Cell Potentials: Standard Reduction Potentials, E_cell = E_cathode − E_anode and Spontaneity
This lesson is part of the course
In this lesson
You read standard reduction potentials from a teaching table, compute the voltage of six cells, decide which ones run on their own and convert the voltage into the free energy ΔG = −nFE.
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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