Applications of standard potentials
Start with the big picture
The standard cell potential, E°, indicates the thermodynamic tendency of a redox reaction: through ΔG° = −nF E°, a positive cell potential corresponds to a negative standard Gibbs free-energy change and a spontaneous reaction. When conditions depart from the standard state, the Nernst equation relates cell potential to the reaction quotient. Electrochemical-series comparisons help forecast electron flow and displacement reactions, while E° values also connect to equilibrium constants. Together, these ideas support applications such as galvanic-cell and battery selection, electrolysis, corrosion assessment, redox titration endpoints, and metal refining. The topic also introduces how potential changes inform ion measurements and sensors, and how midpoint potentials help describe electron transfer in biological systems. Further study considers pH-dependent stability and mixed-potential behavior.
What you'll learn
- Relate standard cell potential to Gibbs free-energy change and reaction spontaneity.
- Use the Nernst equation conceptually to connect cell potential with non-standard conditions.
- Explain how electrochemical-series comparisons predict electron flow and displacement reactions.
- Identify applications of standard potentials in cells, electrolysis, corrosion, and measurement.
- Describe how potentials relate to equilibrium constants and biological redox chains.
Continue your study
Work through the complete notes and reinforce the topic with the study tools available in the full lesson.
