What is the difference between a galvanic cell and an electrolytic cell?

A galvanic cell converts spontaneous chemical energy to electrical energy (delta-G less than 0). An electrolytic cell uses external electrical energy to force a non-spontaneous reaction (delta-G greater than 0). Rechargeable batteries do both depending on discharge or charge mode.

What is a salt bridge and why is it necessary?

A salt bridge connects the two half-cells and maintains electrical neutrality by allowing ions to migrate between them. Without a salt bridge, charge imbalance would quickly stop current flow.

How does the Nernst equation affect cell voltage?

The Nernst equation shows cell voltage depends on reactant and product concentrations. As the cell discharges and Q approaches K (equilibrium constant), voltage decreases toward zero.

Home▸Chemistry & Materials▸Galvanic Cell

⚡ Galvanic Cell

Simulate a galvanic (voltaic) cell: watch electron flow, ion migration in the electrolyte, and electrode reactions. Calculate cell voltage using the Nernst equation with different metal pairs.

Chemistry & Materials3DEasy60 FPS⚡ Plasma

⚙ Under the hood

Pick two electrodes and their ion concentrations to build a Daniell-type cell, then read the Nernst-corrected voltage and Gibbs free energy.

galvanic cellvoltaic cellDaniell cellNernst equationelectrode potentialredox reactionsalt bridgeelectrochemistrycell voltageGibbs free energy

3D · Three.js / WebGL renderer · 60 FPS target · runs fully client-side, no install