When we look at the fate of metals in the environment, the solubility of the met

Question

When we look at the fate of metals in the environment, the solubility of the metal often depends on it’s valence. Consider Fe2+ and Fe3+. Calculate and compare the activity of aqueous iron in equilibrium with each mineral at pH 7 for FeO (wustite forming Fe2+(aq) ) and Fe2O3 (hematite- forming Fe3+ (aq)). Hint: No exchange of e- is occurring in either reaction.

Here are the reactants and products you need to balance for the wustite reaction to get you started. FeO + H+ Fe2+ + H2O

Would you expect to find more iron in solution under oxidizing or reduced conditions? Write a balanced redox reaction showing the transformation of FeO to Fe2O3.

Really just need help with balanced redox equation for FeO to Fe2O3, thanks

Explanation / Answer

The balanced redox reaction is :-

4FeO(s) + O2(g) ----> 2Fe2O3(s)

Oxidation half reaction :-

Fe2+(aq) ----> Fe3+(aq) + 2e-

Reduction half reaction:-

O2(g) + 4e- -----> 2O2-(aq)

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