Use the Table of Standard Reduction Potent would occur spontaneously. Justify your ans balanced equation for each reaction that occ

Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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QUESTION 5
Use the Table of Standard Reduction Potentials (Appendix D) to determine whether each of the following reactions
would occur spontaneously. Justify your answer. Assume that each reaction occurs in aqueous solution. Give a
balanced equation for each reaction that occurs.
a. Will Nitric Acid react with Silver?
b. Will Tin (II) lons react with Iron (II) lons?
(E*Red of Sn + 2e → Sn* is +0.15 V]
c. Will Iron metal react with Iron (II) ions?
d. Will Copper metal react with Copper (II) ions?
Transcribed Image Text:QUESTION 5 Use the Table of Standard Reduction Potentials (Appendix D) to determine whether each of the following reactions would occur spontaneously. Justify your answer. Assume that each reaction occurs in aqueous solution. Give a balanced equation for each reaction that occurs. a. Will Nitric Acid react with Silver? b. Will Tin (II) lons react with Iron (II) lons? (E*Red of Sn + 2e → Sn* is +0.15 V] c. Will Iron metal react with Iron (II) ions? d. Will Copper metal react with Copper (II) ions?
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