Rate Law of an iodine clock reaction

Title: Rate Law of an iodine clock reaction

Objective:

1. To determine the relationship between the concentration of reactant and the rate of
reaction.
2. To determine the rate constant of the experiment, k.
3. To determine the rate law of an iodine clock reaction

Flow chart:




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, Tabulation of data:

Set H20 H2SO4 Kl S2O32- Starch H2O2 Total Temperature(˚C)
(mL) (mL) (mL) (mL) (mL) (mL) volume(mL)
1 43.0 35.0 10.0 10.0 1.0 1.0 100.0 27.5
2 42.0 35.0 10.0 10.0 1.0 2.0 100.0 27.5
3 43.5 35.0 10.0 10.0 1.0 0.5 100.0 27.5
4 33.0 35.0 20.0 10.0 1.0 1.0 100.0 27.5
5 48.0 35.0 5.0 10.0 1.0 1.0 100.0 27.5
6 8.0 70.0 10.0 10.0 1.0 1.0 100.0 27.5
7 68.5 17.5 10.0 10.0 1.0 1.0 100.0 27.5




The initial molarity and initial volume Time/s Average Initial
Set Hydrogen Iodide ion Hydrogen Trial 1 Trial 2 /s rate(Ms-1)
ion M1(0.025M) peroxide
M1(0.36M) M1(0.8M)
1 137.6 139.2 138.4
2 0.016M 62.4 58.6 60.5 2.64x10-4
3 0.004M 238.0 246.2 242.1 1.65x10-5
4 0.005M 62.4 58.6 60.5 8.26x10-5
5 0.00125M 258.5 267.1 262.8 4.76x10-6
6 0.252M 49.9 45.3 47.6 5.29x10-3
7 0.063M 222.2 228.6 225.4 2.80x10-4




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