Chem 113 1st Edition Lecture 21 Outline of Last Lecture I. Solving Equilibrium ProblemsOutline of Current Lecture II. The Simplifying AssumptionIII. Correlating Reaction Direction with ΔG°IV. Manipulating the relationship between ΔG and QCurrent LectureI. The Simplifying Assumptiona. We assume that x ([A]reacting) can be neglected ifi. Kc is relatively smallii. [A]init is relatively largeb. If [ A ]initKc>400, the assumption is justifiedi. Neglecting x introduces an error <5%c. If [ A ]initKc<400, the assumption is not justifiedi. Neglecting x introduces an error >5%II. Correlating Reaction Direction with ΔG°a. ΔG° refers to standard state conditions, which is when all substances are 1 atm or1M.b. Under these conditions Qc = 1 and Qc > Kc, so the forward reaction is NOT spontaneous, however the reverse reaction IS spontaneousc. Under nonstandard conditions, the change in Gibbs energy can be found by usingthe following equationi. ΔG = ΔG° + RT lnQThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.III. Manipulating the relationship between ΔG and Qa. At equilibrium, Q=K and ΔG=0i. ΔG° = −RT lnKb. The ΔG° of a reaction in the gas phase relates to the Kp valuec. The ΔG° of a reaction in the in solution relates to the Kc
View Full Document
Unlocking...