8. If you add enough acid, you will convert all carbonate ions in solution to carbonic acid (H₂CO3). Using the thermodynamic information below, calculate the standard Gibbs free energy (kJ/mol) of this reaction: C(s) + O2(g) → CO₂(g) C(s) + O2(g) → CO₁² (aq) CO₂(g) + H₂O(1)→ H₂CO3(aq) AG=211.8 kJ/mol AH-393.5 kJ/mol; AS°=213.8 J/mol K AH-677.1 kJ/mol; AS°= -56.9 J/mol K AH-20.1 kJ/mol; AS°= -97.3 J/mol K

8. If you add enough acid, you will convert all carbonate ions in solution to carbonic acid (H₂CO3). Using the thermodynamic information below, calculate the standard Gibbs free energy (kJ/mol) of this reaction: C(s) + O2(g) → CO₂(g) C(s) + O2(g) → CO₁² (aq) CO₂(g) + H₂O(1)→ H₂CO3(aq) AG=211.8 kJ/mol AH-393.5 kJ/mol; AS°=213.8 J/mol K AH-677.1 kJ/mol; AS°= -56.9 J/mol K AH-20.1 kJ/mol; AS°= -97.3 J/mol K

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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