# Kinetics

Topics: Chemistry, Reaction rate, Rate equation Pages: 3 (424 words) Published: October 29, 2013
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Iodation of Acetone Lab

Lab Section 232

Introduction
In this experiment the rate law exponents (x and y) and the rate constant (k) were determined for the reaction between acetone and iodine using chemical kinetics. In this situation the rate is how quickly or slowly a chemical reaction occurs. The rate law shows how concentrations in the reaction affect the rate of the reaction. Experimental

After calibrating the spectrometer, an acetone solution was prepared of 10.0mL acetone diluted with distilled water in a 50-mL flask. In the first trial, 1.9mL of distilled water was placed in a cuvette, followed by 0.9mL of 1.0M HCl, 0.8mL of the acetone solution, and 0.5mL of 0.005 M I2 solution. The reaction was timed until the absorbance reached a nominal zero value, which was recorded. In the second trial, the same process was repeated but the concentration of the acetone was doubled. In the third trial the process was the same as the first trial but the concentration of the H+ solution was doubled.

Results
The data shows that as the concentration of each component is doubled, the rate also doubles. The reaction occurred the fastest in Trial 3, where the H+ concentration was doubled, and slowest in Trial 1, where the concentrations were the same.

Data Tables

Part 1 trials and results

Average rate: 2.6e-5

Calculations
Sample Calculations:

Trial 1
Trial 2
Trial 3
[Acetone] (mL)
0.8
1.6
0.8
[H+] (mL)
0.8
0.8
1.6
Rate ( m-1s-1)
2.61e-5
2.5e-5
2.7e-5
Time(sec)
220
117
107

[I2] =

Rate law = K

Avg rate =

Calculations:

Moles of Acetone =

10ml Acetone

rate (trial 1) =

K=

X=
1.88=2
2=2^x
=1

Y=
2=2y
=1

Discussion

In the experiment, the reaction between acetone and iodine was studied with the presence of hydrochloric acid as the catalyst. Because I2 is a colored reactant, the spectrometer was used to measure the time...

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