双盐低度电解质用于低温金属电池
Yongjian Yang1, Yi Yang1, Shoumeng Yang1
1Guangdong Provincial Key Laboratory on Functional Soft Condensed Matter, School of Materials and Energy, Guangdong University of Technology, Guangzhou 51006, China.
ACS applied materials & interfaces
|April 7, 2025
概括
研究人员开发了一种新型的低度双盐电解质,用于金属电池 (SMB),以提高超低温性能. 这种电解质增强了离子导电性,并形成稳定的固体电解质介相 (SEI) 膜,在-40°C下可延长循环寿命.
科学领域:
- 电化学 电化学 电化学
- 材料科学 材料科学 材料科学
- 储能 储能 储能 储能 储能 储能
背景情况:
- 金属电池 (SMB) 的理论容量高,成本低于离子电池.
- 传统的电解质限制了中小企业的超低温性能,原因是不稳定的固体电解质介相 (SEI) 和较差的离子动力学.
- 对于电池周期稳定性来说,SEI膜质量至关重要.
研究的目的:
- 开发一种新型电解质,以提高中小企业在超低温下的性能.
- 为了应对不稳定的SEI和低于最佳的离子动力学在寒冷环境中的挑战.
- 改善中小企业的周期寿命和运营稳定性.
主要方法:
- 一种低度,双盐碳酸盐电解质的配方.
- 研究电解质流动性和离子溶解结构.
- 分析SEI膜的形成和特性.
- 在-40°C的温度下对对称的Na saq saq Na和Na saq saq saq Na3V2(PO4)3全细胞进行电化学测试.
主要成果:
- 新型电解质显著提高了离子运动性能和低温周期寿命.
- 一个对称的细胞表现出了900小时的循环寿命.
- 在Na3V2(PO4) 3的完整电池中,在-40°C的100个循环中保持了70.5 mAh g-1.
- 双盐系统促进了强大的无机SEI膜.
结论:
- 开发的电解质有效地提高了中小企业的超低温性能.
- 这种电解质设计是推进可冷操作的金属电池的有希望的策略.
- 这些发现有助于开发下一代储能解决方案.
相关概念视频
01:19Ionic Strength: Effects on Chemical Equilibria
1.3K
The addition of an inert ionic compound increases the solubility of a sparingly soluble salt. For example, adding potassium nitrate to a saturated solution of calcium sulfate significantly enhances the solubility of calcium sulfate. Le Châtelier's principle cannot predict this shift in the equilibrium. Instead, this could be explained in terms of changes in the effective concentration of the ions in solution in the presence of added inert salt.
In this solution, the primary...
In this solution, the primary...
1.3K
02:21Electrolyte and Nonelectrolyte Solutions
61.9K
Substances that undergo either a physical or a chemical change in solution to yield ions that can conduct electricity are called electrolytes. If a substance yields ions in solution, that is, if the compound undergoes 100% dissociation, then the substance is a strong electrolyte. Complete dissociation is indicated by a single forward arrow. For example, water-soluble ionic compounds like sodium chloride dissociate into sodium cations and chloride anions in aqueous solution.
61.9K
03:00Electrolysis
25.8K
In a galvanic cell, the electrical work is done by a redox system on its surroundings as electrons produced by the spontaneous redox reactions are transferred through an external circuit. Alternatively, an external circuit does work on a redox system by imposing a voltage sufficient to drive an otherwise nonspontaneous reaction in a process known as electrolysis. For instance, recharging a battery involves the use of an external power source to drive the spontaneous (discharge) cell reaction in...
25.8K
02:54Ions as Acids and Bases
23.0K
Salts with Acidic Ions
Salts are ionic compounds composed of cations and anions, either of which may be capable of undergoing an acid or base ionization reaction with water. Aqueous salt solutions, therefore, may be acidic, basic, or neutral, depending on the relative acid-base strengths of the salt’s constituent ions. For example, dissolving the ammonium chloride in water results in its dissociation, as described by the equation:
Salts are ionic compounds composed of cations and anions, either of which may be capable of undergoing an acid or base ionization reaction with water. Aqueous salt solutions, therefore, may be acidic, basic, or neutral, depending on the relative acid-base strengths of the salt’s constituent ions. For example, dissolving the ammonium chloride in water results in its dissociation, as described by the equation:
23.0K
03:45Formation of Complex Ions
23.0K
A type of Lewis acid-base chemistry involves the formation of a complex ion (or a coordination complex) comprising a central atom, typically a transition metal cation, surrounded by ions or molecules called ligands. These ligands can be neutral molecules like H2O or NH3, or ions such as CN− or OH−. Often, the ligands act as Lewis bases, donating a pair of electrons to the central atom. These types of Lewis acid-base reactions are examples of a broad subdiscipline called coordination...
23.0K
01:12Ionic Strength: Overview
1.2K
The ionic strength of a solution is a quantitative way of expressing the total electrolyte concentration of a solution. This concept was first introduced in 1921 by two American physical chemists, Gilbert N. Lewis and Merle Randall, while describing the activity coefficient of strong electrolytes. During the calculation of ionic strength (I or μ), all the cations and anions are considered. However, the concentration (c) of an ion with a greater charge number (z) has a greater contribution...
1.2K