Calculator Inputs
Enter the chemical amount, electrons transferred, and efficiency. The page returns ideal charge, practical charge, ampere-hours, and chart-ready output.
Plotly Graph
The graph compares ideal charge against efficiency-adjusted charge.
Result History and Export Tools
Download saved runs as CSV or PDF. Clear the list anytime.
| Saved At | Sample | Moles | e⁻/mol | Efficiency % | Ideal C | Adjusted C | Ah | kC |
|---|---|---|---|---|---|---|---|---|
| No saved runs yet. Calculate one result to populate the history table. | ||||||||
Example Data Table
These examples show how moles, electron transfer, and efficiency change the final charge requirement.
| Scenario | Moles | e⁻/mol | Efficiency % | Ideal Charge (C) | Adjusted Charge (C) |
|---|---|---|---|---|---|
| Silver Plating | 0.25 | 1 | 100 | 24,121.33 | 24,121.33 |
| Copper Deposition | 0.50 | 2 | 92 | 96,485.33 | 88,766.51 |
| Aluminum Transfer | 1.20 | 3 | 85 | 347,347.20 | 295,245.12 |
Formula Used
Ideal charge: Qideal = n × z × F
Adjusted charge: Qadjusted = Qideal × (η / 100)
Ampere-hours: Ah = Qadjusted / 3600
Electron count: e⁻ count = n × z × NA
- n is moles of substance entered into the calculator.
- z is electrons transferred per mole of substance.
- F is Faraday constant, usually 96485.33212 C/mol e⁻.
- η is current efficiency in percent.
- NA is Avogadro constant, used for electron count.
How to Use This Calculator
- Enter a sample name for easier tracking.
- Type the moles of substance involved in the reaction.
- Enter electrons transferred per mole from the balanced half-reaction.
- Set the current efficiency percentage for real process performance.
- Leave the Faraday constant at default unless your workflow requires another value.
- Choose decimal places and press Calculate Charge.
- Review the result cards, graph, and saved history table.
- Use the CSV or PDF buttons to download your output.
Frequently Asked Questions
1) What does this calculator convert?
It converts moles of reacting substance into electrical charge. The page uses electron transfer count, Faraday constant, and efficiency to estimate required coulombs for electrochemical work.
2) Why do I need electrons transferred per mole?
Charge depends on how many electrons move during the reaction. A one-electron reaction needs less charge than a two-electron or three-electron process for the same number of moles.
3) What is current efficiency?
Current efficiency measures how much supplied charge actually drives the target reaction. Side reactions lower efficiency, so practical charge often becomes smaller or less productive than the ideal value.
4) When should I keep the default Faraday constant?
Use the default in nearly all standard chemistry and electrochemistry work. Only change it when your method, teaching material, or internal standard uses a rounded or custom constant.
5) Does this work for electroplating calculations?
Yes. It is useful for electroplating, electrolysis, redox teaching, battery analysis, and charge planning. Enter correct stoichiometry and efficiency for the most meaningful estimate.
6) Why are ideal and adjusted charge different?
Ideal charge assumes perfect conversion. Adjusted charge applies the efficiency percentage, so it reflects practical operating conditions instead of a loss-free theoretical system.
7) What units does the calculator return?
It returns coulombs, kilocoulombs, ampere-hours, electron moles, and estimated electrons transferred. These outputs help compare laboratory calculations with process and equipment planning.
8) Can I save multiple runs and export them?
Yes. Each calculation is stored in the history table during the session. You can then export the saved runs as CSV or create a PDF summary.