Iodination of Acetone
Estimation of the Activation Energy for the Iodination of Acetone Through the Effect of Temperature on the Rate Constant
Joel Costa, Alex Fuentes, Michael Chea, Rex Nwerem
Dr. Morgan Ferguson
July 9, 2013
ABSTRACT |
It is often important to determine the rate at which a chemical reaction takes place, i.e., how fast it yields the desired products. Temperature is one of the factors that influence the rate of reactions and it does so by providing energy to reactant particles so that a larger fraction of them reach the activation energy necessary to start the reaction. The purpose of this experiment was to estimate the Activation Energy for the Iodination of Acetone through the analysis of the relationship between the rate constant and temperature. Six trials of the reaction were run at different temperatures (over a range of 40.5 ºC) maintaining the reactants concentration constant, and the Activation Energy was determined by means of the graphical analysis of the linearized for of the Arrhenius equation. The Activation energy was estimated to be 74kJmol-1, which represents a 9.9% error with respected to the accepted value of 82kjmol-1.
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Introduction:
Chemical reactions are omnipresent. They are the hidden engine of life, not only in terms of its intrinsic biological dimension, but also from the perspective of industry, commerce and science, tools that ultimately serve the purpose of providing for the needs of society.
Frequently, time and efficiency are key elements that must be addressed to maximize the outcome of a desired reaction, especially in an industrial setting. How fast a certain product can be obtained is related to the field of Chemical Kinetics and implies the need to know (1) the factors that affect the rate of a reaction, (2) the rate law for that specific reaction and (3) the rate constant for the steps of the reaction mechanism. This information is neither deducible from the reaction equation nor from its stoichiometry; it must be
Joel Costa, Alex Fuentes, Michael Chea, Rex Nwerem
Dr. Morgan Ferguson
July 9, 2013
ABSTRACT |
It is often important to determine the rate at which a chemical reaction takes place, i.e., how fast it yields the desired products. Temperature is one of the factors that influence the rate of reactions and it does so by providing energy to reactant particles so that a larger fraction of them reach the activation energy necessary to start the reaction. The purpose of this experiment was to estimate the Activation Energy for the Iodination of Acetone through the analysis of the relationship between the rate constant and temperature. Six trials of the reaction were run at different temperatures (over a range of 40.5 ºC) maintaining the reactants concentration constant, and the Activation Energy was determined by means of the graphical analysis of the linearized for of the Arrhenius equation. The Activation energy was estimated to be 74kJmol-1, which represents a 9.9% error with respected to the accepted value of 82kjmol-1.
|
Introduction:
Chemical reactions are omnipresent. They are the hidden engine of life, not only in terms of its intrinsic biological dimension, but also from the perspective of industry, commerce and science, tools that ultimately serve the purpose of providing for the needs of society.
Frequently, time and efficiency are key elements that must be addressed to maximize the outcome of a desired reaction, especially in an industrial setting. How fast a certain product can be obtained is related to the field of Chemical Kinetics and implies the need to know (1) the factors that affect the rate of a reaction, (2) the rate law for that specific reaction and (3) the rate constant for the steps of the reaction mechanism. This information is neither deducible from the reaction equation nor from its stoichiometry; it must be
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