When table sugar is burned in air, carbon dioxide and water vapor are products, as shown by the following unbalanced chemical equation: C₁₂H₂₂O₁₁(s) + O₂(g) $\rightarrow$ CO₂(g) + H₂O(g)
How many moles of oxygen are required to react completely with 1.26 mol of sugar?

Question

When table sugar is burned in air, carbon dioxide and water vapor are products, as shown by the following unbalanced chemical equation: C₁₂H₂₂O₁₁(s) + O₂(g)

\rightarrow

CO₂(g) + H₂O(g)
How many moles of oxygen are required to react completely with 1.26 mol of sugar?

Quizplus · Accepted Answer

The balanced chemical equation for the combustion of sugar (C12H22O11) is C12H22O11(s) + 12O2(g) → 12CO2(g) + 11H2O(g). This shows that 12 moles of oxygen are required for every mole of sugar. Therefore, for 1.26 moles of sugar, (1.26 moles of sugar) * (12 moles of oxygen/1 mole of sugar) = 15.12 moles of oxygen, which rounds to 15.1 moles, making option A correct.

When Table Sugar Is Burned in Air, Carbon Dioxide and Water