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Iodination of Acetone

The document outlines an experiment to study the kinetics of acid-catalyzed iodination of acetone, demonstrating that the reaction is zero order with respect to iodine concentration. It describes the materials, procedure, and calculations needed to determine the rate constants for different acids used in the reaction. The results include the rate constants for each acid and their ratios, which are to be calculated from the experimental data.

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147 views2 pages

Iodination of Acetone

The document outlines an experiment to study the kinetics of acid-catalyzed iodination of acetone, demonstrating that the reaction is zero order with respect to iodine concentration. It describes the materials, procedure, and calculations needed to determine the rate constants for different acids used in the reaction. The results include the rate constants for each acid and their ratios, which are to be calculated from the experimental data.

Uploaded by

arisports21
Copyright
© © All Rights Reserved
We take content rights seriously. If you suspect this is your content, claim it here.
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KINETICS OF IODINATION OF ACETONE

AIM:
To study the kinetics of acid catalysed iodination of acetone and to compare the given acid
strength.

PRINCIPLE:
Iodination of acetone in the presence of an acid is represented by the equation

CH3COCH3 + I2 + H+ → CH3COCH2I

This reaction is a zero order reaction with respect to iodine concentration. When large excess of
water is used the rate law can be written as dx/dt = k, or x= kt or k = x/t

A plot of ‘x’ vs time ‘t’ gives a straight line with slope ‘k’ in moles/litre/min.

MATERIALS REQUIRED:
Methyl acetate, iodine solution, acid, standard sodium thio sulphate solution, and sodium acetate
solution.

PROCEDURE:
10mL of acetone and 5mL of acid ‘A’ are placed in an iodine flask. The mixture is diluted to
100mL using water and placed in a thermostat for few minutes. 10mL of N/10 Iodine are
pipetted out into the iodine flask, shaken well and on the stop watch. Immediately 5ml of the
reaction mixture are pipetted into a conical flask containing 20% sodium acetate solution and
titrated against std sodium thiosulphate ( N/100) solution using starch indicator. The end point is
noted as volume at zero time. The titration is repeated for an interval of 3 minutes and the titer
values are noted. From these titer values rate constant of the reaction can be calculated. A plot of
titer values on y axis and time on x axis will give a straight line. The slope of the straight line
will be equal to the rate constant. The experiment is repeated using acids B and C. From the rate
constant values the ratio of the acids are calculated.

CALCULATION:
ko = x/t

ko = (Vt –Vo)/(tt-to)

X= (Vthio xNthio)/Vx2
Ratio of acids kA/kA = kB/kA = kC/kA =

Tabulation:
S. No. Time (min) Acid A Acid B Acid C
Vol of KA Vol of kB Vol of KC
thio (mL) thio (mL) thio (mL)
1 0
2 3
3 6
Average =

RESULT:
i) The rate constant for the acid catalysed iodination of acetone using

Acid A = ------ mol lit-1min-1 and ---------- mol lit-1min-1 graphically.

Acid B = ------ mol lit-1min-1 and ---------- mol lit-1min-1 graphically.

Acid C = ------ mol lit-1min-1 and ---------- mol lit-1min-1 graphically.

ii) The ratio of acids A:B:C =

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