One-Pot Synthesis of Nano CuO-ZnO Modified Hydrochar Derived from Chitosan and Starch for the H2S Conversion

A novel kind of hydrochar adsorbent, modified by CuO-ZnO and derived from chitosan or starch, was synthesized for H2S adsorption. The prepared adsorbent was characterized by BET, XRD, EDX, SEM, and XPS. The results showed that the modified hydrochar contained many amino groups as functional groups, and the nanometer metal oxide particles had good dispersion on the surface of the hydrochar. The maximum sulfur capacity reached 28.06 mg/g-adsorbent under the optimized conditions. The amine group significantly reduced the activation energy between H2S and CuO-ZnO conducive to the rapid diffusion of H2S among the lattices. Simultaneously, cationic polyacrylamide as a steric stabilizer could change the formation process of CuO and ZnO nanoparticles, which made the particle size smaller, enabling them to react with H2S sufficiently easily. This modified hydrochar derived from both chitosan and starch could be a promising adsorbent for H2S removal.


Introduction
Hydrogen sulfide (H 2 S), a poisonous, odorous, and corrosive gas, commonly exists in industrial gases such as coal gasification gas, natural gas, and biogas. H 2 S is harmful to humans and livestock, and it not only brings corrosion to metal pipes and reaction devices in the industrial production process, but also causes catalyst poisoning, which affects product quality [1,2]. H 2 S is easy to burn, generating SO 2 as a combustion product. Whether through combustion or direct emissions, it can exert a severe impact on the atmospheric environment. Therefore, H 2 S should be fixed on some materials or removed from the production process and environment.
At present, there are many industrial methods to remove H 2 S. According to production conditions and desulfurization costs, the methods of H 2 S removal in industrial processes can be classified into wet flue gas desulfurization (WFGD) and dry flue gas desulfurization (DFGD) [3,4]. The desulfurizer of WFGD is a liquid that absorbs and separates H 2 S with large processing capacity and mature technology. WFGD has some disadvantages-for example, high energy consumption, secondary pollution, and high regeneration cost. DFGD has mainly been used to remove H 2 S at low concentrations, and it has the advantages of high H 2 S removal efficiency and low cost [5]. The commonly used dry desulfurization methods in industrial processes are the zinc oxide method, iron oxide method, manganese desulfurization method, Claus method, etc. [6][7][8][9][10].
Biochar is defined as a solid, carbon-rich product obtained from biomass through various thermochemical technologies [11][12][13][14]. Pyrochar and hydrochar are two kinds of biochar prepared from the pyrolysis and hydrothermal carbonization (HTC) of biomass [15], respectively. The biomass includes straw, sawdust, the dung of herbivores, etc. [16]. Biochar is a promising alternative adsorbent for toxic gas and wastewater treatment [17,18]. Most researchers have focused on pyrochar, but there are a few reports on the application of hydrochar in H 2 S capture. HTC is an auspicious approach for the use of waste biomass. Compared with pyrochar, hydrochar is suitable for dealing with wet biomass directly, with lower energy consumption [19][20][21]. Hydrochar also has higher yield and cation exchange capacity, and, during the production process, no PAHs are released. On the surface of hydrochar, it has more oxygen-containing functional groups, which is favorable for H 2 S capture and oxidation [22,23]. Although hydrochar has such abundant advantages, it has been rarely used to treat gaseous pollutants, especially H 2 S.
Chitosan, insoluble in water and organic solvents, is a natural macromolecular aminopolysaccharide with a yield second only to cellulose [24]. Moreover, cornstarch is the world's largest source of starch, accounting for approximately 65% of the total amount worldwide [25]. In this work, chitosan and cornstarch were used to synthesize hydrochar, which was modified by CuO-ZnO in a one-pot process. The aim of this work was to explore the formation of CuO-ZnO on hydrochar, the physical and chemical properties of this new material, the desulfurization products, and the mechanisms. This work provides new insights into the development and application of hydrochar products.

Basic Physical and Chemical Properties of Hydrochars
The results of the EDX analyses of the hydrochars are shown in Figure 1. The mass yield (the ratio of product to the original raw biomass), ultimate analysis by EDX (C, O, N, Zn, Cu), specific surface area, pore volume, and average pore diameter are reported in Table 1. It was found that the type of precursor had a significant effect on the yield of hydrochar (Table 1). The mass yields of the solids recovered changed depending on the content and type of the precursor. With the increase in chitosan content, the yield of hydrochar and nitrogen content increased [26], because the hydrochar yield is related to the solubility of the precursors in water, and the solubility of starch is much higher than that of chitosan [24,25]. Simultaneously, the nitrogen in the hydrochar products mainly came from chitosan, and a small amount of nitrogen came from polyacrylamide; therefore, with the increase in the chitosan content, the nitrogen content increased.
Under the same synthetic conditions, when the ratio of chitosan to starch was 1:1, the specific surface area of hydrochar reached 30.102 m 2 /g. It was found that, although the added amount of ZnCl 2 and CuCl 2 in the precursor was the same, the detected content of Zn in the product was much lower than that of copper. One possible reason is that the pH value of the filtrate during hydrothermal carbonization kept decreasing, and ZnO could not remain stable under the slightly acidic conditions, while CuO was stable under the acidic conditions.   Under the same synthetic conditions, when the ratio of chitosan to starch was 1:1, the specific surface area of hydrochar reached 30.102 m 2 /g. It was found that, although the added amount of ZnCl2 and CuCl2 in the precursor was the same, the detected content of Zn in the product was much lower than that of copper. One possible reason is that the pH value of the filtrate during hydrothermal carbonization kept decreasing, and ZnO could not remain stable under the slightly acidic conditions, while CuO was stable under the acidic conditions.
FT-IR spectra of the hydrochars were used to determine the functional groups contained in the sample, and these are shown in Figure 2. The C=C in aromatic groups showed FT-IR spectra of the hydrochars were used to determine the functional groups contained in the sample, and these are shown in Figure 2. The C=C in aromatic groups showed an adsorption peak between 1613 cm −1 and 1718 cm −1 . For carbonyl in -COOH and CO-NH, the regions from 1400 cm −1 to 1500 cm −1 were ascribed to C-N and C-O groups' stretching vibration. The peak at 1033 cm −1 was assigned to C-O stretching or O-H bending vibrations. The broad band at 3400 cm −1 can be assigned to the existence of the N-H structure. Finally, the peaks at 1033 cm −1 and 1403 cm −1 were suggested to be C-N and C-O, respectively. According to the elemental analysis and FT-IR analysis, it was proven that amine groups and oxygen-containing groups on the surface of the hydrochar were abundant.
The surface morphology of several hydrochars is shown in Figure 3. It was found that with the change in the starch and chitosan content in the precursors, the hydrochars presented different microstructures. Among all the hydrochars without polyacrylamide, the precursor starch mainly showed carbon particles and carbon spheres with diameters from 10 µm to 100 µm, while the precursor chitosan mainly had a porous cellular structure. However, the hydrochar with polyacrylamide was dense, with no regular shape, and consisted of some carbon particles, because both chitosan and cationic polyacrylamide contained positive charges, which could make the distribution of the system more uniform. Furthermore, metal oxide clusters were not observed in any of the photomicrographs. The hydrochar samples with different starch and chitosan content were analyzed by XRD  Figure 4), and this showed that the crystallinity of metal oxides in the hydrochar was low. There may be ZnO in S5C5, S5C5N, S10C0, and free Cu in S0C10 due to the reducibility of chitosan [27]. It indicated that the distribution of active metal sites in the hydrochar was relatively uniform or that metal oxides were embedded in carbon spheres or carbon particles [28].
Catalysts 2021, 11, x FOR PEER REVIEW 4 of 15 an adsorption peak between 1613 cm −1 and 1718 cm −1 . For carbonyl in -COOH and CO-NH, the regions from 1400 cm −1 to 1500 cm −1 were ascribed to C-N and C-O groups' stretching vibration. The peak at 1033 cm −1 was assigned to C-O stretching or O-H bending vibrations. The broad band at 3400 cm −1 can be assigned to the existence of the N-H structure. Finally, the peaks at 1033 cm −1 and 1403 cm −1 were suggested to be C-N and C-O, respectively. According to the elemental analysis and FT-IR analysis, it was proven that amine groups and oxygen-containing groups on the surface of the hydrochar were abundant. The surface morphology of several hydrochars is shown in Figure 3. It was found that with the change in the starch and chitosan content in the precursors, the hydrochars presented different microstructures. Among all the hydrochars without polyacrylamide, the precursor starch mainly showed carbon particles and carbon spheres with diameters from 10 μm to 100 μm, while the precursor chitosan mainly had a porous cellular structure. However, the hydrochar with polyacrylamide was dense, with no regular shape, and consisted of some carbon particles, because both chitosan and cationic polyacrylamide contained positive charges, which could make the distribution of the system more uniform. Furthermore, metal oxide clusters were not observed in any of the photomicrographs. The hydrochar samples with different starch and chitosan content were analyzed by XRD (in Figure 4), and this showed that the crystallinity of metal oxides in the hydrochar was low. There may be ZnO in S5C5, S5C5N, S10C0, and free Cu in S0C10 due to the reducibility of chitosan [27]. It indicated that the distribution of active metal sites in the hydrochar was relatively uniform or that metal oxides were embedded in carbon spheres or carbon particles [28]. ZnO PDF#01-1136    Notably, no metal oxide aggregates were observed in any of the samples. Based on previous results [29,30], we believe that both the molecular weight and concentration of PAM significantly affected the morphology of the end-products. For the synthesis of nanoporous materials at a large scale, the approach was facile and had many potential applications. In addition, it was also applicative for the synthesis of other materials with a high surface area and nanoporous structures. It has been suggested that the addition of polyacrylamide can affect the morphology of the hydrochar. As an important capping agent, PAM has been widely used to synthesize materials with various nanostructures (nanorods, nanowires, nanoplates, nanocubes, etc.). The exact function of PAM on the shape selectivity is not yet fully understood; however, we believe that the selective adsorption of PAM on various crystallographic planes (newly formed CuO, ZnO, or hydrochar particles) suppressed their intrinsic anisotropic growth [30]. With an N-C=O group, PAM was easily attached to the surfaces of these materials and limited the growth of the crystal faces. Selective interactions between PAM and the different surface planes of the CuO or ZnO may greatly influence the growth direction and rate and ultimately result in particles with different shapes [30]. For an oxidation catalyst, its effectiveness can be mainly attributed to the adsorption and desorption of gas molecules from its surface.

Effect of Hydrochar Species
In this section, a series of single-factor experiments were carried out to determine the effect of the adsorbent in the desulfurization system. The H 2 S removal efficiency (%) and breakthrough sulfur capacity were selected as the evaluation index. The ratio of chitosan to starch had a significant influence on H 2 S removal. The sulfur capacities of hydrochars with different molar ratios of chitosan to starch under 180 • C were measured and are shown in Figure 5. It can be observed that the sulfur capacity of S5C5 was higher than that of other hydrochars and the addition of polyacrylamide had a great impact on H 2 S adsorption.
In this section, a series of single-factor experiments were carried out to determine the effect of the adsorbent in the desulfurization system. The H2S removal efficiency (%) and breakthrough sulfur capacity were selected as the evaluation index. The ratio of chitosan to starch had a significant influence on H2S removal. The sulfur capacities of hydrochars with different molar ratios of chitosan to starch under 180 °C were measured and are shown in Figure 5. It can be observed that the sulfur capacity of S5C5 was higher than that of other hydrochars and the addition of polyacrylamide had a great impact on H2S adsorption.

Effect of Auxiliary Agents on H 2 S Removal
Cationic PAM, polyvinylpyrrolidone, and neutral PAM were used as the auxiliary agents in the synthesis of the hydrochar. According to the experimental results, it was found that the addition of polyacrylamide and its concentration can affect the sulfur capacity. The effect of different auxiliary agents on H 2 S removal by hydrochar S5C5 is shown in Figure 6. Among the three auxiliary agents, the cationic PAM-synthesized hydrochar showed the best performance for H 2 S removal. In order to explore the best composition of precursors, the PAM concentrations were also optimized, as shown in Figure 7. With the increasing of the PAM concentration from 0.5 g/L to 3.0 g/L, the sulfur capacity decreased. Cationic PAM with a positive charge can attract to and interact with chitosan of a negative charge, leading to a good combination of cationic PAM in hydrochar, but the best amount of cationic PAM depended on the amount of chitosan.

Effect of Auxiliary Agents on H2S Removal
Cationic PAM, polyvinylpyrrolidone, and neutral PAM were used as the auxiliary agents in the synthesis of the hydrochar. According to the experimental results, it was found that the addition of polyacrylamide and its concentration can affect the sulfur capacity. The effect of different auxiliary agents on H2S removal by hydrochar S5C5 is shown in Figure 6. Among the three auxiliary agents, the cationic PAM-synthesized hydrochar showed the best performance for H2S removal. In order to explore the best composition of precursors, the PAM concentrations were also optimized, as shown in Figure 7. With the increasing of the PAM concentration from 0.5 g/L to 3.0 g/L, the sulfur capacity decreased. Cationic PAM with a positive charge can attract to and interact with chitosan of a negative charge, leading to a good combination of cationic PAM in hydrochar, but the best amount of cationic PAM depended on the amount of chitosan.

Effect of Adsorption Temperature on H2S Removal
The effect of adsorption temperature on H2S removal by hydrochar S5C5 is shown in Figure 8. With the desulfurization temperature increasing, the desulfurization ability of hydrochar S5C5 was clearly improved. This result indicated that the desulfurization ability of S5C5 modified by metal oxide was lower than the sorbent derived from the molecular sieve (SBA-15 or MCM-41) with modification or adsorbents with high metal content; however, it was far higher than other types of common active carbon [31][32][33]. As is known, a low temperature is beneficial for H2S adsorption. Raising the temperature could enhance the molecular mobility and interaction between each reactant to promote H2S adsorption by increasing the reaction rate; however, a higher temperature would be an obstruction to H2S adsorption in an exothermic reaction.

Effect of Adsorption Temperature on H 2 S Removal
The effect of adsorption temperature on H 2 S removal by hydrochar S5C5 is shown in Figure 8. With the desulfurization temperature increasing, the desulfurization ability of hydrochar S5C5 was clearly improved. This result indicated that the desulfurization ability of S5C5 modified by metal oxide was lower than the sorbent derived from the molecular sieve (SBA-15 or MCM-41) with modification or adsorbents with high metal content; however, it was far higher than other types of common active carbon [31][32][33]. As is known, a low temperature is beneficial for H 2 S adsorption. Raising the temperature could enhance the molecular mobility and interaction between each reactant to promote H 2 S adsorption by increasing the reaction rate; however, a higher temperature would be an obstruction to H 2 S adsorption in an exothermic reaction. In the adsorption and oxidation process of H2S, the change in the oxygen functional groups on the surface of the hydrochar plays an important role. The quinone and carbonyl groups on the surface of the hydrochar can react with molecular H2S. The C=O bond and C=C bond were broken and combined with H2S to form the S-O bond. This process was endothermic and favored the rising temperature. When the ratio of chitosan to starch is 1:1, the cationic PAM concentration is 0.5 g/L, and the temperature is 230 °C, the maximum sulfur capacity of the hydrochar S5C5 is 28.06 mg/g-adsorbent. In the adsorption and oxidation process of H 2 S, the change in the oxygen functional groups on the surface of the hydrochar plays an important role. The quinone and carbonyl groups on the surface of the hydrochar can react with molecular H 2 S. The C=O bond and C=C bond were broken and combined with H 2 S to form the S-O bond. This process was endothermic and favored the rising temperature. When the ratio of chitosan to starch is 1:1, the cationic PAM concentration is 0.5 g/L, and the temperature is 230 • C, the maximum sulfur capacity of the hydrochar S5C5 is 28.06 mg/g-adsorbent.

Adsorption Mechanism
The adsorption of H 2 S on the hydrochar consisted of three parts: the first part is the reaction of H 2 S with the metal active sites, such as CuO and ZnO [34]; the second part is the reaction of H 2 S with the oxygen-containing functional groups and carbon on the surface of the hydrochar to form C-S bonds and O-S bonds; the third part is the physical adsorption process of H 2 S on the surface of the hydrochar [33].
To further investigate the reaction mechanism, the chemical valence states of the element in the whole process were analyzed by XPS. The XPS spectra of S, Cu, and Zn are shown in Figures 9-11.
The XPS spectrum of S in hydrochar S5C5 after H 2 S adsorption is shown in Figure 9. The valence state of S was confirmed within the binding energy in the range of 162-172 eV. This showed that S 2p3/2 and S 2− 2p2/3 appeared at 167.5 eV and 161.7 eV, respectively. The peak at 163.4 eV may vary due to the existence of the structure of C-S [33]. The Cu + was confirmed by the Cu 2p3/2 binding energy in the range of 930 eV to 937 eV, and it showed that Cu + 2p3/2 appeared at 932.56 eV, and the Cu 2+ was assigned to the binding energy of the XPS contribution from 928 to 937 eV with a satellite contribution in the range of 937-947 eV, and it appeared at 934.61 eV. The Zn 2+ was confirmed by the Zn 2p3/2 that appeared at 1021.77 eV. Therefore, the existing sulfur, zinc, and copper in the hydrochar S5C5 were CuS, ZnS, Cu 2 S, sulfur, and a C-S bond.

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Cu 2p3/2 Figure 9. The XPS spectrum of S in hydrochar S5C5 after H 2 S adsorption. Binding Energy/(eV) Figure 9. The XPS spectrum of S in hydrochar S5C5 after H2S adsorption. The XPS spectrum of S in hydrochar S5C5 after H2S adsorption is shown in Figure 9. The valence state of S was confirmed within the binding energy in the range of 162-172 eV. This showed that S 2p3/2 and S 2− 2p2/3 appeared at 167.5 eV and 161.7 eV, respectively. The peak at 163.4 eV may vary due to the existence of the structure of C-S [33]. The Cu + was confirmed by the Cu 2p3/2 binding energy in the range of 930 eV to 937 eV, and it showed that Cu + 2p3/2 appeared at 932.56 eV, and the Cu 2+ was assigned to the binding energy of the XPS contribution from 928 to 937 eV with a satellite contribution in the range At the same time, copper (II) oxide has a certain oxidation capacity; H 2 S can be oxidized partly to elemental sulfur and a fraction of the sulfide ions that have not been oxidized can form Cu 2 S [35]. Hydrochar, rich in oxygen-containing functional groups, can combine with H 2 S to form a C-S bond and S-O bond [33,36]. Therefore, the form of sulfur after adsorption can be confirmed to be sulfur and a C-S bond. H 2 S also can react with oxygen-containing functional groups to form sulfates in the absence of oxygen [33]. There was no oxygen gas to participate in this adsorption, so sulfate did not exist in the product.

Materials
The reagents, all of analytical grade, used in this experiment were purchased directly without further purification. Copper chloride, zinc chloride, cationic polyacrylamides (CPAM), and chitosan (low viscosity, deacetylation >90%) were purchased from Shanghai Macklin Biochemical Co., Ltd (Shanghai, China). Cornstarch (Pharmaceutical grade) was purchased from Shanghai Aladding Biochemical Technology Co., Ltd (Shanghai, China). H 2 S standard gas of 1% and N 2 of 99.999% were provided by Jinan Deyang Special Gas Co., Ltd (Jinan, China). The solution was prepared using laboratory-made deionized water (18.3 MΩ·cm −1 ).

Preparation of Adsorbent
There were six types of hydrochar synthesized in the experiment. All of them were composed of chitosan and cornstarch, with a cationic polyacrylamide solution (an auxiliary agent) with different dosages. The abbreviation and composition of the synthesized hydrochar samples are shown in Table 2. Taking C5S5 as an example, chitosan (3.60 g), cornstarch (3.60 g), ZnCl 2 (0.84 g), and CuCl 2 (0.84 g) were placed in a mortar, ground evenly with force, and then moved to a glass beaker, following by the addition of 45 mL of cationic polyacrylamide solution (0.5, 1.0, 2.0, and 3.0 g/L). While being treated with ultrasound, the precursors were stirred vigorously until a light blue color appeared. The sample was placed in a hydrothermal reactor and heated up to 230 • C for 4 h. The product was washed repeatedly using deionized water until the pH of the rinsed water stabilized. Other hydrochars were synthesized using the same method with different molar ratios of the precursors.

Characterization of Hydrochar
The characterization of materials was investigated using a Fourier-transform infrared (FTIR) spectrophotometer (IRAffinity-1s, Shimadzu, Kyoto, Japan). X-ray diffraction (XRD) patterns of hydrochar samples were recorded on an X-ray diffractometer (SmartLab, Rigaku, Tokyo, Japan) and carried out in the 2θ range from 10 • to 80 • . The surface morphologies of materials were observed by scanning electron microscope (SEM) apparatus (Regulus 8220, Hitachi, Tokyo, Japan). The element composition and valence state of materials were explored by X-ray photoelectron spectroscopy (XPS) with a multifunctional imaging electron spectrometer (ESCALAB 250XI, Thermo Fisher, Waltham, MA, America). The specific surface areas of materials were measured using the Brunauer-Emmett-Teller (BET) method, and the pore size distribution was calculated using the Barrett-Joymer-Halenda (BJH) method from the isotherm of the adsorption branch with an automatic specific surface area and porosity analyzer (TriStar II 3020, Micromeritics, Norcross, GA, USA).

Batch H 2 S Adsorption Experiments
The mixed gas was prepared by blending H 2 S standard gas with N 2 , both quantified by flow indicators (D08-1F), which were purchased from Beijing Sevenstar Electronics Co., Ltd. (Beijing, China); the concentration of H 2 S was measured by the gas analyzer (TH-990S) from Wuhan Tianhong Instrument Group. After adsorption, the sulfur capability was calculated by Equation (1): C in and C out (mg·m −3 ) were the inlet and outlet concentration of H 2 S in the gas mixture, respectively. A diagram of the test devices for the evaluation of desulfurization performance is shown in Figure 12.

Batch H2S Adsorption Experiments
The mixed gas was prepared by blending H2S standard gas with N2, both quantified by flow indicators (D08-1F), which were purchased from Beijing Sevenstar Electronics Co., Ltd. (Beijing, China); the concentration of H2S was measured by the gas analyzer (TH-990S) from Wuhan Tianhong Instrument Group. After adsorption, the sulfur capability was calculated by Equation (1): Cin and Cout (mg·m −3 ) were the inlet and outlet concentration of H2S in the gas mixture, respectively. A diagram of the test devices for the evaluation of desulfurization performance is shown in Figure 12. To test sulfur capacity, a quartz tube was used and its diameter and height were 6 mm and 100 mm, respectively. The adsorption temperature was controlled by a tube furnace. In the tests, a gas mixture containing 3000 ppm (4617 mg/m 3 ) of H2S (nitrogen as balance gas) was passed through the quartz tube filled with adsorbent of 0.5 g, under a To test sulfur capacity, a quartz tube was used and its diameter and height were 6 mm and 100 mm, respectively. The adsorption temperature was controlled by a tube furnace. In the tests, a gas mixture containing 3000 ppm (4617 mg/m 3 ) of H 2 S (nitrogen as balance gas) was passed through the quartz tube filled with adsorbent of 0.5 g, under a gas flow rate of 100 mL/min. The outlet H 2 S gas was absorbed by KOH solution. The breakthrough sulfur capacity (S b , mg/g) was calculated in the stage from the beginning to when the H 2 S outlet concentration was higher than 20 mg/m 3 by Equation (2).
where S b represents the breakthrough sulfur capacity of sorbents (mg/g), M S and M H 2 S are the molar weight of sulfur (32.06 g/mol) and H 2 S (34.06 g/mol), respectively; m is the weight of sorbents; Q H 2 S is the H 2 S gas flow rate; t is the reaction time for desulfurization (min), and C in and C out are the inlet and outlet concentration of H 2 S (mg/m 3 ), respectively. When t is the saturation adsorption time, Equation (2) was also used to calculate the max sulfur capacity (C m ).

Conclusions
For H 2 S adsorption, this study provides a method for the synthesis of hydrochar, obtained by the hydrothermal reaction of chitosan, starch, cationic polyacrylamide aqueous solution, ZnCl 2 , and CuCl 2 . The experimental results showed that the hydrochar contained many amino groups as functional groups, and the nano-scaled metal oxide particles had good dispersion on the surface of the hydrochar. The amine group significantly reduced the activation energy of H 2 S and CuO-ZnO, which was conducive to the rapid diffusion of H 2 S among the lattices. At the same time, cationic polyacrylamide as a steric stabilizer can change the formation process of CuO and ZnO nanoparticles, making the particle size smaller and allowing it to react more easily with H 2 S sufficiently. When the ratio of chitosan to starch is 1:1, the temperature is 230 • C, and the cationic PAM concentration is 0.5 g/L, the maximum sulfur capacity of the hydrochar S5C5 is 28.06 mg/g-adsorbent. Therefore, modified hydrochar may be a promising adsorbent for H 2 S removal.

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