Galvanic Cell — Interactive Simulation

Choose the anode and cathode. The reduction potentials determine whether a spontaneous current flows.

Anode (oxidation)

Cathode (reduction)

Select the electrodes and press Run Cell.

Now that current is flowing, choose what you want to investigate:

Standard hydrogen electrode (SHE): H₂(g) at 1 atm in 1 M H⁺, E°(H⁺/H₂) = 0.00 V.

E°cell

—

E_ext

0.00 V

Net current

100%

E_ext = E°cell → NET CURRENT = 0

The galvanic action is exactly balanced. Crossing this point drives the reaction in reverse.

⚡ E_ext > E°cell — ELECTROLYSIS

External voltage is now stronger than the cell voltage.

ANODE

—

OXIDATION

FORCED
REACTION

CATHODE

—

REDUCTION

Galvanic cell reactions

Oxidation half-cell: Zn → Zn²⁺ + 2e⁻ | E°red(Zn²⁺/Zn) = −0.76 V

Reduction half-cell: Cu²⁺ + 2e⁻ → Cu | E°red(Cu²⁺/Cu) = +0.34 V

Overall cell: Zn + Cu²⁺ → Zn²⁺ + Cu | E°cell = +1.10 V

Cell potential

E°cell = —

Anode E°red

—

Cathode E°red

—

E°cell

—

Current?

—

What is happening?

Choose an anode and cathode, then run the cell.

E°cell = E°red(cathode) − E°red(anode).

The electron and current directions will be shown when the cell is spontaneous.

Salt bridge (KNO₃): NO₃⁻ moves toward the anode and K⁺ toward the cathode to maintain electrical neutrality.

Note: E° values are standard reduction potentials. Solution colours are intentionally enhanced for visual clarity; actual solution colour depends on ion and concentration.