Effect of Fe(II/III) on tetracycline degradation under UV/VUV irradiation

Yao, Hong; Jin, Peng; Wang, Hui; Fu, Jie

doi:10.1016/j.cej.2016.09.074

Cited by 76 publications

(19 citation statements)

References 53 publications

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“…The results obtained were expected, while several studies describe the mechanisms by which divalent iron enhances the production of sulfate radicals [49,50]. However, it is important to consider that the mechanisms of radical production are multiple.…”

Section: Methylene Blue Discoloration By the Pms/fe 2+ /Uv Systemmentioning

confidence: 59%

“…As can be observed, the combination Fe 2+ with UV-A radiation did not reduce the MB concentration. However, the use of Fe 2+ /UV-C slightly increased the discoloration yield because when Fe 2+ is subjected to UV radiation around 250 nm, it is capable of dissociating water molecules or those of any compound with which it interacts, following the reaction mechanism described in Equation ( 1) [49].…”

Section: Resultsmentioning

confidence: 99%

“…For example, the dissociation action exerted by UV-C radiation on water molecules and PMS, which will provide radicals to the media and reaction intermediates, enhancing or reducing the activity of Fe 2+ to destroy pollutant molecules [13,51]. Other examples of reactions that occur in the media are those related to the oxidation of ferric compounds by the action of water that will provide hydroxyl radicals to the media [49]. Consequently, the decrease of the pollutant would occur not only by the oxidation caused by sulfate radicals, but also by a constant association and dissociation of molecules with iron due to photolysis of ferric compounds and regeneration of Fe 2+ .…”

Section: Methylene Blue Discoloration By the Pms/fe 2+ /Uv Systemmentioning

confidence: 99%

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Study of the Photocatalytic Activity of TiO2 and Fe2+ in the Activation of Peroxymonosulfate

González-Quiles

Andrés

Rodríguez-Chueca

2021

Water

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The increase in world population and human activities are leading to an increase in water stress in many regions of the planet, coupled with a decrease in the quality of water bodies. Advanced oxidation processes have demonstrated great potential for the reduction of almost any organic pollutant; however, it is necessary to intensify this type of treatment in order to reduce contact times and to reach a greater number of pollutants. The generation of sulfate radicals by activation of peroxymonosulfate (PMS) by divalent iron (Fe2+) and/or titanium dioxide (TiO2) were statistically studied to understand the role of these compounds as activators, using methylene blue as target pollutant because of its ease of handling and analysis. A factorial experimental design was used to study the influence of different variables (PMS, Fe2+, and TiO2) in the presence of UV-A or UV-C. There were relevant differences in the discoloration of methylene blue when analyzing the size of the effects and significance of the experiments, when UV-A or UV-C was used, being faster with UV-C. For instance, total discoloration of methylene blue was reached after 60 min with the system PMS/UV-C, while after 90 min only the 59% of methylene blue disappeared in presence of PMS/UV-A. Both Fe2+ and TiO2 in combination with PMS and UV increased the discoloration effect. So, in the presence of Fe2+, total discoloration of methylene blue was observed after 30 min in presence of UV-A, while this yield was reached in 7.5 min under UV-C. In the case of PMS/TiO2, it required 60 min under UV-A radiation to totally remove methylene blue, and around 15 min with UV-C. Statistically, the three variables were observed to have the main effect in combination with UV. Furthermore, the PMS/Fe2+ system has a significant interaction with UV-A and UV-C radiation, while the interaction of PMS/TiO2 was significant under UV-A, but with a negative effect under UV-C, or in other words the high elimination rates observed are achieved by the oxidation potential of UV-C, and the effect of PMS and TiO2 by itself.

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Section: Methylene Blue Discoloration By the Pms/fe 2+ /Uv Systemmentioning

confidence: 59%

Section: Resultsmentioning

confidence: 99%

Section: Methylene Blue Discoloration By the Pms/fe 2+ /Uv Systemmentioning

confidence: 99%

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Study of the Photocatalytic Activity of TiO2 and Fe2+ in the Activation of Peroxymonosulfate

González-Quiles

Andrés

Rodríguez-Chueca

2021

Water

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“…Its presence was ascribed to the fluorescence of C-T complexes of TC with Fe(III)-Cit, which was signalled by Smyk et al [ 36 ]. These complexes should form as the result of electron transfer from the benzene ring onto the quinone ring [ 48 ]. However, their formation requires the presence of a stacking complex formed by a nonoxidized and an oxidized molecule of TC.…”

Section: Resultsmentioning

confidence: 99%

Studies on the Efficiency of Iron Release from Fe(III)-EDTA and Fe(III)-Cit and the Suitability of These Compounds for Tetracycline Degradation

et al. 2022

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Iron ions can be used to degrade tetracycline dispersed in nature. Studies of absorption and fluorescence spectra and quantum chemistry calculations showed that iron is more readily released from Fe(III)-citrate than from Fe(III)-EDTA, so Fe(III)-citrate (Fe(III)-Cit) is more suitable for tetracycline (TC) degradation. At 30 °C, a severe degradation of TC by Fe(III)-Cit occurred as early as after 3 days of incubation in the light, and after 5 days in the dark. In contrast, the degradation of TC by Fe(III)-EDTA proceeded very slowly in the dark. By the fifth day of incubation of TC with Fe(III)-Cit in darkness, the concentrations of the former compound dropped by 55% and 75%, at 20 °C and 30 °C, respectively. The decrease in tetracycline concentrations caused by Fe(III)-EDTA in darkness at the same temperatures was only 2% and 6%, respectively. Light increased the degradation rates of TC by Fe(III)-EDTA to 20% and 56% at 20 °C and 30 °C, respectively. The key role of the light in the degradation of tetracycline by Fe(III)-EDTA was thus demonstrated. The TC degradation reaction showed a second-order kinetics. The rate constants of Fe(III)-Cit-induced TC degradation at 20 °C and 30 °C in darkness were k = 4238M−1day−1 and k = 11,330M−1day−1, respectively, while for Fe(III)-EDTA were 55 M−1day−1 and 226 M−1day−1. In light, these constants were k = 15,440M−1day−1 and k = 40,270 M−1day−1 for Fe(III)-Cit and k = 1012 M−1day−1 and 2050 M−1day−1 at 20 °C and 30 °C; respectively. A possible reason for the higher TC degradation rate caused by Fe(III)-Cit can be the result of its lower thermodynamical stability compared with Fe(III)-EDTA, which we confirmed with our quantum chemistry calculations. Two quantum chemistry calculations showed that the iron complex with EDTA is more stable (the free energy of the ensemble is 15.8 kcal/mol lower) than the iron complex with Cit; hence, Fe release from Fe(III)-EDTA is less effective.

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“…A literature review of E EO for the degradation of TET, CIP, SDZ and SMX displayed a diverse range of values (Table 3). Yao et al [58] evaluated the photodegradation of TET using 41.8 mW/cm 2 UV irradiation, obtaining an E EO value of 8.65 kWh/m 3 /order. Yao et al [58] obtained a higher rate constant than the one obtained in the present study by applying a light irradiation which was three times higher.…”

Section: Energy Consumptionmentioning

confidence: 99%

Photolytic and Photocatalytic Removal of a Mixture of Four Veterinary Antibiotics

Zambrano¹,

García‐Encina²,

Jiménez³

et al. 2022

SSRN Journal

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Effect of Fe(II/III) on tetracycline degradation under UV/VUV irradiation

Cited by 76 publications

References 53 publications

Study of the Photocatalytic Activity of TiO2 and Fe2+ in the Activation of Peroxymonosulfate

Study of the Photocatalytic Activity of TiO2 and Fe2+ in the Activation of Peroxymonosulfate

Studies on the Efficiency of Iron Release from Fe(III)-EDTA and Fe(III)-Cit and the Suitability of These Compounds for Tetracycline Degradation

Photolytic and Photocatalytic Removal of a Mixture of Four Veterinary Antibiotics

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