Question

Iron is prepared industrially by passing carbon monoxide gas through molten iron ore, \(\mathrm{Fe}_{2} \mathrm{O}_{3}\), in a blast furnace at \(1500^{\circ} \mathrm{C}\). Assuming the only products are molten iron and carbon dioxide gas, write a balanced chemical equation for the manufacture of iron.

Short answer

The balanced chemical equation is \(\mathrm{Fe}_{2} \mathrm{O}_{3} + 3\mathrm{CO} \rightarrow 2\mathrm{Fe} + 3\mathrm{CO}_{2}\).

Step-by-step solution

Identify the Reactants and Products

The reactants for this process are iron(III) oxide, \(\mathrm{Fe}_{2} \mathrm{O}_{3}\), and carbon monoxide gas, \(\mathrm{CO}\). The products are molten iron, \(\mathrm{Fe}\), and carbon dioxide gas, \(\mathrm{CO}_{2}\).

Write the Unbalanced Chemical Equation

Write the chemical equation with the reactants on the left side and the products on the right side of the equation: \[\mathrm{Fe}_{2} \mathrm{O}_{3} + \mathrm{CO} \rightarrow \mathrm{Fe} + \mathrm{CO}_{2}.\]

Count and Balance Iron Atoms

On the left side, there are two iron atoms in \(\mathrm{Fe}_{2} \mathrm{O}_{3}\). On the right side, each \(\mathrm{Fe}\) represents one atom. Thus, place a coefficient of 2 in front of \(\mathrm{Fe}\) on the products side: \[\mathrm{Fe}_{2} \mathrm{O}_{3} + \mathrm{CO} \rightarrow 2\mathrm{Fe} + \mathrm{CO}_{2}.\]

Count and Balance Oxygen Atoms

There are three oxygen atoms in \(\mathrm{Fe}_{2} \mathrm{O}_{3}\). Each \(\mathrm{CO}_{2}\) contains two oxygen atoms. To match the oxygen atoms from the reactants to the products, place a coefficient of 3 in front of \(\mathrm{CO}_{2}\): \[\mathrm{Fe}_{2} \mathrm{O}_{3} + \mathrm{CO} \rightarrow 2\mathrm{Fe} + 3\mathrm{CO}_{2}.\]

Count and Balance Carbon Atoms

There are three carbon atoms on the products side in \(3\mathrm{CO}_{2}\). To balance the carbon, place a coefficient of 3 in front of \(\mathrm{CO}\) on the reactants side: \[\mathrm{Fe}_{2} \mathrm{O}_{3} + 3\mathrm{CO} \rightarrow 2\mathrm{Fe} + 3\mathrm{CO}_{2}.\]

Verify Atom Balance

Check that each element has the same number of atoms on both sides of the equation: \(\mathrm{Fe}_{2} \mathrm{O}_{3} + 3\mathrm{CO} \rightarrow 2\mathrm{Fe} + 3\mathrm{CO}_{2}\) is balanced with 2 Fe, 3 C, and 3 O on both sides.

Key concepts

Balancing Equations

Balancing equations in chemistry ensures that the number of each type of atom is the same on both sides of the chemical equation. This follows the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction.Here's how you balance chemical equations:

• First, identify all reactants and products in the reaction.
• Write the unbalanced equation, placing reactants on one side and products on the other.
• Next, count the number of atoms for each element on both sides.
• Adjust coefficients—numbers placed before formulas—to balance the atoms.

For the equation in question, we began by identifying the reactants, \( \mathrm{Fe}_{2} \mathrm{O}_{3} \) and \( \mathrm{CO} \), and products, \( \mathrm{Fe} \) and \( \mathrm{CO}_{2} \). Through balancing, we achieve: \( \mathrm{Fe}_{2} \mathrm{O}_{3} + 3\mathrm{CO} \rightarrow 2\mathrm{Fe} + 3\mathrm{CO}_{2} \). This balanced equation represents the stoichiometry of the reaction, ensuring that iron, carbon, and oxygen atoms are conserved.

Blast Furnace

A blast furnace is a huge structure used in the industrial production of iron, employing high temperatures and chemical reactions to extract iron from its ore. It's fundamental in industrial chemistry as it converts raw iron ore into valuable molten iron.In a blast furnace, iron(III) oxide (\( \mathrm{Fe}_{2} \mathrm{O}_{3} \)) is reacted with carbon monoxide (\( \mathrm{CO} \)) at about 1500°C to produce molten iron and carbon dioxide. This intense heat provides energy for breaking the chemical bonds in the ore.Key processes inside the blast furnace include:

• Chemical reduction of the ore to release iron.
• High temperature to maintain molten iron and facilitate the reaction.
• Please note, the furnace operates continuously for efficient production.

This process not only results in the desired production of iron but also exemplifies the application of thermochemistry and physical chemistry principles.

Industrial Chemistry

Industrial chemistry refers to the large-scale production and use of chemicals in various industries. It bridges the gap between lab chemistry and industrial applications, focusing on optimizing substances for mass production. In industrial chemistry, chemical processes are often scaled up for economic demands. The manufacture of iron in a blast furnace is a prime example, illustrating how controlled chemical reactions can produce materials on a vast scale. Key objectives of industrial chemistry include:

• Improving reaction efficiency for maximum yield.
• Reducing waste and environmental impact.
• Maximizing safety through process control.

By understanding and applying these principles, industrial chemists can create processes that are both economically and environmentally sustainable, thus playing an essential role in modern manufacturing and technology.