Preview

Formal Report- Kinetics of Reaction: the Iodine Clock Reaction

Powerful Essays
Open Document
Open Document
4623 Words
Grammar
Grammar
Plagiarism
Plagiarism
Writing
Writing
Score
Score
Formal Report- Kinetics of Reaction: the Iodine Clock Reaction
factors affecting the kinetics of reaction between peroxodisulfate (vi) and iodide

d. del prado1 and j. belano2
1 department of food science and nutrition, college of home economics
2 department of food science and nutrition, college of home economics university of the philppines, diliman, quezon city 1101, philippines date submitted: january 7, 2013

-------------------------------------------------

-------------------------------------------------
ABSTRACT
-------------------------------------------------

-------------------------------------------------
In everyday life, several reactions are encountered, but still knowledge on how fast these occur and the factors affecting it were still insufficient. This study aimed to determine the different factors affecting the rate of reaction and how these factors affected it. An experiment named iodine clock reaction was done to answer the questions raised. In this study the reaction of iodide ion and peroxodisulfate (VI) ion was analyzed with the help of thiocyanate ion. The experiment was divided into three parts. First, second, and third parts of the experiment were used to examine the effects of the reactant concentrations, temperature and the presence of catalyst to the rate of reaction, respectively. The time before the reaction proceeded was recorded and calculations were done to obtain necessary information. It was identified that increasing the reactant concentration would increase the rate of reaction. Likewise, higher temperature increased the rate. Finally, the presence of catalyst had enormous effect on the reaction rate. It increased as the catalyst was added. Based on the results obtained, it can be concluded that said factors could increase the rate of reaction by increasing the temperature or reactant concentration or by adding a catalyst on the mixture.
-------------------------------------------------

-------------------------------------------------

INTRODUCTION
Until now



References: [1] Bayquen, A.V., Exploring Life Through Science Chemistry. Phoenix Publishing House, Inc., 2009, 177. [2] Mendoza, E.E., Religioso, T.F., Chemistry, 3rd edition. Phoenix Publishing House, Inc., 2008, 347. [3] Bayquen, A.V., Exploring Life Through Science Chemistry. Phoenix Publishing House, Inc., 2009, 178. [4] Mendoza, E.E., Religioso, T.F., Chemistry, 3rd edition. Phoenix Publishing House, Inc., 2008, 344-346. [5] Silberberg, M.S., Principles of General Chemistry, 2nd edition. McGraw-Hill, 2010, 514. [6] Silberberg, M.S., Principles of General Chemistry, 2nd edition. McGraw-Hill, 2010, 527. [13] Silberberg, M.S., Principles of General Chemistry, 2nd edition. McGraw-Hill, 2010, 529. [14] Silberberg, M.S., Principles of General Chemistry, 2nd edition. McGraw-Hill, 2010, 530. [16] Silberberg, M.S., Principles of General Chemistry, 2nd edition. McGraw-Hill, 2010, 529.

You May Also Find These Documents Helpful

  • Powerful Essays

    Vorndam, E. M. (2001). Basic chemistry for investigating living systems. General biology for the college science major (pp. 92-111). Englewood, CO: Hands-On Labs, Incorporated.…

    • 7879 Words
    • 32 Pages
    Powerful Essays
  • Powerful Essays

    Iodine-Clock Reaction

    • 2660 Words
    • 11 Pages

    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.…

    • 2660 Words
    • 11 Pages
    Powerful Essays
  • Good Essays

    To find the order of the reaction with respect to the Hydrogen Peroxide (H2O2), Potassium Iodide (KI) and the Sulphuric Acid (H2SO4) by the use of an Iodine clock reaction.…

    • 4040 Words
    • 22 Pages
    Good Essays
  • Better Essays

    When decreasing the concentration of KIO3, 0.25 M of NaHSO3 was used against the KIO3 (0.1 M, 0.05 M, 0.025 M, 0.0125 M). The final variable tested was temperature. A heat plate was used to test the clock reaction of 0.25 M NaHSO3 and 0.05 M KIO3 at temperatures of 30, 35 and 40 degrees celsius. The experimental data found that as the concentration was decreased by half each time, the rate of reaction lengthened.…

    • 1191 Words
    • 5 Pages
    Better Essays
  • Better Essays

    Gilbert, T.R., R.V. Kriss, N. Foster, G. Davies. 2004. Chemistry The Science In Context. New York, NY: W. W. Norton & Company…

    • 1297 Words
    • 6 Pages
    Better Essays
  • Good Essays

    Antoine-Laurent Lavoisier’s experiments of the late 18th century helped to place the chemistry of life into the context of a larger understanding of chemistry and energetics.…

    • 760 Words
    • 4 Pages
    Good Essays
  • Powerful Essays

    Davidson, K. (2002). Synthetic life, [internet]. San Francisco Chronicle, San Francisco. [accessed 18 JUNE 2008.]…

    • 1189 Words
    • 5 Pages
    Powerful Essays
  • Good Essays

    The experimentally obtained data collected for the reaction between IO3- and HSO3- at various temperatures is clearly supported by the Arrhenius equation. Referring to Graph 1.7, the line of best fits clearly passes through most of the data points displaying a linear relationship between temperature and the rate of the reaction. The R-squared of the graph which is a statistical measure of how close the data are to the fitted regression line is 0.9818. This number is extremely low which indicates that the data points are very close to the theoretically derived calculations.…

    • 1146 Words
    • 5 Pages
    Good Essays
  • Powerful Essays

    Rate Law Lab

    • 1430 Words
    • 6 Pages

    The purpose of this experiment was to determine the rate law graphically from the rate of disappearance and the x y values also the specific rate constant (k). Activation energy was also determined, and the effect of catalyst was evaluated in the reaction between peroxodisulphate ion S2O82-, and iodide ion, I-.…

    • 1430 Words
    • 6 Pages
    Powerful Essays
  • Good Essays

    The detailed system of steps in a reaction is called the reaction mechanism, and it is one of the principal aims of chemical kinetics to obtain information to aid in the elucidation of these mechanisms in order to better understand chemical processes. Reactions usually occur in a stepwise manner with each step proceeding at a different speed. If the rate of reaction is slow enough to measure, this is indicative of a step much slower than the rest of the process, known as the rate limiting step. For most reactions, a steady reaction state is quickly attained in which the concentration of reaction intermediates becomes dependent on the rate limiting step and closely associated steps. From this principle, the common rate law equation was experimentally determined (Eq. 1). Experimentally, the rate of reaction can be determined by altering the concentrations of the reactants. For our experiment we used the method of initial rates.…

    • 757 Words
    • 4 Pages
    Good Essays
  • Powerful Essays

    The aim of this experiment is to find the effect of varying the concentration of iodide ions on the rate of reaction between hydrogen peroxide and an acidified solution of potassium iodide: H2O2(aq) + 2H+(aq) + 2I⁻ → 2H2O(l) + I2(aq) The course of this reaction can be followed by carrying it out in the presence of small quantities of starch and sodium thiosulfate solutions. As the iodine molecules are produced they immediately react with the thiosulfate ions and are converted back to iodide ions: I2(aq) + 2S2O32⁻(aq) → 2I⁻(aq) + S4O62⁻(aq) During this period the reaction mixture remains colourless. But once the thiosulfate ions have been used up, a blue/black colour suddenly appears because the iodine molecules now get the chance to react with the starch. A series of experiments will be carried out in which only the concentration of the iodide ions will be varied. the concentration and volumes of the other chemicals involved will be kept constant as well as the temperature at which the experiments are performed. Since the amount of thiosulfate ions initially present will be the same in each experiment, the appearance of the blue/black colour will always represent the same extent of the reaction. So it t is the time taken for the blue/black colour to appear then we can take 1/t as a measure of the reaction rate*. Apparatus and Chemicals…

    • 1498 Words
    • 6 Pages
    Powerful Essays
  • Powerful Essays

    The purpose for the experiment Chemical Kinetics, a clock reaction is to figure out the reaction rate of a solution regarding its concentration, temperature, and also determine the effects of when a catalyst is present. The experiment resulted that the concentration, as well as its temperature can affect the rate constant inversely the outcome of the rate constant. By conducting the experiment, it is also discovered that the rate order of the reaction resulted as [I-]=1, [BrO3]=1 [H+]=2, the rate constant was averaged out at 33.08 (1/M3s1) and the Activation Energy calculated to be 46 kJ.…

    • 1192 Words
    • 5 Pages
    Powerful Essays
  • Powerful Essays

    Copper Cycle Lab

    • 1613 Words
    • 7 Pages

    Brown T.L., Murphy C.J., LeMay H.E., Langford S.J., Bursten B.E., Sagatys D. (2010) Chemistry the Central Science: a broad perspective 2nd Ed. Pearson Australia Group…

    • 1613 Words
    • 7 Pages
    Powerful Essays
  • Satisfactory Essays

    Iodide Clock

    • 268 Words
    • 2 Pages

    To determine the rate law for this reaction a series of changes in the concentration of peroxydisulfate, [S2O82-], and a series of changes in the catalyst while mean the corresponding changes in time, t, needs to be observed and measured. To measure these changes in concentration over time, a chemical "clock" is needed to change the dark blue color back to a colorless solution. This chemical clock is created by adding a series of measured volumes of thiosulfate ion, S2O32- , to Reaction (1).…

    • 268 Words
    • 2 Pages
    Satisfactory Essays
  • Good Essays

    Ventilation. Wash away spilled liquid with plenty of water. Do NOT absorb in sawdust or other combustible absorbents. Do NOT let this chemical enter the environment. Personal protection: chemical protection suit including self-contained breathing apparatus.…

    • 1241 Words
    • 5 Pages
    Good Essays