Electrochemistry · Galvanic Cell

Galvanic Cell & EMF

Two metals in their salt solutions, wired together. The metal that wants electrons less — the lower standard potential — gives them up at the anode; they travel the wire to the cathode where reduction happens. The salt bridge carries ions to keep both sides neutral. The cell voltage is simply E°cathode − E°anode.

● electrons (through wire) ● cations → ● anions → salt bridge keeps each half-cell neutral

Electrodes

The lower-potential metal becomes the anode automatically.

1.10 V
cell EMF = E°cat − E°an
Anode (oxidation, −)
Zn → Zn²⁺ + 2e⁻
Cathode (reduction, +)
Cu²⁺ + 2e⁻ → Cu
Overall
Zn + Cu²⁺ → Zn²⁺ + Cu
Cell notation: Zn│Zn²⁺ ‖ Cu²⁺│Cu

Try this

Swap the metals between left and right — the physics doesn't care about position, so the anode/cathode labels follow the metal, not the beaker, and the EMF is unchanged. Pick two metals close in the series (Fe & Ni) for a weak cell, or Mg & Ag — the widest gap here — for the strongest voltage.