Advanced Charge to Moles Calculator

Calculator inputs

Use charge directly, or calculate charge from current and time.

Large screens: 3 columns · Small screens: 2 columns · Mobile: 1 column

Calculation mode

Choose the source of total electrical charge.

Substance name

Example: Copper, Silver, Chlorine, Hydrogen.

Charge value

Used when direct charge mode is selected.

Charge unit

Coulombs and battery charge units are supported.

Current value

Used directly in current × time mode.

Current unit

Supports microamps through kiloamps.

Time value

Used directly in current × time mode.

Time unit

Seconds, minutes, and hours are available.

Electrons transferred per mole, n

For Cu²⁺ → Cu, use n = 2.

Molar mass (g/mol)

Optional for mass. Use 0 if not needed.

Current efficiency (%)

Accounts for side reactions and real-world losses.

Faraday constant (C/mol)

Default is 96485.33212 C/mol.

Decimal precision

Controls result formatting in the summary table.

Example data table

These examples assume 100% efficiency and use common electrolysis relationships.

Substance	Charge (C)	n	Molar Mass (g/mol)	Moles Produced	Mass Produced (g)
Silver	4825	1	107.8682	0.0500	5.3934
Copper	9650	2	63.546	0.0500	3.1773
Aluminum	28945.6	3	26.9815	0.1000	2.6982
Chlorine	19297.1	2	70.906	0.1000	7.0906

Formula used

1. Total charge from current and time:
Q = I × t

2. Effective charge after efficiency:
Q_eff = Q × (Efficiency / 100)

3. Moles of electrons:
moles of e⁻ = Q_eff / F

4. Moles of substance formed or consumed:
moles of substance = Q_eff / (n × F)

5. Mass from moles:
mass = moles of substance × molar mass

6. Particles represented:
particles = moles of substance × N_A

Here, Q is charge in coulombs, I is current in amperes, t is time in seconds, n is the number of electrons transferred per mole, F is the Faraday constant, and N_A is Avogadro’s constant.

How to use this calculator

Select whether you want to start with direct charge or with current and time.
Enter the substance name to keep your result labels clear.
Provide the charge, or enter current and time with their units.
Enter the electron-transfer number, n, from the balanced half-reaction.
Add molar mass if you want mass output in grams.
Enter current efficiency if the process is not perfectly efficient.
Click Submit to show the result under the header and above the form.
Use the CSV and PDF buttons to export the results table.

FAQs

1) What does charge to moles conversion tell me?

It shows how much chemical substance can be produced or consumed from a known electrical charge. The conversion is central to electrolysis, plating, and electrochemical yield calculations.

2) Why do I need the electron number, n?

The value of n links charge to the chemical reaction stoichiometry. Different ions need different numbers of electrons, so n changes the moles formed for the same charge.

3) What is the Faraday constant?

The Faraday constant is the charge carried by one mole of electrons. Its accepted value is about 96485.33212 coulombs per mole of electrons.

4) Why is efficiency included?

Real electrochemical systems can waste charge through side reactions, heat, or gas evolution. Efficiency adjusts the theoretical result to a more realistic practical outcome.

5) Can I use current and time instead of charge?

Yes. The calculator can first compute charge using Q = I × t, then convert that charge into moles, mass, and particles using the same electrochemical formulas.

6) What if I do not know the molar mass?

You can still compute moles and electron quantities without molar mass. Mass output only becomes meaningful after you enter a valid molar mass in g/mol.

7) Is this calculator useful for electroplating?

Yes. It is useful for electroplating because deposited mass depends directly on charge, electron transfer number, and molar mass of the plated material.

8) Does this calculator replace a balanced reaction?

No. You still need the correct half-reaction or balanced electrochemical equation to choose n properly. A wrong n gives the wrong chemical yield.