CHEM 102 1nd Edition Lecture 21Outline of Last Lecture I. Le Chatelier’s PrincipleII. Effect of PressureIII. Effect of VolumeIV. TemperatureOutline of Current Lecture I. Example of Le Chatelier’s PrincipleII. Effect of a CatalystIII. Application of Le Chatelier’sIV. Relationship Between ΔG and KCurrent LectureI. Example of Le Chatelier’s Principle- For the equation: N2O4 (g) <-> 2NO2 (g); where ΔH = 58.0 kJ- Determine the changes in: [NO2], K, and Equilibrium shift direction for each situationSituation [NO2] K EquilibriumShiftAdd N2O4Increases No change RightRemove NO2Increases No change RightIncrease Pressure Decrease No Change LeftIncrease Volume Increase No Change RightDecrease Temperature Decrease Decrease LeftDecrease Volume Decrease No Change LeftDecrease Pressure Increase No Change RightII. Effect of a Catalyst- A catalyst lowers the activation energy for the forward reaction and the activation energy for the reverse reaction to the same extent- A catalyst does not affect a shift of equilibrium and does not affect K- A catalyst only decrease the time it takes to reach equilibriumIII. Application of Le Chatelier’sThese 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.- Ammonium is synthesized through: N2 (g) + 3H2 (g) ,-> 2NH3 (g) Kc = 3.6e8 and H =-92 kJ/mol- The reaction occurs slowly at 25C. How do you need to adjust temperature and pressure in order to have a more optimized yield?C Kc10 atm 100 atm 1000 atm209 650 51 82 98467 0.5 4 25 80758 0.014 0.5 5 13IV. Relationship Between ΔG and K- G = G(initial) + RTlnQ- At equilibrium, Q = K and G =
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