If 6.0 Moles Of Zinc React With 6.0 Moles Of Hydrochloric Acid In The Equation $\[ \text{Zn} + 2 \text{HCl} \rightarrow \text{ZnCl}_2 + \text{H}_2 \\]what Is The Limiting Reactant?A. \[$\text{H}_2\$\]B. \[$\text{Zn}\$\]C.

by ADMIN 222 views

Introduction

Chemical reactions are a fundamental aspect of chemistry, and understanding the concept of limiting reactants is crucial in determining the outcome of a reaction. In this article, we will explore the concept of limiting reactants and apply it to a specific chemical equation involving zinc and hydrochloric acid.

What are Limiting Reactants?

A limiting reactant is a reactant that is present in a smaller amount than required to complete the reaction. In other words, it is the reactant that determines the maximum amount of product that can be formed. The limiting reactant is the one that is consumed first, and it is the key factor that determines the outcome of the reaction.

The Chemical Equation

The chemical equation for the reaction between zinc and hydrochloric acid is:

{ \text{Zn} + 2 \text{HCl} \rightarrow \text{ZnCl}_2 + \text{H}_2 \}

In this equation, zinc (Zn) reacts with hydrochloric acid (HCl) to form zinc chloride (ZnCl2) and hydrogen gas (H2).

Given Information

We are given that 6.0 moles of zinc react with 6.0 moles of hydrochloric acid. We need to determine which reactant is the limiting reactant.

Step 1: Write the Balanced Equation

To determine the limiting reactant, we need to write the balanced equation for the reaction. The balanced equation is:

{ 2 \text{Zn} + 4 \text{HCl} \rightarrow 2 \text{ZnCl}_2 + 2 \text{H}_2 \}

Step 2: Determine the Mole Ratio

From the balanced equation, we can see that 2 moles of zinc react with 4 moles of hydrochloric acid. Therefore, the mole ratio of zinc to hydrochloric acid is 1:2.

Step 3: Compare the Given Amounts

We are given that 6.0 moles of zinc react with 6.0 moles of hydrochloric acid. To determine the limiting reactant, we need to compare the given amounts with the mole ratio.

Step 4: Determine the Limiting Reactant

Since the mole ratio of zinc to hydrochloric acid is 1:2, we can see that 6.0 moles of zinc would require 12.0 moles of hydrochloric acid to react completely. However, we are given that only 6.0 moles of hydrochloric acid are present. Therefore, hydrochloric acid is the limiting reactant.

Conclusion

In conclusion, the limiting reactant in the reaction between zinc and hydrochloric acid is hydrochloric acid (HCl). This is because the given amount of hydrochloric acid (6.0 moles) is less than the amount required to react with the given amount of zinc (12.0 moles).

Answer

The correct answer is:

B. Zn\text{Zn} is not the limiting reactant, but rather the amount of HCl\text{HCl} is less than the amount required to react with the given amount of Zn\text{Zn}.

Discussion

The concept of limiting reactants is crucial in determining the outcome of a reaction. In this article, we applied the concept to a specific chemical equation involving zinc and hydrochloric acid. We determined that hydrochloric acid is the limiting reactant in this reaction.

Limiting Reactants in Real-World Applications

The concept of limiting reactants has numerous real-world applications. For example, in the production of chemicals, the limiting reactant determines the maximum amount of product that can be formed. In the production of fuels, the limiting reactant determines the maximum amount of fuel that can be produced.

Conclusion

In conclusion, the concept of limiting reactants is a fundamental aspect of chemistry. Understanding the concept is crucial in determining the outcome of a reaction. In this article, we applied the concept to a specific chemical equation involving zinc and hydrochloric acid. We determined that hydrochloric acid is the limiting reactant in this reaction.

References

  • Chemical Equations and Reactions by OpenStax
  • Chemistry: An Atoms First Approach by Steven S. Zumdahl
  • General Chemistry: Principles and Modern Applications by Linus Pauling

Additional Resources

  • Chemical Reactions and Equations by Khan Academy
  • Limiting Reactants by Crash Course
  • Chemical Reactions and Equations by MIT OpenCourseWare
    Chemical Reactions and Limiting Reactants: A Comprehensive Q&A Guide ====================================================================

Introduction

Chemical reactions are a fundamental aspect of chemistry, and understanding the concept of limiting reactants is crucial in determining the outcome of a reaction. In this article, we will provide a comprehensive Q&A guide on chemical reactions and limiting reactants.

Q1: What is a limiting reactant?

A limiting reactant is a reactant that is present in a smaller amount than required to complete the reaction. In other words, it is the reactant that determines the maximum amount of product that can be formed.

Q2: How do I determine the limiting reactant in a reaction?

To determine the limiting reactant, you need to:

  1. Write the balanced equation for the reaction.
  2. Determine the mole ratio of the reactants.
  3. Compare the given amounts of the reactants with the mole ratio.
  4. Identify the reactant that is present in the smallest amount.

Q3: What is the difference between a limiting reactant and an excess reactant?

A limiting reactant is a reactant that is present in a smaller amount than required to complete the reaction, while an excess reactant is a reactant that is present in a larger amount than required to complete the reaction.

Q4: Can a reactant be both a limiting reactant and an excess reactant at the same time?

No, a reactant cannot be both a limiting reactant and an excess reactant at the same time. If a reactant is present in a smaller amount than required to complete the reaction, it is a limiting reactant. If a reactant is present in a larger amount than required to complete the reaction, it is an excess reactant.

Q5: How do I determine the amount of product that can be formed in a reaction?

To determine the amount of product that can be formed in a reaction, you need to:

  1. Identify the limiting reactant.
  2. Determine the mole ratio of the reactants.
  3. Calculate the amount of product that can be formed using the mole ratio.

Q6: What is the significance of limiting reactants in real-world applications?

Limiting reactants have numerous real-world applications, including:

  1. Production of chemicals: The limiting reactant determines the maximum amount of product that can be formed.
  2. Production of fuels: The limiting reactant determines the maximum amount of fuel that can be produced.
  3. Food production: The limiting reactant determines the maximum amount of food that can be produced.

Q7: Can a reaction have multiple limiting reactants?

No, a reaction cannot have multiple limiting reactants. A limiting reactant is a reactant that is present in a smaller amount than required to complete the reaction. If multiple reactants are present in smaller amounts than required to complete the reaction, it is not possible to determine a single limiting reactant.

Q8: How do I handle a reaction with multiple reactants and multiple products?

To handle a reaction with multiple reactants and multiple products, you need to:

  1. Write the balanced equation for the reaction.
  2. Determine the mole ratio of the reactants.
  3. Identify the limiting reactant.
  4. Calculate the amount of each product that can be formed using the mole ratio.

Q9: Can a reaction have a limiting reactant that is not present in the reaction mixture?

No, a reaction cannot have a limiting reactant that is not present in the reaction mixture. A limiting reactant is a reactant that is present in a smaller amount than required to complete the reaction. If a reactant is not present in the reaction mixture, it cannot be a limiting reactant.

Q10: How do I determine the rate of a reaction?

To determine the rate of a reaction, you need to:

  1. Measure the amount of product formed over time.
  2. Plot a graph of the amount of product formed against time.
  3. Determine the slope of the graph, which represents the rate of the reaction.

Conclusion

In conclusion, understanding the concept of limiting reactants is crucial in determining the outcome of a reaction. By following the steps outlined in this Q&A guide, you can determine the limiting reactant in a reaction and calculate the amount of product that can be formed.

References

  • Chemical Equations and Reactions by OpenStax
  • Chemistry: An Atoms First Approach by Steven S. Zumdahl
  • General Chemistry: Principles and Modern Applications by Linus Pauling

Additional Resources

  • Chemical Reactions and Equations by Khan Academy
  • Limiting Reactants by Crash Course
  • Chemical Reactions and Equations by MIT OpenCourseWare