How does temperature influence electrochemical reaction rates?

The rate of electrochemical reactions is significantly influenced by temperature, primarily due to the impact of temperature on the kinetic energy of the reacting particles. As temperature increases, the kinetic energy of molecules also increases, leading to more frequent and more energetic collisions between reactant species. This elevated energy level enhances the probability that these collisions will overcome the activation energy barrier necessary for the reaction to proceed.

Moreover, higher temperatures can increase the solubility of reactants in electrolytes, thereby facilitating better interaction and reaction rates. This behavior is consistent with the general observation in chemistry, where most reaction rates increase with temperature, following the Arrhenius equation, which expresses the relationship between temperature and reaction rate.

In electrochemical systems, this means that reactions occurring at the electrodes in a galvanic or electrolytic cell generally proceed more quickly at elevated temperatures, enhancing the overall efficiency of the cell. Hence, the statement that higher temperatures generally increase reaction rates aligns well with the principles of thermodynamics and reaction kinetics.