SUMMARY
The Gibbs free energy for an electrochemical cell is defined by the equation G = -nFE, where G represents Gibbs free energy, n is the number of moles of electrons, F is Faraday's constant, and E is the cell potential. The relationship between standard state Gibbs free energy (ΔGθ) and the equilibrium constant (K) is established through the equation ΔGθ = -nFEθ, where Eθ is the standard cell potential. At equilibrium, the free energy change (ΔG) is zero, leading to the conclusion that K equals the reaction quotient Q. Thus, the derived expression relating standard state cell potential and equilibrium constant is ΔGθ = -RT ln(K).
PREREQUISITES
- Understanding of Gibbs free energy and its equations
- Familiarity with electrochemical cells and cell potential
- Knowledge of the relationship between equilibrium constants and reaction quotients
- Basic principles of thermodynamics in chemical reactions
NEXT STEPS
- Study the derivation of the Nernst equation for electrochemical cells
- Explore the relationship between Gibbs free energy and spontaneity of reactions
- Learn about the implications of standard state conditions in thermodynamics
- Investigate the role of temperature in Gibbs free energy calculations
USEFUL FOR
Chemistry students, electrochemists, and anyone studying thermodynamics in relation to chemical reactions will benefit from this discussion.
