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?

See your post above.

To find the mass of carbon dioxide released into the atmosphere when burning 550.0 g of octane, we need to use the given information about the molar masses and the stoichiometry of the reaction.

First, we need to determine the number of moles of octane:

number of moles of octane = mass of octane / molar mass of octane

number of moles of octane = 550.0 g / 114.22 g/mol

number of moles of octane ≈ 4.81 mol

According to the stoichiometry of the combustion reaction, 1 mol of octane produces 8 mol of carbon dioxide. So, we can calculate the moles of carbon dioxide produced:

number of moles of carbon dioxide = number of moles of octane * (8 mol of CO2 / 1 mol of octane)

number of moles of carbon dioxide = 4.81 mol * 8

number of moles of carbon dioxide ≈ 38.48 mol

Finally, to calculate the mass of carbon dioxide, we multiply the number of moles by the molar mass of carbon dioxide:

mass of carbon dioxide = number of moles of carbon dioxide * molar mass of carbon dioxide

mass of carbon dioxide = 38.48 mol * 44.01 g/mol

mass of carbon dioxide ≈ 1695.13 g

Therefore, when burning 550.0 g of octane, approximately 1695.13 g of carbon dioxide is released into the atmosphere.