$2\text{H}_2\text{O}_2(\text{aq}) \rightarrow 2\text{H}_2\text{O}(\ell) + \text{O}_2(\text{g})$ State the type of catalysis for this reaction. Explain your response.
$\text{H}_2\text{O}_2 + 2\text{I}^{-} + 2\text{H}^{+} \rightarrow 2\text{H}_2\text{O} + \text{I}_2$ The initial rate for this reaction is studied using different concentrations of $\text{H}_2\text{O}_2$, $\text{I}^{-}$ and $\text{H}^{+}$. Use the information in Table 3.1 to deduce the rate equation for this reaction. Explain your reasoning.
Using your rate equation from (b)(i) and the data from Experiment 1, calculate the rate constant, $k$, for this reaction. Include the units of $k$.
$\text{CH}_3\text{N}=\text{NCH}_3 \rightarrow \text{N}_2 + \text{C}_2\text{H}_6$ 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, $t_{1/2}$, to show that the reaction is first order.
Use your answer to (c)(i) to calculate the rate constant, $k$, for the decomposition of azomethane.
Describe the effect of increasing temperature on the rate constant and on the rate of a reaction.