Solid manganese(IV) oxide, $\text{MnO}_2$, catalyses the decomposition of hydrogen peroxide. $2\text{H}_2\text{O}_2(\text{aq}) \rightarrow 2\text{H}_2\text{O}(\ell) + \text{O}_2(\text{g})$. State the type of catalysis shown by this reaction. Explain your answer.
Hydrogen peroxide reacts with iodide ions in acidic conditions according to: $\text{H}_2\text{O}_2 + 2\text{I}^- + 2\text{H}^+ \rightarrow 2\text{H}_2\text{O} + \text{I}_2$. Use the information in Table 3.1 to deduce the rate equation for this reaction. Explain your reasoning.
Use your rate equation from (b)(i) together with the Experiment 1 data to calculate the rate constant, $k$, for this reaction. State the units of $k$.
The thermal decomposition of azomethane, $\text{CH}_3\text{N}=\text{NCH}_3$, is examined. $\text{CH}_3\text{N}=\text{NCH}_3 \rightarrow \text{N}_2 + \text{C}_2\text{H}_6$. Fig. 3.1 shows the results obtained. The reaction is first order with respect to $\text{CH}_3\text{N}=\text{NCH}_3$. Use Fig. 3.1 to calculate two half-lives, $t_{\frac{1}{2}}$, to show that the reaction is first order.
Use your result in (c)(i) to calculate the rate constant, $k$, for the decomposition of azomethane.
Describe the effect that increasing temperature has on the rate constant and on the rate of a reaction.