From the values of ΔH and ΔS, predict which of the following reactions would be spontaneous at 25°C: Reaction A: ΔH= 10.5 kJ/mol, ΔS= 30 J/K. mol; Reaction B: ΔH =1.8 kJ/mol, ΔS= -113 J/K.mol. If either of the reactions is nonspontaneous at 25°C, at what temperature might it become spontaneous?
From the values of ΔH and ΔS, predict which of the following reactions would be spontaneous at 25°C: Reaction A: ΔH= 10.5 kJ/mol, ΔS= 30 J/K. mol; Reaction B: ΔH =1.8 kJ/mol, ΔS= -113 J/K.mol. If either of the reactions is nonspontaneous at 25°C, at what temperature might it become spontaneous?
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy
Section: Chapter Questions
Problem 68SCQ: Explain why each of the following statements is incorrect. (a) Entropy increases in all spontaneous...
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From the values of ΔH and ΔS, predict which of the following reactions would be spontaneous at 25°C: Reaction A: ΔH= 10.5 kJ/mol, ΔS= 30 J/K. mol; Reaction B: ΔH =1.8 kJ/mol, ΔS= -113 J/K.mol. If either of the reactions is nonspontaneous at 25°C, at what temperature might it become spontaneous?
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