The spontaneity of a reaction depends both on the enthalpy change, ΔHΔHDelta H, and entropy change, ΔSΔSDelta S. Reactions that release energy produce more stable products, and the universe tends toward disorder. Thus, an exothermic reaction with a positive entropy change will always be spontaneous. Mathematically, this relationship can be represented as ΔG=ΔH−TΔSΔG=ΔH−TΔS where ΔGΔGDelta G is the change in Gibbs free energy and is the Kelvin temperature. If ΔGΔGDelta G is negative, then the reaction is spontaneous. If ΔGΔGDelta G is positive, then the reaction is nonspontaneous as written but spontaneous in the reverse direction. If ΔHΔHDH = -50.0 kJkJ and ΔSΔSDS = -0.300 kJ/KkJ/K , the reaction is spontaneous below a certain temperature. Calculate that temperature. Express your answer numerically in kelvins.
The spontaneity of a reaction depends both on the enthalpy change, ΔHΔHDelta H, and entropy change, ΔSΔSDelta S. Reactions that release energy produce more stable products, and the universe tends toward disorder. Thus, an exothermic reaction with a positive entropy change will always be spontaneous. Mathematically, this relationship can be represented as ΔG=ΔH−TΔSΔG=ΔH−TΔS where ΔGΔGDelta G is the change in Gibbs free energy and is the Kelvin temperature. If ΔGΔGDelta G is negative, then the reaction is spontaneous. If ΔGΔGDelta G is positive, then the reaction is nonspontaneous as written but spontaneous in the reverse direction. If ΔHΔHDH = -50.0 kJkJ and ΔSΔSDS = -0.300 kJ/KkJ/K , the reaction is spontaneous below a certain temperature. Calculate that temperature. Express your answer numerically in kelvins.
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
The spontaneity of a reaction depends both on the enthalpy change, ΔHΔHDelta H, and entropy change, ΔSΔSDelta S. Reactions that release energy produce more stable products, and the universe tends toward disorder. Thus, an exothermic reaction with a positive entropy change will always be spontaneous. Mathematically, this relationship can be represented as
ΔG=ΔH−TΔSΔG=ΔH−TΔS
where ΔGΔGDelta G is the change in Gibbs free energy and is the Kelvin temperature. If ΔGΔGDelta G is negative, then the reaction is spontaneous. If ΔGΔGDelta G is positive, then the reaction is nonspontaneous as written but spontaneous in the reverse direction.
If ΔHΔHDH = -50.0 kJkJ and ΔSΔSDS = -0.300 kJ/KkJ/K , the reaction is spontaneous below a certain temperature. Calculate that temperature.
Express your answer numerically in kelvins.
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 4 steps with 1 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