spectrophotometric determination of the emperical formula coordination compound
PRACTICAL REPORT
NAME: ROXANNE
STUDENT NO: 24681012 MODULE CODE: MCHE 321
EXPERIMENT NO: 2
TITTLE: KINETICS 2: TEMPERATURE OF THE REACTION: OXALIC ACID-POTASSSIUM PERMANGANATE REACTON Title:
Temperature of the reaction: Oxalic Acid-Potassium Permanganate Reaction System
Author:
Miss Cleopatra Saul
Abstract:
The purpose of this experiment is to determine the rate of a chemical reaction (potassium permanganate, KMnO4, + oxalic acid, H2C2O4) as the concentrations are varied and to determine the rate law for the reaction. Since rates depend on temperature, we will also look at the effect of temperature on the rate of this reaction.The reaction rate or the oxidation-reduction between oxalic acid and potassium permanganate, KmnO4 is measured by recording the time elapsed for the purple colour of the permanganate ion to disappear in the reaction.As the temperature increases, the rate constant also increases and the rate of reaction increases as well. Addition of a catalyst reduced the height of the energy barrier and thus increases the rate of reaction. When the temperature is increased by 10oC ,the reaction Factor is= 1.55*10^-2 which is calculated by using the value o the activation energy and changes in temperature
Introduction
Kinetic analyses are often performed in order to refine our understanding of what happens on the molecular level during a chemical reaction. The main use of chemical kinetics is to measure the speed of a chemical reaction. But more importantly, in measuring the speed of a reaction. Rate law is a relationship between concentrations and rate. The reaction rate or the oxidation-reduction between oxalic acid and potassium permanganate, KmnO4 is measured by recording the time elapsed for the purple colour of the permanganate ion to disappear in the reaction. The rate of discharge of the purple colour of permanganate can thus be used as a measure o the rate of the reaction. The over-all reaction between permanganate and oxalic acid
NAME: ROXANNE
STUDENT NO: 24681012 MODULE CODE: MCHE 321
EXPERIMENT NO: 2
TITTLE: KINETICS 2: TEMPERATURE OF THE REACTION: OXALIC ACID-POTASSSIUM PERMANGANATE REACTON Title:
Temperature of the reaction: Oxalic Acid-Potassium Permanganate Reaction System
Author:
Miss Cleopatra Saul
Abstract:
The purpose of this experiment is to determine the rate of a chemical reaction (potassium permanganate, KMnO4, + oxalic acid, H2C2O4) as the concentrations are varied and to determine the rate law for the reaction. Since rates depend on temperature, we will also look at the effect of temperature on the rate of this reaction.The reaction rate or the oxidation-reduction between oxalic acid and potassium permanganate, KmnO4 is measured by recording the time elapsed for the purple colour of the permanganate ion to disappear in the reaction.As the temperature increases, the rate constant also increases and the rate of reaction increases as well. Addition of a catalyst reduced the height of the energy barrier and thus increases the rate of reaction. When the temperature is increased by 10oC ,the reaction Factor is= 1.55*10^-2 which is calculated by using the value o the activation energy and changes in temperature
Introduction
Kinetic analyses are often performed in order to refine our understanding of what happens on the molecular level during a chemical reaction. The main use of chemical kinetics is to measure the speed of a chemical reaction. But more importantly, in measuring the speed of a reaction. Rate law is a relationship between concentrations and rate. The reaction rate or the oxidation-reduction between oxalic acid and potassium permanganate, KmnO4 is measured by recording the time elapsed for the purple colour of the permanganate ion to disappear in the reaction. The rate of discharge of the purple colour of permanganate can thus be used as a measure o the rate of the reaction. The over-all reaction between permanganate and oxalic acid
Bibliography: 1) Atkins, P. W., & De Paula, J. (2006). Physical Chemistry for the Life Sciences. New York, NY: W. H. Freeman and Company.8th ed.p:729-8 2) Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2002). General Chemistry: Principles and Modern Applications. Upper Saddle River, NJ: Prentice-Hall, Inc. 3) Kenneth A. Connors.(1990). Chemical Kinetics, the study of reaction rates in solution, 1990, VCH Publishers 4) Whitten K.W., Galley K.D. and Davis R.E.(1992) . General Chemistry (4th edition, Saunders, p.638-9 5) I. Tinoco, K. Sauer and J.C. Wang.(1995). Physical Chemistry. Principles and Applications in Biological Sciences. (3rd ed., Prentice-Hall. p.328-9