What is the boiling point of a solution of 63.5 g of iodine, 12, in 500.0 g of chloroform, CHCl3? Assume the iodine is nonvolatile and that the solution is ideal. The kb for chloroform is 3.88°C/m and the normal boiling point is 61.3°C. BP = [?] °C Boiling Point (°C) Enter
What is the boiling point of a solution of 63.5 g of iodine, 12, in 500.0 g of chloroform, CHCl3? Assume the iodine is nonvolatile and that the solution is ideal. The kb for chloroform is 3.88°C/m and the normal boiling point is 61.3°C. BP = [?] °C Boiling Point (°C) Enter
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
100%
![**Boiling Point Elevation Calculation Example**
**Problem Statement:**
What is the boiling point of a solution of 63.5 g of iodine, I₂, in 500.0 g of chloroform, CHCl₃? Assume the iodine is nonvolatile and that the solution is ideal.
The \( k_b \) for chloroform is 3.88°C/m and the normal boiling point is 61.3°C.
**Solution:**
To find the boiling point of the solution, use the formula for boiling point elevation:
\[ \Delta T_b = k_b \times m \]
where:
- \( \Delta T_b \) = boiling point elevation
- \( k_b \) = ebullioscopic constant (for chloroform)
- \( m \) = molality of the solution
First, calculate the molality ( \(m\) ) of the solution:
\[ m = \frac{\text{moles of solute}}{\text{kg of solvent}} \]
Calculate the moles of iodine:
- Molar mass of iodine (I₂) = 2 x 126.90 g/mol = 253.8 g/mol
- Moles of iodine = \(\frac {63.5 \text{ g}}{253.8 \text{ g/mol}} ≈ 0.250 \text{ mol}\)
Calculate the mass of solvent in kilograms:
- Mass of chloroform in kg = \(\frac{500.0 \text{ g}}{1000 \text{ g/kg}} = 0.500 \text{ kg}\)
Now, calculate the molality:
\[ m = \frac{0.250 \text{ mol}}{0.500 \text{ kg}} = 0.500 \text{ m} \]
Next, use the boiling point elevation equation:
\[ \Delta T_b = 3.88 \text{ °C/m} \times 0.500 \text{ m} = 1.94 \text{ °C} \]
Finally, add the boiling point elevation to the normal boiling point:
\[ \text{Boiling Point (BP)} = 61.3°C + 1.94°C = 63.24°C \]
**Boiling Point (BP) = 63.24°C**
In the given interactive text box, users can enter the calculated boiling point (63](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F07a40a8c-2023-4125-afaf-f3a8d976c8b9%2F58a59df9-b838-4cce-b9a2-2e55a2155ca2%2Fc6ue57g_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Boiling Point Elevation Calculation Example**
**Problem Statement:**
What is the boiling point of a solution of 63.5 g of iodine, I₂, in 500.0 g of chloroform, CHCl₃? Assume the iodine is nonvolatile and that the solution is ideal.
The \( k_b \) for chloroform is 3.88°C/m and the normal boiling point is 61.3°C.
**Solution:**
To find the boiling point of the solution, use the formula for boiling point elevation:
\[ \Delta T_b = k_b \times m \]
where:
- \( \Delta T_b \) = boiling point elevation
- \( k_b \) = ebullioscopic constant (for chloroform)
- \( m \) = molality of the solution
First, calculate the molality ( \(m\) ) of the solution:
\[ m = \frac{\text{moles of solute}}{\text{kg of solvent}} \]
Calculate the moles of iodine:
- Molar mass of iodine (I₂) = 2 x 126.90 g/mol = 253.8 g/mol
- Moles of iodine = \(\frac {63.5 \text{ g}}{253.8 \text{ g/mol}} ≈ 0.250 \text{ mol}\)
Calculate the mass of solvent in kilograms:
- Mass of chloroform in kg = \(\frac{500.0 \text{ g}}{1000 \text{ g/kg}} = 0.500 \text{ kg}\)
Now, calculate the molality:
\[ m = \frac{0.250 \text{ mol}}{0.500 \text{ kg}} = 0.500 \text{ m} \]
Next, use the boiling point elevation equation:
\[ \Delta T_b = 3.88 \text{ °C/m} \times 0.500 \text{ m} = 1.94 \text{ °C} \]
Finally, add the boiling point elevation to the normal boiling point:
\[ \text{Boiling Point (BP)} = 61.3°C + 1.94°C = 63.24°C \]
**Boiling Point (BP) = 63.24°C**
In the given interactive text box, users can enter the calculated boiling point (63
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 2 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