CHEM 113 1st Edition Lecture 16 Outline of Last Lecture I. Le Chatelier’s PrincipleII. The Effect of ConcentrationIII. The Effect of PressureIV. The Effect of TemperatureV. The Effect of CatalystsOutline of Current Lecture - Equilibrium problem- Clicker Question point- Synthesis of Ammonia- Biosynthesis of isoleucine from threonineCurrent Lecture- Last Equilibrium Problemo Problem 17.15These 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.o To solve this problem, we must first write the expression for Q to investigate the equilibrium. Now we must calculate Q for each scene and the scene that produces Q=K, represents the equilibrium. Comparing Q and K will also help us to determine the direction of the reaction. To find the concentration of each molecule, in this case we simply count the particles for each scene. We know now the following Q values- Scene 1: Q=15- Scene 2: Q=2.0- Scene 3: Q=0.33o For part A where K=2, scene 2 is the correct response because here Q=2o Part B is asking us what is happening in the other two scenes. In scene 1, Q>K therefore the system will proceed towards the reactants. In scene 3, Q<K so the system will proceed towards the products. This is something from a previous lecture.o Part C requires us to look at the H value. It is given that delta H is greater than 0, which means it is an endothermic reaction. From the last lecture we know that when temperature increases, if the reaction is endothermic, it will favor the products.Point brought up by the clicker question- Remember to note the difference between a change in pressure in an overall environment versus a change in pressure of an equilibrium- When looking at an equilibrium problem, inert gases (see heterogeneous equilibrium) do not affect traits of equilibrium at all.The Synthesis of Ammonia- Case study on how Le Chatelier’s principle affects the synthesis of ammonia (NH3)- The N atom is very hard to “fix”, meaning combine with other atoms into useful compounds.- But it can be manipulated industrially through the Haber process- To make this reaction economical, there are three ways to maximize the yield of NH3o 1). Decrease [NH3] by removing NH3 as it forms.o 2). Decrease the volume (increase the pressure) At very high pressure and low temperature, the yield is high but the rate is low. Figure 17.22 shows industrial conditions and how they maximize the yield.o 3). Decrease the temperature An increase in temperature causes the equilibrium to shift towards the reactants, since the reaction is exothermic.Biosynthesis of isoleucine from threonine- Isoleucine is synthesized from threonine in a sequence of five enzyme-catalyzed reactions.- Once enough isoleucine is present, a process called end-product feedback inhibition occurs where the build up of the product inhibits the production of itself, by blocking thefirst enzyme