Catalyst Chemistry Example 1

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Example 1

easy
In the decomposition of hydrogen peroxide, MnO2\text{MnO}_2 acts as a catalyst: 2H2O2→MnO22H2O+O22\text{H}_2\text{O}_2 \xrightarrow{\text{MnO}_2} 2\text{H}_2\text{O} + \text{O}_2. Explain the role of MnO2\text{MnO}_2.

Solution

  1. 1
    MnO2\text{MnO}_2 provides an alternative pathway with lower activation energy for the decomposition.
  2. 2
    It speeds up the reaction but is not consumed — it can be recovered unchanged after the reaction.
  3. 3
    Without the catalyst, H2O2\text{H}_2\text{O}_2 decomposes very slowly at room temperature.

Answer

MnO2 lowers Ea and is not consumed\text{MnO}_2\text{ lowers } E_a\text{ and is not consumed}
Catalysts are essential in both industrial chemistry and biology (where they are called enzymes). They increase reaction rates without altering the products or the equilibrium position.

About Catalyst

A substance that increases the rate of a chemical reaction by providing an alternative pathway with lower activation energy, without being permanently consumed or chemically.

Learn more about Catalyst →

More Catalyst Examples

Example 2 medium

Explain the difference between a homogeneous catalyst and a heterogeneous catalyst. Give one example

Example 3 easy

Enzymes are biological catalysts. Does an enzyme change the [formula] of a biochemical reaction?

Example 4 medium

A catalyst is added to a reaction and the reaction finishes faster. What changes, and what does not

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