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16-3: Le Chatelier’s Principle

16-3: Le Chatelier’s Principle. Le Chatelier’s Principle . If a change is made to a system at equilibrium, the rxn will shift in the direction that will allow it re-establish equilibrium. Concentration .

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16-3: Le Chatelier’s Principle

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  1. 16-3: Le Chatelier’s Principle

  2. Le Chatelier’s Principle • If a change is made to a system at equilibrium, the rxn will shift in the direction that will allow it re-establish equilibrium

  3. Concentration • Adding more of something increases the concentration and will cause the rxn to shift to the other side • Taking something out causes a decrease in conc. and the rxn will shift to that side

  4. Why is it useful? • Le Chatelier’s Principle can be used to maximize the amount of product that a reaction produces.

  5. How would you use a change in concentration to maximize the products? • 2H2(g) + O2(g) 2H2O(g) • If, at equilibrium, there are more reactants than products, take away water as it is produced

  6. Pressure • For gaseous equilibrium systems • If pressure is increased, the rxn will shift in the direction that produces fewer gaseous moles

  7. 2H2(g) + O2(g) 2H2O(g) • 3 moles of gaseous reactants, 2 moles of gaseous products • Increase the pressure. This will push it to the side with fewer gaseous mols.

  8. Temperature • Value of the equilibrium constant depends upon the temperature

  9. Temperature • Is the rxn exothermic or endothermic? • Exothermic – gives off heat. If given heat, absorbs it in the reverse rxn. • Endothermic – requires heat. If heat is taken away, it gets more from the reverse reaction. • Think of heat as a reactant or product.

  10. Temperature • Exothermic: A + B  C + heat • To increase rate, cool it. • Endothermic: A + heat  B + C • To increase rate, heat it.

  11. Temperature • Reaction rate is important, though. • If you cool a rxn too much, the particles do not collide and little to no reaction will occur.

  12. Haber Process • Developed by German chemist, Fritz Haber, during WWI to help Germany produce ammonia for use in explosives

  13. Haber and Einstein

  14. Haber Process • N2 (g) + 3H2(g)  2NH3 (g) + heat • Removed ammonia as it was produced • Increased pressure • 4 mols gaseous reactants, 2 moles gaseous products.

  15. Haber Process • 1914: Haber made head of chemical warfare service, works on gases for chemical warfare • 1918: Haber wins the Nobel Prize in Chemistry • 1933: Haber (who is Jewish) leaves Germany, as Hitler gains more power

  16. Haber Process • Today, the Haber process is still used to make ammonia for fertilizers and cleaning products

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