Question 12W A 5.00 g-sample of KOH(s) at 25.0 C was added to 100.0 g of H2O(1) temperature of the solution had increased. Based on the information given, which of the following best justifies the claim that the dissolution of KOH(s) is a thermodynamically favorable process? room temperature inside an insulated cup calorimeter, and the contents were stirred. After all the KOH(s) dissolved, the The forces between the ions and the water molecules are strọnger than the forces between water molecules, thus AH < 0. Also, the ions become less dispersed as KOH(s) dissolves, thus A AS >0. Therefore, AG < 0. The energy required to break the bonds between the ions in the solid is less than that released as the ion-dipole attractions form during solvation, thus AH < 0. Also, the ions become more B widely dispersed as KOH(s) dissolves, thus AS > 0. Therefore, AG < 0. The average kinetic energy of the particles increases, resulting in AH >0. Also, the ions become more widely dispersed as KOH(s) dissolves, thus AS > 0. Therefore, AG > 0. The average kinetic energy of the particles increases, resulting in AH >0. Also, the ions become more widely dispersed as KOH(s) dissolves, thus AS < 0. Therefore, AG > 0. D

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...
icon
Related questions
Question
Question 12 W
A 5.00 g-sample of KOH(s) at 25.0°C was added to 100.0 g of H2O(1) at room temperature inside an insulated cup calorimeter, and the contents were stirred. After all the KOH(s) dissolved, the
temperature of the solution had increased. Based on the information given, which of the following best justifies the claim that the dissolution of KOH(s) is a thermodynamically favorable process?
The forces between the ions and the water molecules are strọnger than the forces between water molecules, thus AH < 0. Also, the ions become less dispersed as KOH(s) dissolves, thus
AS >0. Therefore, AG < 0.
less than that released as the ion-dipole attractions form during solvation, thus AH < 0. Also, the ions become more
The energy required to break the bonds between the ions in the solid
widely dispersed as KOH(s) dissolves, thus AS > 0. Therefore, AG < 0.
The average kinetic energy of the particles increases, resulting in AH > 0. Also, the ions become more widely dispersed as KOH(s) dissolves, thus AS > 0. Therefore. AG > 0.
D
The average kinetic energy of the particles increases, resulting in AH > 0. Also, the ions become more widely dispersed as KOH(s) dissolves, thus AS < 0. Therefore. AG > 0.
esc
Q Search or enter website name
@
#
$
%
&
Transcribed Image Text:Question 12 W A 5.00 g-sample of KOH(s) at 25.0°C was added to 100.0 g of H2O(1) at room temperature inside an insulated cup calorimeter, and the contents were stirred. After all the KOH(s) dissolved, the temperature of the solution had increased. Based on the information given, which of the following best justifies the claim that the dissolution of KOH(s) is a thermodynamically favorable process? The forces between the ions and the water molecules are strọnger than the forces between water molecules, thus AH < 0. Also, the ions become less dispersed as KOH(s) dissolves, thus AS >0. Therefore, AG < 0. less than that released as the ion-dipole attractions form during solvation, thus AH < 0. Also, the ions become more The energy required to break the bonds between the ions in the solid widely dispersed as KOH(s) dissolves, thus AS > 0. Therefore, AG < 0. The average kinetic energy of the particles increases, resulting in AH > 0. Also, the ions become more widely dispersed as KOH(s) dissolves, thus AS > 0. Therefore. AG > 0. D The average kinetic energy of the particles increases, resulting in AH > 0. Also, the ions become more widely dispersed as KOH(s) dissolves, thus AS < 0. Therefore. AG > 0. esc Q Search or enter website name @ # $ % &
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps

Blurred answer
Knowledge Booster
Thermodynamics
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.
Similar questions
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY