Iodine-Clock Reaction
CHEMICAL KINETICS: IODINE-CLOCK REACTION
DATE SUBMITTED: 14 DECEMBER 2012
DATE PERFORMED: 7 DECEMBER 2012
ABSTRACT
Chemical kinetics involving reaction rates and mechanisms is an essential part of our daily life in the modern world. It helps us understand whether particular reactions are favorable and how to save time or prolong time during each reaction. Experiment demonstrated the how concentration, temperature and presence of a catalyst can change the rate of a reaction. 5 runs of dilution and reaction were made to show the effect of concentration on chemical reactions. A certain run from the previous task was twice duplicated to for a “hot and cold” test for reaction rate. The prior run was again duplicated for a test with catalyst.
The data obtained was graphed in a linear regression form, using the Arrhenius equation: lnk=-EaR-1T+lnA, reaction rate: rate = k[A]x[B]y and other principles held in chemistry. The graph from the results determined that there is a relation between rate and the previously mentioned factors. The results validated the notion that temperature, concentration and catalysts can manipulate chemical kinetics.
INTRODUCTION
Chemical kinetics is an essential part of our lives. It determines the rates of reactions and how quickly reactants are converted to products. These reaction rates tell us how much time it would take to wait for a change, a physical change [1]. Chemical kinetics can be altered and controlled by five different factors, namely: the temperature at which the reaction occurs, application of pressure, concentration of reactants, nature of reactants and the presence of a catalyst. In this experiment, three of these factors are used to determine and validate their effects to the reaction rate, these factors are the temperature, the catalyst and the concentration of the reactants.
S2O82- + 2I- 2SO42- + I2 (1)
The rates of a reaction (2) is defined by the rate law (3), where k is the rate constant, [A] is
DATE SUBMITTED: 14 DECEMBER 2012
DATE PERFORMED: 7 DECEMBER 2012
ABSTRACT
Chemical kinetics involving reaction rates and mechanisms is an essential part of our daily life in the modern world. It helps us understand whether particular reactions are favorable and how to save time or prolong time during each reaction. Experiment demonstrated the how concentration, temperature and presence of a catalyst can change the rate of a reaction. 5 runs of dilution and reaction were made to show the effect of concentration on chemical reactions. A certain run from the previous task was twice duplicated to for a “hot and cold” test for reaction rate. The prior run was again duplicated for a test with catalyst.
The data obtained was graphed in a linear regression form, using the Arrhenius equation: lnk=-EaR-1T+lnA, reaction rate: rate = k[A]x[B]y and other principles held in chemistry. The graph from the results determined that there is a relation between rate and the previously mentioned factors. The results validated the notion that temperature, concentration and catalysts can manipulate chemical kinetics.
INTRODUCTION
Chemical kinetics is an essential part of our lives. It determines the rates of reactions and how quickly reactants are converted to products. These reaction rates tell us how much time it would take to wait for a change, a physical change [1]. Chemical kinetics can be altered and controlled by five different factors, namely: the temperature at which the reaction occurs, application of pressure, concentration of reactants, nature of reactants and the presence of a catalyst. In this experiment, three of these factors are used to determine and validate their effects to the reaction rate, these factors are the temperature, the catalyst and the concentration of the reactants.
S2O82- + 2I- 2SO42- + I2 (1)
The rates of a reaction (2) is defined by the rate law (3), where k is the rate constant, [A] is
References: [1] Ovelette, Robert. Introduction to General, Organic and Biological Chemistry. 1997. Prentice Hall. p. 236 [2] Wright, Cart [3] Whitten K. et. al. Chemistry. 2009. Brooks/Cole, Belmont California. p. 633 [4] Zumdahl,S [5] Tro, Nivaldo. Introductory Chemistry. 2009. Pearson Education Inc. New Jersey p. 560-563 [6] Zumdahl,S