CHEM 122 11th Edition Lecture 36 Outline of Last LectureI. ElectrochemistryII. Oxidation Numbers Outline of Current Lecture I. Balancing redox reactionsII. Electrochemical cellsa. ElectrodesIII. Cell VoltageCurrent LectureBalancing Redox Reactions:1. Divide the reaction into two unbalanced half-reactionsa. Reduction for one eqution and the oxidation for the other equation2. Balance atoms other then H and O.3. Balance O by adding H2O4. Balance H by adding H+ a. Make sure now each half reaction obeys the law of conservation of mass.5. Balance te charge of each half reaction by adding electrons to the more positive side.6. Balance the number of electrons transferred in each half-reaction by multiplying by appropriate coefficents. 7. Add the two half reactions together cancelling out species that appear on apposite sides of the reaction.8. Check to see that the reaction is balanced.a. Atom and charge balanced.Electrochemical cells- Voltaic cells, galvanic cells, and batteries: known as something that use redox reactions to generate electrical energy.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.- Salt Bridge: something to nutrualize the solutions with a charge to maintain electrical balance.- Electrodes: the site for the oxidation and reduction reactionso Anode: electrodes where oxidation occurso Cathode: the electrode where reduction occurs.- Cell diagram: shorthand representation of the electrochemical cell.- Volt: the potential difference required to impart 1 J of energy to a charge of 1 coulomb (C).o Electron charge= 1.6x10^-19 C- Cell Voltage: potential difference in an electrochemical cell.- Cell potential: the difference in potential energy between the two electrode reduction
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