Table of contents

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



Fe(NO3)2 → Fe2O3 + O2 + NO2