Marc DeeleyCarl Caughell, Kristi Kulig
CHEM 126/Section 01
Dates of Experimentation: 10/12/10; 10/19/10
Title: Studying the Rate of Reaction of Potassium Permanganate and Oxalic Acid
Abstract:
The purpose of this experiment was to determine the reaction order and write a rate equation with respect to changes in permanganate ion and oxalic acid concentrations and to examine the effect temperature has on the rate of the reaction 1. In part one, the reactants potassium permanganate (KMnO4) and oxalic acid (H2C2O4), three determinations were performed, each with different initial concentrations of the reactants. Each initial concentration resulted in a unique reaction rate; these rates were then examined using the method of initial …show more content…
A total of three determinations were conducted and each determination was performed using the above procedure. Determination 2 was performed using the above procedure and 1.00 ml of distilled water, 10.00 ml of H2C2O4 and 1.00 ml of KMnO4. Determination 3 was performed using 2.00 ml of distilled water, 5.00 ml of H2C2O4 and 2.00 ml KMnO4. All reactions were performed at room temperature1.
Part 2:
To a test tube containing 6.00 ml of distilled water, 5.00 ml of 0.755M H2C2O4 was added and thoroughly mixed with a glass stirring rod. To a test tube, 1.00 ml of 0.130M KMnO4 was pipetted. Reactants were placed in a warm water bath (31 °C) for 10 minutes. Once ten minutes elapsed, the H2C2O4 solution was quickly added to the KMnO4 solution. After half of the H2C2O4 solution was added, the timer was started and the solution was placed back into the warm water bath. The timer was stopped once the last trace of red disappeared from the solution. Determination 2 was performed using the above procedure and a water bath temperature of 38 °C. Determination 3 was performed using the same procedure and a water bath temperature of 53 °C1. All of the initial concentrations remained the same throughout part two.
Results and Discussion:
Part 1:
With the data in table 2 and the method of initial rates (2), the orders with respect to each reactant were calculated. The order for each reactant was 1, making each reactant first order and the overall reaction, second