Electrochemistry

40 lessons, pages 2056–2095.

  1. Electrochemical Reactions and Energy — Connecting electron transfer with electrical work
  2. Oxidation and Reduction in Cells — Assigning anodic oxidation and cathodic reduction
  3. Galvanic Cell Anatomy — Electrodes, electrolytes and external circuit
  4. Half-Cells and Electron Flow — Separating redox half-reactions in a spontaneous cell
  5. Salt Bridge and Charge Balance — Ionic migration sustaining current in a galvanic cell
  6. Cell Notation — Writing phase boundaries and cell components compactly
  7. Standard Electrode Potentials — Relative reduction potentials under specified standard conditions
  8. Standard Hydrogen Electrode — Reference half-cell and assigned zero potential
  9. Cell EMF from Reduction Potentials — Calculating cathode-minus-anode cell potential
  10. Predicting Redox Spontaneity — Using cell potential to assess reaction direction
  11. Gibbs Energy and Cell Potential — Relating electrical work to reaction free energy
  12. Equilibrium Constant from Standard EMF — Connecting E standard, Gibbs energy and K
  13. Nernst Equation Derivation — Potential dependence on reaction quotient
  14. Nernst Equation at 25 Degrees Celsius — Base-ten logarithm form and electron count
  15. Concentration Cells — Voltage produced by unequal activities of one redox couple
  16. Nonstandard Galvanic Cells — Evaluating potential from actual ion concentrations
  17. pH and Electrode Potential — Hydrogen-ion activity in electrochemical quotients
  18. Batteries and Cell Chemistry — Primary and rechargeable cells as coupled half-reactions
  19. Fuel Cells — Continuous reactant supply and electrochemical conversion
  20. Corrosion as Electrochemistry — Local anodic and cathodic regions on metals
  21. Electrochemical Series and Limitations — Using reduction-potential tables with reaction conditions
  22. Galvanic Cell Mixed Calculations — Integrating notation, stoichiometry, Q and voltage
  23. Electrolytic Cells — Driving nonspontaneous redox with external electrical energy
  24. Electrolysis of Molten Salts — Electrode products when water is absent
  25. Electrolysis of Aqueous Solutions — Competition among water and dissolved-ion reactions
  26. Faraday's Laws of Electrolysis — Product amount proportional to transferred charge
  27. Charge, Current and Time — Calculating electron moles from Q equals It
  28. Product Mass and Gas Volume — Electrolysis stoichiometry from electron count
  29. Electroplating and Industrial Electrolysis — Metal deposition and process efficiency
  30. Ionic Conductance in Solution — Charge transport by migrating cations and anions
  31. Specific Conductivity — Conductivity, resistance and cell geometry
  32. Molar Conductivity — Conductivity normalized by electrolyte amount
  33. Conductivity and Dilution — Contrasting conductivity and molar conductivity trends
  34. Kohlrausch's Law — Independent ionic contributions at infinite dilution
  35. Strong Electrolyte Conductance — Ion interactions and limiting molar conductivity
  36. Weak Electrolyte Conductance — Increased ionization on dilution
  37. Dissociation from Conductivity — Estimating weak-electrolyte ionization using limiting conductance
  38. Electrochemical Measurements and Calibration — Practical voltage and conductivity measurements
  39. Electrochemistry Misconceptions and Checks — Auditing electrode signs, electron counts and units
  40. Electrochemistry Review — Connecting cells, electrolysis, potential and conductance