Faraday Electrolysis Calculator
Mass deposited or dissolved by a current over time, with the charge passed and the moles involved.
Results
Mass
2.37099
g
Electric charge
7200.00
C
Amount of substance
0.03731137
mol
Time
1608.089
min
What this tool does
One mole of electrons carries 96 485 coulombs, and that single constant links an ammeter reading to a mass on a balance. The number of electrons comes from the half-reaction: copper from Cu²⁺ needs two, silver from Ag⁺ needs one, aluminium from Al³⁺ needs three. Real cells always fall short because some current goes into side reactions.
Formula
m = Q × M ÷ (n × F) (F = 96 485,332 12 C/mol)
Variables
| Symbol | Meaning | Unit |
|---|---|---|
i | Current | A |
tm | Time | min |
mm | Molar mass | g/mol |
nz | Electrons exchanged | — |
M | Mass | g |
Q | Electric charge | C |
NM | Amount of substance | mol |
TH | Time | min |
Worked example
- Current2 A
- Time60 min
- Molar mass63.546 g/mol
- Electrons exchanged2
- Mass2.37099 g
- Electric charge7200.00 C
- Amount of substance0.03731137 mol
- Time1608.089 min
Limitations
- For work that must comply with a standard or be signed off, check the result against the applicable code and have it reviewed by a qualified engineer.
- Electrical installations are governed by national wiring rules. Cable sizing also depends on installation method, grouping, ambient temperature and protection devices, which this calculator does not evaluate.
- The formula assumes ideal conditions: no friction losses, no air resistance and no efficiency losses unless you enter them.