Consider The Reaction Below.$\[ 2 C_6 H_{14} + 19 O_2 \rightarrow 12 CO_2 + 14 H_2 O \\]How Many Moles Of Hexane \[$( C_6 H_{14} )\$\] Must Burn To Form 18.4 Mol Of Carbon Dioxide?A. 1.53 Mol B. 3.07 Mol C. 110. Mol D. 175. Mol

by ADMIN 233 views

Understanding the Chemical Reaction

The given chemical reaction is:

2C6H14+19O2→12CO2+14H2O{ 2 C_6 H_{14} + 19 O_2 \rightarrow 12 CO_2 + 14 H_2 O }

This reaction represents the combustion of hexane (C6H14) in the presence of oxygen (O2) to produce carbon dioxide (CO2) and water (H2O).

Balancing the Chemical Equation

To balance the chemical equation, we need to ensure that the number of atoms of each element is the same on both the reactant and product sides. The balanced equation is:

2C6H14+19O2→12CO2+14H2O{ 2 C_6 H_{14} + 19 O_2 \rightarrow 12 CO_2 + 14 H_2 O }

Determining the Mole Ratio

From the balanced equation, we can see that 2 moles of hexane (C6H14) produce 12 moles of carbon dioxide (CO2). To find the mole ratio, we can divide the number of moles of CO2 by the number of moles of C6H14:

Mole ratio = moles of CO2 / moles of C6H14 = 12 mol / 2 mol = 6

This means that for every 1 mole of hexane, 6 moles of carbon dioxide are produced.

Calculating the Number of Moles of Hexane

We are given that 18.4 mol of carbon dioxide is produced. To find the number of moles of hexane required to produce this amount of CO2, we can use the mole ratio:

moles of C6H14 = moles of CO2 / mole ratio = 18.4 mol / 6 = 3.07 mol

Therefore, 3.07 mol of hexane must burn to form 18.4 mol of carbon dioxide.

Conclusion

In this article, we have demonstrated how to balance a chemical equation and use the mole ratio to calculate the number of moles of a reactant required to produce a given amount of product. By following these steps, we can solve stoichiometry problems and gain a deeper understanding of chemical reactions.

Key Takeaways

  • Balancing a chemical equation involves ensuring that the number of atoms of each element is the same on both the reactant and product sides.
  • The mole ratio can be used to calculate the number of moles of a reactant required to produce a given amount of product.
  • Stoichiometry is a crucial concept in chemistry that helps us understand the quantitative relationships between reactants and products in chemical reactions.

Frequently Asked Questions

  • What is the mole ratio of hexane to carbon dioxide in the given reaction?
    • The mole ratio is 1:6, meaning that 1 mole of hexane produces 6 moles of carbon dioxide.
  • How many moles of hexane are required to produce 18.4 mol of carbon dioxide?
    • 3.07 mol of hexane are required to produce 18.4 mol of carbon dioxide.

Additional Resources

  • For more information on balancing chemical equations and stoichiometry, refer to the following resources:
    • Chemistry textbooks and online resources
    • Online tutorials and video lectures
    • Practice problems and worksheets
      Q&A: Balancing Chemical Equations and Stoichiometry =====================================================

Frequently Asked Questions

Q1: What is the purpose of balancing a chemical equation?

A: The purpose of balancing a chemical equation is to ensure that the number of atoms of each element is the same on both the reactant and product sides. This is crucial in understanding the quantitative relationships between reactants and products in chemical reactions.

Q2: How do I balance a chemical equation?

A: To balance a chemical equation, follow these steps:

  1. Write the unbalanced equation.
  2. Count the number of atoms of each element on both the reactant and product sides.
  3. Add coefficients (numbers in front of the formulas of reactants or products) to balance the equation.
  4. Check that the number of atoms of each element is the same on both sides.

Q3: What is the mole ratio in a chemical reaction?

A: The mole ratio is the ratio of the number of moles of one substance to the number of moles of another substance in a chemical reaction. It is used to calculate the number of moles of a reactant required to produce a given amount of product.

Q4: How do I calculate the number of moles of a reactant required to produce a given amount of product?

A: To calculate the number of moles of a reactant required to produce a given amount of product, use the mole ratio:

moles of reactant = moles of product / mole ratio

Q5: 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 calculating the amounts of reactants and products required to produce a given amount of product.

Q6: Why is stoichiometry important in chemistry?

A: Stoichiometry is important in chemistry because it helps us understand the quantitative relationships between reactants and products in chemical reactions. This is crucial in designing and optimizing chemical processes, predicting the yields of products, and understanding the environmental impact of chemical reactions.

Q7: How do I apply stoichiometry in real-world scenarios?

A: Stoichiometry is applied in various real-world scenarios, including:

  • Designing and optimizing chemical processes
  • Predicting the yields of products
  • Understanding the environmental impact of chemical reactions
  • Calculating the amounts of reactants and products required to produce a given amount of product

Q8: What are some common mistakes to avoid when balancing chemical equations?

A: Some common mistakes to avoid when balancing chemical equations include:

  • Not counting the number of atoms of each element on both the reactant and product sides
  • Not adding coefficients to balance the equation
  • Not checking that the number of atoms of each element is the same on both sides

Q9: How do I check if a chemical equation is balanced?

A: To check if a chemical equation is balanced, count the number of atoms of each element on both the reactant and product sides. If the number of atoms of each element is the same on both sides, the equation is balanced.

Q10: What are some resources available for learning more about balancing chemical equations and stoichiometry?

A: Some resources available for learning more about balancing chemical equations and stoichiometry include:

  • Chemistry textbooks and online resources
  • Online tutorials and video lectures
  • Practice problems and worksheets

Conclusion

Balancing chemical equations and stoichiometry are crucial concepts in chemistry that help us understand the quantitative relationships between reactants and products in chemical reactions. By following the steps outlined in this article, you can master these concepts and apply them in real-world scenarios.