Gasohol is a fuel that contains ethanol (C2 H6 O) that burns in oxygen (O2) to give carbon dioxi

step 1 This question is a unit conversion question using stoichiometry and molar mass. To use stoichiom

Gasohol is a fuel that contains ethanol (C2 H6 O) that burns...

Gasohol is a fuel that contains ethanol $\left(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}\right)$ that burns in oxygen $\left(\mathrm{O}_{2}\right)$ to give carbon dioxide and water. $(9.2,9.3)$ $$ \mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}(g)+3 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 2 \mathrm{CO}_{2}(g)+3 \mathrm{H}_{2} \mathrm{O}(g) $$ a. How many moles of $\mathrm{O}_{2}$ are needed to completely react with $4.0 \mathrm{~mol}$ of $\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}$ ? b. If a car produces $88 \mathrm{~g}$ of $\mathrm{CO}_{2}$, how many grams of $\mathrm{O}_{2}$ are used up in the reaction? c. If you add $125 \mathrm{~g}$ of $\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}$ to your fuel, how many grams of $\mathrm{CO}_{2}$ can be produced from the ethanol?

Gasohol is a fuel that contains ethanol $\left(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}\right)$ that burns in oxygen $\left(\mathrm{O}_{2}\right)$ to give carbon dioxide and water. $(9.2,9.3)$
$$
\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}(g)+3 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 2 \mathrm{CO}_{2}(g)+3 \mathrm{H}_{2} \mathrm{O}(g)
$$
a. How many moles of $\mathrm{O}_{2}$ are needed to completely react with $4.0 \mathrm{~mol}$ of $\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}$ ?
b. If a car produces $88 \mathrm{~g}$ of $\mathrm{CO}_{2}$, how many grams of $\mathrm{O}_{2}$ are used up in the reaction?
c. If you add $125 \mathrm{~g}$ of $\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}$ to your fuel, how many grams of $\mathrm{CO}_{2}$ can be produced from the ethanol?

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Key Concepts

Molar Mass Calculations

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole. It is used to convert between the mass of a substance and the number of moles, making it an essential tool for performing quantitative analyses in chemical reactions.

Balanced Chemical Equation

A balanced chemical equation accurately represents the chemical reaction with equal numbers of atoms for each element on both sides of the reaction. It provides the stoichiometric coefficients that indicate the proportions in which substances react and form products, serving as the foundation for stoichiometric calculations.

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in a chemical reaction. It involves using the coefficients from a balanced chemical equation to calculate how much of each substance is needed or produced, ensuring that mass is conserved according to the law of conservation of mass.

Mole Concept

The mole concept is fundamental in chemistry for quantifying the amount of a substance. It relates the number of particles (atoms, molecules, ions) to the mass, allowing chemists to convert between the mass of a sample and the number of particles present using Avogadro's number.

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