Consider the two following half reactions:
Fe(OH)3(s) + 3H3O+ + e- <-> Fe2+(aq)+ 6H2O EoH= 1.06 V; peo= 17.9
NO3-(aq) + 10H3O+ + 8e- <-> NH4+(aq)+ 13H2O EoH= 0.88V; peo= 14.9
(a)Which reaction would you expect to be the oxidation and which the reduction under standard conditions?
(b)Write the full balanced reaction.Show your work.
(c)Assuming that the concentrations ofFe2+(aq), NH4+(aq), and NO3-(aq) are all 10-5M and pH 7, calculate the pE for the redox reaction in (b).
(d)Comment on what the calculated pE in (c) tells you about the environment in which this reaction is occurring.
a)
NO3- reaction will go for oxidation and Fe(OH)3 will go for reduction under standard conditions based on provided values of reduction potentials.
b)
Adding above two equations,
Consider the two following half reactions: Fe(OH)3(s) + 3H3O+ + e- <-> Fe2+(aq)+ 6H2O EoH= 1.06...
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