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Effect of concentration on rate of reaction
Effect of concentration on rate of reaction
Effect of concentration on rate of reaction
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The Landolt Iodine clock reaction is used to show chemical kinetics and reaction mechanisms as well as the effect concentration has on reaction rates. Mechanisms are a very exact and detailed way of telling what happens to molecules at each level in a reaction. Mechanisms include things such as how the molecular geometry of the reagents change throughout the reaction and tells which bonds are broken/formed. In this reaction, two clear liquids are poured together into a beaker and mixed. It yields a clear liquid. However, after waiting for a few minutes, the clear liquid isn’t clear anymore, but is a dark blue. The “clock” in the title of the experiment really isn’t a clock at all. It just refers to the fact that the time that it takes for the solutions to turn a dark blue depends of the concentrations of the reagents used.(1)
There are many variations of this lab that can be done that all illustrate the idea of chemical kinetics. Hydrogen peroxide can be used, as well as iodate, persulfate, and chlorate. The variation of hydrogen peroxide uses the following reagents: hydrogen peroxide, potassium iodide, hydrochloric acid, starch and thiosulfate. The basic reaction for this variation is as followed: H2O2 + 3 I- + 2 H+ → I3- + 2 H2O. The reactants are hydrogen peroxide, hydrogen ions the ions of hydrogen come from the hydrochloric acid), and iodine ions (the iodine ions come from the potassium iodide). In this equation the reactants of liquid hydrogen peroxide, and the ions of the iodine, and hydrogen acid react together to produce triiodide and water as products.
The second reaction in the experiment is as followed: I3S- + 2 S2O32- → 3 I- + S4O62- . The reactants of triiodate and the thiosulfate ions (from the thiosulfate) r...
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... is not the only thing it taught the community of chemists though, it also showed that reactions are able to sit at equilibrium for a while before fully going to completion. After the academy had seen the work he had done in with the reaction, he became a director of the Second Chemical Institute of the Berlin University. He worked here from 1891 to 1905. During this time he also proved the law of concentration of mass and energy to be true, adding to his contributions the science of chemistry. He died in 1910. (3)
This experiment was ground- breaking for many reasons. First, it displayed a clear end that happens after a an defined amount of time.
Works Cited
1.) http://en.wikipedia.org/wiki/Iodine_clock_reaction
2.) http://www.sciencebuddies.org/science-fair-projects/project_ideas/Chem_p091.shtml#background
3.) http://en.wikipedia.org/wiki/Hans_Heinrich_Landolt
middle of paper ... ... The Web. 22 Feb. 2014. http://www.chemheritage.org/discover/online-resources/chemistry-in-history>.
The objective of part A was to determine the rate of the substitution reaction between 1-Chlorobutane and KOH. This information was obtained by using the titration method to record the concentration of KOH over a given amount of time. To start this procedure, 1-Chlorobutane was added to a round bottom flask, which was connected to a reflux apparatus. Once it was observed that reflux had started the KOH was added with EtOH; this is the start of the reaction. The aliquot was then titrated with 0.100 M HCl and the concentration was noted at each interval. By graphing the data one can determine the order of the reaction and the rate of the leaving group. This data will provide the type of the reaction, whether it is SN1 or SN2.
Through the completion of this experiment, the dynamics of stoichiometry are demonstrated by preforming a chemical reaction in a solution. This procedure will ultimately show how limiting reactants are factored into a reaction by using a varying amount of reactants involved. To better understand this concept, it is vital to define stoichiometry; stoichiometry is a way of documenting the amounts of products and reactants involved through a series of coefficients that describes the ration in which the reactants will fuse together and the products form. In this particular lab, the following formula will be used to preform the necessary calculations:
+ 2I¯ (aq) + H[-1] 2O2 (l) ÕI2 (aq) + 2H2O2 (aq) Iodide ions are firstly oxidised by the hydrogen peroxide, as shown in the above equation. The iodine that is then produced reacts immediately reacts with thiosulphate ions as follows: I2 (aq) + 2Na2S2O3 (aq) Õ 2NaI (aq) + Na2S406 (aq) As soon as all of the thiosulphate ions have reacted with the iodine, the excess iodine molecules react with the 2% starch solution that is present in the reaction. This can be seen as an instant change in colour, from a colourless solution, to a deep purple coloured solution. This change in colour denotes the completion of the reaction. Factors affecting the rate of reactions: All chemical reactions occur at a definite rate under particular conditions.
2. In order to determine how fast a reaction is occurring there must be a basis for measurement. There must also be an indicator substances to determine the change that took place. Then there must be a tool to measure the change. In this lab a spectrophotometer was used. The ABS value is the actual value and it is used to determine the rate of change.
Parkington, James Riddick Parkington. Origins and Development of Applied Chemistry. New York: Arno Press, 1975.
Abstract: This week we experimentally determined the rate constant k for the reaction 2HCl (aq) +Na2S2O3 (aq) → S (s) + SO2 (aq) + H2O (l) + 2NaCl (aq). In order to do this the average reaction time was recorded in seconds during two trials. The data from the experiment shows this reaction is in the first order overall: rate=.47s-1 [HCl]0 [Na2S2O3]1. These findings seem to be consistent with the expected results
Ludwig Mond from Germany was the founder of a British chemical industry and the discoverer of many important chemical processes. Chemical processes was what embryos went through to become people well-adapted to their environment. Without deep study into chemistry, the Brave New World wouldn’t have existed.
However, in order to measure the rates of reaction, sodium thiosulphate and starch are added. Sodium thiosulphate is added to react with a certain amount of iodine as it is made. Without the thiosulphate, the solution would turn blue/black immediately, due to the iodine and starch. The thiosulphate ions allow the rate of reaction to be determined by delaying the reaction so that it is practical to measure the time it takes for the iodine to react with the thiosulphate. After the all the thiosulphate has reacted with the iodine, the free iodine displays a dark blue/black colour with the starch. If t is the time for the blue/black colour to appear, then 1/t is a measure of the initial rate.
This is the first reaction in the Harcourt Essen experiment. The iodine is oxidised to produce I2 wh...
In essence, the main objective was to use chemical titration to measure and then calculate the rate of conversion of hydrogen peroxide (H2O2) to water and oxygen by using the enzyme catalase. Other purposes of the lab were; to measure the effects of changes of temperature, pH, enzymes concentration, and substrate concentration on rates of an enzyme. The lab was also an opportunity to see a catalyzed reaction in a controlled experiment. And the last objective was to learn how environmental factors affect the rate of enzyme catalyzed reactions.
One vital process in the human body observed in chemistry is the idea of chemical kinetics. Chemical kinetics is the study of the rate of reactions, or how fast reactions occur.1 Three factors that affect chemical kinetics are concentration, temperature, and catalysis. As the concentration of a substance increases, the rate of the reaction also increases.1 This relationship is valid because when more of a substance is added in a reaction, it increases the likelihood that the
New York: Cambridge, 1990. Read on, John. From Alchemy to Chemistry: A Process of Ideas & Personalities. London: G. Bell, 1957. Roberts, Gareth. A.
Of all the scientists to emerge from the nineteenth and twentieth centuries there is one whose name is known by almost all living people. While most of these do not understand this mans work, everyone knows that his impact on the world is astonishing.
To control the rates of chemical reactions is imperative to the continued existence of our species. Controlled chemical reactions allow us to move forward in society, constantly. We find new ways to provide light and heat our homes, cook our food, and pursue in crafts that benefit our society. There are, however, just as there are advantages, disadvantages to the efficiency of controlling the rate of reactions, which in some cases can be fatal to our scientific development and progression. The growth of humankind necessitates that we must be able to control the rate of chemical reactions.