The equilibrium constant for the reaction AgBr(s) Ag+(aq) + Br– (aq) is the solubility product constant, Ksp = 7.7 × 10–13 at 25°C. Calculate ΔG for the reaction when [Ag+] = 1.0 × 10–2 M and [Br–] = 1.0 × 10–3 M. Is the reaction spontaneous or nonspontaneous at these concentrations? (R = 8.314 J/K • mol) A. ΔG = –97.5 kJ/mol, nonspontaneous B. ΔG = 40.6 kJ/mol, nonspontaneous C. ΔG = 97.5 kJ/mol, spontaneous D. ΔG = 69.1 kJ/mol, nonspontaneous E. ΔG = –69.1 kJ/mol, spontaneous
The equilibrium constant for the reaction AgBr(s) Ag+(aq) + Br– (aq) is the solubility product constant, Ksp = 7.7 × 10–13 at 25°C. Calculate ΔG for the reaction when [Ag+] = 1.0 × 10–2 M and [Br–] = 1.0 × 10–3 M. Is the reaction spontaneous or nonspontaneous at these concentrations? (R = 8.314 J/K • mol) A. ΔG = –97.5 kJ/mol, nonspontaneous B. ΔG = 40.6 kJ/mol, nonspontaneous C. ΔG = 97.5 kJ/mol, spontaneous D. ΔG = 69.1 kJ/mol, nonspontaneous E. ΔG = –69.1 kJ/mol, spontaneous
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter17: Chemcial Thermodynamics
Section: Chapter Questions
Problem 17.59QE: Calculate G for the following reactions and state whether each reaction is spontaneous under...
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The equilibrium constant for the reaction AgBr(s) Ag+(aq) + Br– (aq) is the solubility product constant, Ksp = 7.7 × 10–13 at 25°C. Calculate ΔG for the reaction when [Ag+] = 1.0 × 10–2 M and [Br–] = 1.0 × 10–3 M. Is the reaction spontaneous or nonspontaneous at these concentrations? (R = 8.314 J/K • mol)
A. ΔG = –97.5 kJ/mol, nonspontaneous
B. ΔG = 40.6 kJ/mol, nonspontaneous
C. ΔG = 97.5 kJ/mol, spontaneous
D. ΔG = 69.1 kJ/mol, nonspontaneous
E. ΔG = –69.1 kJ/mol, spontaneous
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