The discussion centers on the conditions for using two key thermodynamic equations related to Gibbs free energy. The first equation, ΔG = -nFEmax, is applicable in electrochemical systems where the Faraday constant (F) is relevant, particularly in calculating the maximum work obtainable from an electrochemical reaction. It is typically used when dealing with processes involving electron transfer and redox reactions.The second equation, ΔG = ΔG° + RT ln(Q), is used in general chemical reactions to relate the standard Gibbs free energy change (ΔG°) to the actual Gibbs free energy change (ΔG) under non-standard conditions, where Q represents the reaction quotient. The two terms on the right-hand side signify the standard state contribution (ΔG°) and the effect of concentration or pressure changes on the system (RT ln(Q)). Understanding when to apply each equation is crucial for accurately analyzing thermodynamic processes in chemistry.
