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Chemistry

Faraday’s Law: Moles of Electrons

Relate electric current and time to transferred electron amount.

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Source & review

Difficulty

Beginner

Read time

3 min

Prerequisites

Basic algebra and molar quantities

Review statusNeeds review

Source

OpenStax, Chemistry 2e, §17.7

Adapted from Teng-Jui Lin’s CHEM 155 equation sheet. The linked textbook reference was used to check the equation and its physical context. Pending editorial review.

Adapted from Teng-Jui Lin, Equation Sheets, under CC BY 4.0.

FormuLab adapted notation and chemical symbols, added variable meanings, units, applicability conditions, and an original worked example.

Definition
Understanding the core concept

Charge passed at constant current is current times elapsed time. Dividing by the Faraday constant converts that charge magnitude into moles of electrons; product yield also depends on reaction stoichiometry and current efficiency.

Variables & Units
Understanding each component
SymbolMeaningUnits
Amount of electrons transferred
Magnitude of steady electric current
Elapsed time
Faraday constant: charge per mole of electrons
Real-World Applications
Where this formula is used in practice

Electrolysis charge

Convert current and elapsed time into transferred electron amount.

Electrodeposition setup

Provide the electron amount before applying product stoichiometry.

Worked Example
Step-by-step calculation with real numbers

Problem

A steady current of 2.00 A flows for 600 s. Find the amount of electrons transferred.

Given

Solution

1
2
3

Final Answer

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