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. |