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Related Concept Videos

Electrolysis03:00

Electrolysis

31.6K
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...
31.6K
Electrodeposition01:08

Electrodeposition

1.9K
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...
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Voltaic/Galvanic Cells02:47

Voltaic/Galvanic Cells

68.4K
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,...
68.4K
Electrochemical Cells01:28

Electrochemical Cells

161
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...
161
Standard Electrode Potentials03:02

Standard Electrode Potentials

52.1K
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...
52.1K
Electrochemical Systems01:24

Electrochemical Systems

105
Electrochemical systems provide a fascinating insight into the dynamic interplay of charged species within various phases. One notable example is the interaction between a membrane permeable to K⁺ ions but not to Cl⁻ ions, separating an aqueous KCl solution from pure water. As K⁺ ions diffuse through the membrane, they generate net charges on each phase, leading to a potential difference between them.Similarly, when a piece of Zn is immersed in an aqueous ZnSO₄ solution,...
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Development and Validation of Chromium Getters for Solid Oxide Fuel Cell Power Systems
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Development and Validation of Chromium Getters for Solid Oxide Fuel Cell Power Systems

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Solid oxide electrolysis: Concluding remarks.

Areum Jun1, Young-Wan Ju1, Guntae Kim1

  • 1Department of Energy Engineering, Ulsan National Institute of Science and Technology (UNIST), Ulsan, Republic of Korea. gtkim@unist.ac.kr.

Faraday Discussions
|October 17, 2015
PubMed
Summary
This summary is machine-generated.

Renewable energy requires effective storage. Chemical energy storage using hydrogen and carbon dioxide offers a scalable solution, overcoming limitations of secondary batteries for sustainable fuel production.

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Probing and Mapping Electrode Surfaces in Solid Oxide Fuel Cells
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Area of Science:

  • Energy science and sustainable technology.
  • Chemical engineering and materials science.

Background:

  • Growing demand for renewable energy sources like solar and wind necessitates efficient energy storage solutions.
  • Current secondary batteries face challenges including high costs, limited capacity, and charge loss over time.
  • Chemical energy storage offers a promising alternative with no capacity constraints.

Purpose of the Study:

  • To explore chemical energy storage as a viable alternative to secondary batteries for renewable energy.
  • To highlight the potential of hydrogen and carbon dioxide as energy carriers.
  • To discuss the role of electrolysis in converting renewable energy into chemical fuels.

Main Methods:

  • Review of renewable energy technologies and their storage requirements.
  • Analysis of limitations associated with conventional secondary batteries.
  • Exploration of chemical energy storage pathways, including water electrolysis and solid oxide electrolysis (SOE).

Main Results:

  • Chemical energy storage, utilizing hydrogen (H2) and carbon dioxide (CO2), presents a scalable solution for renewable energy.
  • Water electrolysis can convert H2O into hydrogen using surplus renewable energy.
  • Solid oxide electrolysis enables the reduction of CO2 and recycling of CO2 and H2O into sustainable hydrocarbon fuels.

Conclusions:

  • Chemical energy storage is essential for matching renewable energy supply with demand.
  • Electrolysis technologies, particularly SOE, are key to producing sustainable fuels from CO2 and H2O.
  • Developing advanced energy storage is critical for a sustainable energy future.