Anode and cathode
Oxidation occurs at the anode and reduction at the cathode. In a spontaneous galvanic cell, electrons move through the external circuit from anode to cathode.
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This model demonstrates how oxidation and reduction are coupled in an electrochemical cell. Change half-cells, concentration, and temperature to explore a simplified cell-potential calculation.
Oxidation occurs at the anode and reduction at the cathode. In a spontaneous galvanic cell, electrons move through the external circuit from anode to cathode.
Using reduction potentials, E°cell = E°cathode − E°anode. A positive E°cell indicates a favorable reaction under standard conditions.
E = E° − (RT/nF) ln Q. R is the gas constant, T absolute temperature, F Faraday’s constant, and Q the reaction quotient.
For a reversible cell, ΔG = −nFE. Under standard conditions, ΔG° = −nFE°.
Real cells can include non-ideal activities, resistance, junction potentials, and electrode kinetics; this simulation is intentionally simplified.
This is an educational model, not a substitute for supervised laboratory procedures.