CHEM 102 1nd Edition Lecture 20Outline of Last Lecture I. Reaction QuotientII. Use K and Initial ConcentrationsIII. ExamplesIV. Le Chatelier’s PrincipleOutline of Current Lecture I. Le Chatelier’s PrincipleII. Effect of PressureIII. Effect of VolumeIV. TemperatureCurrent LectureI. Le Chatelier’s Principle- An increase in the reactant concentration will shift equilibrium to the right- A decrease in the reactant concentration will shift equilibrium to the left- Increase in product concentration will shift equilibrium to the left- Decrease in reactant concentration will shift equilibrium to the rightII. Effect of Pressure- In reactants where n = 0, volume or pressure changes do not affect equilibrium concentrations- In reactions where n does not equal 0, the pressure changes will affect the equilibrium concentrations.- If the pressure increases, there is more stress on the side with moles, The equilibrium will shift toward side with less moles- If the pressure decreases, there is less stress on the side with moles The equilibrium will shift toward the side with more moles- Changes involving inert gases do not affect equilibrium- Changes involved the amount of liquid or solids do not affect equilibriumIII. Effect of Volume- In reactants where n = 0, volume or pressure changes do not affect equilibrium concentrationsThese 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.- In reactions where n does not equal 0, the volume changes will affect the equilibrium concentrations.- If the volume decreases, there is more stress on the side with moles, The equilibrium will shift toward side with less moles- If the volume increases, there is less stress on the side with moles The equilibrium will shift toward the side with more moles- Changes involving inert gases do not affect equilibrium- Changes involved the amount of liquid or solids do not affect equilibriumIV. Temperature Changes- Temperature increases favor endothermic reactions Shift to the right Kc will increase- Temperature decreases favor exothermic reactions Shift to the left Kc will
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