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Iron(II) ion undergoes a disproportionation reaction to give Fe(s) and the iron(III) ion. That is, iron(II) ion is both oxidized and reduced within the same reaction. 3 Fe 2+ (aq) ⇄ Fe(s) + 2 Fe 3+ (aq) (a) What two half-reactions make up the disproportionation reaction? (b) Use the values of the standard reduction potentials for the two half-reactions in part (a) to determine whether this disproportionation reaction is product-favored at equilibrium. (c) What is the equilibrium constant for this reaction?

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Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781337399074
BuyFind

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781337399074

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Chapter
Section
Chapter 19, Problem 99GQ
Textbook Problem

Iron(II) ion undergoes a disproportionation reaction to give Fe(s) and the iron(III) ion. That is, iron(II) ion is both oxidized and reduced within the same reaction.

3 Fe2+(aq) ⇄ Fe(s) + 2 Fe3+(aq)

  1. (a) What two half-reactions make up the disproportionation reaction?
  2. (b) Use the values of the standard reduction potentials for the two half-reactions in part (a) to determine whether this disproportionation reaction is product-favored at equilibrium.
  3. (c) What is the equilibrium constant for this reaction?

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Chapter 19 Solutions

Chemistry & Chemical Reactivity
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