Activation Energy Lab Report

57 THE IODINATION OF ACETONE Part One: Determining the pass judgment for a chemic Reaction The value of a chemical substance reception enume casts on several(prenominal) factors: the nature of the response, the duckings of the reactants, the temperature, and the presence of a achievable catalyst. In this test we give first determine the mildew law for a response by changing more or less of the above variables and meter the appraise of the reply. During Part Two, we will look for the relation amongst the ordinate constant and temperature to discover the activation ability for this reception. In this experiment we will study the kinetics of the reaction in the midst of unity 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 hale 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(prenominal) value, for this lab we will be looking only for whole number values for the orders of reaction (0, 1, 2 are acceptable tho 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 iodised 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 quantity 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 = or simply...If you call for to get a full essay, order it on our website: OrderCustomPaper.com

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