Question

When table sugar is burned in the air, carbon dioxide and water vapor are products as shown by the following unbalanced equation C₁₂H₂₂O₁₁(s) + O₂(g) → CO₂(g) + H₂O(g). How many moles of oxygen gas are required to react completely with 2.0 moles of sugar?

Answer 1

The balanced equation for the combustion of table sugar is C12H22O11(s) + O2(g) → CO2(g) + H2O(g). To calculate the moles of oxygen gas required to react with 2.0 moles of sugar, we can use stoichiometry. By setting up a proportion and solving for x, we find that 24 moles of O2 are required.

Step-by-step explanation:

When table sugar (sucrose) is burned in the air, carbon dioxide (CO2) and water vapor (H2O) are produced. The unbalanced equation for this reaction is C12H22O11(s) + O2(g) → CO2(g) + H2O(g). In order to determine how many moles of oxygen gas are required to react completely with 2.0 moles of sugar, we can use the stoichiometry of the balanced equation.

By balancing the equation, we find that 12 moles of O2 are required to react completely with 1 mole of sugar. Therefore, to calculate the moles of oxygen gas required to react with 2.0 moles of sugar, we can set up a proportion:

12 moles of O2 / 1 mole of sugar = x moles of O2 / 2.0 moles of sugar

Solving for x, we find that x = 24 moles of O2.