Explain what is meant by order of reaction.
Complete Table 4.1 by giving the order of reaction for $[\text{H}^+]$, $[\text{I}^-]$, and $[\text{H}_2\text{O}_2]$, and therefore the overall order of the reaction.
On Fig. 4.1, sketch a line that shows how $[\text{I}^-]$ changes with time.
Two experiments are used to measure the rate of reaction 2. In the first experiment, the initial rate is measured with known concentrations of $\text{NO}_2$ and $\text{O}_3$. In the second experiment, the concentrations of $\text{NO}_2$ and $\text{O}_3$ are both multiplied by four. Predict how the initial rate for reaction 2 changes.
The mechanism for reaction 2 contains two steps. Define rate-determining step.
Suggest equations for the two steps in the mechanism for reaction 2.
From Fig. 4.2, calculate a value for the rate constant, $k$, for this decomposition.
Using your answer to c(i), calculate the half-life, $t_{\frac{1}{2}}$, in seconds, for this decomposition.