QUESTION 2 Answer both parts [TOTAL MARKS: 25] Q2(a) [8 Marks] For the reaction \( \mathrm{A} \xrightarrow{k 1} \mathrm{~B} \xrightarrow{k 2} \mathrm{C} \), draw two sketches showing how the concentrations of \( A, B \) and \( C \) will change during the course of the reaction if (i) \( k_{1} \gg{ } k_{2} \) (ii) \( \mathrm{k}_{1} \ll<<\mathrm{k}_{2} \) In each case, show which step is the rate determining step.
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(i) If \( k_{1} \gg{ } k_{2} \), this means that the first reaction (A to B) is much faster than the second reaction (B to C). Show more…
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The reaction $$2 \mathrm{I}^{-}(a q)+\mathrm{S}_{2} \mathrm{O}_{8}^{2-}(a q) \longrightarrow \mathrm{I}_{2}(a q)+2 \mathrm{SO}_{4}^{2-}(a q)$$ was studied at $25^{\circ} \mathrm{C}$. The following results were obtained where $$\text { Rate }=-\frac{\Delta\left[\mathrm{S}_{2} \mathrm{O}_{8}^{2-}\right]}{\Delta t}$$ a. Determine the rate law. b. Calculate a value for the rate constant for each experiment and an average value for the rate constant.
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