Facile Preparation of a Porous Biochar Derived from Waste Crab Shell with High Removal Performance for Diesel

Han, Xiao; Wu, Zhaodi; Yang, Yi; Guo, Jian; Wang, Yaning; Cai, Lu; Song, Wendong; Ji, Lili

doi:10.32604/jrm.2021.015076

Xiao Han1, Zhaodi Wu1, Yi Yang1, Jian Guo1, Yaning Wang2, Lu Cai3, Wendong Song4 and Lili Ji2,*

1College of Food and Medical, Zhejiang Ocean University, Zhoushan, 316022, China
2Institute of Innovation & Application, Zhejiang Ocean University, Zhoushan, 316022, China
3Donghai Science and Technology College, Zhejiang Ocean University, Zhoushan, 316000, China
4College of Petrochemical and Energy Engineering, Zhejiang Ocean University, Zhoushan, 316022, China
*Corresponding Author: Lili Ji. Email: jll-gb@163.com
Received: 19 November 2020; Accepted: 04 January 2021

Abstract: In this study, a porous biochar material derived from waste crab shell was prepared by one-step hydrothermal carbonization and acetic acid activation method at 180°C, which was characterized by SEM, BET, XRD and FTIR. The results show that the as-prepared crab shell biochar (CSB) exhibits a fluffy irregular layered structure with abundant pores and oxygen-containing functional groups, which can facilitate the adsorption of diesel using CSB. In addition, batch adsorption experiments had been performed, effects of initial diesel concentration, adsorption time, adsorbent dosage and pH on the diesel adsorption using CSB were analyzed, which could be observed that CSB has high removal efficiency for diesel, and the maximum removal rate is up to 80.1%. The adsorption isotherms and kinetic studies were also investigated to determine the adsorption mechanism of diesel using CSB, the results show that the Langmuir model and the pseudo-second-order model are more suitable for describing the adsorption of diesel using CSB, indicating that the adsorption of diesel oil by CSB is monolayer chemical adsorption. This study will provide a theoretical basis for the high-value utilization of waste crab shell, which has a great potential in the treatment of oil spill.

Keywords: Waste crab shell; biochar; adsorption; diesel wastewater

Petroleum, known as the blood of industry, is indispensable to the survival and development of all countries in the world. With the acceleration of industrialization, global petroleum consumption has risen sharply over the last decades, which has reached 4.66 billion metric tons in 2018 [1]. However, at the same time, petroleum and its products could cause environmental pollution in the course of exploitation, refining, storage, transportation and use [2–4], among which, offshore oil spill is one of the main environmental problems that urgently need to be solved in the oil industry. Moreover, oil spills in the natural environment will have disastrous impact on human beings and ecosystems [5,6], and oil contamination usually includes benzene, toluene, ethylbenzene, or petroleum hydrocarbons, which can enter the human body through the food chain, causing acute and chronic poisoning and damaging the nervous system [7]. Thus, it is imperative for effective removal of oil pollution from the environment.

To date, a variety of technologies available for the removal of oil pollution have been developed, such as physical method [8,9], chemical method [10,11] and biological method [12]. Biological methods have a low remediation rate, which makes them very limited in cleaning up oil spills, while chemical methods can easily cause secondary contamination. In contrast, the physical method has the advantages of simple operation, low cost and quick effect, so it has been drawn considerable attention in recent years, among which, adsorption is the most commonly used physical method. The adsorbent can concentrate the liquid oil and convert it into a semi-solid or solid state to remove it from the polluted solution, so as to avoid the harm to the environment, and at the same time, the adsorbed oil can be recycled [13]. Biochar, as one of the representative absorbents, prepared by high-temperature pyrolysis derived from biomass under low oxygen or oxygen-free condition, has attracted more and more attention, because of its relatively high specific surface area, abundant pore structure and rich functional groups (-OH, C=C, C=O, CH2 et al.) on its surface [14,15]. In particular, crustacean waste such as crab shells is an abundant and cheap food waste generated by the food processing industry, with an annual production of 1 million tons [16]. Crab shell is a natural porous structure complex [17] composed of protein (20%–40%), chitin (15%–40%) and calcite (20%–50%) [18] and is considered a highly promising candidate for biochar preparation [19]. The preparation of biochar using crab shells can not only reduce the serious environmental pollution caused by various chemicals or microorganisms decomposed from waste crab shells [19,20], but also produce low-cost, renewable and sustainable biochar raw materials. It has been reported that crab shells have been developed into various biochar materials with rich porous structure and high specific surface area, which are used as bio-adsorbent for the removal of organic dyes, heavy metals, and diesel fuel [21–24]. However, almost all biomass carbon based adsorption modified materials in the literature were treated by high temperature pyrolysis followed by activation with potassium hydroxide [25]. This method not only consumes a lot of energy, but also the process is complex, cumbersome, and highly environmentally friendly [26].

Commonly used biochar preparation methods include high-temperature cracking (also known as oxygen-limited carbonization) and hydrothermal carbonization [27]. Compared with the traditional high-temperature pyrolysis carbonization technology, hydrothermal carbonization has obvious advantages such as low energy consumption, high efficiency of carbon element fixation, and carbide surface rich in oxygen-containing and nitrogen-containing functional groups [28], which can be widely used in various fields. It has great potential for application in wasting biomass treatment/pre-treatment and resource utilization [29,30]. As is well known, the quality and property of biochar depend on the characteristics of raw material and activation method [31,32]. At present, activation method contains physical and chemical activation, among which, chemical activation is extensively employed to prepare biochar due to its advantages of high yield, short time and large specific surface [33,34]. Now, the commonly used chemical activators include KOH [35], H3PO3 [34], NaOH [36], ZnCl2 [32], etc. However, the above activators still face the challenges of high energy consumption and probably causing corrosion to the instrument. The advantages of using organic acids as activators compared to strong acids, bases and salts are environmental friendliness, low cost and the use of low toxic reactants [37]. It has been successfully used as an effective activator for low-temperature preparation of biochar from different types of raw materials such as soybean straw [38], corn cobs [39] and lawn grass [40].

However, to the best of our knowledge, there are few reports on the preparation of crab shell biochar by hydrothermal carbonization using acetic acid as an activator. In this study, a porous biochar derived from waste crab shell was prepared by one-step hydrothermal carbonization and activation method at low temperature using acetic acid as activation reagent. CSB was characterized by SEM, BET, XRD and FTIR. The adsorption properties of as-prepared biochar for diesel oil were investigated by simulating the environment of diesel wastewater. The batch adsorption experiments of diesel were performed using as-prepared absorbent, and the adsorption isotherms and kinetics were also investigated.

Crab shell used in this experiment was obtained from the local market in Zhoushan, China, which was washed with deionized water for several times and dried at 80°C for 2 h. Then the dried crab shell was crushed into powder and used in subsequent pyrolysis experiments. Hydrochloric acid (HCl), sodium hydroxide (NaOH) and acetic acid (CH3COOH) were purchased from Shanghai National Pharmaceutical Chemical Reagent Co., Ltd., China. The chemicals used in this study are analytical and used at reception without further purification.

The pre-treated crab shell powder was soaked in 6% HCl for 4 h at 30°C for decalcification, and then soaked in 6% NaOH for 2 h at 90°C for deproteinization. After being soaked in 50% NaOH for 9 h, the crab shell powder was washed with deionized water for several times until neutral (pH = 7), and then dried in the oven (SENXIN-DGG9030BD, Shanghai, China) at 80°C for 10 h. The pretreated crab shell powder mixed was with 50% acetic acid (crab shell/acetic acid (w/v) = 1:1), then the mixture was carbonized at 180°C for 10 h in the oven. After cooling to room temperature, the prepared crab shell biochar was rinsed using deionized water until neutral, dried in the in the oven at 80°C for 12 h, ground and sieved with 100 mesh, which was denoted as CSB. And in the control group, the pretreated crab shell powder in “2.1 Materials” was denoted as CS.

Surface microstructure and morphology of as-prepared sample were investigated by using scanning electron microscopy (SEM, Hitachi S-4800, Tokyo, Japan) at 5.0 KV. N2 adsorption/desorption isotherm was performed on a static volumetric adsorption analyzer (Micromeritics ASAP 2010, Shanghai, China) and calculated with the method of BET. Meanwhile, X-ray diffraction (XRD) patterns of sample were recorded on an Ultima IV X-ray Diffractometer (Ultima IV, Rigaku Corporation, Tokyo, Japan) in the range of 2θ from 10° to 60°. Moreover, the surface functional groups were analyzed by Fourier transform infrared spectra (FTIR, Nicolet 5700, Thermo Corp., USA).

The standard curve is a curve used to describe the quantitative relationship between the concentration (or content) of the substance to be measured and the response signal values of the analytical instrument. Using the diesel standard solution to draw the diesel standard curve, the corresponding concentration value can be found on the standard curve through the measured absorbance value.

0.3 g diesel was mixed with 5 mL petroleum ether in a 100 mL volumetric flask, diluted with petroleum ether to 100 mL, as the diesel standard solution. Take 0 mL, 5 mL, 10 mL, 15 mL, 20 mL and 25 mL diesel standard solution, respectively, and the constant volume was made up to 25 mL with petroleum ether. The absorbance value was measured with petroleum ether as reference at a wavelength of 256 nm by UV-vis spectrophotometer (Model No. UV 2600, Shimadzu, Shanghai, China), and the diesel standard curve was drawn as shown in Fig. S1.

The as-prepared absorbent was added into 100 mL diesel wastewater for adsorption experiments. The effects of diesel initial concentration, reaction time, initial pH and absorbent dosage on the diesel adsorption were also investigated as shown in Tab. 1. The diesel initial concentration was 100 mg/L, 200 mg/L, 300 mg/L, 400 mg/L, 500 mg/L and 600 mg/L, respectively, the reaction time was 0.5 h, 1 h, 2 h, 3 h, 4 h and 6 h, respectively, the initial pH value was adjusted from 5.0–9.0 with 0.1 mol/L HCl or 0.1 mol/L NaOH and the absorbent dosage was 0.05 g, 0.10 g, 0.15 g, 0.20 g and 0.25 g, respectively. After adsorption, the reaction solution was centrifugal in a desktop high-speed centrifuge (Cence, TG16-WS, Hunan, China) at 1700 g for 5 min, and the supernatant was collected to measure its optical density value (UV 2600, Shimadzu, Japan) at 256 nm. The diesel fuel concentration (C0 and Ce) in diesel wastewater was then calculated from the OD values. The adsorption rate (R) and equilibrium adsorption capacity (qe) of diesel fuel can be calculated according to Eqs. (1) and (2), respectively.

where, the adsorption rate of diesel at equilibrium is denoted as R (%), the adsorption capacity of diesel at equilibrium is denoted as qe, the initial and equilibrium concentrations of diesel wastewater are denoted as C0 and Ce, respectively, and the dosage of CSB and the volume of diesel wastewater solution are denoted as m(g) and V(L), respectively.

0.1 g CSB absorbent was added into 100 mL diesel wastewater with different initial concentrations, respectively, and the adsorption process was carried out for 5 h. The Langmuir and Freundlich adsorption isotherms were used to analyze the equilibrium performance, as follows:

where the equilibrium concentration of diesel fuel is denoted as Ce (mg/L). The adsorption capacity of diesel fuel at equilibrium is denoted as qe (mg/g), and the saturation adsorption capacity is denoted as qm (mg/g). The Langmuir adsorption equilibrium constant is denoted by KL (L/mg) and the Freundlich constant is denoted by KF [(mg/g)(L/mg)1/n], 1/n representing the energy partition depending on the adsorption properties and adsorbent energy.

0.1 g CSB adsorbent was added to 100 mL/L, 300 mg/L and 600 mg/L of 100 mL diesel wastewater and the adsorption capacity of diesel was determined at different adsorption times from 0 to 300 min at 25°C. The adsorption kinetics of the prepared samples were analyzed by proposed primary reaction (PFO) and secondary kinetics (PSO) as follows:

where the amount of diesel adsorbed at adsorption equilibrium and at time t(min) are recorded as qe(mg/g) and qt(mg/g), respectively. The rate constants of PFO and PSO are k1(min−1) and k2(g/mg min), respectively, and the time is recorded as t(min).

SEM is employed to visualize the surface morphology and microstructure of as-prepared samples, as shown in Fig. 1. It could be demonstrated that crab shell exhibits a dense stacked layered structure with a few unevenly distributed grooves in Figs. 1a and 1b. After pyrolysis, CSB shows a fluffy irregular layered structure, including a large number of pores and grooves as indicated in Figs. 1c and 1d (as shown by the red arrow).This is because the chitin derivatives of crab shells acetylation by acid-base treatment of decalcification and deproteinization [41,42] and the activator acetic acid in the process of hydrothermal carbonization of dehydration and decarboxylation, hydrogen bond breakage, free radical reaction breakage [43] and aromatization, condensation and solidification reaction to generate biochar [44,45].The rough surface of crab shell biochar is beneficial to the adsorption of diesel oil, and the loose groove structures are conducive to the adsorption and storage of a large amount of diesel oil [46].

The N2 adsorption isotherm and pore size distribution of as-prepared sample was shown in Fig. 2. According to IUPAC classification [47], the N2 adsorption isotherm of CSB is Type IV, whose bifurcation is irreversible. And there is a hysteresis loop at P/P0 > 0.4 in the adsorption isotherm of CSB, indicating the formation of mesoporous structure. Based on the N2 adsorption bifurcation data, the pore size distribution (PSD) of CSB is further analyzed by using the non-local density functional theory (NLDFT) model [26]. As shown in the Fig. 2b, CSB shows a relatively sharp PSD, centered around 3 nm–5 nm, and PSD is mainly in the range of 3 nm–20 nm, which consists of micropore and mesopore. In addition, the specific surface area and pore volume of CS obtained from N2 adsorption isotherm data are 9.57 m2/g and 0.027 cm3/g, respectively, while those of CSB are 17.01 m2/g and 0.0763 cm3/g, respectively. Compared with CS, the specific surface area of CSB increases by 78%, which was caused by the decarboxylation and dehydration of crab shells during the hydrothermal carbonization process [43]. Some volatile substances such as CO2, CO and H2O overflowed from the pores and destroyed the original structure of crab shells, which led to the gradual formation of micropores and the increase in specific surface area and pore volume of biochar.

Figure 2: N2 adsorption-desorption isotherm and pore size distribution of CS and CSB

The XRD pattern is utilized to analyze the crystal structure and phase analysis of the as-prepared sample, as shown in Fig. 3. It can be seen from the following X-ray diffraction patterns that the observed diffraction peaks located at crystal planes of CaCO3 according to JCPDS database No. 81-2027 [31]. As for the pattern of CS, the observed diffraction peaks located at about 23°, 29°, 39°, 43°and 48°, can be perfectly indexed to the (012), (104), (113), (202), (018) of crystal planes of CaCO3, and there is a diffraction peak at about 2θ = 19° corresponding to (21-2) crystal planes of chitin [48]. After pyrolysis, the CaCO3 peaks are weak, only 23° and 39° diffraction peaks left in the XRD pattern of CSB, while the chitin peak located at 19° obviously strengthens. As is well known, chitin is rich in hydroxyl groups, which could provide abundant binding sites for diesel adsorption using crab shell biochar.

The surface chemical compositions and surface functional groups of as-prepared samples are analyzed by the FT-IR, as illustrated in Fig. 4. The FTIR spectrums of the CS and CSB located at 3273.2 cm−1 and 3259.6 cm−1 are attributed to the axial O-H stretching vibration [38], followed by a peak at 2358.9 cm−1 due to R-N=C=O stretching vibration. The absorption peak at 1668.4 cm−1 in the CS and CSB spectra is attributed to the C=O [49] stretching vibration caused by the carboxyl group (COOH) introduced by acetic acid on the surface of biochar [37]. Furthermore, the adsorption peaks located at 1070.4 cm−1 and 1072.4 cm−1 in the CS and CSB spectra were attributed to symmetric stretching vibrations of X-H due to amine/ester, followed by peaks located at 871.82 cm−1 and 893.04 cm−1 due to out-of-plane bending vibrations of C-H.

The carboxyl functional group is esterified with the alcohol contained in diesel oil, so it may play a key role in the adsorption of diesel oil [49]. Ester group (R-N=C=O), halogen group (X-H) and alkyl group (C-H) are lipophilic groups that can form van der Waals force between diesel and diesel molecules [50]. The hydroxyl groups enriched in CSB can undergo radical substitution reactions with alkanes in diesel fuel [51]. Therefore, it can be speculated that chemisorption is the main driving force for diesel fuel adsorption using CSB. From the above discussion, it can be seen that the reactive groups on the crab shell surface become enriched after activation and are more favorable for diesel adsorption.

Fig. 5a shows the adsorption performances of CSB to different initial diesel concentrations. It could be demonstrated that the residual concentrations of diesel in the adsorption system decrease sharply in 10 mins, decrease gradually as the adsorption time increase until equilibrium, and reach the adsorption equilibrium at 180 mins. It can be calculated that the adsorption rates of as-prepared sample for diesel wastewater at different initial concentrations are 77.7%, 78.3%,79%, 79.5%, 79.7% and 80.1%, respectively, that is the higher the initial concentration of diesel, the greater the adsorption capacity of diesel using CSB. At the beginning of the adsorption time, the high removal rate of diesel using CSB is due to at the initial stage of adsorption, the functional groups on the surface of biochar and the internal pores are well developed and diesel particles can easily adhere to them, and then because the outer surface of the adsorbent is occupied by oil, the oil removal rate decreases and reaches equilibrium [52]. With the increase of diesel solution concentration, the time to reach equilibrium becomes longer, which is because more active sites are occupied, resulting in competitive adsorption, and decreasing the attractiveness of CSB to diesel [53].

Figure 5: Effects of initial diesel concentration (a), adsorption time (b), dosage (c) and pH (d) on the adsorption of diesel by CSB

Fig. 5b shows the effect of adsorption time on the adsorption capacity of diesel using CSB. It can be observed that the diesel adsorption rate first increases rapidly until adsorption equilibrium at 180 min, and the maximum diesel adsorption rate is 80.1%. Initially, the higher adsorption efficiency is due to abundant binding sites available on the surface of CSB, which could enhance the adsorption of diesel. In addition, low solubility and higher hydrophobicity of diesel are beneficial to providing more attraction towards CSB, rendering high adsorption efficiency for diesel using CSB. At adsorption equilibrium stage, the binding sites of CSB have been covered with diesel, and the amount of diesel in solution and the amount of diesel adsorbed on CSB are in dynamic equilibrium [54].

The adsorption capacities of CSB dose for diesel are shown in Fig. 5c. It can be seen that with increasing CSB dose in the range of 0.05 g–0.25 g, the adsorption capacities of CSB for diesel sharply increase and then gradually flatten. That is because there are more binding sites with the increase of CSB, being beneficial to adsorb more diesel, while CSB dose increases to 0.1 g, adsorption system reaches equilibrium, and the adsorption of diesel using CSB tends to be stable.

With the increase of the amount of CSB, its binding sites and adsorption capacity will be increased, however, after reaching its peak, the adsorption capacity of CSB would reach saturation, and the adsorption rate will not be further improved. Moreover, too much biochar will make them adhere together in solution, which will also reduce its specific surface areas, the adsorption sites will also be reduced, so that the adsorption rate will even slightly decrease [55].

Fig. 5d shows the effect of pH in diesel adsorption using CSB in the range of 5 to 9. The adsorption performance of diesel using CSB is favored at pH = 7, where the maximum absorption rate is 70%. This is because under acidic conditions, H+ neutralizes the negative charge on the surface of oil molecules, and the stability is broken, resulting in the condensation of oil droplets [56]. However, with the increase of pH value, the viscosity of diesel decreases by the reaction of organic acids or acidic components in diesel with OH- in solution, and the diesel molecules are easily desorbed and dispersed [57]. Therefore, it can be concluded that electrostatic interaction would be one of the main factors that influence the adsorption capacity of diesel using CSB.

In order to study the adsorption equilibrium, Langmuir and Freundlich adsorption isotherm models were employed to evaluate the equilibrium characteristics. Fig. 6 indicates the fitting of data with these two isotherm models, and Tab. 2 shows the adsorption parameters and regression data of the models. The R2 value of the Langmuir isotherm is 0.996, and that of the Freundlich isotherm is 0.968, thus the Langmuir equation is more suitable for describing the adsorption of diesel using CSB, being used to calculate the adsorption amount of diesel using CSB at equilibrium is 451 mg/g at 25°C, in good combination with experimental data (480.6 mg/g). Thus, it could be demonstrated that the adsorption of diesel using CSB is monolayer surface adsorption [37].

Figure 6: The adsorption isotherm models of diesel using CSB plotted with (a) the Langmuir equation and (b) the Freundlich equation

To investigate the kinetic mechanism of diesel adsorption using CSB, kinetic models were fitted to diesel adsorption data at 100, 300 and 600 mg/L diesel concentrations using pseudo-first order (PFO) model and pseudo-second order (PSO) model. Fig. 7 shows the fit of experimental data to the kinetic model using CSB for diesel fuel, and Tab. 3 shows the results of the kinetic model fit for diesel fuel adsorption using CSB. It can be seen that comparing the R2 values of PSO model and PFO model with three diesel concentrations. The R2 value of PSO model is higher. Therefore, the PSO model is more suitable for describing the adsorption process of CSB on diesel fuel and is used to calculate the adsorption amount of diesel fuel at equilibrium (89.45 mg/g, 258.24 mg/g and 486.32 mg/g) which fits well with the experimental data (77.7 mg/g, 237 mg/g and 480.6 mg/g). It can be possible to conclude that the adsorption of CSB on diesel is a chemisorption, which may involve the electron exchange between the functional groups on the surface of CSB and diesel molecules [58,59].

Figure 7: Adsorption Kinetics of diesel adsorbed by CSB, (a) pseudo first order model; (b) pseudo second order model

Tab. 4 shows the comparison of the maximum adsorption capacities of different adsorbents for diesel. It is observed from the results that CSB has relatively higher adsorption capacity (480.6 mg/g) compared with other adsorbents previously reported in literature. The high adsorption rate of diesel on CSB can be attributed to abundant active sites available and high surface area of CSB, which could adsorb diesel molecules effectively. Furthermore, crab shell as by-product of seafood products, could be easily obtained with low cost and can realize the value-added utilization of waste. Thus, crab shell biochar has great potential for the treatment of oil spill.

Table 4: Comparison of adsorption capacity of different adsorbents for diesel removal

In sum, a novel carb shell biochar was prepared by a one-step hydrothermal carbonization and activation method, in which, acetic acid chosen as activator could achieve low-temperature activation. It can be observed from SEM, BET, XRD and FT-IR characterizations that the as-prepared sample is a fluffy irregular layered structure with abundant pores and oxygen-containing functional groups, being beneficial to the adsorption of diesel using CSB. Moreover, the batch adsorption experiments indicate that CSB has high adsorption performances for diesel, and the maximum removal rate is up to 80.1%. And the Langmuir model and the pseudo-second-order model could better describe the adsorption process of diesel using CSB.

Funding Statement: This study was supported by the Fundamental Research Funds for Zhejiang Provincial Universities and Research Institutes (Nos. 2019J00045, 2019J00025), the General Research Project of Zhejiang Province Education Department (No. Y202044721) and Key Research and Development Projects of Zhejiang Province of China (No. 2018C02043).

Conflicts of Interest: The authors declare that they have no conflicts of interest to report regarding the present study.

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