### QuestionWhat mass (in grams) of aspirin (\(C_9H_8O_4\)) is produced from 67.3 g of \(C_7H_6O_3\) assuming 95.0% yield from the reaction below?\[C_7H_6O_3 (s) + C_4H_6O_3 (l) \rightarrow C_9H_8O_4 (s) + HC_2H_3O_2 (aq)\]### ExplanationIn this question, we need to calculate the theoretical and actual mass of aspirin produced from the given starting material, \(C_7H_6O_3\) (salicylic acid), assuming a reaction yield of 95.0%.### Steps to Solve1. **Balanced Chemical Equation**: \[ C_7H_6O_3 (s) + C_4H_6O_3 (l) \rightarrow C_9H_8O_4 (s) + HC_2H_3O_2 (aq) \] Here, one mole of \(C_7H_6O_3\) reacts with one mole of \(C_4H_6O_3\) to produce one mole of \(C_9H_8O_4\) (aspirin) and one mole of acetate.2. **Molar Mass Calculation**: - Molar mass of \(C_7H_6O_3\) (salicylic acid) = 138.12 g/mol - Molar mass of \(C_9H_8O_4\) (aspirin) = 180.16 g/mol3. **Moles of Salicylic Acid**: \[ \text{Moles of } C_7H_6O_3 = \frac{67.3 \, \text{g}}{138.12 \, \text{g/mol}} \approx 0.487 \text{ mol} \]4. **Theoretical Yield of Aspirin**: \[ \text{Theoretical moles of } C_9H_8O_4 = \text{Moles of } C_7H_6O_3 = 0.487 \

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Answered: oduced from 67.3 g of C₂H6O3 a 5.0%…

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oduced from 67.3 g of C₂H6O3 a 5.0% yield from the reaction belo 7H6O3 (S) + C₂H6O3 (1)→ C9H3O4 C₂H3O₂ (aq).

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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