A galvanic cell converts:

Chemical energy to electrical energy

The correct answer is option 2.Chemical energy to electrical energy.

A galvanic cell is an electrochemical cell that converts chemical energy into electrical energy through spontaneous redox reactions. These cells are commonly used in batteries to provide electrical power for various devices. In a galvanic cell, chemical energy stored in the reactants is converted into electrical energy during the course of redox reactions. This conversion occurs through the transfer of electrons from the reactants in the oxidation half-reaction (anode) to the products in the reduction half-reaction (cathode).

The operation of a galvanic cell relies on two half-reactions occurring at the anode and cathode. At the anode, oxidation takes place, resulting in the loss of electrons by the oxidized species (oxidation half-reaction). At the cathode, reduction occurs, leading to the gain of electrons by the reduced species (reduction half-reaction).

The transfer of electrons from the anode to the cathode creates an electric current in the external circuit connected to the galvanic cell. This flow of electrons constitutes the conversion of chemical energy into electrical energy, which can then be utilized to power external devices connected to the cell.

For example, in a standard zinc-copper galvanic cell, zinc metal undergoes oxidation at the anode (loses electrons to form \(Zn^{2+}\) ions), while copper ions (\(Cu^{2+}\)) are reduced at the cathode to form copper metal. The flow of electrons from zinc to copper through the external circuit generates electrical energy that can be harnessed for practical applications.

In summary, a galvanic cell converts chemical energy stored in reactants into electrical energy through redox reactions occurring at the electrodes, allowing for the generation of electric current that can be used to power electronic devices. Therefore, the correct statement is "Chemical energy to electrical energy."