Electrolysis Calculator

All chemistry tools

Calculate the mass of a substance deposited on an electrode during electrolysis.

Electrical Parameters

Current (I)

Time (t)

Chemical Parameters

Molar Mass (M)

g/mol

Electrons Transferred (n)

Electrolysis Results

Enter parameters to see results

About this calculator

Overview

Electrolysis uses electrical energy to drive non-spontaneous redox reactions, splitting compounds into their constituent elements or depositing metals. Faraday's laws govern this process: the first law states that mass deposited is proportional to charge passed, while the second law relates mass to equivalent weight. This principle enables precise control over electrochemical processes from metal plating to hydrogen production.

💡

Pro Tips

For accurate calculations, ensure time is in seconds and current in amperes - the formula gives mass directly in grams.
The electrons transferred (n) depends on the ion charge: n=1 for Na⁺, n=2 for Cu²⁺, n=3 for Al³⁺.
Faraday's constant F = 96,485 C/mol is exact - use this value for precise calculations.
In practice, efficiency is less than 100% due to side reactions, so actual mass deposited is lower than calculated.
For gas production, use the molar volume: volume (L) = (I × t × 22.4) / (n × F) at STP.
Temperature affects conductivity - higher temperatures generally improve efficiency but may cause side reactions.
Electrode material matters: inert electrodes (platinum) allow gas evolution, while sacrificial anodes dissolve to provide metal ions.
For industrial electrolysis, current density (A/cm²) and electrolyte concentration are optimized for maximum efficiency and product purity.

Fun Facts

"Humphry Davy used electrolysis in 1807 to isolate sodium and potassium, revolutionizing chemistry by discovering reactive alkali metals."
"Michael Faraday formulated his laws of electrolysis in 1833, introducing concepts like electrochemical equivalents that became fundamental to electrochemistry."
"Aluminum was once more valuable than gold because electrolysis wasn't discovered yet - Napoleon III served his most honored guests with aluminum cutlery!"
"The chlor-alkali process produces 70 million tons of chlorine annually via electrolysis, essential for plastics, pharmaceuticals, and water treatment."
"Electrolysis produces 4% of the world's hydrogen, with green hydrogen (from renewable electricity) expected to reach 10 million tons by 2030."
"The Faraday constant (96,485 C/mol) represents the charge of one mole of electrons - it's so precise it's used to define the ampere!"
"In electroplating, a single gram of gold can be spread over 1 million square meters using electrolysis techniques."
"Electrolysis of water produces hydrogen and oxygen in a 2:1 ratio by volume, but requires about 50 kWh per kg of hydrogen - expensive but emissions-free."
"The term 'ion' was coined by Michael Faraday during his electrolysis experiments, from the Greek word for 'wanderer'."
"Hall-Héroult process (1886) uses electrolysis to extract aluminum from ore, dropping the price so much it went from a precious metal to a common one."

Formula: m = (I × t × M) / (n × F), where F = 96485 C/mol