd.) were used in this study. 1 mM NB solution was prepared by adding 0.12306 g of NB to 1 L of pure water and then stirring the mixture for 24 h. 100 mL of this solution and a certain amount (0.025~0.10 g) of ZVI were mixed in a 250 mL Erlenmeyer flask placed in a shaker to allow the NB degradation reaction to occur. Samples were taken after defined reaction durations from the reaction solution to measure the concentration and determine the reaction rate.


### 2.3. Analytical Methods

The NB concentration of the reaction solution was measured using high performance liquid chromatography (HPLC, model 1200, Agilent Co.) equipped with a C-18 column (ZORBAX Eclipse XDB, Agilent Co. Ltd., 150 mm × 4.6 mm, particle size 5μm). Samples were injected using an injection valve equipped with a 20 μL loop. Methanol and water mixture (70 : 30 v/v) was used as mobile phase, with a flow rate of 0.5 mL/min. The UV detector wavelength was set to 280 nm. The changes in morphology, size, and composition of S-ZVI particles were observed using high resolution field emission transmission electron microscope (HR-FETEM, JEM-2100F, JEOL). Gas chromatography mass spectrometer/headspace autosampler (GC/MS, QP2000, Shimadzu Co. Ltd.) equipped with HP 5 MS column (30 m × 0.25 mm × 0.25 μm) was used to analyze the reaction intermediates and to investigate the mechanism for the decomposition of NB by ZVI. After being maintained at 60°C for 2 min, GC/MS temperature was increased to 300°C at a rate of 30°C/min and then was maintained at the final temperature for 6 min.


## 2.1. Zero-Valent Iron

ZVI was synthesized by reducing iron oxide obtained from the pickling line of a steel work located in Gwangyang city, South Korea. This ZVI will be referred to as S-ZVI hereafter. A transfer type reductor and H2 gas were used to reduce iron oxide. The physicochemical characteristics of iron oxide were reported in a previous study [14]. The characteristics and detailed synthesis procedure of S-ZVI were also reported previously [16]. Commercial iron powder (C-ZVI hereafter) with 98% purity and the particle diameter of 120~150 μm was purchased from Kanto Chemical Co. for the purpose of comparison.


## 2.2. Degradation Experiments

Nitrobenzene (C6H5NO2) purchased from Junsei Chemical Co. Ltd. was used as the target pollutant. The pH of reaction solution was adjusted using hydrochloric acid (Daejung Chemicals & Metals Co., Ltd.). Only reagent-grade chemicals and pure water (Daejung Chemicals & Metals Co., Ltd.) were used in this study. 1 mM NB solution was prepared by adding 0.12306 g of NB to 1 L of pure water and then stirring the mixture for 24 h. 100 mL of this solution and a certain amount (0.025~0.10 g) of ZVI were mixed in a 250 mL Erlenmeyer flask placed in a shaker to allow the NB degradation reaction to occur. Samples were taken after defined reaction durations from the reaction solution to measure the concentration and determine the reaction rate.


## 2.3. Analytical Methods

The NB concentration of the reaction solution was measured using high performance liquid chromatography (HPLC, model 1200, Agilent Co.) equipped with a C-18 column (ZORBAX Eclipse XDB, Agilent Co. Ltd., 150 mm × 4.6 mm, particle size 5μm). Samples were injected using an injection valve equipped with a 20 μL loop. Methanol and water mixture (70 : 30 v/v) was used as mobile phase, with a flow rate of 0.5 mL/min. The UV detector wavelength was set to 280 nm. The changes in morphology, size, and composition of S-ZVI particles were observed using high resolution field emission transmission electron microscope (HR-FETEM, JEM-2100F, JEOL). Gas chromatography mass spectrometer/headspace autosampler (GC/MS, QP2000, Shimadzu Co. Ltd.) equipped with HP 5 MS column (30 m × 0.25 mm × 0.25 μm) was used to analyze the reaction intermediates and to investigate the mechanism for the decomposition of NB by ZVI. After being maintained at 60°C for 2 min, GC/MS temperature was increased to 300°C at a rate of 30°C/min and then was maintained at the final temperature for 6 min.


## 3. Results and Discussion

### 3.1. Characterization of S-ZVI

Figure1 shows HR-FETEM images of iron oxide and S-ZVIs. The size of iron oxide particles before the reduction to S-ZVI by H2 gas was approximately 200 nm (Figure 1(a)). This small particle size stems from the abrasion between floating particles during the synthesis in the fluidized bed roaster. The S-ZVI generated from iron oxide using a transfer type reactor was shown to have a much larger size than the iron oxide particles (Figure 1(b)). This was attributed to the sintering among the particles occurring during the reduction reaction at a high temperature (873 K). A previous study reported that the mean particle size of generated using a transfer type reactor increased with increasing reduction temperature [15]. The decomposition of NB using ZVI is usually conducted at low pH conditions to enhance the decomposition rate. In this study, the solution pH was lowered by adding HCl. The corrosion at a low pH was expected to change the morphology and size of ZVI particles. Therefore, the S-ZVI particles used for the NB decomposition at a pH of 2 were observed using HR-FETEM (Figures 1(c) and 1(d)). After the reaction for 30 min, the size of the S-ZVI particles slightly decreased (Figure 1(c)) compared to that before the reaction (Figure 1(b)) and the particle shape became sharper. When the reaction lasted for 60 min, much more significant decrease in particle size was observed (Figure 1(d)). This result indicates that S-ZVI particles were corroded into Fe2+ by the reaction with H+ ions, inducing the reduction of NB, accompanied by the change in particle shape and size. ZVI is dissolved as Fe2+ ions as the reaction proceeds and remaining iron mud can be removed using centrifugation and filtration.Figure 1
HR-FETEM images of iron oxide and S-ZVIs. (a) Iron oxide, (b) as-prepared S-ZVI, (c) S-ZVI after the reaction for 30 min, and (d) S-ZVI after the reaction for 60 min.
(a)
(b)
(c)
(d)The S-ZVI particles synthesized in this study are easily oxidized upon the exposure to air because of their nanoscale size. Therefore, iron particles reduced in the transfer type reactor were first cooled in an oxygen-free hopper and then placed in a nitrogen-filled glass bottle, which was stored in a low-temperature desiccator. Nevertheless, a passivation oxide film is formed on the surface of S-ZVI because of trace oxygen existing around the particles. However, this passivation oxide film has a positive effect of preventing rapid oxidation of S-ZVI. Figure2 compares the HR-FETEM images and energy dispersive spectroscopy (EDS) line scanning profiles of S-ZVI particles before the reaction (a) and after the reaction for 30 min at pH of 2 (b). The iron and oxygen content profiles shown in the right-hand side were obtained along the lines indicated in the left-hand-side images. The oxygen content shown in Figure 2(b) was much smaller than that shown in Figure 2(a), implying the corrosion of passivation oxide film during the NB decomposition reaction. Generally, the passivation oxide film of iron is composed of FeO, Fe2O3, and Fe3O4, which are readily corroded in acids. Reaction (1) is believed to be able to explain the corrosion of the passivation oxide film by HCl, added for pH adjustment:(1)
F
e
x
O
y
s
+
z
H
C
l
a
q
.
⟶
F
e
x
C
l
z
a
q
.
+
y
H
2
O
a
q
.
z
=
2
yFigure 2
HR-FETEM images and EDS line scanning profiles of S-ZVI. (a) As-prepared S-ZVI and (b) S-ZVI after the reaction for 30 min.
(a)
(b)


### 3.2. Effect of pH

The important role of pH in the NB decomposition using ZVI has been reported by several previous studies [17–19]. The effects of pH on the decomposition of NB using S-ZVI were examined in this study. Figure 3 shows the change in pH of reaction solution during the degradation of NB with the S-ZVI dosage of 1.0 g/L and the initial pH of 1.5. The solution pH increased monotonously with reaction time. Previous studies [12, 20] suggested that the corrosion ZVI producing hydroxide ions is the reason of pH increase during the decomposition of NB. O2 is the preferred oxidant under oxic conditions, leading to rapid corrosion as shown in Reaction (2). Further oxidation of Fe2+ may result in the formation of Fe3+:(2)
F
e
0
+
1
2
O
2
+
H
2
O
⟶
F
e
2
+
+
2
O
H
-Under anoxic conditions, on the other hand, water serves as the preferred oxidant as shown in Reaction (3):(3)
F
e
0
+
2
H
2
O
⟶
F
e
2
+
+
H
2
+
2
O
H
-Figure 3
The change in pH of reaction solution during the degradation of NB by S-ZVI. The dosage of S-ZVI was 1.0 g/L and initial pH of solution was 1.5.


### 3.3. Degradation Kinetics of NB by ZVIs

The activity of S-ZVI synthesized in this study was compared with that of C-ZVI. Figure4 shows the NB concentration decays obtained with the two ZVIs. The dosage of ZVI was 1.0 g/L and the solution pH was 2.0. The NB removal using C-ZVI was represented well by the pseudo first-order kinetic model with a reaction rate constant of 0.05032 min−1. On the other hand, the NB removal using S-ZVI could not be explained by a first-order reaction. When the reaction rate constants were calculated based on the first-order kinetics, the reaction rate constant obtained with S-ZVI was 2.65 times larger than that obtained with C-ZVI. This result was attributed to the large difference in the particle diameters of C-ZVI (120~150 μm) and S-ZVI (~500 nm) and hence the large difference in the particle surface area. Reportedly, the dechlorination of halocarbon is influenced strongly by the surface area of ZVI particles [21, 22]. This is in good agreement with the result of this study showing a significant effect of ZVI particle surface area on the NB decomposition rate. This result implies that the reactive sites on the ZVI particles are involved in the decomposition of NB.Figure 4
Comparison of the activities of C-ZVI and S-ZVI for the degradation of NB. The dosage of ZVI was 1.0 g/L and pH of solution was 2.0.In the presence of ZVI, the reduction of nitro group is the dominant process for the transformation of NB. The reduction of NB by ZVI produces aniline during which nitrosobenzene and phenylhydroxylamine are formed as reaction intermediates as shown in Reactions (4)–(7) [12]:(4)
F
e
0
⟶
F
e
2
+
+
2
e
-
(5)
C
6
H
5
N
O
2
+
2
H
+
+
2
e
-
⟶
C
6
H
5
N
O
+
H
2
O
(6)
C
6
H
5
N
O
+
2
H
+
+
2
e
-
⟶
C
6
H
5
N
H
O
H
(7)
C
6
H
5
N
H
O
H
+
2
H
+
+
2
e
-
⟶
C
6
H
5
N
H
2
+
H
2
OThe overall reaction can then be written as(8)
C
6
H
5
N
O
2
+
3
F
e
0
+
6
H
+
⟶
C
6
H
5
N
H
2
+
3
F
e
2
+
+
2
H
2
OThe participation of H+ in the overall reaction indicates the role of pH determining the decomposition rate of NB. Figure 5 compares the decays of NB concentration obtained with different solution pH values (1.5~5). The dosage of S-ZVI was 1.0 g/L. The NB decomposition rate increased with decreasing pH. In particular, the effect of pH was dramatic when pH was lower than 2.5. More than 99.9% of NB was decomposed within 30 min at pH of 1.5. Rejuvenation of ZVI by aqueous Fe2+ was also reported by previous studies [18, 23]. Fe2+ released under weak acidic conditions played a significant role in promoting the reaction [18]. High pH leads to the formation of iron hydroxide precipitates on the ZVI particle surface (passivation oxide film), limiting further dissolution and hence reducing the NB decomposition rate.Figure 5
Decay of NB concentration obtained with different solution pH values. The dosage of S-ZVI was 1.0 g/L.The effect of S-ZVI dosage on the NB decomposition rate was examined. Figure6 compares the NB concentration decays obtained with different dosage levels of S-ZVI. The solution pH was 2.0. The NB removal rate increased with increasing S-ZVI dosage. The pseudo first-order kinetic theory explained well the NB decomposition obtained with small S-ZVI dosage levels, whereas the result obtained with the largest S-ZVI dosage level (1.00 g) could not be represented by the pseudo first-order kinetic theory.Figure 6
Decay of NB concentration obtained with different S-ZVI dosage levels. The solution pH was 2.0.


### 3.4. Reductive Pathways of NB by S-ZVI

GC/MS analysis was performed to investigate the main products and mechanism of NB decomposition by S-ZVI. Figure7 shows the GC/MS spectra of the reductive products of NB obtained with the initial NB concentration of 1 mM, the solution pH of 2.0, the reaction time of 20 min, and the S-ZVI dosage level of 1.00 g/L. Peaks were observed at the retention times of 3.93 min ((a), aniline), 4.80 min ((b), nitrobenzene), 7.45 min ((c), azobenzene), and 8.28 min ((d), azoxybenzene). The reduction of NB by ZVI is known to produce aniline via nitrosobenzene and phenyl hydroxylamine, forming azobenzene and azoxybenzene as reaction intermediates [5]. Figure 7 shows that the reaction for 20 min in the presence of S-ZVI removed NB (peak (b)) considerably, while forming reductive products such as azobenzene, azoxybenzene, and aniline.Figure 7
GC/MS spectra of the reductive products of NB by S-ZVI. Initial concentration of NB: 1 mM; pH of solution: 2.0; reaction time: 20 min.Figure8 shows the aniline content in the product obtained from GC/MS spectra as a function of reaction time. The aniline content initially increased with reaction time but decreased after 50 min. The reduction in the aniline content after 50 min was attributed to the degradation of aniline induced by Fe2+ ions produced by the oxidation of S-ZVI.Figure 8
Content of aniline as a function of reaction time obtained at pH 2.0.Based on the GC/MS analysis results, the mechanism for NB decomposition in the presence of S-ZVI was proposed (Figure9). Hydrated electrons released from Reaction (4) deoxidize NB to nitrosobenzene. Further reduction of nitrosobenzene produces aniline. Azobenzene and azoxybenzene are produced as a result of the combination of reactive intermediates during the deoxidization processes. The biodegradability of aniline is known to be much higher than that of NB [5]. Therefore, NB in wastewaters can be effectively removed by combining the reduction using S-ZVI and subsequent biological processes.Figure 9
Pathways of reductive degradation of NB by S-ZVI.


## 3.1. Characterization of S-ZVI

Figure1 shows HR-FETEM images of iron oxide and S-ZVIs. The size of iron oxide particles before the reduction to S-ZVI by H2 gas was approximately 200 nm (Figure 1(a)). This small particle size stems from the abrasion between floating particles during the synthesis in the fluidized bed roaster. The S-ZVI generated from iron oxide using a transfer type reactor was shown to have a much larger size than the iron oxide particles (Figure 1(b)). This was attributed to the sintering among the particles occurring during the reduction reaction at a high temperature (873 K). A previous study reported that the mean particle size of generated using a transfer type reactor increased with increasing reduction temperature [15]. The decomposition of NB using ZVI is usually conducted at low pH conditions to enhance the decomposition rate. In this study, the solution pH was lowered by adding HCl. The corrosion at a low pH was expected to change the morphology and size of ZVI particles. Therefore, the S-ZVI particles used for the NB decomposition at a pH of 2 were observed using HR-FETEM (Figures 1(c) and 1(d)). After the reaction for 30 min, the size of the S-ZVI particles slightly decreased (Figure 1(c)) compared to that before the reaction (Figure 1(b)) and the particle shape became sharper. When the reaction lasted for 60 min, much more significant decrease in particle size was observed (Figure 1(d)). This result indicates that S-ZVI particles were corroded into Fe2+ by the reaction with H+ ions, inducing the reduction of NB, accompanied by the change in particle shape and size. ZVI is dissolved as Fe2+ ions as the reaction proceeds and remaining iron mud can be removed using centrifugation and filtration.Figure 1
HR-FETEM images of iron oxide and S-ZVIs. (a) Iron oxide, (b) as-prepared S-ZVI, (c) S-ZVI after the reaction for 30 min, and (d) S-ZVI after the reaction for 60 min.
(a)
(b)
(c)
(d)The S-ZVI particles synthesized in this study are easily oxidized upon the exposure to air because of their nanoscale size. Therefore, iron particles reduced in the transfer type reactor were first cooled in an oxygen-free hopper and then placed in a nitrogen-filled glass bottle, which was stored in a low-temperature desiccator. Nevertheless, a passivation oxide film is formed on the surface of S-ZVI because of trace oxygen existing around the particles. However, this passivation oxide film has a positive effect of preventing rapid oxidation of S-ZVI. Figure2 compares the HR-FETEM images and energy dispersive spectroscopy (EDS) line scanning profiles of S-ZVI particles before the reaction (a) and after the reaction for 30 min at pH of 2 (b). The iron and oxygen content profiles shown in the right-hand side were obtained along the lines indicated in the left-hand-side images. The oxygen content shown in Figure 2(b) was much smaller than that shown in Figure 2(a), implying the corrosion of passivation oxide film during the NB decomposition reaction. Generally, the passivation oxide film of iron is composed of FeO, Fe2O3, and Fe3O4, which are readily corroded in acids. Reaction (1) is believed to be able to explain the corrosion of the passivation oxide film by HCl, added for pH adjustment:(1)
F
e
x
O
y
s
+
z
H
C
l
a
q
.
⟶
F
e
x
C
l
z
a
q
.
+
y
H
2
O
a
q
.
z
=
2
yFigure 2
HR-FETEM images and EDS line scanning profiles of S-ZVI. (a) As-prepared S-ZVI and (b) S-ZVI after the reaction for 30 min.
(a)
(b)


## 3.2. Effect of pH

The important role of pH in the NB decomposition using ZVI has been reported by several previous studies [17–19]. The effects of pH on the decomposition of NB using S-ZVI were examined in this study. Figure 3 shows the change in pH of reaction solution during the degradation of NB with the S-ZVI dosage of 1.0 g/L and the initial pH of 1.5. The solution pH increased monotonously with reaction time. Previous studies [12, 20] suggested that the corrosion ZVI producing hydroxide ions is the reason of pH increase during the decomposition of NB. O2 is the preferred oxidant under oxic conditions, leading to rapid corrosion as shown in Reaction (2). Further oxidation of Fe2+ may result in the formation of Fe3+:(2)
F
e
0
+
1
2
O
2
+
H
2
O
⟶
F
e
2
+
+
2
O
H
-Under anoxic conditions, on the other hand, water serves as the preferred oxidant as shown in Reaction (3):(3)
F
e
0
+
2
H
2
O
⟶
F
e
2
+
+
H
2
+
2
O
H
-Figure 3
The change in pH of reaction solution during the degradation of NB by S-ZVI. The dosage of S-ZVI was 1.0 g/L and initial pH of solution was 1.5.


## 3.3. Degradation Kinetics of NB by ZVIs

The activity of S-ZVI synthesized in this study was compared with that of C-ZVI. Figure4 shows the NB concentration decays obtained with the two ZVIs. The dosage of ZVI was 1.0 g/L and the solution pH was 2.0. The NB removal using C-ZVI was represented well by the pseudo first-order kinetic model with a reaction rate constant of 0.05032 min−1. On the other hand, the NB removal using S-ZVI could not be explained by a first-order reaction. When the reaction rate constants were calculated based on the first-order kinetics, the reaction rate constant obtained with S-ZVI was 2.65 times larger than that obtained with C-ZVI. This result was attributed to the large difference in the particle diameters of C-ZVI (120~150 μm) and S-ZVI (~500 nm) and hence the large difference in the particle surface area. Reportedly, the dechlorination of halocarbon is influenced strongly by the surface area of ZVI particles [21, 22]. This is in good agreement with the result of this study showing a significant effect of ZVI particle surface area on the NB decomposition rate. This result implies that the reactive sites on the ZVI particles are involved in the decomposition of NB.Figure 4
Comparison of the activities of C-ZVI and S-ZVI for the degradation of NB. The dosage of ZVI was 1.0 g/L and pH of solution was 2.0.In the presence of ZVI, the reduction of nitro group is the dominant process for the transformation of NB. The reduction of NB by ZVI produces aniline during which nitrosobenzene and phenylhydroxylamine are formed as reaction intermediates as shown in Reactions (4)–(7) [12]:(4)
F
e
0
⟶
F
e
2
+
+
2
e
-
(5)
C
6
H
5
N
O
2
+
2
H
+
+
2
e
-
⟶
C
6
H
5
N
O
+
H
2
O
(6)
C
6
H
5
N
O
+
2
H
+
+
2
e
-
⟶
C
6
H
5
N
H
O
H
(7)
C
6
H
5
N
H
O
H
+
2
H
+
+
2
e
-
⟶
C
6
H
5
N
H
2
+
H
2
OThe overall reaction can then be written as(8)
C
6
H
5
N
O
2
+
3
F
e
0
+
6
H
+
⟶
C
6
H
5
N
H
2
+
3
F
e
2
+
+
2
H
2
OThe participation of H+ in the overall reaction indicates the role of pH determining the decomposition rate of NB. Figure 5 compares the decays of NB concentration obtained with different solution pH values (1.5~5). The dosage of S-ZVI was 1.0 g/L. The NB decomposition rate increased with decreasing pH. In particular, the effect of pH was dramatic when pH was lower than 2.5. More than 99.9% of NB was decomposed within 30 min at pH of 1.5. Rejuvenation of ZVI by aqueous Fe2+ was also reported by previous studies [18, 23]. Fe2+ released under weak acidic conditions played a significant role in promoting the reaction [18]. High pH leads to the formation of iron hydroxide precipitates on the ZVI particle surface (passivation oxide film), limiting further dissolution and hence reducing the NB decomposition rate.Figure 5
Decay of NB concentration obtained with different solution pH values. The dosage of S-ZVI was 1.0 g/L.The effect of S-ZVI dosage on the NB decomposition rate was examined. Figure6 compares the NB concentration decays obtained with different dosage levels of S-ZVI. The solution pH was 2.0. The NB removal rate increased with increasing S-ZVI dosage. The pseudo first-order kinetic theory explained well the NB decomposition obtained with small S-ZVI dosage levels, whereas the result obtained with the largest S-ZVI dosage level (1.00 g) could not be represented by the pseudo first-order kinetic theory.Figure 6
Decay of NB concentration obtained with different S-ZVI dosage levels. The solution pH was 2.0.


## 3.4. Reductive Pathways of NB by S-ZVI

GC/MS analysis was performed to investigate the main products and mechanism of NB decomposition by S-ZVI. Figure7 shows the GC/MS spectra of the reductive products of NB obtained with the initial NB concentration of 1 mM, the solution pH of 2.0, the reaction time of 20 min, and the S-ZVI dosage level of 1.00 g/L. Peaks were observed at the retention times of 3.93 min ((a), aniline), 4.80 min ((b), nitrobenzene), 7.45 min ((c), azobenzene), and 8.28 min ((d), azoxybenzene). The reduction of NB by ZVI is known to produce aniline via nitrosobenzene and phenyl hydroxylamine, forming azobenzene and azoxybenzene as reaction intermediates [5]. Figure 7 shows that the reaction for 20 min in the presence of S-ZVI removed NB (peak (b)) considerably, while forming reductive products such as azobenzene, azoxybenzene, and aniline.Figure 7
GC/MS spectra of the reductive products of NB by S-ZVI. Initial concentration of NB: 1 mM; pH of solution: 2.0; reaction time: 20 min.Figure8 shows the aniline content in the product obtained from GC/MS spectra as a function of reaction time. The aniline content initially increased with reaction time but decreased after 50 min. The reduction in the aniline content after 50 min was attributed to the degradation of aniline induced by Fe2+ ions produced by the oxidation of S-ZVI.Figure 8
Content of aniline as a function of reaction time obtained at pH 2.0.Based on the GC/MS analysis results, the mechanism for NB decomposition in the presence of S-ZVI was proposed (Figure9). Hydrated electrons released from Reaction (4) deoxidize NB to nitrosobenzene. Further reduction of nitrosobenzene produces aniline. Azobenzene and azoxybenzene are produced as a result of the combination of reactive intermediates during the deoxidization processes. The biodegradability of aniline is known to be much higher than that of NB [5]. Therefore, NB in wastewaters can be effectively removed by combining the reduction using S-ZVI and subsequent biological processes.Figure 9
Pathways of reductive degradation of NB by S-ZVI.


## 4. Conclusions

ZVI synthesized from the iron oxide generated in a pickling line at a steel work was applied to the decomposition of NB in wastewater. The reaction activity and mechanism were evaluated experimentally. The conclusions obtained from the experiments are as follows:(1)
The particle size of the synthesized ZVI was larger than that of feedstock iron oxide particles due to sintering. The NB decomposition reaction made the S-ZVI particles smaller.
(2)
HR-FETEM observation indicated the formation of passivation oxide film and the corrosion of iron in the NB solution.
(3)
The NB decomposition rate increased with increasing S-ZVI dosage level and with decreasing pH.
(4)
S-ZVI was superior to C-ZVI in terms of NB decomposition activity, which was attributed to smaller particle size (larger surface area) and hence more reactive sites.
(5)
The solution pH increased monotonously with reaction time. The aniline concentration increased with reaction time up to 50 min and then decreased.
(6)
GC/MS analysis showed that NB is reduced to aniline via reductive products such as azobenzene and azoxybenzene.



---

*Source: 392537-2015-11-25.xml*