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Frontiers of Environmental Science & Engineering

ISSN 2095-2201

ISSN 2095-221X(Online)

CN 10-1013/X

Postal Subscription Code 80-973

2018 Impact Factor: 3.883

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Front. Environ. Sci. Eng.    2016, Vol. 10 Issue (4) : 9    https://doi.org/10.1007/s11783-016-0848-8
RESEARCH ARTICLE
Utilization of nano/micro-size iron recovered from the fine fraction of automobile shredder residue for phenol degradation in water
Jiwan SINGH1,*(),Yoon-Young CHANG1,Jae-Kyu YANG2,Seon-Hong KANG1,Janardhan Reddy KODURU3,*()
1. Department of Environmental Engineering, Kwangwoon University, Seoul 139-701, Republic of Korea
2. Division of General Education, Kwangwoon University, Seoul 139-701, Republic of Korea
3. Graduate School of Environmental Studies, Kwangwoon University, Seoul 139-701, Republic of Korea
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Abstract

Phenol removal by n/m Fe in the presence of H2O2 was highly effective.

Increasing the amounts of n/m Fe and H2O2?increased the phenol removal rate.

Phenol removal was decreased with an increase in the concentration of phenol.

The natural pH (6.9) of the solution was highly effective for phenol removal.

The pseudo-first-order kinetics was best fitted for the degradation of phenol.

The study investigates the magnetic separation of Fe from automobile shredder residue (ASR) (<0.25 mm) and its application for phenol degradation in water. The magnetically separated Fe was subjected to an ultrasonically assisted acid treatment, and the degradation of phenol in an aqueous solution using nano/micro-size Fe (n/m Fe) was investigated in an effort to evaluate the possibility of utilizing n/m Fe to remove phenol from wastewater. The prepared n/m Fe was analyzed by scanning electron microscopy (SEM) and Fourier transform infrared spectroscopy (FTIR). The effects of the dosages of n/mFe, pH, concentration of phenol and amount of H2O2 on phenol removal were evaluated. The results confirm that the phenol degradation rate was improved with an increase in the dosages of n/mFe and H2O2; however, the rate is reduced when the phenol concentration is higher. The degradation of phenol by n/mFe followed the pseudo-first-order kinetics. The value of the reaction rate constant (k) was increased as the amounts of n/m Fe and H2O2 increased. Conversely, the value of k was reduced when the concentration of phenol was increased. The probable mechanism behind the degradation of phenol by n/m Fe is the oxidation of phenol through hydroxyl radicals which are produced during the reaction between H2O2 and n/m Fe.
Keywords Automobile shredder residue (ASR)      Fe      Phenol      Scanning electron microscopy (SEM) and Fourier transform infrared spectroscopy (FTIR)      Mechanism     
PACS:     
Fund: 
Corresponding Author(s): Jiwan SINGH,Janardhan Reddy KODURU   
Issue Date: 30 May 2016
 Cite this article:   
Jiwan SINGH,Yoon-Young CHANG,Jae-Kyu YANG, et al. Utilization of nano/micro-size iron recovered from the fine fraction of automobile shredder residue for phenol degradation in water[J]. Front. Environ. Sci. Eng., 2016, 10(4): 9.
 URL:  
https://academic.hep.com.cn/fese/EN/10.1007/s11783-016-0848-8
https://academic.hep.com.cn/fese/EN/Y2016/V10/I4/9
Fig.1  Separation process and treatment of n/m Fe
Fig.2  (a) SEM image of n/m Fe (b) FTIR spectra of n/m Fe before and after the reaction with phenol
Fig.3  Effects of different amounts of n/m Fe on the phenol degradation process (test conditions: phenol concentration 10 mg·L−1, pH 6.9, concentration of H2O2 100 mM, temperature 25℃)
Fig.4  Phenol degradation efficiency with different doses of n/m Fe (a), (b) pH levels, (c) phenol concentrations and (d) H2O2 concentrations
n/mFe dose /( g·L-1) C0 (phenol) /(m g·L−1) initial pH H2O2 Conc. /mM k/min−1 t1/2 /min R2
0.15 10 6.9 100 0.0125 55.45 0.9469
0.25 10 6.9 100 0.0152 45.60 0.9062
0.50 10 6.9 100 0.0258 26.87 0.8737
1.0 10 6.9 100 0.0164 42.27 0.7401
1.5 10 6.9 100 0.0160 43.32 0.8554
0.50 10 2.0 100 0.0205 33.81 0.6584
0.50 10 3.0 100 0.0120 57.76 0.6954
0.50 10 4.0 100 0.0133 52.12 0.6479
0.50 10 5.0 100 0.0120 57.76 0.6024
0.50 5 6.9 100 0.0652 10.63 0.9718
0.50 20 6.9 100 0.0221 31.36 0.9178
0.50 40 6.9 100 0.0197 35.19 0.8682
0.50 10 6.9 0 0.0015 462.10 0.9217
0.50 10 6.9 25 0.0026 266.60 0.910
0.50 10 6.9 50 0.0063 110.02 0.9657
Tab.1  The kinetic results for phenol degradation by n/mFe
Fig.5  Effects of different pH levels on the phenol degradation process (test conditions: phenol concentration 10 mg·L−1, n/m Fe dose 0.50 g·L−1, concentration of H2O2 100 mM, temperature 25℃)
Fig.6  Effects of different concentrations of phenol on the phenol degradation process (test conditions: pH 6.9, n/m Fe dose: 0.50 g·L−1, concentration of H2O2 100 mM, temperature 25℃)
Fig.7  Effects of different concentrations of H2O2 on the phenol degradation process (test conditions: phenol concentration 10 mg·L-1, pH 6.9, n/m Fe dose: 0.50 g·L−1, temperature 25℃)
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