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The equilibrium constant for the equation       HNO2 (aq)  +  H2O (l)    ⇌    H3O+ (aq)  +  NO2− (aq) is Ka = 5.6 × 10−4 M at 25.0 °C. a) Calculate the value of ΔG°rxn, in kJ/mol, at 25.0 °C. b) Calculate the value of ΔGrxn, in kJ/mol, at 25.0 °C when [NO2−] = [H3O+] = 1.0 ×10−5 M and [HNO2] = 1.00 M.

The equilibrium constant for the equation       HNO2 (aq)  +  H2O (l)    ⇌    H3O+ (aq)  +  NO2− (aq) is Ka = 5.6 × 10−4 M at 25.0 °C. a) Calculate the value of ΔG°rxn, in kJ/mol, at 25.0 °C. b) Calculate the value of ΔGrxn, in kJ/mol, at 25.0 °C when [NO2−] = [H3O+] = 1.0 ×10−5 M and [HNO2] = 1.00 M.

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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The equilibrium constant for the equation

      HNO2 (aq)  +  H2O (l)    ⇌    H3O+ (aq)  +  NO2− (aq)

is Ka = 5.6 × 10−4 M at 25.0 °C.

a) Calculate the value of ΔG°rxn, in kJ/mol, at 25.0 °C.

b) Calculate the value of ΔGrxn, in kJ/mol, at 25.0 °C when [NO2−] = [H3O+] = 1.0 ×10−5 M and [HNO2] = 1.00 M. 

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