Chemistry

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Electrolysis Calculator.

Calculate deposited mass and moles from current, time, molar mass, and electron count using Faraday's law.

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Deposited mass: 2.370988 g

Deposited mass

2.370988g
Amount of substance: 0.037311 mol

Amount of substance

0.037311mol

Educational chemistry arithmetic only. Keep units consistent and verify assumptions against your laboratory or course specification.

Use Cases

Electroplating thickness estimation

Estimate the mass of metal deposited during electroplating to gauge coating thickness for a given current and time.

Example: Calculate copper mass deposited with 2 A for 30 min, Cu molar mass 63.55 g/mol, 2 e⁻.

Chemistry lab calculations

Determine theoretical yield of a product in an electrolysis experiment, useful for verifying experimental results.

Example: Find moles of silver deposited from AgNO₃ with 0.5 A for 10 min, Ag molar mass 107.87 g/mol, 1 e⁻.

Frequently Asked Questions

How does the electrolysis calculator work?
It applies Faraday's law: mass = (current × time × molar mass) / (electrons transferred × Faraday's constant). Moles are then mass divided by molar mass. You input current (A), time (s), molar mass (g/mol), and electrons transferred (e⁻).
What is Faraday's constant and why is it used?
Faraday's constant (≈96485 C/mol) represents the charge of one mole of electrons. It converts the total charge (current × time) into moles of electrons, which then relates to moles of substance via the electron count.
Can I use this calculator for any electrolysis reaction?
Yes, as long as you know the current, time, molar mass of the deposited substance, and the number of electrons transferred per ion. It works for electroplating, metal extraction, and other electrolytic processes.

Tips & Common Mistakes

Tips

  • Ensure time is in seconds; convert minutes to seconds by multiplying by 60.
  • Use the correct number of electrons transferred per ion (e.g., 2 for Cu²⁺, 1 for Ag⁺).
  • Molar mass should be in g/mol; use the atomic or molecular mass of the deposited substance.
  • Double-check units: current in amperes, time in seconds, and molar mass in g/mol for accurate results.

Common Mistakes to Avoid

  • Forgetting to convert time from minutes to seconds, leading to results off by a factor of 60.
  • Using the wrong number of electrons transferred, e.g., using 1 for Cu²⁺ instead of 2.
  • Confusing molar mass with atomic number or using the mass of the compound instead of the element deposited.

Last updated: August 13, 2026