Final answer:
When 5.00 L of propane gas reacts completely, 0.916 moles of water are produced based on the stoichiometry of the balanced chemical equation and the given density of propane.
Step-by-step explanation:
The question asks how many moles of water (H₂O) form when 5.00 L of propane gas (C₃H₈) completely reacts with oxygen to produce water and carbon dioxide. Propane has a density of 2.02 g/L at room temperature, which will be converted to moles and then used to find the moles of water formed using the stoichiometry from the balanced equation C₃H₈ (g) + 5O2(g) → 3CO₂ (g) + 4H₂O(l).
To calculate the moles of water produced, we first convert the volume of propane to moles. Given the density of propane is 2.02 g/L, 5.00 L of propane weighs 5.00 L × 2.02 g/L = 10.10 g. The molar mass of propane (C₃H₈) is about 44.10 g/mol, so the number of moles of propane is 10.10 g / 44.10 g/mol = 0.229 moles. According to the balanced equation, each mole of propane yields 4 moles of water. Therefore, the moles of water produced are 0.229 moles of C₃H₈ × 4 moles of H₂O/mol of C₃H₈ = 0.916 moles of H₂O.