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 given balanced equation shows the formation of sulfur dioxide:

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 (O2) to produce one mole of sulfur dioxide (SO2). 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

To determine the number of moles of sulfur needed 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 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.

In this case, the mole ratio between sulfur and sulfur dioxide is 1:1, meaning that one mole of sulfur produces one mole of sulfur dioxide. To produce 15.0 mol of sulfur dioxide, we need to know how many moles of sulfur are required.

Calculating the Number of Moles of Sulfur

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 is 1:1, we can set up a proportion to relate the number of moles of sulfur to the number of moles of sulfur dioxide:

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.

Conclusion

In conclusion, the balanced equation for the formation of sulfur dioxide is:

S+O2→SO2{ S + O_2 \rightarrow SO_2 }

The mole ratio between sulfur and sulfur dioxide is 1:1, meaning that one mole of sulfur produces one mole of sulfur dioxide. To produce 15.0 mol of sulfur dioxide, we need 15.0 mol of sulfur.

Answer

The correct answer is:

C. 15.0 mol

Additional Information

  • The balanced equation is essential in understanding the stoichiometry of the reaction.
  • The mole ratio between sulfur and sulfur dioxide is 1:1.
  • To produce 15.0 mol of sulfur dioxide, we need 15.0 mol of sulfur.

References

Q&A: The Formation 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+O2→SO2{ S + O_2 \rightarrow SO_2 }

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

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 needed to produce 15.0 mol of sulfur dioxide?

A: To produce 15.0 mol of sulfur dioxide, we need 15.0 mol of sulfur.

Q: What is the relationship between the amounts of reactants and products in a chemical reaction?

A: The relationship between the amounts of reactants and products in a chemical reaction is known as stoichiometry.

Q: What is the importance of the balanced equation in understanding the stoichiometry of a reaction?

A: The balanced equation is essential in understanding the stoichiometry of a reaction, as it provides the mole ratio between the reactants and products.

Q: How can we use the mole ratio to calculate the number of moles of a substance needed to produce a certain amount of another substance?

A: We can use the mole ratio to calculate the number of moles of a substance needed to produce a certain amount of another substance by setting up a proportion and solving for the unknown variable.

Q: What is the correct answer to the question of how many moles of sulfur are needed to produce 15.0 mol of sulfur dioxide?

A: The correct answer is:

C. 15.0 mol

Additional Information

  • The balanced equation is essential in understanding the stoichiometry of the reaction.
  • The mole ratio between sulfur and sulfur dioxide is 1:1.
  • To produce 15.0 mol of sulfur dioxide, we need 15.0 mol of sulfur.

References

Frequently Asked Questions

  • 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: How many moles of sulfur are needed to produce 15.0 mol of sulfur dioxide? A: To produce 15.0 mol of sulfur dioxide, we need 15.0 mol of sulfur.

  • Q: What is the mole ratio between sulfur and sulfur dioxide in the balanced equation? A: The mole ratio between sulfur and sulfur dioxide is 1:1, meaning that one mole of sulfur produces one mole of sulfur dioxide.

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