To determine how many grams of carbon dioxide (CO2) can be produced by burning 4.33 moles of propane (C3H8), you'll need to use the balanced chemical equation for the combustion of propane and the stoichiometry of the reaction.
The balanced chemical equation for the combustion of propane is:
C3H8 + 5 O2 → 3 CO2 + 4 H2O
From this equation, you can see that 1 mole of propane (C3H8) produces 3 moles of carbon dioxide (CO2).
Now, calculate the moles of CO2 produced from 4.33 moles of propane:
Moles of CO2 = 4.33 moles of propane × (3 moles of CO2 / 1 mole of propane)
Moles of CO2 = 4.33 moles × 3 ≈ 13 moles of CO2
Next, convert moles of CO2 to grams using the molar mass of carbon dioxide (CO2):
Molar mass of CO2 = (12.01 g/mol for carbon + 2 * 16.00 g/mol for oxygen) = 44.01 g/mol
Grams of CO2 = Moles of CO2 × Molar mass of CO2
Grams of CO2 = 13 moles × 44.01 g/mol ≈ 572.13 grams
So, approximately 572.13 grams of carbon dioxide can be produced by burning 4.33 moles of propane when oxygen is the excess reactant.