Electrochemistry
Electrochemistry is the study of production of electricity from energy released during spontaneous reactions and the use of electrical energy to bring about non-spontaneous chemical transformations. Electrochemistry is the study of chemical processes that cause electrons to move. This movement of electrons is called electricity, which can be generated by movements of electrons from one element to another in a reaction known as an oxidation-reduction (“redox”) reaction.
Electroanalytical chemistry encompasses a group of quantitative analytical methods that are based upon the electrical properties of an analyte solution when it is made part of an electrochemical cell.
Electrochemical cells consist of two electrodes: an anode (the electrode at which the oxidation reaction occurs) and a cathode (the electrode at which the reduction reaction occurs).
There are two types of electrochemical cells: galvanic (ones that spontaneously produce electrical energy) and electrolytic (ones that consume electrical energy).
An electrolytic cell has an endothermic chemical reaction. The reaction is not spontaneous so a power source is required. Energy is stored in an electrochemical cell. That energy can be released when the cell is allowed to run in a galvanic mode. Electolytic cells reverse the current flow by using an External Power Source, which in this case is a battery. Reverses the half-cell reactions in each compartment.
Nernst Equation is an equation used to calculate the electrical potential of a chemical reaction. In its equilibrium state, the Nernst equation should be zero. It also shows the direct relation between energy or potential of a cell and its participating ions and is expressed as follows:-
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