AP Chemistry
9.6 Free Energy of Dissolution
9.3 Gibbs Free Energy and Thermodynamic Favorability
The dissolution of a solid ionic compound, \(\text{MX}(s)\), in water is represented by the equation below.
\[ \text{MX}(s) \rightleftharpoons \text{M}^+(aq) + \text{X}^-(aq) \]
During the dissolution, the energy required to separate the ions from the crystal lattice exceeds the energy released by the hydration of the ions, resulting in an endothermic process (\(\Delta H^\circ_{\text{soln}} > 0\)). If \(\text{MX}(s)\) dissolves spontaneously in water at \(298\text{ K}\), which of the following statements best explains why the dissolution is thermodynamically favorable?
\[ \text{MX}(s) \rightleftharpoons \text{M}^+(aq) + \text{X}^-(aq) \]
During the dissolution, the energy required to separate the ions from the crystal lattice exceeds the energy released by the hydration of the ions, resulting in an endothermic process (\(\Delta H^\circ_{\text{soln}} > 0\)). If \(\text{MX}(s)\) dissolves spontaneously in water at \(298\text{ K}\), which of the following statements best explains why the dissolution is thermodynamically favorable?
Similar Questions
Tools for a 5
AP aligned mock tests to help you get a 5.
With grading, adaptive explanations, and more.
Find a Quiz
Find, solve, and grade every AP FRQ ever.
Find an FRQ
Stuck on AP Chemistry? Get unstuck with an AP specialist.1 to 1 tutors who know the exam inside out. Understand weeks of material in a single session.Book a SessionSee all our elite tutors
Learn AP Physics from scratch, quickly. This is the only course you'll need for the year.
A self-paced course with everything you need to get a 5. Trusted by over 15,000 students and 200+ schools. Learn fast, or we'll refund your purchase, backed by our 100% satisfaction guarantee.
Explore the Course