Balance Redox Equations
Voltaic Cells
Standard Potentials
Electrical Potential, Equilibrium, and Free Energy
Non Standard Conditions
Electrolytic Cells |
14.1. Assign oxidation numbers (oxidation states) to individual elements in a chemical compound or complex ion.
14.2. Recognize redox reactions; distinguish from reactions not involving oxidation/reduction.
14.3. Stoichiometrically balance both half-reactions and cell reactions involving redox.
14.4. Draw a diagram of a voltaic (galvanic, spontaneous) cell and explain how it works, predicting changes that will occur during discharge.
14.5. Define and identify anode, cathode, oxidation process, reduction process, oxidizing agent, and reducing agent for a redox reaction.
14.6. Calculate E° for a chemical reaction using a standard reduction potential table.
14.7. Predict the products of a redox reaction.
14.8. Calculate and relate values of E°, ∆G°, and K for an oxidation-reduction reaction.
14.9. Calculate E for a redox reaction under non-standard conditions of constituent concentrations and/or pressures.
14.10 Make qualitative predictions on how the Ecell will change under nonstandard conditions and provide a justification based on the direction of the reaction.
14.11. Draw a diagram of an electrolytic (non-spontaneous) cell and explain how it works, predicting changes that will occur during operation.
14.12. Construct a line notation for an electrochemical cell from information concerning the anode, cathode, oxidation process, reduction process, oxidizing agent, and/or reducing agent (v.v.).
14.13. Relate the amount of product(s) produced and/or reactant consumed in an electrolytic cell to the current used, time involved, and moles of electrons associated with the corresponding half-reaction. |