d. Calculate the Gibbs energy and the equilibrium constant for the denaturation of chymotrypsin at pH=2 ant T=310 K. Is the protein stable under these conditions?
d. Calculate the Gibbs energy and the equilibrium constant for the denaturation of chymotrypsin at pH=2 ant T=310 K. Is the protein stable under these conditions?
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
Only answer Part D please
![The denaturation of a biological macromolecule may be described as an equilibrium:
Protein
Denatured
a. Show that the fraction of denatured macromolecules, 0, is related to the equilibrium
constant, Kd, by
K.
1+ Kd
b. At pH=2, the standard enthalpy and entropy of formation for the denaturation of the
enzyme chymotrypsin are 418 kJ/mol and 1.32 kJ K-' mol-', respectively. Use these data
to generate a plot that shows the temperature dependence of 0. Assume the enthalpy and
entropy change to be independent of temperature.
c. The "melting temperature" of a biological molecule is defined as the temperature at
which 0=1/2. Determine the “melting temperature" of chymotrypsin at pH=2.
d. Calculate the Gibbs energy and the equilibrium constant for the denaturation of
chymotrypsin at pH=2 ant T=310 K. Is the protein stable under these conditions?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F91277f70-1158-4ed8-b43a-68abff16ddb2%2Ffe54157f-7e2a-42b7-af4e-4eab84dda57d%2Fi7q5q3f_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The denaturation of a biological macromolecule may be described as an equilibrium:
Protein
Denatured
a. Show that the fraction of denatured macromolecules, 0, is related to the equilibrium
constant, Kd, by
K.
1+ Kd
b. At pH=2, the standard enthalpy and entropy of formation for the denaturation of the
enzyme chymotrypsin are 418 kJ/mol and 1.32 kJ K-' mol-', respectively. Use these data
to generate a plot that shows the temperature dependence of 0. Assume the enthalpy and
entropy change to be independent of temperature.
c. The "melting temperature" of a biological molecule is defined as the temperature at
which 0=1/2. Determine the “melting temperature" of chymotrypsin at pH=2.
d. Calculate the Gibbs energy and the equilibrium constant for the denaturation of
chymotrypsin at pH=2 ant T=310 K. Is the protein stable under these conditions?
Expert Solution
![](/static/compass_v2/shared-icons/check-mark.png)
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 1 images
![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](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](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
![Principles of Instrumental Analysis](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
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](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
![Principles of Instrumental Analysis](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
![Organic Chemistry](https://www.bartleby.com/isbn_cover_images/9780078021558/9780078021558_smallCoverImage.gif)
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
![Chemistry: Principles and Reactions](https://www.bartleby.com/isbn_cover_images/9781305079373/9781305079373_smallCoverImage.gif)
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
![Elementary Principles of Chemical Processes, Bind…](https://www.bartleby.com/isbn_cover_images/9781118431221/9781118431221_smallCoverImage.gif)
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY