# Photodegradation of Methyl Green by Nickel-Dimethylglyoxime/ZSM-5 Zeolite as a Heterogeneous Catalyst

Authors: Alireza Nezamzadeh-Ejhieh; Zahra Shams-Ghahfarokhi
Journal: Journal of Chemistry
 (2013)

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## Abstract

Ni-DMG/ZSM-5 zeolite was prepared by ion exchange and complexation procedures. FT-IR, XRD, SEM, TG, and DTG methods were used for characterization of the raw and modified samples. The prepared composite was used as a catalyst in the photodegradation process of an aqueous solution methyl green (MG) dye under UV irradiation. The effect of key operating parameters such as catalyst dosage, temperature, the initial concentration of the dye, and pH of the samples was studied on the degradation extent of the dye. UV-Vis spectrophotometric measurements were performed for determination of the decolorization and mineralization extents. The optimal operation parameters were found as follows:pH=9, temperature of 60°C, 0.6 g L−1 of the catalyst, and 40 ppm of the dye concentration. The Ni-DMG particles out of zeolite framework did not show significant degradation efficiency. The degradation process obeys the first-order kinetic.


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## Body

## 1. Introduction

The amounts of several pollutants present in the surface and underground waters have increased in the last years. Industrial processes generate a variety of molecules that may pollute waters due to negative impacts for ecosystems and humans (toxicity, carcinogenic, and mutagenic properties). Organic dyes are one of the largest group of pollutants released into waste waters from textile and other industrial processes [1, 2]. Colorants are widely used in different branches of industry, that is, textile, painting, leather, printing, photography, and so forth. Dyes in waste water create aesthetic problems, limit the possible use of the water, and reduce the efficacy of microbial waste water treatment because they may be toxic to microorganisms. Dyes absorb and scatter sunlight which is essential for algae growth [3].Triphenylmethane dyes are one of the most common organic water pollutants and they are used extensively in the textile industry for dyeing nylon, wool, cotton, and silk, as well as for coloring of oil, fats, waxes, varnish, and plastics. The paper, leather, cosmetic, and food industries consume a high quantity of triphenylmethane dyes of various kinds. Cationic triphenylmethane dyes have found widespread use as colorants in industry and as antimicrobial agents. Methyl green (MG) is a basic triphenylmethane-type dicationic dye, usually used for staining solutions in medicine and biology and as a photochromophore to sensitize gelatinous films [4]. Cationic (basic) dyes have been used for paper, polyacrylonitrile, modified polyesters, polyethylene terephthalate, and, to some extent, in medicine. Originally they were used for silk, wool, and tannin-mordanted cotton. These water-soluble dyes yield colored cations in solution and that is why they are called cationic dyes [5]. Because of potential toxicity of dyes and their visibility in surface waters, removal and degradation of organic dyes have been a matter of considerable interest [2]. Traditional physical techniques (coagulation, adsorption on activated carbon, reverse osmosis, etc.) can generally be used for removal of such pollutants. Nevertheless, these methods are usually nondestructive, and the posttreatment of the adsorbent materials or solid wastes is necessary and expensive [6].A relatively newer, more powerful and very promising approach called advanced oxidation processes (AOPs) has been developed and employed to treat dye-contaminated waste water effluents [7]. AOPs are a set of techniques which normally utilize a strong oxidizing species such as ∙OH radicals produced in situ which causes a sequence of reactions thereafter to break down the macromolecule into smaller and less harmful substances. In many cases, the macromolecule is completely broken down to water and carbon dioxide [8]. AOPs include also many techniques, such as methods based on ultrasound [9], plasma [10], and electrohydraulic discharge [11] along with processes based on hydrogen peroxide (H2O2 + UV, Fenton, photo-Fenton, and Fenton-like processes), photolysis, processes based on ozone (O3, O3 + UV and O3 + catalyst) [12], photocatalysis by semiconductors (TiO2/UV) [13, 14], and photoredox reactions of transition metal complexes [15]. Some of the oxides like TiO2 showed outstanding activities [16, 17]. However, the liw surface area, limited thermal stability, and unsuitable mechanical properties prevented their commercial exploitation [18]. In this paper, degradation of methyl green using photoredox reactions of transition metal complexes is investigated.Transition metal complexes play a special role in the environmental processes. Their easiness in change of the oxidation state makes the transition metal ions responsible for most redox processes occurring in nature directly or via a catalytic mechanism. Due to presence of unpaired electrons the metal ions react readily with molecular oxygen, mediating thereby oxygenation of other compounds, especially those constituting the natural organic matter [15].Nickel(ΙΙ) dimethylglyoxime complex (Ni-DMG) is considered on attractive approach for the degradation of methyl green (MG). To increase the activity of semiconductors in photodegradation experiments, suitable supports have been used to improve the efficiency of the photocatalytic process. Among the supports, zeolites have more advantageous owing to their special features such as high surface area, hydrophobic and hydrophilic properties, tunable chemical properties, high thermal stability, and eco-friendly nature [19].  Yan et al. inferred that Al–O units in framework of the zeolite were the photocatalytic active sites [20].  Zeolites modified with transition metal cations have received increasing attention as promising catalysts for a variety of important reactions [21]. Zeolites can serve as hosts to activate transition metal cations, offering a unique ligand system with multiple types of coordination for cations. In addition, the restricted pore size of zeolites could limit the growth or sintering of the nanoparticles of the cation even at high temperatures [22]. ZSM-5 zeolite, with highly ordered micropores, surface acidity, and ion-exchange properties, is one of the most widely applied inorganic materials as catalysts support, adsorbents, and molecular-sized spaces for various chemical or photochemical reactions [23].In the present study, ZSM-5 zeolite was synthesized and characterized with FT-IR, XRD, SEM, TG, and DTG methods. ZSM-5 zeolite was exchanged with Ni(ΙΙ) solution and then nickel (ΙΙ) dimethylglyoxime/ZSM-5 photocatalyst was prepared. The activity of the Ni-DMG/ZSM-5 photocatalyst was evaluated by studying the photocatalytic decolorization of methyl green. The effect of catalyst dosage, methyl green concentration, pH, and temperature was studied on the photodecolorization extent under UV irradiation and corresponding dark controls were also carried out for comparison. Finally, the relative photonic efficiency of Ni-DMG supported catalyst and pure Ni-DMG was compared.


## 2. Experimental

### 2.1.  Materials

MG dye (molecular formula: C27H35Cl2N3), dimethylglyoxime (DMG, C4H8N2O2), sodium silicate (composition: SiO2; (25.2%–28.5%), Na2O (7.5%–8.5%), H2O (63%)), nickel nitrate hexahydrate, hydrochloric acid (37%), tetrapropylammonium bromide (TPABr 98%), aluminum sulfate eighteen hydrate (>99.3%), and other used chemicals were supplied from Merck. The chemical structure of the MG dye is displayed in Figure 1 [4]. Deionized water was used throughout the experiments.Figure 1
Chemical structure of MG.


### 2.2. Synthesis of ZSM-5 Zeolite

2.4984 g (42.7 mmol) sodium chloride and 0.5931 g (0.89 mmol) hydrated aluminum sulfate were dissolved in 10.1200 g (562.2 mmol) distilled water. 1.8945 g (7.12 mmol) tetrapropylammonium bromide, 7.1200 g (395.5 mmol) distilled water, and 1.0883 g (10.88 mmol) sulfuric acid were added with vigorous stirring. 15.0000 g (71.25 mmol SiO2) sodium silicate solution was subsequently added and the mixture was stirred for 60 min. The pH of the mixture was 9.4. The mixture was transferred into the autoclave. The autoclave was kept into an oven at 110°C for about 2 h. Then, the temperature was increased to 230°C and kept at that level for another 5 h. The solid phase obtained was filtered out, washed with water several times, dried at 110°C for about 12–14 h, and subsequently calcined at 540°C for 3 h [24].


### 2.3. Preparation of Catalysts

Ni-ZSM-5 sample was prepared using the conventional ion exchange procedure [25]. 1 g Na-ZSM-5 was added to 50 mL of 0.1 M Ni(NO3)2·6H2O solution with constant stirring at room temperature. After 12 h, the particles were filtered off and washed with deionized water till complete removal of Ni2+ ions. The obtained sample was first dried at 120°C for 12 h and calcined at 500°C for 6 h. The obtained material has a light green color.About 1 g of dried nickel exchanged zeolite was slowly added into the 25 mL DMG (1% in ethanol) and stirred for 24 h. The resulting bright red color material was filtered, washed with excess water, and dried at room temperature. The obtained sample was Ni-DMG/ZSM-5. In a typical preparation of Ni-DMG, 1 g Ni(NO3)2·6H2O was added to a 25 mL of DMG solution, followed by stirring for 30 min. The mixed solution was centrifuged, and the precipitate was washed for several times with distilled water and dried at room temperature. Finally, the red Ni-DMG powder was obtained.


### 2.4. Catalyst Characterization

Fourier transform infrared (FT-IR) spectra of all samples were taken in KBr pellets in the 4000–400 cm−1 region using Nicolet 400D-Impact FT-IR spectrophotometer. Powder X-ray diffraction (XRD) pattern for the ZSM-5 zeolite was carried out using Bruker D8-ADVANCE equipment with an X-ray source of CuKα radiation. Thermograms were performed for the samples (6 mg) using model Setaram STA units in the range of 50–800°C with temperature rise of 10°C min−1. The morphology and crystal size of the samples were visualized by scanning electron microscopy (CAM SCAN 44, Cambridge). The amount of Ni present in the Ni-ZSM-5 and Ni-DMG/ZSM-5 was measured by Atomic absorption spectrometry (AAS) using an atomic absorption spectrometer (Perkin-Elmer 300 Analyst). The MG content of solutions was analyzed using UV-Vis spectrophotometer (Cary 100, Varian, Australia).


### 2.5. Photocatalytic Decolorization Procedure

Photocatalytic decolorization of MG was performed in 40 mL aqueous solution containing 20 ppm MG. A constant weight of 0.6 g L−1 of Ni-DMG/ZSM-5 was added into the solution. The bench-scale system is a cylindrical Pyrex-glass cell with 5 cm inside diameter and 10 cm height. Irradiation experiments were performed using medium pressure Hg lamp (55 W, 332 nm), then it was placed in a 5 cm diameter quartz tube with one end tightly sealed by a Teflon stopper. The lamp and the tube were then immersed in the photoreactor cell with a light path of 30 cm. A magnetic stirrer was continuously working at the bottom of the reaction solution. The experiment was performed at room temperature. After irradiation, the sample was centrifuged to remove the solid catalyst. The MG content was analyzed quantitatively by measuring the absorption band at 632 nm using UV-Vis spectrophotometer. This experiment was carried out by Ni-DMG compound too. The elimination of MG due to adsorption was measured by carrying out similar experiments in dark. The decolorization of MG by Ni-DMG/ZSM-5 catalyst was studied under different initial dye concentrations (10–100 ppm), initial solution pHs (1.0–9.0), solution temperature (25–60°C), and catalyst dosage (0.2–1.0 g L−1) to optimize the reaction conditions. Each experiment was conducted in duplicate.The reaction order with respect to Mg was determined by plotting reaction time versuslog[MG] according to the following equation:
(1)log[C]t=-kt+log[C]0,
where [C]0  and [C]t represent the concentration of the substrate in solution at zero time and t time of irradiation, respectively, and k represents the apparent rate constant (min−1) [16].


## 2.1.  Materials

MG dye (molecular formula: C27H35Cl2N3), dimethylglyoxime (DMG, C4H8N2O2), sodium silicate (composition: SiO2; (25.2%–28.5%), Na2O (7.5%–8.5%), H2O (63%)), nickel nitrate hexahydrate, hydrochloric acid (37%), tetrapropylammonium bromide (TPABr 98%), aluminum sulfate eighteen hydrate (>99.3%), and other used chemicals were supplied from Merck. The chemical structure of the MG dye is displayed in Figure 1 [4]. Deionized water was used throughout the experiments.Figure 1
Chemical structure of MG.


## 2.2. Synthesis of ZSM-5 Zeolite

2.4984 g (42.7 mmol) sodium chloride and 0.5931 g (0.89 mmol) hydrated aluminum sulfate were dissolved in 10.1200 g (562.2 mmol) distilled water. 1.8945 g (7.12 mmol) tetrapropylammonium bromide, 7.1200 g (395.5 mmol) distilled water, and 1.0883 g (10.88 mmol) sulfuric acid were added with vigorous stirring. 15.0000 g (71.25 mmol SiO2) sodium silicate solution was subsequently added and the mixture was stirred for 60 min. The pH of the mixture was 9.4. The mixture was transferred into the autoclave. The autoclave was kept into an oven at 110°C for about 2 h. Then, the temperature was increased to 230°C and kept at that level for another 5 h. The solid phase obtained was filtered out, washed with water several times, dried at 110°C for about 12–14 h, and subsequently calcined at 540°C for 3 h [24].


## 2.3. Preparation of Catalysts

Ni-ZSM-5 sample was prepared using the conventional ion exchange procedure [25]. 1 g Na-ZSM-5 was added to 50 mL of 0.1 M Ni(NO3)2·6H2O solution with constant stirring at room temperature. After 12 h, the particles were filtered off and washed with deionized water till complete removal of Ni2+ ions. The obtained sample was first dried at 120°C for 12 h and calcined at 500°C for 6 h. The obtained material has a light green color.About 1 g of dried nickel exchanged zeolite was slowly added into the 25 mL DMG (1% in ethanol) and stirred for 24 h. The resulting bright red color material was filtered, washed with excess water, and dried at room temperature. The obtained sample was Ni-DMG/ZSM-5. In a typical preparation of Ni-DMG, 1 g Ni(NO3)2·6H2O was added to a 25 mL of DMG solution, followed by stirring for 30 min. The mixed solution was centrifuged, and the precipitate was washed for several times with distilled water and dried at room temperature. Finally, the red Ni-DMG powder was obtained.


## 2.4. Catalyst Characterization

Fourier transform infrared (FT-IR) spectra of all samples were taken in KBr pellets in the 4000–400 cm−1 region using Nicolet 400D-Impact FT-IR spectrophotometer. Powder X-ray diffraction (XRD) pattern for the ZSM-5 zeolite was carried out using Bruker D8-ADVANCE equipment with an X-ray source of CuKα radiation. Thermograms were performed for the samples (6 mg) using model Setaram STA units in the range of 50–800°C with temperature rise of 10°C min−1. The morphology and crystal size of the samples were visualized by scanning electron microscopy (CAM SCAN 44, Cambridge). The amount of Ni present in the Ni-ZSM-5 and Ni-DMG/ZSM-5 was measured by Atomic absorption spectrometry (AAS) using an atomic absorption spectrometer (Perkin-Elmer 300 Analyst). The MG content of solutions was analyzed using UV-Vis spectrophotometer (Cary 100, Varian, Australia).


## 2.5. Photocatalytic Decolorization Procedure

Photocatalytic decolorization of MG was performed in 40 mL aqueous solution containing 20 ppm MG. A constant weight of 0.6 g L−1 of Ni-DMG/ZSM-5 was added into the solution. The bench-scale system is a cylindrical Pyrex-glass cell with 5 cm inside diameter and 10 cm height. Irradiation experiments were performed using medium pressure Hg lamp (55 W, 332 nm), then it was placed in a 5 cm diameter quartz tube with one end tightly sealed by a Teflon stopper. The lamp and the tube were then immersed in the photoreactor cell with a light path of 30 cm. A magnetic stirrer was continuously working at the bottom of the reaction solution. The experiment was performed at room temperature. After irradiation, the sample was centrifuged to remove the solid catalyst. The MG content was analyzed quantitatively by measuring the absorption band at 632 nm using UV-Vis spectrophotometer. This experiment was carried out by Ni-DMG compound too. The elimination of MG due to adsorption was measured by carrying out similar experiments in dark. The decolorization of MG by Ni-DMG/ZSM-5 catalyst was studied under different initial dye concentrations (10–100 ppm), initial solution pHs (1.0–9.0), solution temperature (25–60°C), and catalyst dosage (0.2–1.0 g L−1) to optimize the reaction conditions. Each experiment was conducted in duplicate.The reaction order with respect to Mg was determined by plotting reaction time versuslog[MG] according to the following equation:
(1)log[C]t=-kt+log[C]0,
where [C]0  and [C]t represent the concentration of the substrate in solution at zero time and t time of irradiation, respectively, and k represents the apparent rate constant (min−1) [16].


## 3. Results and Discussion

### 3.1. Catalyst Characterization

#### 3.1.1. X-Ray Diffraction Studies

The X-ray diffraction patterns of ZSM-5 zeolite, Ni-ZSM-5, and Ni-DMG/ZSM-5 are shown in Figure2. The characteristic lines where located at 2θ degree of 8, 9, 23, and 24 (Figure 2(a)) have good agreement with the data of reference Na-ZSM-5 [26]. The presence of the weak peaks in 2θ value of 10° and 27.4° in the Ni-ZSM-5 and Ni-DMG/ZSM-5 patterns (Figure 2(b), (c)), that are not present in the pattern of ZSM-5 (Figure 2(a)), indicate the incorporation of Ni2+ in the zeolite structure. The powder XRD results of ZSM-5 and the host-guest composite materials (Ni-ZSM-5 and Ni-DMG/ZSM-5) show similar diffraction peaks indicative of ZSM-5. But some differences such as increasing or decreasing of some peaks intensity can be observed in the spectra [27]. In fact it can be related to the presence or incorporation of Ni2+ in the matrix structure. Using Sherrer equation [28], crystal sizes of the ZSM-5, Ni-ZSM-5, and Ni-DMG/ZSM-5 were measured by XRD as: 3.6, 3.5 and 3.4 μm, respectively.Figure 2
XRD patterns of Na-ZSM-5 (a), Ni-ZSM-5 (b), and Ni-DMG/ZSM-5 (c).


#### 3.1.2. FT-IR Studies

FT-IR lattice vibration spectra were used to investigate the influence of nickel and Ni-DMG on the zeolite framework. The FT-IR transmission spectra for ZSM-5 zeolite, Ni-ZSM-5, Ni-DMG/ZSM-5, and Ni-DMG are shown in Figure3. From Figure 3(a), the infrared absorption peaks of ZSM-5 appeared at 446, 547, 786, 1077, 1230, 1483, 1637, and 3319 cm−1. The presence of the infrared band at 547 cm−1 has been assigned to the five-membered ring of the pentasil zeolite structure. Additional evidence for ZSM-5 is the asymmetric stretch vibration of the T–O band at 1230 cm−1 (where T is Si or Al), which has been assigned to external linkages (between TO4 tetrahedral) and is a structure-sensitive IR band of ZSM-5 [26, 29, 30].Figure 3
FTIR spectra of Na-ZSM-5 (a), Ni-ZSM-5 (b), and Ni-DMG/ZSM-5 (c).Infrared spectroscopy can reflect the change of the framework configuration of the zeolite host after the incorporation of the guests. In Figure3(b), the FT-IR spectrum of Ni-ZSM-5 shows a distortion of the spectrum between 1250 and 900 cm−1. This region of the spectrum was assigned to asymmetrical T–O–T stretching and is indicative of heteroatom substitution [31]. Changes of the characteristic peaks took place between the host zeolite ZSM-5 (the values in the parentheses) and the host-guest materials Ni-ZSM-5 and Ni-DMG/ZSM-5. For Ni-ZSM-5, the characteristic bands are seen at 456 (446) cm−1, 556 (547) cm−1 (T–O bend), 791 (786) cm−1 (symmetrical stretch), 1080 (1082)cm−1 (asymmetrical stretch), and 1235 (1260) cm−1 that show a shift of some bands as compared with the bands of ZSM-5 host (Figures 3(a) and 3(b)). These results confirm the incorporation of Ni2+ cations into zeolite channels. Furthermore, the presence of the peaks at 2410 and 2960 cm−1 in the Ni-ZSM-5 and Ni-DMG/ZSM-5 spectra, which are not present in the spectrum of ZSM-5, indicates the incorporation of Ni2+ into zeolite. In addition, the greenish blue color after ion exchange with Ni2+ cations can be considered as a primary evidence for incorporation of Ni2+ into zeolite framework.Similar results will be shown for Ni-DMG/ZSM-5 at 467, 568, 805, 1090, and 1290 cm−1 (Figure 3(c)). Comparison of the spectra of (b) and (c) in Figure 3 show the changes due to conversion of Ni2+ ions that is present in zeolite to Ni-DMG. These results demonstrated that the guest Ni-DMG incorporated into the ZSM-5 zeolite had some interactions with the inner surfaces of zeolite host at the same time. The greenish blue color of the Ni-ZSM-5 changes to bright red after precipitation with DMG which confirms conversion of Ni2+ to Ni-DMG in the zeolite.Generally, acidity of the framework increases with increasing the M2+ substitution, but there was no obvious trend in the absorption bands assigned to terminal hydroxyl groups (3734 cm−1), or to the absorption bands assigned to bridging hydroxyl groups associated with a Bronsted site (3650–3600 cm−1) [32].


#### 3.1.3. Thermal Analysis

The TG and DTG curves of ZSM-5, Ni-ZSM-5, and Ni-DMG/ZSM-5 are shown in Figure4. The TG results for ZSM-5 zeolite are similar to the literature [33]. The peak at 200°C (Figure 4(c)) may be related to lose of excess of DMG that remained due to incomplete washing of the zeolite after complexation process. The increase in weight below 350°C is a result of oxygen adsorption.Figure 4
Thermal analysis curves spectra of Na-ZSM-5 (a), Ni-ZSM-5 (b), and Ni-DMG/ZSM-5 (c).


#### 3.1.4. SEM Analysis

The surface morphology of ZSM-5 zeolite ((a), (b)) Ni-ZSM-5 ((c), (d)) and Ni-DMG/ZSM-5 ((e), (f)) was studied by scanning electron microscope and the SEM pictures are presented in Figure5. The images of loaded samples (Ni-ZSM-5 and Ni-DMG/ZSM-5) show that crystallinity is not affected by the Ni2+ loading. But it seems that particles break to pieces with loading Ni2+ in the zeolite. Increasing activity of loaded samples may be related to dwindling in size of particles.SEM images of Na-ZSM-5 ((a), (b)); Ni-ZSM-5 ((c), (d)) and Ni-DMG/ZSM-5 ((e), (f)).
(a)
(b)
(c)
(d)
(e)
(f)


### 3.2. Photocatalytic Decolorization of MG by Ni-DMG/ZSM-5

#### 3.2.1. Effect of Catalyst Concentration

The initial rate of the photocatalytic degradation of many pollutants is a function of the photocatalyst dosage [15, 34]. A series of experiments was carried out to assess the optimum catalyst loading by varying the amount of the catalyst from 0.2 to 1.0 g L−1 with MG concentration (20 ppm). The results depicted in Figure 6 show that the degradation rate increases with increasing the mass of the catalyst, reached the highest value (0.6 g L−1 of the catalyst) and then decreased considerably. The reason for this decrease is thought to be the fact that when the concentration of the catalyst rises, the solid particles increasingly block the penetration of the photons. So the overall number of the photons that can be reached to catalyst particles and hence the production of OH radicals decrease [35]. Another reason may be due to the aggregation of solid particles while using a large amount of catalyst [4, 36]. Also, Figure 6 shows that the removal rates were negligible in the absence of catalyst or dark condition after 3 h control.Figure 6
Effect of Ni-DMG/ZSM-5 dosage on the decolorization efficiency of MG dye; initial dye concentration, 20 ppm; initial pH, 5.3; photocatalyst dosage, (0.2, 0.4, 0.6 and 0.8 g L−1); 55 W Hg lamp; continuous stirring; irradiation time, 180 min; room temperature.Many authors have reported that the kinetic behavior of the photocatalytic reactions obeys the first-order reaction [35, 36]. In order to confirm the speculation, ln(C/C0) was plotted as a function of the irradiation time. The calculated results indicated that the first-order model gives a better fit. The rate constant values, k (min−1), are calculated from the straight-line segment of the first-order plots as a function of the catalyst mass and are listed in Table 1. As the results show, maximum degradation (76.5%) of MG. dye was observed after 120 min with the maximum rate constant (3.6 × 10−2 min−1) in the presence of 0.6 g L−1 of the catalyst. Methyl green alone could not be transformed under UV irradiation, corresponding to the rate constant (k) of 3.0 × 10−5 min−1. In the following experiments, we chose 0.6 g L−1 of Ni-DMG/ZSM-5 as the optimum dosage.Table 1
Rate constant values as a function of various experimental parameters.
Parameter
Value
k × 100 (min−1)
Catalyst amount (g L−1)
0
0.003
0.2
0.9
0.4
1.9
0.6
3.6
0.8
1.7
1.0
0.46
1
0
3
1.1
pH
5
4.6
7
5.2
9
6.1
25
1.8
40
2.4
Temperature (°C)
50
2.7
60
3.5
80
4.3
C
MG (ppm)
10
0.10
20
0.46
40
2.11
60
0.6
80
0.44
100
0.29


#### 3.2.2. Effect of pH

The waste water from the textile industries usually has a wide range of pH values. Generally pH plays an important role both in the characteristics of textile wastes and generation of active sites [37]. Hence, the role of pH on the degradation extent of MG was studied in the pH range of 1–9 in 20 ppm MG concentration containing 0.6 g L−1 of the catalyst. At pHs above 9, the solution was colorless and the λmax of the MG was shifted to UV region (before 250 nm) and hence a decrease in the absorbance of the solution during the degradation process was not distinguishable. Hence, the corresponding results was not measured. The solution of pH was adjusted only prior to irradiation and was not controled during the reaction. As shown in Figure 7, the percentage of decolorization increased with increasing pH. As mentioned in the literature [35], in the initial acidic pHs, concomitant with acidification of the solution by HCl, a high amount of conjugated base is added to the solution. The anion Cl- is able to react with hydroxyl radicals leading to inorganic radical ions (ClO-∙). These inorganic radical anions show a much lower reactivity than ∙OH, so that they do not take part in the dye decolorization. There is also a drastic competition between the dye and anions with respect to ∙OH. Hence, increasing pH shows an increase in the degradation efficiency. Alkaline pHs favor the formation of more OH radicals due to the presence of large quantity of OH- anions in the alkaline medium, which enhances the photocatalytic degradation of MG significantly [25]. In acidic solutions a decrease in the decolorization rate was observed reflecting the difficulty of the dye molecules to approach the catalyst surface due to electrostatic interactions. In other words, at low pH, the adsorption of cationic dye on the surface of the photocatalyst was decreased because the photocatalyst surface will be positively charged and repulsive force is due to decreasing adsorption [34].Figure 7
Effect of solution pH on the MG dye decolorization; 0.6 g L−1 of the catalyst; initial dye concentration, 20 ppm; 55 W Hg lamp; continuous stirring; irradiation time, 180 min; room temperature.Table1 shows the dependence of k on pH. As can be seen, the observed degradation is strongly dependent on pH, occurring efficiently at pH 9. However, we have carried out all the experiments in natural pH (5.3) conditions.At the end of the studies on pH effect, the leached nickel cations were followed by atomic spectroscopy. The results showed that the leached nickel cations increase with decreasing pH, so its extent was significantly increased from pH 3 to 1. But, the leached nickel was not sufficient to determine its value quantitatively and it was only followed qualitatively. This indicates that the Ni-DMG is very stable in the zeolite bed and the leached nickel does not contaminate the solution.


#### 3.2.3. Effect of Temperature

Since the photonic activation occurs at considerably high speeds, it is expected that the photocatalytic system is not sensible to the temperature, and the true activation energy most be then equal to zero. Although considering that the reactions under study occur preferentially in the liquid/solid interface, a nonzero value must be expected as apparent activation energy. It was observed that with increase in the temperature from 25 to 60°C (at a 20 ppm MG concentration containing 0.6 g L−1 catalyst), the percentage of decolorization increases (Figure 8). With increasing in temperature, the exothermic adsorption of the reactants becomes disfavored due to reducing the value of the apparent activation energy [38]. On the other hand, an increase in temperature decreases the solubility of oxygen in water which is not desirable. Higher temperatures will cause significant evaporation of the solution during the experiments. Thus, temperature higher than 80°C is not recommended. The rate constant values (k, min−1) as a function of temperature on the dye decolorization are presented in Table 1.Figure 8
Effect of the reaction temperature on decolorization efficiency; 0.6 g L−1 of catalyst; initial dye concentration, 20 ppm; initial solution pH; 55 W Hg lamp; continuous stirring; irradiation time, 180 min; room temperature.


#### 3.2.4. Effect of Methyl Green Concentration

The degradation efficiency also depends on the initial concentration of the substrate [3]. The MG decolorization was studied over the concentration covering the range from 10 to 100 ppm by maintaining the other parameters constant. The decolorization is the highest at 40 ppm and thereafter decreases (Figure 9). The life time of hydroxyl radicals is very short (only a few nanoseconds) and thus they can only react where they are formed. Increasing the quantity of MG molecules per volume unit logically enhances the probability of collision between organic matter and oxidizing species, leading to an increase in the decolorization efficiency. It is seen that the decolorization efficiency of dye was decreased with increasing the initial concentration to more than 40 ppm. The decrease of the degradation percent with increasing of dye concentration can be due to two reasons. With increasing the amounts of dye, the more of dye molecules will be adsorbed on the surface of the photocatalyst particles and the active sites of the catalyst will be reduced. Therefore, with increasing occupied space of catalyst surface, the generation of hydroxyl radicals will be decreased. Also, increasing the concentration of dye can lead to decreasing the number of photons that is arrived to the surface of catalyst particles. More light is absorbed by molecules of dye and the excitation of photocatalyst particles by photons will be reduced. These results are in good accordance with the literature [34, 37, 39, 40]. This is also simplified in Table 1 where the degradation rate constant (k, min−1) is listed as a function of initial concentration of the dye. It is apparent that the rate of degradation is a quantitative of concentration dependent and the activity was increased with increasing concentration to 40 ppm.Figure 9
Effect of the initial dye concentration on decolorization efficiency of MG; 0.6 g L−1 of catalyst; initial solution pH, 5.3; 55 W Hg lamp; continuous stirring; irradiation time, 180 min; room temperature.


#### 3.2.5. Comparison of MG Degradation over Ni-DMG/ZSM-5 and Ni-DMG

The amount of Ni loaded in zeolite was measured by atomic absorption spectroscopy and to be 0.0343 mmol per gram of Ni-DMG/ZSM-5. To determine whether the degradation of MG by Ni-DMG takes place or not, the catalytic activity of 0.02 g L−1 Ni-DMG was measured under the same above-mentioned experimental conditions. No remarkable activity was noticed due to the presence of Ni-DMG as shown in Table 2. It can be concluded that the degradation process occurs insignificantly in the presence of Ni-DMG. The role of the zeolite might be correlated with the adsorption process, in the sense of high surface area and the decrease of particle size [36]. This, in turn, causes an increase in the photodegradation efficiency. Another reason can be related to hydrophobicity properties of the support that is the major factor for the high degradation. The high hydrophobicity of ZSM-5 can be assigned to the influence of the hydrophobic character of structure directing agent for the synthesis of ZSM-5 (e.g., tetrapropylammonium cations) [41]. Hydrophobicity of ZSM-5 increases the adsorption of hydrophobic MG. Highly siliceous ZSM-5 zeolites with low Al2O3 content are known to have highly hydrophobic surfaces [23]. This observation clearly establishes the importance of support on the activity of degradation of MG.Table 2
Comparison of the photocatalytic activity of supported and unsupported catalysts.
Time (min)
Degradation (%)
Ni-DMG/ZSM-5
Ni-DMG
30
14.2
8
60
38
18.6
90
64
19.1
120
73
22.2


#### 3.2.6. Catalyst Life

The catalyst stability is a factor that needs to be addressed. After several times of use, the catalyst may be partially desorbed into the solution or decomposed into some fragments. Secondly, the catalyst ability may be deactivated by the reaction intermediates or products formed during the dye degradation [42]. Hence, the reusability of Ni-DMG/ZSM-5 catalyst in the degradation of MG was evaluated. The recycling experiments were performed with MG (40 ppm) and Ni-DMG/ZSM-5 (0.6 g L−1). After irradiation (1 h), Ni-DMG/ZSM-5 was recovered by filtration, calcined at 90°C, and tested again for its activity under identical experimental conditions. Ni-DMG/ZSM-5 exhibited almost the same catalytic activity for three cycles of operation. The experiments were repeated under the same conditions, but the temperature of calcination was 230°C. Table 3 summarizes the results of experiments. In all cases, the percentage of decolorization was decreased. Two factors are responsible for such a decrease. First, the catalyst concentration was gradually decreased, due to sample analysis [42]. Second, the Ni-DMG/ZSM-5 catalyst experienced a slow bleaching during the reaction process, as observed above in a homogeneous solution. As can be seen, the percentage of decolorization increases upon enhancing the calcinations temperature from 90 to 230°C. The Ni-DMG/ZSM-5 calcined at 230°C possesses comparatively higher specific surface area than the sample calcined at 90°C.Table 3
Reusability of Ni-DMG/ZSM-5 catalyst in the decolorization of MG.
Number of cycle
Degradation (%)
Calcination in 90°C
Calcination in 230°C
1
80.5
88.0
2
74.0
82.1
3
65.3
74.3The decrease in the activity of the used catalyst must reflect the presence of some adventitious degradation products adsorbed in the zeolite, causing the partial blockage of the pore system or covering the zeolite surface. Preliminary thermal reactivation trials at 230°C did lead to an appreciable degradation of Ni-DMG/ZSM-5 photocatalyst as evidenced visually by the color change. Our results show a good agreement with the literature [34].


#### 3.2.7. Comparing the Work with Other Works in MG Degradation

In previous work [39], MG was decolorized by Fe(II)-o-phenanthroline/zeolite Y nanocluster. Comparing the results shows that in this work a smaller weight of the NiDMG-ZSM-5 (0.6 g L−1) has been used (with respect to 1.0 g L−1 of Fe(II)-o-phenanthroline/zeolite Y nanocluster). This can be related to higher hydrophobicity of ZSM-5 with respect to zeolite Y to adsorb more MG molecules. Biodegradation of some triphenylmethane dyes has been studied [43], and this method has disadvantages with respect to heterogeneous photocatalysis as mentioned in Section 1. Photodegradation of methyl green were studied and the reaction pathway and identification of intermediates was studied by an HPLC [4].


## 3.1. Catalyst Characterization

### 3.1.1. X-Ray Diffraction Studies

The X-ray diffraction patterns of ZSM-5 zeolite, Ni-ZSM-5, and Ni-DMG/ZSM-5 are shown in Figure2. The characteristic lines where located at 2θ degree of 8, 9, 23, and 24 (Figure 2(a)) have good agreement with the data of reference Na-ZSM-5 [26]. The presence of the weak peaks in 2θ value of 10° and 27.4° in the Ni-ZSM-5 and Ni-DMG/ZSM-5 patterns (Figure 2(b), (c)), that are not present in the pattern of ZSM-5 (Figure 2(a)), indicate the incorporation of Ni2+ in the zeolite structure. The powder XRD results of ZSM-5 and the host-guest composite materials (Ni-ZSM-5 and Ni-DMG/ZSM-5) show similar diffraction peaks indicative of ZSM-5. But some differences such as increasing or decreasing of some peaks intensity can be observed in the spectra [27]. In fact it can be related to the presence or incorporation of Ni2+ in the matrix structure. Using Sherrer equation [28], crystal sizes of the ZSM-5, Ni-ZSM-5, and Ni-DMG/ZSM-5 were measured by XRD as: 3.6, 3.5 and 3.4 μm, respectively.Figure 2
XRD patterns of Na-ZSM-5 (a), Ni-ZSM-5 (b), and Ni-DMG/ZSM-5 (c).


### 3.1.2. FT-IR Studies

FT-IR lattice vibration spectra were used to investigate the influence of nickel and Ni-DMG on the zeolite framework. The FT-IR transmission spectra for ZSM-5 zeolite, Ni-ZSM-5, Ni-DMG/ZSM-5, and Ni-DMG are shown in Figure3. From Figure 3(a), the infrared absorption peaks of ZSM-5 appeared at 446, 547, 786, 1077, 1230, 1483, 1637, and 3319 cm−1. The presence of the infrared band at 547 cm−1 has been assigned to the five-membered ring of the pentasil zeolite structure. Additional evidence for ZSM-5 is the asymmetric stretch vibration of the T–O band at 1230 cm−1 (where T is Si or Al), which has been assigned to external linkages (between TO4 tetrahedral) and is a structure-sensitive IR band of ZSM-5 [26, 29, 30].Figure 3
FTIR spectra of Na-ZSM-5 (a), Ni-ZSM-5 (b), and Ni-DMG/ZSM-5 (c).Infrared spectroscopy can reflect the change of the framework configuration of the zeolite host after the incorporation of the guests. In Figure3(b), the FT-IR spectrum of Ni-ZSM-5 shows a distortion of the spectrum between 1250 and 900 cm−1. This region of the spectrum was assigned to asymmetrical T–O–T stretching and is indicative of heteroatom substitution [31]. Changes of the characteristic peaks took place between the host zeolite ZSM-5 (the values in the parentheses) and the host-guest materials Ni-ZSM-5 and Ni-DMG/ZSM-5. For Ni-ZSM-5, the characteristic bands are seen at 456 (446) cm−1, 556 (547) cm−1 (T–O bend), 791 (786) cm−1 (symmetrical stretch), 1080 (1082)cm−1 (asymmetrical stretch), and 1235 (1260) cm−1 that show a shift of some bands as compared with the bands of ZSM-5 host (Figures 3(a) and 3(b)). These results confirm the incorporation of Ni2+ cations into zeolite channels. Furthermore, the presence of the peaks at 2410 and 2960 cm−1 in the Ni-ZSM-5 and Ni-DMG/ZSM-5 spectra, which are not present in the spectrum of ZSM-5, indicates the incorporation of Ni2+ into zeolite. In addition, the greenish blue color after ion exchange with Ni2+ cations can be considered as a primary evidence for incorporation of Ni2+ into zeolite framework.Similar results will be shown for Ni-DMG/ZSM-5 at 467, 568, 805, 1090, and 1290 cm−1 (Figure 3(c)). Comparison of the spectra of (b) and (c) in Figure 3 show the changes due to conversion of Ni2+ ions that is present in zeolite to Ni-DMG. These results demonstrated that the guest Ni-DMG incorporated into the ZSM-5 zeolite had some interactions with the inner surfaces of zeolite host at the same time. The greenish blue color of the Ni-ZSM-5 changes to bright red after precipitation with DMG which confirms conversion of Ni2+ to Ni-DMG in the zeolite.Generally, acidity of the framework increases with increasing the M2+ substitution, but there was no obvious trend in the absorption bands assigned to terminal hydroxyl groups (3734 cm−1), or to the absorption bands assigned to bridging hydroxyl groups associated with a Bronsted site (3650–3600 cm−1) [32].


### 3.1.3. Thermal Analysis

The TG and DTG curves of ZSM-5, Ni-ZSM-5, and Ni-DMG/ZSM-5 are shown in Figure4. The TG results for ZSM-5 zeolite are similar to the literature [33]. The peak at 200°C (Figure 4(c)) may be related to lose of excess of DMG that remained due to incomplete washing of the zeolite after complexation process. The increase in weight below 350°C is a result of oxygen adsorption.Figure 4
Thermal analysis curves spectra of Na-ZSM-5 (a), Ni-ZSM-5 (b), and Ni-DMG/ZSM-5 (c).


### 3.1.4. SEM Analysis

The surface morphology of ZSM-5 zeolite ((a), (b)) Ni-ZSM-5 ((c), (d)) and Ni-DMG/ZSM-5 ((e), (f)) was studied by scanning electron microscope and the SEM pictures are presented in Figure5. The images of loaded samples (Ni-ZSM-5 and Ni-DMG/ZSM-5) show that crystallinity is not affected by the Ni2+ loading. But it seems that particles break to pieces with loading Ni2+ in the zeolite. Increasing activity of loaded samples may be related to dwindling in size of particles.SEM images of Na-ZSM-5 ((a), (b)); Ni-ZSM-5 ((c), (d)) and Ni-DMG/ZSM-5 ((e), (f)).
(a)
(b)
(c)
(d)
(e)
(f)


## 3.1.1. X-Ray Diffraction Studies

The X-ray diffraction patterns of ZSM-5 zeolite, Ni-ZSM-5, and Ni-DMG/ZSM-5 are shown in Figure2. The characteristic lines where located at 2θ degree of 8, 9, 23, and 24 (Figure 2(a)) have good agreement with the data of reference Na-ZSM-5 [26]. The presence of the weak peaks in 2θ value of 10° and 27.4° in the Ni-ZSM-5 and Ni-DMG/ZSM-5 patterns (Figure 2(b), (c)), that are not present in the pattern of ZSM-5 (Figure 2(a)), indicate the incorporation of Ni2+ in the zeolite structure. The powder XRD results of ZSM-5 and the host-guest composite materials (Ni-ZSM-5 and Ni-DMG/ZSM-5) show similar diffraction peaks indicative of ZSM-5. But some differences such as increasing or decreasing of some peaks intensity can be observed in the spectra [27]. In fact it can be related to the presence or incorporation of Ni2+ in the matrix structure. Using Sherrer equation [28], crystal sizes of the ZSM-5, Ni-ZSM-5, and Ni-DMG/ZSM-5 were measured by XRD as: 3.6, 3.5 and 3.4 μm, respectively.Figure 2
XRD patterns of Na-ZSM-5 (a), Ni-ZSM-5 (b), and Ni-DMG/ZSM-5 (c).


## 3.1.2. FT-IR Studies

FT-IR lattice vibration spectra were used to investigate the influence of nickel and Ni-DMG on the zeolite framework. The FT-IR transmission spectra for ZSM-5 zeolite, Ni-ZSM-5, Ni-DMG/ZSM-5, and Ni-DMG are shown in Figure3. From Figure 3(a), the infrared absorption peaks of ZSM-5 appeared at 446, 547, 786, 1077, 1230, 1483, 1637, and 3319 cm−1. The presence of the infrared band at 547 cm−1 has been assigned to the five-membered ring of the pentasil zeolite structure. Additional evidence for ZSM-5 is the asymmetric stretch vibration of the T–O band at 1230 cm−1 (where T is Si or Al), which has been assigned to external linkages (between TO4 tetrahedral) and is a structure-sensitive IR band of ZSM-5 [26, 29, 30].Figure 3
FTIR spectra of Na-ZSM-5 (a), Ni-ZSM-5 (b), and Ni-DMG/ZSM-5 (c).Infrared spectroscopy can reflect the change of the framework configuration of the zeolite host after the incorporation of the guests. In Figure3(b), the FT-IR spectrum of Ni-ZSM-5 shows a distortion of the spectrum between 1250 and 900 cm−1. This region of the spectrum was assigned to asymmetrical T–O–T stretching and is indicative of heteroatom substitution [31]. Changes of the characteristic peaks took place between the host zeolite ZSM-5 (the values in the parentheses) and the host-guest materials Ni-ZSM-5 and Ni-DMG/ZSM-5. For Ni-ZSM-5, the characteristic bands are seen at 456 (446) cm−1, 556 (547) cm−1 (T–O bend), 791 (786) cm−1 (symmetrical stretch), 1080 (1082)cm−1 (asymmetrical stretch), and 1235 (1260) cm−1 that show a shift of some bands as compared with the bands of ZSM-5 host (Figures 3(a) and 3(b)). These results confirm the incorporation of Ni2+ cations into zeolite channels. Furthermore, the presence of the peaks at 2410 and 2960 cm−1 in the Ni-ZSM-5 and Ni-DMG/ZSM-5 spectra, which are not present in the spectrum of ZSM-5, indicates the incorporation of Ni2+ into zeolite. In addition, the greenish blue color after ion exchange with Ni2+ cations can be considered as a primary evidence for incorporation of Ni2+ into zeolite framework.Similar results will be shown for Ni-DMG/ZSM-5 at 467, 568, 805, 1090, and 1290 cm−1 (Figure 3(c)). Comparison of the spectra of (b) and (c) in Figure 3 show the changes due to conversion of Ni2+ ions that is present in zeolite to Ni-DMG. These results demonstrated that the guest Ni-DMG incorporated into the ZSM-5 zeolite had some interactions with the inner surfaces of zeolite host at the same time. The greenish blue color of the Ni-ZSM-5 changes to bright red after precipitation with DMG which confirms conversion of Ni2+ to Ni-DMG in the zeolite.Generally, acidity of the framework increases with increasing the M2+ substitution, but there was no obvious trend in the absorption bands assigned to terminal hydroxyl groups (3734 cm−1), or to the absorption bands assigned to bridging hydroxyl groups associated with a Bronsted site (3650–3600 cm−1) [32].


## 3.1.3. Thermal Analysis

The TG and DTG curves of ZSM-5, Ni-ZSM-5, and Ni-DMG/ZSM-5 are shown in Figure4. The TG results for ZSM-5 zeolite are similar to the literature [33]. The peak at 200°C (Figure 4(c)) may be related to lose of excess of DMG that remained due to incomplete washing of the zeolite after complexation process. The increase in weight below 350°C is a result of oxygen adsorption.Figure 4
Thermal analysis curves spectra of Na-ZSM-5 (a), Ni-ZSM-5 (b), and Ni-DMG/ZSM-5 (c).


## 3.1.4. SEM Analysis

The surface morphology of ZSM-5 zeolite ((a), (b)) Ni-ZSM-5 ((c), (d)) and Ni-DMG/ZSM-5 ((e), (f)) was studied by scanning electron microscope and the SEM pictures are presented in Figure5. The images of loaded samples (Ni-ZSM-5 and Ni-DMG/ZSM-5) show that crystallinity is not affected by the Ni2+ loading. But it seems that particles break to pieces with loading Ni2+ in the zeolite. Increasing activity of loaded samples may be related to dwindling in size of particles.SEM images of Na-ZSM-5 ((a), (b)); Ni-ZSM-5 ((c), (d)) and Ni-DMG/ZSM-5 ((e), (f)).
(a)
(b)
(c)
(d)
(e)
(f)


## 3.2. Photocatalytic Decolorization of MG by Ni-DMG/ZSM-5

### 3.2.1. Effect of Catalyst Concentration

The initial rate of the photocatalytic degradation of many pollutants is a function of the photocatalyst dosage [15, 34]. A series of experiments was carried out to assess the optimum catalyst loading by varying the amount of the catalyst from 0.2 to 1.0 g L−1 with MG concentration (20 ppm). The results depicted in Figure 6 show that the degradation rate increases with increasing the mass of the catalyst, reached the highest value (0.6 g L−1 of the catalyst) and then decreased considerably. The reason for this decrease is thought to be the fact that when the concentration of the catalyst rises, the solid particles increasingly block the penetration of the photons. So the overall number of the photons that can be reached to catalyst particles and hence the production of OH radicals decrease [35]. Another reason may be due to the aggregation of solid particles while using a large amount of catalyst [4, 36]. Also, Figure 6 shows that the removal rates were negligible in the absence of catalyst or dark condition after 3 h control.Figure 6
Effect of Ni-DMG/ZSM-5 dosage on the decolorization efficiency of MG dye; initial dye concentration, 20 ppm; initial pH, 5.3; photocatalyst dosage, (0.2, 0.4, 0.6 and 0.8 g L−1); 55 W Hg lamp; continuous stirring; irradiation time, 180 min; room temperature.Many authors have reported that the kinetic behavior of the photocatalytic reactions obeys the first-order reaction [35, 36]. In order to confirm the speculation, ln(C/C0) was plotted as a function of the irradiation time. The calculated results indicated that the first-order model gives a better fit. The rate constant values, k (min−1), are calculated from the straight-line segment of the first-order plots as a function of the catalyst mass and are listed in Table 1. As the results show, maximum degradation (76.5%) of MG. dye was observed after 120 min with the maximum rate constant (3.6 × 10−2 min−1) in the presence of 0.6 g L−1 of the catalyst. Methyl green alone could not be transformed under UV irradiation, corresponding to the rate constant (k) of 3.0 × 10−5 min−1. In the following experiments, we chose 0.6 g L−1 of Ni-DMG/ZSM-5 as the optimum dosage.Table 1
Rate constant values as a function of various experimental parameters.
Parameter
Value
k × 100 (min−1)
Catalyst amount (g L−1)
0
0.003
0.2
0.9
0.4
1.9
0.6
3.6
0.8
1.7
1.0
0.46
1
0
3
1.1
pH
5
4.6
7
5.2
9
6.1
25
1.8
40
2.4
Temperature (°C)
50
2.7
60
3.5
80
4.3
C
MG (ppm)
10
0.10
20
0.46
40
2.11
60
0.6
80
0.44
100
0.29


### 3.2.2. Effect of pH

The waste water from the textile industries usually has a wide range of pH values. Generally pH plays an important role both in the characteristics of textile wastes and generation of active sites [37]. Hence, the role of pH on the degradation extent of MG was studied in the pH range of 1–9 in 20 ppm MG concentration containing 0.6 g L−1 of the catalyst. At pHs above 9, the solution was colorless and the λmax of the MG was shifted to UV region (before 250 nm) and hence a decrease in the absorbance of the solution during the degradation process was not distinguishable. Hence, the corresponding results was not measured. The solution of pH was adjusted only prior to irradiation and was not controled during the reaction. As shown in Figure 7, the percentage of decolorization increased with increasing pH. As mentioned in the literature [35], in the initial acidic pHs, concomitant with acidification of the solution by HCl, a high amount of conjugated base is added to the solution. The anion Cl- is able to react with hydroxyl radicals leading to inorganic radical ions (ClO-∙). These inorganic radical anions show a much lower reactivity than ∙OH, so that they do not take part in the dye decolorization. There is also a drastic competition between the dye and anions with respect to ∙OH. Hence, increasing pH shows an increase in the degradation efficiency. Alkaline pHs favor the formation of more OH radicals due to the presence of large quantity of OH- anions in the alkaline medium, which enhances the photocatalytic degradation of MG significantly [25]. In acidic solutions a decrease in the decolorization rate was observed reflecting the difficulty of the dye molecules to approach the catalyst surface due to electrostatic interactions. In other words, at low pH, the adsorption of cationic dye on the surface of the photocatalyst was decreased because the photocatalyst surface will be positively charged and repulsive force is due to decreasing adsorption [34].Figure 7
Effect of solution pH on the MG dye decolorization; 0.6 g L−1 of the catalyst; initial dye concentration, 20 ppm; 55 W Hg lamp; continuous stirring; irradiation time, 180 min; room temperature.Table1 shows the dependence of k on pH. As can be seen, the observed degradation is strongly dependent on pH, occurring efficiently at pH 9. However, we have carried out all the experiments in natural pH (5.3) conditions.At the end of the studies on pH effect, the leached nickel cations were followed by atomic spectroscopy. The results showed that the leached nickel cations increase with decreasing pH, so its extent was significantly increased from pH 3 to 1. But, the leached nickel was not sufficient to determine its value quantitatively and it was only followed qualitatively. This indicates that the Ni-DMG is very stable in the zeolite bed and the leached nickel does not contaminate the solution.


### 3.2.3. Effect of Temperature

Since the photonic activation occurs at considerably high speeds, it is expected that the photocatalytic system is not sensible to the temperature, and the true activation energy most be then equal to zero. Although considering that the reactions under study occur preferentially in the liquid/solid interface, a nonzero value must be expected as apparent activation energy. It was observed that with increase in the temperature from 25 to 60°C (at a 20 ppm MG concentration containing 0.6 g L−1 catalyst), the percentage of decolorization increases (Figure 8). With increasing in temperature, the exothermic adsorption of the reactants becomes disfavored due to reducing the value of the apparent activation energy [38]. On the other hand, an increase in temperature decreases the solubility of oxygen in water which is not desirable. Higher temperatures will cause significant evaporation of the solution during the experiments. Thus, temperature higher than 80°C is not recommended. The rate constant values (k, min−1) as a function of temperature on the dye decolorization are presented in Table 1.Figure 8
Effect of the reaction temperature on decolorization efficiency; 0.6 g L−1 of catalyst; initial dye concentration, 20 ppm; initial solution pH; 55 W Hg lamp; continuous stirring; irradiation time, 180 min; room temperature.


### 3.2.4. Effect of Methyl Green Concentration

The degradation efficiency also depends on the initial concentration of the substrate [3]. The MG decolorization was studied over the concentration covering the range from 10 to 100 ppm by maintaining the other parameters constant. The decolorization is the highest at 40 ppm and thereafter decreases (Figure 9). The life time of hydroxyl radicals is very short (only a few nanoseconds) and thus they can only react where they are formed. Increasing the quantity of MG molecules per volume unit logically enhances the probability of collision between organic matter and oxidizing species, leading to an increase in the decolorization efficiency. It is seen that the decolorization efficiency of dye was decreased with increasing the initial concentration to more than 40 ppm. The decrease of the degradation percent with increasing of dye concentration can be due to two reasons. With increasing the amounts of dye, the more of dye molecules will be adsorbed on the surface of the photocatalyst particles and the active sites of the catalyst will be reduced. Therefore, with increasing occupied space of catalyst surface, the generation of hydroxyl radicals will be decreased. Also, increasing the concentration of dye can lead to decreasing the number of photons that is arrived to the surface of catalyst particles. More light is absorbed by molecules of dye and the excitation of photocatalyst particles by photons will be reduced. These results are in good accordance with the literature [34, 37, 39, 40]. This is also simplified in Table 1 where the degradation rate constant (k, min−1) is listed as a function of initial concentration of the dye. It is apparent that the rate of degradation is a quantitative of concentration dependent and the activity was increased with increasing concentration to 40 ppm.Figure 9
Effect of the initial dye concentration on decolorization efficiency of MG; 0.6 g L−1 of catalyst; initial solution pH, 5.3; 55 W Hg lamp; continuous stirring; irradiation time, 180 min; room temperature.


### 3.2.5. Comparison of MG Degradation over Ni-DMG/ZSM-5 and Ni-DMG

The amount of Ni loaded in zeolite was measured by atomic absorption spectroscopy and to be 0.0343 mmol per gram of Ni-DMG/ZSM-5. To determine whether the degradation of MG by Ni-DMG takes place or not, the catalytic activity of 0.02 g L−1 Ni-DMG was measured under the same above-mentioned experimental conditions. No remarkable activity was noticed due to the presence of Ni-DMG as shown in Table 2. It can be concluded that the degradation process occurs insignificantly in the presence of Ni-DMG. The role of the zeolite might be correlated with the adsorption process, in the sense of high surface area and the decrease of particle size [36]. This, in turn, causes an increase in the photodegradation efficiency. Another reason can be related to hydrophobicity properties of the support that is the major factor for the high degradation. The high hydrophobicity of ZSM-5 can be assigned to the influence of the hydrophobic character of structure directing agent for the synthesis of ZSM-5 (e.g., tetrapropylammonium cations) [41]. Hydrophobicity of ZSM-5 increases the adsorption of hydrophobic MG. Highly siliceous ZSM-5 zeolites with low Al2O3 content are known to have highly hydrophobic surfaces [23]. This observation clearly establishes the importance of support on the activity of degradation of MG.Table 2
Comparison of the photocatalytic activity of supported and unsupported catalysts.
Time (min)
Degradation (%)
Ni-DMG/ZSM-5
Ni-DMG
30
14.2
8
60
38
18.6
90
64
19.1
120
73
22.2


### 3.2.6. Catalyst Life

The catalyst stability is a factor that needs to be addressed. After several times of use, the catalyst may be partially desorbed into the solution or decomposed into some fragments. Secondly, the catalyst ability may be deactivated by the reaction intermediates or products formed during the dye degradation [42]. Hence, the reusability of Ni-DMG/ZSM-5 catalyst in the degradation of MG was evaluated. The recycling experiments were performed with MG (40 ppm) and Ni-DMG/ZSM-5 (0.6 g L−1). After irradiation (1 h), Ni-DMG/ZSM-5 was recovered by filtration, calcined at 90°C, and tested again for its activity under identical experimental conditions. Ni-DMG/ZSM-5 exhibited almost the same catalytic activity for three cycles of operation. The experiments were repeated under the same conditions, but the temperature of calcination was 230°C. Table 3 summarizes the results of experiments. In all cases, the percentage of decolorization was decreased. Two factors are responsible for such a decrease. First, the catalyst concentration was gradually decreased, due to sample analysis [42]. Second, the Ni-DMG/ZSM-5 catalyst experienced a slow bleaching during the reaction process, as observed above in a homogeneous solution. As can be seen, the percentage of decolorization increases upon enhancing the calcinations temperature from 90 to 230°C. The Ni-DMG/ZSM-5 calcined at 230°C possesses comparatively higher specific surface area than the sample calcined at 90°C.Table 3
Reusability of Ni-DMG/ZSM-5 catalyst in the decolorization of MG.
Number of cycle
Degradation (%)
Calcination in 90°C
Calcination in 230°C
1
80.5
88.0
2
74.0
82.1
3
65.3
74.3The decrease in the activity of the used catalyst must reflect the presence of some adventitious degradation products adsorbed in the zeolite, causing the partial blockage of the pore system or covering the zeolite surface. Preliminary thermal reactivation trials at 230°C did lead to an appreciable degradation of Ni-DMG/ZSM-5 photocatalyst as evidenced visually by the color change. Our results show a good agreement with the literature [34].


### 3.2.7. Comparing the Work with Other Works in MG Degradation

In previous work [39], MG was decolorized by Fe(II)-o-phenanthroline/zeolite Y nanocluster. Comparing the results shows that in this work a smaller weight of the NiDMG-ZSM-5 (0.6 g L−1) has been used (with respect to 1.0 g L−1 of Fe(II)-o-phenanthroline/zeolite Y nanocluster). This can be related to higher hydrophobicity of ZSM-5 with respect to zeolite Y to adsorb more MG molecules. Biodegradation of some triphenylmethane dyes has been studied [43], and this method has disadvantages with respect to heterogeneous photocatalysis as mentioned in Section 1. Photodegradation of methyl green were studied and the reaction pathway and identification of intermediates was studied by an HPLC [4].


## 3.2.1. Effect of Catalyst Concentration

The initial rate of the photocatalytic degradation of many pollutants is a function of the photocatalyst dosage [15, 34]. A series of experiments was carried out to assess the optimum catalyst loading by varying the amount of the catalyst from 0.2 to 1.0 g L−1 with MG concentration (20 ppm). The results depicted in Figure 6 show that the degradation rate increases with increasing the mass of the catalyst, reached the highest value (0.6 g L−1 of the catalyst) and then decreased considerably. The reason for this decrease is thought to be the fact that when the concentration of the catalyst rises, the solid particles increasingly block the penetration of the photons. So the overall number of the photons that can be reached to catalyst particles and hence the production of OH radicals decrease [35]. Another reason may be due to the aggregation of solid particles while using a large amount of catalyst [4, 36]. Also, Figure 6 shows that the removal rates were negligible in the absence of catalyst or dark condition after 3 h control.Figure 6
Effect of Ni-DMG/ZSM-5 dosage on the decolorization efficiency of MG dye; initial dye concentration, 20 ppm; initial pH, 5.3; photocatalyst dosage, (0.2, 0.4, 0.6 and 0.8 g L−1); 55 W Hg lamp; continuous stirring; irradiation time, 180 min; room temperature.Many authors have reported that the kinetic behavior of the photocatalytic reactions obeys the first-order reaction [35, 36]. In order to confirm the speculation, ln(C/C0) was plotted as a function of the irradiation time. The calculated results indicated that the first-order model gives a better fit. The rate constant values, k (min−1), are calculated from the straight-line segment of the first-order plots as a function of the catalyst mass and are listed in Table 1. As the results show, maximum degradation (76.5%) of MG. dye was observed after 120 min with the maximum rate constant (3.6 × 10−2 min−1) in the presence of 0.6 g L−1 of the catalyst. Methyl green alone could not be transformed under UV irradiation, corresponding to the rate constant (k) of 3.0 × 10−5 min−1. In the following experiments, we chose 0.6 g L−1 of Ni-DMG/ZSM-5 as the optimum dosage.Table 1
Rate constant values as a function of various experimental parameters.
Parameter
Value
k × 100 (min−1)
Catalyst amount (g L−1)
0
0.003
0.2
0.9
0.4
1.9
0.6
3.6
0.8
1.7
1.0
0.46
1
0
3
1.1
pH
5
4.6
7
5.2
9
6.1
25
1.8
40
2.4
Temperature (°C)
50
2.7
60
3.5
80
4.3
C
MG (ppm)
10
0.10
20
0.46
40
2.11
60
0.6
80
0.44
100
0.29


## 3.2.2. Effect of pH

The waste water from the textile industries usually has a wide range of pH values. Generally pH plays an important role both in the characteristics of textile wastes and generation of active sites [37]. Hence, the role of pH on the degradation extent of MG was studied in the pH range of 1–9 in 20 ppm MG concentration containing 0.6 g L−1 of the catalyst. At pHs above 9, the solution was colorless and the λmax of the MG was shifted to UV region (before 250 nm) and hence a decrease in the absorbance of the solution during the degradation process was not distinguishable. Hence, the corresponding results was not measured. The solution of pH was adjusted only prior to irradiation and was not controled during the reaction. As shown in Figure 7, the percentage of decolorization increased with increasing pH. As mentioned in the literature [35], in the initial acidic pHs, concomitant with acidification of the solution by HCl, a high amount of conjugated base is added to the solution. The anion Cl- is able to react with hydroxyl radicals leading to inorganic radical ions (ClO-∙). These inorganic radical anions show a much lower reactivity than ∙OH, so that they do not take part in the dye decolorization. There is also a drastic competition between the dye and anions with respect to ∙OH. Hence, increasing pH shows an increase in the degradation efficiency. Alkaline pHs favor the formation of more OH radicals due to the presence of large quantity of OH- anions in the alkaline medium, which enhances the photocatalytic degradation of MG significantly [25]. In acidic solutions a decrease in the decolorization rate was observed reflecting the difficulty of the dye molecules to approach the catalyst surface due to electrostatic interactions. In other words, at low pH, the adsorption of cationic dye on the surface of the photocatalyst was decreased because the photocatalyst surface will be positively charged and repulsive force is due to decreasing adsorption [34].Figure 7
Effect of solution pH on the MG dye decolorization; 0.6 g L−1 of the catalyst; initial dye concentration, 20 ppm; 55 W Hg lamp; continuous stirring; irradiation time, 180 min; room temperature.Table1 shows the dependence of k on pH. As can be seen, the observed degradation is strongly dependent on pH, occurring efficiently at pH 9. However, we have carried out all the experiments in natural pH (5.3) conditions.At the end of the studies on pH effect, the leached nickel cations were followed by atomic spectroscopy. The results showed that the leached nickel cations increase with decreasing pH, so its extent was significantly increased from pH 3 to 1. But, the leached nickel was not sufficient to determine its value quantitatively and it was only followed qualitatively. This indicates that the Ni-DMG is very stable in the zeolite bed and the leached nickel does not contaminate the solution.


## 3.2.3. Effect of Temperature

Since the photonic activation occurs at considerably high speeds, it is expected that the photocatalytic system is not sensible to the temperature, and the true activation energy most be then equal to zero. Although considering that the reactions under study occur preferentially in the liquid/solid interface, a nonzero value must be expected as apparent activation energy. It was observed that with increase in the temperature from 25 to 60°C (at a 20 ppm MG concentration containing 0.6 g L−1 catalyst), the percentage of decolorization increases (Figure 8). With increasing in temperature, the exothermic adsorption of the reactants becomes disfavored due to reducing the value of the apparent activation energy [38]. On the other hand, an increase in temperature decreases the solubility of oxygen in water which is not desirable. Higher temperatures will cause significant evaporation of the solution during the experiments. Thus, temperature higher than 80°C is not recommended. The rate constant values (k, min−1) as a function of temperature on the dye decolorization are presented in Table 1.Figure 8
Effect of the reaction temperature on decolorization efficiency; 0.6 g L−1 of catalyst; initial dye concentration, 20 ppm; initial solution pH; 55 W Hg lamp; continuous stirring; irradiation time, 180 min; room temperature.


## 3.2.4. Effect of Methyl Green Concentration

The degradation efficiency also depends on the initial concentration of the substrate [3]. The MG decolorization was studied over the concentration covering the range from 10 to 100 ppm by maintaining the other parameters constant. The decolorization is the highest at 40 ppm and thereafter decreases (Figure 9). The life time of hydroxyl radicals is very short (only a few nanoseconds) and thus they can only react where they are formed. Increasing the quantity of MG molecules per volume unit logically enhances the probability of collision between organic matter and oxidizing species, leading to an increase in the decolorization efficiency. It is seen that the decolorization efficiency of dye was decreased with increasing the initial concentration to more than 40 ppm. The decrease of the degradation percent with increasing of dye concentration can be due to two reasons. With increasing the amounts of dye, the more of dye molecules will be adsorbed on the surface of the photocatalyst particles and the active sites of the catalyst will be reduced. Therefore, with increasing occupied space of catalyst surface, the generation of hydroxyl radicals will be decreased. Also, increasing the concentration of dye can lead to decreasing the number of photons that is arrived to the surface of catalyst particles. More light is absorbed by molecules of dye and the excitation of photocatalyst particles by photons will be reduced. These results are in good accordance with the literature [34, 37, 39, 40]. This is also simplified in Table 1 where the degradation rate constant (k, min−1) is listed as a function of initial concentration of the dye. It is apparent that the rate of degradation is a quantitative of concentration dependent and the activity was increased with increasing concentration to 40 ppm.Figure 9
Effect of the initial dye concentration on decolorization efficiency of MG; 0.6 g L−1 of catalyst; initial solution pH, 5.3; 55 W Hg lamp; continuous stirring; irradiation time, 180 min; room temperature.


## 3.2.5. Comparison of MG Degradation over Ni-DMG/ZSM-5 and Ni-DMG

The amount of Ni loaded in zeolite was measured by atomic absorption spectroscopy and to be 0.0343 mmol per gram of Ni-DMG/ZSM-5. To determine whether the degradation of MG by Ni-DMG takes place or not, the catalytic activity of 0.02 g L−1 Ni-DMG was measured under the same above-mentioned experimental conditions. No remarkable activity was noticed due to the presence of Ni-DMG as shown in Table 2. It can be concluded that the degradation process occurs insignificantly in the presence of Ni-DMG. The role of the zeolite might be correlated with the adsorption process, in the sense of high surface area and the decrease of particle size [36]. This, in turn, causes an increase in the photodegradation efficiency. Another reason can be related to hydrophobicity properties of the support that is the major factor for the high degradation. The high hydrophobicity of ZSM-5 can be assigned to the influence of the hydrophobic character of structure directing agent for the synthesis of ZSM-5 (e.g., tetrapropylammonium cations) [41]. Hydrophobicity of ZSM-5 increases the adsorption of hydrophobic MG. Highly siliceous ZSM-5 zeolites with low Al2O3 content are known to have highly hydrophobic surfaces [23]. This observation clearly establishes the importance of support on the activity of degradation of MG.Table 2
Comparison of the photocatalytic activity of supported and unsupported catalysts.
Time (min)
Degradation (%)
Ni-DMG/ZSM-5
Ni-DMG
30
14.2
8
60
38
18.6
90
64
19.1
120
73
22.2


## 3.2.6. Catalyst Life

The catalyst stability is a factor that needs to be addressed. After several times of use, the catalyst may be partially desorbed into the solution or decomposed into some fragments. Secondly, the catalyst ability may be deactivated by the reaction intermediates or products formed during the dye degradation [42]. Hence, the reusability of Ni-DMG/ZSM-5 catalyst in the degradation of MG was evaluated. The recycling experiments were performed with MG (40 ppm) and Ni-DMG/ZSM-5 (0.6 g L−1). After irradiation (1 h), Ni-DMG/ZSM-5 was recovered by filtration, calcined at 90°C, and tested again for its activity under identical experimental conditions. Ni-DMG/ZSM-5 exhibited almost the same catalytic activity for three cycles of operation. The experiments were repeated under the same conditions, but the temperature of calcination was 230°C. Table 3 summarizes the results of experiments. In all cases, the percentage of decolorization was decreased. Two factors are responsible for such a decrease. First, the catalyst concentration was gradually decreased, due to sample analysis [42]. Second, the Ni-DMG/ZSM-5 catalyst experienced a slow bleaching during the reaction process, as observed above in a homogeneous solution. As can be seen, the percentage of decolorization increases upon enhancing the calcinations temperature from 90 to 230°C. The Ni-DMG/ZSM-5 calcined at 230°C possesses comparatively higher specific surface area than the sample calcined at 90°C.Table 3
Reusability of Ni-DMG/ZSM-5 catalyst in the decolorization of MG.
Number of cycle
Degradation (%)
Calcination in 90°C
Calcination in 230°C
1
80.5
88.0
2
74.0
82.1
3
65.3
74.3The decrease in the activity of the used catalyst must reflect the presence of some adventitious degradation products adsorbed in the zeolite, causing the partial blockage of the pore system or covering the zeolite surface. Preliminary thermal reactivation trials at 230°C did lead to an appreciable degradation of Ni-DMG/ZSM-5 photocatalyst as evidenced visually by the color change. Our results show a good agreement with the literature [34].


## 3.2.7. Comparing the Work with Other Works in MG Degradation

In previous work [39], MG was decolorized by Fe(II)-o-phenanthroline/zeolite Y nanocluster. Comparing the results shows that in this work a smaller weight of the NiDMG-ZSM-5 (0.6 g L−1) has been used (with respect to 1.0 g L−1 of Fe(II)-o-phenanthroline/zeolite Y nanocluster). This can be related to higher hydrophobicity of ZSM-5 with respect to zeolite Y to adsorb more MG molecules. Biodegradation of some triphenylmethane dyes has been studied [43], and this method has disadvantages with respect to heterogeneous photocatalysis as mentioned in Section 1. Photodegradation of methyl green were studied and the reaction pathway and identification of intermediates was studied by an HPLC [4].


## 4. Conclusions

The MG dye can be more efficiently degraded by Ni-DMG incorporated zeolite ZSM-5 in the presence of UV light. It is important to choose the optimum degradation parameters for increasing the degradation rate. The catalyst can be reused for dye degradation with slightly less efficiency. Zeolite bed shows an important role in the degradation process so that Ni-DMG out of zeolite framework did not show any considerable degradation efficiency.



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*Source: 104093-2012-12-03.xml*