Studying the Rate of the Reaction of Potassium Permanganate and Oxalic Acid

INTRODUCTION The main theory behind this experiment is that by setting up several apparatuses using varying amount of t-butyl alcohol, distilled water, or an unknown liquid, the freezing point of t-butyl alcohol, the molal freezing point and the molar mass of an unknown can be determined. The equations pertinent to this experiment include the following: mc= ∆Tf=Tf-Tf'=(Kf)(mc) mc= mc= mc= gram molar mass of solute, g mole^-1= kf=∆Tf/ mc mass of unknown ,g=(volume of unknown, mL)(density of unknown, g mL-1)
NaCl(s) + H2O(l) → Na+ (aq) + Cl-(aq) This experiment relates to what is being studied by showing how random error can effect and experiment. This experiment teaches the students how to determine density, volume, and percentage errors.
OBJECTIVE
The objective of this experiment is to determine the order with respect to permanganate ion and to oxalic acid concentration for the reaction of potassium permanganate and oxalic acid solutions. Other goals include, writing a rate equation and determining the effect of increased temperature on the rate of this reaction.
MATERIALS AND EQUIPMENT
The materials required for this experiment include the following:
• 2-50ml Burets
• 60 mL of 0.755M H2C2O4
• 60 mL of 0.13M KMnO4
• Thermometer
• Stirring rod
• Hot Plate
• 6- Clean test tubes
• 2 Buret clamps
• Timer

PROCEDURE Two burets were rinsed, labeled, and filled with one having 0.755M H2C2O4 and the other with 0.13M KMnO4. Exact readings and concentrations of both burets were recorded on the data sheets. For determination 1, 5 mL of H2C2O4 was dispensed from the buret into a test tube. Next 6 mL of distilled water was dispensed into the same test tube and thoroughly mixed. About 1mL of KMnO4 was dispensed into a second test tube. The H2C2O4 solution from the first test tube was quickly transferred to KMnO4 test tube. The timer was started when half of the H2C2O4 solution was poured in. This new mixture was