What is the purpose of measuring electrode potentials in electrochemistry?

Measuring electrode potentials serves a critical role in electrochemistry, primarily for predicting the feasibility and direction of redox reactions. This measurement is based on the concept of standard electrode potentials, which are values that indicate how likely a particular species is to be reduced (gain electrons) compared to a standard hydrogen electrode.

When electrode potentials are measured, they provide insight into the energies involved in redox reactions. A positive potential indicates that the reduction process is thermodynamically favorable, meaning the reaction can occur spontaneously. Conversely, a negative potential suggests that the reaction is not favorable under standard conditions. By comparing the electrode potentials of different half-reactions, one can determine which reaction will proceed and in what direction (i.e., which species will oxidize and which will reduce).

This understanding allows chemists and electrochemists to design and optimize reactions in batteries, fuel cells, and electrochemical sensors, effectively using electrode potentials as a predictive tool for chemical behavior.