Complete the table below: - the order of reaction with respect to $[\text{NO}]$ - the order of reaction with respect to $[\text{O}_2]$ - the overall order of reaction
Use the experiment 1 data to calculate the rate constant, $k$. State the units of $k$. $k =$ ................. , units $=$ .................
Calculate the value of $[\text{NO}]$ in experiment 2. $[\text{NO}] =$ ................. $\text{mol dm}^{-3}$
Define rate-determining step.
Suggest equations for a two-step mechanism for this reaction, stating which of the two steps is the rate-determining step. Peroxodisulfate ions, $\text{S}_2\text{O}_8^{2-}$, react with iodide ions, $\text{I}^-.$ $\text{S}_2\text{O}_8^{2-} + 2\text{I}^- \rightarrow 2\text{SO}_4^{2-} + \text{I}_2$ The rate equation for the reaction in the absence of any catalyst is shown. $\text{rate} = k[\text{S}_2\text{O}_8^{2-}][\text{I}^-]$ step 1 ........................................ step 2 ........................................ rate-determining step = ................................
An excess of peroxodisulfate ions is mixed with iodide ions. Right after 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. iodide ion concentration = ................. $\text{mol dm}^{-3}$