Battery Builder: Galvanic & Electrolytic Cells
Connect electrodes and salt bridges to understand how batteries work and how they recharge.
About this simulation
- What
- An interactive Chemistry simulation of Battery Builder: Galvanic & Electrolytic Cells.
- Who
- Designed for AP, IB, and A‑Level Chemistry students.
- How
- Runs in any modern browser — drag, adjust, and explore in real time.
Updated 2026-01-10
Key Concepts
Galvanic Cells (Voltaic)
Spontaneous redox reactions generate electrical energy (E°cell > 0). Anode is negative, Cathode is positive.
Electrolytic Cells
External electrical energy drives non-spontaneous reactions (E°cell < 0). Anode is positive, Cathode is negative.
Standard Cell Potential
The difference between the reduction potential of the cathode and the anode (E°cell = E°cathode - E°anode).
Understanding Electrochemistry
Electrochemistry is the study of redox reactions that either generate electrical energy or are driven by an external power source. This field is foundational to modern battery technology, electroplating, and chemical sensors.
The two primary systems include Galvanic (Voltaic) cells, which utilize spontaneous chemical reactions to perform work, and Electrolytic cells, which consume external electricity to drive non-spontaneous chemical changes like electrolysis.
Through this interactive builder, you can observe real-time electron flow from the anode (oxidation) to the cathode (reduction), visualize the necessity of a salt bridge for ion migration, and calculate standard cell potentials (E°cell).
Galvanic vs Electrolytic Cells
| Feature | Galvanic Cell | Electrolytic Cell |
|---|---|---|
| Spontaneity | Spontaneous (ΔG < 0) | Non-Spontaneous (ΔG > 0) |
| Energy Conversion | Chemical → Electrical | Electrical → Chemical |
| Anode Charge | Negative (-) | Positive (+) |
| Cathode Charge | Positive (+) | Negative (-) |
Frequently Asked Questions
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