Suggest which measurements could be taken to monitor the rate of this reaction from the information provided.
Explain what the term half-life of a reaction means.
In a different experiment, the decomposition rate of $\text{N}_2\text{O}_5(\text{g})$ is examined. $\text{N}_2\text{O}_5(\text{g}) \rightarrow 2\text{NO}_2(\text{g}) + \tfrac{1}{2}\text{O}_2(\text{g})$ The graph displays the data obtained. The reaction is first order with respect to $\text{N}_2\text{O}_5$. This may be verified from the graph by using half-lives.
Determine the half-life of this reaction. Show how you arrive at your answer on the graph. half-life $= \ldots\ldots\ldots\ldots\ldots\ldots\ldots\ldots\ldots$ s
Suggest what happens to 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 find the rate of reaction at $200\,\text{s}$. Show how you worked it out. rate $= \ldots\ldots\ldots\ldots\ldots\ldots\ldots$ units $= \ldots\ldots\ldots\ldots\ldots\ldots\ldots$
The rate equation for this reaction is given below. rate $= k[\text{N}_2\text{O}_5]$ Using your result from (c)(i), calculate the rate constant, $k$, for this reaction and give its units. $k = \ldots\ldots\ldots\ldots\ldots\ldots$ units $\ldots\ldots\ldots\ldots\ldots\ldots$
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 rate $= k[\text{NO}_2][\text{O}_3]$. Suggest a possible two-step mechanism for this reaction.