The Following Balanced Equation Shows The Formation Of Sulfur Dioxide:${ S + O_2 \rightarrow SO_2 }$How Many Moles Of Sulfur Are Needed To Produce 15.0 Mol Of Sulfur Dioxide?A. 7.50 Mol B. 10.5 Mol C. 15.0 Mol D. 30.0 Mol

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Understanding the Balanced Equation

The balanced equation for the formation of sulfur dioxide is given as:

S+O2→SO2{ S + O_2 \rightarrow SO_2 }

This equation indicates that one mole of sulfur (S) reacts with one mole of oxygen gas (O_2) to produce one mole of sulfur dioxide (SO_2). The balanced equation is essential in understanding the stoichiometry of the reaction, which is the relationship between the amounts of reactants and products.

Stoichiometry and Mole Ratios

Stoichiometry is a crucial concept in chemistry that helps us understand the quantitative relationships between reactants and products in chemical reactions. In this case, the balanced equation shows that one mole of sulfur reacts with one mole of oxygen to produce one mole of sulfur dioxide. This means that the mole ratio of sulfur to sulfur dioxide is 1:1.

Calculating the Number of Moles of Sulfur Needed

To calculate the number of moles of sulfur needed to produce 15.0 mol of sulfur dioxide, we can use the mole ratio from the balanced equation. Since the mole ratio of sulfur to sulfur dioxide is 1:1, we can set up a proportion to solve for the number of moles of sulfur needed:

1 mol S1 mol SO2=x mol S15.0 mol SO2{ \frac{1 \text{ mol S}}{1 \text{ mol SO}_2} = \frac{x \text{ mol S}}{15.0 \text{ mol SO}_2} }

To solve for x, we can cross-multiply:

1×15.0=1×x{ 1 \times 15.0 = 1 \times x }

15.0=x{ 15.0 = x }

Therefore, the number of moles of sulfur needed to produce 15.0 mol of sulfur dioxide is 15.0 mol.

Answer and Explanation

The correct answer is C. 15.0 mol.

The balanced equation shows that one mole of sulfur reacts with one mole of oxygen to produce one mole of sulfur dioxide. Therefore, to produce 15.0 mol of sulfur dioxide, we need 15.0 mol of sulfur.

Conclusion

In conclusion, the balanced equation for the formation of sulfur dioxide is essential in understanding the stoichiometry of the reaction. By using the mole ratio from the balanced equation, we can calculate the number of moles of sulfur needed to produce a given amount of sulfur dioxide. In this case, we found that 15.0 mol of sulfur is needed to produce 15.0 mol of sulfur dioxide.

Additional Information

  • The balanced equation can be used to calculate the number of moles of oxygen needed to produce a given amount of sulfur dioxide.
  • The mole ratio from the balanced equation can be used to calculate the number of moles of sulfur dioxide produced from a given amount of sulfur.
  • The balanced equation can be used to calculate the number of moles of sulfur dioxide produced from a given amount of oxygen.

References

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

Discussion

What is the balanced equation for the formation of sulfur dioxide?

What is the mole ratio of sulfur to sulfur dioxide in the balanced equation?

How can the balanced equation be used to calculate the number of moles of sulfur needed to produce a given amount of sulfur dioxide?

What is the correct answer to the problem?

How can the balanced equation be used to calculate the number of moles of oxygen needed to produce a given amount of sulfur dioxide?

How can the mole ratio from the balanced equation be used to calculate the number of moles of sulfur dioxide produced from a given amount of sulfur?

Q&A: Understanding the Balanced Equation

Q: What is the balanced equation for the formation of sulfur dioxide?

A: The balanced equation for the formation of sulfur dioxide is:

S+O2→SO2{ S + O_2 \rightarrow SO_2 }

Q: What is the mole ratio of sulfur to sulfur dioxide in the balanced equation?

A: The mole ratio of sulfur to sulfur dioxide in the balanced equation is 1:1. This means that one mole of sulfur reacts with one mole of oxygen to produce one mole of sulfur dioxide.

Q: How can the balanced equation be used to calculate the number of moles of sulfur needed to produce a given amount of sulfur dioxide?

A: To calculate the number of moles of sulfur needed to produce a given amount of sulfur dioxide, we can use the mole ratio from the balanced equation. Since the mole ratio of sulfur to sulfur dioxide is 1:1, we can set up a proportion to solve for the number of moles of sulfur needed.

Q: What is the correct answer to the problem?

A: The correct answer is C. 15.0 mol.

Q: How can the balanced equation be used to calculate the number of moles of oxygen needed to produce a given amount of sulfur dioxide?

A: To calculate the number of moles of oxygen needed to produce a given amount of sulfur dioxide, we can use the mole ratio from the balanced equation. Since the mole ratio of sulfur to sulfur dioxide is 1:1, we can set up a proportion to solve for the number of moles of oxygen needed.

Q: How can the mole ratio from the balanced equation be used to calculate the number of moles of sulfur dioxide produced from a given amount of sulfur?

A: To calculate the number of moles of sulfur dioxide produced from a given amount of sulfur, we can use the mole ratio from the balanced equation. Since the mole ratio of sulfur to sulfur dioxide is 1:1, we can set up a proportion to solve for the number of moles of sulfur dioxide produced.

Q: How can the balanced equation be used to calculate the number of moles of sulfur dioxide produced from a given amount of oxygen?

A: To calculate the number of moles of sulfur dioxide produced from a given amount of oxygen, we can use the mole ratio from the balanced equation. Since the mole ratio of sulfur to sulfur dioxide is 1:1, we can set up a proportion to solve for the number of moles of sulfur dioxide produced.

Q: What are some common applications of the balanced equation?

A: The balanced equation has many common applications in chemistry, including:

  • Calculating the number of moles of reactants and products in a chemical reaction
  • Determining the limiting reactant in a chemical reaction
  • Calculating the yield of a chemical reaction
  • Determining the number of moles of a product formed from a given amount of reactant

Q: What are some common mistakes to avoid when using the balanced equation?

A: Some common mistakes to avoid when using the balanced equation include:

  • Not balancing the equation correctly
  • Not using the correct mole ratio
  • Not setting up the correct proportion
  • Not solving for the correct variable

Q: How can I practice using the balanced equation?

A: You can practice using the balanced equation by working through example problems and exercises. You can also try using the balanced equation to solve real-world problems and applications.

Q: What are some resources for learning more about the balanced equation?

A: Some resources for learning more about the balanced equation include:

  • Chemistry textbooks and online resources
  • Online tutorials and videos
  • Practice problems and exercises
  • Real-world applications and examples