Aspirin can be made in the laboratory by reacting acetic anhydride (C₄H₆O₃) with salicylic acid (C₇H₆O₃) to form aspirin (C₉H₈O₄) and acetic acid (C₂H₄O₂). The balanced equation is: C₄H₆O₃ + C₇H₆O₃ → C₉H₈O₄ + C₂H₄O₂ In a laboratory synthesis, a student begins with 3.00 mL of acetic anhydride (density = 1.08 g/mL) and 1.25 g of salicylic acid. Once the reaction is complete, the student collects 1.22 g of aspirin. Determine the limiting reactant. Determine the theoretical yield of aspirin. Determine the percent yield for the reaction.

Verified step by step guidance

Calculate the mass of acetic anhydride using its volume and density: \( \text{mass} = \text{volume} \times \text{density} \).

Convert the mass of acetic anhydride to moles using its molar mass: \( \text{moles} = \frac{\text{mass}}{\text{molar mass}} \).

Convert the mass of salicylic acid to moles using its molar mass: \( \text{moles} = \frac{\text{mass}}{\text{molar mass}} \).

Determine the limiting reactant by comparing the mole ratio of the reactants to the stoichiometry of the balanced equation.

Calculate the theoretical yield of aspirin based on the limiting reactant and then determine the percent yield using the formula: \( \text{percent yield} = \left( \frac{\text{actual yield}}{\text{theoretical yield}} \right) \times 100 \).

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Limiting Reactant

The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. To identify the limiting reactant, one must compare the mole ratios of the reactants based on the balanced chemical equation. The reactant that produces the least amount of product is the limiting reactant.

Theoretical Yield

The theoretical yield is the maximum amount of product that can be generated from a given amount of reactants, as calculated from the balanced chemical equation. It is determined by using the limiting reactant to find out how much product can be formed under ideal conditions, assuming complete conversion and no losses during the reaction.

Percent Yield

Percent yield is a measure of the efficiency of a chemical reaction, calculated by comparing the actual yield of a product obtained from the reaction to the theoretical yield. It is expressed as a percentage and is calculated using the formula: (actual yield / theoretical yield) × 100. This value helps assess how well the reaction proceeded and can indicate potential losses or inefficiencies.

Recommended video:

Guided course

03:09

Percent Yield in Reactions

Related Practice

Textbook Question

Write the balanced equation for the reaction of hydrogen gas with bromine gas.

views

Textbook Question

The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane (C₈H₁₈) and calculate the mass (in kg) of carbon dioxide that is added to the atmosphere per 1.0 kg of octane burned. (Hint: Begin by writing a balanced equation for the combustion reaction.)

views

Textbook Question

Many home barbeques are fueled with propane gas (C₃H₈). What mass of carbon dioxide (in kg) is produced upon the complete combustion of 18.9 L of propane (approximate contents of one 5-gallon tank)? Assume that the density of the liquid propane in the tank is 0.621 g/mL. (Hint: Begin by writing a balanced equation for the combustion reaction.)

Textbook Question

The combustion of liquid ethanol (C₂H₅OH) produces carbon dioxide and water. After 4.62 mL of ethanol (density = 0.789 g/mL) is allowed to burn in the presence of 15.55 g of oxygen gas, 3.72 mL of water (density = 1.00 g/mL) is collected. Determine the percent yield for the reaction. (Hint: Write a balanced equation for the combustion of ethanol.)

views

Textbook Question

The reaction of NH₃ and O2 forms NO and water. The NO can be used to convert P₄ to P₄O₆, forming N₂ in the process. The P₄O₆ can be treated with water to form H₃PO₃, which forms PH₃ and H₃PO₄ when heated. Find the mass of PH₃ that forms from the reaction of 1.00 g of NH₃.

Textbook Question

An important reaction that takes place in a blast furnace during the production of iron is the formation of iron metal and CO₂ from Fe₂O₃ and CO. Determine the mass of Fe₂O₃ required to form 910 kg of iron. Determine the amount of CO₂ that forms in this process.

views