What is the primary function of a galvanic (voltaic) cell?

In a galvanic (or voltaic) cell, the primary function is to generate electricity through spontaneous redox reactions. When a galvanic cell operates, it facilitates a chemical reaction in which reactants undergo oxidation and reduction. This process creates a flow of electrons due to the difference in electric potential between the anode and the cathode, enabling the cell to produce an electric current.

Electrons are released from the anode, where oxidation occurs, and travel through an external circuit to the cathode, where reduction takes place. This movement of electrons constitutes an electric current. Thus, the galvanic cell efficiently converts the chemical energy of the reactants into electrical energy.

While other options mentioned relate to aspects of electrochemistry or energy conversion, they do not capture the primary role of a galvanic cell as accurately as generating electron current using electric potential. For instance, converting electrical energy to chemical energy describes the function of an electrolytic cell, while storing chemical energy pertains to batteries rather than the direct function of galvanic cells. Balancing half-reactions is an important part of understanding redox reactions, but it is not the primary function of the cell itself.