(c) Calculate the mole of acetic anhydride used in this experiment: I mol 6.48 102.09 g g X = 0.0635 mol of acetic anhydride (d) Which is the limiting reactant? Salicylic acid (e) Calculate the theoretical yield of aspirin produced in grams: (f) How many grams of aspirin did you actually obtain in this experiment? (actual yield in gram) (g) Calculate the percent yield of aspirin.
(c) Calculate the mole of acetic anhydride used in this experiment: I mol 6.48 102.09 g g X = 0.0635 mol of acetic anhydride (d) Which is the limiting reactant? Salicylic acid (e) Calculate the theoretical yield of aspirin produced in grams: (f) How many grams of aspirin did you actually obtain in this experiment? (actual yield in gram) (g) Calculate the percent yield of aspirin.
Chemistry
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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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Calculate the theoretical yield, actual yield, and percent yield of aspirin.
![(c) **Calculate the mole of acetic anhydride used in this experiment:**
\[ 6.48 \, \text{g} \times \frac{1 \, \text{mol}}{102.09 \, \text{g}} = 0.0635 \, \text{mol of acetic anhydride} \]
(d) **Which is the limiting reactant?**
Salicylic acid
(e) **Calculate the theoretical yield of aspirin produced in grams:**
(f) **How many grams of aspirin did you actually obtain in this experiment? (actual yield in gram)**
(g) **Calculate the percent yield of aspirin.**](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7859f905-a93a-424f-a5cf-092dfae20bfb%2F161774ac-bae5-4214-90e4-f5241bf9cc94%2Frgd69q_processed.jpeg&w=3840&q=75)
Transcribed Image Text:(c) **Calculate the mole of acetic anhydride used in this experiment:**
\[ 6.48 \, \text{g} \times \frac{1 \, \text{mol}}{102.09 \, \text{g}} = 0.0635 \, \text{mol of acetic anhydride} \]
(d) **Which is the limiting reactant?**
Salicylic acid
(e) **Calculate the theoretical yield of aspirin produced in grams:**
(f) **How many grams of aspirin did you actually obtain in this experiment? (actual yield in gram)**
(g) **Calculate the percent yield of aspirin.**
![**Transcription for Educational Website**
### Experimental Values and Calculations
#### 1. Recorded Values
- **Molar mass of salicylic acid:** 138.12 g/mol
- **Molar mass of acetic anhydride:** 102.09 g/mol
- **Density of acetic anhydride:** 1.08 g/cm³
- **Molar mass of aspirin:** 180.16 g/mol
#### 2. Experimental Data
- **Mass of salicylic acid (g) in this experiment:** 2.970 g
- **Volume of acetic anhydride (ml) in this experiment:** 6.0 ml
- **Mass of aspirin in this experiment:** 4.148 g
#### 3. Calculations
**(a) Calculate the moles of salicylic acid used in this experiment:**
Using the formula:
\[
\text{Moles of salicylic acid} = \frac{\text{Mass of salicylic acid}}{\text{Molar mass of salicylic acid}}
\]
Substitute the values:
\[
2.970 \, \text{g} \times \frac{1 \, \text{mol}}{138.12 \, \text{g/mol}} = 0.0215 \, \text{mol of salicylic acid}
\]
**(b) Calculate the mass of acetic anhydride used in this experiment:**
Using the formula:
\[
\text{Mass of acetic anhydride} = \text{Volume of acetic anhydride} \times \text{Density of acetic anhydride}
\]
Substitute the values:
\[
6.0 \, \text{ml} \times \frac{1.08 \, \text{g}}{1 \, \text{ml}} = 6.48 \, \text{g of acetic anhydride}
\]
---
This document outlines the essential molar masses, experimental data, and calculations necessary in the synthesis of aspirin from salicylic acid and acetic anhydride in a laboratory setting.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7859f905-a93a-424f-a5cf-092dfae20bfb%2F161774ac-bae5-4214-90e4-f5241bf9cc94%2F9qrr7za_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Transcription for Educational Website**
### Experimental Values and Calculations
#### 1. Recorded Values
- **Molar mass of salicylic acid:** 138.12 g/mol
- **Molar mass of acetic anhydride:** 102.09 g/mol
- **Density of acetic anhydride:** 1.08 g/cm³
- **Molar mass of aspirin:** 180.16 g/mol
#### 2. Experimental Data
- **Mass of salicylic acid (g) in this experiment:** 2.970 g
- **Volume of acetic anhydride (ml) in this experiment:** 6.0 ml
- **Mass of aspirin in this experiment:** 4.148 g
#### 3. Calculations
**(a) Calculate the moles of salicylic acid used in this experiment:**
Using the formula:
\[
\text{Moles of salicylic acid} = \frac{\text{Mass of salicylic acid}}{\text{Molar mass of salicylic acid}}
\]
Substitute the values:
\[
2.970 \, \text{g} \times \frac{1 \, \text{mol}}{138.12 \, \text{g/mol}} = 0.0215 \, \text{mol of salicylic acid}
\]
**(b) Calculate the mass of acetic anhydride used in this experiment:**
Using the formula:
\[
\text{Mass of acetic anhydride} = \text{Volume of acetic anhydride} \times \text{Density of acetic anhydride}
\]
Substitute the values:
\[
6.0 \, \text{ml} \times \frac{1.08 \, \text{g}}{1 \, \text{ml}} = 6.48 \, \text{g of acetic anhydride}
\]
---
This document outlines the essential molar masses, experimental data, and calculations necessary in the synthesis of aspirin from salicylic acid and acetic anhydride in a laboratory setting.
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