A solution is made by dissolving 0.626 mol of nonelectrolyte solute in 849 g of benzene. Calculate the frcczing point, T. and boiling point, T, of the solution. Constants can be found in the table of colligative constants. T = T = C
A solution is made by dissolving 0.626 mol of nonelectrolyte solute in 849 g of benzene. Calculate the frcczing point, T. and boiling point, T, of the solution. Constants can be found in the table of colligative constants. T = T = C
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...
Related questions
Question
Answer all
![### Example Problem: Calculating Freezing and Boiling Points using Colligative Properties
#### Problem Statement:
A solution is made by dissolving 0.626 mol of nonelectrolyte solute in 849 g of benzene. Calculate the freezing point, \(T_f\), and boiling point, \(T_b\), of the solution. Constants can be found in the table of colligative constants.
#### Solution Steps:
1. **Identify the given data:**
- Amount of solute (\(n\)): 0.626 mol
- Mass of solvent (benzene, \(m\)): 849 g (or 0.849 kg)
- The molality (\(m\)) of the solution is given by:
\[
m = \frac{n}{\text{mass of solvent in kg}} = \frac{0.626 \text{ mol}}{0.849 \text{ kg}}
\]
2. **Calculate the molality of the solution:**
\[
m = \frac{0.626}{0.849} \approx 0.737 \text{ mol/kg}
\]
3. **Freezing Point Depression:**
The freezing point depression (\(\Delta T_f\)) is calculated using the formula:
\[
\Delta T_f = K_f \cdot m
\]
Here, \(K_f\) is the cryoscopic constant of the solvent. For benzene, \(K_f\) is approximately 5.12 °C/m.
4. **Calculate \(\Delta T_f\):**
\[
\Delta T_f = 5.12 \, \text{°C/m} \times 0.737 \, \text{mol/kg}
\]
\[
\Delta T_f \approx 3.78 \, \text{°C}
\]
5. **Determine the new freezing point:**
Benzene's normal freezing point is 5.5 °C. The new freezing point (\(T_f\)) is:
\[
T_f = 5.5 \, \text{°C} - 3.78 \, \text{°C} \approx 1.72 \, \text{°C}
\]
6. **Boiling Point Elevation:**](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff2609b9a-bccc-4ea0-ab3c-7cfd8cf7907c%2F72bd1a5d-07ed-4d6c-a3e4-ea5550981136%2F9dv8gwk_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Example Problem: Calculating Freezing and Boiling Points using Colligative Properties
#### Problem Statement:
A solution is made by dissolving 0.626 mol of nonelectrolyte solute in 849 g of benzene. Calculate the freezing point, \(T_f\), and boiling point, \(T_b\), of the solution. Constants can be found in the table of colligative constants.
#### Solution Steps:
1. **Identify the given data:**
- Amount of solute (\(n\)): 0.626 mol
- Mass of solvent (benzene, \(m\)): 849 g (or 0.849 kg)
- The molality (\(m\)) of the solution is given by:
\[
m = \frac{n}{\text{mass of solvent in kg}} = \frac{0.626 \text{ mol}}{0.849 \text{ kg}}
\]
2. **Calculate the molality of the solution:**
\[
m = \frac{0.626}{0.849} \approx 0.737 \text{ mol/kg}
\]
3. **Freezing Point Depression:**
The freezing point depression (\(\Delta T_f\)) is calculated using the formula:
\[
\Delta T_f = K_f \cdot m
\]
Here, \(K_f\) is the cryoscopic constant of the solvent. For benzene, \(K_f\) is approximately 5.12 °C/m.
4. **Calculate \(\Delta T_f\):**
\[
\Delta T_f = 5.12 \, \text{°C/m} \times 0.737 \, \text{mol/kg}
\]
\[
\Delta T_f \approx 3.78 \, \text{°C}
\]
5. **Determine the new freezing point:**
Benzene's normal freezing point is 5.5 °C. The new freezing point (\(T_f\)) is:
\[
T_f = 5.5 \, \text{°C} - 3.78 \, \text{°C} \approx 1.72 \, \text{°C}
\]
6. **Boiling Point Elevation:**
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 3 steps with 2 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY