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Intros
Lessons
  1. The effect of catalysts
  2. Why are catalysts important to chemists?
  3. How catalysts affect mechanism and potential energy.
  4. Reaction profile with and without a catalyst.
  5. Heterogeneous catalysts.
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Examples
Lessons
  1. Explain the use of catalyst and their effect on the energy profile of a reaction.
    The decomposition of hydrogen peroxide is shown in the equation below:

    2H2O22H2O+O2\mathrm{2H_2O_2 \to 2 H_2O + O_2}

    1. This reaction is slow but is sped up with a catalyst such as potassium iodide. Show the uncatalyzed and catalyzed reaction pathways on a potential energy diagram. Assume the reaction is exothermic and the catalyzed pathway forms an intermediate.
  2. Explain the use of catalyst and their effect on the energy profile of a reaction.
    The Haber process is an important industrial process to produce ammonia. The equation is below:

    3H2(g)+N2(g)2NH3(g)\mathrm{3H_{2 (g)} + N_{2 (g)} \rightleftharpoons 2NH_{3 (g)} }

    1. For practical reasons, this reaction is always performed with an iron-based catalyst. Explain why this is used and its effect on the position of equilibrium.
    2. Draw two energy profiles for this exothermic reaction, showing a catalyzed and a possible uncatalyzed pathway. Label the reactants and products on these profiles.