Electrochemical Cells & Nernst Equation

The chapter gives an in-depth description of the electrochemical cells and the Nernst equation, which is the foundation of the conversion of energy in chemical systems. The chapter starts by making the difference between galvanic (voltaic) cells that produce electrical energy through spontaneous reactions and electrolytic cells that produce electrical energy through non-spontaneous reactions. It describes cell construction, electrode potentials, and the movement of electrons in redox reactions with a special focus on their importance in batteries, corrosion, and electrolysis in industry. The Nernst equation is presented to compute the potential of the cell at non-standard conditions relating the concentration, temperature and electrode potential to predict the viability of the reaction. Practical uses in metal extraction, electroplating, sensors, and energy storage devices are described, and it was noted how electrochemistry could be useful in the laboratory as well as in the industry. Other challenges that have been discussed in the chapter include the ability to keep electrolytes stable, the degradation of electrodes and energy efficiency. The combination of theoretical knowledge and practical examples enables the students to acquire a complete insight into electronic and chemical principles of cells, quantitative treatment of cell potentials, and methods of their use in the real world of chemicals and industries. This is the necessary knowledge in the fields of battery technology, corrosion engineering, electroplating industries and research in the field of energy storage.