Calculate mass deposited, current required, time, and energy consumption for electrolysis using Faraday's laws with common plating and industrial applications.
Electrolysis is the process of using electrical energy to drive a non-spontaneous chemical reaction, typically the reduction of metal ions at a cathode or the oxidation of species at an anode. Faraday's laws of electrolysis quantify the relationship between the amount of substance produced and the electrical charge passed through the electrolyte.
Faraday's first law states that the mass of substance deposited is directly proportional to the charge passed (Q = I × t). The second law relates the mass to the molar mass and the number of electrons transferred per ion: m = (M × I × t) / (n × F), where F is Faraday's constant (96,485 C/mol). These laws are fundamental to electroplating, electro-refining, chlor-alkali processes, and water splitting.
This calculator handles common industrial and laboratory electrolysis scenarios — from copper electroplating to aluminum smelting to hydrogen production. It accounts for current efficiency (real processes are never 100% efficient), calculates energy costs, and provides reference data for standard electrode potentials and electroplating parameters.
This calculator instantly computes mass deposited, charge required, and energy costs for any electrolysis scenario — saving time for students, plating shop operators, and process engineers who need to plan and verify electrochemical processes. This electrolysis calculator helps you compare outcomes quickly and reduce avoidable mistakes when making day-to-day care decisions. Use the estimate as a planning baseline and confirm final decisions with a qualified professional when risk is high.
Faraday's Law: m = (M × I × t) / (n × F), where m = mass deposited (g), M = molar mass (g/mol), I = current (A), t = time (s), n = electrons transferred per ion, F = 96,485 C/mol. Energy = V × I × t (joules).
Result: Mass = 5.95 g Cu deposited
For copper (M = 63.55, n = 2) at 5 A for 1 hour: Q = 5 × 3600 = 18,000 C. Theoretical mass = (63.55 × 18,000) / (2 × 96,485) = 5.93 g. At 95% efficiency: 5.63 g.
Michael Faraday established these quantitative laws in 1833, providing the first precise connection between electricity and chemistry. The first law says that the mass of substance altered at an electrode is proportional to the quantity of electricity passed. The second law says that for the same charge, the masses of different substances produced are proportional to their equivalent weights (molar mass divided by the number of electrons). Together, these laws enable precise prediction of electrolysis outcomes.
The chlor-alkali industry electrolyzes brine (NaCl solution) to produce chlorine gas, hydrogen gas, and sodium hydroxide — three of the top 10 industrial chemicals by volume. Aluminum production via the Hall-Héroult process consumes about 5% of all electricity generated in the US. Water electrolysis using renewable electricity is a key technology for green hydrogen production in the energy transition.
Electroplating deposits a thin metal layer onto a substrate for corrosion protection, aesthetics, or functional properties (hardness, conductivity). The quality of the deposit depends on current density, bath chemistry, temperature, and agitation. Decorative chrome plating uses chromic acid baths with n = 6 (Cr⁶⁺ → Cr⁰), making it one of the least efficient common plating processes.
F = 96,485 C/mol, the charge of one mole of electrons. It connects electrical measurements to chemical amounts in any electrochemical calculation.
The ratio of actual product mass to theoretical mass. Losses occur from side reactions (H₂ evolution during metal plating), electrical resistance, and ion migration. Industrial Cu plating achieves 95-98%.
From the half-reaction: Cu²⁺ + 2e⁻ → Cu has n = 2; Ag⁺ + e⁻ → Ag has n = 1; Al³⁺ + 3e⁻ → Al has n = 3. The charge on the ion tells you n.
Minimum voltage equals the decomposition potential (from electrode potentials). Real cells need additional overpotential (0.5-2V extra) to overcome kinetic barriers and IR drop.
Major applications: aluminum smelting (Hall-Héroult), chlor-alkali (NaCl → Cl₂ + NaOH), copper refining, zinc electrowinning, electroplating, and water electrolysis for hydrogen fuel. This keeps planning practical and lowers the chance of preventable errors.
Yes: Energy (kWh) = V × I × t / 3,600,000. Multiply by your electricity rate ($/kWh) for the cost.