Potential

(Lecture id-1129)

TOPICS & OBJECTIVES

1010 - Standard Potential
    1010 - Know standard half reactions are written as oxidation under standard conditions (25˚C, 1M, 1atm).
    1020 - Recognize standard electrode potential (E˚) is relative (by convention SHE is zero).
    1030 - Know larger (positive) E˚ are half cells with greater potential for reduction.
    1040 - Know the potential of a cell is E˚cell = E˚cat - E˚an (using reduction potentials).
    1050 - Use standard potentials to determine cell potential.
    1060 - Use standard potential to predict if a redox reaction is spontaneous.
    1070 - Use standard potential to predict if a metal will dissolve in acid.
 
1020 - Free Energy
    1010 - Recognize concentration effects cell potential.
    1020 - Relate free energy to E˚cell, deltaG˚ = -nFE˚cell
    1030 - Relate E˚cell to K, E˚cell = ( 0.0592 / n ) log K
    1040 - Know a reaction in standard state is spontaneous if K > 1, deltaG is < 0, and deltaEcell > 0
    1050 - Use the Nernst Equation to find Ecell = E˚cell - ( 0.0592 / n ) log Q
 
1030 - Batteries & Electrolysis
    1010 - Relate current, time and extent for an electrolysis reaction.
    1020 - Desctibe the differences and advantages of dry cell, alkaline, and lead acid batteries.
    1030 - Describe how fuel cells differ from batteries.
    1040 - Know in all chemical cells oxidation occurs at the anode, reduction at the cathode.
    1050 - Understand electrolysis is driving a non-spontaneous reaction by applying external voltage.
    1060 - Use standard potential to predict which ion will be reduced or oxidized by e;ectrolysis.
    1070 - Given reaction time and current predict the stoiciometric yield of electrolysis.
 


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