SUMMARY
Cell potentials in redox reactions are not multiplied by the coefficients in the balanced equation because they are intensive properties, which remain constant regardless of the amount of substance. The relationship between Gibbs free energy (ΔG) and cell potential (E) is defined by the equation ΔG = -nFE, where n represents the moles of electrons transferred and F is Faraday's constant. This indicates that while ΔG is dependent on the number of moles, the cell potential E remains unchanged by stoichiometric coefficients.
PREREQUISITES
- Understanding of redox reactions and their balanced equations
- Familiarity with Gibbs free energy and its significance in electrochemistry
- Knowledge of intensive vs. extensive properties in chemistry
- Basic grasp of Faraday's constant and its role in electrochemical calculations
NEXT STEPS
- Study the concept of intensive and extensive properties in detail
- Learn about the derivation and applications of the Gibbs free energy equation
- Explore the role of Faraday's constant in electrochemical systems
- Investigate how to calculate standard cell potentials for various redox reactions
USEFUL FOR
Chemistry students, educators, and professionals in electrochemistry or chemical engineering seeking to deepen their understanding of redox reactions and cell potential calculations.