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.

(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?

Transcribed Image Text:

3 Fe²+ (aq) = Fe(s) + 2 Fe³+ (aq)