The complete combustion of 3.00 moles of propane (C₃H₈) can be analyzed through its balanced chemical equation:
C₃H₈(g) + 5O₂(g) → 3CO₂(g) + 4H₂O(g)
This equation indicates that for every 1 mole of propane combusted, 5 moles of oxygen are required, producing 3 moles of carbon dioxide and 4 moles of water. Therefore, to determine the quantities involved in the combustion of 3.00 moles of propane, we can use stoichiometric ratios based on the balanced equation.
According to the stoichiometry:
- 3.00 moles of C₃H₈ will react with 5 times that amount of O₂, which is 15.00 moles of O₂.
- The complete combustion will produce 3 times the amount of CO₂, resulting in 9.00 moles of CO₂.
- It will also produce 4 times the amount of H₂O, which amounts to 12.00 moles of H₂O.
In summary, the correct statements about the complete combustion of 3.00 moles of propane include:
- It requires 15.00 moles of oxygen.
- It produces 9.00 moles of carbon dioxide.
- It produces 12.00 moles of water.
These values are derived directly from the stoichiometric relationships established in the balanced equation, confirming the quantities produced and consumed during the reaction.