The balanced equation for burning octane is: 2 C₈H₁₈(g) + 25 O₂(g) → 18 H₂O(g) + 16 CO₂(g) What weight of H₂O is produced by completely burning 19.8 g of octane?

Question

Quizplus · Accepted Answer

The balanced equation shows that 2 moles of octane produce 18 moles of water. The molar mass of octane is 114.23 g/mol, so 19.8 g of octane is 0.173 mol. This will produce 0.173 mol * 18 mol/2 mol = 1.55 mol of water. The molar mass of water is 18.02 g/mol, so the mass of water produced is 1.55 mol * 18.02 g/mol = 28.1 g.

The Balanced Equation for Burning Octane Is: 2 C8H18(g)

The Balanced Equation for Burning Octane Is: 2 C₈H₁₈(g)