通过用添加的双金属氧化物构建交错的催化表面,用于-O电池中的氧气电极过程2
Zongqiang Sun1, Xiaodong Lin1,2, Chutao Wang1
1State Key Laboratory of Physical Chemistry of Solid Surfaces, Collaborative Innovation Center of Chemistry for Energy Materials (i-ChEM), Engineering Research Centre of Electrochemical Technologies of Ministry of Education, Department of Chemistry, College of Chemistry and Chemical Engineering, Xiamen University, Xiamen, 361005, China.
Advanced materials (Deerfield Beach, Fla.)
|May 28, 2024
概括
研究人员开发了一种用于氧电池的新型-氧化阴极. 这种新材料通过优化放电产品的存储和防止活动部位被动化来提高电池容量和寿命.
科学领域:
- 材料科学 材料科学 材料科学
- 电化学 电化学 电化学
- 储能 储能 储能 储能 储能 储能
背景情况:
- 氧 (Li-O2) 电池具有高的理论能量密度,但实际容量较低.
- 固体排放产品对活点的被动化限制了传统电池的性能.
- 优化放电产品的增长和储存对于推进电池技术至关重要.
研究的目的:
- 开发用于氧电池的先进氧气电极,克服活点被动化的局限性.
- 为了研究一种新的添加双金属-氧化物,具有交错的催化表面 (ICS) 和类似玉米的结构.
主要方法:
- 在碳布上制造含的双金属-氧化物 (CoNiO2-xFx) 与玉米类似的结构.
- 使用与传统方法不同的"竞争性吸附催化机制"来描述材料的催化性能.
- 在电池中的CoNiO2-xFx/CC阴极的电化学测试,以评估特定容量和循环稳定性.
主要成果:
- CoNiO2-xFx/CC的ICS显示出一种具有竞争力的吸附机制,促进氧气转化和Li2O2的增长.
- 在Li2O2形态从表面膜转变为状颗粒的转变有效地防止了活体部位的埋葬.
- 电极的开放式架构促进了高效的氧气捕获/释放和LiO2分解,导致高特异性容量 (30923 mAh g-1) 和延长寿命 (>580周期).
结论:
- 拟议的CoNiO2-xFx/CC阴极通过解决放电产品被动化问题,显著提高了Li-O2电池的性能.
- 具有竞争力的吸附催化机制和独特的纳米结构为开发高性能金属氧化物阴极提供了有前途的战略.
- 这一进步代表了对现有的基于金属氧化物的立电池阴极的重大改进.
相关概念视频
02:47Voltaic/Galvanic Cells
Spontaneous Chemical Reactions
Spontaneous redox reactions occur abundantly in nature. The chemical reaction occurring in a disposable AA battery powering our remote controls is one such example of a spontaneous redox reaction. Another example is the immersion of coiled copper wire into an aqueous silver nitrate solution. The reaction shows a gradual, visually impressive color change from colorless to bright blue and the formation of a grey precipitate on the copper wire. In this experiment,...
Spontaneous redox reactions occur abundantly in nature. The chemical reaction occurring in a disposable AA battery powering our remote controls is one such example of a spontaneous redox reaction. Another example is the immersion of coiled copper wire into an aqueous silver nitrate solution. The reaction shows a gradual, visually impressive color change from colorless to bright blue and the formation of a grey precipitate on the copper wire. In this experiment,...
03:12Batteries and Fuel Cells
A battery is a galvanic cell that is used as a source of electrical power for specific applications. Modern batteries exist in a multitude of forms to accommodate various applications, from tiny button batteries such as those that power wristwatches to the very large batteries used to supply backup energy to municipal power grids. Some batteries are designed for single-use applications and cannot be recharged (primary cells), while others are based on conveniently reversible cell reactions that...
01:28Electrochemical Cells
Electrochemical cells are systems that convert chemical energy into electrical energy or use electrical energy to drive chemical reactions. They consist of two electrodes in contact with an electrolyte, where redox reactions enable electron transfer. Most electrochemical cells include two half-cells connected by an external wire for electron flow and a salt bridge for ion flow. The salt bridge contains an electrolyte solution and maintains charge neutrality by allowing ions—not electrons—to...
01:24Types of Reversible Electrodes
For electrode reversibility to be maintained, all the reactants and products involved in the half-reaction must be present at the electrode. There are several types of reversible electrodes (half-cells).In metal-metal-ion electrodes, a metal balances electrochemically with a solution of its own ions. Examples are Cu2+|Cu and Zn2+|Zn. Metals that react with the solvent, like group 1 and most group 2 metals, which react with water, and zinc, which reacts with aqueous acidic solutions, cannot be...
01:30The Electrical Double Layer
In the region where two bulk phases meet, an intricate electric charge distribution arises due to charge transfer, ion adsorption, molecular orientation, and charge distortion. This complex distribution is commonly referred to as the electrical double layer.When a solid electrode interfaces with ions in an electrolyte solution, the speed of electron transfer dictates the rates of oxidation and reduction. The electrode acquires a charge through the escape of atoms into the solution as cations or...
01:30Processes at Electrodes
The electrode interacts with ions in the electrolyte solution at its interface. The rate of oxidation and reduction depends on the speed at which electrons can transfer through this interface. As ions attach to or leave the electrode surface, the electrode acquires a charge, and an electrical potential forms across the interface, making the process more difficult to reach equilibrium. The charge on the electrode affects the local ion concentrations in the solution, though thermal motion...