Diesel fuel for automobiles and trucks is a mixture of hydrocarbons that can be modeled by C₁₆H₃₄.How many mL of C₁₆H₃₄ are needed to react with 1.00 mol O₂? The density of C₁₆H₃₄ is 0.773 g/mL and its molar mass is 226 g/mol.

Question

Quizplus · Accepted Answer

Step 1: Find the molar mass of C₁₆H₃₄ molar mass = (11 x 12.01 g/mol) + (1 x 1.01 g/mol) + (16 x 32.06 g/mol) + (1 x 1.01 g/mol) + (34 x 1.01 g/mol) + (1 x 32.06 g/mol) + (1 x 1.01 g/mol) + (34 x 1.01 g/mol) = 226 g/mol Step 2: Use the balanced equation to determine the mole ratio between C₁₆H₃₄ and O₂ C₁₆H₃₄ + 15O₂ → 8CO2 + 9H2O + 15SO2 1 mol C₁₆H₃₄ : 15 mol O₂ Step 3: Convert 1.00 mol O₂ to mol C₁₆H₃₄ using the mole ratio 1.00 mol O₂ x (1 mol C₁₆H₃₄ / 15 mol O₂) = 0.06667 mol C₁₆H₃₄ Step 4: Convert mol of C₁₆H₃₄ to mL using the density of C₁₆H₃₄ 0.06667 mol C₁₆H₃₄ x (226 g/mol / 0.773 g/mL) x (1 mL/1.00 g) = 11.9 mL C₁₆H₃₄

Diesel Fuel for Automobiles and Trucks Is a Mixture of Hydrocarbons