1. What is Mass of Substance undergoing Electrolysis?

Definition: This calculator determines the mass of ions reacted or formed during electrolysis based on the electrochemical equivalent, current, and time.

Purpose: It helps in electrochemistry calculations to determine the amount of substance deposited or dissolved during electrolysis.

2. How Does the Calculator Work?

The calculator uses Faraday's first law of electrolysis:

Where:

• \( m_{ion} \) — Mass of ions (kilograms)
• \( Z \) — Electrochemical equivalent of element (kg/C)
• \( I \) — Current (amperes)
• \( t \) — Time (seconds)

Explanation: The mass of substance deposited or dissolved during electrolysis is directly proportional to the quantity of electricity passed through the electrolyte.

3. Importance of Electrolysis Calculations

Details: Accurate mass calculations are crucial in electroplating, metal refining, battery technology, and chemical production.

4. Using the Calculator

Tips: Enter the electrochemical equivalent (default 0.000022 kg/C for copper), current in amperes, and time in seconds. All values must be > 0.

5. Frequently Asked Questions (FAQ)

Q1: What is electrochemical equivalent?
A: It's the mass of substance deposited or dissolved per unit charge (typically in kg/C or g/C).

Q2: How do I find the electrochemical equivalent?
A: It can be calculated as molar mass divided by (n × Faraday constant), where n is the charge number.

Q3: What's a typical value for Z?
A: For copper (Cu²⁺), Z ≈ 0.000022 kg/C; for silver (Ag⁺), Z ≈ 0.000001118 kg/C.

Q4: Does this account for current efficiency?
A: No, this gives theoretical maximum. Actual mass may be less due to side reactions.

Q5: Can I use this for gases produced in electrolysis?
A: Yes, but you'll need to convert mass to volume using the gas's molar mass and density.