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Lecture%2019%20March%2026%20%28Chapter%2021%20--%20Electrochemistry%29-1

# Lecture%2019%20March%2026%20%28Chapter%2021%20--%20Electrochemistry%29-1

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Chapter 21 -- Electrochemistry Lecture 19 March 26, 2009

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What is ∆G o of the cell reaction described by the equation below? Cd (s) + 2Ag + (aq) Cd 2+ (aq) + 2Ag ( s) Standard Reduction Potential E o (V) Cd 2+ (aq) + 2e - Cd (s) -0.403 Ag + (aq) + e - Ag (s) +0.7996 F = 96485.34 C/mol, 1 Joule = C/V, ∆G o = -nFE o (A) -76.53 kJ/mol (A) +76.53 kJ/mol (A) +232.1 kJ/mol (A) -232.1 kJ/mol

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The equilibrium constant for the redox reaction shown below, at 298K, is Cd (s) + 2Ag + (aq) Cd 2+ (aq) + 2Ag ( s) Standard Reduction Potential E o (V) Cd 2+ (aq) + 2e - Cd (s) -0.403 Ag + (aq) + e - Ag (s) +0.7996 E o = (0.0592V/n)logK (A) a very small number (A) zero (A) one (A) a very large number

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Consider the following non-aqueous cell reaction 2Na (l) + FeCl 2 (s) 2NaCl (s) + Fe (s) for which E o cell = 2.35V at 200 o C. What is ∆G o at this temperature? F = 96485.34 C/mol A.453 kJ B.-453 kJ C.907 kJ D.-907 kJ

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Ow!!! Don’t chew on Aluminum Foil if you have dental fillings … electrochemistry explains why it is so painful!

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http://www.farwst.com/fwst/anodgalv/mars01.htm These bolts were submerged in salt water for 5,000 hours – notice that the unprotected iron bolt on the left has corroded, while the Zn protected bolt on the right has not.

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Lecture%2019%20March%2026%20%28Chapter%2021%20--%20Electrochemistry%29-1

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