chm lab Essay

2139 Words9 Pages
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
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
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This is important because the initial presence of reactant KMnO4 can be visualized thus allowing the rate of the reaction to be measured due to a decrease in KMnO4 1. By measuring KMnO4, the reaction rate can be calculated by using equation (4):
Rate=- Δ[KMnO4]/ Δt (4)
Δ[KMnO4] is the difference between initial and after concentrations when reaction is complete Δt= elapsed time1.
In part two, determinations were performed between solutions of KMnO4 and H2C2O4 with constant initial concentrations and varying temperatures to examine the effect on reaction rates. The “Rule of Thumb1” states that when a reaction temperature is raised 10 °C, the reaction rate will double. To prove this theory, temperatures were increased roughly 10°C in every determination to prove that for every 10°C increase in temperature results in doubling the reaction rate1. The reaction rate was calculated using equation (4):
Part 1:
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. The solution was added to a test tube containing 1.00 ml of 0.130M KMnO4. A timer was started after half of the H2C2O4 solution was added. The solution was thoroughly mixed with a glass stirring rod and placed in a spectrometer to visualize the absorbency decrease. The solution was taken out of the spectrometer and placed in a test tube support once the
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