We will use the chemical reaction (called the Haber process, 1st process to fix nitrogen to ammonia industrially) that are in your Equilibrium Notes 3 to show LeChatelier's Principle. 1 N2 (g) + 3 H2 (g) <==> 2 NH3 (g) + Energy (i.e. exothermic rxn) You will use the following template to answer your LeChatlelier's Principle example. You may choose any Stress you want expect the following, i) Add catalyst, ii) Add products, iii)Decreasing temperature, and iv) Decreasing pressure. You should follow work shown in Equilibrium Notes 3. Stress: _______________________________________________________________ How rxn tries to remove stress: _________________________________________________ Circle: Make more product or more reactant (fill in for pressure changes)__________________ Circle: Favoring: Forward rxn or Backward rxn: (fill in for temperature changes) _____________ Circle: Shift Equilibrium to: Left(more reactant) or Right (more product) Side 4 (Find an "real life" application of Equilibrium, chemistry related or not) 1) Write the reversible reaction (even if it is not a chemical system). 2) Draw a picture of the equilibrium condition for this system including what you think the value K (Equilibrium constant) by noting ratio of reactant to product you draw. 3) Explain one way to stress this system out and explain waht LeChatelier's Principle says including drawing a "new Equilibrium bucket" along with "original Equilibrium bucket". |