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Chapter 16 Elements of Electrochemistry Class Notes: ?G = -nFEcell = -RTlnK ?G = ?H - T?S G = Gibbs change in free energy; a thermodynamic quantity E = internal energy of cell F = Faraday's constant n = moles of electrons R = 8.31 constant T = temperature in Kelvin ln = natural log of K or 2.303 log K K = equilibrium coefficient H = enthaply S = entropy I. Redox Reactions - reduction - addition of electrons to an atom, as occurs during the addition of hydrogen to a molecule or the removal of oxygen from it - oxidation - loss of electron density from an atom as occurs upon addition of oxygen to a molecule or upon removal of hydrogen Example: Cu2+ + 2e- [KAK1]- Cu E° = +0.335 Zn2+ + 2e- - Zn E° = -0.799 0.335 - (-0.799) = 1.134 V Ecell = 1.134 Volts For an exothermic spontaneous reaction: ?G <0 E> 0 K>> 1 Reduction --> cathode - more positive E Oxidation --> anode - more negative E ?G = -nFE ?G...

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