Electrochemistry & Batteries

ELECTROCHEMISTRY & BATTERY SIMULATION

▸ Pouring ZnSO₄ + CuSO₄ solutions into 2 beakers…

▸ Dipping electrodes Zn (anode) · Cu (cathode)

▸ Installing KNO₃ salt bridge + wiring through the lamp

▸ Opening electron flow · ionization

▸ Ready — Online. ✅

Voltage & current

🔋 Zn | Zn²⁺ ‖ Cu²⁺ | Cu

E°cell = E°(cathode) − E°(anode)

Anode (oxidation)—

Cathode (reduction)—

Electromotive force—

Current—

Salt bridge—

Mode—

Note

Oxidation = loss of e (at anode); reduction = gain of e (at cathode). Electrons flow through the external wire from anode → cathode; ions swim through the solution to close the circuit. Electrolysis is the reverse: an external source forces the reaction and the electrode signs flip.

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Pick a metal pair / adjust the voltage in the right column · toggle the salt bridge · switch scenarios (cell · electrolysis · plating · corrosion) · click a concept for details

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Cell voltage sags during discharge (polarization) U dischargeE° open-circuit