When 5.0 moles of butane (C_4H_{10}) react completely with oxygen, how many moles of carbon dioxide (CO_2) are produced?

• A. 10 moles
• B. 5.0 moles
• C. 2.5 moles
• D. 20 moles

Answer: (D)

Verified step by step guidance

1. Write the balanced chemical equation for the complete combustion of butane (C_4H_{10}). The general form for combustion of a hydrocarbon is: \(C_xH_y + O_2 \rightarrow CO_2 + H_2O\). For butane, balance the equation: \$2C_4H_{10} + 13O_2 \rightarrow 8CO_2 + 10H_2O$.
2. Identify the mole ratio between butane and carbon dioxide from the balanced equation. According to the equation, 2 moles of butane produce 8 moles of carbon dioxide.
3. Set up a proportion to find the moles of carbon dioxide produced from 5.0 moles of butane using the mole ratio: \(\frac{2 \text{ moles } C_4H_{10}}{8 \text{ moles } CO_2} = \frac{5.0 \text{ moles } C_4H_{10}}{x \text{ moles } CO_2}\).
4. Solve the proportion for \(x\) to find the moles of carbon dioxide produced: \(x = \frac{8}{2} \times 5.0\) moles of \(CO_2\).
5. Interpret the result to understand how many moles of carbon dioxide are produced when 5.0 moles of butane react completely with oxygen.