Propane, C3H8, a fuel used in many outdoor grills, burns in oxygen to produce carbon dioxide gas, CO2, and water vapor, H2O, as shown in the reaction below. If 2.0 mol of propane are burned (reacted with oxygen), how many moles of carbon dioxide will be produced?

• A. 8.0 mol
• B. 4.0 mol
• C. 6.0 mol
• D. 10.0 mol

Answer: (C)

Verified step by step guidance

1. Start by writing the balanced chemical equation for the combustion of propane. The reaction is: $C_3{H}_8+5O_2\to 3{\mathrm{CO}}_2+4H_{2}O$
2. Identify the mole ratio between propane and carbon dioxide from the balanced equation. For every 1 mole of C3H8, 3 moles of CO2 are produced.
3. Determine the number of moles of propane given in the problem, which is 2.0 moles.
4. Use the mole ratio to calculate the moles of carbon dioxide produced. Multiply the moles of propane by the mole ratio: $2.0\times 3=?$
5. Conclude that the calculation will give you the number of moles of carbon dioxide produced when 2.0 moles of propane are burned.