Certain race cars use methanol (CH 3 OH, also called wood alcohol) as a fuel. The combustion of

step 1 So for this problem, we're given this combustion reaction of methanol. And the equation's alread

Certain race cars use methanol (CH 3 OH, also called wood...

Certain race cars use methanol (CH $_{3} \mathrm{OH}$, also called wood alcohol) as a fuel. The combustion of methanol occurs according to the following equation:$$2 \mathrm{CH}_{3} \mathrm{OH}(l)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(l)$$In a particular reaction, 9.8 moles of $\mathrm{CH}_{3} \mathrm{OH}$ are reacted with an excess of $\mathrm{O}_{2}$. Calculate the number of moles of $\mathrm{H}_{2} \mathrm{O}$ formed.

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Key Concepts

Stoichiometry

Stoichiometry involves using quantitative relationships between reactants and products in a chemical reaction. It relies on the conservation of mass to allow calculations of the amounts of substances consumed and produced, ensuring that the overall mass and number of atoms remain consistent throughout the reaction.

Balanced Chemical Equation

A balanced chemical equation represents a reaction in which the number of atoms for each element is the same on both the reactants and products sides. This balance is essential for accurately determining the mole ratios which are used in quantitative reaction calculations.

Mole Ratio

The mole ratio is determined by the coefficients of a balanced chemical equation and expresses the proportional relationship between the moles of one substance and another. This ratio is fundamental in converting between the amounts of different reactants or products in a reaction.

Excess Reagent

An excess reagent is a reactant that is present in a quantity greater than needed to completely react with the limiting reagent. Recognizing an excess reagent is important because it ensures that the calculation of product amounts is based on the limiting reactant, which controls the extent of the reaction.

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