Electrolysis Calculator (Faraday's Law)
Calculate the mass of metal deposited or volume of gas produced during electrolysis using Faradays law of electrolysis.
Electric current in Amperes (A)
Time in seconds (3600s = 1 hour)
Number of electrons transferred (e.g., Cu²⁺ + 2e⁻ → Cu)
Molar mass of element in g/mol (optional - for mass calculation)
What is electrolysis?
Electrolysis uses electrical energy to drive nonspontaneous chemical reactions. In Faraday's law: m = (I·t·M) / (n·F), where m = mass deposited, I = current (A), t = time (s), M = molar mass (g/mol), n = electrons per ion, F = Faraday constant (96,485 C/mol).
What is Faraday's constant?
Faraday constant (F) = 96,485 C/mol = charge per mole of electrons. One mole of electrons has charge of 96,485 Coulombs. Used in all electrolysis calculations. 1 F deposits 1 mole of electrons, which reduces 1/n mole of n-electron ions.
How do you calculate mass deposited?
m = (I × t × M) / (n × F). For 10 A over 1 hour deposited on copper (M=63.55, n=2): m = (10 × 3600 × 63.55) / (2 × 96485) = 11.85 g. The reaction: Cu²⁺ + 2e⁻ → Cu.
What are common electrolysis applications?
Electroplating (Au, Ag, Ni), electrorefining (purifying Cu), electrolytic production of Al, Cl₂ from NaCl, water splitting to H₂ and O₂, anodizing aluminum, electroforming. All use Faraday's law to calculate efficiency.
How do you calculate volume of gas produced?
At STP (0°C, 1 atm): V = (I × t × 22.4) / (n × F) liters. At 25°C, 1 atm: V = (I × t × 24.5) / (n × F). For water electrolysis producing H₂ (n=2): 1 A for 1 hour gives ~0.45 L H₂.