Question: 1. First evaluate the reactants side: Start with FeO3 O 3 -2 total charge -6 0 2. Then evaluate Al. Since aluminum is in

1. First evaluate the reactants side: Start with FeO3 O 3 -2 total charge -6 0 2. Then evaluate Al. Since aluminum is in its elemental form, the oxidation state is zero = 0 3. Then evaluate the products side: Start with AlO3 FeO3 number of atoms oxidation state Fe 2 +3 +6 Al 2 +3 +6 0 3 -2 -6 AlO3 number of atoms oxidation state total charge 0 4. Then evaluate Fe. Since iron is in its elemental form, the oxidation state is zero, 0 5. Finally, write in the values on the equation and evaluate the redox states FeO3(s) + 2Al(s) AlO3(s) + 2Fe(l) +3 -2 +3 -2 overall charge oxidized (losing e') reduced (gaining e') overall charge

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