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In aqueous solutions, redox potential is a measure of the tendency of the solution to either gain or lose electrons in a reaction. A solution with a higher (more positive) reduction potential than some other molecule will have a tendency to gain electrons from this molecule (i.e. to be reduced by oxidizing this other molecule) and a solution with a lower (more negative) reduction potential ...
The nature of the electroactive species (the analyte) in the solution also critically affects the exchange current densities, both the reduced and oxidized form. Less important but still relevant are the environment of the solution including the solvent, nature of other electrolytes, and temperature.
The electrochemical window (EW) of a substance is the electrode electric potential range between which the substance is neither oxidized nor reduced. The EW is one of the most important characteristics to be identified for solvents and electrolytes used in electrochemical applications. The EW is a term that is commonly used to indicate the ...
Organic redox reactions: the Birch reduction. Organic reductions or organic oxidations or organic redox reactions are redox reactions that take place with organic compounds.In organic chemistry oxidations and reductions are different from ordinary redox reactions, because many reactions carry the name but do not actually involve electron transfer. [1]
D is the diffusion coefficient of the species, where subscripts O and R stand for the oxidized and reduced species respectively; C b is the concentration of the O and R species in the bulk; C is the concentration of the electrolyte; A denotes the surface area; Θ denotes the fraction of the O and R species present.
Iron (Fe) has been oxidized because the oxidation number increased. Iron is the reducing agent because it gave electrons to the oxygen (O 2). Oxygen (O 2) has been reduced because the oxidation number has decreased and is the oxidizing agent because it took electrons from iron (Fe).
where k f and k b are the reaction rate constants, with units of frequency (1/time) and c o and c r are the surface concentrations (mol/area) of the oxidized and reduced molecules, respectively (written as c o (0,t) and c r (0,t) in the previous section). The net rate of reaction v and net current density j are then: [Note 2]
A redox indicator (also called an oxidation-reduction indicator) is an indicator which undergoes a definite color change at a specific electrode potential.. The requirement for fast and reversible color change means that the oxidation-reduction equilibrium for an indicator redox system needs to be established very quickly.