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(chemistry) The science of the chemistry associated with the flow of electricity, especially at the surface of an electrode
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Michael Faraday was another early worker, whose major contribution to chemistry was electrochemistry, in which (among other things) a certain quantity of electricity during electrolysis or electrodeposition of metals was shown to be associated with certain quantities of chemical elements, and fixed quantities of the elements therefore with each other, in specific ratios.
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General chemistry courses typically introduce concepts such as stoichiometry, prediction of reaction products, thermodynamics, nuclear chemistry, electrochemistry, chemical kinetics, and many of the rudiments of physical chemistry.
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This is related to a mercury electrode where a metal can be reduced, the metal will often then dissolve in the mercury to form an amalgam that modifies its electrochemistry greatly.
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The concepts taught in a typical general chemistry course are as follows: Stoichiometry Conservation of energy Conservation of mass Elementary atomic theory Periodic table and periodicity Law of constant composition Gas laws Nuclear chemistry Solubility Acid-base chemistry Chemical bonding Chemical kinetics Thermodynamics Electrochemistry Chemical equilibria Media related to General chemistry at Wikimedia Commons
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This acid–base theory was a revival of oxygen theory of acids and bases, proposed by German chemist Hermann Lux in 1939, further improved by Håkon Flood circa 1947 and is still used in modern geochemistry and electrochemistry of molten salts.
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A standard half-cell, used in electrochemistry, consists of a metal electrode in a 1 molar (1 mol/L) aqueous solution of the metal's salt, at 298 kelvins (25 °C).
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Cynthia G. Zoski (Editor) Handbook of Electrochemistry.
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Knowledge of activity coefficients is particularly important in the context of electrochemistry since the behaviour of electrolyte solutions is often far from ideal, due to the effects of the ionic atmosphere.
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Electrode potential, E, in chemistry or electrochemistry, according to a IUPAC definition, is the electromotive force of a cell built of two electrodes: on the left-hand side of the cell diagram is the standard hydrogen electrode (SHE), and on the right-hand side is the electrode in question.
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In electrochemistry, the Nernst equation is an equation that relates the reduction potential of an electrochemical reaction (half-cell or full cell reaction) to the standard electrode potential, temperature, and activities (often approximated by concentrations) of the chemical species undergoing reduction and oxidation.
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His invention gave birth to a new field of science, electrochemistry, and new technologies such as electroplating.
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Electrochemistry, Past and Present.
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The related Nernst equation in electrochemistry gives the difference in electrode potential as a function of redox concentrations.
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1800 Alessandro Volta devises the first chemical battery, thereby founding the discipline of electrochemistry.
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Thus, Volta is considered to be the founder of the discipline of electrochemistry.
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