Answer:
11.09 kg
Step-by-step explanation:
The balanced equation for the combustion of octane (C8H18) can be written as follows:
2 C8H18 + 25 O2 -> 16 CO2 + 18 H2O
From the balanced equation, we can see that for every 2 moles of octane burned, 16 moles of carbon dioxide (CO2) are produced.
Now, let's calculate the molar mass of octane (C8H18) and carbon dioxide (CO2):
Molar mass of octane (C8H18) = (8 * atomic mass of carbon) + (18 * atomic mass of hydrogen)
= (8 * 12.01 g/mol) + (18 * 1.01 g/mol)
= 96.08 g/mol + 18.18 g/mol
= 114.26 g/mol
Molar mass of carbon dioxide (CO2) = (atomic mass of carbon) + (2 * atomic mass of oxygen)
= 12.01 g/mol + (2 * 16.00 g/mol)
= 12.01 g/mol + 32.00 g/mol
= 44.01 g/mol
Now, we can calculate the number of moles of octane in 3.6 kg:
Number of moles of octane = (mass of octane) / (molar mass of octane)
= (3.6 kg) / (114.26 g/mol)
= 3.6 kg / 0.11426 kg/mol
= 31.51 mol
Since the balanced equation shows that for every 2 moles of octane, 16 moles of carbon dioxide are produced, we can calculate the number of moles of carbon dioxide produced:
Number of moles of carbon dioxide = (Number of moles of octane) * (16 moles of CO2 / 2 moles of octane)
= 31.51 mol * (16 mol CO2 / 2 mol octane)
= 252.08 mol
Finally, we can calculate the mass of carbon dioxide produced:
Mass of carbon dioxide = (Number of moles of carbon dioxide) * (molar mass of carbon dioxide)
= 252.08 mol * 44.01 g/mol
= 11,086.93 g
≈ 11.09 kg
Therefore, approximately 11.09 kilograms of carbon dioxide are added to the atmosphere per 3.6 kilograms of octane burned.