1. What is Time required for Flowing of Charge given Mass and Time?

Definition: This calculator determines the time required for electrolysis based on the mass of ions reacted, the electrochemical equivalent of the element, and the electric current.

Purpose: It helps in electrochemical calculations to determine how long a current must be applied to produce or consume a certain mass of material.

2. How Does the Calculator Work?

The calculator uses Faraday's law of electrolysis:

Where:

• \( t_{tot} \) — Total time taken (seconds)
• \( m_{ion} \) — Mass of ions reacted or formed (kg)
• \( Z \) — Electrochemical equivalent of element (kg/C)
• \( i_p \) — Electric current (A)

Explanation: The mass of ions is divided by the product of the electrochemical equivalent and current to determine the required time.

3. Importance of Time Calculation in Electrolysis

Details: Accurate time calculation ensures proper control of electrochemical processes, efficient energy use, and predictable reaction outcomes.

4. Using the Calculator

Tips: Enter the mass of ions in kg, electrochemical equivalent (default 0.022 kg/C), and electric current in amps. All values must be > 0.

5. Frequently Asked Questions (FAQ)

Q1: What is electrochemical equivalent?
A: It's the mass of substance produced or consumed at an electrode per coulomb of charge passed through the electrolyte.

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 number of electrons in the reaction.

Q3: Does this account for current efficiency?
A: No, this gives theoretical time. Actual time may be longer due to side reactions and less than 100% current efficiency.

Q4: What units should I use?
A: Use consistent units - kg for mass, kg/C for electrochemical equivalent, and A for current.

Q5: Can this be used for any electrochemical reaction?
A: Yes, as long as you know the electrochemical equivalent of the substance involved in the reaction.