Question

If ferric oxide is heated strongly in a stream of carbon monoxide gas, it produces molten elemental iron and carbon dioxide gas. Write the unbalanced chemical equation for this process.

Short answer

The unbalanced chemical equation for the reaction between ferric oxide and carbon monoxide is: \(Fe_2O_3 + CO \rightarrow Fe + CO_2\)

Step-by-step solution

Write the given compounds and their formulas

We are given: 1. Ferric oxide - Fe2O3 2. Carbon monoxide - CO 3. Molten elemental iron - Fe 4. Carbon dioxide gas - CO2

Write the unbalanced chemical equation using the provided compounds

Now that we have the correct formulas for each compound, we can combine them to create the unbalanced chemical equation: Fe2O3 + CO → Fe + CO2

Key concepts

Ferric Oxide

Ferric oxide, also known as iron(III) oxide, is a compound with the formula \(Fe_2O_3\). It is commonly found in nature as the mineral hematite. It's a reddish-brown powder and used widely in various industrial applications.

Ferric oxide plays a crucial role in the process of extracting iron from its ores. When heated with carbon monoxide, it undergoes a chemical change.
Understanding the properties of ferric oxide is necessary for comprehending its role in chemical reactions such as the one producing iron.

Some important characteristics of ferric oxide:

• It is not only an iron ore but also a component in magnetic materials.
• Its ability to catalyze reactions makes it valuable in industrial processes.
• When heated, ferric oxide can lose oxygen, which is essential for obtaining pure iron.

Knowing these properties helps you understand why ferric oxide is used in reactions involving iron production.

Chemical Equations

Chemical equations represent reactions exactly like a recipe shows how to make a dish. They show the substances that react, called reactants, and the new substances they form, called products.
In writing chemical equations, we must include the correct chemical formulas for each substance involved. This provides a clear representation of the quantities and substances Pre-reacting and post-reacting.

For the given exercise, the chemical equation involves:

• Ferric oxide \((Fe_2O_3)\) and carbon monoxide \((CO)\) as reactants.
• Molten elemental iron \((Fe)\) and carbon dioxide \((CO_2)\) as products.

The equation can be written as:

\(Fe_2O_3 + CO \rightarrow Fe + CO_2\)

This is an unbalanced equation, which means that the number of atoms for each element is not the same on both sides of the equation. Balancing this equation ensures compliance with the law of conservation of mass, which states that matter cannot be created or destroyed in chemical reactions.

Iron Production

Iron production is a vital industrial process where iron is extracted from its ores, primarily from ferric oxide. This process is a cornerstone of metallurgy and supports many industries, from construction to manufacturing.

The reaction between ferric oxide and carbon monoxide is a reduction-oxidation (redox) reaction.
In this specific reaction, carbon monoxide reduces ferric oxide to molten iron, an essential step in obtaining metallic iron.

During this reaction:

• Ferric oxide provides iron ions.
• Carbon monoxide serves as the reducing agent.
• The process produces carbon dioxide as a by-product.

Hence, this simple yet crucial chemical exercise mirrors the larger industrial practice where these principles are applied on a vast scale. While understanding chemical reactions such as these, one can appreciate the chemical transformations necessary for steel production and various other applications.