Question

Fe(OH)3 > Fe2O3 > Fe > FeSO4 > Fe(OH)2 > FeO > Fe

Answer 1

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Answer 2

This sequence appears to represent the decreasing order of the standard reduction potentials (E°) for different oxidation states of iron (Fe) in aqueous solutions at standard conditions (25°C, 1 atm, pH 7).

The more positive the standard reduction potential, the stronger the tendency of the species to gain electrons and reduce (i.e., undergo reduction reaction), whereas the more negative the E°, the stronger the tendency to lose electrons and oxidize (i.e., undergo oxidation reaction).

The sequence implies that Fe(OH)3 has the highest E° among the listed species, and thus is the most easily reduced. In contrast, Fe has the lowest E°, indicating that it is the least easily reduced and most easily oxidized. The other species fall in between, with Fe2O3 having a higher E° than Fe, FeSO4 having a higher E° than Fe(OH)2 and FeO, etc.

It is worth noting that the sequence may not be valid for non-standard conditions or in the presence of other redox-active species. Also, the thermodynamic tendency to undergo reduction does not necessarily reflect the kinetic rate of the reaction or its feasibility under different conditions.