Question

The addition ${\mathrm{MnO}}_2$ to ${\mathrm{KClO}}_3$ decreases the temperature at which ${\mathrm{KClO}}_3$ decomposes because ${\mathrm{MnO}}_2$ added acts as a _______ catalyst.

Answer 1

Step-I

Positive catalyst:- This catalyst can be considered as the catalyst which initiates the reaction to take place at a faster rate.

For Example:- $$\begin{gathered} {\mathrm{KClO}}_3\underset{{\mathrm{MnO}}_2}{\overset{∆}{\to }}2\mathrm{KCl}+3{\mathrm{O}}_2 \\ (\mathrm{Potassium}(\mathrm{potassium}\left(\mathrm{oxygen}\right) \\ \mathrm{chlorate})\mathrm{chloride}) \end{gathered}$$

When potassium chlorate $\left({\mathrm{KClO}}_3\right)$ is heated in the presence of manganese dioxide $\left({\mathrm{MnO}}_2\right)$ catalyst then, it will decompose to form potassium chloride $\left(\mathrm{KCl}\right)$ and oxygen gas.

In this reaction, ${\mathrm{MnO}}_2$ (manganese dioxide) is acting like a positive catalyst.

This is because it is enhancing the rate of the reaction.