Suggest which measurements could be used to track the rate of this reaction from the information given.
Explain what is meant by the term half-life of a reaction.
In a different experiment, the decomposition of $\text{N}_2\text{O}_5(\text{g})$ is studied. $\text{N}_2\text{O}_5(\text{g}) \rightarrow 2\text{NO}_2(\text{g}) + \tfrac{1}{2}\text{O}_2(\text{g})$ The reaction is first order with respect to $\text{N}_2\text{O}_5$. The graph can be used, via half-lives, to verify this.
Determine the half-life of this reaction. Show your working on the graph.
Suggest the effect on the half-life of this reaction if the initial concentration of $\text{N}_2\text{O}_5$ is halved.
Use the graph in 5(b) to determine the reaction rate at $200\,\text{s}$. Show your working.
The rate equation for this reaction is given below. $\text{rate} = k[\text{N}_2\text{O}_5]$ Use your answer to (c)(i) to calculate the value of the rate constant, $k$, for this reaction, and give its units.
Nitrogen dioxide reacts with ozone, $\text{O}_3$, as shown. $2\text{NO}_2 + \text{O}_3 \rightarrow \text{N}_2\text{O}_5 + \text{O}_2$ The rate equation for this reaction is $\text{rate} = k[\text{NO}_2][\text{O}_3]$. Suggest one possible two-step mechanism for this reaction.