Three-Dimensional S/CeO2/RGO Composites as Cathode Materials for Lithium–Sulfur Batteries

In this paper, the synthesis of the three-dimensional (3D) composite of spherical reduced graphene oxide (RGO) with uniformly distributed CeO2 particles is reported. This synthesis is done via a facile and large-scalable spray-drying process, and the CeO2/RGO materials are hydrothermally compounded with sulfur. The morphology, composition, structure, and electrochemical properties of the 3D S/CeO2/RGO composite are studied using X-ray diffraction (XRD), scanning electron microscope (SEM), transmission electron microscopy (TEM), thermal gravimetric analysis (TGA), Raman spectra and X-ray photoelectron spectroscopy (XPS), etc. The electrochemical performance of the composites as electrodes for lithium–sulfur batteries is evaluated. The S/CeO2/RGO composites deliver a high initial capacity of 1054 mAh g−1, and retain a reversible capacity of 792 mAh g−1 after 200 cycles at 0.1 C. Profiting from the combined effect of CeO2 and RGO, the CeO2/RGO materials effectively inhibit the dissolution of polysulfides, and the coating of spherical RGO improves the structural stability as well as conductivity.


Introduction
With the booming use of electric vehicles and portable electronic devices, the demand for rechargeable batteries that have higher power densities and long-term stability has increased substantially [1,2]. Lithium-sulfur batteries are secondary batteries that have high-energy current density (2600 Wh kg −1 ), as well as great potential for development and application prospects [3]. In addition, in terms of source, cost, and environmental impact, sulfur has also been shown to have unparalleled advantages for being used as a positive electrode [4,5]. However, lithium-sulfur batteries still have some shortcomings [6,7]. First, sulfur insulation reduces the use of cathode-active materials. Second, a large volume change (80%) is produced during charging/discharging, which leads to reduced mechanical properties. Third, the dissolution of polysulfides leads to a shuttle effect between the cathode and anode, and this results in the loss of active materials and poor coulomb efficiency, poor utilization, and obvious degradation [8].
Numerous design methods, including the combination of sulfur and carbon materials [9][10][11], metal oxides [12,13], and conductive polymers [14,15], have been explored to avoid these problems. Among these materials, reduced graphene oxide (RGO) (which is a carbon material) has high surface area, excellent intrinsic conductivity, excellent mechanical flexibility, and chemical stability. Due to these excellent properties, RGO has been widely used to prepare S/RGO composites to mitigate the dissolution of intermediate polysulfides [16,17]. However, the physical interactions between nonpolar RGO and polar polysulfides are weak, and they cannot ensure the long-term confinement of polysulfides during the charging/discharging process, during which the polysulfides remain vulnerable to slow dissolution in electrolytes, thus triggering the "shuttle effect" and resulting in an unsatisfactory calendar life [18]. Polar materials can be firmly combined with polysulfides via chemical adsorption, and thus polysulfides can be effectively captured at the cathode. Many polar host materials for sulfur, including SiO 2 , TiO 2 , Al 2 O 3 , La 2 O 3 and MnO 2 , have thus far been introduced into the cathodes [19][20][21]. For example, Sun et al. reported a method of modifying nitrogen-rich mesoporous carbon using La 2 O 3 nanodots [22]. Their results show that the La 2 O 3 nanoparticles can be used as the adsorption point of polysulfides and oxidation-reduction catalyst. Ding et al. fabricated nanoscale graphene modified with TiO 2 nanocrystals and used it as the sulfur host [23]. The TiO 2 nanocrystals can adsorb dissolved polysulfides and also promote the transmission of charge. CeO 2 , which is a polar substance, is also an excellent adsorbent and catalyst. CeO 2 has been applied to the preparation of cathode materials for lithium sulfur batteries. In addition to effectively slowing down the dissolution of polysulfides in electrolytes, CeO 2 also has a catalytic effect on the redox reaction. However, the conductivity of CeO 2 is relatively low, which inevitably affects the electrochemical performance.
Herein, a simple and large-scale spray-drying technique has been used to prepare RGO coated with CeO 2 particles. The CeO 2 /RGO composites have several apparent advantages. First, spherical RGO greatly improves the conductivity of the electron and ion transmission during the charging/discharging process. In addition, CeO 2 particles provide several strong binding sites for polysulfide intermediates, and keep them bound to the cathode materials during the charging/discharging process, which results in a longer cycle life. Therefore, the S/CeO 2 /RGO cathodes have the advantages of a high reversible capacity, good multiplying performance, and good circulation stability.

Sample Preparation
CeO 2 was synthesized via a precipitation process. Ammonia solution (NH 3 ·H 2 O) was added dropwise to an aqueous solution of Ce(NO 3 ) 3 ·6H 2 O solution, which had a concentration 0.4 mol L −1 , until the pH of the mixture became 10. After stirring for 30 min, the mixture was then left standing for 12 h. The precipitate was filtered out of the solution using a filtration device, and then it was repeatedly washed with water. Afterward, the samples were desiccated at 60 • C for 12 h in an electronic oven. The sample was then calcined at 300 • C for 4 h in a muffle furnace to obtain the desired CeO 2 . The second step was to composite CeO 2 and RGO. A commercially available graphene oxide (GO) solution (2 mg mL −1 ) was mixed with CeO 2 in ratio of 1:5. The mixture was sonicated for 2 h at 50 kHz using an ultrasonic cell crusher at room temperature to obtain a uniformly mixed suspension of CeO 2 /GO. The spray-drying technique was then used to obtain CeO 2 /GO powders. The spray-drying equipment that was used was a normal air pressurizer with an inlet air temperature of 200 • C and a feed rate of 4 mL min −1 . The precursor was calcined in a tube furnace under an argon atmosphere at 900 • C for 2 h to achieve the CeO 2 /RGO composites ( Figure 1). In the final step, sulfur was loaded into the CeO 2 /RGO composite. The weight ratio of CeO 2 /RGO to sulfur was set to 1:2. The mixture was heated at 155 • C, and maintained at this temperature for 12 h to obtain the S/CeO 2 /RGO composites. The chemical equations associated with the preparation of CeO 2 are as follows: (a) Ce 3+ + 3OH − →Ce(OH) 3 ↓ (b) Ce(OH) 3

Electrochemical Measurements
S/CeO2/RGO, acetylene black, and PVDF were mixed using magnetic stirring in a weight ratio of 8:1:1 with N-methylpyrrolidone (NMP) as a solvent to prepare the cathode slurry. N-methylpyrrolidone (NMP) was slowly added to the materials and ground until a similar viscous oil-like slurry was formed. The obtained slurry was then cast on aluminum foil and dried at 60 °C for 12 h in vacuum, and the NMP evaporated completely during the drying process. Aluminum foil was cut into disks, each with a diameter of 15 mm, for use as current collectors. The electrolyte was 1 M of lithium bis (trifluoromethane)sulfonimide (LiTFSI) in a mixed solvent of 1,2-dimethoxyethane (DME) and 1,3-dioxolane (DOL) (1:1 v/v) containing 1 wt % of LiNO3. Cyclic voltammetry (CV) and electrochemical impedance spectroscopy (EIS) were conducted using an electrochemical workstation (CHI660E, Austin, TX, USA) that was operated in the frequency range of 10 kHz to 10 mHz with an amplitude of 10 mV.  [24]. Two feeble peaks of 3D RGO are observed at 26.2° and 43.7° because of a fairly low diffraction intensity of 3D RGO [25]. The other peaks are sulfur peaks (JCPDS No. 42-1278) [26]. A few strong peaks are marked in the figure.

Electrochemical Measurements
S/CeO 2 /RGO, acetylene black, and PVDF were mixed using magnetic stirring in a weight ratio of 8:1:1 with N-methylpyrrolidone (NMP) as a solvent to prepare the cathode slurry. N-methylpyrrolidone (NMP) was slowly added to the materials and ground until a similar viscous oil-like slurry was formed. The obtained slurry was then cast on aluminum foil and dried at 60 • C for 12 h in vacuum, and the NMP evaporated completely during the drying process. Aluminum foil was cut into disks, each with a diameter of 15 mm, for use as current collectors. The electrolyte was 1 M of lithium bis (trifluoromethane)sulfonimide (LiTFSI) in a mixed solvent of 1,2-dimethoxyethane (DME) and 1,3-dioxolane (DOL) (1:1 v/v) containing 1 wt % of LiNO 3 . Cyclic voltammetry (CV) and electrochemical impedance spectroscopy (EIS) were conducted using an electrochemical workstation (CHI660E, Austin, TX, USA) that was operated in the frequency range of 10 kHz to 10 mHz with an amplitude of 10 mV.  [24]. Two feeble peaks of 3D RGO are observed at 26.2 • and 43.7 • because of a fairly low diffraction intensity of 3D RGO [25]. The other peaks are sulfur peaks (JCPDS No. 42-1278) [26]. A few strong peaks are marked in the figure. To further confirm the structural intricacies present in the CeO2/RGO composites, we collected Raman spectra, and the results are shown in Figure 3. All of the CeO2/RGO composites exhibited an inherent mode of graphite structure (D-breathing zone at ~1350 cm −1 and G-breathing zone at ~1580 cm −1 ) and CeO2 structure (F2g mode at ~461 cm −1 ) [27]. The degree of graphitization in the CeO2/RGO composites is low, because the addition of metal oxide leads to an increase in the ratio ID:IG, thereby increasing the defect level of graphene and increasing the conductivity of graphene [28]. As seen in the SEM and TEM images of the CeO2/RGO sample (Figure 4a,b), RGO has been made into a three-dimensional (3D) spherical structure via spray-drying, and CeO2 was distributed uniformly in the RGO. In the corresponding high-resolution TEM image shown in Figure 4c, RGO has lattice spacings of ca. 0.34 nm, which is indexed to the (200) planes, and ca. 0.312 nm, which corresponds to the interspacing of the (111) planes of cubic CeO2 [27]. The selective electron diffraction (SAED) pattern of the composites materials reveals the polycrystalline nature of the materials (Figure 4d) [29]. The above results show that CeO2 and RGO are well combined to form composite materials. To further confirm the structural intricacies present in the CeO 2 /RGO composites, we collected Raman spectra, and the results are shown in Figure 3. All of the CeO 2 /RGO composites exhibited an inherent mode of graphite structure (D-breathing zone at~1350 cm −1 and G-breathing zone at 1580 cm −1 ) and CeO 2 structure (F 2g mode at~461 cm −1 ) [27]. The degree of graphitization in the CeO 2 /RGO composites is low, because the addition of metal oxide leads to an increase in the ratio I D :I G , thereby increasing the defect level of graphene and increasing the conductivity of graphene [28]. To further confirm the structural intricacies present in the CeO2/RGO composites, we collected Raman spectra, and the results are shown in Figure 3. All of the CeO2/RGO composites exhibited an inherent mode of graphite structure (D-breathing zone at ~1350 cm −1 and G-breathing zone at ~1580 cm −1 ) and CeO2 structure (F2g mode at ~461 cm −1 ) [27]. The degree of graphitization in the CeO2/RGO composites is low, because the addition of metal oxide leads to an increase in the ratio ID:IG, thereby increasing the defect level of graphene and increasing the conductivity of graphene [28]. As seen in the SEM and TEM images of the CeO2/RGO sample (Figure 4a,b), RGO has been made into a three-dimensional (3D) spherical structure via spray-drying, and CeO2 was distributed uniformly in the RGO. In the corresponding high-resolution TEM image shown in Figure 4c, RGO has lattice spacings of ca. 0.34 nm, which is indexed to the (200) planes, and ca. 0.312 nm, which corresponds to the interspacing of the (111) planes of cubic CeO2 [27]. The selective electron diffraction (SAED) pattern of the composites materials reveals the polycrystalline nature of the materials (Figure 4d) [29]. The above results show that CeO2 and RGO are well combined to form composite materials. As seen in the SEM and TEM images of the CeO 2 /RGO sample (Figure 4a,b), RGO has been made into a three-dimensional (3D) spherical structure via spray-drying, and CeO 2 was distributed uniformly in the RGO. In the corresponding high-resolution TEM image shown in Figure 4c, RGO has lattice spacings of ca. 0.34 nm, which is indexed to the (200) planes, and ca. 0.312 nm, which corresponds to the interspacing of the (111) planes of cubic CeO 2 [27]. The selective electron diffraction (SAED) pattern of the composites materials reveals the polycrystalline nature of the materials (Figure 4d) [29]. The above results show that CeO 2 and RGO are well combined to form composite materials.  The high-resolution XPS spectrum of 3D Ce is shown in Figure 6a, and demonstrates the presence of a mixed valence state. The O 1s XPS peak at 530.8 eV corresponds to the oxygen in CeO2, and further confirms the presence of CeO2 (Figure 6b) [24]. The O 1s peak at 528.6 eV indicates that there are residual oxygen groups associated with the C atoms in 3D RGO. The C 1s XPS spectrum of S/CeO2/RGO is shown in Figure 6c. The peak observed at 283.34 eV is related to the graphitic carbon in the 3D RGO, and the peak at 286.48 eV is assigned to the C-O bond [30]. In Figure 6d, the binding energies of S 2p3/2 are 163.8 and 164.3 eV, and are attributed to the S-S and S-O species, respectively [30]. The additional small shoulder of 167.7 eV is attributed to the sulfate species, which is associated with sulfur oxidation [31]. The high-resolution XPS spectrum of 3D Ce is shown in Figure 6a, and demonstrates the presence of a mixed valence state. The O 1s XPS peak at 530.8 eV corresponds to the oxygen in CeO 2 , and further confirms the presence of CeO 2 (Figure 6b) [24]. The O 1s peak at 528.6 eV indicates that there are residual oxygen groups associated with the C atoms in 3D RGO. The C 1s XPS spectrum of S/CeO 2 /RGO is shown in Figure 6c. The peak observed at 283.34 eV is related to the graphitic carbon in the 3D RGO, and the peak at 286.48 eV is assigned to the C-O bond [30]. In Figure 6d, the binding energies of S 2p 3/2 are 163.8 and 164.3 eV, and are attributed to the S-S and S-O species, respectively [30]. The additional small shoulder of 167.7 eV is attributed to the sulfate species, which is associated with sulfur oxidation [31]. It is apparent from the TGA curves shown in Figure 7 that the weight drops rapidly when the temperature increases from 200 °C to 293 °C. Since the sulfur is completely evaporated [32], the rapid weight loss is about 64 wt %. Therefore, the overall sulfur content can be estimated to be about 64 wt %. It is apparent from the TGA curves shown in Figure 7 that the weight drops rapidly when the temperature increases from 200 • C to 293 • C. Since the sulfur is completely evaporated [32], the rapid weight loss is about 64 wt %. Therefore, the overall sulfur content can be estimated to be about 64 w %. It is apparent from the TGA curves shown in Figure 7 that the weight drops rapidly when the temperature increases from 200 °C to 293 °C. Since the sulfur is completely evaporated [32], the rapid weight loss is about 64 wt %. Therefore, the overall sulfur content can be estimated to be about 64 wt %. .    Figure 9 shows the charge/discharge curves for lithium-sulfur with the S/CeO2/RGO and S/RGO cathodes at a scan rate of 0.1 C. In the discharge process with the S/CeO2/RGO cathode, two major stages appear in the potential distribution, which are attributed to the two-step electrochemical reaction between lithium and sulfur. A short discharge platform of about 2.3 V indicates the first electrochemical reaction, and is related to the reduction of the S8 form of elemental sulfur [33]. The lower extended plateau around 2.1 V in the discharge curve reflects the subsequent reduction of higher polysulfides to lower polysulfides, and eventually to lithium sulfide Li2S [32]. The S/CeO2/RGO electrode presents a higher initial discharge capacity than the S/RGO electrode during discharge at 0.1 C. Meanwhile, the S/CeO2/RGO electrode shows two higher discharge potential plateaus than the S/RGO electrode. These are all because CeO2 decoration enhances catalytic activity.  Figure 9 shows the charge/discharge curves for lithium-sulfur with the S/CeO 2 /RGO and S/RGO cathodes at a scan rate of 0.1 C. In the discharge process with the S/CeO 2 /RGO cathode, two major stages appear in the potential distribution, which are attributed to the two-step electrochemical reaction between lithium and sulfur. A short discharge platform of about 2.3 V indicates the first electrochemical reaction, and is related to the reduction of the S 8 form of elemental sulfur [33]. The lower extended plateau around 2.1 V in the discharge curve reflects the subsequent reduction of higher polysulfides to lower polysulfides, and eventually to lithium sulfide Li 2 S [32]. The S/CeO 2 /RGO electrode presents a higher initial discharge capacity than the S/RGO electrode during discharge at 0.1 C. Meanwhile, the S/CeO 2 /RGO electrode shows two higher discharge potential plateaus than the S/RGO electrode. These are all because CeO 2 decoration enhances catalytic activity. Figure 9 shows the charge/discharge curves for lithium-sulfur with the S/CeO2/RGO and S/RGO cathodes at a scan rate of 0.1 C. In the discharge process with the S/CeO2/RGO cathode, two major stages appear in the potential distribution, which are attributed to the two-step electrochemical reaction between lithium and sulfur. A short discharge platform of about 2.3 V indicates the first electrochemical reaction, and is related to the reduction of the S8 form of elemental sulfur [33]. The lower extended plateau around 2.1 V in the discharge curve reflects the subsequent reduction of higher polysulfides to lower polysulfides, and eventually to lithium sulfide Li2S [32]. The S/CeO2/RGO electrode presents a higher initial discharge capacity than the S/RGO electrode during discharge at 0.1 C. Meanwhile, the S/CeO2/RGO electrode shows two higher discharge potential plateaus than the S/RGO electrode. These are all because CeO2 decoration enhances catalytic activity. As seen in Figure 10a, the cycle performances of batteries with the S/CeO2/RGO cathode were measured under 0.1 C. The initial discharge capacity was 1054 mAh g −1 , corresponding to a sulfur As seen in Figure 10a, the cycle performances of batteries with the S/CeO 2 /RGO cathode were measured under 0.1 C. The initial discharge capacity was 1054 mAh g −1 , corresponding to a sulfur utilization of 65%. Furthermore, the S/CeO 2 /RGO cathodes enhanced the cyclability of the batteries, retaining a discharge capacity of 792 mAh g −1 even after 200 cycles. On the contrary, the S/RGO cathode ( Figure 10b) delivered a lower discharge capacity of approximately 965 mAh g −1 at the same current rate. After 200 cycles, the discharge capacity quickly decreased to 623 mAh g −1 . The coulombic efficiency of the batteries with the S/CeO 2 /RGO cathode was close to 100%, whereas the coulombic efficiency of the S/RGO cathode was lower than 98%, indicating that the soluble polysulfides from the cathodes were largely adsorbed by the S/CeO 2 /RGO materials.

Results and Discussion
Materials 2018, 11, x FOR PEER REVIEW 9 of 13 utilization of 65%. Furthermore, the S/CeO2/RGO cathodes enhanced the cyclability of the batteries, retaining a discharge capacity of 792 mAh g −1 even after 200 cycles. On the contrary, the S/RGO cathode ( Figure 10b) delivered a lower discharge capacity of approximately 965 mAh g −1 at the same current rate. After 200 cycles, the discharge capacity quickly decreased to 623 mAh g −1 . The coulombic efficiency of the batteries with the S/CeO2/RGO cathode was close to 100%, whereas the coulombic efficiency of the S/RGO cathode was lower than 98%, indicating that the soluble polysulfides from the cathodes were largely adsorbed by the S/CeO2/RGO materials.  Figure 11 shows the rate capability at different current densities of the S/CeO2/RGO and S/RGO cathodes. As the current density increased from 0.1 C to 2 C, the discharge capacity changed steadily; under 0.1 C, 0.5 C, 1 C, and 2 C, for S/CeO2/RGO, the reversible capacities were 1054 mAh g −1 , 807 mAh g −1 , 674 mAh g −1 , and 552 mAh g −1 , respectively, and for S/RGO, the reversible capacities were 948 mAh g −1 , 680 mAh g −1 , 512 mAh g −1 and 394 mAh g −1 , respectively. Apparently, the discharge capacities of the S/CeO2/RGO cathode at each current rate were larger than those of the S/RGO cathode. Moreover, when the current rate returned to 0.1 C, S/CeO2/RGO remains almost at capacity. This is ascribed to the absorbing and catalyzing effects of CeO2 particles on lithium polysulfides during the redox procedures [26].  Figure 11 shows the rate capability at different current densities of the S/CeO 2 /RGO and S/RGO cathodes. As the current density increased from 0.1 C to 2 C, the discharge capacity changed steadily; under 0.1 C, 0.5 C, 1 C, and 2 C, for S/CeO 2 /RGO, the reversible capacities were 1054 mAh g −1 , 807 mAh g −1 , 674 mAh g −1 , and 552 mAh g −1 , respectively, and for S/RGO, the reversible capacities were 948 mAh g −1 , 680 mAh g −1 , 512 mAh g −1 and 394 mAh g −1 , respectively. Apparently, the discharge capacities of the S/CeO 2 /RGO cathode at each current rate were larger than those of the S/RGO cathode. Moreover, when the current rate returned to 0.1 C, S/CeO 2 /RGO remains almost at capacity. This is ascribed to the absorbing and catalyzing effects of CeO 2 particles on lithium polysulfides during the redox procedures [26]. Figure 11 shows the rate capability at different current densities of the S/CeO2/RGO and S/RGO cathodes. As the current density increased from 0.1 C to 2 C, the discharge capacity changed steadily; under 0.1 C, 0.5 C, 1 C, and 2 C, for S/CeO2/RGO, the reversible capacities were 1054 mAh g −1 , 807 mAh g −1 , 674 mAh g −1 , and 552 mAh g −1 , respectively, and for S/RGO, the reversible capacities were 948 mAh g −1 , 680 mAh g −1 , 512 mAh g −1 and 394 mAh g −1 , respectively. Apparently, the discharge capacities of the S/CeO2/RGO cathode at each current rate were larger than those of the S/RGO cathode. Moreover, when the current rate returned to 0.1 C, S/CeO2/RGO remains almost at capacity. This is ascribed to the absorbing and catalyzing effects of CeO2 particles on lithium polysulfides during the redox procedures [26]. As presented in the Figure 12, both the S/CeO2/RGO and S/RGO cathodes display two obvious cathodic peaks and one anodic peak during the cathodic sweep; the peaks at 2.3 and 2.1 V are attributed to the change of elemental sulfur into soluble lithium polysulfide. In the subsequent anodic scan, the obvious peak at 2.4 V corresponds to Li2S8 [34]. Compared with the S/RGO sample, the S/CeO2/RGO sample has a higher charge/discharge peak, which verifies the rapid electron/ion transfer and redox process [35]. The cathode peak potential of the S/CeO2/RGO cathode is about 2.1 V; this is slightly larger than the cathode peak potential of the S/RGO cathode, which is about 1.9 V. The relatively larger cathodic peak potential indicates that the sulfur in the cathode electrode can As presented in the Figure 12, both the S/CeO 2 /RGO and S/RGO cathodes display two obvious cathodic peaks and one anodic peak during the cathodic sweep; the peaks at 2.3 and 2.1 V are attributed to the change of elemental sulfur into soluble lithium polysulfide. In the subsequent anodic scan, the obvious peak at 2.4 V corresponds to Li 2 S 8 [34]. Compared with the S/RGO sample, the S/CeO 2 /RGO sample has a higher charge/discharge peak, which verifies the rapid electron/ion transfer and redox process [35]. The cathode peak potential of the S/CeO 2 /RGO cathode is about 2.1 V; this is slightly larger than the cathode peak potential of the S/RGO cathode, which is about 1.9 V. The relatively larger cathodic peak potential indicates that the sulfur in the cathode electrode can react with Li ions more easily because of the decoration of CeO 2 particles, which demonstrates the catalytic effect of CeO 2 .  To gain further insight into the reaction kinetics, the charge transfer resistance (Rct) of the S/CeO2/RGO and S/RGO cathodes was examined with EIS data (Figure 13). The EIS data demonstrate a semicircle in the medium frequency region and a tail with a slope in the lower frequency region [36]. As presented in Figure 13, the RCT value of the S/CeO2/RGO cathode before cycling is 90, which is lower than that of the S/RGO cathode (120). This phenomenon indicates that the CeO2 particles in spherical RGO can dramatically promote charge transportation during the redox reactions. Therefore, the specific discharge capacity and the rate performance of the S/CeO2/RGO cathode will be considerably enhanced. To gain further insight into the reaction kinetics, the charge transfer resistance (Rct) of the S/CeO 2 /RGO and S/RGO cathodes was examined with EIS data (Figure 13). The EIS data demonstrate a semicircle in the medium frequency region and a tail with a slope in the lower frequency region [36]. As presented in Figure 13, the RCT value of the S/CeO 2 /RGO cathode before cycling is 90, which is lower than that of the S/RGO cathode (120). This phenomenon indicates that the CeO 2 particles in spherical RGO can dramatically promote charge transportation during the redox reactions. Therefore, the specific discharge capacity and the rate performance of the S/CeO 2 /RGO cathode will be considerably enhanced. demonstrate a semicircle in the medium frequency region and a tail with a slope in the lower frequency region [36]. As presented in Figure 13, the RCT value of the S/CeO2/RGO cathode before cycling is 90, which is lower than that of the S/RGO cathode (120). This phenomenon indicates that the CeO2 particles in spherical RGO can dramatically promote charge transportation during the redox reactions. Therefore, the specific discharge capacity and the rate performance of the S/CeO2/RGO cathode will be considerably enhanced. As shown in Table 1, the performance of 3D S/CeO2/RGO cathode is compared with other reported results. The results show that the prepared 3D S/CeO2/RGO cathode has good cycling performance. The discharge specific capacity is stable at 0.1 C, and the decay rate remains at 0.25% for 200 cycles.  As shown in Table 1, the performance of 3D S/CeO 2 /RGO cathode is compared with other reported results. The results show that the prepared 3D S/CeO 2 /RGO cathode has good cycling performance. The discharge specific capacity is stable at 0.1 C, and the decay rate remains at 0.25% for 200 cycles.

Conclusions
The 3D S/CeO 2 /RGO composite materials were successfully synthesized via spray drying. Since this is a very simple synthesis route, high-throughput commercial manufacturing can easily be achieved. When S/CeO 2 /RGO composites are used for cathodes, they retain a capacity of 792 mAh g −1 , even after 200 cycles of operation, under a current density of 0.1 C. Such excellent performance makes the S/CeO 2 /RGO composite a promising candidate for a low-cost, high-performance material for use in lithium-sulfur batteries.