Electrochemistry applies the principles of thermodynamics to chemical reactions that produce or consume electrical energy. In this chapter, we develop the relationships between Gibbs energy, cell potential, equilibrium, and the Nernst equation, providing a thermodynamic framework for understanding electrochemical cells under both standard and non-standard conditions. These concepts are then applied to concentration cells, equilibrium constants, solubility products, and the temperature dependence of electrochemical processes.
Learn how electrochemical cells convert chemical energy into electrical work. You will develop the relationship between Gibbs energy and cell potential and use it to determine whether a redox reaction is spontaneous.
Learn to identify oxidation and reduction half-reactions, the anode and cathode, and interpret standard cell notation. You will also calculate standard cell potentials from standard reduction potentials.
Develop and apply the Nernst equation to calculate cell potentials under non-standard conditions. You will see how changes in concentration affect the voltage produced by an electrochemical cell.
Connect electrochemical measurements to thermodynamics by relating cell potentials, equilibrium constants, and Gibbs energy. Applications include concentration cells and the determination of equilibrium and solubility constants from electrochemical data.
Explore how standard cell potentials change with temperature and how these changes are related to reaction entropy. You will use electrochemical measurements to determine important thermodynamic properties of chemical reactions.