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Zhalfirin88
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Homework Statement
Gasoline consists primarily of octane, C8H18
Calculate the mass of CO2 produced from the complete combustion of 3.79 L (1.00 gallon) of gasoline (assume octane, density = 0.756 g/mL) with excess O2
The Attempt at a Solution
The balanced chemical formula would be:
2C8H18 + 25O2 [tex]\rightarrow[/tex] 16CO2 + 18H2O
For my work:
[tex] 3790mL (octane)* \frac{0.756g(octane))}{mL} * \frac{1 mol (octane)}{114.144g (octane)} * \frac{8 mol (CO_2)}{1 mol (octane)} * \frac {44.00g CO_2}{1 mol CO_2} [/tex]
[tex] = 8835.8957g CO_2 [/tex]
Is it correct? What about significant figures?
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