Ethanol, C2 H6 O, is added to gasoline to produce "gasohol,"...

Ethanol, $\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O},$ is added to gasoline to produce "gasohol," a fuel for automobile engines. How many grams of $\mathrm{O}_{2}$ are required for complete combustion of $421 \mathrm{g}$ of ethanol? $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(\ell)+3 \mathrm{O}_{2}(\mathrm{g}) \longrightarrow 2 \mathrm{CO}_{2}(\mathrm{g})+3 \mathrm{H}_{2} \mathrm{O}$

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Key Concepts

Stoichiometry

Stoichiometry involves using the relationships between the quantities of reactants and products in a chemical reaction, as given by a balanced chemical equation. This concept allows one to determine the amounts of other substances required or produced in a reaction when one substance’s quantity is known.

Balanced Chemical Equations

A balanced chemical equation provides the exact proportions of moles of reactants and products involved in a chemical reaction. It ensures conservation of mass and is essential for accurate stoichiometric calculations, such as determining how much oxygen is needed for the complete combustion of ethanol.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole. It serves as a conversion factor between the mass of a substance in grams and the number of moles, which is fundamental in stoichiometry when transitioning from mass measurements to mole quantities.

Mole-to-Mass Conversions

Mole-to-mass conversion is the process of converting a given amount in moles to grams, using the molar mass as a conversion factor. This concept is critical in chemical calculations to determine the mass of a reactant or product when its mole quantity is known from the balanced chemical equation.

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