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IB Chemistry Power Points


                             Topic 7
                          Equilibrium

www.pedagogics.ca




                    Topic 7.1
Equilibrium: “the extent of a reaction”
   Recall: for a chemical reaction
         actual yield < theoretical yield

   Why? Because
     • Reactants are not pure
     • Not all product is recovered
     • Other competing reactions use up
       reactant to form alternate products

      and some chemical reactions are reversible!
   Equilibrium looks at the extent (of completion)
   of a reversible chemical reaction.
Equilibrium: the extent of a reaction
    Equilibrium = no observable changes over time

    In chemistry we encounter two types of equilibrium
    systems.


Physical/phase equilibrium      Chemical equilibrium
H2O (l)      H2O (g)           N2O4 (g)     2NO2 (g)
Equilibrium: the extent of a reaction
    Equilibrium = no observable changes over time

    In chemistry we encounter two types of equilibrium
    systems.


Physical/phase equilibrium
H2O (l)      H2O (g)
Equilibrium: the extent of a reaction
    Equilibrium = no observable changes over time

    In chemistry we encounter two types of equilibrium
    systems.


Physical/phase equilibrium      Chemical equilibrium
H2O (l)      H2O (g)           N2O4 (g)     2NO2 (g)
Equilibrium: the extent of a reaction
A chemical equilibrium is achieved when:
•     the rates of the forward and reverse reactions are equal and
•     the concentrations of the reactants and products remain constant



    for example
    • Colorless N2O4 decomposes to brown NO2 at room temperature. The
      reaction is reversible.
                              N2O4(g)  2NO2(g).
    • At equilibrium, there is a mixture of N2O4 and NO2.
    • The reaction does not stop.
    • The color remains constant
Key concept 1: at equilibrium, concentrations are constant
Constant concentrations imply that the forward
reaction must be proceeding at the same rate as the
reverse reaction.
                  N2O4(g)     2 NO2(g)
              This is the forward reaction

                2 NO2(g)      N2O4(g).
             This is the reverse reaction

The double arrow implies the process is reversible.
              N2O4(g)          2NO2(g)
Key concept 2: at equilibrium, forward rate = reverse rate


               N2O4(g)     2 NO2(g)




                     2 NO2(g)      N2O4(g)



    “dynamic” implies that at equilibrium
    the reaction continues in both directions

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2012 topic 7.1

  • 1. IB Chemistry Power Points Topic 7 Equilibrium www.pedagogics.ca Topic 7.1
  • 2. Equilibrium: “the extent of a reaction” Recall: for a chemical reaction actual yield < theoretical yield Why? Because • Reactants are not pure • Not all product is recovered • Other competing reactions use up reactant to form alternate products and some chemical reactions are reversible! Equilibrium looks at the extent (of completion) of a reversible chemical reaction.
  • 3. Equilibrium: the extent of a reaction Equilibrium = no observable changes over time In chemistry we encounter two types of equilibrium systems. Physical/phase equilibrium Chemical equilibrium H2O (l) H2O (g) N2O4 (g) 2NO2 (g)
  • 4. Equilibrium: the extent of a reaction Equilibrium = no observable changes over time In chemistry we encounter two types of equilibrium systems. Physical/phase equilibrium H2O (l) H2O (g)
  • 5. Equilibrium: the extent of a reaction Equilibrium = no observable changes over time In chemistry we encounter two types of equilibrium systems. Physical/phase equilibrium Chemical equilibrium H2O (l) H2O (g) N2O4 (g) 2NO2 (g)
  • 6. Equilibrium: the extent of a reaction A chemical equilibrium is achieved when: • the rates of the forward and reverse reactions are equal and • the concentrations of the reactants and products remain constant for example • Colorless N2O4 decomposes to brown NO2 at room temperature. The reaction is reversible. N2O4(g)  2NO2(g). • At equilibrium, there is a mixture of N2O4 and NO2. • The reaction does not stop. • The color remains constant
  • 7. Key concept 1: at equilibrium, concentrations are constant
  • 8. Constant concentrations imply that the forward reaction must be proceeding at the same rate as the reverse reaction. N2O4(g) 2 NO2(g) This is the forward reaction 2 NO2(g) N2O4(g). This is the reverse reaction The double arrow implies the process is reversible. N2O4(g) 2NO2(g)
  • 9. Key concept 2: at equilibrium, forward rate = reverse rate N2O4(g) 2 NO2(g) 2 NO2(g) N2O4(g) “dynamic” implies that at equilibrium the reaction continues in both directions