Given the reaction S + O_2 → SO_2, how many moles of sulfur (S) are required to produce 15.0 mol of sulfur dioxide (SO_2)?

• A. 30.0 mol
• B. 7.5 mol
• C. 15.0 mol
• D. 1.0 mol

Answer: (C)

Verified step by step guidance

1. Write the balanced chemical equation for the reaction: \(\mathrm{S} + \mathrm{O}_2 \rightarrow \mathrm{SO}_2\).
2. Identify the mole ratio between sulfur (S) and sulfur dioxide (SO_2) from the balanced equation. Here, 1 mole of S produces 1 mole of SO_2.
3. Use the mole ratio to set up a conversion from moles of SO_2 to moles of S: \(\text{moles of S} = \text{moles of SO}_2 \times \frac{1 \text{ mole S}}{1 \text{ mole SO}_2}\).
4. Substitute the given amount of SO_2 (15.0 mol) into the conversion to find the moles of sulfur required.
5. Interpret the result to conclude how many moles of sulfur are needed to produce 15.0 moles of sulfur dioxide.