📖 Theory▼

Aim: To verify Faraday's law: the mass of substance deposited/liberated at an electrode is proportional to the charge passed.

Formula: Q = I × t | moles = Q / (n × F) where F = 96485 C/mol

Electrolyte: CuSO₄(aq) with copper electrodes | Cu²⁺ + 2e⁻ → Cu (cathode)

Parameters

0.50 A
10 min

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Results Table

I(A)t(min)Q(C)Mass(g)
No data

Run at two different currents/times — mass ÷ Q should stay constant, confirming Faraday's law.

⚠️ Safety
  • Use a low-voltage DC supply only; connect with dry hands and never bridge the electrodes to short the circuit (overheating/spark risk).
  • Copper(II) sulfate solution is harmful and irritant — avoid skin/eye contact and never taste; wash any splashes.
  • Switch off before adjusting electrodes; wires and electrodes can warm up under prolonged current.
  • Copper salts are a heavy-metal pollutant — collect spent electrolyte in the labelled waste container, do not pour down the sink.
  • Wear goggles; wash hands after handling electrodes and solutions.
CuSO₄(aq) + Anode (Cu) − Cathode (Cu) DC 0 A Q = I × t = — C Mass deposited: — g Faraday constant: F = 96485 C/mol
Calculations
Set parameters and start...