## Introduction

In chemistry, an oxidation-reduction (redox) reaction involves the transfer of electrons between reactants. In this case, we will be discussing the redox reaction between magnesium (Mg) and ferric nitrate (Fe(NO3)3). Through the process of balancing the chemical equation, we can gain a better understanding of the reactants and products involved in this reaction.

## Redox Reaction

The following equations represent the oxidation and reduction reactions taking place in this redox reaction:

*3 Mg0 - 6 e- → 3 MgII (oxidation)*

*3 NV + 3 e- → 3 NIV (reduction)*

*FeIII + 3 e- → Fe0 (reduction)*

Mg acts as a reducing agent, while Fe(NO3)3 acts as an oxidizing agent.

## Word Equation

The word equation for this redox reaction is:

*Magnesium + Ferric Nitrate → Magnesium Nitrate + Iron*

## Input Interpretation

Using the word equation, we can interpret the following equation:

*2 Mg + 3 Fe(NO3)3 → 2 Mg(NO3)2 + 3 Fe*

## Balanced Equation

To balance the chemical equation, we can use stoichiometric coefficients. Starting with the unbalanced equation:

*2 Mg + 3 Fe(NO3)3 → 2 Mg(NO3)2 + 3 Fe*

We can assign variables to each coefficient, resulting in

*c1 2 Mg + c2 3 Fe(NO3)3 → c3 2 Mg(NO3)2 + c4 3 Fe*

Next, we set the number of atoms for Mg, Fe, N, and O equal on both sides of the equation:

*Mg: c1=c3*

*Fe: c2=c4*

*N: 3c2=2c3*

*O: 9c2=6c3*

We then arbitrarily set one coefficient to a value of 1, and solve for the remaining coefficients. In this case, we can set c2 = 1, resulting in:

*c1 = 3/2 c2 = 1*

*c3 = 3/2 c4 = 1*

To eliminate fractional coefficients, we can multiply each coefficient by the least common denominator, which is 2. This results in the balanced equation:

*2 Mg + 3 Fe(NO3)3 → 2 Mg(NO3)2 + 3 Fe*