Final answer:
The kinetics experiment on the reaction between hydrogen peroxide and iodide ion has several limitations, including the dependency on a catalyst, the complexity of the reaction mechanism, and the need for precise experimental methods to determine reaction rates.
Step-by-step explanation:
The kinetics of the reaction between hydrogen peroxide and iodide ion involves a number of limitations that could affect the results of an experiment. The presence of a catalyst, such as iodide ion, is crucial to this reaction as it lowers the activation energy and provides an alternative mechanism. One key limitation is that the reaction mechanism consists of multiple steps, and the rate-determining step dictates the overall rate of reaction. This reaction mechanism includes the formation of IO¯ as an intermediate.
Furthermore, measurements must be taken carefully; for instance, tracking the concentration of hydrogen peroxide every 6 hours at a constant temperature of 40 °C to calculate reaction rates. Accurate determination of instantaneous rates of reaction may require calculus or graphical evaluation, which can introduce experimental errors.
Another important consideration is the role of iron ions when persulfate ions and iodide ions react. Both iron(II) and iron(III) ions can catalyze this reaction, which highlights how additional factors can complicate the kinetics. Therefore, ensuring controlled experimental conditions and accounting for all possible variables is paramount for obtaining accurate results.