CHEM 1442 1st Edition Lecture 2Outline of Last Lecture I. ExamplesII. Physical Transformations of Pure SubstancesIII. Phase DiagramsIV. BondsV. Intermolecular ForcesVI. Comparing Intermolecular ForcesOutline of Current Lecture VII. Molecular GastronomyVIII. Vapor PressureIX. Chapter 16: Kinetics Current LectureMolecular Gastronomy- Science of cooking- “What causes aromas?”o Volatile substances (Aromatic Substances)o “Volatile” – easy to evaporateo How do you compare which molecules are volatile?Vapor PressureRate = Speed (where temperature is constant)These 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.Why does rate of condensation increase but not vaporization?- Because vaporization starts outgoing faster; it is vaporizing first. Condensation increases because there is nothing in the gaseous phase yet.Pressure is increasing because now there is more gas. Originally, there is a vacuum in the container.(Dynamic) Equilibrium = rate of vaporization = rate of condensation- The rate of a forward process = the rate of its reverse process- Equilibrium is indicated by the double arrow- Once the equilibrium is reached, then the equilibrium remains until you disturb the system.- The amount of gas does not change once the equilibrium is reached.Vapor pressure is the pressure of vapor at dynamic equilibrium- The higher the vapor pressure, the more volatile- The higher the vapor pressure, the lower the intermolecular forces because it is easier tobreak the molecule apart- Vapor pressure is temperature-dependento As temperature increases, vapor pressure increasesCommon Misconceptions about Equilibrium:- Amount of water (liquid) = Amount of water (gas) WRONG!- The amount of gas remains the same once the equilibrium is reached because the process stops: No vaporization. No condensation. WRONG!Chapter 16: KineticsStudy of Reaction Speed (Rate of Reaction)A + B C + DTwo (actually three) things need for a reaction to happen:1. A and B need to meet2. A and B must have enough “energy”A “faster” reaction requires:1. A and B meet often (frequency)2. Increasing temperature = increasing energyHow conditions affect rate:1. Higher concentration = faster rate reaction (they meet more frequently)2. Higher temperature = faster rate reaction (more