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Electron transfer reactions are central to myriad processes and properties in soils, and redox potential, quantified as Eh (platinum electrode potential relative to the standard hydrogen electrode) or pe (analogous to pH as -log electron activity), is a master variable, along with pH, that controls and is governed by chemical reactions and ...
Latimer diagrams can be used in the construction of Frost diagrams, as a concise summary of the standard electrode potentials relative to the element.Since Δ r G o = -nFE o, the electrode potential is a representation of the Gibbs energy change for the given reduction.
Redox conditions are measured according to the redox potential (E h) in volts, which represents the tendency for electrons to transfer from an electron donor to an electron acceptor. E h can be calculated using half reactions and the Nernst equation . [ 1 ]
In an electron transport chain, the redox reactions are driven by the difference in the Gibbs free energy of reactants and products. The free energy released when a higher-energy electron donor and acceptor convert to lower-energy products, while electrons are transferred from a lower to a higher redox potential , is used by the complexes in ...
Electron transfer (ET) occurs when an electron relocates from an atom, ion, or molecule, to another such chemical entity. ET describes the mechanism by which electrons are transferred in redox reactions. [2] Electrochemical processes are ET reactions. ET reactions are relevant to photosynthesis and respiration and commonly involve transition ...
Cyclic voltammetry (CV) has become an important and widely used electroanalytical technique in many areas of chemistry. It is often used to study a variety of redox processes, to determine the stability of reaction products, the presence of intermediates in redox reactions, [10] electron transfer kinetics, [11] and the reversibility of a ...
The second electron and proton atom are transferred to the carbon atom adjacent to the N atom. The midpoint potential of the NAD + /NADH redox pair is −0.32 volts, which makes NADH a moderately strong reducing agent. [7] The reaction is easily reversible, when NADH reduces another molecule and is re-oxidized to NAD +.
For example, an enzyme that catalyzed this reaction would be an oxidoreductase: A – + B → A + B – In this example, A is the reductant (electron donor) and B is the oxidant (electron acceptor). In biochemical reactions, the redox reactions are sometimes more difficult to see, such as this reaction from glycolysis: