var nc = 16, fc = new Array(nc); fc[0] = {t:"Anode",d:"An electrode at which an oxidation half-reaction (loss of electrons) takes place."}; fc[1] = {t:"Cathode",d:"An electrode at which a reduction half-reaction (gain of electrons) takes place."}; fc[2] = {t:"Cell Diagram",d:"Symbols that show how the components of an electrochemical cell are connected."}; fc[3] = {t:"Cell Potential (Ecell)",d:"The electromotive force expressed in volts (V) with which an electrochemical cell can push electrons through an external circuit connected to its terminals."}; fc[4] = {t:"Electrochemical Cell",d:"An apparatus that converts chemical energy into electrical work or electrical work into chemical energy."}; fc[5] = {t:"Electrochemistry",d:"The branch of chemistry that examines the transformations between chemical and electrical energy."}; fc[6] = {t:"Electrolysis",d:"A process in which electrical energy is used to drive a nonspontaneous chemical reaction."}; fc[7] = {t:"Electrolytic Cell",d:"A device in which an external source of electrical energy does work on a chemical system, turning reactant(s) into higher-energy product(s)."}; fc[8] = {t:"Electromotive Force (EMF)",d:"Also called voltage, the force pushing electrons through an electrical circuit."}; fc[9] = {t:"Faraday’s Constant (F)",d:"The magnitude of electrical charge in 1 mole of electrons. Its value to three significant figures is 9.65 × 104 C/mol."}; fc[10] = {t:"Fuel Cell",d:"A voltaic cell based on the oxidation of a continuously supplied fuel. The reaction is the equivalent of combustion, but chemical energy is converted into electrical energy."}; fc[11] = {t:"Nernst Equation",d:"An equation relating the potential of a cell (or halfcell) reaction to its standard potential (E°) and to the concentrations of its reactants and products."}; fc[12] = {t:"Standard Cell Potential (Ecell°)",d:"A measure of how forcefully an electrochemical cell, in which all reactants and products are in their standard states, can pump electrons through an external circuit."}; fc[13] = {t:"Standard Hydrogen Electrode (SHE)",d:"A reference electrode based on the half-reaction 2H+(aq) + 2e → H2(g) that produces a standard electrode potential of 0.000 V."}; fc[14] = {t:"Standard Reduction Potential (Ered°)",d:"The potential of a reduction halfreaction in which all reactants and products are in their standard states at 25°C."}; fc[15] = {t:"Voltaic Cell",d:"An electrochemical cell in which chemical energy is transformed into electrical work by a spontaneous redox reaction."};