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Electrochemistry and RED-OX Reactions
Published in Armen S. Casparian, Gergely Sirokman, Ann O. Omollo, Rapid Review of Chemistry for the Life Sciences and Engineering, 2021
Armen S. Casparian, Gergely Sirokman, Ann O. Omollo
Consider the arrangement shown in Figure 7.1. This arrangement is known as an electrochemical cell, and the underlying electrochemical reaction involves simultaneous oxidation and reduction reactions. Electrochemical cells are the basis of the operation of all batteries. If the reactions and current flow are spontaneous, as in any battery, the cell is called a voltaic or galvanic cell. If, instead, electrical energy must be supplied, the cell is called an electrolytic cell, and the process is known as electrolysis.
Electrochemistry
Published in W. John Rankin, Chemical Thermodynamics, 2019
An electrochemical cell that produces electricity as a result of a spontaneous reaction is called a galvanic cell. Batteries and fuel cells are galvanic cells. A cell in which a non-spontaneous reaction is driven by an external source of current is called an electrolytic cell. These cells are used for electrowinning of metals from solutions, electroplating of metals, electrorefining of metals and in other applications.
Flexible and Stretchable Energy Storage
Published in Muhammad Mustafa Hussain, Nazek El-Atab, Handbook of Flexible and Stretchable Electronics, 2019
A battery consists of an anode (where the oxidation half-reaction takes place), electrolyte, and cathode (where reduction half-reaction takes place). Depending on the usage of an external loading circuit, a galvanic cell uses the spontaneous redox reaction to generate electricity with a faradic current from the anode to the cathode. An electrolytic cell uses electricity to force the non-spontaneous chemical reaction to take place. With this in mind, we can divide the battery types into two main types: primary batteries are non-rechargeable batteries that can only work as a galvanic cell. Primary batteries (similar to batteries in cars) utilize conversion electrodes (e.g., FeF3) which undergo a chemical reaction in which its structure is consumed. On the other hand, rechargeable batteries or secondary batteries can be used as both galvanic and electrolytic cells. They utilize intercalation electrodes (graphite, LiCoO2, LiFePO4) that function as a host structure for ionic species (e.g., lithium ions).
Plasma synthesis of ammonia by asymmetric electrode arrangement
Published in Materials and Manufacturing Processes, 2023
F. Baharlounezhad, M.A. Mohammadi, M.S. Zakerhamidi
Electrolysis is the process of passing an electric current through the material to cause a chemical change. This process takes place in an electrolytic cell, a reactor consisting of cathode and anode electrodes immersed in a solution containing positive and negative charged ions. An electrolytic cell, also known as an electrolysis reactor, converts electrical energy into chemical energy. Metal conductors are used as electrodes in electrolysis reactors. Electrodes are responsible for the transmission of electrons in certain circumstances and are also engaged in electrolysis processes in others. The cathode is the electrode that sends electrons to the anode across the electrolyte environment, and the anode is the electrode that receives electrons from the cathode. Electrolysis is widely used in metallurgical engineering [42,43] like electrowinning,[44,45] electrorefining,[46–48] and electroplating.[49,50] The electrodes of an electrochemical system with asymmetric electrode configurations might differ in form, size, material, and design from one another.
Parametric analysis of water electrolysis by dual electrolytes and cells
Published in International Journal of Green Energy, 2019
Ming-Yuan Lin, Lih-Wu Hourng, Kai-Lin Chiou
When the electrodes are placed in an electrolytic cell and the electric current is conducted through the electrolyte solution, cations will move toward the cathode, while anions move to the anode. A chemical reaction is thus completed, and this phenomenon is called electrolysis.