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Consider the figure below which shows AG" for a chemical process plotted against absolute temperature. Which one of the following is an incorrect conclusion, based on the information in the diagram? + AG° T(K) There exists a certain temperature at which AH° = TAS°. AS° > 0 AS° increases with temperature while AH° remains constant. O The reaction is spontaneous at high temperatures. O AH° > 0

Consider the figure below which shows AG" for a chemical process plotted against absolute temperature. Which one of the following is an incorrect conclusion, based on the information in the diagram? + AG° T(K) There exists a certain temperature at which AH° = TAS°. AS° > 0 AS° increases with temperature while AH° remains constant. O The reaction is spontaneous at high temperatures. O AH° > 0

Chemistry
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...
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This question is for practice and not graded. Please elaborate on answer. Thank you.

The image presents a graph depicting the change in standard Gibbs free energy (\(\Delta G^\circ\)) for a chemical process plotted against absolute temperature (\(T(K)\)). The graph displays a linear relationship with a negative slope, where: - The vertical axis represents \(\Delta G^\circ\), with positive values above the origin and negative values below it. - The horizontal axis represents temperature in Kelvin (\(T(K)\)). - The line crosses the \(\Delta G^\circ\) axis, indicating a decrease in \(\Delta G^\circ\) as temperature increases. The accompanying question asks which of the given statements is an incorrect conclusion based on the graph: 1. There exists a certain temperature at which \(\Delta H^\circ = T\Delta S^\circ\). 2. \(\Delta S^\circ > 0\). 3. \(\Delta S^\circ\) increases with temperature while \(\Delta H^\circ\) remains constant. 4. The reaction is spontaneous at high temperatures. 5. \(\Delta H^\circ > 0\).
Transcribed Image Text:The image presents a graph depicting the change in standard Gibbs free energy (\(\Delta G^\circ\)) for a chemical process plotted against absolute temperature (\(T(K)\)). The graph displays a linear relationship with a negative slope, where: - The vertical axis represents \(\Delta G^\circ\), with positive values above the origin and negative values below it. - The horizontal axis represents temperature in Kelvin (\(T(K)\)). - The line crosses the \(\Delta G^\circ\) axis, indicating a decrease in \(\Delta G^\circ\) as temperature increases. The accompanying question asks which of the given statements is an incorrect conclusion based on the graph: 1. There exists a certain temperature at which \(\Delta H^\circ = T\Delta S^\circ\). 2. \(\Delta S^\circ > 0\). 3. \(\Delta S^\circ\) increases with temperature while \(\Delta H^\circ\) remains constant. 4. The reaction is spontaneous at high temperatures. 5. \(\Delta H^\circ > 0\).
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