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The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane (C8H18)

and calculate how many kilograms of carbon dioxide are added to the atmosphere per 3.6 kg
of octane burned. ( Hint
: Begin by writing a balanced equation for the combustion reaction.)

User Ymotov
by
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1 Answer

3 votes

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.

User Banncee
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