Kinetics of the Reaction between Acetone and Iodine
The key aim of this experiment was to identify the rate equation for the acid-catalysed iodination of acetone and to therefore consider the insinuations in the mechanism from the rate formula obtained.
The stoichiometric formula for the response between iodine and acetone is beneath, followed by the interest rate equation (where x, y, z and k will be the values to get obtained): I2 + CH3COCH3 CH3COCH2I + HI
-d[I2]/dt = k [I2]x [CH3COCH3]y [H+]z
The method was performed as follows: Intended for run 1, 20cm3 of acetone, 10cm3 of sulphuric acid and 145cm3 of water was added to a conical flask. 25cm3 of iodine was then added to this solution which started the reaction and instantly, 20cm3 samples of this mixture was added to six flasks. After successive 5 day intervals, salt acetate was added to all the conical flasks in order to prevent the reaction. Flask 1 and 2 had been then titrated, (3 to six turned colourless) using 0. 01M salt thiosulfate and a starch indicator. Treatment was used here to place the starch in when ever before a great irreversible black/blue complex arised. This reaction gave the order for iodine. To find the purchase for acetone, the same procedure was followed but with 10cm3 of acetone instead of 20cm3 and 155cm3 to keep similar total reaction volume. In order to find the order for H+, the procedure was repeated nevertheless 5cm3 of sulphuric acidity was used rather than 10cm3 and again 150cm3 of drinking water was used to keep the total quantity constant. The quantity of iodine added remained unchanged.
The results for each titration for each work are proven below, then their particular graphs:
|RUN 1 | Time (mins)
| |5 |10
|Flask: |1 |2
|Titre: |5. eighty |4. forty five
|RUN 2 | Time (mins)...