An iodine clock kinetics experiment was performed by varying the composition of

Question

An iodine clock kinetics experiment was performed by varying the composition of reactant solutions and measuring resulting rates of reaction Trial 1 Trial 2 Trial 3 Reactant Solution A 10.0 mLI (aq) 10.0 mL (aq) 5.0 mL (aq) 5.0 mL S203(aq) 5.0 mL S203(a) 5.0 mL S203 (aq) Reactant Solution B 10.0 mL S20(aq) 5.0 mL s208(aq) 10.0 mL S2082 (aq) 1.0 mL starch (aq) 1.0 mL starch (aq) 1.0 mL starch (aq) Time to complete10 seconds reaction 20 seconds 20 seconds How do trial 2 and 3 in the above table differ? More than one response is possible Trial 2 has twice as much I as Trial 3 Trial 3 has twice as much S208as Trial 2 Trial 3 has half as much S203- as Trial 2 Trial 2 has half as much starch as Trial 3 Incorrect. One of the three selected mechanisms is correct, but two are not supported by this data. Write out the rate laws for each mechanism to determine the mechanism which corresponds to matching reaction orders with respect to S208and Proposed mechanism 1 Proposed mechanism 2 Proposed mechanism 3 Proposed mechanism 4 Which of the four proposed mechanisms below would be support by these results? Note: there may be more than one answer (scroll down to see all four proposed mechanisms)

Explanation / Answer

Correct answer:Mechanism 2

Rate determining state is that elementary step which is slowest.

now if we consider the reaction rate of trial 1 and trial 2 we can see reaction rate depends on S2O82- concentration.

if we consider the reaction rate of trial 1 and trial 3 we can see reaction rate depends on I- concentration.

so mechanism2 is correct.because mechanism 2 consist both I- and S2O82- in its slowest elementary step.

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