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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The Formation of Sulfur Dioxide: A Balanced Equation

Understanding the Balanced Equation

The balanced equation for the formation of sulfur dioxide is given as: ${ S + O_2 \rightarrow SO_2 }$. This equation indicates that one mole of sulfur (S) reacts with one mole of oxygen gas (O2) to produce one mole of sulfur dioxide (SO2). In this article, we will explore how many moles of sulfur are needed to produce 15.0 mol of sulfur dioxide.

The Mole Ratio

To determine the number of moles of sulfur required to produce 15.0 mol of sulfur dioxide, we need to examine the mole ratio between sulfur and sulfur dioxide in the balanced equation. The balanced equation shows that one mole of sulfur produces one mole of sulfur dioxide. This means that the mole ratio between sulfur and sulfur dioxide is 1:1.

Calculating the Number of Moles of Sulfur

Using the mole ratio, we can calculate the number of moles of sulfur required to produce 15.0 mol of sulfur dioxide. Since the mole ratio is 1:1, we can set up a proportion to solve for the number of moles of sulfur:

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 and divide:

x=1 mol S×15.0 mol SO21 mol SO2{ x = \frac{1 \text{ mol S} \times 15.0 \text{ mol SO}_2}{1 \text{ mol SO}_2} }

x=15.0 mol S{ x = 15.0 \text{ mol S} }

Therefore, 15.0 mol of sulfur are required to produce 15.0 mol of sulfur dioxide.

Conclusion

In conclusion, the balanced equation for the formation of sulfur dioxide shows that one mole of sulfur produces one mole of sulfur dioxide. Using the mole ratio, we can calculate the number of moles of sulfur required to produce 15.0 mol of sulfur dioxide. The result shows that 15.0 mol of sulfur are needed to produce 15.0 mol of sulfur dioxide.

Answer

The correct answer is C. 15.0 mol.

Additional Information

  • The balanced equation for the formation of sulfur dioxide is: ${ S + O_2 \rightarrow SO_2 }$
  • The mole ratio between sulfur and sulfur dioxide is 1:1.
  • 15.0 mol of sulfur are required to produce 15.0 mol of sulfur dioxide.

References

  • Chemistry textbook, chapter 3: Stoichiometry
  • Online resources: Khan Academy, Chemistry LibreTexts

Discussion

This problem requires the application of the mole ratio concept to solve for the number of moles of sulfur required to produce a given amount of sulfur dioxide. The balanced equation provides the necessary information to determine the mole ratio, and the proportion can be set up to solve for the unknown variable. This type of problem is essential in chemistry, as it helps to understand the relationships between different substances and their quantities.

Related Topics

  • Stoichiometry
  • Mole ratio
  • Balanced equations
  • Chemical reactions

Practice Problems

  • How many moles of oxygen gas are required to produce 20.0 mol of sulfur dioxide?
  • What is the mole ratio between sulfur and sulfur trioxide (SO3)?
  • How many moles of sulfur are required to produce 10.0 mol of sulfur dioxide?
    The Formation of Sulfur Dioxide: A Balanced Equation - Q&A

Understanding the Balanced Equation

The balanced equation for the formation of sulfur dioxide is given as: ${ S + O_2 \rightarrow SO_2 }$. This equation indicates that one mole of sulfur (S) reacts with one mole of oxygen gas (O2) to produce one mole of sulfur dioxide (SO2). In this article, we will explore how many moles of sulfur are needed to produce 15.0 mol of sulfur dioxide.

Q&A

Q: What is the mole ratio between sulfur and sulfur dioxide?

A: The mole ratio between sulfur and sulfur dioxide is 1:1, meaning that one mole of sulfur produces one mole of sulfur dioxide.

Q: How many moles of sulfur are required to produce 15.0 mol of sulfur dioxide?

A: Using the mole ratio, we can calculate the number of moles of sulfur required to produce 15.0 mol of sulfur dioxide. Since the mole ratio is 1:1, we can set up a proportion to solve for the number of moles of sulfur:

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 and divide:

x=1 mol S×15.0 mol SO21 mol SO2{ x = \frac{1 \text{ mol S} \times 15.0 \text{ mol SO}_2}{1 \text{ mol SO}_2} }

x=15.0 mol S{ x = 15.0 \text{ mol S} }

Therefore, 15.0 mol of sulfur are required to produce 15.0 mol of sulfur dioxide.

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

A: The balanced equation for the formation of sulfur dioxide is: ${ S + O_2 \rightarrow SO_2 }$

Q: What is the mole ratio between sulfur and sulfur trioxide (SO3)?

A: The mole ratio between sulfur and sulfur trioxide (SO3) is not provided in the balanced equation for the formation of sulfur dioxide. However, we can determine the mole ratio by examining the balanced equation for the formation of sulfur trioxide, which is: ${ S + 3O_2 \rightarrow SO_3 }$. The mole ratio between sulfur and sulfur trioxide is 1:3.

Q: How many moles of oxygen gas are required to produce 20.0 mol of sulfur dioxide?

A: Using the mole ratio, we can calculate the number of moles of oxygen gas required to produce 20.0 mol of sulfur dioxide. Since the mole ratio is 1:1, we can set up a proportion to solve for the number of moles of oxygen gas:

1 mol O21 mol SO2=x mol O220.0 mol SO2{ \frac{1 \text{ mol O}_2}{1 \text{ mol SO}_2} = \frac{x \text{ mol O}_2}{20.0 \text{ mol SO}_2} }

To solve for x, we can cross-multiply and divide:

x=1 mol O2×20.0 mol SO21 mol SO2{ x = \frac{1 \text{ mol O}_2 \times 20.0 \text{ mol SO}_2}{1 \text{ mol SO}_2} }

x=20.0 mol O2{ x = 20.0 \text{ mol O}_2 }

Therefore, 20.0 mol of oxygen gas are required to produce 20.0 mol of sulfur dioxide.

Conclusion

In conclusion, the balanced equation for the formation of sulfur dioxide shows that one mole of sulfur produces one mole of sulfur dioxide. Using the mole ratio, we can calculate the number of moles of sulfur required to produce a given amount of sulfur dioxide. The Q&A section provides additional information and answers to common questions related to the formation of sulfur dioxide.

Answer

The correct answers are:

  • Q1: The mole ratio between sulfur and sulfur dioxide is 1:1.
  • Q2: 15.0 mol of sulfur are required to produce 15.0 mol of sulfur dioxide.
  • Q3: The balanced equation for the formation of sulfur dioxide is: ${ S + O_2 \rightarrow SO_2 }$
  • Q4: The mole ratio between sulfur and sulfur trioxide is 1:3.
  • Q5: 20.0 mol of oxygen gas are required to produce 20.0 mol of sulfur dioxide.

Additional Information

  • The balanced equation for the formation of sulfur dioxide is: ${ S + O_2 \rightarrow SO_2 }$
  • The mole ratio between sulfur and sulfur dioxide is 1:1.
  • 15.0 mol of sulfur are required to produce 15.0 mol of sulfur dioxide.
  • The mole ratio between sulfur and sulfur trioxide is 1:3.
  • 20.0 mol of oxygen gas are required to produce 20.0 mol of sulfur dioxide.

References

  • Chemistry textbook, chapter 3: Stoichiometry
  • Online resources: Khan Academy, Chemistry LibreTexts

Discussion

This Q&A article provides additional information and answers to common questions related to the formation of sulfur dioxide. The balanced equation and mole ratio are essential concepts in chemistry, and understanding these concepts is crucial for solving problems related to chemical reactions.

Related Topics

  • Stoichiometry
  • Mole ratio
  • Balanced equations
  • Chemical reactions

Practice Problems

  • How many moles of sulfur are required to produce 10.0 mol of sulfur dioxide?
  • What is the mole ratio between sulfur and sulfur trioxide (SO3)?
  • How many moles of oxygen gas are required to produce 15.0 mol of sulfur dioxide?