CHEM 102 1nd Edition Lecture 33Outline of Last Lecture I. ElectrochemistryII. Molar Solubility ExampleIII. Precipitation ExampleIV. DemoV. Single Displacement ReactionVI. Oxidation NumbersVII. Largest Oxidation Number ExampleVIII. Oxidation and ReductionOutline of Current Lecture I. Calculate E° of a CellII. Cell PotentialIII. Is Redox Reaction SpontaneousIV. Voltaic Cell DiagramCurrent LectureI. Calculate E° of a Cell- Half reactions are added to give an overall reaction, potentials can be added to give overall cell potential- If half reaction is reversed, the sign is reversed- If half reaction is multiplied, then potential stays the sameII. Cell Potential- E° Cell is the cell under the standard conditions- Magnitude of cell potential is the measure of spontaneity of a redox reaction- More positive the cell potential, the greater the driving force for the redox reaction as written- More positive E° is the cathode- More negative E° is the anodeIII. Is Redox Reaction Spontaneous- More positive E° stays the same- More negative E° has its sign reversed- Balance the electrons- Add the two E° together.These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.- If the E° of the cell s > 0, the reaction is spontaneousIV. Voltaic Cell Diagram- If presented with the reaction: Zn + Cu2+ Zn2+ + Cu- It can be represented as Zn|Zn2+ (1.0m) || Cu2+(1.0M)|Cu The Zn will be oxidized because it will lose e- Cu will be reduced because it will gain e- Zn electrode loses weight Cu electrode gains
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