Use oxidation numbers to show why this is a redox reaction.
In the molecule of $\text{ClO}_2$, chlorine is the central atom. Draw the ‘dot-and-cross’ diagram for $\text{ClO}_2$. Show outer electrons only.
The reaction of $\text{ClO}_2$ with $\text{F}_2$ is shown: $2\text{ClO}_2 + \text{F}_2 \rightarrow 2\text{ClO}_2\text{F}$. The rate of reaction was measured at different concentrations of the two reactants and the results below were obtained. The rate equation is $\text{rate} = k[\text{ClO}_2][\text{F}_2]$.
What does the term order of reaction with respect to a particular reagent mean?
Use the results from experiment 1 to calculate the rate constant, $k$, for this reaction. Include the units of $k$.
Use the data in the table to calculate the initial rate in experiment 2, and $[\text{ClO}_2]$ in experiment 3.
What is meant by the term rate-determining step?
The equation for the reaction between $\text{ClO}_2$ and $\text{F}_2$ is shown: $2\text{ClO}_2 + \text{F}_2 \rightarrow 2\text{ClO}_2\text{F}$ with $\text{rate} = k[\text{ClO}_2][\text{F}_2]$. The mechanism for this reaction has two steps. Suggest equations for the two steps of this mechanism, stating which of the two steps is the rate-determining step.
Using the rate equation, explain why the rate increases as temperature rises.