🤓 Based on our data, we think this question is relevant for Professor Morkowchuk's class at UVA.

Determine the mass of octane used:

$\mathbf{mass}\mathbf{}{\mathbf{C}}_{\mathbf{8}}{\mathbf{H}}_{\mathbf{18}}\mathbf{=}\mathbf{230}\mathbf{}\overline{)\mathbf{mi}}\left(\frac{1\overline{)\mathrm{gal}}}{21.5\overline{)\mathrm{mi}}}\right)\left(\frac{3.78541\overline{)L}}{1\overline{)\mathrm{gal}}}\right)\left(\frac{1\overline{)\mathrm{mL}}}{{10}^{-3}\overline{)L}}\right)\left(\frac{0.69g}{1\overline{)\mathrm{mL}}}\right)\mathbf{=}$**27941.60777 g C _{8}H**

If an automobile travels 230 mi with a gas mileage of 21.5 mi/gal , how many kilograms of CO_{2} are produced?

Assume that the gasoline is composed of octane, C_{8}H_{18} (l), whose density is 0.69 g/mL.

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Based on our data, we think this problem is relevant for Professor Morkowchuk's class at UVA.