Electrochemistry laboratory
Build cells, apply the Nernst equation and calculate electrolysis products from charge.
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Explanation mode
Anode: Zn²⁺/Zn
e⁻ → external circuit
Salt bridge
Cathode: Cu²⁺/Cu
Description of this simulation
Zn²⁺/Zn is oxidized and Cu²⁺/Cu is reduced; the calculated cell potential is 1.103 V.
Quick test · 3 questions
- E°cell
- 1.103 V
- Ecell
- 1.103 V
- Electrons transferred
- 2
- Spontaneous as written?
- Yes
Learning guide
- Learning objective
- Identify electrodes and electron flow, predict voltage, and connect charge to chemical amount.
- Core equation
- E°cell=E°cathode−E°anode; E=E°−RT lnQ/(nF); m=ItM/(nF)
- Why the result changes
- Voltage depends on the difference between half-cell potentials and on composition; electrolysis product depends on total charge and electron stoichiometry.
- Try this challenge
- Reverse the two half-cells and explain why the sign of the cell potential reverses.
- Sources
- IUPAC Gold Book; CODATA 2022; CRC Handbook
What this model shows — and what it simplifies
Educational ModelReduction potentials, the Nernst equation and electron stoichiometry are kept explicit so electrode labels follow the chemistry.
Where do we see this in real life?
Electrochemistry powers batteries, corrosion protection, electroplating and metal refining.
Explain this result
Scientific review record
Building- Module version
- v1 bundled
- Published
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- Last reviewed
- Not yet verified
- Academic level
- School
- Reviewer
- Not publicly assigned
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