Encapsulation of Few-Layer MoS2 in the Pores of Mesoporous Carbon Hollow Spheres for Lithium-Sulfur Batteries

Integrating a highly conductive carbon host and polar inorganic compounds has been widely reported to improve the electrochemical performances for promising low-cost lithium sulfur batteries. Herein, a MoS2/mesoporous carbon hollow sphere (MoS2/MCHS) structure has been proposed as an efficient sulfur cathode via a simple wet impregnation method and gas phase vulcanization method. Multi-fold structural merits have been demonstrated for the MoS2/MCHS structures. On one hand, the mesoporous carbon hollow sphere (MCHS) matrix, with abundant pore structures and high specific surface areas, could load a large amount of sulfur, improve the electronical conductivity of sulfur electrodes, and suppress the volume changes during the repeated sulfur conversion processes. On the other hand, ultrathin multi-layer MoS2 nanosheets are revealed to be uniformly distributed in the mesoporous carbon hollow spheres, enhancing the physical adsorption and chemical entrapment functionalities towards the soluble polysulfide species. Having benefited from these structural advantages, the sulfur-impregnated MoS2/MCHS cathode presents remarkably improved electrochemical performances in terms of lower voltage polarization, higher reversible capacity (1094.3 mAh g−1), higher rate capability (590.2 mAh g−1 at 2 C), and better cycling stability (556 mAh g−1 after 400 cycles at 2 C) compared to the sulfur-impregnated MCHS cathode. This work offers a novel delicate design strategy for functional materials to achieve high performance lithium sulfur batteries.


Introduction
The development of lithium ion (Li-ion) battery technologies cannot meet the ever-growing demand of electric vehicles and automobiles due to their relatively low energy density (387 Wh kg −1 for LiCoO 2 /C) and their relatively high cost. Fortunately, lithium-sulfur (Li-S) batteries have an ultrahigh theoretical energy density (2600 Wh kg −1 ) and high theoretical specific capacity of 1675 mA h g −1 based on the multielectron conversion electrochemistry between lithium and elemental sulfur [1,2]. In addition, elemental sulfur, the main cathode material of Li-S batteries, is eco-friendly and low-cost [3]. Considering those factors, Li-S batteries are considered as next-generation high-energy batteries [4][5][6]. However, several intrinsic problems from sulfur cathodes are impeding the commercial application of lithium-sulfur battery technologies. Firstly, the intrinsic electronic insulating nature of the charged-state elemental S 8 and discharge product (Li 2 S 2 and Li 2 S) leads to slow kinetics, low rate capability, and serious electrochemical polarizations. Secondly, dramatic volume expansion (about 80%) during the conversion reaction from S to Li 2 S brings about pulverization of the electrodes and short electrode

Preparation of MoS2/MCHS Composite
All of the chemicals were used as received. Mesoporous carbon hollow spheres used in this work were prepared by the surfactant-free method using tetrapropyl orthosilicate, resorcinol, and formaldehyde [36]. The MoS2/MCHS composite was synthesized using a simple wet impregnation method and gas phase vulcanization method. Typically, phosphomolybdic acid hydrate (34 mg) was dissolved in 5 mL of ethanol under vigorous stirring for 30 min. Then, 0.1 g of MCHS powder treated with nitric acid was dispersed in the above aqueous solution by ultrasonic method for 30 min, and dried under vacuum at 60 °C for 12 h. Finally, the sample and sulfur powder in a 1:2 mass ratio were heated under Ar atmosphere at 600 °C for 2 h with a heating rate of 5 °C/min to obtain MoS2/MCHS composite.

Preparation of the MoS2/MCHS/S and MCHS/S Composites
The MoS2/MCHS/S and MCHS/S composites were synthesized through a classic melt-diffusion strategy. Briefly, sulfur powder and MoS2/MCHS (or MCHS) in a 3:1 mass ratio were mixed uniformly in a mortar. The mixture was heated at 155 °C for 12 h in a 50 mL Teflon-lined stainlesssteel autoclave. After that, the mixture was heated at 200 °C for 1 h with a heating rate of 10 °C/min in a quartz tube filled with N2 to distribute the sulfur uniformly in MoS2/MCHS composite (or MCHS).

Preparation of MoS 2 /MCHS Composite
All of the chemicals were used as received. Mesoporous carbon hollow spheres used in this work were prepared by the surfactant-free method using tetrapropyl orthosilicate, resorcinol, and formaldehyde [36]. The MoS 2 /MCHS composite was synthesized using a simple wet impregnation method and gas phase vulcanization method. Typically, phosphomolybdic acid hydrate (34 mg) was dissolved in 5 mL of ethanol under vigorous stirring for 30 min. Then, 0.1 g of MCHS powder treated with nitric acid was dispersed in the above aqueous solution by ultrasonic method for 30 min, and dried under vacuum at 60 • C for 12 h. Finally, the sample and sulfur powder in a 1:2 mass ratio were heated under Ar atmosphere at 600 • C for 2 h with a heating rate of 5 • C/min to obtain MoS 2 /MCHS composite.

Preparation of the MoS 2 /MCHS/S and MCHS/S Composites
The MoS 2 /MCHS/S and MCHS/S composites were synthesized through a classic melt-diffusion strategy. Briefly, sulfur powder and MoS 2 /MCHS (or MCHS) in a 3:1 mass ratio were mixed uniformly in a mortar. The mixture was heated at 155 • C for 12 h in a 50 mL Teflon-lined stainless-steel autoclave. After that, the mixture was heated at 200 • C for 1 h with a heating rate of 10 • C/min in a quartz tube filled with N 2 to distribute the sulfur uniformly in MoS 2 /MCHS composite (or MCHS).

Electrochemical Measurements
The electrochemical tests were conducted on standard CR2032-type coin cells assembled in an argon filled glove box. The cathode was fabricated by mixing 70 wt.% MoS 2 /MCHS/S (or MCHS/S), with 20 wt.% carbon black (Super-P) and 10 wt.% poly(vinyl difluoride) (PVDF) in 1-methyl-2-pyrrolidinone (NMP), and the mixture was cast onto a pure Al foil. The mass loading of active materials on Al foil was about 0.5 mg cm −2 . The electrochemical performances of electrodes with a high mass loading of about 1.6 mg cm −2 were also investigated. Besides, a lithium metal foil was served as the counter electrode and separated by a Celgard 2500 membrane separator. The electrolyte was a solution of 1.0 M bis(trifluoromethane)sulfonimide lithium salt and 0.1 M lithium nitrate in dimethyl ether (DME)/dioxolane (DOL) (volume ratio: 1:1). The galvanostatic discharge-charge experiments were carried out using a CT2001A battery tester (Land Electronic Co., Ltd., Wuhan, China) over a voltage range of 1.5 V-3.0 V (vs. Li/Li + ). Cyclic voltammetry (CV) tests were conducted on an Autolab PGSTAT302N electrochemical workstation at a scan rate of 0.1 mV s −1 .

Structure and Morphology
The crystalline structure of both the MoS 2 /MCHS and MCHS structures was evaluated with XRD ( Figure 1a). The broad diffraction at around 2θ = 20-30 • corresponds to amorphous carbon characteristic peaks of MCHS. Three typical diffraction peaks at 33 • , 39 • , and 58 • can be attributed to the (100), (103), and (110) plans of the MoS 2 phase (JCPDS 37-1492), respectively [37]. An invisible peak of the (002) plane (2θ = 14 • ) suggests the presence of "graphene-like" layers that are less than five layers. This result agrees with the results of HRTEM [38]. To determine the content of MoS 2 in the MoS 2 /MCHS structures, a TGA test was performed from room temperature to 800 • C in air ( Figure 1b measurement on a micromeritics ASAP 2020 analyzer (Micromeritics Instrument corp., Atlanta, GA, USA) at 77 K. The composition of the samples was determined by X-ray diffraction (XRD; D-max-gA, Rigaku corp., Tokyo, Japan) with Cu Kα radiation from 5° to 80° (2θ). X-ray photoelectron spectroscopy (XPS) was performed using a PHI 550 spectrometer (Perkin-Elmer corp., Waltham, MA, USA) with Al Kα radiation.

Electrochemical Measurements
The electrochemical tests were conducted on standard CR2032-type coin cells assembled in an argon filled glove box. The cathode was fabricated by mixing 70 wt.% MoS2/MCHS/S (or MCHS/S), with 20 wt.% carbon black (Super-P) and 10 wt.% poly(vinyl difluoride) (PVDF) in 1-methyl-2pyrrolidinone (NMP), and the mixture was cast onto a pure Al foil. The mass loading of active materials on Al foil was about 0.5 mg cm −2 . The electrochemical performances of electrodes with a high mass loading of about 1.6 mg cm − 2 were also investigated. Besides, a lithium metal foil was served as the counter electrode and separated by a Celgard 2500 membrane separator. The electrolyte was a solution of 1.0 M bis(trifluoromethane)sulfonimide lithium salt and 0.1 M lithium nitrate in dimethyl ether (DME)/dioxolane (DOL) (volume ratio: 1:1). The galvanostatic discharge-charge experiments were carried out using a CT2001A battery tester (Land Electronic Co., Ltd., Wuhan, China) over a voltage range of 1.5-V3.0 V (vs. Li/Li + ). Cyclic voltammetry (CV) tests were conducted on an Autolab PGSTAT302N electrochemical workstation at a scan rate of 0.1 mV s −1 .

Structure and Morphology
The crystalline structure of both the MoS2/MCHS and MCHS structures was evaluated with XRD ( Figure 1a). The broad diffraction at around 2θ = 20-30° corresponds to amorphous carbon characteristic peaks of MCHS. Three typical diffraction peaks at 33°, 39°, and 58° can be attributed to the (100), (103), and (110) plans of the MoS2 phase (JCPDS 37-1492), respectively [37]. An invisible peak of the (002) plane (2θ = 14°) suggests the presence of "graphene-like" layers that are less than five layers. This result agrees with the results of HRTEM [38]. To determine the content of MoS2 in the MoS2/MCHS structures, a TGA test was performed from room temperature to 800 °C in air ( Figure  1b). The MoO3 residue after TGA comes from the oxidation of MoS2, so the proportion of MoS2 in the MoS2/MCHS structures was approximately 17.5%. The morphologies of the MoS2/MCHS and MCHS structures were observed with SEM and TEM images. The MCHS structures were prepared by one-pot, surfactant-free polymerization method, which exhibits a rough-surfaced spherical structure with an average diameter of 320 nm ( Figure S1). As shown in Figure 2a, the shape and size of the MoS2/MCHS structures are similar to those of the The morphologies of the MoS 2 /MCHS and MCHS structures were observed with SEM and TEM images. The MCHS structures were prepared by one-pot, surfactant-free polymerization method, which exhibits a rough-surfaced spherical structure with an average diameter of 320 nm ( Figure S1). As shown in Figure 2a structures decreases, which may be caused by the reduced pore diameter under the sulfidation process. Besides, there is no obvious layered structure of MoS 2 on the surface of the MCHS structures. To clarify the distribution of MoS 2 in carbon shell, EDS element mapping is exhibited in Figure 2c. As can be seen, the C, Mo, and S elements are evenly distributed in the sphere. TEM images in Figure 2d and Figure S2a,b reveal that both the MoS 2 /MCHS and MCHS structures have similar radial porous shells, the thickness of which is about 50 nm. The radial pore channels and hollow morphology of both the MoS 2 /MCHS and MCHS structures are convenient for sulfur impregnation. Additionally, such a structure can also buffer volume changes of sulfur and shorten the ion or electron diffusion distance during the charge-discharge process. The HRTEM images were investigated to prove the existence of MoS 2 . Unlike the HRTEM images of MCHS ( Figure S2c Figure 2f indicates that the interplanar spacing of crystallites is 0.62 nm, which corresponds to the lattice spacing of MoS 2 (002) plane [39]. Layered MoS 2 is successfully encapsulated in the pores of the MCHS structures, evidenced in the HRTEM images. Additionally, layered MoS 2 completely surrounded by conductive carbon may facilitate polysulfide conversion kinetics, and thus increase sulfur utilization. To clarify the distribution of MoS2 in carbon shell, EDS element mapping is exhibited in Figure 2c. As can be seen, the C, Mo, and S elements are evenly distributed in the sphere. TEM images in Figure 2d and Figure S2a,b reveal that both the MoS2/MCHS and MCHS structures have similar radial porous shells, the thickness of which is about 50 nm. The radial pore channels and hollow morphology of both the MoS2/MCHS and MCHS structures are convenient for sulfur impregnation. Additionally, such a structure can also buffer volume changes of sulfur and shorten the ion or electron diffusion distance during the charge-discharge process. The HRTEM images were investigated to prove the existence of MoS2. Unlike the HRTEM images of MCHS ( Figure S2c Figure 2f indicates that the interplanar spacing of crystallites is 0.62 nm, which corresponds to the lattice spacing of MoS2 (002) plane [39]. Layered MoS2 is successfully encapsulated in the pores of the MCHS structures, evidenced in the HRTEM images. Additionally, layered MoS2 completely surrounded by conductive carbon may facilitate polysulfide conversion kinetics, and thus increase sulfur utilization. To investigate the pore structures after introducing MoS2, nitrogen adsorption-desorption isotherms measurements were conducted. Figure 3a presents two similar N2 adsorption-desorption isotherms, which show mixed features of type-II isotherm and type-IV isotherm. Type-IV isotherm is characterized by the presence of significant hysteresis loops. Type-II isotherm represents the macropores material, while Type-IV isotherm represents the mesoporous structure. The pore size distribution plots were obtained by the Barrett-Joyner-Halenda (BJH) method (Figure 3b). The surface area and pore volume of the materials are listed in Table S1. After the introduction of MoS2, the main peak of the distribution plots shifts 6 nm towards a smaller pore-size (2 nm), indicating that the encapsulation of MoS2 in the pores of the MCHS structures leads to reduced pore diameter. In addition, the surface area of the MoS2/MCHS structure (727.32 m 2 g −1 ) is slightly smaller than that of the MCHS structure (941.62 m 2 g −1 ), suggesting a slight change of specific surface area produced by the addition of MoS2. Fortunately, the MoS2/MCHS structures basically maintain a large specific To investigate the pore structures after introducing MoS 2 , nitrogen adsorption-desorption isotherms measurements were conducted. Figure 3a presents two similar N 2 adsorption-desorption isotherms, which show mixed features of type-II isotherm and type-IV isotherm. Type-IV isotherm is characterized by the presence of significant hysteresis loops. Type-II isotherm represents the macropores material, while Type-IV isotherm represents the mesoporous structure. The pore size distribution plots were obtained by the Barrett-Joyner-Halenda (BJH) method (Figure 3b). The surface area and pore volume of the materials are listed in Table S1. After the introduction of MoS 2 , the main peak of the distribution plots shifts 6 nm towards a smaller pore-size (2 nm), indicating that the encapsulation of MoS 2 in the pores of the MCHS structures leads to reduced pore diameter. In addition, the surface area of the MoS 2 /MCHS structure (727.32 m 2 g −1 ) is slightly smaller than that of the MCHS structure (941.62 m 2 g −1 ), suggesting a slight change of specific surface area produced by the addition of MoS 2 . Fortunately, the MoS 2 /MCHS structures basically maintain a large specific surface area and a high pore volume, which is beneficial to the infiltration of elemental sulfur and the transport of lithium ions. The pore structures before and after sulfur impregnation are compared in Figure S3 to determine the distribution of sulfur. The pore volume becomes smaller at any pore diameter after sulfur impregnation, due to the S distribution across the entire sphere. Nanomaterials 2019, 9, x FOR PEER REVIEW 6 of 13 surface area and a high pore volume, which is beneficial to the infiltration of elemental sulfur and the transport of lithium ions. The pore structures before and after sulfur impregnation are compared in Figure S3 to determine the distribution of sulfur. The pore volume becomes smaller at any pore diameter after sulfur impregnation, due to the S distribution across the entire sphere.  (Figure 4b) [40]. Additionally, the peak at 227.6 eV could be attributed to the S 2s orbital of MoS2 [41]. In the high-resolution spectrum of S 2p, the peaks at 162 and 164.5 eV are assigned to S 2p3/2 and S 2p1/2, which are associated with the existence of divalent sulfide ions (S 2− ). The 165.7 eV peaks may result from the presence of the bridging disulfide S2 2− . As shown in Figure 4d, the peaks at 284.5 eV are due to the C = C bond in the MCHS structures. The results indicate that the MoS2/MCHS structures were successfully prepared in this research.  (Figure 4b) [40]. Additionally, the peak at 227.6 eV could be attributed to the S 2s orbital of MoS 2 [41]. In the high-resolution spectrum of S 2p, the peaks at 162 and 164.5 eV are assigned to S 2p 3/2 and S 2p 1/2 , which are associated with the existence of divalent sulfide ions (S 2− ). The 165.7 eV peaks may result from the presence of the bridging disulfide S 2 2− . As shown in Figure 4d, the peaks at 284.5 eV are due to the C = C bond in the MCHS structures. The results indicate that the MoS 2 /MCHS structures were successfully prepared in this research. Figure S4a,b show that the morphology of both the MCHS and MoS 2 /MCHS structures were not obviously changed after sulfur impregnation. TGA data were also used to analyze the weight content and thermal stability of sulfur in the MoS 2 /MCHS/S composites, which were obtained between room temperature and 400 • C in N 2 atmosphere ( Figure S5). Considering that the sublimation of elemental sulfur is the reason for the weight loss, the contents of sulfur in both the MCHS/S and MoS 2 /MCHS/S composites are 71.5 and 72.6 wt %, respectively. In addition, the better thermal stability and sulfur retention ability of the MoS 2 /MCHS/S composites are observed due to the higher initial decomposition temperature and lower decomposition rate in early decay. The presence of MoS 2 not only does not decrease the storage space of sulfur, but can load more sulfur on account of the stronger absorption.
A simple visual adsorption test was conducted to verify the interactive activity of the MoS 2 /MCHS structures and the soluble lithium polysulfide ( Figure S6). The Li 2 S 6 solution (0.01 M) with reddish brown color in Figure S6c is prepared by dissolving a stoichiometric amount of sulfur and Li 2 S in a 1:1 (v/v) DOL/DME solvent. The solution color changes from reddish brown to yellow after the addition of the MCHS structures owing to the physical absorptivity towards lithium polysulfides ( Figure S6b). In sharp contrast, the solution is almost completely discolored after adding the MoS 2 /MCHS structures to the lithium polysulfide solution ( Figure S6a). This might be responsible for the synergistic effects from the physical adsorption of the mesoporous carbon hollow spheres and the chemical bond between polar MoS 2 and polysulfide. The strong interaction between the MoS 2 /MCHS structures and lithium polysulfide is beneficial for suppressing the "shuttle effect" of polysulfide and the destruction of Li anodes.  Figure S4a,b show that the morphology of both the MCHS and MoS2/MCHS structures were not obviously changed after sulfur impregnation. TGA data were also used to analyze the weight content and thermal stability of sulfur in the MoS2/MCHS/S composites, which were obtained between room temperature and 400 °C in N2 atmosphere ( Figure S5). Considering that the sublimation of elemental sulfur is the reason for the weight loss, the contents of sulfur in both the MCHS/S and MoS2/MCHS/S composites are 71.5 and 72.6 wt %, respectively. In addition, the better thermal stability and sulfur retention ability of the MoS2/MCHS/S composites are observed due to the higher initial decomposition temperature and lower decomposition rate in early decay. The presence of MoS2 not only does not decrease the storage space of sulfur, but can load more sulfur on account of the stronger absorption.
A simple visual adsorption test was conducted to verify the interactive activity of the MoS2/MCHS structures and the soluble lithium polysulfide ( Figure S6). The Li2S6 solution (0.01 M) with reddish brown color in Figure S6c is prepared by dissolving a stoichiometric amount of sulfur and Li2S in a 1:1 (v/v) DOL/DME solvent. The solution color changes from reddish brown to yellow after the addition of the MCHS structures owing to the physical absorptivity towards lithium polysulfides ( Figure S6b). In sharp contrast, the solution is almost completely discolored after adding the MoS2/MCHS structures to the lithium polysulfide solution ( Figure S6a). This might be responsible for the synergistic effects from the physical adsorption of the mesoporous carbon hollow spheres and the chemical bond between polar MoS2 and polysulfide. The strong interaction between the MoS2/MCHS structures and lithium polysulfide is beneficial for suppressing the "shuttle effect" of polysulfide and the destruction of Li anodes.

Electrochemical Performance
The typical CV curves of both the MoS 2 /MCHS/S cathodes and MCHS/S cathodes were measured over a voltage range of 1.5-3.0 V at a scan rate of 0.1 mV s −1 (Figure 5a and Figure S7). In Figure 5a, the CV curves of the MoS 2 /MCHS/S cathode show two representative reduction peaks at 2.03 and 2.32 V, corresponding to the step-wise reduction of S 8 to the long-chain polysulfides (Li 2 S n , 4 ≤ n ≤ 8) and short-chain polysulfides (Li 2 S 2 /Li 2 S), respectively [41]. The reverse distinguishable oxidation peaks located at 2.49 and 2.68 V are associated with the formation of long-chain polysulfides and elemental sulfur, respectively, suggesting good reaction kinetics. In contrast, two merging oxidation peaks at around 2.52 V are observed in the CV curves of the MCHS/S cathode ( Figure S7), indicating the two-step delithiation process. Furthermore, higher peak current and larger CV enclosed area of the MoS 2 /MCHS/S cathode also indicate the faster electrochemical kinetics (Figure 5b). The potential gap between oxidation and reduction peaks of the MoS 2 /MCHS/S cathodes (0.46 V) are lower than that of the MCHS/S cathodes (0.73 V), which illustrates a lower cell polarization and faster Li ions diffusion in the MoS 2 /MCHS/S cathode [42]. The above analyses suggest that the uniform dispersion of MoS 2 in the MCHS matrix facilitates the capture of polysulfides and boosts the conversion rates of polysulfides.
The galvanostatic charge-discharge profiles of both the MoS 2 /MCHS/S electrode and the MCHS/S electrode at various currents are shown in Figure 6a,b. Two representative discharge plateaus can be observed in the curves of both the MoS 2 /MCHS/S electrode and MCHS/S electrode. At the current rate of 0.1 C, the upper discharge flat at 2.3 V is related to the transformation from sulfur to long-chain polysulfides, while the lower plateau at 2.1 V versus Li/Li + is attributed to the formation of short-chain lithium polysulfides [43]. This result is in agreement with the CV analysis. In Figure 6b, the low potential of around 1.8 V corresponds to the conversion from Li 2 S 2 to Li 2 S [44]. With the increase of the current rate, the voltage of the discharge plateau is more negative and the voltage of the charge flat is more positive, indicating greater polarization. It is noticeable that the polarization of the MoS 2 /MCHS/S cathode is smaller than that of the MCHS/S cathode, especially at high current rate. The clearly visible voltage platform of the MoS 2 /MCHS/S composite can be observed even at the 4 C rate, suggesting a fast electrode reaction. Meanwhile, in comparison to the MCHS/S cathode, the MoS 2 /MCHS/S cathode has a longer plateau due to the strong interaction between soluble polysulfides and MoS 2 , as well as high utilization percentage of sulfur. Figure 5a, the CV curves of the MoS2/MCHS/S cathode show two representative reduction peaks at 2.03 and 2.32 V, corresponding to the step-wise reduction of S8 to the long-chain polysulfides (Li2Sn, 4 ≤ n ≤ 8) and short-chain polysulfides (Li2S2/Li2S), respectively [41]. The reverse distinguishable oxidation peaks located at 2.49 and 2.68 V are associated with the formation of long-chain polysulfides and elemental sulfur, respectively, suggesting good reaction kinetics. In contrast, two merging oxidation peaks at around 2.52 V are observed in the CV curves of the MCHS/S cathode ( Figure S7), indicating the two-step delithiation process. Furthermore, higher peak current and larger CV enclosed area of the MoS2/MCHS/S cathode also indicate the faster electrochemical kinetics (Figure 5b). The potential gap between oxidation and reduction peaks of the MoS2/MCHS/S cathodes (0.46 V) are lower than that of the MCHS/S cathodes (0.73 V), which illustrates a lower cell polarization and faster Li ions diffusion in the MoS2/MCHS/S cathode [42]. The above analyses suggest that the uniform dispersion of MoS2 in the MCHS matrix facilitates the capture of polysulfides and boosts the conversion rates of polysulfides.
. At the current rate of 0.1 C, the upper discharge flat at 2.3 V is related to the transformation from sulfur to long-chain polysulfides, while the lower plateau at 2.1 V versus Li/Li + is attributed to the formation of short-chain lithium polysulfides [43]. This result is in agreement with the CV analysis. In Figure 6b, the low potential of around 1.8 V corresponds to the conversion from Li2S2 to Li2S [44]. With the increase of the current rate, the voltage of the discharge plateau is more negative and the voltage of the charge flat is more positive, indicating greater polarization. It is noticeable that the polarization of the MoS2/MCHS/S cathode is smaller than that of the MCHS/S cathode, especially at high current rate. The clearly visible voltage platform of the MoS2/MCHS/S composite can be observed even at the 4 C rate, suggesting a fast electrode reaction. Meanwhile, in comparison to the MCHS/S cathode, the MoS2/MCHS/S cathode has a longer plateau due to the strong interaction between soluble polysulfides and MoS2, as well as high utilization percentage of sulfur. The rate capabilities of both the MoS2/MCHS/S cathode and the MCHS/S cathode are displayed in Figure S8. The discharge capacities of the MoS2/MCHS/S cathodes are 1680.6, 1094.3, 838.6, 667.6, 590.2, and 453.9 mAh g −1 at rates of 0.1, 0.2, 0.5, 1, 2, and 4 C, respectively. When the current rate returns to 0.1 C, the specific capacity of the MoS2/MCHS/S cathode is maintained at a high reversible capacity of 1037.3 mAh g −1 , implying a good reversibility. Compared with the MCHS/S electrode, the MoS2/MCHS/S electrode remarkably displays an enhanced specific capacity at high current rates (two times higher at 4 C).
Cycling performances of the MCHS/S and MoS2/MCHS/S cathodes at the 0.2 C rate are compared in Figure 6c. The MCHS/S cathode exhibits a lower initial specific capacity (1056.2 mAh g −1 ) and a The rate capabilities of both the MoS 2 /MCHS/S cathode and the MCHS/S cathode are displayed in Figure S8. The discharge capacities of the MoS 2 /MCHS/S cathodes are 1680.6, 1094.3, 838.6, 667.6, 590.2, and 453.9 mAh g −1 at rates of 0.1, 0.2, 0.5, 1, 2, and 4 C, respectively. When the current rate returns to 0.1 C, the specific capacity of the MoS 2 /MCHS/S cathode is maintained at a high reversible capacity of 1037.3 mAh g −1 , implying a good reversibility. Compared with the MCHS/S electrode, the MoS 2 /MCHS/S electrode remarkably displays an enhanced specific capacity at high current rates (two times higher at 4 C).
Cycling performances of the MCHS/S and MoS 2 /MCHS/S cathodes at the 0.2 C rate are compared in Figure 6c. The MCHS/S cathode exhibits a lower initial specific capacity (1056.2 mAh g −1 ) and a severe capacity fading rate of 59.86% after 100 cycles. One possible reason is that the "shuttle effect" caused by soluble polysulfide occurs in this cathode system. In contrast, the MoS 2 /MCHS/S cathode shows a higher discharge of 1079.5 mAh g −1 and a reduced capacity decay rate of 37.40%, indicating that MoS 2 can indeed trap the dissolved polysulfide and effectively suppress the "shuttle effect". The electrochemical performance of electrodes with a high mass loading of about 1.6 mg cm −2 was also investigated in Figure S9. The MoS 2 /MCHS/S cathodes with a relatively high mass loading exhibited comparable specific capacity and cycle performance. Figure S9 compares the cycling performances of the MCHS/S and MoS 2 /MCHS/S cathodes with a high mass loading at the 1.0 C rate. The MCHS/S cathode shows a capacity fading rate of 27.08% after 100 cycles, while the MoS 2 /MCHS/S cathode displays an obviously improved capacity fading rate of 5.07% after 100 cycles. The MoS 2 /MCHS/S cathodes exhibit less capacity decay than the MoS 2 /MCHS/S cathodes at both high mass loading and low mass loading conditions, indicating the superiority of cathode design strategy. It is worth noting that the MoS 2 /MCHS/S electrode displays a significantly improved long-term cycling stability at a higher current rate (2 C). As shown in Figure 6d, the MoS 2 /MCHS/S cathode delivers a high initial discharge capacity of 639.9 mAh g −1 and a high capacity retention rate of 77.65% is obtained after 400 cycles. However, for the MCHS/S cathode, its initial specific capacity and capacity retention rate are 551.8 mAh g −1 and 47.3%, respectively. Compared with the MCHS/S cathode, the electrochemical performances of the MoS 2 /MCHS/S cathode have been unambiguously improved regarding the aspects of rate capability and cycling performance. These results can be ascribed to the unique structure of the MoS 2 /MCHS/S composite. Specifically, by introducing polar MoS 2 in the pores of the carbon shell, the polysulfides, which are generated during the charge and discharge process, can be trapped due to the chemical interaction. Meanwhile, the conductive carbon is tight around the ultrathin multi-layer MoS 2 nanosheet and can provide enough electrons for the redox reaction to facilitate polysulfide conversion. It is worth mentioning that there are enough diffusion paths of Li ions in the MoS 2 /MCHS/S composites, considering the abundant pore structures. Additionally, as Figure S10 shows, the MoS 2 /MCHS/S spheres can retain their morphology after cycling, demonstrating that our material can suppress the volume changes during the repeated sulfur conversion processes. Hence, the delicately-designed MoS 2 /MCHS/S structure is beneficial to accelerate the sulfur conversion kinetics and the synergistic effect could be achieved between physical adsorption of the MCHS structure and the chemical trap of polar MoS 2 , both of which contribute to increased sulfur utilization, improved rate capability, and superior cycling performance.

Conclusions
In conclusion, a simple wet impregnation method and gas phase vulcanization method have been developed to synthesize the unique MoS 2 /MCHS structure as a sulfur host for lithium-sulfur batteries. The intriguing aspect of the architecture is the encapsulation of ultrathin, multi-layer MoS 2 nanosheets in the pores of mesoporous carbon hollow spheres. On one hand, conductive mesoporous carbon hollow spheres can improve the electrical conductivity of sulfur cathodes, shorten the Li ion diffusion distance, and buffer volume changes of sulfur. On the other hand, polar MoS 2 nanosheets uniformly distributed in the mesoporous carbon shell act as the polysulfide-trapping center, where soluble polysulfides are largely anchored and transformed. As expected, the MoS 2 /MCHS/S electrode exhibits a high specific capacity (1094.3 mAh g −1 , 0.2 C), good rate capability (590.2 mAh g −1 , 2 C), and excellent cycling stability (77.65 % capacity retention after 400 cycles at 2 C). The unique electrode design strategy and innovative structure are expected to provide new ideas and versatile methods for fabrication of layered transition metal compounds, which may provide more opportunities for the development of advanced sulfur-based and metal sulfide-based electrode materials.