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Equilibrium

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  1. Equilibrium • Equilibrium is when the rate of forward is the same as reverse; • this refers to speed of the reaction; concentration will remain unchanged, • this does not mean the concentration is equal or must have the same value for each side.

  2. Equilibrium! Only the following will shift a reaction at equilibrium: 1. Change in concentration: If you add more reactant = make more product (R) If you add more product = make more reactant (L)

  3. Remove reactant/remove product Remove reactant = replaces reactant (L) Remove product = replaces product (R)

  4. 3. Change in pressure (must all be gases in equation) Increase pressure = less space = shift to side with smallest amount of moles Decrease pressure = more space = shift to side with greatest amount of moles

  5. Do not be fooled! Change in volume is just another way to say change in pressure!

  6. Change in temperature. Exothermic = heat is a product; heat is released Endothermic = heat is a reactant; heat is absorbed

  7. Test Yourself! 4NH3(g) + 5O2(g)  4NO(g) + 6H2O(g) + heat Which way will the equilibrium shift for the above reaction? • Increase concentration of oxygen • Increase the pressure • Increase the temperature • Remove NO

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