This is an oxidation-reduction (redox) reaction:
8 NV + 8 e- → 8 NIV (reduction)
4 FeII - 4 e- → 4 FeIII (oxidation)
2 O-II - 4 e- → 2 O0 (oxidation)
Fe(NO3)2 is an oxidizing agent, Fe(NO3)2 is a reducing agent, Fe(NO3)2 is a reducing agent.
Word equation
iron(II) nitrate → iron(III) oxide + oxygen + nitrogen dioxide
Input interpretation
Fe(NO3)2 → Fe2O3 + O2 + NO2
iron(II) nitrate iron(III) oxide Oxygen nitrogen dioxide
Balanced equation
Balance the chemical equation algebraically:
Fe(NO3)2 → Fe2O3 + O2 + NO2
Add stoichiometric coefficients, c,, to the reactants and products:
c1 Fe(NO3)2 → c2Fe2O3 + c3O2 + c4O2
Set the number of atoms in the reactants equal to the number of atoms in the products for Fe, N and O:
Fe: c1 = 2c2
N: 2c1 = c4
O: 6c1 = 3c2 + 2c3 + 2c4
Since the coefficients are relative quantities and underdetermined, choose a coefficient to set arbitrarily. To keep the coefficients small, the arbitrary value is ordinarily one. For instance, set c3 = 1 and solve the system of equations for the remaining coefficients:
c1 = 4 c2=2
c3=1 c4=8
Substitute the coefficients into the chemical reaction to obtain the balanced
equation:
Answer:
Fe(NO3)2 → Fe2O3 + O2 + NO2
