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lecture9electrochem2

lecture9electrochem2 - Final Exam Time Location Content...

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Final Exam Time: Tuesday Dec 13, 11:15–1:45pm Location: To be announced Content: Everything Additional office hours: Thursday, Friday, Monday: Chem. Learning Center, 5pm.
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2 Oxidation and Reduction oxidation and reduction must occur simultaneously ± if an atom loses electrons another atom must take them
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Standard Reduction Potential A half-reaction with a strong tendency to be reduced has a large positive half-cell potential ± when two half-cells are connected, the electrons will flow toward that half-reaction. We cannot measure the absolute tendency of a half- reaction, we can only measure it relative to another half-reaction, i.e. relative potential/emf. We select as a standard half-reaction the reduction of H + to H 2 under standard conditions, which we assign an absolute potential = 0 V. ± standard hydrogen electrode, SHE 2H + ( aq, 1M )+2 e - H 2 ( g, 1bar ) H 2 ( g, 1bar ) 2H + ( aq, 1M )+2 e - E o = E o red = E o ox =0V
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Exercise: Sketch and Label the Voltaic Cell Fe( s ) Fe 2+ ( aq ) ⏐⏐ Pb 2+ ( aq ) Pb( s ) Write down the half-reactions and overall reaction. Determine the cell potential under standard conditions. ox: Fe( s ) Fe 2+ ( aq ) + 2 e E ° L = 0.45 V red: Pb 2+ ( aq ) + 2 e Pb( s ) E ° R = 0.13 V tot: Pb 2+ ( aq ) + Fe( s ) Fe 2+ ( aq ) + Pb( s ) E ° = + 0.32 V
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Exercise: Reaction under standard conditions Fe ( s ) + Mg 2+ ( aq ) Fe 2+ ( aq ) + Mg ( s ) Mg ( s ) + Fe 2+ ( aq ) Mg 2+ ( aq ) + Fe ( s ) ox: Mg ( s ) Mg 2+ ( aq ) + 2 e red: Fe 2+ ( aq ) + 2 e Fe ( s ) E ° = E ° R
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lecture9electrochem2 - Final Exam Time Location Content...

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