Lab Report 24 - Kinetics of the Crystal Violet-Sodium Hydroxide Reaction REBECCA FORLOINE LAB PARTNER DANA Having read the Georgia Institute of

Lab Report 24 - Kinetics of the Crystal Violet-Sodium...

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Kinetics of the Crystal Violet-Sodium Hydroxide Reaction REBECCA FORLOINE LAB PARTNER: DANA MARCH 24, 2015 Having read the Georgia Institute of Technology Academic Honor code, I understand and accept my responsibility as a member of the Georgia Tech Community to uphold the Academic Honor Code at all times. In addition, I understand my options for reporting honor violations as detailed in the code.
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Abstract The purpose of this lab was to determine the kinetics of the crystal violet - sodium hydroxide reaction. We had previously studied thermodynamics which would allow us to predict if a reaction would be spontaneous and whether the reaction would be endothermic or exothermic. While this was useful information, it didn’t give any indication to the rate at which a spontaneous reaction would occur. The most important results obtained from this lab was the ability of students to determine the kinetic rate law for a chemical reaction. This experiment demonstrated how the rate constant and activation energy of a chemical reaction could be determined from graphical methods. The major impact of this work was showing students how to manipulate a rate low to solve for the constant, concentrations, or order of reaction. Introduction The rate of a chemical reaction is the change in concentration of a reactant or prudct as a function of time. The rate law establishes the proportionality between the rate of a reaction and the concentration of reactants. For a reaction A+BC, the rate law is given as: Rate=k[A] m [B] n . Activation energy is the energy required to start a chemical reaction and can be derived from the Arrhenius equation which is stated as follows: k = E a RT lnA The general goals of this experiment were to use the isolation method to determine the variables k, m, and n which are the rate law constant, the order with respect to CV, and the order with respect to hydroxide respectively. They can be seen in the following rate law for the following reaction under study. ¿¿ n O H ¿ CV ¿ m ¿ Rate = k ¿ To do this the concentration of one of the reactants was set very high relative to the other so that its concentration did not change too much over the course of the reaction. This helped us find n and m based on which reactant was set at a high concentration.
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