Galvanic vs Electrolytic Cells – AP Chemistry

Learning Objectives

Analyze the electron flow direction (Anode → Cathode).

Compare Galvanic (spontaneous, \(E_{cell} > 0\)) vs Electrolytic (non-spontaneous, \(E_{cell} < 0\)) states.

Observe the Salt Bridge maintaining electrical neutrality.

Key Equations

Standard Cell Potential:

\( E^\circ_{cell} = E^\circ_{red}(cat) - E^\circ_{red}(ano) \)

Gibbs Free Energy:

\( \Delta G^\circ = -n F E^\circ_{cell} \)

Anode vs Cathode

AN OX / RED CAT: Oxidation always occurs at the Anode (mass loss). Reduction always occurs at the Cathode (mass gain).

Tags

electrochemistrygalvanicelectrolyticAP Chemistry

Cell Potential \( E^\circ \)+1.10 V

Gibbs Free Energy \( \Delta G^\circ \)-212.3 kJ

StateSpontaneous

Electrochemical Cell Type

        Anode (Oxidation):

        Zn(s) → Zn²⁺(aq) + 2e⁻

        Cathode (Reduction):

        Cu²⁺(aq) + 2e⁻ → Cu(s)

Simulation Controls

Observe electron flow in the external circuit and ion migration in the salt bridge.