Electrochemical Cells

Galvanic cells turn a spontaneous redox reaction into electricity. Build any cell from ten half-cells, watch the Nernst equation and the discharge curve respond, then meet the batteries in your pocket and the hydrogen fuel cell — with the electrode reactions for each.

Build a galvanic cell

Half-cell 1 + Half-cell 2

Try:

The salt bridge — why it's essential

▪ Completes the circuit by letting ions flow between the half-cells (cations → cathode, anions → anode).

▪ Maintains electrical neutrality — the anode solution gains metal ions and the cathode solution loses them; the bridge balances the charge.

▪ Minimises the liquid-junction potential and stops the two solutions mixing. Made of KCl or KNO₃ in agar-agar (ions of nearly equal mobility). KNO₃ is used with Ag⁺ or Pb²⁺, which would precipitate as chlorides.

Nernst explorer — change the concentrations (298 K)

[Zn²⁺] 1 M

[Cu²⁺] 1 M

Discharge curve — what happens to E_cell as the cell runs (equal 1 L half-cells)

Primary cells — used once, not rechargeable

Secondary cells — rechargeable

Fuel cell

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