相关实验视频

Updated: Jun 7, 2025

Dynamic Electrochemical Measurement of Chloride Ions

Dynamic Electrochemical Measurement of Chloride Ions

Published on: February 5, 2016

化物和电解质稳定性对Mg电池负电极的被动化层演变的影响通过操作EQCM-D揭示

Benjamin W Schick¹, Viktor Vanoppen², Matthias Uhl¹

¹Institute of Electrochemistry, Ulm University, Albert-Einstein-Allee 47, 89081, Ulm, Germany.

Angewandte Chemie (International ed. in English)

|November 10, 2024

概括

可充电电池对储能充满希望. 这项研究表明,稳定的电解质和化物添加剂通过最小化被动化层来提高涂层和剥离效率.

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

背景情况:

可充电电池对于未来的能量储存至关重要,但面临着诸如涂层和剥离中低库伦比效率等挑战.
受电解质成分影响的被动化层的形成,结构和稳定性尚未完全理解,这阻碍了实际应用.

研究的目的:

研究不同电解质系统中的初始涂层和剥离周期.
了解电解质成分和添加剂在被动化层形成中的作用及其对电池性能的影响.

主要方法:

操作电化学石英晶体微平衡与散射监测 (EQCM-D) 结合水力动态光谱学.
在黄金电极上比较基于二三甲硫尼尔) 胺 (Mg (TFSI) 2) 和四基 (hexafluoroisopropyloxy) 酸盐 (Mg (B (hfip) 4) 2) 的电解质,含有或不含有MgCl2.

主要成果:

稳定的Mg[B(hfip) [4]2电解质可以实现高效的,无相间循环,其被动化层归因于在调节过程中形成的电解质污染物.
更有反应性的Mg(TFSI) 2电解质形成厚厚的被动化层,但添加化物减少了被动化的Mg沉积物,并加速了层溶解.
最有效的循环和均沉积发生在电极上没有介相时.

结论:

电解质的稳定性和组成极大地影响了被动化层的形成和电池的性能.
添加剂可以减轻反应电解质中的被动化问题,从而提高循环效率.
实现无相间循环是释放可充电电池潜力的关键.

关键词:

在 EQCM−D 中.电化学电化学电化学水力动力学光谱学 (Hydrodynamic Spectroscopy) 是一种水力动力学光谱学.是的重要组成部分.电池电解质Mg电池电解质Mg电池电解质

更多相关视频

The Effect of Charging and Discharging Lithium Iron Phosphate-graphite Cells at Different Temperatures on Degradation

The Effect of Charging and Discharging Lithium Iron Phosphate-graphite Cells at Different Temperatures on Degradation

Published on: July 18, 2018

Identification and Quantification of Decomposition Mechanisms in Lithium-Ion Batteries; Input to Heat Flow Simulation for Modeling Thermal Runaway

Identification and Quantification of Decomposition Mechanisms in Lithium-Ion Batteries; Input to Heat Flow Simulation for Modeling Thermal Runaway

Published on: March 7, 2022

相关概念视频

Electrogravimetric Analysis: Overview

Electrogravimetric Analysis: Overview

Electrogravimetric analysis measures the weight of an analyte deposited electrolytically onto a suitable working electrode. This method involves applying a potential to a pre-weighed electrode submerged in a solution, which results in the desired substance being deposited through reduction at the cathode or oxidation at the anode. The electrode's weight is recorded after deposition, and the difference in weight gives the analyte's weight in the solution.
To test the completeness of the...

Electrolysis

Electrolysis

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...

Ionic Strength: Effects on Chemical Equilibria

Ionic Strength: Effects on Chemical Equilibria

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...

Electrodeposition

Electrodeposition

Electrodeposition is a technique used to separate an analyte from interferents by electrochemical processes. Here, the analyte is a metal ion that can be deposited on an electrode immersed in the sample solution. The electrochemical setup consists of an anode and a cathode. When an electric current is applied to the setup, oxidation occurs at the anode. At the cathode, which consists of a large metal surface, metal ions undergo reduction and deposit onto the surface.
Electrodeposition can...

Common Ion Effect

Common Ion Effect

Compared with pure water, the solubility of an ionic compound is less in aqueous solutions containing a common ion (one also produced by dissolution of the ionic compound). This is an example of a phenomenon known as the common ion effect, which is a consequence of the law of mass action that may be explained using Le Châtelier’s principle. Consider the dissolution of silver iodide:

Standard Electrode Potentials

Standard Electrode Potentials

On comparing the reactivity of silver and lead, it is observed that the two ionic species, Ag+ (aq) and Pb2+ (aq), show a difference in their redox reactivity towards copper: the silver ion undergoes spontaneous reduction, while the lead ion does not. This relative redox activity can be easily quantified in electrochemical cells by a property called cell potential. This property is commonly known as cell voltage in electrochemistry, and it is a measure of the energy which accompanies the charge...