How Much Iron Can Be Produced from 100 grams of Fe2O3?

In order to understand how much iron can be produced from 100 grams of iron oxide (Fe2O3), it is important to first break down the process involved in this chemical reaction. We need to calculate the molar quantity of ferric oxide (Fe2O3) and then determine the yield of iron (Fe) based on the stoichiometry of the given reaction.

Molar Quantity of Ferric Oxide

The first step in this process is to calculate the molar quantity of ferric oxide (Fe2O3) given the mass. The molar mass of Fe2O3 is composed of the individual molar masses of iron (Fe) and oxygen (O). For iron, the molar mass is approximately 55.85 g/mol, and for oxygen, it is 16.00 g/mol. Therefore, the molar mass of Fe2O3 is:

159.69 g/mol

Given this, the molar quantity of 100 grams of Fe2O3 can be calculated as:

Q(Fe2O3) 100g}{159.69g/mol} 0.626 mol

Chemical Reaction and Stoichiometry

Ferric oxide can be reduced to iron using carbon (CO) as a reducing agent through the following reaction:

Fe2O3 3CO Δ→ 2Fe 3CO2

This reaction is an example of a redox reaction where iron (Fe2O3) is reduced to iron (Fe) and carbon monoxide (CO) is oxidized to carbon dioxide (CO2).

Calculating the Yield of Iron

From the stoichiometry of the chemical reaction, we can see that 1 mole of Fe2O3 produces 2 moles of Fe. Therefore, the molar quantity of iron produced from 0.626 moles of Fe2O3 can be calculated as:

Q(Fe) 2 × 0.626 mol 1.252 mol

Finally, the mass of iron produced can be calculated using its molar mass, which is approximately 55.85 g/mol:

m(Fe) 1.252 mol × 55.85 g/mol 70 g

Therefore, approximately 70 grams of iron can be produced from 100 grams of Fe2O3.

Understanding Iron Production from Ore

This calculation highlights the importance of understanding the chemistry and thermodynamics involved in iron production from iron ore. Iron ore is a critical resource in the production of steel, and knowledge of the chemical reactions and stoichiometry is essential for optimizing the production process in industrial settings.

Fe2O3, or ferric oxide, is a common form of iron ore, and the process of reducing it to metallic iron using carbon is a fundamental step in iron smelting. By understanding the exact amount of iron that can be produced from a given quantity of ore, we can make more informed decisions regarding resource optimization and industrial efficiency.

Additional Considerations

While the above calculation provides a clear theoretical understanding of the iron production process, there are several additional factors that need to be taken into account for practical applications. These include:

Recovery Efficiency: Real-world conditions may not achieve 100% efficiency in the reduction process. Losses during Processing: There may be some loss of iron due to impurities, particle size, or other factors during the smelting process. Energy Requirements: The amount of energy required to drive the chemical reaction can also impact the overall process.

In conclusion, the amount of iron that can be produced from 100 grams of ferric oxide (Fe2O3) is approximately 70 grams, based on the stoichiometry of the chemical reaction. This is a fundamental calculation in the field of chemical engineering and metallurgy.