The Reaction and Its Stoichiometry

Oct 13, 2025 by talynt.org 88 views

Introduction

Chemical reactions are a fundamental concept in chemistry, and understanding the stoichiometry of these reactions is crucial for predicting the amounts of reactants and products involved. In this article, we will explore the stoichiometry of the reaction $2Fe + 3F_2 \rightarrow 2FeF_3$ and determine the amount of fluorine required to produce 20.0 grams of $FeF_3$ .

The Reaction and Its Stoichiometry

The reaction $2Fe + 3F_2 \rightarrow 2FeF_3$ is a simple example of a redox reaction, where iron (Fe) is oxidized and fluorine (F) is reduced. The balanced equation shows that 2 moles of iron react with 3 moles of fluorine to produce 2 moles of iron(III) fluoride ( $FeF_3$ ).

To determine the amount of fluorine required to produce 20.0 grams of $FeF_3$ , we need to first calculate the molar mass of $FeF_3$ . The atomic masses of iron (Fe) and fluorine (F) are 55.85 g/mol and 18.998 g/mol, respectively.

Calculating the Molar Mass of $FeF_3$

The molar mass of $FeF_3$ can be calculated by adding the atomic masses of one iron atom and three fluorine atoms.

Molar mass of $FeF_3$ = atomic mass of Fe + 3 × atomic mass of F = 55.85 g/mol + 3 × 18.998 g/mol = 55.85 g/mol + 56.994 g/mol = 112.844 g/mol

Calculating the Number of Moles of $FeF_3$ Produced

To calculate the number of moles of $FeF_3$ produced, we can use the formula:

Number of moles = mass of substance / molar mass

Number of moles of $FeF_3$ = 20.0 g / 112.844 g/mol = 0.177 mol

Calculating the Number of Moles of Fluorine Required

From the balanced equation, we can see that 3 moles of fluorine are required to produce 2 moles of $FeF_3$ . Therefore, the number of moles of fluorine required to produce 0.177 mol of $FeF_3$ can be calculated as follows:

Number of moles of F2 = (3/2) × number of moles of FeF3 = (3/2) × 0.177 mol = 0.2655 mol

Calculating the Mass of Fluorine Required

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

Mass of substance = number of moles × molar mass

Mass of F2 = 0.2655 mol × 38.000 g/mol (molar mass of F2) = 10.094 g

Conclusion

In this article, we have calculated the amount of fluorine required to produce 20.0 grams of $FeF_3$ from the reaction $2Fe + 3F_2 \rightarrow 2FeF_3$ . The calculation involves determining the molar mass of $FeF_3$ , calculating the number of moles of $FeF_3$ produced, and then calculating the number of moles of fluorine required to produce that amount of $FeF_3$ . Finally, we calculated the mass of fluorine required using the molar mass of fluorine.

Frequently Asked Questions

What is the molar mass of $FeF_3$ ? The molar mass of $FeF_3$ is 112.844 g/mol.
How many moles of $FeF_3$ are produced from 20.0 grams of $FeF_3$ ? 0.177 mol of $FeF_3$ are produced from 20.0 grams of $FeF_3$ .
How many moles of fluorine are required to produce 0.177 mol of $FeF_3$ ? 0.2655 mol of fluorine are required to produce 0.177 mol of $FeF_3$ .
What is the mass of fluorine required to produce 20.0 grams of $FeF_3$ ? The mass of fluorine required to produce 20.0 grams of $FeF_3$ is 10.094 g.

References

Chemistry: An Atoms First Approach, by Steven S. Zumdahl
General Chemistry: Principles and Modern Applications, by Linus Pauling

Introduction

In our previous article, we explored the stoichiometry of the reaction $2Fe + 3F_2 \rightarrow 2FeF_3$ and calculated the amount of fluorine required to produce 20.0 grams of $FeF_3$ . In this article, we will answer some frequently asked questions related to the stoichiometry of this reaction.

Q&A

Q: What is the molar mass of $FeF_3$ ?

A: The molar mass of $FeF_3$ is 112.844 g/mol.

Q: How many moles of $FeF_3$ are produced from 20.0 grams of $FeF_3$ ?

A: 0.177 mol of $FeF_3$ are produced from 20.0 grams of $FeF_3$ .

Q: How many moles of fluorine are required to produce 0.177 mol of $FeF_3$ ?

A: 0.2655 mol of fluorine are required to produce 0.177 mol of $FeF_3$ .

Q: What is the mass of fluorine required to produce 20.0 grams of $FeF_3$ ?

A: The mass of fluorine required to produce 20.0 grams of $FeF_3$ is 10.094 g.

Q: What is the mole ratio of iron to fluorine in the reaction $2Fe + 3F_2 \rightarrow 2FeF_3$ ?

A: The mole ratio of iron to fluorine in the reaction $2Fe + 3F_2 \rightarrow 2FeF_3$ is 2:3.

Q: What is the mole ratio of $FeF_3$ to fluorine in the reaction $2Fe + 3F_2 \rightarrow 2FeF_3$ ?

A: The mole ratio of $FeF_3$ to fluorine in the reaction $2Fe + 3F_2 \rightarrow 2FeF_3$ is 2:3.

Q: How many grams of iron are required to produce 20.0 grams of $FeF_3$ ?

A: To calculate the mass of iron required, we need to first calculate the number of moles of $FeF_3$ produced, which is 0.177 mol. Then, we can use the mole ratio of iron to $FeF_3$ in the reaction, which is 2:2, to calculate the number of moles of iron required. Finally, we can use the molar mass of iron to calculate the mass of iron required.

Number of moles of Fe = (2/2) × number of moles of FeF3 = (2/2) × 0.177 mol = 0.177 mol

Mass of Fe = number of moles × molar mass = 0.177 mol × 55.85 g/mol = 9.893 g

Q: How many grams of fluorine are required to produce 20.0 grams of $FeF_3$ ?

A: We have already calculated the mass of fluorine required to produce 20.0 grams of $FeF_3$ , which is 10.094 g.

Conclusion

In this article, we have answered some frequently asked questions related to the stoichiometry of the reaction $2Fe + 3F_2 \rightarrow 2FeF_3$ . We have calculated the molar mass of $FeF_3$ , the number of moles of $FeF_3$ produced, the number of moles of fluorine required, and the mass of fluorine required to produce 20.0 grams of $FeF_3$ . We have also calculated the mass of iron required to produce 20.0 grams of $FeF_3$ .

Frequently Asked Questions

What is the molar mass of $FeF_3$ ? The molar mass of $FeF_3$ is 112.844 g/mol.
How many moles of $FeF_3$ are produced from 20.0 grams of $FeF_3$ ? 0.177 mol of $FeF_3$ are produced from 20.0 grams of $FeF_3$ .
How many moles of fluorine are required to produce 0.177 mol of $FeF_3$ ? 0.2655 mol of fluorine are required to produce 0.177 mol of $FeF_3$ .
What is the mass of fluorine required to produce 20.0 grams of $FeF_3$ ? The mass of fluorine required to produce 20.0 grams of $FeF_3$ is 10.094 g.
What is the mole ratio of iron to fluorine in the reaction $2Fe + 3F_2 \rightarrow 2FeF_3$ ? The mole ratio of iron to fluorine in the reaction $2Fe + 3F_2 \rightarrow 2FeF_3$ is 2:3.
What is the mole ratio of $FeF_3$ to fluorine in the reaction $2Fe + 3F_2 \rightarrow 2FeF_3$ ? The mole ratio of $FeF_3$ to fluorine in the reaction $2Fe + 3F_2 \rightarrow 2FeF_3$ is 2:3.
How many grams of iron are required to produce 20.0 grams of $FeF_3$ ? 9.893 g of iron are required to produce 20.0 grams of $FeF_3$ .

References

Chemistry: An Atoms First Approach, by Steven S. Zumdahl
General Chemistry: Principles and Modern Applications, by Linus Pauling