Fill in the rate equation for this reaction.
In a reaction, the initial concentrations of NO and $\text{O}_3$ are each $1.20 \times 10^{-6}\ \text{mol dm}^{-3}$. Calculate the initial rate of the reaction. State its units.
The reaction described in (a)(ii) is followed over time. Predict whether the graph of $[\text{NO}]$ against time, under these conditions, shows a constant half-life or not. Explain your answer.
Nitrous oxide, $\text{N}_2\text{O}$, breaks down into its elements. $2\text{N}_2\text{O(g)} \rightarrow 2\text{N}_2\text{(g)} + \text{O}_2\text{(g)}$. At a high temperature, a small amount of platinum wire is added to a large amount of nitrous oxide. The reaction has zero order kinetics. The platinum wire acts as a catalyst. Sketch, on the axes below, a graph of reaction rate against time for the catalysed decomposition of $\text{N}_2\text{O}$ under these conditions.
Sketch a graph, on the axes below, of $[\text{N}_2\text{O}]$ against time for this reaction.
Platinum acts as a heterogeneous catalyst in this reaction. Describe the mode of action of a heterogeneous catalyst.
Suggest a reason why this reaction has zero order kinetics when the amount of nitrous oxide is large and the amount of platinum is small.