rates and equations lab report
DESCRIPTION
The objective of this lab is to determine the rate of the iodination of acetone by differing the amounts of reactants, finding the rate constant (k) and the order of the reaction in terms of each of the reactants.TRANSCRIPT
IODINATION OF ACETONE
CHEMISTRY LAB REPORT
JANUARY 13 th , 2010
LAB PERFORMED BY:
Narendran Sairam and Steven Kraplin and Daniel Glukhov
Table of Contents1. Title Page........................................................................................................................................1
2. Table of Contents...........................................................................................................................2
3. Objective........................................................................................................................................3
4. Equipment......................................................................................................................................3
5. Experimental Procedure.................................................................................................................4
6. Data Tables.....................................................................................................................................5
7. Caculations.....................................................................................................................................5
8. Predictions......................................................................................................................................6
9. Conclusion.....................................................................................................................................6
Objective:
The objective of this lab is to determine the rate of the iodination of acetone by differing the
amounts of reactants, finding the rate constant (k) and the order of the reaction in terms of each of the
reactants.
Equipment: gloves
safety glasses
thermometer (manufactured by Control Company serial no: 61161-283)
two testubes
100 mL of 4M Acetone
100 mL of 1M HCl
100mL of 0.005 M I2
graduated cylinder
125 mL Erlenmeyer flask
distilled water
Experimental Procedure:
1. Prepare for lab by obtaining all the necessary materials in the equipment list.
2. Obtain 10 mL of 4M Acetone, 10 mL of 1M HCl, 20 mL of distilled water and 10 mL of
0.005mL 0.005 M I2.
3. Add the acetone, 1M HCl and water to a 125 mL Erlenmeyer flask and then quickly add the
0.005 M I2 and begin timing.
4. Swirl the mixture until the color disappears completely and the mixture is clear and comparable
to distilled water in another flask of the same type.
5. Record the time taken for the mixture to get to this state.
6. Record the temperature of the final mixture.
7. Repeat steps 2-6 and record data for the second run.
8. Obtain 20 mL of 4M Acetone, 10 mL of 1M HCl, 10 mL of distilled water and 10 mL of
0.005mL 0.005 M I2.
9. Repeat steps 3-6.
10. Repeat steps 8 and 9 and record data for the second run.
11. Obtain 10 mL of 4M Acetone, 20 mL of 1M HCl, 10 mL of distilled water and 10 mL of
0.005mL 0.005 M I2.
12. Repeat steps 3-6.
13. Repeat steps 11 and 12 and record data for the second run.
14. Obtain 10 mL of 4M Acetone, 10 mL of 1M HCl, 10 mL of distilled water and 20 mL of
0.005mL 0.005 M I2.
15. Repeat steps 3-6.
16. Repeat steps 14 and 15 and record data for the second run.
17. Check that you have the times and the temperatures for all the runs.
Data Table:
Mixture Volume of Acetone
(mL)
Volume of 1M HCl
(mL)
Volume of 0.005 M I2 (mL)
Volume of distilled water (mL)
Run time in seconds
Run time in seconds
Temperature in degrees
Celsius
I 10 10 10 20 175 190 20.45
II 20 10 10 10 79 64 21.1
III 10 20 10 10 135 104 19.5
IV 10 10 20 10 335 350 20.5
Mixture Acetone (M)
[H + ] (M)
[I2 ]o
(M)Rate=
[I2 ]o/average time(s -1 )
I 0.80 0.20 0.0010 5.4794 x 10-6
II 1.60 0.20 0.0010 1.3986 x 10-5
III 0.80 0.40 0.0010 9.5693 x 10-6
IV 0.80 0.20 0.0020 5.8394 x 10-6
Calculations:rate of reaction = k[acetone]m [H+]n [I2 ]p
(Rate II) / (Rate I) = 2m = 2.55244◦ m=1.35188
(Rate III) / (Rate I) = 2n = 1.7477◦ n=0.09793
(Rate IV) / (Rate I) = 2p = 0.9689◦ p=0.80439
Average Rate: obtained by plugging the values into the rate equation.
K I II III IV Average
k 5.09769117x 10-5 0.097696104x 10-5 5.097696103x 10-5 5.09769103x 10-5 5.09769487 x 10-5
Prediction: a trial experiment based on the data gathered and the values determined. The amounts of
reactants are randomly assumed. There is no specific reason for picking the numbers that were picked.
amount 4M Acetone: 100 mL
amount 1M HCl : 200 mL
amount 0.005M I2: 300mL
amount distilled water: 400 mL
Initial concentration of Acetone: 4M
Initial concentration of HCl: 1M
Initial concentration of I2: 0.005M
rate of reaction = k[acetone]m [H+]n [I2 ]p = 4.681141 x 10-6 seconds
Rate = [I2 ]o/average time= 1068.11 seconds -1
Conclusion:
I believe that this experiment has not met the expectations because the reaction rate that was
obtained through calculations did not correspond to the result provided by the instructor. This may be
for several reasons. For one, the temperatures of the runs varied and this inconsistency in temperature
affects the rate constant, k. also there may have a decent amount of human error involved in, for
example, measuring out the necessary quantity of reactants, miscalculating something or
misinterpreting the instructions provided. In light of these discrepancies, the obtained results are
justified in the fullest.