# Write the balanced equation for the combustion of isooctane (C8H18) to produce carbon dioxide and...

## Question:

Write the balanced equation for the combustion of isooctane ({eq}C_8H_{18} {/eq}) to produce carbon dioxide and water. Use the smallest possible integers to balance the equation. Also, separate the + sign with 1 space.

Remember that a combustion reaction requires oxygen.

Use the smallest whole number coefficients in your balanced equation.

Write the reactants in the order isooctane then oxygen. Write the products in the order carbon dioxide then water.

Assuming gasoline is 90.0% isooctane, with a density of 0.692 g/mL, what is the theoretical yield (in grams) of CO{eq}_2 {/eq} produced by the combustion of 1.66 x 10{eq}^1 {/eq}{eq}^0 {/eq} gallons of gasoline (the estimated annual consumption of gasoline in the U.S.)?

Remember, there are 3.785 liters in 1 gallon and assume that isooctane is the only carbon containing component of gasoline.

## Combustion

Combustion is a chemical reaction in the presence of oxygen which yields water and carbon dioxide as product. This is an exothermic reaction since it expels energy in the process.

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Balanced chemical reaction

{eq}2C_8H_{18} + 27O_2 \rightarrow 16CO_2 + 18H_2O {/eq}

Convert gallons to liters

{eq}(1.66x10^{10}\,gallons)(3.785\,l...