Electrochemistry by the Numbers: Faraday's Laws, Plating Mass & Thickness, Current Efficiency, Cell Potentials, the Nernst Equation & Battery Capacity
Connect current, charge and chemistry. You will turn amperes and minutes into coulombs and moles, compute the mass and thickness of a plated layer, include current efficiency, plan plating times, read cell potentials from a table, adjust them with the Nernst equation and relate battery capacity in ampere-hours to the chemistry inside, with every cell checked as you go.
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About this course
This course turns electrochemistry into formulas you build yourself. You convert current and time into coulombs, ampere-hours and moles of electrons, then apply Faraday's first law to find the mass of metal a plating job deposits. You turn masses into layer thicknesses in micrometres, compare weighed deposits with theory to get the current efficiency and plan the plating time for a target layer. A fictional job sheet adds racks, rack current and metal use. Finally you compute cell voltages from a table of standard reduction potentials, correct them with the Nernst equation and work out the theoretical capacity of battery materials in mAh per gram.
Lessons
- Charge: Q = I × t, Coulombs vs Ampere-Hours and the Faraday Constant Pro
- Faraday's First Law: From Charge to Moles and Grams of Deposited Metal Pro
- Plating Thickness: Mass ÷ (Density × Area), Micrometres and µm per Hour Pro
- Current Efficiency: Actual vs Theoretical Mass and the Time for a Target Thickness Pro
- Plating Jobs: Parts per Rack, Rack Current, Plating Time and Metal Used Pro
- Cell Potentials: Standard Reduction Potentials, E_cell = E_cathode − E_anode and Spontaneity Pro
- The Nernst Equation: Concentration Effects, Concentration Cells and Temperature Pro
- Battery Capacity: Ampere-Hours, Coulombs and Moles of Active Material Pro