Simulation of working galvanic cell

Chemca.in

Interactive Electrochemistry Lab

Galvanic Cell Simulator

Watch the flow of electrons through the wire and the migration of ions in the salt bridge.

How it Works

A galvanic cell generates electrical energy from spontaneous redox reactions. The metal with the lower (more negative) standard reduction potential acts as the Anode, undergoing oxidation (losing electrons). The metal with the higher standard reduction potential acts as the Cathode, undergoing reduction (gaining electrons).

The Salt Bridge (containing $K^+$ and $NO_3^-$) maintains electrical neutrality. Anions ($NO_3^-$) flow toward the anode to balance the newly formed positive metal ions, while cations ($K^+$) flow toward the cathode to replace the positive charge of the depositing metal ions.

Cell Configuration

Left Half-Cell (Metal / $1\text{M}$ Solution) Zinc (Zn / Zn²⁺) : -0.76 V Iron (Fe / Fe²⁺) : -0.44 V Copper (Cu / Cu²⁺) : +0.34 V Silver (Ag / Ag⁺) : +0.80 V

Right Half-Cell (Metal / $1\text{M}$ Solution) Zinc (Zn / Zn²⁺) : -0.76 V Iron (Fe / Fe²⁺) : -0.44 V Copper (Cu / Cu²⁺) : +0.34 V Silver (Ag / Ag⁺) : +0.80 V

Live Chemical Data

Cell Potential ($E^\circ_{cell}$)

0.00 V

Standard state conditions (1M, 298K)

Anode (Oxidation) - Left

Select electrodes...

E° = 0.00 V

Cathode (Reduction) - Right

Select electrodes...

E° = 0.00 V

🏠 Home 📝 Quiz 📘 Revision Notes ⬇ Downloads 📚 Class Notes ▶ Video Lectures

Get new posts by email

Powered by

📚 Also Read

Lecture Notes

🧪 CHEMCA Virtual Lab

🔬 Experience Chemistry Beyond the Textbook

Explore Chemistry through interactive virtual experiments and simulations. Visualize concepts, perform experiments, understand reactions and learn Chemistry by doing—not just reading. A powerful learning resource for students, teachers and Chemistry enthusiasts worldwide.

🧪 Enter the CHEMCA Virtual Lab →