how many grams of carbon dioxide can be produced by burning 7.04moles of propane
C3H8 + 7O2 ==> 3CO2 + 4H2O
7.04 mols C3H8 x (7 mols O2/1 mol Propane) = 7.04 x 7/1 = ?
To determine the number of grams of carbon dioxide produced by burning 7.04 moles of propane, we need to employ a balanced chemical equation and use stoichiometry.
The balanced equation for the combustion of propane (C₃H₈) is:
C₃H₈ + 5O₂ → 3CO₂ + 4H₂O
From the equation, we can see that for every 1 mole of propane burned, we produce 3 moles of carbon dioxide. Thus, we can set up a ratio:
3 moles CO₂ / 1 mole C₃H₈
To calculate the number of moles of carbon dioxide produced, multiply the given moles of propane (7.04 moles) by the ratio:
7.04 moles C₃H₈ * (3 moles CO₂ / 1 mole C₃H₈) = 21.12 moles CO₂
Now, to convert moles of carbon dioxide to grams, we use the molar mass of carbon dioxide, which is approximately 44 grams per mole.
21.12 moles CO₂ * 44 grams/mole CO₂ = 929.28 grams CO₂
Therefore, burning 7.04 moles of propane can produce approximately 929.28 grams of carbon dioxide.