Input parameters
Results
Enter values above and click “Calculate time” to see results.
- Required charge Q: – C
- Time: – s, – min, – h
- Moles of substance: – mol
- Moles of electrons: – mol e⁻
Calculation history and export
Store multiple scenarios, then export the table as CSV or PDF for documentation or further analysis.
| # | Current (A) | Mass (g) | Molar mass (g/mol) | z | Efficiency (%) | Charge (C) | Time (s) | Time (min) | Time (h) |
|---|
Example data table
Illustrative examples showing how electrolysis time depends on current, mass, and ionic charge number.
| Scenario | Metal | Current (A) | Mass (g) | Molar mass (g/mol) | z | Efficiency (%) | Time (s) | Time (min) | Time (h) |
|---|---|---|---|---|---|---|---|---|---|
| Example 1 | Copper plating | 2.0 | 1.0 | 63.546 | 2 | 100 | 1518 | 25.3 | 0.42 |
| Example 2 | Silver plating | 0.5 | 0.5 | 107.868 | 1 | 100 | 894 | 14.9 | 0.25 |
| Example 3 | Nickel plating | 5.0 | 2.0 | 58.933 | 2 | 100 | 1310 | 21.8 | 0.36 |
Formula used
This calculator is based on Faraday’s law of electrolysis. For a target mass m (g), molar mass M (g·mol⁻¹), ionic charge number z, current I (A) and current efficiency η (%), the required time t is:
t = (m × z × F) / (M × I × η/100)
Here, F is the Faraday constant (96,485.33 C·mol⁻¹). The term η/100 accounts for losses due to side reactions or incomplete current efficiency in real cells.
How to use this calculator
- Measure or choose the constant current you will apply to the electrolytic cell.
- Decide the mass of material you want to deposit or dissolve at the electrode.
- Enter the appropriate molar mass for the species undergoing reduction or oxidation.
- Specify the ionic charge number z (for example, 2 for Cu²⁺ or Zn²⁺).
- Optionally, enter a current efficiency if you know that side reactions occur.
- Click “Calculate time” to obtain charge, time in different units, and mole values.
- Use “Add current result to table” to build a history that can be exported as CSV or PDF.
Overview of Electrolysis Time Calculations
Electrolysis time describes how long a constant current must pass through an electrolytic cell to deposit or dissolve a specified amount of substance. This calculator automates the algebra behind Faraday’s law, saving manual calculation effort and reducing errors during routine laboratory or industrial planning.
Faraday’s Law and Charge Relationships
Faraday’s law links transferred charge with chemical change. The total charge equals current multiplied by time. That charge, divided by the Faraday constant and corrected by ionic charge, determines how many moles of substance are transformed during an electrolytic process.
Key Input Parameters for This Calculator
You provide the applied current, target mass of product or reactant, molar mass, and ionic charge number. Using these, the tool computes the required charge and corresponding time in seconds, minutes, and hours. It also reports intermediate values, helping you understand how each parameter influences timing.
Understanding the Computed Time Outputs
The primary result is the time required in seconds. For convenience, the same duration appears in minutes and hours, useful when planning long industrial runs. Comparing these values helps you quickly judge whether a chosen current is realistic for your experimental schedule and equipment limits.
Worked Example Using Typical Lab Conditions
Imagine plating a metal with a moderate current. Enter the current, desired mass, molar mass, and charge number. The calculator instantly returns charge and timing. You can store several scenarios in the results table, then export them as CSV or PDF for reporting or record keeping.
Connecting Electrolysis with Moles and Stoichiometry
Because Faraday’s law relies on moles, it pairs naturally with mole based tools. For composition problems, you might first use the Mole Fraction Calculator at https://codingace.net/chemistry/mole_fraction.html. To understand amounts more deeply, the Mole Calculator with Steps at https://codingace.net/chemistry/mole_with_steps.html complements this electrolysis time calculator.
Practical Tips for Reliable Experimental Timing
Always verify that units are consistent before trusting any calculation. Check that the electrolyte concentration, temperature, and electrode area remain stable, because these affect efficiency. Combine this calculator with careful measurements of current and mass to build reliable protocols for plating, electrorefining, or analytical electrochemical methods. Remember that theoretical time assumes one hundred percent current efficiency. Real systems often waste charge through side reactions, bubbles, or resistive heating. When possible, compare predicted times with a small pilot experiment and adjust your planned current or duration. Recording both calculated and observed values gradually improves your understanding of each cell, electrolyte, and electrode material. Over time, these refinements turn the calculator into a trusted companion for electrochemical design work.
Frequently asked questions
What units should I use for each input field?
Enter current in amperes, mass in grams, molar mass in grams per mole, and efficiency as a percentage. The calculator converts these consistently to compute charge and time.
How does current efficiency change the calculated time?
If efficiency is below one hundred percent, extra charge is required to achieve the same chemical change. The calculator increases the predicted time to reflect this loss of useful current.
Can I use this tool for gas producing electrolysis?
Yes, as long as you know the appropriate molar mass and charge number for the half reaction producing the gas. Remember that gas collection may introduce additional experimental uncertainties.
Why are results given in seconds, minutes, and hours?
Seconds give a direct connection with the fundamental definition of current. Minutes and hours are often more convenient when planning practical experiments, plating runs, or industrial electrolysis processes.
Does this calculator include concentration or cell resistance effects?
No. It assumes that the chosen current can be maintained without exceeding equipment limits. Concentration polarization and resistance affect voltage, not the time required for a given charge.
Is this calculator suitable for teaching introductory electrochemistry?
It works well in classrooms and labs because students can quickly explore how changing current, mass, or charge number affects time, reinforcing Faraday’s law with numerical experiments.