### This is an **oxidation-reduction** (redox) reaction:

* ** 8 NV + 8 e- → 8 NIV **(reduction)*

*8 NV + 8 e- → 8 NIV*

*(reduction)*

* 4 FeII - 4 e- → 4 FeIII **(oxidation)*

*4 FeII - 4 e- → 4 FeIII*

*(oxidation)*

* 2 O-II - 4 e- → 2 O0 **(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*