# 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.

## Answer and Explanation: 1

Become a Study.com member to unlock this answer! Create your account

View this answerBalanced 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...

See full answer below.

#### Learn more about this topic:

from

Chapter 3 / Lesson 4Learn the combustion reaction definition and what happens in a combustion reaction. Understand the combustion reaction equation and examples of combustion in everyday life.