Science
Galvanic cells.
Definition
An electrochemical cell that converts chemical energy into electrical energy through a spontaneous redox reaction. It consists of two half-cells connected by a salt bridge, with an anode (oxidation) and a cathode (reduction).
How it works · 5 phases
Step by step.
- Oxidation occurs at the anode, releasing electrons
- Electrons flow through an external wire from anode to cathode
- Reduction occurs at the cathode, consuming electrons
- A salt bridge maintains electrical neutrality by allowing ion flow between half-cells
- The cell produces voltage until reactants are consumed
Examples
Real-world.
- 1 A standard zinc-copper cell with Zn anode and Cu cathode
- 2 Alkaline batteries powering a flashlight
- 3 Car batteries using lead-acid galvanic cells
Key Fact
E°cell = E°cathode − E°anode; positive E°cell means spontaneous reaction