Final answer:
Electrochemical cells generate electricity from spontaneous redox reactions, with a positive cell potential indicating spontaneity. Electrolytic cells, conversely, require an external voltage to drive nonspontaneous reactions, signified by a negative cell potential. These processes underpin important industrial applications such as electrolysis and electroplating.
Step-by-step explanation:
Electrochemical and Electrolytic Cells Parameters
An electrochemical cell can either generate electricity from a spontaneous redox reaction or consume electricity to drive a nonspontaneous reaction. Spontaneous reactions in galvanic (voltaic) cells produce an electric current as a consequence of the natural flow of electrons from the reductant to the oxidant. A cell potential that is positive indicates a spontaneous reaction. In contrast, in electrolytic cells, electrical energy is required to drive a nonspontaneous redox reaction. Parameters for this process include the need for an external voltage source to induce electron flow, which overcomes the negative cell potential, signaling nonspontaneity.
Some common electrolytic processes include the electrolysis of molten sodium chloride, the electrolysis of water, and electroplating. Through the application of an external current, nonspontaneous redox reactions are pushed to proceed, which underlie important industrial processes such as metal refining and electroplating. The electric current's flow during electrolysis can be measured to allow for stoichiometric calculations, which is essential for the precise manufacturing of these products.