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29 rate of 0.1 C, respectively, which showed a slight degradation compared to that at 25 ◦C (290 mAh/g). Additionally, Yang-Kook Sun et al. [59] tested a hierarchical ternary poly- meric cathode using the EMS: FEC 98:2 (vol) cosolvent in 0.5 M NaPF6 solution. Attributing to the low-temperature function of the unique cathode and the favorable electrolyte, the full and 100 mAh/g at a 0.75 C rate with slightly different retention capacities of 89% and 92% after 100 cycles at a 0.75 C rate. In Figure 10c, the conventional organic electrolytes based on sodium salt NaClO4 and NaPF6 solvents with organic solvents have a wide electro- Nanomaterials 2022, 12, 3529 17 of 29 cell sandwiched by HC anodes demonstrated appreciable specific capacities of 130 mAh/g was realized after 1000 cycles at 1 C. Under an ultra-high rate of 30 C and a low tempera- chemical window and ideal thermodynamic stability. Meanwhile, in the group of Huang, Yunhui et al. [65] tested the conventional organic electrolyte in the Na V (PO ) O F half- 32422 ture of −30 °C, the discharge capacities still reached 89.2 and 92.1 mAh/g, respectively. cell. By assembling into Na/ Na3V2(PO4)2O2F batteries, a high capacity retention of 93.1% This also proves thatwSaIsBresalwizeitdhafdteirff1e0r0e0ncytcelelseactt1roCd. Uenmdeartaenruialtlrsa-mhigehnrtaiotenoefd30aCbaonvdea,lcowomtebmipneeradture of −30 ◦C, the discharge capacities still reached 89.2 and 92.1 mAh/g, respectively. This with conventional organic electrolytes, exhibit practical electrochemical capabilities at low temperatures. Therefore, with the easy synthesis processes, the conventional organic elec- also proves that SIBs with different electrode materials mentioned above, combined with conventional organic electrolytes, exhibit practical electrochemical capabilities at low tem- trolyte is the most suitable choice for SIB at low temperatures. peratures. Therefore, with the easy synthesis processes, the conventional organic electrolyte is the most suitable choice for SIB at low temperatures. 18 of 28 Figure 10. (a) On the left is the optical picture of the electrolyte in PBNi-ES at −25 ◦C. In the middle Figure 10. (a) On the left is the optical picture of the electrolyte in PBNi-ES at −25 °C. In the middle is the electrolyte at 0 ◦C. On the right is the electrolyte at 25 ◦C. (b) In the EIS spectra, the black line ◦◦ is the electrolyte at 0 °Cre.pOrensetnhtsepreirgfohrtmiasntcheetesltedctarto2l5yteC,ath2e5re°dCl.in(ebr)eIpnretshenetsE0ISCs,paencdtrthae, tbhlueeblilnaeckreplirneseents −25 ◦C. Reproduced with permission from Ref. [19]. Copyright 2018 Elsevier Ltd. (c) The black represents performance tested at 25 °C, the red line represents 0 °C, and the blue line represents −25 °C. Reproduced with permission from Ref. [19]. Copyright 2018 Elsevier Ltd. (c) The black bar rep- bar represents electrochemical windows for different electrolytes, while the green bar represents resents electrochemical windows for different electrolytes, while the green bar represents their ther- their thermal stabilities. The Y axis represents solvents based on PC with 1 M sodium salts and with different other solvents. Reproduced with permission from Ref. [59]. Copyright mal stabilities. The Y axis represents solvents based on PC with 1 M sodium salts and 1 M NaClO4 1 M NaClO 4 The Royal Society of Chemistry 2012. (d) The picture compares different contact angles of various with different other solvents. Reproduced with permission from Ref. [59]. Copyright The Royal So- proportions of ethanol–water. (e) Raman scattering spectra of various proportion of ethanol–water. ciety of Chemistry 2012. (d) The picture compares different contact angles of various proportions of (f) The picture represents the new type of hydrogen bond in the ethanol–water system. Reproduced ethanol–water. (e) Raman scattering spectra of various proportion of ethanol–water. (f) The picture with permission from Ref. [66]. Copyright 2020 American Chemical Society. represents the new type of hydrogen bond in the ethanol–water system. Reproduced with permis- 4.2. Ionic Liquid Electrolytes sion from Ref. [66]. Copyright 2020 American Chemical Society. 4.2. Ionic Liquid Electrolytes Ionic liquids are ionic, noncombustible, and nonvolatile, and salt-like electrolytes can provide broad electrochemical window, as well as high stability and safety. Moreover, it has a broad temperature range that gives a promising low-temperature application hori- zon [67]. Imidazolyl-based ionic liquids, especially those with 1-ethyl-3-methylimidazolyl Ionic liquids are ionic, noncombustible, and nonvolatile, and salt-like electrolytes can provide broad electrochemical window, as well as high stability and safety. Moreover, it has a broad temperature range that gives a promising low-temperature application hori- zon [67]. Imidazolyl-based ionic liquids, especially those with 1-ethyl-3-methylimidazolyl 5 as the cation, have high conductivity and low viscosity, and have been shown to possessPDF Image | Na Ion Batteries Used at Low Temperatures
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