In the combustion of carbon, according to the reaction C + O_2 → CO_2, how many moles of oxygen gas (O_2) are required to produce 7.00 moles of carbon dioxide (CO_2)?

• A. 1.00 mole
• B. 7.00 moles
• C. 3.50 moles
• D. 14.0 moles

Answer: (B)

Verified step by step guidance

1. Write down the balanced chemical equation for the combustion of carbon: \(\mathrm{C} + \mathrm{O}_2 \rightarrow \mathrm{CO}_2\).
2. Identify the mole ratio between oxygen gas (\(\mathrm{O}_2\)) and carbon dioxide (\(\mathrm{CO}_2\)) from the balanced equation. Here, 1 mole of \(\mathrm{O}_2\) produces 1 mole of \(\mathrm{CO}_2\).
3. Set up a proportion using the mole ratio to find the moles of \(\mathrm{O}_2\) needed to produce 7.00 moles of \(\mathrm{CO}_2\).
4. Calculate the moles of \(\mathrm{O}_2\) by multiplying the given moles of \(\mathrm{CO}_2\) by the mole ratio of \(\mathrm{O}_2\) to \(\mathrm{CO}_2\).
5. Interpret the result as the number of moles of oxygen gas required for the combustion to produce 7.00 moles of carbon dioxide.