In a galvanic cell, which component acts as the anode?

In a galvanic cell, the anode is defined as the electrode where oxidation occurs, which is typically the electrode with the lower electrochemical potential. This is because the anode is the source of electrons in the electrochemical reaction. Electrons are generated at the anode and then flow toward the cathode, where reduction occurs.

The rationale behind the anode being the electrode with the lower potential lies in the fact that a lower potential indicates a greater tendency for the electrode material to lose electrons compared to the more noble material at the cathode, which has a higher potential. In standard conditions, the flow of electrons from the anode to the cathode facilitates the movement of ions in the electrolyte, driving the galvanic reaction that produces electrical energy.

The other options present characteristics related to galvanic cells but do not identify the anode correctly. The electrode immersed in a salt bridge does not inherently indicate oxidation and is primarily used to maintain charge balance in the cell. The positive terminal of a battery signifies the location of the cathode in a galvanic setup, and it is not where oxidation takes place. The electrode with a higher potential represents the cathode, where reduction occurs and accepts the electrons generated by the anode. Thus, identifying