Half-cell reduction-reaction voltage depends on oxidized and reduced concentrations, temperature, and number of electrons transferred {Nernst equation}. V = V0 - R * T / (n * ln([Co] - [Cr])), where V is reaction potential, V0 equals standard unit cell potential, R is gas constant, T is temperature, n is number of electrons transferred, Co is oxidized-ion concentration, and Cr is reduced-ion concentration.
Activation energy comes from electric field and from temperature.
valence charge
Electrode voltage is V = V0 + R * T * ln(K / (z * F)), where V is voltage, V0 is standard potential, R is gas constant, T is temperature, K is equilibrium constant, z is absolute value of transferred charge {valence charge}, and F is 1 Faraday. Therefore, exp(-V / (R*T)) = K / (z * F) and K = z * F * exp(-V / (R*T)). Standard potential is at concentration 1 M, pressure 1 atmosphere, and temperature 25 C. Solids have concentration = 1. Voltage is always positive. If V > 0, reaction is spontaneous. At equilibrium, voltage = 0 and current = 0.
Physical Sciences>Chemistry>Inorganic>Oxidation-Reduction>Potential
5-Chemistry-Inorganic-Oxidation-Reduction-Potential
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Date Modified: 2022.0224