Final answer:
To calculate the theoretical yield of CO2 when 1.00 g of glucose is burned, convert the mass of glucose to moles, use the mole ratio to find moles of CO2, and then convert that to grams. The theoretical yield would be 1.464 grams of CO2.
Step-by-step explanation:
To calculate the theoretical yield of carbon dioxide when 1.00 g of glucose is burned, one needs to follow these steps:
- Determine the balanced chemical equation for the reaction, which in this case is: C6H12O6 (glucose) + 6O2 (oxygen) → 6CO2 (carbon dioxide) + 6H2O (water).
- Find the molar mass of glucose and carbon dioxide. The molar mass of glucose (C6H12O6) is 180.16 g/mol, and the molar mass of CO2 is 44.01 g/mol.
- Convert the mass of glucose to moles by dividing by its molar mass. For 1.00 g of glucose, it would be 1.00 g ÷ 180.16 g/mol = 0.00555 mol.
- Use the mole ratio from the balanced equation to calculate moles of CO2 produced from the moles of glucose burned. Since 1 mole of glucose yields 6 moles of CO2, we multiply the moles of glucose by 6.
- Convert the moles of CO2 to grams using the molar mass of CO2. For 0.00555 mol of glucose, the moles of CO2 would be 0.00555 mol × 6 = 0.0333 mol. The mass of CO2 would then be 0.0333 mol × 44.01 g/mol = 1.464 g of CO2.
The theoretical yield of CO2 when 1.00 g of glucose is burned completely is 1.464 grams.