1. Write the Balanced Chemical Equation:
The combustion of octane (C₈H₁₈) produces carbon dioxide (CO₂) and water (H₂O):
2 C₈H₁₈ + 25 O₂ → 16 CO₂ + 18 H₂O
2. Convert Mass of Octane to Moles:
* Molar mass of octane (C₈H₁₈) = 114.23 g/mol
* 1.8 kg octane = 1800 g octane
* Moles of octane = (1800 g) / (114.23 g/mol) = 15.75 mol
3. Use Mole Ratios from the Balanced Equation:
The balanced equation shows that 2 moles of octane produce 16 moles of carbon dioxide.
* Moles of CO₂ = (15.75 mol octane) * (16 mol CO₂ / 2 mol octane) = 126 mol CO₂
4. Convert Moles of CO₂ to Mass:
* Molar mass of CO₂ = 44.01 g/mol
* Mass of CO₂ = (126 mol) * (44.01 g/mol) = 5545.26 g
* Convert grams to kilograms: 5545.26 g = 5.545 kg
Therefore, approximately 5.545 kg of CO₂ is formed from the burning of 1.8 kg of octane.
