Chapter 5, Problem 5.115AP

(a)

Interpretation Introduction

Interpretation: The mineral magnetite $\left({\text{Fe}}_{\text{3}}{\text{O}}_{\text{4}}\right)$ is given to be a magnetic whereas iron $(\text{II)}$ oxide is not. The balanced chemical equation for the formation of magnetite from iron $(\text{II)}$ oxide and oxygen is to be stated.

The enthalpy change of the balanced reaction for formation of ${\text{Fe}}_{\text{3}}{\text{O}}_{\text{4}}$ from iron $(\text{II)}$ oxide and oxygen is to be calculated.

Concept introduction: To balance a general reaction, first metal atoms are balanced then oxygen and hydrogen atoms.

The change in enthalpy for the formation of magnetite $\left(\Delta H_{{\text{Fe}}_{\text{3}}{\text{O}}_{\text{4}}}^{\text{ο}}\right)$ from iron is calculated by the formula,

$\Delta H_{{\text{Fe}}_{\text{3}}{\text{O}}_{\text{4}}}^{\text{ο}}=\frac{q}{n}$

To determine: The balanced chemical equation for the formation of magnetite from iron $(\text{II)}$ oxide and oxygen.

(b)

Interpretation Introduction

To determine: The enthalpy change of the balanced reaction for formation of ${\text{Fe}}_{\text{3}}{\text{O}}_{\text{4}}$ from iron $(\text{II)}$ oxide and oxygen.