Chem208_Lecture_27_Color

Chem208_Lecture_27_Color - Zn → Zn 2 2 e – E° = 0.76...

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1 Among the participants Among the participants : : Prof. John Terry Prof. John Terry (3 (3 -3:30PM) 3:30PM) Prof. Thomas Prof. Thomas Ruttledge Ruttledge (2:30 (2:30 -3PM) 3PM) Feeling Feeling Stressed? Stressed?
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2 Today: Finish Electrochemistry (Ch. 20) - Corrosion/Rust Formation - Electrolytic Cells; Electrolysis Phase Diagrams (Ch. 12.4) Properties of Solutions (Ch. 13) - Concentration Terms (13.2) - Colligative Properties (13.6-9) PS11 can be downloaded or picked up from Room 131
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3 Corrosion of Iron Prevention Options: Both O 2 and H 2 O are necessary Fe acts as the anode, site of oxidation
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4 Use a physical barrier to separate Fe and O 2 /H 2 O - paint, grease, oil - plate with another metal (tin, zinc) Small Scale Compare tendency for oxidation half reactions Fe Fe 2+ + 2 e E° = 0.44 volt Sn Sn 2+ + 2 e E° = 0.14 volt
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Unformatted text preview: Zn → Zn 2+ + 2 e – E° = 0.76 volt Large Scale Provide a sacrificial anode 5 Electrolytic Cells Non-spontaneous chemical reactions are ‘forced’ to take place by using electrical energy eg, 2 NaCl (l) → 2 Na (l) + Cl 2 (g) Electrolysis of aqueous solution can involve the oxidation or reduction of water as well as the dissolved ions. 6 Once the products of an electrolysis reaction are known, the quantity of product formed can be calculated from the-stoichiometry of the half-reaction involved ,-the current used , and-the time of current flow. 7 Industrial Uses of Electrolysis- production of metallic Al and Mg- refining Cu (purification)- electroplating- production of F 2 , Cl 2 , and NaOH 8 The Electric Pickle...
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Chem208_Lecture_27_Color - Zn → Zn 2 2 e – E° = 0.76...

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