Activation Energy Lab Report

57

THE IODINATION OF ACETONE
Part One: Determining the Rate for a chemic Reaction
The value of a chemical reception depends on several(prenominal) factors: the nature of the reaction, the concentrations of the reactants, the temperature, and the presence of a possible catalyst. In this test we give first determine the cast law for a reaction by changing some of the above variables and meter the appraise of the reaction. During Part Two, we will explore the relation amongst the ordinate constant and temperature to discover the activation energy for this reaction. In this experiment we will study the kinetics of the reaction in the midst of iodine and dimethyl ketone:
O C H3C CH3 + I2(aq) H3C H+ O C CH2I + HI(aq)

The rate of this reaction is found to depend on the concentration of the heat content ion (acid, HCl) as well as the concentrations of the reactants (dimethyl ketone and iodine). The rate law for this reaction is

rate = k[acetone]m[H+]n[I2]p
where k is the rate constant for the reaction and m, n, and p are the edicts of the reaction with respect to acetone, hydrogen ions (acid), and iodine, respectively. Although orders of reaction kitty be any value, for this lab we will be looking only for integer values for the orders of reaction (0, 1, 2 are acceptable but not 0.5, 1.3, etc.



) The rate of the reaction can also be expressed as the change in the concentration of a reactant divided by the time interval:

rate =

- ?[ I 2 ] ?t

The iodination of acetone is easily investigated because iodine (I2) has a deep yellow/ chocolate-brown burnish. As the acetone is iodinated and the iodine converted to the iodide anion, this color will disappear, allowing the rate of the reaction to be easily monitored. We can study the rate of this reaction by simply making I2 the limiting reactant in a large excess of acetone and H+ ion. By measuring the time required for the sign concentration of iodine (I2) to be used up completely, the rate of the reaction can be determined by the equation

rate =
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