From the table, work out the order for each reactant, $\text{ClO}^-$ and $\text{NH}_3$. Make your reasoning clear.
State the rate equation for this reaction.
Calculate the rate constant, $k$, for this reaction using the data from experiment 1. Include the units for $k$.
On the axes, sketch a graph showing how $k$ varies as temperature is increased.
Describe how the results from this experiment could be used to verify that the reaction is first-order with respect to $[\text{I}^-]$.
Using this mechanism, deduce the overall equation for this reaction.
Identify the step that contains a redox reaction. Explain your answer.
On the axes, sketch a graph showing how $k$ varies as temperature rises.
A further experiment examined the reaction between chlorate(I) ions and iodide ions in aqueous alkali. A solution containing iodide ions in aqueous alkali was added to a large excess of chlorate(I) ions, and $[\text{I}^-]$ was measured at regular intervals.