MnO2/rGO/CNTs Framework as a Sulfur Host for High-Performance Li-S Batteries.

Lithium-sulfur batteries are very promising next-generation energy storage batteries due to their high theoretical specific capacity. However, the shuttle effect of lithium-sulfur batteries is one of the important bottlenecks that limits its rapid development. Herein, physical and chemical dual adsorption of lithium polysulfides are achieved by designing a novel framework structure consisting of MnO2, reduced graphene oxide (rGO), and carbon nanotubes (CNTs). The framework-structure composite of MnO2/rGO/CNTs is prepared by a simple hydrothermal method. The framework exhibits a uniform and abundant mesoporous structure (concentrating in ~12 nm). MnO2 is an α phase structure and the α-MnO2 also has a significant effect on the adsorption of lithium polysulfides. The rGO and CNTs provide a good physical adsorption interaction and good electronic conductivity for the dissolved polysulfides. As a result, the MnO2/rGO/CNTs/S cathode delivered a high initial capacity of 1201 mAh g−1 at 0.2 C. The average capacities were 916 mAh g−1, 736 mAh g−1, and 547 mAh g−1 at the current densities of 0.5 C, 1 C, and 2 C, respectively. In addition, when tested at 0.5 C, the MnO2/rGO/CNTs/S exhibited a high initial capacity of 1010 mAh g−1 and achieved 780 mAh g−1 after 200 cycles, with a low capacity decay rate of 0.11% per cycle. This framework-structure composite provides a simple way to improve the electrochemical performance of Li-S batteries.


Introduction
With the development of science and technology, the most widely used lithium-ion battery has gradually failed to meet the needs of technological development due to its limited capacity [1,2]. High energy density is the key point of battery development [3,4]. In order to further improve the capacity of secondary batteries, researchers turned their research attention to other battery systems with high energy densities. Among them, the Li-S battery system has attracted widespread attention due to its high theoretical capacity of 1672 mAh g −1 , which is much more than that of Li-ion batteries (~372 mAh g −1 based on graphite anodes) [5]. Therefore, the Li-S batteries have become one of the key research focuses for the next generation battery system, with great developmental potential [6,7].
The typical discharge reaction of Li-S batteries is 16Li + S 8 →8Li 2 S [8]. During this reaction process, a series of soluble intermediates Li 2 S x (Li 2 S 4 , Li 2 S 6 , and Li 2 S 8 ) are produced, which can dissolve in the electrolyte and move between the positive and negative electrodes. This phenomenon is often called the shuttle effect, causing the negative electrode to corrode and the capacity to be significantly reduced. The shuttle effect is one of the main factors limiting the development of Li-S batteries. Physical adsorption and chemical adsorption are two commonly used methods to limit the shuttling of lithium polysulfides in lithium-sulfur batteries. Various porous materials are adopted to block the polysulfides in the pores by physical adsorption. The chemical adsorption can be achieved by the chemical bonding interaction between the polar sulfur hosts and lithium polysulfides. Herein, a carbon-based porous composite containing MnO 2 is designed as a sulfur host to achieve the dual adsorption interaction to improve the electrochemical performance of lithium-sulfur batteries. The developed host material was melted with sulfur at 155 • C and served as a cathode in lithium-sulfur batteries. Physical adsorption materials mainly include carbon materials, such as porous carbon [9], graphene [10], carbon nanotubes [11], and carbon fibers [12], and rely on the large specific surface area [13]. Chemical adsorption materials generally have higher polarity and can form chemical bonds with polysulfides. Therefore, polar molecules can be used to inhibit polysulfide dissolution by producing dipole attraction to polysulfide molecules. Compared with carbon materials without polarity, the interaction between polar materials and polysulfide molecules is greatly enhanced. Among the polar materials, metal oxides are important adsorption materials, including TiO 2 [14], SiO 2 [15], Ti 4 O 7 [16], Al 2 O 3 [17], MgO [18], Co 9 S 8 [19], MoS 2 [20], etc. These materials have a significant effect on the improvement of cycle performance. However, the problem of polar materials is the poor electronic conductivity. Both sulfur and the intermediate products of lithium polysulfides have poor electronic conductivity. Therefore, the sulfur host must have a good electronic conductivity to maintain the electron transfer. In addition, from the EIS test, good conductivity of the sulfur host will induce a low internal resistance and fast reaction kinetics of sulfur. Therefore, the electronic conductivity of the sulfur host is the key factor for deciding the cell performance. In order to improve the electrochemical performance, a regular conductive matrix is urgently needed.
MnO 2 is a highly polar material that is relatively cheap and easily available [21,22]. It has been widely researched in lithium ion batteries [23,24]. There are four phases of MnO 2 , α, β, γ, and δ. Recently, MnO 2 was proposed as a sulfur host in Li-S batteries. For instance, Liang et al. [25] designed a polysulfide mediator δ-MnO 2 for Li-S batteries that displayed an initial capacity of 1300 mA h g −1 at 0.05 C. At the same time, when the S content was 75%, it still had strong chemical adsorption performance. Chen et al. [21] developed a hollow nitrogen-doped micropore-rich carbon (NMRC)@MnO 2 nanocomposite framework as the sulfur host for advanced Li-S batteries. The polar MnO 2 nanosheets and doped nitrogen atoms present a strong chemisorption to lithium polysulfides. Li et al. [26] found that the outstanding performance might be attributed to a combination of adsorption, catalytic properties of MnO 2 , and the conductivity network of carbon. Fernando et al. [27] synthesized a framework consisting of tailored γ-MnO 2 nanorods and an activated biomass-derived carbon (AC/MnO 2 ) as the sulfur host. The initial discharge capacity of the AC/MnO 2 /S composite was 874 mAh g −1 at 0.1 C, much higher than that of the AC/S composite (692 mAh g −1 ). A β-MnO 2 framework for Li-S batteries was also prepared and exhibited good cycling stability [28], because the β-MnO 2 /S offers the advantage of rapid Li + transport through the mesoporous walls of β-MnO 2 , when compared with that of the mesoporous carbon/S composites.
The α-MnO 2 has a three-dimensional open channel structure that can accommodate metal atoms. It has been widely applied in catalysts, and has been proven to have the highest catalytic activity among the four structures (α, β, γ, and δ-MnO 2 ) [29,30]. Based on this, α-MnO 2 may also be used as an adsorbent for polysulfides. However, there are few studies on α-MnO 2 in Li-S batteries. The interactions between the polysulfides and α-MnO 2 should be further explored. Meanwhile, the combination of insulating α-MnO 2 with a conductive matrix is also necessary for improving its performance [31]. Herein, physical and chemical dual adsorption of lithium polysulfides is proposed by designing a novel MnO 2 /rGO/CNTs framework structure consisting of α-MnO 2 nanorods, reduced graphene oxide (rGO), and carbon nanotubes (CNTs), which is prepared by a simple hydrothermal method. This novel framework structure could provide a simple way to confine the shuttling of dissolved polysulfides in Li-S batteries.

Microstructure and Composition
The preparation process is schematically illustrated in Figure 1. The pure MnO 2 was obtained only by the direct hydrothermal reaction. The reduced graphene oxide (rGO) was obtained through two steps of ultrasonic and hydrothermal reactions from graphite oxide. Serving as a template, rGO was used to generate MnO 2 in situ, then, the composite of rGO/MnO 2 was obtained after the addition of KMnO 4 and H 3 PO 4 . One half of the GO was replaced by oxidized CNTs and the other conditions were maintained with the rGO/MnO 2 . The MnO 2 /rGO/CNTs framework was easily obtained.
Molecules 2020, 25, x FOR PEER REVIEW 3 of 11 The preparation process is schematically illustrated in Figure 1. The pure MnO2 was obtained only by the direct hydrothermal reaction. The reduced graphene oxide (rGO) was obtained through two steps of ultrasonic and hydrothermal reactions from graphite oxide. Serving as a template, rGO was used to generate MnO2 in situ, then, the composite of rGO/MnO2 was obtained after the addition of KMnO4 and H3PO4. One half of the GO was replaced by oxidized CNTs and the other conditions were maintained with the rGO/MnO2. The MnO2/rGO/CNTs framework was easily obtained. In order to further characterize the microstructure of the samples, a scanning electron microscope (SEM) was used, as shown in Figure 2. It can be observed from Figure 2 that the MnO2 is composed of many hollow urchin-like pompons with diameters of about 3~6 μm. The surface of the urchin-like pompons consists of many fine nanorods with a diameter of about 20 nm. The growth mechanism of the urchin-like MnO2 structure can be explained by the Ostwald ripening process [32]. The so-called Ostwald ripening refers to the phenomenon where the particles of the second phase grow up at the cost of the dissolution of the first phase particles, driven by the surface energy difference [33]. Generally, permanganate is thermodynamically unstable and can be easily reduced to produce MnO2 (4MnO4 -+ 4H + = 4MnO2 + 3O2 + 2H2O). In an acidic environment or at high temperatures, the reaction occurs spontaneously and rapidly. In the initial stage of the reaction, a large number of manganese dioxide nuclei are generated in a short period of time, and these nuclei are continuously aggregated to form microspheres with a solid core. These microspheres will grow into a one-dimensional MnO2 nanorod as a core, and the nanorods grow epitaxially along the surface of the initial microsphere to form an urchin-like nanostructure. From Figure 2b, it can be seen that rGO is composed of many irregular yarns, more like flakes instead of the regular graphite structure, which indicates that the regular structure of graphite was seriously damaged by oxidation, ultrasonic treatment, and subsequent hydrothermal treatment. Figure 2c shows the morphology of the MnO2/rGO composite. The urchin-like MnO2 is attached to the surface and the defects of rGO. At the same time, the MnO2 and rGO are interwoven and combined perfectly, and the composite has abundant big holes. When CNTs were added into the system of MnO2 and rGO, the morphology of the composite was changed to some extent, as shown in Figure 2d. The MnO2 in the MnO2/rGO/CNTs composite was no longer urchin-like, the MnO2 short nanorods were combined with CNTs and rGO to form a framework-structure composite, which may be attributed to the nucleation particles of  In order to further characterize the microstructure of the samples, a scanning electron microscope (SEM) was used, as shown in Figure 2. It can be observed from Figure 2 that the MnO 2 is composed of many hollow urchin-like pompons with diameters of about 3~6 µm. The surface of the urchin-like pompons consists of many fine nanorods with a diameter of about 20 nm. The growth mechanism of the urchin-like MnO 2 structure can be explained by the Ostwald ripening process [32]. The so-called Ostwald ripening refers to the phenomenon where the particles of the second phase grow up at the cost of the dissolution of the first phase particles, driven by the surface energy difference [33]. Generally, permanganate is thermodynamically unstable and can be easily reduced to produce MnO 2 (4MnO 4 -+ . In an acidic environment or at high temperatures, the reaction occurs spontaneously and rapidly. In the initial stage of the reaction, a large number of manganese dioxide nuclei are generated in a short period of time, and these nuclei are continuously aggregated to form microspheres with a solid core. These microspheres will grow into a one-dimensional MnO 2 nanorod as a core, and the nanorods grow epitaxially along the surface of the initial microsphere to form an urchin-like nanostructure. From Figure 2b, it can be seen that rGO is composed of many irregular yarns, more like flakes instead of the regular graphite structure, which indicates that the regular structure of graphite was seriously damaged by oxidation, ultrasonic treatment, and subsequent hydrothermal treatment. Figure  and combined perfectly, and the composite has abundant big holes. When CNTs were added into the system of MnO 2 and rGO, the morphology of the composite was changed to some extent, as shown in Figure 2d. The MnO 2 in the MnO 2 /rGO/CNTs composite was no longer urchin-like, the MnO 2 short nanorods were combined with CNTs and rGO to form a framework-structure composite, which may be attributed to the nucleation particles of oxidized CNTs. From the HRTEM images of MnO 2 /rGO/CNTs, the MnO 2 short nanorods (diameter of 50 nm and length of about 200 nm) were compounded with carbon nanotubes (diameter of 20-50 nm) and tulle-like rGO (Figure 2g). Meanwhile, the HRTEM image ( Figure 2f) of a single nanorod shows a lattice spacing of 0.5 nm, which corresponds to the (200) crystal plane spacing of α-MnO 2 [34].  The obtained rGO, MnO2, MnO2/rGO, and MnO2/rGO/CNTs were characterized by X-ray diffraction (XRD), as shown in Figure 3a. The diffraction spectra of the obtained MnO2 can be well matched to α-MnO2 (JSCD No.44-0144). The intensity of MnO2 diffraction peaks are low, and the full width at half maxima (FWHM) is large, which indicates that the grain size of the synthesized MnO2 is smaller. The rGO was obtained after ultrasonic and hydrothermal treatment; a broad peak at 24° and a very weak peak at 43° appeared, which were corresponded to the (002) and (101) diffractions of the carbon materials, respectively. However, compared with GO the crystallinity of rGO is greatly reduced. The patterns of the MnO2/rGO and MnO2/rGO/CNTs are quite similar with two diffraction spectra that could be well indexed to α-MnO2 (JSCD No.44-0144), indicating that the MnO2 synthesized is α phase. Except for the characteristic diffraction peak of α-MnO2, a broad peak at 24° and a very weak peak at 43°, corresponding to the diffractions of the carbon materials, were found, indicating the presence of carbon. The thermal stability was characterized by thermal gravimetric analysis (TGA) in air, as given in Figure S1. The content of MnO2 in MnO2/rGO and MnO2/rGO/CNTs are about 49.6 wt% and 50.8 wt%, respectively. The MnO2 content of the two samples is almost the same. The diffraction spectra of rGO/S, MnO2/S, MnO2/rGO/S, and MnO2/rGO/CNTs/S are shown in Figure 3b. The only phase that can be clearly distinguished is S, and neither carbon (rGO and CNTs) nor MnO2 were detected, due to their lower content and crystallinity. Figure 3c,d shows the N2 adsorption-desorption isotherm and pore size distribution curves of MnO2/rGO and MnO2/rGO/CNTs. The N2 adsorption-desorption isotherm of MnO2/rGO exhibits the type III isotherm and H3 hysteresis loop (Figure 3c), indicating a mesoporous or macroporous structure, which is given in the pore size distribution (Figure 3d). MnO2/rGO has a specific surface area of 109 m 2 g −1 and total pore volume of 0.42 cm 3 g −1 . The N2 adsorption-desorption isotherm of MnO2/rGO/CNTs exhibits the type IV isotherm and H1 hysteresis loop (Figure 3c), indicating a uniform mesoporous structure, as given in the pore size distribution (Figure 3d), the pore was concentrated in ~12 nm. The MnO2/rGO/CNTs composite has a higher specific surface area of 232 m 2 g −1 and total pore volume of 0.55 cm 3 g −1 . These abundant mesopores are crucial for achieving high S The obtained rGO, MnO 2 , MnO 2 /rGO, and MnO 2 /rGO/CNTs were characterized by X-ray diffraction (XRD), as shown in Figure 3a. The diffraction spectra of the obtained MnO 2 can be well matched to α-MnO 2 (JSCD No.44-0144). The intensity of MnO 2 diffraction peaks are low, and the full width at half maxima (FWHM) is large, which indicates that the grain size of the synthesized MnO 2 is smaller. The rGO was obtained after ultrasonic and hydrothermal treatment; a broad peak at 24 • and a very weak peak at 43 • appeared, which were corresponded to the (002) and (101) diffractions of the carbon materials, respectively. However, compared with GO the crystallinity of rGO is greatly reduced. The patterns of the MnO 2 /rGO and MnO 2 /rGO/CNTs are quite similar with two diffraction spectra that could be well indexed to α-MnO 2 (JSCD No.44-0144), indicating that the MnO 2 synthesized is α phase. Except for the characteristic diffraction peak of α-MnO 2 , a broad peak at 24 • and a very weak peak at 43 • , corresponding to the diffractions of the carbon materials, were found, indicating the presence of carbon. The thermal stability was characterized by thermal gravimetric analysis (TGA) in air, as given in Figure S1. The content of MnO 2 in MnO 2 /rGO and MnO 2 /rGO/CNTs are about 49.6 wt% and 50.8 wt%, respectively. The MnO 2 content of the two samples is almost the same. The diffraction spectra of rGO/S, MnO 2 /S, MnO 2 /rGO/S, and MnO 2 /rGO/CNTs/S are shown in Figure 3b. The only phase that can be clearly distinguished is S, and neither carbon (rGO and CNTs) nor MnO 2 were detected, due to their lower content and crystallinity. Figure 3c,d shows the N 2 adsorption-desorption isotherm and pore size distribution curves of MnO 2 /rGO and MnO 2 /rGO/CNTs. The N 2 adsorption-desorption isotherm of MnO 2 /rGO exhibits the type III isotherm and H3 hysteresis loop (Figure 3c), indicating a mesoporous or macroporous structure, which is given in the pore size distribution (Figure 3d). MnO 2 /rGO has a specific surface area of 109 m 2 g −1 and total pore volume of 0.42 cm 3 g −1 . The N 2 adsorption-desorption isotherm of MnO 2 /rGO/CNTs exhibits the type IV isotherm and H1 hysteresis loop (Figure 3c), indicating a uniform mesoporous structure, as given in the pore size distribution (Figure 3d), the pore was concentrated iñ 12 nm. The MnO 2 /rGO/CNTs composite has a higher specific surface area of 232 m 2 g −1 and total pore volume of 0.55 cm 3 g −1 . These abundant mesopores are crucial for achieving high S loading and confining lithium polysulfides inside the framework of MnO 2 /rGO/CNTs. The porous framework of MnO 2 /rGO/CNTs not only facilitates the transportation of electrolytes, but also provides abundant active sites for the adsorption of lithium polysulfides.

Electrochemical Performance
The electrochemical performance of the as-prepared rGO/S, MnO2/S, MnO2/rGO/S, and MnO2/rGO/CNTs/S cathodes were evaluated by galvanostatic charge-discharge measurements, as shown in Figure 4. The charge/discharge curves of the four samples at 0.2 C are presented in Figure  4a. There are two main stages in the discharge curves at about 2.3 V and 2.1 V. The high voltage platform is a short platform ascribed to the formation of long-chain lithium polysulfides (Li2S8~Li2S4). The low voltage platform is a long platform ascribed to the formation of short chain polysulfides (Li2S2 and Li2S). The as-prepared rGO/S, MnO2/S, MnO2/rGO/S, and MnO2/rGO/CNTs/S cathodes delivered initial discharge capacities of 1059 mAh g −1 , 640 mAh g −1 , 1134 mAh g −1 , and 1266 mAh g −1 , respectively. The initial discharge capacities of rGO/S, MnO2/rGO/S, and MnO2/rGO/CNTs/S samples are not significantly different, indicating the Coulombic efficiencies of these samples are similar. The initial discharge capacity of MnO2/S is relatively low, indicating the sulfur utilization rate is low, which may be related to the poor conductivity of MnO2 hosts.
The cycling performance of rGO/S, MnO2/S, MnO2/rGO/S, and MnO2/rGO/CNTs/S cathodes are presented in Figure 4b. With the increasing of cycling number, the capacity of the four samples decreased gradually. The capacity of MnO2/rGO/CNTs/S remained the highest (826 mAh g −1 ) after 80 cycles at 0.2 C, which is much higher that other samples. It can be seen from the cycling performance of the above materials that the initial discharge capacity of rGO/S is relatively high, but the capacity

Electrochemical Performance
The electrochemical performance of the as-prepared rGO/S, MnO 2 /S, MnO 2 /rGO/S, and MnO 2 /rGO/CNTs/S cathodes were evaluated by galvanostatic charge-discharge measurements, as shown in Figure 4. The charge/discharge curves of the four samples at 0.2 C are presented in Figure 4a. There are two main stages in the discharge curves at about 2.3 V and 2.1 V. The high voltage platform is a short platform ascribed to the formation of long-chain lithium polysulfides (Li 2 S 8~L i 2 S 4 ). The low voltage platform is a long platform ascribed to the formation of short chain polysulfides (Li 2 S 2 and Li 2 S). The as-prepared rGO/S, MnO 2 /S, MnO 2 /rGO/S, and MnO 2 /rGO/CNTs/S cathodes delivered initial discharge capacities of 1059 mAh g −1 , 640 mAh g −1 , 1134 mAh g −1 , and 1266 mAh g −1 , respectively. The initial discharge capacities of rGO/S, MnO 2 /rGO/S, and MnO 2 /rGO/CNTs/S samples are not significantly different, indicating the Coulombic efficiencies of these samples are similar. The initial discharge capacity of MnO 2 /S is relatively low, indicating the sulfur utilization rate is low, which may be related to the poor conductivity of MnO 2 hosts.
The cycling performance of rGO/S, MnO 2 /S, MnO 2 /rGO/S, and MnO 2 /rGO/CNTs/S cathodes are presented in Figure 4b. With the increasing of cycling number, the capacity of the four samples decreased gradually. The capacity of MnO 2 /rGO/CNTs/S remained the highest (826 mAh g −1 ) after 80 cycles at 0.2 C, which is much higher that other samples. It can be seen from the cycling performance of the above materials that the initial discharge capacity of rGO/S is relatively high, but the capacity retention rate is the lowest, indicating that the adsorption of lithium polysulfides is poor. Although the initial capacity of MnO 2 /S is lower, the capacity retention rate is relatively high, which proves to some extent that α-MnO 2 has a significant effect on the adsorption of lithium polysulfides. The cycle performance of MnO 2 /rGO/S is better than rGO/S and MnO 2 /S, indicating that the combination of MnO 2 and rGO is beneficial to electrochemical performance. After replacing some rGO with CNTs, the three-dimensional frame structure of MnO 2 /rGO/CNTs is established. The capacity and capacity retention rate of the composite increased significantly, indicating that MnO 2 /rGO/CNTs framework structure effectively improved the electrochemical performance by introducing the conductive CNTs. This is related to the pore size distribution of the three-dimensional sulfur-loaded framework structure and the synergistic effect of rGO and CNTs.
The rate performance of rGO/S, MnO 2 /S, MnO 2 /rGO/S, and MnO 2 /rGO/CNTs/S cathodes are presented in Figure 4c. Among them, MnO 2 /rGO/CNTs/S has the best rated performance. The average capacity was 1080 mAh g −1 at 0.2 C, and then decreased to 916 mAh g −1 at 0.5 C, 736 mAh g −1 at 1 C, and 547 mAh g −1 at 2 C. When the current density returned to 0.2 C, the average capacity recovered to 920 mAh g −1 , which is close to its original capacity, indicating a good rate capability in a wide range. This performance may be related to the better conductivity of the materials. In addition, the MnO 2 /rGO/CNTs/S cathode delivered a high initial capacity of 1010 mAh g −1 at 0.5 C and achieved 780 mAh g −1 after 200 cycles (Figure 4d), with a high capacity retention of 77.2%. The capacity decay rate is 0.11% per cycle. Moreover, when compared with the reported MnO 2 -containing composite hosts (Table S1), the MnO 2 /rGO/CNTs/S cathode delivers a comparable or even better electrochemical performance [21,27,[35][36][37][38][39][40].
Molecules 2020, 25, x FOR PEER REVIEW 6 of 11 retention rate is the lowest, indicating that the adsorption of lithium polysulfides is poor. Although the initial capacity of MnO2/S is lower, the capacity retention rate is relatively high, which proves to some extent that α-MnO2 has a significant effect on the adsorption of lithium polysulfides. The cycle performance of MnO2/rGO/S is better than rGO/S and MnO2/S, indicating that the combination of MnO2 and rGO is beneficial to electrochemical performance. After replacing some rGO with CNTs, the three-dimensional frame structure of MnO2/rGO/CNTs is established. The capacity and capacity retention rate of the composite increased significantly, indicating that MnO2/rGO/CNTs framework structure effectively improved the electrochemical performance by introducing the conductive CNTs. This is related to the pore size distribution of the three-dimensional sulfur-loaded framework structure and the synergistic effect of rGO and CNTs. The rate performance of rGO/S, MnO2/S, MnO2/rGO/S, and MnO2/rGO/CNTs/S cathodes are presented in Figure 4c. Among them, MnO2/rGO/CNTs/S has the best rated performance. The average capacity was 1080 mAh g −1 at 0.2 C, and then decreased to 916 mAh g −1 at 0.5 C, 736 mAh g −1 at 1 C, and 547 mAh g −1 at 2 C. When the current density returned to 0.2 C, the average capacity recovered to 920 mAh g −1 , which is close to its original capacity, indicating a good rate capability in a wide range. This performance may be related to the better conductivity of the materials. In addition, the MnO2/rGO/CNTs/S cathode delivered a high initial capacity of 1010 mAh g −1 at 0.5 C and achieved 780 mAh g −1 after 200 cycles (Figure 4d), with a high capacity retention of 77.2%. The capacity decay rate is 0.11% per cycle. Moreover, when compared with the reported MnO2-containing composite hosts (Table S1), the MnO2/rGO/CNTs/S cathode delivers a comparable or even better electrochemical performance [21,27,[35][36][37][38][39][40].     [41,42], there are two reduction peaks and one oxidation peak in the CV curves of typical Li-S batteries. During the reduction process, two peaks appeared at~2.2 V and~2.0 V, corresponding to the conversion of element sulfur to the soluble high-order lithium polysulfides (Li 2 S x , 4 ≤ x ≤ 8) and the soluble high-order polysulfides (Li 2 S x , 4 ≤ x ≤ 8) to insoluble low-order lithium sulfides (Li 2 S 2 , Li 2 S). During the oxidation reaction, the peak at 2.4 V is related to the reversible conversion from insoluble low-order lithium sulfides to element S. The rGO/S, MnO 2 /rGO/S, and MnO 2 /rGO/CNTs/S exhibit characteristic redox peaks of typical Li-S batteries.
With the increase of cycling number, the peak areas of rGO/S show a significant decrease, indicating that the adsorption effect of polysulfide is not obvious. However, the MnO 2 /rGO/S and MnO 2 /rGO/CNTs/S perform much better. The polarization between the reduction peaks and the oxidation peaks of the rGO/S composite is much larger than that of the MnO 2 /rGO/S and MnO 2 /rGO/CNTs/S cathodes. The sharp redox peaks in the CV curves of MnO 2 /rGO/CNTs/S indicate fast-electrochemical kinetics. In addition, the overlap of redox peak positions demonstrates a good electrochemical reversibility, which is consistent with the cycling performance, indicating that the framework structure of MnO 2 /rGO/CNTs is beneficial to the electrochemical reaction process.
Molecules 2020, 25, x FOR PEER REVIEW 7 of 11 The rGO/S, MnO2/rGO/S, and MnO2/rGO/CNTs/S exhibit characteristic redox peaks of typical Li-S batteries. With the increase of cycling number, the peak areas of rGO/S show a significant decrease, indicating that the adsorption effect of polysulfide is not obvious. However, the MnO2/rGO/S and MnO2/rGO/CNTs/S perform much better. The polarization between the reduction peaks and the oxidation peaks of the rGO/S composite is much larger than that of the MnO2/rGO/S and MnO2/rGO/CNTs/S cathodes. The sharp redox peaks in the CV curves of MnO2/rGO/CNTs/S indicate fast-electrochemical kinetics. In addition, the overlap of redox peak positions demonstrates a good electrochemical reversibility, which is consistent with the cycling performance, indicating that the framework structure of MnO2/rGO/CNTs is beneficial to the electrochemical reaction process. The electrochemical impedance spectroscopy (EIS) plots of MnO2/rGO/S and MnO2/rGO/CNTs/S investigated after three cycles (at 2.8 V) are given in Figure 5d. The results could be well fitted by an equivalent circuit in Figure 5d. The two curves have a similar feature. They both have an overlapping semicircle in the high and medium frequency ranges, corresponding to the charge-transfer resistance (Rct) on the solid/electrolyte interface, and an inclined line at low frequencies, owing to the Warburg impedance (Zw) of ion diffusion in the materials. The intersection of the EIS curve in the high frequency region represents the system resistance (Rs). The fitting data of equivalent circuits are presented in Table 1. The values of MnO2/rGO/CNTs/S are much smaller than those of MnO2/rGO/S, which indicates that MnO2/rGO/CNTs framework effectively promotes the reversible electrochemical reaction by enhancing the conductivity of sulfur hosts.   The electrochemical impedance spectroscopy (EIS) plots of MnO 2 /rGO/S and MnO 2 /rGO/CNTs/S investigated after three cycles (at 2.8 V) are given in Figure 5d. The results could be well fitted by an equivalent circuit in Figure 5d. The two curves have a similar feature. They both have an overlapping semicircle in the high and medium frequency ranges, corresponding to the charge-transfer resistance (R ct ) on the solid/electrolyte interface, and an inclined line at low frequencies, owing to the Warburg impedance (Z w ) of ion diffusion in the materials. The intersection of the EIS curve in the high frequency region represents the system resistance (R s ). The fitting data of equivalent circuits are presented in Table 1. The values of MnO 2 /rGO/CNTs/S are much smaller than those of MnO 2 /rGO/S, which indicates that MnO 2 /rGO/CNTs framework effectively promotes the reversible electrochemical reaction by enhancing the conductivity of sulfur hosts.

Preparation of Materials
Synthesis of rGO. First, 11.445 g graphite oxide aqueous solution (GO, prepared by Hummers method, and the concentration of graphite oxide was 1.2 wt%) was sonicated for 10 h and then was put directly into a thermostatic oven (AX-f100, Xiniu Technology company, Beijing, China) at 180 • C for 12 h. The resultant product was freeze-dried and denoted (version, Beijing Biocool Experimental Instrument Co., Ltd., Beijing, China) as rGO.
Synthesis of Urchin-like MnO 2 . Urchin-like MnO 2 was synthesized by a one-step facile method. Briefly, 5.88 g KMnO 4 was dissolved in 30 mL deionized water to prepare the KMnO 4 solution. Then, 6.09 g H 3 PO 4 (85 wt%) was added to the KMnO 4 solution, and then the mixture was transferred into a thermostatic oven at 180 • C for 12 h. The resulting material was washed with deionized water.
Synthesis of MnO 2 /rGO. A mixed solution containing 5.88 g KMnO 4 and 6.09 g H 3 PO 4 were prepared according to the above method. Then, 11.455 g graphite oxide aqueous solution (as above, after sonication for 10 h) was dispersed in the mixed solution by sonication. Then, the mixed solution was transferred into a thermostatic oven at 180 • C for 12 h. The product was washed with deionized water. Finally, the MnO 2 /rGO composite was obtained by the freeze-drying method.
Synthesis of MnO 2 /rGO/CNTs. Multiwalled carbon nanotubes (CNTs, Kelude) were oxidized by the modified Hummers method [43]. In the preparation process of MnO 2 /rGO, one half of GO was replaced by oxidized CNTs, and other conditions were maintained. Finally, MnO 2 /rGO/CNTs was obtained.
The MnO 2 /rGO/CNTs, MnO 2 /rGO/S, MnO 2 /S, and rGO/S composites were prepared by diffusion method. Sulfur powder and MnO 2 /rGO/S, MnO 2 /S, or rGO/S composites were mixed at a mass ratio of 35:65 and then milled, respectively. Subsequently, the mixtures were heated at 155 • C for 12 h and cooled to room temperature. The S content in each sample was about 65%.

Materials Characterization
The structures were characterized by using an X ray diffract meter (XRD) (XRD, XRD-6000, Shimadzu, Tokyo, Japan). The surface morphologies and microstructures were investigated using a scanning electron microscope (SEM) (JSM-7800F, JEOL, Tokyo, Japan) and high-resolution transmission electron microscope (HRTEM) (JEOL JEM-2100F, Tokyo, Japan). The N 2 adsorption-desorption isotherms and pore size distributions were characterized by using a specific surface and pore size distribution analyzer (Autosorb-iQ).

Electrochemical Measurements
The battery was assembled in an argon filled glove box with a 2032 battery case. The slurry, consisting of 80 wt.% active material, 10 wt.% carbon black, and 10 wt.% polyvinylidene difluoride (PVdF), was smeared uniformly on an aluminum foil (Canrd,~20 µm), then was dried at 60 • C for 30 min. The samples were transferred into avacuum oven and kept at 60 • C for 8 h. The mass loading on the electrode was about 2.1 mg cm −2 , and the diameter of the electrode was 1.6 cm. The pure lithium foil was employed as the anode. The separator was Cellgard−2400. The electrolyte was a 1 M lithium bis(trifluoromethanesulfonyl)imide (LiTFSI) solution in DOL and DME (volume ratio 1:1) with 2 wt% LiNO 3 . Galvanostatic charge-discharge tests were completed on a NEWARE test system with a cut-off voltage window of 1.7~2.8 V. Cyclic voltammetry (scanning speed 0.2 mV/s, cut-off voltage window of