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The Catalytic Decomposition of Hydrogen Peroxide

  • Page ID
    3055
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    Chemical Concepts Demonstrated

    • Chemisty of hydrogen peroxide
    • Disproportation reactions
    • Enzyme catalysis

    Demonstration

    • A slice of potato or liver, drops of catalase enzyme (or prick your finger and use your own blood), a small quantity of MnO2, a clean nail and a rusty nail are all added to different crystallizing dishes containing 30% H2O2.
    h2o2.gif

    Observations

    The various items foam in the dishes.


    Explanation (including important chemical equations)

    Hydrogen peroxide undergoes disproportionation. Both oxidation and reduction occur at the same time.

    2 H2O2 (aq) ---> 2 H2O (l) + O2 (g) Enthalpy: -196.1 kJ/mol

    The activation energy of the reaction is about 75 kJ/mol in the absence of catalyst. Platinum metal catalysts can lower the activation energy to about 49 kJ/mol. The catalase enzyme (found in blood) lowers the activation energy to below 8 kJ/mol, which corresponds to an increase in the rate of reaction at physiologial temperatures by a factor of 2 x 10 11 or more.

    Contributors


    The Catalytic Decomposition of Hydrogen Peroxide is shared under a not declared license and was authored, remixed, and/or curated by LibreTexts.

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