Question

When left over a flame a marshmallow is consumed in a combustion reaction. Assuming a marshmallow is made of entirely sucrose, C12H22O11, and after combustion no residual solid remained, the following chemical equation describes this reaction.

C12H22O11(s) + 12 O2(g) → 12 CO2(g) + 11 H2O(g)

Using the chemical equation in Question 1 above, if a second marshmallow was measured and contained 6.94 g of sucrose and is the limiting reactant, what is the theoretical yield, in g, of CO2?

Answer 1

C₁₂H₂₂O₁₁(s) + 12 O₂(g) → 12 CO₂(g) + 11 H₂O(g)

The mass of carbon dioxide produced in the reaction can be calculated as following:

m(CO₂) = m(sucrose) × 12 × Mr(CO₂) / Mr(sucrose) = 6.94 g × 12 × 44 g/mol / 342 g/mol = 10.7 g

Answer: 10.7 g