Battery knowledge · Electrochemistry fundamentals
Faraday’s law of electrolysis
The amount of substance transformed at an electrode is proportional to the charge passed: one mole of electrons per Faraday. It converts a material’s formula into its theoretical capacity in mAh/g. [1]
- Relationship
- m = Q·M / (n·F)
Example
Convert charge to ideal deposited mass
For a hypothetical one-electron species with molar mass 50 g/mol, transferring 1 Ah = 3600 C corresponds to about 1.87 g at 100% Faradaic efficiency. Side reactions reduce the intended deposited amount.
Explore the graph
Electron count and molar mass connect electrical charge to transformed material.
268 mAh/g for 1 electron(s) and 100 g/mol.
Q_theoretical = nF / (3.6M); m = charge × M / (nF)
Illustrative model. Assumes complete Faradaic conversion and 100% utilization. Practical reversible capacity can be lower; the material identity is not inferred from molar mass.
Use in Lemonergy
Connect reaction sites and transport paths.
This is a reference concept. No executable Lemonergy block has been verified for this term.
References & further reading
Technical references
- Quantities, Units and Symbols in Physical Chemistry, 3rd edition, 2nd printing
IUPAC · 2011
Technical reference · Physical-chemistry notation, thermodynamics, electrochemistry and transport quantities.