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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![### Question
What 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?
\[
C_7H_6O_3 (s) + C_4H_6O_3 (l) \rightarrow C_9H_8O_4 (s) + HC_2H_3O_2 (aq)
\]
### Explanation
In 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 Solve
1. **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/mol
3. **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**:
\[
\text{Theoretical moles of } C_9H_8O_4 = \text{Moles of } C_7H_6O_3 = 0.487 \](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F38543b38-0ca2-4898-a226-639f5edfcbc9%2F36f76b53-4996-48e7-b038-c710f4bbb855%2Frgfwy3_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Question
What 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?
\[
C_7H_6O_3 (s) + C_4H_6O_3 (l) \rightarrow C_9H_8O_4 (s) + HC_2H_3O_2 (aq)
\]
### Explanation
In 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 Solve
1. **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/mol
3. **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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