Iodination Of Propanone Lab Report

The Kinetics of the acid-catalyzed iodination of propanone

Raw Data:
Solution A:Propanone 2M
Solution B: Iodine 0.005M
Solution C: Sulfuric acid 1M
Solution D: Distilled water

Table 1
Experiment Volume of solution A ±0.05 (cm3) Volume of solution B ±0.05
(cm3) Volume of solution C ±0.05
(cm3) Volume of solution D ±0.05
(cm3) Total Volume
±0.2 (cm3)
1 2 2 2 4 10
2 4 2 2 2 10
3 6 2 2 0 10
4 2 1 2 5 10
5 2 0.5 2 5.5 10
6 2 2 4 2 10
7 2 2 6 0 10

Table 2
Experiment Time for yellow color to disappear Trial A ±0.2s Time for yellow color to disappear Trial B ±0.2s Time for yellow color to disappear Trial C ±0.2s
1 114.0 102.0 86.2
2 36.0 49.0 51.8
3 37.0 46.0 48.8
4 44.0 45.0 55.6
5 20.0 30.0 28.0
6 55.0 63.0 58.3
7 30.0 33.0 45.0

Table 3
Experiment Concentration
Therefore the change in rate is only due to the change in concentration of A (Propanone). The concentration of propanone in experiment 2 is the double of it in experiment 1. Something similar happens with the rate: In experiment 2 the rate is almost the double than the rate of experiment 1. This means that the order of [C3H6O] is 1.

2) In experiment 4 and 5 [Solution B] is the only one which changes. The concentration of iodine in experiment 5 is the half than in experiment 4. It is noticeable that the rate didn't change much, in fact, this small change might have been produced due to the inaccuracies of the experiment. So it can be said that the order of [I2] is 0.

3) In experiment 5 and 6 [solution B] and [solution C] changes. Nevertheless it has been deduced above that the order of [I2] was cero so the change in rate from experiment 5 to 6 is just because of the change in concentration of solution C. In experiment 5 rate is 1.92, it can be said that this number is pretty close to 2. In experiment 6 the rate is 4.25, number which is close to 4. It can be said that as the rate doubles, the Δ in [solution C] also doubles and the Δ in [solution B] (iodine) does not affect the rate, then the order of [H2SO4] is
∴ the overall order of the reaction is 1+1+0=2.

As the overall order of the reaction is now calculated (2), it is possible to calculate the rate constant for this individual