This is an oxidation-reduction (redox) reaction:

* 6 Br0 + 6 e- → 6 Br-I (reduction)*

* 2 Fe0 - 6 e- → 2 FeIII (oxidation)*

*Br2* is an oxidizing agent, *Fe* is a reducing agent.

### Word equation

* bromine + iron → iron(III) bromide*

### Input interpretation

* Br2 + Fe → Febr3*

* Bromine iron iron(III) bromide*

### Balanced equation

Balance the chemical equation algebraically:

* Br2 + Fe → Febr3*

Add stoichiometric coefficients, c,, to the reactants and products:

* c1Br2 + c2 Fe → c3 Febr3*

Set the number of atoms in the reactants equal to the number of atoms in the products for ** Br **and

*Fe:**Br: 2c1 = 3c3*

*Fe: c2=c3*

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** c2 = 1** and solve the system of equations for the remaining coefficients:

* c1 = 3/2*

* c2 = 1 c3=1*

Multiply by the least common denominator, 2, to eliminate fractional coefficients:

* c1 = 3*

* c2 = 2 c3 = 2*

Substitute the coefficients into the chemical reaction to obtain the balanced

Equation:

** Answer**:

* Br2 + Fe → Febr3*