Assume that a car burns pure octane, C8 H18 (d = .0.703 g / cm^3) (a) Write the balanced equati

step 1 To calculate the volume of carbon dioxide produced with the combustion of octane, we need a bala

Assume that a car burns pure octane, C8 H18 (d = .0.703 g /...

Assume that a car burns pure octane, $\mathrm{C}_{8} \mathrm{H}_{18}$ (d $=$ $\left.0.703 \mathrm{~g} / \mathrm{cm}^{3}\right)$ (a) Write the balanced equation for burning octane in air, forming $\mathrm{CO}_{2}$ and $\mathrm{H}_{2} \mathrm{O}$. (b) If the car has a fuel efficiency of 32 miles per gallon of octane, what volume of $\mathrm{CO}_{2}$ at $25^{\circ} \mathrm{C}$ and $1.0 \mathrm{~atm}$ is generated when the car goes on a $10 .$ -mile trip?

Assume that a car burns pure octane, $\mathrm{C}_{8} \mathrm{H}_{18}$ (d $=$ $\left.0.703 \mathrm{~g} / \mathrm{cm}^{3}\right)$
(a) Write the balanced equation for burning octane in air, forming $\mathrm{CO}_{2}$ and $\mathrm{H}_{2} \mathrm{O}$.
(b) If the car has a fuel efficiency of 32 miles per gallon of octane, what volume of $\mathrm{CO}_{2}$ at $25^{\circ} \mathrm{C}$ and $1.0 \mathrm{~atm}$ is generated when the car goes on a $10 .$ -mile trip?

Key Concepts

Fuel Efficiency and Unit Conversions

Fuel efficiency, such as miles per gallon, connects the physical use of fuel to the chemical quantity consumed. Along with unit conversions for mass, volume, and moles, understanding fuel efficiency is crucial in translating everyday fuel usage into chemical terms that can be used in stoichiometric calculations.

Ideal Gas Law

The ideal gas law, expressed as PV = nRT, relates the pressure, volume, number of moles, and temperature of a gas. It is used to calculate the volume of a gaseous product when the number of moles, temperature, and pressure are known, making it essential for converting chemical amounts into physical gas volumes.

Balanced Chemical Equations

A balanced chemical equation ensures that the number of atoms for each element is equal on both the reactant and product sides. This balance is critical for accurately determining the stoichiometric ratios necessary for quantitative predictions in a chemical reaction.

Combustion Reactions

Combustion reactions involve the burning of a fuel in the presence of an oxidizer, typically oxygen, leading to the formation of products such as carbon dioxide and water. In hydrocarbon combustion, understanding this process is essential because the reaction is exothermic and involves changes in energy along with matter, and it must be accurately balanced to respect the conservation of mass.

Stoichiometry

Stoichiometry is the quantitative relationship between reactants and products in a chemical reaction. It allows for the calculation of how many moles or masses of products are formed from a given amount of reactants using coefficients derived from the balanced chemical equation.

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