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Article

Potassium Ferrite as Heterogeneous Photo-Fenton Catalyst for Highly Efficient Dye Degradation

by
Xinghui Zhang
1,
Zhibin Geng
1,
Juan Jian
2,
Yiqiang He
1,
Zipeng Lv
1,
Xinxin Liu
3 and
Hongming Yuan
1,*
1
State Key Laboratory of Inorganic Synthesis and Preparative Chemistry, College of Chemistry, Jilin University, Changchun 130012, China
2
Key Laboratory of Preparation and Applications of Environmental Friendly Material of the Ministry of Education, College of Chemistry, Jilin Normal University, Changchun 130103, China
3
Institute of Catalysis for Energy and Environment, College of Chemistry and Chemical Engineering, Shenyang Normal University, Shenyang 110034, China
*
Author to whom correspondence should be addressed.
Catalysts 2020, 10(3), 293; https://doi.org/10.3390/catal10030293
Submission received: 18 January 2020 / Revised: 6 February 2020 / Accepted: 3 March 2020 / Published: 4 March 2020
(This article belongs to the Special Issue Photocatalytic Oxidation/Ozonation Processes)
Browse Figures
Versions Notes

Abstract

:
In this work, hexagon-shaped potassium ferrite (K2Fe4O7) crystals with different sizes were prepared using the hydrothermal method. The crystals showed a narrow band gap of 1.44 eV, revealed by UV-visible diffuse reflectance spectroscopy, and was thus used as a heterogeneous Fenton catalyst to degrade methylene blue (MB) and crystal violet (CV) in the presence of green oxidant H2O2 under visible-light irradiation. Among the investigated crystals, the as-prepared one with an average size of 20 µm (KFO-20) exhibited better photocatalytic activity due to its high surface area. When it was used as a photo-Fenton catalyst, 100% MB and 92% CV were degraded within 35 min. Moreover, the catalyst maintained high photocatalytic activity and was stable after four continuous cycles. The trapping experiments showed that the active hydroxyl radical (·OH) was dominant in the photo-Fenton reaction. Therefore, this new photo-Fenton catalyst has great potential for the photocatalytic degradation of dye contaminants in water.

1. Introduction

Dyes are widely used in many industries, including textiles, printing, pulp, and paper. However, they also cause great environmental pollution that threatens public health due to their complicated constitution and high chemical stability. With the rapid development of the global economy, it is estimated that each year almost 2 × 105 tons of dyes are discharged directly into lakes, rivers, and groundwater [1,2,3,4]. Therefore, dye treatment in water systems is increasingly important.
Over the past few decades, many wastewater-treatment technologies have been developed for the removal or degradation of dye contaminants, such as traditional biological treatments, adsorption, coagulation/flocculation, membrane separation, precipitation, ion exchange, and advanced oxidation processes (AOPs). Among these methods, AOPs that include photochemical, catalytic, sonochemical, ozone, electrochemical, and Fenton oxidation can convert or degrade such contaminants into small molecules [5,6,7]. In particular, photo-Fenton oxidation has been proven to be highly effective for dye treatments [8,9]. However, homogeneous photo-Fenton technology exhibits limitations such as loss of catalysts and large iron sludge. To overcome these drawbacks, one potential strategy is using heterogeneous photo-Fenton catalysts to degrade dye contaminants. So far, several iron oxides and iron hydroxides utilised as photo-Fenton catalysts, such as Fe3O4, α-Fe2O3, α-FeOOH, and β-Fe2O3, have been used to catalyse or degrade various kinds of dye molecules due to their good photocatalytic activity, stable structure, and narrow band gap [10,11,12,13,14]. The catalytic activity of metal oxides is closely related to the crystal orientation, crystallinity, nanostructure, morphology, particle size, and surface properties of the material [15,16,17,18,19,20]. To further enhance their catalytic activity, some with nanometre sizes were prepared using nanotechnology [11,21,22]. Other transition metals were introduced into their structure to improve their catalytic activity [23,24,25,26,27]. Recently, iron oxide and carbon composites have also been used to effectively degrade organic dyes [28,29,30,31,32,33].
At present, there is an urgent need for low-cost, resource-friendly, stable iron-based heterogeneous Fenton catalysts for the degradation of dye contaminants in wastewater. The Fenton catalytic properties of iron oxides are strongly dependent on the crystal structural characters, band gap, and oxidation states of iron ions at octahedral and tetrahedral sites. All of the iron oxides mentioned above are constructed from iron octahedral and tetrahedral unites, and adopt either corundum or spinel structures. The search for an iron-based heterogeneous photo-Fenton catalyst with a new crystal structure is a key step towards more effectively degrading dye contaminants. Recently, we successfully synthesised potassium ferrite (K2Fe4O7) using the hydrothermal process [34]. This environmentally friendly iron oxide exhibited superhigh ion conductivity and excellent thermal stability. Its 3D structure consisted of octahedral FeO6 and tetrahedral FeO4 with shared vertices and edges. Therefore, the structure may be developed for use as a powerful candidate for a heterogeneous photo-Fenton catalyst for the degradation of dye molecules.
In this work, we prepared the hexagonal K2Fe4O7 crystals with different sizes using the hydrothermal method. Its band gap was determined by UV-visible diffuse reflectance spectroscopy. Methylene blue (MB) and crystal violet (CV) were selected as models to evaluate the catalytic activity of this iron oxide under photo-Fenton conditions. We then studied the effect of pH value, the concentration of hydrogen peroxide, and particle size on MB degradation. We also evaluated the reusability and stability of the catalyst.

2. Results and Discussion

2.1. Characterisation

SEM images of KFO-20 (Figure 1 a, b), KFO-80 (Figure 1 c, d), and KFO-180 (Figure 1 e, f) show that the obtained K2Fe4O7 crystals each had the same hexagonal shape and smooth surface except for crystal size. The powder XRD patterns of KFO-20, KFO-80, and KFO-180 are shown in Figure 2, where it is clear that all diffraction peaks were consistent with that of K2Fe4O7 reported previously [34]. This indicates that each sample’s structure remained intact and was in a pure phase. Studies showed that, as a result of higher crystallinity, there were fewer lattice defects, which are more conductive to the conduction of the charge carrier. This result is consistent with photoluminescence (PL).
The band gaps of three samples were determined by UV-visible diffuse reflectance spectroscopy measurement. They exhibited the same broad absorption with an absorption edge at about 858 nm (Figure 3a). Band-gap energy was calculated as 1.44 eV according to the equation Eg = hc/λ, where Eg is the energy band gap (eV) and hc = 1240 eV [35]. This narrow band gap was less than those of Fe3O4 [14], α-Fe2O3 [12], α-FeOOH [12], and NiFe2O4 [11], and was thus a favourable candidate to effectively degrade dye molecules in photo-Fenton catalytic processes under low-energy visible-light irradiation. The comparison of various catalytic systems for MB degradation under different photo-Fenton processes is shown in Table 1.
The XPS spectra of KFO-20 and KFO-180 are shown in Figure 3b. There were two obvious peaks with binding energies of 724.2 and 711.3 eV, which corresponded, respectively, to Fe 2p1/2 and Fe 2p3/2. XPS results were in good agreement with those of the reported crystal [34], suggesting that the oxidation state of iron ion in the as-prepared KFO was +3.
The Brunauer-Emmett-Teller (BET) surface area was measured via nitrogen adsorption–desorption experiments. As shown in Figure 3c, the adsorption–desorption isotherms of KFO corresponded to Type IV on the basis of the Brunauer-Deming-Teller classification [39,40]. The specific surface area of KFO-20, KFO-80, and KFO-180 was 63.79, 9.63, and 0.42 m2/g, respectively, which increased with the decrease of particle size. In this work, we found that crystallinity contributed little to MB degradation comparing to the specific surface area.
The photoluminescence (PL) spectrum was used to investigate the recombination behaviour of photogenerated electrons and holes in KFO-20, KFO-80, and KFO-180. The PL emission spectra of the three crystals at an excitation wavelength of 475 nm are shown in Figure 3d. A strong peak near 820 nm caused by the band–band PL phenomenon was observed, which was approximately equal to the band-gap energy of KFO (1.44 eV). However, peak intensity decreased with the decrease of crystal size due to shorter diffusion distance, suggesting that KFO-20 with a lower recombination rate of photogenerated electron-hole pair was expected to have higher photocatalytic activity.

2.2. Photo-Fenton MB Degradation

We first selected KFO-20 as a Fenton catalyst to perform the degradation of MB at pH = 2, 20 mg/L of MB at room temperature in the absence and presence of visible light, and with or without hydrogen peroxide. Degradation results are shown in Figure 4a. With visible-light radiation in the presence of KFO-20 and H2O2 (curve A), 100% of the MB was degraded within 35 min. However, under darker conditions, 46% of the MB was degraded within the same timeframe (curve B), indicating that its Fenton catalytic activity was significantly enhanced by introducing visible light. Only 12% of MB was degraded when the catalyst was not employed due to the self-sensitisation of MB (curve C). MB concentration had no apparent change when without hydrogen peroxide (curve D), confirming that MB degradation was attributed to the photo-Fenton process. The catalytic activity of the catalyst was superior to conventional photo-Fenton catalysts mentioned above [11,12,13,14]. Therefore, it can be concluded that the excellent catalytic activity of this iron oxide is assigned to its structural feature and the nature of the iron ion.

2.2.1. Effect of Catalyst Size

In general, the catalytic activity of heterogeneous Fenton catalysts was proportional to their specific surface area. A larger specific surface area can provide more active sites for a photo-Fenton catalytic process. Therefore, we investigated the effect of different KFO sizes on the degradation of MB under the same conditions. As shown in Figure 4b, about 34% and 24% of degradation were achieved within 35 min for KFO-80 and KFO-180, respectively, due to their different specific surface areas, which was consistent with the results of BET surface-area measurements.

2.2.2. Effect of pH Value

The Fenton oxidation reaction was sensitive to the pH value of the reacting solution. Therefore, the effect of the initial pH value on the degradation of MB (20 mg/L) was investigated by using the KFO-20 photo-Fenton catalyst. Figure 4c gives the removal efficiency of MB at different pH values within 35 min. At pH = 1.5, about 98% of MB degradation was obtained, and 100% of MB was degraded when we increased the pH value to 2.0 because excess H+ acted as a scavenger for the hydroxyl radical (·OH), as shown in Equation (1) [40]. As pH value increased, the removal percentage decreased to 90% at pH = 2.5. Therefore, the photo-Fenton catalyst can be used to effectively degrade MB in the pH range of 1.5–2.5.
·OH + H+ + e− → H2O

2.2.3. Effect of H2O2 Dose

In the heterogeneous Fenton reaction, redox cycling between Fe3+ and Fe2+ was achieved by H2O2. Figure 4d shows the effect of the H2O2 concentration on MB degradation in the presence of the KFO-20 catalyst and visible light. MB degradation increased to 100% when the molar concentration of H2O2 increased from 2 to 10 mM. This could be due to the formation of much ·OH in the photo-Fenton reaction (Equation (2)) [41]. However, 98% of MB was degraded at the concentration of 15 mM, because hydroperoxyl radicals (HO·) that were generated through excessive H2O2 reacting with the ·OH did not contribute to MB degradation (Equations (3)–(5)) [40,42,43,44,45,46]. This scavenging effect has been observed in many photo-Fenton processes.
H2O2 + hv → 2·OH
H2O2 + ·OH → H2O + H2O
H2O2 + HO2· → OH + H2O + O2
H2O + HO· → H2O + O2

2.2.4. Dynamic Degradation

In the photo-Fenton reaction system, a pseudo-first-order kinetic constant model was used to quantitatively evaluate the photocatalytic process. The rate constant was obtained by plotting −ln (C/C0) versus time, as shown in Figure 5a, where C0 and C are the initial concentration and the concentration at time t, respectively. The specific surface area S (m2/g), rate constant, and k (min−1) of KFO are shown in Table 2. The rate constants of KFO-20, KFO-80, and KFO-180 were 0.155, 0.007 and 0.006 min−1, respectively. The rate constant of KFO-20 was 26 times that of KFO-180, and the rate constant of the catalyst increased with the increase of specific surface area.

2.2.5. Total Organic Carbon

In order to determine the degree of mineralisation of MB, the total organic carbon (TOC) removal rates of different KFO sizes were measured using MB as a substrate under the same conditions (Figure 5b). The removal rate of TOC increased with the decrease of KFO sizes. The removal rate of KFO-20 reached 80.5%, which indicated that the KFO-20 effectively mineralised MB.

2.2.6. Universal Applicability of Catalyst

In order to evaluate the photo-Fenton KFO catalysts for other types of dye degradation under the same conditions, experiments of crystal violet (CV) degradation were carried out using catalysts with different sizes. As shown in Figure 6a, KFO-180 and KFO-80 did not produce high degradation efficiency within 35 min. However, 92% of CV was degraded by KFO-20. On the basis of the aforementioned results, the KFO-20 catalyst displayed the best photo-Fenton catalytic activity.

2.2.7. Trapping Experiments

To determine active species that were dominant for the degradation of MB, several scavengers, including 10 mmol/L of p-benzoquinone (BQ), ammonium oxalate (AO), tertiary butyl alcohol (t-BuOH), and silver nitrate (AgNO3), were used to trap these active species; results are shown in Figure 6b. BQ could trap the superoxide anion (·O2−). When BQ was added into the solution, 100% of the MB was degraded within 35 min, indicating that the ·O2− radical has little contribution to the degradation process. After t-BuOH was added as an ·OH scavenger, the degradation rate of the MB was 45%, and the degradation process was significantly inhibited. This indicated that the ·OH radical played a key role in the degradation process. When AO and AgNO3 were used to capture h+ and e−, respectively, 55% and 82% of the MB were degraded. The difference between them came from the contribution of additional ·OH radicals generated by photogenerated holes reacting with H2O2 (Equation (2)).

2.3. Possible Photo-Fenton Catalytic Mechanism

On the basis of the above experiment results, we proposed the photo-Fenton catalytic mechanism of KFO. The decomposed H2O2 and generated hydroxyl radicals on the surface of KFO particles can be described in the following reactions (Equations (2)–(7)). Fe3+ was reduced by adsorbed H2O2 to generate Fe2+ and peroxide hydroxyl radicals (HOO·) on the surface of a catalyst (Equation (6)). Meanwhile, HOO· reacted with hydrogen peroxide in an aqueous solution to produce a highly active hydroxyl radical (·OH) (Equation (4)). The generation of ·OH, which can efficiently degrade organic compounds in photo-Fenton-like reactions, can be described through the reaction between the formed Fe2+ and H2O2 (Equation (7)). Under visible-light irradiation, electron-hole pairs were generated on the surface of KFO (Equation (8)). Subsequently, the photogenerated electrons reduced hydrogen peroxide and reacted with dissolved oxygen to produce HO·, HO−, and ·O2− (Equations (9) and (10)) [44,45,47,48]. Additional ·OH were generated by photogenerated holes that reduced water and hydrogen peroxide (Equations (11) and (12)) [44,45,47,48]. Scheme 1 gives a graphical representation of photo-Fenton MB degradation.
Fe3+ + H2O2 → Fe2+ + HO2·+ H+
Fe2+ + H2O2 → Fe3+ + HO·+ OH−
KFO + hv → KFO (h+ + e−)
e− + H2O2 → HO− + HO
e− + O2 → O2−
h+ + H2O → H+ + HO
h+ + HO− → HO
HO· + MB → degradation products
h+ + MB → degradation products
Therefore, HO· and the h+ hole dominantly oxidised the MB molecule (Equations (13) and (14)).

2.4. Reusability and Chemical Stability

From the view of industrial applications, a catalyst’s chemical stability and reusability are both important. To evaluate the possibility of catalyst reuse, photo-Fenton reaction for MB degradation was successively performed using the KFO-20 catalyst (measurements are described in Supplementary Materials). As exhibited in Figure 7a, it is clearly seen that the catalytic activity of KFO-20 still remained efficient after four cycles under the same conditions. Moreover, after the reaction, the surface morphology of KFO-20 was almost indistinguishable from that of a fresh KFO-20 (Figure 7b). In addition, the powder XRD pattern of the used sample agreed with that of the as-prepared sample (Figure S1), suggesting that it had good chemical stability.

3. Materials and Methods

3.1. Materials

Analytical-grade ferric nitrate (FeNO3·9H2O), potassium hydroxide (KOH), sodium hydroxide (NaOH), barium sulfate (BaSO4), ammonium oxalate (AO), and hydrogen peroxide (H2O2) were purchased from Sinopharm Chemical Reagent Co., Ltd. (Changchun, China). P-benzoquinone (BQ) was supplied by Aladdin Ltd. (Changchun, China). Methylene blue (MB) and crystal violet were obtained from Xinzhong Chemical Reagent Co., Ltd. (Changchun, China). Tertiary butyl alcohol (t-BuOH) and hydrochloric acid (HCl) were acquired from Shanghai Runjie Chemical Reagent Co., Ltd. (Shanghai, China). Silver nitrate (AgNO3) was purchased from Shanghai Chemical Reagent Co., Ltd. (Shanghai, China). Potassium bromide was obtained from Shanghai Macklin Biochemical Co., Ltd. (Changchun, China). All chemicals could be directly used without further treatment.

3.2. Preparation

KFO-20 was prepared using the hydrothermal process on the basis of our ever-reported method [34]. First, we added 4 g of ferric nitrate into 32 mL of deionised water to form a clarifying solution. We slowly added 60 g of potassium hydroxide into a ferric nitrate solution while stirring continuously until the colour became light brown. The mixture was directly added into a Teflon-lined stainless-steel autoclave and heated at 180 oC for 2 h. After cooling down to room temperature, the crystal was washed 10 times with deionised water until its pH was neutralised. The crystal was then dried overnight in a vacuum drying oven at 60 oC. The preparation method of K2Fe4O7 with average sizes of 80 (KFO-80) and 180 µm (KFO-180) can be found in our supporting information.

3.3. Material Characterisation

Powder XRD experiments were performed on a Rigaku D-Max 2550 diffractometer (Tokyo, Japan) with Cu-Kα radiation (λ = 1.5418 Å). SEM images were obtained on a JEOL-6700 scanning electron microscope (Tokyo, Japan). UV-visible diffuse reflectance spectroscopy was performed with a Shimadzu UV-2450 spectrometer (Kyoto, Japan) XPS analysis was performed on a VG Scienta R3000 spectrometer (New York, N. Y., USA) with Al Kα (1486.6 eV) as the X-ray source.

3.4. MB Degradation

The degradation of MB was carried out in the presence of visible light in a cylindrical Pyrex vessel with a PL-300 xenon lamp (Beijing China) (λ > 400 nm) as the analogue sunlight source. During the experiment, the distance between light source and container was kept at 10 cm to ensure the same light intensity. The reaction vessel was equipped with a cooling device to ensure a constant reaction temperature. The initial experiment conditions were as follows: a mixture of 0.03 g of the micron scale catalyst and 100 mL of MB were stirred in dark conditions for 60 min to reach adsorption equilibrium. Then, 10 mM of H2O2 (30% w/v) was added into the solution, and the pH was adjusted to 2. The pH value was adjusted by adding 0.1 M HCl and 0.1 M NaOH. Then, 2 mL of the reaction solution was taken out with a 5 mL disposable syringe at regular intervals, and the catalyst in the solution was removed with a 0.2 µm filter. The concentration of MB remaining in the solution was determined by UV-visible spectroscopy. The degradation rate was calculated using Equation (15), where C0 and C were the initial concentration and the concentration at time t, respectively.
Dr = C/C0

4. Conclusions

Hexagonal K2Fe4O7 crystals with different sizes were successfully prepared under hydrothermal conditions; their narrow band gap was 1.44 eV. Three KFO crystals had specific surface areas of 63.79, 9.63, and 0.42 m2/g, respectively. A small-crystal KFO-20 with a high surface area was used as a photo-Fenton catalyst for the degradation of MB and CV in the presence of green oxidant H2O2 under visible-light irradiation. The degradation rates of MB and CV reached 100% and 92% within 35 min, respectively. Moreover, KFO-20 was shown to have good reusability and stability in the photo-Fenton degradation of MB. The ·OH radical was dominant in the photo-Fenton catalytic reaction. Combining the KFO catalyst and carbon materials with a catalyst of nanometre size could significantly enhance heterogeneous Fenton catalytic activity and be used as an efficient and stable catalyst for the removal of dye contaminants in wastewater in the future.

Supplementary Materials

The following are available online at https://www.mdpi.com/2073-4344/10/3/293/s1, Figure S1: Powder XRD patterns for KFO-20 after four cycles.

Author Contributions

Conceptualisation, Z.G.; software, J.J.; visualisation, Y.H.; investigation, Z.L.; data curation, X.L.; writing—original-draft preparation, X.Z.; writing—review and editing, H.Y. All authors have read and agreed to the published version of the manuscript.

Funding

This research was supported by funds granted by the Natural Science Foundation of Liaoning Province of China (2019-ZD-0481) and the Project of Education Office of Liaoning Province (LQN201909).

Acknowledgments

This work was financially supported by the State Key Laboratory of Inorganic Synthesis and Preparative Chemistry, the Natural Science Foundation of Liaoning Province of China (2019-ZD-0481), and the Project of Education Office of Liaoning Province (LQN201909).

Conflicts of Interest

The authors declare no conflict of interest.

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Catalysts 10 00293 g001 550
Figure 1. SEM images of (a, b) KFO-20, (c, d) KFO-80, and (e, f) KFO-180.
Figure 1. SEM images of (a, b) KFO-20, (c, d) KFO-80, and (e, f) KFO-180.
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Figure 2. Powder XRD patterns of KFO-20, KFO-80, and KFO-180.
Figure 2. Powder XRD patterns of KFO-20, KFO-80, and KFO-180.
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Figure 3. (a) UV-visible diffuse reflectance spectroscopy; (b) XPS spectra of Fe 2p1/2 and Fe 2p3/2 for KFO-20 and KFO-180; (c) N2 adsorption–desorption isotherms measured at 77K of KFO; and (d) photoluminescence (PL) spectra of KFO.
Figure 3. (a) UV-visible diffuse reflectance spectroscopy; (b) XPS spectra of Fe 2p1/2 and Fe 2p3/2 for KFO-20 and KFO-180; (c) N2 adsorption–desorption isotherms measured at 77K of KFO; and (d) photoluminescence (PL) spectra of KFO.
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Figure 4. (a) Degradation efficiency of methylene blue (MB) under different conditions. A: MB + KFO-20 + H2O2 + light; B: MB + KFO-20 + H2O2; C: MB + H2O2 + light; D: MB + KFO-20 + light; (b) degradation efficiency of MB using KFO catalysts with different sizes; (c) degradation efficiency of MB at different pH values; (d) degradation efficiency of MB at various H2O2 concentrations. Reaction conditions: MB concentration, 20 mg/L; KFO mass, 30 mg; H2O2, 10 mM; reaction time, 35 min.
Figure 4. (a) Degradation efficiency of methylene blue (MB) under different conditions. A: MB + KFO-20 + H2O2 + light; B: MB + KFO-20 + H2O2; C: MB + H2O2 + light; D: MB + KFO-20 + light; (b) degradation efficiency of MB using KFO catalysts with different sizes; (c) degradation efficiency of MB at different pH values; (d) degradation efficiency of MB at various H2O2 concentrations. Reaction conditions: MB concentration, 20 mg/L; KFO mass, 30 mg; H2O2, 10 mM; reaction time, 35 min.
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Figure 5. (a) Pseudo-first-order kinetics degradation of MB; (b) total organic carbon (TOC) removal of MB in presence of differently sized KFOs. Reaction conditions: MB concentration, 20 mg/L; KFO mass, 30 mg; H2O2, 10 mM; reaction time, 35 min.
Figure 5. (a) Pseudo-first-order kinetics degradation of MB; (b) total organic carbon (TOC) removal of MB in presence of differently sized KFOs. Reaction conditions: MB concentration, 20 mg/L; KFO mass, 30 mg; H2O2, 10 mM; reaction time, 35 min.
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Figure 6. (a) Degradation efficiency of crystal violet (CV) with KFO catalysts at pH 2; (b) effects of different scavengers on MB degradation at pH 2 in presence of KFO-20, H2O2, and light.
Figure 6. (a) Degradation efficiency of crystal violet (CV) with KFO catalysts at pH 2; (b) effects of different scavengers on MB degradation at pH 2 in presence of KFO-20, H2O2, and light.
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Scheme 1. MB degradation by KFO-20.
Scheme 1. MB degradation by KFO-20.
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Figure 7. (a) Degradation efficiency of MB for KFO-20 at different cycles; (b) SEM image for KFO-20 after four successive cycles.
Figure 7. (a) Degradation efficiency of MB for KFO-20 at different cycles; (b) SEM image for KFO-20 after four successive cycles.
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Table
Table 1. Comparison of various catalytic systems for methylene blue (MB) degradation under different photo-Fenton processes.
Table 1. Comparison of various catalytic systems for methylene blue (MB) degradation under different photo-Fenton processes.
CatalystReaction ConditionDegradation RateTimeReference
NiFe2O4[Catalyst] = 0.2 g/L, [H2O2] = 5 mM, [MB] = 30 mg/L and light irradiation 98.5% 50 min [11]
Fe3O4[Catalyst] = 4 g/L, [H2O2] = 50 mM, [MB] = 100 mg/L, and UV irradiation 20% 60 min [14]
α-Fe2O3[Catalyst] = 0.025 g/L, [H2O2] = 1.10 mM, [MB] = 40 mg/L and UV irradiation 94.7% 80 min [12]
CuFe2O4[Catalyst] = 0.1 g/L, [H2O2] = 20 mM, [MB] = 30 mg/L and light irradiation 80% 80 min [36]
ZnO[Catalyst] = 0.02 g/L, [H2O2] = 5 mM, [MB] = 20 mg/L and light irradiation 4.1% 60 min [37]
TiO2[Catalyst] = 1.0 g/L, [MB] = 50 mg/L and light irradiation 30% 60 min [38]
K2Fe4O7[Catalyst] = 0.03 g/L, [H2O2] = 5 mM, [MB] = 20 mg/L and light irradiation 100% 35 min This article
Table
Table 2. KFO specific surface area S (m2/g) and rate constant k (min−1).
Table 2. KFO specific surface area S (m2/g) and rate constant k (min−1).
S (m2/g)k (min−1)
KFO-2063.790.155
KFO-809.630.007
KFO-1800.420.006

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Zhang, X.; Geng, Z.; Jian, J.; He, Y.; Lv, Z.; Liu, X.; Yuan, H. Potassium Ferrite as Heterogeneous Photo-Fenton Catalyst for Highly Efficient Dye Degradation. Catalysts 2020, 10, 293. https://doi.org/10.3390/catal10030293

AMA Style

Zhang X, Geng Z, Jian J, He Y, Lv Z, Liu X, Yuan H. Potassium Ferrite as Heterogeneous Photo-Fenton Catalyst for Highly Efficient Dye Degradation. Catalysts. 2020; 10(3):293. https://doi.org/10.3390/catal10030293

Chicago/Turabian Style

Zhang, Xinghui, Zhibin Geng, Juan Jian, Yiqiang He, Zipeng Lv, Xinxin Liu, and Hongming Yuan. 2020. "Potassium Ferrite as Heterogeneous Photo-Fenton Catalyst for Highly Efficient Dye Degradation" Catalysts 10, no. 3: 293. https://doi.org/10.3390/catal10030293

APA Style

Zhang, X., Geng, Z., Jian, J., He, Y., Lv, Z., Liu, X., & Yuan, H. (2020). Potassium Ferrite as Heterogeneous Photo-Fenton Catalyst for Highly Efficient Dye Degradation. Catalysts, 10(3), 293. https://doi.org/10.3390/catal10030293

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