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
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter17: Spontaneity, Entropy, And Free Energy
Section: Chapter Questions
Problem 112CWP: The equilibrium constant for a certain reaction increases by a factor of 6.67 when the temperature...
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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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