H2O electrolysis

The electrochemical reactor has two magic properties (1) It causes chemical reaction where equilibrium does not permit reaction in the absence of an electric field and (2) it causes a separation of products because they are generated at different electrodes. The electrode surfaces are catalysts to promote certain reactions. In H2O electrolysis... 

The total cell activation overpotential is the sum of the activation overpotentials at the anode and cathode, as shown in Fig. 13 for the case of H2O electrolysis using Pt electrodes in alkaline solutions. The two overpotentials can be separated by the use of a reference electrode. Thus, the use of reference electrodes is essential for the study of electrocatalysis, since in this case one can individually study the dependence of each electrode overpotential on the current and thus assess the elec-trocatalytic performance of each electrode. The best electrocatalyst, for each charge-transfer reaction is, obviously, the one that minimizes the activation overpotential. 

NaBi02 3H20, cat 4-FhC02-TEMP0, HOAc KI, H2O, electrolysis... 

H2O into H2 and O2 using an electric current passed through the H2O. In H2O electrolysis, an electrical power source is connected to two electrodes, or two plates (typically made from some inert metal such as platinum, stainless steel, or iridium) that are placed in the H2O. Consequently, the H2 will appear in the cathode and O2 in the... 

Aside from chemical cogeneration studies, where the electrocatalytic anodic and cathodic reactions are driven by the voltage spontaneously generated by the solid electrolyte cell, several other electrocatalytic reactions have been investigated in solid electrolyte cells. " These reactions are listed in Table 2. Earlier studies by Kleitz and co-workers had focused mainly on the investigation of electrocatalysts for H2O electrolysis. " Huggins and co-workers were the first to show that other electrocatalytic reactions, such as NO decomposition and CO... 

With the exception of H2O electrolysis, " it is likely that, for all other electrocatalytic reactions listed in Table 2, catalytic phenomena taking place on the gas-exposed electrode surface or also on the solid electrolyte surface, had a certain role in the observed kinetic behavior. However, this role cannot be quantified, since the measured increase in reaction rate was, similarly to the case of the reactions listed in Table 1, limited by Faraday s law, that is. 

Electrolysis. For reasons not fiiUy understood (76), the isotope separation factor commonly observed in the electrolysis of water is between 7 and 8. Because of the high separation factor and the ease with which it can be operated on the small scale, electrolysis has been the method of choice for the further enrichment of moderately enriched H2O—D2O mixtures. Its usefiilness for the production of heavy water from natural water is limited by the large amounts of water that must be handled, the relatively high unit costs of electrolysis, and the low recovery. 

Heavy water [11105-15-0] 1 2 produced by a combination of electrolysis and catalytic exchange reactions. Some nuclear reactors (qv) require heavy water as a moderator of neutrons. Plants for the production of heavy water were built by the U.S. government during World War II. These plants, located at Trad, British Columbia, Morgantown, West Virginia, and Savaimah River, South Carolina, have been shut down except for a portion of the Savaimah River plant, which produces heavy water by a three-stage process (see Deuterium and tritium) an H2S/H2O exchange process produces 15% D2O a vacuum distillation increases the concentration to 90% D2O an electrolysis system produces 99.75% D2O (58). 

Electrolysis applied voltage = 10 V, AcONa, AcOH K2CO3, MeOH, H2O, 80-95% yield."... 

Electrolysis, Bu4N Br, H2O, CH3CN, NaHC03- This method is unsatisfactory for primary and secondary alcohols, aldehydes, olefins, or amines. 

Electrolysis 1.5 V, CH3CN, H2O, UCIO4 or Bu4N-"C104, 50-75% yield. " 1,3-Dithiolanes were not cleaved efficiently, by electrolytic oxidation. 

Electrolysis, CH3CN, H2O, LiC104, 1.5 V, rt, 60-95% yield. The released quinone is removed by forming the bisulfite adduct, which can be washed out with water. 

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