# A Facile Synthesis, Characterization, and Photocatalytic Activity of Magnesium Ferrite Nanoparticles via the Solution Combustion Method

Authors: Loan T. T. Nguyen; Lan T. H. Nguyen; Nhuong Chu Manh; Dung Nguyen Quoc; Hai Nguyen Quang; Hang T. T. Nguyen; Duy Chinh Nguyen; Long Giang Bach
Journal: Journal of Chemistry
 (2019)

---

## Abstract

In this study, we adopted the solution combustion method to synthesize magnesium ferrite (MgFe2O4) using urea as the fuel. Various techniques including TGA, XRD, SEM, TEM, FTIR, UV-Vis DRS, and EDS were employed to characterize the synthesized MgFe2O4 nanoparticles. The XRD analysis revealed that single-phase MgFe2O4 was formed at a calcination temperature of at 500–600°C for 3 hours in the absence of an intermediate phase. TEM analysis also revealed the formation of monodisperse magnesium ferrite nanoparticles, averaged at 30 nm in size. The photocatalytic activity of the synthesized MgFe2O4 nanoparticles against methylene blue dye under visible light was investigated, showing the efficiency of 89.73% after 240 minutes of light irradiation with the presence of H2O2.


---

## Body

## 1. Introduction

Ferrite nanoparticles, MFe2O4 where M is any divalent metal ions such as Mg, Mn, Ni, Co, Fe, Cu, etc, find wide applications in several fields [1]. Depending on the area of application, ferrite nanoparticles need to exhibit distinct characteristics. For example, in order to be suitable as an absorbent for decontamination of wastewater, ferrites should have exceptional chemical reactivity, adsorption capacity, and most importantly, reasonable Ms value, which is critical for magnetic recovery of the adsorbent from the aqueous solution [2]. The choice of synthesis method should also be considered when it comes to exploring the mechanism of formation of ferrite properties. To be specific, the distribution of metallic ions among crystallographic lattice sites, which defines the characteristics of the materials, largely depends on the synthesis method. This effectively makes the method selection crucial when it comes to adapting the materials to the needs of application [1, 3, 4].Usually, the maximum band gap energy of ferrites is approximately 2 eV, allowing the materials to effectively absorb visible light [5]. Furthermore, advantageous magnetic properties also offer ferrites useful applications [6]. Both forms of ferrites, in individual photocatalysts or in combination with others, are accentuated in literature for being separable and reusable from the reaction mixture [5, 7]. One of the typical uses of ferrites is as visible light photocatalysts for the degradation of pollutants in water and wastewater [7–10]. This capability of ferrite catalysts is possible due to effective utilization of light energy, which in turn allows formation of e−/h+ pairs on the photocatalytic surface. The e−/h+ pairs, owing to their susceptibility to oxidation and reduction, play an important role in formation of reactive oxygen species, such as O•H and O2•−, consequently promoting the decomposition of pollutants. Previous studies also suggested the addition of oxidants such as H2O2 into the reaction to create a Fenton-type system [6, 8, 11, 12] aiding the degradation through formation of hydroxyl radicals.Among magnetic ferrites, magnesium ferrite (MgFe2O4) is a typical inverse spinel, where Fe3+ ions are located in the tetrahedral (A) and octahedral (B) sites and Mg2+ ions are located in octahedral sites only [13]. The application of magnesium ferrite is diverse ranging from that in high-density recording media [14] to that in the fields of heterogeneous catalysis [7, 15–17], adsorption [18–20], anode material [21], cancer cure [22], and sensors [23]. In addition, the material is also a soft magnetic n-type semiconducting materials with a narrow band gap (1.9 eV) [24].Methods devised for preparation of magnesium ferrite nanocrystallites included the coprecipitation method [19, 25–28], sol-gel method [20, 29], combustion method [30, 31], hydrothermal method [32], thermal decomposition method [33], and solvothermal method [34]. Among the methods used to synthesize ferrite nanoparticles, the solution combustion synthesis is favored for its simplicity, short reaction time, and low annealing temperature [35]. These advantages have made resulting ferrites to have fine particle size, reduced impurities, and improved physical properties [36]. In the combustion reaction, the fuels play the role of forming complexes with metal cations [35]. Frequently used fuels in previous studies included glycine, urea, citric acid, and EDTA (ethylene diammin tetraacetic acid). In this work, MgFe2O4 nanoparticles are prepared by the solution combustion method with urea as fuel. The structural, chemical composition, thermal, morphology, and photocatalytic activity of MgFe2O4 nanoparticles are investigated.


## 2. Materials and Method

### 2.1. Materials

All chemicals including magnesium nitrate hexahydrate (Mg(NO3)2·6H2O), iron nitrate nonahydrate (Fe(NO3)3·9H2O), urea (CH4N2O), and methylene blue (C16H18ClN3S) were obtained from Merck and used as received.


### 2.2. Preparation of MgFe2O4 Nanoparticles

The combustion preparation of MgFe2O4 with urea fuel in this study is described as follows. First, urea was dissolved in water, followed by an appropriate amount of magnesium nitrate hexahydrate and iron nitrate nonahydrate following the mole ratio for Mg(II)/Fe(III) of 1 : 2 under vigorous stirring to form a mixed solution. Afterwards, the mixed solution was further stirred for 4 hours until gel was formed. The gel was then dried in an oven at 80°C for 10 hours. Finally, the precipitate was calcined at 500–800°C for 3 hours with a heating rate of 5°C·min−1 [37].


### 2.3. Characterizations

The gel precursor was studied for its thermal decomposition behavior through thermogravimetry (TG) and differential thermal analysis (DTA) on a Labsys Evo S60/58988 instrument (Setaram, France) in the temperature range of 30–800°C with the heating rate of 10°C·min−1. The phase of the obtained powder was characterized by X-ray diffraction (XRD) using a D8 Advance diffractometer (Bruker, Madison, WI, USA) with CuKα radiation (λ = 1.5406 Å) in a 2θ angle ranging from 20° to 70° with a step of 0.03°. The crystallite size of spinel (D) was determined by Scherrer formula:(1)D=kλβcosθ,where λ, k, β, and θ are the X-ray wavelength (0.1504 nm), Scherrer constant (0.89), the full width at half maximum measured in radians, and the angle of diffraction of the (311) peak with the highest intensity, respectively. The morphological properties were analyzed by two techniques including scanning electron microscopy (SEM, Hitachi S-4800, Japan) and transmission electron microscopy (TEM, JEOL-JEM-1010, Japan). For sample composition, energy dispersive X-ray spectroscopy (EDX, JEOL JED 2300 Analysis Station, Japan) was employed. The spinel structure is confirmed for formation by Fourier transform infrared spectroscopy (FTIR Affinity-1S, Shimadzu, Japan). The optical absorption spectra were recorded by UV-Vis absorption spectrometer (U-4100, Hitachi, Japan).


### 2.4. Photocatalytic Degradation of Methylene Blue

The conditions in which experiments are conducted include room temperature, pH of approximately 7 for methylene blue (MB), and continuous circulation mode. Prior to the photocatalytic reaction, the adsorption/desorption equilibrium of the aqueous solution containing the suspension was achieved by stirring in dark environment for 30 mins. 50 mg of MgFe2O4 was dispersed into 100 mL of MB aqueous solution (10 mg·L−1). Subsequently, H2O2 was introduced and irradiation on the suspension followed immediately using 40 W Compact lamps, Philips. The photocatalytic efficiency of MB (H) was calculated using the following equation:(2)H=C0−CtC0×100%,where C0 is the concentration of MB (mg·L−1). The subscripts 0 and t denote time points where concentration was measured, at initial equilibrium (0) and after t irradiation time, respectively. Concentration was measured by an ultraviolet-visible spectrophotometer (UV-1700 Shimadzu, Japan) with a wavelength of 664 nm.


## 2.1. Materials

All chemicals including magnesium nitrate hexahydrate (Mg(NO3)2·6H2O), iron nitrate nonahydrate (Fe(NO3)3·9H2O), urea (CH4N2O), and methylene blue (C16H18ClN3S) were obtained from Merck and used as received.


## 2.2. Preparation of MgFe2O4 Nanoparticles

The combustion preparation of MgFe2O4 with urea fuel in this study is described as follows. First, urea was dissolved in water, followed by an appropriate amount of magnesium nitrate hexahydrate and iron nitrate nonahydrate following the mole ratio for Mg(II)/Fe(III) of 1 : 2 under vigorous stirring to form a mixed solution. Afterwards, the mixed solution was further stirred for 4 hours until gel was formed. The gel was then dried in an oven at 80°C for 10 hours. Finally, the precipitate was calcined at 500–800°C for 3 hours with a heating rate of 5°C·min−1 [37].


## 2.3. Characterizations

The gel precursor was studied for its thermal decomposition behavior through thermogravimetry (TG) and differential thermal analysis (DTA) on a Labsys Evo S60/58988 instrument (Setaram, France) in the temperature range of 30–800°C with the heating rate of 10°C·min−1. The phase of the obtained powder was characterized by X-ray diffraction (XRD) using a D8 Advance diffractometer (Bruker, Madison, WI, USA) with CuKα radiation (λ = 1.5406 Å) in a 2θ angle ranging from 20° to 70° with a step of 0.03°. The crystallite size of spinel (D) was determined by Scherrer formula:(1)D=kλβcosθ,where λ, k, β, and θ are the X-ray wavelength (0.1504 nm), Scherrer constant (0.89), the full width at half maximum measured in radians, and the angle of diffraction of the (311) peak with the highest intensity, respectively. The morphological properties were analyzed by two techniques including scanning electron microscopy (SEM, Hitachi S-4800, Japan) and transmission electron microscopy (TEM, JEOL-JEM-1010, Japan). For sample composition, energy dispersive X-ray spectroscopy (EDX, JEOL JED 2300 Analysis Station, Japan) was employed. The spinel structure is confirmed for formation by Fourier transform infrared spectroscopy (FTIR Affinity-1S, Shimadzu, Japan). The optical absorption spectra were recorded by UV-Vis absorption spectrometer (U-4100, Hitachi, Japan).


## 2.4. Photocatalytic Degradation of Methylene Blue

The conditions in which experiments are conducted include room temperature, pH of approximately 7 for methylene blue (MB), and continuous circulation mode. Prior to the photocatalytic reaction, the adsorption/desorption equilibrium of the aqueous solution containing the suspension was achieved by stirring in dark environment for 30 mins. 50 mg of MgFe2O4 was dispersed into 100 mL of MB aqueous solution (10 mg·L−1). Subsequently, H2O2 was introduced and irradiation on the suspension followed immediately using 40 W Compact lamps, Philips. The photocatalytic efficiency of MB (H) was calculated using the following equation:(2)H=C0−CtC0×100%,where C0 is the concentration of MB (mg·L−1). The subscripts 0 and t denote time points where concentration was measured, at initial equilibrium (0) and after t irradiation time, respectively. Concentration was measured by an ultraviolet-visible spectrophotometer (UV-1700 Shimadzu, Japan) with a wavelength of 664 nm.


## 3. Results and Discussion

### 3.1. Structural Characterization

In the precursor, urea is not only to provide sufficient heat for the system but also to ensure the formation of stable complexes with the metal ions to increase their solubility and prevent selective precipitation of metal ions during water removal. The reaction for metal nitrate mixture using urea as the fuel assuming complete combustion may be represented by the following equation [38]:(3)3MgNO32+6FeNO33+20CH4N2O⟶3MgFe2O4+20CO2+32N2+40H2OThe TG/DTA of the ferrite precursor are shown in Figure1(a). It can be observed that there are two exothermal peaks at 137.86°C and 437.04°C. The exothermal peak at 137.86°C has suggested self-combustion, like a process in which the nitrate ions act as an oxidizing agent and urea as fuel. The maximum exothermal peak at 437.04°C could be observed to closely follow a substantial mass loss in the temperature range of 200–450°C, evidencing the occurrence of the decomposition reaction of the ferrite precursor and nitrate. Approximately, the total mass loss that precedes the sharp exothermal reaction is 81.04%, which is consistent with the theoretical result (80.31%). This could be attributable to the relief of gases CO2, H2O, and N2 from the precursor. At temperature higher than 450°C, the weight of the sample remained almost constant. Therefore, the calcining temperature of the samples was selected in the range from 500 to 800°C.Figure 1
TGA/DTA curve of the precursor (a) and FT-IR spectra of the precursor and MgFe2O4 calcined samples at 500–600°C (b).
(a)
(b)Figure1(b) displays the FTIR spectra of the MgFe2O4 precursor and two calcined samples at 500 and 600°C relative to the range of 4000–400 cm−1. For the precursor sample, three broad absorption bands were observed at approximately 3446, 1656, and 1384 cm−1, respectively, corresponding to the presence of hydroxyl groups (-OH), the stretching vibration of the carboxyl group, and the presence of NO3− ions [29]. In the two spectra of the MgFe2O4 calcined at 500–600°C, two bands at 582 and 586 cm−1 and two bands at 443 and 445 cm−1 could be pairwise indexed to the stretching vibrations of metal-oxygen bonds in tetrahedron sites and in octahedron sites, respectively, suggesting the formation of magnesium ferrite [15, 20]. In addition, the absorption broad bands at 3450 and 3425 cm−1 are, respectively, indicative of the stretching mode of H2O molecules and hydroxyl groups, and in turn, the presence of H2O molecules on the surface of MgFe2O4 nanoparticles [24].Figure2 displays different X-ray diffraction patterns of MgFe2O4 nanoparticles with temperature varying from 500 to 800°C. The two ferrite samples calcined at 500–600°C were obtained as single spinel phase with peaks at 220, 311, 400, 511, and 440, corresponding to the cubic spinel structure (JCPDS card. no. 01-071-1232) [26]. It is showed that the increase in temperature is associated with the improvement of MgFe2O4 powders. However, from 700 to 800°C, new phases of α-Fe2O3 were observed. The spinel phase of MgFe2O4 was confirmed by five XRD peaks at 220, 311, 400, 511, and 440 crystal planes. Results reported in Table 1 also indicate that the crystallite size of MgFe2O4 was positively associated with the calcination temperature. As temperature moved from 500 to 800°C with 100°C interval, the average crystallite size was expanded from 18 to 61 nm. For the “a” lattice parameter, XRD spectra showed that for MgFe2O4 nanoparticles, the value fell in the range of 8.344–8.378 Å.Figure 2
X-ray diffraction of MgFe2O4 calcined samples from 500°C to 800°C.Table 1
Average crystallite size, lattice parameter, and unit cell volume of the samples at different calcination temperatures.
t
c (°C)
Average crystallite size (nm)
Lattice constant a (Å)
Cell volume V (Å3)
500
18
8.348
581.76
600
24
8.378
588.06
700
28
8.344
581.06
800
61
8.367
585.75The SEM images of different samples of MgFe2O4 nanoparticles corresponding to four calcination temperature points of 500°C, 600°C, 700°C, and 800°C are shown in Figures 3(a)–3(d). Visually, the images showed consistent implication with the XRD results. To be specific, particle size of the prepared samples were found to be proportionally increasing with temperature. This could possibly be due to the aggregation and coalescence during desiccation.Figure 3
SEM of MgFe2O4 calcined samples at 500°C (a), 600°C (b), 700°C (c), and 800°C (d).
(a)
(b)
(c)
(d)The TEM image of MgFe2O4 synthesized at 500°C is presented in Figure 4(a). Evidently, the magnesium ferrite nanoparticles resulted from the solution combustion method were uniform in terms of morphology and crystallite size and reached the particle size of approximately 30 nm.Figure 4
TEM and EDS of MgFe2O4 calcined sample at 500°C.
(a)
(b)Figure4(b) shows chemical purities and elemental composition of the MgFe2O4 materials produced by energy dispersive X-ray analysis (EDX). The existence of Mg, O, and Fe was determined by their corresponding peaks and the absence of other characteristic peaks. On the contrary, the synthesized sample was pure and did not contain any other elements.The UV-Visible absorption spectrum was obtained to investigate the optical properties of magnesium ferrite calcined at 500–600°C as shown in Figure5. By using the Kubelka–Munk equation, the band gap of MgFe2O4 samples was determined from reflectance spectra via conversion to absorbance [39]. The band gap energy Eg (eV) of the synthesized photocatalyst is calculated by the following equation:(4)Eg=h·cλmax=1240λmax,where h, c, and λmax are the Planck constant (6.62.10−34 J·s·photon−1), the speed of light (3.10−8 m·s−1), and the wavelength at the absorption edge (nm), respectively [40]. At wavelengths 500 and 600°C, λmax of the samples was calculated to be 679 nm and 687 nm, respectively. Therefore, the calculated band gap energy values are 1.83 eV and 1.81 eV for the MgFe2O4 samples calcined at 500°C and 600°C, respectively.Figure 5
The UV-Vis diffuse reflectance spectra of MgFe2O4 calcined at 500–600°C.


### 3.2. Photocatalytic Activity of Magnesium Ferrite Nanoparticles

Nanoparticles of the MgFe2O4 were tested for catalytic activities by performing photo-Fenton-like degradation of MB. Figures 6(a)–6(e) show different UV-Visible spectra of MB with MgFe2O4 photocatalyst corresponding to varying conditions including the calcination temperature of the absorbent, availability of H2O2, and presence of light irradiation.Figure 6
UV-Visible spectra of MB in different conditions and calcination temperatures of MgFe2O4 catalyst: (a) 500°C + dark, (b) 500°C + light, (c) 500°C + H2O2 + dark, (d) 500°C + H2O2 + light, (e) 600°C + H2O2 + light, and (f) the plots of ln (Co/Ct) versus irradiation time (t) in the presence of MgFe2O4 calcined samples at 500°C (1) and 600°C (2).
(a)
(b)
(c)
(d)
(e)
(f)The presence of methylene blue is indicated by the two absorption peaks at 609 nm and 664 nm [7]. It is visibly observed that the color of the MB solution gradually changed from blue to light blue and finally to colorless, which is presumably due to the estrangement of the chromophoric group. In the first two spectra where H2O2 was absent, MB degradation efficiency reached 6.51% (in the dark) and 31.73% (under light irradiation) after 240 minutes, suggesting the positive influence of light on the degradation efficiency. In comparison with the first spectrum, the third spectrum involved the introduction of H2O2, showing a significantly higher efficiency at 35.48%. The last two spectra demonstrated the effect of calcination temperature with the presence of H2O2 and light irradiation. The measured efficiencies were 89.73% and 69.17% corresponding to MgFe2O4 calcined at 500°C and 600°C, respectively. In addition, significant and proportional decline of peak intensity with respect to irradiation time was also recognized in these two spectra. These results suggested that light irradiation, ferrite catalyst, and H2O2 were all required for efficient photo-Fenton degradation of MB dye. Similar results have been reported for NiFe2O4 nanoparticles and CuFe2O4 spheres by various studies [11, 41].Thus, it is possible to affirm that the main factors for the photodegradation of methylene blue are the crystallite size and the surface area of the MgFe2O4 nanoparticles. The particle size of the calcined sample at 500°C is smaller than that of the calcined sample at 600°C. Therefore, the photocatalytic activity of the sample at 500°C is higher than that of the calcined sample at 600°C. This effect was also observed in the case of the methylene blue degradation in the presence of the copper ferrite nanopowders [42] and in the presence of coating titania-silica on cobalt ferrite nanoparticles [43].A pseudo-first-order kinetic model was adopted to describe the degradation process in the heterogeneous Fenton/photo-Fenton catalysis system [11, 44, 45]. Figure 6(f) plots ln (Co/Ct) versus irradiation time (t) for the MgFe2O4 sample, showing an approximated linear relationship between the two variables. This indicates that the photodegradation of MB follows a pseudo-first-order reaction. Calculation of linear slopes revealed that the rate constant (k) for the MgFe2O4 samples calcined at 500°C and 600°C were 0.00956 min−1 and 0.0052 min−1, respectively.


## 3.1. Structural Characterization

In the precursor, urea is not only to provide sufficient heat for the system but also to ensure the formation of stable complexes with the metal ions to increase their solubility and prevent selective precipitation of metal ions during water removal. The reaction for metal nitrate mixture using urea as the fuel assuming complete combustion may be represented by the following equation [38]:(3)3MgNO32+6FeNO33+20CH4N2O⟶3MgFe2O4+20CO2+32N2+40H2OThe TG/DTA of the ferrite precursor are shown in Figure1(a). It can be observed that there are two exothermal peaks at 137.86°C and 437.04°C. The exothermal peak at 137.86°C has suggested self-combustion, like a process in which the nitrate ions act as an oxidizing agent and urea as fuel. The maximum exothermal peak at 437.04°C could be observed to closely follow a substantial mass loss in the temperature range of 200–450°C, evidencing the occurrence of the decomposition reaction of the ferrite precursor and nitrate. Approximately, the total mass loss that precedes the sharp exothermal reaction is 81.04%, which is consistent with the theoretical result (80.31%). This could be attributable to the relief of gases CO2, H2O, and N2 from the precursor. At temperature higher than 450°C, the weight of the sample remained almost constant. Therefore, the calcining temperature of the samples was selected in the range from 500 to 800°C.Figure 1
TGA/DTA curve of the precursor (a) and FT-IR spectra of the precursor and MgFe2O4 calcined samples at 500–600°C (b).
(a)
(b)Figure1(b) displays the FTIR spectra of the MgFe2O4 precursor and two calcined samples at 500 and 600°C relative to the range of 4000–400 cm−1. For the precursor sample, three broad absorption bands were observed at approximately 3446, 1656, and 1384 cm−1, respectively, corresponding to the presence of hydroxyl groups (-OH), the stretching vibration of the carboxyl group, and the presence of NO3− ions [29]. In the two spectra of the MgFe2O4 calcined at 500–600°C, two bands at 582 and 586 cm−1 and two bands at 443 and 445 cm−1 could be pairwise indexed to the stretching vibrations of metal-oxygen bonds in tetrahedron sites and in octahedron sites, respectively, suggesting the formation of magnesium ferrite [15, 20]. In addition, the absorption broad bands at 3450 and 3425 cm−1 are, respectively, indicative of the stretching mode of H2O molecules and hydroxyl groups, and in turn, the presence of H2O molecules on the surface of MgFe2O4 nanoparticles [24].Figure2 displays different X-ray diffraction patterns of MgFe2O4 nanoparticles with temperature varying from 500 to 800°C. The two ferrite samples calcined at 500–600°C were obtained as single spinel phase with peaks at 220, 311, 400, 511, and 440, corresponding to the cubic spinel structure (JCPDS card. no. 01-071-1232) [26]. It is showed that the increase in temperature is associated with the improvement of MgFe2O4 powders. However, from 700 to 800°C, new phases of α-Fe2O3 were observed. The spinel phase of MgFe2O4 was confirmed by five XRD peaks at 220, 311, 400, 511, and 440 crystal planes. Results reported in Table 1 also indicate that the crystallite size of MgFe2O4 was positively associated with the calcination temperature. As temperature moved from 500 to 800°C with 100°C interval, the average crystallite size was expanded from 18 to 61 nm. For the “a” lattice parameter, XRD spectra showed that for MgFe2O4 nanoparticles, the value fell in the range of 8.344–8.378 Å.Figure 2
X-ray diffraction of MgFe2O4 calcined samples from 500°C to 800°C.Table 1
Average crystallite size, lattice parameter, and unit cell volume of the samples at different calcination temperatures.
t
c (°C)
Average crystallite size (nm)
Lattice constant a (Å)
Cell volume V (Å3)
500
18
8.348
581.76
600
24
8.378
588.06
700
28
8.344
581.06
800
61
8.367
585.75The SEM images of different samples of MgFe2O4 nanoparticles corresponding to four calcination temperature points of 500°C, 600°C, 700°C, and 800°C are shown in Figures 3(a)–3(d). Visually, the images showed consistent implication with the XRD results. To be specific, particle size of the prepared samples were found to be proportionally increasing with temperature. This could possibly be due to the aggregation and coalescence during desiccation.Figure 3
SEM of MgFe2O4 calcined samples at 500°C (a), 600°C (b), 700°C (c), and 800°C (d).
(a)
(b)
(c)
(d)The TEM image of MgFe2O4 synthesized at 500°C is presented in Figure 4(a). Evidently, the magnesium ferrite nanoparticles resulted from the solution combustion method were uniform in terms of morphology and crystallite size and reached the particle size of approximately 30 nm.Figure 4
TEM and EDS of MgFe2O4 calcined sample at 500°C.
(a)
(b)Figure4(b) shows chemical purities and elemental composition of the MgFe2O4 materials produced by energy dispersive X-ray analysis (EDX). The existence of Mg, O, and Fe was determined by their corresponding peaks and the absence of other characteristic peaks. On the contrary, the synthesized sample was pure and did not contain any other elements.The UV-Visible absorption spectrum was obtained to investigate the optical properties of magnesium ferrite calcined at 500–600°C as shown in Figure5. By using the Kubelka–Munk equation, the band gap of MgFe2O4 samples was determined from reflectance spectra via conversion to absorbance [39]. The band gap energy Eg (eV) of the synthesized photocatalyst is calculated by the following equation:(4)Eg=h·cλmax=1240λmax,where h, c, and λmax are the Planck constant (6.62.10−34 J·s·photon−1), the speed of light (3.10−8 m·s−1), and the wavelength at the absorption edge (nm), respectively [40]. At wavelengths 500 and 600°C, λmax of the samples was calculated to be 679 nm and 687 nm, respectively. Therefore, the calculated band gap energy values are 1.83 eV and 1.81 eV for the MgFe2O4 samples calcined at 500°C and 600°C, respectively.Figure 5
The UV-Vis diffuse reflectance spectra of MgFe2O4 calcined at 500–600°C.


## 3.2. Photocatalytic Activity of Magnesium Ferrite Nanoparticles

Nanoparticles of the MgFe2O4 were tested for catalytic activities by performing photo-Fenton-like degradation of MB. Figures 6(a)–6(e) show different UV-Visible spectra of MB with MgFe2O4 photocatalyst corresponding to varying conditions including the calcination temperature of the absorbent, availability of H2O2, and presence of light irradiation.Figure 6
UV-Visible spectra of MB in different conditions and calcination temperatures of MgFe2O4 catalyst: (a) 500°C + dark, (b) 500°C + light, (c) 500°C + H2O2 + dark, (d) 500°C + H2O2 + light, (e) 600°C + H2O2 + light, and (f) the plots of ln (Co/Ct) versus irradiation time (t) in the presence of MgFe2O4 calcined samples at 500°C (1) and 600°C (2).
(a)
(b)
(c)
(d)
(e)
(f)The presence of methylene blue is indicated by the two absorption peaks at 609 nm and 664 nm [7]. It is visibly observed that the color of the MB solution gradually changed from blue to light blue and finally to colorless, which is presumably due to the estrangement of the chromophoric group. In the first two spectra where H2O2 was absent, MB degradation efficiency reached 6.51% (in the dark) and 31.73% (under light irradiation) after 240 minutes, suggesting the positive influence of light on the degradation efficiency. In comparison with the first spectrum, the third spectrum involved the introduction of H2O2, showing a significantly higher efficiency at 35.48%. The last two spectra demonstrated the effect of calcination temperature with the presence of H2O2 and light irradiation. The measured efficiencies were 89.73% and 69.17% corresponding to MgFe2O4 calcined at 500°C and 600°C, respectively. In addition, significant and proportional decline of peak intensity with respect to irradiation time was also recognized in these two spectra. These results suggested that light irradiation, ferrite catalyst, and H2O2 were all required for efficient photo-Fenton degradation of MB dye. Similar results have been reported for NiFe2O4 nanoparticles and CuFe2O4 spheres by various studies [11, 41].Thus, it is possible to affirm that the main factors for the photodegradation of methylene blue are the crystallite size and the surface area of the MgFe2O4 nanoparticles. The particle size of the calcined sample at 500°C is smaller than that of the calcined sample at 600°C. Therefore, the photocatalytic activity of the sample at 500°C is higher than that of the calcined sample at 600°C. This effect was also observed in the case of the methylene blue degradation in the presence of the copper ferrite nanopowders [42] and in the presence of coating titania-silica on cobalt ferrite nanoparticles [43].A pseudo-first-order kinetic model was adopted to describe the degradation process in the heterogeneous Fenton/photo-Fenton catalysis system [11, 44, 45]. Figure 6(f) plots ln (Co/Ct) versus irradiation time (t) for the MgFe2O4 sample, showing an approximated linear relationship between the two variables. This indicates that the photodegradation of MB follows a pseudo-first-order reaction. Calculation of linear slopes revealed that the rate constant (k) for the MgFe2O4 samples calcined at 500°C and 600°C were 0.00956 min−1 and 0.0052 min−1, respectively.


## 4. Conclusions

We have successfully synthesized MgFe2O4 nanoparticles using the solution combustion method with urea as fuel. The particle size of prepared samples was showed to be proportional with rising temperature. Phase-pure MgFe2O4 nanoparticles were obtained at 500–600°C for 3 h with the size about 30 nm. UV-Vis also approximated the band gap which ranged from 1.81 to 1.83 eV. The present study also highlighted the role of MgFe2O4 in the degradation (89.73% in 240 minutes) of MB dye, suggesting possible applications of the ferrite for photo-Fenton activity in decontamination of wastewater. Kinetics describing the photodegradation process of two samples calcined at 500°C and 600°C also revealed that the reaction adhered to pseudo-first order with a rate constant (k) of 0.00956 min−1 and 0.0052 min−1, respectively.



---

*Source: 3428681-2019-03-25.xml*