The Effect of Concentration on Cell Potential: The Nernst Equation
{"Image DocumentName": "The Effect of Concentration on Cell Potential: The Nernst Equation", "Image ImageDescription": "\u2022 When a redox reaction is at equilibrium (\uf044G = 0), the Nernst equation reduces to. E\u00bacell = (RT/nF)ln K because Q = K and there is no net transfer of electrons (Ecell = 0) \u2022 Substituting the values of the constants into the Nernst equation with T = 298 K and converting to base-10 logarithms gives the relationship of the actual cell potential (Ecell), the standard cell potential (E\u00bacell), and the reactant and product concentrations at room temperature (contained in Q): Ecell = E\u00bacell \u2013 ( V/n)logQ.", "Image XResolution": "37", "Image YResolution": "37", "Image ResolutionUnit": "Pixels/Centimeter", "Image Software": "SlidePlayer", "Image YCbCrPositioning": "Centered"}