Ch. 17 - Chemical ThermodynamicsSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: The equilibrium constant for the reaction:  AgBr(s) ⇌  Ag+(aq) + Br-(aq) is the solubility product constant, Ksp= 7.7 x 10 -13 at 25°C. Calculate ΔG for the reaction when [Ag+] = 1.0 x 10-2 M and [Br-] = 1.0 x 10-3 M. Is the reaction spontaneous or nonspontaneous at these concentrations? A. ΔG = 69.1 kJ, nonspontaneous B. ΔG = -97.5 kJ, spontaneous C. ΔG = 40.6 kJ, nonspontaneous D. ΔG = -69.1 kJ, spontaneous E. ΔG = 97.5 kJ, nonspontaneous

Problem

The equilibrium constant for the reaction: 

AgBr(s) ⇌  Ag+(aq) + Br-(aq)

is the solubility product constant, Ksp= 7.7 x 10 -13 at 25°C. Calculate ΔG for the reaction when [Ag+] = 1.0 x 10-2 M and [Br-] = 1.0 x 10-3 M. Is the reaction spontaneous or nonspontaneous at these concentrations?

A. ΔG = 69.1 kJ, nonspontaneous
B. ΔG = -97.5 kJ, spontaneous
C. ΔG = 40.6 kJ, nonspontaneous
D. ΔG = -69.1 kJ, spontaneous
E. ΔG = 97.5 kJ, nonspontaneous