*Article* **Sedum Plumbizincicola Derived Functional Carbon for Activation of Peroxymonosulfate to Eliminate Bisphenol A: Performance and Reaction Mechanisms**

**Chao Liu 1,2,†, Zhenxiang Chen 3,†, Ruiqin Kang <sup>1</sup> , Yongsheng Niu 1,\*, Wenhui Su <sup>1</sup> , Xiaolong Wang <sup>1</sup> , Dayong Tian <sup>1</sup> and Ying Xu 2,\***


**Abstract:** Carbon-based functional materials are deemed to be excellent candidates to adsorb contaminants from wastewater, yet their catalytic roles in advanced oxidation processes (AOPs) are still ambiguous. Therefore, four functional carbons (SPFCx) were fabricated in this study under various pyrolysis temperatures by using Sedum plumbizincicola (SP) residues (a kind of phytoremediation plant) as the precursors. Notably, SPFC800 exhibited the best adsorption capacity (*q*<sup>e</sup> = 26.081 mg g−<sup>1</sup> ) toward bisphenol A (BPA) due to its having the largest specific surface area (121.57 m<sup>2</sup> g −1 ). By injecting peroxymonosulfate (PMS, 5.0 mM), BPA (10 mg L−<sup>1</sup> ) could be completely removed within 70 min. More importantly, the BPA removal was stable and effective even in complex wastewater. Interestingly, radicals played minor roles in the SPFC800/PMS system, while nonradical mechanisms (i.e., <sup>1</sup>O<sup>2</sup> and electron-transfer regime) were responsible for the BPA elimination, which was verified by quenching tests, solvent exchange experiments (H2O2→D2O), and electrochemical experiments. Overall, this work may provide a facile and green method for BPA contaminated-wastewater purification and promote the application of AOPs in environmental remediation.

**Keywords:** peroxymonosulfate; pre-adsorption; degradation; nonradical oxidation

### **1. Introduction**

Phytoremediation technology is deemed to be a green environmental protection technology for soil remediation [1–3]. Notably, the core principle of this method is to use hyperaccumulators (e.g., pteris vittata, violabaoshaensis, and ellshohzia splendens) to concentrate the metals from the contaminated soil and then harvest the plants to remove heavy metal pollutants [4,5]. As a result, large amounts of plant-based wastes containing heavy metals are produced during the phytoremediation processes. Notably, these harvests often contain very high concentrations of heavy metals, which may become new sources of pollution upon improper disposal. Therefore, the safe disposal of the harvest is deemed to be an important issue [6,7]. Up until now, several methods (e.g., liquid extraction, landfill, composting treatment, and thermal treatment) have been developed to treat the harvest in the previous studies. Although liquid-phase extraction can effectively extract heavy metals from the plants, the generated extraction liquid needs to be treated, which may cause high treatment costs. In addition, the landfill may take up a lot of land resources, and the ultra-high concentrations of heavy metals in the harvest may migrate into the leachate, which may cause secondary pollution to the soil and groundwater. Therefore, developing an effective, green, and promising technology for the reuse of hyperaccumulator residues is urgent.

**Citation:** Liu, C.; Chen, Z.; Kang, R.; Niu, Y.; Su, W.; Wang, X.; Tian, D.; Xu, Y. Sedum Plumbizincicola Derived Functional Carbon for Activation of Peroxymonosulfate to Eliminate Bisphenol A: Performance and Reaction Mechanisms. *Coatings* **2022**, *12*, 1892. https://doi.org/10.3390/ coatings12121892

Academic Editor: Alexandru Enesca

Received: 27 October 2022 Accepted: 28 November 2022 Published: 5 December 2022

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**Copyright:** © 2022 by the authors. Licensee MDPI, Basel, Switzerland. This article is an open access article distributed under the terms and conditions of the Creative Commons Attribution (CC BY) license (https:// creativecommons.org/licenses/by/ 4.0/).

Recently, thermal treatment technology has been widely recognized. In particular, thermal treatment can prevent metal leaching, which is conducive to harmless disposal. Notably, value-added functional carbon (FC) can be obtained by pyrolyzing these plant residues under oxygen-limited conditions, which may further be used for water decontamination [8–11]. To our satisfaction, the inherent heavy metals can be converted into metal oxide nanoparticles, which can reduce the release of metallic pollutants [12]. Meanwhile, metal species can tailor the structures of carbon materials [13–16]. Recently, FC has been successfully applied for contaminants degradation in advanced oxidation processes (AOPs) by coupling with various oxidants (e.g., hydrogen peroxide (H2O2), periodate (PI), peroxymonosulfate (PMS), and peracetic acid (PAA)) [17–21]. As a result, the specific roles of carbon materials in AOPs were tentatively investigated in previous studies [22–25]. For instance, peroxydisulfate (PDS) could effectively be activated to produce reactive oxygen species (ROS, e.g., SO<sup>4</sup> <sup>−</sup>, O<sup>2</sup> <sup>−</sup> and <sup>1</sup>O2) with the assistance of FC prepared by peanut shells, corn straw, and water hyacinth [26–30]. Despite many attempts, the mechanism of interaction between target pollutants, oxidants, and carbon materials in heterogeneous AOPs remained unclear [31–33].

Due to the large scale of bisphenol A (BPA) utilization, BPA contamination can be found in various environmental compartments (e.g., air, water, and soil), which may cause disease by disrupting the human endocrine system [34]. To this end, several methods (e.g., adsorption, flocculation, and biological treatment) are used for BPA removal [35–38]. Notably, AOPs have been considered as promising methods for BPA elimination in recent years. For example, a series of photocatalysts were designed and applied for the photocatalytic degradation of BPA [34]. However, the constant input of energy may increase the cost of the technology; thus carbon-catalyzed AOPs are deemed to be the promising candidates for pollutants removal.

In this study, Sedum plumbizincicola, which is often used to concentrate heavy metals from contaminated soil, was used for the FC preparation. BPA, which is widely used in the manufacturing industry, was selected as the target pollutant. First, the apparent morphology of the FC was characterized. After that, the adsorptive behaviors of BPA on FC were analyzed by fitting with the kinetic models. Then, the BPA removal was investigated in several AOPs (i.e., FC/PMS, FC/PDS, and FC/H2O<sup>2</sup> systems). Furthermore, the BPA degradation mechanism was systematically explored by quenching tests, solvent exchange tests, and electrochemical experiments. Additionally, the catalytic activity and stability of the FC were also investigated in real water samples. Overall, this work not only provides a facile and low-cost method for the preparation of functional materials toward environmental remediation but also deepens the understanding of carbon-catalyzed AOPs.

#### **2. Materials and Methods**

#### *2.1. Materials*

The BPA (≥99%) was purchased from Aladdin. D2O (99.9%) was purchased from Macklin, Nanjing, China. Quenching agents (e.g., methanol (MeOH, ≥99.9%), L-histidine (*L-his*, 99%), Furfuryl alcohol (FFA, 98%) and *Tert*-butanol (TBA, 99%)) were obtained from Aladdin, Nanjing, China. Other chemicals were at least analytical grade and used without further purification. Ultrapure water (18.25 MΩ) was produced by Spring-S60i + PALL system. In addition, a multifunctional crusher (LINGSUM, 1000C) was used for grinding Sedum plumbizincicola.

#### *2.2. Methods*

#### 2.2.1. Preparation and Characterization of FC

Sedum plumbizincicola, a kind of hyperaccumulator collected in Yunnan, China, was used for the FC preparation. Firstly, sedum plumbizincicola was washed with pure water and then dried at 60 ◦C for 12 h. After that, the dried sedum plumbizincicola was ground to powder, transferred into a crucible, and carbonized in the muffle furnace at the required temperature (i.e., 500 ◦C, 600 ◦C, 700 ◦C, and 800 ◦C) for 2 h. Then, the black solid block was

ground to desired size by using a 100-mesh sieve, washed with the pure water, and dried at 60 ◦C (about 4 h) until constant weight. The final products were designated as SPFCx, in which x was the annealing temperature (i.e., 500 ◦C, 600 ◦C, 700 ◦C, and 800 ◦C). In addition, Field emission scanning electron microscopy (SEM, Fei Quanta 400 FEG, Hillsboro, OR, USA) was used to determine the morphologies of SPFCx. The specific surface area (SBET) was calculated according to the Brunauer-Emmett-Teller equation (Micromeritics ASAP 2020, Micromeritics Instrument Corporation, Norcross, GA, USA).

#### 2.2.2. Adsorption

Adsorption was carried out in several conical flasks (100 mL) that contained 50 mL of BPA solution (10 mg L−<sup>1</sup> ) and 0.2 g L−<sup>1</sup> of SPFCx. At predetermined time intervals, samples were collected, quenched by MeOH and then analyzed by liquid chromatography. The adsorption behaviors of BPA on SPFCx were determined by kinetic studies. Two kinetic models (i.e., pseudo-first and pseudo-second order kinetic models) were selected to analyze the adsorptive behaviors of BPA on SPFCx:

$$\text{Pseudo first} - \text{order kinetic model } : q\_{\text{l}} = q\_{\text{e}} \left( 1 - e^{-k\_{\text{l}} \text{t}} \right) \tag{1}$$

$$\text{Pseudo second} - \text{order kinetic model}: q\_{\text{t}} = \frac{k\_2 q\_{\text{e}}^2 \text{t}}{1 + k\_2 q\_{\text{e}} \text{t}} \tag{2}$$

where, *q*<sup>e</sup> and *q*<sup>t</sup> are the adsorption amounts of BPA on SPFCx at equilibrium and time *t* (mg g−<sup>1</sup> ), respectively. *k*<sup>1</sup> (min−<sup>1</sup> ) and *k*<sup>2</sup> (g mg−<sup>1</sup> min−<sup>1</sup> ) are the corresponding adsorption rate constants, respectively.

#### 2.2.3. Catalytic Degradation of BPA

BPA, an endocrine disruptor, was selected as the target contaminant to assess the catalytic performance of SPFCx. The experiments were conducted as follows: 10 mg SPFCx was first added into the BPA solution (10 mg L−<sup>1</sup> ) and stirred for 40 min to achieve adsorption equilibrium. Then, 5 mM oxidants (e.g., PMS, PDS, and H2O2) were injected into the mixture to initiate the catalytic reaction. At predetermined time intervals, 0.5 mL solution was withdrawn, filtered with a 0.2 mm filter to remove the solid catalyst, and quenched with 0.5 mL methanol for analysis.

The elimination of BPA was also tested in real water matrixes (i.e., pure water (PW), river water (RW) from Taihu in Wuxi, chemical wastewater (WW) collected from a sewage treatment plant in Anyang, and tap water (TW)).

#### 2.2.4. Analytical Methods

The concentration of BPA could be detected by Agilent 1260 High Performance Liquid Chromatography (HPLC, Agilent, Beijing, China) equipped with a reversed-phase C18 column (5 µm, 4.6 × 250 mm). The mobile phase contained water and methanol (15/85, *v*/*v*). The flow rate was 1.0 mL min−<sup>1</sup> and the injection volume was 20 µL. Electrochemical experiments were performed on a CHI660E electrochemical workstation and the details of the analytical methods were provided in the Supplementary Materials Text S1. In addition, the <sup>1</sup>O<sup>2</sup> in SPFC800/PMS systems was identified via electron paramagnetic resonance (EPR, Bruker A320 spectrometer, Bruker, Beijing, China) analysis.

#### **3. Results and Discussion**

#### *3.1. Characterizations*

In order to evaluate the apparent morphology of the prepared SPFCx, SEM images were conducted. As depicted in Figure 1, the particle size of SPFC500 (Figure 1a) was relatively larger than that of the SPFC800 (Figure 1b), indicating that higher pyrolysis temperature might be beneficial for the complete decomposition of the precursors and the finer particle size may endow SPFC800 with larger SBET and more active sites. It was

*Coatings* **2022**, *12*, x FOR PEER REVIEW 4 of 12

**3. Results and Discussion** 

*3.1. Characterizations* 

reported that higher surface areas and more adsorptive sites were beneficial for removing contaminants [39–42]. ported that higher surface areas and more adsorptive sites were beneficial for removing contaminants [39–42].

In order to evaluate the apparent morphology of the prepared SPFCx, SEM images were conducted. As depicted in Figure 1, the particle size of SPFC500 (Figure 1a) was relatively larger than that of the SPFC800 (Figure 1b), indicating that higher pyrolysis temperature might be beneficial for the complete decomposition of the precursors and the finer particle size may endow SPFC800 with larger SBET and more active sites. It was re-

**Figure 1.** SEM images of SPFC500 (**a**) and SPFC800 (**b**). **Figure 1.** SEM images of SPFC500 (**a**) and SPFC800 (**b**).

In order to further verify the enlargement of surface area with the increasing pyrolysis temperature, the nitrogen adsorption method was carried out to measure the SBET of SPFCx. The structure information of SPFCx was summarized in Table 1. The results demonstrated that with the increase of annealing temperature (from 500 to 800 °C), the SBET significantly increased from 36.09 to 121.57 m2 g−1, indicating more adsorptive sites were created, which may be beneficial for accumulating the BPA from the solution. The largest SBET of SPFC800 might be owing to the complete decomposition of contents (e.g., fatty acid esters) in precursors. Moreover, the pore volume of SPFCx also increased (from 0.0277 to 0.0847 cm3 g−1) with increasing pyrolysis temperature, which might be beneficial for producing more active sites. The average pore diameters of SPFCx were between 3.651 and 3.977 nm, suggesting that SPFCx could produce abundant mesoporous pores. Notably, much more meso/micro pores might be formed during higher pyrolysis temperature as evidenced by the smaller pore diameter. The well-interconnected porous structures may contain plenty of nano-spaces/channels, which might be beneficial for the formation of nanoconfinement effects, boosting BPA removal [43,44]. In order to further verify the enlargement of surface area with the increasing pyrolysis temperature, the nitrogen adsorption method was carried out to measure the SBET of SPFCx. The structure information of SPFCx was summarized in Table 1. The results demonstrated that with the increase of annealing temperature (from 500 to 800 ◦C), the SBET significantlyincreased from 36.09 to 121.57 m<sup>2</sup> <sup>g</sup> −1 , indicating more adsorptive sites were created,which may be beneficial for accumulating the BPA from the solution. The largest SBET of SPFC800 might be owing to the complete decomposition of contents (e.g., fatty acid esters) in precursors. Moreover, the pore volume of SPFCx also increased (from 0.0277 to 0.0847 cm<sup>3</sup> g −1 ) with increasing pyrolysis temperature, which might be beneficial for producing more active sites. The average pore diameters of SPFCx were between 3.651 and 3.977 nm, suggesting that SPFCx could produce abundant mesoporous pores. Notably, much more meso/micro pores might be formed during higher pyrolysis temperature as evidenced by the smaller pore diameter. The well-interconnected porous structures may contain plenty of nano-spaces/channels, which might be beneficial for the formation of nanoconfinement effects, boosting BPA removal [43,44].


**Table 1.** The basic information of SPFCx. **Table 1.** The basic information of SPFCx.

#### *3.2. Adsorption*

*3.2. Adsorption*  As shown in Figure 2a,b, BPA molecule could quickly accumulate on SPFCx surface As shown in Figure 2a,b, BPA molecule could quickly accumulate on SPFCx surface within 30 min.

within 30 min. Notably, better correlation coefficients (Table 2, R<sup>2</sup> > 0.982) were obtained by fitting with the pseudo-second-order kinetic model, suggesting the adsorption process might be chemisorption. More specifically, SPFC800 exhibited the highest *q*<sup>e</sup> value of 26.081 mg g−<sup>1</sup> , followed with SPFC700 (21.158 mg g−<sup>1</sup> ), SPFC600 (18.619 mg g−<sup>1</sup> ), and SPFC500 (18.308 mg g−<sup>1</sup> ), indicating the pyrolysis temperature was beneficial for enhancing the adsorption affinity. Thus, it could be speculated that a larger SBET would be obtained under high pyrolysis temperature, which would be beneficial for contaminant adsorption. As depicted in Figure 2c, a good linear relationship between *q*<sup>e</sup> and SBET (R<sup>2</sup> = 0.941) was observed, further confirming that the adsorption of BPA was determined by the specific surface area of SPFCx.

**Figure 2.** pseudo first (**a**); pseudo second (**b**) order kinetic models; and the correlation analysis between *q*e and SBET (**c**). (Experimental conditions: [BPA] = 10 mg L<sup>−</sup>1, and [SPFCx] = 0.2 g L<sup>−</sup>1). **Figure 2.** Pseudo first (**a**); pseudo second (**b**) order kinetic models; and the correlation analysis between *q*<sup>e</sup> and SBET (**c**). (Experimental conditions: [BPA] = 10 mg L−<sup>1</sup> , and [SPFCx] = 0.2 g L−<sup>1</sup> ).


Notably, better correlation coefficients (Table 2, R2 > 0.982) were obtained by fitting **Table 2.** The parameters obtained by fitting with adsorption kinetic equation.

#### confirming that the adsorption of BPA was determined by the specific surface area of SPFCx. *3.3. Catalytic Degradation Performance*

**Table 2.** The parameters obtained by fitting with adsorption kinetic equation. **Biochar Pseudo First-Order Pseudo Second-Order**  *q***<sup>e</sup>** *k***1 R2** *q***<sup>e</sup>** *k***2 R2** SPFC500 17.771 (0.408) 0.862 0.951 18.308 (0.302) 0.0847 0.982 SPFC600 18.084 (0.411) 0.876 0.951 18.619 (0.307) 0.0855 0.982 SPFC700 20.399 (0.509) 0.674 0.949 21.158 (0.323) 0.0521 0.985 SPFC800 25.184 (0.624) 0.724 0.944 26.081 (0.418) 0.0461 0.983 Although H2O<sup>2</sup> was a traditional and effective oxidant that was usually utilized in Fenton and/or Fenton-Like processes, it could hardly oxidize the BPA even with the help of SPFCx (Figure 3a). The removal of BPA in such an oxidation process was almost attributed to the adsorption by SPFCx. However, a moderate synergistic effect was observed between BPA adsorption and BPA oxidation in SPFCx/PDS systems (Figure 3b). Notably, BPA was more rapidly removed by SPFCx/PMS systems (especially SPFC800), which might be attributed to the non-symmetrical structure of PMS, and thus it was easier to be decomposed (Figure 3c). Due to the highest BPA removal rates in SPFC800/PMS systems, the subsequent BPA degradation experiments would be performed in the SPFC800-induced systems (Figure 3d). *Coatings* **2022**, *12*, x FOR PEER REVIEW 6 of 12

**Figure 3.** Catalytic degradation of BPA in SPFCx/H2O2 (**a**); SPFCx/PDS (**b**); SPFCx/PMS (**c**); systems, respectively, and the removal efficiencies of BPA in various oxidation process (**d**). (Experimental conditions: [BPA] = 10 mg L<sup>−</sup>1, [Oxidant] = 5 mM, and [SPFCx] = 0.2 g L<sup>−</sup>1). **Figure 3.** Catalytic degradation of BPA in SPFCx/H2O<sup>2</sup> (**a**); SPFCx/PDS (**b**); SPFCx/PMS (**c**); systems, respectively, and the removal efficiencies of BPA in various oxidation process (**d**). (Experimental conditions: [BPA] = 10 mg L−<sup>1</sup> , [Oxidant] = 5 mM, and [SPFCx] = 0.2 g L−<sup>1</sup> ).

SPCF800/PMS system, quenching experiments were conducted first to demonstrate the involved ROS for BPA removal. Apparently, with the injection of MeOH (Figure 4a, from 500 to 2000 mM), the removal efficiency of BPA was only slightly inhibited, indicating that BPA degradation was not dependent on the radicals (i.e., SO4− and ·OH). Furthermore, a similar phenomenon was observed by using TBA (quencher for ·OH, from 100 to 1000 mM) as the quenching agent, confirming the minor role of ·OH in BPA elimination (Figure 4b). Nevertheless, both *L-his* and FFA (classic quenchers for 1O2) could significantly inhibit the BPA removal, which suggested that 1O2 might be obligated to the BPA removal (Figure 4c,d). In order to further confirm the existence of 1O2 in SPFC800/PMS system, BPA degradation was conducted in D2O, which could prolong the half-life of 1O2. As shown in the inset of Figure 4d, BPA removal was boosted in D2O, demonstrating the vital roles of 1O2

*3.4. Catalytic Mechanism* 

in BPA elimination.

#### *3.4. Catalytic Mechanism*

In order to reveal why BPA could be quickly and effectively removed in SPCF800/PMS system, quenching experiments were conducted first to demonstrate the involved ROS for BPA removal. Apparently, with the injection of MeOH (Figure 4a, from 500 to 2000 mM), the removal efficiency of BPA was only slightly inhibited, indicating that BPA degradation was not dependent on the radicals (i.e., SO<sup>4</sup> <sup>−</sup> and ·OH). Furthermore, a similar phenomenon was observed by using TBA (quencher for ·OH, from 100 to 1000 mM) as the quenching agent, confirming the minor role of ·OH in BPA elimination (Figure 4b). Nevertheless, both *L-his* and FFA (classic quenchers for <sup>1</sup>O2) could significantly inhibit the BPA removal, which suggested that <sup>1</sup>O<sup>2</sup> might be obligated to the BPA removal (Figure 4c,d). In order to further confirm the existence of <sup>1</sup>O<sup>2</sup> in SPFC800/PMS system, BPA degradation was conducted in D2O, which could prolong the half-life of <sup>1</sup>O2. As shown in the inset of Figure 4d, BPA removal was boosted in D2O, demonstrating the vital roles of <sup>1</sup>O<sup>2</sup> in BPA elimination. *Coatings* **2022**, *12*, x FOR PEER REVIEW 7 of 12 *Coatings* **2022**, *12*, x FOR PEER REVIEW 7 of 12

**Figure 4.** The effects of several quenching agents (i.e., MeOH (**a**); TBA (**b**); *L-his* (**c**); and FFA (**d**)) on BPA removal in SPFC800/PMS system and the solvent exchange experiments (inset of d). (Experimental conditions: [BPA] = 10 mg L<sup>−</sup>1, [Oxidant] = 5 mM, [SPFCx] = 0.2 g L<sup>−</sup>1, [MeOH] = 0–2000 mM, [TBA] = 0–1000 mM, [*L-his*] = 0–50 mM, and [FFA] = 0–25 mM). **Figure 4.** The effects of several quenching agents (i.e., MeOH (**a**); TBA (**b**); *L-his* (**c**); and FFA (**d**)) on BPA removal in SPFC800/PMS system and the solvent exchange experiments (inset of d). (Experimental conditions: [BPA] = 10 mg L−<sup>1</sup> , [Oxidant] = 5 mM, [SPFCx] = 0.2 g L−<sup>1</sup> , [MeOH] = 0–2000 mM, [TBA] = 0–1000 mM, [*L-his*] = 0–50 mM, and [FFA] = 0–25 mM). **Figure 4.** The effects of several quenching agents (i.e., MeOH (**a**); TBA (**b**); *L-his* (**c**); and FFA (**d**)) on BPA removal in SPFC800/PMS system and the solvent exchange experiments (inset of d). (Experimental conditions: [BPA] = 10 mg L<sup>−</sup>1, [Oxidant] = 5 mM, [SPFCx] = 0.2 g L<sup>−</sup>1, [MeOH] = 0–2000 mM, [TBA] = 0–1000 mM, [*L-his*] = 0–50 mM, and [FFA] = 0–25 mM).

The EPR test was further conducted to verify the generation of 1O2 in SPFC800/PMS system by using TEMP as the spin-trapping agent (Figure 5). A distinctive triplet signal was detected upon the injection of SPFC800 into the PMS solution, which indicated the existence of 1O2, matching well with the quenching results. The EPR test was further conducted to verify the generation of <sup>1</sup>O<sup>2</sup> in SPFC800/PMS system by using TEMP as the spin-trapping agent (Figure 5). A distinctive triplet signal was detected upon the injection of SPFC800 into the PMS solution, which indicated the existence of <sup>1</sup>O2, matching well with the quenching results. The EPR test was further conducted to verify the generation of 1O2 in SPFC800/PMS system by using TEMP as the spin-trapping agent (Figure 5). A distinctive triplet signal was detected upon the injection of SPFC800 into the PMS solution, which indicated the existence of 1O2, matching well with the quenching results.

**Figure 5.** Electron paramagnetic resonance (EPR) spectra of PMS activation by SPFC800: TEMP-1O2. **Figure 5.** Electron paramagnetic resonance (EPR) spectra of PMS activation by SPFC800: TEMP-1O2. **Figure 5.** Electron paramagnetic resonance (EPR) spectra of PMS activation by SPFC800: TEMP-1O2.

SPFC500, indicating the better conductivity of SBC800, and thus electrons could be easier to transfer on SPFC800 surface than SPFC500. The LSV and I-T curves of SPFC800 were also carried out. As shown in Figure 6b, the current density increased upon the injection of PMS, suggesting the rapid interaction between PMS and SPFC800. Furthermore, another obviously increased current density was detected after adding BPA, which might be owing to the electron transfer among BPA (electron donor), PMS (electron acceptor), and SPFC800 (electric conductor). Similarly, as illustrated in Figure 6c, the current responses showed obvious variations upon the injection of PMS and BPA, revealing the vital role of electron transfer mechanism. The potential of the SPFCx surface was characterized to reveal the electron transfer regime in depth. It was well accepted that the PMS could

SPFC500, indicating the better conductivity of SBC800, and thus electrons could be easier to transfer on SPFC800 surface than SPFC500. The LSV and I-T curves of SPFC800 were also carried out. As shown in Figure 6b, the current density increased upon the injection of PMS, suggesting the rapid interaction between PMS and SPFC800. Furthermore, another obviously increased current density was detected after adding BPA, which might be owing to the electron transfer among BPA (electron donor), PMS (electron acceptor), and SPFC800 (electric conductor). Similarly, as illustrated in Figure 6c, the current responses showed obvious variations upon the injection of PMS and BPA, revealing the vital role of electron transfer mechanism. The potential of the SPFCx surface was characterized to reveal the electron transfer regime in depth. It was well accepted that the PMS could

In addition, electrochemical experiments were performed to verify the occurrence of

In addition, electrochemical experiments were performed to verify the occurrence of electron transfer regime. The EIS results could be used to reveal the resistance of the cat-

In addition, electrochemical experiments were performed to verify the occurrence of electron transfer regime. The EIS results could be used to reveal the resistance of the catalyst. As shown in Figure 6a, SPFC800 possessed a smaller semicircle diameter than SPFC500, indicating the better conductivity of SBC800, and thus electrons could be easier to transfer on SPFC800 surface than SPFC500. The LSV and I-T curves of SPFC800 were also carried out. As shown in Figure 6b, the current density increased upon the injection of PMS, suggesting the rapid interaction between PMS and SPFC800. Furthermore, another obviously increased current density was detected after adding BPA, which might be owing to the electron transfer among BPA (electron donor), PMS (electron acceptor), and SPFC800 (electric conductor). Similarly, as illustrated in Figure 6c, the current responses showed obvious variations upon the injection of PMS and BPA, revealing the vital role of electron transfer mechanism. The potential of the SPFCx surface was characterized to reveal the electron transfer regime in depth. It was well accepted that the PMS could first combine with the catalyst to form the catalyst-PMS complexes (C-PMS\*) with higher oxidation capacity. Notably, the C-PMS\* was formed first and the potential of C-PMS\* significantly increased with the higher dosage of PMS, revealing why BPA generally could be more effectively degraded with higher dosage of oxidants. According to the abovementioned analysis, the reaction mechanism between PMS, BPA, and SPFC800 was elucidated. Nonradicals were the dominant species in the catalytic process, and the SPFC800 could not only directly activate PMS to produce <sup>1</sup>O<sup>2</sup> but accumulate PMS to form the C-PMS\*, leading to effective BPA removal [24,45]. *Coatings* **2022**, *12*, x FOR PEER REVIEW 8 of 12 first combine with the catalyst to form the catalyst-PMS complexes (C-PMS\*) with higher oxidation capacity. Notably, the C-PMS\* was formed first and the potential of C-PMS\* significantly increased with the higher dosage of PMS, revealing why BPA generally could be more effectively degraded with higher dosage of oxidants. According to the abovementioned analysis, the reaction mechanism between PMS, BPA, and SPFC800 was elucidated. Nonradicals were the dominant species in the catalytic process, and the SPFC800 could not only directly activate PMS to produce 1O2 but accumulate PMS to form the C-PMS\*, leading to effective BPA removal [24,45].

**Figure 6.** Electrochemical impedance spectroscopy (EIS) of SPFC500 and SPFC800 (**a**); linear sweep voltammetry (LSV) of SPFC800 with/without PMS and BPA (**b**); I-T curves after adding PMS and BPA (**c**); and the change of SPFC800 potential with injection of different concentrations of PMS (**d**). **Figure 6.** Electrochemical impedance spectroscopy (EIS) of SPFC500 and SPFC800 (**a**); linear sweep voltammetry (LSV) of SPFC800 with/without PMS and BPA (**b**); I-T curves after adding PMS and BPA (**c**); and the change of SPFC800 potential with injection of different concentrations of PMS (**d**).

#### *3.5. Degradation in Real Water 3.5. Degradation in Real Water*

BPA degradation experiments were further conducted in SPFC800/PMS system by adding several interfering substances (i.e., HA, Cl−, and HCO3−). As shown in Figure 7a, the removal of BPA was slightly inhibited by adding 10 mM of HA, which might be owing to that HA could consume PMS and/or the ROS. Similarly, with the injection of HCO3−, the BPA degradation was inhibited, which could be due to that the ROS generated in PMS/SPFC800 system were converted into CO3•− with lower oxidation capacity (Equa-BPA degradation experiments were further conducted in SPFC800/PMS system by adding several interfering substances (i.e., HA, Cl−, and HCO<sup>3</sup> −). As shown in Figure 7a, the removal of BPA was slightly inhibited by adding 10 mM of HA, which might be owing to that HA could consume PMS and/or the ROS. Similarly, with the injection of HCO<sup>3</sup> −, the BPA degradation was inhibited, which could be due to that the ROS generated in PMS/SPFC800 system were converted into CO<sup>3</sup> •− with lower oxidation

tions (3) and (4)). Interestingly, BPA removal was slightly accelerated by adding 10 mM of Cl−, which was attributed to that Cl− may react with PMS and/or the ROS to form Cl•, capacity (Equations (3) and (4)). Interestingly, BPA removal was slightly accelerated by adding 10 mM of Cl−, which was attributed to that Cl− may react with PMS and/or the ROS to form Cl• , synergistically eliminating BPA (Equations (5)–(8)).

$$HCO^{\bullet} + HCO\_3^{-} \rightarrow H\_2O + CO\_3^{\bullet -} \tag{3}$$

$$\rm{SO\_4^{-}} + \rm{HCO\_3^{-}} \rightarrow \rm{SO\_4^{2-}} + \rm{HCO\_3^{-}}, k = 9.1 \times 10^6 \,\rm{M}^{-1}\rm{s}^{-1} \tag{4}$$

$$\rm SO\_4^{-}\rm ^\bullet + Cl^- \rightarrow SO\_4^{2-} + Cl^\bullet \ , k = 2.0 \times 10^8 \,\mathrm{M}^{-1}\rm s^{-1} \tag{5}$$

$$\text{HO}^{\bullet} + \text{Cl}^{\bullet} \to \text{ClOH}^{-\bullet} \tag{6}$$

$$\text{ClO}\,\text{H}^{-\bullet} + \text{H}^{+} \rightarrow \text{Cl}^{\bullet} + \text{H}\_{2}\text{O} \tag{7}$$

$$\text{Cl}^{\bullet} + \text{Cl}^{-} \rightarrow \text{Cl}\_{2}^{-\bullet} \text{ }, \, k = (0.8-2.1) \times 10^{10} \text{ M}^{-1} \text{s}^{-1} \tag{8}$$

**Figure 7.** Elimination of BPA in SPFC800/PMS system after adding interfering substances ((**a**), i.e., HA, Cl<sup>−</sup>, and HCO3<sup>−</sup>) and degradation of BPA in actual water samples; ((**b**), i.e., RW, WW, TW, and PW). (Experimental conditions: [BPA] = 10 mg L<sup>−</sup>1, [Oxidant] = 5 mM, [SPFCx] = 0.2 g L<sup>−</sup>1, [HA] = 5 mg L<sup>−</sup>1, and [Cl−1] = [HCO3<sup>−</sup>] = 5 mM). **Figure 7.** Elimination of BPA in SPFC800/PMS system after adding interfering substances ((**a**), i.e., HA, Cl−, and HCO<sup>3</sup> −) and degradation of BPA in actual water samples; ((**b**), i.e., RW, WW, TW, and PW). (Experimental conditions: [BPA] = 10 mg L−<sup>1</sup> , [Oxidant] = 5 mM, [SPFCx] = 0.2 g L−<sup>1</sup> , [HA] = 5 mg L−<sup>1</sup> , and [Cl−<sup>1</sup> ] = [HCO<sup>3</sup> −] = 5 mM).

<sup>∙</sup> + ଷ ି → ଶ + ଷ ∙ି (3) ସ ି∙ + ଷ ି → ସ ଶି + ଷ ି , = 9.1 ൈ 10Mିଵsିଵ (4) ସ ି∙ + ି → ସ ଶି + <sup>∙</sup> , = 2.0 ൈ 10଼Mିଵsିଵ (5) <sup>∙</sup> + <sup>∙</sup> → ି∙ (6) To further evaluate the feasibility of the SPFC800 for BPA elimination, the BPA degradation experiments were carried out in different water matrixes (Table 3). As shown in Figure 7b, BPA removal did not change in TW and was slightly inhibited in RW, which was due to that RW often contained a lot of impurities, consuming the ROS. In addition, a moderate deterioration was observed in WW, which could be owing to the ultra-high concentrations of coexisting contaminants, which could compete with BPA for the ROS.


ି∙ + ା → <sup>∙</sup> + ଶ (7) **Table 3.** The basic information of the real waters.

#### **4. Conclusions**

**4. Conclusions** 

**Table 3.** The basic information of the real waters. **Water Sample pH CODCr (mg L−1) Cl<sup>−</sup> (mg L−1) NH4+-N (mg L−1) PO43<sup>−</sup> (mg L−1)**  PW 7.2 ± 0.03 <10 0.47 0.09 0.02 TW 7.13 ± 0.03 <10 12.6 1.37 0.138 In this study, a series of sedum plumbizincicola derived functional carbon (SPFCx) catalysts were successfully fabricated. The SPFCx could effectively and rapidly activate PMS for BPA removal. Notably, the catalytic performance was highly decided by the pyrolysis conditions. Among others, SPFC800 exhibited the best catalytic activity because of its highest surface area and pore volumes. In addition, the non-radical pathway (i.e., <sup>1</sup>O<sup>2</sup> and

RW 7.08 ± 0.03 <10 8.52 2.14 0.577

In this study, a series of sedum plumbizincicola derived functional carbon (SPFCx) catalysts were successfully fabricated. The SPFCx could effectively and rapidly activate PMS for BPA removal. Notably, the catalytic performance was highly decided by the pyrolysis conditions. Among others, SPFC800 exhibited the best catalytic activity because of its highest surface area and pore volumes. In addition, the non-radical pathway (i.e., 1O2 and electron transfer regime) rather than the radical pathway dominated the BPA degradation. More importantly, the BPA elimination (>80%) was highly stable and effective even in complex wastewater, demonstrating that the SPFC800/PMS system was

concentrations of coexisting contaminants, which could compete with BPA for the ROS.

electron transfer regime) rather than the radical pathway dominated the BPA degradation. More importantly, the BPA elimination (>80%) was highly stable and effective even in complex wastewater, demonstrating that the SPFC800/PMS system was promising for BPA-contaminated water remediation. Overall, this work may promote the application of AOPs in environmental remediation.

**Supplementary Materials:** The following supporting information can be downloaded at: https: //www.mdpi.com/article/10.3390/coatings12121892/s1, Supporting Information Text S1: Details of electrochemical experiment.

**Author Contributions:** C.L.: writing—original draft, formal analysis, investigation, and visualization. Z.C.: writing—original draft, formal analysis, investigation, and supervision. R.K.: writing reviewing and editing, investigation. Y.N.: writing—reviewing and editing, investigation. W.S.: writing—reviewing and editing, investigation. X.W.: writing—reviewing and editing, investigation. D.T.: conceptualization, methodology. Y.X.: formal analysis, resources, writing—review and editing. All authors have read and agreed to the published version of the manuscript.

**Funding:** This work has been supported by the Research Project of Science and Technology of the Anyang City (2022C01NY016), the Research Project of Science and Technology of the Henan Province (222102320274), PhD research startup foundation of Anyang Institute of Technology (BSJ2021035), Postdoc research startup foundation of Anyang Institute of Technology (BHJ2022005), Postdoc research startup foundation of the Henan Province (202103099), and Major science and technology projects of Anyang (201928).

**Institutional Review Board Statement:** This article does not contain any studies with human participants or animals performed by any of the authors.

**Informed Consent Statement:** Not applicable.

**Data Availability Statement:** Not applicable.

**Conflicts of Interest:** The authors declare no conflict of interest.
