Complete the table below by giving: the order of reaction with respect to $[\text{NO}]$; the order of reaction with respect to $[\text{O}_2]$; the overall order of reaction.
Using the data from experiment 1, Calculate the value of the rate constant, $k$. State the units of $k$.
Calculate the value of $[\text{NO}]$ for experiment 2.
Define what is meant by the term rate-determining step.
Peroxodisulfate ions, $\text{S}_2\text{O}_8^{2-}$, react with iodide ions, $\text{I}^-$. The equation is $\text{S}_2\text{O}_8^{2-} + 2\text{I}^- \rightarrow 2\text{SO}_4^{2-} + \text{I}_2$. The rate equation for the reaction without any catalyst is $\text{rate} = k[\text{S}_2\text{O}_8^{2-}][\text{I}^-]$. Suggest equations for a two-step mechanism for this reaction, and state which step is the rate-determining step.
A large excess of peroxodisulfate ions is mixed with iodide ions. At the instant of mixing, $[\text{I}^-] = 0.00780\,\text{mol dm}^{-3}$. Under the conditions used, the half-life of $[\text{I}^-]$ is $48\,\text{s}$. Calculate the iodide ion concentration $192\,\text{s}$ after the peroxodisulfate and iodide ions are mixed.