# Photo-Fenton Degradation of RB5 Dye in Aqueous Solution Using Fe Supported on Mexican Natural Zeolite

Authors: José Domenzain-Gonzalez; José J. Castro-Arellano; Luis A. Galicia-Luna; Luis Lartundo-Rojas
Journal: International Journal of Photoenergy
 (2019)

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## Abstract

A Mexican natural zeolite (MNZ) was impregnated with Fe at concentrations of 5 and 10 mg FeCl3/g MNZ (MNZ/Fe) in order to study the photo-Fenton degradation of Reactive Black 5 (RB5) dye. Two samples were prepared and calcined at 550 and 700°C for each concentration. These samples were also characterized by the following techniques: X-ray diffraction (XRD) to determine crystalline phases of mineral, X-ray photoelectron spectroscopy (XPS) to observe the elemental composition of the material where the main element was Fe as Fe2p, Mössbauer to establish the phases in the material which were magnetite (Fe3O4), fayalite, and chlorite, Raman to corroborate that magnetite clusters in natural material were presented, and transmission electron microscopy (TEM) by which magnetite nanoparticles were observe on zeolite surface. Afterwards, the catalytic degradation of RB5 dye was performed by photo-Fenton process using a 2.2 W lamp as a radiation source. Four initial concentrations of RB5 dye ((RB5)0) were evaluated which ranged from 40 to 100 mg/L. Then, the evaluation reaction was carried out by UV-Vis spectroscopy to know the change in RB5 concentration and chemical oxygen demand (COD) removal to determine the organic carbon. The best results on the photo-Fenton degradation was 91% discoloration and 68.5% chemical oxygen demand removal based on an initial concentration RB50=100mg/L and 10 mg MNZ/Fe (700°C of calcined temperature) at MNZ/Fe=0.05g/L catalyst dose in aqueous solution, H2O2=3 g/L, pH=2.5, and 180 minutes of reaction time. Subsequently, variations on (RB5)0, pH, (H2O2), and (MNZ/Fe) were assessed in order to optimize the process by keeping 10 MNZ/Fe. The optimal RB5 dye degradation was achieved at RB50=100mg/L in the presence of MNZ/Fe=0.2g/L, H2O2=3 g/L and pH=2.5 where the highest discoloration and chemical oxygen demand removal were 93 and 70.5 at 180 min. Finally, the kinetic reaction was evaluated as a pseudo-first-order kinetics with an apparent rate constant (kapp) of 0.0225 min-1 at latest conditions.


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## Body

## 1. Introduction

Nowadays, the environment pollution is increasing due to the different human activities. The high content of harmful organic and inorganic compounds present in rivers, lakes, and seas represents an unfavorable impact for life development in these ecosystems, in addition to having a pernicious influence on humanity. There are a great variety of pollution sources, which are produced by human activities that affect the soil, air, and liquid effluents. The chemical industry has the greatest impact on pollution increase, since it throws liquid effluents and/or gases with chemical waste to the environment. Some organic pollutant species are resistant to natural degradation process [1, 2]. A notorious example is the textile industry, which often throws wastewater effluents with nonbiodegradable dyes to the environment [3]. In consequence, the development of new processes or materials is needed for the elimination of these compounds based on natural materials. An alternative is the Fenton process which allows obtaining a high efficiency over the effluent treatments and even reaching mineralization in the presence of Fe as a catalyst. Then, a natural zeolite can be used as support and/or promoter since it is constituted by Fe and other metals.The zeolites can be classified as natural or synthetic. Synthetic zeolites have a homogeneous composition, a specific structure, and well-defined properties that depend on the control of the synthesis process. These characteristics allow their application in selective high-performance reactions and are widely used in the industry, but they have a higher cost than natural zeolites. Moreover, natural zeolites have a heterogeneous composition, their structure and properties can vary from one lot to another, and even change their properties and composition in the same sample according to the crystal or the analyzed zone. Despite natural zeolites being not very selective, they are reactive, more abundant, and crystalline aluminosilicates with ion exchange capacity. The latter allows the adsorption of minerals such as K, Na, C, Ca, Mg, and Fe, and hence its application in several chemical reactions. To resume, natural zeolites are a good option as catalysts or catalytic supports where selectivity is not as important as the degradation of organic pollutants in wastewater treatment [4, 5].Zeolites without heterogeneous atoms into its lattice are not photocatalytically active since they do not exhibit any absorption in the UV-Vis region [6], but MNZ has different elements integrated in its composition as Fe that produces photoactive sites of a solid photocatalyst. Besides, the great surface area of MNZ is combined with the absorption capacity and ion exchange provided by its negative charge [7]. It causes an increase in photocatalytic process efficiency. For this reason, it is interesting to increase the amount of Fe in MNZ. Certain ceramics such as zeolites tend to modify their structural properties (porosity, mechanical strength, composition, chemical properties, among other properties) due to calcination processes.Fe is a very useful material in several processes, for example, ammonia production [8] or in organic pollutants degradation [9, 10]. Natural minerals constituted of Fe such as hematite and magnetite, among other compounds [11], which are oxides, oxyhydroxides, and hydrated oxides. Goethite is the most frequent iron species in minerals due it being the most thermodynamically stable compound. The presence of these minerals is related to temperature, humidity, and presence of organic matter of soil origin. For example, hematite is associated with warm regions [12], low temperatures, and high humidity, but high contents of organic matter promote goethite formation [13].An important improvement to the abovementioned process could be Fe nanoparticles, which have many applications in biomedical sciences, removal of heavy metals from aqueous solutions, chemical catalysis, removal of inorganic and organic components, and textile dyes. In the present work, Fe particles were impregnated by incipient wetting method over a Mexican natural zeolite as support with the aim of increasing the Fe concentration. The zeolite impregnated with 5 and 10 mg FeCl3/g MNZ (MNZ/Fe) was used in the RB5 dye degradation by heterogeneous photo-Fenton process. Furthermore, the influence of calcination temperature was determined over Fe species on surface and in the matrix of MNZ/Fe. It was characterized by XRD, XPS, TEM, Mössbauer (MS), and Raman spectroscopy. Meanwhile, UV-Vis spectroscopy and COD removal were used to evaluate the MNZ/Fe catalytic activity.For the catalytic evaluation, calcined temperature and the amount of MNZ/Fe were evaluated at constant H2O2 concentration, catalyst dose in aqueous solution (MNZ/Fe), pH solution, and initial dye concentration (RB5)0. Later, the process was optimized by keeping the radiation source constant and changing the variables (MNZ/Fe), pH solution, (H2O2), and (RB5)0. The evaluation parameters were the discoloration percentage and the COD removal at 180 min. Finally, the apparent rate constant was estimated.


## 2. Materials and Methods

### 2.1. Preparation

The Mexican natural zeolite (catalytic Fe support) had particle sizes of 38–212μm. The methodology for MNZ impregnation was in a wet medium (incipient wetting method), which is described below. A MNZ solution with deionized water was prepared and placed under constant stirring and at pH 3 using HCl (0.5 M, 0.38 in mass fraction provided by Fermont). After 120 min, iron salt (FeCl3, 0.9995 in mass fraction provided by Fermont) was added to the solution at concentrations of 5 and 10 mg FeCl3/g MNZ, pH was adjusted to 3 under stirring by 300 min. Subsequently, the material was filtered off and kept at 50°C to remove humidity, and hence avoid modifications in the zeolite structure.Then, the material was subjected to a calcination process (Vulcan muffle, model 3-130) by increasing temperature at a rate of 2°C/min, with ramps of 100°C and remaining 120 min in each ramp up to reach the desired calcination temperature for 180 min. The calcination temperatures were 300, 600, and 700°C for DXR characterization. Regarding the influence of Fe impregnation, the temperatures were 550 and 700°C. Finally, the calcined MNZ/Fe sample at 700° C was chosen as the best option for catalytic evaluation in the RB5 dye degradation with a concentration of 10 mg MNZ/Fe.


### 2.2. Characterization

In order to determine the zeolitic phases and Fe species in the mineral, MNZ/Fe was characterized by the following techniques: X-ray diffraction (Rigaku, model Miniflex 600), X-ray photoelectron spectroscopy (Thermo Fisher Scientific, K-Alpha XPS spectrometer), Mössbauer spectroscopy (Wissel-Electronik spectrometer), Raman spectroscopy (Olimpus equipment, model BX41-HR800), and transmission electron microscopy (JEOL, model JEM-2100).


### 2.3. Evaluation Process of RB5 Dye Degradation

The catalytic evaluation of MNZ/Fe was carried out by a heterogeneous photo-Fenton reaction for removal of Reactive Black 5 dye (0.55 in mass fraction provided by Sigma-Aldrich). This chemical has three characteristic signals in UV-Vis range at 312, 392, and 597 nm which correspond to naphthalene, azo group, and chromophore that gives color to the molecule, respectively [14, 15].The catalytic evaluation of MNZ/Fe was carried out in a 200 mL batch reactor with constant stirring at 0.785 bar and room temperature (25°C). In this process, 10 mg MNZ/Fe was used at calcination temperature of 700°C, and catalyst doses in aqueous solution (MNZ/Fe) of 0.05, 0.1, 0.15, 0.2, 0.35, 0.5, 1.0, and 1.5 g/L. The effect of pH on process at 2.5, 3.0, 3.5, and 4.5 was observed by dossing HCl. The effect of H2O2 concentration (0.5 in mass fraction provided by Fermont) was also observed with variations of 2, 3, 4, and 5 g/L. Moreover, four initial concentrations of RB5 dye were tested in the range of 40–100 mg/L. In addition, an UV-LED lamp (designed specifically for the geometry of reactor) functioned as the radiation source. The energy provided throughout the lamp improved production of hydroxyl radicals by Fe3+ ions. The LEDs emitted at 405 nm corresponding to 3.06 eV and a power of 2.2 W.RB5 dye removal reactions using MNZ/Fe as a catalyst by the photo-Fenton process were monitored using a UV-Vis spectrophotometer (Ocean Optics, model Jaz) with a radiation source (Analytical Instrument Systems Inc., DT 1000 CE) and optical fibers (Ocean Optics, QP300-1-SR). The calibration curve of the RB5 dye with UV-Vis spectrophotometer was performed from 10 to 100 mg/L each 10 mg/L. The reported data corresponded to the average of triplicated analyses for each concentration, theR2 was reported to be 0.9987 for 597 nm.Finally, the chemical oxygen demand (COD) was determined using the reagents provided by Hanna Instruments in the range of 0-1500 mg/L. 2 mL of the sample were needed for COD quantification, the samples were digested in the presence of dichromate at 150°C for 2 hours (HI reactor 839800-01 by Hanna). Subsequently, the samples were cooled at room temperature and the COD was determined by means of a Hanna photometer (HI 83099).


## 2.1. Preparation

The Mexican natural zeolite (catalytic Fe support) had particle sizes of 38–212μm. The methodology for MNZ impregnation was in a wet medium (incipient wetting method), which is described below. A MNZ solution with deionized water was prepared and placed under constant stirring and at pH 3 using HCl (0.5 M, 0.38 in mass fraction provided by Fermont). After 120 min, iron salt (FeCl3, 0.9995 in mass fraction provided by Fermont) was added to the solution at concentrations of 5 and 10 mg FeCl3/g MNZ, pH was adjusted to 3 under stirring by 300 min. Subsequently, the material was filtered off and kept at 50°C to remove humidity, and hence avoid modifications in the zeolite structure.Then, the material was subjected to a calcination process (Vulcan muffle, model 3-130) by increasing temperature at a rate of 2°C/min, with ramps of 100°C and remaining 120 min in each ramp up to reach the desired calcination temperature for 180 min. The calcination temperatures were 300, 600, and 700°C for DXR characterization. Regarding the influence of Fe impregnation, the temperatures were 550 and 700°C. Finally, the calcined MNZ/Fe sample at 700° C was chosen as the best option for catalytic evaluation in the RB5 dye degradation with a concentration of 10 mg MNZ/Fe.


## 2.2. Characterization

In order to determine the zeolitic phases and Fe species in the mineral, MNZ/Fe was characterized by the following techniques: X-ray diffraction (Rigaku, model Miniflex 600), X-ray photoelectron spectroscopy (Thermo Fisher Scientific, K-Alpha XPS spectrometer), Mössbauer spectroscopy (Wissel-Electronik spectrometer), Raman spectroscopy (Olimpus equipment, model BX41-HR800), and transmission electron microscopy (JEOL, model JEM-2100).


## 2.3. Evaluation Process of RB5 Dye Degradation

The catalytic evaluation of MNZ/Fe was carried out by a heterogeneous photo-Fenton reaction for removal of Reactive Black 5 dye (0.55 in mass fraction provided by Sigma-Aldrich). This chemical has three characteristic signals in UV-Vis range at 312, 392, and 597 nm which correspond to naphthalene, azo group, and chromophore that gives color to the molecule, respectively [14, 15].The catalytic evaluation of MNZ/Fe was carried out in a 200 mL batch reactor with constant stirring at 0.785 bar and room temperature (25°C). In this process, 10 mg MNZ/Fe was used at calcination temperature of 700°C, and catalyst doses in aqueous solution (MNZ/Fe) of 0.05, 0.1, 0.15, 0.2, 0.35, 0.5, 1.0, and 1.5 g/L. The effect of pH on process at 2.5, 3.0, 3.5, and 4.5 was observed by dossing HCl. The effect of H2O2 concentration (0.5 in mass fraction provided by Fermont) was also observed with variations of 2, 3, 4, and 5 g/L. Moreover, four initial concentrations of RB5 dye were tested in the range of 40–100 mg/L. In addition, an UV-LED lamp (designed specifically for the geometry of reactor) functioned as the radiation source. The energy provided throughout the lamp improved production of hydroxyl radicals by Fe3+ ions. The LEDs emitted at 405 nm corresponding to 3.06 eV and a power of 2.2 W.RB5 dye removal reactions using MNZ/Fe as a catalyst by the photo-Fenton process were monitored using a UV-Vis spectrophotometer (Ocean Optics, model Jaz) with a radiation source (Analytical Instrument Systems Inc., DT 1000 CE) and optical fibers (Ocean Optics, QP300-1-SR). The calibration curve of the RB5 dye with UV-Vis spectrophotometer was performed from 10 to 100 mg/L each 10 mg/L. The reported data corresponded to the average of triplicated analyses for each concentration, theR2 was reported to be 0.9987 for 597 nm.Finally, the chemical oxygen demand (COD) was determined using the reagents provided by Hanna Instruments in the range of 0-1500 mg/L. 2 mL of the sample were needed for COD quantification, the samples were digested in the presence of dichromate at 150°C for 2 hours (HI reactor 839800-01 by Hanna). Subsequently, the samples were cooled at room temperature and the COD was determined by means of a Hanna photometer (HI 83099).


## 3. Results and Conclusion

### 3.1. X-Ray Diffraction

Mineral samples were analyzed by X-ray diffraction in order to observe the effect of calcination temperature on zeolite structure. XRD patterns of uncalcined natural zeolite (25°C) and calcined natural zeolite at 300, 600, and 700°C are shown in Figure1. The material was identified as a mixture of different zeolitic phases where the main phase was mordenite-heulandite, erionite-cristobalite as a secondary phase, and quartz as an impurity. Below 17° 2theta, no significant signals were found that yield information about the material characterization.Figure 1
XRD patterns of MNZ/Fe samples for uncalcined at 25°C and calcined at 300, 600, and 700°C: ●: heulandite, ○: mordenite, ♦: erionite, ♢: cristobalite, ▲: quartz.Different signals were grouped from 17° 2theta to 68° 2theta where the most intense signal located at 30.9° 2theta was referred to mordenite (JCPDS: O60239). This highest signal remained for any temperatures (25–700°C); however, the intensity was decreasing above 700°C until mineral disappearance at 900°C [16]. Similar behavior was noted for heulandite (JCPDS: 210131), it disappeared at 600°C due to structure collapses above 500°C [17, 18]. On the opposite, erionite (JCPDS: 39-1379) was constituted in the sample up to 700°C and tends to disappear at 840°C [19], erionite increased its intensity with respect to the uncalcined sample due to heulandite phase disappears. Besides, as natural zeolite does not have a homogeneous composition, so its structure can change from one sample to another.Additionally, it is observed that cristobalite (JCPDS: 075-0923) was contained after calcination treatment (up to 700°C) but it disappears at 1525°C [20]. Contrarily, the signals that were located above 55° 2theta corresponded in their great majority to quartz (JCPDS: 46-1045) [21] and mordenite since these phases prevail after calcination at 700°C. Lastly, it was observed that zeolitic structures persisted after the thermal treatment with the exception of heulandite.


### 3.2. XPS Analysis

X-ray photoelectron spectroscopy analysis gives information about the material surface at a depth not greater than 8 to 10 atomic layers, with aspatialresolution≤6μm. XPS is able to identify the elements from lithium to uranium with exception of hydrogen and helium. The element concentration must be higher than to 0.05% atomic to be detected in the sample [22].XPS spectra were obtained using a K-alpha X-ray photoelectron spectrometer (Thermo Fisher Scientific Co.) with a monochromatic source of Al Kα X-rays (1486.6 eV). The sample diameter was 400 μm. Firstly, it remained in a prechamber for 600 min; then, samples were transferred to the chamber at about 1×10−9 Torr. For each sample, three measurements were carried out in different zones. The analyzer passed energy of 200 eV and 40 eV for the scans collection and high-resolution spectra, respectively. All spectra were calibrated with an adventitious peak C1s at 284.6 eV to detect and compensate for the variable charge at core peaks. The software Thermo Avantage v5.979 was used for the curve fitting of a high-resolution spectrum, and the deconvolution was made using the Shirley method with a Gaussian-Lorentzian contribution 70-30%.Subsequently, Fe species presented in MNZ/Fe were found and identified on the surface. XPS spectra of uncalcined natural zeolite at 25°C as well as calcined at 550 and 700°C are shown in Figure2. The major elements on surface were Si and Al corroborating an aluminosilicate type material. The amount of Si varied from 27.1 to 29 w% while Al was ranging from 8.4 to 8.5 w%. The presence of Na, Mg, Ca, K, and Fe minerals was also observed.Figure 2
XPS spectra of MNZ/Fe: uncalcined at 25°C and calcined at 550 and 700°C.The global composition of MNZ samples impregnated with 10 mg MNZ/Fe are listed in Table1 for different temperatures (uncalcined at 25°C and calcined at 550 and 700°C). It can be noted that the composition of Al, C, Mg, K, and Na did not have a significant change. O and Ca composition diminished by comparing calcined and uncalcined analyses. Meanwhile, Si and Fe (3.9 w%) composition increased after the calcination process about 2 percentage units. These results demonstrated that composition could have variations because of the mineral nature [23]. This was in agreement with the previous work reported by Domenzain et al. [23]. On that research, the composition of Fe in a MNZ without impregnation was about 2.3 w% identified by EDS analyses and 2.6 w% of Fe oxides quantified by atomic absorption.Table 1
MNZ composition impregnated with 10 mg FeCl3/g MNZ for calcined and uncalcined samples.
Name
MNZ/Fe composition (w%)
(25°C)
(550°C)
(700°C)
O 1 s
47.40
46.00
45.00
Si 2p
27.10
29.00
28.60
Al 2p
8.50
8.40
8.50
Ca 2p
4.10
2.00
2.30
C 1 s
4.00
3.70
4.50
Fe 2p
3.90
6.00
6.20
Mg 1 s
2.20
2.30
2.00
K 2p
1.30
1.30
1.80
Na 1 s
0.80
0.20
0.30Fe can be present in natural minerals as different species, one of the most common is the magnetite (Fe3O4), which is a compound of mixed valence and commonly expressed with the notation as (Fe3+)tet(Fe2+Fe3+)octO4. Due to rapid jump of electrons which move with a frequency of approximately 10-11 s at room temperature, the octahedral ions Fe3+ and Fe2+ can be written as Fe2.5+ [24]. In addition, the Mössbauer spectrum of Fe3O4 at room temperature shows only two overlapping sextets which correspond to tetrahedral ions of Fe3+ and octahedral ions of Fe2.5+.XPS spectra of Fe species for uncalcined MNZ/Fe at 25°C and calcined MNZ/Fe at 550 and 700°C are shown in Figure3. These were located between 705 and 740 eV of binding energy. Intensity variations in spectra were observed between calcined and uncalcined samples. The first one contained 3.9 w% of Fe on its surface, whereas the calcined samples (550 and 700°C) had 6 w% and 6.2 w% of Fe, respectively. The Fe spectrum has two representative peaks of Fe3+ ion characteristics of Fe3O4 structure, the main corresponds to Fe 2p3/2 located around 711.48±0.2 eV [25] and the second peak is referred to as 2p1/2 situated in 724.60±0.2 eV. These variations in Fe composition may be attributed to the following aspects: (1) the increase of Fe particles caused by impregnation, (2) the presence of other compounds on material surface that did not allow observing the Fe ions, (3) the change on the mineral structure due to the zeolitic species collapse after calcination, and (d) the amount of each compound varied depending on the analyzed crystal [23].Figure 3
XPS spectra for Fe 2p of calcined and uncalcined MNZ/Fe surface.XPS spectrum of Fe at the core level is depicted in Figure4, ranging from 705 to 740 eV. A characteristic model represented the two main signals of Fe 2p3/2 and Fe 2p1/2 with binding energies of ~711.48±0.2 and ~724.60±0.2 eV which appeared to correspond to iron oxide Fe3+ in Fe3O4 (magnetite) phase [26, 27]. Two signals presented at ~719.08±0.2 and ~732.68±0.2 eV [28] are assigned to reorganization satellites. These are generally described as intrinsic energy losses that take place when the photoelectron leaves the atom in transition metals, such as Fe in metallic form or oxides. These signals showed reorganization characteristics at the core level that corresponded to the 2p energy level. In addition, the position of satellites is very sensitive to oxidation states of iron [29].Figure 4
XPS spectrum at core level of MNZ/Fe in the Fe 2p region.A satellite is an XPS signal of a photon that loses a small amount of energy and appears with a binding energy greater than the main peak. These signals of vibration at core level are caused by an X-ray photon that delivers a portion of its energy to the excitation of a secondary electron instead of giving the total amount of energy to a primary electron [29]. Fe compounds with oxidation state (II) had a shoulder in the photoelectric peak 2p3/2 corresponding to its satellite, while the satellite signal in oxidation state (III) was very characteristic, as shown in Figure 4 at ~720.38±0.2 eV. On Fe species with mixed oxidation states (Fe2+, Fe3+), as is the case of Fe3O4, the satellite of charge transfer disappeared from the spectrum [30, 31]. Also, multiplets of Fe2+ and Fe3+ oxidation states for Fe3O4 species were observed in the 2p3/2 signal. These are presented in Table 2, where the main peaks of magnetite in its oxidation states, Fe3+ had a main peak at ~711.48±0.2 eV, while Fe2+ species were found at ~708.58±0.2 eV.Table 2
XPS spectrum parameters at core level of Fe 2p3/2 for magnetite.
Specie
Chemical
Peak 1 (eV)
Peak 2 (eV)
Peak 3 (eV)
Magnetite
Fe3O4Fe2+
708.30a
709.30b
710.40b
Fe3O4Fe3+
711.30b
712.40c
713.60c
a Refs. [27, 28, 32, 33], b Refs. [25, 27], c Ref. [25].Fe species exposed on MNZ/Fe surface are reported in Table3 for calcined and uncalcined samples. The uncalcined sample contained 43.9 w% of Fe3+ as oxide, 39.7 w% of Fe3+ as oxyhydroxides, and 16.4 w% of Fe2+ as oxide. With regard to calcined samples at 550 and 700°C, the amount of Fe3+, oxide, and oxyhydroxide increased due to oxidation of Fe2+ to Fe3+ [34, 35]. After calcination at 550°C, the amount of Fe3+ as oxide increased to 45.7 w%, the same occurred for oxyhydroxides which increased to 41.4 w%, but Fe2+ decreased to 12.9 w%. Evenly, for calcined sample at 700°C, the oxides increased up to 46.6 w%, oxyhydroxides up to 42.2 w%, and Fe2+ oxides decreased to 11.2 w%. This could be explained because a part of the Fe2+ was oxidized to Fe3+; however, the signals of magnetite and oxyhydroxides were only observed.Table 3
Fe species on the MNZ/Fe surface.
Species
Composition (w%)
Uncalcined
550°C
700°C
Fe2p3, Fe3+ (oxide)
43.90
45.70
46.60
Fe2p3, Fe3+ (oxyhydroxides)
39.70
41.40
42.20
Fe2p3, Fe2+ (oxide)
16.40
12.90
11.20


### 3.3. Mössbauer and Raman Spectroscopy

The Mössbauer spectra of uncalcined and calcined MNZ/Fe are shown in Figure5. The spectra were recorded at 27°C, the adsorption spectra were adjusted with program NORMOS [36], the γ radiation source was 57Co of 925 MBq (25 mCi) inside a rhodium matrix, and the displacement of chemical isomer shift (δ) were given in relation with α-Fe. The observed signals in Figure 5(a) corresponded to Fe2+ and Fe3+ ions. Both were in a proportion of 45.5 w% and 54.5 w%, in that order. These signals are called doublets and are generally present in species that contain magnetic iron [37]. Based on the parameters of Mössbauer doublets, the Fe2+ fraction was related to fayalite species (Fe2+)2SiO4 with a chemical isomer shift of 1.13 mm/s [38]. These species belonged to nesosilicates class commonly found in volcanic rocks, and Fe3+ fraction were associated to magnetite species with a δ=0.24 mm/s [39] as listed in Table 4. The spectrum showed in Figure 5(b) for the MNZ/Fe calcined sample at 700°C presented 15.7% of relative area which corresponded to Fe2+. Two more peaks were identified as Fe3+ with 13% and 71.3%. The doublet of Fe2+ agreed with magnetite species with a δ=0.63 mm/s [40], as well as the second signal of Fe3+ that also coincided with magnetite (δ=0.29 mm/s) [39–41]. The changes in Fe3+ quantity may be due to (a) oxidation process from Fe2+ to Fe3+ caused by MNZ/Fe calcination or (b) heterogeneous nature of mineral that can vary its composition of both Fe and zeolite species. The doublet of Fe3+ species that had a relative area of 13% presented a δ=0.11 mm/s, which was a characteristic of chlorite species [42, 43], this Fe specie was a crystalline aluminosilicate associated to the phyllosilicates group with a condensed chemical formula of (Fe)3(Si,Al)4O10(OH)2(Fe)3(OH)6.Figure 5
Mössbauer spectra of MNZ/Fe: (a) uncalcined at 25°C and (b) calcined at 700°C.
(a)
(b)Table 4
Mossbauer parameters of MNZ/Fe samples.
Sample
δ(mm/s)
Δ (mm/s)
Г (mm/s)
Fe
Relative area (%)
Uncalcined MNZ/Fe
1.13
1.73
0.51
Fe2+
45.5
0.24
0.62
0.51
Fe3+
54.5
Calcined MNZ/Fe at 700°C
0.63
1.47
0.50
Fe2+
15.7
0.11
1.39
0.50
Fe3+
13.0
0.29
1.22
0.50
Fe3+
71.3
δ = isomer shift relative to α-Fe at room temperature; Δ = quadrupole splitting; Г = line width.Additionally, Raman analyses are shown in Figure6. Based on Figure 6(a), a black Fe cluster with an irregular shape and 13.5 μm of diameter was impregnated on the zeolite matrix. This was corroborated with micro-Raman spectrum in Figure 6(b) where signals were presented in lengths of 193, 219, 346, 630, and 668 cm-1 related to magnetite species [44, 45]. Therefore, the acid solution during the impregnation process allowed Fe clustering to be embedded on the mineral surface since the natural zeolite has a negative Z potential at these conditions [7].Figure 6
Raman spectrum for MNZ/Fe calcined at 700°C: (a) optic image and (b) micro-Raman spectrum.
(a)
(b)


### 3.4. Transmission Electron Microscopy (TEM)

The structure and morphology of MNZ impregnated with Fe was attained by TEM analyses and the images were processed through the Digital Micrograph (Gatan Program, version 3.30.2016.0). Each image was calibrated in nanometer scale, later the Fast Fourier Transform (FFT), and finally the inverse FFT were applied to obtain lattice distance for each sample. TEM images depicted in Figure7 belong to uncalcined MNZ/Fe samples.Figure 7
TEM images of uncalcined MNZ/Fe: (a) scale of 100 nm, (b-d) scale of 5 nm.
(a)
(b)
(c)
(d)The MNZ matrix can be observed at a scale of 100 nm from Figure7(a) where the embedded Fe particles have a size of ~8.32 nm, meanwhile an irregular Fe particle was observed in Figure 7(b) with a size of 6.62 nm. In addition, the lattice distance was estimated to be 0.253 nm and the plane (311) is characteristic of crystalline magnetite (Fe3O4) nanoparticles [46]. Based on Figures 7(c) and 7(d) scaled at 5 nm, the spacing of 0.253 nm and a plane of (311) confirmed the presence of magnetite species where Fe particles were found with sizes of 3.89 and 5.67 nm, respectively.Similarly, TEM images of calcined MNZ/Fe samples at 700°C are depicted in Figure8. The zeolite support was observed in Figure 8(a) with irregular incrustations of Fe particles up to 1 nm. The FTT patterns included in Figures 8(b) and 8(c) demonstrated that the lattice distance was 0.49 nm with a plane (111) [47]. This evidence denoted that the crystalline magnetite species were still present after calcination process, and Fe3O4 particles had a size of 19.63 nm (b) and 12.46 nm (c).Figure 8
TEM images of calcined MNZ/Fe at 700°C: (a) scale of 10 nm, (b) scale of 20 nm, and (c) scale of 10 nm.
(a)
(b)
(c)


## 3.1. X-Ray Diffraction

Mineral samples were analyzed by X-ray diffraction in order to observe the effect of calcination temperature on zeolite structure. XRD patterns of uncalcined natural zeolite (25°C) and calcined natural zeolite at 300, 600, and 700°C are shown in Figure1. The material was identified as a mixture of different zeolitic phases where the main phase was mordenite-heulandite, erionite-cristobalite as a secondary phase, and quartz as an impurity. Below 17° 2theta, no significant signals were found that yield information about the material characterization.Figure 1
XRD patterns of MNZ/Fe samples for uncalcined at 25°C and calcined at 300, 600, and 700°C: ●: heulandite, ○: mordenite, ♦: erionite, ♢: cristobalite, ▲: quartz.Different signals were grouped from 17° 2theta to 68° 2theta where the most intense signal located at 30.9° 2theta was referred to mordenite (JCPDS: O60239). This highest signal remained for any temperatures (25–700°C); however, the intensity was decreasing above 700°C until mineral disappearance at 900°C [16]. Similar behavior was noted for heulandite (JCPDS: 210131), it disappeared at 600°C due to structure collapses above 500°C [17, 18]. On the opposite, erionite (JCPDS: 39-1379) was constituted in the sample up to 700°C and tends to disappear at 840°C [19], erionite increased its intensity with respect to the uncalcined sample due to heulandite phase disappears. Besides, as natural zeolite does not have a homogeneous composition, so its structure can change from one sample to another.Additionally, it is observed that cristobalite (JCPDS: 075-0923) was contained after calcination treatment (up to 700°C) but it disappears at 1525°C [20]. Contrarily, the signals that were located above 55° 2theta corresponded in their great majority to quartz (JCPDS: 46-1045) [21] and mordenite since these phases prevail after calcination at 700°C. Lastly, it was observed that zeolitic structures persisted after the thermal treatment with the exception of heulandite.


## 3.2. XPS Analysis

X-ray photoelectron spectroscopy analysis gives information about the material surface at a depth not greater than 8 to 10 atomic layers, with aspatialresolution≤6μm. XPS is able to identify the elements from lithium to uranium with exception of hydrogen and helium. The element concentration must be higher than to 0.05% atomic to be detected in the sample [22].XPS spectra were obtained using a K-alpha X-ray photoelectron spectrometer (Thermo Fisher Scientific Co.) with a monochromatic source of Al Kα X-rays (1486.6 eV). The sample diameter was 400 μm. Firstly, it remained in a prechamber for 600 min; then, samples were transferred to the chamber at about 1×10−9 Torr. For each sample, three measurements were carried out in different zones. The analyzer passed energy of 200 eV and 40 eV for the scans collection and high-resolution spectra, respectively. All spectra were calibrated with an adventitious peak C1s at 284.6 eV to detect and compensate for the variable charge at core peaks. The software Thermo Avantage v5.979 was used for the curve fitting of a high-resolution spectrum, and the deconvolution was made using the Shirley method with a Gaussian-Lorentzian contribution 70-30%.Subsequently, Fe species presented in MNZ/Fe were found and identified on the surface. XPS spectra of uncalcined natural zeolite at 25°C as well as calcined at 550 and 700°C are shown in Figure2. The major elements on surface were Si and Al corroborating an aluminosilicate type material. The amount of Si varied from 27.1 to 29 w% while Al was ranging from 8.4 to 8.5 w%. The presence of Na, Mg, Ca, K, and Fe minerals was also observed.Figure 2
XPS spectra of MNZ/Fe: uncalcined at 25°C and calcined at 550 and 700°C.The global composition of MNZ samples impregnated with 10 mg MNZ/Fe are listed in Table1 for different temperatures (uncalcined at 25°C and calcined at 550 and 700°C). It can be noted that the composition of Al, C, Mg, K, and Na did not have a significant change. O and Ca composition diminished by comparing calcined and uncalcined analyses. Meanwhile, Si and Fe (3.9 w%) composition increased after the calcination process about 2 percentage units. These results demonstrated that composition could have variations because of the mineral nature [23]. This was in agreement with the previous work reported by Domenzain et al. [23]. On that research, the composition of Fe in a MNZ without impregnation was about 2.3 w% identified by EDS analyses and 2.6 w% of Fe oxides quantified by atomic absorption.Table 1
MNZ composition impregnated with 10 mg FeCl3/g MNZ for calcined and uncalcined samples.
Name
MNZ/Fe composition (w%)
(25°C)
(550°C)
(700°C)
O 1 s
47.40
46.00
45.00
Si 2p
27.10
29.00
28.60
Al 2p
8.50
8.40
8.50
Ca 2p
4.10
2.00
2.30
C 1 s
4.00
3.70
4.50
Fe 2p
3.90
6.00
6.20
Mg 1 s
2.20
2.30
2.00
K 2p
1.30
1.30
1.80
Na 1 s
0.80
0.20
0.30Fe can be present in natural minerals as different species, one of the most common is the magnetite (Fe3O4), which is a compound of mixed valence and commonly expressed with the notation as (Fe3+)tet(Fe2+Fe3+)octO4. Due to rapid jump of electrons which move with a frequency of approximately 10-11 s at room temperature, the octahedral ions Fe3+ and Fe2+ can be written as Fe2.5+ [24]. In addition, the Mössbauer spectrum of Fe3O4 at room temperature shows only two overlapping sextets which correspond to tetrahedral ions of Fe3+ and octahedral ions of Fe2.5+.XPS spectra of Fe species for uncalcined MNZ/Fe at 25°C and calcined MNZ/Fe at 550 and 700°C are shown in Figure3. These were located between 705 and 740 eV of binding energy. Intensity variations in spectra were observed between calcined and uncalcined samples. The first one contained 3.9 w% of Fe on its surface, whereas the calcined samples (550 and 700°C) had 6 w% and 6.2 w% of Fe, respectively. The Fe spectrum has two representative peaks of Fe3+ ion characteristics of Fe3O4 structure, the main corresponds to Fe 2p3/2 located around 711.48±0.2 eV [25] and the second peak is referred to as 2p1/2 situated in 724.60±0.2 eV. These variations in Fe composition may be attributed to the following aspects: (1) the increase of Fe particles caused by impregnation, (2) the presence of other compounds on material surface that did not allow observing the Fe ions, (3) the change on the mineral structure due to the zeolitic species collapse after calcination, and (d) the amount of each compound varied depending on the analyzed crystal [23].Figure 3
XPS spectra for Fe 2p of calcined and uncalcined MNZ/Fe surface.XPS spectrum of Fe at the core level is depicted in Figure4, ranging from 705 to 740 eV. A characteristic model represented the two main signals of Fe 2p3/2 and Fe 2p1/2 with binding energies of ~711.48±0.2 and ~724.60±0.2 eV which appeared to correspond to iron oxide Fe3+ in Fe3O4 (magnetite) phase [26, 27]. Two signals presented at ~719.08±0.2 and ~732.68±0.2 eV [28] are assigned to reorganization satellites. These are generally described as intrinsic energy losses that take place when the photoelectron leaves the atom in transition metals, such as Fe in metallic form or oxides. These signals showed reorganization characteristics at the core level that corresponded to the 2p energy level. In addition, the position of satellites is very sensitive to oxidation states of iron [29].Figure 4
XPS spectrum at core level of MNZ/Fe in the Fe 2p region.A satellite is an XPS signal of a photon that loses a small amount of energy and appears with a binding energy greater than the main peak. These signals of vibration at core level are caused by an X-ray photon that delivers a portion of its energy to the excitation of a secondary electron instead of giving the total amount of energy to a primary electron [29]. Fe compounds with oxidation state (II) had a shoulder in the photoelectric peak 2p3/2 corresponding to its satellite, while the satellite signal in oxidation state (III) was very characteristic, as shown in Figure 4 at ~720.38±0.2 eV. On Fe species with mixed oxidation states (Fe2+, Fe3+), as is the case of Fe3O4, the satellite of charge transfer disappeared from the spectrum [30, 31]. Also, multiplets of Fe2+ and Fe3+ oxidation states for Fe3O4 species were observed in the 2p3/2 signal. These are presented in Table 2, where the main peaks of magnetite in its oxidation states, Fe3+ had a main peak at ~711.48±0.2 eV, while Fe2+ species were found at ~708.58±0.2 eV.Table 2
XPS spectrum parameters at core level of Fe 2p3/2 for magnetite.
Specie
Chemical
Peak 1 (eV)
Peak 2 (eV)
Peak 3 (eV)
Magnetite
Fe3O4Fe2+
708.30a
709.30b
710.40b
Fe3O4Fe3+
711.30b
712.40c
713.60c
a Refs. [27, 28, 32, 33], b Refs. [25, 27], c Ref. [25].Fe species exposed on MNZ/Fe surface are reported in Table3 for calcined and uncalcined samples. The uncalcined sample contained 43.9 w% of Fe3+ as oxide, 39.7 w% of Fe3+ as oxyhydroxides, and 16.4 w% of Fe2+ as oxide. With regard to calcined samples at 550 and 700°C, the amount of Fe3+, oxide, and oxyhydroxide increased due to oxidation of Fe2+ to Fe3+ [34, 35]. After calcination at 550°C, the amount of Fe3+ as oxide increased to 45.7 w%, the same occurred for oxyhydroxides which increased to 41.4 w%, but Fe2+ decreased to 12.9 w%. Evenly, for calcined sample at 700°C, the oxides increased up to 46.6 w%, oxyhydroxides up to 42.2 w%, and Fe2+ oxides decreased to 11.2 w%. This could be explained because a part of the Fe2+ was oxidized to Fe3+; however, the signals of magnetite and oxyhydroxides were only observed.Table 3
Fe species on the MNZ/Fe surface.
Species
Composition (w%)
Uncalcined
550°C
700°C
Fe2p3, Fe3+ (oxide)
43.90
45.70
46.60
Fe2p3, Fe3+ (oxyhydroxides)
39.70
41.40
42.20
Fe2p3, Fe2+ (oxide)
16.40
12.90
11.20


## 3.3. Mössbauer and Raman Spectroscopy

The Mössbauer spectra of uncalcined and calcined MNZ/Fe are shown in Figure5. The spectra were recorded at 27°C, the adsorption spectra were adjusted with program NORMOS [36], the γ radiation source was 57Co of 925 MBq (25 mCi) inside a rhodium matrix, and the displacement of chemical isomer shift (δ) were given in relation with α-Fe. The observed signals in Figure 5(a) corresponded to Fe2+ and Fe3+ ions. Both were in a proportion of 45.5 w% and 54.5 w%, in that order. These signals are called doublets and are generally present in species that contain magnetic iron [37]. Based on the parameters of Mössbauer doublets, the Fe2+ fraction was related to fayalite species (Fe2+)2SiO4 with a chemical isomer shift of 1.13 mm/s [38]. These species belonged to nesosilicates class commonly found in volcanic rocks, and Fe3+ fraction were associated to magnetite species with a δ=0.24 mm/s [39] as listed in Table 4. The spectrum showed in Figure 5(b) for the MNZ/Fe calcined sample at 700°C presented 15.7% of relative area which corresponded to Fe2+. Two more peaks were identified as Fe3+ with 13% and 71.3%. The doublet of Fe2+ agreed with magnetite species with a δ=0.63 mm/s [40], as well as the second signal of Fe3+ that also coincided with magnetite (δ=0.29 mm/s) [39–41]. The changes in Fe3+ quantity may be due to (a) oxidation process from Fe2+ to Fe3+ caused by MNZ/Fe calcination or (b) heterogeneous nature of mineral that can vary its composition of both Fe and zeolite species. The doublet of Fe3+ species that had a relative area of 13% presented a δ=0.11 mm/s, which was a characteristic of chlorite species [42, 43], this Fe specie was a crystalline aluminosilicate associated to the phyllosilicates group with a condensed chemical formula of (Fe)3(Si,Al)4O10(OH)2(Fe)3(OH)6.Figure 5
Mössbauer spectra of MNZ/Fe: (a) uncalcined at 25°C and (b) calcined at 700°C.
(a)
(b)Table 4
Mossbauer parameters of MNZ/Fe samples.
Sample
δ(mm/s)
Δ (mm/s)
Г (mm/s)
Fe
Relative area (%)
Uncalcined MNZ/Fe
1.13
1.73
0.51
Fe2+
45.5
0.24
0.62
0.51
Fe3+
54.5
Calcined MNZ/Fe at 700°C
0.63
1.47
0.50
Fe2+
15.7
0.11
1.39
0.50
Fe3+
13.0
0.29
1.22
0.50
Fe3+
71.3
δ = isomer shift relative to α-Fe at room temperature; Δ = quadrupole splitting; Г = line width.Additionally, Raman analyses are shown in Figure6. Based on Figure 6(a), a black Fe cluster with an irregular shape and 13.5 μm of diameter was impregnated on the zeolite matrix. This was corroborated with micro-Raman spectrum in Figure 6(b) where signals were presented in lengths of 193, 219, 346, 630, and 668 cm-1 related to magnetite species [44, 45]. Therefore, the acid solution during the impregnation process allowed Fe clustering to be embedded on the mineral surface since the natural zeolite has a negative Z potential at these conditions [7].Figure 6
Raman spectrum for MNZ/Fe calcined at 700°C: (a) optic image and (b) micro-Raman spectrum.
(a)
(b)


## 3.4. Transmission Electron Microscopy (TEM)

The structure and morphology of MNZ impregnated with Fe was attained by TEM analyses and the images were processed through the Digital Micrograph (Gatan Program, version 3.30.2016.0). Each image was calibrated in nanometer scale, later the Fast Fourier Transform (FFT), and finally the inverse FFT were applied to obtain lattice distance for each sample. TEM images depicted in Figure7 belong to uncalcined MNZ/Fe samples.Figure 7
TEM images of uncalcined MNZ/Fe: (a) scale of 100 nm, (b-d) scale of 5 nm.
(a)
(b)
(c)
(d)The MNZ matrix can be observed at a scale of 100 nm from Figure7(a) where the embedded Fe particles have a size of ~8.32 nm, meanwhile an irregular Fe particle was observed in Figure 7(b) with a size of 6.62 nm. In addition, the lattice distance was estimated to be 0.253 nm and the plane (311) is characteristic of crystalline magnetite (Fe3O4) nanoparticles [46]. Based on Figures 7(c) and 7(d) scaled at 5 nm, the spacing of 0.253 nm and a plane of (311) confirmed the presence of magnetite species where Fe particles were found with sizes of 3.89 and 5.67 nm, respectively.Similarly, TEM images of calcined MNZ/Fe samples at 700°C are depicted in Figure8. The zeolite support was observed in Figure 8(a) with irregular incrustations of Fe particles up to 1 nm. The FTT patterns included in Figures 8(b) and 8(c) demonstrated that the lattice distance was 0.49 nm with a plane (111) [47]. This evidence denoted that the crystalline magnetite species were still present after calcination process, and Fe3O4 particles had a size of 19.63 nm (b) and 12.46 nm (c).Figure 8
TEM images of calcined MNZ/Fe at 700°C: (a) scale of 10 nm, (b) scale of 20 nm, and (c) scale of 10 nm.
(a)
(b)
(c)


## 4. Catalytic Evaluation of MNZ/Fe

Reactive Black 5 (RB5) dye degradation in aqueous solutions was carried out by photo-Fenton heterogeneous process in order to evaluate the catalytic activity of the MNZ impregnated with Fe particles as a catalyst. This kind of metal can promote formation of hydroxyl radicals from peroxide [48–53] and Fe is more feasible to be impregnated by economic and environmental friendly method.Fenton process consists of reaction of Fe2+ with hydrogen peroxide under acid conditions for production of hydroxyl radicals (OH⋅), which is highly reactive [54, 55]. The oxidation mechanism Fe2+ with H2O2 consists of transferring an electron from the valence shell to the hydroxyl radicals and hydroxyl anions (reaction 1) [55, 56]. Other reactions associated with Fenton process are shown in reactions 2–7, which can occur simultaneously [57, 58]. These reactions are reached so quickly and are considered undesirable since hydroxyl radicals are not produced and hence an inhibition of Fenton reaction.
(1)Fe2++H2O2⟶Fe3++OH−+OH•(2)Fe3++H2O2⟷Fe−OOH2++H+(3)Fe−OOH2+⟶OOH⋅+Fe2+(4)Fe2++OH⋅⟶Fe3++OH−(5)H2O2+OH⋅⟶H2O+OOH⋅(6)Fe3++OOH⋅⟶Fe2++O2+H+(7)Fe2++OOH⋅⟶Fe3++OOH−A variant of this process is photo-Fenton reaction [59, 60] in which a photooxidation takes place through a radiation source of Fe3+ hydrated followed by a transfer of photoinduced electrons where Fe2+ and OH⋅ are formed, as shown in equations (8) and (9).
(8)Fe3++H2O→FeOH2++H+(9)FeOH2++hν→Fe2++OH•Finally, the main reaction for the present work between the RB5 dye and hydroxyl ions is presented in equation (10). The preferable products are carbon dioxide and water, but low-molecular-weight compounds could be obtained as secondary products when complete degradation is not achieved.
(10)OH⋅+RB5→lowmolecularweightcompounds+CO2+H2O


### 4.1. Calcination Temperature Effect and Fe Amount

Calcination temperature effect over MNZ impregnated with 5 and 10 mg MNZ/Fe was evaluated for RB5 dye degradation by means of photo-Fenton process. Calcined and uncalcined MNZ/Fe samples were used in different reactions as tabulated in Table5. This evaluation was carried out at initial conditions of pH=2.5, H2O2=3 g/L, RB50=100 mg/L, solution of MNZ/Fe=0.05 g/L, and a radiation source of 405 nm (2.2 W). These conditions were used to avoid shielding and deactivation effects due to catalyst amount in the solution.Table 5
Catalytic evaluation conditions of MNZ impregnated with FeCl3.
Reaction
Calcination temperature (°C)
(MNZ/Fe) (g/L)
MNZ/Fe (mg/g)
MNZ 1
Uncalcined
0.05
—
MNZ 2
Uncalcined
0.05
10
MNZ 3
550
0.05
5
MNZ 4
550
0.05
10
MNZ 5
700
0.05
5
MNZ 6
700
0.05
10
pH=2.5; H2O2=3 g/L; RB50=100mg/L; λ=405nm.The UV-Vis absorption spectrum of (RB5)0 dye at 100 mg/L and its degradation process is observed in Figure 9 ranged each 10 min. Its chromophore signal (597 nm) was the unique one taken into account because it is the most representative. This signal decreases gradually, while the absorbance on the signals at 312 and 392 nm was observed to increase at the beginning of the reaction, but these diminished after 10 min. The absorbance increase in the first 10 minutes could be due to the fact that lower molecular weight compounds were being produced during the RB5 dye removal. These other compound absorbed these wavelengths (392 nm and 312 nm) making it difficult to analyze the signals.Figure 9
UV-Vis spectra of RB5 dye degradation by heterogeneous photo-Fenton process using MNZ/Fe.The kinetics for the RB5 dye discoloration at the conditions described in Table5 is observed in Figure 10.Figure 10
RB5 dye discoloration by heterogeneous photo-Fenton process using MNZ/Fe.In all cases, the discoloration percentage (Dt%) was calculated using equation (11) [61]:
(11)Dt%=C0−CtC0×100Where C0 is referred to as the initial concentration of RB5 dye and Ct denotes the corresponding concentration at a certain time. The MNZ 1 reaction was evaluated using a natural zeolite without Fe impregnated and without radiation source; it can be seen that there was no decrease in RB5 discoloration at these conditions and there was not adsorption of dye in the zeolite matrix, because the UV-Vis spectrum signal of the RB5 dye had not any changes during the process. The reactions MNZ 2, MNZ 3, MNZ 4, MNZ 5, and MNZ 6 were exposed to radiation by LED lamps in order to increase the production of OH⋅ radicals and thus form a greater quantity of hydroxyl ions. A slight decrease in coloration, only 6.5 D180%, was obtained for the MNZ 2 reaction using uncalcined zeolite and impregnated with 10 mg MNZFe. A significant influence of the calcination temperature thought the reaction MNZ 3 produced a discoloration in the order of 25.2 D180%.Subsequently, a great activity was achieved for the first ten minutes of MNZ 4 reaction with 20 D10% in RB5 dye discoloration. However, the activity only reached about 71.5 D180% at the end of the reaction. This effect could be due to abrupt H2O2 consumption after the first ten minutes causing the intervention of hydroxyl ions in secondary reactions that did not degrade RB5 dye [62]. Reaction MNZ 5 produced a gradual discoloration reaching 79.42 D180%. A similar behavior was found in reaction MNZ 6 where a discoloration of 91 D180% was achieved, been the maximum. The effect observed in the last two reactions could be due to the amount of Fe2+ and Fe3+ ions exposed on the MNZ surface, which benefited the interaction of these species with peroxide and light. Therefore, a greater OH⋅ ion formation was promoted and improved the photocatalytic activity in solution. In addition, the increase of Fe3+ concentration as oxide and oxyhydroxides compounds (magnetite and chlorite) also improved the catalytic activity [63].About the kinetics of photocatalytic degradation, the Langmuir–Hinshelwood (L-H) model was utilized to describe the RB5 dye degradation [64–66]. It is expressed as follows:
(12)r=−dCdt=kappCtnwhere r is degradation rate, Ct refers to the concentration at a reaction time t, and kapp is the apparent rate constant, which includes L-H rate constant kL−H, and the adsorption constant kad [64–66], and the superscript n denotes the reaction order.Different modifications to the L-H model are described elsewhere. Dong et al. [67] assumes that adsorption is a fast process and the determining stage for rate constant is the reaction that involves the species present in a monolayer of the solid-liquid interface. Therefore, the final expression for pseudo-first-order reactions is as follows:
(13)lnC0C=kapptIn this work, equation (13) was used for the evaluation of the apparent rate constant and its values are presented in Table 6.Table 6
Apparent rate constant of RB5 dye degradation.
Reaction
kapp(min-1)
R2
MNZ 1
—
—
MNZ 2
0.0005
0.92
MNZ 3
0.0015
0.94
MNZ 4
0.0080
0.94
MNZ 5
0.0083
0.91
MNZ 6
0.0089
0.96kapp was obtained from RB5 concentration and reaction time by means of the linearization of time against ln (C0/C). It is noted that kapp=0 for MNZ 1 reaction because there was a not catalytic activity, meanwhile the highest activity was obtained for MNZ 6 reaction with a kapp=0.0089 min-1 with a correlation coefficient R2=0.96.


### 4.2. Catalyst Dosage Effect

The chemical reactions can improve dye degradations according to the influence of each variable. The best RB5 dye degradation was attained with 10 mg MNZ/Fe calcined at 700°C. Based on these material specifications, the catalyst (MNZ/Fe) dosage effect in solution was analyzed for optimization purposes and avoiding shielding and inhibition effects caused by the catalyst concentration. The reaction conditions from MNZ 6 to MNZ 13 are presented in Table7. The catalyst dosage effect was observed by keeping constant pH=2.5, H2O2=3g/L, RB50=100mg/L, and lamp radiation λ=405 nm (2.2 W).Table 7
RB5 dye discoloration using MNZ/Fe as catalyst.
MNZ/Fe (10 mg FeCl3/g MNZ) @ 700°C
Reaction
(MNZ/Fe)(g/L)
D180%
kapp(min-1)
R2
MNZ 6
0.05
91
0.0089
0.96
MNZ 7
0.10
92
0.0156
0.96
MNZ 8
0.15
92
0.0207
0.92
MNZ 9
0.20
93
0.0225
0.97
MNZ 10
0.35
91
0.0129
0.96
MNZ 11
0.50
86
∗0.04200
0.90
MNZ 12
1.00
79
∗∗0.044700
0.87
MNZ 13
1.50
29
0.0019
0.98
∗kapp determined at 50 min; ∗∗kapp determined at 30 min.The behavior of RB5 dye discoloration with respect to catalyst dosage in solution was measured at 180 min (D180%) as illustrated in Figure 11. The discoloration percentage exceeded 90 D180% at MNZ/Fe=0.05–0.2g/L where the optimum discoloration yielded 93 D180% at 0.2 g/L on MNZ 9 reaction. On the other hand, the discoloration diminished as the (MNZ/Fe) was increasing. The D180% decreases when using 0.35 g/L yielding 91. Consequently, the D180% was decreasing with values of 86, 79 and 29 D180% for catalyst dose of 0.5, 1, and 1.5 g/L, in that order. The low discoloration seemed to be attributed by the deactivation through shielding effect. It is caused by the MNZ opacity in solution where radiation and peroxide amount promoted a re-oxidation of Fe2+ ions [68].Figure 11
Catalyst dosage effect over RB5 dye discoloration at 180 min (D180%).Thekapp values from MNZ 6 to MNZ 13 reactions are reported in Table 7 where pseudo-first-order was assumed for the reaction kinetics. The MNZ 9 reaction has the highest kapp after 180 min of reaction (0.0225 min-1). The kinetic constant was evaluated at 50 and 30 min for MNZ 11 and MNZ 12 reactions, respectively. No apparent change in RB5 dye concentration was noted beyond these times.


### 4.3. pH Effect on the Solution

Heterogeneous materials have a high catalytic activity in Fenton process for dye degradation in a wide pH range [69]. Then, the pH dependence in RB5 dye discoloration was analyzed in the pH interval of 2.5–4.5 and keeping constant MNZ/Fe=0.2 g/L, H2O2=3g/L, and RB50=100mg/L.The discoloration percentage RB5 dye after 180 min of reaction (D180%) is observed in Figure 12 as a function of pH solution. A discoloration of 93 D180% was obtained at pH=2.5 and 91 D180% at pH=3. However, there was no dye discoloration when pH was increased between 3.5 and 4.5.Figure 12
pH effect on RB5 dye discoloration usingMNZ/Fe=0.2g/L as catalyst.


### 4.4. Influence of H2O2 Concentration

The analysis of H2O2 concentration in the solution was carried out by keeping constant the amount of catalyst MNZ/Fe=0.2g/L, initial dye concentration RB50=100mg/L, and a solution acidity pH=2.5. Results depicted in Figure 13 demonstrated that using H2O2=3g/L, the major discoloration yielded 93 D180% with a kapp=0.0225 min-1. Below and above this mentioned concentration, the discoloration seemed to be inhibited as reported by the decrease in the D180% and the kapp. The values were 91 D180% (kapp=0.0131 min-1), 91.2 D180% kapp=0.0153 min-1), and 91 D180% kapp=0.0151 min-1) for (H2O2) fixed at 2.0, 4.0, and 5.0 g/L, respectively. This was because increasing peroxide amount was likely to promote secondary reactions that consume H2O2 and therefore inhibit the RB5 degradation reaction.Figure 13
Effect of H2O2 concentration on RB5 dye degradation using MNZ/Fe=0.2g/L as catalyst.


### 4.5. Initial Concentration of RB5 Dye (RB5)0

The initial concentration of RB5 dye was also studied by keeping constant the amount ofH2O2=3g/L, pH=2.5, and catalyst MNZ/Fe=0.2 g/L. Results are shown in Figure 14. In general, the great activity ocurred in the first reaction minutes. The major discoloration was obtained using RB50=100mg/L on the MNZ 9 reaction with 89 D100% at 100 min; later, the reaction tended to be slow since at 180 min reached 93 D180%. For RB50=80mg/L, the discoloration was gradual but with a slower reaction rate than the reported one by 100 mg/L. 61 D100% was obtained and subsequently the reaction slowed down reaching 72 D180% with a kapp=0.0139min-1 (R2=0.96) at RB50=80mg/L. In addition, a similar behavior like using 80 mg/L was exhibited when the initial concentration of RB5 was reduced to 60 and 40 mg/L. Discoloration yielded 40 D100% and 51 D180% with a kapp=0.0113 min-1 (R2=0.95) for RB50=60mg/L. Subsequently, if RB50=40 mg/L were used, 26 D100% and 34 D180% kapp=0.0113min-1 (R2=0.95) were obtained. The difference observed in Dt% was because on the (RB5)0 decreased, and thus it made it difficult to achieve a suitable interaction between the OH⋅ radicals and the compounds to be removed.Figure 14
Effect of initial concentration of (RB5)0 using MNZ/Fe=0.2 g/L as catalyst.


### 4.6. COD Removal

The removal ofRB50=100 mg/L using different concentrations of MNZ/Fe was determined at pH=2.5, H2O2=3 g/L, and light radiation (405 nm) for measuring chemical oxygen demand (COD) removal. The COD removal percentage after 180 min of reaction (COD180%) is observed in Figure 15.Figure 15
COD removal of RB5 dye.It was determined by equation (14):
(14)CODt%=COD0−CODtCOD0×100The subscripts 0 andt denote the COD removal at initial and fixed time, respectively. The great COD removal was observed at concentrations of 0.05, 0.1, and 0.15 g/L (MNZ/Fe) with degradations of 68.5, 67.7, and 68.5 COD180%, in that order. The highest removal (70.5 COD180%) was achieved with MNZ/Fe=0.2 g/L. The efficiency of the reaction was reduced when the catalyst concentration was increased to 0.35, 0.5, 1, and 1.5 g/L with corresponding removals of 62.8, 61.4, 50, and 30 COD180%. This behavior was probably attributed to an increase on the catalyst amount that inhibited the reaction and the absence of active sites. Moreover, the opacity of the MNZ/Fe probably interfered with the reaction causing a shielding effect and therefore low interaction between the OH⋅ ions and the RB5 dye [68].


## 4.1. Calcination Temperature Effect and Fe Amount

Calcination temperature effect over MNZ impregnated with 5 and 10 mg MNZ/Fe was evaluated for RB5 dye degradation by means of photo-Fenton process. Calcined and uncalcined MNZ/Fe samples were used in different reactions as tabulated in Table5. This evaluation was carried out at initial conditions of pH=2.5, H2O2=3 g/L, RB50=100 mg/L, solution of MNZ/Fe=0.05 g/L, and a radiation source of 405 nm (2.2 W). These conditions were used to avoid shielding and deactivation effects due to catalyst amount in the solution.Table 5
Catalytic evaluation conditions of MNZ impregnated with FeCl3.
Reaction
Calcination temperature (°C)
(MNZ/Fe) (g/L)
MNZ/Fe (mg/g)
MNZ 1
Uncalcined
0.05
—
MNZ 2
Uncalcined
0.05
10
MNZ 3
550
0.05
5
MNZ 4
550
0.05
10
MNZ 5
700
0.05
5
MNZ 6
700
0.05
10
pH=2.5; H2O2=3 g/L; RB50=100mg/L; λ=405nm.The UV-Vis absorption spectrum of (RB5)0 dye at 100 mg/L and its degradation process is observed in Figure 9 ranged each 10 min. Its chromophore signal (597 nm) was the unique one taken into account because it is the most representative. This signal decreases gradually, while the absorbance on the signals at 312 and 392 nm was observed to increase at the beginning of the reaction, but these diminished after 10 min. The absorbance increase in the first 10 minutes could be due to the fact that lower molecular weight compounds were being produced during the RB5 dye removal. These other compound absorbed these wavelengths (392 nm and 312 nm) making it difficult to analyze the signals.Figure 9
UV-Vis spectra of RB5 dye degradation by heterogeneous photo-Fenton process using MNZ/Fe.The kinetics for the RB5 dye discoloration at the conditions described in Table5 is observed in Figure 10.Figure 10
RB5 dye discoloration by heterogeneous photo-Fenton process using MNZ/Fe.In all cases, the discoloration percentage (Dt%) was calculated using equation (11) [61]:
(11)Dt%=C0−CtC0×100Where C0 is referred to as the initial concentration of RB5 dye and Ct denotes the corresponding concentration at a certain time. The MNZ 1 reaction was evaluated using a natural zeolite without Fe impregnated and without radiation source; it can be seen that there was no decrease in RB5 discoloration at these conditions and there was not adsorption of dye in the zeolite matrix, because the UV-Vis spectrum signal of the RB5 dye had not any changes during the process. The reactions MNZ 2, MNZ 3, MNZ 4, MNZ 5, and MNZ 6 were exposed to radiation by LED lamps in order to increase the production of OH⋅ radicals and thus form a greater quantity of hydroxyl ions. A slight decrease in coloration, only 6.5 D180%, was obtained for the MNZ 2 reaction using uncalcined zeolite and impregnated with 10 mg MNZFe. A significant influence of the calcination temperature thought the reaction MNZ 3 produced a discoloration in the order of 25.2 D180%.Subsequently, a great activity was achieved for the first ten minutes of MNZ 4 reaction with 20 D10% in RB5 dye discoloration. However, the activity only reached about 71.5 D180% at the end of the reaction. This effect could be due to abrupt H2O2 consumption after the first ten minutes causing the intervention of hydroxyl ions in secondary reactions that did not degrade RB5 dye [62]. Reaction MNZ 5 produced a gradual discoloration reaching 79.42 D180%. A similar behavior was found in reaction MNZ 6 where a discoloration of 91 D180% was achieved, been the maximum. The effect observed in the last two reactions could be due to the amount of Fe2+ and Fe3+ ions exposed on the MNZ surface, which benefited the interaction of these species with peroxide and light. Therefore, a greater OH⋅ ion formation was promoted and improved the photocatalytic activity in solution. In addition, the increase of Fe3+ concentration as oxide and oxyhydroxides compounds (magnetite and chlorite) also improved the catalytic activity [63].About the kinetics of photocatalytic degradation, the Langmuir–Hinshelwood (L-H) model was utilized to describe the RB5 dye degradation [64–66]. It is expressed as follows:
(12)r=−dCdt=kappCtnwhere r is degradation rate, Ct refers to the concentration at a reaction time t, and kapp is the apparent rate constant, which includes L-H rate constant kL−H, and the adsorption constant kad [64–66], and the superscript n denotes the reaction order.Different modifications to the L-H model are described elsewhere. Dong et al. [67] assumes that adsorption is a fast process and the determining stage for rate constant is the reaction that involves the species present in a monolayer of the solid-liquid interface. Therefore, the final expression for pseudo-first-order reactions is as follows:
(13)lnC0C=kapptIn this work, equation (13) was used for the evaluation of the apparent rate constant and its values are presented in Table 6.Table 6
Apparent rate constant of RB5 dye degradation.
Reaction
kapp(min-1)
R2
MNZ 1
—
—
MNZ 2
0.0005
0.92
MNZ 3
0.0015
0.94
MNZ 4
0.0080
0.94
MNZ 5
0.0083
0.91
MNZ 6
0.0089
0.96kapp was obtained from RB5 concentration and reaction time by means of the linearization of time against ln (C0/C). It is noted that kapp=0 for MNZ 1 reaction because there was a not catalytic activity, meanwhile the highest activity was obtained for MNZ 6 reaction with a kapp=0.0089 min-1 with a correlation coefficient R2=0.96.


## 4.2. Catalyst Dosage Effect

The chemical reactions can improve dye degradations according to the influence of each variable. The best RB5 dye degradation was attained with 10 mg MNZ/Fe calcined at 700°C. Based on these material specifications, the catalyst (MNZ/Fe) dosage effect in solution was analyzed for optimization purposes and avoiding shielding and inhibition effects caused by the catalyst concentration. The reaction conditions from MNZ 6 to MNZ 13 are presented in Table7. The catalyst dosage effect was observed by keeping constant pH=2.5, H2O2=3g/L, RB50=100mg/L, and lamp radiation λ=405 nm (2.2 W).Table 7
RB5 dye discoloration using MNZ/Fe as catalyst.
MNZ/Fe (10 mg FeCl3/g MNZ) @ 700°C
Reaction
(MNZ/Fe)(g/L)
D180%
kapp(min-1)
R2
MNZ 6
0.05
91
0.0089
0.96
MNZ 7
0.10
92
0.0156
0.96
MNZ 8
0.15
92
0.0207
0.92
MNZ 9
0.20
93
0.0225
0.97
MNZ 10
0.35
91
0.0129
0.96
MNZ 11
0.50
86
∗0.04200
0.90
MNZ 12
1.00
79
∗∗0.044700
0.87
MNZ 13
1.50
29
0.0019
0.98
∗kapp determined at 50 min; ∗∗kapp determined at 30 min.The behavior of RB5 dye discoloration with respect to catalyst dosage in solution was measured at 180 min (D180%) as illustrated in Figure 11. The discoloration percentage exceeded 90 D180% at MNZ/Fe=0.05–0.2g/L where the optimum discoloration yielded 93 D180% at 0.2 g/L on MNZ 9 reaction. On the other hand, the discoloration diminished as the (MNZ/Fe) was increasing. The D180% decreases when using 0.35 g/L yielding 91. Consequently, the D180% was decreasing with values of 86, 79 and 29 D180% for catalyst dose of 0.5, 1, and 1.5 g/L, in that order. The low discoloration seemed to be attributed by the deactivation through shielding effect. It is caused by the MNZ opacity in solution where radiation and peroxide amount promoted a re-oxidation of Fe2+ ions [68].Figure 11
Catalyst dosage effect over RB5 dye discoloration at 180 min (D180%).Thekapp values from MNZ 6 to MNZ 13 reactions are reported in Table 7 where pseudo-first-order was assumed for the reaction kinetics. The MNZ 9 reaction has the highest kapp after 180 min of reaction (0.0225 min-1). The kinetic constant was evaluated at 50 and 30 min for MNZ 11 and MNZ 12 reactions, respectively. No apparent change in RB5 dye concentration was noted beyond these times.


## 4.3. pH Effect on the Solution

Heterogeneous materials have a high catalytic activity in Fenton process for dye degradation in a wide pH range [69]. Then, the pH dependence in RB5 dye discoloration was analyzed in the pH interval of 2.5–4.5 and keeping constant MNZ/Fe=0.2 g/L, H2O2=3g/L, and RB50=100mg/L.The discoloration percentage RB5 dye after 180 min of reaction (D180%) is observed in Figure 12 as a function of pH solution. A discoloration of 93 D180% was obtained at pH=2.5 and 91 D180% at pH=3. However, there was no dye discoloration when pH was increased between 3.5 and 4.5.Figure 12
pH effect on RB5 dye discoloration usingMNZ/Fe=0.2g/L as catalyst.


## 4.4. Influence of H2O2 Concentration

The analysis of H2O2 concentration in the solution was carried out by keeping constant the amount of catalyst MNZ/Fe=0.2g/L, initial dye concentration RB50=100mg/L, and a solution acidity pH=2.5. Results depicted in Figure 13 demonstrated that using H2O2=3g/L, the major discoloration yielded 93 D180% with a kapp=0.0225 min-1. Below and above this mentioned concentration, the discoloration seemed to be inhibited as reported by the decrease in the D180% and the kapp. The values were 91 D180% (kapp=0.0131 min-1), 91.2 D180% kapp=0.0153 min-1), and 91 D180% kapp=0.0151 min-1) for (H2O2) fixed at 2.0, 4.0, and 5.0 g/L, respectively. This was because increasing peroxide amount was likely to promote secondary reactions that consume H2O2 and therefore inhibit the RB5 degradation reaction.Figure 13
Effect of H2O2 concentration on RB5 dye degradation using MNZ/Fe=0.2g/L as catalyst.


## 4.5. Initial Concentration of RB5 Dye (RB5)0

The initial concentration of RB5 dye was also studied by keeping constant the amount ofH2O2=3g/L, pH=2.5, and catalyst MNZ/Fe=0.2 g/L. Results are shown in Figure 14. In general, the great activity ocurred in the first reaction minutes. The major discoloration was obtained using RB50=100mg/L on the MNZ 9 reaction with 89 D100% at 100 min; later, the reaction tended to be slow since at 180 min reached 93 D180%. For RB50=80mg/L, the discoloration was gradual but with a slower reaction rate than the reported one by 100 mg/L. 61 D100% was obtained and subsequently the reaction slowed down reaching 72 D180% with a kapp=0.0139min-1 (R2=0.96) at RB50=80mg/L. In addition, a similar behavior like using 80 mg/L was exhibited when the initial concentration of RB5 was reduced to 60 and 40 mg/L. Discoloration yielded 40 D100% and 51 D180% with a kapp=0.0113 min-1 (R2=0.95) for RB50=60mg/L. Subsequently, if RB50=40 mg/L were used, 26 D100% and 34 D180% kapp=0.0113min-1 (R2=0.95) were obtained. The difference observed in Dt% was because on the (RB5)0 decreased, and thus it made it difficult to achieve a suitable interaction between the OH⋅ radicals and the compounds to be removed.Figure 14
Effect of initial concentration of (RB5)0 using MNZ/Fe=0.2 g/L as catalyst.


## 4.6. COD Removal

The removal ofRB50=100 mg/L using different concentrations of MNZ/Fe was determined at pH=2.5, H2O2=3 g/L, and light radiation (405 nm) for measuring chemical oxygen demand (COD) removal. The COD removal percentage after 180 min of reaction (COD180%) is observed in Figure 15.Figure 15
COD removal of RB5 dye.It was determined by equation (14):
(14)CODt%=COD0−CODtCOD0×100The subscripts 0 andt denote the COD removal at initial and fixed time, respectively. The great COD removal was observed at concentrations of 0.05, 0.1, and 0.15 g/L (MNZ/Fe) with degradations of 68.5, 67.7, and 68.5 COD180%, in that order. The highest removal (70.5 COD180%) was achieved with MNZ/Fe=0.2 g/L. The efficiency of the reaction was reduced when the catalyst concentration was increased to 0.35, 0.5, 1, and 1.5 g/L with corresponding removals of 62.8, 61.4, 50, and 30 COD180%. This behavior was probably attributed to an increase on the catalyst amount that inhibited the reaction and the absence of active sites. Moreover, the opacity of the MNZ/Fe probably interfered with the reaction causing a shielding effect and therefore low interaction between the OH⋅ ions and the RB5 dye [68].


## 5. Conclusions

The Mexican natural zeolite (MNZ) studied in this research was constituted by heulandite, mordenite, erionite, and cristobalite phases, so the mineral was a mixture of crystalline aluminosilicates. The Fe composition on the MNZ surface as oxides and oxyhydroxides in the form of magnetite (Fe3+ and Fe2+) was 3.9, 6 y 6.2 w% for samples uncalcined (25°C) and calcined at 550 and 700°C, respectively. Fe particles supported on the surface had sizes from 3.89 to 19.6 nm.91 D180% of discoloration was obtained for the 10 mg MNZ/Fe and calcined at 700°C. The reaction kinetics was assumed as pseudo-first order (n=1). Besides, the D180% decreased with catalyst dose increments, so that when using MNZ/Fe=0.2 g/L the best discoloration (93 D180%) was obtained. This photo-Fenton process had a positive effect on the RB5 discoloration at acidic conditions (pH=2.5 and 3), achieving 93 D180% (pH=2.5). On the contrary, the reaction was inhibited at 3.5 and 4.5. Likewise, the amount of H2O2 and the initial concentration of RB5 dye were analyzed. The discoloration was more efficient with H2O2=3g/L. The reactions were slow after 120 min but the highest activity was achieved using RB50=100mg/L. After 120 min, the (RB5)0 did not represent an important variable, since there was no difference in the D180%.Finally, the highest COD removal was achieved at 180 minutes of reaction (70.5 COD180%) using MNZ/Fe=0.2 g/L. When the catalyst dose in aqueous solution increased to 1.5 g/L, the COD180% was 30. This could be assumed that shielding effects or side reactions that consumed H2O2 were promoted, and hence the reaction efficiency decreased.



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