Final answer:
To calculate the grams of CO₂ produced from the combustion of 72.0 g of C₆H₁₄, we use stoichiometry to first find the moles of hexane, then the moles of CO₂ produced, and finally convert moles of CO₂ to grams, resulting in 220.44 g CO₂.
Step-by-step explanation:
To calculate the grams of CO₂ produced from the combustion of 72.0 g of C₆H₁₄, we will perform stoichiometric calculations. The combustion reaction for hexane (C₆H₁₄) can be written as:
2 C₆H₁₄ + 19 O₂ → 12 CO₂ + 14 H₂O
From this balanced equation, we see that 2 moles of hexane produce 12 moles of CO₂. First, we find the number of moles of C₆H₁₄ using its molar mass (86.2 g/mol):
moles of C₆H₁₄ = 72.0 g / 86.2 g/mol = 0.835 mol
Now, using the stoichiometry of the balanced equation, we calculate the moles of CO₂ produced:
moles of CO₂ = 0.835 mol C₆H₁₄ x (12 mol CO₂ / 2 mol C₆H₁₄) = 5.01 mol CO₂
Finally, we convert the moles of CO₂ to grams using the molar mass of CO₂ (44.0 g/mol):
grams of CO₂ = 5.01 mol x 44.0 g/mol = 220.44 g CO₂
First, we need to determine the moles of C6H14. Using the molar mass of C6H14 (86.2 g/mol), we can calculate:
Moles of C6H14 = Mass of C6H14 / Molar mass of C6H14
Moles of C6H14 = 72.0 g / 86.2 g/mol = 0.836 mol C6H14
According to the balanced chemical equation, 1 mol of C6H14 produces 6 mol of CO2. Therefore, the moles of CO2 produced is:
Moles of CO2 = Moles of C6H14 x 6
Moles of CO2 = 0.836 mol C6H14 x 6 = 5.016 mol CO2
To convert the moles of CO2 to grams, we can use the molar mass of CO2 (44.009 g/mol):
Mass of CO2 = Moles of CO2 x Molar mass of CO2
Mass of CO2 = 5.016 mol CO2 x 44.009 g/mol = 220.84 g
Therefore, 220.84 grams of CO2 are produced in the combustion of 72.0 grams of C6H14.