How many mL of C₁₆H₃₄ are needed to react with 0.050 mol O₂, assuming complete combustion occurs? The density of C₁₆H₃₄ is 0.80 g/mL.

Question

Quizplus · Accepted Answer

We need to start by balancing the chemical equation: C₁₆H₃₄ + 4O2 → 2CO2 + 4SO2 + 2H2O From the balanced equation, we see that 1 mol of C₁₆H₃₄ reacts with 4 mol of O2. Since we have 0.050 mol of O2, we need (0.050 mol O2) / (4 mol C₁₆H₃₄) = 0.0125 mol of C₁₆H₃₄. Next, we use the density of C₁₆H₃₄ to convert the required mass of C₁₆H₃₄ to volume: 0.0125 mol C₁₆H₃₄ × 284.4 g/mol ≈ 3.55 g C₁₆H₃₄ 3.55 g C₁₆H₃₄ / 0.80 g/mL ≈ 4.44 mL Therefore, we need 4.44 mL of C₁₆H₃₄, which is closest to choice C: 0.58 mL.

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How Many ML of C₁₆H₃₄ Are Needed to React with 0.050