Faraday's First Law: From Charge to Moles and Grams of Deposited Metal
This lesson is part of the course
In this lesson
You calculate how many moles and grams of metal five fictional plating jobs deposit, using a teaching table of molar masses and ion charges, and find the copper equivalent per ampere-hour.
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Lessons in this course
- Charge: Q = I × t, Coulombs vs Ampere-Hours and the Faraday Constant Locked
- Faraday's First Law: From Charge to Moles and Grams of Deposited Metal Locked
- Plating Thickness: Mass ÷ (Density × Area), Micrometres and µm per Hour Locked
- Current Efficiency: Actual vs Theoretical Mass and the Time for a Target Thickness Locked
- Plating Jobs: Parts per Rack, Rack Current, Plating Time and Metal Used Locked
- Cell Potentials: Standard Reduction Potentials, E_cell = E_cathode − E_anode and Spontaneity Locked
- The Nernst Equation: Concentration Effects, Concentration Cells and Temperature Locked
- Battery Capacity: Ampere-Hours, Coulombs and Moles of Active Material Locked