Ying-Chao
Huo
ab,
Wen-Wei
Li
*b,
Di
Min
b,
Dan-Dan
Wang
a,
Hou-Qi
Liu
a,
Qin
Kong
a,
Tai-Chu
Lau
ac and
Raymond J.
Zeng
*ab
aAdvanced Laboratory for Environmental Research & Technology (ALERT), USTC-CityU, Suzhou 215123, China. E-mail: rzeng@ustc.edu.cn; Fax: +8655163601592; Tel: +8655163600203
bCAS for Unban Pollutant Conversion, Department of Chemistry, University of Science and Technology of China, Hefei 230026, China. E-mail: wwli@ustc.edu.cn; Fax: +8651287161381; Tel: +8651287161361
cDepartment of Biology and Chemistry, City University of Hong Kong, Tat Chee Avenue, Kowloon, Hong Kong SAR, Hong Kong, China
First published on 15th June 2015
Zero-Valent Iron nanoparticles (nZVI) have been extensively applied for the reduction of various recalcitrant organic contaminants, but their reactivity usually declines over time due to the formation of passive iron oxides. In this study we observed a sustained reactivity of nZVI for the dechlorination of carbon tetrachloride (CT) in water during several consecutive reaction cycles. The dechlorination rate constants increased substantially in Cycle 2, then remained at a high level over several consecutive cycles, and ultimately declined in Cycle 7. In the entire process, the solution pH increased only slightly from 7.0 to 7.8, which was different from other unbuffered nZVI reduction systems reported before. Characterization of the particle surface morphology and composition revealed an important role of Fe oxyhydroxide formation in self-buffering the solution pH and sustaining a high nZVI reactivity. Our study provides new knowledge on the nZVI dechlorination process and may offer implications for extending the lifetime of nZVI in wastewater treatment and environmental remediation applications.
In this study, we aim to clarify how solution pH would change during CT reduction by nZVI, and whether nZVI, which would become aged with the reaction proceeding, could remain its activity. The dechlorination kinetics of nZVI during several consecutive reaction cycles were investigated. Impacts of pH and ferrous ion on the reaction kinetics were also evaluated. The variations in surface morphologies and compositions of Fe materials were characterized by scanning electron microscopy (SEM), energy dispersive spectrometer (EDS), X-ray diffraction (XRD) and X-ray photoelectron spectroscopy (XPS). An unusual high reactivity of nZVI and self-buffering solution pH during the decholorination process was demonstrated in this study. The underlying mechanisms were elucidated.
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Fig. 1 Reductive degradation of CT by nZVI for the first cycle. Lines show the fits of the data to the model of CT degradation and CF formation. Error bars represent the ranges of duplicate samples. |
Two pathways of CT reductive-transformation have been recognized so far: hydrogenolysis and carbene hydrolysis. Hydrogenolysis can occur through one- or two-electron transfer pathway. One-electron reduction of CT generates a trichloromethyl free radical (˙CCl3) that can abstract hydrogen ([H]) to form CF.12 In the two-electron pathway, the formed ˙CCl3 is further reduced to obtain a trichloromethyl carbanion ([:CCl3]−) and form CF.13 The formation of trichloromethyl carbanion during the two-electron hydrogenolysis can further undergo α-elimination pathway to form dichlorocarbene (:CCl2) via carbene hydrolysis.14 In this study, generation of DCM was observed only when a complete degradation of CT was achieved. In addition, methane was not detected throughout the experiments (Fig. S1†). Perchloroethylene (PCE) was detected during the degradation (Fig. S1†), which confirms the presence of trichloromethyl free radical.
The kinetics of CT dechlorination and CF formation in the nZVI system can be described by the pseudo-first-order kinetic equation (eqn (1) and (2)).
CT degradation:
[CT]t = [CT]0e−k1t | (1) |
CF formation:
![]() | (2) |
The fitting curves of CT degradation and CF formation data are also shown in Fig. 1. The correlation coefficients were both above 0.992, indicating a good fitting between the experimental data and kinetic values. The estimated reduction rate constants in the first reaction cycle were 0.213 h−1 for k1 and 0.058 h−1 for k2.
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Fig. 2 Reductive dechlorination kinetics of CT by nZVI for seven cycles. Error bars are the ranges of duplicate samples. |
Interestingly, the CT degradation rate constants showed no significant variation (p > 0.05) during Cycles 2–6, but decreased sharply in Cycle 7. A similar variation trend of CT dechlorination kinetics was observed by Sarathy et al.8 who used nZVI of different aging degrees as the reductive agent. In our study, the aging process occurred spontaneously over the reaction process and pH was not controlled, which can better reflect the real process of nZVI corrosion in natural environment.
The reductive chlorination activity of ZVI is governed by the iron surface components and properties. Notably, anaerobic dechlorination (eqn (3)) and hydrolysis (eqn (4)) are usually accompanied with pH increase and ferrous ions accumulation, which might in turn affect the dechlorination kinetics.
Fe0 + R–Cl + H+ → Fe2+ + R–H + Cl− | (3) |
Fe0 + 2H+ → Fe2+ + H2 | (4) |
It is known that the solution pH could substantially affect the reaction products18 and species of formed Fe oxides.19 On the other hand, the ferrous accumulated during the reaction might play multiple roles in affecting the system reductive activity. For instance, Fe(II) adsorbed on iron oxides could directly reduce a variety of pollutions.20 However, deposition of some iron oxides on the nZVI surface could also significantly block the electron transfer and decrease the reaction activity. To clarify the inter-correlations between pH and ferrous ion and their roles in dechlorination, the CT degradation under different ferrous concentration and initial pH conditions were tested.
Fig. 4a shows that CT was completely dechlorinated within 3 h for Fe(II)-3, while it took 8 and 10 hours for Fe(II)-2 and Fe(II)-1 respectively, and no CT dechlorination occurred in the nZVI-free system. This result suggests that, although ferrous ions itself cannot reduce CT, the CT degradation rate was positively correlated to the ferrous concentration when nZVI was present. The final pH of the mixtures were 8.7, 8.2 and 7.7 for Fe(II)-1, Fe(II)-2, Fe(II)-3, respectively (Fig. 4b). The inverse correlation between pH and the added ferrous amount might be due to: (1) ferrous combines with hydroxide ion to form iron oxides and oxyhydroxides, resulting in decreased OH− concentration; (2) ferrous leads to proton release by substituting the H atom of Fe oxyhydroxides (reactions (5) and (6)).21
≡FeOH + Fe2+ ↔ FeOFe(II)+ + H+ | (5) |
≡FeOH2+ + Fe2+ ↔ FeOFe(II)+ + 2H+ | (6) |
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Fig. 4 (a) CT reductive dechlorination by nZVI with different addition of ferrous and (b) the final pH. Error bars are the ranges of duplicate samples. |
According to the above mechanism, the continously-generated ferrous during the dechlorination might serve as an effective buffer to neutralize the alkali produced from nZVI corrosion, thereby sustaining a stable pH in the entire reaction process (Fig. 3). This self-buffered pH due to formation of iron oxyhydroxides might also be one important reason for the sustained high dechlorination activity of nZVI over the consecutive reaction cycles. As evidenced in Fig. 5, significantly higher CT dechlorination rate was obtained in neutral pH system (0.211 h−1 for pH-7 versus 0.110 h−1 for pH-10). Under alkaline condition, the dechlorination thermodynamics becomes less favorable and meanwhile a thick iron oxides coat would be built on the particle surface, severely blocking the electron transfer from the iron core.9,22,23
SEM examination revealed that the initial nZVI contained abundant nanosphere clusters (Fig. 6a), which was typical of nZVI particles. The nanosphere sizes were in the range of 50–200 nm. The EDS result clearly showed the elemental mapping of Fe and O in the nanonecklace structure (Fig. 6b), implying that the nZVI used in our study was slightly oxidized. This happens frequently during the synthesis, drying, storage and application processes, where nZVI with high activity could be easily oxidized to form a thin layer of iron oxides on the surface when exposed to the atmosphere or water. However, the morphology and components of nZVI changed significantly after three dechlorination cycles. Both the number and size of nanospheres decreased, while large amount of platy Fe oxide minerals with bulk and laminated structures were formed (Fig. 6c and S4b†). Notably, the particle area and the bulk mineral area showed no significant difference in the iron and oxygen contents, indicating a similar composition of the iron hydroxides on the particle surface in the precipitate (Fig. S4b†). In addition, the EDS data showed that the oxygen content increased from 6% in the initial nZVI to 25% after Cycle 3 (Fig. 6b and d). These results confirm that Fe oxyhydroxides were formed accompanied with the continuous ZVI corrosion. These newly-formed porous Fe oxides posed insignificant impacts on the corrosion of the ZVI particles and might even directly contribute to CT dechlorination by utilizing the adsorbed Fe(II).17 At the end of the experiment, more bulk and dense-structured iron precipitates were observed, which might hamper the electron transfer from the buried particles ZVI particles (Fig. S3 and S4†).
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Fig. 6 (a) SEM image and (b) EDS analysis of initial nZVI; (c) SEM image and (d) EDS analysis of aged nZVI after Cycle 3. |
The variations of nZVI composition during reaction were validated by XRD and XPS. Pure Fe, with the XRD peaks of 44.9 and 65.0°, was identified for the initial nZVI Fe (Fig. 7a). However, the XRD signal was weak, indicating a relatively low crystallinity. Meanwhile, no distinct peaks of iron oxides were observed, implying a small amount or poor crystallinity of the oxides shell.24 The XPS spectra revealed that only elements Fe, O, and C existed in the original nZVI (Fig. S5a†). The C1s peak at 284.8 eV should be attributed to the adventitious carbon (Fig. S5b†). For the original nZVI, two narrow distinct peaks of similar intensity, 709.89 eV and 710.95 eV, separated by about 1 eV were detected (Fig. 8a). The peak positions were consistent with the literature values of 709.7 and 710.8 eV assigned to Fe2p3/2 for α-Fe2O3. Two other prominent peaks also occurred, which are ascribed to a satellite band at 719.30 about 8 eV above the Fe (2p3/2) line and the shoulder peak at 724.50 eV in the high resolution spectra.25 These data confirm that the oxide shells of the Fe(0) core were Fe2O3. Besides the predominant peaks of Fe in Fe2O3, a peak at a low binding energy of 706.9 eV, attributed to Fe2p1/2 in pure Fe, was also detected, indicating that the thickness of the Fe2O3 shell was less than 10 nm since the XPS could only detect the photoelectrons from the outer surface of 10 nm.
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Fig. 8 High resolution XPS spectra of (a) Fe2p and (b) O1s for initial nZVI; high resolution XPS spectra of (c) Fe2p and (d) O1s for aged nZVI after Cycle 3. |
After three CT dechlorination cycles, obvious peaks of iron oxides and oxyhydroxides occurred while the peaks of Fe(0) remained, suggesting a significant change of the iron oxides composition. It has been reported that certain iron oxides/oxyhydroxides, such as green rust, ferrihydrite and magnetite, could promote the reductive transformation of contaminants.26,27 The evolution of surface chemical compositions of nZVI during the reaction was further convinced by XPS analysis. The peaks of pure iron disappeared after Cycle 3 (Fig. 8c), likely due to decreased Fe(0) content and the inclusion of Fe particles within the Fe oxides matrixes. The high-resolution XPS spectra of O1s could be fitted by two peaks at binding energies of about 529.77 and 531.02 eV, respectively (Fig. 8b and d). The dominant peak at 529.77 eV is assigned to the lattice oxygen of Fe (Fe2O3), while the other O1s peaks at around 531.02 eV is ascribed to adsorbed hydroxyl (Fe-OHad), lattice hydroxyl (Fe-OHlattice) and water (H2O),28 which we denoted as bonded-OH here. It is obvious that the bounded-OH content increased during the dechlorination, which is in accordance with the strengthened signals of Fe oxyhydroxides detected by XRD (Fig. 7b).
With the further proceeding of dechlorination reactions, other ion oxides such as magnetite, hematite and goethite also occurred at the end of the experiments, as demonstrated by the XRD data (Fig. S6†). The formation of these iron oxides could suppress the reduction of chlorinated organics.29 Therefore, these inactive iron oxides might form a matrix of dense structure and block the electron transfer from the buried nZVI particles. In addition, the amount of nZVI might become limiting at this stage due to continuous consumption. Thus, the decreased nZVI amount might also account for the decreased dechlorination kinetics at Cycle 7.
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Fig. 9 Hypothesized mechanism of sustained CT dechlorination activity of nZVI over consecutive reaction cycles. |
Footnote |
† Electronic supplementary information (ESI) available. See DOI: 10.1039/c5ra07052j |
This journal is © The Royal Society of Chemistry 2015 |