Question

When steel wool (iron) is heated in pure oxygen gas, the steel wool bursts into flame and a fine powder consisting of a mixture of iron oxides ( \(\mathrm{FeO}\) and \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) ) forms. Write separate unbalanced equations for the reaction of iron with oxygen to give each of these products.

Short answer

The two unbalanced equations for the reaction of iron with oxygen to form iron(II) oxide (FeO) and iron(III) oxide (Fe₂O₃) are as follows: 1. Formation of iron(II) oxide (FeO): \(Fe + O_2 \rightarrow FeO\) 2. Formation of iron(III) oxide (Fe₂O₃): \(Fe + O_2 \rightarrow Fe_2O_3\)

Step-by-step solution

Identify the reactants and products

In this reaction, iron (Fe) reacts with oxygen (O2) to form iron(II) oxide (FeO).

Write the unbalanced equation

To write the unbalanced equation, we place the reactants on the left side of the equation and products on the right side. The unbalanced equation for the formation of FeO is: Fe + O2 -> FeO Second unbalanced equation: Formation of iron(III) oxide (Fe2O3)

Identify the reactants and products

In this reaction, iron (Fe) reacts with oxygen (O2) to form iron(III) oxide (Fe2O3).

Write the unbalanced equation

To write the unbalanced equation, we place the reactants on the left side of the equation and products on the right side. The unbalanced equation for the formation of Fe₂O₃ is: Fe + O2 -> Fe2O3

Key concepts

Iron Oxides

Iron oxides are compounds made of iron and oxygen. They are quite prevalent in our everyday lives. Common forms are rust and iron utilized in various industrial processes. Depending on the ratio of iron to oxygen, different iron oxides can form. The two primary types produced during the reaction of iron with oxygen include:

• Iron(II) Oxide (\( \text{FeO} \)): This is formed when the ratio of iron to oxygen is 1:1.


• Iron(III) Oxide (\( \text{Fe}_2\text{O}_3 \)): This occurs when the ratio becomes 2:3.

Both these oxides occur naturally and are involved in various chemical reactions.When steel wool burns, it reacts with oxygen to form these iron oxides. While the formation conditions influence which oxide is more prominent, both are essential in understanding rusting and metal corrosion.

Balancing Equations

Balancing chemical equations is a fundamental skill in chemistry. It ensures the conservation of mass, meaning atoms of each element are equal on both sides of the equation. When writing equations for reactions, including for the formation of iron oxides, it's crucial to balance them.
Let's start with an example, the formation of iron(II) oxide:

• The unbalanced equation starts as: \( \text{Fe} + \text{O}_2 \rightarrow \text{FeO} \).


• To balance it, we need to ensure the number of Fe and O atoms are equal on both sides.


• Balanced equation: \( 2\text{Fe} + \text{O}_2 \rightarrow 2\text{FeO} \).

For iron(III) oxide:

• The initial unbalanced equation is: \( \text{Fe} + \text{O}_2 \rightarrow \text{Fe}_2\text{O}_3 \).


• To balance it, remember the ratio of Fe and O: 2 Fe to 3 O atoms.


• Balanced equation: \( 4\text{Fe} + 3\text{O}_2 \rightarrow 2\text{Fe}_2\text{O}_3 \).

Balancing provides clarity and accuracy in representing the reaction.

Oxygen Reactions

Reactions with oxygen, often known as combustion reactions, are critical in both nature and industry. Oxygen is a reactive element that often combines with different substances, including metals like iron. When iron reacts with oxygen, distinct reactions occur that produce heat and light, observable as flames when steel wool ignites.

• Oxygen as a Reactant: Oxygen generally combines with metals to form metal oxides.


• Exothermic Nature: These reactions typically release energy in the form of heat, making them exothermic.


• Practical Applications: Understanding these reactions helps in controlling and using combustion in industries, as well as predicting and managing rust formation in engineering and construction.

It is essential to understand these fundamental concepts to recognize how oxygen transforms elements like iron through chemical processes.