CHEM 135 1st Edition Lecture 16 Outline of Last Lecture I. Chemical Equilibriuma. Introductionb. DefinitionII. Reversible reactions and Equilibrium Constanta. Definitionsb. Equationsc. ExamplesIII. Heterogeneous Equilibriuma. Definitionb. ExamplesOutline of Current Lecture I. Calculating equilibrium constanta. Examplesb. Kc vs. KpII. Reaction Quotienta. Equation/definitionb. ExamplesCurrent LectureCalculating equilibrium constant from measured concentrationsEx.I2(g) ⇌ 2I(g) Kc=0.011, [I2]eq=0.1M, [I]2=?Keq=[I ]2[I2][I ]2=Keq×[I2][I]eq=0.033 MThese 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.Kc concentrationKp partial pressure The relationship between the two constants is as follows: Kp=Kc(RT)∆nEx. PCl5 decomposes to PCl3 and Cl2. If the initial concentration of PCl5= .200M and it’s final concentration is .120M, what is the equilibrium constant?1. Create an ICE table PCl5PCl3Cl2Initial 0.02 0.0 0.0Change -0.08 +0.08 +0.08Equilibrium 0.12 0.08 0.08Cl¿¿2¿eq¿PCl¿¿¿PC l3¿eq¿¿Keq=¿¿(0.08)(0.08)(0.12)=0.0533Reaction Quotient (Q)K=[products][reactants](at equilibrium) Q=[products][reactants](at any point ∈the reaction)- The reaction quotient determines which direction the reaction will take place. o Q<K= majority of reactants, move to the right to reach eq., RPo Q>K= majority of products, move to the left to reach eq., PREx. The equilibrium constant for the reaction is 2A ⇌ 3B is 2.3. If [A]= 0.10M and [B]=0.050M, which direction will the reaction take place?B ¿3¿A ¿2¿¿Q=¿Q=0.125Q<K, the reaction must proceed to the