Determining the Yield of Fe2O3 from Fe and O2: A Comprehensive Guide

Understanding the chemical reaction between iron (Fe) and oxygen (O2) to form iron(III) oxide (Fe2O3) is crucial in various industrial and academic applications. This guide will walk you through the process of calculating the yield of Fe2O3 from given masses of Fe and O2.

Steps to Determine the Yield of Fe2O3

Step 1: Write the Balanced Chemical Equation Step 2: Calculate the Number of Moles of Each Reactant Step 3: Determine the Limiting Reactant Step 4: Calculate the Moles of Fe2O3 Produced Step 5: Calculate the Mass of Fe2O3 Produced

Step 1: Write the Balanced Chemical Equation

The reaction between iron (Fe) and oxygen (O2) to form iron(III) oxide (Fe2O3) is represented by the following balanced chemical equation:

4Fe 3O2 → 2Fe2O3

Step 2: Calculate the Number of Moles of Each Reactant

To calculate the moles of each reactant, we need their respective molar masses:

Fe: molar mass 55.85 g/mol O2: molar mass 32.00 g/mol

Using the given masses of Fe and O2, we can now calculate the moles:

Moles of Fe: Moles of O2:

Moles of Fe Mass of Fe / Molar mass of Fe 24.0 g / 55.85 g/mol ≈ 0.43 mol

Moles of O2 Mass of O2 / Molar mass of O2 5.00 g / 32.00 g/mol ≈ 0.16 mol

Step 3: Determine the Limiting Reactant

From the balanced equation, we see the mole ratio required for the reaction is 4 moles of Fe to 3 moles of O2. Therefore, the amount of O2 required to fully react with 0.43 moles of Fe is calculated as:

Moles of O2 required (3/4) × 0.43 ≈ 0.3225 mol

Since we only have 0.16 mol of O2, it is the limiting reactant.

Step 4: Calculate the Moles of Fe2O3 Produced

From the balanced equation, 3 moles of O2 produce 2 moles of Fe2O3. Therefore, we can find the moles of Fe2O3 produced from the available O2:

Moles of Fe2O3 (2/3) × 0.16 mol ≈ 0.1067 mol

Step 5: Convert Moles of Fe2O3 to Grams

The molar mass of Fe2O3 is calculated as follows:

Molar mass of Fe2O3 2 × 55.85 3 × 16.00 159.7 g/mol

Now we can find the mass of Fe2O3 produced:

Mass of Fe2O3 Moles of Fe2O3 × Molar mass of Fe2O3

Mass of Fe2O3 0.1067 mol × 159.7 g/mol ≈ 17.05 g

Conclusion

Therefore, approximately 17.05 grams of Fe2O3 will be produced from 24.0 g of Fe and 5.00 g of O2, with O2 being the limiting reactant.

Key Takeaways

The balanced chemical equation for the reaction between iron and oxygen to form iron(III) oxide is 4Fe 3O2 → 2Fe2O3. The limiting reactant determines the maximum amount of product that can be formed. The molar mass is a key factor in converting between moles and mass.

Related Keywords

Iron Oxide Chemical Reaction Molar Mass