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🔋 Electrochemistry Lab

🔋 Electrochemistry Lab

Results

E° (standard): +1.100 V
E (Nernst): +1.100 V
Q = [Zn²⁺]/[Cu²⁺] = 1.000
ΔG = -212.27 kJ/mol
✓ Spontaneous reaction

Nernst Equation

E = E° - (RT/nF) × ln(Q)
E = 1.100 - (8.314×298)/(2×96485) × ln(1.000)
E = 1.100 V

Electrochemistry Lab – Galvanic Cells & Nernst Equation

Electrochemistry connects chemical reactions to electrical energy through electron transfer between oxidized and reduced species. This lab simulator lets you assemble galvanic cells from half-reactions, measure standard reduction potentials, apply the Nernst equation under non-standard conditions, and drive electrolytic reactions like metal plating.

What you can do in this simulation

  • Choose two half-cells from a reduction potential table and assemble a galvanic cell
  • Calculate cell potential (E°cell) from reduction potentials and verify spontaneity via ΔG = -nFE
  • Apply the Nernst equation to see how ion concentration shifts cell voltage
  • Switch to electrolytic mode, set applied voltage, and observe metal deposition reactions
  • Identify anode and cathode processes and track electron flow in the external circuit

Concepts covered

standard reduction potential · Nernst equation · galvanic cell · electrolysis · Faraday's laws · oxidation-reduction

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