exercise 2 - 2+ (converting to Zn ) and Fe 2+ (converting...

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Chemistry 312 Names: Exercise 2: Redox reactions and electrochemical stability Though the questions all seem to require short answers, you may wish to expand your answer to show how you derived it! 1. Balance the following redox equation, assuming it takes place in H 2 O under basic conditions. a. What is the oxidation state of nitrogen in NO 3 ? b. What is the oxidation state of nitrogen in N 2 O 4 ? c. How many electrons are involved in this reaction if you assume that one equivalent of N 2 O 4 forms? 2. a. Using the table of reduction potentials below, calculate E° for the reaction between Zn
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Unformatted text preview: 2+ (converting to Zn ) and Fe 2+ (converting to Fe 3+ ). Don’t forget the units. E° rxn = __________________ b. Would this reaction be spontaneous ? Equivalent question: Is Zn 2+ capable of oxidizing Fe 2+ ? c. Which of F 2 or F – would be capable of oxidizing Fe 2+ ? NO 3 – N 2 O 4 3. Use the standard reduction potential table and water stability (Pourbaix) diagram to answer the following questions. a. Would F 2 be stable in water at pH 7? b. Would Al 3+ be stable in water at pH 14? c. Would Al(s) reduce H + at pH 14? d. Would Mn 2+ be stable in water at pH 0?...
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This note was uploaded on 01/19/2012 for the course CHEM 312 taught by Professor Staff during the Summer '08 term at University of Washington.

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exercise 2 - 2+ (converting to Zn ) and Fe 2+ (converting...

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