Electrochemical Equivalent Calculator Using Faraday's Laws of Electrolysis

Faraday's Laws of Electrolysis

Faraday's Laws of Electrolysis (1833) quantify the relationship between electrical charge passed and the amount of substance deposited or dissolved at an electrode. These laws underpin electroplating, aluminum production, rechargeable batteries, and electrochemical sensors.

⚗️ Electrochemical Equivalent Calculator

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📐 Formula

m = ZIt = (M/nF) × Q

m = mass deposited (g), Z = electrochemical equivalent (g/C), I = current (A), t = time (s), M = molar mass, n = valence electrons, F = Faraday constant (96,485 C/mol).

📝 Worked Example

Deposit copper (M=63.5, n=2) with I=2A for t=3600s:
Q = It = 7200 C
m = (63.5/2×96485) × 7200 = 2.37 g of Cu

📝 How to Use

Select ElementChoose metal from preset list (Cu, Ag, Au, Zn, Ni) or enter molar mass.

Enter Current and TimeCurrent in Amperes, time in seconds or hours.

Calculate MassView grams of metal deposited or dissolved.

Calculate ChargeView total charge passed in Coulombs.

❓ FAQ

What is the Faraday constant?

F = 96,485 C/mol — the charge of one mole of electrons. It connects electrical units to chemical amounts.

Why is aluminum produced by electrolysis and not smelting?

Aluminum's high reactivity means standard smelting doesn't work. Electrolysis of molten Al₂O₃ (Hall-Héroult Process) is required, consuming massive electricity (≈15 kWh/kg Al).

Faraday's Laws of Electrolysis