(a(i))[2]
Use the table data to work out the order for each reactant, $\text{ClO}^-$ and $\text{NH}_3$. Show how you reached your answer.
(a(ii))[1]
Write down the rate equation for this reaction.
(a(iii))[2]
Use the data from experiment 1 to calculate the rate constant, $k$, for this reaction. State the units of $k$ as well.
(a(iv))[1]
On the axes sketch a graph to show how the value of $k$ varies as temperature is increased.
(b(i))[2]
Describe how the results from this experiment can be used to confirm that the reaction is first-order in $[\text{I}^-]$.
(b(ii))[1]
Use this mechanism to work out the overall equation for this reaction.
(b(iii))[1]
Identify a step that involves a redox reaction. Explain your answer.
(iv)[1]
On the axes sketch a graph showing how $k$ changes as temperature rises.