In the body, ethanol (C2 H6 O) reacts according to the following equation: (9.3) C2 H6 O(a q)+3

a. First, we need to find the moles of ethanol. The molar mass of ethanol (C2H6O) is (2 * 12.01)

In the body, ethanol (C2 H6 O) reacts according to the...

In the body, ethanol $\left(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}\right)$ reacts according to the following equation: (9.3) $$ \mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}(a q)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}_{2}(g)+3 \mathrm{H}_{2} \mathrm{O}(l) $$ Ethanol a. How many grams of $\mathrm{O}_{2}$ are needed to react with $8.40 \mathrm{~g}$ of ethanol? b. How many grams of $\mathrm{H}_{2} \mathrm{O}$ are produced from $8.40 \mathrm{~g}$ of ethanol? c. How many grams of $\mathrm{CO}_{2}$ are produced from $8.40 \mathrm{~g}$ of ethanol?

In the body, ethanol $\left(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}\right)$ reacts according to the following equation: (9.3)
$$
\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}(a q)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}_{2}(g)+3 \mathrm{H}_{2} \mathrm{O}(l)
$$
Ethanol
a. How many grams of $\mathrm{O}_{2}$ are needed to react with $8.40 \mathrm{~g}$ of ethanol?
b. How many grams of $\mathrm{H}_{2} \mathrm{O}$ are produced from $8.40 \mathrm{~g}$ of ethanol?
c. How many grams of $\mathrm{CO}_{2}$ are produced from $8.40 \mathrm{~g}$ of ethanol?

Key Concepts

Balanced Chemical Equations

Balanced chemical equations represent the law of conservation of mass by ensuring that the number of atoms for each element is equal on both sides of the reaction. They provide the mole ratios between reactants and products which are essential for converting between different chemical species in stoichiometric calculations.

Mole Concept

The mole concept is a fundamental idea in chemistry that serves as a bridge between the microscopic world of atoms and molecules and the macroscopic world we can measure. It involves using Avogadro’s number to count entities and convert between the mass of a substance and the number of moles, which is critical for quantitative chemical calculations.

Molar Mass

Molar mass is the mass of one mole of a substance, expressed in grams per mole (g/mol). It is derived by summing the atomic masses of the constituent atoms in a compound and is used as a conversion factor between the mass of a sample and the number of moles, enabling quantitative analysis in chemical reactions.

Stoichiometry

Stoichiometry involves the quantitative relationships among reactants and products in a chemical reaction as defined by the balanced chemical equation. It allows chemists to predict the amounts of substances consumed and produced, determining how much of each reactant is needed to produce specific amounts of products.

Dimensional Analysis

Dimensional analysis is a systematic method used to convert units and solve quantitative problems in chemistry. By ensuring that units cancel appropriately at each step of the calculation, this method helps to accurately convert between measurements, such as grams to moles and vice versa.

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