Build custom electrochemical half-cells by pairing metal electrodes (Zn, Cu, Ag, Fe, Pb, Al, Mg). Observe real-time electron flow through external circuit wires, salt bridge ion migration, anode dissolution, cathode electroplating, and Nernst equation voltage shifts.
Interactive Experiment Guide
Start with fundamental scientific principles, launch the simulation, and verify mathematical predictions against real-time outcomes.
Scientific Foundation
Electrochemistry investigates the interconversion of chemical energy and electrical energy through redox (oxidation-reduction) reactions. In a Galvanic cell, spontaneous redox reactions (ΔG < 0) drive electron flow from the anode (oxidation: M → Mⁿ⁺ + ne⁻) to the cathode (reduction: Mⁿ⁺ + ne⁻ → M). In an Electrolytic cell, an external potential overrides thermodynamics to force non-spontaneous reactions (ΔG > 0).
Interactive Simulation Flow
Launch the simulation workspace, adjust parameters in real time, and observe the immediate response in the telemetry and graphical indicator loops.
Frequently Asked Questions
As electrons flow from anode to cathode, excess positive charge builds up in the anode beaker (due to Zn²⁺ generation) while excess negative charge builds up in the cathode beaker (as Cu²⁺ is consumed). The salt bridge permits spectator ions (e.g., K⁺ and Cl⁻) to migrate and maintain electrical neutrality, preventing polarization from stopping the current.