Calculate E° for each of the following reactions, and tell which are spontaneous under standard-state conditions. (a)

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Key Concepts

Standard Electrode Potential (E°)

Standard electrode potential (E°) is a measure of the tendency of a chemical species to be reduced, measured under standard conditions (1 M concentration, 1 atm pressure, and 25°C). It is expressed in volts and is crucial for predicting the direction of redox reactions. A positive E° indicates a spontaneous reaction, while a negative E° suggests non-spontaneity.

Gibbs Free Energy (ΔG)

Gibbs free energy (ΔG) is a thermodynamic potential that indicates the spontaneity of a reaction at constant temperature and pressure. The relationship between E° and ΔG is given by the equation ΔG = -nFE°, where n is the number of moles of electrons transferred and F is Faraday's constant. A negative ΔG corresponds to a spontaneous reaction.

Nernst Equation

The Nernst equation relates the cell potential (E) of an electrochemical reaction to the standard electrode potential (E°) and the concentrations of the reactants and products. It is expressed as E = E° - (RT/nF)ln(Q), where Q is the reaction quotient. This equation allows for the calculation of E under non-standard conditions and helps determine the spontaneity of reactions based on concentration changes.