Gibbs Free Energy & the Equilibrium Constant | ΔG° = -RTlnK | 18.5 General Chemistry

Chad concludes the chapter on Thermodynamics with a lesson on the relationship between Gibbs Free Energy and the Equilibrium Constant. The lesson begins with a discussion of the mathematical relationship between the nonstandard free energy change, the standard free energy change, and the reaction quotient. ΔG = ΔG° + RTlnQ An example calculation of the change in Gibbs free energy under nonstandard conditions is performed. This equation also allows us to draw the following three conclusions: 1. If Q is less than K, then ΔG is negative. 2. If Q is greater than K, then ΔG is positive. 3. If Q is equal to K, then ΔG = 0. The relationship between the standard Gibbs free energy change and the equilibrium constant is then derived from this equation. ΔG° = -RTlnK This equation can be used to calculate the standard Gibbs free energy change at a particular temperature from the equilibrium constant, or to calculate the equilibrium constant at a particular temperature from the standard Gibbs free energy change. An example calculation of the latter is performed. Finally, a graphical representation of Gibbs free energy vs reaction progress is presented. A number of thermodynamic quantities are identified on the graph including the standard Gibbs free energy change, nonstandard delta G, the equilibrium constant and the reaction quotient. I've embedded this playlist as a course on my website with all the lessons organized by chapter in a collapsible menu and much of the content from the study guide included on the page. Check this lesson out at https://www.chadsprep.com/chads-gener... If you want all my study guides, quizzes, final exam reviews, and practice exams, check out my General Chemistry Master Course at https://www.chadsprep.com/genchem-you... 00:00 Lesson Introduction 00:25 Nonstandard ΔG 07:47 ΔG° = -RTlnK 18:28 Graph of ΔG vs Reaction Progress https://www.chadsprep.com/ #generalchemistry #chemistrytutorial #gibbsfreeenergy