# Efficient Oxidative Removal of Organic Pollutants by Ordered Mesoporous Carbon-Supported Cobalt Phthalocyanine

Authors: Yi Chen; Yan Gu; Nan Li; Wangyang Lu; Wenxing Chen
Journal: Journal of Nanomaterials
 (2016)

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## Abstract

Ordered mesoporous carbon (OMC) materials have received attention for use as supports in highly efficient catalytic systems because of their excellent properties. We used epoxy compound 2,3-epoxypropyl trimethylammonium chloride (EPTAC) to modify cobalt tetraaminophthalocyanine (CoTAPc) and obtained a novel catalyst (OMC-CoTAPc-EPTAC) based on OMC-bonded CoTAPc-EPTAC that could oxidize Acid Red 1 (AR1) dyes by hydrogen peroxide (H2O2) activation under neutral conditions. OMC enhanced the catalytic performance of OMC-CoTAPc-EPTAC, which resulted in the combined high catalytic activity and high stability. Because of its large surface area and tunable pore texture, OMC has high substrate accessibility, and the modification of the catalyst with EPTAC could promote adsorption of the target substrate into OMC, which achieved the aim of in situ catalytic oxidation with enrichment of the target substrate and improved the catalytic efficiency significantly. Electron paramagnetic resonance spin-trap experiments confirmed that the OMC-CoTAPc-EPTAC/H2O2 system had a nonradical catalytic mechanism, and the high-valent cobalt-oxo intermediates and generated holes were speculated to act as dominant oxidation species for the catalytic degradation of AR1. These results demonstrated a new strategy for the elimination of low-concentration organic pollutants.


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## Body

## 1. Introduction

Ordered mesoporous carbon (OMC) materials have received considerable attention because of their stable physical and chemical properties and excellent structural characteristics (i.e., large surface area, tunable pore texture, and uniform pore size) [1–5], which shows great promise for application in catalysis, pollutant adsorption, energy storage, and electrochemistry [6–12]. With their porous interfacial structure and controlled mesopore size, OMC materials exhibit great potential for the adsorption of different types of substrates, especially for bulky molecules, and also provide ample space for substrate diffusion [13, 14]. The larger pore size and ordered three-dimensional open channels of the OMC materials provide them with obvious advantages as catalyst carriers for substrate conversion and the reduction of mass transfer limitations.Metallophthalocyanines (MPcs) have been studied as catalysts in many applications [15–19], for example, sulfonated cobalt phthalocyanines have been shown to perform catalytic oxidation of mercaptans to remove most sulfur from petrol in the Merox process [20], which results because their structure correlates with porphyrin complexes and also because they are readily available on a large scale and are inexpensive. MPcs are fascinating catalysts, with the main focus being on catalytic oxidation for various organic pollutants [21–24]. In general, these catalytic reactions with MPcs occur through electron exchange with coordination between the central metal ion and the reactant. The highly conjugated macrocyclic structure of MPcs as an electron donor can result in electron loss after oxidation and as an electron acceptor can gain electrons after reduction. Several factors, such as substituents and supports, are considered to influence the MPcs catalytic properties. In addition, to achieve their separation and recycle, it is important to choose an appropriate support to immobilize MPcs, where the catalyst activity can be maintained or improved and secondary pollution can be controlled. In our previous work, we found that cellulosic fiber-supported MPcs could eliminate organic dyes [25] but were less efficient for the oxidative removal of phenols, possibly because of the poor adsorption of phenols or the low catalytic activity. Some studies also indicated that the introduction of carbon materials could lead to significant enhancement in MPcs activity because of the electron interaction between carbon materials and MPcs [26, 27]. For instance, carbon nanotubes (CNTs) with a special sp2-hybridized structure could enhance the catalytic activity of cobalt phthalocyanine in activating hydrogen peroxide (H2O2) [28, 29]; activated carbon fiber could improve the cobalt phthalocyanine catalytic performance toward phenol oxidation [30] but appears ineffectual for larger substrates.Therefore, OMC may be an ideal candidate to support MPcs with a combined high substrate accessibility and enhanced catalyst activity. Here, we used OMC to bond cobalt tetraaminophthalocyanine (CoTAPc) modified by the epoxy compound, 2,3-epoxypropyl trimethylammonium chloride (EPTAC), and obtained a new catalyst with positively charged quaternary ammonium salt chain (OMC-CoTAPc-EPTAC), where the EPTAC led to a highly efficient adsorption for target substrates, especially for negatively charged substrates. Because of requirements for environmentally friendly development, the clean oxidant H2O2 was used to construct a catalytic oxidation system, OMC-CoTAPc-EPTAC/H2O2. The system accomplished the aim of in situ catalytic oxidation with the enrichment of target substrate, which improves the catalytic efficiency significantly. This system is expected to be applied in the treatment of organic pollutants, especially for microcontaminants that are difficult to remove. In the OMC-CoTAPc-EPTAC/H2O2 system, enhanced catalytic performance was evidenced by the oxidative degradation of the dye Acid Red 1 (AR1). The electron paramagnetic resonance (EPR) spin-trap technique was used to determine the possible mechanism for H2O2 activation by OMC-CoTAPc-EPTAC. Key factors that are likely to influence the oxidation process, such as temperature and H2O2 concentration, were explored, and the stability of the catalytic system was discussed.


## 2. Experimental

### 2.1. Materials and Reagents

AR1 and the spin-trapping reagent 5,5-dimethyl-1-pyrroline N-oxide (DMPO) were obtained from Tokyo Chemical Industry Co., Ltd. Cobalt chloride hexahydrate, urea, and hydrogen peroxide (9.7 M, Sinopharm Chemical Reagent Co., Ltd.) were used as analytical reagents. Doubly distilled water was used throughout the AR1 removal experiments. All other solvents were of spectrometric grade.


### 2.2. Catalyst Preparation

OMC was synthesized from resorcinol, F127, formaldehyde, ethanol, and HCl [31], and CoTAPc was synthesized from 4-nitrophthalic acid, cobalt chloride hexahydrate, and urea [32]. CoTAPc (0.05 g) was dissolved in dimethyl sulfoxide solution. The solution was stirred vigorously and kept at 85°C for 30 min in an oil bath before 0.02 g of EPTAC (n
E
P
T
A
C : n
C
o
T
A
P
c
=
1.5 : 1) was added. After reaction for 5 h, OMC (1 g) was added to the reaction solution, stirring constantly, and then isopropyl nitrite was added to the reaction at 85°C for 12 h. The product was purified by centrifugation and washing with ultrapure water several times. OMC-CoTAPc-EPTAC was obtained after drying. This method was inspired by [33], and the synthesis is shown in Scheme 1 (the part functionalization of the amino groups on CoTAPc, taking the 1 : 4 molar ratio functionalization of the amino groups as the example).Scheme 1
Synthesis of OMC-CoTAPc-EPTAC.


### 2.3. Catalyst Characterizations

Ultraviolet- (UV-) visible (Vis) absorption spectra were acquired at ambient temperature on a Hitachi U-3100 spectrophotometer, and spectra were recorded from 400 to 800 nm. The porous structure of the samples was observed by transmission electron microscopy (TEM) using a JEOL JEM-2010 microscope.Nitrogen (N2) adsorption/desorption isotherms were obtained at –196°C using a Micromeritics ASAP 2020 apparatus. Prior to the measurement, samples were degassed at 180°C for at least 6 h. To calculate the surface area, the Brunauer-Emmett-Teller (BET) model was applied for 0.06
≤
P
/
P
0
≤
0.30. The mesoporous volume was calculated from the amount of nitrogen adsorbed at a relative pressure of 0.95, and the pore size distribution was evaluated using the Barrett-Joyner-Halenda model.Powder X-ray diffraction patterns (XRD) were measured on an HP DX-2700 diffractometer operated at 40 kV and 40 mA and equipped with a graphite monochromator using Cu-Ka radiation. Measurements were achieved for 0.1–80° 2θ with steps of 0.02°.Thermogravimetric analyses (TGA) were carried out on a TG Mettler Toledo STARe apparatus, with a heating rate of 20°C/min from 25 to 800°C in N2 to determine the thermal stability of the samples.The cobalt content in OMC-CoTAPc-EPTAC was confirmed to be 49.42μmol/g by microwave-assisted digestion-flame atomic absorption spectrometry (Thermo Sollar M6).


### 2.4. Catalytic Oxidation

The catalytic activity of OMC-CoTAPc-EPTAC in activating H2O2 in aqueous solution was investigated by the oxidative degradation of AR1. The initial concentration of AR1 was 0.05 mM, and oxidation was initiated when H2O2 (15 mM) was added into the solution in the presence of OMC-CoTAPc-EPTAC (0.4 g/L). All reactions were performed in a container agitated with a magnetic stirrer and heated in a temperature-controlled water bath under neutral conditions. At given times, samples were analyzed with a UV-Vis spectrometer by measuring the removal of AR1 at the maximal wavelength. Stability and reusability were addressed through a cycle of five continuous experiments. For every run, a specific concentration of AR1 was added into the reaction system to maintain the initial 0.05 mM concentration, and 5 mM H2O2 was added to each cycle starting from the next cycle. The catalytic mechanism was analyzed by EPR, and the EPR signals of radicals trapped by DMPO were detected on a Bruker A300 spectrometer.


## 2.1. Materials and Reagents

AR1 and the spin-trapping reagent 5,5-dimethyl-1-pyrroline N-oxide (DMPO) were obtained from Tokyo Chemical Industry Co., Ltd. Cobalt chloride hexahydrate, urea, and hydrogen peroxide (9.7 M, Sinopharm Chemical Reagent Co., Ltd.) were used as analytical reagents. Doubly distilled water was used throughout the AR1 removal experiments. All other solvents were of spectrometric grade.


## 2.2. Catalyst Preparation

OMC was synthesized from resorcinol, F127, formaldehyde, ethanol, and HCl [31], and CoTAPc was synthesized from 4-nitrophthalic acid, cobalt chloride hexahydrate, and urea [32]. CoTAPc (0.05 g) was dissolved in dimethyl sulfoxide solution. The solution was stirred vigorously and kept at 85°C for 30 min in an oil bath before 0.02 g of EPTAC (n
E
P
T
A
C : n
C
o
T
A
P
c
=
1.5 : 1) was added. After reaction for 5 h, OMC (1 g) was added to the reaction solution, stirring constantly, and then isopropyl nitrite was added to the reaction at 85°C for 12 h. The product was purified by centrifugation and washing with ultrapure water several times. OMC-CoTAPc-EPTAC was obtained after drying. This method was inspired by [33], and the synthesis is shown in Scheme 1 (the part functionalization of the amino groups on CoTAPc, taking the 1 : 4 molar ratio functionalization of the amino groups as the example).Scheme 1
Synthesis of OMC-CoTAPc-EPTAC.


## 2.3. Catalyst Characterizations

Ultraviolet- (UV-) visible (Vis) absorption spectra were acquired at ambient temperature on a Hitachi U-3100 spectrophotometer, and spectra were recorded from 400 to 800 nm. The porous structure of the samples was observed by transmission electron microscopy (TEM) using a JEOL JEM-2010 microscope.Nitrogen (N2) adsorption/desorption isotherms were obtained at –196°C using a Micromeritics ASAP 2020 apparatus. Prior to the measurement, samples were degassed at 180°C for at least 6 h. To calculate the surface area, the Brunauer-Emmett-Teller (BET) model was applied for 0.06
≤
P
/
P
0
≤
0.30. The mesoporous volume was calculated from the amount of nitrogen adsorbed at a relative pressure of 0.95, and the pore size distribution was evaluated using the Barrett-Joyner-Halenda model.Powder X-ray diffraction patterns (XRD) were measured on an HP DX-2700 diffractometer operated at 40 kV and 40 mA and equipped with a graphite monochromator using Cu-Ka radiation. Measurements were achieved for 0.1–80° 2θ with steps of 0.02°.Thermogravimetric analyses (TGA) were carried out on a TG Mettler Toledo STARe apparatus, with a heating rate of 20°C/min from 25 to 800°C in N2 to determine the thermal stability of the samples.The cobalt content in OMC-CoTAPc-EPTAC was confirmed to be 49.42μmol/g by microwave-assisted digestion-flame atomic absorption spectrometry (Thermo Sollar M6).


## 2.4. Catalytic Oxidation

The catalytic activity of OMC-CoTAPc-EPTAC in activating H2O2 in aqueous solution was investigated by the oxidative degradation of AR1. The initial concentration of AR1 was 0.05 mM, and oxidation was initiated when H2O2 (15 mM) was added into the solution in the presence of OMC-CoTAPc-EPTAC (0.4 g/L). All reactions were performed in a container agitated with a magnetic stirrer and heated in a temperature-controlled water bath under neutral conditions. At given times, samples were analyzed with a UV-Vis spectrometer by measuring the removal of AR1 at the maximal wavelength. Stability and reusability were addressed through a cycle of five continuous experiments. For every run, a specific concentration of AR1 was added into the reaction system to maintain the initial 0.05 mM concentration, and 5 mM H2O2 was added to each cycle starting from the next cycle. The catalytic mechanism was analyzed by EPR, and the EPR signals of radicals trapped by DMPO were detected on a Bruker A300 spectrometer.


## 3. Results and Discussion

### 3.1. Characterization of OMC-CoTAPc-EPTAC

The UV-Vis absorption spectra of CoTAPc, OMC, and OMC-CoTAPc-EPTAC are shown in Figure1. The CoTAPc spectrum shows a sharp absorption peak at 705 nm and a weaker absorption peak at 412 nm because of the strong electron-donating property of the amino group on the CoTAPc ring. The spectrum does not show any absorption peaks at 400–800 nm for OMC, whereas the OMC-CoTAPc-EPTAC spectrum shows a broad absorption peak at 600–750 nm, which may be explained by the strong electronic interaction between CoTAPc and OMC. Therefore, we conclude that CoTAPc was supported on the OMC.Figure 1
UV-Vis absorption spectra for OMC, CoTAPc, and OMC-CoTAPc-EPTAC (in DMF).The textural properties of OMC and OMC-CoTAPc-EPTAC were investigated using high-resolution TEM and N2 absorption. The OMC surface morphology before and after modification with CoTAPc-EPTAC was studied by TEM (Figure 2). The compounds possessed a well-defined ordered mesoporous structure with uniform size, and the ordered mesostructure of OMC was rarely destroyed after modification with CoTAPc-EPTAC. The pore diameter is not visible in the TEM micrographs because of the superimposition of the three-dimensional mesopore system [34–36]. N2 adsorption/desorption isotherms were used to explore the pore structure and adsorption capacity of the samples further. Figure 3(a) showed an obvious increase in N2 uptake especially in the low-pressure region, which indicates the formation of highly porous carbon. A typical type IV isotherm with H2 hysteresis loops and a significant capillary condensation step for relative pressures of 0.45–0.8 was obtained, which suggests that the mesopore size was almost identical as shown by the corresponding pore size distribution analysis (Figure 3(b)). This confirmed that OMC and OMC-CoTAPc-EPTAC had a narrow ~6 nm pore size distribution in the mesopore range. According to the calculation results of the N2 adsorption/desorption isotherms, the BET surface area of OMC is 636 m2/g, which decreased to 530 m2/g after bonding cobalt tetraaminophthalocyanine. This could be explained by the fact that the interior OMC space was occupied partially by the CoTAPc-EPTAC. The ordered OMC-CoTAPc-EPTAC mesoporous structure was maintained and the OMC support exhibited relatively high adsorption capacity. This was consistent with the TEM observation.Figure 2
(a) and (b) TEM image of OMC calcined at 850°C. (c) and (d) TEM image of OMC-CoTAPc-EPTAC.
(a)
(b)
(c)
(d)Figure 3
(a) N2 sorption isotherm and (b) pore size distribution of OMC and OMC-CoTAPc-EPTAC.
(a)
(b)Additional structural information was obtained from the powder XRD analysis (Figure4). OMC has an XRD pattern with a sharp diffraction peak at 2θ = 24° and weaker peaks at 2θ = 45° that correspond to the (002) and (101) planes of carbon, respectively [37], which means that OMC had some ordered graphite crystallites after high-temperature carbonization. Figure 4 also shows that the diffraction peak of CoTAPc was centered at 2θ = 28°. The diffraction pattern of OMC-CoTAPc-EPTAC was similar to that of OMC, and the supported catalyst had no noticeable effect on the diffraction peaks, except that they were slightly weaker, probably because the crystalline structure of the OMC support was partially destroyed. These observations suggest that the CoTAPc had little influence on the OMC structure. To evaluate the thermal stability of the catalyst, TGA was carried out in N2 (Figure 5). OMC has an excellent thermal stability from 50 to 800°C. CoTAPc mass loss starts to occur at 200°C, and eventually some thermal decomposition will result. The mass loss curve of OMC-CoTAPc-EPTAC lay between that of OMC and CoTAPc, which means that the thermal stability of CoTAPc improved by introducing OMC as the support.Figure 4
XRD patterns for OMC, CoTAPc, and OMC-CoTAPc-EPTAC.Figure 5
TGA for OMC, CoTAPc, and OMC-CoTAPc-EPTAC.


### 3.2. Oxidative Degradation of AR1

To investigate the catalytic performance of OMC-CoTAPc-EPTAC, AR1 in aqueous solution was used as the model for catalytic oxidation. Figure6 shows that AR1 cannot be oxidized directly with H2O2 alone. In our previous work, we found that even in the presence of H2O2 and CoTAPc, almost no removal of target dyes resulted [28]. OMC-supported CoTAPc (OMC-CoTAPc) could only adsorb dyes fractionally, which resulted in a low oxidative removal rate of dyes with H2O2 [38]. Figure 6 shows that in the presence of OMC-CoTAPc-EPTAC alone, a clear decrease in AR1 resulted and the removal rate remained constant because the adsorption process attained equilibrium in a short time. The AR1 concentration decreased significantly when AR1 was exposed to OMC-CoTAPc-EPTAC and H2O2 together. These results suggest that the introduction of EPTAC into the catalyst induced a positive effect on improving the oxidative degradation efficiency of AR1 by facilitating the adsorption of dye into OMC. According to the previously described experiments, we infer that the removal of AR1 in the OMC-CoTAPc-EPTAC/H2O2 system included two processes: adsorption of AR1 into the OMC-CoTAPc-EPTAC and catalytic oxidation of the adsorbed AR1. Figure 7 shows that AR1 adsorption reached equilibrium in a short time without H2O2. Its concentration decreased significantly once H2O2 was added into the adsorption equilibrium system, which indicates that rapid and efficient oxidation of AR1 could be achieved when H2O2 was present in the reaction system and the adsorbed AR1 consumption was replenished continuously from AR1 in the bulk solution until the removal was complete. It is a great achievement that dyes could be enriched rapidly into OMC-CoTAPc-EPTAC and be decomposed in situ. Therefore, we conclude that the OMC-CoTAPc-EPTAC had high-level catalytic activity for AR1 oxidation, and OMC with a large adsorption capacity played a critical role during the degradation.Figure 6
Concentration changes of AR1 (0.05 mM) under different conditions ([OMC-CoTAPc-EPTAC] = 0.4 g/L, [H2O2] = 15 mM, pH 7, and 50°C).Figure 7
Concentration changes of AR1 (0.05 mM) after adsorption equilibrium with or without H2O2 ([OMC-CoTAPc-EPTAC] = 0.4 g/L, [H2O2] = 15 mM, pH 7, and 50°C).Temperature is an important factor that influences the catalytic reaction rate. To investigate the effect of reaction temperature on the OMC-CoTAPc-EPTAC/H2O2 catalytic system, the catalytic oxidation of AR1 was carried out at different temperatures with the result presented in Figure 8. In the presence of H2O2, OMC-CoTAPc-EPTAC could catalyze the oxidative removal of AR1 from 25 to 75°C, and the removal rate of AR1 increased as the reaction temperature increased. This may occur because the thermal energy of the AR1 molecules increased with increase in temperature, which resulted in a higher molecular heat movement speed. It was conducive to dye diffusion into the catalytic active sites, and enhanced the reaction rate. Based on the time courses of ln(C
0/C) at four different temperatures, an Arrhenius plot of ln
⁡
k-1/T is shown in Figure 9, and the activation energy of the oxidative degradation of AR1 in the OMC-CoTAPc-EPTAC/H2O2 system was 49.8 kJ/mol as calculated from the slope of the straight line. In comparison with common catalytic systems [39, 40], the system with a lower activation energy exhibited a high oxidative removal efficiency for AR1 at high temperature.Figure 8
Effect of temperature on catalytic oxidation of AR1 (0.05 mM) ([OMC-CoTAPc-EPTAC] = 0.4 g/L, [H2O2] = 15 mM, and pH 7).Figure 9
Arrhenius plots ofln
⁡
k-1/T with OMC-CoTAPc-EPTAC as catalyst.H2O2 is an environmentally friendly reagent and is used in almost all industrial fields. A reduction in H2O2 dosage is commercially important in chemical reaction processes. The effect of H2O2 dosage on AR1 removal efficiency was explored by varying the initial H2O2 concentration from 7.5 to 100 mM with results as shown in Figure 10. An increase in the initial H2O2 concentration led to a higher rate of AR1 degradation, and when increased above 15 mM, the AR1 concentration decreased sharply. Based on the H2O2 utilization efficiency, a H2O2 concentration of 15 mM was selected as the optimum H2O2 dosage. Compared with the single-walled carbon nanotube-supported CoTAPc (MWCNTs-CoTAPc)/H2O2 catalytic system reported in our previous paper [28], OMC-CoTAPc-EPTAC had a higher catalytic oxidation efficiency at a lower H2O2 concentration. This may be because the higher H2O2 utilization efficiency in the OMC-CoTAPc-EPTAC/H2O2 catalytic system could be ascribed to a different H2O2 activation mechanism or MWCNTs-CoTAPc served as an interfacial catalyst. Substrate adsorption and oxidation occurred at the MWCNT surface, whereas in the OMC-CoTAPc-EPTAC/H2O2 system, a reaction was required for the target substrates and H2O2 to enter into the interior of the OMC support, which significantly improved the H2O2 utilization in this catalytic system.Figure 10
Effect of initial H2O2 concentration on catalytic oxidation of AR1 (0.05 mM) ([OMC-CoTAPc-EPTAC] = 0.4 g/L, pH 7, and 50°C).Stability is another significant issue for catalyst use in practical applications. However, to the best of our knowledge, the supported MPcs usually lose partial activity because barriers to oxidation intermediates are generated in the reaction, or they may suffer from autocatalytic decomposition when the catalytic oxidation reaction is dominated by nonselectiveO
H
∙ [41], which results in a loss of catalytic activity. To study the catalyst stability, it is necessary to carry out continuous cyclic oxidation experiments of AR1 in the catalytic system that involves OMC-CoTAPc-EPTAC and H2O2. Figure 11 shows that the oxidative removal rate of AR1 was ~98% after the first cycle, and the rate was still high with no obvious decrease after five cycles of reuse. This highlights the excellent catalytic properties and good self-reliance regeneration ability of OMC-CoTAPc-EPTAC in repetitive experiments. These findings show that OMC introduction improves the catalytic activity and stability of CoTAPc and provides a transport channel for degradation products, guaranteeing constant substrate adsorption and oxidation, and achieves catalyst recycling.Figure 11
Cyclic catalytic oxidation of AR1 (0.05 mM), 5 mM H2O2 addition at each cycle after the first cycle ([OMC-CoTAPc-EPTAC] = 0.4 g/L, [H2O2] = 15 mM, pH 7, and 50°C).


### 3.3. Analysis of Catalytic Mechanism

A catalytic mechanism that is dominated by hydroxyl radical (O
H
∙) oxidation, high-valency metal-oxo species oxidation, or hole oxidation in the activated H2O2 systems has been reported. To obtain deeper insight into the possible catalytic mechanism of OMC-CoTAPc-EPTAC in activating H2O2, the EPR technique (with DMPO) was used with results shown in Figure 12. Nearly no DMPO-O
H
∙ and DMPO-O
O
H
∙ signals were detected for AR1 in aqueous or methanol solution, which shows that O
H
∙ and O
O
H
∙ were not major intermediates of the catalytic reaction with OMC-CoTAPc-EPTAC. From the EPR results, we concluded that the catalytic oxidation of AR1 occurred through a nonradical pathway, which was different from the common CoTAPc system [30], where the introduction of OMC and the direct-bonding method were considered two key factors that influence the reaction channels. In our previous work, high-valent cobalt-oxo intermediates were achieved by using linear alkylbenzene sulfonate as the fifth ligand on cellulosic fiber-boned cobalt phthalocyanine and these displayed good oxidation capacity under neutral conditions [42]. Our earlier study found that the MWCNTs-CoTAPc/H2O2 system, which was dominated by hole oxidation, exhibited a relatively high catalytic activity for the oxidative removal of adsorbed dyes at neutral pH [28, 29] and that this corresponds to the catalytic performance of the OMC-CoTAPc-EPTAC/H2O2 system. Based on these considerations, we infer that high-valent cobalt-oxo intermediates and generated holes were possible oxidation species during the catalytic reaction, which caused the OMC-CoTAPc-EPTAC/H2O2 system to exhibit a higher catalytic efficiency and better stability.Figure 12
DMPO spin-trapping EPR spectra in aqueous (a) and ethanol (b) solution containing AR1 (0.05 mM) ([OMC-CoTAPc-EPTAC] = 0.4 g/L, [H2O2] = 15 mM, and [DMPO] = 20 mM).
(a)
(b)The possible pathways for the oxidation of AR1 in this catalytic system are shown in Figure13. (a) In the OMC-CoTAPc-EPTAC/H2O2 system, CoTAPc is oxidized by the coordination behavior between H2O2 and the central cobalt ion. Then the relatively high Fermi level of OMC can provide electrons for the reduction of oxidized CoTAPc and the hole-doped OMC is obtained, achieving the rapid oxidation of the target substrate. (b) At the same time, the center cobalt ion of CoTAPc is coordinated axially by OOH−. The heterolytic cleavage of the O-O bond results in the generation of Co(IV)=O with a high oxidation ability to the substrate.Figure 13
The possible pathways for the oxidation of AR1 in this catalytic system ((a) generation of holes in OMC; (b) generation of high-valent cobalt-oxo species).


## 3.1. Characterization of OMC-CoTAPc-EPTAC

The UV-Vis absorption spectra of CoTAPc, OMC, and OMC-CoTAPc-EPTAC are shown in Figure1. The CoTAPc spectrum shows a sharp absorption peak at 705 nm and a weaker absorption peak at 412 nm because of the strong electron-donating property of the amino group on the CoTAPc ring. The spectrum does not show any absorption peaks at 400–800 nm for OMC, whereas the OMC-CoTAPc-EPTAC spectrum shows a broad absorption peak at 600–750 nm, which may be explained by the strong electronic interaction between CoTAPc and OMC. Therefore, we conclude that CoTAPc was supported on the OMC.Figure 1
UV-Vis absorption spectra for OMC, CoTAPc, and OMC-CoTAPc-EPTAC (in DMF).The textural properties of OMC and OMC-CoTAPc-EPTAC were investigated using high-resolution TEM and N2 absorption. The OMC surface morphology before and after modification with CoTAPc-EPTAC was studied by TEM (Figure 2). The compounds possessed a well-defined ordered mesoporous structure with uniform size, and the ordered mesostructure of OMC was rarely destroyed after modification with CoTAPc-EPTAC. The pore diameter is not visible in the TEM micrographs because of the superimposition of the three-dimensional mesopore system [34–36]. N2 adsorption/desorption isotherms were used to explore the pore structure and adsorption capacity of the samples further. Figure 3(a) showed an obvious increase in N2 uptake especially in the low-pressure region, which indicates the formation of highly porous carbon. A typical type IV isotherm with H2 hysteresis loops and a significant capillary condensation step for relative pressures of 0.45–0.8 was obtained, which suggests that the mesopore size was almost identical as shown by the corresponding pore size distribution analysis (Figure 3(b)). This confirmed that OMC and OMC-CoTAPc-EPTAC had a narrow ~6 nm pore size distribution in the mesopore range. According to the calculation results of the N2 adsorption/desorption isotherms, the BET surface area of OMC is 636 m2/g, which decreased to 530 m2/g after bonding cobalt tetraaminophthalocyanine. This could be explained by the fact that the interior OMC space was occupied partially by the CoTAPc-EPTAC. The ordered OMC-CoTAPc-EPTAC mesoporous structure was maintained and the OMC support exhibited relatively high adsorption capacity. This was consistent with the TEM observation.Figure 2
(a) and (b) TEM image of OMC calcined at 850°C. (c) and (d) TEM image of OMC-CoTAPc-EPTAC.
(a)
(b)
(c)
(d)Figure 3
(a) N2 sorption isotherm and (b) pore size distribution of OMC and OMC-CoTAPc-EPTAC.
(a)
(b)Additional structural information was obtained from the powder XRD analysis (Figure4). OMC has an XRD pattern with a sharp diffraction peak at 2θ = 24° and weaker peaks at 2θ = 45° that correspond to the (002) and (101) planes of carbon, respectively [37], which means that OMC had some ordered graphite crystallites after high-temperature carbonization. Figure 4 also shows that the diffraction peak of CoTAPc was centered at 2θ = 28°. The diffraction pattern of OMC-CoTAPc-EPTAC was similar to that of OMC, and the supported catalyst had no noticeable effect on the diffraction peaks, except that they were slightly weaker, probably because the crystalline structure of the OMC support was partially destroyed. These observations suggest that the CoTAPc had little influence on the OMC structure. To evaluate the thermal stability of the catalyst, TGA was carried out in N2 (Figure 5). OMC has an excellent thermal stability from 50 to 800°C. CoTAPc mass loss starts to occur at 200°C, and eventually some thermal decomposition will result. The mass loss curve of OMC-CoTAPc-EPTAC lay between that of OMC and CoTAPc, which means that the thermal stability of CoTAPc improved by introducing OMC as the support.Figure 4
XRD patterns for OMC, CoTAPc, and OMC-CoTAPc-EPTAC.Figure 5
TGA for OMC, CoTAPc, and OMC-CoTAPc-EPTAC.


## 3.2. Oxidative Degradation of AR1

To investigate the catalytic performance of OMC-CoTAPc-EPTAC, AR1 in aqueous solution was used as the model for catalytic oxidation. Figure6 shows that AR1 cannot be oxidized directly with H2O2 alone. In our previous work, we found that even in the presence of H2O2 and CoTAPc, almost no removal of target dyes resulted [28]. OMC-supported CoTAPc (OMC-CoTAPc) could only adsorb dyes fractionally, which resulted in a low oxidative removal rate of dyes with H2O2 [38]. Figure 6 shows that in the presence of OMC-CoTAPc-EPTAC alone, a clear decrease in AR1 resulted and the removal rate remained constant because the adsorption process attained equilibrium in a short time. The AR1 concentration decreased significantly when AR1 was exposed to OMC-CoTAPc-EPTAC and H2O2 together. These results suggest that the introduction of EPTAC into the catalyst induced a positive effect on improving the oxidative degradation efficiency of AR1 by facilitating the adsorption of dye into OMC. According to the previously described experiments, we infer that the removal of AR1 in the OMC-CoTAPc-EPTAC/H2O2 system included two processes: adsorption of AR1 into the OMC-CoTAPc-EPTAC and catalytic oxidation of the adsorbed AR1. Figure 7 shows that AR1 adsorption reached equilibrium in a short time without H2O2. Its concentration decreased significantly once H2O2 was added into the adsorption equilibrium system, which indicates that rapid and efficient oxidation of AR1 could be achieved when H2O2 was present in the reaction system and the adsorbed AR1 consumption was replenished continuously from AR1 in the bulk solution until the removal was complete. It is a great achievement that dyes could be enriched rapidly into OMC-CoTAPc-EPTAC and be decomposed in situ. Therefore, we conclude that the OMC-CoTAPc-EPTAC had high-level catalytic activity for AR1 oxidation, and OMC with a large adsorption capacity played a critical role during the degradation.Figure 6
Concentration changes of AR1 (0.05 mM) under different conditions ([OMC-CoTAPc-EPTAC] = 0.4 g/L, [H2O2] = 15 mM, pH 7, and 50°C).Figure 7
Concentration changes of AR1 (0.05 mM) after adsorption equilibrium with or without H2O2 ([OMC-CoTAPc-EPTAC] = 0.4 g/L, [H2O2] = 15 mM, pH 7, and 50°C).Temperature is an important factor that influences the catalytic reaction rate. To investigate the effect of reaction temperature on the OMC-CoTAPc-EPTAC/H2O2 catalytic system, the catalytic oxidation of AR1 was carried out at different temperatures with the result presented in Figure 8. In the presence of H2O2, OMC-CoTAPc-EPTAC could catalyze the oxidative removal of AR1 from 25 to 75°C, and the removal rate of AR1 increased as the reaction temperature increased. This may occur because the thermal energy of the AR1 molecules increased with increase in temperature, which resulted in a higher molecular heat movement speed. It was conducive to dye diffusion into the catalytic active sites, and enhanced the reaction rate. Based on the time courses of ln(C
0/C) at four different temperatures, an Arrhenius plot of ln
⁡
k-1/T is shown in Figure 9, and the activation energy of the oxidative degradation of AR1 in the OMC-CoTAPc-EPTAC/H2O2 system was 49.8 kJ/mol as calculated from the slope of the straight line. In comparison with common catalytic systems [39, 40], the system with a lower activation energy exhibited a high oxidative removal efficiency for AR1 at high temperature.Figure 8
Effect of temperature on catalytic oxidation of AR1 (0.05 mM) ([OMC-CoTAPc-EPTAC] = 0.4 g/L, [H2O2] = 15 mM, and pH 7).Figure 9
Arrhenius plots ofln
⁡
k-1/T with OMC-CoTAPc-EPTAC as catalyst.H2O2 is an environmentally friendly reagent and is used in almost all industrial fields. A reduction in H2O2 dosage is commercially important in chemical reaction processes. The effect of H2O2 dosage on AR1 removal efficiency was explored by varying the initial H2O2 concentration from 7.5 to 100 mM with results as shown in Figure 10. An increase in the initial H2O2 concentration led to a higher rate of AR1 degradation, and when increased above 15 mM, the AR1 concentration decreased sharply. Based on the H2O2 utilization efficiency, a H2O2 concentration of 15 mM was selected as the optimum H2O2 dosage. Compared with the single-walled carbon nanotube-supported CoTAPc (MWCNTs-CoTAPc)/H2O2 catalytic system reported in our previous paper [28], OMC-CoTAPc-EPTAC had a higher catalytic oxidation efficiency at a lower H2O2 concentration. This may be because the higher H2O2 utilization efficiency in the OMC-CoTAPc-EPTAC/H2O2 catalytic system could be ascribed to a different H2O2 activation mechanism or MWCNTs-CoTAPc served as an interfacial catalyst. Substrate adsorption and oxidation occurred at the MWCNT surface, whereas in the OMC-CoTAPc-EPTAC/H2O2 system, a reaction was required for the target substrates and H2O2 to enter into the interior of the OMC support, which significantly improved the H2O2 utilization in this catalytic system.Figure 10
Effect of initial H2O2 concentration on catalytic oxidation of AR1 (0.05 mM) ([OMC-CoTAPc-EPTAC] = 0.4 g/L, pH 7, and 50°C).Stability is another significant issue for catalyst use in practical applications. However, to the best of our knowledge, the supported MPcs usually lose partial activity because barriers to oxidation intermediates are generated in the reaction, or they may suffer from autocatalytic decomposition when the catalytic oxidation reaction is dominated by nonselectiveO
H
∙ [41], which results in a loss of catalytic activity. To study the catalyst stability, it is necessary to carry out continuous cyclic oxidation experiments of AR1 in the catalytic system that involves OMC-CoTAPc-EPTAC and H2O2. Figure 11 shows that the oxidative removal rate of AR1 was ~98% after the first cycle, and the rate was still high with no obvious decrease after five cycles of reuse. This highlights the excellent catalytic properties and good self-reliance regeneration ability of OMC-CoTAPc-EPTAC in repetitive experiments. These findings show that OMC introduction improves the catalytic activity and stability of CoTAPc and provides a transport channel for degradation products, guaranteeing constant substrate adsorption and oxidation, and achieves catalyst recycling.Figure 11
Cyclic catalytic oxidation of AR1 (0.05 mM), 5 mM H2O2 addition at each cycle after the first cycle ([OMC-CoTAPc-EPTAC] = 0.4 g/L, [H2O2] = 15 mM, pH 7, and 50°C).


## 3.3. Analysis of Catalytic Mechanism

A catalytic mechanism that is dominated by hydroxyl radical (O
H
∙) oxidation, high-valency metal-oxo species oxidation, or hole oxidation in the activated H2O2 systems has been reported. To obtain deeper insight into the possible catalytic mechanism of OMC-CoTAPc-EPTAC in activating H2O2, the EPR technique (with DMPO) was used with results shown in Figure 12. Nearly no DMPO-O
H
∙ and DMPO-O
O
H
∙ signals were detected for AR1 in aqueous or methanol solution, which shows that O
H
∙ and O
O
H
∙ were not major intermediates of the catalytic reaction with OMC-CoTAPc-EPTAC. From the EPR results, we concluded that the catalytic oxidation of AR1 occurred through a nonradical pathway, which was different from the common CoTAPc system [30], where the introduction of OMC and the direct-bonding method were considered two key factors that influence the reaction channels. In our previous work, high-valent cobalt-oxo intermediates were achieved by using linear alkylbenzene sulfonate as the fifth ligand on cellulosic fiber-boned cobalt phthalocyanine and these displayed good oxidation capacity under neutral conditions [42]. Our earlier study found that the MWCNTs-CoTAPc/H2O2 system, which was dominated by hole oxidation, exhibited a relatively high catalytic activity for the oxidative removal of adsorbed dyes at neutral pH [28, 29] and that this corresponds to the catalytic performance of the OMC-CoTAPc-EPTAC/H2O2 system. Based on these considerations, we infer that high-valent cobalt-oxo intermediates and generated holes were possible oxidation species during the catalytic reaction, which caused the OMC-CoTAPc-EPTAC/H2O2 system to exhibit a higher catalytic efficiency and better stability.Figure 12
DMPO spin-trapping EPR spectra in aqueous (a) and ethanol (b) solution containing AR1 (0.05 mM) ([OMC-CoTAPc-EPTAC] = 0.4 g/L, [H2O2] = 15 mM, and [DMPO] = 20 mM).
(a)
(b)The possible pathways for the oxidation of AR1 in this catalytic system are shown in Figure13. (a) In the OMC-CoTAPc-EPTAC/H2O2 system, CoTAPc is oxidized by the coordination behavior between H2O2 and the central cobalt ion. Then the relatively high Fermi level of OMC can provide electrons for the reduction of oxidized CoTAPc and the hole-doped OMC is obtained, achieving the rapid oxidation of the target substrate. (b) At the same time, the center cobalt ion of CoTAPc is coordinated axially by OOH−. The heterolytic cleavage of the O-O bond results in the generation of Co(IV)=O with a high oxidation ability to the substrate.Figure 13
The possible pathways for the oxidation of AR1 in this catalytic system ((a) generation of holes in OMC; (b) generation of high-valent cobalt-oxo species).


## 4. Conclusions

We have obtained a novel catalyst with a positively charged quaternary ammonium salt chain (OMC-CoTAPc-EPTAC) by OMC bonding the CoTAPc-EPTAC. OMC with a tunable pore texture and ordered three-dimensional open channel offered a suitable environment for AR1 accessibility into the active sites. The introduction of OMC into the catalytic system had a “push” effect on the catalytic activity and stability. The higher adsorption capacity of OMC-CoTAPc-EPTAC toward negatively charged substrates was achieved by modifying CoTAPc with EPTAC, which resulted in significant improvement in catalytic efficiency for AR1 oxidation. As expected, the EPR results indicate that the catalytic oxidation of AR1 involved a nonradical mechanism, and the high-valent cobalt-oxo species and generated holes were predicted as appropriate active species. The OMC-CoTAPc-EPTAC/H2O2 system displayed a greater catalytic performance at lower H2O2 dosage and achieved a low cost and high efficiency for practical applications. The combination of adsorption enrichment and in situ catalytic oxidation provides a preferable technology for the treatment of organic pollutants in low concentrations.



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*Source: 6953587-2016-10-12.xml*