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 \(\left(\mathrm{FeO} \text { and } \mathrm{Fe}_{2} \mathrm{O}_{3}\right)\) forms. Write separate unbalanced equations for the reaction of iron with oxygen to give each of these products.

Short answer

The unbalanced equations for the formation of iron oxides are: 1. \(Fe + O_2 \rightarrow FeO\) 2. \(Fe + O_2 \rightarrow Fe_2O_3\)

Step-by-step solution

Reaction 1: Formation of FeO

To write the unbalanced equation for the formation of FeO, we need to identify the reactants and the products. In this case, the reactants are Iron (Fe) and Oxygen (O2), and the product is FeO. The unbalanced equation for the formation of FeO is: \(Fe + O_2 \rightarrow FeO\)

Reaction 2: Formation of Fe2O3

To write the unbalanced equation for the formation of Fe2O3, we need to identify the reactants and the products. In this case, the reactants are Iron (Fe) and Oxygen (O2), and the product is Fe2O3. The unbalanced equation for the formation of Fe2O3 is: \(Fe + O_2 \rightarrow Fe_2O_3\) These are the unbalanced equations for the formation of both iron oxides, FeO and Fe2O3.

Key concepts

Iron Oxides

Iron oxides are compounds composed of iron and oxygen. They occur naturally in various minerals and are commonly found on the Earth's surface. Iron oxides have different forms, with two primary types being iron(II) oxide (FeO) and iron(III) oxide (Fe2O3). These compounds are vital in numerous industrial applications, including the production of steel, pigments, and magnetic materials.

• Iron(II) oxide (FeO): This oxide is formed when iron reacts with oxygen in a 1:1 ratio. The reaction produces FeO, characterized by its black color. FeO is less stable compared to other iron oxides.
• Iron(III) oxide (Fe2O3): Formed when two iron atoms react with three oxygen molecules, this compound is known for its reddish-brown color and higher stability. It is a major component of rust and is widely used in pigments and coatings.

Iron oxides play a crucial role in various environmental and geological processes. They also serve as precursors for other chemical reactions crucial in the metallurgy industry.

Chemical Equations

Chemical equations are symbolic representations of chemical reactions. They detail the reactants (substances you start with) and the products (substances you end up with) as well as the transformation process, using chemical symbols and formulas.
Writing chemical equations involves identifying the reactants and products. Once identified, they are placed on either side of the equation, separated by an arrow indicating the direction of the reaction. In our task involving iron and oxygen:

• The reactants are iron (Fe) and oxygen (O2).
• The products are iron oxides, either FeO or Fe2O3.

Unbalanced equations show the basic transformation. They serve as a starting point before balancing, which ensures that the number of atoms for each element is the same on both sides of the equation, respecting the law of conservation of mass.

Oxidation Reactions

Oxidation reactions are processes where a substance gains oxygen or loses electrons. These reactions are a fundamental part of chemistry and are integral to understanding various natural and industrial processes. Oxidation is usually coupled with reduction, where one species is oxidized and another is reduced, known collectively as redox reactions.
In the case of iron reacting with oxygen:

• Iron (Fe) is oxidized. It loses electrons to form positive iron ions (Fe²⁺ or Fe³⁺).
• Oxygen (O2) gains electrons to form oxide ions (O^2-), completing the oxidation process.

These reactions are not just restricted to iron. Oxidation is seen in everyday phenomena, such as when apples brown upon exposure to air, or when metals corrode. Understanding oxidation reactions allows us to better understand processes like burning, metabolism in the human body, and the operation of batteries.