Explain what is meant by the order of a reaction.
Complete Table 3.2 to state the order of reaction with respect to $[\text{IO}_3^{-}]$, $[\text{H}^+]$, and $[\text{I}^-]$, and the overall order of reaction.
Use your answer to (a)(ii) to sketch lines in Fig. 3.1 to show the relationship between the initial rates and the concentrations of $[\text{IO}_3^{-}]$ and $[\text{I}^-]$.
Use data from Table 3.1 to calculate the rate constant, $k$, for this reaction. Include the units of $k$.
Use data from Table 3.1 to calculate the concentration of hydrogen ions, $[\text{H}^+]$, in experiment 2.
This reaction is carried out again in two separate experiments. The experiments are both at the same temperature and use the same concentrations of $\text{I}^-$ and $\text{IO}_3^-$. One experiment is at pH $1.0$ and the other is at pH $2.0$. Calculate the value of $\dfrac{\text{rate at pH }1.0}{\text{rate at pH }2.0}$.
In aqueous solution, iron(III) ions react with iodide ions, as shown. $2\text{Fe}^{3+} + 2\text{I}^- \rightarrow 2\text{Fe}^{2+} + \text{I}_2$. The initial rate of reaction is first order with respect to $\text{Fe}^{3+}$ and second order with respect to $\text{I}^-$. The mechanism for this reaction has three steps. Each step involves only two ions reacting together. Suggest equations for the three steps of this mechanism. Identify the rate-determining step.