1. What is Electrochemical Equivalent?

Definition: The electrochemical equivalent of an element is the mass of that element (in kilograms) transported by 1 coulomb of electric charge during electrolysis.

Purpose: This calculation is essential in electrochemistry for determining how much substance will be deposited or dissolved during electrolysis.

2. How Does the Calculator Work?

The calculator uses the formula:

Where:

• \( Z \) — Electrochemical equivalent (kg/C)
• \( m_{ion} \) — Mass of ions reacted or formed (kg)
• \( C_{tran} \) — Electric charge transferred through circuit (C)

Explanation: The mass of ions is divided by the total charge transferred to determine how much mass is transported per unit charge.

3. Importance of Electrochemical Equivalent

Details: This value is crucial for designing electrochemical cells, calculating deposition rates in electroplating, and understanding Faraday's laws of electrolysis.

4. Using the Calculator

Tips: Enter the mass of ions in kilograms and the electric charge transferred in coulombs. Both values must be positive numbers.

5. Frequently Asked Questions (FAQ)

Q1: What units should I use for the inputs?
A: Mass should be in kilograms (kg) and charge in coulombs (C) for the result to be in kg/C.

Q2: How precise should my measurements be?
A: For accurate results, measure mass to at least 4 decimal places (milligrams) and charge to 2 decimal places.

Q3: What's a typical value for electrochemical equivalent?
A: Values vary by element. For example, silver is about 1.118 × 10⁻⁶ kg/C, while copper is about 3.29 × 10⁻⁷ kg/C.

Q4: How does this relate to Faraday's constant?
A: Electrochemical equivalent (Z) is related to molar mass (M) and Faraday's constant (F) by Z = M/(nF), where n is the charge number.

Q5: Can I use this for compounds?
A: Yes, but the equivalent will be for the compound as a whole, not individual elements.