Electrochemical Equivalent Calculator
Calculate electrochemical equivalent and mass deposited during electrolysis
Electrolysis Parameters
Enter current, time, molar mass, and valency. Use presets for common metals.
Electrolysis Properties
Faraday's Law
Mass deposited is proportional to charge passed.
Electron Transfer
Higher valency means more electrons per ion.
Equivalent Mass
Z = M / n
Electrochemical Equivalent Formula
Z = M / n, m = (I × t × Z) / F
Where: Z = electrochemical equivalent (g/C), M = molar mass (g/mol), n = valency, I = current (A), t = time (s), F = Faraday's constant (96485 C/mol)
Equivalent Mass
Mass per coulomb of charge
Faraday's Constant
96485 C/mol of electrons
Applications
Electroplating, batteries, analysis
Electrochemical Equivalent Calculator – Calculate Mass Deposition in Electrolysis
Electrochemical equivalent is a fundamental concept in electrochemistry that quantifies the mass of substance deposited or liberated per unit charge during electrolysis. Based on Faraday's laws, our calculator determines the electrochemical equivalent from molar mass and valency, and computes the mass deposited given current and time. Essential for electroplating, battery design, and quantitative electrochemical analysis.
🔹 What is Electrochemical Equivalent?
The electrochemical equivalent (Z) is the mass of a substance that is deposited or liberated at an electrode when one coulomb of electric charge passes through the electrolyte.
It depends on the molar mass and the number of electrons transferred (valency) in the electrochemical reaction.
Units: grams per coulomb (g/C). Used to predict mass changes in electrolysis processes.
Based on Faraday's first law: mass deposited is proportional to charge passed.
🔹 Electrochemical Equivalent Formula
The electrochemical equivalent is calculated as:
Z = M / n Where: Z = Electrochemical equivalent (g/C) M = Molar mass (g/mol) n = Valency (electrons per ion) Mass Deposited: m = (I × t × Z) / F Where: m = Mass deposited (g) I = Current (A) t = Time (s) F = Faraday's constant (96485 C/mol)
🔹 Features of Our Electrochemical Equivalent Calculator
- Calculate electrochemical equivalent from molar mass and valency
- Compute mass deposited based on current, time, and equivalent
- Uses accurate Faraday's constant (96485 C/mol)
- Quick presets for common metals like copper, silver, and zinc
- Step-by-step calculation breakdown for educational purposes
- Mobile-friendly interface for laboratory and field use
🔹 Example Calculations
Example 1: Copper Electroplating
Molar Mass (M) = 63.5 g/mol
Valency (n) = 2
Z = 63.5 / 2 = 31.75 g/C
Current (I) = 1 A, Time (t) = 3600 s (1 hour)
m = (1 × 3600 × 31.75) / 96485 = 114300 / 96485 ≈ 1.185 g
👉 Mass deposited = 1.185 g of copper
Example 2: Silver Deposition from Solution
Molar Mass (M) = 107.9 g/mol
Valency (n) = 1
Z = 107.9 / 1 = 107.9 g/C
Current (I) = 0.5 A, Time (t) = 1800 s (30 minutes)
m = (0.5 × 1800 × 107.9) / 96485 = 48705 / 96485 ≈ 0.505 g
👉 Mass deposited = 0.505 g of silver
🔹 Applications of Electrochemical Equivalent
- 🏭 Electroplating Industry – Precise control of metal coating thickness on surfaces
- 🔋 Battery Technology – Determining capacity and efficiency of rechargeable batteries
- 🧪 Analytical Chemistry – Quantitative analysis through coulometric titrations
- ⚡ Metal Extraction – Calculating yields in electrolytic refining processes
- 🔬 Research Laboratories – Studying reaction mechanisms and electron transfer
🔹 Frequently Asked Questions (FAQs)
Q1. What is Faraday's constant and why is it important?
Faraday's constant (F = 96485 C/mol) represents the charge of one mole of electrons. It's crucial because it links electrical charge to chemical amount in electrochemical reactions.
Q2. How does valency affect the electrochemical equivalent?
Higher valency means more electrons are transferred per ion, reducing the electrochemical equivalent since Z = M/n. For example, copper (n=2) has lower equivalent than silver (n=1).
Q3. Is the calculated mass always accurate in real electrolysis?
In ideal conditions, yes. However, real processes may have inefficiencies due to overpotentials, side reactions, or incomplete current efficiency, leading to slightly different actual masses.
Q4. What units are commonly used for electrochemical equivalent?
The SI unit is grams per coulomb (g/C). In some contexts, milligrams per coulomb (mg/C) or even micrograms per coulomb (µg/C) are used for very small equivalents.
Academic & Scientific References
For further understanding and validation of the formulas used above, we recommend exploring these authoritative resources: