How does temperature affect electrochemical reactions?

Increasing temperature generally increases reaction rates in electrochemical reactions due to the fundamental principles of chemical kinetics. As temperature rises, the kinetic energy of the reactant molecules also increases. This elevated energy means that the molecules move more rapidly and collide with greater force, which raises the frequency and intensity of the collisions between reactants.

In electrochemical systems, such as those found in batteries or electrolytic cells, higher temperatures can also lower the activation energy barrier that must be overcome for the reaction to proceed. This results in a greater number of collisions exceeding the activation energy threshold, thereby promoting faster reaction rates.

Additionally, increasing temperature can enhance the conductivity of electrolytes, leading to improved ionic mobility. This further contributes to increased reaction rates, as ions are more effectively transported to and from the electrodes.

While the other options suggest various incorrect viewpoints, understanding that higher temperatures generally lead to increased reaction rates is fundamental to comprehending the dynamics of electrochemical processes.