Combustion of 1 mol of octane results in the formation of 8 mol of carbon dioxide (CO2) . The molar mass of octane is 114.22 g/mol, and the molar mass of carbon dioxide is 44.01 g/mol. If an engine burns 550.0 g octane as it runs, what mass of carbon dioxide is released into the atmosphere?
mols C8H18 = grams/molar mass
mols CO2 = 8x that
g CO2 = mols CO2 molar mass CO2
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To find the mass of carbon dioxide (CO2) released when 550.0 g of octane is burned, we can follow these steps:
Step 1: Calculate the number of moles of octane:
Number of moles = Mass / Molar mass
Number of moles of octane = 550.0 g / 114.22 g/mol
Step 2: Calculate the number of moles of carbon dioxide produced:
According to the given information, the combustion of 1 mole of octane results in the formation of 8 moles of carbon dioxide.
Number of moles of carbon dioxide = Number of moles of octane x 8
Step 3: Calculate the mass of carbon dioxide produced:
Mass = Number of moles x Molar mass
Mass of carbon dioxide = Number of moles of carbon dioxide x Molar mass of carbon dioxide
Now, let's perform the calculations:
Step 1:
Number of moles of octane = 550.0 g / 114.22 g/mol
Number of moles of octane ≈ 4.814 mol
Step 2:
Number of moles of carbon dioxide = Number of moles of octane x 8
Number of moles of carbon dioxide ≈ 4.814 mol x 8
Number of moles of carbon dioxide ≈ 38.512 mol
Step 3:
Mass of carbon dioxide = Number of moles of carbon dioxide x Molar mass of carbon dioxide
Mass of carbon dioxide ≈ 38.512 mol x 44.01 g/mol
Mass of carbon dioxide ≈ 1695.59712 g
Therefore, approximately 1695.6 g of carbon dioxide is released into the atmosphere when 550.0 g of octane is burned.