How Many Grams Of $Fe_2O_3$ Would Be Required To Make 187 G Of Fe?$ \begin{array}{c} Fe_2O_3 + 3 CO \rightarrow 2 Fe + 3 CO_2 \ Fe 55.85 , \text{g/mol \quad[?] , \text{g} , Fe_2O_3 \end{array} }$

Introduction

In this article, we will explore the stoichiometry of a chemical reaction involving iron(III) oxide (Fe2O3) and carbon monoxide (CO). The reaction is as follows:

Fe2O3 + 3 CO → 2 Fe + 3 CO2

We are given the molar mass of iron (Fe) as 55.85 g/mol and we need to find out how many grams of Fe2O3 would be required to produce 187 g of Fe.

Step 1: Calculate the Number of Moles of Fe

To calculate the number of moles of Fe, we can use the formula:

moles = mass / molar mass

Substituting the given values, we get:

moles Fe = 187 g / 55.85 g/mol = 3.34 mol

Step 2: Calculate the Number of Moles of Fe2O3

From the balanced equation, we can see that 1 mole of Fe2O3 produces 2 moles of Fe. Therefore, the number of moles of Fe2O3 required to produce 3.34 mol of Fe is:

moles Fe2O3 = moles Fe / 2 = 3.34 mol / 2 = 1.67 mol

Step 3: Calculate the Mass of Fe2O3 Required

To calculate the mass of Fe2O3 required, we can use the formula:

mass = moles × molar mass

The molar mass of Fe2O3 is 159.69 g/mol (2 × 55.85 g/mol + 3 × 16.00 g/mol). Substituting the values, we get:

mass Fe2O3 = 1.67 mol × 159.69 g/mol = 266.3 g

Conclusion

Therefore, to produce 187 g of Fe, we would require approximately 266.3 g of Fe2O3.

Discussion

This calculation demonstrates the importance of stoichiometry in chemistry. By understanding the mole ratios between reactants and products, we can predict the amounts of substances required to produce a given amount of product. This is a fundamental concept in chemistry and is essential for designing and optimizing chemical reactions.

Limitations

This calculation assumes that the reaction is 100% efficient, which is not always the case in real-world reactions. In practice, there may be losses due to impurities, side reactions, or other factors that can affect the yield of the desired product.

Future Work

This calculation can be extended to other reactions involving Fe2O3 and other substances. By exploring the stoichiometry of different reactions, we can gain a deeper understanding of the underlying chemistry and develop more efficient methods for producing desired products.

References

• [1] "Chemical Equilibrium" by J. W. Moore and R. G. Pearson
• [2] "Physical Chemistry" by P. W. Atkins and J. de Paula

Appendix

The following table summarizes the calculations performed in this article:

Substance	Molar Mass (g/mol)	Moles	Mass (g)
Fe	55.85	3.34	187
Fe2O3	159.69	1.67	266.3

Introduction

In our previous article, we explored the stoichiometry of the reaction between iron(III) oxide (Fe2O3) and carbon monoxide (CO) to produce iron (Fe) and carbon dioxide (CO2). We calculated the mass of Fe2O3 required to produce 187 g of Fe. In this article, we will answer some frequently asked questions related to this topic.

Q: What is stoichiometry?

A: Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions. It involves the calculation of the amounts of substances required to produce a given amount of product.

Q: Why is stoichiometry important?

A: Stoichiometry is important because it allows us to predict the amounts of substances required to produce a given amount of product. This is essential for designing and optimizing chemical reactions, as well as for scaling up reactions to industrial levels.

Q: How do I calculate the number of moles of a substance?

A: To calculate the number of moles of a substance, you can use the formula:

moles = mass / molar mass

For example, if you have 187 g of Fe and the molar mass of Fe is 55.85 g/mol, you can calculate the number of moles of Fe as follows:

moles Fe = 187 g / 55.85 g/mol = 3.34 mol

Q: How do I calculate the mass of a substance required to produce a given amount of product?

A: To calculate the mass of a substance required to produce a given amount of product, you can use the formula:

mass = moles × molar mass

For example, if you want to produce 187 g of Fe and the molar mass of Fe2O3 is 159.69 g/mol, you can calculate the mass of Fe2O3 required as follows:

mass Fe2O3 = 1.67 mol × 159.69 g/mol = 266.3 g

Q: What are some common mistakes to avoid when calculating stoichiometry?

A: Some common mistakes to avoid when calculating stoichiometry include:

• Not using the correct molar masses of substances
• Not converting units correctly (e.g. from grams to moles)
• Not considering the stoichiometry of the reaction (e.g. the mole ratio between reactants and products)
• Not rounding answers to the correct number of significant figures

Q: How can I apply stoichiometry to real-world problems?

A: Stoichiometry can be applied to a wide range of real-world problems, including:

• Designing and optimizing chemical reactions
• Scaling up reactions to industrial levels
• Predicting the amounts of substances required to produce a given amount of product
• Calculating the yields of chemical reactions
• Optimizing the use of resources in chemical reactions

Conclusion

Stoichiometry is a fundamental concept in chemistry that allows us to predict the amounts of substances required to produce a given amount of product. By understanding the mole ratios between reactants and products, we can design and optimize chemical reactions, as well as scale up reactions to industrial levels. In this article, we have answered some frequently asked questions related to stoichiometry and provided examples of how to apply it to real-world problems.

References

• [1] "Chemical Equilibrium" by J. W. Moore and R. G. Pearson
• [2] "Physical Chemistry" by P. W. Atkins and J. de Paula

Appendix

The following table summarizes the calculations performed in this article:

Substance	Molar Mass (g/mol)	Moles	Mass (g)
Fe	55.85	3.34	187
Fe2O3	159.69	1.67	266.3

Note: The values in the table are rounded to three significant figures.