How Many Moles Of F E 2 S 3 Fe_2S_3 F E 2 ​ S 3 ​ Would Be Produced From The Complete Reaction Of 449 G Of F E B R 3 FeBr_3 F E B R 3 ​ ?Given The Reaction: 2 F E B R 3 + 3 N A 2 S → F E 2 S 3 + 6 N A B R 2FeBr_3 + 3Na_2S \rightarrow Fe_2S_3 + 6NaBr 2 F E B R 3 ​ + 3 N A 2 ​ S → F E 2 ​ S 3 ​ + 6 N A B R Calculate: ? mol F E 2 S 3 \text{? Mol } Fe_2S_3 ? mol F E 2 ​ S 3 ​

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Introduction

In this problem, we are given a chemical reaction between $FeBr_3$ and $Na_2S$ to produce $Fe_2S_3$ and $NaBr$. We are asked to calculate the number of moles of $Fe_2S_3$ produced from the complete reaction of 449 g of $FeBr_3$. To solve this problem, we need to use the concept of stoichiometry, which is the study of the quantitative relationships between reactants and products in chemical reactions.

The Given Reaction

The given reaction is:

$$2FeBr_3 + 3Na_2S \rightarrow Fe_2S_3 + 6NaBr$$

This reaction shows that 2 moles of $FeBr_3$ react with 3 moles of $Na_2S$ to produce 1 mole of $Fe_2S_3$ and 6 moles of $NaBr$.

Calculating the Number of Moles of $FeBr_3$

To calculate the number of moles of $Fe_2S_3$ produced, we first need to calculate the number of moles of $FeBr_3$ that react. We can do this by using the molar mass of $FeBr_3$, which is 295.68 g/mol.

We are given that 449 g of $FeBr_3$ react. To calculate the number of moles of $FeBr_3$, we can use the following formula:

$$\text{moles } FeBr_3 = \frac{\text{mass } FeBr_3}{\text{molar mass } FeBr_3}$$

Plugging in the values, we get:

$$\text{moles } FeBr_3 = \frac{449 \text{ g}}{295.68 \text{ g/mol}} = 1.52 \text{ mol}$$

Calculating the Number of Moles of $Fe_2S_3$

Now that we have the number of moles of $FeBr_3$, we can calculate the number of moles of $Fe_2S_3$ produced. From the balanced equation, we can see that 2 moles of $FeBr_3$ produce 1 mole of $Fe_2S_3$. Therefore, we can set up the following proportion:

$$\frac{2 \text{ mol } FeBr_3}{1 \text{ mol } Fe_2S_3} = \frac{1.52 \text{ mol } FeBr_3}{x \text{ mol } Fe_2S_3}$$

Solving for $x$, we get:

$$x = \frac{1.52 \text{ mol } FeBr_3}{2 \text{ mol } FeBr_3} = 0.76 \text{ mol } Fe_2S_3$$

Conclusion

Therefore, the number of moles of $Fe_2S_3$ produced from the complete reaction of 449 g of $FeBr_3$ is 0.76 mol.

Discussion

This problem requires the application of stoichiometry to calculate the number of moles of a product produced from a given amount of a reactant. The balanced equation provides the necessary information to set up a proportion and solve for the unknown number of moles. This type of problem is commonly encountered in chemistry and is an important tool for chemists to calculate the amounts of reactants and products in chemical reactions.

Limitations

One limitation of this problem is that it assumes that the reaction goes to completion, meaning that all of the $FeBr_3$ reacts to form $Fe_2S_3$. In reality, chemical reactions often do not go to completion, and some of the reactants may remain unreacted. This would affect the calculated number of moles of $Fe_2S_3$ produced.

Future Directions

Future directions for this problem could include exploring the effects of incomplete reactions on the calculated number of moles of $Fe_2S_3$ produced. This could involve using more complex reaction equations or incorporating additional variables, such as temperature or concentration, to model the reaction.

References

• [1] "Chemical Reactions and Stoichiometry". Chemistry LibreTexts.
• [2] "Balanced Chemical Equations". Chemistry LibreTexts.

Keywords

• Stoichiometry
• Chemical reactions
• Balanced equations
• Molar mass
• Moles
• Chemical equations
  

Introduction

In our previous article, we explored the concept of stoichiometry and how it can be used to calculate the number of moles of a product produced from a given amount of a reactant. In this article, we will answer some common questions related to stoichiometry and chemical reactions.

Q: What is stoichiometry?

A: Stoichiometry is the study of the quantitative relationships between reactants and products in chemical reactions. It involves calculating the amounts of reactants and products in a reaction, taking into account the coefficients in the balanced equation.

Q: What is a balanced equation?

A: A balanced equation is a chemical equation in which the number of atoms of each element is the same on both the reactant and product sides. This is achieved by adding coefficients to the reactants and products.

Q: How do I calculate the number of moles of a product produced from a given amount of a reactant?

A: To calculate the number of moles of a product produced, you need to know the molar mass of the product and the amount of the reactant that reacts. You can then use the coefficients in the balanced equation to set up a proportion and solve for the number of moles of the product.

Q: What is the difference between a mole and a gram?

A: A mole is a unit of measurement that represents 6.022 x 10^23 particles (atoms or molecules). A gram, on the other hand, is a unit of mass. While a mole and a gram are related, they are not the same thing.

Q: How do I know if a reaction is complete or not?

A: A reaction is considered complete if all of the reactants have been consumed and the products have been formed. However, in reality, reactions often do not go to completion, and some of the reactants may remain unreacted.

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

A: Some common mistakes to avoid when working with stoichiometry include:

• Not balancing the equation
• Not using the correct coefficients
• Not converting units correctly
• Not considering the limitations of the reaction (e.g. incomplete reactions)

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

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

• Calculating the amount of reactants needed for a reaction
• Determining the yield of a product
• Understanding the limitations of a reaction
• Designing experiments to test hypotheses

Q: What are some common applications of stoichiometry?

A: Some common applications of stoichiometry include:

• Chemical synthesis
• Pharmaceutical manufacturing
• Environmental monitoring
• Materials science

Q: How can I improve my understanding of stoichiometry?

A: To improve your understanding of stoichiometry, try the following:

• Practice solving problems
• Read and understand the balanced equation
• Use online resources and tutorials
• Ask your instructor or a tutor for help

Conclusion

Stoichiometry is a fundamental concept in chemistry that can be used to calculate the amounts of reactants and products in a reaction. By understanding the principles of stoichiometry, you can apply it to a wide range of real-world problems and improve your understanding of chemical reactions.

Discussion

Stoichiometry is a complex topic that requires a deep understanding of chemical reactions and the principles of stoichiometry. By practicing and applying stoichiometry to real-world problems, you can improve your skills and become a more confident chemist.

Limitations

One limitation of this article is that it assumes a basic understanding of chemical reactions and stoichiometry. If you are new to chemistry, you may want to start with a more introductory article or textbook.

Future Directions

Future directions for this article could include exploring more advanced topics in stoichiometry, such as:

• Calculating the energy released or absorbed in a reaction
• Understanding the kinetics of a reaction
• Designing experiments to test hypotheses

References

• [1] "Chemical Reactions and Stoichiometry". Chemistry LibreTexts.
• [2] "Balanced Chemical Equations". Chemistry LibreTexts.

Keywords

• Stoichiometry
• Chemical reactions
• Balanced equations
• Molar mass
• Moles
• Chemical equations