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 Reactant Solution A 10.0 mL I (aq) 10.0 mLI (aq) 5.0 mL S203 (a) 5.0 mL S20(aq) Reactant Solution B 10.0 mL S208 (aq) 5.0 mL S20% (acq) 1.0 mL starch (a) 1.0 mL starch (aq) Time to complete 10 seconds reaction 20 seconds How do trial 1 and 2 in the above table differ? O Trial 1 has twice as much as Trial 2 O Trial 2 has twice as much S203 as Trial 1 O Trial 2 has half as much S20s as Trial 1 O Trial 1 has half as much starch as Trial 2 Almost. There are two additional correct choices. Write out the rate law equations to determine the other mechanism(s) that contain(s) a component that is first order with respect to S208 Proposed mechanism 1 Proposed mechanism 2 Proposed mechanism 3 Proposed mechanism 4 Which of the four proposed mechanisms below would be supported by these results? Note: there may be more than one answer (scroll down to see all four proposed mechanisms)

Explanation / Answer

answers : 2,3 ,4 mechanisms

rate = k [S2O8-2][I-]^2

for mechanism 2 : rate depends on slow step : so rate = k [I-][S2O8^-2]

by solving including fast step : rate = [I-]^2 [S2O8^-2]

for mechanism 3 : rate = [I-][S2O8^-2]

for mechasim : 4 : direct reaction

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