A poistive catalyst increases the activation energy of the reaction.

Answer

### Step-by-Step Solution:

1. **Understanding the Statement**: The statement claims that a positive catalyst increases the activation energy of a reaction. We need to analyze whether this statement is true or false.

2. **Definition of Positive Catalyst**: A positive catalyst is a substance that increases the rate of a chemical reaction. It does this by providing an alternative reaction pathway.

3. **Role of Activation Energy**: Activation energy is the minimum energy required for a reaction to occur. It is the energy barrier that must be overcome for reactants to be transformed into products.

4. **Effect of Positive Catalyst on Activation Energy**: A positive catalyst does not increase the activation energy; instead, it lowers it. By providing an alternative pathway with a lower activation energy, the catalyst allows more reactant molecules to have enough energy to react.

5. **Graphical Representation**: If we were to plot a graph with energy on the y-axis and the progress of the reaction on the x-axis, the activation energy can be represented as the difference in energy between the reactants and the peak of the energy barrier (transition state). The presence of a catalyst would lower this peak, indicating a decrease in activation energy.

6. **Conclusion**: Since a positive catalyst decreases the activation energy rather than increasing it, the original statement is false.

### Final Answer:
The statement "A positive catalyst increases the activation energy of the reaction" is false. A positive catalyst actually decreases the activation energy, thereby increasing the rate of reaction.

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