Final answer:
To find the number of moles of CO₂ produced from 79.0 g of C₃H₈, divide the mass of propane by its molar mass to get the number of moles of C₃H₈ and then multiply by 3 (since 3 moles of CO₂ are produced for every mole of C₃H₈) to get the moles of CO₂. None of the given options are correct.
Step-by-step explanation:
The question asks to calculate the number of moles of CO₂ produced from the combustion of 79.0 g of C₃H₈, assuming excess oxygen is available. First, we must determine the molar mass of C₃H₈. Propane (C₃H₈) has a molar mass of approximately 44.09 g/mol. We then calculate how many moles of C₃H₈ we have by dividing the mass of propane by its molar mass: 79.0 g C₃H₈ ÷ 44.09 g/mol = 1.79 mol C₃H₈.
The balanced chemical equation for the combustion of propane is:
C₃H₈ + 5O₂ → 3CO₂ + 4H₂O
This indicates that for each mole of propane burned, three moles of CO₂ are produced. So, we multiply the number of moles of C₃H₈ by 3 to find the moles of CO₂: 1.79 mol C₃H₈ × 3 = 5.37 mol CO₂. Therefore, more than 4.0 moles of CO₂ will be produced, meaning none of the provided answers (A, B, C, or D) are correct.