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 6.00 mL of acetic anhydride (density= 1.08 g/ mL) and 2.50 g of salicylic acid. Once the reaction is complete, the student collects 1.82 g of aspirin. Determine the limiting reactant, theoretical yield of aspirin, and percent yield forthe reaction.

검증된 단계별 안내

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 coefficients in the balanced equation.

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

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영상 길이:

주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

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 it, 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, which directly affects the yield of the desired product.

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 assumes complete conversion of the limiting reactant into the product without any losses. This value is essential for determining the efficiency of a reaction and is typically expressed in grams or moles.

Percent Yield

Percent yield is a measure of the efficiency of a chemical reaction, calculated by dividing the actual yield of the product obtained from the experiment by the theoretical yield, then multiplying by 100. It provides insight into how effectively the reactants were converted into products and can indicate potential losses due to side reactions, incomplete reactions, or experimental errors.