Identify a change occurring in the reaction mixture that would make it possible to measure the rate of this reaction.
Use the data in the table to show that the reaction is first order with respect to $\text{H}_2(\text{g})$.
Use the data in the table to show that the reaction is first order with respect to $\text{ICl}(\text{g})$.
Complete the rate equation for the reaction between $\text{ICl}(\text{g})$ and $\text{H}_2(\text{g})$.
Use experiment 3 to work out a numerical value for the rate constant, $k$. $k = \ldots$
The reaction $2\text{ICl}(g) + \text{H}_2(g) \rightarrow 2\text{HCl}(g) + \text{I}_2(g)$ is first order with respect to $\text{ICl}(g)$ and first order with respect to $\text{H}_2(g)$. Suggest a mechanism for this reaction. You should assume: • there are two steps in the mechanism, • the first step is much slower than the second step. first step $\ldots \rightarrow \ldots$ second step $\ldots \rightarrow \ldots$
Describe two methods that use these results to show the reaction is first order with respect to concentration of $\text{H}_2(g)$.
Explain why a large excess of $\text{ICl}(g)$ is used.
A chemical reaction may be speeded up by the presence of a catalyst. Explain why a catalyst increases the rate of a chemical reaction.