A certain substance X melts at a temperature of 7.4 °C. But if a 350. g sample of X is prepared with 16. g of urea found to have a melting point of 5.6 °C instead. Calculate the molal freezing point depression constant K of X. Be sure your answer has the correct number of significant digits. -1 1 °C mol - kg X ((NH₂)₂CO) dissolved in it, the sample is
A certain substance X melts at a temperature of 7.4 °C. But if a 350. g sample of X is prepared with 16. g of urea found to have a melting point of 5.6 °C instead. Calculate the molal freezing point depression constant K of X. Be sure your answer has the correct number of significant digits. -1 1 °C mol - kg X ((NH₂)₂CO) dissolved in it, the sample is
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter12: Solutions
Section: Chapter Questions
Problem 12.95QE
Related questions
Question
![A certain substance X melts at a temperature of 7.4 °C. But if a 350. g sample of X is prepared with 16. g of urea
found to have a melting point of 5.6 °C instead. Calculate the molal freezing point depression constant K of X.
Be sure your answer has the correct number of significant digits.
-1
°C mol
• kg
x10
X
((NH₂)₂CO) dissolved in it, the sample is](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe2dac4f4-a9bd-4021-84b9-9c5bd3b78b57%2F43189476-e7e1-46c0-95e9-3901b3ed1981%2F7k7sgjp_processed.png&w=3840&q=75)
Transcribed Image Text:A certain substance X melts at a temperature of 7.4 °C. But if a 350. g sample of X is prepared with 16. g of urea
found to have a melting point of 5.6 °C instead. Calculate the molal freezing point depression constant K of X.
Be sure your answer has the correct number of significant digits.
-1
°C mol
• kg
x10
X
((NH₂)₂CO) dissolved in it, the sample is
Expert Solution
![](/static/compass_v2/shared-icons/check-mark.png)
Step 1
To calculate the molal freezing point depression constant Kƒ of substance X, we first need to calculate the freezing point depression ΔTf caused by adding 16 g of urea to 350 g of X.
ΔTf = Kf·m·i
where Kf is the molal freezing point depression constant, m is the molality of the urea solution, and i is the van't Hoff factor, which is the number of particles into which the solute dissociates in the solution.
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
![Blurred answer](/static/compass_v2/solution-images/blurred-answer.jpg)
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: Principles and Practice](https://www.bartleby.com/isbn_cover_images/9780534420123/9780534420123_smallCoverImage.gif)
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
![Chemistry & Chemical Reactivity](https://www.bartleby.com/isbn_cover_images/9781337399074/9781337399074_smallCoverImage.gif)
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
![Chemistry: The Molecular Science](https://www.bartleby.com/isbn_cover_images/9781285199047/9781285199047_smallCoverImage.gif)
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
![Chemistry: Principles and Practice](https://www.bartleby.com/isbn_cover_images/9780534420123/9780534420123_smallCoverImage.gif)
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
![Chemistry & Chemical Reactivity](https://www.bartleby.com/isbn_cover_images/9781337399074/9781337399074_smallCoverImage.gif)
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
![Chemistry: The Molecular Science](https://www.bartleby.com/isbn_cover_images/9781285199047/9781285199047_smallCoverImage.gif)
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
![Chemistry: An Atoms First Approach](https://www.bartleby.com/isbn_cover_images/9781305079243/9781305079243_smallCoverImage.gif)
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781133611097/9781133611097_smallCoverImage.gif)