Aspirin can be made in the laboratory by reacting acetic anhydride (C4 H6 O3) with salicylic aci

step 1 Let's determine the limiting reactant, theoretical yield of aspirin and percent yield, starting

Aspirin can be made in the laboratory by reacting acetic...

Aspirin can be made in the laboratory by reacting acetic anhydride $\left(\mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{3}\right)$ with salicylic acid $\left(\mathrm{C}_{7} \mathrm{H}_{6} \mathrm{O}_{3}\right)$ to form aspirin $\left(\mathrm{C}_{9} \mathrm{H}_{8} \mathrm{O}_{4}\right)$ andacctic acid $\left(\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}_{2}\right) \cdot$ The balanced equation is: $$\mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{3}+\mathrm{C}_{7} \mathrm{H}_{6} \mathrm{O}_{3} \longrightarrow \mathrm{C}_{9} \mathrm{H}_{8} \mathrm{O}_{4}+\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}_{2}$$ In a laboratory synthesis, a student begins with 3.00 $\mathrm{mL}$ of acetic anhydride (density $=1.08 \mathrm{g} / \mathrm{mL} )$ and 1.25 $\mathrm{g}$ of salicylic acid. Once the reaction is complete, the student collects 1.22 $\mathrm{g}$ of aspirin. Determine the limiting reactant, theorctical yicld of aspirin, and percent yield for the reaction.

Aspirin can be made in the laboratory by reacting acetic anhydride
$\left(\mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{3}\right)$ with salicylic acid $\left(\mathrm{C}_{7} \mathrm{H}_{6} \mathrm{O}_{3}\right)$ to form aspirin $\left(\mathrm{C}_{9} \mathrm{H}_{8} \mathrm{O}_{4}\right)$ andacctic acid $\left(\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}_{2}\right) \cdot$ The balanced equation is:
$$\mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{3}+\mathrm{C}_{7} \mathrm{H}_{6} \mathrm{O}_{3} \longrightarrow \mathrm{C}_{9} \mathrm{H}_{8} \mathrm{O}_{4}+\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}_{2}$$
In a laboratory synthesis, a student begins with 3.00 $\mathrm{mL}$ of acetic
anhydride (density $=1.08 \mathrm{g} / \mathrm{mL} )$ and 1.25 $\mathrm{g}$ of salicylic acid. Once the reaction is complete, the student collects 1.22 $\mathrm{g}$ of aspirin. Determine
the limiting reactant, theorctical yicld of aspirin, and percent yield for
the reaction.

Key Concepts

Stoichiometry

Stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction. It uses the balanced chemical equation to determine how much product can be produced from given amounts of reactants by converting between mass, moles, and molecules.

Limiting Reactant

The limiting reactant is the substance in a reaction that is completely consumed first, thereby limiting the amount of product that can be formed. Identifying the limiting reactant is crucial because it determines the theoretical yield of the reaction.

Theoretical Yield

The theoretical yield is the maximum amount of product that can be generated from a chemical reaction based on the complete consumption of the limiting reactant. It is calculated using stoichiometry and assumes that the reaction goes to completion with no losses.

Percent Yield

Percent yield is a measure of the efficiency of a reaction, defined as the ratio of the actual yield (the amount of product actually obtained) to the theoretical yield, multiplied by 100. It provides insight into the practical aspects of the reaction such as losses, side reactions, or incomplete conversion.

Density and Unit Conversion

Density and unit conversion are essential for translating between units, such as converting volumes to masses using density, or converting masses to moles using molar mass. These conversions are fundamental in preparing reactants and analyzing chemical reactions.

Balanced Chemical Equation

A balanced chemical equation accurately represents the conservation of mass in a chemical reaction by ensuring that the number of atoms for each element is the same on both sides of the equation. It provides the basis for all stoichiometric calculations in the reaction.

Molar Mass and Mole Conversions

Molar mass is the mass of one mole of a substance and is used to convert between the mass of a substance and the number of moles. Mole conversions are a key step in stoichiometry, linking the macroscopic measurements of mass to the molecular scale where the actual reaction occurs.

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