Xinghua Liang*a,
Xi Wua,
Shuaibo Zeng*b,
Wei Xub,
Xingtao Jianga and
Lingxiao Lana
aGuangxi University of Science and Technology, Guangxi Key Laboratory of Automobile Components and Vehicle Technology, Liuzhou 545006, China. E-mail: lxh304@aliyun.com
bChina School of Automotive and Transportation Engineering, Guangdong Polytechnic Normal University, Guangzhou, 510632, China. E-mail: zsbqiche@163.com
First published on 21st July 2021
The slow redox kinetics of polysulfide hinders the rapid and complete conversion between soluble polysulfides and Li2S2/Li2S, resulting in unsatisfactory rate and cycle performance in lithium-sulfur batteries. Electrochemical catalysis, one effective method, promotes the reaction kinetics and inhibits the “shuttle effect”. Here, we present a three-dimensional ordered macro-porous carbon with abundant cobalt–nitrogen–carbon active sites as a matrix catalyst, leading to accelerated polysulfide redox kinetics. In addition, the interconnected conductive frameworks with ordered macro-porous carbon afford fast ion/electron transport and provide sufficient space to adapt to the volume expansion of the sulfur electrode. Owing to the aforementioned advantages, a lithium–sulfur battery with the matrix catalyst delivers a high specific capacity (1140 mA h g−1 at 0.1C) and a low capacity decay rate (0.0937% per cycle over 500 cycles). Moreover, there is a high rate capacity (349.1 mA h g−1) even at the high current density of 2C and sulfur loading of 3.8 mg cm−2 due to the improved polysulfide redox kinetics by a catalytic effect.
Over the history of the lithium-ion battery, scientists have successively developed a variety of positive, negative, and electrolyte materials.7–11 Compared with the current traditional lithium-ion battery anode materials, sulfur, a geographically ubiquitous element with high theoretical specific capacity (1672 mA h g−1), is regarded as one of the most promising cathode materials for lithium-ion batteries.12–14 However, it still suffers from fatal flaws that delay the pace of engineering application, such as the insulative properties of sulfur and low-order lithium sulfide (Li2S2, Li2S),15,16 solubility of high-order lithium sulfide (Li2S8, Li2S6, Li2S4),17,18 volumetric expansibility during discharge,19,20 and low areal sulfur loading.21,22 These features lead to poor cyclic stability and rate performance.
Many approaches have been proposed to solve the abovementioned problems. Various carbon skeletons have been deployed to hold up sulfur by constructing sulfur–carbon composite materials.23 However, the rate performance of Li–S batteries employed with sulfur/carbon cathode showed no significant improvement due to the lack of interface connectivity and electrical conductivity between particles.24,25 Moreover, dissolution of polysulfide compounds is inevitable because the nonpolar carbon material has only a weak physical restriction on the polar polysulfide.26,27 Furthermore, the slow redox kinetics of polysulfide hinders the rapid and complete conversion between soluble polysulfides and Li2S2/Li2S, which is also an important factor restricting the performance of lithium–sulfur batteries.28–31
Here, we report the preparation of a three-dimensional porous carbon (TDPC) with larger pore volume and electrochemical catalytic activity. Encapsulated sulfur particles in TDPC were synthesized through a removable hard-template method (Fig. 1a). Our electrochemical experiments verified the advantages of TDPC as the sulfur host. Firstly, the abundant uniform mesopores in TDPC enabled high sulfur content (68 wt%), and the high ion conductivity allowed fast ion transfer during the discharge–charge reactions. Secondly, the Co nanoparticles and N-doped carbon composite in TDPC enhanced the catalytic effect, which improved the conversion kinetics between liquid-state Li2S6 and solid-state Li2S. Consequently, the fabricated TDPC@S electrodes were tested for good electrochemistry and featured a high discharge specific capacity of 912.8 mA h g−1 at 1C and a low fading rate of 0.0937% per cycle for 500 cycles.
The morphologies and structures of the materials were characterized and analysed by scanning electron microscopy (SEM) combined with energy-dispersive spectrometry (EDS) and transmission electron microscopy (TEM) with elemental mapping. It can be observed that the granuliform SiO2 templates are isolated nanoparticles with a uniform grain size of approximately 400 nm (Fig. 2a). After coating of the packed SiO2 by ZIF, the spherical SiO2 becomes larger and has a dense structure, as shown in Fig. 2b. The EDS clearly reveals the silicon and oxygen element distribution on the ZIF-coated spherical SiO2 (Fig. S1†). As a comparison, there was no silicon element energy spectrum in the EDS spectra after the template was removed, indicating that the SiO2 template has been completely removed by subsequent processes (Fig. S2).† Fig. S3† shows the SEM image of ZIF-coated spherical SiO2 material after carbonization. It is noted that structure of the spherical SiO2 template is not damaged by high temperature. Then, the SiO2 templates were removed by chemical etching technique using KOH as etchant. Fig. 2c shows the SEM image of the obtained TDPC, which presents a good hollow three-dimensional structure. Further study by TEM investigation shows a large number of pore structures inside the TDPC (Fig. 2d). This porous structure can be loaded with more active sulfur, which is conducive to the preparation of high energy density Li–S batteries. At the same time, the high-resolution TEM images also unveil the existence of a mass of cobalt nanoparticles implanted in the TDPC matrix (Fig. 2e and f). To further reveal the elemental distribution within the TDPC matrix, the elemental mappings in overall view and of carbon, cobalt, and nitrogen were performed and are shown in Fig. 2g, demonstrating that there are a large number of holes in the TDPC, and the abovementioned elements are homogenously distributed in the TDPC matrix (Fig. 2h–k). After sulfur impregnation, the obtained TDPC@S maintained the three-dimensional structure (Fig. S4a†). From the elemental mappings shown in Fig. S4b–f,† we clearly observed that the sulfur and cobalt particles are homogenously implanted on the three-dimensional carbon walls.
As shown in the nitrogen adsorption–desorption isotherm of the as-prepared TDPC in Fig. 3a, the curves are a type II isotherm associated with an H3 hysteresis loop. The Brunauer–Emmett–Teller (BET) surface area and total pore volume of the TDPC sample are 426.2 m2 g−1 and 0.85 cm3 g−1, respectively, which are higher than those of the TDPC@S sample (43.2 m2 g−1, 0.23 cm3 g−1) because of the introduction of pure sulfur with a smaller pore volume (12.6 m2 g−1, 0.16 cm3 g−1). The corresponding pore size distributions suggest that the three aforementioned samples have hierarchically distributed pores of different sizes, including micropores and mesopores. For quantitative analysis of sulfur content in the TDPC@S sample, thermogravimetric (TG) measurement was performed. From Fig. 3c, the TDPC sample exhibited only a minimal weight loss at the temperature range of 30 °C to 800 °C when it was treated at 800 °C. Meanwhile, the pure sulfur is entirely lost in the temperature range of 150 °C to 300 °C because of sublimation. Thus, it is confirmed that the sulfur content is 68.65% in the TDPC@S composite. X-ray diffraction (XRD) spectrums of the three composites are shown in Fig. 3d. No obvious peaks of SiO2 are observed in the TDPC material, which suggests the SiO2 template has been completely removed. The XRD spectrum of the TDPC@S shows peaks of both TDPC (36.93°) and pure sulfur (23.08°), indicating the presence of both components. The amorphous states of TDPC and TDPC@S were measured by Raman spectroscopy, as shown in Fig. 3e. The intensity ratios between the D band and G band for TDPC and TDPC@S are 1.03 and 1.02, respectively. The above results indicate that introduction of sulfur particles in TDPC did not change the degree of graphitization. An experiment on adsorption of polysulfide lithium was carried out using TDPC, as shown in Fig. 3f. It is obvious that the solution becomes clarified with the addition of TDPC. This phenomenon shows that TDPC has a good adsorption effect for polysulfide lithium. UV-vis spectroscopy defines the liquid intermediates in the discharging process.32,33 We investigated the UV-vis spectra to demonstrate the adsorption of TDPC on lithium polysulfide. The UV-vis spectrum shows the absorption peak at ca. 418 nm for S42− (Fig. S5†), which has been reported in previous literature.34,35 The UV-vis spectrum of solution 4 showed that the absorption peak intensity of S42− was weakened after the addition of TDPC. The evidence above also indicates the adsorption of polysulfide lithium using TDPC. To further investigate the chemical status of carbon, nitrogen, and cobalt elements in the TDPC@S, the full spectrum and high-resolution C 1s, N 1s, and Co 2p spectrums of the TDPC@S sample were illuminated by X-ray photoelectron spectroscopy (XPS). As shown in Fig. 4a, six normal peaks located at 164.43, 227.51, 286.29, 399.37, 533.74, and 799.08 eV were found, which correspond to the binding energy of S 2p, S 2s, C 1s, N 1s, O 1s, and Co 2p.36,37 The surface composition of the elements mentioned above is estimated to be 9.5% for sulfur, 55.7% for carbon, 8.3% for nitrogen, 21.2% for oxygen, and 5.3% for cobalt. From Fig. 4b, the high-resolution C 1s spectrum can be further convoluted into C–C/CC (284.6 eV), C–N (285.2 eV), and C–O (286.2 eV).38 The high-resolution N 1s spectrum is deconvoluted into four peaks of different signals with binding energies of 398.6, 399.5, 400.6, and 401.3 eV, which are indexed to pyridinic N, pyrrolic N, Co–N, and graphitic N, respectively.39 Peaks at 778.3, 779.6, and 781.5 eV are assigned to metallic Co, Co–O, and Co–N, respectively, which attest to the existence of Co–N bonding.40 Many reports show that the introduction of Co–N bonding and pyridinic-N are beneficial for improving polysulfide redox kinetics.41,42 In the sulfur reduction process, these abundant pyridinic-N and cobalt–nitrogen active sites, as matrix catalyst, accelerate the conversion of lithium polysulfide, leading to enhanced electrode stability.43
The prepared electrode was assembled into a CR2032-type button cell to evaluate the electrochemical performance of TDPC@S as cathode. The TDPC/S cathode and the mixture of sulfur and acetylene black (S/C) cathode were also made into CR2032-type button cells for comparison. Fig. 5a presents the representative electrochemical impedance spectroscopy (EIS) profiles of the batteries with the three aforementioned cathodes at a frequency range of 10−2–105 Hz. According to the equivalent circuit diagram (Fig. S6†), the fitting results show that the TDPC@S electrode has a much smaller Rct than the other two electrodes, indicating that TDPC can effectively facilitate charge transfer and improve the polysulfide redox reactions. To investigate the effects of TDPC on the stability of the electrode, cyclic voltammetry (CV) tests were conducted, as shown in Fig. 5b. The CV profiles display two sulfur reduction peaks, which locate at 2.31 V and 2.03 V in the negative scan, corresponding to the two discharge platforms in Fig. 5d. The fifth CV profile coincides with the first CV profile, verifying that the electrode has good stability. To further evaluate the cycling stability of the Li–S batteries based on TDPC cathode, charge–discharge test was conducted at 0.25C for 100 cycles with a sulfur loading of 3.8 mg cm−2 (Fig. 5c). As shown in Fig. 5d and S7,† the discharge specific capacity of the TDPC@S cathode is 964.36 mA h g−1 at the first cycling. After 100 charge–discharge cycles, the capacity of the electrode dropped to 700.75 mA h g−1, corresponding to a 72.61% capacity retention rate. These values are 60.06% for the TDPC/S cathode and 23.6% for S/C cathode. The potential gap (ΔU) is an important index to evaluate the charge efficiency.44 The ΔU of the TDPC@S electrode is obviously smaller after 100 charge–discharge cycles than that of the other two electrodes, indicating the TDPC@S electrode has a relatively low resistance and polarization. Fig. 5e and f show the rate performance of the three electrodes, which were evaluated at various current densities (from 0.1C to 2C). The discharge specific capacities of the TDPC@S electrode are 1139.2 mA h g−1, 959.9 mA h g−1, 813.5 mA h g−1, 519.6 mA h g−1 and 349.1 mA h g−1 at 0.1, 0.25, 0.5, 1 and 2C, respectively. Those values are 1023.6 mA h g−1, 841.5 mA h g−1, 718.1 mA h g−1, 336.6 mA h g−1, and 151.9 mA h g−1 for the TDPC/S cathode (Fig. S8a†), and 757.8 mA h g−1, 616.0 mA h g−1, 433.1 mA h g−1, 272.1 mA h g−1, and 119.2 mA h g−1 for the S/C cathode (Fig. S8b†) at the relevant rates. More importantly, compared with the other two cathodes, the reversible capacity of the TDPC@S cathode was basically recovered, with the current density back to 0.1C. Such phenomena further prove the TDPC@S cathode has enhanced reaction kinetics.
The long-term cycling performance of the three cathodes was tested at a high rate current density of 1C, as shown in Fig. 6. Compared with the other two cathodes, the cycling curve of the TDPC@S cathode exhibits better cycle stability, with the capacity retention of 62.58% after 500 cycles, corresponding to a capacity decay of only 0.0937% per cycle. These values are 0.476% for the TDPC/C cathode and 1.285% for the S/C cathode. These results further validated that the TDPC@S cathode has better cycle stability than the other two cathodes. Table S1† summarizes the performance of sulfur-based cathodes for Li–S batteries in the published literature. Note that the performance of the TDPC@S cathode is better than (or at least comparable to) the leading results reported for other cathodes (Table S1†).
Fig. 6 Cycling performance of TDPC@S, mixture of sulfur and TDPC, and S/C cathodes at 1C over 500 cycles. |
For TDPC@S, firstly, 12.1 g of sodium thiosulfate was dissolved in a mixture of water and ethanol (v/v = 25 mL:25 mL) under magnetic stirring. Then, 0.3 g of the prepared TDPC was slowly added into the solution. Secondly, 5 mL of diluted hydrochloric acid was added into the solution to form sulfur nanoparticles. We collected the mixture of TDPC and sulfur (TDPC/C) by centrifugation at 8000 rpm for 20 minutes. Lastly, the TDPC@S was obtained after heating at 140 °C for 20 minutes under 200 mL min−1 nitrogen gas flow, which removed the sulfur particles outside the TDPC.
Footnote |
† Electronic supplementary information (ESI) available. See DOI: 10.1039/d1ra02704b |
This journal is © The Royal Society of Chemistry 2021 |