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Van't Hoff studied the temperature dependence of the equilibrium constant, K, using two expressions for the standard Free Energy of a reaction; AG° = - RT In K and AG° = AH° - TAS°. These can be combined in the form of a linear equation, which allows the calculation of the standard enthalpy and entropy changes of a reaction, based on the change of the equilibrium constant, K, with temperature. AH° AS In K = - (*)-(A) R R A reaction is carried out at two temperatures, in an ice bath (0.00°C) and in a boiling water bath (100.00°C). The equilibrium constant, K, is determined at each temperature. At 0.00°C, its value is 5.50E-4. At 100.00°C, its value is 3.22E-4. From this information, determine the values of the following thermodynamic functions for this reaction. Assume that AH° and AS° are independent of temperature, which is generally true over small temperature ranges. What is the value of AH°, in kJ? Submit Answer Tries 0/99 What is the value of AS°, in J/K? Submit Answer Tries 0/99

Van't Hoff studied the temperature dependence of the equilibrium constant, K, using two expressions for the standard Free Energy of a reaction; AG° = - RT In K and AG° = AH° - TAS°. These can be combined in the form of a linear equation, which allows the calculation of the standard enthalpy and entropy changes of a reaction, based on the change of the equilibrium constant, K, with temperature. AH° AS In K = - (*)-(A) R R A reaction is carried out at two temperatures, in an ice bath (0.00°C) and in a boiling water bath (100.00°C). The equilibrium constant, K, is determined at each temperature. At 0.00°C, its value is 5.50E-4. At 100.00°C, its value is 3.22E-4. From this information, determine the values of the following thermodynamic functions for this reaction. Assume that AH° and AS° are independent of temperature, which is generally true over small temperature ranges. What is the value of AH°, in kJ? Submit Answer Tries 0/99 What is the value of AS°, in J/K? Submit Answer Tries 0/99

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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Van’t Hoff equation at two separate temperatures; I have an idea of where to start but still am confused
Van't Hoff studied the temperature dependence of the equilibrium constant, K, using two expressions for the standard Free Energy of a reaction; AG° = - RT In K and AG° = AH° - TAS°. These can be combined in the form of a linear equation, which allows the calculation of the standard enthalpy and entropy changes of a reaction, based on the change of the equilibrium constant, K, with temperature. AH° AS In K = - (FDG) A reaction is carried out at two temperatures, in an ice bath (0.00°C) and in a boiling water bath (100.00°C). The equilibrium constant, K, is determined at each temperature. At 0.00°C, its value is 5.50E-4. At 100.00°C, its value is 3.22E-4. From this information, determine the values of the following thermodynamic functions for this reaction. Assume that AH° and AS° are independent of temperature, which is generally true over small temperature ranges. What is the value of AH°, in kJ? Submit Answer Tries 0/99 What is the value of AS°, in J/K? Submit Answer Tries 0/99
Transcribed Image Text:Van't Hoff studied the temperature dependence of the equilibrium constant, K, using two expressions for the standard Free Energy of a reaction; AG° = - RT In K and AG° = AH° - TAS°. These can be combined in the form of a linear equation, which allows the calculation of the standard enthalpy and entropy changes of a reaction, based on the change of the equilibrium constant, K, with temperature. AH° AS In K = - (FDG) A reaction is carried out at two temperatures, in an ice bath (0.00°C) and in a boiling water bath (100.00°C). The equilibrium constant, K, is determined at each temperature. At 0.00°C, its value is 5.50E-4. At 100.00°C, its value is 3.22E-4. From this information, determine the values of the following thermodynamic functions for this reaction. Assume that AH° and AS° are independent of temperature, which is generally true over small temperature ranges. What is the value of AH°, in kJ? Submit Answer Tries 0/99 What is the value of AS°, in J/K? Submit Answer Tries 0/99
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