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Equilibrium

Equilibrium. Chemical reaction in which reactants are forming as fast as products yet the net concentrations of each remains constant A + B  C + D N 2 + 3H 2  2 NH 3. Equilibrium Constant K. aA + bB  cC + dD K = [C]c [D]d [A]a [B]b

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Equilibrium

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  1. Equilibrium Chemical reaction in which reactants are forming as fast as products yet the net concentrations of each remains constant A + B  C + D N2 + 3H2 2 NH3

  2. Equilibrium Constant K aA + bB  cC + dD K = [C]c [D]d [A]a [B]b Products over reactants

  3. Equilibrium Constant K K > 1000 mostly products K < .001 mostly reactants K = .001 to 1000 equilibrium condition

  4. Lechatlier’s Principle If stress is applied to a system at equilibrium, the system will adjust to relive the stress

  5. Lechatlier’s Principle Possible stresses occur with Concentration, Volume and Temperature

  6. Change in concentration PCl3 + Cl2 PCl5 At equilibrium, the molar concentrations are constant Add PCl5 the reaction will shift to form more PCl3 and Cl2 remove PCl5 the reaction will shift to form less PCl3 and Cl2 Add PCl3 or Cl2 more PCl5 will form Remove PCl3 and Cl2 more will form

  7. Change in volume Reducing the volume or increasing the pressure causes the equilibrium to shift to the side of the equation with the fewest moles N2 g + 3H2 g  2NH3 g 4moles  2 moles H2 g + Br2 g  2HBr g 2moles  2moles

  8. Temperature effects Exothermic Reactants  products + Heat H2 + O2  H2O + 700 Calories Endothermic Heat + Reactants  products CO2 + 2H2 + 90.7 Calories CH3OH

  9. Catalyst effect A catalyst speeds up the rate at which equilibrium is achieved but does not change anything else – this occurs due to lowering the activation energy

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