自回收电子捐赠者抵御了 Cu(I) 电催化剂的不利氧化重建,通过电荷补偿来去除酸盐
Jiaqi Chen1, Yuan Yao1, Yu Yan1
1MIIT Key Laboratory of Critical Materials Technology for New Energy Conversion and Storage, School of Chemistry and Chemical Engineering, Harbin Institute of Technology, Harbin 150001, China.
Water research
|December 14, 2024
概括
酸盐污染是一个全球性的问题. 这项研究引入了一种新的催化剂策略,使用来防止铜氧化,显著改善从水中去除酸盐,以改善环境和人类健康.
科学领域:
- 环境化学环境化学
- 材料科学 材料科学 材料科学
- 电化学 电化学 电化学
背景情况:
- 自然水中酸盐的积累对环境和人类健康构成重大风险.
- 对氨的电化学酸盐还原反应 (eNO3RR) 是在环境条件下酸盐去除的一个有前途的方法.
- 基于铜的eNO3RR催化剂容易氧化为铜,从而降低它们的性能.
研究的目的:
- 制定一个费用补偿策略,以提高基于铜的eNO3RR催化剂的稳定性.
- 提高催化剂的活性和耐用性,以有效地从水中去除酸盐.
主要方法:
- 使用自循环电子捐赠体 (Ti(III)) 来防止铜氧化的电荷补偿策略.
- 使用Ti (III) 修改的Cu2O/Cu催化剂作为概念验证模型.
- 通过间隔电荷转移 (IVCT) 来研究Cu (I) 从Cu (II) 的再生和Ti (III) 的循环利用.
主要成果:
- 与未经修改的Cu2O/Cu相比,Ti-改性Cu2O/Cu催化剂 (Ti-Cu2O/Cu-10) 的活性和耐久性显著提高.
- 在15个连续周期 (30小时) 中,在0.9V与RHE相比,从水中达到约95.0%的酸盐去除 (初始度为60 mg·L−1 NO3−-N).
- (III) 供体成功再生了Cu (I) 并且本身被回收,抵抗催化剂氧化.
结论:
- 电荷补偿策略有效地防止了基于Cu (I) 的eNO3RR催化剂的氧化和重建.
- 这种方法提供了一种可行和可持续的方法,可以更有效和更持久地从水中去除酸盐.
- 这些发现为环境修复中先进的催化材料铺平了道路.
相关概念视频
Voltaic/Galvanic Cells
56.8K
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,...
56.8K
Electrodeposition
597
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...
Electrodeposition can...
597
Balancing Redox Equations
51.7K
Electrochemistry is the science involved in the interconversion of electrical and chemical reactions. Such reactions are called reduction-oxidation, or redox reactions. These important reactions are defined by changes in oxidation states for one or more reactant elements and include a subset of reactions involving the transfer of electrons between reactant species. Electrochemistry as a field has evolved to yield sufficient insights on the fundamental principles of redox chemistry and multiple...
51.7K
Electrolysis
26.0K
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...
26.0K
Ladder Diagrams: Redox Equilibria
428
Ladder diagrams are useful tools for understanding redox equilibrium reactions, especially the effects of concentration changes on the electrochemical potential of the reaction. The vertical axis in the redox ladder diagrams represents the electrochemical potential, E. The area of predominance is demarcated using the Nernst equation.
Consider the Fe3+/Fe2+ half-reaction, which has a standard-state potential of +0.771 V. At potentials more positive than +0.771 V, Fe3+ predominates, whereas Fe2+...
Consider the Fe3+/Fe2+ half-reaction, which has a standard-state potential of +0.771 V. At potentials more positive than +0.771 V, Fe3+ predominates, whereas Fe2+...
428
Standard Electrode Potentials
43.4K
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...
43.4K


![[DPEPhosbcpCu]PF6: A General and Broadly Applicable Copper-Based Photoredox Catalyst](/_next/image?url=https%3A%2F%2Fcloudfront.jove.com%2FCDNSource%2Fteasers%2F59739.jpg&w=3840&q=50)