15.1 Chemical Equilibrium and Equilibrium Constants | General Chemistry

Chad provides a comprehensive lesson on Equilibrium and Equilibrium Constants. First, what is meant by a dynamic equilibrium. When a reaction reaches equilibrium, it is not that the reaction has stopped completely, it is just that it is proceeding in both the forward and reverse directions at the same rate (Forward Rate = Reverse Rate).

Second, equilibrium constants (K) and the law of mass action are introduced. Equilibrium constant expressions are first defined as the ratio of the concentrations of products to reactants and how that typically only aqueous and gaseous species are included. The difference between Kc and Kp is also explained as the equilibrium constant can be written in terms of molar concentrations or partial pressures for reactions involving gases. How to calculate Kp having been given Kc is also demonstrated using a provided equation.

Finally, being given an equilibrium constant for a reaction, it is shown how to determine the equilibrium constant for reactions that are related to the first by a simple stoichiometric ratio (reducing all coefficients by half for instance).

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00:00 Lesson Introduction
00:28 Introduction to Dynamic Equilibrium
02:36 Introduction to Equilibrium Constants
14:42 Kc vs Kp
22:22 Calculating Equilibrium Constants of Related Reactions

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