# Heterogeneous Fenton-Like Catalytic Removal of Methylene Blue Dye in Water Using Magnetic Nanocomposite (MCM-41/Magnetite)

Authors: André E. Nogueira; Isabela A. Castro; Amanda S. Giroto; Zuy M. Magriotis
Journal: Journal of Catalysts
 (2014)

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## Abstract

In this work, MCM-41, magnetite (MAG), and a composite of magnetite and MCM-41 (MCM-MAG) were synthesized by a simple route for the production of active systems in the decomposition of organic waste. The materials were characterized by N2 adsorption/desorption, X-ray diffraction analysis (XRD), temperature programmed reduction (TPR), Fourier transform infrared spectroscopy (FTIR), and transmission electron microscopy (TEM). Our results indicated that the decolorization kinetics of the dyes were in the order of MCM-MAG > MCM-41 > magnetite. Mineralization of the dyes was monitored by total organic carbon (TOC) decrease. The dye solutions could be completely decolorized and effectively mineralized, with an average overall TOC removal 43% for a Fenton-like reaction time of 180 min. The degradation activity of the MCM-MAG was stable during four consecutive experiments, confirming their stability and reusability of the composite. The great advantage of this composite is that it may be easily magnetically recovered and reused.


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## Body

## 1. Introduction

Currently the efficient use of water is important for industry, as it is crucial for sustainable development and public health. In many cases the generation of contaminated effluents with various types of organic waste, which are rich in microbial or bacterial activity, are involved. This is not appropriate for reuse in agriculture and human consumption [1].With regard to organic pollutants, we can highlight the textile dyes, which possess a high capacity to modify the environment due to their strong color and visual pollution and also cause changes in biological cycles mainly affecting photosynthesis processes. Besides these facts, studies have shown that some classes of dyes and their byproducts may be carcinogenic and/or mutagenic [2].In this context, the development of new processes for wastewater treatment in order to immobilize or degrade these compounds in textile industry effluents is very important. An extensively studied alternative is the use of advanced oxidation processes (AOP). These processes are based on the formation of hydroxyl radicals, which are capable of oxidizing contaminants to smaller and less polluting molecules or even mineralize them, turning them into CO2, H2O, and inorganic ions from atoms [3].The development of active heterogeneous systems to promote Fenton chemistry is of considerable interest, since it could offer some advantages over the classical homogeneous Fenton; because there is no sludge formation, the operation is carried out in near neutral pH and there is the possibility of recycling the iron promoter [4].The main feature of this technology is the use of iron as a solid catalyst supported on material with high surface area or in the form of poorly soluble magnetic oxides, facilitating the removal of the catalyst for later reuse [5, 6]. Most works refer to iron catalysts supported on zeolites [7–9] and activated carbon [10, 11] for the degradation of organic compounds [12, 13].The purpose of this study was to report the preparation of a composite based on magnetic iron oxide nanoparticles dispersed inside mesoporous silica MCM-41 and its application to the degradation of methylene blue (MB) by heterogeneous Fenton process.


## 2. Methodology

### 2.1. Synthesis

First, magnetite was prepared by a coprecipitation method, already described in the literature [14]. In a typical procedure, 500 mL of 0.126 mol L−1 FeSO4·7H2O solution, 500 mL of FeCl3·6H2O (0.18 mol L−1), and 9 mL of concentrated HCl solution were quickly added to a basic solution (53 mL) of 30% NH4OH at 60°C under vigorous stirring for 15 minutes. The black precipitate (magnetite) was washed several times until the suspension reached pH 8.The MCM-composite was obtained using 5% of magnetite (m/m). For this, 16 g of Cetyltrimethylammonium surfactant (CTAB) was dissolved in 300 mL of sodium hidroxide solution (0.33 mol L−1). Next, it was slowly added to 37 mL of tetraethyl orthosilicate (TEOS), which was left under stirring for 24 hours at room temperature. Afterwards, the magnetite was added to this suspension and left for 4 more hours. Finally, the composite was washed with distilled water, oven-dried for 6 hours at 60°C, and calcined slowly at 600°C for 4 h under a nitrogen flow (100 mL min−1). Likewise, the synthesis of MCM-41 was performed in the absence of magnetite.


### 2.2. Characterization

The materials were characterized by N2 adsorption/desorption measurements at 77 K in a Quantchrome Autsorb 1 equipment. The surface areas were calculated by the Brunauer-Emmett-Teller (BET) equation and pore size distribution was determined by the Barrett-Joyner-Halenda (BJH) equation [15]. The Fourier transform infrared spectra (FTIR) of adsorbents (in the form of KBr pellets) were measured using a Digilab Excalibur FTS 3000 series spectrometer in the 400–4000 cm−1 range at a resolution of 4 cm−1. Temperature programmed reduction (TPR) was carried out using an Chembet-3000 (Quantchrome) apparatus under a flow of 20 mL min−1 (mixture of 5% H2 in N2), 150 current, and attenuation 16. The X-ray powder patterns were also collected at room temperature in the 2θ range from 5° to 70° with step scan of 0.02° using a Rigaku D/MAX 2500 diffractometer with a rotary anode (Cu Kα radiation) operating at 150 kV and 40 mA. The morphology of the powders was characterized by transmission electron microscopy (TEM) FEI/PHILIPS CM120.


### 2.3. Methylene Blue Removal

#### 2.3.1. Adsorption Kinetics Tests

The adsorption kinetics tests were performed in batch at a temperature of 25 ± 1°C. Aqueous solutions of MB (10 mL) at a concentration of 50 mg·L−1 were placed under constant stirring in contact with 10 mg of the catalyst, for 0, 15, 30, 60, 120, and 180 minutes. The absorption tests were monitored by UV-visible spectroscopy (Shimadzu UV-1601 PC) at 645 nm, the maximum absorption wavelength of MB. This analysis was used as reference experiment to compare to the degradation profile with respect to the reaction Fenton using H2O2 to activate the catalysts.


#### 2.3.2. Degradation Tests

The degradation of MB was performed using 9.9 mL of 50 mg L−1 of dye suspension, 0.1 mL of 30% H2O2, and 10 mg of catalysts. The suspension was maintained under constant stirring (100 rpm) for 0, 15, 30, 60, 120, and 180 minutes. The temperature was set to 25 ± 1°C during the tests.The reuse of the catalysts was also investigated. In a typical test, 100 mg of the MCM-MAG was placed in contact with 100 mL of MB solution (50 mg L−1) and 1 mL of H2O2 under shaker at 130 rpm for 180 min. The catalysts were then recovered by filtration, water-washed in order to remove the excess of adsorbed MB, and dried at 60°C for 4 h. The materials were subsequently used in another oxidation cycle keeping the same standard conditions and ratio of catalyst/dye.The degradation was monitored by UV-visible spectroscopy (Shimadzu UV-1601 PC) at 645 nm, the maximum absorption wavelength of MB, and total carbon analysis was performed in the dye suspension on a Shimadzu 500A TOC analyzer, in synthetic air atmosphere.


## 2.1. Synthesis

First, magnetite was prepared by a coprecipitation method, already described in the literature [14]. In a typical procedure, 500 mL of 0.126 mol L−1 FeSO4·7H2O solution, 500 mL of FeCl3·6H2O (0.18 mol L−1), and 9 mL of concentrated HCl solution were quickly added to a basic solution (53 mL) of 30% NH4OH at 60°C under vigorous stirring for 15 minutes. The black precipitate (magnetite) was washed several times until the suspension reached pH 8.The MCM-composite was obtained using 5% of magnetite (m/m). For this, 16 g of Cetyltrimethylammonium surfactant (CTAB) was dissolved in 300 mL of sodium hidroxide solution (0.33 mol L−1). Next, it was slowly added to 37 mL of tetraethyl orthosilicate (TEOS), which was left under stirring for 24 hours at room temperature. Afterwards, the magnetite was added to this suspension and left for 4 more hours. Finally, the composite was washed with distilled water, oven-dried for 6 hours at 60°C, and calcined slowly at 600°C for 4 h under a nitrogen flow (100 mL min−1). Likewise, the synthesis of MCM-41 was performed in the absence of magnetite.


## 2.2. Characterization

The materials were characterized by N2 adsorption/desorption measurements at 77 K in a Quantchrome Autsorb 1 equipment. The surface areas were calculated by the Brunauer-Emmett-Teller (BET) equation and pore size distribution was determined by the Barrett-Joyner-Halenda (BJH) equation [15]. The Fourier transform infrared spectra (FTIR) of adsorbents (in the form of KBr pellets) were measured using a Digilab Excalibur FTS 3000 series spectrometer in the 400–4000 cm−1 range at a resolution of 4 cm−1. Temperature programmed reduction (TPR) was carried out using an Chembet-3000 (Quantchrome) apparatus under a flow of 20 mL min−1 (mixture of 5% H2 in N2), 150 current, and attenuation 16. The X-ray powder patterns were also collected at room temperature in the 2θ range from 5° to 70° with step scan of 0.02° using a Rigaku D/MAX 2500 diffractometer with a rotary anode (Cu Kα radiation) operating at 150 kV and 40 mA. The morphology of the powders was characterized by transmission electron microscopy (TEM) FEI/PHILIPS CM120.


## 2.3. Methylene Blue Removal

### 2.3.1. Adsorption Kinetics Tests

The adsorption kinetics tests were performed in batch at a temperature of 25 ± 1°C. Aqueous solutions of MB (10 mL) at a concentration of 50 mg·L−1 were placed under constant stirring in contact with 10 mg of the catalyst, for 0, 15, 30, 60, 120, and 180 minutes. The absorption tests were monitored by UV-visible spectroscopy (Shimadzu UV-1601 PC) at 645 nm, the maximum absorption wavelength of MB. This analysis was used as reference experiment to compare to the degradation profile with respect to the reaction Fenton using H2O2 to activate the catalysts.


### 2.3.2. Degradation Tests

The degradation of MB was performed using 9.9 mL of 50 mg L−1 of dye suspension, 0.1 mL of 30% H2O2, and 10 mg of catalysts. The suspension was maintained under constant stirring (100 rpm) for 0, 15, 30, 60, 120, and 180 minutes. The temperature was set to 25 ± 1°C during the tests.The reuse of the catalysts was also investigated. In a typical test, 100 mg of the MCM-MAG was placed in contact with 100 mL of MB solution (50 mg L−1) and 1 mL of H2O2 under shaker at 130 rpm for 180 min. The catalysts were then recovered by filtration, water-washed in order to remove the excess of adsorbed MB, and dried at 60°C for 4 h. The materials were subsequently used in another oxidation cycle keeping the same standard conditions and ratio of catalyst/dye.The degradation was monitored by UV-visible spectroscopy (Shimadzu UV-1601 PC) at 645 nm, the maximum absorption wavelength of MB, and total carbon analysis was performed in the dye suspension on a Shimadzu 500A TOC analyzer, in synthetic air atmosphere.


## 2.3.1. Adsorption Kinetics Tests

The adsorption kinetics tests were performed in batch at a temperature of 25 ± 1°C. Aqueous solutions of MB (10 mL) at a concentration of 50 mg·L−1 were placed under constant stirring in contact with 10 mg of the catalyst, for 0, 15, 30, 60, 120, and 180 minutes. The absorption tests were monitored by UV-visible spectroscopy (Shimadzu UV-1601 PC) at 645 nm, the maximum absorption wavelength of MB. This analysis was used as reference experiment to compare to the degradation profile with respect to the reaction Fenton using H2O2 to activate the catalysts.


## 2.3.2. Degradation Tests

The degradation of MB was performed using 9.9 mL of 50 mg L−1 of dye suspension, 0.1 mL of 30% H2O2, and 10 mg of catalysts. The suspension was maintained under constant stirring (100 rpm) for 0, 15, 30, 60, 120, and 180 minutes. The temperature was set to 25 ± 1°C during the tests.The reuse of the catalysts was also investigated. In a typical test, 100 mg of the MCM-MAG was placed in contact with 100 mL of MB solution (50 mg L−1) and 1 mL of H2O2 under shaker at 130 rpm for 180 min. The catalysts were then recovered by filtration, water-washed in order to remove the excess of adsorbed MB, and dried at 60°C for 4 h. The materials were subsequently used in another oxidation cycle keeping the same standard conditions and ratio of catalyst/dye.The degradation was monitored by UV-visible spectroscopy (Shimadzu UV-1601 PC) at 645 nm, the maximum absorption wavelength of MB, and total carbon analysis was performed in the dye suspension on a Shimadzu 500A TOC analyzer, in synthetic air atmosphere.


## 3. Results and Discussion

### 3.1. Characterizations

In order to investigate the textural properties, N2 adsorption/desorption was evaluated (Figure 1). The adsorption curves show that the amount of N2 adsorbed increases gradually with increasing relative pressure. This can be ascribed to multilayer adsorption. In the range between 0.2 and 0.4 P/P0 the adsorption strongly increases for MCM-41. It is assumed that this is due to condensation of nitrogen in the mesopores. The MCM-MAG and magnetite samples showed Type I isotherms; thus, the predominance of micropores can be expected [16].N2 adsorption and desorption isotherms measured at 77 K (a) and pore size distributions (b).
(a)
(b)The specific surface area was calculated by the BET equation (Figure1(a)). The materials showed high surface area values of 1400, 247, and 118 m2g−1 for MCM-41, MCM-MAG, and magnetite, respectively. The pore size distribution based on BJH calculation method for magnetite, MCM-41, and MCM-MAG was measured (Figure 1(b)). All samples showed a narrow pore distribution wherein MCM-MAG offered the largest pore size (highest peak centered at 18.6 Å) among the three synthesized samples, and MCM-41 had the smallest pore size (approximately 17.5 Å).The infrared spectra are presented in Figure2. The absorption bands between 1220 and 1070 and 800 cm−1 for MCM-41 and MCM-MAG are assigned to asymmetric and symmetric vibrations of the Si–O groups. In the region close to 446 cm−1, the vibration mode of Si–O tetrahedral is observed. The samples showed a broad band at 3455 cm−1, which can be ascribed to the silanol and/or hydroxyl group. The latter suggests adsorbed water [17]. Absorption bands of the magnetite spectrum are observed at 572 and 437 cm−1. These are assigned to Fe–O stretch vibration modes characteristic of Fe3O4 [18]. There were no significant changes in the MCM-MAG spectrum, compared to MCM-41. This can be attributed to an overlap of the characteristic bands of magnetite and MCM-41.Figure 2
FTIR spectrum of the synthesized samples.The synthesized samples were studied by temperature-programmed reduction (TPR) using H2 as a reducing gas (Figure 3). In the measurements of MCM-41 no peak reduction was observed. The H2 consumption profile for MAG-MCM composite and magnetite showed several peaks related to different iron species. These reduction processes are well known and have been reported in Oliveira et al. (2004) [19]. We have
(1)Magnetite⟶Wüstite⟶Fe0(Fe3O4)(FeO)Figure 3
Temperature programmed reduction profiles.The diffractogram patterns were presented in Figure4. The XRD pattern of MCM-41 showed no diffraction angle in the analyzed range; this suggests an amorphous phase formation. In contrast, in the XRD patterns of magnetite and the MCM-MAG composite, the crystalline phase formation was observed. Their diffractograms showed characteristic peaks of the iron magnetite phases (JCPDS: 19-0629) at 2θ = 18.3°, 30.2°, 35.6°, 43.3°, 53.7°, 57.2°, and 62.9° [20].Figure 4
The XRD diffraction patterns of MCM-41, MCM-MAG, and magnetite samples.The crystallite size plays an important role and has a high influence on the surface area of synthesized samples and the surface reactions. Thus, we evaluated the average size of the magnetite crystals produced. To this end, we used the information and the domain of the XRD crystallographic coherence. It was calculated employing Scherrer’s equation. The particle size was about 12 nm [21].Typical TEM micrographs for magnetite and MCM-MAG are shown in Figure5. It is clear that pure Fe3O4 nanoparticles were quite agglomerated, with a mean diameter of 13 nm, while TEM image of MCM-MAG showed less agglomerated magnetite nanoparticles in the surface of MCM-41 with a mean diameter of 11 nm.TEM image and histogram analysis for magnetite, (a) and (b), and MCM-MAG, (c) and (d).
(a)
(b)
(c)
(d)


### 3.2. Methylene Blue Removal

To verify the adsorption and the oxidation effect of the synthesized samples, MB was used as an organic dye model molecule. This compound was chosen due to its ease of monitoring by simple techniques such as UV-visible spectroscopy at its maximum absorption wavelength, 645 nm. The adsorption kinetics process was controlled by measuring the discoloration of the dye solution in a batch adsorption experiment, with the magnetite, MCM-MAG, and MCM-41 (Figure6(a)). We observed that the adsorption capacity was low for the samples, with a maximum at 25%, approximately, for MCM-41. Figure 6(b) shows the MB dye degradation profile in H2O2 presence by heterogeneous reaction.Adsorption kinetics (a) and MB oxidation (b) using the synthesized samples.
(a)
(b)The kinetic study of Fenton process can be performed by assuming that the reaction between hydroxyl radicals and the pollutant is the rate determining step. Thus, by assuming thatOH· instantaneous concentration was a constant, MB degradation could be described by a pseudo-first-order kinetic expression:
(2)-dCdt=k×C·OH×C=kapp×C⟶-ln⁡CC0=kapp×t,
where C is the MB concentration, mg·L−1, k is the reaction rate constant, and kapp is the apparent pseudo-first-order constant. Straight lines passing through the origin fit the degradation data well (the coefficient of linear regression, r, is 0.81, 0.92, and 0.86 for magnetite, MCM-MAG, and MCM-41, resp.) and from the slopes, kapp values were 0.0002, 0.0018, and 0.0013 min−1 for the systems catalyzed by magnetite, MCM-MAG, and MCM-41.Thekapp of the systems with MCM-MAG were higher than that of the system with only magnetite or MCM-41, indicating that composite could improve the degradation efficiency of heterogeneous Fenton reaction. A higher removal was observed for the MCM-MAG composite after 90 min of reaction, suggesting that the combination of magnetite oxide with mesoporous MCM-41 may offer synergistic reaction routes for the catalytic oxidation of target compounds. However, the color removal from the MB solution does not indicate that there was complete oxidation of the dye. To understand the color removal from the dye solution, the degradation reaction was monitored by total organic carbon analysis (TOC) in order to obtain information about the possible mineralization of the organic compound, by removing carbon from the dye solution.From these results we can conclude that the composite was more active in carbon removal from the dye solution after 180 min of reaction, removing 43% of the carbon solution, followed by MCM-41 with 18% and 3% for magnetite, which is consistent with the analysis obtained by UV-VIS, as expected, evidencing the mineralization of the organic compound.The reuse test was performed in order to evaluate the catalytic activity of MCM-MAG during successive experiments and thus to observe the possibility of catalyst reuse. Figure7 shows the discoloration efficiency of MB in four consecutive runs. The result showed that the activity of the MB decreased gradually during four successive runs. However, the result showed that the MCM-MAG maintained high activity for the degradation of MB during four cycle experiments. This indicates that the MCM-MAG is mechanically stable and reusable under these experimental conditions.Figure 7
Multicycle tests for degradation of MB for 180 min with MCM-MAG.


## 3.1. Characterizations

In order to investigate the textural properties, N2 adsorption/desorption was evaluated (Figure 1). The adsorption curves show that the amount of N2 adsorbed increases gradually with increasing relative pressure. This can be ascribed to multilayer adsorption. In the range between 0.2 and 0.4 P/P0 the adsorption strongly increases for MCM-41. It is assumed that this is due to condensation of nitrogen in the mesopores. The MCM-MAG and magnetite samples showed Type I isotherms; thus, the predominance of micropores can be expected [16].N2 adsorption and desorption isotherms measured at 77 K (a) and pore size distributions (b).
(a)
(b)The specific surface area was calculated by the BET equation (Figure1(a)). The materials showed high surface area values of 1400, 247, and 118 m2g−1 for MCM-41, MCM-MAG, and magnetite, respectively. The pore size distribution based on BJH calculation method for magnetite, MCM-41, and MCM-MAG was measured (Figure 1(b)). All samples showed a narrow pore distribution wherein MCM-MAG offered the largest pore size (highest peak centered at 18.6 Å) among the three synthesized samples, and MCM-41 had the smallest pore size (approximately 17.5 Å).The infrared spectra are presented in Figure2. The absorption bands between 1220 and 1070 and 800 cm−1 for MCM-41 and MCM-MAG are assigned to asymmetric and symmetric vibrations of the Si–O groups. In the region close to 446 cm−1, the vibration mode of Si–O tetrahedral is observed. The samples showed a broad band at 3455 cm−1, which can be ascribed to the silanol and/or hydroxyl group. The latter suggests adsorbed water [17]. Absorption bands of the magnetite spectrum are observed at 572 and 437 cm−1. These are assigned to Fe–O stretch vibration modes characteristic of Fe3O4 [18]. There were no significant changes in the MCM-MAG spectrum, compared to MCM-41. This can be attributed to an overlap of the characteristic bands of magnetite and MCM-41.Figure 2
FTIR spectrum of the synthesized samples.The synthesized samples were studied by temperature-programmed reduction (TPR) using H2 as a reducing gas (Figure 3). In the measurements of MCM-41 no peak reduction was observed. The H2 consumption profile for MAG-MCM composite and magnetite showed several peaks related to different iron species. These reduction processes are well known and have been reported in Oliveira et al. (2004) [19]. We have
(1)Magnetite⟶Wüstite⟶Fe0(Fe3O4)(FeO)Figure 3
Temperature programmed reduction profiles.The diffractogram patterns were presented in Figure4. The XRD pattern of MCM-41 showed no diffraction angle in the analyzed range; this suggests an amorphous phase formation. In contrast, in the XRD patterns of magnetite and the MCM-MAG composite, the crystalline phase formation was observed. Their diffractograms showed characteristic peaks of the iron magnetite phases (JCPDS: 19-0629) at 2θ = 18.3°, 30.2°, 35.6°, 43.3°, 53.7°, 57.2°, and 62.9° [20].Figure 4
The XRD diffraction patterns of MCM-41, MCM-MAG, and magnetite samples.The crystallite size plays an important role and has a high influence on the surface area of synthesized samples and the surface reactions. Thus, we evaluated the average size of the magnetite crystals produced. To this end, we used the information and the domain of the XRD crystallographic coherence. It was calculated employing Scherrer’s equation. The particle size was about 12 nm [21].Typical TEM micrographs for magnetite and MCM-MAG are shown in Figure5. It is clear that pure Fe3O4 nanoparticles were quite agglomerated, with a mean diameter of 13 nm, while TEM image of MCM-MAG showed less agglomerated magnetite nanoparticles in the surface of MCM-41 with a mean diameter of 11 nm.TEM image and histogram analysis for magnetite, (a) and (b), and MCM-MAG, (c) and (d).
(a)
(b)
(c)
(d)


## 3.2. Methylene Blue Removal

To verify the adsorption and the oxidation effect of the synthesized samples, MB was used as an organic dye model molecule. This compound was chosen due to its ease of monitoring by simple techniques such as UV-visible spectroscopy at its maximum absorption wavelength, 645 nm. The adsorption kinetics process was controlled by measuring the discoloration of the dye solution in a batch adsorption experiment, with the magnetite, MCM-MAG, and MCM-41 (Figure6(a)). We observed that the adsorption capacity was low for the samples, with a maximum at 25%, approximately, for MCM-41. Figure 6(b) shows the MB dye degradation profile in H2O2 presence by heterogeneous reaction.Adsorption kinetics (a) and MB oxidation (b) using the synthesized samples.
(a)
(b)The kinetic study of Fenton process can be performed by assuming that the reaction between hydroxyl radicals and the pollutant is the rate determining step. Thus, by assuming thatOH· instantaneous concentration was a constant, MB degradation could be described by a pseudo-first-order kinetic expression:
(2)-dCdt=k×C·OH×C=kapp×C⟶-ln⁡CC0=kapp×t,
where C is the MB concentration, mg·L−1, k is the reaction rate constant, and kapp is the apparent pseudo-first-order constant. Straight lines passing through the origin fit the degradation data well (the coefficient of linear regression, r, is 0.81, 0.92, and 0.86 for magnetite, MCM-MAG, and MCM-41, resp.) and from the slopes, kapp values were 0.0002, 0.0018, and 0.0013 min−1 for the systems catalyzed by magnetite, MCM-MAG, and MCM-41.Thekapp of the systems with MCM-MAG were higher than that of the system with only magnetite or MCM-41, indicating that composite could improve the degradation efficiency of heterogeneous Fenton reaction. A higher removal was observed for the MCM-MAG composite after 90 min of reaction, suggesting that the combination of magnetite oxide with mesoporous MCM-41 may offer synergistic reaction routes for the catalytic oxidation of target compounds. However, the color removal from the MB solution does not indicate that there was complete oxidation of the dye. To understand the color removal from the dye solution, the degradation reaction was monitored by total organic carbon analysis (TOC) in order to obtain information about the possible mineralization of the organic compound, by removing carbon from the dye solution.From these results we can conclude that the composite was more active in carbon removal from the dye solution after 180 min of reaction, removing 43% of the carbon solution, followed by MCM-41 with 18% and 3% for magnetite, which is consistent with the analysis obtained by UV-VIS, as expected, evidencing the mineralization of the organic compound.The reuse test was performed in order to evaluate the catalytic activity of MCM-MAG during successive experiments and thus to observe the possibility of catalyst reuse. Figure7 shows the discoloration efficiency of MB in four consecutive runs. The result showed that the activity of the MB decreased gradually during four successive runs. However, the result showed that the MCM-MAG maintained high activity for the degradation of MB during four cycle experiments. This indicates that the MCM-MAG is mechanically stable and reusable under these experimental conditions.Figure 7
Multicycle tests for degradation of MB for 180 min with MCM-MAG.


## 4. Conclusions

In this work MCM-MAG was successfully synthesized, with magnetite particles well dispersed on the surface of MCM-41. The composite showed very good catalytic performance for MB organic dye oxidation in H2O2 presence, after 90 min of reaction, compared with magnetite and MCM-41, suggesting that the combination of magnetite oxide with mesoporous MCM-41 may offer synergistic reaction routes for the catalytic oxidation of target compounds. These studies revealed that the dye removal occurs through a Fenton process system by the composite, whereas for the MCM-41 the dye removal occurs mainly via adsorption. In addition to the high catalytic activity for the MCM-MAG composite in the heterogeneous Fenton reaction, it should also be reported that this process provides an easy recovery of the catalyst due to presence of magnetic properties in the composite. It was also observed that catalytic behavior could be reproduced in consecutive experiments without a considerable drop in the process efficiency.



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*Source: 712067-2014-03-31.xml*