Silver chloride is broken down in this equilibrium reaction: AgCl(s) <--> Ag+(aq) + Cl− (aq). Given the standard enthalpies of formation: HfAgCl= 127.07, HfAg+ = 110, and HfCl- = -190 and their standard entropy values: SAgCl = 100.6, SAg+ = 58.37, and SCl- = 24.90, calculate the reaction's change in free energy (delta Grxn).
Silver chloride is broken down in this equilibrium reaction: AgCl(s) <--> Ag+(aq) + Cl− (aq). Given the standard enthalpies of formation: HfAgCl= 127.07, HfAg+ = 110, and HfCl- = -190 and their standard entropy values: SAgCl = 100.6, SAg+ = 58.37, and SCl- = 24.90, calculate the reaction's change in free energy (delta Grxn).
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter16: Thermodynamics: Directionality Of Chemical Reactions
Section: Chapter Questions
Problem 101QRT: Appendix J lists standard molar entropies S, not standard entropies of formation rS. Why is this...
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Silver chloride is broken down in this equilibrium reaction: AgCl(s) <--> Ag+(aq) + Cl− (aq).
Given the standard enthalpies of formation: HfAgCl= 127.07, HfAg+ = 110, and HfCl- = -190 and their standard entropy values: SAgCl = 100.6, SAg+ = 58.37, and SCl- = 24.90, calculate the reaction's change in free energy (delta Grxn).
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